Group 2 Physical Properties by Cahya Maula Shidiq

2025-01-14 07:49:05 UTC

the metallic radius increases down the group because each element has more electron shells than the last

2025-01-14 07:49:15 UTC

Increasing

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

dewa

2025-01-14 07:49:51 UTC

Increases down the group because more electron shells are added, increasing the distance of outer electrons from the nucleus.

2025-01-14 07:50:23 UTC

from be-ra there’s an increase of electron shells hence increasing the metallic radius aswell

Acintya

2025-01-14 07:50:38 UTC

Nuclear Charge: More protons strengthen atomic attractions.
Electron Number: Additional electrons enhance forces within atoms.
Metal Hardness: Stronger, more rigid bonds require higher energy to break.

Why Metallic Radii increases downward.

2025-01-14 07:50:50 UTC

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.

2025-01-14 07:50:54 UTC

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

Kayl

2025-01-14 07:51:01 UTC

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

ashahar

2025-01-14 07:51:14 UTC

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

Safira

2025-01-14 07:51:35 UTC

Additional energy levels are added, expanding the atomic radius and inner electron shield outer electron from nuclear attraction

2025-01-14 07:52:08 UTC

The density increases due to increased atomic mass, relatively small in atomic radius, effective nuclear charge and additional electron configuration

2025-01-14 07:52:24 UTC

Increasing down the group. Because their atomic mass increase more significantly than their atomic size, leading to a greater mass/unit volume.

Freya

2025-01-14 07:52:39 UTC

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.

Aqila

2025-01-14 07:52:52 UTC

The melting point decreases as you move down the group due to the weaker metallic bonds

dhiyandramail — 2025-01-14 07:52:53 UTC

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

2025-01-14 07:53:21 UTC

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

2025-01-14 07:53:31 UTC

The ionisation energy is affected by the effective nuclear charge, the atomic radius, and the shielding effect of inner electrons

Birru

2025-01-14 07:53:43 UTC

Larger atomic radius, weaker metallic bonding, electron density

Ryu

librarysc — 2025-01-14 07:54:27 UTC

The density decreases then increases due to the volume of the atom increasing as the elements get larger, but the mass increases more

2025-01-14 07:54:56 UTC

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

2025-01-14 07:56:54 UTC

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.