Ionic compounds typically have high melting and boiling points, and are hard and brittle. As solids they are almost always electrically insulating, but when melted or dissolved they become highly conductive, because the ions are mobilized.

The two main types of chemical bonds are ionic and covalent bonds. An ionic bond essentially donates an electron to the other atom participating in the bond, while electrons in a covalent bond are shared equally between the atoms. The only pure covalent bonds occur between identical atoms.

Calcium chloride CaCl2 is the only ionic compound from the given choices.

Properties Shared by Ionic Compounds

• They form crystals.
• They have high melting points and high boiling points.
• They have higher enthalpies of fusion and vaporization than molecular compounds.
• They’re hard and brittle.
• They conduct electricity when they are dissolved in water.
• They’re good insulators.

Ionic compounds contain ions and are held together by the attractive forces among the oppositely charged ions. Common salt (sodium chloride) is one of the best-known ionic compounds. Molecular compounds contain discrete molecules, which are held together by sharing electrons (covalent bonding).

Ionic Compound Properties

• Physical properties of ionic compounds. Due to the presence of the strong force of attraction between the positive and negative ions, ionic compounds are solids and are hard to break.
• Melting and boiling points of ionic compounds.
• The solubility of ionic compounds.
• Conduction of Electricity.

Explanation: Ionic compounds include salts, oxides, hydroxides, sulfides, and the majority of inorganic compounds. Ionic solids are held together by the electrostatic attraction between the positive and negative ions. For example, the sodium ions attract chloride ions and the chloride ion attracts sodium ions.

Answer. Most ionic compounds are soluble in water. This is because polar water molecules have a strong attraction for charged ions. The charged ions become solvated as they dissociate into water.

Ionic bond examples include:

• LiF – Lithium Fluoride.
• LiCl – Lithium Chloride.
• LiBr – Lithium Bromide.
• LiI – Lithium Iodide.
• NaF – Sodium Fluoride.
• NaCl – Sodium Chloride.
• NaBr – Sodium Bromide.
• NaI – Sodium Iodide.

Compounds Examples

• Water – Formula: H2O = Hydrogen2 + Oxygen.
• Hydrogen Peroxide – Formula: H2O2 = Hydrogen2 + Oxygen2
• Salt – Formula: NaCl = Sodium + Chlorine.
• Baking Soda – Formula: NaHCO3 = Sodium + Hydrogen + Carbon + Oxygen3
• Octane – Formula: C8H18 = Carbon8 + Hydrogen18

Classifying compounds as ionic or covalent

1. If a compound is made from a metal and a non-metal, its bonding will be ionic.
2. If a compound is made from two non-metals, its bonding will be covalent.

Both CO2 and H2O have two polar bonds. However the dipoles in the linear CO2 molecule cancel each other out, meaning that the CO2 molecule is non-polar. The polar bonds in the bent H2O molecule result in a net dipole moment, so H2O is polar.

The difference between Ionic and Molecular Compounds is that the electrons of atoms in ionic compounds are transferred between the elements because of the presence of a difference in electronegativity. However, in the case of molecular compounds, the electrons are only shared but not transferred.

The answer has to do with the type of compound that calcium chloride is. Calcium chloride is an ionic compound.

Formula and structure: The chemical formula of calcium chloride is CaCl2, and its molar mass is 110.983 g/mol. It is an ionic compound consisting of the calcium cation (Ca2+) and two chlorine anions (Cl-). The bivalent calcium metal forms an ionic bond with two chlorine atoms, as shown below.

For example, in the reaction of calcium and chlorine, the compound is called calcium chloride. It is composed of Ca2+ cations and Cl– anions; those ions are stable since they have filled valence shells. Its ionic formula is written as CaCl2, the neutral combination of these ions.

Two atoms of Chlorine and one atom of Calcium are near each other. Because of the stronger attraction, each chlorine pulls in one electron from the Calcium atom.

Barium chloride is an ionic compound composed of one barium cation and two chlorine anions.

Since each chlorine atom gained an electron, they each have 17 protons and 18 electrons. This makes each chloride a negative ion with a charge of −1. Oppositely charged ions attract each other, forming an ionic bond. The bonded ions are more stable than the individual atoms were.

In the given elements chlorine (2,8,7) is a non metal with highest electronegativity. Hence, it is most likely to form a negative ion with charge −1.