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How could you predict the presence of a sigma or pi bond in a molecule?
The presence of a sigma will be centered ( with the shared electrons) between the two atoms, such as in water H2O, the sigma will remain between the water and the hydrogen. It will remain in a bonding orbital between the two, the bonding orbital is the region where bonding electrons are likely to be found. As far a pi bond, you know already that there needs to be sigma in order to have a pi, if you have a double bond you can assume that there is one sigma and one pi, if there is a triple bond, you can assume that there will be one sigma and two pi. That's the best way I can explain it, .
Why graphite conduct electricity as other non metals do not?
Graphite has delocalised electrons. It has layer structure (each layer is called graphene). The bonding of the carbons in the layer can be described as sp2 as the bond angles are 120 0. Each C atom has a p orbital perpendicular to the layer that contains a single electron. These p orbitals form pi bonds which spread across the layer.
Where the pi bond in alkene?
The pi bond is one of the two bonds in the double bond. All alkenes contain C=C bond
Back bonding concept in inorganic chemistry?
it is a type of bonding which take place between atoms in a compound ;in which one atom has lone pair of electron and other has vacant orbital placed adjacent to each other. A compound which posses back bonding has pi bonding character because it occurs after formation of sigma bond. Usually ; back bonding causes molecule to get stable as it completes octet. for ex. in borontriflouride , back bonding causes decrease in bond length and increase in bond order.
What does the phrase delocalized electrons mean?
Delocalisation is when electrons are not associated with one atom but are spread over several atoms. So the electrons are not directly bonded with any atoms but effectively 'float' above and below the molecule in electron clouds.
How is the position of electrons involved in metallic bonding different from the position of electrons that form ionic and covalent bonds?
the electrons involved in metallic bonding are delocalised - they are free to move which accounts for electrical conductivity. In ionic bonds the electrons are tightly bound to individual atoms. Generally covalent bonds have localised electrons, in pairs in individual bonds. However there are delocalised electrons in some situations - take graphite extensive pi bonds allow for delocalisation and electrical conductivity.
Is sigma a type of bonding?
Yes, There are two types of bonding sigma and pi.
How many C-O pi bonds are in water?
None. Water does contains only hydrogen and oxygen, so there is no carbon. Further more, all the bonding in water is sigma bonding; there is no pi bonding.
What does delocalized mean?
DelocalisedThe term 'delocalised' refers to an electron which is not 'attached' to a particular atom. For example, in metals, some of the outer electrons are delocalised and are free to move around the whole metal solid. This is why metals conduct electricity. Another example of delocalised electrons is in benzene (C6H6), a cyclic molecule composed of a ring of bonded carbons, with one hydrogen attached to each. In benzene, the electrons in the C-C pi-bonds (basically the double bonds) are delocalised the whole molecule. If you look at the location of these pi-bonding electrons, they are found evenly distributed in a ring around the entire molecule. In this case, the delocalisation can be explained by something called 'resonance forms.' Often, molecules with alternating double bonds show delocalised bonding.However, to truly understand the concept of delocalisation, some basic quantum mechanics must be used, and delocalised bonding in molecules is best explained by molecular orbital theory. In reality, all electrons are somewhat delocalised and are never associated with exactly one bond (in molecules with more than 2 atoms). Some are more localised than others (specific electrons stay mostly with specific bonds), while some are more delocalized (electrons are very free to move about many different bonds in the molecule)
How many sigma and pi bond does ozone molecule has?
Total 2 sigma and 3 pi bonds (one bonding, one non-bonding and one antibonding) for O3
What type of hybridisation in benzene?
sp^2 Due to 3 pi bonds, In reality a single pi 'cloud' of 6 delocalised electrons exists around the ring (refer to resonance structure).
Would you expect SO3 to exhibit delocalized pi bonding?
yes
The creation of new orbitals by the arrangement of valence electrons is known as?
pi bonding
Why ammonia is stronger base than aniline?
The lone pair on the nitrogen of aniline is delocalised into the pi-system of the benzene ring and is therefore less available for attack on a proton.
How could you predict the presence of a sigma or pi bond in a molecule?
The presence of a sigma will be centered ( with the shared electrons) between the two atoms, such as in water H2O, the sigma will remain between the water and the hydrogen. It will remain in a bonding orbital between the two, the bonding orbital is the region where bonding electrons are likely to be found. As far a pi bond, you know already that there needs to be sigma in order to have a pi, if you have a double bond you can assume that there is one sigma and one pi, if there is a triple bond, you can assume that there will be one sigma and two pi. That's the best way I can explain it, .
Why graphite conduct electricity as other non metals do not?
Graphite has delocalised electrons. It has layer structure (each layer is called graphene). The bonding of the carbons in the layer can be described as sp2 as the bond angles are 120 0. Each C atom has a p orbital perpendicular to the layer that contains a single electron. These p orbitals form pi bonds which spread across the layer.
Does pi contain 666?
yes.....6048666, and so on
