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72 Cards in this Set
- Front
- Back
Oxidation # of F
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-1
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Oxidation # of 0
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-2
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Oxidation # of H
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+1 for nonmetals
-1 for metals |
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Oxidation #'s in Groups 1, 2, & 13
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+1, +2, +3
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Ammonium Ion
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NH4+
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Hydroxide
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OH-
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Perchlorate
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ClO3-
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Nitrate
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NO3-
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Bicarbonate/Hydrogen Carbonate
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HCO3-
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Cyanide
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CN-
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Sulfide
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SO4-2
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Carbonate
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CO3-2
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Phosphate
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PO4-3
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Naming Ionic Compounds
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name the element on the left, if it's a transition metal use a roman numeral to indicate charge after crossing, then name the element on the right and change the ending to -ide.
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Naming Binary Molecular Compounds
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name the element on the left with a prefix to indicate number of atoms except one (mono), tehn name the element on the right, changing the ending to -ide and use a prefix to indicate number of atoms.
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Types of Intermolecular Forces in Order of Decreasing Strength
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hydrogen bond > dipole force > london force
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Decreasing Strength of Bonds
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ionic bond > covalent bond > intermolecular force
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Hybridization
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mixture of 2 or more orbitals to make new hybrid orbital of equal energy
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VSEPR Theory
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states repulsion between pairs of VE; used to predict geometry
A = central atom B = atom bonded with central atom E = lone pair on central atom |
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AB2
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linear
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AB3
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planar
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AB2E
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bent
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AB4
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tetrahedral
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AB3E
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pyramidadl
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AB2E2
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bent
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Resonance
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2 or more valid Lewis Structures can be drawn
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lattice energy
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energy released when one mole of a crystalline compound is formed from one mole of it's gaseous inos
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Polar Covalent
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electron pairs shared unequally
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Nonpolar Covalent
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electron pairs shared equally
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Electronegativity Differences
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0 - .4 = nonpolar covalent
.4 - 1.7 = polar covalent 1.7 + = ionic |
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Metal + Nonmetal =
(bond type) |
ionic
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Identical Nonmetal =
(bond type) |
nonpolar covalent
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Different Nonmetals =
(bond type) |
polar covaletn
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Carbon + Hydrogen =
(bond type) |
nonpolar covalent
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Ionization Energy
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energy required to remove one electron from an atom
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Elevtronegativity
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ability of one atom to attract another atom
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Atomic Radius
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1/2 distance between two bonded atoms
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Noble Gases
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Group 18; 8 VE, unreactive
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Halogens
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Group 17; 7 VE, gases, liquids or solids, react with metals to form salts
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Alkaline Earth Metals
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Group 2; 2 VE, react with nonmetals but not as reactive as alkaline metals, solidss
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Alkaline Metals
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Group 1; 1 VE, solids, react voilently with nonmetals
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Valence Electrons
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number of electrons in highest energy level
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Henry Mosely
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1911, student of Rutherford, studied xrays and ordered periodic table by increasing atomic number, leading to periodic law
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Dimitri Mendeleev
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1869, first periodic table arranged by chemical & physical properties and increasing atomic mass.
-predicted discovery of new elements. -reason for periodicity? -why could some elements not be arranged by atomic mass? |
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periodic law
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phys. & chem. properties of elements are periodic properties of their atomic numbers
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orbital notation
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shows orbitals as dashes with occupying electrons as arrows up and down
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Hund's Rule
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orbitals of equal energy are occupied by one electron before any orbitals are occupied by a second electron
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Paule Exclusion Principle
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maximum of 2 electrons can occupy each orbital
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Aufbau Principl
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electron occupies lowest energy level it can recieve
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s orbital
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spherical
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p orbital
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dumbell/peanut
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d orbital
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complex
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electromagnetic radiation formula
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c = yv ; y = c/v ; v = c/y
e = hv |
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c
y v e h |
speed of light
wavelength frequency energy in joles plank's constant |
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electro magnetic spectrum
--> increasing wavelength <-- increasing energy + frequency |
gamma ray > xray > uv light > visible light > infared light > microwaves > radiowaves
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Hertz (Hz)
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1/s
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Avagandro's Number
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particles in a mole
6.022 x 10^23 |
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molecular mass
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grams per mole
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conversions ( molar mass )
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grams > molar mass > moles
atoms > avagandro's number >moles > molar mass >grams |
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Atomic Mass Unit (amu)
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1/12 mass of one carbon (12 atoms)
1 proton = 1 amu 1 neutron = 1 amu 1 electron = 0 amu |
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Atomic Number
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-number of protons and electrons in an element
-smaller whole number |
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Mass Number
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number of protons and neutrons in an isotope of an element
number of neutrons = mass number - atomic number |
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kilo (k)
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10^3
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deci (d)
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/10
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centi (c)
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/10^2
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milli (m)
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/10^3
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micro (u)
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/10^6
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nano (n)
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/10^9
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Ernest Rutherford
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1911; disproved plum pudding model by finding atomic nucleus w/ gold foil experiment
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J J Thompson
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discovered electron using cathod ray tube & proved electrons had aprticle nature. produced plum pudding model
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Dalton's Atomic Theory
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1. all matter composed of atoms
2. all atoms in an element are identical (false) 3. atoms can't be subdivided, created or destroyed (false, can be subdivided) 4. different atoms combine to forn compounds 5. atoms are rearranged in chemical reactions |
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law of definite properties
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chemical compound contains same element in same proportions
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