UNIT 3 – IB MATERIAL Name: ___________________________

BONDING, MOLES & STOICHIOMETRY

ESSENTIALS: Know, Understand, and Be Able To…

Apply the mole concept to substances.

Determine the number of particles and the amount of substance (in moles).

Define the terms relative atomic mass (Ar) and relative molecular mass (Mr).

Calculate the mass of one mole of a species from its formula.

Solve problems involving the relationship between the amount of substance in moles, mass and molar mass.

Deduce chemical equations when all reactants and products are given.

Identify the mole ratio of any two species in a chemical equation.

Calculate theoretical yields from chemical equations.

Determine the limiting reactant and the reactant in excess when quantities of reacting substances are given.

Solve problems involving theoretical, experimental and percentage yield.

Describe the ionic bond as the electrostatic attraction between oppositely charged ions.

Describe how ions can be formed as a result of electron transfer.

Deduce which ions will be formed when elements in groups 1, 2 and 3 lose electrons.

Deduce which ions will be formed when elements in groups 5, 6 and 7 gain electrons.

Describe the covalent bond as the electrostatic attraction between a pair of electrons and positively charged nuclei.

Describe how the covalent bond is formed as a result of electron sharing.

Deduce the Lewis (electron dot) structures of molecules and ions for up to four electron pairs on each atom.

IB Study Guide Page References: p. 6-9

EXPLORE

Lab: Stoichiometry (after unit exam)

ELABORATE

Assignments

ENVISION

TOK Question on Moodle forum

EVALUATE

Quiz in Class

Quiz Corrections

Assignment: Determining Empirical Formula & Molecular Formula from Percent Composition

Assignment: More Practice with Word Equations

• Write the word descriptions below as chemical equations, making sure each chemical

formula is correct

• Include (s), (l), (g), and (aq) after each compound as appropriate

• Balance the equation with the smallest whole-number coefficients.

1) Zinc and lead (II) nitrate (aqueous) react to form zinc nitrate (aqueous) and lead.

2) Aluminum bromide (aqueous) and chlorine gas react to form aluminum chloride (aqueous) and bromine

gas.

3) Sodium phosphate and calcium chloride solution react to form calcium phosphate and sodium chloride

solution.

4) Aluminum and hydrochloric acid solution react to form aluminum chloride (aqueous) and hydrogen gas.

5) Calcium hydroxide solution and phosphoric acid react to form calcium phosphate and water.

6) Copper and sulfuric acid react to form copper (II) sulfate and water and sulfur dioxide.

7) Hydrogen gas and nitrogen monoxide react to form water and nitrogen gas.

Assignment: Gram Gram Calculations

Assignment: Molar Volume Calculations (Gases Only) 1) Calcium carbonate decomposes at high temperatures to form carbon dioxide and calcium oxide:

CaCO3(s) CO2(g) + CaO(s)

How many grams of calcium carbonate will I need to form 3.45 liters of carbon dioxide?

2) Ethylene burns in oxygen to form carbon dioxide and water vapor:

C2H4(g) + 3 O2(g) 2 CO2(g) + 2 H2O(g)

How many liters of water can be formed if 1.25 liters of ethylene are consumed in this reaction?

3) When chlorine is added to acetylene, 1,1,2,2-tetrachloroethane is formed:

2 Cl2(g) + C2H2(g) C2H2Cl4(l)

How many liters of chlorine will be needed to make 75.0 grams of C2H2Cl4?

4) Nitrogen monoxide and oxygen gas combine to form the brown gas nitrogen dioxide. How

many mL of nitrogen dioxide are produced when 3.4 mL of oxygen reacts with an excess of

nitrogen monoxide? Assume conditions of STP. (Remember 1L = 1000mL)

2 NO (g) + O2 (g) 2 NO2 (g)

Assignment: More Molar Volume Calculations (If Needed)

Assignment: Volume - Volume Calculations (Gases Only)

Assignment: # of Particle Calculations - Avogadro 1) How many molecules of oxygen are produced by the decomposition of 6.54 g of KClO3?

2 KClO3 (s) 2 KCl (s) + 3 O2 (g)

How many atoms of oxygen is this?

2) How many molecules of nitrogen monoxide are produced if 92.0 g of nitrogen dioxide is combine with

excess water according to the following reaction? (Not balanced)

__NO2(g) + __H2O (l) __ HNO3 (g) + __NO (g)

3) What is the mass of 99.0 x 10

23 molecules of H2?

4) How many atoms are contained in 13.5 g of Nitrogen gas?

Assignment: More Avogadro Practice (If Needed)

Assignment: Mixed Mole/Stoichiometry Problems

Assignment: More Mixed Mole Problems

Assignment: Limiting Reactants

Assignment: More Limiting Reactants Practice (If Needed)

Assignment: Percent Yield