Every matter has its own set of properties. Physical and chemical properties can be used to classify these properties. Physical properties are those that may be measured or observed without affecting the substance’s identity or composition. Physical properties include odor, color, density, and so on. Chemical properties are those in which the substance undergoes a chemical change. Chemical properties include acidity, basicity, reactivity, and so on. The physical and chemical properties of matter and their measurements are discussed in detail below.
What is Matter?
Any substance with mass and volume that takes up space is referred to be matter. Matter is defined as something with mass that takes up space. Matter makes up all physical structures, and the state or process of matter is an easily recognized property of matter. Solid, liquid, and gas are the three basic states of matter.
Everything in our universe is formed of matter. Substances and atoms are made up of microscopic particles of matter. These atoms make up the items we see and touch every day. The matter is defined as everything that has mass and fills space. The mass of an object determines how much matter it contains.
Physical Properties of Matter
Physical properties of matter are those which can be observed externally or can be measured:
The matter is made up of microscopic particles known as atoms, and they can be represented or interpreted as anything that occupies space. Both the mass and volume properties must be displayed.
The features that allow us to distinguish one substance from another are known as properties. A physical property is a characteristic of matter that is unrelated to its chemical makeup.
Density, colour, hardness, melting and boiling points and electrical conductivity are all physical properties.
Any property that can be measured, such as an object’s density, colour, mass, volume, length, malleability, melting point, hardness, odor, temperature, and so on, is referred to as a property of matter.
We frequently encounter fundamental physical quantities such as mass, length, time, and temperature.
Mass measurement is one of the most common techniques performed by chemists. This is crucial since it indicates the quantity of matter present.
The length, area, and volume of an object are all used to determine its size. The length of an object is one dimension, the area of the object is two dimensions, and the volume of the object is three dimensions of space.
Time is also an interesting measure since it allows us to estimate how long a process or chemical reaction will take.
Temperature is a significant physical quantity that indicates a body’s degree of hotness or coldness. Temperature fluctuations that occur during chemical reactions are of particular interest to chemists.
Chemical Properties of Matter
Chemical properties are properties that can only be measured or observed during the transformation of matter into a certain type of matter. These include reactivity, flammability, and the ability to rust. Reactivity is the tendency of matter to react chemically with other substances. Chemical qualities include flammability, toxicity, acidity, numerous types of reactivity, and heat of combustion. When it comes to differentiating compounds, chemical characteristics are particularly useful. When a substance is being transformed into another substance, only then the chemical qualities can only be observed.
Reactivity– Reactivity is the property of matter that allows it to mix chemically with other substances. Certain materials have high reactivity, whereas others have low reactivity. Even in the presence of water, potassium, for example, is exceedingly reactive. When a pea-sized chunk of potassium is mixed with a small amount of water, it explodes.
Acidity– It is a chemical attribute that describes a substance’s capacity to react with an acid. When certain metals react with different acids, they generate compounds. Acids and bases combine to form water, which neutralizes the acid.
Flammability– It is the property of a substance that allows it to burn. When matter burns, it reacts with oxygen to produce a variety of compounds. A flammable matter is anything that burns, such as wood.
Toxicity – The degree to which a chemical element or a mixture of chemicals can harm an organism is referred to as toxicity.
Thermal Properties of Matter
Thermal properties that are matter related are key to comprehend topics such as temperature and heat alterations. These properties include:
Heat Capacity: Heat capacity (C) is a measure of heat energy that system of a substance requires to increase its temperature by 1 degree Celsius or 1 Kelvin. It expresses the capacity of a thermal energy containing body to maintain its state.
Specific Heat: The specific heat (c) denotes the heat capacity of the substance for its unit mass. This is suggestive of the quantity of heat that has to be added to a certain mass of material to increase its temperature for one degree Celsius or one Kelvin.
Thermal Conductivity: Material efficiency for conduct heat is evaluated via thermal conductivity. Fast heat transferring is caused by high thermal conductivity, and the slower the heat transferring speed is maybe because of low thermal conductivity.
Phase Changes: Phase transformations take place in the form of transition from one state of matter to another—solid, liquid, gas—due to the temperature/pressure variations. This is realized by means of three types of changes, including melting (solid to liquid), boiling (liquid to gas), and condensation (gas to liquid).
Melting Point: The temperature of conversion of a solid substance into a liquid state.
Boiling Point: The process taking place when a liquid changes into a gas.
Evaporation: The transformation process which takes place when a liquid substance turns in a gas at temperatures lower than the boiling ones.
Condensation: When a gas gains energy in the form of heat, it moves into a liquid state.
Sublimation: This is the process in which the solid substance dissociates directly to a gas without going through the liquid state.
Intensive and Extensive Properties of Matter
The matter has either extensive or intensive physical and chemical properties. The amount of matter being weighed is proportional to the extensive properties, including mass and volume. The amount of matter present, for example, has no effect on density or color.
Intense properties of matter- An intensive property is a bulk property, meaning it is a local physical property of a system that is independent of its size or volume of material. The qualities of intensive matter are those that are unaffected by the amount of matter present. For example, pressure and temperature are both intense properties.
Extensive property of matter- An extensive property is a property that is reliant on the amount of matter in a sample. Mass and volume are two of the many extensive properties available. The vast property of a system is determined by its scale or the volume of materials in it. Extensive properties are those in which the value of a system’s property equals the sum of its parts’ values.
Physical and Chemical Changes
Physical Changes: These alterations regard both the states or appearances of matter as well as their inner chemical structure, but the chemical structure is untouched. Examples are such as conversion of state (melting, freezing) and morphing of shape and size (cutting, tearing).
Chemical Changes: The chemical changes, which are reactions, are about creating new substances with a different chemical structure from the grounds of which they come into existence. This may consist of combustions, oxidations, and decomposition reactions.
Expressing a Physical Quantity
A physical quantity’s value is always stated in two parts.
(i) The numerical value
(ii) The unit
For example, a box’s weight, can be stated as 6500 g or 6.5 kg. 6500 or 6.5 is a numerical quantity that conveys no significant information. As a result, every experimental value must be expressed in units.
The standard of reference adopted to measure any physical amount is specified as a unit.
Naturally, a simple unit system for giving numerical values to the observed or calculated quantities is required. Some fundamental units, such as mass, length, and time. These are known as fundamental units since they are independent units that cannot be deduced from any other unit. These units can be used to derive units for other quantities, which are referred to as derived units.
There are various unit systems to choose from. A study committee of the French Academy of Science established a system known as “the metric system” for the first time in 1791, which became popular in the scientific community around the world. The metric system’s core units are the grams for mass, the metre for length, and the litre for volume. In 1957, India adopted the metric system. The metric system is a decimal system in which physical quantity units are connected in powers of ten. A prefix affixed to the unit generally indicates the distinct powers.
SI Units of Physical Quantities
The International System of Units, known as SI units, has been widely adopted by scientists. The General of Weights and Measures adopted these units in 1960. SI units are abbreviations for Systeme Internationale, and the name originates from the French word. In the SI system, there are seven base units. All additional units can be derived from these base units, which correspond to seven important scientific quantities. The following table lists the seven basic SI units.
Physical Quantity
Symbol for quantity
Name of Unit
Symbol
Length
L
meter
m
Time
t
second
s
Mass
m
kilogram
kg
Temperature
T
kelvin
K
Luminous intensity
Iv
candela
cd
Electric current
I
ampere
A
Amount of substance
n
mole
mol
Despite the fact that the SI system’s temperature unit is Kelvin, the Celsius scale (0C) is still widely utilized in our daily lives. These two units are linked in the following way:
Temperature in Kelvin (K) = 0C +273.15
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FAQs on Properties of Matter
What is the significance of matter properties?
Scientists must comprehend the properties of matter. The three fundamental forms of matter are solid, liquid, and gas. Most matter can exist in any of these states, depending on its physical characteristics. Scientists work with a wide variety of materials in particular.
Give the name of a property that is influenced by the amount of matter in a sample.
A property that is dependent on the amount of substance in a sample is known as extensive property.
What are the qualities of matter that may be observed?
Features or qualities of materials or objects that we can describe using our five senses are known as observable properties. Color, texture, hardness, and flexibility can all be assessed using our senses.
What is the SI unit symbol for the amount of substance?
Since a mole is the SI unit for measuring the amount of a substance, it is abbreviated as ‘mol.’
Is matter’s density one of its properties?
The mass-to-volume relationship is reflected by density, which is a physical property of matter. The denser a thing is, the more mass it possesses in a given amount of space. Since different substances have varying densities, so density measurements are important for distinguishing substances.
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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