Q. In which type of bond is the electron density concentrated above and below the bond axis?
-
A.
Sigma bond
-
B.
Pi bond
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C.
Ionic bond
-
D.
Covalent bond
Solution
In a pi bond, the electron density is concentrated above and below the bond axis due to the side-to-side overlap of p orbitals.
Correct Answer:
B
— Pi bond
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Q. What is the effect of increasing the electronegativity difference between two bonded atoms?
-
A.
Increases bond length
-
B.
Decreases bond strength
-
C.
Increases ionic character
-
D.
Decreases dipole moment
Solution
An increasing electronegativity difference leads to greater ionic character in the bond, making it more polar.
Correct Answer:
C
— Increases ionic character
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Q. What is the effect of increasing the electronegativity of atoms in a molecule on its dipole moment?
-
A.
Increases dipole moment
-
B.
Decreases dipole moment
-
C.
No effect
-
D.
Reverses dipole moment
Solution
Increasing electronegativity of atoms in a molecule increases the dipole moment as the difference in charge distribution becomes greater.
Correct Answer:
A
— Increases dipole moment
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Q. What is the primary characteristic of a sigma bond?
-
A.
Formed by side-to-side overlap
-
B.
Formed by end-to-end overlap
-
C.
Weaker than pi bonds
-
D.
Involves d orbitals
Solution
A sigma bond is formed by end-to-end overlap of orbitals, allowing for free rotation around the bond axis.
Correct Answer:
B
— Formed by end-to-end overlap
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Q. What is the primary factor that determines the strength of a covalent bond?
-
A.
Electronegativity
-
B.
Bond length
-
C.
Bond order
-
D.
Molecular weight
Solution
Bond strength increases with bond order. A higher bond order indicates more shared electron pairs, leading to a stronger bond.
Correct Answer:
C
— Bond order
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Q. What type of intermolecular force is primarily responsible for the high boiling point of water?
-
A.
London dispersion forces
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B.
Dipole-dipole interactions
-
C.
Hydrogen bonding
-
D.
Ionic interactions
Solution
Hydrogen bonding is the strongest intermolecular force present in water, significantly raising its boiling point compared to similar molecules.
Correct Answer:
C
— Hydrogen bonding
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Q. Which molecular geometry is associated with a molecule that has two bonding pairs and two lone pairs of electrons?
-
A.
Linear
-
B.
Trigonal planar
-
C.
Tetrahedral
-
D.
Bent
Solution
A molecule with two bonding pairs and two lone pairs adopts a bent geometry due to the repulsion of the lone pairs.
Correct Answer:
D
— Bent
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Q. Which molecular geometry is associated with sp2 hybridization?
-
A.
Linear
-
B.
Trigonal planar
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C.
Tetrahedral
-
D.
Octahedral
Solution
sp2 hybridization results in a trigonal planar geometry, with 120-degree bond angles due to the mixing of one s and two p orbitals.
Correct Answer:
B
— Trigonal planar
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Q. Which molecular shape corresponds to a molecule with a central atom that has one lone pair and three bonding pairs?
-
A.
Tetrahedral
-
B.
Trigonal pyramidal
-
C.
Bent
-
D.
Linear
Solution
A central atom with one lone pair and three bonding pairs adopts a trigonal pyramidal shape due to the repulsion of the lone pair.
Correct Answer:
B
— Trigonal pyramidal
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Q. Which of the following hybridizations corresponds to a tetrahedral molecular geometry?
-
A.
sp
-
B.
sp2
-
C.
sp3
-
D.
dsp3
Solution
Tetrahedral geometry corresponds to sp3 hybridization, where one s and three p orbitals mix to form four equivalent sp3 hybrid orbitals.
Correct Answer:
C
— sp3
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Q. Which of the following molecules has a nonpolar covalent bond?
-
A.
HCl
-
B.
O2
-
C.
NH3
-
D.
H2O
Solution
O2 has a nonpolar covalent bond because it consists of two identical oxygen atoms sharing electrons equally.
Correct Answer:
B
— O2
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