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Chemical Bonds Sodium 11 Na 22.990 Name Atomic Number Symbol Atomic Mass + + + + + proton neutron - electron Orbital Notation Electron Configuration Electron-Dot (Lewis-Dot) Structure + + + + + + + Chemical Bonds Sodium 11 Na 22.990 Name Atomic Number Symbol Atomic Mass 1s + + + + + proton + + + + neutron - + + + electron Orbital Notation Na 1s Electron Configuration Na 1s2 Electron-Dot (Lewis-Dot) Structure Na 2s - - Chemical Bonds Sodium 11 Na 22.990 Name Atomic Number Symbol Atomic Mass 1s - + + + + + proton + + + + neutron - + + + electron Orbital Notation Na 1s Electron Configuration Na 2s 2p 1s2 2s2 Electron-Dot (Lewis-Dot) Structure Na - 2s -- 2px Chemical Bonds Sodium 11 Na 22.990 Name Atomic Number Symbol Atomic Mass 1s - -- -- + + + + + proton + + + + neutron - + + + electron 2pz Orbital Notation Na 1s Electron Configuration Na 2s 2p 1s2 2s2 Electron-Dot (Lewis-Dot) Structure Na 2s 2px 2py Chemical Bonds Sodium 11 Na 22.990 Name Atomic Number Symbol Atomic Mass 1s -- -- - --- + + + + + proton + + + + neutron - + + + electron 2pz Orbital Notation Na 1s Electron Configuration Na 2s 2p 1s2 2s2 2p6 Electron-Dot (Lewis-Dot) Structure Na 2s 2px 2py Chemical Bonds Sodium 11 Na 22.990 Name Atomic Number Symbol Atomic Mass 1s + + + + + proton + + + + neutron - + + + electron 3s 2pz Orbital Notation Na 1s Electron Configuration Na 2s 2p 1s2 2s2 2p6 3s1 Electron-Dot (Lewis-Dot) Structure Na 3s - -- -- - --- 2s 2px 2py Chemical Bonds Sodium 11 Na 22.990 Name Atomic Number Symbol Atomic Mass 1s + + + + + proton + + + + neutron - + + + electron 3s 2pz Orbital Notation Na 1s Electron Configuration Na 2s 2p 1s2 2s2 2p6 3s1 Electron-Dot (Lewis-Dot) Structure Na 3s - -- -- - --- 2s 2px 2py Chemical Bonds Chlorine 17 Cl 35.453 Name Atomic Number Symbol Atomic Mass + + + + + + proton neutron - electron Orbital Notation Electron Configuration Electron-Dot (Lewis-Dot) Structure + + + + + + + + + + + + Chemical Bonds Chlorine 17 Cl 35.453 Name Atomic Number Symbol Atomic Mass 1s + + + + + + proton + + + + + neutron - + + + + + electron Orbital Notation + + Cl 1s Electron Configuration Cl 1s2 Electron-Dot (Lewis-Dot) Structure Cl 2s - - Chemical Bonds Chlorine 17 Cl 35.453 Name Atomic Number Symbol Atomic Mass 1s - + + + + + + proton + + + + + neutron - + + + + + electron Orbital Notation + + Cl 1s Electron Configuration Cl 2s 2p 1s2 2s2 Electron-Dot (Lewis-Dot) Structure Cl - 2s -- 2px Chemical Bonds Chlorine 17 Cl 35.453 Name Atomic Number Symbol Atomic Mass 1s - -- -- + + + + + + proton + + + + + neutron - + + + + + electron Orbital Notation + + Cl 1s Electron Configuration Cl 2s 2p 1s2 2s2 Electron-Dot (Lewis-Dot) Structure Cl 2pz 2s 2px 2py Chemical Bonds Chlorine 17 Cl 35.453 Name Atomic Number Symbol Atomic Mass 1s -- -- - --- + + + + + + proton + + + + + neutron - + + + + + electron Orbital Notation + + Cl 1s Electron Configuration Cl 2s 2p 1s2 2s2 2p6 Electron-Dot (Lewis-Dot) Structure Cl 2pz 2s 2px 2py Chemical Bonds Chlorine 17 Cl 35.453 3pz Name Atomic Number Symbol Atomic Mass 3px 1s + + + + + + proton + + + + + neutron - + + + + + electron Orbital Notation 3py 3s + + 2pz - -- --- - -- -- - - Cl 1s Electron Configuration Cl 2s 2p 1s2 2s2 2p6 3s2 Electron-Dot (Lewis-Dot) Structure Cl 3s 3p 2s 2px 2py Chemical Bonds Chlorine 17 Cl 35.453 3pz Name Atomic Number Symbol Atomic Mass 3px + + + + + + proton - + + + + + electron Orbital Notation - -- - + + + + + neutron 3py 3s + + 2pz Cl 1s Electron Configuration Cl 2s 2p 1s2 2s2 2p6 3s2 3p5 Electron-Dot (Lewis-Dot) Structure Cl 3s 3p -- --- --- 1s 2s 2px 2py Chemical Bonds Be + Name Atomic Number Symbol Atomic Mass proton neutron - electron Orbital Notation Be Electron Configuration Be Electron-Dot (Lewis-Dot) Structure Be Chemical Bonds Beryllium 4 Be 9.012 Name Atomic Number Symbol Atomic Mass 1s + + + proton neutron - + + electron Orbital Notation Be 1s Electron Configuration Be 2s 1s2 2s2 Electron-Dot (Lewis-Dot) Structure Be - 2s - Chemical Bonds Oxygen Name Atomic Number Symbol Atomic Mass 8 O 15.999 1s -- --- + + + proton + + + neutron - + + + electron 2pz Orbital Notation O 1s Electron Configuration O 2s 2p 1s2 2s2 2p4 Electron-Dot (Lewis-Dot) Structure O 2s 2px 2py Draw orbital notations for the following: Draw electron configurations for the following: C C 1s2 2s2 2p2 C Ne 1s2 2s2 2p6 Ne 1s 2s 2p Ne 1s 2s 2p Mg Mg 1s 2s 2p 1s2 2s2 2p6 3s2 Mg P 1s2 2s2 2p6 3s2 3p3 3s P 1s 2s Draw electron-dot (Lewis-Dot) structures for the following: 2p 3s 3p Ca Ca 1s 2s 2p 3s P 3p 1s2 2s2 2p6 3s2 3p6 4s2 4s Ca Forming an Ionic Bond Na Na 1s 2s 2p 3s Sodium chloride Cl Cl 1s 2s 2p 3s 1s 2s Beryllium oxide O O 1s 2s 2p + Na Cl Cl - 3p Be Be Na + Be + + + -O Be+ - O - Chemical Bond -the force that holds two atoms together -formation of chemical bonds allows atoms to form a Noble Gas configuration of valence electrons, allowing them to become more stable and exist at a lower state of potential energy A. Ionic Bond -chemical bond formed by the exchange of electrons between a very electropositive atom (metal) and a very electronegative atom (nonmetal) which results in the formation of oppositelycharged ions, which are strongly attracted to eachother Na+ Cl Ionic compounds + Be+ -O -electronegativity is the tendency for an atom to attract electrons in order to form a chemical bond A. Ionic Bond -ionic bonds are those that have a relative electronegativity difference of more than 1.7 2.1 in -the electronegativity difference is ______ 2.0 in Beryllium oxide Sodium chloride and ______ Chemical Formula Name 1. Na___O___ _______________ 2. Be___Cl___ _______________ 3. K___Br___ _______________ 4. Na___O___ _______________ 5. Na___O___ _______________ 6. Na___O___ _______________ 7. Na___O___ _______________ 8. Na___O___ _______________ 9. Na___O___ _______________ Properties of Ionic Compounds -when ionic compounds form, they form a _____________, crystal lattice a ________________ three-dimensional _________ geometric arrangement of _______ positive and ________ negative ions Na Na -the energy required to separate one _______ mole Na Na Na Na Na Cl Cl (6.02 x 1023) of ions from each other is lattice energy called the ________________, the more Na Na Cl negative the lattice energy, the stronger ________ ______ the attraction between ions Na Na Cl Na Na Na Cl Na Na -the strength of the attraction between ions affects the compound’s __________ physical _________ properties Properties of Ionic Compounds A. Lattice Energy -gather data Compound Lattice Energy LiF -1032 LiCl -852 LiBr -815 LiI -761 NaF -926 NaCl -786 NaBr -752 NaI KF -702 KCl -717 KBr -689 KI -649 -813 Properties of Ionic Compounds A. Lattice Energy -analyze data 0 -200 -400 F Cl Br I -600 -800 -1000 -1200 Li Na K Properties of Ionic Compounds A. Lattice Energy -draw conclusions -the lattice energy is more negative in ionic compounds that have ____________________, smaller ionic radii because the ions are ___________________ more strongly attracted to each other B. Melting and Boiling Points -gather data Compound Melting Point (°C) Boiling Point (°C) NaI 660 1304 KBr 734 1435 NaBr 747 1390 CaCl2 782 1600 Cal2 784 1100 NaCl 801 1413 MgO 2852 3600 Properties of Ionic Compounds B. Melting and Boiling Points -draw conclusions -ionic compounds with higher lattice energies have _________melting and boiling points temps. higher -smaller ions are more ________ strongly attracted to each other, because the _______ nucleus is closer to the _______ valence _________, electrons while ions with larger positive and negative charges are more strongly attracted to each other ________ C. Electrical Conductivity -to conduct electricity, charged particles must be _________________, so ionic free to move compounds generally do not conduct solid but generally do electricity as a _____, liquid or when ______________ dissolved in water as a ______ (electrolyte) _______________ Properties of Ionic Compounds D. Hardness -the ions in ionic compounds with _______________ more negative lattice energies are more _________ strongly attracted to each other, so they tend to be ________ harder For Review 1. Rank the following ionic compounds, in order, from most negative to least negative lattice energy: RbCl, RbF, RbBr, RbI 1. RbF 2. RbCl 3. RbBr 4. RbI 2. Rank the following ionic compounds, in order, from highest to lowest melting point temperature: NaCl, MgCl2, MgO 1. MgO 2. MgCl2 3. NaCl 3. Rank the following ionic compounds, in order, from softest to hardest: Li2O, Li2S, Li2Te, Li2Se 1. Li2Te 2. Li2Se 3. Li2S 4. Li2O 4. Rank the following ionic compounds, in order, from ions most strongly to ions least strongly attracted to each other: MgF2, RbCl, CaF2, CaCl2, MgO 1. MgO 2. MgF2 3. CaF2 4. CaCl2 5. RbCl Naming Ionic Compounds 1. MgF2 ___________________ Magnesium fluoride 2. Rb2S ___________________ Rubidium sulfide 3. Ba(NO3)2 Barium ___________________ nitrate 4. (NH4)2Te ___________________ Ammonium telluride 5. (NH4)3PO4 ___________________ Ammonium phosphate 6. Na2SO4 ___________________ Sodium sulfate 7. Cu3P ___________________________________ Copper(I) phosphide or Cuprous phosphide Iron(III) hydroxide or Ferric hydroxide 8. Fe(OH)3 ________________________________ 9. Cr2(CO3)3 _______________________________________ Chromium(III) carbonate or Chromic carbonate 10. Sn(HCO3)4 __________________________________________ Tin(IV) Hydrogen carbonate or Stannic bicarbonate Metallic Bonds -like ionic compounds, metals in their ______ solid state form ________ lattice structures -each metal atom contributes its _______ valence _________ electrons to a ___________ delocalized _____ sea of electrons, which move freely throughout the solid -without its ________ valence _________, electrons each metal atom forms a _________ metal _______ cation -the attraction between the ________ metallic _________ cation and the _____________ delocalized ___________ electrons is called a _________ metallic _____ bond Properties of Metals -influenced strongly by the strength of attraction between the _______ metallic ________ cation and the number of ____________ delocalized ___________ electrons Properties of Metals A. Melting Point -since it doesn’t matter where the _________ metallic _______ cations are within the _______ lattice __________ structure of the metal, the cations _______ change _________ position easily, while still remaining in ______ close _______ contact melting _______ point with each other, so ________ temperatures are relatively ____ low -the _________ stronger the attraction between ________ metallic ________ cations and the ____ sea of ______________ delocalized __________, electrons the ________ higher the melting point smaller atoms tend to have temperature, so ________ higher melting point temperatures. _______ Properties of Metals A. Melting Point Metallic Element Melting Point (°C) Lithium 180 Sodium 98 Potassium 64 Rubidium 39 Cesium 29 Francium 27 Beryllium 1278 Aluminum 660 Calcium 839 Strontium 764 Barium 725 Radium 700 Properties of Metals A. Melting Point -________ melting _______ point temperatures are _________ increased by increasing the number of ________ valence ________ electrons sea of ______________ delocalized contributed to the _____ electrons ___________ Transition __________ elements like __________. Copper and _________ Tungsten contribute their ______ d _______ ________ orbital electrons as well as their __________ valence __________ electrons to the ____ sea of ________________ delocalized electrons __________ increasing the melting point __________, temperature dramatically. Metallic Element Melting Point (°C) Copper 1083 Tunsten 3410 Iron 1535 Chromium 1857 Silver 962 Properties of Metals B. Malleability & Ductility -because particles in a metal can easily malleable change position, they are __________, or can be __________ hammered _____ into _______ sheets or other shapes easily -because particles in a metal can easily change position, they are __________, ductile drawn into _______ wires or can be __________ _____ C. Durability & Boiling Point -even though particles in a metal can easily change position, they are __________ strongly ____________, attracted to the ____ sea of __________ electrons surrounding them, and are __________ difficult to _______ remove from the metal, giving durability and a high ________ boiling them a high ___________ ______ point temperature as well Properties of Metals D. Conductivity -because __________ delocalized __________ electrons in a metal are free ___ to _____ move while keeping _________ metallic _____ ______ bonds intact, the __________ electrons move _____ heat from place to place easily, so metal are _____ good ___________ conductors of _____ heat -because __________ delocalized __________ electrons in a metal are _____ free ___ to _____, move they move easily as a part of an ________ electrical ________ current when an __________ electrical potential or ________ voltage is applied to the metal, __________ crystal ________ lattice structure of the and the ________ __________ metallic ________ cations allows the __________ electrons to flow without _________ colliding with the ________, cations which allows for little __________ resistance Properties of Metals E. Luster -because ____________ delocalized ___________ electrons are free to move, light __________ absorbing and they can interact with ______, __________ releasing ________ photons of _______, light giving metals their _______ luster ________ (shine) F. Hardness delocalized __________ electrons & Strength -as the number of ___________ contributed to the ____ sea of _________ electrons increases, the strength of the _________ metallic _____ bonds increases, so metals such as _______, Sodium which contribute ____ one ________, electron soft and _____, weak while metals that are relatively _____ contribute their outer __ s electrons plus their inner __ d electrons such as _________, Chromium _____, Iron or _______ Nickel are relatively _____ hard and _______ strong Metal Alloys -because it doesn’t matter what _________ position the _________ metallic ________ cations are in in a metal, it is easy to introduce other _________ metallic __________ cations into the ________ lattice structure of a alloy or ________ mixture of metals metal, creating an ______, -in ______________ substitutional _______, alloys atoms of one kind of metal, Silver are replaced with atoms of another kind of like _______, Copper to form an ______ alloy like ________ Sterling metal, like _______, Silver which has the properties of both metals. Pure _______, _____ Gold is beautiful, rare, and almost completely _________, unreactive and so is highly valuable, but it is too _____ soft to be of much use by itself, so it is ________ alloyed with ________ Silver and ______ Copper 10 carat or _________ 14 carat _____, Gold which is still to make _________ harder and _________ durable beautiful, but much _______ -in ______________ interstitial _______, alloys atoms of another kind of element, like _______, Carbon are inserted into the spaces in between the cations of a metal like _____ Iron to form _______ Carbon ______, steel which is _______, harder ________, stronger and less ________ ductile Iron than _____
