Question

1.A monatomic ion with a charge of -1 has an electronic configuration of 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶.

This ion is a(n) _______cationanion.

What is the chemical symbol of the noble gas this ion is isoelectronic with? .

What is the formula of the ion? .

2.A monatomic ion with a charge of +1 has an electronic configuration of 1s²2s²2p⁶.

This ion is a(n) _______cationanion.

What is the chemical symbol of the noble gas this ion is isoelectronic with? .

What is the formula of the ion?

3.Arrange the following ions in order of increasing ionic radius:

oxide ion, sodium ion, fluoride ion, aluminum ion

4.Arrange the following ions in order of increasing ionic radius:

telluride ion, iodide ion, barium ion, cesium ion

5.Using only the periodic table arrange the following elements in order of increasing ionization energy:

radon, argon, helium, xenon

6.Using only the periodic table arrange the following elements in order of increasing ionization energy:

oxygen, fluorine, boron, lithium

Answer 1

1.The ion is an anion.since -1charge of the ion indicates that the element gains an extra electron.The ion which gain electrons are anions.

The total number

of electrons in the given ion is 54. The noble gas isoelectronic with this ion is Xe (Xenon).

The formula of the given ion is I^{-1.(Iodide ion)}

2.The ion with +1charge means the element loses one electron and forms an ion.such ions are cations.

The total number of electrons in the ion is 10. So the noble gas iso electronic with the given ion is Ne (Neon).

The formula of the given ion is F^-1

3 In the increasing order of ionic radius the given ions can be written as

Aluminium ion,sodium ion,fluoride ion,oxide ion.

Ionic radius is defined as the radius of ions.In the formation of a cation electrons are removed from the atom and the number of positive charge increases and hence the nuclear attraction force also.this results in the reduction of atomic radius.In anions electrons are added to the element and nuclear attraction force reduces and results in increase of ionic radius.

4.barium ion,cesium ion,iodide ion,telluride ion.

5.The increasing order of ionisation energy of given element is as

Radon,Xenon,Argon,Helium.

In a group ionisation energy (the energy required to remove the most loosely bound electron) decreases from top to bottom as the size of the atom increases with increase in atomic number and hence the nuclear attraction on the outermost electron is less.

6.The increasing order of ionisation energy of the given elemens is as

Lithium,Boron,Oxygen,Fluorine.

Along a period ionisation energy increases as there is no increase in atomic size with increase in atomic number.the electrons are added to the same shells.The increase in atomic number results in increase in nuclear attraction over outermost electrons and increase in ionisation energy.