C2 Chemistry Notes

Front 1

Proton number

Back 1

Tells you how many protons there are in the atom. The number of protons is equal to the number of Electrons

Front 2

Mass Number

Back 2

Tells you how many protons+neutrons there are in a atom

Front 3

Electronic Configuration

Back 3

The electrons orbiting the nucleus are arranged in shells or energy levels.

2- first shell

8- second shell

8- third shell

Front 4

Periodic table

Back 4

Rows are called periods (number of shells)

Columns are called Groups (number of electrons in outer shell)

metals on the left

Non-Metals on the far right

Front 5

Bonding

Back 5

All atoms "WANT" to be as stable as a noble gas. Noble gases have complete outer shells therefore they do not need to react or bond with any other element

Front 6

Three types of bonding

Back 6

Type Bonds form between Electrons

Ionic metal/non metal lost or gained

Covalent Non metal/Non metal Shared

Metallic Metal/Metal Electron Cloud

Front 7

Molecules

Back 7

are compounds where the atoms are Covalently bonded

Front 8

Giant Molecular structures ( Macromolecules)

Back 8

Diamond- carbon bonded to four other carbon atoms. Hard substance. Forms a crystal lattice.

Graphite- Carbon bonded to three other carbon atoms. Soft substance. Arranged in layers with free electrons between the layers. Only Non-Metals to conduct electricity.

Silicon Dioxide- Looks like diamond but made up of two different types of atom; silicon and oxygen

Front 9

NANOMOLECULES

Back 9

"Nano" = 1 billionth of a metre, very small particles arranged in different way so that they behave differently to ordinary materials made of the same atoms.

Front 10

Metals

Back 10

Form giant metallic structures. Atoms arranged in layers surrounded by a cloud of DELOCALISED electrons. Metal are strong, ductile and can be hammered into different shapes.

Front 11

Isotopes

Back 11

Are atoms with the same number of protons and electrons but different number of neutrons.

Front 12

Yield

Back 12

Compare how much you actually make with the maximum amount possible

Front 13

Atom Economy

Back 13

Considers the amount of starting materials that end up as useful products.

Front 14

Reversible Reaction

Back 14

Reaction that can go in both directions.

Front 15

Rate of reaction

Back 15

How fast the reactants are turned into products

Front 16

Collision Theory

Back 16

. Particles wil react when they collide with each other

. Particles need to collide with enough energy- this is called activation energy

. Increase the temperature- increase the energy-particles move faster-collisions occur more frequently- rate of reaction increases

. Add a catalyst- activation energy lowered- rate of reaction increases

. Increase the surface area or concentration- more particles react-collisions occur more frequently- rate of reaction increases

Front 17

Exothermic Reaction

Back 17

Means to release heat energy when bonds are broken

Front 18

Endothermic Reaction

Back 18

Absorb heat energy when bonds are made.

Front 19

Electrolysis

Back 19

. Only works when ions are present, this is called an Electrolyte

. Positive ions are attracted to the negative Electrode

. Negative ions are attracted to the positive Electrode

. Positive ion- atom- Gains electron- Reduction

. Negative electron- atom - loses electrons- Oxidation

Front 20

Acids

Back 20

Ph 1-6

Front 21

Alkalis

Back 21

Ph 8-14

Front 22

Neutral

Back 22

Ph 7

Front 23

Indicators

Back 23

Change colour when added to acids or Alkalis

Front 24

Neutralisation

Back 24

Is when an acid is added to an alkali until a neutral solution is produced

Front 25

A Base

Back 25

Is an insoluble alkali

Front 26

Important Reaction

Back 26

Acid+ base--- salt+ water

Acid salt

Hydrochloric Chloride

Sulfuric Sulfate

Nitric Nitrate

Front 27

Second important reaction

Back 27

Acid+ metal---- salt+ hydrogen

Front 28

lines of best fit in Chemistry

Back 28

Are most likely to be CURVES