Honors Chemistry 1: Chapter 4 Study Guide



DAY 1: Section 4.1Before coming to class, you should have:Read section 4.1Completed warm-up practice problems 1-4Paid special attention to trends on the periodic tableKey concepts:Law of octavesPeriodic LawValance ElectronsGroupPeriodWarm-Up Practice Problems:Write the electron configuration AND create an orbital diagram for each of the listed elementsPut your orbital diagram first, and then write the configuration to the right.LithiumSodiumPotassiumRubidiumLook at all of your electron configurations in question 1. What similarities do you see for those four elements? Write the electron configuration AND create an orbital diagram for each of the listed elementsFluorineChlorineBromineIodineLook at all of your electron configurations in question 3. What similarities do you see for those four elements?Write the electron configuration AND create an orbital diagram for each of the listed elementsCarbonSiliconGermaniumTin LeadLook at all of your electron configurations in question 5. What similarities do you see for those five elements?Figure 4.1a: Mendeleev’s PredictionsHow did Mendeleev organize his version of the periodic table?How did the “Law of Octaves” help Mendeleev organize his period table?Why were these “gaps” present in Mendeleev’s periodic table to begin with?How did Mendeleev arrive at these predictions?Figure 4.1b: Blocks of the periodic tableUsing the information in figure 4.1b, list the number of valance electrons for each of the following elements:Sodium: _____Sulfur: _____Oxygen: _____Fluorine: _____Magnesium: _____Aluminum: _____Silicon: _____Carbon: _____Lithium: _____Tin: _____Boron: _____Chlorine: _____Iodine: _____Calcium: _____Neon: _____Argon: _____Barium: _____Strontium: _____Krypton: _____Potassium: _____Arsenic: _____Antimony: _____Lead: _____Xenon: _____Predicting:I’ve repeatedly said that all main group elements want to be noble gases, which is the most stable group of atoms on the periodic table (Think of this as “noble gas envy”). Predict the formula for the following ionic compounds, and think in terms of helping each of these atoms find a way to have the electron configuration of a noble gas:Sodium bonding with ChlorineSodium bonding with BromineSodium bonding with IodineLithium bonding with fluorineSodium bonding with fluorinePotassium bonding with fluorineCalcium bonding with oxygenSodium bonding with oxygenDay 2: Section 4.2 – Touring The Periodic TableBefore coming to class, you should have:Read section 4.2Reviewed section 4.1Key concepts:Main-Group ElementsAlkali MetalsAlkaline Earth MetalsHalogensNoble GasesTransition MetalsProperties of metalsDuctileMalleableLanthanidesActinides AlloysAt the top of each group, label the ionic charge for each element within that group.Figure 4.2a: Looking for trends among the Alkali MetalsAnswer the following:How does the melting point change as the atomic number increases for alkali metals?How does the density change as the atomic number increases for alkali metals?How does the atomic radius change as the atomic number increases for alkali metals?How does metallic hardness change as the atomic number increases for alkali metals?Which element shown as the greatest temperature range in its liquid state?What is the difference in melting points between sodium and potassium?Figure 4.2b: Know the differences between METALS and NONMETALSList a variety of general properties for METALS and NONMETALS:METALS:NONMETALS:Day 3: Section 4.3—Periodic TrendsBefore coming to class, you should have:Read section 4.3Reviewed sections 4.1 and 4.2Key Concepts:Periodic trendIonization EnergyAtomic RadiusBond LengthElectronegativity Electron affinityBoiling/Melting PointFigure 4.3a: What is ionization energy?Important fact about ionization:IN GENERAL, METAL ATOMS TEND TO ___________________ ELECTRONS, AND NONMETAL ATOMS TEND TO ______________ ELECTRONS!!!!Cations and Anions:Cation:Anion:Examples:Write the ionic charge for each of the given atoms once it has ionizedSodium: _____Fluorine: _____Oxygen: _____Nitrogen: ____Sulfur: _____Magnesium: _____Calcium: _____Aluminum: _____List the protons and electrons for each ion listed below:IONProtonsElectronsIONProtonsElectronsCa2+Cu+P3-N3-Br -Au+K+Ba2+Ag +Cl -S2-H+Al3+Na+Fe3+Cs+F -B3+ Figure 4.3b: Trends in Ionization EnergyDefine ionization energy (do it again, even if you have already…it’s very important!!):Explain WHY the trend shown in figure 4.3b exists as you move DOWN groups:Explain WHY the trend shown in figure 4.3b exists as you move ACROSS periods:Figure 4.3c: Ionization energy for main-block elementsGenerally speaking, as the group number increases, the ionization energy ________________________As the atomic number increases WITHIN A GROUP, the ionization energy _________________________Why do the noble gases have such incredibly high ionization energies compared to the rest of the elements shown in this graph? How does this describe their reactivity?Which group (give the name…e.g., halogens, noble gases, alkaline earth metals, alkali metals) has the lowest ionization energy? What does this mean in terms of their reactivity?Figure 4.3d: Trends in atomic radiusExplain the atomic radius trend as you go down a group:Explain the atomic radius trend as you go across a period:Figure 4.3e: Plotting group number as a function of atomic radiusFigure 4.3f: Period trends in IONIC radiusFigure 4.3g: Bond Radius Why is chlorine’s bond radius shorter than iodine’s bond radius?ELECTRONEGATIVITY:Figure 4.3h: Electronegativity TrendsFigure 4.3i: Periodic Trends in electron affinityExplain why the halogens, out of ALL OF THE CHEMICAL GROUPS, have the highest electron affinity:Why is the electron affinity higher in alkali metals than in alkaline earth metals?Figure 4.3j: Periodic Trends in Melting/Boiling PointOf all of the elements shown, which seems to be the “biggest exception” to the general trend in period 6?Why might tungsten have the highest melting and boiling point of all elements in period 6?Approximate the following: Au boiling point: ______Pb melting point: _____Hg freezing point: _______Temp range that barium is a liquid: __________________Section 4.4—Where did the elements come from?Before coming to class, you should have:Read section 4.4Reviewed sections 4.1-4.3Key Concepts:Big Bang TheorySupernovaNuclear FissionNuclear FusionFigure 4.4a: How elements are fused inside of starsSUMMARY OF PERIODIC TRENDSOrder the following elements based on the trend listed:Electronegativity: Pb, Cl, Ba, F, CaAtomic Radius: C, Li, F, N, OAtomic Radius: Ca, Ba, Sr, Mg, BeElectron Affinity: Cl, I, Br, FElectronegativity: K, Li, Rb, Cs, NaIonization energy: Sb, N, Bi, P, AsAtomic & Ionic Radii for common cations and anions ................
................

In order to avoid copyright disputes, this page is only a partial summary.

Google Online Preview   Download