BIO-110 FA5 Study Guide - Midterm Guide: Adenine, Cell Theory, Cholesterol

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13 Apr 2017

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Lecture 1 and 2: intro to cells and chem of life. Simple chemical compounds bind to form carbon containing substances. Water: universal solvent, uses cohesion to stick to other water molecules, adhesion to stick to other substances, water is very polar, dissolves other polar molecules. Carbon: versatile because it can form many covalent bonds. Strength of bonds: covalent, ionic, hydrogen, van der waals. Structure of proteins: non ionized form, ionized form. Four covalent bonds: hydrogen, carboxyl, amino group, r side chain. Bond through peptide bonds: polypeptide chains, link together to create protein through hydrogen bonds. Secondary structure: specialized due to h bonds. Proteins catalysts: enzymes work by lowering activation rate of reaction. Nucleotides: made of phosphate groups, five carbon sugar, nitrogenous bases (purine, pyrimidine) Purines are bigger (two rings), pyrimidines are smaller (one ring: a t 2 bonds, c g 3 bonds, purine- adenine, guanine, pyrimidine cytosine, thymine, uracil. Total # purines is equal to the total # of pyrimidines.

Related Questions

The type of macromolecule found in highest concentration on a weight basis in a HeLa cell is

protein.

lipid.

polysaccharide.

nucleic acid.

water

Co and Zn ions are required by humans in

microgram amounts.

gram or near gram amounts.

kilogram amounts.

d. milligram amounts.

Which description best characterizes the length of a hydrogen bond between water molecules?

About the same length as the calculated van der Waals distance for two water molecules.

About the same length as a covalent O----H bond.

Shorter than a covalent O---H bond.

Longer than a covalent O---H bond, but shorter than the calculated van der Waals distance between water molecules.

Which of the following statements about water is not true?

Water will hydrogen bond into highly ordered structures or "cages" around non-polar molecules.

The electron-rich oxygen atom of one water molecule can interact with an electron-poor hydrogen on another water molecule to form a hydrogen bond.

Water is a key player in the energetics of the hydrophobic effect.

In an ice crystal water molecules pack into open lattices consisting of five-membered oxygen rings.

At 25 degrees celsius liquid water is about 85% as hydrogen bonded as the water in ice, with each molecule in an average of 3.4 hydrogen bonds.

Which of the following is the strongest?

Ionic interactions

Permanent dipole - permanent dipole interactions

London dispersion forces

Co-linear hydrogen bonds

Which of the following is the best explanation for the hydrophobic effect?

It is caused by the attraction of hydrophobic groups for each other.

It is an entropic effect caused by the tendency of hydrophobic groups to increase their entropy by associating with other hydrophobic groups.

It is an entropic effect, caused by the tendency of water molecules to increase their entropy by excluding hydrophobic groups, which they must otherwise surround with highly ordered structures.

It is caused by the attraction of water for hydrophobic groups.

It is an entropic effect, caused by the tendency of water molecules to increase their entropy by forming highly ordered structures around the hydrophobic groups.

Which of the following is NOT defined as a buffer? (pKa PIPES-H⁺ = 6.76; pKa MOPS-H⁺ = 7.15; pKa HEPES-H⁺ = 7.47)

0.15 M MOPS, pH 6.50

0.05 M HEPES-H⁺ / 0.04 M HEPES

0.20 M PIPES, pH 7.97

0.01 M HEPES, pH 7.30

Nitrogen and phosphorus are in the same column of the periodic table. They have similar properties in bonding with other molecules because they have the same number of:

We cannot answer this question definitively because there is not enough information.

What I choose are wrong.

BIO-110 FA5 Study Guide - Midterm Guide: Adenine, Cell Theory, Cholesterol

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