5 Written questions
5 Matching questions
- What are functional groups? Names?
- Does form impact function?
- What are primary producers?
- Draw functional group structure and give molecular formula for: Carbonyl.
- What scale is pH?
- a Small organic molecules with great effects:
Hydroxyl, Carbonyl, Carboxyl, Amino, Sulfhydryl, Phosphate, and Methyl
- b Fix C from atmospheric CO₂ (ex: Plants w/ photosynthesis)
- c A log scale. Each change is 10 times. So when we go up or down, we add a zero to the end.
- d YES!
- e Carbonyl (>CO) (ketones, aldehydes, sugars); C double bonded to O
Ex: Acetone, the simplest ketone
5 Multiple choice questions
(see p. 1 slide 4 in ch. 3)
- Ex: pH = 12, What is the molar concentration of H⁺? OH⁻? H⁺ is 1 x 10⁻¹², OH⁻ is 1 x 10⁻².
- Acids raise the concentration of H⁺ ions in an aqueous solution (decreases the pH number)
Bases lower the concentration of H⁺ ions (increases the pH number)
- Cohesion and Adhesion.
Cohesion - waters ability to stick to ITSELF (other water molecules)
Adhesion - waters ability to stick to OTHER THINGS that are POLAR
- Amino (-NH₂) (acts as a base, amino acids); N single bonded to 2 H's
5 True/False questions
Draw functional group structure and give molecular formula for: Carboxyl.
Example? → Carboxyl (-COOH) acidic properties, components of many biologically important molecules; C double bonded to O and single to OH
Ex: Formic acid or acetic acid
What is a hydrocarbon? Polar or non-polar? → pH is the measurement used to quantify the H⁺ ion concentration in an aqueous (water) solution
Why is water in the solid phase less dense? How does this support life? → Hydrogen bonds keep the molecules spread out, so they don't pack together, making them less dense.
The floating ice insulates the body of water underneath it; if ice sank, then all the bodies of water would freeze solid, making life unlivable.
Describe how and why hydrogen bonds form in water. → Hydrogen bonds are the bonds between two polar molecules - one with a partial positive charge and one with a partial negative charge; water is perfect for this because it has the partial negative of Oxygen and the partial positive of Hydrogen.
How does waters specific heat compare to other solvents specific heat? What properties does it have that allows this? What affect does this have on the climate? → Waters specific heat is much higher that that of other solvents; this is because of hydrogen bonding; this keeps temperatures of places near/on bodies of water consistent