Fundamentals of Chemical Bonding: Core and Valence Electrons

CORE electrons refer to the electrons located close to the nucleus of an atom, providing stability and playing a key role in chemical bonding.

Valence electrons are the electrons in the outermost energy level of an atom and are involved in bonding with other atoms to form molecules. They are typically found in the s and p subshells of an atom's electron configuration.

Valence electrons are the electrons in the outermost shell of an atom that are involved in bonding. Proton electrons, conduction electrons, and inert electrons do not play a role in holding atoms in a chemical bond.

A chemical bond is the force of attraction between 2 atoms in a compound, which helps hold the atoms together. It involves overcoming repulsion between the positively charged nuclei and the negatively charged electrons of the atoms involved.

The Octet Rule states that atoms will gain, lose, or share electrons in order to have a full outer shell with 8 electrons, leading to greater stability.

Atoms can achieve an octet through ionic bonding by transferring electrons to achieve a full outer shell, or through covalent bonding by sharing electrons with another atom. Metallic bonding involves a sea of delocalized electrons, hydrogen bonding is a specific type of dipole-dipole interaction, and van der Waals interactions are weak intermolecular forces.

Ionic bonding involves the transfer of electrons, not sharing, and results in the formation of an ionic compound.

Ionic bond formation occurs between a metal and a non-metal where the metal loses electrons to become a cation and the non-metal gains those electrons to become an anion. This results in a bond between ions of opposite charge.

Ionic compounds typically adopt a crystalline lattice structure where positively charged metal ions are surrounded by negatively charged nonmetal ions. This arrangement helps ensure the overall stability of the compound.

Covalent bonding involves the sharing of pairs of electrons between atoms, unlike ionic bonding which involves the transfer of electrons.

The octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with 8 valence electrons. Hydrogen is an exception to this rule as it only requires 2 electrons to achieve stability, hence forming diatomic molecules like H2.

Covalent compounds are formed by the sharing of electrons between atoms, typically between atoms with similar tendencies to gain or lose electrons. Diatomic elements also exhibit complete covalent bonding due to their nature. The incorrect answers provided do not accurately describe the key features and rules for covalent compounds.

Polar covalent bonds are characterized by unequal sharing of electrons, leading to a partial positive and partial negative charge on the atoms involved. This is different from purely covalent bonds where electrons are shared equally, ionic bonds where electrons are transferred, and metallic bonds which involve a sea of delocalized electrons in a lattice structure.

Water (H2O) is known for having polar covalent bonds because of the unequal sharing of electrons between the partially positive hydrogen (+ve) and the partially negative oxygen (-ve), where the electron is drawn closer to the oxygen atom than the hydrogen atoms. This unequal distribution of electrons creates a partial positive and partial negative charge within the molecule.

Coordinate covalent bonding is a type of covalent bonding where one atom donates a lone pair of electrons to another atom to form a bond. This differs from regular covalent bonding, where electrons are shared between atoms equally. The example given represents the formation of ozone (O3) from oxygen molecules (O2) through coordinate covalent bonding.

Hydrogen bonding is a strong intermolecular force that occurs between a hydrogen atom and a highly electronegative atom such as fluorine (F), nitrogen (N), or oxygen (O). It is not a type of covalent bonding, nor is it a weak force between two hydrogen atoms or an interaction between a hydrogen atom and a metal atom.

Electronegativity is a fundamental concept in chemistry that describes an atom's ability to attract electrons in a chemical bond. It is measured using a numerical scale and plays a crucial role in understanding the nature of chemical reactions.

Electro-negativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself. Fluorine is the most electro-negative element, while Francium is the least electro-negative element.

A polar bond occurs when there is an unequal sharing of electrons due to a difference in electronegativity between the atoms involved.

Nomenclature refers to the systematic way of naming chemical compounds to ensure clarity and consistency in communication within the scientific community.