Class 9 Science Atoms and Molecules

Class 9 Science Atoms and Molecules

I. Multiple Choice questions
Choose the correct option:
1. The atomicity of K₂Cr₂O₇ is
(a) 9 (b) 11
(c) 10 (d) 12
2. The formula for quick lime is
(a) CaCl₂ (b) CaCO₃
(c) Ca(OH)₂ (d) CaO
3. The symbol of cadmium is
(a) Ca (b) Cu
(c) Cm (d)Cd
4. All noble gas molecules are
(a) monoatomic
(c) triatomic
5. The valency of nitrogen in NH₃ is
(a) 1 (b)3
(c) 4 (d) 5
6. The formula of ethanol is C₂H₅—OH. Its molecular mass is
(a) 46 u (b) 34 u
(c) 34 g (d) 46 g
7. How many moles are present in 28 g of nitrogen atoms?
(a) 1 mole (b) 2.3 moles
(c) 0.5 mole (d) 2 moles
8. The molecular mass of x is 106. x among the following is
(a) CaC0₃ (b) S0₃
(c) Na₂C0₃ (d) NaCl
9. Which among the following is not a postulate of Dalton’s atomic theory?
(a) Atoms cannot be created or destroyed.
(b) Atoms of different elements have different sizes, masses and chemical properties.
(c) Atoms of same elements can combine in only one ratio to produce more than one compound.
(d) Atoms are very tiny particles which cannot be divided further.
10. Pick up the wrong pairs/combination
(a) 6.022 x 10²³ molecules of oxygen = 32 g of oxygen
(b) 6.022 x 10²³ ions of sodium = 23 g of Na
(c) 6.022 x 10²³ atoms of C = 24 g of carbon
(d) 6.022 x 10²³ atoms of H = 1 g of H atoms
Answer. 1—(b), 2—(d), 3—(d), 4—(a), 5—(b), 6-(a), 7—(d), 8—(c), 9—(c), 10—(c).

II. Very Short Answer Type Questions
Question 1. Define law of conservation of mass. 
Answer: In a chemical reaction mass can neither be created nor destroyed.
E.g., 2Na + Cl₂ ——–> 2NaCl
2 x 23 + 2 x 35.5 ——> 2(23 + 35.5)

Question 2. Explain law of constant proportion.
Answer: In a chemical substance the elements are always present in definite proportions by mass.
E.g., In water, the ratio of the mass of hydrogen to the mass of oxygen H : O is always 1:8

Question 3. Who coined the term atom?
Answer: John Dalton coined the term atom.

Question 4. Define atom.
Answer: The smallest particle of matter, which can take part in a chemical reaction is called atom.

Question 5. Define molecule.
Answer: The smallest particle of an element or compound which can exist independently is called molecule.

Question 6. Define atomicity.
Answer: The number of atoms constituting a molecule is known as its atomicity.

Question 7. What is atomic mass unit?
Answer: The sum of the atomic masses of all the atoms in a molecule of the substance is expressed.in atomic mass unit. E.g., H₂0 = 1 x 2 + 16 = 18 amu

Question 8. How do atoms exist?
Answer: Atoms exist in the form of atom, molecule or ions.

Question.9. Give the atomicity of phosphorous and nitrogen.
Answer. The atomicity of phosphorus is P₄ i.e., 4.
The atomicity of nitrogen is N₂ i.e., 2.

Question 10. What is an ion?
Answer: Charged atom is called as an ion. The ion can be positively charged called cation or negatively charged called anion.

Question 11. Give one example of cation and anion.
Answer: Cation => Na⁺
Anion => Cl^–

Question 12. Give one difference between cation and anion.
Answer: Cations are positively charged ion.
Anions are negatively charged ion.

Question 13. Give the chemical formula for ammonium sulphate.
Answer: Ammonium sulphate
NH₄⁺ SO₄^2-
Chemical formula —-> (NH₄)₂S0₄.

Question 14. What is Avogadro’s constant?
Answer: The Avogadro’s constant (6.022 x 10²³) is defined as the number of atoms that are present in exactly 12 g of carbon-12.

Question 15. Find the molecular mass of H₂0.
Answer: Molecular mass of H₂0
= (2 x 1) + (16)
= 2 + 16 = 18 u

III. Short Answer Type Questions
Question 1. Give the unit to measure size of atom and give size of hydrogen atom.
Answer: The unit to measure size of atom, is nanometer, size of hydrogen atom is 10^-10m.

Question 2. What is IUPAC, give its one function?
Answer: IUPAC is International Union for Pure and Applied Chemistry. It approves the names of elements.

Question 3. Give the Latin name for sodium, potassium, gold and mercury.
Answer: Sodium —> Natrium, Gold —> Aurum
Potassium —> Kalium, Mercury —> Hydrargyrum

Question 4. What is the ratio by mass of combining elements in H₂0, C0₂ and NH₃?
Answer: H₂O ratio by mass of combining elements 2 : 16 —>1 : 8 (H : O)
C0₂ ratio by mass of combining elements 12 : 32—> 3 : 08 (C : O)
NH₃ ratio by mass of combining elements 14 : 3—>14 : 3 (N : H)

Question 5. Define valency and give the valency for the following elements:
Magnesium, Aluminium, Chlorine and Copper.
Answer: Valency: The combining capacity of an element is called its valency. Valency of the following elements:
Magnesium – 2
Aluminium – 3
Chlorine – 1
Copper – 2

Question 6. What is polyatomic ton? Give one example.
Answer: A group of atoms carrying a charge is known as a polyatomic ion.
E.g., Ammonium – NH₄⁺
Nitrate – N0₃^–

Question 7. Write down the formula for:
Copper nitrate, calcium sulphate and aluminium hydroxide.
Answer: Chemical formula:
Copper nitrate —> Cu(N0₃)
Calcium sulphate —> CaS0₄ Aluminium hydroxide Al(OH)₃

Question 8. What is formula unit mass? How is it different from molecular mass?
Answer: The formula unit mass of a substance is a sum of the atomic masses of all atoms in a formula unit of a compound. The constituent particles of formula unit mass are ions and the constituent particles of molecular mass are atoms.

Question 9. Find the number of moles in the following:
(i) 50 g of H₂O
(ii) 7 g of Na
Answer: Number of moles in
(i) Molar mass of H₂O = 18 g
Given mass of H₂O = 50 g

Question 10. Find the number of atoms in the following:
(i) 0.5 mole of C atom
(ii) 2 mole of N atom
Answer: (i) 0.5 mole of C atom:
Number of atoms in 1 mole of C atom = 6.022 x 10²³ atoms
Number of atoms in 0.5 mole of C atom = 6.022 x 10²³ x 0.5
= 3.011 x 10²³ atoms
(ii) 2 mole of N atom:
Number of atoms in 1 mole of N atom = 6.022 x 10²³ atoms
Number of atoms in 2 mole of N atom = 6.022 x 2 x 10²³
= 1.2044 x 10²⁴ atoms

Question 11. Find the mass of the following:
(i) 6.022 x 10²³ number of O₂ molecules
(ii) 1.5 mole of CO₂ molecule
Answer: (i) 6.022 x 10²³ number of 02 molecules:
Mass of 1 mole of O₂ molecule = 6.022 x 10²³ molecules = 32 g
(ii) 1.5 mole of CO₂ molecule:
Mass of 1 mole of C0₂ molecule = 6.022 x 10²³ molecules = 44 g
Mass of 1.5 mole C0₂ molecule = 44 x 1.5 = 66 g

Question 12. Show the relationship between mole, Avogadro number and mass.
Answer:

Question 13. What are the rules for writing the symbol of an element?
Answer: IUPAC —> International Union of Pure and Applied Chemistry approves name of elements.
Symbols are the first one or two letters of the element’s name in English. The first letter of a symbol is always written as a capital letter (upper case) and the second letter as a small letter (lower case).
e.g., Hydrogen —> H Helium —> He
Some symbols are taken from the names of elements in Latin, German or Greek.
e.g., Symbol of iron is Fe, its Latin name is Ferrum.
Symbol of sodium is Na, its Latin name is Natrium.

Question 14. Explain relative atomic mass and relative molecular mass.
Answer: Relative atomic mass: It can be defined as the number of times one atom of given element is heavier than 1/12 th of the mass of an atom of carbon-12. Relative Molecular Mass: It is defined as the number of times one molecule
of a substance or given element is heavier than 1/12 th of the mass of one atom of carbon-12.

Question 15. The formula of carbon-dioxide is CO₂. What information do you get from this formula? 
Answer: (i) CO₂ represents carbon-dioxide.
(ii) CO₂ is one molecule of carbon-dioxide.
(iii) CO₂ is one mole of carbon-dioxide i.e., it contains 6.022 x 10²³ molecules of carbon dioxide.
(iv) CO₂ contains 1 atom of carbon and two atoms of oxygen.
(v) CO₂ represents 44 g of molar mass.

Question.16. State 3 points of difference between an atom and an ion.
Answer.

Question 17. Calculate the formula unit mass of NaCl and CaCl₂.
(Na = 23, Cl = 35.5, Ca = 40)
Answer: Formula unit mass of NaCl = 23 + 35.5
= 58.5 u
Formula unit mass of CaCl₂ = 40 + (2 x 35.5)
= 40 + 71 = 111 u

Question 18. The ratio by mass for hydrogen and oxygen in water is given as 1 : 8 respectively. Calculate the ratio by number of atoms for a water molecule.
Answer: The ratio by number of atoms for a water molecule are:

Thus, the ratio by number of atoms for water is H : O = 2 : 1.

Question 19. Write down the chemical formula for the following compounds:
(a) Aluminium carbonate
(b) Calcium sulphide
(c) Zinc carbonate
(d) Copper phosphate
(e) Magnesium bicarbonate
(f) Aluminium hydroxide.
Answer: The chemical formula are:

Question 20. Give the atomicity of the following compounds:
(a) Ca(OH)₂ (d) H₂S0₄
(b) Mg(HC0₃)₂ (e) Al₂(S0₄)₃
(c) Cu₂0. (f) MgCl₂
Answer: The atomicity of the molecules are:

Question 21. Explain the difference between 20, 0₂ and 0₃.
Answer: 2O —> It represents 2 atoms of oxygen (cannot exist independently).
O₂ —> It represents one molecule of oxygen (made up of 2 atom) can exist freely.
O₃ —> It represents one molecule of ozone (made up of 3 atoms) it can exist independently.

IV. Long Answer Type Questions
Question 1. (a) How do atoms exist?
(b) What is atomicity?
(c) What are polyatomic ions?
Answer: (a) Atoms of some elements are not able to exist independently. For such elements atoms form molecules and ions. In case of metals and inert gases atoms can exist independently.

(b) The number of atoms constituting a molecule is known as its atomicity.
E.g.,O₃ —> atomicity is 3
O₂ —> atomicity is 2
(c) Polyatomic ions: When more than two atoms combine together and act like an atom with a charge on it is called polyatomic ion.
E.g., OH^–, N0₃^–, NH₄⁺

Question 2. Calculate
(a) the mass of one atom of oxygen
(b) the mass of one molecule of oxygen
(c) the mass of one mole of oxygen gas
(d) the mass of one ion of oxygen
(e) the number of atoms in 1 mole of oxygen molecule
Answer:

Question 3. What is meant by atomic mass, gram atomic mass of an element? Why is the mass have different expressions i.e., ‘u’ and ‘g’?
Answer: The atoms are very tiny and their individual mass cannot be calculated as it is negligible. Hence the mass of atoms is expressed in units with respect to a fixed standard. Initially hydrogen atom with mass 1 was taken as standard unit by Dalton. Later, it was replaced by oxygen atom (0=16). But due to the isotopes the masses were found in fractions instead of whole number. Hence, carbon (C=12) isotope was taken as standard unit and was universally accepted.
The atomic mass unit is equal to one twelfth (1/12) the mass of an atom of carbon-12, its unit is u.
Gramatomic mass: When the atomic mass of an element is expressed in grams, it is called the gramatomic mass of the element.
The mass of atoms, molecules is expressed in ‘u’ and the mass of moles i.e., molar mass is expressed in g.

Question 4. Define a mole. Give the significance of the mole.
Answer: Mole-One mole of any species (atoms, molecules, ions or particles) is that quantity or number having a mass equal to its atomic or molecular mass in grams.
1 mole = 6.022 x 10²³ in number (atoms, molecules, ions or particles)
Significance of the mole
1. A mole gives the number of entities present i.e, 6.022 x 10²³ particles of the substance.
2. Mass of 1 mole is expressed as M grams.

V. Activity-Based Questions

• Take one of the following sets X and Y of chemicals—
  X                                      –               Y
  (i) Copper sulphate – Sodium carbonate
  (ii) Barium chloride – Sodium sulphate
  (iii) Lead nitrate – Sodium chloride
  
• Prepare separately 95% solution of any one pair of substances listed under X and Y in water.
• Take little amount of solution of Y in a conical flask and some solution of X in an ignition tube.
• Hang the ignition tube in the flask carefully; see that the solutions do not get mixed.
• Put a cork on the flask as shown in figure.
• Weigh the flask with its contents carefully.
• Now tilt and swirl the flask, so that the solutions X and Y get mixed.
• Weigh again.
• What happens in the reaction flask?
• Do you think that a chemical reaction has taken place?
• Why should we put a cork on the mouth of the flask?
• Does the mass of the flask and its contents change?

Answer:

• In the reaction flask both the reactants combined to give new products.
• Yes.
• We should put a cork on the mouth of the flask so that no other gases in the air combine or get added into the reaction, neither any gas formed in the reaction should escape.
• No. The mass of the flask before and after reaction do not change.

VI. Value – Based Questions
Question 1. A customer buys a gold jewellery, he is told that the jewellery has 90% gold and the rest copper. He is given a bill which amounts 100% charges of gold. The customer refuses to pay the bill for 100% gold but brings it to 90% gold amount and settles the bill.
(a) How many atoms of gold are present in 1 gram of gold?
(b) What is the ratio of gold and copper in the jewellery?
(c) What value of customer is reflected in the above statement?
Answer: