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5703970
AS-Level Chemistry Module 2 - OCR A
Description
AS - Level Chemistry for exam board OCR A. Module 2 includes Atoms and Moles, Formulas and equations, Reactions and Calculations and Electrons, Bonding and Structure. This is for the new 2015 specification.
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as - level chemistry
ocr a
module 2
new spec
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Resource summary
AS-Level Chemistry Module 2 - OCR A
Atoms and Moles
The Atom
Structure
Protons, Neutrons, Electrons
Nuclear Symbols
Mass number
Atomic Number
Atoms and Ions
Positive or Negative Charge
Isoptoes
Same number of protons, different number of neutrons
Atomic Models
JJ Thomson
Plum Pudding Model
Rutherford's Model
Gold Foil Experiment
Bohr's Model
Four basic principles
Relative Mass
Atomic Mass
Calculating
Isotopic Mass
Molecular Mass
Formula Mass
The Mole
What is a mole?
Molar Mass
Calculations
Gas Volumes
Gas Volume
Ideal Gas Equation
pV=nRT
Concentration Calculations
Moles and Concentration
n=cxV(dm3)
Formulas and Equations
Formulas
Empirical and molecular formulas
Calculating Formulas
Empirical formula
Experimental data
Percentage compositions
Molecular formula
Chemical Equations
Balancing equations
Ionic Equations
Equations and Calculations
Calculating masses
Gas volumes
State symbols
Formulas of Ionic Compounds
Formation of ions
Formulas
Reactions and Calculations
Acids, Bases and Salts
What are they?
Strength of acids and bases
Reactions
Acid-base reactions
Acids and Oxides
Acid and metal oxides
Acid and metal hydroxides
Acids and carbonates
Anhydrous and Hydrous Salts
What are they?
Finding the formula of hydrated salts
Titrations
Performing titrations
Indicators
Practical Techniques
Measuring masses
Volumes of solutions
Standard Solutions
Preparing solutions
Calculations
Titrations Calculatons
Calculating concentration
Polyprotic acids
Calculating volumes
Chemical Yield
Theoretical yield
Percentage yield
Atom Economy
What is it?
Calculating it
Addition and substitution reactions
Atom economy and percentage yield
Atom economy in industry
Oxidation Number
Finding
From formulas
From systematic names
Assigning
Using
Working out systematic names
Working out formulas
Redox Reactions
What are they?
Changing oxidation numbers
Reactions with dilute acids and metals
Electrons, Bonding and Structure
Electronic Structure
Electron Shells
Sub-shells
s-shells
2 electrons, 1 orbital
p-shells
6 electrons, 3 orbitals
d-shells
10 electrons, 5 orbitals
f-shells
14 electrons, 7 orbitals
Shells
1st shell
2 electrons
2nd Shell
8 electrons
3rd shell
18 electrons
4th shell
32 shells
Orbitals
s-sub shells are spherical
p-sub shells are dumb-bell
Electron Configurations
Sub-shell notation
Electrons in boxes
Energy Level Diagrams
Ionic Bonding
Oppositely charged ions are attracted together
Ionic compound forms
Overall charge is 0
Dot and Cross diagrams
Giant Ionic Lattices
Regular shape
Attracted to oppositely charged ions in all directions
Behaviour of Compounds
Electrical Conductivity
Conduct when molten or dissolved
Melting and boiling points
High
Strong electrostatic forces
Solubility
Dissolves in water
Shapes of Molecules
Linear
Berylium Chloride/Carbon Doixide
180 degrees
Trigonal Planar
120 degrees
Boron Triflouride
Tetrahedral
109.5 degrees
Methane, Ammonium ion
Trigonal Pyramidal
Ammonia
107 degrees
Non-linear
104.5 degrees
Water
Trigonal bipyramidal
Phosphorous Pentachloride
120, 90 degrees
Octahedral
90 degrees
Sulphur hexaflouride
Polarisation
Electronegativity
Polar and non-polar bonds
Polar molecules
Predicting bond types
Intermolecular Forces
Induced dipole-dipole interactions
Permanent dipole-dipole interactions
Hydrogen Bonding
Behaviour of simple covalent compounds
Electrical Conductivity
Melting and boiling points
Solubility
Trends in melting and boiling points
Covalent Bonding
Molecules
Non-metals
Share electrons, each atom gets 8 electrons in their outer shell
Dot and cross
Single, Double and triple bonds
Dative covalent
1 atom provides both shared electrons
Special Cases
Boron Triflouride
Sulphur Hexaflouride
Covalent bond strength
Average bond enthalpy
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