Chapter 21: Nuclear Chemistry

Chapter 21: Nuclear Chemistry

21.1 Radioactivity

nucleons – neutron and proton

all atoms of a given element have the same number of protons, atomic number

isotopes – atoms with the same atomic number but different mass numbers

three isotopes of uranium: uranium-233, uranium-235, uranium-238

(superscript is mass number, subscript atomic number)

radionuclides – nuclei that are radioactive

radioisotopes – atoms containing radionuclides

21.1.1 Nuclear Equations

alpha particles – helium-4 particles

alpha radiation – stream of alpha particles

emission of radiation is one way that an unstable nucleus is transformed into a more stable one

superscript = mass number

subscript = atomic number

radioactive decay – when a nucleus spontaneously decomposes

sum of the mass numbers is the same on both sides of the equation

sum of the atomic numbers same on both sides of the equation

radioactive properties of the nucleus are independent of the state of chemical combination of the atom

chemical form does not matter when writing nuclear equations

21.1.2 Types of Radioactive Decay

three most common type of radioactive decay: alpha(α), beta(β), and gamma(γ) radiation

Types of Radiation

Property

α

β

γ

Charge

2+

1-

0

Mass

6.64x10^-24 g

9.11x10^-28 g

0

Relative penetrating power

1

100

10,000

Nature of radiation

electrons

High-energy photons

beta particles – high speed electrons emitted by an unstable nucleus

beta decay results in increasing the atomic number

gamma radiation – high-energy protons

gamma radiation does not change atomic number or mass number or a nucleus

almost always accompanies other radioactive emission

represents the energy lost when the remaining nucleons reorganize into more stable arrangements

positron – particle that has same mass as an electron but opposite charge

represented by

emission of a positron has effect of converting a proton to a neutron  decreasing atomic number of nucleus by 1

electron capture – the capture by the nucleus of an inner-shell electron from the electron cloud surrounding the nucleus

has effect of converting a proton to neutron

Particle

Symbol

Neutron

Proton

Electron

Alpha Particle

Beta Particle

Positron

21.2 Patterns of Nuclear Stability

21.2.1 Neutron-to-Proton Ratio

strong nuclear force – a strong force of attraction between a large number of protons in the small volume of the nucleus
stable nuclei with low atomic numbers up to 20 have nearly equal number of neutrons and protons
for higher atomic numbers, the number of neutrons are greater than the number of protons
the neutron-to-proton ratio of stable nuclei increase with increasing atomic number

belt of stability – area where all stable nuclei are found

ends at bismuth
all nuclei with 84 or more protons are radioactive
an even number of protons and neutrons is more stable than an odd number

determining type of radioactive decay

1) nuclei above the belt of stability
high neutron-to-proton ratios
move toward belt of stability by emitting a beta particle
decreases the number of neutrons and increases the number of protons in a nucleus
2) nuclei below the belt of stability
low neutron-to-proton ratios
move toward belt of stability by positron emission or electron capture
increase number of neutrons and decrease the number of protons
positron emission more common with lower nuclear charges
electron capture becomes more common with increasing nuclear charge
3) nuclei with atomic numbers 84
alpha emission
decreases both number of neutrons and protons by 2

21.2.2 Radioactive Series

some nuclei cannot game stability by a single emission
radioactive series or nuclear disintegration series – series of nuclear reactions that begin with an unstable nucleus to a stable one
three types of radioactive series found in nature

uranium-238 to lead-206, uranium-235 to leat-207, and thorium-232 to lead-208

21.2.3 Further Observations

nuclei with 2, 8, 20, 28, 50, or 82 protons or 2, 8, 20, 28, 50, 82, or 126 neutrons are more stable than with nuclei without these numbers
numbers called magic numbers
nuclei with even number of protons and neutrons more stable than with odd number of protons and neutrons
observations made in terms of the shell model of the nucleus

nucleons reside in shells

magic numbers represent closed shells in nuclei

21.3 Nuclear Transmutations

nuclear transmutations – nuclear reactions caused by the collision of one nucleus with a neutron or by another nucleus

first conversion of one nucleus into another performed by Ernest Rutherford in 1919

converted nitrogen-14 to oxygen-17

21.3.1 Using Charged Particles

particle accelerators – used to accelerate particles at very high speeds
cyclotron, and synchrotron

21.3.2 Using Neutrons

neutrons do not need to be accelerated

21.3.4 Transuranium Elements

transuranium elements – elements with atomic numbers above 92 that are produced by artificial transmutations

21.4 Rates of Radioactive Decay

radioactive decay is a first-order process
has characteristic of half life, which is the time required for half of any given quantity of a substance to react
half-life unaffected by external conditions

21.4.1 Dating

radiocarbon dating assumes that the ratio of carbon-14 to carbon-12 in the atmosphere has been constant for at least 50,000 years
age of rocks can be determined by ratio of uranium-238 to lead-206

21.4.2 Calculations Based on Half-life

rate = kN

k = decay constant, N = nuclei

t = time interval of decay, k = decay constant, N₀ = initial number of nuclei at time zero, N_t = number remaining after time interval

21.5 Detection of Radioactivity

Geiger counter – device used to measure and detect radioactivity
Based on ionization of matter caused by radiation

Phosphors – substances that give off light when exposed to radiation

Scintillation counter – used to detect and measure radiation based on tiny flashes of light produced when radiation strikes a suitable phosphor

21.5.1 Radiotracers

radioisotopes can be used to follow an element through its chemical reactions
isotopes of same element have same properties

radiotracer – radioisotopes used to trace an element

21.6 Energy changes in Nuclear Reactions

E = energy, m = mass, c = speed of light

If system loses mass, it loses energy (exothermic)

If system gains mass, it gains energy (endothermic)

21.6.1 Nuclear Binding Energies

masses of nuclei always less than masses of individual nucleons

mass defect – mass difference between a nucleus and its constituent nucleons
energy is needed to break nucleus into separated protons and neutrons, addition of energy must also have an increase in mass
nuclear binding energy – energy required to separate a nucleus into its individual nucleons

the larger to nuclear binding energy the more stable the nucleus toward decomposition

fission – energy produced when heavy nuclei split

fusion – energy produced when light nuclei fuse

21.7 Nuclear Fission

fission and fusion both exothermic
chain reaction – reaction in which the neutrons produced in one fission cause further fission reactions
in order for a fission chain reaction to occur, the sample of fissionable material must have a certain minimum mass

critical mass – amount of fissionable material large enough to maintain the chain reaction with a constant rate of fission

supercritical mass – mass in excess of a critical mass

21.7.1 Nuclear Reactors

nuclear reactors the fission is controlled to generate a constant power
reactor core consists of fissionable fuel, control rods, a moderator, and cooling fluid
fission products are extremely radioactive and are thus hard to store
about 20 half-lives needed for products to react acceptable levels for biological exposure

21.8 Nuclear Fusion

fusion is appealing because of availability of light isotopes and fusion products are not radioactive
high energies needed to overcome attraction of nuclei

thermonuclear reactions – fusion reactions
lowest temperature required is about 40,000,000 K

21.9 Biological Effects of Radiation

when matter absorbs radiation, the energy of the radiation can cause either excitation or ionization
ionization radiation more harmful than nonionization radiation
most of energy of radiation absorbed by water molecules

free radical – a substance with one ore more unpaired electrons
can attack other biomolecules to produce more free radicals
gamma rays most dangerous
tissues that take most damage are the ones that reproduce at a rapid rate
bone marrow, blood forming tissues, lymph nodes

21.9.1 Radiation Doses

becquerel (Bq) – SI unit for activity of the radiation source; rate at which nuclear disintegrations are occurring
1 (Bq) = 1 nuclear disintegration/s
curie (Ci) = 3.7x10¹⁰ disintegrations/s = rate of decay of 1g of radium
two units used to measure amount of exposure to radiation: gray (Gy) and rad
gray – SI unit of absorbed dose = absorption of 1 J of energy per kilogram of tissue
rad (radiation absorbed dose) – absorption of 1x10^-2 J of energy per kilogram of tissue
1 Gy = 100 rads
relative biological effectiveness – RBE

1 for gamma and beta radiation, 10 for alpha radiation
exact value varies with dose rate, total dose, and type of tissue affected
rem (roentgen equivalent for man) – product of the radiation dose in rads and the RBE of the radiation gibes the effective dosage
rem is unit of radiation damage that is usually used in medicine
number of rems = (number of rads)(RBE)

Sievert (Sv) – SI unit for dosage

1 Sv = 100 rem
annual exposure = 360mrem

21.9.2 Radon

radon exposure estimated to account for more than half annual exposure
half-life of radon is 3.82 days
decays into radioisotope polonium
atoms of polonium can be trapped in lungs giving out alpha radiation causing lung cancer
recommended levels of radon-222 in homes is to be less than 4 pCi per liter of air

	Types of Radiation
Property	α	β	γ
Charge	2+	1-	0
Mass	6.64x10^-24 g	9.11x10^-28 g	0
Relative penetrating power	1	100	10,000
Nature of radiation		electrons	High-energy photons

Particle	Symbol
Neutron
Proton
Electron
Alpha Particle
Beta Particle
Positron