Biological Chemistry Life is made up of matter matter: occupies space & has mass.
Matter – anything that has mass and takes up space Mass – the amount of matter the object...
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Transcript of 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
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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
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Examples:
› graphite
› pepper
› sugar (sucrose)
› paint
› soda
element
hetero. mixture
compound
hetero. mixture
solution
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Matter that has a uniform and definite composition
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Element› composed of identical atoms› EX: copper wire, aluminum foil
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Compound
› composed of 2 or more elements in a fixed ratio
› properties differ from those of individual elements
› EX: table salt (NaCl)
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For example…
Two different compounds, each has a definite composition.
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Variable combination of 2 or more pure substances.
Heterogeneous Homogeneous
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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.
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Solution› homogeneous› very small particles› No Tyndall effect
Tyndall Effect
particles don’t settle EX: rubbing alcohol
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Colloid› heterogeneous› medium-sized particles› Tyndall effect› particles don’t settle› EX: milk
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Suspension› heterogeneous› large particles› particles settle› EX: fresh-squeezed
lemonade
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Examples:
› mayonnaise
› muddy water
› fog
› saltwater
› Italian salad dressing
colloid
suspension
colloid
solution
suspension
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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.
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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)
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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
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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
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Ability of a substance to undergo a chemical reaction and to form new substances.
Example: Rusting is a chemical property of iron.
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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)
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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
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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
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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.
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Ionic bond: held together by opposing electrical charges
Covalent bond: compound is held together by the sharing of the electrons.
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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.