OR Retake ET 13

Front

What is a dsp3 hybrid orbital?

Back

A dsp3 hybrid orbital is formed by the combination of one d orbital, one s orbital, and three p orbitals, resulting in five equivalent orbitals. It is typically found in compounds with trigonal bipyramidal geometry, such as PCl5.

Front

Which compound is a radical?

Back

NO2 is a radical because it has an unpaired electron, making it highly reactive.

Front

How many sigma (σ) and pi (π) bonds are in carbon dioxide (CO2)?

Back

Carbon dioxide (CO2) has 2 sigma (σ) bonds and 2 pi (π) bonds.

Front

What is valence bond theory?

Back

Valence bond theory explains how atoms in a molecule bond by overlapping their atomic orbitals to form covalent bonds.

Front

What is the hybridization of methane (CH4)?

Back

Methane (CH4) has sp3 hybridization, where one s orbital and three p orbitals combine to form four equivalent sp3 hybrid orbitals.

Front

What is the geometry of a molecule with dsp3 hybridization?

Back

The geometry of a molecule with dsp3 hybridization is trigonal bipyramidal.

Front

What is the incorrect statement about valence bond theory?

Back

A dsp4 hybrid orbital does not exist; the correct term is dsp3, which allows for the formation of hypervalent compounds.

Front

What is a hypervalent compound?

Back

A hypervalent compound is a molecule that has more than four pairs of electrons around a central atom, such as SF6.

Front

What is the significance of unpaired electrons in radicals?

Back

Unpaired electrons in radicals make them highly reactive, as they seek to pair up with other electrons.

Front

What type of bonds does nitrogen (N2) have?

Back

Nitrogen (N2) has one sigma (σ) bond and three pi (π) bonds, making it a triple bond.