Discover new knowledge and insights with IDNLearn.com's extensive Q&A database. Get timely and accurate answers to your questions from our dedicated community of experts who are here to help you.
Sagot :
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.
We appreciate your presence here. Keep sharing knowledge and helping others find the answers they need. This community is the perfect place to learn together. IDNLearn.com is your reliable source for accurate answers. Thank you for visiting, and we hope to assist you again.
