CHEMISTRY COMMUNITY

RichardValdez1L

Is ligand every bond connected to a metal? And if so, if we are asked to give the maximum number of places on the ligand that can bind simultaneously to a single metal center, what is that referring to?

RichardValdez1L

Like for example I3-, I'm confused whether this is linear or a trigonal bipyramidal

RichardValdez1L

How do we know when to ignore the lone pair electrons when naming the molecule? Because this can change a trigonal pyramidal to a trigonal planar correct?

RichardValdez1L

Are we going to have to know how to do these type of VSEPR problems for the final?

RichardValdez1L

Why does a lone pair of electrons push away bonds more than a typical atom. For example, "120 degrees" vs "less than 120 degrees"

RichardValdez1L

Does Bronsted just tell you whether the atom is a hydrogen donor or accepter while the lewis tells you whether the atom is an electron donor or accepter? Or is there more to it than that?

RichardValdez1L

So just to clarify, a dipole moment is when there is an angle between two atoms that is anything besides 180 degrees right? If not, can someone give me a conceptual understanding of it?

RichardValdez1L

If a non-polar molecule must contain zero electric dipole moments, does that mean that dipoles can exist as long as they cancel ? Or do they always have to just not exist? And does just having one dipole moment make it polar?

RichardValdez1L

If lewis bases donates electrons and lewis acids accepts electrons does that mean that there is always one base and one acid connected between a bond and the acid is always the one accepting electrons and the bases are always the ones donating?

RichardValdez1L

Why do acids lose hydrogen atoms more easily?

RichardValdez1L

If we have one acid and one base, do we have to do calculations to determine if the product is one or the other or do we just assume it is neutral?

RichardValdez1L

both 2 dimensional and 3 dimensional

RichardValdez1L

I just want to clarify and have this corrected if wrong, first we do the electron configuration diagram we learned for the midterm, then we fill in the valence electrons, all the pairs are considered an atomic orbital and all the single electrons are considered a hybrid orbital, the amount of hybrid...

RichardValdez1L

So it's to my understanding that the bond pairs have to be placed the furthest from each other, but I'm still confused on where exactly to place the lone pair? I remember hearing something about 90 degrees...

RichardValdez1L

What's the significance for the bonds to be as far from each other as possible? Like how is repulsion and electrons involved?

RichardValdez1L

Furthermore on the relationship of these two, lets take boron triflouride for example, three bonding pairs. When we draw the Lewis structure the bonds around 90 degrees away from each other, but if we draw the VSEPR structure they're closer to 120 degrees. Are we still correct if we choose to draw t...

RichardValdez1L

I am also overall confused on why these two topics focus on VALENCE electrons, is it because valence electrons are the only ones pertaining to bonding?

RichardValdez1L

So is it like a rule of thumb that every atom should be as far from the other in determining the molecular shape?

RichardValdez1L

To clarify, polarization is where a molecule may have a positive and negative charge with the atoms contained? If so, what is so important about this concept in regards to this class?

RichardValdez1L

Another iffy topic on the test for me was ionization energy, if the highest ionization trend points toward the top right, then what if we have an molecule such as BrB and PS2. Are we just supposed to guesstimate or is there a method?

RichardValdez1L

After the test last week, I realized I'm still not understanding energies and bond lengths. I get that as the more bonds are added the greater the strength and the shorter the length, but what if we are comparing two single bonds but one is a C-C and the other is a C-P. How would this differ? And wh...

RichardValdez1L

Is the reason 1 and 2 are polar is because the bonds are not opposite each other? Because it's to my understanding that 1 has the largest dipole moment because they bonds are the closest. Also, if anyone can give me a conceptual understanding of what a dipole moment is it would be much appreciated! ...

RichardValdez1L

Is the main purpose of a formal charge on an atom to display whether it draws in electrons such as (-) from the atom connected to it in a Lewis Dot Structure?

RichardValdez1L

So does the formal charge on a molecule such as (SO4)^-2 apply as the overall formal charge to the entire molecule even though it possibly could only be attached to one atom?

RichardValdez1L

Although we know the trend for electronegativity and "FONCl", are we supposed to have the other element's electronegativities memorized or is there a way to calculate it?

RichardValdez1L

Can a single Lewis structure contain an ionic and covalent bond?

RichardValdez1L

Is Boron the only atom that has an incomplete octet?

RichardValdez1L

Why is the expanded valence electron always applied to the central atom? Also do you have to even out the electrons if there are two central atoms or do you have to fill one of the shells completely first?

RichardValdez1L

Is a Lewis Dot structure strictly only for single elements where as Lewis Structure is for 2 or more?

RichardValdez1L

Is one single bond larger than a two double bonds? or three triple bonds? is there any way to calculate this or is this just general knowledge?

RichardValdez1L

I have a hunch its because of its number of electrons but can't quite understand why? Is it because it can't form more than a single bond ?

RichardValdez1L

Is it possible to have 3-4 central atoms if the element has the lowest ionization energy of all?

RichardValdez1L

What are nonpolar covalent bonds and how are they significant in solving a lewis structure?

RichardValdez1L

What is the conceptual difference between a Lewis Structure and a Resonance Structure?

RichardValdez1L

When these numbers are linked towards a bond, it represents the bond length ? And if so, why is it necessary to know the bond length?
Also can we solve for this?

RichardValdez1L

Oh nevermind I figured it out!

RichardValdez1L

I may be wrong, but the trend towards the lowest ionization energy goes from from left to right and from bottom to top ? Or does it just go horizontally to the right?

RichardValdez1L

Do the metals such as lithium, beryllium, sodium and manganese try to gain electrons or lose electrons, since it's technically closer to the noble gases before it?

RichardValdez1L

Can someone please explain the difference between these two?

RichardValdez1L

Is only movements from extremely small sized mass noticeable? Like NEVER cars or balls?

RichardValdez1L

Can 1/2mv^2 and mv be used for the same problem if we're only given kinetic energy or power? Like If we are given power, can we solve for kinetic energy?

RichardValdez1L

Is the work function interhchangeable with power?

RichardValdez1L

For the Rydberg Constant are we supposed to be using 3.29 x 10^15 Hz, or 1.09 x 10^7 m^-1. An explanation would be much appreciated!

RichardValdez1L

What is an incident line and why for the second part of c. we use the E=hv equation?

RichardValdez1L

I have trouble putting together the pieces to comprehending these statements, can someone clarify how they would go about solving this equation? Increasing the brightness of incoming light increases the number of ejected electrons. Increasing the frequency of incoming light can increase the number o...

RichardValdez1L

Perfect response!

RichardValdez1L

I've seen E=hf around and I just wanted to confirm they're the same, and if they're not can someone explain the difference?

RichardValdez1L

If we were asked to solve for the wavelength of light emitted from electrons from lets say a carbon atom, how would we approach the problem since it's no longer a hydrogen atom?

RichardValdez1L

Since the Rydberg formula can solve for either 1/lambda or the delta E (change in energy), does that mean that they are interchangeable in this sense ?

RichardValdez1L

Are we expected to know the electromagnetic spectrum come test time ? like where one series starts and another ends ?

RichardValdez1L

Are we just supposed to understand that electrons and photons act sometimes as waves and sometimes as particles because when using two beams the particles do not collide and the interference patterns for waves? Any clarification would be much appreciated ! :)

RichardValdez1L

Are we just supposed to understand that electrons and photons act sometimes as waves and sometimes as particles because when using two beams the particles do not collide and the interference patterns for waves? Any clarification would be much appreciated ! :)

RichardValdez1L

Do our units for wavelengths have to be meters or are they supposed to align with the units given in the problem?

RichardValdez1L

Does anyone know if our review of chemical and physical principles of chemistry will be needed going forward in the class? And if so, will it be significant?

RichardValdez1L

Must all subscripts be whole numbers ? and if so if we get one that is like 33/2, would just multiplying all other ones and simplifying get us our answer?

RichardValdez1L

If given the elements carbon nitrogen hydrogen and oxygen, how are we supposed to organize (such as CHON or HCNO) them into an empirical/molecular and why?

RichardValdez1L

Similar to the end of the test from last week, to determine the molecular formula we count all of the elements and for the empirical formula we ALWAYS simplify when possible ?

RichardValdez1L

So to clarify the Balmer series consists of all the visible colors we can see such as green, blue, and red?

RichardValdez1L

My TA said always use three sig figs for tests but said she doesn't dock points for it on homework.

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