CHEMISTRY COMMUNITY

quresh3E

The order from strongest bonds to least strong bonds are ion-ion, ion-dipole, dipole-dipole (which include H-bonding), induced dipole-dipole, and induced-dipole induced-dipole (van der waals/london dispersion forces).

quresh3E

I don't think that the atoms with an expanded octet necessarily have to have 10 electrons. However, you should always make sure that your lewis structure with the atom with an expanded octet has the same amount of electrons as the amount you calculated prior.

quresh3E

CCl4 has equal dipoles and no lone pairs so it should be nonpolar.

quresh3E

Bonds strengths are transferrable for the molecule with the same atoms.

quresh3E

Nonpolar bonds don't have different electronegativities, whereas polar bonds do. For example, H20.

quresh3E

Nonpolar bonds don't have different electronegativities, whereas polar bonds do. For example, H20.

quresh3E

If you write the electron configuration you can tell if there is a +1/2 or -1/2 spin.

quresh3E

Yes, the binding energy refers to the threshold energy.

quresh3E

We don't need to know the wave function equations, just the four quantum numbers.

quresh3E

If the range given is +/- 5 then the indeterminancy would be 5. You would have to multiply by two.

quresh3E

For the midterm and for the final, I believe that it is best to learn the concepts of the experiments and the names associated to them.

quresh3E

It is basically many different lewis structures drawn for the same molecule, in which the double bonds differ. However, the total charge for all the resonance structures should be the same.

quresh3E

The main way to tell is if the molecule is asymmetric. You should take the formal charges and draw the S+ and S- accordingly on the atoms. Also, draw arrows to the most electronegative atoms.

quresh3E

The added formal charges of the atoms should be zero. With whatever negative formal charges being on the most electronegative atom.

quresh3E

Expanded Octet- 3rd row and bellow.
Incomplete Octet- First 5 elements and column under Al.

quresh3E

A main distinction between covalent and ionic bonds are that ionic bonds are between a metal and nonmetal. Covalent bonds are between two nonmetals. Additionally, the EN difference for ionic bonds are greater than 2.5 and lower than 1.5 for covalent bonds.

quresh3E

chrisavalos-2L wrote:I was wondering what the trend for electronegativity was, is it the same as ionization energy?

I remember my TA mentioning that it is okay to view them as having the same trends.

quresh3E

Katherine Chhen 3I wrote:For a compound, would the best way to represent it in Lewis structures is to draw out every structure and use double headed arrows?

You have to draw all of the possible Lewis structures and then figure out which one has the formal charge closest to zero.

quresh3E

The resonance structure with the lowest formal change is the most stable. I thought the structure with its formal charge = 0 or closest to 0 was the most stable? You are correct. The structure with the formal charge closest to zero is most stable since that would result in it having no charge of th...

quresh3E

Jorge Ramirez_4H wrote:Is electronegativity important when doing electron configurations?

For electron configurations, you don't really need to know about how electronegative the atom is. It may be more beneficial to know about where it lies in the periodic table in terms of the s,p, and d blocks.

quresh3E

Electronegativity is the ability of an atom to attract a shared pair of electrons. The electronegativity increases as it goes along a period because the atomic number increases, thus increasing the number of protons. The protons make the atom more positive, making it more attracted to electrons.

quresh3E

What exactly is momentum?

quresh3E

What does that mean when he said they were half shell and full shell?

quresh3E

The midterm is on Wednesday, November 6th.

quresh3E

I recommend looking at the example in the book. It is super helpful!

quresh3E

If the total energy of the photon was equal to the work function, and the kinetic energy was zero, then is the electron ejected? How can the electron be ejected if there is no kinetic energy?

quresh3E

Each atom absorbs and emits its own specific amount of energy or quanta. The amount absorbed always equals the amount emitted. However, black bodies can absorb all frequencies.

quresh3E

I worked backwards and solved for the wavelength then inputted it into the E=H*C/v equation. Why is this wrong?

quresh3E

The professor stated that if the energy per photon is greater or equal to the energy needed to remove an electron only then would the increase in light intensity result in more elected e-s. What exactly does this mean?

quresh3E

Why is the equation for kinetic energy 1/2me*ve^2?

quresh3E

I find it super beneficial to watch the modules and do the homework problems right after so then you can apply the concepts just learned.

quresh3E

It is highly unlikely that two reagents would be at the molar specific ratio to be both the limiting reagents. So there are almost never two limiting reactants.

quresh3E

In what types of questions would we have to specify the state (s,g,l)of the product or reactant?

quresh3E

Is there a particular order we have to list our products and reactants?

quresh3E

If you balance the equation and the product has a coefficient that is above 1, would that change the process of finding the limiting reactant?

quresh3E

What is the best way to find the limiting reactant when all of the reactants have coefficients above 1?

CHEMISTRY COMMUNITY

Search found 36 matches

Re: Strongest Bonds

Re: Octet expansion

Re: Polarity

Re: Bond Strengths

Re: electronegativity

Re: electronegativity

Re: n, l ,ml, ms

Re: binding energy

Re: wave function

Re: Heisenberg Uncertainty in Position

Re: Midterm

Re: Resonance structures

Re: drawing dipole moments

Re: Formal charge

Re: Octet Exceptions

Re: Ionic vs Covalent

Re: Trend of Electronegativity

Re: Resonance structures

Re: Formal Charge

Re: Electronegativity

Re: Electronegativity

Re: Heisenberg

Re: Exceptions to Orbital Rules

Re: Midterm

Re: Application

Re: Work Function

Re: Atomic Spectra

Re: Question from module

Re: Photoelectric Effect and Photons

Re: ejecting electons

Re: Video Modules

Re: Two Limiting Reactants

Re: Balancing Reactions

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Re: Limiting Reactant Tips

Re: limiting reactant