NaH is a compound formed by the combination of sodium (Na) and hydrogen (H). When discussing the type of bonding in NaH, it is important to consider the electron configuration of these elements and their ability to gain or lose electrons.
Sodium is a metal and belongs to Group 1 of the periodic table. It has one valence electron in its outermost energy level. This electron is relatively far from the nucleus and experiences a weak attraction, making it easier for sodium to lose this electron and achieve a stable electron configuration. By losing this electron, sodium forms a positively charged ion, Na+.
Hydrogen, on the other hand, is a nonmetal and has one valence electron in its outermost energy level. Hydrogen is highly electronegative and tends to gain an electron to achieve a stable electron configuration. By accepting an electron, hydrogen forms a negatively charged ion, H-.
In NaH, sodium donates its valence electron to hydrogen, resulting in the formation of Na+ and H- ions. These ions are attracted to each other due to their opposite charges, leading to the formation of an ionic bond.
Ionic bonding is a type of chemical bonding that occurs between ions of opposite charges. In this case, the positively charged sodium ion (Na+) is attracted to the negatively charged hydrogen ion (H-), resulting in the formation of an ionic compound.
The ionic bond in NaH is characterized by the strong electrostatic attraction between the Na+ and H- ions. This attraction holds the ions together in a crystal lattice structure, where each sodium ion is surrounded by several hydrogen ions and vice versa.
NaH exhibits ionic bonding due to the transfer of an electron from sodium to hydrogen. The resulting Na+ and H- ions are held together by strong electrostatic forces, forming an ionic compound.