Answer :
Let's analyze the properties of antimony (Sb) and iodine (I) from the given data and predict the ionization energy and electronegativity for Sb and I.
Given Data:
- Antimony (Sb):
- Atomic radius: 145 pm
- First ionization energy: Not explicitly given
- Electron affinity: -103 kJ/mol
- Electronegativity: 2.05
- Iodine (I):
- Atomic radius: 140 pm
- First ionization energy: 1008 kJ/mol
- Electron affinity: -295 kJ/mol
- Electronegativity: Not explicitly given
### Step-by-step prediction and analysis:
#### 1. Ionization Energy:
- Ionization energy tends to increase across a period from left to right and generally decreases down a group. Given that iodine is to the right of antimony in the periodic table, it is likely that iodine will have a higher ionization energy than antimony.
- Given:
- First ionization energy of iodine (I) = 1008 kJ/mol
Based on periodic trends, a reasonable prediction for the first ionization energy of antimony (Sb) is about 50 kJ/mol less than that of iodine:
- First ionization energy of antimony (Sb) ≈ 1008 kJ/mol - 50 kJ/mol = 958 kJ/mol
#### 2. Electronegativity:
- Electronegativity tends to increase across a period from left to right and generally decreases down a group. Since iodine is to the right of antimony, iodine is expected to have a higher electronegativity than antimony.
- Given:
- Electronegativity of antimony (Sb) = 2.05
Based on periodic trends, a reasonable assumption is that the electronegativity of iodine is about 0.5 units higher than that of antimony:
- Electronegativity of iodine (I) ≈ 2.05 + 0.5 = 2.55
### Analysis of Predictions:
We were given multiple prediction statements to choose from:
1. Sb has a lower ionization energy but a higher electronegativity than I.
2. Sb has a higher ionization energy but a lower electronegativity than I.
3. Sb has a lower ionization energy and a lower electronegativity than I.
4. Sb has a higher ionization energy and a higher electronegativity than I.
Comparing the predicted values:
- Ionization energy of Sb = 958 kJ/mol which is lower than the ionization energy of I = 1008 kJ/mol.
- Electronegativity of Sb = 2.05 which is lower than the electronegativity of I = 2.55.
Therefore, the most accurate prediction from the given options is:
- Sb has a lower ionization energy and a lower electronegativity than I.
Hence, the correct prediction is:
Sb has a lower ionization energy and a lower electronegativity than I.
Given Data:
- Antimony (Sb):
- Atomic radius: 145 pm
- First ionization energy: Not explicitly given
- Electron affinity: -103 kJ/mol
- Electronegativity: 2.05
- Iodine (I):
- Atomic radius: 140 pm
- First ionization energy: 1008 kJ/mol
- Electron affinity: -295 kJ/mol
- Electronegativity: Not explicitly given
### Step-by-step prediction and analysis:
#### 1. Ionization Energy:
- Ionization energy tends to increase across a period from left to right and generally decreases down a group. Given that iodine is to the right of antimony in the periodic table, it is likely that iodine will have a higher ionization energy than antimony.
- Given:
- First ionization energy of iodine (I) = 1008 kJ/mol
Based on periodic trends, a reasonable prediction for the first ionization energy of antimony (Sb) is about 50 kJ/mol less than that of iodine:
- First ionization energy of antimony (Sb) ≈ 1008 kJ/mol - 50 kJ/mol = 958 kJ/mol
#### 2. Electronegativity:
- Electronegativity tends to increase across a period from left to right and generally decreases down a group. Since iodine is to the right of antimony, iodine is expected to have a higher electronegativity than antimony.
- Given:
- Electronegativity of antimony (Sb) = 2.05
Based on periodic trends, a reasonable assumption is that the electronegativity of iodine is about 0.5 units higher than that of antimony:
- Electronegativity of iodine (I) ≈ 2.05 + 0.5 = 2.55
### Analysis of Predictions:
We were given multiple prediction statements to choose from:
1. Sb has a lower ionization energy but a higher electronegativity than I.
2. Sb has a higher ionization energy but a lower electronegativity than I.
3. Sb has a lower ionization energy and a lower electronegativity than I.
4. Sb has a higher ionization energy and a higher electronegativity than I.
Comparing the predicted values:
- Ionization energy of Sb = 958 kJ/mol which is lower than the ionization energy of I = 1008 kJ/mol.
- Electronegativity of Sb = 2.05 which is lower than the electronegativity of I = 2.55.
Therefore, the most accurate prediction from the given options is:
- Sb has a lower ionization energy and a lower electronegativity than I.
Hence, the correct prediction is:
Sb has a lower ionization energy and a lower electronegativity than I.
