0
What generally happens to the first ionization energy of the element's within a period as the atomic number of the element's increases?
Wiki User
∙ 12y ago
Ar P Al Na K In general the ionisation energy (this answer refers to first ionisation energy, although most of the principles mentioned here apply to all ionisation energies) increases as one moves across the period, this is due to an increasing nuclear charge and decreasing atomic radius (recall that F=(kq1q2)/r2 ). However there are exceptions to this, notably, on moving from group II to group III we see that ionisation energy decreases, like wise on moving from group V to group VI. The first of these decreases is a result of the additional electron occupying the p orbital (and therefore experiencing a lesser effective nuclear charge). The second decrease (which is less marked) is due to the additional electron being "placed" into an orbital already occupied by another electron (an electron pair is formed), these electrons have the same charge and therefore repel each other, as they are in the same orbital the repulsion is particularly strong, therefore the effective nuclear charge is less and first ionisation energy is lower.
I hope this answer is acceptable, for more information see the Wikipedia article on electronic configuration.
Wiki User
∙ 15y ago
Wiki User
∙ 12y agoFirst ionization energy increases moving from left to right across a period, as the effective nuclear charge experienced by the electrons increased (due to poorer shielding).
Add your answer:
Earn +20 pts
When you go down the periodic table what happens to the ionization energy and why?
As you go across a period, ionization energy tends to increase. The reason for this is that as you move across a period, the outer shell of the atom becomes more complete. Consequently, there is a larger "Z" effect (attraction between the valence electrons and the nucleus) which leads to an increased difficulty in removing electrons. It is important to note that while this trend is generally valid, there are certain exceptions.
What happens to ionization energy as atomic Number increases within a group?
and i thought answers could answer my question, this proofs that they're wrong
What happens to ionization energy when atomic number increases or decreases in a period?
Ionization energy of an element is the energy required to ionize the element or in other words to eject a number of electrons from the most outer shell. For the first ionization energy it is the energy needed to eject 1 electron. Any ionisation energy increases across a period of the periodic table. This is due to the increased nuclear force attracting an electron to the nucleus because there are more protons as you go across. This force requires more energy to overcome and so the IE increases.
What happens when ionization energy change when moving down a group of elements?
the ionization energy is increased because of electronegativity when we move down the group the electronegativity is decrees who hold all electrons hardly to gather that's why the electrons loose easily and become an ion.
What happens to ionization energy as you move across a period?
Because energy is required to remove an electron from a neutral atom, it increases up and right. It increases up a group and to the right a period because in small atoms, electrons are closer to the nucleus were the attraction is stronger. So these are harder to remove. But in larger atoms, electrons are further from the nucleus and are easier to remove. I learned this in my Chemistry class this year. Hope this helps anyone.
What happens to the first ionization energy of the elements as a period is crossed?
Moving from left to right across a period, the first ionization energy increases because it becomes increasingly difficult to remove an electron.
What happens to first ionization energy within groups and periods?
it increases. the nuclear charge also increases
What happens to first ionization energy within groups and across periods?
it increases. the nuclear charge also increases
What happens to first ionization energy within groups across periods?
it increases. the nuclear charge also increases
What happens to your weight when you grow?
It generally increases.
When you go down the periodic table what happens to the ionization energy and why?
As you go across a period, ionization energy tends to increase. The reason for this is that as you move across a period, the outer shell of the atom becomes more complete. Consequently, there is a larger "Z" effect (attraction between the valence electrons and the nucleus) which leads to an increased difficulty in removing electrons. It is important to note that while this trend is generally valid, there are certain exceptions.
What happens to ionization energy as atomic Number increases within a group?
and i thought answers could answer my question, this proofs that they're wrong
What happens to solubility of a substance when their is rise in temperature?
Generally, as temperature increases, solubility increases. There are a few cases where the opposite happens, though.
What happens to the elements masses from left to right on the periodic table?
increases
What happens to ionization energy when atomic number increases or decreases in a period?
Ionization energy of an element is the energy required to ionize the element or in other words to eject a number of electrons from the most outer shell. For the first ionization energy it is the energy needed to eject 1 electron. Any ionisation energy increases across a period of the periodic table. This is due to the increased nuclear force attracting an electron to the nucleus because there are more protons as you go across. This force requires more energy to overcome and so the IE increases.
What happens to the first ionisation energy of the elements when a period is crossed?
Generally, the first ionization energy tends to increase as you move across a period from left to right. This is because the effective nuclear charge increases due to the addition of protons in the nucleus, which requires more energy to remove an electron. However, there can be some exceptions to this trend, especially for elements that have filled or half-filled subshells, which offer additional stability and require more energy to remove an electron.
What happens to the atomic radii of the elements as a group is descended?
As we descend down the group, the atomic radii increases. This is because the number of shells increases.
