CHEMISTRY COMMUNITY

Michael_Navarro_1H

To clarify, if you are dealing with a strong acid, the molarity of the acid will equal the molarity of the H3O+ in solution. So for example, if you were given a solution of HCl with molarity 0.20 M and were asked to calculate the pH of the solution, the molarity of the H3O+ ions in solution would al...

Michael_Navarro_1H

The conjugate base of a strong acid is stable as is, so it does not result in the deprotonization of water which would result in a change in pH. However, the conjugate base of a weak acid is unstable and will therefore pull an H+ from H2O to form an acid and OH- in solution, thereby increasing the pH.

Michael_Navarro_1H

Isn't pKa just calculated by just taking the -log of the Ka value?

Michael_Navarro_1H

If a question like this were to come up on the final, I would find an equation where each variable is included and see if there is a way to relate them together that would assist you in answering the question.

Michael_Navarro_1H

You can also think of pi bonds as relating to double bonds while sigma bonds only refer to single bonds.

Michael_Navarro_1H

There are soft salts that dissociates in water that gives water the soapy feel

Michael_Navarro_1H

The only rule you need to know when the complex ion is negative is to add -ate to the end of the metal involved

Michael_Navarro_1H

Since N has the additional lone pair, it acts as a lone pair donor and thus acts as the base in solution,

Michael_Navarro_1H

Being cis or trans is really dependent on the biological function of the molecule. Having a cis configuration is convenient for the cisplatin chemotherapy drug mentioned in class, but for a different compound with a trans configuration, it may prove to be more effective for its function.

Michael_Navarro_1H

usually in any organic molecule, you would be asked to determine the molecular geometry of a specific atom. For most organic compounds, carbon is the central atom with a tetrahedral geometry.

Michael_Navarro_1H

Hybridization is a way of explaining why certain atoms form the bonds they do -- in the case of Carbon, which only has two unpaired electrons to form bonds, the sp3 hybridization model explains why carbon is capable of forming 4 bonds.

Michael_Navarro_1H

The lone electron pairs have a greater effect on the molecule shape. Looking at H2O for example, we see that the lone pairs on the Oxygen atom changes the shape of water from a theoretical linear geometry to the bent configuration.

Michael_Navarro_1H

Knowing bond angles is pretty much a matter of memorization. We'll be going over plenty of examples in class and be exposed to all the molecular geometries within the VSEPR model and their appropriate bond angles.

Michael_Navarro_1H

Attractive energy is just a determinant of the relative strength of a bond in relation to the energy required to break it. The higher the dissociation energy of a bond, the stronger its attractive energy is.

Michael_Navarro_1H

When drawing a lewis structure, you really don't have to consider either as much. However, when it comes to resonance, then the electronegativity is important to consider as the most electronegative atoms should be those you place a negative FC on if an overall formal charge of zero is not possible ...

Michael_Navarro_1H

Usually, you want to keep the negative charges on the most electronegative atoms and keep the other atoms at a FC of 0.

Michael_Navarro_1H

No, formal charge is only specific to a single atom within the context of molecule and the involvement of its electrons with other atoms.

Michael_Navarro_1H

You can usually determine whether an electronic configuration represents an excited state if the diagram depicts an electron that is not in its appropriate orbital or if it has an irregular spin.

Michael_Navarro_1H

The f orbital only exists when the principal quantum number (n) is at least 4, allowing for the angular momentum number (l) to be 3.

Michael_Navarro_1H

Due to the isoelectronicity principle, we would most likely be given the name of the element and then asked to write the electronic configuration for it.

Michael_Navarro_1H

I wouldn't be too concerned about anything relating to the Schrodinger Wave equation. From what I understand however, psi^2 correlates to the probability density of finding an electron within an orbital.

Michael_Navarro_1H

The De Broglie equation can only be applied to objects with very small mass (such as an electron), moving at a considerable speed in order for a detectable wavelength to result. All matter moves at a wavelength, but only matter with a small mass can be detected.

Michael_Navarro_1H

Essentially, the Schrodinger's Equation allows us to have a mathematical representation for each type of orbital (s,p,d,f) that correlates to their shapes in 3D space

Michael_Navarro_1H

I would use that equation to calculate frequency and then from there stick with v=c/λ or λ=c/v to determine wavelength.

Michael_Navarro_1H

Dr. Lavelle posted a file on his website that contains a whole list of constants that will be useful throughout the quarter--the mass of an electron in addition to everything he has/will cover should be on there.

Michael_Navarro_1H

For our purposes I think the only way to determine the velocity of an electron other than a detector is by utilizing the equation provided to us in class: E(photon) - E(energy remove e-) = 1/2mv^2

Michael_Navarro_1H

As long as you set up conversion questions using dimensional analysis, you should be ready to tackle any problem on the test.

Michael_Navarro_1H

Typically, chemistry questions throw in extraneous information such as the temperature and pressure as a means to distract students from focusing on only the necessary information. In a question such as this, you should know that only the stoichiometric co-efficients as well as the mass of CaCO3 use...

Michael_Navarro_1H

Is the homework for this week just to do 7 problems listed in the "Review of Chemical and Physical Principles" unit?

CHEMISTRY COMMUNITY

Search found 29 matches

Re: pH calculation

Re: Anion affecting ph

Re: pKa and Ka

Re: Heisenberg and Wavelength

Re: Strength of Sigma and Pi Bonds

Re: Bases

Re: Complex Ion

Re: Biological Compounds

Re: Cis and Trans

Re: Organic Molecules

Re: When to hybridized?

Re: Lone Pairs

Re: Bond Angles

Re: Hydrogen Bonding

Re: Electronegativity vs. Ionization Energy

Re: Polar

Re: Formal Charge

Re: Ground state vs. excited state

Re: Orbital Shape for Larger Quantum Numbers

Re: Cation/Anion Electron Configuration

Re: Psi squared meaning

Re: Wave properties

Re: Schrodinger's Equation

Re: Rydberg formula

Re: de Broglie Relationship

Re: Kinetic energy

Re: Unit Conversions [ENDORSED]

Re: Limiting Reactants Post- Module

Week 1 Homework Assignment [ENDORSED]