Free Printable Chapter 3 practice for exam

1.

the distance between peaks of electromagnetic waves is called:

a)

wavelength

b)

frequency

c)

energy

d)

Planck's Constant

2.

A light particle is called a(n):

a)

electromagnetic wave

b)

photon

c)

electron

d)

atom

3.

We see a "rainbow of colors" that when perceived together produce:

a)

black light

b)

white light

c)

gamma rays

d)

x-ray images

4.

What is the wavelength of light (nm) that has a frequency of 6.44 × 10¹³ s^-1 ?

$c\ =\lambda\times\nu$

c = speed of light = $3.00\times10^8\ ms^{-1}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ 1\ nm\ =\ 10^{-9}\ m$

$\lambda\ =\ wavelength\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \nu\ =\ frequency$

a)

6490 nm

b)

932 nm

c)

4660 nm

d)

6.49 × 10^-8nm

5.

The number of waves that pass a fixed point in unit time

a)

astronomical unit

b)

frequency

c)

wavelength

6.

A packet "particle" of electromagnetic energy is known as a

a)

neutron

b)

photon

c)

Hertz

d)

proton

7.

Electromagnetic radiation can sometimes behave like _______ and at other times like __________. Choose two.

a)

a wave

b)

a particle

c)

gravity

d)

matter

8.

When an atom absorbs energy, electrons .....

a)

moves up an energy level

b)

goes down an energy level

c)

are removed from the atom

9.

When electrons move down an energy level, the atom ......

a)

releases equal energy as a photon

b)

splits

c)

bonds to another

10.

How many electrons can fit on the 1st energy level (orbital) for any Bohr Model?

a)

2

b)

6

c)

8

d)

10

11.

Mia, Evelyn, and Arjun are studying the Bohr model for their physics class. According to this model, where are electrons allowed to exist in an atom?

a)

Energy levels or orbits

b)

Conduction band

c)

Valence band

d)

Nucleus

12.

Ethan is studying the Bohr model of the atom and wants to understand the significance of the principal quantum number. What does the principal quantum number represent in the Bohr model?

a)

The principal quantum number determines the shape of the electron's orbital.

b)

The principal quantum number indicates the spin of the electron.

c)

The principal quantum number represents the energy level or atomic orbit of an electron in an atom.

d)

The principal quantum number determines the atomic number of an element.

13.

The electrons move around the nucleus based on the (a) they occupy.

14.

The energy of an electron __________ as it moves further away from the nucleus

a)

increases

b)

decreases

15.

What is the maximum number of electrons in the second energy level?

a)

18

b)

8

c)

32

d)

2

16.

What is the shape of an 'S' subshell?

a)

b)

c)

d)

17.

What is the shape of an 'D' subshell?

a)

b)

c)

d)

18.

What is the shape of an 'P' subshell?

a)

b)

c)

d)

19.

What is the shape of an 'F' subshell?

a)

b)

c)

d)

20.

How many orbitals does an S subshell have?

a)

1

b)

2

c)

3

21.

How many orbitals does a P subshell have?

a)

1

b)

3

c)

5

22.

How many orbitals does a D subshell have?

a)

4

b)

5

c)

3

23.

If an orbital can hold 2 electrons, and a D subshell has 5 orbitals. How many electrons can a D Subshell hold?

a)

5

b)

10

c)

2

d)

6

24.

If an orbital can hold 2 electrons, and a 'S' subshell has 1 orbital. How many electrons can a 'S' Subshell hold?

a)

5

b)

10

c)

2

d)

6

25.

Each p subshell contains _____ orbitals

a)

1

b)

3

c)

5

d)

7

26.

Choose the correct electron configuration for Nitrogen:

a)

1s² 2s² 2p⁶

b)

1s² 2s² 2p⁸

c)

1s² 2s² 2p¹

d)

1s² 2s² 2p³

27.

Choose the s orbital

a)

b)

c)

d)

28.

There are 4 different types of subshells (orbitals) s,p,d,f.

a)

true

b)

false

29.

This orbital diagram represents:

a)

C

b)

B

c)

N

d)

O

30.

What does the number 1 in "1s" stand for?

a)

energy level

b)

s orbitals

c)

p orbitals

d)

the number of electrons

31.

What electron configuration matches an oxygen atom?

a)

1s²2s²2p⁶3s2, 3p⁶4s²3d¹⁰4p⁵

b)

1s²2s²2p⁴

c)

1s²2s²2p⁶

d)

1s²2s²2p⁶3s²3p⁶4s²3d¹

32.

The electron configuration of an atom is 1s²2s²2p⁶. The number of electrons in the atom is

a)

3

b)

6

c)

8

d)

10

33.

1. What is the shape of an s orbital?

a)

sphere

b)

dumbbell

c)

double dumbbell

d)

TOO COMPLEX TO KNOW IT.

34.

What is the shape of a p orbital?

a)

sphere

b)

it's just too complex to thing about it

c)

dumbbell

d)

I don't know this stuff.

35.

How many electrons can each p orbital hold?

a)

6

b)

3

c)

2

d)

4

36.

How many d orbitals are there in a given sublevel?

a)

1

b)

3

c)

5

d)

7

37.

How many p orbitals are there in a sublevel?

a)

2

b)

1

c)

4

d)

3

38.

How likely is it that an electron occupying a p or a d orbital would be found very near an atom’s nucleus?

a)

likely...that's where you find it

b)

not likely

c)

not likely, but there is a f orbital near the nucleus

d)

what's near the orbital

39.

How many electrons can the d sublevel hold?

a)

8

b)

10

c)

2

d)

4

40.

Which is associated with more energy?

a)

2p

b)

2s

c)

3p

d)

1s

41.

Which orbital has the least amount of energy?

a)

p orbital

b)

d orbital

c)

s orbital

d)

What is an orbital?

42.

How many electrons can the first energy level hold?

a)

1

b)

2

c)

8

d)

0

43.

How many orbitals does an s sublevel have?

a)

1

b)

3

c)

5

d)

7

44.

How many orbitals does a d sublevel have?

a)

1

b)

3

c)

5

d)

7

45.

Electrons fill energy levels and sublevels _____ in energy first.

a)

lower

b)

higher

46.

Which of the following statements is true about the 3s and the 4s sublevels?

a)

These sublevels have the same energy

b)

These sublevels are the same distance from the nucleus

c)

These sublevels hold different amounts of electrons

d)

These sublevels have the same shape

47.

The maximum number of electrons that can fit into the 2nd energy level is

a)

2

b)

8

c)

18

d)

32

48.

Region of high probability of finding an electron

a)

atomic orbital

b)

ground state

c)

Heisenberg uncertainty principle

d)

electron configuration

49.

Fill in the blank: The number of orbitals in a 3p sublevel is ____.

a)

1

b)

3

c)

5

d)

7

50.

Fill in the blank: The n = 3 energy level contains ____ orbitals.

a)

1

b)

4

c)

9

d)

16

51.

Which sublevel has a cloverleaf shape?

a)

s

b)

p

c)

d

d)

f

52.

Which sublevel has a variable shape?

a)

s

b)

p

c)

d

d)

f

53.

How many orbitals does an s sublevel have?

a)

1

b)

3

c)

5

d)

7

54.

What are the orbitals for n=4

a)

s

b)

s, p

c)

s, p, d

d)

s, p, d, f

55.

How many f orbitals can an f sublevel hold?

a)

1

b)

7

c)

5

d)

14

56.

What are the orbitals that make up the n=1 energy level?

a)

s

b)

s, p

c)

s, p, d

d)

s, p, d, f

57.

How many atomic orbitals are there in the d sublevel?

a)

3

b)

4

c)

5

d)

6

58.

Electrons fill energy levels and sublevels _____ in energy first.

a)

lower

b)

higher

59.

The second energy level (n=2) contains a total of 5 electrons...how many more electrons can fit in the 2nd energy level?

a)

0

b)

3

c)

5

d)

7

60.

The maximum number of electrons that can fit into the 2nd energy level is

a)

2

b)

8

c)

18

d)

32

61.

Theoretically, the fifth energy level of an atom can hold a maximum of ________ sublevels?

a)

2

b)

4

c)

5

d)

6

62.

Of the following sublevels, which is the highest in energy?

a)

4s

b)

3d

c)

4p

d)

5s

63.

A spherical orbital with 3rd energy level

(a)

64.

An orbital that is one of a set of 3 in 4th shell

(a)

65.

subshells in n=5 shell

(a)

66.

Orbitals in 4d subshell

(a)

67.

Maximum number of electrons in 5f subshell

(a)

68.

Maximum number of electrons in n=4 shell

(a)

69.

Maximum electrons in 3d_yorbital

(a)

70.

Elements in the same group or column have the same ...

a)

# of valence electrons

b)

# of shells

c)

# of protons

d)

Mass Number

71.

Which atom has the largest atomic radius?

a)

potassium (K)

b)

rubidium (Rb)

c)

francium (Fr)

d)

cesium (Cs)

72.

The atom with the largest atomic radius in Group 18 is -

a)

Ar

b)

He

c)

Kr

d)

Rn

73.

Order the following in increasing atomic radii:
Ra, Be, Ca, Rb, H

a)

Ra, Be, Rb, H, Ca

b)

Rb, H, Ca, Be, Ra

c)

Ra, Rb, Ca, Be, H

d)

H, Be, Ca, Rb, Ra

74.

Which one has the largest radius?

a)

Lithium (Li, atomic #3)

b)

Boron (B, atomic #5)

c)

Neon (Ne, atomic #10)

d)

Nitrogen (N, atomic #7)

75.

Which of the following elements would be smaller: indium or gallium?

a)

indium

b)

gallium

c)

both atoms are the same size

d)

cannot be determined

e)

the sizes can vary

76.

Which of the following elements would be larger: potassium or cesium?

a)

potassium

b)

cesium

c)

both atoms are the same size

d)

cannot be determined

e)

the sizes can vary

Chapter 3 practice for exam

Total questions: 76

Worksheet time: 2hrs 57mins

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