Before Bell Rings Study for Ionic Naming Quiz

ETD#13 Give the formula for the following compounds: Calcium Phosphate Lithium Chlorate Lead (II) Oxide Name the following compounds: FeO Ca(OH)2 CuCl2

ETD#14 Give the formula for the following compounds: Calcium Phosphate – Ca3(PO4)2 Lithium Chlorate – LiClO3 Lead (II) Oxide - PbO Name the following compounds: FeO – Iron (II) oxide Ca(OH)2 – Calcium hydroxide CuCl2 – Copper (II) Chloride Remember we only use the roman numerals when the cation (usually a metal) has multiple charges. Ionic compounds are always neutral overall, so we need to have the correct number of each ion to make the total charge equal to zero.

Naming Ionic Compounds Quiz Ion sheet and PT out, everything else away.

Learning Targets I can determine the name/formula for a given molecular compound.

Ionic vs. Covalent -Between 2 non-metals - Sharing electrons Ionic compounds have ionic bonds, meaning electrons have left from one atom and been taken in by another. The bond comes from the opposite charges of the ions. This is why the whole compound needs to be neutral, so that all the ions have the electrons they need. Covalent bonds happen when two atoms share electrons instead of transferring them from one to the other. When two elements for a compound with a covalent bond, we call this a molecular or covalent compound. -Between 2 non-metals - Sharing electrons Polar Covalent (unequal sharing) Non-polar Covalent (equal sharing) - Between metal & non-metal - Transfer of electrons

Molecular/Covalent Bond NOTES Formed by sharing electrons Between two Non-Metals Electronegativity Difference = small On the left is molecular, which means that it is sharing electrons and it is a bond between two non-metals

Carbon Dioxide How do you name this? Naming for molecular compounds is all about adding prefixes to the start of the element. When I say “carbon dioxide”, I know there are two oxygen atoms in the compound because I see the prefix “di-” which means two. I also change the ending of the second element in the compound to –ide. Carbon Dioxide

Rules for molecular bonds NOTES Lower e-negativity atom first 1st Non-Metal normal 2nd Non-Metal ends in –IDE Prefixes are used to show # of atoms Mono – 1, Di – 2, Tri – 3, Tetra – 4, Penta - 5 Mono is NEVER used with the 1st Non-Metal, Here are the rules for molecular naming. The best way to identify a molecular compound is that it will be a compound formed from two non-metals. Whichever nonmetal has a lower electronegativity goes first in the name or formula. This is why it is carbon dioxide and not dioxygen carbide, since carbon has a lower electronegativity than oxygen. The ending of the second nonmetal is always changed to –ide. The different prefixes (beginning part of the name) tell us how many of that atom there are. If the prefix is mono, it means there is one of that atom, like in carbon monoxide (CO). The prefix di- means there are two of that atom, like in carbon dioxide (CO2). Tri- means three, tetra- means four, and penta- means five. The prefix mono- is never used as a prefix for the first nonmetal in the compound, but all of the others are.

Name or Give Formula: N2O3 Dinitrogen Trioxide PCl3 Phosphorus Trichloride Sulfur Trioxide SO3 Dinitrogen Tetrabromide N2Br4 Al2S3 – Is aluminum sulfide. It is not Dialumnium Trisulfide. You do not use the prefixs because aluminum is a metal. You name just like you did at the beginning of the power point Question: How do you name Al2S3?

Now try these! …Be Careful Give the names 1)N2O5 2) AlBr3 3) Be3(PO4)2 4) Cl2O Give the formulas 5) Magnesium Sulfate 6) Calcium Fluoride 7) Diphosphorus Pentafluoride 8) Lithium Nitrite Dinitrogen Pentoxide Aluminum Bromide Beryllium Phosphate Dichlorine monoxide MgSO4 CaF2 P2F5 LiNO2

Acids: NOTES Always starts with a Hydrogen Two types 1) Does not contain oxygen Hydro ______ ic Acid (Blank = name of anion) HBr Hydrobromic Acid H2S Hydrosulfuric Acid When trying to identify what type of compound we are dealing with, the first element in the name or formula tells us a lot. If the compound starts with a metal or cation (other than H), it will be an ionic compound and follow the ionic naming rules. If the compound starts with a non-metal (right of the staircase on the PT), it will be a molecular compound and will follow the molecular naming rules. If the compound starts with a hydrogen (H), it will be an acid. The acids we are learning will always be a combination of hydrogen and an anion. If the anion does not have an oxygen, the name is made by putting hydro- as a prefix and –ic as a suffix to the name of the anion. So if I was writing the name of an acid made with bromine, I add hydro– to the front of the bromine and change the ending to –ic, making hydrobromic acid. The same is true if I am making an acid with sulfur. I add hydro- to the front and change the ending to –ic, making hydrosulfuric acid. Remember this is only for acids without oxygen.

NOTES Example: H2SO4 ate  ic Sulfuric Acid Example: H2SO3 2) Does Contain Oxygen (has a polyatomic), Don’t use hydro Change the ending of the polyatomics ate becomes ic ite becomes ous Example: H2SO4 ate  ic Sulfuric Acid Example: H2SO3 ite  ous Sulfurous Acid If the anion does have oxygen in it, we use different rules that depend on the ending of the anion. Acids with oxygen will have polyatomic anions, so we look at the ending of the anion to help us know the acid’s name. If the anion ends in –ate, the acid it forms will end in –ic. So an acid formed from the sulfate ion (SO4 2-) will have its ending changed from –ate to –ic to make sulfuric acid. If the anion ends in –ite, the acid it forms will end in –ous. So an acid formed from the sulfite ion (SO3 2-) will have its ending changed from –ite to –ous to make sulfurous acid.

I ATE big and got sICk, Take a bITE you little wOUS H2SO4 ate  ic Sulfuric Acid H2SO3 ite  ous Sulfurous Acid Here is a mnemonic device to help you remember. ATE endings have more oxygens than ITE endings, so I ATE big and got sICk reminds us that ATE endings are for the ion with more oxygen atoms (big) and we change the ending to IC (sICk). Take a bITE you little wOUS reminds us that ITE (bITE) endings are for the anion with less oxygen atoms (little) and we change the ending to ous (wOUS).

Writing the formula of an acid Look at charges and use subscripts to make charges neutral Hydronitric Acid H+1 and N-3  H3N Nitrous Acid H+1 and NO2-1  HNO2 Nitric Acid H+1 and NO3-1  HNO3 When writing the formulas for acids, the have to be neutral just like ionic compounds, but all of the positive charge comes from hydrogen. So if the anion has a 2- charge, the formula will start with H2, if the anion has a 3- charge, the formula will start with H3. A good check is to have a number of hydrogen atoms equal to the charge of the anion. + - Ø

With Acids Still: -Ic is Big -Ous is a wuss Nitric Acid vs Nitrous Acid HNo3 HNO2 Notice the endings for acids work the same as the traditional endings for metals that form ions with different charges. With traditional names for metals, the name that ended in –ic always hade the larger charge, just like the acid that has the larger number of oxygen atoms has the –ic ending. The same pattern is seen with the metals with the smaller charge ending in –ous and the acid with the smaller number of oxygen atoms ending in –ous.

Give name HCl Hydrochloric Acid HClO2 Chlorous Acid HClO3 Chloric Acid Give formula Phosphoric acid Hydrophosphoric Acid Hydrochloric Acid Chlorous Acid Chloric Acid H3PO4 H3P Make sure that you remember that the hydro has nothing to do with whether or not there is a hydrogen. All acids by definition have hydrogen. The hydro tells you whether or not the acid has an oxygen.

Try These: HNO3 H3N HNO2 Sulfurous Acid Sulfuric Acid Hydrosulfuric Acid Nitric Acid Hydronitric Acid Nitrous Acid H2SO3 H2SO4 H2S

(NH4)3P LiCl Cu2S CaF2 SO3 NaClO3 N2O Ba(OH)2 H2SO3 Ferric Nitride Diphosphorus tetrafluoride Sodium Sulfate Beryllium Phosphate Magnesium Nitrate Barium Iodide Lithium Carbonate Potassium Acetate Hydrosulfuric Acid Here is a mix of compounds to try. The answers are on the next slide.

(NH4)3P  Ammonium Phosphide LiCl  Lithium Chloride Cu2S  Copper (I) or Cuprous Sulfide CaF2  Calcium Fluoride SO3  Sulfur trioxide NaClO3  Sodium Chlorate N2O  Dinitrogen Monoxide Ba(OH)2  Barium Hydroxide H2SO3 Sulfurous Acid Ferric Nitride  FeN Diphosphorus tetrafluoride  P2F4 Sodium Sulfate  Na2SO4 Beryllium Phosphate  Be3(PO4)2 Magnesium Nitrate  Mg(NO3)2 Barium Iodide  BaI2 Lithium Carbonate  Li2CO3 Potassium Acetate  KC2H3O2 Hydrosulfuric Acid  H2S

Ide ATE BIG, with little bites S-2 = sulfIde SO4-2 = SulfATE SO3-2 = sulfite

Learning Targets I can determine the name/formula for a given molecular compound.

Homework Naming Ionic Compounds WS (from test day) Due next class You should be able to do the Binary Molecular Compounds half of the naming WS you got last class.