Chapter 16.2. What we know so far… Matter is made of atoms.
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The Submicroscopic World Chapter 16.2
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Transcript of Chapter 16.2. What we know so far… Matter is made of atoms.
- Slide 1
- Chapter 16.2
- Slide 2
- What we know so far Matter is made of atoms
- Slide 3
- Atoms are submicroscopic
- Slide 4
- Matter exists in phases Solid
- Slide 5
- Liquid
- Slide 6
- Gas
- Slide 7
- In the SOLID phase Particles are attracted to one another Held together in a tightly packed and fixed 3-d arrangement
- Slide 8
- Microscopic View of a Solid The atoms vibrate but stay close to one another Solids maintain their shape and volume Not easily compressible
- Slide 9
- Intereactive 3-D Diamond Molecule
- Slide 10
- Snowflake Ice Interactive Ice Molecule
- Slide 11
- In the LIQUID phase Particles can move and slide across one another Can assume the shape of their container
- Slide 12
- Microscopic View of a Liquid The atoms vibrate and particles can flow easily past one another Liquids assume the shape of their container
- Slide 13
- Liquids Particles in liquids flow easily across one another
- Slide 14
- Liquids take the shape of their containers
- Slide 15
- In the GASEOUS PHASE The atoms are moving rapidly, and easily across one another. Lots of free space between the particles They assume the shape of their container.
- Slide 16
- Microscopic View of a Gas The atoms are moving rapidly, and easily across one another. Lots of free space between the particles Compressible
- Slide 17
- Gases Conform to the shape of their containers Easily compressed
- Slide 18
- Gases Particles easily flow and move over one another
- Slide 19
- Lets Review YouTube - States of Matter
- Slide 20
- Phase Changes Chapter 16.3
- Slide 21
- Substances can change phases GasesLiquidsSolidsLiquids
- Slide 22
- Substances can change phases GasesLiquidsSolidsLiquids Condensation Freezing Evaporation Melting
- Slide 23
- Substances can change phases GAS SOLID Sublimation
- Slide 24
- Changing Phases
- Slide 25
- Water Cycle Hydrologic Cycle
- Slide 26
- Boiling on the atomic level CLICK The Beaker
- Slide 27
- Boiling Point CLICK The Beaker
- Slide 28
- Heat of Vaporization The amount of energy required to change a liquid to a gas (and vice versa). 2256J/g
- Slide 29
- Heat of Fusion The amount of energy needed to change any substance from solid to liquid ( and vice versa) Water = 334J/g
- Slide 30
- Chapter 16.4
- Slide 31
- Physical Properties Describe the look or feel of a substance Density Texture Phase
- Slide 32
- Every substance has its own set of physical properties
- Slide 33
- Physical Properties CAN Change However The substances identity remains the same SolidGasLiquid
- Slide 34
- Slide 35
- Chemical Properties Characterize the ability of a substance to react with other substances, or to transform from one substance to another.
- Slide 36
- How Substances React or Transform
- Slide 37
- Chemical Changes Change how atoms are Chemically bonded to one another.
- Slide 38
- When we cook with gas..
- Slide 39
- Take another look CH 4 + 2 O 2 CO 2 + 2H 2 O Chemical Reaction
- Slide 40
- During a chemical reaction Changes are made in the way atoms bond together New materials are formed CH 4 + 2O 2 CO 2 + 2H 2 O
- Slide 41
- Chapter 16.6
- Slide 42
- Remember.. Periodic table is a listing of all the known elements Atomic number Symbol Atomic Mass He 2 4.003
- Slide 43
- The way the table is organized tells a lot about the elements properties
- Slide 44
- Metals are on the left side of the periodic table
- Slide 45
- Most of the known elements are metals Malleable Can be hammered and bent into different shapes without breaking
- Slide 46
- Most of the known elements are metals Ductile Can be drawn into thin wires
- Slide 47
- Most of the known elements are metals Good Conductors Heat Electricity Most solid at room temperature
- Slide 48
- Non-metals are on the right side of the periodic table
- Slide 49
- Non-Metals Poor conductors Not malleable Not ductile Can be solid, liquid or gas at room temperature Shatter when hammered Brittle
- Slide 50
- Slide 51
- Metalloids
- Slide 52
- B - Boron Si - Silicon Ge - Germanium As - Arsenic Sb - Antimony Te - Tellurium
- Slide 53
- Metalloids Have both metallic and nonmetallic properties
- Slide 54
- Metalloids Weak conductors Semi- conductors
- Slide 55
- Slide 56
- Slide 57
- Across a period properties gradually change Periodic Trend
- Slide 58
- Smaller Easily lose e- Larger Do not easily lose e-
- Slide 59
- Columns have remarkably similar properties
- Slide 60
- The elements are grouped or in families
- Slide 61
- Slide 62
- Element Families/Grouops
- Slide 63
- Inner Transition Metals
- Slide 64
- Slide 65
- Slide 66
- Chapter 16.7
- Slide 67
- Elements are made of atoms The element gold ( Au) is made entirely of gold atoms
- Slide 68
- The element silver (Ag) is made entirely of silver atoms
- Slide 69
- The element neon, Ne, is composed entirely of neon atoms
- Slide 70
- Elemental Formula A notation that uses the atomic symbol and sometimes a numerical subscript to show how atoms of an element are bonded together. confused?
- Slide 71
- Elemental Formula Tell you how the atoms of an element are arranged. take a look
- Slide 72
- Elemental Gold The smallest unit of the element gold, as it occurs in nature, is the gold atom itself. Use the elements symbol Au
- Slide 73
- The smallest unit of the element silver is the silver atom itself Use the symbol Ag Elemental Silver
- Slide 74
- The smallest unit of the element nitrogen is a nitrogen molecule Use the symbol and subscript numbers Elemental Nitrogen N2N2
- Slide 75
- The smallest unit of the element oxygen is an oxygen molecule Use the symbol and subscript numbers Elemental Oxygen O2O2
- Slide 76
- The smallest unit of the element sulfur is a sulfur molecule Use the symbol and subscript numbers Elemental Sulfur S8S8
- Slide 77
- Compound Material composed of different elements bonded to each other
- Slide 78
- Slide 79
- Compounds Salt NaCl Sodium chloride
- Slide 80
- Chemical formula Salt NaCl Sodium chloride
- Slide 81
- Chemical formula Water H 2 O water
- Slide 82
- Chemical formula Ammonia NH3 ammonia N H H H
- Slide 83
- Compounds have their own identities and properties
- Slide 84
- Chapter 16.8
- Slide 85
- IUPAC International Union for Pure and Applied Chemistry
- Slide 86
- Developed a chemical naming system Name reflects the elements a compound contains How the elements are combined
- Slide 87
- 3 Basic Guidelines #1 The name of the element farthest to the left on the periodic table is followed by the name of the element father to the right, with the suffix -ide added to the latter.
- Slide 88
- Examples of Guideline #1 NaCl - Sodium chloride Li 2 O - Lithium oxide CaF 2 - Calcium fluoride The name of the element farthest to the left on the periodic table is followed by the name of the element father to the right, with the suffix -ide added to the latter. HCl - Hydrogen chloride MgO - Magnesium oxide Sr 3 P 2 - Strontium phosphide
- Slide 89
- 3 Basic Guidelines #2 Use prefixes to designate numbers of elements in compounds Mono-one Di two Tri - three
- Slide 90
- Examples of Guideline #2 Carbon & Oxygen Nitrogen & Oxygen CO Carbon monoxide CO 2 Carbon dioxide NO2 Nitrogen dioxide N2O4 Dinitrogen tetroxide
- Slide 91
- Try this sulfur & oxygen example.. SO 2 SO 3 Sulfur dioxide Sulfur trioxide
- Slide 92
- 3 Basic Guidelines #3 Many compounds have common names
- Slide 93
- Examples of Guideline #3 H2OH2O CH 4 Dihydrogen monoxide ? Water Carbon tetrahydride? Methane
- Slide 94
- You completed Chapter 16! Congratulations!