Question

Arrange the following elements in the increasing order of their metallic character $\mathrm{Mg},\mathrm{Ca},\mathrm{K},\mathrm{Ge},\mathrm{Ga}$

Answer 1

Trend of metallic character:

• Metallic character decreases across a period on moving from left to right. in the periodic table.
• This occurs as a result of an atom's increasing amount of electrons and protons as it moves from left to right in a period.
• Due to the increased nuclear force on the electrons, as a result, losing electrons becomes difficult.
• It increases on moving down in the group in the periodic table.
• One moving down the group, atomic radius increases, making things easier to lose electrons.
• The element that have the most metallic character is Francium$\left(\mathrm{Fr}\right)$.
• The other elements that are metallic in nature are Sodium $\left(\mathrm{Na}\right)$ and Copper $\left(\mathrm{Cu}\right)$.

Order of metallic character

• The left side of the periodic table is where the majority of metallic or electropositive elements are located.
• Gallium $\left(\mathrm{Ga}\right)$ and germanium $\left(\mathrm{Ge}\right)$ belong to the $p-$block, while potassium $\left(\mathrm{K}\right)$, magnesium $\left(\mathrm{Mg}\right)$, and calcium $\left(\mathrm{Ca}\right)$ are part of the $s-$block.
• Compared to $s-$block elements, $p-$block elements are less metallic.
• Due to its position in group $13$ whereas germanium is a member of group $14$, gallium is more metallic in germanium.
• Since potassium is an alkali metal, it will be more metallic than magnesium and calcium.
• Calcium will be more metallic than magnesium since it belongs to group $4\text{'}$s period $4$, whereas magnesium belongs to group$2$'s period $3$.
• The increasing order of the metallic character is:

$\mathrm{Ge}<\mathrm{Ga}<\mathrm{Mg}<\mathrm{Ca}<\mathrm{K}$