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72 Cards in this Set

  • Front
  • Back
Oxidation # of F
-1
Oxidation # of 0
-2
Oxidation # of H
+1 for nonmetals
-1 for metals
Oxidation #'s in Groups 1, 2, & 13
+1, +2, +3
Ammonium Ion
NH4+
Hydroxide
OH-
Perchlorate
ClO3-
Nitrate
NO3-
Bicarbonate/Hydrogen Carbonate
HCO3-
Cyanide
CN-
Sulfide
SO4-2
Carbonate
CO3-2
Phosphate
PO4-3
Naming Ionic Compounds
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.
Naming Binary Molecular Compounds
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.
Types of Intermolecular Forces in Order of Decreasing Strength
hydrogen bond > dipole force > london force
Decreasing Strength of Bonds
ionic bond > covalent bond > intermolecular force
Hybridization
mixture of 2 or more orbitals to make new hybrid orbital of equal energy
VSEPR Theory
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
AB2
linear
AB3
planar
AB2E
bent
AB4
tetrahedral
AB3E
pyramidadl
AB2E2
bent
Resonance
2 or more valid Lewis Structures can be drawn
lattice energy
energy released when one mole of a crystalline compound is formed from one mole of it's gaseous inos
Polar Covalent
electron pairs shared unequally
Nonpolar Covalent
electron pairs shared equally
Electronegativity Differences
0 - .4 = nonpolar covalent
.4 - 1.7 = polar covalent
1.7 + = ionic
Metal + Nonmetal =
(bond type)
ionic
Identical Nonmetal =
(bond type)
nonpolar covalent
Different Nonmetals =
(bond type)
polar covaletn
Carbon + Hydrogen =
(bond type)
nonpolar covalent
Ionization Energy
energy required to remove one electron from an atom
Elevtronegativity
ability of one atom to attract another atom
Atomic Radius
1/2 distance between two bonded atoms
Noble Gases
Group 18; 8 VE, unreactive
Halogens
Group 17; 7 VE, gases, liquids or solids, react with metals to form salts
Alkaline Earth Metals
Group 2; 2 VE, react with nonmetals but not as reactive as alkaline metals, solidss
Alkaline Metals
Group 1; 1 VE, solids, react voilently with nonmetals
Valence Electrons
number of electrons in highest energy level
Henry Mosely
1911, student of Rutherford, studied xrays and ordered periodic table by increasing atomic number, leading to periodic law
Dimitri Mendeleev
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?
periodic law
phys. & chem. properties of elements are periodic properties of their atomic numbers
orbital notation
shows orbitals as dashes with occupying electrons as arrows up and down
Hund's Rule
orbitals of equal energy are occupied by one electron before any orbitals are occupied by a second electron
Paule Exclusion Principle
maximum of 2 electrons can occupy each orbital
Aufbau Principl
electron occupies lowest energy level it can recieve
s orbital
spherical
p orbital
dumbell/peanut
d orbital
complex
electromagnetic radiation formula
c = yv ; y = c/v ; v = c/y
e = hv
c
y
v
e
h
speed of light
wavelength
frequency
energy in joles
plank's constant
electro magnetic spectrum
--> increasing wavelength
<-- increasing energy + frequency
gamma ray > xray > uv light > visible light > infared light > microwaves > radiowaves
Hertz (Hz)
1/s
Avagandro's Number
particles in a mole
6.022 x 10^23
molecular mass
grams per mole
conversions ( molar mass )
grams > molar mass > moles

atoms > avagandro's number >moles > molar mass >grams
Atomic Mass Unit (amu)
1/12 mass of one carbon (12 atoms)

1 proton = 1 amu
1 neutron = 1 amu
1 electron = 0 amu
Atomic Number
-number of protons and electrons in an element
-smaller whole number
Mass Number
number of protons and neutrons in an isotope of an element

number of neutrons = mass number - atomic number
kilo (k)
10^3
deci (d)
/10
centi (c)
/10^2
milli (m)
/10^3
micro (u)
/10^6
nano (n)
/10^9
Ernest Rutherford
1911; disproved plum pudding model by finding atomic nucleus w/ gold foil experiment
J J Thompson
discovered electron using cathod ray tube & proved electrons had aprticle nature. produced plum pudding model
Dalton's Atomic Theory
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
law of definite properties
chemical compound contains same element in same proportions