11th Chemistry Chapter 1 Notes

• Here are the detailed 11th class chemistry notes chapter 1 to help you prepare for your exams.
• Define atom. Give examples
• What are the main points of Dalton’s atomic theory?
• Define molecule. Give examples.
• Define macromolecules. Give an example.
• Define ion. Give examples.
• Define cation. Give an example.
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• What are molecular ions? How are they formed? Give their use. 
• Define isotopes. Give examples.
• The atomic masses may be in fraction. Why?
• Why the isotopes have the same chemical properties but different physical properties? Ans: The isotopes of the same element have same chemical properties as they have same electronic configuration and chemical properties depend upon the number of electrons. They have different physical properties as they have different number of neutrons in the nucleus and physical properties depend upon the nucleus.
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• Comment on how atomic number and atomic mass define stability of isotopes.
• Define mole. Give examples.
• Name the steps involved in the working of mass spectrometer.
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• Mention the methods which can be used for the separation of isotopes. 
• Write the steps involved in the determination of empirical formula?
• Mention the steps involved in combustion analysis. 
• Mention the compounds having same empirical and molecular formula.
• Define Avogadro’s number. Give examples.
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• How Avogadro’s number relates to the masses of chemical substances? 
• Why the experimental yield is mostly less than the theoretical yield?
• Distinguish between actual yield and theoretical yield. 
• Concept of limiting reactant is not applicable to the reversible reactions. Explain it.
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• The reaction of combustion in atmosphere consumes O2 which is in excess. What is limiting reactant?
• Give examples of limiting reactant in daily life.
• Why isotopes have same chemical but different physical properties? 
• Why oxygen cannot be determined directly in combustion analysis?
• 23g of sodium and 238g of uranium have equal number of atoms in them. Justify. 
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• A compound may have same molecular and empirical formula. Justify.
• Law of conservation of mass must be considered during stoichiometric calculations. How? OR How is law of conservation of mass obeyed during stoichiometric calculations?
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• What is the function of an electrometer? Ans: Electrometer is also called an ion collector and develops the electrical current. The strength of the current thus measured gives the relative abundance of ions of a definite m/e value. Similarly, the ions of other isotopes having different masses are made to fall on the collector and the current strength is measured. The current strength in each case gives the relative abundance of each of the isotopes. The same experiment is performed with C-12 isotope and the current strength is compared.
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• Define empirical formula. Ans: It is the simplest formula that gives the small whole number ratio between the atoms of different elements present in a compound. In an empirical formula of a compound, AxBy, there are x atoms of an element A and y atoms of an element B. The empirical formula of glucose (C6H12O6) is CH2O and that of benzene (C6H6) is CH.
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• Define molecular formula. Ans: That formula of a substance which is based on the actual molecule is called molecular formula. It gives the total number of atoms of different elements present in the molecule of a compound. For example, molecular formula of benzene is C6H6 while that of glucose is C6H12O6.
• Define Avogadro's Number. Give examples. Ans: Avogadro's number is the number of atoms, molecules and ions in one gram atom of an element, one gram molecule of a compound and one gram ion of a substance, respectively.