Mr. Bannister
HAHS
CHEM 1B
MIDTERM STUDY GUIDE: * EXAM: Friday, April 4th *
Name: ____________________________________ Date: _________________________Block: _______________
CHAPTER 12:
THINGS TO KNOW:
1.
2.
The 4 measurable properties of gases. ____________, _____________, _____________, ____________.
The units for volume are ___________. The units for temperature are ___________. The units for pressure are ____________.
What does STP mean? What is the value of temperature? What is the value of pressure?
_________________________________________________________________________________________
BOYLE’S LAW
1.
Know the relationship between pressure and volume: As the pressure increases, volume_____________.
a.
A weather balloon with a volume of 1.375 L is released from the Earth’s surface at sea level( 100kPa.) What volume will the
balloon occupy at an altitude where the pressure is 10kPa (1kPa = 1000Pa)? 14 L
CHARLES’LAW
1.
Know the relationship between temperature and volume. As the temperature increases, volume __________.
a.
A balloon filled with oxygen gas occupies a volume of 5.5 L at 25C. What will the volume be at 100C (1000mL = 1L)? 6.9L
GAY-LUSSAC’S LAW
1.
Know the relationship between temperature and pressure (direct or indirect). As the temperature increases, pressure
__________________.
a.
Sample of hydrogen at 47C exerts a pressure of 0.329 atm. The gas is heated to 77C at constant volume. What will its new
pressure be? 0.360 atm
COMBINED GAS LAW
1.
Be able to write the mathematic expression…what is the formula?
a.
2.00 L of a gas is collected at 25.0°C and 745.0 mmHg. What is the volume at STP? 1.8L
IDEAL GAS LAW
1.
Given a set of data, be able to solve for an unknown using the ideal gas law.
a.
How many liters are occupied by a 0.909 mol of nitrogen at 125C and 0.901 atm? 33.0L
Mr. Bannister
HAHS
CHEM 1B
CHAPTER 15:
1.
2.
3.
4.
5.
6.
7.
An ionic bond is formed between a(n) ______________ and a(n) ____________________.
Electrons in the outer most shell are known as _______________________.
Atoms bond in order to obtain ______ electrons. This is known as a(n) _________________.
Metals form a ________ (positive/negative) charge. This is known as a(n) ______________.
Nonmetals form a _________ (positive/negative) charge. This is known as a(n) ______________.
The regular repeating arrangement of ions in an ionic solid is known as a(n) _____________.
Write the electron configuration for the following atoms. Place a box around the valence electrons.
Ge: _____________________________________________________________________
Si: ____________________________________________________________________
K: _____________________________________________________________________
8.
Using the picture below, describe why ionic compounds dissolved in water conduct electricity? Compare it to that of
solid ionic compounds.
Mr. Bannister
HAHS
CHEM 1B
CHAPTER 16:
1.
How many bonds does hydrogen always form and why can it only form that many?
2.
Draw the Lewis Structure for each molecule. Identify the structure’s molecular geometry.
NH4+
H2O
Shape:
Shape:
Cl2
PH3
Shape:
SO42-
Shape:
Shape:
Shape:
3.
Which bond type is the shortest? Explain why.
4.
Which bond type requires the most amount of energy to break?
5.
Classify 3 polar bonds and 3 nonpolar bonds in the compound below.
C I 2O
(carbon, iodine, and oxygen)
Mr. Bannister
HAHS
CHEM 1B
CHAPTER 17:
1.
Describe the hydrogen bonding between molecules in water. Refer to the picture below.
2.
How is hydrogen bonding responsible for the high surface tension and low vapor pressure of water?
3.
What is a surfactant? How does it affect the surface tension of water?
4.
What is the specific heat capacity of water? What does it mean? Why is it a GOOD thing it is higher than most other
things?
Mr. Bannister
HAHS
CHEM 1B
Chapter 11: Thermochemistry – Heat and Chemical Change
1.
What is temperature? What is heat?
2.
What is an endothermic reaction? What is an exothermic reaction?
3.
What is ∆T? BE ABLE TO CALCULATE given two temps (in ⁰C or K or both)
a. What is ∆T for the following?
i. 117⁰C to 154⁰C
ii. 117⁰C to 100⁰C
iii. 565 K to 600 K
iv. 134 K to 54⁰C
4.
What value of ∆H will be exothermic? What value will be endothermic?
5.
What is the ultimate determinant of spontaneity?
6.
Be able to calculate using specific heat capacity
a.
Cp = q/m∆T
b.
Calculate the specific heat capacity of a sample with a mass of 40.4g and an increase in temp from
298K to 343K. It absorbed 745 J of heat
7.
What is a calorimeter? Be able to identify certain parts of it
8.
The heat of formation of a free element in its standard state is always what???
9.
What is the difference between specific heat capacity and molar heat capacity?
10. On a sunny day, why does the concrete deck around an outdoor pool become hot, while the water stays cool?
Mr. Bannister
HAHS
CHEM 1B
Chapter 19: Reaction Rates and Equilibrium
1.
What is the collision theory? What must occur for a reaction to take place?
2.
What is meant by the rate of a chemical reaction?
3.
How can you increase the rate of reaction (speed)?
4.
How does each factor affect the rate of a chemical reaction?
a. Temperature
b. Concentration
c. Particle size
d. Addition of a catalyst
e. Addition of an inhibitor
5.
Does every collision between reacting particles lead to products? Explain
6.
What is the difference between a successful and unsuccessful collision?
7.
Refrigerated food stays fresh for long periods. The same food stored at room temperature quickly spoils. Why?
8.
What do we need catalysts in our bodies? Why can we not just “heat ‘em up”??
9.
What is a reversible reaction?
10. What is LeChatliers Principle?
11. How can changes in equilibrium position be predicted from changes in concentration, temperature, and
pressure?
12. What is the significance of the double sided arrow in a chemical equation?
13. Can a pressure change shift the equilibrium position in every reversible reaction? Explain your answer.
Mr. Bannister
HAHS
CHEM 1B
14. Explain what is meant by the following:
a. Entropy
b.
Enthalpy
c.
Free energy
d.
Spontaneous reaction
e.
Nonspontaneous reaction
15. What can change a reaction from nonspontaneous to spontaneous?
16. Suppose the products in a spontaneous process are more ordered than the reactants. Is the entropy change
favorable or unfavorable?