chapter 3 matter & energy chemistry 100. matter: has mass and takes space. matter
TRANSCRIPT
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Chapter 3
Matter & Energy
Chemistry 100
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Matter: has mass and takes space.
Matter
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States of Matter
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Chemical change (chemical reaction):
substance(s) are used up (disappear) → others form
burning or cooking the egg
Physical change: identities of the substances do not change.(change of state)
evaporation of water or melting
Changes
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T ↑ move fasterKinetic energy ↑
Boiling is a physical change.
Physical Changes
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Physical Changes
Composition of the substance is not affected.
Change of states
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Chemical Changes (reactions)
Water
Electrolysis
Decomposition
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Think about it: Classify each of the following as a physical or chemical change.
• Bleaching clothes
• Burning of wood
• Dissolving of sugar in water
• Melting a popsicle on a warm summer day
• Baking soda (sodium carbonate) forming CO2(g)
• Iron metal melting
Chemical and physical Changes
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Physical and Chemical Properties
Physical Properties: a directly observable characteristic of a substance exhibited as long as no chemical change occurs.
Color, Odor, Volume, State, Density, Melting and boiling point.
Burning wood – rusting of the steel
Chemical Properties: Ability to chemical changes. (forming a new substance(s))
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MatterAnything that occupies
space and mass
Pure substancesFixed composition, con not
be more purified
MixturesA combination of two
or more pure substance
PhysicallySeparable into
ElementCannot be
subdivided by chemical or
physical means
CompoundsElements united
In fixed ratios
HomogeneousmatterUniform
Compositionthroughout
Heterogeneousmatter
Nonuniformcomposition
CombineChemically
To form
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Element: is a substance consists of identical atoms.
Cannot be divided by chemical & physical methods.
Carbon, Hydrogen, Oxygen
116 elements – 88 in nature
Monatomic
Ar He
Diatomic
N2 O2
Polyatomic
S8
Elements
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Element Symbols
The first letter or two first letters of element name:
Oxygen O Silicon Si
Carbon C Argon Ar
Sometimes, two letters are not the first letters:
Chlorine Cl Zinc Zn
Sometimes, old names are used (Latin or Greek):
Iron (Ferrum) Fe Lead (Plumbum) Pb
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Compound: is a pure substance made up of two or more elements in a fixed ratio by mass.
H2O (Water): 2 Hydrogen & 1 Oxygen
CO2: 1 Carbon & 2 Oxygen
20 million compounds
Compounds
Compounds ElementsBy Chemical Methods
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Compounds Formula
Identifies each element Ratios
H2O
Subscript (number of each atom)
Subscript 1 is not written.
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Elements & Compounds
Oxygen(gas)
Hydrogen(gas)
H2O (liquid)
The character of each element is lost when forming a compound.
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Sodium (Na)
NaCl
Chlorine (Cl)
Elements & Compounds
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Compound & molecule
Molecule:
1. the smallest unit of a compound that retains the characteristics of that compound. H2O, CO2
2. atoms of one element bonded into a unit. Buckyballs, C60 oxygen, O2 ozone, O3
NaCl, salt Buckyball, C60 Ethanol, C2H6O
compound---
---molecule
compoundmolecule
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Pure substance & Mixture
Pure substance: same composition
Elements - Compounds
Mixture: different composition
Different water samples (impurities).
Water
Coffee
salad dressing
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Mixture: is a combination of two or more pure substances.
Homogeneous (solutions): uniform and throughout
Air, Salt in water
Heterogeneous: nonuniform
Soup, Milk, Blood, sand in water
Mixtures
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Separation of Mixtures
Mixture Two or more pure substances
Physical Methods
EvaporationVolatility
ChromatographyAdherence to a surface
FiltrationState of matter
(solid/liquid/gas)
DistillationBoiling point
TechniqueDifferent Physical Property
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Separation of Mixtures
Distillation
Filtration
Decantation
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Distillation
Separation by using the differences in boiling points.
Salt & Water
(Physical change)
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Distillation
Distillation Tower
Heater
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Filtration
For Heterogeneous mixtures.
Separation by using the differences in size of particles.
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Salt, Sand and Water
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Separation
ChemicalMethods
Elements
Matter
Pure substances
Compounds
Homogeneous mixtures Heterogeneous mixtures
Physical Methods
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Energy
Kinetic energy (KE): energy of motion
Potential energy: stored energy
Law of conservation of energy
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Heat
units of heat: calorie (cal) or joule (J)
1 cal = 4.184 J
Amount of heat = specific heat capacity× mass × change in temperature
Amount of heat = C × m × (Tf – Ti)
Tf = final temperature
Ti = initial temperature
C = Specific heat capacity (cal/g °C)
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• Specific heat capacity is the energy required to change the temperature of a mass of one gram of a substance by one Celsius degree.
Heat
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• Calculate the amount of heat energy (in joules)
needed to raise the temperature of 6.25 g
of water from 21.0°C to 39.0°C.
• We are told the mass of water and the temperature increase. We look up the specific heat capacity of water, 4.184 J/g°C.
Q = C x m x T
Q = (4.184 J/g°C) x (6.25 g) x (39.0°C – 21.0°C)
Q = 471 J
Practice 1:
Heat
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• A silver-gray metal weighing 15.0 g requires 133.5 J to raise the temperature by 10.°C. Find the heat capacity.
Q = C x m x T
(133.5 J) = C x (15.0 g) x (10.°C)
C = 0.89 J/g°C
Can you determine the identity of the metal using
Table 10.1?
Heat
Practice 2:
Al