The format of this test is MULTIPLE CHOICE - TypePadwaltonhigh.typepad.com/files/fall-semester-review-packet-4.pdfFINAL EXAM REVIEW PACKET Fall Semester 2014 This packet is optional

Honors Chemistry

FINAL EXAM REVIEW PACKET

Fall Semester 2014

This packet is optional and will not count for, replace or be used for ANY grade (or extra credit)

Chemistry Final Review Material

The format of the final exam is MULTIPLE CHOICE. This review packet is intended to inform you of the

content in each unit covered and allow you practice with the content from this semester. It is not intended to

address any specific test question on the final exam. Completion of this packet does not guarantee success on

the Final Exam, but practicing with the content is a great idea.

Unit 1: Scientific Method, Graphing, and Safety

DEFINE:

a. Chemistry

b. scientific method

c. Dependent variable

d. independent variable

1. Identify the following pieces of lab equipment:

3.

Chemistry Final Review Material 1. Safety: Describe an important rule in lab that applies to the following items:

Example: Food: Food is never allowed in lab.

a. Goggles:

b. Accidental Spills

c. Clothing/ Shoes:

d. Smelling Chemicals:

2. Which unit(s) of measurement are usually dependent variables? Which are most often independent variables?

3. Label each kind of graph shown and answer the following questions about the graphs

a. What percent of the sources of chlorine in the stratosphere are CFCs?

b. During which month of the year does Jacksonville usually get the most precipitation? The least?

4. Sequence the following steps for plotting a line graph

________ a. Give the graph a title.

________ b. Choose the ranges for the axes.

________ c. Identify the independent and dependent variables.

________ d. Plot the data points.

________ e. Determine the range of the data that needs to be plotted for each axis.

________ f. Draw the "best fit" line for the data.

________ g. Number and label each axis.

Chemistry Final Review Material Unit 2: Measurement

Uncertainty in Measurements, SigFigs, Sci Notation, Dimensional Analysis, Rounding Rules

DEFINE:

a. accuracy

b. precieion

c. scientific notation

d. significant figures

1. In the measurement 0.503 L, which digit is the estimated digit?

a. 5 b. the 0 immediately to the left of the 3 c. 3 d. the 0 to the left of the decimal point

2. Which two of these are equivalent lengths?

a. 6000 cm b. 0.0600 km c. 60 mm d. 0.600 m

3. Which of these is the smallest length?

a. 6000 cm b. 0.0600 km c. 60 mm d. 0.600 m

4. Convert 600 kilograms to grams

5. Which of the following conversions is/are incorrect.

a. 1 kilometer = 1000 meters c. 500 centimeters = 0.5 meters

b. 100 millimeters = 1 centimeter d. 1 meter = 1000 millimeters

6. The measure of the amount of three-dimensional space that an object occupies is known as:

a. volume b. density c. weight d. mass

7. Convert to 350. mL to Liters

8. Which metric distance is equal to 0.62 miles?

a. One centimeter b. One millimeter c. One meter d. One kilometer

9. In the metric system, the base unit for mass is the:

a. Gram b. Meter c. Liter d. Pound

10. Convert: 500 meters to kilometers

11. Convert 5.0 x 103 mL to liters

12. How many milliliters are in one deciliter?

a. 1 million, or 106 b. 1 thousand, or 103 c. 100, or 102 d. 10, or 101

Chemistry Final Review Material 13. In the metric system, the base unit for length is the:

a. yard b. foot c. mile d. meter

14. Convert 75 mL to cm3

15. Convert to 0.050 kilograms to grams

16. Which of the following are equivalent lengths?

a. 45 000 kilometers b. 45 000 millimeters c. 45 meters d. 450 centimeters

17. Which of the following is the largest mass?

a. 800 centigrams b. 5 kilograms c. 1 000 milligrams d. 100 grams

18. Determine the value of the missing measurement. SHOW YOUR WORK! USE UNITS!

mass = 75 g; volume = 10 cm3; density = _____________

mass = 400 g; density = 15 g/cm3 ; Volume = ____________

volume = 25 cm3; density = 5 g/cm3 ; Mass = ___________

19. Identify the number of sig figs in each of the following:

520 mL _______ 10.002 ns _______

0.0102 ms_______ 0.4051 Pa ______

0.230 kg _______ 0.001 cm _______

25,6000 L ______ 23.0 m _______

20. Calculate using sig fig rules: (Review sigfig rules in calculations http://www.phys.unt.edu/PIC/significant_figures.htm)

a. 0.3287g x 45.2g = c. 12.5kg + 52.68 kg + 2.1 kg =

b. 0.258 mL / 0.36105 mL = d. (1250 cal – (234.207 cal / 52.69 cal) =

21. Write in scientific notation:

8960 _________ 36,000,000 ____________

0.00023 _________ 0.000 000 025 3 ___________

86,000 ___________ 2.04 x 103 ___________

1.23 x 10-5 ________ 1.20 x 10-2 ___________

Chemistry Final Review Material

22. Determine the numeric measurement (include units) associated with each of the following pictures:

Unit 3: Matter

Types of Matter, States of Matter, Physical/Chemical Properties, Physical/Chemical Changes

DEFINE:

a. matter

b. homogeneous

c. heterogeneous

d. mixture

e. pure substance

f. solution

g. physical property

h. chemical property

i. phase changes/changes of state

Use the word bank below to complete each sentence.

Evaporation Condensation Freezing Melting

Element Solution Heterogeneous Homogeneous

Compound Mixture Substances Atoms

Chemistry Final Review Material 1. ______________ occurs when a gas becomes a liquid.

2. All matter is made up of tiny particles called _________.

3. When a solid becomes a liquid, _______________ occurs.

4. An _____________ is made up of only one type of atom.

5. _______________ changes a liquid into a solid.

6. A ______________ is made up of 2 or more substances that are physically combined (and can be separated).

7. When a liquid becomes a gas, ________________ occurs.

8. A mixture that is uniform (evenly spread) throughout the sample is said to be __________________. These types

of mixtures are also known as ___________________.

9. ________________ are 2 more atoms chemically bonded in a definite ratio.

10. A mixture that has uneven distribution of 2 or more substances is called _____________________.

11. Matter is divided into 2 categories: ______________ and Mixtures.

12. Use the words below to complete the concept map.

heterogeneous salt-water mixture sand-water mixture mixtures solutions water

Chemistry Final Review Material 13. Identify the following as either a chemical or physical change:

a. Torn car seat ________ f. Crack in the sidewalk ____ _______

b. Car’s faded paint __ _______ g. Burning a log ___ ___________

c. A car’s rusting hood __ _______ h. Crushing a pop can _____________

d. butter melting _____ ________ i. leaves changing color____ ________

e. alcohol evaporating____ _______ j. wood rotting ___ ____________

14. Identify as an element or a compound:

a. water ___________ c. helium ____ ___________

b. carbon dioxide ____ ______ d. arsenic ______________

15. Identify as a pure substance, heterogeneous mixture or a homogeneous mixture:

a. Alphabet soup____________ d. salt_________________

b. sea water __________ e. granite ____________

c. air___________ f. sugar ______________

Unit 4: Atomic Structure

History of the Atom, Subatomic Particles, Isotopes, Average Atomic Mass

DEFINE:

a. atom

b. electron

c. proton

d. neutron

e. nucleus

f. isotope

g. atomic number

h. mass number

i. average atomic mass

Chemistry Final Review Material 1. Describe the evolution of the model of the atom from Democritus through the present day model.

2. How many protons and electrons are present in a vanadium atom?

3. How many protons and electrons are present in a nitrogen atom?

4. What is the name of the element that has atoms that contain 5 protons?

5. Write the chemical symbol for the ion with 95 protons and 89 electrons.

6. Write the chemical symbol for the ion with 33 protons and 36 electrons.

7. Where are protons located in an atom? What is its charge?

8. Where are electrons located in an atom? What is its charge?

9. Where are neutrons located in an atom? What is its charge?

10. What is the atomic number of helium?

11. What is the atomic mass of oxygen?

12. Complete the table below.

Isotope Symbolic Notation

Number of Protons

Number of Electrons

Number of Neutrons

Hydrogen-1 1 1 0

8 10

Copper-65 36

13. The element copper, Cu, has two naturally occurring isotopes. 69% of all copper consists of atoms with 34

neutrons, 31% of all samples consist of samples with 36 neutrons.

a. What are the two mass numbers? ___________ and ____________

b. Calculate the average atomic mass of copper atoms.

Chemistry Final Review Material Unit 5: Electron Configuration

Arrangement of electrons in the electron cloud

DEFINE:

a. principal energy level

b. valence level

c. sublevel

d. “s” block

e. “p” block

f. “d” block

g. “f” block

1. List the first 4 places electrons can be found in the electron cloud and identify how many electrons each can

contain.

2. Write the orbital notation for:

Ca-20

F-9

Ni-28

Sb-51

3. Write the electron configuration/spectroscopic notation for:

Ca-20

F-9

Ni-28

Sb-51

4. Write the noble gas notation for:

Ca-20

F-9

Chemistry Final Review Material

Ni-28

Sb-51

5. Write the Lewis dot notation for:

Ca-20

F-9

Ni-28

Sb-51

6. How many valence electrons are present in each of the above atoms?

7. How many electrons can be placed into an “s” sublevel? Into a “p” sublevel? Into a “d” sublevel? Into an “f”

sublevel?

8. Which elements will gain electrons to form an ion? Where are these elements located on the Periodic Table?

9. Which elements will lose electrons to form an ion? Where are these elements located on the Periodic Table?

Unit 6: Periodicity

History of the Periodic Table, Characteristics of Elements, Periodic Trends

DEFINE:

a. period

b. group/family

c. metal

d. nonmetal

e. metalloid

Chemistry Final Review Material f. electronegativity

g. electron affinity

h. atomic radius

i. ionic radius

j. ionization energy

1. Answer the following about the Periodic Table:

a. What is the special group name in which Sodium is found?

b. What is the special group name in which Fluorine is located?

c. What is the special group name in which Neon is found?

2. Use the word bank to fill in the appropriate term below.

a. Metals are found primarily on the ________ side of the periodic table (with the exception of _______________).

Nonmetals are found on the _________ side of the table.

b. Columns in the periodic table are called _________________ and the rows are called _________________.

c. The ______________________ are found in group 1. They are the most reactive metals. Group 2 metals are

called the______________ _______________________.

d. The last group (18) are called the _________________________. They are non-reactive or _____________.

e. Salt forming compounds come from group 17, the________________. They are the most reactive nonmetals.

f. Metalloids are found along the “_______________________”, and are often used as semiconductors, like

computer chips.

g. Groups 3 – 13 are called the __________________________, and include the 2 series below the table, the

____________________ &___________________.

h. ______________ have high luster and can conduct electricity and heat. They are also ____________ and

____________.

i. ______________ have no luster, and are poor conductors of heat and electricity.

j. _______________ have properties of both metals and nonmetals.

Groups periods metals nonmetals metalloids

Hydrogen Inert right left staircase

Actinides Halogens Alkali Metals Noble Gases Lanthanides

Ductile malleable Transition Metals Alkaline Earth Metals

Chemistry Final Review Material 3. Determine the charge assigned to each of the following ions:

Aluminum ___ ______ Chloride ___ _____ Copper(II) ___ ______ Zinc ___ _____

Magnesium ___ _____ Sulfur ____ ____ Phosphide ___ ______ Silver ___ _____

4. How does the size of an ion compare to the size of the neutral atom from which it was created?

5. How does an atom’s position on the periodic table provide information on that atom’s size (atomic radius)?

6. What is electronegativity and why do nonmetals have high values for it?

7. Describe the difference in the tendencies of metals and nonmetals to form ions (which is more likely to form a

cation and which is more likely to form an anion

8. Which atom is the largest?

a. Li b. B c. N d. F e. He

9. Which atom is the largest?

a. Li b. K c. Rb d. Cs e. Kr

10. Which atom has the largest ionization energy?

a. Li b. B c. N d. F e. He

11. Which atom has the largest ionization energy?

a. Li b. K c. Rb d. Cs e. Kr

Chemistry Final Review Material

12. Which atom has the largest electron affinity?

a. Li b. B c. N d. F e. He

13. Which atom has the smallest electron affinity?

a. Li b. K c. Rb d. Cs e. Kr

Unit 7: The Mole

Avogadro’s Number, Molar Mass, Molar Volume, Dimensional Analysis

DEFINE:

a. mole

b. Avogadro’s number

c. molar mass/formula mass

d. molar volume

e. STP

f. percent composition

g. empirical formula

1. Answer the following:

a. The representative particle of an element is a(n)___ ________________.

b. The representative particle of an molecular compound is a(n)_______________

c. The representative particle of an ionic compound is a(n)___________ ___.

2. Calculate the molar mass of the following compounds: (Remember to add units)

a. CaCO3___________

b. MgSO4___________

c. NaOH___________

d. KCl ___________

e. Co(NO3)2________________

f. Zn(PO4)2________________

Chemistry Final Review Material

3. Find the mass of 1.112 mol of HF.

4. If you have 66.38 g of KMnO4 find how many moles it is made up of?

5. How many moles of ethane (C2H6) contain 8.46 x 1024 formula units?

6. How many molecules are in 5.1 g of H2O?

7. What is the mass of 22.4 L of H2O?

8. Find the % composition of H in H2O?

9. Find the % composition when 9.02 g of Mg combine completely with 3.48 g of N to form a compound.

10. Calculate the empirical formula for a compound made up of 94.1% O, and 5.9% H.

11. Calculate the empirical formula for a compound made up of 79.8% O, and 20.2% H.

Chemistry Final Review Material Unit 8: Nomenclature

Ionic Compounds

Transferring electrons, ions, nomenclature

DEFINE:

a. ionic bond

b. ionic compound

c. polyatomic ion

d. nomenclature

e. stock system

f. traditional system

g. empirical formula

1. Name or write the formulas for the following:

potassium iodide KOH

barium chloride LiI

lithium bromide AlF3

iron(III) sulfate FeCl2

chromium(III) sulfide MgO

calcium carbonate Co(NO3)2

cobalt(II) fluoride Zn(PO4)2

silver oxide (NH4)SO4

magnesium hydroxide NO

Nickel(II) nitrate AgI

Covalent Compounds

DEFINE:

Chemistry Final Review Material a. molecule

b. Lewis structure

c. single bond

d. double bond

e. triple bond

f. multiple bond

g. sigma () bond

h. pi () bond

i. VSEPR theory

j. molecular geometry

k. polar bond

l. polar molecule

m. nonpolar molecule

1. Name the following molecules:

SiO2 PCl3

SiF4 N2O

SO3 N2O5

2. Write the formula or name for these compounds.

dinitrogen pentoxide P3O4

phosphorus trichloride silicon hexacarbide

selenium monofluoride trisulfur heptabromide

carbon monoxide carbon dioxide

carbon tetrachloride diphosphorus octoxide

3. How are bonds different in ionic and covalent compounds.

Chemistry Final Review Material

4. Why do most atoms form bonds?

5. Which nonmetal groups on the periodic table can form double bonds?

6. Which nonmetal elements can form triple bonds?

7. Which nonmetal elements can only form single bond?

8. Which elements are exceptions to the octet rule when drawing Lewis Structures? Why are they exceptions?

9. What major assumption of the VSEPR theory means that bond angles will be as large as possible and that compound

will exist in 3 dimensional space?

10. In H2S, two hydrogen atoms are bonded to one sulfur atom. Why isn’t the molecule linear?

11. What two factors determine whether or not a molecule is polar?

12. Draw the Lewis Structure for the following molecules, then determine if the molecule is polar or nonpolar.

HCN N2

HF H2S

NH3

Chemistry Final Review Material Unit 9: Chemical Reactions

Words to formulas, Balancing, types, predicting products, Activity Series, Solubility Rules

DEFINE:

a. law of conservation of matter

b. reactant

c. product

d. coefficients

e. precipitate

f. soluble

g. insoluble

h. activity series

1. List the observable indications that a chemical change has occurred.

2. Use the word bank to match the correct term with its definition.

_______________ a. compounds found after the yield sign (right side)

_______________ b. reaction using oxygen to form carbon dioxide, water, and energy

_______________ c. the number and type of atoms on each side of a chemical reaction must be balanced (matter is

not created ordestroyed!)

_______________ d. reaction where 2 elements “switch” places to form 2 new compounds

_______________ e. reaction that forms a more complex substance

________________f. numbers placed before a compound to balance the equation

_______________g. compounds found before the yield sign (left side)

_______________ h. reaction where one element replaces another

decomposition reaction products synthesis reactions

Law of Conservation of Mass single replacement reactions coefficients

double replacement reactions reactants combustion reactions

neutralization reaction

Chemistry Final Review Material _______________ i. reaction involving an acid and a base to form water & salt

_______________ j. reaction that breaks down a complex substance

3. Classify each reaction by type and balance them:

____________ a._____H2O2 _____H2O + _____O2

____________ b. _____Fe + _____O2 Fe2O3

____________ c._____Fe2O3 + _____H2 _____Fe + _____H2O

____________ d. _____Zn + _____H2SO4 _____Zn SO4 + _____H2

4. Predict the products of the following reactions and classify the reaction by its type:

a. NaCl + KNO3

b. Na + O2

c. Cl2 + KF

d. H2O

5. Balance the following equations:

a.__ __ AgNO3 + ___H2S ___Ag2S +___ HNO3

b.___MnO2 + ___HCl ___ MnCl2 + ____H2O + ___Cl2

6. Predict end products and write balanced chemical equations and use (aq), (g), (l) or (s) after each formula.

a. Sodium chloride reacts with lead (II) nitrate to produce…

b. Calcium nitrate reacts with sodium sulfide to produce…

Chemistry Final Review Material

c. Ni + AgCl

d. Fe + O2

e. CH4 + O2

f. Ca(CO3)2 h. H2O + KCl

Unit 10: The Mole

Calculate the Molar Mass for each compound.

H2SO4

Ca(OH)2

Al2(CO3)3

Avogadro’s Number (1 mole) =_________________________

What is the molar mass of sodium bicarbonate (NaHCO3)?

How many molecules of sodium bicarbonate are present in one mole?