Download Name: Date: Chemistry 1 – Midterm Review Sheet Unit 1 – Scientific

Name:
Date:
Chemistry 1 – Midterm Review Sheet
Unit 1 – Scientific Experimentation
Scientific Experimentation
1. An experiment is designed to determine where the hottest part of a
Bunsen flame is located. The height of the beaker above the burner is
varied and how long it takes for the 100mL of water to boil is measured.
a. What is the independent variable in this experiment?
- The height of the beaker above the flame.
b. What is the dependent variable in this experiment?
- The time taken for the water to boil.
height
c. What is a control in this experiment?
- Amount of water (100 mL)
Significant Figures
1. How many significant figures are in each of the following
measurements?
a. 2000 m
______1______
b. 0.0025 cm
______2______
c. 202 mL
______3______
d. 150. kg
______3______
Significant Figures in Calculations
Perform each of the following calculations and express your answer to the correct number of
significant figures.
2. 8.0 g + 11.04 g – 0.01 g = 19.0 g
3. 250kg/10L = 30 kg/L
4. 33.70cm x 0.007cm x 1200cm =
300 cm3
Conversion Factors
Convert each of the following measurements to the given units.
1. 5.0 L =
_____5.0 x 103____cm3
2. 0.025m =
3. 150 cm =
____2.5 x 104_____um
____1.5 x 10-5_____nm
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4. 100in3 =
___2 x 10-3______m3
5. A measurement has a number and a ______unit__________.
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?) SKIP. We will discuss in class!
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 g/mL
1.10
0.90
0.91
1.05
Unit 2 – Properties and Classification of Matter/Chemical Foundations
Chemical and Physical Changes
1. Name four evidences that indicate a chemical change has taken place.
a. Color Change
b. Formation of a precipitate (solid)
c. Formation of a gas
d. Energy Transfer
2. 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 O2 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
3. Which of the following is a physical change?
a. burning gasoline
b. cooking an egg
c. decomposing meat
d. steam condensing on a cold bathroom mirror
e. rusting iron
4. How many of the following are compounds: table salt, carbon, copper, water, mercury?
a. 1
b. 2
c. 3
d. 4
e. 5
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5. A sample of an element contains only one kind of
a. isotope
b. mixture
c. atom
d. pure substance
e. none of these
6. The state of matter for an object that has neither definite shape nor definite volume is
a. solid
b. liquid
c. gaseous
d. elemental
e. mixed
Mixtures
1. Classify each of the following as mixtures or pure substances:
a. NITINOL - Mixture
b. oil and water - Mixture
c. methanol – Pure substance
d. vinegar in water - Mixture
e. a diamond - Pure substance
f. milk - Mixture
2. Which of the mixture(s) in question 1 is/are a homogeneous mixture? Write the letter(s) below.
- A, D
3. Which of the mixture(s) in question 1 is/are a heterogeneous mixture? Write the letter(s) below.
- B, F
4. Which of the mixture(s) in question 1 is/are a colloid? Write
the letter(s) below.
-F
5. 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
Density
1. 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
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2. What volume would be occupied by a piece of aluminum (density = 2.70 g/mL) weighing 85 g?
a. 3.2 x102 mL
b. 229.5 mL
c. 3.2 mL
d. 31 mL
e. none of these
Element Symbols
1. The symbol for the element mercury is
a. Hg
b. Mn
c. Mg
d. Ag
e. Mr
2. Give the symbols for the following elements.
a. lead _____Pb_________
b. iron ____ Fe__________
c. silver ___ Ag___________
Formulas
3. A substance composed of two or more elements combined chemically in a fixed proportion by mass is
a. a compound
b. a mixture
c. an atom
d. a solid
e. none of these
4. How many hydrogen atoms are indicated in the formula (NH4)2C8H4O2?
a. 8
b. 12
c. 20
d. 24
e. none of these
5. The total number of oxygen atoms indicated by the formula Fe2(CO3)3 is
a. 3
b. 6
c. 9
d. 12
e. 18
Early Atomic Theory
6. 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
7 . How many protons, electrons, and neutrons respectively does
a.
b.
c.
d.
e.
127
I have?
53, 127, 74
53, 74, 53
53, 53, 127
74, 53, 127
53, 53, 74
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8. The number of neutrons in one atom of
a.
b.
c.
d.
206
82
Hg is
82
206
124
288
9. Which of the following compounds is ionic?
a. MgO
b. SO3
c. HCl
d. CO2
Periodic Table
10. Which of the following elements is an alkali metal?
a. Ca
b. Cu
c. Fe
d. Na
e. Sc
11. Halogens exist naturally as these types of molecules.
e. Monatomic
f. Diatomic
g. Elements
h. Ionic
12. Which of the following elements is most chemically similar to Ca?
a. Na
b. N
c. O
d. Mg
e. C
13. Rows of the periodic table are called? _________Periods___________________________
14. Columns of the periodic table are called? ______Groups/Families____________________
Unit 3 – Modern Atomic Theory EM Radiation/ Atomic Orbitals
1. The form of EMR that has more energy per photon than X-rays is
i. microwaves
j. radio waves
k. gamma rays
l. infrared rays
m. none of these
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3. 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. ramp-like
d. continuous
e. two of these
4. The form of EMR that has less energy than microwaves is
a. microwaves
b. radio waves
c. gamma rays
d. infrared rays
e. none of these
5. The probability map for an electron is called
a. an orbit
b. a photon
c. an orbital
d. an electron configuration
e. none of these
6. As the principal energy level increases in an atom, the average distance of an electron from the nucleus
______________.
a. increases
b. decreases
c. stays the same
d. varies
e. none of these
7. The shape of an s orbital is
a. spherical
b. dumbbell shaped
c. donut shaped
d. conical shaped
e. none of these
8. A given set of p orbitals consists of ______________ orbital(s).
a. 1
b. 2
c. 3
d. 4
e. 5
9. The maximum number of electrons allowed in each of the p orbitals is
a. 2
b. 4
c. 8
d. 18
e. none of these
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10. A given set of d orbitals consists of ______________ orbital(s).
a. 1
b. 3
c. 5
d. 6
e. none of these
11. The maximum number of electrons allowed in each of the d orbitals is
a. 2
b. 4
c. 8
d. 18
e. 32
Electron Configurations
1. Sodium has how many electrons in its outermost principal energy level?
a. 1
b. 2
c. 6
d. 8
e. 11
2. The number of unpaired electrons in an oxygen atom is
a. 1
b. 2
c. 3
d. 4
e. 5
3. The electron configuration for the phosphorus atom is
a. 1s 22s 22p 63s 23p 3
b. 1s 22s 22p 63s 23p 64s 1
c. 1s 22s 22p 63s 5
d. 1s 22s 22p 63p 5
e. none of these
4. The electron configuration for the carbon atom is
a. 1s 22s 22p 2
b. [He] 2s 4
c. [Ne] 2s 22p 2
d. 1s 22p 4
e. none of these
5. When moving down a group (family) in the periodic table, the number of valence electrons
a. remains constant
b. increases by 2 then 8 then 18 then 32
c. doubles with each move
d. decreases regularly
e. changes in an unpredictable manner
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6. The element with the electron configuration [Kr] 5s 24d 105p 3 is
a. As
b. Sb
c. Nb
d. Pr
e. none of these
Atomic Trends
1. Which of the following atoms has the largest atomic radius?
a. Na
b. Mg
c. Si
d. P
e. C
2.Which of the following atoms has the highest ionization energy?
a. Na
b. Mg
c. Si
d. P
e. Cl
Bonding
1. When electrons are shared unequally, chemists characterize these types of bonds as ______________.
a) polar covalent
b)
c)
d)
e)
ionic
pure covalent
unbalanced
none of these
2. Chemical bonds formed by the attraction of oppositely charged ions are called
a) covalent bonds
b)
c)
d)
e)
magnetic bonds
coordinate bonds
ionic bonds
none of these
3. Which of the following compounds contains one or more covalent bonds?
a) NaCl
b) CaO
c) CO2
d) Cs2 O
e) BaBr2
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4. Which element or ion listed below has the electron configuration 1s22s22p63s23p6?
a) Cl
b) Brc) Se
d) Ca2+
e) two of these
5. A phosphorus atom needs to gain ______________ electrons to achieve a noble gas configuration.
a) 2
b) 3
c) 4
d) 5
e) 6
6. How many lone pairs of electrons are in the Lewis structure for ammonia, NH3?
a) 0
b) 1
c) 2
d) 3
e) 4
7. Choose the correct Lewis structure for the OH- ion.
a)
c)
b)
d)
8. Which of the following has a double bond?
a) H2O
b) C2H2
c) C2H4
d) CNe) none of these
9. What is the correct order of the following bonds in terms of decreasing polarity?
a) N--Cl, P--Cl, As--Cl
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
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Chemical Nomenclature
1. Which of the following is a binary compound?
a) O2
b) HCN
c) H2SO4
d) H2S
e) NaOH
2. The correct name for LiCl is
a) lithium monochloride
b) lithium(I) chloride
c) monolithium chloride
d) lithium chloride
e) monolithium monochloride
3. The correct name for P2O5 is
a) phosphorus(II) oxide
b) phosphorus(V) oxide
c) diphosphorus oxide
d) diphosphorus pentoxide
e) phosphorus pentoxide
4. The binary compound PbCl2 is called
a) Lead chloride
b) Lead (II) chloride
c) Lead (II) chlorate
d) Lead dichloride
e) none of these
5.Name the following acid: HBr
a) Hypobromous acid
b) Bromic acid
c) Hydrobromic acid
d) Bromous acid
e) none of these
6. What is the formula for the ionic compound formed between Potassium and Nitrogen?
a) KN
b) K2N
c) KN3
d) K3N
e) none of these
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