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Bio 101 > Chapter 2 > Flashcards

Chapter 2 Flashcards

The Chemical Foundation of Life

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Biology 101 flashcards
1
Q

acid

A

molecule that donates hydrogen ions and increases the concentration of hydrogen ions in a solution

pH less than 7

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2
Q

adhesion

A

attraction between water molecules and other molecules

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3
Q

aliphatic hydrocarbon

A

hydrocarbon consisting of a linear/open chain of carbon atoms

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4
Q

anion

A

negative ion that is formed by an atom gaining one or more electrons

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5
Q

aromatic hydrocarbon

A

hydrocarbon consisting of closed rings of carbon atoms

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6
Q

Atom

A

the smallest unit of matter that retains all of the chemical properties of an element

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7
Q

Atomic mass

A

calculated mean of the mass number for an element’s isotopes

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8
Q

atomic number

A

total number of protons in an atom

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9
Q

balanced chemical equation

A

statement of a chemical reaction with the number of each type of atom equalized for both the products and reactants

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10
Q

Base

A

molecule that donates hydroxide (OH-) ions or otherwise binds excess hydrogen ions and decreases the hydrogen ions’ concentration in a solution

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11
Q

Buffer

A

substance that resists a change in pH by absorbing or releasing hydrogen (H+) or hydroxide (OH-) ions

Buffers do so by being composed of certain pairs of solutes: either a weak acid plus a salt derived from that weak acid or a weak base plus a salt of that weak base. For example, a buffer can be composed of dissolved acetic acid (HC 2H 3O 2, a weak acid) and sodium acetate (NaC 2H 3O 2, a salt derived from that acid).

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12
Q

Calorie

A

amount of heat required to change the temperature of one gram of water (H2O) by one degree Celsius

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13
Q

Capillary action

A

occurs because water molecules are
attracted to charges on the inner surfaces of narrow tubular structures such as glass tubes, drawing the water molecules to the tubes’ sides. The meniscus in the tube can be higher or lower than the meniscus of the container.

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14
Q

Cation

A

positive ion that is formed by an atom losing one or more electrons

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15
Q

Chemical bond

A

interaction between two or more of the same or different atoms that results in forming molecules

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16
Q

chemical reaction

A

process leading to rearranging atoms in molecules

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17
Q

chemical reactivity

A

the ability to combine and to
chemically bond with each other

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18
Q

cohesion

A

intermolecular forces between water molecules caused by the polar nature of water; responsible for surface tension

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19
Q

compound

A

substance composed of molecules consisting of atoms of at least two different elements

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20
Q

covalent bond

A

type of strong bond formed between two atoms of the same or different elements; forms when 2+ electrons are shared between atoms

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21
Q

dissociation

A

release of an ion from a molecule such that the original molecule now consists of an ion and the charged remains of the original, such as when water dissociates
into H+ and OH

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22
Q

Electrolyte

A

ion necessary for nerve impulse conduction, muscle contractions, and water balance

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23
Q

electron

A

negatively charged subatomic particle that resides outside the nucleus in the electron orbital; lacks functional mass and has a negative charge of -1 unit

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24
Q

electron configuration

A

arrangement of electrons in an atom’s electron shell

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25
Q

electron orbital

A

how electrons are spatially distributed
surrounding the nucleus; the area where we are most likely to find an electron

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26
Q

electron transfer

A

movement of electrons from one element
to another; important in creating ionic bonds

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27
Q

electronegativity

A

ability of some elements to attract electrons (often of hydrogen atoms), acquiring partial negative charges in molecules and creating partial positive charges on the hydrogen atoms

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28
Q

element

A

one of 118 unique substances that cannot break down into smaller substances; each element has unique properties and a specified number of protons

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29
Q

enantiomers

A

Also known as an optical isomer

molecules that share overall structure and bonding patterns, but differ in how the atoms are three dimensionally placed such that they are mirror images of each other

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30
Q

equilibrium

A

steady state of relative reactant and product concentration in reversible chemical reactions in a closed system

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31
Q

evaporation

A

change from liquid to gaseous state at a body of water’s surface, plant leaves, or an organism’s skin

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32
Q

functional group

A

group of atoms that provides or imparts a specific function to a carbon skeleton

Some of the important functional groups in biological molecules include: hydroxyl, methyl, carbonyl, carboxyl, amino, phosphate, and sulfhydryl groups. These groups play an important role in the formation of molecules like DNA, proteins, carbohydrates, and lipids.

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33
Q

geometric isomer

A

isomer with similar bonding patterns differing in the placement of atoms alongside a double covalent bond

Geometric isomers are two or more compounds with the same number and types of atoms, and bonds, but which have different geometries for the atoms.

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34
Q

heat of vaporization of water

A

high amount of energy required for liquid water to turn into water vapor

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35
Q

hydrocarbon

A

molecule that consists only of carbon and hydrogen

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36
Q

hydrogen bond

A

weak bond between slightly positively charged hydrogen atoms and slightly negatively charged atoms in other molecules

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37
Q

hydrophilic

A

describes ions or polar molecules that interact well with other polar molecules such as water

38
Q

hydrophobic

A

describes uncharged nonpolar molecules that do not interact well with polar molecules such as water

39
Q

inert gas

A

(also, noble gas) element with filled outer electron shell that is unreactive with other atoms. They include helium, argon, neon, xenon, krypton, radon, and Oganesson (118: last element)

40
Q

ion

A

atom or chemical group that does not contain equal numbers of protons and electrons. Has a positive or negative charge

41
Q

ionic bond

A

chemical bond that forms between ions with opposite charges (cations and anions)

42
Q

irreversible chemical reaction

A

chemical reaction where reactants proceed unidirectionally to form products

43
Q

isomers

A

molecules that differ from one another even though they share the same chemical formula

44
Q

isotope

A

one or more forms of an element that have different numbers of neutrons

45
Q

law of mass action

A

chemical law stating that the rate of a reaction is proportional to the concentration of the reacting substances

46
Q

Litmus paper

A

(also, pH paper) filter paper treated with a natural water-soluble dye that changes its color as the pH of the environment changes in order to use it as a pH indicator

47
Q

mass number

A

total number of protons and neutrons in an atom

48
Q

Matter

A

anything that has mass and occupies space

49
Q

Molecule

A

2 or more atoms chemically bonded

50
Q

Neutron

A

uncharged particle that resides in an atom’s nucleus; has a mass of 1 amu

51
Q

Nonpolar covalent bond

A

bond type of covalent bond that forms between atoms when 2+ electrons are shared equally between them

52
Q

nucleus

A

core of an atom; contains protons and neutrons

53
Q

octet rule

A

rule that atoms are most stable when they hold eight electrons in their outermost shells

54
Q

orbital

A

region surrounding the nucleus; contains electrons

55
Q

organic molecule

A

any molecule containing carbon (except carbon dioxide)

56
Q

periodic table

A

organizational chart of elements indicating each element’s atomic number and atomic mass; provides key information about the elements’ properties

57
Q

pH scale

A

scale ranging from zero to 14 that is inversely proportional to the hydrogen ions’ concentration in a solution

58
Q

polar covalent bond

A

type of covalent bond that forms as a result of unequal electron sharing, resulting in creating slightly positive and negative charged molecule regions

59
Q

product

A

molecule that is result of chemical reaction

60
Q

proton

A

positively charged particle that resides in the atom’s nucleus; has a mass of one amu and a charge of +1

61
Q

radioisotope

A

isotope that emits radiation comprised of subatomic particles to form more stable elements

62
Q

reactant

A

molecule that takes part in a chemical reaction

63
Q

reversible chemical reaction

A

chemical reaction that functions bidirectionally, where products may turn into reactants if their concentration is great enough

64
Q

solvent

A

substance capable of dissolving another substance

65
Q

specific heat capacity

A

the amount of heat one gram of a
substance must absorb or lose to change its temperature by one degree Celsius

66
Q

sphere of hydration

A

when a polar water molecule surrounds charged or polar molecules thus keeping them dissolved and in solution

67
Q

structural isomers

A

molecules that share a chemical formula but differ in the placement of their chemical bonds

68
Q

substituted hydrocarbon

A

hydrocarbon chain or ring containing an atom of another element in place of one of the backbone carbons

69
Q

surface tension

A

tension at the surface of a body of liquid that prevents the molecules from separating; created by the attractive cohesive forces between the liquid’s molecules

70
Q

Valence shell

A

outermost shell of an atom

71
Q

van der Waals interaction

A

very weak interaction between molecules due to temporary charges attracting atoms that are very close together

72
Q

How many neutrons do carbon-12 and carbon-13 have, respectively?

A

Carbon occurs naturally in three isotopes: carbon 12, which has 6 neutrons (plus 6 protons equals 12), carbon 13, which has 7 neutrons and carbon 14, which has 8 neutrons.

73
Q

how many electrons do elements in group 1 need to lose in order to achieve a stable electron configuration?

How many electrons do elements in groups 14 and 17 need to gain to achieve a stable configuration?

A

Elements in group 1 need to lose one electron to achieve a stable electron configuration. Elements in groups 14 need to gain 4 electrons. Elements in groups 17 1 electron.

The group 1 elements, that is, sodium, hydrogen, and lithium, all possess 1 electron in their outermost shells. This signifies that they can attain a stable configuration and an occupied outer shell by sharing or donating one electron with another molecule or atom like water.

The elements of group 14 possess 4 electrons in their outermost shell permitting them to form many covalent bonds with other atoms by gaining 4 electrons.

On the other hand, the elements of group 17 exhibit 7 electrons in their outermost shells, thus they seem to fill this shell by gaining 1 electron from other molecules or atoms, making them negatively charged ions.

74
Q

cis-trans isomers

A

must be double bonded

75
Q

enantiomers

A

a molecule must have at least four different atoms or groups connected to a central carbon.

76
Q

If xenon has an atomic number of 54 and a mass number of 108, how many neutrons does it have?

A

54

77
Q

Atoms that vary in the number of neutrons found in their nuclei are called

A

Isotope

78
Q

Potassium has an atomic number of 19. What is its electron configuration?

A

shells 1, 2 and 3 are full and shell 4 has one electron

79
Q

Which type of bond represents a weak chemical bond?

A

hydrogen bond

80
Q

When acids are added to a solution, the pH should

A

decrease

81
Q

We call a molecule that binds up excess hydrogen ions in
a solution a(n)

A

base

82
Q

Each carbon molecule can bond with as many
as________ other atom(s) or molecule(s).

A

4

83
Q

Which of the following is not a functional group that can bond with carbon?

A

sodium cannot bond with carbon

84
Q

What property of carbon makes it essential for organic
life?

A

Growth and replication

85
Q

Compare and contrast saturated and unsaturated triglycerides.

A

Saturated triglycerides contain single bonds and are solid at room temperature, while unsaturated triglycerides contain double bonds and are liquid at room temperature.

86
Q

Which statement describes how buffers help prevent drastic swings in pH?

A

Buffers absorb excess hydrogen and hydroxide ions to prevent increases or decreases in pH. An example is the bicarbonate system in the human body.

87
Q

Why are hydrogen bonds and van der Waals interactions necessary for cells?

A

Hydrogen bonds and van der Waals interactions form weak associations between different molecules. They provide the structure and shape necessary for proteins and DNA within cells so that they function properly. Hydrogen bonds also give water its unique properties, which are necessary for life.

88
Q

What makes ionic bonds different from covalent bonds?

A

ionic bonds are created between ions. The electrons are not shared between the atoms, but rather are associated more with one ion than the other. Ionic bonds are strong bonds, but weaker than covalent bonds, meaning it takes less energy to break a ionic bond compared with a covalent bond

89
Q

How many orbitals does each shell have?

A
90
Q

How many electrons can each shell hold?

A

Bio 101 (9 decks)

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