Chemical Bonding Overview

The energy change that occurs when one mole of sodium atoms in the gaseous state loses one electron to form one mole of sodium ions in the gaseous state.

The energy change that occurs when one mole of chlorine atoms gains one electron to form one mole of chloride ions in the gaseous state.

The energy released when one mole of sodium ions and one mole of chloride ions combine to form one mole of solid sodium chloride.

The overall energy change in a chemical reaction.

A chemical reaction that releases energy into its surroundings.

A chemical compound formed by the electrostatic attraction between positively and negatively charged ions.

An atom or group of atoms that has gained one or more electrons and carries a negative charge.

An atom or group of atoms that has lost one or more electrons and carries a positive charge.

The force of attraction that holds ions together in an ionic compound. It involves the transfer of electrons between atoms with different electronegativities.

The smallest whole number ratio of atoms in a compound.

The chemical formula that shows the actual number of atoms of each element in a molecule or compound.

The process of forming an ionic bond by the transfer of electrons from a metal atom to a nonmetal atom.

The energy released when an ionic compound is formed from its constituent elements in their standard states.

A method that uses X-rays to determine the positions of atoms in a crystal, giving us insights into the distances between nuclei.

The distance between the centers of two adjacent atoms in a crystal lattice.

The average distance between the nucleus and the outermost electron shell of an atom or ion.

Atoms or ions that have the same number of electrons and the same electron configuration.

The process of determining the radius of an ion by subtracting half the distance between two identical ions from the distance between a cation and an anion.

Metals, located on the lower left of the periodic table, tend to lose electrons (low ionization energy), forming positively charged ions called cations.

Nonmetals, located on the upper right of the periodic table, tend to gain electrons (high electron affinity), forming negatively charged ions called anions.

Group IA and IIA metals form cations with a charge equal to their group number by losing all their valence electrons ('s' and 'p' electrons). Their electronic configuration becomes like the preceding noble gas.

Group IIIA to VA metals form cations with a charge equal to their group number minus two, by losing only their 'p' valence electrons. They retain their 's' electrons.

The electronic configuration of these cations (Group IIIA to VA) resembles the preceding 'pseudo-noble gas' configuration + ns2 (where 'n' is the principal quantum number).

The charge of an ion is determined by the difference between the number of protons (positive charge) and electrons (negative charge).

The formation of ionic compounds involves the transfer of electrons from a metal atom to a nonmetal atom, resulting in a stable ionic bond.

A strong attractive force that exists between atoms in a substance.

A chemical bond formed by the sharing of electrons between two nonmetal atoms.

A chemical bond formed by the delocalized sharing of electrons between metal atoms.

Electrons in the outermost energy level of an atom.

A shorthand representation of an atom that shows the element symbol surrounded by dots representing valence electrons.

The core of a Lewis Dot Symbol that represents the noble gas configuration of the atom's inner electrons.

The core of a Lewis Dot Symbol that represents the pseudo noble gas configuration of the atom's inner electrons.

A compound formed by the electrostatic attraction between oppositely charged ions.

The process of forming an ionic bond by transferring electrons between atoms.

The electrostatic attraction between oppositely charged ions, causing them to bond together.

The state of matter where a salt is a solid and has a high melting point.

Any substance that conducts electricity when dissolved in water or melted

For cations of the same element, the larger the positive charge, the smaller the ion.

Cations have fewer electrons than their neutral atom counterpart. This results in a stronger pull from the nucleus, causing the ion to shrink.

For anions of the same element, the larger the negative charge, the larger the ion.

Anions have more electrons than their neutral atom counterpart. This leads to increased electron-electron repulsion, causing the ion to expand.

The size of an atom or ion is determined by the average distance of its outermost electrons from the nucleus.

The nucleus of an atom has a positive charge, while the electrons surrounding it have a negative charge.

The attraction between the nucleus and the electrons is what keeps the atom or ion intact.

The repulsion between electrons in the same energy level can cause an increase in ionic size.

The size of an ion is related to the strength of the nuclear attraction and inter-electron repulsion forces.