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Biology > Chemistry of Life > Flashcards

Chemistry of Life Flashcards

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AP® Biology flashcards Biology 101 flashcards
1
Q

Ability to do work

A

Energy

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2
Q

Pure substance and cannot be broken down by chemical means

A

Element

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3
Q

Smallest unit of an element

A

Atom

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4
Q

The number of protons in an atom’s nucleus

A

Atomic number

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5
Q

Number of protons and neutrons in the nucleus

A

Mass number

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6
Q

Atoms of the same element that have different numbers of neutrons but same numbers of protons and electrons

A

Isotope

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7
Q

The average mass of all isotopes of an element

A

Atomic weight

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8
Q

Any of the different forms of the same element and distinguished by the number of neutrons in the nucleus

A

Isotope

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9
Q

Positively charged particle (nucleus)

A

Proton

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10
Q

Has no charge (nucleus)

A

Neutron

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11
Q

Negatively charged and surrounding the nucleus

A

Electron

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12
Q

Mass of electron

A

0

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13
Q

Mass of proton

A

1

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14
Q

Mass of neutron

A

1

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15
Q

Charge of proton

A

+

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16
Q

Charge of electron

A

-

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17
Q

Charge of neutron

A

None

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18
Q

Which of the elements do organisms require in the largest amounts? What are these elements called?

A

C, H, O, N

Bulk elements

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19
Q

Where in an atom are protons, neutrons, and electrons located?

A

Proton and Neutron : NUCLEUS

Electron : SURROUNDS THE NUCLEUS

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20
Q

What does an element’s atomic number indicate?

A

Number of protons in the nucles

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21
Q

What is the relationship between an atom’s mass number and an element’s atomic weight?

A

Mass number - Atomic number = Number of neutron

–> neutron and proton have the same mass

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22
Q

How are the isotopes of an element different from one another?

A

Same number of protons but have different numbers of neutrons

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23
Q

Used to determine the most likely location for an electron relative to its nucleus.

A

Orbitals

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24
Q

How many electrons can each orbital hold?

A

2 electrons

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25
Q

It is a mathematical functions that describes the wave nature of electrons (or electron pairs) in an atom.

A

Orbitals

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26
Q

True or False: The less electrons in an atom, the less orbitals they occupy.

A

True

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27
Q

True or False: The more electrons in an atom, the less orbitals they occupu.

A

False.

The more electrons in an atom, the more orbitals they occupy.

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28
Q

Outermost occupied energy shell.

A

Valence Shell

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29
Q

True or False: Atoms are most stable when their valence electrons are less.

A

False.

atoms are most stable when their valence electrons are full.

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30
Q

Measures the atom’s ability to attract electrons on scale of 0 to 4.

A

Electronegativity of an atom

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31
Q

Attractive force that holds atoms together.

A

Chemical bond.

32
Q

Bonds that are strong but easily breaks in water.

A

Ionic Bonds

33
Q

Bond that are strong where 2 or more atoms share electrons

A

Covalent Bonds

34
Q

Bonds where 1 atom donates 1 or more atom forming oppositly charged ions.

A

Ionic Bonds

35
Q

Bonds where outermost shell is almost empty.

A

Ionic Bonds

36
Q

Bonds that are weak and has an atom with partially negative charge attract atom with partially positive charge.

A

Hydrogen Bonds

37
Q

Bonds where the partial positive charge is always hydrogen.

A

Hydrogen Bonds

38
Q

Bonds that are lopsided union in which 1 nucleus exerts much stronger pull on the shared electrons which is critical to biology.

A

PolarCovalent Bonds

39
Q

The tendency of water molecules to stick together.

A

Cohesion

40
Q

The tendency to form hydrogen bonds with substance other than water.

A

Adhesion

41
Q

Liquid where solute is to be dissolved.

A

Solvent

42
Q

About to dissolve.

A

Solute

43
Q

Consists of 1 or more solutes dissolved in solvent.

A

Solution

44
Q

NaCl (salt)
A. Solute
B. Solution
C. Solvent

A

A. Solute

45
Q

Water
A. Solute
B. Solution
C. Solvent

A

C. Solvent

46
Q

“water-loving”

A

Hydrophilic

47
Q

Readily dissolved in water

A

Hydrophilic

48
Q

“water-fearing”

A

Hydrophobic

49
Q

Do not dissolve or form hydrogen bonds with water

A

Hydrophobic

50
Q

2 or more molecules swap atoms to yield different molecules.

A

Chemical Reaction

51
Q

Starting materials

left of chemical reaction

A

Reactants

52
Q

Results of the reaction

right of chemical reaction

A

Products

53
Q

Contains as much H+ as much as it does OH-

pH = 7

A

Neutral Solution

54
Q

Chemical that adds H+ to a solution making the concentration of H= ions exceed the concentration of OH- ions

A

Acid

55
Q

Has a pH lower than 7

A

Acid

56
Q

Opposite of an acid

A

Base

57
Q

Concentration of H- ion exceed the concentration of H- ions

A

Base

58
Q

Has pH greater than 7

A

basic / Alkaline

59
Q

pH = 14
A. Strongly acidic
B. Extremely BAsic

A

B.Extremely Basic

60
Q

pH = 0
A. Strongly acidic
B. Extremely basic

A

A. Strongly acidic

61
Q

Pairs of weak acids and bases that neutralize changes in pH

A

Buffer Systems

62
Q

Made up of monomers linked together

A

Polymers

63
Q

What are the 4 main types of monomers?

A

sugars, amino acids, fatty acids, and nucleotides

64
Q

Is a molecule that can react together with other monomer molecules to form a larger polymer chain.

A

Monomers

65
Q

Process that joins monomers into polymers

A

Dehydration Synthesis

66
Q

Condensation Reaction

A

Dehydration Synthesis

67
Q

Process where enzyme removes an -OH from 1 molecule and a hydrogen atom from another

A

Dehydration Synthesis

68
Q

Process that breaks polymers into monomers

A

Hydrolysis

69
Q

Process that breaks covalent bonds that link monomers

A

Hydrolysis

70
Q

Process where enzymes use atoms from water to add -OH to 1 molecule and hydrogen atom to another

A

Hydrolysis

71
Q

Organic molecules that consists of carbon, hydrogen and oxygen often proportion is 1:2:1

A

Carbohydrates

72
Q

What is a carbohydrate consist of?

A

C, H, O

73
Q

usually contains 5 or 6 atoms

A

Monisaccharide

74
Q

“two sugars”

A

Disaccharide

75
Q

2 monosaccharide joined by dehydration synthesis

A

Disaccharide

Biology (2 decks)

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