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Chapter 6 “Chemical Names and Formulas” Golden Valley High School Stephen L. Cotton H2OH2O.

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Presentation on theme: "Chapter 6 “Chemical Names and Formulas” Golden Valley High School Stephen L. Cotton H2OH2O."— Presentation transcript:

1 Chapter 6 “Chemical Names and Formulas” Golden Valley High School Stephen L. Cotton H2OH2O

2 Naming Ions l OBJECTIVES: –Identify the charges on monatomic ions by using the periodic table, and name the ions.

3 Naming Ions l OBJECTIVES: –Define a polyatomic ion and write the names and formulas of the most common polyatomic ions.

4 Naming Ions l OBJECTIVES: –Identify the two common endings for the names of most polyatomic ions.

5 Predicting Ionic Charges Group 1A: Lose 1 electron to form 1+ ions H1+H1+H1+H1+ Li 1+ Na 1+ K1+K1+K1+K1+ Rb 1+

6 Predicting Ionic Charges Group 2A: Loses 2 electrons to form 2+ ions Be 2+ Mg 2+ Ca 2+ Sr 2+ Ba 2+

7 Predicting Ionic Charges Group 3A: Loses 3 Loses 3 electrons to form 3+ ions B 3+ Al 3+ Ga 3+

8 Predicting Ionic Charges Group 4A: Lose 4 Lose 4 electrons or gain 4 electrons? Neither! Group 4A elements rarely form ions.

9 Predicting Ionic Charges Group 5A: Gains 3 Gains 3 electrons to form 3- ions N 3- P 3- As 3- Nitride Phosphide Arsenide

10 Predicting Ionic Charges Group 6A: Gains 2 Gains 2 electrons to form 2- ions O 2- S 2- Se 2- Oxide Sulfide Selenide

11 Predicting Ionic Charges Group 7A: Gains 1 electron to form Gains 1 electron to form 1- ions F 1- Cl 1- Br 1- Fluoride Chloride Bromide I 1- Iodide

12 Predicting Ionic Charges Group 8A: Stable noble gases do not form ions! Stable noble gases do not form ions!

13 Predicting Ionic Charges Group B elements: Many transition elements Many transition elements have more than one possible oxidation state. have more than one possible oxidation state. Iron (II) = Fe 2+ Iron (III) = Fe 3+ Note the use of Roman numerals to show charges

14 Naming cations l We will use the Stock system. l Cation - if the charge is always the same (like in the Group A metals) just write the name of the metal. l Transition metals can have more than one type of charge. l Indicate their charge with roman numerals in parenthesis after the name of the metal (Table 6.3 p 144)

15 Predicting Ionic Charges Some of the post-transition elements also Some of the post-transition elements also have more than one possible oxidation state. have more than one possible oxidation state. Tin (II) = Sn 2+ Lead (II) = Pb 2+ Tin (IV) = Sn 4+ Lead (IV) = Pb 4+

16 Predicting Ionic Charges Group B elements: Some transition elements Some transition elements have only one possible oxidation state, such as these three that are always: have only one possible oxidation state, such as these three that are always: Zinc = Zn 2+ Silver = Ag 1+ Cadmium = Cd 2+

17 Naming Anions l Anions are always the same charge l Change the monatomic element ending to – ide l F 1- a Fluorine atom becomes a Fluoride ion.

18 Polyatomic ions are… l Groups of atoms that stay together and have an overall charge, and one name. l Usually end in –ate or -ite l Acetate: C 2 H 3 O 2 1- l Nitrate: NO 3 1- l Nitrite: NO 2 1- l Permanganate: MnO 4 1- l Hydroxide: OH 1- and Cyanide: CN 1- ?

19 Naming and Writing Formulas for Ionic Compounds l OBJECTIVES: –Apply the rules for naming and writing formulas for binary ionic compounds.

20 Naming Ionic Compounds l 1. Name the cation first, then anion l 2. Monatomic cation = name of the element Ca 2+ = calcium ion l 3. Monatomic anion = root + -ide Cl  = chloride CaCl 2 = calcium chloride

21 Naming Ionic Compounds l some metals can form more than one charge (usually the transition metals) l use a Roman numeral in their name: PbCl 2 – use the anion to find the charge on the cation (chloride is always 1-) Pb 2+ is the lead (II) cation PbCl 2 = lead (II) chloride (Metals with multiple oxidation states)

22 Things to look for l If cations have (_), the number in parenthesis is their charge. l If anions end in -ide they are probably off the periodic table (Monoatomic) l If anion ends in -ate or –ite, then it is polyatomic

23 Naming and Writing Formulas for Molecular Compounds l OBJECTIVES: –Interpret the prefixes in the names of molecular compounds in terms of their chemical formulas.

24 Naming and Writing Formulas for Molecular Compounds l OBJECTIVES: –Apply the rules for naming and writing formulas for binary molecular compounds.

25 Molecular compounds are… l made of just nonmetals l smallest piece is a molecule. l can’t use charges to figure out how many of each atom

26 Molecular compounds are easier! l Ionic compounds use charges to determine how many of each. –Have to figure out charges. –May need to criss-cross numbers. l Molecular compounds: the name tells you the number of atoms. l Uses prefixes to tell you the exact number of each element present!

27 Prefixes l 1 = mono- l 2 = di- l 3 = tri- l 4 = tetra- l 5 = penta- l 6 = hexa- l 7 = hepta- l 8 = octa-

28 Prefixes l 9 = nona- l 10 = deca- l To write the name, write two words: PrefixnamePrefixname-ide

29 Prefixes l 9 = nona- l 10 = deca- l To write the name, write two words: l One exception is we don’t write mono- if there is only one of the first element. PrefixnamePrefixname-ide

30 Prefixes l 9 = nona- l 10 = deca- l To write the name, write two words: l One exception is we don’t write mono- if there is only one of the first element. l Normally do not have double vowels when writing names (oa oo) PrefixnamePrefixname-ide

31 Practice by naming these: lN2OlN2O l NO 2 l Cl 2 O 7 l CBr 4 l CO 2 l BaCl 2 (This one will not use prefixes, since it is an ionic compound)

32 Write formulas for these: l diphosphorus pentoxide l tetraiodine nonoxide l sulfur hexafluoride l nitrogen trioxide l carbon tetrahydride l phosphorus trifluoride l aluminum chloride (Ionic compound)

33 Naming and Writing Formulas for Acids and Bases l OBJECTIVES: –Apply three rules for naming acids.

34 Naming and Writing Formulas for Acids and Bases l OBJECTIVES: –Apply the rules in reverse to write formulas of acids.

35 Naming and Writing Formulas for Acids and Bases l OBJECTIVES: –Apply the rules for naming bases.

36 Acids are… l Compounds that give off hydrogen ions when dissolved in water. l Will start the formula with H. l There will always be some Hydrogen next to an anion. l The anion determines the name.

37 Rules for Naming acids 1) If the anion attached to hydrogen ends in -ide, put the prefix hydro- and change -ide to -ic acid HCl - hydrogen ion and chloride ion = hydrochloric acid H 2 S hydrogen ion and sulfide ion = hydrosulfuric acid

38 Naming Acids If the anion has oxygen in it, then it ends in -ate or -ite 2)change the suffix -ate to -ic acid (use no prefix) Example: HNO 3 Hydrogen and nitrate ions = Nitric acid 3)change the suffix -ite to -ous acid (use no prefix) Example: HNO 2 Hydrogen and nitrite ions = Nitrous acid

39 Naming Acids Normal ending ____-ide ____-ate ____-ite Acid name is… hydro-___-ic acid _____-ic acid _____-ous acid

40 Practice by naming these: l HF lH3PlH3P l H 2 SO 4 l H 2 SO 3 l HCN l H 2 CrO 4

41 Writing Acid Formulas – in reverse! Hydrogen will always be listed first The name will tell you the anion Be sure the charges cancel out. Starts with prefix hydro?- there is no oxygen, -ide ending for anion no hydro?, -ate anion comes from -ic, -ite anion comes from -ous

42 Write formulas for these: l hydroiodic acid l acetic acid l carbonic acid l phosphorous acid l hydrobromic acid

43 Names and Formulas for Bases l A base is an ionic compound that produces hydroxide ions (OH 1- ) when dissolved in water. l Bases are named the same way as other ionic compounds: –The name of the cation (which is a metal) is followed by the name of the anion (which is hydroxide).

44 Names and Formulas for Bases l NaOH is sodium hydroxide l Ca(OH) 2 is calcium hydroxide l To write the formula: 1)Write the symbol for the metal cation 2)followed by the formula for the hydroxide ion (OH 1- ) 3)then use the criss-cross method to balance the charges.

45 The Laws Governing Formulas and Names l OBJECTIVES: –Define the laws of definite proportions and multiple proportions.

46 The Laws Governing Formulas and Names l OBJECTIVES: –Apply the rules for naming chemical compounds by using a flowchart.

47 The Laws Governing Formulas and Names l OBJECTIVES: –Apply the rules for writing the formulas of chemial compounds by using a flowchart.

48 Some Laws: l 1. Law of Definite Proportions- in a sample of a chemical compound, the masses of the elements are always in the same proportions. l H 2 O (water) and H 2 O 2 (hydrogen peroxide)

49 Some Laws: l 2. Law of Multiple Proportions- Dalton stated that whenever 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.

50 Same mass of oxygen - Page 275

51 Summary of Naming and Formula Writing l For naming, follow the flowchart- Figure 6.21, page 161

52 Helpful to remember In an ionic compound, the net ionic charge is zero (criss-cross method) 2. An -ide ending generally indicates a binary compound 3. An -ite or -ate ending means there is a polyatomic ion that has oxygen 4. Prefixes generally mean molecular; they show the number of each atom

53 Helpful to remember A Roman numeral after the name of a cation is the ionic charge of the cation l Use the handout sheets provided by your teacher!


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