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BIO 101 > Chapter 2 > Flashcards

Chapter 2 Flashcards

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1
Q

Matter

A

Matter is anything that takes up space and has mass. Organisms are composed of matter.

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2
Q

Element

A

A substance that cannot be broken down to other substances by chemical reactions. Matter is made up of elements.

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3
Q

Compound

A

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

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4
Q

Essential Elements

A

Those needed by an organism to live a healthy life and reproduce.

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5
Q

Trace Elements

A

Required only in minute quantities.

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6
Q

Atom

A

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

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7
Q

Subatomic Particles

A

Smaller particles that compose atoms.

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8
Q

Atomic Nucleus

A

The center mass of an atom. Composed of protons and neutrons.

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9
Q

3 Subatomic Particles

A

Neutrons, Protons, Electrons

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10
Q

Mass Number

A

The sum of protons and neutrons in the nucleus of an element.

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11
Q

Atomic mass

A

The total mass of an atom, can be approximated by the mass number.

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12
Q

Isotope

A

Different atomic forms of an element that differ in the number of neutrons. Radioactive isotopes decay spontaneously, giving off particles and energy.

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13
Q

Energy

A

The capacity to cause change.

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14
Q

Potential energy

A

The energy matter has because of its location or structure.

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15
Q

Electron shells

A

Characteristic average distances from the nucleus inhabited by electrons.

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16
Q

Properties of the electron shell

A

Energy level increases with distance from the nucleus. Electrons can move to higher or lower shells by absorbing or releasing energy respectively.

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17
Q

Valence Shell

A

Outermost shell of an atom. Chemical behavior of an atom mostly depends on the number of electrons in the valence shell.

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18
Q

Valence Electrons

A

Electrons that occupy the valence shell.

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19
Q

Chemical Bonds

A

Attractions between atoms with incomplete valence shells caused by the sharing of valence electrons.

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20
Q

Covalent Bond

A

The sharing of a pair of valence electrons by two atoms. The shared electrons count as a part of each atom’s valence shell.

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21
Q

Molecule

A

Two or more atoms held together by covalent bonds.

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22
Q

Single Bond/Double Bond

A

The sharing of one or two pairs of electrons.

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23
Q

Valence

A

The bonding capacity of an atom, the number of bonds that the atom can form. Usually corresponds to the number of electrons required to complete the atom.

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24
Q

Pure Elements

A

Composed of molecules of one type of atom. Such as H2 and O2.

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25
Q

Compounds

A

Molecules composed of two or more types of atoms.

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26
Q

Electronegativity

A

An atom’s attraction for the electrons of a covalent bond. The more electronegative an atom, the more strongly it pulls shared electrons toward itself.

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27
Q

Nonpolar Covalent Bond

A

Atoms share the electrons equally.

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28
Q

Polar Covalent Bond

A

One atom is more electronegative and the atoms do not share the electrons equally. Causes a partial positive or negative charge for each atom or molecule.

29
Q

Ions

A

Two oppositely charged atoms (or molecules) resulting from one atom stripping electrons from its less electronegative bonding partner.

30
Q

Cation

A

Positively charged ion.

31
Q

Anion

A

Negatively charged ion.

32
Q

Ionic Bond

A

An attraction between an anion and a cation.

33
Q

Ionic Compounds/Salts

A

Compounds formed by ionic bonds.

34
Q

Weak Chemical Bonds

A

Ionic bonds, Hydrogen bonds, Van Der Waals interactions

35
Q

Hydrogen Bond

A

Forms when a hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom nearby.

36
Q

Van der Waals Interactions

A

When electrons are distributed asymmetrically in molecules or atoms resulting in regions of negative or positive charge enabling all atoms and molecules to stick to one another.

37
Q

Chemical Reactions

A

The making and breaking of chemical bonds.

38
Q

Reactants

A

The starting molecules of a chemical reaction.

39
Q

Products

A

The final molecules of a chemical reaction.

40
Q

Chemical Equilibrium

A

When the forward and reverse reaction rates are equal.

41
Q

Emergent Properties of water which contribute to earth’s suitability for life

A

Cohesive behavior, Ability to moderate temperature, Expansion upon freezing, Versatility as a solvent

42
Q

Polar Molecule

A

Molecule whose charge is unevenly distributed (water).

43
Q

Cohesion

A

When molecules stay close together.

44
Q

Adhesion

A

The clinging of one substance to another.

45
Q

Surface tension

A

A measure of how hard it is to break the surface of a liquid.

46
Q

Kinetic energy

A

The energy of motion.

47
Q

Thermal energy

A

A measure of the total kinetic energy due to molecular motion.

48
Q

Temperature

A

The average kinetic energy of molecules.

49
Q

Heat

A

Thermal energy in transfer from one body of matter to another.

50
Q

Calorie

A

The amount of energy needed to raise the temperature of 1g of water by 1 degree celsius.

51
Q

Kilocalories (kcal)

A

1 kcal = 1000 cal.

52
Q

Joule (J)

A

1 J = 0.239 cal or 1 cal = 4.184 J.

53
Q

Specific Heat

A

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

54
Q

Heat of evaporation

A

The heat a liquid must absorb for 1 g to be converted to a gas.

55
Q

Evaporative cooling

A

The process by which as liquid evaporates, its remaining surface remains cool.

56
Q

Solution

A

A liquid that is a homogeneous mixture of other substances.

57
Q

Solvent

A

A dissolving agent of a solution.

58
Q

Solute

A

The substance that is dissolved.

59
Q

Aqueous Solution

A

One in which water is the solvent.

60
Q

Hydration Shell

A

A sphere of water molecules that surround each ion when an ionic compound is dissolved in water.

61
Q

Hydrophilic/Hydrophobic substances

A

Substances which have an affinity for water or do not respectively.

62
Q

Molecular Mass

A

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

63
Q

Hydroxide ion

A

Left behind when a hydrogen ion is transferred from one water molecule to another.

64
Q

Hydronium ion

A

The water molecule which receives the extra proton.

65
Q

Acids

A

Increase the concentration of hydronium ions in water. pH < 7

66
Q

Bases

A

Reduces the concentration of hydronium ions in water. pH > 7

67
Q

pH

A

The negative logarithm of hydronium ion concentration.

68
Q

Buffers

A

Substances that minimize changes in concentrations of H+ and OH- in a solution.

69
Q

Ocean Acidification

A

When CO2 dissolved in seawater forms carbonic acid.

BIO 101 (20 decks)

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