CHEMISTRY COMMUNITY

Ian Hurst 3L

(For homework 14.15c) In the solution manual it lists KOH (aq) as one of the aqueous species. I am confused as to why this is there. Is this a typo?

Ian Hurst 3L

The energy diagram in the book shows that gauche and anti configurations are not equally stable for 1,2-dibromoethane. Why is the anti configuration the most stable while the gauche is sightly less stable? Is this because of torsional or steric strain? or both?

Thanks

Ian Hurst 3L

First Order Rate Law

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Ian Hurst
Lovelyn Edillo
Vinay Sharma

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Ian Hurst 3L

I understand that sawhorse projections are drawn at an angle for the best representation of a structure while Newman projections utilize line intersections to represent carbon bonds. Are there situations where one is preferred over the other? In what situation is optimal to use a sawhorse projection...

Ian Hurst 3L

How do we determine which functional group has priority? Do we just have to memorize the list and just know, for example, that carboxylic groups have higher priority than alcohol groups? Is there another way to figure it out by looking at atomic mass or something? Also, for (E)-4-methlycyclopent-2-e...

Ian Hurst 3L

In the course reader (page 78), it explains that reactants sit on the surface of the catalyst in a reaction (and this is known as adsorption). Although it may look like a typo, adsorption is actually a term that refers to a substance that sticks to the surface (so in a reaction, reactants sticking t...

Ian Hurst 3L

How do catalysts lower the activation energy of a reaction if they are not consumed in the process? If they increase the speed of a reaction and cause more products to be formed, shouldn't they be consumed?

Ian Hurst 3L

I know that delta G= standard G + RTln(Q) and that if the reaction is at standard conditions then delta G goes to 0 but I do not understand why. Can someone explain to me why delta G = 0 when Q=K?

Ian Hurst 3L

I believe the direction of the electron flow is dependent on how you set up the beakers. Regardless of how you set up the beakers, the solution that will be reduced will be on the "right" and the solution that is oxidized will be on the "left." This is in reference to the equatio...

Ian Hurst 3L

I understand that Gibbs free energy is a state function (meaning it doesn't matter how you got there) and that if it's positive you know it is describing a spontaneous reaction (meaning the reaction will go forward without external influence). In the course reader it says that this energy is "f...

Ian Hurst 3L

Can someone explain to me why bonds have an enthalpy and a mean bond enthalpy? (What is the mean bond enthalpy an average of?) Also, which one do we use when solving problems?

Ian Hurst 3L

I understand that higher heat capacities lead to lower slopes (and vise versa for lower heat capacities) on heat supplied vs. temperature diagrams because the substance can store more energy. Does the heat capacity of a substance also effect how much energy is needed in a phase change (for example a...

Ian Hurst 3L

I remember in class Professor Lavelle explained that in weak acid- strong base titrations, strong bases "dominate" weak acids. This means that after the equivalence point there should be a higher concentration of OH- ions. How do you know how to set up a reaction (equilibrium) for chemistr...

Ian Hurst 3L

A polyprotic acid is a compound that can donate more than one proton. Common polyprotic acids are Sulfuric acid (H2SO4) and carbonic acid (H2CO3). You can look at the deprotonation of these compounds as a series of steps. For example, in the first deprotonation, H2CO3 will react with water and form ...

Ian Hurst 3L

I read that as the strength of acids increases as you go down the halogen group on the periodic table (HF --> HI). Why is it that even though the molecules are becoming less polar (and have a lower difference in electronegativity) they are increasing in acidic strength?

Ian Hurst 3L

According to the Ideal Gas Law, pressure increases as temperature increases, and temperature increases as volume increases. Then why doesn't it make sense for pressure to increase as volume to increase? Think of the PV= nRT formula like this (for comparing temperature and volume)--> P= (nRT)/V. If y...

Ian Hurst 3L

K (the equilibrium constant) is derived from the division of products by reactants. (K= [Products]/[Reactants]) A large K (greater than 10^3) means that the reaction favors the formation of products ("equilibrium is shifted to the right"). A small K (less than 10^-3) means that, at equilib...

Ian Hurst 3L

In determining the shape of a compounds and molecules, I always find it best to draw out and write out the generic formula ( A for the central atom, X for the number of atoms surrounding the central atom, and E for the number of lone pairs on the central atom). Note that bent refers to the AX2E2 and...

Ian Hurst 3L

I have a question regarding the molecular structure of BF3. In the book (page 110) it shows a Boron as the central atom, with 3 Fluorines attached with single bonds. In this structure all of the formal charges are 0, however, the central Boron atom only has 6 electrons and does not satisfy the octet...

Ian Hurst 3L

I am confused about the "crystal structure" that forms in ionic bonds. Do all ionic bonds have a crystal structure with cations and anions alternating down a row (Figure 3.5)? And does "lattice energy" only refer to ionic bonds with this structure (or to all crystal structures)?

Ian Hurst 3L

First, lets look at the periodic trends for atomic radius. As you go down the periodic table (from top to bottom), you go from 1s --> 2s -- 3s.. etc... the atomic radius INCREASES (there are more electrons, and each orbital can only hold two electrons, so the more electrons in an element, the bigger...

Ian Hurst 3L

To understand planck's constant (and his hypothesis), the formula it is used with (E=hv), and its importance, you must first understand that light rays push and pull on an electron. This creates the "wave" picture that is shown by figure 1.7 in the book. How fast the cycles (created by the...

CHEMISTRY COMMUNITY

Search found 22 matches

Homework 14.15C

Gauche vs Anti Stability

Re: Video Competition

Sawhorse vs Newman Projection

Determining Priority

Re: Homogeneous and Heterogeneous Catalysts

Catalyst and Activation Energy

Standard G

Re: Work in Electrochemistry

Giffs Free Energy Definition

Bond Enthalpies vs. Mean Bond Enthalpy

Heat Capacity and Phase Change

Strong Acid Vs Weak Base Titrations

Re: Acids and Bases

Strong Vs. Weak Acids

Re: PV=nRT

Re: K Constant

Re: Distinct DIfference between Linear and Bent

BF3 VSEPR Shape

Ionic Bond Structure

Re: Ionic radius

Re: Black body [ENDORSED]