Tags & Description
average atomic mass unit
amu
molar mass unit
g/mol
Erwin Schrodinger
quantum mechanical model of the atom, electrons don't always exist, it's impossible to know speed + location of electron
James Chadwick
discovered the nuetron
quantization
the concept that energy can occur only in discrete units called quanta
Niels Bohr
determine energy is quantized, electrons exist at discreet energy levels (bohr model is useful but wrong)
anion
a negatively charged ion with too many electrons
cation
a positively charged ion with too few ions
ion
atoms of the same type and have the same mass, BUT there is a difference in the number of protons or electrons
isotope
atoms of the same type with different numbers of neutrons
what does n stand for?
the charge (if the protons and electrons aren't the same number you put the net charge here)
what does the Z stand for?
the atomic number (number of protons)
what does the A stand for?
the mass number (protons AND neutrons)
gold foil experiment
alpha particles that were shot at gold foil were deflected when they hit the positive center of gold atoms. The nucleus was discovered as a result of this experiment.
Ernest Rutherford
using the gold foil experiment, he discovered protons and the nucleus
plum pudding model
electrons were randomly distributed within a positively charged cloud
cathode ray experiment
An experiment that showed that electrons had mass and a charge, electrons are ejected from the cathode and accelerated through a voltage
JJ Thompson
used the cathode ray tube to discover electrons
plum pudding model
used spherical model
John Dalton
John Dalton atomic theory
everything is composed of an atoms, they can not be created nor destroyed
all atoms of 1 element are identical
atoms of different elements are different masses and sizes
compounds are comprised of whole number combinations of atoms
a chemical reaction occurs is a rearrangement of atoms
Democritus, stated that the atom is based on what two properties?
they are indivisible and atoms of a type are all the same
Average atomic mass formula
(mass of A times percent A) + (mass of B times percent B) / 100
speed
distance / time
density
mass / volume
rows (horizontal)
periods
columns (vertical)
groups or families
s block
first two groups
p block
right six groups
d block
teen groups (middle of periodic table)
f block
bottom fourteen groups
group 1
alkali metals
group 2
alkaline earth metals
groups 3 - 12
transition metals
group 13
boron family
group 14
carbon family
group 15
pnictogen / nitrogen family
group 16
chalcogen / oxygen family
group 17
halogen family
group 18
noble gases
the s orbital shape
sphere
the p orbital shape
dumbbell
the d orbital shape
clover
isoelectronic
the same electron
why is chromium an electron configuration exception?
the electron can be spread out more evenly (memorize the configuration)
why is copper an electron configuration exception?
the 1st set of electron must be paired up so 3d has more room than 4s (memorize the configuration)
Aufbau Principle
electrons must fill the lowest energy level first
Hund's Rule
electrons will spread out across all available energy levels before pairing up
Pauli Exclusion Principle
that no two electrons can be the same (have the same quantum numbers)
what does the n quantum number stand for
the principal quantum number (it is equivalent to the energy level of the electron)
the electromagnetic spectrum from high energy to low energy
gamma ray - xray - ultraviolet - visible - infrared - microwave - radio
photon
a particle that represent a quantum of light