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Chapter 5 Section 3 Polyatomic Ions and Naming Compounds.

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Presentation on theme: "Chapter 5 Section 3 Polyatomic Ions and Naming Compounds."— Presentation transcript:

1 Chapter 5 Section 3 Polyatomic Ions and Naming Compounds

2 Formulas for Ionic Compounds To write formulas for compounds you must remember that the molecule must be neutral. 1)Hydrogen (H +1 )oxidation # is +1 and Oxygen (O -2 )is -2 2) you need 2 (+1) to cancel out the – 2 3)So 2 Hydrogens are needed to match every Oxygen. (H 2 O) Criss-Cross Method

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4 Polyatomic Ions Ions – elements that have lost/gained electrons Anions – ions have gained electrons & are negative(-) (+)Ca (+) ion-ions that have lost electrons and are positive (+) Polyatomic ions- multiple atoms hooked together that have +/- electrons

5 Polyatomic Ion Con’t Polyatomic ions are covalently bonded atoms that have either too many electrons between them or not enough and are placed in parentheses to show their charges. (OH) - =Hydroxide, (NH 4 ) + =Ammonium are some examples Subscripts tell # of atoms Superscripts tell # of electrons gained/lost

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8 Naming Ionic Compounds Compounds are between Metals & Nonmetals. Metals are always listed 1 st & retain their name Non-metals are always listed 2 nd & their ending is changed to “ide” Sodium (metal)+ chlorine (nonmetal)= sodium chloride

9 Naming Covalent Compounds Use Numerical prefixes To: 1) show how many atoms of the first nonmetals there are in the compound 2) on the second non metal to show how many atoms there are, and change ending to -ide. ideN 2 O 4 = dinitrogen tetraoxide

10 TEST NO Ch. 5 TEST FRIDAY!!!

11 TEST Semester Final Thursday-19 th (1 st, 3 rd, 5 th ) Friday-20 th (2 nd, 4 th, 6 th )


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