Search found 30 matches
- Sun Jun 10, 2018 9:24 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: ethylenediaminetetraacetato (edta)
- Replies: 6
- Views: 1413
Re: ethylenediaminetetraacetato (edta)
edta is very important for one thing because it is the most common hexadentate ligand, meaning it can bind to a central metal atom in up to 6 locations.
- Sun Jun 10, 2018 4:58 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Ligands to Memorize for the Final
- Replies: 2
- Views: 458
Re: Ligands to Memorize for the Final
I created a quizlet that might help people with studying the ligands listed on page 742. https://quizlet.com/_4zgr1g
- Sun Jun 10, 2018 4:52 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: 17.29
- Replies: 2
- Views: 384
Re: 17.29
A good way to think when calculating oxidation number for a complex is to consider all the bonding between the central metal atom and the ligands to be 100% ionic, so when finding the charge on a ligand, consider the ligand separate. For 12.29, this would mean considering each CN- to have a charge o...
- Sun Jun 10, 2018 4:39 pm
- Forum: Sigma & Pi Bonds
- Topic: Pi bonds
- Replies: 3
- Views: 1919
Re: Pi bonds
Hi sylvie,
I know that a pi bond could also occur as a result of an overlap between orbitals that includes a hybridized orbital such as sp2 or sp3.
I know that a pi bond could also occur as a result of an overlap between orbitals that includes a hybridized orbital such as sp2 or sp3.
- Sun Jun 10, 2018 4:30 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Chelating complex
- Replies: 7
- Views: 682
Re: Chelating complex
The minimum number of ligands needed in order to form a chelating complex is 1, an important note: only polydentate ligands can form complexes.
- Sun Jun 10, 2018 3:48 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: ethylenediaminetetraacetato (edta)
- Replies: 6
- Views: 1413
Re: ethylenediaminetetraacetato (edta)
Hi Noah, A double bond is made of a sigma bond and a pi bond. Because of the pi bond, any atom with a double bond cannot rotate or bend--it is fixed so to say. This inability of the atom to reach toward the central metal atom prevents it from binding. So, the two oxygens in EDTA that have double bon...
- Sat Jun 09, 2018 1:25 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Determining Exact Bond Angle [ENDORSED]
- Replies: 2
- Views: 477
Determining Exact Bond Angle [ENDORSED]
Hi all, when determining the bond angle for a molecule that has, say, the VSEPR formula AX2E, meaning it has a bent shape with one lone electron pair, do we need to know the exact bond angle or is it enough to know that the bond angle will be less than 120 degrees because of the extra repelling forc...
- Sat Jun 09, 2018 1:21 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bent vs. Angular
- Replies: 11
- Views: 1144
Re: Bent vs. Angular
Along these same lines, would it still be acceptable to say trigonal planar bent?
- Sat Jun 09, 2018 1:16 am
- Forum: Formal Charge and Oxidation Numbers
- Topic: Perchlorate (ClO4)-
- Replies: 7
- Views: 12427
Re: Perchlorate (ClO4)-
A good general rule when calculating formal charge: make the formal charge on the central atom as close as possible to 0. Also, oxygen is more electronegative than cl so it makes sense for cl to have the additional electron.
- Sat Jun 09, 2018 1:09 am
- Forum: Photoelectric Effect
- Topic: Visible or measurable light
- Replies: 4
- Views: 448
Re: Visible or measurable light
One of the most important things to remember for the visual spectrum that may show up on a test is that blue/violet have the lowest wavelength (close to 400nm) while red has the largest (around 700nm), which means blue light has higher energy than red light.
- Sat Jun 09, 2018 12:55 am
- Forum: Dipole Moments
- Topic: Why can't SO2 form Hydrogen bonds?
- Replies: 3
- Views: 2497
Re: Why can't SO2 form Hydrogen bonds?
I think this question is asking what intermolecular forces would arise between two SO2 molecules, given that there is no hydrogen in SO2, there would be no hydrogen bonding between two molecules of sulfur dioxide, which is why hydrogen bonding is not an answer. However, because SO2 does have oxygen ...
- Fri Jun 08, 2018 11:46 pm
- Forum: Dipole Moments
- Topic: Are London dispersion forces present in every molecule?
- Replies: 2
- Views: 464
Re: Are London dispersion forces present in every molecule?
London dispersion forces exist between any two molecules provided that they are close enough together! They are a result of the electrons in one molecule attracting to the positively charged nuclei of another molecule (This means they are present in both polar and non polar molecules). These dispers...
- Fri Jun 08, 2018 11:39 pm
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: Lyman, Balmer, Paschen, Brackett. etc. series and Wavelength
- Replies: 3
- Views: 668
Re: Lyman, Balmer, Paschen, Brackett. etc. series and Wavelength
The most definite way to assign a light wave to either the lyman or balman series is to look at the energy level change. If the spectral line emitted is a result of the energy level dropping from n≥2 to n=1 then it is a part of the Lyman series If the spectral line emitted is a result of the energy ...
- Sun Jun 03, 2018 9:24 pm
- Forum: Hybridization
- Topic: Clarification
- Replies: 4
- Views: 586
Re: Clarification
Hi, If you could point out specific questions that relate to what your question is talking about that would help, but from my understanding this would mean to look at different types of molecules and how hybridization allows them to be formed ie CH4 is possible because Carbon has the 2SP3 hybridizat...
- Sun Jun 03, 2018 9:16 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: polar and nonpolar molecules
- Replies: 5
- Views: 678
Re: polar and nonpolar molecules
A CH2CL2 molecule is tetrahedral because there are four regions of electron density (VSEPR Model Formula of AX4). The C-H and C-Cl bonds are both polar in nature and looking at a tetrahedral shape, no bonds are opposite eachother and hence no bonds will cancel, causing the molecule to be polar.
- Sun Jun 03, 2018 8:59 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: hw 4.21 a
- Replies: 2
- Views: 350
Re: hw 4.21 a
The shape is called Trigonal Planar because there are two center atoms, each with 3 regions of electron density. The Shape of the molecule is thus more accurately two trigonal planar shapes.
- Sat Jun 02, 2018 1:37 am
- Forum: Hybridization
- Topic: identifying hybridized v unhybridized
- Replies: 1
- Views: 1096
Re: identifying hybridized v unhybridized
If you draw the Lewis structure of a molecule or formula unit then you can find the number of bonds that are responsible for the creation of the compound. Look at the number of unpaired electrons for the center atom in its ground state, ie Carbon's 2Px and 2Py orbitals have unpaired electrons. If th...
- Sat Jun 02, 2018 1:24 am
- Forum: Hybridization
- Topic: Sigma and Pi bonds and its relation to atomic orbitals.
- Replies: 1
- Views: 318
Re: Sigma and Pi bonds and its relation to atomic orbitals.
Sigma and Pi bonds are related to atomic orbital, but I'm not sure it's how you're thinking about it. I'll relate my understanding of sigma and pi bonds. Thinking about the bond between nitrogen and nitrogen in N2, the 2 Nitrogen atoms are bound by a triple bond, with both Nitrogens having 2Px, 2Py,...
- Wed May 30, 2018 11:13 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: How to know what position lone pair electrons will be at?
- Replies: 1
- Views: 289
How to know what position lone pair electrons will be at?
Specifically, I'm a bit confused about why a molecule with the VSEPR Formula AX3E2 would be T-Shaped rather than Trigonal Planar. I'm confused because my understanding was that lone pairs in a molecule tend to be as far apart as possible, and so the two lone pairs would be on opposite sides of the a...
- Wed May 23, 2018 9:58 am
- Forum: Formal Charge and Oxidation Numbers
- Topic: Prioritizing Formal Charge
- Replies: 2
- Views: 450
Prioritizing Formal Charge
Is it best to minimize the formal charge of the center atom or one of the atoms attached to the center atom in order to write the Lewis structure of the overall lowest energy species?
- Wed May 23, 2018 9:52 am
- Forum: Octet Exceptions
- Topic: Maximum number of electrons in expanded octet
- Replies: 1
- Views: 391
Maximum number of electrons in expanded octet
Hi all,
For an expanded octet, is there a limit to the number of valence electrons in the valence shells? Thanks.
For an expanded octet, is there a limit to the number of valence electrons in the valence shells? Thanks.
- Tue May 22, 2018 8:32 pm
- Forum: Ionic & Covalent Bonds
- Topic: Lewis Structures for Covalent Bonds
- Replies: 1
- Views: 349
Lewis Structures for Covalent Bonds
When drawing the lewis structure for (NH4)2CO3, the structure is written as 3 bracketed ions whereas the lewis structures for CH3COOH and (NH2)2CO are written without brackets, why is this?
- Mon May 21, 2018 11:15 pm
- Forum: Lewis Structures
- Topic: Question about Resonance Structures
- Replies: 1
- Views: 345
Question about Resonance Structures
I understand that resonance structures are lewis structures that are all correct for a molecule, why is it important to know all correct resonance structures?
- Sun Apr 15, 2018 10:46 pm
- Forum: Properties of Light
- Topic: What does it mean for all lines in a series to have the same lower energy level?
- Replies: 3
- Views: 313
What does it mean for all lines in a series to have the same lower energy level?
I understand that for all lines in say the Lyman series, all the lines created have the same lower energy level in common. Does this mean that if the given lower energy level that all the spectrum lines of a series have in common lower energy level n=2 and possible higher energy level of n=4,5,6.. t...
- Sun Apr 15, 2018 10:09 pm
- Forum: Properties of Light
- Topic: The Electromagnetic spectrum
- Replies: 5
- Views: 477
Re: The Electromagnetic spectrum
I don't think that memorization, in terms of the exact range of wavelength for every type of electromagnetic radiation, will be needed. However, It will be good to know things like: red visible light has a longer wavelength than blue and violet visible light, ultraviolet light, x rays and gamma rays...
- Sun Apr 15, 2018 9:20 pm
- Forum: *Black Body Radiation
- Topic: Example 1.3 in the textbook
- Replies: 3
- Views: 660
Re: Example 1.3 in the textbook
I think there will be some concept based questions on stefan boltzmann law, at the very least. For the second part of your question, T^4 because it was found that the intensity is not simply directly proportional to T, but it is proportional to T^4 (the temperature to the 4th power). The unit used f...
- Sun Apr 15, 2018 8:53 pm
- Forum: Photoelectric Effect
- Topic: Kinetic Energy [ENDORSED]
- Replies: 2
- Views: 360
Re: Kinetic Energy [ENDORSED]
Is the concept of kinetic energy is the excess energy after a light hits a metal surface and the energy required to eject electron(s) using the light (photons) is more than needed? The kinetic energy of the ejected electron is equal to the energy of the photon - the threshold energy (also known as t...
- Sun Apr 15, 2018 8:45 pm
- Forum: Properties of Light
- Topic: Bright Lines and the Atomic Spectra
- Replies: 2
- Views: 245
Bright Lines and the Atomic Spectra
In the textbook, it is stated that "the brightest line (at 656nm) is red" when light is emitted by excited hydrogen atoms and passed through a prism. Does this mean that other light is emitted but red is the brightest because when the excited hydrogen atoms give off em radiation, 656nm em ...
- Tue Apr 10, 2018 10:14 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: Fundamentals G21
- Replies: 1
- Views: 276
Re: Fundamentals G21
Because the objective of this question is to find the concentration of potassium ions, we need to find how many moles of potassium are in the solution. For every mole of K2S there will be 2 moles of K, so you can multiply the number of moles K2S by 2 to find the number of moles of K in the solution ...
- Sun Apr 08, 2018 11:01 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: G.23 from HW [ENDORSED]
- Replies: 4
- Views: 834
Re: G.23 from HW [ENDORSED]
For this problem, I approached it by thinking that for NaCl, the proportion of Cl ions to NaCl formula units is 1:1, and the proportion of Cl atoms to KCl formula units is also 1:1. Therefore, the concentration of Cl ions in the solution will be the same as the concentration calculated by converting...