1. Energy ______________ is defined as the ability to do work
This energy could be stored energy (_________________ energy) or it could be working energy (____________ energy)
In chemistry, energy is usually measured in units called ________________ (J)
Energy is found in many different forms, all of which can be categorized as either potential energy or kinetic energy

2. Different types of forces
Nuclear:
Chemical:
Intermolecular:
Strength

3. Solids, Liquids, and Gases
On the molecular level:
___________ are in an ordered arrangement; particles are essentially fixed; particles are close together
___________ have more disorder; particles are free to move relative to each other, but are still close together
___________ have total disorder; particles are very far apart and have complete random motion

4. Phase Changes
When a substance changes from one state of matter to another (i.e. water freezing, rubbing alcohol evaporating, dry ice subliming), it is called a ______________________ or ____________________
______________________.
These are _______________ changes (no chemical bonds are broken, only ____________________ forces are broken)
As the temperature goes ______ (energy is added), the molecules move ____________ and spread apart from each other

6. Endothermic/Exothermic
If the change requires energy, it is _________________________
the system gains _______ as the surroundings lose ________
If the change loses energy, it is _________________________
The system loses _________ as the surroundings gain _________

8. What is heat?
_____________________ is a measure of the average kinetic energy of the particles in a sample of matter
___________ is the total sum of the kinetic energies of the particles in a sample
The SI unit for heat is the joule (J), and heat is also sometimes measured in calories (cal)
(1 cal = _____________ J), and we will often talk about energy in kilojoules (kJ)
___________J = 1 kJ

9. What is heat, cont.
When we talk about food calories, we are really talking about how much energy is stored in that sample of food
On labels, one calorie is really equal to one Calorie, which is really a kilocalorie
232 Calories on this label is really
________________ calories

10. Specific Heat Capacity
________________________relates to how much energy it takes 1 gram of substance in order for the temperature to increase by 1 degree Celsius
The _________________ the heat capacity, the more energy it will absorb before getting “hot”
The ______________ the heat capacity, the faster it will appear to get hot, because it does not take very much energy to make the particles move fast and get hot!

11. Relating Heat to Temperature
Specific heat capacity for a substance is in the units
because it is the number of Joules required
to raise one gram of the substance by one
degree Celsius
If the __________________is multiplied by the number of ________ of the substance and the ________________________________that the substance experience, the number of Joules that was added to the substance can be calculated

12. Calculating Heat
Assorted Heat Capacities:
Air: J/g•°C
Water: J/g•°C
Copper: J/g•°C
Human Tissue: 3.5 J/g•°C
q = heat (in Joules) m = mass (in grams) c = specific heat capacity (in J/g•°C) ΔT = the CHANGE in temperature in Celsius, which is calcuated by doing Tfinal-Tinitial, which means ΔT is positive if the temperature goes up, and negative if the temperature goes down

13. The value of q Negative Positive Value of q
Temperature Change of System
Temperature Change of Environment
Endothermic/
Exothermic?
Negative
Positive

14. Example #1
A 4.0-g sample of glass was heated from 1°C to 41°C and was found to have absorbed 32 J of heat.
What is the specific heat capacity of this type of glass?
How much heat did the same glass sample gain when it was heated from 41°C to 71°C?