Free PDF download of Class 12 Chemistry revision notes & short key-notes for Chapter 7 - The p-Block Elements to score high marks in exams, prepared by expert Chemistry teachers from latest edition of CBSE(NCERT) books. Chapter 8 - The d and f Block Elements. Previous Year Question. periodic table are called p-block elements. 2. General electronic configuration of p-block elements: The p- block elements are characterized by the ns2np After studying this unit, you will be able to. • appreciate the general trends in the chemistry of p-block elements;. • describe the trends in physical and chemical.
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In Class XI, you have learnt that the p-block elements are placed in groups 13 to 18 of the periodic table. Their valence shell electronic configuration is ns2np1–6. p block elements notes, p block elements, p block elements pdf, p block elements questions, p block elements ppt, p block element pdf, the p. 9_ p-block fernlowlitiltsi.ml - Read online for free. periodic table are called p-block elements. In p-block elements last incoming electron enters p-orbitals., Group.
Hint: Can be explained on the basis of sp3 hybridisation in NH3 and only s-p bonding , between hydrogen and other elements of the group. In all these cases, the central atom is sp3 hybridized. On moving down from N to Sb, the electronegativity of the central atom goes on decreasing.
This is because of the force of repulsion between the adjacent bond pairs goes on decreasing and the bond angles keep on decreasing from NH3 to SbH3. Thus, bond angles are in the order: 7. Nitrogen does not contains d-orbitals. But NH3 is much more basic than BiH3. Since the atomic size of N is much smaller than that of Bi, therefore, electron density on N-atom is much higher than that on Bi-atom. Thus, the tendency of N in NH3 to donate its lone pair of electrons is much more in comparison to tendency of Bi in BiH3.
Hence, NH3 is more basic than BiH3. It prefers to form P — P single bonds and hence it exists as tetrahedral P4 molecule.
Structure of white and red phosphorus are given below: 7. The extent of catenation depends upon the strength of the element — element bond. Thus, nitrogen shows less catenation properties than phosphorus. On heating, H3 P04 undergoes self — oxidation reduction, i. It can act as oxidizing agent by itself undergoing reduction. Thus, the minimum oxidation state of these elements should be — 2.
Other element being more electropositive than O and S, do not show negative oxidation state. Thus, on the basis of maximum and minimum oxidation states, these elements are justified to be placed in the same group 16 of the periodic table.
Thus, on the basis of hydride formation, these elements are justified to be placed in the same group 16 of the Periodic Table. As a result, oxygen exists as diatomic O2 molecules.
Therefore, O2 is a gas at room temperature. Due to its bigger size and lower electronegativity, sulphur does not form pn-pn multiple bonds.
It prefers to form S — S single bonds. S — S single bond is stronger then O-O single bond.
Thus, sulphur has higher tendency for catenation than oxygen. Due to bigger size, the force of attraction holding the Sg molecules together are much stronger which cannot be overcome by collisions of molecules at room temperature.
Therefore, sulphur is solid at room temperature. Let us consider the reaction of oxygen with monopositve metal, we can have two compounds.
Chapter 3 - Electrochemistry. Chapter 4 - Chemical Kinetics. Chapter 5 - Surface Chemistry. Chapter 8 - The d and f Block Elements. Chapter 9 - Coordination Compounds. Chapter 10 - Haloalkanes and Haloarenes. Chapter 11 - Alcohols, Phenols and Ethers.
Chapter 12 - Aldehydes, Ketones and Carboxylic Acids. Chapter 13 - Amines. Chapter 14 - Biomolecules. Chapter 15 - Polymers. Chapter 16 - Chemistry in Everyday life.
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