CHEMICAL ELEMENTS
ATOMS
1. Define atom.
2. What three subatomic particles make up atoms?
3. What charge does each subatomic particle have?
SUBATOMIC PARTICLE
Proton
Neutron
Electron
CHARGE
4. How does a proton compare to a neutron in relative mass?
5. How does a proton compare to an electron in relative mass?
6. What two subatomic particles make up the nucleus of an atom?
7. Why do electrons remain outside of the nucleus of an atom?
8. Why are atoms electrically neutral?
9. Define element.
10. Element numbers:
Number of elements found in nature
Total number of elements
11. List four elements and their chemical symbols:
ELEMENT
12. Define atomic number.
SYMBOL
ISOTOPES
1. Define isotope.
2. Define radioactive isotope.
3. What can geologists determine using radioactive isotopes?
4. List two ways in which physicians may use radioactive isotopes.
5. Complete the following table regarding the isotopes of Carbon.
Proton number
Electron number
Carbon - 12
Carbon - 13
Carbon - 14
CHEMICAL COMPOUNDS and CHEMICAL BONDS
1. Define compound.
2. List the chemical formulas for the following compounds.
compound
water
table salt
carbon dioxide
chemical formula
3. Define ionic bond.
4. Define ion.
5. An example of an ionic bond: table salt
a. Sodium: one of the elements composing table salt
Number of electrons in the outermost energy level
Number of electrons that tend to be lost
Resultant sodium ion charge
b. Chlorine: the other element composing table salt
Number of electrons in the outermost energy level
Number of electrons that tend to be gained
Resultant chlorine ion charge
Neutron number
6. Define covalent bond.
7. Provide at least one compound that is formed by a covalent bond.
8. How many electrons are shared in each of the following bonds:
Type of Bond
Single Bond
Double Bond
Triple Bond
Number of Electrons Shared
9. Define molecule.
10. Write the chemical formula for one molecule of water.
THE WATER MOLECULE
1. What is the chemical formula for water?
2. Draw the structural formula of water including symbols for positive and negative charge.
3. Why are water molecules considered “polar” molecules?
4. Why are water molecules attracted to one another?
5. Define hydrogen bond.
6. How does the relative strength of a hydrogen bond compare to covalent and ionic bonds?
7. Apply your knowledge!
a. What happens to water when it freezes to form ice?
b. Why is this biologically significant to fish and other aquatic life in Minnesota?
SOLUTIONS AND SOLVENTS
1. Define mixture.
2. Provide two examples of mixtures.
3. List two types of mixtures.
4. Define solution.
5. Define solute.
6. What solution is found in Figure 2.9?
7. What solute is found in Figure 2.9?
8. What solvent is found in Figure 2.9?
pH, CARBON COMPOUNDS, and MACROMOLECULES
1. Draw a diagram of the pH scale and label acid, base, and neutral.
2. How many bonds does each of the following elements form?
Element
Carbon
Nitrogen
Oxygen
Hydrogen
Number of Bonds
3. Define Monomer.
4. Define Polymer.
5. List the four major macromolecules found in the living organisms.
a.
b.
c.
d.
pH Diagram