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

The Lewis dot structure for BF4 would show Boron in the center bonded to four Fluorine atoms. Boron has three valence electrons and each Fluorine has seven valence electrons. Boron would have a formal charge of +1 in this structure.

Answer 3

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 4

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 5

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 6

..

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.. | ..

:f-c-f:

.. | ..

:f:

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Answer 7

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

Answer 8

thetraedric! thetraedric!

Answer 9

F | F-B-F | F