Search found 100 matches
- Thu Mar 11, 2021 5:05 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Reducing/Oxidizing Agent
- Replies: 4
- Views: 273
Re: Reducing/Oxidizing Agent
A reducing agent is the species that gives up electrons in order to reduce a different species, since the reducing agent is giving up electrons this implies it is being oxidized. Th opposite is true for oxidizing agents; an oxidizing agent takes electrons so that a different species can be oxidized,...
- Thu Mar 11, 2021 4:53 pm
- Forum: First Order Reactions
- Topic: textbook 7B.3
- Replies: 4
- Views: 262
Re: textbook 7B.3
I was confused by this too but the question states that all the reactions are first-order so you need the first-order integrated equation regardless, what the 2A does is make you need to multiply [B]final by two (since 2 A are needed to produce 1 B) and then subtract that amount of A from the initia...
- Thu Mar 11, 2021 4:36 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3881634
Re: Post All Chemistry Jokes Here
probably the best xkcd comic to date
- Thu Mar 11, 2021 4:30 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cell Diagrams: Platinum
- Replies: 3
- Views: 253
Re: Cell Diagrams: Platinum
I believe all metals in their solid form are conductive, and I'm pretty sure mercury is conductive too as a liquid metal. The thing about platinum that makes it special is its inertness, otherwise zinc, copper, tin, etc will all work as conductors, as long as its solid it should be conductive. But t...
- Thu Mar 11, 2021 4:19 pm
- Forum: General Rate Laws
- Topic: liquids and solids
- Replies: 6
- Views: 477
Re: liquids and solids
I think generally rate laws are written for species that are all in the same phase, and then if one reactant is in excess (like water) it can be treated as a constant and not a variable. But I don't think there is any rule that says to ignore solids and liquids, you just need to know what is reactin...
- Thu Mar 11, 2021 4:14 pm
- Forum: First Order Reactions
- Topic: Sapling 11 week 10
- Replies: 3
- Views: 190
Re: Sapling 11 week 10
I used so the equation needs to be solved for t in 0.0296 = 0.0611(e^((-3.7x10^-5)(t))) and I got 326.458 minutes for t
Your equation looks right but you have 3x10^-5 in it and not 3.7x10^-5, even that small decimal has a huge effect on the answer
Your equation looks right but you have 3x10^-5 in it and not 3.7x10^-5, even that small decimal has a huge effect on the answer
- Tue Mar 09, 2021 5:25 pm
- Forum: General Rate Laws
- Topic: Sapling #13 confusion
- Replies: 4
- Views: 278
Sapling #13 confusion
So the final rate law has [OH-] in the denominator but that's an intermediate just like HClO, I guess it makes sense being in the denominator since increasing it will consume HClO which is needed in the slow step, but are there any other scenarios where we are allowed to have intermediates in the ra...
- Tue Mar 09, 2021 3:10 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3881634
Re: Post All Chemistry Jokes Here
How im studying for this final
- Tue Mar 09, 2021 11:53 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Deprotonated bases
- Replies: 2
- Views: 307
Re: Deprotonated bases
For this I guess it helps to look at the base version of the H-H equation, pOH = pKb + log(BH+/B) So if pOH < pKb then pOH - pKb is negative, so the equation becomes: -N = log(BH+/B), where -N is just some random negative number then if you get rid of the log by doing 10^ to both sides you get 10^-N...
- Tue Mar 09, 2021 11:42 am
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: Sapling week 9-10. #12
- Replies: 5
- Views: 770
Re: Sapling week 9-10. #12
so the general equation for a half life for an order greater than one (n>1) is \frac{2^{n-1}-1}{(n-1)(k)(C_{o}^{n-1})} so if you divide some half life t2 with initial concentration C2 over another half life t1 with initial concentration C1 you can derive the equation n = \fra...
- Sun Mar 07, 2021 9:30 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: shout cut to determining order with half life and initial concentration
- Replies: 3
- Views: 278
Re: shout cut to determining order with half life and initial concentration
The general equation for a half life for order n is t_{1/2} = \frac{2^{n-1}-1}{(n-1)kC_{o}^{n-1}} so if you divide some half life t2 with initial concentration C2 over another half life t1 with initial concentration C1 you get n = \frac{\ln t_{2}/t_{1}}{\ln C_{1}/C_{2}} + 1 and in this case ...
- Sun Mar 07, 2021 9:00 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Catalysts
- Replies: 4
- Views: 308
Re: Catalysts
I think poisoning is when something enters the site and gets stuck so the enzyme doesn't function anymore, and then denaturing is when the enzyme loses its physical structure to do its function, I quickly looked that up i'm sure there's a better/more specific answer
- Sun Mar 07, 2021 8:55 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Sapling Homework #20
- Replies: 1
- Views: 173
Re: Sapling Homework #20
I used the equation k_{2}/k_{1} = e^{-(E_{a1}-E_{a2})/RT} and k2/k1 is the answer but you have to be really careful about plugging the values in. The Ea values HAVE to be in joules so they both need to be multiplied by 1000, and then R = 8.314, and T is in Kelvins. Also be sure you plug in t...
- Sun Mar 07, 2021 8:38 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Rate constant vs endo/exothermic rxns
- Replies: 1
- Views: 165
Re: Rate constant vs endo/exothermic rxns
i'm not exactly sure either but I think it may depend on the Ea of each reaction. What i'm thinking is if kf < kr but Ea for the forward rxn is 100J/mol and the Ea for the reverse is 50J/mol, then that means the exothermic reverse reaction is more likely and the overall should be exothermic. I don't...
- Sun Mar 07, 2021 8:08 pm
- Forum: Zero Order Reactions
- Topic: Catalysts
- Replies: 6
- Views: 542
Re: Catalysts
I think catalysts help reactions (any order) become so fast that they act like zero-order reactions, without them the order is probably higher. This has to do with the fact that catalysts have special shapes that can make reactions more likely to happen, so the new rate is essentially only dependent...
- Sun Mar 07, 2021 7:54 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: Sapling Week 9/10 HW #6
- Replies: 2
- Views: 1042
Re: Sapling Week 9/10 HW #6
I think it might have to do with the fact that once you put the integrated rate law equations (ln[C] and 1/C) in terms of C, C(t) = A/e^kt and C(t) = A/(1+Akt), respectively, where A = C(0), then you see as time goes on the denominator increases which makes both equations follow a curve that kind of...
- Sun Mar 07, 2021 7:41 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: 7A.17
- Replies: 4
- Views: 275
Re: 7A.17
I remember the same thing happening to me and it honestly makes so sense, I don't know if there's an error or anything, but I did get the order of B as 2 using a different path. I found the order of A to be 2 using exp 1 and 2, then I skipped B and found the order of C to be 2 using exp 3 and 4, THE...
- Sun Mar 07, 2021 7:29 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: sapling #4 week 9/10
- Replies: 4
- Views: 239
Re: sapling #4 week 9/10
The units of k are tricky but here's a good method to figure them out: M/s = (x/y) * (M^n) What is means is the rate is always molarity per seconds, M/s is the rate R (x/y) is the units of k that will make that side equal to M/s And then M^n is the concentration of the reactants to the power of the ...
- Sun Mar 07, 2021 7:21 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: Determining Rate of Reaction with Multiple Reactants
- Replies: 2
- Views: 177
Re: Determining Rate of Reaction with Multiple Reactants
After you know the order of each reactant individually by forcing everything else to be zero-order, you now have the orders of all the reactants and then you add all those up and that's the overall order. So if I have the reaction A + B + C --> D and I found out their respective orders are 1, 0, and...
- Sun Mar 07, 2021 7:14 pm
- Forum: General Rate Laws
- Topic: sapling #2 week 9/10
- Replies: 7
- Views: 380
Re: sapling #2 week 9/10
maybe you're using scientific notation wrong? or not including enough digits? My numbers were a bit different but I did the same thing and it was right.
- Sun Mar 07, 2021 7:07 pm
- Forum: General Rate Laws
- Topic: plotting a graph in experiements?
- Replies: 5
- Views: 340
Re: plotting a graph in experiements?
I don't think theres an ICE box equivalent but if you know the k value, temperature, all initial reactant concentrations, and the rate law, you could use calculus to graph what would happen, but you need prior knowledge as mentioned. Otherwise you have to experimentally determine the a rate law that...
- Sun Mar 07, 2021 7:02 pm
- Forum: Balancing Redox Reactions
- Topic: What does balancing in acid/base mean in terms of solution pH
- Replies: 2
- Views: 253
What does balancing in acid/base mean in terms of solution pH
I know balancing redox in acid means you use H+ in the balancing process and H+ may appear in the overall reaction, and then basic is the opposite with using OH-, but what does that mean about the solution pH? If I balance in acid and H+ is a product, and then balance that in base and OH- becomes a ...
- Sun Mar 07, 2021 6:53 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3881634
Re: Post All Chemistry Jokes Here
What do you think the rate of people disappearing was, zero order? First order?
- Sun Mar 07, 2021 6:50 pm
- Forum: Balancing Redox Reactions
- Topic: Balancing Redox Reaction Tips
- Replies: 6
- Views: 430
Re: Balancing Redox Reaction Tips
So you know the first step, isolate the half reactions after writing out oxidation numbers. After that its just a mess but there is a lot you can do during the process to make sure you're on the right track. First, its very tempting to go right into adding water to balance oxygen in a half reaction ...
- Sun Mar 07, 2021 6:07 pm
- Forum: *Enzyme Kinetics
- Topic: Absorption
- Replies: 3
- Views: 348
Re: Absorption
I cannot remember him specifically describing the difference but I do believe he has mentioned that gases aDsorb onto platinum electrodes and metal catalysts to make the reaction happen faster. I think it might be one of those things that people assume everyone gets even though its kinda confusing, ...
- Thu Mar 04, 2021 9:36 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: What was your favorite chem topic?
- Replies: 137
- Views: 13037
Re: What was your favorite chem topic?
Redox and electrochem are my favorites by far, I love how there are two mini reactions working together and they can all be combined and matched together with their unique potentials
- Thu Mar 04, 2021 8:35 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: changing temp and rxn rates, textbook 7D, number 7 part c
- Replies: 1
- Views: 147
changing temp and rxn rates, textbook 7D, number 7 part c
I'm a little confused as to why increasing temperature changes the k of the forward reaction more than the reverse, I know it has to do with the Ea values but I can't quite wrap my head around it, can anyone explain it?
- Thu Mar 04, 2021 8:02 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Inert Electrodes [ENDORSED]
- Replies: 2
- Views: 232
Re: Inert Electrodes [ENDORSED]
I remember in high school we used graphite for the anode and cathode lol There's also a class of metals called "noble metals" which is kind of a play on the "noble gases" in the sense that these metals so not react very much compared to other elements, some examples include palla...
- Thu Mar 04, 2021 7:50 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3881634
Re: Post All Chemistry Jokes Here
I know i'm late w the redox meme but i hope you enjoy
- Thu Mar 04, 2021 7:43 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: steady-state approximation [ENDORSED]
- Replies: 3
- Views: 316
Re: steady-state approximation [ENDORSED]
Yikes I got lost too, but what really helped me get it was following it step by step and writing down the equations on a sheet of paper to do the math myself to make my brain go through the process visually. What I discovered is the rate of the thing you want (like rate of formation of NO2) is depen...
- Thu Mar 04, 2021 7:29 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: K value
- Replies: 20
- Views: 882
Re: K value
k is always a positive value since it is just a proportionality constant, for example you can say the rate is proportional to the square of concentration and then equate them by saying R = k*(C^2). But we only put the negative sign in front to denote that the reactants are being consumed and to rela...
- Mon Mar 01, 2021 3:03 pm
- Forum: Interesting Applications: Rechargeable Batteries (Cell Phones, Notebooks, Cars), Fuel Cells (Space Shuttle), Photovoltaic Cells (Solar Panels), Electrolysis, Rust
- Topic: Textbook Focus 6O
- Replies: 2
- Views: 330
Re: Textbook Focus 6O
I remember doing a lot more electrolysis in ap chem, one huge suggestion is know the conversions between charge, time, and current. For electroplating this big conversion is really helpful: Current and Time <--> Quantity of charge <--> Moles of Electrons <--> Moles of substance oxidized/reduced <-->...
- Mon Mar 01, 2021 2:02 pm
- Forum: General Rate Laws
- Topic: Number of Reactants
- Replies: 26
- Views: 1147
Re: Number of Reactants
I suppose you could, but only in theory. Dr. Lavelle mentioned it briefly but true third-order reactions are very uncommon. For a fourth-order reaction you would need, I think, four total molecules/atoms/ions interacting in the rate-determining step and that is very very unlikely. But that is only i...
- Mon Mar 01, 2021 1:49 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: Value of k throughout Experiments
- Replies: 5
- Views: 297
Re: Value of k throughout Experiments
k is constant but much like most constants it is dependent upon temperature, so I guess if your reaction is particularly endo/exo-thermic it may be tricky measuring k
- Mon Mar 01, 2021 1:40 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3881634
Re: Post All Chemistry Jokes Here
An appropriate meme for the kinetics unit
- Mon Mar 01, 2021 1:37 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Textbook 6L.7 part b
- Replies: 1
- Views: 169
Re: Textbook 6L.7 part b
So this one is weird and I hate it but the only two reactions that work for this are: O2(g) + 4H+(aq) + 4e- --> 2H2O(l), Ered= +1.23 V O2(g) + 2H2O(l) + 4e- --> 4OH-(aq), Ered= +0.401 V So you have to swap the sides of the second once since its Ered is lower and is less likely to be reduced so it is...
- Mon Mar 01, 2021 1:11 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Textbook Problem 6M.7
- Replies: 4
- Views: 272
Re: Textbook Problem 6M.7
So I looked up all the different potentials for all the metals for part A and the pattern seems to be that they want the reduction potentials for the SAME change in electrons. So for A you need Cu+2 --> Cu, Zn+2 --> Zn, Cr+2 --> Cr, Fe+2 --> Fe, and after you rank these redox potentials from most ne...
- Mon Mar 01, 2021 12:54 pm
- Forum: Zero Order Reactions
- Topic: Rate
- Replies: 2
- Views: 464
Re: Rate
I was confused by that too but this site explains it pretty well: https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Kinetics/02%3A_Reaction_Rates/2.10%3A_Zero-Order_Reactions It basically says zero order...
- Mon Mar 01, 2021 12:40 pm
- Forum: Zero Order Reactions
- Topic: Zero order
- Replies: 8
- Views: 697
Re: Zero order
Going off what Akash said, there's another example of adding a metal catalyst, and adding it makes it so much more likely that a reaction happens that it can change the order of a reactant to be zero since changing reactant concentration will have no effect on how fast the reaction is happening sinc...
- Wed Feb 10, 2021 8:53 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Delta S for Irreversible Reaction
- Replies: 1
- Views: 135
Re: Delta S for Irreversible Reaction
I believe the equations are the same since entropy is a state function and the path to final entropy does not matter, so both of their final entropies are the same. But irreversible processes cannot go back to the initial entropy after the final entropy is met, but reversible (not real) ones can.
- Wed Feb 10, 2021 8:44 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3881634
- Wed Feb 10, 2021 8:07 pm
- Forum: Calculating Work of Expansion
- Topic: How to Know When to use Cp and Cv
- Replies: 4
- Views: 247
Re: How to Know When to use Cp and Cv
so like the subscripts say, you need to know when volume is constant and when pressure is constant. Constant volume is usually in bomb calorimeters or other sealed containers or any situation where NO expansion work is done, so under these conditions the pressure is increasing/decreasing. And then c...
- Wed Feb 10, 2021 7:48 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: specific/molar heat capacity, intensive property
- Replies: 2
- Views: 168
Re: specific/molar heat capacity, intensive property
I think its because specific heat capacity (C sub s) has the dimension of joules per grams degrees Celsius (J/(g*C)). This means for water it will take 4.184 Joules of energy to raise one gram of water by one degree Celsius, and that is ALWAYS true one gram of water at STP, whereas heat capacity (no...
- Thu Feb 04, 2021 2:13 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Discrepancy in deltaH of combustion for 4.7
- Replies: 1
- Views: 117
Discrepancy in deltaH of combustion for 4.7
So I used the tabulated values and the formula deltaH rxn = sum(deltaH formation products) - sum(deltaH formation reactants) to get deltaH rxn for 2 C6H6 (L) + 15 O2 (g) -> 12 CO2 (g) + 6 H2O (g) and I got -6271kJ/mol, so -3135kJ/mol for one mole benzene. But then the textbook says the deltaH combus...
- Wed Feb 03, 2021 9:09 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Change in enthalpy at constant volume (4C.3b)
- Replies: 1
- Views: 131
Change in enthalpy at constant volume (4C.3b)
For 4C.3b the equation for delta H at a constant volume is deltaH = deltaU + nRdeltaT, and the energy put into the system is 765J, and the answer for deltaH is 1275J but I don't get where all this extra energy is coming from if 765J is being introduced. Does this mean the system gets more energy as ...
- Mon Jan 18, 2021 9:28 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Ka and Kb
- Replies: 3
- Views: 154
Re: Ka and Kb
Yeah it can since (Ka)x(Kb) is always equal to Kw=1x10^-14. So since you know Ka you rearrange the equation to get Kb = (Kw)/(Ka)
- Mon Jan 18, 2021 9:06 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 6D9
- Replies: 1
- Views: 141
Re: 6D9
After setting up the ICE chart you get 0.11-x for the E (equilibrium concentration) of HA, or undissociated benzoic acid, since you start off with 0.11M benzoic acid and then it dissociates into H+ and A- (general anion) so you lose some of the initial 0.11M to create [H+] and [A-]. But we also know...
- Mon Jan 18, 2021 8:56 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Ka2 << Ka1
- Replies: 12
- Views: 1187
Re: Ka2 << Ka1
It means that the first deprotonated species contributes so little hydrogen ion that it has a negligible effect on pH. In this case it means that after H2CO3 becomes H+ and HCO3-, technically HCO3- can dissociate into H+ and CO3-2, but that second Ka value (Ka2) is so small that the final [H+] when ...
- Mon Jan 18, 2021 8:40 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Sapling 6.19
- Replies: 1
- Views: 207
Re: Sapling 6.19
For 'a' the lactic acid adds a whole bunch of H+ and in the reaction the concentrations are always in the proportion of Kc (or Keq) so when you add H+ the HbO2- is used up and therefore decreases in concentration. And for 'b' you use similar reasoning, O2 is on the products side so adding a lot of O...
- Mon Jan 18, 2021 8:12 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Textbook 6E.3
- Replies: 1
- Views: 99
Re: Textbook 6E.3
I think it just means that the amount of hydrogen ion contributed by the first deprotonated species is so minimal it has a negligible effect on the pH, I did the first calculation and got 4.18 (4.22 without making x=0) both times. I think Ka2 is only useful in polyprotic titrations, otherwise it can...
- Mon Jan 18, 2021 7:51 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Textbook problem 6E.1
- Replies: 1
- Views: 127
Re: Textbook problem 6E.1
This is a polyprotic acid problem so you need to have the Ka1 and Ka2 values since one hydrogen will dissociate from H2SO4 (a strong acid so it happens completely) and then ANOTHER hydrogen will dissociate from whats left HSO4-, an anion. You dont have to set up an ICE chart for the first dissociati...
- Sun Dec 06, 2020 7:24 pm
- Forum: Air Pollution & Acid Rain
- Topic: acid rain
- Replies: 13
- Views: 1294
Re: acid rain
If you think about statues made by the ancient Greeks and how long ago they were made you would think that they would be long gone because of the rain eroding them constantly. But they lasted so long because only very recently did CO2 levels spike and increase acidity and cause their destruction. Ac...
- Sun Dec 06, 2020 7:14 pm
- Forum: Lewis Acids & Bases
- Topic: textbook 6.5
- Replies: 2
- Views: 127
Re: textbook 6.5
yeah, since SO3 is attached to three oxygens and then gains an attachment to one of the oxygens in H2O2, so SO3 accepts electrons making it a lewis acid, and then H2O2 the lewis base.
- Sun Dec 06, 2020 6:59 pm
- Forum: Polyprotic Acids & Bases
- Topic: multiple deprotonations and sulfuric acid
- Replies: 2
- Views: 183
Re: multiple deprotonations and sulfuric acid
It means the Ka1 for H2SO4 is greater than one so the ratio between H+ and H2SO4 (at eq) is so large that the amount of H2SO4 is trivial. For normal polyprotic acids I cannot think of much importance since the following Ka values are so small the amount of H+ they contribute is also trivial. Polypro...
- Sun Dec 06, 2020 6:52 pm
- Forum: Polyprotic Acids & Bases
- Topic: Textbook 6C.19
- Replies: 7
- Views: 528
Re: Textbook 6C.19
I like to think about it in terms of electronegativity, fluorine is THE most electronegative atom. It is extremely hard to contain it in its diatomic form F2 without it reacting. You will notice that some of the only compounds of noble gases are with fluorine. That is all to say is that when fluorin...
- Sun Dec 06, 2020 6:28 pm
- Forum: Calculating the pH of Salt Solutions
- Topic: AlCl3 pH
- Replies: 1
- Views: 409
Re: AlCl3 pH
The three chlorides are "spectator" ions meaning they do not participate in the reaction so they are ignored. I remember learning this in Ap, so when metal cations are in water they always form a hydrated complex with a number of water molecules twice the value of their oxidation state. So...
- Sun Dec 06, 2020 6:19 pm
- Forum: Acidity & Basicity Constants and The Conjugate Seesaw
- Topic: Pka and Ka
- Replies: 6
- Views: 382
Re: Pka and Ka
pKa literally means "potenz of the acid dissociation constant," potenz is "power" in German which is where the p comes from. It essentially asks for the opposite of value of the exponent of Ka. pKa is used for buffers and choosing indicators, and it can predict pH as well which i...
- Sun Dec 06, 2020 6:13 pm
- Forum: Polyprotic Acids & Bases
- Topic: Box 6E.1
- Replies: 2
- Views: 146
Re: Box 6E.1
I think he may just want us to realize not all acids are strong and not all have just one Ka value if they are polyprotic. I remember we had a longer list like that in high school but it was only used for reference during homework, and it also had Kb and pKb values. I honestly don't know why it is t...
- Sun Dec 06, 2020 6:05 pm
- Forum: Identifying Acidic & Basic Salts
- Topic: Concept of pH
- Replies: 10
- Views: 646
Re: Concept of pH
Acidic and basic solutions are important because they are really prone to electron transfer, meaning they are very reactive. For example, bleaching works because it is very reactive with dyes and ruins the structure that gives dyes their color. pH is important because living organisms take advantage...
- Sun Dec 06, 2020 5:50 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Sapling Week 10: #13 and #14
- Replies: 2
- Views: 171
Re: Sapling Week 10: #13 and #14
For weak bases and acids they exist in an equilibrium with an equilibrium constant Ka (acid dissociation constant). So only a certain amount of protons or hydroxide are dissociated out. This concentration determines the pH, the negative log of [H+] or [OH-]. pKa is the negative log of Ka which is al...
- Sun Dec 06, 2020 5:26 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: 6D.11
- Replies: 1
- Views: 94
Re: 6D.11
So for these you need to figure out where the cations and anions "came from" since salts are produced as the result of acid-base reactions. For example, KBr is formed when KOH and HBr react forming H20 and KBr. Now, we look at what the strength of these two acids and bases are. KOH is a st...
- Sun Dec 06, 2020 5:13 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Sapling #10. How can you tell which solution has a higher pH?
- Replies: 7
- Views: 2072
Re: Sapling #10. How can you tell which solution has a higher pH?
You have to first know which ones are strong acids and strong bases, these will be the highest and lowest pHs. Then, figure out which of those strong acids/bases gives off more H+ or OH-, Sr(OH)2 gives off 2 OH- so it is 'more' basic and has a higher pH. Then, figure out which are weak acids/bases a...
- Sun Dec 06, 2020 5:05 pm
- Forum: Properties & Structures of Inorganic & Organic Bases
- Topic: Equilibrium sign
- Replies: 9
- Views: 916
Re: Equilibrium sign
The Ka values of strong acids and bases are so large that it can be assumed that there is no back and forth between which species are present, there are just protons and anions.
- Sun Dec 06, 2020 5:00 pm
- Forum: Amphoteric Compounds
- Topic: Amphoteric Compound Acid/Base Character
- Replies: 4
- Views: 271
Re: Amphoteric Compound Acid/Base Character
amphoteric is when it can act as either an acid or base, regardless of strength of the acid or base
- Sun Dec 06, 2020 4:51 pm
- Forum: Amphoteric Compounds
- Topic: How to know if a molecule is amphoteric
- Replies: 9
- Views: 2169
Re: How to know if a molecule is amphoteric
Im pretty sure HSO4- is amphoteric, it has a Ka value and can give up protons as well as accept them. Also hydroxide (OH-) is amphoteric since it can accept a proton to become HOH (H20) or give one up to become oxide (02-). There is also the difference between amphoteric and amphiprotic, amphoteric ...
- Mon Nov 30, 2020 1:45 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: TM and coordination compounds
- Replies: 2
- Views: 364
Re: TM and coordination compounds
Water forms hydrates with a lot of compounds meaning it is acting as a lewis base and donating an electron pair. A well-known hydrate is epsom salts, which is magnesium sulfate. Water also forms complexes with other metals like sodium ions and aluminum ions when water dissolves them. I don't know ex...
- Mon Nov 30, 2020 1:08 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Ligands
- Replies: 9
- Views: 486
Re: Ligands
Ligands do not have to bond only with transition metals, aqueous sodium ions (and other metal ions) form hydrated complexes with water.
- Mon Nov 30, 2020 1:02 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: polydentate
- Replies: 4
- Views: 283
Re: polydentate
Polydentate are usually organic structures with ammine groups, which in english is a big carbon- net with a bunch of nitrogen groups, and the nitrogen groups are the ones that bond to the metal. They are usually abbreviated so if you see en, pn, dien, trien, EDTA then these are all polydentate. Then...
- Mon Nov 30, 2020 12:43 pm
- Forum: Naming
- Topic: 9C.3 textbook problem
- Replies: 3
- Views: 315
Re: 9C.3 textbook problem
I think putting oxalato before aquo is part of an old naming system. I found this old chem textbook whose directions for naming coordination compounds says the ligands on the name go "negative, neutral, positive" which is consistent with putting a negative (oxalate) before a neutral (water...
- Mon Nov 30, 2020 12:35 pm
- Forum: Naming
- Topic: Bis-, Tris-, etc
- Replies: 6
- Views: 300
Re: Bis-, Tris-, etc
An example is [Pt(en)2Cl2]Br2 whose name is: Dichlorobis(ethylenediamine)platinum(IV)
Another is the ion [Co(en)2(H20)2] 2+ with the name: Bis(ethylenediamine)diaquocobalt(II)
Another is the ion [Co(en)2(H20)2] 2+ with the name: Bis(ethylenediamine)diaquocobalt(II)
- Sun Nov 22, 2020 9:50 pm
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: Acids/Bases
- Replies: 7
- Views: 723
Re: Acids/Bases
Like someone said about not needing to know this yet but, there are only 7 strong acids that dissolve completely into H+ and anions, and then there are only a few strong bases which are hydroxides of all group one elements and Calcium, Strontium, and Barium. Otherwise any other acid or base only par...
- Sun Nov 22, 2020 9:39 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: Hydrogen Bonding Confusion
- Replies: 3
- Views: 336
Re: Hydrogen Bonding Confusion
They didn't explain it well in the textbook but I was always taught hydrogen bonds are between: 1. A partially positively charged hydrogen that is covalently bonded to a F, O, or N (because hydrogen bonding is "Fon") 2. A lone pair on any F, O, or N This means that water (hydrogen attached...
- Sun Nov 22, 2020 9:28 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Polarity from Lewis Structures
- Replies: 6
- Views: 341
Re: Polarity from Lewis Structures
We can look at electronegativities to see which atom has a higher electron density, and then you can draw dipole arrows which kinda look like this: +--->
the plus end is positive and the arrow end is negative, it will have a higher electron density
the plus end is positive and the arrow end is negative, it will have a higher electron density
- Sun Nov 22, 2020 9:26 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Molecular Shape of Large Molecules
- Replies: 3
- Views: 88
Re: Molecular Shape of Large Molecules
If you're looking at a lewis structure or organic shorthand you can also look at the dashes and bars for bonds to see "shape" of a molecule, since dashes denote a bond going "behind" the paper and bars denote bonds poking "out" of the page.
- Sun Nov 22, 2020 9:23 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Seesaw Shape
- Replies: 8
- Views: 488
Re: Seesaw Shape
The axial atoms are in the most favorable positions because of repulsion and keeping the atoms the furthest apart they can possibly be, and then the two equatorial atoms must be in a bent shape since the electron pair repels them. In this shape all the atoms are the spread the furthest away from eac...
- Sun Nov 15, 2020 8:40 pm
- Forum: Dipole Moments
- Topic: Dipoles vs Ions
- Replies: 5
- Views: 430
Re: Dipoles vs Ions
Like everyone is saying, the difference between the two is how electrons are shared, ionic completely moves the electron but dipoles unequally share them. But the way I like to think about unequal electron sharing in dipoles is the resonance structure. The bond in HF is a single bond where hydrogen ...
- Sun Nov 15, 2020 8:31 pm
- Forum: Dipole Moments
- Topic: Strength of intermolecular forces
- Replies: 3
- Views: 169
Re: Strength of intermolecular forces
I think what it means is dipoles are only temporary and can merge to become neutral, so in the case of two dipoles when they are separated from each other the two dipoles stop reciprocating charge with one another. But a point charge (like an ion) is ALWAYS a point charge no matter how far away it i...
- Sun Nov 15, 2020 8:24 pm
- Forum: Dipole Moments
- Topic: 3F.15 Question
- Replies: 2
- Views: 122
Re: 3F.15 Question
I know we haven't discussed structure yet but AsF5 has no net dipole whereas AsF3 does have a net dipole moment meaning it has partially charged ends. So AsF3 will act like a little magnet and be more difficult to separate leading to it needing more energy to break the dipole-dipole IMFs so it will ...
- Sun Nov 15, 2020 8:14 pm
- Forum: Dipole Moments
- Topic: Hydrocarbons
- Replies: 3
- Views: 193
Re: Hydrocarbons
We usually say induced-dipole induced-dipole because the properties of hydrocarbons change very quickly as the number of carbons in a hydrocarbon increases. So like for methane there is only one carbon and four hydrogens meaning there are very few electrons leading to a very low attraction due to in...
- Sun Nov 15, 2020 8:03 pm
- Forum: Coordinate Covalent Bonds
- Topic: Lewis Diagram
- Replies: 5
- Views: 270
Re: Lewis Diagram
One way you can "know" there is a coordinate covalent bond is when you see these brackets [ ] and a metal and a bunch of molecules/atoms all stuck together in a chemical formula. Like here's a random one: [Pt(NH3)3(Cl3)]Cl. I know the question was for lewis structures so when you see these...
- Sun Nov 08, 2020 6:12 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charge
- Replies: 4
- Views: 301
Re: Formal Charge
This is a hard one but I guess it comes down to how far apart the charges are being distributed, like if there was a single bond between the 0 and -2 in one but a triple between the -1 and -1 then the charges on the -1 -1 are not only closer to zero but they are closer together, and it takes energy ...
- Sun Nov 08, 2020 6:03 pm
- Forum: Polarisability of Anions, The Polarizing Power of Cations
- Topic: Polarizable
- Replies: 3
- Views: 140
Re: Polarizable
To be highly polarizable means that a molecule has so many electrons that sometimes a high density of electrons can be found on just one side of the atom. This high density all one one side creates a very temporary moment of unusually high negative charge, which means the other side without all thes...
- Sun Nov 08, 2020 5:53 pm
- Forum: Resonance Structures
- Topic: Identifying Delocalized Electrons
- Replies: 2
- Views: 190
Re: Identifying Delocalized Electrons
Also, and I know we don't talk a lot about d-block metals in this class, but when "identifying" delocalized electrons keep in mind that most of not all d-block metals do not keep the electrons in their outermost d-orbital very closely attached so they often move freely between themselves a...
- Sun Nov 08, 2020 5:47 pm
- Forum: Resonance Structures
- Topic: delocalized electron energy
- Replies: 3
- Views: 166
Re: delocalized electron energy
I don't know if an electron has a lot of energy per se, other than kinetic energy, do you mean it would take less energy to remove a delocalized electron? Because I would imagine if an electron isn't associated with any one atom then it would take less energy to remove since it is less tightly held,...
- Sun Nov 08, 2020 5:42 pm
- Forum: Resonance Structures
- Topic: Overall Structure of Ion - Sapling #4, W5
- Replies: 3
- Views: 297
Re: Overall Structure of Ion - Sapling #4, W5
Also you can find out which structure contributes the least by looking at experimental bond length. So if a molecule has three bonds and all three are determined to be the same at 155 picometers, but the single bond length would be 200pm and the double bond length would be 140pm, then you can probab...
- Sun Oct 25, 2020 8:23 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Chromium and Copper
- Replies: 5
- Views: 316
Re: Chromium and Copper
This also hold for chromium and coppers entire groups, 6 and 11 respectively. And yeah the d-block is weird since electrons are more stable when "symmetrical" with one another meaning a full or half full outermost d-sub level is most stable.
- Sun Oct 25, 2020 8:15 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: 1E.5 electrons penetrating the nucleus
- Replies: 1
- Views: 88
Re: 1E.5 electrons penetrating the nucleus
I think its bc s-orbitals don't have nodal planes or weird orbital shapes that form around the nucleus like p, d, and f orbitals do. s-orbitals are an evenly distributed sphere that can get very close to the nucleus without touching it so since they're more likely to be closer to the nucleus they ca...
- Sun Oct 25, 2020 8:06 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Advice for studying
- Replies: 92
- Views: 8838
Re: Advice for studying
For me I usually study in little bits rather than all at once or cram so I do one part of the textbook and its corresponding questions, and do a few sapling questions most days. And I also find videos online to be helpful if the textbook doesn't make sense
- Sun Oct 25, 2020 8:02 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Silver Atom
- Replies: 3
- Views: 148
Re: Silver Atom
the entire group 11 follows the same pattern, and then there's another weird group, 6, that fills half of its d orbitals after taking one electron from the outermost s orbital (for chromium its 3d5 4s1) since it is more stable to fill half of the d orbitals, much like how it is more stable to fill a...
- Sun Oct 25, 2020 7:53 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Effective Nuclear Charge
- Replies: 2
- Views: 114
Re: Effective Nuclear Charge
I think "effective nuclear charge" might mean the charges aren't balanced due to shielding and when charges aren't balanced one end of the atom has a different charge than the other leading the atom, despite its equal number of protons and electrons, to have charged ends
- Sun Oct 18, 2020 7:25 pm
- Forum: Properties of Light
- Topic: energy level transfer
- Replies: 7
- Views: 221
Re: energy level transfer
what i understood was the energy given off going between any two n levels is E = -(hR)/(n^2) so as you change n levels near infinity you don't really change and distance and when you don't move you don't do work so the energy change is 0. Honestly I'm not 100% clear on it either since I don't fully ...
- Sun Oct 18, 2020 7:19 pm
- Forum: Properties of Light
- Topic: Work Function
- Replies: 3
- Views: 222
Re: Work Function
The work function is like a threshold yeah, I don't know if theres a more "scientific" way to determine it but I got the impression it can be determined by doing the photoelectric experiment and using hv = p(Ke of electon) + (phi), and then solving for phi.
- Sun Oct 18, 2020 7:14 pm
- Forum: Properties of Light
- Topic: Spectroscopy Question
- Replies: 2
- Views: 92
Re: Spectroscopy Question
the wavelength of the light is different because energy and frequency of light are directly proportional since E = hv, so when larger jumps are made in the Lyman series there is a larger energy change and therefore a higher of frequency of light is emitted, and UV light has a high frequency
- Sun Oct 18, 2020 7:02 pm
- Forum: Trends in The Periodic Table
- Topic: electronegative of the elements in the periodic table
- Replies: 4
- Views: 286
Re: electronegative of the elements in the periodic table
Everything everyone said I agree with just metals in the "d" block (the middle) of the periodic table all have similar properties notwithstanding the group they are in. That is to say they don't act as consistent in groups as group 1, 2, 17, 18 that all act incredibly similar within their ...
- Sun Oct 18, 2020 6:53 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: Reading the Balmer and Lyman series model
- Replies: 3
- Views: 213
Re: Reading the Balmer and Lyman series model
if youre talking abt the model with the lines like n=1, n=2, etc then to read it you have to pay attention to the distance between the levels of n, its confusing but the distance between each level is not constant so the distance between n=1 and n=2 is much larger than the distance from n=3 to n=4, ...
- Fri Oct 09, 2020 4:37 pm
- Forum: Balancing Chemical Reactions
- Topic: Combining Atoms
- Replies: 7
- Views: 330
Re: Combining Atoms
Also another thing about writing out molecular formulas from names is sometimes they'll say "cuprOUS oxide" or "cuprIC oxide" and the thing is a lot of metals have two really common oxidation states (charges) and putting -ous infers the metal has the lower charge whereas putting ...
- Fri Oct 09, 2020 4:07 pm
- Forum: Balancing Chemical Reactions
- Topic: WK 1 Sapling #10
- Replies: 7
- Views: 260
Re: WK 1 Sapling #10
I think the bromine and magnesium are spectators? Like they don't play a meaningful part in the reaction and just end up as ions in solution and don't precipitate out (make a solid). And also this looks like an organic chem reaction so I don't think any of us understand exactly why it is the way it ...
- Fri Oct 09, 2020 3:59 pm
- Forum: Accuracy, Precision, Mole, Other Definitions
- Topic: Finding molar mass of sulfide of metal hydroxide? (E. 15)
- Replies: 3
- Views: 179
Re: Finding molar mass of sulfide of metal hydroxide? (E. 15)
Just be sure to remember the metal has a +2 charge and you need 2 sulfides
- Fri Oct 09, 2020 3:50 pm
- Forum: Accuracy, Precision, Mole, Other Definitions
- Topic: Molar Mass and Molecular Mass Difference?
- Replies: 24
- Views: 4842
Re: Molar Mass and Molecular Mass Difference?
Adding on to the isotope comment, the reason carbon's amu is 12.011 and not 12 is because the 12.011amu is the average of the masses of all carbon isotopes, so while most carbon is 12amu, there is a smaller fraction of carbon in the universe that weights more (13amu and 14amu) so after dividing the ...
- Fri Oct 09, 2020 3:42 pm
- Forum: Accuracy, Precision, Mole, Other Definitions
- Topic: Exercise E.9
- Replies: 6
- Views: 684
Re: Exercise E.9
To answer the part of your question pertaining to why it is hydrated is: a lot of (if not all) metals often form these "coordination complexes" where they bond with certain elements and molecules and ions (most notably water, ammonia, halides, etc.) and since water is extra "sticky&qu...