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.

Filter by
Sorted by
Tagged with
-2
votes
0answers
29 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 ...
-4
votes
0answers
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?
-2
votes
0answers
39 views

Why do F and N don't make a bond? [on hold]

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 ?
1
vote
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 ...
-3
votes
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.
1
vote
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. $<\pu{136 pm}$ ...
-3
votes
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 ...
1
vote
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
votes
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, ...
2
votes
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
votes
0answers
14 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 ...
0
votes
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
votes
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, ...
0
votes
0answers
32 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,...
-1
votes
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
1
vote
0answers
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 ...
1
vote
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
vote
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 ...
1
vote
0answers
55 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
votes
0answers
57 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(...
4
votes
1answer
231 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
votes
0answers
108 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 ...
1
vote
0answers
17 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
votes
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. $\ce{Cl2}$ ...
0
votes
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 ...
1
vote
0answers
73 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 ...
1
vote
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 ...
0
votes
0answers
67 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 ...
0
votes
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 ...
1
vote
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 ...
-1
votes
1answer
363 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
3
votes
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 ...
0
votes
1answer
51 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
votes
1answer
67 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 ...
14
votes
3answers
2k views

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 ...
1
vote
0answers
18 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
votes
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
votes
1answer
35 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}....
1
vote
0answers
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 ...
1
vote
1answer
380 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 ...
-1
votes
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. ...
0
votes
1answer
510 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
vote
1answer
39 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 ...
1
vote
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 ...
1
vote
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
vote
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
votes
1answer
91 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 ...
-1
votes
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?
3
votes
0answers
48 views

Bond lengths in P₄O₁₀

According to JD Lee's Concise Inorganic Chemistry: The double bond $\ce{P=O}$ in $\ce{P4O10}$ contains p(π)–d(π) backbonding, where a full p-orbital on oxygen overlaps with an empty d-orbital on $\...
9
votes
1answer
171 views

How to you show a 3-center 2-electron bond in a Lewis structure?

How would you write $\ce{PCl5}$ or other hyper-conjugate molecules as a Lewis structure that indicates 3-center 2-electron bonds? I have seen depictions [1] for transition metal complexes but not for ...