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Electronegativity decreases along a period. This is because atomic radius increases increases, hence nuclear charge decreases.
atomic radius decreases from bottom to top of the periodic table.
Yes. The atomic radius increases down the group. This is because number of shells increases down the group.
Down a group, the atomic radius increases as the number of shells or energy levels increases.
Along a period, nuclear charge increases. hence, atomic radius decreases.
Electronegativity decreases because the valence electrons are farther from the nucleus.
Electronegativity decreases along a period. This is because atomic radius increases increases, hence nuclear charge decreases.
As atomic radius increases, electronegativity generally decreases. This trend occurs because as the atomic radius increases, the distance between the nucleus and valence electrons increases, resulting in weaker attraction between the nucleus and outer electrons. Consequently, atoms with larger atomic radii tend to have lower electronegativities.
atomic radius decreases from bottom to top of the periodic table.
The atomic radius decreases from left to right and increases from top to bottom
The atomic radius decreases as the atomic number increases due to the fact that there is now a greater quantity of protons in the nucleus emitting greater intramolecular force, pulling the electrons closer towards it. This, thus, decreases the radius.
Yes. The atomic radius increases down the group. This is because number of shells increases down the group.
Electronegativity tends to increase across a period from left to right. This is because as you move across a period, the nuclear charge increases and the atomic radius decreases, leading to a stronger attraction for electrons by the nucleus.
Atomic radius
As you move down a column (group) in the periodic table, the electronegativity decreases, the ionization energy decreases, the electron affinity decreases, and the atomic radius increases.
Down a period the atomic radius increases as the number of shells (or energy levels) increases. Across a period the atomic radius decreases as the effective nuclear charge increases.
Electronegativity decreases as you go down a group in the periodic table. This is because as you move down a group, the atomic radius increases, leading to a decrease in the attraction between the nucleus and the outer electrons, resulting in lower electronegativity values.