instruction stringlengths 15 21.8k |
|---|
The key is that for vinylic and arylic carbocations the positive charge is in a (roughly) $\ce{sp^2}$ orbital - not a $\ce{p}$ orbital. The picture below shows these hybridizations in a vinylic cation on the left and a alkyl cation on the right. So the question becomes, why would creating positive charge in an $\ce{s... |
Why is the reaction between hydroxide and water reversible, when the reaction between oxygen ions and water is not? And is there a reason why the products of reaction 2) are written separately, instead of "2OH"?
1) OH + H2O <> H2O + OH
2) O + H2O > OH + OH |
Why is the reaction between hydroxide and water reversible, when the reaction between oxygen ions and water is not? |
Why is the reaction between hydroxide and water reversible, when the reaction between oxygen ions and water is not? And is there a reason why the products of reaction 2) are written separately, instead of "2OH"?
1) $\ce{OH- + H2O <=> H2O + OH-}$
2) $\ce{O^{2-} + H2O -> OH- + OH-}$ |
All reactions are reversible but some are more reversible than others. Some reactions are so little reversible that they are practically irreversible, like that reaction of yours between oxide anion and water.
It all comes down to comparing the stabilities of reactants and products. The actual question is, why is ox... |
Hydroxide is the strongest base in water (leveling effect). The first posted reaction is symmetric. Given reactant and product sides of the equation, how do you tell them apart?
Oxide is a much stronger base than hydroxide. The second reaction spontaneously proceeds to the right (leveling effect). If you look up... |
Correct, all reactions are reversible, just to different extents. Think about the combustion reaction in your vehicle. Is that reaction reversible? Sure, in that nothing is 100% irreversible. The reversing of the combustion just might take a while. But it's not reversible to any significant extent in the short and medi... |
Correct, all reactions are reversible, just to different extents. Think about the combustion reaction in your vehicle. Is that reaction reversible? Sure, in that nothing is 100% irreversible. The reversing of the combustion just might take a while. But it's not reversible to any significant extent in the short and medi... |
Does anyone know why it is so? Or tell me what are indicative of strong acids? |
Why alkali and alkali earth metals are indicative of a strong acid? |
Given that hydrogen atoms that are attached to a compound must be ionizable for the compound to be an acid, what prevents a hydrogen from being ionized? Is it solubility. If the bond is nonviolent, water could not dissolve the compound, and so hydrogen atoms are not ionizable. Is this correct? |
Alkali and alkali earth metals are not indicative of a strong acid; if anything, they're more indicative of a strong base, but this is one of those half-truths/Santa Claus/tooth fairy level "truths" that general chemistry textbooks tell students. Just because something has an "-OH" in it doesn't make it a base or an ac... |
Alkali and alkali earth metals are not indicative of a strong acid; if anything, they're more indicative of a strong base, but this is one of those half-truths/Santa Claus/tooth fairy level "truths" that general chemistry textbooks tell students. Just because something has an "-OH" in it doesn't make it a base or an ac... |
Alkali and alkali earth metals are not indicative of a strong acid; if anything, they're more indicative of a strong base, but this is one of those half-truths/Santa Claus/tooth fairy level "truths" that general chemistry textbooks tell students. Just because something has an "-OH" in it doesn't make it a base or an ac... |
Alkali and alkali earth metals are not indicative of a strong acid; if anything, they're more indicative of a strong base, but this is one of those half-truths/Santa Claus/tooth fairy level "truths" that general chemistry textbooks tell students. Just because something has an "-OH" in it doesn't make it a base or an ac... |
Alkali and alkali earth metals are not indicative of a strong acid; if anything, they're more indicative of a strong base, but this is one of those half-truths/Santa Claus/tooth fairy level "truths" that general chemistry textbooks tell students. Just because something has an "-OH" in it doesn't make it a base or an ac... |
Alkali and alkali earth metals are not indicative of a strong acid; if anything, they're more indicative of a strong base, but this is one of those half-truths/Santa Claus/tooth fairy level "truths" that general chemistry textbooks tell students. Just because something has an "-OH" in it doesn't make it a base or an ac... |
Alkali and alkali earth metals are not indicative of a strong acid; if anything, they're more indicative of a strong base, but this is one of those half-truths/Santa Claus/tooth fairy level "truths" that general chemistry textbooks tell students. Just because something has an "-OH" in it doesn't make it a base or an ac... |
Exactly, and to expand on what Nicolau mentions, we can discuss the leveling effect. A chemist (can't remember who) found that some acids - e.g. hydrochloric acid and nitric acid - have the same strength in water. How can this be? They're clearly different, yet they have the same strength in water. This is because thes... |
Alkali and alkali earth metals are not indicative of a strong acid; if anything, they're more indicative of a strong base, but this is one of those half-truths/Santa Claus/tooth fairy level "truths" that general chemistry textbooks tell students. Just because something has an "-OH" in it doesn't make it a base or an ac... |
Exactly, and to expand on what Nicolau mentions, we can discuss the leveling effect. A chemist (can't remember who) found that some acids - e.g. hydrochloric acid and nitric acid - have the same strength in water. How can this be? They're clearly different, yet they have the same strength in water. This is because thes... |
Exactly, and to expand on what Nicolau mentions, we can discuss the leveling effect. A chemist (can't remember who) found that some acids - e.g. hydrochloric acid and nitric acid - have the same strength in water. How can this be? They're clearly different, yet they have the same strength in water. This is because thes... |
Exactly, and to expand on what Nicolau mentions, we can discuss the leveling effect. A chemist (can't remember who) found that some acids - e.g. hydrochloric acid and nitric acid - have the same strength in water. How can this be? They're clearly different, yet they have the same strength in water. This is because thes... |
Exactly, and to expand on what Nicolau mentions, we can discuss the leveling effect. A chemist (can't remember who) found that some acids - e.g. hydrochloric acid and nitric acid - have the same strength in water. How can this be? They're clearly different, yet they have the same strength in water. This is because thes... |
This is the procedure I carried out in class:
1. Reduction of nitrobenzene by using tin and $HCl$ acid
2. After the completion of the reaction, $NaOH$ added to neutralize excess acid and dissolve any $Sn(OH)_2$
3. Steam distillation is carried out to obtain suspension of phenylamine
4. Salting carried out where $... |
What's the process called where you can use electricity to separate the oxygen and carbon from water ? Is it electrolysis? Can it be applied to other liquids? |
Which fragmentation is possible at this m/z value for phthalic acid diethyl ester?
I tried mac- Lafferty but it didn't solve my problem. |
Where does the characteristic peak for pthalic acid diethyl ester at m/z 149 originate? |
What's the process called where you can use electricity to separate the oxygen and hydrogen from water? Is it electrolysis? Can it be applied to other liquids? |
Which process is used to separate Hydrogen and Oxygen from Water? |
>Instead of carrying out distillation under reduced pressure at the end of the procedure to remove the ether, could I have just carried out simple distillation?
You could have performed any procedure to remove the solvent:
- Simple distillation - This would be slower than what you did and could overheat the und... |
The fine structure in the diatomic vibrational spectra is based on various population of the rotational levels.
The best demonstration of isotopic effects in vibrational spectra is to switch hydrogen for deuterium.
The frequency of vibration (from [Hooke's Law][1] adapted to a harmonic oscillator) is given by:
... |
"*in excess of 2000 litres of water... per gram of dessicant [sic].*"
1) What is the volume of one gram of desiccant? <BR>
2) What is the volume of 2000 liters of water? <BR>
3) What is the cognitive dissonance?
y = sin(1/x) in the interval (0,1). Rotate about the x-axis. The volume of the cylinder is pi. The... |
How does carbonic acid cause acid rain when Kb of bicarbonate is greater than Ka? Should it not create an alkaline solution? |
How does carbonic acid cause acid rain when Kb of bicarbonate is greater than Ka? |
What is the $\ce{K_a}$ of carbonic acid? Note that sources differ in their $\ce{K_a}$ values, and especially for carbonic acid, since there are two kinds - a pseudo-carbonic acid/hydrated carbon dioxide and the real thing (which exists in equilibrium with hydrated carbon dioxide but in a small concentration - about 4%... |
How does carbonic acid cause acid rain when Kb of bicarbonate is greater than Ka? Should it not create an alkaline solution?
Ka = 4,8*10^-11 (mol/L). Kb = 2,3*10^-8 (mol/L) |
What is the $\ce{K_a}$ of carbonic acid? Note that sources differ in their $\ce{K_a}$ values, and especially for carbonic acid, since there are two kinds - a pseudo-carbonic acid/hydrated carbon dioxide and the real thing (which exists in equilibrium with hydrated carbon dioxide but in a small concentration - about 4%... |
How does carbonic acid cause acid rain when Kb of bicarbonate is greater than Ka? Should it not create an alkaline solution?
Ka = 4,8*10^-11 (mol/L). Kb = 2,3*10^-8 (mol/L). These are the values for HCO3-.
These numbers are from a school book that I read, but it's not in English. It's called "Kjemi 1" by Harald ... |
What is the $\ce{K_a}$ of carbonic acid? Note that sources differ in their $\ce{K_a}$ values, and especially for carbonic acid, since there are two kinds - a pseudo-carbonic acid/hydrated carbon dioxide and the real thing (which exists in equilibrium with hydrated carbon dioxide but in a small concentration - about 4%... |
Exactly, and to expand on what Nicolau mentions, we can discuss the leveling effect. A chemist (can't remember who) found that some acids - e.g. hydrochloric acid and nitric acid - have the same strength in water. How can this be? They're clearly different, yet they have the same strength in water. This is because thes... |
Exactly, and to expand on what Nicolau mentions, we can discuss the leveling effect. A chemist (can't remember who) found that some acids - e.g. hydrochloric acid and nitric acid - have the same strength in water. How can this be? They're clearly different, yet they have the same strength in water. This is because thes... |
What is the $\ce{K_a}$ of carbonic acid? Note that sources differ in their $\ce{K_a}$ values, and especially for carbonic acid, since there are two kinds - a pseudo-carbonic acid/hydrated carbon dioxide and the real thing (which exists in equilibrium with hydrated carbon dioxide but in a small concentration - about 4%... |
Halogenoalkanes aren't very soluble in water because they can't form hydrogen bonds, and the energy required to break hydrogen bonds in water etc is more than is released when new bonds between the halogenoalkane and water are formed. But as fluorine forms hydrogen bonds why couldn't a fluoroalkane form hydrogen bonds ... |
Halogenoalkanes aren't very soluble in water because they can't form hydrogen bonds, and the energy required to break hydrogen bonds in water etc is more than is released when new bonds between the halogenoalkane and water are formed. But as fluorine forms hydrogen bonds why couldn't a fluoroalkane form hydrogen bonds ... |
I had a alcohol today. I have to determine whether it is a secondary or a tertiary alcohol. How do you this? Please explain the procedure and the apparatus. I have the solution waiting in my lab. |
How to differentiate secondary and tertiary alcohol? |
It's hard to evaluate Environmental Tobacco Smoke lifecycle, it can certainly react, be absorbed by organisms, or be diluted in rain, and be emitted again from the ground.
But in the end, I'm interested to understand (as a non expert) if the toxicity (cytotoxicity, genetoxicity) of the compounds decrease over time (... |
> The reaction of $\ce{(C5H5)Fe(CO)2Cl}$ with an
> equimolar amount of $\ce{Li+[C6H5]-}$ gives a product.
> Draw its structure and apply the 18 electron rule.
In a question I was given the molecular weight and percentages of each element in the compound. I worked out that there is $\ce{1 Fe}$, $\ce{13 C}$, $\ce{10... |
Haloalkanes aren't very soluble in water because they can't form hydrogen bonds, and the energy required to break hydrogen bonds in water etc is higher than the energy released when new bonds between the haloalkane and water are formed.
But as fluorine forms hydrogen bonds why couldn't a fluoroalkane form hydrogen ... |
These are the results I got for my experiment. I'm having trouble interpreting the results.
As you should be well aware of, Lithium and Strontium both burn with crimson red when they are placed in a flame. Now, I can't decide which one it is.
Then I was told to do an experiment with the same salt where I had to ... |
Are these structures equivalent?
**Image 1:**
http://i.minus.com/jnojtCx6wYvqD.png
**Image 2:**
![enter image description here][1]
[1]: https://i.stack.imgur.com/diAXS.jpg
|
Equivalent Cyclohexane Structures? |
**PREFACE:** I am no expert on this topic. My questions at the bottom may be off base.
Natural Bond Orbital ([NBO](http://en.wikipedia.org/wiki/Natural_bond_orbital)) analyses translates the complex quantum-mechanical wavefunction into a more tangible Lewis-dot-like formalism (natural Lewis structure). The introdu... |
Natural Bond Orbital (NBO) analyses: Physical significance/interpretation of E(2) 'stabilization energy'? |
**PREFACE:** I am no expert on this topic. My questions at the bottom may be off base.
Natural Bond Orbital ([NBO](http://en.wikipedia.org/wiki/Natural_bond_orbital)) analyses translates the complex quantum-mechanical wavefunction into a more tangible Lewis-dot-like formalism (natural Lewis structure). The introdu... |
**PREFACE:** I am no expert on this topic. My questions at the bottom may be off base. I have some experience with symmetry-adapted perturbation theory (SAPT) when it comes to analyzing intermolecular interactions. The total interaction energy of a system can be quantified in four different energy components includi... |
First, I realise this may not *strictly* quality as chemistry, but it is part of a quantum chemistry/quantum physics course, so I hope it goes through!
I have tried for hours to calculate the commutator of angular momentum in the differential form, but I cannot get the correct answer. This is my first experience wit... |
Would the line structure of formaldehyde, H2COH, simply be a straight line with a OH on the end of the line? |
About two weeks ago I put some ordinary unleaded petrol into a plastic water bottle, as a temporary measure (long story, don't ask!). It has now formed a reddish liquid at the bottom of the bottle.
The bottle was emptied prior to adding the petrol, but probably still contained a small amount of water when the fuel w... |
What is this red substance that has accumulated at the bottom of a plastic bottle full of petrol (see picture)? |
Are the following equivalent structures for 2-dimethylpropane? ![enter image description here][1]
[1]: https://i.stack.imgur.com/yRiRd.jpg |
Equivalent Line Angle Structures? |
Are the following equivalent structures for 2-dimethylpropane? ![enter image description here][1]
I think so, because my rendering simply rotates the cross 45 degrees!
Also, regarding 3,3-diethylpentane, are these both equally valid structures? My rendering seems to look way different but filling in the carbon... |
Is ammonia a nucleophile and hydrogen the electrophile in the B/L acid-base reaction of acietic acid with ammonia?
I say that ammonia is the nucleophile because I drew a curved arrow from the lone pair on the ammonia to the ionizable hydrogen on acetic acid, and I drew a curved arrow from the bonding pair in the hy... |
I have a problem with this graphic, specifically the right hand side.
![enter image description here][1]
[1]: https://i.stack.imgur.com/a4nnv.gif
Why a "sextet" atom (an atom with 6 valence electrons)? I thought only a select few elements (C, N, and O) actually follow the octet rule. |
My book indicates that the following electron pushing is wrong:
![enter image description here][1]
[1]: https://i.stack.imgur.com/1ejqM.png
So what would the right electron pushing diagram be?
I have the following in mind. My rationale is:
1) Electrons attack protons, not the other way around.
2) ... |
My book indicates that the following electron pushing is wrong:
![enter image description here][1]
So what would the right electron pushing diagram be?
I have the following in mind. My rationale is:
1) Electrons attack protons, not the other way around. This is just convention right? Is this just a conce... |
acids are usually corrosive but what determines this? Is it the concentration of the acid or strength of the acid ($K_a$ value)? |
Acids are usually corrosive but what determines this? Is it the concentration of the acid or strength of the acid ($K_a$ value)? |
What are the factors that affect the corrosiveness of an acid? |
How. Does. NaCl. Maintain. Its. Crystalline. Structure. ? Its. a. Good. Question. Because. In. Crystalline. Structure. Of. NaCl. 6. Electrons . of Na+ ion. Is. Surrounded. By. 6. Electrons Of. Cl- ion and. 6. Electrons. Of. Cl- ... |
Where you find this picture? Very misleading. When sextet is mentioned, the better way is to say is lone pair acceptor or Lewis Acid. You simply need one empty molecular orbital on the atom to be able to do all the steps in the picture. In the case for common B, C, N and O they happen to be preferring sixtet. However, ... |
How does $\ce{NaCl}$ maintain its crystalline structure? It is a good question. Because in crystalline structure of $\ce{NaCl}$ 6 electrons of $\ce{Na+}$ ion are surrounded by 6 electrons of $\ce{Cl-}$ ion and 6 electrons of $\ce{Cl-}$ ion are surrounded by 6 electrons of $\ce{Na+}$. So $\ce{NaCl}$ maintains its cryst... |
How does $\ce{NaCl}$ maintain its crystalline structure? It is a good question.
Because in crystalline structure of $\ce{NaCl}$ 6 electrons of $\ce{Na+}$ ion are surrounded by 6 electrons of $\ce{Cl-}$ ion and 6 electrons of $\ce{Cl-}$ ion are surrounded by 6 electrons of $\ce{Na+}$. That's how $\ce{NaCl}$ maintai... |
I just got night contact lenses, and you are supposed to use a "one-step" cleaning solution to clean it over a period of six hours. At the bottom of the lenses case, there is a "titanium plate neutralizer", which causes the liquid to bubble. What is this gas? |
What is formed when hydrogen peroxide reacts with titanium? |
Does corrosion follow the law of conservation of mass? |
Your question is not very clear.
Did you just heat the salt water? Or you have put electrode to electrolysis water? What material is your electrode? Copper?
Let me assume you are using copper electrode to electrolyze brine. Then you will have the following reactions:
Cathode: $\ce{Cu - 2e -> Cu^2+}$
Anode: $\... |
Your question is not very clear.
Did you just heat the salt water? Or you have put electrode to electrolysis water? What material is your electrode? Copper?
Let me assume you are using copper electrode to electrolyze brine. Then you will have the following reactions:
Cathode: $$\ce{Cu - 2e -> Cu^2+}$$
Anode: ... |
What type of probe or probe coating should one use to measure the temperature of a roughly 100c aqueous solution of cupric chloride?
A stainless steel probe seems incorrect. Is a Teflon coated probe sufficient or is something else more appropriate?
Is there a standard way of protecting metal probes in corrosive liqui... |
What is the correct temperature probe for a wet etch solution? |
Why is $Fe(OH_2)_6^{3+}$ fairly acidic? This iron has six water molecules coordinated to it.
In other words, water itself is a very weak acid. But when water is coordinated to iron, it becomes more acidic. I can think of a few reasons; can you think of more?
1) Induction. The negative charge generated through lo... |
Why is $Fe(OH_2)_6^{3+}$ fairly acidic? This iron has six water molecules coordinated to it.
In other words, water itself is a very weak acid. But when water is coordinated to iron, it becomes more acidic. I can think of a few reasons; can you think of more?
1) Induction. The negative charge generated through lo... |
Why is $Fe(OH_2)_6^{3+}$ fairly acidic? This iron has six water molecules coordinated to it.
In other words, water itself is a very weak acid. But when water is coordinated to iron, it becomes more acidic. I can think of a few reasons; can you think of more?
1) Induction. The negative charge generated through lo... |
Why is $Fe(OH_2)_6^{3+}$ fairly acidic? This iron has six water molecules coordinated to it.
In other words, water itself is a very weak acid. But when water is coordinated to iron, it becomes more acidic. I can think of a few reasons; can you think of more?
1) Induction. The negative charge generated through lo... |
Why is $Fe(OH_2)_6^{3+}$ fairly acidic? This iron has six water molecules coordinated to it.
In other words, water itself is a very weak acid. But when water is coordinated to iron, it becomes more acidic. I can think of a few reasons; can you think of more? Also are my reasons valid?
1) Induction. The negative... |
Can a s orbital overlap with a any p orbital to form a sigma bond? |
I just got night contact lenses, and you are supposed to use a "one-step" cleaning solution to clean it over a period of six hours. At the bottom of the lenses case, there is a "titanium plate neutralizer", which causes the liquid to bubble. What is this gas?
Edit: it was platinum, not titanium |
Can a s orbital overlap with any p orbital to form a sigma bond? |
How does boric acid behave as an acid? Is it a Lewis acid or a Bronsted-Lowry acid? |
Stumbled across this interesting practice problem in my organic textbook. I have a few reasons for why $H_4N^+$ is less acidic than $H_3O^+$.
1) Let's assess conjugate stability first. Conjugates are $H_3N$ and $H_2O$. Let's look at central atom oxidation state. Nitrogen in ammonia has an oxidation state of negative... |
I came across this definition.
When discussing nucleophilicity we’re specifically talking about donating a pair of electrons to an atom other than hydrogen (usually carbon). When a species is donating a pair of electrons to a hydrogen (more specifically, a proton, H+) we call it a base.
Website:
http://www.m... |
I came across this definition.
When discussing nucleophilicity we’re specifically talking about donating a pair of electrons to an atom other than hydrogen (usually carbon). When a species is donating a pair of electrons to a hydrogen (more specifically, a proton, H+) we call it a base.
Website:
http://www.m... |
It does not exclude a base of being a nucleophile. It is just that a specific label is provided for a pair of electrons being donated to the hydrogen ion.
Are all bases nucleophiles? There are 2 definitions for a base, a lone pair doner and/or a hydrogen ion accepter. For many compounds, a base is also a nucleophile... |
So I was thinking about corrosion and I came across this structure(see image)
Do you think the inner metal/alloy that is corroding is steel?
Also, what do you think the outer layer (in white) is? perhaps the metal is just coated with paint to avoid corrosion?
Finally, what type of corrosion do you think its ... |
What type of material is this and how is it corroding? |
> how do i find the number of structural and configurational isomers of a given compound?
is there any formula?
example question: find the number of structural and configurational isomers of a bromo compound C5H9Br formed by addition of HBr to 2-pentyne |
>Why is $\ce Co(SCN)_4$ blue?
I simply can't predict the colors of such inorganic salts. I have learnt that $\ce {Co^{2+}}$ salts are pink in color. Also, if the ligand is a strong field ligand ($\ce {SCN-}$ in this case), then the splitting is more and the color should shift to the red side...
Is my concept wron... |
Why is $\ce Co(SCN)_4$ blue? |
Subsets and Splits
No community queries yet
The top public SQL queries from the community will appear here once available.