Search found 107 matches
- Sun Mar 15, 2020 10:06 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: intermediate
- Replies: 26
- Views: 2060
Re: intermediate
Since an intermediate cancels out, you wouldn't write it in the final balanced equation.
- Sun Mar 15, 2020 10:05 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Units for reaction rates
- Replies: 15
- Views: 1127
Re: Units for reaction rates
And since the units for reaction rates are always molarity/ time, this will help you find out the k units.
- Sun Mar 15, 2020 10:04 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: kinetics
- Replies: 9
- Views: 665
Re: kinetics
It's probably wouldn't occur without a catalyst.
- Sun Mar 15, 2020 10:02 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Kinetic vs thermodynamics
- Replies: 8
- Views: 560
Re: Kinetic vs thermodynamics
Kinetics is all about the rate. It involves activation energy, and rate constants, but thermodynamics has to do with Gibbs, entropy, enthalpy, and heat.
- Sun Mar 15, 2020 10:00 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Solving for rates
- Replies: 3
- Views: 351
Re: Solving for rates
The molar ratio, right?
- Fri Mar 06, 2020 11:10 pm
- Forum: First Order Reactions
- Topic: Time Conversions
- Replies: 9
- Views: 1126
Re: Time Conversions
So, it doesn't matter seconds or minutes as long as you have all the same units.
- Fri Mar 06, 2020 11:04 pm
- Forum: First Order Reactions
- Topic: rate constants
- Replies: 30
- Views: 1520
Re: rate constants
Rate constants are always positive because concentrations are always positive.
- Fri Mar 06, 2020 11:00 pm
- Forum: First Order Reactions
- Topic: Rate Law
- Replies: 4
- Views: 643
Re: Rate Law
I don't think he would test us on it, but he probably wants us to have a vague idea of how to do it.
- Fri Mar 06, 2020 10:54 pm
- Forum: First Order Reactions
- Topic: zero, first, and second order
- Replies: 3
- Views: 315
Re: zero, first, and second order
It helps determine the rate of reactions.
- Fri Mar 06, 2020 10:51 pm
- Forum: First Order Reactions
- Topic: first order
- Replies: 3
- Views: 289
Re: first order
A first order reactions only requires one molecule of one type, where a second order reaction needs two molecules colliding.
- Fri Mar 06, 2020 10:49 pm
- Forum: First Order Reactions
- Topic: first order reactions
- Replies: 2
- Views: 256
Re: first order reactions
So, that's why third order reactions are rare. It's uncommon for three molecules to collide simulataneously.
- Fri Mar 06, 2020 10:47 pm
- Forum: General Rate Laws
- Topic: Half Lives
- Replies: 3
- Views: 279
Re: Half Lives
You can think of it AS 2^-X, X being each half life. So two half lives is 2^-2, or 1/4
- Sun Mar 01, 2020 6:37 pm
- Forum: Balancing Redox Reactions
- Topic: When to add H+ or H20
- Replies: 19
- Views: 2492
Re: When to add H+ or H20
It really depends if the solution is acidic, basic, or neutral
- Sun Mar 01, 2020 6:36 pm
- Forum: Balancing Redox Reactions
- Topic: Redox Reactions and Acid/Base Reactions
- Replies: 9
- Views: 757
Re: Redox Reactions and Acid/Base Reactions
Redox reactions change the oxidation numbers
- Sun Mar 01, 2020 6:34 pm
- Forum: Balancing Redox Reactions
- Topic: H+ or H2O
- Replies: 9
- Views: 633
Re: H+ or H2O
Yeah, it really depends if the solution is neutral, basic, or acidic.
- Sun Mar 01, 2020 6:32 pm
- Forum: Balancing Redox Reactions
- Topic: Anode and Cathode
- Replies: 9
- Views: 585
Re: Anode and Cathode
The more positive electronic potential will be at the reduction reaction, which will be in the cathode
- Sun Mar 01, 2020 6:28 pm
- Forum: Balancing Redox Reactions
- Topic: Anode and Cathode
- Replies: 8
- Views: 563
Re: Anode and Cathode
If you're given a diagram, the left is the anode and the right it the cathode. If you aren't given a diagram, the greater electric potential is at the cathode.
- Sun Feb 23, 2020 10:00 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: salt bridge
- Replies: 9
- Views: 673
Re: salt bridge
It makes sure that the flow in the cell continues.
- Sun Feb 23, 2020 9:58 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Le Chatelier’s Principle
- Replies: 11
- Views: 716
Re: Le Chatelier’s Principle
It's all about how it makes one side of the reaction more favorable.
- Sun Feb 23, 2020 9:55 pm
- Forum: Balancing Redox Reactions
- Topic: Test 2
- Replies: 9
- Views: 548
Re: Test 2
It was just moved from week 8 to week 9
- Sun Feb 23, 2020 9:54 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Work
- Replies: 5
- Views: 368
Re: Work
So if it's losing energy to the surroundings, work is negative, while if the system is gaining energy, it is positive.
- Sun Feb 23, 2020 9:51 pm
- Forum: Balancing Redox Reactions
- Topic: Oxidation Numbers/States
- Replies: 8
- Views: 545
Re: Oxidation Numbers/States
Yeah, you need to know the general oxidation states to see what's happening with the half reactions
- Sun Feb 16, 2020 11:35 pm
- Forum: Calculating Work of Expansion
- Topic: Work Equation
- Replies: 6
- Views: 634
Re: Work Equation
It depends if it's reversible.
- Sun Feb 16, 2020 11:32 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Reversible vs Irreversible
- Replies: 7
- Views: 453
Re: Reversible vs Irreversible
Yes, there are different equations to use based on if it's reversible or irreversible.
- Sun Feb 16, 2020 11:31 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: State functions
- Replies: 5
- Views: 272
Re: State functions
Just remember that heat and work are not state functions, most things are.
- Sun Feb 16, 2020 11:30 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Delta U
- Replies: 5
- Views: 388
Re: Delta U
Delta U is zero because there is no potential energy because it's an ideal gas, and no kinetic energy because delta t is zero.
- Sun Feb 16, 2020 11:25 pm
- Forum: Van't Hoff Equation
- Topic: Equilibrium Constant
- Replies: 4
- Views: 312
Re: Equilibrium Constant
Since Q is K at equilibrium, when delta g is at zero, k is used.
- Sun Feb 16, 2020 11:20 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Midterm Curve
- Replies: 45
- Views: 2269
Re: Midterm Curve
Only the whole class is curved
- Mon Feb 10, 2020 2:11 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: Using Cv and Cp
- Replies: 4
- Views: 257
Re: Using Cv and Cp
Cv is for constant volume and Cp is for constant pressure, yes.
- Mon Feb 10, 2020 2:09 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Intensive vs. Extensive
- Replies: 15
- Views: 1362
Re: Intensive vs. Extensive
Intensive properties do not rely on the amount of substance.
- Mon Feb 10, 2020 2:08 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Useful Summary of Thermodynamic Definitions
- Replies: 55
- Views: 18591
Re: Useful Summary of Thermodynamic Definitions
This is insanely helpful, thank you!
- Mon Feb 10, 2020 2:06 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Writing balanced equation for formation reactions
- Replies: 4
- Views: 317
Re: Writing balanced equation for formation reactions
If the equation asks for one mole its alright to put fractions in front for the coefficients.
- Mon Feb 10, 2020 2:06 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Reversible Reactions vs. Irreversible Reactions
- Replies: 6
- Views: 287
Re: Reversible Reactions vs. Irreversible Reactions
The reversible is curved and downscoping, and the irreversible graphs are straight. It shows how less work is done for the irreversible processes.
- Mon Feb 10, 2020 2:03 pm
- Forum: Calculating Work of Expansion
- Topic: Ideal Gas Internal Energy
- Replies: 4
- Views: 177
Re: Ideal Gas Internal Energy
It's an approximation for the heat capacity of a molecule.
- Mon Feb 10, 2020 2:02 pm
- Forum: Phase Changes & Related Calculations
- Topic: Reversible or Irreversible
- Replies: 5
- Views: 318
Re: Reversible or Irreversible
Yeah, the problem should give you some sort of information.
- Sun Feb 02, 2020 7:19 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Phase change
- Replies: 20
- Views: 870
Re: Phase change
It would be positive, because it requires energy to cause the phase change.
- Sun Feb 02, 2020 7:17 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Work
- Replies: 6
- Views: 229
Re: Work
It all depends on the system and the surroundings, and what is doing work on what. Whatever is doing the work will have negative work and vise versa.
- Sun Feb 02, 2020 7:16 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: pressure v. volume
- Replies: 3
- Views: 135
Re: pressure v. volume
As long as there isn't any work being put in, delta u=delta h
- Sun Feb 02, 2020 7:15 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Definition of First Law
- Replies: 9
- Views: 363
Re: Definition of First Law
It's just the one that states the conservation of energy.
- Sun Feb 02, 2020 7:14 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Delta U = Q
- Replies: 8
- Views: 219
Re: Delta U = Q
The work is zero when there is no expansion in volume or change in pressure, because otherwise it would affect the internal energy.
- Sat Jan 25, 2020 9:28 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Calculation methods
- Replies: 6
- Views: 287
Re: Calculation methods
The second method uses averages, so it's the least accurate.
- Sat Jan 25, 2020 9:28 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Heat Capacity
- Replies: 5
- Views: 267
Re: Heat Capacity
So, can you convert between specific and molar heat capacity?
- Sat Jan 25, 2020 9:26 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Bond Enthalpy Method
- Replies: 5
- Views: 244
Re: Bond Enthalpy Method
Yes, Hess's Law should be the most accurate, it doesn't rely on averages
- Sat Jan 25, 2020 9:26 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Standard enthalpy
- Replies: 2
- Views: 177
Re: Standard enthalpy
It's sort of a baseline
- Sat Jan 25, 2020 9:24 pm
- Forum: Phase Changes & Related Calculations
- Topic: State Function
- Replies: 7
- Views: 358
Re: State Function
Anything that isn't dependent on the path is a state function
- Tue Jan 14, 2020 2:23 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Expansion
- Replies: 5
- Views: 186
Re: Expansion
Expanding the container would shift the reaction based on the amount of product or reactant, but with overall change, the Keq would remain unchanged.
- Tue Jan 14, 2020 2:21 pm
- 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
For solving equilibrium constants, you usually just use aqueous compounds or gaseous ones
- Tue Jan 14, 2020 2:18 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: volume change with inert gas
- Replies: 9
- Views: 255
Re: volume change with inert gas
Okay, that makes more sense, thank you
- Tue Jan 14, 2020 2:15 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Excess Reactant in Le Chatelier's Principle
- Replies: 6
- Views: 221
Re: Excess Reactant in Le Chatelier's Principle
The reactants have to be in excess, because Le Chatlier's Principle is based on a reaction in equilibrium, and so it's still going on.
- Tue Jan 14, 2020 2:13 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Effect of Inert Gases
- Replies: 9
- Views: 354
Re: Effect of Inert Gases
Inert gases are relatively stable, and so they don't usually have an effect on the reaction.
- Tue Jan 14, 2020 2:11 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: What is this?
- Replies: 23
- Views: 1480
Re: What is this?
It just shows how a reaction shifts to maintain stability
- Tue Jan 14, 2020 2:08 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Change on Same Side
- Replies: 6
- Views: 247
Re: Change on Same Side
It affects it by making the products more favorable, using up more H2.
- Thu Jan 09, 2020 11:48 am
- Forum: Ideal Gases
- Topic: R constant in PV=nRT
- Replies: 9
- Views: 300
Re: R constant in PV=nRT
For homework though the one on the equation sheet should work
- Thu Jan 09, 2020 11:46 am
- Forum: Ideal Gases
- Topic: Nitrogen gas
- Replies: 5
- Views: 673
Re: Nitrogen gas
Is that because it's relatively stable?
- Thu Jan 09, 2020 11:45 am
- Forum: Ideal Gases
- Topic: K
- Replies: 10
- Views: 525
Re: K
It will be the same, because even if you use partial pressure instead of concentration, you would still be able to convert between the two.
- Thu Jan 09, 2020 11:44 am
- Forum: Ideal Gases
- Topic: Understanding Q
- Replies: 19
- Views: 751
Re: Understanding Q
They're solved exactly the same way.
- Thu Jan 09, 2020 11:44 am
- Forum: Ideal Gases
- Topic: K and Q
- Replies: 13
- Views: 372
Re: K and Q
K is when the reaction is at equilibrium. Q is at all other points in the reaction, and can be used to show which direction the reaction is proceeding.
- Sat Dec 07, 2019 10:44 pm
- Forum: Properties & Structures of Inorganic & Organic Bases
- Topic: Are noble gases considered bases?
- Replies: 9
- Views: 2205
Re: Are noble gases considered bases?
Noble gases are usually unreactive, so they're unlikely to give up electrons or accept them.
- Sat Dec 07, 2019 10:42 pm
- Forum: Conjugate Acids & Bases
- Topic: buffer solutions
- Replies: 5
- Views: 595
Re: buffer solutions
Yeah, he said that we really only need to now how to calculate for strong acids.
- Sat Dec 07, 2019 10:41 pm
- Forum: Conjugate Acids & Bases
- Topic: how to figure out?
- Replies: 12
- Views: 729
Re: how to figure out?
The conjugate base is what is left after the acid gives off a proton.
- Sat Dec 07, 2019 10:40 pm
- Forum: Bronsted Acids & Bases
- Topic: bronsted base and acid
- Replies: 4
- Views: 414
Re: bronsted base and acid
So, the lewis definition is concerned with electrons while the Bronsted definition is involving protons.
- Sat Dec 07, 2019 10:38 pm
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: Oxoacid Strength
- Replies: 6
- Views: 735
Re: Oxoacid Strength
Okay, that makes sense. So, when concerning bond lengths, it's the comparison between hydrogen and another atom.
- Sat Dec 07, 2019 10:35 pm
- Forum: Amphoteric Compounds
- Topic: Amphiprotic
- Replies: 7
- Views: 551
Re: Amphiprotic
Water is an example of this.
- Sun Nov 24, 2019 9:48 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Formation of coordinate covalent bonds
- Replies: 2
- Views: 144
Re: Formation of coordinate covalent bonds
So, the number of coordination compounds depends on the number of bonds that the transition metal will make to neutralize the charge.
- Sun Nov 24, 2019 9:45 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Drawing Structures
- Replies: 4
- Views: 286
Re: Drawing Structures
Yeah, we just draw the lewis structure like we always have
- Sun Nov 24, 2019 9:43 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Coordination Sphere
- Replies: 5
- Views: 424
Re: Coordination Sphere
So water would be outside of the coordination sphere?
- Sun Nov 24, 2019 9:41 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Central atom?
- Replies: 5
- Views: 340
Re: Central atom?
Okay, that makes sense
- Sun Nov 24, 2019 9:35 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Coordination Numbers
- Replies: 4
- Views: 335
Re: Coordination Numbers
Yeah, so to tell the coordination number you have to see the number of bonds, but I think you can predict it based on the number of bonds it is able to form.
- Sun Nov 17, 2019 3:33 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: regions of electron density
- Replies: 10
- Views: 529
Re: regions of electron density
Recognizing regions of electron density does give an idea of the general shape, but the actual atoms give it a name.
- Sun Nov 17, 2019 3:31 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Lone Pairs
- Replies: 5
- Views: 323
Re: Lone Pairs
Lone pairs are regions of electron density, so it does need to be taken into consideration. Like an atom with two attached atoms and no lone pairs will be linear, but if a lone pair was added, it would become bent.
- Sun Nov 17, 2019 3:28 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Dipole moments
- Replies: 4
- Views: 204
Re: Dipole moments
Yeah, the arrow points towards the more electronegative atom
- Sun Nov 17, 2019 3:27 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Can there be lone pairs on the central atom if the shape is linear?
- Replies: 4
- Views: 274
Re: Can there be lone pairs on the central atom if the shape is linear?
If you just had two atoms attached with two lone pairs, it would end up being bent, as the lone pairs wouldn't be able to just be opposite of each other. It would end up looking like a water molecule.
- Sun Nov 17, 2019 3:24 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Can there be lone pairs on the central atom if the shape is linear?
- Replies: 4
- Views: 274
Re: Can there be lone pairs on the central atom if the shape is linear?
I think it depends on the atoms attached
- Sun Nov 17, 2019 3:19 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles
- Replies: 2
- Views: 185
Re: Bond Angles
You don't need to know the exact angle in these cases, just if it's less or more than the expected angle.
- Sun Nov 10, 2019 8:18 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal charge
- Replies: 16
- Views: 933
Re: Formal charge
More electronegative atoms can have a negative formal charge if you need to give them one.
- Sun Nov 10, 2019 8:17 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: formal charge
- Replies: 7
- Views: 443
Re: formal charge
You really only need to do it when they ask for it. But you should when drawing resonance structures just so you can find out if it's more stable.
- Sun Nov 10, 2019 8:16 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Shortcut for Formal Charge
- Replies: 19
- Views: 1668
Re: Shortcut for Formal Charge
Just think about the number of lone electrons and the number of lines.
- Sun Nov 10, 2019 8:15 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: central atom
- Replies: 21
- Views: 1040
Re: central atom
Yes, the central atom should have a zero charge
- Sun Nov 10, 2019 8:14 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charge
- Replies: 9
- Views: 376
Re: Formal Charge
If the compound has no charge, then the formal charge should be zero.
- Sun Nov 10, 2019 8:13 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Calculating formal charge
- Replies: 4
- Views: 263
Re: Calculating formal charge
Valence electrons just show how many bonds can be formed, while formal charge shows the bonds.
- Sat Nov 02, 2019 2:00 pm
- Forum: Lewis Structures
- Topic: Drawing Lewis Structures
- Replies: 4
- Views: 241
Re: Drawing Lewis Structures
If there are multiple places you can place the double bond, that shows resonance. But you'll want to limit the formal charges on each atom.
- Sat Nov 02, 2019 1:58 pm
- Forum: Lewis Structures
- Topic: Expanded Shells
- Replies: 3
- Views: 174
Re: Expanded Shells
Yeah, it becomes the 18-electron rule to reach a noble gas configuration
- Sat Nov 02, 2019 1:54 pm
- Forum: Lewis Structures
- Topic: Exceptions to the Octet
- Replies: 5
- Views: 265
Re: Exceptions to the Octet
Only a few elements really need to form an octet, because after that you reach the d-orbital, the 18-electron rule becomes apparent
- Sat Nov 02, 2019 1:51 pm
- Forum: Lewis Structures
- Topic: central atom
- Replies: 16
- Views: 2230
Re: central atom
It's the least electronegative because it's the one that can form the most bonds
- Sat Nov 02, 2019 1:49 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Midterm
- Replies: 6
- Views: 314
Re: Midterm
I think he said it wouldn't be on the midterm because we hadn't covered it in lecture
- Sun Oct 27, 2019 8:48 pm
- Forum: Trends in The Periodic Table
- Topic: Electron Affinity
- Replies: 6
- Views: 328
Re: Electron Affinity
Okay, that makes more sense.
- Sun Oct 27, 2019 8:47 pm
- Forum: Trends in The Periodic Table
- Topic: Ionization energy
- Replies: 12
- Views: 634
Re: Ionization energy
All you're really supposed to know for Ionization Energies is the trends for lewis structures later.
- Sun Oct 27, 2019 8:46 pm
- Forum: Trends in The Periodic Table
- Topic: Central Atom
- Replies: 13
- Views: 544
Re: Central Atom
Just put the ones that are more left and more down as the central atom, as they have lower ionization energies.
- Sun Oct 27, 2019 8:43 pm
- Forum: Trends in The Periodic Table
- Topic: F orbital
- Replies: 3
- Views: 137
Re: F orbital
Yeah, I think my TA said the same thing
- Sun Oct 27, 2019 8:43 pm
- Forum: Trends in The Periodic Table
- Topic: Electronegativity vs. Electron affinity
- Replies: 8
- Views: 630
Re: Electronegativity vs. Electron affinity
Yes, electron negativity is the ability to attract paired electrons, while electron affinity is the energy used when an electron is added.
- Sun Oct 20, 2019 4:07 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Overlapping
- Replies: 4
- Views: 187
Re: Overlapping
Okay, that makes more sense
- Sun Oct 20, 2019 4:04 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Shell, Subshell, Orbital Terminology
- Replies: 8
- Views: 568
Re: Shell, Subshell, Orbital Terminology
n is just the energy level of the electron, the principal quantum number, and sort of shows the size of the orbital
- Sun Oct 20, 2019 3:58 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Inner e- and Outer e-
- Replies: 14
- Views: 503
Re: Inner e- and Outer e-
The outer electrons feel less of an electrostatic attraction, they're shielded by the inner ones from the nucleus.
- Sun Oct 20, 2019 3:51 pm
- Forum: Properties of Light
- Topic: N levels
- Replies: 8
- Views: 504
Re: N levels
Yeah, the n-levels are just the energy levels that an electron can jump or fall to
- Sun Oct 20, 2019 3:50 pm
- Forum: DeBroglie Equation
- Topic: Mass of electron and photon
- Replies: 5
- Views: 309
Re: Mass of electron and photon
The mass of an electron should be given, but it's 9.109* 10^-31 kg for an electron
- Sun Oct 20, 2019 3:48 pm
- Forum: Properties of Light
- Topic: Unit for Wavelength
- Replies: 34
- Views: 2487
Re: Unit for Wavelength
The general unit is meters, but it wavelength can usually be put in nanometers
- Sun Oct 13, 2019 2:29 pm
- Forum: Properties of Light
- Topic: Large Objects
- Replies: 7
- Views: 1121
Re: Large Objects
So, bigger objects have a wavelength way smaller than 10^-15, so they're not detectable according to de Broglie's equation.
- Sun Oct 13, 2019 2:28 pm
- Forum: Properties of Light
- Topic: Rydberg constant
- Replies: 7
- Views: 286
Re: Rydberg constant
So, when we use the equation, we end by doing Ef-Ei?
- Sun Oct 13, 2019 2:25 pm
- Forum: Properties of Light
- Topic: difference between Rydberg equation and De Broglie equation
- Replies: 5
- Views: 531
Re: difference between Rydberg equation and De Broglie equation
Okay, that makes sense. So, de Broglie's equation shows the relationship of the wavelength, mass, and velocity of a small particle, and Rydberg predicts the energy of an electron moving between energy levels, but only for hydrogen.
- Sun Oct 13, 2019 2:21 pm
- Forum: Properties of Light
- Topic: wavelike properties
- Replies: 4
- Views: 256
Re: wavelike properties
When it says measurable wavelike properties, it just means that it's not smaller than 10^-15, because that's not detectable.