Category: Chemistry

Period Table & Energy Random Retrieval

4

Period Table & Energy Random Retrieval

This quiz contains all the questions in the Period Table & Energy section. The website will pick 10 questions at random.

1 / 10

The synthesis of sulfur trioxide takes place at 380 oC in the presence of a catalyst made from vanadium(V) oxide.

2SO2(g) + O2(g) <=> 2SO3(g) Standard enthalpy change = -297 kJ mol-1

Reasons for not choosing a lower temperature are that:

(i) the product condenses to a solid at a lower temperature

(ii) the proportion of SO3(g) at equilibrium falls if the temperature falls

(iii) the reaction is exothermic

(iv) the catalyst is ineffective at lower temperatures

2 / 10

For which of these equilibria does a change in pressure have no effect on the yield of substances on the right-hand side of the equation?

(i) CH4(g) + H2O(g) <=> 3H2(g) + CO(g)

(ii) 2HI(g) <=> H2(g) + I2(g)

(iii) 2SO2(g) + O2(g) <=> 2SO3(g)

(iv) H2O(g) + CO(g) <=> H2(g) + CO2(g)

3 / 10

Which of these are examples of heterogeneous equilibria?

(i) CaCO3(s) <=> CaO(s) + CO2(g)

(ii) Fe2+(aq) + Ag+(aq) <=> Fe3+(aq) + Ag(s)

(iii) 3Fe(s) + 4H2O(g) <=> Fe3O2(s) + 4H2(g)

(iv)Br2(aq) + H2O(l) <=> HOBr(aq) + H+(aq) + Br-(aq)

4 / 10

Using mean bond dissociation enthalpies, estimate the enthalpy of combustion ΔcH of liquid ethanol

C2H5OH(l) + 3O2(g) => 2CO2(g) + 3H2O(l)

5 / 10

Using enthalpies of combustion ΔcH, calculate the enthalpy change for the hydrogenation of propene:

C3H6(g) + H2(g) => C3H8(g)

Select the data from theenthalpies of combustion ΔcH.

If this question was generated from Random Retrieval, this data can also be found in TOOLS>Data Sheets.

6 / 10

Using enthalpies of formation ΔfH, calculate the enthalpy change for the following hydration process.

Na2S2O3(s) + 5H2O(l) => Na2S2O3•5H2O(s)

Select the data from the 'Selection of Enthalpies of Formation and Combustion' shown above.

If this question was generated from Random Retrieval, this data can also be found in TOOLS>Data Sheets.

7 / 10

Hydrazine burns according to this equation: N2H4(g) + O2(g) -> N2(g) + 2H2O(l)

Calculate the standard enthalpy change for the combustion of hydrazine given that the standard enthalpy of formation of hydrazine is +51 kJmol-1 and of water is -286 kJ mol-1

8 / 10

An example of an endothermic change is the:

9 / 10

What is the oxidation number of CARBON in methanoic acid

HCOOH

10 / 10

Which of these true statements help to explain why the values of the first ionisation enthalpies (energies) of the group 1 metals fall down the group from lithium to caesium?

(i) Down the group, the outer electron gets further from the nucleus

(ii) The charge on the nucleus increases down the group

(iii) Greater shielding means that the attraction between the nucleus and the outer electron reduces down the group

(iv) In all the atoms the outer electron is an s-electron

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Core Organic Chemistry Random Retrieval

15

Core Organic Chemistry Random Retrieval

This quiz contains all the questions in the Core Organic Chemistry section. The website will pick 10 questions at random.

1 / 10

How many functional group isomers of C3H6O2 are there?

It's really difficult to get all of these structures, so don't panic if you miss some. Just spend some time sketching out all the possibilities and remembering some simple rules, e.g carbon forms 4 bonds, oxygen forms 2 etc. Be creative!

2 / 10

A compound X with the molecular formula C4H10O has a broad peak in its IR spectrum at 3500cm-1.

Oxidation of X with excess potassium dichromate(VI) gives a product Y which is not an acid and does not reduce Fehling's solution.

Y has a strong peak in its IR spectrum at 1700cm-1.

Identify X and Y. (See also the data in question 9.)

3 / 10

There are two main peaks in the infra-red spectrum of carbon dioxide.

This shows that carbon dioxide molecules:

4 / 10

The mass spectrum of copper has two significant peaks. The peak at 63 has a relative abundance of 69 and the peak at 65 has a relative abundance of 31.

This shows that the relative atomic mass of copper is:

5 / 10

In a two step synthesis of butanoic acid what is the formula of compound X?

CH3CH2CH2Br -> X -> CH3CH2CH2CO2H

6 / 10

What is the main product of the reaction of 1,2-dichloroethane with a solution of ammonia in ethanol? (Under these conditions ammonia acts as a nucleophile)

7 / 10

The reaction that has the greatest atom economy is:

8 / 10

Which of these alkenes will produce the largest %yield of 2-bromopentane when it is reacted with hydrogen bromide?

9 / 10

What is the H-C-H bond angle in ethene?

10 / 10

Passing the vapour of a liquid mixture of alkanes over strongly heated porcelain chips produces a product which:

(i) is a gas

(ii) is highly flammable

(iii) decolourises a solution of bromine

(iv) is soluble in water.

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Physical Chemistry & Transition Elements Random Retrieval

2

Physical Chemistry & Transition Elements Random Retrieval

This quiz contains all the questions in the Physical Chemistry & Transition Elements section. The website will pick 10 questions at random.

1 / 10

What temperature is required for the determination of a standard cell potential, Eϴcell/V?

[1] 298K

[2] 20oC

[3] 273K

[4] 298 oC

2 / 10

For this question, look at the resource, ‘A Selection of Standard Electrode Potentials’ (‘A Selection of Standard Electrode Potentials’can be found in TOOLS>Data Sheets)

Is Cu2+(aq) capable of oxidising Ag(s)?

3 / 10

Using your half-equations from questions 7 & 8, balance the REDOX equation below.

NO3- + H+ + Cu => Cu2+ + NO2 + H2O

Select the integers that represent the ratio of species in the overall balanced REDOX equation.

If this question appears in a Random Retrieval quiz, you would be best constructing separate half-equations for the species that is oxidised and the species that is reduced prior to working out the overall REDOX equation.

4 / 10

Work out the ratio of the species in the following half-equation.

O2 + e- + H+ => H2O

5 / 10

Using oxidation numbers (states) work out the ratio of the species in the following half-equation.

H2S => S + H+ + e-

6 / 10

In the anti-cancer complex compound [Pt(NH3)2Cl2]

(i) the Pt, N and Cl atoms lie in one plane

(ii) the N-Pt-N angle is 180o

(iii) the Cl-Pt-Cl angle is 90o

(iv) the coordination number of platinum is zero

7 / 10

Which types of chemical bonding feature in crystals of the compound K2[Ni(CN)4]?

(i) ionic bonding

(ii) covalent bonding

(iii) dative covalent bonding

(iv) metallic bonding

8 / 10

Look at the chemical equation below.

CH4(g) + H2O(g)=> CO(g)+ 3H2(g)

By selecting the appropriate data from the ‘Selection of Thermodynamic Data’ in TOOLS, calculate the entropy change, ΔSƟ for the process. Take care with states!

9 / 10

Consider the following equilibrium:

H2(g) + I2(g)<=>2HI(g)

1.50 mol of HI was placed in a sealed vessel and allowed to decompose. At equilibrium, 0.500 mol of HI remained in the vessel

Calculate the value of the mole fraction of HI present in the mixture under these conditions.

10 / 10

When a sample of calcium carbonate reacts with dilute hydrochloric acid, 144 cm3 of carbon dioxide form in 20 seconds at room temperature and pressure.

What is the rate of loss of hydrochloric acid in moles per second. (Volume of 1 mol gas under these conditions = 24 000 cm3)

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Organic Chemistry & Analysis Random Retrieval

6

Organic Chemistry & Analysis Random Retrieval

This quiz contains all the questions in the Organic Chemistry & Analysis section. The website will pick 10 questions at random.

1 / 10

This is the 1H NMR spectrum of:

2 / 10

This is the 13C NMR spectrum of:

3 / 10

Which of these procedures is used on a large scale to recover some value from plastic waste?

(i) burning the plastic in incinerators and using the energy to generate electricity

(ii) re-melting the plastic and spinning the melt into fibres

(iii) heating the waste with catalysts but no air to produce feedstocks for the chemical industry

(iv) washing plastic bottles on high-speed automatic machines so that they can be reused.

4 / 10

The monomer which polymerises to form a plastic which has a smooth, slippery surface and is used to give cooking utensils a non-stick surface is:

5 / 10

Which of these formulae represent glycine in aqueous solution at pH 9?

6 / 10

Which of these properties of benzene are associated with the presence of delocalised electrons?

(i) There are no isomers of 1,2-dichlorobenzene

(ii) Benzene is more stable than might otherwise be expected

(iii) Benzene typically undergoes substitution rather than addition reactions

(iv) Benzene reacts with nucleophiles

7 / 10

What is the main organic product when benzene reacts with 2-iodo-2-methylpropane in the presence of aluminium chloride?

8 / 10

Ethyl ethanoate is heated under reflux with excess aqueous sodium hydroxide. The resulting solution is distilled. The distillate contains:

9 / 10

The reaction of propanone with HCN in the presence of some KCN is an example of:

10 / 10

Which reagent converts butan-2-one to butan-2-ol?

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Chemistry Home

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

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

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

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

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

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Y12 Extended Revision

Year 12 1st Half-Term Revision Exercise

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Year 12 1st Half-Term Revision Exercise – Marks Scheme

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Year 12 Extended Revision – Problem 1

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Year 12 Extended Revision – Problem 1 – Answers

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Year 12 Extended Revision – Problem 2

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Year 12 Extended Revision – Problem 2 – Answers

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Lessons & Primers

Inorganic & General Chemistry

Writing Half Equations

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Writing Half Equations – Answers

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Qualitative Inorganic Analysis 9 Unknown Solids

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Qualitative Inorganic Analysis 9 Unknown Solids – Answers

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The Chemistry of Hydrates

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Handling Dilution Problems

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Titration Theory

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Working Out Oxidation Numbers

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Strategy for Approaching Moles Questions

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Organic Chemistry

Curly Arrows in Organic Chemistry

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Curly Arrows in Organic Chemistry – Answers

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Organic Nomenclature Primer

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Combined Analytical Techniques

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Combined Analytical Techniques – Answers

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Benzene – A Structured Study

Lesson 1

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Lesson 2

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Lesson 3

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Lesson 4

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Benzene – A Structured Study – Answers

Lesson 1 – Answers

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Lesson 2 – Answers

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Lesson 3 – Answers

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Lesson 4 – Answers

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Spectroscopic Data

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Advice for Structural Analysis

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Physical Chemistry

Thermodynamics

Thermodynamics Entropy & Gibbs Energy

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Reaction Kinetics

Reaction Kinetics

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Mechanisms from Orders

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The Arrhenious Equation

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Electrode Potentials

Standard Electrode Potentials

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Enthalpy Changes

Recognising Enthalpy Changes in BH Cycles

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Recognising Enthalpy Changes in BH Cycles – Answers

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Lattice Enthalpy and Born-Haber Cycles

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Enthalpy of Solutions

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Extended Enthalpy Problem

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Extended Enthalpy Problem – Answers

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Support with Laying Out Enthalpy Calculations

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Enthalpy of Combustion and Hess’s Law

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Constructing a Hess Cycle from Equations

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Enthalpy Changes Involved in BH Cycles

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Acid-Base Equilibria

Acid-Base Equilibria: Useful Equations

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Acid-Base Equilibria

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Acid-Base Equilibria: Calculating pH for All Acids Accurately

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Acid-Base Equilibria: Blood Buffering

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Acid-Base Equilibria: Calculating pH of Bases and Salts

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Acid-Base Equilibria: Conjugate Pairs

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Acid-Base Equilibria: Indicators

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Acid-Base Equilibria: pH of Strong Acids and Bases

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Acid-Base Equilibria: pH of Weak Acids

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Acid-Base Equilibria: Strong Acid v Strong Base

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Acid-Base Equilibria: The Effect of Temperature on pH

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Acid-Base Equilibria: Weak Acid v Strong Base

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Chemistry Tools

Inorganic & General Chemistry

OCR Flash Cards

These Revision Flash-Cards are specific to the OCR A Chemistry Specification. 

Each Module (2-6) is presented in a different colour to make them easier to sort.

OCR Topic Titles have been filled in for you so that they match the OCR specification order.

It’s up to you what questions/answers you write on the cards!  

The cards should be folded carefully down the bold black line in the middle of each sheet.

The sheets should be glued on the blank back with a glue stick so that the questions are all on one side and the answers on the other. You may want to lay them under a heavy stack of books to make sure that they are flattened while the glue dries.

Each sheet of 4 questions and answers can then be cut into 4 separate cards. 

Test yourself or get other people to test you on them. Practice, practice, practice!

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Organic Chemistry

Organic Isomerism Blank Infographic

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Organic Isomerism Infographic

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Organic Terms

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Physical Chemistry

Acid-Base Equilibria: Useful Equations

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Enthalpy Change Definitions – Blank

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Entropy Equations Infographic

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Effect of Temperature on Reaction Feasibility

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pH Calculator Tool for Question Writing

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Arrhenious Plot Calculator

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Data Sheets

Inorganic & General Chemistry

Polyatomic Ions

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Organic Chemistry

Table of Functional Groups

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Spectroscopic Data

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Physical Chemistry

A Selection of Enthalpies Changes Useful for Born Haber Cycles

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A Selection of Standard Electrode Potentials

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A Selection of Ka Values & Indicator Ranges

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A Selection of Enthalpy Change Data

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A Selection of Thermodynamic Data

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