# data[].attributes.body
the metallic radius increases down the group because each element has more electron shells than the last

# data[].attributes.body
Increasing

The additional electron shells increase the atomic size, even as the nuclear charge rises

# data[].attributes.body
Increases down the group because more electron shells are added, increasing the distance of outer electrons from the nucleus.

# data[].attributes.body
from be-ra there’s an increase of electron shells hence increasing the metallic radius aswell

# data[].attributes.body
1. ﻿﻿﻿Nuclear Charge: More protons strengthen atomic attractions.

2. ﻿﻿﻿Electron Number: Additional electrons enhance forces within atoms.

3. ﻿﻿﻿Metal Hardness: Stronger, more rigid bonds require higher energy to break.

# data[].attributes.body
Because as you move down the group each element has an extra electron shell compared to the one above it thus making it larger in terms of size.

# data[].attributes.body
the metallic radii increases because of added electron shells, resulting in greater shielding and reduced effective nuclear charge. this allows the outer electrons to be farther from the nucleus

# data[].attributes.body
It generally increases due to atomic mass increase. Ra exceptionally high density results from its large atomic mass and efficient body-centered cubic structure

# data[].attributes.body
Additional energy levels are added, expanding the atomic radius and inner electron shield outer electron from nuclear attraction

# data[].attributes.body
Trend: decreases down the group (with some exceptions).

Reason: Metallic bonds weaken as the atomic size increases, causing the delocalized electrons to be farther from the positively charged nuclei. Exceptions (e.g., Ca) are due to differences in crystal structures

# data[].attributes.body
The density increases due to increased atomic mass, relatively small in atomic radius, effective nuclear charge and additional electron configuration

# data[].attributes.body
Increasing down the group. Because their atomic mass increase more significantly than their atomic size, leading to a greater mass/unit volume.

# data[].attributes.body
Density increases down Group 2 because the atomic mass increases significantly while the increase in atomic volume is relatively smaller, leading to a higher mass-to-volume ratio.

# data[].attributes.body
The melting point decreases as you move down the group due to the weaker metallic bonds

# data[].attributes.body
As you go down group 2, the ionisation energy decreases because of the shielding or screen effect of the outer electrons from the nucleus and so the attraction is weaker and they are more easily removed

# data[].attributes.body
The IE decreases down the group due to its increasing atomic radius, which reduces the nuclear charge. The inner electrons also shield outer electrons ,weakening the attraction. Their valence configuration also facilitates electron removal

# data[].attributes.body
The ionisation energy is affected by the effective nuclear charge, the atomic radius, and the shielding effect of inner electrons

# data[].attributes.body
Larger atomic radius, weaker metallic bonding, electron density

# data[].attributes.body
The density decreases then increases due to the volume of the atom increasing as the elements get larger, but the mass increases more

# data[].attributes.body
The first energy of Group 2 elements decreases as you move down the group. This is because the outermost electrons are further from the nucleus and experience more shielding from the inner electron shell

# data[].attributes.body
The melting point increases when the forces holding the particles together, such as ionic bonds, covalent bonds, or intermolecular forces, are stronger. Stronger bonds require more energy (heat) to break.