0
Fluorine...
it has seven valence electrons and really wants to achieve noble gas configuration (8 out of 8 possible valance electrons). It already has seven and since it is so close to eight, it is very attached to them. It refuses to give them up easily. The more an element "wants" it's electrons the higher ionization energy it will have.
http://www.800mainstreet.com/4/0004-002-Periodic.html
Helium, as it has the highest ionization energy among the noble gases.
Krypton is the noble gas that has four energy levels.Also they are located on the side of the elment for an example Kryptons energy levels are 2,8,18,8.
Krypton is the noble gas that has four energy levels. Also they are located on the side of the elment for an example Kryptons energy levels are 2,8,18,8.
Add your answer:
Earn +20 pts
What element in family IA has the lowest ionization energy?
the lowest ionization energy in IA :hydrogen ,lithiun ,sodium and potassium
How Which element require the greatest amount of energy to remove an electron?
Core electrons. Probably the 1s level would require the most ionization energy to pull these electrons.
Does the first ionization energy increase or decrease from top to bottom for the noble gas family?
The first ionization energy decrease from top to bottom for the noble gas family.
Which family of the periodic table has the strongest tendency to lose electrons and why?
This is the alkali metals family; the ionization energy is lower for these chemical elements.
An atom of an element in family VIA will have what charge when it is ionized?
Ionization can have any number of causes, resulting in any number of ionization states ranging from ±1 to ±(atomic number) for any given atom. In the given context, however, I would assume the actual question intended is, "What is the preferential ionic state of ionically bonded atoms in the VIA periodic family?" The answer to this question is -2.
What element in family IA has the lowest ionization energy?
the lowest ionization energy in IA :hydrogen ,lithiun ,sodium and potassium
Which element has a lower first ionization energy than aluminum (Al)?
The element that has a lower first ionization energy than aluminum (Al) is magnesium (Mg). Magnesium is one period above aluminum on the periodic table, and as you move down a group or family, the ionization energy tends to decrease.
How Which element require the greatest amount of energy to remove an electron?
Core electrons. Probably the 1s level would require the most ionization energy to pull these electrons.
Does the first ionization energy increase or decrease from top to bottom for the noble gas family?
The first ionization energy decrease from top to bottom for the noble gas family.
What is the biggest element in the alkali family?
The biggest element in the alkali family is cesium. It has the largest atomic radius and is the most reactive alkali metal due to its large size and low ionization energy.
Which family of the periodic table has the strongest tendency to lose electrons and why?
This is the alkali metals family; the ionization energy is lower for these chemical elements.
An atom of an element in family VIA will have what charge when it is ionized?
Ionization can have any number of causes, resulting in any number of ionization states ranging from ±1 to ±(atomic number) for any given atom. In the given context, however, I would assume the actual question intended is, "What is the preferential ionic state of ionically bonded atoms in the VIA periodic family?" The answer to this question is -2.
What is an element with a single electron in its highest energy level is probably what type of metal?
An element with a single electron in its highest energy level is likely an alkali metal. Alkali metals like lithium, sodium, and potassium have one electron in their outer energy level, making them highly reactive and likely to form ionic bonds.
What element has 3 energy levels and belongs to the most unreactive group?
The element is 'argon' and belongs to noble gas family.
What exceptions are there in the increase of ionization energies across a period?
There is a slight decrease in ionization energy when moving from Group 2 to Group 13 due to the introduction of a new subshell (s to p transition), causing increased electron shielding. Additionally, there is a slight decrease in ionization energy when moving from Group 15 to Group 16 due to the stable half-filled p orbital that requires more energy to remove an electron.
Does the first ionization energy increase or decrease from top to bottom in periodic table for the alkali metal family?
The first ionization energy generally decreases from top to bottom in the alkali metal family. This is due to the increase in atomic size and the shielding effect from inner electrons, which makes it easier to remove the outermost electron.
What is the general trend in ionization energies of elements in the same chemical family?
The ionization energy generally decreases down a group in the periodic table within the same chemical family. This is because as you move down a group, the outermost electrons are located in higher energy levels, making them farther from the nucleus and thus easier to remove.
