Released
Questions
Chemistry
CA Standards Test
Measure temperature
Measure heat
Measure color of light
Observation  Hypothesis  Theory  Law
(The Atomic Theory)
A well-accepted idea.
Refer to your
Periodic
Table
Chemical Families act the same.
Noble gases are
the hardest to pull an
electron off of.
Alkali metals (Li, Na, K…) are the
easiest atoms to pull an electron off of.
Family 6 has
6 valence electrons.
Most particles missed
the nucleus
A few alpha particles hit
something small and
very dense!
single-atom
Cl2
F2
He
N2
The Diatomic Elements:
HONClBrIF
or
BrINClHOF
The examples contain C, N, H, & O
nonmetals with nonmetals
Use your Periodic Table
Same family as Silicon
Volume decreases x2
Pressure increases x2
At STP, 1.0 mole = 22.4 L
So, half a mole = 11.2 L
The answer is STP (T=273 K & P=1.00 atm)
K -273 = ºC
423 - 273
Remember, no calculator…
The answer is NOT negative.
And
423 – 273  696!
Hint: Read the question before looking at the table of information…
These mix very well
so you can dissolve
alcohol in water or
water in alcohol!
“Like Dissolves Like”
Polar solutes dissolve in
polar solvents.
Nonpolar solutes
dissolve in nonpolar
solvents.
Polar and nonpolar do
not mix (e.g. oil & H2O).
A Proportion!
If 36.2 g dissolves in 100 g of H2O,
How much dissolves in 50 g of H2O?
? moles
2.0 M 
5 Liters
Hint: If the math confuses you, try each answer until you find the right one.
ppm is related to %
solute
%
 100
solvent
solute
ppm 
 1,000,000
solvent
332 g

 1,000,000 
1,000
From the formula sheet:
Heat = mass x (change in Temp) x specific heat
= 30 g (40.0ºC) (0.4 J/g ºC)
= 30 (4)(4) J
= 120 x 4 = 480 J
HCl + NaOH  H2O + NaCl (salt water)
Salt water is neutral!
Our’s looked more like this:
Which answer is NOT
an electrolyte?
Nope… bases are slippery.
Nope… acids + bases form salts.
Nope… they become less acidic… they get neutralized!
Acidic = Low pH
Basic = High pH
Le Châtelier's Principle
Reactants

Products
21
Increase pressure =
decrease in volume
Not enough room… switch to
the side that takes up less room
(fewer moles of gas)
Add heat… shift left
Add liquid… no change
Shift left… make O2
Fewer moles of gas on the right. 5  2
Shift right… use up CO
No change… 2  2
Shift left: use up NO
Shift right… make CO2
H2O(l)  H2O(g)
4
CH3CH2OH is C2H6O
C2H6O + 3O2  2CO2 + 3H2O
Molar mass of carbon-12:
12.00 g/mole
grams
6 grams
moles 

 0.5 moles
molar mass 12 g/mole
Or… 12 grams = 1 mole so… 6 grams = .5 moles
Look up Pt on the Periodic Table
Approximate:
195 g = 1 mole… so 97.6 g = .5 mole
1 mole = 6.02 x 1023 atoms… so .5 mole =
3.01 x 1023 atoms!
Translate:
6.02 x 1023 = 1 mole
1.2 x 1024 = 2 moles
1 mole CO2 and 2 moles H2O are formed.
Use P.O.E.
Process
Of
Elimination
Molar Mass of CH4
12.0 + 4.0 = 16.0 g/mole
grams
96 grams
moles 

 6 moles
molar mass 16 g/mole
Hint: Again… if the math is too much… try each answer out.
52 g Cr = 6.02 x 1023 atoms
13 g Cr = ¼ x 6.02 x 1023 atoms
= 1.5 x 1023 atoms
1 Fe2O3 = 2(55.85) + 3(16.00) = 112 + 48 = 160 grams
3 CO = 3(12.0 + 16.0) = 3(28) = 84 grams
So… 160 grams Fe2O3 is needed
to react with 84 grams of CO!
6(2+16) = 6(18) = 60 + 48 = 108 grams
2(14+3) = 2(17) = 34 grams
108 g H2O  34 g NH3
so…
54 g H2O  17 g NH3
Hint: The numbers have to be simple because you won’t have a calculator.