atomic radius of anions

[asalest 2K]

why is the atomic radius of Br- larger than Na?

[Steph Du 1H]

They aren't in the same row and atomic radius increases as you go down. Br is further down than Na.

[Astha Sahoo 3I]

Br- is one whole shell larger than Na, making it's electrons(especially valence electrons) farther apart from the nucleus, thus giving it a larger electron cloud.

[Chelsea_Guzman_3C]

In the periodic table, the atomic radius decreases along a row from left to right, but increases in a group from top to bottom. Br is found further down the periodic table than Na, so the atomic radius is larger for Br, despite it being on the further right side of the periodic table.

[Anastasia Yulo 1C]

In neutral state, Bromine is smaller than Na due to it's location on the far right of the periodic table. However, Br- is an anion. Anions have bigger ionic radii than their corresponding neutral atoms.

[ShinwooKim_3E]

The general trend of the atomic radius is that it decreases as you go across a period (left to right), and increases from above to below in a group.

[Lung Sheng Liang 3J]

Atomic radius increases as you go down a group, and Br- is below Na.

[Heather Szeszulski 1I]

Atomic radius increases as you go down a group, Br- is a whole shell below Na making it a bigger radius.

[George_Yin_3I]

The atomic radius increases down a group and generally decreases across a period, so Br- is naturally greater in radius than Na.

[George_Yin_3I]

If the two atoms/ions are isoelectronic, then the one with greater proton number is smaller because it means greater effective nuclear charge from the central atom.