CHEMISTRY COMMUNITY

philipraj_1F

When pKa increases, Ka decreases. They are used for weak acids mostly

philipraj_1F

It does not matter that it is a electron, it will be 1-

philipraj_1F

It has to do with the formal charges.

philipraj_1F

Amphiprotic is a special type of amphoteric

philipraj_1F

Myoglobin can bond to one O2 molecule.

philipraj_1F

I do not think we would need to draw hybridization orbitals because we were never thought how to do that, but I think we should know conceptually how they would look and function.

philipraj_1F

If it can dissolve into ions, you must represent it as ions (so covalent molecules stay how they are) and it is net it must be simplified to show only the ions that change in a reaction.

philipraj_1F

Also bronsted acid and bases are a type of Lewis acid and bases.

philipraj_1F

It can be either so it would depend on what the product and other reactant are meaning how it changes.

philipraj_1F

It is more stable when it is less likely to attract a proton and stop being a conjugate base.

philipraj_1F

What are common diatomic molecules with different elements that are not considered polar?

philipraj_1F

What difference in electronegativity values is needed for a dipole moment and how do you calculate this difference if we are not given an electronegativity chart?

philipraj_1F

If two dipole moments cancel out in a molecule due to structure does it still have dipole-dipole bonding? Also, if they cancel would the molecule still be considered polar?

philipraj_1F

Do London Dispersion forces increase from right to left across a periodic table because of less effective nuclear charge causing the atoms to be bigger?

philipraj_1F

How are you supposed to know the difference in electronegativity values in a molecule to tell that there is a dipole moment? And also, if a two atoms typically do not have a dipole moment but the arrangement is asymmetrical, does that cause a dipole moment and for them to be polar?

philipraj_1F

I doubt it would matter but I would go with bent

philipraj_1F

it can only be connected to the oxygen that is single-bound to the nitrogen

philipraj_1F

It varies quarter to quarter based overall on how the classes perform.

philipraj_1F

A smaller molecule has stronger dipole dipole forces

philipraj_1F

It is because the equatorial lone pairs cancel each other out.

philipraj_1F

Radicals have an odd number of electrons, and the more electronegative atom will not have the unpaired electron

philipraj_1F

Antioxidants give an electron to radicals which keeps them from being harmful in the body

philipraj_1F

You would have to use the Rydberg equation to solve that

philipraj_1F

You kind of do need to just memorize bond angles, but it does make sense conceptually because the angles do obviously relate to the shape

philipraj_1F

There are specific atoms that can have in incomplete octet, and you would know if the formal charge is lowest when it has an incomplete octet

philipraj_1F

Like what was said above, the specific mass you are given does not matter as long as the ratio is correct and you convert it to moles.

philipraj_1F

What do we need to know about schrodingers equation and its relation to wave functions and orbitals?

philipraj_1F

The s orbitals are considered to be less stable for an electron than d orbitals once one electron is added to a d orbital. That is why you remove electrons from a s orbital before d orbitals.

philipraj_1F

No, it does also depend on the size of the elements themselves.

philipraj_1F

n1 is the initial energy level and n2 is the final energy level that the electron moves to. It is used to find the wavelength of light that results from an electron moving between energy levels.

philipraj_1F

Longer bonds are less stronger than shorter bonds.

philipraj_1F

A dipole moment is when there is a separation of positive and negative charges between atoms in a molecule, and is a measure of net molecular polarity. It can be seen with Oxygen, where the oxygen atom is more electronegative than the hydrogens and slightly negatively charged, while the hydrogen ato...

philipraj_1F

Higher uneven distribution of charges in a molecule will cause it to be less stable. When the formal charge is closest to zero, that is when it is most stable.

philipraj_1F

It is because you always need energy to remove an electron

philipraj_1F

I think it is not important to know which specific orbital it is, but that the electron distribution among orbitals is correct.

philipraj_1F

When its negative energy is released when an electron is added and when its positive energy is gained when an electron is added

philipraj_1F

For a, the orbitals should fill with parallel electrons in separate orbitals first rather than a pair because that is in a lower energy state. For b, the spin of the electrons in each orbital should all face the same way as that is also a lower energy state.

philipraj_1F

You also need to know that there are exceptions to it with the 4s and 3d orbitals when the s orbitals lose an electron to the d orbitals.

philipraj_1F

All it is that you can only have a maximum of two electrons per orbital.

philipraj_1F

Because of the shape of s orbitals, it is impossible for them to have nodal planes. This is unlike p, d, and f orbitals.

philipraj_1F

It technically doesn't change what is being said, but they want 3d before 4s to arrange it in increasing energy.

philipraj_1F

It depends on what orbital the last electron is in. For example, if the last electron were in the orbital with a magnetic quantum number of +1, then that would be the corresponding magnetic quantum number.

philipraj_1F

I feel that looking over the modules posted on the website after having a lecture on the topic also helps to strengthen my knowledge of the material.

philipraj_1F

What does it mean when it says report the difference as a percentage of the wavelength of the neutron? Question: Protons and neutrons have nearly the same mass. How different are their wavelengths? Calculate the wavelength of each particle when traveling at 2.75 * 10^5 m*s^-1 in a particle accelerat...

philipraj_1F

Frequency is equal to the ratio between the speed of light and wavelength, which stays the same.

philipraj_1F

I think that the speed of light changes depending on the material it travels through. Light moves slower through denser materials as particles can get in its way.

philipraj_1F

It is very helpful as much of what it on the modules is the same as what is on the lectures. So if you ever were confused with a lecture it could be helpful to go back and watch the module associated with it.

philipraj_1F

For sig figs in general, you round to the lowest amount of sig figs when multiplying or dividing, and the least number of decimal places when adding or subtracting. This link on his website explains it: https://lavelle.chem.ucla.edu/wp-content/supporting-files/Chem14A/EVERYTHING_YOU_WANTED_TO_KNOW_A...

philipraj_1F

I think formula units is a name for units in an ionic compound, while atoms refers to that of an element by itself, and molecules refers to that of a covalent compound. You would multiply it by avogadro's number the same way with anything else. So it would be .750 mol KNO3 x (6.022x10^23 formula uni...

philipraj_1F

I don't know about the types of questions, but I found that reviewing problems in the textbook and checking them with the solution manual personally helped me, as well as listing the variations of problems in each section

philipraj_1F

I believe that first you would add the two numbers together, and then you would round the final answer to the least number of significant figures present in any part of the problem (so in this case, round to the tenths place). Today in discussion, my TA mentioned that it is most important that our ...

philipraj_1F

I think we use scientific notation to write the answer with the correct number of significant figures. So if the answer was 12300 but the question only asks for 2 sig figs, we would write it as 1.2 x 10^4. If they do not specify which format we should use does it matter? Is there one that's better ...

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