Physical Science Goal 2 Study Guide (Chemistry)
1. Classifying matter:
a. Homogeneous or heterogeneous (based on uniformity)
i. Kool-aid HO
ii. Italian salad dressing HE
iii. Coffee HO
b. Pure substance or mixture (based on the number of elements or compounds in the
sample)
i. Salt water MX
ii. Oxygen PS
iii. Water PS
c. Metal, nonmetal, or metalloid (based on its location on the periodic table)
i. Sulfur NM
ii. Silicon MT iii. Aluminum M
iv. Sodium M
v. Chlorine NM
d. Element or compound (using its chemical formula)
i. C Ele
ii. CO2 Com iii. CO Com iv. Co Ele
v. O
Ele
2. Fill in the table:
Property
Particle size
Settles out
Tyndall effect
Solution
Small
No
No
Colloid
Medium
No
Yes
Suspension
Large
Yes
Yes
3. Define the following phase changes: melting, vaporization, condensation, freezing.
a. Melting- solid to liquid
b. Vaporization- liquid to a gas
c. Condensation- gas to a liquid
d. Freezing- liquid to a solid
4. Solid, Liquids, and Gases- If heat is added, particles move (faster/slower) and kinetic energy
(increases/decreases). If heat is removed, particles move (faster/slower) and kinetic energy
(increases/decreases)
5. Solid/Liquid Equilibrium- If heat is added, (melting/freezing) occurs as the particles move (farther
apart/closer together) and the attraction between the particles (increases/decreases). If heat is
removed, (melting/freezing) occurs as the particles move (farther apart/closer together) and the
attraction between the particles (increases/decreases).
6. Liquid/Gas Equilibrium- If heat is added, (vaporization/condensation) occurs as the particles move
(farther apart/closer together) and the attraction between the particles (increases/decreases). If
heat is removed, (vaporization/condensation) occurs as the particles move (farther apart/closer
together) and the attraction between the particles (increases/decreases).
7. During a phase change the temperature (increases/decrease/remains constant)
Volume
Shape
Compressibility
Space between
molecules
Energy of molecules
Attraction between
molecules
Solid
Liquid
Definite
Definite
Definite
Shape of the container
Shape of the container
No
No
Yes
Closest
Close
Far apart
Lowest
Strongest
Higher than solid lower
than gas
Lower than solid higher
than gas
Gas
Volume of the
container
Highest
Weakest
8. How are evaporation and vaporization different?
a. Evaporation occurs below the boiling point.
b. Vaporization occurs at the boiling point.
9. Solutions:
a. Solute- the substance that is dissolved in the solvent.
b. Solvent- the substance that dissolves the solute.
c. “Likes dissolve Likes”
i. (Polar/Nonpolar) solvents dissolve polar and ionic solutes.
ii. (Polar/Nonpolar) solvents dissolve nonpolar solutes.
iii. Nonpolar solutes are (soluble/insoluble) in polar solvents.
10. Practice: Solubility Curve
a. What is the solubility of KClat 5C? 28 g
b. What is the solubility of KClat 25C? 35 g
c. What is the solubility of Ce2(SO4)3at 10C? 15 g
d. What is the solubility of Ce2(SO4)3 at 50C? 5 g
e. At 90C, you dissolved 10 g of KCl in 100. g of water. Is
this solution saturated or unsaturated? How do you know?
Unsaturated; below the line about 53 g of KCl can be
dissolved at 90 degrees C.
f. A mass of 100 g of NaNO3 is dissolved in 100 g of water
at 80ºC. Is the solution saturated or unsaturated?
unsaturated
g. As the solution is cooled, at what temperature should
solid first appear in the solution? Explain. 35 degrees C.
The solubility of NaNO3 at 35 degree C is 100 g after that
point excess solute will settle out of solution.
h. Which compound is most soluble at 20 ºC? KI
i. Which is the least soluble at 40 ºC? Ce2(SO4)3
j. Which substance on the graph is least soluble at 10C?
KClO3
11. Practice: Density Problems
a. 100 grams of a liquid completely fill a 200 mL bottle. What is the density of the liquid?
0.5 g/mL
b. A solution has a density of 1.50 g/mL. How many grams are needed to obtain 10.0 mL of
solution? 15 g
c. If a block of copper measures 2.00 cm x 4.00 cm x 5.00 cm and weighs 356 grams, what is
its density?
8.9 g/cm3
d. The density of mercury is 13.6 g/mL.
i. What is the mass of 8.20 mL of mercury? 111.5 g
ii. What volume would 120 grams of mercury occupy?
8.82 mL
12. Properties of Matter:
Property
Melting Point
Boiling Point
Density
Appearance
Conductivity
Metals
High
High
High
Shiny
Yes
Nonmetals
Low
Low
Low
Dull
No
Brittle or Malleable
Malleable and ductile
brittle
13. Fill in the table:
Protons
+1
1 amu
Nucleus
Neutrons
0
1 amu
Nucleus
Electrons
-1
1/2000 amu
Electron cloud
Charge
Relative Mass (amu)
Location
14. Atomic math:
a. protons = atomic number
b. electrons = # protons – charge
c. neutrons = mass number - # protons
d. mass number = # neutrons + # protons
e. Atomic number = number found on the periodic table (or # protons)
f. Charge = # of protons - # electrons
15. Use isotopic notation to write symbols for various isotopes.
𝟑𝟕
𝟑𝟓 1Chlorine-35
𝟏𝟕𝑪𝒍
𝟏𝟕𝑪𝒍
Mass Number
35
37
35
Atomic Number
17
17
17
Protons
17
17
17
Neutrons
18
20
18
Electrons
17
17
18
16. Draw Bohr models from hydrogen to argon including common isotopes and ions. (in class)
a. Carbon-14 atom
b. Chloride ion (-1)
c. Sodium atom
17. Construct dot diagrams, a shorthand notation for Bohr models, using the element symbol and
dots to represent electrons in the outermost energy level. (in class)
a. Sulfur
b. Lithium
c. Aluminum
18. Fill in the following table:
1A
Valence
1
electrons
Oxidation +1
number
Gain/lose Lose 1
electons
2A
2
3A
3
4A
4
5A
5
6A
6
7A
7
8A
8
+2
+3
+/- 4
-3
-2
-1
0
Lose 2
Lose 3
Lose/gain Gain 3
4
Gain 2
Gain 1
Already
stable
19. As you go down a group of metals the reactivity increases, and as you go down a group of nonmetals
the reactivity decreases.
20. Fill in the table
What happens to the
electrons?
What types of
elements are involved?
Ionic
Transferred
Covalent
Shared
Metallic
Sea of electrons
Metal and a nonmetal
Two nonmetals
two metals
21. Name and write formulas for simple binary compounds containing a metal and nonmetal using
representative elements and compounds involving common polyatomic ions: ammonium, acetate,
nitrate, hydroxide, carbonate, sulfate, phosphate.
Chemical Name
Chemical Formula
Chemical Formula
Chemical Name
Potassium oxide
K2O
Na2S
Sodium sulfide
Lithium nitride
Li3N
Na3P
Sodium phosphide
Beryllium sulfide
BeS
MgBr2
Magnesium bromide
Barium chloride
BaCl2
CaO
Calcium oxide
Beryllium fluoride
BeF2
MgS
Magnesium sulfide
Lead(IV) sulfide
PbS2
SnCl2
Tin(II) chloride
Potassium nitrate
KNO3
CaCO3
Calcium carbonate
Ammonium fluoride
NH4F
Ba(OH)2
Barium hydroxide
Aluminum phosphate
AlPO4
MgSO4
Magnesium sulfate
Potassium acetate
KC2H3O2
K2CO3
Potassium carbonate
22. Name and write formulas for binary compounds of two nonmetals using Greek prefixes.
Chemical Name
Chemical Formula
Chemical Formula
Chemical Name
Carbon monoxide
CO
CO2
Carbon dioxide
Sulfur dioxide
SO2
N2O
Dinitrogen monoxide
Carbon tetrachloride
CCl4
N2O5
Dinitrogen pentoxide
Sulfur trioxide
SO3
PBr3
Phosphorus tribromide
23. Use coefficients to balance simple chemical equations involving elements and/or binary
compounds.
a. 2H2O  2H2 +1O2
b. 1ZnS + 2O2  1ZnSO4
c. 2Mg + 1O2  2MgO
d. 2Na + 2H2O  ___H2 + 2NaOH
e. ___Li2CO3 + 2HF  2LiF + ___H2CO3
f. 2NH3  1N2 + 3H2
g. 2Al + 3H2SO4 ___Al2(SO4)3 +3H2
h. ___NaOH + ___HCl ___NaCl + ___H2O
24. Classify the above chemical reactions in question 27 as one of the four types.
a. Decomposition
b. Synthesis
c. Synthesis
d. Single replacement
e. Double replacement
f. Decomposition
g. Single replacement
h. Double replacement
25. Fill in the table:
Identifying ion (H+ or OH-)
pH range
Taste
Feel
Litmus paper test
Phenolphthalein test
Reacts with metals
Reacts with carbonates
Reacts with fats/oils
Conductivity
Acids
H+
0-7
Sour
Sticky
Red
Clear, colorless
Produces hydrogen gas
Yes (produces carbon dioxide)
No
Yes
Bases
OH7-14
Bitter
Slippery
Blue
Pink
No
No
Produces soap
Yes
26. When an acid reacts with a base, the two products will be a salt and water. This is called a
neutralization reaction.
27. Fill in the table:
Symbol
Composition
Mass
Penetrability
Change in the mass
number
Change in the atomic
number
Alpha
4
2𝐻𝑒 or α
2 protons
2 neutrons
4 amu
Paper
Decreases by 4
Beta
0
−1𝑒 or β
1 electron
Gamma
Γ
Energy
1/2000 amu
Wood
No change
no mass
Lead or concrete
No change
Decreases by 2
Increases by 1
No change
28. Fill in the table:
Splitting or joining
Required conditions
Energy released
Nature of the products
Fission
Splitting of a very large nucleus
Room temperature
A lot of energy
Radioactive
Fusion
Combining of two smaller nuclei
Temp. conditions like the Sun
A lot more energy
not radioactive
29. Half-life : the amount of time it will take half of the radioactive particles to undergo decay.
a. What is the half-life of a 100.0 g sample of nitrogen-16 that decays to 12.5 grams in 21.6
seconds? 7.2 seconds
b. All isotopes of technetium are radioactive, but they have widely varying half-lives. If an
800.0 gram sample of technetium-99 decays to 100.0 g of technetium-99 in 639,000 years,
what is its half-life? 213,000 years
c. A 208 g sample of sodium-24 decays to 13.0 g of sodium-24 within 60.0 hours. What is the
half-life of this radioactive isotope? 15 hours
d. If the half-life of iodine-131 is 8.10 days, how long will it take a 50.00 g sample to decay to
6.25 g? 24.3 days
e. The half-life of hafnium-156 is 0.025 seconds. How long will it take a 560 g sample to
decay to one-fourth of its original mass? 0.050 seconds
f. Chromium-48 has a short half-life of 21.6 hours. How long will it take 360.00 g of
chromium-48 to decay to 11.25 g? 108 hours
g. Potassium-42 has a half-life of 12.4 hours. How much of an 848 g sample of potassium-42
will be left after 62.0 hours? 26.5 g