C1- Atomic Structure Flashcards
what are the theee subatomic particles that make up an atom
protons neutrons electrons
proton:
1) relative mass
2) actual mass
3) relative charge
1) 1
2) 1.67x10^-27Kg
3) +1
neutron:
1) relative mass
1) 1
electron:
1) relative mass
2) relative charge
1) 1/1840
2) -1
what subatomic particles are neucleons
protons and neutrons
what is different about isotooes
number of neutrons
what is the mass number equal to
number of protons and neutrons
name three tyoes of isotooes of hydrogen
protium
deuterium
tritium
what is relative atomic mass RAM relative to
1/12 the mass of carbon-12
what dies TOF stand for
time of flight
name two methids of ionisation
electrospray and electron impact
what tyoe if solvent is used in TOF-MS
polar solvent
how are particles accelerated in TOF-MS
using an electric field
all particles are given the same…
kinetic energy
what sorr of oarticles move fastee?
lighter oarticles
how are particles detected in TOF-MS
ions cause an electric current to flow when they hit the detector
what is plotted in a mass spectrum
relative abundance vs mass to charge ratio (m/z)
what is the largest peak in a MS called
base peak
what does the base peak show?
the most stable ion
what dies the peak with the highest mass show?
the molecular ion
what does the molecular ion peak show?
relative molecular mass
what is the wnergy level number called
the principle wuantum number
what happens to the energy levels as you move further from the nucleus?
they get closer together
what is a sub shell
an orbital or combination of orbitals
name to 4 sub shells
s, p, d and f
hiw many electrons can an irbital hold
1
ehy do electrons in the same orbital have opposite spins?
to minimise repulsion
how many s orbitals are there
1 per energy level
how many p orbitals are there
3 per energy level starting at n=3
how many d orbitals are there
5 per energy level starting at n=5
in what order are the sub shells filled
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 7s
whoch is written first 3d or 4s
3d
what do up and down areows represent
the spin of an electron
how are p orbitals filled
1 in each orbital before pairing
why does chromium have the configuration 4s1 3d5
1/2 filled d shell is more stable
why dies copper have the configuration 4s1 3d10
filled d subshell is more stable
why is a full/half full d subshell more stable
symmetry around a nucleus
what happens to metal atoms to form ions
lose electrons
what haooens to non metal atoms to form ions
gain electrons
which electrons are lost first for transition metals 3d or 4s
3d
what is the first ionisation energy?
the energy required to remove mole of electrons from one mol of gaseous atoms to form one mole of gaseous ions
what dies a large gap in successive ionisation energy mean
the electron has been lost from an energy level closer to the nucleus
why do successive ionisation energies increase
greater effective nuclear charge
what is the trend in ionisation emergy down group 2
decreases
what is the GENERAL trend in ionisation energy across period 3
inscreases
why is the first ionisation energy of Al less than Mg
occupying the 3p subshell which is further from the nucleus
why is the first ionisation energy of S less than P
repulsion between paired electrons
