1. Ionic Covalent Metallic
Bonds and bonding
Ionic
Covalent
Metallic

2. Ionic Bonds Electrons are transferred from one atom to another.
Compounds are made.
Involves a metal and a nonmetal
Metal : donates electron(s) so it becomes a positive ion (cation)
Nonmetal receives electron and becomes a negative ion (anion)
So...must have a cation and anion

3. Why do ions exist?
Atoms want a full outer shell of valence electrons (8).
Will gain or lose electrons to achieve this = Octet rule
Then, positive and negative ion attract (bond)

6. Alternating positive and negative ions form crystalline lattice structures
The number and size of ion determines the shape of the crystal

8. Sodium chloride: NaCl

9. Calcium fluoride: CaF2

10. Quartz: SiO2

11. Alum

12. Properties of Ionic Compounds
All properties are a result of the arrangement of cation and anions.
1. Solid, crystalline

13. 2. Hard and brittle
When stuck, the crystal will break along a line of symmetry (fault line)

14. 3. Extremely high melting and boiling points.
Each molecule is strongly attracted to its neighboring molecule (strong intermolecular attraction)

15. Remember…
The bonds are not broken during melting and boiling. The molecules are separated from one another.

16. 4. Readily dissolves in water
The polar water molecule attracts and pulls the cations and anions apart.

17. 5. Non-conductive as a solid, but is conductive when dissolved in solution.
Solid is neutral (cations and anions equal)
When dissolved exists as cations and anions, which carry a charge.

19. What ions exist in our water supply?
Iron
Causes rust spots, dingy clothes
Copper from ground and pipes
Causes green residue
Chlorine and fluorine added to city water
Bad heavy metals: mercury, arsenic, lead

20. Calcium—contributes to “hard water”
Scaling in showers, on cookware
Bathtub ring
Binds to soap and renders in inactive
Won’t lather
Flat hair

22. How do we “soften” hard water?
Ion-exchange resin filter: sodium ions on resin beads are exchanged for calcium ions in hard water. Calcium “sticks” to bead.

25. Covalent Bonds Electrons are shared between atoms
Involves 2 or more nonmetals
Want to fulfill the octet rule.
Molecules are made.
Properties are a result of bond type
(Polar and nonpolar will be discussed later)

27. When the repulsive forces are overcome, the atoms can bond.

28. Energy is released when bonds are made, and when bonds are broken.
This energy can be measured.
How? Heat released, light, etc.
The same amount of energy that is required to make a bond is needed to break the bond.
Energy in = Energy out

29. Covalent bonds:
Can be measured: Bond length is the distance between 2 nuclei.

30. Are flexible: vibrate like a slinky, so bond length is variable.
The longer the bond length, the weaker the bond (lower energy).
The shorter the bond, the stronger the bond (higher energy).

32. Properties of covalent molecules.
1. Can be a solid, liquid, or gas.
The intermolecular attraction between molecules is much weaker than ionic.
Gases: very weak intermolecular forces, so molecules are spread apart

34. 2. When struck, pulverizes or turns into a powder. Can also be soft.

35. 3. Low melting and boiling points
Due to weak intermolecular forces.
Liquids are already melted at room temp.
Gases are already boiled at room temp.

36. 4. Solubility in water is variable.
5. Generally not conductive as a solid, and not conductive when dissolved.
Distilled water is NOT conductive

38. Metallic Bonds Involve only metal atoms
“Sea of electrons” hold adjacent atoms together, and contribute to the properties of metals.

41. Properties of Metallic bonds
1. Shiny solids 2. Malleable (flattens out) and ductile (can be stretched into wires)

42. Pretty high melting points
Insoluble in water.
5. Highly conductive

43. Polar covalent bonds:
Have an uneven distribution of electrons/shared unevenly.
Polar ends have a partial “charge”. More like a pull.
Structure is bent.

44. Nonpolar covalent bond:
Even distribution of electrons between atoms.
No partial charge.
Structure is usually linear (straight).

45. Using electronegativity values to predict bond type:
Electronegativity: a measure of an atom’s tendency to attract electrons.
Higher value = stronger pull.
We use the difference between the electronegativity values of the atoms in a molecule.

47. If the electronegativity difference is:
less than 0.5, then the bond is nonpolar covalent.
between 0.5 and 1.6, the bond is considered polar covalent
greater than 2.0, then the bond is ionic.
between 1.6 and 2.0:
if a metal is involved, then the bond is ionic.
If only nonmetals are involved, the bond is polar covalent.

48. But….structure is overriding factor
Examples:
Sodium chloride: NaCl
Na = Fluorine = 3.1
= ionic
Nitrogen dioxide: NO2
N = O = difference = nonpolar covalent
Carbon dioxide: CO2
C = O = difference = .9
But….structure is overriding factor

49. So….
The type of elements involved is the key determiner between ionic and covalent, and…
The structure of the molecule is the overriding factor in determining polarity.

50. How do we know the shape? Lewis dot structures
Dots represent valence electrons.
Allow us to determine polarity.
Satisfies octet rule.

52. Do some practice:
H2S
CH3OH

53. Lewis dots with double bonds:
Any unshared electrons will form a double or triple bond.
Example: carbon dioxide
Practice: C2H4

54. Naming Covalent Compounds:
Must specify how many of each element there is (unlike ionic compounds)
Ionic: MgCl2 is magnesium chloride
Covalent: CCl2 is carbon dichloride.
Why?

55. How do we know whether it is an ionic or covalent compound?
Ionic is a metal and nonmetal
Covalent is only nonmetals

56. Naming covalent compounds:
Say the first element, then the second, indicating how many of each element
Second elements may have different wording
i.e. sulfur is sulfide, oxygen is oxide
Do not say “mono” for first element.

58. Examples: SCl4 : Silicon tetrachloride CO : Carbon monoxide N2F5 :
Dinitrogen pentafluoride
CCl2F2
Carbon dichloride difluoride