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Molecular & Cellular Biology > Chemical Basis of Life > Flashcards

Chemical Basis of Life Flashcards

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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
Intra-molecular vs Inter-molecular bonds
Ionic & Covalent: Intra-molecular Hydrogen: Inter-molecular
26
Ionic Bond
Electrons are transferred between atoms to form ions. Electrical attraction of opposite charges forms bond. Usually outer shell almost empty or full.
27
Covalent Bond
Electrons are shared between atoms. Usually outer shell hall-full.
28
Types of Covalent Bonds
Single bond, double bond, triple bond
29
Single Covalent Bond
One pair of electrons is shared
30
Double Covalent bond
Two pairs of electrons are shared
31
Triple Covalent bond
Three pairs of electrons are shared
32
Nonpolar Covalent Bonds
Electrons are shared equally
33
Polar Covalent Bonds
Electrons are not shared equally.
34
Electronegativity
An atom's tendency to attract electrons to itself in a chemical bond
35
The most electronegative element
Fluorine
36
The least electronegative element
Francium
37
The ----- the difference between atom electronegativity values, the more polar chemical bond formed between them. (greater or less?)
Greater
38
Ionic bonds happen between:
Metals and non-metals
39
Covalent bonds happen between:
Two non-metals OR metalloids and non-metals
40
Hydrophilic Molecules
Polar, ionic molecules.
41
Do hydrophilic molecules dissolve easily in water?
Yes.
42
Hydrogen bonds form between:
Hydrophilic molecules and water
43
Hydrophobic Molecules
Nonpolar molecules. Water molecules cannot form hydrogen bonds.
44
Do hydrophobic molecules dissolve easily in water?
No.
45
Hydrogen bonding determines these properties of water:
Cohesion Adhesion Surface Tension Moderation of Temp. Changes Ice floating Excellent Solvent
46
Water Properties: Cohesion
Tendency of molecules to stick to same type of molecule
47
Water Properties: Adhesion
Tendency of one type of molecule to stick to a different type of molecule (Ex: flow of water up a tree)
48
Water Properties: Surface Tension
The ability of the surface of a liquid to resist an external force, due to cohesive nature of its molecules
49
Water Properties: Moderating Temperature Changes
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
Water Properties: Ice Floating
Ice H bonds are stable, while liquid H bonds constantly break & reform
51
Water properties: Solvent
Polar & ionic molecules dissolve easily in water
52
Definition of Molarity?
Measure of Concentration
53
Molarity Formula
Number of moles / Volume
54
What are the results of water dissociation?
Hydrogen & Hydroxide ions
55
In water at room temp, concentration of H+ is:
10^-7 moles/liter
56
Pure water pH is:
7
56
Acidic solutions contain more:
H+
56
Basic solutions contain more:
OH-
56
Acidic solutions' pH level is:
Lower than 7
56
Basic solutions' pH level is:
Higher than 7
57
Strong Acids
Acids that completely dissociate in solution
58
Weak Acids
Do not completely dissociate in solution, only partly
59
Acid & Base, which is H+ donor and which is acceptor?
Acid is donor, Base is acceptor
60
NaOH & Ammonia (NH3), which is strong and which is weak base?
NaOH strong, NH3 weak
61
Does salt have affect on H+ when dissolved in water?
No
62
what does pH measure?
H+ concentration
63
pH formula
-log(H+)
64
Examples of Acids
Hydrocloric Acid Carbonic Acid Acetic Acid
65
Examples of Bases
Bicarbonate ion (HCO3-) or Ammonia (NH3)
66
Buffer
A solution that can resist changes in pH
67
When pH increases, the ____ of the buffer ____ H+
acid, releases
68
When pH decreases, the ____ of the buffer ____ H+
Base, absorbs
69
What pH level human blood is kept at?
7.4
70
Chemical Reactions
Occur when chemical bonds are formed, rearranged, or broken
71
Chemical Reactions contain:
Reactants and product(s)
72
3 Patterns of Chemical Reactions
Synthesis reactions Decomposition reactions Exchange reactions
73
Synthesis Reactions
Atoms or molecules combine to form more complex molecule
74
Synthesis Reactions: Anabolic or Catabolic?
Anabolic
75
Decomposition Reactions
Molecule is broken down
76
Decomposition Reactions: Anabolic or Catabolic?
Catabolic
77
Exchange Reactions
Involve both synthesis and decomposition
78
Solutions definition
Homogeneous mixtures of components that may be gases, liquids, or solids.
79
Solute
Substance dissolved
80
Solvent
What is solute dissolved in, usually liquid
81
Mixtures: Suspension
Composed of solid and liquid mixed together
82
Mixtures: Colloids
Composed of solid and liquid, however solids are not visible
83
Emulsion
Mixture of two or more liquids where one is present as droplets distributed throughout
84
Emulsification
Large lipid globules are broken down
85
When electrons remain in a shell (orbit), does the atom gain or lose energy?
Neither

Molecular & Cellular Biology (10 decks)

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