Ch 2 Atomic Structure Flashcards
(20 cards)
Angle of deflection formula
angle of deflection = k x charge/ mass
what is an orbital
a region of space with high probability to find electrons
s orbital characteristics
spherical, symmetrical, non-directional
p orbital characteristics
dumb-bell shape directional
which orbital is more diffused, 2px or 3px
3px (spread over a larger area)
max number of electrons in orbital
2 electrons
special note for electronic energy level
4s lesser energy than 3d (remove and fill 4s first)
but WRITE 3d first
Anomalous electronic configuration
Cr, Cu (both fill up 3d first )
the 3d of both are unusually stable
what does isoelectronic mean
same number of electrons
periodic properties (3)
-more proton, more NC, stronger attraction to nucleus
-increase number of inner shell, more shielding effect
-inner shell number increase, distance between valence e and nucleus increase, weaker attraction
ionisation energy equation
M (g) -> M+ (g) + e
is ionisation energy endo or exo
endothermic
ionisation energy across period
increase IE ax period
irregularities in IE for Al and Mg
1st IE of Al lower than Mg due to shielding effect by 3s e, outweighs increase in NC (easier to remove e)
(same for B and Be)
irregularity of IE for S and P
in S, e removed from doubly occupied 3p orbital, e exp additional inter-electronic repulsion outweighs increase in NC
(same for O and N)
IE down group
IE decreases down group
atomic radius, ionic radius trend
down group: increase
ax period: decrease
Electronegativity trend
ax period: increase
down group: decrease
what is electronegativity
it is the measure of the tendency of an atom to attract a bonded pair of electrons in a covalent bond
explain large increase in ionisation energy
example large increase from 1st to 2nd IE
first electron is from an outer shell, second electron is from an inner shell which is closer to nucleus. stronger attraction between nucleus and atom, much more energy required to remove this electron
also means 1 valence electron
