Group 0 (Edexcel GCSE Chemistry)

Which statement about noble gases is not correct?

Which of the following statements is not a correct statement about helium?

Argon has an atomic number of 18.

What is the electronic configuration for this atom?

(1)

Figure 4

Figure 5

Mendeleev produced one of the earliest periodic tables.

State why he could not include any of the noble gases in his periodic table.

Figure 6

(2)

(1)

boiling point of xenon = ............................ °C

Argon has a boiling point of -186^oC. 

Which would be the best prediction of the boiling point of xenon?

Which of the following lists four noble gases in order of increasing density?

This question is about the noble gases.

Give three characteristic properties of the noble gases.

(1)

(3)

Figure 1

Use the data in Figure 1 to predict the density of krypton.

Higher only

Helium most commonly exists as 2 isotopes, ³He and ⁴He.
The ratio of ⁴He to ³He atoms is 7 000 000 : 1

Explain why the relative atomic mass of helium is 4.00, to 2 decimal places, despite a lighter isotope existing.

The noble gases are inert gases.

Explain why these elements are unreactive.

Inert is used to describe a substance that does not chemically react under given conditions.

Whilst the noble gases are very unreactive, under certain conditions, some noble gases can react to form compounds. For example, krypton can form a solid with fluorine and xenon can form compounds with oxygen and fluorine.

Suggest why helium and neon cannot undergo such reactions.

Suggest why fluorine is able to form compounds with xenon and krypton but bromine is not.

Predict what type of bonding would exist in xenon difluoride, XeF₂. Explain your answer.

The positions of five elements, A, B, C, D and E are shown in the Periodic Table. 

These letters are not the atomic symbols of the elements. 

Suggest one use of E. 

The element below E in the Periodic Table is used to fill electric light bulbs. 

State why this element is used in the light bulb. 

Explain your answer in terms of the electronic structure of the atom. 

Explain the trend in melting point going down Group 0. 

Compare the electronic structure of elements D and E. 

Use the positions of the elements to deduce their electronic configurations and include these in your answer. 

Table 1 shows the electronic structures of five elements.

The letters are not the chemical symbols of the element.

Table 1

Give the letters of two elements that belong to the same group in the periodic table.

State the group that they belong to.

Use Table 1 and the periodic table.

Give the letter of the element that is monatomic.

Explain your answer.

Give the letters of two elements that are gases at room temperature.

Higher Only

A sample of neon contains:

• 90.48 % of neon-20 atoms
• 0.27% of neon-21 atoms
• 9.25 % of neon-22 atoms 

Use this information to calculate the relative atomic mass of neon in this sample.