matter – anything that has mass and takes up space mass – the amount of matter the object...
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Matter – anything that has mass and takes up space
Mass – the amount of matter the object contains
Everything is made up of matter Substance contain only one type of
matter; it is uniform and definite in composition.
Example: table sugar vs. lemonade
MATTER
Can it be physically separated?
Homogeneous Mixture
(solution)
Heterogeneous Mixture Compound Element
MIXTURE PURE SUBSTANCE
yes no
Can it be chemically decomposed?
noyesIs the composition uniform?
noyes
Colloids Suspensions
Examples:
› graphite
› pepper
› sugar (sucrose)
› paint
› soda
element
hetero. mixture
compound
hetero. mixture
solution
Matter that has a uniform and definite composition
Element› composed of identical atoms› EX: copper wire, aluminum foil
Compound
› composed of 2 or more elements in a fixed ratio
› properties differ from those of individual elements
› EX: table salt (NaCl)
For example…
Two different compounds, each has a definite composition.
Variable combination of 2 or more pure substances.
Heterogeneous Homogeneous
Disperses Light
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A physical blend of two or more substances.
Types of Mixtures:1. Homogeneous ( Solution)2. Heterogeneous
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One that has a completely uniform composition
→ components are evenly distributed throughout the sample ex. Salt solution
→ it has a single phase
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One that is not uniform in composition
→ has two or more phases
Ex. Oil and water, salad, milk
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Filtration: process of removing suspended solids from water by passing it through a permeable fabric (filter paper
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Distillation: a liquid is boiled to produce a vapor that is then condensed again to a liquid
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Magnetism: used to separate metals from non-metals.
Ex. A mixture of iron filings and sulfur. - The iron filings will be attracted to the magnet.
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Chromatography: technique used in separating mixtures that are or can be colored (pigments).
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Solubility: property used to distinguish one substance from another. This is a very useful technique.
Evaporation: a useful method of separation a solid mixed into a liquid. The liquid if boiled will turn into its gaseous phase.
Solution› homogeneous› very small particles› No Tyndall effect
Tyndall Effect
particles don’t settle EX: rubbing alcohol
Colloid› heterogeneous› medium-sized particles› Tyndall effect› particles don’t settle› EX: milk
Suspension› heterogeneous› large particles› particles settle› EX: fresh-squeezed
lemonade
Examples:
› mayonnaise
› muddy water
› fog
› saltwater
› Italian salad dressing
colloid
suspension
colloid
solution
suspension
Solid – definite shape & definite volume; particles are packed closely together
Liquid – definite volume, but takes the shape of the container; particles close, but able to move around. Liquids flow, almost incompressible and expand when heated.
Gas – indefinite shape & volume; particles are spread far apart. Gases expand to completely fill the container
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Property Solid Liquid Gas
Shape Definite Indefinite Indefinite
Volume Definite Definite Indefinite
Expansion on heating
Very slight
Moderate Great
Compressibility Nil Almost nil Large
Structural
arrangement
Closely packed
Moderate -
flows
Far apart
(move freely)
Physical Property – a quality or condition of a substance that can be observed or measured without changing the substances composition- color solubility, odor, hardness, density, melting point, boiling point, physical state- physical properties are used to identify unknown substances
A change that does not alter the chemical composition
- Cutting, grinding, bending, temperature change
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Freezing: liquid→ solid
Melting: solid → liquid
Evaporation: liquid → gas
Condensation: gas → liquid
Sublimation: solid → gas
Ability of a substance to undergo a chemical reaction and to form new substances.
Example: Rusting is a chemical property of iron.
odor, production of a gas or solid from a liquid
Something NEW is created!!
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Extensive properties: physical properties that depend on the amount of substance present ex. mass, length
Intensive properties: physical properties that are not dependent on the amount of substance present ex. Density, melting point
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Density depends ONLY on the composition of a substance and NOT the size of the sample
A substance floats because its less dense than its counterparts
A substance sinks because its more dense than its counterparts
Pg 69 Table 3.7 Densities of Common Metals
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The ratio of the mass of an object to its volume.
Density = MassVolume
Units of Density
Solids (g/cm3) liquids (g/mL)
Chemical Symbol – one or two letter’s that represent an element- First letter is always capitalized; the second is always lower case
Chemical Formula – shows the # and type of atoms present
Chemical Reactions – one or more substances change into new substances.
1. Reactants – the starting substances (left side)
2. Products – the substances formed (right side)
Example: Iron + Sulfur → Iron Sulfide
Metals tend to lose electrons and become positive.
Nonmetals tend to gain electrons and become negative.
An ionic compound is formed when a metal combines with a nonmetal. The total charge on any compound is zero.
Ionic bond: held together by opposing electrical charges
Covalent bond: compound is held together by the sharing of the electrons.
In any physical or chemical reaction, mass is neither created nor destroyed; it is conserved.
The mass of the products equals the mass of the reactants.