Lewis Dot Structures Worksheet - Mr. Walsh's Class

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Chemical Bonds – Ionic BondsIdentify the Number of Valance Electrons and Draw the Lewis Dot StructureNotes: Scientists use Lewis Dot Structures to show the valance electrons of an element as dots. Since bonding involves the valance shell electrons only, it is only necessary to illustrate those outer electrons.ElementBohr DiagramGroup Number (PT)# of Valance ElectronsLewis Dot StructureCalciumCarbonHydrogenHeliumOxygenFluorineNeonSodiumAluminumDetermining the Ionic ChargeElementPropertyBefore Making an OctetAfter Making an OctetLielectron config# protons#electronschargeBohr DiagramLewis Dot StructureBeelectron config# protons#electronschargeBohr DiagramLewis Dot StructureBelectron config# protons#electronschargeBohr DiagramLewis Dot StructureSkip CarbonNelectron config# protons#electronschargeBohr DiagramLewis Dot StructureOelectron config# protons#electronschargeBohr DiagramLewis Dot StructureFelectron config# protons#electronschargeBohr DiagramLewis Dot StructureNeelectron config# protons#electronschargeBohr DiagramLewis Dot Making Ions – Ionic Bonds are made of Ions. A strong understanding of Ions is needed.Notes: Remember that Metals tend to lose their electrons, falling back to their inner octet, becoming smaller, forming positive “cations”. Nonmetals tend to gain electrons, filling up their current energy levels, becoming larger, forming negative “anions”. Complete the chart below.ElementLewis Dot # of Valance e-Gain/Lose ___ e-Valance ChargeNa1L 1+1BeClSAlNeKNOCaPBMgLewis Dot, Formula Unit & Naming Practice Sheet Notes: An ionic bond is an attraction of a cation for an anion resulting from the transfer of electrons. Remember, the smaller nonmetals are more electronegative and pull the electrons close, away from the larger, less electronegative metals. When naming ionic compounds, the Metal is named first, followed by the nonmetal with an –ide ending. Ex. Sodium Fluorine becomes Sodium Fluoride.Formula Unit: Lowest whole number ratio of elements in the compound. Ex. Ca3N21. Draw the Lewis Structure for Mg & ClFormula Unit: _________Name of Compound: 2. Draw the Lewis Structure for Mg & SFormula Unit: _________Name of Compound: 3. Draw the Lewis Structure for K & FFormula Unit: _________Name of Compound:4. Draw the Lewis Structure for K & OFormula Unit: _________Name of Compound:5. Draw the Lewis Structure for Be & NFormula Unit: _________Name of Compound:6. Draw the Lewis Structure for Ca & PFormula Unit: _________Name of Compound:7. Draw the Lewis Structure for Al & FFormula Unit: _________Name of Compound:8. Draw the Lewis Structure for Ca & IFormula Unit: _________Name of Compound:9. Draw the Lewis Structure for Rb & OFormula Unit: _________Name of Compound:10. Draw the Lewis Structure for Sr & FFormula Unit: _________Name of Compound:11. Draw the Lewis Structure for Al & ClFormula Unit: _________Name of Compound:12. Draw the Lewis Structure for Mg & PFormula Unit: _________Name of Compound:13. Draw the Lewis Structure for B & OFormula Unit: _________Name of Compound:14. Draw the Lewis Structure for Be & SFormula Unit: _________Name of Compound: Write the Formula / Formula Unit for the following CompoundsDetermining the formula for Magnesium Fluoride? Identify the charges = Mg2+ F1Cross the Charges, Mg2+ F1 = Mg1F2If the subscript is a 1 it does not need to be written. If there is a common subscript such as 2 as in Mg2O2, reduce it to Mg1O1 which is also MgO.Write Formula Unit For the Below Ionic CompoundsNameCation (+)Anion (-)Formula1Sodium ChlorideNa1+Cl1-Na1+1Cl1-1 = NaCl2Aluminum ChlorideAl3+Cl1-3Aluminum Phosphide4Magnesium Oxide5Cesium Fluoride6Strontium Nitride7Lithium Sulfide8Calcium Chloride9Sodium Bromide10Beryllium Iodide11Strontium Fluoride12Aluminum Fluoride13Potassium Nitride14Sodium Sulfide15Lithium Oxide16Calcium OxidePolyatomic Ions WSAmmonium (NH4)1+Carbonate (CO3)2-Chromate (CrO4)2-Dichromate (Cr2O7)2-Hydroxide (OH)1-Nitrate (NO3)1-Nitrite (NO2)1-Sulfate (SO4)2-Sulfite (SO3)2-Phosphate (PO4)3-Write the NAME of each of the following compounds.(NH4)Cl _______________________________Be(SO4) _______________________________(NH4)3N ______________________________MgCl2 ______________________________NH4(NO3)______________________________Sr3(PO4)2 _____________________________Zn(CrO4)2 _____________________________K2(Cr2O7) ______________________________Ga(ClO3)3 ____________________________Cu(OH) ***______________________________(NH4)3(PO4)___________________________Fe(SO4)_____________________________Mg(NO3)2___________________________(NH4)NO2 ____________________________Na2(Cr2O7)____________________________Na(OH) ______________________________Write the CHEMICAL FORMULA for each of the given NAMES…………cross chargescalcium carbonate Ca2+ (CO3)2- = Ca2(CO3)2 = CaCO3barium nitrate_______________________________ = _______________________________ammonium sulfate _______________________________ = _______________________________aluminum hydroxide ______________________________ = ________________________________calcium phosphate_______________________________ = _______________________________cesium nitrate _______________________________ = _______________________________sodium nitrite _______________________________ = _______________________________calcium sulfate_______________________________ = _______________________________beryllium sulfate_______________________________ = _______________________________sodium carbonate_______________________________ = _______________________________magnesium phosphate_____________________________ = _______________________________calcium phosphate_______________________________ = _______________________________Variable Charge CationsNotes: Some cations can have many charges, they are known as variable charge cationsIt is important to note the charge of the cation when naming the ionic compoundEx: Tin (VI) Oxide….where VI is the charge on tin.Draw SnO3 instead as a picture of Atoms:Total Charge on Oxygen = -6Total Charge on Tin = +6Individual Charge on Tin = +6Name of Compound = Tin (VI) OxideDraw Au3N as a picture of Atoms: Name of Compound = ______________Draw Sn2O3 instead as a picture of Atom Name of Compound = ________________Draw Ag1O3 instead as a picture of AtomName of Compound = ________________What is the name of SnO3? Tin Oxide = Wrong AnswerSince tin has more than once charge, the charge needs to be determined so it can be included in the name.The charge on tin was calculated to be +6, therefore the +6 is included in the naming of the compound. Once again, this is only done with metals with more than one charge.What is the name of Sn2O3? What is the name of Cu N?What is the name of Au3N? What is the name of CuNO3?Complete the Following Questions on Formula UnitsWhat is the Formula Unit for Silver (III) Nitride ____________________________What is the Formula Unit for Vanadium (III) Chloride __________________________What is the Formula Unit for Lead (IV) oxide ____________________________What is the Formula Unit for Silver (II) Nitride ____________________________What is the Formula Unit for Vanadium (II) Chloride ___________________________What is the Formula Unit for Lead (II) oxide ____________________________Write the formula for the variable charged binary ionic compounds:Nickel (II) chloride_________________Gold (III) oxide___________________Cobalt (II) phosphide_______________Copper (I) bromide_________________Iron (III) chloride__________________Copper (II) chloride________________Copper (I) bromide_________________Cobalt (II) phosphide_______________Manganese (III) bromide____________Iron (III) fluoride_________________Name the variable charged compounds……use I, II, III, IVPb Br4__________________________Pb3 N2__________________________Cu2 S___________________________Pb O2___________________________Cu Br___________________________Cu O___________________________Ni O2___________________________Cu2 S___________________________Ions in Chemical CompoundsComplete the following table, being sure that the total charge on the resulting compound is zero. IonsChlorideCl1-Hydroxide(OH)1-Nitrate(NO3)1-Sulfate(SO4)2-Sulfide S2-Carbonate (CO3)2-Phosphate(PO4)3-HydrogenHSodiumNaAmmoniumNH41+PotassiumKCalciumCaMagnesiumMgAluminumAlIron (I)FeIron (II)FeStrontiumSrIron (III)FeLead (II)PbTin (IV)SnCopper (I)CuHydrogenH Ionic ReviewElement# of Valance e-# of e- Gain or LoseIonic Charge1Cl2Na3Mg4O5N6Al7XeBelow, pay attention what is given and what is being asked. The chart below is not how the test will be worded. Refer to handouts for additional examples.NameCationAnionChemical Formula8Potassium Sulfide9Potassium Phosphide10Beryllium Fluoride11Sr I212KF13CaO14Copper (II) Fluoride15Tin (I) Sulfide16AgO217Al(CO3)2-18Na(SO4)2-19XenonNAME the Ionic Compound_________________________Ca I2___________________________ Mg O___________________________***Cu S____________________________***Cr N_________________________***V3 (PO4)2 ____________________________Li2S__________________________________________Mg(NO3)2__________________________________________Be3(PO4)2How are Ionic Bonds formed and what is the attractive force within an Ionic Bond? Draw the transfer of electrons within Aluminum Chloride.Using Lewis Dot Structures:Write the Chemical Formula: ______________Draw the transfer of electrons within Barium Sulfide.Using Lewis Dot Structures:Write the Chemical Formula:______________Show what would happen if Ba2+ and F1 bonded.Criss-Cross Name of Compound: ____________Chemical Formula: ___________Show what would happen if Chromium (II) and Sulfur bonded.Criss-CrossName of Compound: ____________Chemical Formula: _____________From the review sheet, list an example of a POLYATOMIC Ion: ______________________From the review sheet, list an example of a BINARY ionic compound: _________________From the review sheet, list an example of a TERNARY ionic compound:________________Explain what is meant when at atom gains or loses an electron in reference to the octet rule.Ho do you distinguish between an ionic and a covalent compound?______________Ionic ReviewElement# of Valance e-# of e- Gain or LoseIonic Charge1Cl2Na3Mg4O5N6Al7XeBelow, pay attention what is given and what is being asked. The chart below is not how the test will be worded. Refer to handouts for additional examples.NameCationAnionChemical Formula8Potassium Sulfide9Potassium Phosphide10Beryllium Fluoride11Sr I212KF13CaO14Copper (II) Fluoride15Tin (I) Sulfide16AgO217Al(CO3)2-18Na(SO4)2-19XenonNAME the Ionic Compound_________________________Ca I2___________________________ Mg O___________________________***Cu S____________________________***Cr N_________________________***V3 (PO4)2 ____________________________Li2S__________________________________________Mg(NO3)2__________________________________________Be3(PO4)2How are Ionic Bonds formed and what is the attractive force within an Ionic Bond? Draw the transfer of electrons within Aluminum Chloride.Using Lewis Dot Structures:Write the Chemical Formula: ______________Draw the transfer of electrons within Barium Sulfide.Using Lewis Dot Structures:Write the Chemical Formula:______________Show what would happen if Ba2+ and F1 bonded.Criss-Cross Name of Compound: ____________Chemical Formula: ___________Show what would happen if Chromium (II) and Sulfur bonded.Criss-CrossName of Compound: ____________Chemical Formula: _____________From the review sheet, list an example of a POLYATOMIC Ion: ______________________From the review sheet, list an example of a BINARY ionic compound: _________________From the review sheet, list an example of a TERNARY ionic compound:________________Explain what is meant when at atom gains or loses an electron in reference to the octet rule.Ho do you distinguish between an ionic and a covalent compound?______________ ................
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