1. Lead II carbonate Formulas: SnO 2 NAMING: Period 8 Day 5 11- 5

2. Naming: Acids are named for their anions Binary: hydro – anion base – ic ending – the word “acid” Acid - Compound that yields H + ions (always starts with an H) – molecular compounds that act like ionics

3. Naming: Acids are named for their anions Binary: hydro – anion base – ic ending – the word “acid” Non-binary: ate ending becomes ic, ite ending becomes ous Examples: HF HBrHNO 3 HNO 2

4. Naming: Acids are named for their anions Binary: hydro – anion base – ic ending – the word “acid” Non-binary: ate ending becomes ic, ite ending becomes ous Examples: Hydrochloric acid Sulfurous acid

5. sulfuric acid hydrofluoric acid carbonic acid Formulas: HC 2 H 3 O 2 HCl H 2 SO 3 NAMING:

6. # 2.57 (parts a-g) AND 2.58 (parts a-e) AND 2.59 (parts a-f) BINDERS!!!

7. Lead II carbonate Phosphoric acid Formulas: H 2 SO 4 SnO 2 NAMING: Periods 1 + 3 Day 5 11-5

8. Phosphorous acid nickel III oxide Formulas: Pb(CO 3 ) 2 HClO 3 NAMING: Periods 3 + 8 Day 6 11-6

9. Ionic Compounds & Polyatomic Ions Oxyanions – polyatomic ions that contain oxygen ate = ending for most common ion (ClO 3 - Chlorate) ite = ending for one less oxygen (ClO 2 - Chlorite) hypo = prefix for another less oxygen (ClO - Hypochlorite) per = prefix for one more than most common (ClO 4 - Perchlorate)

10. Molecule – group of atoms united by covalent bonds (molecules = molecular substance) FORMULAS Empirical -simplified ratio Molecular - How many atoms in a single molecule (not always a simplified ratio, glucose = C 6 H 12 O 6 )

11. FORMULAS Empirical -Simplified ratio Molecular - How many atoms in a single molecule (not always a simplified ratio, glucose = C 6 H 12 O 6 ) Structural - Specifies which atoms are bonded to each other (organic chem)

12. Molecular Element – molecule of atoms of same element – NOT a compound - like O 2, Cl 2, O 3 H BrONClIF = diatomic molecules - these elements naturally occur as diatomic molecules and not singular atoms

13. Binary Molecular Compounds Based on Prefixes 1. Less electronegative first – prefix only if more than one atom 2. Second element – prefix, root of name, ending ide (if only two elements) 3.o or a @ the end of prefix is dropped if name begins with a vowel (monooxide, monoxide)

14. PAGE 60 Mono1 Di2 Tri3 Tetra4 Penta5 Hexa6 Hepta7 Octa8 Nona9 Deca10 Binary Molecular Compounds – prefix system

15. Write the Name: N 2 O 5 SbF 3 Dinitrogen pentoxide Antimony trifluoride Binary Molecular Compounds Write the Formula: Germanium tetraiodide diphosphorous trioxide GeI 4 P2O3P2O3

16. Binary Molecular Compounds Write the Name: As 2 O 5 ICl 3 diarsenic pentoxide iodine trichloride Write the Formula: carbon tetraiodide dinitrogen trioxide CI 4 N 2 O 3

17. Phosphorous acid nickel III oxide Formulas: Pb(CO 3 ) 2 HClO 3 NAMING: Period 1 Day 6 11-6

18. For each compound below, what type is it (covalent, acid, or ionic), and write the name. NO 2 HNO 3 Co 3 (PO 4 ) 2 Day 1 11-9

19. Green = halogens Black = carbons White = hydrogens Red = oxygen Blue = nitrogen Grey / purple = metal

21. Formulas Names

22. For each compound below, what type is it (covalent, acid, or ionic), and write the name. HC 2 H 3 O 2 Cu 3 PO 3 SF 6 Day 2 11-10

23. 23 Molecular compounds −Nonmetals or nonmetals + metalloids −Common names −H 2 O, NH 3, CH 4 −Element furthest to the left in a period and closest to the bottom of a group on periodic table is placed first in formula −If more than one compound can be formed from the same elements, use prefixes to indicate number of each kind of atom −Last element name ends in -ide

24. 24 HIhydrogen iodide NF 3 nitrogen trifluoride SO 2 sulfur dioxide N 2 Cl 4 dinitrogen tetrachloride NO 2 nitrogen dioxide N2ON2Odinitrogen monoxide Molecular Compounds

25. Example 2.7 Name the following molecular compounds: (a)SiCl 4 (b)P 4 O 10

26. Example 2.7 Strategy We refer to Table 2.4 for prefixes. In (a) there is only one Si atom so we do not use the prefix “mono.” Solution (a)Because there are four chlorine atoms present, the compound is silicon tetrachloride. (b)There are four phosphorus atoms and ten oxygen atoms present, so the compound is tetraphosphorus decoxide. Note that the “a” is omitted in “deca.”

27. Example 2.8 Write chemical formulas for the following molecular compounds: (a)carbon disulfide (b) disilicon hexabromide

28. Example 2.8 Strategy Here we need to convert prefixes to numbers of atoms (see Table 2.4). Because there is no prefix for carbon in (a), it means that there is only one carbon atom present. Solution (a)Because there are two sulfur atoms and one carbon atom present, the formula is CS 2. (b) There are two silicon atoms and six bromine atoms present, so the formula is Si 2 Br 6.

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30. 30 An acid can be defined as a substance that yields hydrogen ions (H + ) when dissolved in water. For example: HCl gas and HCl in water Pure substance, hydrogen chloride Dissolved in water (H 3 O + and Cl − ), hydrochloric acid

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32. 32 An oxoacid is an acid that contains hydrogen, oxygen, and another element. HNO 3 nitric acid H 2 CO 3 carbonic acid H 3 PO 4 phosphoric acid

33. 33 Naming Oxoacids and Oxoanions

34. 34 The rules for naming oxoanions, anions of oxoacids, are as follows: 1. When all the H ions are removed from the “-ic” acid, the anion’s name ends with “-ate.” 2. When all the H ions are removed from the “- ous” acid, the anion’s name ends with “-ite.” 3. The names of anions in which one or more but not all the hydrogen ions have been removed must indicate the number of H ions present. For example: –H 2 PO 4 - dihydrogen phosphate –HPO 4 2- hydrogen phosphate –PO 4 3- phosphate

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36. Example 2.9 Name the following oxoacid and oxoanion: (a)H 3 PO 3

37. Example 2.9 Strategy To name the acid in (a), we first identify the reference acid, whose name ends with “ic,” as shown in Figure 2.15. Solution (a)We start with our reference acid, phosphoric acid (H 3 PO 4 ). Because H 3 PO 3 has one fewer O atom, it is called phosphorous acid.

38. 38 A base can be defined as a substance that yields hydroxide ions (OH - ) when dissolved in water. NaOH sodium hydroxide KOH potassium hydroxide Ba(OH) 2 barium hydroxide

39. Hydrate – ionic substances that absorb water into their solid structures Anhydrous substance – opposite of hydrates (water-free) Naming 1. Name ionic compound 2. use prefix to name hydrate

40. Name CuSO 4 5 H 2 O MgSO 4 7 H 2 O Copper (II) sulfate pentahydrate Magnesium sulfate heptahydrate Formula Calcium sulfate dihydrate CaSO 4 2 H 2 O

41. 41 Hydrates are compounds that have a specific number of water molecules attached to them. BaCl 2 2H 2 O LiClH 2 O MgSO 4 7H 2 O Sr(NO 3 ) 2 4H 2 O barium chloride dihydrate lithium chloride monohydrate magnesium sulfate heptahydrate strontium nitrate tetrahydrate CuSO 4 5H 2 O CuSO 4

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43. 43 Organic chemistry is the branch of chemistry that deals with carbon compounds. C H H H OH C H H H NH 2 C H H H COH O methanolmethylamineacetic acid Functional Groups:

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