Chemical Bonding Flashcards
Define metallic bond
electrostatic forces of attraction, between lattice of cations and sea of delocalised electrons in giant metallic substances
Behaviour of valence electrons in metal cation
Mobile and delocalised, move randomly throughout metal cations packed closely in a lattice
Why do metal atoms for cations in solid state
valence elctrons loosely bounded, easily removed
Metallic bonds are <strength> and <direction></direction></strength>
strong, non-directional
strength of metallic bond formula [proportional]
directly proportional to no. of valence e- available for delocalisation per atom / size of metal atm
Why do transition metals have stronger metallic bond than non-transition metals
transition metals have s and d electrons available for delocalisation, smaller cationic radius than s-block elements
define ionic bonds
electrostatic forces of attraction between oppositely-charged ions in giant ionic substances
ionic bonds are <direction></direction>
non-directional
define lattice energy
energy released when 1 mole of solid ionic compound formed from constituent gaseous ions
lattice energy formula [DIRECTLY PROPORTIONAL]
absolute of product of charges divide sum of ionic radius
define covalent bonds
electrostatic forces of attraction between shared pair of electrons and positively-charged nuclei of 2 atoms in simple and giant molecular structures
why is a sigma bond stronger than pi bond
side on overlap less effective than head-on overlap
how many overlapping regions for head-on and side-on overlaps
1 and 2 respectively
