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Unit 5: Bonding and Nomenclature- Ionic and Metallic

Learn about Lewis Dot Structures, types of chemical bonds, metallic bonding, ionic compounds formation, properties of ionic compounds, naming rules for binary and ternary ionic compounds, and practice examples. Understand how ionic compounds are formed and how to name them.

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Unit 5: Bonding and Nomenclature- Ionic and Metallic

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  1. Unit 5: Bonding and Nomenclature- Ionic and Metallic Naming and Writing Ionic Formulas (Notice the word “ION” in Ionic? This means there will be positive and negative charged particles!)

  2. Lewis Dot Structure • Lewis Dot structures are used to represent valance electrons • Remember to follow Hund’s rule Examples: B F Ca • Examples: Na P Mg+2 S Al+3 Cl-1 Si Ar

  3. Chemical Bonds • Defined as forces of attraction that hold two atoms together and allows them to function as a unit • Formed because atoms will be more stable and obtain an octet

  4. Types of Bonds • There are multiple types of bonds possible and they are determined by electronegativity differences: • We will determine the type of bond by which elements are present • Metallic: one or more metals • Ionic: Metal and a non-metal; possible a polyatomic ion • Covalent: 2 nonmetals • Acid: Hydrogen and an anion or polyatomic ion

  5. Metallic Bonds • Metallicbonding is the force of attraction between valence electrons and the metal ions. • It is the sharing of a sea of electrons between many positive ions, where the electrons act as a "glue" giving the substance a definite structure. • Examples: Al, Au, Ag, Cu

  6. Review • Octet Rule- An element will gain, lose, or share electrons in order to obtain a full octet • Metals- Lose electrons; form cations • Non-metals- gains electrons; form anions • Monatomic ion- One element with a charge • Polyatomic ion- a group of elements with an overall charge that function as a unit (common PAI are on back of PT)

  7. +1 0 -2 -1 +2 +3 -3 THESE CAN HAVE VARIABLE CHARGES +2 +1 +2

  8. Ionic Bonds • Form between metal and non-metal ions. • Ionic bonds are formed by the transfer of electrons • Binary Ionic Compound- Made of 2 different elements • Ternary ionic compound- made of more than 2 different elements (there is a PAI present) • AFormula Unit (MgCl2) is the lowest ratio of ions in the compound (this is why we simplify subscripts).

  9. How Ionic Compounds are Formed • The metal loses electrons to the non-metal forming a cation • The non-metal gains electrons from the metal forming an anion • positive charges are very attracted to negative charges which is a type of electrostatic forces of attraction which we call Ionic bonding • When the cation and the anion form an ionic bond, they arrange in a three-dimensional shape called a crystal lattice • There are charged particles present, but the compound has a net charge of zero

  10. Ionic bonds • Ionic compounds are held together by an electrostatic force • These units stick together in a crystal lattice structure.

  11. Properties of Ionic Compounds • Electrically neutral (Overall charge is zero) • High Melting Point • Requires a lot of energy to break bonds • Brittle and Crystalline • Many dissolve in water (soluble) • Solid ionic compounds DO NOT conduct heat or electricity • Electrolyte- conducts electricity when dissolved in water

  12. Naming Ionic Compounds • Binary Type I (simple) • Composed of a metal and a nonmetal • Composed of elements that always contain the same charge • Group 1, Group 2, Group 3, zinc, cadmium and silver • Binary Type II (Roman Numerals) • Composed of a metal and a nonmetal • Composed of metals can form two or more different charges • Transition Metals and Carbon group metals

  13. Rules for Naming Type 1Binary Ionic Compounds •  The cation is named first and the anion is named second • The simple cation takes its name from the element. (ex. calcium would be calcium) • The simple anion takes the name from the element, drop the ending, and adds ide (ex. Sulfur  sulfide; oxygen  oxide)

  14. Binary Type 1 Naming Example • Name Ionic compound containing Ca and Br • CaBr2 • Cation: Ca is Calcium • Anion: Br is Bromine  Bromide • Calcium Bromide • Name the Ionic compound containing Sr and P • Sr3P2 • Cation: Sr is Strontium • Anion: P is Phosphorus  Phosphide • Strontium Phosphide

  15. Practice Naming • Name each of these compounds. • CsF 5. ZnS • KCl 6. Al2S3 • BaH2 7. MgI2 • AlCl3 8. CaBr2

  16. Rules for Naming Type II Ionic Compounds • Some Cations can form multiple charges. • Example: Pb2+ and Pb4+, Cr2+ and Cr2+ and Cr3+, Fe2+ and Fe3+, Au+ and Au3+ • Chemist decided to use roman numerals to specify charge. • Examples: • FeCl2= Iron (II) Chloride • FeCl3= Iron (III) Chloride • The only difference in type two naming is the roman numeral • The old way of naming these compounds was to use the ending –ous for the lower charger and –ic for the higher charge. • Examples: FeCl2= Ferrous Chloride FeCl3 = Ferric Chloride

  17. Practice naming Type II Cations • Write the name of each compound • CoCl3 MnO2 • CuI Fe2O3 • SnBr4 HgO • CuCl PbS • HgCl2

  18. Ternary Ionic compounds Ternary Ionic compounds are formed when there are more than two elements (i.e. there are polyatomic ions present) Ternary can be type 1 or type 2 depending on the cation

  19. Rules for Naming Ternary Ionic Compounds •  The cation is named first and the anion is named second • The simple cation takes its name from the element. (ex. calcium would be calcium; ammonium would stay ammonium) • If the cation is type 2, then you must indicate the charge of the cation ion using roman numerals (ex: Fe+3 Iron (III); Pb+2  Lead (II) ) • If the anion is a polyatomic ion, you use the name of the polyatomic ion (ex. Sulfate sulfate; hydroxide  hydroxide) • If the anion is NOT a polyatomic ion, then follow the type 1 binary ionic compounds rules

  20. Ternary Ionic Compounds Naming Examples • Name the ionic compound containing sodium and sulfate • Na2SO4 • Cation: Na is Sodium • Anion: SO4 is Sulfate  Sulfate • Sodium Sulfate • Name the ionic compound containing aluminum acetate • Al(C2H3O2)3 • Cation: Al is aluminum • Anion: Acetate  acetate • Aluminum acetate • Name the ionic compound containing Mn+4 and Chlorate • Mn(ClO3)4 • Cation: Manganese (IV) • Anion: Chlorate  Chlorate • Manganese (IV) chlorate

  21. Ternary Ionic Compounds • Write the name for the following ternary ionic compounds • Zn(OH)2 • Be2SO4 • Ga(NO2)3 • NH4OH

  22. Writing Formula for Ionic Compounds • Rules to follows for Writing ionic Compounds • Ions are given a subscript to indicate the amount of that ion present in the compound (when adding a subscript to a PAI, you must have parentheses) 1. Chemical compounds must have a net charge of zero (Both + ions and – ions must be present and their charges will cancel each other) 2. Find the charge of the cation and the anion 3. Crisscrossthe charge without the sign: Cationcharge of anionAnionchargeofcation (if the charge is 1 do not write the charge) • If you have more than 1 of a poly atomic ion, you must use parentheses around the PAI 4. Simplify subscripts

  23. Formulas of Ionic Compounds Al3+ O2– In order for ionic compounds to be electronically neutral, the sum of the charges on the cation and anion in each formula must be zero. Aluminum oxide: Al2O3 Sum of charges: 2(+3) + 3(–2) = 0

  24. Examples For Writing Ionic Compounds • Na and Cl Na+ + Cl-NaCl (simplified) Charge: +1 -1 0 • Mg + Cl Mg2+ + Cl- (crisscross) MgCl2 (simplified) Charge:2+ -1  0 • Li and N Li+ + N3- (crisscross) Li3N (simplified) Charge:+1 3- 0 • Ca and S Ca+2 + S-2 (crisscross)  Ca2S2 (need to simplify)  CaS • Ba and hydroxide Ba+2 + OH- (crisscross)  Ba(OH)2 (simplified)

  25. Practice • Write the ionic Compound for the following element combinations. • Calcium and Chlorine • Sodium and Sulfur • Lead (II) and Phosphorous • Calcium and Sulfate • Magnesium and Nitrogen • Aluminum and Oxygen • Lithium and Chlorite • Iron (IV) and Phosphite • Beryllium and Acetate

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