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Molecular & Cellular Biology > Chemical Basis of Life > Flashcards

Chemical Basis of Life Flashcards

1
Q

Matter

A

Anything that has mass and occupies space

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2
Q

3 states of matter

A

solid, liquid, gas

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3
Q

Atoms

A

Fundamental building blocks of matter

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4
Q

Periodic Table

A

Tabular arrangement of chemical elements

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5
Q

Synthetic Elements

A

All above 92, plus 43 and 61

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6
Q

Four elements make up 96.1% of body mass:

A

Hydrogen (H), Oxygen (O), Carbon (C), and Nitrogen (N)

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7
Q

9 elements make up 3.9& of body mass:

A

Calcium (Ca), Phosphorus (P), Potassium (K), Sulfur (S), Sodium (Na), Chlorine (Cl), Magnesium (Mg), Iodine (I), Iron (Fe)

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8
Q

Subatomic Particles

A

Protons, neutrons, electrons

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9
Q

What is at the nucleus of an atom and what is in its orbit?

A

Proton & neutron at nucleus, electrons in orbit

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10
Q

Bohr’s Model of Atom

A

Electrons revolve around the nuclus in energy levels called orbits.

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11
Q

Orbitals

A

Regions of space around nucleus where electrons are likely to be found. Contained in energy levels.

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12
Q

Atomic Number

A

Number of protons in nucleus

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13
Q

Atomic mass

A

Average weight of atom (determined by # of protons & neutrons)

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14
Q

Number of neutrons in an atom

A

Atomic mass number - atomic number

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15
Q

Noble gases

A

They have full outermost shell

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16
Q

Octet Rule

A

Atoms will gain or lose electrons to have a full outer shell of 8e.

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17
Q

Valence

A

Number of electrons in the outermost shell

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18
Q

Isotopes

A

Different forms of atoms of the same element. # of neutrons is different

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19
Q

Radioactive Isotopes

A

Nuclei Unstable. Spontaneously break down into atoms of another element

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20
Q

Compound

A

Cluster of atoms held together by chemical bonds

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21
Q

Molecule vs Compound

A

Molecule is formed when two or more atoms join together chemically. Compound is a molecule that contains at least two different elements.

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22
Q

Chemical formulas; subscript meaning?

A

how many of that kind of atom

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23
Q

Structural formulas

A

Diagram showing how atoms are arranged

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24
Q

Types of chemical bonds

A

Ionic bond, covalent bond, hydrogen bond

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25
Q

Intra-molecular vs Inter-molecular bonds

A

Ionic & Covalent: Intra-molecular
Hydrogen: Inter-molecular

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26
Q

Ionic Bond

A

Electrons are transferred between atoms to form ions. Electrical attraction of opposite charges forms bond.
Usually outer shell almost empty or full.

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27
Q

Covalent Bond

A

Electrons are shared between atoms.
Usually outer shell hall-full.

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28
Q

Types of Covalent Bonds

A

Single bond, double bond, triple bond

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29
Q

Single Covalent Bond

A

One pair of electrons is shared

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30
Q

Double Covalent bond

A

Two pairs of electrons are shared

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31
Q

Triple Covalent bond

A

Three pairs of electrons are shared

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32
Q

Nonpolar Covalent Bonds

A

Electrons are shared equally

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33
Q

Polar Covalent Bonds

A

Electrons are not shared equally.

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34
Q

Electronegativity

A

An atom’s tendency to attract electrons to itself in a chemical bond

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35
Q

The most electronegative element

A

Fluorine

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36
Q

The least electronegative element

37
Q

The —– the difference between atom electronegativity values, the more polar chemical bond formed between them. (greater or less?)

38
Q

Ionic bonds happen between:

A

Metals and non-metals

39
Q

Covalent bonds happen between:

A

Two non-metals OR metalloids and non-metals

40
Q

Hydrophilic Molecules

A

Polar, ionic molecules.

41
Q

Do hydrophilic molecules dissolve easily in water?

42
Q

Hydrogen bonds form between:

A

Hydrophilic molecules and water

43
Q

Hydrophobic Molecules

A

Nonpolar molecules.
Water molecules cannot form hydrogen bonds.

44
Q

Do hydrophobic molecules dissolve easily in water?

45
Q

Hydrogen bonding determines these properties of water:

A

Cohesion
Adhesion
Surface Tension
Moderation of Temp. Changes
Ice floating
Excellent Solvent

46
Q

Water Properties: Cohesion

A

Tendency of molecules to stick to same type of molecule

47
Q

Water Properties: Adhesion

A

Tendency of one type of molecule to stick to a different type of molecule (Ex: flow of water up a tree)

48
Q

Water Properties: Surface Tension

A

The ability of the surface of a liquid to resist an external force, due to cohesive nature of its molecules

49
Q

Water Properties: Moderating Temperature Changes

A

Water absorbs a lot of energy as it heats. Hydrogen bonds resist increase in movement - more energy needed to raise temp.
Water releases a lot of energy as it cools. Hydrogen bonds form, releasing heat.

50
Q

Water Properties: Ice Floating

A

Ice H bonds are stable, while liquid H bonds constantly break & reform

51
Q

Water properties: Solvent

A

Polar & ionic molecules dissolve easily in water

52
Q

Definition of Molarity?

A

Measure of Concentration

53
Q

Molarity Formula

A

Number of moles / Volume

54
Q

What are the results of water dissociation?

A

Hydrogen & Hydroxide ions

55
Q

In water at room temp, concentration of H+ is:

A

10^-7 moles/liter

56
Q

Pure water pH is:

56
Q

Acidic solutions contain more:

56
Q

Basic solutions contain more:

56
Q

Acidic solutions’ pH level is:

A

Lower than 7

56
Q

Basic solutions’ pH level is:

A

Higher than 7

57
Q

Strong Acids

A

Acids that completely dissociate in solution

58
Q

Weak Acids

A

Do not completely dissociate in solution, only partly

59
Q

Acid & Base, which is H+ donor and which is acceptor?

A

Acid is donor, Base is acceptor

60
Q

NaOH & Ammonia (NH3), which is strong and which is weak base?

A

NaOH strong, NH3 weak

61
Q

Does salt have affect on H+ when dissolved in water?

62
Q

what does pH measure?

A

H+ concentration

63
Q

pH formula

64
Q

Examples of Acids

A

Hydrocloric Acid
Carbonic Acid
Acetic Acid

65
Q

Examples of Bases

A

Bicarbonate ion (HCO3-) or Ammonia (NH3)

66
Q

Buffer

A

A solution that can resist changes in pH

67
Q

When pH increases, the ____ of the buffer ____ H+

A

acid, releases

68
Q

When pH decreases, the ____ of the buffer ____ H+

A

Base, absorbs

69
Q

What pH level human blood is kept at?

70
Q

Chemical Reactions

A

Occur when chemical bonds are formed, rearranged, or broken

71
Q

Chemical Reactions contain:

A

Reactants and product(s)

72
Q

3 Patterns of Chemical Reactions

A

Synthesis reactions
Decomposition reactions
Exchange reactions

73
Q

Synthesis Reactions

A

Atoms or molecules combine to form more complex molecule

74
Q

Synthesis Reactions: Anabolic or Catabolic?

75
Q

Decomposition Reactions

A

Molecule is broken down

76
Q

Decomposition Reactions: Anabolic or Catabolic?

77
Q

Exchange Reactions

A

Involve both synthesis and decomposition

78
Q

Solutions definition

A

Homogeneous mixtures of components that may be gases, liquids, or solids.

79
Q

Solute

A

Substance dissolved

80
Q

Solvent

A

What is solute dissolved in, usually liquid

81
Q

Mixtures: Suspension

A

Composed of solid and liquid mixed together

82
Q

Mixtures: Colloids

A

Composed of solid and liquid, however solids are not visible

83
Q

Emulsion

A

Mixture of two or more liquids where one is present as droplets distributed throughout

84
Q

Emulsification

A

Large lipid globules are broken down

85
Q

When electrons remain in a shell (orbit), does the atom gain or lose energy?

Molecular & Cellular Biology (10 decks)

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