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Chapter1 120319075352-phpapp02
1.
Chapter 1 Basic Concepts About
Matter
2.
Chapter 1 Table of
Contents Copyright © Cengage Learning. All rights reserved 2 1.1 Chemistry: The Study of Matter 1.2 Physical States of Matter 1.3 Properties of Matter 1.4 Changes in Matter 1.5 Pure Substances and Mixtures 1.6 Elements and Compounds 1.7 Discovery and Abundance of the Elements 1.8 Names and Chemical Symbols of the Elements 1.9 Atoms and Molecules 1.10 Chemical Formulas
3.
Chemistry: The Study
of Matter Return to TOC Section 1.1 Copyright © Cengage Learning. All rights reserved 3 • The field of study concerned with the characteristics, composition, and transformations of matter. What is Chemistry?
4.
Chemistry: The Study
of Matter Return to TOC Section 1.1 Copyright © Cengage Learning. All rights reserved 4 • Anything that has mass and occupies space. – Mass refers to the amount of matter present in a sample. Matter
5.
Chemistry: The Study
of Matter Return to TOC Section 1.1 Copyright © Cengage Learning. All rights reserved 5 • Includes all things – both living and nonliving Examples: plants, soil, air, bacteria • Various forms of energy such as heat, light, and electricity are not considered to be matter. • The universe is composed entirely of matter and energy. Matter
6.
Section 1.2 Physical States
of Matter Return to TOC Copyright © Cengage Learning. All rights reserved 6 • The classification of a given matter sample in terms of physical state is based on whether its shape and volume are definite or indefinite. • Matter exists in three physical states: Solid Liquid Gas
7.
Section 1.2 Physical States
of Matter Return to TOC Copyright © Cengage Learning. All rights reserved 7 Examples of the Three States of Matter
8.
Section 1.2 Physical States
of Matter Return to TOC Copyright © Cengage Learning. All rights reserved 8 • Physical state characterized by a definite shape and a definite volume. Solid
9.
Section 1.2 Physical States
of Matter Return to TOC Copyright © Cengage Learning. All rights reserved 9 Structure of a Solid
10.
Section 1.2 Physical States
of Matter Return to TOC Copyright © Cengage Learning. All rights reserved 10 • Physical state characterized by an indefinite shape and a definite volume. • Always takes the shape of its container to the extent that it fills the container. Liquid
11.
Section 1.2 Physical States
of Matter Return to TOC Copyright © Cengage Learning. All rights reserved 11 Structure of a Liquid
12.
Section 1.2 Physical States
of Matter Return to TOC Copyright © Cengage Learning. All rights reserved 12 • Physical state characterized by an indefinite shape and an indefinite volume. • Always completely fills its container, adopting both the container’s volume and its shape. Gas
13.
Section 1.2 Physical States
of Matter Return to TOC Copyright © Cengage Learning. All rights reserved 13 Structure of a Gas
14.
Section 1.2 Physical States
of Matter Return to TOC Copyright © Cengage Learning. All rights reserved 14 • The state of matter observed for a particular substance depends on its: – Temperature – Surrounding pressure – Strength of the forces holding its structural particles together
15.
Section 1.2 Physical States
of Matter Return to TOC Copyright © Cengage Learning. All rights reserved 15 Water Can Be Found in All Three States Simultaneously
16.
Section 1.3 Properties of
Matter Return to TOC Copyright © Cengage Learning. All rights reserved 16 • Distinguishing characteristic of a substance that is used in its identification and description. • Each substance has a unique set of properties that distinguishes it from all other substances. • Two General Types: Physical Chemical Property
17.
Section 1.3 Properties of
Matter Return to TOC Copyright © Cengage Learning. All rights reserved 17 • Characteristic of a substance that can be observed without changing the basic identity of the substance. – Color, odor, physical state, melting point, boiling point, and hardness Physical Property
18.
Section 1.3 Properties of
Matter Return to TOC Copyright © Cengage Learning. All rights reserved 18 Concept Check To measure the boiling point of a substance, a liquid must be changed into a gas. Why is boiling point considered a physical property when a gas’ appearance is much different from that of a liquid? Although the appearance is different, the substance is still the same. It’s chemical identity has not changed.
19.
Section 1.3 Properties of
Matter Return to TOC Copyright © Cengage Learning. All rights reserved 19 • Characteristic of a substance that describes the way the substance undergoes or resists change to form a new substance. Example: copper objects turn green in air • Most often the changes result from the reaction of a substance with one or more other substances. • Sometimes energy (like heat or light) can trigger a change (decomposition). Chemical Property
20.
Section 1.3 Properties of
Matter Return to TOC Copyright © Cengage Learning. All rights reserved 20 A Chemical Property of Copper
21.
Section 1.3 Properties of
Matter Return to TOC Copyright © Cengage Learning. All rights reserved 21 Exercise Classify each of the following as a physical or chemical property. a) A marshmallow gets black when roasting it in a campfire. chemical property b) Zinc is a solid at room temperature. physical property c) When rubbing alcohol is rubbed on your skin, it evaporates very quickly. physical property
22.
Section 1.4 Changes in
Matter Return to TOC Copyright © Cengage Learning. All rights reserved 22 • Process in which a substance changes its physical appearance but not its chemical composition. • A new substance is never formed as a result of a physical change. Example: boiling or freezing water Physical Change
23.
Section 1.4 Changes in
Matter Return to TOC Copyright © Cengage Learning. All rights reserved 23 • A process in which a substance undergoes a change in chemical composition. • Involves conversion of the material(s) into one or more new substances. Example: methane reacts with oxygen to form carbon dioxide and water Chemical Change
24.
Section 1.4 Changes in
Matter Return to TOC Copyright © Cengage Learning. All rights reserved 24 Use of the Term Physical
25.
Section 1.4 Changes in
Matter Return to TOC Copyright © Cengage Learning. All rights reserved 25 Use of the Term Chemical
26.
Section 1.4 Changes in
Matter Return to TOC Copyright © Cengage Learning. All rights reserved 26 Concept Check Which one of the following are examples of a chemical change? Pulverizing (crushing) rock salt Burning of wood Dissolving of sugar in water Melting a popsicle on a warm summer day
27.
Section 1.5 Pure Substances
and Mixtures Return to TOC Copyright © Cengage Learning. All rights reserved 27 • Pure substance – a single kind of matter that cannot be separated into other kinds of matter by any physical means. Examples: water or carbon dioxide • Mixture – a physical combination of two or more pure substances in which each substance retains its own chemical identity. Example: salt water Pure Substances vs. Mixtures
28.
Section 1.5 Pure Substances
and Mixtures Return to TOC Copyright © Cengage Learning. All rights reserved 28 • Have variable composition Mixtures Homogeneous Mixture: Heterogeneous Mixture: • Contains only one visibly distinct phase (part), which has uniform properties throughout; solution • Contains visibly different phases (parts), each of which has different properties
29.
Section 1.5 Pure Substances
and Mixtures Return to TOC Copyright © Cengage Learning. All rights reserved 29 Homogeneous Mixtures
30.
Section 1.5 Pure Substances
and Mixtures Return to TOC Copyright © Cengage Learning. All rights reserved 30 Homogeneous vs. Heterogeneous Mixtures
31.
Section 1.5 Pure Substances
and Mixtures Return to TOC Copyright © Cengage Learning. All rights reserved 31
32.
Section 1.5 Pure Substances
and Mixtures Return to TOC Copyright © Cengage Learning. All rights reserved 32 Concept Check Which of the following is a homogeneous mixture? Pure water Gasoline Jar of jelly beans Soil Copper metal
33.
Section 1.6 Elements and
Compounds Return to TOC Copyright © Cengage Learning. All rights reserved 33 • Element – a pure substance that cannot be broken down into simpler pure substances by chemical means such as a chemical reaction, an electric current, heat, or a beam of light. Examples: gold, silver, copper Element
34.
Section 1.6 Elements and
Compounds Return to TOC Copyright © Cengage Learning. All rights reserved 34 • Compound – a pure substance that can be broken down into two or more simpler pure substances by chemical means. Examples: water, carbon dioxide, ammonia Compound
35.
Section 1.6 Elements and
Compounds Return to TOC Copyright © Cengage Learning. All rights reserved 35 A Pure Substance Can Be Either An Element or Compound
36.
Section 1.6 Elements and
Compounds Return to TOC Copyright © Cengage Learning. All rights reserved 36 Compound vs. Mixture
37.
Section 1.6 Elements and
Compounds Return to TOC Copyright © Cengage Learning. All rights reserved 37 1) Compounds have properties distinctly different from those of the substances that combined to form the compound. The components of mixtures retain their individual properties. Distinguishing Between Compounds and Mixtures
38.
Section 1.6 Elements and
Compounds Return to TOC Copyright © Cengage Learning. All rights reserved 38 2) Compounds have a definite composition. Mixtures have a variable composition. Distinguishing Between Compounds and Mixtures
39.
Section 1.6 Elements and
Compounds Return to TOC Copyright © Cengage Learning. All rights reserved 39 3) Physical methods are sufficient to separate the components of a mixture. The components of a compound cannot be separated by physical methods; chemical methods are required. Distinguishing Between Compounds and Mixtures
40.
Section 1.6 Elements and
Compounds Return to TOC Copyright © Cengage Learning. All rights reserved 40 1) Does the sample of matter have the same properties throughout? 2) Are two or more different substances present? 3) Can the pure substance be broken down into simpler substances? To Classify a Sample of Matter
41.
Section 1.7 Discovery and
Abundance of the Elements Return to TOC Copyright © Cengage Learning. All rights reserved 41 • 117 known elements: 88 of the elements occur naturally 29 of the elements have been synthesized
42.
Section 1.7 Discovery and
Abundance of the Elements Return to TOC Copyright © Cengage Learning. All rights reserved 42 Abundance of Elements (in Atom Percent) in the Universe
43.
Section 1.7 Discovery and
Abundance of the Elements Return to TOC Copyright © Cengage Learning. All rights reserved 43 Abundance of Elements (in Atom Percent) in the Earth’s Crust
44.
Section 1.7 Discovery and
Abundance of the Elements Return to TOC Copyright © Cengage Learning. All rights reserved 44 Elemental Composition of the Human Body (in Atom Percent)
45.
Section 1.8 Names and
Chemical Symbols of the Elements Return to TOC Copyright © Cengage Learning. All rights reserved 45 • One- or two-letter designation for an element derived from the element’s name. • Two letter symbols are often, but not always, the first two letters of the element’s name. Chemical Symbol
46.
Section 1.8 Names and
Chemical Symbols of the Elements Return to TOC Copyright © Cengage Learning. All rights reserved 46 • First letter of a chemical symbol is always capitalized and the second is not: H – hydrogen Ba – barium Co – cobalt Pb – lead Ag – silver Chemical Symbol
47.
Section 1.8 Names and
Chemical Symbols of the Elements Return to TOC Copyright © Cengage Learning. All rights reserved 47 • For some elements, the symbol is derived from the Latin name of the element: Ag – silver Au – gold Fe – iron Pb – lead Cu – copper Latin Names
48.
Section 1.9 Atoms and
Molecules Return to TOC Copyright © Cengage Learning. All rights reserved 48 • The smallest particle of an element that can exist and still have the properties of the element. • The limit of chemical subdivision. • Atoms are extremely small particles. Atom
49.
Section 1.9 Atoms and
Molecules Return to TOC Copyright © Cengage Learning. All rights reserved 49 • Group of two or more atoms that functions as a unit because the atoms are tightly bound together. • The limit of physical subdivision. • Behaves in many ways as a single, distinct particle would. • Diatomic molecule – contains two atoms • Triatomic molecule – contains three atoms • Tetraatomic, pentatomic, etc. Molecule
50.
Section 1.9 Atoms and
Molecules Return to TOC Copyright © Cengage Learning. All rights reserved 50 • Molecule in which all atoms present are of the same kind. • Substance containing homoatomic molecules must be an element. Examples: H2, O2, N2, Cl2, P4, S8 Homoatomic Molecule
51.
Section 1.9 Atoms and
Molecules Return to TOC Copyright © Cengage Learning. All rights reserved 51 Homoatomic Molecules
52.
Section 1.9 Atoms and
Molecules Return to TOC Copyright © Cengage Learning. All rights reserved 52 • Molecule in which two or more kinds of atoms are present. • Substance containing heteroatomic molecules must be compounds. Examples: H2O, CO2, N2O4, C12H22O11 Heteroatomic Molecule
53.
Section 1.9 Atoms and
Molecules Return to TOC Copyright © Cengage Learning. All rights reserved 53 Heteroatomic Molecules
54.
Section 1.9 Atoms and
Molecules Return to TOC Copyright © Cengage Learning. All rights reserved 54 Concept Check Classify XeF4 as: 1)diatomic, triatomic, etc. pentatomic 2)homoatomic or heteroatomic heteroatomic 3)element or compound compound
55.
Section 1.10 Chemical Formulas Return
to TOC Copyright © Cengage Learning. All rights reserved 55 • A notation made up of the chemical symbols of the elements present in a compound and numerical subscripts (located to the right of each chemical symbol) that indicate the number of atoms of each element present in a molecule of the compound. Examples: H2O – two atoms of hydrogen, one atom of oxygen Ca3(PO4)2 – three atoms of calcium, two atoms of phosphorus, eight atoms of oxygen
56.
Section 1.10 Chemical Formulas Return
to TOC Copyright © Cengage Learning. All rights reserved 56 Exercise For each of the following chemical formulas, determine how many atoms of each element are present: a) H2SO4 two hydrogen; one sulfur; four oxygen b) Fe2(CO3)3 two iron; three carbon; nine oxygen
Editor's Notes
Although the appearance is different, the substance is still the same. It’s chemical identity has not changed.
Chemical property Physical property Physical property
1 (burning of wood)
gasoline
Although the appearance is different, the substance is still the same. It’s chemical identity has not changed.
Chemical property Physical property Physical property
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