CHEMISTRY COMMUNITY

Stephanie tran 1J

Are there any monatomic ideal gases that don't use the heat capacity constants 5/2R and 3/2R for constant pressure and constant volume

Stephanie tran 1J

what are the trends for reducing and oxidizing power on the periodic table

Stephanie tran 1J

how do you use kinetic data to distinguish between different reaction mechanisms?

Stephanie tran 1J

are there any types of molecules in a chemical equation that you would exclude when calculating reaction enthalpy or entropy?

Stephanie tran 1J

if a problem doesn't make it clear if reversible or irreversible expansion is occurring, how do you know which equation to use for work?

Stephanie tran 1J

besides knowing what the parts of the derived equations stand for like the slope and such, do we need to know how to draw the graphs for zero order, first order, and second order reactions?

Stephanie tran 1J

on the final, will we only need to know units in mol, L, and s or will Kpa show up because it was in the textbook

Stephanie tran 1J

what do the terms labile, nonlabile, and inert mean and how are they significant to calculating gibbs free energy

Stephanie tran 1J

why does gibbs free energy decreases more sharply with temperature for the gas phase of a substance than for the liquid phase?

Stephanie tran 1J

what's residual entropy and do we need to know and understand the concept for the final?

Stephanie tran 1J

To find the entropy of vaporization, why do we have to separate it into 3 steps as in heat the liquid to its boiling point, allow it to vaporize, then cool the vapor?

Stephanie tran 1J

when calculating a change in entropy, does it matter if it is through a reversible or irreversible path?

Stephanie tran 1J

Do we need to know the enthalpy of sublimation for the final?

Stephanie tran 1J

for examples involving calculating energy changes when heating an ideal gas, why do you have to separate the problem into two steps, step 1 being heating at constant volume to the final temperature, and step 2 being allowing the gas to expand isothermally?

Stephanie tran 1J

why is the molar heat capacity of an ideal gas at constant pressure greater than that at constant volume?

Stephanie tran 1J

Do we need to know anything about the equipartition theorem?

Stephanie tran 1J

why are heat and work not state functions?

Stephanie tran 1J

can someone provide some examples where we would have to relate the heat lost or gained by a reaction to the heat gained or lost by the calorimeter? or example for when we would use the q=-qcal equation

Stephanie tran 1J

how is heat capacity an extensive property and what are some other examples of extensive properties in thermodynamics?

Stephanie tran 1J

how are adiabatic and diathermic walls significant to the measurement of heat and what is the difference between the two?

Stephanie tran 1J

In what cases does the internal energy remain constant between the initial and final state and in what cases is the internal energy at 0?

Stephanie tran 1J

why can a system do more work in a reversible expansion versus irreversible expansion?

Stephanie tran 1J

Do we have to know the different types of work on the final like extension, raising a weight, and surface expansion?

Stephanie tran 1J

What are some of the most commonly referenced examples of open, closed, and isolated systems?

Stephanie tran 1J

can someone provide an example of how cis and trans orientations are involved in entropy?

Stephanie tran 1J

Do we need to know troutons rule at all?

Stephanie tran 1J

the equation wasn't specifically used in many examples as only example 9.3 used the equation directly, but the equation is derived to attain the equations for entropy change when there's a change in temperature with constant volume or pressure, and for entropy change of an ideal gas when it expands ...

Stephanie tran 1J

in problems where you need to find the final temperature using the equation, heat lost by ice=- heat gained by water
how do you know whether to use the heat capacity of the ice or the water in the equation?

Stephanie tran 1J

Can someone provide an example of how to estimate the enthalpy of a reaction using mean bond enthalpies and explain the difference between this calculation and when given the bond enthalpies of the products, but not the reactants?

Stephanie tran 1J

I don't understand the concept of how density is involved in solving for heat and why are the dimensions multiplied by the density?
Also, how do you find the mass of water?

Stephanie tran 1J

If you're given the value for pKa, but the compound you're given is a base, then how do you find Kb?

Stephanie tran 1J

according to the textbook definition, amphiprotic specifically pertains to water molecules, but I noticed In the homework problems that amphiprotic referred to other compounds as well acting as both proton donors and acceptors; What's the main difference between amphiprotic and amphoteric and is amp...

Stephanie tran 1J

Which part of the compound when naming it is the lewis acid? Is it the central metal atom? Also, when naming compounds with polydentates, do we have to know more than what is listed in table 17.4 like other than en, dien, and edta?

Stephanie tran 1J

How do polydentates factor into figuring out the coordination number of a compound? Can someone provide an example of that? Also for identifying polydentates, do we only need to memorize table 17.4 for the final or should we know more than the ones listed in the table?

Stephanie tran 1J

to determine the polarity of a molecule, you must first draw the lewis structure of the molecule and in this case, carbon and oxygen are the two central atoms. Carbon has 3 hydrogens and an oxygen attached to it while oxygen has 1 hydrogen and 1 carbon atom attached to it. The oxygen atom has 2 lone...

Stephanie tran 1J

According to the valence-bond theory, bonds form when unpaired electrons in valence-shell atomic orbitals pair; the atomic orbitals overlap end to end to form sigma bonds or side by side to form pi bonds between atoms in a molecule. In addition, for the structure of a molecule, hybrid orbitals are c...

Stephanie tran 1J

The first step to determining and drawing molecular shape is drawing the lowest energy lewis structure of the molecule to determine where the lone pairs go. Then you would go on to determine the shape of the molecule, the bond angles, and hybridization.

Stephanie tran 1J

Why can't molecules with two regions of electron density have a bent shape?

Stephanie tran 1J

sigma and pi bonds are associated with the electron density and how the electrons interact with each other. A sigma bond is formed by the pairing of electron spins in two atomic orbitals on neighboring atoms. sigma bonds are cylindrically symmetrical and they contribute towards an overlap or merging...

Stephanie tran 1J

CCl2 would be predicted to be a linear (bond angle 180º) molecule, and because the two chlorine atoms attached are both of the same electronegativity, the resulting net dipole would be zero because the Cl electronegativity vectors cancel each other out.

Stephanie tran 1J

Why is the hydrogen not attached to the carbon in HOCO? Usually when bonded to hydrogens and oxygens, carbon is the main central atom, so I was confused why the correct structure has the hydrogen attached to the oxygen atom and not the carbon atom?

Stephanie tran 1J

the reasoning behind it is because carbon is slightly less electronegative than sulfur; thus, carbon would be the main central atom with 3 hydrogens surrounding it as carbon atoms are larger than hydrogens which will most likely never be the central atom as they are small, highly electronegative ato...

Stephanie tran 1J

The radical goes on the chlorine atom because it is less electronegative than oxygen so the unpaired electron will be attached to the chlorine atom and because most of the time, you have to satisfy the octet rule for Oxygen first due to its high electronegativity.

Stephanie tran 1J

the larger the central atom, the larger the number of electrons that can surround it and expanded valence shells occur most commonly when the central atom is bonded to small electronegative atoms like F, Cl, and O. The greatest I can think of is iodine heptafluoride which has 7 bonds, but expanded v...

Stephanie tran 1J

the number of valence electrons in d-block elements is most often equal to their group number which is equal to the number of electrons in the "valence shell." for example, scandium metal's electrons per shell are 2,8,9,2 and its outer shell has only 2 electrons, so the valence electron co...

Stephanie tran 1J

Can someone help me how to solve an example like this where you're given the info to treat a hydrogen atom as a one-dimensional box of length 120. pm containing an electron and predict the wavelength of the radiation emitted when the electron falls to the lowest energy level from the next higher ene...

Stephanie tran 1J

The electron is not confined to the nucleus and we now know that the size of an atom is determined by its electrons outside of the nucleus. For hydrogen its measured atomic diameter is 145,000 times its nuclear diameter of 1.7 x 10-15 m. In other words make the (correct) assumption that the electron...

Stephanie tran 1J

Use the above uncertainty in velocity (correct model) to calculate the electron's uncertainty in kinetic energy. Then calculate the uncertainty in kinetic energy per mole of electrons (that is, per mole of hydrogen atoms). Comment on your value. I don't understand how to calculate the uncertainty in...

Stephanie tran 1J

How do you solve a problem where the given information includes that an electron is ejected from a metal due to the photoelectric effect with a velocity in km per second and the work function is given, but you're supposed to calculate the wavelength of the photon absorbed.

Stephanie tran 1J

The wave properties of electrons were discovered through the results of the photoelectric effect and diffraction experiments. Not only did they discover the wave-like properties of electrons, but they also discovered that electromagnetic radiation is particlelike and wavelike. This led towards the a...

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