Score better in Chemistry with these CBSE Class 11 MCQs, ready for 2026-27. Built chapter by chapter, they help Class 11 students get comfortable with the current exam pattern and sharpen problem-solving.
Getting the Most From Chemistry Objective Questions
- Built around the 2026 Chemistry textbook from CBSE, following their latest guidelines.
- A wide range of Class 11 Assertion and Reasoning, Case-based, and Fill-in-the-blanks questions for Chemistry.
- Each Chemistry chapter has its own set, so you can check your understanding topic by topic.
- Every Chemistry MCQ comes with a correct, explained answer - not just the right option.
Browse Class 11 Chemistry MCQs by Chapter
Check out the newest 2026-27 Chemistry question sets below. They're great for self-checking, and for finding out which topics need more work before exams.
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Quick Practice - Try a Few Questions First Pick a chapter below, answer a few questions instantly, then jump to the full set list for more. Q1.The amount of a substance that contains as many elementary particles as there are atoms in 12 grams of carbon 12 is called: Answer: (b) One mole. This quantity, known as Avogadro's number of particles, gives chemists a consistent way to count atoms and molecules.
Q2.The law which states that matter can neither be created nor destroyed in a chemical reaction is known as the: Answer: (b) Law of conservation of mass. It means the total mass of the reactants must equal the total mass of the products formed in any chemical change.
Q3.According to the law of definite proportions, a given compound always contains its constituent elements in: Answer: (b) A fixed ratio by mass. Whether prepared in a laboratory or found in nature, a pure compound shows the same fixed mass ratio of its elements every time.
Q4.Significant figures in a measured quantity indicate: Answer: (b) The reliability or precision of the measurement. Counting them correctly helps avoid claiming more precision in a result than the measuring instrument can actually support.
Q5.The empirical formula of a compound represents: Answer: (b) The simplest whole number ratio of atoms of each element present. The molecular formula can be a whole number multiple of this simplest ratio, depending on the actual size of the molecule.
Q1.The subatomic particle that carries a negative charge and revolves around the nucleus is the: Answer: (c) Electron. Its arrangement around the nucleus in specific energy levels largely determines how an atom behaves chemically.
Q2.According to Bohr's model, electrons revolve around the nucleus in fixed paths called: Answer: (b) Energy shells or orbits. Each of these paths corresponds to a definite energy level, and electrons do not lose energy while moving within one of them.
Q3.The maximum number of electrons that can be accommodated in a given shell is given by the formula: Answer: (d) 2n squared. Here n stands for the shell number, so this formula predicts how many electrons each successive shell can hold at most.
Q4.The quantum number that describes the shape of an orbital is the: Answer: (b) Azimuthal quantum number. Different values of this number correspond to different subshells, such as s, p, d and f, each with its own characteristic shape.
Q5.The Heisenberg uncertainty principle states that it is impossible to simultaneously determine, with complete accuracy, an electron's: Answer: (b) Position and momentum. This principle reflects the wave like nature of very small particles and set the stage for the modern quantum mechanical model of the atom.
Q1.Elements in the modern periodic table are arranged in order of increasing: Answer: (b) Atomic number. This arrangement, based on the number of protons in the nucleus, resolved several inconsistencies found in earlier mass based tables.
Q2.As you move from left to right across a period in the periodic table, atomic size generally: Answer: (b) Decreases. The increasing nuclear charge pulls the electron cloud in more tightly, making atoms progressively smaller across a period.
Q3.Ionisation enthalpy generally shows what trend when moving down a group in the periodic table? Answer: (b) It decreases steadily. As atoms get larger down a group, outer electrons sit farther from the nucleus and are held less tightly, so less energy is needed to remove them.
Q4.Elements that readily lose electrons to form positive ions are generally classified as: Answer: (b) Metals. This tendency to lose electrons and form cations is one of the defining chemical characteristics of metallic elements.
Q5.Electronegativity of an element refers to its tendency to: Answer: (b) Attract shared electrons in a chemical bond. This property helps explain why bonds between certain pairs of atoms end up being polar rather than purely covalent.
Q1.A chemical bond formed by the complete transfer of electrons from one atom to another is called a: Answer: (b) Ionic bond. This transfer typically happens between a metal, which loses electrons, and a non metal, which gains them, forming oppositely charged ions.
Q2.A bond formed by the mutual sharing of electron pairs between two atoms is known as a: Answer: (b) Covalent bond. Both atoms contribute electrons to the shared pair, and this sharing holds the two atoms together.
Q3.The theory that explains molecular shapes based on the repulsion between electron pairs around a central atom is called: Answer: (b) VSEPR theory. Electron pairs, whether bonding or lone pairs, arrange themselves as far apart as possible around the central atom to minimise repulsion.
Q4.A sigma bond is formed by the: Answer: (b) Head on overlap of atomic orbitals along the internuclear axis. This head on overlap produces a bond that is generally stronger than the sideways overlap seen in a pi bond.
Q5.Hydrogen bonding is best described as an attractive force that occurs between: Answer: (b) A hydrogen atom bonded to a highly electronegative atom and another electronegative atom nearby. Elements like oxygen, nitrogen and fluorine are small and highly electronegative enough to support this kind of interaction with hydrogen.
Q1.In thermodynamics, a system that can exchange both matter and energy with its surroundings is called a: Answer: (b) Open system. This is different from a closed system, which can exchange energy but not matter, or an isolated system, which exchanges neither.
Q2.The first law of thermodynamics is essentially a statement of the conservation of: Answer: (b) Energy. It tells us that energy can be converted from one form to another, such as heat to work, but the total amount always stays constant.
Q3.A process that occurs without any exchange of heat between the system and its surroundings is called: Answer: (b) Adiabatic. Even though no heat is exchanged in this kind of process, the temperature of the system can still change due to work being done.
Q4.Enthalpy change of a reaction refers to the: Answer: (b) Heat absorbed or released at constant pressure. For most reactions carried out in open vessels at atmospheric pressure, this is the quantity that is measured experimentally.
Q5.A reaction that releases heat to the surroundings is described as being: Answer: (b) Exothermic. The products of such a reaction generally end up at a lower energy level than the original reactants.
Q1.A state in which the rate of the forward reaction equals the rate of the reverse reaction is called: Answer: (b) Chemical equilibrium. At this point the concentrations of reactants and products no longer change with time, even though both reactions keep occurring.
Q2.According to Le Chatelier's principle, when a system at equilibrium is subjected to a change in conditions, it will: Answer: (b) Shift in a direction that tends to counteract the change. This principle helps predict how factors like concentration, pressure and temperature will shift the position of an equilibrium.
Q3.The equilibrium constant for a reaction is a measure of the: Answer: (b) Relative amounts of products and reactants at equilibrium. A large value generally indicates that the reaction favours the formation of products once equilibrium is reached.
Q4.A substance that increases the hydrogen ion concentration when dissolved in water is classified, in the Arrhenius sense, as a(n): Answer: (b) Acid. This classic definition works well for many common acids, even though later theories broadened the concept further.
Q5.A buffer solution is one that resists significant change in: Answer: (b) pH upon addition of small amounts of acid or base. It typically contains a weak acid along with its conjugate base, or a weak base with its conjugate acid, working together to absorb such changes.
Q1.Oxidation, in terms of electron transfer, is best defined as the: Answer: (b) Loss of electrons. This modern electronic definition works well alongside the older idea of oxidation as the addition of oxygen to a substance.
Q2.Reduction, in terms of electron transfer, is best defined as the: Answer: (b) Gain of electrons. A species that gains electrons in this way is said to be reduced, while it simultaneously helps oxidise another substance.
Q3.In a redox reaction, the substance that gets oxidised while causing another substance to be reduced is called the: Answer: (b) Reducing agent. It donates electrons to the other reactant, and in doing so its own oxidation state increases during the reaction.
Q4.The oxidation number of an atom in its elemental, uncombined form is always taken as: Answer: (c) Zero. This convention applies regardless of the element, whether it exists as single atoms or as a diatomic molecule.
Q5.A disproportionation reaction is one in which: Answer: (b) The same element is simultaneously oxidised and reduced. Part of the atoms of that element end up with a higher oxidation state while another part end up with a lower one.
Q1.Organic chemistry is broadly defined as the study of compounds of the element: Answer: (c) Carbon. Carbon's unique ability to form long chains and rings with itself and other elements gives rise to an enormous variety of compounds.
Q2.Compounds having the same molecular formula but different structural arrangements are called: Answer: (b) Isomers. Even though such compounds share an identical formula, their differing structures often give them noticeably different properties.
Q3.A functional group in an organic molecule is best described as: Answer: (b) A specific group of atoms responsible for the characteristic chemical behaviour of the compound. Compounds sharing the same functional group tend to undergo similar types of chemical reactions.
Q4.The technique used to separate and purify organic liquids based on differences in their boiling points is called: Answer: (b) Distillation. The liquid with the lower boiling point vaporises first and is collected separately as the mixture is gradually heated.
Q5.A homologous series is a group of compounds that: Answer: (b) Differ from each other by a constant CH2 unit and show similar chemical properties. Members of such a series can be represented by a single general formula and tend to show a gradual change in physical properties.
Q1.Hydrocarbons that contain only single covalent bonds between carbon atoms are called: Answer: (b) Alkanes. Because every carbon to carbon bond in these compounds is a single bond, they are also described as saturated hydrocarbons.
Q2.A hydrocarbon containing at least one carbon to carbon double bond is classified as a(n): Answer: (b) Alkene. The presence of this double bond makes such compounds generally more reactive than their fully saturated counterparts.
Q3.Benzene, a common aromatic hydrocarbon, has the molecular formula: Answer: (b) C6H6. Its ring structure with alternating bonds gives it a special stability that is characteristic of aromatic compounds.
Q4.The addition of hydrogen halides to alkenes generally follows a rule known as: Answer: (b) Markovnikov's rule. This rule helps predict which carbon of the double bond the halogen atom is more likely to attach to in an unsymmetrical alkene.
Q5.The process by which saturated hydrocarbons undergo reactions where a hydrogen atom is replaced by another atom or group is called a: Answer: (a) Substitution reaction. Since alkanes lack multiple bonds for addition reactions, this replacement type of reaction is their more typical mode of reacting.
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| Chapter 01 Some Basic Concepts of Chemistry MCQs |
| Chapter 01 Some Basic Concepts of Chemistry MCQs Set 01 |
| Chapter 01 Some Basic Concepts of Chemistry MCQs Set 02 |
| Chapter 02 Structure of Atom MCQs Set 01 |
| Chapter 02 Structure of Atom MCQs Set 02 |
| Chapter 02 Structure of Atom MCQs Set 03 |
| Chapter 03 Classification of Elements and Periodicity in Properties MCQs Set 01 |
| Chapter 03 Classification of Elements and Periodicity in Properties MCQs Set 02 |
| Chapter 03 Classification of Elements and Periodicity in Properties MCQs |
| Chapter 07 Redox Reactions MCQs Set 01 |
| Chapter 07 Redox Reactions MCQs Set 02 |
| Chapter 09 Hydrocarbons MCQs Set 01 |
| Chapter 09 Hydrocarbons MCQs Set 02 |
| Chapter 09 Hydrocarbons MCQs Set 03 |
| Chapter 09 Hydrocarbons MCQs Set 04 |
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FAQs
For the 2026-27 session, MCQs and objective-type questions carry around 20% weightage. CBSE has introduced 30% competency based questions as MCQs and they are important part of the Class 11 Chemistry paper.
You can access the latest chapter-wise MCQs for Class 11 Chemistry for free from StudiesToday.com. All questions are based on the latest syllabus and current academic year.
Yes, our Chemistry practice bank includes the new pattern of Assertion Reasoning and Case Study based MCQs. They have been designed to test the analytical skills of Class 11 students.
Solving Class 11 Chemistry MCQs regularly improves speed and accuracy as these are objective questions can get you 100% marks if your understanding of the topic is clear.
Yes, all Class 11 Chemistry MCQs and answers are accessible on any device at your convenience.
No, all Chemistry Multiple Choice Questions (MCQs), practice papers, and solutions for Class 11 are available for free for students to get more marks school exams.