Sec 4 Chemistry The Periodic Table topical questions

State what is meant by a group and by a period in the Periodic Table.

Element Y has electron arrangement 2.8.7.

1. (a)State which group Y is in.[1]
2. (b)State which period Y is in.[1]
3. (c)Name group Y if it is a halogen with 17 protons.[1]

State the colour and physical state at room temperature of each halogen.

1. (a)Chlorine[1]
2. (b)Bromine[1]
3. (c)Iodine[1]

Name the gas produced when potassium reacts with water, and state the test for it.

The three commonest alkali metals are added to cold water in turn.

1. (a)State what each metal produces that turns universal indicator purple.[1]
2. (b)Name the gas released and give its test.[2]
3. (c)Write the equation for sodium with water.[1]

Match each element to one everyday use, naming the property the use depends on.

1. (a)Give one use for each element.[1]
2. (b)State the property behind one of the uses.[2]

Explain why sodium is more reactive than lithium, referring to electron arrangement.

Chlorine water is added to a solution containing both potassium bromide and potassium iodide.

1. (a)State and explain what happens to the bromide ions.[2]
2. (b)Write the ionic equation for the reaction with iodide ions.[2]
3. (c)State the colour change you would see in the solution.[1]

Explain why argon is used inside light bulbs rather than air.

A solid element melts at 1455 °C, forms green and blue compounds in solution, and is used as a catalyst in hydrogenation of oils.

1. (a)Identify the element.[1]
2. (b)State the block of the Periodic Table it belongs to.[1]
3. (c)Name two properties you used from the information, and one further typical property of its block.[2]

Sodium reacts with water; chlorine reacts with hydrogen. Both are Group VII/I chemistry in action.

1. (a)Write the equation for sodium reacting with water.[2]
2. (b)State two observations when a small piece of sodium is placed on water.[2]
3. (c)Name the compound formed when hydrogen burns in chlorine.[1]

Complete the displacement table: does the added halogen water turn the salt solution coloured (displacement) or unchanged?

1. (a)Complete the three missing results.[3]
2. (b)State the reactivity order the table proves.[1]

Group I and Group VII reactivity run in opposite directions down the table.

1. (a)Explain why Group I metals get MORE reactive going down.[2]
2. (b)Explain why Group VII non-metals get LESS reactive going down.[2]

A halogen W displaces bromine from potassium bromide solution but does not change potassium fluoride solution. The W⁻ ion has 18 electrons.

1. (a)Deduce the proton number and identity of W.[2]
2. (b)State W’s group and period.[2]
3. (c)Write the ionic equation for W displacing bromine.[1]

Three unlabelled halogen solutions are tested: solution P displaces iodine from KI but does not change KBr solution; solution Q displaces bromine from KBr (and would also displace iodine); solution R displaces neither iodine from KI nor bromine from KBr.

1. (a)Identify each solution as a halogen, ranking them by reactivity.[3]
2. (b)Write the equation for Q reacting with KI.[2]
3. (c)Predict and explain what R does with KBr.[1]

Element Z is in Group II, period 4, of the Periodic Table.

1. (a)Deduce the electron arrangement of Z.[2]
2. (b)State whether Z is a metal or non-metal and give the formula of its ion.[2]
3. (c)Write the equation for Z reacting with dilute hydrochloric acid, using Z as its symbol.[2]

Compare Group I metals with transition metals in terms of melting point, hardness, oxidation states, compound colour and catalytic ability.

Melting and boiling data for three halogens are given below.

1. (a)State the physical state of each halogen at room temperature (about 25 °C).[1]
2. (b)Explain why the melting and boiling points rise down the group.[3]
3. (c)Predict the physical state of astatine, At₂, at room temperature, with a reason.[2]