Chemistry 1 - Acids, Bases, and Rates of Reaction

Atomic Number (bottom)

The number of protons in the nucleus of the atom

Mass number (top left)

The total number of protons and neutrons in the nucleus of an atom

Isotope

Atoms with the same number of protons but different number of neutrons

Period

horizontal row on the periodic table. equal to the number of electron shells

Group

Vertical column on the periodic table. atoms in the same group have similar qualities. group number is equal to the number of number of valence electrons

Group 1

Consists of alkali metals, which are highly reactive and have one valence electron.

Group 17

Most reactive group of atoms. Consists of non-metals

Group 18

Least reactive elements (noble gases)

Ionic Bonding

chemical bond that occurs between two atoms (metal and non-metal) when one atom donates one or more electrons to another atom, resulting in the formation of oppositely charged ions.

Ion

An atom that has an electrical charge and has lost or gained valence electrons to get a full valence shell to get stable

Covalent Bonding

sharing of valence electrons between non-metal atoms to get a full valence shell to get stable (Group 14)

Covalent Bonded Gases

Covalently bonded molecules are usually gases because they have weak inter-molecular forces

Hydrochloric Acid

HCl

Nitric Acid

HNO₃

Sulfuric Acid

H₂SO₄

Sodium Hydroxide

NaOH

Potassium Hydroxide

KOH

Calcium Hydroxide

Ca(OH)₂

Element

Substance that contains only one type of atom

Compound

Substance which contains 2 or more types of atoms which are chemically bonded together

Mixture

Substance which contains 2 or more types of atoms which are not chemically bonded together

Acid

A substance that releases hydrogen ions when dissolved in water

Base

a substance which releases hydroxide ions when dissolved in water

Alkali

A base that can be dissolved in water (is soluble in water)

pH Scale

a measure of the concentration (molL^-1) of hydrogen ions in a solution

Dissociation

when acids and alkali break up into their ions when dissolved in water

Strong acid

completely dissociates, releasing all of their hydrogen ions when dissolved in water

Weak acid

partially dissociate, only releasing some of their hydrogen ions when dissolved in water

Strong base

completely dissociates, releasing all of their hydroxide ions when dissolved in water

Weak base

partially dissociate, only releasing some of their hydroxide ions when dissolved in water

Concentration

A measure of how many acid/alkali particles there are per unit volume of water

Acid + Metal Oxide →

salt + water

Acid + metal hydroxide →

salt + water

Acid + metal carbonate →

salt + water + carbon dioxide

Acid + metal bicarbonate →

salt + water + carbon dioxide

pH 1

UI Red

pH 2

UI Red-orange

pH 3

UI Orange

pH 4

UI Orange-yellow

pH 5

UI Yellow

pH 6

UI Yellow-green

pH 7

UI Green

pH 8

UI Blue-green

pH 9

UI Light blue

pH 10

UI Blue

pH 11

UI Dark blue

pH 12

UI Violet

pH 13-14

UI Purple

Particle Theory

All matter is made up of tiny particles which are constantly in motion

particles can be individual atoms, ions, or molecules

Rate of Reaction

A measure of the change in concentration of the reactants or the change in the concentration of the products in a reaction per unit time

Collision theory

two or more reactant particles must collide with sufficient energy and correct orientation for a reaction to occur

Factors affecting rate of reaction

temperature - higher temperature means more kinetic energy means more successful collisions per unit time

concentration - more particles per unit volume means that more collisions between particles are happening per unit time means more successful collisions per unit time

surface area - more particles exposed to collisions means more collisions per unit time which means more successful collisions per unit time

catalyst - lowers the activation energy which means more particles have sufficient energy which means more successful collisions per unit time

Activation energy

minimum amount of energy required for a chemical reaction to proceed

Measuring rate of reaction

How quickly the product is made (gas production, mass change, colour change)

How quickly one of the reactants disappears (mass change, colour change)