Chemistry Paper 1 & 2

Flashcards for Chemistry Paper 1 & 2 Lecture Notes

Melting and Boiling Points

The stronger the forces/bonds between particles, the higher the melting point and boiling point.

Limitations of particle theory

No forces between particles; particles are spheres.

Ionic bonding

Metals with non-metals

Covalent bonding

Non-metals with non-metals

Metallic bonding

A regular arrangement of metal ions with delocalized electrons

Does a Covalent Molecular structure conduct electricity, what is its size and melting point?

No, small, low

Does a Giant Covalent structure conduct electricity, what is its size and melting point?

No, giant, high

Does an Ionic structure conduct electricity, what is its size and melting point?

Yes, giant, high

Does a metallic structure conduct electricity, what is its size and melting point?

Yes, giant, high

Diamond

Hard, 4 bonds on each carbon

Graphite

Soft, 3 bonds on each carbon, delocalised electrons, layers can slide.

Nanotube/Fullerenes

Hexagons, electronics and composites.

Proton Charge

+1

Neutron Charge

0

Electron Charge

-1

Mass number

Number of protons + number of neutrons

Proton number

Number of protons

Why atoms have no overall charge

Same number of protons and electrons

Dalton Model of the Atom

Solid Sphere

JJ Thomson Model of the Atom

Plum Pudding

Rutherford Model of the Atom

Gold Foil Experiment, discovered the nucleus

Bohr Model of the Atom

Electrons orbit the nucleus at specific energy levels

Conservation of mass

Mass of reactants = mass of products

Why does mass appear to decrease in some reactions?

A gas is lost.

Why does mass appear to increase in some reactions?

A gas reacts and joins.

Acid properties

Universal indicator colour is red, pH is 1-6, gives H+ ions in solution

Ionic equation for neutralisation

H+ + OH- -> H20

Moles Equation

Mass / Mr

Avogadro's Constant

6.02 x 10^23

The mass of 1 mole in grams

Relative formula mass(Mr)

Concentration Equation

Moles / Volume

Oxidised Definition

Magnesium gains oxygen

Reduced Definition

Copper oxide loses oxygen

Electrolysis at the anode (+)

Negative ions extracted

Electrolysis at the cathode (-)

Positive ions extracted

Electrolyte in making aluminium

Aluminium oxide in cryolite

Why does the positive electrode need to be replaced when making aluminium?

Carbon reacts with oxygen to make CO2.

Strong Acid

Fully ionised

Weak Acid

Partially ionised

A change in pH number of 1 change

A change in concentration by 10.

Endothermic Reaction

Temperature decreases, heat is taken in from the surroundings.

Exothermic Reaction

Temperature increases, heat is transferred to the surroundings.

Examples of exothermic reactions

Combustion, oxidation, neutralisation

Example of endothermic reactions

Thermal decomposition

Exothermic reaction - energy and bonds

Energy released from making bonds is greater than the energy needed to break bonds.

Exothermic reaction - energy levels

Energy of products is less than reactants

Endothermic reaction - energy levels

Energy of products is more than reactants

Early Periodic Table arrangment

Arranged by atomic weight

Mendeleev's Periodic Table

Left gaps for undiscovered elements

Problems with early periodic tables

Order of atomic weight was not always correct/similar properties at regular intervals

Periodic Table Definition

Elements with similar properties at regular intervals

The max number of electrons in the first shell

2

The max number of electrons in the second shell

8

The max number of electrons in the third shell

8

Elements on the left of the periodic table

Metals

Elements on the right of the periodic table

Non-metals

Metals

Form positive ions

Non-Metals

Form negative ions

Groups in the Periodic Table

Columns

Periods in the Periodic Table

Rows across

Number of outer shell electrons

Group number

Period number

Number of electron shells

Group 0 Properties

Unreactive/inert

Separation techniques

Evaporation/Crystallisation/Distillation/Chromatography

Isotopes are atoms with the…

Same number of protons, different number of neutrons

Relative Atomic Mass Calculation

(% abundance x mass) + (% abundance x mass) / 100

Radius of an atom

1x10^-10m

Radius of a nucleus

1x10^-14m

Group 1 name

Alkali metals

Group 1 Properties

All have 1 electron in their outer shell/more reactive going down the group as it's easier to lose the outer electron

Group 7 name

Halogens

Group 7 properties

All have 7 electrons in their outer shell/Less Reactive going down group 7/Harder to gain an electron