A. Naming Elements and Compounds1. Polyatomic Molecular Elements

halogens, hydrogen, phosphorus, sulfur, oxygen, nitrogen

elements that exist in form instead of form

Chem 20 Review

molecular atomic

***SHPON (8, 2, 4, 2, 2)

2. Molecular Compounds

use prefixes to indicate the number of atoms in the molecule

there are many molecular compounds that still use their common names or IUPAC names (organic molecules)

eg) carbon dioxide =dinitrogen monoxide = CCl4 =

CO2

N2O carbon tetrachloride

eg) hydrogen peroxide, glucose, ammonia, sucrose

non-metals only

3. Acids

see data booklet and Nelson pg 553

Rules

1. hydrogen becomes acid

2. hydrogen becomes acid

3. hydrogen becomes acid

_____ide hydro____ic

_____ate _______ic

_____ite ______ous

Try These:

1. hydrogen iodide =

2. hydrogen phosphate =

3. hydrogen nitrite =

4. hydrogen sulphite =

hydroiodic acid

phosphoric acid

nitrous acid

sulphurous acid

4. Ionic Compounds

name in full then name the with or use

cation (positive ion) anion (negative ion)

eg) NaCl = Mg3(PO4)2 =

sodium chloride magnesium phosphate

look up the symbol for each ion then balance the charges using subscripts

the polyatomic ion name the “ide” ending

when writing formulas,

hydrated ionic compounds contain

indicated by where x is the

eg) CuSO45H2O = copper (II) sulphate pentahydrate

“xH2O”

water in their atomic structures

number of water molecules

Your Assignment: pgs 1-3 in workbook

B. Bonding

recall types of intermolecular forces

London Dispersion – occurs between all moleculesand is the attraction of the electrons in one molecule to the protons in another molecule

Hydrogen Bonding – occurs only when H is bonded to O, F or N

occurs only between polar moleculesDipole-Dipole – and is the electrostatic attraction of the polar ends of molecules

and is the attraction of the H to the O, F or N in another molecule

C. Chemical Reactions1. Classification of Reactions

clues to a chemical reaction:

conservation laws:

1. colour change

2. gas produced

3. energy change

4. precipitate formed

2. energy (1st Law of Thermo)

1. mass - number and kind of atom (balancing)

types of reactions:

1. composition/formation

2. decomposition

3. single replacement

4. double replacement

5. hydrocarbon combustion

6. other

2. Energy in Chemical Reactions

endothermic =

exothermic =

bond energy =

energy is absorbed

energy is released

energy released when bonds are formed or energy absorbed when bonds are broken

3. States of Matter

gives the states of elements at room temperature

all ionic compounds at room temperature

molecular compounds can be at room temperature

periodic table

(by themselves) are solid

solids, liquids or gases

acids are assumed to be

ionic compounds may be when mixed with water

aqueous

aqueous or solid

Your Assignment: pgs 4-5 in workbook

D. Significant Digits

represents the degree of

two different rules are used:

1. Addition/Subtraction:

2. Multiplication/Division:

add or subtract then round to the lowest number of decimal places

accuracy of using measured values

multiply or divide then round to the lowest number of sig digs

E. Solutions and Gases1. Preparation of Solutions

concentration is most commonly measured in

mol/L can also be expressed as

solubility =

solubility is measured in

mol/L

“molarity” or M

the concentration of solute in a saturated solution at a given temperature

g/100 mL

eg) 0.300 mol/L = 0.300 M

molar solubility is measured in

to determine the solubility of an ionic compound, check the solubility table in the Data Booklet

mol/L

Steps for Solution Preparation

1. Calculate the mass of the solute required to achieve a specific concentration and volume.

2. Measure mass.

3. Dissolve the solute in half of the volume of solvent.

4. Transfer solution to a volumetric flask.

5. Bring solution up to final volume and mix by inverting.

2. Dilution of Solutions

when a solution is diluted, only the amount of is increased

the remains constant

solvent (usually water)

number of moles

ViCi = VfCf

Your Assignment: 1. pgs 6-8 in workbook

3. Types of Solutes

nonelectrolytes:

electrolytes:

dissociation of solutes in water:

1. electrolytes:

2. non-electrolytes:

substances that dissolve to yield solutions that do not conduct electricity

substances that dissolve to yield solutions that conduct electricity

eg) molecular compounds

eg) ionic compounds and acids

Na2CO3(s)

C6H12O6(s)

2Na+(aq) + CO3

2-(aq)

C6H12O6(aq)

4. Determining Ionic Concentrations

you can use the concentration of a solute to determine the ion concentrations once it is dissolved in water (dissociated)

Steps

1. Write a balanced dissociation equation.

2. Write down concentration given.

3. Determine the ion concentrations using the mole ratio.

Example

What is the concentration of each ion in a 0.23 mol/L solution of aluminum sulphate?

1 Al2(SO4)3(s)

C = 0.23 mol/L C = 0.23 mol/L C = 0.23 mol/L x 2 1

x 3 1

= 0.46 mol/L = 0.69 mol/L

2 Al3+(aq) + 3 SO4

2-(aq)

Your Assignment: pg 9 in workbook

5. Non Ionic vs. Net Ionic Equations

net ionic reactions are used to show

write the non-ionic reaction, the total ionic reaction and the net ionic reaction

only the reacting ions…spectator ions (non-reacting) are omitted

Example

What is the net ionic reaction for the reaction of bromine and sodium iodide ?

Non Ionic:

Total Ionic:

Net Ionic:

+ Br–(aq)

+ 2Br–(aq)

Br2(l) + NaI(aq) I2(s) + NaBr(aq)2 2

Br2(l) + Na+(aq) + I–

(aq) I2(s) + Na+(aq)2 2 2 2

Br2(l) + 2I–(aq) I2(s)

Your Assignment: pg 10 in workbook

6. Gases

Ideal Gas Law:

STP =

SATP =

conversion to Kelvin =

PV = nRT

273.15 K, 101.325 kPa, 22.4 L/mol

298.15 K, 100 kPa, 24.8 L/mol

273.15 + xC

F. Stoichiometry

Steps

1. Write a balanced chemical (or net ionic) equation.

2. Write down the given information.

3. Find moles of given using n = m, C = n , PV = nRT M V

4. Find moles of wanted using the mole ratio: wanted/given.

5. Find answer to question.

Example 1

If 5.00 g of sodium reacts with excess chlorine gas, how much sodium chloride is produced?

2Na(s) + Cl2(g) 2 NaCl(aq)

m = 5.00 gM = 22.99 g/mol

x gM = 58.44 g/mol

n = m M = 5.00g 22.99 g/mol = 0.217… mol

n = 0.217… mol x 2 2

m = nM = (0.217… mol)(58.44 g/mol) = 12.7 g

Example 2

Liquid bromine is added to 500 mL of a solution containing 0.150 mol/L iodide ion. What mass of iodine will be produced?

2I-(aq) + Br2(l) 2Br-

(aq) + I2(s)

V = 500 mL = 0.500 LC = 0.150 mol/L

x gM = 253.80 g/mol

n = CV = (0.150 mol/L)(0.500 L) = 0.0750 mol

n = 0.0750 mol x 1 2

= 0.0375 mol

m = nM = (0.0375mol)(253.80 g/mol) = 9.52 g

Example 3

If 5.0 g of sodium reacts with 5.0 g of chlorine, how much sodium chloride is produced?

2Na(s) + Cl2(g) 2NaCl(aq)

x g

M = 58.44 g/moln = 0.0705 mol x 2

1 = 0.141…mol

m = nM = (0.141..mol)(58.44 g/mol) = 8.2 g

m = 5.0 gM = 22.99 g/mol

m = 5.0 gM = 70.90 g/mol

n = m M= 5.0 g 22.99 g/mol= 0.217…mol

n = m M= 5.0 g 70.90 g/mol= 0.0705…mol

2 = 0.108…mol

1 = 0.0705…molCl2(g) is limiting

Your Assignment: pgs 11-13 in workbook