5 Questions
Explain the concept of covalent bonding.
Covalent bonding occurs when non-metal atoms share electrons to achieve a full outer energy level.
Describe the covalent bond formation in a hydrogen molecule (H2).
In H2, each hydrogen atom shares an electron to form a single covalent bond, resulting in a full outer energy level for both atoms.
How can covalent bonding be represented?
Covalent bonding can be represented through energy level diagrams, dot and cross diagrams, and stick diagrams.
Explain the covalent bond formation in a chlorine molecule (Cl2).
In Cl2, two chlorine atoms share electrons to achieve a full outer energy level, forming a single covalent bond.
Provide an example of a covalent molecule and explain its bond formation.
Hydrogen chloride (HCl) is a covalent molecule where a hydrogen atom and a chlorine atom share electrons to attain a full outer energy level, creating a covalent bond.
Study Notes
- Covalent bonding occurs between non-metal atoms when they share electrons to achieve a full outer energy level.
- In a hydrogen molecule (H2), each hydrogen atom (non-metal) shares an electron to form a single covalent bond, resulting in a full outer energy level for both atoms.
- Covalent bonding can be represented through energy level diagrams, dot and cross diagrams, and stick diagrams.
- The chlorine molecule (Cl2) consists of two chlorine atoms (non-metals) sharing electrons to achieve a full outer energy level, forming a single covalent bond.
- Hydrogen chloride (HCl) is another example of a covalent molecule, where a hydrogen atom and a chlorine atom share electrons to attain a full outer energy level, creating a covalent bond.
Test your knowledge on covalent bonding and molecules with this quiz. Learn about how non-metal atoms share electrons to achieve a full outer energy level, and explore representations such as energy level diagrams, dot and cross diagrams, and stick diagrams.
Make Your Own Quizzes and Flashcards
Convert your notes into interactive study material.
Get started for free
