Chemistry Final Exam Comprehensive Review Guide

DAY 1 - Atomic Theory, Scientists, Basic Atomic Structure, Nuclear Chemistry

1) List the scientists who developed the atomic theory and their contributions:

2) Describe the experiment that was performed below:

3) Draw a sketch of what the Bohr model looks like:

4) What is meant by electron transition? Give examples:

5) Draw a sketch of the quantum mechanical model:

How is it different than the Bohr model?

6.) _________the smallest particle of an element that retains the properties of that element

_________a positively charged subatomic particle

_________a negatively charged subatomic particle

_________a subatomic particle with no charge

_________the central part of an atom, containing protons and neutrons

_________atoms with the same number of protons, but different numbers of neutrons in the nucleus of an atom

_________the total number of protons and neutrons in the nucleus of an atom

_________The number of protons in the nucleus of an element

_________the weighted average of the masses of the isotopes of an element

_________one-twelfth the mass of a carbon atom having six protons and six neutrons; “AMU”

7.) Complete the table below:

Element Symbol # Protons # Electrons # NeutronsAluminum ( ____ )Sodium ( ____ )Neon ( ____ )Potassium ( ____ )Sulfur ( _____ )

8.) What is an isotope and how can they be written?

9.) How many protons, neutrons, and electrons are there in 40K?

10.) How many protons, electrons, and neutrons are in Carbon-14. 11.) List the different types of radiation, their symbols, and their charges/number:

12.) Carbon -14 is produced when Nitrogen-14 captures an electron, write out the nuclear reaction for this process.

13.) What particle is needed to complete the following equation?

N + ____ C + H

14.)

What is the definition for half-life?

How many half-lives pass if you only have 1/32 of parent remaining?

13) Compare fusion and fission:

DAY 2 - Periodic Trends, Electron Configuration, Bohr Model

1.) Review Bohr model again……draw a sketch showing electron transition.

How is this related to atomic spectra?

What is EMR? Examples?

2.) Groups on the periodic table are ______________ Families on the periodic table are _________________

3.) List all the major groups/families of elements on the periodic table.

4.) What are electron energy levels?

5.) What is the electron configuration ofmercury _______________________________

calcium __________________________________

neon _________________________________

fluorine __________________________________

strontium ______________________________

iron _____________________________________

6.) Define and describe each of the following Periodic Trends -Electronegativity:

Ionization energy:

Atomic Radius (Radii):

7.) Sketch and explain the reasoning for the 3 periodic trends on the periodic table: (DETAILED)

8.) Give the longhand electron configuration for arsenic.

9.) The largest atoms are in the ___ corner of the table.

DAY 3 - Bonding, Nomenclature, Acid & Base Nomenclature

1.) Name the following chemical compounds:

a) PbBr2 __________________________________

b) NH3 __________________________________

c) P4 __________________________________

d) CaS __________________________________

e) H2SO4 __________________________________

f) V(CO3)2 __________________________________

g) P2O5 __________________________________

2.) Write the chemical formulas and identify the type of bonding involved in the following compounds:

a) ammonium nitrate __________________________________

b) fluorine __________________________________

c) boron trichloride __________________________________

d) iron (III) phosphate __________________________________

e) nitric acid __________________________________

f) potassium carbonate __________________________________

g) dinitrogen tetrachloride __________________________________

3.) Write the formula and name the type of bonding that occurs in each of the following compounds:

a) ammonium sulfate __________________________________

b) boron trichloride __________________________________

c) hydrogen fluoride __________________________________

d) dihydrogen monoxide ________________________________

4.) Compare and contrast: (i.e. how are they formed?, how do their physical properties differ?, what are their representative particles called?, etc.)

Ionic Compounds Molecular Compounds

5.) Draw the Lewis Structures for each of the following molecular compounds, and describe the shape of each molecule using VSEPR theory:

water carbon dioxide methane

Find 5 other examples of molecular compounds you can draw the Lewis structures for:

6.) What are the main 5 geometric shapes associated with the VSEPR theory? Draw each of them.

7.) Classify the following as chemical or physical changes, and explain why:rusting of iron

digestion of meat

boiling water

8.) Write formulas for the compounds in:

magnesium fluoride

dinitrogen pentoxide

sodium sulfate

phosphoric acid

9.) Name the compounds:

KNO3 HBr SO3 FeCl3

10.) Draw the Lewis diagram & specify the molecular geometry & polarity:

11.) Explain the difference between a POLAR BOND and a POLAR MOLECULE

12.) Can a molecule have polar bonds but not be a polar molecule? Use methane to explain!

AsH3 BF3

DAY 4 - Chemical Reactions, Reaction Types, Predicting Products

1.) Identify the 5 types of chemical reactions and give an example for each:

Reaction Type Example

2.) What is a hydrocarbon?

Examples:

3.) For each of the following reactions, identify the reaction type, predict the products and balance the equation. Include physical states. Word equations must first be converted to formulas.

____ Li(s) + ____ N2(g)

____ Mg(s) + ____ CrCl3(aq)

____ CoBr2(s)

What does the delta mean?

Reaction Type: _______________________________

Reaction Type: _______________________________

Reaction Type: _______________________________

____ C4H8(g) + ____ O2(g)

Aqueous solutions of potassium bromide and silver nitrate react to form a white precipitate.

Solid nickel is added to an aqueous solution of iron(II) sulfate.

4.) Write the reaction and balance:

Hydrogen and nitrogen react together to produce ammonia gas (note: the reaction is a reversible one - ammonia also breaks up to form hydrogen and nitrogen):

5.) Write the net ionic equation for the following double displacement reaction:

H PO (aq) Ca(OH) (aq) Ca (PO ) (aq) H O(l)

Reaction Type: _______________________________

Reaction Type: _______________________________

Reaction Type: _______________________________

6.) Consider the following double displacement reaction: copper(II) oxide reacts with sulfuric acid to produce copper(II) sulfate and water.

I. Write a balanced chemical equation that describes this reaction.

II. Write a complete and net ionic equation for this reaction.

7.) Predict the precipitate that forms when aqueous solutions of silver nitrate and potassium chloride react to form products in a double-replacement reaction. Include the complete and net ionic equations for this chemical equation as well.

8.) What are some observations that can be made to indicate that a CHEMICAL change has occurred? DESCRIBE

8) What does “reaction rate” really mean?

What factors can affect the rate at which a reaction occurs? LIST AND DESCRIBE EACH IN TERMS OF COLLISION THEORY.

9.) Draw the energy diagrams for an exothermic and endothermic reaction. Label the important part of the energy diagram that we learned in class….

10.) Draw a graph that shows what happens to the concentration of reactants and products as a reaction progresses:

11.) What is a reversible reaction?

Explain what it means for a reaction to reach equilibrium:

DAY 5 - The Mole, Stoichiometry, Percent Composition, Empirical/Molecular Formula

1.) Write the “double mole map” here:

2.) What are examples of representative particles forMolecular compounds:

Ionic compounds:

Individual elements:

3.) How many grams of methane are there in 1.23 x 1024 molecules?

How many liters of carbon dioxide are there in 45 grams?

Convert 5.6678 moles of arsenic to grams:

89.3 liters of water vapor is equivalent to ________________ molecules of water vapor.

How many moles of ammonium sulfate do I have if my sample weighs 496 grams?

Calculate the number of moles in 13.5 g magnesium nitrate (Mg(NO3)2)

4.) Write the formula for molarity:

How is molarity useful / important?

5.) Solve the following molarity problems. Show all work and include correct units!

Find the molarity of a solution in which 58 g of NaCl are dissolved in 2.5 L of solution.

How many grams of KMnO4 should be used to prepare 2.00 L of a 0.500M solution?

What volume of 0.25M solution can be made from 5.0 g of KCl?

Find the molarity of a 450 mL solution containing 13.7 g of ZnSO4.

How many grams of CuCl2 are required to make 75 mL of a 0.20M solution?

6.) Solubility Curve

What kinds of substances have solubility that DECREASES as temperature increases?

How can to tell from the graph? List those substances.

7.) What is the definition of empirical formula?

Describe what the solubility curve is showing:

How many grams of each substance below can dissolve in 100 grams of water at 60° C?

a. NaNO3

b. NH4Clc. Ce2(SO4)3

Classify each of the following as either saturated, unsaturated, or supersaturated:

a. 90 g of NaNO3 at 30 °Cb. 70 g of KNO3 at 40 °Cc. 10 g of NH3 at 90 °C

8.) Identify each of the following as an empirical formula or a molecular formula:

C2H4 __________________ NaCl __________________

H2O __________________ C6H12O6 __________________

H2O2 __________________ N2O4 __________________

NH4 __________________ H2S __________________

9.) Determine the empirical formula of a compound that contains 36.5% sodium, 25.4% sulfur, and 38.1% oxygen.

10.)  An organic compound has an empirical formula of CH and a molecular mass of 78 g.  What is the molecular formula?

11.) Determine the percent composition of Fe3(PO4)2

12.) A 350.0 gram sample of iron ore has been tested to contain 97.7 grams of iron. What is the percentage of iron in the ore?

What percentage of the iron ore IS NOT iron?

13.) What is the empirical formula of a compound that is 52.5% phosphorus and 47.5% oxygen?

14.) Determine the empirical formula of the following compound:10.0% C 0.80% H 89.1% Cl

15.) How many grams of carbon dioxide will be made when 100 grams of methane burn in an excess of oxygen?

16.) Write the empirical formula for a compound that is 26.5% K, 35.4% Cr, 38.1% O.

17.) Review this again!! Write the formula and name AND the type of bonding that occurs in each of the following compounds:

a) ammonium sulfate __________________________________

b) boron trichloride __________________________________

c) hydrogen fluoride __________________________________

d) dihydrogen monoxide ________________________________18.) Find the percentage composition of iron(III) oxide. Formula: _______________

19.) Find the mass percentage of water in copper(II) sulfate pentahydrate.

20.) How many grams of iron can be obtained from a 268-g sample of iron(III) oxide?

21.) A compound used to test for the presence of ozone in the stratosphere contains 96.2% thallium and 3.77% oxygen. What is its empirical formula?

22.) The molecular mass of benzene, an important industrial solvent and know carcinogen, is 78.0 g/mol and its empirical formula is CH. What is the molecular formula of benzene?

23.) Ascorbic acid, or vitamin C, has a percent composition of 40.9% C, 4.58% H, and 54.5% O. Its molecular mass is 176.1 g/mol. Find its empirical and molecular formulas. (HINT: Multiply by 2, 3, or 4 to get whole number subscripts.)

24.) How many magnesium sulfate molecules are in 25.0 g?

25.) Find the molarity of a 750 mL solution containing 346 g of potassium nitrate.

26.) Calculate the number of grams required to make a 50.0 mL solution of 6.0M NaOH.

27.) Find the % composition of copper(II) chloride.

DAY 6 - Gas Laws, Basic Matter, Density

1.) Identify the gas laws that explain these situations. Specify the variables involved and whether they have a direct/inverse relationship.

A balloon pops after floating high into the atmosphere.

A balloon pops in a hot car on a summer day.

Do not store aerosol cans at temperatures above 120F. “Danger of explosion.”

2.) Identify the gas law and solve the problem:A jar is tightly sealed at 22C and 772 torr. What is the pressure inside the jar after it has been heated to 178C?

300.0 mL of gas has a pressure 75.0 kPa. When the volume is decreased to 125.0 mL, what is its pressure?

50.0 L of gas has a temperature of 75C. What is the temp in Celsius when the volume changes to 110 L?

What is the volume of a container that holds 48.0 g of helium at a pressure of 4.0 atm and temperature of 52C?

3.) A gas occupies 325 L at 25C and 98.0 kPa. What is its volume at 70.0 kPa and 15C?

4.) Define: STP Temperature

Kelvin Volume

Air Pressure

5.) What is the meaning of DENSITY?

What is the formula for density?

What are the units for density?

How is density important?

6.) Limestone has a density of 2.72 g/cm3. What is the mass of 24.9 cm3 of limestone?

7.) Helium has a density of 0.017 g/L. What is the volume of a weather balloon that contains 38 g of helium?

8.) A certain metal has a mass of 50 grams and a volume of 18.5 cm³. What is the density of the metal? Identify the metal.

51.15 J of heat was applied to a metal that has a mass of 5 grams. The metal increased in temperature by 10 degrees C. Identify the metal.

9.) What is normal boiling?

What is normal melting?

What is the triple point?

What substance is this a phase diagram for?

10.) How many moles of chloroform gas, CHCl3, are required to fill a 253-mL flask at 100.0C and 940 torr?

11.) You want the pressure inside a bottle to be 75.0 kPa at 23C. At what temperature in Celsius should you seal the bottle when the pressure is 1.12 atm?

12.) A Marshmallow Peep® has a volume of about 45.0 cm3 at 101 kPa. What pressure is required to increase its size to 150.0 cm3 assuming no air escapes from the Peep®.

13.) A bottle containing hydrogen, nitrogen, and oxygen gases has a total pressure of 80 kPa. If the partial pressure of the hydrogen gas and the nitrogen gas in the container equals 10 kPa each, what is the partial pressure of the oxygen gas?

Formula:

DAY 7 - Solutions, Acids/Bases

1.) List the general properties of acids and bases for each category below:

ACIDS BASESTaste

pH range

Feel

What ion does it produce when dissolved in water?

Which ones are “Strong”? What does

that mean?

Arrhenius Theory states:

Brønstead-Lowry Theory states:

1.) Refresh on the pH / pOH formulas. Write down each formula and when you would use it:

2.) A student prepares a 0.80 M solution of potassium hydroxide.

Find the:

a) concentration of hydronium ions in solution

b) pH and pOH

c) the concentration of the hydroxide ions

3.) State whether the following are acids or bases:

Have a sour taste.

React with metals.

Release H+ ions in water

Feel slippery

Turn blue litmus paper red.

Release OH- ions in water

4.) Define acids and bases according to the Arrhenius theory & Brønsted-Lowry theory:

5.) Identify each substance as acid, base, conjugate acid, or conjugate base.

H2S + H2O HS – + H3O+

6. Give the conjugate acids of: NH3 and Br –.

7. Give the conjugate bases of: H3O+ and HSO4–.

8. Find the pH and pOH of 0.75M HCl.

9. Find the molarity of a KOH solution with a pH of 9.5

10. If 43.5 mL of 0.15 M HBr is required to neutralize 25.0 mL of NaOH, what is the molarity of the NaOH?

VOCAB: hydronium ion neutralization reaction

hydrogen ion hydroxide ion

titration equivalence point

strong/weak acid/base

DAY 8 - Reviewing Reference Tables, Kinetics, Equilibrium__________________________________________________________________

1.)Study the energy diagram below:

Is this reaction exothermic or endothermic?

How can you tell?

Draw a line indicating how a catalyst would affect the forward reaction.

The activation energy for the forward reaction is _____________________________

The activation energy for the reverse reaction is _____________________________

The heat of the reaction for the forward reaction is ___________________________

The change in enthalpy for the forward reaction is ___________________________

2.)Explain LeChatelier’s Principle:

3.) N2(g) + 3H2(g) <--> 2NH3 + 91.8 kJ

Explain what would happen to this system if you….

a. Increase the concentration of a product

b. Increase the concentration of a reactant

c. Add a catalyst

d. Increase the pressure of this system

e. Decrease the temperature of this system

DAY 9 - Redox Reactions, Practice Questions1.) Determine the oxidation states of each of the following compounds:

a) ammonium nitrate __________________________________

b) fluorine __________________________________

c) boron trichloride __________________________________

d) iron (III) phosphate __________________________________

e) nitric acid __________________________________

f) potassium carbonate __________________________________

g) dinitrogen tetrachloride __________________________________

2.) In each of the following reactions, determine what was oxidized and what was reduced:

Ca + H2O → CaO + H2Element Oxidized ___________________________

Element Reduced ___________________________

Oxidizing Agent ___________________________

Reducing Agent ___________________________

2 H2 + O2 → 2 H2OElement Oxidized ___________________________

Element Reduced ___________________________

Oxidizing Agent ___________________________

Reducing Agent ___________________________

Cu + 2 AgNO3 → 2 Ag + Cu(NO3)2Element Oxidized ___________________________

Element Reduced ___________________________

Oxidizing Agent ___________________________

Reducing Agent ___________________________

2 AgCl + Co → CoCl2 + 2AgElement Oxidized ___________________________

Element Reduced ___________________________

Oxidizing Agent ___________________________

Reducing Agent ___________________________

Mg + Ca(OH)2 → Ca + Mg(OH)2Element Oxidized ___________________________

Element Reduced ___________________________

Oxidizing Agent ___________________________

Reducing Agent ___________________________

Cu + Zn+2 → Zn + Cu+2

Element Oxidized ___________________________

Element Reduced ___________________________

Oxidizing Agent ___________________________

Reducing Agent ___________________________

3.) Give the oxidation state of each element in the following compounds:

Zn

Pb(NO3)2

Zn(NO3)2

HI

HIO4

H2SO4

CO

CO2

CO3-2

NH3

H2O

H2O2

NO3-

O2

N2

CH4

Other Important Things to Know/Remember:

What are the diatomic molecules?

What does STP mean? What values do they include?

What are the two gas laws equations you should know?

What are the formulas for methane, hydrochloric acid, sulfuric acid, and water vapor?

What are the charges on Al, Zn, and Ag ions, respectively?

What does a combustion equation ALWAYS look like?

What unit is molar mass given in?

What is the molar mass of water, carbon dioxide, oxygen gas, nitrogen gas, and hydrogen gas?

How do the solubility rules work? When do you use them?

What is the activity series for metals and halogens? When do you use them? What do they tell you?

How do you write an equilibrium expression for a reversible reaction?Find and write down a sample problem for this from your textbook.