chapter 3 matter & its properties. volume and mass volume: amount of 3-d space an object...
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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 of matter; measure with a balance
Matter
Matter: anything that has mass and takes up space
Basic Building Blocks of Matter
Atom: smallest unit of an element that maintains the properties of that element
CC
CCarbon Atoms
Elements
Element: pure substance made of only 1 kind of atom
CarbonOxygen
DIATOMIC
MONATOMIC
Compound
Compound: substance made from the atoms of two or more elements chemically bonded
Water
Properties
Chemists use properties to distinguish between substances and to separate them.
Properties
Entire group of substances: example – metals’ distinguishing property is conductivity
Unknown substance conducts electricity well – probably a metal
Properties
Subgroups of substances: Sugars can be reducing or nonreducing
Something called Fehling’s solution can be used to test the sugar
Extensive Properties
Depend on the amount of substance present
Examples: mass, volume, amount of energy in a substance
Intensive Properties
Do not depend on the amount of matter present (independent)
Examples: melting point, boiling point, density, ability to conduct electricity and heat
Intensive vs. Extensive
Imagine heating 100 mL and 400 mL of water, respectively
Boiling point? Heat absorbed? Time to boil?
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.
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.
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
SOLID
Solid: 1. definite volume and shape
2. particles packed together in fixed positions
3. particles vibrate about a fixed position
LIQUID
Liquid: 1. definite volume but indefinite shape 2. takes shape of container 3. particles close but flow around one another
GAS
Gas: 1. no definite shape or volume 2. particles a great distance from each other
SOLIDS, LIQUIDS, & GASES
Change of State Processes
Solid to Liquid: Liquid to Gas: Gas to Liquid: Liquid to Solid: Solid to Gas: Gas to Solid:
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.
Chemical Change/Reaction
Chemical change or chemical reaction: change in which one or more substances are converted into different substances
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
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
Evidence of chemical change
(Add this to outline) Ideas?
Energy and Changes in Matter
Energy is involved in both physical and chemical changes.
Different forms include heat and light.
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)
Energy
Energy in physical and chemical changes may be released or absorbed, but it is not created or destroyed! Law of Conservation of Energy
Classification of Matter
All matter can be classified as:1. pure substances OR
2. mixtures
Mixtures
Mixtures: (def.) blend of two or more kinds of matter, each of which retains its own properties and identity
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)
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)
Separating Mixtures
1. Filtration
2. Paper Chromatography
3. Centrifuge
Pure Substances
Pure substances: (def.) has a fixed composition and differs from a mixture in the following ways:
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)
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.
Pure Substance Examples
Water
Sucrose
Pure substances are compounds or elements
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
The End of Section 1-2!!!!!