in a period size decreases from left to right and hence electrons are more tightly held to the nucleus. so electron gain enthalpy increases across a period .
down the period size increases and thus in general electron gain enthalpy decreses .
Both, electronegativity and ionisation potential, will increase across (from left to right) a period and will decrease down a group.
Due the addition of shell
xenon increases from left to right across periods (first ionization energy)
When moving left to right across the PT the ionization energy increases. As you go down, the ionization energy, decreases.
Two things happen when you move from right to left. First, the number of valence electrons increases from one to eight. Secondly, the number of protons increases from three to ten. There is also the transition from alkali metal to alkaline earth metal to metalloid to nonmetal to halogen to noble gas.
increase from left to right across a period.
ionization energy
xenon increases from left to right across periods (first ionization energy)
When moving left to right across the PT the ionization energy increases. As you go down, the ionization energy, decreases.
Two things happen when you move from right to left. First, the number of valence electrons increases from one to eight. Secondly, the number of protons increases from three to ten. There is also the transition from alkali metal to alkaline earth metal to metalloid to nonmetal to halogen to noble gas.
increase from left to right across a period.
increases from left to right across a period.
ionization energy
Across a period, first ionization energy increases. However, when going down a group, first ionization energy generally decreases. As you go down a group, atoms hove more total electrons so they don't really care that much about their outermost ones.
increases from left to right across a period.
It's carbon. The trend for 1st ionization energy is that it increases as you move left-to-right across a period. As you move in that direction across period 2, ionization energy increases, and since carbon is the most to the right, it has the highest 1st I.E.
As you travel to the right, it increases
First ionization energy increase
Helium (He) has the highest ionization energy, then Neon (Ne) Ionization energy increases as you go across a period from left to right. Ionization energy decreases as you go down a group. Therefore, elements in the upper right of the periodic table have the highest ionization energy.