Search found 57 matches
- Tue Feb 26, 2019 5:39 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Entropy of Fusion
- Replies: 3
- Views: 419
Entropy of Fusion
When finding the entropy of fusion of water, why do you take the entropy of fusion of the liquid state minus the entropy of fusion of the solid state, and not the other way around? Shouldn't it be final - initial state?
- Tue Feb 26, 2019 5:37 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Melting/Spontaneous Processes
- Replies: 3
- Views: 533
Melting/Spontaneous Processes
In the textbook, it says Because the solid and liquid phases are in equilibrium at the melting point, you should expect to find that ΔG=0 at 0.°C. Above that temperature the melting of the solid state is favored, so you should expect that ΔG will be negative at 10.°C. Why does ΔG have to be negative...
- Wed Feb 13, 2019 2:12 pm
- Forum: Phase Changes & Related Calculations
- Topic: 4.18J or 0.38J
- Replies: 8
- Views: 1287
Re: 4.18J or 0.38J
0.38 is the specific heat capacity of copper, not water.
- Sun Feb 10, 2019 8:00 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Using R
- Replies: 10
- Views: 1055
Re: Using R
Units! Check the units the given values are using.
- Sun Feb 10, 2019 7:59 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: 4A.9 7th Edition
- Replies: 3
- Views: 476
Re: 4A.9 7th Edition
Heat capacity is usually a given value. If you see something like this on the midterm, there should be a table or something somewhere that has the heat capacity for a bunch of different things.
- Sun Feb 10, 2019 7:49 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: 4A.9 7th Edition
- Replies: 3
- Views: 476
Re: 4A.9 7th Edition
Heat capacity is usually a given value. If you see something like this on the midterm, there should be a table or something somewhere that has the heat capacity for a bunch of different things.
- Sun Feb 10, 2019 7:48 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: midterm
- Replies: 3
- Views: 406
Re: midterm
You can search "hotdog" to find it. I don't think any solutions are posted though. Also I think someone put a link in the endorsed "midterm" post in this section.
- Sun Feb 03, 2019 8:20 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Enthalpy of Formation
- Replies: 2
- Views: 362
Re: Enthalpy of Formation
Enthalpy of formation can be negative or positive, yes.
- Sun Feb 03, 2019 8:19 pm
- Forum: Phase Changes & Related Calculations
- Topic: State functions and Energy
- Replies: 3
- Views: 454
Re: State functions and Energy
Dr. Lavelle is usually pretty good about always putting something into a class example or homework problem if we need to know it, so if you haven't seen any homework problems on it and we haven't talked about it in class, we probably won't be tested on it.
- Sun Feb 03, 2019 8:16 pm
- Forum: Phase Changes & Related Calculations
- Topic: Water vapor vs boiling water burns
- Replies: 3
- Views: 488
Re: Water vapor vs boiling water burns
Thanks for clarifying this, guys. I was also confused about this during lecture.
- Sun Jan 27, 2019 10:03 pm
- Forum: Ideal Gases
- Topic: pH and pOH
- Replies: 18
- Views: 1999
Re: pH and pOH
If it doesn't tell you explicitly, just go off of what's present in the equation. Which do you end up with in the products - H3O+ or OH-? If it's OH-, then pOH. If it's H3O+, then pH. And of course you can always calculate one once you have the other using the equation pH + pOH = 14.
- Sun Jan 27, 2019 10:00 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: First row question
- Replies: 3
- Views: 491
Re: First row question
They don't have a large enough impact on the pH to significantly change your answer, whether you include them in the calculations or not.
- Mon Jan 21, 2019 11:09 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Finding Concentrations of H3O+ and OH-
- Replies: 2
- Views: 2127
Finding Concentrations of H3O+ and OH-
We did an example in class on Monday of last week where we had: 0.0030M Ba(OH)2 (aq) at 25 degrees Celsius Then we needed to find the concentrations of H3O+ and OH- in the solution. So, the reaction is as follows: Ba(OH)2 --> Ba2+(aq) + 2OH- Since Ba(OH)2 is a strong base, we assume it dissolves com...
- Mon Jan 21, 2019 10:40 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: le chatliers
- Replies: 3
- Views: 341
Re: le chatliers
Yep. Just to add on, the only things in a reaction you have to worry about when we're calculating K values are the gases and aqueous solutions.
- Mon Jan 21, 2019 10:39 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: partial pressures vs. concentrations
- Replies: 3
- Views: 367
Re: partial pressures vs. concentrations
I also think it depends on what the question is asking for. I'm pretty sure that on the exam, Professor Lavelle will specify which one he's looking for. Since the only two states we can use in Kc/Kp calculations are gases and aqueous solutions anyway, we're bound to have problems with only gases rea...
- Mon Jan 21, 2019 10:36 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 12.39
- Replies: 2
- Views: 316
Re: 12.39
This is part of the problems we'll have to do for the test. Calculating Ka/Kb values for substances based on the already known Ka/Kb values of similar compounds/molecules.
- Sun Jan 13, 2019 10:38 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: equilibrium
- Replies: 4
- Views: 432
Re: equilibrium
Dr. Lavelle also said in lecture that he doesn't like when books/students use this phrasing, and prefers the more accurate "this reaction favors the products (sits to the right)" or "this reaction favors the reactants(sits to the left)".
- Sun Jan 13, 2019 10:37 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Le Chatelier's Principle
- Replies: 3
- Views: 405
Re: Le Chatelier's Principle
Just in case this helps focus your studying - while understanding the basic concept is important, Dr. Lavelle did mention in lecture that we don't need to know Le Chatelier's principle.
- Sun Jan 13, 2019 10:35 pm
- Forum: Ideal Gases
- Topic: When to Use PV=nRT
- Replies: 8
- Views: 1719
Re: When to Use PV=nRT
Dr. Lavelle also did a practice problem in lecture on Friday showing when we would use PV=nRT, using V and n to represent concentration.
- Sat Dec 08, 2018 11:14 pm
- Forum: Naming
- Topic: adding "ion" at the end of a name
- Replies: 4
- Views: 456
Re: adding "ion" at the end of a name
I also had this question. Thanks for asking it!
- Sat Dec 08, 2018 10:56 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles
- Replies: 3
- Views: 533
Re: Bond Angles
That makes sense. Thanks for your help!
- Sat Dec 08, 2018 10:10 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles
- Replies: 3
- Views: 533
Bond Angles
Hey guys! Quick question on bond angles in molecular shapes. When we're asked about the bond angles in a molecule, are we providing only the angle between the atoms branched off the center, or also the angles between those atoms and the central atom? To clarify: If you have AX2E, a bent molecule, is...
- Tue Dec 04, 2018 12:40 am
- Forum: Naming
- Topic: "(en)" and "(edta)"?
- Replies: 3
- Views: 400
Re: "(en)" and "(edta)"?
Okay. Thanks!
- Mon Dec 03, 2018 9:40 pm
- Forum: Naming
- Topic: "(en)" and "(edta)"?
- Replies: 3
- Views: 400
"(en)" and "(edta)"?
In 9C.9 (7th) there is a coordination compound [PtCl2(en)2] 2+ and [Cr(edta)] -
What do "en" and "edta" mean in this context?
What do "en" and "edta" mean in this context?
- Mon Dec 03, 2018 9:36 pm
- Forum: Naming
- Topic: Latin Stems
- Replies: 1
- Views: 230
Re: Latin Stems
I think it would suffice to just make note of any examples the textbook uses in the chapter/practice problems. We will probably only encounter the most common ones (like Fe).
- Mon Dec 03, 2018 9:30 pm
- Forum: Naming
- Topic: 9C.5 7th Edition
- Replies: 2
- Views: 336
9C.5 7th Edition
I was wondering if someone could explain this question to me. It says: "Which of the following ligands can be polydentate?" a) HN(CH2CH2NH2)2 b)C03 2- c)H20 d)oxalate For the answers, the book says: a) Has 3 N atoms w/ a lone pair, so can be tridentate b) can bind to a metal ion through ei...
- Mon Dec 03, 2018 9:23 pm
- Forum: Naming
- Topic: 9c.1 7th Edition
- Replies: 3
- Views: 191
Re: 9c.1 7th Edition
Great! Thank you!
- Mon Dec 03, 2018 9:07 pm
- Forum: Naming
- Topic: 9c.1 7th Edition
- Replies: 3
- Views: 191
9c.1 7th Edition
Hello! On part c0 of this question (pg 731), the answer is aquapentacyanocobaltate(III) ion. Is it written "cobaltate" and not simply "cobalt" because of the negative charge of the compound? If so, I assume that's why a) is also hexacyanoferrate(II) ion. How would you name that c...
- Sun Dec 02, 2018 8:28 pm
- Forum: Naming
- Topic: 7.29 6th edition Cobalt vs Colbaltate
- Replies: 1
- Views: 297
Re: 7.29 6th edition Cobalt vs Colbaltate
If the coordination compound is overall negatively charged, you add "ate" to the end of it.
- Sun Dec 02, 2018 8:25 pm
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: LDF
- Replies: 7
- Views: 1716
Re: LDF
Yes. ALso, I believe LDF is interchangeable with quite a few other names (such as induced-dipole induced-dipole), so if you look those up you'll be able to recognize that IMFs that occur in all molecules.
Also, it's helpful for the tests.
Also, it's helpful for the tests.
- Sun Dec 02, 2018 8:21 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: 4.95 6th ed
- Replies: 3
- Views: 412
Re: 4.95 6th ed
You'd probably want to draw the most stable structure (a good idea generally). So, the structure in which the most atoms in the molecule have a formal charge of 0.
- Sun Dec 02, 2018 8:17 pm
- Forum: Hybridization
- Topic: S Hybridization?
- Replies: 5
- Views: 507
Re: S Hybridization?
Yes. We don't do it often on tests/homework I assume because it's just really simple. Hydrogen, for example, would just be "s". It's also kind of rare of an atom in a larger molecule (that isn't Hydrogen) to have only one bond and no lone pairs, so you don't see it too often.
- Sun Dec 02, 2018 8:15 pm
- Forum: Hybridization
- Topic: Hybridization of pi bonds
- Replies: 3
- Views: 412
Re: Hybridization of pi bonds
You don't have to worry about finding the hybridization of specific types ("pi" or "sigma") of bonds. If an atom shares a triple bond with another atom, that atom has a sigma bond and two pi bonds. But it would still only get 1 level of hybridization (in this case, "s")...
- Sun Dec 02, 2018 8:13 pm
- Forum: Hybridization
- Topic: Double and Triple Bonds
- Replies: 17
- Views: 4361
Re: Double and Triple Bonds
Nope. The hybridization of an atom with a single bond would be the same as an atom with a triple bond (all other things being equal). Hybridization is really more about regions of electrons, so making a bond between the same two atoms stronger wouldn't change hybridization in the way a lone pair or ...
- Sun Dec 02, 2018 8:12 pm
- Forum: Hybridization
- Topic: Hybridization of CH3CN
- Replies: 2
- Views: 7860
Re: Hybridization of CH3CN
So if the Nitrogen atom in that molecule has a lone pair and is triple bonded to carbon, then it's hybridization would be sp, because there are two regions of electron density (the triple bond with carbon and the lone pair on Nitrogen itself). The Carbon atom bonded to N has a hybridization of sp, b...
- Sun Dec 02, 2018 8:06 pm
- Forum: Hybridization
- Topic: Sigma bonds
- Replies: 9
- Views: 944
Re: Sigma bonds
I know that when you have a multiple bond like a double or a triple bond, only the first one is a sigma, and all the others are pi bonds. E.g. a triple bond contains one sigma and two pi bonds. But I'm not sure why that is the case structurally.
- Sun Dec 02, 2018 8:04 pm
- Forum: Hybridization
- Topic: Hybridization of bonds abbreviation
- Replies: 2
- Views: 350
Re: Hybridization of bonds abbreviation
Someone who worked on this problem also posted a possible answer in the question "Lyndon's practice question 17"
- Wed Nov 28, 2018 4:06 pm
- Forum: Electronegativity
- Topic: Ionic Character
- Replies: 7
- Views: 1572
Ionic Character
In the textbook, there's a question that says "In which of the following compounds do the bonds have greater ionic character? a)P4O10 b)PCl3". The answer is A. I know that ionic character is determined by the difference in the atoms' electronegativity, but since P seems an equal distance f...
- Sun Nov 18, 2018 11:48 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: 2E.1 7th Edition
- Replies: 2
- Views: 280
Re: 2E.1 7th Edition
You could have more than one lone pair that would either balance it out like a square planar molecule or exist on a different access, and therefore not affect the bond angles.
- Sun Nov 18, 2018 11:47 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Distorted Bond Angles
- Replies: 3
- Views: 3144
Re: Distorted Bond Angles
For an example, you can take a look at a water molecule, which would have 180 degree bond angles if not for the lone pairs which cause the ultimate shape to be bent instead of linear, and the bond angles to be smaller.
- Sun Nov 18, 2018 11:45 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles in 7E 2E.13.b
- Replies: 4
- Views: 485
Re: Bond Angles in 7E 2E.13.b
The solution manual says 109.5, so that’s probably your safest bet. I think that double bonds don’t affect bond angles as much as, say, lone pairs do.
- Sun Nov 18, 2018 11:43 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Position of Lone Pairs in H20
- Replies: 3
- Views: 900
Re: Position of Lone Pairs in H20
That’s a good question. It would probably be because of the polarity of the molecule as a whole and its desire to stay that way.
- Sun Nov 11, 2018 4:04 pm
- Forum: Resonance Structures
- Topic: Drawing resonance structures
- Replies: 5
- Views: 767
Re: Drawing resonance structures
You'd probably want to draw all of them just to be safe, but there are usually only a few resonance structures for the molecules we're working with.
- Sun Nov 11, 2018 4:01 pm
- Forum: Bond Lengths & Energies
- Topic: Covalent Radius
- Replies: 3
- Views: 601
Re: Covalent Radius
Another important note here is that a covalent bond is the sharing of electrons. So when two atoms are covalently bonded, their closeness to one another is because they are sharing electrons, which contribute to their radii. So there may be a sort of "overlap" of those outer valence shells...
- Sun Nov 11, 2018 3:58 pm
- Forum: Bond Lengths & Energies
- Topic: Molar mass and attractive interactions
- Replies: 3
- Views: 436
Re: Molar mass and attractive interactions
Since an element with a bigger molar mass has more protons to give it that high mass, it also has more electrons. I would assume that that would be one reason.
- Sun Nov 04, 2018 11:53 pm
- Forum: Resonance Structures
- Topic: Resonance structures
- Replies: 7
- Views: 905
Re: Resonance structures
They're a related concept. Molecules with resonance will ultimately form hybrid structures of all the different kinds of bonds they can make.
- Sun Nov 04, 2018 11:51 pm
- Forum: Ionic & Covalent Bonds
- Topic: electronegativity troughout a covalent bond
- Replies: 3
- Views: 474
Re: electronegativity troughout a covalent bond
I think that overall the ultimate goal of two atoms in a covalent bond is to become neutral, even though they don't have the electrons to make that happen (fill the valence shell) independently of one another, which is why they share electrons, to become one, mostly neutral, molecule.
- Sun Nov 04, 2018 11:49 pm
- Forum: Ionic & Covalent Bonds
- Topic: electronegativity difference
- Replies: 4
- Views: 586
Re: electronegativity difference
This is kind of a tricky one. In determining which molecule is more covalent, you do want to look to electronegativity, but almost more importantly, you want to look to the proximity of the atoms in the molecule. The closer the electronegativity values of the atoms in the molecule are to one another...
- Sun Nov 04, 2018 11:43 pm
- Forum: Ionic & Covalent Bonds
- Topic: Ionization Energies
- Replies: 13
- Views: 3720
Re: Ionization Energies
There are occasionally exceptions to the trend rules for ionization energy, electronegativity, and atomic radii, but since the general trend for ionization energy is that it increases going up and to the right, and I don't know of any exceptions where an element would have a higher ionization energy...
- Sun Nov 04, 2018 11:41 pm
- Forum: Ionic & Covalent Bonds
- Topic: Nitrogen or Oxygen as Central Atom
- Replies: 2
- Views: 332
Re: Nitrogen or Oxygen as Central Atom
Actually, the central atom is typically decided by which atom is the least electronegative. That would be Nitrogen in this case, so the very basic outline of N2O would be N-N-O (not taking into account the eventual double bonds/lone pairs you'd add in drawing the structure).
- Sun Nov 04, 2018 11:38 pm
- Forum: Ionic & Covalent Bonds
- Topic: Ionic and Covalent
- Replies: 3
- Views: 496
Re: Ionic and Covalent
2 main ways: 1- covalent is between 2 nonmetals. Ionic is generally between nonmetal and metal. 2- covalent bond is the sharing of electrons between two atoms/molecules i.e. they both share one pair of electrons to complete their valence shell. Ionic bond is the giving of electrons from one atom/mol...
- Mon Oct 29, 2018 1:22 am
- Forum: Electronegativity
- Topic: Kr
- Replies: 3
- Views: 507
Re: Kr
As a general rule, elements with a full outer valence shell want to stay that way. Taking away an electron from a full outer valence shell is very difficult due to the amount of energy required to kick the element out of its ideal state (a full outer valence shell).
- Mon Oct 29, 2018 1:20 am
- Forum: Electronegativity
- Topic: Periodic Trends
- Replies: 8
- Views: 857
Re: Periodic Trends
I don't think so. I believe that that rule is applicable to all elements in the periodic table.
- Mon Oct 29, 2018 1:16 am
- Forum: Ionic & Covalent Bonds
- Topic: Question 2B.3 part d
- Replies: 2
- Views: 218
Re: Question 2B.3 part d
Yeah I believe BrF3 is one of those weird molecules that is an exception to the rule.
- Sun Oct 21, 2018 11:56 pm
- Forum: Properties of Light
- Topic: SI Units
- Replies: 6
- Views: 640
Re: SI Units
It's probably good to know all the meter/liter/gram conversions we covered in week one. For example, nano-, mega-, pico-. Additionally, the meaning of each unit is important to determine final units in a problem - see Hertz, Joules.
- Sun Oct 21, 2018 11:52 pm
- Forum: Properties of Light
- Topic: Visible Light
- Replies: 5
- Views: 495
Re: Visible Light
Between 400-700 nm. For the record, the textbook has a really nice diagram (In the 7th Ed., page 6, figure 1A.9) that shows the ranges for all the different types of radiation, including visible light.
- Sun Oct 21, 2018 11:49 pm
- Forum: Properties of Light
- Topic: Quantum Equations
- Replies: 3
- Views: 426
Re: Quantum Equations
It's not necessarily uncommon. Sometimes, you'll need to use multiple equations to get an answer. For example, if you need to find wavelength but you're only given Energy, you can use E=hv to find the frequency (v) and then use that in the equation c=(frequency)(wavelength).