1. Physical Properties and Density
Turk

2. Physical Properties Viscosity Resistance to flow
Decreases when a fluid is heated
Conductivity
Ability to allow heat to flow
Malleability
Can be hammered and change shape without shattering
Hardness
Melting and Boiling points

3. Density is the measure of the “compactness” of a material
How close the atoms or molecules are to eachother
More than “heaviness” - density includes how much space an object takes up!!
All substances have density including liquids, solids, and gases
Bread slice and compacted bread in large flask of water

4. Density = amount of matter per unit volume
Density is the ratio of mass to volume
If the volume stays the same and the mass increases the density will increase
If the mass stays the same and the volume increases The density will decrease

5. The “DMV” Triangle for Volume, Mass, and Density
÷ ÷
D X V
Volume = M D
Mass =
D x V

6. What would take up more space. A kilogram of feathers…
What would take up more space??? A kilogram of feathers….. or a kilogram of steel??
ROCKS - pass around OR

7. What would happen???? Mercury density = 13600kg/m3
Lead density = 11340kg/m3
Sinking vial - make it float

8. Lead floats on liquid mercury!

9. Reporting Measurements
Using significant figures
Report what is known with certainty
Add ONE digit of uncertainty (estimation)
By adding additional numbers to a measurement – you do not make it more precise. The instrument determines how precise it can make a measurement. Remember, you can only add ONE digit of uncertainty to a measurement.
Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 46

10. 1. If the glassware is marked every 10 mLs, the volume you record should be in mLs. (Example A)
2. If the glassware is marked every 1 mL, the volume you record should be in tenths of mLs.
3. If the glassware is marked every 0.1 mL, the volume you record should be in hundredths of mLs. (Example B)
Example B
Example A
0 mL
30 mL
20 mL
1 mL
10 mL
30-mL beaker:
the volume you write in your lab report should be 13 mL
2 mL
Buret marked in 0.1 mL: you record volume as 0.67 mL

11. Practice Measuring cm 1 2 3 4 5 4.5 cm cm 1 2 3 4 5 3.0 cm1 2 3 4 5
4.5 cm cm 1 2 3 4 5
3.0 cm
PRACTICE MEASURING
Estimate one digit of uncertainty.
a) 4.5 cm
b) * 4.55 cm
c) 3.0 cm
*4.550 cm is INCORRECT while 4.52 cm or 4.58 cm are CORRECT (although the estimate is poor)
The better marks the better we can estimate.
Scientist always understand that the last number measured is actually an estimate
Timberlake, Chemistry 7th Edition, page 7

12. Using Significant Figures reflects precision by estimating the last digit
52 ml
.8 ml
What is the certain measurement?
What is the estimated measurement?

13. The instrument determines the amount of precision of the data.
62.4
.00g
What is the certain measurement here?
What is the estimated measurement here?

14. SOLIDS
Ice is less dense than water (which is why lakes and ponds have a thin layer of ice covering in winter, with water underneath)
Various rocks, woods, metals have a characteristic density specific to that substance
Beans/ping pong ball; Big jug of water in a pool

15. Factors affecting Density
Temperature
Pressure
Add several drops of red food color to each of two 250-mL Erlenmeyer flasks; fill them with warm tap water. (If tap water is not warm, heat some tap water on a hot plate to °C.)
Add several drops of blue food coloring to each of the other two 250-mL Erlenmeyer flasks; fill them with cool tap water.
Predict the outcome when one flask is inverted over the other.
Place a paper card on top of the vessel filled with warm water. Invert the flask making sure to hold the card in place. Stack it on top of one of the cool water flasks. Remove the card. Remain prepared to catch the flasks.
  ** Visual here.
Place a paper card on top of the flask filled with cool water. Invert the flask making sure to hold the card in place. Stack it on top of the other warm water flask. Remove the card.
Wide mouth containers may also be used.

16. Factors affecting Density
Dissolved solids – in liquids
Concentration and kind of substances

17. FACTORS AFFECTING DENSITY
ATomS!!!!
FACTORS AFFECTING DENSITY

18. Relative Density
The density of a material or substance, relative to another substance
Expressed in a ratio: water = 1g/cc
Water is the substance to which we generally compare other substances
ALSO known as SPECIFIC GRAVITY
Relative Liquid densities: Oil, colored water, and corn syrup in a graduated cylinder.
An H2O ice cube floats in liquid H2O but floats in rubbing alcohol. A can of diet coke floats in water while a can of regular coke sinks (can determine density of sugar versus NutraSweet using balance).

19. Absolute DENSITY
The density of a material in its closest “packed form”
For water: Absolute Density = 1000kg/m3
at 40C and 1 atm(pressure)
in other words, the greatest density of water is at 40C

20. DETERMINING DENSITY
Regular Shapes – mass, then determine the volume by formula
EX: cubes, cylinders, spheres, cones, etc.
Irregular shapes – mass, then measure displacement of a liquid (usually water) by that irregularly shaped object
Use a graduated cylinder
Add water to a predetermined level - record.
Gently drop in the irregularly shaped object.
Read the graduated cylinder – record.
Subtract the first water level from the second – this is the volume

21. Density Table SINK or FLOAT In Water (D = 1.0 g/mL) Float Float Float
(alcohol)
Float
(fuel)