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Comprehensive Guide to Naming Transition Metals and Polyatomic Compounds

This guide outlines the essential rules for naming ionic compounds, particularly focusing on transition metals and polyatomic ions. For basic ionics, remember to name the metal first, change the non-metal's ending to "ide", and use the criss-cross method for formulas. Transition metals may have multiple charges, indicated by Roman numerals. Polyatomic ions are composed of multiple atoms, maintaining specific names. Examples are provided for clarity in both naming and formula creation, including Barium sulfate and Copper(II) chloride.

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Comprehensive Guide to Naming Transition Metals and Polyatomic Compounds

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  1. Unit 1 – Day 5 Naming Transition Metal and Polyatomic Compounds

  2. Naming Basic Ionics Review • When naming a compound: • List the metal first, and the non-metal second. • Change the non-metal’s ending to “ide” • To give a formula from a name: • Write symbols for both elements • Write their charges above • Criss-cross the charges down as subscripts • Reduce if necessary.

  3. Examples: • Name us: • BeF2 • ZnCl2 • Give formula: • Sodium nitride • Magnesium sulfide • Aluminum iodide

  4. Transition Metals • These are the metals that do not fall under groups 1 through 8. • Examples: Copper, Iron, Gold, Nickel, Zinc • Charges need to be found on the back of your periodic table. • Some of these metals can have more than one charge, so we indicate it with roman numerals

  5. Roman Numerals • I (one) • II (two) • III (three) • IV (four) • V (five) • VI (six)

  6. Naming with Transition Metals • You will need to learn and recognize the six metals with multiple charges. They are listed on the back of your periodic table. • Au, Pb, Cu, Sn, Hg, Fe • When naming, you will need to determine the charge of the metal in order to name it.

  7. Naming with Transition Metals • Examples: • SnF2 • CuO • PbS2

  8. Giving Formulas with Transition Metals • The criss cross method is used. • The roman numeral gives the charge (NOT the number of atoms). • Examples: • Copper (II) chloride • Mercury (I) nitride • Lead (IV) carbide

  9. Polyatomic Ions • Some ions are made up of more than one type of atom. • Examples: • sulfate (SO4)-2, nitrate (NO3)-1, hydroxide (OH)-1 • They behave exactly like all other ions in bonding.

  10. Naming with polyatomics • With polyatomic ions, they already have their ending (ide or ate) so this will not change. • Ions need to be looked up on the back of the table. • Examples: • NaNO3 • Be(OH)2

  11. Giving Formulas of Polyatomics • Look up the formula and charge of a polyatomic ion. • The charge can be used to criss cross. • If you have multiple ions, you need to use brackets to show this. • Example: Al(ClO3)3 (means 3 chlorate ions)

  12. Examples • Barium sulfate • Ammonium hydroxide • Zinc bromate • Iron (III) phosphate

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