exam #3 Flashcards
wahhhhhhh
what is an oxidation-reduction reaction?
electron transfer from one species to another
what is the oxidation number of a free element?
0
what is the oxidation number of a monatomic ion (ion of only one atom)?
the charge of the ion (like Cl- or Be2+)
what is the oxidation number of H in compounds with nonmetals?
+1
what is the oxidation number of F in all compounds?
-1
what is the oxidation number of O in most compounds?
-2
what is the oxidation number for alkali metals? alkaline earth metals?
alkali metals = +1
alkaline earth metals = +2
what is the oxidizing agent?
the reactant that undergoes “GER” and gains electrons
what is the reducing agent?
the reactant that undergoes “LEO” and loses electrons
what is the difference between absorption and emission?
absorption = gaining energy & jumping to a higher energy level (like 2 to 4)
emission = losing energy & falling from an excited state to a lower level (like 4 to 2)
what is the quantum number “n” and what does it say about an orbital?
- principle quantum number
- describes SIZE of the orbital
what is the quantum number “l” and what does it say about an orbital?
- angular momentum number
- describes SHAPE of the orbital
what is the quantum number “ml” and what does it say about an orbital?
- magnetic quantum number
- describes ORIENTATION of the orbital in space
what is the quantum number “ms” and what does it say about an orbital?
- spin magnetic quantum number
- describes ELECTRON SPIN of the orbital
what do s orbitals look like and for what values of n are they possible?
- sphere, sun
- possible for ALL values of n
what do p orbitals look like and for what values of n are they possible
- peanut, pair of pears
- possible for n=2 and higher
what do d orbitals look like and for what values of n are they possible
- dutterfly, dragonfly
- possible for n=3 and higher
what do f orbitals look like and for what values of n are they possible?
- full flower, fish frenzy
- possible for n=4 and higher
how do you know the number of angular nodes?
same as l value of the orbital
what is the aufbau principle?
when electrons are filling an orbital, they fill the lowest energy orbitals first (1s, 2s, etc.)
what is the trick to remembering the ordering of orbitals from lowest to greatest?
1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
6s 6p 6d
7s 7p
(diagonal lines from right to left to tell ordering)
what is the pauli exclusion principle?
each orbital can only contain up to two electrons, and if paired up, the electrons must be of opposite spins
what is hund’s rule? (bus seat rule)
electrons pair up only if they have to
how do you calculate energy when given wavelength?
E = ((hc)/wavelength)
