more little things for unit 1 Flashcards
what is the em spectrum in order of increasing wavelength
gamma, x ray, uv, visible, infrared, microwaves, radio and tv waves
what is the formula for calculating frequency when you know the wavelength and the speed
c = f lamda
what is meant by wave particle duality
em radiation can be regarded as a stream of very small particles called photons. so it can behave as both a wave and a partilcle
how can you calculate the energy of photons of radiation
e = planks constant times by frequency
how can you calculate energy of a wave from avogradros number, planks constant, speed and wavelength
e = avo times plank times speed dividied by wavelength
what do the dark lines on line absorption spectrum represent
the certain wavelengths that have been removed by absorption
what do the lines on line emission spectra represent
distinct wavelength of emitted light
what happens when atoms absorb energy
they become excited
what happens when energy is absorbed
the electrons move up to an outer shell. when they move to a lower energy level, a photon is released as a particular wavelength of light. so when electrons fall back and produce these photons, a line on emission spectra is formed from the energy difference.
what regions of the em spectrum does hydrogen have lines
uv, visible and IR
what is meant by ionisation energy
the energy difference between ground state and the convergence limit
how many subshells can each shell have
up to four.
s, p, d and f
what are the subshells in shell 1
1s
what are the subshells in shell 2
2s, 2p
what are the subshells in shell 3
3s, 3p, 3d
what are the subshells in shell 4+
4s, 4p, 4d, 4f, 5s, 5p, 5d, 5f, 6s, etc etc
which block does an atom with an l value of 0 belong in
s
which block does an atom with an l value of 1 belong in
p
which block does an atom with an l value of 2 belong in
d
which block does an aotm with an l value of 3 belong in
f
which section of the periodic table is the s block
groups 1 and 2
which section of the periodic table is the d block
transition metals
which section of the periodic table is the p block
groups 3-0
which section of the periodic table is the f block
lanthanides and actinides
which block is groups 1-2
s
which block is groups 3-0
p
which block is transition metals
d
which block is lanthanides and actinides
f
what shape are s orbitals
spherical
in what order do orbitals fill up
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 8s
are 4s electrons lost before or after 3d electrons during ionisation to positive ions
before
what is the oxidation number in a free or uncombined element
0
what is the oxidation number in single atom ions
equal to the charge on the ion
what is the oxidation number for hydrogen
+1
what is the oxidation number for oxygen
-2
what must the algebraic sum of all the oxidation numbers in a molecule be
0
what must the algebraic sum of all the oxidation numbers in polyatomic ion be equal to
the charge on the ion
how many pairs of electrons do monodentate ligands donate
1
how do you name a complex
metal symbol first. neg ligands next. neutral ligands next. overall charge written after the square brackets
what is a complex
a central metal ion surrounded by ligands
how do you name a negative ligand
ide becomes ido.
ate becomes ato.
ite becomes ito.
how do you name a neutral ligand
water is aqua
ammonia is amine
co is carbonyl
why can transition metals absorb light
because photons excite electrons in the lower d orbitals up to a higher energy d orbital
why do transition metals make good catalysts
- they can form a variable number of bonds due to the availabliity of unoccupied and hal fiflled d orbitals
- this allows easier formation of intermediate complexs
- this provides reaction pathways of lower energy to proceed
