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The main reason for showing anomalous properties of the first member of a group in s or p-block is
- a)Maximum chemical reactivity
- b)Maximum electronegativity and different configurations
- c)Small size, large charge/radius ratio
- d)Tendency to form multiple bonds
Correct answer is option 'C'. Can you explain this answer?
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The main reason for showing anomalous properties of the first member o...
Due to small size, large charge/radius ratio and high electronegativity, the first elementshows anomalous behaviour.
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The main reason for showing anomalous properties of the first member o...
The main reason for showing anomalous properties of the first member of a group in the s or p-block is the small size and large charge/radius ratio.
Explanation:
The first member of a group in the s or p-block of the periodic table often exhibits anomalous properties compared to the other members of the group. This can be attributed to the unique characteristics of the first element, which include its small size and large charge/radius ratio.
Small Size:
The first element in a group typically has the smallest atomic size compared to the other members of the group. This is because the atomic size generally increases as you move down a group due to the addition of new electron shells. The small size of the first element affects its chemical reactivity and bonding behavior, leading to anomalous properties.
Large Charge/Radius Ratio:
The first element of a group also has a large charge/radius ratio. This means that the positive charge of the nucleus is concentrated in a smaller space, resulting in a higher effective nuclear charge. The large charge/radius ratio influences the electron distribution and bonding characteristics of the first element, making it differ from the other members of the group.
Anomalous Properties:
The small size and large charge/radius ratio of the first element can lead to various anomalous properties, including:
- Different electronic configurations: The first element may have a different electron configuration compared to the other members of the group due to its smaller size and unique electronic structure. This can affect its chemical reactivity and bonding behavior.
- Higher ionization energy: The first element may have a higher ionization energy compared to the other members of the group due to its smaller size and stronger effective nuclear charge. This makes it less likely to lose electrons and form positive ions.
- Greater electronegativity: The first element may exhibit higher electronegativity compared to the other members of the group due to its small size and stronger effective nuclear charge. This affects its ability to attract electrons in chemical reactions.
- Tendency to form multiple bonds: The first element may have a greater tendency to form multiple bonds compared to the other members of the group. This is because its small size and high charge/radius ratio enable stronger bonding interactions.
In conclusion, the small size and large charge/radius ratio of the first member of a group in the s or p-block of the periodic table are the main reasons for its anomalous properties.
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The main reason for showing anomalous properties of the first member of a group in s or p-block isa)Maximum chemical reactivityb)Maximum electronegativity and different configurationsc)Small size, large charge/radius ratiod)Tendency to form multiple bondsCorrect answer is option 'C'. Can you explain this answer?
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