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Midterm Test Review

Total questions: 73

Worksheet time: 1hrs 25mins

Name
Class
Date
1.

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

a)

groups

b)

towers

c)

periods

d)

atomic numbers

2.
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
3.
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 
4.
Electronegativity is...
a)
how good an atom is at attracting 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. 
5.
What is ionization energy?
a)
Energy required to remove an electron
b)
Energy needed to split an electron
c)
Energy required to add an electron
6.

Ionization energy __________ as you go across a period

a)

stays the same

b)

decreases

c)

increases

7.
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
8.
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.
9.

Select the element with the largest atomic radius

a)

Potassium

b)

Scandium

c)

Gallium

d)

Arsenic

10.

Select the element most likely to gain an electron

a)

Bromine

b)

Fluorine

c)

Chlorine

d)

Iodine

11.

Select the element most likely to lose an electron

a)

Magnesium

b)

Sulfur

c)

Barium

d)

Oxygen

12.

Select the sequence that correctly orders from smallest to largest atomic radius

a)

Sn, Y, Ru

b)

Cu, Ga, Br

c)

Al, S, Na

d)

F, N, Li

13.

Select the group that is the most reactive metals

a)

Transition Metals

b)

Alkali Earth Metals

c)

Alkali Metals

d)

Halogens

14.

Select the element that has 3 valence electrons

a)

Calcium

b)

Sodium

c)

Aluminum

d)

Sulfur

15.

Select the sequence of increasing electronegativity.

a)

Sn, Ag, I

b)

I, Sn, Ag

c)

Ag, Sn, I

d)

Sn, I, Ag

16.

What group contains elements with 7 valence electrons

a)

Noble Gasses

b)

Alkali Earth Metals

c)

Halogens

d)

Transition Metals

17.

I am a nonmetal


I am in period 2


I am in group 16/6A

a)

Ba

b)

Si

c)

Ba

d)

O

18.

I am a metal


I am in group 2


I am in period 6


I am…

a)

Mo

b)

Re

c)

S

d)

Ba

19.
All elements found on the left side of the Periodic Table of the Elements have what properties in common?
a)
They conduct heat and electricity 
b)
They are all gases 
c)
They are brittle and dull
d)
They are radioactive
20.
How many Valance electrons does Iodine Have?
a)
6
b)
16
c)
7
d)
17
21.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
22.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
23.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
24.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
25.
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
26.

The 4 orbitals are

a)

s, p, d, f

b)

a, b, c, d

c)

2, 4, 6, 8

27.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
28.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
29.
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
30.
Electrons are paired based on their spin directions, clockwise and counterclockwise, is what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
31.

This orbital diagram represents:

a)

C (6)

b)

B (5)

c)

N (7)

d)

O (8)

32.

Mendeleev arranged the elements in his periodic table in order of

a)

atomic number

b)

number of electrons

c)

mass

d)

number of neutrons

33.

Which classification of elements are gases or dull brittle solids and poor conductors?

a)

Transition metals

b)

Metals

c)

Nonmetals

d)

Metalloids

34.

Which classification of elements are solids, semi-conductors, and have physical properties like metals and chemical properties like nonmetals?

a)

Transition metals

b)

Metalloids

c)

Nonmetals

d)

Metals

35.

Match the following group names

a)

Group 13

1.

Boron group

b)

Group 14

2.

Carbon group

c)

Group 15

3.

Nitrogen group

d)

Group16

4.

Oxygen group

e)

Groups 3-12

5.

Transition metals

36.

Match the following group names:

a)

Group 1

1.

Alkali metals

b)

Group 2

2.

Alkaline earth metals

c)

Group 3

3.

Rare earth metals

d)

Group 17

4.

Halogens

e)

Group 18

5.

Noble gases

37.

Why is Henry Mosley important to the history of the periodic table?

a)

Predicting elements that had not been discovered yet

b)

Arranging the periodic table by atomic MASS

c)

Arranging the periodic table by atomic NUMBER

d)

He was the first person to propose indivisible particles called atomos

38.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
39.

Why do all bonds form?

a)

so the number of protons equals the number of electrons

b)

so an atom can become unstable

c)

to fill the outermost energy level

40.

According to the Octet Rule, atoms of elements react with each other in order to attain ____ electrons in their outermost energy level or shell.

a)

2

b)

4

c)

6

d)

8

e)

10

41.

Lithium is in group 1 of the periodic table, which ion would it form?

a)

Li-

b)

Li2-

c)

Li+

d)

Li2+

42.
A cation is a ____ ion.
a)
negative
b)
positive
43.
A anion will be a ____ ion.
a)
negative
b)
positive
44.

Which of the following would be the correct formula for a compound of Aluminum and Fluorine?

a)

AlF3

b)

Al2F3

c)

AlF2

d)

AlFI

45.

MnOH

(a)  

46.

Al2O3

(a)  

47.
Which of the following is the correct name for MgCl2....
a)
Magnesium Clorine
b)
Magnesium Dicholorine
c)
Magnesium Cloride
d)
Magnesium Dichloride
48.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

49.

Draw the Lewis Dot Structure for Sulfur.

50.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
51.
What molecule is this?
a)
CO
b)
CO2
c)
C2O
d)
C2O2
52.
In a covalent bond, one or more electrons are? 
a)
shared 
b)
lost 
c)
gained 
d)
transferred 
53.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
54.

What is it called if there are three-pairs of electrons being shared?

a)

Triple Bond

b)

Three Single Bonds

c)

Tribond

d)

Double and Single Bond Combo

55.
How many electrons are shared in a double bond?
a)
2
b)
4
c)
6
d)
8
56.

The correct name for CH4 is...

a)

Carbon Hydrogen

b)

Carbon Tetrahydride

c)

Monocarbon hydride

d)

Carbon Hydride

57.
Which of the following gives the correct chemical formula for the compound Dinitrogen Monoxide?
a)
NO
b)
N2O
c)
N2O2
d)
O2N2
58.

Which of the following names matches the chemical formula N2O3?

a)

Dinitrogen triople oxide

b)

Nitrogen oxide

c)

Dinitrogen trioxide

d)

Trioxide nitrogen

59.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Linear
60.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
61.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
62.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
63.
*
a)
trigonal pyramid
b)
linear
c)
bent
d)
angular
64.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
65.
Choose the correct shape for this molecule:
a)
Tetrahedral
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
66.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
67.
Br & Br
a)
Ionic 
b)
Polar Covalent 
c)
Nonpolar Covalent 
68.

Does the following reference Polar, Nonpolar, or both:

"equal sharing of electrons"?

a)

Polar

b)

Nonpolar

c)

Both

69.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
70.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
71.
Which of the following geometries could be nonpolar?
a)
bent
b)
tetrahedral
c)
trigonal pyrimidal
d)
none of the above
72.

What is the difference in electronegativity for HBr?

a)

0.7

b)

1.9

c)

2.0

d)

2.8

73.

What is the difference in electronegativity for 

SO2SO_2  ?

a)

0.5

b)

1.0

c)

2.0

d)

3.5

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