Right Side NOTES ONLY. TN Ch Topic: EQ:

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2 Title and Highlight Right Side NOTES ONLY TN Ch Topic: EQ: Date Reflect Question: Reflect on the material by asking a question (its not suppose to be answered from notes) NOTES: Write out the notes from my website. Use different types of note-taking methods to help you recall info (different color pens/highlighters, bullets, etc) When I lecture we will add more info, so leave spaces in your notes Summary Questions: Write Book Question out and answer it (in another color based on what you read from my notes or textbook. THESE ARE AT THE VERY END OF NOTES

3 Title and Highlight LEFT Side PICTURES, PRACTICE PROBLEMS, ETC TN Ch DRAW ANY PICTURES, FIGURES, AND WRITE OUT ANY PRACTICE PROBLEMS/QUESTIONS. WE WILL ANSWER THEM TOGETHER. LEAVE SPACES SO WE CAN ANSWER QUES.

4 READ Ch (pg ) first then take notes

5 Sodium chloride (NaCl) The properties of a compound are different from the properties of the elements that compose it.

6 A few of the substances we encounter in everyday life are elements. Majority are compounds or molecules. In a compound, the elements combine in fixed, definite proportions. This is known as the Law of Constant Composition.

7 A chemical formula indicates the elements present in a compound and the # of atoms of each. For example, H 2 O is the chemical formula for water; it indicates that water consists of H and O atoms in a 2:1 ratio. The formula contains the symbol for each element with subscripts (little # s) indicating the number of atoms of that element. (don t write 1 s). H 2 O 1 = H 2 O

8 Common chemical formulas include: CO for carbon monoxide (1:1 ratio) CO 2 for carbon dioxide (1:2 ratio). C 12 H 22 O 11 for sugar (sucrose) (12:22:11 ratio). If subscripts change, then the formula no longer is that compound. (Muy importante) H 2 O vs. H 2 O 2

9 CO (carbon monoxide), an air pollutant When inhaled, CO interferes with the blood s ability to carry oxygen, which can be fatal. Called the Sleep of death gas CO 2 is carbon dioxide, produced from combustion and human respiration. We breathe small amounts of it all the time with no harmful effects.but harmful to the planet (aka global warming)!!!

10 1. Chemical formulas list the most metallic elements first. Remember - Metals are on the left side of the P.T. and nonmetals on the upper right side. The formula for table salt is NaCl, not ClNa. 2. In compounds that do not include a metal, the more metal-like element is listed first. (closest nonmetal to the staircase on P.T.)

11 3. Within a group in P.T., elements toward the bottom are more metal-like than elements toward the top. We write SO 2 not O 2 S.

12 Left side!!! The specific order for listing nonmetal elements in a chemical formula is shown in Table 5.1

13 Left side!!!

14 Some formulas contain groups of atoms. Their formula is set off in parentheses with a subscript to indicate the number of that group.

15 Many of these groups of atoms have a charge associated with them and are called polyatomic ions. (Very important for the rest of year!! Hint, hint) To determine the total number in a compound containing a group within parentheses, multiply the subscript outside the parentheses by the subscript for each atom inside the parentheses.

16 Left side!!! Determine the number of each type of atom in Mg(NO 3 ) 2.

17 Left side!!! Practice Problem #3 Determine the number of each type of atom in the following compounds. (a) Al (C 2 H 3 O 2 ) 3 (b) Al 2 (Cr 2 O 7 ) 3 (c) Pb (HSO 4 ) 4 (d) Pb 3 (PO 4 ) 4 (e) (NH 4 ) 3 PO 4 Out of the 5 compounds, which formula represents the greatest total number of atoms?

18 RIGHT side - End of notes Number BQ and write it out Answer it (in another color/highlight it based on what you read from my notes or textbook)

19 READ Ch 5.4 (pg ) first then take notes

20 An empirical formula (e.f.) gives the relative number of atoms of each element in a compound. A molecular formula (m.f.)gives the actual number of atoms of each element in a molecule of the compound. For example, the m.f. for hydrogen peroxide is H 2 O 2, and its e.f. is HO. The molecular formula is always a whole number multiple of the empirical formula.

21 Left side!!!

22 Lets start a little review for the final exam Draw the Matter Chart! (see next slide) Pure substances may be either elements or compounds. Elements may be either atomic or molecular. Compounds may be either molecular or ionic.

23 Left side!!!

24 Atomic elements are those that exist in nature. basic units = atoms. Most of PT (~99%) elements fall into this category. Molecular elements do not normally exist in nature(unstable as single atoms). Diatomic molecules two atoms of that element bonded together. Basic units = molecules (unstable as single atoms) There are 7 diatomic molecules Name them!!

25 Left side!!!

26 Molecular compounds are compounds formed from two or more nonmetals. basic units = molecules. Ionic compounds are compounds formed from a metal and nonmetal contains a cation (+ ions) paired with a anion (- ions). basic units = formula units.

27 Left side!!! a. Krypton b. CoCl 2 c. Nitrogen d. SO 2 e. KNO 3 f. Au g. Na 2 O h. H 2 O

28 RIGHT side - End of notes Number BQ and write it out Answer it (in another color/highlight it based on what you read from my notes or textbook)

29 READ Ch 5.5 (pg ) first then take notes

30 2 types of Compounds ionic bonds molecular bonds (ch 5.8) (M + NM) (NM + NM) (M + PA)

31 ionic bond electrical attraction between ions (charged atoms: cations and anions); e- are taken by one atom and given to another atom (like a magnet). Ionic Compounds Also called Salts ****Ionic bonding only 2 types (sometimes 3 - rare) 1 Metal (cation) + 1 Nonmetal (anion) or 1 Metal (cation) + 1 Polyatomic (anion) (see handout) (The charges are hidden to make a neutral compound.)

32 Metals LOSE electrons. become + ions = CATION

33 Group 1: Lose 1 electron to form 1+ ions H + Li + Na + K + Label this on your PT!

34 Group 2: Loses 2 electrons to form 2+ ions Be 2+ Mg 2+ Ca 2+ Sr 2+ Ba 2+ Label this on your PT!

35 B 3+ Al 3+ Ga 3+ Label this on your PT! Group 13: Loses 3 electrons to form 3+ ions

36 C 4+ Si 4+ Ge 4+ Sn 4+ Pb 4+ Group 14: Loses 4 Electrons Label this on your PT!

37 Nonmetals GAIN electrons from metals become - ions = ANION ending to name changes to -ide

38 N 3- P 3- As 3- Nitride Phosphide Arsenide Label this on your PT! Group 15: Gains 3 electrons to form 3- ions

39 O 2- S 2- Se 2- Oxide Sulfide Selenide Label this on your PT! Group 16: Gains 2 electrons to form 2- ions

40 F 1- Cl 1- Fluoride Chloride Br1- I 1- Bromide Iodide Label this on your PT! Group 17: Gains 1 electron to form 1- ions

41 Label this on your PT! Group 18: Stable Noble gases do not form ions!

42 Predicting Charges on Ions KNOW THESE!!!! Label this on your PT! Cd +2

43 I m Positive! A metal ion atom A nonmetal atom ion I m Negative

44 I m Positive! A metal ion A nonmetal ion I m Negative the transfer of electrons produces ions, which means.. Ionic bonding!!!

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46 cations (+) Metals lose e- anions (-) Nonmetals gain e- monatomic ions one ion Examples: Na + or O -2 polyatomic ions - ions formed from two or more atoms bonded together Examples: NH 4 + or SO 4-2

47 Binary Ionic Compound 2 atoms (M+NM) Step 1 Write cation (metal) then anion (nonmetal) Step 2 Check to see if charges equal zero!!! Step 3 Criss-Cross Method - Cross the charges using subscripts to balance charges if they don t balance out. Don t write 1 s. Ba +2 Cl -1 = BaCl 2

48 Left side!!! Write the correct formula and name the compounds containing the following ions: 1. Na +, S 2-2. Al 3+, Cl - 3. Mg 2+, N 3-4. Al 3+, S 2-5. Zn +2, I Ca +2, O -2

49 RIGHT side - End of notes Number BQ and write it out Answer it (in another color/highlight it based on what you read from my notes or textbook)

50 READ Ch (pg ) first then take notes

51 1 st step in naming an ionic compound be able to identify it as one. (sometimes the hard part) Ionic Compound (I.C.) Lose (+ ions) and gain (- ions) electrons Cation (+ ions) then anion (- ions) 3 types M + NM = binary I.C. (2 elements) M + P.A. = ternary I.C. (more than 2 elements) P.A. + P.A. = ternary I.C.

52 TRICKS Transition and Other Metal Ions KNOW THESE!!!! Cd +2

53 Binary compounds - contain only two different elements. Draw this with notes!!!

54 cations name doesn t change Example: Ba +2 barium ion anions remove the ending and add ide Example: Cl - is not chlorine. chloride ion Naming: Cation (1 st ) then anion (2 nd ) BaCl 2 is barium chloride

55 Left side!!! Element Anion Symbol Anion Name Bromine Br -1 Bromide Chlorine Cl -1 Chloride Fluorine F -1 Fluoride Hydrogen H -1 Hydride Iodine I -1 Iodide Nitrogen N -3 Nitride Oxygen O -2 Oxide Phosphorus P -3 Phosphide Sulfur S -2 Sulfide

56 Left side!! Practice Problem #1: BaI 2 AlF 3 CaSe KBr MgS Sodium chloride Sodium phosphide Magnesium nitride Sodium nitride Aluminum oxide

57 RIGHT side - End of notes Number BQ and write it out Answer it (in another color/highlight it based on what you read from my notes or textbook)

58 READ Ch (pg ) first then take notes

59 Elements that can have more than one possible charge MUST have a Roman Numeral. Roman Numeral = # charge ion. 1+ or or 3+ Cu +, Cu 2+ Fe 2+, Fe 3+ copper(i) ion iron(ii) ion copper (II) ion iron(iii) ion

60 Draw this with notes!!!

61 - Metals with multiple charges use Roman numeral in cation name PbCl 2 Pb 2+ is cation PbCl 2 = lead(ii) chloride

62 Left side!!! Complete the names of the following binary compounds with variable metal ions: FeBr 2 CuCl iron ( ) bromide copper ( ) chloride SnO 2 ( ) Fe 2 O 3 ( ) Hg 2 S ( )

63 Left side!!! Formula Cation Name FeCl 3 (Fe 3+ ) iron (III) chloride CuCl tin (IV) fluoride PbCl 2 Fe 2 S 3 (Fe 3+ ) Copper(II)oxide Lead(II)fluoride CrO 3 Cr 2 O 3

64 Left side!!! It will save you!! no Does the compound have more than 2 elements? yes Is the metal a transition metal or under staircase? Metal (check if T.M. or if under staircase = need R.N.) yes Cation use Roman Numerals no Cation + anion (ide) + Polyatomic names (-ate or -ite)

65 Left side!!!

66 Some ionic compounds contain polyatomic ions (ions that are themselves composed of a group of atoms with an overall charge).

67 Many polyatomic ions are oxyanions, anions containing oxygen. If there are two ions in the series, the one with more oxygen atoms is given the ending - ate and the one with fewer is given the ending -ite. (BOTH SAME CHARGE!!) NO 3 nitrate SO 4 2 sulfate NO 2 nitrite SO 3 2 sulfite

68 If there are more than two ions in the series, then the prefixes hypo-, meaning less than, and per-, meaning more than, are used. ClO hypochlorite BrO hypobromite IO hypoiodite ClO 2 chlorite BrO 2 bromite IO 2 iodite ClO 3 chlorate BrO 3 bromate IO 3 iodate ClO 4 perchlorate BrO 4 perbromate IO 4 periodate

69 Writing Formulas for Ionic Compounds Step 1 write cation (metal) then polyatomic Step 2 Charges have to equal zero!!! Cross the charges if they don t balance out. Step 3-- Use parentheses around polyatomic ion Practice Problems: Write the formula for each ionic compound. copper(ii) bromide Cu +2 Br -1 = CuBr 2 (don t show 1 s) aluminum nitrite Al +3 NO 2-1 = Al(NO 2 ) 3 barium hydrogen carbonate Ba +2 HCO 3-1 = Ba(HCO 3 ) 2

70 Left side!!! 1. aluminum nitrate 2. copper(ii) nitrate 3. Iron (III) hydroxide 4. Tin(IV) hydroxide

71 Left side Practice Problem #4: Write the formula for the following compounds. Lithium chloride Aluminum sulfide Copper(II) oxide f) Iron(III) chloride i) Calcium bicarbonate l Potassium nitrite Potassium perchlorate Ammonium carbonates )Iron(II) phosphate w)

72 Left side!!! Underlined letter = starting element symbol of the polyatomic # consonants = # of oxygen atoms # vowels = # negative charge on the ion

73 Left side!!! use different colors Nick the Camel ate a Creamy Clam for Supper in Phoenix. Manly Brad had an Itch and took Aspirin.

74 Left side!!! Nick Underlined letter = starting element symbol of the polyatomic # consonants = # of oxygen atoms # vowels = # negative charge on the ion N 3 consonants = O 3 1 vowel = - 1 NO 3-1

75 Left side!!! Practice Problem #5: Name the following ionic compounds: NaHCO 3 K 2 SO 3 MgSO 4 KCN Ca(OH) 2 NH 4 NO 3 Zn(NO 3 ) 2 Li 3 PO 4

76 Left side!!! Practice Problem #6: Name the following ionic compounds: CuHCO 3 FeSO 3 CuSO 4 Cr(CN) 3 Cr(PO 4 ) 2 Sn(OH) 2 W(NO 2 ) 5 Ti(CO 3 ) 2 CoPO 4 PbCl 2

77 Left side!!! Practice Problem #7: Write the formula for the following compounds. a) Barium oxide b) Sodium bromide c) Copper(I) oxide d) Iron(II) chloride e) Potassium nitrite f) Calcium hydroxide g) Silver nitrate h) Ammonium chloride i) Lithium phosphate j) Sodium nitrite k) Sodium bicarbonate l) Calcium Carbonate m) Sodium sulfate n) Iron(III) hydroxide o) Copper(II) hypochlorite p) Magnesium sulfite

78 RIGHT side - End of notes Number BQ and write it out Answer it (in another color/highlight it based on what you read from my notes or textbook)

79 READ Ch 5.8 (pg ) first then take notes

80 Ch 5.8 Naming Molecular Compounds Left side!!! Ionic Covalent (molecular) Metals & Nonmetals Only nonmetals lose/gain e- share e-

81 The first step in naming a molecular compound is identifying it as one. Remember - all molecular compounds form from two nonmetals. (no metals) Use PREFIXES - indicate the # atoms in the compound. Draw this with notes

82 Left side!!! Prefixes in Molecular Compounds Number of atoms Prefix Number of atoms Prefix 1 mono- 6 hexa- 2 di- 7 hepta- 3 tri- 8 octa- 4 tetra- 9 nona- 5 penta- 10 deca-

83 Write the formula for dihydrogen monoxide? Anyone want a cold glass of dihydrogen monoxide?

84 Formula Common Name Molecular compounds name H 2 0 Water Dihydrogen monoxide NH 3 Ammonia Nitrogen trihydride

85 1. If there is only one atom of the first element, the prefix mono- is NOT WRITTEN. CO 2 mono carbon di- ox -ide The full name is carbon dioxide.

86 2. The compound N 2 O also called laughing gas, is named according to the first element, nitrogen, with prefix di-, followed by the second element, prefixed by mono-, and the oxide. dinitrogen monooxide (Wrong!!) HOWEVER. Since mono- ends with a vowel and oxide begins with a vowel, an o is dropped and the two are combined as monoxide. The entire name is dinitrogen monoxide.

87 3. (Rule only for oxygen) drop one of the o Do not follow this rule for other elements. Examples: triiodide or tetraarsenide

88 Left side!!! Practice Problem #1: a. P 2 O 5 b. SO 2 c. IF 7

89 Left side!!! Practice Problem #2: Name the following molecules. a. N 2 O 5 b. CO c. Cl 4 F 7 d. SO 3

90 Practice Problem #3: Write the formula for each molecule. a. nitrogen monoxide b. carbon tetrachloride c. diphosphorus nonaoxide

91 RIGHT side - End of notes Number BQ and write it out Answer it (in another color/highlight it based on what you read from my notes or textbook)

92 READ Ch 5.9 (pg ) first then take notes

93 Acids are MOLECULAR compounds (share e-) that form ions when dissolved in water. Composed of hydrogen, written first in their formula, and one or more nonmetals, written second. Categorize acids into two groups: binary acids & oxyacids. Make flowchart for the notes!!!

94 H and 1 nonmetal H and polyatomic Draw this with notes

95 Binary acids are composed of hydrogen and a nonmetal. The names for binary acids have the following form: Draw this with notes

96 HCl(aq) is hydrochloric acid. HBr(aq) is hydrobromic acid. HCl(g) refers to hydrogen chloride molecules in the gas phase, and not to the acid. Give the name of H 2 S(aq) and H 3 P. (Be careful of spelling)

97 2. Naming Oxyacids Draw this with notes

98 Oxyacids are acids that contain oxyanions (polyatomic with oxygen) The number of H + ions depends on the charge of the oxyanion, so that the formula is always charge-neutral (criss-cross).

99 2. If the acid s name ends with -ic without the hydro- prefix, the name of the anion used ends in. -ate Therefore, it is an oxy- acid. Examples: perchloric acid = acetic acid = 3. If the acid s name ends with, -ous the name of the anion used ends in. -ite (It s is also an oxy-acid.) Examples: hypochlorous acid = nitrous acid = sulfurous acid =

100 Left side

101 Left side Naming Oxy-Acids 1. If the name of (X) ends in ate -ic acid 2. If the name of (X) ends in ite -ous acid Practice Problems: Name these acids. H 2 SO 4 H 3 PO 3 HNO 3 H 2 CO 3 HC 2 H 3 O 2 HClO 2 Naming Binary Acids 2 elements If the name of (X) ends in ide hydro- -ic acid Practice Problems: Name these acids. H 2 S HCl HF

102 RIGHT side - End of notes Number BQ and write it out Answer it (in another color/highlight it based on what you read from my notes or textbook)

103 READ Ch 5.10 (pg ) first then take notes

104 Left side

105 Start of 2 nd Sem