Electron configuration and periodicity Flashcards
define the first ionisation energy
the energy required to remove one electron from each atom in one mole of gaseous atoms
general equation for first ionisation energy
E(g) -> E+ (g) + e-
what is needed to remove an electron from an atom
energy
the larger the electrostatic attraction between the electron and the nucleus the
larger the ionisation energy
name three factors that affects ionisation energy
- number of protons
- the shielding
- the size of the atom
why does the number of protons affect ionisation energy
the more protons the greater nuclear charge of the nucleus, so a stronger attraction between valence electrons and the nucleus
why does shielding effect ionisation energy
inner electrons shield the outer electrons from the positive pull of the nucleus
how does the size of the atom effect ionisation energy
greater distance between the outer electron and positive nucleus,weaker attraction
what is the number of successive ionisation energies equal to
the charge on the ion formed `
how does ionisation energy change across a period
it increases
why does ionisation energy increase across a period
with a greater number of protons this increases the nuclear charge,
creating a greater pull to the nucleus meaning more energy is needed to remove the electrons
how does ionisation energy change down a group
it decreases
why does the ionisation energy decrease down a group
the shielding and the number of electron shells increase, this outweighs effects of the nuclear charge. so the nuclear attraction is weaker and the electrons are easily removed
what does atomic emission spectroscopy show evidence of
electrons are present within an atom in quantum shells
in what shell are electron energies lowest
the first shell
what occurs when additional energy is provided to electrons
they are temporarily excited into a higher state, they then return to their more stable, lower energy state. this causes discrete energies to be emitted
what is the point of atomic emission spectroscopy
to identify the elements present within a substance
how many electrons can fit the first quantum shell
two
how many electrons can fit in the second electron shell
eight
how many electrons can fit in the third quantum shell
eighteen
how many electrons can fit in the fourth quantum shell
thirty two
there is a large jump between the 8th and 9th ionisation energies for an element, how many electrons in its outer shell
eight
what is an orbital
a region within an atom that can hold up to two electrons of opposite spin
what is the name and shape of the first orbital
s-orbital, it is spherical
how many electrons can the s-orbital hold
two
what is the shape of the p-orbital
dumbell
how many electrons can the p-orbital hold
six
how many electrons can the d-orbital hold
10 electrons
how many electrons can the f-orbital hold
14 electrons
write out the order of orbitals
s,p,d,f
what is a sub-shell
a group of electrons of the same type of orbital within a shell
write the order of subshells
1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d
6s 6p
7s
how are the full structure of ions different
you must remove the 4s electrons before the 3d
how are the structure of Cr and Cu different
you fill the 3d first, leaving 4s1
why are Cr and Cu full structure different
because its more stable to include a 3d than 4s
when do you fill out 4s2 after 3d
when the element is a transition metal
what block is group 1 and 2 and hydrogen
the s block
what block are the transition metals
the d block
what block are the inner transition metals
the f block
what block is group 0,3,4,5,6,7
the p block
how are blocks decided in the periodic table
according to which sub-shell the last electron occupies
define periodicity
a regularly repeating pattern of atomic, physical and chemical properties with increasing atomic number
