Atomic structure 2 : electron configuration and ionisation energies practice q Flashcards
identify element
[Ne]3s2 3p1
aluminium
by referring to highest energy electron explain why aluminium is a p block element
its highest energy electron is in a p orbital
electron configuration of:
[Ar] 3d2 4s2
titanium
explain why sodium is placed in s block in periodic table
outer e- is in an s sublevel
state the difference in the chemical properties of isotopes of the same element
no difference
electon configuration is the same
identify the element that has a 2- ion with an electron configuraton of 1s2 2s2 2p6
oxygen
The first IE of lithium is higher than that of sodium because..
Na atomic radius is larger - outer electron is further from nucleus
Na outer electron is in third shell so it has additional shielding
meaning effective nuclear charge is decreased
explain w the first ionisation energy of magnesium is greater than the first ionisation energy of magnesium
electron removed from a positive ion
mg+ is smaller than mg
state an explain the general trend in the first ionisation energies of the period 3 elements sodium to chlorine
increases
more protons
smaller atomic radius
same shielding
state how element sulfur deviates from the general trend in the first ionisation energies across period 3
lowers
two pairs of electrons in p orbital repel each other
a general trend exists in the first IE of the period 2 elements lithium to fluroine
what is one element which deviates from this trend
boron/oxygen
state the trend in first ionisation energies in group 2 from beryllium to barium
decreases
electrons removed from shell
atomic radius increases
as group is decende
state and explain the general trend in first IE for the period 3 elements aluminium to argon
increases
same shielding
smaller atomic radius
increased number of protons
