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Chapters
1: Solid State
2: Solutions
3: Electrochemistry
4: Chemical Kinetics
5: Surface Chemistry
Inorganic Chemistry
6: General Principles and Processes of Isolation of Elements
7: p-Block Elements
▶ 8: d-and ƒ-Block Elements
9: Coordination Compounds
Organic Chemistry
10: Haloalkanes and Haloarenes
Chapter 11: Alcohols, Phenols and Ethers
Chapter 12: Aldehydes, Ketones and Carboxylic Acids
Chapter 13: Organic Compounds containing Nitrogen
Chapter 14: Biomolecules
15: Polymers
Chapter 16: Chemistry in Everyday Life
![Nootan solutions for Chemistry Part 1 and 2 [English] Class 12 ISC chapter 8 - d-and ƒ-Block Elements - Shaalaa.com](/images/chemistry-part-1-and-2-english-class-12-isc_6:5f2b1b2038084cf381bfa42c826a928c.jpg "Nootan solutions for Chemistry Part 1 and 2 [English] Class 12 ISC chapter 8 - d-and ƒ-Block Elements")
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Solutions for Chapter 8: d-and ƒ-Block Elements
Below listed, you can find solutions for Chapter 8 of CISCE Nootan for Chemistry Part 1 and 2 [English] Class 12 ISC.
Nootan solutions for Chemistry Part 1 and 2 [English] Class 12 ISC 8 d-and ƒ-Block Elements REVIEW EXERCISES [Pages 476 - 192]
What are transition metals?
Which d-block metals are not normally considered as transition metals? Why?
Explain the magnetic properties of d-block (or transition) elements.
Explain the following about transition metals:
Metallic character
Explain the following about transition metals:
Oxidation states
How is the magnetic moment of a magnetic species related to the number of unpaired electrons?
Why do the transition. elements exhibit complex formation? Explain with suitable examples.
Give a reason for the following:
Cu+2 salts are paramagnetic, while Cu+ salts are diamagnetic.
Give reasons:
First ionisation energy of 5d-series elements are higher than those of 3d-and 4d-transition elements.
Give reasons for the following statement:
Transition metals and most of their compounds show paramagnetic behaviour.
What are transition metals?
In what way are the electronic configuration of transition elements different from those of representptive elements?
K2PtCl6 is a well known compound, whereas the corresponding Ni compound is not known. State a reason for it.
Transition elements show high melting points. Why?
Give reasons:
Transition metals show variable oxidation states.
Explain giving reasons:
A transition metal forms alloys with other transition elements.
Why Zn, Cd and Hg are not called transition metals?
Give reasons for the following:
The transition metals generally form coloured compounds.
Explain giving reasons:
Cd+2 salts are white.
Give reasons:
First ionisation energy of 5d-series elements are higher than those of 3d-and 4d-transition elements.
What are interstitial compounds?
Explain interstitial compounds with reference to transition metals.
Write any four properties of interstitial compounds.
Write the highest oxidation state of the element with atomic number 23.
Explain why transition metals are paramagnetic.
Why are transition elements good catalysts?
The d-electron configuration of Mn2+ and Ti2+ are d5 and d2 respectively. Which one of these ions will be more paramagnetic?
Consider the given standard potential (in volts) in 1 M acidic solution:
Fe2+/Fe : −0.4 V, Fe3+/Fe2+ : +0.8 V,
Mn2+/Mn : −2.1 V, Mn3+/Mn2+ : +1.5 V
- Comment on the relative stabilities of +2 and +3 oxidation states of iron and manganese.
- Which of the two metals may be more easily oxidised to +2 state?
Name the tripositive metal ion represented by the configuration 1s2 2s2 2p6 3s2 3p6 3d3.
Giving reason indicate which one of the following would be coloured:
Cu+, VO2+, Sc3+, Ni2+
(Atomic numbers: Cu = 29, V = 23, Sc = 21, N = 28)
Decide giving reason which one of the following pairs has the property indicated:
Fe or Cu has higher melting point.
Decide giving reason which one of the following pairs has the property indicated:
Co2+ or Ni2+ has lower magnetic moment.
Write the general formula by which the electronic configuration of the transition elements is represented.
Of the ions Co2+, Sc3+ and Cr3+, which ones will give coloured aqueous solutions and how will each of them respond to a magnetic field and why?
[Atomic number: Co = 27, Sc = 21, Cr = 24]
Why do the d-block elements exhibit a larger number of oxidation states than the f-block elements?
How do the transition elements form interstitial compounds? State an industrial advantage of such occurrence.
Name a transition metal which does not exhibit variation in oxidation states in the compounds.
In the transition series, with an increase in atomic number, the atomic radius does not change very much. Why is it so?
How do the oxides of the transition elements in lower oxidation states differ from those in higher oxidation states in the nature of metal-oxygen bonding and why?
Mention the direct consequence of the following factor on the chemical behaviour of the transition elements:
They have incompletely filled d-orbitals in the ground state or in one of the oxidised states of their atoms.
Mention the direct consequence of the following factor on the chemical behaviour of the transition elements:
They contribute more valence electrons per atom in the formation of metallic bonds.
Assign reason for the following:
Ce3+ can be easily oxidised to Ce4+.
Give reasons:
E° value for the Mn3+/Mn2+ couple is much more positive than that for Fe3+/Fe2+.
Assign reason for each of the following:
The transition elements form interstitial compounds.
Variable oxidation states are shown both by representative elements and transition elements. How is the behaviour different for the two groups? Illustrate with one example in each case.
Discuss the general trend in the following property of the 3d transition elements (21-29):
Atomic size
Discuss the general trends in the following properties of the 3d transition elements (21-29):
Oxidation states
Discuss the general trend in the following property of the 3d transition elements (21-29):
Formation of coloured ions
Why do the transition elements have higher enthalpies of atomisation?
How would you account for the following:
The 4d and Sd series of the transition metals have more frequent metal-metal bonding in their compounds than do the 3d metals.
Describe the variability of oxidation states in the first row of the transition elements (Sc-Cu) and indicate the general trend.
Explain the following:
Transition elements tend to be unreactive with increasing atomic number in the series.
Why do the d-block elements exhibit a larger number of oxidation states than the f-block elements?
Give reasons:
Cr2+ is a strong reducing agent whereas Mn2+ is not (Cr = 24, Mn = 25).
Give reasons:
The transition metal ions such as Cu+, Ag+ and Sc3+ are colourless.
Give reasons:
The enthalpies of atomization of transition metals of 3d series do not follow a regular trend throughout the series.
Give reasons:
The radius of Fe2+ (Z = 26) is less than that of Mn2+ (Z = 25).
Explain why Zn2+ salts are white whereas Cu2+ salts are coloured.
Given beside are the electrode potential values, E° for some of the first row transition elements:
| Element | \[\ce{E^\circ_{M^{n+}/M}}\] (V) |
| V (23) | −1.18 |
| Cr (24) | −0.91 |
| Mn (25) | −1.18 |
| Fe (26) | −0.44 |
| Co (27) | −0.28 |
| Ni (28) | −0.25 |
| Cu (29) | +0.34 |
Explain the irregularities in these values on the basis of electronic structures of atoms.
Why do the transition elements have higher enthalpies of atomisation?
Why are transition elements good catalysts?
Which is more paramagnetic, Fe2+ or Fe3+? Give reasons.
Give the relationship between the equivalent mass and molar mass of KMnO4 (molar mass = 158 g mol−1) in acidic medium.
Give the relationship between the equivalent mass and molar mass of KMnO4 (molar mass = 158 g mol−1) in alkaline medium.
Give the relationship between the equivalent mass and molar mass of KMnO4 (molar mass = 158 g mol−1) in neutral medium.
Describe the preparation of potassium permanganate from pyrolusite ore.
Why is K2Cr2O7 generally preferred over Na2Cr2O7 in volumetric analysis although both are oxidising agents?
Describe with chemical equations, what happens when K2Cr2O7 reacts with sodium chloride in the presence of conc. H2SO4.
Describe with chemical equations, what happens when K2Cr2O7 reacts with an acidified solution of Kl?
Describe with the help of chemical equations, the preparation of potassium dichromate from chromite ore.
Give balanced chemical equations for what happens when acidified potassium dichromate solution reacts with ferrous sulphate solution.
Give balanced chemical equations for what happens when acidified potassium dichromate solution reacts with hydrogen sulphide gas.
Draw the structure of \[\ce{Cr2O^{2-}_7}\] ion.
Describe with the help of chemical equations, the preparation of potassium dichromate from chromite ore.
Write balanced equations for the action of acidified potassium dichromate solution on potassium iodide solution.
Give balanced chemical equations for what happens when acidified potassium dichromate solution reacts with ferrous sulphate solution.
Write the uses of potassium dichromate.
Describe the preparation of potassium permanganate from pyrolusite ore.
Describe with an example the oxidising actions of permanganate ion in alkaline media. What alkali are actually used for?
Describe with an example the oxidising actions of the permanganate ion in acidic media. What acids are actually used for?
Mention two uses of potassium permanganate in the laboratory.
Give balanced chemical equations for the following reaction:
Between acidified potassium dichromate and potassium iodide.
Give balanced chemical equations for the following reaction:
Between potassium permanganate and oxalic acid in the presence of dilute sulphuric acid.
Give balanced chemical equations for the following reaction:
Chromite ore is fused with NaOH in air.
Write the complete chemical equation for the following:
An alkaline solution of KMnO4 reacts with an iodide.
Write the complete chemical equation for the following:
An excess of SnCl2 solution is added to a solution of mercury (II) chloride.
A green chromium compound (A) on fusion with alkali gives a yellow compound (B) which on acidification gives an orange coloured compound (C). ‘C’ on treatment with NH4Cl gives an orange coloured product (D), which on heating decomposes to give back (A). Identify A, B, C and D. Write equations for reactions.
What are actinoids? Give three examples.
Discuss briefly the physical properties of actinoids.
Discuss briefly the chemical properties of actinoids.
Give two examples of lanthanoid elements.
What are the common oxidation states exhibited by lanthanoids?
What are actinoids? Give three examples.
What is Lanthanoid contraction?
Write any two consequences of Lanthanoid Contraction.
What are the different oxidation states exhibited by the lanthanoids?
One among the lanthanoids, Ce (III) can be easily oxidised to Ce (IV). Explain.
Why is the separation of lanthanoid elements difficult?
Name the lanthanoid element which exhibits a +4 oxidation state besides the +3 oxidation state.
What is the basic difference between the electronic configuration of transition and inner transition elements?
How would you account for the following:
There is a greater range of oxidation states among the actinoids than among the lanthanides.
How would you account for the following?
All scandium salts are white.
How would you account for the following?
Chemistry of the actinoids is much more complicated than that of the lanthanoids.
The outer electronic configuration of two members of the lanthanoid series are as follows:
4f1 5d1 6s2 and 4f7 5d0 6s2.
What are their atomic numbers? Predict the oxidation states exhibited by these elements in their compounds.
Compare the chemistry of actinoids with that of the lanthanoids with special reference to atomic and ionic sizes.
Compare the chemistry of actinoids with that of the lanthanoids with special reference to oxidation state.
Nootan solutions for Chemistry Part 1 and 2 [English] Class 12 ISC 8 d-and ƒ-Block Elements VERY SHORT ANSWER TYPE QUESTIONS [Pages 495 - 496]
What are transition elements?
To which group of the periodic table do the transition elements belong?
Why are transition elements also called d-block elements
What are inner transition elements?
Name the d-subshells which successively get filled in the three series of transition elements.
Write the general electronic configuration of the elements belonging to the first transition series.
Write the electronic configuration of actinium.
Would you regard zinc, cadmium and mercury as transition elements?
How do the atomic radii of transition elements vary across a particular series?
What type of lattices are possessed by transition elements?
Among nickel (II) and platinum (II) compounds, which are more stable?
Among nickel (IV) and platinum (IV) compounds, which are more stable?
Write all the possible oxidation states of Cr.
Write the different oxidation states of manganese.
What is the most common oxidation state of the elements of first transition series?
What type of bonds are formed by transition elements in the +2 oxidation state?
What type of bonds are formed by transition elements in the +3 oxidation state?
What type of bonds are formed by transition elements in higher oxidation states?
In what type of compounds do the transition elements exhibit their highest oxidation states?
What is the highest oxidation state shown by a transition element?
Do transition elements form compounds in the oxidation state 0?
How is the stability of a particular oxidation state in aqueous medium of a transition element related to its standard electrode potential?
What type of transitions impart colour to the transition metal ions?
What is the colour of transition metal ions having completely filled and empty d-orbitals?
Give reasons for the following statement:
Transition metals and most of their compounds show paramagnetic behaviour.
What is the magnetic behaviour of cu+ ion?
Do transition metal ions undergo complex formation?
Write the general formulae of the oxides formed by first row transition elements.
What is the nature of oxides of first row transition elements formed in the lower oxidation states?
Give an example of spinel.
Write the ionic equation representing the oxidising nature of potassium dichromate.
Which ion can be detected by the chromyl chloride test?
How is the equivalent mass of potassium dichromate related to its molecular mass in acidic medium?
Name the mineral from which potassium permanganate is manufactured.
Write the ionic equation representing the oxidising nature of potassium permanganate in the neutral medium.
How is the equivalent mass of KMnO4 related to its molecular mass in acidic medium?
What is the most common oxidation state exhibited by the elements of the vanadium group?
How does the nature of the oxides of manganese vary with an increase in the oxidation state?
How many elements are present in the lanthanoid series?
How many elements are present in the actinoid series?
Write the general electronic configuration of lanthanoids.
Write the general electronic configuration of actinoids.
What is the most common oxidation state of actinoids?
Why is La3+ ion diamagnetic in nature?
What is the colour of La3+ ion.
What is the colour of Ce3+ ion?
What is the colour of Gd3+ ion?
What is the total contraction in atomic radius in going from Ce to Lu?
What factor is responsible for the abnormal increase in the densities of the elements of third transition series?
Do lanthanoids form complexes with π-bonding ligands?
Why are the ionisation potentials of the elements of third transition series higher than the expected ones?
With what type of ligands do lanthanoids form complexes?
What is Misch metal?
Write the general electronic configuration of actinoids.
What is the most common oxidation state exhibited by actinoids?
Which subshell does get filled in actinoids?
Among lanthanoids and actinoids, which have a higher tendency to form complexes?
What may be the stable oxidation state of the transition element with the following d electron configurations in the ground state of its atom?
3d3
What may be the stable oxidation state of the transition element with the following d electron configurations in the ground state of its atom?
3d5
What may be the stable oxidation state of the transition element with the following d electron configurations in the ground state of its atom?
3d8
What may be the stable oxidation state of the transition element with the following d electron configurations in the ground state of its atom?
3d4
Name the oxometal anions of the first series of the transition metals in which the metal exhibits the oxidation state equal to its group number.
Calculate the number of unpaired electrons in the following gaseous ions:
Mn3+, Cr3+, V3+ and Ti3+. Which one of these is the most stable in an aqueous solution?
Which metal in the first series of transition metals exhibits +1 oxidation state most frequently and why?
Write the electronic configurations of the element with the atomic number 61.
Write the electronic configuration of the element with the atomic number 91.
Write the electronic configuration of the element with the atomic number 101.
Write the electronic configurations of the element with the atomic number 109.
Nootan solutions for Chemistry Part 1 and 2 [English] Class 12 ISC 8 d-and ƒ-Block Elements SHORT ANSWER TYPE QUESTIONS [Pages 496 - 497]
What are the transition elements and why are they called so?
How are the transition elements classified?
Write the electronic configuration of the elements of the 3d-series.
Explain the exceptional electronic configuration of Cr.
Explain the exceptional electronic configuration of Cu.
Define transition elements.
Why Zn, Cd and Hg are not called transition metals?
Why do the atomic radii of transition elements decrease with increase in atomic number across a particular series?
Why does Cu have a greater atomic radius than that of Ni?
Why do transition elements exhibit metallic character?
Transition elements show high melting points. Why?
Why do transition elements have much higher boiling points?
Why is the increase in the first ionisation energy of transition elements not very regular with increase in atomic number?
Why are the ionisation potentials of the elements of third transition series higher than the expected ones?
Why are Ni (II) compounds more stable than Pt (II) compounds, but Ni (IV) compounds are less stable than Pt (IV) compounds?
How are E° values helpful in explaining the stability of transition metal ions in aqueous medium?
Give reasons:
Transition metals show variable oxidation states.
Give reasons for the following:
The transition metals generally form coloured compounds.
What are d-d transitions?
How do d-d transitions impart colour to transition metal ions?
Why is the Cu+ ion colourless?
Why is the Zn2+ ion colourless?
Why is the Sc3+ ion colourless?
Why is the Ti4+ ion colourless?
Explain the paramagnetic behaviour of transition metal ions.
Why do the elements present in the middle of a transition series exhibit the maximum paramagnetic behaviour?
Knowing the number of unpaired electrons, how would you calculate the magnetic moment of a transition metal ion?
Why does the presence of an unpaired electron make a transition metal ion paramagnetic?
Why do Sc3+ ions not show paramagnetic behaviour?
Account for the diamagnetic behaviour of Zn2+ ions.
Explain why transition metals and their compounds act as a catalyst.
Give a reason for the following:
Transition metals possess a great tendency to form complex compounds.
What are interstitial compounds and how are they formed by transition elements?
Account for the following:
Transition metals form alloys.
Write the general characteristics of first row transition metal halides.
What are the general characteristics of first row transition metal oxides?
Write the structure of Cu (II) chloride.
Write the chemical equations involving the preparation of K2Cr2O7 from chromite ore.
What happens when potassium dichromate is heated strongly?
What happens when potassium dichromate is treated with an alkali?
What happens when potassium dichromate is treated with acidified ferrous sulphate?
What happens when H2S is passed in an acidified solution of K2Cr2O7?
Write the ionic equation representing the oxidising nature of K2Cr2O7 in an acidic medium.
Calculate the equivalent mass of K2Cr2O7 in an acidic medium.
Describe the chromyl chloride test.
Draw the structure of the chromate ion.
Write the structures of the dichromate ion.
Describe the preparation of potassium permanganate from pyrolusite ore.
Write the ionic equation representing the oxidising nature of potassium permanganate in the neutral medium.
Write the ionic equations to represent the oxidising nature of KMnO4 in an acidic solution.
Write the ionic equations to represent the oxidising nature of KMnO4 in alkaline solution.
Why is KMnO4 capable of exhibiting oxidising properties in neutral, alkaline as well as in acidic solutions?
What is the action of heat on potassium permanganate?
What happens when KMnO4 is warmed gently with conc. H2SO4?
What happens when KMnO4 is treated with an aqueous solution of MnSO4?
What happens when KMnO4 is treated with Kl?
What happens when KMnO4 is treated with an acidified solution of oxalic acid?
What is the action of KMnO4 in an acidic medium on the following?
H2S
Write a balanced equation.
What is the action of KMnO4 in an acidic medium on the following?
SO2
Write a balanced equation.
What is the action of KMnO4 in an acidic medium on the following?
Na2SO3
Write a balanced equation.
What is the action of KMnO4 in an acidic medium on the following?
HCl
Write a balanced equation.
What is the action of KMnO4 in an acidic medium on the following?
CH3CH2OH
Write a balanced equation.
Why is KMnO4 used for sterilizing wells of drinking water?
Write the general characteristics of the elements of group 7.
What are platinum metals?
Write the common oxidation state of platinum metals.
What are ferrous metals?
Write the common oxidation state of ferrous metals.
What are coinage metals?
Write the general characteristics of coinage metals.
What are inner transition elements?
How are inner transition elements classified?
What are the names, symbols and atomic numbers of all lanthanoids?
Why are the electronic configurations of lanthanoids not known with certainty?
Why does praseodymium possess electronic configuration 4f3 6s2 instead of the expected one, 4f2 5d1 6s2?
Why do lanthanoids exhibit variable oxidation states?
Why do lanthanoid ions having the same number of unpaired electrons have different values of magnetic moments?
Which type of transitions are responsible for the colour of lanthanoid cations?
What is Lanthanoid contraction?
How do lanthanoid contraction affect the following property of the elements placed after lanthanoids?
Atomic and ionic radii.
How do lanthanoid contraction affect the following property of the elements placed after lanthanoids?
Basicity of oxides.
How do lanthanoid contraction affect the following property of the elements placed after lanthanoids?
Densities.
Write any two consequences of Lanthanoid Contraction.
Why do lanthanoids not possess much tendency to form complexes?
Write the composition of misch metal.
Write the composition of pyrophoric alloys.
Mention the important uses of misch metal.
Mention the important uses of pyrophoric alloys.
Write the names, symbols and electronic configuration of the elements having atomic numbers 89-93.
Write the most stable oxidation states of all the actinoids.
What are actinoids and why are they called so?
Discuss the main points of similarity between lanthanoids and actinoids.
Distinguish between lanthanoid and actinoids.
Write two uses of lanthanoids.
Write any two uses of actinides.
In neutral or faintly alkaline solution, 8 moles of permanganate anion quantitatively oxidize thiosulphate anions to produce X moles of a sulphur containing product. Find the magnitude of X.
Nootan solutions for Chemistry Part 1 and 2 [English] Class 12 ISC 8 d-and ƒ-Block Elements LONG ANSWER TYPE QUESTIONS [Pages 497 - 498]
What are transition elements?
How are the transition elements classified?
Discuss the important physico-chemical characteristics of transition elements.
Discuss the following property with respect to transition elements:
Melting and boiling points.
Discuss the following property with respect to transition elements:
Ionisation energies.
Discuss the following property with respect to transition elements:
Oxidation states.
Discuss the following property with respect to transition elements:
Magnetic behaviour.
Discuss the following property with respect to transition elements:
Colour of ions.
Give reasons:
Transition metals show variable oxidation states.
Write the oxidation state of the elements of first transition series. What conclusion may be drawn from these oxidation states?
Why do the transition elements have higher enthalpies of atomisation?
How would you account for the following: Transition metals form complex compounds.
Give reasons for the following:
Most of the compounds formed by transition elements are coloured.
Give reasons for the following:
Many of the transition metals and their compounds act as catalysts.
Give reasons for the following statement:
Transition metals and most of their compounds show paramagnetic behaviour.
Discuss the nature of oxides of first row transition elements.
Discuss the nature of halides of first row transition elements.
Discuss the nature of sulphides of first row transition elements.
Describe with the help of chemical equations, the preparation of potassium dichromate from chromite ore.
Write a note on the chromyl chloride test.
Describe the preparation of potassium permanganate from pyrolusite ore.
How do the potassium permanganate salt react towards heat?
How does the potassium permanganate salt react towards conc. H2SO4?
How does the potassium permanganate salt react towards hydrogen peroxide?
Discuss in detail the oxidising character of potassium permanganate in neutral solutions. Give at least two reactions in the given case.
Discuss in detail the oxidising character of potassium permanganate in alkaline solutions. Give at least two reactions in the given case.
Discuss in detail the oxidising character of potassium permanganate in acidic solutions. Give at least two reactions in the given case.
Mention some important uses of the potassium permanganate salt.
What are inner transition elements?
How are inner transition elements classified?
Discuss the occurrence of the inner transition elements in nature.
Write the electronic configuration of inner transition elements.
What are lanthanoids?
Write the electronic configuration of lanthanoids and give suitable explanations for them.
What are the different oxidation states exhibited by the lanthanoids?
Discuss the stability of lanthanoids in aqueous solutions.
Distinguish between lanthanoid and actinoids.
Explain the magnetic behaviour exhibited by the tripositive lanthanoid ions.
Why is the magnetic behaviour of the tripositive lanthanoid ions not a linear function of the number of unpaired electrons present in them?
Explain why most of the tripositive ions of lanthanoids are coloured.
What are f-f transitions?
What is Lanthanoid contraction?
What are the causes of lanthanide contraction?
Write any two consequences of Lanthanoid Contraction.
What are actinoids? Give three examples.
Write the names and electronic configuration of actinoids.
Discuss the important characteristics of actinoids.
What are actinoids? Give three examples.
Discuss the main points of similarity between lanthanoids and actinoids.
Distinguish between lanthanoid and actinoids.
Write two uses of lanthanoids.
Write any two uses of actinides.
Nootan solutions for Chemistry Part 1 and 2 [English] Class 12 ISC 8 d-and ƒ-Block Elements OBJECTIVE (MULTIPLE CHOICE) TYPE QUESTIONS [Pages 498 - 503]
Choose the correct option in the following questions.
Transition elements belong to ______.
s-block
p-block
d-block
f-block
The general electronic configuration of transition elements is ______.
`(n - 1) d^{1 - 5)`
`(n - 1) d^(1 - 10) ns^1`
`(n - 1) d^(1 - 10) ns^2`
none
The number of d-electrons in Fe2+ (At.no. of Fe = 26) is ______.
2
4
6
8
Which of the following has the maximum number of unpaired electrons?
Zn
Fe2+
Ni3+
Cu+
Which of the following shows oxidation state of +8?
Ir
Pt
Rh
Os
A metal ion from the first transition series has a magnetic moment (calculated) of 3.87 BM. The number of unpaired electrons present in the ion is ______.
1
2
3
4
The number of unpaired electrons in Ni2+ is ______.
0
2
4
8
The ions of d-block elements show colour because ______.
they absorb some energy for d-s transition.
they absorb some energy for p-d transition.
they absorb some energy for d-d transition.
they do not absorb any energy.
The maximum oxidation state of osmium is ______.
+6
+7
+8
+5
Which of the following oxides of chromium is amphoteric in nature?
CrO
Cr2O3
CrO3
CrO5
Which of the following metals is used in incandescent lamps?
Fe
Mo
Zr
W
The number of moles of KMnO4 that will be needed to react with one mole of sulphide ion in acidic solution is ______.
`2/5`
`3/5`
`4/5`
1
The lanthanoid contraction is responsible for the fact that ______.
Zr and Y have about the same radius.
Zr and Nb have smaller oxidation state.
Zr and Hf have about the same radius.
Zr and Zn have the same oxidation state.
Which of the following elements involve gradual filling of 5f-level?
Lanthanoids
Actinoids
Transition metals
Coinage metals
The equivalent mass of K2Cr2O7 in acidic medium is equal to ______.
molecular mass
`1/2` × molecular mass
`1/5` × molecular mass
`1/6` × molecular mass
Which transition metal is used as a catalyst in the manufacture of vegetable ghee?
Fe
Cr
Co
Ni
Which lanthanoid is most commonly used?
Lanthanum
Neodymium
Terbium
Cerium
The electronic configuration of gadolinium (Atomic number 64) is ______.
[Xe] 4f3 5d5 6s2
[Xe] 4f7 5d2 6s1
[Xe] 4f7 5d1 6s2
[Xe] 4f8 5d6 6s2
[Xe] 4f8 5d9 6s2
[Xe] 4f6 5d2 6s2
Which metal has the lowest melting point?
Cs
Hg
Mn
Cu
Which of the following ions is expected to have the highest magnetic moment?
Zn2+
Ti3+
Sc3+
Mn2+
Which of the following is paramagnetic?
Cu2+
Ag+
Zn2+
Au+
Stainless steel contains mainly iron and carbon along with ______.
Co and Mn
Mn and Ni
Cr and Co
Ni and Cr
Addition of high proportions of manganese makes steel useful in making rail tracks because manganese ______.
gives hardness to steel.
helps the formation of oxides of iron.
can remove oxygen and sulphur.
can show highest oxidation state of + 7.
In the dichromate dianion ______.
4 Cr-O bonds are equivalent.
6 Cr-O bonds are equivalent.
all Cr-O bonds are equivalent.
all Cr-O bonds are non-equivalent.
Among the following, identify the species with an atom in +6 oxidation state.
\[\ce{MnO^-_4}\]
\[\ce{Cr(CN)^3-_6}\]
\[\ce{NiF^{2-}6}\]
CrO2Cl2
The least pure commercial form of iron is ______.
cast ion
wrought iron
steel
haematite
The temperature in the slag formation zone in the blast furnace is ______.
1775-2000K
875-1075 K
1075-1475 K
1075-975 K
The steel used for making rock drills and safes is ______.
stainless steel
nickel steel
invar
manganese steel
When iron is treated with moderately conc. HNO3, the gas evolved is ______.
H2
NH3
NO
NO2
The chemical composition of rust is ______.
Fe2O3.xH2O
Fe3O4.xH2O
FeO.xH2O
Fe3O4
Chlorargyrite is an ore of ______.
Cu
Ag
Au
Fe
‘915 fine silver’ consists of ______.
9.15% silver
91.5% silver
100% silver
0% silver
Which of the following is an ore of copper?
Pyrargyrite
Sylvine
Siderite
Azurite
The metallurgy of copper involves ______.
self-reduction process
carbon reduction process
elecrolytic reduction process
hydrometallurgical process
The molten metal obtained from Bessemer converter in the metallurgy of copper is called blister copper. It ______.
is 100% pure copper.
is about 50% pure copper.
consists of blisters due to the liberation of dissolved air.
consists of blisters due to the liberation of dissolved SO2.
When copper is exposed to moist air, its surface is coated with a green layer of ______.
verdigris, CuCO3.Cu(OH)2 only
bronchanite, CuSO4.3Cu(OH)2 only
atacamite, CuCl2.3Cu(OH)2 only
all of the above
The percentage of silver in German silver is ______.
0%
10%
50%
100%
Dental amalgam used for filling teeth consists of ______.
Ag and Hg
Au and Hg
Au, Sn and Hg
Ag, Sn and Hg
This question contains Statement-1 and Statement-2. Of the four choices given after the statements, choose the one that best describes the two statements.
Statement 1: Zn2+ is diamagnetic.
Statement 2: Two electrons are lost from 4s orbital to form Zn2+.
Statement-1 is false, Statement-2 is true.
Statement-1 is true, Statement-2 is true; Statement-2 is a correct explanation for Statement-1.
Statement-1 is true, Statement-2 is true; Statement-2 is not a correct explanation for Statement-1.
Statement-1 is true, Statement-2 is false.
Which of the following statements is not correct when a mixture of NaCl and K2Cr2O7 is gently warmed with conc. H2SO4?
A deep red vapour is evolved.
The vapour when passed into NaOH solution gives a yellow solution of Na2CrO4.
Chlorine gas is evolved.
Chromyl chloride is formed.
In the dichromate dianion, the Cr-O-Cr bond angle is ______.
90°
120°
126°
131°
The chemical processes in the production of steel from haematite ore involve ______.
reduction
oxidation
reduction followed by oxidation
oxidation followed by reduction
Among the following, identify the species with an atom in +6 oxidation state.
\[\ce{MnO^-_4}\]
\[\ce{Cr(CN)^3-_6}\]
\[\ce{NiF^{2-}6}\]
CrO2Cl2
The chemical composition of slag formed during the smelting process in the extraction of copper is ______.
Cu2O + FeS
FeSiO3
CuFeS2
Cu2S + FeO
In the standardisation of Na2S2O3 using K2Cr2O7 by iodometry, the equivalent weight of K2Cr2O7 is ______.
(molecular weight)/2
(molecular weight)/6
(molecular weight)/3
same as molecular weight
Which of the following ions has the maximum magnetic moment?
Mn2+
Fe2+
Ti2+
Cr2+
Most common oxidation states of Ce (Cerium) are ______.
+3, +4
+2, +3
+2, +4
+3, +5
Ce3+, La3+, Pm3+ and Yb3+ have ionic radii in the increasing order as ______.
La3+ < Ce3+ < Pm3+ < Yb3+
Yb3+ < Pm3+ < Ce3+ < La3+
La3+ = Ce3+ < Pm3+ < Yb3+
Yb3+ < Pm3+ < La3+ < Ce3+
The number of d-electrons retained in Fe2+ (At. no. Fe = 26) ion is ______.
3
4
5
6
The radius of La3+ (Atomic number of La = 57) is 1.06 Å. Which one of the following given values will be closest to the radius of Lu3+ (Atomic number of Lu = 71)?
1.60 Å
1.40 Å
1.06 Å
0.85 Å
Of the following outer electronic configuration of atoms, the highest oxidation state is achieved by which one of them?
(n − 1) d8 ns2
(n − 1) d5 ns1
(n − 1) d3 ns2
(n − 1) d5 ns2
Cerium (Z = 58) is an important member of the lanthanoids. Which of the following statements about Cerium is incorrect?
The common oxidation states of cerium are + 3 and + 4.
The +3 oxidation state of cerium is more stable than the +4 oxidation state.
The +4 oxidation state of cerium is not known in solutions.
Cerium (IV) acts as an oxidising agent.
During the process of electrolytic refining of copper, some metals present as impurity settle as anode mud. These are ______.
Fe and Ni
Ag and Au
Pb and Zn
Se and Ag
The lanthanoid contraction is responsible for the fact that ______.
Zr and Y have about the same radius.
Zr and Nb have smaller oxidation state.
Zr and Hf have about the same radius.
Zr and Zn have the same oxidation state.
The ‘spin-only’ magnetic moment [in units of Bohr magneton, (µβ)] of Ni2+ in aqueous solution would be ______. (Atomic number of Ni = 28)
2.84
4.90
0
1.73
Lanthanoid contraction is caused due to ______.
the appreciable shielding on outer electrons by 4f-electrons from the nuclear charge.
the appreciable shielding on outer electrons by 5d-electrons from the nuclear charge.
the same effective nuclear charge from Ce to Lu.
the imperfect shielding on outer electrons by 4f-electrons from the nuclear charge.
The incorrect statement among the following is:
d-block elements show irregular and erratic chemical properties.
La and Cu have partially filled d-orbitals and no other partially filled orbitals.
The chemistry of various lanthanoids is very similar
4f and 5f orbitals are equally shielded
The actinoids exhibit more number of oxidation states in general than the lanthanoids. This is because ______.
the 5f-orbitals are more buried than the 4f-orbitals
there is a similarity between 4f and 5f-orbitals in their angular part of the wave function.
the actinoids are more reactive than the lanthanoids.
the 5f-orbitals extend farther from the nucleus than the 4f-orbitals.
Which of the following ions will exhibit colour in aqueous solution?
La3+ (Z = 57)
Ti3+ (Z = 22)
Lu3+ (Z = 71)
Se3+ (Z = 21)
Which one of the following ions has electronic configuration [Ar] 3d6?
(At. no.: Mn = 25, Fe = 26, Co = 27, Ni = 28)
Ni3+
Mn3+
Fe3+
Co3+
Which of the following pairs has the same size?
Fe2+, Ni2+
Zr4+, Ti4+
Zr4+, Hf4+
Zn2+, Hf4+
For the four successive transition elements (Cr, Mn, Fe and Co), the stability of +2 oxidation state will be there in which of the following order?
(At. no.: Cr = 24, Mn = 25, Fe = 26, Co = 27)
Fe > Mn > Co > Cr
Co > Mn > Fe > Cr
Cr > Mn > Co > Fe
Mn > Fe > Cr > Co
Which of the following elements is present as the impurity to the maximum extent in the pig iron?
Carbon
Silicon
Phosphorus
Manganese
Acidified K2Cr2O7 solution turns green when Na2SO3 is added to it. This is due to the formation of ______.
\[\ce{CrO^{2-}_4}\]
Cr2(SO3)3
CrSO4
Cr2(SO4)3
Aluminium is extracted from alumina (Al2O3) by electrolysis of a molten mixture of ______.
Al2O3 + HF + NaAIF4
Al2O3 + CaF2 + NaAIF4
Al2O3 + Na3AIF6 + CaF2
Al2O3 + KF + Na3AIF5
In the extraction of copper from its sulphide ore, the metal is finally obtained by the reduction of cuprous oxide with ______.
copper (I) sulphide (Cu2S)
sulphur dioxide (SO2)
iron sulphide (FeS)
carbon monoxide (CO)
Identify the alloy containing a non-metal as a constituent in it.
invar
steel
bell metal
bronze
Which of the following statements is not true?
on passing H2S, through acidified K2Cr2O7 solution, a milky colour is observed.
Na2Cr2O7 is preferred over K2Cr2O7 in volumetric analysis.
K2Cr2O7 solution in acidic medium is orange in colour.
K2Cr2O7 solution becomes yellow on increasing the pH beyond 7.
In acidic medium, H2O2 changes \[\ce{Cr2O^{2-}_7}\] to CrO5 which has two (-O-O-) bonds. Oxidation state of Cr in CrO5 is ______.
+5
+3
+6
−10
The reaction of aqueous KMnO4 with H2O2 in acidic conditions gives ______.
Mn4+ and O2
Mn2+ and O2
Mn2+ and O3
Mn4+ and MnO2
Reason of lanthanoid contraction is ______.
negligible screening effect of ‘f’ orbitals.
increasing nuclear charge.
decreasing nuclear charge.
decreasing screening effect.
Which of the following arrangements does not represent the correct order of the property stated against it?
V2+ < Cr2+ < Mn2+ < Fe2+: paramagnetic behaviour
Ni2+ < Co2+ < Fe2+ < Mn2+: ionic size
Co3+ < Fe3+ < Cr3+ < Sc3+: stability in aqueous solution
Sc < Ti < Cr < Mn: number of oxidation states
Four successive members of the first row transition elements listed below with atomic numbers. Which one of them is expected to have the highest \[\ce{E^{\circ}_{M^{3+}/M^{2+}}}\] value?
Cr (Z = 24)
Mn (Z = 25)
Fe (Z = 26)
Co (Z = 27)
Which series of reactions correctly represent chemical relations related to iron and its compound?
\[\ce{Fe ->[Dil. H2SO4] FeSO4 ->[H2SO4, O2] Fe2(SO4)3 ->[Heat] Fe}\]
\[\ce{Fe ->[O2, heat] FeO ->[dil. H2SO4] FeSO4 ->[Heat] Fe}\]
\[\ce{Fe ->[Cl2, heat] FeCl3 ->[Heat, air] FeCl2 ->[Zn] Fe}\]
\[\ce{Fe ->[O2, heat] Fe3O4 ->[CO, 600^\circ] FeO ->[CO, 700^\circ] Fe}\]
The colour of KMnO4 is due to ______.
M → L charge transfer transition
d-d trannsition
L → M charge transfer transition
σ-σ* transition
The correct statement(s) about Cr2+ and Mn3+ is(are):
[Atomic numbers of Cr = 24 and Mn = 25]
Cr2+ is a reducing agent.
Mn3+ is an oxidizing agent.
both Cr2+ and Mn3+ exhibit d4 electronic configuration.
when Cr2+ is used as a reducing agent, the chromium ion attains d5 electronic configuration.
Fe3+ is reduced to Fe2+ by using ______.
H2O2 in presence of NaOH
Na2O2 in water
H2O2 in presence of H2SO4
Na2O2 in presence of H2SO4
Which of the following compounds is metallic and ferromagnetic?
TiO2
CrO2
VO2
MnO2
Which one of the following statements is correct when SO2 is passed through acidified K2Cr2O7 solution?
The solution turns blue.
The solution is decolourized.
SO2 is reduced.
Green Cr2(SO4)3 is formed.
The electronic configuration of Eu (Atomic no. 63) Gd (Atomic no. 64) and Tb (Atomic no. 65) are:
[Xe] 4f6 5d1 6s2, [Xe] 4f7 5d1 6s2 and [Xe] 4f8 5d1 6s2
[Xe] 4f7 6s2, [Xe] 4f7 5d1 6s2 and [Xe] 4f9 6s2
[Xe] 4f7 6s2, [Xe] 4f8 6s2 and [Xe] 4f8 5d1 6s2
[Xe] 4f6 5d1 6s2, [Xe] 4f7 5d1 6s2 and [Xe] 4f9 6s2
The reason for greater range of oxidation states in actinoids is attributed to ______.
the radioactive nature of actinoids.
actinoid contraction.
5f, 6d and 7s levels having comparable energies.
4f and 5d levels being close in energies.
Hydrogen peroxide oxidises [Fe(CN)6]4− to [Fe(CN)6]3− in acidic medium but reduces [Fe(CN)6]3− to [Fe(CN)6]4− in alkaline medium. The other products formed respectively are:
(H2O + O2) and H2O
(H2O + O2) and (H2O + OH−)
H2O and (H2O + O2)
H2O and (H2O + O−)
The oxidation states of Cr in [Cr(H2O6]Cl3, [Cr(C6H6)2] and K2[Cr(CN)2(O)2(O2) (NH3)] respectively are ______.
+3, +4 and +6
+3, +2 and +4
+3, 0 and +6
+3, 0 and +4
Match the metal ions given in Column I with the spin magnetic moments of the ions given in Column 11 and assign the correct code:
| Column I | Column II | ||
| 1. | CO3+ | i. | `sqrt 8` BM |
| 2. | Cr3+ | ii. | `sqrt 35` BM |
| 3. | Fe3+ | iii. | `sqrt 3` BM |
| 4. | Ni2+ | iv. | `sqrt 24` BM |
| v. | `sqrt 15` BM |
1 2 3 4 iv i ii iii 1 2 3 4 i ii iii iv 1 2 3 4 iv v ii i 1 2 3 4 iii v i ii
Which one of the following ions exhibits d-d transition and paramagnetism as well?
\[\ce{MnO^-_4}\]
\[\ce{Cr2O^{2-}_7}\]
\[\ce{CrO^{2-}_4}\]
\[\ce{MnO^{2-}_4}\]
Consider the hydrated ions of Ti2+, V2+, Ti3+ and Sc3+. The correct order of their spin-only magnetic moments is ______.
Sc3+ < Ti3+ < V2+ < Ti2+
Sc3+ < Ti3+ < Ti2+ < V2+
Ti3+ < Ti2+ < Sc3+ < V2+
V2+ < Ti2+ < Ti3+ < Sc3+
The highest possible oxidation states of uranium and plutonium, respectively are ______.
4 and 6
6 and 4
7 and 6
6 and 7
The correct order of the first ionization enthalpies is ______.
Ti < Mn < Zn < N
Zn < Ni < Mn < Ti
Mn < Ti < Zn < Ni
Ti < Mn < Ni < Zn
Given
\[\ce{CO^{3+} + e- -> CO^{2+}}\]; E° = +1.81 V
\[\ce{Pb^{4+} + 2e- -> Pb^{2+}}\]; E° = +1.67 V
\[\ce{Ce^{4+} + e- -> Ce^{3+}}\]; E° = +1.61 V
\[\ce{Bi^{3+} + 3e- -> Bi^}\]; E° = +0.20 V
Oxidizing power of the species will increase in the order:
Co3+ < Ce4+ < Bi3+ < Pb4+
Co3+ < Pb4+ < Ce4+ < Bi3+
Ce4+ < Pb4+ < Bi3+ < Co3+
Bi3+ < Ce4+ < Pb4+ < Co3+
The metal that gives hydrogen gas upon treatment with both acid as well as base is ______.
mercury
zinc
iron
magnesium
Match the catalyst with the process:
| Catalyst | Process | ||
| (i) | V2O5 | (a) | The oxidation of ethyne to ethanal |
| (ii) | TiCl4 + Al(CH3)3 | (b) | Polymerisation of alkynes |
| (iii) | PdCl2 | (c) | Oxidation of SO2 in the manufacture of H2SO4 |
| (iv) | Nickel complexes | (d) | Polymerisation of ethylene |
Which of the following is the correct option?
(i)-(c), (ii)-(a), (iii)-(d), (iv)-(b)
(i)-(c), (ii)-(d), (iii)-(a), (iv)-(b)
(i)-(a), (ii)-(b), (iii)-(c), (iv)-(d)
(i)-(a), (ii)-(c), (iii)-(b), (iv)-(d)
When neutral or faintly alkaline KMnO4 is treated with potassium iodide, iodide ion is converted into ‘X’. ‘X’ is:
IO−
I2
\[\ce{IO^-_4}\]
\[\ce{IO^-_3}\]
The oxidation state of Cr in CrO6 is ______.
+4
−6
+12
+6
The manganate and permanganate ions are tetrahedral due to ______.
The π-bonding involves overlap of p-orbitals of oxygen with d-orbitals of manganese.
There is no π-bonding.
The π-bonding involves overlap of p-orbitals of oxygen with p-orbitals of manganese.
The π-bonding involves overlap of d-orbitals of oxygen with d-orbitals of manganese.
The calculated spin only magnetic moment of Cr2+ ion is ______.
3.87 BM
4.90 BM
5.92 BM
2.84 BM
The number of protons, neutrons and electrons in \[\ce{^175_71Lu}\], respectively, are ______.
71, 104 and 71
104, 71 and 71
71, 71 and 104
175, 104 and 71
Identify the incorrect statement.
Cr2+(d4) is a stronger reducing agent than Fe2+(d6) in water.
The transition metals and their compounds are known for their catalytic activity due to their ability to adopt multiple oxidation states and to form complexes.
Interstitial compounds are those that are formed when small atoms like H, C or N are trapped inside the crystal lattices of metals.
The oxidation states of chromium in \[\ce{CrO^{2-}_4}\] and \[\ce{Cr2O^{2-}_7}\] are not the same.
The incorrect statement (s) among (a)-(c) is (are):
- W(VI) is more stable than Cr(VI).
- In the presence of HCl, permanganate titrations provide satisfactory results.
- Some lanthanoid oxides can be used as phosphorus.
(a) only
(b) and (c) only
(b) only
(a) and (b) only
In the sixth period, the orbitals that are filled are ______.
6s, 5f, 6d, 6p
6s, 5d, 5f, 6p
6s, 6p, 6d, 6f
6s, 4f, 5d, 6p
The correct electronic configuration and spin-only magnetic moment (BM) of Gd3+(Z = 64), respectively, are ______.
[Xe] 5f7 and 7.9
[Xe] 5f7 and 8.9
[Xe] 4f7 and 7.9
[Xe] 4f7 and 8.9
Zr (Z = 40) and Hf (Z = 72) have similar atomic and ionic radii because of ______.
Having similar chemical properties
Belonging to same group
Diagonal relationship
Lanthanoid contraction
The incorrect statement among the following is:
Actinoids are highly reactive metals, especially when finely divided.
Actinoid contraction is greater for element to element than lanthanoid contraction.
Most of the trivalent lanthanoid ions are colourless in the solid state.
Lanthanoids are good conductors of heat and electricity.
Given below are two statements: One is labelled as Assertion A and the other is labelled as Reason R:
Assertion A: Size of Bk3+ ion is less than Np3+ ion.
Reason R: The above is a consequence of the lanthanoid contraction.
In the light of the above statements, choose the correct answer from the options given below.
A is false but R is true.
Both A and R are true but R is not the correct explanation of A.
A is true but R is false.
Both A and R are true and R is the correct explanation of A.
Given below are two statements:
Statement I: The E° value for \[\ce{\frac{Ce^{4+}}{Ce^{3+}}}\] is +1.74 V.
Statement II: Ce is more stable in Ce4+ state than Ce3+ state.
In the light of the above statements, choose the correct answer from the options given below:
Both Statement I and Statement II are correct.
Statement I is incorrect but statement II is correct.
Both Statement I and Statement II are incorrect.
Statement I is correct but statement II is incorrect.
Given below are two statements:
Statement I: Potassium permanganate on heating at 573K forms potassium manganate.
Statement II: Both potassium permanganate and potassium manganate are tetrahedral and paramagnetic in nature.
In the light of the above statements, choose the most appropriate answer from the options given below.
Statement I is true but statement II is false.
Both statement I and statement II are true.
Statement I is false but statement II is true.
Both statement I and statement II are false.
The common positive oxidation states for an element with atomic number 24, are ______.
+2 to +6
+1 and +3 to +6
+1 and +3
+1 to +6
In the neutral or faintly alkaline medium, KMnO4 oxidises iodide into iodate. The change in oxidation state of manganese in this reaction is from ______.
+6 to +4
+7 to +3
+6 to +5
+7 to +4
Match List-I with List II.
| List I (ores) | List II (composition) | ||
| (i) | Haematite | (A) | Fe3O4 |
| (ii) | Magnetite | (B) | ZnCO3 |
| (iii) | Calamine | (C) | Fe2O3 |
| (iv) | Kaolinite | (D) | [Al2(OH)4 Si2O5] |
Choose the correct answer from the options given below:
(i) - (C), (ii) - (A), (iii) - (B), (iv) - (D)
(i) - (C), (ii) - (A), (iii) - (D), (iv) - (B)
(i) - (A), (ii) - (C), (iii) - (B), (iv) - (D)
(i) - (A), (ii) - (B), (iii) - (C), (iv) - (D)
Gadolinium has a low value of third ionisation enthalpy because of ______.
high exchange enthalpy
high electronegativity
high basic character
small size
Cerium (IV) has a noble gas configuration. Which of the following is a correct statement about it?
It will not prefer to undergo redox reactions.
It will prefer to gain electron and act as an oxidizing agent.
It will prefer to give away an electron and behave as reducing agent.
It acts as both oxidizing and reducing agent.
Among the following which is the strongest oxidizing agent?
Mn+3
Fe+3
Ti+3
Cr+3
The most common oxidation state of lanthanoid elements is +3. Which of the following is likely to deviate easily from +3 oxidation state?
Ce (At. no. 58)
La (At. no. 51)
Lu (At. no. 71)
Gd (At. no. 64)
The f-orbitals are half and completely filled respectively in lanthanide ions:
(Given: Atomic no. Eu = 63, Sm = 62, Tm = 69, Tb = 65, Yb = 70, Dy = 66)
Eu+2 and Tm+2
Sm+2 and Tm+2
Tb+4 and Yb+2
Dy+2 and Yb+2
Which one of the lanthanoids given below is the most stable in divalent form?
Ce (Z = 58)
Sm (Z = 62)
Eu (Z = 63)
Yb (Z = 70)
Nootan solutions for Chemistry Part 1 and 2 [English] Class 12 ISC 8 d-and ƒ-Block Elements FILL IN THE BLANKS TYPE QUESTIONS [Pages 504 - 505]
The d-block elements show a transitional behaviour between that of the elements of ______ block and ______ block.
The third transition series involves the filling of ______ subshell.
The electronic configuration of lanthanum (At. no. 57) is [Xe] ______.
Copper can be regarded as a transition element in ______ oxidation state.
The atomic radii of transition elements belonging to a particular series ______ with increase in atomic number.
The transition metals have ______ and ______ lattices which are characteristic of the ______.
On moving across a transition series, the melting points first ______, attain a ______ value and then ______.
The ionisation energies of transition elements lie between those of ______ block and ______ block elements.
The oxidation state for which E° value is more ______ will be more stable in aqueous medium.
The highest oxidation state shown by Mn is ______.
The bonds formed by transition metals in lower oxidation states are ______ while those formed in higher oxidation states are ______.
The colour of transition metal ions is due to ______ transitions.
The transition metals ions having completely filled d-orbitals are ______ and ______.
The magnitude of magnetic moment of a transition metal ion depends upon the number of ______ electrons present in it.
V2O5 is used as a catalyst in the manufacture of ______.
CuO is ______ in nature, whereas Cu2O is ______ in nature.
Fe3O4 may be regarded as a mixture of ______ and ______.
TiCl4 on hydrolysis gives ______ and ______.
\[\ce{Cr2O^{2-}_7 + 14H+ + 6e- -> 2}\]______ + 7H2O
The colour of chromyl chloride vapours is ______.
\[\ce{Cr2O^{2-}_7}\] ions possess ______ equivalent Cr-O bonds.
In neutral solution, equivalent mass of KMnO4 is ______ of its molecular mass.
\[\ce{MnO^-_4 + 2H2O + 3e- ->}\] ______ + 4OH−
In alkaline solution, KMnO4 oxidises KI to ______ but in acidic solution it oxidises KI to ______.
The transition metal used for making analytical weights is ______.
The elements of group 11 are also called ______ metals.
The paramagnetism of lanthanoids is due to both ______ and ______.
The basicity of oxides and hydroxides of lanthanoids decreases with increase in atomic number due to ______.
The exceptionally higher densities of the elements of the third transition series are due to ______.
The predominant oxidation state of actinoids is ______.
Nootan solutions for Chemistry Part 1 and 2 [English] Class 12 ISC 8 d-and ƒ-Block Elements ASSERTION-REASON TYPE QUESTIONS [Page 505]
Assertion: Zn, Cd and Hg cannot be regarded as transition elements.
Reason: These elements do not belong to the d-block of the periodic table.
If both Assertion and Reason are CORRECT and Reason is the CORRECT explanation of the Assertion.
If both Assertion and Reason are CORRECT but Reason is not the CORRECT explanation of the Assertion.
If Assertion is CORRECT but Reason is INCORRECT.
If Assertion is INCORRECT but Reason is CORRECT.
Assertion: When a solution of sodium argentocyanide is treated with scrap zinc, silver gets precipitated.
Reason: Zinc is more electropositive than silver.
If both Assertion and Reason are CORRECT and Reason is the CORRECT explanation of the Assertion.
If both Assertion and Reason are CORRECT but Reason is not the CORRECT explanation of the Assertion.
If Assertion is CORRECT but Reason is INCORRECT.
If Assertion is INCORRECT but Reason is CORRECT.
Assertion: Zn2+ ion is diamagnetic.
Reason: The electrons are lost from 4s-orbital to form Zn2+ ion.
If both Assertion and Reason are CORRECT and Reason is the CORRECT explanation of the Assertion.
If both Assertion and Reason are CORRECT but Reason is not the CORRECT explanation of the Assertion.
If Assertion is CORRECT but Reason is INCORRECT.
If Assertion is INCORRECT but Reason is CORRECT.
Assertion: The pair of elements Zr-Hf, Nb-Ta, Mo-W, ..., Pd-Pt, Ag-Au possess almost the same values of atomic radii.
Reason: The occurrence of lanthanoid contraction cancels the expected increase in the atomic radii values from Hf to Hg.
If both Assertion and Reason are CORRECT and Reason is the CORRECT explanation of the Assertion.
If both Assertion and Reason are CORRECT but Reason is not the CORRECT explanation of the Assertion.
If Assertion is CORRECT but Reason is INCORRECT.
If Assertion is INCORRECT but Reason is CORRECT.
Assertion: The most common oxidation state exhibited by actinoids is +2.
Reason: All actinoids possess two electrons in 7s subshell.
If both Assertion and Reason are CORRECT and Reason is the CORRECT explanation of the Assertion.
If both Assertion and Reason are CORRECT but Reason is not the CORRECT explanation of the Assertion.
If Assertion is CORRECT but Reason is INCORRECT.
If Assertion is INCORRECT but Reason is CORRECT.
Assertion: The basic strength of oxides and hydroxides of lanthanoids decrease with increase in atomic number.
Reason: The size of cation of lanthanoids increases with increase in atomic number.
If both Assertion and Reason are CORRECT and Reason is the CORRECT explanation of the Assertion.
If both Assertion and Reason are CORRECT but Reason is not the CORRECT explanation of the Assertion.
If Assertion is CORRECT but Reason is INCORRECT.
If Assertion is INCORRECT but Reason is CORRECT.
Nootan solutions for Chemistry Part 1 and 2 [English] Class 12 ISC 8 d-and ƒ-Block Elements 'NCERT TEXT-BOOK, Exercises [Pages 505 - 508]
Write down the electronic configuration of Cr3+.
Write down the electronic configuration of Pm3+.
Write down the electronic configuration of Cu+.
Write down the electronic configuration of Ce4+.
Write down the electronic configuration of Co2+.
Write down the electronic configuration of Lu2+.
Write down the electronic configuration of Mn2+.
Write down the electronic configuration of Th4+.
Why are Mn2+ compounds more stable than Fe2+ towards oxidation to their +3 state?
Explain briefly how +2 state becomes more and more stable in the first half of the first row transition elements with increasing atomic number?
To what extent do the electronic configurations decide the stability of oxidation states in the first series of the transition elements? Illustrate your answer with examples.
What may be the stable oxidation state of the transition element with the following d electron configurations in the ground state of its atom?
3d3
What may be the stable oxidation state of the transition element with the following d electron configurations in the ground state of its atom?
3d5
What may be the stable oxidation state of the transition element with the following d electron configurations in the ground state of its atom?
3d8
What may be the stable oxidation state of the transition element with the following d electron configurations in the ground state of its atom?
3d4
Name the oxometal anions of the first series of the transition metals in which the metal exhibits the oxidation state equal to its group number.
What is Lanthanoid contraction?
Write any two consequences of Lanthanoid Contraction.
What are the characteristics of the transition elements and why are they called transition elements?
Which of the d-block elements may not be regarded as the transition elements?
In what way is the electronic configuration of the transition elements different from that of the non-transition elements?
What are the different oxidation states exhibited by the lanthanoids?
Give reasons for the following statement:
Transition metals and most of their compounds show paramagnetic behaviour.
Why do the transition elements have higher enthalpies of atomisation?
Give reasons for the following:
The transition metals generally form coloured compounds.
How would you account for the following?
Transition metals and their compounds act as catalysts.
What are interstitial compounds?
Why are interstitial compounds well known for transition metals?
How is the variability in oxidation states of transition metals different from that of the non-transition metals? Illustrate with examples.
Describe the preparation of potassium dichromate from iron chromite ore. What is the effect of increasing pH on a solution of potassium dichromate?
Describe the oxidising action of potassium dichromate and write the ionic equation for its reaction with iodide.
Describe the oxidising action of potassium dichromate and write the ionic equation for its reaction with iron (II) solution.
Describe the oxidising action of potassium dichromate and write the ionic equation for its reaction with H2S.
Describe the preparation of potassium permanganate. How does the acidified permanganate solution react with iron (II) ions? Write the ionic equation for the reaction.
Describe the preparation of potassium permanganate. How does the acidified permanganate solution react with SO2? Write the ionic equation for the reaction.
Describe the preparation of potassium permanganate. How does the acidified permanganate solution react with oxalic acid? Write the ionic equation for the reaction.
For M2+/M and M3+/M2+ systems the E° values for some metals are as follows:
Cr2+/Cr −0.9 V, Cr3+/Cr2+ −0.4 V
Mn2+/Mn −1.2 V, Mn3+/Mn2+ +1.5 V
Fe2+/Fe −0.4 V, Fe3+/Fe2+ +0.8 V
Use this data to comment upon:
- the stability of Fe3+ in acid solution as compared to that Cr3+ or Mn3+ and
- the ease with which iron can be oxidised as compared to a similar process for either chromium or manganese metal.
Predict which of the following will be coloured in the aqueous solution?
Ti3+, V3+, Cu+, Sc3+, Mn2+, Fe3+ and Co2+. Give reasons for each.
Compare the stability of +2 oxidation state for the elements of the first transition series.
Compare the chemistry of actinoids with that of lanthanoids with special reference to electronic configuration.
Compare the chemistry of actinoids with that of the lanthanoids with special reference to atomic and ionic sizes.
Compare the chemistry of actinoids with that of the lanthanoids with special reference to oxidation state.
Compare the chemistry of actinoids with that of the lanthanoids with special reference to chemical reactivity.
How would you account for the following:
Of the d4 species, Cr2+ is strongly reducing while manganese (III) is strongly oxidising.
How would you account for the following:
Cobalt (II) is stable in aqueous solutions, but in the presence of complexing reagents, it is easily oxidised.
How would you account for the following:
The d1 configuration is very unstable in ions.
What is meant by ‘disproportionation’?
Give two examples of disproportionation reactions in aqueous solution.
Which metal in the first series of transition metals exhibits +1 oxidation state most frequently and why?
Calculate the number of unpaired electrons in the following gaseous ions:
Mn3+, Cr3+, V3+ and Ti3+. Which one of these is the most stable in an aqueous solution?
Give an example and suggest a reason for the following feature of the transition metal chemistry:
The lowest oxide of transition metal is basic, the highest is amphoteric/acidic.
Give an example and suggest a reason for the following feature of the transition metal chemistry:
A transition metal exhibits the highest oxidation state in oxides and fluorides.
Give an example and suggest a reason for the following feature of the transition metal chemistry:
The highest oxidation state is exhibited in oxoanions of a metal.
Indicate the steps in the preparation of K2Cr2O7 from chromite ore.
Indicate the steps in the preparation of KMnO4 from pyrolusite ore.
What are alloys?
Name an important alloy which contains some of the lanthanoid metals.
Mention uses of alloys.
What are inner transition elements?
Decide which of the following atomic numbers are the atomic numbers of the inner transition elements:
29, 59, 74, 95, 102, 104
The chemistry of the actinoid elements is not so smooth as that of the Lanthanoids. Justify this statement by giving some examples from the oxidation state of these elements.
Which is the last element in the series of the actinoids? Write the electronic configuration of this element. Comment on the possible oxidation state of this element.
Use Hund’s rule to derive the electronic configuration of Ce3+ ion and calculate its magnetic moment on the basis of ‘spin-only’ formula.
Name the members of the lanthanoid series which exhibit +4 oxidation state and those which exhibit +2 oxidation state. Try to correlate this type of behavior with the electronic configurations of these elements.
Compare the chemistry of actinoids with that of lanthanoids with special reference to electronic configuration.
Compare the chemistry of actinoids with that of the lanthanoids with special reference to oxidation state.
Compare the chemistry of actinoids with that of the lanthanoids with special reference to chemical reactivity.
Write the electronic configurations of the element with the atomic number 61.
Write the electronic configuration of the element with the atomic number 91.
Write the electronic configuration of the element with the atomic number 101.
Write the electronic configurations of the element with the atomic number 109.
Compare the general characteristics of the first series of the transition metals with those of the second and third series metals in the respective vertical columns. Give special emphasis on the following point:
Electronic configurations
Compare the general characteristics of the first series of the transition metals with those of the second and third series metals in the respective vertical columns. Give special emphasis on the following point:
Oxidation states
Compare the general characteristics of the first series of the transition metals with those of the second and third series metals in the respective vertical columns. Give special emphasis on the following point:
Ionisation enthalpies
Compare the general characteristics of the first series of the transition metals with those of the second and third series metals in the respective vertical columns. Give special emphasis on the following point:
Atomic sizes
Write down the number of 3d electrons in the following ion:
Ti2+
Indicate how would you expect the five 3d orbitals to be occupied for this hydrated ions (octahedral).
Write down the number of 3d electrons in the following ion:
V2+
Indicate how would you expect the five 3d orbitals to be occupied for this hydrated ions (octahedral).
Write down the number of 3d electrons in the following ion:
Cr3+
Indicate how would you expect the five 3d orbitals to be occupied for this hydrated ions (octahedral).
Write down the number of 3d electrons in the following ion:
Mn2+
Indicate how would you expect the five 3d orbitals to be occupied for this hydrated ions (octahedral).
Write down the number of 3d electrons in the following ion:
Fe2+
Indicate how would you expect the five 3d orbitals to be occupied for this hydrated ions (octahedral).
Write down the number of 3d electrons in the following ion:
Fe3+
Indicate how would you expect the five 3d orbitals to be occupied for this hydrated ions (octahedral).
Write down the number of 3d electrons in the following ion:
Co2+
Indicate how would you expect the five 3d orbitals to be occupied for this hydrated ions (octahedral).
Write down the number of 3d electrons in the following ion:
Ni2+
Indicate how would you expect the five 3d orbitals to be occupied for this hydrated ions (octahedral).
Write down the number of 3d electrons in the following ion:
Cu2+
Indicate how would you expect the five 3d orbitals to be occupied for this hydrated ions (octahedral).
Comment on the statement that elements of the first transition series possess many properties different from those of heavier transition elements.
What can be inferred from the magnetic moment value of the following complex species?
| Example | Magnetic Moment (BM) |
| K4[Mn(CN)6] | 2.2 |
What can be inferred from the magnetic moment value of the following complex species?
| Example | Magnetic Moment (BM) |
| [Fe(H2O)6]2+ | 5.3 |
What can be inferred from the magnetic moment value of the following complex species?
| Example | Magnetic Moment (BM) |
| K2[MnCl4] | 5.9 |
Nootan solutions for Chemistry Part 1 and 2 [English] Class 12 ISC 8 d-and ƒ-Block Elements QUESTIONS FROM ISC EXAMINATION PAPERS [Pages 509 - 510]
What is a flux?
Give an example of flux, writing the relevant equation.
Name the important ores of silver. Describe the extraction of silver from these ores.
Sodium cyanide is used in the extraction of silver from its ore. Explain why it is used and write the relevant equation.
Write the chemical equation for the reactions involved in the extraction of copper from copper pyrites.
MacArthur-Forrest process is used for the extraction of ______.
aluminium
copper
silver
tin
Copper pyrites is an ore of copper.
Describe the process by which copper pyrites is concentrated.
Copper pyrites is an ore of copper.
Describe all the steps, with equations, to convert the concentrated ore to blister copper.
Copper pyrites is an ore of copper.
Describe the process of conversion of blister copper to pure copper.
Describe the extraction of silver from its sulphide ore by the cyanide process.
State the common oxidation state of lanthanides.
State the common oxidation state of actinides.
In a given transition series, there is no significant change in the atomic radii of elements with increase in atomic number. Explain why.
What is the electronic configuration of a chromium atom (Z = 24)? Give a reason for your answer.
Give the balanced equations for the conversion of argentite (Ag2S) to metallic silver.
Give a balanced equation for the following reaction:
Acidified potassium permanganate and oxalic acid.
Explain why transition metals form complex compounds.
In a given transition series, the atomic radius does not change very much with increasing atomic number. Explain.
Write a balanced equation for the following reaction:
Sodium sulphite and acidified potassium permanganate.
Give a reason for the following:
Zn2+ salts are white but Cu2+ salts are blue in colour.
Give a reason for the following:
Fluorine gives only one oxide but chlorine gives a series of oxides.
How is potassium dichromate prepared from a sample of chromite ore? Give balanced equations for the chemical reactions involved.
Name the important ores of silver. Describe the extraction of silver from these ores.
Give a reason for the following:
Transition metals possess a great tendency to form complex compounds.
The paramagnetic character in the 3d-transition series elements increases up to Mn and then decreases.
Give balanced equations for the following reactions:
Silver nitrate is added to dilute solution of sodium thiosulphate.
Give balanced equations for the following reaction:
Potassium dichromate is treated with acidified ferrous sulphate solution.
How will you obtain pure potassium permanganate (KMnO4) crystals from its ore, pyrolusite? Give the steps involved and the reactions.
What is Lanthanoid contraction?
Write the general electronic configuration of inner transition elements.
Give balanced equation for the following reaction:
Potassium permanganate is heated with concentrated hydrochloric acid.
Why does the density of transition elements increase from Titanium to Copper? (at. no. Ti = 22, Cu = 29)
Why Zinc is not regarded as a transition element?
Explain why Mn2+ is more stable than Fe2+ towards oxidation to +3 state. (At. no. of Mn = 25, Fe = 26)
Give reasons for the following:
The transition metals generally form coloured compounds.
Why do zirconium and Hafnium exhibit similar properties?
Complete and balance the following chemical equation:
\[\ce{KMnO4 + KI + H2SO4 ->}\] _____ + _____ + _____ + ______
Complete and balance the following chemical equation:
\[\ce{K2Cr2O7 + H2SO4 + H2S ->}\] ______ + ______ + ______ + ______
Complete and balance the following chemical equation:
\[\ce{KMnO4 + H2SO4 + FeSO4 ->}\] ______ + ______ + ______ + ______
Complete and balance the following chemical equation:
\[\ce{KMnO4 + SO2 + H2O ->}\] ______ + ______ + ______
Which trivalent ion has the maximum size in the Lanthanoid series, i.e., Lanthanum ion (La3+) to Luteium ion (Lu3+)?
(at. no. of Lanthanum = 57 and Lutetium = 71)
Explain why Cu2+ is paramagnetic, but Cu+ is diamagnetic. (at. no. of Cu = 29)
Explain why transition elements form alloys.
Explain why Zn2+ salts are white whereas Cu2+ salts are coloured.
Explain why transition metals and their compounds act as a catalyst.
Complete and balance the chemical equation:
\[\ce{KMnO4 + H2SO4 + H2C2O4 ->}\] ______ + ______ + ______ + ______
Complete and balance the following chemical equation:
\[\ce{K2Cr2O7 + H2SO4 + KI ->}\] ______ + ______ +______ + ______
Complete and balance the chemical equation:
\[\ce{K2Cr2O7 + H2SO4 + FeSO4 ->}\] ______ + ______ + ______ + ______
Why Zn2+ ions are colourless while Ni2+ ions are green in colour?
Why Zn2+ ions are colourless while Cu2+ ions are blue in colour?
Give reasons for the following statement:
Transition metals and most of their compounds show paramagnetic behaviour.
Why does the density of transition elements increase from Titanium to Copper? (at. no. Ti = 22, Cu = 29)
Explain the following:
K2Cr2O7 acts as a powerful medium oxidising agent in acidic
Paramagnetic compounds are generally ______ and contain ______ electrons.
The size of the trivalent cations in the lanthanoid series decreases steadily as the atomic number increases. What is this phenomenon called?
Give reasons for the following:
The transition metals generally form coloured compounds.
Solutions for 8: d-and ƒ-Block Elements
Nootan solutions for Chemistry Part 1 and 2 [English] Class 12 ISC chapter 8 - d-and ƒ-Block Elements
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Concepts covered in Chemistry Part 1 and 2 [English] Class 12 ISC chapter 8 d-and ƒ-Block Elements are Overview of d-and f-Block Elements.
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