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Bio 111 > Chapter 2 > Flashcards

Chapter 2 Flashcards

1
Q

Define matter

A

Anything that takes up space and has mass

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2
Q

Define elements

A

Matter is made up of elements which are Substances that cannot be broken by chemical reactions. There are 92 naturally occuring elements

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3
Q

List the most common elements of living organisms

A

Carbon, hydrogen, oxygen, and nitrogen

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4
Q

What are essential and trace elements?

A

Trace elements: other than CHON (calcium, K, Na, S, Mg, Cl)

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5
Q

What are some imbalances (deficiencies and excesses)

A

Iodine imbalances: hypothyroidism
Excess: hyperthyroidism

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6
Q

Atoms are basic units of life and composed of

A

subatomic particles

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7
Q

Molecules

A

two or more atoms chemically bonded

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8
Q

Compounds

A

two or more different elements bonded

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9
Q

True or false all compounds are molecules, but not all molecules are compounds

A

True

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10
Q

Describe the interrelationship between protons, neutrons, electrons, atomic mass, and atomic number

A

Protons_neutrons make up weight in nucelus
atomic number is same as number of protons

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11
Q

Define isotopes and calculate using half-life

A

same number of protons, differ in neutrons, most are stable however radioactive are unstable and spontaneously give off particles and energy

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12
Q

Radioactive Isotopic

A

half-life measurements
carbon turns into nitrogen

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13
Q

BLANK elements have similar chemical properties

A

vertical column

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14
Q

Calculate valency and what it means in biology

A

valency is 8, full valence are unreactive or inert
tendency to react when not full is called combining power

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15
Q

Electronegativity criteria

A

More protons
more electrons
distance from nucleus

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16
Q

Non-polar covalent

A

atoms that have similar electrongeativites and share equally

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17
Q

polar covalent

A

atoms that have different electronegativties and share unequally

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18
Q

ionic

A

atoms that are so electronegativites that they strip bonding partners

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19
Q

Weak chemical bonds

A

reinforces the shape of large molecules, allows for reversible interactions

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20
Q

hydrogen

A

hydrogen bonds form when an H atom is attached to FON

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21
Q

how can chemical reactions build up molecules or break them down

A

converts reactants into products; bonds must be broken to form new bonds in products

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22
Q

Chemical Reactions are reversible true or false

A

true

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23
Q

Energy is released when products are formed

A

Exothermic

24
Q

Energy needed to break bonds

A

endothermic

25
Water properties
* biological medium on earth * all living things need water * 3/4 of earth is water, reason why earth is hospitable, emergent properties contribute
26
Water's Polarity
allows 4 hydrogen bonding, makes hydrophillic interactions, or hydrophobic with nonpolar like fats
27
Water's Properties: Cohesion
Cohesion is attraction of h-bonds in h20 creates surface tension and shrinks liquid surfaces to smallest area
28
Water's Properties: Adhesion
attraction to non-water molecules allows for capillary action to flow water against gravity (plants)
29
Water's high heat capacity and heat of vaporization
water has highest heat capacity, takes long to cool/heat up High heat of vaporization (liquid to gas) acts as heat sink or reservoir allows for cooling and homeostasis
30
Water's states: Gas, Liquid, Solid
hydrogen bonds changes behavior When heated, H2O boils and H bonds break causing J20 to escape When cooled, H20 freezes and sold H20 is less dense that liquid
31
Universal solvent H20
Solute(dissolved), solvent (liquid doing dissolving), and solution (mixture of solvent and solute)
32
Water's solvent properties
polar H20 can interact with ionic compounds and dissolve them each particle is surrounded by sphere of hydration or hydration shell that pull apart ionic
33
PH
water dissociates into pH which is very reactive, reversible affects changes in concentration of ions which affects pH disrupts weak bonds of proteins and cell structures results in the formation of acids and bases
34
PH logarithmic scale
change from ph 3-4 is by a factor of 10
35
pH, H+, OH-
more h is more acidic (lower pH), ratios of h and oh is inversely related
36
Acids, bases, and buffers
organisms want to maintain neutral ph buffers minimizes changes in oh or h concentrations which reduce ph change * consists of weak-acid base pair that reversibly combines with hydrogen ions accepts h when excess or donates when basic
37
Why is carbon important for life?
backbone for proteins, carbs, lipids, and nucleic acids
38
Describe the unique structure of carbon and its importance
has covalent bonds with 4 different atoms
39
Explain what hydrocarbons are
Simplest organic molecule ex: methane Ch4 covalent bonds in hydrocarbons store energy hydrophobic regions don't dissolve in water
40
Hydrocarbon Rings
* common in biological organisms aromatic rings (5 or 6 carbon rings) single or double bonds nitrogen can substitute carbon MOST COMMON BENZENE FOUND IN AMINO ACIDS AND cholesterol
41
Isomers
compounds with same number and types of atoms (arranged differently)
42
Define, list, and provide examples of the 3 important classes of isomers * Structural * Geometric * Enantiomer
* Structural: butane and isobutane * Geometric: cis-trans * Enantiomer: flip
43
Structural Isomers
* different covalent bond arrangement * same molecular formula * varying functions based on shape ex: pentane, 2-methylbutane
44
Geometric Isomers
Different in spatial arrangement around DOUBLE bonds (cis or trans)
45
Enantiomer Isomers
4 different groups bonded to asymmetrical carbon can have mirror images cannot superimpose two structures onto each other
46
Enantiomer Isomers Significane
Biological chemistry and regulation depends on molecular interactions AND shape of molecule Super important in industry, food, pharma, medicine
47
Define functional/chemical groups
Most reactive parts of molecules, helps organic compounds dissolve in water, hydrogen bonds- VERY IMPORTANT For biological molecules
48
Explain their importance/role in biological molecules
allows them to dissolve in water and form biological molecules
49
Differentiate function groups: Hydroxyl (O-H)
* found in alcohol and sugars Polar- due to oxygen increases solubility and hydrophilic example: ethanol
50
Carbonyl (C=O)
* found in simple sugars * aldehydes (terminal) * Ketones (internal) * one or the other on every monosaccaride Polar (hydrophillic)
51
Carboxyl (COOH)
* found in fatty acids and amino acids * polar acts as acid
52
Amino (NH2)
* found in EVERY amino acids * polar (hydrophillic) * acts as base and will bind free H+ ions
53
Sulfhydryl (S-H)
* found in amino acids * helps form a cross-link to stabilize protein structure polar due to sulphur (hydrophilic)
54
Methyl (Ch3)
Common in DNA (gene expression) nonpolar (hyddrophobic) * Nonreactive (used in sex hormones lipids)
55
Phosphate
found in every nucleotide and phospholipids Hydrophillic
56
Where do you find each of these (which biomolecules?)
Hydroxl, carbonyl (sugars/carbs) Sulfhydrl, amino acid (proteins) Carboxyl (proteins and lipids) Phosphate and methyl (nucleic acid)

Bio 111 (3 decks)

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