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Worksheets

JEE PRACTICE

Total questions: 163

Worksheet time: 2hrs 1mins

Name
Class
Date
1.

The boiling points of hydridehahahs of group 16 are in the order

a)

H2O > H2Te > H2S > H2Se

b)

H2O > H2S > H2Se > H2Te

c)

H2O > H2Te > H2Se > H2S

d)

None of these

2.

Nitrogen is chemically inert. Why?

a)

Due to presence of double bond require more energy to break

b)

Due to presence of triple bond require more energy to break

c)

Triple bond requires less energy to break

d)

None of the above

3.

Ammonia is liquid phosphene gas . Why?

a)

Due to more molar mass ammonia has maximum vanderwall force of attraction

b)

Due to more molar mass , ammonia has less vander wall force of attraction

c)

Due to presence of inter molecular hydrogen bonding in ammonia

d)

Due to absence of hydrogen bonding in ammonia

4.

Nitrogen cannot exhibit co valancy more than four due to

a)

Presence of vacant d orbitals

b)

Due to large size

c)

Due to absence of vacant d orbitals

d)

Due to inert nature

5.

Among the hydrides of 15th group , which is strong reducing agent?

a)

Ammonia

b)

Phosphine

c)

Arsine

d)

Bismuthine

6.

Ammonia is a Lewis base and act as complexing agent.

a)

It accepts electron pair

b)

It is neither electron pair donar or acceptor

c)

It act as electron pair donar.

d)

It exhibit covalency more than five

7.
  1. XeF6 on complete hydrolysis produces
a)

XeOF 4

b)

XeO2F 2

c)

Xe O 3

d)

Xe O 2

8.

3.Among the following , which is the strongest oxidising agent?

a)

Cl 2

b)

F 2

c)

Br 2

d)

I 2

9.

4.Which of the following is strongest acid among all ?

a)

HI

b)

HF

c)

HBr

d)

HCl

10.

5.The shape of I F 7

a)

T shape

b)

trigonal bipyramidal

c)

linear

d)

pentagonal bipyramidal

11.

The oxidation number of I in HIO 4

a)

+4

b)

+3

c)

+ 7

d)

+ 5

12.

The colour of chorine gas

a)

yellow

b)

reddish brown

c)

greenish yellow

d)

violet

13.

The correct order of acidic strength of hydrogen halides are

a)

HF<HCl<HBr<HI

b)

HF<HBr<HCl<HI

c)

HI<HBr<HCl<HF

d)

HI<HCl<HBr<HF

14.

Pick out the correct statement

a)

Chlorine water on standing loses its yellow colour due to the formation of HBr

b)

Bleaching property of chlorine is due to the formation of nascent oxygen

c)

Chlorine converts SO2 to SO3

d)

The bleaching effect of chlorine is temporary.

15.

The only one oxoacid of fluorine is

a)

HOF2

b)

HOFO

c)

HOF

d)

HOF3

16.

In the interhalogen compound XX', which among the following statement is correct

a)

X is larger halogen, X' is smaller halogen

b)

X is smaller halogen, X' is larger halogen

c)

Both X and X' are of the same size

d)

Size of X and X' doesn't matter

17.

When Cl2 and F2 are reacted in equal volumes, the product formed is

a)

ClF2

b)

ClF

c)

ClF3

d)

Cl2F

18.

Sulphur in the vapour state is diamagnetic.

a)

True

b)

False

19.
Most reactive elemental gas. 
a)
Oxygen
b)
Fluorine
c)
Chlorine
d)
Hydrogen
20.
Chalcogens are 
a)
Group 15 elements
b)
Group 16 elements
c)
Group 17 elements
d)
Group 18 elements
21.
How many elements are in the Noble Gas family?
a)
4
b)
5
c)
6
d)
7
22.
All elements in the Halogen family react violently because 
a)
Halogens have 1 valence electron that they give away readily to other elements in reactions
b)
Halogens have 7 valence electrons which gives up massive energy when they give all seven to other elements
c)
Halogens need only 1 electron which they will violently take from other elements 
d)
Halogens only react violently with water 
23.

Bismuth is a

a)

Metalloids

b)

Non metal

c)

Metal

d)

None of the above

24.

Nitrogen and phosphorus are

a)

Non metals

b)

Metals

c)

Metalloids

d)

None of the above

25.

P-block elements are those elements in which last electron enters in

a)

P ortibal

b)

S orbital

c)

d orbital

d)

None of the above

26.

In group 15 elements as we move down the group

a)

Non metallic character increase

b)

Metallic character increase

c)

Both

d)

None the above

27.

Maximum covalency of nitrogen is

a)

6

b)

8

c)

9

d)

4

28.

It is the strongest oxidising agent and most reactive element among the halogens.

a)

F

b)

Cl

c)

Br

d)

I

29.

Which of the following elements can be involved in pπ–dπ bonding?

a)

Carbon

b)

Nitrogen

c)

Boran

d)

Phosphorous

30.

Bond dissociation enthalpy of E—H (E = element) bonds is given below. Which of the compounds will act as strongest reducing agent?

Compound NH3 PH3 AsH3 SbH3

Δdiss (E—H)/kJ mol–1 389 322 297 255

a)

NH3

b)

PH3

c)

AsH3

d)

SbH3

31.

Which of the following elements does not show allotropy?

a)

Nitrogen

b)

Bismuth

c)

Antimony

d)

Arsenic

32.

Which of the following statements is wrong?

a)

Single N–N bond is stronger than the single P–P bond.

b)

PH3 can act as a ligand in the formation of coordination compound with transition elements.

c)

NO2 is paramagnetic in nature.

d)

Covalency of nitrogen in N2O5 is four

33.

A brown ring is formed in the ring test for NO3– ion. It is due to the formation of

a)

[Fe(H2O)5 (NO)]2+

b)

FeSO4.NO2

c)

[Fe(H2O)4(NO)2]2+

d)

FeSO4.HNO3

34.

Which of the following are peroxoacids of sulphur?

a)

H2SO5 and H2S2O8

b)

H2SO5 and H2S2O7

c)

H2SO5 and H2S2O8

d)

H2S2O6 and H2S2O7

35.

In solid state PCl5 is a _________.

a)

covalent solid

b)

octahedral structure

c)

ionic solid with [PCl6]+ octahedral and [PCl4]– tetrahedra

d)

ionic solid with [PCl4]+ tetrahedral and [PCl6]– octahedra

36.

SF6 is known but SCl6 is not________

a)

Due to small size of fluorine six F – ion can be accomodated around sulphur whereas chloride ion is comparatively larger in size, therefore, there will be interionic repulsion

b)

Due to absence of vacant d orbital

c)

Chlorine have more electron gain enthalpy than

d)

none of these

37.

How many electrons do Halogens have in their outer shell?

a)

0

b)

1

c)

6

d)

7

38.

Which of the "Halogens" has yellowish green color?

a)

Chlorine

b)

Bromine

c)

Flourine

d)

Iodine

39.

As you move down the group, halogens' reactivity...

a)

increases

b)

decreases

c)

doesn't change

d)

shows no trend.

40.
At room temperature, iodine is a....
a)
Gas
b)
Liquid
c)
Solid
41.

The nucleus of which halogen is best at attracting electrons?

a)

fluorine

b)

iodine

c)

bromine

d)

chlorine

42.

Which of the halogens could able to make the strongest ionic bond with Sodium metal?

a)

Iodine

b)

Bromine

c)

Chlorine

d)

Flourine

43.

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

a)

decreases, increases

b)

increases, increases

c)

increases, decreases

d)

stays the same, increases

44.

Which halogen would be able to replace chlorine in sodium chloride?

a)

Flourine

b)

Bromine

c)

Iodine

d)

Astatine

45.

Which statement is true about halogens?

a)

Form covalent compounds with other non-metallic elements

b)

A less reactive halogen will displace a more reactive element form its ionic salt

c)

Form ionic compound with hydrogen

d)

form negative ion of charge -2

46.

The process by which solid iodine particles change directly to gas without first becoming a liquid is called ____.

a)

evaporation

b)

ionization

c)

condensation

d)

sublimation

47.

Choose the best answer: Halogens exist as

a)

atoms

b)

diatomic molecules

c)

triatomic molecules

d)

ions

48.

The melting and boiling points of halogens __________ down group VII.

a)

stay the same

b)

decrease

c)

increase

49.

The most reactive halogen in group VII is

a)

fluorine

b)

chlorine

c)

bromine

d)

iodine

50.

Fluorine is able to displace bromine from sodium bromide solution because

a)

fluorine is more reactive than bromine

b)

fluorine is less reactive than bromine

c)

sodium is very reactive

51.

The halogens above bromine in Group VII are

a)

darker in colour

b)

gases

c)

less reactive

d)

more dense

52.

Chloride, Cl-, has a -1 charge because during reaction, chlorine atom

a)

accepted 1 electron

b)

lost 1 electron

c)

lost 2 electrons

d)

accepted 2 electrons

53.

The number of valence electrons each halogen atom has is

a)

1

b)

6

c)

7

d)

8

54.

The chemical formula of sodium bromide is

a)

NaBr2

b)

NaBr3

c)

NaBr

d)

NaBr4

55.

The following halogens are placed in order of increasing reactivity:

a)

Iodine, bromine, chlorine, fluorine

b)

Fluorine, bromine, chlorine, iodine

c)

Chlorine, fluorine, bromine, iodine

d)

Iodine, chlorine, fluorine, bromine

56.

When chlorine gas is delivered into a solution of potassium bromide,

a)

potassium chloride and bromine is formed.

b)

there is no observable reaction.

c)

the solution remains colourless.

d)

chlorine is unable to displace bromine.

57.

At room temperature, iodine is a....

a)

Gas

b)

Liquid

c)

Solid

58.

Which halogen has the lowest melting point and boiling point?

a)

Fluorine

b)

Bromine

c)

Iodine

d)

Chlorine

59.

In order to become stable, halogens need to.....

a)

Gain an electron

b)

Lose an electron

60.

At room temperature, chlorine is...

a)

a yellow-green gas

b)

a brown gas

c)

a green liquid

d)

a brown liquid

61.

Which halogen is a liquid in room conditions?

a)
b)
c)
d)
62.

Which halogen is a reddish-brown liquid in room conditions?

a)

Iodine

b)

Chlorine

c)

Fluorine

d)

Bromine

63.

The chemical formula of the molecule shown is

a)

CHCl

b)

CH2Cl

c)

CH4

d)

CH3Cl

64.

What is observed when chlorine gas is bubbled into colourless aqueous potassium iodide?

a)

Brown solution formed.

b)

Reaction mixture stays colourless.

c)

Effervescence is observed.

d)

Yellow-green solution formed.

65.

Cl2 (g)  +  2NaBr (aq)  →  2NaCl (aq)  +  Br2 (aq)

This is a __________________ reaction.

a)

neutralization

b)

displacement

c)

decomposition

d)

combustion

66.

Chlorine atom and argon atom both have ................

a)

3 electron shells

b)

8 valence electrons

c)

3 valence electrons

d)

8 electron shells

67.

What two types of atoms make a covalent bond?

a)

2 non-metals

b)

1 metal and 1 non-metal

c)

2 metals

68.

What type of bond involves the sharing of electrons between atoms?

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

69.

Identify the following compound as ionic or covalent: SO2

a)

ionic

b)

covalent

70.

Identify the following compound as ionic or covalent: Ca(OH)2

a)

ionic

b)

covalent

71.

When naming covalent compounds,

a)

roman numerals are needed but no prefixes required

b)

both roman numerals or prefixes are not required

c)

both roman numerals and prefixes must be included

d)

prefixes are needed but roman numerals are not required

72.
SiCl4
a)
silicon tetrachloride
b)
silicon quadchloride
c)
monosilicon tetrachloride
d)
silicon chloride
73.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
74.
What is the name of Br6F10 ?
a)
Bromium fluoride
b)
Hexabromine fluoride
c)
Bromium decafluoride
d)
none of the above
75.
What is the OFFICIAL name for H2O
a)
Hydrogen Oxide
b)
Oxygen Dinitride
c)
Agua
d)
Dihydrogen Monoxide
76.
A covalent compound made of one sulfur and two oxygen atoms would be named
a)
sulfur dioxide.
b)
sulfur oxide.
c)
disulfur oxide.
d)
sulfide oxygen.
77.

Select the correct formula for the

COVALENT COMPOUND

diphosphorus trioxide

a)

PO

b)

P3O2

c)

PO2

d)

P2O3

78.

Select the correct formula for the

COVALENT COMPOUND

carbon tetrachloride

a)

CCl

b)

CCl2

c)

C4Cl2

d)

CCl4

79.
Which of the following describes covalent bonds?
a)
Bonds form because of opposite charges
b)
Bonds form to fill outer electron shells
c)
Electrons are transferred between atoms
d)
Covalent bonds are magical
80.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
81.
What region of the periodic table contains atoms that form covalent bonds?
a)
the left side
b)
the middle
c)
the right side
d)
top left
82.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
83.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
84.
The desire for an element to have 8 atoms around it is called 
a)
Octet Rule
b)
Resonance
c)
Ionization energy
d)
Electronegativity
85.
Which of the following elements wants to bond 3 times
a)
Oxygen
b)
Phosphorous
c)
Fluorine
d)
Germanium
86.
Which of the following is a Diatomic Molecule 
a)
K2
b)
C2
c)
S2
d)
N2
87.
What is the name of this Compound
a)
P2O5
b)
Phosphorous PentaOxide
c)
Diphosphorous pentaoxide
d)
Phosphourous Oxide
88.
What is the formula for this Compound
a)
PCl
b)
PCL5
c)
PCl5
d)
Phosphorous Penta Chloride
89.
What is the name of this Molecule shape
a)
Tetrahedral
b)
Trigonal Pyramidal 
c)
Trigonal bipyramidal
d)
Bent
90.

Carbon is in 4A, so how many bonds can it form based on electrons needed to fill its outer shell?

a)

1

b)

3

c)

4

d)

5

91.

Which formula is for phosphorus trichloride?

a)

KCl3

b)

PCl3

c)

K3Cl

d)

P3Cl

92.
What is the formula for Hydrosulfuric Acid?
a)
H2(SO3)
b)
H2S
c)
H2(SO2)
d)
H2(SO4)
93.
Name HF
a)
hydrofluoric acid
b)
Hypofluoric acid
c)
hydrogen fluorine acid
d)
fluoric acid
94.
Name the acid: H3PO3
a)
hydrophosphoric acid
b)
phosphorous acid
c)
phosphoric acid
d)
phosphoric hydroxide
95.
What is the formula for nitric acid?
a)
HNO2
b)
HNO3
c)
HNO4
d)
H2NO3
96.
What is the formula for perchloric acid?
a)
H3ClO3
b)
H3ClO4
c)
HClO3
d)
HClO4
97.
HNO2
a)
hydronitrogen
b)
hydrogen nitrogen oxygen
c)
nitrous acid
d)
nitric acid
98.
HBr
a)
hydrogen bromine acid
b)
hydrobromide acid
c)
hydrobromic acid
99.

What is the name of Si3H8?

(a)  

100.

What is the name of CF4?

(a)  

101.

What is the formula for tetranitrogen hexahydride

a)

N5H7

b)

N6H8

c)

N4H6

d)

N3H10

102.

What is the name of P8Br10

(a)  

103.

What is the formula for heptacarbon nonaiodide

a)

C8I6

b)

C5I4

c)

C6I10

d)

C7I9

104.

What is the name of ClF?

(a)  

105.

What is the formula for dihydrogen monosulfide?

a)

H2S

b)

H10S9

c)

H3S4

d)

HS2

106.

What is the name of NBr3

(a)  

107.

What is the name of Si6F8

(a)  

108.

What is the formula for pentasulfide dichloride?

a)

S5Cl2

b)

S4Cl2

c)

S7Cl2

d)

S4Cl3

109.

What is the name of H10N8

(a)  

110.

Which of the following is the formula of heptacarbon nonachloride?

a)

C9Cl7

b)

C6Cl4

c)

C7Cl9

d)

C5Cl6

111.

The reactant that limits the extent of the reaction is called the (a)   .

112.

The (a)   of a chemical reaction is the amount of product produced by the reaction in reality.

113.

A(n) (a)   is a ratio between the number of moles of any two substances in a balanced chemical equation.

114.

If a portion of reactant remains after the reaction is completed, then that reactant is said to be the (a)   .

115.

The (a)   is the maximum amount of product that can be produced from a given amount of reactant.

116.

(a)   is the study of the numerical relationships between products and reactants in a chemical reaction.

117.

The (a)   of a reaction gives the ratio of the actual yield to the theoretical yield.

118.

The amount of product formed during a reaction depends on the (a)   .

119.

Rarely does the actual yield of a reaction equal the (a)   .

120.

Stoichiometry is based on the law of conservation of ___.

a)

charge

b)

volume

c)

reactants

d)

mass

121.

In a balanced chemical equation, the numbers of individual particles and the numbers of moles of particles are represented by the ___.

a)

chemical symbols

b)

coefficients

c)

subscripts

d)

molar masses

122.

Mole ratios for a reaction are obtained from the ___.

a)

balanced chemical equation

b)

total mass of products

c)

periodic table

d)

molar masses

123.

In the decomposition reaction of compound AB into substances A and B, what is the number of mole ratios that can be formed?

a)

3

b)

9

c)

6

d)

1

124.

Calculating the mass of a reactant and product from the number of moles of another product or reactant in a chemical equation is an example of a ___.

a)

mass-to-mass conversion

b)

mole-to-mole conversion

c)

mass-to-mole conversion

d)

mole-to-mass conversion

125.

Limiting a reactant is often accomplished by ___.

a)

using an excess of another reactant

b)

overcoming conservation of mass

c)

slowing down a chemical reaction

d)

producing excess product

126.

In a reaction, substances A and B form substance C. If the actual mole ratio of substance B to substance A is less than the balanced equation mole ratio of substance B to substance A, substance B is the ___.

a)

product

b)

actual yield

c)

limiting reactant

d)

excess reactant

127.

Percent yield of a product is a measure of a reaction's ___.

a)

heat production

b)

spontaneity

c)

rate

d)

efficiency

128.

The actual yield of a product is ___.

a)

independent of the reactants

b)

the same as its theoretical

c)

a negative value

d)

measured experimentally

129.

2C8H18 (g) + 25O2 (g) → 16CO2 (g) + 18H2O(l)2C_8H_{18\ \left(g\right)}\ +\ 25O_{2\ \left(g\right)}\ \rightarrow\ 16CO_{2\ \left(g\right)}\ +\ 18H_2O_{\left(l\right)}

How many molecules of carbon dioxide are represented by the equation?

(a)  

130.

2C8H18 (g) + 25O2 (g) → 16CO2 (g) + 18H2O(l)2C_8H_{18\ \left(g\right)}\ +\ 25O_{2\ \left(g\right)}\ \rightarrow\ 16CO_{2\ \left(g\right)}\ +\ 18H_2O_{\left(l\right)}

How many moles of octane are represented by the equation?

(a)  

131.

2C8H18 (g) + 25O2 (g) → 16CO2 (g) + 18H2O(l)2C_8H_{18\ \left(g\right)}\ +\ 25O_{2\ \left(g\right)}\ \rightarrow\ 16CO_{2\ \left(g\right)}\ +\ 18H_2O_{\left(l\right)}

What is the simplified mole ratio of the octane to carbon dioxide. (Write your ratio using the format A:B, where A and B are your numbers)

(a)  

132.

2C8H18 (g) + 25O2 (g) → 16CO2 (g) + 18H2O(l)2C_8H_{18\ \left(g\right)}\ +\ 25O_{2\ \left(g\right)}\ \rightarrow\ 16CO_{2\ \left(g\right)}\ +\ 18H_2O_{\left(l\right)}

What is the simplified mole ratio of oxygen to octane. (Write your ratio using the format A:B, where A and B are your numbers)

(a)  

133.

A solid is a state of matter that has a(n)

a)

indefinite volume and indefinite shape

b)

definite volume and a definite shape

c)

definite volume and an indefinite shape

d)

indefinite volume and a definite shape

134.
In which state of matter are particles packed tightly together in fixed positions?
a)
gas 
b)
solid
c)
liquid
d)
plasma
135.
Particles of a liquid
a)
are tightly packed together and stay in a fixed position
b)
have no viscosity
c)
decrease in volume with increasing temperature
d)
are free to move in a container but are in close contact with one another
136.
In which state of matter do particles spread apart and fill all the space available to them? 
a)
crystal
b)
liquid
c)
gas
d)
solid
137.
The change from a  liquid to solid, or the reverse of melting, is called
a)
condensation
b)
boiling
c)
sublimation
d)
freezing
138.

The freezing point of water is the same as its

a)

melting point

b)

boiling point

c)

sublimation point

d)

evaporation point

139.

An uncovered pot of soup is simmering on a stove, and there are water droplets on the wall above the back of the stove. What sequence can you infer has occurred?

a)

melting, then boiling

b)

freezing, then thawing

c)

vaporization, then condensation

d)

condensation, then vaporization

140.
The amount of space that a gas takes up is its
a)
volume
b)
mass
c)
pressure
d)
density
141.
Which state of matter undergoes changes in volume most easily?
a)
solid
b)
liquid
c)
gas
d)
frozen
142.
During the process of sublimation
a)
a solid turns directly into a gas
b)
a solid turns into a liquid
c)
a gas turns directly into a solid 
d)
 a liquid turns into a gas
143.

In a(n) (a)   , the particles are packed closely together, but they can move past each other freely.

144.

The common state of matter that does not have a definite shape or a definite volume is a(n) (a)   .

145.

The characteristic temperature at which a pure solid changes to a liquid is its (a)   point.

146.

A shrinking puddle is an example of (a)   , or vaporization that takes place only on the surface.

147.

(a)   occurs when a liquid changes to a gas below its surface as well as at the surface.

148.

In which state of matter are the particles least able to move?

a)

A

b)

B

c)

C

149.

Which of these three states represents a liquid?

a)

A

b)

B

c)

C

150.

Which of these three states would you expect to be the most affected by the volume of its container?

a)

A

b)

B

c)

C

151.

The most penetrating form of nuclear radiation is

a)

gamma rays

b)

beta rays

c)

alpha rays

d)

positrons

152.

In an atom, the strong nuclear force acts on

a)

protons and neutrons

b)

protons only

c)

protons, neutrons, and electrons

d)

neutrons only

153.

During the process of electron capture, an electron from outside the nucleus joins with a proton to form...

a)

a neutron

b)

a gamma ray

c)

a positron

d)

another proton

154.

The half life of calcium-47 is about 5 days. Starting with 64g of this isotope, what would be the amount remaining after 20 days?

a)

8g

b)

16g

c)

4g

d)

32g

155.

One product of all nuclear fusion reaction is

a)

a larger nucleus

b)

electrons

c)

protons

d)

neutrons

156.

Mass is lost or gained in ___.

a)

all nuclear fusion reactions

b)

all chemical reactions

c)

all nuclear fission reactions

d)

all chemical and nuclear reactions

157.

A chain reaction will NOT take place in a piece of uranium if ___.

a)

the piece of uranium is too large

b)

there are too many neutrons

c)

the temperature is too low

d)

there are too few neutrons

158.

One of the most serious problems surrounding the use of nuclear power plants is ___.

a)

the high cost of coolant needed

b)

a lack of uranium

c)

initiating a chain reaction in the fuel

d)

finding a way to dispose of spent fuel rods

159.

Fusion reactions require ___.

a)

very rare elements for use as fuel

b)

incredibly high temperatures

c)

very heavy nuclei

d)

no initial energy

160.

When this isotope decays by beta emission, the isotope formed is ___.

a)

b)

c)

d)

161.

The isotope formed by the alpha decay of this isotope is.

a)

b)

c)

d)

162.

The decay of this Tm isotope yields this Er isotope and ___.

a)

γ\gamma

b)

e-

c)

e+

d)

163.

Atoms located above the band of stability on a graph of numbers of neutrons versus number of protons are usually unstable because they contain too many ___.

a)

neutrons

b)

protons

c)

nucleons

d)

electrons

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