1. Chapter 7: Ionic and Metallic Bonding Chapter 9: Naming Compounds and Writing Formulas

2. Electron Configuration Exceptions P. 136 Cr – [Ar] 4s 2 3d 4 - does not occur Cr – [Ar] 4s 1 3d 5 – occurs Why? Greater stability is achieved with half filled 3d 5 orbitals.

3. Another example: Cu – [Ar] 4s 2 3d 9 - does not occur Cu – [Ar] 4s 1 3d 10 – occurs Why? Greater stability is achieved with completely filled 3d 10 orbitals. Other Exceptions that follow this pattern: Ag, Au P. 208 - Q - 58 and 59

4. Valence Electrons Dictate Chemical Properties Representative Elements – look at the Group # Symbolically represented by Electron Dot Structures P. 193 - #8

5. Remember Stability Octet Rule – atoms want to obtain a noble gas electron configuration ns 2 np 6 Metals – lose electrons to gain the octet of the next lowest energy level –Cations Non-Metals – gain electrons to obtain a complete octet –Anions

6. Cation Formation K 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 reactive Metals – lose electrons to gain the octet of the next lowest energy level K 1s 2 2s 2 2p 6 3s 2 3p 6 unreactive K  K +1 + e -

7. Cations – lose electrons

8. Transition Metals: Pseudo Noble Gas Configurations Ag - 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 4d 10 5s 1 Options – lose 11 electrons or gain 7 Neither happens Ag loses 1 electron to gain a pseudo noble gas configuration Ag 1+ - 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 4d 10

9. Transition Metals – Why Multiple Charges? Fe - 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 Can become Fe 2+ or Fe 3+ Fe 2+ Fe 3+ loses the 4s 2 electron sloses the 4s 2 electrons and one 3d electron Creates 5 half filled 3d orbitals

11. Anion Formation Cl 1s 2 2s 2 2p 6 3s 2 3p 5 reactive Non Metals – gain electrons to complete their octet Cl 1- 1s 2 2s 2 2p 6 3s 2 3p 6 unreactive Cl + e -  Cl 1- A Halide

12. Anions – end in -ide Gain electrons

13. Ionic Bonds form Ionic Compounds Electrostatic attraction of cations and anions Neutral compounds Binary compounds – MgO, not CaSO 4

14. Ionic Bonds

15. P. 208 - Q - 66

16. Practice Show how the following form ionic compounds. –Electron configuration, orbital diagram and electron dot diagrams 1.3 Sodium atoms and one Nitrogen Atom 2.2 Lithium atoms and one Oxygen Atom 3.1 Strontium atom and 2 Fluorine Atoms P. 196 - Q - 12 and 13

17. Ionic Compounds Chemical Formula – the type and number of atoms in smallest representative unit of a substance Formula unit – the lowest whole number ratio of ions in an “ionic compound”

18. Naming Ions Monatomic Ions – a single atom with a charge –Cations - K 1+, Ca 2+ –Anions – O 2-, N 3- Drop the ending and add –ide Polyatomic ions – charged ions containing more than one atom

19. Polyatomic Ions Most end in -ate or -ite NO 3 - Nitrate NO 2 - Nitrite SO 4 2- Sulfate SO 3 2- Sulfite more oxygen atoms - suffix –ate fewer oxygen atoms - suffix -ite

20. Bonding Nomenclature – Naming Ionic Compounds and Binary Molecular Compounds Are they a metal and a non-metal or a metal and a polyatomic ion? Are they 2 non-metals? Does the cation have one oxidation number? Does the cation have multiple oxidation numbers? State the name of the cation. State the name of the anion. Drop the ending and add – ide. Do not change if it is a polyatomic ion. State the name of the cation. State the name of the anion. Drop the ending and add – ide. Do not change if it is a polyatomic ion. State the oxidation number of the cation in Roman numerals. Use the anion to determine the charge. State the name of the 1st element. State the name of the 2nd element. Drop the ending and add –ide. Add prefixes to identify the number of each element 1 – mono*6 – hexa 2 – di7- hepta 3 – tri8 - octa 4 – tetra 9 - nona 5- penta10- deca * used only on the 2 nd element Ionic CompoundBinary Molecular Compound Ex. Na 1+ Ex. Fe 2+ or Fe 3+ Ex. SodiumEx. Iron Ex. Sodium Bromide Ex. Sulfate Ex. Iron (III) Sulfate Ex. Dicarbon Hexafluoride Fe ( ) SO 4 2- SO 4 2- Fe must be 3+ because there are 2 Fe ions and the sulfate ions have a 6- charge. NaBr, Fe 2 (SO 4 ) 3, C 2 H 6

21. Bonding Nomenclature – Writing Formulas for Ionic Compounds and Binary Molecular Compounds Are they a metal and a non-metal or a metal and a polyatomic ion? Are they 2 non-metals? Write the symbol of the cation and the anion. Assign charges to each. Remember that roman numerals apply to the cation. Are they balanced? Rewrite the symbols without the charges. Rewrite the symbols and symplify the crossed charges. Do not write the crossed charge if it was a 1. Write the symbol of each element. Each prefix identifies the quantity of each element. Write the number as a subscript for each corresponding prefix. 1 – mono*6 – hexa 2 – di7- hepta 3 – tri8 - octa 4 – tetra 9 - nona 5- penta10- deca * used only on the 2 nd element Ionic CompoundBinary Molecular Compound No Cross the charges. yes

22. Properties of Ionic Compounds Depend on attraction of bonded elements Na and Cl –+ surrounded by – –- surrounded by + Forms a crystal lattice –Size and number of ions determine the shape

23. Properties - continued Melting and boiling points and hardness –Depend on attraction of ions –Greater attraction = ↑MP, BP and hardness Mg 2+ O 2- Greater attraction

24. Continued Non conductor of electricity –Ions are static Conduct electricity when in water or melted –Ions free to move –Called electrolytes when dissolved in water

25. Exothermic nature Ionic compounds release energy upon formation because they are becoming more stable

26. Does the size of the ion influence the lattice energy? Does the charge of the ion influence the lattice energy? Lattice Energy - energy needed to separate one mole of ions

27. Lattice energy energy needed to separate one mole of ions –Depends on size of ions –Smaller the ion the greater the attraction –Proximity to the nucleus –Depends on the charge of the ion Greater the charge the greater the attraction P. 199 Q - 22

28. Metallic Bonds Electron Sea Model Atoms outer energy levels overlap Electrons move freely from atom to atom (delocalized electrons, s and d electrons) Cations are formed Metallic bond forms when delocalized electrons are attracted to the metallic cations P. 203 - Q - 23

29. Aufbau Diagram Equal energies – 2 p Sublevels have different energy levels Energy levels overlap

30. Properties of Metals Explained Mobile cations and electrons Moderate melting pts. extreme boiling pts. malleable and ductile

31. Strong Attraction for each other durability Mobile electrons good conductors of heat and electricity Interaction with photons of light luster Amount of delocalized electrons ↑electrons ↑strength and hardness s block weak, d block hard P. 203 – 26, 27 - P. 207 - Q – 46, 47, 48, 51

32. Alloys – mixture of 2 or more elements that have metallic properties superior to their parent element

33. Types of Alloys – Tech and Society (Page 204-205) Substitutional – similar size elements are substituted with one another –Stainless steel, pewter, gold Interstitial – extremely small atoms fill in the holes between much larger atoms Properties become more desirable –Carbon-steel – much harder, stronger, less ductile than iron alone, corrosion resistant P. 203 - Q - 25