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89 Cards in this Set
- Front
- Back
- 3rd side (hint)
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q
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heat in Joules
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transfer of energy from a warmer body to a cooler body
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H
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enthalpy in Joules
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delta H = delta U + (P)(delta U)
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U
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internal energy
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for a system with no volume change and no work, internal energy = heat
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endothermic reaction
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change in enthalpy is positive
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q>0
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work
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any transfer of energy that is not heat
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First Law of Thermodynamics
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energy of a system and surroundings its always conserved
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Heat of Reaction
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change in enthalpy = change in heat of formation - change in heat of reaction
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Standard Enthalpy of Formation
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change in enthalpy for a reaction that creates one mole of a compound from its raw elements in their standard states
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delta H f
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Electrostatic Energy
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potential energy associated with the separation of two electrical charges
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Types of Kinetic Energy
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thermal energy, mechanical energy, electrical energy, acoustic energy
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Electrical Energy
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movements of electrons through a conductor
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Types of Potential Energy
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gravitational energy, chemical energy, electrostatic energy
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Thermal Equilibrium
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no further temperature change offurs
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- energy transfer of heat is random
- goes from object at higher temperature to object at lower temperature - object of higher heat (at beginning) loses thermal energy |
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Specific Heat Capacity
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the energy transferred as heat that is required to raise the temperature of 1 gram of a substance by 1 kelvin
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q= Cm(change in temp)
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Internal Energy
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sum of the potential and kinetic energies of the atoms, molecules, or ions in a system
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Strong acid
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- no carbon
- halogens - ions in net ionic equations - 100% dissociation -strong electrolytes |
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Weak Acid
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-have carbon
- molecules in net ionic equations - <5% dissociation |
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Strong Base
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- metal + hydroxide
- usually alkali metals |
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Strong Acid + Strong Base
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H+ + OH- yields H20
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Strong Acid + Weak Base
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H+ + B yields BH+
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Weak Acid + Strong Base
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HA + OH- yields A- + H20
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Weak Acid + Weak Base
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HA + B yields A- + BH+
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Metal Carbonates + Acid
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new metal salt + C02 (g) + H20 (l)
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gas-forming
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Metal Sulfite + Acid
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new metal salt + SO2 (g) + H20 (l)
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gas-forming
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Ammonium Salt + Strong Base
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metal salt + NH3 (g) + H20 (l)
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gas-forming
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HCl
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hydrochloric acid
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strong acid
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HBr
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hydrobromic acid
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strong acid
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HI
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hydroiodic acid
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strong acid
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HNO3
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nitric acid
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strong acid
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HClO4
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perchloric acid
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strong acid
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H2SO4
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sulfuric acid
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strong acid
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H3PO4
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phosphoric acid
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weak acid
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H2CO3
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carbonic acid
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weak acid
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CH3CO2H
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acetic acid
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weak acid
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H2C4H4O6
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tartaric acid
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weak acid
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H3C6H5O7
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citric acid
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weak acid
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HC9H7O4
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asprin
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weak acid
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LiOH
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lithium hydroxide
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strong base
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NaOH
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sodium hydroxide
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strong base
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KOH
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potassium hydroxide
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strong base
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Ba(OH)2
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barium hydroxide
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strong base
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NH3
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ammonia
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weak base
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First Rule for Assigning Oxidation Numbers
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each atom in a pure element has an oxidation number of zero
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Second Rule for Assigning Oxidation Numbers
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for monatomic ions the oxidation number is equal to the charge of that ion
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Third Rule for Assigning Oxidation Numbers
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when combined with another element, the oxidation number of fluoride is (-1)
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Fourth Rule for Assigning Oxidation Numbers
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oxidation number of oxygen is (-2) unless
- combined with fluorine - forms peroxides - in super oxides |
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Fifth Rule for Assigning Oxidation Numbers
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Cl, Br, and I have oxidation numbers of (-1) unless combined with oxygen or fluorine
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Sixth Rule for Assigning Oxidation Numbers
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the oxidation number of hydrogen is (+1) except in metal hydrides
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Seventh Rule for Assigning Oxidation Numbers
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algebraic sum of oxidation numbers of atoms in a compound must be zero unless in a polyatomic ion where sum = charge of ion
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Eighth Rule for Assigning Oxidation Numbers
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oxidation numbers of group 1 and 2 elements are +1 and +2 respectively
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Common Oxidizing Agents
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O2, F2, Cl2, Br2, I2, HNO3, MnO4-, CrO42-, Cr2O72-
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Common Reducing Agents
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H2, pure metals (Na, K, Fe, Al)
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Standard State
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the most stable form of a substance in the physical state that exists at a pressure of 1 bar and at a specified temperature
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^rH
delta r H degrees |
pure, unmixed reactants in their standard states have formed pure, unmixed products in their standard states
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Enthalpy in an Endothermic Reaction
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(+)
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Calorimetry
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energy evolved or required as heat in a chemical or physical process is measured by this
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Coffee Cup Calorimeter
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constant pressure
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Bomb Calorimeter
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constant volume
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Hess's Law
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if a reaction is the sum of two or more other reactions, then the change of enthalpy-r for the overall process is the sum of the change in enthalpy-r of all those reactions
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Standard Molar Enthalpies of Formation
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the enthalpy change for the formation of 1 mol of a compound directly from its component elements in their standard states
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Formula for Enthalpy Change of a Reaction
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sum of heat of formation of products- sum of reactants
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Electromagnetic Radiation
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type of radiation including light, microwaves, radio waves, x-rays, etc
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Frequency (nu)
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units = 1/s or hz
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Wavelength (lambda)
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units = meters
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Longest Wavelength on Visible Spectrum
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red
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Highest Frequency and Energy on Visible Spectrum
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violet
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Planck's Law
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electromagnetic radiation emitted is caused by vibrating atoms in the heated object
- each atom (oscillator) had a fundemental frequency and emitted radiation only had certain energies |
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Planck's Equation
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E = nhv
E = hv |
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Quantization
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only certain energies are allowed
- Planck's constant is a proportionality constant |
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Photoelectric Effect
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electrons are ejected when light strikes the surface of a metal but only if the frequency of the light is high enough
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Photons
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massless particles of light that are particle-like and are proportional the the frequency of the radiation as defined by Planck's equation
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Line Emission Spectrum
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spectrum of light created by passing a beam of light from excited atoms through a prism
- spectrum is limited |
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Ground State
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atom with its electrons in the lowest possible energy levels
- n=1 - electrons closest to nucleus as possible - energy is as negative as possible - as n increases, distance from the nucleus increases |
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Excited States
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electrons have less negative energy values (higher energy values)
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Electron Density
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- psi squared
- probability of finding an electron in a given point in space |
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Psi
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value of wave function
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Orbital
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defines the region of space in which an electron is most likely to be located
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Principal Quantum Number
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n = energy of orbital = shell = size of orbital
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Azimuthal Quantum Number
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l = shape of orbital = subshell = number of planar nodes
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Magnetic Quantum Number
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ml = orientation of orbital within subshell
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Subshell Labels
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s, p, d, f
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Number of Subshells in a Shell
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n
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Number of Orbitals in a Subshell
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2L + 1
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Number of Orbitals in a Shell
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n squared
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Nodal Surface
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surface on which the electron has no probability of being found
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Dimagnetic
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electrons slightly repelled by magnetic field
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Paramagnetic
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slightly attracted to magnetic field
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Ferromagnetic
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very attracted to magnetic field
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Order of Electromagnetic Spectrum from Highest Frequency to Lowest Frequency
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y-rays, x-rays, UV, visible light, IR, microwave, FM radio, AM radio, long radio
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