Grade 11 Chemistry Review

Front 1

Energy Level

Back 1

The valence shell where the electrons are located, the closer to the nucleus the greater the energy.

Front 2

Nuclear Charge

Back 2

The total charge of the protons in the nucleus, or the atomic number.

Front 3

Ionization Energy

Back 3

The amount of energy required to move an electron from an atom or ion in the gaseous state.

Front 4

Electronegativity

Back 4

The ability of an atom to attract electrons when bonded to another atom.

Front 5

Electron Affinity

Back 5

Energy given off when an electron is added to a neutral atom.

Front 6

pH

Back 6

A number between 0 and 14 that indicates if a solution is an acid or a base based on the H concentration. pH = -log[H] H = 10^-pH

Front 7

The Bronsted-Lowry Concept

Back 7

Acids are proton [H cations] donors and bases are proton acceptors. The acid becomes the conjugate base.

Front 8

H-Bonding

Back 8

A dipole-dipole attraction that is very strong, between H and F, O or N. Roughly five times stronger than dipole-dipole forces.

Front 9

Binary Covalent Compounds

Back 9

Combinations of two non-metals. The element with the lower electronegativity is written first. The ending of the second element is removed and replaced with -ide. The number of atoms of each element is indicated by prefixes (mono, di, tri, tetra, penta, hexa...)

Front 10

Binary Ionic Compounds

Back 10

Combination of a metal with a non-metal. Metal is written first, followed by the anion with the suffix -ide. For metals with multiple charges, the charge is indicated by (II). In the word equation, -ic indicates a higher valence and -um indicates a lower valence.

Front 11

Polyatomic ions

Back 11

Nick the Camel had a Clam Supper in Phoenix

Front 12

Binary Acids

Back 12

Acids formed by combining hydrogen with one other element. Hydro______ic acid (common) or aqueous hydrogen _______ide (IUPAC)

Front 13

Oxyacids

Back 13

Acid formed by combining hydrogen with a polyatomic ion containing oxygen. -ate becomes -ic. -ite becomes -ous.

Front 14

Acid Salts

Back 14

A compound formed when some of the hydrogen atoms are replaced by a metal. (Ex: sodium hydrogen carbonate)

Front 15

Hydrated Salts

Back 15

Compound that contains water in its structure [Ex : copper (II) sulfate pentahydrate]

Front 16

Combustion Reactions

Back 16

Complete combustion - sufficient oxygen, produces water vapour and carbon dioxide

Incomplete combustion - insufficient oxygen, produces carbon dioxide, water, carbon monoxide and carbon soot

Front 17

Percentage Composition

Back 17

-divide the mass of the element by the mass of the compound

Front 18

The Mole

Back 18

6.02x10^23

-a quantity

Front 19

Empirical Formula

Back 19

-The molecular formula in lowest terms

To calculate :

1. percent composition to mass

2. mass to mole

3. divide by small

4. multiply until whole

-The molecular formula can be found by dividing the total mass by the mass of the empirical formula. This number is then multiplied by the empirical formula.

Front 20

The formula of a hydrate

Back 20

-find the moles of water (hydrate-anhydrate) x molar mass

-find the moles of the anhydrate

-divide water by anhydrate

Front 21

Percent Yield

Back 21

-calculate the theoretical yield of the reaction

-(actual / theoretical) x 100

Front 22

Percent Error

Back 22

(experimental - theoretical) / experimental

Front 23

Solubility

Back 23

-The stronger the intermolecular forces of a substance, the more soluble it will be

-like dissolves like, therefore the more similar the formula of the solute to that of the solvent, the more soluble it is

Front 24

Concentration

Back 24

quantity of solute / quantity of solution

Front 25

Making molar solutions from a solid

Back 25

-multiply the volume of the final solution by the desired concentration and the molar mass of the compound

Front 26

Making molar solutions from a liquid

Back 26

-C1V1 = C2V2

Front 27

Net Ionic Equations

Back 27

-some ions exist only as aqueous in chemal equations (spectator ions)

- these ones can be cancelled out if they are the exact same on both side of the equation

Front 28

Solubility Categories

Back 28

-High>0.1M

-Low<0.1 M

-Insoluble = negligible

Front 29

Neutralization

Back 29

Acid + Base -> Water + Salt

Front 30

Titration

Back 30

-the amount of acid or base needed to neutralize

1. Write balanced chemical equation

2. L a -> mol a -> mol b -> L b

Front 31

Charles's Law

Back 31

Front 32

Boyle's Law

Back 32

Front 33

Gay-Lussac's Law

Back 33

Front 34

Combined Gas Law

Back 34

Front 35

Ideal Gas Law

Back 35

-n = 8.31

Front 36

STP

Back 36

-0 degrees celcius

-101.325 kPa

-22.4L

Front 37

SATP

Back 37

-25 degrees celcius

-100 kPa

-24.8L

Front 38

Pressure Conversions

Back 38

101.3kPa = 1atm = 760mm Hg

1 torr = 1mm Hg

Front 39

Dalton's Law of Partial Pressure

Back 39

-the total pressure of a mixture of gases is equal to the sum of the pressures of the individual gases

-the molecules of a gas act independently from that of another

Front 40

Vapour Pressure

Back 40

If a gas is collected over water, 3 corrections must be made in order to find the volume of dry gas.

1. The level of water inside and outside the tube must be level

2. The water vapour pressure must be subtracted from the atmospheric pressure

3. Find the new volume using the combined gas law