Show the acceptable Lewis structure to form covalent bond in the
following compounds:
a. NH3
b. H2O
c. HCl
d. PH3
e. H2
Answer (1)
Answer:Here are the acceptable Lewis structures for the given compounds, showing covalent bonds:A. NH3 (Ammonia) Nitrogen (N) is the central atom with 5 valence electrons. It shares one electron with each of the three hydrogen (H) atoms, forming three single covalent bonds. Nitrogen also has one lone pair of electrons.B. H20 (Water) Oxygen (O) is the central atom with 6 valence electrons. It shares one electron with each of the two hydrogen (H) atoms, forming two single covalent bonds. Oxygen also has two lone pairs of electrons.C. HCl (Hydrogen Chloride) Hydrogen (H) and Chlorine (Cl) each share one electron to form a single covalent bond.D. PH3 (Phosphine) Phosphorus (P) is the central atom with 5 valence electrons. Similar to NH3, it shares one electron with each of the three hydrogen (H) atoms, forming three single covalent bonds. Phosphorus also has one lone pair of electrons.E. H2 (Hydrogen Gas) Each hydrogen (H) atom shares its single electron with the other hydrogen atom, forming a single covalent bond. In these Lewis structures, a single line (-) represents a single covalent bond (a shared pair of electrons). Lone pairs of electrons (not involved in bonding) are often shown as dots. The structures aim to satisfy the octet rule (except for hydrogen, which only needs 2 electrons) for each atom involved
