Chapter 1. Matter. Table of Contents. 1. Matter 2. States of Matter 3. Classification of Matter 4. Properties of Matter 5. Separation of Mixtures
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1 Matter Table of Contents 1. Matter 2. States of Matter 3. Classification of Matter 4. Properties of Matter 5. Separation of Mixtures
2 1. Matter Warm up Look at the list of words below: peanut butter, water, fish, light, garbage, time, motion, the human brain, carbon dioxide, air, yourself, an idea, tree, energy, wind, dream, atom Sort the words into three categories: matter, not matter, or not sure. Why is a clear definition of matter important to the study of chemistry?
3 1. Matter Matter is the stuff that s all around you: the metal and plastic of a telephone, the paper and ink of a book, the glass and liquid of a bottle of soda, the air you breathe, and the materials that make up your body. A more formal definition of matter is anything that takes up space and has mass. Mass or weight?
4 1. Matter
5 1. Matter Is air matter, too?
6 1. Matter Air has mass.
7 1. Matter What about fire?
8 1. Matter Section Review 1. Which one is not matter and why? A. Helium gas B. Water C. Salt D. Space
9 1. Matter Section Review 1. Which one is not matter and why? A. Helium gas B. Water C. Salt D. Space
10 1. Matter Section Review 2. Matter includes all of the following EXCEPT? A. Air B. smoke C. spray D. nightmare
11 1. Matter Section Review 2. Matter includes all of the following EXCEPT? A. Air B. smoke C. spray D. nightmare
12 1. Matter Section Review 3. Two features that distinguish matter are A. Mass and velocity B. Weight and velocity C. Mass and volume D. Weight and volume
13 1. Matter Section Review 3. Two features that distinguish matter are A. Mass and velocity B. Weight and velocity C. Mass and volume D. Weight and volume
14 1. Matter Section Review 4. How do you describe a block of wood is a matter? 4. Matter has two common properties, mass and volume. Mass of wood block can be measured and its volume is calculated from its height, depth and length.
15 1. Matter Section Review 5. How does mass differ from weight? 5. Mass is the quantity of matter, measured by equal arm balance, and is constant in everywhere. But weight is the force applied on matter by gravity, is measured by spring balance, and is not constant in everywhere.
16 2. States of Matter Warm up List down some consumer products in different states of matter. Which states of matter are common and which of them are rare? What are the substances in your body found in different states?
17 2. States of Matter The states of matter are the physical forms of matter which are solid, liquid, gas, and plasma.
18 2. States of Matter In solid state, definite shape and volume, particles are very close to each other. In liquid state, definite volume, but not definite shape, particles move and slide over one another. In gaseous state, not definite volume or shape, move freely in all directions, far apart from one another. Plasma state can be seen at extremely hot temperatures. Stars, lightning, sun, fluorescent light are examples for plasma state.
19 2. States of Matter
20 2. States of Matter
21 2. States of Matter
22 2. States of Matter Phase Change
23 2. States of Matter Phase Change
24 2. States of Matter
25 2. States of Matter
26 2. States of Matter
27 2. States of Matter Section Review 1. In Which state of matter particles are able to move in all directions? A. Liquid B. Gaseous C. Solid D. Plasma
28 2. States of Matter Section Review 1. In Which state of matter particles are able to move in all directions? A. Liquid B. Gaseous C. Solid D. Plasma
29 2. States of Matter Section Review 2. What are the physical state of clouds, rain and snow? A. solid, liquid, gaseous B. liquid, gaseous, solid C. solid, liquid, liquid D. gaseous, liquid, solid
30 2. States of Matter Section Review 2. What are the physical state of clouds, rain and snow? A. solid, liquid, gaseous B. liquid, gaseous, solid C. solid, liquid, liquid D. gaseous, liquid, solid
31 2. States of Matter Section Review 3. Which of the following substances are able to expand and fill their containers? apple, gasoline, air, orange juice, stone, water steam A. apple, orange juice, stone B. gasoline, air, water steam C. air, water steam D. orange juice, gasoline
32 2. States of Matter Section Review 3. Which of the following substances are able to expand and fill their containers? apple, gasoline, air, orange juice, stone, water steam A. apple, orange juice, stone B. gasoline, air, water steam C. air, water steam D. orange juice, gasoline
33 2. States of Matter Section Review 4. Which of the following characteristics of matter in liquid state? A. Definite volume B. Shapeless C. Its particles can move and slide over one another. D. All of the above
34 2. States of Matter Section Review 4. Which of the following characteristics of matter in liquid state? A. Definite volume B. Shapeless C. Its particles can move and slide over one another. D. All of the above
35 2. States of Matter Section Review 5. What is called when matter becomes gaseous from solid state? A. Sublimation B. Deposition C. Boiling D. Freezing
36 2. States of Matter Section Review 5. What is called when matter becomes gaseous from solid state? A. Sublimation B. Deposition C. Boiling D. Freezing
37 2. States of Matter Section Review 6. The state of matter in which particles are rigidly held in fixed positions is the A. vaporous state. B. gaseous state. C. solid state. D. liquid state.
38 2. States of Matter Section Review 6. The state of matter in which particles are rigidly held in fixed positions is the A. vaporous state. B. gaseous state. C. solid state. D. liquid state.
39 2. States of Matter Section Review 7. A sample of matter can be poured from container to container. It takes the shape of its container but only takes up a certain volume. Based on this information, the sample is in the state.
40 2. States of Matter Section Review 7. A sample of matter can be poured from container to container. It takes the shape of its container but only takes up a certain volume. Based on this information, the sample is in the liquid state.
41 2. States of Matter Section Review 8. Why can a gas fill the entire volume of its container? 8. Gas particles have little attraction for each other and can easily and quickly move from one place to another.
42 3. Classification of Matter Warm up List down some matters that you usually use and classify them with respect to usages? What are the criteria to classify matter? What are the benefits of classifying matter?
43 3. Classification of Matter Classifying Matter
44 3. Classification of Matter Pure substances A pure substance is a sample of matter, either a single element or a single compound, that has definite chemical and physical properties.
45 3. Classification of Matter Elements Elements are pure substances that contain one kind of atom. shown by symbols such as Ag, S, C, Na, Ca, Li, O, H etc. There are 116 elements known today, 92 of them are natural. cannot be broken down into another substances. smallest unit of an element is an atom. some elements, such as oxygen, phosphorus, sulfur, and carbon, have many different molecular forms. An allotrope is one of a number of different molecular forms of an element.
46 3. Classification of Matter Elements, continued Elements are further classified as metals and non metals. Metals, are good conductors of electricity, are solids at room temperature (25 o C), except Hg, have metallic shiny color, can be hammered into sheets, malleability can be drawn into wires, ductility.
47 3. Classification of Matter Metals and Nonmetals in the periodic table
48 3. Classification of Matter Some Metals and Their uses Lithium, Li
49 3. Classification of Matter Some Metals and Their uses Sodium, Na
50 3. Classification of Matter Some Metals and Their uses Potassium, K
51 3. Classification of Matter Some Metals and Their uses Calcium, Ca
52 3. Classification of Matter Some Metals and Their uses Chromium, Cr
53 3. Classification of Matter Some Metals and Their uses Iron, Fe
54 3. Classification of Matter Some Metals and Their uses Gold, Au
55 3. Classification of Matter Elements, continued Nonmetals, don not conduct electricity, except for graphite. can be solid, liquid, or gaseous at room temperature, have dull color, are brittle, can not be drawn into wires.
56 3. Classification of Matter Some Nonmetals and Their uses Carbon, C
57 3. Classification of Matter Some Nonmetals and Their uses Phosphorus, P
58 3. Classification of Matter Some Nonmetals and Their uses Nitrogen, N
59 3. Classification of Matter Some Nonmetals and Their uses Oxygen, O
60 3. Classification of Matter Comparing Metals, Metalloids and Nonmetals
61 3. Classification of Matter Metalloids
62 3. Classification of Matter Comparing Metals, Metalloids and Nonmetals
63 3. Classification of Matter
64 3. Classification of Matter Compounds A compound is a chemical combination of two or more different elements joined together in a fixed proportion with a unique set of chemical and physical properties. A molecule is the smallest unit of a compound. Water we drink, hydrochloric acid in our stomach, sodium chloride as a table salt etc are all compounds. More than 10 million compounds are known and the number keeps growing.
65 3. Classification of Matter Compounds, continued The properties of the compound are different from the properties of the elements that compose the compound. silver + bromine = silver bromide
66 3. Classification of Matter Compounds, continued
67 3. Classification of Matter Compounds, continued
68 3. Classification of Matter Compounds, continued A formula is a combination of the chemical symbols that show what elements make up a compound and the number of atoms of each element. Compound Formula Caffeine C 8 H 10 N 4 O 2 Sugar C 6 H 12 O 6 Salt NaCl Compounds can be broken down into their elements, though often with great difficulty.
69 3. Classification of Matter Mixtures A mixture is a combination of two or more substances that are not chemically combined. An alloy is a solid mixture.
70 3. Classification of Matter Mixtures, continued Mixtures; proportions of materials can change, properties reflect the properties of the substances it contains, can be decomposed into components by physical methods, can be either homogeneous or heterogeneous. A homogenous mixture describes something that has uniform structure or composition throughout. Air, gasoline, syrup, vinegar, coins, salty water, etc are homogeneous mixtures. They are called solutions as well.
71 3. Classification of Matter Mixtures, continued
72 3. Classification of Matter Mixtures, continued A heterogeneous mixture has different properties in different regions of the mixture. Sand-water, oil-water, soil, tea, milk, blood, fog, etc are heterogeneous mixtures.
73 3. Classification of Matter Mixtures, continued A heterogeneous mixture has different properties in different regions of the mixture. Sand-water, oil-water, soil, tea, milk, blood, fog, etc are heterogeneous mixtures.
74 3. Classification of Matter Mixtures, continued
75 3. Classification of Matter Section Review 1. Which is NOT a property of metals? A. malleability B. ability to conduct heat and electricity C. unreactivity D. capable of being stretched
76 3. Classification of Matter Section Review 1. Which is NOT a property of metals? A. malleability B. ability to conduct heat and electricity C. unreactivity D. capable of being stretched
77 3. Classification of Matter Section Review 2. Which statement is NOT true for nonmetals? A. They have characteristics of both metals and nonmetals. B. Many are gases at room temperature. C. They have low conductivity. D. There are fewer nonmetals than metals.
78 3. Classification of Matter Section Review 2. Which statement is NOT true for nonmetals? A. They have characteristics of both metals and nonmetals. B. Many are gases at room temperature. C. They have low conductivity. D. There are fewer nonmetals than metals.
79 3. Classification of Matter Section Review 3. A list of pure substances could include A. bread dough. B. vinegar (5% acetic acid). C. vitamin C (ascorbic acid). D. sea water.
80 3. Classification of Matter Section Review 3. A list of pure substances could include A. bread dough. B. vinegar (5% acetic acid). C. vitamin C (ascorbic acid). D. sea water.
81 3. Classification of Matter Section Review 4. Which of the following is an element? A. BaCl 2 B. CO C. Ne D. CaCO 3
82 3. Classification of Matter Section Review 4. Which of the following is an element? A. BaCl 2 B. CO C. Ne D. CaCO 3
83 3. Classification of Matter Section Review 5. The mixtures which have uniform structure are A. blood, rain water and air. B. carbon dioxide in water, bronze and steel. C. soil, cement and dust in air. D. alcohol-water, tea, aspirin.
84 3. Classification of Matter Section Review 5. The mixtures which have uniform structure are A. blood, rain water and air. B. carbon dioxide in water, bronze and steel. C. soil, cement and dust in air. D. alcohol-water, tea, aspirin.
85 3. Classification of Matter Section Review 6. Which of the following statements about compounds is true? A. A compound contains only one element. B. A compound can be classified as either heterogeneous or homogeneous. C. A compound has a defined ratio by mass of the elements that it contains. D. A compound varies in chemical composition depending on the sample size.
86 3. Classification of Matter Section Review 6. Which of the following statements about compounds is true? A. A compound contains only one element. B. A compound can be classified as either heterogeneous or homogeneous. C. A compound has a defined ratio by mass of the elements that it contains. D. A compound varies in chemical composition depending on the sample size.
87 3. Classification of Matter Section Review 7. The two types of matter that are pure substances are and. 7. The two types of matter that are pure substances are elements and compounds.
88 3. Classification of Matter Section Review 8. Identify the pure substances below Air, He, brass, soil, water, vinegar, ketchup, ice, milk, sodium, sugar, tea, cake, table salt, blood A. Air, vinegar, ice, blood, sugar, milk B. Cake, water,, ice, sodium, He C. Water, tea, milk, table salt, sugar, brass D. He, water, ice, sodium, sugar, table salt
89 3. Classification of Matter Section Review 8. Identify the pure substances below Air, He, brass, soil, water, vinegar, ketchup, ice, milk, sodium, sugar, tea, cake, table salt, blood A. Air, vinegar, ice, blood, sugar, milk B. Cake, water,, ice, sodium, He C. Water, tea, milk, table salt, sugar, brass D. He, water, ice, sodium, sugar, table salt
90 3. Classification of Matter Section Review 9. Iron and sulfur, when heated, form an iron sulfide that has different properties from either iron or sulfur. This iron sulfide is an example of a(n). 9. Iron and sulfur, when heated, form an iron sulfide that has different properties from either iron or sulfur. This iron sulfide is an example of a compound.
91 3. Classification of Matter Section Review 10. Mach the column A and B A B 1. Salty water 2. Iron 3. Ammonia 4. Milk 1. Compound 2. Homogeneous mixture 3. Heterogeneous mixture 4. Element
92 4. Properties of Matter Warm up List down some items in your classroom and define them with some properties. How do you change some properties of matter? For example cutting paper. Which of these properties are reversible?
93 4. Properties of Matter
94 4. Properties of Matter Chemical Properties The ability of a substance to combine with or change into one or more other substances is called a chemical property. Flammability, rusting, acidity, reactivity with water are examples for chemical properties. A chemical change occurs whenever a new substance is made.
95 4. Properties of Matter Physical Properties A physical property of a substance is a characteristic that does not involve a chemical change. Physical properties can be extensive or intensive. Mass, volume, or weight are extensive properties of matter. Intensive properties of matter do not depend on the amount given. They are sometimes called distinctive or characteristic properties. Color, odor, taste, solubility, density, conductivity, melting and boiling points, hardness, luster, etc are all intensive properties.
96 4. Properties of Matter
97 4. Properties of Matter Physical Properties
98 4. Properties of Matter Physical Properties, continued Physical properties of a substance can be determined without changing the nature of a substance.
99 4. Properties of Matter Physical Properties, continued a. Density The density of an object is the mass of the object divided by volume of the object. mass m density = or d = volume v Densities are expressed in derived units such as g/cm 3 or g/ml. The density of a substance is the same no mater what the size of the sample is.
100 4. Properties of Matter Physical Properties, continued a. Density
101 4. Properties of Matter Physical Properties, continued Because the density of a substance is the same for all samples, you can use this property to help identify substances.
102 4. Properties of Matter Physical Properties, continued Example 1 Calculate the density of 105 g silver with a volume of 10 cm 3. Solution
103 4. Properties of Matter Physical Properties, continued Example 2 Calculate the mass of a cubic iron block with a 3-cm side length. (d Fe = 7.86 g/cm 3 ) Solution
104 4. Properties of Matter Physical Properties, continued
105 As it s known, substance expands in volume when it is heated. Whereas, temperature of water raises from 0 o C up to 4 o C, its volume instead of increasing decreases. That s why ten thousand tones icebergs in spite of their weight floats on the water.
106 4. Properties of Matter Physical Properties, continued b. Melting Point (mp) and Freezing Point (fp) Melting point is the temperature at which a solid starts to become a liquid. And freezing point is the temperature of the reverse change. For example water melts or freezes at 0 o C whereas iron melts 1535 o C. b. Boiling Point (bp) A boiling point is a temperature at which a liquid becomes a gas. For instance alcohol boils at 78 o C, but it is 1 o C for butane gas. Boiling point depends on pressure. Evaporation or boiling?
107 4. Properties of Matter Physical Properties, continued
108 4. Properties of Matter Physical Properties, continued
109 4. Properties of Matter Physical Properties, continued
110 4. Properties of Matter Physical Properties, continued Example 3 Find the physical states of the substances A, B and C at room temperature. Substance Melting Point ( o C) Boiling Point ( o C) A B C Solution A is gas, B is solid, C is liquid.
111 4. Properties of Matter Physical Properties, continued d. Solubility Solubility is the a amount of substance dissolved in a given solvent at a given temperature. A solutions is prepared by dissolving a solute in a solvent. Solubility of substances are measured in 100 g H 2 O at a particular temperature. For instance solubility of sugar is 190 g /100 g H 2 O at 20 o C, while it is 10 g /100 g H 2 O for baking soda.
112 4. Properties of Matter Section Review 1. Osmium, Os, is the densest metal known. What is its density in g/cm 3 when 50 g of a sample of Os occupies 2.22 cm 3 volume? 1.
113 4. Properties of Matter Section Review 2. You are given three samples of wood, copper and plastic rod with densities of 0.6 g/cm 3, 7.86 g/cm 3 and 1.02 g/cm 3, respectively. How do they stand when they are put in water?(assume density of water is 1 g/cm 3 )
114 4. Properties of Matter Section Review 2. The densest one is copper, it is placed at the bottom. Plastic rod has the same density with water, therefore it stands wherever it is put. Wood, has the least density among all, floats above water.
115 4. Properties of Matter Section Review 3. How many phase changes occur when an ice cube is heated until all becomes gas at 130 o C? A. 1 B. 2 C. 3 D. 4
116 4. Properties of Matter Section Review 3. How many phase changes occur when an ice cube is heated until all becomes gas at 130 o C? A. 1 B. 2 C. 3 D. 4
117 4. Properties of Matter Section Review 4. Which of the following can be used to identify substances? A. Volume B. Solubility C. Mass D. Length
118 4. Properties of Matter Section Review 4. Which of the following can be used to identify substances? A. Volume B. Solubility C. Mass D. Length
119 4. Properties of Matter Section Review 5. Find the physical states of the substances X, Y and Z at 45 o C. Substance Melting Point ( o C) Boiling Point ( o C) X Y Z X is gas, Y and Z are liquids.
120 4. Properties of Matter Section Review 6. Why does water boil at the peak of Mt.Everest at 70 o C but not at 100 o C? 6. Because liquids boil when their vapor pressures equal to air pressure. And air pressure is lower at higher altitudes than that of sea level.
121 5. Separation of Mixtures Warm up How do you separate oil from water? Which properties of matter can be used to separate mixtures, chemical or physical? Why do we need to separate mixtures?
122 5. Separation of Mixtures A. By Means of The Use of Electricity In a mixture if one component is attracted by electricity it can be separated from the mixture by electrified objects. For example in pepper-salt mixture pepper can be removed by electrified ebonite rod. B. By Means of The Use of A Magnet Iron, cobalt and nickel are the metals which are attracted by magnet. Mixtures containing one of these metals can be separated by use of magnet. For example iron-sulfur powder is separated by magnet.
123 5. Separation of Mixtures C. By Means of Density Differences Mixtures containing immiscible liquids can be separated by using density differences. For instance oil-water mixture is separated by using a separatory funnel in this technique. D. By Means of Solubility Some mixtures such as sand-salt contain substances with different solubilities. These type of mixtures can easily be separated by using filter paper. Only soluble component is able to pass through filter paper.
124 5. Separation of Mixtures E. By Means of The Process of Distillation Mixtures containing miscible liquids can be separated by distillation process. For example alcohol-water solution in which its components have different boiling points is separated by distillation. Petroleum refining is a good example for distillation in industry.
125 5. Separation of Mixtures E. By Means of The Process of Distillation
126 5. Separation of Mixtures Section Review 1.Which method can be used to separate salty water? A. Distillation B. Filtration C. Evaporation D. By using magnet
127 5. Separation of Mixtures Section Review 1.Which method can be used to separate salty water? A. Distillation B. Filtration C. Evaporation D. By using magnet
128 5. Separation of Mixtures Section Review 2.Which of the following substances can be separated by physical methods? oil-water, CO 2 gas, vinegar, Zn, salt-iron powder, soil, HCl, ayran, H 2 O A. CO 2 gas, H 2 O, Zn, HCl B. oil-water, CO 2 gas, vinegar, H 2 O C. salt-iron powder, ayran, HCl, soil D. ayran, oil-water, vinegar, salt-iron powder, soil
129 5. Separation of Mixtures Section Review 2.Which of the following substances can be separated by physical methods? oil-water, CO 2 gas, vinegar, Zn, salt-iron powder, soil, HCl, ayran, H 2 O A. CO 2 gas, H 2 O, Zn, HCl B. oil-water, CO 2 gas, vinegar, H 2 O C. salt-iron powder, ayran, HCl, soil D. ayran, oil-water, vinegar, salt-iron powder, soil
130 5. Separation of Mixtures Section Review 3. In the separation of petroleum which property of matter is used? A. Density B. Solubility C. Conductivity D. Boiling point
131 5. Separation of Mixtures Section Review 3. In the separation of petroleum which property of matter is used? A. Density B. Solubility C. Conductivity D. Boiling point
132 5. Separation of Mixtures Section Review 4. In the separation of salt-sand-naphthalene mixture which component is separated first? A. naphthalene B. sand C. salt
133 5. Separation of Mixtures Section Review 4. In the separation of salt-sand-naphthalene mixture which component is separated first? A. naphthalene B. sand C. salt
134 5. Separation of Mixtures Section Review 5. Suggest a method to separate a mixture of salt-chalk dust. 5. First mixture is put in some water. Salt is miscible in water but not chalk dust, it dissolves thus chalk dust separated from the mixture by filtration. To separate salt from water it must be evaporated.
135 End of the chapter 2
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