1. Characteristics of States of Matter Solid Liquid Gas -
Retains a fixed volume and shape - Not easily compressible - Does
not flow easily - Assumes the shape of the part of the container
which it occupies - Not easily compressible - Flows easily -
Assumes the shape and volume of its container - Compressible -
Flows easily
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2. Pressure-Temperature Relationship in Gases Combined Gas Law:
According to the law, if volume remains constant, pressure will
change in proportion to temperature. KiloPascal (kPa) - metric unit
for pressure Kelvin (k) - Standard International unit of
temperature 101kPa 0.100m 3 = 303kPa 0.100m 3 273k 819k
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3. Atomic Structure 1803 John Dalton proposed an "atomic
theory"John Daltonatomic theory with spherical solid atoms based
upon measurableatoms properties of mass. Solid Sphere Model 1898 JJ
Thomson used a CRT to experimentallyJJ ThomsonCRT determine the
charge to mass ratio of an electron. Plum Pudding Model / Electrons
1911 Rutherford Nucleus is dense, small, andRutherford positively
charged. Electrons are located outside the nucleus. Planetary Model
/ Nucleus 1922 Niels Bohr Developed an explanation ofNiels Bohr
atomic structure that underlies regularities of the periodic table
of elements. Electron Shells
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4. Element, Compound, Mixture, & Alloy Element - A
substance composed of atoms having an identical number of protons
in each nucleus. Elements cannot be reduced to simpler substances
by normal chemical means. Compound - A chemical bond consisting of
atoms or ions of two or more different elements in definite
proportions that cannot be separated by physical means. Mixture - A
composition of two or more substances that are not chemically
combined with each other and are capable of being separated. Alloy
- A homogeneous mixture or solid solution of two or more metals,
the atoms of one replacing or occupying interstitial positions
between the atoms of the other.
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5. Balancing Chemical Equations Valence shells must balance out
electrons: Iron - is +3 valent Oxygen - is -2 valent Therefore 4Fe
+ 3O 2 --> 2Fe 2 O 3 4(+3) 3(-4) 2(+6) 2(-6) +12 -12 +12
-12
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6. Chemical Bonding (Page 1 of 2) Ionic Bond:electrons are
transferred forming positive & negative ions that attract
Electron transfer of sodium to chlorine yields Ionic bond forming
sodium chloride Covalent Bond:atoms share electrons Two types of
covalent bonds: Nonpolar BondsPolar Bonds (electrons equally
shared) (electrons unequally shared) H2H2 H2OH2O
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6. Chemical Bonding (Page 2 of 2) Fact: When comparing a polar
and nonpolar molecule with similar molar mass, the polar one
generally has a higher boiling point.
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7. Reaction Types A single-displacement reaction is where one
element appears to move out of one compound and into another. A
reaction of the type: A + BX --> AX + B A double-displacement
reaction is where parts of two reacting structures swap places. A
reaction of the type: AB + CD --> AD + CB A combination
(synthesis) reaction is where two or more substances are bonded
together to produce a single product. A reaction of the type: A + B
--> AB Decomposition is the fragmentation of a chemical compound
into elements or smaller compounds. A reaction of the type: AB
--> A + B
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8. Hookes Law Hooke's Law of elasticity is an approximation
that states that the amount by which a material body is deformed
(the strain) is related to the force causing the deformation (the
stress). For systems that obey Hooke's law, the extension produced
is directly proportional to the load: F = -kx - x is the distance
the spring is elongated by - F is the restoring force exerted by
the spring - k is the spring constant or force constant of the
spring
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9. Newtons Laws Third Law - For every action (force applied)
there is an equal but opposite reaction (equal force applied in the
opposite direction). First Law - An object will stay at rest or
move at a constant velocity (constant speed in a straight line)
unless acted upon by an unbalanced force. Second Law - The rate of
change of the momentum of a body is directly proportional to the
net force acting on it, and the direction of the change in momentum
takes place in the direction of the net force.
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10. Waveforms (Page 1 of 2) I II III IV I - Amplitude II, III -
Wavelength or Period IV - Peak to Peak Crest Trough
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10. Waveforms (Page 2 of 2) Types of waves: Frequency is the
measurement of the number of times a repeated event occurs per unit
of time. To calculate the frequency of an event, the number of
occurrences of the event within a fixed time interval are counted,
and then divided by the length of the time interval. 1s The
frequency of these waves = 3Hz
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11. Wave Effects (Page 1 of 2) This source of waves is moving
to the left. The frequency is higher on the left, and lower on the
right. The Doppler Effect is the apparent change in frequency and
wavelength of a wave that is perceived by an observer moving
relative to the source of the waves. Constructive Interference: Two
waves in phase with troughs & peaks line up / add amplitudes
Destructive Interference: Two waves out of phase with troughs &
peaks / subtract amplitudes A = I A 1 -A 2 I A = A 1 +A 2
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11. Wave Effects (Page 2 of 2) Diffraction is the bending of
waves around obstacles and the spreading out of waves beyond
openings.
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12. Static Electricity Like charges repel. Unlike charges
attract.
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13. Current Electricity (Page 1 of 2) Series Circuits Current
remains constant but voltage drops differently across components of
the circuit that have resistance. Parallel Circuits Voltages across
components are the same, but each component drops different amounts
of current.
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13. Current Electricity (Page 2 of 2) In order for the second
bulb to be inserted in series with the first, it must be placed in
a position where it will drop voltage that is running throughout
the entire circuit, not just across one of the parallel
resistors.
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14. Converting Energy Rectifier changes AC (alternating
current) to DC (direct current) Motor electrical energy -->
mechanical energy Generator chemical energy --> mechanical
energy --> electrical energy Transformer steps-up or steps-down
electrical energy
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15. Circular Velocity / Acceleration The velocity vector v is
always perpendicular to the position vector R. The circular motion
of the velocity is shown in the circle on the right, along with its
constant acceleration.
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16. Phase Changes Sublimation Solids subliming into gases must
gain energy. Condensation Gases condensing into liquids or liquids
condensing into solids must lose (release) energy. Melting Solids
melting into liquids must gain energy. Evaporation Liquids
evaporating into gases must gain energy. gain energy lose
energy
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17. Thermal Energy Thermal Energy The average kinetic energy of
molecules in a system