Search found 117 matches
- Fri Mar 13, 2020 12:12 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Kinetics vs thermodynamics
- Replies: 3
- Views: 353
Re: Kinetics vs thermodynamics
Kinetics describes the pathway of reactions, with an emphasis on the activation energy that signifies the energy difference between the free energy of reactants and the transition state. Kinetic analysis is about the speed or rate of reaction, using experimental techniques to observe reactant & ...
- Fri Mar 13, 2020 11:42 am
- Forum: First Order Reactions
- Topic: Pseudo-First Order Reaction
- Replies: 4
- Views: 373
Re: Pseudo-First Order Reaction
In addition, if there are more than two reactants, you could make the initial concentration of all reactants except one very large so that as the reaction proceeds, the concentration of only one reactant actually changes.
- Fri Mar 13, 2020 11:24 am
- Forum: Zero Order Reactions
- Topic: Zeroeth, First, Second meaning
- Replies: 6
- Views: 634
Re: Zeroeth, First, Second meaning
The units of k:
first-order: s^-1, second-order: (s^-1)*(mol^-1)*(L), zero-order: (mol)(L^-1)*(s^-1);
first-order: s^-1, second-order: (s^-1)*(mol^-1)*(L), zero-order: (mol)(L^-1)*(s^-1);
- Fri Mar 13, 2020 10:36 am
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Endo VS Exo
- Replies: 4
- Views: 433
Re: Endo VS Exo
I think that whether a reaction is endothermic or exothermic depends only on the final Gibbs free energy and initial Gibbs free energy. If the reactants have higher free energy, then the reaction is exothermic; if the products have higher free energy, then the reaction is endothermic.
- Fri Mar 13, 2020 9:40 am
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Activated Complex Model
- Replies: 2
- Views: 243
Re: Activated Complex Model
Just to add, the activated complex is also named transition state. Also, at a higher temperature, there is a higher probability that a portion of the particles has gained enough energy needed to take part in the reaction; however, higher temperature makes faster reaction but temperature doesn't itse...
- Sat Mar 07, 2020 12:54 am
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Reaction Profiles
- Replies: 3
- Views: 670
Re: Reaction Profiles
Exactly, and this relates back to the fact that the slowest elementary step is the rate determining step and it determines the rate of the overall reaction. In other words, the overall reaction rate is not determined by any faster step. Therefore, the peak in the reaction profile just implies the ac...
- Sat Mar 07, 2020 12:49 am
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Molecularity
- Replies: 4
- Views: 413
Re: Molecularity
Yes, it's termolecular for the elementary step. In addition, I think it's worth notifying that molecularity means the number of species in an elementary step (rather than the overall reaction), which is followed by each elementary step's rate law directly.
- Sat Mar 07, 2020 12:41 am
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: pseudo rate law
- Replies: 2
- Views: 267
Re: pseudo rate law
Many reactions actually have many reactants, but determining the order of each together is very hard and complex, so we make the concentration of one reactant very small while the others very large (concentrations essentially constant) so that the reaction rate depends only on the small concentratio...
- Sat Mar 07, 2020 12:20 am
- Forum: General Rate Laws
- Topic: Lecture Question
- Replies: 3
- Views: 349
Re: Lecture Question
Exactly. So when there is no product, the forward reaction rate would not be disrupted/counteract by reverse reaction, because no product is present and thus no product can return to reactant.
- Fri Mar 06, 2020 11:13 pm
- Forum: General Rate Laws
- Topic: Differential Rate Law
- Replies: 3
- Views: 303
Re: Differential Rate Law
And I think that differential rate law is actually the source of integrated rate law (obtained by integrating the differential rate law on both sides). Also, differential rate law could give the plot of rate versus time.
- Fri Mar 06, 2020 9:38 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Study Advice
- Replies: 73
- Views: 7126
Re: Study Advice
I generally attend TA's review sessions talking about outlines that contain concepts not sound familiar to me to get a big picture of what I need to know. And Lyndon's review session is outstandingly helpful, in which he would help us go through potential tricky questions. Professor Lavelle's lectur...
- Fri Feb 28, 2020 10:26 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Anode vs Cathode
- Replies: 15
- Views: 875
Re: Anode vs Cathode
how do you determine it based on the cell potentials? especially if the values are similar? I believe that we should then check the formula sheet or appendix, and choose the substance with more positive reduction potential as the cathode. I think there should always be a difference that is not too ...
- Fri Feb 28, 2020 9:45 pm
- Forum: General Rate Laws
- Topic: Overall reaction order
- Replies: 4
- Views: 342
Re: Overall reaction order
We set rate 1/rate 2 equal to 2 in the example because the ratio of the initial rates between experiment 1 and experiment 2 is 2 and the units cancel out. And the initial rates of [NH4+] doesn't change, so, after applying equation: rate = k[NH4+]^n*[NO2-]^m, we are left with the ratio between initia...
- Fri Feb 28, 2020 9:07 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Electrolyte
- Replies: 4
- Views: 298
Re: Electrolyte
In addition, to be an electrolyte, a substance doesn't have to completely dissolve in a solvent. Strong electrolytes would completely dissolve, whereas weak electrolytes would only partially dissolve.
- Fri Feb 28, 2020 8:45 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Calculating Standard Potentials
- Replies: 4
- Views: 368
Re: Calculating Standard Potentials
And remember that because standard potential energy is an intensive property, we don't need to multiply by coefficients.
- Fri Feb 28, 2020 8:32 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Metals in galvanic cell
- Replies: 1
- Views: 220
Re: Metals in galvanic cell
I think that to decide which metal to be the cathode, we need to look into the standard reduction potential table, which is provided in the textbook's section that talks about standard reduction potential and its appendix, and will also be provided during tests and exams. The metal with higher posit...
- Fri Feb 28, 2020 8:22 pm
- Forum: Balancing Redox Reactions
- Topic: How to tell if its being reduced or oxidized
- Replies: 15
- Views: 2142
Re: How to tell if its being reduced or oxidized
When the oxidation number of an element in a reactant increases when it becomes a product, it is oxidized; when the oxidation number of an element in a reactant decreases when it becomes a product, it is reduced. The previous sentence holds because being reduced means gaining electrons while being o...
- Sun Feb 23, 2020 10:35 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: STP
- Replies: 13
- Views: 767
Re: STP
Exactly. And I believe that we don't need to remember this, because the meaning of STP would be given and clearly explained when it appears on the test, just like what happened in the midterm.
- Sun Feb 23, 2020 10:29 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Nernst Equation and Le Chatelier's Principle
- Replies: 3
- Views: 559
Re: Nernst Equation and Le Chatelier's Principle
I think that Nernst Equation and Le Chaterlier's Principle support each other. According to Le Chatelier's Principle, the cell potential should change in corresponding ways when concentrations change in specific ways. Supportively, by manipulating variables in known equation, the Nernst Equation is ...
- Sun Feb 23, 2020 10:24 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: salt bridge
- Replies: 9
- Views: 673
Re: salt bridge
It allows redox reaction to take place continuously in a galvanic cell. Without the salt bridge, as electrons go from anode to cathode, the redox reaction would stop due to charge build up.
- Sun Feb 23, 2020 10:16 pm
- Forum: Balancing Redox Reactions
- Topic: Reduction?
- Replies: 13
- Views: 688
Re: Reduction?
Oxidation: loss of electrons, increase in oxidation number;
Reduction: gain of electrons, decrease in oxidation number;
Reduction: gain of electrons, decrease in oxidation number;
- Sun Feb 23, 2020 10:14 pm
- Forum: Balancing Redox Reactions
- Topic: spontaneous
- Replies: 15
- Views: 857
Re: spontaneous
What exactly is the standard reduction potential and why does it have to be positive for the reaction to be spontaneous? The standard reduction potential is tabulated for compounds with respect to standard hydrogen electrode. It is a measure of the electron-pulling power of the reaction occurring a...
- Sun Feb 23, 2020 10:03 pm
- Forum: Balancing Redox Reactions
- Topic: 6K.1
- Replies: 6
- Views: 349
Re: 6K.1
The oxidation number of oxygen and hydrogen generally remain the same, but mostly not in the situation when they have an oxidation number of 0. When balancing the half reactions, you could add water to balance oxygen. Then, if the reaction takes place in acidic solution, you could add H+ to balance ...
- Sun Feb 16, 2020 10:42 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: External force
- Replies: 6
- Views: 453
Re: External force
Just to add something. In free expansion, there is no external force present, and the surrounding is actually vacuum, and the process is irreversible because the external pressure is constant and equals 0. Moreover, in a reversible pathway, the external pressure could actually either infinitesimally...
- Sun Feb 16, 2020 10:33 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: 3/2R & 5/2R
- Replies: 9
- Views: 749
Re: 3/2R & 5/2R
I think it would be under the situation that there is an ideal gas that is monoatomic, linear, or non-linear, and molar heat capacity is not given.
- Sun Feb 16, 2020 9:16 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: S = 0
- Replies: 21
- Views: 1191
Re: S = 0
S just means entropy, rather than change in entropy that should be denoted as ΔS. Entropy is almost never 0 (the entropies of all perfect crystals approach zero as the absolute temperature approaches zero; "perfect crystal" refers to a substance in which all the atoms are in a perfectly or...
- Sun Feb 16, 2020 7:14 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Example 4I.3
- Replies: 3
- Views: 343
Re: Example 4I.3
I agree with the peer above's explanation. In addition, the initial & final states are the same because the process is isothermal, so, according to ΔS = q(rev)/T, ΔS should be the same.
- Sun Feb 16, 2020 7:02 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Pizza Rolls #5
- Replies: 5
- Views: 397
Re: Pizza Rolls #5
For Part A, you have to add up three different delta S values to find the total change of entropy in the system. This includes deltaS for H2 container expansion, deltaS of Krypton gas for container expansion, and deltaS based on temperature change. Since entropy is a state function, this allows us ...
- Sun Feb 16, 2020 6:55 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Units in Entropy Equation for Volume
- Replies: 5
- Views: 349
Re: Units in Entropy Equation for Volume
I think that the substitution is correct but unnecessary, because the substitution needs even more information. The unit of entropy is always J/k, and you can remember this by the second law of thermodynamics, that is delta S = q/T, in which q has a unit of J and T has a unit of K.
- Sat Feb 08, 2020 9:48 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Standard Free Energy of Formation Units
- Replies: 2
- Views: 503
Re: Standard Free Energy of Formation Units
I think that the unit of deltaS standard of reaction is J/K, because delta S = q/T; the unit of deltaH standard of reaction is kJ/mol. Since G = H -TS, G should have the same unit as H, so I think that the unit of standard free energy of formation is also kJ/mol.
- Sat Feb 08, 2020 12:44 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Units for heat of reaction
- Replies: 9
- Views: 294
Re: Units for heat of reaction
I think that the unit should just be kJ/mol, because I think that adding or removing something from a unit would make things weird and even the unit invalid. If you want specify that you are calculating enthalpy of formation of a particular substance, you could specify that at the beginning of your ...
- Sat Feb 08, 2020 12:40 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Delta H and qp
- Replies: 8
- Views: 204
Re: Delta H and qp
I think that delta H = qp, because "qp" means heat transferred under constant pressure. And by definition, change in enthalpy equals the heat absorbed or released at constant pressure.
- Sat Feb 08, 2020 12:30 am
- Forum: Phase Changes & Related Calculations
- Topic: Environment
- Replies: 4
- Views: 235
Re: Environment
Also, by global warming, the ecological environment would be significantly changed, leading to the extinguish of many species because they cannot adapt the new ecological environment anymore. The destruction on the ecosystem might be so severe that even ecosystems that cover large areas and sustain ...
- Sat Feb 08, 2020 12:23 am
- Forum: Phase Changes & Related Calculations
- Topic: 4B.5
- Replies: 7
- Views: 484
Re: 4B.5
Yes, and remember to pick ideal gas constant with correct units or convert 750 torr to 750/760 atm; also remember to be consistent with either J or kJ when adding energies.
- Sat Feb 08, 2020 12:03 am
- Forum: Phase Changes & Related Calculations
- Topic: phase changes, temperature constant?
- Replies: 11
- Views: 634
Re: phase changes, temperature constant?
The change of a substance from a phase of a lower energy to a phase of a higher energy requires heat to break intermolecular interactions between molecules, thereby making the substance have higher potential energy between molecules (usually, the volume of a substance: solid state < liquid state < g...
- Sat Feb 01, 2020 12:11 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: biological examples
- Replies: 7
- Views: 314
Re: biological examples
In addition, ATP is less stable than ADP, because ATP has an additional phosphate group that is connected to the other part of the ATP by a chemical bond with very high energy.
- Fri Jan 31, 2020 10:40 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Bomb Calorimeter
- Replies: 5
- Views: 2449
Re: Bomb Calorimeter
Yes. In addition, bomb calorimeter is an isolated system, so neither the matter nor the energy could be exchanged between the system (inside of bomb calorimeter) and the surrounding (outside of the bomb calorimeter). Therefore, the internal energy of bomb calorimeter is constant.
- Fri Jan 31, 2020 10:29 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: qp=deltaH
- Replies: 2
- Views: 114
Re: qp=deltaH
In lecture, the definition of enthalpy is given: the amount of heat released or absorbed at a constant pressure.
- Fri Jan 31, 2020 10:07 pm
- Forum: Phase Changes & Related Calculations
- Topic: Cv and Cp
- Replies: 9
- Views: 451
Re: Cv and Cp
The change in enthalpy is equal to heat released or absorbed only when the reaction happens at a constant pressure. So the value of q(heat) calculated by Cp is equal to change in enthalpy, but not by Cv.
- Fri Jan 31, 2020 9:46 pm
- Forum: Phase Changes & Related Calculations
- Topic: Enthalpy of sublimation?
- Replies: 8
- Views: 1485
Re: Enthalpy of sublimation?
Vaporization, melting (fusion), and sublimation are all exothermic reactions, so the change of enthralpy of each of these three reactions has a positive value. delta H(vap) = H(vapor) - H(liquid); delta H(fus) = H(liquid) - H(solid); delta H(sub) = H(vapor) - H(solid); So delta H(sub) = delta H(fus)...
- Fri Jan 31, 2020 9:34 pm
- Forum: Phase Changes & Related Calculations
- Topic: Homework 4A.9
- Replies: 3
- Views: 168
Re: Homework 4A.9
I think that your reasoning is exactly correct. And I believe that it doesn't matter which side you would like to put the negative sign on. The only thing matter is that one substance is losing heat whereas the other one is gaining heat, so if we set the change in heat of one substance negative, the...
- Sat Jan 25, 2020 8:54 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Bond Enthalpies and gas phases
- Replies: 2
- Views: 159
Re: Bond Enthalpies and gas phases
Is it because the bond enthalpies are measured in the gas phase? We could actually still make good use of bond enthalpies in gas phase by adding enthalpy of vaporization when calculating bond enthalpies in liquid phase.
- Sat Jan 25, 2020 8:46 pm
- Forum: Phase Changes & Related Calculations
- Topic: Bond Enthalpies
- Replies: 5
- Views: 127
Re: Bond Enthalpies
For diatomic molecules, they are accurate, because they are directly measured for those molecules. For all others are averages from many different molecules containing the bond, and thus inaccurate.
- Sat Jan 25, 2020 8:44 pm
- Forum: Phase Changes & Related Calculations
- Topic: Phase changes
- Replies: 7
- Views: 227
Re: Phase changes
Temperature remain constant during a phase change, because the increase in internal energy would be used to break intermolecular forces and to increase the distance between molecules. For example, the density of gas is less than that of liquid, which is less than that of solid.
- Sat Jan 25, 2020 8:39 pm
- Forum: Phase Changes & Related Calculations
- Topic: Constant pressure and constant volume
- Replies: 3
- Views: 182
Re: Constant pressure and constant volume
Pressure and volume are two totally different measurements, because they measure different parameters of substances and have different units. However, change in pressure, under many circumstances, could imply change in volume, and vice versa, according to the ideal gas law, PV = nRT.
- Sat Jan 25, 2020 8:22 pm
- Forum: Phase Changes & Related Calculations
- Topic: Celsius and Kelvin
- Replies: 11
- Views: 458
Re: Celsius and Kelvin
Celsius is always 273 units larger than Kelvin. However, they luckily have the same length of each unit. Consequently, since 0 Kelvin is defined by the temperature of absolute zero but 0 Celsius is defined by the temperature of ice-water mixture, they would never have the same numerical value for an...
- Sat Jan 25, 2020 8:10 pm
- Forum: Phase Changes & Related Calculations
- Topic: Standard State
- Replies: 3
- Views: 85
Re: Standard State
The standard state for a solution is actually 1M at 1 atm. And the reason why it's 1 atm may be that the atmospheric pressure at sea level is 1 atm, so it's convenient to define 1 atm as standard state for gases (and liquids).
- Sat Jan 18, 2020 10:42 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Le Chatliers Principle In relation to pressure
- Replies: 6
- Views: 280
Re: Le Chatliers Principle In relation to pressure
According to the ideal gas law, PV = nRT, P = nRT/V = concentration (=n/V) * RT. So [partial pressure = concentration * RT].
- Sat Jan 18, 2020 10:39 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: 5.61a
- Replies: 3
- Views: 168
Re: 5.61a
I believe that increasing the partial pressure of O2 is achieved by means of adding more O2 gas particles. And remember that P (partial pressure) = concentration * R * T (temperature).
- Sat Jan 18, 2020 10:32 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: 5J.1 a)
- Replies: 5
- Views: 136
Re: 5J.1 a)
If the partial pressure of CO2 is increased, then the concentration of the product is increased. According to Le Chatelier's principle, the reaction would then shift to the left and favor the reactants. As a result, H2 would be consumed along with CO2 to form more reactants, thereby leading to a dec...
- Sat Jan 18, 2020 10:18 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: 5 %
- Replies: 4
- Views: 258
Re: 5 %
Exactly! And also if the percentage ionization of a substance is less than 5%, then the percent of the substance that is ionized is relatively small compared to the initial concentration of the substance, so we could disregard the decrease in the amount of the substance when mentioning the substance...
- Sat Jan 18, 2020 9:39 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Identifying Acids, Bases, and Salts in a Rxn
- Replies: 4
- Views: 252
Re: Identifying Acids, Bases, and Salts in a Rxn
If Ka or Kb of a substance is given, then it's a weak acid/base. The conjugate base of a weak acid is basic, whereas of a strong acid is not, the conjugate acid of a weak base is acidic, whereas of a strong base is not.
- Fri Jan 17, 2020 11:40 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Quick way
- Replies: 7
- Views: 371
Re: Quick way
The example Dr. Lavelle gave in class was if you added Helium to a reaction occurring within a sealed container. While the pressure of the reaction is increasing, it has no effect on the equilibrium because adding gas doesn't have any effect on the actual concentration of either the products or rea...
- Sat Jan 11, 2020 11:18 pm
- Forum: Ideal Gases
- Topic: Gas Laws
- Replies: 6
- Views: 186
Re: Gas Laws
I think that the other gas laws could actually all be easily derived from the ideal gas law, PV = nRT.
- Sat Jan 11, 2020 10:54 pm
- Forum: Ideal Gases
- Topic: Units for K
- Replies: 29
- Views: 1269
Re: Units for K
Actually, the equilibrium constant K has unit, but to include the unit would make the calculation much more complex (and the numerical value of K would be a little bit different--so little that it would be much more convenient to not include a unit for K. To have K have no unit, we would write molar...
- Sat Jan 11, 2020 10:43 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 5G.9
- Replies: 3
- Views: 119
Re: 5G.9
P(O2)/P(O3) isn't the equilibrium constant of this reaction, but P(O2)^3/P(O3)^2 is. Remember that a^2/b^3 = 5 doesn't mean that a/b = 5. Because the equilibrium concentration is different in these two cases, only equilibrium constant would be the same when comparing these two conditions.
- Sat Jan 11, 2020 10:28 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Meaning of K [ENDORSED]
- Replies: 4
- Views: 213
Re: Meaning of K [ENDORSED]
I don't think that the equilibrium constant K is the rate at which these reactions occur. K is the ratio of products and reactants at equilibrium. We could speed up the rate by adding reactants, and in other ways according to Le Chatelier's principle.
- Sat Jan 11, 2020 10:14 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Catalysts
- Replies: 7
- Views: 192
Re: Catalysts
All the function and examples of catalysts are exact and useful. In addition, catalysts decreases activation energy by stabilizing the transition state (having lower energy). In biological systems, without catalysts, mostly enzymes, many reactions important for metabolism and maintaining homeostasis...
- Sat Jan 11, 2020 10:02 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Different K's
- Replies: 5
- Views: 304
Re: Different K's
I think that when the reactants and products, except pure liquids and solids, are all gases, we should use Kp, whereas using Kc is also okay. But when they are not. we can only use Kc.
- Fri Dec 06, 2019 2:29 pm
- Forum: Air Pollution & Acid Rain
- Topic: Acid Rain
- Replies: 6
- Views: 723
Re: Acid Rain
Sulfuric dioxide comes from burning petroleum products, coal, etc., and reacts with water vapor to form acidic rain. Clean coal contains less percentage of sulfur, whereas dirty coal contains more percentage of sulfur.
- Fri Dec 06, 2019 2:17 pm
- Forum: Octet Exceptions
- Topic: Octet exception
- Replies: 14
- Views: 1287
Re: Octet exception
Michelle Song 3I wrote:Boron and Aluminum are also exceptions in that they can form only 3 bonds.
Exactly. But to be more specific, without any additional lone pairs, the number of valence electrons around boron and aluminum is then only 6, not reaching octet.
- Fri Dec 06, 2019 2:08 pm
- Forum: Bond Lengths & Energies
- Topic: Hydrogen Bonding
- Replies: 13
- Views: 1112
Re: Hydrogen Bonding
Hydrogen bonding occurs between a hydrogen atom that is bonded to N/O/F and a N/O/F atom with at least one lone pair.
- Fri Dec 06, 2019 10:06 am
- Forum: Conjugate Acids & Bases
- Topic: Conjugate Base
- Replies: 4
- Views: 334
Re: Conjugate Base
nickianel_4b wrote:^^I know that it becomes CH3COO- just from practice, but can someone remind me again why it donates the H+ at the end and not one of the H+ ions attached to the C?
-COOH, or carboxyl group, is the organic acidic group, so when losing a proton, the proton would come from the carboxyl group.
- Fri Dec 06, 2019 9:34 am
- Forum: Amphoteric Compounds
- Topic: Amphiprotic vs Amphoteric
- Replies: 5
- Views: 596
Re: Amphiprotic vs Amphoteric
But doesn't losing or gaining of electrons (amphiprotic) mean acting as an acid or base (amphoteric)?
- Sun Dec 01, 2019 4:40 pm
- Forum: Properties & Structures of Inorganic & Organic Bases
- Topic: Are noble gases considered bases?
- Replies: 9
- Views: 2205
Re: Are noble gases considered bases?
No, because they are unreactive, therefore unwilling to accept or donate electrons because they have already reached their octet. By the way, molecules don't have to be classified as either acid or base. And also remember that there are amphoteric molecules that could act as either acid or base depe...
- Sun Dec 01, 2019 4:11 pm
- Forum: Polyprotic Acids & Bases
- Topic: H2SO4 vs H2CO3
- Replies: 4
- Views: 4524
Re: H2SO4 vs H2CO3
H2SO4 is more readily to donate H atoms than H2CO3 because S is more electronegative by having more protons (in 4th period, while C is in 3rd period) and thus have more electron density withdrawing power.
- Sun Dec 01, 2019 3:23 pm
- Forum: Polyprotic Acids & Bases
- Topic: Polyprotic Question!
- Replies: 12
- Views: 1784
Re: Polyprotic Question!
If an acid is polyprotic is it stronger? A polyprotic acid isn't necessarily stronger than a monoprotic acid. Whether an acid is strong depends on the equilibrium constant for acids, Ka = ([A-][H+])/[AH]. Having more number of H atoms in a molecule doesn't necessarily mean that the molecule is more...
- Sun Dec 01, 2019 3:06 pm
- Forum: Polyprotic Acids & Bases
- Topic: How can you tell
- Replies: 18
- Views: 1028
Re: How can you tell
If there's more than one H in front of the anion, let's say, H2SO4, or H3PO4 It'll be polyprotic because there is more than 1 hydrogen in front. Exactly! We should count the number of H atoms in the front of the anion, rather than count all H atoms, because not all H atoms would play a role in dona...
- Sun Dec 01, 2019 3:02 pm
- Forum: Conjugate Acids & Bases
- Topic: Water as an Acid/Base
- Replies: 20
- Views: 1568
Re: Water as an Acid/Base
Yes, and essentially, this rule works because it means the same thing as determining water acts as an acid or a base according to whether water donates/accepts protons (Bronsted's definition).
- Sun Dec 01, 2019 2:28 pm
- Forum: Amphoteric Compounds
- Topic: Identifying Them?
- Replies: 12
- Views: 896
Re: Identifying Them?
An amphoteric compound can be identified as both a acid and a base in different reactions.
- Sun Nov 24, 2019 10:04 am
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Oxidation State
- Replies: 4
- Views: 342
Re: Oxidation State
Besides all the important, useful rules and hints mentioned by previous peers, when trying to decide the oxidation state of TM, we could solve the problem by knowing the charge on the molecule overall and figuring out oxidation states of all atoms other than the TM.
- Sun Nov 24, 2019 9:54 am
- Forum: Lewis Acids & Bases
- Topic: Hydronium ion
- Replies: 5
- Views: 304
Re: Hydronium ion
I think that in the cases that acids dissolve in water, the actual reason why acids lower the pH is that they easily release a hydrogen atom that is then taken by water to form a hydronium ion, lowering the pH of the solution.
- Sun Nov 24, 2019 9:40 am
- Forum: Biological Examples
- Topic: myoglobin and hemoglobin
- Replies: 3
- Views: 210
Re: myoglobin and hemoglobin
Exactly, and also remember that whether the oxygen is absorbed or de-absorbed depends on the local partial pressure of oxygen. In addition, the reason why transition metals locate as the central atom is that TM 1) have many oxidation states --> good for electron transfer 2) often bound to a cage-lik...
- Sun Nov 24, 2019 9:33 am
- Forum: Biological Examples
- Topic: Heme Complex
- Replies: 5
- Views: 369
Re: Heme Complex
Hi, Could someone reiterate the significance of Fe as the central atom in the Heme complex, and how that relates to its function? Thank you! Hi there, According to professor Lavelle's lecture and his slides: The Fe atom plays a role in binding one oxygen molecule, and therefore could perform the fu...
- Sat Nov 23, 2019 1:21 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: Best Approach to Find IMFs
- Replies: 11
- Views: 825
Re: Best Approach to Find IMFs
Personally, I would prefer to draw the Lewis structure first to see whether the molecule is ionic (ionic-ionic, ionic-dipole) -->whether polar (ionic-dipole, dipole dipole, dipole-induced dipole), or nonpolar (dipole-induced dipole, induced dipole-induced dipole), with the help of either net dipole ...
- Sat Nov 23, 2019 12:40 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: Hydrogen Bonding Atoms
- Replies: 6
- Views: 325
Re: Hydrogen Bonding Atoms
I think that hydrogen bonding could form between a hydrogen atom bound to an N/O/F atom and an N/O/F atom with lone pair electrons.
- Fri Nov 15, 2019 10:59 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Molecular Geometry vs Electron Geometry
- Replies: 2
- Views: 144
Re: Molecular Geometry vs Electron Geometry
The electron geometry considers all regions of electron density, regardless of bonding pairs electrons or lone pairs electrons; the molecular shape considers only bonding regions. Consequently, when the electron geometry is the same, depending on the number of lone pairs electrons, the molecular sha...
- Thu Nov 14, 2019 11:52 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: 4.3 Draw the structures and name the shapes of the following molecules: (a) HCN; (b) CH2F2.
- Replies: 4
- Views: 1599
Re: 4.3 Draw the structures and name the shapes of the following molecules: (a) HCN; (b) CH2F2.
How do you know that the two bonds with hydrogen are next to each other, versus across the molecule from each other? I think that it does't matter, and there are 2 reasons. 1) they are all single bonds, so arranging the hydrogen atoms next to each other or across from each other doesn't make differ...
- Wed Nov 13, 2019 3:30 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Shape
- Replies: 8
- Views: 476
Re: Shape
Yes, because we are only trying to name the shape of molecules.
- Wed Nov 13, 2019 3:24 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: molecular shape
- Replies: 8
- Views: 537
Re: molecular shape
There are several general rules to help determine, and thus memorization is required. To determine the molecular shape, both lone pair electrons and bonding pair electrons need to be considered; professor Lavelle hasn't discussed this in lecture yet. However, to name the shape of the molecule, only ...
- Wed Nov 13, 2019 3:16 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Methane VSEPR
- Replies: 7
- Views: 419
Re: Methane VSEPR
In order for the amount of repulsion to be minimized, the distance between bonding pair should be maximized, that is, keeping the bonding regions of electrons as far apart from each other as possible. Unlike Lewis structure that is 2-dimensional, VSEPR model is actually 3-D, allowing bonding regions...
- Tue Nov 12, 2019 12:36 am
- Forum: DeBroglie Equation
- Topic: De Broglie Wavelength
- Replies: 23
- Views: 3441
Re: De Broglie Wavelength
De Broglie's wavelength equation applies to any moving particle with momentum so that the particle has wavelike properties, such as electrons, neutrons, and protons. However, only when the particle has extremely small mass would the wavelike property be noticeable.
- Tue Nov 12, 2019 12:23 am
- Forum: Quantum Numbers and The H-Atom
- Topic: Rydberg equation
- Replies: 9
- Views: 551
Re: Rydberg equation
We are actually totally allowed to use the Rydberg equation, whereas using the (final - initial) form of the the Rydberg equation could give us a better understanding of the concept and therefore what we are doing. And I believe that using the form of equation recommended by professor Lavelle elimin...
- Tue Nov 12, 2019 12:15 am
- Forum: Quantum Numbers and The H-Atom
- Topic: Orbital angular momentum
- Replies: 4
- Views: 418
Re: Orbital angular momentum
The angular momentum quantum number (l) describes the shape of the atomic orbital.
Allowed values: l = 0 (s-orbital), 1(p-orbital), 2(d-orbital), ..., n-1; each l is called a subshell.
Allowed values: l = 0 (s-orbital), 1(p-orbital), 2(d-orbital), ..., n-1; each l is called a subshell.
- Mon Nov 11, 2019 11:11 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: central atoms
- Replies: 7
- Views: 376
Re: central atoms
According to the information I collected online, the first ionization energy of oxygen is 1313.94 kJ/mol and that of chlorine is 1251.19 kJ/mol. So the ionization energy of Cl is lower than that of oxygen, making Cl reasonable to be put as the central atom.
- Mon Nov 11, 2019 10:58 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Difference Between Lewis Structure and VSEPR Model
- Replies: 3
- Views: 7450
Re: Difference Between Lewis Structure and VSEPR Model
Lewis structure clearly shows number of atoms, valence electrons, and types of bonds in a simple way. However, unlike the VSEPR model, Lewis structure doesn't represent the shape of the molecule or bond angles.
- Mon Nov 11, 2019 10:52 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Hydrogen Bonding
- Replies: 3
- Views: 146
Re: Hydrogen Bonding
When a compound melts, it goes from solid to liquid, increasing the distance between molecules. Hydrogen bonding is a strong intermolecular force, so with hydrogen bonding, increasing the distance between molecules within a compound is harder, requiring more energy, thereby resulting in a higher mel...
- Sun Nov 03, 2019 5:32 pm
- Forum: Bond Lengths & Energies
- Topic: HW: 2D Q5c
- Replies: 2
- Views: 112
Re: HW: 2D Q5c
The electronegativity of O is greater than that of S, because they have the same number of valence electrons, but O has more effective nuclear charge, because O has more protons, therefore more positive charges, in the nucleus.
- Sun Nov 03, 2019 4:27 pm
- Forum: Octet Exceptions
- Topic: 2C.3
- Replies: 3
- Views: 212
Re: 2C.3
The most favorable structure should be the one with 0 formal charges on each atom. If it is impossible to have each atom with 0 formal charge, then the atoms with negative formal charge should be the ones with greatest electronegativity.
- Sun Nov 03, 2019 9:20 am
- Forum: Polarisability of Anions, The Polarizing Power of Cations
- Topic: Polarizable vs Polarizing
- Replies: 6
- Views: 321
Re: Polarizable vs Polarizing
Since in forming covalent bonds, electrons are shared between neighboring atoms, an increase in covalent character means that even though in forming ionic bonds, electrons from the less electronegative atom are taken by the more electronegative atom, the less electronegative atom would actually attr...
- Sun Nov 03, 2019 9:04 am
- Forum: Dipole Moments
- Topic: Dipole Moments
- Replies: 3
- Views: 108
Re: Dipole Moments
The difference in electronegativity between neighboring atoms leads to difference in charge, which generates an electric field and could be measured.
dipole moment = charge * distance between atoms (bond length)
dipole moment = charge * distance between atoms (bond length)
- Sun Nov 03, 2019 1:03 am
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal charge equation
- Replies: 3
- Views: 142
Re: Formal charge equation
Yes, it works, because it is actually equivalent to the formal formula, numerically. As long as not written formally in exams, I think that using this equation instead is much faster in calculation and harder to make mistakes.
- Sun Nov 03, 2019 12:19 am
- Forum: Ionic & Covalent Bonds
- Topic: Bond Strength
- Replies: 3
- Views: 138
Re: Bond Strength
Indeed, F has greater electronegativity than Cl. I think it is because of greater electronegativity, electrons are pulled to F by a greater electrostatic force than to Cl.
- Fri Oct 25, 2019 11:26 am
- Forum: Ionic & Covalent Bonds
- Topic: Isoelectronic Atoms
- Replies: 6
- Views: 403
Re: Isoelectronic Atoms
Being isoelectronic elements means that they have the same number of valence electrons. However, this doesn't mean that they have similar chemical properties, partially because they have different nuclear charges. I think that when mentioning isoelectronic, the elements aren't in the state of atom. ...
- Fri Oct 25, 2019 11:12 am
- Forum: Resonance Structures
- Topic: Formal Charge
- Replies: 13
- Views: 1421
Re: Formal Charge
Yes, it matters. The most ideal situation is to have 0 formal charges on each atom. If it cannot be 0, then it is best to have the least absolute sum value of formal charges with the most negative on the most electronegative element.
- Thu Oct 24, 2019 8:50 pm
- Forum: Ionic & Covalent Bonds
- Topic: octet rule
- Replies: 6
- Views: 269
Re: octet rule
There are many exceptions to the octet rule. The octet rule works mainly well for elements in the first three periods, because they don't have d-orbitals. Since the 4th period, the electron cloud become relatively big (having d-orbitals), therefore allowing electrons more than eight as valence elect...
- Thu Oct 24, 2019 8:28 pm
- Forum: Trends in The Periodic Table
- Topic: blocks
- Replies: 13
- Views: 655
Re: blocks
I think that remembering that s is on the left, p is on the right, d is in the middle, and f is at the bottom would be enough for this course. And remember that f-block is actually inserted in the 6th and 7th period, between s-block and d-block.
- Thu Oct 24, 2019 8:19 pm
- Forum: Trends in The Periodic Table
- Topic: bond length
- Replies: 9
- Views: 451
Re: bond length
I believe that we don't need to know how to calculate bond length throughout chem 14A. However, I think it is necessary to know that the bond length of triple bond is shorted than double bond, which is shorter than single bond. There are three pairs of shared electrons in triple bond, so the forces ...
- Thu Oct 24, 2019 8:01 pm
- Forum: Trends in The Periodic Table
- Topic: Effective Nuclear Charge
- Replies: 5
- Views: 222
Re: Effective Nuclear Charge
Because the inner electrons shield outer electrons from electrostatic attraction of the positive nucleus, the outer electrons feel a reduced electrostatic attraction, resulting in an effective nuclear charge. In my opinion, the larger the effective nuclear charge, the higher the first ionization ene...
- Sun Oct 20, 2019 12:08 am
- Forum: Trends in The Periodic Table
- Topic: Electronegativity vs. Electron Affinity?
- Replies: 11
- Views: 1706
Re: Electronegativity vs. Electron Affinity?
If an element has a high electronegativity, does that mean it has higher electron affinity? I believe so because for one of our practice questions, the answer was something along the lines "If an element has a high ionization energy and a higher electron affinity, it is also highly electronega...