Orbital Hybridization 1

Each carbon atom in ethyne forms two sp hybrid orbitals by mixing one 2s and one 2p orbital, along with two unhybridized p orbitals. The sp hybrid orbitals form sigma bonds with hydrogen and the other carbon, while the unhybridized p orbitals form pi bonds.

The strength of a C-C single bond is 348 kJ/mol, a double bond is 612 kJ/mol and a triple bond is 837 kJ/mol.

Triple bonds are shorter than double bonds, which are shorter than single bonds. Bond length decreases as the number of bonds between the atoms increases.

Sp hybridization involves mixing one 2s and one 2p orbital to form two equivalent sp hybrid orbitals.

Nitrogen exhibits sp3 (tetrahedral), sp2 (trigonal planar) hybridisation.

Ammonia's nitrogen atom has an sp3 hybridization, resulting in a tetrahedral geometry, but its pyramidal shape is due to lone pair repulsion.

Oxygen exhibits sp3 (tetrahedral) hybridisation..

Water's oxygen atom has an sp3 hybridization, resulting in a tetrahedral geometry, but its bent shape is due to lone pair repulsion.

Mixing atomic orbitals to form new, hybrid orbitals. This is essential for covalent bonding in molecules.

A region in space where an electron is most likely to be found.

An example of a molecule with sp3 hybridized carbon.

An example of a molecule with sp2 hybridized carbon.

An example of a molecule with sp hybridized carbon.

The electron arrangement of carbon atoms before hybridization.

Moving an electron from a lower energy orbital to a higher energy orbital to enable hybridization.

A single covalent bond between atoms, characterized by head-on overlap of orbitals.

A covalent bond formed by sideways overlap of p orbitals.

Sharing of electron pairs between atoms to form molecules.

New hybrid orbitals with intermediate shapes based on mixing atomic orbitals.

Simplest element with 1 electron.

Atomic orbitals are a representation of the probability of finding an electron in a specific region around an atom's nucleus. They describe the electron's energy level and spatial distribution within the atom.

S orbitals are spherical in shape, meaning that the probability of finding an electron is equal in all directions around the nucleus.

P orbitals have a dumbbell shape with two lobes along the x, y, or z axis. The probability of finding an electron is higher in the lobes.

Hybridization refers to the mixing of atomic orbitals of an atom to create new hybrid orbitals that have different shapes and energies than the original orbitals.

Hybridization allows atoms to form more stable and stronger bonds, explaining the geometry and bonding characteristics of many molecules, particularly organic molecules.

Linus Pauling, a Nobel Prize winner in chemistry, established the foundations of modern quantum chemistry, including the significance of orbital hybridization.

Carbon with sp3 hybridization has a tetrahedral geometry, meaning the four hybrid orbitals are arranged in a 3-dimensional pyramid shape with bond angles of 109.5 degrees.

Carbon with sp2 hybridization has a trigonal planar geometry, meaning the three hybrid orbitals lie in the same plane with bond angles of 120 degrees.

Carbon with sp hybridization exhibits a linear geometry. The bond angles are 180 degrees.

Ethyne, also known as acetylene, has a linear molecular geometry due to the sp hybridization of its carbon atoms. The bond angle between the carbon and hydrogen atoms is 180°.

A type of covalent bond formed by the sideways overlap of p orbitals. These bonds are weaker than sigma bonds and occur in addition to sigma bonds in double (C=C) and triple (C≡C) bonds.

Triple bonds (C≡C) are stronger and shorter than double bonds (C=C), which are stronger and shorter than single bonds (C-C). This is due to increased overlap of orbitals.

Ammonia has a pyramidal shape due to the sp3 hybridization of its nitrogen atom. The lone pair of electrons on nitrogen exerts a stronger repulsion than the bonding pairs, causing the molecule to bend.

Water has a bent shape due to the sp3 hybridization of its oxygen atom. The two lone pairs of electrons on oxygen strongly repel the bonding pairs, resulting in a smaller bond angle.

Nitrogen can exhibit sp3 (tetrahedral) and sp2 (trigonal planar) hybridization depending on the molecule it forms. For instance, ammonia exhibits sp3 hybridization, while nitrogen in the nitrate ion exhibits sp2 hybridization.

Oxygen commonly exhibits sp3 hybridization (tetrahedral) in molecules like water. This hybridization leads to a bent shape due to the influence of lone pairs.