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Fall Semester Exam Review

Total questions: 55

Worksheet time: 55mins

Name
Class
Date
1.
Mr. S. sets up an experiment to see how the mass of a ball affects the distance it rolls off a ramp.  Identify the independent variable.
a)
distance traveled by the ball
b)
height of the ramp
c)
mass of the ball
d)
weight of the ball
2.
A student is planning an experiment to find out how the height from which he drops a ball affects how high the ball bounces. The dependent variable is the _____.
a)
Diameter of the ball
b)
Force acting on the ball
c)
Height that the ball bounces
d)
Height from which the ball is dropped
3.
Recording data on how yellow or orange leaves turn in October by describing them as "green" "slightly yellow" "very yellow" or "orange" is ____ data
a)
quantitative
b)
qualitative
4.
Convert 17 m to cm:
a)
0.17 cm
b)
0.017 cm
c)
1,700 cm
d)
170 cm
5.
7,000 g = ____ kg
a)
70
b)
700
c)
7
d)
0.07
6.
How many significant figures does the following number have: 0.002040
a)
6
b)
4
c)
3
d)
2
7.
Round 0.010229 to four sig figs
a)
1022
b)
1023
c)
0.01023
d)
0.01022
8.
What is the measurement 1042 Liters rounded to 2 significant figures? 
a)
1040 L
b)
1.1 x 103 L
c)
1.0 x 103 L
d)
1050 L
9.
This particle is found in the nucleus and has no charge
a)
Neutron
b)
Proton
c)
Electron
10.
This contains most of the mass of an atom
a)
Electron Cloud
b)
Nucleus
c)
Electron
11.
Which particle is responsible for the chemical properties of an atom?
a)
Neutron
b)
Protons
c)
Valence Electrons
d)
Nucleus
12.
What element is pictured?
a)
Hydorgen
b)
Boron
c)
Beryllium
d)
Arsenic
13.
The atomic number for Oxygen is 8, so
a)
there are 8 protons in the atom
b)
the atomic mass is less than 8
c)
the mass of the atom is 8
d)
the atom is decaying
14.
We use the periodic table to calculate...
a)
mass
b)
molar mass
c)
moles
15.

Which has more particles?

a)
1 mole H2O
b)
1 mole Al(OH)3
c)
1 mole NaCl
d)
There are all the same
16.
What is the molar mass of sodium?
a)
11
b)

22.99

c)
45.98
d)
3
17.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
18.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
19.
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
20.
High frequency waves have _________ wavelengths.
a)
varying
b)
long
c)
the same
d)
short
21.
All electromagnetic waves have the same...
a)
frequency
b)
speed
c)
wavelength
d)
energy
22.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
23.
What usually forms the positive ion?
a)
Metal
b)
Non Metals
c)
None
24.
What happens when the sodium atom loses an electron?
a)
It become negatively charged 
b)
It become positively charged
c)
none
25.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
26.
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
27.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
28.
Which of the following formulas represents the harmful gas, carbon monoxide?
a)
CO
b)
CO2
c)
NO
d)
SO2
29.
Which compound contains covalent bonds?
a)
NaI
b)
K2O
c)
N2O3
d)
BeO
30.
The name of Mg₃N₂ is
a)
manganese nitride
b)
magnesium nitride
c)
magnesium (III) nitride
d)
trimagnesium dinitride
31.
The name of Al₂(SO₄)₃ is
a)
aluminum sulfur oxide
b)
aluminum sulfate
c)
aluminum trisulfate
d)
aluminum (III) sulfate
32.
The name of Ni₂O₃ is
a)
nickel (II) oxide
b)
nickel (III) oxide
c)
nickle oxide
d)
dinickel trioxide
33.
The chemical formula of iron (III)bromide is
a)
FeBr
b)
Fe(III)Br
c)
FeBr₃
d)
Fe₂Br₃
34.
The name of SO₃ compound is
a)
sulfate
b)
sulfur oxide
c)
sulfur trioxide
d)
monosulfur trioxide
35.
The name of P₄S₁₀ is
a)
phosphorous sulfide
b)
phosphorus sulfide
c)
tetraphosphorus decasulfide
d)
phosphorus (X) sulfide
36.

What percentage of the total atomic mass of lithium phosphide (Li3P) is composed of phosphorus?

a)

13%

b)

29%

c)

40%

d)

60%

37.

What is the correct formula for Magnesium sulfate heptahydrate?

a)

MgSO4·7H2O

b)

MgSO4·5H2O

c)

MgSO4·2H2O

d)

Mg2SO4·7H2O

38.

What is the molar mass of Copper(II) nitrate?

a)

187.56 g/mol

b)

241.60 g/mol

c)

125.55 g/mol

d)

164.55 g/mol

39.

A compound that attracts and holds water in the structure forming a crystalline substance is called a(n)

a)

anhydrous material

b)

hydrate

c)

electrolyte

d)

alloy

40.

A 15.67 g sample of a hydrate of magnesium carbonate was heated to drive off the waters of hydration. The mass after heating was reduced to 7.58 g. Calculate the percent water by mass in the original hydrate.

a)

7.58 %

b)

8.09%

c)

48.37%

d)

51.63%

41.

Avery, Samuel, and Hannah are in a chemistry class. Their teacher asked them to identify the formula with the lowest whole # ratio of elements in a compound. What is this formula called?

a)

Molecular Formula

b)

Chemical Formula

c)

Empirical Formula 

d)

Distance Formula

42.

Which of the following could be a molecular formula with the empirical formula of CH2O?

a)

CH2O2

b)

CHO

c)

C3H5O3

d)

C2H4O2

43.

What is the empirical formula for:

C3H18

a)

CHO

b)

CO6

c)

CH2

d)

CH6

44.
Groups on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
45.

Group 1: These metals are extremely reactive. They all have one valence electron. They are shiny and silver in color. They are soft and can be cut with a knife.

a)

Transition Metals

b)

Alkali Metals

c)

Alkaline Metals

d)

Lanthanides

46.

Group 17: All nonmetals. Very reactive. Poor conductors of heat and electricity. Tend to form salts with metals. Example NaCl: sodium chloride which is known as table salt. These elemtns have 7 valence electrons (Group # minus 10).

a)

Boron Group

b)

Oxygen Group

c)

Nitrogen Group

d)

Halogens

47.

Which elements in the periodic table are least

likely to combine with other elements?

a)

halogens

b)

noble gases

c)

alkaline earth metals

d)

transition metals

48.
How many atoms of carbon are in 6.00g of carbon?
a)
1.20x1024atoms C
b)
6.02x1023atoms C
c)
3.01x1023atoms C
d)
1.50x1023atoms C
49.
How many moles are in 16.94g of water?
a)
16.94 mol H2O
b)
0.9401 mol H2O
c)
305.3 mol H2O
d)
1.063 mol H2O
50.
What is the mass in grams of 5.90 mol C8H18?
a)
.0512 g
b)
19.4 g
c)
673 g
d)
389 g
51.

Which EM waves have the highest energy & are the most dangerous?

a)

radio

b)

gamma rays

c)

infrared

d)

x-rays

52.
Which has the LONGEST wavelength and, therefore, the lowest frequency/energy
a)
Gamma Rays
b)
Radio Waves
c)
Visible Light
d)
Infrared rays
53.
A wave with a large wavelength will have a ______ frequency and _____ energy
a)
high, low
b)
high, high
c)
low, high
d)
low, low
54.
24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu.
What is the average mass of this element?
a)
74.92 amu
b)
24.97 amu
c)
75.01 amu
d)
74.51 amu
55.

What is the noble gas configuration for Cobalt?

a)

[Kr] 4s2 3d7

b)

[Kr] 4s2 4d7

c)

[Ar] 4s2 3d7

d)

[Ar] 4s2 4d7

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