AS IE and electron configuration

1

What is the total number of orbitals in a sulfur atom which contain at least one electron?

3

5

8

9

1

A

B

C

D

1

A

B

C

D

1

A

B

C

D

1

Which equation represents the first ionisation energy of iodine?

A I₂(s) → 2I⁺(g) + 2e⁻

B I₂(g) → 2I⁺(g) + 2e⁻

C ¹⁄₂I₂(s) → I⁺(g) + e⁻

D I(g) → I⁺(g) + e⁻

The graph shows the first ionisation energies of some consecutive elements from Periods 2 and 3 of the Periodic Table.

The letters used to label the elements are not their chemical symbols.

1

Which element has only one p orbital containing a pair of electrons?

A element U

B element V

C element W

D element X

1

Which is a reason why fluorine has a higher first ionisation energy than oxygen?

A a fluorine atom has fewer unpaired electrons

B a fluorine atom has fewer shells of electrons

C a fluorine atom has more electrons

D a fluorine atom has more protons

1

Which is the equation for the second ionisation of element J?

A J(g) → J²⁺(g) + 2e^–

B J⁺(g) → J²⁺(g) + e^–

C J⁺(g) → J³⁺(g) + 2e^–

D J²⁺(g) → J³⁺(g) + e^–

This question is about the ionisation energies of the elements in Period 2 of the Periodic Table.

The first ionisation energies of the Period 2 elements are shown

1

Give an equation that represents the first ionisation energy of lithium. Include state symbols

2

Explain why there is a general increase in the first ionisation energy across the period.

2

Explain why the first ionisation energy of oxygen is lower than that of nitrogen

2

This question is about barium and barium compounds.

1

Write an equation, including state symbols, for the third ionisation energy of barium.

1

AS IE and electron configuration

What is the total number of orbitals in a sulfur atom which contain at least one electron?

Which equation represents the first ionisation energy of iodine?

Which element has only one p orbital containing a pair of electrons?

Which is a reason why fluorine has a higher first ionisation energy than oxygen?

Which is the equation for the second ionisation of element J?

Give an equation that represents the first ionisation energy of lithium. Include state symbols

Explain why there is a general increase in the first ionisation energy across the period.

Explain why the first ionisation energy of oxygen is lower than that of nitrogen

Write an equation, including state symbols, for the third ionisation energy of barium.

State how the graph confirms that barium is in Group 2 in the Periodic Table

What is the total number of orbitals in a sulfur atom which contain at least one electron?

What is the electronic configuration of a nitrogen atom?

What is the electronic configuration of an oxygen atom in its ground state?

Which is the electronic configuration of chromium?

Which equation represents the first ionisation energy of iodine?

Which element has only one p orbital containing a pair of electrons?

Which element is the least reactive?

Which element has the greatest second ionisation energy?

Which is a reason why fluorine has a higher first ionisation energy than oxygen?

Which is the equation for the second ionisation of element J?

Give an equation that represents the first ionisation energy of lithium. Include state symbols

Explain why there is a general increase in the first ionisation energy across the period.

Explain why the first ionisation energy of oxygen is lower than that of nitrogen

All the successive ionisation energies of nitrogen are shown in the table.
Explain the trend in the successive ionisation energies of nitrogen.

Write an equation, including state symbols, for the third ionisation energy of barium.

State how the graph confirms that barium is in Group 2 in the Periodic Table

Which element is the least reactive?

Which element has the greatest second ionisation energy?

AS IE and electron configuration

AS IE and electron configuration

What is the total number of orbitals in a sulfur atom which contain at least one electron?

Which equation represents the first ionisation energy of iodine?

Which element has only one p orbital containing a pair of electrons?

Which is a reason why fluorine has a higher first ionisation energy than oxygen?

Which is the equation for the second ionisation of element J?

Give an equation that represents the first ionisation energy of lithium. Include state symbols

Explain why there is a general increase in the first ionisation energy across the period.

Explain why the first ionisation energy of oxygen is lower than that of nitrogen

Write an equation, including state symbols, for the third ionisation energy of barium.

State how the graph confirms that barium is in Group 2 in the Periodic Table

What is the total number of orbitals in a sulfur atom which contain at least one electron?

What is the electronic configuration of a nitrogen atom?

What is the electronic configuration of an oxygen atom in its ground state?

Which is the electronic configuration of chromium?

Which equation represents the first ionisation energy of iodine?

Which element has only one p orbital containing a pair of electrons?

Which element is the least reactive?

Which element has the greatest second ionisation energy?

Which is a reason why fluorine has a higher first ionisation energy than oxygen?

Which is the equation for the second ionisation of element J?

Give an equation that represents the first ionisation energy of lithium. Include state symbols

Explain why there is a general increase in the first ionisation energy across the period.

Explain why the first ionisation energy of oxygen is lower than that of nitrogen

All the successive ionisation energies of nitrogen are shown in the table.Explain the trend in the successive ionisation energies of nitrogen.

Write an equation, including state symbols, for the third ionisation energy of barium.

State how the graph confirms that barium is in Group 2 in the Periodic Table

Which element is the least reactive?

Which element has the greatest second ionisation energy?

All the successive ionisation energies of nitrogen are shown in the table.
Explain the trend in the successive ionisation energies of nitrogen.