1. Matter, Energy, and Measurement Home Work-1.16, 1.17, 1.19, 1.21, 1.25, 1.27,1.33, 1.37, 1.38, 1.39, 1.41, 1.45, 1.47, 1.48, 1.49, 1.51, 1.57, 1.59, 1.69, 1.73

2. Chemistry Why? The universe consists of three things: Matter, Energy, Empty Space Matter- is anything that has mass and takes up space.

3. Chemistry Chemistry- is the science that deals with matter: the structure and properties of matter and the transformations from one form of matter to another. Matter can undergo two types of changes

4. Changes Chemical Change: also called a chemical reaction, substances are used up (they disappear) and others are formed to take their place. Examples:

5. Changes Physical Change- changes in which the identity of a substance remains unchanged. (usually involves changes in state and/or appearance) Examples:

6. Properties of Matter There are two types of properties: Chemical properties: the chemical reactions a substance undergoes Physical Properties: properties that do not involve chemical reactions such as: density, color, melting point, physical state

7. The Scientific Method The scientific method establishes a process that provides a foundation of evidence to back up all scientific information!! It has four parts!!!

8. The Scientific Method Fact- is a statement based on direct experience. It is a consistent and reproducible observation. Hypothesis- is a statement that is proposed without actual proof, to explain the Fact and/or relationships betweens different Facts.

9. The Scientific Method Tests- Designed experiments or observations used to determine the validity of the Hypothesis. Theory- the formulation of an apparent relationship of certain observed phenomena, which has been verified to some extent. (A Hypothesis with evidence from the Tests to support it!!)

10. Serendipity Serendipity- is chance observation. Accidental discovery.

11. Experimental Notation This system provides an easy way to express very large and/or very small numbers It is based on the power of tens system Examples:

12. Adding and Subtracting in EN Appendix 1 page A-1 Numbers must have the same exponent Add/subtract coefficients Leave exponent as is Examples:

13. Multiply and Divide in EN First multiply/divide Coefficients Then Add exponents for multiplication, Subtract exponents for division. Examples:

14. Significant Figures Appendix 2 page A-5 Defined as: The number of digits of a measured number that have uncertainty only in the last digit. Examples:

15. Rules 1)Nonzero digits are Always significant 2)Zeros at the beginning of a number are Never significant 3)Zeros between nonzero digits are Always significant

16. Rules (cont) 4) Zeros at the end of a number that has a decimal point are Always significant 5)Zeros at the end of a number with no decimal point May or May Not be Significant.

17. Sig. Figs. In E.N In E.N., the EN number must contain the same number of Sig. Figs. as the original number.

18. Sig. Figs in Functions Multiplication/Division- answer must have the same number of sig figs as the one with the Fewest sig figs.

19. Sig. Figs in Functions (cont) Addition/Subtraction- sig fig not relevant. The answer must contain the same number of decimal places as the one with the Fewest.

20. Rounding If the digit to be dropped is 5,6,7,8 or 9, we round up Otherwise, we simply drop the digit.

21. Defined/Counted Numbers Numbers that are defined, or counted, are treated as though they have infinite significant figures. Example:

22. Measurements A measurement consists of TWO parts: a number and a unit. The units must always be present.

23. English Units Mass- pounds Length- miles, inch, feet, etc Volume- gallons, pints, quarts, etc Time- Seconds

24. Metric Units Mass- gram, kilogram Length- meter, kilometer Volume- Liter, milliliter Time- Seconds SI Units are typically the same as metric units, just more specific!

25. Metric System Establishes a base unit, and other units are related to that base unit by powers of 10.

26. Length English 12 inches = 1 foot 3 feet = 1 yard 1760 yards = 1 mile Metric –Base unit is the meter 1 kilometer = 1000 meters 1 millimeter = 0.001 meters

27. Metric Prefixes PrefixSymbolValue giga G10 9 1 billion megaM10 6 1 million kilok10 3 1 thousand BASE UNIT decid10 -1 one-tenth centic10 -2 one- hundreth millim10 -3 one-thousandth micro  10 -6 one-millionth nanon10 -9 one-billionth

28. Volume Volume is space. The volume of a substance is the amount of space it occupies Base unit= Liter

29. Mass Mass is the quantity of matter in an object Base Unit= Gram There is a difference between Mass and Weight!!!!!

30. Time The base unit for time is Seconds. This is the same in all 3 systems!!

31. Temperature Base unit= Celsius or centigrade ( o C) English system uses Fahrenheit ( o F) The following can be used to convert between the two: o F = (9/5) o C + 32 o C = (5/9) x ( o F – 32) The SI temperature unit uses the Kelvin (K) K= o C + 273 0K = Absolute zero!!!

32. Comparisons LengthMass 1 in = 2.54 cm1 oz = 28.35 g 1 m = 39.37 in1 lb = 453.6 g 1 mile = 1.609 km1 kg = 2.205 lb

33. Comparisons VolumeTemperature 1 qt = 0.946 L0 K = -459 o F = -273 o C 1 gal = 3.785 L 233K = -40 o F= -40 o C 1 L = 33.81 fl oz273K = 32 o F= 0 o C 1 fl oz = 29.57 mL310K = 98.6 o F= 37 o C 1L = 1.057 qt373K = 212 o F = 100 O C 1 mL = 1 cc = 1 cm 3

34. Unit Conversions Factor-Label Method- we multiply and divide units with numbers using conversion factor. Using a conversion factor is the same thing as multiply by 1, only the units cancel out!!!!

35. Examples Convert 2,750 L into kL. Convert 120 lbs to grams.

36. More Examples Convert 3.5 miles to meters Convert 900 g/ml to lbs/qt

37. States of Matter Matter can exist in three states- Solid, Liquid and Gas Gases- no definite shape or volume, highly compressible Liquids- no definite shape, but do have definite volume, only slightly compressible Solids- Definite shape and volume, essentially noncompressible

38. Density Density- the mass of a substance per unit of volume. –All states of matter have a density. –When two liquids are mixed and one does not dissolve in the other, the one with the lower density floats on top!! –Density is calculated by dividing the mass of a substance by its volume d= m/v

39. Density Density is a physical property and always has the same value at a given temperature Density usually decreases as temperature increases because the mass remains the same while the volume increases EXCEPTION: WATER!!! From 4-100 o C density increases, but from 0-4 o C it actually decreases!!!

40. Specific Gravity Numerically, it is the same as density, only it has no units. It is the density of a substance compared to water.

41. Energy Energy- the capacity to due work Kinetic Energy is energy of motion KE increases when either an object moves faster or a heavier object is moving.

42. Energy Potential Energy (PE) is stored energy The PE possessed by an object arises from its capacity to move or cause motion.

43. Forms of Energy Mechanical, light, heat, and electrical energy –Kinetic energies possessed by all moving objects Chemical energy and Nuclear energy –Potential energies

44. Chemical Energy The energy stored within chemical substances and given off when they take part in a chemical reaction. Examples:

45. Energy Various forms of energy can be converted from one to another Example Law of Conservation of Energy- Energy can neither be created nor destroyed.

46. Heat Heat is the form of energy that most frequently accompanies chemical reactions HEAT AND TEMPERATURE ARE DIFFERENT!!! Heat is a form of energy, temperature is a measurement.

47. Heat (cont) The Heat unit is usually a calorie calorie- the amount of heat necessary to raise the temperature of 1 gram of water by 1 o C. This is a small unit so kilocalories is typically used (1 kcal = 1000 calories

48. Nutritionists use the word Calorie to mean the same thing as kilocalorie, so: 1 Cal = 1000 cal = 1 kcal The SI unit is the Joule (J) 1 cal = 4.184 J

49. Specific Heat The amount of heat necessary to raise the temperature of 1 g of any substance by 1 o C. Each substance has its own specific heat Is this a physical property or chemical property? Specific Heat can be used to calculate the amount of heat needed or used Amt of Heat Used = SH x m x (T 2 -T 1 )

50. Aluminum has a SH of.22, Iron has a SH of.11. How much heat is required to raise the temperature of 100 grams of each from 30 o C to 100 o C? Fun with SH!!!