Hi everyone!
Just a quick question:
why is core charge always positive?

Thank you!

    PizzaMaster

    Since core charge is given by number of protons in nucleus - number of non-valence e-s, and the number of non-valence e-s is always less than the number of protons in nucleus, core charge will always be positive

      Can someone help me with this chemistry question?

      There are a number of structural isomers for the molecular formula C4H10O. (Mass Spec Graph) Identify the fragment at 29 m/z.

      The two possible answers are [C2H5]+ or [COH]+

      My question is.... shouldn't the [COH] have a charge of +2? The molecule has lost two hydrogens...? not just 1 like in C2H5.....

      Or does one electron drift off with the hydrogen, and the other one just happen to stay with the molecule?

      Thanks!
      -G

        God For the purposes of VCE chem, you should assume that all fragments have a +1 charge.

        "Or does one electron drift off with the hydrogen, and the other one just happen to stay with the molecule?"

        This is called a radical, since they're uncharged, they won't be detected by the mass spec machine since it can only "see" charged fragments

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            Struggling a bit with states for organic reaction pathways, always messing up gaseous and liquid states. Any tips?

              robinsonada

              H2SO4 should be (l) when it's catalysing an esterification because it's concentrated

              Oxidising reagents are written as H+(aq)/Cr2O72- (aq) or H+(aq)/MnO4- (aq)

              H2O will be (g) in alkene hydration since it's conducted at 300˚C

              All reactants for esterification are (l) and not (aq) since water can hydrolyse the ester product back into the reactants

                Hi everyone,
                just quickly,
                does a high melting point also mean that an element will have a high boiling point too?
                thank you!

                  PizzaMaster
                  Most of the time - i'd say yes. High melting point means high intermolecular forces - which shouldn't disappear when it becomes a liquid. (Although, knowing chemistry...... )

                    Can someone help with finding the splitting patterns in butanal?

                    My question is.... for the hydrogen bonded to the C=O group, should it be a triplet or a singlet?

                    If a triplet, shouldn't that mean the CH2 group (also bonded to the C=O) should be a quartet?

                    Thanks! 🙂

                      God
                      The carbonyl hydrogen should be a triplet. The H environment on the alpha carbon has complex splitting so I don’t think VCAA will ask you that (it will be a quartet by the n+1 rule, but the reality is that the aldehyde H and the CH2 are in very different chemical environments that split the alpha carbon’s H environment by different amounts, so the observed pattern has a lot of overlapping peaks and isn’t a quartet. You’d call this a multiplet)

                        Im currently doing U2 Aos1 but i don't get ions and charges at all

                          When you are oxidising a primary alcohol, how do you prevent the reaction from going all the way to a carboxylic acid? It will first make an aldehyde, but how do I prevent the aldehyde from becoming oxidised?

                          Alcohol ---> Aldehyde ----> Carboxylic acid MnO4-(aq) / H+(aq)

                            Will
                            In uni chem you learn that you wouldn't use acidified dichromate (Jones reagent) or acidified permanganate if you want an aldehyde final product because they're strong oxidising agents that will oxidise any aldehyde formed into a carboxylic acid. You'd use Swern's reagent or Ley's reagent (TPAP) if you want to oxidise a 1˚ alcohol to an aldehyde because they're weaker oxidants that don't over-oxidise the alcohol to a carboxylic acid

                              Will

                              To reduce carboxylic acid production when oxidising alcohols:

                              • Limit the heat
                              • Limit the oxidising agent
                              • Remove the aldehydes as it is produced.

                                  God
                                  I know it's what your teacher may have taught you (I was taught that mild oxidation under 60˚C produces aldehydes in high school too), but this one of those really shameless lies taught in VCE chem. Acidified permanganate or dichromate is aqueous, and in aqueous solutions, aldehydes react with H2O to form geminal diols (an alcohol that has 2 hydroxyl groups attached to the same carbon). Hence you can't actually make a pure sample of aldehyde with the oxidising reagents you learned about in VCE, only its geminal diol (hydrate) form which has very different chemical properties from aldehydes

                                    I have trouble understanding hydrogen/carbon groups environments.
                                    I can identifying them, I just seem to get tripped up on whether different hydrogens are part of the same group.
                                    My common mistake is believing that two carbon environments are part of the same environment, when they are in reality different.

                                    For carbon/hydrogen sections to be a part of the same environment does the molecule HAVE to be symmetrical?

                                      Will

                                      If there is a H-environment identical to another in the molecule, then yes it's symmetrical. One hack I learned in uni for identifying whether or not 2 given environments are chemically equivalent is to pretend to cut off the C atom the H-environment is attached to from the rest of the molecule. You repeat it for the other environment (with a separate structure) and then you compare if the rest of the molecule is identical in both cases. If it is, then these 2 environments are equivalent (will post a visual example)

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