Chapter 2 study Guide
1. Why is it so important that we understand chemistry?
It forms the foundation of our world, explaining how everything around us is made up of chemicals and interacts
with each other.
2. Define:
a. Matter- Anything that has mass and takes up space
b. List the three states of matter- Solid, Liquid and Gas
c. Energy- Is the capacity to do work or put matter into motion
d. Kinetic energy- Energy in motion
e. Potential energy- Stored energy
3. What are the different forms of energy?
Electrical energy, Chemical energy and mechanical energy
4. Explain energy conversions. What is the result when it is not efficient?
Energy can be converted from one form to another. It is inefficient, because energy such as heat can be lost
which can partly make the energy unusable.
5. What are elements? What are the 4 elements that comprise the majority of the human body? Why is each so
important? Which one is the most abundant in the human body?
Substances that cannot be broken down or destroyed by simple chemical methods. Carbon, Nitrogen, Hydrogen
and oxygen. They form the basis of all matter. Oxygen.
6. What are the 9 elements that make up most of the rest?
Calcium
Potassium
Sodium
Sulfur
Chlorine
Iodine
Phosphorus
Magnesium
Iron
7. Define:
a. Atom- Smallest unit of functional life
b. Atomic symbol- One-two letter chemical shorthand for each element
c. Proton (where are they found?) Found in the nucleus and has a positive charge
d. Neutron (where are they found?) Found in the nucleus and has a neutral charge
e. Electron (where are they found?) Found outside of the nucleus and has a negative charge
, f. Atomic number- Number of protons in the nucleus
g. Mass number- Total number of protons and neutrons in the nucleus
h. Atomic weight- The average mass numbers of all isotope forms of an atom
i. Isotope- Structural variants of the same element
j. Radioisotope- Isotopes that decompose to more stable forms
k. Molecule (include example)- General term for two or more atoms bonded together. H2
l. Compound (include example)- Specific molecule that has two or more different kinds of atoms bonded
together. C6H12O6
m. Mixture (include example)- Two or more components that are physically intermixed. Chocolate milk is
an example of a mixture.
i. Homogenous- Mixture where parts are equally mixed together
ii. Heterogenous- Mixture where parts are not dissolved together and have a non-uniform
composition
n. Solution (include example)- A mixture where one substance is evenly dissolved in another substance.
Sugar being dissolved in water.
o. Solvent (include example)- A substance that has the ability to dissolve other substances. Water
p. Solute (include example)- A substance that has the ability to be dissolved in another substance. Salt.
q. Colloid or emulsion (include example)- A mixture of two substances where very small particles of one
substance are spread evenly throughout the other. Jell-O
r. Suspension (include example)- A substance does not dissolve in another substance. Example: Blood.
8. What is molarity and how is a 1M solution created?
Is the number of moles of solute per liter of solvent. The 1M solution is created by adding the amount of the
substance’s molecular weight in grams to enough water to make one liter of solution.
9. What is Avogadro’s number?
6.02x10^23
10. What is a chemical bond?
Energy relationships between electrons of reacting atoms.
11. What is an electron shell? How many electrons can each shell hold?
The areas around the nucleus. The shells can hold different amounts of electrons depending on how far away
from the nucleus the shell is. First shell can hold a maximum of two electrons, the second shell can hold a
maximum of 8 and so on.
12. What is the valence shell? Why is it so important?
The outermost electron shell. Holds the electrons that are involved in chemical reactions.
13. Define the octet rule.
The rule of eights. Atoms tend to have 8 electrons in their valance shells.
1. Why is it so important that we understand chemistry?
It forms the foundation of our world, explaining how everything around us is made up of chemicals and interacts
with each other.
2. Define:
a. Matter- Anything that has mass and takes up space
b. List the three states of matter- Solid, Liquid and Gas
c. Energy- Is the capacity to do work or put matter into motion
d. Kinetic energy- Energy in motion
e. Potential energy- Stored energy
3. What are the different forms of energy?
Electrical energy, Chemical energy and mechanical energy
4. Explain energy conversions. What is the result when it is not efficient?
Energy can be converted from one form to another. It is inefficient, because energy such as heat can be lost
which can partly make the energy unusable.
5. What are elements? What are the 4 elements that comprise the majority of the human body? Why is each so
important? Which one is the most abundant in the human body?
Substances that cannot be broken down or destroyed by simple chemical methods. Carbon, Nitrogen, Hydrogen
and oxygen. They form the basis of all matter. Oxygen.
6. What are the 9 elements that make up most of the rest?
Calcium
Potassium
Sodium
Sulfur
Chlorine
Iodine
Phosphorus
Magnesium
Iron
7. Define:
a. Atom- Smallest unit of functional life
b. Atomic symbol- One-two letter chemical shorthand for each element
c. Proton (where are they found?) Found in the nucleus and has a positive charge
d. Neutron (where are they found?) Found in the nucleus and has a neutral charge
e. Electron (where are they found?) Found outside of the nucleus and has a negative charge
, f. Atomic number- Number of protons in the nucleus
g. Mass number- Total number of protons and neutrons in the nucleus
h. Atomic weight- The average mass numbers of all isotope forms of an atom
i. Isotope- Structural variants of the same element
j. Radioisotope- Isotopes that decompose to more stable forms
k. Molecule (include example)- General term for two or more atoms bonded together. H2
l. Compound (include example)- Specific molecule that has two or more different kinds of atoms bonded
together. C6H12O6
m. Mixture (include example)- Two or more components that are physically intermixed. Chocolate milk is
an example of a mixture.
i. Homogenous- Mixture where parts are equally mixed together
ii. Heterogenous- Mixture where parts are not dissolved together and have a non-uniform
composition
n. Solution (include example)- A mixture where one substance is evenly dissolved in another substance.
Sugar being dissolved in water.
o. Solvent (include example)- A substance that has the ability to dissolve other substances. Water
p. Solute (include example)- A substance that has the ability to be dissolved in another substance. Salt.
q. Colloid or emulsion (include example)- A mixture of two substances where very small particles of one
substance are spread evenly throughout the other. Jell-O
r. Suspension (include example)- A substance does not dissolve in another substance. Example: Blood.
8. What is molarity and how is a 1M solution created?
Is the number of moles of solute per liter of solvent. The 1M solution is created by adding the amount of the
substance’s molecular weight in grams to enough water to make one liter of solution.
9. What is Avogadro’s number?
6.02x10^23
10. What is a chemical bond?
Energy relationships between electrons of reacting atoms.
11. What is an electron shell? How many electrons can each shell hold?
The areas around the nucleus. The shells can hold different amounts of electrons depending on how far away
from the nucleus the shell is. First shell can hold a maximum of two electrons, the second shell can hold a
maximum of 8 and so on.
12. What is the valence shell? Why is it so important?
The outermost electron shell. Holds the electrons that are involved in chemical reactions.
13. Define the octet rule.
The rule of eights. Atoms tend to have 8 electrons in their valance shells.
