Look+Here!

Test 14: What to study?

 * 1) This test will include concepts covering electrochemistry (the role of electrons in reactions) and nuclear chemistry. 25 multiple choice questions will cover mostly electrochemistry and nuclear with a few questions to review pH and acids/bases. 2 points each.
 * 2) The driving force of a oxidation-reduction (redox) reaction is the transfer of electrons.
 * 3) Some metals are more likely to lose electrons than others. They oxidize easily.
 * 4) Electrons are lost during oxidation; electrons are gained during reduction. // LEO says GER. //
 * 5) Substances (which include metals) that are oxidized are also known as reducing agents.
 * 6) Substances (which include metals) that are reduced are also known as oxidizing agents.
 * 7) Redox reactions containing ions can be balanced by using the half reaction method.
 * 8) Batteries utilize the transfer of electrons to produce electric current.
 * 9) Electodes are poles on a battery where current leaves and enters the battery.
 * 10) There are two types of electrodes: the anode and the cathode.
 * 11) Oxidation takes place at the anode and reduction takes place at the cathode.
 * 12) Electrolytes are used in batteries to provide a medium for the ions to move through.
 * 13) Corrosion takes place when metals return to their natural state.
 * 14) There are several ways to slow or prevent corrosion: paint, a primer coating containing zinc, the formation of a natural oxide coating and cathodic protection--which uses reducing agent such as magnesium.
 * 15) Make sure you know how to explain how lead acid storage, alkaline dry cell and NiCad batteries work. You are also expected to know the reaction for the battery and be able to explain how each battery works.
 * 16) Voltaic/galvanic cells can be constructed by using two metals with a difference in electrode potentials.
 * 17) When designing a voltaic cell, the metal with the higher electrode potential will serve as the cathode. The other metal will act as the anode where oxidation takes place.
 * 18) The two half cells in a voltaic cell are often connected by a porous barrier, porous plug or salt bridge.
 * 19) The potential of a cell can be calculated the following way. E = Cathode - Anode (as used in the text).
 * 20) Be able to determine the oxidation states of compounds. For example, in carbon dioxide, carbon is +4 and oxygen is -2.
 * 21) Nuclear chemistry is the study of the nucleus.
 * 22) Atoms in nuclear chemistry are known as nuclides.
 * 23) Nuclides are often identified by their isotopes. An example is carbon-14.
 * 24) Nuclides undergo decay by producing alpha particals (helium nuclei) and beta particals (electrons).
 * 25) Nuclear decay takes place to make nuclides more stable. A stable neutron to proton ratio for larger nuclides is 1.5:1. Nuclear decay will take place until this ratio is met. The band of stability lies within a n:p ratio of 1:1 to 1.5:1.
 * 26) Nuclear fission involves the splitting of nuclides (the atom bomb). Fusion involves the fusion of two smaller nuclides (the sun).
 * 27) Nuclear reactors use fission to produce heat which in turn will heat up water to turn turbines (which produce electricity).
 * 28) Breeder reactors produce additional fissionable fuel.
 * 29) RBMK reactors are Soviet-style reactors which use control rods. Control rods absorb neutrons.
 * 30) U.S.-style reactors use water to control their reactors.
 * 31) Moderating rods are used to moderate the rate of the nuclear reaction.
 * 32) Fuel rods contain uranium fuel.
 * 33) A half life is the amount of time needed for half of the original sample to remain. For example: if the half life of sample X is 6.0 hours you have 10 grams of sample X, only 5 grams will remain after 6.0 hours, and only 2.5 grams after 12.0 hours (two half lives).
 * 34) Know the penetrating abilities of the following types of radiation (from highest to lowest): gamma, beta, alpha.

//** GO LAKERS!!! **//

L-level classes: Which metal was used to protect the nail in my in-class cathodic protection demo? K-level classes: Which solution (name or formula) was used in my in-class cathodic protection demo? Good Luck!
 * Thanks for checking out the website.** **//There will be a 2 polano max on this test. Polanos cannot be defaced or torn.// For an extra credit point on this test, you must take the original test on Monday, May 18. Answer this question on your colored sheet.**



Test 13: What to study?

 * 1) There will be 25 multiple choice questions and questions on your "colored" paper. The multiple choice questions will come from chapter 19 (no questions form the past).
 * 2) Know 4-5 properties of acids and bases.
 * 3) What is pH? What is pOH?
 * 4) What is the value for Kw?
 * 5) How is Kw used to find [H3O+]? How is it used to find [OH-]?
 * 6) Remember that pH + pOH = 14.00.
 * 7) If...[H3O+] > [OH-] = acidic; then [H3O+] < [OH-]: basic; and [H3O+] = [OH-]: neutral
 * 8) The number of decimal places used for pH/pOH = the number of significant figures used in the concentration of the acid/base.
 * 9) Be sure to know how to find conjugate acids and bases. HNO3 is a strong acid and will produce a weak conjugate base, (NO3-).
 * 10) Strong acids fully dissociate, producing the maximum amount of hydronium ions possible. Therefore the concentration of the acid is the same as the concentration of hydronium ions.
 * 11) Strong bases fully dissociate, producing the maxiumum amount of hydroxide ions possible. Therefore the concentration of the base is the same as the concetration of the hydroxide ions.
 * 12) Be sure that you are able to name acids. No oxygen, use "hydro-ic acid". For example: HF is hydrofluoric acid. For an acid with oxygen, do not use "hydro". Remember **-ate to -ic**; **-ite to -ous**. For example: HNO3 has nitrate (-ate to -ic), so it is named nitric acid. Another example: HNO2 has nitrite (-ite to -ous), so it is named nitrous acid.
 * 13) Be sure to know how to solve for a titration (neutralization) problem such as those found on WS 11-4. They are stoichiometry problems so make sure to balance the equation first. Remember that molarity is equal to moles/liter!
 * 14) You will also need to be able to solve for problems using Ka. These are used for weak acids. It is important to know how to determine the [H3O+] by using Ka and its corresoponding equilibrium expression.


 * Thanks for checking out the website.** **//There will be a 2 polano max on this test. Polanos cannot be defaced or torn.//

For an extra credit point on this test, you must take the original test on Wednesday, April 22. Answer this question on your colored sheet.** L-level classes: Which indicator gives a different color for each pH level? K-level classes: What is the active ingredient in TUMS? Write the formula.

Test 12: What to study?
> an equation and correctly write the equilibrium expression. Show all work or no credit!
 * 1) There will be 30 multiple choice questions and seven to nine questions on your "colored" paper. Some of the questions on the colored paper will be statements that have been used in class. The rest will be problems like the ones worked on in class.
 * 2) Most of the multiple choice questions will come from previous tests. Make sure to review your old review sheets.
 * 3) Equilibrium is a dynamic state--it is constantly moving and changing. These reactions are reversible as indicated by the "double arrow".
 * 4) Be able to
 * 1) K = [products]/[reactants]
 * 2) When writing a K//eq// expression, do not include reactants or products that are in the liquid or solid states.
 * 3) Recall that the coefficients found in the balanced equation will be written as powers in the equilibrium expression.
 * 4) A large K indicates that equilibrium favors the right side of the equation (products). A small K means that equilibrium lies toward the left side of the equation (reactants).
 * 5) Most of the time, atmospheres are used to measure concentrations of gases. Moles/liter can also be used.
 * 6) In performing a K//sp// problem, do not include solids in the expression. Be sure to balance your equation and notice the mole ratios.
 * 7) You may be asked to solve for K//sp//, which means that you will have to convert the solubility from grams/liter to moles/liter. Use this solubility as your "x" in the expression.
 * 8) If you have an equation such as PbI2 (s) --> Pb +2 (aq) + 2I- (aq), don't forget to double the concentration for the iodide ion (and then square it).
 * 9) Le Chatelier's Principle states that if a system at equilibrium is disturbed, the system wil shift in a direction that will relieve the stress.
 * 10) There are three factors that can cause a shift in equilibrium: pressure, concentration and temperature.
 * 11) Review intermolcular forces.
 * 12) Review vapor pressure.
 * 13) What is meant by polar versus nonpolar?
 * 14) Review boiling, evaporation, vaporization, sublimation, etc.,.
 * 15) Review enthalpy (delta H), entropy (delta S) and Gibbs free energy (delta G).
 * 16) Review the reaction pathways.


 * Thanks for checking out the website.** **//There will be a 2 polano max on this test. Polanos cannot be defaced or torn.//

For an extra credit point on this test, you must take the original test on Monday, April 13. Answer this question on your colored sheet. These questions are from the demo performed on Thursday, April 9:** If you are in period 2, answer this question: What color would the solution be if it was acidic? If you are in period 3, answer this question: Which acid was used? If you are in period 4, answer this question: Which base was used? If you are in period 5, answer this question: Which indicator solution was used? If you are in period 6, answer this question: What color would the solution be if it was basic? Good Luck!

Test 11: What to study?

 * 1) One calorie = 4.184 joules
 * 2) One **C**alorie = 1000 calories (one nutritional **C**alorie = 1 kcal). Notice the C is capitalized. Don't expect to see **C**alorie on the test.
 * 3) Know about specific heat and heat capacity.
 * 4) Know how to use: q = m*c*deltaT
 * 5) Each substance has its own value for "c". See page 492.
 * 6) Heat is the transfer of energy.
 * 7) Temperature is a measure of the average kinetic energy found in a sample of particles.
 * 8) Know about: the //heat of formation//, the //heat of combustion// and the //heat of reaction//.
 * 9) Enthalpy cannot be measure directly. One can measure the //change// in enthalpy.
 * 10) Negative delta H = exothermic reaction.
 * 11) Positive delta H = endothermic reaction.
 * 12) Most reactions in nature tend toward disorder.
 * 13) Entropy is the measure of disorder in the universe.
 * 14) Positive delta S = disorder.
 * 15) Negative delta S = order.
 * 16) Gibbs Free Energy is a function of of delta H and delta S.
 * 17) Free energy is used to determine reaction spontaneity.
 * 18) Positive delta G = nonspontaneous.
 * 19) Negative delta G = spontaneous.
 * 20) Reactions are affected by the nature of the reactants, the concentration of the reactants, temperature, the surface area of the reactants and the presence of reactants.
 * 21) The collision theory is used to explain how reactions take place. Reactions require enough energy to break the old bonds in addition to the proper orientation of the reactants.
 * 22) Be sure to know and understand the reaction pathway diagrams for exothermic and endothermic reactions.
 * 23) The slowest step is the rate-determining step.
 * 24) A rate law includes the concentrations of reactants that influence the reaction rate.
 * 25) **K-level:** Make sure that you look over the problems assigned on Page 881-882 (1-10). These problems are fair game for your test.

Test 10: What to study?

 * 1) This test will have 42 multiple choice/matching questions, much of it review questions from Test 9. Problems: one on solving molarity, one on solving liters of solution using molarity, one on boiling point elevation/freezing point depression, one dilution problem, one question requiring you to complete the equation of a double replacement (PPT) reaction along with its overall ionic and net ionic equations and one "essay" question on types of electrolytes. You may also be asked to solve for molality and another question asking for net ionic equations (like your PPT lab).
 * 2) Know the three measures of concentation discussed in class: molarity, molality and percent concentration (by mass).
 * 3) Molarity = moles of solute / liters of solution (M =mol/L)
 * 4) Molality = moles of solute / kg of solvent (//m// = mol / kg)
 * 5) % concentration (by mass) = mass of solute / mass of solution x 100% (% conc. = mass/mass x 100%)
 * 6) If sucrose (a sugar) is nonpolar, why does it dissolve in water?
 * 7) What are spectator ions?
 * 8) What is a colligative property? What affects colligative properties? (see page 471)
 * 9) What determines how much high a boiling point will be elevated? Or how much lower the freezing point will be lowered?
 * 10) For L-level, be able to find the molarity of a solution. For K-level, know how to find molarity and the molarity of ions present in solution (look at WS 10-3).
 * 11) Be sure to know the differences between the terms saturated, unsaturated and supersaturated.
 * 12) Be able to identify whter a compound will be soluble or insoluble in water (i.e.: NaCl is soluble).
 * 13) What is the Kinetic Molecular Theory?
 * 14) What are the differences between boiling, evaporation and vaporization?
 * 15) What are intermolecular forces? Know the three discussed in class (hydrogen, dipole-dipole, London dispersion forces).
 * 16) Be able to determine which molecular force is present within a given substance.
 * 17) Why are intermolecular forces inportant in terms of state of matter?
 * 18) What is surface tension? Adhesion? Cohesion?
 * 19) Why does water have such a high boiling point (compared to other liquids)?
 * 20) How is it possible to make water boil at room temperature?
 * 21) FYI--Nonpolar molecules are typically covalently bonded (i.e., carbon disulfide).
 * 22) What is the temperature of a solid water/liquid water mixture? Assume 1 atm of pressure.
 * 23) What is the temperature of a liquid water/gaseous water mixture? Assume 1 atm of pressure.
 * 24) How does evaporation occur? What is happening on the molecular level?
 * 25) What can be said of two liquids' attractive forces if they have different vapor pressures?
 * 26) What is equilibrium?
 * 27) Which substance will have a lower vapor pressure, ethanol or methanol? Why?
 * 28) What must be present in a solution for it to conduct electricity?
 * 29) What will happen to the amount of water vapor in a sealed bottle if the temperature was increased?
 * 30) Remember:"like dissolves like". Polar dissolves polar. Nonpolar dissolves nonpolar.
 * 31) What is a solute? What is a solvent? What is a solution?
 * 32) Be able to explain how intermolecular forces govern the boiling points of certain substances.

Shh...Want an credit point on this test? The fine print...To be eligible, you must take the original test (this offer does not apply to make-up tests).**
 * Thanks for checking out the website. //There will be a 2 polano max on this test.//

If you are taking the L-level test, answer this question by placing the answer above your name on your blue problems sheet: Write the formula for sucrose.

If you are taking the K-level test, answer this question placing the answer above your name on your purple problems sheet: What is the the theoretical freezing point depression from the demo on March 4th's class?

Test 9: What to study?

 * 1) What is the Kinetic Molecular Theory?
 * 2) What are the differences between boiling, evaporation and vaporization?
 * 3) What are intermolecular forces? Know the three discussed in class (hydrogen, dipole-dipole, London dispersion forces).
 * 4) Be able to determine which molecular force is present within a given substance.
 * 5) Why are intermolecular forces inportant in terms of state of matter?
 * 6) What is surface tension? Adhesion? Cohesion?
 * 7) Know the 5 types of solids discussed in class: molecular, covalent network, ionic, metallic, and amorphous. Be able to identify examples on the test. Also be able to explain the properties of each type of solid. Study up on Table 13-4 (page 402).
 * 8) Why does water have such a high boiling point (compared to ther liquids)?
 * 9) How is it possible to make water boil at room temperature?
 * 10) FYI--Nonpolar molecules are typically covalently bonded (i.e., carbon disulfide).
 * 11) What is the temperature of a solid water/liquid water mixture? Assume 1 atm of pressure.
 * 12) What is the temperature of a liquid water/gaseous water mixture? Assume 1 atm of pressure.
 * 13) How does evaporation occur? What is happening on the molecular level?
 * 14) What can be said of two liquids' attractive forces if they have different vapor pressures?
 * 15) What is equilibrium?
 * 16) Which substance will have a lower vapor pressure, ethanol or methanol? Why?
 * 17) What must be present in a solution for it to conduct electricity?
 * 18) What will happen to the amount of water vapor in a sealed bottle if the temperature was increased?
 * 19) Why do liquids diffuse more slowly than gases?
 * 20) What would happen to our planet's water supply if water was nonpolar?
 * 21) What happens to the solubility of a gas (in a soda bottle) if the temperature was increased?
 * 22) What is Henry's Law?
 * 23) What determines the solubility of a particular solute?
 * 24) What is the Tyndall Effect? Which type of mixture exhibits the Tyndall Effect?
 * 25) Remember:"like dissolves like". Polar dissolves polar. Nonpolar dissolves nonpolar.
 * 26) What is a solute? What is a solvent? What is a solution?
 * 27) What can be done to speed up the dissolving process?
 * 28) Molarity is moles of solute / liters of solution. (M = mol/L).
 * 29) Be able to solve for the molar heat of fusion/vaporization. (Q=n*Hf; Q=n*Hv)
 * 30) Be able to solve an ideal gas problem. Be able to change pressures and temperatures.
 * 31) Be able to explain how intermolecular forces govern the boiling points of certain substances.
 * 32) If you were in class on 2/16: study the powerpoint presented in class, it will help! If not, study what is listed above.

Shh...Want two extra credit points on this test? The fine print...To be eligible, you must in the class (this offer does not apply to make-up tests).**
 * Thanks for checking out the website.

If you are taking the L-level test, answer this question by placing the answer above your name on your blue problems sheet: Which salt is/was to be used in our solubility lab?

If you are taking the K-level test, answer this question by according to the version you get during the test by placing the answer above your name on your purple problems sheet: If you get version A: Which liquid substance was demonstrated in class to have a higher vapor pressure than that of water? Give the specific name. If you get version B: Which element was the coil used in the "superheated steam demo" made of?

Test 8: What to study?

 * 1) What is the Kinetic Molecular Theory?
 * 2) What is pressure?
 * 3) What are the units for pressure?
 * 4) What is a barometer? How does it work?
 * 5) Know the gas laws discussed in class: Boyle's Law, Charles' Law, Gay-Lussac's Law, Combined Gas Law, Dalton's Law of Partial Pressures, Avogadro's Law, Ideal Gas Law, and Graham's Law.
 * 6) At STP (273 K, 101.3 kPa), 1 mole of any gas = 22.4 liters.
 * 7) What is an ideal gas? What is a real gas?
 * 8) What is water vapor pressure? How can it be determined?
 * 9) Be able to perform a gas stiochiometry calculation (like your lab).
 * 10) Be ready to solve for Boyle's Law and Charles' Law. Also expect to see problems involving STP, Dalton's Law of Partial Pressures, the Ideal Gas Law and Graham's Law of Effusion. These problems may vary between L-level and K-levels tests.
 * 11) Stuff from previous tests...
 * 12) Know which atoms have the smallest atomic radius.
 * 13) Know the shapes of common ions.
 * 14) Know how to balance a combustion reaction.
 * 15) Be able how to identify different types of reactions.
 * 16) Be able to name a compound from it's formula.
 * 17) The famous experiments!

Shh...Want to earn two extra credit points on this test? The fine print...To be eligible, you must in the class (this offer does not apply to make-up tests).**
 * Thanks for checking out the website.

If you are taking the L-level test, answer this question by placing the answer above your name on your blue problems sheet: The artificial lung demo demonstrated which gas law?

If you are taking the K-level test, answer this question by according to the version you get during the test by placing the answer above your name on your purple problems sheet: If you get version A: How many atmospheres of pressure will a scuba diver experience at a depth of 20 meters? If you get version B: How many atmospheres of pressure will a scuba diver experience at a depth of 40 meters?

Test 7: What to study?

 * 1) What is stoichiometry?
 * 2) How do you determine a mole ratio?
 * 3) The steps for solving a stoichiometry problem: (1) balance the equation, (2) change from grams to moles, (3) use mole ratios, and (4) change from moles to grams.
 * 4) You can also use Humna's technique: [[file:Humna's stoichiometry formula.doc]]
 * 5) Remember that molar mass is the mass of one mole of a substance: i.e., one mole of water is 18.02 grams/mol.
 * 6) Percent yield = (actual yield / theoretical yield) x 100%. Actual yield can be determined experimentally. Theoretical yield can be determined mathematically (stoichiometry). It is possible to have a yield greater than 100%. The unit for percent yield is %.
 * 7) A limiting reactant limits the amount of product that can be made. The limiting reactant is entirely spent in a chemical reaction. The reactant that is left over is called the excess reactant. The amount of product made is dependent on the amount of the limiting reactant present.
 * 8) Determining the limiting reactant is done so by finding what you "have" and "need" as instructed in class.
 * 9) TEST FORMAT: 30 mult. choice (all review questions), and 4 problems. The first two problems will be worth 25 points each. You are expected to be able to balance each equation and perform a stoichiometry calculation. The last two problems will include a percent yield calculation and a limiting reactant problem (10 points each).
 * 10) No other problems from previous tests will be on Test 7, but you should know the following:
 * 11) Know the clues that a chemical reaction has taken place.
 * 12) What must remain unchanged during a chemical reaction?
 * 13) Know the CRT and Gold Foil experiments.
 * 14) What happens to the ions not involved in a precipitate reaction?
 * 15) Know the shapes of some common ions (such as nitrate, sulfate and phosphate)?
 * 16) Know the differences between ions, isomers and isotopes.
 * 17) Given the percent compositions of elements in a compound, be able to solve for the emprical and molecular formulas.
 * 18) What is meant by the term "soluble"?
 * 19) What if an extra-terrestrial visitor showed you a periodic table with elements similar to our own table? Be able to determine the correct formula.
 * 20) Be able to balance chemical equations.
 * 21) Know how to identify types of reactions (i.e., synthesis, decomposition, etc.,).
 * 22) Know how to properly name compounds if given a formula. Know how to properly write a formula given the compound's name.
 * 23) **//FIGHT ON!  (+2 points) //**

Test 6: What to study?

 * 1) What are the four clues that a reaction has taken place?
 * 2) On which side of a chemical equation will you find the reactants? Products?
 * 3) What do the symbols (s), (l), (g), and (aq) represent?
 * 4) Why must chemical equations be balanced?
 * 5) What does the Law of Conservation of Mass (Matter) state? The number of atoms must be the same on both the reactant and product sides of the chemical equation.
 * 6) Know the 5 major types of reactions: synthesis, decomposition, combustion, single replacement and double replacement.
 * 7) Know that there are two types of double replacement reactions: acid-base and precipitate.
 * 8) Be sure to understand how to use the solubility rules found on Page 920.
 * 9) Be aware of the activity series and how it is used. (Which metal is more reactive? Aluminum or copper? Iron or copper? Zinc or copper?) Activity series table is found on page 288. Also see the download section of this site to see a downloadable file of the activity series.
 * 10) Know the four types of "exception" decomposition reactions. (Chlorates, carbonates, hydroxides and acids).
 * 11) Know the method for balancing combustion reactions in which the hydrocarbon has an even number of carbons.
 * 12) Know the four driving forces of reactions: the formation of water, formation of a gas, formation of a solid, and the transfer of electrons.
 * 13) Be able to successfully identify the type of reaction, determine the products and properly balance a chemical equation (worksheets 6-6 to 6-10).
 * 14) You will be given "data" from a experiment, similar to that of the lab performed during this unit. Be able to calculate and determine the correct empirical formula.
 * 15) Be sure to study previous review sheets!
 * 16) Review chemical nomenclature.
 * 17) Be able to calculate and solve for molecular formula.
 * 18) Know how to write a noble gas configuration.
 * 19) Be able to draw a Lewis structure, determine the shape and indicate whether the structure exhibits resonance.
 * 20) Given the number of protons and neutrons of hypothetical atoms, be able to determine which pairs of atoms are isotopes.
 * 21) Know the bond angles of molecules (VSEPR).
 * 22) Know "Gold foil experiment".
 * 23) Be able to look at a diagram of atoms and determine the reaction's chemical equation.
 * 24) Remember: the last group on the periodic table represents the noble gases (charge of 0).
 * 25) Be able to identify the shape of s and p orbitals. Be able to distinguish between s and p orbitals of different energy levels.
 * 26) Be able to determine the number or neutrons of an isotope (i.e., oxygen-15).
 * 27) Review the orbital diagram rules: aufbau, Hund's and Pauli.
 * 28) The probability map for an electron is called a(n).
 * 29) How are elements ordered in the modern periodic table?
 * 30) What is the energy required to remove an electron from an atom also known as?
 * 31) //Problems to include: naming, completing chemical equations and balancing, Lewis structures and shapes, a noble gas configuration, a lab problem, and a molecular formula problem. This will account for 60 points on the test.//

Good Luck and **// FIGHT ON, beat the Bruins! //**

Test 5: What to study?

 * 1) Know how to name binary compounds (Type I, Type II, and Type III).
 * 2) What are the oxidation states (charges) for Aluminum, Zinc and Silver?
 * 3) Know how to name compounds with polyatomic ions (i.e., silver nitrate, iron (II) phosphate). //**Page 224:** **Memorize them!**//
 * 4) Know how to name acids (binary: hydrochloric acid; and oxyacids: sulfuric acid).
 * 5) What is molar mass? How can you determine the molar mass of a compound (i.e.: NaCl)?
 * 6) Be able to solve for percent composition. [(Total mass of an element in compound / molar mass) x 100%)]
 * 7) Know how to find the empirical formula of a compound (given % composition). [% -> g -> mol -> ratios -> empirical formula]
 * 8) Know how to determine the molecular formula of a compound (given the empirical formula). [molecular molar mass / empirical mass = ratio. ratio x empirical formula = molecular formula. For example if x = 6, then 6(CH2O) = C6 H12 O6]
 * 9) Be sure to study previous review sheets!
 * 10) What are "bonds"
 * 11) What are the differences in bond length for a single, double and triple bond?
 * 12) Which bond is strongest: single, double or triple?
 * 13) Which type of bond holds together atoms within a polyatomic ion?
 * 14) What are isomers? What are ions? What are isotopes?
 * 15) What is VSEPR?
 * 16) Be able to give an example for each molecular shape.
 * 17) Of all the molecular shapes, which do not follow the octet rule?
 * 18) Be able to distinguish from a list of molecules, which one exhibits resonance.
 * 19) Why are the bond angles of trigonal pyramids less than that of tetrahedrons?
 * 20) Be able to explain the difference in covalent, ionic and metallic bonding (and the properties of each).
 * 21) Go over material from previous tests!
 * 22) Know how to solve for density.
 * 23) Know how to write a noble gas configuration.
 * 24) Know how to calculate moles from atoms or grams.
 * 25) Know how to calculate mass from atoms.
 * 26) Know the periodic trends (ionization energy, atomic radii, etc.,).
 * 27) How are s and p orbitals shaped?
 * 28) Know the aufbau principle, Hund's rule and the Pauli exclusion principle!
 * 29) What is frequency?
 * 30) Which colors of photons have the most energy? The least?
 * 31) Be able to determine which orbital designations are possible.
 * 32) Orbitals are probability maps.
 * 33) Gold Foil, CRT, and the scientists!
 * 34) Be able to calculate the number of neutrons in an isotope (i.e., oxygen-15).
 * 35) //Problems to include: three Lewis structures and "shapes"; two noble gas configurations; ten names/formulas; one percent composition problem; one empirical formula problem; and one molecular formula problem. This section is worth 60 points.//

Test 4: What to study?

 * 1) What are "bonds"?
 * 2) What are the differences between ionic, covalent and polar covalent bonds?
 * 3) What must happen for an ionic bond to form?
 * 4) Which elements are typically involved in ionic bonds?
 * 5) Which elements are typically found in covalent bonds?
 * 6) How are electronegativity values used to determine types of bonds? (Use Page 169)
 * 7) What is polarity? How can it be determined?
 * 8) What is the octet rule?
 * 9) What is a Lewis dot structure? Draw the structure for water.
 * 10) What are the differences in bond length for a single, double and triple bond?
 * 11) Which bond is strongest: single, double or triple?
 * 12) Which type of bond holds together atoms within a polyatomic ion?
 * 13) What are isomers? What are ions? What are isotopes?
 * 14) What is VSEPR?
 * 15) Be able to give an example for each molecular shape.
 * 16) Of all the molecular shapes, which do not follow the octet rule?
 * 17) Be able to distinguish from a list of molecules, which one exhibits resonance.
 * 18) Why are the bond angles of trigonal pyramids less than that of tetrahedrons?
 * 19) Be able to explain the difference in covalent, ionic and metallic bonding (and the properties of each).
 * 20) Go over material from previous tests!
 * 21) Know how to solve for density.
 * 22) Know how to write a noble gas configuration.
 * 23) Know how to calculate moles from atoms or grams.
 * 24) Know how to calculate mass from atoms.
 * 25) Know the periodic trends (ionization energy, atomic radii, etc.,).
 * 26) How are s and p orbitals shaped?
 * 27) Know the aufbau principle, Hund's rule and the Pauli exclusion principle!
 * 28) What is frequency?
 * 29) Which colors of photons have the most energy? The least?
 * 30) Be able to determine which orbital designations are possible.
 * 31) Orbitals are probability maps.
 * 32) Gold Foil, CRT, and the scientists!
 * 33) Be able to calculate the number of neutrons in an isotope (i.e., carbon-14).


 * [[image:Cation.jpg width="256" height="256" caption="Courtesy of: http://people.wcsu.edu/nigroa/chem_100.htm"]] ||
 * Courtesy of: http://people.wcsu.edu/nigroa/chem_100.htm ||

Test 3: What to study?

 * 1) What are ions? Why must an element become an ion?
 * 2) Be able to determine the charge of an ion based on the number of electrons present.
 * 3) What determines the chemical similarities within a chemical family?
 * 4) What is the role of valence electrons in relation to the reactivity of an element?
 * 5) What is continuous spectra?
 * 6) What is emission spectra? What does an element's emission spectra represent?
 * 7) What causes emission spectra?
 * 8) For which elements were emission spectra observed during class (with your spectroscopes)?
 * 9) If you were to compare several photons (red, blue, violet), which would have the highest energy?
 * 10) What is the difference between an electron's ground state and its excited state?
 * 11) What is the value for Planck's constant?
 * 12) What is frequency? Wavelength?
 * 13) How do determine the energy of a photon? Be able to solve for it.
 * 14) What is the range (in nanometers) for visible light?
 * 15) How is the wave theory of light related to the photoelectric effect?
 * 16) Be able to explain the Bohr model of the hydrogen atom. What was wrong with his model and which parts of his model are accepted today?
 * 17) What is an electron configuration? What is an orbital?
 * 18) How are s, p, d, and f orbitals different? In which energy levels would you expect to find each?
 * 19) Be able to identify orbital (s, p, d, f) if pictured on the test.
 * 20) What is the maximum number of electrons that can occupy an orbital (box)?
 * 21) Know how to draw an orbital diagram (boxes), be able to write an electron configuration (1s2, 2s2,...), and be able to write a noble gas configuration (i.e., [Ar] 4s2).
 * 22) Be able to write the electron configuration for ions.
 * 23) Be able to apply the three rules of configurations: aufbau, Pauli and Hunds.
 * 24) What are the four quantum numbers? What can be determined by each number?
 * 25) If the principal quantum number is 2, determine the possible angular momentum values. ( //answer// = 0, 1 or s and p).
 * 26) Be sure to know the four periodic trends discussed in class (atomic radius, ionic radius, ionization energy and electronegativity). What happens to each as you move across a period? What happens to each as you move down a group.
 * 27) From previous tests...know the major experiments, the important people discussed in class, the chemical families and groups.
 * 28) Be able to change from grams to moles / moles to grams / atoms to grams...
 * 29) Be able to solve for density.


 * Test 2: What to study?**
 * 1) Chemical and physical properties. Know how to identify them.
 * 2) Chemical and physical changes. How can you tell which one has happened?
 * 3) What is matter?
 * 4) How to solve for density? (D = m/v). What is volume by displacement?
 * 5) Know examples of elements, compounds and mixtures.
 * 6) How do you know when to distill a mixture? When would you filter a mixture?
 * 7) What are some examples of pure substances?
 * 8) Who were the six people discussed in class? What were their contributions?
 * 9) Know about the Cathode Ray Tube experiment. What was the outcome?
 * 10) Know about the Gold Foil experiment. What was the outcome?
 * 11) What is the atomic number of an element? What does this number represent?
 * 12) What does the average atomic mass of an element represent?
 * 13) How do you determine the number of protons, neutrons and electrons in an element's atom?
 * 14) Which parts of Dalton's atomic theory are not accepted in modern atomic theory? Why?
 * 15) What are groups? What are periods?
 * 16) Which family is represented by group 1? Group 2? Groups 3 - 12? Group 17? Group 18?
 * 17) What is a mole? What is avogadro's number?
 * 18) What is molar mass? What is the molar mass of carbon?
 * 19) How is molar mass different than atomic mass? How are they similar?
 * 20) Compare and contrast the three states of matter discussed in class.

Mass - Mole - Atoms Conversions > [|<< First] > > [|< Previous] [|Next >] [|Last >>]
 * Convert from grams to moles, divide the mass by the element's molar mass
 * To convert from moles to atoms, multiply the number of moles by Avogadro's number (6.022 E23)
 * To convert from atoms to moles, divide the number of atoms by Avogadro's number (6.022 E23)
 * To convert from moles to grams, multiply the number of moles by the element's molar mass.