Radioactivity is the spontaneous emission of radiation from unstable atomic nuclei. It's a natural process that transforms one element into another, discovered by Henri Becquerel in 1896 while studying uranium salts.
This section explores the types of radioactive decay: alpha, beta, and gamma. We'll learn about their characteristics, how to balance nuclear equations, and the concept of decay series. Understanding these processes is crucial for nuclear physics applications.
Radioactivity and its origins
Discovery and fundamental concepts
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Radioactivity describes spontaneous emission of radiation from unstable atomic nuclei transforming one element into another
Henri Becquerel discovered radioactivity in 1896 while studying uranium salts
Marie and Pierre Curie conducted further investigations expanding knowledge of radioactive elements
Natural radioactivity occurs in elements with atomic numbers greater than 83 (uranium, thorium, radium)
Artificial radioactivity induced in stable nuclei through nuclear reactions (technetium-99m, cobalt-60)
Causes and characteristics of radioactivity
Instability in radioactive nuclei arises from imbalance in proton-neutron ratio or excess nuclear energy
Half-life characterizes rate of radioactive decay unique to each radioisotope
Half-life remains independent of external factors (temperature, pressure)
Radioactive decay follows first-order kinetics decay rate proportional to number of radioactive nuclei present
Decay constant (λ) relates to half-life through equation: t 1 / 2 = ln ( 2 ) λ t_{1/2} = \frac{\ln(2)}{\lambda} t 1/2 = λ l n ( 2 )
Types of radioactive decay
Alpha decay
Emission of alpha particle (two protons and two neutrons) from parent nucleus
Reduces atomic number by 2 and mass number by 4
Alpha particles highly ionizing but least penetrating (stopped by sheet of paper)
Energy spectrum discrete peaks due to quantized nuclear energy levels
Example decay equation: 88 226 R a → 86 222 R n + 2 4 H e _{88}^{226}Ra \rightarrow _{86}^{222}Rn + _{2}^{4}He 88 226 R a → 86 222 R n + 2 4 He
Beta decay
Three forms beta-minus (β⁻), beta-plus (β⁺), and electron capture
β⁻ decay emits electron and antineutrino (neutron converts to proton)
β⁺ decay emits positron and neutrino (proton converts to neutron)
Electron capture inner orbital electron captured by nucleus converting proton to neutron
Beta particles moderately ionizing and penetrating (stopped by thin aluminum sheet)
Energy spectrum continuous due to energy sharing between emitted particles
Example β⁻ decay: 6 14 C → 7 14 N + − 1 0 e + ν ˉ e _{6}^{14}C \rightarrow _{7}^{14}N + _{-1}^{0}e + \bar{\nu}_{e} 6 14 C → 7 14 N + − 1 0 e + ν ˉ e
Gamma decay
Emission of high-energy photons (gamma rays) from excited nucleus
No change in atomic number or mass number
Gamma rays least ionizing but most penetrating (requires thick lead shielding)
Energy spectrum discrete peaks corresponding to nuclear energy level transitions
Often accompanies alpha or beta decay as nucleus de-excites
Example gamma decay : 27 60 C o ∗ → 27 60 C o + γ _{27}^{60}Co^* \rightarrow _{27}^{60}Co + \gamma 27 60 C o ∗ → 27 60 C o + γ
Balancing nuclear decay equations
General principles
Nuclear decay equations must balance atomic number (Z) and mass number (A) on both sides
Conservation of electric charge and nucleon number fundamental to balancing equations
Use correct superscript and subscript notation for each particle (mass number top, atomic number bottom)
Account for all emitted particles including neutrinos and antineutrinos in beta decay
Specific decay equations
Alpha decay equation: Z A X → Z − 2 A − 4 Y + 2 4 H e _{Z}^{A}X \rightarrow _{Z-2}^{A-4}Y + _{2}^{4}He Z A X → Z − 2 A − 4 Y + 2 4 He
Beta-minus decay equation: Z A X → Z + 1 A Y + − 1 0 e + ν ˉ _{Z}^{A}X \rightarrow _{Z+1}^{A}Y + _{-1}^{0}e + \bar{\nu} Z A X → Z + 1 A Y + − 1 0 e + ν ˉ
Beta-plus decay equation: Z A X → Z − 1 A Y + + 1 0 e + ν _{Z}^{A}X \rightarrow _{Z-1}^{A}Y + _{+1}^{0}e + \nu Z A X → Z − 1 A Y + + 1 0 e + ν
Electron capture equation: Z A X + − 1 0 e → Z − 1 A Y + ν _{Z}^{A}X + _{-1}^{0}e \rightarrow _{Z-1}^{A}Y + \nu Z A X + − 1 0 e → Z − 1 A Y + ν
Gamma decay equation: Z A X ∗ → Z A X + γ _{Z}^{A}X^* \rightarrow _{Z}^{A}X + \gamma Z A X ∗ → Z A X + γ
Decay series and daughter nuclides
Decay series concepts
Decay series describes sequence of radioactive decays from parent nuclide to stable daughter nuclide
Common naturally occurring decay series uranium series, thorium series, actinium series
Each series starts with long-lived parent nuclide ends with stable isotope of lead
Branching decay occurs when parent nuclide decays via multiple modes with specific branching ratios
Example uranium-238 decay series involves 14 steps before reaching stable lead-206
Daughter nuclides and equilibrium
Daughter nuclides products of radioactive decay may be radioactive or stable isotopes
Secular equilibrium arises when parent nuclide half-life much longer than daughter nuclides
In secular equilibrium ratio of parent to daughter nuclides remains constant over time
Equation for secular equilibrium: λ 1 N 1 = λ 2 N 2 \lambda_1 N_1 = \lambda_2 N_2 λ 1 N 1 = λ 2 N 2
Where λ₁, N₁ are decay constant and number of atoms of parent, λ₂, N₂ for daughter
Applications of decay series
Radiometric dating determines age of geological samples (carbon-14 dating, uranium-lead dating)
Nuclear forensics analyzes radioactive materials to determine origin and history
Understanding behavior of naturally occurring radioactive materials (NORM) in environment
Radon gas mitigation in buildings based on understanding uranium decay series
Radioactive tracers in medical imaging (technetium-99m from molybdenum-99 decay)