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Ionic and Covalent Bonding

Ionic and Covalent Bonding. Chapter 8/9. Chemical Formula. Indicates the composition of a compound and the # of atoms in one molecule of an element Molecule – smallest particle of a substance that retains the composition and properties of that substance. Two Types of Molecules.

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Ionic and Covalent Bonding

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  1. Ionic and Covalent Bonding Chapter 8/9

  2. Chemical Formula • Indicates the composition of a compound and the # of atoms in one molecule of an element • Molecule – smallest particle of a substance that retains the composition and properties of that substance

  3. Two Types of Molecules • Monatomic Molecule – each molecule consists of a single atom • Ex: Ne, Ar and Ca Diatomic Molecule – each molecule contains 2 atoms - there are seven diatomic molecules - H2, O2, N2, Cl2, F2, Br2, I2

  4. Major Classes of Compounds • Ionic Compounds – metal and a nonmetal bonded together • Molecular Compounds – two or more nonmetals bonded together

  5. Examples • CaCl2 - • SO2 – • BaO – • CCl4 -

  6. Atomic Structure

  7. Atomic Structure (cont’d) Atomic Number – Whole number on the periodic table - tells us the number of p+ - tells us the number of e- in the neutral state Ex: C has _________ p+ and e-

  8. Atomic Structure (cont’d) Atomic Mass - the average mass of an atom - tells us the number of pt and n0 together Therefore: # of neutrons = atomic mass – atomic number

  9. Ionic Substances • 1) A metal combines with a nonmetal • 2) Electrons are transferred from the metal to the nonmetal • 3)Elements no longer have a net charge of zero • 4) Ions – (charged particles) are formed

  10. Ionic Substances • An element in an uncombined state has equal numbers of protons and electrons. • Ex: Na 11 p+ Cl 17 p+ 11 e-17 e- 0 charge 0 charge

  11. Lose Electron • 1) Typically metals • 2) Atom now has more p+ than e- • 3) An overall + charge • 4) “Cation”

  12. Gain Electron • 1) Typically a nonmetal • 2) Atom now has more e- than p+ • 3) An overall – charge • 4) “anion”

  13. Na + Cl  NaCl • 1) each Na atom loses one e- • Na now has 11 p+ and 10 e- net charge +1 2) each Cl atom gains one e- - Cl now has 17 p+ and 18 e-  net charge -1 *** the attraction between the + ion and the – ion is what allows the bond to form

  14. Predicting Formulas of Ionic Compounds • The total net charge in an Ionic Compound MUST be ZERO • Ex: Mg and F

  15. Rules for Writing Formulas of Ionic Compounds • Write the symbols for the two elements Ex: Cation (Metal) always comes first 2) Determine the charge of each element 3) Determine the subscripts of each element Remember – the net charge must equal zero

  16. Polyatomic Ions • Groups of atoms of more than one element that carry a charge • Act as a single ion • Do not usually break up during a chemical rxn • Sulfate – SO4-2

  17. List of Polyatomic Ions • The sooner you learn them – the better!!!!! The formula of the ion is placed in parentheses and the subscript is placed outside the parentheses ex: Al +3 and SO4-2 Al2(SO4)3

  18. Write the correct formulas for: • Ba and Cl • Li and S • Sr and PO4-3 • NH4+1 and S • Al and S

  19. Naming Ionic Compounds Binary Compounds – compounds made up of two elements - name of cation stays the same - name of anion – ending changes to –ide Ex: NaCl – sodium chloride

  20. Naming Ionic Compounds (cont’d) Ternary Compounds – compounds made up of three or more elements - usually include a polyatomic ion - both ion names stay the same Ex: MgSO4 - magnesium sulfate ** Exception – when NH4+1 bonds with a single element (ex: NH4+1 and O) the ending changes to -ide

  21. Metals with more than 1 charge • Copper + 1 and +2 • Lead +2 and +4 • Iron +2 and +3 • Tin +2 and +4

  22. Stock System • CuCl2 vs. CuCl • Both compounds CAN NOT be named Copper Chloride – we need some way of distinguishing between the two

  23. Stock System • Name of metal is followed by a Roman Numeral which indicates the charge of the cation *** look at previous example

  24. Traditional System ● Uses suffixes at the end of the metals Latin root ● Smaller of the two ions receives suffix of – ous ● Larger of the two ions receives suffix of -ic

  25. Traditional System Fe +2 ferrous Pb +2 plumbous Fe +3 ferric Pb +4 plumbic Cu +1 cuprous Sn +2 Stannous Cu +2 cupric Sn +4 Stannic

  26. Formulas of Molecular Compounds • Molecular Compounds – made up of molecules rather than ions • 2 or more nonmetals bonded through the sharing of electrons

  27. Oxidation # • Apparent charge of an atom as it attracts or repels e- from another atom • Oxygen typically has a -2 oxidation #

  28. Example N2O nitrogen (II) oxide N = +1 NO nitrogen ( ) oxide N = N2O3 nitrogen ( ) oxide N = NO2 nitrogen ( ) oxide N = N2O5 nitrogen ( ) oxide N =

  29. Traditional System • Uses prefixes to indicate subscripts on each atom SubscriptPrefix** Mono is never used with the 1 Mono 1st element in the name of the 2 di compound (ex: CO and CO2) 3 tri 4 tetra 5 penta 6 hexa 7 hepta 8 octa

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