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Naming Chemicals

Naming Chemicals. Chapter 9. Naming and Writing Stuff. Ions Ionic Compounds Molecular Compounds Acids and Bases Formulas and Names. Monatomic Ions. Cations Anions –ide. Ions of Transition Metals I. Refer to the main 8 Groups we’ve seen as being in set Group A

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Naming Chemicals

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  1. Naming Chemicals Chapter 9

  2. Naming and Writing Stuff • Ions • Ionic Compounds • Molecular Compounds • Acids and Bases • Formulas and Names

  3. Monatomic Ions • Cations • Anions • –ide

  4. Ions of Transition Metals I • Refer to the main 8 Groups we’ve seen as being in set Group A • Refer to the other Groups as being in set Group B • If you look at your periodic tables, you should notice that labeling • These are the transition metals

  5. Ions of Transition Metals II • Many have multiple charges • Exception: • Silver Ag+ • Cadmium Cd2+ • Zinc Zn2+

  6. Ions of Transition Metals III • Roman numerals = valence e- • Go from low to high: (think Oh, I See - OIC) • –ous • –ic

  7. POLYATOMIC IONS • (More than one atom make up an ion) • ALL are negatively charged • EXCEPT ammonium NH4+ andHg22+ • Sometimes Hydrogen @ the beginning: • H+ ion present • Write as “Hydrogen Something” • E.g. Hydrogen Phosphate HPO42- • Go from low to high (“I ate”) • –ite • –ate

  8. Binary Ionic Compounds • An Ionic Compound with 2 components to it • Components can be 2 • Atoms • Molecules • 2 Essential Steps: • Write the CATION, then ANION (go +  -) • Balance the charges

  9. Compounds with Polyatomic Ions • Same process as with binary ionic compounds

  10. Molecular Compounds • Look at the prefix to tell you how many atoms of that element are in each molecule. • N2O – dinitrogenmonoxide • CO – carbonmonoxide • If the first atom is only 1, leave off the mono-

  11. ACIDS & BASES Ia • Normally, you have a compound that gets dissolved in water. • These can even be gasses • To indicate they are dissolved in water, we will note them as (aq) • (aq) is the abbreviation for aqueous

  12. ACIDS & BASES Ib • Water dissolves itself and splits up into H+ and (OH-) • Nonmetals are usually anions (-), so they would want to be near a positively charged H+ • Since we write the cation first, acids will begin with H • Metals are usually cations (+), so they would want to be near a negatively charged (OH-) • Since we write the anion last, bases will end with OH • So, in general, a nonmetal dissolved in water will form an acid • A metal dissolved in water will form a base

  13. ACIDS & BASES – Acids 1 • When the anion ends in –ide • Front of name gets: hydro- • End of name gets: –ic • Add: acid • HCl • hydrogen chloride (aq)  Hydrochloricacid

  14. ACIDS & BASES – Acids 2 • If anion ends in –ite • Front drops hydrogen • End gets –ous • Add: acid • H2SO3 • hydrogen sulfite (aq) sulfurousacid • If anion ends in –ate • Front drops hydrogen • End gets –ic • Add: acid • HNO3 • hydrogen nitrate (aq): nitricacid • Very similar to –ide, but no hydro-

  15. ACIDS & BASES – Bases • BASES • End in Hydroxide (OH) • NaOH – Sodium Hydroxide

  16. Last note… see pages 262, 277-278… • Remember to flip the charges with the number of atoms to balance compounds. • Example: Fe3+O2- • Flip: Fe2O3 • Charges: (3+)*2 + (2-)*3 = +6 + -6 = 0 • Remember there is a very handy flowchart on pages 277-278 to help name chemicals given their formulas and vice-versa

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