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Quantum Mechanics and Stereochemistry

Total questions: 100

Worksheet time: 1hrs 1mins

Name
Class
Date
1.

Isomerism that arises out of the difference in spatial arrangement of atoms or groups about the doubly bonded carbon atoms are called?

a)

Structural Isomerism

b)

Stereoisomerism

c)

Geometrical Isomerism

d)

Optical Isomerism

2.

Does this molecule exhibit optical isomerism?

a)

Yes

b)

No

3.

Does this molecule exhibit optical isomerism?

a)

Yes

b)

No

4.

Does this molecule exhibit optical isomerism?

a)

Yes

b)

No

5.

Define chirality centre

a)

also known as chiral carbon

b)

a type of enantiomer

c)

a sp3 hybridised carbon with four different groups or atoms attached to it

d)

optically active compounds

6.

Can enantiomer rotates plane-polarised light?

a)

Yes in all situations

b)

No because it is optically active

c)

Yes but it can only rotate the polarised light in opposite direction

d)

No due to its restricted rotation of carbon-carbon double bond

7.

Isomerism that arises out of the difference in spatial arrangement of atoms or groups about the doubly bonded carbon atoms are called?

a)

Structural Isomerism

b)

Stereoisomerism

c)

Geometrical Isomerism

d)

Optical Isomerism

8.

How to determine that a molecule exhibit cis-trans isomerism?

a)

Restricted rotation in a carbon-carbon single bond of alkenes

b)

Each carbon of a site of restricted rotation has 2 different atoms or groups attached to it

c)

Exist in cyclic compouds only

d)

Similar chemical properties

9.

Which of the following compounds is the enantiomer of the above compound?

a)
b)
c)
d)

All of them.

10.

Choose the incorrect option regarding isomerism:

a)

They differ in both physical and chemical properties

b)

They have different molecular formula

c)

There are two types of isomerism : Structural and Stereoisomerism

d)

Geometric and optical isomerism are two types of stereoisomerism

11.

Optical activity of a molecule is due to

a)

lack of plane of symmetry

b)

Presence of asymmetric carbons

c)

molecular asymmetry

12.

Optical isomers have different

a)

Molecular formula

b)

structures

c)

conformations

d)

configurations

13.

The instrument used to measure the optical activity of a compound

a)

Polarimeter

b)

Galvanometer

c)

Potentiometer

d)

optical meter

14.

The chiral molecule should contain the following symmetry elements

a)

Plane of symmetry

b)

Centre of symmetry

c)

Alternate axis of symmetry

d)

None of the above

15.

What property can be assigned to a carbon atom that has four different atoms or structural groups attached to it?

a)

isomerity

b)

chirality

c)

chivalry

d)

geometry

16.
How many chiral center is found in C2H5CH(OH)CH2OH?
a)
1
b)
2
c)
3
d)
4
17.
Which of the following statement is FALSE about optical isomers?
a)
At least 1 asymmetrical chiral center
b)
Mirror images of each other
c)
Non superimposable
d)
carbon center bonded to 4 groups
18.

A compound capable of forming optical isomers:

a)

has a carbon with 4 different groups

b)

is at least 4 carbons long

c)

has a mirror image

d)

reflects plane polarised light

19.

Optcial isomers have:

a)

polarised light

b)

non-superimposable mirror images

c)

mirror images

d)

superimposable mirror images

20.

Restriction of rotation about the c=c is responsible for

a)

Geometrical isomerism

b)

Stereoisomerism

c)

Metamerism

d)

All

21.

In absolute method functional group in cis isomer located cis to each other can be converted to

a)

Cyclic lactones

b)

Anhydrides

c)

Amides

d)

All

22.

By using method of cyclization cis form of maleic acid form

a)

Maleic anhydride

b)

Fumaric acid

c)

Tartaric acid

d)

Lactic acid

23.

Different xray analysis methods used for determination of geometrical isomerism is

a)

Nmr

b)

Uv

c)

Mass

d)

All

24.

Energy used for the conversion of staggered form to eclipsed form of ethane is

a)

3 kcal/mole

b)

4kcal/mole

c)

5kcal

d)

6kcal

25.

Conformations of nbutane are

a)

Antiperiplanar

b)

Anticlinal

c)

Synclinal

d)

All

26.

Energy released for conversion of chair form to halfchairform

a)

11kcal/mole

b)

12kcal/mole

c)

Both

d)

None

27.

In a stereoisomer, ________ means "on the same side" and ______ means "across from."

a)

cis; trans

b)

cis; L

c)

D; L

d)

trans; cis

28.

The two Geometric isomers shown are called:

a)

Cis/trans 1,2 dichloroethane

b)

Cis/trans 1,2 dichloroethene

c)

Cis/trans 1,2 chloroethane

d)

Cis/trans 1,2 chloroethene

29.

Can enantiomer rotates plane-polarised light?

a)

Yes in all situations

b)

No because it is optically active

c)

Yes but it can only rotate the polarised light in opposite direction

d)

No due to its restricted rotation of carbon-carbon double bond

30.

chiral centre: a ______ atom bonded with _______ different groups

a)

carbon , four

b)

hydrogen, two

c)

oxygen , four

d)

oxygen, two

31.

The number of optically active isomers of tartaric acid is

a)

4

b)

2

c)

3

d)

1

32.

Racemic mixture is formed by mixing two

a)

Chiral compounds

b)

meso compounds

c)

diastereomers with chiral carbon

d)

enantiomers with chiral carbon

33.

Which one of the following will exhibit conformational isomerism?

a)

Ethylene

b)

methane

c)

chloromethane

d)

propane

34.

Most stable conformation of cyclohexane is

a)

chair

b)

boat

c)

twist boat

d)

half chair

35.

The energy barrier for rotation of C-C bond in ethane is

a)

4 kcal/mol

b)

5 kcal/mol

c)

3 kcal/mol

d)

2 kcal/mol

36.

Which of the following compound has gauche as it stable conformer?

a)

n-butane

b)

n-propane

c)

1,2-dicloroethane

d)

1,2-dihydroxyethane

37.

Which of the following shows syn /anti isomerism?

a)

azo compounds

b)

oximes

c)

hydrazines

d)

amines

38.

The most unstable conformer in cyclohexane?

a)

Boat

b)

Chair

c)

Twist boat

d)

half chair

39.

Which of the following conformers is not a transition state?

a)

Boat

b)

half chair

c)

fully eclipsed

d)

twist boat

40.

Which other factor along with torsion decide the stability of conformer?

a)

Intermolecular hydrogen bonding

b)

Intramolecular hydrogen bonding

c)

coordinate bonding

d)

ionic bonding

41.

Identify the conformation

a)

Boat

b)

Chair

c)

twist boat

d)

half chair

42.
How many quantum numbers are needed to describe the energy state of an electron in an atom?
a)
1
b)
2
c)
3
d)
4
43.
The angular momentum quantum number indicates the
a)
orientation an orbital around the nucleus.
b)
shape of an orbital.
c)
direction of the spin of the electron in its orbital.
d)
main energy level of an orbital.
44.
An electron fro which n=4 has more ____ than an electron for which n=2.
a)
spin
b)
particle nature
c)
energy
d)
wave natrue
45.
The set of orbitals that are dumbbell shaped and directed along the x, y, and z axes are called 
a)
d orbitals.
b)
p orbitals.
c)
f orbitals.
d)
s orbitals
46.
The total number of orbitals that can exist at the second main energy level is
a)
2
b)
3
c)
4
d)
8
47.
How many orientations can an d orbital have about the nucleus?
a)
1
b)
2
c)
3
d)
5
48.
The distance traveled between two successive peaks of a waves is the
a)
speed
b)
frequency
c)
wavelength
d)
energy
49.
A line spectrum is produced when an electron moves from one energy level
a)
into the nucleus.
b)
to another position in the same sublevel.
c)
to a higher energy level.
d)
to a lower energy level.
50.
If electrons in an atom have the lowest possible energies, the atom is in the
a)
ground state.
b)
inert state.
c)
excited state.
d)
radiation-emitting state.
51.
An orbital that can never exist according to the quantum description of the atom is
a)
6d.
b)
3f.
c)
3d.
d)
8s.
52.
According to the Bohr model of the atom, the single electron of a hydrogen atom circles the nucleus
a)
in specific, allowed orbits.
b)
in one fixed orbit at all times.
c)
at any of an infinite number of distances, depending on its energy.
d)
counterclockwise.
53.
The statement that no two electrons in the same atom can have the same four quantum numbers is
a)
the Pauli exclusion principle.
b)
Hund's rule.
c)
Bohr's law.
d)
the Aufbau principle.
54.

Photoelectric effect provides the evidence for the ______ nature of radiation.

a)

dual

b)

wave

c)

particle

d)

electromagnetic

55.

If the brightness of a beam of light increases without changing its color, the ______ will increase.

a)

number of photons

b)

frequency of the light

c)

energy of the photons

d)

wavelength of the photons

56.

Light of a given wavelength is used to illuminate the surface of a metal. However, no photoelectrons are emitted. In order to cause electrons to be ejected, light of __________ should be used.

a)

lower energy

b)

higher intensity

c)

shorter frequency

d)

higher frequency

57.

What is the energy, in eV, of a photon that has a wavelength of 620 nm?

a)

1eV

b)

2eV

c)

3eV

d)

4eV

58.

The energy of a photon is directly proportional to its _____ and inversely proportional to its ______.

a)

intensity - speed

b)

wavelength - frequency

c)

frequency - wavelength

d)

intensity - wavelength

59.

In the photoelectric effect, if the incident photons have a wavelength that is larger than the threshold wavelength, _______.

a)

electrons will be ejected from the metal surface

b)

there will be photoelectric current

c)

no electrons will be emitted from the metal surface

d)

the kinetic energy of the ejected electrons increases

60.

What does the slope of the graph represent?

a)

Speed of light

b)

Mass of a photon

c)

Planck's constant

d)

Stopping potential

61.

A metal with a work function of 3.5 eV is exposed to photons with an energy of 3.7 eV. What is the maximum kinetic energy of the emitted photoelectrons?

a)

0.2 eV

b)

0.9 eV

c)

1.1 eV

d)

7.7 eV

62.

What is the energy of a photon with a frequency of 5x1014 Hz? (you need to do calculation. You have enough time)

a)

2.5x10-19 J

b)

3.0x10-19 J

c)

3.3x10-19 J

d)

4.5x10-19 J

63.

A particle of light is called a...

a)

Photoelectron

b)

Photon

c)

Proton

d)

Electron

64.

The only way to increase the number of photoelectrons emitted is by increasing the _________ of the light

a)

Intensity

b)

Wavelength

c)

Frequency

d)

Energy

65.

What color of light has the greatest energy per photon?

a)

Red

b)

Green

c)

Blue

d)

Violet

66.

The energy of photoelectrons emitted from a metal surface can be increased by

a)

using light of higher frequency.

b)

using light of longer wavelength.

c)

using light of higher intensity.

d)

using monochromatic, polarized light.

67.
The photoelectric effect only occurs if the light shining on the metal is:
a)
coherent.
b)
above a minimum intensity.
c)
above a minimum frequency.
d)
above a minimum wavelength.
68.
The equation for the photoelectric effect is 
eV = hf - Φ
The graph of electron energy against frequency is
a)
a straight line through the origin
b)
 a straight line gradient h
c)
a straight line with a positive y intercept
d)
not a straight line
69.

The SI unit of frequency is the __________.

a)

meter

b)

second

c)

hertz

d)

meter per second

70.

When light of specific frequencies is shined on a surface, electrons are ejected from the surface. This is the idea behind...

a)

Quantization of Energy

b)

Photoelectric Effect

c)

Compton Effect

d)

deBroglie Waves

e)

Uncertainty Principle

71.

Compton effect expt. is carried out with

a)

x ray

b)

gama ray

c)

visible light

d)

heat waves

72.

Compton scattering establishes

a)

photonic nature of electromagnetic wave

b)

wave nature of electromagnetic wave

c)

both wave and particle nature of electro magnetic

d)

electron is a matter

73.

Elements of low atomic mass are preferred in Compton effect

a)

low atomic mass elements are easily available

b)

with low atomic mass coulombic attaraction is less and greater probability of making electron free

c)

with low atomic mass coulombic attaraction is high and greater probability of making electron free

d)

with low atomic mass coulombic attaraction is less and lesser probability of making electron free

74.

In Compton effect we use X-ray because

a)

it is easy to produce

b)

it has very small wave length

c)

x-ray photon has very high energy

d)

it is a X-ray diffraction experiment

75.

The ratio of de Broglie wave length of a moving proton and moving electron is

a)

2:1

b)

1:2

c)

1:1

d)

3:1

76.
What element is represented in this Bohr Model?
a)
Helium
b)
Hydrogen
c)
Argon
d)
Silver
77.

How many electrons can the 3rd energy level hold?

a)

1

b)

18

c)

16

d)

2

78.

How many valence electrons chlorine (Cl) contain?

a)

1

b)

3

c)

6

d)

7

79.

Neils Bohr's atomic theory is similar to the concept of the

a)

solar system

b)

circles with dots

c)

spinning wheel

d)

None of the above

80.

'Quantum numbers' are...

a)

used to describe amount of things an atom can react with.

b)

used when describing number of electrons.

c)

used when describing the energy levels available to atoms and molecules.

d)

used when labelling parts of a wave.

81.

When an electron absorbs enough energy, it jumps up to a higher level. This is called

a)

absorption state

b)

excitation state

c)

emission state

d)

relaxation state

82.

According to Bohr, the energy absorbed by an electron upon excitation comes in a fixed amount called

a)

exact energy

b)

fixed energy

c)

quantized energy

d)

None of the above

83.
Which statement about the photoelectric effect is correct?
a)
Electrons are emitted instantaneously.
b)
Electrons are not emitted below a certain wavelength.
c)
You can change the energy of the electrons by changing the intensity.
d)
Electron energy is independent of frequency.
84.

In Heisenberg's uncertainty principle the uncertainty of ----& ----is discussed

a)

Position & mass

b)

Positon and temperature

c)

Postion and velocity

d)

Position and energy

85.

What is momentum?

a)

the speed of a particle

b)

mass times velocity

c)

the total movement in a system

d)

mass divided by velocity

86.

Consequence of Heisenberg's uncertainty principle is ---------

a)

Rules out the 2dimensional path around the nucleus for the electrons

b)

Predict the existence of region around nucleus for the electrons

c)

Establishes the wave character for the electrons

d)

All the above statements

87.

If uncertainty in position of an electron is zero, the uncertainty in its momentum will be

a)

< h/4ℼ

b)

>h/4ℼ

c)

0

d)

∞

88.

Calculate the uncertainty in the position of particle if the uncertainty in momentum is 1x10-3gcm/s

a)

0.527x10-24cm

b)

0.302x10-24cm

c)

1.325x10-23cm

d)

1.206x10-23cm

89.

What are the shapes of p orbitals ?

a)

cloverleaf

b)

spherical

c)

dumbbell

90.

How many 4d orbitals are there in an atom?

a)

1

b)

3

c)

5

91.

Write a set of quantum numbers for a 4d orbital.

a)

(4,1,0, -1/2)

b)

(4,2,-2, +1/2)

c)

(4,0,2,-1/2)

92.

How many electrons can occupy any single subshell orbital?

a)

1

b)

2

c)

6

d)

10

93.
An electron occupies the lowest energy orbital that can receive it.
a)
Hund’s rule
b)
Pauli exclusion principle
c)
Bohr model of the atom
d)
Aufbau principle
94.
All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Core Notation
95.
As particles are exposed to colder temperatures they _____
a)
speed up
b)
slow down
c)
stay the same
d)
become ions
96.
What is the change of state from a solid straight to a gas called?
a)
melting
b)
evaporating
c)
freezing
d)
sublimation
97.
An inflated balloon is placed in a refrigerator. Which statement describes the movement of the gas particles in the balloon?
a)
The particles move more slowly and become closer together.
b)
The particles move more slowly and become further apart.
c)
The particles move faster and become closer together.
d)
The particles move faster and become further apart. 
98.
Hund’s rule states…
a)
Atomic orbitals have opposite spins and 2 electrons each
b)
Electrons occupy orbitals of highest energy first and energy level changes as you go up
c)
Electrons occupy orbitals of lowest energy first, starting with 1s
d)
Electrons occupy orbitals of equal energy, one electron enters EACH orbital ONE AT A TIME until orbitals of the entire energy level have one electron with the SAME SPIN.
99.
The quantum number "n" represents:
a)
electron spin
b)
orbital
c)
sublevel
d)
main energy level
100.
Which scientist developed the Quantum Mechanical
a)
E. Schroedinger
b)
W. Heisenberg
c)
J. Dalton
d)
N. Bohr

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