06.01 Energy

Page 1: Introduction
Reflect on the role of speed in substance dissolution.

Page 2: What are the different forms of energy?
Define: 
•	Energy:
•	Work:
•	Potential energy:
•	Kinetic energy:

What are joules?

Complete the chart with some examples of energy.
Kinetic	Potential	

		

		

Page 3: How is energy conserved during physical and chemical processes?
Complete the sentences:
•	According to the law of conservation of energy,
•	A gasoline car in use releases _____________ energy and _______________ energy.
List the types of energy at the Hoover Dam:
•	
•	
Provide two examples of ways of conserving energy:
•	
•	

Define "conservation of energy":

Page 4: How is heat different than temperature?
Explain the interaction and motion of sugar and coffee particles:
Complete the sentences:
•	The temperature of a substance is determined by

•	Hotter objects have

•	Temperature measures the

Complete the chart with the units of measurement:
Unit of measurement	Description	Unit	Freezing point of water	Boiling point of water	

					

Complete the sentence: Absolute zero is

True (T) or false (F)?
_____ Scientists have been able to achieve a temperature of 0 K or -273.15 °C.

06.02 Kinetic Molecular Energy

Page 1: Introduction
Reflect on the volcanoes and lightning phenomena:

Page 2: What is the interaction between kinetic energy, motion, and the temperature of particles?
Explain the change in tire pressure:
Define: Kinetic theory of matter:
List what is known about the kinetic theory of matter:

	

List the two ways in which particles in matter are observed to interact with heat. Feel free to draw:
1.	
2.	
Complete the sentences:
•	Hotter objects have
•	Cooler Objects
•	Temperature is always the
Explain how thermometers work:

Page 3: How do particle arrangement and motion differ between the states of matter?
Describe the four types of matter.

Complete the sentences:
•	In solids, particles are
•	In liquids or gases, particles are
Interactive. Complete the charts below with information about each matter:
	Solid	Liquid	Gas	Plasma	
Description	
				
Arrangement of particles					
Motion					
Shape					
Volume					
Compressibility					

Page 4: What are the characteristics of gases?
Complete the chart about the properties of gases. Feel free to draw too:
Density

		
Compressibility

Expansion

Diffusion

Fluidity

Page 5: How are the properties of gases measured?
Complete the chart with the most commonly used measurements to describe gases in chemistry:
Physical Characteristics and Variable	Typical unit	

		

Define: Pressure:
Write the Units of pressure of 1 atmosphere:
Convert 10 atm to mm Hg: 

Page 6: What are the postulates for the kinetic molecular theory of gases?
Define:
•	Kinetic molecular theory:
•	Ideal gas:
Complete the sentences:
•	The kinetic molecular theory of gases is helpful to understand
•	An ideal gas behaves
True (T) or false (F)?
_____ In real life, most gases are quite ideal.

Interactive: Describe each postulate of the kinetic molecular theory:
Postulate	Description	
The particles of a gas are in constant random motion. 		
Gases consist of large numbers of tiny particles. 		
Collisions between gas particles are elastic.		
No forces of attraction or repulsion are experienced between gas particles.		
The average kinetic energy of the particles of a gas is directly proportional to their temperature.		

06.03 Phase Changes Journal (Notes)
Note: This is NOT the lab assignment. This is for your notes, not to be submitted.
Page 1: Introduction
Reflect on the "snow vapor" phenomenon.

Page 2: What are the transition points for each phase change?
Define: Phase transition:
Complete the sentence: Phase changes are caused by

Interactive: Complete chart with information about the transition points from one state of atter to another:
Transition	Description	
Melting
		
Freezing 
		
Boiling
		
Condensation

Write the relationship between transition points:

Define: Dewpoint of the day:
Complete the sentences: The dewpoint
•	The dewpoint depends on
•	The dewpoint is associated with
•	The dewpoint is close to the current air temperature when there is 

Page 3: What is the effect of energy in phase transitions of matter?
Interactive: Explain the demonstration on the sample of water in your own words:

Complete the sentences:
•	Water stays in a liquid state as the temperature and kinetic energy of the molecules increase from 0 °C to 100 °C. This consistency indicates that 

•	At the melting and boiling points, the temperature

•	The energy needed to overcome all the intermolecular forces between molecules must be __________ than the potential energy of the bonds between molecules.
•	When all the intermolecular bonds are ____________, the transition between phases is complete.
•	The energy of any substance includes the ________, ________, and _________ _________ of its particles

Page 4: How are changes in temperature and states of matter represented in heating and cooling curves?
Define:
•	Heating curves
•	Cooling curves
•	Both curves show

A heating curve shows:
A cooling curve shows:

Interactive. Complete the charts with information about phase transitions of water: 
Solid:
	
Melting Point:
	
Liquid:
	
Boiling Point:
	
Gas:

Gas:
	
Liquid-Gas Phase Change:
	
Liquid:
	
Solid-Liquid Phase Change:
	
Solid:

06.04 Gas Laws

Page 1: Introduction
Reflect on the information about the Siberian region.

Page 2: What is the purpose of scientific laws?
Define: Scientific law:
Complete the sentences about scientific law:
•	A scientific law is based on
•	It is tested
•	It continues to be

True (T) or false (F)?
_____ Because laws and theories are developed for different purposes, laws never become theories and theories do not become laws.
Describe:
Newton's Law of Universal Gravitation

Gas Laws

Page 3: How do changes in pressure, temperature, volume, and mole amount affect gases?
Complete the sentences:
•	Gas particles move
•	They respond to these four factors:
1.	
2.	
3.	
4.	
Interactive: Complete the sentences about pressure gauges:
•	If the volume of a sample is large, the pressure will be _______ and there will be _______ particle collisions.
•	In the volume of a sample is small, the pressure will be _______ and _______ collisions will occur.
•	If the number of particles decreases, the number of collisions will _____________.
•	If the number of particles increases, the number of collisions will _____________.
•	If temperature decreases, the number of collisions will ________________.
•	If temperature increases, the number of collisions will ________________.

Page 4: How do scientific laws predict the behavior of gases?
Video. Complete the sentences:
•	To understand and predict how gases behave, we first need to understand the relationships between
Describe the different experiments on gases.

List the four initial and final factors variables:
Initial quantities

	Final quantities	

Complete the sentences:
•	Temperature is represented by the unit ______________________.
•	In gas problems, the phrase standard temperature is ____________________ or the standards pressure is ____________________.

Interactive. Complete the chart with information about gas laws:
Law	Relationship	Gas Behavior	Constants	
Boyles’s Law
				
Charles’s Law
				
Gay-Lussac’s Law
				
Avogadro’s Law

Copy the examples of each gas law being applied.
Example	Givens	Solutions	
1.30 L of a gas is at 5.0 atm. What will its volume be at a pressure of 6.0 atm?			
A gas is collected and found to fill 3.50 L at 350 K. What will its volume be at a temperature of 273 K?			
The pressure of a gas is 2.75 atm at 350 K. What will its pressure be at a standard temperature of 273 K?			
5.76 moles of a gas are in a 5-mL balloon. If a girl blows into the balloon and increases its volume by 2 mL, what will be its new molar amount?			

06.05 Gas Laws
No journal notes for this lesson

06.06 Honors Ideal Gas Behavior

Page 1: Introduction
Reflect about how a gas behaves when its temperature changes:

Page 2: How can ideal gas relationships predict the volume of gases in a chemical reaction?
Write the relationship between mole and volume ratios:
Write:
•	The mole ratio:
•	The volume ratio:

Use the coefficients as a volume ratio to determine how many milliliters of carbon dioxide gas can be produced when 206.5 milliliters of oxygen gas react with excess carbon monoxide:
2CO(g) + O2(g) → 2CO2(g)

Page 3: How does the ideal gas law show the relationship between the properties of gas?
Complete the sentence about the ideal gas law:
•	It describes
•	It does not explain

Video. Complete the sentences:
•	The three factors that determine the movements of atoms are ________________.
•	Multiple versions of gas laws have been combined into one equation that's called the __________________________. This law is expressed as ____________________. 

List the meaning of:
o	P =
o	V =
o	n =
	o	R =
o	T =	
The ideal gas equation is an ______________, not an __________ description of the behavior of gas.
Write the equation of the Ideal Gas Law:		Complete the chart:
Solving for	Typical units	

	

	

Page 4: How are calculations performed using the ideal gas law?
Video. Combine the ideal gas law equation with stoichiometry to determine how many liters of hydrogen gas can be produced at 289 Kelvin and 1.3 atmospheres if 38 grams of aluminum metal reacts with excess hydrochloric acid.

Determine how many liters of hydrogen gas can be produced at 300.0 Kelvin and 0.970 atmospheres if 52.0 grams of magnesium metal react with excess hydrochloric acid:
Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq)
Step 1
	
Step 2
	
Step 3
	
Step 4
	
Step 5

Determine how many grams of sodium chloride can react with 18.3 liters of fluorine gas at 1.20 atmospheres and 299 Kelvin:
F2(g) + 2NaCl(s) → Cl2(g) + 2NaF(s)
Step 1
	
Step 2
	
Step 3
	
Step 4
	
Step 5

Page 5: How does a gas being at STP affect ideal gas calculations?
Complete the sentences or statements: 
•	According to Avogadro’s principle, equal volumes
•	STP stands for
•	At STP, one mole of any gas
•	Standard temperature is
•	Standard pressure is

Fill in the blanks. When the volume is 22.4 L.

Helium	
Oxygen Gas	
Nitrogen Gas	
1 mol He	
1 mol O2	
1 mol N2	

	

	
1 atm	
1 atm	
1 atm	
	Write the factors in the mole to volume conversion when the gas is at STP:

	

Determine how many grams of calcium oxide (lime) are produced when 50.0 liters of carbon dioxide are produced at STP: CaCO3(s) → CaO(s) + CO2(g)