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.
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
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)
Electronegativity increases across a period (left to right) and decreases down a group (up to down)
increases left to right along a
period
decreases on descending a group.
Down a group, electronegativity of the elements decreases. Across a period, electronegativity of the elements increases.
Electronegativity increases across a period (left to right).
Electronegativity increases from left to right.
From going left-right in a period, the electronegativity increases. By going up-down in a group, the electronegativity decreases. (those 2 are what they are looking for)
On the periodic table there is no such order of first and second as asked in the question.
Electronegativity increases as you move up and to the right. (apex) <3 kw
Electronegativity increases across (left to right) the periodic table and decreases on going down.
Electronegativity increases from left to right.
from above to down negetivity decreeses
From going left-right in a period, the electronegativity increases. By going up-down in a group, the electronegativity decreases. (those 2 are what they are looking for)
Electronegativity is not found on the Periodic Table of the Elements.
On the Periodic Table of elements, electronegativity increases as you move left to right across a period.
On the periodic table there is no such order of first and second as asked in the question.
Periodic table of elements provides us a lot of information about element's intrinsic properties. We can get the atomic weight of an element by looking at the periodic table. Trends about the electronegativity and atomic size can also be computed.
Electronegativity increases as you move up and to the right. (apex) <3 kw
Electronegativity increases across (left to right) the periodic table and decreases on going down.
Fluorine
electronegativity
Their metallic properties increase and their atomic radii increase.This can be checked with the Reference Table S with the atomic radii and metallic properties. Easy, right?