Lab exam

Chemistry: Based off the types of chemical reactions lab. Be familiar with all nomenclature, balancing, naming reactions, and predicting products

  1. Naming Ionic and Covalent bonds

  • Ionic: A metal and a non metal

  • Covalent: Two non-metals

  • First element remains unchanged for both bonds

  • Last element changes to ide

  • For covalent: Prefixes for numbers

  • Ionic: No prefixes

  • Covalent prefixes: Mono, Di, Tri, Tetra, Penta, Hexa, hepta, Octa, Nona, Deca

  • Mono is not used for the FIRST element but USED for SECOND element

  • Ionci Compund Octet Rule: So for ionic compound we have to balance the charges to amke it neutral so we need to do the cross method


  • Multivalent Ions (so basically those elements with teo ro more charges suchs as Fe(iron)

  • Use ROMAN NUMERALS

  • PRACTICE!!!

  • NAMING POLYATOMIC IONS: 

  • Same Charges(meaning this would cancel their charges out):

 -  magnesium carbonate → MgCO3 

 - LiC2H3O2 → lithium acetate (C2H3O2 = acetate)

      -  Different charges:

- aluminum sulfate → Al2(SO4)3  (Al = 3+ and SO4 = 2-)

- Ca(OH)2 → calcium hydroxide

    - Both are Polyatomic ions

- ammonium sulfate → (NH4)2 SO4   (SO4 = 2- and NH4 = 1+)

NH4NO3 → ammonium nitrate

  • ACIDS:

  • Binary Acids (Hydrogen + Nonmetal):

       -  Structure: H+nonmetalH+nonmetal

                               - Naming Rule:

 - Use the prefix “hydro-”

 - Use the root of the nonmetal's name.

 - Add the suffix “-ic acid.”

Examples: HClHCl: Hydrochloric acid

  •  Oxyacids (Hydrogen + Polyatomic Ion):

    • These acids contain oxygen. The name depends on the polyatomic ion:

      • If the ion ends in "-ate":

  • Replace "-ate" with "-ic acid."

  • If the ion ends in "-ite":

  • Replace "-ite" with "-ous acid."

Examples: 

1. HNO3HNO3​: Nitric acid (from nitrate, NO3−NO3−​) 

     2. HNO2HNO2​: Nitrous acid (from nitrite, NO2−NO2−​)

  • Binary Acids (No Oxygen):
    HClHCl: Hydrochloric acid
    HBrHBr: Hydrobromic acid

  • Oxyacids (With Oxygen):

  • "-ate" → "-ic acid"
    1. HNO3HNO3​: Nitric acid
    2. H2CO3H2​CO3​: Carbonic acid

  • "-ite" → "-ous acid"
    1. HNO2HNO2​: Nitrous acid
    2. H2SO3H2​SO3​: Sulfurous acid

  • BASES: 

  • Bases typically consist of a metal cation (positive ion) and the hydroxide anion OH−OH−.

  • The name of the base is similar to the naming of ionic compounds: name the metal first, followed by "hydroxide."

  • If the metal can have multiple oxidation states (like transition metals), include a Roman numeral to indicate the charge.

  • Example: Fe(OH)₃

  • Iron(III) hydroxide

  • (Iron has a 3+ charge, so it is named as Iron(III))

  1. TYPES OF REACTION:

  • Synthesis:

   A + B → AB

            Example: 2H2​+O2​→2H2​O

Naming: "Hydrogen gas combines with oxygen gas to form water."

      -     Decomposition:

  AB → A + B

Example: 2KClO3​→2KCl+3O2​

Naming: "Potassium chlorate decomposes to form potassium chloride and oxygen gas."

  •  Single Displacement Reaction:

   A + BC → AC + B  

Example: Zn+CuSO4​→ZnSO4​+Cu

Naming: "Zinc displaces copper in copper(II) sulfate to form zinc sulfate and copper."

  • Double Displacement Reaction:

   AB + CD → AD + CB

Example: NaCl+AgNO3​→NaNO3​+AgCl

Naming: "Sodium chloride reacts with silver nitrate to form sodium nitrate and silver chloride."

  • Combustion Reaction:

   Fuel + O₂ → CO₂ + H₂O 

Example: CH4​+2O2​→CO2​+2H2​O

Naming: "Methane burns in oxygen to produce carbon dioxide and water."

  • Acid Base Reaction (Neutrilization)

  Acid + Base → Salt + Water

Example: H2​SO4​+2NaOH→Na2​SO4​+2H2​O

Naming: "Sulfuric acid reacts with sodium hydroxide to form sodium sulfate and water."