Ionic Compounds and Their Properties

The video tutorial explains how to write the Lewis structure for potassium sulfate (K2SO4). It begins by identifying potassium as a metal and sulfate as a polyatomic ion composed of non-metals. The tutorial describes the formation of ionic compounds through electron transfer from metals to non-metals, resulting in ionic bonds. Potassium, being in group one of the periodic table, transfers its valence electron to the sulfate ion, forming a positive charge. The video illustrates the Lewis structure as a formula unit, representing the repeating pattern in the crystal structure of the ionic compound. The tutorial concludes with a summary of the process and thanks to the viewers.

What type of ion is sulfate in the compound K2SO4?

• Monatomic ion

• Anion

• Polyatomic ion

• Cation

What happens to the valence electrons of metals in ionic compounds?

• They are shared with non-metals.

• They are transferred to non-metals.

• They remain with the metal.

• They are lost to the environment.

How many valence electrons does potassium have?

• One

• Four

• Three

• Two

What charge does potassium acquire after losing an electron?

• No charge

• Positive

• Neutral

• Negative

Which group on the periodic table does potassium belong to?

• Group 2

• Group 4

• Group 3

• Group 1

What is the result of opposite charges in ionic compounds?

• They repel each other.

• They form covalent bonds.

• They attract each other.

• They become neutral.

What do the brackets in the Lewis structure of K2SO4 indicate?

• Loss and gain of electrons

• Sharing of electrons

• Neutrality of the compound

• Presence of covalent bonds

What is the main characteristic of an ionic bond?

• No electron movement

• Transfer of electrons

• Formation of molecules

• Sharing of electrons

What is a formula unit in the context of ionic compounds?

• A molecule

• The simplest ratio of ions

• A single atom

• A covalent bond

What type of structure does K2SO4 form?

• Crystalline

• Liquid

• Gaseous

• Amorphous