CHEMISTRY COMMUNITY

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This video should help answer your question: https://www.youtube.com/watch?v=NNXvokAcSuE

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A molecule is said to have resonance when its structure cannot be adequately described by a single Lewis structure. Since a weaker base has a stronger conjugate acid, a compound whose conjugate base enjoys resonance stabilization will be more acidic.

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pH decreases with increase in temperature. But this does not mean that water becomes more acidic at higher temperatures. In the case of pure water, there are always the same concentration of hydrogen ions and hydroxide ions and hence, the water is still neutral (even if its pH changes)

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A conjugate acid is formed by a proton (H+). A conjugate base is what is left over after an acid has donated a proton.

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This video helped me a lot. I would recommend it. https://www.youtube.com/watch?v=NNXvokAcSuE

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Only use suffix -ate if the complex has a negative charge.

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[Mn(en)2I2]2+

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The coordination is simply the amounts of ligands present. For example (NH3)5 ... The coordination number is 5. However if there are two ligands present then you will add those two together. For example [Co(NH3)4(F2)3 Then you would add the number of ligands and that would be your coordination numbe...

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You will need to know the molarity of the NaOH. Let's assume the solution is 0.1M. NaOH is a strong base, so this will produce 0.1mol/L of OH ions in solution. This will produce a pH of 13. You will need to take the negative log of 0.1 to find the pOH. This will work out to be 1. Since pH + pOH = 14...

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Ones to remember would be: NH3, CN, EN, and H2O. These are most used.

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Well you're not really looking to balance the reaction on this problem. Its more of finding out how many atoms of each molecule (H, C, O) you have.

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I'm the same way and don't like using pens but what I do is do my work in the small space of a corner paper and once I get it down I just rewrite it bigger on the other corner. Hope this helps. (:

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It all depends on the formal charge. Remember that you add bonds + dots to figure out the formal charge.

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No they do not. (single, double, triple) bonds are all the same value in hybridization

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From the previous final exams I've seen, yes it does ask for characteristics. Just to be safe, I would recommend to memorize them regardless.

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Im not sure if we'll be tested on it but I would recommend you memorize them just in case.

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a) Tridentate ligand: This is because there are three Nitrogens in this structure that each have a lone pair. No other atoms have a lone pair. b) Mono or bidentate Ligand: This is because CO3 can bind to one or two oxygen atoms. c) Monodenate ligand: Even through oxygen has two lone pairs, the metal...

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Yes all molecules contain the intermolecular LDF.

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Thank you Dr. Lavelle for going out of your way for students. He goes above and beyond to see his students succeed, which is incredibly amazing. Thank you for making learning chemistry fun!

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Yes the lone pairs are taken into consideration. The number of hybrid orbitals is equal to the number of regions around the atom.

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No they do not. All bonds (single, double, triple) are considered as one bond. Hybridization is really more about regions of electrons.

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Shundeen Martinez 1D wrote:Can something just have a hybridization of s if it only is connected to one region of electron density?

Yes it's possible to have a hybridization of only s.

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Single, double and triple bonds are all one electron density.

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This video should help answer your question: https://www.youtube.com/watch?v=4xl0BD-tMeA

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Basically, whenever there is a lone pair on top, that means they will push down on the bonds, causing them to have an angle less than 109.5.

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The common examples of such elements are hydrogen (stable with only 2 valence electrons), beryllium (stable with only 4 valence electrons) and boron and aluminum (stable with only 6 valence electrons).

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505168807 wrote:Would it also be correct to say that the more polar a molecule is, the more soluble it is?

Yes because polar molecules do dissolve in water as they form hydrogen bonds.

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Roni Touboul wrote:Whats the difference between a Lewis acid and Lewis base?

Lewis Acid: a species that accepts an electron pair and will have vacant orbitals
Lewis Base: a species that donates an electron pair and will have lone-pair electrons

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What is VSPER? What do you use it for? The VSEPR theory, sometimes pronounced 'vesper', stands for Valence Shell Electron Pair Repulsion. It states that repulsion between the sets of electron bond pairs surrounding an atom in a compound causes these sets to be oriented as far apart as possible, giv...

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905085650 wrote:When we draw Lewis structures on the midterm, do we have to draw all resonance structures or just give one structure that works? Thank you!!

I've looked at a few past midterms and they usually state if they want all resonance or just one structure.

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Hi! I am bit confused on why the statement below is false, if someone could clarify this for me thank you! (c) Electrons having l =2 are better at shielding than electrons having l = 1. The higher the value for l, the higher the orbital is, so it's further away from the nucleus. When l=1, an electr...

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Hi, I was wondering what were the exceptions to electron affinity that we had to know? This exception rule is actually orbital filling rule. For two electrons to be in same orbital they need to have different spins (Pauli exclusion principal). This electron pairing requires additional energy and th...

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what does degeneracy mean and how do we determine it for orbitals? Also when do we use orbital, shell, and subshell, I find myself using these words interchangeably. Degeneracy basically means of which orbital.bThe degeneracy of s=1, p=3, d=5, f=7 Think of it this way: Shell is n, subshell is l (in...

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Could someone please explain what the difference is between electronegativity and electron affinity. In lecture they seemed like the same thing and they seem to have the same trends on the periodic table. Can these terms be used interchangeably? The difference between the two is that electronegativ...

CHEMISTRY COMMUNITY

Search found 34 matches

Re: Defining Acids and Bases

Re: Resonance and acids

Re: Water

Re: Conjugate Acid/Base

Re: how to determine pH of salt solutions easily

Re: naming

Re: Compound formula

Re: number

Re: Calculating pH

Re: Ligands

Re: midterm question

Re: Can We Take The Final In Pencil?

Re: Lewis Structure bonds

Re: Double and Triple Bonds

Re: Questions

Re: Latin prefixes

Re: Question 17.33 (Sixth Edition)

Re: LDF

Re: Thank you to Professor Lavelle

Re: lone pairs

Re: Double and Triple Bonds

Re: S Hybridization?

Re: double and triple bonds

Re: Steps to figure out hybridization

Re: Bond angles

Re: Incomplete octet

Re: Solubility in Water

Re: Acid vs base [ENDORSED]

Re: VSPER

Re: Resonance Structures on the Midterm

Re: 2.37 (c)

Re: Exceptions to Electron Affinity

Re: Degeneracy

Re: Electronegativity vs Electron Affinity