Review Before Predicting Products

Review Before

Predicting Products

Reviewing Metals and Nonmetals (Unit 1-2)

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

Categorize

Options (15)

calcium

Mg

Cl

Fluorine

O

C

sulfur

N

Ar

He

Fe

Cu

Zn

silver

Au

Sort the elements into metals and nonmetals

Metal

Nonmetal

Reviewing Ionic vs Covalent (Unit 3)

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

A compound that only contains nonmetals is covalent

Categorize

Options (14)

NaCl

MgBr₂

calcium sulfide

carbon monoxide

CO₂

sulfur hexafluoride

CCl₄

KOH

LiF

BaCl₂

Na₂SO₄

KF

H₂O

NH₃

Categorize the compounds as ionic or covalent

Ionic

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

Drag and Drop

Aluminum (Al) and iodine (I) bond ionically because aluminum is a metal that loses electrons to form a ​

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charge (Al⁺³), while iodine is a nonmetal that gains electrons to form a ​

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charge (I⁻¹). Using the swap and drop method, the charge of aluminum (3) becomes the ​

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for iodine, and the charge of iodine (1) becomes the subscript for aluminum, resulting in the formula ​

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. This ensures the compound is neutral, with three negatively charged iodide ions balancing the one positively charged aluminum ion.

Drag these tiles and drop them in the correct blank above

+3

-1

subscript

AlI₃

+1

-3

Al3I

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)

Drag and Drop

The seven diatomic elements—hydrogen (H₂), nitrogen (N₂), ​

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(O₂), fluorine (F₂), chlorine (Cl₂), bromine (​

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), and iodine (I₂)—exist naturally as molecules made of ​

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atoms because they are more stable this way. These elements are all ​

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, and they form ​ covalent bonds to share electrons and achieve a full outer energy level. A common way to remember them is the acronym ​

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or by noting that they form a "7" shape on the periodic table, plus hydrogen.

Drag these tiles and drop them in the correct blank above

oxygen

Br₂

two

nonmetals

metals

ionic

"BrINClHOF"

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!

Match

Match the following reactions to the correct type of reaction. Remember, "replacement" and "displacement" can be used interchangeably, so "single displacement" means "single replacement."

• Synthesis

• Decomposition

• Single Displacement

• Double Displacement

• Combustion

2Na + Cl₂ → 2NaCl

CaCO₃ → CaO + CO₂

Zn + 2HCl → ZnCl₂ + H₂

HCl + NaOH → NaCl + H₂O

2C₂H₆ + 7O₂ → 4CO₂ + 6H₂O

• 2Na + Cl₂ → 2NaCl

• CaCO₃ → CaO + CO₂

• Zn + 2HCl → ZnCl₂ + H₂

• HCl + NaOH → NaCl + H₂O

• 2C₂H₆ + 7O₂ → 4CO₂ + 6H₂O

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).

Multiple Choice

What is the correct coefficient for O₂ when balancing the following equation?

__ C + O₂ → CO₂

• 1

• 2

• 3

• 4

Multiple Choice

What is the missing coefficient for Al in the balanced equation below?

__ Al + 3CuCl₂ → 2AlCl₃ + 3Cu

• 1

• 2

• 3

• 4

Multiple Choice

What coefficient should be placed in front of O₂ to balance this combustion reaction?

C₃H₈ + __ O₂ → 3CO₂ + 4H₂O

• 3

• 4

• 5

• 6

Multiple Choice

What are the correct coefficients to balance the following equation?

Na₃PO₄ + CaCl₂ → NaCl + Ca₃(PO₄)₂

• 1, 1, 3, 2

• 2, 3, 6, 1

• 3, 2, 6, 1

• 1, 2, 3, 2