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], [intermolecular-forces], etc.

Filter by
Sorted by
Tagged with
0
votes
0answers
32 views

Can any two atoms form a diatomic molecule (they can be the same or different elements)? [closed]

I was looking at this pdf - http://staff.ustc.edu.cn/~luo971/2010-91-CRC-BDEs-Tables.pdf and it lists different bond disassociation energies of diatomic molecules. However many of the diatomic ...
-2
votes
0answers
9 views

Predict the hybridisation state of each carbon atom in the following compounds [closed]

Predict the hybridisation state of each carbon atom in the following compounds: CH3 CH2 C CH CH2=CH-C-O-O-CH3 CO2
-1
votes
1answer
42 views

How can I make AgNO3 more basic? [closed]

Is there anything that I can add to the AgNO3 solution that will make it more basic without forming a precipitate such as reacting with OH or HCl? Please be more specific and give an example.
2
votes
0answers
19 views

Is the total ionic-dipole bond (hydrogen bonds) acting on an ion stronger than the lattice energy holding the ions together?

When magnesium chloride dissolves in water, its $\Delta H^⦵_\mathrm{sol}$ is negative. Since $\Delta H^⦵_\mathrm{sol} = \Delta H^⦵_\mathrm{hyd} - \Delta H^⦵_\mathrm{latt},$ this means $-\Delta H^⦵_\...
0
votes
1answer
65 views

what will the products be when AgNO3 reacts with [Cu(NH3)4(H2O)2]2+? [closed]

I'm trying to increase the pH of the $\ce{AgNO3}$, the only way was using complexation of ammonia and decided to use $\ce{[Cu(NH3)4(H2O)2]^{2+}}$. The only problem is that I don't know if this complex ...
-2
votes
1answer
26 views

why is energy released when a chemical bonds is formed? [closed]

why is energy released when a chemical bonds is formed?
3
votes
1answer
57 views

Does direction matter in breaking a bond?

Im not sure if this question belongs here or in another community. I was wondering if the direction that we apply a force in order to break a bond matters and how it affects strength. Say we have one ...
-3
votes
0answers
12 views

Order of covalency of compounds [closed]

What is the order of covalency among the four compounds, SnCl2,SnCl4,SnF2 and SnF4,and why?? And please tell the reason behind it
1
vote
0answers
24 views

Hybridization theory (orbitals used in different hybridizations)

Why is $d_{x²-y²}$ orbital used in $sp^3d$ (square pyramidal geometry) while $d_{z^2}$ orbital in $sp^3d$ (trigonal bipyramidal geometry)? I came across this information while reading J.D.Lee Concise ...
-1
votes
0answers
31 views

Are Br2 and Cl2 electrophiles [closed]

Are $\ce{Br2}$ and $\ce{Cl2}$ electrophiles Since they have vacant d-orbitals, they can accomodate more electrons and can behave as electron deficient species. Thus should be electrophiles.
0
votes
1answer
19 views

For an electron arrangement diagram, is it necessary to show the inner electron shells or is it customary to only show the valency electrons?

Which electron arrangement diagram is correct? The one that shows all electron shells or the one that only shown the valence electron shell?
0
votes
0answers
25 views

Reactivity of dinitrogen vs carbon monoxide [closed]

As far as I understand, the 3-fold bonds in $\ce{N2}$ (dinitrogen) and $\ce{CO}$ (carbon monoxide) are the strongest among all bonds. This explains why $\ce{N2}$ is inert and not reactive at all. But ...
1
vote
1answer
55 views

Why are the acidities for H-CH3 and H-OH so different?

I was comparing the acidity of H-CH3 and H-OH, and a lot of things weren't making sense. Generally, the process of turning H-X into $H^{+}$ and $X^{-}$ can be broken into 2 hypothetical steps: 1.) ...
-2
votes
0answers
17 views

How is the hibridization of different compounds with hydrogen affected by the size of atoms it bonds on? [duplicate]

In our study material it is stated that elements of the second period, (in groups 6,7) tend to hibrydize their orrbitals in order to form bonds with for lets say hydrogen. But elements in higher ...
1
vote
0answers
17 views

Why is average bond enthalpy measured by homolytic fission?

Average bond enthalpy: the energy required for 1 mole of a specific gaseous bonds to undergo homolytic fission Why specifically homolytic fission? Is it to allow comparison, but if that were the case,...
3
votes
1answer
85 views

Why is the carbon monoxide triple bond stronger than the nitrogen-nitrogen triple bond?

The $CO$ triple bond has a bond enthalpy of 1072 kJ/mol while the $N_2$ triple bond has a bond enthalpy of 945 kJ/mol, at least according to my source. The molecules are isoelectronic, so I couldn't ...
1
vote
0answers
37 views

If all bond angles in AX₃ are the same, then which of the following are correct conclusions about AX₃?

Question If all bond angles in $\ce{AX3}$ are the same, then which of the following are correct conclusions about $\ce{AX3}?$ (A) $\ce{AX3}$ must be polar. (B) $\ce{AX3}$ must be planar. (...
0
votes
1answer
20 views

Reason behind more Reactivity of Unsaturated Hydrocarbons [closed]

My textbook says that unsaturated hydrocarbons are more reactive than saturated ones. But double and triple bonds are stronger than single bonds. What is the explanation for this?
0
votes
1answer
42 views

Why do certain signals in proton NMR experience extensive splitting despite only having 1 neighbour?

I came across the compound 3-methylpentan-2-ol. Looking at its proton NMR spectra, it seems there is a lot of splitting for the signal at 4 ppm. I'm assuming that the 4 ppm represents the proton in ...
-1
votes
1answer
47 views

Covalent Bonds and Ionic Bonds [duplicate]

Covalent bond is a strong bond compared to Ionic Bonds but Ionic Compounds have higher melting and boiling points then covalent compounds. Why?
0
votes
1answer
46 views

For bond dissociation energies (BDEs) of double and triple bonds, is number shown in tables for that second or third bond? Or all of them?

Simple, 'dumb' question.... Is the kJ/mol number given in tables of bond strengths or bond dissociation energies , when it comes to double and triple bonds, just for the 'last' bond or for both (or ...
-4
votes
1answer
35 views
-1
votes
0answers
25 views

Does phosphate anion have coordinate covalent bond or not? [duplicate]

My guess is it does not. I tried to use formal charge on its Lewis diagram and find out that the three extra electrons are distributed to three oxygen atoms of $\ce{PO4^3-}$ which shows there isn't ...
5
votes
1answer
97 views

For molecular orbitals, how is an energy of zero set or defined?

When labeling the energies of molecular orbitals, often some anti-bonding MOs are shown with a positive energy. For example, MolCalc has the following energies for methane (the anti-bonding MO #8 at +...
2
votes
0answers
45 views

Multiple bonds solely with sp3 hybridised orbitals? [duplicate]

I have fond that similar question has been asked already (why don't carbons use sp3 instead of sp2 orbitals to make double bonds?), but I don't think it was formulated in a manner that was ...
-2
votes
1answer
50 views

Why do ionic compounds form in the exact ratios that they do instead of more variable ratios? [closed]

I read that e.g. $\ce{Mg^{2+}}$ and $\ce{Cl-}$ come together because of electrostatic force or coulomb force and form an ionic bond. Then why is the formula $\ce{MgCl2}$? Why does one $\ce{Mg^{2+}}$ ...
0
votes
1answer
117 views

Why do boiling points of alkanes and alcohols become closer with increased chain length

I came across this graph, which clearly shows a large difference between the boiling points of alkanes and their equivalent alcohols. However, it is clear that as chain length increases, the ...
0
votes
0answers
76 views

Why is H2Te the strongest acid among the following?

Among H2S, H2Se, H2Te the strongest acid is H2Te. The reason being that the bond strength in it the weakest so it dissociates easily. But my question is that why does it looses H+ in first place ...
3
votes
0answers
34 views

Discussion about Warren-Cowely Parameter

The Warren-Cowely Parameter (WCP) for short range solution order is defined as: $$\mathrm{WCP}_{ij} = 1 - \frac{Z_{ij}}{x_j \cdot Z_i}$$ where $Z_{ij}$ is the partial Coordination Number (CN) of ...
2
votes
1answer
58 views

Only valence shell electrons participate in bonding then how is Cr in H2CrO4 forming 6 covalent bonds although it has only 1 valence electron?

The structure of $\ce{H2CrO4}$ is as follows: Shell configuration of chromium is 2,8,13,1 i.e. it has only 1 valence electron and only valence electron participate in bonding but Chromium in the ...
6
votes
3answers
844 views

Do metals form covalent bonds besides ionic and cordinate bond? [closed]

My chemistry textbook says that metals form ionic or cordinate bonds whereas non metals form covalent bonds. But in another textbook I read that Lithium, Beryllium, Aluminium, Chromium, Manganese etc, ...
0
votes
1answer
74 views

Why aren't all bonds in cyclobutadiene not equal? [duplicate]

Cyclobutadiene is like benzene in that it has alternating single and double bonds in a ring. However, it's bonds are not the same length, the double bonds being shorter than single bonds. The molecule ...
1
vote
0answers
36 views

Why sigma bond has C2 symmetry not C∞?

I have seen some books indicated sigma bond has C2 symmetry. I understand pi and delta bond change their signs about C2 and C4 rotation about bond axis, but I don't understand why sigma bond has C2 ...
7
votes
1answer
100 views

Heats of formation of neutral molecules and homolytic vs heterolytic bond dissociation in mass spectrometry

I am currently studying the textbook Mass Spectrometry, third edition, by Jürgen H. Gross. Chapter 2.4.3 Bond Dissociation Energies and Heats of Formation says the following: Great efforts have ...
0
votes
0answers
29 views

Bonding in molten silicon dioxide

Solid silicon dioxide has a giant lattice structure with single covalent bonds, while in the gas phase it has a molecular carbon dioxide-like structure. But what about in the liquid phase? Would it ...
0
votes
0answers
28 views

Why are stable ionic charges so strongly related to the group number?

Why do lighter elements have ionic charges so strongly related to the group number? For example, why does $\ce{Al}$ only show +3 ionic charge? The basic concept of stability in an ionic compound is ...
1
vote
0answers
20 views

Why do diplumbenes (Pb=Pb double bonded compounds) break apart in hydrocarbon solution?

In group 14, the double bond becomes increasingly weaker down the group. Our lecturer told us that many distannenes ($\ce{>Sn=Sn<}$) and almost all diplumbenes ($\ce{>Pb=Pb<}$) dissociate ...
3
votes
1answer
208 views

Geometry of Ni(acac)2

The complex $\ce{Ni(acac)2}$ is paramagnetic as expected , i.e it has two unpaired electrons giving rise to a magnetic moment of $ \sqrt{8}$ BM but doesn't have the tetrahedral geometry consistent ...
2
votes
2answers
109 views

How energy is released when chemical bond is formed?

In books it is commonly written that whenever a chemical bond is formed the energy of the molecules/atoms gets lowered and hence energy is released. This is generally explained by diagrams like this ...
1
vote
0answers
10 views

In vivo, does it take energy to move double bonds from cis to trans long chain unsaturated fatty acids

In vitro, long chain fatty acids may yield more energy when bonds break, but in vivo, I understood that energy is burned before unsaturated fatty acids can be oxidized because the side groups with ...
5
votes
0answers
132 views

How much electron hybridization and bonding occurs in liquid helium?

Helium is the only element which does not freeze at atmospheric pressure, and only forms a liquid at around 4 Kelvin due to weak van der Waals forces. I'm interested in knowing roughly how much ...
1
vote
0answers
70 views

Comparison of I-F, Br-F, and Cl-F bond strengths

From Chemistry of the Elements by Greenwood and Earnshaw [1, p. 833]: Figure 17.9 Mean bond energies of halogen fluorides. This shows the mean bond energy for $\ce{X-F}$, where $\ce{X}$ is a ...
4
votes
2answers
77 views

What repulsion keeps non-hydrogen atoms at a distance: between inner shells or between nuclei?

Bonded or not, when two atoms or ions come closer than the bond distance or the van der Waals distance, the energy increases drastically. What is the underlying cause of that repulsion? The repulsion ...
1
vote
3answers
93 views

Strength of Hydrogen Bond and Angle

This link has a short paragraph on the very first page, which says: "There are two useful criteria to evaluate the presence and the strength of a H-bond. The first is to look at the distance between ...
2
votes
1answer
53 views

How to check whether intramolecular hydrogen bonding takes place in cyclic compounds?

How can we confirm or have a clear idea whether hydrogen bonding is taking place in substituents of cyclic compounds? For example, it takes place in ortho-nitrophenol, but it doesn't take place in ...
3
votes
1answer
71 views

How to calculate the energy to dissociate a bond into neutral atoms?

I am self studying chemistry through MiT ocw 5.111 . On practice exam 2 problem 2 there is a question which states the following ...
3
votes
0answers
51 views

Counting the number of conjugated pi bonds in a complex aromatic molecule

So for multiple bonds to be conjugated, they must be in an alternating double bond – single bond – double bond, etc arrangement. However, do they need to be continuous? In my textbook, they count the ...
0
votes
0answers
33 views

On steric effects and stereoelectronic effects

From what I understand, stereoelectronic effects are the structure, reactivity, and physical properties of molecules as a result of relative arrangement of orbitals in space. Steric effects result ...
-1
votes
1answer
109 views

Lewis acidity comparison of boron and aluminium trichlorides

Lewis acidity is a function of electron deficiency on the acceptor atom, which in this case is $\ce{B}$ and $\ce{Al}$ respectively. Back donation is better as is the case of $\ce{B}$, due to better ...
0
votes
2answers
68 views

Why doesn't Oxygen form coordinate covalent bonds? [closed]

We know that an Oxygen atom has two lone pairs. Why doesn't oxygen then form coordinate covalent bonds using those since it has nothing to lose?

1
2 3 4 5
23