Question

Which of the following is the smallest in size? A)I- B)I C)Br D)Br-

Answer 1

Answer:

C---Br ---bromine

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Answer 2

Answer:

Explanation:

• The number of electrons surrounding the nucleus is the only distinction between an atom and its ions.

• The covalent radii and Ionic radii in 'nm' for Bromin $(Br)$   and Iodine   $(I)$ are given as follows:

$\begin{array}{lll}\text { Element } & Covalent Radii & Ionic Radii \\\text { Br } & 0.1142 & 0.196 \\\text { I } & 0.1333 & 0.216\end{array}$

• The negative ion is much larger than the atom that created it. In fact, the negative ion can be twice the size of the neutral atom.
• The relative size of positive and negative ions has important implications for ionic compound structure. Positive ions are frequently so small that they pack into the gaps between planes of adjacent negative ions.
• Hence, $Br-$  and $I-$ are larger than its positive ions $Br$  and $I$ respectively.
• So, the negative ions are eliminated from options.
• Out of $Br$ and $I$ , the smallest element is $Br$  based on the Ionic radii.
• Hence, $Br$ is smallest in size than $Br- , I$ and $I-$.

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