What is the bond dissociation energy order of F2, Cl2, Br2, and I2?
Cl2 > Br2 > F2 > I2
Why does N have a higher bond dissociation energy than N2+?
According to Molecular orbital theory:N2 have 6 more electrons in a bonding atomic orbital so it’s bond order is 3, whereas N2+ has only 5 in bonding so it's bond order is 2.5.Bond dissociation energy is directly proportional to Bond order of a molecule so N2 has more bond dissociation energy.AMMusani.
Bond Dissociation Energy Chemistry Help!?
Source: General Chemestry ninth edition pg 360 table 9.5 N tripple bond energy is 942 kj/mol N-O is 201 kj/mol When your forming bonds take the negative breaking take the positive because breaking bonds releases heat. Sum of the enthalpy = energies of bonds broken - energy of bonds formed Ok so whats formed? It's an O2 bond! Almost there O-O is 142 kj/mol O=O is 494 kj/mol Im confused about which number to use for that, Answer should be something like 2(201)-142 Or 2(201)-494 Two times 201 bc there is two mol on the left side for every one mol of O2 on right ...
Why is the dissociation energy of a Florine (F2) molecule lower compared to other halo (chlorine, bromine and iodine) molecules?
Bond Length:Bond Dissociation Energy:F-F: 156.9 kJ/molCl-Cl: 242.58 kJ/molBr-Br: 193.87 kJ/molI-I: 152.55 kJ/molBond dissociation energy of F2 is lower than Cl2 and Br2 (though not I2, due to the low electronegativity of iodine).Why?Fluorine is a highly electronegative element.From the picture we can see that the fluorine molecule is a pretty small one as compared to its group members. Atomic number is 9, 1s(2)2s(2)2p(5), seven electrons on its outermost shell and a very small atomic radius.Two fluorine atoms must come together to share a pair, so that the octet is completed.But these many electrons concentrated on two small nuclei and separated over comparatively a very small distance repel each other.Hence the F-F bond is weakened.[Note: This is similar to the low BDE of peroxide bond (-O-O-), where the lone pairs of oxygen atoms repel each other, eg. H2O2. Its BDE is 142 kJ/mol]
Between N2 and N2+, which has less bond energy and why?
N2+ has less bond energy. This is because, according to molecular orbital theory, it has fewer electrons in bonding orbitals.The diagram above is the molecular orbital diagram for N2. The highest electron on the diagram is the highest energy electron, and thus the electron that would be removed to make N2+. As you can see the orbital where this electron resides is lower than the non-bonding orbitals on the side. This means that having an electron in this orbital increases stability. Taking this electron away reduces stability.
What is the relationship between the dissociation energy of N2 and N2+?
Based on the Molecular Orbital Theory, N2 has a bond order of 3 whereas N2+ has a bond order of 2.5. In this case, greater the bond order, more will be the bond strength and hence greater would be it’s bond energy.
What is the bond dissociation energy between two H2 gas molecules?
This is kind of a cool bit of chemical trivia:The hydrogen gas bond dissociation energy is large: 436 kJ/mol. In fact, it pretty much sets the record for diatomic molecules joined by a single bond.Other diatomic molecules with single bonds would include:F--F: 156.9 kJ/molCl--Cl: 242 kJ/molBr--Br: 192 kJ/molI--I: 151 kJ/molMultiple-bond diatomic molecules:O==O: 497 kJ/molN:::N: 945 kJ/molSo, as you can see, the hydrogen-hydrogen bond energy is very high, comparable to the bond dissociation energy of oxygen.Cheers!
Use bond energy values to estimate delta H?
The bond energy is the energy required to break up a bound. The energy to from a bond is the negative bond energy. Hence the heat of reaction is approximately the sum of the bond energies of the reactants minus the sum of the bond energies of the products. a) H2 + Cl2 → 2 HCl The bonds are H2 one H-H bond Cl2 one Cl-Cl bond HCl one H-Cl bond Hence: ΔH = D(H-H) + D(Cl-Cl) - 2·D(H-Cl) = 432kJ/mol + 240kJ/mol - 2 · 428kJ/mol = -184kJ/mol b) N2 + 3 H2 → 2 NH3 The bonds are N2 one N≡N bond (triple bond) H2 one H-H bond NH3 three N-H bonds Hence: ΔH = D(N≡N) + 3·D(H-H) - 2·3·D(N-H) = 942kJ/mol + 3·432kJ/mol - 6·386kJ/mol = -78kJ/mol
Why does H2 have higher bond energy than F2?
I believe that this problem is related to the bond lengths and the number of electrons.Both molecules contain a same covalent bond. However, the bond length and the number of electrons are not the same. If we take a look only to the bond length and neglect the fact that the electrons are different in number, we know that H2 will have shorter bond length than F2. This indicates that the bond energy of H2 is higher than F2. Now if we consider the number of electrons, the valence electrons of F is more than the valence electrons of H. As electrons repel each other, higher number of electrons means higher repulsion, and to conclude, lower bond energy (as the bond is easily broken).
If all combustion reactions are exothermic then why N2+O2 is endothermic?
Note: since you( when this question was asked) are in tenth grade, it might be a bit hard to understand. You will learn the reason I'm eleventh grade. So you can ignore the first paragraph for now.All would be a wrong word here. The amount of energy absorbed or released during a reaction depends on several factors. To name the most important ones: activation energy and enthalpy of reaction.Simply put, we need to find out whether the products are more stable than the reactants or not.Therefore on this case we have the formation of NO, which is much less stable than N2 or O2. The bond dissociation energy of N2 is 946kj/mol(magnitude) which is very high. Therefore N2 is almost inert to reactions at low temperatures.So we need to supply energy to break the triple bond in N2 and similarly the double bonds in O2.Therefore this reaction is endothermic.If you look at combustion of methane, the bond dissociation energy (C-H and O-O bonds) is much lesser than the energy released (due to formation of C=O and O-H bonds). Therefore the reaction is exothermic.I hope you understand the difference