Ionic Bonds and Valence Electrons

The video tutorial explains how to draw the Lewis structure for barium fluoride (BaF2). It covers the nature of ionic compounds, where valence electrons are transferred from metals to non-metals. Barium, a group 2 element, has two valence electrons, while fluorine, a group 17 element, has seven. The tutorial details how barium transfers its electrons to fluorine, resulting in a two-plus charge for barium and a negative charge for each fluorine. The use of brackets to denote ionic charges is also explained, emphasizing the difference from covalent bonds.

What type of compound is formed when barium and fluorine combine?

• Covalent compound

• Ionic compound

• Metallic compound

• Molecular compound

How many valence electrons does barium have?

• 1

• 2

• 7

• 8

In which group is fluorine found on the periodic table?

• Group 1

• Group 2

• Group 17

• Group 18

What happens to the valence electrons of barium in the formation of barium fluoride?

• They are transferred to fluorine.

• They are shared with fluorine.

• They are lost to the environment.

• They remain with barium.

What charge does barium have after losing its valence electrons?

• 1+

• 2+

• 1-

• 2-

Why are brackets used around the ions in the Lewis structure?

• To show the transfer of electrons.

• To denote the atomic mass.

• To highlight the atomic number.

• To indicate shared electrons.

What is the charge on each fluorine ion after gaining an electron?

• 2-

• 1-

• 2+

• 1+

How does an ionic bond differ from a covalent bond?

• Ionic bonds involve transferring electrons.

• Ionic bonds involve sharing electrons.

• Covalent bonds involve losing electrons.

• Covalent bonds involve transferring electrons.

What is the main characteristic of an ionic compound?

• Electrons are shared unequally.

• Electrons are transferred from non-metal to metal.

• Electrons are shared equally.

• Electrons are transferred from metal to non-metal.