Yes
Hybridisation is a mathematical technique in valence bond theory used "create" new (higher energy) orbitals from base atomic orbitals so that the new orbitals point along bond axes. Valence bond theory as its name suggests focuses on the localised electron pair. Other bonding theories such as molecular orbital theory do not hybridise the base atomic orbitals. Both theories have their merits.
Energy levels are formed into sublevels which contain specific numbers of orbitals, each of which can contain two electrons with opposite spins. The s sublevel has 1 orbital, the p sublevel has 3 orbitals, the d sublevel has 5 orbitals, and the f sublevel has 7 orbitals.
Oxygen, because it only has four orbitals in its valence shell to accomodate extra electrons.
The energy is higher.
The energy is higher.
Hybridisation is a mathematical technique in valence bond theory used "create" new (higher energy) orbitals from base atomic orbitals so that the new orbitals point along bond axes. Valence bond theory as its name suggests focuses on the localised electron pair. Other bonding theories such as molecular orbital theory do not hybridise the base atomic orbitals. Both theories have their merits.
Hybridisation is a mathematical technique in valence bond theory used "create" new (higher energy) orbitals from base atomic orbitals so that the new orbitals point along bond axes. Valence bond theory as its name suggests focuses on the localised electron pair. Other bonding theories such as molecular orbital theory do not hybridise the base atomic orbitals. Both theories have their merits.
Energy levels are formed into sublevels which contain specific numbers of orbitals, each of which can contain two electrons with opposite spins. The s sublevel has 1 orbital, the p sublevel has 3 orbitals, the d sublevel has 5 orbitals, and the f sublevel has 7 orbitals.
Oxygen, because it only has four orbitals in its valence shell to accomodate extra electrons.
The energy is higher.
Different number of neutrons result in different isotopes:Hydrogen - 1 proton, no neutronsDeuterium - 1 proton, 1 neutronTritium - 1 proton, 2 neutrons (radioactive)Different oxidation states by exchanging electrons between higher energy "hidden" orbitals and valence orbitals:Ferrous - Iron with 2 electrons in valence orbitalsFerric - Iron with 3 electrons in valence orbitals
The energy is higher.
The energy is higher.
The energy is higher.
The energy is higher.
The electrons become excited and move to higher energy orbitals.
this is not a general rule. pi orbitals are always higher in energy than sigma orbitals due to side wise overlapping which is less effective than head on overlappig. however in atoms with atomic number less than 7 the sigma orbital due to overlapping of p orbitals is higher in energy than the pi orbitals formed due to sidewise overlapping of p orbitals