Search found 42 matches
- Sat Mar 12, 2016 6:20 pm
- Forum: *Alkanes and Substituted Alkanes (Staggered, Eclipsed, Gauche, Anti, Newman Projections)
- Topic: Determining most stable conformation
- Replies: 1
- Views: 636
Determining most stable conformation
In the 2013 final question 8c, there is a Newman projection. How do you determine which conformation cyclohexane is by just looking at the newman projection?
- Sat Mar 12, 2016 1:27 am
- Forum: *Cycloalkanes
- Topic: Cycloalkanes substituent?
- Replies: 1
- Views: 612
Re: Cycloalkanes substituent?
I would assume so. The cyclic structure is a substituent if the straight chain is longer than the cyclic structure.
- Sat Mar 12, 2016 1:25 am
- Forum: *Electrophiles
- Topic: Electrophiles vs Nucleophiles
- Replies: 1
- Views: 667
Re: Electrophiles vs Nucleophiles
An electrophile is a species that wants to gain an electron. Usually this results in a polar bond between two elements. For example, HBr would be an electrophile as the Bromine in this compound pulls on the shared electrons, causing a positive charge around H and a negative charge around Br. A nucle...
- Fri Mar 11, 2016 11:34 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Deciding which should be oxidizing and reducing agent
- Replies: 1
- Views: 559
Re: Deciding which should be oxidizing and reducing agent
Yes, the species that gets oxidized should have the lower of the two standard reduction potentials.
- Fri Mar 11, 2016 11:28 pm
- Forum: *Constitutional and Geometric Isomers (cis, Z and trans, E)
- Topic: Priority in Methyl vs Fluorine
- Replies: 1
- Views: 1794
Priority in Methyl vs Fluorine
Hello,
I just faced a problem where apparently a methyl group has higher priority than a fluorine; is this true? My thought process was that the fluorine should have more priority as it has a higher atomic number over carbon.
Thanks
I just faced a problem where apparently a methyl group has higher priority than a fluorine; is this true? My thought process was that the fluorine should have more priority as it has a higher atomic number over carbon.
Thanks
- Wed Mar 09, 2016 4:44 pm
- Forum: *Constitutional and Geometric Isomers (cis, Z and trans, E)
- Topic: Textbook problem - chain structure with cis and trans
- Replies: 1
- Views: 483
Textbook problem - chain structure with cis and trans
For the example on page 17 of the organic chemistry textbook, why is (E)-3,7-Dimethylocta-1,3,7-triene trans and not cis? Doesn't the atom group attached the double bonds indicate that this is a cis stricture?
- Wed Feb 24, 2016 10:15 pm
- Forum: *Cycloalkanes
- Topic: Ring Substituents
- Replies: 1
- Views: 628
Ring Substituents
Is it possible for a cyclic structure to have another cyclic structure as a substituent? For example is it possible for a cyclopentane structure to have a cyclopropyl substituent?
Thanks!
Thanks!
- Sun Feb 14, 2016 6:02 pm
- Forum: General Rate Laws
- Topic: Steady State and Pre Equilibrium Approach
- Replies: 1
- Views: 580
Steady State and Pre Equilibrium Approach
When do we know to use the steady state or pre equilibrium approach in determining whether a proposed elementary mechanism matches an observed rate law? Are there definitive clues to look out for?
Thank You
Thank You
- Thu Feb 04, 2016 6:14 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Enthalpy of Vaporization
- Replies: 1
- Views: 594
Re: Enthalpy of Vaporization
This is the process where you let the water heat to the vaporizing temperature (100 C), let it vaporize at that temperature, and then let it cool back down to the initial temperature (25 C). Water cannot normally vaporize at 25C, we have to use this special process to calculate the value of it.
- Thu Jan 28, 2016 10:48 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: internal energy state function
- Replies: 1
- Views: 589
Re: internal energy state function
Internal energy is a state function because it doesn't matter how one got to the final state of a certain system. A system could do 100 J of work and end up at a particular internal energy. Another system could do 100,000 J of work and arrive at the same internal energy. Regardless of how much work ...
- Tue Jan 26, 2016 10:56 pm
- Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
- Topic: entropy
- Replies: 1
- Views: 580
Re: entropy
Entropy increases with heavier atoms as heavier atoms have more vibrational energy than lighter atoms. Additionally, entropy increases with molecular complexity. Meaning when there are more atoms attached to the central atom of a certain compound, the entropy of that particular compound increases. A...
- Tue Jan 26, 2016 10:51 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Clarification of State Properties
- Replies: 1
- Views: 419
Re: Clarification of State Properties
U is internal energy.
- Sun Jan 24, 2016 3:08 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Question 8.65
- Replies: 1
- Views: 621
Re: Question 8.65
The desired reaction for a standard enthalpy of formation of any compound is just a balanced chemical reaction between the constituent elements in their standard states as reactants forming the desired compound as the product. For example, in this problem the desired standard enthalpy of formation i...
- Wed Jan 20, 2016 4:49 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: Interpreting Residual Entropies
- Replies: 1
- Views: 783
Interpreting Residual Entropies
When you are interpreting residual entropies for of a particular compound, how do you know how many orientations it can assume? The example in the textbook showed that FClO 3 had four orientations as it was tetrahedral. Is the molecular shape the only indicator of how many orientations a compound ca...
- Sun Jan 17, 2016 12:28 am
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Qsystem = -Qsurroundings help
- Replies: 2
- Views: 2981
Re: Qsystem = -Qsurroundings help
Inadvertently, yes. The negative sign basically shows that whatever work a system performs is absorbed by its surroundings. Contrarily, whatever work is performed on the system by the surroundings is absorbed by the system and lost by the surroundings. They are equal and opposite.
Hope that helped!
Hope that helped!
- Sun Jan 17, 2016 12:25 am
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Thermodynamics: Entropy
- Replies: 2
- Views: 696
Re: Thermodynamics: Entropy
I think it is more along the lines of an increase in the expansion of gas will cause an increase in entropy. Entropy is a measure of disorder. Now, there is thermal disorder, disorder from increasing the thermal motion of molecules (heating a substance). There is also positional disorder, which is w...
- Sun Jan 10, 2016 8:18 pm
- Forum: Phase Changes & Related Calculations
- Topic: Homework 8.27
- Replies: 6
- Views: 2762
Re: Homework 8.27
For problems involving irreversible expansion you would use w = -PexΔV.
For problems involving reversible, isothermal expansion, you would use w = -nRT x ln(vf/vi)
The problem usually specifies the type of expansion you're dealing with.
For problems involving reversible, isothermal expansion, you would use w = -nRT x ln(vf/vi)
The problem usually specifies the type of expansion you're dealing with.
- Sun Jan 10, 2016 8:13 pm
- Forum: Phase Changes & Related Calculations
- Topic: Heating Curve
- Replies: 1
- Views: 558
Re: Heating Curve
I'm assuming you're referring to 8.43, not 8.41. And you're correct in saying that the right answer is c; the solutions manual confirms this answer.
- Sun Jan 10, 2016 8:08 pm
- Forum: Phase Changes & Related Calculations
- Topic: Self-Test 8.9B
- Replies: 1
- Views: 631
Re: Self-Test 8.9B
You wouldn't use the Hvap= H(vapor)- H(liquid) formula for this question. All you have to do is find the enthalpy of formation in terms of kJ/mol. This involves converting the amount of methanol they gave in grams to mols and then dividing the amount of heat it took to vaporize to this amount by you...
- Sat Jan 09, 2016 5:36 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Calculating heat, work, and change in internal energy
- Replies: 1
- Views: 539
Re: Calculating heat, work, and change in internal energy
Heat transferred under constant volume can be calculated by finding the change in internal energy, ΔU. Heat transferred under constant pressure can be calculated b finding the change in enthalpy, ΔH.
- Sat Jan 09, 2016 5:30 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: q and Enthalpy
- Replies: 1
- Views: 487
Re: q and Enthalpy
I'll take a mathematical perspective to show why q = Enthalpy at constant pressure: Change in Enthalpy as a state function can be represented by the equation: ΔH = ΔU + PΔV. Where H is enthalpy, U is internal energy, P is pressure, and V is volume. To show that q = enthalpy at constant pressure we c...
- Fri Dec 04, 2015 8:36 pm
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: Uncertainty Equation
- Replies: 1
- Views: 502
Re: Uncertainty Equation
You would use the Heisenburg Uncertainty Equation.
ΔpΔx≥h/4π
ΔpΔx≥h/4π
- Fri Dec 04, 2015 8:32 pm
- Forum: Properties & Structures of Inorganic & Organic Bases
- Topic: Acid Strength
- Replies: 1
- Views: 995
Re: Acid Strength
Dr. Lavelle had an excellent explanation of this exact problem in his review session for the final. Basically, CH 3 is a more electron rich species than H is, and therefore has more of a negative charge associated with it. In fact H is basically considered a positive species. Because of this, CH 3 d...
- Fri Dec 04, 2015 8:28 pm
- Forum: *Making Buffers & Calculating Buffer pH (Henderson-Hasselbalch Equation)
- Topic: Henderson-Hasselbalch
- Replies: 1
- Views: 520
Re: Henderson-Hasselbalch
You use the HH equation when the reaction involves a weak acid and its conjugate base. Usually this implies that the K a value is going to be smaller than 1 x 10 -4 . However if the K a value is larger than that value then it is safer to go with the ICE box. Essentially, the HH equation is an approx...
- Fri Nov 27, 2015 8:57 pm
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: Electronegativity and acid strength
- Replies: 4
- Views: 14404
Re: Electronegativity and acid strength
The more electronegative a certain atom is in a molecule, the more it draws on the electron density of the overall molecule. This pulling actually results in a higher stabilization state for the molecule. Therefore, the more electronegative a particular element is, the harder it pulls, and the more ...
- Fri Nov 27, 2015 8:50 pm
- Forum: Identifying Acidic & Basic Salts
- Topic: Ions as Bases
- Replies: 2
- Views: 688
Re: Ions as Bases
Sodium is not included because it is a spectator ion, so we just tend to leave it out.
- Fri Nov 27, 2015 8:48 pm
- Forum: Lewis Acids & Bases
- Topic: Acid and Base Neutralization
- Replies: 1
- Views: 584
Acid and Base Neutralization
In order for acids and bases to neutralize each other, do they have to have the relatively close amounts to one another? Or can you have a lot of base and add a little acid to neutralize the two? (or vice versa).
- Mon Nov 16, 2015 11:26 pm
- Forum: Naming
- Topic: Drawing ICE box
- Replies: 1
- Views: 545
Re: Drawing ICE box
This is when calculating reaction quotient (Q c ) is very helpful. Remember, you use the same process to calculate Q c as you do to calculate the equilibrium constant. As Dr. Lavelle has outlined in class, if the reaction quotient is less than the equilibrium constant, (Q c < K c ) then the reaction...
- Mon Nov 16, 2015 11:19 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: ICE Table
- Replies: 1
- Views: 280
Re: ICE Table
The ice table is required when the initial molarities of reactants and or products are given, but the equilibrium molarities are not. Typically, the equilibrium constant is provided and using the ice box, you have to solve for the change in concentrations for the reactants and products.
- Mon Nov 16, 2015 11:17 pm
- Forum: Naming
- Topic: Coordination Compounds
- Replies: 1
- Views: 462
Re: Coordination Compounds
The roman numerals after the cation name specifies the charge that the cation (central atom has). In the problem that you provided, since NH 3 has a neutral charge, we are left with two chlorines (one inside the coordination complex, and one outside). These two chlorines amount to a net -2 charge. A...
- Sat Nov 14, 2015 7:41 pm
- Forum: Naming
- Topic: Alphabetical Order in Naming?
- Replies: 1
- Views: 570
Alphabetical Order in Naming?
Hello,
When naming a coordination compound, does a greek prefix play a role in the alphabetization? For example if a compound contained diammine and chloro, would the chloro come first since C comes before D? Or do we disregard the D and say that diammine comes before chloro? Thank You!
When naming a coordination compound, does a greek prefix play a role in the alphabetization? For example if a compound contained diammine and chloro, would the chloro come first since C comes before D? Or do we disregard the D and say that diammine comes before chloro? Thank You!
- Sat Oct 31, 2015 7:01 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Dissociation Energy
- Replies: 2
- Views: 713
Re: Dissociation Energy
It isn't something we have to calculate, at least for this class. However, there are general rules for which bonds between atoms might be stronger than other bonds. Normally, shorter bonds are stronger than longer bonds (i.e. triple > double > single). Additionally, bonds between atoms that have lon...
- Sat Oct 31, 2015 6:54 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Lewis structure of SO2Cl2
- Replies: 1
- Views: 5830
Re: Lewis structure of SO2Cl2
Yes, according to the general rules of formal charge, if sulfur had double bonds with both oxygen atoms, the entire compound would technically be considered in a lower energy, more stable state. However, remember that formal charge is just a general set of rules you can follow, it doesn't mean that ...
- Sun Oct 25, 2015 4:21 pm
- Forum: Lewis Structures
- Topic: HW #3.57b
- Replies: 1
- Views: 569
HW #3.57b
Why is it that in the Lewis structure of the hydrogen sulfite ion, the sulfur is not attached to hydrogen? Instead, the sulfur is attached to three oxygens and the hydrogen is attached to one of the oxygens. Why is this?
- Fri Oct 16, 2015 5:59 pm
- Forum: Ionic & Covalent Bonds
- Topic: Compounds having Ionic/Covalent Characteristics
- Replies: 1
- Views: 698
Compounds having Ionic/Covalent Characteristics
What other properties are examined to determine whether a compound having an electronegativity between 1.5 and 2.0 is more ionic or more covalent? Professor Lavelle mentioned a compound's solubility in water can be indicative its chemical properties. Any other properties we can look at to tell wheth...
- Fri Oct 16, 2015 5:52 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Determining principle quantum number
- Replies: 1
- Views: 426
Re: Determining principle quantum number
The principle quantum number is always the period the element is located in. In this case, iron would have n=4, as it is in the fourth period. Principle quantum number is unrelated to which orbital electrons are being added to.
- Fri Oct 16, 2015 4:44 pm
- Forum: Ionic & Covalent Bonds
- Topic: Diatomic Molecules
- Replies: 3
- Views: 807
Re: Diatomic Molecules
Yes. Another shorthand phrase that is helpful for me to remember which elements are HON and the halogens. Another good one is Have No Fear Of Ice Cold Beer.
- Fri Oct 16, 2015 4:40 pm
- Forum: Resonance Structures
- Topic: Stability in Resonance Structures
- Replies: 1
- Views: 514
Re: Stability in Resonance Structures
Resonance structures are unique in that the electrons present in the structure are delocalized, meaning that they are not associated with one particular atom or bond in the chemical structure. This state of delocalization is the reason why resonance structures are generally more stable than non-reso...
- Sat Oct 10, 2015 12:34 am
- Forum: Trends in The Periodic Table
- Topic: Electron Affinity Trends
- Replies: 1
- Views: 443
Electron Affinity Trends
For both ionization energies and size there are general trends that have relatively few exceptions within their trends. However, electron affinities seem to be all over the place. Although it is true that the upper right elements generally have high electron affinities, there is not the same constan...
- Sat Oct 10, 2015 12:28 am
- Forum: Trends in The Periodic Table
- Topic: Exceptions to Ionization energy trends?
- Replies: 3
- Views: 42431
Re: Exceptions to Ionization energy trends?
Bryan did a great job of explaining. Basically, there is a greater electron-electron repulsion force within the oxygen atom than there is within the nitrogen atom because the eighth electron in oxygen is paired with an electron that is already occupying an orbital. This repulsion of electrons in the...
- Thu Oct 01, 2015 11:58 pm
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: Initial and Final Energy Levels
- Replies: 1
- Views: 1944
Initial and Final Energy Levels
Question (1.15): In the UV spectrum of atomic Hydrogen, a line is observed at 102.6 nm. Determine the values of n for the initial and final energy levels of the electron during the emission of energy that leads to this spectral line. I understand that you first have to use the λν = c formula to calc...
- Thu Oct 01, 2015 11:41 pm
- Forum: Photoelectric Effect
- Topic: eV to J
- Replies: 1
- Views: 474
Re: eV to J
There are 1.6022 x 10^(-19) Joules for every electron volt.