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1. CALCULATOR USE FOR SCIENTIFIC NOTATION
• PUT INTO SCIENTIFIC NOTATION ______ TO GET ANSWERS IN SCI NOT
• PUT INTO ________ MODE TO GET DECIMAL NUMBERS
2. TI-83 PLUS MODE BUTTON AND ARROW KEYS
3. TI-83 CHANGING MODES
• PRESS “_____” KEY, THEN USE ARROW KEYS TO HIGHLIGHT “____”, THEN
PRESS “ENTER”
4. TI-83 EXITING MODES
• PRESS “2ND” THEN “_____”, WHICH IS SAME KEY AS “_____” KEY
5. TI-30X CHANGING MODES
• PRESS 2ND BUTTON, THEN PRESS ________ BUTTON
• USE ARROW KEYS TO HIGHLIGHT “____”
6. TI-83 ENTERING NUMBERS IN SCI NOT
• ENTER ___________
• PRESS “2ND”, THEN “___” NOT “_____”, THEN ENTER EXPONENT
7. TI-83 SCREEN VIEW
• “E” REPRESENTS “______”
• NUMBER AFTER “E” IS ________
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8. TI-30X ENTERING NUMBERS IN SCI NOT
• ENTER ______________
• PRESS “2ND”, THEN “____” NOT “X 10”, THEN ENTER EXPONENT
9. TI-30X SCREEN VIEW
• “E” REPRESENTS “_____”
• NUMBER AFTER “E” IS _______
10. ENTERING NEGATIVE EXPONENTS
• PRESS ________________ KEY JUST BEFORE ENTERING EXPONENT
11. NEGATIVE EXPONENT SCREEN VIEW
• NOTE NEGATIVE SIGN BEFORE EXPONENT
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12. SCI NOT MATH EXAMPLES
• DO NOT NEED TO ENTER PARENTHESES
• (2.4 x 105) + (5.8 x 104)= ?
• (9.3 x 107) (5.1 x 102) = ?
• (8.5 x 10-5) / (2.7 x 10-3) = ?
• (4.6 x 10-3) - (3.1 x 10-4) = ?
13. FACTOR LABEL
• A METHOD OF CHANGING ______ (LABELS) BY MULTIPLYING BY A
CONVERSION _______
• ALIGN UNWANTED UNITS DIAGONALLY SO THEY _______
14. CONVERSION EXAMPLE
• CONVERT 55 MILES TO km
•
•
•
•
THIS ARRANGEMENT CANCELS MILES AND LEAVES KILOMETERS PER HOUR
ANSWER IS _______
UNITS MUST ACCOMPANY ANSWER!
15. CONVERSION EXAMPLE CONTINUED
• TABLE BELOW SHOWS ANOTHER WAY TO SET THIS UP (NOTICE RED
DIAGONAL UNITS WILL CANCEL)
• UNITS DETERMINE NUMBER PLACEMENT!
• MULTIPLY LIKE FRACTIONS TO GET ANSWER
55 miles 1.609 km
1 mile
16. CONV. EXAMPLE 2
• CONVERT 20 FEET TO METERS
• _____________
• ANSWER IS _____
• TABLE FORM SHOWN BELOW (DIAGONAL UNITS CANCEL)
20 ft 1 m
3.3 ft
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17. CONV. EXAMPLE 3
• CONVERT 15,250 INCHES TO METERS
• ________
• ANSWER IS ___
• TABLE FORM SHOWN BELOW (NOTICE HOW DIAGONAL UNITS CANCEL
15,250 in 1 ft
1m
12 in 3.3 ft
18. CONV. EXAMPLE 4
• CONVERT 2350 SECONDS TO HOURS
• ______
• ANSWER IS ____
2350 s 1 min 1 h
60 s
60 min
19. COLLECTIVE UNITS
• MEAN A SPECIFIC NUMBER
• PAIR =
• QUARTET =
• DOZEN =
•
1 MOLE =
= _____
– CALLED ______________ NUMBER
20. MOLE-PARTICLE CONVERSIONS
• USE 1 MOLE = 6.02 x 1023 AS A CONVERSION FACTOR
21. MOLE-PARTICLE EXAMPLES
• HOW MANY ATOMS IN 2.3 MOLES OF HELIUM?
• HOW MANY MOLECULES IN 4.7 MOLES OF O2?
• HOW MANY MOLES IN 5.9 x 1025 ATOMS OF ARGON?
• HOW MANY MOLES IN 3.7 x 1030 MOLECULES OF Cl2?
22. ATOMIC MASS REVIEW
• WEIGHTED AVERAGE _____ OF THE NATURALLY OCCURING ISOTOPES OF
AN ELEMENT
• UNITS ARE _____
• FOUND ON THE PERIODIC TABLE
• ROUND OFF TO MATCH DATA IN PROBLEM, IF NO DATA, USE __ DECIMAL
PLACE
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23. WHAT IS THE ATOMIC MASS OF…
• H
• Li
• O
• Na
• Cu
• Cl
24. MOLAR MASS
• THE MASS OF ________ OF A SUBSTANCE
• SAME NUMBER AS ATOMIC MASS, BUT UNIT IS _____
25. WHAT IS THE MOLAR MASS OF…
• He
• Mg
• S
• K
• Cr
• Br
26. MOLAR MASS OF A COMPOUND
• H2O IS MADE OF 2 ATOMS OF H AND 1 ATOM OF O
• CALCULATE THE MOLAR MASS BY _______
27. FIND THE MOLAR MASS OF…
• MgCl2
• CaCrO4
• Al2(SO4)3
• Ga2(CO3)3
28. MASS TO MOLES
• USE FACTOR-LABEL CONVERSION
• INCLUDE SUBSTANCE AS PART OF THE UNIT
• CONVERSION FACTOR IS MOLAR MASS OF SUBSTANCE
Given in grams 1 mole
Molar mass in grams
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29. MASS TO MOLES EXAMPLES
• HOW MANY MOLES IS 15.0 g OF CARBON?
• HOW MANY MOLES IS 250.0 g OF IRON?
30. MOLES TO MASS
• REVERSE THE PROCESS
31. MOLES TO MASS EXAMPLES
• WHAT IS THE MASS OF 3.2 MOLES OF LEAD?
• WHAT IS THE MASS FO 0.8 MOLES OF COPPER?
32. HOW ABOUT COMPOUNDS
• USE THE SAME PROCESS, BUT USE THE MOLAR MASS OF THE COMPOUND
IN THE CONVERSION FACTOR
33. MASS OF COMPOUNDS TO MOLES EXAMPLES
• HOW MANY MOLES IS 20.5 g OF WATER?
• HOW MANY MOLES IS 42.8 g OF NaCl?
34. MOLES OF COMPOUNDS TO MASS EXAMPLES
• WHAT IS THE MASS OF 6.4 MOLES OF WATER?
• WHAT IS THE MASS OF 0.75 MOLES OF KBr?
35. STANDARD CONDITIONS FOR GASES
• ___ ATMOSPHERE OF PRESSURE
• ____ FOR TEMPERATURE
• TOGETHER THESE ARE CALLED STANDARD TEMPERATURE AND PRESSURE
• ABBREVIATION IS ___
36. STANDARD MOLAR VOLUME
• 1 MOLE OF GAS OCCUPIES _____ L AT STP
• 1 MOLE = _____ L IS A CONVERSION FACTOR FOR ALL GASES
37. MASS-VOLUME PROBLEMS
• USE THE MOLAR VOLUME TO CALCULATE THE VOLUME OF GAS IN
REACTIONS AT STP
38. MOLAR VOLUME EXAMPLE
• WHAT IS THE VOLUME OF 32.4 MOLES OF H2?
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39. SOLUTION COMPOSITION
• HAS TWO PARTS: _________ AND ___________
• AMOUNT OF SOLUTE IS ______
• DILUTE MEANS _______ SOLUTE
• CONCENTRATED MEANS _____ OF SOLUTE
• QUANTIFIED BY CONCENTRATION UNITS
40. MOLARITY
• UNIT OF CONCENTRATION
• _______ OF SOLUTE PER _______ OF SOLUTION
• VOLUME OF SOLUTION ≠ VOLUME OF SOLVENT
• UNIT IS ___ FOR MOLAR
• C = _____
41. CONCENTRATION EXAMPLES
• WHAT IS THE CONCENTRATION OF
– 1.25 L OF SOLUTION CONTAINING 20.0 g OF CaCl2 AS THE SOLUTE?
– 500 mL OF SOLUTION CONTAINING 15.0 g of NaOH?
42. MORE CONC. EXAMPLES
• HOW MANY MOLES OF SOLUTE ARE IN
– 325 mL OF 0.1 M KNO3?
– 1.5 L OF 0.4 M NaCl?
43. EVEN MORE CONC. EXAMPLES
• WHAT VOLUME OF 0.5 M BaBr2 SOLUTION CONTAINS 0.25 MOLES OF
SOLUTE?
• WHAT VOLUME OF 0.8 M Mg(OH)2 SOLUTION CONTAINS 0.5 MOLES OF
SOLUTE?
44. CONVERSION REVIEW
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45. TWO STEP CONVERSION EXAMPLES
• HOW MANY MOLECULES ARE IN 25.0 g OF SODIUM?
• WHAT IS THE VOLUME OF 100.0 g OF O2?
• WHAT MASS OF SOLUTE IS IN 25 mL OF 0.1 M KOH?
46. PERCENT COMPOSITION
• MASS OF AN _________ / MASS OF __________
• THIS GIVES A DECIMAL THAT IS CONVERTED TO PERCENT
47. PERCENT COMPOSITION FROM FORMULA
• ASSUME 1 ______
• DETERMINE MOLAR MASS OF EACH CONSTITUENT
• MULTIPLY BY SUBSCRIPTS
• DIVIDE BY MOLAR MASS OF COMPOUND
48. PERCENT COMPOSITION EXAMPLE
• FIND PERCENT COMPOSITION OF
– Al2O3
– MgC2O4
49. EMPIRICAL FORMULA FROM PERCENT COMPOSITION
• ASSUME _____ g OF COMPOUND
• CHANGE PERCENTS TO MASS
• FIND MOLES OF EACH ELEMENT
• FIND SMALLEST RATIO OF MOLES
• USE AS SUBSCRIPTS
50. EMPIRICAL EXAMPLES
• FIND EMPIRICAL FORMULAS
– 17.09% Mg, 37.39% Al, 44.98% O
– 26.57% K, 35.36% Cr, 38.07% O
51. EMPIRICAL FORMULA FROM MASS DATA
• CONVERT MASS TO MOLES
• FOLLOW PREVIOUS STEPS FOR FORMULA FROM PERCENT COMPOSITION
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52. MORE EMPIRICAL EXAMPLES
• FIND EMPIRICAL FORMULAS
– 88 g OF COMPOUND CONTAINS 24 g OF CARBON, REMAINING IS OXYGEN
– 0.2636 g OF PURE Ni REACTS WITH OXYGEN, FINAL MASS OF NICKEL
OXIDE IS 0.3354 g
53. MOLECULAR FORMULAS
• MOLECULAR FORMULA = ____________
• n = (MOLAR MASS OF COMPOUND) / (MASS OF EMPIRICAL FORMULA)
54. MOLECULAR EXAMPLES
• FIND MOLECULAR FORMULAS
– 65.2% ARSENIC, 34.8% OXYGEN, MOLAR MASS IS 459.6 g
– 71.65% Cl, 24.27% C, AND 4.07% H, MOLAR MASS IS 98.96 g
55. HYDRATE
• A SUBSTANCE THAT HAS ________ CHEMICALLY ATTACHED
• A _____ SYMBOLIZES THE CHEMICAL BOND (NOT A MULTIPLICATION SIGN)
• A ____________ INDICATES THE NUMBER OF WATER MOLECULES ATTACHED
TO EACH FORMULA UNIT
56. HYDRATE EXAMPLES
• CuSO4  5H2O
• Na2CO3  10H2O
57. HYDRATE COMPONENTS
• WATER OF ____________ – THE WATER ATTACHED TO THE HYDRATE
• OFTEN CAN BE REMOVED BY _______
• ___________________ – COMPOUND LEFT AFTER WATER OF HYDRATION
REMOVED
58. DEHYDRATING A HYDRATE
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59. EMPIRICAL FORMULA OF HYDRATE
• NEED MASS OF HYDRATE AND MASS OF ANHYDROUS SALT (AFTER
HEATING)
• MASS OF WATER = MASS OF ________ - MASS OF _________
• CALCULATE MOLES OF ANHYDROUS SALT AND WATER OF HYDRATION
• MAKE RATIO AND SIMPLIFY TO SMALLEST WHOLE NUMBERS
• SHOULD BE 1 TO SOMETHING
60. HYDRATE EXAMPLE
• MASS OF HYDRATE IS 154.0 g AND MASS OF ANHYDROUS SALT (Na2S) IS
50.0 g
• MASS OF HYDRATE IS 50.0 g AND MASS OF ANHYDROUS SALT (CaCl2) IS
37.8 g
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