Search found 104 matches
- Wed Mar 11, 2020 3:59 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Change in Ecell
- Replies: 5
- Views: 318
Re: Change in Ecell
Will Ecell increase if the size of the anode metal is increased? Does the metal have anything to do with it? And will Ecell increase if a substance is added to the cathode side? I do not think that changing the size of the anode metal (if you mean the actual electrode) will have an affect on Ecell....
- Wed Mar 11, 2020 3:57 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: finding k
- Replies: 3
- Views: 236
Re: finding k
When looking at multiple mechanisms and asked to find the rate law and k that matches the desired overall reaction, how do you figure out if the rate law of the proposed mechanism is the same as the actual rate law? I think you have to be given the actual rate law, or see which one makes the most s...
- Wed Mar 11, 2020 3:54 pm
- Forum: First Order Reactions
- Topic: 7B. 3)
- Replies: 1
- Views: 171
Re: 7B. 3)
Since you know how much the concentration of B rises, you can figure out that the concentration of A will decrease by this much, 0.034M and make sure to multiply it by 2 (because there is a coefficient of 2 in front of A). From there you subtract that amount from the original concentration of A to f...
- Wed Mar 11, 2020 2:26 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: text problem 4A.5
- Replies: 3
- Views: 290
Re: text problem 4A.5
Since the problem tells you that the system is at constant pressure, you use Pex, which is for an irreversible system.
- Wed Mar 11, 2020 2:24 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: test problem 4A.5 continued
- Replies: 3
- Views: 367
Re: test problem 4A.5 continued
You always use w=Pex x (delta)V for an irreversible expansion because the change in volume is measurable. For a reversible process you use the other equation because the change in volume is infinitestimally small. For the reversible expansion, pressure falls as the volume increases which is reflecte...
- Wed Mar 04, 2020 1:01 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 6M.13
- Replies: 1
- Views: 185
Re: 6M.13
Actually MnO4- is reduced, but it is the oxidizing agent. The reduction reaction serves as the oxidizing agent. In contrast, the Ce3+ to Ce4+ is the oxidation reaction, but Ce3+ is the reducing agent. I hope this helps!
- Wed Mar 04, 2020 12:58 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: When to use Platinum as an electrode
- Replies: 4
- Views: 331
Re: When to use Platinum as an electrode
Usually you use platinum, but graphite or any other non-reactive metal would suffice.
- Wed Mar 04, 2020 11:19 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: 6.65
- Replies: 3
- Views: 334
Re: 6.65
Since you are at equilibrium, you are solving for E knot.
- Wed Mar 04, 2020 11:18 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: 6n.21
- Replies: 1
- Views: 258
Re: 6n.21
I think its just a biological application that we should be aware of, but didn't go over in class. Basically to form rust, iron is oxidized by O2 and H2O.
- Wed Mar 04, 2020 11:17 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Calculating Gibbs Free Energy
- Replies: 6
- Views: 419
Re: Calculating Gibbs Free Energy
deltaG= -nFE: You only take into account the moles of electrons (the stoichiometric coefficient in front of the electron), because the coefficients in front of the compounds do not affect Ecell.
- Sat Feb 29, 2020 7:12 pm
- Forum: General Rate Laws
- Topic: Third Order Reactions
- Replies: 4
- Views: 1011
Re: Third Order Reactions
However, I think you would also say a reaction is third order, if it is first order with respect to one of the products, and second order with respect to another.
- Sat Feb 29, 2020 7:10 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 6L #7c
- Replies: 1
- Views: 163
6L #7c
I am very confused how the book got a cell diagram that contained KOH as the aqueous compound on the anode side instead of just OH-. Also why is there Ni(s) on the cathode side and no OH- present?
- Sat Feb 29, 2020 7:03 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Writing half reactions
- Replies: 1
- Views: 149
Re: Writing half reactions
Usually you are given the reduction half reactions, so you have to reverse the anode in order to get the oxidation half reaction, as you already have the reduction half reaction for the cathode. If you do not know which is the anode and the cathode, then you pick the less positive/more negative reac...
- Sat Feb 29, 2020 7:00 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 6L, #7b
- Replies: 1
- Views: 140
6L, #7b
This question asked you to write out the half reactions and cell diagram for the reaction: H+ + OH- --> H2O. I use the half reactions that involved H+ and H2(g) cancelled out. However the book's work showed a use of OH- and O2(g) canceling out. It would have gotten me back to the correct reaction, b...
- Sat Feb 29, 2020 6:55 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: 6N3
- Replies: 1
- Views: 215
6N3
I am getting a different answer than the solution manual when it asks you to predict the potential of each cell. I am using the E = E*-(0.0592/n x lnQ), but the book uses 0.025693/n. Which constant is correct, because I thought Dr. Lavelle told us the first one in lecture, but all the work in the bo...
- Wed Feb 19, 2020 5:44 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Derivations
- Replies: 5
- Views: 281
Re: Derivations
I think you should be able to understand why the derivations work concept wise, but you probably don't have to memorize them. Most of the equations needed should be given on the equation sheet.
- Wed Feb 19, 2020 5:42 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: 5G 21
- Replies: 1
- Views: 167
5G 21
I am confused on why the components that make up the delta G*r are different for a, b, and c. For a only the product is considered (H2O, g), for b the product (CO2, g) is subtracted from one of the reactants (CO, g), and for part C, the reactant (CaCO3, s) is subtracted from the sum of the products ...
- Wed Feb 19, 2020 5:38 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: 5G 17
- Replies: 1
- Views: 191
5G 17
I am confused on why the answer in the book said that the I was the reactant and the I2 was the product in the graph, when the equation we were given said the reverse. Is this just a typo, or can someone explain why it should be this way?
- Wed Feb 19, 2020 5:36 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Salt Bridge
- Replies: 2
- Views: 177
Re: Salt Bridge
Since the electrons are being taken from the solution with an anode (the oxidation reaction) and being transferred to the solution with a cathode (the reduction reaction), the cathode side is going to be more negatively charged, and the anode side more positively charged. However negatively charge i...
- Wed Feb 19, 2020 5:33 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cell Potentials
- Replies: 2
- Views: 184
Re: Cell Potentials
I think the standard just means that the system is at equilibrium, where as when it is not standard, it is the potential that is required to reduce or oxidize the ions.
- Wed Feb 12, 2020 11:04 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Summary of Units
- Replies: 3
- Views: 202
Re: Summary of Units
My TA said it is better to use kJ for ∆H, and J for the other values. Do you think this is really important, or is it just a preference?
- Wed Feb 12, 2020 1:07 pm
- Forum: Calculating Work of Expansion
- Topic: reversible/irreversible exansions
- Replies: 1
- Views: 141
reversible/irreversible exansions
When you are calculating the work and then applying that to the internal energy equation, is internal energy always equal to 0 for reversible/isothermal expansions, but only sometimes equal to 0 for irreversible reactions? How do you know the delta U for an irreversible reaction?
- Wed Feb 12, 2020 12:51 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Why are exothermic reactions generally spontaneous?
- Replies: 16
- Views: 1150
Re: Why are exothermic reactions generally spontaneous?
Is this related to the relationship between ∆G and the direction of a spontaneous reaction? Does a spontaneous reaction have a -∆G and proceed in the forward direction?
- Wed Feb 12, 2020 12:42 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Constant Pressure and Volume
- Replies: 1
- Views: 80
Constant Pressure and Volume
When you are calculating the change in entropy in response to a change in volume, would you use the nR value for constant pressure denoted by a P (5/2 x R)?
- Wed Feb 12, 2020 12:37 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Analysis of Gibbs Free Energy Equation
- Replies: 4
- Views: 311
Analysis of Gibbs Free Energy Equation
On the outline when it says "explain how how ∆S is related to ∆H for a change at constant temperature and pressure and explain the relationship" I am a little confused. Like I know the general equation to relate the two, but is there a trend that when you increase ∆S, ∆H will either increa...
- Thu Feb 06, 2020 11:58 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Delta H and qp
- Replies: 8
- Views: 168
Re: Delta H and qp
You said you can make assumptions about delta H when pressure is constant, so can you make assumptions about internal energy when volume is constant? If so, what would they be?
- Thu Feb 06, 2020 11:54 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: units
- Replies: 4
- Views: 139
Re: units
When you are calculating the specific heat capacity this will be in grams, but when you are calculating the molar heat capacity this will be in moles. As far as degrees C goes, what every your constant is given in (kelvin or celcius) is what you will have to work with. It does not seem to matter tha...
- Thu Feb 06, 2020 3:59 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: using ratios for R
- Replies: 3
- Views: 80
using ratios for R
I think I understand when to use the ratios for R in terms of when to plug it into my calculations, but what is the point of them and what do they mean?
- Thu Feb 06, 2020 3:57 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: when to use standard enthalpy
- Replies: 1
- Views: 50
when to use standard enthalpy
When do you use standard enthalpy of formation vs just enthalpy? I understand the difference is that standard enthalpy means all products and reactants are in their standard states, but why/when would it be better to use one or the other?
- Thu Feb 06, 2020 3:52 pm
- Forum: Phase Changes & Related Calculations
- Topic: equation
- Replies: 2
- Views: 91
equation
When you are determining the change in enthalpy, I know you have to take into account any phase changes. I know with bond enthalpies you add the delta H of the phase change(s) (to/from gas form) to the delta H of bonds broken to find the delta H of the reaction. But, when you are trying to determine...
- Fri Jan 31, 2020 1:55 am
- Forum: Phase Changes & Related Calculations
- Topic: phase change heat supplied
- Replies: 3
- Views: 135
Re: phase change heat supplied
Don't forget to add the enthalpy of any state changes when you are calculating the enthalpy for a reaction. This phase change from liquid to gas is crucial in determining how much energy will be left or used after the reaction.
- Fri Jan 31, 2020 1:49 am
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Reversible Reactions
- Replies: 5
- Views: 215
Re: Reversible Reactions
Reversible reactions usually take place when weak acids and bases are involved, as opposed to strong acids and bases.
- Fri Jan 31, 2020 1:48 am
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Isolated vs Closed [ENDORSED]
- Replies: 34
- Views: 4166
Re: Isolated vs Closed [ENDORSED]
When something is insulate that means there is not a relationship with the surroundings, and therefore it would be an isolated system. An example of an isolated system is something that occurs in a bomb calorimeter.
- Fri Jan 31, 2020 1:45 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: 4C 3
- Replies: 1
- Views: 128
4C 3
In 4C #3 you are given 765J of energy transferred as heat to 0.820mol Kr(g) at 298K and 1.00atm. When given constant pressure you plug in n((5/2)R)deltaT and constant volume is the same, but the ratio is 3/2. Where do these ratios come from?
- Fri Jan 31, 2020 1:40 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: benzene mean bond
- Replies: 1
- Views: 91
Re: benzene mean bond
I recall that in the book, it said this applied specifically to benzene. However, I think that any example where there is resonance (meaning half the C-C bonds are single and half are double, but in reality they are all a hybrid of single/double bonds) would have that bond enthalpy.
- Mon Jan 20, 2020 4:53 pm
- Forum: Ideal Gases
- Topic: Acid and Bases
- Replies: 16
- Views: 511
Re: Acid and Bases
Yes, you are correct, a pH<7 is acidic, pH=7 is neutral, and pH>7 is basic.
- Mon Jan 20, 2020 4:51 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: 6B 9
- Replies: 1
- Views: 38
6B 9
Was anyone else getting different concentrations of H3O+ for ii when they put it in their calculator? I was getting something to the 1.50 x 10^-15, but that was different than what the book had.
- Mon Jan 20, 2020 4:49 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Sig Figs for pH/pOH
- Replies: 7
- Views: 334
Sig Figs for pH/pOH
Is there a special way to calculate sig figs for pH and pOH? I feel like this might have been mentioned in class, but now I am getting confused if this is for my chem lab instead? Do you determine sig figs based off of the decimal places of the numbers you are given or vice versa?
- Mon Jan 20, 2020 4:47 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Directionality of Acid/Base Equations
- Replies: 4
- Views: 119
Directionality of Acid/Base Equations
How do we know if the acid/base equations are reversible? Are strong acid/base equations never reversible, and weak ones always are?
- Mon Jan 20, 2020 4:46 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: 6D 15
- Replies: 1
- Views: 100
6D 15
Does anyone understand how we determine the Kb for AlCl3 on 6D 15b? I thought you would multiply the Kb of Cl- by 3 and that Al would count as a spectator ion, but the chemical equation was very complicated and confusing. Would this first way be correct, and if not why does it not work?
- Wed Jan 15, 2020 5:53 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: effect on K
- Replies: 3
- Views: 160
Re: effect on K
I think this question is referring to problems like 5H #1. In this example you are given an equilibrium equation, and in one instance the coefficients are halved, in which case you take the square root (or to the 1/2 power) of K. In the other case, the coefficients are multiplied by 2, in which case...
- Wed Jan 15, 2020 5:51 pm
- Forum: Ideal Gases
- Topic: approximate ideal gas law
- Replies: 3
- Views: 147
Re: approximate ideal gas law
I think this is necessary when you are trying to find the equilibrium constant K. For example, if you are trying to solve for Kc and you are given the partial pressure, you can then plug that into PV=nRT to solve for n/V which is the molarity or concentration. Once you have the problem in terms of c...
- Wed Jan 15, 2020 5:48 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 5I.29 Barr units
- Replies: 3
- Views: 130
Re: 5I.29 Barr units
No, when you are given bar as units that means you solve for Kp not Kc. In this case you create your ICE table in terms of partial pressure instead of concentration, so the volume is not part of the equation.
- Wed Jan 15, 2020 4:30 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: volume's effect on K
- Replies: 7
- Views: 196
Re: volume's effect on K
Yes, volume, pressure, and changes in concentration have no effect the value of K, only temperature can change the value of the K constant.
- Wed Jan 15, 2020 4:28 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Conjugate Seesaw and Kw
- Replies: 3
- Views: 114
Re: Conjugate Seesaw and Kw
We relate everything to Kw because it is equal to the concentration of H3O+ times the concentration of OH-. These can then be used to determine the pH and pOH, or the Ka/Kb and pKa/pKa using logarithmic functions. So it is the other side of the equation that makes Kw so useful.
- Wed Jan 08, 2020 12:45 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Composite Equations
- Replies: 3
- Views: 1418
Re: Composite Equations
When I did this problem, I used:
H2 + Cl2 <--> 2HCl
2BrCl <--> Br2 + Cl2
The Cl2's cancel out to get the complete reaction, and both are listed at 300K in the book.
H2 + Cl2 <--> 2HCl
2BrCl <--> Br2 + Cl2
The Cl2's cancel out to get the complete reaction, and both are listed at 300K in the book.
- Wed Jan 08, 2020 12:43 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Reaction Quotient > Equilibrium Constant
- Replies: 4
- Views: 167
Re: Reaction Quotient > Equilibrium Constant
I think it is kind of like thinking of it in terms of the reverse reaction (so in this case the products are acting like reactants). But, I also don't think the limiting reactant concept really applies because you are trying to reach equilibrium (instead of trying to complete a reaction to completio...
- Wed Jan 08, 2020 12:39 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: K vs Kp vs Kc
- Replies: 9
- Views: 326
Re: K vs Kp vs Kc
If the question just asks for K, you can choose between Kc and Kp by looking at other information in the problem. If dealing with aqueous solutions you should probably find Kc, but if dealing with gaseous solutions, it might be better to calculate Kp. This seems to be the general trend, but may not ...
- Wed Jan 08, 2020 12:36 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Chem Equilibrium Part 2 Post-Assessment, #30
- Replies: 1
- Views: 51
Chem Equilibrium Part 2 Post-Assessment, #30
"A mixture of 2.5 moles H2O and 100 g of C are placed in a 50 L container and allowed to come to equilibrium subject to the following reaction: C(s) + H2O (g) ⇌ CO (g) + H2 (g). The equilibrium concentration of hydrogen is found to be [H2] = 0.040 M. Calculate the equilibrium constant Kc of thi...
- Wed Jan 08, 2020 12:33 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Chem Equilibrium Part 2 Post-Assessment, #29
- Replies: 2
- Views: 108
Chem Equilibrium Part 2 Post-Assessment, #29
I am confused how you solve this problem from the post-assessment: "A researcher fills a 1.00 L reaction vessel with 1.84 x 10-4 mol of BrCl gas and heats it to 500 K. At equilibrium, only 18.3 % of the BrCl gas remains. Calculate the equilibrium constant, assuming the following reaction is tak...
- Wed Dec 04, 2019 1:43 pm
- Forum: Acidity & Basicity Constants and The Conjugate Seesaw
- Topic: 6C19 parts a and c
- Replies: 3
- Views: 176
Re: 6C19 parts a and c
Thank you, your explanation was really helpful!
- Wed Dec 04, 2019 9:59 am
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: 6C 21 part b
- Replies: 2
- Views: 98
6C 21 part b
Can someone give an explanation of why formic acid (HCOOH) is a stronger acid than acetic acid (CH3COOH) because the one in the textbook was a little confusing and unclear to me?
- Wed Dec 04, 2019 9:57 am
- Forum: Acidity & Basicity Constants and The Conjugate Seesaw
- Topic: 6C19 parts a and c
- Replies: 3
- Views: 176
Re: 6C19 parts a and c
I had the same questions for parts d and f, and also why do you not consider different amount of H's in part d?
- Wed Dec 04, 2019 9:56 am
- Forum: Acidity & Basicity Constants and The Conjugate Seesaw
- Topic: 6C19 parts a and c
- Replies: 3
- Views: 176
6C19 parts a and c
I am confused when you use which rule to identify which compound is the stronger acid. In lecture we mainly discussed bond length and anion stability, but the textbook solutions only justified their reasoning with bond length to say that HCl was stronger than HF (in part a). I thought you would use ...
- Wed Dec 04, 2019 9:52 am
- Forum: Acidity & Basicity Constants and The Conjugate Seesaw
- Topic: 6C19 parts b and e
- Replies: 1
- Views: 99
6C19 parts b and e
For HClO and HClO2 (part b) and HNO3 and HNO2 (part e) the book claimed that the compound with more O's would be a stronger acid because more O's meant more electronegativity helping to pull e- of H atom out of H-O bond, which I think makes sense, so do you always go with the atom with more O's if t...
- Wed Dec 04, 2019 9:45 am
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: 6B.3 (b)
- Replies: 3
- Views: 277
Re: 6B.3 (b)
For part b, is there a formula that tells us we can plug in the (200 x 0.025)/250 to the -log, or are we just doing the conversion to molarity using M1V1=M2V2 inside the pH=-log[H3O+] formula?
- Wed Dec 04, 2019 9:40 am
- Forum: Bronsted Acids & Bases
- Topic: Bronsted Acids/Bases in Equations
- Replies: 5
- Views: 367
Bronsted Acids/Bases in Equations
When you are supposed to identify the Bronsted acid and Bronsted base in a chemical equation, will they both always be on the left side of the equation (like are they always going to be the reactants)? If not, can you give an example where the Bronsted acid and/or base is on the right side of the eq...
- Tue Nov 26, 2019 9:54 am
- Forum: Hybridization
- Topic: How to write
- Replies: 3
- Views: 126
Re: How to write
If you count the number of valence electrons, you can determine the atoms hybridization. For example if you have a Carbon atom, which has 2 electrons in the 2s and 2 electrons in the 2p orbitals, then these orbitals would combine to form a hybridization of sp3. This means that now the Carbon atom ca...
- Tue Nov 26, 2019 9:50 am
- Forum: Hybridization
- Topic: Focus 2.57
- Replies: 4
- Views: 286
Re: Focus 2.57
I'm confused, is this question asking you to write out the hybridizations for each sigma and pi bond like in 2.47 or is it asking for the hybridizations of the central atoms?
- Tue Nov 26, 2019 9:49 am
- Forum: Hybridization
- Topic: Focus 2.45
- Replies: 3
- Views: 230
Re: Focus 2.45
I have a question on this problem. I understand how to determine hybridization when it is a simple compound such as BF3, but I do not understand how we find the multiple hybrids from a big compound like this. Do the two hybridizations in the parentheses represent the hybridizations of the molecules ...
- Tue Nov 26, 2019 9:45 am
- Forum: Naming
- Topic: Problem #3 part d, from 9C
- Replies: 1
- Views: 144
Problem #3 part d, from 9C
I was confused on the problem where you are supposed to write out the formula of the compound sodium bisoxalato (diaqua) ferrate (III). My formula had the oxolato before the water, but the answer from the solutions said the water should be first (and written as OH2 instead of H2O. How do you know wh...
- Tue Nov 26, 2019 9:38 am
- Forum: Administrative Questions and Class Announcements
- Topic: Final Exam Content
- Replies: 14
- Views: 766
Re: Final Exam Content
I think the final exam is cumulative, so everything we have learned this quarter.
- Thu Nov 21, 2019 3:45 pm
- Forum: Dipole Moments
- Topic: Rod and Spherically Shaped Molecules
- Replies: 3
- Views: 123
Rod and Spherically Shaped Molecules
In instantaneous dipoles, when we learned that two rod-shaped molecules are closer, and thus the intermolecular forces will be stronger, than two spherically-shaped molecules. But is there a way of knowing which shape the molecule is, rod or spherical?
- Thu Nov 21, 2019 3:42 pm
- Forum: Sigma & Pi Bonds
- Topic: Need to Know
- Replies: 3
- Views: 196
Re: Need to Know
I think the main thing you need to know/most of what we learned is that one sigma bond occurs in any type of bond, single, double, or triple. For pi bonds there will be 0 in a single bond, 1 in a double bond, and 2 in a triple bond.
- Thu Nov 21, 2019 3:39 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Test 2
- Replies: 14
- Views: 735
Re: Test 2
I think you are also supposed to know the VSEPR Model, dipole moments and how that is related to polarity, the strength of different intermolecular forces. Anything that is on Homework 3F and 2E may be on the test.
- Thu Nov 21, 2019 3:35 pm
- Forum: Hybridization
- Topic: 2F.1
- Replies: 3
- Views: 169
Re: 2F.1
Yes I think the question is asking for the orientation of the orbitals. It is asking if they oriented towards the corners or opposite of each other.
- Thu Nov 21, 2019 3:31 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Angular vs. Bent
- Replies: 5
- Views: 198
Angular vs. Bent
When we are determining the molecular shape of a compound that has a central atom with two bonded pairs and two lone pairs, is the name of this shape "angular" or "bent"? I think they are the same thing, if they are not what is the difference between the two? If they are the same...
- Thu Nov 14, 2019 9:42 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles Exceptions
- Replies: 6
- Views: 332
Re: Bond Angles Exceptions
Yes, difference in bond angles in a tetrahedral may occur if the atoms surrounding the central atom differ. For example the bigger atom will cause bigger bond angles (than 109.5 degrees) between it and the other atoms (because the electrons will repel each other more) and the other bond angles will ...
- Thu Nov 14, 2019 9:39 am
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: Melting Point 3F.5
- Replies: 2
- Views: 98
Re: Melting Point 3F.5
For part d, there is no opportunity for Hydrogen bonding in C[2]H[4], and Hydrogen bonds are stronger so that is why CH[3]OH would have a higher melting point (hydrogen bonds can occur between the H's and O's). For part b, I am unsure though since there are the same amount of H and O molecules allow...
- Thu Nov 14, 2019 9:34 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Lone Pairs
- Replies: 5
- Views: 308
Re: Lone Pairs
Are the lone pairs always going to cause a bent shape, or will there be times when the lone pairs are opposite of each other?
- Thu Nov 14, 2019 9:32 am
- Forum: Bond Lengths & Energies
- Topic: Strongest Bonds
- Replies: 11
- Views: 884
Strongest Bonds
In our notes it says bonds between two ions have -250kJ of energy and are most favorable. Is the next most favorable type of bond, a Hydrogen bond?
- Thu Nov 14, 2019 9:30 am
- Forum: Dipole Moments
- Topic: Dipole-Dipole vs. Dipole-Induced Dipole
- Replies: 1
- Views: 146
Dipole-Dipole vs. Dipole-Induced Dipole
What is the difference in characteristics of molecules with dipole-dipole bonds vs. molecules with dipole-induced dipole bonds? I know that virtually all molecules have London dispersion forces and that polar molecules will have dipole-dipole forces, but is it possible for a molecule to have both di...
- Wed Nov 06, 2019 3:03 pm
- Forum: Electronegativity
- Topic: Determining Electronegativity
- Replies: 4
- Views: 197
Re: Determining Electronegativity
Since SiCl has a greater difference in electronegativity than SiBr (increases going to the right, but then decreases to go down the group to get to Br), SiCl will be more electronegative than SiBr.
- Wed Nov 06, 2019 2:58 pm
- Forum: Lewis Structures
- Topic: Expanded Octets
- Replies: 6
- Views: 470
Re: Expanded Octets
Overall, if an expanded octet can be formed (is past 2p orbitals) to yield lower formal charges on the central atom, will this always be a more stable structure?
- Wed Nov 06, 2019 2:56 pm
- Forum: Lewis Structures
- Topic: Lewis acids vs Lewis bases
- Replies: 3
- Views: 230
Re: Lewis acids vs Lewis bases
I understand that Lewis acids and bases form a coordinate covalent bond, but is there a difference between the characteristics of a coordinate covalent bond and an ordinary covalent bond?
- Wed Nov 06, 2019 2:53 pm
- Forum: Bond Lengths & Energies
- Topic: Bond strengths
- Replies: 9
- Views: 511
Re: Bond strengths
Bond length and bond strength have an inverse relationship. A longer bond such as a single bond is weaker, while a shorter bond such as a triple bond will be stronger.
- Wed Nov 06, 2019 2:52 pm
- Forum: Lewis Structures
- Topic: Lewis structure for Nitrate
- Replies: 4
- Views: 200
Re: Lewis structure for Nitrate
I don't think we need to focus on electron affinity when determining which atom to put a negative formal charge on. The main thing is if you have to choose between two, give the atom with the lower electronegativity a negative charge.
- Wed Nov 06, 2019 2:48 pm
- Forum: Lewis Structures
- Topic: 2C5 a)
- Replies: 2
- Views: 134
Re: 2C5 a)
Is there a way to determine which atom the unpaired electron will go on when doing problems involving radicals?
- Sun Nov 03, 2019 8:56 am
- Forum: Octet Exceptions
- Topic: Tungsten Electronic Configuration [ENDORSED]
- Replies: 2
- Views: 83
Re: Tungsten Electronic Configuration [ENDORSED]
I asked Professor Lavelle about this question during office hours and he said he did not realize that this was included on the homework, and that he is taking it off for next year because it is more complicated than we need to know. I think he also did an explanation somewhere on Chemistry Community...
- Sun Nov 03, 2019 8:53 am
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: s and d orbital
- Replies: 1
- Views: 60
Re: s and d orbital
It is lower energy to add electrons to the s orbital than to the d orbitals (for example you add 4s before 3d). However, when you are removing electrons from subshells, you will remove from the s subshell before d. The exceptions comes to play when you have placed two electrons in the 4s subshell an...
- Sun Nov 03, 2019 8:46 am
- Forum: Lewis Structures
- Topic: Lewis Structures for ionic compounds
- Replies: 2
- Views: 67
Re: Lewis Structures for ionic compounds
If most bonds exhibit both ionic and covalent properties to varying degrees, do we ever draw ionic compounds as Lewis Structures instead of two ions next to each other? Is there an example of this? I can't think of anytime when this would be the case. If you have an ionic compound then you are going...
- Sun Nov 03, 2019 8:39 am
- Forum: Resonance Structures
- Topic: "Equivalent" resonance structures
- Replies: 2
- Views: 148
Re: "Equivalent" resonance structures
I think the answer to your second question would be yes, structures that have resonance with one another should have the same numbers of single/double/triple bonds. These bonds would be moved around however, causing the formal charges for the individual elements in the diagram to change. These are n...
- Sun Nov 03, 2019 8:34 am
- Forum: Electronegativity
- Topic: Electronegativity
- Replies: 9
- Views: 376
Re: Electronegativity
I doubt that we will be given the electronegativity table, I think we will just have to base it off of our knowledge of the general trend. Also, the electronegativity rule is not true 100% of the time, especially when the values are very close. We did an example in my discussion class and when we tr...
- Fri Oct 25, 2019 6:28 pm
- Forum: Resonance Structures
- Topic: Delocalized
- Replies: 4
- Views: 130
Re: Delocalized
When there are delocalized electrons you get a resonant structure, meaning there is an average Lewis structure that best represents the actual formation of electrons in a compound.
- Fri Oct 25, 2019 6:26 pm
- Forum: Octet Exceptions
- Topic: Formal Charge
- Replies: 2
- Views: 141
Re: Formal Charge
If a triple bond yields a formal charge closer to 0 than one or multiple double bonds, then yes triple bonds would be more stable than double bonds (so long as the octet rule is satisfied).
- Fri Oct 25, 2019 6:23 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charge
- Replies: 5
- Views: 169
Re: Formal Charge
In response to the question about knowing what the formal charge should add up to, a compound should have a formal charge of 0, if it does not have a positive or negative charge. However if it is an ionic compound with a charge, then it should not add up to 0. When there are multiple possible struct...
- Fri Oct 25, 2019 6:20 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charge
- Replies: 5
- Views: 169
Re: Formal Charge
Sometimes there will not be other possible ways to draw a structure for example, if the central atom is bonded to 4 elements and cannot form an expanded octet, then no double bonds will occur. However if there are other possibilities, such that the central atom is not bonded to the maximum amount of...
- Fri Oct 25, 2019 6:17 pm
- Forum: Lewis Structures
- Topic: Resonance or Lone pair?
- Replies: 2
- Views: 113
Re: Resonance or Lone pair?
Also if you are unsure if there should be a lone pair or a double bond, which would cause resonance in the Lewis structure, you should calculate the formal charges of each and which ever one is lower will be the better/more accurate structure.
- Fri Oct 25, 2019 6:13 pm
- Forum: Octet Exceptions
- Topic: Resonance structures
- Replies: 5
- Views: 251
Re: Resonance structures
I think any of the possible Lewis dot structures are acceptable. If you note that there is resonance, and maybe explain why, then it should be okay to only include one of the possible structures.
- Thu Oct 17, 2019 11:35 pm
- Forum: Einstein Equation
- Topic: kJ/mol
- Replies: 4
- Views: 276
Re: kJ/mol
To the person who asked if you should always convert kJ to J, when you are using other values with units that involve J, yes you should 100% convert kJ to J. However, if it is your final answer, you would probably be fine leaving it either way.
- Thu Oct 17, 2019 11:27 pm
- Forum: Properties of Light
- Topic: 1A.5
- Replies: 6
- Views: 179
Re: 1A.5
Yes, it will probably be important to know (on exams) the different types of wavelengths both in terms of the order from long to short wavelengths and from low to high energy.
- Thu Oct 17, 2019 11:25 pm
- Forum: Properties of Light
- Topic: What are the units of hertz
- Replies: 41
- Views: 1998
Re: What are the units of hertz
As mentioned above Hz is equivalent to s^-1, which is why you can often cancel out Hz when you have m/s in your calculations.
- Thu Oct 17, 2019 11:20 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: 1D 13 Part A
- Replies: 2
- Views: 112
1D 13 Part A
I was wondering how you are supposed to solve part a of number 13, because I thought the question was just asking for how many possible values of l there could be with a principle quantum number of n=4. However, the answer says there are 7 possible values not 4, how do you arrive at this answer?
- Thu Oct 17, 2019 11:17 pm
- Forum: DeBroglie Equation
- Topic: 1B.15a
- Replies: 2
- Views: 188
Re: 1B.15a
I was wondering the same thing because I tried to use those equations, but I did not get the correct answer. The worked out solution manual used the equation wavelength=h(mv)^-1, and I don't remember learning this equation in lecture, so how are we supposed to solve this problem?
- Thu Oct 10, 2019 3:58 pm
- Forum: Limiting Reactant Calculations
- Topic: general questions
- Replies: 11
- Views: 978
Re: general questions
Finding a limiting reactant allows you to calculate the amount of product that is going to be produced. Thus the next step in a limiting reactant problem is often to find the amount of a certain product produced, but it may also be to find the amount of excess reactant that is left over after the re...
- Thu Oct 10, 2019 3:53 pm
- Forum: Accuracy, Precision, Mole, Other Definitions
- Topic: # of molecules and formula units?
- Replies: 5
- Views: 344
Re: # of molecules and formula units?
Yes, you use Avogadro's constant to find both, but the units may be different. Obviously molecules are the units when calculating the number of molecules, but when calculating formula units, your answer can be in terms of molecules or formula units. At least that is how the answers were to the homew...
- Wed Oct 09, 2019 4:38 pm
- Forum: Properties of Light
- Topic: Speed of Light
- Replies: 4
- Views: 226
Re: Speed of Light
Yes the constant is the speed of light in a vacuum, but I believe you can still use it even if the problem does not specify that it takes place inside a vacuum.
- Wed Oct 09, 2019 4:35 pm
- Forum: Empirical & Molecular Formulas
- Topic: Naming Random Comounds
- Replies: 3
- Views: 173
Naming Random Comounds
I have a question regarding when we are solving for an empirical or molecular formula: some of the problems, then have you name the compound. For example in L39, the formula ends up being SnO2, and its name is tin (IV) oxide. But how are we supposed to know that it is tin (IV)? Do we need to know co...
- Wed Oct 09, 2019 4:30 pm
- Forum: Limiting Reactant Calculations
- Topic: Need help on question M.9 for chem 14a
- Replies: 6
- Views: 5220
Re: Need help on question M.9 for chem 14a
In general, when you are writing a net ionic equation (like in this problem), how do you know which ions are spectator ions? Since some of the ions are going to be spectator ions, do those ions still need to be balanced on both sides of the equation?
- Tue Oct 01, 2019 11:12 pm
- Forum: Significant Figures
- Topic: E1 Sig Figs
- Replies: 4
- Views: 234
Re: E1 Sig Figs
When there are 0's without a decimal point, such as the number 200, they do not count toward the sig figs- this number has 1 sig fig. But if the 0's are after the decimal point, such as the number 2.00, they do count toward the sig figs- this number has 3 sig figs. Finally if there are 0's before a ...