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General Chemistry — Atoms, Bonding, Stoichiometry & Gases flashcards

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Quantum numbers and electron configuration, periodic trends with their reasons, bonding and Lewis structures, VSEPR and polarity, intermolecular forces, mole and stoichiometry problems, concentration units, gas laws and real-gas behavior, and thermochemistry.

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Learn deck · part of General Chemistry I/II · written against: Standard two-semester sequence. Updated 2026-10-10.

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  1. What does each of the four quantum numbers describe, and what values can it take?
    • n sets the shell and energy (1, 2, 3…);
    • l sets the subshell shape (0 to n − 1, labeled s, p, d, f);
    • mlm_l sets the orbital's orientation (−l to +l);
    • msm_s is the spin (+½ or −½). No two electrons in an atom share all four.
    Atomic Structure & Quantum Numbers
  2. State the Aufbau principle, Hund's rule and the Pauli exclusion principle.
    • Aufbau: fill orbitals from lowest energy upward (1s 2s 2p 3s 3p 4s 3d…);
    • Hund: within a subshell, give each orbital one electron with parallel spins before pairing any;
    • Pauli: no two electrons can share all four quantum numbers, so an orbital holds at most two, spin-paired.
    Electron Configuration
  3. How does atomic radius change across a period and down a group, and why?
    It shrinks across a period because the rising effective nuclear charge pulls the same shell inward, and grows down a group as new shells are added and inner electrons shield more. Francium and cesium are the largest atoms; helium, neon and fluorine among the smallest.
    Periodic Trends
  4. What are the steps for drawing a Lewis structure?
    • Count the total valence electrons (adjusting for charge);
    • place the least electronegative non-hydrogen atom in the center;
    • connect atoms with single bonds;
    • complete the outer atoms' octets;
    • put leftovers on the central atom;
    • and convert lone pairs into multiple bonds if the center still lacks an octet. Finish by checking formal charges.
    Lewis Structures
  5. What molecular shapes and bond angles go with two to six electron domains when there are no lone pairs?
    • 2 domains → linear, 180°;
    • 3 → trigonal planar, 120°;
    • 4 → tetrahedral, 109.5°;
    • 5 → trigonal bipyramidal, 90° and 120°;
    • 6 → octahedral, 90°.
    • Domains — single, double or triple bonds and lone pairs — spread out to minimize repulsion.
    VSEPR · Hybridization & Polarity
  6. Rank the intermolecular forces from strongest to weakest, and what is required for hydrogen bonding?
    For molecules of similar size: ion–dipole > hydrogen bonding > dipole–dipole > London dispersion. Hydrogen bonding needs a hydrogen bonded to N, O or F interacting with a lone pair on another N, O or F.
    Intermolecular Forces
  7. How many molecules are in 9.0 g of water?
    9.0 g ÷ 18.0 g/mol = 0.50 mol, and one mole holds 6.022 × 10²³ particles, so 3.0 × 10²³ molecules (and three times as many atoms). The molar mass in grams is the bridge between the balance and Avogadro's number.
    Moles & Stoichiometry
  8. State the ideal gas law with the common values of R, and give the molar volume at STP.
    PV=nRTPV = nRT⁠, with R = 0.08206 L·atm/(mol·K) or 8.314 J/(mol·K), and T in kelvin. One mole of ideal gas occupies 22.4 L at STP (0 °C, 1 atm; 22.7 L at the IUPAC 1 bar standard).
    Gas Laws
  9. What are the main postulates of the kinetic molecular theory of gases?
    Gas particles have negligible volume, move constantly and randomly, exert no attractive or repulsive forces on one another, collide elastically, and have an average kinetic energy that depends only on absolute temperature — KEavg=32RTKE_{avg} = \frac{3}{2}RT per mole.
    Kinetic Molecular Theory & Real Gases
  10. What are the sign conventions for exothermic and endothermic processes, and for heat and work in the first law?
    • Exothermic: heat leaves the system, ΔH < 0 (combustion, freezing);
    • Endothermic: heat enters, ΔH > 0 (melting, dissolving ammonium nitrate);
    • In ΔE=q+w\Delta E = q + w⁠, both q and w are positive when energy flows into the system.
    Thermochemistry

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About these cards

Review status: Second-reader reviewed, with corrections applied.

Checked against:

  • OpenStax Chemistry 2e, consulted as a reference; no text copied.
  • Checked against Zumdahl, Zumdahl & DeCoste, Chemistry, 10th ed. (Cengage, 2018) (reference only; no text copied).

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