Class 9 Chemistry Chapter 1 Fundamentals of Chemistry Important Short Questions 2024

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Class 9 Chemistry Chapter 1 Notes

Post TopicShort Questions
Book CodeChemistry
Class9th Class
Chapter/FullFull Book / All Chapters
BoardPunjab Board

Class 9 Chemistry Chapter 1 Fundamentals of Chemistry Short Questions Notes

  • Chemistry is the study of the composition and properties of matter. It has different branches.
  • Substances are classified into elements and compounds.
  • Elements consist of only one type of atom.
  • Compounds are formed by the chemical combination of atoms of the elements in a fixed ratio.
  • Mixtures are formed by mixing up elements or compounds in any ratio. They are classified as homogeneous and heterogeneous mixtures.
  • Each atom of an element has a specific atomic number (Z) and a mass number or atomic mass (A).
  • The atomic mass of an atom is measured relative to a standard mass of C-12.
  • The relative atomic mass of an element is the mass of an element compared with 1/12 mass of an atom of the C-12 isotope.
  • Atomic mass unit is 1/12 of the mass of one atom of C-12, lamu = 1.66  l0 g
  • The empirical formula is the simplest type of chemical formula, which shows the relative number of atoms of each element in a compound.
  • The molecular formula gives the actual number of atoms of each element in a molecule.
  • Formula mass is the sum of atomic masses of all the atoms in one formula unit of a substance.
  • An atom or group of atoms having a charge on it is called an ion. If it has a positive
  • charge it is called a cation and if it has a negative charge it is called an anion.
  • There are different types of molecules: monoatomic, polyatomic, homoatomic, and heteroatomic.
  • The number of particles in one mole of a substance is called Avogadro’s number. The value of this number is 6.02 10 It is represented as N A
  • The amount of a substance having 6.02 10 particles is called a mole. The quantitative definition of the mole is atomic mass, molecular mass, or formula mass expressed in grams.
  • Define industrial chemistry and analytical chemistry.
  • How can you differentiate between organic and inorganic chemistry?
  • Give the scope of biochemistry.
  • How does a homogeneous mixture differ from a heterogeneous mixture?
  • What is the relative atomic mass? How is it related to gram?
  • Define the empirical formula with an example.
  • State three reasons why you think air is a mixture and water a compound.
  • Explain why are hydrogen and oxygen considered elements whereas water is a compound.
  • What is the significance of the symbol of an element?
  • State the reasons: soft drink is a mixture and water is a compound.
  • Classify the following into elements, compound, or mixture:
  • i He and H
  • ii CO and Co
  • iii Water and milk 2
  • iv Gold and brass
  • v Iron and steel
  • Define atomic mass unit. Why is it needed?
  • State the nature and name of the substance formed by combining the following:
  • i Zinc + Copper
  • ii Water + Sugar
  • iii Aluminium + Sulphur
  • iv Iron + Chromium + Nickel
  • Differentiate between molecular mass and formula mass, which of the following has a molecular formula? H O, NaCl, KI, H SO 2 2 4
  • Which one has more atoms: 10 g of Al or 10 g of Fe?
  • Which one has more molecules: 9 g of water or 9 g of sugar (C H O )? 12 22 11
  • Which one has more formula units: 1 g of NaCl or 1 g of KC1?
  • Differentiate between homoatomic and heteroatomic molecules with examples.
  • In which one of the following the number of hydrogen atoms is more? 2 moles of HC1 or 1 mole of NH (Hint: 1 mole of a substance contains as much number 3 of moles of atoms as are in 1 molecule of a substance

Chemistry Chapter 1 Short Questions PDF Download

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Chemistry Chapter 1 Short Questions


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