marmar atomic structure Flashcards
(48 cards)
what are charges and weights
of the fundamental particles and how are they arranged in an atom
proton - +1 weight 1
neutron- 0 weight 1
electron- -1 weight 1/2000
protons and electrons are placed in the nucleus and electrons prbit around the nucleus in 3d fields called
orbitals
how may kinds
of orbitals are there and what order do they fill up in
s , p , d , f
how many s orbitals can fit
in one energy level
1
how many p orbitals can fit in one energy
level ?
3
how many d orbitals can fit in one energy level
5
how many f orbitals can fit
in one energy level
7
how many electrons can be placed in one orbital ?
describe the electrons
2 electrons with opposite spins
how do the electrons
fill up each set of orbitals
they fill up one in each orbital and them two - bus analogy
define
an
orbital
a region of
space
you are likely to find an electron
how does the periodic table show which orbital the element should end
in
- transitional metals d
- non metals p
- reactive metals ( far right ) s
- bottom bar f
what is the rule about 4s and 3d
the shells fill up
3s 3p 4s 3d 4p 4d 4f
what are the two exceptions to the 4s 3d rule
copper and chromium fill 3d then 4s
what should the electron configuration
for an ion be the same as
the noble gas on the period above it
whats the electron notation for a magnesium atom - atomic number 12
1s(2)2s(2)2p(6)3s(2)
whats the electron comfiguration for a magnesium ion ? if the atomic number of magnesium is 12
1s(2)2s(2)2p(6)
define first ionisation energy ?
the energy needed to remove on
mole of electrons from one
mole of gaseous ayoms to form one mile
of positive ions
define second ionisation energy
the energy required to
remove one mole of electrons
from one
mole of gaseous charged positive ions
what is successive ionisation energy
often a group of several ionisation energies . each one is the removal of an electron from the shells of an
atom or ion
how do you tell what group an atom is in from
its successive ionisation energy table
of graph
you see when the first big jump is and after how many values . the number of values before the first big jump represents the number of electrons on the outermost shell
which shell requires the most energy to remove an electron from
shell 1 - closest to nucleus strongest attraction least shielding
describe in details the graph of first ionisation energy in the third period
- na goes up
- mg goes up
- al goes down
- si goes up
- p goes up
- s goes down
- cl goes up
- ar goes up
why does the ionisation energy in al and s change , and what is the change
the ionisation energy required decreases
this is because aluminiums first electron is a lone electron in 3p orbital
sheilding from the 3s orbital means the electron is lost easier
the electron is easier to remove from sulphur because the final electron is placed in the first full pair of electrons in the 3px orbital .this means there is an increase in repulsive forces making it easier to to be removed
how do first ionisation energy change down a group ?
it decreases -mainly because the atomic radius increases
describe a graph of atomic radius across the third period
na ——->Ar
high atomic radius——>low atomic radius
