The final electron of a P block element enters one of the three p-orbitals of the shell in which it is found. There are six groups of p-block elements since a p-subshell has three degenerate p-orbitals, each of which may hold two electrons.
Because of their tendency to lose an electron, P block elements are lustrous and typically strong conductors of electricity and heat. In a P-block element like gallium, you may find some astonishing characteristics of elements. It’s a metal that melts in your palm. Because silicon is a key component of glass, it is also one of the most significant metalloids in the p-block group.
Table of Contents
Phosphine
Phosphine is a phosphorus hydride with the formula PH3. Phosphine is a hazardous gas that is inflammable. It is commonly made in enterprises and labs due to its important industrial applications.
Phosphine may be found in human blood, urine, and saliva in nature.
Structure and Formula of Phosphine
Phosphine has a trigonal pyramidal structure. The lone pair of electrons present on phosphorus causes the molecule’s symmetry to alter. sp3 hybridization occurs in phosphorus. Three bound pairs and one lone pair of electrons are present. The angle of the H–P–H bond is 93.5o, while the length of the P–H bond is 1.42 pm.
Preparation of Phosphine
Hydrolysis of metal phosphides with calcium phosphide- Metal phosphides react with water or HCl to produce phosphine.
Ca3P2+6H2O→2PH3+3Ca(OH)2
Ca3P2+6HCl→2PH3+3CaCl2
From phosphorus acid- Pure phosphine is formed via the breakdown of H3PO3.
4H3PO3→3H3PO4+PH3
Preparation from Phosphorus- Heating white phosphorus in a concentrated NaOH solution in an inert CO2 environment produces PH3.
P4+3NaOH+3H2OPH3+3NaH2PO2
Purification of Phosphine
Pure phosphine is a non-flammable substance. Due to the presence of P2H4 or P4 vapours, it becomes combustible. Phosphine is refined by absorbing it in HI and converting it to PH4l. When you combine this with potassium hydroxide, you get phosphine.
PH4I+KOH→PH3+KI+H2O
Physical Properties of Phosphine
It’s a colourless gas that’s extremely dangerous.
As previously stated, phosphorus in its pure form is non-flammable. It is, nevertheless, combustible due to the presence of P4 vapour. When phosphorus comes into touch with oxidising substances like HNO3, chlorine, or bromine vapours, it can catch fire. It can catch fire even if just a little amount or traces of these oxidising chemicals are present.
It has a distinct rotten fish odour to it.
It’s just slightly soluble in water.
It has a boiling point of –87.7∘ Celsius.
Chemical Properties of Phosphine
Phosphine, like ammonia, is a Lewis base. When it reacts with HI, HBr, and HCl, it produces phosphonium compounds.
PH3+Hl→PH4l
PH3+HBr→PH4Br
PH3+HCl→PH4Cl
Combustibility- When phosphorus is burned, it produces phosphorus pentoxide and water.
2PH3+4O2→P2O5+3H2O
PH3+4Cl2→PCl5+3HCl
Under normal circumstances, it will not ignite. It explodes with flame when heated, releasing phosphoric acid.
When exposed to oxidising substances such as HNO3, Cl2 and Br2, it explodes dramatically.
PH3 in water decomposes in the presence of light to produce red P and H2O.
PH3(H2O)→P(red)+H2O
Copper phosphide and mercuric phosphide are generated when phosphine is absorbed in copper sulphate or mercuric chloride.
3CuSO4+2PH3→Cu3P2+3H2SO4
3HgCl2+2PH3→Hg3P2+6HCl
Uses of Phosphine
Phosphine is a chemical that is used to make metallic phosphides.
Holme’s signal and Smokescreens contain phosphorus.
Holme’s signal:
The fact that phosphine spontaneously combusts makes it a likely candidate for use in Holme’s signal. When ships require assistance, calcium carbide and calcium phosphide-filled containers are pierced and tossed into the water. Acetylene and phosphine gases are produced as a result of the interaction with water. These gases emit a signal when they burn in the air.
Smoke screen:
When calcium phosphide is soaked in water, it creates a considerable amount of phosphine, resulting in a smoke screen. During the conflict, this was employed to hide the troops from the enemy.
In rodent and insect control formulations, phosphine fumigants are utilised.
Sample Questions (FAQS)
Question 1: What are the properties of phosphine?
Answer
Phosphine is a colourless, very toxic gas.
It has a distinctive rotten-fish odour.
It has a low water solubility.
Question 2: What are the uses of phosphine?
Answer
Phosphine is employed in the smoke screen, Holme’s signal, and insecticides and rodenticides as a fumigant.
Question 3: What is the structure of phosphine?
Answer
With a lone pair of electrons on P, the structure is trigonal bipyramidal. Three bound pairs and one lone pair of electrons are present. The angle of the connection is 93.5 degrees. The length of the P–H bond is 1.42 Armstrong.
Question 4: How is phosphine gas prepared in the laboratory?
Answer
White phosphorus is burned with a strong NaOH solution in a CO2 inert environment to produce phosphine in the laboratory.
P4+3NaOH+3H2O→PH3+3NaH2PO2
Question 5: How to purify phosphine?
Answer
Phosphine is refined by absorbing impurities in HI, yielding PH4l, which is then treated with potassium hydroxide to get phosphine.
PH4l+KOH→KI+H2O+PH3
Question 6: What is Phosphine?
Answer
Phosphine has the formula PH3 and is a phosphorus hydride. Phosphine is a volatile and dangerous gas. Because of its vital industrial applications, it is routinely manufactured in businesses and laboratories.
In nature, phosphine may be found in human blood, urine, and saliva.
Neeraj Anand, Param Anand
Er. Neeraj K.Anand is a freelance mentor and writer who specializes in Engineering & Science subjects. Neeraj Anand received a B.Tech degree in Electronics and Communication Engineering from N.I.T Warangal & M.Tech Post Graduation from IETE, New Delhi. He has over 30 years of teaching experience and serves as the Head of Department of ANAND CLASSES. He concentrated all his energy and experiences in academics and subsequently grew up as one of the best mentors in the country for students aspiring for success in competitive examinations.
In parallel, he started a Technical Publication "ANAND TECHNICAL PUBLISHERS" in 2002 and Educational Newspaper "NATIONAL EDUCATION NEWS" in 2014 at Jalandhar. Now he is a Director of leading publication "ANAND TECHNICAL PUBLISHERS", "ANAND CLASSES" and "NATIONAL EDUCATION NEWS".
He has published more than hundred books in the field of Physics, Mathematics, Computers and Information Technology. Besides this he has written many books to help students prepare for IIT-JEE and AIPMT entrance exams. He is an executive member of the IEEE (Institute of Electrical & Electronics Engineers. USA) and honorary member of many Indian scientific societies such as Institution of Electronics & Telecommunication Engineers, Aeronautical Society of India, Bioinformatics Institute of India, Institution of Engineers. He has got award from American Biographical Institute Board of International Research in the year 2005.
CBSE Class 11 Chemistry Syllabus is a vast which needs a clear understanding of the concepts and topics. Knowing CBSE Class 11 Chemistry syllabus helps students to understand the course structure of Chemistry.
Unit-wise CBSE Class 11 Syllabus for Chemistry
Below is a list of detailed information on each unit for Class 11 Students.
UNIT I – Some Basic Concepts of Chemistry
General Introduction: Importance and scope of Chemistry.
Nature of matter, laws of chemical combination, Dalton’s atomic theory: concept of elements, atoms and molecules.
Atomic and molecular masses, mole concept and molar mass, percentage composition, empirical and molecular formula, chemical reactions, stoichiometry and calculations based on stoichiometry.
UNIT II – Structure of Atom
Discovery of Electron, Proton and Neutron, atomic number, isotopes and isobars. Thomson’s model and its limitations. Rutherford’s model and its limitations, Bohr’s model and its limitations, concept of shells and subshells, dual nature of matter and light, de Broglie’s relationship, Heisenberg uncertainty principle, concept of orbitals, quantum numbers, shapes of s, p and d orbitals, rules for filling electrons in orbitals – Aufbau principle, Pauli’s exclusion principle and Hund’s rule, electronic configuration of atoms, stability of half-filled and completely filled orbitals.
UNIT III – Classification of Elements and Periodicity in Properties
Significance of classification, brief history of the development of periodic table, modern periodic law and the present form of periodic table, periodic trends in properties of elements -atomic radii, ionic radii, inert gas radii, Ionization enthalpy, electron gain enthalpy, electronegativity, valency. Nomenclature of elements with atomic number greater than 100.
UNIT IV – Chemical Bonding and Molecular Structure
Valence electrons, ionic bond, covalent bond, bond parameters, Lewis structure, polar character of covalent bond, covalent character of ionic bond, valence bond theory, resonance, geometry of covalent molecules, VSEPR theory, concept of hybridization, involving s, p and d orbitals and shapes of some simple molecules, molecular orbital theory of homonuclear diatomic molecules(qualitative idea only), Hydrogen bond.
UNIT V – Chemical Thermodynamics
Concepts of System and types of systems, surroundings, work, heat, energy, extensive and intensive properties, state functions. First law of thermodynamics – internal energy and enthalpy, measurement of U and H, Hess’s law of constant heat summation, enthalpy of bond dissociation, combustion, formation, atomization, sublimation, phase transition, ionization, solution and dilution. Second law of Thermodynamics (brief introduction) Introduction of entropy as a state function, Gibb’s energy change for spontaneous and nonspontaneous processes. Third law of thermodynamics (brief introduction).
UNIT VI – Equilibrium
Equilibrium in physical and chemical processes, dynamic nature of equilibrium, law of mass action, equilibrium constant, factors affecting equilibrium – Le Chatelier’s principle, ionic equilibrium- ionization of acids and bases, strong and weak electrolytes, degree of ionization, ionization of poly basic acids, acid strength, concept of pH, hydrolysis of salts (elementary idea), buffer solution, Henderson Equation, solubility product, common ion effect (with illustrative examples).
UNIT VII – Redox Reactions
Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reactions, in terms of loss and gain of electrons and change in oxidation number, applications of redox reactions.
UNIT VIII – Organic Chemistry: Some basic Principles and Techniques
General introduction, classification and IUPAC nomenclature of organic compounds. Electronic displacements in a covalent bond: inductive effect, electromeric effect, resonance and hyper conjugation. Homolytic and heterolytic fission of a covalent bond: free radicals, carbocations, carbanions, electrophiles and nucleophiles, types of organic reactions.
UNIT IX – Hydrocarbons
Classification of Hydrocarbons Aliphatic Hydrocarbons: Alkanes – Nomenclature, isomerism, conformation (ethane only), physical properties, chemical reactions. Alkenes – Nomenclature, structure of double bond (ethene), geometrical isomerism, physical properties, methods of preparation, chemical reactions: addition of hydrogen, halogen, water, hydrogen halides (Markovnikov’s addition and peroxide effect), ozonolysis, oxidation, mechanism of electrophilic addition. Alkynes – Nomenclature, structure of triple bond (ethyne), physical properties, methods of preparation, chemical reactions: acidic character of alkynes, addition reaction of – hydrogen, halogens, hydrogen halides and water.
Aromatic Hydrocarbons:
Introduction, IUPAC nomenclature, benzene: resonance, aromaticity, chemical properties: mechanism of electrophilic substitution. Nitration, sulphonation, halogenation, Friedel Craft’s alkylation and acylation, directive influence of functional group in monosubstituted benzene. Carcinogenicity and toxicity.
To know the CBSE Syllabus for all the classes from 1 to 12, visit the Syllabus page of CBSE. Meanwhile, to get the Practical Syllabus of Class 11 Chemistry, read on to find out more about the syllabus and related information in this page.
CBSE Class 11 Chemistry Practical Syllabus with Marking Scheme
In Chemistry subject, practical also plays a vital role in improving their academic scores in the subject. The overall weightage of Chemistry practical mentioned in the CBSE Class 11 Chemistry syllabus is 30 marks. So, students must try their best to score well in practicals along with theory. It will help in increasing their overall academic score.
CBSE Class 11 Chemistry Practical Syllabus
The experiments will be conducted under the supervision of subject teacher. CBSE Chemistry Practicals is for 30 marks. This contribute to the overall practical marks for the subject.
The table below consists of evaluation scheme of practical exams.
Evaluation Scheme
Marks
Volumetric Analysis
08
Salt Analysis
08
Content Based Experiment
06
Project Work
04
Class record and viva
04
Total
30
CBSE Syllabus for Class 11 Chemistry Practical
Micro-chemical methods are available for several of the practical experiments. Wherever possible such techniques should be used.
A. Basic Laboratory Techniques 1. Cutting glass tube and glass rod 2. Bending a glass tube 3. Drawing out a glass jet 4. Boring a cork
B. Characterization and Purification of Chemical Substances 1. Determination of melting point of an organic compound. 2. Determination of boiling point of an organic compound. 3. Crystallization of impure sample of any one of the following: Alum, Copper Sulphate, Benzoic Acid.
C. Experiments based on pH
1. Any one of the following experiments:
Determination of pH of some solutions obtained from fruit juices, solution of known and varied concentrations of acids, bases and salts using pH paper or universal indicator.
Comparing the pH of solutions of strong and weak acids of same concentration.
Study the pH change in the titration of a strong base using universal indicator.
2. Study the pH change by common-ion in case of weak acids and weak bases.
D. Chemical Equilibrium One of the following experiments:
1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either of the ions. 2. Study the shift in equilibrium between [Co(H2O)6] 2+ and chloride ions by changing the concentration of either of the ions.
E. Quantitative Estimation i. Using a mechanical balance/electronic balance. ii. Preparation of standard solution of Oxalic acid. iii. Determination of strength of a given solution of Sodium hydroxide by titrating it against standard solution of Oxalic acid. iv. Preparation of standard solution of Sodium carbonate. v. Determination of strength of a given solution of hydrochloric acid by titrating it against standard Sodium Carbonatesolution.
F. Qualitative Analysis 1) Determination of one anion and one cation in a given salt Cations‐ Pb2+, Cu2+, As3+, Al3+, Fe3+, Mn2+, Ni2+, Zn2+, Co2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4+ Anions – (CO3)2‐ , S2‐, NO2‐ , SO32‐, SO2‐ , NO ‐ , Cl‐ , Br‐, I‐, PO43‐ , C2O2‐ ,CH3COO‐ (Note: Insoluble salts excluded)
2) Detection of ‐ Nitrogen, Sulphur, Chlorine in organic compounds.
G) PROJECTS Scientific investigations involving laboratory testing and collecting information from other sources.
A few suggested projects are as follows:
Checking the bacterial contamination in drinking water by testing sulphide ion
Study of the methods of purification of water.
Testing the hardness, presence of Iron, Fluoride, Chloride, etc., depending upon the regional variation in drinking water and study of causes of presence of these ions above permissible limit (if any).
Investigation of the foaming capacity of different washing soaps and the effect of addition of Sodium carbonate on it.
Study the acidity of different samples of tea leaves.
Determination of the rate of evaporation of different liquids Study the effect of acids and bases on the tensile strength of fibres.
Study of acidity of fruit and vegetable juices.
Note: Any other investigatory project, which involves about 10 periods of work, can be chosen with theapproval of the teacher.
Practical Examination for Visually Impaired Students of Class 11
Below is a list of practicals for the visually impaired students.
A. List of apparatus for identification for assessment in practicals (All experiments) Beaker, tripod stand, wire gauze, glass rod, funnel, filter paper, Bunsen burner, test tube, test tube stand, dropper, test tube holder, ignition tube, china dish, tongs, standard flask, pipette, burette, conical flask, clamp stand, dropper, wash bottle • Odour detection in qualitative analysis • Procedure/Setup of the apparatus
B. List of Experiments A. Characterization and Purification of Chemical Substances 1. Crystallization of an impure sample of any one of the following: copper sulphate, benzoic acid B. Experiments based on pH 1. Determination of pH of some solutions obtained from fruit juices, solutions of known and varied concentrations of acids, bases and salts using pH paper 2. Comparing the pH of solutions of strong and weak acids of same concentration.
C. Chemical Equilibrium 1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of eitherions. 2. Study the shift in equilibrium between [Co(H2O)6]2+ and chloride ions by changing the concentration of either of the ions.
D. Quantitative estimation 1. Preparation of standard solution of oxalic acid. 2. Determination of molarity of a given solution of sodium hydroxide by titrating it against standard solution of oxalic acid.
E. Qualitative Analysis 1. Determination of one anion and one cation in a given salt 2. Cations – NH+4 Anions – (CO3)2-, S2-, (SO3)2-, Cl-, CH3COO- (Note: insoluble salts excluded) 3. Detection of Nitrogen in the given organic compound. 4. Detection of Halogen in the given organic compound.
Note: The above practicals may be carried out in an experiential manner rather than recording observations.
We hope students must have found this information on CBSE Syllabus useful for their studying Chemistry. Learn Maths & Science in interactive and fun loving ways with ANAND CLASSES (A School Of Competitions) App/Tablet.
Frequently Asked Questions on CBSE Class 11 Chemistry Syllabus
Q1
How many units are in the CBSE Class 11 Chemistry Syllabus?
There are 9 units in the CBSE Class 11 Chemistry Syllabus. Students can access various study materials for the chapters mentioned in this article for free at ANAND CLASSES (A School Of Competitions).
Q2
What is the total marks for practicals examination as per the CBSE Class 11 Chemistry Syllabus?
The total marks for the practicals as per the CBSE Class 11 Chemistry Syllabus is 30. It includes volumetric analysis, content-based experiment, salt analysis, class record, project work and viva.
Q3
Which chapter carries more weightage as per the CBSE Syllabus for Class 11 Chemistry?
The organic chemistry chapter carries more weightage as per the CBSE Syllabus for Class 11 Chemistry.
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