Simple Binary Ionic Compounds - Appohigh

Simple Binary Ionic CompoundsIonic compounds are compounds formed by the combination of a cation and a anion.(Think: "metal plus nonmetal"). Ionic compounds are more commonly known as"salts." Binary ionic compounds are compounds containing only two elements, asdemonstrated in the examples below.When writing formulas for ionic compounds, we use subscripts to indicate how many ofeach atom is contained in the compound. Remember that even though ions havecharges, ionic compounds must be neutral. Therefore, the charges on the cation andthe anion must cancel each other out. In other words, the net charge of an ioniccompound equals zero.Example 1:For a salt containing sodium ion, Na , and chloride, CI", the ratio is one to one. Thepositive charge on the sodium ion cancels out the negative charge on the chloride.( 1) (-1) 0Therefore, the formula for the salt is NaCI. (The actual formula is Na-iCli, but chemistsomit subscripts of 1).Example 2:For a salt containing calcium ion, Ca2 , and chloride, CI", the ratio can't be one to one.( 2) (-1) 1Remember that ionic compounds must be neutral. In order to yield a neutral compound,two chlorides must bond to the calcium ion:( 2) 2(-1) 0So, the formula for this salt is CaCfe.Nomenclature:When naming ionic compounds, simply write the element name of the metal followed bythe ion name of {he nonmetal. (Remember: the metal ion (cation) is always writtenfirst!)NaCI is called "sodium chloride," and CaCb is called "calcium chloride."

Nomenclature Worksheet 2:Simple Binary Ionic CompoundsPlease complete the following table:Name of Ionic CompoundFormula of Ionic Compound1. Sodium bromide2. Calcium chloride3. Magnesium sulfide4. Aluminum oxide5. Lithium phosphide6. Cesium nitride7. Potassium iodide8. Barium fluoride9. Rubidium nitride10.Barium asPa18.CS2S19.SrF220.NaCI

Polyatomic IonsPolyatomic ions contain two or more different atoms (polyatomic means "many atoms")Here are some common examplesaammonium ion, N H / (the only positive polyatomic ion you need to know)b"ATE" ions - contain an atom bonded to several oxygen atomsNitiate NOjCarbonate CO32cSulfate SO42Chlorate CIO3"ITE" ions, remove one oxygen from the ATE' ion and keep the same chargeNitrite NO2Chlorite - CIO2dPhosphate PO43Acetate ChHCO;Phosphite PO33Sulfite SO32Other common complex ionsHydroxide - OHCyanide - CNIonic Compounds Containing Polyatomic IonsAs you vo already learned, ionic compounds are formed by the combination of apositive ion (cation) and a negative ion (anion) This is the same when dealing simpleions or complex ions Be careful to note however, that complex ions are groupedtogether and should not he separated In other words don't ever separate the sulfateICon SO4 into sulfur and oxygen If it's written as a group, keep it as a group!Since complex ions come in groups, things can get tncky when using subscripts As aresult, we use parentheses to separate the ion from the subscriptIf we need two sulfates in a coirpou id we wite ISCH) if we need three nitrates in a compound, we wrte (NOjhAnd just as before the net charge of the compound must be zero For a saltcontaining sodium ion Na', and ni'rate, NO the ratio would be 1 1 since the positiveand negative charges cancel out Thetefoie, the formula is NaNCh and is called sodiumnitrate (Note no parentheses are necessary here)For a salt containing calcium ion, Ca2 , and nitrate, NO3, the ratio must be 1 2 (onecalcium ion for every two nitrates) So the formula would be Ca(N03)2.

Nomenclature Worksheet 3:Ionic Compounds Containing Polyatomic IonsPlease complete the following table:Name of ionic CompoundFormula of Ionic Compound1. Sodium chromate2. Calcium carbonate3. Magnesium nitrate4. Aluminum sulfate5. Lithium phosphate6. Ammonium chloride7. Cesium chlorate8. Potassium sulfate9. Barium acetate10.Rubidium 0.NH4OH

Ionic Compounds Containing Transition MetalsThe transition metals are the elements located in the middle of the periodic table (in groups 312 Unlike the group 1A and 2A metal ions, the charges of transition metal ions are not easilydetermined by their location on the periodic table Many of them have more than one charge(also known as an oxidation state) There are eight transition metals that you should highlighton your periodic tableCo, Cr, Cu, Fe, Mn, Hg, Sn, and PbEach of these elements form more than one ion and therefore must be labeled accordinglyFor example, iron forms two ions Fe2 and Fe3 . We ccall these ions "iron (II) ion" and "iron (IIion" respectively (See "Table of Transition Metal Ions"When naming any ion from the elements listed above, you MUST include a Roman numeral inparentheses following the name of the ion The this roman numeral is equal to the charge onthe ion We don't include the " " because all metal ions are positive Here are two moreexamplesPb4 "lead (IV) ion"cr "chromium (III) ionSimilarly, when naming a compound containing one of these transition metals, you mustinclude the Roman numeral as well "Iron Chloride" isn't specific enough since the compoundcould contain either iron (II) or iron (III) ion You must specify the charge on the ironIron (II) chloride contains the Fe2 ion When combined with chloride, CI, we know the formulamust be FeCIaIron (III) chloride contains the Fe3 ion This time, three chlorides are required to form a neutralcompound Therefore, the formula is FeCIsBy looking at the formula of an ionic compound, we can determine the charge (oxidationstate) of the metal.Example Write the name of C02O31234Recognize that Co, cobalt, is a transition metal This means that you must include a Romannumeral after its name So, the basic name will be Cobalt ( ) OxideTo find the charge on cobalt, use oxide as a key Oxide has a charge o f - 2 so three oxideswill have a charge of - 6What balances a - 6 charge 9 A 6 chargei So, the positive half of the compound mustequal 6Since there are two cobalt ions, the charge is split between them So, each one has a 3charge Therefore, we are using the Co3 ion and the compound is called cobalt (III) oxide.Remember that anions (negative ions) always have a definite charge When dealing withcompounds containing transition metals, look to the anion first Determine the charge of theanion and then solve to figure out the charge of the cationWhen dealing with metals other than the transition metals, you don't need Roman numerals Inother words, calcium ion, Ca2 is always 2 Don't call CaCIs "calcium (II) chloride " Its name is"calcium chloride"

Nomenclature Worksheet 4:Ionic Compounds Containing Transition MetalsPlease complete the following table:Name of Ionic CompoundFormula of Ionic Compound1. Copper (II) sulfate2. Copper (I) oxide3. Chromium (III) cyanide4. Cobalt (II) hydroxide5. Silver bromide6. Zinc nitrate7. Iron (III) acetate8. Lead (IV) 214.CuCIOs15.Cr(OH)316.HgzO

Nomenclature Worksheet 5:Ionic Compounds SummaryName the following compounds:Give the formula for each compound:1. CaF223.sodium fluoride2. Na2024. potassium sulfide3. BaS25.calcium carbonate4. CUSO426. magnesium hydroxide5. Fe20327.zinc nitrate6. HgCfe28.silver acetate7. AgN0329.copper (II) oxide8. MgCOs30.iron (III) chloride9. KC2H3O23 1 . barium chromate10.K2Cr2O732.aluminum oxide11.AI(OH)333.lead (II) sulfate12.PbBr234.tin (IV) oxalateIS.ZnSOs35.calcium phosphate14.NaHC0336.lithium permanganateI5.NH4CI37. mercury (I) nitrate16.Li3P0438. radium sulfite17.SnCl239.chromium (III) chloride18.AI(N02)340.ammonium sulfide19.Rb2Cr044 1 . copper (II) acetate20.KMnO442.calcium bicarbonate21.CuCI43.tin (II) oxide22.FeS0444.silver sulfite

Naming Binary Covalent CompoundsBinary covalent compounds come from the combination of two nonmetals (or anonmetal and a metalloid). These compounds do not involve ions; as a result, theyhave a slightly different naming system. Chemists use prefixes to indicate the numberof atoms in each compound. The prefixes are listed in the table below:# of OctaNonaDecaWhen naming binary covalent compounds, the first element name is given followed bythe second element with an "ide" ending. The first element gets a prefix when there ismore than one atom in the compound* The second element ALWAYS gets a prefix.Here are some examples:CompoundNameNO*N2ONitrogen MonoxideDinitrogen MonoxideNitrogen DioxideDinitrogen TrioxideDinitrogen TetraoxideDinitrogen PentaoxideNO2*N2O3N2O4N205Notice that the prefix "mono" is omitted in these casesPrefixes are necessary when naming covalent compounds because the atoms cancombine in any whole number ratio. N2O, for example, cannot simply be called"nitrogen oxide," because there are several other compounds that contain nitrogen andoxygen. We must specify that there are two nitrogen atoms bonded to a single oxygenatom.When dealing with ionic compounds, there is only one way for a cation and a nion tocombine to form a neutral compound. As a result, there is no need to use prefixes.This is why CaCb is called "calcium chloride," rather than "calcium dichloride."

Nomenclature Worksheet 6Binary Covalent CompoundsPlease complete the followngName of Covalent1carbon dioxide2phosphorus trnodide3sulfur dichloride4mtroaen tnfluonde5dioxygen difluondetableCompoundFormula of Covalent6N2F4fSCI48CIF39S1O2Compound10 P40,oDetermine whether the following compounds are covalent or ionic and give them theirproper names1Ba(N03)22CO3PCI34Kl5CF46MgO7CU2S8SO?9NCI310 XeFe

Mar 18, 2015 · Remember that ionic compounds must be neutral. In order to yield a neutral compound, two chlorides must bond to the calcium ion: ( 2) 2(-1) 0 So, the formula for this salt is CaCfe. Nomenclature: When naming ionic compounds, simply write the element na