Bonding Flashcards
why is ionic bonding stronger with smaller ions
less shielding/ smaller atomic radius
what is the structure of ionic crystals
giant lattice of crystals
covalent bond definition
shared pair of electrons
co-ordinate bond definiton
shared pair electrons from only one of the bonding atoms
metallic bonding definition
electrostatic force of attraction between delocalised electrons and positive metal ions
factors affecting electronegativity
number of protons- more=more electronegative
shielding, atomic radius
when would bonds with a big electronegativity difference NOT be polar
if the molecule is symmetrical- then the dipoles cancel out
what affects the strength of metallic bonding
Number of protons/ Strength of nuclear attraction. The more protons the stronger the bond
Number of delocalised electrons per atom (the outer shell electrons are delocalised) The more delocalised electrons the stronger the bond
- Size of ion. The smaller the ion, the stronger the bond.
name and bond angle of shape with 2 bonding 0 lone pairs
180, linear
name and bond angle of shape with 3 bonding 0 lone pairs
trigonal planar, 120
name and bond angle of shape with 4 bonding 0 lone pairs
tetrahedral, 109.5
name and bond angle of shape with 5 bonding 0 lone pairs
trigonal bipyrimiday, 120 and 90
name and bond angle of shape with 6 bonding 0 lone pairs
octahedral, 90
name and bond angle of shape with 3 bonding 1 lone pairs
trigonal pyrimidal, 107
name and bond angle of shape with 2 bonding 2 lone pairs
bent, 104
trend of electronegativity across a period
increases as atomic number increases, atomic radius decreases and shielding stays the same
why does electronegativity decrease down the group
shielding decreases
what increases the strength of Van Der Waals forces
increasing number of electrons/ size of atom
what are the 4 types of crystal structure
ionic, metallic, molecular and macromolecular
