Do you have enough knowledge about ionic compounds and their properties? If yes, play this trivia quiz and prove it to us. An ionic compound in chemistry is a chemical compound made up of ions (cations and anions) that are held by electrostatic forces, commonly known as ionic bonding. Here, we have asked some questions related to those bonds. So, if you think you can easily answer the questions asked here. Take the quiz now. All the best, buddy!
The electrostatic forces of attraction between the positive and negative ions holding the lattice together are very strong and a lot of energy is required to break them apart.
The electrostatic forces of attraction between the positive ions holding the lattice together are very strong and a lot of energy is required to break them apart.
The electrostatic forces of attraction between the positive and electrons holding the lattice together are very strong and a lot of energy is required to break them apart.
The electrostatic forces of attraction between the cations and anions holding the lattice together are very weak and a less energy is required to break them apart.
When hit with a hammer, the like-charged ions line up together and they draw closer together due to electrostatic attraction and this causes the ionic compound to shatter.
When hit with a hammer, the opposite-charged ions line up together and they attract due to electrostatic forces and this causes the ionic compound to shatter.
When hit with a hammer, the like-charged ions line up together and they repel due to electrostatic repulsion and this causes the ionic compound to shatter.
When hit with a hammer, the cations disperse and they repel due to electrostatic repulsion and this causes the ionic compound to shatter.
Flourine. Reason- metal forms cation as it tends to lose electrons.
Calcium. Reason - non-metal forms cation as it tends to gain electrons
Flourine. Reason - non-metal forms cation as it tends to lose electrons.
Calcium. Reason - metal forms cation as it tends to lose electrons.
MgO2
CaO2
MgO
CaO
2 Mg 2+ : 1 Cl-
1 Mg 2+ : 2 Cl-
2 Mg 2+ : 3 Cl-
1 Mg 2+ : 1 Cl-
Calcium oxide
Potassium oxide
Sodium oxide
Barium oxide
AlS
Al2S
AlS3
Al2S3
As a solid
As a liquid
When dissolved in water
When warmed slightly
Soft
Conduct electricity when dissolved in water
High melting and boiling points
Crystal lattice structure
A chemical compound
An ionic chalice
A crystal lattice
An ionic bond