CHEMISTRY COMMUNITY

Ella Bouris

Here's an answer of an answer from another post that might help. "Re: particular d-block metals form amphoteric oxides? Postby Chem_Mod » Sun Aug 21, 2011 10:46 am We covered metal oxides and hydroxides (e.g., NaOH) which are basic compounds. We also covered non-metal oxides (e.g., H2SO4, H3PO4...

Ella Bouris

For notating the composition of a bond, such as C2sp2, why do you put the 2 before the orbital hybridization?

Ella Bouris

Are the review sessions tonight still happening or are those cancelled as well?

Ella Bouris

I heard no new lecture was given in the 11am lecture since all classes after noon were cancelled

Ella Bouris

What does the final grading scale break down to in this class? On the syllabus it says that a passing grade is a C- which is a 50% and I was wondering if that still holds or if theres been a change to it

Ella Bouris

To determine if they are acidic, basic, or amphoteric, do you have to draw Lewis structures or is there another way to do it? For example, in the solutions manual it says that BaO is basic, but how do you tell?

Ella Bouris

For 12.51 a, the explanation in the solutions manual is confusing me. I know just by memorization that HCl is a strong acid and HF is not, but why would HF not be stronger if F is more electronegative than Cl (using the logic from part c,d, and f)?

Ella Bouris

There shouldn't be a difference I think- it's more the context of the problem. If you define something using the Bronsted definition, that carries through the entire problem so a Bronsted acid would have a Bronsted base, and same with a Lewis acid.

Ella Bouris

Would Mg or Na have a smaller second ionization energy? I know Na has a smaller first ionization energy but does that same trend carry on with second ionization energies?

Ella Bouris

Do the electron configurations for the d block transition metals all have a 4s1 subshell? Or just the two exceptions Cu and Cr?

Ella Bouris

At our UA session yesterday they said either was fine, the most important things was consistency in your answers, so if you use the new naming conventions, use them for everything, and same with the old ones.

Ella Bouris

I've been looking it up and my understanding is that for something to be polydentate, there has to be multiple molecules each with a lone e- pair available for bonding. So for something to be bidentate, it doesn't just have to have two lone pairs but one lone pair each on two atoms to make them avai...

Ella Bouris

Not quite sure specifically what Lavelle would want, but to be safe I'd go with the two notations in the book- C2O4 or O2CCO2. If you're talking about naming with the full versus abbreviated name, it looks to be interchangeable in the same way that EN is with ethylenediamine.

Ella Bouris

I'm having trouble just understanding how to determine if a molecule is mono, bi, etc dentate. Do I need to draw a Lewis structure?

CHEMISTRY COMMUNITY

Search found 14 matches

Re: D-Blocks

Bond Notation

Review Session Cancellation? [ENDORSED]

Re: 1pm lecture cancelled? [ENDORSED]

Grading Scale [ENDORSED]

12.17

HF

Re: Different from Bronsted and Conjugate

Second Ionization Energy

Electron configurations of d block elements

Re: 17.29 a and c

Re: Help understanding polydentate

Re: Oxalate

Help understanding polydentate