Questions tagged [bond]
For questions about chemical bonds (ionic/covalent/etc.), their properties (length, energy, angle, etc.) or their relation to other molecular properties (intermolecular forces/dipole moment/etc.). Do not confuse this tag with [lewis-structures], [dipole], [intermolecules-forces], etc.
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Why are double bonds shorter than single bonds?
We're told in chemistry class that the order of bond length is:
triple < double < single
Can anyone explain WHY this is the case? Is it because multiple bonds involve stronger attraction ...
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0answers
38 views
Why highly electropositive elements form strong bases?
I know that elements like sodium form hydroxides completely dissociate in water than magnesium hydroxide. I came to a conclusion that the nature of bonding may affect this result, that is ostensibly ...
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0answers
32 views
Non-Metallic properties shown by some metals [on hold]
I want to ask why Li, Be and Mg which are metals show Non-Metallic properties. I know they have small atomic size and high electronegativity as compared to other metals, but I don't know the reason ...
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38 views
Least/Lowest London Dispersion Force! [on hold]
What/Which would be the least London Dispersion Force? In the human body.
And How many eV would it be?
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0answers
39 views
Why do F and N don't make a bond? [closed]
The electronic Configuration of F has 2p5 in the end and N has 2p1 in the end.
So N can give one of it's electron to F to aquire stability? Why dosen't this happen ?
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1answer
56 views
Can atomicity be infinity?
My chemistry teacher told us that graphite or diamond had an atomicity of infinity. However, the definition of molecule in my testbook is
A molecule is the smallest part of an element or compound ...
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0answers
9 views
Species having greater Dipole moment [closed]
Which will have greater net dipole moment, arrange in ascending order? CH3Cl,CH2Cl2,CHCl3. Explain why.
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0answers
26 views
Bond length in hydrogen chloride
The interatomic distances in $\ce{H2}$ and $\ce{Cl2}$ are $74$ and $\pu{198 pm},$ respectively. Find the bond length of $\ce{HCl}.$
a. $\pu{136 pm}$
b. $>\pu{136 pm}$
c. $<\pu{136 pm}$
...
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0answers
19 views
Name a compound or molecule in which pi bondas are stronger than sigma bonds [closed]
According to the rule sigma bond is always stronger than pi bonds but is there any exception. Please explain the reasons too.
Name a compound or molecule in which pi bondas are stronger than sigma ...
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0answers
45 views
How is it possible to melt diamonds? [duplicate]
On another thread on this website it mentioned how it was possible to melt diamonds, but what would be the micro-level occur for that to happen. This question applies to Silicon Oxide aswell. They ...
3
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1answer
60 views
How does resonance fail in approximating chemical structures?
In the book "Concise Inorganic Chemistry" by Prof. JD Lee, it says here:
These contributing structures do not actually exist. The $\ce{CO3^2-}$ does not consist of a mixture of these structures, ...
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0answers
36 views
Hydrogen Bonding by Carbenes
A hydrogen bond is formed between hydrogen attached to highly electronegative atoms (nitrogen, oxygen, and fluorine) which are small in size too and the non-bonding pair of electrons of another such ...
2
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0answers
15 views
C-C bond lengths in hydrocarbons
We had a question in a rest comparing the bond lengths of hydrocarbons fluorides, and the answer key says CF3- CF3's supposed to have a longer C-C bond than H3C- CH2--F.
Why is this so? Wouldn't the ...
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1answer
64 views
Why does bubbling carbon dioxide through calcium hydroxide result in a precipitate?
Why does the addition of carbon dioxide to calcium hydroxide create the precipitate calcium carbonate? What happens chemically for such a molecule to form? How exactly do their interactions come into ...
2
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0answers
34 views
Bond Dissociation Energy in Water [duplicate]
Why do the bond dissociation energies of the O−H bonds in water differ? Is it related to an increase in lone pair-bond pair repulsions upon the breaking of the first O−H bond (decrease in stability, ...
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0answers
33 views
Lewis structure and bond order of polyiodides
I am trying to draw the lewis structure of triiodide, pentaiodide and heptaiodide-anions. But I am not sure about them, especially not about the heptaiodide-anion (see image).
The second question is,...
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2answers
27 views
Basic bond strength concept
I saw C-H bond is stronger than C-C bond... Is this because of the following reasons?
1) C-H bond is shorter than C-C bond.
2) C-H bond is more ionic than C-C bond.
I
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29 views
Is bonds in CO is all 3 coordinate bonds or 2 covalent and 1 coordinate bonds?
Below image is as available in India's Class 11 NCERT Chemistry book vol 1 Page 104. I am confused as it states all 3 bonds are kind of coordinate bonds. Should it not start with 2 covalent bonds and ...
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0answers
44 views
Bonding in Sulphur dioxide [duplicate]
In Concise Inorganic Chemistry by J.D.Lee (Adapted by Sudarsan Guha, Fourth Edition), on page 82, under section 3.8 - Types of Covalent Bonds (Sigma and Pi Bonds) it is given (for Sulphur dioxide ...
1
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1answer
47 views
Why is trichloromethane more acidic than trifluoromethane? [duplicate]
In Concise Inorganic Chemistry by JD Lee (4th edition; adapted by Sudarshan Guha), page 78 under the topic "Back Bonding" it is given:
$\ce{CHCl3}$ is more acidic than $\ce{CHF3}$ which is ...
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0answers
58 views
Why is back bonding not possible in sulfur dichloride?
In Concise Inorganic Chemistry by JD Lee (4th edition; adapted by Sudarshan Guha), page 76 under the topic "Back Bonding" it is given:
For $\ce{SCl2}$ the bond angle is 102° since the lone pair of $...
2
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0answers
58 views
Why are B-O-H and B-O-C angles in B(OH)3 and B(OCH3)3, respectively are higher than normal?
In Concise Inorganic Chemistry by JD Lee (4th edition; adapted by Sudarshan Guha), page 77 under the topic "Back Bonding" it is given:
The $\mathrm{2p}\pi$-$\mathrm{2p}\pi$ back bonding in $\ce{B(...
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1answer
243 views
Dipole moment in NF3 versus NH3
The usual explanation for the molecular dipole moment of NF$_3$ being smaller than that of NH$_3$, despite the N-F dipole being stronger than the N-H dipole, is that influence of the lone electron ...
6
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0answers
110 views
Why is the dipole moment of XeF$_6$ zero? [duplicate]
In Concise Inorganic Chemistry by JD Lee (4th edition; adapted by Sudarshan Guha), page 73 under the section 3.6 (VSEPR Theory chapter Chemical Bonding):
...according to this theory, the position ...
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0answers
18 views
what is the bonding energy of I2 and I3-?
I need some information of bonding energy.
I found that the bonding energy of $\ce{I2}$ is $\pu{151 kJ/mol}$ (https://www.chegg.com/homework-help/dimethyl-ether-ch3och3-ethanol-ch3ch2oh-constitutional-...
2
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1answer
69 views
Coordinate bonds between molecules
For the following question
Which molecules react to form a dative/coordinate bond?
A. $\ce{CH4}$ and $\ce{NH3}$
B. $\ce{C2H2}$ and $\ce{Cl2}$
C. $\ce{NH3}$ and $\ce{HF}$
D. $\ce{Cl2}$ ...
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1answer
55 views
Does it sometimes take energy to create a chemical bond? [duplicate]
Wikipedia says so:
Bonds can also be broken apart. Since most bonds require energy to form, they also give off energy when they are broken. But before most bonds break, the molecule has to be ...
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0answers
74 views
Why are sulfur trioxide and nitrate not isoelectronic, even though both have the same number of outer electrons?
Though $\ce{SO3}$ has the same number of outer electrons as $\ce{NO3-}$, the two are not isoelectronic.
This statement is from JD Lee, but I could not understand why is he calling these two molecules ...
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0answers
33 views
Why do the d orbitals contract when pairing of electrons start, because the size should increase due to increase in energy
The energy of an orbital is proportional to its mean radial distance, and since the 3d orbital is much larger it is much higher in energy than the 3s and 3p orbitals
All references from JD Lee ...
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0answers
68 views
Why does nitrogen molecule have greater ionization energy than nitrogen atom?
I am studying an article in my book that $\ce{N2}$ molecule has higher ionisation than $\ce{N}$ atom and I have no clue it may be because of strong triply bonded atom then why this is not applicable ...
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0answers
26 views
Plaster of Paris
One of my Chemistry professors said that the hard mass formed after adding water to Plaster of Paris, cannot be converted back into Plaster of Paris. However, he said that the original Gypsum can be ...
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2answers
40 views
Bonding in the nitrate anion [duplicate]
Hi so I was studying chemical bonding where i encountered a problem which is stated below.
When we talk about ${NO_3}^-$ we draw its structure as following
But the thing which I dont understand is ...
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1answer
379 views
Maximum bond energy is in F2, N2 or O2? [closed]
I think that it should be F2 because F is smaller than N and O thus having a small bond length. And small bond length means greater energy (my teacher told me)
But the answer is N2
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1answer
42 views
Facing a problem in enthalpy calculation
If 1 mole of gaseous carbon atoms are converted into diamonds, calculate enthalpy change of process given that bond enthalpy of $\ce{C-C}$ bond is $\pu{400 kJ mol-1}.$
According to me, the answer ...
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1answer
52 views
Calculating bond energy given the enthalpy value of burning reaction
The burning enthalpy (exothermic) of $\ce{NO +O2 ->NO2}$ is $\pu{57 kJ mol^-1}$ and $\ce{O=O}$ bond energy is $\ce{494 kJ mol^{-1}}$, then what is the bond energy of $\ce{N-O}$ ?
So I balanced the ...
2
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1answer
69 views
Antibonding, Nonbonding and Bonding orbitals
Recently I came across nonbonding orbitals. I know something about bonding and antibonding orbitals and their formation, but I have no idea about nonbonding orbitals. Could someone explain their ...
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3answers
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Why does a tetrahedral molecule like methane have a dipole moment of zero?
I was studying chemical bonding when I noticed something odd.
We say compounds like $\ce{CCl4}$ and $\ce{CH4}$ have a tetrahedral geometry (which is a 3D structure) but when we talk about their ...
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0answers
19 views
Nature of the bonding in hexaaquaaluminium complex
$\ce {[Al(H2O)6]^3+}$ is a well-known complex ion formed by the $\ce {Al^3+}$. I have always had the understanding that only the aqua complexes of transition metal ions, such as $\ce {[Fe(H2O)6]^3+}$, ...
2
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0answers
24 views
What's the mechanism behind mineral oil loosening cyanoacrylate bonds?
Per industry literature I found that mineral oil is used to loosen out "super glue" and aid in removal from skin. I am exploring the chemistry of this loosening and I am intrigued. Please help me find ...
0
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1answer
36 views
Calculating bond dissociation enthalpy of F-F bond
$$\ce{N2 + 3 F2 -> 2 NF3} \quad ΔH = \pu{-263 kJ mol-1}$$
The bond dissociation enthalpies of the nitrogen triple bond and nitrogen–flourine bond are $\pu{946 kJ mol-1}$ and $\pu{272 kJ mol-1}....
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28 views
Bond dissociation energy calculation
I am looking for methods to determine the dissociation free energy in a precise way, ideally from a simulations. My hope is to get the most precise values possible that are specific to the structure ...
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1answer
382 views
Which molecule has maximum bond angle amongst BF₃, BCl₃ and BBr₃? [closed]
$\ce{Br}$ is the least electronegative from the given compounds. So, in $\ce{BBr3}$ the electrons will be the closest towards boron and thus due to electron-electron repulsions $\ce{BBr3}$ will have ...
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1answer
58 views
Is fluorine also hybridised in carbon tetrafluoride?
I had read that when an atom forms multiple bonds, it hybridises it's orbitals to minimise the repulsion and decrease the overall energy. But do the terminal atoms also exist in hybridised form?
E.g. ...
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1answer
522 views
What kind of bonds (σ or π) are formed by px, py and pz orbitals? [closed]
Our chemistry teacher said that two $\mathrm{p}_z$ orbital only form sigma bond whereas two $\mathrm{p}_x$ and two $\mathrm{p}_y$ orbitals form only pi bond.
He also stated that only $\mathrm{p}_z$...
1
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1answer
40 views
Reduction of conjugated double bond by sodium borohydride
Some of my teachers were debating about whether a double bond in conjugation with a ketone is reduced or not by $\ce{NaBH4}.$ One of my teachers presented the evidence from Clayden which had an ...
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0answers
26 views
Amphoterism and the Metal and Non-Metal Oxides/Hydroxides. Why does amphoterism occur in these? [closed]
I am having trouble understanding why Beryllium Oxide and Aluminum Oxide are amphoteric. Also, while they are not oxides, Aluminum and Beryllium Chloride as well.
Most of the things I have been ...
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0answers
15 views
Reaction enthalpy using bond energy in resonating molecules
To find out and enthalpy of a reaction using bond energy we use the formula
$$\Delta H = \sum\Delta_\mathrm{bond}H_\mathrm{reactants} - \sum\Delta_\mathrm{bond}H_\mathrm{products}$$
since we use all ...
1
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1answer
52 views
Hydration, Coordinate Bonding, and Reduction Potential in Groups 1 and 2 Elements [closed]
Whenever an alkali metal such as Lithium is hydrated/solvated, coordinate bonding occurs and it is the high hydration enthalpy of lithium which makes it the strongest reducing agent in aqueous ...
0
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1answer
92 views
Bond dissociation energy among halogens [duplicate]
Among the halogens, why is it that the fluorine has the lowest bond dissociation enthalpy, considering the fact that fluorine is the smallest and the internuclear distance between the fluorine ...
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1answer
33 views
How can we find out the type of bonding present in a compound or a molecule?
For example, if the bonding in diamond, ice, MgO or CO2 is to determine, how can I find it out? How to determine van der Waals forces?
