Search found 35 matches
- Tue Dec 04, 2018 1:55 pm
- Forum: Naming
- Topic: When to use -ate
- Replies: 1
- Views: 263
Re: When to use -ate
You use the suffix -ate at the end of the metal name when the entire complex has a negative charge. In this problem the complex has a 2- charge which explains the utilization of the suffix -ate.
- Mon Dec 03, 2018 9:50 pm
- Forum: Naming
- Topic: "(en)" and "(edta)"?
- Replies: 3
- Views: 391
Re: "(en)" and "(edta)"?
en= ethylenediamine
edta=Ethylenediaminetetraacetic acid
These are the abbreviated forms of these compounds when they are a ligand.
edta=Ethylenediaminetetraacetic acid
These are the abbreviated forms of these compounds when they are a ligand.
- Mon Dec 03, 2018 4:34 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: 6th Edition 17.37
- Replies: 2
- Views: 355
Re: 6th Edition 17.37
The coordination number for:
a) 4
b) 2
c) 6
d) 6
The coordination number for c would come from the fact that there are four bonds coming from (en) and two from cl
For d, there are six bonds which is implied through the name of the complex.
a) 4
b) 2
c) 6
d) 6
The coordination number for c would come from the fact that there are four bonds coming from (en) and two from cl
For d, there are six bonds which is implied through the name of the complex.
- Mon Dec 03, 2018 4:25 pm
- Forum: Conjugate Acids & Bases
- Topic: Neutral Ligands
- Replies: 1
- Views: 272
Neutral Ligands
In regards to neutral ligands, are we just expected to memorize which compounds are neutral or is there a way to determine if they are neutral?
- Mon Nov 26, 2018 9:16 pm
- Forum: Sigma & Pi Bonds
- Topic: 2F.17 7th ed: Pi bond
- Replies: 2
- Views: 378
Re: 2F.17 7th ed: Pi bond
When there is a single bond there is 1 sigma bond and 0 pi bonds. When there is a double bond, there is 1 sigma bond and 1 pi bond. When there is a triple bond, there is 1 sigma bond and 2 pi bonds. Hope this helps! :)
- Mon Nov 26, 2018 9:12 pm
- Forum: Hybridization
- Topic: Electron Density and Hybridization
- Replies: 1
- Views: 367
Re: Electron Density and Hybridization
Yes, regions of electron density do match up with the number of hybridized orbitals. For problem 2F.13, it asks for the hybrid orbitals of each carbon atom. So when you draw the lewis structure of CH2CHCN, there should be three regions of electron density around two of the three carbon atoms and two...
- Mon Nov 26, 2018 4:04 pm
- Forum: Bond Lengths & Energies
- Topic: Atom Size and Bond Strength
- Replies: 2
- Views: 416
Re: Atom Size and Bond Strength
A larger atom would result in a weaker bond because the nucleus of the atom doesn't have a strong hold of the outer most electrons. I believe when we refer to the size of the atom, we discuss its molecular mass, atomic number, and atomic radius interchangeably but when discussing bonding, I think at...
- Tue Nov 20, 2018 10:36 pm
- Forum: Polarisability of Anions, The Polarizing Power of Cations
- Topic: higher polarizability
- Replies: 4
- Views: 442
Re: higher polarizability
The smaller cation has higher polarizing power because of its electronegativity. Because of its small size and the fact that it wants electrons, the cation is able to hold onto electrons better. So overall, the smaller the atomic/ionic radius, the more polarizing power the atom/cation has. (charge a...
- Tue Nov 20, 2018 3:45 pm
- Forum: Hybridization
- Topic: Regions of electron density
- Replies: 6
- Views: 746
Re: Regions of electron density
I believe that is correct!
regions of electron density around the central atom= number of hybrid orbitals
regions of electron density around the central atom= number of hybrid orbitals
- Tue Nov 20, 2018 2:16 pm
- Forum: Electronegativity
- Topic: Electronegativity and Polarity
- Replies: 3
- Views: 462
Re: Electronegativity and Polarity
As electronegativity decreases, polarizability increases.
- Mon Nov 19, 2018 6:16 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bold/Dashed Lines in Bonds
- Replies: 4
- Views: 600
Re: Bold/Dashed Lines in Bonds
Hello, the bold and dashed lines within the lewis structure represent the 3D position of an atom within the molecule. When it is a bold line, that means that the atom is more towards the foreground. When it is a dashed line, that means that the atom is more towards the background. I believe you can ...
- Tue Nov 13, 2018 8:53 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Homework Focus 2A
- Replies: 3
- Views: 453
Re: Homework Focus 2A
If this problem is from the 7th edition textbook, the correct answer is [Ar]3d^10 because the question asks for the electron configuration of Cu+ not Cu^2+.
- Tue Nov 13, 2018 7:22 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Lowest Energy Lewis Structures
- Replies: 3
- Views: 406
Re: Lowest Energy Lewis Structures
I believe that it would be best to use the Lewis Structure with the lowest energy and with octet exceptions because it would give a more accurate representation of the shape of the molecule. If we were to ignore formal charges and octet exceptions, we might miss a crucial double bond that could help...
- Tue Nov 13, 2018 7:16 pm
- Forum: Octet Exceptions
- Topic: octet exceptions
- Replies: 2
- Views: 354
Re: octet exceptions
The first four elements also have octet exceptions where they do not obtain an octet of electrons. This is due to the fact that the first four elements are stable/feel complete with the amount of electrons they currently have. Another exception would consist of elements such as Boron and Aluminum wh...
- Tue Nov 13, 2018 2:19 pm
- Forum: Lewis Structures
- Topic: VSEPR Model
- Replies: 2
- Views: 348
Re: VSEPR Model
I believe you can determine whether a molecule is color or nonpolar based on its charge distribution. When you draw the lewis structure, if there is symmetric distribution of charge, then the molecule would be nonpolar. If you draw the lewis structure and there is an uneven distribution of charge, t...
- Thu Nov 08, 2018 3:22 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: Hydrogen Bonds vs. Ion-Dipole Bonds
- Replies: 5
- Views: 2596
Re: Hydrogen Bonds vs. Ion-Dipole Bonds
I believe the reason why Hydrogen Bonds are stronger than ion-dipole interactions is because Hydrogen bonds involve greater differences in electronegativity. This can then create a large electric dipole of positive and negative charges.
- Wed Nov 07, 2018 4:47 pm
- Forum: Octet Exceptions
- Topic: Resonance Structures
- Replies: 7
- Views: 839
Re: Resonance Structures
I know this is a pretty simple question but, how do we indicate resonance structures? Can we just draw the structures next to one another or is there a more formal indication? I think one way to indicate resonance structures is to draw out one lewis structure. Then from there see if 1. the structur...
- Wed Nov 07, 2018 4:36 pm
- Forum: Octet Exceptions
- Topic: List of octect exceptions
- Replies: 6
- Views: 674
Re: List of octect exceptions
I believe the exceptions we have learned so far consists of: 1. Electron deficiency- which is when there is less than an octet, therefore causing a fourth bond to be made. For example: BF3, since Boron is short one bond to complete its octet, it would seek out another F atom to form BF4-.This would ...
- Wed Nov 07, 2018 10:44 am
- Forum: Resonance Structures
- Topic: bond length
- Replies: 5
- Views: 641
Re: bond length
Bond lengths could be the same because of resonance. Resonance molecules do not have one true lewis structure, but rather a variety of structures. Because of this, the resonance lewis structure of a given molecule would be a hybrid of all the possible structures that could be created. This would mak...
- Fri Nov 02, 2018 6:37 pm
- Forum: Octet Exceptions
- Topic: Number of Unpaired Electrons
- Replies: 2
- Views: 474
Re: Number of Unpaired Electrons
Hello,
when you do the electron configuration diagram for 3d^8 three orbitals would be filled out of the five orbitals available. Two orbitals would have only one electron in them-making them unpaired.
https://www.adichemistry.com/jee/qb/coordination-chemistry/1/q1-3.png
when you do the electron configuration diagram for 3d^8 three orbitals would be filled out of the five orbitals available. Two orbitals would have only one electron in them-making them unpaired.
https://www.adichemistry.com/jee/qb/coordination-chemistry/1/q1-3.png
- Wed Oct 31, 2018 4:06 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Degeneracy
- Replies: 4
- Views: 778
Re: Degeneracy
Hello,
the S orbital is not degenerate because its l value= 0 therefore making the m1 value=0. This makes the s orbital have 0 degeneracy.
the S orbital is not degenerate because its l value= 0 therefore making the m1 value=0. This makes the s orbital have 0 degeneracy.
- Tue Oct 30, 2018 9:58 pm
- Forum: Lewis Structures
- Topic: central atoms
- Replies: 8
- Views: 791
Re: central atoms
Hello,
the central atom is usually the atom with the lowest ionization energy.
the central atom is usually the atom with the lowest ionization energy.
- Mon Oct 29, 2018 11:03 am
- Forum: Ionic & Covalent Bonds
- Topic: Midterm
- Replies: 2
- Views: 343
Re: Midterm
Hello,
this was posted on the Chem 14A website under announcements : Midterm covers: Fundamentals, Quantum, Bonding to end of 3.11 (6 Ed.) and to end of 2C (7 Ed.)
this was posted on the Chem 14A website under announcements : Midterm covers: Fundamentals, Quantum, Bonding to end of 3.11 (6 Ed.) and to end of 2C (7 Ed.)
- Wed Oct 24, 2018 4:26 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Ground vs Excited State
- Replies: 3
- Views: 423
Re: Ground vs Excited State
Hello,
this would be considered as an excited state because it does not follow Hund's Rule. The second electron should have filled in the next orbital rather than pairing up in the first one, if it followed this rule.
this would be considered as an excited state because it does not follow Hund's Rule. The second electron should have filled in the next orbital rather than pairing up in the first one, if it followed this rule.
- Tue Oct 23, 2018 8:30 pm
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: Exercise 1.45, 6th Edition
- Replies: 1
- Views: 201
Re: Exercise 1.45, 6th Edition
It looks like you're correct. Dr. Lavelle has 1.45 on his list of solution manual errors.
Here is the link:https://lavelle.chem.ucla.edu/wp-content/supporting-files/Chem14A/Solution_Manual_Errors_6Ed.pdf
Hope this helps!
Here is the link:https://lavelle.chem.ucla.edu/wp-content/supporting-files/Chem14A/Solution_Manual_Errors_6Ed.pdf
Hope this helps!
- Tue Oct 23, 2018 8:24 pm
- Forum: Photoelectric Effect
- Topic: Wavelength Calculation
- Replies: 2
- Views: 412
Re: Wavelength Calculation
Use the equation Energy= hc/(wavelength). Then use the energy of the photon you got from part b, which should be 2.25 x 10^-17J. Rearrange the equation so that you are solving for wavelength so it would be: wavelength= hc/energy Then plug in 6.626 x 10^-34 for h and 3.0 x 10^8 for c and divide by 2....
- Wed Oct 17, 2018 2:18 pm
- Forum: Einstein Equation
- Topic: 7th Edition 1B.15
- Replies: 3
- Views: 262
Re: 7th Edition 1B.15
For this problem use the equation: Energy= hc/(wavelength). Then use the energy of the photon you got from part b, which should be 2.25 x 10^-17J. Rearrange the equation so that you are solving for wavelength so it would be: wavelength= hc/energy Then plug in 6.626 x 10^-34 for h and 3.0 x 10^8 for ...
- Tue Oct 16, 2018 8:17 pm
- Forum: Properties of Light
- Topic: Wave-Like Properties Value
- Replies: 2
- Views: 200
Re: Wave-Like Properties Value
I believe Dr. Lavelle said that the cut off would be 10^-15 and anything smaller than that is undetectable.
- Tue Oct 16, 2018 5:02 pm
- Forum: Properties of Electrons
- Topic: electromagnetic radiation
- Replies: 3
- Views: 408
Re: electromagnetic radiation
The number of photons in a light beam affects the brightness of the whole beam, whereas the frequency of the light controls the energy of each individual photon. In the Photoelectric effect electrons are ejected from a metal surface based on the amount of energy absorbed. So, a certain threshold has...
- Wed Oct 10, 2018 11:03 am
- Forum: Photoelectric Effect
- Topic: Packets of Energy
- Replies: 2
- Views: 137
Re: Packets of Energy
Planck proposed the idea that light and other forms of electromagnetic waves were released in certain packets of energy. This became known as "Quanta" because quanta by definition, is a discrete amount of energy proportional between its magnitude and frequency. So, this is known as Planck'...
- Tue Oct 09, 2018 10:24 pm
- Forum: Limiting Reactant Calculations
- Topic: Percent Yield [ENDORSED]
- Replies: 13
- Views: 2894
Re: Percent Yield [ENDORSED]
So for a theoretical yield, it is the amount(grams) of product that you receive through calculations considering that the conditions of the experiment are perfect. One way to think about theoretical yield is the amount you calculated on paper. As for the actual yield, it is the amount(grams) of prod...
- Sun Oct 07, 2018 3:39 pm
- Forum: Significant Figures
- Topic: Rounding molar mass on the periodic table
- Replies: 3
- Views: 1778
Re: Rounding molar mass on the periodic table
For calculations, use the given molar mass on the periodic table without rounding. Round based on the amount of sig figs at the end of your calculation.
- Mon Oct 01, 2018 9:09 pm
- Forum: General Science Questions
- Topic: Periodic Table
- Replies: 16
- Views: 1664
Re: Periodic Table
Typically, it is best not to round the atomic weights of the elements before using it for calculations because your final answer would not be as accurate as it could be. Usually, you would round at the end of your calculation depending on the amount of significant figures there are. You determine th...
- Mon Oct 01, 2018 8:51 pm
- Forum: Accuracy, Precision, Mole, Other Definitions
- Topic: Question E.9: Epsom Salts
- Replies: 2
- Views: 413
Re: Question E.9: Epsom Salts
When given the name of the compound, I usually like to write out the symbols of the elements. So in the case of this problem, start off with Magnesium. Its symbol would be Mg and then move onto Sulfate. Since Sulfate is not on the periodic table, try utilizing a common ions chart where you will find...
- Sun Sep 30, 2018 1:36 pm
- Forum: Balancing Chemical Reactions
- Topic: Question H21 (6th Edition)
- Replies: 2
- Views: 317
Re: Question H21 (6th Edition)
(1) : Balance N first because it appears the less within the equation. 2C10H15N + O2 --> CO2 + H2O + CH4N2O (2): Balance H, there are 30 H on the left side and a total of 6 H on the right, leaving the (4 H) alone, that would be 30-4= 26/2= 13 as your coefficient for H2O 2C10H15N + O2 --> CO2 + 13H2O...