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Understanding Chemical Formulas and Naming: Ionic and Covalent Bonds

This guide provides a comprehensive overview of chemical formulas, focusing on the octet rule and how atoms react to achieve a full outer shell through various bonding types. It explains ionic bonds and covalent bonds, including how to identify ions, write ionic formulas, and name ionic compounds according to specific rules. Learn the differences between cations and anions, the process of naming transition metal compounds, and how to handle polyatomic ions. Ideal for students and chemistry enthusiasts looking to reinforce their understanding of chemical nomenclature and bonding.

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Understanding Chemical Formulas and Naming: Ionic and Covalent Bonds

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  1. Chemical Formula and Naming

  2. Octet rule: atoms react to acquire a full outer shell: • Give away an e- to another atom. • Take an e- from another atom. • Share an e-with another atom. Ionic bond Covalent bond An ION is an atom that has lost or gained an electron. Lose e- – positive ion OR cation. (metals) Gain e- – negative ion OR anion. (nonmetals)

  3. Writing Rule 1: Write the symbol of the metallic element first. Beryllium combines with Chlorine + 2 - 1 Be Cl Rule 2: Place the combiningcapacityof one element as a subscript of the other element.

  4. Rule 3:Leave subscripts with a value of 1 out. Be Cl2 1 • Two Naming rules: • Write the full name of the metal ionfirst. • Name the non-metal iondropping the last • part of the name and adding the suffix “ide”. beryllium chlor ide

  5. Rule 4: Reduce the subscripts if possible. Magnesium combines with Sulfur + 2 - 2 Mg S MgS magnesium sulph ide

  6. Transition metals can give away different numbers of electrons. To avoid confusion: Brackets are used to show how many electrons the Transition metal is giving away.

  7. Iron (II) chloride Iron (III) chloride + 2 - + 3 - 1 1 Fe Cl Fe Cl FeCl2 FeCl3

  8. Write the name of the ionic compound: +4 -2 + - 1 Pb O PbO 2 lead oxide (IV)

  9. Covalent Compound: Contain two or more NON-METAL atoms. Formed by SHARING valence electrons to fill outer shell – octet rule. • A molecule is the smallest unit of a covalent compound. Non-metal + Non-metal = covalent bonding

  10. Step 1: firstnon-metal is named with a prefix to show the number of atoms. We do not use “mono” for the first non-metal. Step 2: secondnon-metal is named with a prefix AND with the “ide” ending. N O 2 4 nitrogen oxide di tetra dinitrogen tetroxide

  11. Writing formulas Step 1: Write the symbol of each element. Step 2: Use a subscriptto show the number of each type of atom given by the prefix. Do not reducecovalent formulas. di phosphorus oxide penta PO 2 5

  12. Polyatomic Ions (poly = many) Groups of covalently bonded atoms that act as ions. Polyatomic ions function as one unit with one charge – lose or gain electrons. DO NOT change the subscripts of polyatomic ions. Al(C2H3O2)3

  13. Write the name of the ionic compound: + - 1 Al C2H3O2 Al(C2H3O2) 3 aluminum acetate

  14. Ni(NO3)2 • magnesium sulfate • KMnO4 • iron (III) hydroxide • Ca(C2H3O2)2 • silver chromate • PbCO3 • tin (IV) sulfate • Na2HPO4 • ammonium nitrite nickel (II) nitrate MgSO4 potassium permanganate Fe(OH)3 calcium acetate Ag2CrO4 lead (II) carbonate Sn(SO4)2 sodium hydrogen phosphate NH4NO2

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