## Search found 13 matches

Fri Dec 04, 2015 10:36 am
Forum: Identifying Acidic & Basic Salts
Topic: Final: Strong/ Weak Acids/Bases
Replies: 11
Views: 952

### Final: Strong/ Weak Acids/Bases

For the final, do we need to memorize any of the strong acids/bases and weak acids/bases given on the list int he course reader? If so, which ones?
Mon Nov 23, 2015 6:52 pm
Forum: Bronsted Acids & Bases
Topic: Understanding Bronsted acids and bases
Replies: 2
Views: 457

### Re: Understanding Bronsted acids and bases

No, depending on the reaction there can be more than one acid or base and sometimes one molecule can act as both(amphoteric).
Sun Nov 22, 2015 10:05 pm
Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
Topic: Homework 12.67: Ranking solutions according to pH
Replies: 1
Views: 375

### Homework 12.67: Ranking solutions according to pH

How are you supposed to rank in order of increasing pH without doing any calculations or do you have to do calculations?
a.) 1.00 x 10^-5 M HCL
b.) 0.20 M CH3NH3
c.) 0.20 M NH4Cl
d.) 0.20 M NaCN
Thu Nov 19, 2015 6:00 pm
Forum: Naming
Topic: Quiz 3 Prep: #2
Replies: 2
Views: 452

### Quiz 3 Prep: #2

For number two on the practice quiz, would you put a charge around the brackets when writing the formula for Pentaamminebromocobalt(III)? Because cobalt has a +3 charge, bromine has -1 making the whole thing -2.
Tue Nov 17, 2015 11:32 pm
Forum: Naming
Topic: Oxidation Number in Naming
Replies: 1
Views: 337

### Oxidation Number in Naming

I'm confused as to why the oxidation of certain compounds appears and sometimes it does not. For example, for tetraamminediaquacobalt(III) bromide, the number within the parenthesis is apparent in the chemical formula as shown respectively: [Co(NH3)4(h20)2]Br3. However, for sodium bisoxalato(diaqua)...
Mon Nov 09, 2015 11:15 am
Forum: Naming
Topic: Naming in the Correct Order
Replies: 1
Views: 277

### Naming in the Correct Order

Does it matter which order you name coordination compounds? For example, the question is to name potassium hexacyanoidochromate(III) and the answer is [K3(Cr)(CN)6] but would it matter if you wrote it as [K3(CN)6(Cr)]?
Fri Nov 06, 2015 3:20 pm
Forum: Administrative Questions and Class Announcements
Topic: Weekly Question
Replies: 5
Views: 1132

### Weekly Question

Is there a deadline for the weekly question? For instance I posted a question on Sunday for week five, but would this count as the week 5 question on Chemistry Community or was it posted to late? (it was the Sunday before week 6)
Fri Nov 06, 2015 3:04 pm
Forum: NEWS & RESOURCES
Topic: NO+ vs N2
Replies: 6
Views: 6611

### Re: NO+ vs N2

It will affect the shape by causing the s and p orbitals of O in NO to be lower. This is because O has a higher ionization energy than N so it is "weighed down". However, since Nitrogens atomic number is lower than 8, you must put the pi2px and pi2py orbitals before the sigma2pz orbital si...
Sun Nov 01, 2015 12:36 pm
Forum: Determining Molecular Shape (VSEPR)
Topic: Xenon Trioxide
Replies: 2
Views: 1164

### Re: Xenon Trioxide

You can determine whether or not to use single or double bonds by fulfilling the octet rule. The central atom must, unless exceptions apply, have eight bonds. If drawing the structure first with single bonds and several lone pairs does not add up to the number of valence electrons, then change one b...
Fri Oct 23, 2015 4:33 pm
Forum: Hybridization
Topic: Hybridization and Electron Spins
Replies: 1
Views: 264

### Hybridization and Electron Spins

How exactly do you determine the hybridization of a compound from it's electron spins? Also when do you put the spins as parallel and nonparallel (two arrows or one)? For example the energy level diagram for carbon in ethene is 2p: two single arrows and 2s: one double arrow to give 2sp^2, but how is...
Fri Oct 16, 2015 2:28 pm
Forum: Lewis Structures
Topic: Drawing a Lewis Structure with a double/triple bond
Replies: 4
Views: 910

### Re: Drawing a Lewis Structure with a double/triple bond

In order to determine whether or not you use triple/double bonds instead of more lone pairs you must calculate the number of valence electrons. For example, for O2 you have 2(6 e) = 12 e. If you drew the lewis structure with more lone pairs, there would be too many electrons so instead you add a dou...
Wed Oct 07, 2015 5:10 pm
Forum: Quantum Numbers and The H-Atom
Topic: Chapter 2, Question 19 Part B
Replies: 1
Views: 298

### Chapter 2, Question 19 Part B

The question asks how many values of ml are allowed for an electron in a 6d-subshell? I understand that to find the magnetic quantum number, it can be any number in-between -l and +l, but I am wondering if since the 6d-subshell is in the d- orbital , is l automatically 2? If not, how do you determin...
Thu Oct 01, 2015 3:46 pm