Increases on moving left to right
The tendency to lose electrons generally increases as you move from left to right across a period on the periodic table. This is because the elements on the left side have fewer electrons in their outer shell and are more likely to lose electrons to achieve a stable electron configuration.
Electronegativity is the tendency of an atom in a compound to attract electrons towards itself. It is a measure of an atom's ability to form bonds with other atoms by attracting shared electrons. Electronegativity values range from 0 to 4. Electronegativity increases from left to right across a period and decreases down a group on the periodic table.
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.
As you move across a period, elements have the same number of electron shells but different numbers of valence electrons. This leads to differences in reactivity and chemical properties across the period.
Why not?If two atoms have the same number of protons, they're the same element. Therefore, unless they're electrically charged, they must have the same number of electrons as well. So the number of electrons in two different elements must be different if the atoms are electrically neutral.
The tendency to lose electrons generally increases as you move from left to right across a period on the periodic table. This is because the elements on the left side have fewer electrons in their outer shell and are more likely to lose electrons to achieve a stable electron configuration.
they get more electrons the farther right the get
as you move across a period, you are more and more likely to gain electrons
The number of valence electrons for the elements increases across a period, from 1 (group 1) to 8 (group 18).
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 the tendency of an atom in a compound to attract electrons towards itself. It is a measure of an atom's ability to form bonds with other atoms by attracting shared electrons. Electronegativity values range from 0 to 4. Electronegativity increases from left to right across a period and decreases down a group on the periodic table.
The ionisation energy increases across a period. Across a period, nuclear charge increases. The tendency to loose electron decreases.
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.
The number of valence electrons increases from left to right across a period.
The number of valence electrons for the elements increases across a period, from 1 (group 1) to 8 (group 18).
As you move across a period, elements have the same number of electron shells but different numbers of valence electrons. This leads to differences in reactivity and chemical properties across the period.