Name ____________________________________ Date ______________ ID _____________________
Chemistry (2)
Interim Assessment – Third Grading Period
1. As you examine the elements in period four, going from left to right, you notice atomic size generally
decreases. This is best explained by the fact that
protons are being added to each element which makes them have more mass, resulting in a smaller
atom.
the nucleus becomes denser and so the atoms of an element become much smaller than the atoms of
the element before it.
as the number of protons in the nucleus increase, the outer electrons are pulled in closer which
decreases the overall size of the atom.
metals, being harder than nonmetal, will aways have atoms that are larger than nonmetals.
2. Ionization energy, simply stated, is the energy needed to remove an electron from an atom. Which of
the following elements has the highest ionization energy?
Nitrogen
Magnesium
Copper
Lithium
3. A new element is discovered and given the symbol Sa. It has an electron configuration that ends in
4s2 4p3 and is placed in group 5A (15). The electron dot diagram for Sa should be
Chemistry (2)
Interim Assessment (3)
Page 1
4. Metal atoms become metal ions by
gaining electrons
losing electrons
gaining protons
losing protons
5. Which of the following, when combined, will form an ionic bond?
Pb and Cr
S and O
Li and F
N and N
6. Which of the following is a property of ionic compounds?
Most are hard and have a metallic appearance.
They are often found as liquids at room temperature.
When dissolved in water they conduct an electrical current.
Generally they have rather low melting points.
7. Metals are conductors of electrical current. This is explained by the fact that
electrons in metals are mobile and can drift freely.
metals have more electrons than nonmetals.
metals can be melted and formed into long strands.
magnetic force lines push electrons out of metallic atoms.
Chemistry (2)
Interim Assessment (3)
Page 2
8. Which of the following structures is an example of covalent bonding?
9. Gasoline will dissolve a greasy spot on a cotton shirt, but it cannot dissolve sugar. Ordinary water
can dissolve sugar but not greasy spots. Water and gasoline do not mix. Gasoline is described as
having a non-polar structure while water is described as being polar. Which of the following substances
can you infer will dissolve in gasoline?
salt
detergent
powder milk flakes
butter
10. What is the major factor that determines if a substance is a solid, liquid, or gas at room temperature?
The type of bonding it displays.
The mass of the molecular structure.
The position of its elements on the periodic table.
The mass to density ratio of its components.
11. Which of the following compounds is composed of formula units?
He
O2
MgF2
CC14
Chemistry (2)
Interim Assessment (3)
Page 3
12. Which of the following polyatomic ions contains the most oxygen atoms?
Ammonium
Nitride
Sulfite
Phosphate
13. Which of the following is classified as a binary molecular compound?
CaS
NO2
KOH
H2
14. The name of a compound contains a prefix. This indicates the compound
is binary molecular.
is binary ionic.
contains a polyatomic ion.
must contain oxygen atoms.
15. Iodine is in group 7A(17). When it becomes an ion, how many electrons does it gain?
1
7
17
10
16. The correct name for the chemical compound A1F3 is
Aluminum Tri-Fluorine
Aluminum Fluoride
Aluminum Fluorate
Aluminum Fluorite
Chemistry (2)
Interim Assessment (3)
Page 4
17. When Methane (CH4) is completely burned in the presence of Oxygen (O2), what are the products
that are formed?
Carbon and hydroxide
Ozone
Carbon and water
Water and carbon dioxide
18. Identify the correct formula for Copper(II) Nitride
CuN2
CuN
Cu3N2
Cu2N3
19. Use the chemical equation below to the question.
A1(NO3)3 +
CaS
A12S3 +
Ca(NO3)2
Which sequence of coefficients are in the correct order to correctly balance the chemical reaction?
6, 1, 5, 5
2, 3, 1, 3
3, 2, 2, 3
1, 4, 2, 3
20. Use the chemical equation below to answer the question.
HC1 + NaOH
HOH + NaC1
This chemical equation is an example of a
reaction.
Double replacement
Synthesis
Combustion
Displacement
Chemistry (2)
Interim Assessment (3)
Page 5
21. In a balanced chemical equation you are given one mole of Ni(OH)2. Use information contained in
the periodic table to calculate how many grams of the compound you have.
48.2
75.6
92.7
104.4
22. A balanced chemical reaction produced one hundred twenty five (125) grams of Gold (Au). This
moles of Gold.
amount is equivalent to
0.63
1.45
19.09
322.44
23. The following is a word equation for a chemical reaction: Gasoline is combined with oxygen to
produce carbon dioxide, water vapor, heat and light. What must happen for this reaction to occur?
Heat must be added to start the reaction.
The liquid must be in a sealed metal container.
There must be more gasoline molecules than oxygen molecules.
The air must be free of moisture.
Use the periodic table to answer question 24.
24. Based on their placement on the periodic table, which element listed below is not expected to take
place in chemical reactions?
Hydrogen
Helium
Aluminum
Iodine
Chemistry (2)
Interim Assessment (3)
Page 6
Name___________________________ Date___________________ ID ____________
Chemistry (2) Interim Assessment
Third Grading Period
Answer Document
1. _____
2. _____
3. _____
4. _____
5. _____
6. _____
7. _____
8. _____
9. _____
10. _____
11. _____
12. _____
13. _____
14. _____
15. _____
16. _____
17. _____
18. _____
19. _____
20. _____
21. _____
22. _____
23. _____
24. _____
Ion Chart
For use on IPC and Chemistry Interim Assessments
Common Monatomic Ions
+1
Li
Na
K
Rb
Cs
Cu
Ag
+2
Ba
Mg
Ca
Sr
Cu
Fe
Be
Hg
Sn
Co
Mn
Cr
Pb
Ni
Zn
+3
Al
Fe
Cr
Mn
Co
+4
Pb
Sn
-3
N
P
As
-2
O
S
Se
-1
F
Cl
Br
I
Common Polyatomic Ions
-1 Charge
Formula
Name
-2 Charge
Formula
Name
-3 Charge
Formula
Name
C2H3O2
Acetate
HPO4
HCO3
Hydrogen
Carbonate
Hydrogen
Sulfate
Nitrite
Nitrate
Cyanide
Hydroxide
Permanganate
Chlorite
Chlorate
SO3
Hydrogen
Phosphate
Sulfite
SO4
Sulfate
CO3
CrO4
Cr2O7
SiO3
Carbonate
+1 Charge
Chromate
NH4
Ammonium
Dichromate
Silicate
HSO4
NO2
NO3
CN
OH
MnO4
ClO2
ClO3
PO3
Phosphite
PO4
Phosphate
D=
Q = (m)(∆T)(Cp )
d
t
v − vi
a= f
∆t
s=
Momentum = mass × velocity
p = mv
Force = mass × acceleration
F = ma
6
Work = force × distance
W = Fd
7
P=
mv 2
2
GPE = mgh
Energy = mass × (speed of light) 2
E = mc 2
Velocity of a wave = frequency × wavelength
v = fλ
11
Gravitational potential energy = mass × acceleration due to gravity × height
10
KE =
9
work output
× 100
work input
1
Kinetic energy = 2 (mass × velocity 2)
% efficiency =
8
W
t
WO
%=
× 100
WI
work
time
4
Power =
3
Speed =
5
distance
time
final velocity − initial velocity
Acceleration =
change in time
2
gained or
mass in
change in
specific
=
( heat
lost by water ) ( grams )( temperature )( heat )
m
v
1
mass
volume
0
Density =
Centimeters
FORMULA CHART
for Grades 10–11 Science Assessment
12
I=
V
R
P = VI
Electrical energy = power × time
E = Pt
15
Electrical power = voltage × current
14
voltage
resistance
13
Current =
16
17
Constants/Conversions
c = speed of light = 3 × 10 8 m/s
19
speed of sound = 343 m/s at 20°C
18
g = acceleration due to gravity = 9.8 m/s 2
1 cm 3 = 1 mL
20
1 wave/second = 1 hertz (Hz)
1 calorie (cal) = 4.18 joules
1000 calories (cal) = 1 Calorie (Cal) = 1 kilocalorie (kcal)
newton (N) = kgm/s 2
joule (J) = Nm
watt (W) = J/s = Nm/s
volt (V)
ampere (A)
ohm (Ω)
13
14
7
6
5
4
3
2
1
6
VIB
7
VIIB
8
9
VIII
10
11
IB
12
IIB
Ti
47.88
Sc
44.956
Scandium
39
Y
88.906
Ca
40.08
Calcium
38
Sr
K
39.098
Potassium
37
Rb
Lanthanum
89
Ac
227.028
56
Ba
137.33
Barium
88
Ra
226.025
Radium
55
Cs
132.905
Cesium
87
Fr
(223)
Francium
91.224
(261)
Rf
104
Hafnium
178.49
Hf
72
Zirconium
Rutherfordium
Actinide Series
Lanthanide Series
Actinium
138.906
La
57
Yttrium
87.62
Strontium
85.468
Rubidium
Zr
40
Titanium
22
20
19
21
24.305
Magnesium
Mg
Na
Sodium
12
11
22.990
9.012
Beryllium
6.941
Lithium
(98)
Tc
43
Manganese
54.938
Mn
25
144.24
(145)
Pm
61
Hassium
(265)
Hs
108
Osmium
190.23
Os
76
Ruthenium
101.07
Ru
44
Iron
55.847
Fe
26
91
Pa
231.036
Protactinium
90
Th
232.038
Thorium
Uranium
238.029
U
92
Neptunium
237.048
Np
93
Praseodymium Neodymium Promethium
140.908
Cerium
140.12
Nd
60
59
Pr
58
Ce
Bohrium
(263)
Seaborgium
(262)
Bh
107
Rhenium
186.207
Re
75
(262)
Sg
106
Tungsten
183.84
W
74
Molybdenum Technetium
95.94
Mo
42
Chromium
51.996
Cr
24
Dubnium
Db
105
Tantalum
180.948
Ta
73
Niobium
92.906
Nb
41
Vanadium
50.942
V
23
Plutonium
(244)
Pu
94
Samarium
150.36
Sm
62
Meitnerium
(266)
Mt
109
Iridium
192.22
Ir
77
Rhodium
102.906
Rh
45
Cobalt
58.933
Co
27
Americium
(243)
Am
95
Europium
151.97
Eu
63
(269)
110
Platinum
195.08
Pt
78
Palladium
106.42
Pd
46
Nickel
58.69
Ni
28
69.72
48
Mercury
200.59
Hg
80
Cadmium
112.41
Cd
Thallium
204.383
Tl
81
Indium
114.82
In
49
Gallium
65.39
Zinc
Ga
31
Zn
30
Aluminum
26.982
Al
13
Boron
Lead
207.2
Pb
82
Tin
118.71
Sn
50
Germanium
72.61
Ge
32
Silicon
28.086
Si
14
Carbon
12.011
C
6
14
IVA
64
Curium
(247)
Cm
96
Gadolinium
157.25
Gd
65
Berkelium
(247)
Bk
97
Terbium
158.925
Tb
66
Californium
(251)
Cf
98
Dysprosium
162.50
Dy
67
Einsteinium
(252)
Es
99
Holmium
164.930
Ho
30.974
P
15
Nitrogen
14.007
N
7
15
VA
Fermium
(257)
Fm
100
Erbium
167.26
Er
68
Bismuth
208.980
Bi
83
Antimony
121.763
Sb
51
Arsenic
74.922
As
33
Phosphorus
Name
Mass numbers in parentheses are those of
the most stable or most common isotope.
Gold
196.967
Au
79
Silver
107.868
Ag
47
Copper
63.546
Cu
29
10.81
5
VB
B
Be
5
Li
13
IIIA
4
1.008
3
4
IVB
Atomic mass
2
IIA
3
IIIB
Si
28.086
Symbol
Silicon
14
Atomic number
Hydrogen
H
1
Group
1
IA
Periodic Table of the Elements
Nobelium
(259)
No
102
Ytterbium
173.04
Yb
70
Astatine
(210)
At
85
Iodine
126.904
I
53
Bromine
79.904
Br
35
Chlorine
35.453
Cl
17
Fluorine
18.998
F
9
17
VIIA
Lawrencium
(262)
Lr
103
Lutetium
174.967
Lu
71
Radon
(222)
Rn
86
Xenon
131.29
Xe
54
Krypton
83.80
Kr
36
Argon
39.948
Ar
18
Neon
20.179
Ne
10
Helium
4.0026
Revised October 15, 2001
Mendelevium
(258)
Md
101
Thulium
168.934
Tm
69
Polonium
(209)
Po
84
Tellurium
127.60
Te
52
Selenium
78.96
Se
34
Sulfur
32.066
S
16
Oxygen
15.999
O
8
16
VIA
He
2
18
VIIIA