@M.A.R. Sure. I'll convert my comment to an answer later then.
Please take a look at the homework policy to see how you can improve your post. Essentially, you need to explain what specific issue you are facing, or show what you have tried to obtain the answer. meta.chemistry.stackexchange.com/questions/141/… — Zhe6 hours ago
@Zhe is that copy pasted from one of my comments? ;)
Nothing wrong with that. Just wanted to give you a heads up that the homework policy is likely to be modified in the near future and until then all my comments will be customly written.
I'm just not 100% sure how to summarise our current stance in one "stock comment". I don't really want to say "homework copy-pastes are not allowed" because that feels a bit unfriendly
Oh, I just realized how the dramatic the message you quotes is. Sheds some tears And regarding the first one, it was a 'generic' Klaus, meaning Klaus, you, and a bunch of people I missed. Anyway thanks for voicing your opinion. — M.A.R.6 hours ago
Shit. Autocarrot randomly inserted a bunch of words into my first sentence. It looks HORRIBLE
Barbituric acid or malonylurea or 6-hydroxyuracil is an organic compound based on a pyrimidine heterocyclic skeleton. It is an odorless powder soluble in water. Barbituric acid is the parent compound of barbiturate drugs, although barbituric acid itself is not pharmacologically active.
It remains unclear why the German chemist Adolf Baeyer chose to name the compound that he discovered "barbituric acid". In his textbook Organic Chemistry, the American organic chemist Louis Frederick Fieser (1899–1977) initially speculated that the name stemmed from the German word Schlüsselbart (literally, the beard...
Welcome to The Periodic Table ramanujan! Here are our chat guidelines and it's recommended that you read them. If you want to turn Mathjax on, follow the instructions in this answer. Happy chatting!
Welcome to The Periodic Table ramanujan! Here are our chat guidelines and it's recommended that you read them. If you want to turn Mathjax on, follow the instructions in this answer. Happy chatting!
Anyone happens to know what the C-Cl bond moment in CCl4 is? Can't seem to find it anywhere :/ [Although I did find out that the C-Cl bond moment in CH3-Cl is: 1.86 Debyes, I have a feeling it won't be the same for CCl4 ]
I wonder who this U. Grant is we’re supposted to be helping and whether that person is related to Mr Research Grant. Pls tel lme kthxbai. — Jan2 mins ago
@orthocresol I have Cl and Ar, and I need to say which one has more electron affinity giving quantitative arguments. It's clear to me that Cl is more into electron-sex than Ar, after all Ar is in a serial relationship with it's 2s2 and 2p6 orbitals
But how to quantitatively argument on that I'm not sure, my prof doesn't enjoy my human behaviour analogies I believe
Why in the MOT diagram of NO, once you fully populate the bonding sigma and pi orbitals of 2p the remaining electron goes to the antibonding pi and not the antibonding sigma?
Also, does my MOT diagram look okay? I know the anti-bonding sigma for 2s should've been visibly higher than the bonding one is lower (weird to say this) but I ran out of space :v
To obtain the electronic configuration of NO from NO+ diagram you need to add an electron in an antibonding orbital. Then the strengh of the bond will be reduce and the it will increase the size. So NO+ has a smaller bond than NO.
@BernardMeurer Yeah, exactly. Although to be honest, you don't even need to count antibonding or bonding electrons.
Yeah, precisely what @9-BBN said.
Or you think of it the other way round: to produce NO+ from NO, you remove one electron from an antibonding orbital. This strengthens the bond which makes it shorter.
"Using the periodic table, calculate the dipole momentum in Debye of the simple bond N-O, indicate in which atoms are the partial positive and negative charges"
@BernardMeurer I don't know of any such formula, to be honest. If you want an actual dipole moment the only way I know of to calculate it is the physics way: $\vec{\mu} = \sum q\vec{d}$
You cannot make a negative difference of electronegativity it doesn't make sense and you cannot make one more than the most electronegative - the less one with will be less than 3.98
"Determine the wavelength of the photoelectrons removed from a rhodium anion (Rh-) with a radiation of 488nm, knowing that the electroaffinity of Rh is 110,27 kJ/mol"
So, this one I can kind of make sense of
So for Rh to get an electron it must be charged with 110.27Kj/mol of energy, right?
So for Rh- to lose that electron it would need the same energy
It's the last step that I don't see how to do, do I need de-broglie?
That's very odd, normally questions ask about the kinetic energy of the photoelectron. To convert the energy to a wavelength, yes, you need the de Broglie relation.