1. Warmup (5 min) 1.Bozo Joe was asked to write the formula for silver nitrate. He wrote (NO)Ag3. What did he do wrong? 2. When one formula unit of barium phosphate dissociates, how many ions are produced? Write this equation. You need your packet today

2. Find crystal models! Solids and Naming Molecular Compounds and Acids

3. Solids amorphous solids show no definite structure, supercooled liquids. SiO 2 (glass), plastic, rubber crystalline solids orderly, repeating, 3 dimensional pattern atomic, ionic, and molecular

4. Metallic solids: atoms release their valence electrons, forming cations fixed in a “sea” of mobile electrons e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- +++++++++ +++++++++ +++++++++ Atomic Solids - “network covalent crystals” -crystals and clusters of pure elements (noble gases, metals, graphite, etc)

5. Molecular Solids all nonmetal atoms, held together with covalent bonds molecules held together by intermolecular forces in a pattern that maximizes the attractive forces between the molecules ex. sucrose, ice

6. CaF 2 Ionic solids cations and anions held together with ionic bonds arranged in a crystal lattice that maximizes ion interaction anions are packed close, with the small cations occupying the “holes” ZnS

7. Dissociation of Compounds What is happening between each water molecule and each cation and anion in the ionic compound? Ionic compounds separate into ions when dissolved in water NaCl(s)  Na + (aq) + Cl - (aq) Ions are more attracted to the water molecules than to each other! Write an equation showing the dissociation of potassium dichromate in water. K 2 Cr 2 O 7 (s)  2K + (aq) + Cr 2 O 7 2- (aq)

8. Molecular compounds dissociate into individual molecules when they dissolve in water - some don’t even dissolve in water at all Write an equation showing how carbon tetrafluoride (CF 4 ) dissolves in water CF 4 (s)  CF 4 (aq) Write an equation showing how table sugar (C 12 H 22 O 11 ) dissolves in water C 12 H 22 O 11 (s)  C 12 H 22 O 11 (aq) Write an equation showing how aluminum permanganate dissolves in water Al(MnO 4 ) 3 (s)  Al 3+ (aq) + 3MnO 4 - (aq)

9. Ionic compounds have high melting points Molecular compounds have low melting points WHY???? weakerstronger Van der waals forces (IM) triple covalent bond single covalent bond double covalent bond ionic bond force strength Melting of Compounds heat energy causes particles to move faster and intermolecular forces will weaken and break Melting point depends on strength of the forces holding the structure together

10. So, what would we call the molecule below? (H 2 NCONH 2 ) 2 Diurea This molecule can be referred to as: H 2 NCONH 2 or CH 4 ON 2 or urea Naming Molecular Compounds

11. Write the prefix that represents each number below: 1234512345 mon di tri tetr pent 6 7 8 9 10 hex hept oct non dec

12. nitrogen triodide dihydrogen monoxide phosphorous pentachloride carbon monoxide tetraphosphorus decoxide dinitrogen tetroxide nitrogen trihydride a.NI 3 b.H 2 O c.PCl 5 d.CO e. P 4 O 10 f. N 2 O 4 g. NH 3 Name each molecular compound below *if there is only 1 of the first element then there is no need for mono!

13. a. dinitrogen trioxide b. carbon tetrachloride c. dinitrogen pentoxide d. germanium tetrahydride e. silicon dioxide f. tetraphosphorus hexoxide Write the formula of each molecular compound N2O3N2O3 CCl 4 N2O5N2O5 GeH 4 SiO 2 P4O6P4O6

14. Name the following compounds: a.UF 6 b.Cu(NO 3 ) 2 c. SF 6 d. N 2 H 4 e. Mg(OH) 2 f. SnCl 2 g. Na 2 CO 3 h. H 3 PO 4 uranium hexafluoride copper (II) nitrate sulfur hexafluoride dinitrogen tetrahydride magnesium hydroxide tin(II) chloride sodium carbonate hydrogen phosphate (this has other accepted names)

15. C C C C C Name the molecule shown: 8 carbon atoms 9 hydrogen atoms 2 oxygen atoms 4 nitrogen atoms C8H9O2N4C8H9O2N4 Octocarbon-nonohydrogen- dioxygen-tetranitride But NO ONE calls it that. Common names: Caffeine 3,7-dihydro-1,3,7-trimethyl- 1H-purine-2,6-dione 1,3,7-trimethylxanthine; trimethylxanthine

16. How do you name each of these? H 2 SH 2 SO 4 H 2 SO 3 The name for each of these compounds is NOT “sulfuric acid”. They are all different! HClHClO 2 HClO 3 HClO 4 The name for each of these compounds is NOT “hydrochloric acid”. They are all different!

17. Naming Acids Binary Acids: an acid that contains H and one other element Rules for naming binary acids: 1. Prefix “hydro” is used. 2. The root of the anion is used. 3. The suffix “ic” is used. 4.The word “acid” is 2 nd word in the name. Ex. HCl H 2 S Hydrochloric acid Hydrosulfuric acid

18. Oxyacids: an acid with H, oxygen, and a 3 rd element (usually a nonmetal). Rules for naming oxyacids: 1. No prefix is used. 2. The root of the anion is used. 3. Change “ite” suffix to “ous”; change the “ate” suffix to “ic” (I ate an icky bug) 4.The word “acid” is 2 nd word in the name. Ex. H 2 SO 4 H 2 SO 3 sulfate sulfite Sulfuric acidSulfurous acid