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Is a bonding orbital a molecular orbital whose energy is higher than that of the atomic orbitals from which it is formed?
no, it's a molecular orbit that can be occupied by two electrons of a covalent bond(:
Why will the He2 molecule will not form according to MOT?
The hypothetical He2 molecule would from from a formation of molecular orbitals from Helium's 1s orbitals. Whenever a molecular orbital is formed, there are two options, the constructive interference (bonding) MO, which has a lower energy than the atomic orbitals, and the destructive interference (antibonding) MO, which has a higher energy than the atomic orbitals. Since each He contributes two electrons to the molecule, there are enough electrons to fill both the bonding and antibonding MOs, giving an overall bond order of zero. This means the molecule does not hold together. Compare this to H2 where each atom only contributes one electron, filling only the bonding MO, giving a bond order of 1.
What is molecular orbitals extending over more that two atoms called?
Delocalised
Which molecular shape has two lone pairs and two bonding pairs of electrons around the central atom?
linear
Bonding orbitals in diatomic oxygen?
I wanted explain it using an MO diagram but it's a little difficult to write in this format. I'll just go through with how to construct it and the results. Firstly, note that the atomic orbitals of the Oxygen elements are of the same energy levels so we can draw them parallel with respect to the diagram: OrbitalsO O We can then draw in the electron configuration with respect to each individual atom. It follows that: Orbitals2p _|_|_2s _1s _Orbitals2p +-|+-|_2s +-1s +- *where +/- indicates sign of coefficient of electron spin number* Now that the two atoms are interacting, the probability regions defined by Schrodinger's wave equation are altered and new "molecular" solutions/orbitals are defined. Because of the nature and behavior of waves, and by application of the photoelectric effect, different interactions lead to different consequences. If a wave is in phase with another wave they result in an increased amplitude: this gives electrons the most ideal energy position and may result in a decrease of energy over atomic configurations.However, it also means that there will be times of destructive interference as opposed waves collide. This collision leads to nodes of complete interference and oppose the bonding of the elements. Such regions are known as anti-bonding orbitals. Now we can draw in our molecular orbitals and fill them according to the aufbau principle, where electrons will fill according to the lowest possible energy state. Also note that the 2pσ bond in Oxygen is the lowest in energy as it is larger than nitrogen.Anti-Bonding Orbitals denoted by * 2P :-2pσ* 2pπ* 2pπ 2pσ2S :- 2sσ* 2sσ1S : -1sσ* 1sσFrom 1sσ, the energy increases in each molecular orbital. Using both Oxygen atom's electrons we fill the orbitals. The diagram will have these results:2P :-2pσ* 2pπ* + +2pπ +- +-2pσ + -2S :- 2sσ* +-2sσ +-1S : -1sσ* +-1sσ + -The idea is that the electrons left 2 half filled degenerate orbitals. This makes Oxygen a diradical. If we now calculate the bond order to see which state the elements favor. Bond order is the half the difference of bonding electrons to anti-bonding electrons. Here we have (10 bonding - 6 anti-bonding)/2. 4/2 = 2. Therefore:By molecular orbital Theory, the gas O2 is energetically favored to the elemental Oxygen and is of Bond order 2. It will have a double bond.
Indicate how bonding is explained in term of molecular orbitals?
When two atoms combine, the overlap of their atomic orbitals produces molecular orbitals. An atomic orbital belongs to a particular atom, whereas a molecular orbital belongs to a molecule as a whole. Much like an atomic orbital, two electrons are required to fill a molecular orbital. A bonding orbital is a molecular orbital occupied by the two electrons of a covalent bond
Why dihelium does not exist?
Molecular orbitals: dihelium has two electrons in the bonding orbital and two in the antibonding orbital. That why it does not exists.
Is a bonding orbital a molecular orbital whose energy is higher than that of the atomic orbitals from which it is formed?
no, it's a molecular orbit that can be occupied by two electrons of a covalent bond(:
How many anti bonding orbitals are there in an O2 molecule?
there are two
What do two hydrogen atoms bonded together form?
A hydrogen bond is the attractive interaction of a hydrogen atom with an electronegative.When two hydrogen atoms come together to form the hydrogen molecule, the atomic s orbitals of each atom are combined to form two molecular orbitals. One of these new orbitals is the result of the addition of the two atomic orbitals, while the other is created by a subtraction of these orbitals. In the addition, a reinforcement of the wave function occurs in the region between the two nuclei. Physically, this means the electron density increases in the area between the two nuclei. This increase in electron density causes a corresponding increase in the attraction of each positively charged nucleus for the negatively charged overlap region. It is this increased attraction that holds the hydrogen molecule together and creates the bonding molecular orbital. Because the bonding molecular orbital is generated from atomic s orbitals, it is called a σ (sigma) bonding molecular orbital.
Why can't you have two carbon atoms joined by 4 covalent bonds?
A carbon-carbon quadruple bond does not exist because that much electron density between the two nuclei would cause too much electrostatic repulsion. This prevents the electrons from grouping so tightly in such a small space. To find the actual bond order of a carbon-carbon bond, one would have to draw out a molecular orbital diagram. One would find that the molecular orbitals caused by the 1s and 2s atomic orbitals would have both bonding and antibonding orbitals filled, making them irrelevant to finding the bond order. The 2p orbitals give rise to two degenerate bonding pi orbitals, both of which are filled. Since there are no antibonding orbitals filled above the pi orbitals, the bond order is two.
Why will the He2 molecule will not form according to MOT?
The hypothetical He2 molecule would from from a formation of molecular orbitals from Helium's 1s orbitals. Whenever a molecular orbital is formed, there are two options, the constructive interference (bonding) MO, which has a lower energy than the atomic orbitals, and the destructive interference (antibonding) MO, which has a higher energy than the atomic orbitals. Since each He contributes two electrons to the molecule, there are enough electrons to fill both the bonding and antibonding MOs, giving an overall bond order of zero. This means the molecule does not hold together. Compare this to H2 where each atom only contributes one electron, filling only the bonding MO, giving a bond order of 1.
Why nitrogen is diamagnetic while contains unpaired electrons?
If you are going by the electron configuration of nitrogen then the unpaired electrons in the 2p shell would indicate that it is paramagnetic. However experiments show that it is diamagnetic. You must remember that nitrogen is a diatomic element and as such is found as N2. The molecular orbital theory explains how there are no unpaired electrons in the bonds between the two N atoms. The 1s and 2s molecular orbitals are completely filled and all of the bonding 2p orbitals are also filled. There are no electrons in the any of the 2p anti-bonding orbitals. Seeing a molecular orbital diagram for N2 will clarify what i mean.
What is molecular orbitals extending over more that two atoms called?
Delocalised
How is a molecular orbital formed?
In molecular orbital theory, MO theory, molecular orbitals are "built" from atomic orbitals. A common approach is to take a linear combination of atomic orbitals (LCAO), specifically symmetry adapted linear combinations (SALC) using group theory. The formation of a bond is essentially down to the overlap of the orbitals, the orbitals being of similar energy and the atomic orbital wave functions having the correct symmetry.
What is the two kinds of chemical bonding?
ionic and covalent:)
Molecular orbital that can be occupied by two electrons of a covalent bond?
The answer is bonding orbital.
