Search found 12 matches
- Fri Dec 08, 2017 1:58 pm
- Forum: Lewis Acids & Bases
- Topic: Bronsted vs. Lewis
- Replies: 6
- Views: 926
Re: Bronsted vs. Lewis
I feel on the exam they will ask you what type of acid or base it is (Bronsted or Lewis) and both are different ways to describe an acid or base. Depending on which version they ask for is what mindset you will see the molecule and the reaction in
- Fri Dec 08, 2017 1:56 pm
- Forum: Acidity & Basicity Constants and The Conjugate Seesaw
- Topic: Reason for not including water
- Replies: 6
- Views: 721
Re: Reason for not including water
We do not include water because it present in such a great quantity that the reaction will not change how much there is. Also water is a pure liquid and a solvent therefore it can technically be both.
- Mon Dec 04, 2017 8:15 am
- Forum: Sigma & Pi Bonds
- Topic: Difference between Bonds [ENDORSED]
- Replies: 7
- Views: 1108
Re: Difference between Bonds [ENDORSED]
The first bond made is a sigma bond, any bond after that becomes a pi bond
- Mon Dec 04, 2017 8:15 am
- Forum: Resonance Structures
- Topic: Naming coordination compounds [ENDORSED]
- Replies: 3
- Views: 563
Re: Naming coordination compounds [ENDORSED]
apparently the "-ido" is a new form of naming but "chloro-", "cyano-"etc are still valid according to Lavelle. Both should be fine.
- Wed Nov 29, 2017 3:18 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Order of ligands [ENDORSED]
- Replies: 2
- Views: 392
Order of ligands [ENDORSED]
So I know that when naming a coordination complex the ligands must be in alphabetical order, however when converting from the name to the formula does the order of the ligands after the TM matter? or is there a certain order they need to be in?
dentates
How are you able to tell when a molecule is a mono,bi,tri etc -dentate?
- Mon Nov 20, 2017 8:03 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Radicals
- Replies: 4
- Views: 590
Re: Radicals
A radical is typically an odd number of electrons. if there are two then they can form a lone pair and no longer be radicals
- Mon Nov 20, 2017 8:02 am
- Forum: Sigma & Pi Bonds
- Topic: double bonds
- Replies: 5
- Views: 886
Re: double bonds
When two atoms are bound by more than one covalent bond, the remaining orbitals overlap and form a pi bond
- Wed Nov 15, 2017 8:02 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Radicals and electrons
- Replies: 3
- Views: 497
Re: Radicals and electrons
I'd say put it on the atom with the lower electronegativity, but also compare how many electrons an atom needs for the octet as well as the formal charge of the entire molecule and how you can achieve that depending on the placement fo the lone electron
- Wed Nov 15, 2017 7:55 pm
- Forum: Electronegativity
- Topic: Isoelectronic [ENDORSED]
- Replies: 11
- Views: 1446
Re: Isoelectronic [ENDORSED]
When an atom and ion have the same charge. For example, O- and F (not sure if O- exists but im using it to get the point across)
isoelectronic by definition are atoms which contain the same amount of electrons
isoelectronic by definition are atoms which contain the same amount of electrons
- Sun Nov 05, 2017 7:27 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Lewis Structures
- Replies: 6
- Views: 755
Re: Lewis Structures
I think the 3d models of molecules are the actual shape based on mathematical functions and i assume experiments that may have been used to accurately predict the location of an atom in the molecule. Hope this helps
- Sun Nov 05, 2017 7:25 pm
- Forum: Resonance Structures
- Topic: Delocalized
- Replies: 7
- Views: 853
Re: Delocalized
From what i understood and wrote in my notes, for an electron to be delocalized means it can be shared in different positions of the molecule. For example with benzene, an electron can be bonded between different carbon atoms, not some set three.