Chapter 9 Naming Ions

Monatomic Ions Ionic compounds consists of a positive metal ion and a negative nonmetal ion combined in a proportion such that their charges add up to a net charge of zero. NaCl – consists of one Na+ and one Cl-. Monatomic ions consists of a single atom with a positive or negative charge resulting from the loss or gain of one or more valence electrons.

Monatomic Ions - Cations Cations tend to lose valence electrons. (1+ charge – lose 1 electron, 2+ charge – lose 2 electrons, etc. ) When the metals in Groups 1A, 2A, and 3A lose electrons, they form cations with positive charges equal to their group number. The name of the cations of the Group 1A, 2A and 3A are the same as the name of the metal, followed by the word ion or cation. Na+ is sodium ion, Ca2+ is calcium ion, Al3+ is aluminum ion.

Monatomic Ions - Anions Nonmetals tend to gain electrons for form anions, so the charge of a nonmetallic ion is negative. The charge of any ion of a Group A nonmetal is determined by subtracting 9 from the group number. Group 7A form anions with a 1- charge (7-8 = -1) Anion names start with the stem of the element name and end in –ide. Anion of fluorine is fluoride ion (F-), anion of chlorine is chloride ion (Cl-)

Ions of Transition Metals Many of the transition metals (Group 1B – 8B) form more than one cation with different ionic charges. Two methods are used to name these ions. Stock System – a roman numeral in parentheses is placed after the name of the element to indicate the numerical value of the charge. Fe2+ is iron(II) ions Fe3+ is iron(III) ion. Classical – name of the element is used to form the root name for the element. Fe2+ is ferrous ion Fe3+ is ferric ions

Ag1+ silver Cd2+ cadmium Zn2+ zinc Au1+ gold(I) / aurous Au3+ gold(III) / auric Co2+ cobalt(II) / cobaltous Co3+ cobalt(III) /cobaltic Cr2+ chromium(II) / chromous Cr3+ chromium(III) /chromic Cu1+ copper(I) / cuprous Cu2+ copper(II) /cupric Fe2+ iron(II) / ferrous Fe3+ iron(III) / ferric Hg1+ mercury(I) / mercurous Hg2+ mercury(II) / mercuric Mn2+ manganese(II) Mn3+ manganese(III) Mn4+ manganese(IV) Ni2+ nickel(II) / nickelous Ni3+ nickel(III) / nickelic Pb2+ lead(II) /plumbous Pb4+ lead(IV) / plumbic

Polyatomic Ions Polyatomic Ions are composed of more than one atom. Sulfate ions (SO42-) is composed of one sulfur atom and four oxygen atoms. Polyatomic ions are a tightly bound group of atoms that behave as a unit and carry a charge. The names of most polyatomic anions end in –ite or –ate.

+1 CHARGE ion name NH4+ ammonium H3O+ hydronium Hg22+ mercury(I) -1 CHARGE ion name H2PO3- dihydrogen phosphite H2PO4- dihydrogen phosphate HCO3- hydrogen carbonate HSO3- hydrogen sulfite HSO4- hydrogen sulfate NO2- nitrite NO3- nitrate OH- hydroxide CH3COO- acetate

-1 CHARGE ion name CrO2- chromite CN- cyanide CNO- cyanate CNS- thiocyanate O2- superoxide MnO4- permanganate ClO- hypochlorite ClO2- chlorite ClO3- chlorate ClO4- perchlorate -1 CHARGE ion name BrO- hypobromite BrO2- bromite BrO3- bromate BrO4- perbromate IO- hypoiodite IO2- iodite IO3- iodate IO4- periodate AlO2- aluminate N3- azide

-2 CHARGE ion name HPO32- hydrogen phosphite HPO42- hydrogen phosphate CO32- carbonate SO32- sulfite SO42- sulfate S2O32- thiosulfate SiO32- silicate -2 CHARGE ion name C22- carbide C2O42- oxalate CrO42- chromate Cr2O72- dichromate C4H4O62- tartrate MoO42- molybdate O22- peroxide S22- disulfide

-3 CHARGE -4 CHARGE ion name PO33- phosphite P2O74- pyrophosphate PO43- phosphate PO23- hypophosphite AsO33- arsenite AsO43- arsenate

End of Section 9.1

Naming Binary Ionic Compounds A binary compound is composed of two elements and can be either ionic or molecular (covalent) To name any binary ionic compound, place the cation name first, followed by the anion name. Cs2O is cesium oxide NaBr is sodium bromide Cu2O is copper(I) oxide CuO is copper(II) oxide

Writing Formulas Binary Ionic Compounds Write the symbol of the cation and then the anion. Add whatever subscripts are needed to balance the charges. The positive charge of the cation must balance the negative charge of the anion so that the net ionic charge of the formula is zero. K+ + Cl-  KCl Ca2+ + Br-  CaBr2 Fe3+ + O2-  Fe2O3 Use the crisscross method – the numerical value of the charge of each ion is crossed over and becomes the subscript for the other ion.

Writing Formulas Polyatomic Ionic Compounds An –ate or –ite ending on the name of a compound indicates that the compound contains a polyatomic anion that includes oxygen. Write the symbol for the cation followed by the formula for the polyatomic ion and balance the charges. Ca2+ + NO3-  Ca(NO3)2 Sr2+ + SO32-  SrSO3 Li+ + CO32-  Li2CO3 Use the crisscross method – the numerical value of the charge of each ion (polyatomic too) is crossed over and becomes the subscript for the other ion.

Naming Polyatomic Ionic Compounds First recognize that the compound contains a polyatomic ion. State the cation first and then the anion NaClO sodium hypochlorite (NH4)2C2O4 ammonium oxalate Li2CO3 lithium carbonate

End of Section 9.2

Naming Molecular Compounds Binary ionic compounds are composed of the ions of two elements, a metal and a nonmetal. Binary molecular compounds are composed of two elements, two nonmetals and they are not ions. Binary molecular compounds are composed of molecules, not ions, so ionic charges cannot be used to write formulas or to name them. In addition, when two nonmetallic elements combine, the often do so in more than one way. (CO, CO2) Prefixes in the names of binary molecular compounds help distinguish compounds containing different amounts of the same two elements.

Naming Molecular Compounds The prefix in the name of a binary molecular compound tells how many atoms of each element are present in each molecule of the compound. Prefix Number mono- 1 di- 2 tri- 3 tetra- 4 penta- 5 hexa- 6 hepta- 7 octa- 8 nona- 9 deca- 10

Naming Molecular Compounds The names of all binary molecular compounds end in –ide. CO is carbon monoxide CO2 is carbon dioxide If just one atom of the first element is in the formula, omit the prefix mono- Name the elements in order listed in the formula Use prefixed to indicate the number of each kind of atom The suffix of the name of the second element is –ide. N2O is dinitrogen monoxide SF6 is sulfur hexafluoride.

Writing Formulas Molecular Compounds Use the prefixes in the name to tell you the subscript of each element in the formula. Then write the correct symbols for the two elements with the appropriate subscripts. Silicon Carbide SiC Dinitrogen tetraoxide N2O4 Diphosphorus trioxide P2O3

End of Section 9.3 End of Chapter 7

Naming Acids Acid is a compound that contains one or more hydrogen atoms and produces hydrogen ions (H+) when dissolved in water. When naming acids, the acid consists of an anion combined with as many hydrogen ions s are needed to make the molecule electrically neutral. The general chemical formulas of acids is HnX. X is a monatomic or polyatomic anion n is a subscript indication the number of hydrogen ions combined with the anion.

Naming Acids Three rules are used to name acids. The name depends on the name of the anion and its suffix (-ide, -ite, -ic) a. When the name of the anion ends in –ide, the acid name begins with the prefix hydro-. b. The stem of the anion has the suffix –ic and is followed by the word acid. H+ + Cl-  HCl Hydrogen ion chloride ion hydrochloric acid H+ + S2-  H2S Hydrogen ion sulfide ion hydrosulfuric acid

Naming Acids Three rules are used to name acids. The name depends on the name of the anion and its suffix (-ide, -ite, -ic) a. When the anion name ends in –ite, the acid name is the stem of the anion with the suffix –ous, followed by the word acid H+ + SO32-  H2SO3 Hydrogen ion sulfite ion sulfurous acid H+ + IO2-  HIO2 Hydrogen ion iodite ion iodous acid

Naming Acids Three rules are used to name acids. The name depends on the name of the anion and its suffix (-ide, -ite, -ic) a. When the anion name end in –ate, the acid name is the stem of the anion with the suffix –ic followed by the word acid. H+ + NO3-  HNO3 Hydrogen ion nitrate ion nitric acid H+ + SO42-  H2SO4 Hydrogen ion sulfate ion sulfuric acid

Writing Formulas for Acids Use the rules for writing the names of acids in reverse to write the formula for acids. Hydrobromic acid Hydro indicates the bromide ion HBr Phosphorous acid -ous indicates the phosphite ion H3PO3 Formic acid -ic and beginning with the anion name indicates the formate ion HCOOH

Bases A base is an ionic compound that produced hydroxide ions (OH-)when dissolved in water. Bases are named the same way as other ionic compounds – the name of the cation is followed by the name of the anion. NaOH is sodium hydroxide To write the formulas for bases, write the symbol for the cation followed by the formula for the hydroxide ion. (balance the ionic charges jusat as you do for any ionic compound) Aluminum hydroxide – Al3+ + OH-  Al(OH)3 Ammonium hydroxide – NH4+ + OH-  NH4OH

End of Section 9.4 End of Chapter 7

Laws Governing Formulas & Names Law of Definite Proportions A chemical formula tells you (by subscripts) the ratio of atoms of each element in the compound. Ratios of atoms can also be expressed as ratios of masses. 100 g of MgS breaks down into 43.12g Mg and 56.88g of sulfur. 100g MgS 1 mol MgS 1 mol Mg 24.305g Mg = 43.12g Mg 56.4g MgS 1 mol MgS 1 mol Mg 100g MgS 1 mol MgS 1 mol S 32.06g S = 56.88g S 56.4g MgS 1 mol MgS 1 mol S

Laws Governing Formulas & Names The ratios of these masses is 43.12/56.88 = 0.758:1 The mass ratio of 0.758:1 does not change no matter how the magnesium sulfide is formed or the size of the sample. Law of Definite proportions states that in samples of any chemical compound, the masses of the elements are always in the same proportions. MgS illustrates the law of definite proportions

Laws Governing Formulas & Names The Law of Multiple Proportions Water (H2O) and hydrogen peroxide (H2O2) are formed by the same two elements, they have different physical and chemical properties. Each compound obeys the law of definite proportions in every sample of hydrogen peroxide. (16g O : 1g H) In every sample of water, the mass ratio of O to H is always 8:1 (8g O: 1g H) If a sample of H2O2 has the same mass of H as a sample of H2O, the ratio of the mass of O in the two compounds is exactly 2:1

Laws Governing Formulas & Names 16 g O (in H2O2 has 1g H) = 16 = 2 = 2:1 8 g O (in H2O has 1 g H) 8 1 Law of multiple proportions states that whenever the same two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers.

End of Chapter 9