CHEMISTRY COMMUNITY

505194972 3k

were they based on a specific due date each week or as long as we got 30 in total it counts?

505194972 3k

It completely ionizes

505194972 3k

Polarizablilty is the how easily the electrons can be distorted (anion). Polarizing power is the ability of a molecule to skew the electrons of a another molecule (cation).

505194972 3k

duverge_maciel wrote:Why do pi bonds not allow bound atoms to rotate?

Professor Lavelle gave a very good example in lecture when he held two pencils parallel between his two hands and when he twisted them the pencils fell. if the atom rotated the bonds would break. I believe the pi bond stabilizes the molecule.

505194972 3k

for test 3 should we go about to study (the book) chapter 4 on molecular structures and shapes or should we focus on studying what the lectures are about? Since the test is supposed to be similar to the homework problems. Professor Lavelle often stresses that it is most helpful to do the homework p...

505194972 3k

Mariah Hill wrote:Will we have to know how to calculate the strength or length of the bonds?

No we should not have to know that. I believe in class when professor Lavelle would give us values for the strength/length he mentioned that he had looked up that value.

505194972 3k

single bonds: 1 sigma bond
double bonds: 1 sigma 1 pi bond
triple bond: 1 simga 2 pi bonds
and so on
This is a good tool to remember/ keep in mind

505194972 3k

I believe professor lavelle said we would not need to know how to draw the shapes. Just the lewis diagrams and know what shape it is but not actually drawing it.

505194972 3k

I believe for polyatomic molecules you count the total number of bonds (sigma and pi) and then count the bond groups (areas of electron density but not lone pairs) and divide the two. for anything less you just count the number of bonds between the two molecules.

505194972 3k

What is the interaction potential energy telling us? What do we use it to determine? Does it have anything to do with whether their is a dipole moment and how strong that dipole moment is?

505194972 3k

How does the interaction between ions and dipoles determine the phase of something (i.e. liquid solid etc.)? Do we need to know specifically which interactions cause certain states?

505194972 3k

the VSEPR model explains experimentally observed shape of molecules.

505194972 3k

So I know in lecture we have been discussing how the d orbital is written before the s. I have never understood why this is. Could someone explain why this is and does it happen every time no matter if either orbital is full? Is there ever a time when the d orbital is written after the s in the grou...

505194972 3k

I believe the reason is because with two bonds mean a stronger hold between the two atoms so they are pulled closer together. while a single bond is held more loosely between the two atoms and would not be held as tightly making it longer. hopefully that helps.

505194972 3k

I'm not sure if i completely understand your question but valance electrons in an atom are the electrons in the outer shell. So for example, Carbon has 4 valence electrons but the amount of bonds can vary based on what other element it is bonding with and what gives all atoms involved a complete oct...

505194972 3k

I believe ionic bonds typically involve metals with nonmetals and covalent bonds deal with nonmetals bonding with other nonmetals. In ionic bonding metals lose electrons and nonmetals gain within the bond to form the octet while in covelant the atoms share the electrons.

505194972 3k

This relates to electron repulsion in that two electrons of the same charge will repulse each other.

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Ionization energy is the energy needed to remove an electron from an atom in the gas phase. So it's looking at how strongly a nucleus is holding on to its electrons. The easier it is to remove an electron the lower the ionization energy will be. For example elements in the first column want an octet...

505194972 3k

Dhwani Krishnan 1F wrote:Do emission and absorption spectra look the same? Or are they "opposites" of each other?

They should look the same because when an electron is excited it is absorbed with a certain energy then when it relaxes back the same amount of energy is emitted.

505194972 3k

The uncertainty for something very small like an electron should be relatively large because its so small its much harder to be certain about its position or momentum. The uncertainty of something like a ball or a car would be smaller because those are more easily seen and measured.

505194972 3k

No, not all wavelengths of light are absorbed. Only wavelengths that have a frequency that corresponds to a specific energy level. Some wavelengths have frequencies that land between two energy levels and that means the light will pass right through, I believe, and not be absorbed.

505194972 3k

Those units are exactly the same and work just fine. It is personal preference I suppose.

505194972 3k

is the problem asking you to convert some distance to energy? I.e wavelength to energy because then there are formulas that can do that.

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In most cases rounding up from .5 is not precise enough and you often have to multiply by a value to make it a whole number, specifically when doing empirical/molecular formulas.

505194972 3k

Ashley Zhu 1E wrote:After finding the energy of a photon using the equation, E = hf (f = frequency), you just need to divide the total energy emitted (11J) by the energy per photon to get the number of photons: 11J/(1.074 x 10^-19 J).

How did you find that value for energy per photon?

505194972 3k

I'm not sure how many intermediate steps are in the solution manual but I would show as many steps as time allows you to because the more steps you show the more likely you are to receive partial credit even if your final answer is wrong.

505194972 3k

The problem is asking about an electron and an electron's mass is a constant which is 9.11 x 10^-31.

CHEMISTRY COMMUNITY

Search found 27 matches

Re: Discussion Posts

Re: HClO4 Strength

Re: polarizability

Re: pi-bonds

Re: Test 3

Re: Determining Bond Strength with Resonance

Re: multiple sigma bonds

Re: Molecular shape on test

Re: Determining bond order

Interaction potential energy equation

phases caused by interactions

Re: VSEPR Model

ground state configuration set up

Re: Bond Lengths [ENDORSED]

Re: covalent bonds

Re: Difference Between Ionic and Covalent Bonds

Re: Lewis Structure for Compounds

Re: Ionization Energy

Re: Atomic Spectra

Re: Realistic Values

Re: Atomic Spectra

Re: Preferred Units for Tests and Homework

Re: Conversion

Re: Rounding Off of 5

Re: Calculating amount of photons

Re: Problem solving, intermediate steps

Re: de Broglie Relationship