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Bio 111 > Chapter 2 > Flashcards

Chapter 2 Flashcards

1
Q

Anything that occupies space and has mass

A

Matter

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2
Q

A pure substance that cannot be broken down into simpler substances by ordinary chemical of physical techniques

A

Element

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3
Q

The smallest unit that retains the chemical and physical properties of an element

A

Atoms

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4
Q

An element that occurs in organisms in very small quantities. In nutrition a mineral el required by organisms only in small amounts

A

Trace elements

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5
Q

The name of a molecule written in chemical shorthand

A

Formula

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6
Q

A unit of atoms combined chemically in fixed numbers and ratios

A

Molecules

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7
Q

The part of an atom which consists of subatomic particles called protons and neutrons

A

Atomic nucleus

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8
Q

A molecule whose component atoms are different

A

Compounds

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9
Q

Uncharged subatomic particle in the nucleus of an atom

A

Neutrons

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10
Q

A subatomic particle in the nucleus of an atom that carries one unit of charge

A

Protons

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11
Q

Negatively charged particles outside the nucleus of an atom

A

Electrons

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12
Q

The number of protons in the nucleus of each kind of atom

A

Atomic number

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13
Q

A distinct form of the atoms of an element, all with the same number of protons but different number of neutrons

A

Isotopes

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14
Q

The total number of protons and neutrons in the atomic nucleus

A

Mass number

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15
Q

The amount of matter in an object

A

Mass

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16
Q

A standard unit of mass, around 1.66 x 10 - 23 grams

A

Dalton

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17
Q

The giving off of particles of matter and energy by decaying nuclei

A

Radioactivity

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18
Q

A measure of the pull of gravity of an object

A

Weight

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19
Q

An unstable, radioactive isotope

A

Radioisotope

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20
Q

A dating technique that uses clockwork decay of unstable isotopes to estimate the age of organic material, rocks, or fossils that contain them

A

Radiometric dating

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21
Q

The region of space where the electron lives most of the time

A

Orbital

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22
Q

Isotope used to label molecules so that they can be tracked as they pass through biochemical reactions

A

Tracers

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23
Q

Regions of space within an atom where electrons are found. Also referred to as shells

A

Energy levels

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24
Q

Regions of space within an atom where electrons are found. Also referred to as energy levels

A

Shells

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25
Q

Link formed when atoms of reactive elements combine into molecules

A

Chemical bonds

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26
Q

An electron in the outermost energy level of an atom

A

Valence electrons

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27
Q

A bond that results from electrical attractions between atoms that gain or lose valence electrons completely

A

Ionic bonds

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28
Q

A positively charged ion

A

Cation

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29
Q

A negatively charged ion

A

Anion

30
Q

Bond formed be electron sharing between atoms

A

Covalent bonds

31
Q

Bond in which electrons are shared equally or nearly equally. The atoms have no charge

A

Non polar covalent bond

32
Q

The measure of the tendency of an atom to attract electrons to itself in a chemical bond (that is, to become negative)

A

Electronegativity

33
Q

Bond in which electrons are shared unequally

A

Polar covalent bond

34
Q

Association that occurs when polar molecules attract and align themselves with other polar molecules and with charged ions and molecules

A

Polar associations

35
Q

In chemistry and biology, referring to polar molecules that associate readily with water

A

Hydrophilic

36
Q

Association that occurs when non polar molecules clump together

A

No polar associations

37
Q

Non-covalent bond formed by unequal electron sharing between hydrogen atoms and oxygen, nitrogen or sulfur atoms

A

Hydrogen bond

38
Q

In chemistry and biology, referring to non polar substances that are excluded by water and other polar molecules

A

Hydrophobic

39
Q

The three dimensional arrangement of the atoms in a molecule. Aka it’s shape

A

Molecular geometry

40
Q

Weak molecular attractions over short distances

A

Van der waals forces

41
Q

A reaction that occurs when atoms or molecules interact to form new chemical bonds or break old ones

A

Chemical reactions

42
Q

The atoms or molecules entering a chemical reaction

A

Reactants

43
Q

An atom or molecule leaving a chemical reaction

A

Products

44
Q

An arrangement formed when a water molecule in liquid water establishes an average of 3.4 hydrogen bonds with its neighborS

A

Water lattice

45
Q

A rigid, crystalline structure formed when a water molecule in ice forms four hydrogen bonds with neighboring molecules

A

Ice lattice

46
Q

A chemical reaction written in balanced form

A

Chemical equations

47
Q

The amount of heat required to raise 1g of water by 1•C; known as a small calorie; when capitalized, a unit equal to 1000 small calories

A

Calorie

48
Q

The amount of heat required to increase the temperature of a given quantity of water

A

Specific heat

49
Q

The scientific unit equivalent to a Calorie and equal to 1000 small calories

A

Kilocalorie

50
Q

The heat required to give water molecules enough energy of motion to break loose from liquid water and form a gas

A

Heat of vaporization

51
Q

The high resistance of water molecules to separation

A

Cohesion

52
Q

The force that places surface water molecules under tension, making them more resistant to seperate on than the underlying water molecules

A

Surface tension

53
Q

A surface coat of water molecules that covers other polar and charged molecules and ions

A

Hydration layer

54
Q

A membrane with two molecular layers

A

Bilayer

55
Q

The water in a solution in which the hydration layer prevents polar molecules or ions from reassociating

A

Solvent

56
Q

Substance formed when molecules and ions separate and are suspended individually, surrounded by water molecules

A

Solution

57
Q

The number of molecules or ions in a substance in a unit volume of space

A

Concentration

58
Q

The molecules of a substance dissolved in water

A

Solute

59
Q

The weight of a element in grams, equal to the mass number

A

Atomic weight

60
Q

The number 6.022 x 10^23, derived by deciding the atomic weight of any element by the weight of an atom of that element

A

Avogadro’s number

61
Q

The weight of a molecule in grams, equal to the total mass number of its atoms

A

Molecular weight

62
Q

The number of moles of a substance dissolved in 1L of solution

A

Molarity

63
Q

Amount of substance that contains as many atoms or molecules as there are atoms in exactly 12g of carbon-12, which is 6.022 x 10^23

A

Mole

64
Q

The separation of water to produce positively charged hydrogen ions and hydroxide ions

A

Dissociate

65
Q

The term indicating that a reaction may go from left to right or from right to left, depending on conditions

A

Reversible

66
Q

Proton donor that releases H+ (and anions) when dissolved in water

A

Acids

67
Q

Proton acceptor that reduces the H1 concentration of a solution

A

Bases

68
Q

The numerical scale from 1 to 14 used by scientists to measure acidity

A

pH scale

69
Q

The concentration of H+ in a water solution, as compared with the concentration of OH-

A

Acidity

70
Q

Substance that compensates for pH changes by absorbing or releasing H+

A

Buffers

71
Q

Rainfall with low pH, primarily created when gaseous wilder dioxide (SO2) dissolved in water vapor in the atmosphere, forming a sulfuric acid

A

Acid precipitation

Bio 111 (3 decks)

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