CHAPTER 1-Chemistry-Matter-Elements-Atoms-Molecules-States of Matter (Gas/Liquid/Solid)-Pure Substance-Elements-Compounds-Mixtures-Law of Constant Composition (Law of Definite Proportions)-Solutions-Physical Properties-Chemical Properties-Intensive Properties-Extensive Properties-Physical Change-Chemical Change-Changes of State-Scientific Method-Hypothesis-Scientific Law-Theory-Metric System-SI Units-Mass-Celsius Scale-Kelvin Scale-Density-Accuracy-Precision-Significant Figures-Conversion Factor-Dimensional Analysis

1) Which of the following represents a chemical change?   (a) water boiling   (b) iodine subliming    (c) sugar dissolving in water   (d) natural gas burning    (e) ice melting

2) How many carbon atoms are contained in 4.2 g of C3H6?   (a) 1.8 x 10^23  (b) 9.0 x 10^23  (c) 6.0 x 10^23  (d) 1.8 x 10^24  (e) 6.0 x 10^24

3) A weighing tray has a mass of 9.11 g. 3.2 g of NaOH is added to this tray. The total mass of the tray and the NaOH should be recorded as:   (a) 4.1 g  (b) 4.11 g  (c) 4.111 g  (d) 4.100 g  (e) 4.10 g

4) A combination of sand, salt, and water is an example of a________.  (a) homogeneous mixture  (b) heterogeneous mixture  (c) compound  (d) pure substance  (c) solid

5) The law of constant composition says_________.  (a) that the composition of a compound is always the same  (b) that all substances have the same composition  (c) that the composition of an element is always the same  (d) that the composition of a homogeneous mixture is always the same  (e) that the composition of a heterogeneous mixture is always the same

1) Show all work and use the correct set up, units, and number of sig figs. Convert 32 mph to km/sec (1.6 km = 1 mile)

2) A solid white substance A is heated strongly in the absence of air. It decomposes to form a new white substance B and a gas C. The gas has exactly the same properties as the product obtained when carbon is burned in an excess of oxygen. Based on these observations, can you determine whether A and B and the gas C are elements or compounds? Explain your conclusions for each substance.

1. Which of the following is an example of a chemical change?a) Mixing Iron and Sulfur Powderb) Breaking Glassc) Formation of Cloudsd) Rotting of Fruit

2. If the high temperature for the day is predicted to reach 88 ˚F, what is the predicted temperature in ˚C?a) 304 ˚Cb) 31 ˚Cc) 159 ˚Cd) 67 ˚C

3. 1 Megameter is equal to how many meters?a) 10b) 1000c) 1000000d) 1000000000

4. Which is an example of a compound?a) Bronzeb) Silverc) Goldd) Platinum

5. Which is an example of an element?a) Earthb) Marsc) Mercuryd) Venus

Free Response Questions

1. A package of aluminum foil contains 50ft2 of foil, which weighs approximately 8.0 oz. Aluminum has a density of 2.70 g/cm3. What is the approximate thickness of the foil in millimeters?

2. (a) What is the difference between a hypothesis and a theory? (b) Explain the difference between a theory and a scientific law. Which addresses how matter behaves, and which addresses why it behaves that way?

Chapter 2:

AtomsSubatomic ParticlesDalton’s Atomic Theory of MatterLaw of Conservation of Mass/MatterLaw of Constant CompositionLaw of Multiple ProportionsCathode RaysRadioactivityNucleusProtons, Neutrons, ElectronsElectronic ChargeAtomic Mass Unit AngstromAtomic NumberMass NumberAtomic SymbolIsotopesAtomic WeightPeriodic TablePeriodsGroupsMetals/Metallic ElementsNonmetals/Nonmetallic ElementsMetalloidsMoleculeDiatomic MoleculeChemical FormulaMolecular CompoundsMolecular FormulasEmpirical FormulasStructural Formula IonCationAnionPolyatomic IonsIonic CompoundChemical NomenclatureOxyanionsAcidsBinary Molecular CompoundsOrganic ChemistryHydrocarbonsAlcoholAlkanes

1) The symbols 11H, 2

1H, 31H represent three different

(a) Homologs(b) Isotopes(c) Isomers(d) Allotropes(e) Conformations

2)An isotope has the atomic number of 8 and a mass number of 17. This element(a) Is an isotopic form of oxygen(b) Has 8 neutrons(c) Has 9 protons if it is in ionic form(d) Is an isotopic form of fluorine(e) Has 17 electrons 

3) Which of the following ions has the same number of electrons as Br-

(a) Ca+2

(b) K+

(c) Sr+2

(d) I-

(e) Cl-

4) For which of the following pairs are the atoms most likely to form an ionic compound?(a) Carbon and Oxygen(b) Calcium and Chlorine(c) Chlorine and Oxygen(d) Sodium and Magnesium (e) Chlorine and Neon

5) The discovery of the electron came from:(a) The gold foil experiment(b) Dalton’s Atomic Theory(c) The plum pudding model(d) Cathode ray experiments(e) The calculation of the mass/charge relationship

1) The element boron consists of two isotopes, 10B and 11B. Their masses, based on the carbon scale, are 10.01 and 11.01, respectively. The abundance of 10

5B is 20.0% and the abundance of 11

5B is 80.0%. What is the atomic mass of boron? 

2) What ionic compound is formed with the ions of Strontium (Sr) and Phosphorus (P) combined? Label which ion is the cation and which ion is the anion.

1. Nitrogen Gas is bubble through an aqueous solution of calcium Bromate. Besides water, this statement refers to which chemical formulas?A) N and CaBrO3

B) N2 and CaBrO4

C) N2 and CaBrO3

D) N and CaBrO3

E) N and Ca (BrO)3

2. Magnesium Nitride reacts with water to form ammonia and magnesium hydroxide. Besides water, this statement refers to which chemical formulas?A) Mg3N2 , NH3 , and Mg(OH)2

B) Mg(NO3)2 , NH4+ , and MgH2

C) Mg(NO3)2 , NH3 , and MgH2

D) Mg(NO2)2 , NH4+ , and Mg(OH)2

E) Mg3N2 , NH3 , and MgOH

3. Which of the following compounds contains four carbon atoms?A) PropaneB) Butanoic acidC) Ethyl methyl etherD) 2-pentanolE) Heptanal

4. Which is true of the 243Am3+ ion? Protons Electrons NeutronsA) 95 92 243B) 95 98 243C) 95 95 148D) 95 92 148E) 92 95 148

5. The correct name for the compound Cu3N is:A) Copper (III) NitrideB) Copper NitrogenC) Copper (II) NitrateD) Copper (I) NitrideE) Copper (III) Nitrate

1) Using the periodic table to guide you, predict the chemical formula and name of the compound formed by the following elements. (A) Ga and F (B) Li and H (C) AL and I (D) K and S

2) Predict wheather each of the following compounds is ionic or molecular.A) B2H6

B) CH3OHC) LiNO3

D) Sc2O3

E) CsBrF) NOCLG) NF3

H) Ag2SO4

Chapter 3

Stoichiometry-Mole RatioReactants-Products-Combination (Synthesis)Reaction-Single Replacement ReactionDouble Replacement reactionDecomposition Reaction-Combustion Reaction-Avagadro's Number-Mole-Limiting Reactant-Theoretical Yield-Precent Yield-Empirical Formula-Molecular Formula-

2. The percentage of oxygen in C8H12O2 is:a.(16/140)(100)b. (32/140)(100) c. (16/124)(100)d. (140/32)(100)e. (32/124)(100)

3. A compound contains 48% O, 40.0 % Ca, and the remainder is C. What is the empirical formula?

A) O3C2Ca2B) O3CCa2C) O3CCa     D) O3CCa2E) O2CCa

4. Given the unbalanced equation: Al + O2 = Al2O3 When this equation is completely balanced using the smallest whole numbers, what is the sum of the coefficients?A) 9  B) 7C) 5D) 4

5. What is the empirical formula of the compound whose molecular formula is P4O10?A) POB) PO2C) P2O5    D) P8O20

Balance the following equation

___C0 +___ H2 > ____ C8H18 + ______H2O

Combustion of 8.652 grams of a compound containing C, H, O, and N yields 11.088g CO2, 3.780 grams of H20 and 3.864 grams of NO2.

a. How many moles of C, H, and N are contained in the sample?

b. How many grams of Oxygen are contained in the sample?

c. What is the simplest formula of the compound?

d. If the molar mass of the compound lies between 200 and 300, what is its molecular formula?

e. Write and balance a chemical equation for the combustion of the compound.How many liters of hydrogen are  needed to react with 10 liters of nitrogen gas in the reaction forming ammonia?

2.)What is the total number of atoms in 0.260 mol of glucose?

1.)How many moles of Al are there in 2.16 mol of Al2O3?a. 2.16b. 1.08c. 4.32 d. 10.8

2.)What is the empirical formula of a compound whose molecular formula is P4O10?a. POb. PO2

3. P2O5

4. P8O20

3. What is the Percent by mass of oxygen in magnesium oxide, MgO?a. 20%b. 40% c. 50%d. 60%

4.)In the chemical equation _CH4+_Cl2--->_CCl4+_HCl, what are the correct coefficients?a. 0,4,0,4 b.4,8,4,2c.2,5,2,4d.1,5,2,3

5.)What is the mass in grams of 3.0 x 1023 molecules of CO2?a. 22 g b. 44 gc. 66 gd. 88 g

Chapter 4:

Aqueous Solutions• Solvent• Solutes• Dissociate • Dissolve• Electrolyte• Non-electrolyte• Strong Electrolyte• Weak Electrolyte• Solvation• Chemical Equilibrium• Precipitation Reactions• Precipitate• Solubility• Exchange/MetathesisReactions• Molecular Equation• Complete Ionic Equation• Spectator Ions• Net Ionic Equation• Acids• Bases• Strong Acids & Bases• Weak Acids & Bases• Neutralization Reaction• Oxidation Reduction (redox)Reaction (OIL RIG)• Oxidation• Reduction• Oxidation Number• Displacement Reactions• Activity Series• Concentration• Molarity (M)• Dilution• Titration• Standard Solution• Equivalence Point• Acid-Base Indicators

1. Consider the equation: Cl2(g)+2KI(aq )--> I2(s)+KCl(aq), which species was oxidized?a. Cl2b. K+c. I-d. I2e. Cl-

2. How many grams of NaOH are needed to prepare 500 mL of a 1.0M solution?a. 40 gramsb. 20 gramsc. 200 gramsd. 400 gramse. 12.5 grams

3. How many millimeters of 0.2M FeCl3 solution would be necessary to precipitate all of the Ag+ from 60mL of a 0.6M AgNO3 solution? (Hint: write a balanced equation)a. 10 mLb. 30 mLc. 60 mLd. 90 mLe. 180 mL

4. The definition of a precipitate reaction is:a. A reaction that results in a soluble productb. A reaction that results in an insoluble productc. A reaction where water is producedd. A reaction when an acid and a base are mixede. A reaction when electrons are transferred as reactants

5. What mass of KCl is needed to precipitate the silver ions from 15.0 mL of 0.200M AgNO3 solution?

a. 0.16 g KClb. 29 g KClc. 18 g KCld. 0.4456 g KCle. 0.227 g KCl

1. Label the following reactions with as many labels as possible (Synthesis, Decomposition, Single Replacement, Double Replacement, Redox, neutralization, precipitation)

a. Ca(OH)2(aq)+2HNO3 --> Ca(NO3)2(aq) + 2H20

b. Fe2O3(s)+3CO(g) --> 2Fe(s)+3CO2(g)

c. CuBr2(aq)+2NaOH(aq) --> Cu(OH)2(s)+NaBr(aq)

d. Cl2(g)+NaI(aq) --> I2(s)+2NaCl(aq)

2. HCl, HBr, and HI are strong acids, yet HF is a weak acid. What does this mean in terms of the event to which these substances are ionized in solution?

1. What is the concentration of a solution of HCL if 400 mL ofdistilled water is added to 10 mL of stock solution?a. 400. Mb. 410 Mc. 1.25 Md. 0.250 Me. 0.244 M

2. The difference between a strong acid and a weak acid is:a. A strong acid is more concentrated than a weak acidb. A weak acid is more soluble in water than a strong acidc. Strong acids have more hydrogens per molecule than weakacidsd. Weak acids cannot conduct electrical currents in solutione. Strong acids are more completely dissociated compared toweak acids

3. Which of the following species is reduced in the following netionicreaction:2HNO3(aq) + 3H3AsO3(aq) 2NO(g) + 3H3AsO4(aq) + H20(l)a. HNO3b. H3AsO3c. NOd. H3AsO4e. H2O

4. Which substance will not form a gas upon mixing with anaqueous acid?a. NaHCO3(s)b. CaS(s)c. Ca(s)d. K2SO3(s)e. Al2O3(s)

5. Which of the following is not a strong electrolyte:a. CH3CO2Hb. KClc. KNO3d. NaClO4

6. One commercial method used to peel potatoes is to soak them in a solution of NaOH for a short time, remove them from the NaOH and spray off the peal. The concentration of the NaOH is normally in the range of 3 to 6 M. The NaOH is analyzed periodically. In one such analysis, 45.7 mL of 0.500 M H2SO4 is required to neutralize a 20.0 mL sample of the NaOH solution. What is the concentration of the NaOH solution?

7. Write the net ionic equation for the precipitation reaction that occurs when solutions of calcium chloride and sodium carbonate are mixed.

The net ionic equation for the reaction between iron and copper (II) chloride is:A) Fe+CuCl2àCu+FeCl2

B) Fe+Cu2++2Cl-àCu+Fe2++2Cl-

C) Fe+Cu2+àCu+Fe2+

D) Fe2++CuCl2àCu2++FeCl2

E) Cu2++2Cl-àCuCl2

 If 53 grams of Na2Cl3 (Molar Mass 106g) are added to a 500 mL solution of 0.50 M NaCl solution, what will the resulting concentration of the Na+ ion be?A) 0.10 MB) 0.50 M C) 0.75 M D) 1.5 M E) 2.5 M 50.0 mL of 1.0 M CaCl2 were required to precipitate out all of the silver in a 100 mL solution of AgNO3 to create AgCl.

A) 0.10 MB) 0.50 MC) 1.0 MD) 2.5 ME) 5.0 M Which of the following species is reduced in the following net-ionic reaction?2HNO3(aq)+3H3AsO3(aq)à2NO(g)+3H3AsO4(aq)+H2O(l)

A) HNO3 B) H3AsO3 C) NO D) H3AsO4 E) H2O When copper chloride reacts with sodium sulfide the spectator ions are:A) Copper and Sulfide B) Sodium and Chloride C) Chloride and Sulfide D) No ions are spectators E) All 4 ions are spectators   1.  2M potassium hydroxide solution is titrated with a 0.1M nitric acid solution.Balanced Equation:What would be observed if the solution was titrated well past the equivalence point using bromthymol blue as the indicator? (Bromthymol blue is yellow in acidic solution and blue in basic solution.)  

2.  Propane is burned completely in excess oxygen gas.Balanced Equation:When the products of there action are bubbled through distilled water, is the resulting solution neutral, acidic, or basic? Explain.

Chapter 5Thermodynamics:Thermochemistry:Energy:

Work:Force:Heat:Kinetic Energy:Potential Energy:Joule:Calorie:System:Surroundings:First Law of Thermodynamics:Inertial Energy:Endothermic:Exothermic:State Function:Enthalpy:Enthalpy of Reaction:Calorimeter:Calorimetry:Heat Capacity:Specific Heat:Molar Heat Capacity:Bomb Calorimeter:Hess’s LawEnthalpy of Formation:Standard Enthalpy Change:Standard Enthalpy of Formation:

1) Which change will result in an increase in enthalpy of the system?a) Burning a candleb) Freezing waterc) Evaporating alcohold) Dropping a balle) Condensing steam

2) Given the following data, what is the heat of formation of methane gas?I. CH4+2O2CO2+2H2O H=-803kJII. H2+1/2O2H2O H=-242kJIII. C+O2CO2 H=-394kJIV. C+1/2O2CO H=-111kJ

a)-803kJ/molb)-75kJ/molc)+167kJ/mold)+208kJ/mole)-1439kJ/mol

3) Which of the following is endothermic?a) rusting ironb) making ice cubes

c) cooking an eggd) a candle flame

4) A 2.200g sample of quinone (C6H4O2) is burned in a bomb calorimeter whose total heat capacity is 7.854kJo/C. The temperature of the calorimeter increases from 23.44oC to 30.57oC. What is the heat of combustion per gram of quintone.a)-25.5 kJ/molb)-330 kJ/molc)44 kJ/mold)990 kJ/mol

5) Calculate the Kinetic energy in Joules of a 45g golf ball moving at 61 m/s.a)6966Jb)95Jc)84Jd)-990J

Free Response

1) What are the three laws of thermodynamics?1.

2.

3.

2) How much heat is released when 4.50g of methane gas is burned in a constant pressure system?

1) Energy is Measured in a) Degreesb) Joulesc) gramsd) liters

3) Calculate the work done on the system when 1.00 mol of gas held behind a piston expands irreversibly from a volume of 1.00 dm3 to a volume of 10.0 dm3 against an external pressure of 1.00 bar.

a) -5710 JB) -900 Jc) +1000 Jd) +9120 J

4) 1.00 mol of gas in a cylinder is compressed reversibly by increasing the pressure from 1.00 bar to 10.0 bar at a constant temperature of 500 K. Calculate the work done on the gas by the compression.A) +9570 Jb) +3740 Jc) +37.4 kJd) +5710 J

5) The temperature of a copper block of mass 423g rises by 10.1°C. Calculate the heat transferred, given that the specific heat capacity of copper is 385 J K-1 kg-1.a) 385 JB) 1.63 kJc) 1.10 kJd) 25.6 kJ

Free Response1) Imagine a book falling from a shelf. At a particular moment during its fall, the book has a kinetic energy of 13 J and a potential energy with respect to the floor of 72 J. How does the books kinetic and potential energy change as it continues to fall?

2) What is its total kinetic energy at the instant just before it strikes the floor?

 

1) What is the change in internal energy for the following? A system absorbs 45 kJ of heat and does 5 kJ of work to the surroundings.a. 45 kJb. -45 kJc. 40 kJd. 50 kJe. -50 kJ

2) The value of the change in heat for the reaction is -70 kJ.                            kJ of heat are released when 14 grams of hydrogen gas are completely reacted.a. 5 kJb. 10 kJ

c. 140 kJd. 490 kJe. 980 kJ

3) The temperature of a 10g sample of metal increase from 20°C to 30°C when 30 J of heat are added to it. The specific heat capacity of the metal is:a. 3.3 J/°Cb. 0.3 J/°Cc. 30 J/°Cd. 3.3 J/(g°C)e. 0.3 J/(g°C)

4) What is the molar heat of fusion of a substance that required 45 kJ to melt 38 grams of the substance? (the molar mass of the substance is 152 grams/mol)a. 11 kJb. 180 kJc. 90 kJd. 3 kJe. 6 kJ

5) Which of the following statements are true for the statment: "When a substance was dissolved in water, the temperature of the solution increased."

I. The process was endothermicII. The process is exothermic

III. The enthalpy of the process can be calculated by multiplying the temperature change and heat capacity of the system.

IV. The heat that caused the temperature change came from the surroundings.

a. Ib. IIc. I and IIId. II and IIIe. I,III, and IV

1) If a system absorbs 53 kJ of heat and does 3 kJ of work, what is the change in internal energy?

2) How much heat is released when 4.50 g of methane gas is burned in a constant pressure system?

Chapter 6

electronic structureWavelength λfrequency ν

AmplitutdeElectromagnetic radiation:Visible spectrumLine spectrum:Photon:A quantumThe speed of light =Planck’s constant =The uncertainty principle:Quantum numbers: Electrons of an atom represent the density of that atom and their place on the periodic table The Pauli Exclusion Principle:

Orbitals (S,P,D.F) Electron configuration:Paramagnetic:Diamagnetic: Ground state electron configuration:An excited state configuration:Electron shell:Subshell:Degenerate orbitals:Hund’s Rule (Bus seat rule):Valence electrons:Core electrons:

Quantum Number Principle Azimuthal Magnetic Spin

Symbol n l ml ms

Possible values 1, 2, 3, 4, 5… 0, 1, 2, 3…ns, p, d, f

-l, …0… +l + 1/2

Electron/ Orbital characteristic

size shape orientation Magnetic spin

  1.what is the maximum number of electrons that can fill the 5f subshell?        A.2   B.5   C.10.   D.14.   E.18

  2.a blue line in the atomic emission spectrum of hydrogen has a wavelength of 434nm. What is the energy of this light per mole of photon?     A. (10^6)(6.63)(3.00)(6.02)/(434) kJ/mol     B. (10^3)(6.63)(3.00)(6.02)/(434) kJ/mol     C. (10^6)(6.63)(3.00)(6.02)/(434) J/mol     D. (10^3)(6.63)(3.00)(6.02)/(434) J/mol     E. (10^3)(434)(6.02)/(6.63)(3.00) kJ/mol

  3.which set of quantum numbers is not allowed?     A.(2,2,1,1/2).   B.(3,2,0,-1/2).    C.(4,3,-3,1/2).   D.(5,3,-2,1/2).    E.(6,2,-1,1/2)

4.According to Heisenberg's uncertainty prunciple, if you know the position of the electron you won't know the...  A.speed.     B. shape of the orbital it's in.    C. Energy.   D. Momentum.      E. principle quantum number.

5. Wavelength and frequency are     A. Directly related.    B. proportional.     C. Inversely related.    D second cousins.    E.the same

1. An electromagnetic wave has a wavelength of 656nm. How much energy is there in a mole of photons?

2.. Write the Noble gas configuration of cobalt.

1.) What is the wavelength of light that has a frequency of 6.0×10∆14 Hz?

a. 2000nmb. 500nmc. 200nmd. 2.0×106 nme. 5.0×10-7 nm

2.) The outer most electron in a ground state potassium atom can be described by which of the following sets of four quantum numbers?

a. 4, 0, 0, ½b. 4, 1, 0, ½

c. 4, 1, 1, ½d. 5, 0, 0, ½e. 5, 1, 0, ½

3.) One type of sunburn occurs on exposure to UV light of wavelength in the vicinity of 325nm. What is the energy of a photon of this wavelength?

a. 6.11×10∆-19 J/photonb. 3.2×10∆-8 J/photonc. 680 KJ/photond. 12×6∆-19 KJ/photon

4.) Arrange the following types of electromagnetic radiation in order of increasing wavelength:

a. Radio waves < ultra violet< green light< red light<infrared< X-rays

b. Green light< red light< infrared< X-rays< radio waves< ultra violet

c. X-rays< ultra violet< green light< red light< infrared< radio waves

d. Red light< radio waves< infrared< green light< ultra violet< X-rays

5.) Gaseous atoms of which of the following elements are paramagnetic in their ground states?I. NaII. MgIII. AlIV. P

a. I, II, III, IVb. I, II, III onlyc. I, III, IV onlyd. II onlye. III, IV only

Which orbital is the biggest?a)1sb)3pc)3sd)4de)2f

The outermost electron in a ground state K atom can be described bywhich of the following sets of four quantum numbers?a)4,0,0,1/2b)4,1,0,1/2c)4,1,1,1/2

d)5,0,0,1/2e)5,1,0,1/2

What visible color has the longest wavelength?a)purple d)greenb)yellow e)bluec)red

Which wave would cause the most damage?a)microwavesb)infraredc)ultra-violetd)X rayse)gamma rays

How many orientations does a d orbital have?a)1b)2c)3d)4e)5

1) In a condensed electron configuration, what does the symbol [Xe] represent?

2) What is the ground state configuration of V?

3) If human height were quantized in one-foot increments, what would happen to the height of the child as she grows?

4) Explain how the existence of line spectra is consistent with Bohr’s theory of quantized energies for the electron in the hydrogen atom.

Chapter 7

noble gases force of attraction core electrons shielding effect

atomic radius nonmetals alkali metals halogens valence orbitals effective nuclear charge bonding atomic radius isoelectronic series ionization energy electron affinity metallic character

1) In general, as you go across a period in the periodic table from left to right the atomic radius:

a) Decreasesb) Increases c) Stays the same

2) In general, as you go across a period in the periodic table from left to right the electron affinity becomes: a) Increasingly negative b) Decreasingly negative c) Stays the same

3) The ion with the largest diameter is: a) Br- b) Cl- c) F- d) I-

4) In general, as you go across a period in the periodic table from left to right the first ionization energy: a) Stays the same b) Increases c) Decreases

5) How many unpaired electrons does Ni2+ contain when the electron configuration is written out?a) 1b) 2c) 4d) None

1) What is the general relationship between the size of an atom and its first ionization energy? Which element in the periodic table has the largest ionization energy? Which has the smallest?

2) Which will experience the greater effective nuclear charge, the electrons in the n = 3 shell in Ar or in the n = 3 shell in Kr? Which will be closer to the nucleus? Explain

1) Which list of elements is arranged in order of increasing atomic size (largest last)?A) Be, Mg, Ca, Sr, BaB) Ba, Sr, Ca, Mg, BcC) Be, Ca, Ba, Mg, SrD) Be, Ba, Ca, Mg, SrE) Ba, Sr, Ca, Be, Mg

2) Which sequence is arranged in order of increasing ionization energies, lowest to highest? A) Be, B, C, N, O B) B, Be, C, O, NC) Be, B, C, O, ND) B, Be, C, N, OE) O, N, C, B, Be

3) Electrons in the 1s subshell are much closer to the nucleus in Ar than in He due to the larger ______ in Ar. A) nuclear chargeB) paramagnetism C) diamagnetism D) Hund’s ruleE) azimuthal quantum number

4) ______ is isoelectronic with argon and _____ is isoelectronic with neon. A) Cl-, Cl+

B) F+, F-

C) Ne-, Kr+

D) Ne-, Ar+

E) Cl-,F-

5) In which set of elements would all members be expected to have very similar chemical properties?A) N, O, FB) Na, Mg, KC) O, S, SeD) S, Se, SiE) Ne, Na, Mg

1)A) What is meant by the term effective

nuclear charge?

B) How does the effective nuclear charge experienced by the valence electrons of an atom vary going from left to right across a period of the periodic table?

2) A) What is an isoelectronic series?

B) Which neutral atom is isoelectronic with each of the following ions: Al3+, Ti4+, Br-, Sn2+.

Chapter 8

Chemical bondsionic bondscovalent bondsmetallic bondsLewis symbol (Lewis dot structure)octet rulelattice energyelectron configurationsingle bonddouble bondtriple bondbond lengthbond polaritynonpolar covalent bondpolar covalent bondelectronegativitypolar moleculedipoledipole momentformal chargeresonance structuresvalence electronsbond enthalpy

Multiple Choice1. As the number of bonds increases, the bond

lengtha. decreasesb. increasesc. is not affected (stays the same)d. there is not enough information to

know

2. Of the molecules, which bond is most polar?a. HIb. HFc. H2d. HBre. none are polar

3. Which of the following elements will tolerate less than a full octet of electrons?

a. Ib. Nac. Bd. Oe. none of the above

4. Which pair of ions has the highest lattice energy?

a. Na+ and Br-

b. Li+ and F-c. Cs+ and F-d. Li+ and O2-e. K+ and F-

5. Resonance structures differ by:a. number and placement of electronsb. number and placement of atomsc. number of electrons onlyd. placement of atoms onlye. number of atoms onlyf. placement of electrons only

Free Response1. Draw the Lewis structures for IF6+ and Sulfur

Trioxide

2. Find the enthalpy change for the following reaction:

C3H8 (g) + 5 O2 (g) 3 CO2 (g) + 4 H2O (g)

H-C 413H-O 463C-C 348C=C 614O-O 146C-O 358C=O 799O=O 495

Chapter 9

Bond angles

VSEPRBonding pairElectron domainNonbonding pair (or lone pair)Electron-domain geometry

LinearTrigonal planarTetrahedralTrigonal BipyramidalOctahedral

Molecular geometryLinearTrigonal planarBentTetrahedralTrigonal pyramidalTrigonal BipyramidalSee sawT-ShapedOctahedralSquare pyramidalSquare planar

Bond dipolePolar vs. nonpolar molecules Valence-bond theoryHybrid orbitalsHybridizationSigma bondsPi bondDelocalized

The electron domain and molecular geometry of BrO2

- is __________.A)  tetrahedral, trigonal planarB)  trigonal planar, trigonal planarC)  trigonal pyramidal, linearD)  tetrahedral, bentE)  trigonal pyramidal, seesaw

The hybridizations of nitrogen in NF3 and NH3 are _________ and _________, respectively.A)  sp2, sp2

B)  sp, sp3

C)  sp3, spD)  sp3,sp3

E)  sp2, sp3

PCl5 has _________ electron domains and a ________ molecular arrangement.A)  6, trigonal bipyramidalB)  6, tetrahedralC)  5, square pyramidalD)  5, trigonal bipyramidalE)  6, seesaw

Which set does not contain a linear species?A)  CO2, SO2, NO2

B)  H2O, HCN, BeI2 

C)  OCN-, C2H2, OF2

D)  I3-, BrF3, SCN-

E)  H2S, ClO2-, NH2

-

What is the best estimate of the H-O-H bond angle in H3O+?A)  109.5ºB)  107ºC)  104.5ºD)  116ºE)  120º

Free Response Questions

An AB3 molecule is described as having a trigonal bipyramidal electron-domain geometry.  How many nonbonding domains are on atom A? Explain.

Why are there no sp4 or sp5 hybrid orbitals?

Chapter 10atmospheretorr

mm HgBoyle's LawCharles's LawUnnamed RelationshipCombined Gas LawAvogadro's HypothesisAvogadro's LawIdeal Gas EquationIdeal GasStandard Temp. and PressureDalton's Law of Partial PressuresMole FractionKinetic-molecular TheoryRoot mean square speedEffusionDiffusionGraham's Lawmean fee pathvan der Waal's equationDeviation from ideal behaviorSTPCollected over water (Partial Pressures)   1.Suppose you are given 2 1-L flasks and told that one contains a gas of molar mass 30, the other a gas of molar mass 60, both at the same temperature. The pressure in flask A is X atm, and the mass of the gas is 1.2g. The pressure in flask B is .5X atm and the mass is 1.2g. Which flask contains the gas of molar mass 60? 

What properties of gases can you point to that support the assumption that most of the volume in a gas is empty space?

1. Under which of the following conditions will a 1-L sample of Kr gas act the most ideal?a. .1 atm and 273 Kb. 1.0 atm and 273 K

c. 10 atm and 400 Kd. .1 atm and 400Ke. 1.0 atm and 400 K

2. Which of the following gases is most likely to act ideally under STP?a. Krb. CCl4c. Hed. O2e. N2

3. Which increases when a gas is heated at constant volume?I. PressureII. Kinetic energy of moleculesIII. Attractive forces between moleculesa. I onlyb. II onlyc. III onlyd. I and II onlye. I and III only

4. Effusion is:a. The spread of a substance from a high concentration to low concentrationb. The spread of a substance through a tiny holec. The macroscopic behavior of gases at the atomic and molecular leveld. The ease at which an atom gains an electron

5. What is the conversion factor between atm and torr? mmHg and torr?a. 1 atm = 765 torr, 1mmHg =1 torrb. 1 mmHg =700 torrc. 2 atm = 760 torr, 1 mmHg = 760 torrd. 1 atm = 760 torr, 760 mmHg = 760 torr