Gen Chemistry 09-10
Semester 1 Final Exam Study Guide
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Final Exam Schedule
Find your class period and time. DO NOT be late. You will not be compensated for time you are late
and your name will be turned into the office. There is NO excuse to miss the final exam.
Monday, Dec. 21
8:10-9:40
9:50-11:20
11:20-12:15
12:20-1:50
2:00-3:30
Period 1
Period 2
Lunch
Period 5
Period 6
Tuesday, Dec. 22
8:10-9:40
9:50-11:20
11:20-12:15
12:20-1:50
2:00-3:30
Period 3
Period 4
Lunch
Period 7
Period 8 Make ups
1
Classify the following as either a hypothesis or observation.
1) A blue flame will heat water faster than an orange flame.
2) The skittle is red.
3) Adding fertilizer to water will help the tree grow better than just using water alone.
4) The reaction gave off gas.
5) The color of the liquid is bright blue.
Convert the following values to the given unit.
6) 76.3 kg = ___________ g
7) 579 L = ____________ mL
8) 1289.6 km = ________ m
9) 43 m = ____________ mm
10) 38.4321 HL= _______ L
11) How do you determine the density of an object from a volume and mass?
12) How do you determine the volume of an object from a density and mass?
13) How do you determine the mass of an object from a volume and density?
14) Define compound.
15) Define element
16) Define heterogeneous mixture
17) Define homogeneous mixture.
Classify the following as one of the above choices from 14-17.
18) Potassium sulfide, K2S
19) Fruit salad
20) Gasoline
21) Oxygen
22) Sand mixed with iron filings
2
23) For each of the following scientists, explain the information they discovered, and why they are
important.
Scientist
John Dalton
Information they discovered
Why are they important?
JJ Thomson
Ernst Rutherford
Neils Bohr
Erwin
Schroedinger
24) What are valence electrons and why are they so important?
25)
Location
Proton
Neutron
Electron
Charge
Mass
26) Draw the lewis dot structure for the each of the following elements:
a. Helium
d. Sulfur
b. Sodium
e. carbon
3
27) Directions: Label the following on the Periodic Table Below
Metals
Non-Metals
Rare Earth Metals
Halogens
Alkaline Earth Metals
Noble Gases
Transition Metals
Metalloids
Alkali Metals
Most reactive metal
Group with 5 valence electrons
Charges on group A elements
4
Gen Chem 09-10
Sem 1 Review
27) What is an ion?
28) What is an isotope?
29) What is a group on the periodic table?
30) A period?
31) For each of the following trends, you must be able to explain what happens as you move
down a group, across a period, and why.
Atomic
Radius
As you
move down
a group
Why?
As you move
across a
period
Why?
Ionization
Energy
Atomic
Mass
ReactivityNonmetals
ReactivityMetals
32)An ionic bond is formed when…
A
A metal and a nonmetal share electrons.
B
A metal takes the electrons away from a nonmetal.
C
Two nonmetals share electrons.
D
A nonmetal takes electron away from a metal.
5
Gen Chem 09-10
Sem 1 Review
33) A covalent bond is formed when…
A
Two nonmetals share electrons
B
A metal and a nonmetal share electrons.
C
A metal takes the electrons away from a nonmetal.
D
A nonmetal takes electrons away from a metal.
34) A polyatomic ion is when…
A
The same as a covalent compound.
B
An element with a charge.
C
When two or more atoms are neutral.
D
When two or more bonded elements have a collective charge.
35) Use these choices to answer the following questions. Each choice can be used more than
once. Each question has only one answer.
A
B
C
Acid
Ionic
Covalent
a) CCl4
b) Hg(OH)2
c) Rb2SO3
d) Radon Difluoride
e) Carbonic Acid
f) Tungsten (I) Sulfite
g) HNO3
h) Cobalt (IV) Arsenate
6
Gen Chem 09-10
Sem 1 Review
IONIC COMPOUND NOMENCLATURE
Define binary compound and describe
how to name them.
Ex) sodium chloride, Lithium bromide,
Magnesium bromide, Calcium
chloride
Describe how to name a compound
containing a polyatomic ion.
Describe how to write the formula for a
binary ionic compound.
Ex) NaCl, LiBr, MgBr2, CaCl2
Transition elements can have more than
one charge. How do you name ionic
compounds that contain transition
elements?
Ex) Potassium cyanide, Sodium
Ex) Iron (III) bicarbonate, Iron (II)
hydroxide, Sodium nitrate, Ammonium chloride, Manganese (IV) oxide
chloride, Calcium phosphate
Describe how to write the formula of an
ionic compound containing polyatomic
ions.
Ex) KCN, NaOH, NaNO3, NH4Cl,
Ca3(PO4)2
How do you write the formula for ionic
compounds that contain transition
elements?
Ex) Fe(HCO3)3, FeCl2, MnO2
7
Gen Chem 09-10
Sem 1 Review
COVALENT COMPOUND NOMENCLATURE
Complete the following graphic organizer by filling in each square with information that best explains the statement in each box.
What are physical and chemical properties of covalent
compounds?
Define diatomic molecule, list the names of all 7, and list their
formula
When naming covalent compounds, what rules should you
follow?
Ex) Nitrogen dioxide
Dinitrogen monoxide
When writing the formula for covalent compounds, what rules
should you follow?
Ex) NO2
N2O
8
Gen Chem 09-10
Sem 1 Review
Given the name, identify each of the following as Ionic (I), covalent (C), or acid (A). Then, write
the formula.
_____ 35. sulfuric acid
__________________________________________
_____ 36. sodium hydroxide
__________________________________________
_____ 37. sodium bromide
__________________________________________
_____ 38. barium hydroxide
__________________________________________
_____ 39. manganese (IV) oxide
__________________________________________
_____ 40. sulfur dioxide
__________________________________________
_____ 41. iron (II) sulfide
__________________________________________
_____ 42. hydrochloric acid
__________________________________________
_____ 43. potassium permanganate__________________________________________
_____ 44. sulfur trioxide
__________________________________________
_____ 46 copper (II) hydroxide
__________________________________________
_____ 47. ammonium sulfide
__________________________________________
_____ 48. nickel (II) bromide
__________________________________________
_____ 49. iron (II) oxide
__________________________________________
_____ 50. acetic acid
__________________________________________
Given the formula, identify each of the following as Ionic (I), covalent (C), or acid (A). Then,
write the name.
_____ 51. CaCO3
________________________________________________
_____ 52. FeO
________________________________________________
_____ 53. H2CO3
________________________________________________
_____ 54. AgCl
________________________________________________
_____ 55. N2O
________________________________________________
_____ 56. Ba(OH)2
________________________________________________
_____ 57. Na2S
________________________________________________
9
Gen Chem 09-10
Sem 1 Review
_____ 58. KrCl2
________________________________________________
_____ 59. H3PO4
________________________________________________
_____ 60. (NH4)2SO4
________________________________________________
_____ 61. HC2H3O2
________________________________________________
_____ 62. Zn(NO2)2
________________________________________________
_____ 63. CuSO4
________________________________________________
_____ 64. XeF4
________________________________________________
_____ 65. NaOH
________________________________________________
The Mole
66) How big is a mole? It’s the same as Avogadro’s number.
67) How do you convert from molecules to moles?
68) How do you convert from atoms to moles?
69) How do you convert from atoms or molecules to grams?
Draw one graphic organizer than summarizes how to convert from particles to moles and from
moles to grams.
70) How many moles are in 3.54x1024 atoms of Cu?
71) How many molecules are in 8.7 moles of Ne?
10
Gen Chem 09-10
Sem 1 Review
72) How many moles of S8 are in 12.3x1025 molecules of S8?
73) How many moles are there in 150 grams of Al(OH)3?
74) How many moles are there in 68 grams of CuSO4?
75) How many grams are there in 4.4 moles of Fe2(SO4)3?
76) A 200 mg tablet of vitamin C is how many ounces? (this is the recommended daily
allowance of vitamin C)
77) A car traveling 70 mph has a speed of how many meters per second?
78) Find the mass in grains of a .800 g aspirin tablet. (Given: 1000 milligrams = 15.4 grains).
11
Gen Chem 09-10
Sem 1 Review
79) For the ice cream lab we need to use cream. Find the number of cups of cream in 2.5
gallons. (Given: 1 pint= 2 cups).
90) Calculate the number of hours in 29 years, 1 month, and 4 days. (The number of hours I will
be old on your first day of holiday break)
82) Use the graph to answer the next questions.
D
E
C
B
A
Which letter(s) represent a phase change?
Which letter(s) represent states of matter?
Which letter(s) represent a change in kinetic energy?
Which letter(s) represent a change in potential energy?
When are the molecules changing speed?
12
Gen Chem 09-10
Sem 1 Review
83) Define the following words:
a. Group (on the periodic table)
f. Atomic radius
b. Period (on the periodic table)
g. atom
c. Ionization Energy
h. Atomic number
d. Reactivity
i. Periodic
e. Malleable
Note: The following will be given to you on the final exam, but on a separate sheet.
Conversion Factors
1 in = 2.540 cm
1 m =1.0936 yd
5280 ft = 1 mi
1 mi = 1.6093 km
3 ft = 1 yd
12 in = 1 ft
1 lb = 454 g
16 oz = 1 lb
1 kg = 2.205 lb
1 calorie = 4.184 Joule
1.0567 qt = 1 L
1 fluid oz = 30 ml
2 cups = 1 pint
2 pint = 1 qt
4 qt = 1 gal
1 gal = 3.7854 L
1 gal = 3785 cm3
1 tsp = 5 ml
3 tsp = 1 Tbs
m = meter
mi = mile
ft = feet
in = inch
yd = yard
lb = pound
oz = ounce
L = liter
qt = quart
tsp = teaspoon
gal = gallon
Tbs = tablespoon
kilo – hecto – deka – BASE – deci – centi - milli
MASS
PARTICLES
Molar
Mass
Avogadro’s
Number
MOLES
Molar
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