Oxidation number is defined as the total number of electrons that an atom either gains or loses to form a chemical bond with another atom. Let’s learn about oxidation number in detail, including its rules and steps to calculate it with the help of examples.

Oxidation Number-Definition, How To Find, Examples, Difference between Oxidation & Reduction

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Oxidation number is defined as the total number of electrons that an atom either gains or loses to form a chemical bond with another atom. Let’s learn about oxidation number in detail, including its rules and steps to calculate it with the help of examples.

Oxidation Number Definition

Oxidation Number is defined as the charge, whether positive or negative gained by an atom of an element when they form bonds with atoms of other elements either by sharing or transferring electrons.

  • The charge that appears as an oxidation number is the number of electrons lost, gained or shared by the atom during the formation of a bond with atoms of another element in a molecule.
  • It can be positive, negative, zero or fraction depending upon the situation.
  • The oxidation number of an atom is often referred to as its oxidation state.
  • It is generally assigned to atoms in the reaction in which they undergo oxidation and reduction. Such a reaction in which atoms either get oxidised or get reduced is called a redox reaction. The word redox is an acronym of two words reduction and oxidation. 

Note – In assigning oxidation numbers, we simplify the molecular complexity by assuming complete electron transfer, treating bonds as fully ionic. For example, in CO, carbon’s oxidation state is simplified by assuming complete electron loss to oxygen.

List of Oxidation Numbers

ElementOxidation Number
Hydrogen (H)+1
Oxygen (O)-2
Fluorine (F)-1
Chlorine (Cl)-1
Bromine (Br)-1
Iodine (I)-1
Group 1 metals (e.g., Li, Na, K)+1
Group 2 metals (e.g., Mg, Ca, Ba)+2
Group 13 metals (e.g., Al)+3
Group 14 elements (e.g., C in CH4)-4
Group 15 elements (e.g., N in NH3)-3
Group 16 elements (e.g., S in H2S)-2
Group 17 elements (e.g., Cl in HCl)-1

Oxidation number of elements from 1 to 30

H+1
He0
Li+1
Be+2
B+3
C-4/+4
N-3/+3
O-2
F-1
Ne0
Na+1
Mg+2
Al+3
Si-4/+4
P-3/+3/+5
S-2/+4/+6
Cl-1
Ar0
K+1
Ca+2
Sc+3
Ti+2/+3/+4
V+2/+3/+4/+5
Cr+2/+3/+6
Mn+2/+3/+4/+6/+7
Fe+2/+3/+4/+6
Co+2/+3
Ni+2/+3/+4
Cu+1/+2
Zn+2
  

How to Find Oxidation Number

The oxidation number of an atom is the number of electrons lost or gained to form bonds with heteroatoms in a particular molecule. The molecule can be neutral (its overall charge is zero) or may be charged (it has some overall positive or negative charge).

To find the oxidation number of an atom we need to follow the following steps:

Step 1: Assume the oxidation number of the atom to be X which you need to calculate.

Step 2: Mention the oxidation state of other bonded atoms and multiply it with the number of such atoms present in one molecule.

Step 3: Write the oxidation number of all the atoms in the molecule in a linear sum format and equate it to the overall charge of the molecule.

Step 4: Solve for X.

We can learn it with the help of examples below.

Oxidation Number of Sulphur in H2SO4

Oxidation number is defined as the total number of electrons that an atom either gains or loses to form a chemical bond with another atom. Let’s learn about oxidation number in detail, including its rules and steps to calculate it with the help of examples.

Oxidation Number of Sulphur in H2SO4

Solution:

Step 1: Assume the oxidation number of sulphur to be x

Step 2: The oxidation number for Hydrogen is +1 and for O is -2.

Step 3: Since the overall charge on the molecule is 0, therefore 2(+1) + X + 4(-2) = 0

Step 4: 2 + X – 8 = 0 ⇒ X – 6 = 0 ⇒ X = +6

Hence, the oxidation number of Sulphur in H2SO4 is +6

Oxidation Number of Chromium in Cr2O72-

Oxidation number is defined as the total number of electrons that an atom either gains or loses to form a chemical bond with another atom. Let’s learn about oxidation number in detail, including its rules and steps to calculate it with the help of examples.

Oxidation Number of Chromium in Cr2O72-

Solution:

Step 1: Assume the oxidation number for Chromium be X

Step 2: The oxidation number for oxygen is -2

Step 3: Since the molecule has an overall charge of -2 the equation can be written as 2X + 7(-2)=-2

Step 4: 2X – 14 = -2 ⇒ 2X = +12 ⇒ X = +6

Hence the oxidation number of chromium in Cr2O72- is +6.

It should be noted that in one molecule there can be different oxidation numbers for the same atom. This can be understood from the following example

Multiple Oxidation Numbers of an Atom in a Molecule

Now will learn how to calculate multiple oxidation numbers of an atom in a molecule discussed below:

Oxidation Number of Nitrogen in Ammonium Nitrate i.e. NH4NO3

Solution:

Step 1: In this case, we will split the molecule into two ions Ammonium ion (NH4+) and Nitrate ion (NO3–)

Step 2: We will find the oxidation number of Nitrogen in each ion. Assume the oxidation number for Nitrogen to be X in each case

Step 3: For the Ammonium ion, since the molecule has an overall +1 charge, hence equation can be written as X + 4(+1) = +1

Step 4: Solving the equation X + 4 = 1 ⇒ X = -3

Step 5: In the case of nitrate ion, the oxidation number for oxygen is -2 and the molecule has an overall charge of -1.

Step 6: Hence equation, in this case, will be X + 3(-2) = -1

Step 7: Solving the equation we get X – 6 = -1 ⇒ X = +5

Hence the oxidation number of Nitrogen in ammonium nitrate is -3 and +5

In the above examples, we saw that some atoms have fixed oxidation numbers. To understand why some atoms have fixed atomic numbers we need to look at the following mentioned rules of oxidation number.

Oxidation Number Rules

These are the rules to assign constant oxidation numbers to atoms of an element:

Rule 1: The total of all the atoms in a molecule’s oxidation numbers equals zero.

e.g. In KMnO4, the oxidation number of K is +1, the oxidation number of Mn is +7 and the oxidation number of oxygen is −2.

Rule 2: An atom’s oxidation number is always 0 in its most basic form.

e.g. The oxidation number of H, O, N, P, S, Se, Cu, Ag in their element forms is H2, O2, N2, P4, S8, Se8, Cu, Ag respectively, is zero.

Rule 3: Alkali metals (Li, Na, K, Rb, Cs) have an oxidation number of +1 in their compounds.

e.g. In NaCl, the oxidation number of Na is +1.

Rule 4: Alkaline earth metals (Be, Mg, Ca, Sr, Ba) usually have a +2 oxidation number in their compounds.

e.g. The oxidation number of Mg in MgO is +2.

Rule 5: Except in metal hydrides, the oxidation number of H in its compound is always +1.

e.g. In HCl, the oxidation number of H is +1 and in NaH (Sodium hydride), the oxidation number of H is −1.

Rule 6: The fluorine oxidation number is 1 in all its compounds.

e.g. In NaF, the oxidation number of F is −1.

Rule 7: The charge of an ionic compound is equal to the sum of all oxidation states of all the atoms in the compound. 

e.g. In SO42- the oxidation number of Sulphur is +6. The oxidation number of oxygen is −2. Hence the sum is +6+4(-2) = 6-8 = -2.

Rule 8: Except for oxygen and fluorine, the maximum oxidation number of any element is equal to its group number.

e.g. The oxidation number of sulphur in H2S2O8, K2S2O8, S2O–28 and H2SO5 is +6 due to the presence of a peroxide bond.

Rule 9: It’s possible that not all atoms of the same element have the same oxidation number in certain compounds. We get the average result when we compute the oxidation number for that element in such components.

e.g. One sulphur atom in Na2S2O3 has an oxidation number of +6, whereas the other sulphur atoms have an oxidation number of -2. As a result, the average sulphur oxidation state number in Na2S2O3 is +2.

Oxidation number is defined as the total number of electrons that an atom either gains or loses to form a chemical bond with another atom. Let’s learn about oxidation number in detail, including its rules and steps to calculate it with the help of examples.

Rule 10: Carbon in organic molecules can have any oxidation number between -4 and +4.

e.g. in HCHO, the oxidation number of carbon is zero.

Rule 11: The common oxidation number of an element is equivalent to its group number from IA to IV A. The formula (Group number –8) gives the common oxidation number of any element from V A to VIII-A.

e.g. 

  • Oxidation number of I A group elements = +1.
  • Oxidation number of II A group elements = +2.
  • Oxidation number of III A group elements = +3.
  • Oxidation number of IV A group elements = +4.
  • Oxidation number of V A group elements = –3.
  • Oxidation number of VI A group elements = –2.
  • Oxidation number of VII A group elements = –1.
  • Oxidation number of VIII A group elements = 0.

Rule 12: C, N, P, and S have oxidation numbers of 4,–3,–3 and –2 in all carbides, nitrides, phosphides, and sulphides, respectively.

e.g. In Mg3N2, the oxidation number of Nitrogen is −3.

Rule 13: In all Metal carbonyls, the oxidation number of metals is zero. 

e.g. In Ni(CO)4, the oxidation number of Ni is zero.

Rule 14: Except for peroxide, superoxides, oxyfluorides, and ozonides, oxygen has an oxidation number of -2 in most of its oxides.

e.g. In Na2O, the oxidation number of O is −2. 

Exceptional Cases for Oxidation Number of Oxygen

There are some exceptional cases for the oxidation number of Oxygen, which are

  • Peroxides: The oxidation number of oxygen in peroxides is 1.  Examples, are H2O2, and Na2O2.
  • Oxidation number of oxygen in fluorine compounds is +2. Examples are F2O or OF2, etc.
  • Superoxides: The oxidation number of oxygen in superoxides is –1/2.
  • Ozonides: Each oxygen atom in an ozonide has an oxidation number of –1/3.

Fixed Oxidation Levels in Atoms, Molecules, and Ions

In neutral atoms and molecules, the overall oxidation state is zero. For example, elements like sodium, magnesium, and iron have an oxidation state of zero. The same goes for neutral molecules like oxygen, chlorine, water, ammonia, methane, and potassium permanganate.

In homo-polar molecules, each atom’s oxidation state is also zero. For instance, in an oxygen molecule, the oxidation state of each oxygen atom is zero.

On the other hand, the oxidation state of charged ions equals the net charge of the ion. This means:

  • All alkali metal ions have an oxidation state of +1.
  • All alkaline earth metal ions have an oxidation state of +2.
  • All boron family metal ions have an oxidation state of +3.
  • Hydrogen has an oxidation state of +1 in a proton (H+) and -1 in a hydride.
  • Oxygen has an oxidation state of -2 in an oxide ion (O2-) and -1 in a peroxide ion (O-O2-).”

Oxidation Number Examples

As of now, we know the basic rules to calculate the Oxidation Number, hence we will find the Oxidation Number of some common compounds which we come across frequently in chemistry.

We will find the Oxidation Number of the following compounds:

Oxidation Number of Manganese in KMnO4

Solution:

 Let the oxidation number of Manganese in KMnO4 be equal to X

The oxidation number of Potassium = +1

The oxidation number of oxygen is =  –2

⇒1 + (X) + 4×(–2)=0

⇒1 + X – 8 = 0

⇒X -7 = 0

⇒X = +7

The oxidation number of Manganese in KMnO4 is +7.

Oxidation Number of Carbon in Na2CO3

Solution:

Oxidation number of oxygen is = –2

Oxidation number of Sodium = +1

Let the oxidation number of carbon be X

⇒2(+1) + X + 3(–2) = 0

⇒2 + X – 6 = 0

⇒X – 4 = 0

⇒X = +4

Therefore X = +4

Oxidation Number of Carbon in Na2CO3 is +4 

Oxidation Number of Nitrogen in Ammonium Nitrite

Solution:

Ammonium Nitrite is an ionic compound containing NH4+ and NO2– ions.

Oxidation number of nitrogen in NH4+

Let oxidation number of N atom is x

⇒ x + 4 = +1

⇒ x = 1 – 4 = -3

Oxidation number of nitrogen in NO2–

Let oxidation number of Nitrogen atom be Y

Y + 2(-2) = -1

⇒ Y – 4 = -1

⇒ Y = -1 + 4 = +3

Thus, one atom of Nitrogen in Ammonium Nitrite is in the -3 oxidation state, while the other nitrogen atom is in the +3 oxidation state.

Oxidation Number of Carbon in CN–

Solution:

Let Oxidation Number of C atom in CN– be x, Oxidation Number for N atom is -3 and the overall charge on the molecule is -1. 

⇒ x – 3 = -1

⇒ x = -1 + 3 = +2

Hence, Carbon atom has oxidation number of +2 in CN–

Oxidation Number of N in NH3

Solution:

Let Oxidation Number of N in NH3 be x and we know that Oxidation Number of H is +1.

⇒ x + 3(+1) = 0

⇒ x + 3 = 0

⇒ x = -3

Hence, the Oxidation Number of N atom in NH3 is -3.

Difference between Oxidation and Reduction

Oxidation: The loss of electrons or a rise in the positive oxidation state or decrease in the negative oxidation state of an atom, an ion, or specific atoms in a molecule is referred to as oxidation.

Reduction: The gain of electrons or a drop in the positive oxidation state or increase in the negative oxidation state of an atom, an ion, or specific atoms in a molecule is referred to as reduction . It is referred toas reduction in the oxidation state.

AspectOxidationReduction
DefinitionLoss of electronsGain of electrons
Oxidation stateIncreaseDecrease
Electron transferElectrons are lost or removed from a speciesElectrons are gained or added to a species
ReactivitySpecies acts as an electron donorSpecies acts as an electron acceptor
ExamplesRusting of iron, combustion reactionsReduction of metal ions, hydrogenation reactions

Related:

Oxidation Number- FAQs

What is Oxidation Number?

The charge that appears on an atom of an element when it bonds with atoms of other elements in a molecule is called Oxidation Number.

What is the Common Oxidation Number of Inert Gases?

Inert gases have an oxidation number of zero.

What are the Rules for Calculating Oxidation Numbers?

The rules for oxidation numbers are:

  1. The total of all the atoms in a molecule’s oxidation numbers equals zero.
  2. An atom’s oxidation number in its most basic form is always zero.
  3. In their compounds, the oxidation number of alkali metals (Li, Na ,K ,Rb ,Cs) is always +1.
  4. In their compounds, the oxidation number of alkaline earth metals (Be ,Mg ,Ca ,Sr ,Ba) is always +2.
  5. Except in metal hydrides, the oxidation number of H in its compound is always +1.
  6. Fluorine has an oxidation number of 1 in all of its compounds.
  7. Except for peroxide, super oxides, oxyfluoride, and ozonides, the oxidation number of oxygen in most of its oxides is -2.
  8. Carbon in organic molecules can have any oxidation number between -4 and +4.

What is the Oxidation Number of Mercury(Hg) in Amalgam?

Mercury amalgam has a zero-oxidation number. Each element in an alloy or amalgam has an oxidation number of zero.

What is the Oxidation Number of Oxygen in O3 and in MgO?

  • Oxidation number of O in O3 = 0
  • Oxidation number of O in MgO = –2

What are the Oxidation Numbers of Oxide and Hydride ions?

The oxidation number for oxide ion is -2 and that of hydride ion is -1.

What is the Oxidation Number of Sulphur in S8?

S8 is a polyatomic molecule, it is in its most basic form. As a result, sulphur’s oxidation number in this molecule is zero.

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.

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CBSE Class 12 Chemistry Syllabus Download PDF

Below is the CBSE Class 12 Syllabus along with the marking scheme and time duration of the Chemistry exam.

S.NoTitleNo. of PeriodsMarks
1Solutions107
2Electrochemistry129
3Chemical Kinetics107
4d -and f -Block Elements127
5Coordination Compounds127
6Haloalkanes and Haloarenes106
7Alcohols, Phenols and Ethers106
8Aldehydes, Ketones and Carboxylic Acids108
9Amines106
10Biomolecules127
Total70

CBSE Class 12 Chemistry Practical Syllabus along with Marking Scheme

The following is a breakdown of the marks for practical, project work, class records, and viva. The total number of marks for all parts is 15. The marks for both terms are provided in the table below.

Evaluation Scheme for ExaminationMarks
Volumetric Analysis08
Salt Analysis08
Content-Based Experiment06
Project Work and Viva04
Class record and Viva04
Total30

CBSE Class 12 Chemistry Syllabus (Chapter-wise)

Unit -1: Solutions

  • Raoult's law.
  • Colligative properties - relative lowering of vapour pressure, elevation of boiling point, depression of freezing point, osmotic pressure, determination of molecular masses using colligative properties, abnormal molecular mass.
  • Solutions, Types of solutions, expression of concentration of solutions of solids in liquids, solubility of gases in liquids, solid solutions.
  • Van't Hoff factor.

Unit -2: Electrochemistry

  • Redox reactions, EMF of a cell, standard electrode potential
  • Nernst equation and its application to chemical cells
  • Relation between Gibbs energy change and EMF of a cell
  • Kohlrausch's Law
  • Electrolysis and law of electrolysis (elementary idea)
  • Dry cell-electrolytic cells and Galvanic cells
  • Conductance in electrolytic solutions, specific and molar conductivity, variations of conductivity with concentration.
  • Lead accumulator
  • Fuel cells

Unit -3: Chemical Kinetics

  • Rate of a reaction (Average and instantaneous)
  • Rate law and specific rate constant
  • Integrated rate equations and half-life (only for zerfirst-order order reactions)
  • Concept of collision theory (elementary idea, no mathematical treatment)
  • Factors affecting rate of reaction: concentration, temperature, catalyst;
  • Order and molecularity of a reaction
  • Activation energy
  • Arrhenius equation

Unit -4: d and f Block Elements  

  • Lanthanoids- Electronic configuration, oxidation states, chemical reactivity and lanthanoid contraction and its consequences.
  • Actinoids- Electronic configuration, oxidation states and comparison with lanthanoids.
  • General introduction, electronic configuration, occurrence and characteristics of transition metals, general trends in properties of the first-row transition metals – metallic character, ionization enthalpy, oxidation states, ionic radii, color, catalytic property, magnetic properties, interstitial compounds, alloy formation, preparation and properties of K2Cr2O7 and KMnO4.

Unit -5: Coordination Compounds  

  • Coordination compounds - Introduction, ligands, coordination number, color, magnetic properties and shapes
  • The importance of coordination compounds (in qualitative analysis, extraction of metals and biological system).
  • IUPAC nomenclature of mononuclear coordination compounds.
  • Bonding
  • Werner's theory, VBT, and CFT; structure and stereoisomerism

Unit -6: Haloalkanes and Haloarenes  

  • Haloarenes: Nature of C–X bond, substitution reactions (Directive influence of halogen in monosubstituted compounds only). Uses and environmental effects of - dichloromethane, trichloro methane, tetrachloromethane, iodoform, freons, DDT.
  • Haloalkanes: Nomenclature, nature of C–X bond, physical and chemical properties, optical rotation mechanism of substitution reactions.

Unit -7: Alcohols, Phenols and Ethers   

  • Phenols: Nomenclature, methods of preparation, physical and chemical properties, acidic nature of phenol, electrophilic substitution reactions, uses of phenols.
  • Ethers: Nomenclature, methods of preparation, physical and chemical properties, uses.
  • Alcohols: Nomenclature, methods of preparation, physical and chemical properties (of primary alcohols only), identification of primary, secondary and tertiary alcohols, mechanism of dehydration, and uses with special reference to methanol and ethanol.

Unit -8: Aldehydes, Ketones and Carboxylic Acids   

  • Carboxylic Acids: Nomenclature, acidic nature, methods of preparation, physical and chemical properties; uses.
  • Aldehydes and Ketones: Nomenclature, nature of carbonyl group, methods of preparation, physical and chemical properties, mechanism of nucleophilic addition, the reactivity of alpha hydrogen in aldehydes, uses.

Unit -9: Amines    

  • Diazonium salts: Preparation, chemical reactions and importance in synthetic organic chemistry.
  • Amines: Nomenclature, classification, structure, methods of preparation, physical and chemical properties, uses, and identification of primary, secondary and tertiary amines.

Unit -10: Biomolecules     

  • Proteins -Elementary idea of - amino acids, peptide bond, polypeptides, proteins, structure of proteins - primary, secondary, tertiary structure and quaternary structures (qualitative idea only), denaturation of proteins; enzymes. Hormones - Elementary idea excluding structure.
  • Vitamins - Classification and functions.
  • Carbohydrates - Classification (aldoses and ketoses), monosaccharides (glucose and fructose), D-L configuration oligosaccharides (sucrose, lactose, maltose), polysaccharides (starch, cellulose, glycogen); Importance of carbohydrates.
  • Nucleic Acids: DNA and RNA.

The syllabus is divided into three parts: Part A, Part B, and Part C. Part A consist of Basic Concepts of Chemistry, which covers topics such as atomic structure, chemical bonding, states of matter, and thermochemistry. Part B consists of Topics in Physical Chemistry, which includes topics such as chemical kinetics, equilibrium, and electrochemistry. Part C consists of Topics in Organic Chemistry, which covers topics such as alkanes, alkenes, alkynes, and aromatic compounds.

Basic Concepts of Chemistry:

  • Atomic structure: This section covers the fundamental concepts of atomic structure, including the electronic configuration of atoms, the Bohr model of the atom, and the wave nature of matter.
  • Chemical bonding: This section covers the different types of chemical bonds, including ionic, covalent, and metallic bonds, as well as the concept of hybridization.
  • States of the matter: This section covers the three states of matter - solid, liquid, and gas - and the factors that influence their properties.
  • Thermochemistry: This section covers the principles of thermochemistry, including the laws of thermodynamics and the concept of enthalpy.

Chapters in Physical Chemistry:

  • Chemical kinetics: This section covers the study of the rate of chemical reactions and the factors that influence it, including the concentration of reactants, temperature, and the presence of catalysts.
  • Equilibrium: This section covers the principles of chemical equilibrium, including the concept of Le Chatelier's principle and the equilibrium constant.
  • Electrochemistry: This section covers the principles of electrochemistry, including the concept of half-cell reactions, galvanic cells, and electrolysis.

Chapters in Organic Chemistry:

  • Alkanes: This section covers the properties and reactions of alkanes, including their structure, isomerism, and combustion.
  • Alkenes: This section covers the properties and reactions of alkenes, including their structure, isomerism, and addition reactions.
  • Alkynes: This section covers the properties and reactions of alkynes, including their structure, isomerism, and addition reactions.
  • Aromatic compounds: This section covers the properties and reactions of aromatic compounds, including their structure, isomerism, and electrophilic substitution reactions.

In addition to the topics covered in the syllabus, the CBSE Class 12 Chemistry exam also tests students on their analytical and problem-solving skills, as well as their ability to apply the concepts learned in the classroom to real-world situations.

Students can also check out the Tips for the Class 12 Chemistry Exam. They can easily access the Class 12 study material in one place by visiting the CBSE Class 12 page at ANAND CLASSES (A School Of Competitions). Moreover, to get interactive lessons and study videos, download the ANAND CLASSES (A School Of Competitions) App.

Frequently Asked Questions on CBSE Class 12 Chemistry Syllabus

Q1

How many chapters are there in the CBSE Class 12 Chemistry as per the syllabus?

There are 10 chapters in the CBSE Class 12 Chemistry as per Syllabus. Students can learn all these chapters efficiently using the study materials provided at ANAND CLASSES (A School Of Competitions).

Q2

What is the marking scheme for CBSE Class 12 Chemistry practical exam according to the syllabus?

The marking scheme for CBSE Class 12 Chemistry practical exam, according to the syllabus, is 8 marks for volumetric analysis, 8 marks for salt analysis, 6 marks for the content-based experiment, 4 marks for the project and viva and 4 marks for class record and viva.

Q3

Which is the scoring chapter in Chemistry as per CBSE Class 12 syllabus?

The chapter Electrochemistry in Chemistry is the scoring chapter as per CBSE Class 12 syllabus.

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