CHEMISTRY COMMUNITY

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So we know which form of R to use based off of the formula sheet provided to us? Can someone clairfy the possible unit values (atm or joules or Torr) per form of R?

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Just to clarify/confirm - environment, fossil fuels, and alternative fuels will not be on the midterm exam? If they will be, what topics are they associated with...thermodynamics?

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Will we need to be able to identify the difference between statistical vs residual entropy on the midterm?

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Both Q and K are calculated using the same equations - Q can calculate a particular point of the reaction / K calculates the reaction at equilibrium!

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Reading the textbook and working through the practice problems provided in each section - in addition to the homework problems per week - really helped better my understanding behind the details of the ideal gases and thermodynamics!!

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Will the bond dissociation energies definitely be given?

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Are the basic units for enthalpy always kJ?

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Multiplying the equilibrium constants of the two equations gives you the final outcome of the reaction

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Is the ICE table used purely to find missing concentrations?

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It varies based on reaction. You know whether Kp and Kc are the same based on your calculations!

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I think we are fine labeling the units for Kp as either bars or atmosphere. Whereas, Kc is identified in molar/moles.

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K is found using concentrations at equilibrium, BUT to calculate Q do we just use the initial concentrations or concentrations at any given time?

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By doubling the the number of moles of a specific molecule, do the coefficients and exponents work proportional to one another in order to maintain the equilibrium of K?

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Can someone further explain how to rank strong acids versus bases?

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Intramolecular forces are the forces that hold atoms together within a molecule. Intermolecular forces are forces that exist between molecules.

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The next test, following the midterm, is week 9 - after Thanksgiving. Can anyone provide a list of the remaining topics (dipole moments, sigma/pi bonds, and electronegativity) that will be covered on the week 9 test?

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Do dipole moments always rely on whether a molecule is polar or nonpolar?

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Why is it a tetrahedral and not a trigonal planar? Are there other examples of this other than with H3O+?

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When you say regions of electron density, are you referring to using the periodic table? Could you explain how to look for this please?

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^What are the exceptions for the octet rule in triple bonds?

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Does anyone have a good way to remember the degrees per shape?

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Weak (longer) bonds are easily broken and more likely involved in reaction.
Strong (shorter) bonds are harder to break and less reactive.

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Strength of a bond is measured by its' dissociation energy (the energy required to break a bond)

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What is covalent bond dissociation? Could someone please simplify the process... thank you!!

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Can someone please explain whether dipole moments are always polar or not? Thanks!!

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I find it helpful to read the textbook, but I also get confused a lot after! I then will watch Crash Course on Youtube for whatever concept it is that I am confused by. They often work through examples and explain the topic step by step. I think it really helps for clarity and betters my understandi...

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How can we apply paramagnetism in chemistry 14A? Can someone possible provide an example? I would appreciate it!!

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Elements increase in atomic size down the periodic table, as they gain shells, and decrease across the periodic table (from left to right)!

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Atomic radius... - increases in atomic size down the periodic table, as shells increase - decreases across the periodic table from left to right Ionization energy (the energy needed to add to remove an electron)... - decreases down the periodic table - increases across the period table from left to ...

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The equation Ek=hv-work will always help you find your solution, in this case!

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I understand that... The E in E = hv represents the energy of a photon. The E in Ek = 1/2(mv^2) represents the excess energy after an electron is removed from a metal. ...but, can someone please clarify what the specific values are that we need to assign as hv and 1/2(mv^2)? Sorry if this was alread...

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SHELL --> n = 1,...,infinity
SUBSHELL --> l = {0,...,n-1}
ORIENTATION OF ORBITAL SPIN --> ml = {-l,...+l}
SPIN --> ms = {-1/2, +1/2}

These are the fundamental rules needed to determine sub-shell notation, electron configuration, valence electrons, unpaired electrons, etc.!

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I know we have not needed to yet, but will we need to be able to apply Schrodinger's Equation on the midterm exam?

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Old chemists never die, they just stop reacting.

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Why do chemists like nitrates so much?
They're cheaper than day rates.

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Have you heard the one about a chemist who was reading a book about helium?
He just couldn't put it down.

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I have been reviewing each concept after lecture by watching the Crash Course videos on YouTube. They have been helpful in clarifying and breaking down what is being taught in class. I definitely recommend watching a few. Hope it helps!

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Does anyone know roughly how long the midterm exam will be?

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I am a pre-med, first year student who needed this advice, especially regarding the chemistry series. Thanks so much!!

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In drawing out an orbital diagram for an element, can someone explain the easiest steps to take? I know you have to take the electron configuration and work from there, but how can you be sure that your orbital diagram correctly translates from the electron configuration?

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Is O2 or P4 the limiting reactant for part a? Can someone please explain which and why. Thanks so much!

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Going off of what the initial post asked, does anyone know a more simple, yet speedier way to balance even the more general equations? Any faster method than just moving through the equation, element by element?

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Are we definitely provided a periodic table for the test? We are also permitted to use calculators during the test, correct?

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Problem F5 asks for the mass percentage composition of L-carnitine, C7H15NO3, a compound taken as a dietary supplement to reduce muscle fatigue. My first step was to take each element and multiple its' coefficient by its' molar mass: 7C --> 7(12.01) = 84.07 15H --> 15(1.01) = 15.15 1N --> 1(14.007) ...

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