CBSE Class 12 Chemistry Questions and basic easy to learn concepts/ notes Database for chapter The p Block Elements. Based on CBSE and CCE guidelines. Download pdf of class 12 chemistry notes chapter 7 P – Block Elements made by expert teachers. These notes will clear all your doubt and help you to score. P - Block Elements Class 12 Notes is considered as one of the most important chapters to be studied for class 12 CBSE board examination. Download the PDFs.
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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. In Class XI, you have learnt that the p-block elements are placed Objectives. Diversity in chemistry is the hallmark of p–block elements manifested .. Page 12 . In p-block elements the last electron enters the outermost p orbital. As we know oxidation state shown by a p-block element is equal to the .. 2B N H +12H. →.
The students should practice these Questions to gain perfection which will help him to get more marks in CBSE examination. The preparation should be in a manner which helps the students to concentrate more in areas which carry more marks. Download File: The p Block Elements. Skip to main content. Assignments Assignments for Class 12 Chemistry with important questions and answers for all chapters in book for Class 12 Chemistry as per syllabus issued by
Chapter 2 - Solutions. 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. Previous Year Paper for Class 12 Maths. Previous Year Paper for Class 12 Physics. Previous Year Paper for Class 12 Chemistry. Previous Year Paper for Class 12 Biology. Previous Year Paper for Class 12 English. Previous Year Paper for Class 12 Hindi.
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Class 10th. Class 9th. Class 8th. Class 7th. Class 6th. Class 13th Droppers. State Board. Study Material. Previous Year Papers. Mock Tests. Sample Papers. Reference Book Solutions. Due to the presence —of triple bond betweep the two N-atoms, the bond dissociation energy is large As aresult of this N2 is inert and unreactive whereas, phosphorus exists as a tetratomic molecule, containg P — P single bond.
Due to the presence of single bond, the bond dissociation energy is weaker kJmol-1 than N a N triple bond As a result of this, phosphorus is much more reactive than nitrogen. Hydrides: All elements of group 15 form gaseous hydrides of the type MH3.
In all the hydrides the central atom is sp3 hybridized and their shape is pyramidal due to presence of lone pair of electrons. The molecules of other hydrides are not associated.
The ionic character of trihalides increases as we move down the group. Except NCl3 all the trihalides are hydrolysed by water.
This is due to the absence of d-orbitals in nitrogen. Bi cannot form BiX3 because of reluctance of 6s electrons of Bi to participate in bond formation.
M in MX5 is sp3 as hybridised and shape is trigonal pyramidal. The axial bonds in MX5 are weaker and longer, So MX5 are less stable and decompose on heating eg: Oxides: a Nitrogen forms a number of oxides. Nitrogen has an electronegativity value 3. Phosphorus have an electronegativity value Write the chemical equations of the reactions. In laboratory, nitrogen is prepared by heating an equimolar aqueous solution of ammonium chloride and sodium nitrite.
As a result of double decomposition reaction, ammonium nitrite is formed.
Ammonium nitrite is unstable and decompose to form nitrogen gas. On heating with dil HN03, copper gives copper nitrate and nitric oxide. Resonating structures of N02 are: 7. 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.