How to draw a dot and cross diagram of carbon MONOXIDE?

Question

The only diagrams i can find are of carbon DIOXIDE i want MONOXIDE ahhh :(
Please dont tell me how to draw one of CO2 i can do that :(

Answer 1

There is a triple bond and C and O each have one lone pair.



But, here is an update. When drawing Lewis structures we don't use dots and crosses. That is an antiquated approach. The reason is that in a compound, all of the electrons belong to the entire molecule, not to individual atoms. This is the influence that molecular orbital theory has had on Lewis structures: no crosses, only dots (and dashes for bonding pairs.)



Take a look: http://3.bp.blogspot.com/_Jpm5bX4HPaw/TOA2WZzXnjI/AAAAAAAAAes/gHD9_zcZNrY/s400/Lewis-structures-of-carbon-monoxide-and-hydrogen-cyanide.jpg



======= Follow up ========



It's not really a question of one atom or another "giving" electrons. When drawing a Lewis structure we add up all of the valence electrons and then distributing them within the Lewis structure according to a series of guidelines.



1. Compute total of valence electrons

2. Decide on which element is the central atom

3. Construct the skeleton structure of the molecule and connect each terminal atom to the central atom by a single bond (a pair of electrons) represented by a dashed line

4. Complete the octet of the terminal atoms

5. If there are not enough electrons to give an octet to the central atom, then consider using a double or triple bond.

6. If there are "left-over" electrons, place them on the central atom, even if it means having more than 8.

7. Use formal charges to pick the best from among several possible Lewis structures

Answer 2

Sorry, but can't really draw dot-and-cross diagrams on here. I suspect the best way to go about it is to say that there are a number of resonance structures (canonical forms). The (only?) one that gives eight electrons on both the carbon and the oxygen is to have three bonds between the atoms, one of which is a dative bond with the oxygen providing both the electrons (but why would the more electronegative element do this??) --------------------------------------... Whilst entirely agreeing with "pisgahchemist" that all the electrons in a molecule belong to the molecule as a whole, and can no longer be allotted to any particular atom, it is very difficult to see how covalent bonding can be taught to 14-16 year olds without the use of something based on the dot-and-cross diagram, and I'm sure new text-books at this level (and A-Level as well) in the UK will continue to use them. I have certainly introduced MO Theory and other theories to A-Level students, but the dot-and-cross diagram still has quite a life left at this level at least ... even if only for the dreadfully pragmatic reason that that is what GCSE and A-Level examiners will expect from them. ========even more follow-up===================== Agree again with pisgahchemist's philosophy and have, as far as possible, always avoided teaching ideas that need 'unteaching' later. However, as I said above, UK public examinations and examiners up to 16 (GCSE) and 18 (A-Level) will expect dots and crosses, and still use the term 'dative bond'. Not helpful, I admit, and a sign that much 'education' in the UK is exam-driven ... but there we are! Hope we haven't confused you even more, Ammar A ?!

Answer 3

Carbon Dioxide Dot And Cross

Answer 4

Proper care need to be taken when drawing the 'dot and cross' diagram of carbon monoxide, CO. Care need to be taken to demonstrate knowledge that carbon monoxide contain co-ordinate bonding, known as dative covalent bonding.



In covalent bonding, the two atoms (which can be of same or different elements) that are sharing the electrons contribute the same number of electrons. For example, in methane, the hydrogen atom and carbon atom 'contribute' one atom each, forming a single bond. However, this is not the case for co-ordinate bonding. The only similarity is that both covalent bond and co-ordinate bond involve the sharing of electrons.



This is applies to other compounds like boron trifluoride and aluminium chloride. These compounds, although they contain a metal and a non-metal, they are not ionic compounds, but compounds containing co-ordinate (or dative covalent) bond.



For readers from Singapore (perhaps in other countries too), please take note that this is only in the GCE 'A' Level Syllabus. This is not in the GCE 'O' Level Syllabus.

Answer 5

This Site Might Help You.



RE:

How to draw a dot and cross diagram of carbon MONOXIDE?

The only diagrams i can find are of carbon DIOXIDE i want MONOXIDE ahhh :(

Please dont tell me how to draw one of CO2 i can do that :(

Answer 6

Draw the carbon and oxygen atom sharing two pairs of electrons each. This is a double bond. But then add another pair from the oxygen atom to the bonding electrons. This is a dative covalent bond as both electrons come from one atom. There should now be a triple bond between the atoms and the oxygen and carbon atom should have a lone pair each not involved in bonds

Answer 7

Check out http://en.wikipedia.org/wiki/File:Carbon_Monoxide-2.svg

and the commentary at http://en.wikipedia.org/wiki/Carbon_monoxide



You can get the triple bond by typing ≡

(the & initates a code and the ; terminates it.)



That and other HTML codes for Greek characters and arrows can be found at

http://htmlhelp.com/reference/html40/entities/symbols.html

Answer 8

:C(Triple bond-there's really no way to draw one here)O:



I disagree:



:C:::O:



:C≡O:



≡ is a math symbol meaning "exactly equal to"

Answer 9

You deleted your question in the middle of my answering it? Ha ha.

Anyway, do you mean the structural formula?

That would be as follows



:C(Triple bond-there's really no way to draw one here)O: