AP Chemistry Unit 2 Quiz: Bonds, Shapes, and Intermolecular Forces
Quick, free AP Chem Unit 2 practice with instant answers and short explanations.
This AP Chemistry Unit 2 quiz helps you review bonds, Lewis structures, molecular shape, polarity, and intermolecular forces. You'll get instant results with short explanations to build speed and confidence. Continue with a deeper run on our chemistry unit 2 practice test, or brush up earlier topics with the ap chemistry unit 1 test. Want a quick organic refresher? Try the functional group quiz.
Study Outcomes
- Analyze Bond Types -
Differentiate among ionic, covalent, and metallic bonds by examining electronegativity values and predicting bond character.
- Predict Molecular Geometry -
Use VSEPR theory to determine the three-dimensional shapes and bond angles of molecules in the Unit 2 review chemistry topics.
- Evaluate Intermolecular Forces -
Assess how hydrogen bonding, dipole - dipole interactions, and London dispersion forces affect boiling points, melting points, and solubility.
- Calculate Formal Charges and Resonance -
Assign formal charges and draw resonance structures to identify the most stable Lewis structures for given molecules and ions.
- Interpret Orbital Hybridization -
Describe sp, sp², and sp³ hybridizations, explaining how orbital mixing influences bond length, bond strength, and molecular shape.
- Apply Lewis Structures to Formulas -
Construct accurate Lewis dot structures to derive molecular and ionic formulas, reinforcing concepts tested in the AP Chemistry Unit 2 practice test.
Cheat Sheet
- VSEPR Theory and Geometry -
Valence shell electron pair repulsion (VSEPR) theory predicts 3D molecular shapes by minimizing electron pair repulsion using the AXE method. For example, an AB4 molecule like CH4 adopts a tetrahedral geometry with 109.5° bond angles (source: University of California). Use mnemonics such as "see-saw," "T-shaped," and "square planar" to easily recall trigonal bipyramidal derivatives.
- Covalent vs. Ionic Bond Energy -
Understanding differences between ionic, polar covalent, and nonpolar covalent bonds is crucial for the ap chemistry unit 2 practice test, as bond strength directly correlates with bond type. Ionic bonds (e.g., NaCl) typically have high lattice energies, while single covalent bonds like H - H require lower bond dissociation energies; consult NIST for precise values. Remember that greater electronegativity differences produce stronger ionic character and higher overall bond energies.
- Electronegativity and Molecular Polarity -
Use the Pauling scale to assign electronegativity values and determine bond polarity - ΔEN > 0.5 usually indicates a polar covalent bond (source: ACS Publications). For example, H2O's bent shape and polar O - H bonds create a net dipole moment, reinforcing the "like dissolves like" concept in unit 2 review chemistry. Sketching arrows toward the more electronegative atom helps visualize molecular polarity on chemistry test unit 2 style questions.
- Formal Charge and Resonance Stabilization -
Calculating formal charges (FC = valence electrons − ½ bonding electrons − nonbonding electrons) helps pinpoint the most stable Lewis structures (source: Brown University). Compare multiple resonance forms - like NO3− - and favor structures with minimal formal charge separation and negative charges on more electronegative atoms. Practice drawing resonance hybrids to boost accuracy and confidence for your ap chem unit 2 practice test.
- Intermolecular Forces and Physical Properties -
Recognize how London dispersion, dipole - dipole interactions, and hydrogen bonding influence boiling points and solubility (source: American Chemical Society). For instance, HF's strong hydrogen bonds cause an unusually high boiling point compared to other hydrogen halides. Linking these forces to molecular geometry reinforces key concepts in the chemistry unit 2 test and sharpens your exam performance.
