Search found 23832 matches
- Tue Oct 27, 2015 2:45 am
- Forum: Lewis Structures
- Topic: Lewis Structure of Amine Ion
- Replies: 1
- Views: 449
Re: Lewis Structure of Amine Ion
This has two bonding groups and two lone pairs, so it's the same shape as water (bent)
- Tue Oct 27, 2015 2:42 am
- Forum: Hybridization
- Topic: Easy trick for hybridization
- Replies: 1
- Views: 692
Re: Easy trick for hybridization
This won't work with things that have lone pairs. NH3 is sp3 hybridized because it still has 4 regions of electron density.
- Tue Oct 27, 2015 2:41 am
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: M.O. Energy Diagram
- Replies: 1
- Views: 346
Re: M.O. Energy Diagram
You will count the total electrons then place them into the MO's using the same rules as you would for atomic orbitals (singly-occupied before double-occupied, singly-occupying electrons have the same spin, two electrons per orbital)
- Tue Oct 27, 2015 2:39 am
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: Energy Levels for Antibonding Molecular Orbitals
- Replies: 1
- Views: 332
Re: Energy Levels for Antibonding Molecular Orbitals
Imagine you have two waves that interfere constructively very strongly. You take one of the waves and shift it half-wavelength, then now your two waves will interfere destructively very strongly. So the more stable the bonding orbital, the more unstable its corresponding antibonding orbital.
- Tue Oct 27, 2015 2:35 am
- Forum: Hybridization
- Topic: Increasing the s-character of Hybrid Orbitals
- Replies: 1
- Views: 1269
Re: Increasing the s-character of Hybrid Orbitals
Increasing s-character increases the bond angle.
sp3 has 25% s-character and is 109.5 degrees
sp2 has 33% s-character and is 120 degrees
sp has 50% s-character and is 180 degrees
sp3 has 25% s-character and is 109.5 degrees
sp2 has 33% s-character and is 120 degrees
sp has 50% s-character and is 180 degrees
- Tue Oct 27, 2015 2:33 am
- Forum: Photoelectric Effect
- Topic: Creating Lewis structure.
- Replies: 1
- Views: 550
Re: Creating Lewis structure.
You will use a double bond if you find that
1. you ran out of electrons while placing electrons, therefore you need to share some of them
2. you can get a better (lower) formal charge by making a double bond
1. you ran out of electrons while placing electrons, therefore you need to share some of them
2. you can get a better (lower) formal charge by making a double bond
- Mon Oct 26, 2015 9:34 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR Practice
- Replies: 31
- Views: 14760
Re: VSEPR Practice
Hey guys, please try and post any questions in the appropriate forum category from now on. It is getting a little off topic in this thread.
- Mon Oct 26, 2015 9:33 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR Practice
- Replies: 31
- Views: 14760
Re: VSEPR Practice
How do you determine when to look at unpaired electrons in subshells or at the nuclear charge in order to figure out which atom has a greater ionization energy and/or electron affinity? Only in cases where there is a half/fully filled subshell (the exceptions) would the electrons matter (and you're...
- Mon Oct 26, 2015 9:30 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR Practice
- Replies: 31
- Views: 14760
Re: VSEPR Practice
AlexNguyen15 wrote:Will we need to know all of the VSEPR shapes or just the ones we covered in class? For example pentagonal bipyramidal, square pyramidal, and T-shaped?
You should be able to answer any of them.
- Mon Oct 26, 2015 8:42 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR Practice
- Replies: 31
- Views: 14760
Re: VSEPR Practice
Adriana Juarez 1 wrote:Will we need to know paramagnetism and diamagnetism for this quiz? It's in our practice quizzes but I'm not sure if we've gone over it yet.
Adriana, nope. Only material up to hybridization is fair game for the quiz.
- Mon Oct 26, 2015 7:56 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR Practice
- Replies: 31
- Views: 14760
Re: VSEPR Practice
What does "greater eff. nuclear charge" mean in relation to ionization energy and electron affinity trends? Would that be a good enough explanation for the quiz? For IE, the greater effective nuclear charge means that it is harder to pull off an electron because it is being held tighter. ...
- Mon Oct 26, 2015 6:21 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR Practice
- Replies: 31
- Views: 14760
Re: VSEPR Practice
AlexNguyen15 wrote:Could the lewis structure for (S03)2- be drawn with 3 single bonds and a lone pair? Or for the quiz should we always draw the lewis structure that has the most formal charges of 0?
You would always want the lowest energy Lewis structure, so that would be the one with the minimized formal charges.
- Mon Oct 26, 2015 4:16 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR Practice
- Replies: 31
- Views: 14760
Re: VSEPR Practice
Hello! I had a question about the first set of practice questions. For XeOF4, why is it necessary to give Xe a lone pair and O a double bond? Why not use that lone pair to complete Oxygen's octet and eliminate the need for the double bond? -Adriana Adriana, oxygen does have a complete octet. If the...
- Mon Oct 26, 2015 4:11 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR Practice
- Replies: 31
- Views: 14760
Re: VSEPR Practice
Anna Nordstrom 1A wrote:Why is XeO3F2 nonpolar? Isn't there an extra O that doesn't "cancel out" with the others?
Anna, the three oxygens will "cancel each other out" while the two fluorines will do the same. Remember all three of them are on the same plane in a circular shape around the central atom.
- Mon Oct 26, 2015 2:11 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Naming the molecular geometry vs regions of electrons
- Replies: 1
- Views: 411
Re: Naming the molecular geometry vs regions of electrons
When asked the shape (molecular geometry) of a molecule only name the shape (molecular geometry).
Name the shape = molecular geometry = position of atoms around the central atom
Name the shape = molecular geometry = position of atoms around the central atom
- Mon Oct 26, 2015 1:44 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles
- Replies: 1
- Views: 1239
Re: Bond Angles
Hello Maria, Good question, if you look at page 80 of your course reader, you will see that the strength of repulsion is listed as: lone-lone pair>lone-bonding pair>bonding-bonding pair. As an example consider methane (CH4) and the sulfite ion (SO3 2-). Methane is tetrahedral in shape and has 4 equi...
- Mon Oct 26, 2015 1:36 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Ionic vs Covalent Lewis Structure
- Replies: 1
- Views: 545
Re: HW Problem 4.19
The Lewis structure for (CH3)2Be is: H3C-Be-CH3 Based on the difference in the electronegativities of C(2.5) and Be(1.5) you can see that the difference is of 1, which places the character of the bond within the covalent region (difference of >2 is considered ionic and difference of <1.5 is consider...
- Mon Oct 26, 2015 8:53 am
- Forum: Bond Lengths & Energies
- Topic: Solution Manual Typo for 3.89 b
- Replies: 1
- Views: 525
Re: Solution Manual Typo for 3.89 b
Because the C is involved in a double bond
- Mon Oct 26, 2015 8:52 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Determining Polar and Non Polar Molecules
- Replies: 2
- Views: 624
Re: Determining Polar and Non Polar Molecules
You could not really look at the Lewis structure and determine the symmetry unless you memorized all the shapes. If you looked st the VSEPR model and did the same thing, it would be much easier to determine from this.
- Mon Oct 26, 2015 8:51 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Lewis Structures
- Replies: 1
- Views: 303
Re: Lewis Structures
If the charges match with the overall charge.
- Mon Oct 26, 2015 8:50 am
- Forum: Octet Exceptions
- Topic: HW 3.97
- Replies: 1
- Views: 462
Re: HW 3.97
Phosphorus is very unique with this structure. Don't worry about drawing anything like this, it is more of a cool fact rather.
- Sun Oct 25, 2015 11:10 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Determining Carbon Compound Angles
- Replies: 1
- Views: 331
Re: Determining Carbon Compound Angles
There are two central atoms. Each will be trigonal planar and have bond angles of 120˚. And yes, since other organic compounds will have the same arrangements it will be true for other organic compounds.
- Sun Oct 25, 2015 10:57 pm
- Forum: Electronegativity
- Topic: Strongest CX bond, where X is a halogen
- Replies: 2
- Views: 2309
Re: Strongest CX bond, where X is a halogen
Think about the relative sizes. Fluorine is much smaller => shorter bond => stronger bond.
- Sun Oct 25, 2015 10:55 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: BF3 VSEPR Shape
- Replies: 1
- Views: 848
Re: BF3 VSEPR Shape
It is an exception.
- Sun Oct 25, 2015 10:53 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Molecular Orbital Theory
- Replies: 1
- Views: 442
Re: Molecular Orbital Theory
The order you gave is the exact opposite. Either the book is backwards or perhaps you read it the opposite way?
- Sun Oct 25, 2015 10:44 pm
- Forum: Ionic & Covalent Bonds
- Topic: Ionic and Covalent Character
- Replies: 2
- Views: 643
Re: Ionic and Covalent Character
You can think of them in those terms, the ionic and covalent character are really complimentary properties so that is perfectly fine. The size plays a role in a way, however since size is related to electronegativity (eg: effective nuclear charge) it is really all related.
- Sun Oct 25, 2015 10:42 pm
- Forum: Octet Exceptions
- Topic: Double or Single bond in ClO (problem 59, part a)
- Replies: 1
- Views: 607
Re: Double or Single bond in ClO (problem 59, part a)
Including a double bond would exceed the octet of one of the atoms.
- Sun Oct 25, 2015 10:41 pm
- Forum: Lewis Structures
- Topic: Lewis Structure Chapter 3 #59
- Replies: 1
- Views: 331
- Sun Oct 25, 2015 10:41 pm
- Forum: Lewis Structures
- Topic: Lewis structure of chlorine monoxide, ClO
- Replies: 2
- Views: 6097
Re: Lewis structure of chlorine monoxide, ClO
It seems that the correct answer is based off molecular orbital arguments that are outside of the scope of this course. I am sure if you had to draw this structure, your answer would be perfectly acceptable provided you included your justification.
- Sun Oct 25, 2015 10:35 pm
- Forum: Hybridization
- Topic: S Character
- Replies: 1
- Views: 377
Re: S Character
viewtopic.php?f=42&t=6594
Please look for your question before asking it, especially as this question has been asked 5-6 times today.
Please look for your question before asking it, especially as this question has been asked 5-6 times today.
- Sun Oct 25, 2015 10:25 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Configuration question
- Replies: 1
- Views: 434
Re: Configuration question
Generally manganese will not be in the +1 oxidation state. Due to the order in which electrons would be removed, I would predict the second option is more stable. However, you would only be able to tell by experimental data.
- Sun Oct 25, 2015 10:14 pm
- Forum: Hybridization
- Topic: hybridization exceptions
- Replies: 1
- Views: 445
Re: hybridization exceptions
There are not any that are crucial in regards to this class or anything you might be asked.
- Sun Oct 25, 2015 10:09 pm
- Forum: Hybridization
- Topic: Fall 2012 #3
- Replies: 1
- Views: 401
Re: Fall 2012 #3
That notation should be fine.
When it comes to bonds between two different atoms, you can average their atomic number to see if it is the result is closer to nitrogen or oxygen's atomic number and use the corresponding molecular orbital scheme.
When it comes to bonds between two different atoms, you can average their atomic number to see if it is the result is closer to nitrogen or oxygen's atomic number and use the corresponding molecular orbital scheme.
- Sun Oct 25, 2015 10:07 pm
- Forum: Dipole Moments
- Topic: Diamagnetic?
- Replies: 1
- Views: 558
- Sun Oct 25, 2015 10:02 pm
- Forum: Octet Exceptions
- Topic: Octet Exceptions
- Replies: 1
- Views: 523
- Sun Oct 25, 2015 10:02 pm
- Forum: Octet Exceptions
- Topic: Lone Electron Placement on Radicals
- Replies: 1
- Views: 392
Re: Lone Electron Placement on Radicals
The lone electron would be placed on the carbon to minimize formal charges.
i.e. H-O-C=O gives formal charges of 0,0,0 and 0 if the lone electron is placed on carbon.
i.e. H-O-C=O gives formal charges of 0,0,0 and 0 if the lone electron is placed on carbon.
- Sun Oct 25, 2015 10:02 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: Bond order equaling .5
- Replies: 1
- Views: 1113
Re: Bond order equaling .5
Diborane is an example of a molecule with a bond order of 1/2. As you mentioned, bond order is indicative of the number of bonds between a pair of atoms. The higher the bond order, the greater the relative stability.
- Sun Oct 25, 2015 9:51 pm
- Forum: Octet Exceptions
- Topic: Octet Exception D-Orbitals
- Replies: 1
- Views: 391
Re: Octet Exception D-Orbitals
Yes. Molecules with expanded octets involve highly electronegative terminal atoms, and a nonmetal central atom found in the third period or below, which those terminal atoms bond to.
- Sun Oct 25, 2015 9:49 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: Valence e- configuration
- Replies: 1
- Views: 406
Re: Valence e- configuration
It is referring to how many electrons are in each orbital.
- Sun Oct 25, 2015 9:48 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: T-shaped molecules
- Replies: 1
- Views: 527
Re: T-shaped molecules
It's true that lone pairs repel more strongly than bonding electrons, but the effect is not completely taking over all other repulsions. A compromise must be made. In particular, 90-degree interactions between lone pairs and bonding pairs needs to be avoided. If the lone pairs occupy the axial posit...
- Sun Oct 25, 2015 9:46 pm
- Forum: Hybridization
- Topic: Shape
- Replies: 2
- Views: 514
Re: Shape
Resonance does make a difference in molecular shape.
- Sun Oct 25, 2015 9:44 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Lone pairs and Molecular Shape
- Replies: 3
- Views: 610
- Sun Oct 25, 2015 9:44 pm
- Forum: Octet Exceptions
- Topic: Sulfur and its expanded octet property
- Replies: 2
- Views: 921
Re: Sulfur and its expanded octet property
It cannot attain anything higher than that, and will never come close to having nine substituents. Think about the relative size of the atoms bonded to sulfur. You would not be able to fit more than six bonded atoms.
- Sun Oct 25, 2015 9:41 pm
- Forum: Coordinate Covalent Bonds
- Topic: Involvement in Lewis Acid-Base Rxns
- Replies: 1
- Views: 648
Re: Involvement in Lewis Acid-Base Rxns
The "coordinate" prefix simply serves to indicate the origin of the electrons in the bond. No, B and Al are not the only elements typically involved in Lewis Acid/Base reactions.
- Sun Oct 25, 2015 9:38 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Homework 3.39 Lewis Structures
- Replies: 1
- Views: 383
Re: Homework 3.39 Lewis Structures
If there is a charge on the molecule or atom, you will need to put it in brackets with the appropriate charge.
- Sun Oct 25, 2015 9:36 pm
- Forum: Hybridization
- Topic: Question on 4.25
- Replies: 2
- Views: 715
Re: Question on 4.25
There is free rotation around the bonds. You would never be able to make it stay in one position unless it was a double bond.
- Sun Oct 25, 2015 9:34 pm
- Forum: Hybridization
- Topic: Lone Pairs and Hybridization
- Replies: 1
- Views: 471
Re: Lone Pairs and Hybridization
It is not in a unhybridized p-orbital because all three p-orbitals are hybridized, meaning there are no p-orbitals left. Since we know the experimentally determined shape is tetrahedral, it must be in a hybridized orbital.
- Sun Oct 25, 2015 7:15 pm
- Forum: Lewis Structures
- Topic: BF3 valence electron placement
- Replies: 2
- Views: 1378
Re: BF3 valence electron placement
Boron is sp2 hybridized in BF3, and the third p-orbital remains unhybridized and empty, so that Boron lacks an octet.
- Sun Oct 25, 2015 7:13 pm
- Forum: Lewis Structures
- Topic: HW 3.89
- Replies: 2
- Views: 297
Re: HW 3.89
This question cannot be answered without more information. Please provide more information.
- Sun Oct 25, 2015 7:12 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: formal charge
- Replies: 3
- Views: 662
Re: formal charge
Yes, but it will not always be possible. Remember that it's most important to satisfy the octet rule for second period elements.
- Sun Oct 25, 2015 7:09 pm
- Forum: Hybridization
- Topic: Hybridization involving d orbital
- Replies: 1
- Views: 362
Re: Hybridization involving d orbital
The position does not matter, usually it is written as dsp3 for AX5-type molecules and d2sp3 for AX6-type molecules.
- Sun Oct 25, 2015 6:59 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Stable Lewis Structures
- Replies: 1
- Views: 257
Re: Stable Lewis Structures
The ideal bonding number is the same as giving something a 0 formal charge. Eg. if oxygen has an octet and two bonds, then its formal charge is 6 - 4 - (4/2) = 0. And if nitrogen has an octet and three bonds, then its formal charge is 5 - 2 - (6/2) = 0. This works well for H, O, N, C, F. But somethi...
- Sun Oct 25, 2015 6:56 pm
- Forum: Hybridization
- Topic: Hybridization in general
- Replies: 4
- Views: 990
Re: Hybridization in general
All atoms involved in covalent bonding are hybridized. You can tell what kind of hybridization it is by counting the number of regions of electron density.
- Sun Oct 25, 2015 5:47 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: Atomic Orbitals to Molecular Orbitals
- Replies: 1
- Views: 345
- Sun Oct 25, 2015 5:43 pm
- Forum: Lewis Structures
- Topic: Quiz 2 Preparation, Fall 2013, #9
- Replies: 3
- Views: 424
Re: Quiz 2 Preparation, Fall 2013, #9
I apologize, the orbitals labeled "2s" should be labeled "2p"
- Sun Oct 25, 2015 5:41 pm
- Forum: Lewis Structures
- Topic: Quiz 2 Preparation, Fall 2013, #9
- Replies: 3
- Views: 424
Re: Quiz 2 Preparation, Fall 2013, #9
You would have to use MO theory to answer this question I believe. We have not learned it yet.
- Sun Oct 25, 2015 5:27 pm
- Forum: Hybridization
- Topic: Paramagnetism vs Diamagnetism
- Replies: 1
- Views: 427
Re: Paramagnetism vs Diamagnetism
Diamagnetic materials create an induced magnetic field in a direction opposite to an externally applied magnetic field, and are repelled by the applied magnetic field. In contrast, the opposite behavior is exhibited by paramagnetic materials.
- Sun Oct 25, 2015 5:24 pm
- Forum: Electronegativity
- Topic: Chlorine and Oxygen
- Replies: 1
- Views: 574
Re: Chlorine and Oxygen
Please post the full question so I can see precisely what you are referring to.
- Sun Oct 25, 2015 5:23 pm
- Forum: Lewis Structures
- Topic: Question 39 in chapter 3 - Lewis structure determination
- Replies: 2
- Views: 454
Re: Question 39 in chapter 3 - Lewis structure determination
This is an ionic compound, therefore there will not actually be any covalent bonds.
- Sun Oct 25, 2015 5:18 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR Practice
- Replies: 31
- Views: 14760
Re: VSEPR Practice
Here is the solution for you guys. Again, I want to emphasize these practice exercises are not meant to take place of your assigned problems. Rather, they are meant to supplement them and give you a chance to apply what you already know. But you should definitely be studying additional problems as w...
- Sun Oct 25, 2015 4:16 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Sigma bonds and Pi Bonds
- Replies: 8
- Views: 2557
Re: Sigma bonds and Pi Bonds
It is arbitrary.
- Sun Oct 25, 2015 4:15 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Quiz #2 content
- Replies: 1
- Views: 505
Re: Quiz #2 content
Those topics will not be on the quiz but you can practice them if you wish.
- Sun Oct 25, 2015 4:15 pm
- Forum: Bond Lengths & Energies
- Topic: Question 3.89 Bond Lengths
- Replies: 3
- Views: 1108
Re: Question 3.89 Bond Lengths
Can you post the full question so that it is clear what you are asking?
- Sun Oct 25, 2015 4:14 pm
- Forum: Hybridization
- Topic: Chapter 4 question 1 help please
- Replies: 2
- Views: 736
Re: Chapter 4 question 1 help please
I am super confused, can you post a picture that explains what you are talking about?
- Sun Oct 25, 2015 4:13 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: Quiz 2
- Replies: 2
- Views: 516
Re: Quiz 2
no
- Sun Oct 25, 2015 4:13 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: Bond order
- Replies: 1
- Views: 313
- Sun Oct 25, 2015 4:11 pm
- Forum: Resonance Structures
- Topic: Polar Charges
- Replies: 1
- Views: 471
Re: Polar Charges
You do not have to draw the arrows, it may help but it is not required. You will have to be able to determine if a molecule is polar or non polar.
- Sun Oct 25, 2015 4:10 pm
- Forum: Hybridization
- Topic: Hybridization
- Replies: 1
- Views: 457
Re: Hybridization
Hybridization is considered when there are more than one bond coming from an atom. That is why only central atoms are considered hybridized. For example, the hydrogens in water are not considered hybridized. Or with CH 2 O, the carbonyl oxygen is not considered hybridized. We only consider the carbo...
- Sun Oct 25, 2015 4:08 pm
- Forum: Hybridization
- Topic: Hybridization of atoms
- Replies: 2
- Views: 495
Re: Hybridization of atoms
Yes it would be wrong. Hybridization only applies if the atom is bonded to more than one additional atom. Since hydrogen can only form one bond, we do not consider it in that manner.
- Sun Oct 25, 2015 4:05 pm
- Forum: Lewis Structures
- Topic: Quiz 2 Prep Fall 2013 Question 9
- Replies: 1
- Views: 331
Re: Quiz 2 Prep Fall 2013 Question 9
You would use molecular orbital diagrams to determine this. You will not need to know it for this quiz.
- Sun Oct 25, 2015 3:56 pm
- Forum: Electronegativity
- Topic: Debye units
- Replies: 1
- Views: 803
Re: Debye units
A debye is just a non-SI unit of electric dipole moment. It will tell you the same thing, just different units.
- Sun Oct 25, 2015 3:53 pm
- Forum: Lewis Structures
- Topic: ClO2 Lewis Structure
- Replies: 3
- Views: 3312
Re: ClO2 Lewis Structure
Would you be able to post a picture so I can see for sure what you are talking about?
- Sun Oct 25, 2015 3:51 pm
- Forum: Lewis Structures
- Topic: Element Arrangements & Lone Pairs
- Replies: 1
- Views: 390
Re: Element Arrangements & Lone Pairs
Hey Yusrah,
Either way is fine. It is more important to place them correctly when drawing the VSEPR representation of the molecule. The Lewis structure is just to represent the bonds and lone pairs present.
Either way is fine. It is more important to place them correctly when drawing the VSEPR representation of the molecule. The Lewis structure is just to represent the bonds and lone pairs present.
- Sun Oct 25, 2015 3:50 pm
- Forum: Electronegativity
- Topic: Electronegativity and The Mulliken Equation
- Replies: 1
- Views: 696
Re: Electronegativity and The Mulliken Equation
At least for this quiz, no. Just the general trends
- Sun Oct 25, 2015 3:48 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: Diagrams used in MO Theory
- Replies: 1
- Views: 412
Re: Diagrams used in MO Theory
I believe I understand what you are asking and the reason for this is orbital mixing. Since the orbital energies are different past that point, they will mix in an uneven manner resulting in the orbitals you have noticed. That is why the order of the molecular orbitals is sometimes different dependi...
- Sun Oct 25, 2015 1:14 pm
- Forum: Resonance Structures
- Topic: Incomplete octets
- Replies: 2
- Views: 591
Re: Incomplete octets
BF3 does not have a double bond, because this would place a +1 formal charge on fluorine, the most electronegative of all elements. Boron in this compound has an incomplete octet with only 6 valence electrons around it.
- Sat Oct 24, 2015 11:49 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: More Seesaw Questions
- Replies: 3
- Views: 503
Re: More Seesaw Questions
No, the two Cl that are in the same plane are the top Cl and the right Cl, and their bond angle would be ~90˚ (it is a right angle). The 180˚ angle would be between the Cl on the right, and the plane line that occurs between the two Cl's that are pointing back and forward.
- Sat Oct 24, 2015 11:34 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Lone pairs and polarity
- Replies: 1
- Views: 352
Re: Lone pairs and polarity
They have a huge impact on polarity because they are such dense areas of electron density. If the electron pair is asymmetrical with regards to the geometry (H2O) it will be polar. If the electron pairs are symmetrical with regards to the geometry (XeF4) it will be non polar.
- Sat Oct 24, 2015 11:29 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Oxidation States
- Replies: 1
- Views: 384
Re: Oxidation States
Nickel will not go to krypton or argon electron configurations. Its major oxidation state is 2, however it is possible to have oxidation states of 1, 2, 3, 4, -1, -2.
- Sat Oct 24, 2015 11:21 pm
- Forum: Dipole Moments
- Topic: Net Dipole Moment of a Trigonal Pyramidal
- Replies: 1
- Views: 1004
Re: Net Dipole Moment of a Trigonal Pyramidal
Yes for the most part. It is more important to realize that the dipoles won't cancel and it will be polar. Since different sources use different conventions for which direction the arrow points, it is not good to rely solely on that method. But as stated, it is more important to realize that they wo...
- Sat Oct 24, 2015 11:18 pm
- Forum: Resonance Structures
- Topic: 3.57 part a
- Replies: 1
- Views: 461
Re: 3.57 part a
There are three resonance structures that are equivalent, I am not sure what your fourth one is. In your proposed structure of three double bonded oxygens, there would be a 2- formal charge on the sulfur atom, along with an expanded octet. The two 1- charges will be the better choice by far because ...
- Sat Oct 24, 2015 11:13 pm
- Forum: Hybridization
- Topic: Axial vs. Equatorial Lone Pair
- Replies: 1
- Views: 398
Re: Axial vs. Equatorial Lone Pair
Would you be able to provide an example? I am not entirely clear what you mean.
- Sat Oct 24, 2015 11:12 pm
- Forum: Bond Lengths & Energies
- Topic: How to Find Bond Length
- Replies: 1
- Views: 836
Re: How to Find Bond Length
You would not be able to determine the bond length unless you had experimental data that actually had the bond lengths. Using the resonance forms allows you to predict that the length would be between that of a S-O single bond and S=O double bond. You cannot accurately say anything other than that u...
- Sat Oct 24, 2015 11:10 pm
- Forum: Hybridization
- Topic: Bonds Decrease
- Replies: 1
- Views: 444
- Sat Oct 24, 2015 11:09 pm
- Forum: Bond Lengths & Energies
- Topic: Bond Energies..?
- Replies: 1
- Views: 445
Re: Bond Energies..?
I do not understand the question, would you be able to provide an example for what you are talking about?
- Sat Oct 24, 2015 11:09 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charge and its significance
- Replies: 2
- Views: 1161
Re: Formal Charge and its significance
The location in regards to central/non-central does not matter as much as the atom itself. Generally, charges would be better placed on the more electronegative atom. If that happens to be the central atom, it would be best there. If that is a bonded atom, it would be best there.
- Sat Oct 24, 2015 11:07 pm
- Forum: Lewis Structures
- Topic: Isolobal Analogy
- Replies: 1
- Views: 410
Re: Isolobal Analogy
It may be possible, but probably not likely. The isolobal principle applies "if the number, symmetry properties, approximate energy and shape of the frontier orbitals and the number of electrons in them are similar – not identical, but similar." That is a lot of things that must be in comm...
- Sat Oct 24, 2015 10:59 pm
- Forum: Resonance Structures
- Topic: Resonance hybrid of nitryl chloride
- Replies: 1
- Views: 477
Re: Resonance hybrid of nitryl chloride
No, by definition covalent bond is shared. There is a formal positive charge on nitrogen and a formal negative charge on the single bonded oxygen. Placing two double-bonded oxygens with the chlorine single bond gives nitrogen ten valence electrons and therefore is not a valid answer.
- Sat Oct 24, 2015 10:55 pm
- Forum: Lewis Structures
- Topic: Element Arangement
- Replies: 1
- Views: 287
Re: Element Arangement
For the Lewis structure, only the bonding and lone pair placement really matters. The order is not a big deal. For the drawing, you would probably put the bonded atoms symmetrically around the central atom for both a Lewis structure and a VSEPR model. The VSEPR model is where it would be important t...
- Sat Oct 24, 2015 10:50 pm
- Forum: Ionic & Covalent Bonds
- Topic: Charges
- Replies: 1
- Views: 414
Re: Charges
Would you be able to provide examples? That is a fairly broad question
- Sat Oct 24, 2015 10:49 pm
- Forum: Hybridization
- Topic: HW 4.43
- Replies: 1
- Views: 447
- Sat Oct 24, 2015 10:49 pm
- Forum: Hybridization
- Topic: Quiz 2 Preperation #1 (Fall 2013)
- Replies: 2
- Views: 511
Re: Quiz 2 Preperation #1 (Fall 2013)
Yes, that is what the 2 means. Some books will use it, some will not. Since we are only talking about the valence shell, a lot of sources will only refer to the hybridization without the principal quantum number.
- Sat Oct 24, 2015 10:47 pm
- Forum: Electronegativity
- Topic: Electronegativity of Cl and N
- Replies: 2
- Views: 903
Re: Electronegativity of Cl and N
This is not really a good question (for the book, I don't mean you shouldn't have asked it) in that you would not really be able to determine this qualitatively using the trends. Some books have them about equal, and others have what you mentioned. The electronegativity trend increases towards the u...
- Sat Oct 24, 2015 10:39 pm
- Forum: Hybridization
- Topic: Hybridization
- Replies: 1
- Views: 435
Re: Hybridization
I am sorry, I am a little confused by the question. The central sulfur atom is sp3 hybridized. That is the extent of a question you could be asked. Since there is resonance on the oxygen atoms, it is kind of tricky to apply the hybridization to them.
- Sat Oct 24, 2015 10:33 pm
- Forum: Hybridization
- Topic: Unhybridized Orbitals
- Replies: 1
- Views: 715
Re: Unhybridized Orbitals
That would be one method. However, the more general method is just determine the hybridization. For example, in ethene both carbons are sp 2 hybridized. Since there are 3 p orbitals, one must be unhybridized in order for the double bond overlap to occur. If you had ethyne, both carbons would be sp h...
- Sat Oct 24, 2015 10:30 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles for Angular, T-shaped, etc.
- Replies: 4
- Views: 1116
- Sat Oct 24, 2015 10:30 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles for Angular, T-shaped, etc.
- Replies: 4
- Views: 1116
Re: Bond Angles for Angular, T-shaped, etc.
Just try and keep in mind the spatial orientation of the molecules and the shapes that are present. In the illustration below, it is a seesaw molecular shape. The two chlorines and the lone pair are all on the same axis in a circular shape. Thats how we can determine the bond angle is around 120. Th...
- Sat Oct 24, 2015 10:13 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: Quiz 2
- Replies: 2
- Views: 515
Re: Quiz 2
No, only the material that was covered up to hybridization
- Sat Oct 24, 2015 10:13 pm
- Forum: Hybridization
- Topic: s-character
- Replies: 1
- Views: 431
- Sat Oct 24, 2015 10:11 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: More Seesaw Questions
- Replies: 3
- Views: 503
Re: More Seesaw Questions
Hey Tania, I attached a picture that hopefully explains this. Basically, the electron pair wants to reduce interactions with all the other "clouds" (bonds) of electron density. Please keep in mind the depiction of bond angle distortion is highly exaggerated just to illustrate the point, bu...