Resolved Question
Why giant ionic substance conduct electricity and why giant substances (except graphite) do not?
by joeyeehu...
Chemistry
Best Answer - Chosen by Voters
Giant ionic substance can conduct electricity only in aqueous state or in molten state. In solid state, it cannot conduct electricity because the ions are not mobile.
Giant metallic substance can conduct electricity either in solid or in molten states. This is so because it has delocalised electrons that can act as charge carrier.
Giant covalent compounds cannot conduct electricity neither in solid nor molten states.
Although graphite is a covalently bonded, it has one delocalised electron per carbon atom.
( sp2 hybridised orbitals). Hence it can conduct electricity.
Monday 31 August 2009
CaF2 - Acidic or Basic
Resolved Question
Is CaF2 (calcium fluoride) acidic or basic? Is Ca(OH)2 a strong or weak base?
So I learned to look at where each ion came from.
Ex: NaCl is a neutral salt because NaOH is a strong base and HCl is a strong acid.
If you have NaF, this is slightly basic since NaOH is a strong base and F comes
from HF which is a weak acid...
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by joeyeehu...
Chemistry
Best Answer - Chosen by Voters
You are right. CaF2 is slightly basic.The reason is HF is a weak acid ( but it is very corrosive).When dissolved in water, the F- ion formed will undergoes hydrolysis reaction with water molecules forming HF and OH-. Thats why, it is basic.
F- + H2O ---------------> HF + OH-
Ca(OH)2 is a strong base.
Is CaF2 (calcium fluoride) acidic or basic? Is Ca(OH)2 a strong or weak base?
So I learned to look at where each ion came from.
Ex: NaCl is a neutral salt because NaOH is a strong base and HCl is a strong acid.
If you have NaF, this is slightly basic since NaOH is a strong base and F comes
from HF which is a weak acid...
Report Abuse
by joeyeehu...
Chemistry
Best Answer - Chosen by Voters
You are right. CaF2 is slightly basic.The reason is HF is a weak acid ( but it is very corrosive).When dissolved in water, the F- ion formed will undergoes hydrolysis reaction with water molecules forming HF and OH-. Thats why, it is basic.
F- + H2O ---------------> HF + OH-
Ca(OH)2 is a strong base.
Thursday 27 August 2009
Bond length
Open Question
Chemistry:
Why are Triple Bond lengths shorter than Single and Double Bonds?
In Chemistry class we were told to hypothesize why we think bond lengths get shorter as multiple bonds increase, my question is, can someone explain it to me?I know that bond lengths in pecometers for C - C Single bonds is 154, in C - C Double bonds is 133, and 120 in C - C Triple bonds.
My assumption is that as more electrons become "shared" between the Carbon atoms, the orbitals become closer together. But why?
I know in the single bonds they are sp3, the double bond is sp2 and the triple bond is sp, does orbital shape have anything to do with why they are closer?
And I aslo know there are two pi bonds in the sp hybridized, C - C triple bonds, only one in the sp2 double bond and no pi bonds in the single bonded Carbon atoms. Does pi bonds havre anything to d with bond length?
I guess all this information just has me condused, maybe someone can set me straight?
Thnaks alot!
Answers (1)
by Timothy
There is an important electrostatic potential energy component to chemical bonding. When a bond forms, more electron density accumulates in the region between the positively charged nuclei than would be there if the electron "clouds" of the atoms just stayed the same as they are in isolated atoms. Since the electrons are negatively charged, when the probability of finding the electrons is greater in the region between the nuclei, the positively-charged nuclei are drawn together as they are attracted to the negatively charged electron density.
Thus, the electrons are the negatively charged "glue" that brings the positively charged nuclei together. In double and triple bonds, more electron density piles up in the region between the nuclei, so the nuclei are drawn together even more closely by their attraction to the electron density.
However, π bonds don't build up electron density directly between the nuclei, so π bonds don't add as much to the bond strength as σ bonds which do. π bonds shorten the bonds too, but their shortening effect is not as great as the effect of the σ bonds. Of course, π bonds always add to the effect of the σ bonds and therefore double bonds (σ + one π) and triple bonds (σ + two π) are stronger and shorter than single σ bonds alone.
Q: "I know in the single bonds they are sp³, the double bond is sp² and the triple bond is sp, does orbital shape have anything to do with why they are closer?"
A: Actually, yes. s orbitals are a little more contracted than p orbitals and the optimal distance between atoms for accumulating bonding electron density is consequently a little shorter when sp² hybrids are involved that when sp³ hybrids are involved; when sp hybrids are involved, the bonds a shortened a little bit more than when sp² hybrids are involved.
This small shortening can be seen by comparing the C–H bond distances in acetylene (H–C≡C–H, d(sp-CH) = 106 pm), ethylene (H₂C=CH₂, d(sp²-CH) = 108.7 pm) and ethane (H₃C–CH₃, d(sp³-CH) = 109.4 pm).
The differences in hybridization are less important than the difference due to bond order, however.
Full disclosure: This argument is fine as far as it goes, but there is also an important electronic kinetic energy contribution to bonding that requires a more sophisticated knowledge of the quantum mechanics of chemical bonds. I haven't attempted to explain that...
Source(s):
Chemistry professor
Chemistry:
Why are Triple Bond lengths shorter than Single and Double Bonds?
In Chemistry class we were told to hypothesize why we think bond lengths get shorter as multiple bonds increase, my question is, can someone explain it to me?I know that bond lengths in pecometers for C - C Single bonds is 154, in C - C Double bonds is 133, and 120 in C - C Triple bonds.
My assumption is that as more electrons become "shared" between the Carbon atoms, the orbitals become closer together. But why?
I know in the single bonds they are sp3, the double bond is sp2 and the triple bond is sp, does orbital shape have anything to do with why they are closer?
And I aslo know there are two pi bonds in the sp hybridized, C - C triple bonds, only one in the sp2 double bond and no pi bonds in the single bonded Carbon atoms. Does pi bonds havre anything to d with bond length?
I guess all this information just has me condused, maybe someone can set me straight?
Thnaks alot!
Answers (1)
by Timothy
There is an important electrostatic potential energy component to chemical bonding. When a bond forms, more electron density accumulates in the region between the positively charged nuclei than would be there if the electron "clouds" of the atoms just stayed the same as they are in isolated atoms. Since the electrons are negatively charged, when the probability of finding the electrons is greater in the region between the nuclei, the positively-charged nuclei are drawn together as they are attracted to the negatively charged electron density.
Thus, the electrons are the negatively charged "glue" that brings the positively charged nuclei together. In double and triple bonds, more electron density piles up in the region between the nuclei, so the nuclei are drawn together even more closely by their attraction to the electron density.
However, π bonds don't build up electron density directly between the nuclei, so π bonds don't add as much to the bond strength as σ bonds which do. π bonds shorten the bonds too, but their shortening effect is not as great as the effect of the σ bonds. Of course, π bonds always add to the effect of the σ bonds and therefore double bonds (σ + one π) and triple bonds (σ + two π) are stronger and shorter than single σ bonds alone.
Q: "I know in the single bonds they are sp³, the double bond is sp² and the triple bond is sp, does orbital shape have anything to do with why they are closer?"
A: Actually, yes. s orbitals are a little more contracted than p orbitals and the optimal distance between atoms for accumulating bonding electron density is consequently a little shorter when sp² hybrids are involved that when sp³ hybrids are involved; when sp hybrids are involved, the bonds a shortened a little bit more than when sp² hybrids are involved.
This small shortening can be seen by comparing the C–H bond distances in acetylene (H–C≡C–H, d(sp-CH) = 106 pm), ethylene (H₂C=CH₂, d(sp²-CH) = 108.7 pm) and ethane (H₃C–CH₃, d(sp³-CH) = 109.4 pm).
The differences in hybridization are less important than the difference due to bond order, however.
Full disclosure: This argument is fine as far as it goes, but there is also an important electronic kinetic energy contribution to bonding that requires a more sophisticated knowledge of the quantum mechanics of chemical bonds. I haven't attempted to explain that...
Source(s):
Chemistry professor
Saturday 22 August 2009
Half life
Resolved Question
Half life question...?
Hi, can someone give me a hand with this, i think i got the right idea, but it don't seem to give me the answer provided.
The radioactive isotope 51Cr is used to evaluate the lifetime of red blood cells.Its t½ = 27.7 days. A hospital laboratory has 80.0 mg of 51Cr. How much of 51Cr is left after 85 days?
Answer given = 9.6mg
by joeyeehu...
Best Answer - Chosen by Asker
All radioactive decay is a first order reaction.
First, you have to calculate the rate constant, k = 0.693/ t1/2
Therefore, k = 0.693 / 27.7
First order equation: ln Ao/A = kt
......................................ln 80/A = (0.693/27.7)(85)
Solving for A will give you the required answer.
Ao = initial mass
A = the mass after time,t
Half life question...?
Hi, can someone give me a hand with this, i think i got the right idea, but it don't seem to give me the answer provided.
The radioactive isotope 51Cr is used to evaluate the lifetime of red blood cells.Its t½ = 27.7 days. A hospital laboratory has 80.0 mg of 51Cr. How much of 51Cr is left after 85 days?
Answer given = 9.6mg
by joeyeehu...
Best Answer - Chosen by Asker
All radioactive decay is a first order reaction.
First, you have to calculate the rate constant, k = 0.693/ t1/2
Therefore, k = 0.693 / 27.7
First order equation: ln Ao/A = kt
......................................ln 80/A = (0.693/27.7)(85)
Solving for A will give you the required answer.
Ao = initial mass
A = the mass after time,t
Buffer solutions
Resolved Question
Which of the following canot function as a buffer solution:
HCN and KCN,
HF and NaF,
HNO3 and NaNO3,...?
HNO2 and NaNO2, or
NH3 and (NH4)2 SO4
by joeyeehu...
Best Answer - Chosen by Voters
In order to function as a buffer, it must have two components:
a) a weak acid and its conjugate base or
b) a weak base and its conjugate acid
HNO3 is a strong acid, therefore HNO3 and NaNO3 cannot function as a buffer.
The rest are buffer solutions.
Which of the following canot function as a buffer solution:
HCN and KCN,
HF and NaF,
HNO3 and NaNO3,...?
HNO2 and NaNO2, or
NH3 and (NH4)2 SO4
by joeyeehu...
Best Answer - Chosen by Voters
In order to function as a buffer, it must have two components:
a) a weak acid and its conjugate base or
b) a weak base and its conjugate acid
HNO3 is a strong acid, therefore HNO3 and NaNO3 cannot function as a buffer.
The rest are buffer solutions.
Resolved Question
Need Help With This Rate Equation Question?
Following rate equation was determined from reaction
NO2+CO=NO+CO2:
Rate=k[NO2][CO]
The following mechanism has been proposed:
NO2 + CO=ONOCO (slow)
ONOCO= NO+CO2 (fast)
Determine if this mechanism is consistent with rate equation?
I wasn't fully sure if I done this correct but since the first reaction in the mechanism is slow it's the rate determining step and so the rate must be Rate=k[NO2][CO].
Can someone confirm this or do I need more info?
by joeyeehu...
Best Answer - Chosen by Asker
You are right in saying that the slow step is the rate determining step and you can write the rate equation from it. But the question is whether the mechanism proposed is consistent with the rate equation?
To confirm this, just add the two elementary steps proposed. You will get the overall equation. This shows that the mechanism proposed is consistent with the rate equation.
ONOCO is called the intermediate and it will not feature in the overall equation. If you get the intermediate in the overall equation, then the mechanism proposed is not correct.
Need Help With This Rate Equation Question?
Following rate equation was determined from reaction
NO2+CO=NO+CO2:
Rate=k[NO2][CO]
The following mechanism has been proposed:
NO2 + CO=ONOCO (slow)
ONOCO= NO+CO2 (fast)
Determine if this mechanism is consistent with rate equation?
I wasn't fully sure if I done this correct but since the first reaction in the mechanism is slow it's the rate determining step and so the rate must be Rate=k[NO2][CO].
Can someone confirm this or do I need more info?
by joeyeehu...
Best Answer - Chosen by Asker
You are right in saying that the slow step is the rate determining step and you can write the rate equation from it. But the question is whether the mechanism proposed is consistent with the rate equation?
To confirm this, just add the two elementary steps proposed. You will get the overall equation. This shows that the mechanism proposed is consistent with the rate equation.
ONOCO is called the intermediate and it will not feature in the overall equation. If you get the intermediate in the overall equation, then the mechanism proposed is not correct.
Resolved Question
How we can find hybridization state of carbon in organic compounds?
eg CH2=C=CH2(all 1st 2nd & 3rd carbons)?
by joeyeehu...
Best Answer - Chosen by Asker
For carbon, to determine the types of hybridisation formed, all you have to do is to determine the number of atoms or groups that are attached to the carbon atom.
If the number is:
a) 2 --------------------> sp
b) 3 --------------------> sp2
c) 4 --------------------> sp3
So, the first carbon ----------> 3 -----------> sp2
..... the second carbon -----> 2 -----------> sp
......the third carbon ------------3 ------------> sp2
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How we can find hybridization state of carbon in organic compounds?
eg CH2=C=CH2(all 1st 2nd & 3rd carbons)?
by joeyeehu...
Best Answer - Chosen by Asker
For carbon, to determine the types of hybridisation formed, all you have to do is to determine the number of atoms or groups that are attached to the carbon atom.
If the number is:
a) 2 --------------------> sp
b) 3 --------------------> sp2
c) 4 --------------------> sp3
So, the first carbon ----------> 3 -----------> sp2
..... the second carbon -----> 2 -----------> sp
......the third carbon ------------3 ------------> sp2
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Friday 21 August 2009
Resolved Question
What are the H-C-C,CCC and HCH Bond angle in butane?
what about others? Like methane, ethane, propane.
by joeyeehu...
Best Answer - Chosen by Voters
The structural formula of butane is CH3CH2CH2CH3.
All the carbon atoms are bonded to 4 neighbouring atoms tetrahedrally.
Just imagine that you are the carbon atom and you are in the centre of a triangular based pyramid.
The four neighbouring atoms attached to you are at the four corners of the pyramid.
All the bond angles will be 109.5 degree.
The same applies to methane, ethane and propane.
What are the H-C-C,CCC and HCH Bond angle in butane?
what about others? Like methane, ethane, propane.
by joeyeehu...
Best Answer - Chosen by Voters
The structural formula of butane is CH3CH2CH2CH3.
All the carbon atoms are bonded to 4 neighbouring atoms tetrahedrally.
Just imagine that you are the carbon atom and you are in the centre of a triangular based pyramid.
The four neighbouring atoms attached to you are at the four corners of the pyramid.
All the bond angles will be 109.5 degree.
The same applies to methane, ethane and propane.
Thursday 20 August 2009
Resolved Question
Why H2O has bond angle 105 but H2S has only 91.5?
by joeyeehu...
Best Answer - Chosen by Asker
Both oxygen and sulphur are in Group 16.
There are two lone pair each in H2O as well as in H2S.
But oxygen is more electronegative than sulphur.
Hence, the bonding pair of electrons in O-H bonds are drawn closer to O.
These electrons experience greater repulsive force compared to that in H2S.
Therefore, the HOH angle is greater than HSH angle.
Asker's Comment:
this answer is more understandable with simple laguage so a student like me will like this answer more than others
Why H2O has bond angle 105 but H2S has only 91.5?
by joeyeehu...
Best Answer - Chosen by Asker
Both oxygen and sulphur are in Group 16.
There are two lone pair each in H2O as well as in H2S.
But oxygen is more electronegative than sulphur.
Hence, the bonding pair of electrons in O-H bonds are drawn closer to O.
These electrons experience greater repulsive force compared to that in H2S.
Therefore, the HOH angle is greater than HSH angle.
Asker's Comment:
this answer is more understandable with simple laguage so a student like me will like this answer more than others
Resolved Question
What's the ionic product of water, Kw?
by joeyeehu...
Best Answer - Chosen by Asker
Water dissociates slightly to form ionsH2O <==========> H+ + OH-
The equilibrium constant Kw = [H+] [OH-]
[H2O] is left out from the equation as its concentration is virtually constant. (due to high concentration compared to the concentration of ions).
At 25 degree C, [H+] = [OH-] = 1.0 x 10^-7
Hence, Kw = 1.0 x 10^-14
What's the ionic product of water, Kw?
by joeyeehu...
Best Answer - Chosen by Asker
Water dissociates slightly to form ionsH2O <==========> H+ + OH-
The equilibrium constant Kw = [H+] [OH-]
[H2O] is left out from the equation as its concentration is virtually constant. (due to high concentration compared to the concentration of ions).
At 25 degree C, [H+] = [OH-] = 1.0 x 10^-7
Hence, Kw = 1.0 x 10^-14
Resolved Question
Is Thymol blue a suitable indicator for the following titrations?
Is Thymol blue (pKa=8.9) suitable indicator for each of the following titrations?
a) 0.10M HCL versus 0.10M KOH
b) 0.10M CH3COOH versus 0.10M KOH?
c) 0.10M HNO3 versus 0.10m NH3?
by joeyeehu...
Best Answer - Chosen by Asker
The choice of an indicator depends on the pH when the equivalent point is achieved.
The pH when the equivalent point is achieved must coincide with the pH range of the indicator.
a) is a titration of strong acid and strong base.
The equivalent point occurs between pH 3 to 10.
b) is a weak acid and strong base. The equivalent point occurs between pH 7 to 13
c) is a strong acid and a weak base. The equivalent point occurs between pH 3 to 7.
Hence, thymol blue (pKa = 8.9) is suitable to be used in (a) and (b) as it will change colour when the equivalent point is reached.
(c) is not suitable because it wont change colour eventhough the equivalent point is reached,.
Is Thymol blue a suitable indicator for the following titrations?
Is Thymol blue (pKa=8.9) suitable indicator for each of the following titrations?
a) 0.10M HCL versus 0.10M KOH
b) 0.10M CH3COOH versus 0.10M KOH?
c) 0.10M HNO3 versus 0.10m NH3?
by joeyeehu...
Best Answer - Chosen by Asker
The choice of an indicator depends on the pH when the equivalent point is achieved.
The pH when the equivalent point is achieved must coincide with the pH range of the indicator.
a) is a titration of strong acid and strong base.
The equivalent point occurs between pH 3 to 10.
b) is a weak acid and strong base. The equivalent point occurs between pH 7 to 13
c) is a strong acid and a weak base. The equivalent point occurs between pH 3 to 7.
Hence, thymol blue (pKa = 8.9) is suitable to be used in (a) and (b) as it will change colour when the equivalent point is reached.
(c) is not suitable because it wont change colour eventhough the equivalent point is reached,.
2. Balance the redox equations by the ion-electron method:
Br2 --> Br2O3- + Br-(in basic solution)?
It is easier to balance equations in basic solution by first balancing them in acidic solution.
1. Break up the reaction into two half-reactions.Br2 -----> Br2O31-Br2 -----> Br1-
2. Balance the main atoms; in this case, BrBr2 -----> Br2O31-
(Br already balanced)Br2 -----> 2Br1-
3. Balance the O by adding H2OBr2 + 3H2O -----> Br2O31-Br2 -----> 2Br1-
4. Balance the H by adding H+Br2 + 3H2O -----> Br2O31- + 6H+Br2 -----> 2Br1-
5. Balance the charges by adding e- to the more positive sides of each half-reaction.
Br2 + 3H2O -----> Br2O31- + 6H+ + 5e- (oxidation)Br2 + 2e- -----> 2Br1- (reduction)
6. Make the e- gained and lost equal. Multiply the top equation by 2 and the bottom one
by 5.2Br2 + 6H2O -----> 2Br2O31- + 12H+ + 10e-5Br2 + 10e- -----> 10Br1-
7. Add the two half-reactions.7Br2 + 6H2O -----> 2Br2O31- + 10Br1- + 12H+
The equation is balanced for an acidic solution.
8. To convert the equation to a basic solution, add the same number of OH- to each side of the
equation as there are H+.12OH- + 7Br2 + 6H2O -----> 2Br2O31- + 10Br1- + 12H+ + 12OH-
9. Combine the H+ and OH- to make water.
12OH- + 7Br2 + 6H2O -----> 2Br2O31- + 10Br1- + 12H20
10. Simplify the H2O12OH- + 7Br2 -----> 2Br2O31- + 10Br1- + 6H20
The equation is balanced for a basic solution. Note that both sides are -12 in charge and that
all atoms are balanced.
Br2 --> Br2O3- + Br-(in basic solution)?
It is easier to balance equations in basic solution by first balancing them in acidic solution.
1. Break up the reaction into two half-reactions.Br2 -----> Br2O31-Br2 -----> Br1-
2. Balance the main atoms; in this case, BrBr2 -----> Br2O31-
(Br already balanced)Br2 -----> 2Br1-
3. Balance the O by adding H2OBr2 + 3H2O -----> Br2O31-Br2 -----> 2Br1-
4. Balance the H by adding H+Br2 + 3H2O -----> Br2O31- + 6H+Br2 -----> 2Br1-
5. Balance the charges by adding e- to the more positive sides of each half-reaction.
Br2 + 3H2O -----> Br2O31- + 6H+ + 5e- (oxidation)Br2 + 2e- -----> 2Br1- (reduction)
6. Make the e- gained and lost equal. Multiply the top equation by 2 and the bottom one
by 5.2Br2 + 6H2O -----> 2Br2O31- + 12H+ + 10e-5Br2 + 10e- -----> 10Br1-
7. Add the two half-reactions.7Br2 + 6H2O -----> 2Br2O31- + 10Br1- + 12H+
The equation is balanced for an acidic solution.
8. To convert the equation to a basic solution, add the same number of OH- to each side of the
equation as there are H+.12OH- + 7Br2 + 6H2O -----> 2Br2O31- + 10Br1- + 12H+ + 12OH-
9. Combine the H+ and OH- to make water.
12OH- + 7Br2 + 6H2O -----> 2Br2O31- + 10Br1- + 12H20
10. Simplify the H2O12OH- + 7Br2 -----> 2Br2O31- + 10Br1- + 6H20
The equation is balanced for a basic solution. Note that both sides are -12 in charge and that
all atoms are balanced.
Tuesday 11 August 2009
Resolved Question
Calculate Ksp from titration experiment???10 points?
0.025L of Solution A [ Ca(OH)2 with 0.0125M of NaOH]...titrated against 0.0120L of HCl. [HCl] =0.1034
To break it down...
FIND: [OH-] from titration[OH-] from NaOH
[OH-] from Ca (OH)2 (by subtraction)[Ca2+]
Solubility of Ca(OH)2 in molL-1Ksp
by joeyeehu...
Best Answer - Chosen by Asker
No. of moles of HCl = 0.1034 x 0.0120 = 1.2408 x 10^-3 mol
That means total no. of moles of OH- = 1.2408 x 10^-3 mol
No. of moles of OH- from NaOH = 0.0125 x 0.025 = 3.125 x 10^-4
ThereforeNo. of moles of OH- from Ca(OH)2 = 1.2408 x 10^-3 - 3.125 x 10^-4= 9.283 x 10^-4
mol
Volume of solution A is 0.025L
Hence, [OH-] from Ca(OH)2 = 9.283 x 10^-4/ 0.025 M= 0.037132 M
[Ca2+] = 0.037132/2
Ksp = [Ca2+] [OH-]^2. = ( 0.037132) X { 0.037132/2 }^2. = 1.28 x 10^-5
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thanks
Calculate Ksp from titration experiment???10 points?
0.025L of Solution A [ Ca(OH)2 with 0.0125M of NaOH]...titrated against 0.0120L of HCl. [HCl] =0.1034
To break it down...
FIND: [OH-] from titration[OH-] from NaOH
[OH-] from Ca (OH)2 (by subtraction)[Ca2+]
Solubility of Ca(OH)2 in molL-1Ksp
by joeyeehu...
Best Answer - Chosen by Asker
No. of moles of HCl = 0.1034 x 0.0120 = 1.2408 x 10^-3 mol
That means total no. of moles of OH- = 1.2408 x 10^-3 mol
No. of moles of OH- from NaOH = 0.0125 x 0.025 = 3.125 x 10^-4
ThereforeNo. of moles of OH- from Ca(OH)2 = 1.2408 x 10^-3 - 3.125 x 10^-4= 9.283 x 10^-4
mol
Volume of solution A is 0.025L
Hence, [OH-] from Ca(OH)2 = 9.283 x 10^-4/ 0.025 M= 0.037132 M
[Ca2+] = 0.037132/2
Ksp = [Ca2+] [OH-]^2. = ( 0.037132) X { 0.037132/2 }^2. = 1.28 x 10^-5
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Resolved Question
Chemistry question- general organic?
Explanation of inductive effect and how it effects acidic behaviour??
by joeyeehu...
Best Answer - Chosen by Asker
Inductive effect can be divided into two types, positive inductive and negative inductive.A group or atom is said to have a positive inductive effect if it tends to push away electrons away from them(electron donating group). I will increase the electron charge density of its neighbour. Example of such group is the alkyl group ( CH3, C2H5 ).Electron withdrawing group will attract the electrons toward itself (negative inductive effect), ex. F, Cl, NO2. They will reduce the electron charge density of the O--H bond. This will weaken the O--H bond and the molecule is able to donate the H+ more easily. It increases acidic behaviour. ( acid is a proton(H+) donor )
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Asker's Comment:
Chemistry question- general organic?
Explanation of inductive effect and how it effects acidic behaviour??
by joeyeehu...
Best Answer - Chosen by Asker
Inductive effect can be divided into two types, positive inductive and negative inductive.A group or atom is said to have a positive inductive effect if it tends to push away electrons away from them(electron donating group). I will increase the electron charge density of its neighbour. Example of such group is the alkyl group ( CH3, C2H5 ).Electron withdrawing group will attract the electrons toward itself (negative inductive effect), ex. F, Cl, NO2. They will reduce the electron charge density of the O--H bond. This will weaken the O--H bond and the molecule is able to donate the H+ more easily. It increases acidic behaviour. ( acid is a proton(H+) donor )
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