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Types of Compounds

Types of Compounds. Chapter 5. Objectives 5.1. 5.1 Apply ionic charge to writing formulas 5.1 Apply formulas to name ionic compounds 5.1 Interpret the information in a chemical formula. Ionic “Bonds”. Instead of Formula’s: Ratio’s

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Types of Compounds

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  1. Types of Compounds Chapter 5

  2. Objectives 5.1 • 5.1 Apply ionic charge to writing formulas • 5.1 Apply formulas to name ionic compounds • 5.1 Interpret the information in a chemical formula

  3. Ionic “Bonds” • Instead of Formula’s: Ratio’s • Some atom’s want more electrons than the other wants to give up • So they bind to two, or three • Example: Li and O, Li wants to give up only 1 electron, but O wants 2 electrons

  4. Practice Question • What ratio of Mg and N are needed to make an Ionic compound that has a neutral charge? • Draw a Lewis electron dot diagram for N • Draw a Lewis electron dot diagram for Mg • What ratio of Na and Br are needed to make an Ionic compound that has a neutral charge?

  5. +1 +2 General Ionic Charges -3 -2 -1

  6. Ionic Nomenclature • Only use Ionic Nomenclature when dealing with Ionic compounds • An ionic compound is formed when a metal and a non metal come together and electrons are completely lost and gained

  7. Fixed Oxidation State • Some Metals will always lose the same amount of electrons. These metals have Fixed Oxidation States • Alkali Metals = +1 • Alkaline Earth Metals = +2 • Aluminum = +3

  8. Ionic Nomenclature • Binary Compounds of Metals with Fixed Charges: Given Formula, Write the Name • The order for names in a binary compound is first the cation, then the anion. • Use the name of cation with a fixed oxidation state directly from the periodic table. • The name of the anion will be made from the root of the element's name plus the suffix "-ide."

  9. Practice Naming • What is the name of the following? • MgO • Magnesium Oxide • NaF • Sodium Flouride • CaS • Calcium Sulfide

  10. Ionic Nomenclature • Given Name, Write Formula • The order in a formula is first the cation, then the anion. • You must know the charges associated with each cation and anion. • The sum of the positive charge and the sum of the negative charges MUST add up to zero. • You MAY NOT adjust the charges of the cations or anions to get a total charge of zero. • You MAY adjust the subscripts to get a total charge of zero.

  11. COMPOUNDS FORMED FROM IONS CATION + ANION ---> COMPOUND Na+ + Cl- --> NaCl A neutral compound requires equal number of + and - charges.

  12. Formulas of Ionic Compounds Formulas of ionic compounds are determined from the charges on the ions atoms ions  – Na  +  F :  Na+ : F :  NaF  sodium + fluorine sodium fluoride formula Charge balance: 1+ 1- = 0

  13. Hint • Cross the charges to find the amount you need. • If it can be reduced, then do so • Ie if both are 2, then it is 1

  14. Ionic Nomenclature • What is the formula of the following? • Potassium Oxide • K2O • Strontium Chloride • SrCl2 • Magnesium Nitride • Mg3N2

  15. Ionic Nomenclature • Potassium Phosphide • K3P • Magnesium Sulfide • MgS • Radium Flouride • RaF2

  16. Variable Charges • The transition metals have variable charges, they are happy with losing a variety of electrons • This is because they can also lose some of there D electrons and be stable

  17. Transition Metals Elements that can have more than one possible charge MUST have a Roman Numeral to indicate the charge on the individual ion. 1+ or 2+ 2+ or 3+ Cu+,Cu2+ Fe2+, Fe3+ copper(I) ion iron(II) ion copper (II) ion iron(III) ion

  18. Variable Charges • Formula to Name • 1) Find the charge of the cation by • Finding total charge of anion and dividing by number of cations • Example: FeCl3 • We have 3 Chlorines, each has a -1 charge • The Fe needs to be +3 to balance it out • 2) Say the cation with its Roman Numeral • Iron (III) Chloride

  19. Variable Charges • What is the name? • AuF3 • Gold (III) Flouride • AgF • Silver (I) Flouride • PbO2 • Lead (IV) Oxide

  20. Variable Charges • SnF2 • Tin (II) Flouride • MnO2 • Manganese (IV) Oxide • CrN • Chromium (III) Nitride • Sn3N4 • Tin (IV) Nitride

  21. Variable Charges • Name to Formula • The Roman Numeral tells you the charge • Balance the formula • Iron (III) Oxide • Fe has a +3 charge as denoted by the III • Oxygen always has a -2 charge • Cross them (Balance) • Fe2O3

  22. Variable Charge • What’s the formula? • Lead (IV) Sulfide • PbS2 • Copper (I) Chloride • CuCl • Silver (I) Nitride • Ag3N

  23. Variable Charge • Gold (III) Arsenide • AuAs • Tin (II) Bromide • SnBr2 • Cobalt (III) Oxide • Co2O3

  24. Writing a Formula Write the formula for the ionic compound that will form between Ba2+ and Cl. Solution: 1. Balance charge with + and – ions 2. Write the positive ion of metal first, and the negative ion Ba2+ Cl Cl 3. Write the number of ions needed as subscriptsBaCl2

  25. Learning Check Write the correct formula for the compounds containing the following ions: 1. Na+, S2- a) NaS b) Na2S c) NaS2 2. Al3+, Cl- a) AlCl3 b) AlCl c) Al3Cl 3. Mg2+, N3- a) MgN b) Mg2N3 c) Mg3N2

  26. Solution 1. Na+, S2- b) Na2S 2. Al3+, Cl- a) AlCl3 3. Mg2+, N3- c) Mg3N2

  27. Naming Compounds Binary Ionic Compounds: • 1. Cation first, then anion • 2. Monatomic cation = name of the element • Ca2+ = calciumion • 3. Monatomic anion = root + -ide • Cl- = chloride • CaCl2 = calcium chloride

  28. Naming Binary Ionic Compounds • Examples: NaCl ZnI2 Al2O3 sodium chloride zinc iodide aluminum oxide

  29. Learning Check Complete the names of the following binary compounds: Na3N sodium ________________ KBr potassium ________________ Al2O3 aluminum ________________ MgS _________________________

  30. Mixed Review • Given the name, write the formula • Given the formula, write the name • 1) Sodium Oxide • 2) Lead (II) Nitride • 3) Cesium Iodide • 4) RbF • 5) AuO

  31. Mixed Review • 6) SrCl2 • 7) CoS • 8) Ag2Se • 9) Manganese (IV) Chloride • 10) Radium Nitride

  32. Answers to Review • 1) Na2O • 2) Pb3N2 • 3) CsI • 4) Rubidium Flouride • 5) Gold (II) Oxide

  33. Answers to Review • 6) Strontium Chloride • 7) Cobalt (II) Sulfide • 8) Silver (I) Selenide • 9) MnCl4 • 10) Ra3N2

  34. Objectives 5.2 • 5.2 Apply organic nomenclature to name hydrocarbons • 5.2 Distinguish among allotropes of an element. • 5.2 Apply formulas to name molecular compounds

  35. Naming Molecular Compounds All are formed from two or more nonmetals. CO2 Carbon dioxide Ionic compounds generally involve a metal and nonmetal (NaCl) BCl3boron trichloride CH4 methane

  36. Molecular (Covalent) Nomenclaturefor two nonmetals • Prefix System (binary compounds) 1. Less electronegative atom comes first. 2. Add prefixes to indicate # of atoms. Omit mono- prefix on the FIRST element. Mono- is OPTIONAL on the SECOND element (in this class, it’s NOT optional!). 3. Change the ending of the second element to -ide.

  37. PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- NUMBER 1 2 3 4 5 6 7 8 9 10 Molecular Nomenclature Prefixes

  38. Molecular Nomenclature: Examples • CCl4 • N2O • SF6 • carbon tetrachloride • dinitrogen monoxide • sulfur hexafluoride

  39. More Molecular Examples • arsenic trichloride • dinitrogen pentoxide • tetraphosphorus decoxide • AsCl3 • N2O5 • P4O10

  40. Learning Check Fill in the blanks to complete the following names of covalent compounds. CO carbon ______oxide CO2 carbon _______________ PCl3 phosphorus _______chloride CCl4 carbon ________chloride N2O _____nitrogen _____oxide

  41. Learning Check 1. P2O5 a) phosphorus oxide b) phosphorus pentoxide c) diphosphorus pentoxide 2. Cl2O7 a) dichlorine heptoxide b) dichlorine oxide c) chlorine heptoxide 3. Cl2 a) chlorine b) dichlorine c) dichloride

  42. A flow chart for naming binary compounds.

  43. Mixed Practice • Dinitrogen monoxide • Potassium sulfide • Copper (II) nitrate • Dichlorine heptoxide • Chromium (III) sulfate • Iron (III) sulfite • Calcium oxide • Barium carbonate • Iodine monochloride

  44. Mixed Practice • BaI2 • P4S3 • Ca(OH)2 • FeCO3 • Na2Cr2O7 • I2O5 • Cu(ClO4)2 • CS2 • B2Cl4

  45. Polyatomic Ions NO3- nitrate ion NO2- nitrite ion

  46. Polyatomic Ions You can make additional polyatomic ions by adding a H+ to the ion! CO3-2 is carbonate HCO3– is hydrogen carbonate H2PO4– is dihydrogen phosphate HSO4– is hydrogen sulfate

  47. Ternary Ionic Nomenclature Writing Formulas • Write each ion, cation first. Don’t show charges in the final formula. • Overall charge must equal zero. • If charges cancel, just write symbols. • If not, use subscripts to balance charges. • Use parentheses to show more than one of a particular polyatomic ion. • Use Roman numerals indicate the ion’s charge when needed (stock system)

  48. Monatomic Ions

  49. Examples of Older Names of Cations formed from Transition Metals(you do not have to memorize these)

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