CHAPTER 6 Chemical Bonding - Mchsapchemistry

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NameDatePeriodAccelerated ChemistryCHAPTER 6 Chemical BondingSECTION 1 Introduction to Chemical BondingOBJECTIVES1. Define Chemical bond.2. Explain why most atoms form chemical bonds.3. Describe ionic and covalent bonding.4. Explain why most chemical bonding is neither purely ionic or purley5. Classify bonding type according to electronegativity differences.SECTION 2 Covalent Bonding and Molecular CompoundsOBJECTIVES1. Define molecule and molecular formula.2. Explain the relationships among potential energy, distance betweenapproaching atoms, bonds length and bond energy.3. State the octet rule.4. List the six basic steps used in writing Lewis dot Structures.5. Explain how to determine Lewis structures for molecules containing singlebonds, multiple bonds or both.6. Explain why scientists use resonance structures to represent some molecules.SECTION 3 Ionic Bonding and Ionic compoundsOBJECTIVES1. Compare and contrast the chemical formula for a molecular compound witone for an ionic compound.2. Discuss the arrangements of ions in crystals.3. Define lattice energy and explain its significance.4. List and compare the distinctive properties of ionic and molecularcompounds.5. Write the Lewis structure for a polyatomic ion given the identity of the atomscombined and other appropriate information.Anderson - MCHSModern Chemistry1Chemical Bonding

NameDatePeriodAccelerated ChemistrySECTION 4 Metallic BondingOBJECTIVES1. Describe the electron-sea model of metallic bonding, and explain why metalsare good electrical conductors.2. Explain why metal surfaces are shinny.3. Explain why metals are malleable and ductile but ionic crystallinecompounds are not.SECTION 5 Molecular GeometryOBJECTIVES1. Explain VSEPR theory.2. Predict the shapes of molecules or polyatomic ionis using VSEPR theory.3. Explain how the shapes of molecules are accounted for by hybridizationtheory.4. Describe dipole – dipole forces, hydrogen bonding, induced dipoles andLondon Dispersion Forces and their effects on properties such as boilingpoint and melting point.5. Explain what determines molecular polarity.Anderson - MCHSModern Chemistry2Chemical Bonding

NameDatePeriodAccelerated ChemistryChapter 6 VocabularyChemical BondingSec 6-1 Introduction to Chemical BondingChemical bondNonpolar covalent bondIonic bondingPolarCovalent bondingPolar covalent bondSec 6-2 Covalent Bonding and Molecular CompoundsMoleculeElectron dot notationMolecular compoundLewis structureChemical formulaSingle bondMolecular formulaMultiple bondBond energyresonanceSec 6-3 Ionic Bonding and Ionic CompoundsIonic compoundLattice energyFormula unitPolyatomic ionSec 6-4 Metallic BondingMetallic bondingMalleabilitySec 6-5 Molecular GeometryVSEPR theoryHybridizationhybrid orbitalsIntramolecular forceductilityIntermolecular forcedipolehydrogen bondingLondon dispersion forcesAnderson - MCHSModern Chemistry3Chemical Bonding

NameDatePeriodAccelerated ChemistryAnderson - MCHSModern Chemistry4Chemical Bonding

NameDatePeriodAccelerated ChemistryCHAPTER 6 STUDY GUIDEChemical BondingSECTION 1 INTRODUCTION TO CHEMICAL BONDINGSHORT ANSWER Answer the following questions in the space provided.1. A chemical bond between atoms results from the attraction between thevalence electrons and of different atoms.(a) nuclei(c) isotopes(b) inner electrons(d) Lewis structures2. A covalent bond consists of(a) a shared electron.(b) a shared electron pair.(c) two different ions.(d) an octet of electrons.3. If two covalently bonded atoms are identical, the bond is identified as(a) nonpolar covalent.(c) ionic.(b) polar covalent.(d) dipolar.4. A covalent bond in which there is an unequal attraction for the sharedelectrons is(a) nonpolar.(c) ionic.(b) polar.(d) dipolar.5. Atoms with a strong attraction for electrons they share with another atomexhibit(a) zero electronegativity.(c) high electronegativity.(b) low electronegativity.(d) Lewis electronegativity.6. Bonds that possess between 5be(a) ionic.(b) pure covalent.and 50ionic character are considered to(c) polar covalent.(d) nonpolar covalent.7. The greater the electronegativity difference between two atoms bondedtogether, the greater the bond’s percentage of(a) ionic character.(c) metallic character.(b) nonpolar character.(d) electron sharing.8. The electrons involved in the formation of a chemical bond are called.9. A chemical bond that results from the electrostatic attraction between positive andionic bond negative ions is called a(n) .Anderson - MCHSModern Chemistry5Chemical Bonding

NameDatePeriodAccelerated ChemistrySECTION 1 continued10. If electrons involved in bonding spend most of the time closer to one atom ratherthan the other, the bond is .11. If a bond’s character is more than 50.ionic, then the bond is called a(n)12. A bond’s character is more than 50 ionic if the electronegativity differencebetween the two atoms is greater than .13. Write the formula for an example of each of the following compounds:Answers will vary.a. nonpolar covalent compoundb. polar covalent compoundc. ionic compound14. Describe how a covalent bond holds two atoms together.15. What property of the two atoms in a covalent bond determines whether or not thebond will be polar?16. How can electronegativity be used to distinguish between an ionic bond and acovalent bond?17. Describe the electron distribution in a polar-covalent bond and its effect on thepartial charges of the compound.Anderson - MCHSModern Chemistry6Chemical Bonding

NameDatePeriodAccelerated ChemistryCHAPTER 6 STUDY GUIDEChemical BondingSECTION 2 COVALENT BONDING AND MOLECULAR COMPOUNDSSHORT ANSWER Answer the following questions in the space provided.1. Use the concept of potential energy to describe how a covalent bond formsbetween two atoms.2. Name two elements that form compounds that can be exceptions to the octet rule.3. Explain why resonance structures are used instead of Lewis structures to correctlymodel certain molecules.4. Bond energy is related to bond length. Use the data in the tables below to arrangethe bonds listed in order of increasing bond length, from shortest bond to longest.a.BondBond energy (kJ/mol)H FH IH ClH Br569299432366Anderson - MCHSModern Chemistry7Chemical Bonding

NameDatePeriodAccelerated ChemistrySECTION 2 continuedb.BondBond energy (kJ/mol)C CC CC C3468356125. Draw Lewis structures to represent each of the following formulas:a. NH3b. H2Oc. CH4d. C2H2e. CH2OAnderson - MCHSModern Chemistry8Chemical Bonding

NameDatePeriodAccelerated ChemistryCHAPTER 6 STUDY GUIDEChemical BondingSECTION 3 IONIC BONDING AND IONIC COMPOUNDSSHORT ANSWER Answer the following questions in the space provided.1. The notation for sodium chloride, NaCl, stands for one(a) formula unit.(c) crystal.(b) molecule.(d) atom.2. In a crystal of an ionic compound, each cation is surrounded by a numberof(a) molecules.(c) dipoles.(b) positive ions.(d) negative ions.3. Compared with the neutral atoms involved in the formation of an ioniccompound, the crystal lattice that results is(a) higher in potential energy.(c) equal in potential energy.(b) lower in potential energy.(d) unstable.4. The lattice energy of compound A is greater in magnitude than that ofcompound B. What can be concluded from this fact?(a) Compound A is not an ionic compound.(b) It will be more difficult to break the bonds in compound A than thosein compound B.(c) Compound B has larger crystals than compound A.(d) Compound A has larger crystals than compound B.5. The forces of attraction between molecules in a molecular compound aregenerally(a) stronger than the attractive forces among formula units in ionicbonding.(b) weaker than the attractive forces among formula units in ionicbonding.(c) approximately equal to the attractive forces among formula units inionic bonding.(d) equal to zero.6. Describe the force that holds two ions together in an ionic bond.7. What type of energy best represents the strength of an ionic bond?Anderson - MCHSModern Chemistry9Chemical Bonding

NameDatePeriodAccelerated ChemistrySECTION 3 continued8. What types of bonds are present in an ionic compound that contains a polyatomicion?9. Arrange the ionic bonds in the table below in order of increasing strength fromweakest to strongest.Ionic bondLattice energy (kJ/mol)NaCl787CaO3384KCl715MgO3760LiCl86110. Draw Lewis structures for the following polyatomic ions:a. NH 4b. SO 2411. Draw the two resonance structures for the nitrite anion, NO 2 .Anderson - MCHSModern Chemistry10Chemical Bonding

NameDatePeriodAccelerated ChemistryCHAPTER 6 STUDY GUIDEChemical BondingSECTION 4 METALLIC BONDINGSHORT ANSWER Answer the following questions in the space provided.1. In metals, the valence electrons are considered to be(a) attached to particular positive ions. (c)immobile.(b) shared by all surrounding atoms.(d) involved in covalent bonds.2. The fact that metals are malleable and ionic crystals are brittle is bestexplained in terms of their(a) chemical bonds.(c) enthalpies of vaporization.(b) London forces.(d) polarity.3. As light strikes the surface of a metal, the electrons in the electron sea(a) allow the light to pass through.(b) become attached to particular positive ions.(c) fall to lower energy levels.(d) absorb and re-emit the light.4. Mobile electrons in the metallic bond are responsible for(a) luster.(c) electrical conductivity.(b) thermal conductivity.(d) All of the above.5. In general, the strength of the metallic bond moving from left toright on any row of the periodic table.(a) increases(c) remains the same(b) decreases(d) varies6. When a metal is drawn into a wire, the metallic bonds(a) break easily.(c) do not break.(b) break with difficulty.(d) become ionic bonds.7. Use the concept of electron configurations to explain why the number of valenceelectrons in metals tends to be less than the number in most nonmetals.Anderson - MCHSModern Chemistry11Chemical Bonding

NameDatePeriodAccelerated ChemistrySECTION 4 continued8. How does the behavior of electrons in metals contribute to the metal’s ability toconduct electricity and heat?9. What is the relationship between the enthalpy of vaporization of a metal and thestrength of the bonds that hold the metal together?10. Draw two diagrams of a metallic bond. In the first diagram, draw a weakmetallic bond; in the second, show a metallic bond that would be stronger. Besure to include nuclear charge and number of electrons in your illustrations.a.b.Note: In the strong bond, the charge on the nucleus and the number ofelectrons must be greater than in the weak bond.11. Complete the following table:MetalsIonic CompoundsComponentsOverall chargeConductive in the solid stateMelting pointHardnessMalleableDuctileAnderson - MCHSModern Chemistry12Chemical Bonding

NameDatePeriodAccelerated ChemistryCHAPTER 6 STUDY GUIDEChemical BondingSECTION 5 MOLECULAR GEOMETRYSHORT ANSWER Answer the following questions in the space provided.1. Identify the major assumption of the VSEPR theory, which is used to predict theshape of atoms.2. In water, two hydrogen atoms are bonded to one oxygen atom. Why isn’t water alinear molecule?3. What orbitals combine together to form sp3 hybrid orbitals around a carbon atom?4. What two factors determine whether or not a molecule is polar?5. Arrange the following types of attractions in order of increasing strength, with 1being the weakest and 4 the strongest.hydrogen bondingionicdipole-dipoleLondon dispersion6. How are dipole-dipole attractions, London dispersion forces, and hydrogenbonding similar?Anderson - MCHSModern Chemistry13Chemical Bonding

NameDatePeriodAccelerated ChemistrySECTION 5 continued7. Complete the following table:FormulaLewis structureGeometryPolarH 2SCCl4BF3H 2OPCl5BeF2SF6Anderson - MCHSModern Chemistry14Chemical Bonding

NameDatePeriodAccelerated ChemistryCHAPTER 6 STUDY GUIDEChemical BondingMIXED REVIEWSHORT ANSWER Answer the following questions in the space provided.1. Name the type of energy that is a measure of strength for each of the followingtypes of bonds:a. ionic bondb. covalent bondc. metallic bond2. Use the electronegativity values shown in Figure 20, on page 161 of the text, todetermine whether each of the following bonds is nonpolar covalent, polar covalent,or ionic.a.d. H HH Fe. H Cb.Na Clf. H Nc. H O3. How is a hydrogen bond different from an ionic or covalent bond?4. H2S and H2O have similar structures and their central atoms belong to the samegroup. Yet H2S is a gas at room temperature and H2O is a liquid. Use bondingprinciples to explain why this is.Anderson - MCHSModern Chemistry15Chemical Bonding

NameDatePeriodAccelerated ChemistryMIXED REVIEW continued5. In what way is a polar-covalent bond similar to an ionic bond?6. Draw a Lewis structure for each of the following formulas. Determine whetherthe molecule is polar or nonpolar.a. H2Sb. COCl2c. PCl3d. CH2O.Anderson - MCHSModern Chemistry16Chemical Bonding

Modern Chemistry 1 Chemical Bonding CHAPTER 6 Chemical Bonding SECTION 1 Introduction to Chemical Bonding OBJECTIVES 1. Define Chemical bond. 2. Explain why most atoms form chemical bonds. 3. Describe ionic and covalent bonding. 4. Explain why most chemical bonding is neither purely ionic or purley 5. Classify bonding type according to .

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