Naming Ionic Compounds A. Binary Ionic Compounds B. Compounds in Water C. Ionic Compounds with Polyatomic Anions and Cations

Transcription

1 Chapter 5: Nomenclature Rules or I Love It When a Plan Comes Together I. Types of Compounds A. Molecular B. Ionic II. III. IV. Naming Ionic Compounds A. Binary Ionic Compounds B. Compounds in Water C. Ionic Compounds with Polyatomic Anions and Cations Naming Molecular Compounds Naming Acids A. Binary Acids B. Acids from Oxyanions V. Writing Formulas from Names

2 I. Types of Compounds 2,3,7,8-tetrachlorodibenzo-p-dioxin Organic mostly C, H, and a small amount of other elements, generally with a C- backbone Inorganic all others without the C- backbone 2 potassium cyanide H 2 O dihydrogen monoxide Chemistry is the BOMB! A) Molecular Compounds Covalent Bonds - sharing of electrons between elements non-metal - non-metal B) Ionic Compounds Ionic Bonds - transfer of electrons between elements metal - non-metal

3 II. Naming Ionic Compounds A) Binary Ionic Compounds 3 Types of Binary Ionic Compounds Type 1 - contain metals that form only one ion of specific charge Type 2 - contain metals that can form ions with different charges Type 1 - most main group elements plus Ag, Zn, Cd, Ni Type 2 - most transition metals and inner transition metals plus Ga, In,Tl, Sn, Pb, Bi, Po*

4 Rules for Naming Binary Ionic Compounds 1. Cation Anion 4 2. Name of Cation =Type 1 - name of neutral metal =Tpye 2 - name of neutral metal (R.N.) Cmpd Cation Anion Cation Name 3. Name of Anion = root name of neutral element with -ide ending Cmpd Cation Anion Anion Name

5 C.) Ionic Compounds with Polyatomic Anions and Cations 5 Polyatomic Ion ion composed of multiple atoms Examples Exception to Rule Rule Molecular Compd. no metals Ionic Cmpd. metal and non-metal

6 6 Formulas for Ionic Compounds with Polyatomic Ions Ions Formula Fomula Ions

7 B.) Compounds in Water H 2 O Ionic and Molecular??? 7 igcsetuition.blogspot.com

8 I. WHAT IS AN AQUEOUS SOLUTION? 8 1. What is a solution? Solution - a homogeneous mixture of two or more substances (solute(s) and solvent) Solvent - Solute(s) - chemical in the largest amount chemical dissolved in the solvent 2. What does aqueous mean? (aq) aqueous (s) solid

9 II. Aqueous Compounds: 9 1. Electrolyte - Compound that dissolves in water to produces ions 2. Non-Electrolyte - compound that dissolves but does not produce ions in water 1. Electrolytes Strong Electrolyte - H 2 O for every molecule or formula unit that dissolves we get at least two ions Weak Electrolyte - only a small fraction of the compounds that dissolve produce ions

10 Soluble Ionic Compounds 1. Are all strong electrolytes 2. Dissociate into constituent ions 10

11 Soluble Molecular Compounds (Acids) - molecular compound with H listed first in the formula or with an H after COO in the formula (this H or H s can be transferred) HI CH 4 HC 2 H 3 O 2 CH 3 COOH H 3 PO 4 11 Properties of Acids Strong Acids

12 Acids Continued 12 Weak Acid - acid dissolves but only a small fraction of particles ionize to produce H 3 O +

13 Bases - bases produce OH- when dissolved in water 13 Ionic Molecular Our Class (Chem. 130)

14 2. Non-Electrolytes 14 - dissolve but do not produce ions - molecular compounds that are neither acids nor bases

15 Examples Compound Formula Cation Anion Name 15

16 Naming Ionic Compounds With Polyatomic Ions 1. Name Cation (R.N. if needed) 2. Name Anion (memorize) 16 Help Distinguishing Between Oxyanions Oxyanion - element bonded with oxygen to form an anion Increasing # s of Oxygen

17 Examples 17 Oxyanion Non-metal # O s Name Original Ion Added H New Ion Name

18 Oxyanions with Halogens 18 Cl - ClO - or OCl -, ClO 2 -, ClO 3 -, ClO 4 - Br - BrO - or OBr -, BrO 2 -, BrO 3 -, BrO 4 - I - IO - or OI -, IO 2 -, IO 3 -, IO 4 - Increasing # s of Oxygen Ion Formula Name

19 19 Practice Compound Formula Cation Anion Name

20 III. Naming Molecular Compounds BINARY MOLECULAR COMPOUNDS 20

21 Rules for Names and Formulas of Inorganic Binary Molecular Cmpds Element furthest to the left and lowest on the P.T. is usually written first in the name and formula 2. In the name, numbers of atoms are given by Greek prefixes (mono not used for first element) and the second element has ide added to the root name of the element 3. If the element starts with an a or o, the a or o is dropped from the end of the greek prefix

22 Examples 22

23 IV. Naming Acids

24 A. Naming Binary Acids Rules 1. Name of the acid = the root name of the second element with hydro as a prefix and ic as a suffix Add word acid Non-Metal Acid Formula Name

25 B. Naming Acids from Oxyanions 25 - Add H to oxyanions Increasing # s of Oxygen Increasing # s of Oxygen

26 EXAMPLES 26 Oxyanion Acid Formula Name

27 V. Writing Formulas from Names 27 Name Potassium hydroxide Lead(IV) oxide Ammonium perchlorate Cobalt(III) nitrate Calcium hypoiodite Aluminum sulfite Sodium phosphide Cation Anion Compound Formula

28 Hydrobromic Acid 28 Carbon tetrachloride Iodous acid Hypochlorous acid