a) it generally increases
b) it does not change
c) it varies unpredictably
d) it generally decreases
ughhh i wish someone would answer this.....mr.lyon makes his exams study guides to long...
d
In a group the first ionization energy decrease going down.In a period the first ionization energy increase from left to right.
xenon increases from left to right across periods (first ionization energy)
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).
ionization energy
Moving from left to right across a period, the first ionization energy increases because it becomes increasingly difficult to remove an electron.
Ionization energy increases as you go across a period, but as you go down a group it decreases.
what is the reason for ionization energy across a period
In a group the first ionization energy decrease going down.In a period the first ionization energy increase from left to right.
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.
xenon increases from left to right across periods (first ionization energy)
Phosphorus. Across the period, first ionization energy increases.
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).
increases from left to right across a period.
ionization energy
Moving from left to right across a period, the first ionization energy increases because it becomes increasingly difficult to remove an electron.
The ionisation energy increases across a period. Across a period, nuclear charge increases. The tendency to loose electron decreases.
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.