Review Before Predicting Products

Reviewing Metals and Nonmetals (Unit 1-2)

Check your periodic table. Do you
have the metals and nonmetals
labelled?

Reviewing Ionic vs Covalent (Unit 3)

When a metal bonds with a nonmetal, it’s ionic

A compound that only contains nonmetals is covalent

Reviewing Ionic Bonding (Unit 3)

To write the ionic compound’s formula, we have to look up the charges of
the two ions, and then do the “swap and drop” (or your other preferred
method) to figure out the subscripts.

Example:

magnesium chloride

Mg is +2, Cl is -1

Mg+2 Cl-1

swap and drop the 2 and the 1

Mg1Cl2 but we don’t usually write “1,” so it becomes: MgCl2

Reviewing Ionic Bonding (Unit 3)

To write the ionic compound’s formula, we have to look up the charges of
the two ions, and then do the “swap and drop” (or your other preferred
method) to figure out the subscripts.

Example:

calcium oxide

Ca is +2, O is -2

Ca+2 O-2

swap and drop the 2s

Ca2O2 but reduce to lowest whole number = CaO

Reviewing Diatomics (Unit 3)

There are 7 elements that are naturally diatomics

When these elements are not bonded to another element (by itself in the
equation), they get a subscript of 2.

They are:

H2, N2, O2, F2, Cl2, Br2, I2

The subscript of 2 is only for when they are by themselves, not when they
bond to a different element. If they bond to a different element, you can do
the swap and drop to figure out the correct subscripts (see previous slide)

Reviewing Types of Reactions (Unit 4)

Synthesis A+B→ AB (one product)

Decomposition AB → A + B (one reactant)

Combustion Hydrocarbon + O2 → CO2 + H2O

Single Replacement A + BC → AC + B (single element on both sides)

Double Replacement AB + CD → AD + CB (all compounds, cations swap)

Our next topic/unit is about predicting the products of these 5 types of
reactions, if given the reactants. We will still be classifying and balancing too!

Reviewing Conservation of Mass/Matter (Unit 4)

Balancing chemical reactions ensures that the number of atoms of each
element is the same on both sides of the equation, following the Law of
Conservation of Mass.

This is done by adding coefficients (numbers in front of compounds)
without changing the chemical formulas (subscripts).