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Atomic.

Total questions: 86

Worksheet time: 2hrs 52mins

Name
Class
Date
1.

1. What element is represented in this Bohr Model?

a)

Carbon

b)

Hydrogen

c)

Aluminum

d)

Lithium

2.

In the Bohr model, how do electrons travel?

a)

Electrons move in and out of the nucleus

b)

Electrons do not move

c)

Electrons move in circular orbits around the nucleus

d)

Electrons move in a straight line

3.

What is n defined as in the Bohr's atomic model?

a)

a letter

b)

Principal quantum number

c)

Principal quantum variable

d)

a quantitiy

4.

What is the spectrum region for Balmer series?

a)

Visible

b)

Ultraviolet

c)

Infrared

d)

X-rays

5.

How the second line in the Balmer series of the hydrogen spectrum is formed?

a)

n=6 to n=4

b)

n=3 to n=1

c)

n=5 to n=3

d)

n=4 to n=2

6.

For Lyman series, the first line is the

a)

highest energy

b)

highest frequency

c)

longest wavelength

d)

none of the above

7.

Which line spectrum series in ultraviolet region?

a)

Lyman

b)

Balmer

c)

Paschen

d)

Brackett

8.

Which of the following is the first postulate of Bohr's atomic model?

a)

Electron moves in circular orbits around the nucleus

b)

The energy of an electron in a hydrogen atom is quantised

c)

If energy is supplied, electron absorbs the energy and is promoted from a lower energy level to a higher energy level

d)

At excited state, the electron is unstable. It will fall back to lower energy level and releases a specific amount of energy (photon) in the form of light

9.

Which of the following is the second postulate of Bohr's atomic model?

a)

Electron moves in circular orbits around the nucleus

b)

The energy of an electron in a hydrogen atom is quantised

c)

If energy is supplied, electron absorbs the energy and is promoted from a lower energy level to a higher energy level

d)

At excited state, the electron is unstable. It will fall back to lower energy level and releases a specific amount of energy (photon) in the form of light

10.

Which of the following is the third postulate of Bohr's atomic model?

a)

Electron moves in circular orbits around the nucleus

b)

The energy of an electron in a hydrogen atom is quantised

c)

If energy is supplied, electron absorbs the energy and is promoted from a lower energy level to a higher energy level

d)

At excited state, the electron is unstable. It will fall back to lower energy level and releases a specific amount of energy (photon) in the form of light

11.

Which of the following is the fourth postulate of Bohr's atomic model?

a)

Electron moves in circular orbits around the nucleus

b)

The energy of an electron in a hydrogen atom is quantised

c)

If energy is supplied, electron absorbs the energy and is promoted from a lower energy level to a higher energy level

d)

At excited state, the electron is unstable. It will fall back to lower energy level and releases a specific amount of energy (photon) in the form of light

12.

What is the spectrum region for Lyman series?

a)

Visible

b)

Ultraviolet

c)

Infrared

d)

X-rays

13.

What is the spectrum region for Paschen series?

a)

Visible

b)

Ultraviolet

c)

Infrared

d)

X-rays

14.

What is the spectrum region for Brackett series?

a)

Visible

b)

Ultraviolet

c)

Infrared

d)

X-rays

15.

What is the spectrum region for Pfund series?

a)

Visible

b)

Ultraviolet

c)

Infrared

d)

X-rays

16.

1. What element is represented in this Bohr Model?

a)

Carbon

b)

Hydrogen

c)

Aluminum

d)

Lithium

17.

In the Bohr model, how do electrons travel?

a)

Electrons move in and out of the nucleus

b)

Electrons do not move

c)

Electrons move in circular orbits around the nucleus

d)

Electrons move in a straight line

18.

Which of the following is the first postulate of Bohr's atomic model?

a)

Electron moves in circular orbits around the nucleus

b)

The energy of an electron in a hydrogen atom is quantised

c)

If energy is supplied, electron absorbs the energy and is promoted from a lower energy level to a higher energy level

d)

At excited state, the electron is unstable. It will fall back to lower energy level and releases a specific amount of energy (photon) in the form of light

19.

Which of the following is the second postulate of Bohr's atomic model?

a)

Electron moves in circular orbits around the nucleus

b)

The energy of an electron in a hydrogen atom is quantised

c)

If energy is supplied, electron absorbs the energy and is promoted from a lower energy level to a higher energy level

d)

At excited state, the electron is unstable. It will fall back to lower energy level and releases a specific amount of energy (photon) in the form of light

20.

Which of the following is the third postulate of Bohr's atomic model?

a)

Electron moves in circular orbits around the nucleus

b)

The energy of an electron in a hydrogen atom is quantised

c)

If energy is supplied, electron absorbs the energy and is promoted from a lower energy level to a higher energy level

d)

At excited state, the electron is unstable. It will fall back to lower energy level and releases a specific amount of energy (photon) in the form of light

21.

Which of the following is the fourth postulate of Bohr's atomic model?

a)

Electron moves in circular orbits around the nucleus

b)

The energy of an electron in a hydrogen atom is quantised

c)

If energy is supplied, electron absorbs the energy and is promoted from a lower energy level to a higher energy level

d)

At excited state, the electron is unstable. It will fall back to lower energy level and releases a specific amount of energy (photon) in the form of light

22.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
23.

What is the light that you can see called?

a)

observatory light

b)

ultraviolet light

c)

visible light

d)

infrared light

24.
According to the Bohr Model, electrons are only found in specific orbits around the nucleus called __________________________
a)
Energy Levels
b)
Electron Lanes
c)
Electron Places
d)
Atomic Mass
25.

Bohr discovered that electrons are located in

a)

the nucleus

b)

inside protons

c)

electron cloud

d)

circular orbits around the nucleus

26.

When atoms _____________ energy, their electrons move to higher energy levels. These electrons _____________ energy by emitting light when they return to lower energy levels.

a)

lose, absorb

b)

absorb, lose

c)

lose, lose

d)

absorb, absorb

27.

An electron jumps from 5th shell to 2nd shell then find the number of spectral line

a)

4

b)

5

c)

6

d)

3

28.

 Energy of 2nd shell for Li(2+)Li^{\left(2+\right)}

a)

-25 ev

b)

-30.6 ev

c)

25 ev

d)

20 ev

29.

orbital Containing highest energy is

a)

6s

b)

4f

c)

3d

d)

2p

30.

The velocity of electron in 3rd orbit of hydrogen atom will be...

a)

0.729×10^8cm/s

b)

6.564×10^8cm/s

c)

19.692×10^8cm/s

d)

0.243×10^8cm/s

31.

Select the pair of atoms which have same no. Of electrons in their outermost shell

a)

Na,Ca

b)

Mg,Fe

c)

Li,K

d)

N,O

32.

The debroglie wavelength associated with a ball of mass 1kg having kinetic energy 0.5joule is

a)

6.626×10^-34m

b)

13.20×10^-34m

c)

10.38×10^-21m

d)

6.626×10-34Amstrong

33.

How many electrons are present in n=3, l=1, m= -1 0 +1

a)

2

b)

6

c)

10

d)

14

34.

For n=7, the value of l is

a)

l=6,5,4,3,2,1

b)

l= 6

c)

l=7

d)

l= 5

35.

De Broglie equation

a)

relates the momentum of a mass to its wavelength

b)

relates the energy of a mass to its wavelength

c)

relates the frequency of a mass to its wavelength

d)

relates the work function of a mass to its wavelength

36.

If the kinetic energy of an electron is increased four times, the wavelength of the de-Broglie wave associated with it would become:

a)

Two times

b)

Half

c)

One fourth

d)

Four times

37.

Calculate the wavelength in nanometer associated with a proton moving at 1.0x103 m/s (mass of proton = 1.67x10-27 kg and h= 6.63x10-34 Js)

a)

2.5 nm

b)

14.0 nm

c)

0.032 nm

d)

0.40 nm

38.

The radius of the second Bohr orbit for the hydrogen atom is:

a)

1.65 A

b)

4.76 A

c)

0 529 A

d)

2.12 A

39.

The energy required to break one mole of Cl-Cl bonds in Cl2 is 242 kJ/mol. The longest wavelength of light capable of breaking a single Cl-Cl bond is (c= 3x108 m/s and NA = 6.02x1023 mol):

a)

494 nm

b)

594 nm

c)

640 nm

d)

700 nm

40.

Ionisation energy of He+ is 19.6x10-18 J/atom. The energy of the first stationary state (n=1) of Li2+ is:

a)

8.82x10-17 J/atom

b)

4.41x10-16 J/atom

c)

-4.41x10-17 J/atom

d)

-2.2x10-15 J/atom

41.

The frequency of light emitted for the transition n=4 to n=2 of He+ is equal to the transition in H atom corresponding to which of the following:

a)

n=3 to n=1

b)

n=2 to n=1

c)

n=3 to n=2

d)

n=4 to n=3

42.

Based on the equation ΔE=−2.0x10−18 J(11n2 2−1n12)\Delta E=-2.0x10^{-18\ }J\left(\frac{1}{\frac{1}{n_{2\ }^2}-\frac{1}{n_1^2}}\right) the wavelength of the light that must be absorbed to excite hydrogen electron from level n=1 to level n=2 will be (h= 6.625x10-34 Js, C= 3x108 m/s)

a)

2.650x10-7 m

b)

1.325x10-7 m

c)

1.325x10-10 m

d)

5.300x10-10 m

43.

The de-Broglie wavelength of a car of mass 1000kg and velocity 36km/hr is:

a)

6.626x10-31 Js

b)

6.626x10-34 Js

c)

6.626x10-38 Js

d)

6.626x10-30 Js

44.

If the binding energy of the electron in a hydrogen atom is 13.6 eV, the energy required to remove the electron from the first excited state of Li2+ is:

a)

13.6 eV

b)

30.6 eV

c)

122.4 eV

d)

3.4 eV

45.

According to Bohr's theory, the angular momentum of an electron in 5th order orbit is:

a)

25h/pi

b)

1.0h/pi

c)

10h/pi

d)

2.5h/pi

46.

The de-Broglie wavelength of a tennis ball of mass 60g moving with a velocity of 10 m/s is approximately :

a)

10-31 m

b)

10-16 m

c)

10-25 m

d)

10-33 m

47.

In a hydrogen atom, if the energy of an electron in the ground state is 13.6 eV, then that in the second excited state is:

a)

1.51eV

b)

3.4eV

c)

6.04eV

d)

13.6eV

48.

In the Bohr series of lines of hydrogen spectrum, the third line from the red end corresponds to which on of the following inter-orbit jumps of the electron for Bohr orbits in an atom of hydrogen.

a)

5→25\rightarrow2

b)

4→14\rightarrow1

c)

2→52\rightarrow5

d)

3→23\rightarrow2

49.

Which of the following sets of quantum numbers is correct for an electron present in 4f orbital?

a)

n=4, l=3, m=+4,s=+1/2

b)

n=3, l=2, m=-2,s=+1/2

c)

n=4, l=3, m=+1,s=+1/2

d)

n=4, l=4, m=-4,s=-1/2

50.

The number of d-electrons retained in Fe2+ (at. no. of Fe= 26) ion is:

a)

4

b)

5

c)

6

d)

3

51.

Which of these statement related to the hydrogen atom is correct?

a)

3s orbital is lower in energy than 3p orbital.

b)

3p orbital is lower in energy than 3d orbital.

c)

3s and 3p orbitals are of lower energy than 3d orbital.

d)

3s,3p and 3d orbitals all have the same energy.

52.

Which of the following sets of quantum numbers represents the highest energy of an atom?

a)

n=3, l=1, m=1, s=+1/2

b)

n=3, l=2, m=1, s=+1/2

c)

n=4, l=0, m=0, s=+1/2

d)

n=3, l=0, m=0, s=+1/2

53.

The outer electronic configuration of Gd (Atomic no. 64) is:

a)

4f4 5d4 6s2

b)

4f7 5d1 6s2

c)

4f3 5d5 6s2

d)

4f8 5d0 6s2

54.
The electrons that are on the outer most region of the atom
a)
Shell Electrons
b)
Violent Electrons
c)
Valence Electrons
55.
This unit is represented by the combined number of protons and neutrons
a)
Atomic Mass
b)
Atomic Number
c)
Mass Number
56.
This number is represented by the number of protons in the atom
a)
Atomic Mass
b)
Atomic Number
c)
Mass Number
57.
The negative charge particles that float around the outside of the atom
a)
Proton
b)
Neutron
c)
Electron
58.
The area of the atom where protons and neutrons are found
a)
Electron Cloud
b)
Nucleus
c)
Energy Level
59.
A positively charged particle found in the nucleus of the atom
a)
Proton
b)
Electron
c)
Neutron
60.
The smallest possible unit matter can be divided into while still maintaining its properties.
a)
Proton
b)
Atom
c)
Element
61.
The different energy levels of electrons as they orbit the nucleus
a)
Electron Cloud
b)
Orbitals (Energy Levels)
c)
2, 8, 18, 32
62.
Most of the mass in an atom is made up of _____________________?
a)
protons and electrons
b)
protons and neutrons
c)
neutrons and electrons
d)
electrons and quarks
63.
What does the C represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
64.

What does the 6 represent?

a)

Atomic mass

b)

atomic number

c)

chemical symbol

d)

element name

65.
If an atom has 12 positively charged subatomic particles, which of the following must it also have to be considered a neutral atom?
a)
12 neutrons
b)
12 electrons
c)
12 protons
d)
24 protons and neutrons
66.
Protons and Electrons balance the charge of an atom.
a)
True
b)
False
67.
Electric charges that are different _______ each other.
a)
Attract
b)
Repel
68.
Electric charges that are alike _______ each other.
a)
Attract
b)
Repel
69.
What charge does a proton have?
a)
negative (-)
b)
positive (+)
c)
neutral or no charge (0)
70.
What charge does an electron have?
a)
negative (-)
b)
positive (+)
c)
neutral or no charge (0)
71.
If a substance has a higher number of electrons than protons on its surface, what type of charge does it have?
a)
A positive charge.
b)
A negative charge.
c)
A neutral charge
d)
No charge at all
72.

This particle determines the identity of an atom.

a)

proton

b)

neutron

c)

electron

d)

gluon

73.

Who discovered protons?

a)

Bohr

b)

Thompson

c)

Dalton

d)

Rutherford

74.

Using your periodic table, how many electrons are in a neutral atom of Sodium?

a)

11

b)

23

c)

16

d)

32

75.

Which of the following contributes to the total mass of the atom (select all that apply)

a)

neutrons

b)

electrons

c)

protons

d)

isotopes

76.

Who said the atom was like a plum pudding?

a)

Rutherford

b)

Dalton

c)

Thompson

d)

Bohr

77.

Who said the electrons orbited the nucleus like the planets orbit the sun

a)

Rutherford

b)

Thompson

c)

Bohr

d)

Dalton

78.

Using your periodic table, how many neutrons would be in an atom of Beryllium (Be)

a)

9

b)

4

c)

5

d)

11

79.

Which of the following has 12 protons?

a)

Carbon

b)

Magnesium

c)

Manganese

d)

Calcium

80.

The number 16 for the atomic element sulfur is the

a)

ionic number

b)

isotope

c)

atomic mass

d)

atomic number

81.

The center of an atom is called the ________________.

a)

electron cloud

b)

nucleus

c)

neutrion

d)

nuetron

82.

How many electrons does sulfur have

a)

16

b)

32

c)

48

d)

12

83.

What were J. J. Thomson's three contributions to the atomic theory?

a)

Discovered the electron

b)

Discovered the nucleus -did the gold foil experiment

c)

Used the cathode ray tube in his discovery

d)

Created a model of the atom with electrons moving around the nucleus in fixed orbits

e)

Created the "plum pudding" model of the atom

84.

What is Neils Bohr's contribution to the atomic theory?

a)

Created the atomic theory

b)

Created a model of the atom with electrons moving around the nucleus in a fixed orbits

c)

Discovered that the proton had a positive charge

d)

Believed that atoms of a given element are identical

e)

Discovered the electron

85.

What were Ernest Rutherford's three contributions to atomic theory?

a)

Discovered that the atom is mostly empty space

b)

Discovered the nucleus- did the gold foil experiment

c)

Used the cathode ray tube in his discovery

d)

Discovered the electron

e)

Discovered that the proton had a positive charge

86.

How many neutrons are in Tungsten

a)

110

b)

74

c)

183

d)

258

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