They increase from left to right.
Atomic size increases from top to bottom in a group due to increase in theshieldingeffect.As you go down the group shielding from core electrons increases (as more core electrons are added), therefore valence electrons experience weaker attraction forces from the nucleus and are located further away from it, resulting in an increase in size.If you move across a period the attraction between the nucleus and valence electrons increases because the number of protons and the number of valence electrons both go up whereas the number of core electrons stays the same (shielding decreases). In this case the size decreases.
The number of valence electrons increases from left to right across a period.
stays the same Well... that's not really true... the number of them stays the same, but several things happen to them. First off they are further from the nucleus. And they are further shielded by additional electrons between the valence and nucleus. This causes a looser association and tends to make the atom more volatile.
The number of valence electrons for the elements increases across a period, from 1 (group 1) to 8 (group 18).
the no. of electrons increses
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".
The number of valence electrons increases.
The number of valence electrons increases as you go across a period. For example in period 2 the number of valence electrons rises from 1 in Li up to 8 in neon.
Atomic size increases from top to bottom in a group due to increase in theshieldingeffect.As you go down the group shielding from core electrons increases (as more core electrons are added), therefore valence electrons experience weaker attraction forces from the nucleus and are located further away from it, resulting in an increase in size.If you move across a period the attraction between the nucleus and valence electrons increases because the number of protons and the number of valence electrons both go up whereas the number of core electrons stays the same (shielding decreases). In this case the size decreases.
The number of valence electrons increases from left to right across a period.
stays the same Well... that's not really true... the number of them stays the same, but several things happen to them. First off they are further from the nucleus. And they are further shielded by additional electrons between the valence and nucleus. This causes a looser association and tends to make the atom more volatile.
The number of valence electrons for the elements increases across a period, from 1 (group 1) to 8 (group 18).
They don't have the same number. that's what makes thme all different
The number of valence electrons for the elements increases across a period, from 1 (group 1) to 8 (group 18).
the no. of electrons increses
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.
Electron configuration is the arrangement of elements according to their increasing atomic numbers whiles period is the arrangement of elements according to the increasing number of valence electrons.