CHEMISTRY COMMUNITY

Rylee Nelsen 3A

Hi, are you going to post a final review packet? Thanks!

Rylee Nelsen 3A

In the chart that Professor Lavelle posted on the class website it has the New IUPAC Name Convention, are we going to need to know those for the final?

Rylee Nelsen 3A

Yes we are supposed to know the names of ligands, here is a link to a quizlet thank could be helpful: https://quizlet.com/_5pyzad

Rylee Nelsen 3A

I am confused as to how you calculate the oxidation number for ligands in a coordinate compound? If someone could give an example that would be greatly appreciated!

Rylee Nelsen 3A

It is cumulative and in lecture, Professor Lavelle said that each unit will be equally on the final! It is only 8 questions so basically 1 or 2 questions per concept.

Rylee Nelsen 3A

Does the structure of an atom have anything to do with whether it is a lewis acid or base?

Rylee Nelsen 3A

Are we going to have to draw out the hybridization of an atom for the test?

Rylee Nelsen 3A

You can find the hybridization of an atom by finding the number of bonding regions plus the number of lone pairs around the central atom (steric number). If the steric number is 4, the atom is s p 3 hybridized. If the steric number is 3, the atom is s p 2 hybridized.

Rylee Nelsen 3A

I am confused as to how you determine whether an angle is less than 109.5 degrees? Could someone give me an example?

Rylee Nelsen 3A

Yes, the molecular geometry for both would be bent. However, they would have different electron geometries.

Rylee Nelsen 3A

Yes, when you use the vsepr model you need to be using the most stable Lewis structure to determine the number of lone pairs. So, you need to find the formal charges for the atoms in order determine the electron geometry.

Rylee Nelsen 3A

Dipole moments only occur in polar molecules when there is a difference in electronegativity. If you draw the arrows on the Lewis structure there will be a dipole moment when the arrows do not cancel out, meaning they are not pointing is opposite directions basically.

Rylee Nelsen 3A

Will we have to do actual calculations to determine bond length?

Rylee Nelsen 3A

Can someone explain to me the difference between the electron geometry and the molecular geometry for the VSEPR model?

Rylee Nelsen 3A

I made a chart for the VSEPR model that shows each lewis structure and the particular shape, angle and # of lone pairs that it corresponds to. I would just memorize some of them, it makes it easier to identify atoms.

Rylee Nelsen 3A

In the periodic table electronegativity generally follows the trend of increasing left to right. However, this trend does not include the noble gases and fluorine has the highest electronegativity instead of Ne or He.

Rylee Nelsen 3A

I would say that finding the lowest possible formal charge to create the most stable Lewis structure is more important because there are various exceptions to the octet rule so you cannot always base where a structure is correct if each atom has a full octet.

Rylee Nelsen 3A

An induced dipole is an attraction that occurs when a polar molecule induces a dipole in an atom or in a nonpolar molecule by changing the arrangement of electrons in the nonpolar species. For example, with HCl and Argon, the electrons on an argon atom are distributed around the nucleus of the atom....

Rylee Nelsen 3A

For the SOCl2 the oxygen atom and two chlorine atoms are both singularly bonded to sulfur. Also, sulfur has a lone pair. So, because there are four regions of electron density with one lone pair, then the shape would be trigonal pyramidal. In part b, all of the OSCL angles would be the same because ...

Rylee Nelsen 3A

What I have gathered is that the smaller the size of a the cation the greater its polarizing power and the greater the covalent bond will be. So, as the charge on the ion increases, the electrostatic attraction of the cation for the outer electrons of the anion also increases and then it will be abl...

Rylee Nelsen 3A

Yes, the angles depend on the structure of the molecule so for example Trigonal Planar has 0 lone pairs and is 120 degrees, Tetrahedral also has zero lone pairs and is 109.5 degrees and a T - shape has 2 lone pairs and is 90 degrees. Hope this helps!

Rylee Nelsen 3A

Test 3 starts on November 27th in discussion sections so it doesn't affect Thanksgiving break.

Rylee Nelsen 3A

The conversion factor is 1.602 x 10^19 joule = 1 electron volt.

Rylee Nelsen 3A

Polarizability is the ability for a molecule to be polarized (have its electron cloud distorted by the pull of the smaller atom, and it increases as the volume occupied by electrons increases. Whereas polarization power is the ability of a cation to distort an anion. If the degree of polarization is...

Rylee Nelsen 3A

Lone pair electrons are related to the strengths of bonds because electrons naturally repel each other, when they’re located on neighboring atoms they will create a repulsion that weakens the bond. So, as the number of lone pairs on neighboring atoms increases, the dissociation energy decreases.

Rylee Nelsen 3A

Bond dissociation energy is similar to Bond energy, as both are different terms. Bond dissociation energy one is the measure of the strength of the bond where as bond energy is the total energy contained in a chemical bond.

Rylee Nelsen 3A

It's a type of weak chemical bond that occurs when the partially positive hydrogen atom participating in a polar covalent bond in a molecule attracts partially negative atom or atoms of neighboring molecules.

Rylee Nelsen 3A

If they are asking for the most stable Lewis structure then the formal charges are necessary but just to be safe I would put them.

Rylee Nelsen 3A

You have to make sure that the elements symmetrically spaced, that the element with the lowest ionization energy is in the middle and that the formal charges are the lowest to make the most stable structure.

Rylee Nelsen 3A

There are many elements that are exceptions to the octect rule, like all of the third period elements can have expanded octets like CL and Br. The octect rule also doesn’t apply when there are odd valence electrons but the elements cannot share electrons between each other.

Rylee Nelsen 3A

Degenerate orbitals have the same energy levels. The degeneracy of orbitals is basically when they have the same values of n but different values of l. Hope this helps!

Rylee Nelsen 3A

Lewis Acids are electron pair acceptor and bases are electron pair donors.

Rylee Nelsen 3A

Effective nuclear charge increases across the period and decreases going down a group.

Rylee Nelsen 3A

Will the work function always be given to us when solving a problem are will there be a scenario where we will have to find it ourselves?

Rylee Nelsen 3A

If you're having trouble, I would recommend watching this video https://www.youtube.com/watch?v=Mlu_v8rE1TY. It explains the process very clearly, and lets you see the organization of a limiting reactant problem! Hope that helps!

Rylee Nelsen 3A

I am pretty sure that an electron is quantized when electrons are emitted from a metal's surface when light of a certain frequency shines on it, releasing a photon.

Rylee Nelsen 3A

The threshold energy is basically the minimum kinetic energy required to remove an electron. Also, the energy of photoelectrons emitted when light hits a metal depends on the frequency. When light with the right frequency is shone onto a metal surface, electrons are emitted from the surface.

CHEMISTRY COMMUNITY

Search found 37 matches

Re: DOWNLOAD SESSION WORKSHEETS HERE - Sundays 4-6pm (Karen) [ENDORSED]

New IUPAC Name Convention - coordinate compounds

Re: Ligand

oxidation numbers for ligands

Re: Final Exam

lewis acid and bases

Hybridization

Re: When to hybridized?

Bond angles

Re: Bent - Lone Pairs

Re: Does formal charge apply to the VSEPR Model?

Re: Polarity

Bond length

vsepr model

Re: vsepr shape

Re: Electronegativity

Re: Octet vs formal charge

Re: Induced-dipole

Re: Determining VSEPR bond angles

Re: Cations and polarizing power

Re: Bond Angles

Re: Test 3 dates?

Re: Kiloelectron volt to Joule

Re: Polarizability vs Polarizing Power

Re: Covalent bond dissociation energy

Re: Calculating Dissociation Energy

Re: Hydrogen Bonds

Re: Formal charges

Re: Lewis Structure

Re: Number of electrons in relation to Octet

Re: Degeneracy

Re: Lewis Acids and Bases

Re: Effective Nuclear Charge

Kinetic energy

Re: How to determine the limiting reactant???? [ENDORSED]

Re: Meaning of Quanta/Quantized

Re: Threshold Energy