1 CHAPTER 9: CHEMICAL NAMES AND FORMULAS Sections 1-5 (Read pages 252-285) Chapter 9 Vocab 2 Acid Base Binary compound
Law of definite proportions Law of multiple proportions Monatomic ion Polyatomic ion Section 9.1: Naming Ions Read pages 252-259 Monatomic Ions 4 Ions that consist of a single atom with a positive or negative charge resulting from the loss or gain of one or more valence electrons Two Types
Positive Ions Cations Negative Ions Anions Cations 5 Positively charged ions Metal atom loses electrons Name stays the same
Example: Name of Element: Aluminum Number of Valence Electrons: 3 Charge on Ion: +3 Name of Ion: Aluminum Naming Cations Practice 6 Element # of Valence Electrons Ion Formed Name of Cation
Sodium Calcium 1 2 2 Na+ Ca2+ Mg2+ Sodium Calcium Magnesiu m Magnesiu m
What is the rule for naming cations? DONT CHANGE THE NAME. Anions 7 Negatively charged ions Nonmetal atom gains electrons Name changes to ide ending Example: Name of Element: Iodine Number of Valence Electrons: 7
Charge on Ion: -1 Name of Ion: Iodide Naming Anions Practice 8 Element # of Valence Electrons Ion Formed Name of Anion Nitroge n Sulfur Fluorine
5 N3- Nitride 6 7 S2F- Sulfide Fluoride What is the rule for naming anions? CHANGE THE ENDING TO IDE Note:
9 Groups 14 (4A) and 18 (8A) usually do not form ions 10 Ions of Transition Metals 11 Many of the transition metals form more than one cation with different ionic charges
Not all transition metals have more than one charge Charges must be determined from the number of electrons lost These colorful solutions contain the transition metal ions Co3+, Cr3+, Fe3+, Ni2+, and Mn2+. Two Methods to Name Transition Metal Ions 12 1. 2. Stock System
Classical Method IUPAC International Union of Pure and Applied Chemistry Stock System 13 Preferred method of naming A Roman numeral in parentheses is placed after the name of the element to indicate the numerical value of the charge Number Roman Numeral
1 I 2 II 3 III 4 IV 5 V
6 VI 14 Stock System Naming Practice Ion Formed # Electrons Lost Stock Name Cu+ 1 Cu2+
2 Pb2+ Pb4+ 2 4 Copper (I) ion Copper (II) ion Lead (II) ion Lead (IV) ion Classical Method 15
In the past, scientists used the Latin names of elements. Example: Ferrum is Latin for Iron. Ferr- is the root of this word. Iron forms two ions: Fe2+ and Fe3+ Ion names: Fe2+ is the ferrous ion Fe3+ is the ferric ion 16 Practice Problems 17 a) Selenide (anion) b) Barium (cation)
c) Phosphide (anion) Polyatomic Ions 18 What does the prefix poly mean? MANY Polyatomic ions are composed of more than one atom
Tightly bound groups of atoms that behave as a unit and carry a charge The names of most polyatomic ions end in ite or ate Different Endings Ammonium NH4+ Cyanide CNHydroxide OH- 19 20
Polyatomic Ions to memorize! Formula NO3OHClO3SO42CO32PO43- Name Nitrate Hydroxide Chlorate Sulfate Carbonate Phosphate A closer look at a polyatomic ion 21 Name: Phosphate
PO Superscript: shows the charge on the polyatomic ion 34 What is the subscript on Phosphorus? 1 Subscript: shows the number of atoms of that An important note: 22
Pay close attention to the names! Example: Sulfide = S2- Sulfate = SO42- Sulfite = SO32- Quick Quiz Section 9.1 1. Which of the following are positively
charged polyatomic ions? 24 (I) ammonium ion (II) perchlorate ion (III) iron (II) ion a. I only b. II only c. III only d.
I and III 2. If the name of an ion ends in -ite or -ate, the ion is a 25 a. b. c. d. polyatomic cation. polyatomic anion. transition metal cation. monatomic anion. Section 9.2: Naming and Writing Formulas for Ionic Compounds Read pages 260-266
Different Types of Ionic Compounds 27 Simple Ionic Compounds (last chapter!) Ionic Compounds Involving Transition Metals 1. 2. 1. 2. 3. Transition metals with only 1 charge Transition metals with more than 1
possible charge Ionic Compounds Involving Polyatomic Ions Binary Ionic Compounds 28 What does the prefix bi mean? TWO A binary ionic compound is composed of two elements a metal and a nonmetal Naming Binary Ionic Compounds 29
If you know the formula of the ionic compound, you can write the name To name any binary ionic compound, place the cation name first, followed by the anion Naming Simple Ionic Compounds (last chapter) 1 Metal + 1 Nonmetal 30 CaCl2 What is the
name of the cation? What is the name of the anion? Calciu Chloride m Naming Simple Ionic Compounds (last chapter) 1 Metal + 1 Nonmetal 31 Li2O What is the name of the
cation? What is the name of the anion? Lithiu Oxide m Naming Ionic Compounds Containing a Transition Metal with ONE possible charge 1 Transition Metal + 1 Nonmetal 32 ZnS WAIT! Whats special about the
Zinc is a transition metal. It has 1 possible cation? charge. What is the name of the We dont need cation? a Roman numeral because there is only 1 possible What is the name of the anion? Zin Sulfid Naming Ionic Compounds Containing a Transition
Metal with more than one possible charge 1 Transition Metal + 1 Nonmetal 33 Cu2O Whats special about the Copper is a transition metal. It has two possible charges (+1 or cation? +2). Dont forget the roman numeral!!! (based on oxygens charge) What is the
name of the cation? Copper (I) What is the name of the What is the anion? charge on an Oxid e oxygen ion? 2- Naming Ionic Compounds Containing a Transition Metal with more than one possible charge 34
1 Transition Metal + 1 Nonmetal CuO What is the name of the cation? What is the name of the anion? Copper (II) Oxide Try It! 35
Name the following binary ionic compounds: 1. 1. 2. 2. 3 3. NaF FeCl 3. FeCl2 Sodium Fluoride Iron (III) Chloride
Iron (II) Chloride Writing Binary Ionic Formulas 36 If you know the name of a binary ionic compound, you can write the formula! Write the symbol of the cation and then the anion. Then, add the subscripts that are needed to balance the charges.
The positive charge of the cation must balance the negative charge of the anion so that the net ionic charge of the compound is neutral. Remember the crisscross method? 37 1.Determine the charge on each ion. 2.Cross the charges. 3.Reduce if necessary. 4.Name the compound. Simple Ionic Compounds Formulas 38 Write the formula for Sodium Bromide.
First: What is the cation? Second: What is the anion? Na + Br NaB - Ionic Compounds with Transition Metals 39 Write the formula for Iron (III) Oxide.
First: What is the cation? Second: What is the anion? Fe 3 + O Fe2O3 2- 40 K3N CuS
NaI K2S CaI2 What is a polyatomic ion? 41 Tightly bound groups of atoms that behave as a unit and carry a charge Polyatomic Ions behave as a UNIT. 42 You CANNOT change the charge or the number of atoms of each element in a
polyatomic ion or you will change the identity of that ion!! ClO ClO 2 ClO 3 ClO 4 Hypochlorite Chlorite Chlorate Perchlorate Naming Compounds with Polyatomic Ions
43 To name a compound containing a polyatomic ion, state the cation first, and then the anion. Just like naming binary ionic compounds! Except you DO NOT change the anion name! Naming Compounds with Polyatomic Ions Example 44 CaSO4
Whats special about the anion?SO4 is a polyatomic ion.is the What name of the cation? What is the name of the anion? Calciu Sulfat Naming Compounds with Polyatomic Ions Example 45 AlPO4 What is the
name of the cation? What is the name of the anion? Aluminu Phospha m te Naming Compounds with Polyatomic Ions Example 46 NaCH3COO What is the name of the cation?
What is the name of the anion? Sodium Acetate Be aware you cant forget about your transition metals! 47 CuSiO3 What is the name of the cation? Copper (II) What is the
name of the anion? SiO3 is called silicate Silicate 2- 48 Writing the Formula of a Compound Containing a Polyatomic Ion Remember: Polyatomic ions behave as a unit. You cannot change the assigned subscript.
Write the symbol for the cation, followed by the formula for the polyatomic ion, then balance the charges. Use parentheses. Writing Formulas w/ Polyatomic Ions Example 49 Write the formula for Aluminum Chromate. 3
Al+ 2- CrO4 Al2(CrO4)3 Writing Formulas w/ Polyatomic Ions Example 50 Write the formula for Ammonium Sulfide. NH +
S 4 (NH4)2S 2- Writing Formulas w/ Polyatomic Ions Example 51 Write the formula for Ammonium Sulfate. NH4 +
SO4 2- (NH4)2SO4 Remember there can still be compounds with transition metals! 52 Write the formula for Tin (II) Cyanide. 2 Sn + CN Sn(CN)2
- 53 a. Mg(OH)2 b. K2SO4 Ionic That is a representative metal or transition metal with only 1 charge That is a transition metal with multiple possible
charges Bonded to a polyatomic ion 54 Name cation (name stays same) Name anion (ending in ide) Name cation (use roman numerals) Name anion (ending in ide) Name cation (see above) Name anion
(polyatomic name) Try It! 55 Write the formulas of the following binary ionic compounds: Tin (IV) sulfide 1. SnS2 2. Mg(NO3)2 2. Magnesium nitrate 3. Calcium bromide 3. CaBr2 4. NaOH 4. Sodium hydroxide 1. Quick Quiz
Section 9.2 1. The correct name for CrCl3 is 57 a. b. c. d. chromium chlorine. chromium(III) chloride. monochromium trichloride. chromium(III) trichloride. 2. What is the correct formula for strontium nitride? 58
a. b. c. d. Sr3N2 SrN2 Sr2N3 Sr3N 3. Which one of the following compounds is named correctly? 59 a. b. c. d. sodium chlorite, NaClO
potassium nitrate, KNO3 sodium acetate, Na2C2H3O2 lithium sulfate, Li2SO3 Whats Next? 60 Book Work Page 258 (#8-9) Page 266 (#17-19) Page 258 #8 and 9 8. #17-19 Write the symbol for the ion of each element. Classify the ion as an anion or cation, and name the ion.
a. Potassium b. Oxygen c. Tin (2 electrons lost) d. Bromine e. Beryllium f. Cobalt (3 electrons lost) 9. Write the symbol or formula (including charge) for each of the following ions. a. Ammonium ion b. Tin (II) ion c. Chromate ion d. Nitrate ion Page 266 a. Beryllium Chloride b. Cesium Sulfide c.
Sodium Iodide d. Strontium Oxide 17. Write the formulas of these polyatomic compounds: a. Chromium (III) nitrate b. Sodium perchlorate c. Magnesium hydrogen carbonate d. Calcium acetate 18. Identify any incorrect formulas and explain your reasoning. a. Mg2(SO4)3
b. Rb3As c. BeCl3 d. NaF 17. Write the formulas of the following compounds: 61 #8 Write the symbol for the ion of each element. Classify the ion as an anion or cation, and name the ion. 62 a. Potassium K+, cation, Potassium
b. Oxygen O2-, anion, Oxide a. Tin (2 electrons lost) Sn2+, cation, Tin (II) b. Bromine Br-, anion, Bromide c. Beryllium Be2+, cation, Beryllium d. Cobalt (3 electrons lost) Co3+, cation, Cobalt (III)
#9 Write the symbol or formula (including charge) for each of the following ions. 63 a. Ammonium ion NH4 + c. Tin (II) ion Sn Chromate ion CrO42- d. Nitrate ion NO3-
b. 2+ #17 Write the formula for these binary compounds. 64 a. b. c. d. Beryllium Chloride Cesium Sulfide Sodium Iodide Strontium Oxide a. b.
c. d. BeCl2 Cs2S NaI SrO #18 Write the formula these compounds containing polyatomic ions. 65 a. b. c. d. Chromium (III) nitrate Sodium Perchlorate
Magnesium hydrogen carbonate Calcium acetate a. b. c. d. Cr(NO3)3 NaClO4 Mg(HCO3)2 Ca(C2H3O2)2 or Ca(CH3COO)2 #19 Identify any incorrect formulas. Explain your answer. 66 a.
b. c. d. be MgSO Mg2(SO4)Should 3 Rb3As Should be BeCl 2 BeCl3 NaF Section 9.3: Naming and Writing Formulas for Molecular Compounds Read pages 268-270 68
Binary Molecular Compounds A binary molecular compound is composed of two elements both are nonmetals Binary molecular compounds do not contain ions they are made of molecule s 69 Carbon and oxygen combine to form carbon monoxide (CO) and carbon
dioxide (CO2), but these two invisible gases are very different. Sitting in a room with small amounts of CO2 in the air would not present any problems. If the same amount of CO were in the room, you could die of asphyxiation. A naming system that distinguishes between these two compounds is needed. Naming Binary Molecular Compounds 70 Use prefixes The prefix in the name of a binary molecular compound tells how many atoms of each element are present in each molecule of the compound
Steps for Naming a Binary Molecular Compound 71 1. 2. Confirm that the compound is a binary molecular compound. Name the elements in the order that they appear in the formula a. b. Use prefixes to indicate the number of each kind of atom. The name of the first element stays the same. The ending of the second element
changes to ide. Quick Example Add it to your notes! 72 S2Br4 d sulfu tetr bromid a e i r Special Rules 73 If there is only one atom of the first element in the formula, drop the mono- CCl4 is called carbon tetrachloride, NOT
Ifmonocarbon tetrachloride. the element begins with a vowel, drop the vowel on the end of the prefix. Exceptions: Di- and Tri- CO is called carbon monoxide, NOT carbon monooxide. Naming Binary Molecular Compounds Example 1 74 N2 d nitroge monoxide i n O Naming Binary Molecular Compounds
Example 2 75 Cl2O8 d chlorin octoxid i e e Try It! 76 Write the names of the following binary molecular compounds: CBr4 2. N2H4 3. PCl5
4. S2F10 1. 1. 2. 3. 4. Carbon tetrabromide Dinitrogen tetrahydride Phosphorus pentachloride Disulfur decafluoride Writing Formulas for Binary Molecular Compounds 77
Use the prefixes in the name to tell you the subscript of each element in the formula. Then, write the correct symbols for the two elements with the appropriate subscripts. Writing Formulas for Binary Molecular Compounds Example 1 78 Dinitrogen trioxide N2O3
Writing Formulas for Binary Molecular Compounds Example 2 79 Iodine heptafluoride I F7 Try it! 80 a. b. c. d. Carbon disulfide Tribromine octoxide Silicon monocarbide
Dihydrogen monoxide a. b. c. d. CS2 Br3O8 SiC H 2O Ionic That is a representative metal or transition metal with only 1 charge Name cation
(name stays same) Name anion (ending in ide) That is a transition metal with multiple possible charges Name cation (use roman numerals) Name anion (ending in ide) Bonded to a polyatomic ion
81 Name cation (see above) Name anion (polyatomic name) Covalen t Name compound using prefixes Second element ends in -ide Quick Quiz Section 9.3 1. Which of the following compounds
is named INCORRECTLY? 83 a. b. c. d. CS2, carbon disulfide BCl3, boron trichloride IF7, iodine heptafluoride PCl5, phosphorus hexachloride 2. Which of the following molecular compounds is named INCORRECTLY? 84 a. b.
c. SbCl3, antimony trichloride C2O5, dicarbon pentoxide CF4, carbon tetrafluoride 3. The correct formula for tetraphosphorus trisulfide is 85 a. b. c. d. P3S4 S3P4
P4S3 S4P3 Section 9.4: Naming and Writing Formulas for Acids and Bases Read pages 271-273 Naming Acids 87 Acid - a compound that contains one or more hydrogen atoms and produces hydrogen ions (H+) when dissolved in water Hydrogen is most commonly listed first in the compound
Formula: HnX NOTE: Acids do not have to have hydrogen first, but usually do. Rules for Naming Acids 88 Three rules Dependent on the anion (the non hydrogen part) Rule #1
89 When the name of the anion ends in ide, the acid name begins with hydro-. The stem of the anion has the suffix ic and is followed by acid. Simply if there is no oxygen in the acid formula, the formula for the name is hydroroot-ic acid. Example HCl Cation Hydrogen
Anion Chloride Name of Acid Hydrochloric Acid Rule #2 90 When the anion name ends in ite, the acid name is the stem of the anion with the suffix ous followed by the word acid. Formula for name: Root-ous acid Example HClO2 Cation
Hydrogen Anion Chlorite Name of Acid Chlorous acid Rule #3 91 When the anion name ends in ate, the acid name is the stem of the anion with the suffix ic followed by the word acid. Formula for name: Root-ic acid Example
HClO3 Cation Hydrogen Anion Chlorate Name of Acid Chloric acid Weird Roots 92 Sulfur and Phosphorus Sulfur Sulfuric, Sulfurous Phosphorus Phosphoric, Phosphorous Practice Problems
93 Name the following acids: 1. H2SO3 1. 2. HNO3 1. 3. Nitric Acid HBr
1. 4. Sulfurous Acid Hydrobromic Acid H3PO3 1. Phosphorous Acid PO33- is phosphite Writing Formulas for Acids 94
Use the rules in reverse Example: Write the formula for hydrocyanic acid. Hydro-root-ic acid means the anion ends in ide. The cation is Hydrogen (H+). The anion is Cyanide (CN-). The formula for the acid is HCN. Practice Problems 95
Write the formulas for the following acids: 1. Hydroiodic acid 1. 2. Carbonic acid 1. 3. H2CO3 Carbonous acid 1. 4.
HI H2CO2 Acetic acid HC 2 H3O2 CO22- is carbonite Names and Formulas of Bases 96
Base a compound that produces hydroxide ions (OH-) when dissolved in water Named the same way as an ionic compound: Name of cation, then name of anion. Anion is usually hydroxide (OH-) but it does not have to be. Example: NaOH Cation:
Sodium Anion: Hydroxide Name of Base: Sodium Hydroxide Try it! 97 Provide the appropriate name or formula of the following bases: Potassium hydroxide 1. 1. KOH Be(OH)2
2. 1. Beryllium Hydroxide RbOH 3. 1. Rubidium Hydroxide Aluminum hydroxide 4. 1. Al(OH)3 A base to take note of:
98 NH3 is ammonia. This is an example of a base that does NOT contain a hydroxide ion. Weird Roots 99 Sulfur and Phosphorus Sulfur Sulfuric, Sulfurous Phosphorus Phosphoric, Phosphorous
Ionic 10 0 Acid That is a representative metal or transition metal with only 1 charge Name cation (name stays same) Name anion (ending in ide) That is a
transition metal with multiple possible charges Name cation (use roman numerals) Name anion (ending in ide) Bonded to a polyatomic ion Name cation (see above) Name anion (polyatomic name)
If the anion is hydroxide (OH-) then you have a base Covalen t Name Does not contain any oxygen (Anion ends in ide) compound using prefixes (second element ends in ide) Hydro(root)ic
acid Anion ends in ite (Root)ous acid Anion ends in ate (Root)ic acid Molecular Naming Review 101 CO2 2. CO 3. P2O5 4. N2O 5. SO2 6. CBr4 1.
PBr5 2. ICl3 3. NI3 4. N2O3 1. 1. 2. 3. 4. 5. 6. 7. 8. Dinitrogen tetroxide Sulfur trioxide
Nitrogen monoxide Nitrogen dioxide Diarsenic pentoxide Phosphorus trichloride Carbon tetrachloride Dihydrogen monoxide Acid/Base Naming Review 102 1. 2. 3. 4. 5. 6. 7.
8. 9. Sodium hydroxide Sulfurous acid Hydrosulfuric acid Phosphoric acid Ammonia Hydrocyanic acid Calcium hydroxide Iron (III) hydroxide Hydrophosphoric acid 11. HF H2S 12.
H2CO3 10. 14. LiOH HNO2 15. Co(OH)2 16. H2SO4 17.
Be(OH) 2 13. Quick Quiz Section 9.4 104 1. An acid is a compound that produces WHAT when dissolved in water? a. b. c. d. Hydroxide ions Hydrogen ions Polyatomic ions
Molecules 105 2. Which of the following formulas is correct for the base: Calcium Hydroxide a. b. c. d. CaOH2 CaH CaOH Ca(OH)2 Whats Next? 106
Practice Problems 22. Write the names of the following a. Diphosphorus trioxide compounds: 22. Write the molecular formulas of a. NCl3 the following compounds: d. SO3 a. Phosphorus pentachloride b. BCl3 e. N2H4 29. Name the following acids: b. Iodine heptafluoride
c. Nl3 f. N2O3 c. Chlorine trifluoride 29. HNO 2 23. Write the formulas or names of d. the following compounds: 30. Iodine HMnO4dioxide a. CS2 31. HCN 23. The name a student gives for the b. Carbon tetrabromide 32. H2S molecular
compound SiCl4 is c. Cl2O7 30. Name the following bases:Is this monosilicon trichloride. name correct? Explain. 29. LiOH 30. Pb(OH)2 31. Mg(OH)2 32. Al(OH)3 31. Write formulas for each of the following acids and bases: 29. Carbonic acid 30. Sulfurous acid 31. Iron (III) hydroxide 107
#22 Write the names for these molecular compounds. 108 a. b. c. d. e. f. NCl3 BCl3 Nl3 SO3 N2H4 N2O3 a.
b. c. d. e. f. Nitrogen trichloride Boron trichloride Nitrogen triodide Sulfur trioxide Dinitrogen tetrahydride Dinitrogen trioxide #23 Write the formulas or names for these molecular compounds. 109 a.
CS2 c. Carbon tetrabromide Cl2O7 d. Diphosphorus trioxide b. a. b. c. d. Carbon disulfide
CBr4 Dichlorine heptoxide P2O3 #24 Write the formulas for these binary molecular compounds. 110 a. b. c. d. Phosphorus pentachloride Iodine heptafluoride Chlorine trifluoride Iodine dioxide
a. b. c. d. PCl5 IF7 ClF3 IO2 #25 The name a student gives for the molecular compound SiCl4 is monosilicon trichloride. Is this name correct? Explain. 111 Silicon tetrachloride #29 Give the names of these acids.
112 A. B. C. D. HNO2 HMnO4 HCN H2 S A. B. C. D. Nitrous acid Permanganic
acid Hydrocyanic acid Hydrosulfuric acid #30 Write the names of these bases. 113 A. B. C. D. LiOH A. Pb(OH)2 B. Mg(OH)2 C. Al(OH)3 D.
Lithium hydroxide Lead (II) hydroxide Magnesium hydroxide Aluminum hydroxide #32 Write the formulas of the following acids and bases: 114 A. B. C. D. Carbonic acid Sulfurous acid Iron (III) hydroxide Strontium
hydroxide A. B. C. D. H2CO3 H2SO3 Fe(OH)3 Sr(OH)2 Section 9.5: The Laws Governing Formulas and Names Read pages 274-279 The Laws Governing Formulas and Names 116
The rules for naming and writing formulas are possible because elements form compounds in predictable ways. Two Important Laws The Law of Definite Proportions The Law of Multiple Proportions 117 The Law of Definite Proportions States that in samples of any chemical compound, the masses of the elements are
always in the same proportions. So what does that mean? Law of Definite Proportions Continued 118 Water What is the formula for water? H2O What is the atomic mass of Oxygen? 16.00
What is the atomic mass of Hydrogen? 1.00 What is the mass ratio of Oxygen to Hydrogen in water? 16:2 which reduces to 8:1 Hydrogen Peroxide Dihydrogen Dioxide What is the formula for hydrogen peroxide? H2O2
What is the mass ratio of Oxygen to Hydrogen in water? 32:2 which reduces to 16:1 Regardless of how much you have, the ratio of masses is always the same! Both water and hydrogen peroxide are composed of hydrogen and oxygen. 119 But they have different properties. Law of Multiple Proportions 120
Whenever the same two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers. Two Compounds (X and Y) contain equal masses of Element B. The ratio of the masses of Element A in these compounds is 5:10 or 1:2. Main Idea: 121
In any chemical compound, the elements are always in the same proportion by MASS. Guidelines for Writing the Chemical Formula of a Compound 122 1. 2. 3. 4. An ide ending generally indicates a binary compound.
An ite or ate ending means a polyatomic ion that contains oxygen is in the formula. Prefixes in a name generally indicate that the compound is molecular. A Roman numeral after the name of a cation shows the charge of the cation. Naming Review 123 1. 2. 3. H in front of the formula? Its an acid! OH in the formula? Its a base! (Ionic name) Metal present? Its ionic!
1. 4. Check to see if you have a transition metal with multiple charges. Only nonmetals? Its covalent! Naming Practice 124 Formula Name Sodium chloride BrF3 LiNO3 Dinitrogen
tetrahydride Potassium hydroxide Rb2O Hydrofluoric acid Ionic or Molecular? Naming Practice Answers 125 Formula Name NaCl BrF3
Sodium chloride Bromine trifluoride Ionic or Molecular? Ionic Molecular LiNO3 Lithium nitrate Ionic N2H4 Molecular Rb2O
Dinitrogen tetrahydride Potassium hydroxide Rubidium oxide HF Hydrofluoric acid Ionic KOH Ionic Ionic Whats Next? 126
Book Work Page 279 (#35, 39-41) #35 What two laws describe how chemical compounds form? 127 The Law of Definite Proportions The Law of Multiple Proportions #39 Name these compounds: 128 a.
b. c. CaCO3 a. Calcium carbonate PbCrO4 b. Lead (II) chromate SnCr2O7 c. Tin (II) dichromate #40 Write the formulas for these compounds: 129 a. Tin (II) hydroxide Sn(OH) b. Barium Fluoride 2
Ba #40 Identify the incorrect names or formulas. 130 a. b. c. d. Calcium (II) oxide Aluminum oxide Na2C2O4 Mg(NH4)2
