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Chemical Bonding: Interactions of Matter Review

This chapter discusses electron arrangements, electron dot diagrams, and different types of chemical bonds, such as ionic and covalent bonds. Practice creating electron dot diagrams and naming ionic compounds.

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Chemical Bonding: Interactions of Matter Review

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  1. Chemical Bonding Chapter 1 Interactions of Matter

  2. REVIEW • Identify the 4 atoms whose models are on the bulletin board. • How did you identify these elements?

  3. Electron Arrangements Remember electrons arrange in energy levels outside the nucleus.

  4. Electron Dot Diagrams • Show ONLY outer level electrons • Also called Lewis diagrams • Begin with the element’s symbol • Use the PT to determine the number of outer level electrons • Place up to 2 dots per side for a total of up to 8 electrons • Put the first 2 dots together on one side, then put single dots on the remaining sides until you have to pair them

  5. Electron Dot Diagrams • Ex: 1 electron X

  6. Electron Dot Diagrams • Ex: 2 electrons X

  7. Electron Dot Diagrams • Ex: 3 electrons X Choose a clockwise or counterclockwise direction and fill empty sides with an electron before pairing any electrons.

  8. Electron Dot Diagrams • Ex: 4 electrons X Choose a clockwise or counterclockwise direction and fill empty sides with an electron before pairing any electrons.

  9. Electron Dot Diagrams • Ex: 5 electrons X Choose a clockwise or counterclockwise direction and fill empty sides with an electron before pairing any electrons.

  10. Electron Dot Diagrams • Ex: 6 electrons X Choose a clockwise or counterclockwise direction and fill empty sides with an electron before pairing any electrons.

  11. Electron Dot Diagrams • Ex: 7 electrons X Choose a clockwise or counterclockwise direction and fill empty sides with an electron before pairing any electrons.

  12. Electron Dot Diagrams • Ex: 8 electrons X THIS IS THE MOST ELECTRONS THAT EVER ARE INCLUDED IN ELECTRON DOT DIAGRAMS.

  13. Electron Dot Diagrams • Time to practice what you’ve learned • For the following elements, create electron dot diagrams using M&M’s as electrons. Be sure to write large size symbols on your paper. • YUM, but no eating allowed until all your work is checked and is correct! BRING IN YOUR ATOMIC MODEL TOMORROW!

  14. CHEMICAL BONDING • The number of electrons in the ____________ energy level determines whether an atom will form bonds. • These electrons are also called ___________ electrons. • Atoms bond to get a ________ outer level. • For all E levels beyond the first, the outermost E level is considered to be full if it contains ______ (#) electrons. • The first E level is full with ____ (#) electrons. • Why are noble gases nonreactive?

  15. CHEMICAL BONDING • Atoms bond by __________, ____________, or ___________ electrons to have a filled outermost energy level containing 8 valence electrons. • ___(#) types of bonds hold atoms together. • IONIC BOND- force of electrostatic attraction between 2 oppositely charged ______. • Ions form when electrons are _________________. • COVALENT BOND- force of attraction between nuclei of atoms and the electrons _______________ by the atoms. • Neutral atoms held by covalent bonds are called __________________. • METALLIC BOND- force of attraction between a ____________ charged metal ion and the electrons in a metal.

  16. IONIC BONDS • Chem 4 Kids example • METALS • have a low/high number of valence electrons. • metals lose/gain electrons when bonding. • form positive/negative ions. • NONMETALS • have a low/high number of valence electrons. • lose/gain electrons when bonding. • form positive/negative ions. • ions end in –ide

  17. IONIC BONDS

  18. Naming IONIC compounds Binary compounds- contain only 2 elements • negative ion ends in -ide • Ex: Name NaCl • Ex: Name AlF3 • Ex: Name Li2S • compounds are neutral so use subscripts to make (+)=(-) • Write the chemical formula for • Ex: strontium sulfide • Ex: potassium oxide • Ex: calcium chloride • Ex: barium nitride

  19. Naming IONIC compounds Binary compounds- containing transition elements • Transition metals- the charge is in parenthesis following the name of the metal except for Ag, Cd, and Zn (see PT) • ex: chromium (II) chloride • ex: iron (III) oxide • Ex: NiF2 vs. NiF • Ex: CrI4 vs. CrI2

  20. Naming IONIC compounds What about compounds with more than 2 elements • Look on page 159 for polyatomic ions • Polyatomic ions- groups of atoms that are bonded together with a charge • Usually end in -ate • Ex: BaSO4 • Ex: potassium phosphate • Ex: iron (III) carbonate

  21. IONIC BONDS- metal ion + nonmetal ion • CHARACTERISTICS OF IONIC COMPOUNDS • Hard, brittle solids at room temp • High melting and boiling points • Ions are held in a crystal lattice • Conduct electricity when dissolved in H2O

  22. Quick Review Barium sulfide Aluminum carbonate NaClO3 SiO2 Dinitrogenpentoxide

  23. COVALENT BONDS • Unlike ionic bonds with transferred electrons, covalent bonds __________ electrons. IONIC BOND COVALENT BOND

  24. COVALENT BONDS • Unlike ionic bonds that generally form between metals and nonmetals, covalent bonds form between ________________. • Classify the bonds as ionic or covalent • Na-Cl • H-O • C-O • Ca-F • N-N • Cr-S NOTE: Group 14 has a strange e-dot diagram

  25. COVALENT BONDS • Use electron dot diagrams to model molecules • Examples: • H2 • H2O • NH3 • Cl2

  26. COVALENT BONDS • Some molecules are simple with only one element • 7 elements are not found in nature as atoms • They always are found in pairs- called diatomic N2 O2 F2 And H2 (always the exception) Cl2 Br2 I2

  27. COVALENT BONDS • EXAMPLES OF COVALENT COMPOUNDS • water • plastic • sugar • Gasoline oils & fats • CHARACTERISTICS OF COVALENT COMPOUNDS • Do NOT conduct an electrical current • Low melting and boiling points • Lightweight molecules: generally gases and liquids at room temp • Heavier molecules: generally solids at room temp

  28. COVALENT COMPOUNDS • Naming covalent compounds involves using prefixes to indicate the number of atoms in the formula. • Website w/prefixes and rules

  29. COVALENT COMPOUNDS • When atoms share electrons, they don’t always share them equally. • Nonpolar covalent compounds: share e- equally • Will not conduct an electrical current at all • All diatomic molecules are nonpolar • Polar covalent compounds: share e- unequally • Can conduct an electrical current

  30. COVALENT COMPOUNDS • Polarity affects how chemicals mix. • “Like dissolves like.” • Nonpolar compounds mix with other nonpolar compounds. • Ex: • Polar compounds mix with other polar compounds. • Ex: • Nonpolar compounds will not mix with polar compounds. • Ex: • How does this affect how soap is made?

  31. METALLIC BONDS • EXAMPLES CONTAINING METALLIC BONDS • Cu, Fe • Alloys- mixtures of metals • EX: brass, bronze, steel • CHARACTERISTICS OF METALS • Malleable & ductile • Good conductors • “sea of electrons” allows metals to be shaped without breaking • Close metal atoms have overlapping outer E levels • Valence electrons can move freely between positive metal ions

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