Locate fluorine (F) on the partial periodic table provided in Figure 2.2. Predict its relative electronegativity compared to hydrogen, sodium, and oxygen. State the number and type of bond(s) you expect it would form if it reacted with sodium (Na).

Electronegativity is a measure of an atom's ability to attract and hold onto electrons when forming chemical bonds. It is a key factor in determining how atoms interact with each other. In the periodic table, electronegativity generally increases across a period from left to right and decreases down a group. Fluorine, being in the top right corner of the periodic table, is the most electronegative element.

Chemical bonding refers to the forces that hold atoms together in compounds. The main types of bonds are ionic, covalent, and metallic. When sodium (Na) reacts with fluorine (F), an ionic bond is expected to form due to the transfer of an electron from sodium to fluorine, resulting in the formation of Na+ and F- ions. Understanding the type of bond helps predict the properties of the resulting compound.

Periodic trends are patterns observed in the periodic table that illustrate how certain properties of elements change across periods and down groups. These trends include atomic radius, ionization energy, and electronegativity. Recognizing these trends is essential for predicting the behavior of elements, such as the relative electronegativity of fluorine compared to hydrogen, sodium, and oxygen, which influences their bonding characteristics.