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?
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.
What else can I help you with?
What happens to ionization energy as atomic Number increases within a group?
Ionization energy generally decreases as atomic number increases within a group. This is because the distance between the outermost electron and the nucleus increases, resulting in weaker attraction and lower energy required to remove the electron.
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.
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 the group 1 elements as you go down the table?
As you go down Group 1 in the periodic table, the reactivity of the elements increases due to the decrease in ionization energy and increase in atomic size. The metals become more reactive with water and air as you move down the group.
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 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 ionization energy as atomic Number increases within a group?
Ionization energy generally decreases as atomic number increases within a group. This is because the distance between the outermost electron and the nucleus increases, resulting in weaker attraction and lower energy required to remove the electron.
What happens to your weight when you grow?
It generally 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 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
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 the group 1 elements as you go down the table?
As you go down Group 1 in the periodic table, the reactivity of the elements increases due to the decrease in ionization energy and increase in atomic size. The metals become more reactive with water and air as you move down the group.
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.
