This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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Step 1a: Definition of covalent bond A covalent bond is a chemical bond formed when two atoms share one or more pairs of valence electrons to achieve stable electron configurations. Step 1b: Definition of covalent compounds Covalent compounds are substances composed of molecules formed by covalent bonds between non-metal atoms. They typically have low melting and boiling points and do not conduct electricity in any state. Examples: H_2O (water), CO_2 (carbon dioxide), CH_4 (methane). Step 1c: Definition of ionic bond and compounds where found An ionic bond is a chemical bond formed by the electrostatic attraction between oppositely charged ions, resulting from the complete transfer of electrons from a metal atom (forms cation) to a non-metal atom (forms anion). Ionic bonds are found in the following compounds: NaCl (sodium chloride), KCl (potassium chloride), MgO (magnesium oxide), CaCl_2 (calcium chloride). Step 2: Bond found in the following compounds (common examples) Assuming typical examples like: a. NaCl: Ionic bond. b. HCl: Covalent bond (polar). c. H_2O: Covalent bonds. d. AlCl_3: Covalent bond (if listed). Step 3: Formation of ionic bond with diagram (e.g., NaCl) Ionic bond formation in NaCl: Sodium (Na, group 1, 1 valence electron) loses 1 electron to achieve stable octet. Na → Na^+ + e^- Chlorine (Cl, group 17, 7 valence electrons) gains 1 electron to achieve stable octet. Cl + e^- → Cl^- The Na^+ and Cl^- ions are held together by strong electrostatic attraction. Diagram description (Lewis structure): Na atom: [Na] · (1 dot) loses dot → [Na^+] Cl atom: :Cl· (7 dots) gains dot → [:Cl:]^- Ionic lattice: Na^+ Cl^- Na^+ Step 4: Formation of covalent bond with diagram (e.g., H_2) Two hydrogen atoms each with 1 valence electron share a pair. H · + · H → H:H Shared pair (single bond) allows both to have duet. For H_2O: Oxygen shares 1 electron with each H. Lewis: Central O with two lone pairs, single bonds to two H. H-O-H (Note: Simple text representation; actual diagram shows dots for shared pairs.)