The first ionisation energy is the energy required to remove the most loosely bound electron from a neutral atom in its ground state. It generally increases across a period (from left to right) on the periodic table and decreases down a group (from top to bottom).

Sulphur (S) is in the 3rd period and 16th group of the periodic table.

1. Aluminium (Al) is in the 3rd period and 13th group. It is to the left of Sulphur in the same period, so it has a lower first ionisation energy.

2. Silicon (Si) is in the 3rd period and 14th group. It is also to the left of Sulphur, so it has a lower first ionisation energy.

3. Nitrogen (N) is in the 2nd period and 15th group. It is above and to the left of Sulphur, so it has a lower first ionisation energy.

4. Oxygen (O) is in the 2nd period and 16th group. It is directly above Sulphur, so it has a lower first ionisation energy.

5. Fluorine (F) is in the 2nd period and 17th group. It is above and to the right of Sulphur, so it has a higher first ionisation energy.

6. Phosphorus (P) is in the 3rd period and 15th group. It is to the left of Sulphur in the same period, so it has a lower first ionisation energy.

7. Chlorine (Cl) is in the 3rd period and 17th group. It is to the right of Sulphur in the same period, so it has a higher first ionisation energy.

8. Sodium (Na) is in the 3rd period and 1st group. It is far to the left of Sulphur in the same period, so it has a much lower first ionisation energy.

9. Neon (Ne) is in the 2nd period and 18th group. It is above and to the right of Sulphur, so it has a higher first ionisation energy.

So, the elements that have a first ionisation energy greater than that of Sulphur are Fluorine (F), Chlorine (Cl), and Neon (Ne). Therefore, there are 3 elements with a higher first ionisation energy than Sulphur.

Question

The first ionisation energy is the energy required to remove the most loosely bound electron from a neutral atom in its ground state. It generally increases across a period (from left to right) on the periodic table and decreases down a group (from top to bottom).

Sulphur (S) is in the 3rd period and 16th group of the periodic table.

1. Aluminium (Al) is in the 3rd period and 13th group. It is to the left of Sulphur in the same period, so it has a lower first ionisation energy.

2. Silicon (Si) is in the 3rd period and 14th group. It is also to the left of Sulphur, so it has a lower first ionisation energy.

3. Nitrogen (N) is in the 2nd period and 15th group. It is above and to the left of Sulphur, so it has a lower first ionisation energy.

4. Oxygen (O) is in the 2nd period and 16th group. It is directly above Sulphur, so it has a lower first ionisation energy.

5. Fluorine (F) is in the 2nd period and 17th group. It is above and to the right of Sulphur, so it has a higher first ionisation energy.

6. Phosphorus (P) is in the 3rd period and 15th group. It is to the left of Sulphur in the same period, so it has a lower first ionisation energy.

7. Chlorine (Cl) is in the 3rd period and 17th group. It is to the right of Sulphur in the same period, so it has a higher first ionisation energy.

8. Sodium (Na) is in the 3rd period and 1st group. It is far to the left of Sulphur in the same period, so it has a much lower first ionisation energy.

9. Neon (Ne) is in the 2nd period and 18th group. It is above and to the right of Sulphur, so it has a higher first ionisation energy.

So, the elements that have a first ionisation energy greater than that of Sulphur are Fluorine (F), Chlorine (Cl), and Neon (Ne). Therefore, there are 3 elements with a higher first ionisation energy than Sulphur.

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