Search found 30 matches
Search found 30 matches • Page 1 of 1
- Mon Jun 04, 2018 6:34 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: pi and sigma bonds
- Replies: 3
- Views: 198
I'm not quite sure of what you are asking for, but I'll write down my notes from what Professor Lavelle said in class. The bonds basically hold the atoms in a coordinate compound together. Sigma bonds: 2 orbitals, each with 1 electron; interact end-to-end to form 1 sigma-bond; allow bound atoms to r...
- Wed May 23, 2018 10:18 am
- Forum: Formal Charge and Oxidation Numbers
- Topic: Prioritizing Formal Charge
- Replies: 2
- Views: 218
I'm not sure if this is correct, but I remember that it is best if the center atom has a formal charge of zero but generally, the idea is to get all elements to be as close to 0 as possible.
- Wed May 23, 2018 10:16 am
- Forum: Octet Exceptions
- Topic: Maximum number of electrons in expanded octet
- Replies: 1
- Views: 171
The most electrons you can add to an expanded octet is 10 because ultimately, you're filling up the d orbital and that can only hold up to 10.
- Fri May 18, 2018 1:07 pm
- Forum: Lewis Structures
- Topic: Exceptions to the Octet
- Replies: 5
- Views: 247
I remember my TA saying that you can add up to 10 extra electrons since it is the d block that is involved in the expanded octet and it can hold ten electrons.
For more complicated compounds such as the H2C(NH2)COOH given in part c of 3.41, how would you go about figuring out specifically which elements are bound to which ones and in which order? It seems like a rather arduous process to test out possible combinations until you get one that gives the right...
Thanks so much: the replies really cleared it up! A follow-up question: if the correct lewis structure is a combination of the possible "correct" ones, why would we still need to calculate formal charge? Is that just to determine the result of resonance?
- Sun May 06, 2018 9:19 pm
- Forum: Empirical & Molecular Formulas
- Topic: Test 1/ Question 8 [ENDORSED]
- Replies: 6
- Views: 468
For this, you wouldn't need the mass of the molecule. The structures themselves give you the molecular formula since it shows you exactly how many of each element is in the molecule. You can literally count the how many of each element there are and that is basically the molecular formula. To get th...
- Sun May 06, 2018 9:15 pm
- Forum: Ionic & Covalent Bonds
- Topic: Covalent vs. Ionic
- Replies: 3
- Views: 210
First off, covalent bonds are between nonmetals and ionic bonds are between a metal and nonmetal. The biggest, and most important, difference is that elements in an ionic bond are more aggressive so it kind of takes the electron, which produces a charge for the overall molecule. Covalent bond elemen...
- Mon Apr 30, 2018 3:50 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: cation or anion?
- Replies: 4
- Views: 241
How do you know if an element will be a cation or anion if it is the same distance away from 2 different noble gases? Will they provide you with the information?
My TA said that just as you know the general ranges and order of the wavelengths you should be fine. She did say that it would be best if you knew that visible light is 400 to 700 nm.
- Sun Apr 22, 2018 6:11 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Test Number 1
- Replies: 10
- Views: 572
The average for my section was around a 22/40. My friend told me that her TA said that they would try to make it so that most people at least passed but I don't know how exactly that's gonna happen. They did say that they were aware of how hard it was and that for test number 2, they would include a...
- Sun Apr 15, 2018 9:04 pm
- Forum: Ideal Gases
- Topic: Reading the textbook [ENDORSED]
- Replies: 134
- Views: 91876
I think reading the textbook definitely helps. Personally, I feel like it gives me a better overview of the big topics I am supposed to be learning. Professor Lavelle's lecture tend to be a little more focused on one specific topic and one specific example so I read the textbook to link ideas togeth...
Yes, you are exactly right! The only difference is that an ionic bond is a bond between a metal and a nonmetal and then a metallic bond is between 2 metals. Again, just look at the periodic table to determine whether an element is a nonmetal or metal.
To put it simply, a covalent bond is a bond between 2 nonmetals. You can just look up the elements on the periodic table to determine if it is a nonmetal. They are to the right of the "staircase"-like divider.