1. Reactants
2. Products

1. The starting materials in a chemical reaction
2. The substances formed in a chemical reaction.

Which elements are gases at room temperature? Which are liquids? Which are solids?

Gases: H₂, N₂, O₂, F₂, Cl₂, He, Ne, Ar, Kr, Xe, Rn

Liquids: Hg, Br

Solids: All the rest

Balance equations:

1. H₂ + O₂ ↔ H₂O
2. Sn + O₂ ↔ SnO₂

1. 2H₂ + O₂ ↔ 2H₂O
2. Balanced

Balance equations:

1. H₂ + N₂ ↔ NH₃
2. NaCl + Br₂ ↔ NaBr + Cl₂

1. 3H₂ + N₂ ↔ 2NH₃
2. 2NaCl + Br₂ ↔ 2NaBr + Cl₂

Diatomic

List 7 diatomic elements found in nature

A molecule composed of two atoms.

H₂, N₂, O₂, Cl₂, F₂, Br₂, I₂

Write a balanced equation-

1. Sulfur and oxygen form sulfur dioxide
2. Dinitrogen pentoxide forms nitrogen and oxygen

1. S + O₂ ↔ SO₂
2. 2N₂O₅ ↔ 2N₂ + 5O₂

1. Synthesis or combination
2. Decomposition

1. A reaction where 2 or more elements form a compound.

N₂ + 3H₂ ↔ 2NH₃;

2H₂ + O₂ ↔ 2H₂O

  2. A reaction where a compound breaks down into elements.

CO₂ ↔ C + O₂;

2CaO ↔ 2Ca + O₂

1. Single replacement
2. Double replacement

1. A reaction involving the replacement in a compound of an element by another element.

Zn + CuCl₂ ↔ Cu + ZnCl₂

   2. A reaction where two ionic substances "trade" anions.

NaCl + AgNO₃ ↔ NaNO₃ + AgCl

Identify type of reaction:

1. Mg + H₂SO₄ ↔ H₂ + MgSO₄
2. Ca + Br₂ ↔ CaBr₂

1. Single replacement
2. Combination

Identify type of reaction:

1. FeS ↔ Fe + S
2. KI + AgOH ↔ KOH + AgI

1. decomposition
2. double replacement

Precipitation

Give an example

Two ionic solutions are mixed and an insoluable product is formed.

(Double replacement)

NaCl + AgNO₃ ↔ NaNO₃ + AgCl (solid)