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Chemistry Semester 1 Final Review

Total questions: 88

Worksheet time: 3hrs 55mins

Name
Class
Date
1.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
2.
Which of the following is the correct electron configuration for a phosphorus  atom?
a)
1s2 2s2 2p6 3s2 3p3
b)
1s2   2s2   3p3 
c)
1s2 2s2 2p6 3s2 3p6 
d)
1s2 2s2  3s2 2p6 3p3
3.
How many electrons should Carbon have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
4.

This is a correct dot diagram for oxygen (O)?

a)

true

b)

false

5.
Elements in the same column of the periodic table always have the same # of _______ as one another.
a)
Protons
b)
Neutrons
c)
Electrons
d)
Valence Electrons
6.

Match the following elements with their correspomding number of valence electrons

a)

1

1.

Hydrogen

b)

2

2.

Magnesium

c)

3

3.

Aluminum

d)

7

4.

Bromine

e)

6

5.

Oxygen

7.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
8.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
9.
The proper formula for magnesium hydroxide:
a)
MgOH
b)
Mg2OH
c)
Mg(OH)2
d)
Mg2OH2
10.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

11.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin (IV) Selenide

c)

Tin selenide

d)

Tin (II) triselenide

12.
Each column in the periodic table is called a _________ .
a)
period
b)
group
c)
cluster
d)
unit
13.
Groups on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
14.

Elements in the same group have : (2 correct answers)

a)

Similar chemical properties

b)

Similar names

c)

Same number of outer (valence) electrons)

d)

The same number of protons

15.

The yellow elements (right side) are called 

a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
16.

The blue elements (left side) are called 

a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
17.
The atomic number is equal to _.
a)
the number of protons and electrons
b)
the number of neutrons only
c)
the total number of protons and neutrons
d)
the number of protons neutrons and electrons
18.
What is the charge on a lithium atom that looses 1 electron?
a)
+1
b)
0
c)
-1
d)
-2
19.
How many protons does this isotope of titanium have? Hint titanium has an atomic number of 22.
a)
48
b)
22
c)
26
d)
70
20.

A negatively charged ion that has gained electrons to satisfy the octet rule (metals do this)

a)

Anion

b)

Cation

c)

Neutral Atom

d)

Isotope

21.

A positively charged ion that has lost electrons to satisfy the octet rule (non-metals do this)

a)

Anion

b)

Cation

c)

Neutral Atom

d)

Isotope

22.

Atoms of the same element that have different mass than expected because they have a different number of neutrons.

a)

Neutral Atom

b)

Ion

c)

Isotope

d)

Cation

23.

If an atom has 9 protons and 10 electrons it has a charge of ____.

a)

0

b)

-1

c)

+1

d)

-2

24.

How many neutrons does Pb-209 have?

a)
127
b)
209
c)
82
d)
291
25.

How many protons does Phosphorous-30 have?

a)
30
b)
16
c)
12
d)
15
26.

This isotope has:

​ (a)   protons

8 electrons

​ (b)   neutrons

mass number of ​ (c)  

Choose from the below words
8
11
19
20
10
18
9
27.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

28.
Subatomic particle with a charge of 0
a)
neutron
b)
proton
c)
electron
d)
quark
29.
What element is represented in this Bohr Model? 
a)
Carbon
b)
Hydrogen
c)
Aluminum
d)
Lithium
30.

How many atoms are present in a 13.5 gram sample of beryllium?

a)

1.5 particles

b)

9 particles

c)

4.03 x1023 particles

d)

9.02 x1023 particles

31.

A sample of silver contains 5.71 x 1022 atoms. How many moles of silver are present?

a)

3.43 x 1046 moles

b)

0.0529 moles

c)

0.0948 moles

d)

10.5 moles

32.
Calculate the mass of iron in a sample of iron ore containing 2.61x1023 iron atoms.
a)
0.433g
b)
24.2g
c)
44g
d)
6.02g
33.

In addition and subtraction, the significant figures in the answer must reflect the

a)

average number of significant figures in the problem.

b)

number in the calculation with the most significant figures.

c)

number in the calculation with the fewest significant figures.

d)

least precise measurement in the calculator (i.e. least number of decimal places)

34.

In division and multiplication, the answer must not have more significant figures than the

a)

average number of significant figures in the problem.

b)

least precise measurement in the calculation (i.e. least number of decimal places)

c)

number in the calculation with the fewest significant figures.

d)

number in the calculator with the most significant figures.

35.
What is the volume of liquid in this graduated cylinder?
a)
40.0 mL
b)
40.3 mL
c)
43.0 mL
d)
44.0 mL
36.

What is the length of line C on this ruler

a)

2.2 cm

b)

2.25 cm

c)

2.255 cm

d)

2.03 cm

37.
On this digital scale, which digit is the uncertain digit?
a)
1
b)
2
c)
6
d)
4
38.

To make a proper measurement...

a)

write down only the certain digits.

b)

write down all certain digits and one estimated digit (the uncertain digit)

c)

write down all certain digits and a few estimated digits.

d)

look at the instrument carefully

39.

Calculate and give the answer with proper sig fig for the following equation: 65.12+5.0+25.25=

40.

How many significant figures are there in 0.000854 grams?

41.

Calculate and give the answer with proper sig fig for the following equation: 3.54/10.0=

42.
Change from standard form to scientific notation: 0.004078
a)
4.078  x  10-3
b)
4.078  x  103
c)
40.78  x  10-4
d)
.4078  x  10-2
43.

Multiply:

(3.4 x 105)(1.2 x 10-3)

a)

4.08 x 10-8

b)

4.6 x 102

c)

4.08 x 102

d)

4.08 x 10-15

44.
How would you write 4.3756 x 104 in standard form?
a)
437,560,000
b)
0.00043756
c)
43,756
d)
4,3756
45.
It is a measure of how close measurements come to each other when they are made in the same way
a)
Accuracy
b)
Precision
c)
Error
d)
Extrapolation
46.

How close a measurement is to the accepted value is called..

a)

Accuracy

b)

Precision

c)

Significant

d)

Estimate

47.

You know 1000 mg = 1 g.  Convert 2.5 grams into milligrams.

a)

25 mg

b)

25,000 mg

c)

250 mg

d)

2500 mg

48.

Convert 565,900 seconds into days.

a)

4.5 days

b)

5.5 days

c)

6.5 days

d)

7.5 days

49.

Convert 125 seconds to years.

a)

3.96 x 10-6

b)

2.38 x 10-4

c)

51.4

d)

.528

50.

How does electronegativity predict the type of bonding between elements?

a)

Similar electronegativities form ionic bonds

b)

Electronegativity doesn't affect bonding type

c)

Similar electronegativities form covalent bonds, large differences form ionic bonds.

d)

Large differences in electronegativity form covalent bonds

51.

Which element has a greater ELECTRONEGATIVITY, sulfur (S) or tellurium (Te)?

a)

sulfur

b)

tellurium

52.

Which element has a greater ELECTRONEGATIVITY, aluminum (Al) or sulfur (S)?

a)

aluminum

b)

sulfur

53.

A mole is:

a)

A furry animal

b)

6.02 x 10^23 of something

c)

An atom of an element

d)

The number of atoms in a compound

54.

A covalent compound contains:

a)

2 metals

b)

1 metal and 1 nonmetal

c)

2 nonmetals

d)

zero atoms

55.

A bond where electrons are transferred from one atom to another is called a:

a)

Covalent bond

b)

Ionic bond

c)

Metallic bond

d)

Strong bond

56.
Name group 1 on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
noble gases
d)
halogens
57.
Name group 2 on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
d)
transition metals
58.
Name group 18 on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
transition metals
d)
noble gases
59.
Name groups 3 - 12 on the periodic table.
a)
noble gases
b)
halogens
c)
metalloids
d)
transition metals
60.
Name group 17 on the periodic table.
a)
transition metals
b)
metalloids
c)
halogens
d)
alkali metals
61.
Elements in the same ________ are more chemically similar.
a)
group
b)
period
c)
club
d)
table
62.

Which element is in Group 6 Period 4

A
B
C
D
63.

Choose the group(s) that are highly electronegative and form a -1 charge.

A
B
C
D
E
F
G
H
I
64.

Label the parts of the periodic table with the correct characteristics that match it.

a)

unreactive

b)

non metals

c)

soft metals, will take electrons

d)

strong, colorful

e)

very reactive

f)

radioactive

g)

lamps, fluorescent

1
2
3
4
5
1)
2)
3)
4)
5)
65.

Label the parts of the periodic table with the correct characteristics that match it.

a)

look like metals behave like non metals

b)

unreactive

c)

non metals

d)

soft metals, will take electrons

e)

strong, colorful

f)

very reactive

g)

radioactive

h)

lamps, fluorescent

1
2
3
4
5
1)
2)
3)
4)
5)
66.
Visible spectrum is shown below. Which light has the highest energy?
a)
Red light
b)
Yellow light
c)
Green light
d)
Blue light
67.

When heated, electrons are ____________.

a)

annoyed

b)

irritated

c)

excited

d)

angered

68.

When an electron transitions from a low energy level to a high energy level, the electron...

a)

absorbs energy and moves away from the nucleus

b)

emits energy and moves closer to the nucleus

c)

absorbs energy and moves closer to the nucleus

d)

emits energy and moves away from the nucleus

69.
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
70.

Which of the following names and formulas are correctly paired together?

a)

sodium oxide - NaO

b)

calcium sulfite - Ca2(SO3)2

c)

barium bromate - Ba(BrO2)2

d)

lithium chromate - Li2CrO4

e)

potassium phosphide - KP3

71.

What is the correct name of Ag2SO4?

a)

silver sulfoxide

b)

silver sulfate

c)

silver sulfite

d)

silver tetrasulfoate

72.

What is the correct formula of strontium hydroxide?

a)

SrH

b)

SrOH

c)

Sr(OH)2

d)

SrH2

73.
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
74.
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
75.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
76.

Which ion has the smallest radius?

a)

Ga3+

b)

K+

c)

Ca2+

d)

Cl-

e)

S2-

77.
Of the elements Ca, Be, Ba, and Sr, which has the largest atomic radius?
a)
Be
b)
Ba
c)
Ca
d)
Sr
78.

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

79.

Which of the following elements GAINS 1 electron in order to attain an octet?

a)

sodium

b)

calcium

c)

helium

d)

boron

e)

chlorine

80.

Which of the following elements LOSES 2 electrons in order to attain an octet?

a)

lithium

b)

magnesium

c)

helium

d)

sulfur

e)

bromine

81.
Which has the greater EN: 
N or C?
a)
C
b)
N
82.
Which has the greater EN: 
H or F?
a)
H
b)
F
83.
What is ionization energy?
a)
Energy needed to destroy an atom
b)
Energy required to remove an electron
c)
Energy needed to split an electron
d)
Energy required to add an electron
84.

As you look down a group, ionization energy and electronegativity

a)

increases

b)

decreases

85.

As you look from left to right across a period, ionization energy and electronegativity both

a)

increase

b)

decrease

86.

Which element has the greater ionization energy?

a)

Magnesium (Mg)

b)

Phosphorus (P)

87.

Which element has the greater ionization energy?

a)

Iodine (I)

b)

Chlorine (Cl)

88.

Covalent is a bond formed by the sharing of electrons. Occurs between two nonmetals.

a)

True

b)

False

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