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bio test 1 > chapter 2 > Flashcards

chapter 2 Flashcards

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1
Q

essential element

A

A chemical element required for an organism to survive, grow, and reproduce.`

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2
Q

specific heat

A

The amount of heat that must be absorbed or lost for 1 g of a substance to change its temperature by 1C.

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3
Q

matter

A

Anything that takes up space and has mass.

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4
Q

element

A

Any substance that cannot be broken down to any other substance by chemical reactions.

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5
Q

atomic nucleus

A

An atom’s dense central core, containing protons and neutrons.

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6
Q

mass number

A

The sum of the number of protons and neutrons in an atom’s nucleus.

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7
Q

potential energy

A

The energy that matter possesses as a result of its location or spatial arrangement (structure).

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8
Q

electron shell

A

An energy level of electrons at a characteristic average distance from the nucleus of an atom.

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9
Q

valence electron

A

An electron in the outermost electron shell.

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10
Q

inert

A

Chemically unreactive because the valence shell is full.

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11
Q

molecule

A

Two or more atoms held together by covalent bonds.

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12
Q

molecular formula

A

A way to represent just the atoms of a molecule.

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13
Q

single bond

A

The sharing of a pair of valence electrons by two atoms.

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14
Q

double bond

A

The sharing of two pairs of valence electrons by two atoms.

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15
Q

ionic bond

A

A chemical bond resulting from the attraction between oppositely charged ions.

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16
Q

van der Waals interactions

A

Weak attractions between molecules or parts of molecules that results from transient local partial charges

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17
Q

polar molecule

A

A molecule (such as water) with an uneven distribution of charges in different regions of the molecule.

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18
Q

kinetic energy

A

The energy associated with the relative motion of objects. Moving matter can perform work by imparting motion to other matter.

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19
Q

evaporative cooling

A

The process in which the surface of an object becomes cooler during evaporation, a result of the molecules with the greatest kinetic energy changing from the liquid to the gaseous state.

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20
Q

molecular mass

A

The sum of the masses of all the atoms in a molecule; sometimes called molecular weight.

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21
Q

molarity

A

A common measure of solute concentration, the number of moles of solute per liter of solution.

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22
Q

hydroxide ion

A

A water molecule that has lost a proton OH-

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23
Q

pH

A

A measure of hydrogen ion concentration equal to -log [H+] and ranging in value from 0 to 14.

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24
Q

compound

A

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

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25
What four elements make up 96% of living matter?
carbon, hydrogen, oxygen, nitrogen
26
trace element
An element indispensable for life but required in extremely minute amounts.
27
atom
The smallest unit of matter that retains the properties of an element.
28
subatomic particles
The parts that make up an atom.
29
neutron
A subatomic particle having no electrical charge (electrically neutral), with a mass of 1 dalton, found in the nucleus of an atom.
30
proton
A subatomic particle with a single positive electrical charge, with a mass of 1 dalton, found in the nucleus of an atom.
31
electron
A subatomic particle with a single negative charge and a minute mass, and move around the nucleus of an atom.
32
atomic number
The number of protons in the nucleus of an atom, unique for each element and designated by a subscript.
33
atomic mass
The total mass of an atom, which is the mass in grams of 1 mole of the atom.
34
energy
The capacity to cause change, especially to do work (to move matter against an opposing force).
35
periodic table of the elements
A tabular arrangement of the chemical elements, organized on the basis of their atomic number (number of protons in the nucleus), electron configurations, and recurring chemical properties.
36
valence shell
The outermost energy shell of an atom, containing the valence electrons involved in the chemical reactions of that atom.
37
chemical bond
An attraction between two atoms, resulting from a sharing of outer shell electrons or the presence of opposite charges on the atoms.
38
covalent bond
A type of strong chemical bond in which two atoms share one or more pairs of valence electrons.
39
structural formula
A way to represent the atoms of a molecule, and the bonds with lines.
40
valence
The bonding capacity of a given atom; the number of covalent bonds an atom can form usually equals the number of unpaired electrons in its outermost shell.
41
electronegativity
The attraction of a given atom for the electrons of a covalent bond.
42
nonpolar covalent bond
A type of bond in which electrons are shared equally between two atoms of similar electronegativity.
43
polar covalent bond
A bond between atoms that differ in electronegativity. The shared electrons are pulled closer to the more electronegative atom, making it slightly negative and the other atom slightly positive.
44
ion
An atom or group of atoms that has gained or lost one or more electrons, thus acquiring a charge.
45
cation
A positively charged ion.
46
anion
A negatively charged ion.
47
ionic compound
A compound resulting from the formation of an ionic bond; also called a salt.
48
salt
A compound resulting from the formation of an ionic bond; also called an ionic compound.
49
hydrogen bond
A type of weak chemical bond that is formed when the sightly positive hydrogen atom of a polar covalent bond in one molecule is attracted to the slightly negative atom of a polar covalent bond in another molecule or in another region of the same molecule, weak bonds are important because they are reversible
50
chemical reaction
The making and breaking of chemical bonds, leading to changes in the composition of matter.
51
What are the four emergent properties of water?
1. Cohesive behavior 2. Ability to moderate temperature 3. Expansion upon freezing 4. Versatility as a solvent
52
cohesion
The linking together of like molecules, often by hydrogen bonds.
53
Adhesion
An attraction between molecules of different substances
54
surface tension
A measure of how difficult it is to stretch or break the surface of a liquid.
55
thermal energy
Kinetic energy due to the random motion of atoms and molecules; energy in its most random form.
56
temperature
A measure in degrees of the average kinetic energy (thermal energy) of the atoms and molecules in a body of matter.
57
heat
Thermal energy in transfer from one body of matter to another.
58
calorie
The amount of heat energy required to raise the temperature of 1g of water by 1C; also the amount of heat energy that 1 g of water releases when it cools by 1C.
59
kilocalorie
A thousand calories; the amount of heat energy required to raise the temperature of 1 kg of water by 1C.
60
evaporation
Transformation from a liquid to a gas.
61
heat of vaporization
The quantity of heat a liquid must absorb for 1g of it to be converted from the liquid to the gaseous state.
62
solvent
The dissolving agent of a solution. Water is the most versatile one.
63
solute
A substance that is dissolved in a solution.
64
aqueous solution
A solution in which water is the solvent.
65
hydration shell
The sphere of water molecules around a dissolved ion.
66
hydrophilic
Having an affinity for water.
67
hydrophobic
Having no affinity for water; tending to coalesce and form droplets in water
68
hydrogen ion
A single proton with a charge of 1+. The dissociation of water leads to its generation, along with a hydroxide ion (OH-).
69
hydronium ion
A water molecule that has an extra proton bound to it; H3O+, commonly represented as H+.
70
acid
A substance that increases the hydrogen ion concentration of a solution.
71
base
A substance that reduces the hydrogen ion concentration of a solution.
72
buffer
A solution that contains a weak acid and its corresponding base. Minimizes changes in pH when acids or bases are added to the solution.
73
strong acids and bases
dissociate completely in water
74
ocean acidification
Increases CO2 levels in atmosphere which leads to oceans absorbing CO2 and carbonic acid forms this lower pH of oceans, coral reefs are at risk due to less CO3 avail for them to form calcium shells

bio test 1 (3 decks)

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