CHEMISTRY COMMUNITY

becca_vandyke_4b

You can also use the -ate rule to name polyatomic ions. For example NO3- has a negative one charge so its nitrate whereas NO2- is nitrite because it has 2 oxygens verses 3.

becca_vandyke_4b

Memorize the oxidation numbers of the polyatomic ions like SO4 and use previous knowledge of ions on the periodic table's charge like Cl being -1 and then you deduce the charge of the transition metal since they can differ.

becca_vandyke_4b

I would make sure to know the names for all the strong acids and bases. And how to name these if given the compound.

becca_vandyke_4b

You also need to know how to calculate their oxidation number in a compound since their oxidation number can differ.

becca_vandyke_4b

Are we going to get the same equation sheet for the final thats been on the tests? Trying to figure out if I need to memorize any equations.

becca_vandyke_4b

I would also make sure to know the polyatomic ions!

becca_vandyke_4b

This is touching on thermochemistry which I believe will not be covered on the test. I think he was just touching on the energy exerted and used during the formation or breaking of bonds to show which ones are stronger/weaker.

becca_vandyke_4b

The number of hybridized orbitals matches the number of electron density regions in the shape of the molecule. So if there are four electron density regions it could be sp3. I don't think there is such thing as sp4 because the p-orbital only has three sub-orbitals.

becca_vandyke_4b

I thought he said that we will not need to know bond angle. That we will be asked to draw the Lewis Structure and then name the shape.

becca_vandyke_4b

I think the main argument of polarity in terms of molecular shape is the idea that the shape affects the polarity of a molecule. If a molecule is octahedral and all the bonds in the molecule have the same charge, then the molecule overall will be non-polar which will affect properties such as meltin...

becca_vandyke_4b

I don't think you need to know the bond angle. But know that a lone pair lone pair repulsion is greater than a bond pair repulsion.

becca_vandyke_4b

I believe that electron geometry affects molecular geometry. For example, if the lone pairs were not arranged in the way they are on a water molecule, then the shape wouldn't be bent.

becca_vandyke_4b

A stronger IMF leads to a higher boiling point. Therefore, a compound with strong intermolecular forces would have a high boiling point causing more energy to be needed to change the state from liquid to gas.

becca_vandyke_4b

Bond length is the average of all the bonds added up in the molecule. So you would be given the different bond lengths, then you would add them up and divide them by the number of bonds.

becca_vandyke_4b

In terms of coulombs law, as the radius increases, the attraction between the negative electrons and the positive protons inside the nucleus decreases. Therefore, the electrons are more easily removed from the atom. In an element like F, the atomic radius is smaller because the zeff is higher for th...

becca_vandyke_4b

If an atom is in the 3p block or lower, they have an empty d-orbital which allows them to have an expanded octet.

becca_vandyke_4b

I would just go by the idea that if a compound is a salt, aka an ionic bond, you draw them separate. But if it is a molecule, aka a covalent bond, you draw it together.

becca_vandyke_4b

Do you use de Broglie when calculating wave length for an electron and c=lambda times frequency for a photon?

becca_vandyke_4b

I agree with what is stated above. A good example of this is Na+ on the first column of the periodic table and Cl- in the 17th column on the periodic table. Na loses one electron by donating it to Cl. The Na+ is a cation and Cl- is an anion.

becca_vandyke_4b

if it is a positive charge, you take electrons away from the ground state. If it is a negative charge, you add electrons to the ground state.

becca_vandyke_4b

you find the ground state by looking at the periodic table and seeing where the element falls and what s, p, or d orbitals it already fills. And then to get the 3+ charge you take away three electrons from the ground state.

becca_vandyke_4b

I believe we will not need to use the d-orbital on the test for this week. So I would just understand that there are 5 d orbitals and 3 p orbitals.

becca_vandyke_4b

That equation is known as coulombs law. I think we won't be doing calculations involving it, but instead understanding how it relates to concepts within an atom.

becca_vandyke_4b

Do we need to know how to write out electron configurations for the d-orbital? or is it only s and p orbitals?

becca_vandyke_4b

I think one of the main ideas is that when an electron "jumps" from a higher energy level to a lower one the energy given off is seen as light. That's why when doing a calculation of an electron moving between the different energy levels when an electron goes to lower one the energy of tha...

becca_vandyke_4b

I think one of the big main points of learning of this effect was 1) the experiment did not occur as expected and 2) drawing the model can help us figure out how to do the math with the different types of energy, such as the energy of photon going towards the metal, the threshold energy, and the ene...

becca_vandyke_4b

You use the mass of the electron when calculating the momentum (p) in the problem. I believe the example he gave us listed the velocity of the electron but not the mass of it. So to calculate p=(m)(v) he plugged in the mass which I guess is considered a constant.

becca_vandyke_4b

I think in my discussion our TA wrote molar mass out as Mr (but that might just be what she does) where as molarity is always a capital M. I would make sure you don't mix that up in because there are other equations in chemistry such as p=mv for momentum problems where m=mass.

becca_vandyke_4b

For the states of the compounds you also have to know if they are soluble or not (but he said we don't need to know the rules yet) but anyways some compounds like those with NO3- are soluble in water so they become aqueous. I think you can just look at a solubility chart right now for the problems a...

becca_vandyke_4b

My TA said that if you do more than 7 problems that you should copy down 7 problems on a separate page and turn those in because they have to grade so many. She also said that we could write down the problem number not the whole problem.

CHEMISTRY COMMUNITY

Search found 30 matches

Re: Anions

Re: Determining oxidation number

Re: Naming of acids

Re: Transition metals

Re: About the test

Re: Ligand Names

Re: Energy of Interactions

Re: Hybridization

Re: Test 3

Re: Polarity and Nonpolarity of the Same Molecule

Re: Bond Angle

Re: Electron geometry vs Molecular geometry

Re: Interionic/Intermolecular Forces

Re: Bond Length

Re: Radius

Re: Expanded Octets

Re: 7th edition 2B.9

Re: Calculating Wavelength of electron

Re: periodic table

Re: Electron Configuration of Cations

Re: Ground State

Re: Slight Confusion

Re: Multi electron atoms

Re: Test 2 Material

Re: Energy emitted by electrons

Re: Purpose of the Photoelectric Effect

Re: Example from Friday's Lecture (10/12/18)

Re: V=n/c

Re: Naming Compounds

Re: Textbook Homework Assignment