Why Does Group 1 Have The Largest Atomic Radius?

Why do alkali metals have the largest radius?

Alkali metals have largest covalent radii because

they poses only 1 electron in their outer level and good screening in inner level

and that results lower force of attraction.

Which element in group 1 has the largest atomic radius?

What group has the highest atomic radius?

Atomic radii vary in a predictable way across the periodic table. As can be seen in the figures below, the atomic radius increases from top to bottom in a group, and decreases from left to right across a period. Thus, helium is the smallest element, and

francium

is the largest.

Which noble gas has the largest atomic radius?

• Helium (highest ionization level in the periodic table)
• Neon.
• Argon.
• Krypton.
• Xenon.
• Radon.

What element in the alkali family has the largest atomic radius?

According to the periodic table

Cesium metal

atom has the largest atomic radius.

What has the smallest atomic radius?

Helium

has the smallest atomic radius. This is due to trends in the periodic table, and the effective nuclear charge that holds the valence electrons close to the nucleus.

Which alkali metal is largest?

Cesium

is the largest atom among alkali metal.

What has the largest atomic radius?

Smallest and Largest Atomic Radius

Francium

has the largest atomic size on the periodic table, and helium has the smallest atomic size.

What has a bigger radius Br or Br explain?

The bromide ion Br- has

the larger radius.

The additional electron in the anion causes more electron-electron repulsion. The electrons spread out more in space resulting to the larger radius of an anion than its parent atom.

Which element in the group has the largest atomic number?

Which inert gas has the largest atomic radius?

<br> Statement-2: In case of noble gases van der Waal’s radius is defined and there is much inter electronic repulsions.

Why do noble gases have smallest atomic radius?

Noble gases don’t form (or don’t easily form) bonds. Therefore their van der Waals radius is measured. The rationale here is based on the fact that

noble gases have very low chemical reactivity

and their measured atomic radii are non-bonded. An explanation lies in the electronic configuration of noble gases.

Which halogen has the smallest atomic radius?

Does S or O have a larger atomic radius?

Consequently

for the neutral atoms, S would be larger than O

. For the sulfide ion, reinforcing this effect is the large, excess 2- charge that greatly increases the radius of S2- as compared with the neutral S atom.