Search found 102 matches
- Mon Mar 09, 2020 12:33 am
- Forum: Balancing Redox Reactions
- Topic: Half rxns
- Replies: 27
- Views: 1521
Re: Half rxns
https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Supplemental_Modules_(Analytical_Chemistry)/Electrochemistry/Redox_Chemistry/Balancing_Redox_reactions Here's a pretty helpful link! In an acidic solution, the reaction is balanced after you've added your H+ to balance the hydrogens and el...
- Mon Mar 09, 2020 12:30 am
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: n in NFE
- Replies: 64
- Views: 4240
Re: n in NFE
Remember that it's the number of electrons after you balance your equations (so the number of electrons transferred in the cathode half reaction should equal the number of electrons transferred in the anode half reaction, which should equal your value of n).
- Mon Mar 09, 2020 12:28 am
- Forum: Balancing Redox Reactions
- Topic: Reversing the anode
- Replies: 10
- Views: 743
Re: Reversing the anode
The values in the table are always standard reduction potentials, so since the anode is being oxidized and not reduced, the sign gets flipped.
- Mon Mar 09, 2020 12:25 am
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: 7D.5
- Replies: 1
- Views: 232
Re: 7D.5
I think that might be an error in the manual because I solved the problem without subtracting 0.59 and I still got 2.72 x 10^(10) as my final answer. Also, if you subtract 0.59, you actually end up with (k'/k) = 0.588, which isn't right.
- Mon Mar 09, 2020 12:19 am
- Forum: Balancing Redox Reactions
- Topic: balancing reactions
- Replies: 6
- Views: 526
Re: balancing reactions
https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Supplemental_Modules_(Analytical_Chemistry)/Electrochemistry/Redox_Chemistry/Balancing_Redox_reactions This link was super helpful to me! The only big difference between balancing in an acidic vs. basic solution is: in an acidic solution, ...
- Mon Mar 02, 2020 12:40 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: what's happening in galvanic cells
- Replies: 2
- Views: 228
Re: what's happening in galvanic cells
The electrons are moving from the anode to the cathode because the anode is being oxidized (losing electrons) while the cathode is being reduced (gaining electrons). When you look at the standard reduction potentials for the half-reactions, the reaction in the cathode half cell should have a more po...
- Mon Mar 02, 2020 12:36 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Nernst
- Replies: 10
- Views: 658
Re: Nernst
It's an equation that helps you find the cell potential under non-standard conditions & relates the Q value to the cell potential.
- Mon Mar 02, 2020 12:33 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: concentration cell
- Replies: 3
- Views: 268
Re: concentration cell
Yeah! A concentration cell has the same ion on both sides, but different concentrations. I'm not sure how it can be compared to a galvanic cell though, sorry. I guess it could be compared to a galvanic cell because like a galvanic cell, it doesn't require an external source plugged to an outlet and...
- Mon Mar 02, 2020 12:30 am
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: n in Equation
- Replies: 6
- Views: 456
Re: n in Equation
One thing to remember is that you should always take the balanced number of moles of electrons for the reaction as your value of n.
- Mon Mar 02, 2020 12:29 am
- Forum: Balancing Redox Reactions
- Topic: Cell Diagrams
- Replies: 5
- Views: 382
Re: Cell Diagrams
The double vertical lines represent separation of the cells, with your anode on the left and cathode on the right. On the anode side, let's say you have both Fe (s) and Fe2+ (aq) present because you're trying to show that Fe (s) --> Fe2+ (aq) + 2 e- and on the cathode side you have Cu(s) and Cu2+ (a...
- Sat Feb 29, 2020 4:15 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Pt in cell diagrams
- Replies: 3
- Views: 253
Re: Pt in cell diagrams
If there’s no solid conducting metal in one half of the cell diagram, then that half will have a platinum electrode.
- Mon Feb 24, 2020 1:07 am
- Forum: Administrative Questions and Class Announcements
- Topic: Thermo
- Replies: 3
- Views: 299
Re: Thermo
I feel like it's just a lot of practice with the homework problems he assigned since there's just so much math involved. Also, going through the book and writing down important equations (and when to use them/what conditions) also helps.
- Mon Feb 24, 2020 1:04 am
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: G(not) and G
- Replies: 15
- Views: 767
Re: G(not) and G
Rafsan Rana 1A wrote:Isn't the equation G = Gnot + RTlnQ ?
Yes, it should be delta G = delta G(naught) + RTlnQ.
- Mon Feb 24, 2020 1:00 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Nernst Equation usage
- Replies: 6
- Views: 401
Re: Nernst Equation usage
You'd use it to relate the reduction potential (under non-standard conditions) to the standard electrode potential. At any point in the reaction, you can find the cell potential using this equation.
- Mon Feb 24, 2020 12:57 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Galvanic vs. electrolytic
- Replies: 4
- Views: 331
Re: Galvanic vs. electrolytic
This diagram is pretty helpful too.
- Mon Feb 24, 2020 12:51 am
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: S = 0
- Replies: 21
- Views: 1220
Re: S = 0
S just means entropy, rather than change in entropy that should be denoted as ΔS. Entropy is almost never 0 (the entropies of all perfect crystals approach zero as the absolute temperature approaches zero; "perfect crystal" refers to a substance in which all the atoms are in a perfectly o...
- Mon Feb 17, 2020 11:11 pm
- Forum: Balancing Redox Reactions
- Topic: Electrical energy and Chemical energy
- Replies: 2
- Views: 224
Re: Electrical energy and Chemical energy
In addition to the answer above, you can also tie this to the first law of thermodynamics (energy is neither created nor destroyed but rather transferred from one form to another). So, this would be an example of the conversion.
- Mon Feb 17, 2020 11:05 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Midterm Curve
- Replies: 45
- Views: 2330
Re: Midterm Curve
Individual tests aren't curved :(
- Mon Feb 17, 2020 11:02 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Exothermic rxns being spontaneous
- Replies: 5
- Views: 467
Re: Exothermic rxns being spontaneous
Although reactions being exothermic/endothermic and spontaneous/nonspontaneous are closely related, you should also keep in mind that not all exothermic reactions will be spontaneous. When checking for spontaneity, look at the delta G sign (meaning you need the sign of delta H AND the sign of delta ...
- Mon Feb 17, 2020 10:55 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Van't Hoff
- Replies: 6
- Views: 324
Re: Van't Hoff
Isn't it assumed to be at constant temperature as well as pressure?
- Mon Feb 17, 2020 10:50 pm
- Forum: Balancing Redox Reactions
- Topic: Oxidation numbers [ENDORSED]
- Replies: 4
- Views: 365
Re: Oxidation numbers [ENDORSED]
For the example in class on Friday ((H+) + (MnO4)- + 5(Fe 2+)) --> Mn2+ + 5(Fe)3+ + 4H20), we know that oxygen always has an oxidation number of -2 so in Mn(O4)-, 4(-2) = -8 so Mn + (-8) = -1 meaning that Mn has to have +7 charge on the reactants side. On the products side, we're told that the overa...
- Mon Feb 10, 2020 1:57 am
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Cv
- Replies: 3
- Views: 217
Re: Cv
I think they'll be provided on the formula sheet but here are the formulas you'd use anyways:
Ideal gas: Cp = (5/2)R
Ideal gas: Cv = (3/2)R
Ideal gas: Cp = (5/2)R
Ideal gas: Cv = (3/2)R
- Mon Feb 10, 2020 1:44 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: q=CΔT
- Replies: 5
- Views: 340
Re: q=CΔT
Yes, I believe you would use this equation for calorimetry problems. Can someone explain to me why you don't use mass?
- Mon Feb 10, 2020 1:40 am
- Forum: Administrative Questions and Class Announcements
- Topic: Midterm Conversion
- Replies: 3
- Views: 241
Re: Midterm Conversion
I think you'll be given this value, but just for reference 1 L times atm = 101.325 J.
- Mon Feb 10, 2020 1:36 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Enthalpy Definition
- Replies: 2
- Views: 140
Re: Enthalpy Definition
Yes, enthalpy will only equal heat of a reaction at constant pressure.
- Mon Feb 10, 2020 1:32 am
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: irreversible vs reversible
- Replies: 3
- Views: 192
Re: irreversible vs reversible
Here's a graphical representation of both. One thing to note is that the work done under a reversible process will always be greater than that done under irreversible, as you can see.
- Mon Feb 03, 2020 2:16 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: state functions
- Replies: 10
- Views: 385
Re: state functions
Examples: energy, pressure, volume, temperature, density, heat capacity
Non-examples: work, heat
Non-examples: work, heat
- Mon Feb 03, 2020 2:12 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: taking phase change into account
- Replies: 5
- Views: 180
Re: taking phase change into account
Also, in addition to what is being said above, something to remember: whenever you're dealing with phase changes, you have to calculate the heat required in 2 different steps. For example, if you're trying to go from a block of ice at 0 degrees to water at 50 degrees, you first need to find the heat...
- Mon Feb 03, 2020 2:09 am
- Forum: Student Social/Study Group
- Topic: Test 1 Solution
- Replies: 6
- Views: 563
Re: Test 1 Solution
I don't think it'll be posted online because only the midterm answers were posted for Chem 14A last quarter, but you can ask your TA to go over it with you. Or you can post a specific question here.
- Mon Feb 03, 2020 2:05 am
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: kinetics
- Replies: 8
- Views: 244
Re: kinetics
We haven't gone over kinetics yesterday but he mentioned it a little in class to emphasize that delta G could tell us about a reaction's spontaneity (but a spontaneous reaction isn't necessarily a fast one because to find out about a reaction's speed/rate you'd have to consider kinetics and not ther...
- Mon Feb 03, 2020 2:01 am
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: States of a system
- Replies: 3
- Views: 81
Re: States of a system
For the example he gave us in class, we had 2 possible states (represented by the two circular ends) and 2 particles (A and B), so we do (# of states)^(# of particles) = 2^2 = 4 microstates possible.
- Mon Jan 27, 2020 2:43 pm
- Forum: Student Social/Study Group
- Topic: midterm/final
- Replies: 12
- Views: 2274
Re: midterm/final
I feel like I studied for the tests, midterm, and final the same way though. Even if they are structured a little differently, they're basically all word problems so doing the book problems and going over notes is still the best way to study.
- Mon Jan 27, 2020 2:38 pm
- Forum: Phase Changes & Related Calculations
- Topic: State Property
- Replies: 6
- Views: 213
Re: State Property
Could someone also explain why heat is not a state property? Thanks! If it's heat given off under constant pressure, then it's basically enthalpy so yes, it would be a state property because the path DOES matter as you take into account what intermediate steps where needed to get to the final tempe...
- Mon Jan 27, 2020 2:34 pm
- Forum: Student Social/Study Group
- Topic: Chemical Bonding Recording
- Replies: 1
- Views: 132
Re: Chemical Bonding Recording
That's really cool! I like how you can see the rhenium atoms travelling around and then coming into the carbon nanotubes -- makes the concept of bond formation and breaking easier to visualize on a microscopic level.
- Mon Jan 27, 2020 2:27 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Extensive vs intensive propeties
- Replies: 5
- Views: 379
Re: Extensive vs intensive propeties
Also, what is the difference between intensive properties and state properties? State properties don't really take into account the "path" of how the substance was prepared (like altitude, pressure, volume, temperature). I think you mean to ask about the difference between intensive and e...
- Mon Jan 27, 2020 2:21 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Units for temperature?
- Replies: 11
- Views: 580
Re: Units for temperature?
The change in heat per celsius is the same as the change in heat per kelvin, so you could use either.
- Mon Jan 20, 2020 3:26 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Identifying endothermic vs exothermic
- Replies: 7
- Views: 318
Re: Identifying endothermic vs exothermic
You can also look at bond enthalpies or use Hess's Law to figure out the total energy on the reactants and products side or the energy needed to form/break the bonds and if delta H < 0, it's exothermic and if delta H > 0, it's endothermic.
- Mon Jan 20, 2020 3:21 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Effect of Increasing Temperature on an Equilibrium System
- Replies: 4
- Views: 455
Re: Effect of Increasing Temperature on an Equilibrium System
It might help if you view heat as another reactant (for an endothermic reaction) or as another product (for an exothermic reaction). If you add more of a reactant, according to Le Chatelier's, the effect of the change will need to be minimized so the reaction will proceed to the right. So in an endo...
- Mon Jan 20, 2020 3:14 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: ice table
- Replies: 5
- Views: 264
Re: ice table
The ICE table is just supposed to help you write your equilibrium constant expression and to track changes in the concentrations of the reactants and products. Your final Kc expression won't include solids and liquids, so you wouldn't have any values for them in your ICE table.
- Mon Jan 20, 2020 3:11 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Pressure changes
- Replies: 7
- Views: 227
Re: Pressure changes
The easy way to tell what changes will occur is to see how the moles of gas on the reactants and products sides differ. If the volume (moles of gas) is lower on the products side, then the reaction shifts to the right but if the volume (moles of gas) is higher on the products side, the reaction shif...
- Mon Jan 20, 2020 3:06 am
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: 6B.11
- Replies: 2
- Views: 178
Re: 6B.11
Yes, Na2O (s) + H2O (l) ⇌ 2Na+ (aq) + 2OH- (aq) is the correct reaction
- Thu Jan 16, 2020 9:38 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Percent Ionization
- Replies: 11
- Views: 389
Re: Percent Ionization
If you don't use the quadratic equation, you still want to justify your reason for ignoring the "-x" terms in your equilibrium by saying that since x is less than 5% of the initial concentration, its change is negligible.
- Thu Jan 16, 2020 9:33 am
- Forum: Acidity & Basicity Constants and The Conjugate Seesaw
- Topic: kA and kB
- Replies: 3
- Views: 241
Re: kA and kB
Yes, and you observe the same thing with H+ concentration and pH as well. The higher the H+ concentration, the lower the pH and the stronger the acid. It's just in the nature of natural logarithms.
- Thu Jan 16, 2020 9:29 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Today's lecture
- Replies: 5
- Views: 189
Re: Today's lecture
pKa is dependent on Ka so if the Ka is greater than 10^-7, then the pKa would be less than 7 but if Ka is less than 10^-7, then the pKa would be greater than 7.
Matt Sanruk 2H wrote:Wouldn't pKa give an integer thats less than 7?
- Thu Jan 16, 2020 9:21 am
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Approximation
- Replies: 6
- Views: 389
Re: Approximation
In class, he also said that if your Ka is less than 10^(-3), then you can generally approximate by ignoring the "-x" term but you might want to justify it on the test by explaining that since x is less than 5% of the initial concentration, it's considered a negligible difference so it can ...
- Thu Jan 16, 2020 9:18 am
- Forum: Ideal Gases
- Topic: R constant
- Replies: 6
- Views: 284
Re: R constant
It generally won't tell you exactly what R value to use, but all the constants are given in the formula sheet so depending on whether pressure is reported in atm or kilopascals, you'll know which R-value to use. Lavelle gives you 4 different values for the R constant on his formula sheet during test...
- Thu Jan 09, 2020 12:29 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 5G.1C
- Replies: 3
- Views: 156
Re: 5G.1C
If you start with a higher reactant pressure, you'll have a lower reactant volume (because increasing pressure tends to compress volume) so the equilibrium will actually shift left to make up for that loss in volume, according to Le Chatelier's Principle. So, with the reaction shifting left, the equ...
- Thu Jan 09, 2020 12:23 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 5I.29
- Replies: 2
- Views: 89
Re: 5I.29
5% Rule: If x/(initial concentration) < 5%, then you can ignore the "-2x" term but if not, then you'd need to use the quadratic formula. Make sure you write out the rule to justify ignoring the "-x" terms whenever you have this type of problem
- Thu Jan 09, 2020 12:17 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: K of Ionic Compounds in Solution
- Replies: 4
- Views: 223
Re: K of Ionic Compounds in Solution
Basically, it's telling you to ignore spectator ions like Li+, Na+, K+, Rb+, Sr2+, Ba2+, Cl-, Br-, I-, NO3-, ClO4-, SO4(2-), etc. because these ions occur in the same form on the left and right side of the chemical equation. So when you're writing your equilibrium constant expression they'd cancel a...
- Thu Jan 09, 2020 12:07 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: ICE tables
- Replies: 1
- Views: 69
Re: ICE tables
Yes, so for example if you have 2NO2 in equilibrium with N2O4, your left hand side of the ICE table would be (initial concentration of 2NO2) - 2x and your right hand side would be (initial concentration of N2O4) + x.
- Thu Jan 09, 2020 12:00 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 5I.23
- Replies: 1
- Views: 104
Re: 5I.23
Whenever you make an ICE table, you should be listing the concentration values, not the number of moles.
- Tue Dec 03, 2019 2:21 pm
- Forum: Naming
- Topic: Oxidation Number
- Replies: 3
- Views: 152
Re: Oxidation Number
Here's an example:
K2CrO4
we know that K has a charge of +1 so 2(+1) = +2 and O has a charge of -2 so -2(4) = -8. The molecule is neutral and we're trying to find the oxidation number of the transition metal so (+2) + Cr - 8 = 0 so Cr = +6.
K2CrO4
we know that K has a charge of +1 so 2(+1) = +2 and O has a charge of -2 so -2(4) = -8. The molecule is neutral and we're trying to find the oxidation number of the transition metal so (+2) + Cr - 8 = 0 so Cr = +6.
- Tue Dec 03, 2019 2:10 pm
- Forum: Hybridization
- Topic: Conceptual meaning of hybridization
- Replies: 3
- Views: 240
Re: Conceptual meaning of hybridization
In hybridization, you basically have atomic orbitals mixing into new hybrid orbitals in order to better pair electrons to form chemical bonds in VSEPR (affecting molecular geometry and bonding properties). And yes, this does lower the energy of the molecule, so hybridized molecules are more stable.
- Tue Dec 03, 2019 2:01 pm
- Forum: Identifying Acidic & Basic Salts
- Topic: deciding whether the solution of a salt is basic, acidic, or neutral
- Replies: 5
- Views: 667
Re: deciding whether the solution of a salt is basic, acidic, or neutral
If, in the presence of water, a salt gains an H+ (becoming an acid) and produces OH- ions, the solution will be basic. If, in the presence of water, a salt loses an H+ (becoming a base) and produces H+ ions, the solution will be basic. ex: C2H3O2 (-) (aq) + H2O (l) ---> HC2H3O2 (aq) + OH- (aq) so ba...
- Tue Dec 03, 2019 1:31 pm
- Forum: Lewis Acids & Bases
- Topic: diff b/w lewis acid and base
- Replies: 12
- Views: 730
Re: diff b/w lewis acid and base
Also, generally speaking, anions will act as Lewis bases (donate an electron pair) while cations act as Lewis acids (accept an electron pair)
- Tue Dec 03, 2019 1:29 pm
- Forum: Acidity & Basicity Constants and The Conjugate Seesaw
- Topic: pKa vs Ka
- Replies: 6
- Views: 476
Re: pKa vs Ka
For a very weak acid, the Ka can be an extremely small number, so to deal with such numbers, we use the pKa, which converts the Ka values to larger numbers we're more familiar with. It also allows for convenience with graphing.
- Tue Nov 26, 2019 2:51 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Oxidation Number vs. Coordination Number
- Replies: 8
- Views: 1411
Re: Oxidation Number vs. Coordination Number
Here's an example of a problem involving coordination numbers: In Co(NH3)6, the coordination number is 6 because you have 6 ligands attached to the central atom Co. CO3 (2-) has a coordination number of 3 because of the 3 oxygens surrounding the carbon atom. You can relate coordination numbers to mo...
- Tue Nov 26, 2019 2:43 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Oxidation state
- Replies: 3
- Views: 254
Re: Oxidation state
For example, if you want to find the oxidation number for Cr in CrCl3, you have to start off by figuring out the charges you DO know (the charges of the non-TM ions). Group 17 elements have an oxidation number of -1 so 3(-1) = -3. The charge of the overall molecule is 0 and we only have one Cr atom,...
- Tue Nov 26, 2019 2:38 pm
- Forum: Bronsted Acids & Bases
- Topic: Memorizing the Bronsted Acids and Bases
- Replies: 4
- Views: 351
Re: Memorizing the Bronsted Acids and Bases
It will be helpful (later on, in Chem 14B) to know all the strong acids because there are only 7 and any acid that isn't one of those 7 will automatically be weak. So when we do more acid-base equilibria that involve math, it'll be pretty useful. Here they are: 1) HClO4 - perchloric acid 2) HClO3 - ...
- Tue Nov 26, 2019 2:27 pm
- Forum: Lewis Acids & Bases
- Topic: Lewis vs Bronsted Acids and Bases
- Replies: 3
- Views: 562
Re: Lewis vs Bronsted Acids and Bases
So the Bronsted acid/base theory deals with PROTON transfer (Bronsted acids donate a proton while Bronsted bases accept a proton). The Lewis acid/base theory deals with ELECTRON PAIR transfer (Lewis acids accept an electron pair while Lewis bases donate an electron pair). Generally, all Bronsted aci...
- Tue Nov 26, 2019 2:19 pm
- Forum: Bronsted Acids & Bases
- Topic: Definition
- Replies: 5
- Views: 191
Re: Definition
In addition to the previous answer, you can look at the following examples: - Acetic acid (CH3COOH) is a Bronsted acid because it donates a hydrogen atom to water -- it's a proton donor basically, so you're left with CH3COO- (the conjugate base). And in this case, water would be the Bronsted base be...
- Thu Nov 21, 2019 12:11 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angle of bent
- Replies: 17
- Views: 1390
Re: Bond Angle of bent
Also, if you're dealing with water, the shape is also bent but the bond angle would be 104 degrees due to the presence of 2 lone pairs, which pushes the bonded atoms even closer together, further reducing the bond angle.
- Thu Nov 21, 2019 12:08 am
- Forum: Dipole Moments
- Topic: Intermolecular forces
- Replies: 2
- Views: 279
Re: Intermolecular forces
SBr4 is a nonpolar molecule because the central atom (S) is surrounded by 4 identical (Br) molecules that are equivalent in their electronegativity, so the dipoles cancel each other out, and as a result, there is no dipole-dipole interaction. The individual bonds can still be polar but the whole mol...
- Thu Nov 21, 2019 12:03 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles
- Replies: 6
- Views: 406
Re: Bond Angles
The presence of lone pairs causes a higher repulsion since in terms of repulsion, lone pair---lone pair > lone pair---bonded atom > bonded atom---bonded atom, so the lone pair will take the place of a bonded atom and essentially exert greater repelling force against the other atoms, pushing them clo...
- Wed Nov 20, 2019 11:56 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Name confusion
- Replies: 4
- Views: 303
Re: Name confusion
You'll only be expected to name the shape molecularly (not electronically). So in your case, you'd name the molecules as T-shaped because trigonal bipyramidal only tells you that there are 5 regions of electron density (assuming that atoms also count as electron-rich areas). 5 regions of electron de...
- Wed Nov 20, 2019 11:51 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: Strengths of forces
- Replies: 4
- Views: 305
Re: Strengths of forces
Hydrogen bonds will always be stronger than other dipole-dipole interactions because hydrogen bonds occur between a partially positive hydrogen atom and a highly electronegative atom (N, O, F), so the dipole will automatically be at one of its strongest in a hydrogen bond, and therefore, the polarit...
- Thu Nov 14, 2019 3:13 am
- Forum: Electronegativity
- Topic: oxygen vs nitrogen electronegativity
- Replies: 3
- Views: 1833
Re: oxygen vs nitrogen electronegativity
Oxygen's ionization energy is lower than that of nitrogen because nitrogen has 3 electrons in the p-shell so it's half-full but oxygen has 4 electrons so there will be one set of paired electrons and 2 unbonded electrons, making it less stable. To be more stable, we're more likely to pull out the ex...
- Thu Nov 14, 2019 3:05 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Difference between molecular shape
- Replies: 3
- Views: 307
Re: Difference between molecular shape
Seesaws: 1 LP, seesaw molecular shape, trigonal bipyramidal electron arrangement, bond angles of 90 and 120 degrees Tetrahedral: 0 LP, tetrahedral molecular shape, tetrahedral electron arrangement, bond angles of 109.5 degrees Trigonal pyramidal: 1 LP, trigonal pyramidal molecular shape, tetrahedral...
- Thu Nov 14, 2019 2:46 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles Exceptions
- Replies: 6
- Views: 387
Re: Bond Angles Exceptions
Adding on to those answers above, since Cl is a larger atom than H (larger radius) and its electron density is also higher, it'll tend to push the H atom inward more, reducing the angle further (so it's less than 109.5 degrees). You can observe the same with CH3F too.
- Thu Nov 14, 2019 2:34 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Axial vs Equatorial Lone Pairs
- Replies: 2
- Views: 217
Re: Axial vs Equatorial Lone Pairs
Lone pairs in particular will occupy equatorial positions because that's where they face the least repulsion (more energetically favorable). For example, for a trigonal bipyramidal structure, if you have the lone pair on the axial plane, it'll be 90 degrees away from 3 regions of electron density bu...
- Thu Nov 14, 2019 2:17 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Memorization
- Replies: 15
- Views: 1043
Re: Memorization
You might be able to use this table to help you conceptualize the models
https://web.gccaz.edu/~kimld88531/VSEPR%20handout.pdf
https://web.gccaz.edu/~kimld88531/VSEPR%20handout.pdf
- Fri Nov 08, 2019 7:03 pm
- Forum: Dipole Moments
- Topic: Dipole - Dipole vs. Hydrogen Bonding
- Replies: 7
- Views: 1723
Re: Dipole - Dipole vs. Hydrogen Bonding
N,O, and F tend to bond with H in a hydrogen bond and since they're more electronegative, they'll result in a higher polarity with the positive hydrogen so the bond will also be stronger than a normal dipole-dipole.
- Fri Nov 08, 2019 6:47 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Reference Table for VSEPR
- Replies: 3
- Views: 251
- Fri Nov 08, 2019 6:24 pm
- Forum: Dipole Moments
- Topic: Hydrogen Bonds
- Replies: 6
- Views: 354
Re: Hydrogen Bonds
For hydrogen bonds and dipole-dipole bonds, you're looking at the strength of the bond between partially + and partially - atoms. Since N,O, and F usually bond with H in a hydrogen bond and they tend to be more electronegative, they'll result in a higher polarity against the positive hydrogen so the...
- Fri Nov 08, 2019 6:15 pm
- Forum: Lewis Structures
- Topic: Hybridization
- Replies: 2
- Views: 251
Re: Hybridization
Hybridized orbitals tend to have lower energy states than unhybridized ones, so it's mostly for stability. It also helps predict the molecular geometry better by VSEPR (so bonds are more accurate in distance/angles).
- Fri Nov 08, 2019 6:07 pm
- Forum: Dipole Moments
- Topic: Electric Dipole Moment
- Replies: 2
- Views: 115
Re: Electric Dipole Moment
It's basically a measure of how polarizable a system is. It'll tell you how the + and - electrical charges are spread with the equation p = q*d where q = magnitude and d = distance between a pair of opposite charges.
- Sun Nov 03, 2019 11:57 pm
- Forum: Trends in The Periodic Table
- Topic: Atomic Radius
- Replies: 30
- Views: 3199
Re: Atomic Radius
The radius increases as you go down a group (because you're adding more shells) and decreases as you go to the right across a period (because electrons are added to the same shell and the electrostatic attraction increases L-->R so the increasing nuclear charge draws them inwards and radii length de...
- Sun Nov 03, 2019 11:51 pm
- Forum: Properties of Electrons
- Topic: Rydberg Constant
- Replies: 2
- Views: 192
Re: Rydberg Constant
So you'd use it for atomic spectra (since the energy at a specific shell is denoted by -hR/n^2) and you could find the frequency emitted from one level to another by doing E(final) - E(initial). You'd apply En = -hR/n^2 to the two different n values (or shells) and then subtract the two to find the ...
- Sun Nov 03, 2019 11:39 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal charge
- Replies: 16
- Views: 949
Re: Formal charge
If you can't narrow it down, you might want the negative formal charge to be on the more electronegative atom. For example, you can refer to #12 on the Dino Nuggets Midterm, where we ultimately chose our structure to be N --- N - O instead of N -- N -- O because we'd rather have the -1 charge on the...
- Sun Nov 03, 2019 11:26 pm
- Forum: Trends in The Periodic Table
- Topic: ionization energy vs electronegativity
- Replies: 4
- Views: 196
Re: ionization energy vs electronegativity
Ionization energy is the amount of energy you need to remove an electron from an atom/ion while electronegativity is how likely an atom is to gain/attract an electron.
- Sun Nov 03, 2019 2:15 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: paul and hundd rules
- Replies: 4
- Views: 297
Re: paul and hundd rules
They might ask you to identify which rule is being violated when filling shells (like they did for #9j on the Dino Nuggets practice midterm). So it would help to know that Pauli's Exclusion Principle says you can only have 2 electrons per orbital that must be spin-paired and that Hund's Rule says th...
- Sat Oct 26, 2019 6:20 pm
- Forum: Ionic & Covalent Bonds
- Topic: "Delocalized" Electrons
- Replies: 5
- Views: 259
Re: "Delocalized" Electrons
Delocalized electrons are basically the electrons that aren't fixed to any particular atom or covalent bond. They're the ones that you see go back and forth, from one atom to another, resulting in the resonance structures we see for molecules like benzene (where the double bonds constantly change po...
- Sat Oct 26, 2019 6:06 pm
- Forum: Ionic & Covalent Bonds
- Topic: Resonance (all bonds are a hybrid of different bonds)
- Replies: 10
- Views: 422
Re: Resonance (all bonds are a hybrid of different bonds)
I've noticed that for molecules like carbonate and benzene, they may have you draw out all the resonance forms OR you can use dotted lines to represent the bonds that change from one structure to another. Here's an example.
- Sat Oct 26, 2019 5:55 pm
- Forum: Ionic & Covalent Bonds
- Topic: + and - ions
- Replies: 3
- Views: 277
Re: + and - ions
1. Fe^+ has the same config as Mn. 2. Fe^- has the same config as Co. 3. Fe^+ means that Fe lost an electron. 4. Fe^- means that Fe gained an electron. You can think of Fe as initially a neutral molecule [Fe]. But by adding a minus sign after it, as [Fe]^-, you're saying that it has one additional e...
- Sat Oct 26, 2019 5:28 pm
- Forum: Lewis Structures
- Topic: Homework 2C #15
- Replies: 3
- Views: 177
Re: Homework 2C #15
Also, just some general rules for finding the lowest energy resonance structure:
- most atoms with FC = 0
- lower FC in general (negative is good too!)
- resonance forms with opposite sign charge on adjacent atoms
- most electronegative atoms
- most number of octets
- most atoms with FC = 0
- lower FC in general (negative is good too!)
- resonance forms with opposite sign charge on adjacent atoms
- most electronegative atoms
- most number of octets
- Sat Oct 26, 2019 5:01 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charge
- Replies: 7
- Views: 459
Re: Formal Charge
It also helps you keep track of the electrons and can help you predict the reactivity of the molecule. It assumes that all electrons are shared equally so you don't have to worry about bond polarity contributing to differences in potential. It'll help more when we do coordinate covalent complexes la...
- Sun Oct 20, 2019 2:27 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Overlapping
- Replies: 4
- Views: 194
Re: Overlapping
The reason the orbitals overlap more as you move away from the nucleus is because the distance between the shells decreases so as they move closer together, the orbitals overlap more. As a result, the potential energy drops and new electrostatic interactions and bonds between the orbitals form.
- Sun Oct 20, 2019 2:20 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Aufbau Principle
- Replies: 3
- Views: 194
Re: Aufbau Principle
It's basically the "building up" principle, which helps you determine electron configuration. It says electrons with lower energy levels with tend to fill up first. Here's a diagram of the order.
- Sun Oct 20, 2019 1:52 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Structure of electrons
- Replies: 5
- Views: 198
Re: Structure of electrons
This picture might help. Orbitals are arranged into shells and subshells. Shells are orbitals with the same value of n & subshells are orbitals with the same value of n and l. In the picture, you'll notice that anything from energy level "2" is of the same shell (so 2s and 2p belong to...
- Sun Oct 20, 2019 1:12 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Short Hand
- Replies: 11
- Views: 476
Re: Short Hand
So you want to base your shorthand off of the last element in the previous row (the last noble gas before your element). Chromium belongs in period 4 so you'd go to the previous row (period 3) and move to the last element (group 18), which is Argon. The "s" block consists of groups 1-2, th...
- Sun Oct 20, 2019 1:10 am
- Forum: Quantum Numbers and The H-Atom
- Topic: Magnetic Spin
- Replies: 4
- Views: 191
Re: Magnetic Spin
The magnetic spin is used in the context of the spin magnetic number (the fourth quantum number that you use to describe an electron), so it is somewhat important. We denote the spin with either a +1/2 or a -1/2, which means the electron either spins clockwise or counterclockwise. No 2 electrons in ...
- Sun Oct 20, 2019 12:42 am
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Spin up and spin down
- Replies: 13
- Views: 1200
Re: Spin up and spin down
You only really need to know about the electron spins in the context of the spin magnetic number (the fourth quantum number that you use to describe an electron). We denote the spin with either a +1/2 or a -1/2, which means the electron either spins clockwise or counterclockwise. No 2 electrons in t...
- Thu Oct 10, 2019 10:00 pm
- Forum: Properties of Light
- Topic: Electromagnetic Spectrum
- Replies: 5
- Views: 299
Re: Electromagnetic Spectrum
I don't think you'll need to memorize the exact wavelengths, but you should have a good idea of where the different waves lie in relation to one another. It might also help to come up with examples for each. The "types of EM Radiation" picture in this site is pretty nice. https://www.brita...
- Thu Oct 10, 2019 9:44 pm
- Forum: Accuracy, Precision, Mole, Other Definitions
- Topic: Rounding with basic calculator
- Replies: 16
- Views: 968
Re: Rounding with basic calculator
Use the "Ans" key on your calculator whenever possible. We're allowed to use scientific calculators but not graphing calculators, so you should be able to store values. Also, I generally leave at least 5 numbers after each decimal point (for each step) and apply sig figs at the very end.
- Thu Oct 10, 2019 9:37 pm
- Forum: Balancing Chemical Reactions
- Topic: Importance of the State of Molecules
- Replies: 6
- Views: 658
Re: Importance of the State of Molecules
The state will usually be given to you in the problem (ex: 25ml of precipitate means solid, NaOH dissolved in water means aqueous). When we do acids/bases and solubility equilibria especially, you'll become familiar with which compounds dissociate in water (nitrates, acetates, compounds with group 1...
- Thu Oct 10, 2019 9:28 pm
- Forum: Balancing Chemical Reactions
- Topic: H 1
- Replies: 6
- Views: 629
Re: H 1
Also, oxygen won't generally be present in a reaction as one oxygen atom alone. Oxygen is a diatomic molecule, so it'll only show up in a reaction as O2. Here's a list of other diatomic molecules (hydrogen, oxygen, fluorine, bromine, iodine, nitrogen, chlorine.. AKA HOFBrINCl).
- Thu Oct 10, 2019 9:16 pm
- Forum: Significant Figures
- Topic: Final Answer
- Replies: 4
- Views: 274
Re: Final Answer
As Brian was saying, you want to make sure you're using the right number of sig figs first. Generally, if you're doing a lab and you're measuring amounts, it's better to use the whole number because it's easier to conceptualize 25ml than 2.5x10^(-2)L, but when you're answering a problem on paper, le...
- Thu Oct 03, 2019 3:04 am
- Forum: Significant Figures
- Topic: Powers of 10
- Replies: 10
- Views: 640
Re: Powers of 10
When performing calculations, you generally want to keep the powers (especially if you're dealing with a very small or large number). After calculations, you could express the powers in simpler units (just for convenience or when in a lab setting, where you can't measure negative exponents of 10). S...
- Thu Oct 03, 2019 2:56 am
- Forum: Accuracy, Precision, Mole, Other Definitions
- Topic: Fundamental E. 15 Question...
- Replies: 3
- Views: 1394
Re: Fundamental E. 15 Question...
One thing to keep in mind is that when you're trying to find the molecular formula of the sulfide, you shouldn't just add an "S" to the metal. Based on the molar mass of the metal, you should try and identify it so that you can figure out its charge. If you know it's charge, you can then f...
- Thu Oct 03, 2019 2:47 am
- Forum: Accuracy, Precision, Mole, Other Definitions
- Topic: Different types of formulas
- Replies: 2
- Views: 194
Re: Different types of formulas
I think it's more important to distinguish between an empirical formula (which shows you the simplest whole number ratio of atoms of each element in the compound) and a molecular formula (which shows the actual number of atoms of each element in a compound). A lot of sources online are using the ter...