Describe the trends in electronegativity in the periodic table?

Answer 1

Electronegativity increases across a period , this is because the Atomic radius of elements decrease due to the nuclear charge increasing.Decending a group electronegativity decreases because atomic radius increases due to electrons moving into new main energy levels (spdf), so the most elecronegative element is fluorine Hope that helps ! x

If you didn't understand this, I am deeply sorry.

Answer 2

v Trend-wise, as one moves from left to right across a period in the Periodic Table, the electronegativity increases due to the stronger attraction that the atoms obtain as the nuclear charge increases. Moving down a group, the electronegativity decreases due to the longer distance between the nucleus and the valence electron shell, thereby decreasing the attraction, making the atom have less of an attraction for electrons or protons

Answer 3

Electronegativity is a measure of an atom's "pull" on electrons. It is affected by the distance from the nucleus, electron-electron charge repulsion, and the effective nuclear charge acting on the electron.

First, electronegativity is higher the closer an atom's valence electron ring is to the nucleus (distance), so is the highest in the upper right corner of the table, with Flourine being the highest (4.0). (In case you forgot, as you go down a group, atomic radius increases, and as you go across a period (left-to-right), atomic radius decreases because there are more protons pulling the electrons in)

Second, electron-electron charge repulsion has little effect on the electronegativity of an atom. It mainly is cited for the electron affinity of an atom, so I won't mention it here.

Lastly, the effective nuclear charge (Zeff) acting on the outermost electron affects electronegativity. Flourine has 9 total electrons and 4 in-between (aka 'screening') electrons, so has a Zeff of 5 (9-4=5). As you move left across a period, Zeff decreases, but it stays the same going down a group (in that case, distance is the main factor)

Answer 4

Electronegativity generally increases moving from left to right across a period and decreases moving down a group in the periodic table. This is because the effective nuclear charge of an atom increases across a period due to more protons in the nucleus, causing atoms to attract electrons more strongly. Within a group, the effective nuclear charge remains relatively constant, leading to a decrease in electronegativity down the group.

Answer 5

Electronegativity increases across a period (left to right) and decreases down a group (up to down)

Answer 6

increases left to right along a
period

decreases on descending a group.

Answer 7

Down a group, electronegativity of the elements decreases. Across a period, electronegativity of the elements increases.

Answer 8

Electronegativity increases across a period (left to right).