Shapes Flashcards
2 bonding
linear 180 straight line
three bonding
trigonal planar, 120 equilateral triangle
four bonding
tetrahedral 109.5 one up, one a bit right, wedge down, dashes a bit left
three bonding one lone
trigo al pyramidal, 107, same as tetrahedral but lone goes uo
two bonding two lone
bent, 104.5, cross with top two lone
six bonding
octahedral 90 top dashes bottom wedges vertical lines
electronegativity
relative tendency of an atom in a covalent bond to attract electrons in the covalent bond to itself
what makes electronegativity increase:
proton/charge increase, atomic radius decrease (across period) and shielding decrease (up a group)
what’s a polar covalent molecule
covalent but with dipoles
symmetric molecules
all bonds are identical and there aren’t any lone pairs as dipoles cancel out with no net dipole moment
electronegativity difference above 1.8=
ionic bond
why do like pairs repel more
as electrons are only in one atom the charge density is greater