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Chemical Bonding: Understanding the Basics for New Substances Formation

Exploring atoms, valence electrons, ionic bonds, covalent bonds, metallic bonds, and predicting types of bonds. Learn about ionization energy, electron affinity, and properties of compounds formed. Discover the significance of crystal lattice and oxidation numbers in compound formation.

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Chemical Bonding: Understanding the Basics for New Substances Formation

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  1. Chapter 7 Notes Book chapter 5 Video #18

  2. 7-1 Chemical Bonding -Atom: basic building block of matter -114 elements (video #19, 20) *Chem bonding: combining of atoms of elements to form new substances

  3. -Electrons and nrg Levels -2,8,8 *Valence e-: -Stable vs Nonstable

  4. Ex’s

  5. -Electrons and Bonding -e- in the outermost nrg level determines whether or not the atom will form chem bonds.

  6. 7-2 Ionic Bonding *Ionic bonding: transfer of e- *Ion: charged particle - Gaining or losing of e- - + or - atoms - Electromagnetic force hold opp charges together

  7. -Ionization nrg and Electron Affinity *Ionization: 1. Nrg needed to remove e- 2. Ionization nrg for atoms with many e-, is high 3. Atoms with few e-, is low

  8. Ion ex:

  9. NaCl--everyone is happy

  10. *Electron Affinity: tend to attract e-

  11. -Arrangement of Ions in Ionic Compounds *Crystal lattice: regular repeating arrangement -gives great stability -accounts for certain physical properties ex: ionic cmpnd high MP

  12. -Each ionic cmpnd has a characteristic crystal lattice

  13. -Ionic Properties -rigid crystal -conduct elect when melted or dissolved in H2O -probably a metal and nonmetal (from groups 16 or 17) -high melting points

  14. http://www.nd.edu/~aseriann/CHAP9.html/sld022.htm

  15. 7-3 Covalent Bonds *Cov Bon: sharing of e- -between atoms that have high ionization nrg and high electron affinities(Neither atom loses e- easily)

  16. Ex

  17. Covalent bonds form between: 2 nonmetals or a nonmetal and hydrogen

  18. Covalent or ionic? • Na and Cl • ionic • C and H • covalent • C and S • covalent • Ca and S • ionic

  19. -Nature of the Covalent Bond -Simplest is between H atoms *Electron-Dot Diagram: show only valence e- Ex’s: *Diatomic elements: always exist as 2 atoms cov. bonded

  20. -Formation of Molecules *Molecule: combination of atoms formed by a cov. Bond. -smallest part. Of a cov bonded substance that has all the prop. of that substance

  21. -Cov bonded solids tend to have low mp. *network solids: -high mp -large molecules -atoms continue to bond to one

  22. http://www.nd.edu/~aseriann/CHAP9.html/sld038.htm

  23. -Polyatomic ion *group of covalently bonded atoms that act like a single atom when combining with other atoms ex: NH4

  24. Compounds containing polyatomic ions are named by using your polyatomic ion chart.

  25. 7-4 Metallic Bonds *outer e- of the atoms form a common e- cloud -sea of mobile e- accounts for many of the properties of metals ex: malleable, ductile

  26. http://www.nd.edu/~aseriann/CHAP9.html/sld007.htm

  27. -metal ions can slide by each other and the e- are free to flow -also accounts for the high electric conductivity and high MP

  28. 7-5 Predicting Types of Bonds -Compounds formed between elements that lose e- easily and those that gain e- easily will have ionic bonds. ex: metal and a nonmetal

  29. -Compounds formed between elements that tend to gain e-’s will have covalent bonds. ex: between nonmetals ?MgF; OCl; KCl; SBr; CaS

  30. -Combining Capacity of Atoms *Oxidation #: -some elements have more than one oxidation #; it depends on the other atoms with which it bonds

  31. -Using Oxidation # -Use to predict how atoms will combine and what the formula for the resulting cmpnds will be. ~the sum of the ox must = 0 EX’s:

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