Question

Explain the diagonal relationship between Boron and Silicon. Use chemical equations, where possible. ​

Answer 1

Answer :-

$\rightarrow$ Due to small size and similar charge/mass ratio,boron differs from other group 13 members, but it resembles closely with silicon , the second elements of group 14 to exhibit diagonals relationship, Some important similarities between boron and silicon are given below ;

$\star$ Both boron and silicon are typically non metals , having high melting point, and boiling point with nearly same densities low atomic volumes and a bad conductor of current . However both are semiconductor.

$\star$ Both of them do not form cation and form only covalent compounds.

$\star$ Both exists in amorphous and crystalline state and exhibit allotropy.

$\\{\orange{\underline{\red{\underline{Additional\: information}}}}}$

The diagonal relationship between Boron and Silicon shows Anamolous behaviour in its group because of its small size and non availability of D oribital it resembles as silicon the second member of the next higher group.

(1) Formation of acids

$\rightarrow$ Boron and silicon forms weak acids as $\color{green}H_{3}BO_3$ and $\color{green}H_{4}SlO_{4}$

(2) Nature

$\rightarrow$ Both the elements are semiconductor.

(3) Cation/Anion

$\rightarrow$ Both silicon and boron do not form captions.

(4) Metals/ Non metals

$\rightarrow$ Both boron and silicon are non-metals.

(5) oxides formation

$\rightarrow$ Boron form boxides and silicon form silicides.

$\color{red}{3}$ mg + $\color{red}{2}$ B $\rightarrow$$Mg_{3}$$\rightarrow$ Magnesium boride.

2mg + Si $\rightarrow$ $Mg_{2}$Si $\rightarrow$ Magnesium silicide

Answer 2

Answer:

Because crossing and descending the periodic table have opposing effects, there is a diagonal relationship. It is primarily owing to the polarising power of ions.

Explanation: 

In the 2nd and 3rd periods of the periodic table (the first$20$elements), a diagonal relationship is believed to exist between certain pairs of diagonally adjacent elements.

• Because crossing and descending the periodic table have opposite effects, a diagonal relationship emerges. When crossing a period of the periodic table, the size of the atoms decreases, and when descending a group, the size of the atoms grows.
• Similarly, as the period progresses, the elements get more covalent, less reducing, and more electronegative, but as the group progresses, the elements become more ionic, basic, and less electronegative.
• As a result, the changes balance out whether descending a group or crossing by one element, and elements with identical characteristics and chemistry are frequently identified.
• Silicon and boron are both semiconductors. They produce acidic oxides when they are hydrolyzed in water.