Matter Chapter 3 1

Why does soda fizz when you open the bottle? Why is the sun hot? When iron rusts, what’s happening?

Copyright©2004 by Houghton Mifflin Company. All rights reserved. Objectives Observe and explain the difference between states of matter. Copyright©2004 by Houghton Mifflin Company. All rights reserved.

3-1 Universe Classified Matter is the part of the universe that has mass and volume There are three states of matter Solid, liquid, and gas Chemistry is the study of matter The properties of different types of matter The way matter behaves when influenced by other matter and/or energy 3

Some Criteria for the Classification of Matter Composition (elements and compounds) State (solid, liquid, gas) Properties

States of Matter YES YES YES YES YES NO YES NO NO NO NO YES Property Solid Liquid Gas Definite mass Definite volume Definite shape Compressible Molecule Drawing Examples YES YES YES YES YES NO YES NO NO NO NO YES

States of Matter Property Solid Liquid Gas Yes No Definite mass Definite volume No Definite shape Compressible Molecule Drawing Examples rock, cookie, gold bar Water, oil Air, helium, nitrogen

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Figure 3.1: Liquid water takes the shape of its container.

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Figure 3.11: In ice, the water molecules vibrate randomly about their positions in the solid. Their motions are represented by arrows. Copyright©2004 by Houghton Mifflin Company. All rights reserved. Copyright © Houghton Mifflin Company.All rights reserved.

Figure 3.12: Equal masses of hot water and cold water separated by a thin metal wall in an insulated box. Copyright©2004 by Houghton Mifflin Company. All rights reserved. Copyright © Houghton Mifflin Company.All rights reserved.

Figure 3.13: The H2O molecules in hot water have much greater random motions than the H2O molecules in cold water. Copyright©2004 by Houghton Mifflin Company. All rights reserved. Copyright © Houghton Mifflin Company.All rights reserved.

Figure 3.14: The water samples now have the same temperature (50°C) and have the same random motions. Copyright©2004 by Houghton Mifflin Company. All rights reserved. Copyright © Houghton Mifflin Company.All rights reserved.

Condensation gas  liquid Freezing liquid  solid Phase Changes Melting solid  liquid Condensation gas  liquid Freezing liquid  solid Deposition gas  solid Evaporation liquid  gas Sublimation solid  gas *Boiling: Evaporation occurring beneath the liquid’s surface.

Gallium metal has such a low melting point (30°C) that it melts from the heat of a hand.

NAME THAT PHASE CHANGE

Video - https://www.youtube.com/watch?v=wln6WSv-cro

Copyright©2004 by Houghton Mifflin Company. All rights reserved. Objectives Explain the difference between elements and compounds. Copyright©2004 by Houghton Mifflin Company. All rights reserved.

3-3 Elements and Compounds a pure substance same composition throughout Contains only one type of atom Can not be broken down into simpler substances by ordinary chemical reactions (not a nuclear reaction) 11

Chemical Symbols of Elements System started by Jons Berzelius (Sweden, 1779-1848) 90-91 naturally occurring elements One or two first letters of name of the element. Many elements names have roots from: Latin, Greek, mythology, geography, names of scientists.

Examples: Americium, Am Einsteinium, Es Bromine, Br Helium, He Lead(Plumbum), Pb Niobium, Nb Iron (Ferrum), Fe Mendelevium, Md Examples of other elements: O2, H2, I2

Compound – chemical combination of two or more elements Have two properties in common with elements: 1. pure substance 2. Homogeneous – same chemical composition at all times

Compounds cont. Have two properties that differ from elements: two or more elements that are chemically combined, in a definite ratio 2. Compounds can be broken down by chemical reactions using energy: a) decomposition - uses heat b) electrolysis - uses electricity

> 10 million compounds elements are represented by symbols compounds are represented by chemical formulas chemical formula 1. symbol --> tells which elements are present in compounds 2. subscript (little # lower right) --> tells the number of atoms of each element

Properties of Compounds Distinguishing Elements and Compounds Properties of Compounds Compounds have different properties from their individual elements. When the elements sodium and chlorine combine chemically to form sodium chloride, there is a change in composition and a change in properties. Sodium chloride (commonly known as table salt) is a white solid.

Breaking down Compounds Distinguishing Elements and Compounds Breaking down Compounds Breaking down NaCl Sodium is a soft gray metal.

Breaking down Compounds Distinguishing Elements and Compounds Breaking down Compounds Breaking down NaCl Chlorine is a pale yellow poisonous gas.

Classification of Matter (by composition)

Classification of Matter 12

3-4 Mixtures Mixtures can be classified as: Homogeneous Mixtures Heterogeneous Mixtures 12

Homogeneous mixture = uniform throughout, appears to be one layer Also called solutions Examples: olive oil, salt water, lemonade, coffee, air The substances in the olive oil are evenly distributed throughout the mixture

Example: Stainless Steel A homogeneous mixture of: -Iron (Fe) -Chromium (Cr) -Nickel (Ni)

Heterogeneous mixture = non-uniform, contains regions with different properties than other regions - Examples: oil and vinegar, salad, chicken soup

Pure Substances vs. Mixtures All samples have the same physical and chemical properties Constant Composition  all samples have the same composition Homogeneous Separate into components based on chemical properties Mixtures Different samples may show different properties Variable composition Homogeneous or Heterogeneous Separate into components based on physical properties All mixtures are made of pure substances 13

Figure 3.4: When table salt is stirred into water (left), a homogeneous mixture called a solution forms (right). Copyright©2004 by Houghton Mifflin Company. All rights reserved. Copyright © Houghton Mifflin Company.All rights reserved.

Copyright©2004 by Houghton Mifflin Company. All rights reserved. Identity Each of the following as a Pure Substance, Homogeneous Mixture or Heterogeneous Mixture Gasoline A stream with gravel on the bottom Copper metal Copyright©2004 by Houghton Mifflin Company. All rights reserved. 14

Copyright©2004 by Houghton Mifflin Company. All rights reserved. Identity Each of the following as a Pure Substance, Homogeneous Mixture or Heterogeneous Mixture Gasoline a homogenous mixture A stream with gravel on the bottom a heterogeneous mixture Copper metal A pure substance (all elements are pure substances) Copyright©2004 by Houghton Mifflin Company. All rights reserved. 15

3-5 Separation of Mixtures Separate mixtures based on different physical properties of the components Evaporation Volatility Chromatography Adherence to a Surface Filtration State of Matter (solid/liquid/gas) Distillation Boiling Point Technique Different Physical Property Copyright©2004 by Houghton Mifflin Company. All rights reserved. 16

Example: Separate iron filings from sulfur using a magnet.

Filtration: separates a solid from a liquid in a heterogeneous mixture

-separate dissolved solids from a liquid in a homogeneous mixture Figure 3.6: Distillation of a solution consisting of salt dissolved in water. -separate dissolved solids from a liquid in a homogeneous mixture -uses boiling and condensation. Copyright©2004 by Houghton Mifflin Company. All rights reserved. Copyright © Houghton Mifflin Company.All rights reserved.

Distillation of Crude Oil (Refining) Crude Oil is a mixture of Hydrocarbons

Distillation of Crude Oil

Chromatography separates mixtures of substances into their components. Paper Chromatography Chromatography separates mixtures of substances into their components. They all have: a stationary phase (a solid, or a liquid supported on a solid) and a mobile phase (a liquid or a gas). Copyright©2004 by Houghton Mifflin Company. All rights reserved. Copyright © Houghton Mifflin Company.All rights reserved.

Copyright©2004 by Houghton Mifflin Company. All rights reserved. Properties of Matter Copyright©2004 by Houghton Mifflin Company. All rights reserved.

Extensive Properties mass – Volume – The volume of a basketball is greater than the volume of a golf ball. a measure of the amount of matter the object contains. of an object is a measure of the space occupied by the object.

Who has a greater volume?

Extensive Properties An extensive property is a property that depends on the amount of matter in a sample. Examples: mass and volume Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. .

Copyright©2004 by Houghton Mifflin Company. All rights reserved. Objectives Observe and explain the difference between states of matter. Explain the difference between physical and chemical changes. Copyright©2004 by Houghton Mifflin Company. All rights reserved.

Intensive Properties An intensive property is a property that depends on the type of matter in a sample, not the amount of matter. Examples include: - Hardness of an object -Color Softness -Boiling point Absorbency -Odor Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. .

Is changing phase a physical or chemical change?

3-2 Physical and Chemical Properties and Changes Copyright©2004 by Houghton Mifflin Company. All rights reserved.

Properties of Matter Physical Properties are the characteristics of matter that can be changed without changing its composition Characteristics that are directly observable Examples: Color, odor, hardness, density, melting point, boiling point, state, solubility. 4

Example: Physical Properties Substance State Color Melting Point (C°) Boiling Point (C°) Density (g/cm3) Oxygen O2 Gas Colorless -218 -183 0.0014 Mercury Hg Liquid Silvery-white -39 357 13.5 Bromine Br2 Red-brown -7 59 3.12 Water H2O 100 1.00 Sodium Chloride NaCl Solid White 801 1413 2.17

Copyright©2004 by Houghton Mifflin Company. All rights reserved. Properties of Matter Chemical Properties are the characteristics that determine how the composition of matter changes as a result of contact with other matter - Examples: burning, decompose, reactivity, corrode, tarnish, explode, ferment Copyright©2004 by Houghton Mifflin Company. All rights reserved.

Classify Each of the following as Physical or Chemical Properties The boiling point of ethyl alcohol is 78°C. Diamond is very hard. Sugar ferments to form ethyl alcohol. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 5

Classify Each of the following as Physical or Chemical Properties The boiling point of ethyl alcohol is 78°C. Physical property – describes inherent characteristic of alcohol – boiling point Diamond is very hard. Physical property – describes inherent characteristic of diamond – hardness Sugar ferments to form ethyl alcohol. Chemical property – describes behavior of sugar – forming a new substance (ethyl alcohol) Copyright©2004 by Houghton Mifflin Company. All rights reserved. 6

Changes in Matter Physical Changes are changes to matter that do not result in a change in the composition State Changes – boiling, melting, condensing Breaking, splitting, grinding, cutting Chemical Changes involve a change in the composition of the substance Produce a new substance Chemical reaction Reactants  Products 8

Indications of a Chemical Reaction Color change Solid forms (precipitate) Gas bubbles Odor Temperature change Fizzing Copyright©2004 by Houghton Mifflin Company. All rights reserved.

Formation of a Precipitate Cu(OH)2 Precipitate

Classify Each of the following as Physical or Chemical Changes Iron metal is melted. Iron combines with oxygen to form rust. Sugar ferments to form ethyl alcohol. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 9

Classify Each of the following as Physical or Chemical Changes Iron is melted. Physical change – describes a state change, but the material is still iron Iron combines with oxygen to form rust.. Chemical change – describes how iron and oxygen react to make a new substance, rust Sugar ferments to form ethyl alcohol. Chemical change – describes how sugar forms a new substance (ethyl alcohol) Copyright©2004 by Houghton Mifflin Company. All rights reserved. 10

Oxygen combines with the chemicals in wood to produce flames Oxygen combines with the chemicals in wood to produce flames. Is a physical or chemical change taking place? Source: Jim Pickerell/ Stone/Getty Images

Burning of Methane CH4 +2O2  CO2 + 2H2O l_______________l l_________________l l l reactants products

Burning of Methane CH4 + 2O2 CO2 + 2H2O

In a chemical change, what happens to matter that appears to be lost?

The Law of Conservation of Mass (Antoine Lavoisier) In any chemical or physical change, mass is neither created or destroyed Mass is CONSTANT

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