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WorksheetsCovalent Bonding Exam Review
Total questions: 25
Worksheet time: 20mins
What is the definition of a covalent bond?
A bond formed by sharing electrons
A bond formed by transferring electrons
A bond formed by metallic interactions
What is the difference between ionic and covalent bonds?
Ionic bonds involve electron transfer, covalent bonds involve electron sharing
Both involve electron sharing
Both involve electron transfer
Which type of covalent bond is the strongest and shortest?
Single bond
Double bond
Triple bond
What is the octet rule and what are its exceptions?
Atoms aim for 8 valence electrons; exceptions include H, B, Be, and expanded octets
Atoms aim for 6 valence electrons; exceptions include H and B
Atoms aim for 8 valence electrons; no exceptions
How does electronegativity affect bond polarity?
Higher electronegativity difference increases bond polarity
Lower electronegativity difference increases bond polarity
Electronegativity does not affect bond polarity
What is the definition of polar vs nonpolar bonds?
Polar bonds have unequal electron sharing; nonpolar bonds have equal sharing
Polar bonds have equal electron sharing; nonpolar bonds have unequal sharing
Polar bonds involve electron transfer; nonpolar bonds involve electron sharing
What are the electronegativity difference ranges for bond types?
<0.5 for nonpolar, 0.5–1.7 for polar, ≥1.8 for ionic
<0.5 for polar, 0.5–1.7 for ionic, ≥1.8 for nonpolar
<0.5 for ionic, 0.5–1.7 for nonpolar, ≥1.8 for polar
What is the definition of a polar molecule?
A molecule with uneven electron distribution
A molecule with even electron distribution
A molecule with no electron distribution
How does molecular symmetry affect polarity?
Symmetrical molecules are nonpolar; asymmetrical molecules are polar
Symmetrical molecules are polar; asymmetrical molecules are nonpolar
Symmetry does not affect polarity
Why do lone pairs make molecules polar?
Lone pairs create asymmetry in electron distribution
Lone pairs create symmetry in electron distribution
Lone pairs do not affect polarity
Which molecules are polar: H₂O, NH₃, SO₂?
H₂O and NH₃
SO₂ and NH₃
H₂O, NH₃, and SO₂
Which molecules are nonpolar: CO₂, CH₄, BF₃, XeF₂?
CO₂ and CH₄
BF₃ and XeF₂
CO₂, CH₄, BF₃, and XeF₂
What is VSEPR theory?
Valence Shell Electron Pair Repulsion Theory
Valence Shell Electron Pair Attraction Theory
Valence Shell Electron Pair Sharing Theory
How do lone pairs affect bond angles?
Lone pairs decrease bond angles
Lone pairs increase bond angles
Lone pairs do not affect bond angles
What is the relationship between bond order, bond strength, and bond length?
Higher bond order means stronger and shorter bonds
Higher bond order means weaker and longer bonds
Bond order does not affect strength or length
Which IMFs are present in H₂O, CH₄, NH₃, HF, Cl₂?
Hydrogen bonding in H₂O and HF; LDF in CH₄ and Cl₂; Dipole–Dipole in NH₃
Hydrogen bonding in CH₄ and Cl₂; LDF in H₂O and HF; Dipole–Dipole in NH₃
Hydrogen bonding in NH₃ and Cl₂; LDF in H₂O and HF; Dipole–Dipole in CH₄
True or False: Lone pairs always make a molecule polar.
True
False
True or False: H₂O has hydrogen bonding.
True
False
True or False: CO₂ has polar bonds but is a nonpolar molecule.
True
False
True or False: LDF forces occur only in nonpolar molecules.
True
False
True or False: Ionic bonds share electrons.
True
False
True or False: Polar molecules have uneven electron distribution.
True
False
Predict the shape, polarity, and IMF of XeF₂, SF₆, and PF₃.
Explain why XeF₂ is nonpolar even though it has lone pairs.
Compare the bond angles of CH₄, NH₃, and H₂O and explain why they differ.
