1. Flashcards for Unit 1

2. Matter
Anything that has mass & occupies space.

3. A measure of the gravitational pull on matter.
You would weigh less on the moon!
Weight

4. Mass A measure of the quantity of matter.
You would have the same mass on the moon.
Mass

5. A series of steps followed to solve problems, including collecting data, forming a hypothesis, testing the hypothesis, and stating conclusions.
Scientific Method

6. A fact you take in with your senses.
Observation

7. A testable statement
Hypothesis

8. An inference
Conclusion

9. Scientific Law Describes what happens. Often stated mathematically.
Summarizes many (thousands of) observations.
Scientific Law

10. A model that tries to explain why nature behaves a certain way
A model that tries to explain why nature behaves a certain way. May be modified.
Theory

11. 7
How many fundamental units in the SI system?

12. Fundamental or Base Unit
Physical quantity that must be measured. It cannot be calculated.

13. Derived Unit
A unit defined as a combination of fundamental units.

14. Unit of mass
Kilogram
Fundamental Unit

15. Unit of time
Second
Fundamental Unit

16. Unit of length
Meter
Fundamental Unit

17. Unit of temperature
Kelvin
Fundamental Unit

18. Space or Capacity
Volume
Derived Unit

19. Metric Unit of Volume
10 cm X 10 cm 10 cm
Liter
Derived Unit

20. 1000 cm3 = 1 Liter
? cm3 = 1 Liter
Derived Unit

21. 1000 mL = 1 Liter
? milliliter = 1 Liter
Derived Unit

22. 1 mL = 1 cm3
? milliliter = 1 cm3
Derived Unit

23. What is the mass of 1 liter of pure H2O?
1 kilogram
What is the mass of 1 liter of pure H2O?
Mass/Volume relationship

24. What is the volume of 1 kg of pure H2O?
1 liter
What is the volume of 1 kg of pure H2O?
Mass/Volume relationship

25. What is the mass of 1 cm3 of pure H2O?
1 gram
What is the mass of 1 cm3 of pure H2O?
Mass/Volume relationship

26. What is the volume of 1 gram of pure H2O?
1 cm3 or 1 mL
What is the volume of 1 gram of pure H2O?
Mass/Volume relationship

27. Kilogram Second Meter Kelvin Mole Unit of Mass Unit of Time
Unit of Length
Unit of Temperature
Unit of Amount of Substance
Unit of Volume: derived
(Space or capacity)
Kilogram
Second
Meter
Kelvin
Mole
Liter, milliliter, cubic centimeter

28. Freezing Point of water in the Kelvin scale.
Physical Constant

29. Boiling Point of water in the Kelvin scale.
Physical Constant

30. Freezing Point of water in the centigrade scale.
Physical Constant

31. Boiling Point of water in the centigrade scale.
Physical Constant

32. Another name for freezing point.
Ice / water equilibrium

33. Another name for boiling point.
Steam / water equilibrium

34. 100 cm = 1 meter
? cm in 1 meter
Conversion Fact

35. 1000 mm = 1 meter
? mm in 1 meter
Conversion Fact

36. 1000 m = 1 kilometer
? m in 1 km
Conversion Fact

37. 1000 mg = 1 gram
? mg in 1 g
Conversion Fact

38. Mass / Volume
Density

39. Describes how matter is packed into space.
Density

40. grams / cm3 for solids
grams / ml for liquids
Units of Density

41. M D V
Density

42. How close a measured value is to an accepted value.
Accuracy

43. How close a series of measurements are to one another.
Precision

44. Low Scatter
High Precision

45. Measured value – Accepted value x 100%
Percent Error
Table T, reference tables

46. A measure of the average kinetic energy of the particles of a system.
Temperature

47. K = C + 273
C to K
Table T, reference tables

48. Scientific Notation The number is written as a product of 2 numbers:
- a number between 1 & 10
- a power of 10
Scientific Notation

49. Negative exponent so the number is between 0 and 1:
0.002
2 X 10-3

50. Positive exponent so the number is greater than 1:
500
5 X 102

51. 3.45 X 10-17 Convert 345 X 10-19 to scientific notation.
So the 2nd factor must increase by a factor of 100.
The 1st factor got smaller by a factor of 100.
Convert 345 X to scientific notation.

52. Significant Figures All known digits plus 1 estimated digit.
From the perspective of the person MAKING the measurement.

53. 5400.145 cm Decimal Present – Pacific side 7 sig figs 1 2 3 4 5 6 7
Start counting at 1st nonzero # and count until the end of the number. cm
Interpreting someone else’s measurements. 1 2 3 4 5 6 7
7 sig figs

54. 0.0175 g Decimal Present – Pacific side 3 sig figs 1 2 3
Start counting at 1st nonzero # and count until the end of the number. g 1 2 3
Interpreting someone else’s measurements.
3 sig figs

55. 4855 g Decimal Absent – Atlantic side 4 sig figs 4 3 2 1
Start counting at 1st nonzero # and count until the end of the number.
4855 g 4 3 2 1
4 sig figs

56. 4000 mm Decimal Absent – Atlantic side 1 sig fig
Start counting at 1st nonzero # and count until the end of the number.
4000 mm 1
1 sig fig

57. Rule for sig figs in Addition and Subtraction
Answer has same number of decimal places as the addend with the least number of decimal places.
Rule for sig figs in Addition and Subtraction

58. 77.2 cm is correct! 28.0 cm But what do you report? 23.538 cm 25.68 cm
Least # of decimal places ! cm cm
25.68 cm
But what do you report? + cm

59. Rule for sig figs in Multiplication & Division
Answer has same number of significant figures as the factor with the least number of significant figures.
Rule for sig figs in Multiplication & Division

60. 24 m X 3.26 m = 78.24 m2 78 m2 is correct! But what do you report?
2 sig figs
3 sig figs
24 m X 3.26 m = m2
But what do you report?

61. c) 2.7 g/cm3 2.749 g/cm3 d) 0.36 cm3/g 2.75 g/cm3 2 sf
3 sig figs
An aluminum cube has a mass of 4.75 grams. The dimensions of the cube are 1.2 cm X 1.2 cm X 1.2 cm. What is the density of the cube?
2 sf
“Volume” = cm3

62. Calculating density by water displacement.
Final Volume = mL
Initial Volume = 40.0 mL
Mass of rock = 54.0 g
Density of rock = 9.0 g/mL
Volume of rock = 6.0 mL
2 sig figs – determined by the digits in the difference not by the raw data!
Calculating density by water displacement.

63. 5 sig figs 1 sig fig 58.5 grams of NaCl = 1 mole. Calculated from P.T.
g 1 mole = moles
58.5 grams
 0.8 M
moles/1. Liter = 0.75 M
5 sig figs
1 sig fig
A solution contains grams of NaCl dissolved in 1. Liter of H2O. What is the molarity expressed to the correct sig figs?

64. Data Table independent variable – controlled by scientist (column 1)
2 columns plus title
independent variable – controlled by scientist (column 1)
dependent variable – measured variable (column 2)
Data Table

65. 2 axes plus title
independent variable – controlled by scientist (column 1) – GOES on X-AXIS
dependent variable – measured variable (column 2) – GOES on Y-AXIS
Graph

66. Y-axis
Y = mX + b
X-axis
Linear Relationship

67. Y-axis
Y = mX
X-axis
Direct Relationship

68. Y-axis
XY = k where k is a constant
X-axis
Inverse Relationship

69. Y-axis
X-axis
Graph of a Constant