What are the trends in the modern periodic table?
THE TRENDS IN MODERN PERIODIC ARE STATED BELOW;
Elements show periodicity because of their valence shell configuration. All elements showing periodicity in properties have the same number of electrons in the last or valence shell. The properties that will be discussed here are:
- Atomic radius
- Ionisation potential
- Electron affinity
- Electronegativity
- Metallic character
Atomic Radius: The atomic radius is usually considered as the distance from the centre of the nucleus to the outermost shell i.e., to a point where the electron density is effectively zero.
Across the period i.e., from left to right: Atomic radius decreases
Down the group i.e., from top to bottom: Atomic radius increases
Reason: Across the period, the effective nuclear charge increases. This is due to the fact that the number of electrons increase (in the same subshell), increasing the number of protons in the nucleus. This pulls the valence shell of electrons in an atom towards itself, thus decreasing the atomic radius. But as we move down the group, the number of orbits keeps on increasing along with the number of protons. The space required to accommodate the extra orbits takes prevalence and therefore the atomic size increases.
The given animation explains the change in atomic size as we move down the group.
Ionisation Potential: It is the energy required to remove one mole of electrons from the valence shell of one mole of isolated gaseous atoms. Across the period i.e., from left to right: Ionisation potential increases
Down the group i.e., from top to bottom: Ionisation potential decreases
Reason: Across the period, the effective nuclear charge increases. This causes the atomic radius to decrease, thus getting the valence shell closer to the nucleus. This makes it difficult to remove electrons. But as we move down the group, the number of orbits keeps on increasing along with the number of electrons. The distance from the nucleus coupled with the interference of the electron between the nucleus and the valence shell renders the valence electrons weakly bound to the nucleus.
Electronegativity: The tendency of an atom to attract a bonding pair of electron towards itself when combined in a compound is called electronegativity.
Across the period i.e., from left to right: Electronegativity increases
Down the group i.e., from top to bottom: Electronegativity decreases
Reason: Across the period, the effective nuclear charge increases, thus decreasing the atomic radius. This favours the increase in electronegativity of elements across the period. But as we move down the group, the number of orbits keeps on increasing and therefore the atomic size increases and the electronegativity decreases.
Metallic character: It is defined as the tendency of an atom to lose electrons.
Across the period i.e., from left to right: Metallic character decreases
Down the group i.e., from top to bottom: Metallic character increases
Reason:Across the period, the effective nuclear charge increases, thus decreasing its atomic radius. This favours the increase of electronegativity and therefore the tendency to lose electrons is low. This accounts for the decrease in the metallic character along a period. But as we move down the group, the number of orbits keeps on increasing and therefore the atomic size increases. This means that the electronegativity decreases. This enhances the loss of electrons and therefore the metallic character increases down a group.
THE TRENDS IN MODERN PERIODIC ARE STATED BELOW;
Elements show periodicity because of their valence shell configuration. All elements showing periodicity in properties have the same number of electrons in the last or valence shell. The properties that will be discussed here are:
- Atomic radius
- Ionisation potential
- Electron affinity
- Electronegativity
- Metallic character
Atomic Radius: The atomic radius is usually considered as the distance from the centre of the nucleus to the outermost shell i.e., to a point where the electron density is effectively zero.
Across the period i.e., from left to right: Atomic radius decreases
Down the group i.e., from top to bottom: Atomic radius increases
Reason: Across the period, the effective nuclear charge increases. This is due to the fact that the number of electrons increase (in the same subshell), increasing the number of protons in the nucleus. This pulls the valence shell of electrons in an atom towards itself, thus decreasing the atomic radius. But as we move down the group, the number of orbits keeps on increasing along with the number of protons. The space required to accommodate the extra orbits takes prevalence and therefore the atomic size increases.
The given animation explains the change in atomic size as we move down the group.
Ionisation Potential: It is the energy required to remove one mole of electrons from the valence shell of one mole of isolated gaseous atoms.Across the period i.e., from left to right: Ionisation potential increases
Down the group i.e., from top to bottom: Ionisation potential decreases
Reason: Across the period, the effective nuclear charge increases. This causes the atomic radius to decrease, thus getting the valence shell closer to the nucleus. This makes it difficult to remove electrons. But as we move down the group, the number of orbits keeps on increasing along with the number of electrons. The distance from the nucleus coupled with the interference of the electron between the nucleus and the valence shell renders the valence electrons weakly bound to the nucleus.
Electronegativity: The tendency of an atom to attract a bonding pair of electron towards itself when combined in a compound is called electronegativity.
Across the period i.e., from left to right: Electronegativity increases
Down the group i.e., from top to bottom: Electronegativity decreases
Reason: Across the period, the effective nuclear charge increases, thus decreasing the atomic radius. This favours the increase in electronegativity of elements across the period. But as we move down the group, the number of orbits keeps on increasing and therefore the atomic size increases and the electronegativity decreases.
Metallic character: It is defined as the tendency of an atom to lose electrons.
Across the period i.e., from left to right: Metallic character decreases
Down the group i.e., from top to bottom: Metallic character increases
Reason:Across the period, the effective nuclear charge increases, thus decreasing its atomic radius. This favours the increase of electronegativity and therefore the tendency to lose electrons is low. This accounts for the decrease in the metallic character along a period. But as we move down the group, the number of orbits keeps on increasing and therefore the atomic size increases. This means that the electronegativity decreases. This enhances the loss of electrons and therefore the metallic character increases down a group.
