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General Chemistry, 5 th ed. Whitten, Davis & Peck

General Chemistry, 5 th ed. Whitten, Davis & Peck. Chapter 4 Definitions Left click your mouse to continue. DIRECTIONS. This slide show presentation is designed to function like flash cards. To check your answer, and/or to move on to the next slide, simply left click your mouse. BASE.

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General Chemistry, 5 th ed. Whitten, Davis & Peck

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  1. General Chemistry, 5th ed.Whitten, Davis & Peck Chapter 4 Definitions Left click your mouse to continue. Created by Tara L. Moore, MGCCC

  2. DIRECTIONS • This slide show presentation is designed to function like flash cards. • To check your answer, and/or to move on to the next slide, simply left click your mouse. Created by Tara L. Moore, MGCCC

  3. BASE • A substance that produces OH- ions in aqueous solution. • Strong soluble bases are soluble in water and are completely dissociated. • Weak bases ionize only slightly. Created by Tara L. Moore, MGCCC

  4. BINARY ACID A binary compound in which H is bonded to one of the less metallic nonmetals. Created by Tara L. Moore, MGCCC

  5. BINARY COMPOUND A compound consisting if two elements; may be ionic or molecular. Created by Tara L. Moore, MGCCC

  6. CHEMICAL PERIODICITY The variation in properties of elements with their positions in the periodic table. Created by Tara L. Moore, MGCCC

  7. COMBUSTION REACTION A highly exothermic reaction (release heat) of a substance with oxygen, usually with a visible flame. Created by Tara L. Moore, MGCCC

  8. DISPLACEMENT REACTION A reaction in which one element displaces another from a compound. Created by Tara L. Moore, MGCCC

  9. DISPROPORTIONATION REACTION A redox reaction in which the oxidizing agent and the reducing agent are the same element. Created by Tara L. Moore, MGCCC

  10. DISSOCIATION In aqueous solution, the process in which a solid ionic compound separates into its ions. Created by Tara L. Moore, MGCCC

  11. ELECTROLYTE • A substance whose aqueous solutions conduct electricity. • Remember: ions are charged particles. Movement of charged particles conducts electricity. • Ionic compounds are electrolytes Created by Tara L. Moore, MGCCC

  12. FORMULA UNIT EQUATION An equation for a chemical reaction in which all formulas are written as complete formulas. Created by Tara L. Moore, MGCCC

  13. GROUP (FAMILY) • The elements in a vertical column of the periodic table. • Elements in a group have similar chemical and physical properties Created by Tara L. Moore, MGCCC

  14. IONIZATION In aqueous solutions, the process in which molecular compound separates to form ions. Created by Tara L. Moore, MGCCC

  15. METALLOIDS • Elements with properties intermediate between metal and nonmetals • B, Si, Ge, As, Sb, Te, Po, and At Created by Tara L. Moore, MGCCC

  16. NET IONIC EQUATION • An equation that results from canceling spectator ions and eliminating brackets from a total ionic equation • The net ionic equation for ALL reactions of strong acids with strong soluble bases that form salts and water is H+ + OH- H2O Created by Tara L. Moore, MGCCC

  17. NEUTRALIZATION The reaction of an acid with a base to form a salt. Created by Tara L. Moore, MGCCC

  18. NONELECTROLYTE • A substance whose aqueous solutions do not conduct electricity. • Molecular compounds are nonelectrolytes Created by Tara L. Moore, MGCCC

  19. OXIDATION • Loss of electrons • Gain oxygen • Loss of hydrogen • An algebraic increase in oxidation number • Remember: electrons are negative, therefore if you are losing electrons, you oxidation number will change in the positive direction • If the item is being oxidized, then it serves as the reducing agent Created by Tara L. Moore, MGCCC

  20. OXIDATION NUMBERS Arbitrary numbers that can be used as mechanical aids in writing formulas and balancing equations Created by Tara L. Moore, MGCCC

  21. OXIDATION-REDUCTION REACTION A reaction in which oxidation and reduction occur; also called redox reactions Created by Tara L. Moore, MGCCC

  22. PERIOD • The element in a horizontal row of the periodic table • Elements in a period have properties that change progressively across the table Created by Tara L. Moore, MGCCC

  23. PERIODICITY Regular periodic variations of properties of elements with atomic number (and position in the periodic table) Created by Tara L. Moore, MGCCC

  24. PERIODIC LAW The properties of the elements are periodic functions of their atomic numbers. Created by Tara L. Moore, MGCCC

  25. PRECIPITATE An insoluble solid that forms and separates from a solution. Created by Tara L. Moore, MGCCC

  26. PSEUDOBINARY IONIC COMPOUND A compound that contains more than two elements but is named like a binary compound. Created by Tara L. Moore, MGCCC

  27. REDUCTION • Gain of electrons • Loss of oxygen • Gain of hydrogen • An algebraic decrease in oxidation number • Remember: electrons are negative, so if you are gaining electrons, the oxidation number will be in the negative direction • if an item is being reduced, then it serves as the oxidizing agent. Created by Tara L. Moore, MGCCC

  28. REVERSIBLE REACTION A reaction that occurs in both directions; indicated by double arrows Created by Tara L. Moore, MGCCC

  29. SALT A compound that contains a cation other than H+ and an anion other than OH- or O-2 Created by Tara L. Moore, MGCCC

  30. SEMICONDUCTOR A substance that does not conduct electricity at low temperatures, but does so at higher temperatures. Created by Tara L. Moore, MGCCC

  31. SPECTATOR IONS • Ions in solution that do not participate in a chemical reaction • When looking at a total ionic equation, the spectator ions are the ones whose oxidation state does not change • Are not shown in a net ionic equation Created by Tara L. Moore, MGCCC

  32. STRONG ACID • An acid that ionizes (separates into ions) completely, or very nearly completely, in dilute aqueous solutions • EX: H2SO4, HNO3, HCl, HClO3, HClO4, HI, HBR Created by Tara L. Moore, MGCCC

  33. STRONG ELECTROLYTE • A substance that conducts electricity well in dilute aqueous solution. • Three major classes of solutes are strong electrolytes: strong acids, strong soluble bases and most soluble salts Created by Tara L. Moore, MGCCC

  34. STRONG SOLUBLE BASE • Metal hydroxide that is soluble in water and dissociates completely in dilute aqueous solution • EX: LiOH, NaOH, KOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2 Created by Tara L. Moore, MGCCC

  35. TERNARY ACID A ternary compound containing H, O, and another element, often a nonmetal Created by Tara L. Moore, MGCCC

  36. TOTAL ION EQUATION An equation for a chemical reaction written to show the predominant form of all species in aqueous solution or in contact with water. Created by Tara L. Moore, MGCCC

  37. WEAK ACID • An acid that ionizes only slightly in dilute aqueous solution • EX: HF, HC2H3O2, HCN, HNO2, H2CO3, H3PO4, H2SO3, (COOH)2 Created by Tara L. Moore, MGCCC

  38. WEAK BASE • A molecular substance that ionizes only slightly in water to produce an alkaline (base) solution • EX: NH3, CH3NH2, C6H5NH2 Created by Tara L. Moore, MGCCC

  39. WEAK ELECTROLYTE A substance that conducts electricity poorly in dilute aqueous solution. Created by Tara L. Moore, MGCCC

  40. METALS • Outer shells contain few electrons, usually three or four • Form cations (positive ions) by losing electrons • Form ionic compounds with nonmetals • Solid state characterized by metallic bonding Created by Tara L. Moore, MGCCC

  41. NONMETALS • Outer shells contain four or more electrons • Form anions (negative ions) by gaining electrons • Form ionic compounds with metals and molecular (covalent) compounds with other nonmetals • Covalently bonded molecules; noble gases are monatomic Created by Tara L. Moore, MGCCC

  42. METALLIC CHARACTER Increases from top to bottom and from right to left with respect to position in the periodic table Created by Tara L. Moore, MGCCC

  43. NONMETALLIC CHARACTER Increases from bottom to top and from left to right in the periodic table Created by Tara L. Moore, MGCCC

  44. HALOGENS • Will displace less active (heavier) halogens from their binary slats • Order of increasing activity: I2 < Br2< Cl2< F2 Created by Tara L. Moore, MGCCC

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