1. Matter and Energy

2. I. Matter Matter is anything that has mass and volume Mass Volume
Amount of matter
Measured in grams (g)
Volume
Space matter occupies
Measured in milliliters (mL), liters (L) or cubic centimeters (cm3 )
Two types of matter
Pure substances
Mixtures

3. A. Pure Substances Uniform composition Two Types
The same throughout the sample
Two Types
Elements
Compounds

4. 1. Elements Simplest form of matter
Smallest part called atom
Cannot breakdown
Represented using a capital letter or capital letter and lower case letter
Carbon (C)
Sodium (Na)

5. 2. Compound Two or more elements chemically joined in a specific ratio
Properties of the compound are different than the elements that make it up
Compounds can be broken down
Decomposed
Examples
Water (H2O)
Hydrogen peroxide (H2O2)

6. B. Mixture Two or more substances physically joined in any ratio
Keep the properties of their components (parts)
Can be separated by physical means
Exist in two forms
Heterogeneous
Homogeneous

7. Heterogeneous Homogeneous
Visible difference between components (parts)
No visible differences between components (parts)
Called a solution
Represented using (aq)

8. C. Properties of matter Physical Properties Chemical Properties
Properties that can be observed without changing the substance
Chemical Properties
Properties that show how a substance reacts (changes)

9. Density—a physical property used to identify a substance Density = mass
volume

10. Determine the density of an object with a mass of 59
Determine the density of an object with a mass of 59.3g and a volume of 84.2 mL.
Density = Mass ÷ Volume
d = 59.3g ÷ 84.2mL
d = .704g/mL
Determine the mass of an object with a density of 0.94g/mL and a volume of 24.8 mL.
Solve for mass
Mass = Density x Volume
m = 0.94g/mL x 24.8mL
m = 23.3g
Determine the volume of an object with a density of 1.47g/mL and a mass of 28.6g.
Solve for volume
Volume = Mass ÷ Density
v = 28.6g ÷ 1.47g/mL
v = 19.5mL

11. II. Energy Energy is the driving force behind change
Cannot be created or destroyed
It can change its form
Two types of energy
Kinetic
Energy of motion
Potential
Stored energy

12. A. Measurements involving energy
1. Temperature
Average kinetic energy of particles
Measured using a thermometer (unit: degrees)
Fahrenheit
Celsius
Kelvin
To convert
°F to °C -- use °C = 5/9( °F - 32)
°C to ° F -- use °F = 9/5 °C + 32
°C to K -- use K = °C + 273
K to °C – use K = °C + 273

13. 2. Calorimetry Measures the actual energy (q) in a system
Related to mass (m), specific heat capacity (C) and temperature change (∆T)
Measured using a calorimeter (unit: joules)
To calculate energy use Reference Table T

14. How many joules are required to heat 40g water at 30°C to 80°C?
q = m C ∆T
q = 40g x 4.18J/g°C x 50°C
q = 8360J

15. 5000J were added to 30g water at 25°C. What is the new temperature?
q = m C ∆T
5000J = 30g x 4.18J/g°C x ∆T
5000 = x ∆T
∆T = 39.9 ~ 40
T new =
T new = 65°C

16. How many joules are needed to melt 100g ice at 0°C
q = m Hfus
q = 100g x 334J/g
q = 33400J

17. III. Phases of Matter
Solids
Liquids
Gases

18. A. Solids Matter that has specific shape and specific volume
Atoms closely packed together
Cannot be compressed

19. B. Liquids
Matter that has a specific volume but takes the shape of the container
Atoms are close but have some space between them
Cannot be compressed
Can be poured

20. C. Gases Matter that takes the shape and volume of the container
Atoms have free space between them
Compressible
Can be poured

21. D. Phase Changes If energy is added… If energy is removed…
Solid to liquid
Melting
Liquid to gas
Boiling
Solid to gas
Sublimation
Liquid to solid
Freezing
Gas to liquid
Condensing
Gas to solid
Deposition

22. E. Phase Diagram
Boil
Gas
Temperature
Melt
Liquid
Solid
Time

23. Heat of
Vaporization
Gas
Temperature
Heat of
Fusion
Liquid
Solid
Time

24. Kinetic Energy Potential Energy Temperature Potential Energy Kinetic
Kinetic
Energy
Potential
Energy
Temperature
Potential
Energy
Kinetic
Energy
Kinetic
Energy
Time

25. F. Gas Laws Gas volume is controlled by pressure and temperature
1. Units
Volume
mL L cm3
Pressure
atm kPa
Temperature
°C K is the only unit to be used

26. F. Gas Laws 2. Boyle Law As pressure increases, volume decreases
P1V1 = P2V2
3. Charles Law
As temperature increases, volume increases
V1 = V2
T T2

27. Converting pressure units
Convert 1.9 atm to kPa
101.3 kPa = x kPa
1 atm 1.9 atm
(101.3)(1.9) = (1)(x)
x = kPa
Convert 180 kPa to atm
101.3 kPa = 180 kPa
1 atm x atm
(101.3) (x) = (1)(180)
x = 1.8 atm

28. 20 mL of CO2(g) at 1. 2 atm is compressed to 15 mL
20 mL of CO2(g) at 1.2 atm is compressed to 15 mL. What is the new pressure of the gas?
P1V1 = P2V2
20 mL = volume (V)
1.2 atm = pressure (P)
15 mL = volume (V)
(1.2 atm)(20 ml) = P2(15 ml)
P2 = 1.6 atm

29. 100 mL of NH3(g) at 25°C is heated to 50°C
100 mL of NH3(g) at 25°C is heated to 50°C. What is the new volume of the gas? V1 = V2 T1 T2 25°C = 298 K 50°C = 323 K 100 ml = V2 298 K 323 K (100)(323) = (298) V = 298V V2 = 108 ml

30. When 500 mL of NH3(g) at 25°C was cooled, its new volume became 250 mL
When 500 mL of NH3(g) at 25°C was cooled, its new volume became 250 mL. What is the Celsius temperature of the gas? V1 = V2 T1 T2 25°C = 298 K 500 ml = 250 mL 298 K T2 (298)(250) = (500) T = 500 T T2 = 149 K 149 K = °C °C