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Unit 2 Test Review - PT and Electrons

Total questions: 42

Worksheet time: 1hrs 24mins

Name
Class
Date
1.
Which of the following elements has the biggest atomic radius?
a)
Rubidium
b)
Calcium
c)
Copper
d)
Potassium
2.
The nonmetal family that is the most reactive is the....
a)
noble gases
b)
halogens
c)
alkali metals
d)
alkaline earth metals
3.

Valence electrons are the

a)

outer most electrons in an atom

b)

total electrons in an atom

4.

USE THE PERIODIC TABLE

How many valence electrons does Phosphorus have?

a)

31

b)

5

c)

15

d)

4

5.

How many valence electrons does Carbon have?

a)

4

b)

6

c)

14

d)

12

6.
How many valence electrons are found in atoms of group 14?
a)
4
b)
3
c)
14
d)
16
7.

A conductor is something that ..

a)
can be drawn into a wire
b)
breaks or shatters easily
c)
heat and electricity can go through
d)

is heavy for its size

8.

Which is expected to be the largest atom, based on its location on the periodic table?

a)

Na

b)

Mg

c)

Ca

d)

K

9.

Which photon has the longest wavelength?

a)

blue

b)

red

c)

infrared

d)

ultraviolet

10.

As you move down the periodic table atoms get bigger. This is because ___.

a)

The atoms have more mass.

b)

The atoms have more protons.

c)

The atoms have more energy levels

d)

The atoms have more nuetrons

11.

Which is NOT correctly matched?

a)

Na = alkaline earth metal

b)

Ni = transition metal

c)

N = nonmetal

d)

Rn = noble gas

12.

An electron falls from a high to low energy level. What happens?

a)

the electron lands in the nucleus

b)

the atom shrinks in size

c)

a photon of light is released

d)

a beam of radioactivity is released

13.

Which element is most chemically similar to oxygen?

a)

Carbon

b)

Nitrogen

c)

Fluorine

d)

Phosphorus

e)

Selenium

14.

What is the distance between two peaks of a wave?

a)

Wavelength

b)

Frequency

c)

Amplitude

d)

Oscillation

15.

The number of waves that pass a fixed point in 1 second.

a)

Wavelength

b)

Frequency

c)

Amplitude

d)

Oscillation

16.

period

a)

Elements that occur in vertical columns on the periodic table.

b)

A horizontal row of elements in the periodic table

c)

Found in group two of the periodic table; highly reactive

d)

A subatomic particle that has a negative charge

17.

Elements that occur in vertical columns on the periodic table.

a)

Neutron

b)

metalloids (semimetals)

c)

groups

d)

Proton

18.

metalloids (semimetals)

a)

Elements that occur in vertical columns on the periodic table.

b)

an element that has both metallic and nonmetallic properties

c)

not able to conduct heat or electricity, little to no metallic luster

d)

found in group one of the periodic table; highly reactive

19.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
20.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
21.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
22.
What does the 6 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
23.

What period is Lead (Pb) in?

a)

6

b)

4

c)

Metals

d)

14

24.

Light is given off from an atom when...

a)

electrons move to a higher shell

b)

electrons drop from a higher shell

25.
If light hitting the atom has just the right amount of energy, the electron will ___
a)
absorb it and jump down
b)
absorb it and jump up
c)
emit it and jump up
d)
emit it and jump up
26.

The _______________ determines the color of visible light.

a)

wavelength (and frequency)

b)

speed

c)

amplitude

d)

particles of the medium

27.

The low level energy state for an electron is called the ______________________.

a)

excited state

b)

low state

c)

ground state

d)

elevated state

28.
Why are line emission spectra of elements called "atomic fingerprints"?
a)
They are all the same
b)
They are all unique
c)
They are all similar
d)
They all contain colored light
29.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

30.

What is the configuration for Carbon?

a)

1s2 2p2

b)

1s2 2s2 2p2

c)

1s1 1s2 2s2 2p2

31.

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

a)

Cobalt

b)

Nickel

c)

Manganese

d)

Chromium

32.

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

33.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
34.

What does Pauli exclusion principle state ?

a)

states that each electron occupies the lowest energy orbital available

b)

states that -no two electrons in the same orbital can have the same spin

c)

states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals

35.

What is the maximum number of electrons that an s orbital can have?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

36.

How many electrons can the d sublevel hold?

a)

8

b)

10

c)

2

d)

4

37.

How many electrons can be found in a p sublevel?

a)
2
b)
3
c)
4
d)
6
38.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
39.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
40.
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)
41.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
42.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z

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