Chapter 3 Matter & Its Properties. Volume and Mass Volume: amount of 3-D space an object occupies;...
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Transcript of Chapter 3 Matter & Its Properties. Volume and Mass Volume: amount of 3-D space an object occupies;...
![Page 1: Chapter 3 Matter & Its Properties. Volume and Mass Volume: amount of 3-D space an object occupies; all matter has volume Mass: measure of the amount.](https://reader036.fdocuments.net/reader036/viewer/2022081506/5697bf8a1a28abf838c8a6e4/html5/thumbnails/1.jpg)
Chapter 3
Matter & Its Properties
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Volume and Mass
Volume: amount of 3-D space an object occupies; all matter has volume
Mass: measure of the amount of matter; measure with a balance
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Matter
Matter: anything that has mass and takes up space
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Basic Building Blocks of Matter
Atom: smallest unit of an element that maintains the properties of that element
CC
CCarbon Atoms
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Elements
Element: pure substance made of only 1 kind of atom
CarbonOxygen
DIATOMIC
MONATOMIC
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Compound
Compound: substance made from the atoms of two or more elements chemically bonded
Water
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Properties
Chemists use properties to distinguish between substances and to separate them.
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Properties
Entire group of substances: example – metals’ distinguishing property is conductivity
Unknown substance conducts electricity well – probably a metal
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Properties
Subgroups of substances: Sugars can be reducing or nonreducing
Something called Fehling’s solution can be used to test the sugar
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Extensive Properties
Depend on the amount of substance present
Examples: mass, volume, amount of energy in a substance
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Intensive Properties
Do not depend on the amount of matter present (independent)
Examples: melting point, boiling point, density, ability to conduct electricity and heat
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Intensive vs. Extensive
Imagine heating 100 mL and 400 mL of water, respectively
Boiling point? Heat absorbed? Time to boil?
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Physical Property
Physical Property: characteristic can be observed or measured without changing the identity of the substance
Example: melting or boiling point; color, size, etc.
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Physical Change
Physical Change: change in a substance that does not involve a change in the identity of the substance
Example: grinding, cutting, melting, etc.
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Special Physical Changes: CHANGES OF STATE
Changes of State: special physical changes in which a substance changes from one state to another
The 3 common states are solid, liquid, and gas
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SOLID
Solid: 1. definite volume and shape
2. particles packed together in fixed positions
3. particles vibrate about a fixed position
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LIQUID
Liquid: 1. definite volume but indefinite shape 2. takes shape of container 3. particles close but flow around one another
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GAS
Gas: 1. no definite shape or volume 2. particles a great distance from each other
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SOLIDS, LIQUIDS, & GASES
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Change of State Processes
Solid to Liquid: Liquid to Gas: Gas to Liquid: Liquid to Solid: Solid to Gas: Gas to Solid:
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Chemical Property
Chemical property relates to a substance’s ability to undergo changes that transform it into different substances
Ex: iron rusting, silver tarnishing, match burning, etc.
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Chemical Change/Reaction
Chemical change or chemical reaction: change in which one or more substances are converted into different substances
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Chemical Equations
Reactants: substances that react in a chemical change (left side of chemical equation)
Products: substances that are formed in a chemical change (right side of chemical equation)
Reactants Products
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Law of Conservation of Matter
(Add this to outline) In a chemical reaction, matter cannot
be lost nor gained.
Matter may rearrange but cannot be created nor destroyed.
Mass of reactants = mass of products
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Evidence of chemical change
(Add this to outline) Ideas?
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Energy and Changes in Matter
Energy is involved in both physical and chemical changes.
Different forms include heat and light.
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Energy
Uses include: 1. provide energy for a physical change (i.e. melting) 2. provide energy for a chemical
change (i.e. decomposition of water)
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Energy
Energy in physical and chemical changes may be released or absorbed, but it is not created or destroyed! Law of Conservation of Energy
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Classification of Matter
All matter can be classified as:1. pure substances OR
2. mixtures
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Mixtures
Mixtures: (def.) blend of two or more kinds of matter, each of which retains its own properties and identity
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Mixtures
Properties of a Mixture: are a combination of the properties of its components
Composition of a Mixture: must be specified (in a % of mass or volume)
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Homogeneous v. Heterogeneous
Homogeneous: uniform in composition; same proportion of components throughout (ex. Salt water solution)
Heterogeneous: not uniform throughout (ex. Mixture of clay and water)
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Separating Mixtures
1. Filtration
2. Paper Chromatography
3. Centrifuge
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Pure Substances
Pure substances: (def.) has a fixed composition and differs from a mixture in the following ways:
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Pure Substances
1. Every sample of a given pure substance has exactly the same characteristic properties
(unlike mixtures whose properties depend upon the relative amounts of mixture’s components)
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Pure Substances
2. Every sample of a given pure substance has exactly the same composition
Ex. All pure water is always 11.2% H and 88.8% O by mass.
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Pure Substance Examples
Water
Sucrose
Pure substances are compounds or elements
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Laboratory Chemicals and Purity
Chemicals in lab treated like pure chemicals BUT all have some impurities
Impurities can sometimes affect the results of a reaction
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The End of Section 1-2!!!!!