3.  Ionic Bonding – electrical attraction between large numbers of cations and anions (metals & nonmetals); forms solid crystals  Octet rule: Atoms tend to achieve a noble gas electron configuration when forming a chemical bond. (oct = 8; s & p orbitals add to 8; ns 2 p 6 )  Use electron dots to predict the formulas for the compound formed between a) Li and Br b) Na and S see pg. 203

4.  Cation anion formula name

5. 1) Crystalline solids at room temperature *denoted by letter (c) ; 3D crystalline network; where each cation is surrounded by anions 2) HIGH MELTING POINTS! ex/ NaCl melts at 800 o C (1,474 o F) 3) Conduct electricity if dissolved in water (ions separate) & when in a molten state.

7. The chlorine atom gains seven electrons when it becomes an ion.

8. A) NaCl B) ClNa C) Na 7 Cl 1 D) SCl

9. A) ZnN B) Zn 2 N C) Zn 3 N 2 D) ZnN 2 E) Zn 2 N 3 F) ZnN 3

10. A) Anions B) Cations C) Valence electrons D) Orbital electrons

11. A) Negative two B) Positive two C) IDK D) Positive one

12. A) None B) One C) Six D) eight

13. A cation is positively charged because it will gain electrons to have a stable electron configuration like a noble gas.

14. The name of PbO is lead(II) oxide

15.  The charge of an anion is negative.

16.  When an aluminum atom loses its valence electrons, what is the charge on the resulting ion?  a. 2+  b. 3+  c. 2–  d. 1+

17. The electron configuration of a fluoride ion, F –, is  a. 1s 2 2s 2 2p 5.  b. the same as that of the neon atom.  c. 1s 2 2s 2 2p 6 3s 1.  d. the same as that of a potassium ion.

18. A) Fe 2 O 3 B) Fe 2 O 2 C) FeO D) Fe 3 O 2

19. An ionic compound is a. electrically neutral. b. composed of anions and cations. c. held together by ionic bonds d. all of the above

20. Which element when combined with chlorine would most likely form an ionic compound? a. lithium b. phosphorus c. oxygen d. bromine

21. A) Co 3 N 2 B) Co(NO 3 ) 2 C) Co(NO 3 ) 3

22. Metallic bonding - between metal atoms; valence electrons are shared equally in a “sea of electrons” *This explains the properties of metals!  The valence electrons are mobile and can drift freely from one part of the metal to another.  Electrons are delocalized & gives metals Multidirectional strength (stretching & sheets)

23. When a metal is subjected to pressure, the metal cations easily slide past one another (hence malleable & ductile) If an ionic crystal is struck with a hammer, the blow tends to push the positive ions close together. The positive ions repel one another, and the crystal shatters (brittle). Sea of electrons Metal cation Force Metal cation Strong repulsions Nonmetal anion MetalIonic crystal

24. Which of the following models can describe the valence electrons of metals? A.A body-centered cube B.Octets of electrons C.A rigid array of electrons D.A sea of electrons