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BIL 150 > Ch. 2: The Chemical Context of Life > Flashcards

Ch. 2: The Chemical Context of Life Flashcards

1
Q

Matter

A

anything that has mass and takes up space

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2
Q

Pure Substance

A

elements and compounds

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3
Q

Element

A

cannot be broken down further (ex: H)

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4
Q

Compound

A

a substance composed of two or more elements; can be broken down further (ex: H2O)

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5
Q

Trace Elements

A

required in only minute (very small) quantities

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6
Q

Atom

A

smallest unit of matter that still retains the properties of an element

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7
Q

Which elements compose ~96% of living matter?

A

Oxygen (O), Carbon (C), Hydrogen (H), and Nitrogen (N)

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8
Q

Subatomic Particles

A

particles that compose atoms; protons, neutrons, electrons

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9
Q

Neutron

A

neutral charge

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10
Q

Proton

A

positive charge

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11
Q

Electron

A

negative charge

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12
Q

Atomic Nucleus

A

dense core where protons and neutrons are packed tightly; electrons surround an atom, forming a cloud

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13
Q

What is the atomic mass unit (amu)?

A

Dalton

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14
Q

Atomic Number

A

number of PROTONS in an element; tells the number of protons AND electrons in an element (because they balance each other out, so must be equal); ex: 2He means 2 protons in helium nucleus (Helium is second element on periodic table)

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15
Q

What does the atomic number dictate?

A

The location of an element on the periodic table (ex: Oxygen has an atomic number of 8, making it the 8th element on the periodic table)

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16
Q

Mass Number

A

total number of protons and neutrons in a nucleus

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17
Q

How do you find the number of neutrons?

A

Subtract the atomic number from the mass number (ex: 4/2 He, 4-2 = 2 neutrons)

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18
Q

Atomic Mass

A

total mass of an atom

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19
Q

What will all isotopes always have the same number of?

A

they will always have the same number of protons as the original element

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19
Q

Isotopes

A

different atomic forms of the SAME element

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20
Q

Radioactive Isotope

A

nucleus decays spontaneously, releasing particles and energy, which can serve as tracers to track atoms

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21
Q

Half-Life

A

“parent” isotope decays into its “daughter” isotope at a FIXED rate; the time it takes for 50% of the isotope to decay

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22
Q

How does potential energy vary with distance? (relating to electrons and nucleus)

A

the more distant an electron is from the nucleus, the greater potential energy there is

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23
Q

Electron Shells

A

each has a characteristic average distance to the nucleus; the first shell closest to the nucleus has the lowest potential energy

24
Q

How do electrons move between shells?

A

when an electron absorbs energy, it moves to a shell farther out from nucleus; when it loses energy, it moves to a shell closer to the nucleus

25
Q

How many electrons can the first shell hold?

A

No more than 2; the maximum is 2

26
Q

How many electrons can the second shell hold?

A

a maximum of 8

27
Q

Which shell is most responsible for the chemical behavior of an atom?

A

the outermost shell (valence shell) and the number of electrons it has

28
Q

Valence electrons

A

electrons on the outermost shell

29
Q

Valence shell

A

outermost electron shell

30
Q

What happens when an atom has a completed valence shell?

A

it is unreactive; inert

31
Q

Orbital

A

the 3-dimensional space where an electron is found 90% of the time; a component of electron shell

32
Q

How many electrons can occupy a single orbital?

A

no more than 2

33
Q

How many electrons can the four orbitals of the second shell hold?

A

8 electrons

34
Q

Chemical Bond

A

attraction that holds atoms together

35
Q

Covalent Bond

A

the sharing of a pair of valence electrons by two atoms

36
Q

Molecule

A

two or more atoms held together by covalent bonds

37
Q

Single Bond

A

one pair of shared electrons

38
Q

Double Bond

A

2 pairs of shared electrons

39
Q

Valence

A

bonding capacity; usually equal to the number of electrons required to complete the atom’s outermost (valence) shell

40
Q

What does valence generally determine?

A

how many covalent bonds that atom will form

41
Q

Electronegativity

A

the attraction of a particular atom for the electrons of a covalent bond; atoms attract shared bonding electrons to varying degrees

42
Q

How does electronegativity affect the pull of shared electrons?

A

The more electronegative an atom is, the more strongly it pulls shared electrons toward ITSELF; it wants to bring them closer

43
Q

Nonpolar Covalent Bond

A

a covalent bond between two atoms of the SAME element in which the electrons are shared EQUALLY since the atoms have the same electronegativity

44
Q

Polar Covalent Bond

A

when one atom is bonded to a more electronegative atom, so the electrons of the bond are not shared equally (they are pulled closer to the atom with greater electronegativity)

45
Q

Ions

A

atoms or molecules that have an electrical charge

46
Q

Cation

A

ion w/ positive charge

47
Q

Anion

A

ion w/ negative charge

48
Q

Ionic Bond

A

attraction between cations and anions; any two ions of opposite charge can form an ionic bond

49
Q

Ionic Compounds (Salts)

A

compounds formed by ionic bonds; they do not consist of molecules

50
Q

How does an ion become a cation?

A

loses an electron

51
Q

How does an ion become an anion?

A

gain an electron

52
Q

Hydrogen Bond

A

noncovalent attraction between a hydrogen atom and an electronegative atom

53
Q

van der Waals interactions

A

occur only when atoms and molecules are very close together, enables atoms and molecules to stick to each other; individually weak

54
Q

Reactant

A

starting material in a chemical reaction

55
Q

Product

A

resulting material in a chemical reaction

56
Q

What happens during chemical reactions?

A

matter is conserved; it cannot be destroyed or created, only electrons can be rearranged

57
Q

Chemical Equilibrium

A

the point at which the reactions offset one another EXACTLY

BIL 150 (3 decks)

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