matter chapter 3 1
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Why does soda fizz when you open the bottle? Why is the sun hot? When iron rusts, what’s happening?TRANSCRIPT
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Matter
Chapter 3
Why does soda fizz when you open the bottle?
Why is the sun hot? When iron rusts, what’s happening?
Objectives
• Observe and explain the difference between states of matter.
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3-1 Universe Classified
• Matter is the part of the universe that has mass and volume
- There are three states of matterSolid, 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
Some Criteria for the Classification of Matter
• Composition (elements and compounds)
• State (solid, liquid, gas)
• Properties
States of Matter
YES YES YES
YES YES
YES
NO
NO
NO
NO
NO
YES
States of Matter
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Figure 3.1: Liquid water takes the shape of its container.
• Teacher Website Select Interactive 1
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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.
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Figure 3.12: Equal masses of hot water and cold water separated by a thin metal wall in an insulated box.
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Figure 3.13: The H2O molecules in hot water have much greater random motions than the H2O molecules in cold water.
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Figure 3.14: The water samples now have the same temperature (50°C) and have the same random motions.
Phase ChangesMelting solid liquidCondensation gas liquid
Freezing liquid solid
Deposition gas solid
Evaporation liquid gasSublimation 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
Objectives
• Explain the difference between elements and compounds.
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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)
Element
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 substance2. Homogeneous – same chemical composition at all times
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Compound
Compounds cont.
Have two properties that differ from elements:
1.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 heatb) electrolysis - uses electricity
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> 10 million compounds
•elements are represented by symbols•compounds are represented by chemical formulas
•chemical formula1. symbol --> tells which elements are present in compounds2. subscript (little # lower right) --> tells the number of atoms of each element
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When the elements sodium and chlorine combine chemically to form sodium chloride, there is a change in composition and a change in properties.
Properties of Compounds
• Sodium chloride (commonly known as table salt) is a white solid.
Distinguishing ElementsDistinguishing Elementsand Compoundsand Compounds
Compounds have different properties from their individual elements.
Breaking down Compounds
Breaking down NaCl
•Sodium is a soft gray metal.
Distinguishing ElementsDistinguishing Elementsand Compoundsand Compounds
Breaking down NaCl
Breaking down Compounds
• Chlorine is a pale yellow poisonous gas.
Distinguishing ElementsDistinguishing Elementsand Compoundsand Compounds
Classification of Matter(by composition)
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Classification of Matter
P u re S ub s ta n ceC o n s tan t C o m p o s it ion
H o m o ge n e o us
M ix tu reV a ria b le C o m p o s it ion
M a tte r
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3-4 Mixtures
Mixtures can be classified as:•Homogeneous Mixtures
•Heterogeneous Mixtures
• Homogeneous mixture = uniform throughout, appears to be one layer– Also called solutions
– Examples: olive oil, salt water, lemonade, coffee, air
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The substances in the olive oil are evenly distributed throughout the mixture
Example: Stainless SteelA 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
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Pure Substances vs. Mixtures• Pure Substances
– 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
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Figure 3.4: When table salt is stirred into water (left), a homogeneous mixture called a solution forms (right).
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Identity Each of the following as a Pure Substance, Homogeneous Mixture or
Heterogeneous Mixture
Gasoline
A stream with gravel on the bottom
Copper metal
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Identity Each of the following as a Pure Substance, Homogeneous Mixture or
Heterogeneous MixtureGasoline
– a homogenous mixture
A stream with gravel on the bottom– a heterogeneous mixture
Copper metal– A pure substance (all elements are pure substances)
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3-5 Separation of Mixtures• Separate mixtures based on different
physical properties of the components
EvaporationVolatility
ChromatographyAdherence to a Surface
FiltrationState of Matter (solid/liquid/gas)
DistillationBoiling Point
TechniqueDifferent Physical Property
Example: Separate iron filings from sulfur using a magnet.
Filtration: separates a solid from a liquid in a heterogeneous mixture
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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.
Distillation of Crude Oil (Refining)
• Crude Oil is a mixture of Hydrocarbons
Distillation of Crude Oil
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).
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Properties of Matter
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Extensive Propertiesmass –
Volume –
–The volume of a basketball is greater than the volume of a golf ball.
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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?
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An extensive property is a property that depends on the amount of matter in a sample. Examples: mass and volume
Extensive Properties
Objectives
• Observe and explain the difference between states of matter.
• Explain the difference between physical and chemical changes.
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– 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
Intensive Properties
Is changing phase a physical or chemical change?
3-2 Physical and Chemical Properties and Changes
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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.
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 Liquid Red-brown -7 59 3.12
Water H2O Liquid Colorless 0 100 1.00
Sodium Chloride
NaCl Solid White 801 1413 2.17
Example: Physical Properties
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
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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.
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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 pointDiamond 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)
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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
Indications of a Chemical Reaction
• Color change• Solid forms (precipitate)• Gas bubbles• Odor• Temperature change• Fizzing
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Formation of a Precipitate
Cu(OH)2
Precipitate
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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.
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Classify Each of the following as Physical or Chemical Changes
Iron is melted.– Physical change – describes a state change, but the
material is still ironIron 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)
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 MethaneCH4 +2O2 CO2 + 2H2O
l_______________l l_________________l l l
reactants products
Burning of MethaneCH4 + 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
END
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