CHEMISTRY COMMUNITY

amogha_koka3I

Does a higher oxidizing power (more power to oxidize another atom) also mean its most likely to gain electrons/become reduced?

amogha_koka3I

These are for the integrated rate laws correct?

amogha_koka3I

It is also similar to the van't hoff equation which I think is given, so you can remember it that way.

amogha_koka3I

Will we be required to know how to derive half-life equations for each order of reaction

amogha_koka3I

^the resources are helpful, but I don't think we will be required to know exactly how to derive using calculus since it wasn't a prereq for this class, just as long you understand the concepts behind it

amogha_koka3I

I don't have 7th edition for the textbook, do you think you could specify which problem you are talking about?

amogha_koka3I

This corresponds with the equation delta G=-nFE because if the cell potential is positive then delta G is negative which makes it spontaneous, and if cell potential is negative, delta G is positive making the reaction non-spontaneous.

amogha_koka3I

Which equation are you talking about? For example, if you are talking about n in the delta G=-nFE, then n is the number of electrons.

amogha_koka3I

For balancing half reactions in both acidic and basic solutions, first balance the elements that are not Hydrogen or Oxygen. Then balance the O atoms by adding H20. For the next step: in acidic solution, balance H by using H+. But In basic solution, balance H by using H20 to the side of each half re...

amogha_koka3I

Can spontaneity be determined by solely looking at the cell potential value?

amogha_koka3I

There is also an equation that consists of delta G and delta G naught together and are distinguished through the reaction quotient Q?

amogha_koka3I

Do the two vertical lines in the notation represent the salt bridge?

amogha_koka3I

So the lowest level of degeneracy we will encounter is 1?

amogha_koka3I

On the class website he said "Test 2 covers all topics on Gibbs free energy and electrochemistry up to the Nernst equation."

amogha_koka3I

Do we assume isothermal, reversible, and at equilibrium are all synonymous in this class?

amogha_koka3I

Are entropy and enthalpy directly proportional?

amogha_koka3I

So we look only at gas moles and not at the changes in the other phase moles?

amogha_koka3I

I think the best way to look at it is what units you want the answer to be in. If you need the answer in joules, it's best to use 8.314 and make sure to convert all the factor in the equation to joules. For example the conversion factor between atm.L to J is 101.325.

amogha_koka3I

Will we get the same answer even if we do the long method of all breaking all the reactant bonds and forming all the product bonds?

amogha_koka3I

Is insulation and the lack of it also a good indicator of the type of system it is?

amogha_koka3I

So when there's an increase in enthalpy, heat was added to the system and vice versa?

amogha_koka3I

If you still need some practice or clarification, I find it helpful to watch videos online like Khan Academy.

amogha_koka3I

The videos he posts with them are very similar to the lectures in class too so if you forget to write something down or miss something, those videos are very helpful.

amogha_koka3I

I believe Professor Lavelle told us that most equations and constants we need to know will be given in the equation sheet we are provided with for every test.

amogha_koka3I

I also believe it is significant because when solving weak base/weak acid problems, you can convert from Ka to Kb using the Kw constant = [H3O+][OH-] = 1.0 x 10^-14

amogha_koka3I

I believe to get Ka you need to do 10^(-pka). Once you get the value for Ka, you divide 14 (KW) by the Ka in order to get Kb. If this is giving you the wrong answer you can also try this: 14-pka=pkb. Then do 10^(-pkb) in order to get the Kb value. Essentially both ways should get you the same answer...

amogha_koka3I

I had a similar question and found a post on chemistry community for it:
viewtopic.php?t=8560
Hope it helps!

amogha_koka3I

Should we specify Qc And Qp just like we differentiate between Kc and Kp?

amogha_koka3I

Are solids and liquids not included in calculating Kc AND Kp or just Kc?

amogha_koka3I

Is it the same case for liquids as it is for solids?

amogha_koka3I

Can someone also explain why we right H2O as OH2 in the drawings?

amogha_koka3I

So molecules that have hydrogen bonding also have dipole-dipole and ldf as well?

amogha_koka3I

So just to confirm, does polarity have anything to do with if there are single, double, or triple bonds?

amogha_koka3I

The notes in the past lecture said that stronger acids have higher Ka values.

amogha_koka3I

Does anyone know what the above sections correspond to in the 7th edition.

amogha_koka3I

An example is [Fe(CN)₆]4−. The oxidation state of the compound is 4- and the number for CN is -1 for 6 molecules so it is -6. You then subtract -6 from -4 to get the +2 oxidation number for Fe.

amogha_koka3I

I think the patterns for such molecules would follow that of SO3, but I would search for exceptions just in case so you don't make generalizations.

amogha_koka3I

Which edition are you looking at? I'm think this information is in the textbook for edition 6.

amogha_koka3I

So does identifying molecular shape include knowing how to identify electron density shape as well?

amogha_koka3I

Don't forget to account for the plus charge on the molecule as well.

amogha_koka3I

So regardless of the molecule being ionic or covalent, it has LDF?

amogha_koka3I

For the people whose discussions are cancelled Thursday and Friday, can we attend any discussions Monday-Wednesday?

amogha_koka3I

So is this an easy way to look at it: electron geometry/arrangement takes into account lone pairs of the central atom whereas molecular shape simply considers the shared bonds?

amogha_koka3I

So just to confirm there is no more than one sigma bond in any bond/atom interaction?

amogha_koka3I

So hydrogen bonds consist of three different intermolecular forces: hydrogen bond, dipole-dipole, and london?

amogha_koka3I

I think the other names were London, Dispersion and Van Der Waals.
Hope this helps!

amogha_koka3I

It has to do with the electronegativity difference between atoms. Molecules with atoms of same electronegativity have no dipole movement whereas a molecule such as HF has dipole movement due the electronegativity difference.

amogha_koka3I

As said above it's best to review the trend of atomic radius first. Then review which element is the cation and which one is the anion, based on that you can figure out if the atom increased or decreased in size.

amogha_koka3I

Diagonal relationships also exist within other trends and certain pairs of elements I think.

amogha_koka3I

The transition metals don't have a traditional method to identify valence electrons like the other groups, but I don't think we have gone over in class how to determine how many valence electrons each transition metal has.

amogha_koka3I

So in these cases, I believe a completely full or half full d sub-level is more stable than a partially filled level. So an electron from the 4s orbital is 'excited' and rises to a 3d orbital. For example for copper it goes from 3d9 to 3d10 and the s orbital goes from 4s2 to 4s1. Hope that helps!

amogha_koka3I

Because the question says it is the emission of energy, meaning the release of energy we can assume the initial energy level is n=3 and the final is n=1 because energy is released when an electron falls from a higher energy level to a lower.

amogha_koka3I

I believe C is true because when frequency decreases, the wavelength increases (it sort of drags out the wave). This in turn decreases the slope of the wave which correlates to the extent of change in the electrical field. Hope this helps!

amogha_koka3I

Will we be required to know how to derive De Broglie's Equation?

amogha_koka3I

Hey! So this question was actually discussed in chemistry community before so I'm posting the link below, hope it helps! https://lavelle.chem.ucla.edu/forum/viewtopic.php?t=5786 In short, you know n1=2 because it is a Balmer series and n2=7 by counting. Use the equation E = -hR/n^2 you can find the ...

amogha_koka3I

So you can use 1.097 x 10^7 as the Rydberg constant but when using it, you have to use a different Rydberg equation. So it might be easier to stick with the constant and equation we were given in class.

amogha_koka3I

It is negative because the electron's energy has decreased and the energy is released as electromagnetic radiation, hope this helps!

amogha_koka3I

I am also confused on this topic. In the HW problem 11 for chapter 1, we are asked to compare two figures and their spectral lines. I'm not sure where to start with this question and what exactly is common to their lines?

amogha_koka3I

When answering questions about wavelengths, is it best to write the units as meters or nanometers?

amogha_koka3I

Yes, you're right! It is based on the ratio of atoms in each molecule, you find how many moles of K there are in each of the three molecules and then add them up to get the total amount of moles of K.
Hope this helps!

amogha_koka3I

On fundamental M question 9a edition 6, we are asked to write a net ionic equation. Is this going to be on our first test?

amogha_koka3I

We multiply 144 by 2 because 144pm is the radius and we want the diameter of the atom.

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