Chemistry. Homework p. 193 #3-11, p. 207 - 208 # 31-32, 35-40, 55-56, 58-59, 62-63, 65 – DUE WEDNESDAY p. 199 # 16, 18-20, p. 207-208 # 42,45 – DUE THURSDAY.

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Chemistry Slide 2 Homework p. 193 #3-11, p. 207 - 208 # 31-32, 35-40, 55-56, 58-59, 62-63, 65 DUE WEDNESDAY p. 199 # 16, 18-20, p. 207-208 # 42,45 DUE THURSDAY Quiz over Table 7.2 on Wends, Nov 9 Test over Ch. 7 on Tuesday, Nov. 15 (tentative) Slide 3 Review 1. What is an ion? ion an atom with a positive or negative charge (an electron has been lost or gained) 2. Where on the periodic table are the metals located? Nonmetals? Slide 4 Valence Electrons Core Electrons inner electrons, do not participate in bonding Valence Electrons outer electrons, electrons in the highest occupied energy level number of valence electrons largely determines the chemical properties of an element So which electrons in an electron configuration are core and valence? Be [He] 2s 2 P [Ne] 3s 2 3p 3 CoreValenceCoreValence Slide 5 So how do I find this valence number? The valence electrons an atom has is the same as its group number for a representative (main group) element Slide 6 So how do I find this valence number? So how many valence electrons would Na have? 1 Iodine? 7 Krypton? 8 Slide 7 How do I keep track of all these valence electrons? Valence electrons are VERY important for chemistry and reactions! Why? Chemists have electron dot structures diagrams that show valence electrons as dots Slide 8 How do I keep track of all these valence electrons? What do you notice about valence electrons down a group? Electron configuration remains the same down a group, only the core electrons change Slide 9 Practice How many valence electrons does Al have? Draw the Lewis dot structure. Electron configuration: Valence Electrons: Lewis dot structure: [Ne] 3s 2 3s 1 3 Slide 10 Crystal Structures In crystalline materials, elements repeat in repetition to give a 3D arrangement known as a crystal lattice A unit cell is the smallest part of the lattice that represents the entire lattice (repeated part) 4 types of unit cells: Primitive Body-centered Face-centered Hexagonal close-packed Slide 11 Crystal Structures Primitive body-centered Hexagonal close-packed face-centered Slide 12 Part I: Metals Crystal coordination number (CN): number of neighbors to an atom in a unit cell Example: simple cubic is 6 Slide 13 Part I: Metals Crystal coordination number (CN): number of neighbors to an atom in a unit cell Face-centered: 12 Body-Centered: 8 Hexagonal: 12 Slide 14 Lets Think! We know noble gases are very stable. How can we get the other elements to become stable like the noble gases? Hint: Think of valence electrons! Slide 15 Octet Rule All elements want eight valence electrons (except H and He) Why? Achieve noble gas configuration, most STABLE 2 electrons come from the s subshell and 6 from the p subshell Why can H and He NOT have eight valence electrons (Hint: they are considered stable with TWO valence electrons) No p subshell! Slide 16 Octet Rule Elements will tend to gain or lose enough electrons to fulfill their octet Will metallic elements gain or lose electrons? Lose, much easier to lose electrons than gain electrons Will nonmetallic elements gains or lose electrons? Gain, much easier to gain electrons (can also share electrons) Slide 17 Octet Rule Metallic elements lose electrons Why? In simple termseasier to lose than to gain to form the octet Nonmetallic elements gain electrons Why? In simple terms, easier to gain a few electrons than lose them Now lets consider periodic trends! Nuclear attraction across: Shielding effect across: Kinetic energy across: This means: Increases across, nonmetals held tighter than metals Remains constant, does not offset nuclear attraction Remains constant Metals hold onto their electrons less tightly so it is easier for metals to lose their electrons. Additionally, nonmetals hold onto their electrons tighter. This trend, and the fact that nonmetals have higher electron affinity, means nonmetals tend to gain electrons. Slide 18 Octet Rule If metals lose electrons, they will form ions. Will these ions be negatively or positively charged? If nonmetals gain electrons, will their ions be negatively or positively charged? Slide 19 Octet Rule Ions get special names to distinguish between those ions that are positively charged and those that are negatively charged Cation positively charged ion Lets try sodium! Electron configuration: Original electron dot diagram: How many electrons will it lose? New electron dot diagram: New electron configuration [Ne] 3s 1 [Ne] 1 Na + Slide 20 Octet Rule Ions get special names to distinguish between those ions that are positively charged and those that are negatively charged Cation positively charged ion Slide 21 Octet Rule - Cations Ions get special names to distinguish between those ions that are positively charged and those that are negatively charged Cation positively charged ion Slide 22 I wonder Mg has the electron configuration of [Ne] 3s 2. How many electrons would it lose or gain stability? 2 Will it take more or less energy to remove the second electron than the first electron? Lets use electron dot structures to show its loss of 2e - Slide 23 Octet Rule - Cations We just did one example of formation of a cation from Group 1 and Group 2. What can we say about the general formation of cations from Group 1 and the general fromation of cations from Group 2? Group 1 form +1 cation Group 2 form + 2 cation Slide 24 What about those transition metals? Its extremely hard for transition metals to lose enough electrons to form a noble gas configuration. Why? They would have to lose all the s and d electrons! The transition metals ending with ns 1 (n-1)d 10 can lose that 1s electron to achieve pseudo noble-gas electron configuration What is one element that does this? Elements with the configuration ns 1 (n-1)d 5 can also lose that 1s electron to achieve half shell stability What is one element that can do this? Slide 25 What about those transition metals? Slide 26 Octet Rule - Anions Ions get special names to distinguish between those ions that are positively charged and those that are negatively charged Anion negatively charged ion Lets try chlorine! Electron configuration: Electron diagram: How many electrons will it gain? New electron diagram: New electron configuration [Ne]3s 2 3p 5 [Ne]3s 2 3p 6 1 Cl - Slide 27 Octet Rule - Anions Ions get special names to distinguish between those ions that are positively charged and those that are negatively charged Anion negatively charged ion Slide 28 Octet Rule - Anions Ions get special names to distinguish between those ions that are positively charged and those that are negatively charged Anion negatively charged ion Slide 29 I wonder O has the electron configuration of [He] 2s 2 2p 4. How many electrons would it gain to gain stability? 2 Will it take more or less energy to gain the second electron than the first electron? Lets use electron dot structures to show its gain of 2e - Slide 30 Octet Rule - Anions How many electrons need to be gained by each group in group 5,6, and 7 to be stable? Slide 31 Octet Rule Slide 32 Common Ions Everyone loves memorizing stuff in chemistry! Lets memorize some more! (Trust me, itll make your life 10x easier if you just memorize them now and get it over with!) Slide 33 Common Ions Slide 34 Lets Think! We all know that certain elements will bond together to form molecules, such as NaCl (table salt). Why is this? Hint: Think of valence electrons. Slide 35 Ionic Bonding Ionic compound composed of metal cations and nonmetal anions They are still electrically neutral Why? The charges of the cation and anion cancel out The negatively charged anion and the positively charged cation attract each other by electrostatic forces (force holding a cation and anion together due to their charge) Slide 36 Ionic Bonding Ionic compound composed of metal cations and nonmetal anions Lets go back to the formation of NaCl Whats the electron configuration of Na? Of Cl? Their valence electrons can add together to form an ionic compoundnow both elements are happyjust like Justin and Selena! [Ne] 3s 1 [Ne] 3s 2 3p 5 Slide 37 Ionic Bonding Ionic compound composed of metal cations and nonmetal anions Slide 38 Ionic Bonding Ionic compound composed of metal cations and nonmetal anions Slide 39 Ionic Bonding Ionic compound composed of metal cations and nonmetal anions Slide 40 Ionic Bonding So Na + and Cl - combine to form NaCl NaCl is the chemical formula or a way to show the kinds and numbers of atoms in the smallest unit of a substance So there is 1 Na + for every 1 Cl - What would Mg +2 and Cl -1 form? There is 1 Mg +2 for every 2 Cl -1 so MgCl 2 Think of it this way: the charges have to become neutral Slide 41 Ionic Bonding The charges must become neutral What about Sr +2 and F - ? SrF 2 Slide 42 Ionic Bonding Another way to do it is balance out the charges Ex: 1 Mg has a +2 charge and 1 O has a -2 charge. The charges are already balanced! So we have.MgO What about. 1 Be has a +2 charge and 1 Br has a -1 charge. How many Br will be needed to balance out the charges? 2so that gives us. BeBr 2