Electronegativity is affected by: atomic number of the element, distance between the nucleus of an atom and the valence electrons or sometimes by the so-called "d-block contraction".
On the Periodic Table of elements, electronegativity increases as you move left to right across a period.
The trend for first ionization energy
The electronegativity increase across the period and down the group it itdecreases for non metals
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.
Electronegativity decreases across a period because the effective nuclear charge increases. This causes the attraction between the electrons and the nucleus to become stronger, making it harder for atoms to attract additional electrons and thus reducing electronegativity.
Yes, as you move from left to right across the period.
First ionization energy has a trend similar to that of electronegativity.
An increase in atomic number within a specific period corresponds to an increase in the number of protons in the nucleus of the atom. This leads to a higher positive charge, causing the outer electrons to be more strongly attracted to the nucleus. As a result, the atomic size tends to decrease across a period as atomic number increases.
Electronegativity increases as you move across a period in the periodic table because the number of protons in the nucleus increases, leading to a stronger attraction for electrons in the outer shell.
Electronegativity increases across a period because the effective nuclear charge, or the positive charge felt by the outer electrons, increases as you move from left to right across the periodic table. This stronger attraction between the nucleus and the outer electrons results in higher electronegativity values.
Electronegativity generally increases across a period from left to right due to an increase in effective nuclear charge, making it harder for atoms to release electrons. It tends to decrease down a group as the atomic size increases, leading to weaker attraction for valence electrons.
Ionization energy has a trend similar to electronegativity. Both properties generally increase across a period from left to right and decrease down a group in the periodic table. This is because both involve the attraction between electrons and the nucleus of an atom.