Search found 101 matches
- Sat Mar 14, 2020 7:33 pm
- Forum: General Rate Laws
- Topic: average rate
- Replies: 4
- Views: 384
Re: average rate
The negative just means that the reactant concentration is decreasing over time, which makes sense given that they are consumed as the reaction progresses.
- Sat Mar 14, 2020 7:32 pm
- Forum: General Rate Laws
- Topic: Factors Affecting k
- Replies: 83
- Views: 7692
Re: Factors Affecting k
Generally, k increases with temperature.
- Sat Mar 14, 2020 7:32 pm
- Forum: General Rate Laws
- Topic: rate laws
- Replies: 8
- Views: 703
Re: rate laws
Yes, the overall rate would depend on the slowest step.
- Sat Mar 14, 2020 6:49 pm
- Forum: General Rate Laws
- Topic: integrals and derivatives
- Replies: 7
- Views: 632
Re: integrals and derivatives
I don't believe any derivations or integrals will be tested; the formulas are all provided on the equation sheet.
- Sat Mar 14, 2020 5:46 pm
- Forum: General Rate Laws
- Topic: half life
- Replies: 5
- Views: 473
Re: half life
You would use the same integrated rate law depending on the order of reaction and set concentration to 1/4, 1/8, etc. of the initial concentration and solve for t.
- Thu Mar 05, 2020 10:05 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Electromotive force (emf)
- Replies: 9
- Views: 671
Electromotive force (emf)
Can someone explain what emf is exactly and if we need to know anything about it other than that it represents max work?
- Thu Mar 05, 2020 10:04 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: max work and cell potential
- Replies: 3
- Views: 270
Re: max work and cell potential
Assuming temperature and pressure are constant, work can only be done electrochemically. In this case, max work can be calculated as the amount of charge (signified by nF, moles of electrons*charge in coulombs per one mole of electrons) multiplied by the potential difference they are traveling acros...
- Thu Mar 05, 2020 10:02 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: reduction and oxidation
- Replies: 4
- Views: 308
Re: reduction and oxidation
Whichever species has the higher positive standard reduction potential will act as the oxidizing agent and be reduced.
- Thu Mar 05, 2020 10:01 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Temperature
- Replies: 2
- Views: 237
Re: Temperature
If the reaction is exothermic, increasing the temperature will decrease K, and if the reaction is endothermic, increasing the temperature will increase K.
- Thu Mar 05, 2020 10:00 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: lnQ vs logQ
- Replies: 5
- Views: 404
Re: lnQ vs logQ
I think both of these equations can basically be used interchangeably.
- Wed Feb 26, 2020 12:01 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Standard Cell Potential
- Replies: 4
- Views: 313
Re: Standard Cell Potential
Eo is under standard conditions, while E changes as the reaction progresses.
- Mon Feb 24, 2020 9:26 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Eo as an intensive property
- Replies: 9
- Views: 676
Re: Eo as an intensive property
Because intensive properties do not change when amount of substance is changed, this is most relevant when it comes to balancing redox reactions. Multiplying an entire half reaction by any constant does not change Eo.
- Mon Feb 24, 2020 9:24 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Galvanic vs. electrolytic
- Replies: 4
- Views: 332
Re: Galvanic vs. electrolytic
In a galvanic cell, electrons flow spontaneously, but in an electrolytic cell, electrical energy drives electron flow in the opposite direction (nonspontaneous).
- Mon Feb 24, 2020 9:22 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Maximum Potential and Voltage
- Replies: 6
- Views: 457
Re: Maximum Potential and Voltage
The value for the maximum electrical potential difference between the cathode and anode is the voltage of the cell.
- Mon Feb 24, 2020 9:18 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Flow of Galvanic cell
- Replies: 3
- Views: 220
Re: Flow of Galvanic cell
Cations from the salt bridge travel to the solution surrounding the cathode, not the cathode itself, in order to balance out the negative charge buildup in solution as positive cations are precipitated out of the solution. Otherwise, buildup of charge would prevent electrons from flowing through the...
- Mon Feb 24, 2020 9:13 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Galvanic/voltaic cell
- Replies: 6
- Views: 499
Re: Galvanic/voltaic cell
All galvanic cells are electrochemical cells; a galvanic cell specifically refers to an electrochemical cell in which a voltage difference across a cathode/anode drives a spontaneous redox reaction.
- Tue Feb 18, 2020 12:12 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Equilibrium
- Replies: 15
- Views: 843
Re: Equilibrium
Delta G is zero at equilibrium because the concentrations of products and reactants are not changing and neither the forward nor reverse reaction is favored; given that the system isn't doing work, there is nothing that would cause a change in free energy of the system.
- Tue Feb 18, 2020 12:10 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: delta G vs. delta G naught
- Replies: 6
- Views: 462
Re: delta G vs. delta G naught
Delta G naught is a constant for a given chemical equation (measured under standard conditions) while delta G changes as the reaction progresses and conditions change.
- Tue Feb 18, 2020 12:09 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: 5G.17
- Replies: 2
- Views: 227
Re: 5G.17
As the reaction progresses, I is being converted to I2, which is shown as [I] decreases as [I2] increases proportionally. Eventually, once the system reaches equilibrium, the concentrations of the reactants and products remain constant.
- Tue Feb 18, 2020 12:06 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: importance of -RTlnk
- Replies: 7
- Views: 491
Re: importance of -RTlnk
∆Gº=-RTlnK is derived from the equation ∆G = ∆Gº + RT lnQ; if the reaction is at equilibrium and no work is being done, ∆G is equal to zero and Q=K which is where the equation comes from.
- Tue Feb 18, 2020 12:02 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: ∆G = ∆Gº + RT lnQ
- Replies: 12
- Views: 2676
Re: ∆G = ∆Gº + RT lnQ
∆Gº refers to change in Gibbs free energy under standard conditions (usually this value will be given)
∆G refers to change in Gibbs free energy for the system (this is usually what we will be calculating for)
∆G refers to change in Gibbs free energy for the system (this is usually what we will be calculating for)
- Sat Feb 15, 2020 11:56 am
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Delta U = 0
- Replies: 8
- Views: 559
Re: Delta U = 0
Any time there is no change in temperature, delta U is zero.
- Sat Feb 15, 2020 11:54 am
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Negative work
- Replies: 14
- Views: 976
Re: Negative work
When a system does work, it loses energy in the process, so the value for w is negative.
- Sat Feb 15, 2020 11:53 am
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Meaning of q=-w
- Replies: 14
- Views: 2409
Re: Meaning of q=-w
When the change in internal energy is zero, it means that all the heat added to the system must be used by the system to do work.
- Sat Feb 15, 2020 11:52 am
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Intensive and Extensive Properties
- Replies: 8
- Views: 1899
Re: Intensive and Extensive Properties
Extensive properties depend on the amount of substance (heat capacity) while intensive properties are applicable to the substance in general (specific heat)
- Sat Feb 15, 2020 11:48 am
- Forum: Calculating Work of Expansion
- Topic: Positive or negative work
- Replies: 15
- Views: 2202
Re: Positive or negative work
Generally we refer to everything from the perspective of the system, which means that positive work means that work is being done on the system. You can also think of doing work ON some system as adding energy to it, so it makes sense that work is positive.
- Tue Feb 04, 2020 8:07 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: question on lecture notes about closed system
- Replies: 5
- Views: 217
Re: question on lecture notes about closed system
It is important to note that the beaker does not insulate because this ensures that transfer of heat can still occur (otherwise it would be an isolated system).
- Tue Feb 04, 2020 7:59 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: closed vs isolated
- Replies: 14
- Views: 505
Re: closed vs isolated
The main difference is that heat exchange can still occur in a closed system but not in an isolated system.
- Tue Feb 04, 2020 7:58 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Work done BY vs work done ON
- Replies: 9
- Views: 321
Re: Work done BY vs work done ON
When work is done BY a system, it is using energy in order to do the work, so w is negative. When work is done ON a system, the system absorbs energy so w is positive.
- Tue Feb 04, 2020 7:57 pm
- Forum: Calculating Work of Expansion
- Topic: second equation
- Replies: 8
- Views: 280
Re: second equation
In this case, the only time you would need to integrate would be if asked to derive the equation, in which case you would need to understand each step of the integral on a conceptual level. For actual calculations you can just use the formula.
- Tue Feb 04, 2020 7:55 pm
- Forum: Calculating Work of Expansion
- Topic: temperature
- Replies: 7
- Views: 435
Re: temperature
As an example, change in temperature from 0C to 100C = 100C. If you convert to K, you get 273K to 373K = 100K.
- Sat Feb 01, 2020 6:13 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Calorimeter
- Replies: 3
- Views: 193
Re: Calorimeter
In the equation, q represents heat of the substance reacted inside the calorimeter and C(cal) is the heat capacity of the calorimeter. The idea is that when heat is lost by the chemical reaction, it is gained by the calorimeter and vice versa so the negative sign is necessary.
- Sat Feb 01, 2020 6:09 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Closed vs isolated systems
- Replies: 24
- Views: 962
Re: Closed vs isolated systems
A closed system allows for exchange of heat with its surroundings (has the ability to release and/or absorb heat) while an isolated system does not.
- Sat Feb 01, 2020 6:07 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Closed Systems
- Replies: 8
- Views: 450
Re: Closed Systems
The main difference is insulation. Even if a system is sealed and no exchange of matter is occurring, heat exchange can still occur (e.g. a heat pack gives off heat)
- Sat Feb 01, 2020 6:05 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: isolated system
- Replies: 13
- Views: 646
Re: isolated system
An example would be any sealed, insulated container. Technically insulation is never perfect, and a very minimal amount of heat exchange can still occur between system and surroundings, but not enough to have any significant impact on calculations.
- Sat Feb 01, 2020 5:00 pm
- Forum: Calculating Work of Expansion
- Topic: External Pressure in Reversible Expansion
- Replies: 1
- Views: 81
External Pressure in Reversible Expansion
What are some actual practical ways external pressure can constantly change during reversible expansion in order to remain equal to the pressure of the gas in the system?
- Thu Jan 23, 2020 12:20 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Values for pKb and pKa
- Replies: 3
- Views: 236
Re: Values for pKb and pKa
Low pKa and low pH are generally associated with each other, while high pKa and high pH are also associated with each other. The same is true for pKb and pOH.
- Thu Jan 23, 2020 12:18 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: H20 in the ICE table
- Replies: 26
- Views: 1579
Re: H20 in the ICE table
H2O could be included if it is in the gas phase and you are calculating Kp. Otherwise it should be excluded if it is liquid (which most of the time it will be).
- Thu Jan 23, 2020 12:17 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Exothermic vs. Endothermic reactions
- Replies: 12
- Views: 995
Re: Exothermic vs. Endothermic reactions
A question that asks if a reaction is endothermic or exothermic should provide delta H, in which if delta H is positive, the reaction is endothermic and if it is negative, the reaction is exothermic.
- Thu Jan 23, 2020 12:15 am
- Forum: Ideal Gases
- Topic: Inert Gases and Equilibrium
- Replies: 6
- Views: 302
Re: Inert Gases and Equilibrium
Adding an inert gas does not affect the equilibrium constant because it does not affect the partial pressure of any reactants/products.
- Thu Jan 23, 2020 12:13 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 5% rule
- Replies: 13
- Views: 662
Re: 5% rule
Also keep in mind x cannot be approximated to zero if it is by itself. So values like x, x^2, etc. would be kept but values like 0.1-x, 0.1+x, etc. can be approximated to 0.1
- Sat Jan 18, 2020 6:42 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Temperature Change
- Replies: 9
- Views: 612
Re: Temperature Change
If a reaction is endothermic (requires heat), then addition of heat drives the reaction forward because the heat is used similarly to another reactant. The same concept applies if heat is removed, or also for exothermic reactions.
- Sat Jan 18, 2020 6:35 pm
- Forum: Ideal Gases
- Topic: "omitting" the units
- Replies: 7
- Views: 666
Re: "omitting" the units
As mentioned in this thread, because the units in the numerator and the denominator are the same, you can think of K as "unitless" because it just indicates the direction and degree of reaction.
- Sat Jan 18, 2020 6:25 pm
- Forum: Ideal Gases
- Topic: Ideal Gas Law
- Replies: 5
- Views: 241
Re: Ideal Gas Law
Based on lectures/homework problems, the main use of the ideal gas law has been to convert between pressure and concentration of a gas.
- Sat Jan 18, 2020 6:23 pm
- Forum: Ideal Gases
- Topic: Solids and Liquids [ENDORSED]
- Replies: 10
- Views: 596
Re: Solids and Liquids [ENDORSED]
Regardless of conditions, solids and liquids will be pure substances with a concentration of 1, so for calculating the equilibrium constant of a reaction, they would have no effect.
- Sat Jan 18, 2020 6:18 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Eq. constants & solubility
- Replies: 3
- Views: 187
Re: Eq. constants & solubility
When given a dissolution reaction, it would make sense that if the forward reaction is favored (which means the Ksp value is high), the reactant is highly soluble.
- Wed Jan 08, 2020 7:11 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Small K value and Large K value
- Replies: 10
- Views: 755
Re: Small K value and Large K value
In lecture, Lavelle said that if the value is between the two limits neither the reactant nor the product is favored and it is in a sort of intermediate state. Does that mean that we most likely won't be asked a question on whether the reactants or products are favored if the K value falls between ...
- Wed Jan 08, 2020 7:09 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Partial Pressure of gas
- Replies: 5
- Views: 251
Re: Partial Pressure of gas
There are several units for pressure, but as long as you stay consistent with the same unit, the Kp value should be the same.
- Wed Jan 08, 2020 7:08 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: K for Gases
- Replies: 12
- Views: 398
Re: K for Gases
For gases you should use Kp, because gases would have a "concentration" in the same way as aqueous solutions, as there is not really a solvent. Instead, the equivalent of concentration for a gas would be its partial pressure.
- Wed Jan 08, 2020 7:04 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Partial Pressure
- Replies: 3
- Views: 206
Re: Partial Pressure
Yes, in this case the partial pressures would be different because the moles of gas are different but the volume of the containers that they are in is the same.
- Wed Jan 08, 2020 7:03 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Partial Pressures
- Replies: 4
- Views: 175
Re: Partial Pressures
Nope, partial pressure can vary based on several factors (e.g. temperature, moles of gas, volume of container).
- Thu Dec 05, 2019 8:56 pm
- Forum: Lewis Acids & Bases
- Topic: Memorizing Charges of Transition Metals
- Replies: 9
- Views: 869
Re: Memorizing Charges of Transition Metals
It may be more intuitive to memorize the charges of common ligands (from the chart) and use that combined with net charge of the compound/complex in order to calculate the charge of the transition metal cation.
- Thu Dec 05, 2019 8:54 pm
- Forum: Bronsted Acids & Bases
- Topic: HF is a weak acid?
- Replies: 8
- Views: 1207
Re: HF is a weak acid?
Due to the smaller size of fluorine, the H-F bond is very strong, preventing much dissociation in water and thus preventing HF from donating a proton.
- Thu Dec 05, 2019 8:53 pm
- Forum: Bronsted Acids & Bases
- Topic: Difference between bronsted and conjugate
- Replies: 2
- Views: 150
Re: Difference between bronsted and conjugate
Bronsted acids are proton donors and Bronsted bases are proton acceptors. When an acid donates its proton it becomes the conjugate base and when the base accepts the proton it becomes the conjugate acid.
- Thu Dec 05, 2019 8:48 pm
- Forum: Conjugate Acids & Bases
- Topic: Double Arrows
- Replies: 3
- Views: 357
Re: Double Arrows
Not sure if you will be penalized, but it would probably be best to get used to including double arrows for equilibrium reactions.
- Thu Dec 05, 2019 8:47 pm
- Forum: Bronsted Acids & Bases
- Topic: Bronsted vs. Lewis Definitions
- Replies: 2
- Views: 159
Re: Bronsted vs. Lewis Definitions
The Lewis definition is just broader, so all Bronsted acids and bases will work as Lewis acids and bases as well. The only difference would be when dealing with compounds that don't have H+, in which case it would only work as a Lewis acid/base.
- Sat Nov 30, 2019 8:45 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: coordination number
- Replies: 8
- Views: 452
Re: coordination number
Coordination number just refers to the total number of bound ligands in the coordination sphere.
- Sat Nov 30, 2019 8:44 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Ligands
- Replies: 3
- Views: 272
Re: Ligands
A ligand must have a lone pair; otherwise it would be unable to bind to the central cation and form a coordination complex.
- Sat Nov 30, 2019 8:43 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Polydentate
- Replies: 3
- Views: 211
Re: Polydentate
A ligand is polydentate if it has multiple sites at which it can bind to a cation. The shape would look similar to an incomplete ring(s) with lone pairs at the ends.
- Sat Nov 30, 2019 8:41 pm
- Forum: Amphoteric Compounds
- Topic: compounds
- Replies: 5
- Views: 368
Re: compounds
Any compound is considered amphoteric if it acts as both an acid and a base, in other words it can either donate a proton or accept one (e.g. H2O)
- Sat Nov 30, 2019 8:33 pm
- Forum: Lewis Acids & Bases
- Topic: acid v. base?
- Replies: 16
- Views: 997
Re: acid v. base?
Lewis bases should have a lone pair to donate while lewis acids are usually positively charged and therefore able to accept an electron pair.
- Sun Nov 24, 2019 11:46 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bent vs linear
- Replies: 56
- Views: 4463
Re: Bent vs linear
If there are either one or two electron pairs on the central atom along with the two bonded atoms, it would result in bent shape. Otherwise, the molecule would be linear in shape.
- Sun Nov 24, 2019 11:44 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles
- Replies: 7
- Views: 510
Re: Bond Angles
When the central atom has one or more lone pairs, the higher strength of electron pair-electron pair and electron pair-bonded pair repulsion compared to bonded pair-bonded pair repulsion results in the bonds being pushed to form smaller angles.
- Sun Nov 24, 2019 11:42 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: AXE Format
- Replies: 34
- Views: 1363
Re: AXE Format
I think it would be okay to just put AXE and the 1s would be redundant.
- Sun Nov 24, 2019 11:41 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Hydrogen Bonding
- Replies: 13
- Views: 750
Re: Hydrogen Bonding
Yes, generally with the conditions necessary for hydrogen bonding to occur, which is hydrogen bonded to a very electronegative atom (F, O, or N), the resulting molecule would be polar.
- Sun Nov 24, 2019 11:40 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: T-shape
- Replies: 21
- Views: 1781
Re: T-shape
You would get a T-shape with the formula AX3E2, so three bonded atoms (two along the y-axis) and one approximately perpendicular to them with two lone pairs.
- Tue Nov 12, 2019 9:37 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: Induced dipole vs dipole
- Replies: 3
- Views: 175
Re: Induced dipole vs dipole
An induced dipole refers to when a polar molecule induces a dipole moment in a nonpolar molecule when they are near each other. For example, if the nonpolar molecule is near a positive dipole of a polar molecule, its electrons would be attracted towards it, forming a negative dipole. While the nonpo...
- Tue Nov 12, 2019 9:29 pm
- Forum: Electronegativity
- Topic: dipole moments
- Replies: 7
- Views: 347
Re: dipole moments
If you visualize the electron cloud surrounding a molecule, it would make sense that the more electronegative atom(s) would pull the shared electrons closer to itself, forming a negative dipole moment on that region of the molecule and a positive dipole moment on the opposite end.
- Tue Nov 12, 2019 9:27 pm
- Forum: Bond Lengths & Energies
- Topic: Van Der Waals BP
- Replies: 6
- Views: 325
Re: Van Der Waals BP
Forces that affect boiling point are based on the strength of the intermolecular forces, so the ones that would most affect BP are the ones that are the strongest. So ionic interactions would have the highest effect, followed by hydrogen bonding, then ion-dipole interactions, and the last few all b...
- Tue Nov 12, 2019 9:19 pm
- Forum: Dipole Moments
- Topic: Strength of Interactions
- Replies: 4
- Views: 171
Re: Strength of Interactions
I believe h-bonding is the strongest type of intermolecular force that can exist in covalent molecules as it is the strongest dipole-dipole interaction. But in general, ion-ion attraction is the strongest intermolecular force due to the large charge difference that exists between atoms.
- Tue Nov 12, 2019 9:13 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR model
- Replies: 4
- Views: 392
Re: VSEPR model
VSEPR stands for Valence Shell Electron Pair Repulsion, and VSEPR theory refers to the concept that molecular shape can be determined (at least for smaller molecules) based on the number of bonded atoms and lone pairs due to their tendency to maximize distance from each other. The AXE formula just i...
- Sun Nov 10, 2019 4:53 pm
- Forum: Bond Lengths & Energies
- Topic: Strongest Bond
- Replies: 15
- Views: 7364
Re: Strongest Bond
For intermolecular forces:
LDF/Van der Waals < dipole-dipole < h-bonds (the strongest type of dipole-dipole attraction)
LDF/Van der Waals < dipole-dipole < h-bonds (the strongest type of dipole-dipole attraction)
- Sun Nov 10, 2019 4:41 pm
- Forum: Dipole Moments
- Topic: Polarity
- Replies: 8
- Views: 263
Re: Polarity
Generally, if there is a particular part of the molecule that is more electronegative and the shape of the molecule does not allow for the charges to cancel (e.g. if the structure is not symmetrical), then the molecule is polar.
- Sun Nov 10, 2019 4:39 pm
- Forum: Coordinate Covalent Bonds
- Topic: Coordinate Covalent Bond
- Replies: 8
- Views: 638
Re: Coordinate Covalent Bond
Simply put, a coordinate covalent bond occurs when one atom provides both electrons used in the bond, as opposed to one electron from each atom in a normal covalent bond.
- Sun Nov 10, 2019 4:37 pm
- Forum: Resonance Structures
- Topic: Resonance Structures
- Replies: 3
- Views: 149
Re: Resonance Structures
The common exceptions of atoms that do not require at least a full octet are the first four elements, along with boron and aluminum. Otherwise, there aren't really any naturally occurring examples of an element that doesn't fill its octet so any resonance structures that break the rule wouldn't be v...
- Sun Nov 10, 2019 4:34 pm
- Forum: Ionic & Covalent Bonds
- Topic: polarizing power
- Replies: 7
- Views: 448
Re: polarizing power
Yes; because these elements are located in the second period, they do not have access to the empty 3d orbital and cannot hold an expanded octet.
- Sat Nov 02, 2019 3:25 pm
- Forum: DeBroglie Equation
- Topic: Converting mass to kilograms for de broglie
- Replies: 7
- Views: 303
Re: Converting mass to kilograms for de broglie
Yes, you would need to convert to kilograms because Planck's constant, h, uses kilograms.
- Sat Nov 02, 2019 3:23 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: determining the number of orbitals
- Replies: 7
- Views: 332
Re: determining the number of orbitals
The quantum number that you would want to use to determine the number of orbitals in a given subshell would be l, which identifies the actual subshell: s (l=0), p (l=1), d (l=2), or f (l=3). They have 1, 3, 5, and 7 orbitals respectively.
- Sat Nov 02, 2019 3:20 pm
- Forum: Photoelectric Effect
- Topic: Ionization Energy vs Threshold Energy
- Replies: 4
- Views: 327
Re: Ionization Energy vs Threshold Energy
Threshold energy (represented by the work function) is relevant to the photoelectric effect because it refers to the energy required to remove a single electron from a certain metal surface. On the other hand, ionization energy is defined as the energy required to remove an electron from an atom in ...
- Sat Nov 02, 2019 3:17 pm
- Forum: Coordinate Covalent Bonds
- Topic: Difference between coordinate covalent and covalent bond
- Replies: 6
- Views: 10111
Re: Difference between coordinate covalent and covalent bond
In a coordinate covalent bond, one atom provides both of the bonding valence electrons.
- Sat Nov 02, 2019 3:10 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: What are the octet exceptions?
- Replies: 11
- Views: 550
Re: What are the octet exceptions?
Elements beyond the third row of the periodic table are able to hold extra valence electrons beyond the octet because they have an unfilled d-orbital.
- Sun Oct 27, 2019 6:20 pm
- Forum: Resonance Structures
- Topic: Resonance
- Replies: 8
- Views: 230
Re: Resonance
Resonance just refers to the concept that a single molecule is not restricted to a rigid structure. Rather, it can change into unique resonance structures.
- Sun Oct 27, 2019 6:19 pm
- Forum: Lewis Structures
- Topic: Lone pair
- Replies: 8
- Views: 421
Re: Lone pair
Yep, as previous answers stated, lone pairs just refer to a pair of electrons in an orbital that are not shared with another atom.
- Sun Oct 27, 2019 6:17 pm
- Forum: Ionic & Covalent Bonds
- Topic: Covalent Bonds
- Replies: 11
- Views: 581
Re: Covalent Bonds
Yes, covalent bonds can only be formed between two nonmetals.
- Sun Oct 27, 2019 6:15 pm
- Forum: Ionic & Covalent Bonds
- Topic: Valence Electrons
- Replies: 16
- Views: 807
Re: Valence Electrons
For the s and p block elements, the number of valence electrons is just the group number, but it can vary for the d block based on electron configuration. Charged ions may also carry extra or fewer valence electrons.
- Sun Oct 27, 2019 6:13 pm
- Forum: Sigma & Pi Bonds
- Topic: Single vs. Double bonds
- Replies: 15
- Views: 2014
Re: Single vs. Double bonds
Because there are more electrons being shared between the atoms, there is a greater attractive force that pulls the atoms closer together, shortening bond length.
- Fri Oct 18, 2019 4:52 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: Nodal Plane
- Replies: 4
- Views: 175
Re: Nodal Plane
A nodal plane is just a planar area in which electrons cannot be located. Due to the spherical shape of the s-orbital, it does not have any.
- Fri Oct 18, 2019 4:51 pm
- Forum: Properties of Electrons
- Topic: effective nuclear charge
- Replies: 5
- Views: 376
Re: effective nuclear charge
I don't think we will be expected to calculate a specific value for effective nuclear charge, but to conceptually understand it, effective nuclear charge can be used to determine which energy state an electron is in due to the shielding effect.
- Fri Oct 18, 2019 4:46 pm
- Forum: Properties of Light
- Topic: Equations and Constants
- Replies: 6
- Views: 285
Equations and Constants
Are there any specific equations or constants that aren't provided on the formula sheet but will be included on tests?
- Fri Oct 18, 2019 4:43 pm
- Forum: Photoelectric Effect
- Topic: Intensity v Frequency
- Replies: 5
- Views: 351
Re: Intensity v Frequency
Intensity is determined by amplitude of a wave while frequency is determined by the length (specifically how short) a wave is. In the famous photoelectric effect experiment, it was determined that the energy of light is proportional to frequency, rather than the expected which was amplitude/intensit...
- Fri Oct 18, 2019 4:39 pm
- Forum: Properties of Electrons
- Topic: Momentum
- Replies: 11
- Views: 336
Re: Momentum
Like previous answers mentioned, momentum is mass * velocity. So, if an object is moving at a slow velocity but has a large mass, it can still have a substantial momentum.
- Wed Oct 09, 2019 6:29 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: Symbols for Molarity
- Replies: 8
- Views: 1315
Re: Symbols for Molarity
Yes, as previous answers mentioned, they refer to the same thing. I believe "c" is used in general reference to some concentration while "M" is a more specific reference to molarity, which is a specific measure defined as mol/L.
- Wed Oct 09, 2019 6:27 pm
- Forum: Significant Figures
- Topic: %Mass Composition
- Replies: 12
- Views: 827
Re: %Mass Composition
The same rules for significant figures should still apply, and generally that would be anywhere from 4-5 sig figs based on what's given in the problem.
- Wed Oct 09, 2019 6:24 pm
- Forum: Balancing Chemical Reactions
- Topic: Fractions
- Replies: 34
- Views: 1526
Re: Fractions
It's generally good practice to convert all the coefficients to integers, as that gives the most accurate representation of the chemical reaction.
- Wed Oct 09, 2019 6:06 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: Polyatomic ions on Test 1
- Replies: 4
- Views: 268
Re: Polyatomic ions on Test 1
For the first test, it won't be required to have the names and formulas of polyatomic ions memorized, but I believe they will not always be provided in future tests.
- Wed Oct 09, 2019 6:04 pm
- Forum: SI Units, Unit Conversions
- Topic: SI Units
- Replies: 2
- Views: 259
Re: SI Units
One angstrom is 10^-10 meters (m), or 100 picometers (pm).
- Thu Oct 03, 2019 4:53 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: Molarity
- Replies: 9
- Views: 399
Re: Molarity
Molarity is relevant when dealing with solutions. By doing molarity calculations, you can determine the moles of solute and how you may need to dilute the solution.
- Thu Oct 03, 2019 4:21 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: Molality vs Molarity
- Replies: 2
- Views: 141
Re: Molality vs Molarity
Both are generally used to refer to solution concentration. Molarity, as we know, is calculated as moles of solute/L of solvent. Meanwhile, molality is moles solute/kg solvent. I think most of the time though, molarity is the preferred measurement to use.
- Thu Oct 03, 2019 4:19 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: Molar Mass Clarification
- Replies: 3
- Views: 137
Re: Molar Mass Clarification
Molar mass refers to the mass in grams of one mole of a certain particle. For atoms, the molar mass is indicated on the periodic table (same as atomic mass). For molecules, just add up the molar masses of all its constituents.
- Thu Oct 03, 2019 4:14 pm
- Forum: Accuracy, Precision, Mole, Other Definitions
- Topic: Avogadro's Number?
- Replies: 16
- Views: 972
Re: Avogadro's Number?
As the previous answers mentioned, it's just a specific name for the number 6.022 x 10^23. Generally you would just think of it as a mole.