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Understanding Ionic and Molecular Compounds: Nomenclature and Lewis Structures

This comprehensive review focuses on ionic and molecular compounds, exploring key aspects such as the formation of cations and anions, electron exchange, and the distinction between ionic and molecular bonding. Additionally, it covers nomenclature for binary compounds, including the use of prefixes and changes in element names. The review also introduces acid nomenclature, highlighting how to name acids based on their anions. Finally, it discusses Lewis dot structures, illustrating how to represent and predict molecular shapes using valence electrons.

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Understanding Ionic and Molecular Compounds: Nomenclature and Lewis Structures

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  1. Unit 6 Notes – Chapters 4 & 12 Mr Nelson 2009

  2. Ionic Compounds – Review • Made up of ions • Cations (+) & Anions (-) • Metals & Nonmetals (or polyatomic ions) • Exchange of electrons • Charges Balance

  3. Molecular Compounds – Intro • No ions • Charges will not balance • Composed of two nonmetals • Sharing of electrons • Covalent bonding • Naming is based on prefixes

  4. Nomenclature of Binary Compounds • If both elements are nonmetals we must use prefixes. • The 1st element only gets a prefix if it is greater than 1. • 2nd element always gets a prefix and change the ending to -ide

  5. Nomenclature of Binary Compounds • Example of a molecular comp: • CO2 • CO • CCl4

  6. Nomenclature of Binary Compounds • If the prefix ends with a or o and the name of the element begins with a vowel, the two successive vowels are combined into one. N2O5: dinitrogen pentoxide

  7. Practice • PCl5 dihydrogen monoxide • SF6 carbon trichloride • N2O disulfur hexoxide • NO2 nitrogen triiodide

  8. Naming Acids • An acid is any compound that starts with a hydrogen • When naming an acid: • 1st locate the anion (- charge)

  9. Acid Nomenclature • If the anion in the acid ends in -ide, change the ending to -icacid and add the prefix hydro- . • HCl: hydrochloric acid • HBr: hydrobromic acid

  10. Acid Nomenclature • If the anion in the acid ends in -ite, change the ending to -ousacid. • HClO: hypochlorous acid • HClO2: chlorous acid

  11. Acid Nomenclature • If the anion in the acid ends in -ate, change the ending to -icacid. • HClO3: chloric acid • HClO4: perchloric acid

  12. Warm Up • HBr Chlorous Acid • FeS Copper(I) fluoride • PBr5 dinitrogen dioxide • KSO4 nitrogen monoxide • CCl4 hydroiodic acid • HNO3 potassium nitrate • LiCl phosphoric acid

  13. Lewis Dot Structures • ONLY Valence (outer) electrons are involved. • You can do Lewis dot structures for atoms and for compounds • Lewis dot structures tell you the structure of a molecule of a compound, help predict shape.

  14. Lewis Dot Structure Example • Example: Bromine • Number of valence electrons _____

  15. Find the sum of valence electrons of all atoms in the polyatomic ion or molecule. PCl3 Steps to Writing Lewis Structures 5 + 3(7) = 26

  16. Writing Lewis Structures • Arrange element symbols to show how atoms are connected – show electrons as dots. • Draw in the valence electrons of each of the atoms Keep track of the electrons:

  17. Writing Lewis Structures • Connect the lines to form single bonds. • 1 line = 2 electrons Keep track of the electrons:

  18. Writing Lewis Structures • Finish by checking for octets. • Hydrogen only needs 2 electrons to be happy Keep track of the electrons:

  19. Writing Lewis Structures • If the central atom does not have an octet… …form multiple bonds until it does. Example: HCN

  20. Exceptions! • Boron and Aluminum are okay with only 6 valence electrons around it • BF3

  21. Exceptions • If the Lewis Dot Structure you are drawing is an ion: • Use [] and specify the charge • Add or subtract electrons • Positive charges take away electrons • Negative charges add electrons • Example: Br-

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