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BIO101 > Ch. 2 Life's Chemical Basis > Flashcards

Ch. 2 Life's Chemical Basis Flashcards

1
Q

element

A

most basic form of matter that occupies space, has mass, pure substance;
** 95% of body weight of living organisms are made up of only 4/92 naturally occurring elements** (carbon, hydrogen, oxygen, nitrogen)

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2
Q

atom

A

smallest particle of an element

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3
Q

atomic structure

A

how protons, neutrons, electrons are arranged

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4
Q

atomic number

A

number of protons of one atom in that element

all atoms of that particular element have the same atomic number

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5
Q

mass number

A

number of protons +number of neutrons

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6
Q

electron levels

A

shell order: 2,8,16(8 and 8)

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7
Q

isotope

A

atoms that have different number of neutrons (different mass number)
ex. C12 has 6 protons, 6 neutrons
C14 has 6 protons, 8 neutrons

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8
Q

radioistopes

A

isotope with unstable nucleus, emits energy– used in medical imaging (MRI, CAT)
breaks down through radioactive decay (alpha, beta, gamma)

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9
Q

free radical

A

fragment of a molecule that has an ‘unpaired electron’ in its outer electron shell
** very reactive and will pull other electrons away from molecule (carcinogens), damages DNA**

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10
Q

what determines whether atoms will interact?

A

the number of electrons and arrangement in outer electron shell

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11
Q

chemical bonding

A

when 2 or more atoms share/gain/give up an electron, links atoms to molecules

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12
Q

molecule

A

2 or more atoms bonded together

ex. H2

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13
Q

compound

A

2 or more different elements bonded together in AN EXPECTED RATIO
ex. H2O

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14
Q

mixture

A

2 or more elements intermingling but not combining

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15
Q

types of mixtures

A

colloid: particles remain suspended and will not settle out
example: mayonnaise
suspension: particles are suspended but may settle out over time
example: blood

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16
Q

chemical bookkeeping

A

use symbols for elements when writing formulas

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17
Q

glucose

A

C6H12O6

18
Q

photosynthesis’s reactants and products

A

12H2O+6CO2—->C6H12O6 (sugar) +6CO2+6H2O

19
Q

law of conservation of mass

A

matter can not be created or destroyed

20
Q

types of chemical bonding

A
  • covalent
  • ionic
  • hydrogen
21
Q

covalent bonding

A

atoms share a pair of electrons to fill the outermost shell and create a more stable element
ex. molecular hydrogen (H2)

22
Q

ionic bonding

A 
atom transfer electrons-- element has gained or lose an electron
\+charge: more protons than electrons
-charge: more electrons than protons
**oxidation: loss of electrons
**reduction: gain of electrons
23
Q

hydrogen bonding

A

molecule joined to hydrogen by polar covalent bonds

  • no true net charge
  • oppositely charge atoms attract
24
Q

what is a water molecule?

A
  • a polar covalent molecule
  • oxygen end has a slight negative charge
  • hydrogen ends has slight positive charge
25
Q

properties of water (1)

A
  1. shows polarity–causes its cohesiveness
    • hydrophilic=polar
    • hydrophobic=non-polar
      * *water’s cohesion/adhesion causes evapotranspiration (plants get water to tops of trees and leaves**
26
Q

properties of water (2)

A
  1. has temperature stabilizing effects
    -evaporation -freezing
    -ability to absorb large amounts of heat before
    changing temperature
27
Q

properties of water (3)

A
  1. universal solvent

- because ions/ polar molecules easily dissolve in water

28
Q

solute vs solvent

A

solute: substance being dissolved
solvent: substance doing the dissolving

29
Q

why are hydrogen bonds so important

A
  • hydrogen bonds are weaker than covalent bonds

- hydrogen bonds give water its unusual properties

30
Q

cohesion

A

like molecules attract

31
Q

adhesion

A

unlike molecules attract

32
Q

what about acids, bases, buffers?

A

water easily breaks into hydrogen (H+) ions and hydroxide (OH-) ions
**most influential of these ions is the H+ ion

33
Q

acid

A

donate H+ when dissolved in water

–acidic solutions have a pH<7

34
Q

bases

A

accept H+ when dissolved in water

—basic solutions have a pH>7

35
Q

buffer systems

A

chemicals that can combine with/release H+ in order to keep the pH of a solution stable

36
Q

pH scale

A

measures of H+ concentration in a solution

  • change in 1 unit on scale means 10x the change in H+ concentration
  • greater the H+ concentration, lower the pH number
37
Q

diagram of the pH scale

A

0———7———14

  • highest H+ and most acidic at zero
  • neutral is at 7
  • most basic and lowest H+ at 14
38
Q

weak acids

A

reluctant H+ donors

ex. carbonic acid

39
Q

strong acids

A

completely give up H+ when dissolved

ex. HCl

40
Q

acid rain

A

pH5

-a lot comes from the sulfur dioxide; dissolves in water vapor

41
Q

salts

A

compounds that release ions other than H+ and OH- when dissolved in water

BIO101 (9 decks)

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