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Which of the following arrangment for the three halogens Cl, Br and I when placed in the order of their increasing electron afffinity is correct?
- a)Cl, Br, I
- b)I, Br, Cl
- c)Br, Cl, I
- d)I, Cl, Br
Correct answer is option 'B'. Can you explain this answer?
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Which of the following arrangment for the three halogens Cl, Br and I ...
Electron affinity decrease as the electronegativity decrease and the size of atom increase.so, correct order would be from iodine to chlorine, electron affinity increase.
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Which of the following arrangment for the three halogens Cl, Br and I ...
Increasing Electron Affinity:
Electron affinity is the energy change that occurs when an electron is added to a neutral atom to form a negative ion. It is a measure of an atom's attraction for an additional electron. The general trend for electron affinity is to increase from left to right across a period and decrease down a group in the periodic table.
Arrangement of Halogens:
The halogens, which include chlorine (Cl), bromine (Br), and iodine (I), are located in Group 17 (Group VIIA) of the periodic table. As we move down the group, the atomic radius increases, and the electron affinity decreases.
Explanation:
The correct arrangement for the three halogens (Cl, Br, and I) in increasing electron affinity is option B, which is I, Br, Cl.
Reasoning:
- Iodine (I) has the highest atomic number and the largest atomic radius among the three halogens. The larger atomic radius leads to a weaker attraction for an additional electron, resulting in the lowest electron affinity.
- Bromine (Br) has a smaller atomic radius compared to iodine but larger than chlorine. It has a higher electron affinity than iodine but lower than chlorine.
- Chlorine (Cl) has the smallest atomic radius among the three halogens. It has the highest electron affinity due to its smaller atomic size and stronger attraction for an additional electron.
Therefore, the correct arrangement of the three halogens in increasing electron affinity is I (Iodine), Br (Bromine), and Cl (Chlorine), as given in option B.
Electron affinity is the energy change that occurs when an electron is added to a neutral atom to form a negative ion. It is a measure of an atom's attraction for an additional electron. The general trend for electron affinity is to increase from left to right across a period and decrease down a group in the periodic table.
Arrangement of Halogens:
The halogens, which include chlorine (Cl), bromine (Br), and iodine (I), are located in Group 17 (Group VIIA) of the periodic table. As we move down the group, the atomic radius increases, and the electron affinity decreases.
Explanation:
The correct arrangement for the three halogens (Cl, Br, and I) in increasing electron affinity is option B, which is I, Br, Cl.
Reasoning:
- Iodine (I) has the highest atomic number and the largest atomic radius among the three halogens. The larger atomic radius leads to a weaker attraction for an additional electron, resulting in the lowest electron affinity.
- Bromine (Br) has a smaller atomic radius compared to iodine but larger than chlorine. It has a higher electron affinity than iodine but lower than chlorine.
- Chlorine (Cl) has the smallest atomic radius among the three halogens. It has the highest electron affinity due to its smaller atomic size and stronger attraction for an additional electron.
Therefore, the correct arrangement of the three halogens in increasing electron affinity is I (Iodine), Br (Bromine), and Cl (Chlorine), as given in option B.
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Which of the following arrangment for the three halogens Cl, Br and I when placed in the order of their increasing electron afffinity is correct?a)Cl, Br, Ib)I, Br, Clc)Br, Cl, Id)I, Cl, BrCorrect answer is option 'B'. Can you explain this answer?
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