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Unit 2 - Periodicity & Electron Configuration Test Review

Total questions: 63

Worksheet time: 2hrs 36mins

Name
Class
Date
1.

The energy level tells us what about an electron?

a)

location of the valence electrons

b)

shape of the electron cloud

c)

speed of the electron

d)

spin of the electron

2.

Which of the following statements are FALSE about electron configuration?

a)

electrons in the same orbital must have opposite spin

b)

electrons enter orbitals of the highest energy level first

c)

electrons enter orbitals of the lowest energy level first

d)

orbitals can be occupied by no more than 2 electrons

3.

If five electrons are available to fill five empty 3d orbitals, how will the electrons be distributed in the five orbitals?

a)

five electrons in one orbital, none in the other four

b)

one electron in each orbital

c)

two electrons in the first and second orbitals, one electron in the third orbital

d)

five electrons cannot enter the 3d orbitals

4.

How many unpaired electrons are in an phosphorus atom (atomic #15)?

a)

0

b)

1

c)

2

d)

3

5.

How many valence electrons are in a sulfur atom (atomic #16)?

a)

2

b)

6

c)

8

d)

16

6.

The correct noble gas notation for Osmium (Os) is:

a)

[Xe] 6s25d6

b)

[Xe] 6s24f145d6

c)

[Kr] 5s24d106s25d6

d)

[Kr] 5s24d106s24f145d6

7.

Which of the three major subatomic particles play the most important role in determining the physical and chemical properties of an element?

a)

electron

b)

neutron

c)

proton

d)

they are all important

8.

The horizontal rows on the periodic table are called the:

a)

families

b)

groups

c)

periods

d)

families and groups

9.

Vertical columns on the periodic table are called:

a)

families

b)

groups

c)

periods

d)

families and groups

10.

The period where an element is located tells us:

a)

the number of energy levels

b)

the number of valence electrons

c)

the number of energy levels and valence electrons

d)

none of the above

11.

Predict the conductivity of cadmium based on its location on the periodic table.

a)

Cd will conduct heat/electricity

b)

Cd will not conduct heat/electricity

c)

Cd is a metalloid and has dual properties

d)

More information is needed

12.

The alkaline earth metals family ____________ electrons to form _____________ charged ions.

a)

loses, negatively

b)

gains, negatively

c)

loses, positively

d)

gains, positively

e)

None of these

13.

Which elements have the most similar chemical properties

a)

Na, K, Cs

b)

Fe, Co, Ni

c)

H, He, Cl

d)

B, Si, As

14.

Which of the following is a metalloid?

a)

Helium

b)

Germanium

c)

Copper

d)

Lithium

15.

Which of the following is NOT a diatomic element?

a)

C

b)

N

c)

O

d)

F

16.

The amount of energy needed to remove the most loosely held electron from an atom is known as:

a)

electron affinity

b)

electronegativity

c)

ionization energy

d)

joule energy

17.

A measure of the desire for electrons in a chemical bond is known as:

a)

atomic radius

b)

electronegativity

c)

ionic radius

d)

ionization energy

e)

none of the above

18.

Compare F, Fe, Fr. Which one has the largest atomic radius

a)

F

b)

Fe

c)

Fr

d)

Cannot be determined

19.

Compare Ca, Zn, As, and Br. Which one has the smallest atomic radii.

a)

Ca

b)

Zn

c)

As

d)

Br

20.

Elements in Group 7A or 17 on the periodic table (the halogens):

a)

behave similarly

b)

have 7 valence electrons

c)

increase in atomic radius as you move from top to bottom

d)

all of these are correct

e)

none of these are correct

21.

Lithium is a(n) __________ metal, therefore it is expected to react violently with water.

a)

Alkali

b)

Alkaline Earth

c)

Inner Transition

d)

Transition

22.

In a compound containing sodium and chlorine, which is a nonmetal?

a)

sodium

b)

chlorine

c)

both are metals

d)

neither are metals

23.

Which group of elements contains a metal, metalloid, and a nonmetal?

a)

K, Li, Cs

b)

Au, Ag, Cu

c)

Pb, Sn, Ge

d)

Co, As, Kr

24.

Which of the following is a metal?

a)

Mercury

b)

Iodine

c)

Carbon

d)

Antimony

25.

Why is ionization energy higher at the top of the periodic table?

a)

Electrons are father away from the nucleus

b)

Electrons are closer to the nucleus

c)

Mendeleev determined it

d)

None of these

26.

Which of these following would require a greater amount of energy to remove an electron?

a)

Halogen

b)

Alkali Metal

c)

Alkaline Earth Metal

d)

Noble Gas

27.

Which of the following has the smallest ionization energy?

a)

Fluorine

b)

Aluminum

c)

Silver

d)

They all have the same ionization energy

28.

The most electronegative element on the periodic table is:

a)

Fluorine

b)

Francium

c)

Helium

d)

Need more information to determine

29.

Compare Li, Be, B, and C. Which has the smallest electronegativity value?

a)

B

b)

Be

c)

C

d)

Li

30.

Which scientist arranged the periodic table by increasing atomic mass and left gaps for yet to be discovered elements was

a)

Bohr

b)

Mendeleev

c)

Moseley

d)

Schrodinger

31.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
32.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
33.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
34.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
35.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
36.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
37.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
38.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
39.
What does Pauli exclusion principle state ?
a)
states that each electron occupies the lowest energy orbital available
b)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
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
40.
What does Hund's rule states ?
a)
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
b)
states that each electron occupies the lowest energy orbital available
c)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
41.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
42.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
43.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
44.

Which area on the periodic table represents the electrons in the "d" sublevel?

a)

representative elements

b)

columns 3-8

c)

rare earth elements

d)

transition elements

45.
Anions are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
46.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
47.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

48.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
49.
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
50.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
51.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
52.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
53.
Ionization energy is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
54.
Electronegativity is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
55.
Which element has the smaller atomic radius: potassium (K) or bromine (Br)?
a)
potassium (K)
b)
bromine (Br)
56.
Which element has the greatest ionization energy: Aluminum (Al)    or    Chlorine (Cl)?
a)
Aluminum (Al)
b)
Chlorine (Cl)
57.
Which element has the greatest electronegativity: Nitrogen (N) or Arsenic (As)?
a)
Nitrogen (N)
b)
Arsenic (As)
58.
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
59.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
60.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
61.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
62.
Electronegativity is...
a)
the ability of an atom to attract/ accept electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
63.
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

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