F_CHEM-T 03

• Nuclear Chemistry


  is the subdiscipline of chemistry that is concerned with changes in the nucleus of elements. These changes are the source of radioactivity and nuclear power.
• Nuclear Chemistry 


  is the study of nuclear reactions, with an emphasis on their uses in chemistry and their effects on biological systems.
• Modern Nuclear Chemistry


  sometimes referred to as radiochemistry, has become very interdisciplinary in its applications, ranging from the study of the formation of the elements in the universe to the design of radioactive drugs for diagnostic medicine.
• Nuclear Energy 


  refers to the energy accompanying nuclear reactions.
• Nuclear Energy


  is the energy in core of an atom which can be released when the bonds are broken or fused. Nuclear energy can be produced either by the fusion (combining atoms) or fission (splitting of atoms) process and this energy can be used to produce electricity.
• Nuclear Reactions


  refers to changes participated by the particles (protons and neutrons or collectively known as nucleons) inside the atom of an element together with other particles.
• Nuclear Reactions


  this does not obey the Law of Conservation of Mass/ Matter and the Law of Conservation of Energy
• Mass and Energy in Nuclear Reactions


  can be created or destroyed. any loss in mass during nuclear reaction is transformed to energy based on Einstein's equation
• Proton


  the index particle of an atom. it determines the identity of the element an atom belongs
• Proton


  the number of protons in an element determines its atomic number. Hydrogen (H) is the lightest element and has 1 proton. Uranium (U) is the heaviest naturally occurring element and has 92 protons.
• Proton


  has a mass if 1.00728 atomic mass unit (amu)
• Proton 


  has a charge designated as +1
• Neutron


  similar in size to protons and also inhabit the nucleus of atoms
• Neutron


  has a mass of 1.00867 amu
• Neutron


  the number of neutrons in an atom in an element's most stable configuration is usually greater than the number of protons, with this disparity becoming larger as atomic number increases.
• Neutron


  the number of protons plus neutrons in an atom (nucleons) is its mass number (A). thus the number of neutrons in an atom is its atomic mass number minus its atomic number, or n = A - Z
• Electron


  are tiny and has a mass of 0.000549 amu
• Electron


  negatively charged particles
• Electron


  orbiting the protons and neutrons that make up an atom's nucleus, in manner of planets orbiting the sun.
• Positron


  is a particle of matter with the same mass as an electron (0.000549 amu) but opposite charge
• Positron


  are emitted in the positive beta decay of proton-rich radioactive nuclei and are formed in pair production
• Positron


  it is a form of antimatter because when it encounters an electron the two completely annihilate to yield energy
• Gamma Particle


  a stream of electromagnetic radiation having a wavelengths shorter than those of x-rays and therefore greater energy and penetrating power
• Gamma Particle


  are given off by unstable nuclei during radioactive decay and electron-positron annihilation
• Gamma Particle


  the emission of gamma rays by a nucleus is called gamma decay
• Gamma Particle


  symbol Y
• Gamma Particle 


  have no electrical charge associated with them
• Alpha Particle


  is a helium nucleus; it consists of two protons and two neutrons
• Alpha Particle


  it has no electrons to balance the two positively charged protons
• Alpha Particle


  are emitted by neutron rich unstable nuclei
• Alpha Particle


  mass is 4 u (unified atomic mass unit)
• Alpha Particle


  symbol a
• Beta Particle


  also called beta ray or beta radiation
• Beta Particle


  symbol B
• Beta Particle

  is a high-energy, high speed electron or positron emitted by the radioactive decay of atomic nucleus during the process of beta decay
• Nuclidic Notation


  notation showing the properties of the nucleus of an atom of element based on the given mass number/ atomic mass (A) and atomic number (Z)
• Isotopes


  refer atoms of the same element having the same number of protons (same Z) but differ in the number of neutrons (different A)
• Nuclide


  nucleus of a specific or particular type of isotope
• Isotopic Mass/ Weight


  the mass of one specific or particular type of isotope
• Atomic Mass/ Weight


  the average mass contributed by all the existing isotopes of an element