Search found 116 matches
- Tue Mar 10, 2020 6:22 pm
- Forum: Administrative Questions and Class Announcements
- Topic: 14B acids and bases section
- Replies: 2
- Views: 229
Re: 14B acids and bases section
Since 14B acids and bases builds upon info from the 14a section, I think it would be useful to review it if necessary.
- Tue Mar 10, 2020 6:19 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: delta g
- Replies: 6
- Views: 420
Re: delta g
I think based on the information you are given. If it isn't as standard temp, use g= delta h - t delta s.
- Tue Mar 10, 2020 6:17 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: reaction mechanism
- Replies: 2
- Views: 184
Re: reaction mechanism
We can predict a potential pathway, but not verify any elementary steps as being the correct ones.
- Tue Mar 10, 2020 6:15 pm
- Forum: Second Order Reactions
- Topic: 2nd Order Slope
- Replies: 2
- Views: 138
Re: 2nd Order Slope
The reverse reaction will be. Since concentration of a reactant decreases as a rxn progresses, 1/[R] will increase.
- Tue Mar 10, 2020 6:13 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Angular dependence
- Replies: 2
- Views: 265
Re: Angular dependence
The angular dependence is taken into account by the pre-exponential factor, A, which you can think of as the likelihood/probability of a rxn happening based on a collision. So when A is large, k is larger, and when A is smaller, k is smaller because k and A are directly related thru the Arrhenius eqn.
- Tue Mar 10, 2020 6:10 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Using Equilibrium constants to predict solubility
- Replies: 4
- Views: 279
Re: Using Equilibrium constants to predict solubility
The relationship btwn K and the constants is K= k/k', which means that when k is high, the rxn favors the products and when k' is high, the rxn favors the reactants.
- Thu Mar 05, 2020 11:43 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: thermodynamically stable
- Replies: 6
- Views: 519
Re: thermodynamically stable
Thermodynamic stability can be identified by looking at delta G. Something stable will be in its lowest energy form and will therefore be unlikely to react.
- Thu Mar 05, 2020 11:39 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Standard Potentials
- Replies: 4
- Views: 325
Re: Standard Potentials
They are based on the reaction with the standard hydrogen electrode.
- Thu Mar 05, 2020 11:39 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Cell potential
- Replies: 6
- Views: 524
Re: Cell potential
It will decrease the concentration. To find out how this affects cell potential, you can plug numbers into E=-RT/nF lnQ with alterations to Q. For instance, if the cathode's concentration decreases, cell potential will increase.
- Thu Mar 05, 2020 11:36 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: same solutions in cell diagram
- Replies: 2
- Views: 215
Re: same solutions in cell diagram
They are in the same solution when they are all at either the anode or cathode. Commas denote same side and state. The straight line refers to different phases.
- Thu Mar 05, 2020 11:33 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Electrode masses
- Replies: 8
- Views: 580
Re: Electrode masses
If you increase the mass of electrodes the battery will have a longer lifetime. Cell potential will not change
- Thu Feb 27, 2020 11:10 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 6L.5 part d
- Replies: 2
- Views: 213
Re: 6L.5 part d
Au (s) is the electrode. Even though it is submerged in solution, it has not dissociated and is therefore is solid.
- Thu Feb 27, 2020 11:08 pm
- Forum: Balancing Redox Reactions
- Topic: Direction of Reaction
- Replies: 3
- Views: 262
Re: Direction of Reaction
Based on Q in the Nernst equation. If [P] > [R] then Ecell is negative. If [P] < [R] then Ecell is positive
- Thu Feb 27, 2020 10:56 pm
- Forum: Balancing Redox Reactions
- Topic: 6K. 5b
- Replies: 3
- Views: 323
Re: 6K. 5b
Balance the electrons in the oxidation reaction because the stoichiometric coefficient applies to the # of e- as well
- Thu Feb 27, 2020 10:23 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Electrolyte
- Replies: 4
- Views: 299
Re: Electrolyte
An electrolyte is a salt like KOH or NaCl. It completely ionizes in solution
- Thu Feb 27, 2020 10:20 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 6L7 (b) HW
- Replies: 3
- Views: 277
Re: 6L7 (b) HW
Yeah I was a bit confused about how the oxidation numbers don't change, but it can be broken down to reduction and oxidation half reactions: reduction: 4e- + O2 + 2H2O --> 4OH- oxidation: 2H2O --> 4H+ + O2 + 2e- How do we know that O2 is involved? Like why is it not Red: 2H+ + 2e- -> H2 Oxid: 2OH- ...
- Thu Feb 27, 2020 9:15 pm
- Forum: Balancing Redox Reactions
- Topic: Acidic/Basic Solutions
- Replies: 3
- Views: 243
Re: Acidic/Basic Solutions
I believe we will be given that information.
- Sun Feb 23, 2020 10:29 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: platinum
- Replies: 4
- Views: 274
Re: platinum
Platinum is inert and won't interfere w the redox rxn. Other inert materials could be used as well, such as graphite.
- Sun Feb 23, 2020 10:24 am
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: n
- Replies: 13
- Views: 785
Re: n
Which eqn are you referring to? N is the number of moles, not R.
- Sun Feb 23, 2020 10:08 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: standard conditions
- Replies: 8
- Views: 565
Re: standard conditions
all solutes present at 1 mol/L and all gases at 1 bar
- Sun Feb 23, 2020 10:06 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Positive Voltage
- Replies: 2
- Views: 211
Re: Positive Voltage
Yes, because its positive value means that delta G will be negative, therefore the rxn is spontaneous. If the standard potential is negative, that means the reverse rxn is spontaneous.
- Sun Feb 23, 2020 10:01 am
- Forum: Balancing Redox Reactions
- Topic: Oxidation States
- Replies: 7
- Views: 419
Re: Oxidation States
Elements in Groups 1, 2, 6, and 7 generally will carry the same oxidation state as the charge of the cation/anion they form. Therefore, assigning their oxidation states first allows us to find the oxidation state of an unknown oxidation state. Also, knowing the charges of polyatomic cations and anio...
- Sat Feb 15, 2020 9:58 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Enthalpy
- Replies: 26
- Views: 1232
Re: Enthalpy
A state function relies on initial and final values, not the pathway taken.
- Sat Feb 15, 2020 9:46 pm
- Forum: Calculating Work of Expansion
- Topic: work = 0
- Replies: 14
- Views: 1349
Re: work = 0
In a vacuum, there is nothing to push against, therefore no work is performed.
- Sat Feb 15, 2020 9:42 pm
- Forum: Van't Hoff Equation
- Topic: Van't Hoff Equation
- Replies: 4
- Views: 265
Re: Van't Hoff Equation
The T cancels because it is in both numerator and denominator
- Sat Feb 15, 2020 9:42 pm
- Forum: Van't Hoff Equation
- Topic: Constant
- Replies: 3
- Views: 170
Re: Constant
A good way to figure out which R to use it to see what units you need to cancel in order to get the desired units
- Sat Feb 15, 2020 9:40 pm
- Forum: Calculating the pH of Salt Solutions
- Topic: How do you know if something is a salt solution?
- Replies: 6
- Views: 738
Re: How do you know if something is a salt solution?
A salt will dissociate into its constituent ions in water, so the ion that is an acid or base will act the same way as a normal acid/base and you will solve it the same way.
- Sat Feb 15, 2020 9:35 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Equilibrium
- Replies: 15
- Views: 834
Re: Equilibrium
At equilibrium, the system does not have a preference for the forward or reverse rxn, so neither would spontaneously occur
- Wed Feb 12, 2020 9:57 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Bond Enthalpy
- Replies: 2
- Views: 195
Re: Bond Enthalpy
Reactants have their bonds broken, which is endothermic, so it is positive. Products have their bonds formed, which is exothermic, thus negative.
- Mon Feb 10, 2020 12:43 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: 4C.3
- Replies: 1
- Views: 56
Re: 4C.3
they give you the value for q, you can find Cv and Cp from the ideal gas heat capacity eqn, and you're given Ti, so you're just solving for Tf.
- Mon Feb 10, 2020 12:38 am
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Intensive Property
- Replies: 3
- Views: 124
Re: Intensive Property
Heat capacity is an intensive property because it depends on the amount of matter that you start with. Heat capacity is defined as the energy that it takes to raise 1mol of substance by 1 degree c, and it takes more energy to raise 1 mol of a complex molecule by 1 degree C than it does a simple one...
- Mon Feb 10, 2020 12:37 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: 4D.3
- Replies: 2
- Views: 186
Re: 4D.3
Use the qcal= Ccal x delta T to get q, which is delta U because delta U is equal to q at constant volume
- Mon Feb 10, 2020 12:36 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: HW 4D7
- Replies: 4
- Views: 156
Re: HW 4D7
For gases, the change in enthalpy is defined by that equation. This is because when gas is produced work is done to clear the other gases so the enthalpy is lower than the internal energy. This is explained in detail on pg 274 in the textbook (4D.2) Where does that formula come from? Shouldn't nRT ...
- Mon Feb 10, 2020 12:34 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: when to change sign of enthalpies
- Replies: 7
- Views: 406
Re: when to change sign of enthalpies
Flipping the sign accounts for flipping the equation because we have changed from an endo to exo or exo to endo rxn.
- Mon Feb 10, 2020 12:32 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: gas constant
- Replies: 3
- Views: 134
Re: gas constant
Use the gas constant that properly aligns with those units.
- Mon Feb 10, 2020 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: standard entropy meaning
- Replies: 3
- Views: 208
Re: standard entropy meaning
standard entropy is entropy at standard conditions, which is at a chosen temp (generally 25)
- Mon Feb 10, 2020 12:31 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Midterm Review #12b
- Replies: 4
- Views: 293
Re: Midterm Review #12b
would the enthalpies for the reactants and products in steps 1 and 3 be both positive? or would reactants be positive and products be negative? if the calculation for q in step 1 is positive because final temp is higher than initial and in step 3 it is negative because final temp is lower than init...
- Mon Feb 10, 2020 12:27 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: % dissociation
- Replies: 5
- Views: 373
Re: % dissociation
Calculate the amount of H+ and divide by orginal amount of acid then multiply by 100
- Wed Feb 05, 2020 11:10 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: 4f.13
- Replies: 1
- Views: 97
Re: 4f.13
351.5K is the BP temp of ethanol, so you only have to calculate the entropy at the phase change, so delta S = delta H of vap / T at BP
- Wed Feb 05, 2020 9:03 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: enthalpy of formation
- Replies: 2
- Views: 122
Re: enthalpy of formation
Yes because all atoms that form diatomic molecules are in those molecules under standard conditions.
- Wed Feb 05, 2020 9:01 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: 4F.9
- Replies: 2
- Views: 131
Re: 4F.9
P and V have an inverse relationship
- Wed Feb 05, 2020 9:00 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: Microstates
- Replies: 7
- Views: 219
Re: Microstates
microstates/degeneracy is the number of positions a molecule/atom can occupy.
- Wed Feb 05, 2020 8:58 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: 4F.1a
- Replies: 4
- Views: 176
Re: 4F.1a
Maggie Eberhardt - 2H wrote:can someone explain to me how the answer to this problem (0.341 J/Kxs) is positive even though the equation you use to solve it is -(rate of heat generation)/temperature = -100/293???
The body is generating heat, so delta H is positive for the surroundings.
- Thu Jan 30, 2020 10:15 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Enthalpy Unit
- Replies: 6
- Views: 193
Re: Enthalpy Unit
No, other units can represent it, but we use kJ by convention.
- Thu Jan 30, 2020 10:12 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: qp and qv
- Replies: 8
- Views: 383
Re: qp and qv
When volume is not constant, the gas is either expanding or compressing, so there is some work done. Therefore, that energy from work contributes to the delta H and must be factored in.
- Thu Jan 30, 2020 10:08 pm
- Forum: Phase Changes & Related Calculations
- Topic: standard reaction enthalpy vs. standard enthalpy of formation
- Replies: 7
- Views: 1080
Re: standard reaction enthalpy vs. standard enthalpy of formation
Reaction enthalpy is the enthalpy of the overall reaction, while enthalpy of formation corresponds to a specific element.
- Thu Jan 30, 2020 10:06 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Calorimeter
- Replies: 4
- Views: 252
Re: Calorimeter
The heat released by the chemical reaction will be equal to the heat absorbed by the calorimeter. So,
(mass of calorimeter) x (C of calorimeter) x (change in temp) = (mass of substance) x (Cs) x (change in temp)
(mass of calorimeter) x (C of calorimeter) x (change in temp) = (mass of substance) x (Cs) x (change in temp)
- Thu Jan 30, 2020 2:00 pm
- Forum: Calculating Work of Expansion
- Topic: Work equation
- Replies: 5
- Views: 203
Re: Work equation
Since energy is used to do work, the system is losing energy, and that loss is represented by the minus sign.
- Tue Jan 21, 2020 8:11 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: pKa, Ka, and strength of acid
- Replies: 3
- Views: 110
Re: pKa, Ka, and strength of acid
Since Ka is the ratio of products to reactants, and a product is H3O+, when the concentration of H3O+ is higher, the Ka will be higher.
- Tue Jan 21, 2020 8:08 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Temperature
- Replies: 2
- Views: 136
Re: Temperature
Endothermic:
R + heat <-> P
Exothermic:
R <-> P + heat
Adding heat in an endothermic rxn will push it right, and adding heat in an exothermic rxn will push it left
R + heat <-> P
Exothermic:
R <-> P + heat
Adding heat in an endothermic rxn will push it right, and adding heat in an exothermic rxn will push it left
- Tue Jan 21, 2020 8:04 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: partial pressure
- Replies: 5
- Views: 282
Re: partial pressure
There is also Pa or kPa, which has a more significant difference. I think if it is necessary to convert we will be given the conversion factor.
- Tue Jan 21, 2020 8:03 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Calculator
- Replies: 4
- Views: 192
Re: Calculator
I think they want us to have a non-programmable calculator, so any scientific calculator would be safe to bring.
- Tue Jan 21, 2020 8:02 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: 6B.9
- Replies: 2
- Views: 90
Re: 6B.9
Yes, whenever the H+/OH- concentration is greater than 1, pH/pOH will be negative
- Tue Jan 14, 2020 10:12 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Kw
- Replies: 16
- Views: 459
Re: Kw
Both, as they refer to the same thing.
- Tue Jan 14, 2020 10:11 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: When to approximate
- Replies: 5
- Views: 161
Re: When to approximate
We should be able to approximate in binomials as well. If you approximate it or solve it fully out, you get the same value.
- Tue Jan 14, 2020 10:05 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Autoprotolysis
- Replies: 8
- Views: 242
Re: Autoprotolysis
ELu 1J wrote:It occurs naturally and emphasizes the amphoteric nature of water (the ability to both give and accept a proton).
The ability to accept and donate a proton is amphiprotic, while amphoteric is the ability to react with both acids and bases. :)
- Tue Jan 14, 2020 9:57 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 5.H.3
- Replies: 3
- Views: 180
Re: 5.H.3
You would multiply the Ks of the two reactions that form the given reaction since you can think of their separate eq constants being combined into one equilibrium constant.
- Tue Jan 14, 2020 9:55 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 5I.19
- Replies: 2
- Views: 113
Re: 5I.19
To solve this problem, you need to make an ICE table. The initial concentrations of H2 and I2 can be found by dividing the number of moles by the volume of the flask. Then, we can find H2's equilibrium concentration by multiplying its initial value by 0.6. If we say that the concentration of H2 chan...
- Sat Jan 11, 2020 9:48 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Change in pressure
- Replies: 5
- Views: 272
Re: Change in pressure
When pressure is increased due to compression (volume of container being changed), the equilibrium will shift to the side with less moles. If pressure is increased by adding a gas not involved in the reaction, the equilibrium will not change (as the concentrations of the gases involved in the rxn ar...
- Sat Jan 11, 2020 9:42 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Response of Equilibria to Change
- Replies: 3
- Views: 231
Re: Response of Equilibria to Change
The concentration is the real reason why it is affected. When pressure increases, volume decreases, so concentration increases. For example, if pressure is doubled, then volume is Concentration=moles/(1/2)V=2mol/V. So, in this case, concentration would be doubled.
- Sat Jan 11, 2020 9:36 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Thermodynamically Stable
- Replies: 3
- Views: 173
Re: Thermodynamically Stable
A quick way to determine which is more stable is to compare the K values: if K is high products are favored, and when K is low, reactants are favored. Whichever has a lower K value would favor the reactants more so than the other.
- Sat Jan 11, 2020 9:34 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 5G.9
- Replies: 3
- Views: 120
Re: 5G.9
There would be different amounts of O2 and O3 because of the different concentrations. This ratio does not refer to the eq. constant, so they would not be the same.
- Sat Jan 11, 2020 9:32 pm
- Forum: Ideal Gases
- Topic: Units of Pressure
- Replies: 8
- Views: 299
Re: Units of Pressure
Most likely the value we need will be provided, just check that the units in the constant match up with the pressure unit.
- Thu Dec 05, 2019 2:05 pm
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: determining stronger acid
- Replies: 1
- Views: 125
Re: determining stronger acid
Yes, there is a periodic trend insofar as electronegativity and atomic size play a role. Larger atoms bonded to H have weaker bonds, so they are stronger acids.
- Thu Dec 05, 2019 2:03 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Polydentate Ligands
- Replies: 2
- Views: 184
Re: Polydentate Ligands
A ligand is polydentate if it can bind to a metal atom at more than one location. The best way to figure this out would be looking at the Lewis structure and seeing if it could orient itself in such a way that makes multiple bonds possible. For example, H2O is monodentate because its bent structure ...
- Thu Dec 05, 2019 2:01 pm
- Forum: Lewis Acids & Bases
- Topic: Equilibrium Arrows for Acid/Base
- Replies: 1
- Views: 101
Re: Equilibrium Arrows for Acid/Base
When it is a strong acid or base, use a one-way arrow because it completely dissociates. With weak acids and bases, there is both dissociation and formation occurring, so use a two way arrow.
- Thu Dec 05, 2019 2:00 pm
- Forum: Air Pollution & Acid Rain
- Topic: Acid rain
- Replies: 2
- Views: 261
Re: Acid rain
carbon dioxide + water -> carbonic acid
CO2 (g) + H2O (l) -> H2CO3 (aq)
sulfur dioxide and nitrogen oxides can also lead to acid rain:
SO2 + H2O -> H2SO4
2NO2 + H2O -> HNO3 + HNO2
CO2 (g) + H2O (l) -> H2CO3 (aq)
sulfur dioxide and nitrogen oxides can also lead to acid rain:
SO2 + H2O -> H2SO4
2NO2 + H2O -> HNO3 + HNO2
- Thu Dec 05, 2019 1:56 pm
- Forum: Conjugate Acids & Bases
- Topic: Hydrogen Question
- Replies: 2
- Views: 217
Re: Hydrogen Question
Not necessarily, removal of one hydrogen is the conjugate base of an acid. For instance, H2CO3 has the conjugate bases HCO3- and CO3 2-
- Thu Dec 05, 2019 1:55 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: coordination number
- Replies: 6
- Views: 244
Re: coordination number
I generally approach these problems by first identifying what ligands are in the coordinate sphere, so for (a), the ligand is chlorine. Since we know that Cl has a -1 charge and that there are four of them, that means the charge of nickel plus the charge of the chlorines will equal the charge of the...
- Sun Dec 01, 2019 7:36 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Weak vs. Strong Acids
- Replies: 3
- Views: 102
Re: Weak vs. Strong Acids
The strength or weakness of an acid depends on how much it dissociates in solution. When it does not 100% dissociate, it is not a strong acid or strong base.
- Sun Dec 01, 2019 7:34 pm
- Forum: Conjugate Acids & Bases
- Topic: Difference
- Replies: 2
- Views: 175
Re: Difference
A conjugate acid is when a base takes a H+ ion and a conjugate base forms when an acid loses its H+ ion
- Sun Dec 01, 2019 7:31 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: coordinate bonds
- Replies: 1
- Views: 120
Re: coordinate bonds
Yes, if a lone pair is covalently bonded to another atom, then both electrons being shared come from the same atom, and therefore it is a coordinate covalent bond.
- Sun Dec 01, 2019 7:22 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: pH of Weak Acid and Bases
- Replies: 4
- Views: 355
Re: pH of Weak Acid and Bases
We can find the pH of a weak acid or base using its Ka or Kb value. Use the equilibrium equation to solve for the concentration of H+. Then, take the -log of that concentration.
The equilibrium expression would look like this:
Ka= [H+][A-] / [HA]
The equilibrium expression would look like this:
Ka= [H+][A-] / [HA]
- Sun Dec 01, 2019 7:14 pm
- Forum: Lewis Acids & Bases
- Topic: Lewis v. Bronsted
- Replies: 2
- Views: 124
Re: Lewis v. Bronsted
The Bronsted definition refers to the donation or acceptance of a H+ ion while the Lewis definition refers to the donation or acceptance of an electron pair. In this way, the Lewis definition is much broader and can include other species like transition metals being oxidized and reduced, while the B...
- Mon Nov 25, 2019 11:45 pm
- Forum: Sigma & Pi Bonds
- Topic: Unhybridized Orbital vs Spin Pair?
- Replies: 8
- Views: 484
Re: Unhybridized Orbital vs Spin Pair?
Also, the unhybridizied orbital is lower energy than the hybridized orbital, and electrons will go to the lowest energy state possible.
Re: 9C3d
The OH2 is just to emphasize that the lone pair on the oxygen atom is what is coordinate to the central metal atom. Both are technically correct though.
- Tue Nov 19, 2019 2:42 pm
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: H2SeO4
- Replies: 2
- Views: 163
Re: H2SeO4
Tetrahedral shapes will never be nonpolar if there are different atoms bonded, even though the way we draw it in 1D makes it seem like it.
- Tue Nov 19, 2019 2:40 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Question 2F3 part b
- Replies: 3
- Views: 217
Re: Question 2F3 part b
I think that both the structure w/ two double bonds and the structure w/ one double bond and one single bond are acceptable, so they are just giving answers for both.
- Tue Nov 19, 2019 9:09 am
- Forum: Lewis Structures
- Topic: Octet Rule
- Replies: 7
- Views: 658
Re: Octet Rule
Formal charge is an indicator of stability, so considering the formal charge of a bonded atom is useful in determining whether or not it will break the octet rule. If breaking the octet rule results in a FC=0, it is likely more stable, and therefore more likely to be the correct lewis structure.
- Tue Nov 19, 2019 9:07 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: States and Intermolecular forces
- Replies: 4
- Views: 301
Re: States and Intermolecular forces
Yes, solids have higher intermolecular forces, which is why we can think of the molecules composing a solid as being held together more tightly than those of a liquid or gas. A good way to remember this is to think about the Halogens and how F, the least polarizable of the group, is a gas, while Iod...
- Tue Nov 19, 2019 9:01 am
- Forum: Electronegativity
- Topic: H-bonding Question
- Replies: 2
- Views: 247
Re: H-bonding Question
Yes, because of the alcohol group, there is H-bonding. For a molecule to have H-bonding, hydrogen must be bonded to O, N, or F, and those atoms must also have a lone pair.
- Thu Nov 14, 2019 2:37 pm
- Forum: Dipole Moments
- Topic: question 3f.5
- Replies: 3
- Views: 209
Re: question 3f.5
Since Iodine is bigger, it has more electrons and outer valence electrons experience shielding from the positively charged nucleus. Thus, iodine is more polarizable than chlorine. This trend holds true as you move down the group. For BP, intermolecular attractions are more important than intramolecu...
- Thu Nov 14, 2019 2:33 pm
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: How to remember strength of different intermolecular forces
- Replies: 5
- Views: 829
Re: How to remember strength of different intermolecular forces
You can make a visual model of the intermolecular attractions by drawing the Lewis structures. Based on how close the electrons or nucleus of one molecule/atom can get to another nucleus or electron pair, you can distinguish what will be stronger. For instance, H forms Hydrogen bonds with lone pairs...
- Thu Nov 14, 2019 2:29 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Electrons
- Replies: 9
- Views: 482
Re: Electrons
Emma Joy Schaetz 1E wrote:Is this always true?
Yes, this is always true, as electrons will always be negatively charged and thus repel one another. Minimizing repulsion will always result in more stability.
- Wed Nov 13, 2019 10:39 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR usage
- Replies: 5
- Views: 339
Re: VSEPR usage
Yes, molecular shape affects intermolecular interactions, as it influences how closely together they can get, or how close another molecule or atom can get to the central atom. For example, linear molecules can pack more closely together than tetrahedrals. Also, if a central atom is attached to four...
- Wed Nov 13, 2019 10:33 pm
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: dipole moment clarification
- Replies: 6
- Views: 381
Re: dipole moment clarification
Dipole moments are describing intermolecular forces. As the electron distribution in one molecule forms areas of partial negative charge and areas of partial positive charge, it influences the partial charges in another molecule due to repulsive forces. Polar molecules have a permanent dipole, there...
- Sat Nov 09, 2019 1:02 pm
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: instantaneous dipoles
- Replies: 3
- Views: 246
Re: instantaneous dipoles
Number of electrons and shape of the molecule are often interrelated, as a molecule with more electrons will be larger. When comparing electrons with similar numbers of electrons, then shape will likely be a determining factor.
- Sat Nov 09, 2019 12:57 pm
- Forum: Resonance Structures
- Topic: 2.7 - How to determine main structure if formal charges are equal?
- Replies: 2
- Views: 116
Re: 2.7 - How to determine main structure if formal charges are equal?
Usually, it is best to have differing FC side by side (like a -1 next to +1) rather than the same FC side by side (like +1 next to +1) because it is unlikely that there would be two same charge centers in close proximity due to repulsive forces.
- Sat Nov 09, 2019 10:06 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: 3F.1
- Replies: 1
- Views: 155
Re: 3F.1
The central Se atom is single bonded to two OH groups and double bonded to two O. The OH groups will be polar w/ partial positives on H and partial negatives on O. Also, since the electron distribution is different for the single and double bonds, some areas on the molecule will “concentrate” more e...
- Sat Nov 09, 2019 9:55 am
- Forum: Dipole Moments
- Topic: Hydrogen Bonds
- Replies: 6
- Views: 343
Re: Hydrogen Bonds
Since it is bonded to N, O, or F, which are highly electronegative, H’s one electron will be pulled away from it. So that means H is basically just a proton and therefore negatively charged atoms will be highly attracted to it.
- Tue Nov 05, 2019 7:59 pm
- Forum: Electronegativity
- Topic: Homework Question 2D.5 Part a
- Replies: 2
- Views: 117
Re: Homework Question 2D.5 Part a
Larger atoms in bonds have more covalent character than smaller atoms (due to shielding and distance from nucleus increase). Since Iodine is larger, HI will have more covalent character.
- Thu Oct 31, 2019 2:20 pm
- Forum: Electronegativity
- Topic: Electronegativity difference
- Replies: 2
- Views: 141
Re: Electronegativity difference
If we are expected to use exact electronegativities, I believe the values will be provided. Without those values, we can make assumptions as to the electronegativities of atoms based on periodic trends. As you move up and right, electronegativity increases. Therefore, we can assume the electronegati...
- Thu Oct 31, 2019 2:16 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: Help with Textbook problem G.7
- Replies: 1
- Views: 253
Re: Help with Textbook problem G.7
Multiply the percent of KNO3 by the total mass of the solution:
510 x 0.0545 = 27.8 g KNO3
Since the components of the solution are KNO3 and water, the remaining mass will be that of water.
510-27.8= 482.2g H2O
510 x 0.0545 = 27.8 g KNO3
Since the components of the solution are KNO3 and water, the remaining mass will be that of water.
510-27.8= 482.2g H2O
- Thu Oct 31, 2019 2:13 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charge
- Replies: 4
- Views: 201
Re: Formal Charge
No, charge will always be a whole number. Whenever we divide by two in the FC equation, the numerator will be an even number, as it refers to pairs of electrons.
- Thu Oct 31, 2019 2:10 pm
- Forum: Lewis Structures
- Topic: 2B.7
- Replies: 2
- Views: 134
Re: 2B.7
Using formal charge is a helpful way to confirm the identity of E, as we know that an element w/ 5 VE is likely to be the central atom. We could also subtract the electrons accounted for by Cl and O from the total # of electrons and be left with 5 electrons. Since we are told that E is in period 3, ...
- Thu Oct 31, 2019 2:02 pm
- Forum: Lewis Structures
- Topic: Radical
- Replies: 2
- Views: 104
Re: Radical
Species with an odd number of electrons have an unpaired electron. Take CH3 for example: there are 7 electrons total, so carbon will have 3 pairs and 1 single electron. This, by definition, makes it a radical. The converse is true, as even numbers of electrons form pairs.
- Wed Oct 23, 2019 7:43 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: 2A.5
- Replies: 4
- Views: 183
Re: 2A.5
I believe the same thing happens for part d because the 6 s and p orbitals are farther from the nucleus and are therefore more "loosely" held. So when it becomes an ion, electrons are lost from there first.
- Wed Oct 23, 2019 7:35 pm
- Forum: Electronegativity
- Topic: Electronegativity
- Replies: 14
- Views: 665
Re: Electronegativity
Electronegativity also decreases down the periodic table because as more shells are added, the more distant the positive nucleus is from other electrons it would attract; thus the electrostatic forces of attraction are weaker.
- Wed Oct 23, 2019 7:21 pm
- Forum: Photoelectric Effect
- Topic: Hw Help 1B.5
- Replies: 1
- Views: 92
Re: Hw Help 1B.5
Electron diffraction gives evidence that EM radiation acts like a wave instead of a particle. Black body radiation and the atomic spectra both give evidence that energy is emitted/absorbed discretely (thus evidence of particle nature), however the photoelectric effect is what confirmed that EM radia...
- Wed Oct 23, 2019 7:14 pm
- Forum: Lewis Structures
- Topic: Number of valence electrons
- Replies: 3
- Views: 179
Re: Number of valence electrons
Elements in the third period and after generally have exceptions to the octet rule where they can take on more electrons than eight. However, prior to that, H and He will not follow the octet rule, but rather the "duet rule" because they will only try to fill up their s orbital. Boron also...