c7-Inorg Flashcards
what is the first ionisation energy
the energy required to remove one electron from each atom in one mole of gaseous atoms of an element to form one mole of gaseous 1+ ions
how does atomic radius affect attraction
the greater the distance between the nucleus and the outer electrons the less the nuclear attraction
how does nuclear charge affect attarction
ht emore protons there are in an atom, the greater the attraction between the nucleus and the outer electrons
how does electron shielding affect attraction
electrons are negatively charged, there is repulsion between inner shell electrons and outer shell electrons, this repulsion is called shielding and reduces the attraction between the nucleus and the outer electrons
why are successive ionisation energies higher
as the electrons get removed, the atomic readius will decrease and the nuclear attraction will subsequently increase. this means that the ionisation energy will increase because is taked more energy to remove the electron
what is the def for the second ionisation energy
the energy required to remove one electron from each ion in one mole of gaseous 1+ ions od an element to form one mole of gaseous 2+ ions
how do you know that electrons are being pulled from a new shell
a sudden jump in the ionisation energy indicated that the electron is removed from a different shell
why does ionisation energy increase so suddenly when removing electrons from a new shell thats closer
because the new shell will be closer to the nucleus, meaning that there will be greater nuclear attraction. there will also be reduced shielding
what happens to ionisation energies when going downa group
it decreases going down a group
why does the first ionisation energy decrease when going down a group
-atmoic redius increases
-more inner shells so shielding increases
-nuclear attraction on outer electrons decreases
why does the first ionisation energy from beryllium to boron drop accross period two
-is signifies the filling of a new subshell
-from beryllium to boron, the 2p subshell in boron gains an electron. the 2p subshell has a higher energy than the 2s, meaning that the electron in the 2p is easier to remove hence the lower first ionisation energy
what is a property that is constant in all metals
they can conduct charge
what is metallic bonding
metallic bonding is the strong electrostatic attraction between cations and delocalised electrons
what is a giant metallic lattice
this is where billions of metal aatoms are held together by metallic bonding
common properties of metals:
-strong metallic bonds
-high electrical conductivity
-high melting and boiling points
