Why the atomic size of inert gas is comparatively bigger than Group 17 element of the same period?

Noble gases have bigger atomic size than halogens because van de Waals radii are bigger than covalent radii.

Is size of inert gases larger than halogens?

Size of atoms of inert gases are smaller than those of the preceding halogens.

Why are the atomic size of group 18 elements larger than that of group 17 elements?

Across the period in the periodic table, atomic size decreases up to halogens(group-17 elements) but increases in noble gases(group-18 elements). This is because in case of inert or noble gases all the orbitals are completely filled and hence inter electronic repulsions are maximum.

Why do noble gases have larger atomic size than the elements in the same period?

Noble gasses have comparatively large atomic sizes because they have vander waals’ radii only which are expected to have larger magnitude where as other memebers of a period have either covalent or metallic radii which are less in magnitude.

Why inert gases have bigger atomic size?

Now, the actual reason of that why noble gases have comparatively large atomic sizes is because in case of inert or noble gases all the orbitals are completely filled means they have s2p6 configuration and hence inter electronic repulsions are maximum resulting they do not form molecules, Moreover in case of noble …

Why inert gas has largest size in period?

The atomic radius decreases along the period but the inert gases have the maximum radius in a period because of the increase in the Van der Waals radii in case of the inert gases. Since, the Van der Waals radii are larger than the covalent radii, the inert gases have largest atomic radii in the respective periods.

Why the size of the atom of an inert gas is bigger than that of the preceding halogen atom?

Explanation: This is because of the inter-electronic repulsion in the noble gases’ atoms. They have their octet complete, and hence the repulsion creates a wobbling force, due to which the size of the atom increases. This makes the size of the atoms of noble gases larger than their preceding halogens.

Why does the size of an element decrease across a period?

Across a period, effective nuclear charge increases as electron shielding remains constant. A higher effective nuclear charge causes greater attractions to the electrons, pulling the electron cloud closer to the nucleus which results in a smaller atomic radius.

Why atoms with large atomic radii and low ionisation potential are more metallic in nature?

Metals are electropositive in nature i.e. they can lose one or more electrons easily. Atoms with large atomic radii and low ionisation potential can easily lose one or more electrons as the nuclear pull on the outer electrons is less. As such these atoms are more metallic in nature.

Which of the following atom has largest size?

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.

How the atomic size vary in a group and across a period explain with suitable example?

Across the period from left to right there is a decrease in atomic size with increase in nuclear charge of the element. Atomic size increases down the group because of the addition of extra shells. So, as we move from group 1 to group 18 the size of the atom will decrease due to increased effective nuclear charge.

Why is the atomic radii of inert gas greater?

In case of inert or noble gases, the shells are completely filled with electrons and they are stable. So the electrons tend to be away from each other to minimise this repuksion, leading to an increased atomic size of the noble gases.

Why is the atomic size of noble gases larger than other elements?

Thus as, Vanderwaal’s radius is greater than covalent radius, the atomic size of noble gases is larger than other elements of same period. Let’s keep it simple.

Why is atomic size expressed in terms of VanderWaal’s radius?

Moreover in case of inert gases, the atomic size is expressed in terms of Vanderwaal’s radius because, noble gases do not form covalent bonds while other form covalent bonds and hence their atomic radii is expressed in covalent radius. Generally atomic size decreases while moving from left to right in the periodic table.

Why does the size of atoms increase as we move from halogens?

The size of atoms abruptly increases as we move from halogens to inert gases. Because the Interatomic electronic force in inert gases is more as compared to the halogens completely filled orbitals since the atomic size is expressed in terms of Van Der Waals radius.

Why are noble gas radii not accurate to understand how big atoms?

Because the Interatomic electronic force in inert gases is more as compared to the halogens completely filled orbitals since the atomic size is expressed in terms of Van Der Waals radius. The noble gas atoms look bigger, even though they are not. Therefore, noble gas radiiare not accurate to understand how big noble gas atoms really are.

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