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Chemistry Final Review
Lab Stuff:
1.
Identify the following equipment. What is it used for? Could you identify it from a picture?
a.
b.
c.
d.
e.
f.
g.
2.
Beaker
Graduated cylinder
Balance
Goggles
flask
Tongs
Striker
Concepts & lab reports: Distinguish between the following. What are they used for? Define
them. Could you write an appropriate one?
a.
b.
c.
d.
e.
f.
g.
h.
precipitate
reference material (reference solution)
control
variable
purpose
hypothesis
data
conclusion
Water Unit:
1.
2.
Define the following. How could you experimentally test for each? How would you
separate the components? Give two examples of each.
a.
Solution
b.
Colloid
c.
Suspension
Do the following conversions. Show your work. Indicate the type of measurement (distance,
volume or mass)
100 km =
25 dm =
60 mL =
0.053 g =
75.8 mL =
m
cm3
kg
L
Page 1 of 10
3.
Identify the following as physical or chemical property. What is it? Define it.
a.
b.
c.
d.
e.
f.
g.
h.
density
surface tension
polar bonds
liquid at room temperature
boiling point
conductive
dissolves ionic compounds
breaks down into H2 (g) and O2
(g)
4.
Draw and label a picture of a water molecule. Explain it in terms of being polar. Show Hbonds between different water molecules.
5.
Why does table salt (NaCl) dissolve in water but not cooking oil?
6.
Define the following: solute, solvent and solution
Page 2 of 10
Use the following two figures to answer questions 7 – 12 and your text for the oxygen solubility curve
7. What mass of KNO3 will dissolve in 100 g of
water at 50°C?
8. What mass of KCl will dissolve in 100 g water
at this temperature?
9. a. 25 g of KNO3 is dissolved in 100 g of
water at 30°C. Is this solution saturated,
unsaturated or supersaturated?
9b.
In order to make this solution saturated,
how much more KNO3 must be added?
10.
What is the minimum mass of water to
dissolve 30 g KNO3 at 30°C?
11.
What mass of oxygen can be dissolved in
1000 g of water at 30°C?,
20°C?
12.
What mass of oxygen can be dissolved in 100 g of water at 20 °C?
13.
Fill in the following table indicating if the substance would be soluble or insoluble?
Polar Solute
Non-polar Solute
Ionic solute
Polar Solvent
Non Polar Solvent
14.
Identify each as an acid, base or neutral substance. If it is neutral indicate the kind of
substance it is. Indicate the pH of the solution formed from this substance.
a.
c.
NaBr
HBr
b.
d.
NaOH
HNO3
Page 3 of 10
15.
Identify products, reactants, elements, symbols, coefficients, subscripts and compounds in
the following equations:
a.
Ca (s) + 2 H2O (l)
Ca(OH)2 (aq) + H2 (g)
b.
6 H2O + 4 NO
4 NH3 + 5 O2
16.
Balance the equation:
AgNO3
+
BaCl2
Ba(NO3)2
+
AgCl
17.
An element is found that is a good conductor of electricity, is ductile, brittle and doesn’t react
with an acid. Classify this element. Indicate what it is as well as what it is not.
18.
The current periodic table is arranged according to increasing
19.
Elements in the same vertical column are in the same ____________ or ___________ and
.
have similar physical and chemical properties due to similar
20.
21.
.
Define and give examples of:
a.
element
b.
ion
c.
compound
Fill in the following table:
Name
Symbol
Atomic
Number
#
protons
#
neutrons
Electron configuration
Atomic Mass
(units =
)
Hydrogen
Cu
7
197
Page 4 of 10
22.
Percent Composition – calculate the percent copper in Copper (II) sulfate. Write the formula
first.
23.
Assigning Oxidation Numbers – K, Ba, Al, Cs, S, Li, Br, and assign which element will be
the positive or negative within a compound (electronegativity).
24.
Redox Reactions – given an equation, can you answer… who is oxidized? Reduced?
Oxidizing agent? Reducing agent? Number of electrons transferred?
25.
How many total electrons are in Li +1?
26.
Which has a full octet? Na, Xe, F, Na+1
27.
Draw the electron dot structure of the following:
a.
C2H6
b.
C2H4
S-2?
c.
MgCl2
28.
Draw two isomers of C6H14
29.
Draw and name an alkane, alkene and alkyne with two carbons.
30.
The molar heat of combustion of C6H14 is 4141 kJ per mole. How much heat is generated in
25 moles are burned?
31.
The specific heat of water is 4.2 J/g°C. How many joules are released if 10 g of water are
heated from 25 °C to 37 °C?
Page 5 of 10
32.
Which of the following:
a.
b.
c.
CH4
C3H8
C12H26
has the highest boiling point
is the most viscous (define viscous too)
has the greatest intermolecular forces (define IMF too)
33.
How could CH4 and C12H26 be separated?
34.
Finish the equation. Idenitify the type of reaction and the structures involved:
C5H11OH + H2CCOOH
35.
Our bodies burn sugar forming water and carbon dioxide as follows:
C6H12O6 + 6 O2
36.
6 H2O + 6 CO2
a.
If your body needs 20 moles of O2 and you eat 45 moles of sugar, which is the
limiting reactant?
b.
How much water is produced?
Which food type provides
a.
b.
c.
structure
energy
the most calories per gram
37.
Name four factors which affect the reaction rate and explain each.
38.
Relate amino acids to proteins.
Page 6 of 10
39.
Classify the following endothermic or exothermic? Label the activation energy.
40.
Referring to alpha, beta and gamma rays…
a.
b.
c.
d.
which are the most penetrating?
which are particles?
write the symbol for each.
what can stop each of these?
41.
What did Rutherford’s Gold foil experiment prove? How?
42.
A radioisotope has a half life of 5 minutes. If you have 400 g, how much is left in 30
minutes?
43.
Describe and important role of the world’s ozone layer.
44.
Explain the role of CFC’s in ozone depletion. Use equations.
45.
How many moles in 18.6 L of CO gas?
46.
Compare weak versus strong acids or bases.
Page 7 of 10
47.
Given the following elements:
a.
b.
c.
Na Mg Li K
Which element is in the fourth energy level?
Which are in the same family/group?
Which are in the same period?
48.
How many valence electrons does S have?
Ca?
Rb?
49.
Which is saturated? C2H4
50.
What is the difference between exothermic and endothermic reactions?
51.
What does the atomic number stand for?
52.
Will suspensions exhibit the Tyndall effect? Can solid materials be filtered from them?
53.
How does benzene differ from other cyclic hydrocarbons?
54.
Is the following reaction endothermic or exothermic?
C2H6
N2 + 3 H2
2 NH3 + Energy
55.
What is the molar mass of BaSO4?
56.
What are the differences between alcohols, ethers, esters and carboxylic acids?
57.
What is hard water?
58.
What is heat capacity?
Page 8 of 10
59.
35 g of ethanol is dissolved in 115 g of water. What is the concentration of ethanol in water?
In solution?
60.
If you have 30 moles of NaOH, how many molecules do you have?
61.
What are the seven diatomic elements? How can you remember them?
62.
What types of substances are removed from mixtures using filtration? Adsorption?
Distillation?
63.
Describe the path of a single water molecule through the hydrologic cycle.
64.
Write the formulas for the compounds formed between the element or ion pairs listed below:
a.
b.
c.
d.
65.
magnesium and sulfur
barium and iodine
aluminum and carbonate ion
ammonium and phosphate ions
Balance the following equations:
H2O + NO
AgNO3 + AlCl3
66.
NH3
+ O2
Al(NO3)3
+ AgCl
Estimate the boiling point of krypton if the bp of Ar is -186 °C and that of Xe is -112 °C.
Page 9 of 10
67.
A flask contains 3.5 moles of sugar C12H22O11. How many molecules found in the flask?
How many grams are in the flask?
68.
Predict whether the following reactions will occur:
CuCl2 + Al
NaNO3 + Zn
69.
Which of the following is a Redox reaction? In each Redox reaction, identify the substance
that is oxidized, the substance that is reduced, the oxidizing agent, the reducing agent.
2 NaNO3 + BaI2
Ba(NO3)2 + 2 NaI
ZN + 2 AgNO3
Zn(NO3)2 + 2 Ag
70.
Calculate the density of an object that has a mass of 38.45 g and occupies 24.7 mL.
71.
What does it mean to soften hard water?
Page 10 of 10