How many bonds can oxygen hold with other atoms?

Question

need real answers please help

Answer 1

Depends.

I'm going to assume straight off you mean covalent interactions. How are you defining "bonds"? Is it the number of orbital overlaps, or the number of lines you draw in the Lewis structure, so that multiple bonds count multiple times? Or is it just the number of atoms you're connected to?

In sodium hydroxide, the [OH]– ion has one OH covalent bond.
In water, the H2O molecule has two O-H covalent bonds, one single bond to each H.
In the hydronium ion, the [H3O]+ ion has three O-H covalent bonds, one single bond to each H.

If you don't like H, we can make versions of those with O-C bonds instead: ethoxide, diethyl ether, triethyloxonium.

In dioxygen, the OO double bond means two covalent bonds (number of lines in the Lewis structure), but connected to one atom, so it's one bonding interaction. In [O2]+, the bond oder is 2.5. In [O2]–, it's 1.5. In [O2]2– , it's just 1.

In nitrosonium [NO]+, or carbon monoxide CO, it's three bonds.
In nitric oxide, [NO], it's 2.5 covalent bonds.
In [NO]–, it's two covalent bonds. In each case O is connected to just one other atom.

In [NO3]–, there's an effective N-O bond order of 1 and 1/3.
In ozone, O3, each individual O-O bond order is 1.5, so the central O has a total of three bonds and is connected to two other atoms. In [NO2], the N-O bond order is 1.75.

In a metal aquo complex like [Ni(OH2)6]2+, each O is connected to three atoms, usually described as single bonds. In a terminal metal oxo compound, there's an M-O double or triple bond, depending on the compound and who you're talking to. Sometimes those are anionic, with a metal cation like Li+ or Na+ sitting on the other end of the O, so that could be four bonds. In a bridging metal oxo, M-O-M, there are certainly cases where it could be argued that you have two bonding interactions to *each* metal (i.e. M=O=M, in effect), so that's also a total of four bonds at one O atom. There are side-on bridging peroxo compounds, where the [OO]2- group sits sideways between two metals, so that each O is connected to the three other atoms.

So a glib "one double or two single" is a ridiculous and wholly misleading oversimplification. Without even getting away from binary compounds and ions of H, C, N, and O, O can be found forming bond orders of 1, 1.33, 1.5, 1.75, 2, 2.5, and 3, to either one, two, or three other atoms. If you go to metal compounds, you can push the number of bonds to 4.

Answer 2

Two covalent bonds - either two singles or one double. (The latter: Consider acetone or formaldehyde.)

SEVERAL MORE bonds of a "water of hydration" type. Depends on the pH of the solution and whether any metal oxides are present. The "hydration" bond is looser than a formal chemical bond but strong enough to hang around for a while. Most I've seen is three such bonds but one non-chemical bond is most commonl.

Answer 3

Oxygen can have two single bonds, as with water--2 single hydrogens attached to the one oxygen.
Or oxygen can have one double bond, like diatomic O2, where it is bound to itself.

Answer 4

it can hold up to 2 single bond or 1 double bond to achieve stability which is eight valence electron

Answer 5

it can hold 2 single bonds, or 1 double bond.

Answer 6

covalent bond

Answer 7

this is not real research.