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Author Topic: Lewis Structures  (Read 6065 times)

Offline Les the Scientist

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Lewis Structures
« on: 02/02/2006 16:39:21 »
Could someone clarify this for me.

The negative ion [IF3Cl]-

Am I right in thinking that this would have 2 lone pairs and a single bond between each F & Cl atom ?  Wouldn't this give it 12 outer electrons though ?  I assume this doesn't follow the 'octet' rule yeah ?

Cheers





 

Offline rosy

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Re: Lewis Structures
« Reply #1 on: 02/02/2006 18:52:50 »
Iodine will form single bonds to the F and the Cl's, so 4 sigma bonds... and has another 4 electrons (including the extra one for the negative charge), giving two lone pairs.
Which I think is what you meant?
Yes, it ignores the octet "rule"... iodine has d orbitals to keep extra electrons in.
 

Offline Les the Scientist

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Re: Lewis Structures
« Reply #2 on: 03/02/2006 02:20:32 »
Ah, marvellous.  Yeah, that was what I meant. :o)
 

Offline Les the Scientist

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Re: Lewis Structures
« Reply #3 on: 05/02/2006 18:19:29 »
Because of these lone pairs, which will repel each other the most, I assume the structure will be square planar ?  With the lone pairs at each end of what would be an octahedron yeah ?
 

Offline rosy

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Re: Lewis Structures
« Reply #4 on: 06/02/2006 19:32:15 »
I think so.
 

Offline mac2005

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Re: Lewis Structures
« Reply #5 on: 13/02/2006 20:41:01 »
hey there im new to chemistry and just trying to figure out the structure of [IF3Cl]- and its driving me nuts any ideas?
 

Offline rosy

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Re: Lewis Structures
« Reply #6 on: 13/02/2006 23:29:33 »
Read the posts above!!
 

Offline mac2005

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Re: Lewis Structures
« Reply #7 on: 14/02/2006 11:22:39 »
thanks nearly there now
quote:
Originally posted by rosy

Read the posts above!!

 

Offline yvonne rutter

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Re: Lewis Structures
« Reply #8 on: 10/03/2006 21:14:25 »
Yet another open uni cheater! Please have the good grace to do the work by yourself like me. (And the only reason I'm looking is because I wanted to see if my assumptions were correct).
 

Offline Ophiolite

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Re: Lewis Structures
« Reply #9 on: 11/03/2006 11:39:10 »
To steal from one person is plagiarism.
To steal from many people is research.
To steal from no one is madness.
"Great wits to madness are near allied, when thin partitions do their bonds divide."  


Observe; collate; conjecture; analyse; hypothesise; test; validate; theorise. Repeat until complete.
 

Offline Les the Scientist

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Re: Lewis Structures
« Reply #10 on: 13/03/2006 01:50:19 »
I don't honestly see any problem with asking people for advice on here.  I had already outlined my reasoning and what I thought to be the answer.  If someone else has the foresight to sign up to this forum and join the discussion then good for them.  Not asking for help is like trying to pass your driving test without having lessons first.... very foolish.

See you at the residential school in the summer !
 

Offline Ophiolite

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Re: Lewis Structures
« Reply #11 on: 20/03/2006 12:47:08 »
Les, I agree with you. Had you asked people to declare and explain the electron structure of the ion then yvonne rutter's objection would have been valid. You did not. You gave your understanding and asked for confirmation. That is good sense.
I would be interested to hear how yvonne distinguishes between your approach, where you state what you believe and ask for confirmation, and her approach, where she pieces the solution together by reading text books, course notes and thoughts. To an impartial observer there is no apparent difference.


Observe; collate; conjecture; analyse; hypothesise; test; validate; theorise. Repeat until complete.
 

The Naked Scientists Forum

Re: Lewis Structures
« Reply #11 on: 20/03/2006 12:47:08 »

 

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