Reactions

Front

The Law of Conservation of Mass

Back

 a fundamental idea in science that says matter cannot be created or destroyed in a chemical reaction. Instead, the atoms present at the beginning of the reactions (the reactants) are simply rearranged to form the substance at the end of the reaction (the products).

Front

Why is it best to demonstrate the Law of Conservation in a closed system

Back

As mass cannot be created or destroyed, it can only be rearranged. In a closed system mass cannot enter or escape so the mass stays the same in all closed systems.

Front

Cation

Anion

Back

A positively charged ion, it has lost electrons

A negatively charged ion, it has gained electrons

Front

Ionic compounds

Back

when a metal reacts with a non-metal. The metal gives away electrons to the non-metal forming ions. The metal becomes a positive ion (cation) and the non-metal becomes a negative ion (anion)

Front

What are the steps to write an ionic compound formula?

Back

1. 1. Identify that the compound is ionic with a metal and non-metal

2. 2. Identify the valencies/charges of the ions using a periodic table

3. 3. Write the metal atom and its charge first and the non-metal atom or group and its charge second

4. 4. Use the crossover method to swap the charges of the atoms

5. 5. Simplify ratios if possible

6. 6. Use brackets if there is more than one polyatomic io

Front

Find the formulas for:

Na and Cl

Mg and I

Al and S

Back

Front

Naming ionic compounds

Back

1. 1. The metal atom is named first and keeps its full name

2. 2. The non-metal atom is named second and the end of its name is replaced with -ide (only for single ions)

Front

Name these compounds:

K₂O

1. AlCl₃

2. BaCO₃

Back

Potassium oxide

Aluminium chloride

Barium carbonate

Front

Naming formulas of polyatomic ions

• Ethanoate

• Ammonium

• Carbonate

• Hydroxide

• Hydrogen carbonate

• Nitrate

• Nitrite

• Phosphate

• Sulfate

Back

• Ethanoate (CH₃COO⁻ )

• Ammonium (NH₄⁺)

• Carbonate (CO₃²⁻)

• Hydroxide (OH⁻)

• Hydrogen carbonate (HCO₃⁻)

• Nitrate (NO₃⁻)

• Nitrite (NO₂)

• Phosphate (PO₄³⁻)

• Sulfate (SO₄²⁻)

Front

Name the polyatomic ions

• (CH₃COO⁻ )

• (NH₄⁺)

• (CO₃²⁻)

• (OH⁻)

• (HCO₃⁻)

• (NO₃⁻)

• (NO₂)

• (PO₄³⁻)

• (SO₄²⁻)

Back

• Ethanoate (CH₃COO⁻ )

• Ammonium (NH₄⁺)

• Carbonate (CO₃²⁻)

• Hydroxide (OH⁻)

• Hydrogen carbonate (HCO₃⁻)

• Nitrate (NO₃⁻)

• Nitrite (NO₂)

• Phosphate (PO₄³⁻)

• Sulfate (SO₄²⁻)