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65 Cards in this Set
- Front
- Back
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Acid
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Substance that increase the concentration of hydrogen ions, H+ in solution when dissolved in water
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Base
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Substance that increases the concentration of hydroxide ions, OH- in solution when dissolved in water
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Salt
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Any compound whose anion (-) comes from an acid and whose cation (+) comes from a base
Ex.) Na+ and Cl- |
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Strong electrolytes
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dissolve/ionize completely in water
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Weak electrolytes
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do not ionize completely in water
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Metal oxides
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react with H2O to form a base
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Non-metal oxides
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react with H2O to produce a base
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Oxidation
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losing electrons
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Reduction
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gaining electrons
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Gas-Forming Reactions
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produces a gas as a product (CO2, SO2, SO3, H2)
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Electronegativity
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Increases as you go across and decreases as you go down the periodic table
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Titration
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Generally in acid/base:
To find [HA] |
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Potential Energy
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Dependent upon the position of an object
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1st Law Thermodynamics
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Energy of the universe is constant. Energy can not be created or destroyed
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Hess' Law
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When reactants are converted to products, the overall change in enthalpy is the same whether the reaction takes place in one step or in a series of steps
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Wave
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vibrating disturbance that transmits energy
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Wavelength
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distance between two identical lines
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Amplitude
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distance from middle line to the top of a crest or the bottom of a trough
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Frequency
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the # of wave cycles that pass a certain point in one second
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Speed of Light
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All electromagnetic radiation travels at this speed
(3.0x10^8 m/s) |
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Standing wave
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two or more points of zero amplitude (string that is plucked)
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UV Catastrophe
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Plank - Energy can only be absorbed in "packets" rather than all together
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Photoelectric Effect
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Light bundles = quanta of photons
Evidence = light intensity is related to energy of the light |
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Neils Bohr
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When light emitted from H-gas was split by prism - only a couple light colors showed (spectrum was split)
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Rhyberg Equations
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Describes energy of energy level
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De Broglie
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An electron can behave both as a wave and particle
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Schrodinger: Quantum Mechanical view of the atom
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1. The behavior of an electron in an atom is best described as quantized
2. Each wave function is associated with an allowed Evalue for the electron 3. The energy of an electron is quantized |
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Heisenberg Uncertainty Principle
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You can not determine the exact position and velocity of an electron simultaneously
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Quantum Numbers:
N |
The Principle Numbers:
Defines the size of an orbital and energy of an electron |
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Quantum Numbers:
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The Angular Momentum Numbers
Each value corresponds to a different orbital shape |
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Quantum Numbers:
ml |
The Magnetic Number;
Tells the orientation in space of an orbital |
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Pauli Exclusion Principle
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No two electrons can have the same four quantum numbers: no orbital can hold more than 2 electrons
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Aufbau Principle (Building Up)
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Electrons are assigned to shells and subshells of increasingly higher energy
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Hund's Rule
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The most stable arrangement of electrons is that with maximum number of unpaired electrons
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Paramagnetic
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Unpaired electrons
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Diamagnetic
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Paired electrons
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Valence Electrons
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How many electrons are in the outer shell of an atom
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Atomic radius
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1/2 the distance between two nuclei in adjacent, neutral molecules
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Ionization Energy
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Energy required to remove one electron from a gaseous atom in its ground state
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Electronegativity
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Tendency of atoms to attract shared electrons
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Nonpolar
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Share electrons evenly
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Polar
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Share electrons unevenly
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Ionic Bonds
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large differences in electronegativity
- electrons are TRANSFERRED not shared |
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Electron Affinity
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energy required to gain an electron
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Covalent Bonds
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Electrons are shared between atoms
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Exceptions to Drawing Lewis Structures
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Elements in period 3 or below can have an expanded octet
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Electromagnetic Radiation
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Theory (James Clerk Maxwell) to describe forms of radiation in terms of wave-like electric and magnetic fields
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Frequency
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# of waves that pass a given point in some unit of time
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Visible Spectrum of Light
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ROY G BIV
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Formal Charge
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Determines what resonance structure is better than the others
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Resonance Structures
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All structures should have the same number of electrons.
Position of all elements should remain the same. |
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Isomers
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Different structural layout
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Molecular Geometry
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Ex.) Linear, Trigonal pyramidal
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Lattice Energy
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Energy needed to put together a compound
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Bond Order
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# of shared pairs/# of linked pairs
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Bond Energy
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Enthalpy change for breaking a bond in a molecule of reactants in the gaseous state
Breaking bonds = endothermic Forming bonds = exothermic |
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Linus Pauling
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Valence Bond Theory: Bonding is the result of orbital overlap
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Sigma bonds
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Single bonds electron density is a long bond axis (stronger than pi bonds)
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Orbitals
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Region of space where you're most likely to find an electron in an atom
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Pi Bonds
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account for double bonds and can't exist without sigma bonds and can only occur if on same plane
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Isomers
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Compounds with the same molecular formula but different structures (Geometric vs. Structural)
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Hydrocarbons
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Made of only carbons and hydrogens
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Alkanes
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Saturated
No double bonds Formula: CxH2x+2 |
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Alkenes
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Unsaturated
Double bonds Formula: CxH2x |
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Alkynes
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Unsaturated
Triple bonds Formula: CxH2x-2 |
