CHEMISTRY
1. Lab Safety
Review the Lab safety procedures in your plastic sleeve
2. Lab Equipment
Review the different types of equipment used throughout the year
3. Metrics
1. Convert 200m to km: _____.2km________________
2. Convert 40mL to L: _______.04L_______________
3. What are the metric base units used for the following:
Mass_______gram_________________
Length ________meter________________
Volume _______liter________________
4. Matter
4. What is the equation for density? ____D=M/V_____________________________
5. Compare the density of helium to the density of the air? The density of helium is
less. When you fill a balloon with helium, it floats
6. Definition of matter – anything that has mass and takes up space
7. Six states of matter – solid, liquid, gas, plasma, Bose-Einstein condensate,
Fermionic condensate
8. Which of the states of matter:
have mass and volume?
all
have definite volume?
solids and liquids
have definite shape?
solids
Which state of matter has the least energy? ______condensates_______________
Which state of matter has the most energy? ___plasma______________________
9. Is light from a fire matter? Why or why not? No, although you can see it, it does
not take up any space or have any mass
10. Name these changes in state.
gas to liquid
condensation
liquid to gas
solid to gas
sublimation
liquid to solid
solid to liquid
melting
gas to solid
evaporation
freezing
deposition
5. Mixtures
11. Compare homogeneous and heterogeneous mixtures – homogenous mixtures are
combinations of 2 or more substances that are evenly spread throughout, heterogeneous
are not evenly distributed
Give 2 examples of a heterogeneous mixture salad, chocolate chip cookie
Give 2 examples of a homogeneous mixture sugar cookie, jello
12. Solution – a physical combination of two or more substances that are physically
combined
13. Solute – substance that does dissolve
14. Solvent – substance that does the dissolving
15. Supersaturated – mixture that is holding more solute than typically allowed
16. Saturated vs. Unsaturated Solution – saturated is a mixture that is completely full of
solute while unsaturated means it is not full.
17. What are 6 different ways that you can separate a mixture? Distillation, picking and
sorting, magnetism, filtration, evaporation, sifting
6. Chemical and Physical Properties and Chemical and Physical Change
18. Classify as: physical or chemical property, or physical or chemical change.
tastes like peanuts
P property
baking brownies
C change
boiling point
P property
reacting to acid
C change
melting ice
P change
rusting
C change
______
19. What are 5 signs of a chemical change? Change in smell, taste, bubbling, change in
temperature, precipitate forms, change in volume
7. Periodic Table
*Review all learned elements with their appropriate spelling and symbols.
19.
Row
Period
Column
Group
Family
Chlorine
3
3
17
VII
halogens
Lithium
2
2
1
I
alkali metals
Aluminum
3
3
13
III
Boron
P=15
20. Complete this diagram for Phosphorus.
K - L - M
2 - 8 - 5
N=16

Charge, location and mass of neutrons (0), in the nucleus, 1 amu

Charge, location and mass of electrons (-), outside nucleus (electron cloud) 0amu

Charge, location and mass of protons (+), in the nucles, 1 amu

What is the formula for neutrons? Atomic number - # of protons
What does the GROUP tell you on the periodic table? Number of valence electrons
What does the PERIOD tell you on the periodic table? Number of electrons shells
What does the COLUMN tell you on the periodic table? All have similar chemical
properties
24. Nickel:
Atomic number -
28
Atomic mass -
58.69 amu
Number of neutrons -
31
Number of protons - 28
Number of electrons -
28
Electron configuration -
2-8-16-2
Valence electrons -
2
Is the last shell full?
no
Period -
4
Family -
transition metal
Group -
none
8. Classification of Matter
25. Element is to _____atom_____________ as compound is to ____molecule_________
26. Circle the correct words:
Hydrogen peroxide (H2O2) is a/n element/compound and a/n atom/molecule
Oxygen (O2) is a/n element/compound and a/n atom/molecule
9. Conservation of Matter and Mass
Is the equation balanced?
C2H6 + O2

CO2
+ H2O
C–2
C–1
H–6
H–2
O–2
O–3
3Fe + 4H2O →
Fe3O4 +
Fe – 3
Fe – 3
H–8
H–8
O–4
O–4
no
4H2
yes
The number you put in front to balance an equation is called a
coefficient
Reactants are on the ______left_______ side of the equation
Products are on the ______right_______ side of the equation
Determine the number of elements, number of atoms, and molecular mass.
Al(SO4)3
Al 1 x
27 amu
=
27 amu
S
3 x
32 amu
=
96 amu
O 12 x
16 amu
=
192 amu
16
3
elements
16
atoms
315 amu
mass
315 amu
3Zn(NO3)2
3
elements
Zn 3 x
65 amu
=
195 amu
27
atoms
N 6
x
14 amu
=
84 amu
567
mass
O 18 x
16 amu
=
288 amu
27
GEOLOGY/ GROUNDWATER
1. Minerals
1. What two elements make up most the Earth’s crust? ____silicon___ & __oxygen____
2. List the five requirements for a substance to be considered a mineral.
__solid__________________________________________________
__naturally occurring_______________________________________
__inorganic_______________________________________________
__definite chemical composition______________________________
___crystal structure__________________________________________
3. Match the following definitions with their terms.
___f___
a mineral’s resistance to scratching
a. streak
___e___
how a mineral reflects light
b. fracture
___d___
breakage along a flat plane
c. specific gravity
___a___
powder left behind by mineral when scratched
on a porcelain plate
d. cleavage
___c___
weight relative to that of water
e. luster
___b___
jagged breakage
f. hardness
4. What is the Moh’s Scale? Describe it.
A scale from 1-10 that compares the hardness of minerals to other minerals and objects. 1
is the softest, 10 is the hardest.
5. Determine the specific gravity of a mineral sample with mass of 80 grams that
displaces 40 ml of water. Show your work and include units.
40 ml of water = 40 g of water
80 g
=
40 g
____2___NO UNITS
2. Rocks
6. Label the following diagram.
Sedimentary Rocks
heat and pressure
Igneous Rocks
Metamorphic Rocks
melt + crystallize
7. Choose the letter of the rock type described by each statement.
I - igneous
S - sedimentary
M - metamorphic
s
a. form in layers collecting over time
i
b. can be intrusive or extrusive
s
c. formed from remains of plants + animals m
d. can be foliated or non-foliated
s
e. formed from pieces of other rocks
i
f. classified as felsic or mafic
i
g. texture depends on the rate of cooling
s
h. most likely to contain fossils
s
i. form from cementation and compaction
i
j. form from molten rock
m
k. form from heat and pressure
s
l. form when minerals come out of
solution
8. Compare extrusive and intrusive igneous rocks.
Extrusive - formed quickly outside of the volcano (results in small/no crystals)
intrusive - form slowly over time from magma inside the volcano (results in larger
crystals)
9. Compare chemical, clastic, and organic sedimentary rocks.
Chemical – formed from minerals precipitating out of water
Organic – formed from once living things
Clastic – made from pieces of other rock
10. Compare dynamic and thermal metamorphism.
Dynamic – formed mostly from pressure in mountain building – foliated
Thermal – formed mostly from heat when magma contacts rock – non-foliated
3. Groundwater
11. Compare point source and non point source plumes. Point source – can identify a
specific spot where contamination started – concentration decreases with distance. Nonpoint source – widespread contamination that is equal throughout an area
12. In the parts per million lab, the red food coloring is not visible at a concentration of
1ppb. Why? the amount of food coloring left is too small to be seen with the naked eye
13. The allowable limit of a cancer causing chemical is .05 ppm. A code 3 well contains
0.01-1.5 ppm. Is the well safe? Explain. Maybe, it could be either way but you would not
want to take the risk.
14. List and describe the three types of sampling techniques.
1. scattered- random spots on a map
2. clustered – sampling done in one specific location
3. linear – testing done in a straight line
15. Define these terms.
a. aquifer – water bearing rock formation
b. aquitard -
layer underneath the surface that does not allow water to pass through
c. groundwater – water stored underground in rock and soil
d. impermeable – does not allow water to pass through
e. permeability – the ability of water to pass through a material
f. porosity -
the amount of water that can be held by a material; depends on size of
pores and the extent in which they are connected
g. parts per million – number of parts by weight of a substance per million; used to
measure contamination levels
16.
Well
Contamination
Code
1
a. Which of the well contamination codes are
considered “unsafe”? ______3 - 6_________
2
3
4
5
6
Level of
Contamination
Not detectable – 0.01
ppm
0.011 – 0.75 ppm
0.76 – 1.05 ppm
1.06ppm – 5 ppm
5ppm – 7ppm
>7ppm
MCL = 1 ppm
b. Draw the plume. Shade in the area that are unsafe. It should be color-coded. Be
sure to include a key.
c. Is this point source or non-point source pollution? How do you know?
This is a point source. The contamination occurs in ranges, with concentrations
decreasing outward from the source.