Name:
Chemistry 1 – Midterm Review Sheet
2013-2014
Unit 1 – Properties and Classification of Matter and Energy
Element Symbols
1.
Give the symbols for the following elements. a.
lead ______Pb________
Date: b.
c.
d.
iron ______Fe________ silver ____Ag_________ antimony _____Sb________
Chemical and Physical Changes
2.
Name four evidences that indicate a chemical change has taken place. a.
Formation of a precipitate b.
Gas formation c.
Energy transfer d.
Color change
3.
Classify each of the following as a chemical change or a physical change . Write CC or PC. a.
A pile of snow gradually vaporizes. - PC b.
Cu burns in the presence of O
2
to form CuO. - CC c.
An antacid tablet fizzes and releases carbon dioxide gas when it comes in contact with HCl in the stomach. - CC d.
A sugar cube dissolves in water. - PC
4.
Which of the following is a physical change? a.
b.
burning gasoline cooking an egg c.
decomposing meat d.
steam condensing on a cold bathroom mirror e.
rusting iron
5.
Circle the following which are compounds: a.
table salt b.
c.
d.
e. carbon copper water mercury
6.
A sample of an element contains only one kind of a.
b.
isotope mixture c.
d.
e.
atom pure substance none of these
7.
The state of matter for an object that has neither definite shape nor definite volume is a.
b.
solid liquid c.
d.
e.
gaseous elemental mixed
1

Mixtures
8.
Classify each of the following as mixtures or pure substances: a.
oil and water - mix b.
methanol – P.S.
c.
vinegar in water- mix d.
a diamond – P.S.
e.
milk - mix
9.
Which of the mixture(s) in question 8 is/are a homogeneous mixture? Write the letter(s) below.
C (solution)
10.
Which of the mixture(s) in question 8 is/are a heterogeneous mixture? Write the letter(s) below.
A (Suspension) and E (Colloid)
11.
Which of the mixture(s) in question 8 is/are a colloid? Write the letter(s) below. - E
12.
Which mixture can be separated by using the equipment shown to the right? a.
A homogeneous solution of sugar in water b.
A heterogeneous mixture of sand and water c.
A homogeneous mixture of salt and water
Energy
13.
Are the following processes exothermic or endothermic? a.
When solid HCl is dissolved in water, the solution gets hotter. - Exo b.
Natural gas (CH
4
) is burned in a furnace. - Exo c.
When concentrated NH
4
Cl is added to water, the solution gets very cold. - Endo d.
Water is boiled in a tea kettle. – Endo (water absorbs heat)
Unit 2 – Scientific Experimentation
Significant Figures
14.
a.
2000 m
How many significant figures are in each of the following measurements?
______1______ b.
0.0025 cm ______2______ c.
202 mL d.
150. kg
______3______
______3______
Significant Figures in Calculations
Perform each of the following calculations and express your answer to the correct number of significant figures.
15.
(8.0 g + 11.04 g) – 0.01 g = 19.0 g
16.
250kg/10L = 30 kg/L
2

17.
Conversion Factors
Convert each of the following measurements to the given units.
18.
5.0 L =
33.70cm x 0.007cm x 1200cm = 300 cm 3
_____5.0 x 10 3 ____cm 3
0.025m = ____2.5 x 10 4 _____um 19.
20.
150 cm = ____1.5 x 10 -5 _____nm
21.
100in 3 = ___2 x 10 -3 ______m 3
Precision and Accuracy
The density of water was measured by three different students. Who was more accurate in his/her calculations? What was his/her accuracy? (Hint: What is the accepted value for the density of water in g/mL?) Jim= most precise… most consistent measurements ( +/- 0.01)
Jon % error = 4%, Jim % error = 0 % , Joanna % error = 1 %... Jim is also most accurate
Trials
1
2
3
4
Jon g/mL
1.00
1.25
0.95
0.94
Jim g/mL
1.02
1.00
0.99
0.98
Joanna
1.10
0.90
0.91
1.05
g/mL
Density
22.
Water has a density of 1.0 g/mL. Which of the objects will float in water? a.
Object 1: mass = 50.0 g; volume = 60.8 mL b.
Object II: mass = 65.2 g; volume = 42.1 mL c.
Object III: mass = 100.0 g; volume = 20.0 mL a. II b. III c. I d. II, III e. I, III
23.
What volume would be occupied by a piece of aluminum (density = 2.70 g/mL) weighing 85 g? a. 3.2 x10 2 mL b. 229.5 mL c. 3.2 mL d. 31 mL e. none of these
D = m/V – > V = m/D = 85 g / 2.70 g/mL = 31.48 mL
3

Unit 3 – Atomic Structure and Nuclear Chemistry
Early Atomic Theory
24.
The scientist whose alpha-particle scattering experiment led him to conclude that the nucleus of an atom contains a dense center of positive charge is
a. J. J. Thomson
b. Lord Kelvin
c. Ernest Rutherford
d. William Thomson
e. James Chadwick
Atomic Structure
2 5 . How many protons, electrons, and neutrons respectively does 127 I have? a.
b.
c.
d.
e.
53, 127, 74
53, 74, 53
53, 53, 127
74, 53, 127
53, 53, 74
26.
The number of neutrons in one atom of 206 Hg is
82 a.
b.
c.
d.
82
206
124
288
27.
Write the alpha decay of the following elements a.
Lead-210 210
82
Pb ! →
2
4
He +
206
80
Hg b.
Radon-222 222
86
Rn ! →
2
4 He +
218
82
Pb c.
28.
a.
Uranium-238 238
92
U !
2
4 He +
234
90
Th
Write the beta decay of the following elements:
C-14 14
6
C ! →
0
− 1 e +
14
7
N
4

b.
Na-20 20
11
Na ! →
0
− 1 e +
20
12
Mg
Unit 4 –Electrons in Atoms and Periodic Trends
29.
The form of EMR that has more energy per photon than X-rays is a.
b.
c.
d.
e.
microwaves radio waves gamma rays infrared rays none of these
30.
The energy levels of the hydrogen atom (and all atoms) are ______________, meaning that only certain discrete energy levels are allowed. a.
varied b.
quantized c.
d.
e.
ramp-like continuous two of these
31.
The form of EMR that has less energy than microwaves is a.
b.
radio waves c.
microwaves gamma rays d.
e.
infrared rays none of these
32.
The probability map for an electron is called a.
an orbit b.
c.
a photon an orbital d.
e.
an electron configuration none of these
33.
As the principal energy level increases in an atom, the average distance of an electron from the nucleus ______________. a.
increases b.
c.
decreases stays the same d.
e.
varies none of these
34.
The shape of an s orbital is a.
b.
spherical dumbbell shaped c.
d.
e.
donut shaped conical shaped none of these
5

35.
A given set of p orbitals consists of ______________ orbital(s). a.
1 d.
b.
c.
2
3 e.
4
5
36.
The maximum number of electrons allowed in each of the p orbitals is a.
b.
c.
d.
2
4
8
18 e.
none of these
38.
The maximum number of electrons allowed in each of the d orbitals is a.
b.
c.
d.
e.
2
4
8
10
32
Electron Configurations
39.
Sodium has how many electrons in its outermost principal energy level? a.
1 b.
2 c.
d.
e.
6
8
11
37.
A given set of d orbitals consists of ______________ orbital(s). a.
b.
c.
1
3
5 d.
e.
6 none of these
40.
The number of unpaired electrons in an oxygen atom is a.
1 b.
2 c.
3 d.
e.
4
5
41.
Which element or ion listed below has the electron configuration 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 ? a) Cl b) Br c) Se d)
2+ e) two of these
42.
The electron configuration for the phosphorus atom is a.
b.
c.
d.
1
1
1
1 s s s s
2
2
2
2
2 s
2 s
2
2 s s
2
2
2
2
2 p
2 p
2 p
2 p
6
6
6
6
3 s
3 s
3 s
3 p
2
2
5
5
3 p
3 p
3
6 4 s 1 e.
none of these
6

43.
5. The electron configuration for the carbon atom is a.
b.
c.
d.
1 s
1 s
2 2 s
[He] 2
[Ne] 2
2 2 p
2 2 p
4 s s
4
2
2 2 p 2 e.
none of these
44.
When moving down a group (family) in the periodic table, the number of valence electrons a.
remains constant b.
c.
increases by 2 then 8 then 18 then 32 doubles with each move d.
e.
decreases regularly changes in an unpredictable manner
45.
The element with the electron configuration [Kr] 5 s 2 4 d 10 5 p a.
As b.
Sb c.
Nb
Atomic Trends
46.
Which of the following atoms has the largest atomic radius ? a.
b.
c.
d.
Na
Mg
Si
P
3 is d.
e.
Pr none of these e.
C
47.
Which of the following atoms has the highest ionization energy ? a.
Na b.
c.
Mg
Si d.
e.
P
Cl
48.
3. A phosphorus atom needs to gain ______________ electrons to achieve a noble gas configuration.
a) 2 b) 3 c) 4 d) 5 e) 6
Periodic Table
49.
Which of the following elements is an alkali metal? a.
Ca b.
c.
Cu
Fe d.
Na e.
Sc
50.
Halogens exist naturally as these types of molecules. a.
Monatomic b.
Diatomic c.
Elements d.
Ionic a)
7

51.
Which of the following elements is most chemically similar to Ca? a.
Na b.
c.
N
O d.
Mg e.
C
52.
Rows of the periodic table are called? ____________Periods_____________________
53.
Columns of the periodic table are called? _________Groups/Families_____________
Unit 5 – Chemical Bonding
54.
When electrons are shared unequally, chemists characterize these types of bonds as ______________.
a) polar covalent d) unbalanced b) e) ionic none of these c) pure covalent
55.
Chemical bonds formed by the attraction of oppositely charged ions are called
a) covalent bonds b) magnetic bonds c) coordinate bonds
d) ionic bonds e) none of these
56.
Which of the following compounds contains one or more covalent bonds? a) NaCl b) CaO c) CO
2 d) Cs
2
O e) BaBr
2
57.
How many lone pairs of electrons are in the Lewis structure for ammonia, NH
3
? a) 0 b) 1 c) 2 d) 3 e) 4
58.
Choose the correct Lewis structure for the OH ion. a) c) b) d)
59.
Which of the following has a double bond? a) H
2
O b) C
2
H
2 c) C
2
H
4 d) CN – e) none of these
60.
What is the correct order of the following bonds in terms of decreasing polarity? a)
b) P--Cl, N--Cl, As--Cl c) As--Cl, N--Cl, P--Cl d) P--Cl, As--Cl, N--Cl e) As--Cl, P--Cl, N--Cl
8