Are you searching for the IX Chemistry Guess Paper 2026 based on the latest board paper pattern? Here you’ll find 100% important questions, MCQs, short and long questions, and chapter-wise important concepts that are most expected in the 2026 board exams.
Welcome to the IX Chemistry Guess Paper 2026 prepared by Inam Jazbi, your trusted source for quality educational content and exam preparation. This post includes chapter-wise important MCQs, short questions, and long questions carefully selected from past board papers, new syllabus, and model tests to help you score top marks in your upcoming exams.
Whether you’re following the new textbook or revising for your final term, this Chemistry Class 9 Guess Paper 2026 by Inam Jazbi highlights the most expected questions, repeated concepts, and key topics every student must prepare.
💡 What’s Inside:
Start revising today with Inam Jazbi’s trusted Guess Paper 2026 and make your Chemistry exam success guaranteed!Get ready to ace your IX Chemistry exam 2026 with these reliable and accurate guess papers — your shortcut to success!
ðŸ§
Related Posts:
https://learnchemistrybyinamjazbi.blogspot.com/2025/05/ix-chemistry-notes-2025-new-concise.html
https://learnchemistrybyinamjazbi.blogspot.com/2025/02/ix-chemistry-important-mcqs-of-text.html
https://learnchemistrybyinamjazbi.blogspot.com/2025/02/x-chemistry-mcqs-for-board-paper-2025.html
https://learnchemistrybyinamjazbi.blogspot.com/2024/08/ixxii-valency.html
https://learnchemistrybyinamjazbi.blogspot.com/2024/07/ix-conceptual-chemistry-book-by-dr-inam.html
https://learnchemistrybyinamjazbi.blogspot.com/2024/07/ix-model-test-questions-chemistry-test.html
https://learnchemistrybyinamjazbi.blogspot.com/2024/06/ix-model-test-questions-class-9.html
https://learnchemistrybyinamjazbi.blogspot.com/2024/05/fundamentals-of-chemistry.html
https://learnchemistrybyinamjazbi.blogspot.com/2024/03/ix-chemistry-model-test-questions-of.html
Q1. Define any three of the following:
Valency, Electronegativity, electron affinity, Tyndall effect, free radical, molecular ion, mole, molar volume, empirical and molecular formula, Molarity, Solubility, concentration, false solution, mass/volume percent, Freezing Point, alloy, heterogenous mixture, absolute zero, allotropy, Dobereiner’s law of Triads, Newland’s law of Octaves, Mendeleev’s Periodic law, Periodicity, periodic trend, modern, periodic law, electronegativity, electrolysis.
Q2.Write down three differences between any one of the following:
(i) Alkali metal and halogens
(ii) Ionic, covalent bond and dative bond
(iii) elements, compounds and mixtures
(iv) Ionic compounds and covalent compounds
(v) Solution, suspension and Colloid
(vi)
metal,
metals and metalloids
(vii) Atom and molecule and ion
(viii) Molecule and molecular ion
and free radical
(ix) Alkali metals and alkaline earths
(x) Cation and anion
(xi)
Ion and
free radical
Q3. The following statements belong to which branch of chemistry? Identify:
(i) that chlorofluoro compounds are responsible for depletion of ozone layer.
(ii) That investigates the properties of ammonia gas.
(iii) That find out the quantity and quality of paracetamol in Panadol tablet.
OR
What is chemistry? Define its main
branches briefly.
ORWhat is meant by atomic number and mass number? Define and give uses of isotopes. Discuss the isotopes of Hydrogen or carbon or uranium. Mention the number of electrons, protons & neutrons in following atoms:
OR
Differentiate between empirical and molecular formula. Describe relationship between empirical and molecular formula? Find out molecular formula of a compound if its empirical formula is CH2O and molecular mass 60 amu. Complete the following chart:
Q4. Identify group and period in the periodic
table of the following elements
(i) 3Li or 8O or 15P
(ii) 9F or 11Na and 17Cl
(iii) 12Mg
or 13 Al or 14Si
OR
An element has 7 (or 1 or 2 or 8)
electrons in its M-shell. Answer the following questions:
(i) Determine
its atomic number and give its Electronic configuration.
(ii) Identify
the group, period and block of given element.
(iii)
Write down three characteristics of
the belonging group. Also write down the name and symbol of radioactive element of this group.
OR
Define symbol. How is symbol of
an element written? Write down names and symbols of element starting with C, S,
N, O and B
Q5. Write down one contribution of
any 6 scientists in the field of chemistry.
OR
Draw
the electronic dot and cross structures for H2, N2, O2,
CH4, NH3 and C2H2.
Q6. Write chemical formulae and one use of any three of the following compounds:
Sand (SiO2), Limestone (CaCO3), Sodium nitrate (NaNO3), table salt (NaCl), sal ammoniac (NH4Cl), Caustic soda (NaOH), caustic potash (KOH), washing soda (Na2CO3.10H2O), baking soda (NaHCO3), soda ash (Na2CO3), Epsom salt (MgSO4.7H2O), gypsum (CaSO4.2H2O), oleum (H2S2O7), marsh gas (CH4), blue vitriol (CuSO4.5H2O), sugar (C12H22O11), ethyl alcohol, Acetylene, Ethylene.
OR
What is coordinate covalent bond? Explain
with two examples.
OR
Define metallic bond. How are metallic bonds
formed?
Q7. Write down any three points of atomic
model proposed by Schrodinger or Bohr.
Or
Describe wave particle duality of electron
of De Broglie Hypothesis? Prove that modern theory of De Broglie is related with Einstein and
Plank's equations.
OR
Give three properties of canal
rays.
Q8. Write down electronic
configuration of 5B, 9F, 7N, 11Na, 13Al,
15P, 20Ca, 19K+, 8O2−, 16S2−, 12Mg2+,
17Cl−.
OR
Justify that Rutherford atomic model has
defects? What are Limitations of Bohr's Atomic Model?
OR
What is shielding effect? Explain how shielding effect influence the periodic trends?
Q9. Balance the
any three of the following chemical equations:
2KClO3 → 2KCl + 3O2
2Ba(NO3)2
→ 2BaO +
4NO2 + O2
2Na + 2H2O → 2NaOH + H2
2NH3
+ 3Cl2 → N2 + 6HCl
MnO2
+ 4HCl → MnCl2 + 2H2O
+ Cl2
4NH3 + 5O2 → 4NO + 6H2O
4Zn
+ 10HNO3 → 3H2O+ NH4NO3 +
4Zn(NO3)2
3CuO + 2NH3 → 3Cu + N2
+ 3H2O
2KNO3 → 2KNO2
+ O2
Ca + 2H2O → Ca(OH)2 + H2
2NaHCO3
→ Na2CO3 + CO2 + H2O
OR
How
is electronegative value determined the formation of chemical bond? Describe ionic character in covalent bond.
OR
What is meant by bond pair, lone pair and unpaired electrons? How many unpaired electrons are there in oxygen atom and nitrogen atom? How many lone pairs are there in nitrogen molecule and oxygen molecule?
Q10. What is KMT? Give its main postulates with respect to three states
of matter.
OR
What is diffusion and Graham’s law
of diffusion of gases? Which gas from among CO2, CH4 and
NH3 will diffuse the fastest
and why? Give the reason.
OR
Define ionization energy or electron affinity. Describe trend in group and period with examples of any one them.
Q11. Differentiate between amorphous and
Crystalline Solids?
OR
Explain the solute-solvent interaction to prepare sodium chloride solution.
Q12. Define electrochemical reaction and redox
reaction. Write down 2 differences between oxidation and reduction and oxidizing agent and reducing agent with
examples. Give an example of redox reaction and also Identify oxidizing and reducing agents of
the following chemical reaction:
Zn
+ Cl2 → ZnCl2
OR
Differentiate
between electrolytes and non-electrolytes with examples. Identify strong and
weak electrolytes from the
following:
HCl (S), KI (S), NaOH (S), H2S (W), CH3COOH (W), NH4OH (W), NaCl (S), C2H5OH (W)
Q13.
What is corrosion of metal and rusting?
Name the methods which are used to protect metal from corrosion. How cathodic protection prevent metal from
corrosion?
OR
Write down the composition of following alloys:
Brass (Cu-Zn,[4:1]), Bronze (Cu-Sn-Zn) [9:1], Bell metal (Cu-Sn), Monel (Ni-Cu-Fe), Amalgam (Hg-Ag-Cu- Zn), Pewter (Sn-Cu-Pb-Sb-Bi), White gold (Au-Pb-Ag-Cu (18 karat), Duralumin (Al-Cu-Mg-Ni)
Q14.What are
metalloids? Write names and symbols of any 5 metalloids.
OR
Write names and symbols of some
noble metals. Explain inertness of noble metals.
OR
Define Moh Scale. What are Soft &
Hard Metals? Differentiate
between sodium and iron as soft and hard metal.
OR
Differentiate between metal and metals. Identify the elements as metals, non-metals and metalloids from the following: C, Ca, Sb, S, Sr, Se, K, P, N, Ba, Ge, I, Al, B, As
Q15. What is the boiling point? How boiling point is affected by different factors? How boiling point of a substance is affected by atmospheric pressure?
Q16. What is
density, how the density of liquid is affected by temperature and pressure?
OR
What is
plasma? Explain plasma with the daily life examples?
OR
Explain importance of Silver and gold.
Q17. Describe the construction of electrochemical cell. Write down names of two types of electrochemical cells. Write down 4 applications of electrolytic cells or electrolysis.
Q18. Give reason:
(i)
Why gasoline does not dissolve in water?
(ii)
Alkali metals are not found in free state in nature, why?
(iii)
Why ionic compounds conduct electricity in molten or in aqueous solutions only?
(iv)
Why the solubility of a salt increases with the increase in temperature?
(v)
Explain why table salt has a very high melting point.
(vi)
Atomic radii increase down a group and decrease across a period.
(vii)
Alkali metals have the largest while halogens have the smallest atomic radii in
their period.
(viii)
Shielding effect of inner electrons remains the same across a period.
(ix)
Ionization energy, electron affinity and electronegativity show same trends
across a period.
(x)
Covalent bonds are strong and hard to break but why most of the covalent
compounds have low melting and boiling
points.
(xi)
Why the rate of diffusion of gases is rapid than that of liquids?
(xii)
How does electron differ from proton or neutron?
(xiii)
Helium diffuses faster than methane.
Q19. Discuss Rutherford’s Alpha particles scattering experiment &
write down the postulates of his atomic model.
OR
Determine the demarcation of periodic table
in to s, p, d and f blocks.
OR
Write down 6 postulates of Bohr’s atomic model.
Q20. Define ionic bond. Discuss the formation of sodium chloride (NaCl) or
magnesium oxide.
OR
What is meant by covalent bond and coordinate covalent bond? Describe the formation of a covalent bond between two nonmetallic atoms. Explain single, double and triple covalent bond with examples. Explain dative bond with two examples.
Q21. Describe the
Boyle's law or Charles’s law with example.
OR
Define vapour pressure. How equilibrium state involved in vapour pressure of liquids in close system? Describe the factors which affect on vapour pressure
Q22. Define
the term solubility. How does nature of solute and solvent determine the extent
of dissolution? Why the solubility of a salt increases with the increase in
temperature?
OR
Discuss discharge tube experiment for the
discovery of electrons with 4 properties of cathode rays.
OR
Explain the importance of glues and epoxy resins in our society.
Q23. State
and explain Faraday’s Laws of electrolysis.
OR
What is electroplating? How steel object can
be electroplated with zinc, tin and silver?
Q25. Explain electronegative character of non-metals or electropositive
character of metals. Discuss the reactivity of
Halogens
OR
What
are transition elements? Give their types. Give their 4 general properties.
Q26.Explain the experiment to test CO32‒, Cl‒ and I‒ ions and Zn2+,
Mg2+, Ca2+ and Ba2+ ions.
OR
What
is allotropy? Describe different allotropes of carbon.
OR
Describe the construction and working of lead battery or dry cell.
Q27. What are molecules? Discuss its six types
with examples.
OR
What are mixtures? Gives its examples. Discuss its two types with examples.
Q28. Compare of reactivity of Alkali and Alkaline Earth Metals
Q29.Identify the highly electronegative and
electropositive groups of the Periodic table. Enlist the elements present in
these groups. Give four common characteristics of each of these groups.
Numericals
Q30. Calculate
the number of moles, number of molecules present in 8g of C6H12O6?
(answer; 0.04, 2.40 x 1022 molecules)
OR
Calculate
the number of moles, number of molecules and number of atoms present in 10 g of
H2SO4
(answer; 0.10 mole, 6.02 x 101022,
4.214 x 1023 atoms)
Q31.What is the
mass of oxalic acid (C2H2O4) required to
prepare 100 cm3 volume of 2M oxalic acid solution?
Or
What is the
molarity of the solution prepared by dissolving 1.25 g of HCl gas into enough
water to make 30 cm3
of solution?
Q32. Determine the percentage concentration of the
solution obtained by dissolving 10g sugar in 140g water
OR
A solution
of 20 cm3 of alcohol is dissolved in 80cm3 of water.
Calculate the concentration (v/v) of solution.
Q33. 10M HNO3 solution is
available in laboratory. How would you prepare 500 cm3 of 0.1M
solution?
OR
A
sample of sulphuric acid has the molarity 20M. How many cm3 of
solution should you use to prepare 500 cm3 of 0.5M H2SO4? (Answer; 12.5cm3)
Q34. The 800 cm3 of a gas is enclosed in a container
under a pressure of 750 mm. If the volume is reduced to 250 cm3, what will be the
pressure?
OR
A
sample of Hydrogen gas has a volume of 350 cm3 at 40oC.
If gas is allowed to expand up to 700 cm3 at constant pressure. Find out its final
temperature? (answer; 626 K)
Q35. Calculate the number of atoms present in 9.2 g of calcium.
1. Mole fraction is denoted by:
(a) X (b) Z (c) N (d) M
2. Noble gases are stable because their valance shell have complete (except Helium)
(a) Duplet (b) Octet (c) Sixtet (d) None of them
3. At room temperature, most of the ionic
compounds are:
(a) Amorphous Solid (b) Crystalline Solid
(c) Liquid (d) Gas
4. 101325 Pascal
= …………. atm
(a) 1 (b) 2 (c) 3 (d) ½
5. Which of the following gas diffuses faster?
(a) Oxygen (b) Chlorine (c) Fluorine (d) Nitrogen
6. Hexane is an example of this type of solvent:
(a) Polar (b) non polar (c) Ionic (d) Universal
7. 12 g of magnesium’s (Mg) is equal to:
(a) 1 moles (b) 2 moles (c) 3 moles (d) Half mole
8. The size of particles in suspension is:
(a) Greater than 103 nm (b) Less than 103nm
(c) 102nm (d) 10-2nm
9. This one of
the following is non-electrolyte:
(a) Aqueous HCI (b) Aqueous NaCl
(c)
Benzene (d) Molten KCl
10. This one is an alloy:
(a) Brass (b) Steel (c) Bronze (d) All of them
11. 3 g equivalent weight of Al is equal to:
(a) 1 g (b) 9 g (c) 27 g (d) 54 g
12. This gas turns lime water milky
(a) CO2 (b) O2 (c) NO2 (d) N2
13. This halogen exists in gaseous state:
(a) Fluorine (b) Chlorine (c) Iodine (d) Both a and b
14. This element is metalloid:
(a) Br (b) Sb (c) S (d) Sr
15. No Definite shape and definite volume is the property of:
(a) Gas (b) Plasma (c) Liquid (d) Solid
16. The pH value of acidic solution is:
(a) Less than 7.0 (b) 7.0 (c) Greater than 7.0 (d) 14.0
17. The horizontal rows of elements in the Modern periodic table are called:
(a) Group (b) period (c) Series (d) Rows
18. W=Z x A x T, this equation was proved by:
(a) Michael Faraday (b) Alexandro Volta (c) Galvani (d) Madam Currie
19. One
Faraday is equal to:
(a) 96560 Coulombs (b) 95650 Coulombs
(c)
96650 Coulombs (d) None of these
20. It is the longest period of the periodic table:
(a) 2 (b) 6 (c) 7 (d) 5
21. In
jellies, solute and solvent are:
(a) Sugar and water (b) Water and fat
(c) Water & fruit
pulp (d)
Air and water
22. This one of the following compounds contains all three chemical bonds that are, Ionic, Covalent, Co-Ordinate Covalent Bond
(a)NaCl (c) NH4Cl (c) CH4 (d) CO2
23. This acid is also known as "Vitamin-C":
(a)Ascorbic acid (b) Acetic acid (d) Carbonic acid (d) Oxalic acid
24. Taste of acids are:
(a) Bitter (b) Sour (c) Sweet (d) Neutral
25. Sugar is
an example of:
(a) Strong Electrolyte (b) Weak Electrolyte
(c) Non-Electrolyte (d) Electrolyte
26. The process in which molecules escape from the surface of a liquid is called:
(a)Boiling (b) Evaporation (c) Sublimation (d) Melting
27. Bases turns red litmus paper into:
(a) Pink Colour (b) Orange Colour (c) blue (d) white
28. The symbol of Sodium is:
(a) S (b) So (c) Na (d) Ne
29. C-14 has the Neutron:
(a) 14 (b) 12 (c) 7 (d) 8
30. Al2O3 is ………. in nature.
(a) Basic (b) Acidic (c) Amphoteric (d) Neutral
31. The empirical formula of Glucose is:
(a) CH2O (b) C2HO (c) CHO (d) CHO2
32. 44 a.m.u of carbon dioxide is equal to:
(a) Molar Mass (b) Molecular Mass (c) Atomic Mass (d) Mass Number
33. In NaCl crystal lattice each Na ion is surrounded by:
|
(a) |
6 Cl‒
ions |
(b) |
6 Na+ ions |
(c) |
8 Cl‒ ions |
(d) |
12 Cl‒ ions |
34. Which one is oxidizing agent?
|
(a) |
Al |
(b) |
H2S |
(c) |
Cl2 |
(d) |
NaH |
35. Which one of the following is a
non-polar molecule?
|
(a) |
NH3 |
(b) |
HCl |
(c) |
CH4 |
(d) |
H2O |
36. The
empirical formula of formaldehyde is:
|
(a) |
CH2O |
(b) |
C2HO |
(c) |
CH0 |
(d) |
CHO2 |
37. Which pair
of elements is chemically similar?
|
(a) |
K, Cr |
(b) |
Cu, Ca |
(c) |
F, Cl |
(d) |
N, O |
38. One atmospheric pressure is equal to:
|
(a) |
10325 Pascal |
(b) |
106075 Pascal |
(c) |
10523 Pascal |
(d) |
101325 Pascal |
39. Which of the following have sharp melting point
in solids?
|
(a) |
Plastic |
(b) |
Rubber |
(c) |
Glass |
(d) |
Diamond |
40. The shielding effect across the period:
|
(a) |
Increases |
(b) |
Decreases |
(c) |
Moderate |
(d) |
Remain same |
41. If nucleon number of potassium is 39, number of
neutrons will be:
|
|
(a) |
39 |
(b) |
19 |
(c) |
20 |
(d) |
29 |
42. Which one of the following is most penetrating?
|
|
(a) |
Electron |
(b) |
Proton |
(c) |
alpha
particle |
(d) |
Neutron |
43. If
proton number is 19, electron configuration will be:
|
|
(a) |
2, 8, 9 |
(b) |
2, 8, 8,
1 |
(c) |
2, 8, 1 |
(d) |
2, 8, 3 |
44. Which
one of the following is most penetrating?
|
|
(a) |
Beta particle |
(b) |
Gamma
rays |
(c) |
alpha particle |
(d) |
None |
45. Name
the material of screen which used in Rutherford atomic model:
|
|
(a) |
Aluminum foil |
(b) |
Aluminum sulphide |
(c) |
sodium sulphide |
(d) |
zinc sulphide |
46. 4th and 5th
period in periodic table are known as
|
(a) |
Short period |
(b) |
Long
period |
(c) |
Very long period |
(d) |
Normal period |
47. Which one of the following
decreases along the period?
|
(a) |
Ionization
Energy |
(b) |
Atomic Radius |
(c) |
Electronegativity |
(d) |
Electron Affinity |
48. The ionization energy across
the period:
|
(a) |
Increases |
(b) |
Decreases |
(c) |
Moderate |
(d) |
Remain same |
49. In group electron affinity
values decreases from top to bottom because:
|
(a) |
Atomic
size normal |
(b) |
Atomic size increases |
(c) |
Atomic size decreases |
(d) |
Atomic size same |
50. Interaction between highly
electron deficient hydrogen and highly electronegative atom is called
|
(a) |
ionic
bond |
(b) |
metallic
bond |
(c) |
hydrogen
bond |
(d) |
covalent
bond |
51. Number of electrons lost by
atoms of group IIIA equals:
|
(a) |
1 |
(b) |
2 |
(c) |
3 |
(d) |
4 |
52. Which
of the following gas diffuses fastest?
|
(a) |
Ammonia |
(b) |
Methane |
(c) |
Ethyne |
(d) |
Ethene |
53. Which one is not strong acid?
|
(a) |
HF |
(b) |
HBr |
(c) |
HI |
(d) |
HCl |
54. The
vapour pressure of a liquid increases with the increase of:
|
(a) |
Pressure |
(b) |
polarity of molecules |
(c) |
intermolecular forces |
(d) |
temperature |
55. One atmospheric
pressure is equal to:
|
(a) |
760 torr
|
(b) |
1 torr |
(c) |
10.7 psi |
(d) |
101.325 Pascal |
56. Which
of the following have sharp melting point in solids?
|
(a) |
Plastic |
(b) |
Rubber |
(c) |
Glass |
(d) |
NaCl |
57. The
density of gases increases when its:
|
(a) |
Pressure
increased |
(b) |
Temperature increased |
(c) |
Volume increased |
(d) |
None of these |
58. Solubility
is usually expressed in grams of the solute dissolved in ________gram of a
solvent
|
(a) |
10 grams |
(b) |
100
grams |
(c) |
500 grams |
(d) |
1000 grams |
59. 2 moles
of sodium chloride (NaCl) is equal to:
|
(a) |
123 grams |
(b) |
135 grams |
(c) |
158 grams |
(d) |
117 grams |
60. Molarity
of a solution which is prepared by dissolving 40 g sodium chloride in 500cm3
of solution is:
|
(a) |
1.4 M |
(b) |
1.5 M |
(c) |
1.33 M |
(d) |
1.36 M |
61. Which solution contains more water?
|
(a) |
1.0M |
(b) |
0.75M |
(c) |
0.5M |
(d) |
0.25M |
62. Which one is oxidizing agent?
|
(a) |
Al |
(b) |
H2S |
(c) |
F2 |
(d) |
NaH |
63. Chlorine can be displaced by _________
|
(a) |
Br |
(b) |
I |
(c) |
F |
(d) |
At |
64. Al2O3 and ZnO are ………. in nature.
|
(a) |
basic |
(b) |
Acidic |
(c) |
Amphoteric |
(d) |
Neutral |
65. Which one forms weak electrolyte solution with
water?
|
(a) |
HCl |
(b) |
KOH |
(c) |
NaCl |
(d) |
Ch3COOH |
66. 1g equivalent weight of Al is equal to ……..
|
(a) |
9 g |
(b) |
27 g |
(c) |
54 g |
(d) |
1 g |
67. Which substance can conduct electricity by the
movement of ions?
|
(a) |
Copper |
(b) |
Graphite
|
(c) |
Sodium chloride |
(d) |
Mercury |
68. Which one metal belongs to alkaline earth metals?
|
(a) |
B |
(b) |
Bi |
(c) |
Br |
(d) |
Ba |
69. One Faraday = Coulombs
|
(a) |
96500 Coulombs |
(b) |
96600 Coulombs |
(c) |
96700 Coulombs |
(d) |
96800 Coulombs |
70. Number of molecules present in 18 grams of water
(H2O) is:
|
(a) |
6.02 x 1023 |
(b) |
6.02 x 1024 |
(c) |
6.02 x 1030 |
(d) |
6.02 x 1034 |
71. Symbol of Potassium is:
|
(a) |
P |
(b) |
K |
(c) |
S |
(d) |
O |
72. The number of
electrons in S2−
is:
|
(a) |
20 |
(b) |
19 |
(c) |
18 |
(d) |
16 |
73. the
5th period of periodic table contains total ……………. elements.
|
(a) |
32 |
(b) |
8 |
(c) |
18 |
(d) |
2 |
74. Which one of the following diffuses faster than
oxygen with molar mass of 32 g/mol?
|
(a) |
Cl2 |
(b) |
F2 |
(c) |
SO2 |
(d) |
NH3 |
75. Which one of
the following is a non-polar molecule?
|
(a) |
NH3 |
(b) |
HCl |
(c) |
CH4 |
(d) |
H2O |
76. The mass of 1 atom of diamond is equal to
|
(a) |
1.99 x 10-23 g |
(b) |
12 g |
(c) |
1.99 x 1023
g |
(d) |
1.66 x 10-24 g |
77. The process of converting a solid into liquid at its melting point is
called:
|
(a) |
Fusion |
(b) |
Vaporization |
(c) |
Evaporation |
(d) |
Diffusion |
78. Elements of group VII-A are known as:
|
(a) |
Alkaline Earth
Metals |
(b) |
Alkali Metals |
(c) |
Halogens |
(d) |
Inert gases |
79. This one of the following is an ionic compound:
|
(a) |
H2O |
(b) |
NH3 |
(c) |
NaCl (or KCl) |
(d) |
CO2 |
80. The only liquid metal is:
|
(a) |
Bromine |
(b) |
Zinc |
(c) |
Mercury |
(d) |
Sodium |
81. It is the heaviest sub-atomic particle:
|
(a) |
Photon |
(b) |
Neutron |
(c) |
Proton |
(d) |
Electron |
82. If nucleon number of calcium
is 40, number of neutrons will be:
|
|
(a) |
39 |
(b) |
19 |
(c) |
20 |
(d) |
29 |
83. The isotope C-12 is present
in abundance of:
|
|
(a) |
96.9% |
(b) |
97.6% |
(c) |
98.8% |
(d) |
99.7% |
84. Which one is
metalloid?
|
(a) |
Br |
(b) |
Se |
(c) |
S |
(d) |
Sr |
85. Which gas can
turn lime water milky?
|
(a) |
O2 |
(b) |
NO2 |
(c) |
CO2 |
(d) |
N2 |
86. Which compound
is known as lunar caustic?
|
(a) |
KNO3 |
(b) |
AgNO3 |
(c) |
NaOH |
(d) |
NaNO3 |
87. Which pair of elements is chemically similar?
|
(a) |
K, Cr |
(b) |
Cu, Ca |
(c) |
Mg, Ca |
(d) |
N, O |
88. Which one of
the following is a non-polar molecule?
|
(a) |
NH3 |
(b) |
HCl |
(c) |
N2 |
(d) |
H2O |
89. solution of known
concentration is called:
|
(a) |
Concentrated
solution |
(b) |
Saturated
solution |
(c) |
Standard solution |
(d) |
Dilute solution |
90. Alum is a
|
(a) |
Normal salt |
(b) |
Double salt |
(c) |
Mixed salt |
(d) |
Basic salt |
91. The pH value of human blood is:
|
(a) |
7.35-7.45 |
(b) |
7.8 |
(c) |
7.2 |
(d) |
7.0 |
92. A dative bond
is always formed between the two:
|
(a) |
Like and unlike atoms |
(b) |
Similar atoms |
(c) |
Unlike atoms |
(d) |
Like atoms |
93. A suspension of droplets of one liquid into
another in which it is not soluble is called
|
(a) |
Foam |
(b) |
Emulsion |
(c) |
Mud |
(d) |
Smoke |
94. The number of moles of solute dissolved in per kilogram of solvent is
called:
|
(a) |
Molarity |
(b) |
Molality |
(c) |
Normality |
(d) |
Solubility |
95. Gases possess neither definite shape nor definite:
|
(a) |
Mass |
(b) |
Volume |
(c) |
Density |
(d) |
State |
96. The process of converting a liquid into vapours at its boiling point
is called:
|
(a) |
Fusion |
(b) |
Vaporization |
(c) |
Evaporation |
(d) |
Diffusion |
97. The force which holds atoms together in a molecule or crystal is
called:
|
(a) |
Polar bond |
(b) |
Dative bond |
(c) |
Chemical bond |
(d) |
Ionic bond |
98. Elements of group VII-A are known as:
|
(a) |
Alkaline Earth
Metals |
(b) |
Alkali Metals |
(c) |
Halogens |
(d) |
Inert gases |
99. This one of the following is an ionic compound:
|
(a) |
H2O |
(b) |
NH3 |
(c) |
MgO |
(d) |
CO2 |
100. The number of periods/series in Mendeleev’s periodic table is:
|
(a) |
13 |
(b) |
12 |
(c) |
14 |
(d) |
10 |
101. The only liquid non-metal is:
|
(a) |
Bromine |
(b) |
Zinc |
(c) |
Mercury |
(d) |
Sodium |
102. It is the lightest sub-atomic particle:
|
(a) |
Photon |
(b) |
Neutron |
(c) |
Proton |
(d) |
Electron |
103. The average mass number of all naturally found
isotopes of an element is called:
|
(a) |
Atomic mass unit |
(b) |
Mass number |
(c) |
Atomic mass |
(d) |
Formula mass |
104. In water (H2O) the ratio by mass between Hydrogen and
Oxygen is:
|
(a) |
3:8 |
(b) |
1:8 |
(c) |
1:16 |
(d) |
3:4 |
105. The empirical formula of Glucose is:
|
(a) |
CH2O |
(b) |
C2HO |
(c) |
CH0 |
(d) |
CHO2 |
106. The study of Hydrocarbons and their derivatives is called:
|
(a) |
Inorganic
Chemistry |
(b) |
Physical
Chemistry |
(c) |
Organic
Chemistry |
(d) |
Biochemistry |
107. It is the best disinfectant:
|
(a) |
Fluorine |
(b) |
Iodine |
(c) |
Bromine |
(d) |
Chlorine |
108. The bond formed by mutual sharing of electrons between the atoms is
called:
|
(a) |
Electrovalent
bond |
(b) |
Covalent bond |
(c) |
Dative bond |
(d) |
Ionic bond |
109. Electro-Chemical Equivalent of an element is represented by:
|
(a) |
M |
(b) |
Z |
(c) |
X |
(d) |
N |
110. Basic unit of electric current is
|
(a) |
coulomb |
(b) |
joule |
(c) |
ampere |
(d) |
volt |
111. The electronegativity of carbon is
|
(a) |
2.1 |
(b) |
3.0 |
(c) |
2.5 |
(d) |
1.0 |
112. Einstein’s mass energy equivalence is given by E =
|
(a) |
mv |
(b) |
mc2 |
(c) |
mv2 |
(d) |
mc |
113. Charge on an electron in coulomb is:
|
(a) |
1.602 x 10-19 |
(b) |
1.602 x 10-17 |
(c) |
1.67 x 10-18 |
(d) 1.6 x 10-16 |
114. Which pair of elements is chemically similar?
|
(a) |
K, Cr |
(b) |
Cu, Ca |
(c) |
Na, K |
(d) |
N, O |
115. Solutions are:
|
(a) |
Colloids |
(b) |
Transparent |
(c) |
Opaque |
(d) |
None of these |
116. Number of molecules present in 36 grams of water (H2O)
is:
|
(a) |
6.02 x 1023 |
(b) |
2 x 6.02 x 1023 |
(c) |
3 x 6.02 x 1023 |
(d) |
6.02 x 1034 |
117. Symbol of silicon is:
|
(a) |
S |
(b) |
Se |
(c) |
Si |
(d) |
Sc |
118. Caca-cola contains this acid:
|
(a) |
Acetic acid |
(b) |
carbonic acid |
(c) |
formic acid |
(d) |
Boric acid |
119. The number of electrons in P3− is:
|
(a) |
20 |
(b) |
19 |
(c) |
18 |
(d) |
16 |
120. Which one of the following gas is also known as
marsh gas?
|
(a) |
Ethane |
(b) |
Ethyne |
(c) |
Methane |
(d) |
Ethene |
121. Basic unit of electric charge is
|
(a) |
joule |
(b) |
coulomb |
(c) |
ampere |
(d) |
Volt |
122. the
5th period of periodic table contains total ……………. elements.
|
(a) |
32 |
(b) |
8 |
(c) |
18 |
(d) |
2 |
123. Which one of the following diffuses faster than
oxygen with molar mass of 32 g/mol?
|
(a) |
Cl2 |
(b) |
F2 |
(c) |
SO2 |
(d) |
N2 |
124. Which one of the following substances contains
covalent bonds but also conducts electricity?
|
(a) |
Copper |
(b) |
Graphite
|
(c) |
Iron |
(d) |
Sodium |
125. Blood is one of the following:
|
(a) |
Element |
(b) |
Compound |
(c) |
Mixture |
(d) |
Metal |
126. Empirical
formula of CH3COOH is
|
(a) |
C2H4O2 |
(b) |
CH2O |
(c) |
CH4CO2 |
(d) |
CHOC |
127. Dobereiner arranged elements in
|
(a) |
Triads |
(b) |
Octaves |
(c) |
Groups and
period |
(d) |
Sub-groups |
128. Line spectrum of hydrogen was studied by
|
(a) |
Max Planck |
(b) |
Albert Einstein |
(c) |
Neil Bohr |
(d) |
De Broglie |
129. The radioactive element in VIIA group is
|
(a) |
Radium |
(b) |
Francium |
(c) |
Radon |
(d) |
Astatine |
130. The radioactive element in IA group is
|
(a) |
Rubidium |
(b) |
Francium
|
(c) |
Cesium |
(d) |
Potassium |
131. It is considered as the fourth state of matter
|
(a) |
Gas |
(b) |
Plasma
|
(c) |
Liquid |
(d) |
Solid |
132. This is the isotope of hydrogen which contains
greater number of neutron:
|
(a) |
Protium |
(b) |
Deuterium |
(c) |
Tritium |
(d) |
Hydrogen |
133. Synthetic resin binds two surfaces together by
this bonding
|
(a) |
Hydrogen bonding |
(b) |
Ionic bonding |
(c) |
Covalent bonding
|
(d) |
Metallic bond |
134. Which one
of the following is a polar compound?
|
(a) |
CH4 |
(b) |
H2S |
(c) |
H2O |
(d) |
O2 |
135. Noble gases
are stable because their valence shell contains these number of electrons
except helium
|
(a) |
4 |
(b) |
6 |
(c) |
8 |
(d) |
10 |
136. All transition elements are
|
(a) |
Non-metals |
(b) |
Metals
|
(c) |
Metalloids |
(d) |
Gases |
137. According to Avogadro’s law, one gram mole of
any gas at STP occupies volume:
|
(a) |
22.4 mm3 |
(b) |
22.4 cm3 |
(c) |
22.4dm3 |
(d) |
22.4 m3 |
138. Dry cell produces a potential of:
|
(a) |
1.0 volt |
(b) |
1.5
volt |
(c) |
2.0 volt |
(d) |
12 volt |
139. Leakage
of helium gas through a gas balloon is an example of:
|
(a) |
Diffusion |
(b) |
Effusion
|
(c) |
Evaporation |
(d) |
Mobility |
140. It is
type of dipole-dipole interaction:
|
(a) |
Covalent bond |
(b) |
Hydrogen
bond |
(c) |
Metallic bond |
(d) |
Ionic bond |
141. 5% m/m aqueous solution means that 5 g of solute is dissolved in:
|
(a) |
90 g of water |
(b) |
95
g of water |
(c) |
100 g of water |
(d) |
105 g of water |
142. The
branch of chemistry that deals with the compounds in living organisms is called
as:
|
(a) |
Analytical
chemistry |
(b) |
Biochemistry chemistry |
(c) |
Organic chemistry |
(d) |
Physical chemistry |
143. Au is the
chemical symbol for:
|
(a) |
Gold |
(b) |
Silver |
(c) |
Aluminium |
(d) |
Argon |
144. The
symbol of silver is:
|
(a) |
Ag |
(b) |
Au |
(c) |
Si |
(d) |
Sn |
145. This
atomic model is known as the quantum mechanical model of the atom:
|
(a) |
Schrodinger
atomic model |
(b) |
Rutherford atomic model |
(c) |
Dalton’ atomic model |
(d) |
Bohr’s atomic model |
146. Which of the following gas diffuses faster?
|
(a) |
Oxygen |
(b) |
Chlorine |
(c) |
Fluorine |
(d) |
Helium |
147. Benzene is an example of this type of
solvent:
|
(a) |
Polar |
(b) |
Non-polar |
(c) |
Ionic |
(d) |
Universal |
148. 69 g of
sodium is equal to
|
(a) |
1mole |
(b) |
2moles |
(c) |
3 moles |
(d) |
4 moles |
149. The size of particles in suspension is
|
(a) |
103
nm |
(b) |
102 nm |
(c) |
Less than 103
nm |
(d) |
Greater than 103
nm |
150. 1 g
equivalent weight of Al is equal to
|
(a) |
1 g |
(b) |
9g |
(c) |
27g |
(d) |
54 g |
151. This one is an alloy
|
(a) |
Graphite |
(b) |
Steel |
(c) |
Mercury |
(d) |
Water |
152. This one of the following is non-electrolyte
|
(a) |
Molten KCl |
(b) |
Urea |
(c) |
Aqueous NaCl |
(d) |
Aqueous HCl |
153. This halogen exist in liquid state
|
(a) |
Fluorine |
(b) |
Chlorine |
(c) |
Bromine |
(d) |
Iodine |
154. This halogen exist in solid state
|
(a) |
Fluorine |
(b) |
Chlorine |
(c) |
Bromine |
(d) |
Iodine |
155. This element is a metalloid
|
(a) |
Br |
(b) |
Si |
(c) |
S |
(d) |
Sr |
156. This element is a metalloid
|
(a) |
B |
(b) |
Ge |
(c) |
As |
(d) |
All of them |
157. Natrium is the Latin name of this element:
(a) Nitrogen (b) Neon
(c) Sodium (d) Nickel
158. In
chemical reaction ZnO + H₂ → Zn + H₂O, it is reduced:
(a) H (b) H₂ (c) Zn (d) O
159. CO₃²⁻ is a/an:
(a) Cation (b) Anion (c) Molecule (d) Molecular ion
160. There
are three sub-shells in
(a) N-shell (b) M-shell (b) L-shell
(b) K-shell
161. Boron
is a:
(a)
Metalloid (b)
Metal (c)
Non-metal (d) Transition metal
162. Atomic
radius is measured in:
|
(a) |
Yard |
(b) |
Feet |
(c) |
Inch |
(d) |
Angstrom |
163. This
term would be the same for 1mole of oxygen gas and 1 mole of water?
(a)
atoms (b) mass (c) molecules (d)
volume