#chemistry chapter 2 chemical bonding and structure

1. What type of bond involves the transfer of electrons from one atom to another?
A) Covalent bond
B) Ionic bond
C) Metallic bond
D) Hydrogen bond

2. Which of the following elements is most likely to form an ionic bond with chlorine?
A) Oxygen
B) Nitrogen
C) Sodium
D) Carbon

3. A covalent bond involves:
A) Sharing of protons
B) Transfer of electrons
C) Sharing of electrons
D) Transfer of neutrons

4. In a metallic bond, electrons are:
A) Shared between two specific atoms
B) Transferred to one atom
C) Delocalized over many atoms
D) Fixed in place

5. Which is a property of ionic compounds?
A) Conduct electricity as solids
B) Have low melting points
C) Dissolve easily in water
D) Are soft and flexible

6. Which molecule contains a polar covalent bond?
A) O2
B) N2
C) H2O
D) Cl2

7. Which of the following shapes is predicted for a molecule with 2 bonding pairs and 0 lone pairs?
A) Linear
B) Bent
C) Trigonal planar
D) Tetrahedral

8. According to VSEPR theory, what is the shape of a molecule with 4 bonding pairs and 0 lone pairs?
A) Square planar
B) Tetrahedral
C) Trigonal pyramidal
D) Bent

9. What is the bond angle in a trigonal planar molecule?
A) 90°
B) 104.5°
C) 120°
D) 180°

10. The VSEPR theory is based on the idea that:
A) Electrons attract each other
B) Electrons around a central atom repel each other
C) Nuclei repel each other
D) Bonds are rigid

11. Which of the following molecules has a bent shape?
A) CO2
B) CH4
C) H2O
D) BF3

12. Which statement about metallic bonding is correct?
A) Metals have low conductivity
B) Metallic bonding involves delocalized electrons
C) Metals are brittle
D) Metallic bonds are directional

13. Valence Bond Theory (VBT) explains bonding by:
A) Delocalization of electrons
B) Overlap of atomic orbitals
C) Transfer of electrons
D) Repulsion of electron clouds

14. In VBT, the formation of a sigma (σ) bond is due to:
A) Sideways overlap of orbitals
B) End-to-end overlap of orbitals
C) Transfer of electrons
D) Delocalization

15. A pi (π) bond results from:
A) Head-on overlap of orbitals
B) Sideways overlap of p orbitals
C) Overlap of s orbitals
D) Transfer of electrons

16. In Molecular Orbital Theory (MOT), bonding molecular orbitals are formed by:
A) Addition of atomic orbitals
B) Subtraction of atomic orbitals
C) Non-overlapping orbitals
D) Hybridization

17. In MOT, an antibonding orbital is indicated by:
A) A positive overlap
B) A star (*) symbol
C) A delta (Δ) symbol
D) No symbol

18. Which of the following species has a bond order of 2?
A) O2
B) O2+
C) N2
D) O2–

19. Which molecule has a triple bond?
A) CO2
B) CH4
C) N2
D) H2O

20. In VSEPR theory, lone pairs cause:
A) Bond angles to increase
B) Bond angles to decrease
C) No change in bond angles
D) Formation of ionic bonds

Answer :

1. B) Ionic bond
2. C) Sodium
3. C) Sharing of electrons
4. C) Delocalized over many atoms
5. C) Dissolve easily in water
6. C) H₂O
7. A) Linear
8. B) Tetrahedral
9. C) 120°
10. B) Electrons around a central atom repel each other
11. C) H₂O
12. B) Metallic bonding involves delocalized electrons
13. B) Overlap of atomic orbitals
14. B) End-to-end overlap of orbitals
15. B) Sideways overlap of p orbitals
16. A) Addition of atomic orbitals
17. B) A star (*) symbol
18. A) O₂
19. C) N₂
20. B) Bond angles to decrease

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