Ionic and Covalent Bonding
Compare how metals and non-metals form ionic and covalent bonds.
Atoms bond to gain a stable outer electron shell.
- Explain electron transfer and sharing.
- Describe properties of ionic and covalent compounds.
- Predict the type of bond from element types.
Ionic Bonding
A metal atom loses electrons to become a positive ion; a non-metal gains them to become a negative ion. Opposite ions attract strongly. Example: sodium loses one electron to chlorine, forming Na⁺Cl⁻.
Covalent Bonding
Two non-metals share electrons. A hydrogen molecule (H₂) shares one pair; water (H₂O) has two O–H covalent bonds; carbon dioxide has double bonds.
Properties
- Ionic — high melting points, dissolve in water, conduct when molten or dissolved.
- Covalent (simple molecular) — low melting points, often do not conduct electricity.
Magnesium (metal) + oxygen (non-metal) → ionic bond, MgO.
Carbon (non-metal) + oxygen (non-metal) → covalent bond, CO₂.
Practice
- Explain how sodium and chlorine form ions.
- Predict whether each pair forms an ionic or covalent bond: K and Cl; N and O; Ca and O.
- Give two properties of ionic compounds.
Recap
Ionic bonds transfer electrons between metals and non-metals. Covalent bonds share electrons between non-metals.
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Atomic Structure and Bonding
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