because the more valence electrons a element has, the more it wants to become a noble gas. The pull is stronger because it is trying to get other electrons.
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.
Ionization energy increases as you go across a period, but as you go down a group it decreases.
The ionisation energy increases across a period. Across a period, nuclear charge increases. The tendency to loose electron decreases.
increases from left to right across a period.
The ionisation energy increases across a period. Across a period, nuclear charge increases. The tendency to loose electron decreases.
xenon increases from left to right across periods (first ionization energy)
Phosphorus. Across the period, first ionization energy increases.
increases.
increases from left to right across a period.
Ionization energy generally increases across a period as a result of a higher nuclear charge, however there are some exceptions such as Boron which has a lower ionization energy than Beryllium (because it is in a P orbital), and Oxygen which has a lower ionization energy than nitrogen (Because ionization decreases the electron electron repulsion in its orbitals).
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.
Ionization energy increases as we go across a period. Its value decreases as we go down a group.