chemistry grade 10

• Solids


  • Definite shape and volume
  • Particles tightly packed together with strong forces of attraction
  • Not easily compressible
• Solids


  • Wood
  • Metal
  • Plastic
• Liquids


  • Definite volume but take the shape of the container
  • Particles close together but not fixed in position
  • Less compressible than solids but more compressible than gases

  
• Liquids


  • Water
  • Oil
  • Alcohol
• Gases


  • No definite shape or volume
  • Particles far apart and move freely at high speeds
  • Weak forces of attraction between particles
  • Highly compressible
• Gases


  • Oxygen
  • Nitrogen
  • Carbon dioxide
• Kinetic Molecular Theory of Gases


  Theory emphasizing that gas travels at constant, random, straight-line motion

  
• Postulates of Kinetic Molecular Theory

  • Gases are composed of very tiny particles (molecules)
  • No intermolecular forces between gas molecules
  • Molecules in constant, random, straight-line motion
  • Molecules constantly collide with each other and container walls
  • Average kinetic energy of molecules proportional to temperature (Kelvin)

  
• Volume


  Amount of space an object is occupying or enclosed within a container
• Units of volume


  • cubic kilometer (km³)
  • hectometer cubic (hm³)
  • decameter cubic (dam³)
  • cubic meter (m³)
  • liter (L)
  • cubic decimeter (dm³)
  • cubic centimeter (cm³)
  • cubic millimeter (mm³)
• Mole


  Unit of measurement used to specify the amount or mass of a substance
• Temperature


  Measure of hotness or coldness expressed in Celsius, Fahrenheit, and Kelvin
• Temperature conversion formulas


  • T_F = 1.8C + 32
  • T_C = 5/9(F - 32)
  • T_K = C + 273.15
  • T_C = K - 273.15
  • T_K = 5/9(F - 32) + 273.15
  • T_F = (K - 273.15)(1.8) + 32
• Pressure


  Force exerted by gas molecules colliding with surfaces or container walls
• Units of pressure


  • atmosphere (atm)
  • torr
  • millimeters of mercury (mmHg)
  • pascal (Pa)
  • pound per square inch (psi)
  • bar
• Boyle's Law


  When temperature is held constant, the volume of a fixed amount of gas is inversely proportional to its pressure

  
• Boyle's Law


  P_1V_1 = P_2V_2
• Charles' Law


  The volume of a fixed amount of gas is directly proportional to the temperature in Kelvin units

  
• Charles' Law


  V_1/T_1 = V_2/T_2
• Gay-Lussac's Law


  When volume of a fixed amount of gas is held constant, pressure is directly proportional to the temperature

  
• Gay-Lussac's Law


  P_1/T_1 = P_2/T_2
• Avogadro's Law


  Equal volumes of all gases at the same pressure and temperature contain the same number of molecules
• Avogadro's Law


  V_1/n_1 = V_2/n_2
• Combined Gas Law


  Ratio of the product of pressure and volume and the absolute temperature of a gas is equal to a constant

  
• Combined Gas Law


  (P_1V_1)/T_1 = (P_2V_2)/T_2
• Ideal Gas Law


  PV = nRT, where R is the ideal gas constant

  
• Ideal Gas


  • Particles have negligible volume
  • Particles are uniform in size
  • No intermolecular forces
  • No energy loss upon collision
  • Constant, random, straight-line motion

  
• Chemical Reaction


  Process where chemical bonds are broken or formed, accompanied by heat/light production, precipitate formation, gas evolution, color change, or temperature change
• Chemical Change


  Substances being converted to entirely new substances, cannot be easily reverted
• Atoms


  Smallest unit of matter composed of electrons, protons, and neutrons, with balanced number of protons and electrons
• Ions


  Atoms that are electrically charged, either positively or negatively due to imbalance of protons and electrons
• Chemical Bonding


  Process where elements are connected by a chemical bond, resulting in different compound behaviors
• Ionic Bonding


  Bonding formed from electrostatic attraction between oppositely charged ions, with gain or loss of valence electrons
• Covalent Bonding


  Bonding where atoms share electrons, can be polar (unequal sharing) or nonpolar (equal sharing)
• Chemical Equation


  Symbolic representation of a chemical reaction, with reactants on the left and products on the right
• Symbols used in chemical equations

  • + (addition)
  • → (produces/forms/yields)
  • ↑ (gas evolved)
  • ↓ (precipitate formed)
  • ⇄ (reversible reaction)
  • (s) (solid state)
  • (l) (liquid state)
  • (g) (gas state)
  • (aq) (aqueous solution)
  • Δ (heat supplied)
  • Pt (catalyst or solvent)
• Combination/Synthesis Reaction


  Two or more reactants combine to form a single product
• Combination/Synthesis Reaction


  A + B → AB
• Decomposition Reaction


  A single reactant is broken down into two or more products
• +


  To indicate that the substances are being added or mixed together