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Worksheets11 chem liquid and solids
Total questions: 63
Worksheet time: 5hrs 15mins
Name
Class
Date
1.
1. Isotopes differ in:
a)
Properties with respect to their mass number
b)
Properties with respect to their proton number
c)
Isotopes don’t differ as they have same number of electrons and protons
d)
All of the above
2.
2. Isotopes are:
a)
Chemically similar
b)
Physically dissimilar
c)
Chemically dissimilar
d)
Both a and b
3.
3. Ionization energy depends upon:
a)
Atomic/ionic radii
b)
Proton to electron ratio
c)
Shielding effect
d)
All of the above
4.
4. 2nd ionization energy of Mg is higher than the first because:
a)
Metallic character of Mg+1 is less than that of Mg
b)
Nuclear pull for Mg+1electron is more than that for the Mg atom
c)
Size of Mg+1 is greater than Mg+2
d)
Both a and b
5.
5. With the increasing atomic number, ionization energy increases along a period because:
a)
No change in shielding effect along a period
b)
Nuclear pull increases with the increase in the number of protons
c)
Atomic/ionic size decreases along a period
d)
All of the above
6.
6. The correct set of four quantum numbers for the valence electron of rubidium (Z = 37) is:
a)
n = 5, 1 = 0, m = 0 and s = +1/2
b)
n = 5, 1 = 1, m = 1 and s = +1/2
c)
n = 5, 1 = 1, m = 0 and s = +1/2
d)
n = 6, 1 = 0, m = 0 and s = +1/2
7.
7. The electron configuration of K(19) is:
a)
1s3 2s3 2p5 3s3 3p5
b)
1s2 2s2 2p6 3s2 2p5 4s2
c)
1s2 2s2 2p6 3s2 3p6 4s1
d)
None of the above
8.
8. The number of d-electrons in Fe+2 (Z=26) is not equal to:
a)
p electrons in Ne (Z = 10)
b)
d electrons in Fe (Z = 26)
c)
s electrons in Mg (Z = 12)
d)
p electrons in Ar (Z = 17)
9.
9. The electronic configuration of an element is 1s2 2s2 2p3. This represents a/an:
a)
Ground state
b)
Hybridized state
c)
Excited-state
d)
Molecular state
10.
10. In which of the following, all have the same number of electrons:
a)
Cl–, Br– and I–
b)
H–, H and H+
c)
F–, Ne and Na+
d)
Li+, Na+ and K+
11.
11. Identify the correct order of increasing energy:
a)
1s < 2s < 3s
b)
2s > 3s > 1s
c)
1s > 2s > 3s
d)
None of the above
12.
12. The shapes of s orbitals is circular and their size:
a)
Increase with the increase in principal quantum number
b)
Decrease with the increase in principal quantum number
c)
Remains the same with the change in principal quantum number
d)
None of the above
13.
13. The place between the two orbitals is called:
a)
Free zone
b)
Nodal surface
c)
Neutral zone
d)
Resonance area
14.
14. Shapes of p orbitals:
a)
Circular
b)
Dumb-bell
c)
Elliptical
d)
Complex
15.
15. The correct number of degenerate orbitals:
a)
s = 2, p = 6, d = 10, f = 14
b)
s = 3, p = 1, d = 5, f = 7
c)
s = 1, p = 3, d = 5, f = 7
d)
s = 1, p = 3, d = 7, f = 5
16.
16. The ion that is iso-electronic with CI atom is:
a)
CN–
b)
O+2
c)
N+2
d)
O–2
17.
17. Which of the following particles would on losing an electron has its outermost p-orbital as half-filled?
a)
Nitrogen atom
b)
O+ ion
c)
P-1 ion
d)
S+1 ion
18.
18. The ionic specie having more electrons than neutrons is:
a)
Mg+2
b)
O2–
c)
Na+
d)
F-1
19.
19. Which pair of electrons of elements will have the same chemical properties?
a)
2, 24
b)
2, 4
c)
13, 22
d)
3, 11
20.
20. An orbital which is spherically symmetrical is:
a)
p-orbital
b)
s-orbital
c)
d-orbital
d)
f-orbital
21.
21. The value of e/m for the electron is:
a)
1.7588 x 1011 kg C-1
b)
1.7588 x 10-11 Ckg-1
c)
1.7588 x 1011 kg C-1
d)
1.7588 x 1011 Ckg-1
22.
22. A nodal plane in an orbital is the plane where the electron density is:
a)
Maximum
b)
Negetive
c)
Zero
d)
Positive
23.
23. How many times the mass of neutrons is greater than the mass of an electron?
a)
1480
b)
2000
c)
1840
d)
1200
24.
24. The mass of an oxygen atom is:
a)
2.657 x 10-23g
b)
2.657 x 1023
c)
16g
d)
32g
25.
25. The mass of a neutron is:
a)
Same as that of proton
b)
A little bit smaller than that of proton
c)
Slightly more than that of proton
d)
Slightly less than that of proton
26.
26. The smallest charge of electricity which has been measured on any particle is:
a)
Charge on the positive ray of He gas
b)
Charge on particles
c)
Charge on any droplet in Millikan Experiment
d)
Charge on an electron
27.
27. Which of the following has highest ionization energy value?
a)
Li
b)
Be
c)
H
d)
He
28.
28. Greater shielding effect corresponds to ionization energy value:
a)
Greater
b)
Lesser
c)
Remain the same
d)
No effect
29.
29. The mass of a proton is:
a)
9.1 x 10-10 g
b)
9.1 x 10-18 g
c)
1.672 x 10-27 kg
d)
9.1 x 10-31 kg
30.
30. Which group shows the abnormal behavior in trend of ionization energy in periods?
a)
Group I-A
b)
Group III-A
c)
Group-VI-A
d)
Both b and c
31.
Q. 1. I heard Islamian genius saying that glass must be a super cooled liquid. The reason that he might have in his mind is that glass has
a)
a. definite volume
b)
b. definite shape
c)
c. crystalline structure
d)
d. no crystalline structure
32.
Q. 2. Some substances are good conductors of electricity in both the solid and liquid states. These substances are generally
a)
a. ionic substances
b)
b. metallic substances
c)
c. molecular solids
d)
d. covalent network solids
33.
Q. 3. Air can be distilled fractionally because the constituents of the air
a)
a. can be liquefied
b)
b. have different boiling points
c)
c. are gases at room temperature
d)
d. have different densities
34.
Q. 4. There are three different substances, Argon, Hydrochloric acid, and Hydroiodic acid. The correct sequence in which the boiling point increases is
a)
a. Ar < HCI < HI
b)
b. HI > HCI > Ar
c)
c. HCI < HI < Ar
d)
d. HI > Ar > HCI
35.
Q. 5. A student put two eggs A and B in HCI solution. After 5 minutes he took them out for weighing but egg dropped in water accidentally. The student was able to take it out after 30 minutes. He weighed it. Its weight was 40.33 grams. Weight of egg "B" was also 40.33 grams. Islamian genius told him that if both eggs have been dropped in water, the weight of egg "B" would have been
a)
a. greater than that of egg "A"
b)
b. less than that of egg "A"
c)
c. equal to that of egg "A"
d)
d. unaffected instead
36.
Q. 6. Keeping in mind different factors which affect the melting point of a substance, the compound having the highest melting point among the following is
a)
a. NaCI
b)
b. RbCI
c)
c. LiCI
d)
d. CsCI
37.
Q. 7. Islamian genius told his followers that in a crystal the atoms are located at the position of
a)
a. zero potential energy
b)
b. infinite potential energy
c)
c. maximum potential energy
d)
d. minimum potential energy
38.
Q. 8. Keeping in mind the concept of charge density, the compound having the highest lattice energy is
a)
a. KCI
b)
b. MgO
c)
c. LiBr
d)
d. NaF
39.
Q. 9. Meniscus is the shape of the surface of a liquid in a cylindrical container. It may be concave, convex or plane. For molten metals
a)
a. meniscus is concave
b)
b. meniscus is convex
c)
c. meniscus is plane
d)
d. meniscus may be concave or convex depending on the nature of the metal
40.
Q. 10. All of the following substances are crystalline except
a)
a. Ice
b)
b. Carbon (diamond)
c)
c. Sucrose
d)
d. Plastic
41.
Q. 11. All of the following have cleavage planes except
a)
a. ionic crystals
b)
b. covalent crystals
c)
c. molecular crystals
d)
d. metallic crystals
42.
Q. 12. Coordination number of Na+ in NaCI is
a)
a. 1
b)
b. 4
c)
c. 2
d)
d. 6
43.
Q. 13. For a crystal system a b c and the example for this crystal system is
a)
a. CuSO4. 5H2O
b)
b. Na2B4O7. 10H2O
c)
c. ZnSO4. 7H2O
d)
d. BaSO4. 4H2O
44.
Q. 14. A student said I will preserve my father's dead body in a time capsule for 1000 years. Islamian genius told him that the atmosphere of the capsule must contain
a)
a. O2
b)
b. SO2
c)
c. CO2
d)
d. Ar
45.
Q. 15. All of the following have crystals except
a)
a. diamond
b)
b. NaCI
c)
c. KBr
d)
d. CdS
46.
Q. 16. Kerosene is liquid at room temperature due to
a)
a. hydrogen bonding
b)
b. organic nature
c)
c. dipole-dipole forces
d)
d. molecular size
47.
Q. 17. All of the following are network solids except
a)
a. SiO2
b)
b. Graphite
c)
c. S8
d)
d. Diamond
48.
Q. 18. Honey contains glucose and fructose along with some other ingredients, it has greater viscosity due to
a)
a. hydrogen bonding
b)
b. irregular shape of the molecules
c)
c. irregular shape of the molecules and strong intermolecular forces
d)
d. greater molecular size
49.
Q. 19. Boiling point of phosphine (PH3) is -87.8 oC while that of silane (SiH4) is -111 oC. Phosphine has a greater boiling point because
a)
a. dipole moment of PH3 is greater than that of SiH4
b)
b. PH3 has greater molecular size
c)
c. Molecular weight of SiH4 is less than that of PH3
d)
d. Actually the boiling of SiH4 is greater than that of PH3
50.
Q. 20. Rate of evaporation of petrol is greater than that of water at room temperature because
a)
a. petrol molecules do not have any hydrogen bond
b)
b. petrol is an organic compound
c)
c. water molecules have a small size
d)
d. petrol molecules have a greater size
51.
Q. 21. Substance having the highest boiling point among the following is
a)
a. HF
b)
b. HCI
c)
c. Br2
d)
d. HBr
52.
Q. 22. Boiling points of different substances are given below CH4 = - 161 oC C2H6 = -89 oC CI2 = -34.6 oC F2 = -188 oC The data shows that the vapor pressure of
a)
a. CI2 > C2H6 > CH4 > F2
b)
b. CI2 > F2 > CH4 > C2H6
c)
c. C2H6 > CH4 > F2 > CI2
d)
d. F2 > CH4 > C2H6 > CI2
53.
Q. 23. Which of the following statements is correct for the statement “Vapour pressure of water at 0 oC is 5 mmHg”
a)
a. boiling point of water will be 0 oC at 5 mmHg
b)
b. boiling point of water will be 0 oC
c)
c. if external pressure is 5 mmHg then water will boil at 0 oC
d)
d. boiling point of water is 100 oC at 760 mmHg pressure
54.
Q. 24. What is the typical range of the hydrogen bond
a)
a. 5 – 25 kJ per mole of bonds
b)
b. 5 – 25 kJ per molecule
c)
c. 500 kJ per mole of bonds
d)
d. 1 – 2 kJ per mole of bonds
55.
Q. 25. Hydrogen bond is unimportant in
a)
a. DNA structure
b)
b. The liquid properties of water
c)
c. Liquid HF
d)
d. Liquid CH4
56.
Q. 26. All of the following acids have a hydrogen bond in the liquid state except
a)
a. sulfuric acid
b)
b. nitric acid
c)
c. hydrofluoric acid
d)
d. hydrochloric acid
57.
Q. 27. Which of the following statements is incorrect?
a)
a. dispersion force is the weakest type of intermolecular interactions
b)
b. the strong intermolecular attractions in H2O result from hydrogen bonding
c)
c. boiling point of H2S is less than H2O
d)
d. boiling point of non-polar substances tends to decrease with increasing molecular weight
58.
Q. 28. A white substance melts with some decomposition at 730 oC. As a solid, it is a non-conductor of electricity but it dissolves in water to form a conducting solution. The white substance is
a)
a. a covalent network solid
b)
b. an ionic solid
c)
c. a molecular solid
d)
d. a metallic solid
59.
Q. 29. Keeping in mind different factors which affect the boiling point of a substance, the element having the highest boiling among the following is
a)
a. He
b)
b. F2
c)
c. Ne
d)
d. Br2
60.
Q. 30. The increasing vapor pressure caused by heating a liquid is due to
a)
a. increase intermolecular interactions
b)
b. increasing potential energy of molecules
c)
c. increasing kinetic energy of molecules
d)
d. decreasing surface tension
61.
Q. 31. Covalent network crystals have
a)
a. higher melting point than molecular crystals
b)
b. lower melting point than molecular crystals
c)
c. discrete molecules linked by Van der Waals forces
d)
d. hydrogen bonding
62.
Q. 32. Keeping in mind different factors which affect the boiling point of a liquid, the element having the lowest boiling point among the following is
a)
a. F2
b)
b. CI2
c)
c. Br2
d)
d. I2
63.
Q. 33. A chemist was able to measure the value of lattice energy of KCI to be 690 kJ/mol. From this experiment, he concluded that
a)
a. lattice energy of KBr is 630 kJ/mol and that of KI is 665 kJ/mol
b)
b. lattice energy of KBr is 665 kJ/mol and that of KI is 630 kJ/mol
c)
c. lattice energy of KBr is 765 kJ/mol and that of KI is 730 kJ/mol
d)
d. lattice energy of KBr is 730 kJ/mol and that of KI is 765 kJ/mol
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