Ionization Energy&

Ionic Radii vs Atomic Radii

By: Santiago Velásquez

What is an ion?!An ion is a charged atom or molecule. It is

charged because the number of electrons do not equal the number of protons in the atom or molecule.

What is an ion?!An ion is a charged atom or molecule. It is

charged because the number of electrons do not equal the number of protons in the atom or molecule.

What is first ionization energy?

 Ionization is a process in which atoms lose or gain electrons and become ions.

What is first ionization energy?

 Ionization is a process in which atoms lose or gain electrons and become ions.

The first ionization energy is therefore a measure of the strength of the attraction between the outermost electrons and the nucleus.

What is first ionization energy?

 Ionization is a process in which atoms lose or gain electrons and become ions.

The first ionization energy is therefore a measure of the strength of the attraction between the outermost electrons and the nucleus.

1st, 2nd, and 3rd ionization energies

The symbol I1 stands for the first ionization energy and the symbol I2 stands for the second ionization energy

Each succeeding ionization energy is larger than the preceding energy. This means that I1<I2<I3<...<In will always be true.

Ionic Radii Atomic Radii

Atomic Radius (Radii)The boundaries of an atom are fuzzy, and an

atom’s radius can vary under different conditions.

To compare different atomic radii, they must be measured under specified conditions.

Atomic radius - one-half the distance between the nuclei of identical atoms that are bonded together.

Atomic Radii

Atomic Radii• Atoms tend to be smaller as you go from left to

right on the periodic table. • This is due to increasing positive charge in the

nucleus, pulling the electrons closer to the center.• Atoms tend to be larger down a group.

• This trend is due to the increasing size of the electron cloud as electrons fill up larger energy levels.

Atomic Radii

Ion Radius (Radii)Positive ions tend to be smaller than neutral

atoms. The larger the positive charge, the smaller the

ion. Again, this is due to increasing positive charge

in the nucleus, pulling the electrons closer to the center.

Ion Radii

Ion RadiiPositive ions tend to be smaller than neutral

atoms. The larger the positive charge, the smaller the

ion. Again, this is due to increasing positive charge

in the nucleus, pulling the electrons closer to the center.

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