CHEMISTRY COMMUNITY

Schem_student

So you use bis-, tris-, and tetrakis- if there are multiple of the same ligand ?
This is an example.
[Co(H2NCH2CH2NH2)3]2(SO4)3
Answer:
tris(ethylenediamine)cobalt(III) sulfate

Schem_student

What is the difference between writing H20 for aqua from the name or or OH2?

Schem_student

Also be aware that AXE is a specific VSEPR Group that will help you determine MG or molecular geometry.

Schem_student

Because of resonance we never really can predict the exact location of the double bond between the atoms so we define the bond length as an average between the single and double bonds

Schem_student

I got confused by this one too! Just think about hybridization labels of central atoms in terms of amount of atoms bonded not if they are double or single bonds. Therefore there are only 3 atoms bonded around C so it would be sp2.

Schem_student

The question asks if you expect the bond angle to increase or decrease as the s-character of the hybrids increase in example sp3 or sp2? I am confused conceptually on how the s-character would grow in size and how they are directly proportional.

Schem_student

When asked to draw the best lewis structure for C3H4 you would want the structure with the most formal charges of atoms= 0 which will help you determine where the double bonds should go.

Schem_student

AX2 is the most common linear structure along with AX2E3 both of which have 180 degree bonds. The lone pairs do not effect the bond angle because electron electron repulsion.

Schem_student

Sigma bonds are made up of two orbitals in which 1 electron from each atom interact end to end. This is an s-s orbital overlap and allows for rotation. A pi bond is made up of a side by side overlap of orbitals and prevents rotation.

Schem_student

Xenon tetraflouride has 6 regions of electron density because of the two lone pairs on the central Xe in the lewis dot structure. If you add electrons of Xe(8 electrons) + 4 F (4x 7 electrons) = 36 electrons which could create 18 pairs. 16 pairs are taken by the bonding of Xe to the 4 Fluorines and ...

Schem_student

ClF3 has 3 atoms bonded and two lone pairs which create a total of 5 regions of electron density which denotes a T shape. The net dipole moment would be pointing to the lone pairs making it polar. As for the dipoles of the other atoms in the molecule, Cl has greater electronegativity than the F atom...

Schem_student

Does it matter which atoms you orient where when you draw the molecular structure for a molecule that is trigonal planar?

Schem_student

Also you can learn molecular shape alot easier if for some lewis structures you start to draw them similar to their Molecular shape. This can be true for bent, trigonal planar, and seesaw.

Schem_student

That is the hardest part when it comes to molecular shape because there is a large difference between elctron denisty domains that are lone pairs vs bonding pairs. The lone pair domain affects the elctrons involved in the bonding pairs significantly more than a bonding pair would. The electron elect...

Schem_student

Also it is important to just understand how lone pairs affect the bond angles of shapes like triginal pyramidal for example making the bond angle less than 109.5 degrees.

Schem_student

What about cations or postively charged atoms in the p block? Do cations follow the same trend as their neutral atoms?

Schem_student

You would first want to convert the nm to m of the ejected electron then utilize the De broglie equation to find velocity of the ejected electron . The velocity you find you then end up putting in the Kenetic Energy Formula= 1/2 mv^2 and add the KE to work function after converting value from KJ to ...

Schem_student

I was wondering how you would determine the Lewis structure for MgCl2 ? Would you attach both Cls to the central atom Mg or would you treat it similar in structure to the salt NH4Cl and create the structure of Ammonium together and have the Cl have a full octet in a sperate bracket? I have seen both...

Schem_student

You must use E= freq x h but make sure to convert KJ to joules because planc's constant is in J x s.

Schem_student

Flourine and Chlorine have gretaer electron affinities because of their need to fufill their octet and become more stable atoms. If CL and F were to recieve an electron they would reach the goal of having a noble gas configuration of Argon and Neon.

Schem_student

The debroglie equation and hypothesis are validated in part by electron diffraction by a crystal.

Schem_student

Thank you ! @Henri_de_Guzman_3L I see that it is more stable as a full 3d orbital so it takes the electron from the 4s. This would then be the same then for Chromium.

Schem_student

Question 2A.5 asks for the ground state electron configuration for Cu + which is isolectronic with Ni which would have a configuration of [Ar]3d^8 4s^2 why then is the solution [Ar] 3d^10 ?

Schem_student

The principle quantum number n is used to distinguish atomic orbitals that have similar energies that we consider to be in the same shell. The principle quantum # can be used to find other quantum numbers such as l=n-1.

Schem_student

The first thing to understand is that n is the principle quantum number and because items have the same energy they are known to be in the same shell. These shells can be synonymously labeled by the value of n. Next, is the quantum number l which is known as an orbital angular momentum qunatum numbe...

Schem_student

When I was going through the quantum world problem section I was confused about using l=n-1 but if we were given 5d then l= 2 not l=5-1which would gove you l=4. Why is it always l=2 for d subshell even when we are in the shell n=5?

Schem_student

For Test 2 Levelle said to understand everything up until your last lecture last week.

Schem_student

It does help to do problems outside of what we have covered so far in the case of the problem sets due on a non-testing week because it helps prepare for future topics that levelle covers in lecture.

Schem_student

The question asks how many quantum numbers exist when n=7. I assumed L = n-1 which means L equals anything from 0-6. Or is there only quantum numbers between 0-4 ?

CHEMISTRY COMMUNITY

Search found 29 matches

Re: bis-,tris-,tetrakis-

9C.3 7TH EDITION NAMING

Re: AXE formula

Re: Question 3.119

Re: 2F.13 7th Ed

2F.15 7th edition

Re: Hypothetical Shape Question

Re: Linear structure with lone pairs

Re: Sigma vs pi bonds

Re: Xenon Tetrafluoride

Re: Polarity

Position of atoms in Trigonal Planar

Re: Arrangement vs Shape

Re: Homework Question 4.5 (6th edition)

Re: Will we have to calculate bond angles?

Re: Sizes of ions and neutral atoms

Re: work function and frequency

Lewis Structures for Ionic Compunds

Re: Exam 2 Question 4A

Re: Electron Affinity

Re: DeBroglie Equation and experiment

Re: 2A.5 7th edition

2A.5 7th edition

Re: Principle Quantum #

Re: Quantum Numbers

Angular Momentum Quantum Numbers

Re: Test 2

Re: Homework

1D.13