chaper 8 done Flashcards
Whats the structure if silicon and why has it got a high bp
giant covalent macromolecule
strong covelant bonds
alot of energy needed to overcome
What is the structure of phosphorus and sulphur and why does sulphur have a higher bp
simple molecular structure
more electrons in sulphur and bigger molecule
stronger vdw so more energy needed to overcome
why are metals malleable
the layers can slide as there isnt repulsion caused between layers as charge is distributed equally
why does aluminium have a high bp than mg
al forms a more charged ion
more delocalised electrons
so stronger forces of attraction between nuclei and elctons so stronger metallic bond
why does group 1 always have the largest atomic radius in a period
same amount of shells and shielding but lowest nuclear charge so less pull
General trend for first ionisation energies in a period?
they increase
Reason why ionisation energy drops in group 3 and and then group 6?
P orbitals starts to fill up and that experiences shielding from the s orbital and there is more distance from the nucleus.
in group 6 electrons start pairing up in p orbitals and therefore experience repulsion.
3rd ioniataion energy of aluminum
al2+= Al3+ +e- (all in gaseous state)
why is the 2nd ionisation energy of group 4 lower than group 3
because its in p orbital so it experinces repulsion
why is 2nd ionisation energy higher?
More positive ion so more energy needed to seperate
what molecules to Sulphur and phospurus form
simple molecules
S8 and P4
why is the ionisation energy of every element endothermic?
Energy is needed to overcome the forces of attraction between the positive nucleus and the negative outer shell electrons.
why does group 1 always have the highest 2nd ionisation energy out of the period?
because the electron on the most outer shell was removed so the second electron is much closer to the nucleus
