no, you don't have to know them
they weren't covered in class
Search found 62 matches
- Mon Mar 07, 2016 1:36 pm
- Forum: *Cyclohexanes (Chair, Boat, Geometric Isomers)
- Topic: Boat vs. twist boat conformation
- Replies: 1
- Views: 768
Re: Boat vs. twist boat conformation
Twist boat is preferred over boat. It's because when twisted, the torsional strain lessens.
- Wed Mar 02, 2016 4:21 pm
- Forum: *Alkanes
- Topic: Tert-butyl's Common Name
- Replies: 1
- Views: 585
Re: Tert-butyl's Common Name
It's because its a substituent. The longest chain that the substituent has is 2 carbons, so ethyl, because the carbon in the substituent is connected to the main chain by that middle carbon, so that carbon has to be in the longest chaing, then you can only get ethane as the longest unbroken chain st...
- Fri Feb 26, 2016 1:40 pm
- Forum: *Alkanes
- Topic: Alphebetizing rules in naming Organic Compounds
- Replies: 2
- Views: 635
Re: Alphebetizing rules in naming Organic Compounds
Basically, prefixes don't count only when your quantifying them. So like di-, tri-. Those kinds of prefixes don't count. But the common name ones like iso or neo do count when alphabetizing.
- Tue Feb 23, 2016 8:33 pm
- Forum: *Alkanes
- Topic: How to prioritize hydrocarbon chains of different length?
- Replies: 2
- Views: 504
Re: How to prioritize hydrocarbon chains of different length
What do you mean by the halogen gets the priority over the double bond. Wouldn't the double bond get priority since it changes the name of the hydrocarbon? And if there is a halogen, isn't it no longer considered a hydrocarbon?
- Wed Feb 17, 2016 10:40 pm
- Forum: General Rate Laws
- Topic: Pseudo Rate Law
- Replies: 2
- Views: 2018
Re: Pseudo Rate Law
Pseudo rate laws are important in that they help us figure out the overall rate law when a reaction has more than one reactant and all the concentrations are changing. Since there are so many variables, the pseudo rate law helps simplify the problem and you can focus on one reactant at a time.
- Sun Feb 07, 2016 1:55 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: equations
- Replies: 2
- Views: 718
equations
When asked for a K value, there are 3 equations that you could use: deltaG=-RTlnK E=E(naught)-(RT/nF)lnQ --> 0 = E(naught)-(RT/nF)lnK and E=E(naught) - (0.0592/n)logQ --> 0=E(naught) - (0.0592/n)logK But you get different answers using each of the equations for the same problem. Why? and how do you ...
- Sun Feb 07, 2016 12:18 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Midterm 2013 3A
- Replies: 1
- Views: 369
Midterm 2013 3A
For the part on work,
I understand how you get w=-PdeltaV=-delta(n)RT
but if there is no change in moles, how does this equation work?
I understand how you get w=-PdeltaV=-delta(n)RT
but if there is no change in moles, how does this equation work?
- Sat Feb 06, 2016 5:38 pm
- Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
- Topic: Midterm 2011 2B
- Replies: 2
- Views: 783
Midterm 2011 2B
The question states that Container A: 1 mol of ideal monatomic gas Container B: 1 mol of diatomic gas, not vibrationally active Container C: 1 mol of diatomic gas, vibrationally active. The answer states that the containers, in order of increasing change in entropy is B<C<A Why is A the greatest. I ...
- Sat Feb 06, 2016 4:32 pm
- Forum: Calculating Work of Expansion
- Topic: When to use which formula
- Replies: 3
- Views: 778
Re: When to use which formula
But if you know the initial and final volume, don't you know the change in volume?
- Sat Feb 06, 2016 4:09 pm
- Forum: General Rate Laws
- Topic: Integrated Rate Law
- Replies: 1
- Views: 417
Re: Integrated Rate Law
Yes, when Prof Lavelle derived it for us in class, we used the equation
A --> P. Thus a=1
A --> P. Thus a=1
- Wed Feb 03, 2016 4:08 pm
- Forum: Balancing Redox Reactions
- Topic: E not
- Replies: 1
- Views: 438
Re: E not
E naught, is the standard reduction potential for each half reaction. The E naught of the entire cell looks at the difference between the two E values of the each half reaction. So, if you multiply both sides by the molar coefficient, the difference between the two values is the same. So, E naught i...
- Fri Jan 29, 2016 10:34 pm
- Forum: Balancing Redox Reactions
- Topic: O3--> O2
- Replies: 2
- Views: 1106
O3--> O2
how is this a reduction reaction? Aren't the charges on both 0?
The solution manual says to add 2e-, but why? there is not change in charge.
The solution manual says to add 2e-, but why? there is not change in charge.
- Wed Jan 27, 2016 11:06 am
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Isothermal and reversible
- Replies: 3
- Views: 837
Isothermal and reversible
What exactly does this mean?
Also, in def it says isothermal is deltaT is 0. So wouldn't that make q=0? But in problems, it says that deltaU=0. Why?
Also, in def it says isothermal is deltaT is 0. So wouldn't that make q=0? But in problems, it says that deltaU=0. Why?
- Mon Jan 25, 2016 12:36 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
- Replies: 2
- Views: 619
Residual
What exactly is residual entropy, and why does the book say the equation S=kBlnW is statistical entropy?
- Mon Jan 25, 2016 12:34 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: Bond Formation
- Replies: 2
- Views: 632
Re: Bond Formation
bonds broken is positive and bonds formed is negative
- Mon Jan 25, 2016 12:32 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
- Replies: 2
- Views: 660
Re: Residual Entropy
It is not always ln2
In more general terms, it is lnA^N where A is the number of positions there are, and N are the number of particles available to fill a position.
In more general terms, it is lnA^N where A is the number of positions there are, and N are the number of particles available to fill a position.
- Sun Jan 24, 2016 5:13 pm
- Forum: Calculating Work of Expansion
- Topic: equations
- Replies: 1
- Views: 374
equations
In my discussion, we went through examples that used w= p(deltaV) and then w=integral from V2->V1(PdV) when do we use which one?
- Wed Jan 20, 2016 8:03 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Calculating W
- Replies: 2
- Views: 525
Re: Calculating W
I think we are assuming that each state has equal energy. I don't think you have to worry about them reacting with each other. For the sake of the example, I think we just assume that they don't.
- Wed Jan 20, 2016 7:59 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Reversible and irreversible
- Replies: 1
- Views: 546
Re: Reversible and irreversible
Well, a reversible process means that it can be undone without any change in the thermodynamic state. It is a very slow process in which all heat would be transferred to work, but this is an ideal process. It doesn't happen real life. A irreversible process is the opposite. It is a faster process th...
- Wed Jan 20, 2016 7:51 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Monoatomic and Diatomic
- Replies: 2
- Views: 633
Re: Monoatomic and Diatomic
I may be wrong, but you have to assume that the gas will act like an ideal gas, or they will tell you that it does. From there, if you know the molecule, you should know if it is monatomic or diatomic, like He is monatomic, but O2 is diatomic.
- Tue Jan 12, 2016 5:43 pm
- Forum: Phase Changes & Related Calculations
- Topic: Equation W=delta U-q in problem 8.7
- Replies: 1
- Views: 573
Re: Equation W=delta U-q in problem 8.7
You basically just rearrange the equation delta U= w + q
To use it, you plug and chug.
In context of this question, delta U = 982 J
q= 492 J
so w= 982-492J = 490J
To use it, you plug and chug.
In context of this question, delta U = 982 J
q= 492 J
so w= 982-492J = 490J
- Mon Jan 11, 2016 12:44 am
- Forum: Phase Changes & Related Calculations
- Topic: Enthalpy of Reaction
- Replies: 1
- Views: 355
Enthalpy of Reaction
How do you estimate the enthalpy of formation in problem 8.67?
The answer key says that H(f,water(l))=deltaH(f,water(gas)) - deltaH(vap)
but I don't understand where they got that from and how the bond breakdown works.
The answer key says that H(f,water(l))=deltaH(f,water(gas)) - deltaH(vap)
but I don't understand where they got that from and how the bond breakdown works.
- Mon Jan 11, 2016 12:32 am
- Forum: Phase Changes & Related Calculations
- Topic: Sublimation
- Replies: 2
- Views: 552
Re: Sublimation
Well, sublimation is when a solid changes directly into a gas. It skips the liquid stage. You can see why this happens when you look at a phase diagram http://d32ogoqmya1dw8.cloudfront.net/images/research_education/equilibria/h2o_phase_diagram_-_color.v2.jpg"onclick="window.open(this.href);return fa...
- Sun Jan 10, 2016 10:28 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Enthalpy density
- Replies: 1
- Views: 405
Enthalpy density
Why is the answer to 8.51, the enthalpy density positive 239000 and not negative? If energy is released, isn't that supposed to be a negative value?
- Sun Jan 10, 2016 4:49 pm
- Forum: Phase Changes & Related Calculations
- Topic: Heating Curve
- Replies: 1
- Views: 558
Heating Curve
For 8.41, it says The following data were collected for a new compound used in cosmetics: !Hfus" 10.0 kJ·mol$1, !Hvap" 20.0kJ·mol1; heat capacities: 30 J·mol$1 for the solid; 60 J·mol$1 for the liquid; 30 J·mol$1 for the gas. Which heating curve below best matches the data for this compoun...
- Wed Jan 06, 2016 3:15 pm
- Forum: Phase Changes & Related Calculations
- Topic: Steam v Water
- Replies: 4
- Views: 1204
Re: Steam v Water
It's because steam can get to a higher temperature than liquid water can. Liquid water can only get to 100C before it starts vaporizing, while steam can get even hotter.
- Fri Dec 04, 2015 8:15 pm
- Forum: *Making Buffers & Calculating Buffer pH (Henderson-Hasselbalch Equation)
- Topic: Henderson-Hasselbalch
- Replies: 1
- Views: 520
Henderson-Hasselbalch
Is there anyway to know when to use Henderson-Hasselbalch and when to use ICE box, or are they always interchangeable?
- Tue Dec 01, 2015 9:33 pm
- Forum: Polyprotic Acids & Bases
- Topic: finding pH
- Replies: 2
- Views: 698
finding pH
In class, Professor Lavelle said that we use only Ka1 to determine pH for polyprotic acids and bases. With the exception of H2SO4 where we use Ka2 too. But then in some of the textbook problems they either give you Ka2 or expect you to find it. How do you know when to use Ka2 in determining pH and h...
- Tue Dec 01, 2015 4:36 pm
- Forum: Calculating the pH of Salt Solutions
- Topic: Determining if a compound is a salt
- Replies: 1
- Views: 499
Re: Determining if a compound is a salt
A salt is an ionic compound composed of an anion and a cation. Under acids and bases, it is formed during a neutralization reaction. Since it is compound composed of balanced charges of anions and cations, salt have no net charge.
- Tue Nov 24, 2015 1:57 pm
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: HF Acid
- Replies: 3
- Views: 773
Re: HF Acid
It is because HF has such a strong bond that it does not dissociate very easily. A strong acid is one that dissociates completely. So HF is not a strong acid.
- Tue Nov 24, 2015 1:51 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Determining pH
- Replies: 3
- Views: 1248
Re: Determining pH
so what you have to do is find the concentration of H3O+ by using the ICE box. Once you find the concentration, you use the pH=-log[H3O+] and once you find the pH, you can order them.
- Sun Nov 22, 2015 2:49 pm
- Forum: Conjugate Acids & Bases
- Topic: Relative base strength.
- Replies: 1
- Views: 498
Relative base strength.
Looking at problem 12.49, how can you tell if BrO- is stronger or C17H19O3N is a stronger base? Is it based off it's size or do you need to the the Ka value? Is there an easy way to look and know?
- Sun Nov 22, 2015 2:47 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: HF, HCl, HBr, and HI Acid Strength
- Replies: 1
- Views: 6045
Re: HF, HCl, HBr, and HI Acid Strength
It's because HF has the strongest bond that it makes it the weakest out of all of them. The stronger the acids, the more easily it dissociates in solution. Since HF has the strongest bond, it doesn't dissociate as easily as HI does, making it weaker.
- Sun Nov 22, 2015 1:19 pm
- Forum: Bronsted Acids & Bases
- Topic: Determining Acids and Bases
- Replies: 5
- Views: 1117
Re: Determining Acids and Bases
There is no way to tell through structure or anything like that. You simply have to know which ones are strong and the rest are weak.
Common strong acids are HCl, H2SO4, HBr, HI, HClO4, HNO3, HClO3.
Common strong bases are column one hydroxides and column two hydroxides starting with Ca.
Common strong acids are HCl, H2SO4, HBr, HI, HClO4, HNO3, HClO3.
Common strong bases are column one hydroxides and column two hydroxides starting with Ca.
- Fri Nov 20, 2015 1:44 pm
- Forum: Conjugate Acids & Bases
- Topic: Proton Transfer Equilibria and Conjugate acid-base pairs
- Replies: 1
- Views: 2646
Re: Proton Transfer Equilibria and Conjugate acid-base pairs
H2SO4 +H2O <--> H3O + HSO4
acid: H2SO4
CB: HSO4
Since it is polyprotic
HSO4 + H2O <--> H3) +SO4
acid: HSO4
CB: SO4
The overall reaction would be
H2SO4 + 2H20 <--> 2H3O + SO4
acid: H2SO4
CB: SO4
acid: H2SO4
CB: HSO4
Since it is polyprotic
HSO4 + H2O <--> H3) +SO4
acid: HSO4
CB: SO4
The overall reaction would be
H2SO4 + 2H20 <--> 2H3O + SO4
acid: H2SO4
CB: SO4
- Wed Nov 18, 2015 1:25 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Chelating Complex
- Replies: 2
- Views: 658
Re: Chelating Complex
A coordination complex will form a chelating complex if the ligands have a lone pair that can form a bond, and if the two ligands are close enough together to form one. i.e. two NH2 attached on opposite sides of a benzene ring will not form a chelating complex even though they have the lone pair, si...
- Wed Nov 18, 2015 1:19 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Shape of Coordination Compound
- Replies: 1
- Views: 550
Re: Shape of Coordination Compound
You have to use Crystal Field Theory, which we did not learn in class, nor are we responsible for knowing. but if you are really interested, this does a pretty good job of explaining it http://chemwiki.ucdavis.edu/Inorganic_Chemistry/Crystal_Field_Theory/Crystal_Field_Theory"onclick="window.open(thi...
- Wed Nov 18, 2015 1:14 pm
- Forum: Lewis Acids & Bases
- Topic: How do you determine if an element is an Acid or Base?
- Replies: 2
- Views: 838
Re: How do you determine if an element is an Acid or Base?
Also, since certain compounds are amphoteric, you have to see how they react with other compounds in order to determine that as well.
- Wed Nov 18, 2015 1:13 pm
- Forum: Lewis Acids & Bases
- Topic: Strong Acids and Bases
- Replies: 2
- Views: 516
Re: Strong Acids and Bases
In other words, it is simply 10^-pH
- Wed Nov 18, 2015 1:09 pm
- Forum: Ideal Gases
- Topic: Total Pressure of a System
- Replies: 1
- Views: 524
Re: Total Pressure of a System
You just add the partial pressures together. The partial pressure already takes the mole fraction into account, in the sense that the partial pressure of a gas is the total pressure times the mole fraction.
- Mon Nov 09, 2015 2:06 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Aqueous Solutions in Equilibrium Constant Calculations
- Replies: 1
- Views: 481
Re: Aqueous Solutions in Equilibrium Constant Calculations
Yes. The only ones you wouldn't include are solids and liquids. Aqueous solutions and gases are included in the equation.
- Mon Nov 09, 2015 2:04 pm
- Forum: Ideal Gases
- Topic: Effect of inert gasses on equilibrium
- Replies: 1
- Views: 528
Re: Effect of inert gasses on equilibrium
It is because it is not the pressure that causes the shift, it is the concentration of the gases. When you add the inert gas, it doesn't react with any of the gases in the container, so the concentration of the gases involved in the reaction stays the same so there is no shift. When you adjust the p...
- Sat Oct 31, 2015 5:50 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: heteronuclear diatomic molecules
- Replies: 1
- Views: 341
heteronuclear diatomic molecules
When it comes to the diatomic molecules when one atom is Z<8 and the other is Z>8, how do you draw the energy diagram. The bonding sigma is above the bonding pi right, just like in the diagram when Z<8. If that's true, how do we draw the VSEPR one on the sides. I know one is lower in energy than the...
- Sat Oct 31, 2015 5:45 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: Molecular Orbital Theory Order
- Replies: 1
- Views: 306
Re: Molecular Orbital Theory Order
When the atomic number is less than 8, the bonding sigma is above the bonding pi, and when it is 8 and above, the bonding sigma is below the bonding pi.
At least for homonuclear diatomic molecules.
At least for homonuclear diatomic molecules.
- Fri Oct 30, 2015 3:29 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: electronegativity and energy diagrams
- Replies: 1
- Views: 508
electronegativity and energy diagrams
In the hw, its 4.57 (c). I was wondering how the molecular energy diagram might tell you in the molecular orbitals, wether the electrons will have a higher probability of being at N or at O in the NO+ molecule. Does this have to do with the electronegativity of the molecule? or do you get this from ...
- Sat Oct 24, 2015 9:15 pm
- Forum: Hybridization
- Topic: Hybridization of XeF4
- Replies: 1
- Views: 1570
Re: Hybridization of XeF4
If you draw out the lewis structure for it, you find that the molecule has 6 areas of electron density. So, it has a hybridization of sp3d2. Unlike shape, the hybridization relies upon the number of areas of electron density, not on the number of atoms it is bonded to.
- Sat Oct 24, 2015 9:13 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: Quiz 2
- Replies: 2
- Views: 522
Quiz 2
Will we have to know bond order, molecular orbitals, paramagnetic/diamagnetic, for quiz 2? We didn't go over them in class but they are in the practice tests.
- Tue Oct 20, 2015 6:13 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR Shapes and Lone Pair Electrons on central atom
- Replies: 1
- Views: 387
Re: VSEPR Shapes and Lone Pair Electrons on central atom
If you have a linear structure with lone pairs, it simply means that the repulsion of the lone pairs act equally on the other two molecules so that they aren't pushed past the 180 bond angle. For example, If you had a molecule of AX2E3, it would still be considered linear. (It is trigonal bipyramida...
- Tue Oct 20, 2015 6:08 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Strengths of Repulsions
- Replies: 3
- Views: 679
Re: Strengths of Repulsions
Atom is another way of saying bonded. The electrons are bonded to another atom, instead of being a free lone pair.
- Sun Oct 18, 2015 4:55 pm
- Forum: Ionic & Covalent Bonds
- Topic: polarizability
- Replies: 2
- Views: 715
Re: polarizability
Basically, the bigger the atom, the more polarizable it is, and the smaller the atom (typically cations), the more polarizing power it has. This is because the smaller the atom, the stronger the pull from the nucleus is. Also, it has less electrons to shield the pull. With polarizability, the bigger...
- Tue Oct 13, 2015 7:03 pm
- Forum: Trends in The Periodic Table
- Topic: Electron Affinity vs Ionization Energy
- Replies: 3
- Views: 812
Re: Electron Affinity vs Ionization Energy
Ionization energy is the energy required to remove an electron from an atom while electron affinity is how easily an atom will accept an electron into its shells.
- Tue Oct 13, 2015 7:01 pm
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: Absorbing vs Emitting energy
- Replies: 2
- Views: 458
Re: Absorbing vs Emitting energy
Also, an electron can both emit and absorb energy creating its respective spectrums. So when it absorbs energy, like ChemMod said, it shows up as dark lines on a colorful spectrum, while when the electron emits energy, it shows up as a colored line on a black spectrum.
- Sat Oct 10, 2015 4:52 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: Chapter 2 question 85
- Replies: 1
- Views: 362
Re: Chapter 2 question 85
Well, you know that as n, or your principle quantum number, increases, the space between the levels becomes smaller and smaller. So, with the bigger atoms, where n is large, the space between the energy levels is so small, that small changes can cause the electrons to jump around and change the norm...
- Sat Oct 10, 2015 4:50 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Beginning the F orbital for electron configurations
- Replies: 2
- Views: 601
Re: Beginning the F orbital for electron configurations
The f block starts in row 6, after Barium, and starts with the 4f orbital in the Lanthanoids.
- Wed Oct 07, 2015 3:17 pm
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: Infrared Spectroscopy
- Replies: 1
- Views: 573
Infrared Spectroscopy
This is for hw problem number 55 for chapter 1. How do I go about finding the frequency if given the reciprocal centimeters? What exactly are the reciprocal centimeters? Is it frequency divided by speed of light?. If so, do I have to change the cm to m?
- Mon Oct 05, 2015 2:14 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Degenerate Orbitals
- Replies: 1
- Views: 549
Re: Degenerate Orbitals
I don't think that degeneracy really occurs. I think it more just is. If you have a one electron ion or a Hydrogen atom, the orbitals are degenerate.
- Mon Oct 05, 2015 1:55 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Homework 2.37b the nature of shielding in different orbitals
- Replies: 2
- Views: 1089
Re: Homework 2.37b the nature of shielding in different orbi
For shielding, it is not that the electrons closer to the nucleus necessarily block the pull. It is that the farther out the electron is, the more electron electron repulsion there is, which acts to counter the pull of the positively charged nucleus. S orbitals are better at shielding because the el...
- Fri Oct 02, 2015 2:51 pm
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: Psi in the Born interpretation of the wave function
- Replies: 1
- Views: 602
Re: Psi in the Born interpretation of the wave function
Psi is just the height of the wave at a said position, in other words, the amplitude. But it has no physical significance the way psi^2 does. I think the graphs were there just to show you the comparison and to act as a visual to explain that we use the sin or cos function.
- Fri Oct 02, 2015 2:49 pm
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: Heisenberg delta p and delta x
- Replies: 3
- Views: 1047
Re: Heisenberg delta p and delta x
I'm pretty sure that you would put 8. If you look at the example from the lecture about the atom diameter, you are using the entire range, not just the +/- of it, if that makes any sense. In other words, if you assume that the center of the atom is zero, then it would be +/-8.5x10^-16, but we used t...
- Wed Sep 30, 2015 4:13 pm
- Forum: *Black Body Radiation
- Topic: Information not taught
- Replies: 1
- Views: 641
Information not taught
I noticed while doing the homework that some of the problems deal with topics that were not taught, such as specifics about black body radiation, and Z dependent Rydberg relationship. Are we required to know these for tests? Will we go over it in class?
- Fri Sep 25, 2015 4:46 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Homework
- Replies: 5
- Views: 1106
Homework
Do we have to read the entire chapter assigned for homework on top of the problems? I started reading Chapter 1 but it seems to cover a lot more information than I think we will cover in class. Do we have to read all 54 pages or just do the practice problems?