The elements are barium and radium - atomic radius 215 pm.
Beryllium (Be) is the group 2 element with the smallest atomic radius. This is due to its higher nuclear charge relative to its size, which results in a stronger attraction between the nucleus and the electrons, pulling them closer. As you move down the group, atomic radii increase because additional electron shells are added, outweighing the increase in nuclear charge.
The element within period 2 with the greatest nuclear charge is neon. This is because neon has more protons in its nucleus compared to the other elements in period 2, giving it the highest nuclear charge.
There's no charge within the atom of each group since there is a same number of electrons (negatively charged) and protons ( positively charged). The charge does not change unless after ionic bonding. The atomic charge changes depending on the reaction.
In the ground state, an atom of each of the elements in Group 2 (the alkaline earth metals) has a different atomic radius due to increasing nuclear charge as you move down the group. This increased nuclear charge pulls the electron cloud closer to the nucleus, resulting in a larger atomic radius. Additionally, the presence of more electron shells as you go down the group contributes to this increase in size, despite the stronger nuclear attraction. Thus, while they all have similar chemical properties, their atomic sizes vary significantly.
the effective nuclear charge on barium is 2.
Beryllium (Be) is the group 2 element with the smallest atomic radius. This is due to its higher nuclear charge relative to its size, which results in a stronger attraction between the nucleus and the electrons, pulling them closer. As you move down the group, atomic radii increase because additional electron shells are added, outweighing the increase in nuclear charge.
1.5
The element within period 2 with the greatest nuclear charge is neon. This is because neon has more protons in its nucleus compared to the other elements in period 2, giving it the highest nuclear charge.
Group 1 and Group 2 metals have larger atomic radii and low effective nuclear charge, making it easier for them to lose electrons rather than gain them. This results in lower electronegativity values for these metals.
There's no charge within the atom of each group since there is a same number of electrons (negatively charged) and protons ( positively charged). The charge does not change unless after ionic bonding. The atomic charge changes depending on the reaction.
In the ground state, an atom of each of the elements in Group 2 (the alkaline earth metals) has a different atomic radius due to increasing nuclear charge as you move down the group. This increased nuclear charge pulls the electron cloud closer to the nucleus, resulting in a larger atomic radius. Additionally, the presence of more electron shells as you go down the group contributes to this increase in size, despite the stronger nuclear attraction. Thus, while they all have similar chemical properties, their atomic sizes vary significantly.
the effective nuclear charge on barium is 2.
The ionic charge of a group 1A, 2A, or 3A ion is determined by the number of electrons lost or gained to achieve a full valence shell. Group 1A ions lose 1 electron to attain a +1 charge, group 2A ions lose 2 electrons for a +2 charge, and group 3A ions lose 3 electrons for a +3 charge.
Sodiumis in group 1 and its cation is charge +1. Calcium is in group 2 and the cahrge on its cation is +2. etc.
+ve 2
The most common charge (or valency) is -2. But there are compounds formed by elements of group VIA with valency from -2 to +6
1: 1+ 2: 2+ 13: 3+ 14: 4+/- 15: 3- 16: 2- 17: 1- 18: Neutral Transition metals (elements between groups 2 and 13) are able to have varied charges that there is no real rule for.