How does ionization energy down a group relate to trend in atomic radius as atomic number increases down a group?

Answer 1

ionization energies (IE) have to do with things called ions. Ions are atoms which have gained or lost electrons. The ionization energy is the amount of energy it takes to detach one electron from a neutral atom. Some elements actually have several ionization energies. When this is the case, we refer to them as the "first ionization energy" or 'I', "second ionization energy" or 'I2', and so on. Notice that the energy variable follows Ii where i is the orbital from which the electron is lost. Ionization is endothermic meaning that the atom or molecule increases its internal energy (takes energy from an outside source).

Answer 2

• ''The ionization energy of an element is the minimum quantity of energy which is required to remove an electron from the outermost shell of its isolated gaseous atom in its ground state''

Trend in Periodic Table

Ionization energy decreases down the GROUP because the size of the atom increases down the group and also the nuclear attraction become less due to the increase in size so the electrons that are present in the outermost shell become loosely bonded so the minimum amount of energy is required to remove an electron from the outermost shell.

• Ionization energy decreases along the PERIOD because the electrons became more in the period due to the increase in atomic number more over the nuclear attraction become more along the period so it is not easy to remove an electron from the outermost shell so the ionization energy increases along the period.

Answer 3

Ionization energy (aka ionization potential), which is the amount of energy required to remove an electron from an atom (meaning to form a cation [positive charge]), increasesgoing across a period (row) and decreases going down a group or family (column).

Note: the above trends are for GROUP A Elements

Explanation: The reason it increases going across a period is because the number of outermost electrons increases going across the periods. The atomic radius (size of atom going from nucleus to outermost electron shell) decreases going across periods, meaning that as an electron is added to an element's outermost shell a proton is also added to the nucleus. This increases the attraction between the electrons and the protons in the nucleus, meaning there will be an increase in energy required to remove an electron. Plus, elements with more valence electrons are going to be more likely to attract electrons to gain a noble gas configuration (octet rule). (Think of the Group A numbers as representing the number of valence electrons a group number has). Thus, the energy required to remove those outermost electrons is going to increase.

The reason it decreases going down a family/group is because the atomic radius increases going down a family/group. This means that the distance between the outermost electrons and the atomic nucleus increases, meaning the attraction between those electrons and the radius is weaker. Thus, the energy required to remove those outermost electrons is going to decrease.

Atomic radius, or the size of an element going from the nucleus to the outermost shell, is going to decrease going across periods and will increase going down a group/family.

Explanation: The reason atomic radius decreasesgoing across periods is because as stated earlier in this answer, whenever an electron is added to an atom going across periods, a proton is also added. The attraction between the electrons in the outermost shell and the protons in the nucleus increases. Thus, the distance between the nucleus and the outermost electrons (atomic radius) decreases.

The reason atomic radius increases going down a group/family is because the number of valence electrons (and protons) increases as the atomic number increases. There will be new electron shells added going down a group/family because of this. Thus, the atomic radius increases going down a group/family.

Answer 4

Ionization energy decreases down a periodic table column as the atomic number increases, because as the atomic number increases, the valence electrons have more inner shells between the valence electrons and the atom's nucleus, thereby reducing the electrostatic attractive force between the nucleus and the valence electrons.

Answer 5

as atomic radius increases, ionisation energy decreases.

Answer 6

Atomic radius is inversely proportional to first ionization energy

As Atomic radius INCREASE, Ionization energy DECREASE

Answer 7

Ionization energy increases from left to right across a period, and decreases down a group.

Answer 8

== ==