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

Ch.2 The Chemical Context of Life 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
Covalent bonds
Chemical bond that shares a pair Of valence electrons by two atoms
26
Single bond
A paired of shared electrons
27
Double bond
Sharing two pairs of valence electrons
28
Valence
Bonding capacity, equals the number of electrons required to complete the atoms outermost valence shell
29
Electronegativity
The attraction of a particular atom for the electrons of a covalent bond
30
Nonpolar covalent bond
Two atoms of the same element equally sharing electrons because the two atoms have same electronegativity
31
Polar covalent bonds
An atom is bonded to a more electronegative atom, the electrons are not shared equally
32
Ion
A charged atom ( molecule )
33
Cation
Positively charged ion
34
Anion
Negatively charged ion
35
Ionic bond
Attraction between cations and anions
36
Ionic compound (salts)
Compounds formed by ionic bonds
37
Hydrogen bond
Noncovalent attraction between a hydrogen and electronegative atom
38
Van der Waals interactions
Individually weak atoms occurred when atoms and molecules are very close together
39
Chemical reactions
The making and breaking of chemicals bonds, leading to changes in the composition of matter
40
Chemical equilibrium
The point at which the reactions offset one another exactly
41
Polar molecule
Unequal sharing of electrons and water's V-like shape, Overall charge is unevenly distributed
42
Cohesion
The linking together of like molecules, often by hydrogen bonds
43
Adhesion
The clinging of one substance to another
44
Surface tension
A measure of how difficult it is to stretch or break the surface of a liquid
45
Kinetic energy
The energy of motion
46
Thermal energy (total thermal energy)
The random movement of atoms or molecules | Total thermal energy of a body of matter - depends on part of the matter's volume
47
Temperature
Represents the average kinetic energy I the molecules, regardless of volume
48
Heat
Thermal energy in transfer from one body of matter to another
49
Calorie
The amount of her it takes to raise the temperature of 1 g of water by 1 degrees Celsius
50
Kilocalorie
The quantity of heat required to raise the temperature of 1 kilogram of water by 1 degrees Celsuis
51
Specific heat
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
Joule
Energy unit 1 joule = 0.239 cal. | 1 cal. = 4.184 j
53
Heat of vaporization
The quantity of her a liquid must absorb for 1 g of it to be converted from liquid to the gaseous state
54
Evaporative cooling
Occurs because the "hottest" molecules, those with the greatest kinetic energy, are the ones most likely to leave as gas
55
Solution
A liquid that is a completely homogenous mixture of two or more substances
56
Solvent
The dissolving agent of the solution
57
Solute
The substance that is dissolved
58
Aqueous solution
One In which water is the solvent
59
Hydration shell
The sphere of water molecules around each dissolved ion
60
Hydrophilic
Any substance that has an affinity for water
61
Hydrophobic
Substance that are nonionic and nonpolar ( otherwise cannot form hydrogen bonds) repel water
62
Molecular mass
The sum of the masses of all the atoms in a molecule
63
Mole
An exact number of objects 6.02x10^23 ( Avogadro's number)
64
Molarity
The number of moles of solute per liter of solution
65
Hydrogen ion
A single proton with a charge of 1+
66
Hydroxide ion
A single proton that has a charge of 1-
67
Hydronium ion
A water molecule that has an extra proton bound to it ( H3O+)
68
Acid
A substance that increase the hydrogen ion concentration of a solution
69
Base
A substance that reduces the hydrogen ion concentration of a solution
70
Ph of a solution
``` Negative logarithm (base 10) of the hydrogen ion concentration ( ph = - log[H+] ) ```
71
Buffer
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
The reactivity of an atom arises from...
The existence of unpaired electrons in the valence shell
73
The mole of table sugar and a mole of vitamin C are equal in their mass of
Number of molecules

AP Bio (13 decks)

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