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Unit 3 Practice

Total questions: 38

Worksheet time: 59mins

Name
Class
Date
1.

The electron configuration of an atom determines how the atom reacts with other atoms. Examine the periodic table and determine which of the following substances is least likely to react with another substance.

a)

Bromine (Br)

b)

Gold (Au)

c)

Neon (Ne)

d)

Sodium (Na)

2.

How many energy levels does Xenon have?

a)

2

b)

3

c)

5

d)

6

3.

According to periodic trends, hydrogen would have it's valence electrons in what sublevel?

a)

S

b)

P

c)

D

d)

F

4.

According to periodic trends, most transition metals (mainland metals) have their valence electrons in what sublevel?

a)

S

b)

P

c)

D

d)

F

5.

1s2 2s2 is which element?

a)

Lithium

b)

Beryllium

c)

Helium

d)

Boron

6.

Which element is 1s2 2s2 2p6 3s2 3p6 4s2 3d7?

a)

Cobalt

b)

Nickel

c)

Manganese

d)

Chromium

7.

Write the configuration for Oxygen

a)

1s2 2s2 1p4

b)

2s2 2p4

c)

1s2 2s2 3p4

d)

1s2 2s2 2p4

8.

Which element is 1s2 2s2 2p6 3s2 3p6 4s1?

a)

Sodium (Na)

b)

Lithium (Li)

c)

Potassium (K)

d)

Calcium (Ca)

9.

Choose the correct configuration for Zinc

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d9

c)

1s2 2s2 2p6 3s2 3p6 3s2 3d10

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d8

10.

Choose the correct element for 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

a)

Chlorine

b)

Bromine

c)

Krypton

d)

Sulfur

11.
Which electron configuration belongs to Copper (Cu)?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d8
b)
1s2 2s2 2p6 3s2 3p6 4s2 3d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 3d10
12.

What is the electronic configuration of iron (Fe)?

a)
1s22s22p63s23p64s23d6
b)
1s22s22p63s23p63d8
c)
1s22p63s23p64s23d6
d)
1s22s22p63s23p64s13d6
13.

Which of the following is the electron configuration for Fluorine

a)
b)
c)
d)
14.

Light is emitted when electrons

a)

move from one atom to another.

b)

collide with one another, releasing energy.

c)

move from a lower energy level to a higher energy level.

d)

move from a higher energy level to a lower energy level.

15.
As a distant star moves away from Earth, the light given off by the star has a measurably lower frequency. What happens to the wavelength and energy of the photons of light when the frequency becomes lower?
a)
The wavelength becomes longer, and the energy decreases.
b)
The wavelength becomes shorter, and the energy decreases.
c)
The wavelength becomes longer, and the energy increases.
d)
The wavelength becomes shorter, and the energy increases.
16.
The distance from one point to the next corresponding point on a wave is called the ________________.
a)
waveform
b)
peak
c)
amplitude
d)
wavelength
17.

Describe the waves the arrow is pointing at.

a)

long wavelength / low energy

b)

long wavelength / high energy

c)

short wavelength / low energy

d)

short wavelength / high energy

18.

Describe the waves the arrow is pointing at.

a)

long wavelength / low energy

b)

long wavelength / high energy

c)

short wavelength / low energy

d)

short wavelength / high energy

19.

As the wavelength of a wave gets longer, what is also true? 

a)

  1. Frequency of the wave will increase

b)

  1. Energy of the wave with increase

c)

Frequency of the wave will decrease

d)

The wave will travel at a slower speed

20.
Wavelengths on the right side of the Electromagnetic spectrum are ______________.
a)
short
b)
long
c)
average
21.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
22.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
23.

What atom matches this electron configuration?

1s2 2s2 2p6 3s2

a)

Neon (Ne)

b)

Magnesium (Mg)

c)

Aluminum (Al)

d)

Potassium (K)

24.

Given the frequencies, which color has the highest energy?

a)

Violet

b)

Red

c)

Green

25.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
26.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
27.
Atomic radius generally increases as we move __________.  
a)
down a group and from right to left across a period 
b)
up a group and from left to right across a period 
c)
down a group and from left to right across a period 
d)
up a group and from right to left across a period 
28.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
29.
Which of the following will have a higher ionization energy than arsenic (As)?
a)
Gallium (Ga)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
30.

What is the correct lewis dot diagram for Boron?

a)
b)
c)
d)
31.

What is the missing part of the sequence for the electron configuration of Neon

1s2 , _, 2p6

a)

2s2

b)

3s2

c)

2s6

d)

1s1

32.

Order the elements S, Cl, and F in terms of increasing atomic radius.

a)

S, Cl, F

b)

Cl, F, S

c)

F, S, Cl

d)

F, Cl, S

e)

S, F, Cl

33.

Which statement regarding these Group 2 elements best supports the data?

a)

More energy levels, electrons in lower energy levels shield electrons in higher energy levels so the radius gets larger

b)

More energy levels, electrons in higher energy levels shield electrons in the lower energy levels so the radius gets smaller

c)

the mass of the atom is bigger

d)

the mass of the atom is smaller

34.

Which element in the pair of adjacent elements, Mg and Na,has a higher first ionization energy?

a)

Na

b)

Mg

35.

Which group of elements has the lowest ionization energies?

a)

Alkali Metals (Group 1)

b)

Alkaline Earth Metals (Group 2)

c)

Halogens (Group 17)

d)

Noble Gases (Group 18)

36.

Select the element with the lowest ionization energy.

a)

Barium

b)

Beryllium

c)

Magnesium

d)

Strontium

37.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
38.

How many valence electrons are represented here?

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2

a)

2

b)

12

c)

4

d)

10

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