1. 1 st e- transferred 2 nd Ions form 3 rd Opposite ions attract Bond is formed by EMF Compound is made Ionic Compounds

2. Rules ➢ Transfer of e- from a metal to a nonmetal so that all atoms get an octet of valence electrons ➢ Zero Rule is met so that the total sum of the ion charges add up to zero ▪Total electrons lost = Total electrons gained ▪ Law of conservation of matter is obeyed ▪ Stable and neutral compound is produced

3. Ionic Compounds ➢ Metal cation comes first in the name and formula and keeps the name of the element ➢ Nonmetal anion comes second in the name and formula and changes the element name to end in “ide” ➢ Each ion symbol beings with a capitalized letter ➢ The number of cations and anions needed to meet the zero rule are shown by using subscripts but subscripts of 1 aren’t shown

4. Examples Magnesium Fluoride MgF 2

5. Examples Aluminum Oxide

6. Zero Rule…Short Cut Metal transfers e- to nonmetal → ions form→ EMF makes bond → Ionic Compound Ca +2 and F -1 → CaF 2 Al +3 and O -2 → Al 2 O 3 Na +1 and P -3 → Na 3 P Notice any pattern with ion charges and subscripts in the formula?

7. Criss Cross Method 1 st – Get the ion charges 2 nd – Drop the charge but keep the number 3 rd – Reduce the numbers If possible 4 th – Cross over numbers to get formula subscripts

8. Transition Metal Compounds Some metals in the d block can shift e- between orbitals, altering the number of valence e- they have for making an octet a) The same element can create more than one type of ion

9. Transition Metal Compounds b) Roman numerals are used to indicate the number of e- lost and which form of the ion occurs i) roman numeral only appears in the name ii) roman numeral DOES NOT APPEAR in the formula

10. Transition Metal Compounds c. Follow the same rules for forming the compound ✓ Metal cation is first ✓ Nonmetal anion is second ✓ Met Zero Rule - octet for all atoms, ion charges cancel out ✓ Metal ion keeps its name (roman numeral if dual form) ✓ Nonmetal name ends in “ide” Cobalt II & Phosphorus Co +2 P -3 Co 3 P 2 Cobalt II Phosphide Cobalt III & Phosphorus Co +3 P -3 CoP Cobalt III Phosphide Tin IV & Sulfur Sn +4 S -2 SnS 2 Tin IV Sulfide Zinc & Chlorine Zn +2 Cl -1 ZnCl 2 Zinc Chloride

11. Determining Compound Names You CANNOT just uncross to get the name of a compound CaCl 2 Is NOT Calcium II Chloride CrO 3 Is NOT Chromium III Oxide You Have to figure out which form of the ion meets the zero rule 1 st Determine possible names for the ions Ca = CalciumCl = Chloride only options so……………. CaCl 2 is calcium chloride

12. Determine Compound Names 1 st - Determine the possible names for the ions CrO 3 Cr = Chromium IICr = Chromium IIICr = Chromium VI O = Oxide 2 nd - Figure out form of the ion will make that formula Cr +2 O -2 CrO NOPE Cr +3 O -2 Cr 2 O 3 NOPE Cr +6 O -2 CrO 3 YUP! CrO 3 Is Chromium VI Oxide

13. Polyatomic Ions Poly (group) atomic (of atoms) ions (charged) Polyatomic ion: a group of atoms that form a permanent team and act as a single ion Sulfur has 6 valence e- x 1 atom = 6e- Oxygen has 6 valence e- x 4 atoms = 24e- 30 valence e- Gaining 2 more e- Completes the octet Gives Charge of -2 Makes a “happy” group of atoms

14. Polyatomic Ions Naming - differs to distinguish polyatomic from monatomic ions monatomic ions → end in “ide” polyatomic ions → end in “ite” or “ate” Monatomic S -2 … Sulfide Monatomic O -2 … Oxide Polyatomic SO 4 -2... Sulfate Polyatomic SO 3 -2... Sulfite

15. Polyatomic Ions All polyatomic ions and their correct names are given on your ion sheet and are denoted with an *

16. Polyatomic Ions Formula Writing – IF the ion is polyatomic AND you need more than one use ( ) when writing the formula Monatomic – No ( ) Polyatomic only 1, no ( ) More than 1 use ( )

17. Polyatomic Ions ExampleAluminum & Carbonate Al +3 CO 3 -2 Zero Rule need 2 Al +3 Al +3 need 3 CO 3 -2 CO 3 -2 CO 3 -2 No ( ) Al 2 CO 33 looks like 1 carbon, 33 oxygen Use ( ) Al 2 (CO 3 ) 3 clear you have 3 carbonate groups ion group (inside) number to meet zero rule ( ) outside subscript

18. Polyatomic Ions Cu +1 CO 3 -2 Cu 2 CO 3 Calcium Nitrate Potassium Sulfate Zinc Phosphate Copper I Carbonate

19. Different Players = Different Method Metals get a stable octet by losing electrons Nonmetals get a stable octet by gaining electrons Metal & Nonmetal = complementary actions; transfer e- Nonmetal & Nonmetal = clashing actions; must share e- Different players Different product Different naming system

20. Covalent Bonding Type of bond formed when nonmetallic atoms join together to achieve stability…NO METALS INVOLVED

21. Covalent Bonding Energy level overlap allows shared electrons to be in both atoms electron cloud and valence octet at the same time Shared electrons are equally attracted to both nuclei Bond is created by EMF, but weaker than the EMF of ionic

22. Covalent Bonding 1. Valence electrons are shared so that all atoms obtain an octet and achieve stability No adding or removing of electrons, only sharing Law of conservation – you cannot create or destroy matter No Charges! Why? #e- = #p+ no gaining or losing

23. Naming Covalent Molecules Prefix Method ❑ First element keeps its name and has the lower group number ❑ Prefix is used to indicate the atoms present in the chemical ❑ Mono is not used with the first element

24. Naming Covalent Molecules Second element changes its name to end in “ide” Another prefix gives the number of atoms in the chemical Format: Prefix-First Element Prefix-Second Element-ide As 2 O 3 2=di 3=tridiarsenic trioxide S 4 F 10 4 = tetra 10= decatetrasulfur decafluoride ICl 1= 1 st no mono 1 = monoiodine monochloride

25. Formulas For Covalent Molecules ❑ Prefix = subscript ❑ Element name = symbol phosphorus trichlroide1 P and 3 ClPCl 3 dinitrogen pentoxide2 N and 5 ON 2 O 5 carbon monoxide1 C and 1 O CO

26. Your Turn Part 1: Give the formula for each of the covalent molecules named below 1) Carbon tetrachloride CCl 4 2) Sulfur hexafluoride SF 6 3) Dinitrogen pentoxide N 2 O 5 4) Tricarbon OctahydrideC 3 H 8 5) Silicon disulfide SiS 2 Part 2: Provide the name for the covalent molecule formulas shown below 6) NONitrogen Monoxide 7) As 2 S 3 Diarsenic trisulfide 8) P 4 O 10 Tetraphosphorus Decoxide 9) PBr 5 Phosphorus pentabromide 10) B 2 H 6 Diboron hexahydride

27. A substance’s molar mass is the mass in grams of one mole of the compound. Molar Mass is also called Molecular Weight Molar Mass Ca:1 x 40.08= 40.08 g C:1 x 12.01= 12.01 g O:3 x 16.00= 48.00 g Calculate the molar mass of CaCO 3 100.09 g

28. Quick Check What is the molar mass of sulfur dioxide? SO 2 S1 x 32.07 g O + 2 x 16.00 g SO 2 64.07 g SO 2 = 64.07 g

29. Law of Definite Proportions/ Percent Composition A specified compound has a set formula so it will always contains the same proportion of elements by mass Ratio or percentages of the masses of the elements that make up a compound is set or “definite” Always the same part of the whole Regardless of the sample size or mass

30. RATIO OF THE MASSES RELATES TO RATIO OF ATOMS size of sample doesn’t matter double size = double mass = double elements 1/10 th size = 1/10 th the mass = 1/10 th the atoms The ratio of elements stays the same A COMPOUNDS FORMULA IS DEFINITE

31. Also called mass percent OR percent by mass The composition of a compound in terms of the weight or “How much a compound’s weight is due to an element” Percent Composition First, we must find the molar mass of the compound (Percent composition)

32. Find the percent composition of carbon in ethanol (C 2 H 5 OH) First, find the molar mass of the compound C:2 x 12.01=24.02 g H:6 x 1.008=6.048 g O:1 x 16.00=16.00 g 1 mole of C 2 H 5 OH has a mass of 46.07g (Percent composition)

33. Find the percent composition of carbon in ethanol (C 2 H 5 OH) Percent composition = 24.02 g C 46.07 g C 2 H 5 OH X 100% (Percent composition) Percent composition = 52.14 % Carbon

34. Writing Equations – What goes in must come out ….Law of Conservation – Coefficients – change the amount of a chemical – Subscripts - change the formula, violate zero rule

35. Key Terms – Rxn = reaction 2 Al + 3 CuCl 2 → 3 Cu + 2 AlCl 3 – Reactants Substance(s) that enter a reaction (starting materials) Written on the left side of the arrow – Products Substance(s) that are formed by the reaction (ending materials) Written on the right side of the arrow

36. Key terms Symbol – represents an element – Ag, Cl 2, K Formula – represents a compound or molecule – MgSO 4, NH 3 Al + CuCl 2 → Cu + AlCl 3 Some Elements Can Never Be Along If Not In a Compound They Pair With Themselves BrINCl HOF Twins Symbol Formula

37. Key terms 2 Al + 3CuCl 2 → 3 Cu + 2 AlCl 3 Subscripts – Indicates the number of atoms in a compound Example CuCl 2 = Cl - Cu - Cl = one copper atom, two chlorine atoms – Written below a symbol – Cannot be changed Coefficients – Indicates the number of moles/molecules of a compound Example 3CuCl 2 = Cl-Cu-Cl Cl-Cu-Cl Cl-Cu-Cl – Written in front of a symbol or formula – Can be changed WHY NOT? WHY?

38. Equations Must – Represent known facts (correct formulas) – Adhere to the Law of Conservation of Mass (balanced equation) Total mass reactants = total mass of products atoms present in reactants are still present in the reactants

39. Balancing Rules & Hints Do NOT change subscripts Balance using coefficients, multiple by them Balance elements first one at a time Do polyatomic ions, that appear on both sides, second Balance H & O last For repeats, keep track of the them separately, then add them If it doesn’t balance, try doubling the coefficients and double check your formulas