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Covalent Bonds
Term | Definition |
---|---|
1st element when naming a covalent compound | prefix is used when there are more than 1 that correspond to the # of the element used (mono- is not used) |
2nd element when naming a covalent compound | prefixes are always used that correspond to the # of the element used (including mono-), -ide ending is used |
covalent bonds | very strong, atoms share electrons, only nonmetals/right side of periodic table is used |
di- | 2 |
tri- | 3 |
tetra- | 4 |
penta- | 5 |
mono- | 1 |
hexa- | 6 |
hepta- | 7 |
octo- | 8 |
nona- | 9 |
deca- | 10 |
if an O is next to an A or another O | the A or O on the prefix is dropped |
VESPR theory | valence, electrons, shell, pair, repulsion |
single bond | one pair of electrons is shared, represented by a regular line (-) |
double bond | two pairs of electrons are shared, represented by 2 lines (=) |
triple bond | three pairs of electrons are shared, strongest bond, represented by three lines (≡) |
all atoms want to get to... | 8 valence electrons ---> stable |
how many atoms are needed to make a bond angle | 3 |
hydrogen is an exception because | it only needs 2 valence electrons to be stable instead of 8 |
central atoms | have the most places to bond (carbon) |
linear (2 atoms) | no bond angle |
linear (3 atoms) | 180 |
bent | 104.5, 3 atoms, 2 bonds, 2 unshared pairs |
planar triangular | 120, 4 atoms, 3 bonds |
tetrahedral | 109.5, 5 atoms, 4 bonds |
pyramidal | 107, 4 atoms, 3 bonds, 1 unshared pair |
unshared pairs | pairs of electrons that aren't bonded to anything, take up more space than a bond, make the bond angle smaller |
triangle in diagram | an atom is in front |
dotted line in diagram | an atom is behind |
valence electrons are found by | the last digit of the column number on the periodic table |
coordinate covalent bonds | when one atom brings no/extra electrons and bonds to the central atom's electrons, creates a charge, brackets with the charge are used ([]) |
negative charge | electrons are gained |
positive charge | electrons are lost |
electronegativity difference | how strong the bond is |
0-0.45 | non polar |
0.45-1.95 | polar |
1.95 + | ionic |
nonpolar covalent bond | no negative/positive ends |