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GEN CHEM 2 > ch 21+23 > Flashcards

ch 21+23 Flashcards

for final

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1
Q

nucleons

A

particles that exist in the nucleus (protons and neutrons)

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2
Q

isotopes have different ——-

A

masses

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3
Q

radionuclides

A

radioactive nuclei

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4
Q

alpha decay

A

loss of an alpha particle (He nucleus)

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5
Q

beta decay

A

loss of a beta particle

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6
Q

gamma decay

A

loss of high energy radiation

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7
Q

electron capture

A

an electron from the surrounding electron cloud is absorbed into the nucleus

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8
Q

positron emission

A

nucleus emits a positron

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9
Q

positron

A

a particle that has the same mass as an electron but an opposite charge

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10
Q

alpha particle

A

+2 charge

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11
Q

beta particle

A

-1 charge

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12
Q

gamma particle

A

neutral charge

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13
Q

an atom w/ more than —— proton will have repulsions between protons

A

one

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14
Q

stable nuclei typically have a ——- proton to neutron ratio

A

one to one

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15
Q

belt of stability

A

shows us which nuclides are stable

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16
Q

nuclei with an ——- number of protons and neutrons tend to be more stable

A

even

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17
Q

a nucleus can change identity if….

A

struck by a neutron or by another nucleus

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18
Q

elements after —— were discovered by bombarding isotopes w/ neutrons

A

uranium

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19
Q

synthetics have a —– half life

A

shorter

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20
Q

geiger counter

A

measures the amount of activity present in a radioactive sample

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21
Q

phosphors

A

substances that absorb radioactivity and emit light

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22
Q

radiotracers

A

radioisotopes used to study a chemical reaction

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23
Q

mass defect

A

mass difference

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24
Q

nuclear binding energy

A

energy needed to separate a nucleus into its individual nucleons

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25
Q

fission

A

heavy nuclei gets split into smaller nuclei

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26
Q

fusion

A

smaller nuclei come together

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27
Q

commercial nuclear plants use…

A

fission

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28
Q

critical mass

A

minimum mass required for a chain reaction to occur

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29
Q

supercritical mass

A

more than critical mass and the chain reaction cannot be controlled (explosions, weapons…)

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30
Q

control rods

A

block the paths of neutrons keeping the system from reaching supercritical mass

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31
Q

thermonuclear reactions

A

small atoms are combines and a lot of energy is released (sun)

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32
Q

ionizing radiation

A

leads to ion formation (gamma or X ray)

33
Q

nonionizing radiation

A

the remainder of electromagnetic radiation

34
Q

relative biological effectiveness (RBE)

A

used to show how much biological effect there is from radiation

35
Q

of rem =

A

(# of rad)(RBE)

36
Q

metallurgy

A

the science of extracting metals from their natural sources

37
Q

as one goes from left to right a ——— then an ——– is seen in the radius of transition metals

A

decrease, increase

38
Q

isoelectronic

A

same electron configuration

39
Q

diamagnetic

A

all electrons are paired in orbitals

40
Q

paramagnetic

A

contains unpaired electrons

41
Q

ferromagnetism

A

the unpaired spins influence each other leading to a net magnetic moment (all same direction)

42
Q

antiferromagnetic

A

unpaired electrons align opposite each other (spins cancel each other out)

43
Q

ferrimagnetism

A

have spins aligned opposite, but not equal, so no cancellation

44
Q

ligands

A

molecules and ions which bind to metal centers as a Lewis base

45
Q

lewis acid in a metal-ligand bond

A

metal

46
Q

lewis base in a metal-ligand bond

A

ligand

47
Q

the coordination number depends on the….

A

size of the metal and ligand

48
Q

monodentate

A

have only one donor atom

49
Q

bidentate

A

have two donor atoms

50
Q

polydentate

A

have three or more donor atoms

51
Q

chelating (sequestering) agents

A

bi and polydentate ligands combine w/o strong attraction (used to remove ions from solution, and treat lead poisoning)

52
Q

chlorophylls

A

are porphyrins that contain Mg2+, green color

53
Q

iron

A

ferrate

54
Q

copper

A

cuprate

55
Q

lead

A

plumbate

56
Q

silver

A

argentate

57
Q

gold

A

aurate

58
Q

tin

A

stannate

59
Q

isomers

A

have the same molecular formula but different arrangement of atoms

60
Q

structural isomers

A

same molecular formula but different connections

61
Q

stereoisomers

A

same connections but different 3D orientations

62
Q

linkage isomers

A

ligand is bound to the metal by different atom

63
Q

coordination sphere isomer

A

differ by which compounds or ions are part of the complex

64
Q

cis

A

ligands on adjacent bonds

65
Q

trans

A

ligands on opposite bonds

66
Q

stereoisomers are only found in ——- and ——- 3D arrangements

A

square planar and octahedral

67
Q

optical isomers (enantiomers)

A

mirror images of one another that don’t superimpose on each other

68
Q

dextrorotary

A

rotates plane polarized light to the right

69
Q

levorotary

A

rotation to the left of plane polarized light

70
Q

racemic mixture

A

mixture of dextrorotary and levorotary

71
Q

degenerate

A

orbitals are same energy

72
Q

orbitals that point toward ligands would be ——– in energy than those that do not point toward ligands

A

higher

73
Q

crystal field splitting energy

A

energy difference between the orbitals

74
Q

ligand field theory

A

increasing theta and strength of interaction :
Cl<F<H2O<NH3<en<NO2<CN

75
Q

stronger ligand fields

A

-large splitting
-high field
-absorb light at SHORTER wavelength
-low spin

76
Q

weaker ligand fields

A

-small splitting
-low field
-absorb light at LONGER wavelength
-high spin

77
Q

high spin filling

A

normal filling (fill all before pairing)

78
Q
A

GEN CHEM 2 (3 decks)

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