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env 201 > ch 1 > Flashcards

ch 1 Flashcards

1
Q

metals

A

most elements are metal; shiny, conduct metal and electricity.

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2
Q

non metals

A

sulfur, chlorine, oxygen. have varied appearance and do not conduct well.

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3
Q

noble gasses

A

inert element, does not undergo chemical reactions. (helium, neon, aragon)

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4
Q

atomic number

A

protons

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5
Q

atomic mass

A

protons + neutrons

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6
Q

nucleus (3)

A
  • neutrons: no charge.
    -protons: positively charged.
  • both are of equal mass.
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7
Q

electron shell

A
  • electrons : negatively charged
  • very light.
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8
Q

an atom is neutral when:?

A

protons = #electrons

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9
Q

hydrogen exception

A

contains one electron, one proton and no neutrons.

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10
Q

isotopes

A

atoms of the same elements, with same number of protons and electrons but different number of neutrons so different mass.

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11
Q

valency

A

combining power of atoms
number of electrons needed (gained, lost, or shared) to satisfy octet rule.

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12
Q

valency gives rise to: (3)

A

-elements classified by: properties and atom number.
-groups (vertical): determine valency
-periods (horizontal)

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13
Q

electrons in outermost shell responsibility

A

interactions between atoms to form molecules.

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14
Q

covalent bonds

A

atoms sharing bonds

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15
Q

ionic bonds

A

atoms gain or lose electrons

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16
Q

cation

A

positive ion

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17
Q

anion

A

negative ion

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18
Q

electronegativity

A

a measure of an atom’s attraction for the electrons it shares in a covalent bond

—->
I. increases this way on periodic table.

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19
Q

polar bonds

A

difference in atoms’ electronegativities in a bond creates a polar bond net dipole moment.

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20
Q

a polar covalent bond

A

is a covalent bond in which the electrons are not equally shared but rather displaced towards the more electronegative atom.

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21
Q

hydrogen bond

A

electrostatic attraction between atom bearing a partial positive charge in one molecule and an atom bearing a partial negative charge in a neighboring molecule.

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22
Q

electrolytes

A

substances that will dissociate in solution

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23
Q

intramolecular bonds

A

bonds existing within molecules (strong bonds)

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24
Q

intermolecular bonds

A

bonds existing between molecules (weaker bonds)

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25
Q

molecules

A

bringing more than one atom together

26
Q

compounds

A

if you bring two or more different atoms together

27
Q

all _ are _

A

all compounds are molecules but not all molecules are compounds

28
Q

covalent compounds

A

bonds formed where the shared electrons, are contributed from both atoms.

29
Q

coordinate/dative bonds

A

covalent bonds formed where the electrons are contributed by both atoms

30
Q

complexes

A

molecules that contain one or more of coordinate/ dative bonds

31
Q

coordination compounds

A

compounds that contain complexes.

32
Q

dative bond requirements (2)

A
  • two atoms must be present as either (ion, atom or part of a molecule)
  • lewis acid + lewis base —> complex
33
Q

lewis acid

A

atom that accepts electrons

34
Q

lewis base/ligand

A

atoms with a lone pair of electrons

35
Q

chelating agent (3)

A

-if ligands have more than one atom with a lone pair of electrons.
- chemical that can form several bonds to a single metal ion
- multidentate ligand
- chemical that can form a soluble complex molecule

36
Q

lewis acid + chelating agent =

A

chelate (complex)

37
Q

porphyrin ring (4)

A

-chelate.
-act as active sites
-in chlorophyll A (for photosynthesis)
-in hemoglobin (needed for mammalian respiration.

38
Q

EDTA (3)

A
  • chelating agent
  • improve detergent efficiency
  • impose environmental threat by forming chelates with Pb and Hg, (soluble in water) -> making them available for uptake by living organisms.
39
Q

Molecular ions

A

molecules that carry net charge

40
Q

oxidation state (2)

A
  • the actual charge on the atom or a notional charge (-,+,0)
  • the imaginary charge the atom would have if the shared electrons where divided equally between identical atoms and to the more electronegative atom in different atoms.
41
Q

organic compounds

A

compounds containing C and H covalently bonded together, and other elements.

42
Q

complexation reactions (6)

A
  • also called “Lewis acid-base reaction”
  • result in dative bonds
    -lewis acid + lewis base = complex
  • metal + ligand = complex
  • Importance: affect availability of metal to organisms. i.e changes solubility of metals
  • humic material + cu (vital micronutrient) –> complex
43
Q

Acid-base reactions (5)

A

Bronsted Lowry
- acid: H+ (proton) donors
- bases: H+ (proton) acceptors / hydroxide donors
- conjugate base: product remaining after acid loses proton
- conjugate acid: product formed after base gains proton

44
Q

amphoteric

A

chemical that can act as either acid or base, based on reaction.

45
Q

Precipitation reaction (2)

A
  • reactions that occur in solution in which one or more products are insoluble in solvent (mostly water)
  • important: affects chemicals, solubility, transfer, and toxicity
46
Q

Redox reactions (oxidation, reduction, redox process, oxidizing agent, reducing agent ) (5)

A
  • oxidation: loss of electrons
  • reduction: gain of electrons
    -redox process: transfer of e’s in the reaction
  • oxidizing agent: substance reduced in reaction
  • reducing agent: substance oxidized in reaction
47
Q

steps to balancing REDOX reactions (9)

A
  1. write separate reduction, oxidation reactions.
  2. for each half reaction:
    - balance elements (except O and H)
    - balance O with H2O
    - balance H using H+
    - balance charge using electrons
  3. if necessary, multiply by integer to equalize electron count.
  4. add half reactions
  5. check that elements and charges are balanced.
48
Q

Hydrolysis

A

reaction where one of its reactants is water
- acid hydrolysis
- basic hydrolysis
-Importance: weathering of rocks.

49
Q

Free radical reactions (9)

A
  • molecules mostly contain an even number of electrons- behaves as pairs
    -molecules that have one or more unpaired electrons is called “free radical” or “radical”
  • highly reactive
  • free radicals leads to chain reactions by producing other free radicals and other products.
  • radicals form as a result of:
    • collision with another molecule
    • collision with atom at high speed “thermal reaction”
    • absorbs light “photochemical reaction”
    • reacting with excited species.
50
Q

Atmospheric Ozone Depletion by CFCs (draw)

A

First, UV radiation breaks a carbon- halogen bond
photon (λ < 220nm) + CCl2F2 —-> CClF2 + Cl- ( free radicals )

51
Q

Transumation Process

A

process: reactions that change the nuclei of one atom to another atom
- nucleus 1 —- nuclear reaction —-> nucleus 2
- nucleus of atom consist of nucleons (proton + neutrons)
- Nuclear binding energy (E): energy holding the protons and neutrons together (released during nuclear rxn)
- the higher the binding energy, the more stable the atoms.
- E=mc^2

52
Q

Radioactivity vs Natural radiation (“background radiation)

A

Average annual dose to the general population. natural sources mainly radon, manmade sources mainly medical x - ray.

53
Q

sources of radiation (natural) (4)

A
  • radon
  • internal
  • terrestrial
  • cosmic
54
Q

sources of radiation (man-made) (3)

A
  • consumer product
  • nuclear medicine
  • medical x ray
55
Q

Types of Nuclear Reactions
- nuclear fission

A
  • Breaking apart of heavy nuclei to form two or more nuclei of roughly similar mass (total) + release of energy.
    • a few rxns do not need outside simulation
  • nuclear fission rxns can be simulated through neutrons
56
Q

Types of Nuclear Reactions
- nuclear fusion

A
  • Bringing together of two light nuclei + release of energy.
  • happens in the stars, naturally.
  • occurs on earth, artificially, by fast moving nuclei or nucleons.
57
Q

Types of Nuclear Reactions
- nuclear Decay

A

disintegration of one nuclei into another (daughter nucleus) without external initiation (alpha, beta. gamma decay).

58
Q

Radioactive decay

A

when atoms ( with atomic number greater than 83, which are unstable) undergo spontaneous radioactive disintegration.

59
Q

Radioisotopes / radionuclides

A
  • nuclei that undergo radioactive decay
    -produce radiation (alpha, beta, gamma)
    -may have harmful effects on environment and humans based on their energy.
60
Q

Chemical reactions vs nuclear reactions

A

C: atoms retain their identity
N: atoms usually change from one element to another

C: Reactions involve only electrons, usually only outermost electrons.
N: reactions involve mainly protons and neutrons. valence electrons irrelevant.

C: raising temp can speed up rxn rates
N: rxn rates unaffected by temp changes.

C: energy absorbed/given off by reactions is comparatively small.
N: rxns sometimes involve enormous changes in energy.

C: mass is conserved, the mass of products equals the mass of starting materials.
N: huge changes in energy accompanied by measurable changes in mass (E=MC^2)

env 201 (3 decks)

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