the lewis structure for each of the following species except ____ contains a triple bond?
N3-
O2 2+
N2
NO+
HCCH
I'm not very fast at these things but I think I can draw a triple bond for all but N3^-.
Try them and see what you think.
You can go to google and type in
lewis structures and the substance and find most of them I think.
To determine the Lewis structure of each species and identify the one that does not contain a triple bond, we need to understand Lewis structures and the rules for drawing them.
Lewis structures represent the valence electron arrangement for atoms in a molecule using dots and lines. The number of dots around an atom represents its valence electrons, and the lines represent bonds between atoms.
Let's go through each species and draw their Lewis structures:
1. N3-
To determine the number of valence electrons for N3-, we add the valence electrons of nitrogen (5) with the charge of -1, giving us a total of 16 electrons (5 x 3 + 1). Since it has a negative charge, this means it gained an electron.
To draw the Lewis structure for N3-, we place the three nitrogen atoms in a row, each connected by a single bond. We then add three lone pairs (dots) on each nitrogen atom, totaling 16 electrons. There are no triple bonds in this structure.
N≡N - N
2. O2 2+
Oxygen (O) normally has 6 valence electrons. With a 2+ charge, it means it lost two electrons. Since we have two oxygen atoms, the total number of valence electrons is 10 (6 - 2) x 2.
To draw the Lewis structure for O2 2+, we place the two oxygen atoms in a row, connected by a double bond (two lines). We add three lone pairs (dots) around each oxygen atom, totaling 10 electrons. There is no triple bond in this structure.
O = O
3. N2
Nitrogen (N) has 5 valence electrons. To draw the Lewis structure for N2, we connect the two nitrogen atoms with a triple bond, represented by three lines. We add three lone pairs (dots) around each nitrogen atom, totaling 10 electrons. This structure has a triple bond.
N ≡ N
4. NO+
To determine the number of valence electrons for NO+, we add the valence electrons of nitrogen (5) and oxygen (6) with the charge of +1, giving us a total of 12 electrons (5 + 6 + 1). Since it has a positive charge, this means it lost an electron.
To draw the Lewis structure for NO+, we place the nitrogen atom in the center and connect it with an oxygen atom using a double bond (two lines). We add two lone pairs (dots) on the oxygen atom and one lone pair on the nitrogen atom, totaling 12 electrons. There is no triple bond in this structure.
N≡O+
5. HCCH
To draw the Lewis structure for HCCH (acetylene), we need to consider the valence electrons of hydrogen (1) and carbon (4). Hydrogen has 1 valence electron, and carbon has 4 valence electrons.
We connect the two carbon atoms with a triple bond (three lines) and add two hydrogen atoms, each connecting to a different carbon atom with single bonds (one line each). We add three lone pairs (dots) around each carbon atom and one lone pair on each hydrogen atom. This structure has a triple bond.
H-C≡C-H
Based on our analysis, the Lewis structure that does not contain a triple bond is NO+.