chapter7_eseb

** - **Chapter 7 - Formulas and Chemical Compounds** (textbook pages 218 - 259) Edited by Sydney I and Julia B
 * Inorganic Chemistry Chemical




 * Vocabulary **
 * __monatomic ion__ - ion formed from single atom
 * __binary compound__ - compound composed of two elements
 * __nomenclature__ - a naming system of binary ionic compounds using the compound's negative and positive ions
 * __oxyanion__ - a polyatomic ion that contains oxygen
 * __salt__ - an ionic compound composed of a cation and the anion from an acid
 * __oxidation numbers (oxidation states)__ - in order to indicate the general distribution of electrons among the bonded atoms in a molecular compoud or a polyatomic ion atoms composing the compound or ion are assigned
 * __formula mass__ - any molecule, formula unit, or ion is the sum of the average atomic masses of all atoms represented in its formula
 * __percentage composition__ - the percentage by mass of each element in a compound
 * __empirical formula__ - consists of the symbols for the elements combined in a compound, with subscripts showing the smallest whole-number mole ration of the different atoms in the compound

~ **IONIC** - a metal is present ("H" is considered a non-metal) ~ **COVALENT-** no metal is present ~ **HYDRATE** - H20 is present ~ **ACID -** must have "H" at the beginning and be aqueous(aq), meaning it dissolves in water

**Naming Covalent Compounds**

1.) Tell the number of each element using a prefix. 2.) Change the ending of teh second element to "-ide". //*If only one atom of the first element is present, you do NOT use "mono".//

//Examples:// P4O10 = tetraphosphorus NO2 = nitrogen dioxide H2O = dihydrogen monoxide N2O4 = dinitrogen tetraoxide


 * = **PREFIXES** ||
 * = mono -//1// ||
 * = di - //2// ||
 * = tri - //3// ||
 * = tetra - //4// ||
 * = penta - //5// ||
 * = hexa - //6// ||
 * = hepta - //7// ||
 * = octa - //8// ||
 * = nona - //9// ||
 * = deca - //10// ||

 <span style="font-size: 110%; color: rgb(8,8,212); font-family: 'Palatino Linotype','Book Antiqua',Palatino,serif;">
 * Rules for Naming Binary (meaning two) Ionic Compounds Containing Main Group Metals**

1.) Say the name of the cation (__HINT__: the cation is first). 2.) Say the name of the anion with an "-ide" ending.

//Examples:// K2O ~ potassium oxide CaF2 ~ calcium fluoride Li2S ~ lithium sulfide

magnesium nitride ~ Mg3N2 sodium phosphide ~ Na3P calcium oxide ~ CaO

<span style="font-size: 110%; color: rgb(212,12,12); font-family: 'Palatino Linotype','Book Antiqua',Palatino,serif;">**Naming Binary Ionic Compounds with a D-Block Metal**

//Example:// Fe2+Cl22- ~ iron (II) chloride Fe3+Cl33- ~ iron (III) chloride Cu2+O2- ~ copper (II) oxide Cu2+Cl22- ~ copper (II) chloride //Cl=1- charge but since there are two, (-1)*2=2-charge//

<span style="color: rgb(0,0,0);">Give the name of the element and if the charge is greater change the ending to "-//ic//" and if the charge is lesser, change the ending of the name to //"-ous//"
 * Alternative way...**

(mercuric/mercurous) || 1+ or 2+ ||
 * <span style="font-size: 110%; color: rgb(0,0,0);">**<span style="color: rgb(0,0,0);">Latin Name ** || <span style="font-size: 110%; color: rgb(0,0,0);">**<span style="color: rgb(0,0,0);">Element ** || ** Charge ** ||
 * ferrum || iron || 2+ or 3+ ||
 * cuprum || copper || 1+ or 2+ ||
 * stannium || tin || 2+ or 4+ ||
 * plumbum || lead || 2+ or 4+ ||
 * Hg || mercury

//Examples://

Cu2S ~ cupric sulfide or copper (I) sulfide FeBr2 ~ iron (II) bromide or ferric bromide SnCl4 ~ stannic chloride or tin (IV) chloride

lead (II) iodine ~ PbI2 cobalt (II) fluoride ~ CoF2 stannous oxide ~ SnO

<span style="font-size: 110%; color: rgb(245,15,147); font-family: 'Palatino Linotype','Book Antiqua',Palatino,serif;">**Naming Ternary (meaning 3 or more) Ionic Compounds**

1.) Say the name of the cation. 2.) If the metal is in the d-block, give the charge. 3.) Say the name of the anion.

//Examples:// sodium sulfate ~ Na(SO4) cobalt (II) nitrate ~ CO(NO3)2 iron (II) dichromate or ferrous dichromate ~ FeCr2O7 CuNO3 ~ copper (I) nitrate (NH4)Cl ~ ammonium chloride

The difference in the prefix and/or suffix happens when oxygens are either dropped or added. per, -ate = one added -ate = most common in nature -ite = one dropped hypo, -ite = two dropped, least common in nature

//Examples:// ClO4- = __<span style="color: rgb(0,0,0);">per __chlor__ate__ ClO3- = chlor__ate__ (most common) ClO2- = chlor__ite__ ClO- = __hypo__chlor__ite__

SO52- = __per__sulf__ate__ SO42- = sulf__ate__ (most common) SO32- = sulf__ite__ SO22- = __hypo__sulf__ite__

<span style="font-size: 110%; color: rgb(230,194,25); font-family: 'Palatino Linotype','Book Antiqua',Palatino,serif;">**Naming Hydrates**

//Examples:// FeSO4*5H2O = iron (II) sulfate Ca(NO3)2*2H2O = calcium nitrate dihydrate

<span style="font-size: 110%; color: rgb(45,188,225); font-family: 'Palatino Linotype','Book Antiqua',Palatino,serif;">**Naming Acids** <span style="font-family: Arial,Helvetica,sans-serif;">2.) Change anion ending to "-ic". <span style="color: rgb(0,0,0); font-family: Arial,Helvetica,sans-serif;">3.) Say "acid". || <span style="font-size: 90%; color: rgb(0,0,0); font-family: Arial,Helvetica,sans-serif;">1.) __NO HYDRO__ 2<span style="color: rgb(0,0,0);">.) Use anion to determine the acid name: "-ate" goes to "-ic" "-ite" goes to "-ous" 3<span style="color: rgb(0,0,0); font-family: Arial,Helvetica,sans-serif;">.) Say "acid". <span style="color: rgb(0,0,0);"> || //Examples:// H2CO3(aq) ~ carbonic acid HClO(aq) ~ hypochlorous acid HI(aq) ~ hydroiodic acid H2CrO4(aq) ~ chromic acid H2SO3(aq) ~ sulfurous acid
 * <span style="font-family: Arial,Helvetica,sans-serif;">**Binary** || <span style="font-family: Arial,Helvetica,sans-serif;">**Ternary** ||
 * <span style="font-family: Arial,Helvetica,sans-serif;">1.) Say "hydro".


 * <span style="font-size: 110%; color: rgb(11,218,32); font-family: 'Palatino Linotype','Book Antiqua',Palatino,serif;">Polyatomic Ions (also called Radicals) **


 * **Name** || **Formula** ||
 * <span style="color: rgb(255,13,10);">Ammonium || NH4+ ||
 * <span style="color: rgb(244,74,52);">Carbonate || CO32- ||
 * <span style="color: rgb(255,86,0);">Chlorate || ClO3- ||
 * <span style="color: rgb(234,198,16);">Chromate || CrO42- ||
 * <span style="color: rgb(11,218,32);">Cyanide || CN- ||
 * <span style="color: rgb(0,128,0);">Dichromate || Cr2O72- ||
 * <span style="color: rgb(6,102,183);">Sulfate || SO42- ||
 * <span style="color: rgb(16,154,218);">Phosphate || PO43- ||
 * <span style="color: rgb(159,78,244);">Hydroxide || OH- (correctly -OH) ||
 * <span style="color: rgb(136,12,136);">Nitrate || NO3- ||
 * <span style="color: rgb(225,9,161);">Permanganate || MnO4- ||
 * <span style="color: rgb(244,62,161);">Peroxide || O22- ||
 * <span style="color: rgb(255,10,31);">Thiocyanate || SCN- ||
 * <span style="color: rgb(237,60,12);">Mercury (I) || Hg22+ ||
 * <span style="color: rgb(244,197,16);">Acetate || C2H3O2- ||
 * <span style="color: rgb(144,226,24);">Oxalate || C2O42- ||
 * <span style="color: rgb(30,200,164);">Thiosulfate || S2O32- ||

Directions: Please write if it is ionic, covalent, an acid, or a hydrate and give its name or formula. 1. Fe2+
 * <span style="font-size: 110%; color: rgb(166,8,166); font-family: 'Palatino Linotype','Book Antiqua',Palatino,serif;">Practice Problems **

2. N2O5

3. sulfuric acid

4. CH3COOH

5. hydrofluoric acid

6. lead (IV) oxide

7. KF

8. phosphorus (III) iodine

9. Hg3(PO4)2

10. HF

Works Cited Davis, Frey, et al. __Modern Chemistry.__ Orlando: Holt, Rinehart, and Winston, 2006. http://www.lycos.com/info/acetic http://chemistry.alanearhart.org/Images/chemist.gif