OZ1 (Intermolecular Forces + Electronegativity) Flashcards
describe the trend of electronegativity down a group and across a period
decreases down a group as shielding increases and atomic radius increases so charge density is reduced
increases along a period as the atomic radius decreases and charge density increases
how is a permanent dipole formed
if there are two significantly different electronegativities a polar bond forms and the more electronegative atom draws more of the negative charge towards itself
what are polar molecules
where there is a difference in polarity across the molecule and the bonds do not cancel out, they can align with others to form a lattice of molecules
what are induced dipoles
when the electron arrangement is influenced by the distributions of electrons on another particle
what does the strength of induced dipoles depend on
the larger the Mr, the stronger the forces
as chain length increases, mr increases so ID does causing a higher BP
branching means they’re less able to pack tightly together so the distance they cover increases and the forces are weakened so they have a lower BP
how do IM forces vary down group 7
the Mr increases down the group so IM does too which means it takes more energy to break them
what is hydrogen bonding between
the hydrogen atom and nitrogen, oxygen or fluorine
the lone pair of electrons on these en atoms forms a bond with the polar postier H atom
why does ice have a lower density than water
the hydrogen bonds hold the molecules in a rigid structure with a lot of air gaps
what do hydrogen bonds cause in alcohols
a higher boiling point than alkanes with similar Mr, the lone pair of electrons on the O forms hydrogen bonds with the H on the -OH