Science

• Types of Chemical Reactions

  Synthesis, Decomposition, Single Displacement, and Double Displacement reactions.
• Chemical Change Examples

  Burning, Rusting, Cooking, Photosynthesis, Combustion of Fossil Fuels, Dry Cleaning, and Plastic Degradation.
• Chemical Change


  A process where one or more substances are transformed into new substances with different properties, often irreversible.
• Identifying Chemical Changes

  Color, Odor, Taste, Texture, Temperature Change, Sound, Gas Release, Heavy or Light Consistency, Emission of Light, and Unusual Appearance.
• Physical Properties Examples

  Temperature, Density, Color, Texture, and Shape.
• IUPAC

  International Union of Pure and Applied Chemistry, created a standardized set of rules used to name chemical compounds
• Identifying compound type 1. the formula begin with hydrogen (H)

  2. bonds are covalent(contains only non-metal elements)

  3. contains a polyatomic ion
• Binary ionic compounds


  Contain only two different elements
• Polyatomic ionic compounds


  Contain a metal cation and a polyatomic ion
• Writing chemical formulas for regular binary ionic compounds

  1. Determine the charge (oxidation number) on each element

  2. Use the crossover rule to find the chemical formula
• Subscripts must be reduced to their lowest common denominator
• Naming ionic compounds

  Take the name of the metal element and follow it with the name of the non-metal element, with the ending changed to -ide
• Naming ionic compounds

  • NaCl = sodium chloride
  • MgO = magnesium oxide
  • AlN = aluminum nitride
• Nomenclature of binary compounds

  • AgCl (silver chloride)
  • Li2O (lithium oxide)
  • MgBr2 (magnesium bromide)
  • ZnO (zinc oxide)
  • KF (potassium fluoride)
  • BaS (barium sulfide)
  • Rb2S (rubidium sulfide)
• Ionic Compound


  A type of compound formed when two or more atoms share one or more electrons to form ions, resulting in the formation of a bond between them.
• MgCl2


  Magnesium Chloride: A white crystalline solid, used as a disinfectant
• NaNO3

  Sodium Nitrate: A white crystalline solid, used as a fertilizer
• CaO

  Calcium Oxide, Calcium Oxide: A white solid, highly reactive substance
• Polyatomic Ion


  A group of atoms that have a collective charge, either positive (cation) or negative (anion), composed of multiple atoms bonded together and carry a charge.
• Ca(NO3)2

  Calcium Nitrate: A white crystalline solid, used as a fertilizer and in the manufacture of textiles
• MgSO4


  Magnesium Sulfate: A white crystalline solid, used in medical treatments and as a laxative
• Al2(CO3)3


  Aluminum Carbonate: A white solid, used as a pigment and in the production of ceramics
• Ionic Compounds with Polyatomic Ions


  Ionic compounds that contain polyatomic ions, which are groups of atoms that have a positive or negative charge.
• Ionic Compounds with Multivalent Elements


  Ionic compounds where one or more of the elements involved are multivalent, exhibiting more than one oxidation state.
• Molecular/Covalent Compounds

  Molecular/covalent compounds formed by the sharing of electrons between atoms, exhibiting specific oxidation states.
• Ionic Compound vs Molecular Compound


  Ionic Compound: Formed by electrostatic forces between oppositely charged ions.
• Molecular Compound


  Molecular compound: Formed by covalent bonds between atoms, where electrons are shared between atoms.
• Molecular Compound Examples

  Water (H2O), ammonia (NH3), carbon dioxide (CO2), and methane (CH4)
• Ionic Compound Examples

  Table salt (NaCl), calcium carbonate (CaCO3), and copper sulfate (CuSO4)
• Carbon Tetrachloride


  CCl4
• Aluminum Chloride


  AlCl3
• Lead (IV) Oxide


  PbO2
• Copper (II) Nitrate


  Cu(NO3)2
• Here are the chemical formulas for the ionic compounds:1. Aluminum chloride: AlCl32. Lead (IV) oxide: PbO23. Copper (II) nitrate: Cu(NO3)2
• Molecular compounds are made up of neutral, nonmetal atoms that share electrons in covalent bonds.
• in a combustion reaction a hydrocarbon reacts with oxygen to produce carbon dioxide and water
• in a balanced chemical equation, the number of atoms of reactants is less than the number of atoms of products
• Law of Conservation of Mass


  During a chemical reaction, the total mass of the reactants is equal to the total mass of the products.
• Double Displacement Reaction


  A type of chemical reaction where two compounds swap partners to form two new compounds, resulting in the exchange of ions or radicals
• Single Displacement Reaction


  A type of chemical reaction where one element displaces another element from a compound, resulting in a new compound