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As one proceeds down the group 7A elements, the first ionization energy decreases. this means that the outermost electron is more readily removed as we go down a group.
Wiki User
∙ 9y ago
Wiki User
∙ 6y agoAs the atomic number increases within a group, the ionization energy decreases .
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What general statement can summarize the trend in the ionization energy when moving across a period of element?
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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.
What has the greatest first ionization energy Li Be B or C?
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.
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 trend does the ionization energy follow going across the periodic table?
The correct answer is: The ionization energy increases because there are more protons to pull on the electrons.
What is is the trend across a period?
what is the reason for ionization energy across a period
What is the general trend in ionization energy?
increases from left to right across a period.
What is the general trend in first ionization energy?
increases from left to right across a period.
What general statement can summarize the trend in the ionization energy when moving across a period of element?
123
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.
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 has the greatest first ionization energy Li Be B or C?
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.
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.
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 accounts for the general trend in the first ionuization energy of the elements within a period?
As you go from right to left in a period in the periodic table the ionization energy increases. While going from top to bottom in a group in the periodic table the ionization energy decreases .
What is a general rule you can use for the ionization energy trend on the periodic table?
The trend for ionization energy is:left to right across a period, it increases;top to bottom down a group, it decreases.It has to do with the amount of attraction the positively charged nucleus has on the number of electrons in the outer energy level and the distance between them.
What trend in ionization energy do you see as you go across a period row on the periodic table what causes this trend?
It is a trend in itself, it isn't caused by a trend.
