Group 1 (Edexcel GCSE Chemistry)

Which statement explains why Group 1 metals get more reactive further down the group?
 

Lithium, sodium and potassium are reactive metals in group 1 of the periodic table.

Sodium metal tarnishes in air to form a layer of sodium oxide on its surface.
0.92 g of sodium combined with 0.32 g of oxygen in this oxide.

Calculate the empirical formula of this sodium oxide.
(relative atomic masses: O = 16, Na = 23)

You must show your working.

............Na (............) + 2H₂O (............) ............NaOH (............) + H₂ (............)

In an experiment equal-sized pieces of lithium, sodium and potassium are added to separate samples of water.

Figure 14

Describe, in detail, how the teacher would demonstrate this experiment safely, showing how the results give the order of reactivity of the metals.

(6)

Explain, in terms of electronic configurations, the increase in reactivity from lithium to sodium to potassium.

Sodium reacts with water to form sodium hydroxide solution and hydrogen. 

Which of the following balanced symbol equations with state symbols is correct? 
 

Which of the following is not a property of Group 1 metals?

Some of the elements in the periodic table are metals.
The electronic configuration of a metal is 2.8.3

Which row shows the group and period of the periodic table where this metal is found?

(2)

(3)

Higher Only

A sample of lithium contains

7.59% of lithium-6
92.41% of lithium-7.

Calculate the relative atomic mass of lithium in this sample.

Give your answer to two decimal places.
You must show your working.

When lithium is added to water, a gas is produced. 

Which test and result would correctly identify this gas?

When sodium reacts with water an alkaline solution is formed.

Which statement about why this happens is true?

The first four elements in group 1 are lithium, sodium, potassium and rubidium.

Rubidium reacts with water to form rubidium hydroxide and hydrogen.

2Rb(s) + 2H₂O(l) → 2RbOH(aq) + H₂(g)

An example of an endothermic reaction is the reaction between rubidium hydroxide and ammonium carbonate, (NH₄)₂CO₃.
This reaction forms rubidium carbonate, Rb₂CO₃, ammonia and one other product.

Write the balanced equation for this reaction.

The elements in Group 1 become more reactive as you go down the group. 

Potassium is below sodium in Group 1. 

Both metals are added to water. 

Predict one observation you would see that shows potassium is more reactive than sodium.

Write the balanced symbol equation for the reaction between potassium and water. 

You should include state symbols in your answer. 

Explain why potassium is more reactive than sodium. 

Potassium reacts with oxygen to form potassium oxide. 

Explain why potassium oxide has a high melting point. 

Group 1 metals are located in the Periodic Table. 

Explain why they are called the alkali metals. 

Sodium hydroxide is produced when sodium is added to water. 

Sodium hydroxide reacts with sulfuric acid in a neutralisation reaction. 

Suggest why sodium needs to be stored under oil. 

Sodium is a Group 1 metal. 

Sodium is able to conduct electricity. 

Explain why. 

Element Z has the following properties:

• It is a solid at room temperature
• Does not conduct heat or electricity
• Forms simple molecules with non-metals
• Forms giant ionic lattices with metals in which it has a 1- ion

Select the formula of the compound formed when element Z reacts with calcium from the list below.

Explain your answer using the information provided.

Calcium is a Group 2 metal. Group 2 metals show similar trends in reactivity to Group 1 metals as you go down the group. 

Magnesium is another Group 2 metal.

Explain why, in terms of atomic structure, magnesium reacts in a similar way to calcium with element Z but it is less reactive than calcium.