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

Which of these systems is NOT in a state of dynamic equilibrium?

2 / 10

Using enthalpies of combustion ΔcH, calculate the enthalpy change for the cracking of butane:

C4H10(g) => C2H6(g) + C2H4(g)

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.

3 / 10

An example of an endothermic change is the:

4 / 10

The total O.N. of all the halogen atoms in these compounds ClO-, BrO-, ICl, XeF4 is:

5 / 10

The oxidising agent used to extract bromine from sea water in a displacement reaction is:

6 / 10

Which of the following increase from left to right along the series Mg - Ca - Sr - Ba?

(i) the thermal stability of the nitrates

(ii) the thermal stability of the carbonates

(iii) the solubility of the hydroxides in water

(iv) the solubility of the sulfates in water

 

7 / 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

 

8 / 10

A white crystalline solid gives a pale green colour in a flame. Adding silver nitrate to an acidified solution of the solid produces a white precipitate. The solid is:

9 / 10

What is the oxidation number of CARBON in

CCl4

10 / 10

What is the oxidation number of CARBON in

C2H6

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Core Organic Chemistry Random Retrieval

16

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

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.)

2 / 10

Infra-red absorption ranges for some bonds are as follows:

C-H, 2850 - 3300 cm-1

C=C, 1620 - 1680 cm-1

C=O, 1680 - 1750 cm-1

C-O, 1000 - 1300 cm-1

O-H (alcohols), 3230 - 3550 cm-1

O-H (acids), 2500 - 3000 cm-1

The IR spectrum of propanal has one particularly strong absorption peak

This can be expected to be at:

3 / 10

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

CH3CH2CH2Br -> X -> CH3CH2CH2CO2H

4 / 10

Three halogenoalkanes differ in the rate with which they react with aqueous sodium hydroxide. The order of the rates of reaction is:

5 / 10

What is the formula of 2-bromo-3-methylpentane?

6 / 10

What type of reaction takes place on passing the vapour of ethanol over hot aluminium oxide? (Water and an alkene are produced)

7 / 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)

8 / 10

Name the alkene CH3CH(CH3)CH=CHCH3.

9 / 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.

10 / 10

An alkane in petrol is:

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Physical Chemistry & Transition Elements Random Retrieval

4

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

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)

Under standard conditions, can Mg2+(aq) be reduced to Mg(s) by Ca(s)?

2 / 10

Which of the following can act as a bidentate ligand in the formation of complexes with metal ions?

(i) S2O32-

(ii) C2O42-

(iii) SCN-

(iv) H2NCH2CH2NH2

3 / 10

What enthalpy change is represented by the following equation?

S-(g) + e-=> S2-(g)

4 / 10

For which of these compounds would expect the best agreement between the values of the lattice energy derived from experimental data (with the help of the Born-Haber cycle) and the values calculated from theory on the assumption that the bonding in the crystals is purely ionic?

5 / 10

The lattice enthalpy for magnesium oxide is -3850 kJ mol-1.

The energy needed to break up 0.1 mol MgO into gaseous ions at 298K is:

 

[1] -38.5 kJ mol-1

[2] -385 kJ mol-1

[3] +385 kJ mol-1

[4] +3850 kJ mol-1

6 / 10

Which of these compounds give an alkaline solution when mixed with water?

(i) NH4Cl

(ii) NH3

(iii) CH3CH2OH

(iv) CH3CO2Na

7 / 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 Kp (in units: kPa-2) under these conditions.

8 / 10

Consider the following equilibrium:

N2(g) + O2(g) <=>2NO(g)

1.80 x 10-3 mol of N2 was mixed with 2.40 x 10-3 mol of O2 and 7.20 x 10-3 mol of NO and the mixture sealed in a container. The mixture was left until no further observable change in composition took place. At this point, 4.80 x 10-3 mol of O2 was present in the mixture.

Calculate the value of the mole fraction of O2 present in the mixture under these conditions.

9 / 10

By inspection of this experimental data, what is the rate equation for this reaction?

10 / 10

By inspection of this experimental data, what is the rate equation for this reaction?

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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 13C NMR spectrum of:

2 / 10

Which of these statements is true of a solution of a racemic mixture?

(i) It contains asymmetric molecules,

(ii) It is a mixture of enantiomers,

(iii) It contains equal amounts of optical isomers,

(iv) It rotates the plane of polarised light

3 / 10

Which of these types of isomerism are examples of stereoisomerism.

(i) chain isomerism

(ii) E/Zisomerism

(iii) functional group isomerism

(iv) optical isomersim

4 / 10

Step 8:

5 / 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.

6 / 10

Which of these polymers would you expect to have the strongest intermolecular (interchain) forces as a result of the presence of polar covalent bonds?

7 / 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

8 / 10

The reaction mixture must be completely dry during a Friedel-Crafts acylation or alkylation reaction to:

9 / 10

During the synthesis of an ester from a carboxylic acid and an alcohol the extent of conversion of the carboxylic acid to its ester at equilibrium increases if:

(i) the alcohol is added in excess

(ii) concentrated sulfuric acid is added

(iii) the ester distills off from the reaction mixture as it forms

(iv) an acid catalyst is added

10 / 10

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

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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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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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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 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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