General Chemistry 1 Study Notes

Common Polyatomic Ions

  • Name - Formula
  • Acetate - C₂H₃O₂⁻
  • Ammonium - NH₄⁺
  • Carbonate - CO₃²⁻
  • Hydrogen Carbonate (Bicarbonate) - HCO₃⁻
  • Hydroxide - OH⁻
  • Nitrate - NO₃⁻
  • Nitrite - NO₂⁻
  • Phosphate - PO₄³⁻
  • Sulfate - SO₄²⁻
  • Sulfite - SO₃²⁻
  • Hydrogen Sulfate (Bisulfate) - HSO₄⁻
  • Permanganate - MnO₄⁻
  • Cyanide - CN⁻
  • Chromate - CrO₄²⁻

SI Prefix Multipliers

  • Prefix - Symbol - # Base in Prefix - # Prefix in Base
  • Peta - P - 10¹⁵
  • Tera - T - 10¹²
  • Giga - G - 10⁹
  • Mega - M - 10⁶
  • Kilo - k - 10³
  • Deci - d - 10¹
  • Centi - c - 10²
  • Milli - m - 10³
  • Micro - μ - 10⁻⁶
  • Nano - n - 10⁻⁹
  • Pico - p - 10⁻¹²

Isotopes of Neon

  • Ne-20: 90.48%
  • Ne-21: 0.27%
  • Ne-22: 9.25%

Temperature Scales

  • Celsius Scale: 0°C (freezing point of water), 100°C (boiling point of water)
  • Kelvin Scale: Absolute zero at 0 K, K = °C + 273.15

Classification of Matter

  • States: Solid, Liquid, Gas
  • Matter: Comprised of pure substances and mixtures.
    • Mixtures: Heterogeneous and Homogeneous
    • Compounds: Elements combined chemically.

Atomic Structure

  • Atoms are composed of protons, neutrons, and electrons.
  • Atomic Number: Number of protons in the nucleus.
  • Electron Configuration: Distribution of electrons in orbitals.

The Mole Concept

  • Mole (mol): Amount of substance containing 6.022imes10236.022 imes 10^{23} particles (Avogadro’s number)
  • Molar Mass: Mass of 1 mole of a substance.

Periodic Properties

  • Periodic Law: Properties repeat when elements are arranged by increasing atomic mass.
  • Trends: Ionization energy, electronegativity, atomic radius.

Chemical Bonds

  • Types: Ionic, Covalent, Metallic.
  • Lewis Structures: Used to represent valence electrons and predict bonding scenarios.

Chemical Reactions

  • Equations: Express reactants and products.
  • Balancing: Must ensure same number of each atom on both sides.

Solutions and Concentrations

  • Molarity (M): Moles of solute per liter of solution.
  • Dilutions: M1V1 = M2V2

Acids and Bases

  • Arrhenius Acid/Base: Substance that generates H⁺/OH⁻ in solution.
  • Bronsted-Lowry Definition: Acids are proton donors, bases are proton acceptors.