What is the Lewis dot structure for BF4?

Answer 1

The dot structure for tetraflouroborate starts with the B atom in the center with four single bonds at each cardinal direction. On each of these single bonds is one F atom which also has three pair of dots on the unbonded side. The Lewis structure for BF4 has the four F atoms single bonded to the B atom in the center. Each F atom then has a pair of dots on each unbonded side.
Bromine tetraflouride has a Lewis dot structure similar to that of methane. A single B atom in the center, with four single dashes showing bonds to single F atoms. Each F atom then has three pair of dots on each unattached side.

Answer 2

I'm pretty sure it looks like this:

F3B-NH3

The separate molecules (the structure of which can be found on Wikipedia) are both slightly unstable due to an excess/lack of electrons in the outer shell.

BF3 only has the equivalent of 6 electrons around the central B atom, whereas NH3 has the full 8, but two of those in a free pair - which makes it pretty nucleophilic at that point.

What basically happens is that the free pair on the N Atom both go into a single covalent bond to the B atom, a so called "Dative" bond, forming something similar to a C-C bond.

Answer 3

The dot structure of boron triflouride starts with a single B atom in the middle. On three sides are singly bonded F atoms that also have six dots each.

Answer 4

The dot structure for BF4 starts with the B atom in the center. On each side there is a single bond with an F atom. Each F atom then has three pair of dots, one on each unbonded side.

Answer 5

..

:f:

.. | ..

:f-c-f:

.. | ..

:f:

..

Answer 6

Br has 4 covalent bonds with each F, overall charge is negative.

Answer 7

thetraedric! thetraedric!

Answer 8

F | F-B-F | F