CHEMISTRY COMMUNITY

Ramsha Dis1B

When a ligand is bound in two places it forms a ring-like structure.

Ramsha Dis1B

In one of the review sessions they said that typically if the two lone pairs, one from one atom of the same compound and another from the other, are about 90 degrees from each other than it's able to be bidentate. Because most coordination compounds turn out to be octahedral, they have 90 degree bon...

Ramsha Dis1B

Yeah, you would write bis- because there is already a di- in the ligand itself, just like Sydney said. My TA also extended on the reason we have to do that. Writing bis- allows you to know that there is two ethylenediamines rather than two ethylens with two amines because that is not the case since ...

Ramsha Dis1B

Also, the way I think about it is that the metal's oxidation number must cancel out with what it's bonded to. And when that's bonded to more molecules it all has to equal to the charge that's given usually on the outside of the brackets. You usually know (or they are given) the charge for the other ...

Ramsha Dis1B

Also, I read somewhere that if a coordination compound contains at least one non-monodentate ligand, its considered a chelates. So I guess in a way its any coordination compound with a ligand, I think. And it also says that chelates are typically organic and an example of a chelate is the porphyrin ...

Ramsha Dis1B

Because of the negative 2 charge two of the Oxygen atoms have an extra lone pair of electrons so only those atoms want to bind to another atom. When one bonds it will be monodentate and when both Oxygen atoms bond to a different atom it will be bidentate.

Ramsha Dis1B

I think it might be in the "electron cloud," or the valence shells of both the atoms that are bonded together.

Ramsha Dis1B

So how would you actually form a molecular orbital? Like with what orbital, the atomic or hybrid of an atom with another? Can you please give an example of a molecular orbital, I don't understand how that would look like, or come to be?

Ramsha Dis1B

Also, to add on in terms of when you look at the atomic orbital, Boron for example has 2s full and 2p with only one electron. So, when you separate the electrons individually to make the hybrid when wanting to make a bond with three other atoms there are three spots to bond. The hybridization will b...

Ramsha Dis1B

You are able to also tell what the hybridization is based on how many regions of electron density there are so you can look at it that way, if Al or B have two regions of electron density the hybridization will be sp and if they have three then it will be sp^2. I think that how high it will go for t...

Ramsha Dis1B

You can think of it like the atom with a slightly negative has an arrow close by it that starts from the atom with the slightly positive charge which has a positive sign close by it. The line on that side looks like a positive sign.

Ramsha Dis1B

Does polarizing power only apply to cations? Can anions also have polarizing power and if they can, what would be the pattern? For cations its typically the smallest has more polarizing power, but how about for anions?

Ramsha Dis1B

Does polarizability only refer to Anions? Will there ever be a question that asks for the polarizability for a cation?

Ramsha Dis1B

Is an induced-dipole interaction equivalent in strength as a dipole-dipole interaction? I think it is because technically it's still a dipole-dipole interaction but would it be a little weaker since it's induced?

Ramsha Dis1B

I don't completely understand the fluctuating concept. I know that in order to attract each other one side of the atom becomes slightly negative by the electrons and another atom becomes slightly positive, but why is it called fluctuation? Do electrons keep moving around making the bonded side of th...

Ramsha Dis1B

When we draw the lewis structure for molecules that have 4 or more atoms do we have to show the 3D shape by putting a small triangle and the lines to show that one atom is behind or in front of the central atom?

Ramsha Dis1B

You can use the atomic radius to determine how strong the bonds will be between two atoms that bond together. If there is a bigger radius between two atoms that are bonded together and you compare the strength of the bond to another two bonded together, you can tell which will be stronger, and stay ...

Ramsha Dis1B

I agree with Albert, since it becomes a hybrid, the bond lengths would all average out and so maybe that's why they are all the same.

Ramsha Dis1B

If I understand your question correctly, I think that we can not be sure of the exact position of the electrons because of the resonance structures. the "blended characteristic" that your referring to is just the resonance hybrid.

Ramsha Dis1B

The problem is: The meter was defined in 1963 as 1650763.73 wavelengths of radiation emitted by krypton-86. What is the wavelength of this krypton-86 radiation?To what region of the electromagnetic spectrum does this wavelength correspond? what energy does one photon of this radiation have? I did no...

Ramsha Dis1B

Once you find the energy, you set that equal to -hR/4^2 - (-hR/n^2), which can be written as -hR(1/16 - 1/n^2). Next you divide -hR on both sides and then subtract 1/16. After, divide by the negative and flip the whole equation so it is 1 over whatever is on the other side and just n^2 on the right ...

Ramsha Dis1B

Oh okay, so if is asking the degeneracy for 3s it would be 3 too? And if it was asking for 4p it would be 4?

Ramsha Dis1B

I don't understand what degeneracy means and how we determine the degeneracy of a certain orbital, like 3p. How would you determine that?

Ramsha Dis1B

What's an easier way to understand the difference between the Aufbau Principle and Hund's Rule? Can someone please explain them too?

Ramsha Dis1B

How do you describe the interpretation of atomic orbitals in terms of probability?

Ramsha Dis1B

What are the factors affecting the energy of an electron in a many-electron atom?

Ramsha Dis1B

What does the uncertainty principle actually calculate?

Ramsha Dis1B

What does it mean when they say that the energies on the right of an expression have to be proportional to hR/n2, to have accounted for Rydberg’s formula?

Ramsha Dis1B

HI, can someone explain the Bohr frequency condition to me please. I don't fully understand how the textbook explains it?

Ramsha Dis1B

The empirical formula represents the relative number of atoms.

Ramsha Dis1B

The element which occurs the least is the one that you balance first.

Ramsha Dis1B

I believe that first you can write the soluble ionic compounds as dissociated ions to get the complete ionic equation but you still have leave out the spectator ions (the ones that stay the same in the reactant and product side) from the equation since they do not change.

CHEMISTRY COMMUNITY

Search found 32 matches

Re: How to tell if something is a chelate

Re: CO3^2-

Re: Naming with bis-

Re: Oxidation number

Re: Chelate

Re: Polydentate Ligands for resonance structures

Re: Pi Bond

Re: Hybrid vs. Molecular Orbitals

Re: Deficient Octets

Re: Deficient Octets

Re: How do you draw dipole moments

polarizing power

Polarizability

induced-dipole

Fluctuation

Molecular shape and structure

Re: What are the trends useful for?

Re: Double Bonds and Single Bonds in Resonance Structures

Re: Electron movements

#28 Atomic Spectroscopy Post-Assessment for module

Re: Post Module Assessment #42

Re: Degeneracy

Degeneracy

Aufbau Principle and Hund's Rule

atomic orbitals

electrons

Uncertainty Principle

H-Atom

Bohr frequency condition

Re: Definition of Empirical Formula

Re: Order of balancing an equation

Re: Fundamental M.9 [ENDORSED]