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As we move down a group, electronegativity of elements generally:
- a)Increases
- b)Decreases
- c)Increases and then decreases
- d)Decreases and then increases
Correct answer is option 'B'. Can you explain this answer?
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As we move down a group, electronegativity of elements generally:a)Inc...
Electronegativity
Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. It is a fundamental property of elements and plays a crucial role in determining the nature of chemical compounds and reactions.
Trends in Electronegativity
The electronegativity of elements generally follows specific trends as we move across periods and down groups in the periodic table. Across a period, electronegativity generally increases from left to right due to the increasing effective nuclear charge and decreasing atomic radius.
Down a Group
As we move down a group in the periodic table, the electronegativity of elements generally decreases. This trend can be explained by several factors:
Increasing Atomic Size
As we move down a group, the atomic size or atomic radius of elements increases. This is due to the addition of new energy levels or shells as we move from top to bottom. The increase in atomic size means that the outermost electrons are farther away from the nucleus, resulting in a weaker attraction towards incoming electrons. Therefore, elements lower in a group have lower electronegativity values.
Shielding Effect
The increase in atomic size also leads to an increase in the number of inner electrons or electron shells. These inner electrons act as a shielding effect, repelling the outermost electrons from the positive charge of the nucleus. As a result, the effective nuclear charge experienced by the outermost electrons decreases down a group. With a weaker attraction, the electronegativity of elements decreases.
Distance from the Nucleus
The distance between the outermost electrons and the nucleus plays a significant role in determining electronegativity. As we move down a group, the distance between the outermost electrons and the nucleus increases, resulting in a weaker attraction. The outermost electrons are held less tightly, making it easier for another atom to attract them and form a bond. This decrease in electron-attracting ability leads to a decrease in electronegativity.
Therefore, as we move down a group, the electronegativity of elements generally decreases. This trend can be attributed to increasing atomic size, the shielding effect of inner electrons, and the distance between the outermost electrons and the nucleus.
Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. It is a fundamental property of elements and plays a crucial role in determining the nature of chemical compounds and reactions.
Trends in Electronegativity
The electronegativity of elements generally follows specific trends as we move across periods and down groups in the periodic table. Across a period, electronegativity generally increases from left to right due to the increasing effective nuclear charge and decreasing atomic radius.
Down a Group
As we move down a group in the periodic table, the electronegativity of elements generally decreases. This trend can be explained by several factors:
Increasing Atomic Size
As we move down a group, the atomic size or atomic radius of elements increases. This is due to the addition of new energy levels or shells as we move from top to bottom. The increase in atomic size means that the outermost electrons are farther away from the nucleus, resulting in a weaker attraction towards incoming electrons. Therefore, elements lower in a group have lower electronegativity values.
Shielding Effect
The increase in atomic size also leads to an increase in the number of inner electrons or electron shells. These inner electrons act as a shielding effect, repelling the outermost electrons from the positive charge of the nucleus. As a result, the effective nuclear charge experienced by the outermost electrons decreases down a group. With a weaker attraction, the electronegativity of elements decreases.
Distance from the Nucleus
The distance between the outermost electrons and the nucleus plays a significant role in determining electronegativity. As we move down a group, the distance between the outermost electrons and the nucleus increases, resulting in a weaker attraction. The outermost electrons are held less tightly, making it easier for another atom to attract them and form a bond. This decrease in electron-attracting ability leads to a decrease in electronegativity.
Therefore, as we move down a group, the electronegativity of elements generally decreases. This trend can be attributed to increasing atomic size, the shielding effect of inner electrons, and the distance between the outermost electrons and the nucleus.
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As we move down a group, electronegativity of elements generally:a)Inc...
As we move down a group, atomic size increases which means that the valence electrons are much farther from the nucleus and hence experience less force of attraction. Hence the electronegativity decreases down the group.
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As we move down a group, electronegativity of elements generally:a)Increasesb)Decreasesc)Increases and then decreasesd)Decreases and then increasesCorrect answer is option 'B'. Can you explain this answer?
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