Warm Ups 2016-2017.

Warm Ups

Layout of Your Warm ups Number each Warm Up
No more than two Warm-ups per page Include the problem and the answer Show all work for math problems

1 If you have been heating glassware, how should you pick it up?
What do you do if there is an accident in the lab? Long hair should always be ___________ ________ in the laboratory. Never leave a lit Bunsen burner __________. _________________ shoes are recommended in the lab.

2 When should you wear goggles in the lab?
If a chemical splashes on your skin, what should you do? What should you do with unused chemicals? How should you handle glass that you have been heating? Should all chemicals be considered dangerous in the lab?

3 explain what went wrong in these lab situations
Diana and Mike were going to be late to their next class. After rushing to put away a few materials, they left the rest of the materials on the lab table. The teacher was not in the room yet. Jake began weighing chemicals, touching them with his hands. His nose itched, so he rubbed it. Cindy broke a test tube. Carefully she picked up pieces with one hand and placed them in her other hand. Then she dumped the glass pieces into the wastebasket.

4 label each as a chemical or physical change
Liquid water freezing Gasoline burning Cooking an egg If 2 clear liquids are mixed and small clumps fall to the bottom of the container. A cube of orange colored sugar is dissolved into water resulting in an orange liquid.

Lab directions Follow all directions
Finish on time – if you are done early, clean up and work on lab questions Leave your lab area exactly as you found it! Homework is on the front desk – just do the front page

5 Make 2 qualitative observations about the picture.

6 List the 3 of the 6 state changes.
How do you change matter from one state to another? Is changing states a physical or chemical change?

7 A Bunsen burner mixes what two substances together?
What colors are a gas flame? What laboratory tool is used to light a Bunsen burner? Name 2 branches of Chemistry.

8 Sketch the heating curve of water. Label all the state changes.
Where are there two states coexisting?

9 What happens to temperature as a substance changes from one state to another? Temperature is the measure of ________________. What is the difference between an element and a compound? Compare homogeneous and heterogeneous mixtures.

10 What types of mixtures exhibit the Tyndall effect?
What are the two main types of heterogeneous mixtures? What part of a solution is the solvent? What is an alloy? Why is water considered the “universal solvent”?

11 What is the solubility of KCl at 60o C?
If you have 130 g of KNO3 at 40o C is it saturated, unsaturated, or supersaturated? If you start with a saturated solution of NaCl at 50o C and then cool it to 20o C, how much material will precipitate out?

12 Determine whether the following are chemical or physical changes:
What is the main factor used to distinguish between the different kinds of mixtures? Determine whether the following are chemical or physical changes: Paper burning Paper tearing A metal and gas combining to form a white crystal Water boiling CO2 subliming to form a gas Sugar dissolving in water

13 List 5 physical and 5 chemical properties of water.
Using your qualitative observation skills, name 5 ways to determine the difference between a banana and a ham sandwich. Try to think of properties that can be used to tell any banana from any ham sandwich.

14 Classify each of the following as a(n): element, compound, homogeneous mixture, heterogeneous mixture Oatmeal Silicon dioxide Lemonade Chicken noodle soup Xenon Carbon monoxide Salt water

When you finish your lab
Turn off your Hot Plate (do NOT get rid of the Zn and ZnCl2) Clean up your lab space and finish your lab questions Study for your test (retake tickets!)

15 Classify each of the following as a physical or chemical change
Salt dissolves in water Grass grows A nail rusts A rock is split Determine the state change Water is placed out in winter (up north) Ice forms on the outside a liquid nitrogen container What is KMT?

16 how many significant figures in each of the following?
8.01 80.1 80 8001 0.0081

17 How many significant figures do the following number have: 0.004
3.854 5004 56.02 58.00 100.0 1000

18 perform the operation and answer with the correct significant digits
= 4.328 x =

19 use dimensional analysis to solve
14 centuries to years $3.50 to quarters 900 cm to meters

20 convert the following 104 km = _______ m 198 g = _______ kg
6.3 cm = _____ mm 45oC = _____

21 How many grams in 1 mol of the following: Ga Pt Ba
How many moles in the following 102.91g of Rh 265.82g Cs 8.00g O

22 6.95 x 1023 atoms Zn  g 2.99 moles Li  g 8.94 moles N  atoms

23 6.34 mol Sr  atoms 9.04 g H  atoms What is the density of an object that has a mass of 8.56 g and a volume of mL? What is the mass of an object that has a density of g/cm3 and a volume of 3.25 cm3?

24 How many significant figures? 90.001
Round to 3 significant figures – Calculate. Show the intermediate steps. (7.843 x 6.34) = Convert using dimensional analysis: 143.2m  in Convert  364K = oC A piece of wood that measures 3.0 cm by 6.0 cm by 4.0 cm has a mass of 80.0 grams. What is the density of the wood? Would the piece of wood float in water? (volume = L x W x H)

When you are finished with your quiz
Make sure you have included your version on your paper! Turn in your quiz Get a Test Review and a Lab paper Begin the lab If you have time, find the density of multiple samples. Please return each sample you have measured to the box in the front of the room as you are finished.

25 How many grams does 0.500 moles of Br weigh?
If a doctor finds that his patient has a mass of 65 kilograms, how heavy is the patient in grams? How many weeks are there in 34 hours? How hot is 4500 C in Kelvin? 349 cm cm cm =

26 Who was the first person to describe “atoms”?
Name 3 more scientists who added to Atomic Theory. Describe “plum pudding” model of the atom and how it was developed. Who discovered the nucleus? What experiment did he use?

29 A radio station broadcasts at a frequency of 5.90 x 105 Hz. What is the wavelength of the radio waves? Electrons have properties of both _____ and _____. Wavelength and frequency are _____ related.

30 What is average atomic mass of Lithium if 7.42% exists as 6Li (6.015 amu) and 92.58% exists as 7Li (7.016 amu)? _____ was the first person to suggest the existence of atmos. The law of conservation of mass states that mass is not ____ nor ____ in chemical reactions. There are ____ postulates to Dalton’s Atomic Theory. ____ discovered the electron. _____discovered the nucleus.

31 Magnesium occurs in nature in three isotopic forms:
24Mg (78.70% abundance) amu 26Mg (11.17% abundance) amu 25Mg (10.13% abundance) amu Calculate the atomic mass of Magnesium from this data

32 Calculate the energy of light that has a frequency of 1.5 x 1015 Hz. A photon has the energy of 1.78 x J, calculate its frequency.

33 What is the Orbital Configuration of: C P Zn As

34 What is the Electron Configuration of: C P Zn As

35 What is the Nobel Gas Configuration of: C P Zn As

36 The _______ ______ number gives the main energy level.
The ______ ______ number gives the shape of the sublevel. The ________ number gives the orientation around the nucleus. The _____ number gives the direction an electron is traveling. Complete the electron configuration of S using noble gas notation.

37 What is the difference between Meneleev’s Periodic Table and modern Periodic Table? What is the Octet rule and what are valence electrons? Name the major groups of the PT Give all three types of electron configurations for Cl.

38 Explain Hund’s rule. Explain the Aufbau principle.
Explain the Pauli Exclusion principle. How many electrons are in an atom with ending electron configuration 4d6? What element has an electron configuration that ends in 3p5?

39 __________ is the father of the modern periodic table.
The original periodic table was arranged by atomic ________. What parts of Dalton’s theory were proven false? How many p+, n0, and e- in 34S-2?

40 Put the following elements in order from least to greatest atomic radius: V, Ga, Br, K Why is water considered the “universal solvent”? Convert 42.2km to miles if 2.54cm=1in and 5280ft=1mi What is the electron configuration for B?

41 How many electrons would each of the following have to gain or lose to become stable while forming an ion? What ion would they form? Na Mg Al Si P Cl Ar

42 What kind of an ion is K+? How many electrons has Br- gained or lost? What is the noble gas configuration of O-2? How many valence electrons does Nitrogen have? What type of bond does Na – Cl form?

43 What is the most common ion formed by the following: Ca N Ga I
What is the relationship between length of the bond and bond energy? How are ionic bonds formed? How are covalent bonds formed?

44 Name the shape of the following: SeF2 AsI3 SiF4 OBr6 NH4+ NF5

45 Draw a Lewis Dot diagram for the following
Ca Kr Name the shape of the following, are they polar or nonpolar? CH4 H2O NH3

46 Longer bonds are ______ and have _______ bond energy than shorter bonds. Covalent bonds are formed by the _______ of electrons. A cation has a ______ charge. The 3 Intermolecular Forces are… Put them in order of increasing strength. The greater the IMF the ____________ the melting point and boiling point. What force gives water it’s unique properties? What shape will be formed by the following: NF5 CCl4 BaF2

47 Name 3 properties of ionic and covalent compounds
How many p+, n0, and e- in 40K+? What is KMT?

48 Write the formula for the following ionic compounds:
Lithium phosphide Calcium bromide Boron nitride Indium sulfide Name the following ionic compounds: Al2S3 K2O Li2O CaBr2

49 Give the name for the following compounds: KBr Mn2O3 S2O3 CrSO3
Give the formula for the following compounds: lithium oxide Vanadium IV oxide Aluminum hydrogen carbonate Iron III cyanide

50 Give the formula for the following compounds:
Give the name for the following compounds: CoBr3 Zn3P2 CuSO3 LiNO2 Give the formula for the following compounds: Sodium hydroxide Manganese IV carbonate Potassium cyanide Lead IV oxide

51 Give the formula for the following compounds:
Give the name for the following compounds: KBr Mn2O3 S2O3 CrSO3 Give the formula for the following compounds: Dinitrogen monoxide Dihydrogen monoxide Vanadium V hydrogen carbonate Iron III oxide

52 Give the name for the following compounds: Be(NO2)2 H3PO4 SiO2 PCl3
H2SO3 Zn(ClO3)2 Give the formula for the following compounds: Dinitrogen trioxide Nitric acid carbonic acid Dicarbon tetrabromide Ammonium cyanide Hydroflouric acid

52 answers Give the name for the following compounds:
Be(NO2)2 Berillium nitrite H3PO4 Phosphoric Acid SiO2 Silicon dioxide PCl3 Phosphorous trichloride H2SO3 Sulfurous Acid Zn(ClO3)2 Zinc II chlorate Give the formula for the following compounds: Dinitrogen trioxide N2O3 Nitric acid HNO3 carbonic acid H2CO3 Dicarbon tetrabromide C2Br4 Ammonium cyanide NH4CN Hydroflouric acid HF

53 Give the name for the following compounds: AuBr H2SO4 N2O3 Fe(OH)3
CS2 Give the formula for the following compounds: Vanadium II Phosphite Sulfur hexachloride Hydrosulfuric acid Aluminum hydroxide Tetraphosphorus trisulfide

53 answers Give the name for the following compounds:
AuBr Gold I Bromide H2SO4 Sulfuric Acid N2O3 Dinitrogen trioxode Fe(OH)3 iron III hydroxide CS2 carbon disulfide Give the formula for the following compounds: Vanadium II Phosphite V3(PO3)2 Sulfur hexachloride SCl6 Hydrosulfuric acid H2S Aluminum hydroxide Al(OH)3 Tetraphosphorus trisulfide P4S3

54 Name the following compounds NF3 P2O5 HF S4N2 H3PO4
Give the formula for the following compounds sulfurous acid dinitrogen trisulfide phosphorus pentabromide hydrobromic acid dicarbon hexachloride

55 Wavelength and frequency are _____ related.
Light reflected from a green leaf has a frequency of 6.12x1014 Hz what’s its wavelength? 15.34g B=____ mol B 2.92 x 1023 atoms F =______g F 2.19mol C=________gC

56 find the molar mass and then convert
79.85g Fe2O3 = ________ moles 3.01×1024 formula units (NH4)2SO4 = __________ g 2.00 mol of ScCl3 =___________ g

57 find the molar mass and then convert
302.7 g of ScCl3 =___________ moles 23 moles of H2O = ____________ molecules

58 find the molar mass and the % composition
NaOH (NH4)2S

59 find the molar mass and the % composition
MnBr2•4H2O

59 What’s the empirical formula of a molecule containing
65.5% carbon, 5.5% hydrogen, and 29.0% oxygen?

60 find the empirical formula of the following compound
63.5% Ag, 8.2% N, 28.3% O

61 Find the molecular formula: A compound with empirical formula C2HCl that has a molar mass of 302g/mol

62 An unknown compound is found to contain 47.0% K, 14.5% C, and 38.5% O. What is the empirical formula? If the experimental molar mass is g/mol, what is the molecular formula? Find the molecular formula: A compound with empirical formula C6H8O that has a molar mass of 290g/mol

63 A compound containing 5.93% H and 94.07% O has an experimental molar mass of g/mol. What is the empirical formula and the molecular formula of the compound? Find the molar mass and the percent composition of NaBr How many moles are in 5.55g of CO2?

64 The law of conservation of mass states that mass is not ____ nor ____ in chemical reactions. ________ is the father of modern atomic theory. ____ discovered the electron. _____discovered the nucleus. Name: CaC03:________________________; MnCl2:__________________; N2O2:________________ Write formulas for: aluminum chloride:_________;oxygen difluoride:_______; nickel III nitrate:___________

65 Hydrocarbons are organic compounds made of ____ & ____?
What is an allotrope. What is the molecular formula of an alkane that has 17 C? What is the name of C7H16? C generally makes _____ bonds.

66 C forms _____ covalent bonds.
_______ are hydrocarbons that only have single bonds. _______ are hydrocarbons that have at least one double bond. _______ are hydrocarbons that have at least one triple bond. Draw 4 isomers of C9H20.

67 What is the electron configuration of Si?
How many valence electrons does S have? CH2-CH3 CH3-CH2-C-CH2-CH CH3 CH2-CH3 CH3-CH-CH-CH2-CH-CH2-CH CH CH3 3,5-diethyl 4-propyl octane

68 skip

69 How many p+, n0, and e- are in: 136C:______________ 4521Sc:_____________2412Mg+2:_____________ What would you do to a gas to make it a plasma? What’s the wavelength of violet light with frequency of 4.26x1014 Hz? Determine energy (in joules) of a photon w/ frequency of 6.55x1017Hz. Draw the structure and give the VSEPR shape of SiCl4. Draw the structure and give the VSEPR shape of NH3.

71 Name 3 Chemical and 3 Physical properties of matter.
What is the orbital configuration of oxygen? How does the electronegativity trend on the periodic table? Round to 2 significant figures.

72 NH4OH: ____ N, ____ H, _____O __C +__O2 →__CO : ___C___, ___O___
Determine the number of each kind of atoms for the following: NH4OH: ____ N, ____ H, _____O __C +__O2 →__CO : ___C___, ___O___

73 Balance each equation __Al +__Fe2O3 →__Fe +__Al2O3 __C +__O2 →__CO
__NH4OH +__FeCl3 → __Fe(OH)3 +__NH4Cl

74 Classify each reaction as synthesis, decomposition, single displacement, double displacement, or combustion. 2Al + Fe2O3 → 2Fe + Al2O3 2C + O2 → 2CO 3NH4OH + FeCl3 → Fe(OH)3 + 3NH4Cl

75 Balance and classify each reaction as synthesis, decomposition, single displacement, double displacement, or combustion. ___Al + ___HCl → ___H2 + ___AlCl3 __BaS + __ PtF2 → __ BaF2 + __ PtS __C5H12 + __O2 → CO2 + __H2O

76 Balance and classify the following reactions: ____N2 + ___H2O  ___NH4NO2 ____ NaBr + ____ H3PO4 → ____ Na3PO4 + ____ HBr When sodium metal reacts with iron (II) chloride, iron metal and sodium chloride are formed.

77 ____ Ag2SO4 + ____ NaNO3 → ____ Na +____ CaCO3 →
Predict the products of the following reactions: ____ Ag2SO4 + ____ NaNO3 → ____ Na +____ CaCO3 →

78 ____ LiOH + ____ Fe(NO3)3 → Calcium iodide + heat 
If needed, write the formulas for the reactants. Then determine the type of reaction and write the formulas for the products. Finally, balance the equations. If required, use the activity series the determine if the reaction will occur. 1) ____ C2H2 + ____ O2 → ____ LiOH + ____ Fe(NO3)3 → Calcium iodide + heat  Aluminum + oxygen 

79 Complete the following conversions. 76.37g CaCl2=______ mol CaCl2
After the correct formula for a reactant in an equation has been written, the a. subscripts are adjusted to balance the equation. b. formula should not be changed. c. same formula must appear as the product. d. symbols in the formula must not appear on the product side of the equation. Which equation is NOT balanced? a) 2H2 + O2  2H2O b) H2 + H2 + O2  H2O + H2O c) 4H2 + 2O2  4H2O d) 2H2 + O2  H2O 79 Complete the following conversions. 76.37g CaCl2=______ mol CaCl2 28.36g H2O = ______molecules H2O

80 2P(s) + 3Cl2(g) → 2PCl3(g) Using the equation above, how many mol PCl3 can be made from 4.1mol Cl2? Using the equation above, how many mol PCl3 can be made from 0.12mol P? Using the equation above, how many mol Cl2 are required to make 10mol PCl3? Using the equation above how many mol Cl2 are needed to completely react 12.9mol P?

81 C10H8 + 12 O2 → 10 CO2 + 4 H2O Use the equation above to answer the following questions. How many mol H2O can be made from 4.12mol O2? How many mol O2 are used to completely react 24.81mol C10H8? How many mol CO2 are produced when 6.10mol O2 are consumed?

81 C10H8 + 12 O2 → 10 CO2 + 4 H2O Use the equation above to answer the following questions. How many g H2O can be made from 4.12mol O2? How many mol O2 are used to completely react g C10H8? How many mol CO2 are produced when 61.00g O2 are consumed?

82 2CO + O2→ 2CO2 Use the above equation to complete the following calculations. How many mol CO2 can be made from 3.10mol O2? How many g O2 are needed to produce 23.19g CO2? How many mol O2 are needed to completely react 5.81mol CO? How many moles CO2 can be produced from 21.76mol CO? How many g O2 are needed to completely react 3.19g CO2?

82 2CO + O2→ 2CO2 How many mol CO2 can be made from 3.10mol O2?
Use the above equation to complete the following calculations. How many mol CO2 can be made from 3.10mol O2? How many g O2 are needed to produce 23.19g CO2? How many g O2 are needed to completely react 5.81mol CO? How many g CO2 can be produced from 21.7g CO? How many mol O2 are needed to completely react 3.19g CO2?

Al + 6HCl  3H2 + 2AlCl3 How many g AlCl3 can be produced from 29.57g Al? How many g HCl are required to produce 17.28g H2? How many mol HCl are needed to completely react 3.12mol Al? How many moles H2 can be made from 2.01mol HCl?

Al + 6HCl  3H2 + 2AlCl3 How many g AlCl3 can be produced from 29.57g Al? How many g HCl are required to produce 17.28g H2? How many mol HCl are needed to completely react 3.12g Al? How many grams H2 can be made from mol HCl?

84 8 Fe + S8 → 8 FeS How many mol FeS can be made from 3.12mol S8?
How many g S8 are required to produce 27.00g FeS? How many g FeS can be produced from 9.25g Fe? How many mol FeS can be produced from 9.25mol Fe?

84 8 Fe + S8 → 8 FeS How many mol FeS can be made from 3.12mol S8?
How many g S8 are required to produce 27.00g FeS? How many g FeS can be produced from 9.25mol Fe? How many molecules FeS can be produced from 9.25g Fe?

Al + 3H2SO4 → Al2(SO4)3 + 3H2 How many g H2 can be made from 13.00g H2SO4? How many mol Al are needed to completely react with 6.18mol H2SO4? How many g H2 can be made from 6.18g Al? How many mol Al are needed to make 6.18mol Al2(SO4)3?

Al + 3H2SO4 → Al2(SO4)3 + 3H2 How many g H2 can be made from 13.00g H2SO4? How many g Al are needed to completely react with 6.18mol H2SO4? How many mol H2 can be made from 6.18g Al? How many mol Al are needed to make 6.18mol Al2(SO4)3?

86 CuCl2 + 2 NaNO3 → Cu(NO3)2 + 2 NaCl If 15.0 grams of copper (II) chloride react with 20.0 grams of sodium nitrate, (a) what is the limiting reactant, (b) what is the theoretical yield of sodium chloride, and (c) how much of the excess reactant remains?

87 4P+5O2P4O10 If 35.25g P reacts with 35.25g O2, find (a) the limiting reactant (b) the theoretical yield of P4O10 (c) and how much of the excess reactant remains?

88 3 NH4NO3 + Na3PO4 → (NH4)3PO4 + 3 NaNO3 Assuming we started with 30.0 grams of ammonium nitrate and 50.0 grams of sodium phosphate, what is the a) limiting reactant, b) theoretical yield of sodium nitrate, c) amount of excess reactant?

89 Mg + 2 HNO3 → Mg(NO3)2 + H2 If I start this reaction with 40. grams of magnesium and an excess of nitric acid, how many grams of hydrogen gas will I produce? If 1.7 grams of hydrogen is actually produced, what was my percent yield of hydrogen?

90 4P+5O2P4O10 If 35.25g P reacts with 35.25g O2 and 59.40g P4O10 is produced, find (a) the limiting reactant (b) the theoretical yield (c)how much of the excess reactant remains (d) the percent yield.

91 Fe + 3 NaBr → FeBr3 + 3 Na Find the actual yield of Na if the theoretical yield is 34.82g Na and the % yield is 87.38%. What is the actual yield of FeBr3 if g NaBr completely reacts and the reaction has a 91.30% yield?

92 2 HgO → 2Hg + O2 What volume of O2 can be produced from the decomposition of g HgO according to the following equation? (DO2=1.43g/L)

CO(g) + O2(g)→ 2CO2(g) If the density of O2 = 1.428g/L, how many L of O2 are needed to make 9.10mol CO2? If the density of O2 = 1.428g/L and the density of CO2= 1.977g/L, how many L of CO2 can be produced from 7.91g O2? What volume of CO measured at STP is needed to make 8.27 mol CO2?

Al + 3H2SO4 → Al2(SO4)3 + 3H2 If 43.23g Al reacts with 41.98g H2SO4 and 0.71g H2 is created, find (a)the limiting reactant (b)the theoretical yield (c) how much of the excess reactant remains (d)the % yield.

95 5kL =_____mL What is the charge of the compound MgCl2?
What parts of Dalton’s Theory were proven false? What happens when an e- goes from ground state to excited state? Who discovered the e-? What did we learn from Rutherford? Where are the metalloids found on the periodic table? What is the charge of the compound MgCl2? Compare 1H t0 3H. What block does [Xe]6s24f145d106p1 belong to? Motion of ______ causes London dispersion or Van der Waals forces. What is the shape of a compound with a triple bond? What causes a water molecule to be bent? What is the VSEPR shape of BCl3?

96 4.56 bar = ____mmHg 32.85 psi = ____ kPa 775.3 torr = _____ Pa
1atm=760.mmHg= kPa=760.torr=1.0bar=14.7psi=101325Pa 4.56 bar = ____mmHg 32.85 psi = ____ kPa 775.3 torr = _____ Pa 5.64 bar = ____ atm

97 List the 6 properties of gases.
1atm=760.mmHg= kPa=760.torr=1.0bar=14.7psi=101325Pa mmHg = ______ atm kPa = ______ torr

98 If I have 5.6 liters of gas in a piston at a pressure of 1.5 atm and compress the gas until its volume is 4.8 L, what will the new pressure inside the piston be? If I have 45 liters of helium in a balloon at 250 C and increase the temperature of the balloon to 550 C, what will the new volume of the balloon be? A toy balloon has an internal pressure of 1.05 atm and a volume of 5.0 L. If the temperature where the balloon is released is 250 C, what will happen to the volume when the balloon rises to an altitude where the pressure is atm and the temperature is -150 C? Draw the Lewis structures for methane, CH4, and ammonia, NH3. What are their VSEPR shapes?

99 I’ve got a car with an internal volume of 12,000 L. If I drive my car into the river and it implodes, what will be the volume of the gas when the pressure goes from 1.0 atm to 1.4 atm? The volume of a gas is 25.3mL at 25.5oC and 0.56atm. What will the volume be at 15.2oC and atm? What is the Nobel Gas configuration of Uranium?

100 I have 130 liters of gas in a piston at a temperature of 2750 C. If I cool the gas until the volume decreases to 85 liters, what will temperature of the gas be? A mixture of oxygen, hydrogen and nitrogen gases has a total pressure of 12.4 atm. If the partial pressure of H2 is 5.2 atm and the partial pressure of N2 is 1.3 atm, what is the partial of the O2? How do these properties trend on the periodic table? Atomic Radii Electonegetivity Ionization Energy

101 The volume of a gas is 25.3mL at 25.5oC and 0.56atm. What will the volume be at 15.2oC and 0.932atm? How many moles of Oxygen are there in 15.3L at 23oC and 1.05 atm? If I have a mixture of Cl2, N2, and Ne and the total pressure is 4.5atm with the partial pressure of Cl2 1.34atm and the partial pressure of Ne 0.543atm, what is the partial pressure of N2? Find the percent composition of CuBr2.

102 What mass of oxygen gas occupies 3.17L at a pressure of 1.0atm and temperature 30.0⁰C? A cylinder contains samples of hydrogen, oxygen, and neon gases. If the total pressure in the cylinder is 2.0atm. the hydrogen gas has a pressure of 1.1 atm, and the neon gas has a pressure of 0.3 atm, what is the pressure of the oxygen gas? What is the Celsius temperature of 39.37g Ne that has a volume of 2.74L at 0.651atm. V1=831mL, P1=219kPa, V2=376mL, P2=?kPa

103 According to Kinetic Molecular Theory(KMT):
Gas particles are small and very ___ _____ in relation to their size. There is no _______ between gas particles. Gas particles are in constant, rapid, random _______. There is no energy lost in collisions b/c collisions are _____. Average kinetic energy is _______ to temperature (K). If pressure ↑ , volume _____. If temperature ↑, volume _______. If temperature ↓, pressure ______. V & T are (directly/inversley) related. V & P are (directly/inversley) related. P & T are (directly/inversley) related.

104 What pressure in kPa is exerted by 2.5L CO2 at 400.0K that has a mass of 35.0g. What is the mass of 12.5L SO2 that has a pressure of 1.2atm at 12°C? If the total pressure of a container is 932mmHg, and the container contains H2O vapor, xenon gas with a pressure of 115mmHg and nitrogen gas with a pressure of 297mmHg, what is the pressure of the H2O vapor? An unknown gas is collected over H2O at 30⁰C If the atmospheric pressure is 780.0mmHg, what is the pressure of the unknown gas?

C6H O2 → 12CO2 + 14H2O According to the above equation, if all measurements are made at the same temperature and pressure, how many liters CO2 can be made from 34.10L O2? According to the above equation, how many liters CO2 at -20.0⁰C and 1.05atm pressure can be made from 12.5L O2 measured at STP? According to the above equation, how many g C6H14 can be made from 3.18L CO2 at ⁰C and 1.29atm? If the CO2 is collected over water at 25.0 ⁰C when the barometer reads 765.0mmHg, what is the pressure of the CO2? 25 ⁰C= 23.8mmHg)

106 Name the following compounds: BrCl TeO3 MgF2
How many significant figures do the following have: .00347 205 1000 Draw the Lewis Structure for SO2. Is it polar?

107 A collision requires ___ to be effective. Only enough energy
True/False Key factors that influence the rate of chemical reactions include pressure/volume, concentration, surface area, temperature and catalysts. If the temperature of the reactants is increased, the rate of the reaction will decrease. Which of the following statements about a catalyst is true? A catalyst can initiate a reaction. A catalyst can accelerate a reaction. A catalyst can be consumed during a reaction. A catalyst can be changed during a reaction. A collision requires ___ to be effective. Only enough energy Favorable orientation Enough energy and favorable orientation A reaction mechanism. Which of the following will dissolve most rapidly? Sugar cubes in a cold water Sugar cubes in hot water Powdered sugar in cold water Powdered sugar in hot water

108 How much heat in joules has to be removed from 225g of water to lower its temperature from 25.0oC to 10.0oC? Cp = 4.18 J/goC What is the specific heat of silicon if it takes 192J to raise the temperature of 45.0g of Si by 6.0oC?

109 Temperature is a measure of the ________ _________ _______ of a substance? ________ is the energy transferred during a reaction. In an endothermic reaction ___________ have more energy than ___________. In an exothermic reaction _____________ have more energy than ___________. Specific heat is the amount of energy required to raise the temp of _____ of a substance ____ or ____. When g of steam drops in temperature from °C to 50.0 °C, how much heat energy is released? Cp = 2.06J/goC A student places a 23.00g sample of 99⁰C in a calorimeter containing 25⁰C. The two samples come to 50⁰C. What is the specific heat of the metal? What amount of heat is required to raise the temperature of 85.9 g of water by 17.0°C? The specific heat of water is J/g°C.

110 What mass of BeNO3 is dissolved in 0.50 L of a 3.33M solution?
What is the molality of a solution in which 20.g of KCl is dissolved in 250.Kg of water? What is the quantity of solution made if you have 220g of BaCl2 in a 0.60M solution? How many Kg of water would you need to make a 1.27m solution with 288g of CaCl2?

111 What is the molality of a solution that contains 3.66g NaCl and 1.50 Kg water. What is the molarity of a solution if grams of NaCl is dissolved to make liters of solution. How many grams of BeCl2 would you need to add to 125 mL of water to make a molal solution?

112 What is the definition of specific heat? What type of reaction is this: If I make a solution by adding 83 grams of NaOH to 750 mL of water what is the molarity of the solution? What is the molality of the solution? How much heat must be absorbed by 375 grams of water to raise its temperature by 25° C? The specific heat of water is 4.18J/goC List 3 of the 6 types of energy.

Write the formula if none is provided
Assign Oxidation Numbers Any free element is 0 A monatomic ion is the charge of the ion F in a compound is always -1 The more electronegative atom gets its normal charge GP 1= +1, GP 2= +2, Al = +3 Hydrogen is +1 unless with a metal, then it is -1 Oxygen is -2 unless: with F it is +2 and in peroxides is -1 Calculate the rest of the oxidation numbers so that: The sum of oxidation numbers for molecules is 0 The sum of oxidation numbers for ions is the charge of the ion.

113 Give the oxidation number of each element in the following:
O2 O______ MgCl2 Mg_____, Cl______ NH4NO3 N_____, H_____, N_____, O_____ Cr2(CO3)3 Cr______, C_____, O_____ SO4-2 S_____, O_____

114 What is the final temperature when 625 grams of water at 75.0° C loses 7.96 x 104J? T/F Key factors that influence the rate of chemical reactions include pressure/volume, concentration, surface area, temperature and catalysts. Given the equation: 2A(g) + B(s) ↔ C(g) + D(g), Which direction will the reaction shift with each of the following changes. Add C? Remove A? Increase pressure? Remove D? Add B? Give the oxidation number of each element in the following: H2O HNO3 Na2SO4 H3PO4 734 grams of lithium sulfate are dissolved to make 2500 mL of solution. T/F If the temperature of the reactants is increased, the rate of the reaction will decrease

115 Write the formulas for these Acids: Hydrochloric acid Nitric acid
Sulfurous acid Name these Acids: HBr H2SO4 H3PO4

116 An Arrhenius base makes ______ in water.
An Arrhenius acid makes ______ in water. An Arrhenius base makes ______ in water. A Bronsted-Lowery acid is a proton _____. A Bronsted-Lowery base is a proton ______. ________ taste sour. ________ taste bitter. Write the dissociation equation for KOH. Write the dissociation equation for H2S

117 Identify the acid, base, conjugate acid and conjugate base in the following equation: HCl + H2O -> H3O+ + Cl- What is the pH of the following concentrations of HF: 1.0 x 10-4 M 1.0 x 10-8 M 1.0 x 10-12M M

118 How many electrons would each of the following have to gain or lose to become stable while forming an ionic bond? Na Mg S What is the concentration of [OH-] and [H3O+] if the pH of the solution is 6? Calculate the [H3O+], [OH-], pH, and pOH of the following: 0.045M copper II hydroxide

119 Calculate the [H3O+], [OH-], pH, and of a solution if the pOH is 3.16

120 Calculate the [H3O+], [OH-], and pOH of a solution if the pH is 4.213 Find the pH if the hydronium concentration of the solution is 1.00 x 10-4M

121 Would the following substance produce [H3O+] or [OH-] ions? How many? HCl KOH Ca(OH)2 H2SO4 H3PO4 What concentration of [H3O+] or [OH-] ions would be produced by the following substances? 1.5M HCl 0.453M KOH 0.045M Ca(OH)2 2M H2SO4 0.5M H3PO4

122 Calculate the [H3O+], [OH-], pH, and pOH of the following: 0.045M H2S Calculate the [H3O+], [OH-], pH, and pOH of the following: 1.05 x 10-4 M KOH M1V1=M2V2 A student titrates 50. mL HCl sol’n of unknown concentration with 25 mL of 0.65 M NaOH to reach the equivalence point. What is the concentration of the HCl sol’n in moles/L (M)?

123 How many mL of a 0.55M solution of HCl would be needed to titrate 20.0 mL of M KOH?

124 What type of ion would the following produce in an aqueous solution: HBr H2SO4 KOH Sr(OH)2 Label the conjugate acid/base pairs in the following equation: HClO4(aq) + H2O(l) ⇄ H3O+(aq) + ClO4–(aq) Pure water contains __________, __________ and _____________. Calculate the [H3O+] for a 0.035M Al(OH)3 solution.

125 Strong acids ______________ dissociate while weak acids _____________ dissociate. An ______________ substance can act as either and acid or a base. Find [H3O+], [OH-], pH, pOH of 0.37M H2S.

126 Write the dissociation equation for H2CO3.
Write the dissociation equation for Mg(OH)2. Calculate the [H3O+] for a 0.075M Al(OH)3 solution. 0.215 M KOH was titrated with 20.00mL of an acid. If the initial buret reading was 2.00mL and the final buret reading was mL. What is the molarity of the acid?

128 Determine if the following are stable: (AN<20 N/Z=1, AN>20 N/Z=1.5 Nitrogen-14 Vanadium-53 Bismuth-209 Write the decay equations for the following: Americium – 247 by beta decay Platinum – 175 by alpha decay Cobalt – 54 by positron decay Gallium – 67 by electron capture

129 Write the equation for each of the following:
Polonium-210 undergoes alpha decay Barium-140 undergoes beta decay Lithium-7 undergoes positron emission Oxygen-17 undergoes electron capture

130 Write the alpha decay equation for uranium-238.
Write the beta decay equation for potassium-22. Chemical reactions involve transfer or sharing of ___________ while nuclear reactions involve changes in the ____________. Binding energy comes from when the ____________ was formed. The more/less binding energy, the more/less stable the atom.

131 What is the half-life of an element if 12.5% remains after 36 hours? What is the original amount a sample of Co-60 (half-life= 5 years) if 3.76g remains after 25 years? How much of a 457.2g sample of Ra-226 (half-life = 1599)will remain after 6396 years? How long would it take 57.3g of Einsteinium-247 to decay to 7.16g if its half-life is minutes?

132 From 1946 to1958, the US detonated 23 nuclear weapons on the Bikini Atoll in the SW Pacific leaving behind large amounts of radioactive Cs If the half-life of 137Cs is years, when would the islands be habitable again (amount remaining < 1%)? If the half-life for the radioactive decay of zirconium-84 is 26 minutes and I start with a 175 gram sample, how much will be left over after 104 minutes?

133 If it takes 300 years to go from 500g 14C to 31.25g 14C, what is the half-life of 14C? The half-life of Po-218 is 3.0 min. What % would remain after 24 min? Write the equation for the alpha decay of sulfur-32. Write the equation for the beta decay of cobalt-60.

135 If a sample of U-238 (half-life= 4.47 x 109 years) decays until only 6.25% remains, how many years have passed? If a 60.0g sample of Fe-61 (half-life = 6.00 min) is present after 36 min, how much did you start with? The half-life of radium-224 is 3.66 days. What was the original mass if g remains after days?

134 What is the job of the coolant in a reactor?
Label each as a characteristic of fission or fusion. Splits atoms 2 atoms make one Powers stars Powers nuclear power plants Makes high level radioactive waste Makes no radioactive waste

135 The greater the mass defect, the _______ the nuclear binding energy, the ____ stable the nuclide. 3 uses of nuclear chemistry are _______________, _____________, ______________. ______ radiation occurs from a large dose in a short period of time; _______ radiation exposure occurs from small doses over a long period. ___ is a unit that measures biological effect of radiation exposure. A dose of ____ rem results in death. The minimum amount of fissionable material needed to sustain a chain reaction is __________

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