Search found 31 matches
- Mon Dec 03, 2018 5:44 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: pOH
- Replies: 5
- Views: 918
Re: pOH
Just know that pOH is the -log[OH-] and a low pOH means that the solution is more basic. While we're on this topic, does anyone know why a low pKA means that it is a stronger acid? The higher the pKA value, the more tight the proton is held. Since one of the properties of a strong acid is its abili...
- Mon Dec 03, 2018 5:19 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Chelates
- Replies: 4
- Views: 480
Re: Chelates
Does this mean that molecules that can act as chelates are polydentate?
- Mon Dec 03, 2018 5:17 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Tetrahedral vs. square-planar
- Replies: 6
- Views: 1815
Re: Tetrahedral vs. square-planar
What is the difference between tetrahedral and square planar in terms of coordination compounds? I know that for square planar there are four ligands at the corners of a square, but I am unsure of how to discern it from the tetrahedral ligand coordination complex.
- Mon Nov 26, 2018 3:23 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: test #3
- Replies: 14
- Views: 1536
Re: test #3
according to the website, it says all of molecular shape and bonding will be on test #3 but we haven't covered bond order, diamagnetism, or paramagnetism. so will these subjects be on test #3 or not ? In one of the other posts Dr. Lavelle said that bond order questions are "fair game." I'...
- Mon Nov 26, 2018 3:13 pm
- Forum: Hybridization
- Topic: Hybridization & Types of Bonds [ENDORSED]
- Replies: 3
- Views: 397
Re: Hybridization & Types of Bonds [ENDORSED]
Every bond has one sigma bond, the number of pi bonds depends on whether it is a double or triple bond.
- Mon Nov 26, 2018 3:08 pm
- Forum: Sigma & Pi Bonds
- Topic: Which bond would break first.
- Replies: 15
- Views: 2729
Re: Which bond would break first.
If pi bonds are weaker than sigma bonds then why are double and triple bonds stronger than single bonds?
- Wed Nov 21, 2018 2:17 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles
- Replies: 13
- Views: 2358
Re: Bond Angles
Yes I believe we are supposed to remember bond angles. I think the easiest thing to do is memorize them, but you can always try to visualize by drawing out the Lewis structure. That may get frustrating on a test with limited time though.
- Wed Nov 21, 2018 2:14 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: predicting dipole moments
- Replies: 4
- Views: 428
Re: predicting dipole moments
If a molecule does have a symmetrical molecular shape, such as the tetrahedral, that doesn't necessarily entail that the molecule is nonpolar. I would say that if all 4 atoms surrounding the central atom are the same and the net dipoles cancel out, then the molecule is nonpolar.
- Wed Nov 21, 2018 2:07 pm
- Forum: Hybridization
- Topic: Hybridization
- Replies: 6
- Views: 544
Re: Hybridization
You can determine hybridization by counting the number of electron densities surround the central atom in a Lewis Structure. For example, H2O has 4 regions of electron density: the central oxygen atom has 2 lone pairs and 2 hydrogen atoms bonded. Since there are 4 regions of electron density, the hy...
- Mon Nov 12, 2018 11:15 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Tetrahedral versus Trigonal Pyramidal
- Replies: 3
- Views: 391
Re: Tetrahedral versus Trigonal Pyramidal
Why does a tetrahedral have bond angles of 109.5 degrees while a trigonal pyramidal have bond angles of less than 109.5 degrees. Is it because the lone pair on the trigonal pyramidal is closer to the central atom and pushes the other atoms closer together? Yep it's because the lone pair repels the ...
- Mon Nov 12, 2018 11:11 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: determining VSEPR models
- Replies: 6
- Views: 554
Re: determining VSEPR models
While determining VSEPR formulas, does the E represent the total number of electrons not bonded or a collective lone pair? For example if the central atom had 2 electrons that aren't bonded would the E in the formula be E1 or E2?
- Mon Nov 12, 2018 11:03 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Homework Problem: SOCl2 bond angles
- Replies: 1
- Views: 401
Homework Problem: SOCl2 bond angles
In the 6th Edition Chapter 4 HW #7 part b, how do the lone pair electrons on the sulfur atom repel the bonded pairs with O and Cl equally?
- Thu Nov 08, 2018 9:21 pm
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: Polarizability and Dispersion Forces
- Replies: 2
- Views: 502
Re: Polarizability and Dispersion Forces
Venya Vaddi 1H wrote:If an atom or molecule is more polarizable, does this mean that its dispersion forces are stronger?
Yes, dispersion forces are stronger because the molecules are able to attract to each other more.
- Thu Nov 08, 2018 9:19 pm
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: Distortion, Polarizability
- Replies: 2
- Views: 712
Re: Distortion, Polarizability
Polarizability is how easily an element can be distorted. It depends on the number of electrons and the size of the atom or molecule. The more electrons an atom has, the more polarizable it is because the nuclear charge of the atom has less of an effect. As polarizability increases, dispersion force...
- Thu Nov 08, 2018 9:02 pm
- Forum: Ionic & Covalent Bonds
- Topic: Ionic vs Covalent Bonds
- Replies: 18
- Views: 1804
Re: Ionic vs Covalent Bonds
Covalent bonds are associated with the sharing of electrons between two nonmetals while Ionic bonds involve the transfer of electrons between a metal and nonmetal, which involves lattice energy. Ionic bonds are extremely stronger than covalent bonds because of the smaller distance between Ionic bon...
- Thu Nov 01, 2018 1:03 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal charge purpose
- Replies: 40
- Views: 7184
Re: Formal charge purpose
kellyzhang1210 wrote:why is the element most stable when its formal charge is 0?
When the formal charge of an element is 0, it's in the neutral state, which means that the amount of electrons is kind of "balanced" so that's why there is less instability.
- Thu Nov 01, 2018 1:00 pm
- Forum: Electronegativity
- Topic: Electroegativity
- Replies: 9
- Views: 1282
Re: Electroegativity
Do you think there will be any circumstances where we have to identify electronegativity trends between elements that are really close together because that seems a little ambiguous?
- Thu Nov 01, 2018 12:44 pm
- Forum: Resonance Structures
- Topic: Resonance
- Replies: 8
- Views: 976
Re: Resonance
When we have to draw Lewis Structures on the midterm do you think we'll have to draw every resonance structure possible?
- Sat Oct 27, 2018 2:54 pm
- Forum: Trends in The Periodic Table
- Topic: Ionization Energy and Electron Affinity
- Replies: 9
- Views: 1869
Re: Ionization Energy and Electron Affinity
Why are electrons that are further away from the nucleus easier to remove?
- Sat Oct 27, 2018 2:50 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Electron Affinity [ENDORSED]
- Replies: 7
- Views: 768
Re: Electron Affinity [ENDORSED]
So are elements with high electron affinity most likely to form anions?
- Sat Oct 27, 2018 1:11 pm
- Forum: DeBroglie Equation
- Topic: Nodal Planes
- Replies: 4
- Views: 534
Re: Nodal Planes
There aren't any electrons on these nodal planes correct?
- Mon Oct 15, 2018 9:33 pm
- Forum: Properties of Electrons
- Topic: Electrons in a stable state?
- Replies: 6
- Views: 607
Re: Electrons in a stable state?
So electrons in higher energy states contain higher potential energy, while electrons in lower energy states contain lower potential energy? Does this mean that electrons in higher energy states are more unstable than electrons in lower energy states? Yes, they are more unstable because the higher ...
- Mon Oct 15, 2018 8:20 pm
- Forum: Properties of Electrons
- Topic: Electrons in a stable state?
- Replies: 6
- Views: 607
Re: Electrons in a stable state?
So electrons in higher energy states contain higher potential energy, while electrons in lower energy states contain lower potential energy? Does this mean that electrons in higher energy states are more unstable than electrons in lower energy states?
- Mon Oct 15, 2018 8:17 pm
- Forum: Properties of Light
- Topic: Momentum of Photon
- Replies: 4
- Views: 385
Re: Momentum of Photon
What are some examples of particles or objects that don't have any momentum? Is that even possible?
- Mon Oct 15, 2018 8:13 pm
- Forum: Photoelectric Effect
- Topic: Photoelectric effect
- Replies: 5
- Views: 451
Re: Photoelectric effect
I have a question from Chapter 1 in the 6th edition of the textbook, regarding question 22. Why does the photoelectric effect best support the idea that electromagnetic radiation has the properties of particles?
- Mon Oct 08, 2018 9:20 pm
- Forum: Administrative Questions and Class Announcements
- Topic: DOWNLOAD SESSION WORKSHEETS HERE - Sundays 4-6pm (Karen) [ENDORSED]
- Replies: 135
- Views: 39231
Re: DOWNLOAD SESSION WORKSHEETS HERE - Sundays 4-6pm (Karen) [ENDORSED]
Thanks so much for this it was really helpful!
- Mon Oct 08, 2018 9:17 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Solutions Manual
- Replies: 9
- Views: 1869
Re: Solutions Manual
I find the solutions manual pretty helpful because sometimes it's easier to just see the work and understand what the question is trying to ask based off of that.
- Mon Oct 08, 2018 9:15 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Type of calculator
- Replies: 8
- Views: 1109
Re: Type of calculator
I'm using that calculator too! It should be fine since it's non-graphing and non-programmable.
- Thu Oct 04, 2018 3:18 pm
- Forum: Significant Figures
- Topic: Decimal point
- Replies: 14
- Views: 922
Re: Decimal point
Does that mean 120. has 3 sig figs and 120 has two sig figs?
- Thu Oct 04, 2018 3:13 pm
- Forum: Student Social/Study Group
- Topic: Homework Format
- Replies: 3
- Views: 411
Re: Homework Format
My TA said that writing the question is not necessary but you can always check with your TA to make sure.
- Wed Oct 03, 2018 4:49 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Registering/Creating Your Chemistry Community Account
- Replies: 40
- Views: 101020
Re: Registering/Creating Your Chemistry Community Account
For the Peer Learning Sessions, is there a link to sign up for spots or can you just drop in during the designated sessions?