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Why is an iodine ion more stable than a chloride ion?
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+ Inorganic chemistry
+ Ions
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+ Iodine
+ Organic chemistry
Posted by
Mounir Shita
Why is an iodine ion more stable than a chloride ion?
HI is a stronger acid than HCl, so the conjugate base I- will be weaker and stable ion than Cl- ion.
The effective nuclear chare of I-..ion is higher than that of Cl-ion. So the electron charge density of I- ion is strongly attracted by its nucleus than that in Cl-. So I- is less reactive than Cl-.
HI is a stronger acid than HCl, so the conjugate base I- will be weaker and stable ion than Cl- ion.
The effective nuclear chare of I-..ion is higher than that of Cl-ion. So the electron charge density of I- ion is strongly attracted by its nucleus than that in Cl-. So I- is less reactive than Cl-.
I think you mean to compare iodide (I-) (never say iodine ion because a halide ion with -1 O.S. always end with a suffix -ide) and chloride (Cl-) ions.
A general comparison between the stability of two ions can be made by considering a few factors, provided they either belong to the same group or same period.
Size is use to determine the stability among anions belonging to same group.
Electronegativity is used to determine the stability among anions of different groups.
I- and Cl- belong to same group, so we should compare their sizes. I- is larger in size as it belongs to the 5th period, the negative charge will be more dispersed or spread in the I- compared to Cl-, thus making I- more stable than Cl-.
I think you mean to compare iodide (I-) (never say iodine ion because a halide ion with -1 O.S. always end with a suffix -ide) and chloride (Cl-) ions.
A general comparison between the stability of two ions can be made by considering a few factors, provided they either belong to the same group or same period.
Size is use to determine the stability among anions belonging to same group.
Electronegativity is used to determine the stability among anions of different groups.
I- and Cl- belong to same group, so we should compare their sizes. I- is larger in size as it belongs to the 5th period, the negative charge will be more dispersed or spread in the I- compared to Cl-, thus making I- more stable than Cl-.
HI is a stronger acid than HCl, so the conjugate base I- will be weaker and stable ion than Cl- ion.
The effective nuclear chare of I-..ion is higher than that of Cl-ion. So the electron charge density of I- ion is strongly attracted by its nucleus than that in Cl-. So I- is less reactive than Cl-.
HI is a stronger acid than HCl, so the conjugate base I- will be weaker and stable ion than Cl- ion.
The effective nuclear chare of I-..ion is higher than that of Cl-ion. So the electron charge density of I- ion is strongly attracted by its nucleus than that in Cl-. So I- is less reactive than Cl-.
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I think you mean to compare iodide (I-) (never say iodine ion because a halide ion with -1 O.S. always end with a suffix -ide) and chloride (Cl-) ions.
A general comparison between the stability of two ions can be made by considering a few factors, provided they either belong to the same group or same period.
I think you mean to compare iodide (I-) (never say iodine ion because a halide ion with -1 O.S. always end with a suffix -ide) and chloride (Cl-) ions.
A general comparison between the stability of two ions can be made by considering a few factors, provided they either belong to the same group or same period.
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