Question:
Give one major drawback of Dalton's atomic theory of matter.
Answer:
One of the major drawbacks of Dalton's atomic theory of matter is that atoms were thought to be indivisible (which cannot be divided). We now know that under special circumstances, atoms can be further divided into still smaller particles called electrons, protons and neutrons. So, atoms are themselves made up of three particles : electrons, protons and neutrons.
Atoms and Molecules
Q 1.
Fill in the blanks:
The atomic mass of sodium is 23. The gram atomic mass of sodium is _________.
Q 2.
What is the chemical symbol for iron?
Q 3.
Define molecule. What are its important properties?
Q 4.
(i) State the law of constant proportions.
(ii) Show that water illustrates the law of constant proportions.
Q 5.
Fill in the blanks:
The chemical symbol of mercury is _________.
Q 6.
Fill in the blanks:
One mole of water contains ______________ molecules.
Q 7.
Magnesium is two times heavier than C-12 atom, what shall be the mass of Mg atom in terms of atomic mass units? (Given mass of C-12 atom = 12u)
Q 8.
Name one element each which forms diatomic and tetra atomic molecule.
Q 9.
Fill in the blanks:
The mass of 5 moles of ammonia (NH
3) is __________.
Q 10.
Name the international organization who approves names of elements.
Q 11.
Write the chemical symbols of the following:
(i) Gold
(ii) Iron
(iii) Chlorine
(iv) Mercury
Q 12.
Give four examples of diatomic molecules.
Q 13.
What is gram-atomic mass of an element?
Q 14.
Define 'formula mass' of a compound.
Q 15.
Give the names of the elements present in the following compounds.
(a) Quick lime
(b) Hydrogen bromide
(c) Baking powder
(d) Potassium sulphate.
Q 16.
Calculate the number of molecules of phosphorus (P
4) present in 31 gram of phosphorus.
Q 17.
How many atoms are there in 0.25 mole of hydrogen ?
Q 18.
Which postulate of Dalton’s atomic theory is the result of the law of conservation of mass?
Q 19.
Fill in the blanks:
According to law of definite proportions, in a chemical substance the elements are always present in __________ proportions by mass.
Q 20.
What are ionic compounds?
Q 21.
Convert 12 g of oxygen gas into moles.
Q 22.
What is the mass of 5 moles of sodium carbonate (Na
) ?(Atomic masses : Na = 23 u ; C = 12 u ; O = 16 u)
Q 23.
Which postulate of Dalton’s atomic theory can explain the law of definite proportions?
Q 24.
Write down the formulae of
(i) sodium oxide
(ii) aluminium chloride
(iii) sodium suphide
(iv) magnesium hydroxide
Q 25.
What is gram-molecular mass of a substance?
Q 26.
Calculate the number of aluminium ions present in 0.051 g of aluminium oxide.
(
Hint: The mass of an ion is the same as that of an atom of the same element. Atomic mass of Al = 27 u)
Q 27.
(a) What is meant by the 'molar mass'of a substance ? State the unit in which molar mass usually expressed.
(b) Calulate the molar masses of the following substances. Write the results with proper units
(1) Ozone molecule, O
Q 28.
Explain with example that law of conservation of mass is valid for chemical reactions.
Q 29.
Write the chemical formulae of the following. Also identify the ions present.
(a) Magnesium chloride
(b) Calcium oxide
(c) Copper nitrate
(d) Aluminium chloride
(e) Calcium carbonate.
Q 30.
How many moles are there in 4.6 gms of Sodium(Na)?
Q 31.
Who established the two important laws of chemical combinations?
Q 32.
What are the postulates of Dalton's atomic theory?
Q 33.
Fill in the blanks:
Mass of 2 Hydrogen atoms is __________.
Q 34.
Based on type of substance, how molecules are classified?
Q 36.
Write down the names of compounds represented by the following formulae:
(i) Al
2(SO
4)
3 (ii) CaCl
2 (iii) K
2SO
4 (iv) KNO
3 (v) CaCO
3
Q 37.
Define mole. What is its significance?
Q 38.
What is the mass of
(a) 1 mole of nitrogen atoms?
(b) 4 moles of aluminium atoms (Atomic mass of aluminium = 27)?
(c) 10 moles of sodium sulphite (Na
2SO
3)?
Q 39.
Write the formulae of the following compounds. Also name the elements present in them.
(a) Water
(b) Ammonia
(c) Methane
(d) Sulphur dioxide
(f) Ethanol
Q 40.
Which element has the smallest atom in size?
Q 42.
Give examples of triatomic molecules.
Q 43.
Calculate the formula unit masses of ZnO, Na
2O, K
2CO
3, given atomic masses of Zn = 65 u, Na = 23 u, K = 39 u, C = 12 u, and O = 16 u.
Q 44.
If one mole of carbon atoms weighs 12 gram, what is the mass (in gram) of 1 atom of carbon?
Q 45.
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)?
Q 46.
Find out number of atoms in 15 moles of He.
Q 47.
Write down the formulae for the following compounds :
(a) Calcium oxide
(b) Magnesium hydroxide
Q 48.
State Law of constant proportions. Explain with an example.
Q 49.
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?
Q 50.
When 3.0 g of carbon is burnt in 8.00 g oxygen, 11.00 g of carbon dioxide is produced. What mass of carbon dioxide will be formed when 3.00 g of carbon is burnt in 50.00 g of oxygen? Which law of chemical combination will govern your answer?
