1. Calculate molecular mass for the following:
a)Na2CO3 b)MgCl2 c)NaNO3 d)CuSO4 e)H2SO4
2.Give the postulates of Dalton’s atomic theory
3. Give *symbol and valency* of : Potassium, Barium,
Aluminium, Calcium, Cobalt, Fluorine, Lead, Zinc,
Iodine, Sulphide.
4.Write the names of the following compounds :
(a) NiS
(b) Mg(NO3)2
(c) Na2SO4
(d) Al(NO3)3 (e) K3PO4
(f) Ca3N2
5. Explain about Rutherford's alpha particle scattering experiment.
6. Draw Bohr's model of an atom with four shells. Name the shells and no.of electrons.
Answers
Explanation:
In a reaction 5.3 g of sodium carbonate reacted with 6 g of ethanoic acid. The products were 2.2 g of carbon dioxide, 0.9 g water and 8.2 g of sodium ethanoate. Show that these observations are in agreement with the law of conservation of mass carbonate.
Ans.
Sodium carbonate + Ethanoic acid → Sodium ethanoate + Carbon dioxide + Water
5.3 g + 6 g → 8.2 g + 2.2 g + 0.9 g
LHS RHS
11.3 g = 11.3 g
(Mass of reactant) (Mass of product)
This shows, that during a chemical reaction mass of reactact = mass of product.
2. Hydrogen and oxygen combine in the ratio of 1 : 8 by mass to form water. What mass of oxygen gas would be required to react completely with 3 g of hydrogen gas?
Ans. Ratio of H : O by mass in water is:
Hydrogen : Oxygen → H2O
1 : 8 = 3 : x
x = 8 × 3
∴ 24 g of oxygen gas would be required to react completely with 3 g of hydrogen gas.
3. Which postulate of Dalton's atomic theory the result of the law of conservation of mass?
Ans. The postulate of Dalton's atomic theory that is the result of the law of conservation of mass is-the relative number and kinds of atoms are constant in a given compound. Atoms cannot be created nor destroyed in a chemical reaction.
4. Which postulate of Dalton's atomic theory can explain the law of definite proportions?
Ans. The relative number and kinds of atoms are constant in a given compound.
NCERT TEXTBOOK PAGE 35
1. Define the atomic mass unit.
Ans. One atomic mass unit is equal to exactly one-twelfth (1/12th) the mass of one atom of carbon-12. The relative atomic masses of all elements have been found with respect to an atom of carbon-12.
2. Why is it not possible to see an atom with naked eyes?
Ans. Atom is too small to be seen with naked eyes. It is measured in nanometres.
1 m = 109 nm
NCERT TEXTBOOK PAGE 35
1. Write down the formulae of
(i) Sodium oxide
(ii) Aluminium chloride
(iii) Sodium sulphide
(iv) Magnesium hydroxide
Ans. The formulae. are
(i) Formula bf Sodium Oxide
Symbol → Na O
Charge → +1 –2
Formula → Na2O
(iii) Formula of Sodium Oxide
Symbol → Na S
Charge → + 1 –2
Formula → Na2S
(ii) Formula of aluminium chloride
Symbol → Al Cl
Charge → +3 –1
Formula → A1C13
(iv) Formula of magnesium hydroxide
Symbol → Mg OH
Charge 1
Formula → Mg(OH)2
2. Write down the names of compounds represented btthe following formulae:
(i) Al2(SO4)3 (ii) CaCl2 (iii) K2SO4 (iv) KNO3
(v) CaCO3
Ans. (i) A12(SO4)3 → Aluminium sulphate
(ii) CaC12 → Calcium chloride
(iii) K∴SO4 → Potassium sulphate
(iv) KNO3 → Potassium nitrate
(v) CaCO3 → Calcium carbonate
3. What is meant by the term chemical formula?
Ans. The chemical formula of the compound is a symbolic representation of its composition, e.g., chemical formula of sodium chloride is NaCl.
4. How many atoms are present in a
(i) H2S molecule and
(ii) PO43– ion?
Ans. (i) H2S → 3 atoms are present
(ii) PO43– → 5 atoms are present
NCERT TEXTBOOK PAGE 40
1. Calculate the molecular masses of H2, O2, C12, CO2, CH4, C2H6, C2H4, NH3, CH3OH.
Ans. The molecular masses are:
H2 ⇒ 1 × 2 → 2u
O2⇒ 16 × 2 → 32u
Cl2 ⇒ 35.5 × 2 → 71 u
CO2 ⇒ 1 × 12 + 2 × 16 = 12 +32 = 44 u
CH4 ⇒ 1 × 12 + 4 × 1 = 16 u
C2H6 ⇒�n2 × 12 + 6 × 1 = 30 u
C2H4 ⇒ (2 × 12) + (4 × 1) = 28 u
NH3 ⇒ (1 × 14) + (3 × 1) = 17 u
CH3OH ⇒ 12 + (3 × 1) + 16 + 1 = 32 u
2. Calculate the formula unit masses of ZnO, Na2O, K2Co3 given atomic masses of Zn=65 u, Na = 23 u, K = 39 u, C = 12u, and O = 16 u.
Ans. The formula unit mass of
(i) ZnO = 65 u + 16 u =.81 u
(ii) Na2O = (23 u × 2) + .16 u : = 46u+ 161.u.
= 62 u
(iii) K2CO3 = (39 u × 2) + 12 u + 16 u × 3
= 75 u + 12u = 48u = 138u
NCERT TEXTBOOK PAGE 42
1. If one mole of carbon atoms weigh 12 grams, what is the mast (in grams) of 1 atom of carbon?
Ans. 1 mole of carbon atoms 6.022 × 1023 atoms = 12 g
Mass of 1 atom = ?
∴ Mass of 1 atom of carbon
=1.99 × 10–23 g
2. Which has more number of atoms, 100 grams of sodium or 100 grams of iron (given atomic mass of Na = 23 u, Fe = 56 u)?
Ans.