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.
0
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2answers
62 views
Why are triple covalent carbon to carbon bonds drawn linearly in skeletal structure? [duplicate]
In the link see that cyclic C-C structure with a triple covalent bond is drawn with an angle, probably the only way to draw it but why is it drawn linearly in non-cyclic and not like single or double ...
0
votes
0answers
32 views
When we tear a piece of paper do some of the molecules fall of as we tear? [duplicate]
So I mean are some of the molecules lost(fall of) while we tear the paper? Or all the molecules present in the sheet of paper just get divided in the two new pieces created?
0
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0answers
26 views
Trend of thermal stability of Group 2 chlorides down the group [duplicate]
Thermal stability of group 2 chlorides follows the order: $\ce{BeCl2>MgCl2>CaCl2}$.
Talking about carbonates of group 2 metals, the thermal stability increases as we move down the group due to ...
2
votes
1answer
75 views
Is a hydrogen molecule smaller than hydrogen atom?
Recently I came across a textbook of physical chemistry which stated the following:
In the formation of a stable hydrogen molecule, two hydrogen atoms share a pair of electrons between them and two ...
1
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0answers
36 views
Justify this statement whether correct or incorrect . He2^+ has the same energy as two isolated He atoms [closed]
My explanation : how can a stable molecule be at the same energy level as two isolated inert gas atoms?? Is this even possible?
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1answer
46 views
Comparing strength of the C-H, N-H, and O-H bonds
$$
\begin{align}
\ce{CH4(g) + Cl(g) &-> CH3(g) + HCl(g)} &\quad ΔH^\circ &= \pu{-14 kJ mol-1}_\mathrm{rxn}\\
\ce{NH4(g) + Cl(g) &-> NH2(g) + HCl(g)} &\quad ΔH^\circ &= \...
1
vote
1answer
26 views
What are the other ways (if they exist) that atoms can gain or lose electrons that aren't bonding?
I know that electrons can be isolated through human intervention from their atoms. My question rather concerns if electrons are ever lost or gained naturally. I recognize that this is a stupid ...
1
vote
1answer
38 views
Relation between ionic resonance energy and polarity
The ionic resonance of the bonds are given as follows:
$$
\begin{array}{cr}
\ce{A-B} & 24.3 \\
\ce{A-C} & 50.6 \\
\ce{A-D} & 102.3 \\
\ce{A-E} & 105.9
\end{array}
$$
Which of ...
-1
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0answers
65 views
Why can Boric Acid form H-bonds?
Boric acid has a layered structure in which individual $\ce{H_3BO_3}$ units are connected by hydrogen bonds, but $\ce{H_3BO_3}$ has zero net dipole moment so H-bonding should be absent if it is just a ...
11
votes
3answers
972 views
Elements other than carbon that can form many different compounds by bonding to themselves?
My textbook says the following:
Unique among the elements, carbon can bond to itself to form extremely strong two-dimensional sheets, as it does in graphite, as well as buckyballs and nanotubes.
...
-6
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0answers
22 views
Why isn't lithium a diatomic element? [duplicate]
Lithium seems to be a perfect fit to be a diatomic element. Could two Li atoms form a bond to become a diatomic element?
0
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1answer
89 views
Does dilithium exist? [duplicate]
Lithium has two electrons in $\mathrm{1s}$, filling the first energy level; and one valence electron in $\mathrm{2s}$. Could two $\ce{Li}$ atoms form a bond to create $\ce{Li2}$; like $\ce{O2}$ or $\...
5
votes
1answer
59 views
Can a double bond extend beyond the plane and if so, how would it be drawn?
Can double and triple bonds, etc., extend beyond the plane in a Lewis structure, and if so, how are they represented? I.e., how would 1 and 2 in this image be drawn if they were doubles or triples?
1
vote
1answer
48 views
What happens when an ionic compound is boiled? [duplicate]
Do ionic compounds such as NaCl become individual ions such as one Na ion and one Cl ion or are they hold together by ionic bonds even when they are boiled. Thanks in advance.
0
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1answer
46 views
Why is there a lone pair in thionyl fluoride?
Why is there a lone pair in $\ce{SOF2}$? I drew its structure, which according to me should look like this:
Why is there a lone pair on sulfur? Isn't its octet complete? If yes, why should it expand ...
1
vote
2answers
33 views
Predict the number and nature of bonds using Molecular Orbital Theory
I found the following question in a high school chemistry problem book:
According to Molecular Orbital Theory which of the following is true:
(A) In $C_2$ molecule both the bonds are $\pi$ ...
1
vote
1answer
55 views
Sigma bonds, pi bonds and the puzzling symmetry of methane [duplicate]
My A-Level Chemistry textbook assures me that:
a sigma bond is formed when two s orbitals overlap.
a pi bond is formed when two p orbitals overlap.
all single bonds between carbon and any other atom ...
0
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1answer
24 views
Definition of Lattice Energy
From previous studies, I recalled in my lecture theatre today that lattice energy was the energy released when an ionic compounds is formed from individual atoms in the gaseous state. I thought this ...
0
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0answers
44 views
Which has greater N-O bond length: NO or NOCl?
I came across this question. According to me NO should have a shorter bond length as it has a triple bond, while NOCl has a double bond.
But the answer is given that NO has greater bond length than ...
2
votes
1answer
51 views
Why is $1s-1s$ orbital overlapping stronger than $2p_x-2p_x$ orbital overlapping?
Assume the x-axis to be the internuclear axis. Hence, both $1s-1s$ and $2p_x-2p_x$ will form $\sigma$ bonds.
Also consider the fact that $p$ orbitals have more directional characteristics.
Given the ...
1
vote
1answer
34 views
What is the correlation between electronegativity and the sharing of electrons?
For example in a C-O bond, the electronegativity difference is 1.2. does this mean that the Oxygen has 1.2 of the shared electrons and Carbon 0.8 (or some other numbers)? Is there a specific equation ...
-1
votes
1answer
100 views
How is energy released when a chemical bond is formed? [closed]
Chemical reactions are classed as endothermic or exothermic.
Defn: exothermic
(of a reaction or process) accompanied by the release of heat.
The heat is released when the chemical bonds in the ...
2
votes
0answers
42 views
Why is it not possible for seven close copper atoms to come together to gain a noble-gas configuration of valence electrons?
My textbook says the following about metallic bonding:
The metal copper has one valence electron. The valence electrons of nearby copper atoms are shared in a similar way to covalently bonded ...
3
votes
0answers
55 views
Can the Lewis dot structure of SO2 be experimentally verified?
I have just watched 2 different videos on the Lewis dot structure of sulfur dioxide, $\ce{SO2}$. One says it is
$$\ce{O=S=O}$$
and the other says
$$\ce{^-O-S^+=O <-> O=S^+-O-}$$
The first ...
1
vote
1answer
50 views
Textbook Claim: “… in all cases it is the electrostatic force acting between charged particles that is responsible for all the forms of bonding.” [duplicate]
I am reading an introductory semiconductor physics textbook. The textbook states the following:
Several types of atomic bonding have been identified, including ionic, covalent, van der Waals, ...
2
votes
1answer
52 views
electron donation affecting carbonyl bond strength
I have been told that electron donation decreases carbonyl bond strength and thus decreases the bond stretch frequency, but electron withdrawal increases it.
This does not seem to make any sense as ...
0
votes
1answer
23 views
Why are higher oxides of non-metals more acidic?
I have studied that if the electronegativity difference between O- and element M is more then it is a basic oxide and if the difference is less then it is an acidic oxide. However, it is a fact that ...
8
votes
1answer
299 views
Does the Location of Line-Dash-Wedge Notations Matter?
In Line-Dash-Wedge notation, when illustrating that an atom or bond is directed towards or away from the viewer (solid triangle for coming forward, dotted lines for going back), does the location of ...
1
vote
2answers
48 views
molecular orbital theory [closed]
i read in my textbook that the energy diagram of moleculal orbits is different for atoms nitrogen and below them.
my question is which one of the energy diagrams to use in heteronuclear compounds like ...
0
votes
1answer
49 views
Why aren't all bond lengths equal in cyclobutadiene? [closed]
even when there is a possibility of conjugation why aren't bond lengths equal?
1
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0answers
25 views
Is the 12-6 Lennard Jones potential a good description of van der Waals interaction energy?
It seems to me that the Lennard Jones potential oversimplifies the more complex nature of van der Waals forces. However, in most of the MD simulation package, this is generally accepted.
1
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0answers
22 views
Metallic Versus Covalent Bonding
Given that a metal's low ionisation energy is often used to explain the metallic bond (as are other factors such as temperature and pressure and possibly a number of other factors), is there any known ...
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votes
1answer
35 views
Electric conductivity
Well I was wondering why some materials have a higher resistivity than others . So I took two elements randomly . I picked carbon and silicon . Carbon has lower resistivity than silicon and obviously ...
1
vote
2answers
84 views
During formation and breaking of bonds, can the terms potential energy and bond energy be used interchangeably?
My chemistry professor uses these terms interchangeably and I was wondering if they refer to the same thing. From what I understand, bond energy is the energy required to break one mole of covalently ...
1
vote
1answer
32 views
When a bond is formed between an electophile and a nucleophile, they both lose energy and become more stable right?
This is a section from clayden's organic chemistry textbook. I do not understand why it says energy gain and not energy loss
0
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1answer
29 views
Is there any difference between thermal energy at room temperature in fluids(water) vs air?
Context of the question: I was reading on hydrogen bonds, specifically how close they are to the thermal energy of the fluids. So I googled the value of thermal energy at room temperature, which was $\...
2
votes
1answer
64 views
Reaction energy of oxygen and hydrogen
From the bonding energy of following bonds that I found in a Wikipedia article, I calculated the reaction energy that would be released when oxygen and hydrogen are reacted to produce water. The phase ...
18
votes
4answers
945 views
Does a neutral dimercury molecule exist?
Is a neutral $\ce{Hg2}$ molecule possible, as a gas under extremely low (partial) pressures? What is the enthalpy of formation or similar?
It is my impression that usual mercury vapors are monatomic? ...
-1
votes
2answers
166 views
Why does bond breaking in ATP release energy? [duplicate]
We always come across that formation of bonds releases energy, and bond breaking requires energy, but in the case where ATP converts into ADP or AMP (bond breaking), energy is released. Why?
Further, ...
0
votes
0answers
27 views
My problem with Tollen's reagent [duplicate]
The formula of Tollen's reagent is $\ce{[Ag(NH3)2]+}$. What is the bond existing between the silver(I) atom and the ammonia groups? Because ammonia is stable, it doesn't need to gain or donate any ...
1
vote
0answers
30 views
Drawing bonds and delocalised electrons in condensed formulae
The $\LaTeX$ mhchem package provides commands for drawing bonds within condensed chemical formulae. Some of them have a clear allocation to covalent bonds while others have not. Single, double, and ...
0
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0answers
35 views
How do three-electron bonds work in MO theory?
When we're taught MO theory in basic chemistry, a rule-of-thumb hammered into our heads is that an orbital takes up to 2 electrons with opposite spins. Sigma or pi bonds are represented by stable ...
0
votes
2answers
100 views
What would be the intermolecular forces between the molecules of methanetetrol?
Methanetetrol has the following chemical formula: $\ce{CO4H4}$. It is also referred to as orthocarbonic acid.
Since the molecule has a molecular geometry of a tetrahedron, similar to that of a ...
2
votes
1answer
158 views
Why is carbon monoxide a monodentate ligand
Carbon monoxide has lone pairs on both the carbon and the oxygen atoms. However, I have never seen any complex where the oxygen atom or both the oxygen and the carbon atoms are the donors.
I know ...
10
votes
1answer
379 views
Explanation of the strength of phosphorus-oxygen bond
When discussing the Wittig reaction, Clayden's Organic Chemistry cites the strength of the $\ce{P=O}$ formed in triphenylphosphine oxide as a driver of the reaction through enthalpy:
The $\ce{P=O}$ ...
2
votes
0answers
56 views
Why doesn't lithium form dilithium crystals? (Calling Mr.Spock) [duplicate]
Hydrogen is in the first column of the periodic table. At STP it is a diatomic gas. When cooled and/or under pressure it forms a crystalline solid of di-hydrogen molecules. Calculations indicate that ...
-4
votes
2answers
135 views
What is the bond in H2O (water) molecule ? And why? [duplicate]
Is it covalent or coordinate covalent bond ? Because it can be a bond between O and 2 H atoms and so it will be covalent bond . And it can be a bond between H (+ve) ion and Oh(-ve)ion and it will be ...
-2
votes
1answer
55 views
How hydrogen molecule is formed? [closed]
How two hydrogen atoms come close to form a bond ? Textbooks refer to a potential energy diagram but what i cant understand is what is this potential energy if the atoms are neutral . How they come ...
9
votes
1answer
292 views
Explanation for bond lengths in trans-hexatriene
Hexatriene is an unsaturated hydrocarbon with six carbon atoms and five carbon-carbon bonds, three of which are double bonds.
However, the bond lengths of the $\ce{C=C}$ bonds are not the same. The ...
1
vote
1answer
88 views
Why does covalent nature in ionic solids increase the lattice energy?
I have observed in my textbooks that ionic solid that have a greater covalent character tend to have higher lattice energy. Can this be generalised as fact?
