Chemistry 100 - Review Sheet for Exam #1

• Units of measurement
• SI (Internations system of units)
• Metric system
• Metric units of measurement:
  • Length - meter (m)
  • Volume - Liter (L)
  • Mass - gram (g)
  • Temperature
    • Celsius (oC)
    • Kelvin (K)
  • Time - seconds (s)
• Scientific notation
• Measured number
• Exact number
• Signifcant Figures
• Rounding numbers
• SI and metric prefixes
  • Giga (G) — 10⁹
  • Mega (M) — 10⁶
  • kilo (k) —10³
  • centi (c) — 10^-2
  • milli (m) — 10^-3
  • micro (m) — 10^-6
  • nano (n) — 10^-9
• Measurements
• Precision
• Accuracy
• Conversion factors
  • 2.54 cm/in
  • 5280 ft/mile
  • 12 in/ft
  • 3 ft/yd
  • 454 g/lb
  • 1 cm³ = 1 mL
• Percent as conversion factors
• Density (D = mass/vol)
• Specific gravity

Chapter 3: Radioactivity

• Element
• Atomic number (Z)
• Isotope
• Isotope mass (number)
• a particle
• Helium nucleus (⁴₂He)
• b particle
• Electron (⁰_-1e)
• Radioactive decay equations
• Half life
• Fusion
• Fission

• Elements
• Chemical symbols
• Periodic table
• Groups (vertical columns)
  • Alkali metals (Group I)
  • Alkaline earth metals (Group II)
  • Halogens (Group VII)
  • Noble Gases (Group VIII)
• Periods (horizontal rows)
• Metals
• Non-metals
• Daltons atomic theory
  • Atom
  • Electron (negative)
  • Proton (positive)
  • Neutron (neutral)
• Atomic mass (amu)
• Isotopes
  • Atomic number (Z)
  • Mass number (protons + neutrons)
• Average atomic mass
• Electron arrangement
• Periodic law
• Energy levels

Chapter 4: Compounds and Their Bonds

• Valence electrons
• Electron-dot structures
• Ions
• Octet rule
• Compounds
• Cations (postively charged ions)
• Anions (negatively charged ions)
• Predicting charge for ionic compunds
  • Metals
    • Group I always +1
    • Group II always +2
    • Aluminum always +3
  • Non-metals (Group No. - 8)
    • Group VII always -1 (Cl^-)
    • Group VI always -2 (O^2-)
    • Group V always -3 (N^3-)
• Ionic compounds
• Naming ionic compounds
  • Group I and II metals, plus Al
  • Transition metals
• Covalent bonds
• Molecule
• Sharing electrons between different elements
• Multiple covalent bonds
• Steps for writing electron-dot structures
• single, double and triple bonds
• Electronegativity value
• Polar covalent bond
• Nonpolar covalent bond
• Polar molecules
• Polyatomic ions (e.g., NO₃^-, SO₄^2-, OH^-, NH₄⁺)
• Naming polyatomic ions
• Formulas for compounds with polyatomic ions
• Naming compounds with polyatomic ions