IPC Final Exam Review

Multiple Choice Questions

1. Substances Composition

   • All substances are built from atoms (d).

2. Elements on Earth

   • About 90 elements are found on Earth (b).

3. Homogeneous Mixture

   • A solution is a homogeneous mixture of small particles (a).

4. Settling Mixture

   • A mixture that settles upon standing is a suspension (c).

5. Light Scattering Mixture

   • A solution does not scatter light (a).

6. Material Characteristics

   • A physical property can be observed without changing the substance identity (a).

7. Change in Matter

   • A change in size, shape, or state of matter is a physical change (a).

8. Separation Process

   • Distillation separates substances by evaporating and recondensing (d).

9. Homogeneity in Mixtures

   • A suspension is not homogeneous (a).

10. Scattering of Light

    • The Tyndall effect describes the scattering of light by colloids (a).

11. Example of Colloid

    • Smoke is a colloid (c).

12. Physical Changes

    • Examples: boiling water, bursting balloon, melting candle (b).

13. Color of Ink

    • The color of ink is a physical property (b).

14. Combining Substances

    • Combined substances retaining properties form a mixture (d).

15. Homogeneous Mixture Name

    • Another name for a homogeneous mixture is a solution (c).

16. Gasoline Reaction

    • When gasoline is burned, new substances are formed (b).

17. Matter Composition

    • An element is matter composed of one type of atom (c).

18. Smallest Element Unit

    • An atom is the smallest piece retaining element properties (a).

19. Atomic Nucleus Charge

    • The nucleus is positively charged (a).

20. Neutron Charge

    • Neutrons have no charge (d).

21. Electron Charge

    • Electrons have a negative charge (b).

22. Atom Energy Levels

    • Each energy level holds a maximum number of electrons (d).

23. Dot Diagrams

    • Dot diagrams represent outer electrons (d).

24. Particles of Matter

    • Quarks make up protons and neutrons (d).

25. Proton Charge

    • Protons have a positive charge (a).

26. Chemical Symbol

    • A chemical symbol represents the name of an element (a).

27. Periodic Table Rows

    • Horizontal rows are called periods (d).

28. Element Isotopes

    • Atoms with different neutrons are isotopes (d).

29. Transition Elements

    • Elements in groups 3-12 are transition elements (b).

30. Mass Number Calculation

    • Atom with 26 protons, 26 electrons, and 30 neutrons has mass number 56 (d).

31. Liquid Metal

    • Mercury is the only liquid metal at room temperature (d).

32. Metal and Nonmetal Bonds

    • Metals lose electrons forming ionic bonds (a).

33. Metallic Bonding

    • Positively charged ions surrounded by electron cloud is metallic bonding (d).

34. Radioactive Element

    • An element whose nucleus breaks down, emitting particles is radioactive (d).

35. Transition Elements on Periodic Table

    • Groups 3-12 are known as transition elements (d).

36. Disconnected Periodic Table Rows

    • Two rows are the inner transition metals (d).

37. Carbon Allotrope

    • Graphite is a soft carbon allotrope used as a lubricant (d).

38. Solid to Gas Process

    • Sublimation describes solids changing directly to gas (c).

39. Hydrogen Reaction with Metals

    • Hydrogen gains one electron (b).

40. Different Element Forms

    • Allotropes are different forms with different properties (a).

41. Room Temperature Metals

    • Most metals are solids (b).

42. Hard Carbon Allotrope

    • Diamond is a hard carbon allotrope used in jewelry (b).

43. Wire Formation

    • Metals are ductile (a).

44. Alkaline Earth Metals

    • Group with two outer electrons is the alkaline earth metals (a).

45. Synthetic Elements

    • Found in the actinides group (a).

46. Hydrogen's Grouping

    • Grouped with alkali metals due to one electron in outer level (b).

47. Periodic Table Line Elements

    • Elements along stair-step line are metalloids (c).

48. Element Examples

    • Copper, sulfur, oxygen are elements (a).

49. Chemical Formula

    • Represents compound elements and atom count (a).

50. H2O

    • Known as water (d).

51. Chemical Bonds

    • A bond holds atoms together in a compound (a).

52. Charged Particles

    • A charged particle is an ion (c).

53. Shared Electron Bonds

    • Shared electron bonds are covalent bonds (b).

54. Compound Element Representation

    • Shown in a chemical formula (b).

55. Charged Atom Groups

    • A group acting as one charged atom is a polyatomic ion (a).

56. Chemical Formula Numbers

    • Atom count shown by subscripts (d).

57. Shared Electrons Bond

    • Atoms sharing electrons form a covalent bond (b).

58. Electron Exchange Name

    • Named as oxidation number (c).

59. Stable Atom Electrons

    • Most atoms need 8 electrons to be stable (d).

60. Neutral Compound Oxidation Sum

    • Always zero (b).

61. Noble Gases and Compounds

    • Do not form compounds; outer energy levels are filled (d).

62. NaCl

    • Known as sodium chloride (a).

63. Hydrogen in Ammonium Acetate

    • Contains 7 hydrogen atoms (c).

64. Oxidation Number Display

    • Shown with a superscript (c).

65. Homogeneous Mixture

    • Solution has the same composition throughout (b).

66. Cube Surface Area

    • Splitting increases surface area greater than original (a).

67. Dilute Solution

    • Contains a small amount of solute (b).

68. Polar Molecules

    • Have positive and negative areas (a).

69. Solubility

    • Maximum solute amount dissolved is solubility (a).

70. Saturated Solution

    • Contains all solute it can hold at temperature (d).

71. Solute in Solution

    • The solute is the substance being dissolved (a).

72. Gaseous Solution Example

    • Air is an example of a gaseous solution (a).

73. Soda Pop Solvent

    • The water is the solvent in soda pop (a).

74. Non-electrolyte Substance

    • Does not conduct electricity (b).

75. Crystal to Solution

    • Dissociation separates particles into solution (b).

76. Surface Area Impact

    • Increasing it increases dissolving speed (c).

77. Gas Solubility in Liquid

    • Faster if cooled (b).

78. Concentrated Solution Description

    • Described as concentrated (c).

79. Alloy Solution

    • An alloy is a solid solution (c).

80. Increasing Solute Dissolving

    • Stir the solution (a).

81. Universal Solvent

    • Water is small, polar, fits among solute molecules (b).

82. Chemical Reaction

    • A change converting substances into new ones (a).

83. Reactants

    • Substances that react are reactants (d).

84. Reaction Products

    • New substances are products (c).

85. Reactant Coefficients

    • Numbers to the left are coefficients (b).

86. Balanced Chemical Equation

    • Same number of each element's atoms on both sides (b).

87. Product in Equation

    • To the right of arrow is a product (d).

88. Reactant in Equation

    • On the left side of arrow is a reactant (a).

89. Balanced Equation Example

    • Example: AgNO3 + NaCl → AgCl + NaNO3 (c).

90. Conservation of Mass Law

    • Mass of products equals mass of reactants (d).

Matching Questions

Charges

• 91. Proton: a
• 92. Neutron: c
• 93. Electron: b

Descriptions

• 94. Nucleus: b
• 95. Negative Ion: d
• 96. Ionic Bond: e
• 97. Element Symbol: i
• 98. Neutral Particle: k
• 99. Compound: h
• 100. Polar Molecule: g
• 101. Formula Combination: j
• 102. Number of Atoms: l
• 103. Positive Ion: c
• 104. Electron: a
• 105. Covalent Bond: f

Properties

• 106. Lustrous: a
• 107. Malleable: b
• 108. Ductile: c

Solutions

• 109. Solute: b
• 110. Solvent: a
• 111. Solution: c
• 112. Unsaturated: d
• 113. Saturated: f
• 114. Supersaturated: e

Acids and Bases

115. Coffee pH - Coffee is a weak acid (c).

116. Compound in Solution - Compound formed from negative and positive ions is a salt (c).

117. Solution Clues - Bitter taste, slippery feel indicates a base (b).

118. Weak Base Example - Ammonia produces only a few ions (c).

119. H+ Producer - Substance that produces H+ in solution is an acid (a).

120. Solution Strength - Refers to ease of ion formation (d).

121. pH Measurement - Measures acidity or basicity (c).

122. Color Change Indicators - Change color in presence of acid/base (d).

123. Acid Physical Property - Sour taste is a physical property (c).

124. Neutralization Reaction - Acid and base produce salt and water (b).

125. OH– Producer - Produces OH– in solution is a base (b).

126. pH Measurement - Measures concentration of hydronium ions (d).

127. Weak Base - Base that partly ionizes (d).

128. H3O+ Units - Known as hydronium ions (b).

129. Concentration Process - Using known concentration solution to find another is titration (d).

130. Acidic Solution pH - pH less than 7 (a).

131. pH Scale Range - Defines acidity on scale of 0-14 (b).

132. Basic Solution Ions - Contains more hydroxide ions (c).

133. Titration Standards - Solution with known concentration is standard solution (d).

134. Neutral Solution - Contains equal hydrogen and hydroxide is neutral (c).

These notes cover an extensive review for an IPC final exam, focusing on key concepts from atomic structure and periodic table to chemical reactions, solutions, acids, and bases.