CHEMISTRY COMMUNITY

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not necessarily polarizability has more to do with the size of an electron cloud or the charge on a polarizing agent. when looking at two nonpolar molecules with only London Dispersion Forces CH4 and CCl4, the CCl4 would have a high er boiling point and therefore a stronger bond than CH4 because it ...

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there is a whole explanation in the book in topic 9C!! the book says the chlorine gets replaced with water so the hydrogens can form H bonds with the lone pair on nitrogen in Guanine but dr lavelle just said that the chlorine gets replaced by the nitrogen in guanine i dont think we will have to know...

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an orbital is hybridized to make everything more stable. when determining the correct hybridization for an atom, you include all the possible electron-dense regions (or bonding regions) which includes lone pairs.

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acid rain is a biological example of acids and bases. carbon dioxide reacts with water to form carbonic acid and hydronium which decreases the pH of the rain. this has many biological implications such as ocean acidification which is destroying ecosystems (especially with the large output of carbon ...

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the strength of an acid has to do with how weak the bonds are in comparison to other acids. usually, the main factor that determines this is shielding (because there is a larger electron cloud). i dont think resonance has as big of an impact on acid strength versus something like shielding

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It is different from polydentate because it forms a ring structure due to the fact that two parts of the ligand bind to one central atom

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ShravanPatel4G wrote:Are there any unbonded electron pairs on the central atom?

If yes, then this molecule can act as a Lewis Base

Is the valence shell of the central atom filled?

If not, then this molecule can act as a Lewis Acid

THANK YOU!

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Parker Smith wrote:Will we lose points on the Final if we use the Rydberg equation for potential atomic spectra problems?

what is the Rydberg equation again?

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I am having trouble identifying lewis acids and bases because they aren't like traditional bronstead acids and bases that are easier to pick out

Does anyone have any tips or examples?

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Which nomenclature should we use when naming coordination compounds?
ex.
Chlorine:
Chloro or Chlorido

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Why does CCl4 have a higher Boiling Point when CH4 has a shorter bond length?

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can someone explain the difference between chelating compounds and polydentate compounds?

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ligands can attach to a transition metal to form a Heme Complex. This then allows for an open binding site. In the example of myoglobin, the open binding site is used to transport oxygen (o2 binds to the transition metal that is bound to the ligand). but there are many more biological applications o...

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as long as dipoles (differences in electronegativity) cancel out symmetrically around the central atom, the molecule will be nonpolar

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induced dipole= van der waal's forces= london forces, right? not exactly all bonds have some sort of van der waal's forces/london forces however, induced dipole is when the charge/polarity of a polar molecule causes a nonpolar molecule to have an instantaneous dipole. van der waals/london forces ar...

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anything that has two boding regions (could be bonds or lone pairs) have an sp hybridization

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usually when given huge molecules like that the atoms are arranged in order of which they are writtem.

For example given CH2CHCN,

the order of the "backbone" of the lewis strucrure would be C-C-C-N and then add in the hydrogens

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He is also including Sigma and Pi bonds on the test which he is going over during Monday's lecture

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he is also going to test us on Pi and Sigma bonds which he is covering on monday.

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also what he covers about sigma and pi bonds on monday will be on the test

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i think they are just always equally distributed unless there is a lone pair

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If all atoms around the central atom are the same, equally distributed, and there are no lone pairs then it is nonpolar.

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The elctrons arent bound to another atom so there is more repulsion. Most likely there is no attraction from another atomn's protons.

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Water molecules use both hydrogens for hydrogen bonding.

But always remember, hydrogen bonding is always with the elements F, O, and N

F, O, and N always have to have a lone pair for there to be any hydrogen bonding

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Also, a trend that goes with it.

Atoms that are larger (and therefore have more electrons) are more Polarizable.

Atoms that are smaller (and have fewer electrons) have more Polarizing Power.

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Structures with a charge are more likely to contribute to a resonance hybrid because the electrons are delocalized in resonance hybrids.

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Michelle Xie 3A wrote:A lewis base would donate a pair of electrons and a lewis acid would accept a pair of electrons.

What is the acid/base name for the definition that says it donates/accepts protons? Is that a Bronsted acid/base?

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Yes, I believe it can be. Whatever we are doing in class is allowed for homework problems.

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Yes! You are correct. Polarizability increases as molecular mass increases because, as molar mass increases so does the number of electrons in an atom. The more electrons there are, the more polarizability an atom has.

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what is the difference between electronic transitions in atomic orbitals (atomic spectroscopy) and electronic transitions in molecular orbitals (molecular spectroscopy)?

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noble gasses are just, VERY special :)

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having an EMPTY d shell allows for an expanded octet because there is space for more electrons. In contrast, atoms without an empty d orbital cant form expanded octets because there are no shells for the electrons to go in

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a lot of them have different charges so usually, they will specify in the problem

like iron has a +2 +3 and +4 charge it just depends on the reaction

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it depends on how many empty d or p orbitals there are to determine how many times it can expand an octet.

I dont think it is only empty d orbitals because sulfur can become an expanded octet and it deosnt have an empty d orbital only a p orbital to "tap into"

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Work function is also known as threshold energy which is the amount of energy needed to remove an electron from a metal. So, it is similar to ionization energy but ionization energy is with elements in the gas ohase while this equation with work function is with metals

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They are also more reactive beacuse the electrons have so many possibilities of where they could be at one time. The fancy word for it is delocalization but it makes more sense to me by thinking of it as in we just dont know where they could be because there are multiple favorable structures

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As you move across a period, atoms have higher electron affinity because they want to fill their valence shell. For example, Lithium is less likely to gain an electron because they want to "get rid of" the one they already have in their 2s shell versus Fluorine that wants an electron to co...

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Phosphorus, Chloride, and Sulfur are all exceptions to the Octet Rule and can all, therefore, have an expanded octet.
This is because, they have that 2p orbital to "tap into" unlike elements such as Oxygen, Nitrogen, and Flouride.

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ionic bonds are stronger than covalent bonds

but, covalent network bonds are the strongest of all bonds and include compounds like diamond and graphite

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Electrons are delocalized when there is resonance in the structure of the molecule. Delocalization means the electron isn't bound to stay in one subshell, instead it can "move around" from subshell to subshell per se. That is why we draw all the possible structures when we draw resonance b...

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Their delocalized electrons also give them a lower activation energy which makes them more stable.

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what I always do in the back of my notebook is write down all the equations we learn because some aren't on the constants sheet!:)

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2 words...

KAHN. ACADEMY.

especially for equilibrium and acids and bases!!

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So, spin states depend on how many electrons you have in one orbital. for example, lets say we are dealing with the P orbital which has 3 basically domains (Px, Py, and Pz) each electron can be in. When adding electrons to a system, one must distribute each electron to Px Py and Pz BEFORE adding 2 e...

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Can someone please explain what Px, Py, Pz are and how they relate to -1,0,1? Px Py and Pz are the different parts of an orbital that an electron can occupy. the quantum number "m" refers to the specific electrons within an orbital shell. they are basically the same thing so -1,0,1 is the...

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To explain the symmetry aspect (I am confused about the density part as well), the s orbital has symmetry because it is in the shape of a sphere so any way you cut it/look at it, it will be the same meaning the electrons will be in that vicinity the p and d orbitals do not have symmetry because thei...

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Hi!

You can only do percent yield problems if they give you the experimental data so if they give it to you I would do it just in case.

Remember percent yield is,

100(actual yield/theoretical yield)= percent yield.

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Because we have to take tests in pen I do homework and notes in pen so I get used to working around mistakes. It also makes me do my work slower and more diligently since I don't want to mess up in pen

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KatherineValdez_4B wrote:So we can get partial credit if we show our work and we have the right idea, but mess up the calculations?

yes I remember my TA saying we get partial credit for calculations and showing work.

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There are also lots of calculators that have periodic tables inside and different chemistry programs with conversions.

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Hello! Constructive interference occurs when two different waves are acting IN phase and the result is more energy. Destructive interference occurs when two different waves are acting OUT OF phase and the result is less energy. Waves are in phase when their troughs and peaks match up and they are ou...

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covalent network are the strongest (ex. diamond and graphite) are stronger than ionic however covalent bonds themselves are usually weaker than ionic bonds.

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They would be the same thing! Only if the number in the ones place was a zero would you need a decimal to include it in your sig figs.

ex.
114 - 3 sig figs
110 - 2 sig figs
110. - 3 sig figs

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I love to tell chemistry jokes!! But I only get a reaction periodically...

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It is easiest to write your decimal number as a fraction so you can just divide by the denominator and make every coefficient and integer! I hope this helps.

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Hello! I usually round with the consideration of sig figs. So, when multiplying or dividing, you always round to the least specific place (ex. 10.0/1 would just have one sig fig because "1" is the least specific). I usually round according to sig figs during the entire problem so I get in ...

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