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FORMULAS AND EQUATIONS

FORMULAS AND EQUATIONS. Topic 2 in Review Book Page 26 HW Page 30 Q 1 to 13. FORMULAS. Qualitative information : what elements make up a compound. H 2 SO 4 (H,S,O) Quantitative information : ratio in which atoms of different elements are combined 2:1:4

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FORMULAS AND EQUATIONS

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  1. FORMULAS AND EQUATIONS • Topic 2 in Review Book Page 26 • HW Page 30 Q 1 to 13

  2. FORMULAS • Qualitative information: what elements make up a compound. H2SO4 (H,S,O) • Quantitative information: ratio in which atoms of different elements are combined • 2:1:4 • Remember in the symbol of an element the first letter is capital, the second lower case. • CO is a compound • Co is an element

  3. TYPES OF FORMULAS • Empirical Formula • Simplest ratio possible between the atoms in the formula • Molecular Formula • For covalently bonded compounds. It shows the ratio in which the atoms are actually combined in a compound. • Structural Formula • It shows the bonds between the atoms. • Formula Unit • For ionic compounds. • Always empirical.

  4. OXIDATION NUMBERS OR OXIDATION STATES (ON) • The charge or partial charge assigned to an atom in a compound. In the periodic table SELECTED OXIDATION STATES are indicated. • The addition of the ON in a compound is ALWAYS ZERO!!! COMPOUNDS HAVE NO CHARGE!!!

  5. THE NUMBERS IN A FORMULA • SUBSCRIPTS • Are used to indicate the ratio of the atoms in a formula. • COEFFICIENT Is written in FRONT of the formula. It is applied to the entire formula. Tell us how many units of the formula are present. • Polyatomic Ions • Group of atoms joined by covalent bonds that have a charge. Table E

  6. TYPE OF COMPOUNDS • Binary: 2 elements in the compound • Ending IDE * exceptions • OH-( Hydroxides) • Ternary: 3 elements in the compound • Quaternary: 4 elements in the compound

  7. NOMENCLATURE • How to name compounds. • Rules for formula writing • IUPAC (International Union of Pure and Applied Chemistry). • Is the organization that dictates all the rules for naming chemicals.

  8. Some rules that you need to learn • Binary compounds have an ide ending • *The less electronegative element goes always first (Metals – Non Metals) • *For elements with more than 1 Oxidation Number (ON) the Stock system indicates the ON in parenthesis in roman numerals. • For molecular compounds prefixes can be used to indicate number of atoms in the formula (non-IUPAC) • Carbon dioxide CO2.

  9. Common Prefixes

  10. Atomic Mass Unit ( AMU ) • is one-twelfth the mass of a carbon-12 atom. • Atomic Mass • The weighted average mass of the atoms in naturally occurring sample of the element.

  11. FORMULA MASS • The sum of the atomic masses of all the atoms in a formula. (for ionic compounds) • MOLECULAR MASS • (for molecular compounds) • The unit for them is amu.

  12. Gram formula mass GFM The formula mass in grams. The mass of one mole of formulas or molecules. For ionic substances GRAM MOLECULAR MASS The molecular mass in grams. The mass of one mole of molecules. For substances containing covalent bonds

  13. Percent Composition • Represents the composition as a percentage of each element compared with the total mass of the compound.

  14. Hydrates • A crystal that contains water molecules attach to it in a fixed ratio. • Water of hydration: the water in the hydrate • Anhydrous: The crystal that lost the water of hydration.

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