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What are the metallic trends concerning electronegativity and ionization energy?
Electronegativity decrease going down in a group and increase from left to right; but this isn't a general rule.A similar situation is also with the ionization energy.
How does the first ionization energy change going down and across the periodic table?
In a group the first ionization energy decrease going down.In a period the first ionization energy increase from left to right.
Which is more reactive sodium or barium?
sodium because it's the first group and first group are the most
What is the Trend in first ionization energy across a period?
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.
Why does the second ionization energy of Group 1 Elements greater than the first ionization energy of Group 1 Elements?
It takes more energy to knock off two electrons
What is the trend ionization energy?
From left to right on the periodic table, ionization energy increases. From top to bottom in a column (group) the ionization energy decreases.
What are the metallic trends concerning electronegativity and ionization energy?
Electronegativity decrease going down in a group and increase from left to right; but this isn't a general rule.A similar situation is also with the ionization energy.
Which of the group IIIA (13) elements has the largest ionization energy?
The element with the highest first ionization energy in group 14 is carbon.
How does the first ionization energy change going down and across the periodic table?
In a group the first ionization energy decrease going down.In a period the first ionization energy increase from left to right.
Which is more reactive sodium or barium?
sodium because it's the first group and first group are the most
An atom has a first ionization energy of 496 kJmol and a second ionization energy of 4560 kJmol What group of the periodic table would the atom be in?
group 1
What is the Trend in first ionization energy across a period?
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.
Why does the second ionization energy of Group 1 Elements greater than the first ionization energy of Group 1 Elements?
It takes more energy to knock off two electrons
Elements that have the highest first ionization energy?
Helium (He) has the highest first ionization energy. Ionization energy increase as you go across the periodic table from left to right
What elements has the highest first ionization energy out of strontium magnesium beryllium calcium?
Beryllium will have the highest. Down a group ionization energy decreases.
What are the element within any giving periodic table would always have the lowest first ionization energy?
Francium in group 1 has the lowest first ionization energy.
In ionization energy how does the property varies within a group?
The ionization energy decrease moving down in a group.
