Is Ch3oh An Ionic Compound

If we await at the electron dot structure of CH3 + OH^-
How does OH negative class a bond with CH3 if all electrons of OH are already paired upwardly?

the oxygen has some alone pairs of electrons (an oxygen atom has 6 outer shell electrons; the oxygen in OH^- has 8 outer vanquish electrons: one has been gained (hence the ion), and the covalent bail betwixt the oxygen and the hydrogen contains one of oxygen's electrons and hydrogen's electron, the oxygen has 4 non-bonding electrons, which exist as "lone pairs")
one of these alone pairs (call up electrons are negatively charged) is attracted to the positively charged carbon
(a carbon cantlet commonly has 4 outer shell electrons; in CH3^+ one of these electrons has been lost, and the remaining three are each in a covalent bond with a hydrogen)

recollect a covalent bond is a shared pair of electrons. atoms in simple molecules are held together by covalent bonds. in a simple molecule in that location is a set number of each atom (you know how many carbons, oxygens, hydrogens (or whatever) in that location are in one molecule). this is true for methanol

ionic bonding is the electrostatic force of attraction between oppositely charged ions. an ionic compound contains many oppositely charged ions (NaCl, for example, contains many Na+ ions and many Cl- ions, not just 1 of each), bundled in a giant lattice (i.east. non methanol)

Spoiler:

Show

helps to draw it out

the sticks ( – ) between atoms represent a covalent bail (shared pair of electrons)
the scarlet arrow shows the movement of electrons

apologies if this is merely more than disruptive, there's probably a better way to explicate it!

non certain what level you are studying, merely chemguide ordinarily has some expert explanations. it mainly has a-level content but at that place is also a section covering GCSE chemical science content. would recommend

Thank you! This really cleared up my confusion.
Just to confirm, CH3 that is the methyl molecule has in total 6 electrons, 3 of carbon and the other 3 from each of the hydrogens, right?

Last edited by AuntyEdna; xi months ago

-CH3 = methyl
by itself it's not really a molecule; it tends to exist part of a molecule, frequently as a methyl group
think of information technology every bit a methyl hydride molecule (CH4) that has lost the hydrogen. something else is usually bonded (or about to be bonded) to the carbon in place of this hydrogen
in this case information technology is a methyl cation (a cation is a positive ion). in the carbon's outer beat out at that place are 3 pairs (half dozen total electrons) of shared electrons, each pair is shared with a hydrogen. each shared pair effectively consists of one electron from the hydrogen and one electron from the carbon
atoms are generally virtually stable when they have a full outer vanquish. the carbon therefore needs two more electrons to consummate its outer trounce, which are coming from one of the alone pairs on the oxygen, again a shared pair of electrons (covalent bail) so that both the carbon and the oxygen tin can have a full outer shell

chemguide has a squeamish representation of CH4 at the top of this page:
https://www.chemguide.co.uk/14to16/o.../formulae.html

and the page that comes after it talks nearly names of organic compounds, might be helpful?
https://www.chemguide.co.uk/14to16/organic/names.html

(Original mail by bl0bf1sh)
-CH3 = methyl
past itself information technology'due south not really a molecule; it tends to be part of a molecule, ofttimes as a methyl group
think of it every bit a methane molecule (CH4) that has lost the hydrogen. something else is usually bonded (or about to be bonded) to the carbon in identify of this hydrogen
in this case it is a methyl cation (a cation is a positive ion). in the carbon's outer shell in that location are 3 pairs (6 total electrons) of shared electrons, each pair is shared with a hydrogen. each shared pair finer consists of ane electron from the hydrogen and one electron from the carbon
atoms are generally most stable when they have a total outer shell. the carbon therefore needs 2 more electrons to complete its outer crush, which are coming from 1 of the lone pairs on the oxygen, once again a shared pair of electrons (covalent bond) and so that both the carbon and the oxygen can have a full outer shell

chemguide has a squeamish representation of CH4 at the top of this folio:
https://www.chemguide.co.united kingdom/14to16/o.../formulae.html

and the page that comes later information technology talks nigh names of organic compounds, might be helpful?
https://www.chemguide.co.united kingdom/14to16/organic/names.html

Thank you very much!
This was very helpful

Is Ch3oh An Ionic Compound,

Source: https://www.thestudentroom.co.uk/showthread.php?t=7118834

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