1. 1 CALCULATOR USE FOR SCIENTIFIC NOTATION PUT INTO SCIENTIFIC NOTATION MODE TO GET ANSWERS IN SCI NOT PUT INTO NORMAL MODE TO GET DECIMAL NUMBERS

2. 2 TI-83 PLUS MODE BUTTON AND ARROW KEYS

3. 3 TI-83 CHANGING MODES PRESS “MODE” KEY, THEN USE ARROW KEYS TO HIGHLIGHT “SCI”, THEN PRESS “ENTER”

4. 4 TI-83 EXITING MODES PRESS “2ND” THEN “QUIT”, WHICH IS SAME KEY AS “MODE” KEY

5. 5 TI-30X CHANGING MODES PRESS 2ND BUTTON, THEN PRESS SCI/ENT BUTTON USE ARROW KEYS TO HIGHLIGHT “SCI”

6. 6 TI-83 ENTERING NUMBERS IN SCI NOT ENTER COEFFICIENT PRESS “2ND”, THEN “EE” NOT “X 10”, THEN ENTER EXPONENT

7. 7 TI-83 SCREEN VIEW “E” REPRESENTS “X 10” NUMBER AFTER “E” IS EXPONENT

8. 8 TI-30X ENTERING NUMBERS IN SCI NOT ENTER COEFFICIENT PRESS “2ND”, THEN “EE” NOT “X 10”, THEN ENTER EXPONENT

9. 9 TI-30X SCREEN VIEW “E” REPRESENTS “X 10” NUMBER AFTER “E” IS EXPONENT

10. 10 ENTERING NEGATIVE EXPONENTS PRESS CHANGE SIGN KEY JUST BEFORE ENTERING EXPONENT

11. 11 NEGATIVE EXPONENT SCREEN VIEW NOTE NEGATIVE SIGN BEFORE EXPONENT

12. 12 SCI NOT MATH EXAMPLES DO NOT NEED TO ENTER PARENTHESES (2.4 x 10 5 ) + (5.8 x 10 4 )= ? (9.3 x 10 7 ) (5.1 x 10 2 ) = ? (8.5 x 10 -5 ) / (2.7 x 10 -3 ) = ? (4.6 x 10 -3 ) - (3.1 x 10 -4 ) = ?

13. 13 FACTOR LABEL A METHOD OF CHANGING UNITS (LABELS) BY MULTIPLYING BY A CONVERSION FACTOR ALIGN UNWANTED UNITS DIAGONALLY SO THEY CANCEL

14. 14 CONVERSION EXAMPLE CONVERT 55 MILES TO km (55 miles)(1.609 km / mile) THIS ARRANGEMENT CANCELS MILES AND LEAVES KILOMETERS ANSWER IS 88.5 km UNITS MUST ACCOMPANY ANSWER! 14

15. 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 15 55 mile1.609 km 1 mile

16. 16 CONV. EXAMPLE 2 CONVERT 20 FEET TO METERS (20 ft)(1 m / 3.3 ft) ANSWER IS 6.1 m TABLE FORM SHOWN BELOW (DIAGONAL UNITS CANCEL) 16 20 ft1 m 3.3 ft

17. 17 CONV. EXAMPLE 3 CONVERT 15,250 INCHES TO METERS (15,250 in)(1 ft / 12 in)(1 m / 3.3 ft) ANSWER IS 385.1 m TABLE FORM SHOWN BELOW (NOTICE HOW DIAGONAL UNITS CANCEL 17 15,250 in1 ft1 m 12 in 3.3 ft

18. 18 CONV. EXAMPLE 4 CONVERT 2350 SECONDS TO HOURS (2350 s)(1 min / 60 s)(1 h / 60 min) ANSWER IS 0.6 h 18 2350 s1 min1 h 60 s60 min

19. 19 COLLECTIVE UNITS MEAN A SPECIFIC NUMBER PAIR = 2 QUARTET = 4 DOZEN = 12 1 MOLE = 6.02 x 10 23 = 602,000,000,000,000,000,000,000 –CALLED AVOGADRO’S NUMBER

20. 20 MOLE-PARTICLE CONVERSIONS USE 1 MOLE = 6.02 x 10 23 AS A CONVERSION FACTOR

21. 21 MOLE-PARTICLE EXAMPLES HOW MANY ATOMS IN 2.3 MOLES OF HELIUM? HOW MANY MOLECULES IN 4.7 MOLES OF O 2 ? HOW MANY MOLES IN 5.9 x 10 25 ATOMS OF ARGON? HOW MANY MOLES IN 3.7 x 10 30 MOLECULES OF Cl 2 ?

22. 22 ATOMIC MASS REVIEW WEIGHTED AVERAGE MASS OF THE NATURALLY OCCURING ISOTOPES OF AN ELEMENT UNITS ARE amu FOUND ON THE PERIODIC TABLE ROUND OFF TO MATCH DATA IN PROBLEM, IF NO DATA, USE 1 DECIMAL PLACE

23. 23 WHAT IS THE ATOMIC MASS OF… H Li O Na Cu Cl

24. 24 MOLAR MASS THE MASS OF 1 MOLE OF A SUBSTANCE SAME NUMBER AS ATOMIC MASS, BUT UNIT IS GRAM

25. 25 WHAT IS THE MOLAR MASS OF… He Mg S K Cr Br

26. 26 MOLAR MASS OF A COMPOUND H 2 O IS MADE OF 2 ATOMS OF H AND 1 ATOM OF O CALCULATE THE MOLAR MASS BY 2(1.0 g) + 1(16.0 g) = 18.0 g

27. 27 FIND THE MOLAR MASS OF… MgCl 2 CaCrO 4 Al 2 (SO 4 ) 3 Ga 2 (CO 3 ) 3

28. 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

29. 29 MASS TO MOLES EXAMPLES HOW MANY MOLES IS 15.0 g OF CARBON? HOW MANY MOLES IS 250.0 g OF IRON?

30. 30 MOLES TO MASS REVERSE THE PROCESS GIVEN IN MOLES MOLAR MASS IN GRAMS 1 MOLE

31. 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. 32 HOW ABOUT COMPOUNDS USE THE SAME PROCESS, BUT USE THE MOLAR MASS OF THE COMPOUND IN THE CONVERSION FACTOR

33. 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. 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. 35 STANDARD CONDITIONS FOR GASES 1 ATMOSPHERE OF PRESSURE 0°C FOR TEMPERATURE TOGETHER THESE ARE CALLED STANDARD TEMPERATURE AND PRESSURE ABBREVIATION IS STP

36. 36 STANDARD MOLAR VOLUME 1 MOLE OF GAS OCCUPIES 22.4 L AT STP 1 MOLE = 22.4 L IS A CONVERSION FACTOR FOR ALL GASES

37. 37 MASS-VOLUME PROBLEMS USE THE MOLAR VOLUME TO CALCULATE THE VOLUME OF GAS IN REACTIONS AT STP

38. 38 MOLAR VOLUME EXAMPLE WHAT IS THE VOLUME OF 32.4 MOLES OF H 2 ?

39. 39 SOLUTION COMPOSITION HAS TWO PARTS: SOLUTE AND SOLVENT AMOUNT OF SOLUTE IS VARIABLE DILUTE MEANS LITTLE SOLUTE CONCENTRATED MEANS LOT OF SOLUTE QUANTIFIED BY CONCENTRATION UNITS

40. 40 MOLARITY UNIT OF CONCENTRATION MOLES OF SOLUTE PER LITER OF SOLUTION VOLUME OF SOLUTION ≠ VOLUME OF SOLVENT UNIT IS M FOR MOLAR C = n / V

41. 41 CONCENTRATION EXAMPLES WHAT IS THE CONCENTRATION OF – 1.25 L OF SOLUTION CONTAINING 20.0 g OF CaCl 2 AS THE SOLUTE? –500 mL OF SOLUTION CONTAINING 15.0 g of NaOH?

42. 42 MORE CONC. EXAMPLES HOW MANY MOLES OF SOLUTE ARE IN –325 mL OF 0.1 M KNO 3 ? –1.5 L OF 0.4 M NaCl?

43. 43 EVEN MORE CONC. EXAMPLES WHAT VOLUME OF 0.5 M BaBr 2 SOLUTION CONTAINS 0.25 MOLES OF SOLUTE? WHAT VOLUME OF 0.8 M Mg(OH) 2 SOLUTION CONTAINS 0.5 MOLES OF SOLUTE?

44. 44 CONVERSION REVIEW

45. 45 TWO STEP CONVERSION EXAMPLES HOW MANY MOLECULES ARE IN 25.0 g OF SODIUM? WHAT IS THE VOLUME OF 100.0 g OF O 2 ? WHAT MASS OF SOLUTE IS IN 25 mL OF 0.1 M KOH?

46. 46 PERCENT COMPOSITION MASS OF AN ELEMENT / MASS OF COMPOUND THIS GIVES A DECIMAL THAT IS CONVERTED TO PERCENT

47. 47 PERCENT COMPOSITION FROM FORMULA ASSUME 1 MOLE DETERMINE MOLAR MASS OF EACH CONSTITUENT MULTIPLY BY SUBSCRIPTS DIVIDE BY MOLAR MASS OF COMPOUND

48. 48 PERCENT COMPOSITION EXAMPLE FIND PERCENT COMPOSITION OF – Al 2 O 3 –MgC 2 O 4

49. 49 EMPIRICAL FORMULA FROM PERCENT COMPOSITION ASSUME 100 g OF COMPOUND CHANGE PERCENTS TO MASS FIND MOLES OF EACH ELEMENT FIND SMALLEST RATIO OF MOLES USE AS SUBSCRIPTS

50. 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. 51 EMPIRICAL FORMULA FROM MASS DATA CONVERT MASS TO MOLES FOLLOW PREVIOUS STEPS FOR FORMULA FROM PERCENT COMPOSITION

52. 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. 53 MOLECULAR FORMULAS MOLECULAR FORMULA = N(EMPIRICAL FORMULA) N = (MOLAR MASS OF COMPOUND) / (MASS OF EMPIRICAL FORMULA)

54. 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. 55 HYDRATE A SUBSTANCE THAT HAS WATER CHEMICALLY ATTACHED A DOT SYMBOLIZES THE CHEMICAL BOND (NOT A MULTIPLICATION SIGN) A COEFFICIENT INDICATES THE NUMBER OF WATER MOLECULES ATTACHED TO EACH FORMULA UNIT

56. 56 HYDRATE EXAMPLES CuSO 4  5H 2 O Na 2 CO 3  10H 2 O

57. 57 HYDRATE COMPONENTS WATER OF HYDRATION – THE WATER ATTACHED TO THE HYDRATE OFTEN CAN BE REMOVED BY HEATING ANHYDROUS SALT – COMPOUND LEFT AFTER WATER OF HYDRATION REMOVED

58. 58 DEHYDRATING A HYDRATE

59. 59 EMPIRICAL FORMULA OF HYDRATE NEED MASS OF HYDRATE AND MASS OF ANHYDROUS SALT (AFTER HEATING) MASS OF WATER = MASS OF HYDRATE - MASS OF ANHYDROUS SALT CALCULATE MOLES OF ANHYDROUS SALT AND WATER OF HYDRATION MAKE RATIO AND SIMPLIFY TO SMALLEST WHOLE NUMBERS SHOULD BE 1 TO SOMETHING

60. 60 HYDRATE EXAMPLE MASS OF HYDRATE IS 154.0 g AND MASS OF ANHYDROUS SALT (Na 2 S) IS 50.0 g MASS OF HYDRATE IS 50.0 g AND MASS OF ANHYDROUS SALT (CaCl 2 ) IS 37.8 g