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Because energy is required to remove an electron from a neutral atom, it increases up and right. It increases up a group and to the right a period because in small atoms, electrons are closer to the nucleus were the attraction is stronger. So these are harder to remove. But in larger atoms, electrons are further from the nucleus and are easier to remove.
I learned this in my Chemistry class this year. Hope this helps anyone.
Wiki User
∙ 11y ago
Wiki User
∙ 13y agoWhile moving from left to right (across a period) the ionization energy increases.
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What is is the trend across a period?
what is the reason for ionization energy across a period
What is the general trend of ionization energy as you go across the periodic table?
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.
What has the highest first ionization energy phosphorous calcium sodium or aluminum?
Phosphorus. Across the period, first ionization energy increases.
How does Ionization Energy behave along the Periodic Table?
Ionization energy increases as we go across a period. Its value decreases as we go down a group.
What trend in ionization energy occurs going across a period on the periodic table and why?
The ionisation energy increases across a period. Across a period, nuclear charge increases. The tendency to loose electron decreases.
What is is the trend across a period?
what is the reason for ionization energy across a period
What happens to the first ionization energy of the elements as a period is crossed?
Moving from left to right across a period, the first ionization energy increases because it becomes increasingly difficult to remove an electron.
How does ionization energy of elements in the same period change?
Ionization energy increases as you go across a period, but as you go down a group it decreases.
What is the general trend of ionization energy as you go across the periodic table?
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.
Which element in the fifth period has the highest ionization energy?
xenon increases from left to right across periods (first ionization energy)
What has the highest first ionization energy phosphorous calcium sodium or aluminum?
Phosphorus. Across the period, first ionization energy increases.
Is it ionization energy is a periodic property?
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).
What is the general trend in ionization energy?
increases from left to right across a period.
Moving across a period on the periodic table from left to right?
ionization energy
What trend in ionization energy occurs across a period on the periodic table and why?
The ionisation energy increases across a period. Across a period, nuclear charge increases. The tendency to loose electron decreases.
Which elements has the highest ionization energy?
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.
How does Ionization Energy behave along the Periodic Table?
Ionization energy increases as we go across a period. Its value decreases as we go down a group.
