In terms of valence electrons, what must happen for an ionic bond to form between initially neutral atoms? What kind of atoms are likely to do what you describe? Give an example.

An ionic bond forms when electrons from one atom are transferred to another atom, resulting in the formation of ions. One atom becomes a positively charged cation and the other becomes a negatively charged anion. These ions are then attracted to each other due to their opposite charges, resulting in an ionic bond.

Valence electrons are the electrons present in the outermost shell of an atom. In order for an ionic bond to form between initially neutral atoms, the following must happen: 1. One atom must lose valence electrons, turning into a cation with a positive charge. 2. The other atom must gain the lost valence electrons, turning into an anion with a negative charge.

Ionic bonds typically occur between a metal and a non-metal atom. Metal atoms tend to lose their valence electrons because they have fewer electrons in their valence shell, which requires less energy to lose than to gain more electrons to achieve a stable shell. On the other hand, non-metal atoms tend to gain electrons to achieve a stable, full valence shell.

Let's consider the ionic bond formation between sodium (Na) and chlorine (Cl). 1. Sodium (Na) has one valence electron (2,8,1 electron configuration) and is a metal. It becomes a cation (Na+) by losing its valence electron, which requires less energy than gaining seven more electrons to achieve a stable shell. 2. Chlorine (Cl) has seven valence electrons (2,8,7 electron configuration) and is a non-metal. It becomes an anion (Cl-) by gaining one electron, which allows it to achieve a stable, full valence shell (2,8,8 electron configuration). 3. The resulting positively charged Na+ ion and negatively charged Cl- ion are attracted to each other, forming an ionic bond and creating the ionic compound sodium chloride (NaCl), also known as table salt.