What are some real-world examples of substances that exhibit ionic versus covalent bonding?
Answers:
Ionic and covalent bonding are two fundamental types of chemical bonds that occur between atoms. Here are some real-world examples of substances that exhibit each type of bonding:
Ionic Bonding
Ionic bonds typically form between metals and non-metals where electrons are transferred from one atom to another. The resulting ions are held together by electrostatic forces. Here are some examples:
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Sodium Chloride (NaCl): Common table salt is a classic example of an ionic compound. Sodium (Na) donates an electron to chlorine (Cl), forming Na⁺ and Cl⁻ ions, which attract each other.
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Magnesium Oxide (MgO): In this compound, magnesium (Mg) loses two electrons to become Mg²⁺, while oxygen (O) gains those electrons to form O²⁻, resulting in the formation of MgO.
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Calcium Fluoride (CaF₂): Calcium (Ca) loses two electrons to form Ca²⁺ ions, and each fluorine (F) atom gains one electron to become F⁻, resulting in the ionic compound CaF₂.
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Potassium Bromide (KBr): Potassium (K) donates one electron to bromine (Br), resulting in K⁺ and Br⁻ ions, which form the ionic compound KBr.
Covalent Bonding
Covalent bonds often form between non-metal atoms that share electrons to achieve stable electron configurations. Here are some examples:
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Water (H₂O): Each hydrogen (H) atom shares one electron with oxygen (O), leading to two covalent bonds in a water molecule.
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Carbon Dioxide (CO₂): In this molecule, carbon (C) forms two double covalent bonds with two oxygen atoms by sharing two pairs of electrons with each oxygen.
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Methane (CH₄): In methane, carbon shares four electrons with four hydrogen atoms, resulting in four single covalent bonds.
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Glucose (C₆H₁₂O₆): This simple sugar contains a complex structure of carbon, hydrogen, and oxygen atoms bonded together through covalent bonds.
Summary
- Ionic Compounds: Sodium chloride (NaCl), magnesium oxide (MgO), calcium fluoride (CaF₂), potassium bromide (KBr).
- Covalent Compounds: Water (H₂O), carbon dioxide (CO₂), methane (CH₄), glucose (C₆H₁₂O₆).
Understanding these examples provides insight into how different elements interact to form compounds with distinct properties.
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