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Step 1:I'll solve this problem by providing five clear examples of covalent bonds with explanations:
Step 2:: Hydrogen Molecule (H₂)
- Represented by $$H - H
- Two hydrogen atoms share their electrons to form a single covalent bond - Each hydrogen atom contributes one electron to create a stable electron pair
Step 3:: Water Molecule (H₂O)
- Represented by $$H - O - H
- Oxygen atom shares electrons with two hydrogen atoms - Forms a bent molecular structure - Creates polar covalent bonds due to electronegativity differences
Step 4:: Carbon Dioxide (CO₂)
- Represented by $$O = C = O
- Central carbon atom forms double covalent bonds with two oxygen atoms - Linear molecular geometry with symmetrical electron sharing
Step 5:: Methane (CH₄)
- Represented by $$H - C - H
- Central carbon atom forms single covalent bonds with four hydrogen atoms - Tetrahedral molecular structure
Step 6:: Nitrogen Gas (N₂)
- Represented by $$N \equiv N
- Two nitrogen atoms form a triple covalent bond - Extremely strong bond, making nitrogen gas very stable
Final Answer
Five examples of covalent bonds are hydrogen (H₂), water (H₂O), carbon dioxide (CO₂), methane (CH₄), and nitrogen gas (N₂).
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