AP Chemistry
Terms
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- Aufbau Principle
- - when building an electron configuration of atom, electrons are placed in orbitals, subshells, and shells in order of increasing energy
- Pauli Exclusion Principle
- - within an atom, no two electrons can have the same set of quantum numbers
- Hund's Rule
- - when an electron is added to a subshells, it will always occupy an empty orbital if one is available
- Diamagnetic
-
- elements with all e- paired up
- unaffected by magnetic fields - Paramagnetic
-
- elements with unpaired e-
- affected by magnetic fields - what does quantized mean?
-
- electrons only exist at certain energy levels
- " a stairs" - energy of an e-
-
En = -2.178 x 10^-18 /n^2
in joules
En = the energy of the e-
n= the principal quantum number - relationship of energy and electronamgnetic radiation
-
change in E = hf = hc/λ
Change in E = energy change
h= plank's constant
f= frequency
λ= wavelength
c= speed of light - speed of light
-
= 3.00 x 10^8 m/sec
speed of light = λf - Planks's constant
- = 6.63 x 10^-34 joule/sec
- de Broglie equation
-
= λ = h/ mv
λ= wavelength
m = mass of particle
v = speed of particle
mv= p = momentum of particle
h= plank's constant - Heisenbergy uncertainty principle
-
- impossible to know both position and momentum of e-
- electron orbital is probabilty of e- found in that region - Quantum theory
-
- E is quantized
E = hf - electron affinity
- - energy when an atom gains an e-
- electronegativiy
- - how strongly the nucleus attracts e-
- which is greater, 1st of 2nd ionization energy?
-
2nd > 1st
; remaining valence electron is closer to the nucleus - what did Milikan do?
-
- found charge of e-
- behavior of charged oil drops in electric field - What did Rutherford do?
-
- found hard nucleus and empty atom
- charged particles at gold foil - What did Neils Bohr do ?
- -predicited that electrons orbit the nucleus at specific fixed radii
- can a theory be proven correct?
-
- no
; can be supported through experimentation but not proved - what did de Broglie discover?
- matter has wave charcateristics
- atomic radius
-
- size decreases when closer to the nucleus
- * top of periodic chart - anion
-
- negativley charge atom
- electron is added - cation
-
- postively charge atom
- electons are removed - to ionize
-
- to remove and e
- forms a cation -
which is larger;
Ca or Ca 2+ ? -
Ca > Ca 2+
; Ca 2+ has less e- so nucleus pulls electons closer to the nucleus -
which is larger?
O or O 2- ? -
O 2- > O
; O has less e- than O 2-, so effective nuclear charge of 0 2- is greater that O and is able to pull farther away fronm the nucleus - what did Dalton do?
- - atoms never created or destroyed
- Dmiritri Medeleev and Lothar Meyer
- - developed periodic table
- what did J.J. Thompson do?
-
- plum pudding model
-wathced deflection of charges in cathode ray tube
- atoms have positive and negative particles
- idea of electrons and protons - what do shell tell?
-
- average distance of e- from nucleus
- higher shell means more energy - what does subshell tell?
- -shape of electron's orbital
- what does orbital tell?
- - orientation of electron's orbital in space
- what do the Quantum numbers describe?
-
the position of electron
- each electron has four quantum numbers - what do spin tell?
- - direction electron spins
-
n
l
ml
ms -
- shell
- subshell
- orbital
- spin