IPC Final Exam Study Guide

Name: Class: Date: IPC Final Exam Review Indicate the answer choice that best completes the statement or answers the question. 1. All substances are built from__________. a. compound b. oxygen c. metals d. atoms 2. About ______ elements are found on Earth. a. 9 b. 90 c. 900 d. 9000 3. A(n) ______ is a homogeneous mixture of particles so small they cannot be seen without microscopes and will never settle to the bottom of their container. a. solution b. element c. molecule d. plasma 4. A(n) ______ is a mixture that settles upon standing. a. solution b. colloid c. suspension d. element 5. A(n) ______ is a mixture that does not scatter light. a. solution b. colloid c. suspension d. element 6. Any characteristic of a material that you can observe without changing the identity of the substances that make the material is a(n) ______. a. physical property b. chemical property c. invisible property d. none of these 7. A change in size, shape, or state of matter is called a(n) ______ change. a. physical b. chemical c. atomic d. impossible 8. The process for separating substances in a mixture by evaporating a liquid and recondensing its vapor is called ______. a. precipitation b. sifting c. distribution d. distillation 9. A(n) ______ is not homogeneous. a. suspension b. element c. compound d. solution 10. The scattering of light by colloids is called ______. a. the Tyndall effect b. conservation c. air pollution d. suspension 11. Smoke is an example of a ______. a. substance b. solution c. colloid d. suspension 12. Three examples of physical changes are ______. a. freezing of water, evaporation of gasoline, and rusting of a nail b. boiling of water, bursting of a balloon, and melting of a candle c. sawing of wood, crushing of a can, and toasting a marshmallow d. burning of gasoline, rotting of an egg, and exploding of fireworks 13. The color of ink is a ______. a. chemical property b. physical property c. chemical change d. physical change 14. When two or more substances are combined so that each substance maintains its own properties, the result is a(n) ______. a. chemical change b. element c. compound d. mixture 15. ______ is another name for a homogeneous mixture. a. Suspension b. Substance c. Solution d. Liquid 16. When gasoline is burned in an engine, ______. a. gasoline evaporates b. new substances are formed c. mass is lost d. mass is gained 17. A(n) ______ is matter that is composed of one type of atom. a. compound b. mixture c. element d. molecule 18. The smallest piece of an element that still retains the properties of the element is a(n) ______. a. atom b. molecule c. compound d. plasma 19. The nucleus of an atom is ______ charged. a. positively b. negatively c. variably d. none of these 20. Neutrons have ______ charge. a. positive b. negative c. variable d. no 21. Electrons have ______ charge. a. positive b. negative c. variable d. no 22. Each energy level of an atom has a maximum number of ______ it can hold. a. neutrons b. quarks c. protons d. electrons 23. Dot diagrams are used to represent ______. a. the structure of the nucleus b. atomic number c. isotopes d. outer electrons 24. Particles of matter that make up protons and neutrons are ______. a. electrons b. isotopes c. atoms d. quarks 25. Protons have ______ charge. a. positive b. negative c. variable d. no 26. A chemical symbol represents the ______of an element. a. name b. structure c. reaction d. type 27. Horizontal rows of the periodic table are called ______. a. groups b. families c. clusters d. periods 28. Atoms of the same element with different numbers of neutrons are called ______. a. metalloids b. radioactive c. transition elements d. isotopes 29. Elements in groups 3 through 12 are called ______. a. metalloids b. transition elements c. noble gases d. isotopes 30. A certain atom has 26 protons, 26 electrons, and 30 neutrons. Its mass number is ______. a. 26 b. 30 c. 52 d. 56 31. _____ is the only metal that is not solid at room temperature. a. Steel b. Aluminum c. Copper d. Mercury 32. When metals combine with nonmetals, the atoms of the metals tend to lose electrons, forming _____ bonds. a. ionic b. covalent c. triple d. unbreakable 33. In _____ bonding, positively charged metallic ions are surrounded by a cloud of electrons. a. ionic b. covalent c. triple d. metallic 34. A(n) _____ element is one in which the nucleus breaks down and gives off particles and energy. a. stable b. gaseous c. metallic d. radioactive 35. Elements in Groups 3 through 12 on the periodic table are known as _____ elements. a. gaseous b. noble c. radioactive d. transition 36. The two rows of elements that seem to be disconnected from the rest of the periodic table are the _____. a. nonmetals b. halogens c. noble gases d. inner transition metals 37. An allotrope of carbon that is soft and can be used as a lubricant is _____. a. silicon b. diamond c. sand d. graphite 38. The process by which a solid changes directly to a gas without first becoming a liquid is called _____. a. condensation b. ionization c. sublimation d. evaporation 39. When hydrogen reacts with active metals, it _____. a. shares electrons b. gains on electron c. loses one electron d. loses two electron 40. Different forms of the same element that have different properties because of different atom arrangements are called _____. a. allotropes b. carbons c. silicons d. graphites 41. At room temperature, most metals are _____. a. liquids b. solids c. radioactive d. gases 42. An allotrope of carbon that is hard and is often used in jewelry is ______. a. silver b. diamond c. quartz d. graphite 43. Metals can be used as wire because they are _____. a. ductile b. malleable c. shinny d. alloys 44. A group of elements that have two electrons in its outer energy level is the ______. a. alkaline earth metals b. halogens c. alkali metals d. actinides 45. Synthetic elements are found in which of the following groups? a. actinides b. alkali metals c. oxides d. halogens 46. Hydrogen is grouped with the alkali metals because it _____. a. is a metal b. has one electron in its outer energy level c. it is a gas d. does not readily form compounds 47. Elements that lie along the stair-step line of the periodic table are _____. a. liquids b. metals c. metalloids d. radioactive 48. Copper, sulfur, and oxygen are examples of ______. a. elements b. compounds c. mixtures d. colloids 49. A chemical ______ tells what elements a compound contains and the exact number of the atoms of each element in a unit of that compound. a. formula b. table c. dot diagram d. chart 50. H2O is also known as ______. a. carbon b. mercury c. nickel d. water 51. A chemical ______ is the force that holds atoms together in a compound. a. bond b. element c. compound d. formula 52. A charged particle is known as a(n) ______. a. plasma b. gas c. ion d. neutron 53. The attraction that forms between atoms when they share electrons is known as a(n) ______ bond. a. ionic b. covalent c. simple d. net 54. The elements that make up a compound and the number of atoms of each element in a unit of the compound can be shown in a ______. a. chemical symbol b. chemical formula c. subscript d. subscript 55. A group of atoms that acts together as one charged atom is a ______. a. polyatomic ion b. negative ion c. molecule d. crystal 56. In chemical formulas, the number of atoms in a unit of the compound is shown by numbers called ______. a. oxidation numbers b. superscripts c. hydrates d. subscripts 57. A chemical bond that occurs when atoms share electrons is a(n) ______ bond. a. ionic b. covalent c. polyatomic d. magnetic 58. The name given to the number of electrons an atom gains, loses, or shares is the ______. a. ionic number b. atomic number c. oxidation number d. atomic mass 59. How many electrons are needed in the outer energy levels of most atoms for the atom to be chemically stable? a. 2 b. 4 c. 6 d. 8 60. The sum of the oxidation numbers in a neutral compound is always ______. a. one b. zero c. a positive number d. a negative number 61. Why do the noble gases not form compounds readily? a. They have no electrons. b. They have empty outer energy levels. c. They have seven electrons in their outer energy levels. d. Their outer energy levels are completely filled with electrons. 62. What is the name of the compound with the formula NaCl? a. sodium chloride b. chlorine sodiate c. sodium dichloride d. sodium chlorate 63. How many hydrogen atoms are present in one molecule of ammonium acetate, NH4C2H3O2? a. 3 b. 4 c. 7 d. 11 64. The oxidation number of an atom is shown with a ______. a. subscript b. positive number c. superscript d. negative number 65. A(n) _____ is a mixture that has the same composition, color, and density throughout. a. element b. solution c. mixture d. plasma 66. If a cube is split in half, the surface area of the pieces will be _____ that of the cube. a. greater than b. less than c. the same as d. none of these 67. A dilute solution has _____ of solute in the solvent. a. a large amount b. a small amount c. an unlimited amount d. none of these 68. _____ molecules have a positive area and a negative area. a. Polar b. Nonpolar c. Organic d. Gaseous 69. _____ is the maximum amount of a solute that can be dissolved in a given amount of solvent at a given temperature. a. Solubility b. Volume c. Density d. A solution 70. A solution that contains all the solute it can at a given temperature is called _____. a. filled b. calcified c. unsaturated d. saturated 71. In a solution, the substance that is being dissolved is the _____. a. solute b. solvent c. liquid d. gas 72. The air that you breathe is an example of a(n) _____ solution. a. gaseous b. solid c. liquid d. amalgam 73. In soda pop, the solvent would be the _____. a. water b. carbon dioxide c. sugar d. flavoring 74. A substance that does not conduct an electric current when it forms a solution is a(n) _____. a. electrolyte b. nonelectrolyte c. polar substance d. salt 75. The process by which the particles in a crystal are separated and drawn into solution by water is called _____. a. ionization b. dissociation c. polarity d. saturation 76. Increasing the surface area of a solid _____. a. slows the speed of dissolving b. has no effect on the speed of dissolving c. increases the speed of dissolving d. causes the solid to ionize 77. The solubility of a gas in a liquid occurs faster if the liquid is _____. a. heated b. cooled c. under low pressure d. an electrolyte 78. The concentration of a solution that contains a large amount of solute in the solvent could be described as _____. a. unsaturated b. polar c. concentrated d. dilute 79. An alloy is an example of a _____ solution. a. gaseous b. liquid c. solid d. dilute 80. Which of the following will speed up the dissolving of a solid solute in water? a. Stir the solution. b. Cool the solution. c. Grind up the solvent. d. Freeze the solute. 81. Water is sometimes referred to as the universal solvent because _____. a. it has no separated positive and negative areas b. it is a small molecule and can fit easily among the molecules of many solutes. c. it has a polar and a nonpolar end d. its molecules can slip easily among molecules of a nonpolar solvent 82. A(n) _____ reaction is a change in which one or more substances are converted into new substances. a. chemical b. physical c. state d. electrical 83. The substances that react are called _____. a. nuclear reactors b. elements c. compounds d. reactants 84. The new substances produced in a reaction are called _____. a. elements b. compounds c. products d. reactants 85. Numbers to the left of formulas for reactants are called _____. a. superscripts b. coefficients c. elements d. formulas 86. A(n) _____ chemical equation has the same number of atoms of each element on both sides. a. false b. balanced c. imbalanced d. physical 87. Each substance to the right of the arrow in a chemical equation is a ______. a. catalyst. b. precipitate. c. reactant. d. product. 88. Each substance on the left side of the arrow in a chemical equation is a ______. a. reactant. b. product. c. coefficient. d. catalyst. 89. An example of a balanced chemical equation is ______. a. AgNO3 + NaCl→.4AgCl + 2NaNO3 b. 2AgNO3 +2NaCl.→3AgCl + 2NaNO3. c. AgNO3 + NaCl→.AgCl+ NaNO3. d. AgNO3 + 2NaCl + AgCl→AgCl +3NaNO3. 90. According to the law of conservation of mass, how does the mass of the products in a chemical reaction compare with the mass of the reactants? a. The mass of the products is greater. b. The mass of the reactants is greater. c. There is no relationship. d. The masses are equal. Match each item with the correct term. a. positive charge b. negative charge c. no charge 91. proton 92. neutron 93. electron Match each term with the correct description below. a. electron b. nucleus c. positive ion d. negative ion e. ionic bond f. covalent bond g. polar molecule h. compound i. symbol j. formula k. molecule l. subscript 94. positively charged center of atom 95. a charged atom that has gained one or more electrons 96. positive ion and negative ion joined together 97. represents an element 98. neutral particle formed when atoms share electrons 99. substance that contains two or more elements 100. particle in which electrons are shared unequally 101. combination of symbols 102. represents number of atoms 103. a charged atom that has lost one or more electrons 104. negative particle in an atom 105. atoms joined together by sharing electrons Match the properties with their characteristics. a. lustrous b. malleable c. ductile 106. reflects light 107. can be hammered or rolled into sheets 108. can be drawn into wires Match each item with the correct description below. a. solvent b. solute c. solution d. unsaturated e. supersaturated f. saturated 109. the substance being dissolved 110. the substance doing the dissolving 111. a mixture that has the same composition throughout 112. can dissolve more solute at a given temperature 113. contains all the solute it can hold at a given temperature 114. contains the most solute possible 115. Coffee has a pH of about 5. Coffee is a ____. a. strong acid b. Strong base c. Weak acid d. Weak base 116. A ____ is a compound formed in solution from the negative ion of an acid and the positive ion of a base. a. detergent b. glycerin c. salt d. soap 117. A bitter taste and a slippery feel are clues that a solution is probably a(n) ____. a. acid b. base c. hydrate d. salt 118. Ammonia is a weak base because it produces ____ ions in solution. a. strong b. weak c. only a few d. many 119. A(n) ____ is a substance that produces H+ ions in a water solution. a. acid b. base c. salt d. alcohol 120. ____ of a solution refers to the ease with which an acid or base forms ions in solution. a. Acidity b. Concentration c. pH d. Strength 121. ____ measures how acidic or basic a substance is. a. An ester b. A base c. pH d. The hydronium ion 122. ____ change color in the presence of an acid or a base. a. Acids b. Glycerins c. Buffers d. Indicators 123. One physical property of acids is a _____. a. slippery feel b. pink color c. sour taste d. presence of hydrogen 124. In a ____ reaction, an acid and a base produce salt and water molecules. a. decomposition b. neutralization c. dilute d. concentrated 125. A(n) ____ is a substance that produces OH– ions in a solution. a. acid b. base c. salt d. alcohol 126. pH measures the ____ of hydronium ions in a solution. a. versatility b. neutralization c. strength d. concentration 127. A base that only partly ionizes in a solution is a ____ base. a. concentrated b. dilute c. strong d. Weak 128. H3O+ units are also known as ____. a. hydrogen ions b. hydronium ions c. hydroxide ions d. hydroxyl groups 129. A process that uses a solution of known concentration to find the concentration of another solution is called ____. a. hydration b. neutralization c. ionization d. titration 130. An acidic solution would have a pH of _____. a. less than 7 b. more than 7 c. 7 or above d. 7 or below 131. The pH scale allows scientists to define the acidity of a substance on a scale of _____. a. 0-7 b. 0-14 c. 1-7 d. 1-14 132. A basic solution contains more _____ ions than hydrogen. a. oxygen b. nitrogen c. hydroxide d. sulfide 133. In a titration, the ____ is the solution for which the concentration is known. a. indicator b. hydrate c. normal solution d. standard solution 134. A solution that contains equal concentrations of hydrogen and hydroxide ions is _____. a. an acid b. a base c. neutral d. ionized Powered by Cognero Page

Name:

Class:

Date:

IPC Final Exam Review

Indicate the answer choice that best completes the statement or answers the question.

1. All substances are built from__________.
 
	a. 
	compound
	b. 
	oxygen
	 
	c. 
	metals
	d. 
	atoms

2. About ______ elements are found on Earth.
 
	a. 
	9
	b. 
	90
	 
	c. 
	900
	d. 
	9000

3. A(n) ______ is a homogeneous mixture of particles so small they cannot be seen without microscopes and will never settle to the bottom of their container.
 
	a. 
	solution
	b. 
	element
	 
	c. 
	molecule
	d. 
	plasma

4. A(n) ______ is a mixture that settles upon standing.
 
	a. 
	solution
	b. 
	colloid
	 
	c. 
	suspension
	d. 
	element

5. A(n) ______ is a mixture that does not scatter light.
 
	a. 
	solution
	b. 
	colloid
	 
	c. 
	suspension
	d. 
	element

6. Any characteristic of a material that you can observe without changing the identity of the substances that make the material is a(n) ______.
 
	a. 
	physical property
	b. 
	chemical property
	 
	c. 
	invisible property
	d. 
	none of these

7. A change in size, shape, or state of matter is called a(n) ______ change.
 
	a. 
	physical
	b. 
	chemical
	 
	c. 
	atomic
	d. 
	impossible

8. The process for separating substances in a mixture by evaporating a liquid and recondensing its vapor is called ______.
 
	a. 
	precipitation
	b. 
	sifting
	 
	c. 
	distribution
	d. 
	distillation

9. A(n) ______ is not homogeneous.
 
	a. 
	suspension
	b. 
	element
	 
	c. 
	compound
	d. 
	solution

10. The scattering of light by colloids is called ______.
 
	a. 
	the Tyndall effect
	b. 
	conservation
	 
	c. 
	air pollution
	d. 
	suspension

11. Smoke is an example of a ______.
 
	a. 
	substance
	b. 
	solution
	 
	c. 
	colloid
	d. 
	suspension

12. Three examples of physical changes are ______.
 
	a. 
	freezing of water, evaporation of gasoline, and rusting of a nail
	 
	b. 
	boiling of water, bursting of a balloon, and melting of a candle
	 
	c. 
	sawing of wood, crushing of a can, and toasting a marshmallow
	 
	d. 
	burning of gasoline, rotting of an egg, and exploding of fireworks

13. The color of ink is a ______.
 
	a. 
	chemical property
	b. 
	physical property
	 
	c. 
	chemical change
	d. 
	physical change

14. When two or more substances are combined so that each substance maintains its own properties, the result is a(n) ______.
 
	a. 
	chemical change
	b. 
	element
	 
	c. 
	compound
	d. 
	mixture

15. ______ is another name for a homogeneous mixture.
 
	a. 
	Suspension
	b. 
	Substance
	 
	c. 
	Solution
	d. 
	Liquid

16. When gasoline is burned in an engine, ______.
 
	a. 
	gasoline evaporates
	b. 
	new substances are formed
	 
	c. 
	mass is lost
	d. 
	mass is gained

17. A(n) ______ is matter that is composed of one type of atom.
 
	a. 
	compound
	b. 
	mixture
	 
	c. 
	element
	d. 
	molecule

18. The smallest piece of an element that still retains the properties of the element is a(n) ______.
 
	a. 
	atom
	b. 
	molecule
	 
	c. 
	compound
	d. 
	plasma

19. The nucleus of an atom is ______ charged.
 
	a. 
	positively
	b. 
	negatively
	 
	c. 
	variably
	d. 
	none of these

20. Neutrons have ______ charge.
 
	a. 
	positive
	b. 
	negative
	 
	c. 
	variable
	d. 
	no

21. Electrons have ______ charge.
 
	a. 
	positive
	b. 
	negative
	 
	c. 
	variable
	d. 
	no

22. Each energy level of an atom has a maximum number of ______ it can hold.
 
	a. 
	neutrons
	b. 
	quarks
	 
	c. 
	protons
	d. 
	electrons

23. Dot diagrams are used to represent ______.
 
	a. 
	the structure of the nucleus
	b. 
	atomic number
	 
	c. 
	isotopes
	d. 
	outer electrons

24. Particles of matter that make up protons and neutrons are ______.
 
	a. 
	electrons
	b. 
	isotopes
	 
	c. 
	atoms
	d. 
	quarks

25. Protons have ______ charge.
 
	a. 
	positive
	b. 
	negative
	 
	c. 
	variable
	d. 
	no

26. A chemical symbol represents the ______of an element.
 
	a. 
	name
	b. 
	structure
	 
	c. 
	reaction
	d. 
	type

27. Horizontal rows of the periodic table are called ______.
 
	a. 
	groups
	b. 
	families
	 
	c. 
	clusters
	d. 
	periods

28. Atoms of the same element with different numbers of neutrons are called ______.
 
	a. 
	metalloids
	b. 
	radioactive
	 
	c. 
	transition elements
	d. 
	isotopes

29. Elements in groups 3 through 12 are called ______.
 
	a. 
	metalloids
	b. 
	transition elements
	 
	c. 
	noble gases
	d. 
	isotopes

30. A certain atom has 26 protons, 26 electrons, and 30 neutrons. Its mass number is ______.
 
	a. 
	26
	b. 
	30
	 
	c. 
	52
	d. 
	56

31. _____ is the only metal that is not solid at room temperature.
 
	a. 
	Steel
	b. 
	Aluminum
	 
	c. 
	Copper
	d. 
	Mercury

32. When metals combine with nonmetals, the atoms of the metals tend to lose electrons, forming _____ bonds.
 
	a. 
	ionic
	b. 
	covalent
	 
	c. 
	triple
	d. 
	unbreakable

33. In _____ bonding, positively charged metallic ions are surrounded by a cloud of electrons.
 
	a. 
	ionic
	b. 
	covalent
	 
	c. 
	triple
	d. 
	metallic

34. A(n) _____ element is one in which the nucleus breaks down and gives off particles and energy.
 
	a. 
	stable
	b. 
	gaseous
	 
	c. 
	metallic
	d. 
	radioactive

35. Elements in Groups 3 through 12 on the periodic table are known as _____ elements.
 
	a. 
	gaseous
	b. 
	noble
	 
	c. 
	radioactive
	d. 
	transition

36. The two rows of elements that seem to be disconnected from the rest of the periodic table are the _____.
 
	a. 
	nonmetals
	b. 
	halogens
	 
	c. 
	noble gases
	d. 
	inner transition metals

37. An allotrope of carbon that is soft and can be used as a lubricant is _____.
 
	a. 
	silicon
	b. 
	diamond
	 
	c. 
	sand
	d. 
	graphite

38. The process by which a solid changes directly to a gas without first becoming a liquid is called _____.
 
	a. 
	condensation
	b. 
	ionization
	 
	c. 
	sublimation
	d. 
	evaporation

39. When hydrogen reacts with active metals, it _____.
 
	a. 
	shares electrons
	b. 
	gains on electron
	 
	c. 
	loses one electron
	d. 
	loses two electron

40. Different forms of the same element that have different properties because of different atom arrangements are called _____.
 
	a. 
	allotropes
	b. 
	carbons
	 
	c. 
	silicons
	d. 
	graphites

41. At room temperature, most metals are _____.
 
	a. 
	liquids
	b. 
	solids
	 
	c. 
	radioactive
	d. 
	gases

42. An allotrope of carbon that is hard and is often used in jewelry is ______.
 
	a. 
	silver
	b. 
	diamond
	 
	c. 
	quartz
	d. 
	graphite

43. Metals can be used as wire because they are _____.
 
	a. 
	ductile
	b. 
	malleable
	 
	c. 
	shinny
	d. 
	alloys

44. A group of elements that have two electrons in its outer energy level is the ______.
 
	a. 
	alkaline earth metals
	b. 
	halogens
	 
	c. 
	alkali metals
	d. 
	actinides

45. Synthetic elements are found in which of the following groups?
 
	a. 
	actinides
	b. 
	alkali metals
	 
	c. 
	oxides
	d. 
	halogens

46. Hydrogen is grouped with the alkali metals because it _____.
 
	a. 
	is a metal
	 
	b. 
	has one electron in its outer energy level
	 
	c. 
	it is a gas
	 
	d. 
	does not readily form compounds

47. Elements that lie along the stair-step line of the periodic table are _____.
 
	a. 
	liquids
	b. 
	metals
	 
	c. 
	metalloids
	d. 
	radioactive

48. Copper, sulfur, and oxygen are examples of ______.
 
	a. 
	elements
	b. 
	compounds
	 
	c. 
	mixtures
	d. 
	colloids

49. A chemical ______ tells what elements a compound contains and the exact number of the atoms of each element in a unit of that compound.
 
	a. 
	formula
	b. 
	table
	 
	c. 
	dot diagram
	d. 
	chart

50. H2O is also known as ______.
 
	a. 
	carbon
	b. 
	mercury
	 
	c. 
	nickel
	d. 
	water

51. A chemical ______ is the force that holds atoms together in a compound.
 
	a. 
	bond
	b. 
	element
	 
	c. 
	compound
	d. 
	formula

52. A charged particle is known as a(n) ______.
 
	a. 
	plasma
	b. 
	gas
	 
	c. 
	ion
	d. 
	neutron

53. The attraction that forms between atoms when they share electrons is known as a(n) ______ bond.
 
	a. 
	ionic
	b. 
	covalent
	 
	c. 
	simple
	d. 
	net

54. The elements that make up a compound and the number of atoms of each element in a unit of the compound can be shown in a ______.
 
	a. 
	chemical symbol
	b. 
	chemical formula
	 
	c. 
	subscript
	d. 
	subscript

55. A group of atoms that acts together as one charged atom is a ______.
 
	a. 
	polyatomic ion
	b. 
	negative ion
	 
	c. 
	molecule
	d. 
	crystal

56. In chemical formulas, the number of atoms in a unit of the compound is shown by numbers called ______.
 
	a. 
	oxidation numbers
	b. 
	superscripts
	 
	c. 
	hydrates
	d. 
	subscripts

57. A chemical bond that occurs when atoms share electrons is a(n) ______ bond.
 
	a. 
	ionic
	b. 
	covalent
	 
	c. 
	polyatomic
	d. 
	magnetic

58. The name given to the number of electrons an atom gains, loses, or shares is the ______.
 
	a. 
	ionic number
	b. 
	atomic number
	 
	c. 
	oxidation number
	d. 
	atomic mass

59. How many electrons are needed in the outer energy levels of most atoms for the atom to be chemically stable?
 
	a. 
	2
	b. 
	4
	 
	c. 
	6
	d. 
	8

60. The sum of the oxidation numbers in a neutral compound is always ______.
 
	a. 
	one
	b. 
	zero
	 
	c. 
	a positive number
	d. 
	a negative number

61. Why do the noble gases not form compounds readily?
 
	a. 
	They have no electrons.
	 
	b. 
	They have empty outer energy levels.
	 
	c. 
	They have seven electrons in their outer energy levels.
	 
	d. 
	Their outer energy levels are completely filled with electrons.

62. What is the name of the compound with the formula NaCl?
 
	a. 
	sodium chloride
	b. 
	chlorine sodiate
	 
	c. 
	sodium dichloride
	d. 
	sodium chlorate

63. How many hydrogen atoms are present in one molecule of ammonium acetate, NH4C2H3O2?
 
	a. 
	3
	b. 
	4
	 
	c. 
	7
	d. 
	11

64. The oxidation number of an atom is shown with a ______.
 
	a. 
	subscript
	b. 
	positive number
	 
	c. 
	superscript
	d. 
	negative number

65. A(n) _____ is a mixture that has the same composition, color, and density throughout.
 
	a. 
	element
	b. 
	solution
	 
	c. 
	mixture
	d. 
	plasma

66. If a cube is split in half, the surface area of the pieces will be _____ that of the cube.
 
	a. 
	greater than
	b. 
	less than
	 
	c. 
	the same as
	d. 
	none of these

67. A dilute solution has _____ of solute in the solvent.
 
	a. 
	a large amount
	b. 
	a small amount
	 
	c. 
	an unlimited amount
	d. 
	none of these

68. _____ molecules have a positive area and a negative area.
 
	a. 
	Polar
	b. 
	Nonpolar
	 
	c. 
	Organic
	d. 
	Gaseous

69. _____ is the maximum amount of a solute that can be dissolved in a given amount of solvent at a given temperature.
 
	a. 
	Solubility
	b. 
	Volume
	 
	c. 
	Density
	d. 
	A solution

70. A solution that contains all the solute it can at a given temperature is called _____.
 
	a. 
	filled
	b. 
	calcified
	 
	c. 
	unsaturated
	d. 
	saturated

71. In a solution, the substance that is being dissolved is the _____.
 
	a. 
	solute
	b. 
	solvent
	 
	c. 
	liquid
	d. 
	gas

72. The air that you breathe is an example of a(n) _____ solution.
 
	a. 
	gaseous
	b. 
	solid
	 
	c. 
	liquid
	d. 
	amalgam

73. In soda pop, the solvent would be the _____.
 
	a. 
	water
	b. 
	carbon dioxide
	 
	c. 
	sugar
	d. 
	flavoring

74. A substance that does not conduct an electric current when it forms a solution is a(n) _____.
 
	a. 
	electrolyte
	b. 
	nonelectrolyte
	 
	c. 
	polar substance
	d. 
	salt

75. The process by which the particles in a crystal are separated and drawn into solution by water is called _____.
 
	a. 
	ionization
	b. 
	dissociation
	 
	c. 
	polarity
	d. 
	saturation

76. Increasing the surface area of a solid _____.
 
	a. 
	slows the speed of dissolving
	 
	b. 
	has no effect on the speed of dissolving
	 
	c. 
	increases the speed of dissolving
	 
	d. 
	causes the solid to ionize

77. The solubility of a gas in a liquid occurs faster if the liquid is _____.
 
	a. 
	heated
	b. 
	cooled
	 
	c. 
	under low pressure
	d. 
	an electrolyte

78. The concentration of a solution that contains a large amount of solute in the solvent could be described as _____.
 
	a. 
	unsaturated
	b. 
	polar
	 
	c. 
	concentrated
	d. 
	dilute

79. An alloy is an example of a _____ solution.
 
	a. 
	gaseous
	b. 
	liquid
	 
	c. 
	solid
	d. 
	dilute

80. Which of the following will speed up the dissolving of a solid solute in water?
 
	a. 
	Stir the solution.
	b. 
	Cool the solution.
	 
	c. 
	Grind up the solvent.
	d. 
	Freeze the solute.

81. Water is sometimes referred to as the universal solvent because _____.
 
	a. 
	it has no separated positive and negative areas
	 
	b. 
	it is a small molecule and can fit easily among the molecules of many solutes.
	 
	c. 
	it has a polar and a nonpolar end
	 
	d. 
	its molecules can slip easily among molecules of a nonpolar solvent

82. A(n) _____ reaction is a change in which one or more substances are converted into new substances.
 
	a. 
	chemical
	b. 
	physical
	 
	c. 
	state
	d. 
	electrical

83. The substances that react are called _____.
 
	a. 
	nuclear reactors
	b. 
	elements
	 
	c. 
	compounds
	d. 
	reactants

84. The new substances produced in a reaction are called _____.
 
	a. 
	elements
	b. 
	compounds
	 
	c. 
	products
	d. 
	reactants

85. Numbers to the left of formulas for reactants are called _____.
 
	a. 
	superscripts
	b. 
	coefficients
	 
	c. 
	elements
	d. 
	formulas

86. A(n) _____ chemical equation has the same number of atoms of each element on both sides.
 
	a. 
	false
	b. 
	balanced
	 
	c. 
	imbalanced
	d. 
	physical

87. Each substance to the right of the arrow in a chemical equation is a ______.
 
	a. 
	catalyst.
	b. 
	precipitate.
	 
	c. 
	reactant.
	d. 
	product.

88. Each substance on the left side of the arrow in a chemical equation is a ______.
 
	a. 
	reactant.
	b. 
	product.
	 
	c. 
	coefficient.
	d. 
	catalyst.

89. An example of a balanced chemical equation is ______.
 
	a. 
	AgNO3 + NaCl→.4AgCl + 2NaNO3
	 
	b. 
	2AgNO3 +2NaCl.→3AgCl + 2NaNO3.
	 
	c. 
	AgNO3 + NaCl→.AgCl+ NaNO3.
	 
	d. 
	AgNO3 + 2NaCl + AgCl→AgCl +3NaNO3.

90. According to the law of conservation of mass, how does the mass of the products in a chemical reaction compare with the mass of the reactants?
 
	a. 
	The mass of the products is greater.
	 
	b. 
	The mass of the reactants is greater.
	 
	c. 
	There is no relationship.
	 
	d. 
	The masses are equal.

Match each item with the correct term.
a. 
	positive charge
	b. 
	negative charge
	c. 
	no charge

91. proton

92. neutron

93. electron

Match each term with the correct description below.
a. 
	electron
	b. 
	nucleus
	c. 
	positive ion
	d. 
	negative ion
	e. 
	ionic bond
	f. 
	covalent bond
	g. 
	polar molecule
	h. 
	compound
	i. 
	symbol
	j. 
	formula
	k. 
	molecule
	l. 
	subscript

94. positively charged center of atom

95. a charged atom that has gained one or more electrons

96. positive ion and negative ion joined together

97. represents an element

98. neutral particle formed when atoms share electrons

99. substance that contains two or more elements

100. particle in which electrons are shared unequally

101. combination of symbols

102. represents number of atoms

103. a charged atom that has lost one or more electrons

104. negative particle in an atom

105. atoms joined together by sharing electrons

Match the properties with their characteristics.
a. 
	lustrous
	b. 
	malleable
	c. 
	ductile

106. reflects light

107. can be hammered or rolled into sheets

108. can be drawn into wires

Match each item with the correct description below.
a. 
	solvent
	b. 
	solute
	c. 
	solution
	d. 
	unsaturated
	e. 
	supersaturated
	f. 
	saturated

109. the substance being dissolved

110. the substance doing the dissolving

111. a mixture that has the same composition throughout

112. can dissolve more solute at a given temperature

113. contains all the solute it can hold at a given temperature

114. contains the most solute possible

115. Coffee has a pH of about 5. Coffee is a ____.
 
	a. 
	strong acid
	 
	b. 
	Strong base
	 
	c. 
	Weak acid
	 
	d. 
	Weak base

116. A ____ is a compound formed in solution from the negative ion of an acid and the positive ion of a base.
 
	a. 
	detergent
	 
	b. 
	glycerin
	 
	c. 
	salt
	 
	d. 
	soap

117. A bitter taste and a slippery feel are clues that a solution is probably a(n) ____.
 
	a. 
	acid
	 
	b. 
	base
	 
	c. 
	hydrate
	 
	d. 
	salt

118. Ammonia is a weak base because it produces ____ ions in solution.
 
	a. 
	strong
	 
	b. 
	weak
	 
	c. 
	only a few
	 
	d. 
	many

119. A(n) ____ is a substance that produces H+ ions in a water solution.
 
	a. 
	acid
	 
	b. 
	base
	 
	c. 
	salt
	 
	d. 
	alcohol

120. ____ of a solution refers to the ease with which an acid or base forms ions in solution.
 
	a. 
	Acidity
	 
	b. 
	Concentration
	 
	c. 
	pH
	 
	d. 
	Strength

121. ____ measures how acidic or basic a substance is.
 
	a. 
	An ester
	 
	b. 
	A base
	 
	c. 
	pH
	 
	d. 
	The hydronium ion

122. ____ change color in the presence of an acid or a base.
 
	a. 
	Acids
	 
	b. 
	Glycerins
	 
	c. 
	Buffers
	 
	d. 
	Indicators

123. One physical property of acids is a _____.
 
	a. 
	slippery feel
	 
	b. 
	pink color
	 
	c. 
	sour taste
	 
	d. 
	presence of hydrogen

124. In a ____ reaction, an acid and a base produce salt and water molecules.
 
	a. 
	decomposition
	 
	b. 
	neutralization
	 
	c. 
	dilute
	 
	d. 
	concentrated

125. A(n) ____ is a substance that produces OH– ions in a solution.
 
	a. 
	acid
	 
	b. 
	base
	 
	c. 
	salt
	 
	d. 
	alcohol

126. pH measures the ____ of hydronium ions in a solution.
 
	a. 
	versatility
	 
	b. 
	neutralization
	 
	c. 
	strength
	 
	d. 
	concentration

127. A base that only partly ionizes in a solution is a ____ base.
 
	a. 
	concentrated
	 
	b. 
	dilute
	 
	c. 
	strong
	 
	d. 
	Weak

128. H3O+ units are also known as ____.
 
	a. 
	hydrogen ions
	 
	b. 
	hydronium ions
	 
	c. 
	hydroxide ions
	 
	d. 
	hydroxyl groups

129. A process that uses a solution of known concentration to find the concentration of another solution is called ____.
 
	a. 
	hydration
	 
	b. 
	neutralization
	 
	c. 
	ionization
	 
	d. 
	titration

130. An acidic solution would have a pH of _____.
 
	a. 
	less than 7
	 
	b. 
	more than 7
	 
	c. 
	7 or above
	 
	d. 
	7 or below

131. The pH scale allows scientists to define the acidity of a substance on a scale of _____.
 
	a. 
	0-7
	 
	b. 
	0-14
	 
	c. 
	1-7
	 
	d. 
	1-14

132. A basic solution contains more _____ ions than hydrogen.
 
	a. 
	oxygen
	 
	b. 
	nitrogen
	 
	c. 
	hydroxide
	 
	d. 
	sulfide

133. In a titration, the ____ is the solution for which the concentration is known.
 
	a. 
	indicator
	 
	b. 
	hydrate
	 
	c. 
	normal solution
	 
	d. 
	standard solution

134. A solution that contains equal concentrations of hydrogen and hydroxide ions is _____.
 
	a. 
	an acid
	 
	b. 
	a base
	 
	c. 
	neutral
	 
	d. 
	ionized

Transcript for:IPC Final Exam Study Guide

Transcript for:
IPC Final Exam Study Guide