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AP Bio > Ch.2 The Chemical Context of Life > Flashcards

Ch.2 The Chemical Context of Life Flashcards

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AP® Biology flashcards Biology 101 flashcards
1
Q

Atom

A

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

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2
Q

Subatomic particles

A

Tiny bits of matter composed of even smaller parts

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3
Q

Neutrons

A

Electrically neutral

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4
Q

Protons

A

Electrically positive charged

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5
Q

Electrons

A

Electrically negative charged

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6
Q

Atom nucleus

A

Where protons and neutrons are tightly packed in a dense core

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7
Q

Dalton

A

Measurement unit used to measure atoms (atomic mass unit)

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8
Q

Atomic number

A

Number of protons and electrons, written to left of the symbol of an element

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9
Q

Mass number

A

The sum of protons and neurons in the nucleus of an atom, written to the left of an element’a symbol

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10
Q

Atomic mass

A

Approx. the total mass of an atom

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11
Q

Isotopes

A

Different atomic forms of the same element, have more neutrons than other atoms of the same element

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12
Q

Radioactive isotope

A

One in which the nucleus decays spontaneously giving off particles and energy

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13
Q

Energy

A

The capacity to cause change, doing work

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14
Q

Potential energy

A

The energy that matter possess because of it’s location or structure

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15
Q

Element

A

A substance that cannot be broken down to other substances by chemical reactions

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16
Q

Compound

A

A substance consisting of two or more different elements combined in a fixed ratio

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17
Q

Emergent properties

A

Matter not possessed by it’s constituents

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18
Q

Essential elements

A

What organism need to live a healthy life and reproduce

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19
Q

Trace elements

A

Required elements by an organism in only minute quantities

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20
Q

Goiter

A

Iodine deficiency

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21
Q

Electron shells

A

Where electrons are located, the energy level

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22
Q

Valence electrons

A

The outermost electrons in a electron shell

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23
Q

Valence shell

A

The outermost electron shell

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24
Q

Inert

A

Chemically unreactive

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25
Q

Covalent bonds

A

Chemical bond that shares a pair Of valence electrons by two atoms

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26
Q

Single bond

A

A paired of shared electrons

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27
Q

Double bond

A

Sharing two pairs of valence electrons

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28
Q

Valence

A

Bonding capacity, equals the number of electrons required to complete the atoms outermost valence shell

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29
Q

Electronegativity

A

The attraction of a particular atom for the electrons of a covalent bond

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30
Q

Nonpolar covalent bond

A

Two atoms of the same element equally sharing electrons because the two atoms have same electronegativity

31
Q

Polar covalent bonds

A

An atom is bonded to a more electronegative atom, the electrons are not shared equally

32
Q

Ion

A

A charged atom ( molecule )

33
Q

Cation

A

Positively charged ion

34
Q

Anion

A

Negatively charged ion

35
Q

Ionic bond

A

Attraction between cations and anions

36
Q

Ionic compound (salts)

A

Compounds formed by ionic bonds

37
Q

Hydrogen bond

A

Noncovalent attraction between a hydrogen and electronegative atom

38
Q

Van der Waals interactions

A

Individually weak atoms occurred when atoms and molecules are very close together

39
Q

Chemical reactions

A

The making and breaking of chemicals bonds, leading to changes in the composition of matter

40
Q

Chemical equilibrium

A

The point at which the reactions offset one another exactly

41
Q

Polar molecule

A

Unequal sharing of electrons and water’s V-like shape, Overall charge is unevenly distributed

42
Q

Cohesion

A

The linking together of like molecules, often by hydrogen bonds

43
Q

Adhesion

A

The clinging of one substance to another

44
Q

Surface tension

A

A measure of how difficult it is to stretch or break the surface of a liquid

45
Q

Kinetic energy

A

The energy of motion

46
Q

Thermal energy (total thermal energy)

A

The random movement of atoms or molecules

Total thermal energy of a body of matter - depends on part of the matter’s volume

47
Q

Temperature

A

Represents the average kinetic energy I the molecules, regardless of volume

48
Q

Heat

A

Thermal energy in transfer from one body of matter to another

49
Q

Calorie

A

The amount of her it takes to raise the temperature of 1 g of water by 1 degrees Celsius

50
Q

Kilocalorie

A

The quantity of heat required to raise the temperature of 1 kilogram of water by 1 degrees Celsuis

51
Q

Specific heat

A

The amount of heat that must be absorbed or lost for 1 g of that substance to change its temperature by 1 degrees Celsuis

52
Q

Joule

A

Energy unit 1 joule = 0.239 cal.

1 cal. = 4.184 j

53
Q

Heat of vaporization

A

The quantity of her a liquid must absorb for 1 g of it to be converted from liquid to the gaseous state

54
Q

Evaporative cooling

A

Occurs because the “hottest” molecules, those with the greatest kinetic energy, are the ones most likely to leave as gas

55
Q

Solution

A

A liquid that is a completely homogenous mixture of two or more substances

56
Q

Solvent

A

The dissolving agent of the solution

57
Q

Solute

A

The substance that is dissolved

58
Q

Aqueous solution

A

One In which water is the solvent

59
Q

Hydration shell

A

The sphere of water molecules around each dissolved ion

60
Q

Hydrophilic

A

Any substance that has an affinity for water

61
Q

Hydrophobic

A

Substance that are nonionic and nonpolar ( otherwise cannot form hydrogen bonds) repel water

62
Q

Molecular mass

A

The sum of the masses of all the atoms in a molecule

63
Q

Mole

A

An exact number of objects 6.02x10^23 ( Avogadro’s number)

64
Q

Molarity

A

The number of moles of solute per liter of solution

65
Q

Hydrogen ion

A

A single proton with a charge of 1+

66
Q

Hydroxide ion

A

A single proton that has a charge of 1-

67
Q

Hydronium ion

A

A water molecule that has an extra proton bound to it ( H3O+)

68
Q

Acid

A

A substance that increase the hydrogen ion concentration of a solution

69
Q

Base

A

A substance that reduces the hydrogen ion concentration of a solution

70
Q

Ph of a solution

A 
Negative logarithm (base 10) of the hydrogen ion concentration 
( ph = - log[H+] )
71
Q

Buffer

A

A substance that minimizes changes in the concentrations of H+ and OH - In a solution ( accepting hydrogen ions from the solution when they are in excess and donating hydrogen ions to the solution when the have been deplete)

72
Q

The reactivity of an atom arises from…

A

The existence of unpaired electrons in the valence shell

73
Q

The mole of table sugar and a mole of vitamin C are equal in their mass of

A

Number of molecules

AP Bio (13 decks)

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