I SOTOPES  All atoms of the same element have the same physical and chemical properties  But they are not all identical  The number of protons of an element must be identical for those atoms to be identified as that element  The number of neutrons can be different 11 H11 H 21 H21 H 31 H31 H 1

Learning Task  Workbook page 1, 2 and 5

3 12 p+ 12 n 12 e- 50 p+ 68 n 50 e- Mg Sn

E NERGY LEVEL DIAGRAMS ________ S Cl Mg 16 p+ 16 n 17 p+ 18 n 12 p+ 12 n First 3 energy levels, max number of electrons that can be represented are: 1 st = 2, 2 nd = 8, 3 rd = 8, 4 th ?, 5 th ? Electrons in the highest energy level are called valence electrons. 4

C OMPOUNDS  can be separated into simpler substances by chemical but not physical means i.e. heating  Compounds are composed of elements combined together  Salt - NaCl 5

I ONS - ALL ABOUT STABILITY  Happy atoms are stable ions. They do not normally change their structure  Unhappy atoms are unstable. They want to change their structure by:  Giving away an electron or electrons  Taking an electron or electrons 6

I ONS  Atoms like to have their electrons in full energy levels  Atoms that have a nearly full outer energy level like to take electrons from other atoms  Atoms that have only one or two electrons in their outer energy level like to give away electrons 7

I ON F ORMATION E XAMPLE 12 p+ 12 n Mg 2e- 8e- 2e

I ON FORMATION EXAMPLE – MAGNESIUM ION 12 p+ 12 n Mg 2+ 2e- 8e

F ORMATION OF THE CHLORIDE ION 17 p+ 18 n Cl 2e- 8e- 7e

F ORMATION OF THE CHLORIDE ION 17 p+ 18 n Cl - 2e- 8e e- 11

D RAWING E NERGY L EVEL D IAGRAMS FOR IONS Mg _______ Ca _______ Na F p+ 12n 11p+ 12n 9p+ 10n 20p+ 20n

I ONS C ONTINUED  Metals __________ electrons to form __________ ions.  Non-metals __________ electrons to form ___________ ions.  The names of negative ions end in ______  What happens to the names of metallic ions? give away positive accept negative ide nothing 13

N AMING I ONS  Positive ions - same name as atom  Negative ions - ending is changed to ‘ide’  ie. Fluorine gains an electron and becomes fluoride 14

L EARNING A CTIVITIES  Complete energy level diagrams on pages 3 & 4 of your workbook  Page 6 and 7 on ions! 15

S ECTION 1.5 – C LASSIFYING C OMPOUNDS Nelson Reference: Pages

F ORMATION OF IONIC COMPOUNDS 17

C OMPOUNDS  Metals and non-metals combine to form _________ compounds.  If a compound formula begins with a metal or the ion NH 4 + it is an ___________ compound. ionic 18

N AMING B INARY I ONIC C OMPOUNDS  Name the metallic ion first, followed by the non- metallic ion ends in “ide”  Ionic compounds always start with metal or an ammonium ion  Write the symbol and charge for each ion  Compounds are electrically neutral - they have no charge - zero.  Use subscripts to equalize the total number of positive and negative charges 19

P REDICTING IONIC COMPOUND FORMULAS 20 (x)Al 3+ + (y)O 2- = Na + Cl - +=NaCl = 0 (x)3 + + (y)2 - = 0

(x)Al 3+ + (y)O 2- = Na + Cl - +=NaCl = 0 (2)3 + + (3)2 - = 0 21 P REDICTING IONIC COMPOUND FORMULAS

(2)Al 3+ + (3)O 2- = Na + Cl - +=NaCl = 0 (2)3 + + (3)2 - = 0 Al 2 O 3 22 Alternatively – use the Kriss Kross will make you want to jump, jump method!

M ULTIVALENT METALS  In groups 3 through 12, many metals form more than one type of charged ion.  Naming is done with the Stock system. The charge on the metallic ion with a number indicating the charge on the ion with Roman numerals  To determine the metal ion’s charge  Find the charge of the non-metal ion  Determine the charge necessary for the compound to have no charge  Name the compound with a roman numeral in brackets after the metal ion I.e. tin (IV) chloride 23

M ULTIVALENT METALS  Fe 2 O 3  The charge on the O is 2-  There are 3 O so there are 6 negative charges  Therefore there needs to be 6 positive charges  There are 2 iron ions so the charge on each is  3+  The name is iron (III) oxide 24

M ULTIVALENT METALS  PbS  The charge on the sulphide ion is 2-  The charge on the lead ion is then  2+  Lead (II) sulphide 25

I ONIC COMPOUNDS COMPOSED OF THREE ELEMENTS  These compounds are composed of a metal or the ammonium ion combined with a polyatomic ion. (a complex ion)  Most of these ions end in ate or ite ammonium  The only positively charged polyatomic ion is ammonium  Two ions end in ‘ide’ - hydroxide and hydrogen sulfide 26

C OMPLEX IONS (P OLYATOMIC IONS ) 27 PO 5 3- perphosphate PO 4 3- phosphate PO 3 3- phosphite PO 2 3- hypophosphite SO 5 2- persulfate SO 4 2- sulfate SO 3 2- sulfite SO 2 2- hyposulfite CO 4 2- percarbonate CO 3 2- carbonate CO 2 2- carbonite CO 2- hypocarbonite NO 4 - pernitrate NO 3 - nitrate NO 2 - nitrite NO - hyponitrite ClO 4 - perchlorate ClO 3 - chlorate ClO 2 - chlorite ClO - hypochlorite

F ORMULAS FOR IONIC COMPOUNDS CONTAINING COMPLEX IONS  Write the two ions with their charges  Use subscripts to balance the number of positive and negative charges equal  If a subscript is required for the complex ion put the complex ion in brackets  Examples:  Sodium carbonate  Strotium hydroxide  Tin (IV) sulfite 28

N AMING IONIC COMPOUNDS CONTAINING COMPLEX IONS  Always name the two ions  The first ion is the metal or the ammonium ion  The second ion is the negatively charged complex ion as named on the back of your periodic table.  Examples: 1. FeSO 3 (s) 2. Cu 2 CO 3 (s) 3. Cr 2 (SO 4 ) 3 (s) 29

L EARNING A CTIVITIES TO BE C OMPLETED :  Pages 8-12 all on naming Ionic Compounds! 30