Classify each substance as being either ionic, molecular (i.e. all covalent bonds in the compound) or both (some ionic bonds and some covalent bonds in the compound)

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Classify each substance as being either ionic, molecular (i.e. all covalent bonds in the compound) or both (some ionic bonds and some covalent bonds in the compound). If you classify a substance as having both ionic and molecular components, draw a Lewis Dot Structure for the compound and clearly indicate which part of the compound is ionic in nature and which part is molecular (covalent). KClO Li2SO3 NH3 Cl2 KF NaSO4 HCl (gas) CCl4 SrCl2 CO2
. Classify each substance as being either ionic, molecular (i.e. all covalent bonds in the
compound) or both (some ionic bonds and some covalent bonds in the compound). If you
classify a substance as having both ionic and molecular components, draw a Lewis Dot
Structure for the compound and clearly indicate which part of the compound is ionic in nature
and which part is molecular (covalent).
KClO Li2SO3 NH3 Cl2 KF
NaSO4 HCl (gas) CCl4 SrCl2 CO2

The Correct Answer and Explanation is :

Let’s classify each substance based on its chemical composition and bonding:

  1. KClO (Potassium Chlorate):
  • Type: Ionic and Molecular (both).
  • Explanation: Potassium (K) is a metal and chlorine (Cl) is a non-metal, which typically forms ionic bonds with potassium. The oxygen (O) atoms in the compound are covalently bonded to chlorine. This results in a combination of ionic and covalent bonding in KClO.
  1. Li2SO3 (Lithium Sulfite):
  • Type: Ionic and Molecular (both).
  • Explanation: Lithium (Li) is a metal, and sulfur (S) and oxygen (O) are non-metals, forming ionic bonds between lithium and the sulfate (SO3) group. The bonding within the sulfate group itself is covalent.
  1. NH3 (Ammonia):
  • Type: Molecular (Covalent).
  • Explanation: Ammonia consists of nitrogen (N) and hydrogen (H), both non-metals. The bonds between them are covalent, making this a purely molecular compound.
  1. Cl2 (Chlorine gas):
  • Type: Molecular (Covalent).
  • Explanation: Chlorine gas is composed of two chlorine atoms (Cl) bonded covalently.
  1. KF (Potassium Fluoride):
  • Type: Ionic.
  • Explanation: Potassium (K) is a metal, and fluorine (F) is a non-metal. Potassium transfers an electron to fluorine, forming an ionic bond.
  1. NaSO4 (Sodium Sulfate):
  • Type: Ionic and Molecular (both).
  • Explanation: Sodium (Na) is a metal and sulfate (SO4) is a polyatomic ion with covalent bonds within the sulfate group. The bond between sodium and sulfate is ionic, while the bonds inside the sulfate ion are covalent.
  1. HCl (gas):
  • Type: Molecular (Covalent).
  • Explanation: Hydrogen (H) and chlorine (Cl) are both non-metals, and the bond between them is covalent.
  1. CCl4 (Carbon Tetrachloride):
  • Type: Molecular (Covalent).
  • Explanation: Carbon (C) and chlorine (Cl) are non-metals, and they form covalent bonds.
  1. SrCl2 (Strontium Chloride):
  • Type: Ionic.
  • Explanation: Strontium (Sr) is a metal, and chlorine (Cl) is a non-metal. The bond between them is ionic.
  1. CO2 (Carbon Dioxide):
    • Type: Molecular (Covalent).
    • Explanation: Carbon (C) and oxygen (O) are both non-metals, and the bonds between them are covalent.

Summary of Classification:

  • Ionic: KF, SrCl2.
  • Molecular (Covalent): NH3, Cl2, HCl, CCl4, CO2.
  • Ionic and Molecular: KClO, Li2SO3, NaSO4.

For those with both ionic and molecular components, such as KClO, Li2SO3, and NaSO4, the ionic bonds involve a metal and a non-metal, and the molecular part contains covalent bonds, typically between non-metals.

If you’d like to see a Lewis Dot structure for any of these compounds, feel free to ask!

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