Deck 2: An Introduction to the Chemical Basis of Life

Question 1

Which of the following elements is a bacterial micronutrient?

A) carbon
B) chlorine
C) hydrogen
D) nitrogen

Answer 1

B

Question 2

The chemical symbol for ________ is ________. (Select all that apply)

A) carbon; Ca
B) oxygen; O
C) potassium; K
D) magnesium; Mn

Answer 2

B,C

Question 3

Elements with similar chemical properties are organized in the same ________ of the periodic table.

A) row
B) quadrant
C) column
D) color block

Answer 3

C

Question 4

The atomic nucleus of an atom is composed of ________.

A) positively charged protons
B) positively protons and electrically neutral neutrons
C) electrically neutral neutrons and negatively charged electrons
D) electrically neutral protons

Question 5

Each proton and neutron have a mass of one atomic mass unit (amu). Using this information from the periodic table, determine the mass of sodium (Na).

A) 11 amu
B) 12 amu
C) 23 amu
D) 34 amu

Question 6

Isotopes of an element differ from each other by the ________.

A) number of neutrons they possess
B) number of valence shell electrons
C) arrangement of their electrons in orbitals
D) arrangement of their electrons in the atomic nucleus

Question 7

Radioisotopes of an element ________. (Select all that apply)

A) are highly reactive and preferentially participate in chemical reactions
B) emit energy
C) can be used in diagnostic procedures such as indium scans
D) have additional electrons in their valence shell

Question 8

Orbitals ________. (Select all that apply)

A) represent the volume of space where an atom's electrons are most likely to be found
B) are associated with different energy shells
C) contain a maximum of 8 electrons
D) may be spherical or pear-shaped

Question 9

Valence shell electrons ________. (Select all that apply)

A) are located exclusively in the s orbitals
B) participate in chemical reactions
C) have the highest associated energy
D) can be shared with the valence shell of an adjacent atom

Question 10

When an atom loses a valence shell electron, it ________. (Select all that apply)

A) becomes a cation
B) participates in polar covalent bonds
C) can become part of a polar molecule
D) can form an ionic bond with an anion

Question 11

When two adjacent atoms of similar electronegativity share a pair of electrons, ________. (Select all that apply)

A) it promotes the formation of hydrogen bonds with surrounding atoms
B) a strong polar covalent bond is formed
C) a strong nonpolar covalent bond is formed
D) van der Waals forces are generated

Question 12

When two adjacent atoms unequally share a pair of electrons, ________. (Select all that apply)

A) the resulting bond is highly unstable
B) a strong polar covalent bond is formed
C) a strong nonpolar covalent bond is formed
D) a polar molecule is formed

Question 13

Two adjacent nitrogen atoms share 3 pairs of electrons resulting in the formation of ________.

A) a nonpolar covalent bond
B) a triple nonpolar covalent bond
C) a combination of polar and nonpolar covalent bonds
D) a triple polar covalent bond

Question 14

When a pair of valence shell electrons are shared by two atoms with significantly different electronegativity values, ________.

A) a polar covalent bond forms
B) the electron pair of the bond is positioned closer to the atom with the lower electronegativity
C) an ionic bond forms
D) the electronegativity values of the two atoms equalize

Question 15

Weak electrostatic attraction between a hydrogen atom participating in a polar covalent bond and a slightly negative region of a molecule results in the formation of a(n) ________.

A) ionic bond
B) double covalent bond
C) van der Waals interaction
D) hydrogen bond

Question 16

In the chemical equation below, glucose is a(n) ________.

A) reactant
B) product
C) intermediate complex
D) equilabrator

Question 17

Chemical equilibrium describes ________.

A) a reaction that has run to completion
B) a reaction that has converted all reactant into product
C) a reaction that involves only one reactant and one product
D) a situation where the rate of the forward reaction is exactly equal to the rate of the reverse reaction

Question 18

Hydrogen bonds between water molecules in solid form ________. (Select all that apply)

A) make it less dense than its liquid form
B) allow it to serve as a layer of surface insulation to provide a thermally stable aquatic habitat in the winter
C) are very stable and space the molecules closer together
D) can convert to covalent bonds when ice melts

Question 19

Because of its extreme hydrogen bonding, water has a high specific heat so it ________. (Select all that apply)

A) heats up slowly
B) cools down slowly
C) maintains a thermally stable aquatic environment
D) requires the addition of a lot energy to break all of these weak intermolecular bonds

Question 20

Evaporation of sweat ________. (Select all that apply)

A) leads to cooling that is essential for maintaining a constant body temperature
B) is due to water's high specific heat
C) elevates the pH level of the skin
D) leaves elevated salt levels on the skin which serve to inhibit pathogen growth

Question 21

What unique feature of water is highlighted in this photo?

A) Water's ability to serve as an excellent solvent
B) Water's high specific heat
C) Water's high heat of vaporization
D) Water's cohesive nature

Question 22

Which of the following is FALSE?

A) Water is a polar molecule
B) Water exists in nature in all three physical states
C) Hydrogen bonds tend to form between water molecules
D) Solid water is (ice) is denser than liquid water

Question 23

A ________ is the substance used to dissolve materials.

A) solute
B) solvent
C) solution
D) hydration shell

Question 24

An aqueous solution ________. (Select all that apply)

A) uses water as a solvent
B) dissolves hydrophobic solutes
C) forms hydration shells around the solutes
D) is always characterized by a neutral pH

Question 25

The molecular weight of glucose is 181.18 g/mol. To make 250 ml of a 0.25 M glucose solution, you would dissolve ________ g of glucose in 250 ml of water.

A) 11.32
B) 18.11
C) 45.26
D) 181.18

Question 26

Acids ________. (Select all that apply)

A) accept hydrogen ions from a solution
B) increase the pH when a buffer is added
C) have a pH value below 7
D) turn phenol red fuchsia

Question 27

Acid rain is a serious environmental problem. A sample of rainwater collected in the Adirondack Mountains had an H⁺ concentration of 10^-4 mol/L. The pH of this sample was ________.

A) 0.0001
B) -4
C) 4
D) 10,000

Question 28

If the pH of a solution is increased from pH 5 to pH 7, it means that the concentration of H⁺ is ________ than it was at pH 5.

A) 2 times lower
B) 10 times greater
C) 100 times greater
D) 100 times lower

Question 29

To minimize the pH change when an acid or base is added to a solution, a ________ is needed.

A) ketone
B) pH indicator
C) isotope
D) buffer

Question 30

Which of the following represent ways to increase the molecular diversity of organic molecules? (Select all that apply)

A) varying the length of the carbon skeleton
B) the presence of multiple bonds in the carbon skeleton
C) branching of the carbon skeleton
D) substitution of functional groups for a hydrogen

Question 31

Which functional group acts as an acid by donating a hydrogen ion to the solution?

A) Ketone
B) Methyl
C) Carboxyl
D) Hydroxyl

Question 32

Identify this functional group.

A) aldehyde
B) thiol
C) carboxyl
D) hydroxyl

Question 33

How many covalent bonds can be formed by one carbon atom?

A) 1
B) 2
C) 4
D) 8

Question 34

Glucose and fructose represent ________ isomers. (Select all that apply)

A) structural
B) optical
C) enantiomer
D) radioactive

Question 35

The figure below illustrates ________ isomers. (Select all that apply)

A) structural
B) optical
C) enantiomer
D) radioactive

Question 36

What is the chemical mechanism by which cells degrade polymers into monomers?

A) Ionic monomer bonding
B) Dehydration synthesis
C) Hydrolysis
D) Polymerization

Question 37

What process does a cell use to recycle monomers?

A) Ionic monomer bonding
B) Dehydration synthesis
C) Hydrolysis
D) Polymerization