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Arrange the elements in decreasing order of first ionization energy.
Rank from highest to lowest first ionization energy. To rank items as equivalent, overlap them.

In, Ge, Se, Cs

PART B:
Arrange the elements in order of decreasing first ionization energy. Rank from highest to lowest first ionization energy. To rank items as equivalent, overlap them.

element x (radius (pm): 110)
element y (radius (pm): 199)
element z (radius (pm): 257)

Respuesta :

Answer:

The decreasing order of first ionization energy: Se > Ge > In > Cs

The decreasing order of first ionization energy: x > y > z

Explanation:

Ionization energy refers to the energy needed to completely pull out an electron from the valence shell of a neutral gaseous atom.

First ionization energy is the energy involved in the removal of first valence electron.

In the periodic table, down the group, as atomic radius of elements increases, the ionization energy decreases

Whereas, across a period, as atomic radius of elements decreases, the ionization energy increases.

PART (A):

Position of the given elements in the periodic table:

Indium (In): Group 13, period 5

Germanium (Ge): Group 14, period 4

Selenium (Se): Group 16, period 4

Caesium (Cs): Group 1, period 6

Thus, the increasing order of atomic radius: Se < Ge < In < Cs

Therefore, the decreasing order of first ionization energy: Se > Ge > In > Cs

PART (B):

Given elements:

element x: radius = 110 pm

element y: radius = 199 pm

element z: radius = 257 pm

Thus, the increasing order of atomic radius: x < y < z

Therefore, the decreasing order of first ionization energy: x > y > z

adioabiola

Here, we are required to arrange elements in decreasing order of first ionization energy.

(a) Se > Ge > In > Cs

(b) element x > element y > element z

The ionization energy of an atom is simply defined as the amount of energy required to completely pull out an electron from the outermost shell of the atom.

  • The first ionization energy of an atom is the amount of energy required to completely remove the first valence electron.

  • The first ionization energy of an atom is inversely proportional to the atomic radius of the atom;

As such, the larger the atomic radius, the lower the first ionization energy and vice versa.

In the periodic table, the atomic radius of elements increases down a group and decreases across a period.

The position of the elements given in the periodic table is as follows;

  • Indium (In): Group 13, period 5

  • Germanium (Ge): Group 14, period 4

  • Selenium (Se): Group 16, period 4

  • Caesium (Cs): Group 1, period 6

(a) Ultimately, the arrangement of the elements in decreasing order of first ionization energy from highest to lowest is;

Se > Ge > In > Cs

(b) As we know, the first ionization energy of atoms decreases as there atomic radius increases and vice versa.

The elements and their atomic radius are as follows;

  • element x (radius (pm): 110)
  • element x (radius (pm): 110)element y (radius (pm): 199)
  • element x (radius (pm): 110)element y (radius (pm): 199)element z (radius (pm): 257)

Therefore, to rank the elements in order of decreasing first ionization energy; we have;

element x > element y > element z

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