Supplemental Instruction
Iowa State University / Leader: / Lauren
Course: / Biol 212
Instructor: / Dr. Coffman/Powell-Coffman
Date: / 8/28/2017
- Matching terms and definitions
Word / Definition
1[1] / Proton / a / Academic support model
2[2] / Neutron / b / This type of bond is observed between separate water molecules in solution
3[3] / Electron / c / Term used to describe water’s ability to stick to itself
4[4] / Period / d / A measure of the concentration of hydrogen atoms in solution
5[5] / Group / e / Term used when a something is both hydrophilic and hydrophobic
6[6] / Electronegativity / f / A substance that is polar could also be described as…
7[7] / Covalent / g / A substance that is nonpolar could also be described as…
8[8] / Ionic / h / This term describes an element’s tendency to attract an electron
9[9] / Hydrogen / i / The neutral parts of an atom
10[10] / Adhesion / j / This is used to slow changes in pH in a solution
11[11] / Cohesion / k / The negatively charged parts of an atom
12[12] / Hydrophilic / l / This type of bond is found in solid NaCl
13[13] / Hydrophobic / m / The positively charged parts of an atom
14[14] / Amphipathic / n / A horizontal section on the Periodic Table.
15[15] / Acid / o / Minor component in solution
16[16] / Base / p / A solution that decreases the concentration of H+
17[17] / pH / q / Dissolves other substances
18[18] / Buffer / r / Term used to describe water’s ability to stick to other objects
19[19] / SI / s / A group of bonded atoms
20[20] / Molecule / t / A solution that increases the concentration of H+
21[21] / Solute / u / A vertical section on the periodic table
22[22] / Solvent / v / This type of bond is found between atoms in an H2O molecule
2. Compare and contrast the different types of bonds: Hydrogen, Ionic, and Covalent
Suggestion: use a venn diagram
3. Compare and contrast the two types of covalent bonds
Suggestion: use a venn diagram
4. Define electronegativity and describe its pattern on the periodic table.
5. Label the pH scale below
6. Determine whether the following solutions are acidic or basic:
- pH = 10 ______
- pH = 7.6______
- pH = 1 ______
- pH = 4.57 ______
7. pH changes[23]
- If pH increases, what happens to the [H+] and [OH-] concentrations?[24]
- If pH decreases, what happens to the [H+] and [OH-] concentrations?[25]
8. Cellular function[26]
- Name four cellular functions necessary for life
- Explain why these are necessary for life
- Describe the structures responsible for this process
9. Draw valence electron diagrams for fluorine and selenium
10. Draw the lewis structure for NaI
11. Draw the lewis structure for NH3
12. Draw a molecule of NaI dissolved in water, indicate the hydrogen bonding.
13. Describe Pasteur's experiment.
14. Practicing pH related math.
- Find the pH of milk whose concentration of hydrogen ions, [H+] = 4 x 10-7 moles/liter.[27]
- Find the concentration of hydrogen ions, [H+], for vinegar with a pH = 3.1.[28]
- Calculate the pOH of a solution with 1 x 10-12 [-OH][29].
- pH + pOH = _____.[30]
- [H+] + [-OH] = ______.[31]
[1]M
[2]I
[3]K
[4]N
[5]U
[6]H
[7]V
[8]L
[9]B
[10]R
[11]C
[12]F
[13]G
[14]E
[15]T
[16]P
[17]D
[18]J
[19]A
[20]S
[21]O
[22]Q
[23]
[24]pH increase, OH increases
[25]pH decreases H+ increases
[26]RICEE: replication, information, communication, energy, equilibrium
[27]Using pH = −log[H+]:
pH = −log(4 x 10-7)
pH ≈ −(−6.4)
pH ≈ 6.4
[28]Using pH = −log[H+]:
3.1 = −log[H+]
Multiplying each side by −1:
−3.1 = log[H+]
Raising both sides to power of 10:
10−3.1 = [H+]
[H+] ≈ 7.94 x 10-4 moles/liter
[29]pOH=−log(1×10−12)=12.0
[30]14
[31]1*10 -14