Search found 107 matches
- Sun Mar 13, 2022 12:56 pm
- Forum: Environment, Ozone, CFCs
- Topic: Uncatalyzed vs catalyzed
- Replies: 9
- Views: 4652
Re: Uncatalyzed vs catalyzed
Catalyzed reaction makes use of another compound (that is not present in the overall equation) to help reduce the activation energy and speed up the rate of reaction. An example of this could be how ATP Synthase speeds up the conversion of ADP into ATP by helping increase the likelihood of favorable...
- Sun Mar 13, 2022 12:50 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Temperature Impact
- Replies: 6
- Views: 298
Re: Temperature Impact
Increasing temperature doesn't change the amount of gases in the mixture. While increasing temperature increases the total overall pressure in a mixture if volume remains constant, it does not change partial pressure like compressing the mixture would. Thus, it is only the equilibrium constant that ...
- Sun Mar 13, 2022 12:47 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: Determination of microstate
- Replies: 3
- Views: 294
Re: Determination of microstate
Drawing a lewis structure can help. A molecule that lies in 1 plane (such as a benzene derivative) then can be rotated in different positions to find the possible number of microstates. Then, raise the number of microstates to the power of the number of particles to find W
- Sun Mar 13, 2022 12:45 pm
- Forum: First Order Reactions
- Topic: rate constant
- Replies: 10
- Views: 428
Re: rate constant
depending on the units of the y-axis, the slope can be used to find the rate constant.
For 0 and 1st order, k = -slope
For 2nd order, k = slope
For 0 and 1st order, k = -slope
For 2nd order, k = slope
- Sun Mar 13, 2022 12:41 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: clarification on k
- Replies: 25
- Views: 920
Re: clarification on k
The value of the rate constants depend on the arrhenius equation. However, making changes such as adding a catalyst can increase both the reverse and forward rate by decreasing the energy of the activated complex
- Sun Mar 13, 2022 12:39 pm
- Forum: Ideal Gases
- Topic: ideal gas
- Replies: 10
- Views: 531
Re: ideal gas
A gas that has no interaction with other molecules and that move randomly. We also assume they take up no volume. In reality, they do not exist since everything takes up space and will interact with other particles at least a little bit, but it can be used to approximate
- Fri Mar 11, 2022 12:06 am
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: A
- Replies: 13
- Views: 575
Re: A
How come on Achieve #15, the A value is much larger than 1?
- Sun Mar 06, 2022 11:45 pm
- Forum: Zero Order Reactions
- Topic: Wednesday Lecture Week #9 More Questions
- Replies: 4
- Views: 221
Re: Wednesday Lecture Week #9 More Questions
It isn't that k is negative, but rather the slope in the graphs where the plot would be linear shows a negative slope.
This is observed in the 0th and 1st order reactions and it is due to the nature of the integration that does not remove the negative sign from the initial -d[A]/dt.
This is observed in the 0th and 1st order reactions and it is due to the nature of the integration that does not remove the negative sign from the initial -d[A]/dt.
- Sun Mar 06, 2022 11:31 pm
- Forum: Second Order Reactions
- Topic: Determining reaction order
- Replies: 5
- Views: 204
Re: Determining reaction order
If the graphs are scaled properly with [A], ln[A], and 1/[A] vs time, then the graphs can be useful.
Positive linearity in the 1/[A] vs time graph indicates 2nd order
Negative linearity in the ln[A] vs time graph indicates 1st order
Negative linearity in the [A] vs time graph indicates 0th order
Positive linearity in the 1/[A] vs time graph indicates 2nd order
Negative linearity in the ln[A] vs time graph indicates 1st order
Negative linearity in the [A] vs time graph indicates 0th order
- Sun Mar 06, 2022 11:26 pm
- Forum: General Rate Laws
- Topic: Rates of reactions
- Replies: 7
- Views: 276
Re: Rates of reactions
The reaction rate may be given to use, or we may have to calculate it. Recall the first equation Dr. Lavelle showed us about reaction rate. The rate of formation/removal of a substance can be interchanged with the unique reaction rate: For the reaction: aA → bB + cC Unique rate = -1/a ( d[A]/dt ) = ...
- Sun Mar 06, 2022 11:22 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: k vs. k'
- Replies: 6
- Views: 270
Re: k vs. k'
When trying to find the overall reaction order, it can be helpful to do multiple experiments to find n,m,l, etc. So k' just refers to the psuedo rate constant for rate law where there is only a noticeable change in one reactant. It can be useful to find the real rate constant after the overall react...
- Sun Mar 06, 2022 11:14 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Half life and rate constant
- Replies: 25
- Views: 879
Re: Half life and rate constant
Only in the first order reactions. Remember that both a 0th and 2nd order reaction require the initial concentration of the reactant to determine the half life. These observations are consistent with the integrated rate laws that Dr. Lavelle derived in class last week.
- Mon Feb 28, 2022 1:03 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cell Diagrams
- Replies: 9
- Views: 356
Re: Cell Diagrams
What is the difference between using a different metal for an electrode than using the same one as the one in the reaction?
- Mon Feb 28, 2022 1:01 am
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Magnitude of the Cell Potential
- Replies: 4
- Views: 162
Re: Magnitude of the Cell Potential
This means that the equations 2Fe3+ + 6e- => 2Fe Fe3+ + 3e- => Fe have the same standard reduction potentials. This becomes useful when balancing more complicated redox reactions with different numbers of electrons needed or produced, because the reduction potential stays the same no matter what coe...
- Mon Feb 28, 2022 12:55 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Nernst Equation
- Replies: 4
- Views: 183
Re: Nernst Equation
Nernst equation is used to calculate the Cell Potential under any conditions and concentration ratios of product to reactant. As electrons from the oxidized metal flow toward the cathode, the Cell Potential will slowly decrease and will become 0 at which point the "battery is dead"
- Mon Feb 28, 2022 12:51 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Gibbs Free Energy with Phase Changes
- Replies: 2
- Views: 135
Re: Gibbs Free Energy with Phase Changes
At the Boiling point, the phases Co-exist and the formation of either full gas or liquid will not occur unless the temperature increases or decreases from this point.
- Mon Feb 28, 2022 12:46 am
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Determining reaction spontaneity using ΔS
- Replies: 3
- Views: 163
Re: Determining reaction spontaneity using ΔS
If you are given or solve for the Delta S of a system, then it must be used in conjunction with the gibbs free energy equation (ΔG = ΔH − T * ΔS) If ΔG is negative, then the reaction will be spontaneous If you are given or solve for the Delta S of the Universe, and determine that it is positive, the...
- Mon Feb 21, 2022 4:46 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: E=0
- Replies: 9
- Views: 457
Re: E=0
At equilbrium, the concentrations of the products and reactants (the substances in the anode and cathode) are not changing. Equilibrium means that Delta G is 0.
This must mean that there is no net electron transfer, thus the cell potential (voltage) will be 0 V.
This must mean that there is no net electron transfer, thus the cell potential (voltage) will be 0 V.
- Mon Feb 21, 2022 4:41 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Concentration and Cell Potential
- Replies: 3
- Views: 156
Re: Concentration and Cell Potential
As Dr. Lavelle explained on Friday's lecture, these batteries start out at a maximum voltage (most negative Delta G). However, as the reaction proceeds, the product to reactant ratio increases and thus the forward reaction that generates voltage becomes less favorable. So as Delta G decreases, so do...
- Mon Feb 21, 2022 4:37 pm
- Forum: Balancing Redox Reactions
- Topic: Achieve HW #5
- Replies: 2
- Views: 273
Re: Achieve HW #5
Since the Mn goes from a +7 to a +4, it is reduced and therefore an oxidizing agent. Since the S goes from a -2 to a 0, it is oxidized and therefore a reducing agent. Balance both the half reactions by adding the right number of electrons, water molecules, and H+'s to both reactions (only the Mn red...
- Mon Feb 21, 2022 4:32 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Entropy due to pressure
- Replies: 4
- Views: 264
Re: Entropy due to pressure
Yes it definitely can. If the temperature rises in a constant volume calorimeter or any sort of constant volume system, then by PV=nRT, both the pressure and temperature increases. Dr. Lavelle mentioned the equation for a constant Volume gas undergoing entropy change as change in entropy ∆S = n*Cv*l...
- Mon Feb 21, 2022 4:25 pm
- Forum: Van't Hoff Equation
- Topic: Equilibrium Constant
- Replies: 6
- Views: 265
Re: Equilibrium Constant
Just to add on to what was said above, the equation should more specifically be ∆G°= -RTlnK. Make sure to know the difference between ∆G an ∆G°, because ∆G changes as the ratio of products to reactants changes during the course of a reaction.
- Sun Feb 13, 2022 3:00 am
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Spontanteous
- Replies: 41
- Views: 1256
Re: Spontanteous
A spontaneous reaction means that the products are naturally favored in a reaction. When delta G is negative, this occurs
- Sun Feb 13, 2022 2:56 am
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Entropy
- Replies: 4
- Views: 154
Re: Entropy
Entropy is useful because it can help tell us whether a reaction is favorable. For example, we would think that if a reaction needs a great input of heat (endothermic) to proceed, we would think that it is not favorable. However, if the degree of disorder increases substantially enough or if the rea...
- Sun Feb 13, 2022 2:52 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: Residual Entropy vs. Thermal Entropy
- Replies: 2
- Views: 129
Re: Residual Entropy vs. Thermal Entropy
Residual entropy is the difference between the non-equilbrium state and the crystal state of a substance at a temp close to absolute zero. Basically, a molecule that can exist in more than 1 state, like COF2, will have more residual entropy than BF3 (symmetries). Thermal entropy, however, is just th...
- Sun Feb 13, 2022 2:47 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: What is Gibb's Free Energy?
- Replies: 3
- Views: 115
Re: What is Gibb's Free Energy?
Gibbs free energy is the maximum amount of non-expansion, reversible work that can occur inside of a thermodynamically isolated system at a constant temperature and pressure. A negative value means that the reaction is spontaneous, and a reaction at equilibrium has no change in gibbs free energy
- Sun Feb 13, 2022 2:39 am
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Entropy and degeneracy
- Replies: 5
- Views: 233
Re: Entropy and degeneracy
They are both related. Degeneracy is the specific number of ways you can achieve a certain state, while Entropy is calculated with the equation: S=kb ln(W). So while it is not a 1:1 relationship, as W increases - so does S.
- Mon Feb 07, 2022 1:25 am
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Delta U Gas Expansion
- Replies: 5
- Views: 268
Re: Delta U Gas Expansion
Although this doesn't occur very often in real life, the example of isothermal reversible expansion explains this concept very well. Since the process occurs in infinitesimal steps, all of the added heat to the system is converted into work. As mentioned in the previous reply, the internal energy st...
- Mon Feb 07, 2022 1:19 am
- Forum: Calculating Work of Expansion
- Topic: Why is the PV curve vertical initially for irreversible expansion?
- Replies: 4
- Views: 200
Why is the PV curve vertical initially for irreversible expansion?
I don't get why the volume basically doesn't change at all in the first step of an irreversible expansion. In my head, it makes sense for the system to expand quickly if the external pressure was quickly reduced.
- Mon Feb 07, 2022 1:18 am
- Forum: Calculating Work of Expansion
- Topic: Work of Irreversible vs Reversible Expansions
- Replies: 2
- Views: 151
Work of Irreversible vs Reversible Expansions
Could someone explain why the work for an irreversible process, like a constant pressure expansion, requires less work?
- Mon Feb 07, 2022 1:07 am
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Boltzmann equation
- Replies: 2
- Views: 127
Re: Boltzmann equation
I'm pretty sure we don't have to know the derivation of the equation, we just have to know how to use it. This might also include solving for W since Lavelle went over this in lecture, using:
W = (number of possible states)^number of particles
W = (number of possible states)^number of particles
- Mon Feb 07, 2022 1:02 am
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: T change reversible v irreversible
- Replies: 2
- Views: 133
Re: T change reversible v irreversible
In an isothermal reversible expansion, the reason the temperature stays the same is because it is a very slow process and all the heat that enters the system is converted into work that then expands the system. This is different from irreversible expansion where the temp decreases first. I was also ...
- Sun Jan 30, 2022 11:56 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: qp = ∆H rxn
- Replies: 1
- Views: 120
Re: qp = ∆H rxn
I believe in cases of constant pressure, like the closed system example Lavelle gave on Friday's lecture, qp is equated to delta H, NOT delta H (rxn).
This is straight from the Outline 3 document:
Distinguish ∆U and ∆H and show how they are related. When q = qP then ∆U = ∆H - P∆V
This is straight from the Outline 3 document:
Distinguish ∆U and ∆H and show how they are related. When q = qP then ∆U = ∆H - P∆V
- Sun Jan 30, 2022 11:34 pm
- Forum: Phase Changes & Related Calculations
- Topic: State Property
- Replies: 15
- Views: 510
Re: State Property
A state property just means that the path that you take to get from start to end does not affect its value. Energy, temperature, mass, density, etc. are all state functions because their values don't depend on the pathway to get there. However, if you look at work and heat, the specific path matters...
- Sun Jan 30, 2022 11:16 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Releasing energy and absorbing energy
- Replies: 5
- Views: 211
Re: Releasing energy and absorbing energy
I would say that a negative delta H always means that heat was given off. As we might learn later in this course, total the change in gibbs free energy could be positive when delta H is negative and vice versa. But yes, the sign on the delta H can indicate whether or not heat left or was introduced ...
- Sun Jan 30, 2022 11:12 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Textbook 4E. 5
- Replies: 5
- Views: 414
Re: Textbook 4E. 5
Since each of the 6 carbons is already attached to a hydrogen before, you don't need to worry about breaking and/or re-forming those bonds in your calculations. Drawing the structure as shown above on a problem like this definitely helps!
- Sun Jan 23, 2022 2:35 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Textbook 4A. 9
- Replies: 3
- Views: 138
Re: Textbook 4A. 9
Since the amount of energy that the copper gives off is equal to the amount of energy that the water takes in, you can set the equations up as so:
qw=-qc
(57)(4.18)(Tf-22) = -(20)(0.38)(Tf-100)
Solve for Tf, it should be between 22 and 100.
qw=-qc
(57)(4.18)(Tf-22) = -(20)(0.38)(Tf-100)
Solve for Tf, it should be between 22 and 100.
- Sun Jan 23, 2022 1:16 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Heat Capacity
- Replies: 10
- Views: 816
Re: Heat Capacity
Because it allows us to still perform calculations on the energy change within a system without having to know the specific amounts of moles or reaction equations. Take the first question from the week 3 discussion section. All we have to know is the heat capacity (in this case calculating it from a...
- Sun Jan 23, 2022 12:58 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: textbook 4.d 1
- Replies: 1
- Views: 170
Re: textbook 4.d 1
All you need is an understanding of stoichiometry here. So they tell us that 358.8 kJ of Energy is absorbed/required per mole of this reaction. So for the first part, since there is 1 mol of s8/mol of rxn, we can just multiply the 358.8 kJ /mol rxn * 1.25 mol rxn to get 448.5 kJ. Do the same stoichi...
- Sun Jan 23, 2022 12:36 pm
- Forum: Calculating Work of Expansion
- Topic: Reversible Processes vs. Irreversible processes
- Replies: 3
- Views: 356
Re: Reversible Processes vs. Irreversible processes
Yes, you explained it pretty well. Irreversible processes do not return to equilibrium (e.g. turn from expansion back to compression) with only a small change of say the external environment. This would be the case in say an isothermal reversible expansion, where the outside pressure matches the ins...
- Sat Jan 22, 2022 9:32 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Internal Energy
- Replies: 3
- Views: 468
Re: Internal Energy
Knowing how much work was done on/by the system as well as how much heat was added or removed from the system help determine the change in internal energy, since Delta U = q+w. This is important because energy is constantly being transformed from one form to another, leaving certain systems and ente...
- Sat Jan 22, 2022 9:25 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Melting (fusion)
- Replies: 27
- Views: 1055
Re: Melting (fusion)
Since the final product (liquid) has more energy than the reactants (solid), energy must have been added into the system. Hence, it is exothermic. However, I was kinda confused why the Delta H fus representing melting, because doesn't fusion mean bringing particles together??
- Sun Jan 16, 2022 3:40 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: pH value
- Replies: 39
- Views: 2866
Re: pH value
when more [H+] is introduced into the system, the solution becomes more acidic
- Sun Jan 16, 2022 3:29 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Weak acids creating low pH
- Replies: 4
- Views: 210
Re: Weak acids creating low pH
pH in a solution is not only determined by the acid dissociation constant. It's concentration also will affect the pH. It is very possible to have a weak acid that is just present in a very large concentration that then creates a very low pH. This would not be the case if we took a strong acid like ...
- Sun Jan 16, 2022 3:25 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Catalysts
- Replies: 11
- Views: 370
Re: Catalysts
catalysts can only affect the rate at which a reaction proceeds toward equilibrium, and as a result adding or removing it does not affects any values in the equilibrium equation. Only changes in temperature, concentrations of products or reactants, and pressure could cause a shift toward equilibrium.
- Sun Jan 16, 2022 3:23 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Salts in Acid/Base Problems
- Replies: 2
- Views: 107
Re: Salts in Acid/Base Problems
the cations in group 1 and 2 are conjugates of strong bases and so they would not reform bases in solution. That is why we consider them spectator ions. The conjugates of weak acids or bases, however, will react at equilibrium to change the pH. For, example, the CO3 2- in K2CO3 would reform HCO3- at...
- Sun Jan 16, 2022 3:11 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: HW - #10
- Replies: 4
- Views: 181
Re: HW - #10
For every mole of N2O4 that is produced after the extra product is added, 2 moles of NO2 are used up. I thought of the reaction going in the opposite way, so I put N2O4 on the numerator and NO2 on the denominator of the equilibrium expression.
- Sun Jan 09, 2022 1:19 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: yield of product
- Replies: 7
- Views: 768
Re: yield of product
When product is removed at equilibrium, the reverse reaction decreases and "doesn't push back" as hard. Thus, equilibrium shifts right as the reactants react to create more of the product that was lost.
- Sun Jan 09, 2022 1:11 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Endothermic and Exothermic Reactions
- Replies: 4
- Views: 181
Re: Endothermic and Exothermic Reactions
Basically adding heat will always cause an endothermic reaction to become more favorable (since adding heat helps get the required energy for the reaction). So when heat is given off in a reaction (exothermic) the reverse reaction will need be endothermic. That is why the reverse reaction, or formin...
- Thu Jan 06, 2022 10:15 am
- Forum: Ideal Gases
- Topic: Why is K=1 rare?
- Replies: 44
- Views: 1479
Re: Why is K=1 rare?
There is almost always going to be a set of products that is more or less stable than the reactants. This is because unique configurations all have unique energies due to their arrangements and chemical makeup, so that's why its rare to find products with the same favorability of formation.
- Thu Jan 06, 2022 10:08 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: net ionic equations
- Replies: 2
- Views: 124
Re: net ionic equations
Net ionic equations help us easily see what needs to go into the equilibrium constant equation. The spectator ions, if placed into the equation, would just cancel each other out.
- Thu Jan 06, 2022 10:03 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: When Q < K
- Replies: 11
- Views: 404
Re: When Q < K
When Q<K, it means that the ratio of product/reactant is less than what it should be at equilibrium. So to increase this ratio to get to equilibrium, reactants must get used up to make products so the forward reaction would be favored in this instance.
- Sat Dec 04, 2021 2:35 am
- Forum: Hybridization
- Topic: Bonding of Hybridized Orbital
- Replies: 3
- Views: 318
Re: Bonding of Hybridized Orbital
Hybridized orbitals overlap head on and cannot form pi bonds. Pi bonds can only result from un-hybridized p orbitals that do not allow free rotation and overlap side to side
- Sat Dec 04, 2021 1:16 am
- Forum: Trends in The Periodic Table
- Topic: Degenerate?
- Replies: 7
- Views: 679
Re: Degenerate?
Thanks for the explanation. However I am still confused on how this would apply to atom like Helium. Even though it has multiple electrons, wouldn't the only available orbital be 1s? Because there are no other values of l in the first energy level right? "This degeneracy of orbitals with the sa...
- Sat Dec 04, 2021 12:52 am
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Degenerate Orbitals
- Replies: 5
- Views: 712
Re: Degenerate Orbitals
I believe in multiple electron systems, all orbitals cannot be degenerate due to electron-electron repulsion that distinguishes for example 2s from 2p at different energies. However, in single electron systems, without such repulsion, all orbitals will be degenerate. And as stated above by Darlene, ...
- Sat Dec 04, 2021 12:29 am
- Forum: Photoelectric Effect
- Topic: Work Function
- Replies: 19
- Views: 1336
Re: Work Function
Work function is just the energy required for an electron to be ejected from the metal by a photon. The overall equation is Photon Energy (hv) - Work Function = Kinetic Energy of electron (0.5mv^2)
- Fri Dec 03, 2021 11:53 pm
- Forum: Photoelectric Effect
- Topic: Intensity of light
- Replies: 5
- Views: 554
Re: Intensity of light
That's right, increasing the intensity simply increases the quantity of photons in a given beam of light, and it doesn't change the Energy of any single photon.
- Sun Nov 28, 2021 1:29 pm
- Forum: Hybridization
- Topic: Octet Expansion
- Replies: 5
- Views: 276
Re: Octet Expansion
Since the d-orbital is in the same principal energy level as a given s and p, leaking electrons from the d orbital to form bonds in period 3+ elements can create a molecule with a lower energy (more stable). This is because if a molecule was forced to place electrons into say the 4s level instead of...
- Sun Nov 28, 2021 1:24 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: pH Scale
- Replies: 9
- Views: 346
Re: pH Scale
a pH can be be below 0 in the case of superacids, where the chemical potential of protons is higher than it is in pure sulfuric acid. This causes the mixture to behave as if there is greater than a 1.0 molarity of Proton, for example 1.1. Taking the negative log of this molarity would result in a ne...
- Sun Nov 28, 2021 1:20 pm
- Forum: Bronsted Acids & Bases
- Topic: Ka of Strong Acids
- Replies: 10
- Views: 595
Re: Ka of Strong Acids
Strong acids are not given a Ka because they are assumed to almost fully dissociate in water. The Ka values would be so large (since the equilibrium would favor the forward reaction) that it would not be productive to compare the Ka's among strong acids. However, weak acids often favor the reverse r...
- Sun Nov 28, 2021 1:16 pm
- Forum: Industrial Examples
- Topic: Cisplatin Vs. Transplatin
- Replies: 7
- Views: 1561
Re: Cisplatin Vs. Transplatin
Having both the chlorines on the same side of the platinum allows a coordination complex to form to the adjacent guanines on the DNA molecule. However, in the trans form, such a complex could not form. This is why the cisplatin is a much more effective chemo drug as it prevents DNA replication
- Sun Nov 28, 2021 1:06 pm
- Forum: Biological Examples
- Topic: Biological Examples on the final
- Replies: 4
- Views: 213
Re: Biological Examples on the final
Similar to how Dr. Lavelle explained how cisplatin works with DNA, we may be given a new scenario where we have to apply concepts about coordination compounds. I'm guessing that many biological compounds form chelates (ligands which form rings that include the central metal atom), so it may be worth...
- Sun Nov 28, 2021 12:53 pm
- Forum: Naming
- Topic: Achieve week 9 #1
- Replies: 17
- Views: 682
Re: Achieve week 9 #1
Im pretty sure the answer is "triamminetrichlorocobalt(III)"
However, I thought that if there would be 2 of the same prefixes, then you would have to change one. Why wouldn't the first tri- change to tris- ?
However, I thought that if there would be 2 of the same prefixes, then you would have to change one. Why wouldn't the first tri- change to tris- ?
- Fri Nov 19, 2021 4:57 pm
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: Strong Acids and Bases?
- Replies: 2
- Views: 113
Re: Strong Acids and Bases?
I believe we have to 'memorize them', or at least some of the common ones. Here is a list to them! https://chem.libretexts.org/Bookshelves/General_Chemistry/Book%3A_ChemPRIME_(Moore_et_al.)/11%3A_Reactions_in_Aqueous_Solutions/11.09%3A_Strong_Acids_and_Bases I think it's pretty easy to memorize that...
- Fri Nov 19, 2021 4:38 pm
- Forum: Amphoteric Compounds
- Topic: General question
- Replies: 14
- Views: 602
Re: General question
A perfect example of an amphoteric molecule is water, because it could either gain a proton to become hydronium or lose a proton to become hydroxide. Another example, is HSO4-, which is an important buffer in biological systems. It is formed after hydrogen sulfate donates a proton, and the resulting...
- Fri Nov 19, 2021 4:34 pm
- Forum: Bronsted Acids & Bases
- Topic: What determines acidity?
- Replies: 1
- Views: 151
What determines acidity?
Take glucose and HCl. Both are polar molecules that have dipole-dipole interactions, and have hydrogens with partial positive charges. However, HCl separates (dissociates) into ions in solution, whereas individual glucose molecules stay together and are each surrounded by water molecules (they disso...
- Fri Nov 19, 2021 4:27 pm
- Forum: Bronsted Acids & Bases
- Topic: Acids in solution
- Replies: 5
- Views: 398
Re: Acids in solution
Whenever pH or acidity is mentioned, it always means that there is an accompanying solution. Without water or solution, these acids would be normal molecules that are not actively donating protons. It is only until acid comes into contact with water (such as pouring HCl onto your skin) causes the ti...
- Fri Nov 19, 2021 4:21 pm
- Forum: Properties & Structures of Inorganic & Organic Bases
- Topic: relative acidity
- Replies: 5
- Views: 604
Re: relative acidity
In solution, an anion can be stabilized by ion-dipole interactions with electropositive hydrogens for example(-15 kJ/mol). This would reduce the energy of the anion, stabilizing it.
- Fri Nov 19, 2021 4:18 pm
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: Acid and Base characteristics
- Replies: 6
- Views: 306
Re: Acid and Base characteristics
The strength of Bronsted Acids is often determined by how strong the H-A bond is. For instance, a hydrogen bonded to the oxygen is much more easily ionized in solution when compared to say methylamine. If you were to view 3-D electrostatic potential maps of these molecules, the stronger acids will h...
- Mon Nov 15, 2021 4:02 pm
- Forum: Lewis Structures
- Topic: Bent and linear vsepr models
- Replies: 4
- Views: 201
Re: Bent and linear vsepr models
I'm pretty sure there isn't really a shape we assign to a central atom that only has 1 bond. If anything, there needs to be at least 2 bonded atoms to determine a proper angle.
- Mon Nov 15, 2021 3:56 pm
- Forum: Hybridization
- Topic: Pi Bonds [ENDORSED]
- Replies: 38
- Views: 1839
Re: Pi Bonds [ENDORSED]
That is correct, the lower energy hybrid orbitals will make sigma bond(s) first, and the remaining un-hybridized p orbitals can make higher energy pi bonds.
- Mon Nov 15, 2021 3:51 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Xe
- Replies: 41
- Views: 2131
Re: Xe
Similar to any other expanded octet atom, we would only be able to determine the shape if we knew which atoms and how many were bonded. For example, XeF2 would have 3 lone pairs and be linear, but XeF4 would have 2 lone pairs and be square planar. In summary, since Xe has no formal charge, match the...
- Mon Nov 15, 2021 3:29 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Weeks 7 and 8 Homework, Question 5
- Replies: 16
- Views: 556
Re: Weeks 7 and 8 Homework, Question 5
The axial atoms are the ones that are on the y-axis, and the equatorial ones are on the x-axis. This is similar to thinking about the axial atoms like the north and south pole, and the equatorial ones are the ones along the equator
- Mon Nov 15, 2021 3:18 pm
- Forum: Sigma & Pi Bonds
- Topic: N2 hybridization
- Replies: 3
- Views: 188
Re: N2 hybridization
Yes, the hybrid model would be correct
- Tue Nov 09, 2021 12:18 am
- Forum: Formal Charge and Oxidation Numbers
- Topic: Radicals
- Replies: 4
- Views: 129
Radicals
Can someone explain why the textbook says that NO2- is a radical (2C #1). I believe that it should be NO2 that is a radical, not NO2-.
- Sun Nov 07, 2021 3:08 pm
- Forum: Dipole Moments
- Topic: Polar bonds
- Replies: 2
- Views: 113
Re: Polar bonds
Unless there are 2 identical elements, there will almost always be some difference in electronegativity between atoms in a bond. However, in the case of C-H, that difference is so low that no significant dipole-dipole interactions ever arise. However, if the difference starts becoming higher than th...
- Sun Nov 07, 2021 3:04 pm
- Forum: Ionic & Covalent Bonds
- Topic: Ionic characteristics in covalent bonds
- Replies: 6
- Views: 252
Re: Ionic characteristics in covalent bonds
The more the difference between electronegativity there is, the more ionic character a covalent bond will have. Having a majority ionic character will cause the substance to be structured in more of a lattice, as the atoms will act more as ions rather than share electrons with a covalent bond. Havin...
- Sun Nov 07, 2021 2:57 pm
- Forum: Ionic & Covalent Bonds
- Topic: Intermolecular Forces
- Replies: 10
- Views: 401
Re: Intermolecular Forces
dipole-dipole interactions are found between 2 polar molecules (such as H-F and NH3), whereas dipole-induced-dipole is when a polar molecule casuses a non polar molecule to become polar to shifting electron density (H-F and O=O). Dr. Lavelle mentioned that they both have a strength of -2 kJ/mol
- Thu Nov 04, 2021 12:57 pm
- Forum: Ionic & Covalent Bonds
- Topic: Hydrogen Bonding
- Replies: 6
- Views: 232
Re: Hydrogen Bonding
Basically in molecules with stronger intermolecular forces, it becomes harder to melt or boil it. In a molecule like water (H20), the difference in electronegativity between the hydrogen and oxygen makes the dipole interactions much stronger than in H2S, and as a result the water molecules want to &...
- Thu Nov 04, 2021 12:50 pm
- Forum: Lewis Structures
- Topic: Lewis Structures and Resonance
- Replies: 10
- Views: 349
Re: Lewis Structures and Resonance
The structure with the least distribution of formal charge would be the most stable - also placing negative charges on more electronegative atoms will increase the stability of the molecule. However, in many cases there are many "equivalent" resonance structures. The example Dr. Lavelle me...
- Sun Oct 31, 2021 6:50 pm
- Forum: Lewis Structures
- Topic: Lewis Structures for expanded Octets
- Replies: 5
- Views: 151
Re: Lewis Structures for expanded Octets
So then how come Chlorine doesn't make 7 bonds? Is there even a maximum number of bonds an atoms can make?
- Sun Oct 31, 2021 6:48 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charge and Lewis Structure
- Replies: 4
- Views: 210
Re: Formal Charge and Lewis Structure
So yes, in general having O formal charge across a molecule makes it the most stable. However, if there happens to be charge in the molecule, it would be best to place negative charge on the most electronegative elements, and positive charge on the most electropositive elements. For example, it woul...
- Sun Oct 31, 2021 6:44 pm
- Forum: Electronegativity
- Topic: trends
- Replies: 41
- Views: 1428
Re: trends
Atoms with a larger radius would have lower electronegativity due to having a lower effective nuclear charge. Adding electron shells increases the shielding effect and prevents the protons in the nucleus from "holding on" as tightly to the valence electrons. So it would be harder to attrac...
- Sun Oct 31, 2021 6:38 pm
- Forum: Lewis Structures
- Topic: Lewis Structures for expanded Octets
- Replies: 5
- Views: 151
Lewis Structures for expanded Octets
For elements besides the ones Dr. Lavelle showed in class (Phosphorous and Sulfur), how are we supposed to know if say an element with d or f electrons would be more stable with 4 or 5 bonds? Is there some rule or concept that tells us why PCl5 is more stable than PCl4?
- Sun Oct 31, 2021 6:35 pm
- Forum: Coordinate Covalent Bonds
- Topic: Lewis Acid and Base
- Replies: 6
- Views: 243
Re: Lewis Acid and Base
Lewis Acids are compounds that accept electrons, such as boron in BF3. Lewis bases are compounds that donate electrons, such as F- donating 2 electrons to Boron in BF3. The resulting bond is a coordinate covalent bond, meaning that both electrons in the new B-F bond both came from the same species)....
- Sun Oct 31, 2021 6:22 pm
- Forum: Polarisability of Anions, The Polarizing Power of Cations
- Topic: Cause of cation polarization
- Replies: 3
- Views: 165
Re: Cause of cation polarization
So yes, in general, a higher charged cation would have more polarizing power. However, if you were to compare to cations of the same charge (e.g. Mg 2+ vs Ca 2+), then the atom with the smaller atomic radius would have a higher polarizing power. This would be due to the fact that the smaller cation ...
- Thu Oct 28, 2021 12:13 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: formal charge
- Replies: 4
- Views: 203
Re: formal charge
Having a negative formal charge on a more electronegative (and vice versa having a positive formal charge on the more electropositive atom) will be more stable. Since oxygen is more electronegative, it is thus more stable with a negative charge. This helps us determine which Lewis structures are mos...
- Mon Oct 25, 2021 7:08 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Aufbau Principle
- Replies: 12
- Views: 935
Re: Aufbau Principle
Tha Aufbau principle is also called the building up principle, and it means that electrons will (generally) fill lower energy orbitals before filling higher energy ones. For example, 2s would be filled before electrons start to fill 2p.
- Mon Oct 25, 2021 7:04 pm
- Forum: Trends in The Periodic Table
- Topic: E- and Valence Shells [ENDORSED]
- Replies: 16
- Views: 892
Re: E- and Valence Shells [ENDORSED]
Adding an electron to a filled valence shell would cause for the energy of the molecule to increase as the electron would have to occupy a new shell. This is why noble gases often do not react in nature due to the fact that they are very stable and electrons neither want to leave or join.
- Mon Oct 25, 2021 7:00 pm
- Forum: Resonance Structures
- Topic: Delocalized electrons
- Replies: 9
- Views: 562
Re: Delocalized electrons
The term delocalized means that the electron density of a particular double bond or charge is not bound to one electron and the lowest energy (most stable) form of the molecule involves that electron density being distributed across multiple areas of the molecule.
- Mon Oct 25, 2021 6:57 pm
- Forum: Lewis Structures
- Topic: Valence Electrons
- Replies: 12
- Views: 864
Re: Valence Electrons
Usually, we can calculate the valence electrons by looking at the s and p orbitals. So Dr. Lavelle just counts across a period and skips over the f and d blocks, to count the number of electrons that would be in the outermost shell.
- Mon Oct 25, 2021 6:54 pm
- Forum: Ionic & Covalent Bonds
- Topic: Ionization energy
- Replies: 4
- Views: 329
Re: Ionization energy
The gaseous state minimizes all other potential forces from interfering (such as the increased particle-particle interactions in solids and liquids), so that the Ionization energy can most closely depict how much energy is needed to remove one electron.
- Mon Oct 18, 2021 1:05 am
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: H hat/2pi vs H/4pi [ENDORSED]
- Replies: 2
- Views: 289
Re: H hat/2pi vs H/4pi [ENDORSED]
H hat is generally used in higher level courses with more complex derivations, but as long as you know how to interchange the constants there should be no issue. H hat is the reduced form of planck's constant, with quantizes angular momentum. H hat = h/2pi
- Mon Oct 18, 2021 12:59 am
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Px,Pz [ENDORSED]
- Replies: 3
- Views: 197
Re: Px,Pz [ENDORSED]
Generally, a +1 would indicate px - However, I remember Dr. Lavelle stating that it was more important that we stay consistent with whatever is provided to us (it would be given to us on an exam) versus trying to remember what is what - since different books go by different rules.
- Mon Oct 18, 2021 12:57 am
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: spin [ENDORSED]
- Replies: 11
- Views: 449
Re: spin [ENDORSED]
Spin states have to with the angular momentum of an electron. +1/2 means the spin is up, and if you use the right hand rule you'd see that the electron would be going counter-clockwise. And vice versa for the -1/2 spin
- Mon Oct 18, 2021 12:50 am
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: 4s vs 3d subshells
- Replies: 4
- Views: 261
4s vs 3d subshells
After the lecture, I still have a question about 4s and 3d subshells. Does the 4s subshell have more energy than the 3d one? Some other online sources were saying otherwise so I'm not quite sure what is true
- Mon Oct 18, 2021 12:44 am
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Ground state vs Excited state [ENDORSED]
- Replies: 7
- Views: 334
Re: Ground state vs Excited state [ENDORSED]
An electron in an excited state will be in a different subshell or shell, so the configuration would be different. Although the total number of electrons would stay the same.
- Sun Oct 10, 2021 4:59 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: London Dispersion Forces
- Replies: 12
- Views: 989
Re: London Dispersion Forces
They are temporary induced dipoles that occur in all molecules, but are most observed in non-polar molecules. This effect, caused by the rapidly shifting electrons in their electron clouds, creates temporary regions of partial positive charge and temporary regions with partial negative charge. These...
- Sun Oct 10, 2021 4:52 pm
- Forum: Trends in The Periodic Table
- Topic: effective nuclear charge and shielding
- Replies: 4
- Views: 307
Re: effective nuclear charge and shielding
effective nuclear charge of an element is defined as the atomic number of the element - the number of non-valence electrons. Going across across a row increases the number of protons but does not increase the number of shielding (non-valence) electrons. Thus there is a higher pull from the nucleus o...
- Sun Oct 10, 2021 4:42 pm
- Forum: Properties of Electrons
- Topic: What does this symbol mean?
- Replies: 18
- Views: 2679
Re: What does this symbol mean?
That symbol is used to relate 2 values that are proportional to each other. For example, in Planck's equation E=hv, the energy of a photon is directly proportional to the photon's frequency