Lakhmir Singh solutions for Chemistry [English] Class 10 chapter 3 - Metals and Non-metals [Latest edition]

Name one metal which exists in a liquid state at room temperature.

Why are metals called electropositive elements?

Why are non-metals called electronegative elements?

Name the most abundant metal in the earth’s crust.

Name the most abundant non-metal in the earth’s crust.

Name one metal which has a low melting point.

Name the metal which is the poorest conductor of heat.

State whether the following statement is true or false:

Non-metals react with dilute acids to produce a gas which burns with a ‘pop’ sound.

From amongst the metals sodium, calcium, aluminium, copper and magnesium, name the metal:

1. which reacts with water only on boiling, and
2. another which does not react even with steam.

What changes in the colour of iron nails and copper sulphate solution do you observe after keeping the iron nails dipped in copper sulphate solution for about 30 minutes?

What is aqua-regia?

Name two special metals which are insoluble in common reagents but dissolve in aqua-regia.

Give the name and formula of two acidic oxides.

Give the name and formula of two basic oxides.

What name is given to those metal oxides which show basic as well as acidic behaviour?

Name two metals which form amphoteric oxides.

A copper coin is kept immersed in a solution of silver nitrate for some time. What will happen to the coin and the colour of the solution?

Which property of copper and aluminium makes them suitable for making cooking utensils and boilers?

Which property of copper and aluminium makes them suitable for making electric wires?

Write the name and formula of a metal hydride.

Write the name and formula of a non-metal hydride.

Name the metal which has been placed at the bottom of the reactivity series.

Name the metal which has been placed at the top of the reactivity series.

Name the metal which has been placed just below copper in the reactivity series.

Which of the two metals is more reactive?

Copper or silver

Name one metal which is stored in kerosene oil.

Name one non-metal which is stored under water.

Write an equation for the reaction of:

Sodium with oxygen

Write an equation for the reaction of:

Magnesium with oxygen

Name two metals which are used for making electric wires.

Name two metals which are used for making domestic utensils and factory equipment.

Name two metals which are used for making jewellery and to decorate sweets.

Which metal foil is used for packing some of the medicine tablets?

Name the non-metal which is used:

To convert vegetable oil into vegetable ghee (solid fat).

Name the non-metal which is used:

As a rocket fuel (in liquid form).

Name the non-metal which is used:

To make electrodes of dry cells.

Name the non-metal which is used:

To preserve food materials.

Name the non-metal which is used:

In the vulcanisation of rubber.

Name one property which is characteristic of metals.

Name one property which is characteristic of non-metals.

What is meant by “brittleness”?

Which type of elements usually show brittleness?

Metals or non-metals

What will happen if a strip of zinc is immersed in a solution of copper sulphate?

What will happen if a strip of copper is kept immersed in a solution of silver nitrate (AgNO₃)?

What changes in the colour of iron nails and copper sulphate solution do you observe after keeping the iron nails dipped in copper sulphate solution for about 30 minutes?

How would you show that silver is chemically less reactive than copper?

Give reasons for the following:

Blue colour of copper sulphate solution is destroyed when iron filings are added to it.

Name a non-metal having a very high melting point.

Which property of graphite is utilised in making electrodes?

Name two non-metals which are both brittle and non-ductile.

Explain why, the surface of some metals acquires a dull appearance when exposed to air for a long time.

Complete and balance the following equation:

\[\ce{Na + O2 ->}\]

Complete and balance the following equation:

\[\ce{Na2O + H2O ->}\]

Complete and balance the following equation:

\[\ce{Fe_{(s)} + H2O_{(g)} ->[Red heat]}\]

Complete and balance the following equation:

\[\ce{Cu(NO3)2_{(aq)} + Zn_{(s)} ->}\]

Magnesium liberates ______ gas on reacting with hot boiling water.

The white powder formed when magnesium ribbon burns in oxygen is of ______.

Ordinary aluminium strips are not attacked by water because of the presence of a layer of ______ on the surface of aluminium.

A metal having low melting point is ______ but a non-metal having very high melting point is ______.

Calcium is a ______ reactive metal than sodium.

What is meant by saying that the metals are malleable and ductile? Explain with examples.

Name two metals which are both malleable and ductile.

Which property of iron metal is utilised in producing iron sheets required for making buckets?

Which property of copper metal is utilised in making thin wires?

Name two metals which react violently with cold water. Write any three observations you would make when such a metal is dropped into water. How would you identify the gas evolved, if any, during the reaction?

With the help of examples, describe how metal oxides differ from non-metal oxides.

Which of the following elements would yield an acidic oxide?

Na, S, C, K, H

Which of the following elements would yield a basic oxide?

Na, S, C, K, H

Which of the following elements would yield a neutral oxide?

Na, S, C, K, H

What are amphoteric oxides?

Give two examples of amphoteric oxides.

Choose the acidic oxides, basic oxides and neutral oxides from the following:

Na₂O; CO₂; CO; SO₂; MgO; N₂O; H₂O

Which of the following are amphoteric oxides:

MgO, ZnO, P₂O₃, Al₂O₃, NO₂

What is the nature of the oxide SO₂? What happens when it is dissolved in water? Write the chemical equation of the reaction involved.

What is the nature of the oxide Na₂O? What happens when it is dissolved in water? Write the chemical equation of the reaction involved.

What type of oxides are formed when non-metals react with oxygen? Explain with an example.

What type of oxides are formed when metals combine with oxygen? Explain with the help of an example.

Explain why, metals usually do not liberate hydrogen gas with dilute nitric acid.

Name two metals which can, however, liberate hydrogen gas from very dilute nitric acid.

How do metals react with hydrogen? Explain with an example.

How do non-metals react with hydrogen? Explain with an example.

What happens when calcium reacts with chlorine? Write an equation for the reaction which takes place.

What happens when magnesium reacts with very dilute nitric acid? Write an equation for the reaction involved.

Arrange the following metals in order of their chemical reactivity, placing the most reactive metal first:

Magnesium, Copper, Iron, Sodium, Zinc, Lead, Calcium

What happens when a rod of zinc metal is dipped into a solution of copper sulphate? Give chemical equation of the reaction involved.

A copper plate was dipped in AgNO₃ solution. After certain time, silver from the solution was deposited on the copper plate. State the reason why it happened. Give the chemical equation of the reaction involved.

State five uses of metals.

State five uses of non-metals.

State one use of the following metal:

Copper

State one use of the following metal:

Aluminium

State one use of the following metal:

Iron

State one use of the following metal:

Silver

State one use of the following metal:

Gold

State one use of the following metal:

Mercury

State one use of the following non-metal:

Hydrogen

State one use of the following non-metal:

Carbon (as Graphite)

State one use of the following non-metal:

Nitrogen

State one use of the following non-metal:

Sulphur

Name the metal which is used in making thermometers.

Why does aluminium not react with water under ordinary conditions?

Name two metals which can displace hydrogen from dilute acids.

Name two metals which cannot displace hydrogen from dilute acids.

Why is sodium kept immersed in kerosene oil?

Why is white phosphorus kept immersed under water?

Can we keep sodium immersed under water? Why?

Describe the reaction of potassium with water. Write the equation of the reaction involved.

Write equations for the reactions of iron with steam. 

Which gas is produced when dilute hydrochloric acid is added to a reactive metal?

Give one example, with equation, of the displacement of hydrogen by a metal from an acid.

Name two metals (other than zinc and iron) which can displace hydrogen from dilute hydrochloric acid?

What is the action of water on sodium? Write the equation of the chemical reactions involved.

What is the action of water on magnesium? Write equations of the chemical reactions involved.

What is the action of water on aluminium? Write the equation of the chemical reaction involved.

You are given samples of three metals - sodium, magnesium and copper. Suggest any two activities to arrange them in order of their decreasing reactivities.

Write one reaction in which aluminium oxide behaves as a basic oxide and another in which it behaves as an acidic oxide.

What special name is given to substances like aluminium oxide?

Name another metal oxide which behaves like aluminium oxide.

What happens when calcium reacts with water? Write the chemical equation of the reaction of calcium with water.

Write the chemical equation of the reaction which takes place when iron reacts with dilute sulphuric acid. What happens when the gas produced is ignited with a burning matchstick?

You are given a dry cell, a torch bulb with holder, wires and crocodile clips. How would you use them to distinguish between samples of metals and non-metals?

State any five physical properties of metals.

State any five physical properties of non-metals.

Name two physical properties of sodium in which its behaviour is not as expected from its classification as a metal.

Name two physical properties of carbon in which its behaviour is not as expected from its classification as a non-metal.

Name two metals whose melting points are so low that they melt when held in the hand.

Metals are said to be shiny. Why do metals generally appear to be dull? How can their brightness be restored?

What are metals?

Name five metals.

Name a metal which is so soft that it can be cut with a knife.

Name the metal which is the best conductor of heat and electricity.

What happens when a metal reacts with dilute hydrochloric acid? Explain with the help of an example.

Write the equation for the reaction of:

Magnesium with dilute hydrochloric acid.

Name the products formed in the given case. Also indicate the physical states of all the substances involved.

Write the equation for the reaction of:

Aluminium with dilute hydrochloric acid.

Name the products formed in the given case. Also indicate the physical states of all the substances involved.

Write the equation for the reaction of:

Zinc with dilute hydrochloric acid.

Name the products formed in the given case. Also indicate the physical states of all the substances involved.

Write the equation for the reaction of:

Iron with dilute hydrochloric acid.

Name the products formed in the given case. Also indicate the physical states of all the substances involved.

Define non-metals.

Give two examples of non-metals.

Name a non-metal which conducts electricity.

Name a non-metal having lustre (shining surface).

Name a non-metal which is extremely hard.

How do non-metals react with oxygen? Explain with an example. Give equation of the reaction involved. What is the nature of the product formed? How will you demonstrate it?

What is meant by the reactivity series of metals?

Arrange the following metals in an increasing order of their reactivities towards water:

Zinc, Iron, Magnesium, Sodium

Hydrogen is not a metal but still it has been assigned a place in the reactivity series of metals. Why?

Name one metal more reactive than hydrogen.

Name one metal less reactive than hydrogen.

Name one metal which displaces copper from copper sulphate solution.

Name one metal which does not displace copper from copper sulphate solution.

Name one metal which displaces silver from a silver nitrate solution.

Name one metal which does not displace silver from a silver nitrate solution.

State any three differences between the physical properties of metals and non-metals.

Differentiate between metals and non-metals on the basis of their chemical properties.

State three reasons (of which at least one must be chemical) for believing that sodium is a metal.

State three reasons (of which at least one must be chemical) for believing that sulphur is a nonmetal.

Which non-metal has been placed in the reactivity series of metals?

The elements whose oxides can turn phenolphthalein solution pink are ______.

“Is malleable and ductile”. This best describes:

One of the following is not a neutral oxide. This is:

A basic oxide will be formed by the element ______.

An acidic oxide is produced by the element ______.

You are given a solution of AgNO₃. Which of the following do you think cannot displace Ag from AgNO₃ solution?

Out of aluminium, copper, calcium and tin, the most reactive metal is ______.

The least reactive metal among the following is:

An element X reacts with hydrogen, when heated, to form a covalent hydride H₂X. If H₂X has a smell of rotten eggs, the element X is likely to be ______.

Out of the following oxides, the amphoteric oxide is:

The metals which can produce amphoteric oxides are ______.

An element X forms two oxides XO and XO₂. The oxide XO is neutral but XO₂ is acidic in nature. The element X is most likely to be ______.

The elements whose oxides can turn litmus solution blue are ______.

The elements whose oxides can turn litmus solution red are ______.

Zinc oxide is a metal oxide. Which of the following term best describes the nature of zinc oxide:

A metal less reactive and another metal more reactive than hydrogen are ______.

An element E reacts with water to form a solution which turns phenolphthalein solution pink. The element E is most likely to be ______.

An element reacts with oxygen to give a compound with a high melting point. This compound is also soluble in water. The element is likely to be ______.

Which one of the following four metals would be displaced from the solution of its salt by the other three metals?

An element is soft and can be cut with a knife. It is very reactive and cannot be kept open in the air. It reacts vigorously with water. The element is most likely to be ______.

Which of the following metal exists in the liquid state?

Which of the following non-metal is a liquid?

Which of the following pair of reactants can undergo a displacement reaction under appropriate conditions?

An element E forms an oxide E₂O. An aqueous solution of E₂O turns red litmus paper blue.

1. What is the nature of the oxide E₂O?
2. State whether element E is a metal or a non-metal.
3. Give one example of an element like E.

Metal A burns in air, on heating, to form an oxide A₂O₃ whereas another metal B burns in air only on strong heating to form an oxide BO. The two oxides A₂O₃ and BO can react with hydrochloric acid as well as sodium hydroxide solution to form the corresponding salts and water.

1. What is the nature of oxide A₂O₃?
2. What is the nature of oxide BO?
3. Name one metal like A.
4. Name one metal like B.

An element X forms two oxides XO and XO₂. The oxide XO has no action on litmus solution but oxide XO₂ turns litmus solution red.

1. What is the nature of oxide XO?
2. What is the nature of oxide ХО₂?
3. Would you call element X a metal or a non-metal? Give reason for your choice.
4. Can you give an example of element like X?

State and explain the reaction of the following metal with a solution of copper sulphate:

Gold

State and explain the reaction of the following metal with a solution of copper sulphate:

Copper

State and explain the reaction of the following metal with a solution of copper sulphate:

Zinc

State and explain the reaction of the following metal with a solution of copper sulphate:

Mercury

1. Name two physical properties of carbon in which its behaviour is not as expected from its classification as a non-metal.
2. State an important property in which these metal chloride and non-metal chloride differ.
3. Why do they differ in this property?

In a solution of lead acetate, a strip of metal M was dipped. After some time, lead from the solution was deposited on the metal strip. Which metal is more reactive, M or lead?

\[\ce{CuSO4_{(aq)} + Fe_{(s)} -> FeSO4_{(aq)} + Cu_{(s)}}\]

\[\ce{FeSO4_{(aq)} + Zn_{(s)} -> ZnSO4_{(aq)} + Fe_{(s)}}\]

On the basis of the above reactions, indicate which is most reactive and which is least reactive metal out of zinc, copper and iron.

Which of the following reactions will not occur? Why not?

1. \[\ce{MgSO4_{(aq)} + Cu_{(s)} -> CuSO4_{(aq)} + Mg_{(s)}}\]
2. \[\ce{CuSO4_{(aq)} + Fe_{(s)} -> FeSO4_{(aq)} + Cu_{(s)}}\]
3. \[\ce{MgSO4_{(aq)} + Fe_{(s)} -> FeSO4_{(aq)} + Mg_{(s)}}\]

In nature, metal A is found in a free state while metal B is found in the form of its compounds. Which of these two will be nearer to the top of the activity series of metals?

If A, B, C, D, E, F, G, H, I, J and K represent metals in the decreasing order of their reactivity, which one of them is most likely to occur in a free state in nature?

Name a metal for the given case:

It does not react with cold as well as hot water but reacts with steam.

Name a metal for the given case:

It does not react with any physical state of water.

When calcium metal is added to water, the gas evolved does not catch fire but the same gas evolved on adding sodium metal to water catches fire. Why is it so?

A zinc plate was kept in a glass container having CuSO₄ solution. On examining it was found that the blue colour of the solution is getting lighter and lighter. After a few days, when the zinc plate was taken out of the solution, a number of small holes were noticed in it. State the reason and give chemical equation of the reaction involved.

What is the name of the chemical bond formed?

By the sharing of electrons between two atoms.

What is the name of the chemical bond formed?

By the transfer of electrons from one atom to another.

Name a carbon containing molecule which has two double bonds.

What would be the electron-dot structure of carbon dioxide which has the formula CO₂?

What type of chemical bond is formed between:

Potassium and bromine

What type of chemical bond is formed between:

Carbon and bromine

What do we call those particles which have more or less electrons than the normal atoms?

What do we call those particles which have more electrons than the normal atoms?

What do we call those particles which have less electrons than the normal atoms?

The atomic number of sodium is 11. What is the number of electrons in Na⁺?

The atomic number of chlorine is 17. What is the number of electrons in Cl⁻?

The atomic number of an element X is 8 and that of element Y is 12. Write down the symbols of the ions you would expect to be formed from their atoms.

Write down the electronic configuration of the magnesium atom.

(At. No. of Mg = 12)

Write down the electronic configuration of the magnesium ion.

(At. No. of Mg = 12)

Write down the electronic configuration of the sulphur atom.

(At. No. of S = 16)

Write down the electronic configuration of the sulphide ion.

(At. No. of S = 16)

What type of chemical bonds are present in a solid compound which has a high melting point, does not conduct electricity in the solid state but becomes a good conductor in the molten state?

State whether the following statement is true or false:

The aqueous solution of an ionic compound conducts electricity because there are plenty of free electrons in the solution.

What type of bond is present in hydrogen chloride?

What type of bond is present in oxygen?

Write the electron-dot structure for the following molecule:

NaCl

Write the electron-dot structure for the following molecule:

Cl₂

What type of bonds are present in a water molecule?

Draw the electron-dot structure of water (H₂O).

What type of bond is present in methane (CH₄)?

What type of bond is present in sodium chloride (NaCl)?

State one major difference between covalent and ionic bonds.

Give one example of a covalent compound.

Give one example of an ionic compound.

What type of bond is present in the following molecule?

H₂

What type of bond is present in the following molecule?

CH₄

What type of bond is present in the following molecule?

Cl₂

What type of bond is present in the following molecule?

O₂

Draw the electron-dot structure of the H₂ molecule.

Draw the electron-dot structure of the CH₄ molecule.

Write the electron-dot structure for the following molecule:

Cl₂

Draw the electron-dot structure of the O₂ molecule.

Which inert gas electron configuration do the Cl atoms in Cl₂ molecule resemble? What is this electron configuration?

Which of the following compounds are ionic and which are covalent?

Urea, Cane sugar, Hydrogen chloride, Sodium chloride, Ammonium chloride, Carbon tetrachloride, Ammonia, Alcohol, Magnesium chloride.

Give one example of the following:

A molecule containing a single covalent bond.

Give one example of the following:

A molecule containing a double covalent bond.

Give one example of the following:

A molecule containing a triple covalent bond.

Give one example of the following:

A compound containing an ionic bond.

Two atoms of the same element combine to form a molecule. The bond between them is known as ______ bond.

Two chlorine atoms combine to form a molecule. The bond between them is known as ______.

In forming oxygen molecule, ______ electrons are shared by each atom of oxygen.

In forming N₂ molecule, ______ electrons are shared by each atom of nitrogen.

The number of single covalent bonds in C₂H₂ molecule are ______.

Melting points and boiling points of ionic compounds are generally ______ than those of covalent compounds.

What is a covalent bond?

What type of bond exists in CCl₄?

What type of bond exists in CaCl₂?

What is an ionic bond?

What type of bond is present in oxygen?

What is an ion? Explain with examples.

What is the nature of the charge on a cation?

What is the nature of the charge on an anion?

Name the cation and anion present in MgCl₂. Also write their symbols.

What type of chemical bond is present in the chlorine molecule? Explain your answer.

Explain the formation of a chlorine molecule on the basis of electronic theory of valency.

Giving one example, state what are ionic compounds.

Compare the properties of ionic compounds and covalent compounds.

Explain why:

Covalent compounds have generally low melting points.

Why do ionic compounds have high melting points?

Give two general properties of ionic compounds.

Give the characteristic properties of covalent compounds.

State one test by which sodium chloride can be distinguished from sugar.

Explain why, ionic compounds conduct electricity in solution whereas covalent compounds do not conduct electricity.

Which of the following will conduct electricity and which not?

MgCl₂, CCl₄, NaCl, CS₂, Na₂S

Give reasons for your choice.

Name one ionic compound containing chlorine.

Name one covalent compound containing chlorine.

How will you find out which of the water soluble compound A or B is ionic?

Explain why, ionic compounds conduct electricity in solution whereas covalent compounds do not conduct electricity.

Give the formula of the compound that would be formed by the combination of the following pair of elements:

Mg and N₂

Give the formula of the compound that would be formed by the combination of the following pair of elements:

Li and O₂

Give the formula of the compound that would be formed by the combination of the following pair of elements:

Al and Cl₂

Give the formula of the compound that would be formed by the combination of the following pair of elements:

K and H

What are noble gases?

What is the characteristic of the electronic configuration of noble gases?

What is the cause of chemical bonding (or chemical combination) of atoms of elements?

Write electron-dot structures for magnesium.

Write the electron-dot structure for oxygen.

Show the formation of MgO by the transfer of electrons.

What are the ions present in the MgO compound?

Draw the electron-dot structure of a hydrogen chloride molecule:

1. Which inert gas does the H atom in HCl resemble in electron arrangement?
2. Which inert gas does the Cl atom in HCl resemble in electron arrangement?

What type of bonding would you expect between the following pair of elements?

Calcium and Oxygen

What type of bonding would you expect between the following pair of elements?

Carbon and Chlorine

What type of bonding would you expect between the following pair of elements?

Hydrogen and Chlorine

Describe how sodium and chlorine atoms are changed into ions when they react with each other to form sodium chloride, NaCl. What is the name given to this type of bonding?

(At. No of sodium = 11; At. No. of chlorine = 17)

What is the difference between:

A cation and an anion.

How are cations formed?

How are anions formed?

Give the name and symbol of one cation.

Give the name and symbol of one anion.

Using electron-dot diagrams which show only the outermost shell electrons, show how a molecule of nitrogen, N₂, is formed from two nitrogen atoms. What name is given to this type of bonding?

(Atomic number of nitrogen is 7)

Draw the electron-dot structure of the following compound and state the type of bonding in the given case:

CO₂

Draw the electron-dot structure of the following compound and state the type of bonding in the given case:

MgO

Draw the electron-dot structure of the following compound and state the type of bonding in the given case:

H₂O

Draw the electron-dot structure of the following compound and state the type of bonding in the given case:

HCl

Draw the electron-dot structure of the following compound and state the type of bonding in the given case:

MgCl₂

Using electron-dot diagrams which show only the outermost shell electrons, show how a molecule of oxygen, O₂, is formed from two oxygen atoms. What name is given to this type of bonding?

(At. No. of oxygen = 8)

Draw the electron-dot structure of the following compound and state the type of bonding in the given case:

KCl

Draw the electron-dot structure of the following compound and state the type of bonding in the given case:

NH₃

Draw the electron-dot structure of the following compound and state the type of bonding in the given case:

CaO

Draw the electron-dot structure of the following compound and state the type of bonding in the given case:

N₂

Draw the electron-dot structure of the following compound and state the type of bonding in the given case:

CaCl₂

Explain why, a salt which does not conduct electricity in the solid state becomes a good conductor in molten state.

Write down the electronic configuration of the sodium atom.

Write down the electronic configuration of the chlorine atom.

How many electrons are there in the outermost shell of a sodium atom?

How many electrons are there in the outermost shell of a chlorine atom?

Show the formation of NaCl from sodium and chlorine atoms by the transfer of electron(s).

Why has sodium chloride a high melting point?

Name the anode and the cathode used in the electrolytic refining of impure copper metal.

Write the electron arrangement in a magnesium atom.

Write the electron arrangement in an oxygen atom.

How many electrons are there in the valence shell of a magnesium atom?

How many electrons are there in the valence shell of an oxygen atom?

Show on a diagram the transfer of electrons between the atoms in the formation of MgO.

Name the solvent in which ionic compounds are generally soluble.

Why are aqueous solutions of ionic compounds able to conduct electricity?

What is the electronic configuration of a sodium atom?

What is the electronic configuration of an oxygen atom?

What is the number of outermost electrons in a sodium atom?

What is the number of outermost electrons in an oxygen atom?

Show the formation of Na₂O by the transfer of electrons between the combining atoms.

Why are ionic compounds usually hard?

How is it that ionic compounds in the solid state do not conduct electricity but they do so when in molten state?

Write the electron arrangement in a magnesium atom.

Write down the electron arrangement in a chlorine atom.

How many electrons are there in the valence shell of a magnesium atom?

How many electrons are there in the valence shell of a chlorine atom?

Show the formation of magnesium chloride from magnesium and chlorine by the transfer of electrons.

State whether magnesium chloride will conduct electricity or not. Give reason for your answer.

Why are covalent compounds generally poor conductors of electricity?

The atomic number of an element X is 19. The number of electrons in its ion X⁺ will be ______.

The atomic number of an element Y is 17. The number of electrons in its ion Y⁻ will be ______.

The atomic numbers of four elements A, B, C and D are 6, 8, 10 and 12 respectively. The two elements which can react to form ionic bonds (or ionic compound) are ______.

The atomic numbers of four elements P, Q, R and S are 6, 10, 12 and 17 respectively. Which two elements can combine to form a covalent compound?

The solution of one of the following compounds will not conduct electricity. This compound is:

The electronic configurations of three elements X, Y and Z are:

X: 2

Y: 2, 8, 7

Z: 2, 8, 2

Which of the following is correct regarding these elements?

Which one of the following property is generally not exhibited by ionic compounds?

The electrons present in the valence shell of a noble gas atom can be ______.

The atomic number of an element X is 16. The symbol of ion formed by an atom of this element will be ______.

The number of protons in the nucleus of one atom of an element Y is 5. The symbol of ion formed by an atom of this element will be ______.

Out of KCl, HCl, CCl₄ and NaCl, the compounds which are not ionic are ______.

Element X reacts with element Y to form a compound Z. During the formation of compound Z, atoms of X lose one electron each whereas atoms of Y gain one electron each. Which of the following property is not shown by compound Z?

One of the following compounds is not ionic in nature. This compound is:

The rechargeable battery used in a mobile phone hand set is usually ______.

The number of protons in one atom of an element X is 8. What will be the number of electrons in its ion X²⁻?

If the number of protons in one atom of an element Y is 20, then the number of electrons in its ion Y²⁺ will be ______.

The noble gas having only two electrons in its valence shell is ______.

A covalent molecule having a double bond between its atoms is ______.

The molecules having triple bond in them are ______.

One of the following contains a double bond as well as single bonds. This is:

Which of the following has a triple bond as well as single bonds?

Two non-metals combine with each other by the sharing of electrons to form a compound X.

1. What type of chemical bond is present in X?
2. State whether X will have a high melting point or low melting point.
3. Will it be a good conductor of electricity or not?
4. Will it dissolve in an organic solvent or not?

A metal combines with a non-metal by the transfer of electrons to form a compound Y.

1. State the type of bonds in Y.
2. What can you say about its melting point and boiling point?
3. Will it be a good conductor of electricity?
4. Will it dissolve in an organic solvent or not?

The electronic configurations of three elements X, Y and Z are as follows:

1. Which two elements will combine to form an ionic compound?
2. Which two elements will react to form a covalent compound?

Give reasons for your choice.

An element A has 4 valence electrons in its atom whereas element B has only one valence electron in its atom. The compound formed by A and B does not conduct electricity. What is the nature of chemical bond in the compound formed? Give its electron-dot structure.

In the formation of a compound XY₂ atom X gives one electron to each Y atom. What is the nature of bond in XY₂? Give two properties of XY_2.

An element ‘A’ has two electrons in the outermost shell of its atom and combines with an element ‘B’ having seven electrons in the outermost shell, forming the compound AB₂. The compound when dissolved in water conducts electric current. Giving reasons, state the nature of chemical bond in the compound.

The electronic configurations of two elements A and B are given below:

1. What type of chemical bond is formed between the two atoms of A?
2. What type of chemical bond will be formed between the atoms of A and B?

Four elements A, B, C and D have the following electron arrangements in their atoms:

1. What type of bond is formed when element C combines with element D?
2. Which element is an inert gas?
3. What will be the formula of the compound between A and C?

An element X of atomic number 12 combines with an element Y of atomic number 17 to form a compound XY₂. State the nature of chemical bond in XY₂ and show how the electron configurations of X and Y change in the formation of this compound.

The electronic configurations of three elements A, B and C are as follows:

1. Which of these elements is a metal?
2. Which of these elements are non-metals?
3. Which two elements will combine to form an ionic bond?
4. Which two elements will combine to form a covalent bond?
5. Which element will form an anion of valency 1?

The electronic configurations of four particles A, B, C and D are given below:

Which electronic configuration represents:

1. magnesium atom?
2. oxygen atom?
3. sodium ion?
4. chloride ion?

The atomic number of an element X is 12.

1. What must an atom of X do to attain the nearest inert gas electron configuration?
2. Which inert gas is nearest to X?

The atomic number of an element Y is 16.

1. What must an atom of Y do to achieve the nearest inert gas electron arrangement?
2. Which inert gas is nearest to Y?

You can buy solid air-freshners in shops. Do you think these substances are ionic or covalent? Why?

Give the formulae of the chlorides of the elements X and Y having atomic numbers of 3 and 6 respectively. Will the properties of the two chlorides be similar or different? Explain your answer.

A zinc ore gave CO₂ on treatment with a dilute acid. Identify the ore and write its chemical formula.

What chemical process is used for obtaining a metal from its oxide?

Write two methods of preventing the rusting of iron.

What is meant by galvanisation? Why is it done?

Name the metal which is used for galvanising iron.

Explain why, iron sheets are coated with zinc.

Why do we apply paint on iron articles?

Give a reasons for the following:

Carbonate and sulphide ores are usually converted into oxides during the process of extraction of metals.

Name a reducing agent that may be used to obtain manganese from manganese dioxide.

Name an alloy of lead and tin.

Give the composition of an alloy called solder. State its one property and one use.

What is an amalgam?

How many carats is pure gold? Why is pure gold not suitable for making ornaments?

Name one method for the refining of metals.

State two conditions for the rusting of iron.

In one method of rust prevention, the iron is not coated with anything. Which is this method?

Name two alloys of iron. What elements are present in these alloys?

Give reasons:

Platinum, gold and silver are used to make jewellery.

Which metal becomes black in the presence of hydrogen sulphide gas in air?

Name the gas in air which tarnishes silver articles slowly.

Silver metal does not combine easily with oxygen but silver jewellery tarnishes after some time. How?

Write the composition of the alloy called bronze.

Give two uses of bronze.

Why does a new aluminium vessel lose shine so soon after use?

Why do gold ornaments look new even after several years of use?

Name two metals which are highly resistant to corrosion.

Which property of ‘solder’ alloy makes it suitable for welding electrical wires?

Explain why, carbon cannot reduce oxides of sodium or magnesium.

Why are the metals like Na, K, Ca and Mg never found in their free state in nature?

Name one metal each which is extracted by:

Reduction with carbon.

Name one metal each which is extracted by:

Electrolytic reduction.

Name one metal each which is extracted by:

Reduction with aluminium.

Name one metal each which is extracted by:

Reduction with heat alone.

The corrosion of iron is called ______.

______ and ______ are necessary for the rusting of iron.

The process of depositing a thin layer of zinc on iron articles is called ______.

Tiffin boxes are electroplated with ______ but car bumpers are electroplated with ______ to protect them from rusting.

The corrosion of copper produces a ______ coating of basic copper carbonate on its surface.

Brass is an alloy of copper and ______.

Bronze is an alloy of copper and ______.

The non-metal present in steel is ______.

The alloy in which one of the metals is mercury is called an ______.

The electrical conductivity and melting point of an alloy is ______ than that of pure metals.

The rocky material found with ores is called ______.

What is a thermite reaction? Explain with the help of an equation.

State one use of a thermite reaction.

Which one of the methods given in column I is applied for the extraction of each of the metals given in column II:

Give reasons why copper is used to make hot water tanks and not steel (an alloy of iron).

Explain why, the surface of some metals acquires a dull appearance when exposed to air for a long time.

Why does aluminium not corrode right through?

What is meant by ‘anodising’? Why is it done?

Why is an iron grill painted frequently?

Explain why, though aluminium is more reactive than iron, yet there is less corrosion of aluminium when both are exposed to air.

Name the method by which aluminium metal is extracted.

Give the name and chemical formula of one ore of copper.

How is zinc extracted from its carbonate ore (calamine)? Explain with equations.

Name two metals which occur in nature in free state as well as in combined state.

Name one ore of manganese. Which compound of manganese is present in this ore? Also write its chemical formula.

A zinc ore on heating in air forms sulphur dioxide. Describe briefly any two stages involved in the conversion of this concentrated ore into zinc metal.

How does the method used for extracting a metal from its ore depend on the metal’s position in the reactivity series? Explain with examples.

Explain giving one example, how highly reactive metals (which are high up in the reactivity series) are extracted.

Describe with one example, how moderately reactive metals (which are in the middle of reactivity series) are extracted.

How are the less reactive metals (which are quite low in the reactivity series) extracted? Explain with the help of an example.

What is meant by refining of a metal?

Name the most widely used method for the refining of impure metals obtained by various reduction processes. Describe this method with the help of a labelled diagram by taking the example of any metal.

Define the term mineral.

Define the term ore.

Define the term gangue.

What is meant by the ‘concentration of ore’?

Name one ore of copper (other than cuprite). Which compound of copper is present in this ore? Also, write its chemical formula.

Explain how, a reduction reaction of aluminium can be used for welding cracked machine parts of iron. Write a chemical equation for the reaction involved.

What is corrosion?

Name any two metals which do not corrode easily.

What is the corrosion of iron known as?

Give reasons.

Aluminium is a highly reactive metal, yet it is used to make utensils for cooking.

What is meant by ‘rusting of iron’?

With the help of labelled diagrams, describe an activity to find out the conditions under which iron rusts.

What is an alloy?

How is an alloy made?

What elements are present in steel?

Give one use of the following substance:

Brass

How are the properties of steel different from those of pure iron?

Give the constituents of brass.

Name two metals which resist corrosion due to the formation of a thin, hard and impervious layer of oxide on their surface.

Name five methods of preventing rusting of iron.

What are the constituents of stainless steel?

What are the special properties of stainless steel?

Name an alloy of copper. State its chemical composition and any one use.

Explain why, when a copper object remains in damp air for a considerable time, a green coating is formed on its surface. What is this process known as?

Explain how painting of an iron gate prevents it from rusting.

How does the electrical conductivity of copper alloys, brass and bronze, differ from that of pure copper?

What is meant by 22 carat gold?

Name the metals which are usually alloyed with gold to make it harder.

Explain giving equation, what happens when:

ZnCO₃ is heated in the absence of air?

Explain giving equation, what happens when:

A mixture of Cu₂O and Cu₂S is heated.

For the reduction of a metal oxide, suggest a reducing agent other than carbon.

Explain why, an aqueous solution of sodium chloride is not used for the electrolytic extraction of sodium metal.

How are metals refined by the electrolytic process?

Describe the electrolytic refining of copper with the help of a neat labelled diagram.

Name the chemical compound which is electrolysed in molten state to obtain aluminium metal. Which gas is evolved during this process?

Name the chemical compound which is electrolysed in molten state to obtain sodium metal. Which gas is produced in this process?

Name the gas produced when calamine ore is calcined.

Name the gas evolved when cinnabar ore is roasted.

Name two metals which are found in nature mainly in the free state (as metallic elements).

Name two metals which are always found in combined state.

What iron compound is present in haematite ore? Also write its chemical formula.

What is the difference between a mineral and an ore?

Which metal is extracted from cinnabar ore?

Name one ore of sodium. Name the sodium compound present in this ore and write its chemical formula.

How is sodium metal extracted? Explain with the help of equation of the reaction involved.

Name three other metals which are extracted in a manner similar to sodium.

Name the metal which is extracted from haematite ore.

Name one ore of aluminium. Name the aluminium compound present in this ore and write its chemical formula.

How is aluminium metal extracted? Explain with the help of an equation.

Name the electrode at which aluminium metal is produced.

Which gas is produced during the extraction of aluminium? At which electrode is this gas produced?

Which metal is extracted from bauxite ore?

Give the name of one ore of iron. Which iron compound is present in this ore? Write its chemical formula.

Describe the extraction of zinc metal from its sulphide ore (zinc blende). Write equations of the reactions involved.

Explain why, the galvanised iron article is protected against rusting even if the zinc layer is broken.

Name a common metal which is highly resistant to corrosion.

Name the metal which is extracted from the ore called ‘rock salt’.

Name two ores of zinc. Write the names of the chemical compounds present in them and give their chemical formulae.

Explain how, mercury is extracted from its sulphide ore (cinnabar). Give equations of the reactions involved.

In the electrolytic refining of a metal M, what would you take as anode, cathode and electrolyte?

Name any five metals which are purified by electrolytic refining method.

Which metal is extracted from calamine ore?

Name one ore of mercury. Which mercury compound is present in this ore? Write its chemical formula.

How is copper extracted from its sulphide ore (copper glance), Cu₂S? Explain with equations of the reactions involved.

What is an alloy?

Give two examples of alloys.

How are the properties of an alloy different from those of the constitutent elements?

An ore of manganese metal is ______.

Which of the following is an iron ore?

The metal which can be extracted from the bauxite ore is ______.

The two metals which can be extracted just by heating their sulphides in air are ______.

A common metal which is highly resistant to corrosion is ______.

An important ore of zinc metal is ______.

The major ore of aluminium is known as ______.

The two metals which are extracted by means of electrolytic reduction of their molten salts are ______.

In stainless steel alloy, iron metal is mixed with ______.

If copper is kept exposed to damp air for a considerable time, it gets a green coating on its surface. This is due to the formation of ______.

Which of the following alloys contains mercury as one of the constituents?

Which of the following is an ore of mercury metal?

Calamine ore can be used to extract one of the following metals. This metal is:

Which of the following pair of metals exists in their native state in nature?

Which of the following reactants are used to carry out the thermite reaction required for welding the broken railway tracks?

Which of the following alloys contains a non-metal as one of the constituents?

During the refining of an impure metal by electrolysis, the pure metal is a deposited ______.

Which of the following metals can be obtained from haematite ore?

Brass is an alloy of ______.

The metal which is always present in an amalgam is ______.

Manganese metal is extracted from manganese dioxide by a reduction process by making use of ______.

The metal which can be extracted simply by heating the cinnabar ore in air is ______.

During galvanisation, iron metal is given a thin coating of one of the following metals. This metal is ______.

Which of the following metals are extracted by the electrolysis of their molten chlorides?

Rock salt is an ore of one of the following metals. This metal is ______.

The articles made of silver metal become dark on prolonged exposure to air. This is due to the formation of a layer of its ______.

A sulphide ore is converted into metal oxide by the process of ______.

The metal which can be extracted from pyrolusite ore is ______.

Calamine ore can be converted into zinc oxide by the process of ______.

Zinc blende ore can be converted into zinc oxide by the process of ______.

An element A which is a part of common salt and kept under kerosene reacts with another element B of atomic number 17 to give a product C. When an aqueous solution of product C is electrolysed then a compound D is formed and two gases are liberated.

1. What are A and B?
2. Identify C and D.
3. What will be the action of C on litmus solution? Why?
4. State whether element B is a solid, liquid or gas at room temperature.
5. Write formula of the compound formed when element B reacts with an element E having atomic number 5.

A metal which exists as a liquid at room temperature is obtained by heating its sulphide ore in the presence of air.

1. Name the metal and write its chemical symbol.
2. Write the name and formula of the sulphide ore.
3. Give the equations of chemical reactions involved in the production of metal from its sulphide ore.
4. Name a common device in which this metal is used.
5. Can this metal displace copper from copper sulphate solution? Why?

No chemical reaction takes place when granules of a rusty-brown solid A are mixed with the powder of another solid B. However, when the mixture is heated, a reaction takes place between its components. One of the products C is a metal and settles down in the molten state while the other product D floats over it. It was observed that the reaction is highly exothermic.

1. What could the solids A and B be?
2. What are the products C and D most likely to be?
3. Write the chemical equation for the reaction between A and B leading to the formation of C and D. Mention the physical states of all the reactants and products in this equation and indicate the heat change which takes place.
4. What is the special name of such a reaction? State one use of such a reaction.
5. Name any two types of chemical reactions under which the above reaction can be classified.

In an electrolytic tank, aluminium metal is being extracted by the electrolysis of molten aluminium oxide using carbon electrodes. It is observed that one of the carbon electrodes is gradually burnt away and has to be replaced.

1. Which carbon electrode (cathode or anode) is burnt away?
2. Why is this carbon electrode burnt away?

A metal X which is resistant to corrosion is produced by the electrolysis of its molten oxide whereas another metal Y which is also resistant to corrosion is produced by the reduction of its oxide with carbon. Metal X can be used in powder form in thermite welding whereas metal Y is used in making cathodes of ordinary dry cells.

1. Name the metals X and Y.
2. Which of the two metals is more reactive: X or Y?
3. Name one ore or metal X. Also write its chemical formula.
4. Name one ore of metal Y. Also write its chemical formula.
5. Name one alloy of metal X and one alloy of metal Y.

When an object made of metal A is kept in air for a considerable time, it loses its shine and becomes almost black due to the formation of a layer of substance B. When an object made of another metal C is kept in damp air for a considerable time, it gets covered with a green layer of substance D. Metal A is the best conductor of electricity whereas metal C is the next best conductor of electricity.

1. What is metal А?
2. What is metal C?
3. Name the substance B.
4. Name the substance D
5. What type of chemical can be used to remove the green layer from metal C and clean it? Why?

Four metals P, Q, R and S are all obtained by the reduction of their oxides with carbon. Metal P is used to form a thin layer over the sheets of metal S to prevent its corrosion. Metal Q is used for electroplating tiffin boxes made of metal S whereas metal R is used in making car batteries. Metals Q and R form an alloy called solder. What are metals P, Q, R and S? How have you arrived at this conclusion?

A black metal oxide XO₂ is used as a catalyst in the preparation of oxygen gas from potassium chlorate. The oxide XO₂ is also used in ordinary dry cells. The metal oxide XO₂ cannot be reduced satisfactorily with carbon to form metal X.

1. Name the metal X.
2. Name the metal oxide XO₂.
3. Which reducing agent can be used to reduce XO₂ to obtain metal X?
4. Name another metal which can also be extracted by the reduction of its oxide with the above reducing agent.

Metals X and Y can be recovered from the anode mud left behind after the electrolytic refining of copper metal. The coins made of metal X look new even after several years of use but the coins made of metal Y lose their shine gradually and get blackened soon. When metal X is alloyed with a small amount of metal Y, it becomes hard and hence suitable for making ornaments. What are metals X and Y? Also state the colour of metal X.

Assertion (A): To have 2 or 8 electrons in the outermost shell of an atom is always considered to be the most stable arrangement of atoms.

Reason (R): Though 8 electrons in the outermost shell always impart stability to an atom, but 2 electrons in the outermost shell of an atom impart stability only when the outermost shell is the first shell (K shell), and no other shells are present in the atom.

Assertion (A): The two important characteristics of metal elements are malleability and ductility. 

Reason (R): The property which allows the metals to be drawn into thin wires is called malleability. On the other hand, the property which allows the metals to be hammered into thin sheets is called ductility.

Assertion (A): Mercury is a less reactive metal which is quite low in the activity series. Mercury metal can be extracted just by heating its sulphide ore in air.

Reason (R): The reduction of metal oxide to form metal by using aluminium powder as a reducing agent is called a thermite reaction (or thermite process).

Assertion (A): Although solid ionic compounds are made up of ions but they do not conduct electric current in the solid state. Ionic solids conduct electricity when dissolved in water or when melted.

Reason (R): In solid ionic compounds, the ions are held together in fixed positions by strong electrostatic forces and cannot move freely. When an ionic solid is dissolved in water or melted, the crystal structure is broken down and ions become free to move and hence conduct electricity.