Metals Vs. Non-Metals; Dot Diagrams; Ions

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Name:Period:Metals are on the left side. Non-metals on the right.Metals tend to lose electrons. Non-metals gain them tight.Metals versus Non-MetalsThe dividing line is the red or bold black linefrom between Boron and Aluminum down andto the right. Everything to the left is a metal:to the right, non-metal. One exception (don’tya just hate that?!) is hydrogen – a non-metal.Sodium (Na) is a metal.Oxygen is a non-metal.Metal or lium:SilverHelium:NitrogenNon-metal Br36KrMetalsEasy to remember by which sideiron (Fe) is on—the left side!Put the correct number of valenceelectrons around the chemicalsymbol in this order in pairs:485Ne22HeNon-MetalsOn either side of the divide arethe metalloids or semi-metals—they have characteristics ofboth: B, Si, Ge, As.Dot Diagrams (sometimes known as Lewis dot diagrams) are a depiction of anatom’s valence electrons. They are a powerful tool in helping you understand,see, and even predict molecular bonding.Dot Diagrams1Ch. 19:1Metals vs. Non-Metals; Dot Diagrams; IonsNotice that the electrons arein pairs not a circle.37Why would the electronsspread out around the atominstead of bunching up?6Neon has 8 valence electrons(in the right hand column).Neon has no unoccupied spaces.It is full.LiLithium, with 1 valence electron(first column).CCarbon has 4 valence electronsOOxygen has 6 valence electrons.How many more before it’s full?.Draw the Dot Diagrams for the following elements:BerylliumSodiumHeliumCarbonBoronCopyright 2003, C. Stephen Murray

Name:Ch. 19:1Period:If you change the number of protons you change the element.If you change the number of neutrons you change the isotope.If you change the number of electrons you change the ion.IonsNeutral atoms have an equalnumber of protons and electrons.A neutral atom has a net electricalcharge of zero.Why would atoms gain or loseelectrons? To fulfill the octet ruleand end up with a full outer shellof electrons. Metals will loseelectrons and make positive ions(cations); non-metals will gainelectrons and make negative ions(anions).LithiumLiLithiumLi 1 Loses anelectron3p3n3 protons ( 3)3 electrons (-3) 3 –3 0Neutral atom!3 protons ( 3)2 electrons (-2) 3 –2 1positive ion!Protons – electrons ion chargeCations cough up electrons Lose electrons ( ion).METALSAnions accept electrons Gain electrons (- ion).NON-METALSWhat is the charge of anatom with 16 protons and18 electrons?Ex. How many electrons does Mg 2 have?Na 1 p - e charge12 (Mg) - e 212 2 e12—2 ee 10 electronsChemical symbolORIf Oxygen gains 2 electronswhat charge will it have?Ion NotationCharge(1 electron lost)An ion is an atomwith a net charge;that has gained orlost electrons.3p3np – e chargeIf Beryllium loses 2 electronswhat charge will it have?You also could have found this byknowing Mg has 12 protons andelectrons if neutral. A 2 chargemeans it is a cation—it lost 2electrons 12—2 10 electrons.How many electrons does Cl 1– have?How many electrons does N 3– have?How many electrons does Al 3 Give the ion notation for an atom with20 protons and 18 electrons.Give the ion notation for an atom with6 protons and 2 electrons.Give the ion notation for an atom with15 protons and 18 electrons.Copyright 2003, C. Stephen Murray

Name:Period:Ch. 19:2BondingWhy haven’t you grown up recognizing all of the elements around you? Becausemost substances are compounds. Very few elements are stable enough to existpure. Instead they react with other elements to form compounds. Why?.Chemical BondingOctet Rule—atoms strive toachieve a full set of valenceelectrons. This is usually 8 (whatare the exceptions). Atoms aremore stable with a full outer shell.Why? Having a few more protons morethan closest noble gas, metals have toomuch shielding—the electrons don’t fellmuch attraction to the nucleus. Non-metalhave more protons and can attract moreelectrons to the energy level.To fulfill the octet rule atoms willlose, gain, or share electrons. Atomswill get 8 valence electrons the fastest way: metals will lose electrons;non-metals will gain electrons.Ion—a non-neutral atom (different number of protons and electrons). To find chargeor number of electrons, use: protons—electrons charge OR p - e chargeIon Notation ReviewMg 2 Give the ion notation for an atomwith 20 protons and 18 electrons.Give the ion notation for Sulfurwith 18 electrons.Charge(2 electrons lost)Chemical symbolCations — positive ions (metals);Losers of electrons.Anions — negative ions (non-metals);Gainers of electrons.What force will the two above ions feel?Why?Ionic Bonds—Bonds of attractionIonic bonds occur between metal and non-metal ions.By itself sodiumis very reactive(it will explodein water).So itloses oneelectron.Now, it has a full setof 8 outer electrons.It becomes a positiveion (a cation).Na1 NaAnd opposites attract1 Na1-ClTo forma stablecompound.Will these ions make compounds?Chlorine (a poisonousgas) has 7 valenceelectrons so it needsone more to be stable.So itgains oneelectron.ClNaClNow, it has a full setof 8 outer electrons.It is a ion with a 1 charge (a cation).Cl1-Sodium Chloride —Table salt.Will these elements make ionic compounds?Mg 2 and Li 1 ?Ca 2 and F 1- ?K and Li?Al and F ?Na 1 and O 2- ?O 2- and Cl 1- ?Be and Cl?Fe and O?Copyright 2003, C. Stephen Murray

Name:Ch. 19:2Period:Covalent Bonds—Cooperative BondingSometimes there are no opposites around to formionic bonds (Oh, NO!), but atoms will still find away to get to that full shell of 8 valence electrons.So instead of gaining extra electrons they SHARETHEM. This is called a COVALENT BOND.ClSharing one electron eachShort cut notationfor a single bond.Draw the covalent bond between 2 Nitrogens:OOOOOShort cut notationfor a double bond.Sharing 2 electrons eachDraw the covalent bond between 2 Fluorines:Ionic or covalent bonds?MgOPO5 CaOCO2BeF2 SO2The ions charges that atoms gain when they lose or gain their valenceelectrons are the number of electrons they can gain or lose when bonding.We call these Oxidation Numbers.Oxidation NumbersOxidation Numbers1Cl—ClCl ClClEach oxygen needs2 more electrons.OCovalent bonds happenbetween two 5Br36KrTransition MetalsFind the Oxidation Numbers for the following:BeHOHeClAlNPLiArYou can figure out how to make stable ionic compounds from the oxidation numbers.Lithium (1 ) can give 1 electron; Oxygen (2-) needs 2 to be full. So Oxygen needs2 Lithiums to balance as a compound.Make ionic compounds from:Write the chemicalEx.Makeabalancedionicsymbols with thecompound of Calcium and Oxygen.oxidation numbers.Na and S:Al and Cl:Making Ionic Compounds1 Li1 O 22Li1 23 Li2OO 12-Cross thenumbers notthe signs.Reducenumbers ordrop ones.1. Ca 2 O 2-Chemical symbols andoxidation numbers.2. Ca 2 O 2-22Cross the numbersnot the signs3. CaO (2s reduce)Reduce numbers anddrop ones.Copyright 2003, C. Stephen Murray

Name:Period:Most elements react to form compounds. Elements do this to gain a fullset of valence electrons (Octet Rule— “If I 8 I full”).Bonding ReviewIonic Compounds occur betweenmetals and non-metals becausemetals become cations (positiveions) and non-metals becomeanions (negative ions). Andopposites attract.Covalent Compounds occur betweennon-metals. Because neither elementwill give up their electrons (too manyprotons), they share electrons to complete the full set of 8.Polyatomic Compounds arecompounds with 3 or more elements.These are just large ionic compounds.They happen because sometimeswhen two elements react they don’tfulfill the octet rule and end up with anet electrical charge.Oxygens sharing to gain8 electrons eachOpposites attractBe2 Ch. 19:3More Chemical BondingCl1-OOOBig opposites attract, tooOMg2 4 shared electrons(2 from each)Cross the number not thesign to get:BeCl2OBeryllium ChlorideONO3-Mg(NO3)2Short cut notationfor a double bond.Magnesium nitrateIonic, Covalent, or Polyatomic?K2O(Potassium oxide)AlF3(Aluminum fluoride)Li2CrO4(Lithium chromate)Ca3N2(Calcium nitride)CO2(Carbon dioxide)MgCO3(Magnesium carbonate)SiCl4(Silicon tetrachloride)NaCl(Sodium chloride—table salt)Use dot diagrams like puzzle pieces.For ionic compounds rememberthat the metal is actually losing theelectron to the non-metal.NaClMaking Ionic CompoundsOr use the “cross the numbernot the sign” method:Ca12 Cl12This compound will be stablebecause the net charge is zero.1(2) 2(-1) 2 - 2 0Na ClMake Balanced Ionic CompoundsLi and NCa and OAl and ClNa and NeIonic compounds are balanced if thenet charge is zero. Use this formula:Number of atomsof element 1 and 2O1(N1) O2(N2) CNNet charge- if zero,then it isan ioniccompoundOxidationnumbers ofion 1 and 2Using the formula above show that Na2Ois balanced.Copyright 2003, C. Stephen Murray

Name:Ch. 19:3Period:Covalent Bonds—Diatomic MoleculesSeeing how covalent bonds connect together is easyfor single bonds, like chlorine. Yet it can be hard tosee for triple bonds like Nitrogen. For compounds itcan get even more difficult.ClOOOOCl—ClCl ClSharing one electron eachEach line stands for a sharedpair of electrons: 1 from eachEach oxygen needs2 more electrons.OClDiatomic molecules have 2 atoms ofthe same element. N, O, F, ClShort cut notationfor a single bond.Draw the covalent bond between two Bromineatoms:OShort cut notationfor a double bond.Sharing 2 electrons eachTwo Tricks—1) If you cover one of the atoms up with a piece of paper (or a finger) youcan see if the other atom has the necessary 8 electrons.Draw the covalent bond between two Fluorineatoms:2) The number of extra electrons you need to make 8 goes on the sharingside of the chemical symbol. Ex. Nitrogen has 5 valence electrons andneeds 3 more to be full, so put 3 electrons on the side toward the other N.When trying to figure out covalentcompounds, it may take some timeand creativity. Remember to look atthe atoms as puzzle pieces.Covalent CompoundsDraw the covalent compound of CO2:Ex. Make Sulfur Dichloride (SCl2)6 valenceelectrons7 valenceelectronsSClClTip: it can help to drawthe electrons differently(like x’s and o’s) for thedifferent elements. Thiscan help you keep trackfrom where the electronscame.Move them around until eachatom has 8 electrons by sharing.Draw the covalent compound of NF3:Short hand notationS ClCl S ClClEach bar is a sharedelectron pairDraw the covalent compound of CH4 (methane):Make Carbon monoxide (CO)OCCarbonhasonly 6COOxygen needs 2 more electrons,but carbon needs 4. Eitheroxygen will have too many, orcarbon will have too few.This is why CO is an unstable,poisonous compound! It willreact with oxygen in your body toform CO2 and could kill you!Copyright 2003, C. Stephen Murray

Flinn Scientific’s Student Safety ContractPURPOSEScience is a hands-on laboratory class. Youwill be doing many laboratory activitieswhich require the use of hazardouschemicals. Safety in the science classroom isthe #1 priority for students, teachers, andparents. To ensure a safe science classroom,a list of rules has been developed and provided to you in this student safety contract.These rules must be followed at all times.Two copies of the contract are provided. Onecopy must be signed by both you and a parent or guardian before you can participate inthe laboratory. The second copy is to be keptin your science notebook as a constantreminder of the safety rules.GENERAL RULES1. Conduct yourself in a responsible manner at all times in the laboratory.2. Follow all written and verbal instructions carefully. If you do not understanda direction or part of a procedure, ask theinstructor before proceeding.3. Never work alone. No student may workin the laboratory without an instructorpresent.4. When first entering a science room, donot touch any equipment, chemicals, orother materials in the laboratory areauntil you are instructed to do so.5. Do not eat food, drink beverages, orchew gum in the laboratory. Do not uselaboratory glassware as containers forfood or beverages.6. Perform only those experiments authorized by the instructor. Never do anything in the laboratory that is not calledfor in the laboratory procedures or byyour instructor. Carefully follow allinstructions, both written and oral.Unauthorized experiments are prohibited.7. Be prepared for your work in the laboratory. Read all procedures thoroughlybefore entering the laboratory.8. Never fool around in the laboratory.Horseplay, practical jokes, and pranksare dangerous and prohibited.9. Observe good housekeeping practices.Work areas should be kept clean and tidyat all times. Bring only your laboratoryinstructions, worksheets, and/or reportsto the work area. Other materials (books,purses, backpacks, etc.) should be storedin the classroom area.10. Keep aisles clear. Push your chair underthe desk when not in use.11. Know the locations and operating procedures of all safety equipment includingthe first aid kit, eyewash station, safetyshower, fire extinguisher, and fire blanket. Know where the fire alarm and theexits are located.12. Always work in a well-ventilated area.Use the fume hood when working withvolatile substances or poisonous vapors.Never place your head into the fume hood.13. Be alert and proceed with caution at alltimes in the laboratory. Notify theinstructor immediately of any unsafeconditions you observe.14. Dispose of all chemical waste properly.Never mix chemicals in sink drains.Sinks are to be used only for water andthose solutions designated by theinstructor. Solid chemicals, metals,matches, filter paper, and all other insoluble materials are to be disposed of inthe proper waste containers, not in thesink. Check the label of all waste containers twice before adding your chemical waste to the container.15. Labels and equipment instructions mustbe read carefully before use. Set up anduse the prescribed apparatus as directedin the laboratory instructions or by yourinstructor.16. Keep hands away from face, eyes,mouth and body while using chemicalsor preserved specimens. Wash yourhands with soap and water after performing all experiments. Clean all worksurfaces and apparatus at the end of theexperiment. Return all equipment cleanand in working order to the proper storage area.17. Experiments must be personally monitored at all times. You will be assigned alaboratory station at which to work. Donot wander around the room, distractother students, or interfere with the laboratory experiments of others.18. Students are never permitted in thescience storage rooms or preparationareas unless given specific permissionby their instructor.19. Know what to do if there is a fire drillduring a laboratory period; containersmust be closed, gas valves turned off,fume hoods turned off, and any electrical equipment turned off.20. Handle all living organisms used in alaboratory activity in a humane manner.Preserved biological materials are to betreated with respect and disposed ofproperly.“Your Safer Sourcefor Science Supplies”21. When using knives and other sharpinstruments, always carry with tips andpoints pointing down and away. Alwayscut away from your body. Never try tocatch falling sharp instruments. Graspsharp instruments only by the handles.22. If you have a medical condition (e.g.,allergies, pregnancy, etc.), check withyour physician prior to working in lab.CLOTHING23. Any time chemicals, heat, or glasswareare used, students will wear laboratorygoggles. There will be no exceptions tothis rule!24. Contact lenses should not be worn in thelaboratory unless you have permissionfrom your instructor.25. Dress properly during a laboratory activity. Long hair, dangling jewelry, andloose or baggy clothing are a hazard inthe laboratory. Long hair must be tiedback and dangling jewelry and loose orbaggy clothing must be secured. Shoesmust completely cover the foot. No sandals allowed.26. Lab aprons have been provided for youruse and should be worn during laboratory activities.ACCIDENTS AND INJURIES27. Report any accident (spill, breakage,etc.) or injury (cut, burn, etc.) to theinstructor immediately, no matter howtrivial it may appear.28. If you or your lab partner are hurt,immediately yell out “Code one, Codeone” to get the instructor’s attention.29. If a chemical splashes in your eye(s) oron your skin, immediately flush withrunning water from the eyewash stationor safety shower for at least 20 minutes.Notify the instructor immediately.30. When mercury thermometers are broken, mercury must not be touched.Notify the instructor immediately.HANDLING CHEMICALS31. All chemicals in the laboratory are to beconsidered dangerous. Do not touch,taste, or smell any chemicals unlessspecifically instructed to do so. Theproper technique for smelling chemicalfumes will be demonstrated to you.32. Check the label on chemical bottlestwice before removing any of the contents. Take only as much chemical asyou need.33. Never return unused chemicals to theiroriginal containers.P.O. Box 219, Batavia, IL 605101-800-452-1261 Fax: (866) 452-1436flinn@flinnsci.com www.flinnsci.com 2004, Flinn Scientific, Inc. All Rights Reserved. Reproduction permission is granted to science teachers who are customers of Flinn Scientific, Inc. Batavia, Illinois, U.S.A. No part of this material may be reproduced or transmitted in any form or by any means, electronic or mechanical, including, but not limited to photocopy, recording, or any information storage and retrieval system, without permission in writing from Flinn Scientific, Inc.

Flinn Scientific’s Student Safety Contract34. Never use mouth suction to fill a pipet.Use a rubber bulb or pipet pump.35. When transferring reagents from onecontainer to another, hold the containersaway from your body.36. Acids must be handled with extremecare. You will be shown the propermethod for diluting strong acids. Alwaysadd acid to water, swirl or stir the solution and be careful of the heat produced,particularly with sulfuric acid.37. Handle flammable hazardous liquids overa pan to contain spills. Never dispenseflammable liquids anywhere near an openflame or source of heat.38. Never remove chemicals or other materials from the laboratory area.39. Take great care when transporting acidsand other chemicals from one part of thelaboratory to another. Hold themsecurely and walk carefully.HANDLING GLASSWAREAND EQUIPMENT40. Carry glass tubing, especially longpieces, in a vertical position to minimizethe likelihood of breakage and injury.41. Never handle broken glass with yourbare hands. Use a brush and dustpan toclean up broken glass. Place broken orwaste glassware in the designated glassdisposal container.42. Inserting and removing glass tubingfrom rubber stoppers can be dangerous.Always lubricate glassware (tubing, thistle tubes, thermometers, etc.) beforeattempting to insert it in a stopper.Always protect your hands with towelsor cotton gloves when inserting glasstubing into, or removing it from, a rubber stopper. If a piece of glasswarebecomes “frozen” in a stopper, take it toyour instructor for removal.43. Fill wash bottles only with distilledwater and use only as intended, e.g., rinsing glassware and equipment, or addingwater to a container.44. When removing an electrical plug fromits socket, grasp the plug, not the electrical cord. Hands must be completely drybefore touching an electrical switch,plug, or outlet.45. Examine glassware before each use.Never use chipped or cracked glassware.Never use dirty glassware.46. Report damaged electrical equipmentimmediately. Look for things such asfrayed cords, exposed wires, and looseconnections. Do not use damaged electrical equipment.47. If you do not understand how to use apiece of equipment, ask the instructor forhelp.48. Do not immerse hot glassware in coldwater; it may shatter.HEATING SUBSTANCES49. Exercise extreme caution when using agas burner. Take care that hair, clothingand hands are a safe distance from theflame at all times. Do not put any substance into the flame unless specificallyinstructed to do so. Never reach over anexposed flame. Light gas (or alcohol)burners only as instructed by the teacher.50. Never leave a lit burner unattended.Never leave anything that is beingheated or is visibly reacting unattended.Always turn the burner or hot plate offwhen not in use.51. You will be instructed in the propermethod of heating and boiling liquids intest tubes. Do not point the open end ofa test tube being heated at yourself oranyone else.52. Heated metals and glass remain veryhot for a long time. They should be setaside to cool and picked up with caution. Use tongs or heat-protectivegloves if necessary.53. Never look into a container that is beingheated.54. Do not place hot apparatus directly onthe laboratory desk. Always use an insulating pad. Allow plenty of time for hotapparatus to cool before touching it.55. When bending glass, allow time for theglass to cool before further handling. Hotand cold glass have the same visualappearance. Determine if an object is hotby bringing the back of your hand closeto it prior to grasping it.QUESTIONS56. Do you wear contact lenses?! YES ! NO57. Are you color blind?! YES ! NO58. Do you have allergies?! YES ! NOIf so, list specific allergies“Your Safer Sourcefor Science Supplies”AGREEMENTI, ,(student’s name) have read and agreeto follow all of the safety rules setforth in this contract. I realize that Imust obey these rules to ensure myown safety, and that of my fellow students and instructors. I will cooperateto the fullest extent with my instructorand fellow students to maintain a safelab environment. I will also closelyfollow the oral and written instructionsprovided by the instructor. I am awarethat any violation of this safety contract that results in unsafe conduct inthe laboratory or misbehavior on mypart, may result in being removedfrom the laboratory, detention, receiving a failing grade, and/or dismissalfrom the course.Student SignatureDateDear Parent or Guardian:We feel that you should be informedregarding the school’s effort to createand maintain a safe science classroom/laboratory environment.With the cooperation of the instructors, parents, and students, a safetyinstruction program can eliminate,prevent, and correct possible hazards.You should be aware of the safetyinstructions your son/daughter willreceive before engaging in any laboratory work. Please read the list of safetyrules above. No student will be permitted to perform laboratory activitiesunless this contract is signed by boththe student and parent/guardian and ison file with the teacher.Your signature on this contract indicates that you have read this StudentSafety Contract, are aware of the measures taken to ensure the safety ofyour son/daughter in the science laboratory, and will instruct your son/daughter to uphold his/her agreementto follow these rules and proceduresin the laboratory.Parent/Guardian SignatureDateP.O. Box 219, Batavia, IL 605101-800-452-1261 Fax: (866) 452-1436flinn@flinnsci.com www.flinnsci.com 2004, Flinn Scientific, Inc. All Rights Reserved. Reproduction permission is granted to science teachers who are customers of Flinn Scientific, Inc. Batavia, Illinois, U.S.A. No part of this material may be reproduced or transmitted in any form or by any means, electronic or mechanical, including, but not limited to photocopy, recording, or any information storage and retrieval system, without permission in writing from Flinn Scientific, Inc.

Metals vs. Non-Metals; Dot Diagrams; Ions Metals versus Non-Metals Dot Diagrams Metals are on the left side. Non-metals on the right. Metals tend to lose electrons. Non-metals gain them tight. Dot Diagrams (sometimes known as Lewis dot diagrams) are a depiction of an atom’s valence elect

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