CHEMISTRY COMMUNITY

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How do we predict the product of a SN2 reaction?

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How do you calculate it?

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Q3A. Balance the following redox equation which takes place under basic conditions.
MnO2(s) + ClO-(aq) -> MnO4^2-(aq)+Cl-(aq)

How do I do this?

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OIL RIG

Oxygen is losing - oxidizing agent gains electrons

Reduction is gaining - reducing agent loses electron

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In the syllabus it says that we're going to go over chapters 8, 9, 11, 14, and 15 throughout the quarter. Is the final going to include any other chapters or just these?

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Large = more complex = more possible orientations = higher entropy
Small = less complex = less possible orientations = lower entropy

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You write it without it since it has no affect

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It’s different units depending on the rate order because each order has different powers the concentration is raised to so using the rate law you get different units for k in each rate order.

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Reactant concentrations, temperature, solvent and catalyst properties

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The rate law relates the rate of a reaction to the concentration or pressure of the reactants. The rate of a reaction is proportional to the concentration or pressure of the reactants modified by the reaction order.

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A first order reaction will have an overall order of one, the sum of all the exponents will be 1. A second order reaction will have an overall order of 2, the sum of all the exponents will be 2.

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It's not always necessary, it's just better

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Yes you’re right

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An electrochemical series is a series of chemical elements arranged in order of their standard electrode potentials. The series shows the order in which metals replace one another from their salts.

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I'm not sure how to approach this problem or what formula to use. Can someone please explain how to do solve this. "Dr. Lavelle picks up the ice cream that he has just heated up (-2.8 degree C) and accidentally drops it on the ground and can’t eat it. Tears streaming down, he watches as half of...

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Yeah^^simply put, the oxidation number shows you the charge

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Vibration causes disorder which means an increase in entropy. Diatomic molecules would have greater entropy because the more complex the molecule the more entropy there is.

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I kept wondering the same thing but during today's review session Lyndon said you'd use Cp when it specifically states "at constant pressure" in the problem.

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Entropy values are given as standard molar entropy which is the entropy of one molecule of a substance as standard state conditions. The standard molar entropy of any substance increases as the temperature increases.

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I think my ta had said it's on chapters 8, 9, and 11

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Why is "The contents of an ideal cooler at 3 degrees C" an isolated system and not closed?

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Exothermic/Endothermic: refer to transfer of heat or changes in enthalpy
Exergonic/Endergonic: refer to changes in free energy

Positive enthalpy change is endergonic because heat is absorbed and the products are higher in energy than the reactants

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A microstate is a specific way that the energy of a system can be arranged. Microstates tend to be indistinguishable from each other which means the more indistinguishable the higher the entropy.

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The question was pretty vague so I was also wondering how specific we were supposed to be because all I answered was that "Energy can't be created or destroyed, conservation of energy."

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Perfect- got it, thank you!

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I think it doesn't decrease since it's at maximum entropy when it reaches equillibrium.

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Just to clarify, for Chem 14b, will test 1 include Reversible and Isothermal Expansions?

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Yes most likely; always pay attention to and use correct sig figs in chemistry.

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Exothermic reminds me of exit and the first 2 letter in endothermic reminds me of in (enter).

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A thermochemical equation is a balanced chemical equation that has the physical states of all reactants and products along with the energy change. The reaction is endothermic if energy is a reactant and exothermic if energy is a product.

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Hi,

Dr. Lavelle noted in his syllabus "Please note we are not using the 7th edition. Students can use it but it is more expensive."

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Chels Zh 1D wrote:Generally speaking, salts are the products of acids and bases, an ionic compound composing of cation and anion.

In addition to this, salts have an overall electrical charge of 0 therefore they are electrically neutral.

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My TA said the values will be given in the exam therefore we don't need to memorize them

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Species is referring to atoms, molecules, ions, elements, etc., being subjected to a chemical process

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In the example from this page, K is being used to calculate the concentration of a species at equilibrium.

The example asks what PPCl3 is at equilibrium.

How do you go from KP = PPCl3 PCl2 / PPCl5 to PPCl3 = KP PPCl5 / PCl2 ?

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Kc is the ratio of products/reactants at equilibrium, Q is the direction a reaction will proceed.

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The problem is:

For the complex ions listed below, determine the oxidation state and the coordination number of the central metal ion.
[Pt(CN)(NH3)3]^+

My question is, how do you find the oxidation state? Also, I got the coordination number 4, is that correct?

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The method I used to practice naming ligands was I wrote the ligand on one side of a flashcard and the name of it on the back. I repeatedly went through the flashcards and looked at the name and named the ligand (checking the back to see if I was correct) or vice versa (looked at the ligand side of ...

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For part b of problem 3.25, the answer is In2S3 but for In I got +3 and for S I got +6. How do you get In2S3? Same for part d; the answer is H2Te but for H I got +1 and for Te I got +6, the answer is H2Te not H6Te.

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In order to find the number of unpaired electrons you first have to write the electron configuration. Then, you can either draw the valence orbitals or picture it in your head and see how many electrons are unpaired. For example, if the electron configuration ends with 3p^4 you would have to know th...

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(b) is not possible because l = 0 so ml must also = 0
(c) is not possible because the maximum value l can have is n - 1 and since n = 4, 4 - 1 = 3 so the maximum l can be is 3 not 4

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A dipole is a positive charge next to an equal but opposite negative charge. A dipole moment (μ) is the magnitude of the dipole.

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For each of the following ground-state atoms, predict the type of orbital (1s, 2p, 3d, 4f, etc.) from which an electron will be removed to form the +1 ion: (a) Ge; (b) Mn; (c) Ba; (d) Au.

The answers are: (a) 4p; (b) 4s; (c) 6s; (d) 6s

What method should I use to get the correct answers?

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Do we have to know the Angstroms for chemical bonds or just that double bonds are shorter than single bonds and triple bonds are shorter than double bonds?

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Anions gain electrons, cations lose electrons

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Problem 57 from Chapter 1 in the textbook:

Lines in the Balmer series of the hydrogen spectrum are observed at 656.3, 486.1, 434.0, and 410.2 m. What is the wavelength of the next line in the series?

How do you start off/solve this problem?

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Do we have to know how to draw electron configurations for the exam on Wednesday?

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When light undergoes reflection, refraction, and diffraction it acts as a wave. When it packages its energy in small quanta it acts as a series of photons.

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I'm going through the "The Quantum World" notes in the course reader and after reviewing the first worked example: "The following questions relate to the same metal used in a series of photoelectric experiments. If 3.61 x 10^-19 J is required to remove an electron with zero kinetic en...

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A wave like property that electrons have is the discrete atomic energy levels. Another wave like property that electrons have is the diffraction of electrons from crystal planes in solid materials.

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Light can't simultaneously be a pure wave and photon therefore there are not any instances where it acts as both.

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