Ionic Compounds and Ionic Bonding. Periodic Table Review. Slide 1 / 130 Slide 2 / 130. Slide 4 / 130. Slide 3 / 130. Slide 6 / 130.

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1 Slide 1 / 130 Slide 2 / 130 Ionic ompounds and Ionic onding Slide 3 / 130 Slide 4 / 130 Table of ontents: Ionic ompounds and Ionic onding Periodic Table Review Valence lectrons and the Octet Rule Ions Ionic onding Properties of Ionic ompounds Predicting an Ionic ompound's Formula Naming Ionic ompounds lick on the topic to go to that section Formulas and Names of Ionic ompounds with Transition Metals Polyatomic ions Formula and Names of ompounds with Polyatomic ions (Ternary Ionic ompounds) Polyatomic Patterns Periodic Table Review Return to Table of ontents Slide 5 / 130 Periodic Table - Review The periodic table is "periodic" because of certain trends that are seen in the elements. Some of these trends can be seen in the properties of atoms we covered in the last unit: atomic size, ionization energy, electronegativity and metallic character. Would you predict that elements from the same family/group would have similar physical and chemical properties? Slide 6 / 130 The Periodic Table of the lements The periodic table can be divided into three large classifications of elements. What type of elements are highlighted in blue, in yellow and in pink? What is unique about the elements that are highlighted in pink? Si Ge s Sb Te?

2 Slide 7 / 130 Slide 8 / 130 Metallic haracter of the lements What the relationship between metallic character and effective nuclear charge? re they directly or inversely related? Is it accurate to say "lement is more metallic than element " even if element is a non-metal? More metallic Less metallic Non-metallic Si Ge s Sb Te? 1 In the periodic table, the elements are arranged in. alphabetical order order of increasing atomic number order of increasing metallic properties order of increasing neutron content F reverse alphabetical order I don't know how to answer this. Most metallic Slide 8 () / In the periodic table, the elements are arranged in. alphabetical order order of increasing atomic number order of increasing metallic properties order of increasing neutron content F reverse alphabetical order I don't know how to answer this. Slide 9 / lements exhibit similar physical and chemical properties. with similar chemical symbols with similar atomic masses in the same period of the periodic table on opposite sides of the periodic table in the same group of the periodic table Slide 9 () / lements exhibit similar physical and chemical properties. with similar chemical symbols with similar atomic masses in the same period of the periodic table on opposite sides of the periodic table in the same group of the periodic table Slide 10 / Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? Li, Na s, a a, Si Ga, Ge, O

3 Slide 10 () / Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? Li, Na s, a a, Si Ga, Ge, O Slide 11 / Which one of the following is a nonmetal? W Sr Os Ir S Slide 11 () / Which one of the following is a nonmetal? W Sr Os Ir S Slide 12 / Potassium is a and chlorine is a. metal, nonmetal metal, metal metal, metalloid metalloid, nonmetal nonmetal, metal Slide 12 () / 130 Slide 13 / Potassium is a and chlorine is a. metal, nonmetal metal, metal metal, metalloid metalloid, nonmetal nonmetal, metal Valence lectrons and the Octet Rule Return to Table of ontents

4 Slide 14 / 130 Review: Octet Rule toms tend towards having complete outer shells of electrons (remember stability). full outer shell will have: 2 electrons in the s subshell and 6 electrons in the p subshell ( s 2 p 6 configuration) Octet rule: atoms tend towards having a total of 8 electrons Slide 15 / 130 Valence lectrons Valence electrons are the electrons in the highest occupied energy level of an element s atoms. The valence electrons determine the chemical properties of an element. Why do you think this would be true? Valence electron 8 valence electrons make an octet Which elements on the periodic table have a complete outer shell? What is true about these elements relative chemical reactivity? To find the number of valence electrons in an atom of a representative element (elements found in the s and p blocks), simply look at its group number. toms in group 3 have 3 valence electrons, atoms in group 17 have 7 valence electrons, etc. Slide 16 / 130 Valence lectrons Number of valence 1 2 electrons in neutral atoms: Slide 17 / How many valence electrons does potassium have? There is one exception: helium has only 2 valence electrons. Slide 17 () / How many valence electrons does potassium have? Slide 18 / How many valence electrons does luminum have?

5 Slide 18 () / How many valence electrons does luminum have? Slide 19 / How many valence electrons does arium have? Slide 19 () / How many valence electrons does arium have? Slide 20 / rsenic (s) has 6 valence electrons. True False Slide 21 / 130 Slide 22 / 130 Ions Ions Ions are atoms or groups of atoms that have become charged by either gaining or losing electrons. ations are positive and are formed by elements on the left side of the periodic chart (metals). nions are negative and are formed by elements on the right side of the periodic chart (nonmetals). Return to Table of ontents

6 Slide 23 / 130 Slide 24 / 130 The Formation of ations The Formation of ations Metals usually give up/lose valence electrons to become more stable. This often results in a noble gas (8 electron) outer shell. Na atom Na+ ion Na : 1s 2 2s 2 2p 6 3s 1 Na +1 : 1s 2 2s 2 2p 6 Ne atom loses e- 3s 2p 2s 1s Loss of valence electrons 11p 11e- 11p 10e- How many electrons does the Na + ion have? The Na + ion is smaller than the Na atom. o you remember what factors cause this reduction in size? Slide 25 / 130 The Formation of ations ations of Group 1 elements always have a charge of 1+. ations of Group 2 elements always have a charge of 2+. Slide 26 / 130 The Formation of nions Nonmetals usually gain valence electrons. This results in a noble gas (8 electrons) outer shell l: 1s2 2s2 2p6 3s2 3p5 l - 1s2, 2s2, 2p6, 3s2, 3p6 r atom 3p Mg Mg e - Magnesium atom (electrically neutral, charge = 0) Magnesium ion (+2 indicates 2 units of positive charge) (2 in front of e - indicates 2 units of negative charge) 3s 2p 2s How many electrons does the l - have? Slide 27 / 130 The Formation of nions Slide 28 / 130 The Formation of nions l atom l - ion nions of Group 15 (5) elements always have a charge of 3 - nions of Group 16 (6) elements always have a charge of 2-17P 17e - Gains an e- 17p 18e - The l - ion is larger than the l atom. o you remember what factors cause this increase in size? nions of Group 17 (7) elements always have a charge of 1 - onsider Group 14 (4) elements, what common charge(s) would you predict for these elements?

7 Slide 29 / Metals tend to electrons and nonmetals tend to electrons. Slide 29 () / Metals tend to electrons and nonmetals tend to electrons. gain, gain lose, lose gain, lose lose, gain neither, they keep their electrons gain, gain lose, lose gain, lose lose, gain neither, they keep their electrons Slide 30 / nions tend to be and cations tend to be. metals, metals nonmetals, nonmetals metals, nonmetals Slide 30 () / nions tend to be and cations tend to be. metals, metals nonmetals, nonmetals metals, nonmetals nonmetals, metals metalloids, metalloids nonmetals, metals metalloids, metalloids Slide 31 / Metals lose electrons to form cations True False Slide 31 () / Metals lose electrons to form cations True False True

8 Slide 32 / nions are formed from nonmetals True False Slide 32 () / nions are formed from nonmetals True False True Slide 33 / Nonmetals tend to lose electrons forming ions True False Slide 33 () / Nonmetals tend to lose electrons forming ions True False False Slide 34 / This is the ion formed from a calcium atom a + a 2+ Slide 34 () / This is the ion formed from a calcium atom a + a 2+ a - a 2- a - a 2-

9 Slide 35 / 130 Slide 35 () / Phosphorous forms an ion with a charge of Phosphorous forms an ion with a charge of Slide 36 / 130 Slide 36 () / luminum forms an ion with a charge of luminum forms an ion with a charge of Slide 37 / 130 Slide 37 () / Of the following, contains the greatest number of electrons. 18 Of the following, contains the greatest number of electrons. P 3+ P P 2- P 3+ P P 2- P 3- P 2+ P 3- P 2+

10 Slide 38 / Oxygen forms an ion with a charge of Slide 38 () / Oxygen forms an ion with a charge of Slide 39 / Iodine forms an ion with a charge of Slide 39 () / Iodine forms an ion with a charge of Slide 40 / This is the ion formed from nitrogen N - N 2- N 3+ Slide 40 () / This is the ion formed from nitrogen N - N 2- N 3+ N 3- N 3-

11 Slide 41 / Predict the charge of the most stable ion of S? Slide 41 () / Predict the charge of the most stable ion of S? Slide 42 / What would be the expected charge on the gallium (Ga) ion? Slide 42 () / What would be the expected charge on the gallium (Ga) ion? Slide 43 / 130 Slide 44 / 130 Introduction to hemical onds There are three basic types of bonds: Ionic onding Ionic - The electrostatic attraction between ions ovalent - The sharing of electrons between atoms Metallic - ach metal atom bonds to other metals atoms within a "sea" of electrons (covered in a later unit) Return to Table of ontents

12 Slide 45 / 130 Ionic onding Slide 46 / 130 Ionic onding lectronegativity is how strongly an atom attracts electrons. toms with a high electronegativity will be able to attract electrons away from atoms with a much lower electronegativity. Neutral atom 1 valence electron Low lectronegativity + ation This removal of electrons can occur when the difference in electronegativity between the two atoms is approximately 1.7 or higher. Once a positive and negative ion are formed, they will be attracted to each other via the electrostatic force: F = k q 1 q 2 r 2 Note: The heavier nonmetals from 4,6,5th groups ( In, Tl, Sn, Pb, Sb i ) may act like metals Neutral atom 7 valence electrons High lectronegativity - nion The atom with high electronegativy attracts valence electrons from the atom with lower electronegativity. When the atoms become oppositely charged ions the electrostatic force of attraction brings them together. lectrostatic force of attraction = bond F = k q1 q2 r 2 Slide 47 / 130 Slide 48 / 130 Ionic onding ompounds composed of cations and anions are called ionic compounds. lthough they are composed of ions, ionic compounds are electrically neutral. Ionic onds When sodium and chlorine are close together, sodium's valence electron flies off and "harpoons" the chlorine atom. The result is a sodium cation (+) next to a chloride anion (-) These oppositely charged two ions attract: they reel one another together to form an ionic bond. The electrostatic forces that hold ions together in ionic compounds are called ionic bonds. Na l Na+ l- 1s 2 2s 2 2s 2 2p 6 3s 1 1s 2 2s 2 2p 6 3s 2 3p 5 1s 2 2s 2 2p 6 1s 2 2s 2 2p 6 3s 2 3p 6 1s 2 2s 2 2p 6 1s 2 2s 2 2p 6 3s 2 3p 6 Ne r Slide 49 / 130 Slide 50 / 130 Ionic onds The electron transfer process in creating an ionic bond: Na l The dots represents the valence electrons in an atom. click here for an animation of this reaction

13 Slide 51 / 130 Slide 51 () / 130 Slide 52 / 130 Slide 52 () / 130 Slide 53 / 130 Slide 53 () / 130

14 Slide 54 / Which of the following compounds would you expect to be ionic? Slide 54 () / Which of the following compounds would you expect to be ionic? H2 O O2 H2 O O2 Srl2 Srl2 SO2 H2S SO2 H2S Slide 55 / 130 Slide 56 / 130 [*] Properties of Ionic ompounds Properties of Ionic ompounds They are crystalline solids at room temperature They have high melting points They conduct electricity when melted (molten) or dissolved in water (aqueous) Return to Table of ontents Slide 57 / 130 Slide 58 / 130 Formula Units chemical formula shows the kinds and numbers of atoms in the smallest representative unit of a substance. formula unit is the lowest whole-number ratio of ions in an ionic compound. Predicting an Ionic ompound's Formula very ionic compound has a 3 array of positive and negative ions. Return to Table of ontents

15 Slide 59 / 130 Predicting an Ionic ompound Formula Potassium (K) with an electronegativity of 0.8 and oxygen (O) with an electronegativity of 3.5 will form an ionic compound. What is the formula for an ionic compound of potassium and oxygen? Slide 60 / 130 Predicting an Ionic ompound Formula What is the formula for an ionic compound of Mg and N? How many additional valence electrons does N want? 3 K How many additional valence electrons does oxygen want? 2 How many valence electrons does potassium have? 1 How many potassium atoms will it take to give oxygen the electrons it needs? 2 K O The formula unit is K2 O lways Metal First (low electonegativity) Slide 61 / 130 Mg Mg Mg How many valence electrons does Mg have to offer? 2 How many Mg atoms will it take to give how many N the electrons it needs? (Find the lowest common multiplier first.) N N 3 Mg : 2 N The formula unit is Mg 3 N 2 Slide 62 / 130 lternate Method If you don't like finding least common multipliers, you can use this alternative method: 1. Write down the ions side by side along with their charge. lways write the metal first. 2. "riss-cross" the numerical values of the charges. 3. Reduce subscripts to lowest ratio. Mg Mg Mg N N Slide 63 / 130 Predicting an Ionic ompound Formula What is the compound formed between Mg and S? Mg +2 S -2 Mg2S2 The chemical formula would have to be the lowest ratio of ions. What would you predict would be the formula for this compound? Predicting an Ionic ompound Formula xample: Write the formula for calcium sulfide. Step 1: Identify the cation & write its common ion alcium is in group 2 a 2+ Step 2: Identify the anion & write its formula Sulfur is in group 6 S 2- Step 3: riss-cross; reduce subscripts if necessary a 2+ S 2- a2s2 as Slide 64 / The formula for the ionic compound between s and O is: so2 Os 2 s2o Os 2 I don't know how to do this. MgS Move for

16 Slide 64 () / The formula for the ionic compound between s and O is: so2 Os 2 s2o Os 2 I don't know how to do this. Slide 65 / The ionic compound formed between a and N is: an a 2N 2 a 3N 2 a 2N 3 I don't know how to do this. Slide 65 () / The ionic compound formed between a and N is: an a 2N 2 a 3N 2 a 2N 3 I don't know how to do this. Slide 66 / The ionic compound formed between l and O l 3O 2 l 2O 3 lo l 2O 2 I don't know how to do this. Slide 66 () / The ionic compound formed between l and O l 3O 2 l 2O 3 lo l 2O 2 I don't know how to do this. Slide 67 / What is the ionic compound formed between a and l? al a3l2 l 2a 3 No compound is formed.

17 Slide 67 () / 130 Slide 68 / What is the ionic compound formed between a and l? al a3l2 l 2a 3 No compound is formed. 32 What is the ionic compound formed between P and r? P 3 r rp This compound is not considered ionic (rp) 2 I don't know how to do this. Slide 68 () / 130 Slide 69 / What is the ionic compound formed between P and r? 33 What is the formula for sodium phosphide? P 3 r rp SP 3 NaP This compound is not considered ionic (rp) 2 I don't know how to do this. Na 3 P NaP 3 I don't know how to do this. Slide 69 () / 130 Slide 70 / What is the formula for sodium phosphide? 34 What is the formula for strontium bromide? SP 3 Srr NaP Na 3 P NaP 3 I don't know how to do this. Srr 2 Sr 2 r rsr 2

18 Slide 70 () / What is the formula for strontium bromide? Srr Srr 2 Sr 2 r rsr 2 Slide 71 / The formula for barium sulfide is a2s2. True False Slide 71 () / 130 Slide 72 / The formula for barium sulfide is a2s2. True False Naming Ionic ompounds False Slide 73 / 130 Naming inary Ionic ompounds - ations Many cations have the same name as the original, neutral atom. harge Formula Name +1 H + Li + K + s + g + Hydrogen ion Lithium ion Potassium ion esium ion Silver ion Slide 74 / 130 Return to Table of ontents Naming inary Ionic ompounds - nions ll monoatomic anions end in "-ide". The ions that are produced from Group 7 (or 17) elements are called halide ions. an you guess the origin of the name halides? Group 15 Group 16 Group Mg 2+ a 2+ a 2+ d 2+ l 3+ Magnesium ion alcium ion arium ion admium ion luminum ion Nitride N 3- Phosphide P 3- Sulfide S 2- hloride l - Oxide O2- Fluoride F- romide r - Iodide I -

19 Slide 75 / 130 Naming inary Ionic ompounds inary (two-element) compounds are named by writing the name of the cation followed by the name of the anion. The name of the cation is the same as the metal name. The name of the anion is the name of the non-metal with the suffix changed to -ide. Slide 76 / The correct name for Na2S is Sodium sulfate Sodium sulfide i-sodium sulfide Sulfur nitride inary ionic compounds end in "-ide." xamples: Nal = sodium chloride KI = Li2 S = potassium iodide Move for lithium sulfide Slide 76 () / 130 Slide 77 / The correct name for Na2S is Sodium sulfate Sodium sulfide i-sodium sulfide Sulfur nitride 37 The correct name for SrO is. strontium oxide strontium hydroxide strontium peroxide strontium monoxide strontium dioxide Slide 77 () / 130 Slide 78 / The correct name for SrO is. 38 The correct name for l2o3 is. strontium oxide strontium hydroxide strontium peroxide strontium monoxide strontium dioxide aluminum trioxide dialuminum oxide dialuminum trioxide aluminum oxide aluminum hydroxide

20 Slide 78 () / 130 Slide 79 / The correct name for l2o3 is. aluminum trioxide dialuminum oxide dialuminum trioxide aluminum oxide aluminum hydroxide Names and Formulas of Ionic ompounds with Transition Metals Slide 80 / 130 ations formed by Transition lements Slide 81 / 130 Return to Table of ontents ations formed by Transition lements Recall that s-block metals and some p block elements like aluminum have only one possible ionic charge, based on the Octet Rule. However, most transition metals (d block elements) can have more than one ionic charge. For this reason, there is a system for designating the charge on each ion , , Si Ge s ,+3 +2,+4 Sb Te? Sn, Pb from the p-block are called post-transition metals and will form more than one type of ion and behave like transition metals. The 2+ charge is very common among the transition metals as they lose their two "s" electrons first, before losing others from their "d" orbital Slide 82 / 130 ations Formed by Transition lements Slide 83 / 130 Silver, Zinc, and admium Ions Why do these ions only have one possible charge? Let's look at their electron configurations. Only common transition metals are shown. Silver, cadmium and zinc only form one cation, g +, d 2+ and Zn 2+ Note the two mercury cations, which one is a polyatomic ion? Tin (Sn) and Lead (Pb) act like transition metals and they share two common charges, why do you think this is true? The "d" orbital of both zinc and cadmium are full and therefore very stable so the only electrons it will lose are the two "s" electrons... Zn: [r]4s 2 3d 10 Zn 2+ : [r]3d 10 The "d" orbital is also full with silver as it has largely taken an electron from it's own "s" orbital to make stabilize the "d" orbital. Therefore, it only has 1 electron left to lose. g: [Kr]5s 1 4d 10 g + : [Kr]4d 10

21 Slide 84 / 130 ations formed by Transition lements We will use the Stock naming system (Roman numerals) to name transition metals. Slide 85 / 130 Writing Formulas with Transition Metals The charge on the cation is indicated by the Roman numeral, as shown in this example. Formula Name u opper (I) ion +1 Iron (III) oxide Fe 3+ O 2- Write ion formulas. o +2 Fe +2 Mn +2 Pb +2 r +3 Fe +3 obalt (II) ion Iron (II) ion Manganese (II) ion lead (II) ion hromium (III) ion Iron (III) ion Fe 3+ O 2- Fe2 O3 riss-cross charges. Reduce if necessary. What would be the names of u 2+ and Mn 7+? Slide 86 / 130 Writing Formulas with Transition Metals The charge on the cation is indicated by the Roman numeral, as shown in this example. Tin (IV) oxide Sn 4+ O 2- Write ion formulas. Slide 87 / Which metal is capable of forming more than one cation? K s a l Sn Sn 4+ O 2- riss-cross charges. Sn2O4 SnO2 Reduce if necessary. Slide 87 () / Which metal is capable of forming more than one cation? K s a l Sn Slide 88 / Which metal is not capable of forming more than one cation? u u Fe Sn l

22 Slide 88 () / Which metal is not capable of forming more than one cation? u u Fe Sn l Slide 89 / 130 Formulas with Transition Metals In order to correctly name a formula containing a transition metal, it is necessary to first determine the charge on the cation. Since all compounds are neutral, then the total positive cation charge must equal the total negative anion charge. In other words: Total cation charge + Total anion charge = 0 (charge of cation) (# of cations) + (charge of anion) (# of anions) = 0 Slide 90 / 130 xample Formula with Transition Metals In the case of Fel3, we make the following substitutions: Slide 91 / 130 Formulas with Transition Metals short cut method is to "uncriss-cross" the ions, but you must always double check your ions (or you'll get in trouble!). (charge of cation) (# of cations) +(charge of anion) (# of anions) = 0 Fel3: Fe1 l3 Uncriss-cross. (x) (1) + (-1) (3) = 0 Thus x = 3 and the cation is Fe 3+ or iron(iii). heck the ions Fe 3+ l 1- l does form a 1-ion and Fe is Iron (III) 3+ Iron (III) loride Slide 92 / 130 Formulas with Transition Metals 41 The name of Fel3 is Slide 93 / 130 ro: Here's another practice problem. r 1 O 1 Uncriss-cross. heck the ions iron chloride iron (II) chloride iron (III) chloride iron(i)chloride r + O - O forms a 2- ion and r+ does not exist! (this formula had to be reduced from r 2 O 2 ) hromium (II) Oxide

23 41 The name of Fel3 is Slide 93 () / 130 Slide 94 / The correct formula for tin (IV) oxide is: iron chloride iron (II) chloride iron (III) chloride iron(i)chloride SnO 2 SnO Sn 4O 4 Sn 4O 2 SnO 2 Slide 94 () / The correct formula for tin (IV) oxide is: Slide 95 / The formula for copper (II) sulfide is SnO 2 SnO Sn 4O 4 Sn 4O 2 SnO 2 us2 us u2 S2 (us)2 u 2S Slide 95 () / The formula for copper (II) sulfide is us2 us u2 S2 (us)2 u 2S Slide 96 / Which one of the following compounds is copper(i) chloride? ul ul2 u 2l u 2l 2 u 3l 2

24 Slide 96 () / Which one of the following compounds is copper(i) chloride? Slide 97 / The charge on the cation in the salt Fe2O3 is. ul ul2 u 2l u 2l 2 u 3l Slide 97 () / The charge on the cation in the salt Fe2O3 is [*] Slide 98 / What is the charge on zirconium ion in ZrO2? Slide 98 () / 130 Slide 99 / 130 [*] 46 What is the charge on zirconium ion in ZrO2? The correct name of the compound V 2O 3 is vanadium(ii)oxide. True False

25 Slide 99 () / The correct name of the compound V 2O 3 is vanadium(ii)oxide. True False Slide 100 / The correct name for u 3N is: copper nitride copper (I) nitride copper (II) nitride copper(iii)nitride copper(iii) nitrogen False: Vanadium (VI) oxide Slide 100 () / 130 Slide 101 / The correct name for u 3N is: copper nitride copper (I) nitride copper (II) nitride copper(iii)nitride copper(iii) nitrogen Polyatomic Ions Slide 102 / 130 Return to Table of ontents Slide 103 / 130 Polyatomic Ions polyatomic ion is a group of atoms bonded together that have a charge and acts like a single unit or ion. They are not free compounds and like other ions, are not found free in nature. They are found combined with other ions. Sulfate = (SO 4) 2- Nitrate = (NO 3) - arbonate = (O 3) 2- Polyatomic Ions Most of the polyatomic ions contain oxygen atoms. Many anions names end with -ite or -ate In ite/ate pairs, the ion with fewer oxygen atoms will have the ite ending xamples: sulfite /sulfate nitrite /nitrate Note that the suffix does not indicate the actual number of O atoms. Use ( ) to keep the atoms together. o not change the subscripts inside the "( )"

26 . Slide 104 / 130 Polyatomic Ions Familiarize yourself with the polyatomic ions on your reference sheet e careful of -ide, -ite, and -ate! H + = proton or hydrogen ion ] Slide 105 / 130 Formulas and Names of Ionic ompounds with Polyatomic Ions (Ternary Ionic ompounds) or bicarbonate Slide 106 / 130 Writing Formulas for Ternary Ionic ompounds Ternary ionic compounds, compounds that contain 3 or more elements, are neutral, just like binary ionic compounds. Therefore, the goal is to find the lowest ratio of cations to anions that will yield a neutral compound. This ratio is represented in a formula unit. xamples of formula units Slide 107 / 130 Return to Table of ontents Writing Formulas for Ternary Ionic ompounds (con't) To write a formula, the criss-cross method can again be used. xample: Write the formula for lithium phosphate. Step 1: Identify the cation & write its formula Lithium is in group 1 --> Li + Step 2: Identify the anion & write its formula Phosphate is a polyatomic ion --> PO 4 3- ao3 gno3 Zn(2H3O2)2 Na2SO3 Step 3: riss-cross; reduce subscripts if necessary Li 1+ PO 4 3- Li 3(PO 4) 1 or simply Li 3(PO 4) Slide 108 / 130 Writing Formulas for Ternary Ionic ompounds xample: Write the formula for calcium nitrite. a 2+ (NO 3) - a(no3)2 When writing formulas with polyatomic ions, there are two important things to remember: 1) It is helpful to use " ( ) " to keep the atoms together, keeping the charge OUTSI the ( ) For example: nitrate (NO3) 1- carbonate (O 3) 2- Slide 109 / 130 Writing Formulas for Ternary Ionic ompounds xample 1: Write the formula for lithium chlorate. Li +1 (lo 3) -1 = Li(lO 3) = LilO 3 Move for Note: The ( ) are removed because only 1 chlorate ion is present. xample 2: Write the formula for manganese(iii) carbonate. Mn 3+ (O 3) 2- = Mn 2(O 3) 3 Move for Note: The ( ) are needed here because more than one carbonate ion are present 2) NVR alter any symbols or subscripts INSI the "( )". Once finished, if there is no subscript outside of the "( )", remove the "( )"

27 Slide 110 / The formula for aluminum phosphate is: Slide 110 () / The formula for aluminum phosphate is: lpo4 lpo4 l3(po4) l3(po4) l2(po4)3 l2(po4)3 l3(po4)3 l3(po4)3 Slide 111 / What would be the correct formula for cobalt(iii) carbonate? o 3O 3 o 2O 3 o 2(O 3) 3 Slide 111 () / What would be the correct formula for cobalt(iii) carbonate? o 3O 3 o 2O 3 o 2(O 3) 3 o 3(O 3) 2 oo 3 o 3(O 3) 2 oo 3 Slide 112 / The formula for sodium hydroxide is Slide 112 () / The formula for sodium hydroxide is Na (OH)2 Na (OH)2 NaOH NaOH Na(OH2) Na(OH2) Na(HO) Na(HO) NaOH2 NaOH2

28 Slide 113 / The formula for calcium sulfate is Slide 113 () / The formula for calcium sulfate is aso4 aso4 a2(so4)2 a(so3) a2(so3)2 as a2(so4)2 a(so3) a2(so3)2 as Slide 114 / 130 Slide 114 () / How many nitrate ions are present in the formula of aluminum nitrate? (Write the formula first to find out.) How many nitrate ions are present in the formula of aluminum nitrate? (Write the formula first to find out.) : l(no 3) 3 Slide 115 / How many total ions (cations and anions) are present in the formula of lithium acetate? Slide 115 () / How many total ions (cations and anions) are present in the formula of lithium acetate? : Li( 2H 2O 2)

29 Slide 116 / 130 PRTI Writing Formulas for Ionic ompounds omplete the table by filling in the formula for the ionic compound formed by each pair of cations and anions, as shown for the first pair. Slide 117 / 130 PRTI Writing Formulas for Ternary Ionic ompounds Write the formula for the following compounds: 1. Magnesium iodide MgI 2 2. alcium sulfite aso 3 3. arium hydrogen carbonate a(ho 3) 2 Move for answer 4. Iron (III) phosphate FePO 4 Slide 118 / 130 Naming Ternary Ionic ompounds Ternary ionic compounds contain three or more different elements due to the presence of polyatomic ion(s). Just as in binary ionic compounds, the name of the cation is given first, followed by the name of the anion. Names of ternary compounds often end in -ite or -ate. xamples Slide 119 / The correct name for NalO is sodium chlorate sodium chloride sodium chlorite sodium chloride oxide sodium hypochlorite ao3 Zn(2 H3 O2)2 gno3 Na2 SO3 calcium carbonate zinc acetate silver Move nitrate for sodium answer sulfite Slide 119 () / 130 Slide 120 / The correct name for NalO is 56 Mg(HO3)2 is sodium chlorate sodium chloride sodium chlorite sodium chloride oxide sodium hypochlorite Magnesium carbonate Magnesium hydrogen carbonate Magnesium hydroxide Magnesium carboxide Magnesium dibicarbonate

30 56 Mg(HO3)2 is Slide 120 () / 130 Magnesium carbonate Magnesium hydrogen carbonate Magnesium hydroxide Magnesium carboxide Magnesium dibicarbonate Slide 121 / mmonium carbonate is NH4 O3 (NH4)2O3 NH4(O3)2 (NH4)2O2 Slide 121 () / 130 Slide 122 / mmonium carbonate is NH4 O3 (NH4)2O3 NH4(O3)2 (NH4)2O2 Naming Ternary Ionic ompounds If the formula involves a transition or post transition element, you must first deduce the charge so it can be included in the name. For example: Name u 2O 3 For example: Name Ni(NO 3) 2 1. Un-criss cross the charges. 1. Un-criss cross the charges. u 2 (O 3) Ni (NO 3) 2 2. u carries a +1 charge 2. Ni carries a +2 charge So... this compound is called copper(i) carbonate So... this compound is called nickel(ii) nitrate Move for answer Slide 123 / What would be the proper name for Ga 2(SO 3) 3? gallium sulfite gallium (I) sulfite gallium (III) sulfite gallium (III) sulfate Slide 123 () / What would be the proper name for Ga 2(SO 3) 3? gallium sulfite gallium (I) sulfite gallium (III) sulfite gallium (III) sulfate Note: Gallium is not a transition metal so it's charge is known and therefore should Move not be for written. explanation Note: Gallium is not a transition metal so it's charge is known and therefore should Move not be for written. explanation

31 Slide 124 / Which would be the correct name for uf 3? gold (I) flouride gold(iii) flouride gold flouride gold flourine gold triflouride Slide 124 () / Which would be the correct name for uf 3? gold (I) flouride gold(iii) flouride gold flouride gold flourine gold triflouride Note: Gold is a transition metal so it's charge is not known. Move for explanation You must deduce it and it should be written. Move for explanation Note: Gold is a transition metal so it's charge is not known. You must deduce it and it should be written. Slide 125 / What would be the correct name for Sn(O 3) 2? tin carbonate tin(ii) carbonate tin carbide tin tetracarbonate tin (IV) carbonate Slide 125 () / What would be the correct name for Sn(O 3) 2? tin carbonate tin(ii) carbonate tin carbide tin tetracarbonate tin (IV) carbonate Slide 126 / 130 Slide 127 / 130 Polyatomic Patterns Tips for remembering polyatomic ions using patterns: oron, arbon, and Nitrogen polyatomic ions have a maximum of 3 oxygens. Polyatomic Patterns orate O 3 3- arbonate O 3 2- Nitrate NO 3 1- orite O 2 3- arbonite O 2 2- Nitrite NO 2 1- harges: Return to Table of ontents

32 Slide 128 / 130 Polyatomic Patterns Tips for remembering polyatomic ions using patterns: Phosphorus and Sulfur polyatomic ions have a maximum of 4 oxygens. Phosphate PO 4 3- Sulfate SO 4 2- Phosphite PO 3 3- Sulfite SO 3 2- harges: -3-2 Slide 129 / 130 Polyatomic Patterns Tips for remembering polyatomic ions using patterns: ll of the halogens follow the same naming pattern: Per-ate = 4 oxygens, ---ate = 3 oxygens, ---ite = 2 oxygens, --- hypo-ite = 1 oxygen. Perchlorate lo 4 1- hlorate lo 3 1- hlorite lo 1-2 harge: -1 Hypochlorite lo 1- Slide 130 / 130