What is the Lewis dot structure of nitrogen fluoride?

Answer 1

Double bond to one oxygen, single bond to the other. This means one electron left over on nitrogen atom. The result is that the N atom does not have a full octet. This is why nitrogen dioxide tends to dimerise into N2O4, in which the nitrogens can share electrons and achieve full octets.

In nitrogen dioxide, the bond order is actually 1.5, an "average" of the double and single bonds, which are delocalised to form the 1.5 bond order.

Answer 2

Formula is NF3 F has 7 valence electrons and N has 5.. so the 3 fluorine atoms share their 7th electron with nitrogen so that they both have a full octet of (8) electrons. You will also need to show the non-bonding pairs of electrons. Nitrogen will have one pair, while fluorine will have 3. So on the diagram below simply put 6 dots around F and 2 on top of N (as shown). ..

F - N - F

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F

Answer 3

The Lewis dot structure of nitrogen fluoride (NF3) shows nitrogen bonded to three fluorine atoms. Nitrogen has five valence electrons, and fluorine has seven valence electrons. The Lewis structure for NF3 shows a single bond between nitrogen and each fluorine atom, with three lone pairs on nitrogen.

Answer 4

Two dots to the left, two dots on top, one dot on the right