Search found 115 matches
- Wed Mar 10, 2021 10:09 am
- Forum: General Rate Laws
- Topic: Rate determining step
- Replies: 38
- Views: 1590
Re: Rate determining step
The slow step is the rate-determining step since the rate cannot go faster than the slowest rate, and as a result, the reaction depends on this step.
- Wed Mar 10, 2021 10:08 am
- Forum: *Enzyme Kinetics
- Topic: catalyst
- Replies: 23
- Views: 2735
Re: catalyst
Enzymes are a kind of catalyst that lower the activation energy for a reaction, which lowers their energy barrier, allowing for the reaction rate to increase.
- Wed Mar 10, 2021 10:05 am
- Forum: First Order Reactions
- Topic: Graphing
- Replies: 20
- Views: 1004
Re: Graphing
As others have said, I don't think we would be tested on how to graph but we may be tested on how to interpret the graphs. Also, even if the graphs won't necessarily show up on the test, I would still spend some time trying to understand them since it'll help you understand how it all conceptually w...
- Wed Mar 10, 2021 10:02 am
- Forum: Zero Order Reactions
- Topic: Overall reaction order
- Replies: 22
- Views: 1159
Re: Overall reaction order
As others have said, it is possible if all the individual reactants are zero-order as well. However, I haven't seen any problems like that in the textbook or Sapling, so I assume it is rare and doesn't really occur. I would assume that the rate of the reaction would be based on the rate constant only.
- Wed Mar 10, 2021 9:59 am
- Forum: General Rate Laws
- Topic: Sapling #13 confusion
- Replies: 4
- Views: 276
Re: Sapling #13 confusion
Intermediates are not included in rate laws since they are products of one reaction which immediately become reactants in the next reaction.
- Wed Mar 10, 2021 9:56 am
- Forum: General Rate Laws
- Topic: Final Exam
- Replies: 19
- Views: 819
Re: Final Exam
Yes, it will be cumulative and will include everything from Week 1 to Week 10.
- Sat Mar 06, 2021 12:15 am
- Forum: Balancing Redox Reactions
- Topic: How to Determine if a Reaction is in Basic or Acidic Solution?
- Replies: 53
- Views: 3273
Re: How to Determine if a Reaction is in Basic or Acidic Solution?
Yes, the problem should specify since there's no way for us to know otherwise.
- Sat Mar 06, 2021 12:14 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Adding Pt(s)
- Replies: 12
- Views: 714
Re: Adding Pt(s)
As others have said, you use Pt(s) when there is no solid metal conductor. You only need to add it to the side that does not have a solid metal conductor (you may not need it for both sides).
- Sat Mar 06, 2021 12:11 am
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: 6L.1
- Replies: 4
- Views: 339
Re: 6L.1
Yes, n is the moles of electrons transferred. After you balance the half-reactions, you should be able to see how many electrons were transferred (which is your value for n).
- Sat Mar 06, 2021 12:09 am
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Textbook Question 6M. 13 Part c
- Replies: 4
- Views: 267
Re: Textbook Question 6M. 13 Part c
Yeah, I was having some trouble with that question as well, but once I read it, I realized that we just have to use the equation that is given (and therefore, since it is not spontaneous, the cathode & anode you end up with make sense).
- Sat Mar 06, 2021 12:06 am
- Forum: Balancing Redox Reactions
- Topic: states of matter
- Replies: 58
- Views: 2499
Re: states of matter
Yeah, for certain problems on Sapling, they required states of matter. In general, for Sapling, I would include all aspects unless it specifically says you don't have to.
- Fri Feb 26, 2021 10:46 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Labeling/Drawing Cell Diagrams
- Replies: 4
- Views: 293
Re: Labeling/Drawing Cell Diagrams
I think that the questions on the exam would be framed in a way in which we would have to be able to gather information from drawing out a cell diagram (similar to 14A where we didn't have questions about what the correct Lewis structure was but for many problems, we had to draw out the Lewis struct...
- Fri Feb 26, 2021 10:43 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Gibbs Free Energy Equation and n
- Replies: 13
- Views: 618
Re: Gibbs Free Energy Equation and n
Yes, it is the moles of electrons being transferred after balancing the redox reaction.
- Fri Feb 26, 2021 10:42 pm
- Forum: Balancing Redox Reactions
- Topic: Oxidizing Vs Reducing agent
- Replies: 39
- Views: 2113
Re: Oxidizing Vs Reducing agent
An oxidizing agent is being reduced (it gains electrons and oxidizes another substance) while a reducing agent is being oxidized (since it loses electrons and reduces another substance).
- Fri Feb 26, 2021 10:39 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Thermodynamics delta G
- Replies: 13
- Views: 939
Re: Thermodynamics delta G
Gibbs free energy determines whether or not a reaction is spontaneous (or thermodynamically favorable) in a given direction. A reaction with a negative gibbs free energy is said to be spontaneous while a reaction with a positive gibbs free energy is non-spontaneous.
- Wed Feb 24, 2021 4:45 pm
- Forum: Balancing Redox Reactions
- Topic: Sapling Glitch?
- Replies: 8
- Views: 491
Re: Sapling Glitch?
I had a problem with sapling earlier in the quarter where it wouldn't let me edit or delete anything. I just emailed Dr. Lavelle and he contacted Sapling and it was fixed the next day so I could redo the problem and get full points for it.
- Thu Feb 18, 2021 11:42 pm
- Forum: Van't Hoff Equation
- Topic: Textbook 5G.21
- Replies: 3
- Views: 370
Re: Textbook 5G.21
You would first have to calculate delta Gr, using the delta Gf values found in the appendix. Then, you would plug that into the equation delta Gr = -RTlnK. Remember, in order to find K, you would have to do e^-(Gr/RT).
- Thu Feb 18, 2021 11:38 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: qrev
- Replies: 27
- Views: 1667
Re: qrev
qrev refers to the amount of heat transferred in a reversible reaction.
- Thu Feb 18, 2021 11:35 pm
- Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
- Topic: Comparing Molar Entropies of Different Compounds
- Replies: 9
- Views: 1956
Re: Comparing Molar Entropies of Different Compounds
Yes, so a larger molecule (heavier molecule) has higher entropy since the energy levels are closer together, meaning they are more accessible. Complex molecules also have higher entropy (as seen through W since they would be able to occupy more orientations/positions). Ranking from highest entropy t...
- Thu Feb 18, 2021 11:29 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Textbook 4D.7
- Replies: 4
- Views: 312
Re: Textbook 4D.7
I was having the same issue with that question, but I think that the temperature, pressure, volume, etc will be made more clear on the exam (or it will just say standard conditions).
- Thu Feb 18, 2021 11:28 pm
- Forum: Calculating Work of Expansion
- Topic: work of expansion and constant pressure
- Replies: 3
- Views: 189
Re: work of expansion and constant pressure
If the reaction is irreversible, then yes that is the correct equation. If it is not (it's an isothermal reversible expansion), use w=-nRTln(V2/V1). However, based on textbook problems, I think it will be pretty clear whether or not it's irreversible or reversible.
- Sat Feb 13, 2021 9:15 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Temperature and Volume
- Replies: 10
- Views: 555
Re: Temperature and Volume
An increase in volume increases entropy since the molecules are able to occupy more states. An increase in temperature will also increase entropy since the movement of particles increases, which increases disorder.
- Sat Feb 13, 2021 9:11 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Bozemann's constant
- Replies: 4
- Views: 234
Re: Bozemann's constant
I don't think there's a difference. I tried to search online to see if there was a difference, but it seems like k and Kb are used interchangeably, but feel free to correct me if I'm wrong.
- Sat Feb 13, 2021 9:08 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Units
- Replies: 20
- Views: 763
Re: Units
Yes, as others have said, I think both kJ and J are fine, but just make sure when you're doing the problem, it's all in kJ or J.
- Fri Feb 12, 2021 11:07 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Work Equation for Ideal Gas
- Replies: 5
- Views: 284
Re: Work Equation for Ideal Gas
I would be familiar with those equations even if they aren't provided on the equation sheet since there are a couple of textbook problems that require you to use them (and some of the exam questions come from the textbook problems).
- Fri Feb 12, 2021 11:04 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Kelvin conversion
- Replies: 40
- Views: 3413
Re: Kelvin conversion
As others have stated, the conversion for celsius into kelvin is C + 273 = Kelvin.
- Wed Feb 03, 2021 2:17 pm
- 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: Carbon Monoxide Example from Lecture
- Replies: 6
- Views: 319
Re: Carbon Monoxide Example from Lecture
Like the others have said, W takes into account all the different possibilities of orientations that can occur. In the lecture slide, it showed how for one CO molecule there are two possibilities for its positions: C on the left and O on the right or C on the right and O on the left. Then, because w...
- Wed Feb 03, 2021 2:13 pm
- 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: Degeneracy (W)
- Replies: 7
- Views: 279
Re: Degeneracy (W)
I don't think degeneracy has any units because it is just the number of different states that could exist for the particular situation you are presented with.
- Wed Feb 03, 2021 2:11 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Delta S total
- Replies: 6
- Views: 375
Re: Delta S total
The total entropy (S total) is S(system) + S(surroundings)
- Wed Feb 03, 2021 2:09 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: How to know the sign for work
- Replies: 26
- Views: 1040
Re: How to know the sign for work
Like others have said, the difference is in the wording. If work is being done BY the system, then it is negative, but if work is being done ON the system, it is positive.
- Wed Feb 03, 2021 2:02 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Grades for Chemistry Community
- Replies: 21
- Views: 885
Re: Grades for Chemistry Community
Yeah, I have the same issue. Since Week 5 isn't over yet, we only need to have completed 20 posts (5 posts a week for 4 weeks), so it technically should be out of 20 points. Hopefully the grades will be updated at the end of this week to reflect what we actually got out of 25 points.
- Tue Feb 02, 2021 11:16 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: R Constant
- Replies: 91
- Views: 6734
Re: R Constant
You should choose the R value for which the units cancel out so that the only units that remain in the overall equation are the ones for the variable you are trying to solve for. It is definitely helpful to write out all the units and then physically cross them out so that you can clearly see which ...
- Sat Jan 30, 2021 5:12 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Molar and Specific Heat Capacity
- Replies: 6
- Views: 285
Re: Molar and Specific Heat Capacity
Like the others have stated, they are not interchangeable since molar heat capacity is for 1 mole while specific heat capacity is for 1 gram. Depending on whether the substance is given in moles or grams, you would use the appropriate one.
- Sat Jan 30, 2021 5:09 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: change in celsius = change in kelvin
- Replies: 22
- Views: 8002
Re: change in celsius = change in kelvin
The change in Kelvin and Celsius would remain the same because they increase/decrease at the same rate. The only difference is that they have different starting points (Kelvin = Celsius + 273). For example, the change in temperature from 0 celsius to 1 celsius = 1, and in the Kelvin equivalent, 273 ...
- Sat Jan 30, 2021 5:05 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Temperature vs Heat
- Replies: 5
- Views: 263
Re: Temperature vs Heat
Yes, I agree with the others, while temperature and heat are closely related, I think thermodynamics mostly focuses on the transfer of heat (which inevitably would have an effect on the surrounding temperature).
- Fri Jan 29, 2021 12:43 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Topic 4D.23
- Replies: 2
- Views: 203
Re: Topic 4D.23
The equation for forming N2O5 is N2 + (5/2)O2 --> N2O5. You would have to write one more equation for the formation of NO (N2 + O2 --> 2NO). For this problem, all you have to do is essentially reform the three equations so that they add up to the final one. You would want the products & reactant...
- Fri Jan 29, 2021 12:37 pm
- Forum: Phase Changes & Related Calculations
- Topic: Thermo Midterm Topics
- Replies: 2
- Views: 139
Re: Thermo Midterm Topics
Yes, I agree, the best way to prepare would be to make sure you understand how to do all the textbook & sapling problems related to thermochemistry for this midterm.
- Fri Jan 22, 2021 6:59 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: reaction enthalpy of O2
- Replies: 4
- Views: 697
Re: reaction enthalpy of O2
Yes, like the others have said, the standard enthalpy of formation of an element in its most stable form is 0. This means that O2 is the most stable form of oxygen that exists in nature, and thus would have a standard enthalpy of formation equals 0.
- Fri Jan 22, 2021 6:57 pm
- Forum: Phase Changes & Related Calculations
- Topic: Vapor vs gas
- Replies: 121
- Views: 12429
Re: Vapor vs gas
Yes they are the same thing!
- Fri Jan 22, 2021 6:55 pm
- Forum: Phase Changes & Related Calculations
- Topic: H and q
- Replies: 47
- Views: 1768
Re: H and q
q is the measurement for heat (in joules) and H is for enthalpy. While enthalpy is a state property (not dependent on the path taken to obtain that state), heat is not.
- Fri Jan 22, 2021 6:51 pm
- Forum: Phase Changes & Related Calculations
- Topic: Carbon (graphite form)
- Replies: 6
- Views: 308
Re: Carbon (graphite form)
Like the others have said, I would think that all we have to know is that graphite is the most stable form of carbon and the standard enthalpy of formation is 0 kJ/mol (since the standard enthalpy of formation of an element in its most stable form is 0).
- Fri Jan 22, 2021 6:49 pm
- Forum: Phase Changes & Related Calculations
- Topic: Endothermic v. Exothermic
- Replies: 139
- Views: 15112
Re: Endothermic v. Exothermic
Yes, endothermic reactions have a positive delta H since they require energy while exothermic reactions have a negative delta H since they release energy.
- Fri Jan 22, 2021 6:47 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Enthalpy units
- Replies: 7
- Views: 446
Re: Enthalpy units
Yes, the units for ΔHf are kJ/mol while the units for ΔHrxn are just kJ (since it is representing the total of the overall reaction).
- Thu Jan 14, 2021 9:29 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Weel 1/2 Sapling Question #6
- Replies: 3
- Views: 191
Re: Weel 1/2 Sapling Question #6
In order to get the desired equation, 2NH3(g)+3I2(g)↽−−⇀N2(g)+6HI(g), you have to add two of the equations that are given. From the four equations given, we can see that adding the first and third one will get us our desired equation. However, realize that the first equation must be multiplied by 3 ...
- Thu Jan 14, 2021 9:22 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: pKA and pH
- Replies: 8
- Views: 246
Re: pKA and pH
pKa & pKb tells you how strong a particular acid/base is, while pH and pOH simply tell you the concentration of OH- and H3O+. However, both are used to describe acids and bases.
- Thu Jan 14, 2021 9:19 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: pKA, pKB, KA, KB
- Replies: 7
- Views: 387
Re: pKA, pKB, KA, KB
Yes, the stronger the base, the larger the Kb value and lower the pKb value.
- Thu Jan 14, 2021 9:17 pm
- Forum: Ideal Gases
- Topic: Thermodynamics in Equilibirum
- Replies: 6
- Views: 247
Re: Thermodynamics in Equilibirum
I would look at outlines 1 & 2 on his website because those are the ones we've done/are doing so far. The bullet points on the outlines tell you all the material you need to know.
- Wed Jan 13, 2021 12:54 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: q vs k
- Replies: 62
- Views: 2762
Re: q vs k
Q is the reaction quotient (taken at any time during the reaction). If you let the reaction go until it reaches equilibrium, Q should equal K (since K is the equilibrium constant).
- Wed Jan 13, 2021 12:51 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Temperature
- Replies: 45
- Views: 1473
Re: Temperature
Yes, as others stated above, you would need to know whether the reaction is endothermic or exothermic (given by delta h).
- Wed Jan 06, 2021 1:05 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Small and Large K values
- Replies: 3
- Views: 188
Re: Small and Large K values
I think that these values are just chosen as they are both clearly very small or large values, so if the value of K was greater/less than that, it would definitely imply that it sits to the left/right.
- Wed Jan 06, 2021 1:00 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: When K=1
- Replies: 2
- Views: 212
Re: When K=1
I think that that is possible looking at it mathematically (for example if the equation is 2R --> P where [R] = 2 mol/L and [P] = 4 mol/L, then K = 2^2/4 = 1). However, I think it is still rare for this to occur, but feel free to correct me if I'm wrong.
- Wed Jan 06, 2021 12:53 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Quadratic Equations
- Replies: 7
- Views: 369
Re: Quadratic Equations
If you have two positive values, chances are one of them is larger than the initial concentrations. If x is larger than the initial concentration, then the equilibrium concentration value becomes negative, which is impossible.
- Wed Jan 06, 2021 12:50 pm
- Forum: Ideal Gases
- Topic: Units of Temperature
- Replies: 82
- Views: 3951
Re: Units of Temperature
We use Kelvin.
- Wed Jan 06, 2021 12:49 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: change in pressure
- Replies: 8
- Views: 425
Re: change in pressure
There would be no change as the moles on both side are equal (the reaction is not favored to go to any side).
- Tue Dec 15, 2020 5:29 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Chem community points
- Replies: 16
- Views: 835
Re: Chem community points
They will be updating the points in a few days (since we were given an extension).
- Mon Dec 07, 2020 10:16 am
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: coordination compounds
- Replies: 4
- Views: 225
Re: coordination compounds
Yes, as Dr. Lavelle mentioned in the lecture, the most common prefixes are mono-, di-, tri-, tetra-, penta-, hexa-.
- Mon Dec 07, 2020 9:59 am
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: Why is HF not classified as a strong acid?
- Replies: 19
- Views: 1071
Re: Why is HF not classified as a strong acid?
HF is not a strong acid as F is so electronegative, which means that HF does not easily dissociate into H+ and F- easily in water. This is why, as atomic radius increases, the acids become stronger as they are able to dissociate much easier.
- Mon Dec 07, 2020 9:56 am
- Forum: Bronsted Acids & Bases
- Topic: Bronsted Acids and Bronsted Bases
- Replies: 4
- Views: 263
Re: Bronsted Acids and Bronsted Bases
Bronsted Acids are proton donors (donate H+) while Bronsted Bases are proton acceptors (accept H+). Typically, Bronsted Acids have hydrogen (for example: HCl) which dissociates into H+ ions in water to form H3O+.
- Mon Dec 07, 2020 9:53 am
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Sapling Question 9 (Week 10)
- Replies: 5
- Views: 304
Re: Sapling Question 9 (Week 10)
You would first find the pOH = -log[OH-]. Then, using the value for pOH, you can find the pH by doing 14-pOH = pH. Once you've converted all of your values to pH, you can see which is more acidic and which is more basic (acids have pH < 7, bases have pH > 7).
- Mon Dec 07, 2020 9:50 am
- Forum: Amphoteric Compounds
- Topic: Amphoteric Compound Acid/Base Character
- Replies: 4
- Views: 270
Re: Amphoteric Compound Acid/Base Character
I think that an amphoteric compound tends to be a weak acid/base as it can be either acid or base. I would imagine that it would be difficult for a strong acid to behave as a base and vice versa.
- Mon Dec 07, 2020 9:47 am
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: Negative pH of acid
- Replies: 16
- Views: 736
Re: Negative pH of acid
I think that the pH scale goes from 0-14 (as it is found by finding -log[H+]). In order for the pH to be negative, the concentration of H+ would have to be greater than 1M.
- Sun Dec 06, 2020 11:20 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: pH vs pOH
- Replies: 9
- Views: 430
Re: pH vs pOH
Yes, the pOH scale also goes from 1-14, where 7 is neutral. Also, pOH + pH = 14.
- Thu Dec 03, 2020 10:08 pm
- Forum: Properties & Structures of Inorganic & Organic Bases
- Topic: Inorganic and Organic
- Replies: 7
- Views: 795
Re: Inorganic and Organic
Organic compounds (or at least most of them) contain C-H bonds (an example is C6H12O6 which is glucose). Inorganic compounds do not have C-H bonds.
- Thu Dec 03, 2020 10:03 pm
- Forum: Hybridization
- Topic: pcl3
- Replies: 8
- Views: 827
Re: pcl3
There are four regions of electron density (three single bonds and one lone pair). Thus, the hybridized orbital that corresponds to four regions of electron density is sp3 (as there are four orbitals, one for each region of electron density).
- Thu Dec 03, 2020 9:59 pm
- Forum: Naming
- Topic: Sapling 9 #1
- Replies: 7
- Views: 334
Re: Sapling 9 #1
I agree with the answer given above. The Cl2 that is outside of the brackets is not a part of the coordination sphere, so you would write it separately instead of grouping it with the chlorine inside the brackets. Thus, instead of it being trichloro, it would be simply chloro to represent the chlori...
- Thu Dec 03, 2020 9:56 pm
- Forum: Bronsted Acids & Bases
- Topic: Bronsted Acids and Bases
- Replies: 7
- Views: 248
Re: Bronsted Acids and Bases
A Bronsted Acid is a proton donor while a Bronsted Base is a proton acceptor. It is just another way to define/distinguish between acids and bases (another way acids and bases are described is Lewis Acid (electron pair acceptor) and Lewis Base (electron pair donor).
- Thu Dec 03, 2020 9:51 pm
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: pH Chart
- Replies: 16
- Views: 694
Re: pH Chart
I think we would need to memorize it. However, it is pretty simple to remember (<7 is an acid, >7 is a base, 7 is neutral).
- Thu Nov 26, 2020 8:26 pm
- Forum: Hybridization
- Topic: Sp3d or dsp3
- Replies: 22
- Views: 2230
Re: Sp3d or dsp3
It can be written either way, they both work and represent the same thing.
- Thu Nov 26, 2020 8:24 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: Coordination Compounds
- Replies: 5
- Views: 208
Re: Coordination Compounds
Yes, I agree with the other answers given. OH2 and H2O are the same compound, however, it was written as OH2 to show the bonding order.
- Thu Nov 26, 2020 8:21 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR Chart
- Replies: 18
- Views: 1015
Re: VSEPR Chart
Yes, I think that we're expected to have the molecular shapes & bond angles memorized. However, there are many great infographics & charts online that concisely explain everything and I think Dr. Lavelle also does a really good job going in depth in his lectures.
- Thu Nov 26, 2020 8:20 pm
- Forum: Hybridization
- Topic: Lecture 23 Question
- Replies: 2
- Views: 185
Re: Lecture 23 Question
Yes, I think that might have been an error since I also think that ethene has two sp2 hybridization orbitals.
- Thu Nov 26, 2020 8:18 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Lone Pair Volume
- Replies: 4
- Views: 157
Re: Lone Pair Volume
With lone pairs, they are more delocalized than bonding electrons. As a result, lone pairs have greater electron-electron repulsion compared to bonding electrons, so they would want to be farther away.
- Thu Nov 26, 2020 8:16 pm
- Forum: Hybridization
- Topic: Single Bonds and Sigma Bonds
- Replies: 23
- Views: 1195
Re: Single Bonds and Sigma Bonds
Yes, all single bonds are sigma bonds while double bonds have 1 sigma and 1 pi bond and triple bonds have 1 sigma and 2 pi bonds.
- Sun Nov 22, 2020 5:41 pm
- Forum: Hybridization
- Topic: Pi and Sigma Bonds
- Replies: 10
- Views: 449
Re: Pi and Sigma Bonds
Yes, I agree with the others. Sigma and pi bonds occur with all covalent bonds. However, single bonds only have a sigma bond while double & triple bonds have sigma & pi bonds.
- Thu Nov 19, 2020 4:55 pm
- Forum: Dipole Moments
- Topic: Dipole Moments and Electronegativity
- Replies: 2
- Views: 128
Re: Dipole Moments and Electronegativity
Technically electronegativity is quantifiable (each element has a specific electronegativity number) so if those numbers were given to you, you would be able to find the exact difference. However, for now, we just need to know the trend that electronegativity follows and we don't need to do exact ca...
- Thu Nov 19, 2020 4:52 pm
- Forum: Electronegativity
- Topic: Most Electronegative Element
- Replies: 5
- Views: 323
Re: Most Electronegative Element
Helium is a noble gas, so it does not want more electrons as its valence shell is already full. Fluorine, on the other hand, is a halogen, and only needs one more electron to form an octet. Thus, it has the higher electronegativity.
- Thu Nov 19, 2020 4:48 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: London Forces [ENDORSED]
- Replies: 19
- Views: 874
Re: London Forces [ENDORSED]
Yes, LDF are found in all molecules and they are the weakest of all the intermolecular forces.
- Thu Nov 19, 2020 4:46 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Shape Names
- Replies: 50
- Views: 2585
Re: Shape Names
Yes, it is called bent as there are two lone pairs of electrons and two pairs of bonded electrons.
- Thu Nov 19, 2020 4:41 pm
- Forum: Dipole Moments
- Topic: Midterm 2 Results
- Replies: 7
- Views: 446
Re: Midterm 2 Results
I think that we can expect it to take around the same time as last time (I'm guessing we'll get our scores sometime next week, after everyone has taken the midterm this week).
- Sun Nov 15, 2020 6:48 pm
- Forum: Ionic & Covalent Bonds
- Topic: Textbook 2A.23
- Replies: 1
- Views: 83
Re: Textbook 2A.23
So for all of these questions, you would have to use the expected charges. For a, we know that magnesium has a +2 charge in order to be stable and arsenic has a -3 charge to be stable. To form the chemical formula, you would use the charges to decide how many of each ion is needed to make a stable c...
- Thu Nov 12, 2020 12:39 pm
- Forum: Ionic & Covalent Bonds
- Topic: textbook 2C.1
- Replies: 4
- Views: 127
Re: textbook 2C.1
Some species have an odd number of valence electrons, and therefore cannot form a full octet, and may have an unpaired electron (known as a radical). For this problem, I would draw each Lewis structure to see which structures have an unpaired electron.
- Thu Nov 12, 2020 12:32 pm
- Forum: Lewis Structures
- Topic: Radicals
- Replies: 12
- Views: 329
Re: Radicals
Radicals have one unpaired electron (for example, in NO). Radicals form when species have an odd number of valence electrons (for example, N has 5 valence electrons).
- Thu Nov 12, 2020 12:25 pm
- Forum: Lewis Structures
- Topic: Textbook Problem 2B.9
- Replies: 1
- Views: 119
Re: Textbook Problem 2B.9
For this problem, I first determined the number/moles of each atom/molecule. So for example, for part a, which is ammonium chloride, you know that ammonium is NH4 and chloride (chlorine) is just Cl. In order for both of them to be stable, NH4 needs to get rid of one electron and Cl needs to gain an ...
- Thu Nov 12, 2020 12:18 pm
- Forum: Dipole Moments
- Topic: Liquid vs. Solid vs. Gas
- Replies: 5
- Views: 252
Re: Liquid vs. Solid vs. Gas
In the lecture, it was mentioned that high polarizability means higher attractive force. The greater the number of electrons, the more polarizable it is. When there is high polarizability, and therefore more attraction, instead of it being a liquid, it would form a more waxy solid (as seen in the le...
- Wed Nov 11, 2020 6:54 pm
- Forum: Dipole Moments
- Topic: Sapling #17
- Replies: 8
- Views: 4100
Re: Sapling #17
London dispersion forces occur between all molecules and are also known as Van der Waals forces and induced dipole-induced dipole forces in the lecture. In this question, you would look at only nonpolar molecules as they would only exhibit London dispersion forces (others would exhibit London disper...
- Sun Nov 08, 2020 8:16 pm
- Forum: Coordinate Covalent Bonds
- Topic: Just to clear it up
- Replies: 16
- Views: 1048
Re: Just to clear it up
Yes this is true as the Lewis base is the one donating electrons while the Lewis acid gains the electrons.
- Wed Nov 04, 2020 11:05 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Representing Electron Configurations for P-orbitals
- Replies: 6
- Views: 259
Re: Representing Electron Configurations for P-orbitals
Yes, I believe that is correct. You would have one electron in each of the px, py, and pz orbitals to have the lowest energy.
- Wed Nov 04, 2020 2:50 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charge and Stability
- Replies: 7
- Views: 216
Re: Formal Charge and Stability
A stable structure is one that has a formal charge of 0. This is because it would have the lowest energy.
- Tue Nov 03, 2020 1:23 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charge and Lewis Structures
- Replies: 10
- Views: 546
Re: Formal Charge and Lewis Structures
I think that finding the formal charge is a good way to check that your Lewis structure is the most stable. I agree, I think that it is mostly used for structures with resonance as they have multiple Lewis structures for the molecule.
- Tue Nov 03, 2020 12:26 pm
- Forum: Resonance Structures
- Topic: Resonance and double bonds
- Replies: 4
- Views: 102
Re: Resonance and double bonds
This is also a double bond related question. How do we exactly know when there has to be a double bond when creating the Lewis Structure? We know what bonds to use based on the amount of available valence electrons and the octet rule. For example, in NO3-, if you try to use only single bonds, you w...
- Mon Nov 02, 2020 10:56 pm
- Forum: Lewis Structures
- Topic: charge by square bracket
- Replies: 8
- Views: 1729
Re: charge by square bracket
Yes, the charge represents the charge of the polyatomic ion/molecule. NO3 has a -1 charge, hence the -1 sign at the top right. This is because the Lewis structure drawing itself cannot showcase the specific charge of the molecule, so it is shown in this way.
- Mon Nov 02, 2020 10:54 pm
- Forum: Lewis Structures
- Topic: sides
- Replies: 12
- Views: 627
Re: sides
Yes I agree, it can be on any side. What matters is that the number of electrons add up to the available valence electrons and that the appropriate bonds are used (single, double, triple).
- Sun Nov 01, 2020 7:45 pm
- Forum: Ionic & Covalent Bonds
- Topic: Different Bonds
- Replies: 8
- Views: 374
Re: Different Bonds
Ionic bonds form between a metal and a nonmetal atom (an example from the lecture: KCl, potassium chloride). In an ionic bond, the electron transfer results in an an octet of electrons for each atom. The cations lose electrons and the anions gain electrons. In covalent bonds, however, cations cannot...
- Fri Oct 30, 2020 8:59 pm
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: h vs. ħ?
- Replies: 11
- Views: 5575
Re: h vs. ħ?
h-bar is h/2pi. You can use either equation, but personally, I prefer just remembering h and using ∆p ∆x ≥ h/4π.
- Fri Oct 30, 2020 8:56 pm
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: Units for Uncertainty in Position
- Replies: 6
- Views: 236
Re: Units for Uncertainty in Position
The uncertainty in position refers to the position of the electron (which is in meters), so it would also be in meters.
- Thu Oct 29, 2020 4:26 pm
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: En and E
- Replies: 3
- Views: 143
Re: En and E
En refers to the energy at an energy level, n. The E in E=hv refers to the energy of the incoming photon, while Ek in Ek = 1/2 mv^2 refers to the energy of the electron.
- Thu Oct 29, 2020 4:22 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: l=4
- Replies: 13
- Views: 557
Re: l=4
l could be 4, but I think that in this class, we'll only deal with elements up to l=3.
- Thu Oct 29, 2020 4:20 pm
- Forum: DeBroglie Equation
- Topic: p
- Replies: 19
- Views: 898
Re: p
p represents momentum, which can be found by multiplying mass and velocity.
- Wed Oct 21, 2020 9:03 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Problem 1D.13
- Replies: 4
- Views: 126
Re: Problem 1D.13
For this question, l refers to the orbital angular momentum, which is found by finding n-1. However, the l values that are possible are everything from 0 up to n-1. Therefore, when n=7, the possible values can be 0, 1, 2, 3, 4, 5, 6 which are 7 total values.
- Wed Oct 21, 2020 8:58 pm
- Forum: *Shrodinger Equation
- Topic: Schrodinger's Equation
- Replies: 3
- Views: 113
Re: Schrodinger's Equation
We haven't learned how to utilize it mathematically yet, however, conceptually, it essentially describes the concept that an electron (which has wavelike properties and indeterminacy in momentum) can be described by a wave function.