Search found 108 matches
- Mon Mar 08, 2021 12:36 pm
- Forum: First Order Reactions
- Topic: 1st Order Reactions
- Replies: 29
- Views: 1979
Re: 1st Order Reactions
Both graphs describe 1st order reactions, the difference is that one expresses the integrated rate law while the other is based on the differential rate law.
- Mon Mar 08, 2021 12:34 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Rate Laws for Slow Step/Overall
- Replies: 14
- Views: 947
Re: Rate Laws for Slow Step/Overall
You would not include intermediates in the overall rate law. Usually, the intermediate is also in an elementary step that is fast reversible, so you can come up with an expression for the intermediate in terms of other species in the fast reversible elementary step and then replace the intermediate ...
- Mon Mar 08, 2021 12:31 pm
- Forum: Zero Order Reactions
- Topic: kind of reaction
- Replies: 25
- Views: 1217
Re: kind of reaction
A zero order reaction has a constant rate; it does not depend on concentration. When you plot concentration vs time for a 0 order reaction, the resultant graph should be a line with negative slope, and the slope = -k.
- Mon Mar 08, 2021 12:26 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Molecularity and Mechanism
- Replies: 2
- Views: 228
Re: Molecularity and Mechanism
As you stated, the reaction mechanism is the specific pathway or steps through which a reaction occurs. Those steps are typically elementary reactions, and molecularity is a way of classifying these elementary reactions based on the number of species involved in the reaction. The molecularity of an ...
- Mon Mar 08, 2021 12:23 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Rate Limiting Steps
- Replies: 6
- Views: 499
Re: Rate Limiting Steps
For a reaction mechanism that is proposed to have multiple steps (multiple elementary reactions that comprise the overall reaction), the rate-limiting step is the elementary reaction with the slowest rate. This slowest step is the step that determines the rate of the entire reaction, so the rate law...
- Mon Mar 01, 2021 11:01 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Potential Solutions Manual Error 6M1
- Replies: 2
- Views: 204
Re: Potential Solutions Manual Error 6M1
Since E(cell) for the given cell is negative, this means that the left half-cell is the cathode and the right half-cell is the anode because of the way the cell potential is reported. This is what the textbook says about this (Focus 6L.3, pg 551): "In summary, the sign of the cell potential rep...
- Mon Mar 01, 2021 10:53 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Calculating Ka from Redox Reaction
- Replies: 2
- Views: 271
Re: Calculating Ka from Redox Reaction
You need to take the square root of the K value because the original reaction you use is 2HF --> 2H+ + 2F-, but the reaction for Ka is HF --> H+ + F-. Dividing the stoichiometric coefficients by 2 is the same as raising the K value to the power of 1/2 (taking the square root), so the result is the K...
- Mon Mar 01, 2021 10:49 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Textbook 6K.5
- Replies: 2
- Views: 175
Re: Textbook 6K.5
a) Because you know that Br- --> BrO3- is the oxidation reaction since the oxidation state of Br changes from -1 to +5, the 2 remaining species must be involved in the reduction reaction. Therefore, O3 --> O2 is the unbalanced reduction half-reaction. b) I think it's just a rule of thumb to always b...
- Mon Mar 01, 2021 10:41 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 6L7a
- Replies: 3
- Views: 236
Re: 6L7a
For 6L.7 (a), you essentially have to come up with 2 half-reactions (one oxidation and one reduction) so that when combined the overall reaction gives AgBr(s) <--> Ag+(aq) + Br-(aq). For the oxidation half-reaction: Ag(s) + Br-(aq) --> AgBr(s) + e- For the reduction half-reaction: Ag+(aq) + e- --> A...
- Mon Mar 01, 2021 10:37 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: E(cell) negative
- Replies: 7
- Views: 1080
Re: E(cell) negative
Yes, if the E(cell) for the given reaction as written is negative, it means that the reverse reaction is favorable :)
- Wed Feb 24, 2021 10:37 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Order for Species in Cell Diagram
- Replies: 1
- Views: 138
Order for Species in Cell Diagram
When an electrode has 2 species in the same phase, in what order do we list the species in the cell diagram? For example, for Fe2+ (aq) —> Fe3+ (aq) + e- is the electrode Pt(s)|Fe2+(aq), Fe3+(aq) or the other way around? What is the rule for this?
- Mon Feb 22, 2021 12:06 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Anode and Cathode
- Replies: 4
- Views: 333
Re: Anode and Cathode
I believe the convention is to always place the anode on the left in the cell diagram, and the cathode always goes to the right.
- Mon Feb 22, 2021 12:05 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: sapling week7/8 #9
- Replies: 1
- Views: 106
Re: sapling week7/8 #9
You would just look up the standard potentials for the half reactions Cr/Cr3+ and Ag/Ag+ in the table. After you find these values, change the sign of E naught for one of the half-reactions so that adding the 2 values yields a positive voltage. Hope this helps!
- Mon Feb 22, 2021 12:00 pm
- Forum: Balancing Redox Reactions
- Topic: Oxygen
- Replies: 12
- Views: 712
Re: Oxygen
The oxidation number of oxygen in O2 and O3 is 0, and in most other compounds it will have an oxidation number of -2. The exception to this rule is peroxides, in which oxygen will have a -1 oxidation number.
- Mon Feb 22, 2021 11:57 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Entropy and Gibbs Free Energy
- Replies: 6
- Views: 423
Re: Entropy and Gibbs Free Energy
If the entropy of the universe increases, then the process is spontaneous/thermodynamically favorable (has a Gibbs free energy value that is negative). If the entropy of the universe does not increase in the course of the reaction/process, then it is not spontaneous/thermodynamically favorable. It h...
- Mon Feb 22, 2021 11:55 am
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Voltage
- Replies: 4
- Views: 252
Re: Voltage
Voltage is the same thing as the maximum potential difference but not the same as maximum work. However, voltage/maximum potential difference are related to maximum work through the equation wmax = -nFE. Hope this helps!
- Wed Feb 17, 2021 11:46 am
- Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
- Topic: Mass vs Entropy
- Replies: 8
- Views: 2383
Re: Mass vs Entropy
To add on, more massive atoms have larger molar entropy because they have a greater number of fundamental particles (electrons, protons, etc.), so they have a greater number of possible states.
- Wed Feb 17, 2021 11:44 am
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: textbook question 4B.3b
- Replies: 5
- Views: 333
Re: textbook question 4B.3b
Yes, that's the equation you use! Delta U = 982 J = 492 J + w, so w = 982 J - 492 J = 490 J. Hope this helps!
- Wed Feb 17, 2021 11:39 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Textbook 5J.15
- Replies: 5
- Views: 402
Re: Textbook 5J.15
To find K at 150 degrees celsius, you would first need to find delta S naught and delta H naught of the reaction using the standard values in Appendix 2A. Then, you would plug those into delta G naught = delta H naught - T(delta S naught), with T = 150+273 = 423K. Delta G naught = -RTlnK, so K = e^(...
- Wed Feb 17, 2021 11:35 am
- Forum: Student Social/Study Group
- Topic: Sapling on midterm 2
- Replies: 6
- Views: 359
Re: Sapling on midterm 2
Yes, all of Sapling 5/6 will be on the midterm, plus the questions from Sapling 3/4 not relating to Hess's Law, bond ethalpies, and delta H of formation.
- Wed Feb 17, 2021 11:33 am
- Forum: Third Law of Thermodynamics (For a Unique Ground State (W=1): S -> 0 as T -> 0) and Calculations Using Boltzmann Equation for Entropy
- Topic: Standard molar entropy
- Replies: 4
- Views: 272
Re: Standard molar entropy
When these problems talk about fundamental particles, they are referring to the number of protons, neutrons, and electrons in the atom. An atom with a greater molar mass and a larger number of electrons, protons, etc. will have a higher standard molar entropy, as there are more possible positions. H...
- Mon Feb 08, 2021 12:07 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Using T1 and T2 for an isothermal process
- Replies: 4
- Views: 322
Re: Using T1 and T2 for an isothermal process
The equations with T1 and T2 Prof. Lavelle discussed today are for calculating delta S when the temperature is changing. To calculate delta S for isothermal expansions, we would use delta S = qrev/T rather than delta S = nCpln(T2/T1). Hope this helps!
- Mon Feb 08, 2021 12:05 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: q_rev
- Replies: 5
- Views: 278
Re: q_rev
I believe qrev refers to the q value for the reversible isothermal expansion!
- Mon Feb 08, 2021 12:03 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Reversible reaction effeciency
- Replies: 4
- Views: 226
Re: Reversible reaction effeciency
I believe reversible reactions are considered more efficient because less energy as heat is lost to the surroundings due to the process being done slowly, and maximum work is done.
- Mon Feb 08, 2021 11:58 am
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Role of delta Hrxn and T in entropy changes
- Replies: 1
- Views: 104
Role of delta Hrxn and T in entropy changes
At the end of lecture, Prof. Lavelle mentioned that delta Hrxn plays an important role in entropy changes at lower temperatures, but I'm not sure why. Wouldn't delta Hrxn be more significant to entropy changes at higher temperatures?
- Mon Feb 08, 2021 11:27 am
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Which R to use
- Replies: 42
- Views: 3087
Re: Which R to use
You would use 8.314 because that value would give you work with units of Joules.
- Mon Feb 01, 2021 2:04 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Qp = ΔH
- Replies: 6
- Views: 362
Re: Qp = ΔH
Qp = delta H because by definition, delta H is the change in energy due to heat at a constant pressure.
- Mon Feb 01, 2021 12:10 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Do CC work for bruin cast videos
- Replies: 6
- Views: 272
Re: Do CC work for bruin cast videos
I don't have an option for CC either :(
- Mon Feb 01, 2021 12:07 pm
- Forum: Calculating Work of Expansion
- Topic: Negative Sign in w = -PdeltaV
- Replies: 5
- Views: 278
Re: Negative Sign in w = -PdeltaV
Here is the explanation from the textbook: "The work done by the expanding gas is Pexternal * delta V. At this point, you need to adopt the sign convention. When a system expands, it loses energy as work. so, when delta V is positive (an expansion), w is negative. Therefore, w = -Pexternal * de...
- Mon Feb 01, 2021 12:00 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: External Pressure
- Replies: 32
- Views: 1108
Re: External Pressure
External pressure refers to the pressure acting outside the system (on the outside of the piston), and it is the pressure that the system must push against to do work.
- Mon Feb 01, 2021 11:54 am
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: What P when solving for work?
- Replies: 5
- Views: 125
Re: What P when solving for work?
We use external pressure!
- Mon Feb 01, 2021 11:53 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Negative Heat Capacities
- Replies: 9
- Views: 424
Negative Heat Capacities
Can heat capacities be negative? If so, what do negative heat capacities mean?
- Mon Jan 25, 2021 12:45 pm
- Forum: Phase Changes & Related Calculations
- Topic: States at Standard Temp / Pressure
- Replies: 6
- Views: 206
Re: States at Standard Temp / Pressure
I think it's a good idea to know the phases of some of the common elements/molecules, but I don't think Prof Lavelle will expect us to know the standard states of some of the more obscure ones.
- Mon Jan 25, 2021 12:41 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: qsys v. qsurr
- Replies: 7
- Views: 361
Re: qsys v. qsurr
Typically, the reaction itself is considered the system, and the solvent, typically water, inside the calorimeter is considered the surroundings.
- Mon Jan 25, 2021 12:38 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: endo/exothermic reactions
- Replies: 13
- Views: 479
Re: endo/exothermic reactions
Hi!
In general, breaking bonds is an endothermic process because it requires an input of energy. For an endothermic reaction, the amount of energy required to break the bonds in the reaction will be larger than the energy released form bond formation.
In general, breaking bonds is an endothermic process because it requires an input of energy. For an endothermic reaction, the amount of energy required to break the bonds in the reaction will be larger than the energy released form bond formation.
- Mon Jan 25, 2021 12:32 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Clarification on the sign of q
- Replies: 3
- Views: 189
Re: Clarification on the sign of q
In this case, the system would be the chemical reaction itself, and the surroundings would be the solution inside the calorimeter. Since qp = m*Cp*(delta T) calculates heat with respect to the water/solution surrounding the reaction, it is qsurr. To find qsys (q of the reaction itself), you would ha...
- Mon Jan 25, 2021 12:27 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Textbook 4E.7 part b
- Replies: 3
- Views: 133
Re: Textbook 4E.7 part b
As the previous answer stated, multiplying the bond enthalpy for the O-H bond by 2 just means that you have 2 O-H bonds that are being broken. It helps to draw out the lewis structures of the molecules in question for the bond enthalpy problems :)
- Wed Jan 20, 2021 12:42 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: amphoteric vs amphiprotic
- Replies: 10
- Views: 339
Re: amphoteric vs amphiprotic
As the previous answers stated, an amphoteric substance can behave as both an acid and base in reactions. Amphiprotic refers to a substance that can donate and accept H+ ions (protons). Amphiprotic substances are amphoteric, but amphoteric substances aren't always amphiprotic because some acids and ...
- Wed Jan 20, 2021 12:37 pm
- Forum: Phase Changes & Related Calculations
- Topic: Phase Changes of Water Graph
- Replies: 7
- Views: 373
Re: Phase Changes of Water Graph
Like the previous answer stated, the enthalpy of vaporization is always greater than the enthalpy of fusion because a phase change from solid to liquid only weakens the intermolecular attractions enough so that the molecules can slide around each other, but liquid to gas requires the intermolecular ...
- Wed Jan 20, 2021 12:33 pm
- Forum: Phase Changes & Related Calculations
- Topic: Steam causing severe burns
- Replies: 5
- Views: 201
Re: Steam causing severe burns
Yes! Your analysis is definitely correct. For example, something like liquid nitrogen, which only has LDFs, will take significantly less energy/heat to vaporize compared to water as it has very weak intermolecular attractions among its molecules, so its enthalpy of vaporization will be a smaller val...
- Wed Jan 20, 2021 12:30 pm
- Forum: Phase Changes & Related Calculations
- Topic: Steam causing severe burns
- Replies: 19
- Views: 907
Re: Steam causing severe burns
It's also because your face isn't coming into contact with 1mol (around 18g) of steam at once, just a small amount of steam reaches your face. And as the previous answer stated, the steam has already come into contact with the lower-temperature air, which has cooled it down.
- Wed Jan 20, 2021 12:28 pm
- Forum: Phase Changes & Related Calculations
- Topic: Endothermic v. Exothermic
- Replies: 139
- Views: 15179
Re: Endothermic v. Exothermic
Just a side note: fusion, vaporization, and sublimation aren't really reactions because there aren't any chemical bonds being broken, they're considered phase changes and are physical changes because it's just the intermolecular attractions that are being overcome.
- Mon Jan 11, 2021 11:47 am
- Forum: Administrative Questions and Class Announcements
- Topic: Upvoting responses
- Replies: 2
- Views: 151
Re: Upvoting responses
I see a small upwards pointing arrow in the lower right corner of each reply, but I'm not sure if students can click on it.
- Mon Jan 11, 2021 11:45 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Sapling 5J.5 d)
- Replies: 3
- Views: 231
Re: Sapling 5J.5 d)
Like the previous answer stated I think it's an issue with the textbook problem and not your conceptual understanding, because you're approaching it correctly! My textbook also had 2HD(g) <--> H2(g) + D2(g).
- Mon Jan 11, 2021 11:39 am
- Forum: Administrative Questions and Class Announcements
- Topic: Audio-Visual Focus-Topics
- Replies: 2
- Views: 116
Re: Audio-Visual Focus-Topics
Yes, I believe so! Everything that's posted on the Chem 14B class website is what's offered.
- Mon Jan 11, 2021 11:33 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Textbook 5I.3
- Replies: 3
- Views: 223
Re: Textbook 5I.3
I think you're using the wrong K. I used K=160 for H2 + I2 <---> 2HI @ 500K and I got 2.1 * 10^-5 M. Hope this helps!
- Mon Jan 11, 2021 11:21 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Large Kc for Cubic Equations
- Replies: 6
- Views: 465
Re: Large Kc for Cubic Equations
It is possible to have large Kc values with the Kc expression being cubic. The cubic nature of the expression depends on what information is given in the problem. However, I don't think we'll get problems like this on any exams just because as you said it does get more complicated to solve since we ...
- Mon Jan 11, 2021 11:14 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Textbook Problem 5.35
- Replies: 1
- Views: 129
Re: Textbook Problem 5.35
Hi! For this problem, the first thing you should do is create an ICE table based on the graph. The graph tells you the initial concentrations of A (about 28 M), B (0 M), and C (0 M), and it also shows you the equilibrium concentrations of A (about 18 M), B (5 M), and C (10 M). Based on the differenc...
- Mon Jan 04, 2021 2:23 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Post Module 1A #26
- Replies: 2
- Views: 170
Re: Post Module 1A #26
The correct answer is A, equilibrium constants are useful because they are one number that gives us information about the relative concentrations of reactant and product. K is the ratio of the equilibrium concentrations of products to the reactants raised to their respective stoichiometric coefficie...
- Mon Jan 04, 2021 2:19 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Module 1A #12
- Replies: 2
- Views: 118
Re: Module 1A #12
You're correct, C is false! At equilibrium, the forward and reverse reactions do still occur, just at the same rate.
- Mon Jan 04, 2021 12:42 pm
- Forum: Administrative Questions and Class Announcements
- Topic: 14B Discussion Sections
- Replies: 4
- Views: 251
14B Discussion Sections
When will TAs officially be assigned? My discussion section is tomorrow but I don't see who my TA is on myUCLA.
- Mon Jan 04, 2021 12:35 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 5J.5 (part d) Textbook Problem
- Replies: 4
- Views: 231
Re: 5J.5 (part d) Textbook Problem
I also think this might be an error in the solutions. Prof Lavelle mentioned in one of the module videos that one of the situations in which there would be no change is if the pressure was increased by adding an inert gas (which doesn't affect the volume and therefore the concentration), but in this...
- Mon Jan 04, 2021 12:24 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Chem Equilibrium Pt.4 Post-Assess
- Replies: 4
- Views: 136
Re: Chem Equilibrium Pt.4 Post-Assess
Hi! Like the previous response stated, a negative delta H indicates an exothermic reaction, as heat is being released/lost from the reaction system. You would consider the heat that is released to be a product of the reaction. Therefore, if temperature is increased, you are essentially increasing a ...
- Mon Dec 07, 2020 10:59 am
- Forum: Quantum Numbers and The H-Atom
- Topic: probabilty of finding e- in a location
- Replies: 6
- Views: 504
Re: probabilty of finding e- in a location
^^ Yeah we only did conceptual stuff, we don't need to know how to calculate the exact probability. However, it might be helpful to know how many nodes (areas with 0 probability of electron density) each subshell in an atom has. The total number of nodes in a subshell = n-1, # of angular nodes = l, ...
- Mon Dec 07, 2020 10:54 am
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: practice problem 1D 19
- Replies: 2
- Views: 243
Re: practice problem 1D 19
Yes, those are correct! The number of orbitals in a subshell is equal to the number of possible ml values for the specific value of l. For 4p, l = 1 so ml = -1, 0, 1; therefore 4p has 3 orbitals.
- Mon Dec 07, 2020 10:40 am
- Forum: Conjugate Acids & Bases
- Topic: What is a conjugate acid or base?
- Replies: 13
- Views: 1588
Re: What is a conjugate acid or base?
A conjugate acid is the resulting species when a base accepts a proton, and a conjugate base is the species that results when an acid gives off a proton. For example, the conjugate acid of the base NH3 is NH4+, as NH3 + H+ --> NH4+. The conjugate base of H2SO4 is HSO4-, since H2SO4 donating a proton...
- Mon Dec 07, 2020 9:49 am
- Forum: Hybridization
- Topic: Book Problem F1
- Replies: 3
- Views: 140
Re: Book Problem F1
By relative orientations I think they mean the relative arrangement of the hybrid orbitals. For sp3, each of the 4 hybrid orbitals points to one corner of a tetrahedron. For sp2, each hybrid orbital points to a corner of an equilateral triangle. Hope this helps!
- Mon Dec 07, 2020 9:47 am
- Forum: Biological Examples
- Topic: Difference between Myoglobin and heme complex
- Replies: 9
- Views: 620
Re: Difference between Myoglobin and heme complex
I agree with the previous answer, the heme complex + the hystidine protein make up myoglobin.
- Mon Nov 30, 2020 11:09 am
- Forum: General Science Questions
- Topic: midterm 2 answers
- Replies: 30
- Views: 2265
Re: midterm 2 answers
Yeah I think you have to meet with your TA to go over your midterm!
- Mon Nov 30, 2020 11:00 am
- Forum: Naming
- Topic: Formula from Naming
- Replies: 3
- Views: 251
Re: Formula from Naming
The textbook has a set of rules in Focus 9C.1 (Toolbox 9C.1) for writing the formulas and naming the compounds! For writing the formula, the textbook says to write the chemical symbol of the central metal atom first and then write the symbols of the ligands in alphabetical order. For different ligan...
- Mon Nov 30, 2020 10:57 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Equatorial/ Axial Planes
- Replies: 14
- Views: 915
Re: Equatorial/ Axial Planes
You would place a lone pair on the equatorial vs axial plane based on which position would limit the number of 90 degree interactions with the other atoms in the molecule, since these interactions are unfavorable.
- Mon Nov 30, 2020 10:54 am
- Forum: Naming
- Topic: Using ido or o
- Replies: 24
- Views: 964
Re: Using ido or o
Just a heads up, the textbook uses the -ido convention but the Sapling HW uses o!
- Mon Nov 30, 2020 10:52 am
- Forum: Naming
- Topic: Sapling Homework W9 Problem#1
- Replies: 5
- Views: 299
Re: Sapling Homework W9 Problem#1
Hi! I had trouble with this one too, but the book has a helpful list of rules in Focus 9C.1 for naming coordination compounds/complexes. First, everything enclosed by the brackets is part of the complex ion. The complex ion has an overall charge of +1, as Cl is -1 and the whole coordination compound...
- Sat Nov 28, 2020 11:05 pm
- Forum: Hybridization
- Topic: Normalized vs Unnormalized hybrid orbitals
- Replies: 3
- Views: 230
Re: Normalized vs Unnormalized hybrid orbitals
So I have no clue, so I tried to research what it might be, and I'm getting conflicting answers, one of which says that it's simply perpendicular to each other (normal to each other), and the other of which says they are standardized to one another. The first definition makes the most sense to me, ...
- Sat Nov 28, 2020 5:53 pm
- Forum: Hybridization
- Topic: Normalized vs Unnormalized hybrid orbitals
- Replies: 3
- Views: 230
Normalized vs Unnormalized hybrid orbitals
What does it mean for hybrid orbitals to be normalized vs unnormalized?
- Sat Nov 28, 2020 11:21 am
- Forum: Ionic & Covalent Bonds
- Topic: lone pairs -polar molecule
- Replies: 15
- Views: 1331
Re: lone pairs -polar molecule
I don’t think you can assume that any molecule with a central atom that has lone pairs is polar. For example, XeF2 is non polar, and it has 3 lone pairs on the central atom. The lone pairs are arranged at 120 degrees to each other and the F-Xe-F bond angle is 180 degrees, so there is a 0 net dipole ...
- Mon Nov 23, 2020 2:11 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Discussion
- Replies: 2
- Views: 99
Re: Discussion
I don't think there will be discussions on Thursday or Friday, but I'm not sure if students in those discussions will have to make it up.
- Mon Nov 23, 2020 1:59 pm
- Forum: Hybridization
- Topic: regions of electron density
- Replies: 7
- Views: 401
Re: regions of electron density
Just to add on, an unpaired electron on a radical like NO2 is also considered to be a region of electron density.
- Mon Nov 23, 2020 12:58 pm
- Forum: Hybridization
- Topic: Energy Level of sp3d and sp3d2
- Replies: 2
- Views: 224
Re: Energy Level of sp3d and sp3d2
Dr. Lavelle mentioned that the energy of the hybrid orbitals is the average of the energies of the atomic orbitals used.
- Mon Nov 23, 2020 12:54 pm
- Forum: Ionic & Covalent Bonds
- Topic: Polar/ Nonpolar
- Replies: 25
- Views: 1341
Re: Polar/ Nonpolar
FionaHunter21 wrote:Are there dipole moments between all atoms with a difference in electronegativity or just the polar bonds?
I believe all bonded atoms with a difference in electronegativity exhibit a dipole, but the magnitude/strength of the dipole is given by mu = |q|*d (charge * distance between the atoms).
- Mon Nov 23, 2020 12:49 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Radicals and Biradicals in VSEPR Model
- Replies: 4
- Views: 233
Re: Radicals and Biradicals in VSEPR Model
I agree with the previous answer, Dr. Lavelle mentioned in one of his lectures that the unpaired electron in radicals like NO2 is considered a region of electron density.
- Mon Nov 16, 2020 1:14 pm
- Forum: Trends in The Periodic Table
- Topic: Z effective
- Replies: 2
- Views: 351
Re: Z effective
The effective nuclear charge refers to the protons/nucleus of an atom, not the electrons. In terms of periodic trends, the effective nuclear charge increases as you go across a period because the atomic number increases and electrons are being added to the same energy level. It decreases down a grou...
- Mon Nov 16, 2020 1:05 pm
- Forum: Lewis Structures
- Topic: Identifying lewis acids and bases
- Replies: 5
- Views: 569
Re: Identifying lewis acids and bases
Cations, molecules with electron deficient central atoms (like BF3), and molecules with polar double bonds (like CO2) tend to be lewis acids since they are more likely to accept an electron pair. Anions and molecules with lone pairs (like H2O) tend to be lewis bases since they have electrons to dona...
- Mon Nov 16, 2020 1:01 pm
- Forum: Dipole Moments
- Topic: Dipole moment vs dipole bond
- Replies: 5
- Views: 478
Re: Dipole moment vs dipole bond
A dipole moment is a partial positive charge and partial negative charge within a molecule, though the molecule is as a whole electrically neutral. For example, the hydrogens in H2O have a partial positive charge and the oxygen has a partial negative charge due to the electronegativity difference be...
- Mon Nov 16, 2020 12:53 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: Polarizability
- Replies: 3
- Views: 200
Re: Polarizability
To add on, in terms of periodic trends polarizability tends to increase as you go down a group because the atomic radius and the number of electrons increase.
- Mon Nov 16, 2020 12:47 pm
- Forum: Polarisability of Anions, The Polarizing Power of Cations
- Topic: Periodic Table Trends
- Replies: 4
- Views: 406
Re: Periodic Table Trends
For anions, polarizability increases as you go down a group since the atomic radius and number of electrons increases and the effective nuclear charge decreases. In general, the larger the radius and the more electrons an atom has, the more polarizable. For polarizing power, the smaller the atomic r...
- Mon Nov 09, 2020 1:27 pm
- Forum: Bond Lengths & Energies
- Topic: London (dispersion) force
- Replies: 3
- Views: 141
Re: London (dispersion) force
London dispersion forces are induced dipole-induced-dipole interactions. Basically, when non-polar molecules collide their electron densities are shifted, forming a temporary delta negative and delta positive side. This induces the neighboring molecule to form a temporary dipole as well and produces...
- Mon Nov 09, 2020 1:11 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: Lecture 17 Question (IMF)
- Replies: 3
- Views: 126
Re: Lecture 17 Question (IMF)
I believe Professor Lavelle mentioned it's the energy per mole of the given interaction. For example, if there was 1 mole of Na+ and Cl- interactions, the amount of energy released due to the ion-ion interactions would be 250 kJ.
- Mon Nov 09, 2020 1:07 pm
- Forum: Ionic & Covalent Bonds
- Topic: Temporary vs Permanent Dipole Moments
- Replies: 2
- Views: 666
Re: Temporary vs Permanent Dipole Moments
An example of a molecule with a permanent dipole is H2O; the difference in electronegativity between the O and Hs causes the electrons to be pulled towards O, creating a permanent delta negative and delta positive side. Temporary dipoles occur when molecules that are otherwise non-polar, like N2, co...
- Mon Nov 09, 2020 1:01 pm
- Forum: Polarisability of Anions, The Polarizing Power of Cations
- Topic: Can an Anion be Polarizing
- Replies: 4
- Views: 158
Re: Can an Anion be Polarizing
I think the electrons on the anion are referred to as polarizable and the cation as polarizing and not the other way around because the protons in the nucleus of the cation don't "move" due to the attractive force they experience from the electrons of the anion. It is the electrons that ar...
- Mon Nov 09, 2020 12:56 pm
- Forum: Bond Lengths & Energies
- Topic: Negative energies? [ENDORSED]
- Replies: 7
- Views: 751
Re: Negative energies? [ENDORSED]
In terms of thermodynamics, if you think about the molecule/compound as a system, anything that increases the energy of the system, for example putting in energy to break bonds, makes delta E positive. When energy is released, delta E is negative. The intermolecular/interionic interactions have nega...
- Mon Nov 02, 2020 4:06 pm
- Forum: Resonance Structures
- Topic: Delocalization of Electrons
- Replies: 2
- Views: 112
Re: Delocalization of Electrons
For non-resonance structures, electrons are localized.
- Mon Nov 02, 2020 4:04 pm
- Forum: Lewis Structures
- Topic: Bent or Angular?
- Replies: 18
- Views: 1173
Re: Bent or Angular?
I believe angular is 2 atoms bonded to the central atom with 1 lone pair, and bent is 2 atoms bonded to the central atom with 2 lone pairs.
- Mon Nov 02, 2020 3:42 pm
- Forum: General Science Questions
- Topic: Finals
- Replies: 39
- Views: 2451
Re: Finals
Will the final also be multiple choice?
- Mon Nov 02, 2020 3:41 pm
- Forum: Resonance Structures
- Topic: Energy and Stability in Delocalization
- Replies: 3
- Views: 130
Re: Energy and Stability in Delocalization
Here is the textbook's explanation for why it increases stability (it's in Focus 2B): "As well as delocalizing electrons over the atoms, resonance also lowers the energy below that of any single contributing structure and helps to stabilize the molecule. This lowering of energy occurs for quant...
- Mon Nov 02, 2020 3:25 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Electron Shells
- Replies: 7
- Views: 300
Re: Electron Shells
The angular momentum quantum number l, which tells us about the subshells in each shell, is determined by the principle quantum number (n=3 in this case). For n=3, l can be 0...n-1 which is 0, 1, and 2, corresponding to s, p, and d.
- Mon Nov 02, 2020 2:50 pm
- Forum: Resonance Structures
- Topic: Delocalization of Electron
- Replies: 2
- Views: 138
Re: Delocalization of Electron
Delocalized electrons are electrons that do not "belong" to a particular atom or are not associated with a specific bond in the molecule. Here is the textbook's explanation for why it increases stability (it's in Focus 2B): "As well as delocalizing electrons over the atoms, resonance ...
- Mon Oct 26, 2020 12:42 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Subshell Definition
- Replies: 9
- Views: 475
Re: Subshell Definition
Within a particular energy level (n), all electrons with the same angular momentum quantum number (l) are in the same sub-shell, and all electrons with the same n, l, and ml (magnetic quantum number) are in the same orbital.
Hope this helps!
Hope this helps!
- Mon Oct 26, 2020 12:16 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Radial vs Angular Nodes
- Replies: 2
- Views: 133
Radial vs Angular Nodes
What is the difference between radial and angular nodes, and how many do each of the orbitals (s, p, d, f) have?
- Mon Oct 26, 2020 12:11 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Determining Spin in orbitals [ENDORSED]
- Replies: 5
- Views: 275
Re: Determining Spin in orbitals [ENDORSED]
He drew 3 up-spin electrons first because according to Hund's Rule, electrons occupy empty orbitals in the same sub-shell before pairing up. As for why the up-spin electrons are drawn first, I think it just has to do with convention.
- Mon Oct 26, 2020 12:04 pm
- Forum: Photoelectric Effect
- Topic: Photoelectric Effect [ENDORSED]
- Replies: 4
- Views: 281
Re: Photoelectric Effect [ENDORSED]
If you think about EM radiation as a wave of oscillating electric and magnetic fields that are perpendicular to each other, the frequency is related to how the electric field changes, or oscillates, with time. The greater the frequency, the faster the field changes/oscillates. The smaller the freque...
- Mon Oct 26, 2020 11:57 am
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Orbital vs. Subshell
- Replies: 13
- Views: 856
Re: Orbital vs. Subshell
Within a particular energy level (n), all electrons with the same angular momentum quantum number (l) are in the same sub-shell, and all electrons with the same n, l, and ml (magnetic quantum number) are in the same orbital. Here's an explanation with a helpful graphic: https://chemistry.stackexchan...
- Mon Oct 19, 2020 2:26 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Multiple choice test?
- Replies: 7
- Views: 387
Re: Multiple choice test?
That's what I heard too, some of the TAs said it was all multiple choice.
- Mon Oct 19, 2020 2:23 pm
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: Textbook Problem 1B27
- Replies: 6
- Views: 312
Re: Textbook Problem 1B27
Delta v should be 10 m/s. I believe this is an error in the book's solution. Here's a full list of errors in the solution manual:
https://lavelle.chem.ucla.edu/wp-conten ... rs_7Ed.pdf
https://lavelle.chem.ucla.edu/wp-conten ... rs_7Ed.pdf
- Mon Oct 19, 2020 2:03 pm
- Forum: Properties of Light
- Topic: Properties of Light
- Replies: 5
- Views: 89
Re: Properties of Light
As the previous answer stated, the equation is E = hv. The photoelectric effect demonstrated that light exhibits properties of particles and also demonstrated the relationship between energy and frequency of photons.
- Mon Oct 19, 2020 1:18 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Question about Midterms
- Replies: 9
- Views: 281
Re: Question about Midterms
^^ Thanks!
- Mon Oct 19, 2020 1:16 pm
- Forum: Photoelectric Effect
- Topic: Circular Standing Wave model
- Replies: 2
- Views: 114
Re: Circular Standing Wave model
The circular standing wave model is just a math model that was developed to reconcile electrons having wave-like properties and having quantized energy states. In this model, each stable circular standing wave (with whole number wavelengths) around the nucleus represents an energy level (n=1, 2, 3.....
- Mon Oct 19, 2020 1:06 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Question about Midterms
- Replies: 9
- Views: 281
Re: Question about Midterms
Does anyone know if we'll also be given the wavelengths corresponding to the different regions of the EM spectrum, or will we need to just know it?
- Mon Oct 12, 2020 5:04 pm
- Forum: Properties of Light
- Topic: video modules
- Replies: 10
- Views: 345
Re: video modules
They're not mandatory but they are helpful, and the videos are pretty short so it won't take too much time to check them out!
- Mon Oct 12, 2020 4:02 pm
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: Identifying n1 and n2
- Replies: 4
- Views: 1093
Identifying n1 and n2
How do you identify which energy level is n1 and which is n2 for frequency = R(1/(n1)^2 - 1/(n2)^2)? Is n1 always the initial energy level and n2 always the final energy level?