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Chemical bonding is at the heart of understanding how different substances come together to form new materials with unique properties. There are several types of bonds, but the focus here is on the two main categories: ionic and covalent bonds. As you may recall from your studies, atoms bond together to achieve a full outer shell of electrons, mimicking the stability of noble gases in the periodic table. This drive towards stability is what powers the formation of chemical bonds.

When exploring chemical bonding, it's also crucial to understand how these interactions relate to the periodic table. Metals found on the left side have a tendency to lose electrons, leading to the formation of ionic bonds with non-metals on the right side which are keen on gaining those electrons. The sharing of electrons between non-metals, though, results in covalent bonds. Simply put, the type of bond an atom participates in is influenced by its position on the periodic table and its electron configuration.

Digging deeper into the concept of electron configuration reveals much about why certain elements form the types of bonds they do. Every atom desires to achieve an electron configuration that is, in terms of energy, the most favorable. This often means having a set of 'full' outer shells. For many atoms, this requires the gain, loss, or sharing of electrons.

This is where ionic and covalent bonds come into play. In an ionic bond, a metal atom, usually with few valence (outer shell) electrons, will transfer electrons to a non-metal atom with a nearly full valence shell. However, in a covalent bond, atoms tend to share electrons to fill their valence shells, without complete transfer. The trend across the periodic table from losing to gaining electrons helps us predict the type of bonding that will occur between different elements.

Ionic compounds are fascinating in their crystalline structure and they exhibit a distinctive set of properties due to the strong electrostatic forces at work within their lattice. These compounds generally possess high melting and boiling points, meaning they require substantial amounts of energy to break the ionic bonds. This makes ionic substances like table salt solid at room temperature.

Other intriguing properties arise when ionic compounds are in the molten state or dissolved in water. In these situations, the ions are free to move, which allows ionic compounds to conduct electricity, making them electrolytes. This is the principle behind the electrical conductivity of solutions used for electrolytes in batteries and bodily fluids. Thus, these properties can be tied to the movement and nature of ions in different states of matter.

Covalent compounds, on the other hand, exhibit a different suite of properties due to their shared electrons. These compounds tend to have lower melting and boiling points compared to ionic compounds because the forces holding the molecules together—while strong within the molecule—are weaker in between molecules. In most cases, this results in covalent substances being liquids or gases at room temperature.

Moreover, covalent compounds are typically poor conductors of electricity due to the absence of free-moving charged particles. This characteristic is why substances such as oil or plastic, which are covalent in nature, are often used as electrical insulators. The physical states and conductivity of covalent compounds are important considerations when understanding their role in chemical processes and their applications in everyday life.