Covalent Bonding: Sharing Electrons to Form Stable Molecules

The video explains how atoms seek stability by achieving full outer electron shells, often through covalent bonding. It covers the formation of single, double, and triple covalent bonds using examples like fluorine, oxygen, and nitrogen. The video also discusses how atoms with different electron needs, such as hydrogen and nitrogen, form compounds like ammonia. Various representations of covalent bonds, including molecular formulas and 3D models, are introduced. The concept of valency is explained, showing how it helps determine molecular formulas, exemplified by carbon sulfide.

Why do atoms strive to have a full outer shell of electrons?

• To increase their size

• To change their state of matter

• To become more reactive

• To achieve stability

What type of bond is formed when two fluorine atoms share electrons?

• Metallic bond

• Double covalent bond

• Ionic bond

• Single covalent bond

How many pairs of electrons are shared in a double covalent bond?

• Two pairs

• Four pairs

• One pair

• Three pairs

What is the result when hydrogen and nitrogen react to form ammonia?

• Hydrogen chloride

• Ammonia

• Water

• Nitrogen dioxide

Which model provides a three-dimensional representation of molecules?

• Lewis structure

• Structural formula

• Ball and stick model

• Dot and cross model

What is valency?

• The number of protons in an atom

• The number of covalent bonds an atom can form

• The number of electrons in the inner shell

• The number of neutrons in an atom

How many bonds does carbon form in carbon sulfide?

• Two bonds

• Three bonds

• Four bonds

• Five bonds