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Bio 111 > Chapter 2 > Flashcards

Chapter 2 Flashcards

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Biology 101 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
Q

Water properties

A
  • biological medium on earth
  • all living things need water
  • 3/4 of earth is water, reason why earth is hospitable, emergent properties contribute
26
Q

Water’s Polarity

A

allows 4 hydrogen bonding, makes hydrophillic interactions, or hydrophobic with nonpolar like fats

27
Q

Water’s Properties: Cohesion

A

Cohesion is attraction of h-bonds in h20 creates surface tension and shrinks liquid surfaces to smallest area

28
Q

Water’s Properties: Adhesion

A

attraction to non-water molecules allows for capillary action to flow water against gravity (plants)

29
Q

Water’s high heat capacity and heat of vaporization

A

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
Q

Water’s states: Gas, Liquid, Solid

A

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
Q

Universal solvent H20

A

Solute(dissolved), solvent (liquid doing dissolving), and solution (mixture of solvent and solute)

32
Q

Water’s solvent properties

A

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
Q

PH

A

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
Q

PH logarithmic scale

A

change from ph 3-4 is by a factor of 10

35
Q

pH, H+, OH-

A

more h is more acidic (lower pH), ratios of h and oh is inversely related

36
Q

Acids, bases, and buffers

A

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
Q

Why is carbon important for life?

A

backbone for proteins, carbs, lipids, and nucleic acids

38
Q

Describe the unique structure of carbon and its importance

A

has covalent bonds with 4 different atoms

39
Q

Explain what hydrocarbons are

A

Simplest organic molecule ex: methane Ch4
covalent bonds in hydrocarbons store energy
hydrophobic regions don’t dissolve in water

40
Q

Hydrocarbon Rings

A
  • 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
Q

Isomers

A

compounds with same number and types of atoms (arranged differently)

42
Q

Define, list, and provide examples of the 3 important classes of isomers
* Structural
* Geometric
* Enantiomer

A
  • Structural: butane and isobutane
  • Geometric: cis-trans
  • Enantiomer: flip
43
Q

Structural Isomers

A
  • different covalent bond arrangement
  • same molecular formula
  • varying functions based on shape
    ex: pentane, 2-methylbutane
44
Q

Geometric Isomers

A

Different in spatial arrangement around DOUBLE bonds (cis or trans)

45
Q

Enantiomer Isomers

A

4 different groups bonded to asymmetrical carbon can have mirror images cannot superimpose two structures onto each other

46
Q

Enantiomer Isomers Significane

A

Biological chemistry and regulation depends on molecular interactions AND shape of molecule
Super important in industry, food, pharma, medicine

47
Q

Define functional/chemical groups

A

Most reactive parts of molecules, helps organic compounds dissolve in water, hydrogen bonds- VERY IMPORTANT For biological molecules

48
Q

Explain their importance/role in biological molecules

A

allows them to dissolve in water and form biological molecules

49
Q

Differentiate function groups: Hydroxyl (O-H)

A
  • found in alcohol and sugars
    Polar- due to oxygen
    increases solubility and hydrophilic
    example: ethanol
50
Q

Carbonyl (C=O)

A
  • found in simple sugars
    * aldehydes (terminal)
    * Ketones (internal)
  • one or the other on every monosaccaride
    Polar (hydrophillic)
51
Q

Carboxyl (COOH)

A
  • found in fatty acids and amino acids
  • polar acts as acid
52
Q

Amino (NH2)

A
  • found in EVERY amino acids
  • polar (hydrophillic)
  • acts as base and will bind free H+ ions
53
Q

Sulfhydryl (S-H)

A
  • found in amino acids
  • helps form a cross-link to stabilize protein structure
    polar due to sulphur (hydrophilic)
54
Q

Methyl (Ch3)

A

Common in DNA (gene expression)
nonpolar (hyddrophobic)
* Nonreactive (used in sex hormones lipids)

55
Q

Phosphate

A

found in every nucleotide and phospholipids
Hydrophillic

56
Q

Where do you find each of these (which biomolecules?)

A

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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