chem 102 final all Flashcards
what is an ionic bond
- electrons are not shared
- large electronegativity difference; usually > 2.0
what is a covalent bond
- bonds created by sharing electrons with other atoms
what is a pure covalent bond (non-polar bond)
- electrons are evenly shared
- little to no electronegativity difference in bonding ( < 0.4)
what is a polar covalent
- bonding electrons are unevenly distributed; atoms partial charges and usually an EN difference of 0.4 to 2.0
which bonds are more polar
higher EN difference = higher bond polarity
lower EN difference = lower bond polarity
VSPER theory
- linear: 180, 2 bonds, no lone pairs
- trigonal planar: 120, 3 bonds, no lone pairs
- trigonal bent: < 120, 3 bonds, one lone pair bond
- tetrahedral: 109, 4 bonds, no lone pairs
- trigonal pyramidal: < 109, 4 bonds , one lone pair
- tetrahedral bent: < 109, 4 bonds, two lone pairs
electron geometry
determined by the number of electron groups
molecular geometry
takes bonds and electrons into consideration, but in the naming it focuses on the atomic bonds (from the push of the electrons)
carbon abilities
forms many compounds because it has the tendency to form four covalent bonds; ability to form double and triple bonds; and the tendency to catenate (bond to other carbon atoms to form chains)
alkane
single bond; 2n + 2
alkene
double bond; 2n
alkyne
triple bond; 2n - 2
isomers (geometric)
cis trans = orientation based on the molecules that are incapable of rotating
isomers (structural)
molecules with the same molecular formula but difference structures
naming (ochem)
meth - 1
eth - 2
prop - 3
but - 4
pent -5
hex - 6
hept - 7
oct - 8
non - 9
dec - 10
