Chapter 3 Atoms And Molecules

Question 1. Which of the following correctly represents 360 g of water?

(i) 2 moles of H$_2$O

(ii) 20 moles of water

(iii) $6.022 \times 10^{23}$ molecules of water

(iv) $1.2044 \times 10^{25}$ molecules of water

(a) (i)

(b) (i) and (iv)

(c) (ii) and (iii)

(d) (ii) and (iv)

Question 2. Which of the following statements is not true about an atom?

(a) Atoms are not able to exist independently

(b) Atoms are the basic units from which molecules and ions are formed

(c) Atoms are always neutral in nature

(d) Atoms aggregate in large numbers to form the matter that we can see, feel or touch

Question 3. The chemical symbol for nitrogen gas is

(a) Ni

(b) N$_2$

(c) N$^+$

(d) N

Question 4. The chemical symbol for sodium is

(a) So

(b) Sd

(c) NA

(d) Na

Question 5. Which of the following would weigh the highest?

(a) 0.2 mole of sucrose (C$_{12}$ H$_{22}$ O$_{11}$)

(b) 2 moles of CO$_2$

(c) 2 moles of CaCO$_3$

(d) 10 moles of H$_2$O

Question 6. Which of the following has maximum number of atoms?

(a) 18g of H$_2$O

(b) 18g of O$_2$

(c) 18g of CO$_2$

(d) 18g of CH$_4$

Question 7. Which of the following contains maximum number of molecules?

(a) 1g CO$_2$

(b) 1g N$_2$

(c) 1g H$_2$

(d) 1g CH$_4$

Question 8. Mass of one atom of oxygen is

(a) $\frac{16}{6.023 \times 10^{23}}$ g

(b) $\frac{32}{6.023 \times 10^{23}}$ g

(c) $\frac{1}{6.023 \times 10^{23}}$ g

(d) 8u

Question 9. 3.42 g of sucrose are dissolved in 18g of water in a beaker. The number of oxygen atoms in the solution are

(a) $6.68 \times 10^{23}$

(b) $6.09 \times 10^{22}$

(c) $6.022 \times 10^{23}$

(d) $6.022 \times 10^{21}$

Question 10. A change in the physical state can be brought about

(a) only when energy is given to the system

(b) only when energy is taken out from the system

(c) when energy is either given to, or taken out from the system

(d) without any energy change

Question 11. Which of the following represents a correct chemical formula? Name it.

(a) CaCl

(b) BiPO$_4$

(c) NaSO$_4$

(d) NaS

Question 12. Write the molecular formulae for the following compounds

(a) Copper (II) bromide

(b) Aluminium (III) nitrate

(c) Calcium (II) phosphate

(d) Iron (III) sulphide

(e) Mercury (II) chloride

(f) Magnesium (II) acetate

Question 13. Write the molecular formulae of all the compounds that can be formed by the combination of following ions

Cu$^{2+}$, Na$^+$, Fe$^{3+}$, C1$^-$, SO$_4^{2-}$, PO$_4^{3-}$

Question 14. Write the cations and anions present (if any) in the following compounds

(a) CH$_3$COONa

(b) NaCl

(c) H$_2$

(d) NH$_4$NO$_3$

Question 15. Give the formulae of the compounds formed from the following sets of elements

(a) Calcium and fluorine

(b) Hydrogen and sulphur

(c) Nitrogen and hydrogen

(d) Carbon and chlorine

(e) Sodium and oxygen

(f) Carbon and oxygen

Question 16. Which of the following symbols of elements are incorrect? Give their correct symbols

(a) Cobalt CO

(b) Carbon c

(c) Aluminium AL

(d) Helium He

(e) Sodium So

Question 17. Give the chemical formulae for the following compounds and compute the ratio by mass of the combining elements in each one of them. (You may use appendix-III).

(a) Ammonia

(b) Carbon monoxide

(c) Hydrogen chloride

(d) Aluminium fluoride

(e) Magnesium sulphide

Question 18. State the number of atoms present in each of the following chemical species

(a) CO$_3^{2-}$

(b) PO$_4^{3-}$

(c) P$_2$O$_5$

(d) CO

Question 19. What is the fraction of the mass of water due to neutrons?

Question 20. Does the solubility of a substance change with temperature? Explain with the help of an example.

Question 21. Classify each of the following on the basis of their atomicity.

(a) F$_2$

(b) NO$_2$

(c) N$_2$O

(d) C$_2$H$_6$

(e) P$_4$

(f) H$_2$O$_2$

(g) P$_4$O$_{10}$

(H) O$_3$

(i) HCl

(j) CH$_4$

(k) He

(l) Ag

Question 22. You are provided with a fine white coloured powder which is either sugar or salt. How would you identify it without tasting?

Question 23. Calculate the number of moles of magnesium present in a magnesium ribbon weighing 12 g. Molar atomic mass of magnesium is 24g mol$^{-1}$.

Question 24. Verify by calculating that

(a) 5 moles of CO$_2$ and 5 moles of H$_2$O do not have the same mass.

(b) 240 g of calcium and 240 g magnesium elements have a mole ratio of 3:5.

Question 25. Find the ratio by mass of the combining elements in the following compounds. (You may use Appendix-III)

(a) CaCO$_3$

(d) C$_2$H$_5$OH

(b) MgCl$_2$

(e) NH$_3$

(c) H$_2$SO$_4$

(f) Ca(OH)$_2$

Question 26. Calcium chloride when dissolved in water dissociates into its ions according to the following equation.

CaCl$_2$ (aq) $\rightarrow$ Ca$^{2+}$ (aq) + 2Cl$^-$ (aq)

Calculate the number of ions obtained from CaCl$_2$ when 222 g of it is dissolved in water.

Question 27. The difference in the mass of 100 moles each of sodium atoms and sodium ions is 5.48002 g. Compute the mass of an electron.

Question 28. Cinnabar (HgS) is a prominent ore of mercury. How many grams of mercury are present in 225 g of pure HgS? Molar mass of Hg and S are 200.6 g mol$^{-1}$ and 32 g mol$^{-1}$ respectively.

Question 29. The mass of one steel screw is 4.11g. Find the mass of one mole of these steel screws. Compare this value with the mass of the Earth ($5.98 \times 10^{24}$kg). Which one of the two is heavier and by how many times?

Question 30. A sample of vitamic C is known to contain $2.58 \times 10^{24}$ oxygen atoms. How many moles of oxygen atoms are present in the sample?

Question 31. Raunak took 5 moles of carbon atoms in a container and Krish also took 5 moles of sodium atoms in another container of same weight. (a) Whose container is heavier? (b) Whose container has more number of atoms?

Question 32. Fill in the missing data in the Table 3.1

Table 3.1

Question 33. The visible universe is estimated to contain $10^{22}$ stars. How many moles of stars are present in the visible universe?

Question 34. What is the SI prefix for each of the following multiples and submultiples of a unit?

(a) $10^3$

(b) $10^{-1}$

(c) $10^{-2}$

(d) $10^{-6}$

(e) $10^{-9}$

(f) $10^{-12}$

Question 35. Express each of the following in kilograms

(a) $5.84 \times 10^{-3}$ mg

(b) 58.34 g

(c) 0.584g

(d) $5.873 \times 10^{-21}$g

Question 36. Compute the difference in masses of $10^3$ moles each of magnesium atoms and magnesium ions.

(Mass of an electron = $9.1 \times 10^{-31}$ kg)

Question 37. Which has more number of atoms?

100g of N$_2$ or 100 g of NH$_3$

Question 38. Compute the number of ions present in 5.85 g of sodium chloride.

Question 39. A gold sample contains 90% of gold and the rest copper. How many atoms of gold are present in one gram of this sample of gold?

Question 40. What are ionic and molecular compounds? Give examples.

Question 41. Compute the difference in masses of one mole each of aluminium atoms and one mole of its ions. (Mass of an electron is $9.1 \times 10^{-28}$ g). Which one is heavier?

Question 42. A silver ornament of mass ‘m’ gram is polished with gold equivalent to 1% of the mass of silver. Compute the ratio of the number of atoms of gold and silver in the ornament.

Question 43. A sample of ethane (C$_2$H$_6$) gas has the same mass as $1.5 \times 10^{20}$ molecules of methane (CH$_4$). How many C$_2$H$_6$ molecules does the sample of gas contain?

Question 44. Fill in the blanks

(a) In a chemical reaction, the sum of the masses of the reactants and products remains unchanged. This is called ————.

(b) A group of atoms carrying a fixed charge on them is called ————.

(c) The formula unit mass of Ca$_3$ (PO$_4$)$_2$ is ————.

(d) Formula of sodium carbonate is ———— and that of ammonium sulphate is ————.

Question 45. Complete the following crossword puzzle (Fig. 3.1) by using the name of the chemical elements. Use the data given in Table 3.2.

Table 3.2

Question 46. (a) In this crossword puzzle (Fig 3.2), names of 11 elements are hidden. Symbols of these are given below. Complete the puzzle.

1. Cl

2. H

3. Ar

4. O

5. Xe

6. N

7. He

8. F

9. Kr

10. Rn

11. Ne

(b) Identify the total number of inert gases, their names and symbols from this cross word puzzle.

Question 47. Write the formulae for the following and calculate the molecular mass for each one of them.

(a) Caustic potash

(b) Baking powder

(c) Lime stone

(d) Caustic soda

(e) Ethanol

(f) Common salt

Question 48. In photosynthesis, 6 molecules of carbon dioxide combine with an equal number of water molecules through a complex series of reactions to give a molecule of glucose having a molecular formula C$_6$ H$_{12}$ O$_6$. How many grams of water would be required to produce 18 g of glucose? Compute the volume of water so consumed assuming the density of water to be 1 g cm$^{-3}$.