Shapes of Molecules and Intermolecular Forces Flashcards
how many bonded/lone pairs and bond angle in a pyramidal
3 bonded pairs, one lone pair , 107 degrees
how many bonded/lone pairs and bond angle in a non-linear shape
2 bonded pair , 2 lone pair , 104.5 degrees
how many bonded/lone pairs and bond angle in a linear shape
2 bonded pairs , 180 degrees
ow many bonded/lone pairs and bond angle in trigonal planar
3 bonding pairs, 120 degrees
how many bonded/lone pairs and bond angle in octrahedral
6 bonding pairs , 90 degrees
what is electronegativity?
attraction of a bonded atom for the shared pair of electrons in a covalent bond
how does electronegativity change across periodic table?
nuclear charge increases and atomic radius decreases
what are the most electronegative atoms?
non metals , nitrogen, oxygen , fluorine, chlorine
what are the least electronegative atoms?
group 1 metals including lithium , sodium , potassium,
what is the electronegativity difference in each bond type?
covalent = 0
polar covalent = 0-1.8
ionic = greater than 1.8
when is a bond non-polar
1) if bonded atoms are the same ( pure covalent bond)
2) if bonded atoms have similar or same electronegativity
what is a polar covalent bond?
a bond will be polar when the bonded atoms are different and have different electronegativity values
how are induced dipole-dipoled formed
movement of electrons produce an instananeous dipole which induces a dipole on a neighbouring molecule. The induced dipole induces further dipoles on neighbouring molecules which then attract one another
which element has higher boiling point ( helium , 2 electrons) ( neon, 10 electrons) ( argon, 18 electrons)
argon has highest boiling point as there are more electrons so larger instantaneous and induced dipoles therefore greater induced dipole-dipole interactions and attractive forces between molecules as a result more energy needed to oversome the intermolecular forces.
what is the solubility of non-polar molecular substances
when added to non-polar solvent, intermolecular forces form weakening intermolecular forces in the molecular lattice which breaks it down and dissolves
insoluble in polar solvents as intermolecular bonding in polar solvent is too strong to be broken