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Orbital hybridisation: Quiz
  

Question 1: Hybridisation is not required to describe molecules, but for molecules made up from ________, nitrogen and oxygen (and to a lesser extent, sulfur and phosphorus) the hybridisation theory/model makes the description much easier.
CarbonGoldAluminiumUranium

Question 2: Hybridisation theory is not as practical for quantitative calculations as ________.
Computational chemistryMolecular orbital theoryHartree–Fock methodChemical bond

Question 3: Hybridised orbitals are very useful in the explanation of the shape of ________ for molecules.
Hartree–Fock methodElectron configurationMolecular orbital theoryMolecular orbital

Question 4: It gives a simple orbital picture equivalent to ________.
Lewis structureNoble gasOxygenChemical bond

Question 5: The chemical bonding in compounds such as ________ with triple bonds is explained by sp hybridization.
AlkeneAlkaneAldehydeAlkyne

Question 6: That is, for a tetrahedrally coordinated carbon (e.g., ________, CH4), the carbon should have 4 orbitals with the correct symmetry to bond to the 4 hydrogen atoms.
PropaneMethanolOxygenMethane

Question 7: However, methylene is a very reactive molecule (see also: ________) and cannot exist outside of a molecular system.
ZincPersistent carbeneCarbonCarbene

Question 8: In CH4, four sp3 hybridised orbitals are overlapped by ________'s 1s orbital, yielding four σ (sigma) bonds (that is, four single covalent bonds).
HydrogenNitrogenHeliumOxygen

Question 9: The hybridisation theory was promoted by chemist ________[2] in order to explain the structure of molecules such as methane (CH4).
Linus PaulingRoger AdamsGlenn T. SeaborgMelvin Calvin

Question 10: Problems with hybridisation are especially notable when the d orbitals are involved in bonding, as in ________ and organometallic chemistry.
Inorganic chemistryPeriodic tableElectrochemistryCoordination complex
















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