Category: Chemistry

Period Table & Energy Random Retrieval

8

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

This is the equilibrium in a solution of bromine in water:

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

The orange colour of bromine disappears on adding

(i) sodium bromide

(ii) water

(iii) dilute hydrochloric acid

(iv) sodium hydroxide solution

2 / 10

A small crystal of iodine is dissolved in hexane to give a violet coloured solution. After adding an equal volume of colourless, aqueous potassium iodide and shaking, the system reaches equilibrium with the hexane layer floating on top of the aqueous layer. At equilibrium:

(i) the concentrations of iodine in the two layers are the same

(ii) the iodine in the hexane turns brown

(iii) the iodine molecules stop moving between the two layers

(iv) the concentrations in each layer stop changing

3 / 10

The value that you obtain for the enthalpy of combustion ΔcH of liquid ethanol using mean bond enthalpies is different from the value obtained experimentally, or by using enthalpy of formation ΔfH of liquid ethanol.

What is the most significant reason for this?

4 / 10

A solution of Br2 and KI were mixed. Then shaken with cyclohexane. Which is correct?

(i) the bromine is reduced

(ii) the cyclohexane layer goes brown

(iii) the cyclohexane layer goes purple

(iv) the iodine is reduced

5 / 10

The electron configuration of a chloride ion is:

6 / 10

All the oxides of the metals Mg, Ca, Sr and Ba:

(i) are basic

(ii) consist of giant structures of ions

(iii) form nitrates when they react with dilute nitric acid

(iv) are freely soluble in water

 

7 / 10

What is the oxidation number of OSMIUM in

OsO4

8 / 10

What is the oxidation number of NITROGEN in

NH3

9 / 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

10 / 10

In the periodic table a periodic pattern is:

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Core Organic Chemistry Random Retrieval

20

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


Choose one of the following options:

2 / 10


Choose one of the following options:

3 / 10

4 / 10

5 / 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:

6 / 10

Which of these pairs of compounds react to form 2-bromopropane as one of the products?

(i) prop-1-ene and hydrogen bromide at room temperature

(ii) propane and bromine in ultraviolet light

(iii) propan-2-ol on heating with sodium bromide

(iv) propan-1-ol and hydrogen bromide on heating

7 / 10

Heating butan-1-ol with a mixture of sodium bromide and concentrated sulfuric acid produces 1-bromobutane. During the preparation the reaction mixture turns orange due to the formation of:

8 / 10

An alcohol consists of 64.9% carbon, 13.5% hydrogen and 21.6% oxygen.

What is the molecular formula of the compound? (Relative atomic masses: C = 12, H = 1, O = 16)

9 / 10

What is the name for this structure:

CH3CH(CH3)CH(CH3)CH2CH3?

10 / 10

Which of these hydrocarbons is an alkane?

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Physical Chemistry & Transition Elements Random Retrieval

7

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

In an EDTA complex with a copper(II) ion

(i) there are six ligand molecules,

(ii) there are four dative bonds between oxygen atoms and the metal ion,

(iii) the overall charge on the complex ion is zero,

(iv) there are two dative bonds between nitrogen atoms and the metal ion

2 / 10

Which first-row d-block metal has the main oxidation state +2 and forms colourless compounds?

3 / 10

What is the pH of a 0.01 mol dm-3 solution of methanoic acid given that for this acid: Ka = 1.6 x 10-4 mol dm-3 at 298K ?

4 / 10

Consider the following equilibrium for the Haber-Bosch process:

3H2(g) + N2(g) <=>2NH3(g)

32.0 mol of H2 was combined with 12.0 mol of N2 and the mixture sealed and pressurised in a vessel of volume 2.00 dm3. The mixture was left until no further observable change in composition took place. At this point, 4.00 mol of NH3 was found to be present in the mixture. The pressure was recorded as 200 000 kPa.

Calculate the value of Kc (in units: mol-2 dm6) under these conditions.

5 / 10

Consider the values of the equilibrium constant for this reversible reaction:

H2(g) +I2(g) <=> 2HI(g)

Temperature: 500K, value of Kc = 160

Temperature: 1000K, value of Kc = 54.

This information shows that:

(i) HI decomposes rapidly at 500 K

(ii) Raising the temperature causes the equilibrium to shift to the left

(iii) Raising the pressure causes the equilibrium to shift to the right

(iv) The reaction is exothermic

6 / 10

For which of the following equilibria, does raising the pressure favours the formation of products?

(i) H2(g) + C(s) <=> H2(g) + CO(g)

(ii) 4NH3(g) + 5O2(g) <=> 4NO(g) + 6H2O(g)

(iii) 2HCl(g) + I2(g) <=> 2HI(g) + Cl2(g)

(iv) 2SO2(g) + O2(g) <=> 2SO3(g)

7 / 10

Which of the following are examples of heterogeneous equilibria?

(i) CaCO3(s) <=> CaO(s) + CO2(g)

(ii) 2CrO42-(aq) + 2H+(aq) <=> Cr2O72-(aq) + H2O(l)

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

(iv) Co2+(aq) + 6NH3(aq) <=> [Co(NH3)6]2+(aq)

8 / 10

What value should go in the blank box in the table?

9 / 10

What are the units of k for this reaction?

[1] s-1

[2] mol-1 dm3 s-1

[3] mol-2 dm6 s-1

[4] mol-3 dm9 s-1

10 / 10

Which of these are examples of kinetic stability?

(i) A solution of hydrogen peroxide can be stored at room temperature

(ii) Hydrogen does not ignite in air at room temperature

(iii) Aluminium does not corrode in moist air

(iv) Magnesium oxide does not decompose on heating

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Organic Chemistry & Analysis Random Retrieval

10

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

Which of these compounds are chiral?

(i) propan-1-ol,

(ii) propan-2-ol,

(iii) butan-1-ol,

(iv) butan-2-ol

3 / 10

When propene react with hydrogen bromide the main intermediate is:

4 / 10

NOT ON OCR SPEC. Hint: Esters can be hydrolysed and the initial stage in the mechanism is nucleophilic attack using an oxygen lone pair of the water molecule. RO- is the leaving group and becomes ROH.

18O is a ‘radiolabelled oxygen’.

The reaction of ethyl ethanoate with H218O produces:

5 / 10

Which of these chemical species are nucleophiles with react with halogenoalkanes?

(i) cyanide ions

(ii) hydroxide ions

(iii) ammonia molecules

(iv) ammonium ions

6 / 10

Step 2:

7 / 10

Which of the following molecules would you predict to be the most basic?

8 / 10

Which of the following molecules is/are examples of 2o amines?

(i) 

(ii)

(iii) 

(iv) 

9 / 10

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

10 / 10

Treating ethanal with hydrogen cyanide in the presence of some KCN and then hydrolysing the product with hot hydrochloric acid (which converts a cyano / nitrile group RCN, to RCOOH) produces:

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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 Extended Revision – Problem 1

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Year 12 Extended Revision – Problem 1 – 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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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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