CHEMISTRY COMMUNITY

cristinapadilla_1E

In order to really break this down to know that it is trigonal pyramidal, you must understand the notation used in VSEPR Model. A is the central atom X is the number of bonded atoms E is the number of lone pairs One example of a trigonal pyramidal shaped molecule is NH3. N is the central atom, there...

cristinapadilla_1E

Some amphoteric examples we discussed in lecture are:
BeO, Al2O3, Ga2O3, SnO2, Sb2O5, and PbO2

cristinapadilla_1E

In the fundamentals J portion of the 7th edition textbook it talks about Arrhenius Acids/Bases. I don't recall learning about those types during lecture. Does anybody know if we need to know this for the final exam and what are some key distinguishers between Arrhenius and Bronsted acids/bases? Than...

cristinapadilla_1E

Memorizing common polyatomic ion formulas as well as their chargers will only benefit you for the exam!

cristinapadilla_1E

Although looking at a molecule simply to determine whether or not it is polar or nonpolar, it is more accurate to use VESPR theory in order to deduce whether it is or not forsure.

cristinapadilla_1E

The structures does affect whether or not it is an acid or a base. The resonance of a molecule is what affects it due to the ranging kPa value.

cristinapadilla_1E

During the lecture, it was stated how transition metals are often bound to cage-like molecules. Are there any other examples other than the porphyrin ligand one we went over in class? I am having trouble visualizing it.

cristinapadilla_1E

To add on to what s-character is and how to determine how much s-character is present, triple bonds have more s-character than single bonds. The more s-character, the shorter and tighter the bond is.

cristinapadilla_1E

What is the reasoning and how can we deduce why bond strength goes in this order:

lone-lone pair > lone-bonding pair > bonding-bonding pair

cristinapadilla_1E

In class we discussed the sulfite ion SO3 2-. I still don’t understand why the bond angle would be 106 rather than 109.5. Can someone explain?

cristinapadilla_1E

I thought that linear shaped molecules can’t have dipole moments. How is O2 an exception to this?

cristinapadilla_1E

Bond lengths are given and in Angstrom units.

cristinapadilla_1E

We started the molecular shape and structure topic and covered VSESPR models and a few shapes.

cristinapadilla_1E

In class we covered three important shapes so far. They are linear (180 degrees w/ 2 bonding pairs), trigonal planar (120 degrees w/ 3 bonding pairs), and tetrahedral (109.5 degrees w/ 4 bonding pairs).

cristinapadilla_1E

All molecule structures are 3D!

cristinapadilla_1E

The units for molar mass are grams per mol.

cristinapadilla_1E

What are the trends in first ionization energies throughout the periodic table?

cristinapadilla_1E

When drawing Lewis structures, follow this format: 1) Count the number of valence electrons for each atom. 2) Count atom with lowest ionization energy as the central atom (H is never the central atom). 3) Arrange atoms symmetrically around central atom. 4) Calculate the formal charges so that they a...

cristinapadilla_1E

I know we went over one example in lecture that displayed isoelectronic molecules. Can someone give another series of examples?

cristinapadilla_1E

Covalent radius is just the radius of two atoms (nonmetals) that are joined by covalent bonds.

cristinapadilla_1E

In terms of electron affinity, there are patterns that you must recognize and memorize. As you go across a period, electron affinity increases. As you go down a group, electron affinity decreases.

cristinapadilla_1E

Covalent radius only pertains to atoms present in a covalent bond whereas atomic radius can be of any atom.

cristinapadilla_1E

F-orbitals have more complicated shapes, meaning that there are more lobes. Having more lobes means that there is a more complicated shape in regards to displaying itself on a plane.

cristinapadilla_1E

We brushed upon this in class, but I just want to clarify.. Why are the subscripts in the d-orbitals squared? Is it because there are four lobes? For example One of the orbitals has an electron density distribution located along the x and y axis: d (subscript x^2 -y^2)

cristinapadilla_1E

There is a page of formulas and a periodic table on the front of the test!

cristinapadilla_1E

Ev (energy volts) =1.6 X 10^-19 J

cristinapadilla_1E

They descend one level at a time since each level is discrete and not continuous.

cristinapadilla_1E

Work function, also known threshold energy, is the minimum energy required to release an electron.

cristinapadilla_1E

Based off of experience from taking the quiz today, calculators are not provided. They sell cheap ones at the bookstore!

cristinapadilla_1E

Molecular weight is the gravitational pull whereas mass is the quantity of matter.

cristinapadilla_1E

Limiting reactant is the reactant with the least amount of mol produced.

cristinapadilla_1E

Also, to understand why it is calcium sulfide is because the subscript on OH is 2. By noticing the subscript you can deduce that the metal must be from the second group due to its charge.

cristinapadilla_1E

O2 will always be one of the reactants and the products will always be H2O and CO2.

CHEMISTRY COMMUNITY

Search found 33 matches

Re: AX3E

Re: Examples

Bronsted Acids/Bases Vs. Arrhenius Acids/Bases

Re: Naming

Re: Polar Molecules

Re: lewis acid and bases

Transition Metals and their binding

Re: s-character

Bond strength

Sulfite Ion and its Bond Angle

Linear Shape of O2

Re: Bond Lengths

Re: Molecular Shape

Re: Different Shapes

Re: Trigonal Planar

Re: Molar Mass

Trends in first ionization energies

Re: Drawing Lewis Structures

Isoelectronic Molecules

Re: Covalent Radius

Re: Electron Affinity

Re: Atomic Radius

Re: Difference in orbitals

Orbital Notations

Re: chem test tmrw

Re: Unit conversion in 1B.5

Re: Photoelectric Effect

Re: Work function

Re: Calculators

Re: Molecular weight vs molar mass

Re: Limiting Reactants

Re: Finding the Molar Mass of a metal

Re: Combustion Reactions.