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BIOL1190 > CH 2: Self Study > Flashcards

CH 2: Self Study Flashcards

1
Q

chemistry

A

science of matter

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2
Q

matter

A

all the properties of organisms depends on how atoms are arranged in molecules and how molecules are arranged in cells
- structure dictates function

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3
Q

chemical element

A

substance that only contains one type of atom, different from atoms of other elements

  • cannot be broken down
  • 26 elements that are essential for life
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4
Q

atom

A

smallest unit of matter that still retains the properties of an element

  • made of 3 types of subatomic particles: protons, neutrons, electrons
  • # of protons = # number of electron –> neutral charge
  • atoms of different elements vary in # of subatomic particles
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5
Q

proton

A
  • subatomic particle of an atom

- +1 positive charge

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6
Q

netron

A
  • subatomic particle of an atom

- neutral/no charge

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7
Q

electron

A
  • subatomic particle of an atom
  • -1 negative charge
  • determines how an atom interacts with another atom
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8
Q

atomic number

A
  • # of p+ in nucleus

- unique to each element

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9
Q

mass number

A
  • sum of protons plus neutrons in the nucleus

- all atoms of an element have same number of p+ but may differ in number of neutrons

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10
Q

isotope

A

2 atoms of an element that differ in # of neutron

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11
Q

radioactive isotopes

A

nucleus decays spontaneously giving off particles and en-

  • dangerous to life b/c causes mutations in DNA
  • can be useful in biological research and medicine as tracers
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12
Q

electron shells

A

regions surrounding the nucleus on which e- move around
- 1st shell: 2e-
- 2nd shell: 8e-
- 3rd shell: 8e-
the farther the e- from the nucleus, the more en- it has

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13
Q

valence electrons

A
  • e- in outermost shell/valence shell
  • chemical behaviour of an atom is determined by the valence e-
  • atoms in which the outermost shell is not completely filled with e- tend to be chemically reactive
  • elements with full valence shell: chemically inert
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14
Q

valence of an element

A
  • number of e- needed to complete outermost shell

- = # of covalent bonds an element can form

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15
Q

ions

A

of protons and electrons is not equal

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16
Q

cation

A

positively charged ion

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17
Q

anion

A

negatively charged ion

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18
Q

covalent bonds

A
  • forces that hold atoms together to make compounds and molecules
  • sharing a pair of valence e- by 2 atoms
  • very strong
  • usually involves atoms with 3-5 e- in their valence shell
  • forms stable molecules: full valence shell
  • shared pair of e- counts as part of each atom’s valence shell
    • # of single covalent bonds an atom can form = to # of addeitional e- needed to fill its outer shell
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19
Q

compound

A
  • substance that contains 2+ different elements

- can be broken into different types of atoms

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20
Q

molecule

A
  • 2+ atoms sharing e-
  • can be same or different types of atoms
  • involve covalent bonds
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21
Q

octet rule

A
  • two atoms are more likely to interact if the interaction will leave them both with 8 e- in their valence shell (full valence shell)
  • atoms can donate or share e-
  • enables prediction of how atoms of different elements will interact
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22
Q

ionic bonds

A
  • interactions between ions of opposite charge
  • e- donor atom becomes positively charged and e- acceptor atom becomes negatively charged
    • charged particles attracted to each other forming ionic bond
  • not very strong
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23
Q

compounds formed by ionic bonds

A
  • not considered molecules
  • composed of 2 different atoms, present in set ratio (ex. NaCl –> table salt)
  • crystal lattice structure common to salts
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24
Q

electronegativity

A
  • atom’s attraction for the shared e- of bond (covalent)
  • the more electronegative atom, the more strongly it pulls e- towards itself
  • low electronegativity: C H P
  • high electronegativity: O N S
25
Q

non-polar covalent bond

A

when e- are equally shared

26
Q

polar covalent bonds

A

when e- are not equally shared by the 2 types of atoms

  • more electronegative atom becomes partially negative because it has pulled the electron from the less electronegative atom towards it
  • less electronegative atom becomes partially positive because its e- has been pulled away by the more electronegative atom
27
Q

polar molecules

A
  • molecules that are predominantly comprise of polar-covalent bonds
  • ex. sugar (has multiple hughly electronegative O atoms in polar-covalent bonds)
28
Q

non-polar molecules

A
  • molecules that are predominantly comprised of non-polar covalent bonds
  • ex. oil (does not have highly electronegative O atoms)
29
Q

water molecule

A
  • polar: neutral overall but has a slightly negative pole and 2 slightly positive poles
30
Q

hydrogen bonding

A
  • charged region on each H2O molecules are attracted to oppositely charged region on neighbouring H2O molecules forming weak bonds
  • entermolecular bonds: links btw molecules
  • non-covalent interaction: no bond is formed, it’s an attraction of polar regions of 2 different molecules
  • very weak: constantly formed and destroyed
31
Q

water

A
  • inorganic compond (lacks carbon)

- solvent of life

32
Q

water as solvent of life

A
  • life orginated and evolved in water
  • water makes earth habitable
  • most organisms live in water
  • 60-90% of cell mass is water
  • all metabolic processes of the body occur in aqueous environment
  • water is substrate for many cellular reactions
33
Q

water - properties

A
  1. highly cohesive
    - tendency of molecules to stick together
    - creates surface tension
  2. high heat capacity
    - allows water to resist temperature changes
  3. expands upon freezing
    - allows for liquid water to remain all year round
  4. versatile solvent
    - dissolves a wide variety of solutes due to polarity of its molecules
34
Q

solution

A
  • liquid that is a homogenous mixture of substances

- composed of solvent and solute

35
Q

solvent

A

dissolving agent of solution

36
Q

solute

A

substance that is dissolved in a solution

37
Q

hydrophilic substance

A
  • “water-loving”
  • has affinity for water
  • molecules are typically polar and/or charged
38
Q

hydrophobic substance

A
  • “water-fearing”
  • does not have affinity for water
  • molecules are relatively non-polar
39
Q

hydration sphere

A

water forms a hydration sphere around ions, separating the Na+ and Cl- from each other and breaking the ionic bonds that held NaCl together

  • ionic bonds broken down due to polar bonds in water molecules
  • O in H2O surrounds Na+ ion
  • H in H2O surrounds Cl- ion

water can also dissolve polar molecules
- the dissolved polar molecules remain intact in aqueous solutions b/c covalent bonds are too strong to be broken by water

40
Q

H+ and OH-

A
  • highly reactive
  • changes in their concentration can drastically affect other cherged molecules in a cell
  • H+ and OH- concentrations are equal in water
  • adding acids or bases chamges their concentrations
41
Q

acid

A
  • chemical compound that donates H+ ions to solutions

- the more acidic a solution, the higher the [H+]

42
Q

base

A
  • chemical compound that acceots H+ ions and removes them from a solution
  • the more basic a solution, the lower the [H+]
43
Q

pH scale

A
  • measures [H+] in a solution
  • ranges from 0 (most acidic) to 14 (most basic) - pH7 is neutral –> [H+] = [OH-]
  • expressed in terms of negative logarithms (10x change)
44
Q

buffer

A
  • substances that rsist changes in concentrations of H+ and OH- in a solution
  • maintain pH of solution at a constant level (not necessarily neutral) - contribute to hoemostasis
  • they accept H+ ions from solution when they are in excess
  • they donate H+ ions to solution when they have been depleted
45
Q

first law of thermodynamics

A

en- cannot be created or destroyed; en- can only be transferred or changed from one form to another

46
Q

energy

A
  • capacity to do work
  • transformed into useable form by enzyme-controlled chemical reactions
  • 2 types: kinetic and potential
47
Q

work

A
  • moving things from one place to another

- causing an alteration in something

48
Q

kinetic energy

A
  • en- that an object has due to its motion

- ex. heat

49
Q

potential energy

A
  • en- stored in a system due to its position or configuration
  • aka stored en-
  • ex. chemical energy
50
Q

reactants

A

starting molecules of a chemical reaction

51
Q

products

A

final molecules of a chemical reaction

52
Q

chemical reactions and energy

A
  • en- involved every time a chemical reaction takes place
  • kinetic en- can be converted to potential en- and viceversa
    • potential en- stored in bonds
    • en- released when chemical bonds are formed
    • breakign bonds requires en-
53
Q

catabolic pathways

A
  • release en- by breaking down complex molecules in simpler compounds
  • exergonic = release en-
54
Q

anabolic pathways

A
  • consume en- to build complex molecules from simpler ones

- endergonic = requires en

55
Q

exergonic reaction

A

releases en-

56
Q

endergonic reaction

A

consumes en-

57
Q

spontaneous reactions

A
  • chemical reaction that occurs due to kientic en- of reactants
  • tiny particles of matter are constantly in motion and thus bumping into each other
  • if two or more molecules bump into each other with enough kinetic en-, the impact will shake up the valence e- resulting in either the formation or breaking of bonds
58
Q

activation energy

A
  • amount of kinetic en- required to get a reaction going

- takes en- to break chemical bonds and initiate a reaction - supplied by kinetic energy

59
Q

enzymes

A
  • catalyst protein that speed up a chemical reaction by lowering the amount of activation energy

BIOL1190 (7 decks)

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