Flashcards for:
Chemical Bonding and Parental Gratitude

Molecular orbitals are formed by the linear combination of atomic orbitals from different atoms. When atomic orbitals overlap constructively, bonding molecular orbitals are formed, whereas destructive overlap results in anti-bonding molecular orbitals.

The Chotila Mata Ji method simplifies bonding order calculation by using a mnemonic or a particular algorithm to quickly identify the bonding order based on the number of electrons in the molecular orbitals.

The magnetic properties of a molecule can be determined by examining the number of unpaired electrons in its molecular orbitals. If there are unpaired electrons, the molecule is paramagnetic; if all electrons are paired, it is diamagnetic.

Unpaired electrons generate a magnetic dipole, making the molecule paramagnetic. Thus, the molecule is attracted to a magnetic field. In contrast, molecules with all paired electrons are diamagnetic and repel magnetic fields.

Anti-bonding molecular orbitals result from the destructive interference of atomic orbitals. They have higher energy than the original atomic orbitals and can weaken or destabilize a molecule when occupied by electrons.

The Sigma star (σ*) orbital is an anti-bonding molecular orbital. Occupation of this orbital by electrons can weaken the bond between atoms because it has a higher energy level and destructively interacts with atomic orbitals.

The Molecular Orbital Theory describes the combination of atomic orbitals (like 1s, 2s, 2p orbitals) to form molecular orbitals that extend over a molecule. It helps in understanding the bonding structure within a molecule. Each molecular orbital can hold two electrons with opposite spins.

Bonding order is calculated as half the difference between the number of bonding electrons and anti-bonding electrons: (Bonding electrons - Anti-bonding electrons) / 2.

Paramagnetic substances have unpaired electrons and are attracted to magnetic fields, whereas diamagnetic substances have all paired electrons and are repelled by magnetic fields.

Understanding molecular orbitals allows chemists to predict the bonding characteristics, stability, magnetic properties, bond length, and bond energy of molecules. It provides a more detailed and accurate picture of how atomic orbitals combine and influence molecular structure.

N2 (molecular nitrogen) is an example of a diamagnetic molecule because all of its electrons are paired in its molecular orbitals.

Molecular orbital diagrams show the distribution of electrons in bonding and anti-bonding orbitals. By identifying the presence of unpaired electrons in these diagrams, one can predict if a molecule is paramagnetic (with unpaired electrons) or diamagnetic (with all paired electrons).

O2 (molecular oxygen) is an example of a paramagnetic molecule because it has unpaired electrons in its molecular orbitals.

The molecular orbital diagram of hydrogen involves the combination of two 1s atomic orbitals to form a bonding molecular orbital (Sigma 1s) and an anti-bonding molecular orbital (Sigma star 1s).

Bonding order indicates the stability of a bond; the higher the bonding order, the stronger the bond. It also predicts bond length and bond energy.