Studied by 34 people
triple covalent bond
a covalent bond sharing six electrons
Metalic bonds
A
Wavelength
the distance from one point to the next similar point.
Amplitude
The distance from the origin to the crest or the trough on a wave.
Frequency
the number of waves to pass in a period of time.
Electromagnetic spectrum
range of all electromagnetic radiation
Electromagnetic waves
radio waves, microwaves, infrared radiation, visible light, ultraviolet radiation, x-rays, cosmic rays, gamma rays
Photons
packets of light. each frequency carries its own specific amount of energy (quantized).
E=hv
Equation for energy
3x10^8
Speed of light
c=lv
speed of light equation
Bright-light spectrum
each element when excited will give off light and when refracted it will have its own distinct separate lines of color, each with its own frequency.
l (lamda)
wavelength symbol
h
planks constant symbol
v
frequency symbol
c
speed of light symbol
ground state
when electrons are in its lowest energy configuration
excited atoms
atoms that have absorbed a specific amount of energy. electrons have been bumped up to upper energy levels and are unstable.
ionization energy
the energy required to remove a mole of electrons from a mole of gas atoms.
Heisenberg uncertainty principle
we don’t know the momentum or position of a particle.
Orbital
an area of high probability of finding an electron
n, l, m, s
quantum numbers (letters)
energy level
principal (first) quantum number
sublevels
the shape of an orbital
s, p, d, f
sublevels (listed)
double lobes
shape of a P orbital
circular
shape of s orbital
sublevels
second quantum number
orientation around the x, y, z axes
third quantum number
spin
fourth quantum number
hund’s rule
electrons fill one orbital at a time (only two electrons in one orbital) with opposite spin
Cr, Cu
Hund’s rule exceptions
Electron configuration
the procedure of organizing electrons in atoms from the orbital with the highest energy. assumed to be in the ground stateAufbau principle
shielding effect
inner electrons block outer electrons therefore the larger the atom, the more ______
Aufbau principle
electrons fill one sub level to the next.
valance electrons
electrons in the outer energy level
4s1 3d10
Cu last two terms of e configuration
4s1 3d5
last two terms of Cr configuration
core electrons
electrons that are not in the outer energy level
Pauli exclusion principle
no 2 electrons can have the same set of 4 quantum numbers.
Atomic radius
1/2 the distance between two nuclei of two like atoms in a solid crystal
electronegativity
the attraction that an atom has between a shared pair of electrons and its positive nucleus.
e affinity
energy change for adding an electron to an atom in a gaseous state
Ionic bonds
B
1000s of covalent bonds
C
Intermolecular force
D
Cu, Ag, K, Pb
E
NaCl, MgSO4,
F
Graphite, glass, diamonds
G
Ice, dry ice, sugar, organic solid
H
High
I
High
J
High
K
low
L
Yes
M
No
N
Graphite-yes, diamond-no
O
No
P
crystal lattice, metallic bond, network covalent, molecular
4 types of crystal solids
Crystal lattice
a regular and repeated structure. organized
ionic bonds
an electrostatic attraction due to opposite charges
Metallic bond
an attraction of positive ions to a sea of electrons
Network covalent
crystal in which thousands of atoms are covalently bonded to each other. giant molecule
molecular
solid held together by weak intermolecular forces
valence electrons
electrons in the outer or highest occupied energy level
lewis dot structures
shows valance electrons as dots
octet rule
atoms will gain, lose, or share electrons in order to have the same configuration as the closest noble gas.
covalent bond
an attraction of a shared pair of valence electrons to the positive nuclei.
single covalent bonds
a covalent bond sharing two electrons
double covalent bonds
a covalent bond sharing four electrons
unshared electrons
orbitals of electrons, usually in pairs, not shared b/w two atoms
resonant structures
two or more valid electron dot formulas for a single molecule
sigma bond
bonding orbitals that overlap head to head. there is one _____ in either a single, double, or triple bond
pi bond
bonding orbitals that overlap side by side. occur in double and triple bond
Valence shell electron pair repulsion
VSEPR acronim meaning
VSEPR
orbitals of electrons, bonding and nonbonding, will move geometrically as far away from each other as possible.
linear
A
trigonal planar
B
bent
C
tetrahedral
D
trigonal pyramidal
E
bent
F
180
G
120
H
less than 120
I
109.5
J
greater than 109.5
K
less than 109.5
L
LDF
M
LDF
N
LDF, Dip-dip, h-bond
O
LDF
P
LDF, Dip-dip, h-bond
Q
LDF, Dip-dip, h-bond
R
NP
S
NP
T
polar
U
NP
V
polar
W
polar
X
Note 
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