An element has successive ionization enthalpies as 940 (first),2080,3090,4140,7030,7870,16000 and 19500 kJ `mol^(-1)`. To which group of the periodic table does this element belong?

Options

A. 14
B. 15
C. 16
D. 17

Answer

To determine the group of the periodic table to which the element belongs based on its successive ionization enthalpies, we can follow these steps:

### Step 1: Analyze the Ionization Energies
The given successive ionization enthalpies are:
- 1st: 940 kJ/mol
- 2nd: 2080 kJ/mol
- 3rd: 3090 kJ/mol
- 4th: 4140 kJ/mol
- 5th: 7030 kJ/mol
- 6th: 7870 kJ/mol
- 7th: 16000 kJ/mol
- 8th: 19500 kJ/mol

### Step 2: Identify Trends in Ionization Energies
Observe the trend in the ionization energies:
- The first to the sixth ionization energies show a gradual increase.
- However, there is a significant jump between the 6th (7870 kJ/mol) and the 7th (16000 kJ/mol) ionization energies.

### Step 3: Interpret the Large Jump
The large increase in ionization energy from the 6th to the 7th indicates that the 6th electron is being removed from a much more stable electron configuration, likely a noble gas configuration. This suggests that the element has 6 valence electrons.

### Step 4: Determine the Electron Configuration
Since the element has 6 valence electrons, its outer electron configuration can be represented as:
- ns² np⁴ (where n is the principal quantum number).

### Step 5: Identify the Group
Elements with 6 valence electrons belong to Group 16 of the periodic table (also known as the chalcogens). This group includes elements like oxygen, sulfur, and selenium.

### Conclusion
Based on the analysis of the ionization enthalpies, the element belongs to Group 16 of the periodic table.

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