Water

Question 1

High melting point, boiling point, and heat of vaporization

Answer 1

Special characteristics of water

Question 2

H-O-H tetrahedral bond angle is what?

Answer 2

104.5 degrees

Question 3

The result of the unequal electron sharing in water

Answer 3

A polar molecule

Question 4

A bond between an oxygen atom of one water molecule and the hydrogen bond of another. Hydrogen can bond with FON

Answer 4

Hydrogen bond

Question 5

Why are hydrogen bonds responsible for the high melting point of water?

Answer 5

So much thermal energy is required to break a large enough portion of hydrogen bonds to cause the crystal lattice of ice to melt.

Question 6

Strong hydrogen bonds are is which, a straight line or an L shape

Answer 6

A straight line

Question 7

Compounds that dissolve easily in water

Answer 7

Hydrophilic

Question 8

Compounds that are not easily dissolved in water

Answer 8

Hydrophobic

Question 9

Why is there an increase in entropy when a salt is dissolved in water?

Answer 9

Ions of the salt separate which provides a lot more freedom of motion compared to ions in a lattice. The freedom creates disorder which increases entropy

Question 10

Does dissolving hydrophobic compounds increase or decrease entropy of water

Answer 10

Decreases entropy because water molecules are forced to become a ‘cage’ around non-polar molecules. Creates less disorder

Question 11

Compounds that contain regions of polar and non-polar

Answer 11

Amphipathic

Question 12

Stable structures of amphipathic compounds in water.

Answer 12

Micelles

Question 13

Forces that hold non-polar regions of molecules together. Due to the system minimizing the number of water molecules that interact with the non-polar compound, NOT attraction between non-polar regions

Answer 13

Hydrophobic interactions

Question 14

When two uncharged atoms are close together and their electron clouds influence each other. Brings the two nuclei close together

Answer 14

van der Waals interactions

Question 15

Vapor pressure, boiling point, melting point, osmotic pressure. Comes from the fact that the concentration of water is lower in solutions than in pure water

Answer 15

Colligative properties

Question 16

Water moves from a region of _ concentration to _ concentration

Answer 16

High concentration to low concentration

Question 17

Water movement across a semipermeable membrane driven by differences in osmotic pressure

Answer 17

Osmosis

Question 18

Solutions of osmolarity equal to that of a cell’s cytosol

Answer 18

Isotonic

Question 19

Solutions with higher osmolarity than that of the cytosol. Water moves out of the cell

Answer 19

Hypertonic

Question 20

Solution with lower osmolarity than the cytosol. Water moves into the cell

Answer 20

Hypotonic

Question 21

When a cell bursts because of too much water pressure

Answer 21

Osmotic lysis

Question 22

When blood plasma pH falls below 7.4

Answer 22

Acidosis

Question 23

When blood plasma gets higher than 7.4

Answer 23

Alkalosis

Question 24

Aqueous solutions that resist change in pH when small amounts of acid or base are added

Answer 24

Buffers

Question 25

Flat zone where a given amount of acid or base added to the system has much less effect on pH than the same amount added outside of that zone

Answer 25

Buffering region

Question 26

Reaction where elements of water are eliminated

Answer 26

Condensation reaction

Question 27

Reaction when elements of water are added

Answer 27

Hydrolysis reaction

Question 28

High specific heat of water is useful because

Answer 28

It allows water to act as a ‘heat buffer’ which keeps an organism’s temperature constant despite surrounding heat fluctuations

Question 29

Ice being less dense than liquid water is important because

Answer 29

It keeps large frozen bodies of water from sinking to the bottom, killing all organisms beneath it