CHEMISTRY COMMUNITY

salvadoralvizo1J

Which is stronger/harder to break: sigma or pi bonds?

salvadoralvizo1J

How many sigma and pi bonds are present in a molecule with 4 bonds??

salvadoralvizo1J

No, he will probably provide us with one on the exam if we even need one. It's important to know the general trend is anything and that Fl is the most electronegative atom.

salvadoralvizo1J

We're not expected to know the MO theory right? i know he mentioned it briefly in class...

salvadoralvizo1J

Whatt exactly do you mean by split? i know that strong acids tend to disassociate in water completely.

salvadoralvizo1J

This has to do with cis and trans configuration. If the dipole bonds are on the same side of the molecule [cis], then its polar. If the bonds are on opposite sides of the molecule [trans] , it's nonpolar because they cancel!

salvadoralvizo1J

Yes, since iodine is beyond the 3p orbital it can and will form an expanded octet.

salvadoralvizo1J

I had the same question last week. The order doesn't matter, but I believe writing the d at the end is preferred.

salvadoralvizo1J

My TA said they will be as specific a possible on those types of questions. You can probably just write bent unless otherwise specified.

salvadoralvizo1J

Yes, it is the same thing and I had the same confusion.

salvadoralvizo1J

Yes, we are expected o know significant digits since the midterm.

salvadoralvizo1J

It is also basically the same as a bond number.

salvadoralvizo1J

One of the ways acid rain is harmful is due to its higher acidity. Its lower pH values would greatly harm the pH levels of marine life as well as terrestrial soil, causing lots of damage.

salvadoralvizo1J

Yeah, its one of the learning objectives.

salvadoralvizo1J

Because it completely dissasociates in water.

salvadoralvizo1J

A proton walks into a bar. He's visibly depressed and disheveled. "Why the long face?" the bartender asks. The proton sighs. "I found out my wife has been unfaithful," he replies. "How do know?" asks the bartender. "Well, you see, I've always been faithful to my wi...

salvadoralvizo1J

On question 4.13 D, shouldn't the middle N have one lone pair because this has the lowest formal charge? Then why do the Ns have double or triple bonds?

salvadoralvizo1J

Lewis structure simply gives us the basics of valence electrons, ie how many pairs there are, how many single double or triple bonds, how many electrons in general. VSEPR actually tells you the angle of the shapes in a 3-D perspective. All electrons wish to be as far away from each other as possible...

salvadoralvizo1J

There is an expanded orbital due to the fact that elements on this horizontal group have access to an extra ten orbitals that are other wise used up on other groups.

salvadoralvizo1J

P would have one lone pair due to the fact that this has a formal charge of 0. It would also affect VSEPR shape, as it lone pairs have lower pull. Think of the example in class when he pulled the little ball and only the stick was sticking out.

salvadoralvizo1J

Atoms that fall on the 3P orbital would have a higher tendency to form double and triple bonds due to the fact that these atoms are the exceptions to the octet rule, and may be able to hold up to an extra 20 electrons.

salvadoralvizo1J

If having a formal charge of 0 means that an atom is most stable, then why do atoms like chlorine tend to have a negative charge when isolated (ie Cl-)?

salvadoralvizo1J

Elements on the third row on the p-orbital have higher energy than 3-D electrons. Since third row electrons don't have any electrons on the 3D orbital, valence electrons can fill in the empty row.

salvadoralvizo1J

What is the specific equation for finding the energy of mass for this one problem why do we have to multiply the energy of the the sodium light with the moles and avogrado"s number?

salvadoralvizo1J

How many configuration exceptions are we supposed to memorize on top of Chromium and Copper? Also, is it true that all exceptions to the rule are below Cr and Cu on the periodic table?

salvadoralvizo1J

Are we expected to know orientations and descriptions of the "P sub x/y/z" orbitals beyond the fact that their lobes are oriented along their respective axes?

salvadoralvizo1J

Is there any particular reason as to why orbitals are named the way they are, or where these letters chosen at random?

salvadoralvizo1J

Since there is only one electron in a typical Hydrogen atom, it would interact with the nucleus at a constant rate.

salvadoralvizo1J

I believe its UV light.

CHEMISTRY COMMUNITY

Search found 29 matches

pi and sigma bonds

four bonds

Re: electronegativity chart

final [ENDORSED]

Re: Acids and Bases

Re: Chapter 4 [ENDORSED]

Re: Help on HW#4.9 [ENDORSED]

Re: sp^3d or dsp^3

Re: Final [ENDORSED]

Re: Bent/angular [ENDORSED]

Re: Sig Figs for Final

Re: Coordination number [ENDORSED]

Re: ACID RAIN

Re: pH

Re: Strong Acid

Re: Post All Chemistry Jokes Here

4.13 D

Re: VSEPR confusion

Re: Expanded Octet

Re: PF3 molecular geometry

Re: Lewis Structure [ENDORSED]

Re: Formal charge purpose

Re: Concept of Exceptions

Question 1.25b

Electron Configuration Exceptions

Question 2.13

Re: Why does 4s fill up before 3d?

Re: Orbital shell in Hydrogen

Re: Lyman Series