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Chemistry Name: Period:

Chemistry Semester 1 Final Exam Review Packet

1. What is the difference between a hypothesis and a theory?

2. Distinguish between quantitative and qualitative observations.

States of Matter 1. Diagram and describe the particles in a GAS:

2. Diagram and describe the particles in a LIQUID:

3. Diagram and describe the particles in a SOLID:

4. Which state of matter has the greatest amount of energy?

5. List the parts of the kinetic molecular theory for gases:

6. What is “sublimation”?

7. Distinguish between melting and freezing:

8. Distinguish between vaporization and condensation:

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9. Distinguish between vaporization and evaporation:

10. Convert 0.857 atm to mm Hg. Show all work and units.

11. Convert 0.955 atm to kilopascals. Show all work and units.

Atomic and Molecular Structure 1. List Dalton’s atomic theory:

2. Diagram and label JJ Thomson’s atomic model:

a. What did JJ Thomson discover?

3. Diagram and label Rutherford’s atomic model:

a. What two conclusions did Rutherford make about the atom?

4. What is the difference between mass number and atomic number? 5. What is an isotope?

6. What is the difference between mass number and average atomic mass?

7. Which elements have similar chemical properties?

8. What do all atoms of a given element have the same number of?

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9. Differentiate between period and group.

10. Where are metals, semi-metals, and nonmetals located on the periodic table?

11. What are some common characteristics of metals?

12. What are some common characteristics of nonmetals?

13. Where are alkali metals, alkaline earth metals, halogens, noble gases, and transitions metals located?

14. Use your periodic table to complete the table below

ATOM SYMBOL ATOMIC NUMBER

MASS NUMBER

# OF PROTONS

# OF ELECTRONS

# OF NEUTRONS

Fe 56 26 26 CHLORINE 17 18

ARGON 40 18 22 Al 27 13 13

HYDROGEN 1 1 1 TITANIUM 48 22

Periodic Table

1. How is the periodic table arranged?

2. Fill in the following chart

ELEMENT GROUP NAME METAL/NONMETAL/METALLOID Chromium

Iodine Potassium Vanadium Lithium

Neon Californium

Barium Strontium Platinum

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3. Which element is more like lithium in terms of properties, sodium or beryllium? Why?

4. Which element has more electrons in its valence shell, sodium or magnesium?

5. Which element is closer to achieving noble gas configuration, magnesium or lithium?

6. How many valence electrons do the following atoms have? a. Magnesium b. Carbon c. Argon d. Helium e. Silicon f. Potassium g. Sulfur h. Calcium i. Hydrogen

7. How does the size of an atom’s nucleus compare to the entire atom?

8. How does the trend of atomic radius change going across a period? Why?

9. Hoe does the trend of atomic radius change going down a group? Why?

10. What is electronegativity, and what is the most electronegative element?

Nuclear Processes 1. What is meant by the “electromagnetic force”? 2. What is meant by the term “nuclear force”? 3. What is the difference between fission and fusion?

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4. Which process takes place for the formation of the Sun (a star)? 5. Fill in the following chart.

PARTICLE NUCLEAR SYMBOL STRENGTH alpha (α)

beta (β)

gamma (γ)

7. Fill in the following chart:

a.

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90234Th→−1

0e + ____

e.

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64155Eu→−1

0e + ____

b.

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____→ 92232U+0

0γ

f.

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47111Ag→−1

0e + ____

c.

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92245U+−1

0e + ____

g.

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3270Ge→30

66Zn + ____

d.

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47111Ag→2

4He + ____

h.

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92245U+2

4He + ____

Modern Atomic Theory

1. How did Bohr describe an atom? (you may use words or a labeled diagram to describe)

2. What was wrong with Bohr’s atomic model?

3. What does Heisenberg’s Uncertainty Principle tell us? 4. Fill in the table below:

Quantum Number Symbol Meaning Possible Values Principal

Angular Momentum

Magnetic

Spin

5. How many electrons are described by the quantum number n = 4?

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6. How many possible electrons are described by the quantum numbers n = 4 and l = 1?

7. Describe or define the following rules/principles: a. Aufbau Principle:

b. Hund’s Rule:

c. Pauli Exclusion Principle:

8. Fill in the table below for Gallium (Ga): Orbital Notation:

Complete Electron Configuration:

Noble Gas Configuration:

Chemical Bonds

1. Describe how a cation and an anion form.

2. What do metals typically do when they become ions? What about nonmetals?

3. What type of elements bond together in ionic bonds? Covalent bonds? Metallic bonds?

4. How do electrons in ionic bonding interact? Covalent bonding? Metallic bonding? 5. How does the relative size of an anion and cation compare to its neutral atom?

6. Which element would calcium more likely bond with, oxygen or fluorine?

7. Which element would nitrogen more likely bond with, magnesium or chlorine?

8. Which element will react more readily with chlorine, sodium or magnesium?

9. What is an element that Lithium might bond with?

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9. What is an element that Sulfur might bond with?

10. What are the three properties of ionic bonds? Covalent bonds?

11. Draw Lewis Dot Structures for the following compounds

a. CH4

b. CH2Cl2

c. NH3

d. CH3OH

e. H2O

f. O2

g. N2

h. HCN

i. C2H2

12. Describe the arrangement of atoms in crystalline solids.

13. What is the force that holds the positive and negative ions in the crystal of NaCl?

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14. Draw a picture representing ionic, covalent, and metallic bonding. Label each. 15. Label each of the following compounds as ionic or covalent.

a. C6H12O6

b. NaCl

c. NH2CH2

d. SiO2

e. H2O

f. MgBr2

1. What’s Rule #1 for naming?

2. In what type of naming do we use PREFIXES?

3. When do you need to use ROMAN NUMERALS?

4. Name the following polyatomic ions:

a. CN- ______________________

b. NO3- ______________________

c. PO43- ______________________

d. NO2- ______________________

Nomenclature

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e. OH- ______________________

f. CO32- ______________________

g. C2H3O2- ______________________

5. Write the names of the following:

a. NaCl _________________________________

b. AgNO3 _________________________________

c. KOH _________________________________

d. ZnSO4 _________________________________

e. Fe(OH)3 _________________________________

f. CO2 _________________________________

g. AlCl3 _________________________________

h. NH4I _________________________________

i. CaSO4 _________________________________

j. N2O4 _________________________________

k. PbO2 _________________________________

6. Write the formulas for the following (show your work): a. Sulfur dioxide _________________________________

b. Carbon tetrachloride _________________________________

c. Lithium hydroxide _________________________________

d. Ammonium phosphate _________________________________

e. Iron (II) carbonate _________________________________

f. Silver iodide _________________________________

g. Gold (III) chloride _________________________________

h. Copper (II) sulfate _________________________________

i. Nitrogen monoxide _________________________________

j. Magnesium nitride _________________________________

k. Ammonium nitrate _________________________________

l. Ammonium nitride _________________________________

Equations & Reactions

1. Balance each of the following equations:

a. _____ CaCl2 + _____ Li2O à ______ CaO + _____ LiCl

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b. _____ Al2S3 + _____ Cu à ______ CuS + _____ Al

c. _____ Na3P + _____ MgBr2 à ______ Mg3P2 + _____ NaBr

d. _____ Ba3(PO4)2 + _____ Na2CO3 à ______ Na3PO4 + _____ BaCO3

e. _____ C2H6 + _____ O2 à ______ H2O + _____ CO2

2. Label the reaction type. Then, complete and balance. a. K + F2 à Rxn Type:______________

b. HCl + Mg à Rxn Type:______________

c. Na2S + Be(OH)2 à Rxn Type:______________

d. BaF2 + NaNO3 à Rxn Type:______________

e. Ca3(PO4)2 + K2SO4 à Rxn Type:______________

f. Zn(NO3)2 + Mg à Rxn Type:______________

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g. Ca(NO3)2 + Al2(CO3)3 à Rxn Type:______________

h. C3H8O + O2 à Rxn Type:______________

3. When fluorine gas comes in contact with calcium metal at high temperatures, solid calcium fluoride is produced. Write the balanced chemical equation.

4. When aqueous beryllium chloride reacts with aqueous silver nitrate, aqueous beryllium nitrate and solid silver chloride form. Write the balanced chemical equation.

5. What are the signs that a chemical reaction has occurred?

6. List an example of a physical change.

7. List an example of a chemical change. Sig Figs and Unit Conversions

1. Finish the following rules for sig figs:

a. Nonzero digits are _________________________________. b. Leading zeros are _________________________________. c. In-between zeros are _________________________________. d. Trailing zeros are __________________________________________________.

2. How many sig figs in the following numbers?

a. 3.401 x 103 __________________ b. 0.0050 __________________

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c. 500 __________________ d. 6.0001 __________________

3. Write the following numbers in scientific notation

a. 301 __________________ b. 0.05106 __________________ c. 50.54 x 104 __________________ d. 501.01 x 10-5 __________________

4. Complete the following table:

Property/Measurement Base Unit Lab Instrument Length meter (m) Ruler Volume

Time Temperature

Energy Calorimeter Amount

5. Convert 0.406 kL to L. Show all work.

6. Convert 2410.1 micrograms to kilograms. Show all work.

7. Convert 5.01 x 104 meters to centimeters. Show all work.

8. You have a piece of aluminum that occupies a volume of 30.0 mL and has a mass of 81 grams. What is its density? Show your work.

9. You have a piece of zinc metal and measure its mass to be 275.7 grams. If the density of zinc is 7.1 g/mL, what is the volume of the zinc metal? Show all work.