1. Ch. 13 - Liquids & Solids I. Bonding Review
See Chapter 5 Notes Bonding Types:
Chart on 3 types of bonds -

2. A. Inter… and Intra…
Intermolecular Forces
Intramolecular
Forces

3. A. Inter… and Intra… Attractive forces between molecules.
Chemical bonds within molecules.

4. B. Types of Chemical Bonds
IONIC
“COVALENT”
Bond Formation
e- are transferred from metal to nonmetal
e- are shared between two nonmetals
Type of Structure
crystal lattice
Both intra- and inter-
Physical
State
solid
liquid or gas
Melting
Point
Low (Intermolecular force breaks)
high
Solubility in
Water
yes
usually not
Electrical Conductivity
yes (solution or liquid) no
Other
Properties
Strong bonds
Weak bonds

5. B. Types of Chemical Bonds
IONIC
TRUE COVALENT
Bond Formation
e- are transferred from metal to nonmetal
e- are shared between two nonmetals
Type of Structure
crystal lattice
true molecules
Physical
State
solid
Solid (SiO2 /diamond)
Melting
Point
high
Very high
Solubility in
Water
yes no
Electrical Conductivity
yes (solution or liquid) no
Other
Properties
Strong bonds
Strongest bond

6. B. Types of Chemical Bonds
Difference in the elements’ e-negs determines bond type:
> 2.0 Ionic
0.4 – 2.0 Polar C
< 0.4 Nonpolar C

7. B. Types of Chemical Bonds
METALLIC
Bond Formation
e- are delocalized among metal atoms
Type of Structure
“electron sea”
Physical
State
solid
Melting
Point
very high
Solubility in
Water no
yes (any form)
Electrical Conductivity
Other
Properties
malleable, ductile, lustrous

8. Types of IMF(InterMF)

9. C. Types of IMF
London Dispersion Forces
View animation online.

10. C. Types of IMF Dipole-Dipole Forces + -
View animation online.

11. C. Types of IMF
Hydrogen Bonding

12. B. Types of Chemical Bonds
Ionic Bonding - Crystal Lattice
RETURN

13. B. Types of Chemical Bonds
Covalent Bonding - True Molecules
Diatomic Molecule -7
RETURN

14. B. Types of Chemical Bonds
Metallic Bonding - “Electron Sea”
RETURN

15. Molecular Formula: The actual formula for a molecule.
Problem:
A compound has an empirical formula of ClCH2 and a molecular weight of g/mol. What is its molecular formula?
Strategy:
Find the mass of the empirical unit.
Figure out how many empirical units are in a molecular unit.
Write the molecular formula.

16. Strategy:
Find the mass of the empirical unit. Mass of empirical unit = mass Cl + mass C + 2(mass H) Mass of empirical unit = (1.008) = g/mol
Figure out how many empirical units are in a molecular unit. # of empirical units = (mass of molecular unit/ mass of empirical unit) (98.96 g/mol) / (49.47 g/mol) = empirical units per molecular unit
Write the molecular formula. It takes two empirical units to make a molecular unit, so, the molucular formula is: Dichloro Ethane Cl2C2H4

17. The percent composition (percentage composition) of a compound is a relative measure of the mass of each different element present in the compound. To calculate the percent composition (percentage composition) of a compound
Calculate the molecular mass (molecular weight, formula mass, formula weight), MM, of the compound
Calculate the total mass of each element present in the formula of the compound
Calculate the percent composition (percentage composition): % by weight (mass) of element     = (total mass of element present ÷ molecular mass) x 100

18. Calculate the molecular mass (MM): MM = 22.99 + 35.45 = 58.44
Examples
Calculate the percent by weight of sodium (Na) and chlorine (Cl) in sodium chloride (NaCl)
Calculate the molecular mass (MM): MM = = 58.44
Calculate the total mass of Na present: 1 Na is present in the formula, mass = 22.99
Calculate the percent by weight of Na in NaCl: %Na = (mass Na ÷ MM) x 100 = (22.99 ÷ 58.44) x 100 = 39.34%
Calculate the total mass of Cl present: 1 Cl is present in the formula, mass = 35.45
Calculate the percent by weight of Cl in NaCl: %Cl = (mass Cl ÷ MM) x 100 = (35.45 ÷ 58.44) x 100 = 60.66%
    The answers above are probably correct if %Na + %Cl = 100, that is,     = 100.

19. Calculate the percent by weight of each element present in sodium sulfate (Na2SO4).
Calculate the molecular mass (MM): MM = (2 x 22.99) (4 x 16.00) =
Calculate the total mass of Na present: 2 Na are present in the formula, mass = 2 x = 45.98
Calculate the percent by weight of Na in Na2SO4: %Na = (mass Na ÷ MM) x 100 = (45.98 ÷ ) x 100 = 32.37%
Calculate the total mass of S present in Na2SO4: 1 S is present in the formula, mass = 32.06
Calculate the percent by weight of S present: %S = (mass S ÷ MM) x 100 = (32.06 ÷ ) x 100 = 22.57%
Calculate the total mass of O present in Na2SO4: 4 O are present in the formula, mass = 4 x = 64.00
Calculate the percent by weight of O in Na2SO4: %O = (mass O ÷ MM) x 100 = (64.00 ÷ ) x 100 = 45.06%
    The answers above are probably correct if %Na + %S + %O = 100, that is,     = 100

21. Melting / Freezing : Vaporization / Condensation: Sublimation / Deposition

22. Questions:
1. What is the most likely state of matter when particles are moving slow or fast?
2. How do Intermolecular forces determine the state of matter?
3. What type of IMF do gas particles have? Name the other two and strength of force.
Draw and label the heating curve of water
4. What does the heating curve graph show us?
5. What does each plateau indicate?
6. What temp is the heat of fusion of ice? The heat of vaporization of water?
7. Why is there NOT a temp change during the phase changes?