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AP Bio > Chemical Context of Life > Flashcards

Chemical Context of Life Flashcards

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AP® Biology flashcards Biology 101 flashcards
1
Q

Atom

A

basic unit of matter; made of smaller subatomic particles

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2
Q

Subatomic particles that make up an atom

A

Protons, neutrons, electrons

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3
Q

What makes up an atom?

A

Nucleus, electrons, protons, neutrons, empty space, electron shells, valence shell, electron cloud

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4
Q

Proton

A

Positively charged particles

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5
Q

Neutron

A

Particles with no charge

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6
Q

What makes up the nucleus of an atom

A

Protons and neutrons

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7
Q

What is the charge of an atom (USUALLY)

A

neutral

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8
Q

Strong nuclear force

A

force that holds the protons and neutrons in the nucleus of an atom together

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9
Q

What takes up 99% of the mass of an atom?

A

nucleus

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10
Q

Where is the nucleus of an atom located?

A

center of an atom

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11
Q

How do you measure the mass of the nucleus of an atom?

A

With atomic mass units (A.M.U) or daltons

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12
Q

One proton is equal to…

A

1 AMU (or dalton)

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13
Q

Electron

A

Negatively charged particle with 1/1840 mass of a proton. Electrons are in constant motion in the space surrounding the nucleus because they are attracted to the positive charge of the protons but do not bond with them because of their fast motion.

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14
Q

There are ____ amount of protons and neutrons in the nucleus of an atom.

A

an equal (usually)

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15
Q

What is the charge of an (most) atom?

A

Neutral because they have an even amount of electrons and protons.

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16
Q

Electron Cloud

A

the space in which the electrons revolve around the nucleus

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17
Q

Valence Shell

A

Outermost shell of an atom; contains valence electrons

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18
Q

Electron shell vs Electron Cloud

A

Electron Shell - used to visualize where electrons are, and how many are on each level
Electron Clod - describes location and energy of electrons

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19
Q

Element

A

pure substance that consists entirely of one type of atom that cannot be broken down by simple chemical means

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20
Q

More than ___ elements are known but only about ____ are commonly found in living organisms

A

100; 24

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21
Q

How are elements written?

A

One or two letter symbols (Na, H)

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22
Q

Atomic Number

A

amount of protons in the nucleus; written bottom left

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23
Q

Isotope

A

Elements with differing amounts of neutrons (Carbon-6, Carbon-7,etc.)
(Elements can be isotopes of one another)

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24
Q

Mass number

A

total amount of protons and neutrons (written top left)

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25
Q

How are isotopes identified?

A

by their mass number

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26
Q

Atomic mass

A

Average mass of all of the isotopes of a given element

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27
Q

96% of living matter is made of __ elements:

A

4; nitrogen, oxygen, carbon, and hydrogen

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28
Q

Radioactive Isotope

A

Isotopes that have a radioactive nuclei, which decays spontaneously because they have a very different amount of neutrons from the original amount which can lead to a change in the number of protons and subsequently the identity

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29
Q

Uses of radioactive isotopes

A

Can be dangerous, but also used to treat cancer, determine the age of rocks and fossils, kill bacteria, etc.

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30
Q

Compound

A

a substance formed by the chemical combination of two or more elements, in the same (never changes) proportions (can be ionic bonded or covalently bonded)

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31
Q

Chemical Formula

A

shows the composition of compounds (H20, NaCl)

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32
Q

Chemical Bonds

A

bonds that hold the atoms in molecules/elements together. Formed with the valence electrons

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33
Q

Main types of Chemical Bonds

A

Ionic bonds and covalent bonds

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34
Q

Ionic Bonds

A

formed when one or more electrons are transferred from one atom to another.
(because one atom has too many valence electrons and needs to give away to get 8 –> gives to atom with less than 8 valence electrons)

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35
Q

Covalent Bonds

A

formed when electrons are shared by atoms.
(because both electrons need 8 valence electrons but not give any away)

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36
Q

Ion

A

positively or negatively charged atoms

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37
Q

molecule

A

the smallest unit of most compounds; formed when atoms COVALENTLY bond

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38
Q

Van der Waals Forces

A

When atoms covalently bond to form molecules there is sometimes a charge that forms, (positive or negative) because one atom might have a stronger pull on the electrons being shared than the other atom. This causes molecules to be attracted to one another (if one positive and other negative). This INTERMOLECULAR force is extremely weak.

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39
Q

Octet Rule

A

Atoms always want an outer layer of 8 valence atoms (reason for bonds)

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40
Q

Single Bond

A

2 shared electrons

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41
Q

Double Bond

A

4 shared electrons

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42
Q

Triple bond

A

6 shared electrons

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43
Q

Important Chemical Formulas

A

Glucose; Water

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44
Q

Water

A

H20

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45
Q

Glucose

A

C6H1206

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46
Q

Electronegativity

A

The relative ability of an atom IN A BOND to attract electrons to itself

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47
Q

Trace Elements

A

elements that are required by an organism in small quantities

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48
Q

Examples of trace elements

A

Fe, I, Cu

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49
Q

Electron Affinity

A

the energy change associated with adding an electron to a gaseous atom.

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50
Q

Matter

A

anything with mass/ takes up space

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51
Q

How many elements exist in nature

A

92

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52
Q

How can compounds be bonded

A

ionically or covalently

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53
Q

Essential Elements

A

elements that an organism needs to healthily live + reproduce

54
Q

What are the essential elements

A

CHON

55
Q

The essential elements are the same for all organisms
True or False

A

False

56
Q

Why is too much of a trace element bad for an orgnism

A

it can be toxic for them

57
Q

Mass of proton

A

1.7 x 10^-24g

58
Q

Mass of neutron

A

1.7 x 10^-24g

59
Q

Mass of electron

A

1/1840 mass of a proton

60
Q

Matter

A

anything that has mass or takes up space

61
Q

Atom

A

smallest unit of matter which consists of subatomic particles

62
Q

What subatomic particle identifies the identity of an element

A

protons

63
Q

Which subatomic particle determines the reactivity (chemical behavior) of an element

A

electrons

64
Q

The amount of protons usually = the amount of what

A

electrons

65
Q

Does the nucleus have a charge

A

yes positive

66
Q

What are the essential elements

A

C H O N

67
Q

Isotopes

A

different number of neutrons in the same element

68
Q

What happens to energy when a radioactive isotope spontaneously decays

A

energy is released

69
Q

Why do radioactive isotopes spontaneously decay

A

because of the large difference between the number of protons and neutrons

70
Q

Subatomic particles

A

the things that make up an atom

71
Q

Common uses of radioactive isotopes in biology

A

1) Radioactive Tracers
2) Radiometric Dating

72
Q

Radioactive Tracers

A

put into “biologically active molecules” and used to track atoms which allow the tracers to be analyzed with imaging instruments when the atoms with tracers one secreted or still in body

73
Q

What is the bad side of radioactive tracers

A

too much radioactivity can damage cells

74
Q

Does hydrogen have neutrons

A

no

75
Q

Radiometric Dating

A

finding the exact date that fossils were alive (good for evolution) with half life

76
Q

Half Life

A

the time it takes for 50% of the parent isotope to decay into the daughter isotope; not affected by ANYTHING

77
Q

Radiometric Dating

A

using half life to mathematically calculate how many years have gone by

78
Q

Energy

A

the capacity to cause change (objects always want to have less energy because that is more stable)

79
Q

Potential Energy

A

energy that matter possesses because of its location OR structure

80
Q

Do all electrons on af atom have the same potetntial energy? explain

A

no the ones nearer have more (DISTANCE AKA LOCATION)

81
Q

Cocentric

A

word to describe how the distance between the shells of an atom increase when there’s more

82
Q

Inert

A

the non reactive noble gasses

83
Q

Formula for how many electrons can fit in a shell

A

2n^2
where n = # of level

84
Q

Electron shell

A

shells are js predictions of energy levels in 2D -> the ayr actually made of 3D orbitals which are diff shapes and sizes and determine where e- are found

85
Q

Different orbital names

A

s p d f

86
Q

What is the chance that you will find an electron in an orbital

A

90%

87
Q

How many orbitals can occupy an orbital at one time

A

2

88
Q

Which electron shell has the highest amount of potential energy and why

A

the first one because u have to absroeb energy to move up a level to overcome the attraction to the positive nucleus

89
Q

Chemical bonds

A

attractions that hold atoms together

90
Q

What is the strongest chemical bond

A

covalent

91
Q

Covalent bond

A

sharing ve- between 2 atoms to make a MOLECULE

92
Q

How are covalet bonds drawn

A

Lewis Dot Structures or Structural Formulas

93
Q

Valence

A

bonding capacity of an element in a covalent bond (how many electrons an element can share)

94
Q

Electronegativity

A

the pull of an atom on electrons

95
Q

What is electronegativity caused by

A

the amount of ve-, the atomic radius

96
Q

Atomic radius

A

how far the positively charged nucleus is from the negatively charged valence shell

97
Q

What are the 2 types of covalent bonds

A

nonpolar and polar

98
Q

Nonpolar covalent

A

no partial charges (both elements have equal pull) -> made when 2 elements are the same or between C and H or S and H

99
Q

Polar Covalent

A

there are partial charges (elements have diff pull; one is more EN) –> made between diff elements except C and H or S and H

100
Q

Ionic bond

A

bond bc element takes ve- away from other element bc of high EN difference

101
Q

What do ionic bonds creates

A

ions

102
Q

What are the different types of ions

A

cations(+) and anions(-)

103
Q

The compounds formed by ionic bonds are called what

A

ionic compounds or salts

104
Q

What shape do ionic compounds make

A

crystal lattice

105
Q

Ionic bonds are made between what types of elements

A

nonmetal and metal

106
Q

Why are covalent bonds stronger than ionic bonds

A

IN BIOLOGY!!!!! this is bc basically all of bio is in aqueous solutions and ionic compounds dissociate in aqueous solutions and its harder for molecules to break up in water

107
Q

What are the strong chemical bonds

A

ionic and covalent

108
Q

What are the weak chemical bond s

A

hydrogen bonds
wan der waals forces

109
Q

Hydrogen bonds

A

when H forms a covalent bond with N O or F and creates a dipole

110
Q

Why are H bonds formed

A

bc N O and F are all highly electronegative and H gains a positive partial charge which allows it to be attracted to another highly En element

111
Q

Van der Waals forces

A

weak bonds that occur when atoms and molecules are close together and they form bonds because of regions of brief positive and negative charges

112
Q

When are van der waals forces strong

A

when theres alot of them

113
Q

Van der Waals forces aka

A

London dispersion forces

114
Q

Why is molecular shape important

A

bc the molecular geometries are important because it determines how biological molecules recognize each other and interact

115
Q

Chemical Reactions

A

breaking/forming of bonds which leads to a change in the composition of matter

116
Q

Why is the number of reactants important

A

bc the # needs to be balanced for an equation to be true and its important to know the mole ratio to determine the amt of products

117
Q

Reversible Reaction

A

reactions that are true when products -> reactions and the other way around

118
Q

Chemical Equilibrium

A

in a reversible reaction, the point when both reactions are occurring at the same rate and the concentrations of everything are relatively the same (particular ratio)

118
Q

Reversible reaction symbol

A

⇌

119
Q

Molecules are made by what type(s) of bond

A

covalent

120
Q

Compounds are made by what type(s) of bond

A

ionic or covalent

121
Q

Compound

A

2 diff or same atoms in a fixed ratio

122
Q

Diatomic molecules are not compounds true or false

A

false

123
Q

molecules ____ (are/not always) compounds, compounds (are/not always) _____

A

are; not always

124
Q

Column on periodic table is called

A

l is vertical
groups or families

125
Q

Row on periodic table is called

A

period

126
Q

families are together why

A

similar reactivity bc same ve-

127
Q

peiods are together why

A

same amt of shells

128
Q

periodic table is organized by

A

increasing atomic number

129
Q

Vitalism vs Mechanism

A

the idea that before the 1900s people thought that physical sciences (chem + physics) could not equal science of the body because life was special but after the Urey Miller experiment, people have realized that the body obeys the same rules as chem and physics

AP Bio (66 decks)

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