CHEMISTRY COMMUNITY

Molly Oakes 1A

Usually, but some elements can have expanded octets. I believe elements after Ne on the periodic table can have expanded octets.

Molly Oakes 1A

You count single bonds as two if you're plugging them into the equation (because they get divided by two in the equation), but you can count them as one to skip dividing by two.

Molly Oakes 1A

Correct, as Lewis acids and bases are defined by whether they accept or donate electrons.

Molly Oakes 1A

Instead of using the equation, I take the number of valence electrons that the atom has and subtract 1 for each lone pair electron and one for each single bond attached to that atom. Maybe this is what you are referring to.

Molly Oakes 1A

alexagreco1A wrote:I understand the concept of a radical, but when drawing Lewis structures, how do we decide which element has the unpaired electron?

I believe you place the radical where it makes sense to due to formal charge.

Molly Oakes 1A

Pi bonds come from the overlap of parallel p orbitals on adjacent atoms. Rotation would break the side-by-side positioning.

Molly Oakes 1A

I believe they are of equal importance, but formal charge clarifies which one you should use in each situation.

Molly Oakes 1A

Cations have polarizing power (ability to distort anions) and anions have polarizability (ability to be distorted by cations).

Molly Oakes 1A

I believe so. I am not aware of any exceptions.

Molly Oakes 1A

I do not believe there is a difference besides naming for our purposes.

Molly Oakes 1A

They have an electronegativity difference of 1.7, which is large enough to be considered an ionic bond.

Molly Oakes 1A

I think you initially connect your atoms with single bonds and then use formal charge to distribute the rest of the electrons.

Molly Oakes 1A

Zeros between two significant digits and zeros to the right of the decimal point are significant. Trailing zeros in a whole number with no decimal shown are NOT significant. For example, if it just says 230, there are only two significant figures. However, if it says "230." the decimal ind...

Molly Oakes 1A

Making the formal charge as close to zero as possible determines the best Lewis structure.

Molly Oakes 1A

formal charge = valence electrons - lone pair electrons - 1/2(bonding electrons)

Lone pair electrons are dots and bonding electrons are lines.

Molly Oakes 1A

Objects like cars and balls are too big to exhibit measurable wavelike qualities. Wavelike properties are noticeable on microscopic scales.

Molly Oakes 1A

You know velocity and I believe the mass of an electron is a constant. Therefore, you have mass, velocity, and Planck's, so you can use De Broglie's equation.

Molly Oakes 1A

Light acts as a stream of particles, or photons, in the photoelectric effect. The flow of photons is a wave.

Molly Oakes 1A

I think you can memorize it based on the blocks of the periodic table.

Molly Oakes 1A

It is my understanding that orbital placement is related to the number of electrons, not energy levels. The earlier Bohr model has to do with energy levels.

Molly Oakes 1A

I think it has to due with planes. There will be a p-orbital in the x plane, a p-orbital in the y plane, and a p-orbital in the z plane.

Molly Oakes 1A

I could see it being mentioned on the test because I believe it was discussed in class.

Molly Oakes 1A

Intensity is the number of electrons and affects the height of the wave.

Molly Oakes 1A

I am focusing on the order of increasing frequency and wavelength of the visible light colors.

Molly Oakes 1A

Lyman series: lower energy level is n=1
Balmer series: n=2
Paschen series: n=3
Brackett series: n=4

Molly Oakes 1A

I use 16.00

Molly Oakes 1A

Yes, I would default to SI units.

Molly Oakes 1A

You multiply everything by the denominator of the fraction to make the numbers whole while maintaining the right ratio.

Molly Oakes 1A

I believe they can be used interchangeably.

Molly Oakes 1A

Volume is the amount of space something takes up, while density is the amount of mass per unit within that volume.

CHEMISTRY COMMUNITY

Search found 30 matches

Re: Central atom and octet rule?

Re: Formal charge

Re: Donating electrons

Re: Formal Charge Shortcut

Re: Radicals

Re: Pi bonds

Re: Bonds or Lone Pairs more important?

Re: Polarizing power

Re: Shorter bond length always leads to stronger bond?

Re: London Dispersion, Induced dipole- Induced dipole, Van Der Waals

Re: Electronegativity difference

Re: When to use lone pairs or bonds

Re: Zeros in Sig Figs

Re: Formal charge purpose

Re: formal charge equation

Re: Is this movement noticeable?

Re: Calculating wavelength of an electron

Re: Wave and Particle

Re: 2.25

Re: The concept of Orbitals

Re: 2.13

Re: amplitude and intensity

Re: Significance of intensity [ENDORSED]

Re: Wavelengths

Re: hw chapter 1 question 11

Re: Which mass of oxygen should be used? [ENDORSED]

Re: Length Units

Re: Whole numbers

Re: Reagent vs. Reactant [ENDORSED]

Re: Volume V Density [ENDORSED]