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Chemistry – Matter and Change
Chapter TWO
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Objectives for Unit 2 SPI – Interpret the periodic table to describe an element’s atomic makeup. SPI – Distinguish among elements and compounds. SPI – Classify as physical or chemical change. SPI – Compare and contrast heat/temperature changes in chemical/physical processes. SPI – Investigate solids, liquids, and gasses in terms of energy and particle spacing.
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More Objectives for Unit 2
You will also be able to… - Define and describe “Chemistry” - List the different types of Chemistry - Describe how to separate a mixture - Describe the periodic table and how it is arranged
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*Matter: composed of mass and takes up space.
Chemistry: the study of composition, structure, and properties of matter* and the changes it undergoes. *Matter: composed of mass and takes up space.
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Branches of Chemistry Organic Chemistry – carbon-containing compounds.
Inorganic Chemistry – no carbon Physical Chemistry – properties and changes of matter and their relation to energy. Analytical Chemistry – identification of components and composition of materials. Biochemistry – substances and processes occurring in living things. Theoretical Chemistry – use of math and computers to understand chemical behavior and to design/predict the properties of NEW compounds.
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Elements and Compounds
All matter is composed of atoms. Copper pipe is made of copper atoms. Oxygen gas is made of oxygen atoms. Atoms of two or more elements bond together to make compounds. CO2 (___ carbon atom and ___ oxygen atoms) H2O2 (___ hydrogen atoms & ___ oxygen atoms) An element is a pure substance made of only one kind of atom. Carbon is an element made of only carbon atoms.
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SOLID - LIQUID - GAS - PLASMA
Physical Properties A characteristic that can be observed or measured without changing the identity of the substance. Examples: boiling and freezing points Physical Change: does not involve a change in identity of the substance…cutting, melting, boiling, freezing, tearing. Change of State: physical change from one state to another. Solid Liquid (Melting) Liquid Solid (Freezing) Solid Gas (Subliming) Gas Solid (Deposition) Liquid Gas (Evap./Boil) Gas Liquid (Condensing) SOLID LIQUID GAS PLASMA
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STATES OF MATTER SOLID: Examples Definite Shape Definite Volume
Particles move slowly and are close together Video: Potassium Examples Sodium metal (Na) Ice (H2O) Gold at room temp. (Au)
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STATES OF MATTER LIQUID: Video: Mercury Examples No Definite Shape
Definite Volume Particles move a little faster than solids and more freely. Video: Mercury Examples Mercury (Hg) Bromine (Br2) Water (H2O) Gold at high temp. (Au)
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STATES OF MATTER GAS: Video: Chlorine Examples No Definite Shape
No Definite Volume Particles move very quickly and are far apart. Video: Chlorine Examples Neon (Ne) Steam (H2O) Chlorine gas (Cl2)
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STATES OF MATTER PLASMA: Video: What is Plasma? Examples
High Temperature Atoms lose electrons easily Video: What is Plasma? Examples Sun Fluorescent Bulbs
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STATES OF MATTER LIQUID SOLID GAS
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Chemical Properties… …relate how chemicals undergo change.
Chemical Change (reaction): when substances are converted into NEW substances. Reactants REACT. Products are PRODUCED. reactant + reactant product carbon + oxygen carbon dioxide C O2 CO2 Alkali Metals in Water
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Chemical Properties… …relate how chemicals undergo change.
Chemical Change (reaction): when substances are converted into NEW substances. Reactants REACT. Products are PRODUCED. reactant + reactant product sodium + water sodium hydroxide + hydrogen gas Na H2O NaOH + H2
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Chemical Properties… …relate how chemicals undergo change.
Chemical Change (reaction): when substances are converted into NEW substances. Reactants REACT. Products are PRODUCED. reactant + reactant product Potassium + water potassium hydroxide + hydrogen gas K H2O KOH + H2
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Chemical Properties… …relate how chemicals undergo change.
Chemical Change (reaction): when substances are converted into NEW substances. Reactants REACT. Products are PRODUCED. reactant + reactant product Rubidium + water rubidium hydroxide + hydrogen gas Rb H2O RbOH + H2
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Classification of Matter Mixtures Compounds Elements Homogeneous
Pure Substances Homogeneous (air, sugar in water) Heterogeneous (wood, blood) Compounds (water, salt, sugar) Elements (gold, oxygen) “Solutions”
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Mixtures vs. Pure Substances
Blend of two or more types of matter (each retains its own identities and properties.) Salt-Water…is both salt and water. Tastes like salt and tastes like water. Mixture of metals: alloy -24 k. gold = only gold -18 k. gold = gold, silver, copper PURE SUBSTANCES Every sample has exactly the same properties. Every sample has exactly the same composition. Pure water is always 11.2% hydrogen and 88.8% oxygen.
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Classification of Matter Mixtures Compounds Elements Homogeneous
Pure Substances Homogeneous (air, sugar in water) Heterogeneous (wood, blood) Compounds (water, salt, sugar) Elements (gold, oxygen) “Solutions”
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Separation of Mixtures
DISTILLATION Boil mixture. Liquid boils off, leaving solid minerals behind. Collect the boiled vapor in a condenser. Collected liquid is pure(er). Ex: Seawater or Moonshine FILTRATION Pour mixture onto a mesh, like filter paper. Liquid passes through paper. Solid is left on the paper. Ex: Charcoal water filters
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INTRO to the Periodic Table
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GROUPS (or families) are VERTICLE
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PERIODS are HORIZONTAL.
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Metals are Left. Nonmetals are Right
METALLOIDS are on Zig-Zag Line.
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Groups you should know…
Alkali Metals Alkaline Earth Metals Transition Metals Rare Earth Metals Metalloids Nonmetals Inert “Nobel” Gases
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Vocabulary Review Chemistry Solid Atom Liquid Compound Gas Element
Change of State Physical Change Mass, Matter Chemical Change Chemical Reaction Mixture Homogeneous Heterogeneous Solid Liquid Gas Plasma Reactant Product Pure Substance Group (Family) & Period Metal Nonmetal Metalloid
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Important Information
Test on ___________! - Chapter 2 - Scientific Method Review - Lab Safety & Equipment - Graphing Review Bring: Pencil & Calculator Book (for after test)
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Next Unit… Chapter 5 Measurements & Calculations
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