Question

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Why does bromine (Br) have a smaller atomic radius than scandium (Sc)?
A. Scandium (Sc) has more energy shells than bromine (Br), making its atoms bigger.
B. Bromine (Br) has less neutrons than scandium (Sc), so it does not have as much mass.
C. Bromine (Br) has more electrons, which makes its energy sublevels more negative, which pulls them closer to the positively charged nucleus.
D. Electrons are added from right to left across the periodic table, so bromine (Br) does not have as many as scandium (Sc).

Answer 1

Answer:

Option (C) Bromine (Br) has more electrons, which makes its energy sublevels more negative, which pulls them closer to the positively charged nucleus.

Answer 2

Atomic radius is the size of the atom that measures from the center to the outermost electron.  Bromine has a smaller atomic radius because of more number of electrons. Thus, option C is correct.

What is the periodic trend of radii?

The elements are placed in the periods and groups in the periodic table based on the atomic number. Bromine belongs to group 17, period 4 in the periodic table, and scandium (Sc) to group 3, period 4.

In the periodic trend, the atomic radii of the element in the period decrease when moving from left-right. Here bromine and scandium both belong to the same period but differ in the group.

The number of electrons in bromine is more than the scandium element that in turn increases the force of attraction towards the nucleus making them have smaller radii.

Therefore, bromine has smaller radii.

Learn more about atomic radii here:

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