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What trend it does the first ionization energy follow going across the periodic table?
The first ionization energy tends to increase across a period from left to right on the periodic table. This is due to the increasing nuclear charge and decreasing atomic radius, which leads to a stronger attraction between the electrons and the nucleus.
What trend the first ionization energy follow in the periodic table?
It decreases when going down a group.
What trend in ionization energy occurs going across a period on the periodic table and why?
Ionization energy generally increases across a period from left to right on the periodic table. This trend occurs because as you move across a period, the number of protons in the nucleus increases, resulting in a greater nuclear charge. This stronger attraction between the nucleus and the outer electrons requires more energy to remove an electron, thus increasing the ionization energy.
What are the exceptions in ionization energy within the periodic table?
Exceptions in ionization energy within the periodic table occur when there is a significant decrease in ionization energy going from one element to the next. This can happen when there is a half-filled or fully-filled subshell, which results in increased stability and lower ionization energy. Examples include the group 3 elements (B, Al, Ga, In, Tl) and the group 6 elements (Cr, Mo, W).
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 are trends in ionzation energy?
from left to right in a row on the periodic table the ionization energy increases. going down a column the ionization energy decreases.
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.
How the electronegativity trend related to the first ionization energy trend?
Electronegativity and first ionization energy both increase going up the Periodic Table.
How is the electronegative trend relate to the first ionization energy trend?
Electronegativity and first ionization energy both increase going up the Periodic Table.
What trend does the first ionization energy follow in the periodic?
It decreases when going down a group.
What trends does the first 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 trend does the first ionization energy follow going down the periodic?
The first ionization energy decreases because the outermost electron is farther from the nucleus. Apex
What trend it does the first ionization energy follow going across the periodic table?
The first ionization energy tends to increase across a period from left to right on the periodic table. This is due to the increasing nuclear charge and decreasing atomic radius, which leads to a stronger attraction between the electrons and the nucleus.
What trend the first ionization energy follow in the periodic table?
It decreases when going down a group.
What trend in ionization energy occurs going across a period on the periodic table and why?
Ionization energy generally increases across a period from left to right on the periodic table. This trend occurs because as you move across a period, the number of protons in the nucleus increases, resulting in a greater nuclear charge. This stronger attraction between the nucleus and the outer electrons requires more energy to remove an electron, thus increasing the ionization energy.
How does the first ionization energy change going down and across the periodic table?
As you move down a group on the periodic table, the first ionization energy generally decreases due to the increasing atomic size and shielding effect of inner electrons. Across a period, the first ionization energy generally increases because the effective nuclear charge increases, making it harder to remove an electron.
What trend does the first ionization energy follow going down periodic table?
The first ionization energy decreases because the outermost electron is farther from the nucleus. Apex
