Category: Chemistry

1.66g of potassium hydroxide was dissolved in deionised water and made up to 100cm³ in a volumetric flask.

25.0cm³ samples were titrated against nitric acid solution of concentraion 0.300 mol dm^-3.

A mean titre of 23.45cm³ of nitric acid solution was obtained.

Calculate the percentage purity, by mass, of the original solid. (Don't include the % symbol and give answer to 1 decimal place!)

Calculate the pH of a solution created by the addition of 20.0cm³ 0.150 mol dm^-3 barium hydroxide (Ba(OH)₂) solution to 60.0 cm³ 0.200 mol dm^-3 hydrochloric acid solution.

Remember to give your answer to 3 sig.fig.

By titration, it was found that an average titre of 21.30cm³ of 0.100 mol dm^-3 solution of sulfuric acid was required to just neutralise a 25.00 cm³ sample of potassium hydroxide solution. Calculate the concentraion of the potassium hydroxide solution.

The equation for the reaction is

2KOH_(aq)+H₂SO_4(aq)=>K₂SO_4(aq)+H₂O_(aq)

By titration, it was found that an average titre of 19.75cm³ of 0.200 mol dm^-3 solution of hydrochloric acid was required to just neutralise a 10.00 cm³ sample of lithium hydroxide solution. Calculate the concentraion of the lithium hydroxide solution.

The equation for the reaction is

LiOH_(aq)+HCl_(aq)=>LiCl_(aq)+H₂O_(aq)

By titration, it was found that an average titre of 25.00cm³ of 1.75 mol dm^-3 solution of nitric acid was required to just neutralise a 50.00 cm³ sample of potassium hydroxide solution. Calculate the concentraion of the potassium hydroxide solution.

The equation for the reaction is

KOH_(aq)+HNO_3(aq)=>KNO_3(aq)+H₂O_(aq)

By titration, it was found that an average titre of 28.80cm³ of 2.00 mol dm^-3 solution of potassium carbonate was required to just neutralise a 50.00 cm³ sample of sulfuric acid solution. Calculate the concentraion of the sulfuric acid solution.

The equation for the reaction is

K₂CO_3(aq)+H₂SO_4(aq)=>K₂SO_4(aq)+H₂O_(aq)+CO_2(g)

By titration, it was found that an average titre of 45.25cm³ of 0.100 mol dm^-3 solution of hydrochloric acid was required to just neutralise a 20.00 cm³ sample of barium hydroxide solution. Calculate the concentraion of the barium hydroxide solution.

The equation for the reaction is

Ba(OH)_2(aq)+2HCl_(aq)=>BaCl_2(aq)+2H₂O_(aq)

By titration, it was found that an average titre of 19.10cm³ of 0.250 mol dm^-3 solution of sulfuric acid was required to just neutralise a 10.00 cm³ sample of potassium hydroxide solution. Calculate the concentraion of the potassium hydroxide solution.

The equation for the reaction is

2KOH_(aq)+H₂SO_4(aq)=>K₂SO_4(aq)+H₂O_(aq)

By titration, it was found that an average titre of 22.25cm³ of 0.100 mol dm^-3 solution of hydrochloric acid was required to just neutralise a 20.00 cm³ sample of lithium hydroxide solution. Calculate the concentraion of the lithium hydroxide solution.

The equation for the reaction is

LiOH_(aq)+HCl_(aq)=>LiCl_(aq)+H₂O_(aq)

By titration, it was found that an average titre of 25.00cm³ of 0.100 mol dm^-3 solution of hydrochlorc acid was required to just neutralise a 25.00 cm³ sample of sodium hydroxide solution. Calculate the concentraion of the sodium hydroxide solution.

The equation for the reaction is

NaOH_(aq)+HCl_(aq)=>NaCl_(aq)+H₂O_(aq)

Calculate the concentration of Ba(NO₃)₂ in a solution of volume 1100.00cm³ that contains 76.0 g of Ba(NO₃)₂

Ba=137.3 N=14.0 O=16.0

Calculate the concentration of NH₄NO₃ in a solution of volume 0.724dm³ that contains 50.0 g of NH₄NO₃

N=14.0 O=16.0 H=1.0

Calculate the concentration of C₁₂H₂₂O₁₁ in a solution of volume 33.00cm³ that contains 7.20 g of C₁₂H₂₂O₁₁

H=1.0 C=12.0 O=16.0

Calculate the concentration of lithium hydroxide in a solution of volume 1.05dm³ that contains 65.0 g of lithium hydroxide

Li=6.9 O=16.0 H=1.0

Calculate the concentration of potassium hydrogencarbonate in a solution of volume 900cm³ that contains 50.0 g of potassium hydrogencarbonate

K=39.1 H=1.0 C=12.0 O=16.0

Calculate the concentration of barium nitrate in a solution of volume 22.50cm³ that contains 0.670 g of barium nitrate

Ba=137.3 N=14.0 O=16.0

Calculate the concentration of aluminium sulfate in a solution of volume 250.00cm³ that contains 5.00 g of aluminium sulfate

S=32.1 Al=27.0 O=16.0

Calculate the volume of solution in dm³ that would contain 0.300 mol of H⁺ ions if the concentration of the solution is 2.00 mol dm^-3

Calculate the volume of solution in cm³ that would contain 0.750 mol of sodium hydroxide if the concentration of the solution is 6.00 mol cm^-3

Calculate the number of moles of silver nitrate in a solution of volume 1.10 dm³ and a concentration of 1.30 mol dm^-3

Calculate the volume of gas (in dm³) of 0.200 mol of neon if the gas is at a temperature of 25^oC and a pressure of 101kPa

Calculate the volume of gas (in cm³) of 0.00250 mol of neon if the gas is at a temperature of 473K and a pressure of 150000Pa

Calculate the volume of gas (in dm³) of 0.400 mol of sulfur hexafluoride if the gas is at a temperature of 273K and a pressure of 40.0kPa

Calculate the temperature of a sample of methane (in ^oC) if 3.00 mol of methane has a volume of 34.2dm³ and is at a pressure of 150000Pa

Calculate the number of moles of gas present at r.t.p in 18.0 dm³ of propane.

Calculate the number of moles of gas present at r.t.p in 900 cm³ of sulfur hexafluoride.

Calculate the number of moles of gas present at r.t.p in 96.0 dm³ of methane.

Calculate the number of moles of gas present at r.t.p in 12.0 m³ of hydrogen.

Calculate the number of moles of gas present at r.t.p in 1200 cm³ of oxygen.

Calculate the number of moles of gas present at r.t.p in 36.0 dm³ of neon .

Calculate the number of moles of ammonia if you have 100 g of ammonia

N=14.0 H=1.0

Calculate the number of moles of aluminium sulfate if you have 100 g of aluminium sulfate

S=32.1 Al=27.0 O=16.0

Calculate the number of moles of CuSO₄ if you have 479 g of CuSO₄

S=32.1 Cu=63.5 O=16.0

Calculate the number of moles of N₂ if you have 28.0 g of N₂

N=14.0

Calculate the number of moles of O₂ if you have 4.00 g of O₂

O=16.0

Calculate the mass of aluminium oxide that you would have if you had 6.00 mol of aluminium oxide

Al=27.0 O=16.0

Calculate the mass of barium nitrate that you would have if you had 0.620 mol of barium nitrate

Ba=137.3 N=14.0 O=16.0

Calculate the mass of chlorine that you would have if you had 0.200 mol of chlorine

Cl=35.5

Calculate the mass of I₂ that you would have if you had 0.450 mol of I₂

I=126.9

Calculate the mass of Cl₂ that you would have if you had 4.00 mol of Cl₂

Cl=35.5

Which of the following solutions contains most potassium hydroxide (KOH)?

What mass of

CO₂

could be obtained by heating 5g of calcium carbonate?

Balance this equation:

P₄+O₂=>P₄O₁₀

Using the balanced equation, how many moles of oxygen molecules are required to react with 1 mole of phosphorous molecules?

A compound with empirical formula CH₂ has a relative molecular mass of 84. Which of the following is the molecular formula of the compound?

Combustion of 7.8g of potassium produced 14.2g of an oxide. Which of the following is the simplest formula of the oxide of potassium formed?

BaCO₃

Calculate the mass of 6.02 x10²³atoms of oxygen

Calculate the mass of 0.00200 mol of sodium atoms

Calculate the relative molecular mass (formula mass) of sodium iodide, Nal

Calculate the relative atomic mass (to one decimal place) of element, B if element B is a mixture of two isotopes, ¹⁰B and ¹¹B. There is one atom of ¹⁰B to every four atoms of ¹¹B.

Which is the most typical reaction of an amine in organic synthesis?

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

How many peaks would you expect to see in the ¹³C spectrym of 2,5-dimethyltetrahydrofuran?

What is the value of the rate constant, k for this reaction at this temperature?

Consider the following equilibrium:

H_2(g) + I_2(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.

If pressures are measured in pascals (Pa) what are the units of K_p for this equilibrium:

2H_2(g) + O_2(g) <=> 2H₂O_(g)

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

H_2(g) +I_2(g) <=> 2HI_(g)

Temperature: 500K, value of K_c = 160

Temperature: 1000K, value of K_c = 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

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

Br^- => Br₂ + e^-

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)

When pieces of tin (Sn) are added a yellow solution of acidified ammonium vanadate(V) containing the VO₂⁺_(aq) ion and the mixture allowed to stand for a few minutes, what colour will be observed in the solution?

High resistance voltmeters are required for accurate values of E^ϴcell/V to be measured.

What statement best describes the reasoning behind the use of a high resistance voltmeter?

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)?

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

Br^- => Br₂ + e^-

When four bromide ions combine with a cobalt(II) ion

(i) the charge on the complex ion is 2-

(ii) the shape of the complex ion is tetrahedral

(iii) the coordination number of the cobalt atom is 4

(iv) the name of the complex is the tetrabromocobalt (II) ion

Look at the chemical equation below.

2NaHCO_3(s)=> Na₂CO_3(s)+ H₂O_(g)+ CO_2(g)

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

For which of these species is the value of the electron affinity positive?

(i) F

(ii) Cl

(iii) O

(iv) O^-

These are four values for the hydration enthalpies of ions:

-361 kJ mol^-1, -559 kJ mol^-1, -2003 kJ mol^-1, -2537 kJ mol^-1.

These ions from left to right are:

pH = 2.9 for a solution which contains equal concentrations of chlorethanoic acid and sodium chlorethanoate. What is the pH of the solution after mixing it with twice its own volume of pure water?

Consider the following equilibrium for the Haber-Bosch process:

3H_2(g) + N_2(g) <=>2NH_3(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 K_c (in units: mol^-2 dm⁶) under these conditions.

Consider the following equilibrium:

2SO_2(g) + O_2(g) <=>2SO_3(g)

8.00 mol of SO₂ was mixed with 5.00 mol of O₂ and the mixture sealed in a heated vessel of volume of 1.00 dm³. The mixture was left until no further observable change in composition took place. At this point, 2.00 mol of O₂ was present in the mixture and the pressure was recorded as 200 kPa.

Calculate the value K_c (in units: mol^-1 dm³) under these conditions.

Consider the following equilibrium for the reaction that generates hydrogen for use in the Haber-Bosch Process:

CH_4(g) + H₂O_(g) <=>CO_(g) + 3H_2(g)

140 mol of CH₄ was mixed with 100 mol of H₂O and the mixture given time to reach equilibrium. At this point, 240 mol of H₂ was present in the mixture.

Calculate the value of the mole fraction of CH₄ present in the mixture under these conditions.

This is the ¹H NMR spectrum of:

How many peaks would you expect to see in the ¹³C spectrym of 2,5-dimethyltetrahydrofuran?

The two compounds formed on heating 3-bromo-2-methylpentane with KOH in ethanol (which causes elimination!) are:

(i) alkenes,

(ii) position isomers,

(iii) hydrocarbons,

(iv) E/Z isomers

When propene react with hydrogen bromide the main intermediate is:

Which of these statements defines a free radical?

Step 4:

Which of these molecules does NOT consist of one or more chains of amino acids?

(i) The hormone insulin

(ii) The filaments in muscle fibres

(iii) The enzyme in saliva, amylase

(iv) The genetic material, DNA

Which of these compounds are solids at room temperature?

(i) propane

(ii) propanoic acid

(iii) propylamine

(iv) 2-aminopropanoic acid

Which types of change are involved in this sequence of reactions, though not necessarily in the order listed?

CH₃CO-C₆H₅ -> CH₃CO-C₆H₄-NO₂ -> CH₃CHOH-C₆H₄-NO₂ -> CH₃CH(OCOCH₃)-C₆H₄-NO₂

(i) esterification

(ii) reduction

(iii) nitration

(iv) hydrolysis

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

Which of these statements about atomic and ionic radii are true?

(i) Atomic radii increase down group 2

(ii) Ionic radii increase down group 7

(iii) Atomic radii decrease across period 3

(iv) In period 3 the ionic radii are smaller than the atomic radii

What is the oxidation number of NITROGEN in

NaNH₂

Which of these ions has the greatest polarising power?

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

The total heat capacity of a calorimeter is 2000 J K^-1.

The standard enthalpy of combustion of propane is -2200 kJ mol^-1

Calculate the expected temperature rise on heating the calorimeter by burning 0.0500 mol of fuel from a propane burner assuming that all the energy heats the calorimeter.

Take care with units.

Using enthalpies of formation Δ_fH, calculate the enthalpy change for the following reaction.

2NaHCO_3(s) => Na₂CO_3(s) + H₂O_(l) + CO_2(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.

How many neutrons are there in an atom of boron with mass number 9 and atomic number 4?

What is the electronic configuration of carbon?

Enter your answer in the following format 1s2 2s2 etc. (note the space between each sub-shell!) Follow the aufbau order of sub-shell filling.

What is the electronic configuration of sodium? Enter your answer in the following format 1s2 2s2 etc. (note the space between each sub-shell!) Follow the aufbau order of sub-shell filling

In which of these solids are there two types of bonding: one strong and one weak?

(i) diamond

(ii) ice

(iii) sodium chloride

(iv) graphite

In which of these elements are the atoms or molecules closely packed but free to move around sliding past each other at room temperature?

(i) mercury

(ii) argon

(iii) bromine

(iv) iodine

Which of these elements has a relatively low boiling point (below 500 ^oC)?

In a close-packed metal structure:

(i) there are no spaces between the atoms

(ii) the atoms are arranged in layers

(iii) the crystal breaks if the layers slide past each other

(iv) each atom touches 12 nearest neighbours.

In which of these molecules do the intermolecular forces arise largely from attractions between temporary dipoles?

What is/are the bond angle(s) found in PCl₅?

(i) 90^o

(ii) 104.5^o

(iii) 120^o

(iv) 180^o

A chloride ion and an argon atom have the same:

(i) number of protons

(ii) number of electrons

(iii) atomic number

(iv) electron configuration

How many sulfate ions are there in 0.01 mol aluminium sulfate?

(The Avogadro constant = 6.02 x 10²³ mol^-1)

What is the electronic configuration of sulfide? Enter your answer in the following format 1s2 2s2 etc. (note the space between each sub-shell!) Follow the aufbau order of sub-shell filling.

What is the electronic configuration of scandium? Enter your answer in the following format 1s2 2s2 etc. (note the space between each sub-shell!) Follow the aufbau order of sub-shell filling.

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

C₂H₅OH_(l) + 3O_2(g) => 2CO_2(g) + 3H₂O_(l)

Using enthalpies of formation Δ_fH, calculate the enthalpy of combustion Δ_cH of ethanol:

C₂H₅OH_(l) + 3O_2(g) => 2CO_2(g) + 3H₂O_(l)

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.

The energy needed to atomise 1 mol of gaseous ethene, C₂H₄ is 2087 kJ mol^-1. Calculate the average bond enthalpy for a C-H bond given that the bond enthalpy for the C=C bond is +347 kJ mol^-1.

The total heat capacity of a calorimeter is 2000 J K^-1.

The standard enthalpy of combustion of propane is -2200 kJ mol^-1

Calculate the expected temperature rise on heating the calorimeter by burning 0.0500 mol of fuel from a propane burner assuming that all the energy heats the calorimeter.

Take care with units.

Chlorine disproportionates when it reacts with:

Bubbling carbon dioxide into an aqueous solution of calcium hydroxide produces a white precipitate of:

The reaction of calcium with water produces:

What is the electron configuration of a magnesium atom?

What is the oxidation number of CHROMIUM in

Cr₂O₇^2-

In the periodic table a periodic pattern is:

Choose one of the following options:

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

This shows that carbon dioxide molecules:

The number of peaks in the mass spectrum of an element indicates the number of:

What are the conditions for converting 1,2-dichlorethane into ethane-1,2-diol?

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

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

The reaction that has the greatest atom economy is:

Burning a hydrocarbon fuel such as methane gas in a limited supply of air is dangerous because under these conditions one of the products is:

What is the name for this structure:

CH₃CH(CH₃)CH(CH₃)CH₂CH₃?

The members of the homologous series of alkanes:

(i) are all straight-chain compounds

(ii) have the general formula C_nH_(2n + 2)

(iii) have identical chemical properties

(iv) show a regular gradation of physical properties as the number of carbon atoms increases.

Choose one of the following options:

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

Using enthalpies of formation Δ_fH, calculate the enthalpy of combustion Δ_cH of ethanol:

C₂H₅OH_(l) + 3O_2(g) => 2CO_2(g) + 3H₂O_(l)

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.

Which of these reactions can be reversed by changing the conditions in a typical advanced chemistry laboratory?

(i) CuSO₄.5H₂O_(s) -> CuSO_4(s) + 5H₂O(l)

(ii) 2Mg_(s) + O_2(g) -> 2MgO_(s)

(iii) NH_3(g) + HCl_(g) -> NH₄Cl_(s)

(iv) CH_4(g) + 2O_2(g) -> CO_2(g) + 2H₂O_(l)

The first five ionisation energies of an element in kJ/mol are: 419, 3051, 4412, 5877, 7975. The element is in:

An element M has two electrons in its outer shell. An element X has seven electrons in its outer shell. What is the likely formula of the compound of X and Y?

An element X has the electron configuration 1s²2s²2p². Element Y has the electron configuration 1s²2s²2p⁵. What is the likely formula of the compound of X and Y?

Dilute hydrochloric acid reacts with:

(i) zinc to form zinc chloride and hydrogen

(ii) copper(II) oxide to form copper(II) chloride and water

(iii) zinc carbonate to form zinc chloride, carbon dioxide and water

(iv) copper to form copper(II) chloride and hydrogen

What are the products of the acid hydrolysis of methyl propanoate?

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:

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:

Which of these reagents are nucleophiles?

(i) Br₂

(ii) NH₃

(iii) NO₂⁺

(iv) CN^-

Which of these molecules are polar?

(i) trans but-2-ene,

(ii) trans 1,2-dichloroethene,

(iii) cis but-2-ene,

(iv) cis 1,2-dichloroethene

An alloy of platinum with rhodium is the catalyst used:

(i) in catalytic converters to cut pollution from motor vehicles

(ii) in the synthesis of ammonia from nitrogen and hydrogen

(iii) in the oxidation of ammonia to NO_(g) during the manufacture of nitric acid

(iv) in the hydrogenation of vegetable oils.

What are the units of k for this reaction?

Which of the following are examples of heterogeneous equilibria?

(i) CaCO_3(s) <=> CaO_(s) + CO_2(g)

(ii) 2CrO₄^2-_(aq) + 2H⁺_(aq) <=> Cr₂O₇^2-_(aq) + H₂O_(l)

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

(iv) Co²⁺_(aq) + 6NH_3(aq) <=> [Co(NH₃)₆]²⁺_(aq)

Consider the following equilibrium:

N_2(g) + O_2(g) <=>2NO_(g)

5.00 x 10^-3 mol of N₂ was mixed with 4.00 x 10^-3 mol of O₂ and 11.0 x 10^-3 mol of NO and the mixture sealed in a container. The volume of the container was 0.500 dm³. The mixture was left to form a stable equilibrium. At this point, 9.00 x 10^-3 mol of NO was present in the mixture. The pressure was recorded as 45000 kpa

Calculate the value of K_p (no units) under these conditions.

Consider a cell constructed from the following half-cells:

Mg²⁺_(aq) + 2e^- <=> Mg_(s) E^ϴcell/V = -2.37

Ag⁺_(aq) + e^- <=> Ag_(s) E^ϴcell/V = +0.80

If the solution of Mg²⁺_(aq) was 2.00 mol dm^-3, would you expect to see a greater or smaller value of E^ϴcell/V than you would if the cell was set-up under standard conditions?

In which of the following industrial conversions is a chemical species (atoms, molecule or ion) oxidised to give the element:

(i) iron ore oxide to iron

(ii) potassium iodate(V) to iodine

(iii) copper(II) sulfate to copper

(iv) sodium chloride to chlorine

In a titration, 25 cm³ of 0.100 mol dm^-3 potassium hydroxide was neutralised by 12.5 cm³ dilute nitric acid. What was the concentration of the nitric acid?

In the family of hydrocarbons called alkanes:

(i) the boiling points of the straight chain compounds rise as the number of carbon atoms increases

(ii) the intermolecular forces arise from attractions between temporary dipoles

(iii) in any pair of isomers the compound with the more highly branched molecules has the lower boiling point

(iv) the unbranched compounds are all liquids at room temperature.

Which of these bonds are polar covalent bonds?

(i) C-C

(ii) H-Br

(iii) N-N

(iv) C=O

In which of these solids are there two types of bonding: one strong and one weak?

(i) diamond

(ii) ice

(iii) sodium chloride

(iv) graphite

In which of these molecules do the intermolecular forces arise largely from attractions between permanent dipoles?

Which of these molecules are overall polar?

(i) CH₃Cl

(ii) CH₂Cl₂

(iii) CHCl₃

(iv) CCl₄

Which of these compounds consist of molecules which are linear?

(i) water

(ii) beryllium chloride

(iii) sulfur dioxide

(iv) carbon dioxide

Which of these materials consist of a giant structure of ions?

(i) magnesium oxide

(ii) silicon dioxide

(iii) potassium fluoride

(iv) silicon chloride

What is the molecular formula of a hydrocarbon which consists of 82.8% carbon and has a relative molecular mass estimated in the range 50 and 60.