Search found 105 matches
- Sat Mar 12, 2022 3:31 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Change in Entropy
- Replies: 3
- Views: 223
Change in Entropy
In the reaction C(s) + O2(g) into CO2 (g), does entropy decrease or increase? It goes from two moles to one so that would decrease entropy but carbon also goes from solid to gas so I'm not sure.
- Sat Mar 12, 2022 1:43 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Gibbs and Entropy
- Replies: 7
- Views: 294
Re: Gibbs and Entropy
Gibbs free energy and entropy are related by the equation deltaG = deltaH - TdeltaS. That means when there is an increase in entropy there is a decrease in Gibbs free energy. A process becomes more spontaneous the more disordered it becomes in a way.
- Sat Mar 12, 2022 1:33 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Catalysts
- Replies: 33
- Views: 1001
Re: Catalysts
For the most part the catalyst will appear in the first step of the reaction. However, it is possible for it to pop up in a later elementary reaction I believe. The important to differentiate a catalyst that appears later and an intermediate is that an intermediate will be a product first while the ...
- Sat Mar 12, 2022 1:25 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: Molecularity
- Replies: 5
- Views: 234
Re: Molecularity
Molecularity is the number of reactants that you have and not the total number of substances you have. So the number of moles you have on the reactant side is the molecularity that you have in an elementary step.
- Sat Mar 12, 2022 1:18 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Rate Constants Change with Temperature
- Replies: 4
- Views: 176
Re: Rate Constants Change with Temperature
I don't think it does. For the equation k = Ae^(-Ea/RT). Raising the temperature of a lower activation energy would increase the rate constant more than if you were to do it at a higher activation energy. In this equation, e is raised to the negative (Ea/RT) so lower activation energies result in hi...
- Fri Mar 11, 2022 11:22 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Entropy Change
- Replies: 10
- Views: 1436
Entropy Change
How can you tell if entropy change is positive or negative based on the chemical equation? Is it based on the change of states or number of moles?
- Wed Mar 09, 2022 9:27 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Steady-State Approach
- Replies: 1
- Views: 79
Steady-State Approach
Why is the steady-state approach more general than the pre-equilibrium approach? Also, is there a better one to use?
- Sun Mar 06, 2022 11:49 am
- Forum: Zero Order Reactions
- Topic: nth Order Reactions?
- Replies: 4
- Views: 240
Re: nth Order Reactions?
It technically is possible. However, these reactions happen when all these molecules collide with each other at the same time. The more molecules needed to collide or the higher the order of reaction, the less likely the collision happens. If the collision doesn't happen then the reaction doesn't re...
- Sun Mar 06, 2022 11:46 am
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Different Products
- Replies: 4
- Views: 175
Different Products
If a reaction can have two different products and one product has a lower activation energy than the other one, does that mean one product doesn't form at all?
- Sun Mar 06, 2022 11:00 am
- Forum: Zero Order Reactions
- Topic: No Effect
- Replies: 23
- Views: 787
No Effect
How is it possible for a reaction to be zero order? Why can changing the concentration of a reactant have no effect on the rate of reaction?
- Sun Mar 06, 2022 10:53 am
- Forum: General Rate Laws
- Topic: Reactant concentration in initial reaction rates
- Replies: 4
- Views: 168
Re: Reactant concentration in initial reaction rates
When calculating initial reaction rate, we only focus on the initial reaction concentration and not the product concentration because the reaction has not technically started. The initial reaction rate is when t=0 so at that time there are only reactants and no products formed yet. This also makes c...
- Sun Mar 06, 2022 10:51 am
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Can a reaction only be kinetically OR thermodynamically controlled?
- Replies: 8
- Views: 496
Re: Can a reaction only be kinetically OR thermodynamically controlled?
I feel like a reaction can be controlled by both kinetics and thermodynamics. Thermodynamics tells us what direction the reaction is going. It tells us if the reaction will form products or reactants. Kinetics controls how fast the reaction reaches equilibrium. So you can control a reaction by makin...
- Sun Feb 27, 2022 4:11 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Cell Potential
- Replies: 37
- Views: 1206
Re: Cell Potential
It means that the reverse reaction is spontaneous.
- Sun Feb 27, 2022 4:10 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: closed system
- Replies: 5
- Views: 274
Re: closed system
Combustion itself should be exothermic. Maybe in lecture there was something else to that problem or explanation where the heat released is balanced out by something so that the overall temperature stays the same.
- Sun Feb 27, 2022 3:58 pm
- Forum: Calculating Work of Expansion
- Topic: Temp in Irreversible vs Reversible Rxn
- Replies: 3
- Views: 250
Re: Temp in Irreversible vs Reversible Rxn
A reversible reaction work is done in infinitesimal increments. As a result, the change is really close to 0 and the overall system doesn't really change, so temp is constant. A irreversible reaction has a noticeable change in the system especially in volume. That's why temperature changes.
- Sun Feb 27, 2022 3:54 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Sign of Entropy and Gibbs
- Replies: 4
- Views: 235
Re: Sign of Entropy and Gibbs
If entropy is negative, this means that the disorder of the system goes down. In other words, the system becomes more organized. Since the entropy of the universe is always increasing, this means that the entropy of the surroundings must increase and the increase has to be bigger than the decrease o...
- Thu Feb 24, 2022 7:06 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Change in Property
- Replies: 3
- Views: 202
Change in Property
So for delta S and delta G, the change is larger in the gas phase of a substance than the liquid or solid phase. Is this also true for enthalpy or delta H?
- Thu Feb 24, 2022 5:56 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: Entropy
- Replies: 1
- Views: 67
Entropy
Why is it that a heavier atom will have more thermally accessible vibrational energy levels and thus higher entropy?
- Sun Feb 20, 2022 5:42 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Metal Conductor
- Replies: 2
- Views: 110
Metal Conductor
Why is a metal like Platinum a good material to use in the batteries?
- Sun Feb 20, 2022 5:38 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Eº vs E
- Replies: 5
- Views: 264
Re: Eº vs E
S is just the entropy of the reaction or whatever you're looking at. S with the degree is the entropy under standard conditions. This means it is the entropy under a specific set of conditions. S is more general. It could be the same value as S with the degree if it has the same conditions as the st...
- Sun Feb 20, 2022 5:33 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Entropy Changes
- Replies: 3
- Views: 172
Re: Entropy Changes
Non-spontaneous processes do have a decrease in entropy. I may be wrong. but I'm pretty sure that the entropy of the universe is always increasing. As a result, the entropy of the system can decrease if the increase in entropy of the surroundings is greater than the decrease so there is an overall i...
- Sun Feb 20, 2022 5:29 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Achieve #7
- Replies: 5
- Views: 265
Re: Achieve #7
To find the enthalpy of vaporization, you divide the amount of energy produced by the heater by the difference in moles of the molecule. It's good to know that a watt is 1J/sec. To find the entropy of vaporization, you take what you got for enthalpy of vaporization and divide that by the boiling poi...
- Sat Feb 19, 2022 6:22 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Achieve 19
- Replies: 4
- Views: 158
Achieve 19
For the Achieve Week 5 problem 19, why do we use the R=8.314 gas constant if we are dealing with bars?
- Sun Feb 13, 2022 8:56 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: Entropy vs. Enthalpy
- Replies: 8
- Views: 336
Re: Entropy vs. Enthalpy
Enthalpy (H) is talking about the total heat content of the system. Entropy (S) is the disorder of the system or the number of possible positions the molecules can be in. They do have a direct relationship with each other but they aren't the same. DeltaS = deltaH/Temperature.
- Sun Feb 13, 2022 8:51 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Biology
- Replies: 3
- Views: 192
Biology
Why is Gibb's free energy a good thing to use to determine the spontaneity of biological reactions?
- Sun Feb 13, 2022 8:47 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: entropy
- Replies: 2
- Views: 107
Re: entropy
Entropy has a direct relationship with temperature. Change in entropy has an inverse relationship with temperature.
- Sun Feb 13, 2022 3:04 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Gibbs free energy and Work
- Replies: 2
- Views: 102
Gibbs free energy and Work
Why is Gibbs free energy the maximum for work?
- Sun Feb 13, 2022 2:09 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: K=0
- Replies: 2
- Views: 122
K=0
Entropy is 0 when K=0 and there are no impurities. I understand why K needs to be 0 but why can't there be any impurities? Since K=0, does everything kind of stop and entropy would be 0 regardless if there were impurities?
- Sun Feb 06, 2022 7:33 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Achieve week 4 question 18
- Replies: 4
- Views: 439
Re: Achieve week 4 question 18
You would use PV=nrT to calculate the change in volume of this reaction. I'm pretty sure you assume initially the volume is 0 so whatever you get from that equation is the deltaV. You use that to find work(w) using w=-PdeltaV. Then to find specific heat you use the 5R/2 with the R they give you, thi...
- Sun Feb 06, 2022 7:04 pm
- Forum: Calculating Work of Expansion
- Topic: Work of a Reversible Reaction
- Replies: 1
- Views: 93
Re: Work of a Reversible Reaction
I don't believe we will use any other equation for reversible reactions because integrals are really the only thing that can measure the infinitely small difference in volume of the system.
- Sun Feb 06, 2022 7:01 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Entropy, and Energy
- Replies: 3
- Views: 162
Re: Entropy, and Energy
I think entropy increases when energy increases as well. Entropy is a measure of disorder. When you put energy into molecules they get excited and move around more, thus causing more disorder. However, if you are talking about a system losing energy, the entropy of the surroundings will increase but...
- Sun Feb 06, 2022 6:58 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: System at Equilibrium (Internal Energy)
- Replies: 1
- Views: 82
Re: System at Equilibrium (Internal Energy)
Internal energy is at a minimum because there is no net exchange of energy anymore. If internal energy was above its minimum, the system would probably lose energy until it no longer can.
- Sun Feb 06, 2022 6:54 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Kw vs H+ and OH-
- Replies: 7
- Views: 519
Re: Kw vs H+ and OH-
You can't always assume [H30+]=[OH-]. However, for ex 6A.21 in the textbook, it tells you that you are dealing with water. Water has a pH of 7 which means that water is neutral and [H30+]=[OH-]. However, acids and bases have unequal concentrations and you would need to use ICE tables and have a litt...
- Sun Jan 30, 2022 3:58 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Negative pH
- Replies: 33
- Views: 3405
Re: Negative pH
A negative pH just means that the solution is really, really acidic. Its [H30+] is so high that the log of it is positive, thus resulting in the negative pH.
- Sun Jan 30, 2022 3:55 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Entropy of a system
- Replies: 3
- Views: 116
Entropy of a system
I know that entropy is always increasing. However, is it possible for entropy to decrease for a system?
- Sun Jan 30, 2022 3:51 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Breaking Bonds and Making Bonds
- Replies: 21
- Views: 801
Re: Breaking Bonds and Making Bonds
Breaking bonds require energy because the bonds are already in a stable place and don't want to change. You have to force them to change by putting energy into them. Forming bonds release energy because the molecule is going to a stable place so a lower potential energy. By going to a lower potentia...
- Sun Jan 30, 2022 3:47 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Phases of matter and specific heat
- Replies: 16
- Views: 730
Re: Phases of matter and specific heat
No, the specific heat changes based on state of matter and what type of compound it is.
- Sun Jan 30, 2022 3:44 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Entropy of a System
- Replies: 1
- Views: 67
Entropy of a System
How do scientists measure entropy? I don't quite get how people can measure disorder.
- Sun Jan 30, 2022 3:43 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Do all reactions have some level of equilibria?
- Replies: 5
- Views: 305
Re: Do all reactions have some level of equilibria?
Yeah you're right that all chemical reactions have a reverse reaction. It's just that some reaction's reverse reaction is so small that we can pretty much say the reaction goes to completion.
- Sun Jan 23, 2022 11:14 am
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Heat Melting or Boiling
- Replies: 11
- Views: 425
Re: Heat Melting or Boiling
The temperature remains constant during the phase change because the energy being added isn't being used to increase the kinetic energy of the particles. Instead, the energy is being used to break the bonds between the molecules and make them move more freely.
- Sun Jan 23, 2022 11:13 am
- Forum: Phase Changes & Related Calculations
- Topic: Steam vs Boiling Water
- Replies: 13
- Views: 475
Re: Steam vs Boiling Water
When you change something from one state of matter to another, you need energy. The energy being added to water when it is being evaporated doesn't increase the temperature of the water but instead is used to break the bonds of the water molecules. As a result, boiling water and steam have about the...
- Sun Jan 23, 2022 11:10 am
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: calculating protonation percentage
- Replies: 3
- Views: 213
Re: calculating protonation percentage
If it's protonation percentage, it should be concentration of conjugate divided by initial concentration of the molecule because we want to know how much of that initial concentration actually protonated.
- Sun Jan 23, 2022 11:07 am
- Forum: Calculating Work of Expansion
- Topic: Reversible Expansion vs Free Expansion
- Replies: 1
- Views: 69
Re: Reversible Expansion vs Free Expansion
I think the biggest difference is that free expansion is a type of irreversible reaction, so it is different from a reversible reaction.
- Sun Jan 23, 2022 11:04 am
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Entropy of a System
- Replies: 3
- Views: 91
Entropy of a System
How can the entropy of a system decrease?
- Sun Jan 16, 2022 3:40 pm
- Forum: Acidity & Basicity Constants and The Conjugate Seesaw
- Topic: Hwmk 2 Achieve Question 5
- Replies: 2
- Views: 160
Re: Hwmk 2 Achieve Question 5
If you're talking about concentration, then you use the concentration you found of BH+ and OH- to find the concentration of B. Since H20 is a liquid, it isn't used to find the equilibrium constant. As a result the equilibrium constant is equal to ([OH-]*[BH+])/[B]. The equilibrium constant is alread...
- Sun Jan 16, 2022 11:29 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Temperature and K Value
- Replies: 6
- Views: 288
Re: Temperature and K Value
Enthalpy values are needed to see if the reaction is endothermic or exothermic. You could also maybe tell if the reactions is two reactants combining to form one product then it's exothermic because bond formation releases energy. If the reactions is one reactant splitting apart to form two products...
- Sun Jan 16, 2022 11:24 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Approximations
- Replies: 7
- Views: 294
Re: Approximations
Yeah the rule is that if Ka is less than 10^-3 you can approximate. I think Lavelle mentioned you could do 10^-4 to be safe because some instances of 10^-3 it might not be <5%. If it's greater than 5% than you need to redo the problem without the approximation and hope it doesn't get too ugly.
- Sun Jan 16, 2022 11:18 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Calculating equilibrium and concentrations
- Replies: 6
- Views: 241
Re: Calculating equilibrium and concentrations
You generally use ice boxes when you want to find the concentration of reactants or products after equilibrium. You can usually identify the type of problem when they give you the molecules in the reaction, the Ka, and the initial concentration of at least one molecule.
- Sun Jan 16, 2022 11:11 am
- Forum: Polyprotic Acids & Bases
- Topic: polyprotic bases
- Replies: 3
- Views: 247
Re: polyprotic bases
Polyprotic bases can accept multiple protons. Usually this means they have a neg charge greater than one so that they can accept those protons. You can also check their conjugate acid and see if that is also polyphonic.
- Sat Jan 08, 2022 4:52 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: ICE tables as representations of changes (C)
- Replies: 2
- Views: 99
Re: ICE tables as representations of changes (C)
Whatever is being consumed or used to make the other molecules is -nX. Whatever is being made is +nX.
- Sat Jan 08, 2022 4:50 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Textbook Problem 5J.5 part B - Le Chatlier & Pressure
- Replies: 2
- Views: 97
Re: Textbook Problem 5J.5 part B - Le Chatlier & Pressure
The reason why the reactants are favored is because H20 is a liquid. When calculating these problems, we don't include solids and liquids. As a result, there are two moles of gas on the products side and only one mol of gas on the reactants side.
- Sat Jan 08, 2022 4:47 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: When to use Quadratic Formula
- Replies: 5
- Views: 178
Re: When to use Quadratic Formula
When you have k={products]/[reactants] and you multiply it out, if there is a x^2 then you use the quadratic formula to find the possible values of x.
- Sat Jan 08, 2022 4:44 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: ICE table: Change in concentration
- Replies: 4
- Views: 248
Re: ICE table: Change in concentration
If it's a reactant, it will be -X because it is being used up in the reaction. If it is a product, it will be +X because the molecule is being formed. However, you have to check the stoichiometric coefficients of the balanced reaction. That coefficient will determine whether it is a -1X or a -2X or ...
- Sat Jan 08, 2022 4:41 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: How Do Limiting Reagents Play Into Le Chatelier's Principle?
- Replies: 2
- Views: 255
Re: How Do Limiting Reagents Play Into Le Chatelier's Principle?
I think limiting reagents are really only a thing when the reaction goes to completion. So the reaction would have to pretty much use up all the available reactants to form products. In that case, there wouldn't be an equilibrium because equilibrium doesn't have the reaction go to completion.
- Wed Dec 01, 2021 2:58 pm
- Forum: Polyprotic Acids & Bases
- Topic: KA
- Replies: 4
- Views: 261
Re: KA
I believe because water is the solvent. It is there to help with the process and assumed to be in excess. As a result, we don't really need to know the concentration of water.
- Wed Dec 01, 2021 2:46 pm
- Forum: Conjugate Acids & Bases
- Topic: Spectator ion
- Replies: 3
- Views: 176
Re: Spectator ion
I believe so. It also deals with the fact that strong acid or base would have a very stable cation or anion. That's why it is strong because the resulting cation or anion doesn't want to react, so there barely is a reverse reaction. As a result, the resulting cation or anion is probably going to be ...
- Wed Dec 01, 2021 2:43 pm
- Forum: Lewis Acids & Bases
- Topic: Lewis Acids
- Replies: 4
- Views: 270
Re: Lewis Acids
A Lewis acid accepts an electron pair. A Bronsted acid donates a proton, usually a H+. An Arrhenius acid is just a compound that increases the H+ concentration in solution. I think we mainly just focus on Lewis and Bronsted in 14a. The Lewis definition is more general than the Bronsted definition
- Wed Dec 01, 2021 2:39 pm
- Forum: Properties & Structures of Inorganic & Organic Bases
- Topic: Strong acid and base dissociation
- Replies: 4
- Views: 389
Re: Strong acid and base dissociation
Yeah we assume that they completely dissociate in water. That's why we don't see a Ka or Koh value with them.
- Wed Dec 01, 2021 2:38 pm
- Forum: Naming
- Topic: Coordination compound vs complex
- Replies: 2
- Views: 190
Re: Coordination compound vs complex
I believe a coordinate complex is just a metal center with ligands around it. The coordinate compound is the overall neutral molecule that is made up of coordinate complexes. The complexes can have charges but the compound is neutral.
- Wed Dec 01, 2021 2:37 pm
- Forum: Conjugate Acids & Bases
- Topic: Spectator ion
- Replies: 3
- Views: 176
Re: Spectator ion
The spectator ion will usually be a component of a strong acid or base. For example in KF, K+ ends up being the spectator ion because KOH is a strong base while HF is a weak acid.
- Wed Dec 01, 2021 2:35 pm
- Forum: Properties of Electrons
- Topic: Energy Levels
- Replies: 3
- Views: 552
Energy Levels
Is the n=1 level the same distance away from the nucleus for all atoms?
- Sun Nov 28, 2021 12:12 pm
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: Acids as H+ Donors
- Replies: 9
- Views: 407
Re: Acids as H+ Donors
When an acid is called strong, it doesn't mean that the molecule itself has strong bonds. A strong acid is one that will dissociate completely or almost completely which is why they have longer, weaker bonds. A weak acid actually has the strong acids because it doesn't dissociate completely, thus ma...
- Sun Nov 28, 2021 12:03 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Determining binding sites of ligands
- Replies: 4
- Views: 195
Re: Determining binding sites of ligands
I believe the number of binding sites is equal to the number of electron pairs the molecule has to bind because each site the ligand donates one electron pair.
- Wed Nov 24, 2021 4:33 pm
- Forum: Properties & Structures of Inorganic & Organic Bases
- Topic: Relative Strength
- Replies: 7
- Views: 329
Relative Strength
Does bond length/bond strength or the stability of the anion matter more when determining the relative strengths of acids?
- Wed Nov 24, 2021 4:16 pm
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: Resonance and bond lengths
- Replies: 6
- Views: 265
Resonance and bond lengths
How is an anion stabilized by resonance?
- Sun Nov 21, 2021 11:03 pm
- Forum: Hybridization
- Topic: Nodal Planes
- Replies: 1
- Views: 136
Nodal Planes
What does it mean when a nodal plane contains the internuclear axis?
- Sun Nov 21, 2021 3:47 pm
- Forum: Hybridization
- Topic: Hybridization Clarification
- Replies: 3
- Views: 132
Re: Hybridization Clarification
Yep, hybridization is just two atoms bonding and sharing their electrons at the most stable level. This level ends up being between the 2p and 2s level so the two levels hybridize and we get the most stable hybridized orbital.
- Sun Nov 21, 2021 3:20 pm
- Forum: Bronsted Acids & Bases
- Topic: Acids & Bases
- Replies: 4
- Views: 231
Re: Acids & Bases
A weak acid typically has strong intramolecular forces while a strong acid has weak intramolecular forces. So typically acids that have longer bonds or some other weaker bonds are going to be the stronger acid. This is because the weaker the bond, the more the molecule dissociates in solution. Stron...
- Sun Nov 21, 2021 3:16 pm
- Forum: Bronsted Acids & Bases
- Topic: Acids & Bases
- Replies: 3
- Views: 126
Re: Acids & Bases
There are some ways to tell if a molecule is an acid or a base. The two main ways I know are that if there is a OH at the end of a molecule it is probably a base, because that oxygen can receive an electron pair. If there is just an H at the end of the molecule, it is probably an acid. There may be ...
- Sun Nov 21, 2021 3:13 pm
- Forum: Amphoteric Compounds
- Topic: Aqueous solutions
- Replies: 6
- Views: 340
Aqueous solutions
What exactly is the difference between an aqueous solution and a liquid?
- Tue Nov 16, 2021 1:04 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Size of atoms
- Replies: 12
- Views: 535
Size of atoms
Why is it that compounds with different size atoms still have the same shape as other compounds? For example, a molecule that has 6 hydrogen atoms is octahedral and a compound with 3 hydrogen and 3 chlorine atoms have the is also octahedral. Wouldn't the different size of the chlorine atom push the ...
- Tue Nov 16, 2021 12:45 am
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Resonance and bond lengths
- Replies: 5
- Views: 284
Resonance and bond lengths
Why exactly are the experimentally proven bond lengths of a molecule the average of the different bond lengths it has? So why doesn't the electron pair in a double bond stay there and not influence the other bond lengths in a molecule?
- Sun Nov 07, 2021 4:12 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Regarding Isoelectronic Ions
- Replies: 1
- Views: 109
Re: Regarding Isoelectronic Ions
I believe they have similar chemical properties since they share the same number of electrons.
- Sun Nov 07, 2021 4:08 pm
- Forum: Ionic & Covalent Bonds
- Topic: Hydrogen Bonding- Achieve #13
- Replies: 2
- Views: 91
Re: Hydrogen Bonding- Achieve #13
In this problem there are 8 possible hydrogen bonds because each N can form 2 because there is a pair of lone electrons and the oxygen can form 4 more because it has two pairs of lone electrons. Each lone electron on N or O can form a hydrogen bond.
- Sun Nov 07, 2021 4:03 pm
- Forum: Coordinate Covalent Bonds
- Topic: coordinate covalent bond
- Replies: 5
- Views: 363
Re: coordinate covalent bond
A coordinate covalent bond is when two atoms create a bond together by sharing two electrons. However, instead of each atom sharing one of its atoms, a coordinate covalent bond involves one atom donating two electrons in the electron sharing while the other atom doesn't have any to share. An example...
- Sun Nov 07, 2021 4:00 pm
- Forum: Dipole Moments
- Topic: Dipole-Dipole interactions
- Replies: 5
- Views: 317
Re: Dipole-Dipole interactions
Dipole-dipole movements usually are associated with non polar molecules. Polar molecules still experience them but we don't really talk about them because polar molecules have much stronger bonding such as covalent or ionic bonding. Induced dipole movement is the same as London Dispersion Forces. Th...
- Sun Nov 07, 2021 3:57 pm
- Forum: Trends in The Periodic Table
- Topic: Electronegativity
- Replies: 6
- Views: 801
Re: Electronegativity
Electronegativity is the measure of an atom's tendency to attract an electron during bonding. So as you move across a period, an electron has more electrons and gets closer to completing its octet. As a result, its electronegativity increases because it wants to attract an electron to complete the o...
- Fri Oct 29, 2021 7:54 pm
- Forum: Dipole Moments
- Topic: Dipole Moment Distance
- Replies: 2
- Views: 174
Re: Dipole Moment Distance
I think it is because the further away the two atoms are, the more prominent the charges on each atom are. There is a bigger separation or difference in charge in the atoms are more spread out.
- Fri Oct 29, 2021 7:46 pm
- Forum: Electronegativity
- Topic: trends
- Replies: 41
- Views: 1428
Re: trends
Yeah, you can think of it that atoms with a larger atomic radius will have its electrons farther away from the nucleus, so the pull from the nucleus is less. In addition, there are probably more electrons in between the valence electrons and nucleus so the electron-electron repulsion is also going a...
- Fri Oct 29, 2021 7:41 pm
- Forum: Ionic & Covalent Bonds
- Topic: electronegativity of ionic and covalent bonds
- Replies: 5
- Views: 243
Re: electronegativity of ionic and covalent bonds
If the difference is between 1.5 and 2, I think you need to conduct experiments to see if the molecule has more covalent or ionic bonds.
- Fri Oct 29, 2021 7:34 pm
- Forum: Lewis Structures
- Topic: How to know between which atoms to make a double bond
- Replies: 3
- Views: 106
Re: How to know between which atoms to make a double bond
I think when making Lewis Dot Diagrams, you prioritize giving electron pairs to the atoms with smaller ionization energies. So we would give Nitrogen its electron pairs first and then any excess electrons that need to be made into double bonds would be with atoms with higher ionization energy like t...
- Fri Oct 29, 2021 7:25 pm
- Forum: Resonance Structures
- Topic: Bond Lengths
- Replies: 3
- Views: 134
Re: Bond Lengths
I think they use x-ray spectroscopy to find the diffraction patterns. The patterns are then used to find exactly how long the bond lengths are.
- Fri Oct 22, 2021 10:36 am
- Forum: DeBroglie Equation
- Topic: Achieve #15
- Replies: 3
- Views: 226
Re: Achieve #15
I used De Broglie's equation to find the momentum of the electron. Then I found the velocity of the electron since we already know the mass of the electron. Then kinetic energy is 0.5mv^2. Then convert that answer from joules to eV.
- Fri Oct 22, 2021 10:32 am
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: 3d and 4s subshell
- Replies: 17
- Views: 940
Re: 3d and 4s subshell
Yeah the 4s orbital will be filled before the 3d orbital. A helpful thing to look at for this is the periodic table. If you read it from left to right, it will tell you the order that the orbitals get filled above. For example, in the 4th row, the s comes before the d so that tells us that the 4s is...
- Fri Oct 22, 2021 10:28 am
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: order s, p, d, f... why?
- Replies: 3
- Views: 199
Re: order s, p, d, f... why?
I believe this is partly due to the shape of the orbitals and the order they come in. S orbitals are spherical in nature, while the other orbitals have specific shapes which might make them higher in energy. In addition, there is electron to electron repulsion. The p orbital comes after the s orbita...
- Fri Oct 22, 2021 10:24 am
- Forum: Balancing Chemical Reactions
- Topic: N vs N2
- Replies: 20
- Views: 6093
Re: N vs N2
Since it is talking about a nitrogen atmosphere, I think it means that the nitrogen is just in the air. Nitrogen as a gas only appears as N2 and not N. So in this situation it would be N2. As long as it talks about nitrogen being a gas or in the atmosphere, it should be N2. The problem will probably...
- Fri Oct 22, 2021 10:22 am
- Forum: Properties of Light
- Topic: Molecule Emission Spectrum
- Replies: 4
- Views: 200
Re: Molecule Emission Spectrum
It is the same for molecules and compounds.
- Fri Oct 15, 2021 4:57 pm
- Forum: Trends in The Periodic Table
- Topic: Electron Shielding
- Replies: 6
- Views: 221
Re: Electron Shielding
How does electron shielding affect the properties of the element or atom?
- Fri Oct 15, 2021 4:50 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Aufbau's Principle and electron diagrams
- Replies: 2
- Views: 101
Re: Aufbau's Principle and electron diagrams
When do you know if the next level s series is lower in energy than the current level's d series?
- Fri Oct 15, 2021 4:46 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Aufbau Principle
- Replies: 3
- Views: 134
Re: Aufbau Principle
It is 3d^5 4s^1 instead of 3d^4 4s^2 because it is more stable for the electrons to fill out the 3d series instead of fill out 4s and partially fill out 3d.
- Fri Oct 15, 2021 4:44 pm
- Forum: Properties of Electrons
- Topic: Wave properties
- Replies: 4
- Views: 229
Re: Wave properties
Why do some things like light travel in a wavelike shape instead of a different shape?
- Fri Oct 15, 2021 4:40 pm
- Forum: *Shrodinger Equation
- Topic: Topic 1D.1 and 1D.2
- Replies: 2
- Views: 144
Re: Topic 1D.1 and 1D.2
I'm pretty sure any equation we need to know will be on the equation sheet Dr. Lavelle provided for us. If it's not there, we probably don't need to know that equation.
- Fri Oct 15, 2021 4:36 pm
- Forum: Properties of Electrons
- Topic: Quantum Description of Atoms
- Replies: 6
- Views: 291
Re: Quantum Description of Atoms
Electrons with stationary energy can only exist at discrete energy levels. Since electrons can only stay in these level, only certain wavelengths are allowed inside an atom. Do the certain wavelengths that are allowed inside an atom vary between each individual atom? Or are the same certain wavelen...
- Fri Oct 15, 2021 4:31 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Determining Ground State of Elements with Larger Atomic Numbers
- Replies: 1
- Views: 104
Re: Determining Ground State of Elements with Larger Atomic Numbers
A good way to know what orbital an element is in is to see what block the element is in. Check to see to see if it is in the s, p, d, or f block. Once you know which block, you have to figure out what level that s, p, d, or f is in. To do this, check which row of the periodic table the element is in...
- Sat Oct 09, 2021 4:42 pm
- Forum: DeBroglie Equation
- Topic: Wavelike Properties
- Replies: 8
- Views: 286
Re: Wavelike Properties
Are wavelengths smaller than 10^15 undetectable to us currently with our technology or is this as small as theoretically possible that humans can detect wavelengths?
- Sat Oct 09, 2021 4:33 pm
- Forum: Properties of Electrons
- Topic: Quantum Description of Atoms
- Replies: 6
- Views: 291
Re: Quantum Description of Atoms
Electrons with stationary energy can only exist at discrete energy levels. Since electrons can only stay in these level, only certain wavelengths are allowed inside an atom.
- Sat Oct 09, 2021 4:21 pm
- Forum: DeBroglie Equation
- Topic: If the velocity was extremely small
- Replies: 5
- Views: 262
Re: If the velocity was extremely small
I think it is possible for the waves of larger masses to be detected, maybe not from the technology we currently have, with a smaller velocity. The only problem I could see with this is that once you have a large enough mass, the wavelength it produces is so tiny that I doubt it could ever be detect...
- Sat Oct 09, 2021 3:51 pm
- Forum: Properties of Electrons
- Topic: Electron diffraction
- Replies: 3
- Views: 118
Re: Electron diffraction
All matter has wavelike properties. It's just that these wavelike properties are only noticeable for moving objects with extremely small mass such as an electron. Since the electron is small enough to display wavelike properties, it has diffraction patterns just like waves.
- Sat Oct 09, 2021 3:35 pm
- Forum: General Science Questions
- Topic: Rusty on High School Chem [ENDORSED]
- Replies: 347
- Views: 504102
Re: Rusty on High School Chem [ENDORSED]
Does anyone know how to tell if a molecule is an acid or a base just by looking at its molecular formula?
- Thu Sep 30, 2021 3:19 pm
- Forum: Balancing Chemical Reactions
- Topic: Actual vs. theoretical yield [ENDORSED]
- Replies: 42
- Views: 3185
Re: Actual vs. theoretical yield [ENDORSED]
What are some of the ways/reasons the actual yield might end up being smaller than the theoretical yield? The main ways why actual yield might end up being smaller is that there are side reactions that happen along with the main reaction because it is nearly impossible to create a perfect space in ...