1. What does a bond dipole represent in a polar covalent bond?
A.
Separation of positive and negative charges
B.
Complete transfer of electrons
C.
Equal sharing of electrons
D.
Formation of a metallic lattice
Correct Answer:
Separation of positive and negative charges
Explanation:
A bond dipole represents the separation of partial positive and partial negative charges in a polar covalent bond.
2. The bond dipole in a polar covalent bond is caused by unequal sharing of:
A.
Protons
B.
Neutrons
C.
Bonding electrons
D.
Nuclei
Correct Answer:
Bonding electrons
Explanation:
A bond dipole arises when the bonding electrons are shared unequally between two bonded atoms.
3. Which symbol is commonly used to represent bond dipole moment?
A.
μ
B.
λ
C.
ρ
D.
σ
Correct Answer:
μ
Explanation:
The Greek letter μ (mu) is commonly used to denote dipole moment, including bond dipole moment.
4. In a polar bond, the atom with greater electronegativity generally acquires:
A.
A partial positive charge
B.
A partial negative charge
C.
A complete positive charge
D.
No charge at all
Correct Answer:
A partial negative charge
Explanation:
The more electronegative atom attracts the bonding electrons more strongly and therefore develops a partial negative charge.
5. What is the usual unit of dipole moment used in chemistry?
A.
Debye
B.
Pascal
C.
Joule
D.
Kelvin
Correct Answer:
Debye
Explanation:
Dipole moments, including bond dipoles, are commonly expressed in the unit Debye (D).
6. A bond between two identical atoms generally has a bond dipole moment of:
A.
Zero
B.
One Debye
C.
Two Debye
D.
An infinitely large value
Correct Answer:
Zero
Explanation:
Identical atoms have the same electronegativity and share bonding electrons equally, so their bond dipole moment is zero.
7. The magnitude of a bond dipole moment depends mainly on the charge separation and the:
A.
Distance between the charges
B.
Number of neutrons
C.
Mass of the molecule only
D.
Boiling point of the substance
Correct Answer:
Distance between the charges
Explanation:
Bond dipole moment depends on the magnitude of separated charge and the distance between the centers of positive and negative charge.
8. In a bond dipole representation, the arrowhead generally points toward the:
A.
More electronegative atom
B.
Less electronegative atom
C.
Central nucleus only
D.
Atom with greater atomic mass
Correct Answer:
More electronegative atom
Explanation:
The dipole arrow is conventionally directed toward the more electronegative atom, which carries the partial negative charge.
9. Which bond is expected to have a bond dipole?
A.
H–H
B.
Cl–Cl
C.
H–Cl
D.
N–N
Correct Answer:
H–Cl
Explanation:
Hydrogen and chlorine have different electronegativities, so the H–Cl bond has unequal electron sharing and a bond dipole.
10. A larger electronegativity difference between two bonded atoms generally produces a:
A.
Smaller bond dipole
B.
Larger bond dipole
C.
Zero bond dipole
D.
Bond with equal charge distribution
Correct Answer:
Larger bond dipole
Explanation:
A greater electronegativity difference causes greater charge separation in the bond, usually resulting in a larger bond dipole.
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