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Why does rubidium not follow the general trend of ionization energy in its group?
I suppose that this trend is normal.
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.
How is the electronagativity trend related to the first ionization energy trend?
Electronegativity and first ionization energy both increase as you move up the periodic table
What other trend is similar to periodic trend for electronegativity?
The trend for first ionization energy
How is the electronegativity trend related to the first ionization energy level?
When electronegativity decrease the first ionization energy also decrease.
What is the general trend in ionization energy?
increases from left to right across a period.
Which property has a trend similar to that of electronegativity?
First ionization energy has a trend similar to that of electronegativity.
How does the electronegativity trend explain the first ionization energy trend?
The electronegativity trend and the first ionization energy trend both increase as you move from left to right across a period in the periodic table due to the increasing effective nuclear charge. Higher electronegativity indicates a stronger pull on electrons, making it harder to remove an electron, thus increasing the first ionization energy.
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
The periodic trend for electronegativity is similar to what trend?
Ionization energy would be similar.
Which diagram correctly depicts the general trend in first ionization energy?
The general trend in first ionization energy increases across a period from left to right on the periodic table, as the effective nuclear charge increases and electrons are held more tightly. Conversely, ionization energy decreases down a group, as additional electron shells are added, which increases the distance between the nucleus and the outermost electrons, making them easier to remove. Therefore, a diagram illustrating this trend would show a rising slope across periods and a downward slope down groups.
