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How Do We Make Compounds?

How Do We Make Compounds?. Why do atoms bond?. Octet Rule : Every atom wants 8 electrons to fill the valence shell (outer most shell) Ion : Charged atom (Ca +2 ) Polyatomic Ion : Two or more atoms bonded together to form an ion (SO 4 -2 ). What are Ionic, Covalent and Metallic Bonds?.

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How Do We Make Compounds?

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  1. How Do We Make Compounds?

  2. Why do atoms bond? • Octet Rule: Every atom wants 8 electrons to fill the valence shell (outer most shell) • Ion: Charged atom (Ca+2) • Polyatomic Ion: Two or more atoms bonded together to form an ion (SO4-2)

  3. What are Ionic, Covalent and Metallic Bonds? • Ionic Bond: An electron is transferred from one element to another (metal to nonmetal) • Covalent Bond: Electrons are shared (nonmetal to nonmetal) • Metallic Bond: Sea of electrons (Metal to Metal)

  4. Name the first element Keep the root of the 2nd element, drop the ending & add “ide” Now add the prefixes The first element does not need the prefix mono Prefixes: Mono (1) Di (2) Tri (3) Tetra (4) Penta (5) Hexa (6) Hepta (7) Octa (8) Nona (9) Deca (10) Name CO2 Name CCl4 How Do We Name Molecular (covalent) Molecules?

  5. How Do We Name Ionic Compounds? • Name the first element. Use the root of 2nd element and add “ide” (no prefixes) • If there is a transition metal, determine the charge and add Roman Numerals • If there is a polyatomic ion, name the first element and name the polyatomic ion. • Name: CaCl2, FeO, NaOH

  6. How Do We Determine Empirical & Molecular Formulas? • Empirical Formula: Chemical Formula that shows the relative numbers and kinds of atoms in the simplest ratio (CH2O) • Molecular Formula: Chemical formula that shows the actual number and kinds of atoms (C6H12O6) • Structural Formula: Formula that shows the location of the atoms relative to one another

  7. Empirical Formula: • Given a percent → Change to Mass • Change Mass to Moles • Determine the Ratio • Molecular Formula: • Same as above, then determine molar mass of empirical formula • Divide given mass/empirical mass • Multiply empirical formula by that number

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