CHEMISTRY COMMUNITY

spark99

It would be square pyramidal

spark99

Acidity increases with the increase of electronegativity.

spark99

H2Se has a higher boiling point because it has a larger London dispersion force. You can figure this out because Se is larger than S, and the bigger the molecule, the bigger the dispersion force. The larger the intermolecular forces, the higher the boiling point will be.

spark99

Due to the high repulsive energy that lone pairs have, you have to think of the best possible place to put it so that the molecule is the most stable. Thus, when placing lone pairs, putting it in the equitorial position provides the most stability.

spark99

When there is a lone pair, the molecule has to be the in the best optimum position available so that the electrons are equally spread apart. So for example, when there is a lone pair in a AX3E2, the best optimum place for the lone pair is in the equitorial axes.

spark99

This is beacause an atom that has half-filled or full orbitals are more stable. For oxygen, its electron configuration is 1s2 2s2 2p4, and nitrogen's is 1s2 2s2 2p3. Nitrogen has half-filled 2p orbitals, so losing an electron would cause it to become more unstable. However, oxygen can become more st...

spark99

When an electron absorbs energy, it goes into an excited state. When it returns to its unexcited state, the electron loses energy by emitting it through light.

spark99

For seesaw, you have approximately 90,120, and 180 degrees. For T-shape, you would have 90 degrees and 180 degrees.

spark99

It should be 90 and 180 degree

spark99

The VSEPR model should be linear. As for the Lewis structure, you should have one of the iodine being a central atom with one bond to each iodine atom. The central atom has 3 lone pairs, and the other two iodine atoms also have 3 lone pairs.

spark99

Yes, bond length and bond strength usually have a correlation. The longer the bond, the weaker the bond; The shorter the bond, the stronger the bond.

spark99

It means that the VSEPR model can give you the quantitative shapes of the molecules like tetrahedral or trigonal planar or something. However, when there are lone pairs involved, the VSEPR model cannot give you an exact measurement of the bond angles due to the higher electron repulsion, thus it can...

spark99

Yeah, I don't you have to take molecular shapes into consideration when drawing Lewis Structures. However, I do think you should be able to recognize molecular shape when looking at a Lewis Structure from the electron density.

spark99

Hydrogen bonds have higher melting and boiling point because they have some of the highest intermolecular forces, so a large amount of energy is needed to separate them.

spark99

S^-2 is bigger because it has more electrons that is free to move around more.

spark99

I'm not 100% sure, but I think you would draw the shape of the p orbital, but would draw one on the x-axis, one on the y-axis, and one on the z-axis.

spark99

Can someone explain why we use [Ar] You can use Atomic radius to also tell ionization energy. The general trend for atomic radius is that it decreases from left to right across the period, which means the nucleus has a greater pull on the electrons, causing their radius to be smaller. So, ionizatio...

spark99

Ionization energy has a general trend that increases left to right across and decreases down a group. Ionization energy is the energy required to remove an electron from an atom, so to answer your question, yes.

spark99

Can someone explain to me the exception for copper and chromium? I heard it in the lecture, but I had trouble understanding it. Please clarify this for me.

spark99

Ionization energy is the energy required to remove the outermost bound electron. Ionization energy increases from left to right on the periodic table. Electron affinity is kind of like the opposite. It is the energy change that occurs when a neutral atom attracts an electron to become a negative ion...

spark99

One of the biggest reasons is that hydrogen bonds are intermolecular forces, which happens between two atoms in the same molecule. A hydrogen bond is merely an electromagnetic attraction, not really a bond.

spark99

Yeah I believe electron configuration won't be on test 2. Lavelle said the test will be on information up until Friday's lecture, and we haven't learned electron configuration yet.

spark99

First, you have to recognize that ultraviolet light is included in the Lyman series, which means its initial n is n=1. This can be found in your book. Then, you can use the Rydberg equation: v=R((1/n1^2)-(1/n2^2) Now that we now that its initial is n=1, you plug in 1 in n1. v=R((1/1^2)-(1/n2^2) In t...

spark99

The possible values are 0,1,2,3,4,5,6
The allowed values of L are 0,1,2,...,n-1.

spark99

I think it depends on your TA, but I heard in a lecture and Lavelle said that you can turn in hw from the fundamental chapter if you wish to review more. I did some of the fundamental problems in my hw for week 2 as well because I needed the practice for the test.

spark99

First, you convert 0.500 g of KCL, K2s, K3Po4 into moles. Then, you multiply the moles by the mole ratio between the moles of potassium and the compound. 0.500g KCl= .0067 mol *1 0.500g K2S= .0045 mol*2 0.500g K3PO4= .0023 mol*3 Then, you just add the results for the total amount of moles of potassi...

spark99

The photoelectric effect affects only metals, but yes to answer your question, it can affect everyday objects. Technically, it will lose mass, but it is of negligible quantity.

spark99

Can someone tell me how to do E9 (b)? I have 7th edition.

spark99

Yeah I think it's fine. I personally don't do it because it's more confusing for me.

spark99

yeah, I think you would have to state the state of the compound when doing chemical equations. Sometimes you can tell what state it's in by the context of the question. However, there are solubility rules you can memorize if you search them up online.

CHEMISTRY COMMUNITY

Search found 30 matches

Re: A X5 E

Re: Electronegativity & Acid Strength

Re: Review questions

Re: Trigonal Bipyramidal

Re: VSEPR (lone pairs taking axial vs equatorial positions)

Re: Ionization Energy

Re: excitation

Re: Seesaw and T-Shape

Re: bond angle

Re: Lewis and VSEPR for I3-

Re: Bond Length

Re: Repulsion Strength

Re: Effect of Molecular Shape on Lewis Structure

Re: H bonds and melting points

Re: Which Ion is larger?

Re: Drawing orbitals

Re: What are the trends useful for?

Re: Ionization Energies

Copper and Chromium Exception

Re: Ionization energy and electron affinity

Re: Hydrogen Bonds

Re: 2.43 Electron Configurations

Re: Prob 1.15 6th Ed.

Re: Homework Question 1.D13

Re: Homework for Week 2 [ENDORSED]

Re: G.21

Re: Photoelectric Effect

Formula Units

Re: Stoichiometric coefficients

Re: state of compounds