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the change in a system's internal energy is the sum of the heat aded to the system and the work done in the system
Delta E= Q+W
First Law of Thermodynamics
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the outermost electrons in an atom
valence electrons
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light consists of bundles or "packets" of energy that travels as electromagnetic waves
Quantum Theory of Light
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mass of a substance per unit volume
density
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theoretical gas that adheres exactly to the gas laws and assumptions of kinetic energy
ideal gas
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-packs the most atoms into the smallest amount of space
-also called cubic close packing
face-centered cubic arrangement
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-moderately strong force that exists between neighboring polar molecules due to the attraction of oppositely charged ends
-strongest intermolecular force
dipole-dipole force
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relatively strong force between molecules that contain hydrogen covalently bonded to nitrogen, oxygen, or fluorine; present in water, ammonia, and hydrogen fluoride
hydrogen bond
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-weak force that exists between all molecules, both polar and nonpolar, due to the formation of instantaneous dipoles
- strongest intermolecular force effecting the element iodine
london force
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negatively charged particles
electron
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bonding situation in which electrons are shared by more than two atoms
delocalization (or resonance)
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the simplest ratio of atoms in a compound
empirical formula
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allows three electron pairs to get as far apart as possible
trigonal planar geometry
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-involve replacing one element in a compound with another
A + BC --> B + AC
single-displacement reaction
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-characterized by the sharing of a "sea" of delocalized electrons among many atoms
-produces substances that are characteristically malleable and ductile
-metal
metallic bond
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-randomness of a substance or system
-second law states entropy is always increasing
entropy
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two polar bonds point symmetrically in opposite direction
nonpolar
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simplest repeating unit in a crystal
unit cell
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atoms of the same element that differ in their mass numbers
isotopes
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a bond that involves the sharing of four electrons
double bond
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the sharing of one or more electron pairs between two atoms
covalent bond (has no metal)
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very hard and very high melting point
covalent network
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the amount of heat required to cause a unit rise in temperature of a unit mass of a substance
specific heat
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characterizes by the transfer of electrons from one atom to another
ionic bond
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metal + nonmetal
ionic bond
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solid whose particles are characterized by a regular, repeating three-dimensional pattern
crystalline solid
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elements ten to react chemically to achieve a noble-gas electron configuration weather by losing, gaining, or sharing of electrons
octet rule
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-covalent bond where bonding electron pair is closer to the more electron negative element
-unequal sharing of electrons
polar bond
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-enthalpy change is negative
-warmer then the reactance
exothermic (chemical) reaction
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molecule having two bonding pairs and two nonbonding pairs of electrons around the central atom
angular geometry
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the heat per unit mass required to melt a substance at its normal melting point
heat of fusion
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the position and momentum of small particles such as electrons cannot be precisely measured simutaneously
uncertainty principle
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energy associated with an object's motion or movement
kinetic energy
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used to predict whether a bond is primarily ionic or primarily covalent
electron negativity
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the two values for absolute zero
0k and -273.15 C
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causes the bright lines in the spectrum of glowing hydrogen gas
electrons dropping from higher to lower energy levels
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the speed of light in a vacuum
3.00 x 108 m/s
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determines an atom's identity as an element
protons
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the electronegativity of an element
- |..............largest
- \/..................|
- smallest <------
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equation of the ideal gas law in the usual form
- PV= nRT
- Pressure x volume = number of moles x ideal gas constant x temperature
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type of charge an electron possesses
negative
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alkaline earth metals
row 2
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how to change centimeters to millimeters
K H Da U D C M
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