Chemical Names and Formulas. Overview Metals and Non-Metals Ions and Ionic Charges Types of Compounds Systematic Names -Writing Names and Formulas
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1 Chemical Names and Formulas Overview Metals and Non-Metals Ions and Ionic Charges Types of Compounds Systematic Names -Writing Names and Formulas
2 Naming Compounds Tutorial General Information Binary Ionic Compounds Ternary Ionic Compounds/Poly-atomic Ions Naming w/metals that have more than 1 charge (Transition Metals) Molecular Compounds Naming Acids
3 Metals and Nonmetals Stairway Of Division on Periodic Table C, P, Se, I, Rn and to the right are nonmetals B, Si, As, Ge, Sb, Te, Po, At are semimetals All others are metals
4 Ions Cations Positively Charged Atoms i.e. Na + Anions Negatively Charged Atoms i.e. Cl -
5 IONIC CHARGES Group I -> 1+ Group II -> 2+ Group III -> 3+ Group IV -> 4+
6 IONIC CHARGES Group V -> 3- Group VI -> 2- Group VII -> 1- Group VIII -> Noble Gases
7 TYPES OF COMPOUNDS Ionic Compounds composed of positive and negative ions. usually formed from a metal and non-metal. these elements are not attached to one another.
8 TYPES OF COMPOUNDS Ionic Compounds con t Examples NaCl CaBr 2 KI
9 CHEMICAL FORMULAS Definition shows the kind and numbers of atoms in the smallest representative unit of the substance. i. e. NaCl
10 IONIC COMPOUNDS A formula unit is the lowest whole number ratio of ions in an ionic compound. i.e. Na 2 Cl 2 -> NaCl There is no such thing as a molecule of NaCl!!!!!!!!!
11 NAMING COMPOUNDS Your ability to name compounds and write formula s hinges on your ability to recognize whether a compound is Ionic or Molecular.
12 BINARY IONIC COMPOUNDS Binary means 2 elements Ionic means a metal and a nonmetal (or cation and anion) Writing Formulas charges must balance so compound charge is neutral.
13 BINARY IONIC COMPOUNDS Writing Formulas from Names 1st word = CATION 2nd word = ANION name with ide ending.
14 BINARY IONIC COMPOUNDS NaBr Sodium Bromide MgF 2 Magnesium Fluoride
15 BINARY IONIC COMPOUNDS Potassium Chloride Aluminum Oxide notice ending of name is ide! K + Cl - -> KCl Al 2 3+ O > Al 2 O 3
16 Polyatomic Ions Definition tightly bound groups of atoms that behave as a unit and carry a charge. Example SO 3 2-, NO 2-, ClO 2 -
17 TERNARY IONIC COMPOUNDS Ternary means 3 different elements Usually contain Poly-atomic Ions Ionic means cation and anion
18 TERNARY IONIC COMPOUNDS:Writing Formulas Ca 2+ CO > Calcium CaCO 3 Carbonate
19 TERNARY IONIC COMPOUNDS: Naming Calcium Ca(NO 3 ) 2 Nitrate
20 Naming with Transition Metals First word = CATION Second word = ANION You need to determine what charge is on the transition metal if more than one exists.
21 Naming Transition Metals Copper (I) Cu 2 O Oxide
22 Writing Formulas with Transition Metals FeCl 3 Iron (III) Chloride Iron (II) FeCl 2 Chloride
23 TYPES OF COMPOUNDS Molecular Compounds composed of molecules in which elements share electrons. usually composed of 2 nonmetals. these elements are attached
24 MOLECULAR FORMULA Definition shows the numbers and kinds of atoms present in a molecule of a compound. i. e. CO
25 TYPES OF COMPOUNDS Molecular Compounds con t Examples CS 2 SiO 2 BF 3
26 BINARY MOLECULAR COMPOUNDS Binary means 2 elements Molecular means 2 nonmetals NO ionic charges are present
27 Naming Binary Molecular Compounds Prefixes are used to show how many atoms are present in each molecule. mono, di, tri,tetra, penta, hexa, hepta, octa, nona, deca
28 Writing Binary Molecular Compounds CO 2 Carbon Dioxide no mono prefix is used on first element Di means 2 oxygens!!
29 Naming Binary Molecular Compounds 2 ways it s done! (prefix + element name) i.e. N 2 O dinitrogen monoxide
30 Naming Binary Molecular Compounds (prefix + element root + ide) i.e. PCl 3 Phosphorous Trichloride All binary compounds end in ide!!!
31 Do You Understand Ions? How many protons and electrons are in Al? 13 protons, 10 (13 3) electrons How many protons and electrons are in Se 2-? 34 protons, 36 (34 + 2) electrons
32 Oxidation Numbers The charge the atom would have in a molecule (or an ionic compound) if electrons were completely transferred to the more electronegative atom. Metal ions in Family 1, 2, 3, and 13 have one, positive oxidation number; Group 1 metals are +1, Group 2 metals are +2, Groups 3 and 13 metals are +3. Li +, Li = +1; Mg 2+, Mg = +2 Sc 3+, Sc = +3; Al 3+, Al = +3
33 Let s Check for Understanding: Oxidation Numbers Lithium ion = Li +, therefore the oxidation # = +1; Magnesium ion = Mg 2+, therefore the ox. # = +2 Aluminum ion = Al 3+, therefore the ox. # = +3
34 Oxidation Numbers (cont.) The oxidation number of a transition metal ion is positive, but can vary in magnitude. Mostly 2+. Why? Nonmetals can have a variety of oxidation numbers, both positive and negative numbers which can vary in magnitude. Mostly, however, Group 14 = 4+/-, Group 15 = 3-, Group 16 = 2- and Group 17 = 1-. Why?
35 Oxidation Numbers (cont.) Free elements (uncombined state) have an oxidation number of zero. Each atom in K or Be for example has the same oxidation number: zero.
36 Assigning Oxidation Numbers
37 Assigning Oxidation Numbers Alkali Metals = +1
38 Assigning Oxidation Numbers Alkaline Earth Metals = +2
39 Assigning Oxidation Numbers Alkaline Earth Metals = +2
40 Assigning Oxidation Numbers Group 13 Boron Group = +3
41 Assigning Oxidation Numbers Group 15 Nonmetals = -3
42 Assigning Oxidation Numbers Group 16 Nonmetals = -2
43 Assigning Oxidation Numbers Halogens = -1
44 Assigning Oxidation Numbers Transition and Post Transition Metals generally have multiple oxidation numbers
45 Assigning Oxidation Numbers Except: Ag 1+, Zn 2+, Cd 2+
46 Assigning Oxidation Numbers Also, because of the glitch, these two families will tend to be 1+, not 2+
47
48 Oxidation Numbers How to determine oxidation numbers for elements that can have several possibilities: The most electronegative element will generally retain its negative oxidation number. The least electronegative element will generally retain its positive oxidation number. Use this information to determine the other oxidation numbers.
49 The oxidation number of fluorine is always 1. (unless fluorine is in elemental form, F 2 ) The sum of the oxidation numbers of all the atoms in a molecule or ion is equal to the charge on the molecule or ion. Example: CuF; F= -1; Therefore Cu = +1
50 The oxidation number of hydrogen is +1 HF; F= -1, therefore H = except when it is bonded to metals in binary compounds. In these cases, its oxidation number is 1. NaH; Na= +1, therefore H = +1-1
51 The oxidation number of oxygen is usually 2. In H 2 O 2 and O 2 2- it is 1. H 2 O; H = +1, O= -2 SO 3 ; O = -2 x 3 = -6, S = +6
52 Oxidation numbers of all the atoms in HCO 3-? HCO 3 - O = -2 H = +1 3 x (-2) + 1 +? = -1 C = +4
53 Find the Oxidation numbers of all the elements in the following? IF 7 F = -1 7 x (-1) +? = 0 I = +7
54 An atom has 14 protons, 18 electrons and 20 neutrons. The element (or ion) is 1. Si 2. Mg 3. Ar 4. Si 4-5. Si Ar 4-7. Ar 4+
55 An atom has 15 protons, 10 electrons and 17 neutrons. What element (or ion) is it? 1. Ne 2. P 3. Ne P Ne 5-6. P 5-
56 How many total electrons does the following ion have? F - 1. One 2. Two 3. Seven 4. Eight 5. Nine 6. Ten
57 Na + is called a(n) 1. Cution 2. Anion 3. Polyatomic ion 4. Monatomic ion 5. Ipad
58 NO - is called a(n) 1. Cation 2. Antion 3. Polyatomic ion 4. Monatomic ion 5. Ionion
59 How many total electrons does the following ion have? O 2-1. One 2. Two 3. Seven 4. Eight 5. Nine 6. Ten
60 How many total electrons does the following ion have? Mg One 2. Two 3. Seven 4. Eight 5. Nine 6. Ten
61 What is the general oxidation number for Zn, z = 30?
62 What is the general oxidation number for Cl, z = 17?
63 What is the general oxidation number for Cu, z = 29?
64 What is the general oxidation number for Ni, z = 28?
65 Which of the following is isoelectronic to Na +? 1. F + 2. Al Mg + 4. Ne
66 Which of the following is isoelectronic to Na +? 1. F + 2. Al Mg + 4. Ne +
67 N 3- is a(n)? 1. anion 2. cation 3. diatomic molecule 4. polyatomic ion
68 NH 4 + is a(n)? 1. anion 2. cution 3. diatomic molecule 4. polyatomic ion
69 Na + is a(n)? 1. anion 2. cation 3. diatomic molecule 4. polyatomic ion
70 Oxidation numbers of all the elements in the following? NaIO 3 Na = +1 O = -2 3 x (-2) + 1 +? = 0 I = +5
71 Oxidation numbers of all the elements in the following? K 2 Cr 2 O 7 O = -2 K = +1 7 x (-2) + 2 x (+1) + 2 x (?) = 0 Cr = +6
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