P block elements class 11 - Boron Family | One Shot Hindi | JEE CBSE NCERT NEET

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Timestamps:
0:00 Introduction
0:43 P-Block elements
2:02 Importance of p-block elements
3:21 Properties of p-block elements.
7:38 Periodic table Trends
8:27 Group-13 Boron Family
11:22 Group-13:Trends Physical properties
11:43 Boron Family:Electronic Configuration
14:15 Group 13 Trends:Atomic &Ionic radii
21:13 Group 13 Trends Density
22:58 Group 13 Trends: Melting & Boiling point
25:56 Group 13 Trends: Ionization Enthalpy
27:57 Group 13 Trends: Electronegativity
30:12 Group 13 Trends: Metallic character
30:44 Group 13 Trends: Reducing property
32:27 Boron family: Oxidation State
39:31 Boron family: Nature of Compounds
42:10 Group 13 Trends: Chemical properties
42:49 Group 13 Trends: Reaction with Air
48:45 Group 13 Trends: Reaction with acids
1:00:10 Group 13 Trends: reaction with Base
1:04:14 Group 13 Trends: reaction with halogens
1:07:35 Boron family: Aluminium Halides
1:08:34 P block: Diagonal relationship

There are six groups of p–block elements in the periodic table numbering from 13 to 18. Boron, carbon, nitrogen, oxygen, fluorine and helium head the groups. Their valence shell electronic configuration is ns2np1.Boron in available limited quantities. Aluminium is readily available on our planet. It is the third most abundant element available. P-block metals have classic metal characteristics: they are shiny, they are good conductors of heat and electricity, and they lose electrons easily. Generally, these metals have high melting points and readily react with nonmetals to form ionic compounds.While moving down the group, atomic radius of elements increases. In Boron family, Atomic radius of Ga is less than AI.This is due to the variation of inner core of electronic configuration. The ionisation enthalpy decreases from top to bottom, but, in case of, Boron family, there is an increase and decrease in ionisation energies from Al to Tl. Because d and f electrons have low shielding effect. Electronegativity decreases from B to Al and then it increases this is because of difference in atomic size of elements. The outer electronic configuration of group 13 elements in ns2np1. So,oxidation state is +3. Boron and Aluminium shows oxidation state of +3 whereas, other elements of the group shows oxidation state of +3 and +1. But+1 is most stable oxidation state. Boron family reacts with halogens to form trihalides. Boron does not react with air. At high temperature boron burns in air forming B2O3. Aluminium reacts with air and forms thin layer of oxide on its surface. It prevents further oxidation of Al2O3. At very high temperature they react with nitrogen forming nitride. Boron does not react with acids and alkalies
even at moderate temperature; but aluminium dissolves in mineral acids and aqueous alkalies and thus shows amphoteric character .

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