chem test 2

schrodingers & heisenberg atom

cloud of electrons and explained how electrons jump

heisenberg uncertainty principle

we cannot state where an electrons exactly is on any given time but we do know the region it exists (it is on)

bohrs atom

included electrons circling the nucleus in orbits

orbital

region where electron is found 90% of the time (2 electrons can fit in the orbital)

how many orbitals does sublevel S have?

1

how many orbitals does sublevel P have?

3

how many orbitals does sublevel D have?

5

how many orbitals does sublevel F have?

7

sublevel S & P

4 total orbitals (1+3) (x2= total # of electrons)

sublevel S, P, & D

9 total orbitals (1+3+5) (x2= total # of electrons)

sublevel S, P, D, & F

16 total orbitals (1+3+5+7) (x2= total # of electrons)

what 2 things does the energy level indicate

amount of energy an electron has and how far they are from nucleus

what 2 things does the subevel indicate

number of electrons & shapes (direction they are travelling)

pauli exclusion principle

maximum of 2 electrons per orbital opposite signs (roomates who dont like eachother)

aufbau principle

fill lowest energy orbital first (few expectations to this rule except Cu, Cr, Ag, & Au because having half full on completley full d sublevel by taking one s e- is more stable)

hunds rule

max # of unpaired electrons in equal energy orbital

atomic emissions spectra

pattern of light color emitted by electrons

electron jumping to higher energy level

the absorption of a photon (bundle) of energy (matches difference between two energy levels)

photon

packet of light that an electron absorbs/ emits

electron jumping back down to ground state

releases its energy by emitting a photon (packet of energy) which causes an electron to emit light

elements emitting light with particular color ‘fingerprint’

their electrons occupy energy levels & every element has a different # of protons/ electron (they absorb different frequencies of photon energy)

ground state

normal energy level/ sublevel (write it with electron configuration)

excited state

greater than normal energy level for electron

what kind of light emits a mixture of frequencies?

sunlight, LED light

different colors of light when burning fireworks

different metals produce different colors when burned because they absorb different frequencies of photons

electronegativity

ability of an atom to attract electrons in compound (F= highest, Fr= lowest)

ionization energy

energy needed to remove atom/ existing electron (F= highest, Fr= lowest)

atoms get smaller, electronegativity increases, & ionization energy increases (as you go left to right across PT within same group)

because of increase # of protons & increase in nuclear charge (proton pull) (elements are less inclined to lose electrons & want one more)

proton pull

increases as you move left to right, it affects period trend because # of proton in nucleusnincrease (protons have stronger pull in nucleus on valence e-)

atoms get bigger, electronegativity decreases, & ionization energy decreases (as you go top to bottom on PT)

because youre adding layers of electrons & distance from nucleus (shielding, creates interference between nucleus & valence e- which causes electronegativity & ionization energy to decrease)

shielding

distance from nucleus, interference from inner electrons, it affects group trend because it increases as you move down a column, as you move down PT there are many layers of electrons that create interference between nucleus & valence e- (Fr= high shielding, Fe= low shielding)

smallest atomic size

closest to right/ farthest up because proton pull, less energy levels (layers)

lowest electronegativity

closest to left/ farthest down because more shielding (group trend) & less proton pull

highest ionization energy

closest to right/ farthest up because less shielding (higher on PT) & more proton pull, electrons are difficult to remove from atom

why does increasing the # of protons make the element/ atom smaller & electronegativty/ ionization energy higher?

because of shrinking of atom, as you increase the p+ they pull on valence e- more

why does increasing shielding make the element/ atom bigger & electronegativty/ ionization energy lower?

because shielding makes more energy levels, creates interference between nucleus (p+) % valence e-, extra electron shells are added as you go down which increases inner-electron shielding/ distance which weakens nucleus oull on outer electrons