Understand Lewis Dot Structures: Cl F & Triple Bonds

[Shay10825]

What would the Lewis structure look like for Cl F? Would it look like this:
http://img53.exs.cx/my.php?loc=img53&image=dot8pn.png

How do you know when there is a triple bond?

~Thanks

 

[vincentchan]

they shared one electron only...

 

[Shay10825]

How do you know how many electrons they share?

 

[dextercioby]

In the case of halogens,it's the octet (8 electrons in the last shell) rule.

Daniel.

 

[Shay10825]

So since there is one electron left that one bonds? If there were 2 left then those 2 would bond?

 

[Shay10825]

So would H O Cl look like:

http://img60.exs.cx/my.php?loc=img60&image=dot21ni.png

 

[dextercioby]

No,no,remember that in one covalent bond,there must be two electrons,one coming from each atom.On the last shell halogens have 7 electrons and they want to make 8.To do that through one covalent bond,they must share one electron.So they have only one electron AVAILABLE.

Daniel.

PS.For oxygen,sulphur and selenium,the situation is practically the same,just that 1->2 in every sentence because they have 7->6 electrons in the last shell.

 

[dextercioby]

So would H O Cl look like:

http://img60.exs.cx/my.php?loc=img60&image=dot21ni.png

Nope.Let's put one pair of electrons by one "bar",either vertical/horizontal.The hypochlorous acid has the Lewis structure:

$$H-\underline{\overline{O}}-\underline{\overline{Cl}}|$$

Daniel.

 

[vincentchan]

just memorize... in the 7th column of the perioder table, all elements has one electron to shared ... in the 6th column... all elements has two electron to shared...

 

[Shay10825]

So there are all single bonds there. How do you know when there is a double or triple bond? Like for C2 H2 there is a double bond and N2 has a triple bond. How do you know this?

 

[dextercioby]

The octet rule in the case of electronegative elements is essential.
For the nitrogen molecule,the triple bond gives the only viable Lewis structure.As for ethane,the same thing would apply to the Carbon atoms.They must have 8 electrons in their last shell,since they can share only one with one H atom,they must have a double bond.

Daniel.

PS.These things are really much more complicated,but,since it is a K-12 forum,no QM allowed.

 

[Shay10825]

In C2 H2 why can't it look like this?:
http://img143.exs.cx/my.php?loc=img143&image=dot34jd.png

Can electrons stand alone like that (the ones in red) or do they always have to be in pairs?

 

[Shay10825]

PS.These things are really much more complicated,but,since it is a K-12 forum,no QM allowed.

What's QM stand for?

 

[dextercioby]

In C2 H2 why can't it look like this?:
http://img143.exs.cx/my.php?loc=img143&image=dot34jd.png

Can electrons stand alone like that (the ones in red) or do they always have to be in pairs?

It's better if u always try to put them in pairs.Your structure is correctly written
$$H-C\equiv C-H$$

Daniel.

 

[dextercioby]

What's QM stand for?

Quantum Mechanics,a very interesting and difficult discipline of Theoretical Physics.

Daniel.

 

[Shay10825]

Ok I think I understand. So if they can make another bond then they should?

 

[dextercioby]

Ok I think I understand. So if they can make another bond then they should?

What does the last phrase mean??They "should"... Give an example.


Daniel.

 

[Shay10825]

For example:

C2 H2 should not look like this:
http://img38.exs.cx/my.php?loc=img38&image=dot39es.png
because they can form another bond since there are 2 electrons (the ones in red) left over.

 

[dextercioby]

For example:

C2 H2 should not look like this:
http://img38.exs.cx/my.php?loc=img38&image=dot39es.png
because they can form another bond since there are 2 electrons (the ones in red) left over.

Since we're speaking about the acetylene (ethyne) molecule,there are no electrons "left over".They're all hooked up in covalent bonds.2 simple (between C and H) and one triple (between the 2 C elements).

Daniel.

 

[Shay10825]

Since we're speaking about the acetylene (ethyne) molecule,there are no electrons "left over".They're all hooked up in covalent bonds.2 simple (between C and H) and one triple (between the 2 C elements).

Ok i understand.

Thanks

 

[Gokul43201]

Shay, you're missing the trick here :

1) First draw the dot-structure for each atom individually. Make sure you give them all the right number of valence electrons : Cl = 7, F = 7, H = 1, O = 6, C = 4, etc. The total number of valence electrons from all the relevant atoms must be fixed (ie : during bonding, no valence electrons are destroyed or created). Also, if you use different symbols to represent the electrons of the different atoms, it might be easier for you.

2) Bring the atoms together and make them "share" electrons so that, if you include the shared electrons, each atom has 8 valence electrons (except for H, which needs only 2).

Examples :

    + +                * *                     + +      * *
+         +                  *              +        +        *
     Cl                  F         ----->       Cl       F 
+                   *        *              +        *        *
    + +                * *                     + +      * *

7 electrons          7 electrons              octets for each     


                                                   +
                                                   *
  ~        +         *                        ^    +    *
  H     +  C  +   *  C  *     H    ----->   H    C *  C   H
           +         *        ^               +    +    ^
                                                   *
1 elec    4 elec    4 elec  1 elec        duet octet octet duet

After you start feeling comfortable with the method you can use just dots.

 

[Shay10825]

ok I have another question. If it says NO2+ would it look like this:

http://img43.exs.cx/my.php?loc=img43&image=dot40hz.png

 

[dextercioby]

Nope,u've given a link to a page where you had an incorect description for the NO,not $NO_{2}^{+}$.

Think about it again.

Daniel.

 

[Shay10825]

No it's $NO^{2+}$

 

[dextercioby]

Well,then the ion u indicated does not exist.This ion does,however:[itex]NO^{+} [/tex].The ion must have a total of 11 electrons.The oxigen mut complete its octet,which means that the nitrogen cannot.<br /> The only possible Lewis structures for the $NO^{+}$ are<br /> $$\cdot \overline{N}=\overline{O}|$$<br /> <br /> $$|\overline{N}-\overline{\underline{O}}|$$<br /> <br /> The first one seems to be the "orthodox" one,but the second one is correct as well.<br /> <br /> Daniel.[/itex]

 

[Shay10825]

Well,then the ion u indicated does not exist.

The problem says:
Draw Lewis structures for the following polyatomic ions:
$NO^{2+}$ is one of the ones listed

 

[Gokul43201]

Shay, according to your picture, N has a valency of 3 or O has a valency of 4.

Moreover, it's likely $NO_2^+$. I've never heard of $NO^{2+}$, and neither has dexter.

 

[Shay10825]

Shay, according to your picture, N has a valency of 3 and O has a valency of 4.

I'm sorry. Could I add the other 2 electrons anywhere?

 

[dextercioby]

I'm sorry.I've got it.I didn't think of it to be possible,though.

$$\cdot\overline{N}=\overline{O}\cdot$$

Daniel.

PS.The unpaired electrons can be bonded with a halogen.

 

[Gokul43201]

Shay, even if it is $NO^{2+}$, your approach is incorrect. Read my first post with an explanation of how to tackle such problems. Do it one step at a time. You could start by adding the necessary number of electrons to make a neutral molecule, and them take them away in the end.

Dexter, you've drawn $NO^+$