CHEMISTRY COMMUNITY

005384106

How do you determine which step is fast/slow?

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Because many of the review sessions had to be canceled, what else are you guys doing to study?

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In what situation would S(total) ever be = 0? S can only be 0 for a molecule at 0K which is theoretically unacheivable. If is is 0 between reactants and products in a reaction, that is because they had the same entropy value with opposite signs (coincidence) I just wanted to clarify to make sure I ...

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What is the reaction quotient, Q? Can you determine it by concentration values or K?

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Do you always add the H2O at opposite ends of where you have added OH or H+?

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Does autoprotolysis have to do with the donation acceptance of a hydrogen ion but amphiprotic means donation and accepting of protons, and so do acids and bases take place in amphiprotic processes?

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What role do the spectator ions play in this reaction?

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When using an ICE Table, can you ever have a starting value of products, or is it always 0?

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Was O2 a catalyst or an intermediate in this example?

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How do you know if you have a radical molecule?

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Besides adding a catalyst, can increasing the temperature, increasing pressure, or decreasing volume speed up a reaction with the large activation energy?

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Besides adding a catalyst, how else can you lower activation energy?

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I also, have a question on this topic. Will we need to come up with each step or will each step be given?

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Alternatively, when the products are at a higher point than the reactants then it is an exergonic reaction, but a large activation energy will mean that the reaction might be slower because the reaction requires more energy for the reaction to take place.

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Does the larger the order mean that the more collisions will occur?

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How do you determine the rate of formation?

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Why do we measure the voltage difference of two cells?

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How do you calculate for EMF?

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Is the left side is the anode that dissolves, what happens to the right side (cathode)?

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What is a salt reaction?

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In what situation would S(total) ever be = 0?

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At what point do you add elections to the half reaction?

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What does it mean when a reaction is spontaneous?

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How do you know if you have -deltaG or G>0

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What does the cathode and the anode do?

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How do you know if you are dealing with a pure substance?

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In what situation would you only use the R constant, 8.314 instead of multiplying the constant with a fraction?

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Why does R need to be multiplied by 3/2 for constant volume and 5/2 for constant pressure?

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How do I know when I need to use the ideal gas law?

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In 4B. 9 there is a situation where no energy is transferred as heat, what does this mean if delta U = work function?

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I know that K represents the equilibrium constant, but what does Q represent in this situation? In this situation, Q would represent the state of the reaction at a point where equilibrium has not been reached yet. This is why they are asking about which direction the reaction will occur ("left...

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How do o convert my work function -1.48125 L•atm into Juoles. I was thinking about using an ideal gas constant but I don’t have K/mol units that will cancel out so that I am left with juoles.

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What is the units for temperature that we use in these problems?

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will we ever need to do any conversions for units? do these problems always need to be in kJ?

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Can someone please explain why the answer to this problem is negative instead of positive?

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Are Cs and Cm both constants? Can I chose to use Kelvin or Celcius or do I need to use a certain unit unit of measurement in the measurement for specific head of the heat equation.

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If K is 10^-3 then do you assume that x can be represented as 0.

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During Friday’s lecture, is method 3 a way to solve for enthalpy formation by subtracting the enthalpy of products by reactants?

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As Lavelle talked about in lecture, Why is graphite the most stable form of carbon?

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For Friday’s lecture when we talked about bond enthalpies, are the energy values for each product and reactant going to be given? How can we solve for these values?

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Are there any salts that can strongly affect pH? Or do most salts have no affect on pH?

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In class we talked about how HCl and NaOH when mixed make NaCl which neutralizes a solution. What are other examples of this?

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What are all of the coordination compounds that we should look at besides cisplatin and hemoglobin?

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What is the difference between boiling an melting point?

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Can someone please explain in what situations we would need to solve calculations for a buffer?

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does the amount of significant figures for the molar concentration determine the amount of significant figures used after the decimal place of a pH?

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I find making flash cards helps me understand concepts and memorize them easier.

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How can there be different values for Kc and Kp if they are both equilibrium constants of a reaction?

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What is the difference of Kp and Kc?

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Why aren’t solids and liquids included in the equilibrium constant?

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In what instances would the state of a molecule be important? (gaseous, aqueous, solid, or liquid)

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How can a solution reach equilibrium?

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I am confused with the equilibrium ratio when using molarity values compared to the equilibrium ratio using partial pressure. Can someone please explain this to me. Thank you

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How do you solve for Q in this situation?

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I know that K represents the equilibrium constant, but what does Q represent in this situation?

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Do the salts always need to have the involvement of the sodium ion?

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Are the hydrogen protons the polyprotic acids that are donated?

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“How can you predict the number of bonding sites for a given cation?”

I think the lone pairs of a cation will allow for the bonding site of an anion.

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I think it’s just that cobalt is water soluble and helps metabolism of the vitamin into your nervous system.

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Respiratory acidosis is a condition that occurs when the lungs can't remove enough of the carbon dioxide (CO2) produced by the body. Excess CO2 causes the pH of blood and other bodily fluids to decrease, making them too acidic. ... Oxygen passes from the lungs into the blood. CO2 passes from the blo...

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Acid rain is caused by a chemical reaction that begins when compounds like sulfur dioxide and nitrogen oxides are released into the air. These substances can rise very high into the atmosphere, where they mix and react with water, oxygen, and other chemicals to form more acidic pollutants, known as ...

005384106

I always like to look over my tests and nock out the easiest questions before I answer the harder ones. That was I make sure I get some good points.

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Make sure you know the biological functions of transition metals and important ligands (I think they’re ligands: Vitiman B 12, Cisplatin, Myoglobin, Hemoglobin)

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So Fe cation bonds to O2? Is this what allows the more than one complexes to be bonded?

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I think sp2 is fine. The 2 at the beginning only clarifies the energy level.

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a compound containing a ligand (typically organic) bonded to a central metal atom at two or more points.

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Katherine Chhen 3I wrote:What about AX2E3 since it is linear and not bent?

You cannot have all 3 electrons together because there would be a lot of electron electron repulsion, therefore 2 electrons and one electron would repel from the 2 atoms and allow for this linear shape

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I also learned that your conjugate acid is the one that looks the most similar to your base. And vice versa

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Would we also use these prefixes if we were using oxalato?

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A hydrogen bond is the bond between a hydrogens atom and an N, O, or F atom. You can create intermolecular hydrogen bond by binding one of these atoms from one molecule, with an oxygen from another molecule.

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How do you find if dipoles cancel out?

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Does hybridization depend on the number of bonds between atoms?

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How do you know if a molecule has London dispersion forced?

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This was very helpful in helping me determine when you make double bonds/ triple bonds/ single bonds.

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What is the difference between lone-lone pair repulsion, lone-bonding pair repulsion, and bonding- bonding pair repulsion? I thought there was only repulsion differences of 2 types such as a lone pair electron pair and an atom.

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Do lone pair electrons have a stronger force of repulsion of atoms compared to the strength of atoms repelling against each other?

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Is it possible for an acid/base molecule to be covalent?

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The Heisenberg uncertainty principle states that it is impossible to know simultaneously the exact position and momentum of a particle. So the more defined the position is determined, the momentum is less known, and vice versa.

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How do you identify the partial charge in a compound?

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How do you know if a molecule is polar covalent or non polar?

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How do you know when an atom has more covalent character?

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Have we ever been asked questions about solving for lattice energy? Or is it just a concept? If we can solve for it how would we do that?

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This is a question: so in high school I thought all atoms had 2 electrons in the first sub shell, and in all of the next sub shells the valence electrons were 8. So do all atoms that have a d orbital are able to have more than 8 electrons in a Sub shell?

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When drawing lewis structures, you should look at the compound and notice where the atoms are placed on the electron negativity scale. The least electronegative atom is usually your central atom. However there are exceptions such as noble cases. Also sometimes the least moles of the atom in the comp...

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When writing electron configuration you need to write it in numerical order. So the correct answer would be 3d 4s. :)

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005384106 wrote:Why does sulfur have a double bond in the Lewis structure instead of leaving the electrons as valence electrons?

I am referring to this problem that we did during lecture.

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Why does sulfur have a double bond in the Lewis structure instead of leaving the electrons as valence electrons?

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I didn’t understand why oxygen received a negative charge instead of silver. Can someone please explain this to me?

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In what kinds of scenarios or questions would we need to use the Rydberg equation? You use the Rydberg equation in scenarios where electrons are moving to different energy levels, or for solving the amount of energy is present on an energy level. Both scenarios are different equations using the R u...

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I have seen different equations for solving problems about electrons moving to different energy levels using the Rydberg equation and I was wondering what is the correct value of R?

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Why is there more energy the farther an atom is from a nucleus?

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Why do electrons “spin”? And what does the spin (up/down) represent?

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What does. kinetic energy represent?

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Can I clarify why the n is always less that 1 of l.

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Does l represent energy level?

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How does an atoms energy level relate to n and l?

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I have found it easiest to find the limiting reactant by solving for how much product can be produced. This can be used by solving for the amount of moles there are of each reactant and using the molar ratio to solve for the grams of a product and whichever reactant produces the smaller amount of pr...

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On Wednesday I have my first test. I was wondering if questions about the quantum section will be asked or is it just a question about fundamentals/high school chem

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The law of conservation of mass refers to chemical reactions, which is why in nuclear reactions, this is not true. The law states that in a chemical reaction, the total mass of the reactants must equal the total mass of the products. This means that matter cannot be created or destroyed, and so the ...

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First, you need to find which metal element is represented by M in the given compound. You can do this by subtracting the mass of the hydrogen and the oxygens from the molar mass given. 74.10 - ( 2x1.008+2x15.999) =39.94 g/mol Now using the periodic table you will be able to see that the element wit...

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