<span>A.the elements that make up the compound
Tis the answer.</span>
Answer:
Electron affinity increases when moving left to right of the period.
Explanation:
Electron affinity is the amount of energy released when an isolated gaseous atom accepts electron to form the corresponding anion.
Trend of electron affinity across the period:-
- Across the period, the electron affinity increases as there is an increase in effective nuclear charge.
- Due to this, there is more force of attraction between the nucleus and the valence electrons when moving left to right in a period.
- Thus, more amount of energy is released when an electron is being gained in the neutral atom to form anion.
- Thus, electron affinity increases when moving left to right of the period.
Thus,
Al : -44 kJ/mol
Si : -120 kJ/mol
P : -74 kJ/mol
S : -200.4 kJ/mol
Cl : -384.7 kJ/mol
Al, Si, P, S, Cl are the members of third period and thus, left to right, the electron affinities of the elements increases as can be seen from the literature values.
A.
In a solid there is the least amount of room in between each particle and they are organized.
B. Is a liquid
C. I think it’s plasma but ik it is not a solid
D. Gas
Answer:
B.) their electrons are assigned to the s and p orbitals only
Explanation:
Once you get to the fourth row on the periodic table, the transition metals are introduced. The transition metals are located in the d-block and their electrons fill up d orbitals. When an element in the p-block (the right side of the table) is in one of these rows, the d-block has to fill up first.
