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Practice Test - Light & the e- (Ch 11)

Total questions: 40

Worksheet time: 55mins

Name
Class
Date
1.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
2.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
3.

How many orbitals are there in a d sublevel?

a)
1
b)
3
c)
5
d)
7
4.

How many orbitals are there in a p sublevel?

a)
2
b)
1
c)
4
d)
3
5.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
6.

What is this element? 
1s22s22p63s23p64s23d104p6

a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
7.

How many electrons can the first principal energy level hold?

a)
1
b)
2
c)
8
d)
0
8.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
9.

What electron configuration matches a neon atom?

a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
10.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
11.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
12.

There are 4 different types of sublevels: s,p,d,f.

a)
true
b)
false
13.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
14.
Which wave has the greatest amplitude?
a)
The blue wave
b)
The red wave
15.
High frequency waves have _________ wavelengths.
a)

varying

b)

long

c)

the same

d)

short

16.
The distance between two crests or two troughs of a wave is called:
a)
frequency
b)
amplitude
c)
wavelength
d)
hertz
17.
Which wave has a greater frequency?
a)
A
b)
B
18.

Which color on the visible spectrum has the longest wavelength?

a)

blue

b)

green

c)

yellow

d)

red

19.

Which wave in the diagram has the greatest energy?

a)

1

b)

2

c)

3

d)

4

20.
Which wave in the diagram has the greatest wavelength?
a)
1
b)
2
c)
3
d)
4
21.

When an electron in the _______state absorbs energy, it goes to the ________ state.

a)

lower, excited

b)

ground state, higher state

c)

ground state, excited state

d)

excited state, ground state

22.

What are spectral lines?

a)

Dark or bright lines in a spectrum that correspond to specific wavelengths of light emitted or absorbed by an atom or molecule.

b)

Lines that indicate the density of a liquid

c)

Lines that indicate the pressure of a gas

d)

Lines that indicate the temperature of a star

23.

What is the purpose of flame tests in atomic emission?

a)

The purpose of flame tests in atomic emission is to create a chemical reaction between the sample and the flame.

b)

The purpose of flame tests in atomic emission is to identify the presence of specific elements in a sample based on the color of the flame produced when the sample is heated.

c)

The purpose of flame tests in atomic emission is to determine the pH level of the sample based on the color of the flame produced.

d)

The purpose of flame tests in atomic emission is to measure the temperature of the flame produced when the sample is heated.

24.

What is the relationship between spectral lines and energy levels?

a)

Spectral lines are produced when photons transition between different energy levels in an atom.

b)

Spectral lines are produced when neutrons transition between different energy levels in an atom.

c)

Spectral lines are produced when electrons transition between different energy levels in an atom.

d)

Spectral lines are produced when protons transition between different energy levels in an atom.

25.

According to the Bohr model, what are energy levels in atoms?

a)

The fixed energies an electron can have in an atom.

b)

The specific frequencies of light emitted by an element.

c)

The distances between crests of waves.

d)

The different colors of light in the atomic emission spectrum.

26.

What does the Bohr model represent with its orbits?

a)

The different elements in the periodic table.

b)

The energy levels of the electrons in the atom.

c)

The specific wavelengths of light emitted by the element.

d)

The distances between crests of waves.

27.

The picture shows an atom in the ground state absorbing energy and the electron jumps to the excited state. Which state has higher energy?

a)

Ground State

b)

Excited State

28.

The number of wave cycles to pass a given point per unit of time.

a)

Amplitude

b)

Wavelength

c)

Frequency

29.

When atoms absorb energy, electrons ..............energy level

a)

move to higher

b)

move to lower

c)

stays in the same

30.
Emission of light from an atom occurs when an electron
a)
drops from a higher to a lower energy level.
b)
   jumps from a lower to a higher energy level.   
c)
   moves within its atomic orbital.
d)
falls into the nucleus.
31.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
32.

True or False: The ground state is the highest energy state of an atom.

a)

True

b)

False

33.

What type of sublevel is shown in the image?

a)

s

b)

p

c)

d

d)

f

34.
The maximum distance from the center line to the top of the crest or the bottom of the trough is called the __________ of the wave.
a)
amplitude of the wave
b)
wavelength of the wave
c)
frequency of the wave
d)
speed of the wave
35.
What is the lowest point on a wave?
a)
amplitude
b)
peak
c)
trough
d)
wavelength
36.
High frequency waves have _________ wavelengths.
a)
varying
b)
long
c)
the same
d)
short
37.
The unit of frequency is ___.
a)
meters
b)
nanometers (nm)
c)
m/s
d)
Hertz
38.
All waves carry
a)
energy
b)
light 
c)
matter
d)
particles
39.

What is the energy of a photon that has a frequency of 3.0 x 1020 Hz?


Remember that ...

c = 3.0 x 10 8 m/s

h = 6.626 x 10-34 J s

4 lines
40.

EXTRA CREDIT:

Pick the correct configuration for a potassium ion. 


a)

1s22s22p63s1

b)

1s22s22p63s23p6

c)

1s22s22p63s23p64s1

d)

1s22p83s1

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