Name_______________________________________________________ Date ___________________ Period ________
Midterm Review
Academic Chemistry 2015
This packet is a general overview of the main topics covered in the first semester of Academic Chemistry. All of the
class material is NOT included and students are strongly encouraged to study notes and review previous assignments.
READING EQUIPMENT
1.
The diagram below represents a portion of a buret. What is
the reading of the meniscus to the correct number of
significant figures?
2.
A student has to measure the volume of a liquid in a
graduated cylinder. Based on the diagram below, what is
the volume to the correct number of significant figures?
__________ mL
__________ mL
MEASUREMENT
3. Convert the following numbers to scientific notation:
a.
4.
6.
c. ________________ 0.000809
_______________ 7.63 x 10-4
b. ________________ 9.8 x 105
c. _______________ 5.41 x 103
How many significant figures are in the following?
a.
_______103900.0
c. ________0.0010430
e. _______190300
b.
_______0.0034
d. ________5.370 x 104
f. ________6.626 x 10-34
Round the following to the number of significant figures indicated in parenthesis.
a.
7.
b. ________________ 301
Expand the following to standard notation:
a.
5.
________________ 9067.4
______________2.0896 x 108 (4)
b. ______________45063004 (3)
c. ______________ 0.03046 (2)
Perform the following math functions. Record the answer to the correct number of significant figures.
a.
(130.0 g – 125.0 g)/130.0 g =
___________________________
b.
9.5 mm + 17.286 mm – 1.4445 mm =
___________________________
c.
2.34 cm x 5.78 cm x 8.42 cm =
___________________________
Solve the following density and % error problems. Show all work, including appropriate equations, and correct substitution of values
into the equations with units. Round your answers to the correct number of significant figures and make sure the answer has a unit.
8.
In a lab, you reacted a piece of aluminum foil with copper (II) sulfate to produce solid copper. At the end of the experiment, you
measured 17.6 g of copper. You should have been able to recover 20.0 g of copper. What is your % error?
9.
An irregularly shaped piece of iron with a mass of 47.5 grams was placed into a graduated cylinder that initially contained 50.0
mL of water. The final volume in the graduated cylinder is 62.0 mL. Calculate the density of the iron.
10. A solid has a density of 1.25 g/mL and a volume of 20.0 mL. Calculate the mass of the solid.
Solve the following metric and American conversion problems using dimensional analysis. Show all work with units and round your
answers to the correct number of significant figures. Report your answers in scientific notation. (You can find all of the conversion
factors needed for this section in your notes)
11. Convert 125 cm to km.
12. Convert 78.5 cm to µm.
13. Convert 0.7891 L to nL.
14. Convert 16.2 ft to mi.
15. Convert 5.44 qt to mL.
16. Convert 53.00 m/s to km/hr.
17. Convert 44.0 L/s to gal/min
MATTER
1.
Define the following terms: Matter, Pure substance, Mixture, Element, Compound, Homogeneous Mixture, and
Heterogeneous Mixture.
2.
Classify each of the materials below.
Material
Water vapor
Lead pipe
Soda
Pure Substance or
Mixture
Pure Substance
Element
Compound
Mixture
Homogeneous
Heterogeneous
Pure Substance
Pure Substance or
Mixture
Material
Element
Compound
Mixture
Homogeneous
Heterogeneous
Aqueous solution of
copper (II) sulfate
Carbon dioxide (CO2)
Chocolate chip cookie
Magnesium ribbon
Bronze
(copper and tin)
Ozone (O3)
Potassium Nitrate
(KNO3)
Liquid Mercury (Hg)
3.
Label the following pictures as: element, compound, mixture of two elements or mixture of two compounds.
A.
4.
B.
C.
D.
Place an X in each box that describes the property.
Chemical
Property
Bromine is a reddish-brown liquid
The combustibility of oxygen gas
A 3.5 g sample of magnesium
The density of water is 1.00 g/mL
Iron metal is able to conduct electricity
H2 gas reacts vigorously with O2 to form H2O
The tendency of ethyl alcohol to burn
Aluminum is a shiny metal
The temperature at which water freezes
The volume of isopropyl alcohol is 50.0 mL
Physical
Property
INTENSIVE
Physical
Property
EXTENSIVE
5.
Put an X in the box that best describes each of the following changes of matter.
Physical
Change
Chemical
Change
Physical
Change
Cutting your hair
Two clear liquids are mixed and a
yellow color forms
Mixing sugar and water
Baking cookies
Making a peanut, pretzel and cereal
mixture
Diamonds are used to scratch glass
Baking soda reacting with vinegar to
produce H2 gas
A tree burns to form ashes
A piece of metal is bent in half
A piece of paper is crumpled up
Methanol is burned and leaves a
residue
Water freezes to form ice
An aspirin is crushed into a powder
A piece of metal corrodes
Copper turns green when exposed to
the environment
A banana rots
6.
Chemical
Change
The graph below represents changes of state for an unknown substance. What is the boiling point of the substance? What is
the melting point of the substance? What phase change occurs from t2 to t1 and from t3 to t4?
ATOMIC STRUCTURE AND NUCLEAR CHEMISTRY
1.
Know the scientists (Rutherford, Thomson, Bohr, Dalton, Millikan) and their discoveries.
2.
Fill in the missing information in the table below. All atoms below are electrically neutral.
Element
Symbol
Hyphen Notation
Nuclear
Symbol
Protons (p+)
Neutrons (n0)
Electrons
(e-)
25
53
12
35
As
Mass
Number (A)
11
45
75
227
89
Ac
Atomic
Number (Z)
3.
Decide if the following are isotopes (yes or no)
_____ b) Nitrogen – 14
Carbon – 14
_____ a) 39 protons and 50 neutrons
39 protons and 61 neutrons
_____ c) 199F and
18
9F
4.
Naturally occurring element X exists in three isotopic forms: X-159 (159.37 amu, 30.60% abundance), X-163 (162.79 amu,
15.79% abundance) and X-164 (163.92 amu, 53.61% abundance). Calculate the average atomic mass.
5.
Naturally occurring oxygen is 99.76% oxygen-16, 0.037% oxygen -17 and 0.204% oxygen-18. Calculate the average atomic mass
of oxygen.
6.
What is the trend for atomic radius (size of an atom) across a period? ________________________________________________
7.
What is the trend for atomic radius (size of an atom) down a group? _________________________________________________
8.
Which is the largest atom in group 2?
9.
Which is the smallest atom in period 3? __________
__________
The smallest?
__________
The largest?
__________
10. Does Sr or Al have a smaller atomic radius? Why? Explain in terms of nuclear charge, shielding and/or energy levels.
11. Put the following elements in order of increasing atomic radius: Ag, S, Si, Sr, Cu, Ra
____________________________
12. How does the size of an aluminum atom change when it becomes an ion with a charge of 3+?
a. It becomes smaller by losing 3 electrons
c. It becomes larger by losing 3 electrons
b. It becomes smaller by gaining 3 electrons
d. It becomes larger by gaining 3 electrons
13. How does the size of an chlorine atom change when it becomes an ion with a charge of 1-?
a. It becomes smaller by losing 1 electron
c. It becomes larger by losing 1 electron
b. It becomes smaller by gaining 1 electron
d. It becomes larger by gaining 1 electron
14. Balance the following nuclear equations.
1H


4
a.
3
b.
198
c.
_____ 
d.
239
e.
3
f.
14
g.
9
1H
2
+
86Rn
94Pu
1H
+
6C

4Be
+
4
2He
2He
0
-1e
+
+ _____
+ _____
237
93Np
+ _____ 
2
1H
241
95Am
 _____ +
14
7N
4
2He
+
1
1H
+
1
0n
1
0n
+ _____

12
6C
+ _____
15. Write a balanced nuclear equation for each of the following nuclear processes.
a.
Thorium-232 is bombarded by an alpha particle.
b.
Bismuth-209 absorbs a neutron and releases a beta particle.
6.
The first 4 steps in the decay series of thorium-232 is α, β, β, α. Write a balanced equation for each step in this decay series.
Step 1: __________________________________________________
Step 2: __________________________________________________
Step 3: __________________________________________________
Step 4: __________________________________________________
LIGHT AND ELECTRON CONFIGURATIONS
1.
Know the rules for electron configuration (Hund’s Rule, Pauli Exclusion Principle and Aufbau Principle).
2.
Write the complete electron configuration for the potassium atom.
3.
Write the complete electron configuration for the antimony atom.
4.
Write the complete electron configuration for the magnesium ION.
5.
Write the complete electron configuration for the bromide ION.
6.
Write the noble gas (shorthand) electron configuration molybdenum atom.
7.
Write the noble gas (shorthand) electron configuration for the lead atom.
8.
Determine the number of valence electrons for the following electron configurations.
9.
a.
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3
____________________
b.
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1
____________________
c.
1s2 2s2 2p6 3s2 3p4
____________________
Name the elements from the ground state or excited state electron configuration shown. Circle the excited state electron
configurations.
a.
1s2 2s2 2p6 3s2 3p6 4s2 3d8 4p4
____________________
d. [Xe] 6s25d14f5____________________
b.
1s2 2s2 2p6 3s2 3p5
____________________
e. [Ar]4s23d25s1 ____________________
10. Violet light has a wavelength of 4.10 x 10-12 m. What is the frequency?
11. Green light has a frequency of 6.01 x 1014 Hz. What is the wavelength, in m?
12. Calculate the wavelength, in m, of radiation with a frequency of 8.0 x 10 14 Hz.
13. A helium laser emits light with a wavelength of 633 nm. What is the frequency of the light?
14. Calculate the energy, in Joules, of a photon of red light whose wavelength is 3.81 x 10 -3 nm.
15. Determine the energy, in Joules, of a photon whose wavelength is 4.257 x 10 -7 nm.
NOMENCLAUTRE
Write the formula for the given compound names. Must have smallest possible whole number ratio of ions for the ionic compounds.
Write the compound name, spelled correctly, for the given formulas.
Compound Name
Work
Formula
Formula
1.
Ammonium
nitrate
16. PbBr2
2.
Hydrobromic acid
17. N2O3
3.
Boron trichloride
18. P4S7
4.
Iron (III)
hypochlorite
19. CaS
5.
Calcium sulfite
20. Au3P
6.
Potassium
carbonate
21. Al2(CO3)3
7.
Dinitrogen
tetrachloride
22. Ba3(PO4)2
8.
Phosphoric acid
23. Pt(OH)4
9.
Sulfur
hexafluoride
24. Pd3(PO4)4
10. Aluminum acetate
25. N4O6
11. Copper (I)
carbonate
26. HClO3
12. Zinc chloride
27. CaCl2
13. Nickel (II)
cyanide
28. Ti(CrO4)2
14. Chlorous acid
29. P3O8
15. Chromium (VI)
sulfate
30. Mn2(SO3)3
Compound Name
CHEMICAL BONDING
1. What is ionization energy? What is the trend for ionization energy across a period and down a group?
2.
Why does strontium have a lower ionization energy than iodine? Explain in terms of nuclear charge, shielding and/or energy
levels.
3.
Place the following elements in order of decreasing ionization energy: O, Te, S, Se
4.
What is electronegativity? What is the trend for electronegativity across a period and down a group?
5.
Why does oxygen have a higher electronegativity than selenium? Explain in terms of nuclear charge, shielding and/or energy
levels.
6.
Place the following elements in order of increasing electronegativity: K, As, Zn, Br
____________________________
____________________________
7.
Match the characteristic to the type of bond it represents. Write the letter of the answer to the left of the characteristic letter.
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
k.
l.
8.
9.
most are insoluble in water
contains only metal atoms
involves the sharing of valence electrons between atoms
conducts electricity in their molten or dissolved forms
contains a “sea” of mobile (delocalized/free flowing) electrons
low melting and boiling points
brittle and breaks easily
conducts heat and electricity due to free flowing electrons
exist as whole molecules instead of ions
are ductile and malleable
most are soluble in water
formed when one or more valence electrons are transferred from one atom to another
A. Ionic Bond
B. Metallic Bond
C. Covalent Bond
Circle the correct terms to correctly complete the following sentences:
a.
Metal atoms tend to (LOSE or GAIN) electrons and form (CATIONS or ANIONS).
b.
Non-metal atoms tend to (LOSE or GAIN) electrons and form (CATIONS or ANIONS).
Draw the Lewis structure for the following IONIC COMPOUNDS:
Calcium fluoride
Formula: CaF2
Rubidium sulfide
Formula: ________
3. Cobalt (II) nitride Formula: ________
10. Draw the Lewis structure for the following COVALENT COMPOUNDS or POLYATOMIC IONS.
NO31-
Total v. e- ______
SiCl4
SO2
Total v. e- ______
COF2 (C is central)
Total v. e- ______
-
Total v. e ______
PCl3
Total v. e- ______
SF6
Total v. e- ______
XeF51+
Total v. e- ______
TeCl4
Total v. e- ______