chapter 7 Flashcards
what is the trend across the periods in terms of energy shells
each period starts with a new highest shell
what is the trend going down a group
atomic radius increases , electronic shielding increases
what is ionisation energy
how easily an atom loses electrons
what is first ionisation energy
energy requires to remove one electron from each atom of a mole of a gaseous atom to form one mole of gaseous 1+ ions
what would the first ionisation energy equation for Na be
Na(g) = Na+ + e-
how does atomic radius affect nuclear attraction
The greater the distance between nucleus and electron the lesser the attraction
do B and Al have greater ionisation energies then Be and Mg respectively
no they have less ionisation energy as there are subshells so it is easier to remove 2p1 than 2p2
describe metallic bonding
cations fixed in place
delocalised electrons
how strong is the electrostatic forces of attraction in metallic bonding
metallic bonding has the strongest forces of electrostatic attraction
why does melting point decrease from si and c onwards
goes from giant covalent bonds to simpple covalent bonds
what is group one often called
alkali metals
what is the name of group 2 metals
alkaline earth metals
what is the name of group 0 elements
noble gases
write the second ionisation energy of He
He + = He 2+ +e-
is the first 2p electron easier to remove then a 2s electron
yes as 2 p sub shell has a higher energy
