The Periodic Table & Trends (Cambridge (CIE) IGCSE Chemistry)

An element, M, has the electron distribution 2 + 8 + 18 + 3.

Which group in the Periodic Table is element M likely to be in?

Extended Only

Predict whether element M is a poor or a good conductor of electricity.
Give a reason for your answer.

Binary compounds contain two atoms per molecule, for example HCl.
Identify an element which could form a binary compound with element M.

Extended Only

Predict the formula of the sulfate of M. The formula of the sulfate ion is SO₄ ^2-.

Extended Only

The hydroxide of M is a white powder which is insoluble in water.
Describe how you could show that this hydroxide is amphoteric.

For each of the following, name an element which matches the description.

It is the only non-metal which is a good conductor of electricity.

Inert electrodes are made from this metal.

An element which can form an ion of the type X^3–.

It has the same electron distribution as the calcium ion, Ca²⁺.

The element is in Period 5 and Group VI.

Element Z is in Period 3 and Group V. Identify element Z.

Helium, neon and argon are noble gases.

Explain, in terms of the electronic structure, why neon is unreactive.

Copper is a transition element. It can have variable oxidation states.

State two other chemical properties of transition elements which make them different from Group I elements.

Aqueous chlorine reacts with aqueous magnesium bromide.

 Cl₂ + MgBr₂ → Br₂ + MgCl₂

 How does this reaction show that chlorine is more reactive than bromine?

What colour is bromine in aqueous solution?

Complete the word equation to show the halogen and halide compound which react to form the products iodine and sodium chloride. 

Explain, in terms of the reactivity of the halogens, why aqueous bromine will not react with aqueous sodium chloride.

The symbols of the elements in Period 2 of the Periodic Table are shown. 

Li  Be  B  C  N  O  F  Ne

For each of the following, give the symbol of an element from Period 2 which matches the description.

Each element may be used once, more than once or not at all.

Which element has atoms with only two electrons in the outer shell?

Which element is a monoatomic gas?

Which element is a soft metal stored in oil?

Which element has atoms with only seven protons?

The table below includes information about some of the elements in Period 2.

Why does neon exist as single atoms but fluorine exists as molecules?

What determines the order of the elements in a period?

Extended Only

When liquid nitrogen boils the following change occurs.

N₂(l) → N₂(g)

The boiling point of nitrogen is very low even though the bond between the atoms in a nitrogen molecule is very strong. Suggest an explanation.

Extended Only

Draw a diagram showing the arrangement of the outer shell (valency) electrons in a molecule of nitrogen.

The table below gives the electron distributions of atoms of different elements.

element electron distribution

For each of the following, select an element or elements from the table that matches the description. Each element may be selected once, more than once or not at all.

These two elements are in the same group.

This element forms a fluoride with a formula of the type XF₃.

This element reacts violently with cold water.

Separate: Chemistry and Extended Only

This element has a macromolecular structure similar to that of diamond.

The only oxidation state of this element is 0.

This element is bromine.

This element is a good conductor of electricity.

Use your copy of the Periodic Table to help you answer some of these questions.

Predict the formulae of the following compounds.

i) nitrogen fluoride .........................

ii) phosphorus sulfide ...................

Deduce the formulae of the following ions.

i) Selenide 

ii) Gallium 

Extended Only

Use the following ions to determine the formulae of the compounds.          

ions     OH^–    Cr³⁺    Ba²⁺    SO₄^2–

compounds

i) Chromium(III) sulfate 

ii) Barium hydroxide 

In the Periodic Table, the elements are arranged in columns called Groups and in rows called Periods.

i) Complete the table for some of the elements in Period 3.

[2]

ii) What is the relationship between the group number and the number of valency electrons?

[1]

iii) Explain the relationship between the number of valency electrons and the valency: For the elements Na to Al, For the elements P to Cl.

[4]

Extended Only

Across a period, the elements change from metallic to non-metallic.

i) Describe how the type of oxide changes across this period.

[2]

ii) Describe how the type of bonding in the chlorides formed by these elements changes across this period.

[2]

Separate: Chemistry Only

Trends can be observed in the way Group I and Group VII elements react. 

Suggest why Group I elements lithium, sodium and potassium are all stored in paraffin oil.

Separate: Chemistry and Extended Only

Caesium, Cs, is below potassium in Group I.

i) Give a similarity and a difference between the reactions of potassium with water and caesium with water.

similarity..........................................................

difference........................................................

[2]

ii) Give the chemical equation for the reaction between caesium and water.

[2]

Separate: Chemistry Only

Table 5.1 gives some information about the halogens. Complete the table by predicting the physical state of astatine at room temperature and the colour of astatine.

Table 5.1

Extended Only

A student investigates the reactivity of some halogens.

She uses these solutions of halogens and their halides.

• bromine, chlorine and iodine

• sodium bromide, sodium chloride and sodium iodide

She adds each halogen solution to each halide solution.

Table 5.2 shows her results.

Table 5.2

i) Explain how these results show the order of reactivity of bromine, chlorine and iodine.

[3]

ii) Suggest why the student does not need to add bromine solution to sodium bromide solution.

[1]

iii) The ionic equation for the reaction between bromine and sodium iodide is

Br₂ (aq) + 2I⁻ (aq) → I₂ (aq) + 2Br⁻ (aq)

Explain why this is a redox reaction.

[2]