1. Flashcards for Ionic & Metallic Bonding

2. What particle is transferred in ionic bonding? Electron

3. How do you identify an ionic formula? Metal + Nonmetal

4. How do you identify a covalent formula? All Nonmetals

5. What do metals do in ionic bonding? Metals lose electrons & form positive ions.

6. What is a positive ion called? A cation

7. What do nonmetals do in ionic bonding? Nonmetals gain electrons & form negative ions.

8. What is a negative ion called? An anion

9. Lewis structures of ionic substances Show all positive ions & all negative ions. Use square brackets to enclose symbol of each ion & put charge outside

10. Ion formation Atoms form ions to achieve the noble gas configuration of the nearest noble gas

11. Ion formation Group I metals always form ions with a +1 charge. Group II metals always form ions with a +2 charge. Transition metals may form more than one kind of positive ion.

12. Nonmetal Ions Nonmetals form negative ions in ionic compounds. The positive oxidation states for the nonmetals are used in covalent compounds.

13. Group 1 metals form … +1 ions

14. Group 2 metals form … +2 ions

15. Group 17 nonmetals form … -1 ions

16. Group 18 nonmetals form … They don’t form ions. There the noble gases!

17. Group 16 nonmetals form … -2 ions

18. Lewis Dot Structures for Ionic Compounds Have square brackets and charges. Charges add up to 0. Positive ion has no dots. Negative ion has 8 dots.

19. Lewis diagram of sodium chloride [Na] +1 [:Cl:] -1 :

20. Lewis diagram of calcium chloride [Ca] +2 [:Cl:] -1 [:Cl:] -1 :

21. Lewis diagram of aluminum chloride [Al] +3 [:Cl:] -1 [:Cl:] -1 [:Cl:] -1 :

22. Lewis diagram of aluminum sulfide [Al] +3 [:S:] -2 [:S:] -2 [:S:] -2 [Al] +3 :

23. Why do atoms form bonds? To get the same electron configuration as the nearest noble gas.

24. What is a chemical bond? Force of attraction that holds 2 atoms together.

25. What are the properties of ionic compounds? 1)Hard, brittle 2)High melting point, high boiling point 3)Low vapor pressure 4)Poor conductors of heat 5)Solids do not conduct electricity at all 6)Melts & solutions do conduct a current 7)Ions in solution react quickly

26. What is the structure of ionic compounds? Crystal lattice: lattice points are positive & negative ions.

27. Empirical Formula Subscripts in chemical formula have smallest whole number ratio

28. Empirical Formula Ionic compounds only have empirical formulas.

29. Formulas Symbols & Subscripts

30. Subscripts in chemical formulas Microscopic scale – give atomic ratios Macroscopic scale – give mole ratios

31. Crystal lattice Regular, repeating pattern in 3 dimensions.

32. Compounds are electrically … Neutral.

33. Molecular Formula Gives exact composition of molecule.

34. Binary Ionic Compound Contains 2 elements

35. What are the properties of metals? 1)Luster 2)Good conductors of heat & electricity 3)Malleable & ductile 4)Low ionization energy & low electronegativity 5)High mp, high bp & low vapor pressure

36. What is the structure of metals. Crystal lattice: all lattice points are positive ions.

37. Delocalized electrons Valence electrons in metals are free to roam throughout the metal.

38. Sea of mobile electrons Phrase used to describe valence electrons in metallic bonding.