Question

What are the three basic types of chemical bonds? What happens to electrons in the bonding atoms in each type?

Short answer

The three basic types of chemical bonds are ionic (transfer of electrons), covalent (sharing of electrons), and metallic (free-moving 'sea' of electrons).

Step-by-step solution

Identify the Types of Chemical Bonds

The three basic types of chemical bonds are ionic bonds, covalent bonds, and metallic bonds.

Describe Electron Interaction in Ionic Bonds

In ionic bonds, electrons are transferred from one atom to another, creating ions. One atom loses electrons and becomes positively charged (cation), while the other gains electrons and becomes negatively charged (anion).

Describe Electron Interaction in Covalent Bonds

In covalent bonds, electrons are shared between atoms to fill their outer shells. Each shared electron pair forms a bond, and this sharing can be equal (nonpolar covalent bond) or unequal (polar covalent bond).

Describe Electron Interaction in Metallic Bonds

In metallic bonds, electrons are delocalized and move freely among the positively charged metal ions. This 'electron sea' allows metals to conduct electricity and heat and also provides them with malleability.

Key concepts

Ionic Bonds

Ionic bonds are fascinating phenomena where atoms quite literally exchange electrons to achieve greater stability. Imagine a schoolyard where children are playing a game of swapping cards. In chemistry, certain atoms have 'cards' (electrons) that they wish to give away and others are eager to collect them. When one atom gives up an electron, it becomes a cation with a positive charge, since it now has fewer electrons than protons.

The atom that collects this electron turns into an anion, gaining a negative charge as its electron count exceeds its number of protons. This transfer of electrons transforms the atoms into ions, like players scoring points to win the game. The opposite charges of these ions attract each other, just as the two ends of a magnet do, forming an ionic bond. For example, in table salt (NaCl), sodium (Na) donates an electron to chlorine (Cl), creating a bond that holds them together. This type of bond is typically found between metals and non-metals.

Covalent Bonds

Covalent bonds are all about teamwork. Rather than hoard electrons for themselves, atoms involved in covalent bonds share electrons in a communal manner to fill their outer electron shells, akin to carpooling. Just like friends sharing a ride to work to save resources, atoms that share electrons benefit from each other.

Each shared pair of electrons forms a bond that ties the atoms together. These can be shared equally where the bonded atoms exert similar pull on the electrons, resulting in nonpolar covalent bonds. Sometimes, as in the case of water (H2O), one atom, like oxygen, might have a stronger pull, leading to an unequal sharing of electrons and polar covalent bonds. Oxygen holds the shared electrons closer more often than the hydrogens do, creating a slight imbalance in charge. Because of this sharing, molecules formed by covalent bonds, such as DNA and proteins, give shape and function to the matter of life.

Metallic Bonds

Metallic bonds are the mavericks of bonding, characterized by a 'sea' of delocalized electrons surrounding metal ions. This is much like a group of dancers moving freely on a dance floor among fixed dance partners (metal ions).

The electrons are not tied to any one atom but instead flow freely among the positively charged metal ions. This freedom of movement of the electrons allows metals to conduct electric current and heat with ease - much like the dancers' fluid movements might make it easy to quickly pass messages across a crowded room. Furthermore, the metallic bond is behind the ductility and malleability of metals; it's like the dancers being able to switch partners without any disruptions to the overall dance, allowing the shape of the metal to change without shattering. This type of bonding is unique to metals and alloys, explaining properties that we rely on in building structures and in manufacturing electronics.