CHM 201 CBT PRACTICE TEST

Take your time to read instructions before taking this test.

There are 40 questions which you are to answer in 15 minutes that gives you roughly 30 seconds per question.

If you can get at least 60%, you can be rest assured that you’ll ace CHM 201 exam

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In a normal exam you will be asked between 40 – 60 questions but I only arranged 40 questions

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Inorganic Chemistry

1 / 40

1.

The purest and most stable form of silica is ____________

A. Quartz

B. Tridymite

C. Flint

D. Cristobalite

2 / 40

2.

Which one of the following compounds is formed when carbides are decomposed by water or dilute acids?

A. Methanol

B. Propanal

C. Ethylene

D. Acetylene

3 / 40

3.

Other halogens apart from fluorine exhibit variable oxidation states due to ________.

A. Other halogens have vacant d orbital whereas fluorine doesn't

B. None of the options

C. Other halogens have vacant p orbital whereas fluorine doesn't

D. All the options

4 / 40

4.

Which of the options below indicates how carbon behaves differently from other members of Group 4?

A. Carbon has a maximum covalency of 6 while other members have 4

B. Carbon has a much higher electronegativity and higher ionisation energy than other elements in the group

C. Carbon forms complex compounds while the other members do not

D. Carbon forms solid oxides while the other members do not

5 / 40

5.

The compound among the options below with the least bond energy is ___________.

A. SbH3

B. BiH3

C. NH3

D. PH3

6 / 40

6.

_____ is the main types of halides formed by Group 5 elements.

A. pentahalides

B. Dihalides

C. trihalides

D. Tetrahalides

7 / 40

7.

Tin is obtained by the ______.

A. Oxidation of oxides of tin with carbon

B. Oxidation of oxides of tin with Fe

C. Reduction of oxides of tin with H

D. Reduction of oxides of tin with carbon

8 / 40

8.

Tin exhibit polymorphism because of _____________ .

A. It has a stable configuration

B. It is a metal as well as a metalloid

C. It exists in two crystalline forms

D. It can function as a conductor and semi-conducto

9 / 40

9.

The bond energy of N-N bond in hydrazine is very small due to _______.

A. Repulsion of the nonbonding electrons which weaken the N-N bond

B. Attraction and repulsion between N-N bond and N-H bond in hydrazine

C. Repulsion between N-N bond and N-H bond in hydrazine

D. Attractive and repulsion of the nonbonding electrons and the N-N bond in hydrazine

10 / 40

10.

The difference between silica and silicate is ________

A. Silica is made of SiO2 units whereas silicate is made of SiO4 units

B. Silica is made of SiO4 units whereas silicate is made of SiO6 units

C. Silica is made of SiO6 units whereas silicate is made of SiO2 units

D. Silica is made of SiO4 units whereas silicate is made of SiO2 units

11 / 40

11.

The forms of carbon include _________.

A. Coke and carbon black

B. Coke, charcoal and carbon black

C. Coke and charcoal

D. Charcoal and carbon black

12 / 40

12.

Group 5 elements form compounds mainly in two oxidation states, namely ____________.

A. +3 and +6

B. +3 and +2

C. +3 and +5

D. +2 and +5

13 / 40

13.

The most stable hydride of phosphurous is _________.

A. Phosphorus dihydride

B. Phosphorus pentahydride

C. Phosphine

D. Phosphide

14 / 40

14.

____________ are formed by combination of carbon with some transition metals.

 

A. Alloys

B. Polymers

C. Interstitial carbides

D. Coordination compounds

15 / 40

15.

The tendency of gaining an electron to acquire a stable noble gas configuration makes the halogens ________.

A. Have low electron affinity

B. susceptible to oxidation

C. High electron affinity

D. Low ionization energy

16 / 40

16.

Boron and silicon combine with carbon to form ___________.

 

A. Methanides

B. Catenate compounds

C. Acetylides

D. Covalent carbides

17 / 40

17.

Mineral silicates plays an important role in national economy because from it is produced _______.

A. Glass, paints,ceramics

B. Glass, ceramics,cement

C. Plastics, ceramics,paints

D. Cement,plastics,glass

18 / 40

18.

Dilute nitric acid will oxidise HI to ____________.

A. H

B. HIO3

C. I

D. HIO4

19 / 40

19.

In the gaseous state phosphorus exist as _________,

A. P4

B. P

C. P2

D. P6

20 / 40

20.

Silica gel is _____________ form of Silicon dioxide.

A. Gaseous

B. Semi solid

C. Amorphous

D. Crystalline

21 / 40

21.

All the elements of Group 5 can expand their octet except _____________.

A. Arsenic

B. Phosphorus

C. Nitrogen

D. Bismuth

22 / 40

22.

Sandstone, granite and slate are examples of ________.

A. Carbides

B. Cristobalite

C. Natural silicates

D. Silica

23 / 40

23.

Concentrated nitric acid readily oxidises solid non metals and metalloids to their respective _____________.

A. Ions

B. Salts

C. Hydrides

D. Oxoacids or hydrated oxides

24 / 40

24.

________ occurs in the elemental state as diamond and graphite.

A. germanium

B. Silicon

C. Tin

D. Carbon

25 / 40

25.

Ammonifying bacteria present in the soil decompose plants and animals when they die into ________

A. Nitrogen and oxides

B. Nitrogenous and hydrides

C. Ammonium and hydrides

D. Nitrogen and ammonium compounds

26 / 40

26.

Hydrazine can act as a coordinating ligand forming complexes with metal ions because of _________.

A. Hydrazine is highly reactive

B. The bond energy of N-N bond in hydrazine is very small

C. Hydrazine is stable

D. It has lone pairs of electrons

27 / 40

27.

Ammonia functions as an electron donor because of __________.

A. All the options

B. Lone pair of electron on the nitrogen atom available for donation

C. None of the options

D. The nitrogen atom being more electronegative than hydrogen draws the electron pair it shares with hydrogen to itself, and can therefore donate it

28 / 40

28.

Hydrazine has how many lone pairs of electrons?

 

A. 2

B. 1

C. 3

D. 0

29 / 40

29.

The chief constituent of glass is ____________.

A. Silica

B. Silicone byhydride

C. Silicate

D. Silicone

30 / 40

30.

The reaction C6H6 + HNO3 will give _____________.

 

A. C6H5NO3 + H2

B. C6H5NO + H2O2

C. C6H5NO2 + H2O2

D. C6H5NO2 +H2O

31 / 40

31.

Dilute nitric acid will oxidise H2S to ____________.

A. H2S03

B. H

C. H2SO4

D. S

32 / 40

32.

Which of the options below shows how carbon behaves differently from the rest of the elements in its group?

A. Carbon form both gaseous and solid oxides whereas others form only gaseous oxides

B. Carbon has a maximum covalency of 4 and can therefore form complex compounds

C. Carbon is the only element in the group that can form stable derivatives with double and triple bonds

D. Carbon has a much lesser electronegativity than other elements in the group

33 / 40

33.

The element with the highest electron affinity amongst the halogens is ___________.

A. Chlorine

B. Astatine

C. Bromine

D. Fluorine

34 / 40

34.

Concentrated nitric acid behaves as an ______________.

A. Reducing agent

B. Oxidizing agent

C. None of the options

D. Redox agent

35 / 40

35.

Carbon dioxide is used in fire extinguishers because of ________.

A. It forms carbonates with bases

B. It can be transformed to solid called dry ice

C. It is an acidic oxide

D. It does not support combustion

36 / 40

36.

The tendency of ________ to form multiple bonds easily is due to its high bond energy and small atomic radius.

A. Lead

B. Silicon

C. Germanium

D. Carbon

37 / 40

37.

The reactivity of the various allotropes of phosphorus towards other substances decreases in the order?

A. Black-red-white-brown

B. brown-white-red-black

C. Red-brown-black-white

D. White-black-brown-red

38 / 40

38.

Diamond are used in jewellery on account of their ______.

A. Hard structure

B. Crystalline nature

C. High purity

D. High refractive index and dispersive power

39 / 40

39.

Superphosphate of lime is a more effective fertilizer than phosphate rock because of _________.

 

A. Ca(H2PO4)2 is highly reactive

B. Ca(H2PO4)2 is oxidising

C. Ca(H2PO4)2 is reducing

D. Ca(H2PO4)2 is water soluble

40 / 40

40.

_________ are formed by elements of 1,2, 3,11,12 and13 except boron.

A. Covalent carbides

B. organic carbides

C. Ionic carbides

D. Interstitial carbides

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