Unit 3- Atomic Models

dalton

indivisible atom

thomson

charged particles, plum pudding atom

rutherford

gold foil experiment, mass in center, nucleus, mostly empty space

bohr

planetary atom, discovered electron energy levels, rungs of a ladder w/ different energy needed for quantum jumps

quantum mechanical atom (schrodinger)

used math to describe the behavoir and energy of the electron in hydrogen

part 2

electron is shown by where it was not a fixed position (electron cloud)

what is the max # of electrons in any one orbital

2

what is the principle quantum level

energy level- n

s, p, d, f

s= 1 orbital p= 3 orbitals, d= 5 orbitals, f= 7 orbitals

number of sublevels

=n or equal to principle energy level

number of orbitals

n squared

number of electrons

2n squared

what is rule 1

aufbau principle fill the lowest energy level first

what is rule 2

Pauli exclusion principle max number of 2 electrons per orbital and must have opposite spins

what is rule 3

hunds rule, must have max number of unpaired electrons filled one at a time

isoelectric

having no overall charges, protons and neutrons balance each other out

ion

any atom that has an electrical charge which is caused by the loss or gain of electrons

what is the speed of light

c= 3.0 × 10 to the 8 m/s or c= wavelength x frequency

what are the 7 parts of the electromagnetic spectrum from least frequency to most

radio, microwave, IR, vis, uv, x-ray, gamma

do wavelength and frequnecy have a direct ro inverse

inverse

do wavelength and e have a direct or inverse

inverse

do frequency and e have direct or inverse

direct

what is Planck’s constant 

h=6.6× 10 to the -34

what is the ground state

is safe

what is the excited state

gains energy and electrons move up an energy level depending

when it goes to energy level 1

U.V

when it goes down to energy level 2

V.S

energy level 3 and above

I.R