Category: Chemistry

Important Ground Rules for Completing these Quizzes

Please read!

Only use the data from the A Level Periodic Table which shows the appropriate number of decimal places and correct spellings. All exam boards have a common Periodic Table at A level.

Entering numerical answers

• All your answers should be to 3 significant figures where relevant.
• Use the relative atomic mass values from the A Level Periodic Table to calculate relative molecular/formula masses.

Carry out your calculations on paper. Check them carefully for spelling and significant figures before entering your answers into the quiz.

Some examples are offered below. Please look at them.

Example 1

Question: Calculate the mass present in 0.250 mol of zinc.

Answer: 0.250 x 63.5=15.875

You should only enter 15.9 Any other answer will be marked as incorrect so be careful!

Example 2

Question: Calculate the mass in 1.50 mol of chromium

Answer: 1.50 x 52.0=78

You should only enter 78.0 Any other answer will be marked as incorrect so be careful!

Example 3

Question: Calculate the number of moles of chromium present in 0.780 g of chromium

Answer: 0.78/52.0=0.015

You should only enter 0.0150        Any other answer will be marked as incorrect so be careful!

Example 4

Question: Calculate the relative formula mass of calcium carbonate CaCO­3

Answer: 40.1 + 12.0 + (3 x 16.0) = 100.1

You should only enter 100.1        Note that this is to 4 significant figures. This is the level of accuracy provided by the A Level Periodic Table.

Entering Chemical Names

There are some simple rules.

• All letters are lowercase.
• The roman numerals are uppercase versions of the letters v& i
• There is one space each side of the bracketed roman numerals and the text.
• Correct spellings of elements are only those on your periodic table. e.g. sulfur not sulphur.

Example 1

Question:    Name a compound with the formula Fe₂(SO₄)­₃

Answer:       iron (III) sulfate

Example 2

Question:    Name a compound with the formula MnO₂

Answer:       manganese (IV) oxide

Entering Chemical Formulae

There are some simple rules.

You are unable to enter subscripts or superscripts into the quiz answer box.

To enter a chemical formula, ignore subscripts and superscripts.

Example 1

Question:    Write down the formula hydrogen peroxide.

Answer:       H2O2

Example 2

Question:    Write down the formula aluminium nitrate

Answer:       Correct formula is Al(NO­₃)₃

You enter    Al(NO3)3

Foundations in Chemistry – Module 2

This module is designed to build upon the fundamental concepts learned in GCSE Chemistry.

Models that were sufficient to explain and predict the chemistry at GCSE level are modified and extended to be able to explain the properties and reactions of a wider range of chemical species that are encountered at Advanced Level.

Examples of this include:

• refining the model of electronic structure of atoms and ions to explain the formation of compounds where atoms expand their octet.
• development of the ideal gas equation for the calculation of the amount of gases under non-standard conditions.
• introduction of the oxidation numbers model to allow students to identify REDOX reactions for more challenging examples that don’t involve simple ions.
• explanation and application of electronegativity to allow students to appreciate the non-binary nature of bonding, i.e. ionic ‘v’ covalent. Also, electronegativity is used to explain the polarity of bonds and the resulting strength of intermolecular forces.

Foundations in Chemisty

• M2S1 – Atomic Structure
• M2S2 – Electronic Configurations
• M2S3 – Moles
• M2S4 – Hydrates
• M2S5 – Ionic Structure and Bonding
• M2S6 – Covalent Structures and Bonding
• M2S7 – Shapes of Molecules
• M2S8 – Intermolecular Forces
• M2S9 – Metallic Structures and Bonding
• M2S10 – States of Matter and Structures
• M2S11 – Acid Base Reactions 1
• M2S12 – Redox Reactions

Period Table & Energy – Module 3

This module focuses mainly on the inorganic and physical branches of chemistry. Many topics within this module will be familiar to students from GCSE but those foundations will be built open.

Skills developed in Module 2: Foundations in Chemistry, will be necessary to underpin the learning in the module.

Examples of concept developed in the module include:

• the concept of periodicity will be studied from several perspectives including the variation in the sizes of atoms, first ionization energies as evidence for electronic structure, and the nature of bonding within elements across a period.
• study of the chemistry of Group 2 and a comparison with Group 1, studied at GCSE.
• further study of the chemistry of Group 7 to demonstrate the ability of the halogens to form higher oxidation states in compounds.
• more sophisticated explanations of the effect of conditions on reaction rates by the use of Maxwell-Bolzman distribution profiles.
• a more quantitative approach to the description of equilibrium position through the calculation of equilibrium constant, Kc.
• the simple understanding of energy changes in chemical reactions, introduced in GCSE, will be strengthened by defining several specific enthalpy changes and by the application of Hess’s Law.

Period Table & Energy

• M3S1 – Periodicity
• M3S2 – Oxidation Numbers
• M3S3 – Group 2
• M3S4 – Group 7
• M3S5 – Enthalpy Changes Year 1
• M3S6 – Enthalpy Calculations for Year 1
• M3S7 – Equilibrium

Core Organic Chemistry – Module 4

• This module extends some of the physical chemistry topics that were introduced in Module 3. These include:
  • a quantitative approach will be taken towards the explanation of the factors affecting rate including concentration and temperature.
  • rate equations will be developed for chemical processes to predict the effect of a change in concentration of a reactant upon the rate of reaction and to allow reaction mechanisms to be suggested.
  • equilibrium position will be further quantified and extended to cover the equilibrium constant, Kp.
  • equilibrium position in acid-base equilibria will be quantified using equilibrium constant Ka. This will be applied to estimate the pH of strong and weak acids, and partially neutralised weak acids (buffers)
  • lattice enthalpies will be explained and calculated using Born-Haber Cycles.
  • thermodynamics will be studied at a basic level so that reaction feasibility can be predicted at varied temperatures. The topic will include the concept of entropy and Gibbs (free) Energy.
  • electrochemistry will be covered so that the function of disposable, rechargeable and fuel cells can be understood.
  This module also introduces some new concepts associated with the chemistry of transition elements. In order to explain some of the aspects of transition metal chemistry, the application of REDOX understanding will be further developed.

Core Organic Chemistry

• M4S1 – Alkanes
• M4S2 – Alkenes
• M4S3 – Alcohols
• M4S4 – Haloalkanes
• M4S5 – Instrumental Analysis IR & MS
• M4S6 – Year 1 Isomerism
• M4S7 – Year 1 Organic Nomenclature

Physical Chemistry & Transition Elements – Module 5

• This module extends some of the physical chemistry topics that were introduced in Module 3. These include:
  • a quantitative approach will be taken towards the explanation of the factors affecting rate including concentration and temperature.
  • rate equations will be developed for chemical processes to predict the effect of a change in concentration of a reactant upon the rate of reaction and to allow reaction mechanisms to be suggested.
  • equilibrium position will be further quantified and extended to cover the equilibrium constant, Kp.
  • equilibrium position in acid-base equilibria will be quantified using equilibrium constant Ka. This will be applied to estimate the pH of strong and weak acids, and partially neutralised weak acids (buffers)
  • lattice enthalpies will be explained and calculated using Born-Haber Cycles.
  • thermodynamics will be studied at a basic level so that reaction feasibility can be predicted at varied temperatures. The topic will include the concept of entropy and Gibbs (free) Energy.
  • electrochemistry will be covered so that the function of disposable, rechargeable and fuel cells can be understood.
  This module also introduces some new concepts associated with the chemistry of transition elements. In order to explain some of the aspects of transition metal chemistry, the application of REDOX understanding will be further developed.

Physical Chemistry & Transition Elements

• M5S1 – Kinetics 1
• M5S2 – Kinetics 2
• M5S3 – Kinetics and Orders of Reaction
• M5S4 – Mechanisms and Orders
• M5S5 – Calculating Mole Fractions
• M5S6 – Equilibria Kc & Kp
• M5S7 – Calculating Kc and Kp
• M5S8 – Acid Base Equilibria 2
• M5S9 – Born Haber Cycles
• M5S10 – Enthalpy Changes for Born-Haber
• M5S11 – Entropy and Gibbs Energy
• M5S12 – Transition Elements
• M5S13 – Complex Ions
• M5S14- Half Equations for REDOX
• M5S15 – REDOX equations from half-equations
• M5S16 – Electrode Potentials 1
• M5S17 – Electrode Potentials 2
• M5S18 – Electrode Potentials 3

Organic Chemistry & Analysis – Module 6

In this module, more organic families with new functional groups will be introduced. General principles of organic chemistry, learned in Module 4, will be applied to help name, explain and predict the chemistry of these new organic families. The new families include:

• aromatic molecules (arenes)
• carboxylic acids their derivatives (esters, anhydrides, acyl chlorides)
• nitrogen containing groups; amines, amides and amino acids

The concept of polymerisation, first introduced at GCSE, will be expanded to cover addition and condensation polymerisation (polyesters and polyamides).

Organic synthesis will be extended to cover reaction sequences covering several steps.

The analytical technique of Nuclear Magnetic Resonance (NMR) spectroscopy will be introduced as a sensitive technique for identifying the arrangement of atoms in organic chemical structures. Interpretation of NMR, IR and Mass Spectra, will be used in combination to confirm the identity of organic molecules.

Organic Chemistry & Analysis

• M6S1 – Carbonyls
• M6S2 – Carboxylic Acids & Esters
• M6S3 – Arenes
• M6S4 – Amines & Amides
• M6S5 – Amino Acids
• M6S6 – Polymers
• M6S7 – Organic Synthesis
• M6S8 – Organic Mechanisms
• M6S9 – Organic Summary
• M6S10 – Isomerism Year 2
• M6S11 – NMR Problems

Inorganic & General Chemistry

Writing Half Equations

Writing Half Equations – Answers

Qualitative Inorganic Analysis 9 Unknown Solids

Qualitative Inorganic Analysis 9 Unknown Solids – Answers

The Chemistry of Hydrates

Handling Dilution Problems

Titration Theory

Working Out Oxidation Numbers

Strategy for Approaching Moles Questions

Organic Chemistry

Curly Arrows in Organic Chemistry

Curly Arrows in Organic Chemistry – Answers

Organic Nomenclature Primer

Combined Analytical Techniques

Combined Analytical Techniques – Answers

Benzene – A Structured Study

Lesson 1

Lesson 2

Lesson 3

Lesson 4

Benzene – A Structured Study – Answers

Lesson 1 – Answers

Lesson 2 – Answers

Lesson 3 – Answers

Lesson 4 – Answers

Spectroscopic Data

Advice for Structural Analysis

Physical Chemistry

Thermodynamics

Thermodynamics Entropy & Gibbs Energy

Reaction Kinetics

Reaction Kinetics

Mechanisms from Orders

The Arrhenious Equation

Electrode Potentials

Standard Electrode Potentials

Enthalpy Changes

Recognising Enthalpy Changes in BH Cycles

Recognising Enthalpy Changes in BH Cycles – Answers

Lattice Enthalpy and Born-Haber Cycles

Enthalpy of Solutions

Extended Enthalpy Problem

Extended Enthalpy Problem – Answers

Support with Laying Out Enthalpy Calculations

Enthalpy of Combustion and Hess’s Law

Constructing a Hess Cycle from Equations

Enthalpy Changes Involved in BH Cycles

Acid-Base Equilibria

Acid-Base Equilibria: Useful Equations

Acid-Base Equilibria

Acid-Base Equilibria: Calculating pH for All Acids Accurately

Acid-Base Equilibria: Blood Buffering

Acid-Base Equilibria: Calculating pH of Bases and Salts

Acid-Base Equilibria: Conjugate Pairs

Acid-Base Equilibria: Indicators

Acid-Base Equilibria: pH of Strong Acids and Bases

Acid-Base Equilibria: pH of Weak Acids

Acid-Base Equilibria: Strong Acid v Strong Base

Acid-Base Equilibria: The Effect of Temperature on pH

Acid-Base Equilibria: Weak Acid v Strong Base