inorganic chemistry

what is electromagnetic radiation?

a family of waves that transfer energy, move at the speed of light and can travel through a vacuum

what does EM radiation display?

wave particle duality

what are the particle properties of EM radiation?

when emitted or absorbed EM radiation acts like a stream of particles

what is a photon photon?

an EM particle that holds a fixed quatra of energy proprtional to its frequency

what is a quatra?

a fixed packet of energy of a certain wavelength and frequency

what are the wave properties of EM radiation?

EM radiation displays both wavelength and frequency

describe bohrs model of an atom?

atoms have fixed energy levels that each contain electrons, electrons can move between these levels when the emit/absorb radiation

what is an absorption spectra?

a spectra with gaps that shows what energy of photons are absorbed by atoms for electrons to be promoted

what is an emission spectra?

a spectra with lines that show what energy photons are emitted by falling electrons in an atom (electrons must first be promoted by providing them with energy via heat)

why are spectra useful?

each element produces a unique spectra so they can be used to identify elements

what do the intensity of lines in a spectra show?

the concentration of an element as there are more electrons making that transition.

what occurs when energy is transferred to an atom

promotion of electrons to higher energy levels

what happens when an electron falls from a higher energy level to a lower one

photons are emitted that correspond to the energy gap

what do electrons display?

wave particle duality

what type of waves are electrons?

stationary waves, they vibrate in time but do not move in space

what do different wavelengths of electron do?

they inhabit different areas of space known as orbitals

what is an orbital?

a region in space where you are likely to find an electron

how many electrons can an orbital hold?

2 electrons with opposite spins

how can you describe the location of an electron in an atom?

by using the 4 quantum numbers, no two electrons will have the same quantum numbers

what does the principle quantum number (n) represent?

the energy level an electron is on

what is the range for the quantum number n?

1 to infinty

what does the angular momentum quantum number (l) represent

the type of orbital that the electron is in

what is the range for quantum number l

0 to (n-1), we only use 0-3

what shape is an s orbital?

spherical

what energy level do s orbitals start at?

n=1

what is the l value for an s orbital?

l=0

what shape is a p orbital?

peanut shaped or 8

what energy level do p orbitals begin at

n=2

what is the value of l for a p orbital?

l=1

what is the shape of a d orbital?

3 pettled flower or + but rounded

what energy level do d orbitals begin at?

n=3

what is the value of l for a d orbital

l=2

what energy level do f orbitals begin at?

n=4

what is the value of l for an f orbital?

l=3

what does the magnetic quantum number (m_l) represent

the orientation of the orbital the electron is in

what is the range of values for m_l?

-l to +l

how many orientations does the s orbital have?

1

how many orientations does the p orbital have

3

how many orientations does the d orbital have?

5

how many of each orbital does an energy level contain?

one of each orientation of orbital that is present on that level

what does the magnetic sin quantum number (m_s) represent?

the spin of the electron in the orbital

what is the range of values for m_s

+1/2 or -1/2 this represents up spin or down spin

what is Heisenberg’s uncertainty principle

it is impossible to determine the momentum and position of an electron at the same time. it can only be determined where it has the highest probability of being.

what is the Aufbau principle

electrons occupy the lowest available energy level so fill orbitals in order of increasing energy

what is Pauli’s exclusion principle?

no two electrons have the same 4 quantum numbers so each orbital can hold 2 electrons of opposite spin

what is Hund’s rules of maximum multiplicity?

when in orbitals of equal energy electrons will remain unpaired until all orbitals are occupied and will then pair up with opposite spin

what does degenerate mean

have the same amount of energy, applies to orbitals of the same type on the same level

which orbital is higher in energy 3d or 4s

3dw

which orbital will fill and empty first 3d or 4s?

4s

what does spectroscopic notation show

the energy level, type of orbital and number of electrons in that type of orbital

what do boxes and arrows represent in orbital box noation?

boxes= an orbital arrows= an electron

what is the s block in the periodic table?

far left hand side

what is the p block in the periodic table?

far right hand side

what is the d block in the periodic table?

transition metals

what is the f block in the periodic table?

bottom block

when are atoms more stable

when degenerate orbitals are empty, full or half full

why do Cr and Cu only have one 4s electron?

it is more stable for the second electron to be in the 3d orbital

what type of electron repels more strongly?

unbonded electrons

how are electrons arranged around atoms?

to minimise repulsion

what is the molecular shape for 2 electron pairs?

linear

what is the molecular shape for 3 electron pairs?

trigonal planarwh

what is the molecular shape for 4 electron pairs?

tetrahedral

what is the molecular shape for 5 electron pairs?

trigonal bipyramidal

what is the molecular shape for 6 electron pairs

octahedral

what is a transition metal?

a metal that has at least 1 ion with an incomplete d sup-shell

what does the oxidation sate of an atom relate to?

its oxidation number

what does oxidation number show?

the number of electrons added/removed from an atom it is the same as its charge

what does the sum of oxidation numbers in a molecule =?

the charge of the molecule

what is the oxidation number of an atom

0

in most compounds what is the oxidation number of oxygen?

-2i

n most compounds what is the oxidation number of hydrogen

+1

how many oxidation states do transition metals have?

many with varying stabilities and colours

when does a redox reaction occur?

when there is a change in oxidation state

what is a oxidation reaction?

when there is an increase in an atoms oxidation number

what is a reduction reaction

when there is a decrease in an atoms oxidation number

what type of oxidation state do oxidising agents have?

high

what type of oxidation state do reducing agents have?

low

what is a ligand

a negative ion or molecule with non-bonding electrons that forms dative covalent bonds with a metal ion to form a complex

what is a dative covalent bond?

a covalent bond where one atom supplies both of the electrons

what is classifaction of ligands based on?

the number of binding sites, monodentate, bidentate….

what is the co-ordiation number of a complex?

the number of dative covalent bonds between a ligand and a metal ion

what ion is written first in ionic compounds?

positive ion

what makes up a complexes name?

number of ligands, type of ligand, metal

how is the number of ligands represented?

prefix of mono, bi, tri…

how to the names of most ligads end?

with an o eg. flourido, iodido

what is the name for a water ligand?

aqua

what is name for a carbon monoxide ligand

carbonylw

what is the name for an ammonia ligand

ammine

what is the name for a C₂O₄ ^2- ligand?

oxalato

how is a positive metal ion in a complex written?

normally

how is a negative metal ion written in a complex

with ate at the end, some use latin name

what is the name for a negative iron ion in a complex?

ferrate

what is the name for a negative copper ion in a complex?

cuprate

what is the colour of a surface caused by

the reflection of that wavelength of light

what effect do ligands have on the d orbitals of the metals?

they cause them to split so they are no longer degenerate

why do ligands cause d orbital splitting

approaching ligands cause electrons in orbitals lying on the axis to be repelled

what causes colour in complexes?

electrons absorb light to be promoted between split d orbitals, the wavelength adsorbed corresponds to the energy gap

what is a strong field ligand?

ligand that causes a large split in d orbitals

what is a weak field ligand?

ligand that causes a small split in d orbitals

what is the spectrochemical series?

ligands ranked in the order of their ability to split d orbitals