Chemistry Final Review Guide

Unit 1: How to Be a Scientist

Metric Conversions: Convert the following measurements. Show work. REMEMBER TO INCLUDE UNITS!

1. 5.64 grams to milligrams

2. 350 millimeters to decimeters

3. 0.0473kilometers to meters

4. 21 liters to centiliters

5. 7000 milligrams to grams

6. 333 decameters to kilometers

7. 0.49855 kilograms to milligrams

8. 552 milliliters to centiliters

9. 34.4 meters to decimeters

10. 125.6 centigrams to grams

Significant Figures: Write the number of significant figures of each number.

1. 0.0036 _______________

2. 509 _______________

3. 4.345 _______________

4. 90420 _______________

5. 1000 _______________

6. 0.0700 _______________

7. 5,000,000. _______________

8. 99807 _______________

9. 120300 _______________

10. 40 _______________

11. Explain the importance of recording precise measurements during an experiment.

12. List the steps you would take to find the density of a textbook. Make sure you state the equipment you

may need to use.

13. Write the base unit for each measurement.

Mass = __________ volume = __________ length = ___________

14. What are the possible units of density? How do you know this?

Unit 2: Density

1. What is density? (explain in words…not just the formula!)

2. A student measures the mass of an 8 cm3 block of brown sugar to be 12.9 g. What is the density of the brown sugar?

3. A chef fills a 50 mL container with 43.5 g of cooking oil. What is the density of the oil?

4. Calculate the mass of a liquid with a density of 2.5 g/mL and a volume of 15 mL.

5. Calculate the volume of a liquid with a density of 5.45 g/mL and a mass of 65 g.

6. A machine shop worker records the mass of an aluminum cube as 176 g. If one side of the cube measures 4 cm, what is the density of the aluminum?

7. A teacher performing a demonstration finds that a piece of cork displaces 23.5 mL of water. The piece of cork has a mass of 5.7 g. What is the density of the cork?

8. A carver begins work on the following block of granite that weighs 2700 g. What is the density of the granite?

9. A graduated cylinder has a mass of 50 g when empty. When 30 mL of water is added, the graduated cylinder has a mass of 120 g. If a rock is added to the graduated cylinder, the water level rises to 75 mL and the total mass is now 250 g. What is the density of the rock?

10. A man sees a famous bronze statue in the middle of a city. He wishes to know how much mass the statue has, but he is not allowed to put it on any kind of scale. The man knows the volume of the statue and knows it is made of solid bronze. What is the best way for the man to determine the object’s mass? Explain why this is a good method. (Hint: what kind of property is density?)

11. Use the reference table and your density skills to find the identity of the following mystery objects.

12. What is buoyancy? What are the units of buoyancy?

13. Is there buoyancy acting on you as you read this? If so, what is causing this buoyancy force?

14. What is Archimedes’ Principle?

15. If you throw something into a pond and it floats, how much does the amount of water displaced by the object weigh?

16. The box to the right is floating in water. Find the buoyancy force keeping the block afloat!

17. Explain how we determined the relative density of gases in our lab? BE DETAILED IN YOUR EXPLANATION. Draw diagrams to help you explain!

READ THIS: Density is the amount of MASS in a given space. This is similar to ENERGY DENSITY, which is the amount of ENERGY in a given amount of fuel. A Btu is a unit of energy…it is short for a “British thermal unit.” Answer the following question:

18. You measured the Btu’s from two different fuels; gasoline and diesel. You burned 22 gallons of diesel, and this released 2,826,736 Btu of energy. You also burned 29 gallons of gasoline, and it produced 3,253,879 Btu of energy. Calculate the energy density of each fuel type.

19. Why does a Volkswagen Jetta with a diesel engine get more miles per gallon than a Jetta that has a gasoline engine?

20. A square piece of aluminum foil, 8.0 in. on a side, is found to weigh 1.863 g. What is the thickness of this foil, in mm? (The density of aluminum is 2.70g/cm3).

21. The diameter of metal wire is often referred to by its American wire gauge number. A 16-gauge wire has a diameter of 0.05082 in. What length of wire, in meters, is there in a 1.00-lb. spool of 16-gauge copper wire? The density of copper is 8.92 g/cm3

DENSITY MEGA-CHALLENGE!

You will need to research what a “mole” is. Hint: it is a large number…do not attempt this problem without a scientific calculator! Complete on a separate sheet of paper!

How many Cu atoms are present in a 1.00-m length of 20-gauge copper wire? (A 20 gauge wire has a diameter of 0.03196 in.; density of Cu = 8.92 g/cm3.)

Unit 3: Periodic Table and Classification of Matter

1. Label the protons, electrons, and neutrons on the atom.

a. Which subatomic particles are found in the nucleus?

Use the periodic table to help answer questions.

2. What is the atomic radius? Explain the direction in which the atomic radius of elements increases on the

periodic table.

3. a.) Using the image, what can we find out about a certain element using the

periodic table?

b.) What else can the periodic table tell us? List at least 3 other ways it is organized.

4. Which element is more electronegative: chlorine or aluminum? Explain how you know this.

5. Which element is more reactive: rubidium or phosphorous? Explain how you know this.

6. Which of the following elements would be a good conductor of electricity: hydrogen, copper, or

germanium. Why?

7. Which family has high reactivity: alkali metals or halogens? Why?

8. Using the periodic table, find the following for the element Silicon:

a. Atomic number ___________

b. Atomic mass ___________

c. Protons ___________

d. Neutrons ___________

e. Electrons __________

f. Group __________

g. Family __________

Valence Electrons

1. Where are valence electrons located in an atom?

2. Draw a Bohr model and state how many valence electrons for the following elements:

a.) Oxygen b.) Aluminum

c.) Chlorine d.) Calcium

3. Draw a Lewis Structure for the following elements:

a.) Nitrogen b.) Carbon

c.) Fluorine d.) Sodium

Phase Changes

1. A glass of water and a glass of ethanol are placed on a hot plate. The ethanol is boiling faster than the

water. Why is that?

2. Use the phase diagram to answer the following questions.

a. Evaporation is happening at which

letter?

b. Matter is a liquid at which letter?

c. Melting happens at which letter?

d. More heat energy is applied at which

phase change: C or E?

e. Letter D is what state of matter?

Elements, Compounds, Mixtures

For the following statements, answer with element, compound, or mixture. If it is a mixture, state whether it is

homogenous or heterogeneous.

1. H2O ____________________ _____________________

2. Aluminum ____________________ _____________________

3. Sugar water ____________________ _____________________

4. Neon ____________________ _____________________

5. Carbon dioxide ____________________ _____________________

6. H2SO4 ____________________ _____________________

7. Cookie dough ____________________ _____________________

8. Gold ____________________ _____________________

9. NaCl and water ____________________ _____________________

10. Define a solution. Explain what a solute and a solvent are and give an example for each.

11. What method did we use in lab to separate an insoluble solid from a solution? How did we do this?

Physical vs. Chemical

For the following properties, list if it is physical (P) or chemical (C).

1. Boiling point ____________________

2. Ability to rust ____________________

3. Elasticity ____________________

4. Freezing point ____________________

5. Ability to burn ____________________

6. Reactivity ____________________

7. Brittleness ____________________

8. Transparency ____________________

For the following changes, list if it is physical (P) or chemical (C)

1. Cutting hair ___________________

2. Growing grass ___________________

3. Frying an egg ___________________

4. Breaking a pencil ___________________

5. Rust on nail ___________________

6. Water turns into steam ___________________

7. Stretch a rubber band ___________________

8. Light a grill ___________________

Unit 4: Chemical Bonds and Organic Molecules

1. What part of the atom is involved in bonds?

2. What happens in an ionic bond?

3. What happens in a covalent bond?

4. What kind of bonds does carbon like to make?

5. How many bonds do the following elements usually make?a. Carbonb. Oxygenc. Hydrogen

6. What are the C-H-N-O-P-S elements and what is their significance?

7. Ionic Bonds - Draw the Lewis structures for each atom, draw arrows to show the transfer of electrons, write the charge for each ion, and then write the chemical formula (ex: H20 is the chemical formula for water.)

(A) Potassium + Iodine (B) Magnesium + Oxygen (C) Lithium + Nitrogen

8. Covalent Bonds – Draw the Lewis structures for each atom, and write the chemical formula. Lastly, name the covalent compound you have drawn. (A) Fluorine + Fluorine (B) 3 Hydrogen + 1 Phosphorus (C) 2 Hydrogen + 1 Sulfur

9. Complete the table below regarding biological macromolecules

Macromolecule Elements that make it Examples Picture (write

tips to identify) Function

Carbohydrates

Proteins

Lipids

Nucleic Acids

10. What is the difference between a polar and a non-polar bond?

11. Determine the type of bond (ionic, polar covalent, or non-polar covalent ) that will form between atoms of the following elements and show the polarity of the bond if it is polar covalent. It would probably help you to do this by drawing Lewis dot structures.

a. Ca and Cl

b. C and S

c. Mg and F

d. N and O

e. H and O

f. S and O

12. The bonds between the following pairs of elements are covalent. Using the table showing electronegativity (last page of packet), calculate the electronegativity difference for the atoms that are bonded in the following molecules. Rank the bonds from highest to lowest polarity.

SHOW WORK HERE RANK

a. H—Cl 1._____

b. H—C 2._____

c. H—F 3._____

d. H—O 4._____

e. H—H 5._____

f. S—Cl 6._____

13. Remember that an entire molecule may be polar or non-polar. Decide whether the molecules (A – E) below would be polar or non-polar followed by an explanation for your answer.

Structure Polar or Non-polar ExplanationA

B

C

D

E

14. What is a hydrogen bond? Show what a hydrogen bond might look like between some water molecules.

15. What important macromolecule in your body’s cells is held together by hydrogen bonds?

A.

B.

C.

D.

E.