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Matter and Math Chemistry 131 Chapter 1. Physical Properties Dimensional Analysis MatterFormulas.

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Presentation on theme: "Matter and Math Chemistry 131 Chapter 1. Physical Properties Dimensional Analysis MatterFormulas."— Presentation transcript:

1 Matter and Math Chemistry 131 Chapter 1

2 Physical Properties Dimensional Analysis MatterFormulas

3 Matter and its Classification This section deals with how we categorize the types of matter into distinct and coherent subgroups. In addition it build a connection map between the different groups.

4 Matter Everything of substance around you is matter. Whatever has mass is matter. There is a lot more to it than this, but we will start here. Can be subdivided into…

5 Pure Substances & Mixtures Matter can be divided into two subgroups, the Pure Substance and the Mixture. Pure substances are those composed of only one element, while mixtures are a combination of at least two elements.element Can be further subdivided into…

6 Heterogeneous Mixtures & Solutions Heterogeneous mixtures can be physically separated while solutions cannot. Solutions must be chemically separated.

7 Matter can be divided into two subgroups, the Pure Substance and the Mixture. Pure substances are those composed of only one element, while mixtures are a combination of at least two elements.element Can be further subdivided into… Pure Substances & Mixtures

8 Compounds & Elements Compounds are where more than one atom is bonded together in some fashion. Elements are individual atoms. Can be further subdivided into…

9 Molecular Compounds & Ionic Compounds Molecular compounds, or molecules, are those where the atoms are covalently bonded together. The atoms in ionic compounds are held together by ionic bonds.covalently bonded ionic bonds

10 Compounds & Elements Compounds are where more than one atom is bonded together in some fashion. Elements are individual atoms. Can be further subdivided into…

11 Three Classes, or Groups…

12 Metals Metals are those elements on the far right and middle of the periodic table. They hold their outer electrons loosely, have luster, are ductile, malleable, and conductive.periodic tableouter electrons ductilemalleable conductive

13 Metalloids have properties of both metals and nonmetals, they have luster are typically ductile or malleable to a limited degree and are semi conductive.semi conductive

14 Nonmetals are brittle in their solid forms (though they may be in gaseous or liquid forms at room temperature). Typically they are electrical insulators.insulators

15 Now for the big picture…

16 Matter Mixtures Pure Substances Elements Metals Metalloids Nonmetals Compounds Ionic Compounds Molecular Compounds SolutionsHeterogeneous Mixtures

17 So how do we describe compounds?

18 Chemical Formulas Chemical formulas are the shorthand of chemistry, the language if you will. There are rules to its grammar and syntax that we need to learn and follow as we go through the course.

19

20 What is the compound composed of? Take the molecule apart, down to its constituent atoms.

21

22 What is there? Now you need to identify the atoms by their elements, in our kits they have standard colors, black for carbon, red for oxygen and white for hydrogen.

23 Oxygen Carbon Hydrogen

24 How many of each?

25 Oxygen = 1 Carbon = 2 Hydrogen = 6

26 Can we abbreviated anything? Writing out the names of each element every time would be tedious, so each element has an abbreviation, a chemical symbol, to represent it. These symbols may be obvious (O for oxygen) or obscure (W for tungsten, because it used to be Wolfram). These are the symbols used on the Periodic Table.

27 Oxygen = O Carbon = C Hydrogen = H

28 So what do we have now?

29 Oxygen = 1 O Carbon = 2 C Hydrogen = 6 H

30 Now add the grammar? The grammar, or syntax, of chemistry is such that elements present as a single atom are represented by their symbol. Elements that are represented by more than one atom are have their atomic symbol followed by a subscript with the number of atoms for that element.

31 Oxygen = O Carbon = C 2 Hydrogen = H 6

32 Start with the element with the highest number of bonds. Well get into this more later, but the highest number of bonds means the highest number of available electrons and these are the core of how chemistry works.

33 Oxygen = O Carbon = C 2 Hydrogen = H 6 Bonds are the holes in this model… little hard to see

34 Okay… C 2 … then what?

35 Add the rest in… C 2 H 5 OH

36 Wait… why not C 2 H 6 O 2 or C 2 O 2 H 6 ?

37 Sometimes it isn’t as simple… Let us look at the compound again

38

39 Notice how the OH can be taken off as a distinct unit?

40 Functional Groups… hence… C 2 H 5 OH Functional groups are substructures of a compound with specific structure and similar functions. They are written separately in the formulas to emphasize their role in the overall structure and function of the compound.

41 Now you try one

42 CH 3 OH

43 Physical Properties This section deal with the difference between what it means to undergo a physical versus chemical change.

44 What is a Physical Property? Physical Properties of matter are those that can be measured or observed without the matter undergoing a chemical change.

45 Observations can be either Qualitative or Quantitative

46 Qualitative is Subjective

47 Observations can be either Qualitative or Quantitative

48 Quantitative is Objective

49 What types of Quantitative measures can we do?

50 Mass Mass is a measure of the amount of matter you have. This is recorded in grams (g) or kilograms (kg). Commonly this is referred to as weight, though technically weight is the mass within a specific gravity field. In other words, the weight may vary, but the mass will not.

51 Volume Volume is a measure of the amount of space matter occupies. This is commonly measured in units such as liter (L), milliliter (mL) or cubic meter (m 3 )

52 Density Density is a derived measurement, it is calculated by dividing the mass of an object by its volume.derived measurement

53 Dimensional Analysis In this section we are going to work on problems to strengthen your ability to do the basic math required in this course.

54 Time for the MATH!

55

56 Ooo, dreams of fractions

57 It isn’t that bad, really.

58 Liar…

59 No Honest… let’s try…

60 Try this one. Answer = 3/8 1.Square 1/2 = 1/4 2.Multiple that by 1/2 = 1/8 3.Add that to 1/4, with the least common denominator as 8 = 3/8

61 How about this one?

62 Now a little more… try to figure out these conversions. Hint, check your books for the conversion factors.

63 Complete the following conversions A. 1.54 kg = __________g B. 3.46 cm = __________ µm C. 12.4 ml = __________ l D. 2.3 × 10 3 in = ___________ m 1540 346000 0.0124 58.42

64 Try these, they are density equations. A. A liquid that has a mass of 125 g per 120 ml, what is the density in g/ml? B. A solid has a mass of 0.025 kg per 100 cm 3, what is the density in g/cm 3 ? 1.04 g/ml 0.25 g/cm 3

65 Now to ramp it up a bit… Calculate the density of the following materials in g/ml. A. 49 lbs./fl. oz. B. 3.79 × 10 -4 kg/l A. 751.65 g/ml B. 3.79 × 10 -4 g/ml

66 How to use Dimensional Analysis Trust me, it will help.

67 Let us look at this one again… Calculate the density of the following materials in g/ml. A. 49 lbs./fl. oz.

68 What are you trying to determine?

69 Let us look at this one again… Calculate the density of the following materials in g/ml. A. 49 lbs./fl. oz. How many grams/ml?

70 Right, but let’s rewrite that…

71 Let us look at this one again… Calculate the density of the following materials in g/ml. A. 49 lbs./fl. oz.

72 Now put in what we know already…

73 Let us look at this one again… Calculate the density of the following materials in g/ml. A. 49 lbs./fl. oz.

74 Now we need to go from one set of units to the other, do them one at a time. Let’s start with the pounds…

75 Let us look at this one again… Calculate the density of the following materials in g/ml. A. 49 lbs./fl. oz.

76 Notice how pounds are above and below the fraction line. These cancel out each other. If we solve it here, we would be in g/fl. oz.

77 Let us look at this one again… Calculate the density of the following materials in g/ml. A. 49 lbs./fl. oz.

78 Now do the same with the fluid ounces to milliliters.

79 Let us look at this one again… Calculate the density of the following materials in g/ml. A. 49 lbs./fl. oz.

80 See how each step is another step towards what we were looking for, now the fl. oz. cancel.

81 Let us look at this one again… Calculate the density of the following materials in g/ml. A. 49 lbs./fl. oz.

82 Now when we plug and chug the only units left are g/ml… time to hit the calculator.

83 Let us look at this one again… Calculate the density of the following materials in g/ml. A. 49 lbs./fl. oz.

84 Significant Figures


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