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? Metals lose electrons & form positive ions.

6. What do nonmetals do? Nonmetals gain electrons & form negative ions.

7. 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

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

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

10. 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

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

12. Subscripts in formulas Tell how many atoms of that element are present. No subscript means “1.”

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

14. Empirical Formula Ionic compounds only have empirical formulas.

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

16. Compounds are electrically … Neutral.

17. Writing formulas from the ions for binary compounds. Write the ions, positive 1 st. If the superscripts (charges) do NOT add to zero, “criss-cross.” Na +1 S -2 becomes Na 2 S

18. Molecular Formula Gives exact composition of molecule.

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

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

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

22. Metallic Bonds Formulas have metals only.

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

24. 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.

25. Lewis Dot Structures for NaCl [Na] + [:Cl:] - : :

26. Lewis Dot Structures for NaOH [Na] + [:O:H] - : :

27. Group 1 metals form … +1 ions

28. Group 2 metals form … +2 ions

29. Group 16 nonmetals form … -2 ions

30. Group 17 nonmetals form … -1 ions

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

32. Binary Compounds Composed of 2 elements! (2 uppercase letters)

33. Naming Binary Ionic Compounds: Stock System Name positive ion 1 st (metal). Name negative ion 2 nd (nonmetal). Change ending to –ide. If metal has more than 1 oxidation state, use Roman numeral to specify which.

34. NaCl Binary Ionic Cmpd. Na has only 1 oxidation state. Sodium Chloride

35. FeCl 2 Binary Ionic Cmpd. Fe has 2 possible oxidation states. Iron (II) chloride

36. Fe(NO 3 ) 3 Contains a polyatomic. Fe has 2 possible oxidation states. Iron (III) Nitrate

37. Polyatomic Ion A group of covalently bonded atoms that carries a charge. Can form ionic bonds with other ions. Have names.

38. NaNO 3 NO 3 = nitrate ion Sodium nitrate

39. Cu(NO 3 ) 2 NO 3 = nitrate ion Copper has more than one oxidation state. The copper here must have a +2 charge. Copper (II) nitrate.

40. Cu 2 SO 4 SO 4 = sulfate ion Copper has more than one oxidation state. The copper here must have a +1 charge. Copper (I) sulfate.