Class 9 Science CBSE Test Paper for Atoms and Molecules

Given below are the Class 9 Science CBSE Test Paper for Atoms and Molecules
a) Concepts questions
b) Calculation problems
c) Multiple choice questions
d) Long answer questions
e) Fill in the blank's
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Question 1
State the law of mass conservation.
Law of mass conservation states that, mass can neither be created nor destroyed in a chemical reaction or a physical transformation.
Question 2
What do you understand by the law of constant proportion?
According to the Law of constant proportion, a chemical compound always has its compounding elements in definite proportion by mass, irrespective of the source and the type of chemical reaction.
Question 3.
Who was responsible for coining the term atom?
In modern science, John Dalton widely used it and he can be said to be responsible for coining it, but a more factually correct answer would be a Greek philosopher who goes by the name of Lucretius.
Question 4
What is an atom?
Atom is the smallest particle of matter which can take part in a chemical reaction.
Question 5.
What is a molecule?
A molecule is a group of atoms bonded together which represents the most fundamental unit of a chemical compound capable of taking part in a chemical reaction.
Question 6
What is atomicity?
Atomicity is the number of atoms in a molecule.
Question 7
Define atomic mass unit.
The Atomic mass unit is the sum of the atomic masses of all the atoms in a molecule.
Question 8.
Define ion.
An ion is an atom or a molecule with an electric charge (+ve or -ve), caused by gain or loss of a single or multiple electrons.
Question 9
Provide a difference between cations and anions, along with an example for each.
Cations are positively charged ions, e.g.  Fe2+ whereas, anions are negatively charged ions, e.g. F
Question 10
Define Avogadro’s constant.
Avogadro’s Constant (6.022 x 1023) is the number of atoms of an element present in one mole of that element.
Question 11
(a)Explain how atoms exist.
(b)What do you understand by atomicity?
(c) Explain polyatomic ions.
(a) Atoms of most elements don’t exist independently they exist as molecules, for molecules are more stable. However, atoms of inert gasses are chemically unreactive and they exist independently. E.g. helium.
(b) Atomicity is the number of atoms in a molecule. E.g. The atomicity of H2O = 3.
(c) A polyatomic ion is an ion composed of multiple atoms acting as a single charged unit.
Question 12
Explain atomic mass and gram atomic mass. Why does mass have different expressions viz,   ‘u’ and ‘gm’?
Atomic mass is the unit in which the mass of an atom is expressed, where one atomic mass unit is 1/12ththe mass of a carbon-12 atom.
Gram atomic mass is the atomic mass of an element expressed in grams.
The mass of an atom or a molecule is expressed in ‘u’, whereas, the molar mass is expressed in ‘gm’.
Question 13
Define a mole. Give the importance of the mole.
One mole of atoms, molecules, or particles is that amount of the particle(atoms, molecules and ions) whose mass is equal to that particle’s atomic or molecular mass in grams. 1 mole = 6.022 x 1023 particles of that substance.
Importance of a mole: -
  • Atoms and molecules are very small. So, it gets bothersome weighing them in grams and trying to count them. Mole concept, however, allows us to count atoms and molecules by weighing macroscopic amounts of materials.
  • It gives us a universally accepted standard of mass.
  • It provides a standard for reaction stoichiometry.  
    Question 14
    How many molecules are present in 1 ml of water?
     we know that density of water is 1gm/ml.
    Hence, 1 gm water will = 1 ml water.
     Now, we have molecular mass of water H2O = 1x2 + 16 = 18 gm
    18 gm of water contain 6.022 x 1023 molecules
    1 gm of water will contain = (6.022 x 1023)/18 molecules = 0.33 x 1023 molecules
     So, the no. of molecules of water in 1ml of water = 3.3 x 1022
Question 15.
Calculate the molecular mass of glucose, C 6H12 O6.
Molecular mass of C6H12 O= (12 x 6) + 12 + (16 x 6)
= 180u.
 Question 16.
H2O is the formula for water. What information do you get from this formula?
  • H2O represents water
  • H2O is a single molecule of water
  • H2O is a single mole of water. Thus, it contains 6.022 x 1023 molecules of water.
  • H2O contains 2 atoms of hydrogen and 1 atom of oxygen.
  • H2O has a molar mass of 18g
Question 17
What is the formula unit mass of CaCl2 and NaCl.
(Na = 23, Cl=35.5, Ca=40)
Formula Unit Mass of NaCl = 23 + 35.5 = 58.5u
Formula Unit Mass of CaCl2= 40+(2 x 35.5)= 111u.
Question 18
(i) Name the body which approves the nomenclature of elements and compounds.
 (ii) The symbol of sodium is written as Na and not as S. Give reason.
(iii) Name one element which form diatomic and one which form tetra atomic molecules.
(i) IUPAC (International Union of Pure and Applied Chemistry)
(ii) Latin name of sodium is Natrium. The first two letters (Na) of this name represents the symbol of sodium.
 (iii) Oxygen forms diatomic molecules and phosphorus forms tetra atomic molecules.
Question 19
10.0 g CaCO3 on heating gave 4.4 g of CO2 and 5.6 g of CaO. Show that these observations are in agreement with law of conservation of mass.
 Mass of reactants: 10gm
Mass of product = 4.4 + 5.6 = 10g
Since Mass of reactants is equal to Mass of products , therefore these observations are in agreement with law of conservation of mass.
Question 20
Why are Dalton's symbol not used in chemistry?
Dalton was the first scientist to use the symbol for the name of the elements a specific sense but it was difficult to memorize and in uses so Dalton's symbol are not used in chemistry
Question 21
What is the difference between 2O, O2 and O3.
2O represents 2 atoms of oxygen, and it is not possible for it to exist independently.
O2 represents an oxygen molecule which has two constituent oxygen atoms.
O3 represents a single ozone molecule and it does exist independently.
Question 22
Find out
(1) the mass of a single oxygen atom
(2) the mass of a single oxygen molecule
 (3) the mass of a mole of oxygen gas
(4) the mass of an oxygen ion
(5) the number of atoms in a mole of an oxygen molecule.
(1) Mass of a single oxygen atom
1 mole of oxygen atom = 16gm =6.022 x 1023 atoms
Therefore, Mass of one oxygen atom = 16/6.022 x 1023 = 2.65 x 10-23 gm
(2) Mass of a single oxygen atom
1 molecule oxygen = O=2 x 16 = 32u
(3) Mass of a mole of oxygen gas
1 mole of oxygen = O= 2 x 16 =32u
(4) Mass of an oxygen ion = mass of an oxygen atom (since electrons have negligible mass)
(5) Number of atoms in a mole of oxygen molecule
We know, 1 mole of oxygen molecule, O2 = 6.022 x 1023 molecules.
1 molecule of O2= 2 atoms
Therefore in a mole of O, there are                       =6.022 x 1023 x 2 atoms
= 1.022 x 1024 atoms.
Question 23
What is the atomicity of oxygen and phosphorous?
Atomicity of oxygen, O2= 2 and atomicity of phosphorous, P4= 4.
Question 24
How many moles of SO2 have same mass as 3 moles of oxygen?
mass of 3 moles of oxygen = 3 x 16 = 48g Now, mass of SO2 = 32 + 2 x16 = 64g as 64g of SO2 = 1 mole then 48 g of SO2 = (1/64)x 48 =0.75 mole


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