Why does electronegativity increase as you move left to right across a period?

Answer 1

As you move across a period from left to right, the number of protons increases, and the number of electrons increases in the valence shell. This makes the attraction between the electrons and protons stronger and stronger, and therefore the atomic radius of the atom decreases. This means that any atoms flying by with available weak bonded electrons will bond with this element because the distance between the valence shell and protons decrease making the attraction to the nucleus stronger for free electrons.

Answer 2

Because it becomes closer to Flourine. Flourine is most electronegative on Periodic Table.
It increases from left to right across a period as core charge increases because there is an increase in protons, which means increase in strength to attract more electrons to the valance shell.

And just extra info,

It decreases down a group because the atoms increase in atomic size, meaning there is more distance between the negative valence electrons and positive nucleus which weakens their attraction.

Answer 3

electronegativity is a measure of how tightly elements hold on to valence electrons in a covalent bond. (Nobel gases are excluded from this pattern).

before we can understand this it is important to note the pattern involving atomic radius. as we descend the periodic table the elements get bigger, as a result the valence electrons are farther away from the positive mass (protons in the nuclei) so there is less attractive force holding them. As we move left to right atoms generally have more valence electrons as we approach the Nobel gases (exclude transition metals for now). The octet configuration for the valence shell tells us that each atom strives for 8 valence electrons. If we look at the valence electrons of magnesium for example, we find 2 valence electrons on this element. it would be much easier for Mg to loss its electrons than hold onto six more. likewise if we look at a halogen (chlorine) it has 7 valence electrons and since it is very close to the octet, it holds tightly onto those electrons. If we put these patterns together we find that Florine is the most electronegitive and francium is the least.

Answer 4

Electronegativity increases moving across a period from left to right because the atoms in the same period have the same number of energy levels but the number of protons increase as you go from atom to atom across a period increasing the attraction between the nucleus and the outer energy level resulting in a greater ability for atoms to attract electrons to it.

Answer 5

It increases from left to right across a period as core charge increases because there is an increase in protons, which means increase in strength to attract more electrons to the valance shell.

And just extra info,

It decreases down a group because the atoms increase in atomic size, meaning there is more distance between the negative valence electrons and positive nucleus which weakens their attraction.

Answer 6

Electronegativity increases as you move left to right across a period because the effective nuclear charge—the positive charge experienced by an electron—increases. This stronger attractive force by the nucleus pulls the shared electrons closer to the more electronegative atom, leading to higher electronegativity values.

Answer 7

it increases because each row in the periodic table has to end with a noble gas, and a noble gas has to have atleast 8 elcectrons.

Answer 8

This is because the attraction of bonding electrons by an atom increases with nuclear charge(At.No.) and decrease of atomic radius.both these factors operate as we move to the right in period

Answer 9

Electronegativity increases along a period.As we move from left to right, it increases.