1. Flashcards for Ionic & Metallic Bonding

2. What particle is transferred in ionic bonding?
Electron
What particle is transferred in ionic bonding?

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

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

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

6. What is a positive ion called?
A cation
What is a positive ion called?

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

8. What is a negative ion called?
An anion
What is a negative ion called?

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
Lewis structures of ionic substances

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

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. +1 ions
Group 1 metals form …

14. +2 ions
Group 2 metals form …

15. -1 ions
Group 17 nonmetals form …

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

17. -2 ions
Group 16 nonmetals form …

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.
Lewis Dot Structures for Ionic Compounds

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

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

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

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

23. Na+1(g) + Cl-1(g)  NaCl(s)
Change in energy when one mole of a crystalline ionic compound is formed from its gas phase ions.
Na+1(g) + Cl-1(g)  NaCl(s)
Lattice Energy

24. Formation of ionic compounds
Is very exothermic!
Formation of ionic compounds

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

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

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

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

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

30. Ionic compounds only have empirical formulas.

31. Symbols & Subscripts
Formulas

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

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

34. Compounds are electrically …
Neutral.
Compounds are electrically …

35. Gives exact composition of molecule.
Molecular Formula

36. Contains 2 elements
Binary Ionic Compound

37. What are the properties of metals?
Luster
Good conductors of heat & electricity
Malleable & ductile
Low ionization energy & low electronegativity
High mp, high bp & low vapor pressure
What are the properties of metals?

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

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

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