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Chapter 2 Atoms, Molecules, and Ions Matter Matter is anything that has mass and takes up space 2 Atomic Theory of Matter Atoms are the fundamental building blocks of matter championed by John Dalton (1803 – 1807) 3 © 2015 Pearson Education, Inc. Atomic Theory of Matter An element is composed of atoms Atoms are the smallest particle of an element that still have the properties of the element 4 © 2015 Pearson Education, Inc. Atomic Theory of Matter Atoms of an element are identical in mass and other properties Atoms of different elements have different properties and different atomic weights 5 © 2015 Pearson Education, Inc. Atomic Theory of Matter In a chemical reaction, the mass of the products equals the mass of the reactants Law of conservation of mass 6 © 2015 Pearson Education, Inc. Atomic Theory of Matter Samples of a pure compound always contain the same elements in the same mass proportion Law of constant composition 7 © 2015 Pearson Education, Inc. Atomic Theory of Matter Deduced… When elements combine, they do so in the ratio of small whole numbers Law of Multiple Proportions 8 © 2015 Pearson Education, Inc. SUBATOMIC PARTICLE DISCOVERY 9 The Electron (Cathode Rays) • High voltage produced radiation • Particles are negatively charged • J. J. Thomson is credited with their discovery (1897) 10 © 2015 Pearson Education, Inc. The Electron Thomson measured the charge/mass ratio of the electron to be 1.76 108 coulombs/gram (C/g) 11 © 2015 Pearson Education, Inc. Millikan Oil-Drop Experiment (Electrons) • Robert Millikan (1909) • Determined charge of the electron • 1.60 x 10-19 C • Calculated mass of electron • 9.10 x 10-29 g © 2015 Pearson Education, Inc. The Atom, circa 1900 “Plum pudding” model put forward by Thomson 13 © 2015 Pearson Education, Inc. Discovery of the Nucleus In 1910 Ernest Rutherford shot particles (positive charge) at a thin sheet of gold foil and observed the pattern of scatter of the particles 14 © 2015 Pearson Education, Inc. The Nuclear Atom Particles deflected at large angles disproved Thomson’s model could not be correct 15 © 2015 Pearson Education, Inc. The Nuclear Atom Particles deflected at large angles disproved Thomson’s model could not be correct In 1911, Rutherford presented his interpretation 16 © 2015 Pearson Education, Inc. MODERN VIEW OF ATOMIC STRUCTURE 17 Atom Composition • Atoms are made of subatomic particles 1. Electron have a negative (-) electrical charge 2. Proton has a positive (+) electrical charge 3. Neutron has no charge 18 Subatomic Particles Arrangement • Location of subatomic particles – Protons and neutrons are located in the nucleus • Nucleus is small, dense and positively charged • >99.6% of an atom’s mass is found in the nucleus 19 Subatomic Particles Arrangement • Location of subatomic particles – Electrons are located in the electron cloud • Space is mostly empty and negatively charged • Electrons move rapidly around the nucleus 20 Subatomic Particles Arrangement • Atoms – Are neutral – Contain the same number of protons and electrons 21 Subatomic Particles in an Atom • Every element has a set number of protons assigned to it (protons and neutrons) – All carbon atoms contain 6 protons – All nitrogen atoms contain 7 protons – All oxygen atoms contain 8 protons The number of protons in a atom is called its atomic number (Z) In a neutral atom the atomic number = number of electrons 22 Subatomic Particles in an Atom • Mass number reports the number of protons and neutrons in an atom (protons and neutrons) mass # = # of protons + . # of neutrons 23 Subatomic Particles in an Atom (protons and neutrons) - number of protons = atomic number (Z) - number of electrons = atomic number (Z) - number of neutrons = mass number – atomic number =A-Z 24 Subatomic Particles in an Atom Element - number of protons = atomic number (Z) - number of electrons = atomic number (Z) - number of neutrons = mass number – atomic number =A-Z 25 Subatomic Particles in an Atom # protons = 9 # electrons = 9 # neutrons = 10 # protons = 79 # electrons = 79 # neutrons = 118 26 Number of neutrons in an atom do not have to equal number of protons in an atom 27 Subatomic Particles in an Atom # protons = 6 # electrons = 6 # neutrons = 5 % abundance = trace # protons = 6 # electrons = 6 # neutrons = 6 % abundance = 98.89% # protons = 6 # electrons = 6 # neutrons = 7 % abundance = 1.11% # protons = 6 # electrons = 6 # neutrons = 8 % abundance = trace • Elements may have different forms • The amount of each naturally occurring form differ • Isotope – have equal number of protons but a different amount of neutrons – Element not in abundance 28 Atomic Weight • Atomic mass # protons = 6 # electrons = 6 # neutrons = 5 % abundance = trace # protons = 6 # electrons = 6 # neutrons = 6 % abundance = 98.89% – Mass of one type of isotope – defined as one twelfth (1/12) of the mass of an atom of carbon-12 – 1 amu = 1.66054 × 10–24 g • Atomic weight (average atomic mass) # protons = 6 # electrons = 6 # neutrons = 7 % abundance = 1.11% # protons = 6 # electrons = 6 # neutrons = 8 % abundance = trace – Atomic Weight = Ʃ [(isotope mass) × (fractional natural abundance)] – Units amu 29 Atomic Weight • Atomic mass calculated for carbon # protons = 6 # electrons = 6 # neutrons = 5 % abundance = trace # protons = 6 # electrons = 6 # neutrons = 6 % abundance = 98.89% 1. Multiply each isotope’s relative mass by the percent abundance 12 6 C : 12.000 amu * 0.9889 = 11.87 amu 13 6 C : 13.003 amu * 0.0111 = 0.144 amu 2. Sum products from multiplication to get average atomic mass # protons = 6 # electrons = 6 # neutrons = 7 % abundance = 1.11% # protons = 6 # electrons = 6 # neutrons = 8 % abundance = trace C: 11.87 amu + 0.144 amu = 12.01 amu 30 PERIODIC TABLE 31 Periodic Table • A systematic organization of the elements • Elements are arranged in order of atomic number 32 © 2015 Pearson Education, Inc. Periodic Table What does this mean? 33 © 2015 Pearson Education, Inc. Periodic Table • Atomic number (Z) – Number of protons in the atom © 2015 Pearson Education, Inc. 34 Periodic Table • Atomic symbol or chemical symbol – 1 or 2 letter designation of an element © 2015 Pearson Education, Inc. 35 Periodic Table • Atomic weight – Average mass of an atom’s isotope weighted by its percent abundance © 2015 Pearson Education, Inc. 36 Periodic Table • The rows are called periods • Columns are called groups • Elements in the same group have similar chemical properties 37 © 2015 Pearson Education, Inc. Periodic Table: Group Names These five groups are known by their names 38 © 2015 Pearson Education, Inc. Periodic Table • Metals are on the left side of the periodic table • Some properties of metals include • shiny luster • conducting heat and electricity • solidity (except mercury) 39 © 2015 Pearson Education, Inc. Periodic Table • Nonmetals are on the right side of the periodic table (except H) • Are solid (like carbon), liquid (like bromine), or gas (like neon) at room temperature 40 © 2015 Pearson Education, Inc. Periodic Table • Elements on the steplike line are metalloids (except Al) • Properties are sometimes like metals and sometimes like nonmetals 41 © 2015 Pearson Education, Inc. MOLECULES AND MOLECULAR COMPOUNDS 42 Molecules Aggregation of Atoms Molecule is a group of two or more atoms bonded together 43 © 2011Pearson Education, Inc.. Molecules • Diatomic molecules contain two atoms • Some naturally occurring diatomic molecules – – – – Hydrogen Nitrogen Oxygen Chlorine 44 Molecules • Molecule that contain two or more types of atoms are called molecular compounds 45 Chemical Formulas Chemical formula states the relative number and type of atoms present in a molecule 46 Chemical Formulas • Molecular formulas – Type of chemical formula – Provides the exact number of atoms of each element in a compound • Subscript to the right of the symbol of an element gives this information – Almost always contain only nonmetals 47 © 2015 Pearson Education, Inc. Chemical Formulas • Molecular formula – Gives actual number of atoms present in a compound • Empirical formula – Gives smallest whole number ratio of atoms present in a compound 48 Picturing Molecules • Structural formulas – Show the order in which atoms are attached – Do NOT depict the threedimensional shape of molecules • Perspective drawings – Show the threedimensional order of the atoms in a compound 49 © 2015 Pearson Education, Inc. IONS AND IONIC COMPOUNDS 50 Ions • Electron transfer produces ions • Ion is a charged atom or molecule – – – – Occurs because of loss or gain of an electron Cation is a positively charged ion Anion is a negatively charged ion Ion charge is directly related to the number of electrons lost or gained 51 © 2015 Pearson Education, Inc. Ions: Predicting Charge • Ions – Cations are formed by metals – Anions are formed by nonmetals 52 © 2015 Pearson Education, Inc. Polyatomic ions • Polyatomic ions – Atoms in ion bonded covalently – Are not molecules – Pieces of a compound 53 Ionic Compounds • Ionic compounds – Formed from cations and anions – Generally contain metals and nonmetals – Use empirical formulas 54 Ionic Compounds: Writing Formulas • Because compounds are electrically neutral, one can determine the formula of a compound this way: – Charge on the cation becomes the subscript on the anion – Charge on the anion becomes the subscript on the cation – If these subscripts are not in the lowest whole-number ratio, divide them by the greatest common factor 55 Way of naming compounds NOMENCLATURE 56 Compound Classification • Rules for naming ionic and molecular compounds differ 1st classify compound as ionic or molecular 57 Compound Classification • There is no sharp dividing line between ionic and covalent bond • For purposes of naming – Compounds consisting of metal and nonmetals are ionic – Compounds consisting of only nonmetals are molecular – Exception: • Polyatomic ion of nonmetals replace the metal ion in an ionic compound • Metalloid elements are considered nonmetals 58 Compound Classification • Fixed-charge metal – Only forms one type of positive ion • Variable-charge metal – Forms more than one type of positive ion Ionic Charge +1 Ionic Charge +2 Ionic Charge +3 Li+ Be2+ Al3+ Na+ Mg2+ Ga3+ K+ Ca2+ Rb+ Sr2+ Cs+ Ba2+ Ag+ Zn2+ Cd2+ 59 Compound Classification • Fixed-charge metal – Only forms one type of positive ion • Variable-charge metal – Forms more than one type of positive ion 60 © 2015 Pearson Education, Inc. NOMENCLATURE FOR IONIC COMPOUNDS 61 Ions Nomenclature • Ionic compounds are based on the name of the ions they are composed • Rules for cations 1. Fix-charged metal ions take full name of element plus the word ion - Na+ Ca2+ Al3+ sodium ion calcium ion aluminum ion 62 Ions Nomenclature • Rules for cations 2. Variable-charge metal ions • Take full name of element followed by a Roman numeral (in parentheses) that represent the charge magnitude plus the word ion - Fe2+ - Fe3+ - Cu2+ iron (II) ion iron (III) ion copper (II) ion 63 Ions Nomenclature • Rules for cations 2. Variable-charge metal ions (Older naming system) • Use suffix –ic for the ion of higher charge • Use suffix –ous for the ion of lower charge 3. Cations formed from nonmetal atoms end in –ium - NH4+ ammonium ion - H3O+ hydronium ion 64 Ions Nomenclature • Rules for anions names 1. Nonmetal ions take the stem of the name of the element followed by the suffix –ide and the word ion 65 © 2015 Pearson Education, Inc. Naming Polyatomic Ions Polyatomic ions must be memorized 66 © 2015 Pearson Education, Inc. Patterns in Oxygen Containing Anions Nomenclature • The most common oxyanion of an element ends in -ate: – ClO3− is chlorate • Oxyanion that has one fewer oxygen then the most common oxyanion ends in -ite: – ClO2− is chlorite • Prefix hypo- indicates one O atom fewer than the oxyanion ending in ite: – ClO− is hypochlorite • Prefix per- indicates on more O atom than the oxyanion ending in -ate: – ClO4− is perchlorate 67 Patterns in Oxygen Containing Anions Nomenclature • Central atoms on the second row have a bond up to three oxygens • Central atoms on the third row have a bond up to four oxygens • Charges increase as you go from right to left 68 © 2015 Pearson Education, Inc. Ionic Compounds Nomenclature • Naming fixed-charge ionic compounds – Full name of metallic element is given first – Nonmetal element name follows with the stem of the name attached with the suffix –ide – Name of compound contains sufficient information to determine chemical formula NaF MgF2 Na2O Be3N2 sodium fluoride magnesium fluoride sodium oxide beryllium nitride 69 Binary Ionic Compounds Nomenclature • Naming variable-charge binary ionic compounds – Full name of metallic element with a Roman numeral appended is given first – Nonmetal element name follows with the stem of the name attached with the suffix –ide CuO Cu2O Mn2S3 AuCl3 copper (II) oxide copper (I) oxide manganese (III) sulfide gold (III) chloride 70 Polyatomic Ionic Compounds Nomenclature • Name of polyatomic ionic compounds are derived in a similar way as binary ionic compounds – If polyatomic ion positive, name is substituted for metal – If polyatomic ion negative, name is substituted for the nonmetal minus the word ion – If both polyatomic ions, substitute names of polyatomic ions 71 Polyatomic Ionic Compounds Nomenclature • Name of polyatomic ionic compounds are derived in a similar way as binary ionic compounds Na3PO4 Fe(NO3)3 NH4CN sodium phosphate iron (III) nitrate ammonium cyanide 72 ACID NOMENCLATURE 73 Acid Nomenclature • Acid – Hydrogen containing molecular compound that yields hydrogen ions (H+) • Naming Acids – naming system applies if acid is dissolved in water – If anion does not contain oxygen and ends in -ide • Prefix hydro• Suffix –ic • Add acid HCl: hydrochloric acid HCN: hydrocyanic acid 74 Acid Nomenclature • If anion does contain oxygen – If anion ends in –ate • Suffix –ic • Add acid HNO3: nitric acid HClO4: perchloric acid – If anion ends in –ite • Suffix –ous • Add acid HNO2: nitrous acid HClO: hypochlorous acid 75 Acid Nomenclature • Series of oxyacid nomenclature 76 © 2015 Pearson Education, Inc. BINARY MOLECULAR COMPOUND NOMENCLATURE 77 Binary Molecular Compound Nomenclature • Binary molecular compound only has two nonmetallic elements present • List nonmetals in a chemical formula by increasing nonmetallic behavior – Element with highest atomic number is listed first if in same group • Name compound in the order listed in chemical formula 78 © 2015 Pearson Education, Inc. Binary Molecular Compound Nomenclature • Naming binary molecular compounds – Full name of first nonmetal is given first – Second nonmetal name follows with the stem of the name attached with the suffix –ide – Numerical prefixes giving numbers of atoms present follow both nonmetals N2O5 Dinitrogen Pentoxide dinitrogen pentoxide PF3 S4N4 phosphorus tetrasulfur trifluoride phosphorus tetranitride tetrasulfur trifluoride tetranitride 79 © 2015 Pearson Education, Inc. NOMENCLATURE SIMPLE ORGANIC COMPOUNDS 80 Nomenclature of Organic Compounds • Organic chemistry – Study of carbon – Own system of nomenclature • Alkanes contain only hydrogen and carbon • Stem of name refers to number of carbons Nomenclature of Organic Compounds • Alcohol – Replace a hydrogen with –OH – Suffix becomes –ol – Determine type of compound by studying the suffix 83 EXAMPLE ATOMIC NUMBER, ATOMIC SYMBOL, AND ELEMENT NAME List the atomic symbol and atomic number for each element. (a) (b) (c) (d) silicon potassium gold antimony SOLUTION As you become familiar with the periodic table, you will be able to quickly locate elements on it. At first you may find it easier to locate them in the alphabetical listing on the inside back cover of this book, but you should become familiar with their positions in the periodic table. 84 EXAMPLE CLASSIFYING ELEMENTS AS METALS, NONMETALS, OR METALLOIDS Classify each element as a metal, nonmetal, or metalloid. (a) Ba (b) I (c) O (d) Te SOLUTION (a) Barium is on the left side of the periodic table; it is a metal. (b) Iodine is on the right side of the periodic table; it is a nonmetal. (c) Oxygen is on the right side of the periodic table; it is a nonmetal. (d) Tellurium is in the middle-right section of the periodic table, along the line that divides the metals from the nonmetals; it is a metalloid. 85 EXAMPLE GROUPS AND FAMILIES OF ELEMENTS To which group or family of elements does each element belong? (a) Mg (b) N (c) K (d) Br SOLUTION (a) (b) (c) (d) Mg is in Group 2A; it is an alkaline earth metal. N is in Group 5A. K is in Group 1A; it is an alkali metal. Br is in Group 7A; it is a halogen. 86 EXAMPLE ATOMIC NUMBERS, MASS NUMBERS, AND ISOTOPE SYMBOLS What are the atomic number (Z), mass number (A), and symbols of the carbon isotope that has 7 neutrons? SOLUTION You can determine that the atomic number (Z) of carbon is 6 (from the periodic table). This means that carbon atoms have 6 protons. The mass number (A) for the isotope with 7 neutrons is the sum of the number of protons and the number of neutrons. A = 6 + 7 = 13 So, Z = 6, A = 13, and the symbols for the isotope are C-13 and 87 EXAMPLE NUMBERS OF PROTONS AND NEUTRONS FROM ISOTOPE SYMBOLS How many protons and neutrons are in the chromium isotope SOLUTION #p+ = Z = 24 The number of protons is equal to Z (lower left number). The number of neutrons is equal to A (upper left number) – Z (lower left number). #n = A – Z = 52 – 24 = 28 SKILLBUILDER | Numbers of Protons and Neutrons from Isotope Symbols How many protons and neutrons are in the potassium isotope Answer: 19 protons, 20 neutrons 88 EXAMPLE WRITING CHEMICAL FORMULAS Write a chemical formula for each compound. (a) the compound containing two aluminum atoms to every three oxygen atoms (b) the compound containing three oxygen atoms to every sulfur atom (c) the compound containing four chlorine atoms to every carbon atom Aluminum is the metal, so list it first. SOLUTION (a) Al2O3 Sulfur is below oxygen on the periodic table and it occurs before oxygen in Table 5.1, so list it first. (b) SO3 Carbon is to the left of chlorine on the periodic table and it occurs before chlorine in Table 5.1, so list it first. (c) CCl4 89 EXAMPLE WRITING CHEMICAL FORMULAS Continued SKILLBUILDER | Writing Chemical Formulas Write a chemical formula for each compound. (a) the compound containing two silver atoms to every sulfur atom (b) the compound containing two nitrogen atoms to every oxygen atom (c) the compound containing two oxygen atoms to every titanium atom Answers: (a) Ag2S (b) N2O (c) TiO2 90 EXAMPLE CLASSIFYING SUBSTANCES AS ATOMIC ELEMENTS, MOLECULAR ELEMENTS, MOLECULAR COMPOUNDS, OR IONIC COMPOUNDS Classify each substance as an atomic element, molecular element, molecular compound, or ionic compound. (a) krypton (b) CoCl2 (c) nitrogen (d) SO2 (e) KNO3 SOLUTION (a) Krypton is an element that is not diatomic; therefore, it is an atomic element. (b) CoCl2 is a compound composed of a metal (left side of periodic table) and nonmetal (right side of the periodic table); therefore, it is an ionic compound. (c) Nitrogen is an element that is listed as diatomic in Table 5.2; therefore, it is a molecular element. (d) SO2 is a compound composed of two nonmetals; therefore, it is a molecular compound. (e) KNO3 is a compound composed of a metal and two nonmetals; therefore, it is an ionic compound. 91 EXAMPLE NAMING IONIC COMPOUNDS CONTAINING A METAL THAT FORMS ONLY ONE TYPE OF CATION Name the compound MgF2. SOLUTION The cation is magnesium. The anion is fluorine, which becomes fluoride. Its correct name is magnesium fluoride. SKILLBUILDER | Naming Ionic Compounds Containing a Metal That Forms Only One Type of Ion Name the compound KBr. Answer: potassium bromide SKILLBUILDER PLUS Name the compound Zn3 N2. Answer: zinc nitride 92 EXAMPLE Naming Ionic Compounds Containing a Metal That Forms More Than One Type of Cation Name the compound PbCl4. SOLUTION The name for PbCl4 consists of the name of the cation, lead, followed by the charge of the cation in parentheses (IV), followed by the base name of the anion, chlor-, with the ending -ide. The full name is lead(IV) chloride. We know the charge on Pb is 4+ because the charge on Cl is 1–. Since there are 4 Cl– anions, the Pb cation must be Pb4+. PbCl4 lead(IV) chloride SKILLBUILDER | Naming Ionic Compounds Containing a Metal That Forms More Than One Type of Cation Name the compound PbO. Answer: lead(II) oxide 93 EXAMPLE NAMING IONIC COMPOUNDS CONTAINING A POLYATOMIC ION Name the compound K2CrO4. SOLUTION The name for K2CrO4 consists of the name of the cation, potassium, followed by the name of the polyatomic ion, chromate. K2CrO4 potassium chromate SKILLBUILDER | NAMING IONIC COMPOUNDS CONTAINING A POLYATOMIC ION Name the compound Mn(NO3)2. Answer: manganese(II) nitrate 94 EXAMPLE NAMING MOLECULAR COMPOUNDS Name each compound. (a) CCl4 (b) BCl3 (c) SF6 SOLUTION (a)The name of the compound is the name of the first element, carbon, followed by the base name of the second element, chlor, prefixed by tetra- to indicate four, and the suffix -ide. CCl4 carbon tetrachloride (b) The name of the compound is the name of the first element, boron, followed by the base name of the second element, chlor, prefixed by tri- to indicate three, and the suffix -ide. BCl3 boron trichloride (c) The name of the compound is the name of the first element, sulfur, followed by the base name of the second element, fluor, prefixed by hexa- to indicate six, and the suffix -ide. The entire name is sulfur hexafluoride. SF6 sulfur hexafluoride 95 EXAMPLE Naming Binary Acids Give the name of H2S(aq). The base name of S is sulfur, so the name is hydrosulfuric acid. SOLUTION H2S (aq) hydrosulfuric acid SKILLBUILDER | Naming Binary Acids Name HF(aq). Answer: hydrofluoric acid 96 EXAMPLE Naming Oxyacids Name HC2H3O2(aq). The oxyanion is acetate, which ends in -ate; therefore, the name of the acid is acetic acid. SOLUTION HC2H3O2(aq) acetic acid SKILLBUILDER | Naming Oxyacids Name HNO2(aq) Answer: nitrous acid 97 Conceptual Checkpoint An atom composed of which of these particles would have a mass of approximately 12 amu and be charge-neutral? (a) 6 protons and 6 electrons (b) 3 protons, 3 neutrons, and 6 electrons (c) 6 protons, 6 neutrons, and 6 electrons (d) 12 neutrons and 12 electrons Answer: (c) The mass in amu is approximately equal to the number of protons plus the number of neutrons. In order to be chargeneutral, the number of protons must equal the number of electrons. 98 Conceptual Checkpoint Which statement is NEVER true? (a) An element can be both a transition element and a metal. (b) An element can be both a transition element and a metalloid. (c) An element can be both a metalloid and a halogen. (d) An element can be both a main-group element and a halogen. Answer: (b) An element can be both a transition element and a metalloid. 99 Conceptual Checkpoint Carbon has two naturally occurring isotopes: and Using circles to represent protons and squares to represent neutrons, draw the nucleus of each isotope. 100 Conceptual Checkpoint If an atom with a mass number of 27 has 14 neutrons, it is an isotope of which element? (a) silicon (b) aluminum (c) cobalt (d) niobium Answer: (b) This atom must have (27 − 14) = 13 protons; the element with an atomic number of 13 is Al. 101 What is the charge on the electron, the proton, and the neutron, respectively? A. B. C. D. E. –1,+1,+1 –1,+1,–1 –1, 0,+1 –1,+1, 0 +1,+1, 0 102 What is the charge on the electron, the proton, and the neutron, respectively? A. B. C. D. E. –1,+1,+1 –1,+1,–1 –1, 0,+1 –1,+1, 0 +1,+1, 0 103 Which of the following subatomic particles has the least mass? A. B. C. D. E. Electron Neutron Proton Two of the above All of the above 104 Which of the following subatomic particles has the least mass? A. B. C. D. E. Electron Neutron Proton Two of the above All of the above 105 What subatomic particle(s) is/are found in the nucleus? A. B. C. D. E. Electron Neutron Proton Two of the above All of the above 106 What subatomic particle(s) is/are found in the nucleus? A. B. C. D. E. Electron Neutron Proton Two of the above All of the above 107 Which element has the chemical symbol “Pb”? A. B. C. D. E. Mercury Polonium Platinum Tungsten Lead 108 Which element has the chemical symbol “Pb”? A. B. C. D. E. Mercury Polonium Platinum Tungsten Lead 109 What is the chemical symbol for potassium? A. B. C. D. E. Po P Pt Pb K 110 What is the chemical symbol for potassium? A. B. C. D. E. Po P Pt Pb K 111 How many protons are in one silver atom? A. B. C. D. E. 47 60 94 108 154 112 How many protons are in one silver atom? A. B. C. D. E. 47 60 94 108 154 113 Which of the following elements is a metalloid? A. B. C. D. E. Aluminum Silicon Tin Phosphorus Iodine 114 Which of the following elements is a metalloid? A. B. C. D. E. Aluminum Silicon Tin Phosphorus Iodine 115 Which of the following elements is a metalloid? A. B. C. D. E. Arsenic Bismuth Carbon Iodine Gallium 116 Which of the following elements is a metalloid? A. B. C. D. E. Arsenic Bismuth Carbon Iodine Gallium 117 Strontium is in which of the following groups? A. B. C. D. E. Halogens Noble gases Alkaline earth metals Alkali metals Transition metals 118 Strontium is in which of the following groups? A. B. C. D. E. Halogens Noble gases Alkaline earth metals Alkali metals Transition metals 119 Chlorine is in which of the following groups? A. B. C. D. E. Halogens Noble gases Alkaline earth metals Alkali metals Transition metals 120 Chlorine is in which of the following groups? A. B. C. D. E. Halogens Noble gases Alkaline earth metals Alkali metals Transition metals 121 The sum of neutrons and protons in a given nucleus is referred to as the A. B. C. D. E. proton number. mass number. atomic number. isotope number. neutron number. 122 The sum of neutrons and protons in a given nucleus is referred to as the A. B. C. D. E. proton number. mass number. atomic number. isotope number. neutron number. 123 How many electrons are in the bromide ion? A. B. C. D. E. 35 36 46 70 80 124 How many electrons are in the bromide ion? A. B. C. D. E. 35 36 46 70 80 125 How many electrons, protons, and neutrons respectively are in the iron(III) ion, 56Fe3+? A. B. C. D. E. 23, 26, 30 26, 26, 30 26, 26, 56 26, 26, 26 29, 26, 30 126 How many electrons, protons, and neutrons respectively are in the iron(III) ion, 56Fe3+? A. B. C. D. E. 23, 26, 30 26, 26, 30 26, 26, 56 26, 26, 26 29, 26, 30 127 What is the symbol for an ion having 12 protons and 10 electrons? A. B. C. D. E. Si2+ Si Mg2+ Ne Ne2– 128 What is the symbol for an ion having 12 protons and 10 electrons? A. B. C. D. E. Si2+ Si Mg2+ Ne Ne2– 129 What is the symbol for an ion having 15 protons and 18 electrons? A. B. C. D. E. Ph3– Ar P3+ Cl– P3– 130 What is the symbol for an ion having 15 protons and 18 electrons? A. B. C. D. E. Ph3– Ar P3+ Cl– P3– 131 How many electrons are in the scandium ion, Sc3+? A. B. C. D. E. 45 42 48 24 18 132 How many electrons are in the scandium ion, Sc3+? A. B. C. D. E. 45 42 48 24 18 133 Which atom has the same number of protons as 59Ni? A. B. C. D. E. 59Fe 58Ni 59Co 141Pr 102Rh 134 Which atom has the same number of protons as 59Ni? A. B. C. D. E. 59Fe 58Ni 59Co 141Pr 102Rh 135 The nucleus of a fluorine-19 atom contains A. B. C. D. E. 19 protons and 19 electrons. 19 protons and 0 electrons. 9 protons and 10 electrons. 19 protons and 19 neutrons. 9 protons and 10 neutrons. 136 The nucleus of a fluorine-19 atom contains A. B. C. D. E. 19 protons and 19 electrons. 19 protons and 0 electrons. 9 protons and 10 electrons. 19 protons and 19 neutrons. 9 protons and 10 neutrons. 137 Which of the following species has 10 electrons and 14 neutrons? A. B. C. D. E. 27Al3+ 27Al 14N3– 24Mg2+ 20Ne 138 Which of the following species has 10 electrons and 14 neutrons? A. B. C. D. E. 27Al3+ 27Al 14N3– 24Mg2+ 20Ne 139 Isotopes have A. B. C. D. E. the same number of protons, but different numbers of neutrons. the same number of protons and neutrons. the same chemical symbol. the same number of electrons and neutrons. Two of the above 140 Isotopes have A. B. C. D. E. the same number of protons, but different numbers of neutrons. the same number of protons and neutrons. the same chemical symbol. the same number of electrons and neutrons. Two of the above 141 Which of the following is characteristic of metals? A. B. C. D. E. Solid at room temperature Malleable Ductile Located toward the left side of the periodic table All of the above 142 Which of the following is characteristic of metals? A. B. C. D. E. Solid at room temperature Malleable Ductile Located toward the left side of the periodic table All of the above 143 Which of the following is NOT a part of Dalton’s atomic theory? A. B. C. D. E. Each element is composed of small indestructible particles called “atoms.” Atoms of a given element are identical to each other. Matter is neither created nor destroyed. Atoms combine in simple, whole-number ratios to form compounds. All of the above are part of the atomic theory. 144 Which of the following is NOT a part of Dalton’s atomic theory? A. B. C. D. E. Each element is composed of small indestructible particles called “atoms.” Atoms of a given element are identical to each other. Matter is neither created nor destroyed. Atoms combine in simple, whole-number ratios to form compounds. All of the above are part of the atomic theory. 145 The nucleus of an atom contains a. b. c. d. protons and neutrons. protons and electrons. electrons and neutrons. protons, neutrons, and electrons. 146 The nucleus of an atom contains a. b. c. d. protons and neutrons. protons and electrons. electrons and neutrons. protons, neutrons, and electrons. 147 Two atoms with the same atomic number but different mass numbers are called a. b. c. d. mutants. isomers. isotopes. symbiots. 148 Two atoms with the same atomic number but different mass numbers are called a. b. c. d. mutants. isomers. isotopes. symbiots. 149 Select the incorrect statement about the mass and volume of an atom. a. The mass is determined mostly by the protons and neutrons. b. The volume is mostly empty space. c. The mass is concentrated in the nucleus. d. The volume is determined by the arrangement of the protons. 150 Select the incorrect statement about the mass and volume of an atom. a. The mass is determined mostly by the protons and neutrons. b. The volume is mostly empty space. c. The mass is concentrated in the nucleus. d. The volume is determined by the arrangement of the protons. 151 Metals and nonmetals react to form ________ compounds. a. b. c. d. molecular mixed empirical ionic 152 Metals and nonmetals react to form ________ compounds. a. b. c. d. molecular mixed empirical ionic 153 Positive ions are called a. b. c. d. positrons. anions. cations. nucleons. 154 Positive ions are called a. b. c. d. positrons. anions. cations. nucleons. 155 The elements located in Group VIIA (Group 17) on the periodic table are called a. b. c. d. alkali metals. noble gases. chalcogens. halogens. 156 The elements located in Group VIIA (Group 17) on the periodic table are called a. b. c. d. alkali metals. noble gases. chalcogens. halogens. 157 Which name is incorrectly paired with the formula? a. b. c. d. hydroxide ion; OH– barium(II) chloride; BaCl2 ammonia; NH3 sulfur dioxide; SO2 158 Which name is incorrectly paired with the formula? a. b. c. d. hydroxide ion; OH– barium(II) chloride; BaCl2 ammonia; NH3 sulfur dioxide; SO2 159 Acids produce _____ ions. a. b. c. d. OH–1 OH+1 H+1 H–1 160 Acids produce _____ ions. a. b. c. d. OH–1 OH+1 H+1 H–1 161 NaOCl is named a. b. c. d. sodium chlorate. sodium chlorite. sodium perchlorate. sodium hypochlorite. 162 NaOCl is named a. b. c. d. sodium chlorate. sodium chlorite. sodium perchlorate. sodium hypochlorite. 163 LiNO3 is named a. b. c. d. lithium nitrate. lanthanum nitrate. lanthanum nitrite. lithium nitrite. 164 LiNO3 is named a. b. c. d. lithium nitrate. lanthanum nitrate. lanthanum nitrite. lithium nitrite. 165 The formula for aluminum carbonate is a. b. c. d. Al2(CO3)3. AlCO3. Al2C3. Al3(CO3)2. 166 The formula for aluminum carbonate is a. b. c. d. Al2(CO3)3. AlCO3. Al2C3. Al3(CO3)2. 167 Fe2O3 is named a. b. c. d. diiron trioxide. iron(III) oxide. ferrous oxide. ironic oxide. 168 Fe2O3 is named a. b. c. d. diiron trioxide. iron(III) oxide. ferrous oxide. ironic oxide. 169 Which acid is not an oxyacid? a. b. c. d. hydrochloric acid nitric acid sulfurous acid acetic acid 170 Which acid is not an oxyacid? a. b. c. d. hydrochloric acid nitric acid sulfurous acid acetic acid 171 HIO4 is named a. b. c. d. iodic acid. iodous acid. periodic acid. hydrogen iodate. 172 HIO4 is named a. b. c. d. iodic acid. iodous acid. periodic acid. hydrogen iodate. 173 Cl2O7 is named a. b. c. d. chlorine(VII) oxide. dichlorine hexaoxide. dichlorine heptaoxide. bichlorine heptaoxide. 174 Cl2O7 is named a. b. c. d. chlorine(VII) oxide. dichlorine hexaoxide. dichlorine heptaoxide. bichlorine heptaoxide. 175 C3H8 is named a. b. c. d. ethane. propane. propanol. pentane. 176 C3H8 is named a. b. c. d. ethane. propane. propanol. pentane. 177