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Consider the oxides Li2O, CO2, B2O3. Which oxide would be the most acidic? - Chemistry

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प्रश्न

Consider the oxides Li2O, CO2, B2O3.

Which oxide would be the most acidic?

एक पंक्ति में उत्तर
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उत्तर

CO2 is the most acidic oxide.

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अध्याय 7: Modern Periodic Table - Exercises [पृष्ठ १०९]

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बालभारती Chemistry [English] Standard 11 Maharashtra State Board
अध्याय 7 Modern Periodic Table
Exercises | Q 5. (K)(b) | पृष्ठ १०९

संबंधित प्रश्न

Write the atomic number of the element present in the third period and a seventeenth group of the periodic table.


Use the periodic table to answer the following question.

Identify an element that would tend to gain two electrons.


Assign the position of the element having an outer electronic configuration in the periodic table.

ns2 np4 for n = 3


Assign the position of the element having an outer electronic configuration in the periodic table.

(n - 1)d2 ns2 for n = 4


Assign the position of the element having an outer electronic configuration in the periodic table.

(n - 2) f7 (n - 1)d1 ns2 for n = 6


Write the outer electronic configuration of the following using the orbital notation method. Justify.

Po (belongs to period 6 and group 16)


Answer the following.

La belongs to group 3 while Hg belongs to group 12 and both belong to period 6 of the periodic table. Write down the general outer electronic configuration of the ten elements from La to Hg together using the orbital notation method.


Answer the following question.

The electronic configuration of some element is given below:

1s2

In which group and period of the periodic table the element is placed?


Answer the following question.

The electronic configuration of some element is given below:

1s2 2s2 2p6

In which group and period of the periodic table the element is placed?


Consider the oxides Li2O, CO2, B2O3.

Give the formula of an amphoteric oxide.


The first ionisation enthalpies of \[\ce{Na, Mg, Al}\] and \[\ce{Si}\] are in the order:


Which of the following sets contain only isoelectronic ions?

(i) \[\ce{Zn^{2+}, Ca^{2+}, Ga^{3+}, Al^{3+}}\]

(ii) \[\ce{K+ , Ca^{2+}, Sc^{3+}, Cl-}\]

(iii) \[\ce{P^{3-}, S^{2-}, Cl- , K+}\]

(iv) \[\ce{Ti^{4+}, Ar, Cr^{3+}, V^{5+}}\]


An element belongs to 3rd period and group-13 of the periodic table. Which of the following properties will be shown by the element?

(i) Good conductor of electricity

(ii) Liquid, metallic

(iii) Solid, metallic

(iv) Solid, non metallic


How would you explain the fact that first ionisation enthalpy of sodium is lower than that of magnesium but its second ionisation enthalpy is higher than that of magnesium?


How does the metallic and non-metallic character vary on moving from left to right in a period?


Justify the given statement with suitable examples— “the Properties of the elements are a periodic function of their atomic numbers”.


Write down the outermost electronic configuration of alkali metals. How will you justify their placement in group 1 of the periodic table?


E.N. of Si is ______. (Covalent radius of Si = 1.175 Å)


\[\ce{_92U^235}\] is a member of VI B group. The new element formed by the emission of α-particle will be a member of ______ group.


The IUPAC nomenclature of an element with electronic configuration [Rn] 5f146d17s2 is ______.


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