CHEMISTRY COMMUNITY

ThomascnguyenDis1J

I believe so. Doing the homework problems helps a lot with knowing how to calculate pH or pOH for strong and weak bases and acids.

ThomascnguyenDis1J

Would using OH2 instead of H2O be wrong on a test? Is it not interchangable?

ThomascnguyenDis1J

I don't think so Cienna, but I would ask your TA first

ThomascnguyenDis1J

What does the term "coordination" refer to with the concept of "coordination number"

ThomascnguyenDis1J

What makes the weak acids/bases weak and the strong acids/bases strong?

ThomascnguyenDis1J

Can this idea be applied to identifying any compound?

ThomascnguyenDis1J

Thank you Michael, this really clarified the topic for me!!

ThomascnguyenDis1J

Are there any compounds that serve as exceptions to the formulas we've learned in class?

ThomascnguyenDis1J

When dealing with multiple compounds bonding to each other, what is the best way to determine its molecular shape?

ThomascnguyenDis1J

Will we ever be told to draw out the vsepr model for a molecule?

ThomascnguyenDis1J

I ran into this same problem and had a difficult time understanding what to do. I just don't understand why we cannot treat the two molecules the same way.

ThomascnguyenDis1J

Would we need to know the specific bond angles of each molecule?

ThomascnguyenDis1J

The formal charge must always equal to the charge of the entire molecule.

ThomascnguyenDis1J

An easy way to remember how to find formal charge is take the atom's valence electrons and subtract it with the number of dots and lines around it on the lewis structure

ThomascnguyenDis1J

I think there was a resonance structure question on the midterm but it did not specifically state to draw resonance so would one structure suffice?

ThomascnguyenDis1J

An exception to take note of when viewing trends on the periodic table is that of Nitrogen and Carbon. Due to Nitrogen's half sub shell, it has greater stability and doesn't need an electron as much as Carbon does so that means Nitrogen has a lower electron affinity than Carbon.

ThomascnguyenDis1J

Some exceptions include the ionization energy of Oxygen and Nitrogen. Nitrogen has a lower ionization energy than Oxygen because Nitrogen's half sub shell offers it more stability than Oxygen.

ThomascnguyenDis1J

Thank you so much for the review session! It really helped clarify so many topics for me.

ThomascnguyenDis1J

What is the relationship between the uncertainty of momentum and the uncertainty of wavelength?

ThomascnguyenDis1J

Would a 3p orbital have the same energy level as a 4p orbital? Would these two be considered degenerate?

ThomascnguyenDis1J

Removing an electron gives the atom a greater positive charge, converting it into a cation. This causes the remaining electrons to have a greater attraction to the nucleus.

ThomascnguyenDis1J

Just thinking conceptually, how does a wave function describe the characteristics of an electron?

ThomascnguyenDis1J

I believe it is possible to find the work function if given only the frequency of the photon, using the equation:

E=hv, which will then equal the work function to eject the electron.

ThomascnguyenDis1J

Rydberg formula can be used for other elements I believe, giving us a spectral line for any element. My question is, are those spectral lines of other elements than hydrogen visible to the human eye?

ThomascnguyenDis1J

Thank you, Catherine for the clarification. This really helped me picture the change of an electron's wavelength in my head and give me a greater understanding.

ThomascnguyenDis1J

Could the orbital angular momentum quantum number be simply described as the number of electrons on an atom's orbital shell? If not, could someone describe it in greater detail?

ThomascnguyenDis1J

I'm sorry, but could you clarify the difference between having something quantized rather than continuous.

ThomascnguyenDis1J

Will we only need to know the concept of it for this test? Or should we do practice problems to understand how to do it?

ThomascnguyenDis1J

Thank you Ania for the explanation. It really helped a lot. So would you say that if they ask you for any net equation and there is a reactant and product that does not change, they would just cancel each other out?

ThomascnguyenDis1J

In the textbook, it says that to predict how much product can be formed in a reaction, you can use the mole ratio for the reaction to relate the amount of a reactant consumed to the amount of molecules produced. Could someone clarify this for me?

CHEMISTRY COMMUNITY

Search found 30 matches

Re: Final Exam

Re: Water as a ligand

Re: OH2 vs H2O

Re: Coordination Number

Re: Weak and Strong Acids/Bases

Re: Identifying the acid and base

Re: Polarity

Exceptions to VSEPR

Re: 4.19 6th edition

Re: Naming the Shape

Re: 2 Lone Pairs, Placement

Re: Shapes Not covered in Lecture

Re: Formal Charge and the Octet Rule

Re: Formal Charge

Re: Resonance Structures on the Midterm

Re: Electron Affinity

Re: Periodic Trends

Re: MIDTERM PRACTICE - Garlic Bread Review Session [ENDORSED]

Uncertainty Equation

Re: Degeneracy

Re: Atomic Radius

Re: Schrodinger Equation

Re: Work Function

Re: Rydberg formula

Re: Energy Level Question

Re: energy transitions

Re: Electron Question

Re: Combustion Analysis? [ENDORSED]

Re: Fundamental M.9 [ENDORSED]

Mole-to-mole predictions [ENDORSED]