Do you have 11 protons?
Because you're sodium fine!
Search found 102 matches
- Mon Mar 09, 2020 11:14 am
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3642220
- Mon Mar 09, 2020 11:12 am
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3642220
Re: Post All Chemistry Jokes Here
I heard that Oxygen and Magnesium were going out and I was like OMg
- Mon Mar 09, 2020 11:06 am
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Derivation of Arrhenius
- Replies: 2
- Views: 709
Re: Derivation of Arrhenius
The Arrhenius Equation is k=Ae-Ea/RT
So if you take the ln of that you will get lnk = -Ea/RT + lnA
If you have 2 reactions, subtracting lnk1 from lnk2 will get you:
lnk2 - lnk1 = -Ea/RT2 -(-Ea/RT1) + lnA - lnA
Which will simplify to:
ln(k2/k1) = -Ea/R (1/T2 - 1/T1)
So if you take the ln of that you will get lnk = -Ea/RT + lnA
If you have 2 reactions, subtracting lnk1 from lnk2 will get you:
lnk2 - lnk1 = -Ea/RT2 -(-Ea/RT1) + lnA - lnA
Which will simplify to:
ln(k2/k1) = -Ea/R (1/T2 - 1/T1)
- Mon Mar 09, 2020 10:59 am
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Defining Arrhenius
- Replies: 2
- Views: 220
Re: Defining Arrhenius
I don't believe so, just know the Arrhenius Equation in regards to chemical kinetics:
K=Ae-Ea/RT where A is the frequency factor or pre-exponential factor (indicates # collisions with correct orientation)
K=Ae-Ea/RT where A is the frequency factor or pre-exponential factor (indicates # collisions with correct orientation)
- Mon Mar 09, 2020 10:46 am
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Microscopic Reversibility
- Replies: 3
- Views: 299
Re: Microscopic Reversibility
Microscopic reversibility means that the reaction has the same intermediates (same pathway) in both the forward and reverse directions.
- Mon Mar 02, 2020 10:19 am
- Forum: First Order Reactions
- Topic: First Order Reaction
- Replies: 4
- Views: 391
Re: First Order Reaction
PranaviKolla2B wrote:Does someone have a good video explaining how to find a first order reaction vs a second?
These videos explain reaction orders pretty well!
https://www.youtube.com/watch?v=2LMdj91x2HA
https://www.youtube.com/watch?v=VXfbzwAv2Dc
- Mon Mar 02, 2020 10:19 am
- Forum: First Order Reactions
- Topic: First Order Reaction
- Replies: 4
- Views: 391
Re: First Order Reaction
What are characteristics that indicate a first order reaction If the reaction rate increases proportionally with the reactant concentration, then it's a first order reaction (assuming there's only 1 reactant) because the exponent is 1 in the rate equation. Rate = k[A] n For example, if the reaction...
- Mon Mar 02, 2020 10:10 am
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: Units k
- Replies: 3
- Views: 642
Re: Units k
It depends on the rate equation.
Rate = k[A]n[B]m
So if the overall rxn order is 1 (n+m), then k would be in units of 1/s since you're trying to get the rate units to equal mol/L-s.
If the overall rxn order is 2, then k would be in units of L/mol-s, etc.
Rate = k[A]n[B]m
So if the overall rxn order is 1 (n+m), then k would be in units of 1/s since you're trying to get the rate units to equal mol/L-s.
If the overall rxn order is 2, then k would be in units of L/mol-s, etc.
- Mon Mar 02, 2020 10:02 am
- Forum: First Order Reactions
- Topic: preferred form of rates
- Replies: 2
- Views: 239
Re: preferred form of rates
Both of them are correct but the first one is preferred because the generally accepted unique rate equation is -1/a d[A]/dt = 1/b d[B]dt = 1/c d[C]/dt
In the second one it's harder to see the relationship between the coefficients.
In the second one it's harder to see the relationship between the coefficients.
- Mon Mar 02, 2020 9:57 am
- Forum: General Rate Laws
- Topic: determining rate
- Replies: 2
- Views: 257
Re: determining rate
Given multiple experiments with the initial concentration of reactants and the initial rate listed, you can divide one experiment over the other to determine how changes in concentration affect the rate. For example, if doubling the concentration of one reactant doubles the rate, then we know that t...
- Mon Feb 24, 2020 10:36 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Work and Battery system
- Replies: 6
- Views: 435
Re: Work and Battery system
Yes, work (max) equals delta G under constant temperature and pressure.
- Mon Feb 24, 2020 10:26 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Nernst
- Replies: 7
- Views: 551
Re: Nernst
The n comes from the equation ΔG = -nFE which is used to derive the nernst equation.
Since F is in units of C/mole, multiplying that by n (moles) would cancel out the units.
Since F is in units of C/mole, multiplying that by n (moles) would cancel out the units.
- Mon Feb 24, 2020 10:08 am
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Eo as an intensive property
- Replies: 9
- Views: 648
Re: Eo as an intensive property
Therefore, it's a property of matter that does not change even if the amount of matter changes.
- Mon Feb 24, 2020 10:05 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 6L.3-d Water and oxygen cell reaction?
- Replies: 1
- Views: 192
Re: 6L.3-d Water and oxygen cell reaction?
O2 + 4H+ + 4e- -> 2H2O E(anode)=1.23V
O2 + 2H2O + 4e- -> 4OH E(cathode)=0.40V
Reverse the first equation since it's the anode and add the two equations together
You should get 4H2O -> 4H+ + 4OH- which simplifies to
H2O -> H+ + OH-
E(cell) will be 0.40V - 1.23V = -0.83V
O2 + 2H2O + 4e- -> 4OH E(cathode)=0.40V
Reverse the first equation since it's the anode and add the two equations together
You should get 4H2O -> 4H+ + 4OH- which simplifies to
H2O -> H+ + OH-
E(cell) will be 0.40V - 1.23V = -0.83V
- Mon Feb 24, 2020 10:00 am
- Forum: Balancing Redox Reactions
- Topic: Oxidation Number
- Replies: 3
- Views: 440
Re: Oxidation Number
Yes. By definition, the oxidation number of an atom is the charge on that atom.
I don't believe there is a difference, it's just that we conventionally use the term "oxidation number" when talking about redox reactions.
I don't believe there is a difference, it's just that we conventionally use the term "oxidation number" when talking about redox reactions.
- Tue Feb 18, 2020 12:13 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Entropy Changes
- Replies: 3
- Views: 278
Re: Entropy Changes
You can see how entropy increases with an increase in volume in the equation ∆S = nRln(V2/V1)
Similarly, entropy also increases with an increase in temperature in the equation ∆S = nCln(T2/T1)
Similarly, entropy also increases with an increase in temperature in the equation ∆S = nCln(T2/T1)
- Tue Feb 18, 2020 12:06 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Pizza Roll's
- Replies: 3
- Views: 354
Re: Pizza Roll's
You would use delta H = nC(delta T) for each of the reactants or products.
- Tue Feb 18, 2020 12:00 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Midterm: Cp,m and Cv,m
- Replies: 3
- Views: 407
Re: Midterm: Cp,m and Cv,m
For monoatomic gases, Cv would be 3/2 R and Cp would be 5/2 R.
For linear/diatomic molecules, Cv would be 5/2 R and Cp would be 7/2 R.
For nonlinear molecules, Cv would be 3R and Cp would be 4R.
For linear/diatomic molecules, Cv would be 5/2 R and Cp would be 7/2 R.
For nonlinear molecules, Cv would be 3R and Cp would be 4R.
- Tue Feb 18, 2020 11:54 am
- Forum: Phase Changes & Related Calculations
- Topic: Heat required for sublimation
- Replies: 2
- Views: 347
Re: Heat required for sublimation
To clarify, for phase transitions you use the equation q=n(deltaH) and for heating you use the equation q=mC(deltaT).
- Tue Feb 18, 2020 11:51 am
- Forum: Phase Changes & Related Calculations
- Topic: 4C.11
- Replies: 2
- Views: 313
Re: 4C.11
To further elaborate on that,
1) the enthalpy change of the ice melting would be n(delta H)
2) the enthalpy of the rising the ice temperature from 0C to 20C would be mC(deltaT)
1) the enthalpy change of the ice melting would be n(delta H)
2) the enthalpy of the rising the ice temperature from 0C to 20C would be mC(deltaT)
- Tue Feb 18, 2020 11:43 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: sign of delta G
- Replies: 9
- Views: 4443
Re: sign of delta G
You can also alter the concentration of products to reactants in order to change the G value. if you increase the amount of product, the lnK part of the expression will become greater, making the G value more negative. Delta G will be negative, thus the reaction will be more spontaneous. If you decr...
- Mon Feb 10, 2020 9:20 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Entropy of universe
- Replies: 3
- Views: 305
Re: Entropy of universe
Adding on, a reaction can be spontaneous even when delta S is negative if delta H is negative enough, as long as the delta G value is negative.
delta G = delta H - T(delta S)
delta G = delta H - T(delta S)
- Mon Feb 10, 2020 9:16 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Gibbs Free Energy calculation
- Replies: 3
- Views: 242
Re: Gibbs Free Energy calculation
We need to know the concept of Gibbs free energy because it tells us whether a reaction will be spontaneous or not. If delta G is negative, the reaction is spontaneous, and the products will have less free energy than the reactants. If delta G is positive, the reaction is NOT spontaneous, and the pr...
- Mon Feb 10, 2020 8:58 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: fractions
- Replies: 3
- Views: 203
Re: fractions
Also, it's 3R for a nonlinear molecule at constant volume.
At a constant pressure, it's 5/2R if monoatomic, 7/2 if diatomic, and 4R if the molecule is nonlinear.
At a constant pressure, it's 5/2R if monoatomic, 7/2 if diatomic, and 4R if the molecule is nonlinear.
- Mon Feb 10, 2020 8:53 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: types of heat capacities
- Replies: 3
- Views: 267
Re: types of heat capacities
Heat capacity is the amount of heat energy required to raise the temperature of a substance by 1 degrees C. It is extensive because it depends on how much mass there is. The units are in J/C. Specific heat capacity is the heat capacity divided by a certain amount of mass. It is intensive because the...
- Mon Feb 10, 2020 8:37 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Review Session #3b
- Replies: 2
- Views: 125
Re: Review Session #3b
Here's my work if that helps!
- Mon Feb 03, 2020 10:26 am
- Forum: Calculating Work of Expansion
- Topic: Integral Calculations
- Replies: 3
- Views: 188
Re: Integral Calculations
You use the integral in a pressure vs volume graph to find the work of expansion Since W=-PdeltaV, calculating the integral would give the area under the line (W) For irreversible expansions, just calculating the rectangular area would be enough But for reversible expansions, you have to use the int...
- Mon Feb 03, 2020 10:19 am
- Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
- Topic: molar mass
- Replies: 3
- Views: 3731
Re: molar mass
Work off of the variables you're given. As long as the units cancel out, you should be fine!
- Mon Feb 03, 2020 10:13 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: Boltzmann Equation
- Replies: 4
- Views: 161
Re: Boltzmann Equation
The Boltzmann Equation is: S = KBlnW
It shows the relationship between entropy and the number of ways the atoms or molecules of a thermodynamic system can be arranged.
It shows the relationship between entropy and the number of ways the atoms or molecules of a thermodynamic system can be arranged.
- Mon Feb 03, 2020 10:09 am
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Thermodynamics Laws
- Replies: 4
- Views: 157
Re: Thermodynamics Laws
The first law of thermodynamics is the conservation of energy. The second law of thermodynamics is that the entropy of any isolated system always increases. The third law of thermodynamics is that the entropy of a pure crystalline substance at absolute zero is 0. I think just keep these laws in mind...
- Mon Feb 03, 2020 9:48 am
- Forum: Calculating Work of Expansion
- Topic: Midterm Question Involving Integrals
- Replies: 3
- Views: 250
Re: Midterm Question Involving Integrals
I'm not sure, but here's the equations sheet if you want to take a look at it!
https://lavelle.chem.ucla.edu/wp-conten ... ations.pdf
https://lavelle.chem.ucla.edu/wp-conten ... ations.pdf
- Mon Jan 27, 2020 11:04 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Heat Transfer
- Replies: 2
- Views: 162
Re: Heat Transfer
I did heat released by metal = -heat absorbed by water
20.0 x 0.39 x (100-T) = -50.7 x 4.18 x (T-22)
and got T = 24.8 C or about 25 C
20.0 x 0.39 x (100-T) = -50.7 x 4.18 x (T-22)
and got T = 24.8 C or about 25 C
- Mon Jan 27, 2020 10:53 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Standard Enthalpy of Diatomic Gases
- Replies: 4
- Views: 212
Re: Standard Enthalpy of Diatomic Gases
Other examples of diatomic molecules that have zero standard enthalpy include H2, N2, F2, (O2), I2, Cl2, Br2 (Have No Fear Of Ice Cold Beer)
- Mon Jan 27, 2020 10:49 am
- Forum: Phase Changes & Related Calculations
- Topic: revere reactions
- Replies: 7
- Views: 194
Re: revere reactions
To add to that, yes going down a phase is exothermic because from gas to liquid, water would release a great deal of energy. This is the reason for severe steam burns that Dr. Lavelle was talking about last week in class. It's also why sweating (evaporation of liquid water to gas) cools you down bec...
- Mon Jan 27, 2020 10:47 am
- Forum: Phase Changes & Related Calculations
- Topic: Combustion
- Replies: 5
- Views: 186
Re: Combustion
Examples of combustion would occur in this format:
- Mon Jan 27, 2020 10:44 am
- Forum: Phase Changes & Related Calculations
- Topic: Enthalpy w/ Temp
- Replies: 6
- Views: 223
Re: Enthalpy w/ Temp
It makes sense that as temperature increases, so does enthalpy if we refer back to the equation:
delta G = delta H - T(delta S)
delta G = delta H - T(delta S)
- Tue Jan 21, 2020 11:35 am
- Forum: Phase Changes & Related Calculations
- Topic: removing heat from system
- Replies: 6
- Views: 726
Re: removing heat from system
Yes, if a reaction is exothermic, it will always release energy and delta H will always be less than 0.
- Tue Jan 21, 2020 11:33 am
- Forum: Phase Changes & Related Calculations
- Topic: heating curve
- Replies: 3
- Views: 571
Re: heating curve
I believe it's shown in this diagram
- Tue Jan 21, 2020 11:31 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Delta H
- Replies: 10
- Views: 777
Re: Delta H
When delta H is positive, is it endothermic or exothermic? And if H is negative? If delta H is positive, that means the sum of the enthalpy of reactants is LARGER than the sum of the enthalpy of products. This means that the reaction is endothermic, or uses heat. If delta H is negative, the sum of ...
- Tue Jan 21, 2020 11:27 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Heat Capacity Intensive or Extensive?
- Replies: 4
- Views: 676
Re: Heat Capacity Intensive or Extensive?
There is a general rule that thermodynamic properties that are extensive are written in capital letters: V (volume), C (heat capacity), etc. Properties that are intensive are written in lower case. Exceptions are temperature and pressure which are generally represented by upper case letters T and P,...
- Tue Jan 21, 2020 11:20 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: van't hoff's equation
- Replies: 3
- Views: 160
Re: van't hoff's equation
I don't think so either, but in case we do it's this:
- Mon Jan 13, 2020 10:03 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Which liquids to use
- Replies: 7
- Views: 201
Re: Which liquids to use
We never use pure solids (s) or liquids (l) in calculating equilibrium, but we do use gaseous (g) and aqueous (aq) substances. Maybe he was referring to the liquid concentration in the aqueous substance.
- Mon Jan 13, 2020 9:38 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Question from discussion section
- Replies: 2
- Views: 192
Re: Question from discussion section
First find the initial concentrations of A and B by dividing moles of A and B by the overall volume (6L). Then plug this information along with the equilibrium concentration of A into the ICE table. Assuming they give you the equilibrium constant, you should then be able to find x, which will in tur...
- Mon Jan 13, 2020 9:32 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Change in Pressure
- Replies: 6
- Views: 207
Re: Change in Pressure
When the pressure of a system is decreased, a quick way to determine which direction the reaction will shift is seeing which side has the greater number of moles. The side with the greater number of moles will be favored. Conversely, when the pressure of a system is increased, the side with the fewe...
- Mon Jan 13, 2020 9:30 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 5G.9
- Replies: 4
- Views: 176
Re: 5G.9
DesireBrown1J wrote:For c, would the 2nd container with 0.50 mol O3 have a larger ratio of PO2/PO3 because it has a greater overall partial pressure?
I'm not completely sure as I think we would need more information in order to calculate the ratio PO2/PO3
- Mon Jan 13, 2020 9:26 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: K and Q
- Replies: 6
- Views: 353
Re: K and Q
To add to that, by solving for Q and comparing it to K, you can see what direction the reaction will proceed.
If Q<K, the reaction will proceed to the right (products side).
If Q>K, the reaction will proceed to the left (reactants side).
If Q=K, the reaction is at equilibrium.
If Q<K, the reaction will proceed to the right (products side).
If Q>K, the reaction will proceed to the left (reactants side).
If Q=K, the reaction is at equilibrium.
- Thu Jan 09, 2020 1:47 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Value of Kc and Kp
- Replies: 6
- Views: 208
Re: Value of Kc and Kp
Bryce Barbee wrote:Can someone please explain to me how to ask a question on Chem Community. I cannot figure it out. Thanks
Go back one page and scroll to the top. You should see a "new topic" button with a star next to it
- Thu Jan 09, 2020 1:40 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 5G. 3
- Replies: 5
- Views: 171
Re: 5G. 3
For gases, we can use either pressure or concentration (Kp or Kc), but for aqueous solutions, we can only use concentration to find Kc.
- Thu Jan 09, 2020 12:10 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Chemical Activity of a Compound
- Replies: 5
- Views: 151
Re: Chemical Activity of a Compound
The chemical activity of a compound is equal to [compound]/[compound] ° where ° stands for its standard value. This usually cancels out to equal 1. Therefore, we just leave out the chemical activity of a compound when writing out the Kc equation and just use the values for concentration (ignoring th...
- Thu Jan 09, 2020 12:04 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 5G.9
- Replies: 4
- Views: 176
Re: 5G.9
PO2/PO3 will be different because the ratio of the reactant to the product is different at equilibrium point for different amounts of starting reactant.
Only (PO2)^3/(PO3)^2 or (PO3)^2/(PO2)^3 are guaranteed to be the same because they are the equilibrium constant and the inverse of it.
Only (PO2)^3/(PO3)^2 or (PO3)^2/(PO2)^3 are guaranteed to be the same because they are the equilibrium constant and the inverse of it.
- Thu Jan 09, 2020 11:57 am
- Forum: Ideal Gases
- Topic: Review Ideal Gases
- Replies: 6
- Views: 334
- Mon Dec 02, 2019 1:43 am
- Forum: Conjugate Acids & Bases
- Topic: Strength of Conjugate Acids and Bases
- Replies: 3
- Views: 255
Re: Strength of Conjugate Acids and Bases
Similarly, conjugate acids of strong bases are weak.
- Mon Dec 02, 2019 1:41 am
- Forum: Conjugate Acids & Bases
- Topic: conjugate acids/bases
- Replies: 4
- Views: 486
Re: conjugate acids/bases
A conjugate acid is a base with a hydrogen ion added to it.
A conjugate base is what is left over after an acid has donated a proton during a chemical reaction.
A conjugate base is what is left over after an acid has donated a proton during a chemical reaction.
- Mon Dec 02, 2019 1:34 am
- Forum: Polyprotic Acids & Bases
- Topic: Polyprotic acids and bases
- Replies: 2
- Views: 227
Re: Polyprotic acids and bases
Polyprotic acids are acids that can lose more than one proton per molecule in acid-base reactions. Examples: H2SO4, H2CO3 Polyprotic bases are bases that can accept more than one proton per molecule in acid-base reactions. Examples: [SO4]2-, [CO3]2- In titration curves, they will have multiple equiv...
- Mon Dec 02, 2019 1:05 am
- Forum: Amphoteric Compounds
- Topic: Amphoteric Compounds
- Replies: 2
- Views: 110
Re: Amphoteric Compounds
It can only act as an acid or a base one at a time.
An example would be water either accepting or donating a hydrogen ion.
An example would be water either accepting or donating a hydrogen ion.
- Mon Dec 02, 2019 1:03 am
- Forum: Amphoteric Compounds
- Topic: Determining Acidic or Basic
- Replies: 2
- Views: 238
Re: Determining Acidic or Basic
An amphoteric compound can be either an acid or a base, but only one at a time.
It can either accept or donate a hydrogen ion.
It can either accept or donate a hydrogen ion.
- Mon Nov 25, 2019 9:40 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Molecular shape and central atom
- Replies: 3
- Views: 233
Re: Molecular shape and central atom
Here's a diagram to make it easier to visualize
- Mon Nov 25, 2019 9:37 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Molecular shape and central atom
- Replies: 3
- Views: 233
Re: Molecular shape and central atom
To determine its shape from using VSEPR, you would just have to count the number of bonding pairs and lone pairs it has and match it to its corresponding molecular geometry.
- Mon Nov 25, 2019 9:33 am
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: bond order
- Replies: 4
- Views: 389
Re: bond order
It can also be defined as half of the difference between the number of bonding and antibonding electrons.
- Mon Nov 25, 2019 9:31 am
- Forum: Hybridization
- Topic: Examples of Hybridization
- Replies: 2
- Views: 154
Re: Examples of Hybridization
Yes, this is because octahedral structures have 6 electron domains
- Mon Nov 25, 2019 9:29 am
- Forum: Hybridization
- Topic: Are terminal atoms hybridized?
- Replies: 2
- Views: 367
Re: Are terminal atoms hybridized?
In the case of CS2, the S atoms have 1 double bond with C and 2 lone pairs, so it would also have 3 electron domains and yes it would be hybridized to sp2 as well.
As for terminal atoms that are halogens, it just depends again on counting the number of electron domains the atoms have.
As for terminal atoms that are halogens, it just depends again on counting the number of electron domains the atoms have.
- Mon Nov 18, 2019 12:21 am
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3642220
Re: Post All Chemistry Jokes Here
Think like a proton and be positive!
- Mon Nov 18, 2019 12:19 am
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3642220
- Mon Nov 18, 2019 12:18 am
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3642220
Re: Post All Chemistry Jokes Here
What kind of dogs do chemists have?
Laboratory retrievers!
Laboratory retrievers!
- Mon Nov 18, 2019 12:15 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Test 2
- Replies: 6
- Views: 440
Re: Test 2
also it's not cumulative nor will it include hybridization
- Mon Nov 18, 2019 12:04 am
- Forum: Student Social/Study Group
- Topic: Bond Angles
- Replies: 6
- Views: 515
Re: Bond Angles
I believe notating it as <109.5 degrees is fine, but if asked you should still know that H2O has a smaller bond angle because of its 2 lone pair-lone pair repulsions, compared to just 1 in NH3.
- Mon Nov 11, 2019 5:54 pm
- Forum: Student Social/Study Group
- Topic: Chem 14B
- Replies: 10
- Views: 762
Re: Chem 14B
I'm taking chem 14B as well next quarter!
But I heard 14BL is better taken with 14C or after 14C if possible because of the level of knowledge you're expected to know.
But I heard 14BL is better taken with 14C or after 14C if possible because of the level of knowledge you're expected to know.
- Mon Nov 11, 2019 5:48 pm
- Forum: Dipole Moments
- Topic: Dipole Moment
- Replies: 6
- Views: 344
Re: Dipole Moment
To add to that, the arrow always points to the lowercase delta negative sign, and a line strikes through the arrow at the lowercase delta positive sign (making a cross or a "+" to help you remember it)
- Mon Nov 11, 2019 5:30 pm
- Forum: Electronegativity
- Topic: Formula for Difference
- Replies: 7
- Views: 523
Re: Formula for Difference
If anything, the electronegativity values will be given if on a test.
The trends are increasing as you go up a column and also to the right across a period.
The trends are increasing as you go up a column and also to the right across a period.
- Mon Nov 11, 2019 5:28 pm
- Forum: *Liquid Structure (Viscosity, Surface Tension, Liquid Crystals, Ionic Liquids)
- Topic: Bonds vs Shapes [ENDORSED]
- Replies: 4
- Views: 1262
Re: Bonds vs Shapes [ENDORSED]
To add to that, the dipoles can get closer together due to the greater surface area in rod-shaped molecules than spherical-shaped molecules, thus increasing the intermolecular forces.
- Mon Nov 11, 2019 5:24 pm
- Forum: *Liquid Structure (Viscosity, Surface Tension, Liquid Crystals, Ionic Liquids)
- Topic: Polarizability and States
- Replies: 3
- Views: 603
Re: Polarizability and States
The greater the molecular mass, the greater the electron cloud distortion and polarizability. London dispersion forces tend to be stronger between molecules that are easily polarized. Thus, with a higher intermolecular force, the melting point/boiling point will also tend to be higher because more e...
- Tue Nov 05, 2019 12:03 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Why is it 4f14 if there are 15 elements in that row
- Replies: 2
- Views: 1489
Re: Why is it 4f14 if there are 15 elements in that row
Lanthanum is actually the first element of the 5d orbital, cerium through lutetium would be part of the f block
- Mon Nov 04, 2019 12:40 am
- Forum: Electronegativity
- Topic: Electronegativity Ex.
- Replies: 3
- Views: 255
Re: Electronegativity Ex.
HCl has a greater ionic character than HI because hydrogen and chlorine's electronegativity difference is greater than that of hydrogen and iodine.
Remember that electronegativity increases right across a period and up a group!
Remember that electronegativity increases right across a period and up a group!
- Mon Nov 04, 2019 12:34 am
- Forum: Lewis Structures
- Topic: Drawing Lewis Structures
- Replies: 3
- Views: 173
Re: Drawing Lewis Structures
Naji Sarsam 4G wrote:2.) The charge of the central atom especially should either be 0 or negative (because it is the most electronegative atom); preferably 0 though
The central atom should be the least* electronegative atom
- Mon Nov 04, 2019 12:27 am
- Forum: Coordinate Covalent Bonds
- Topic: Single, double, and triple bonds
- Replies: 6
- Views: 244
Re: Single, double, and triple bonds
The greater the electronegativity/electron affinity, the greater the pull on the electrons by the positively charged nucleus. Since fluorine is more electronegative than chlorine, the H-F single bond will be shorter than the H-Cl single bond. And as you increase the # of bonds (double, triple), you ...
- Mon Nov 04, 2019 12:16 am
- Forum: Lewis Structures
- Topic: formal charge
- Replies: 4
- Views: 161
Re: formal charge
It can be calculated through FC = [# of valence electrons on atom] – [(# of lone pair electrons) + (# of shared electrons)/2]
- Mon Nov 04, 2019 12:09 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: Interionic and Intermolecular forces
- Replies: 2
- Views: 249
Re: Interionic and Intermolecular forces
Do you remember if he mentioned it will be covered in the midterm?
- Mon Oct 28, 2019 12:33 am
- Forum: Bond Lengths & Energies
- Topic: Chemical Bonds
- Replies: 4
- Views: 186
Re: Chemical Bonds
Picture yourself on top of a tree: you have high potential energy and are in a very unstable state.
Similarly, atoms don't like having a high potential energy; they'd rather create a bond and be stable at their lowest potential energy state.
Similarly, atoms don't like having a high potential energy; they'd rather create a bond and be stable at their lowest potential energy state.
- Mon Oct 28, 2019 12:27 am
- Forum: Lewis Structures
- Topic: Choosing the central atom
- Replies: 16
- Views: 799
Re: Choosing the central atom
Ionization energy increases as you go up a column and to the right of a period. It's the energy required to remove an electron.
- Mon Oct 28, 2019 12:23 am
- Forum: Electronegativity
- Topic: Fluorine's Electronegativity
- Replies: 6
- Views: 490
Re: Fluorine's Electronegativity
Adding to that, ignoring noble gases, fluorine also has little shielding effect since its electrons are close to the nucleus in the n=2 shell. Thus, the protons in the nucleus have a stronger pull on the electrons than in any other element.
- Mon Oct 28, 2019 12:16 am
- Forum: Electronegativity
- Topic: isoelectronic atoms
- Replies: 2
- Views: 157
Re: isoelectronic atoms
On the contrary, I think that an atom that is isoelectronic with another atom of a fewer number of protons will attract more electrons, thus be more electronegative. Take for example N and F^2+. Although they both each have 7 electrons, fluorine will obviously attract more electrons because there is...
- Mon Oct 28, 2019 12:09 am
- Forum: Ionic & Covalent Bonds
- Topic: Polarity
- Replies: 6
- Views: 277
Re: Polarity
Yes! An example of a polar covalent bond would be water (H2O), where most of the negative charge is from the oxygen on one side of the molecule and the positive charge of the hydrogen atoms is on the other side of the molecule. An example of a nonpolar covalent bond would be carbon dioxide (CO2), wh...
- Mon Oct 21, 2019 12:22 am
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3642220
- Mon Oct 21, 2019 12:20 am
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3642220
- Mon Oct 21, 2019 12:15 am
- Forum: Photoelectric Effect
- Topic: Threshold Energy
- Replies: 7
- Views: 527
Re: Threshold Energy
I think that "ejected" just means that the electron is released from the atom. The detector that is used to measure the KE of the ejected electron has a slightly positive charge, thus causing it to move.
- Mon Oct 21, 2019 12:09 am
- Forum: Photoelectric Effect
- Topic: Video module Test
- Replies: 3
- Views: 183
Re: Video module Test
Or, you could use the combined equations of E=hv and c=v(wavelength) to get (wavelength)=hc/E and solve for wavelength!
Hope that helps :)
Hope that helps :)
- Mon Oct 21, 2019 12:00 am
- Forum: *Shrodinger Equation
- Topic: derivation
- Replies: 5
- Views: 285
Re: derivation
Yupp, his constants and equations sheet can be found on his website or here
https://lavelle.chem.ucla.edu/wp-conten ... ations.pdf
https://lavelle.chem.ucla.edu/wp-conten ... ations.pdf
- Mon Oct 14, 2019 1:38 am
- Forum: Student Social/Study Group
- Topic: Study Group Fall 2019
- Replies: 32
- Views: 2831
Re: Study Group Fall 2019
Count me in! :)
- Mon Oct 14, 2019 1:34 am
- Forum: Student Social/Study Group
- Topic: Grades
- Replies: 18
- Views: 1196
Re: Grades
KayleyW_3L wrote:In addition to wondering when the Test 1 grades will be posted, I am also curious whether there is partial credit on the exams?
I asked my TA and there's definitely partial credit given on exams if you show your work!
- Mon Oct 14, 2019 1:32 am
- Forum: Student Social/Study Group
- Topic: Best Sessions
- Replies: 12
- Views: 481
Re: Best Sessions
Generally in step-up sessions, what's the usual TA to student ratio and about how much time do they spend with each student trying to understand the concepts?
- Mon Oct 14, 2019 1:28 am
- Forum: Student Social/Study Group
- Topic: Textbook Readings
- Replies: 4
- Views: 256
Textbook Readings
Do you guys find the textbook readings to be more helpful for studying or other resources such as videos/lectures? I'm asking because I don't know if I'm missing any important information that's covered in the textbook that's not covered in Dr. Lavelle's videos or lectures. I feel like what tends to...
- Mon Oct 14, 2019 1:15 am
- Forum: Balancing Chemical Reactions
- Topic: H 1
- Replies: 6
- Views: 621
Re: H 1
Another tip is to generally start out balancing the element that shows up the least often in the equation and then work from there, eventually getting to elements in diatomic molecules such as H2 or O2 that stand alone and are easy to balance by themselves (just add a coefficient in front)
- Mon Oct 07, 2019 9:01 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3642220
- Mon Oct 07, 2019 9:01 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3642220
Re: Post All Chemistry Jokes Here
Yes, I am positive!
- Mon Oct 07, 2019 9:00 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3642220
Re: Post All Chemistry Jokes Here
The one true bro
- Mon Oct 07, 2019 8:57 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3642220
Re: Post All Chemistry Jokes Here
Chemistry jokes are sodium funny!
I slapped my neon that one!
I slapped my neon that one!
- Mon Oct 07, 2019 8:30 pm
- Forum: Ideal Gases
- Topic: Reading the textbook
- Replies: 262
- Views: 151624
Re: Reading the textbook
Personally I find that every time I read the textbook, I tend to fall asleep because it's just that long and boring, especially when you're new to the material. What I usually will do however is take notes of the summary and important formulas/equations. Once I have grasped the basic concepts, I wil...
- Fri Oct 04, 2019 12:58 am
- Forum: Properties of Light
- Topic: Speed of Light
- Replies: 41
- Views: 2851
Re: Speed of Light
Speed of light is a constant and will be given during tests/exams.
The link of the constants and equations sheet is on his website but I'll link it here!
https://lavelle.chem.ucla.edu/wp-conten ... ations.pdf
The link of the constants and equations sheet is on his website but I'll link it here!
https://lavelle.chem.ucla.edu/wp-conten ... ations.pdf
- Fri Oct 04, 2019 12:54 am
- Forum: Limiting Reactant Calculations
- Topic: Reviewing High School Chem Tips
- Replies: 10
- Views: 861
Re: Reviewing High School Chem Tips
Honestly chemmybear has a lot of great resources for high school chemistry topics.
I also remember watching a lot of Bozeman videos, he explained the topics in a very easy-to-understand way.
Here are the links below!
http://chemmybear.com/
http://www.bozemanscience.com/ap-chemistry/
I also remember watching a lot of Bozeman videos, he explained the topics in a very easy-to-understand way.
Here are the links below!
http://chemmybear.com/
http://www.bozemanscience.com/ap-chemistry/
- Fri Oct 04, 2019 12:47 am
- Forum: Molarity, Solutions, Dilutions
- Topic: Converting Before or After?
- Replies: 10
- Views: 611
Re: Converting Before or After?
Convert the units first if you're going to be canceling them out with other units. You want to make sure that like units cancel out like units. For example, you would not do 5kg x 1mol/18.02g, you would change the 5kg to 5000g first to make sure you're left with only moles when you cancel out the gr...