Chemistry Theories of Covalent Bonding and Shapes of Molecules Mcqs Test Online

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Question 1 of 10

Chemistry

1. H–O–H bond angle in H₂O is 104.5° and not 109.28° because of

High electronegativity of oxygen

Lone pair – lone pair repulsion

Lone pair – bond pair repulsion

Bond pair – bond pair repulsion

Question 1 of 10

Question 2 of 10

2. Which is not characteristic of π bond?

π bond is formed when a sigma bond already exist

π bond results from lateral overlap of atomic orbitals.

π bond are formed from hybrid sp orbitals

π bond may be formed by the overlapping of p and /or d-orbitals.

Question 2 of 10

Question 3 of 10

3. The percentage of ionic character of bond between two atoms is calculated from the difference between their

Electron negativities

Electron affinities

Ionic

Ionization energies

Question 3 of 10

Question 4 of 10

4. Greater the dipole moment

Greater is the ionic nature

Smaller is the ionic nature

None

Lesser is the polarity

Question 4 of 10

Question 5 of 10

5. A diatomic molecule has a dipole moment of 1.2 D. If its bond distance is 1.0A°. What fraction of electric change ‘e’ exsits on each atom?

12% of e

25% of e

18% of e

30% of e

Question 5 of 10

Question 6 of 10

6. According to VESPR theory, the most probable shape of the molecule having 4 electron pairs around the central atom is

Hexagonal

Octahedral

Tetragonal

Linear

Question 6 of 10

Question 7 of 10

7. Sp³ hybridization is important in describing the bonding in:

CCl₄

AgCl

H₃O⁺

NH₄⁺

Question 7 of 10

Question 8 of 10

8. The geometry of PF₅ molecules is

Planar

Trigonal bipyramidal

Square planar

Tetrahederal

Question 8 of 10

Question 9 of 10

9. The bond energies of F₂, Cl₂, Br₂, and I₂ are 37, 58, 46 and 36k Cals, respectively. The strongest bond formed is in:

I₂

Cl₂

Br₂

F₂

Question 9 of 10

Question 10 of 10

10. In the formulation of N₂⁺ from N₂, the electron is removed from

σ pz orbital

σ px orbital

π*₂p orbital

π₂p orbital

Question 10 of 10

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