unit 1 atomic structure n.
Skip this Video
Loading SlideShow in 5 Seconds..
UNIT 1 ATOMIC STRUCTURE PowerPoint Presentation
Download Presentation

Loading in 2 Seconds...

play fullscreen
1 / 32

UNIT 1 ATOMIC STRUCTURE - PowerPoint PPT Presentation

  • Uploaded on

UNIT 1 ATOMIC STRUCTURE . RADIOACTIVE DECAY NCCS 1.1.4. Radioactive Decay. Radioactive decay is the spontaneous disintegration of a nucleus into a slightly lighter nucleus, accompanied by emission of particles, electromagnetic radiation, or both.

I am the owner, or an agent authorized to act on behalf of the owner, of the copyrighted work described.
Download Presentation

PowerPoint Slideshow about 'UNIT 1 ATOMIC STRUCTURE' - italia

An Image/Link below is provided (as is) to download presentation

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.

- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript
unit 1 atomic structure



NCCS 1.1.4


Radioactive Decay

Radioactive decay is the spontaneous disintegration of a nucleus into a slightly lighter nucleus, accompanied by emission of particles, electromagnetic radiation, or both.

Nuclear radiation is particles or electromagnetic radiation emitted from the nucleus during radioactive decay.

An unstable nucleus that undergoes radioactive decay is a radioactive nuclide.

All of the nuclides beyond atomic number 83 are unstable and thus radioactive.

Protons and neutrons are called nucleons.

An atom is referred to as a nuclide.

radioactive nuclide emissions
Radioactive Nuclide Emissions

A nuclide’s type and rate of decay depend on the nucleon content and energy level of the nucleus.

Below are some examples of the type of radioactive decay that can occur.


Types of Radioactive Decay

Alpha Emission

  • An alpha particle (α) is two protons and two neutrons bound together and is emitted from the nucleus during some kinds of radioactive decay.
  • Alpha emission is restricted almost entirely to very heavy nuclei.

Types of Radioactive Decay, continued

Beta Emission

  • Abeta particle (β) is an electron emitted from the nucleus during some kinds of radioactive decay.
  • To decrease the number of neutrons, a neutron can be converted into a proton and an electron.
  • The atomic number increases by one and the mass number stays the same.

Types of Radioactive Decay, continued

Positron Emission

  • A positron is a particle that has the same mass as an electron, but has a positive charge, and is emitted from the nucleus during some kinds of radioactive decay.
  • To decrease the number of protons, a proton can be converted into a neutron by emitting a positron.
  • The atomic number decreases by one and the mass number stays the same.



Types of Radioactive Decay, continued

Electron Capture

  • In electron capture, an inner orbital electron is captured by the nucleus of its own atom.
  • To increase the number of neutrons, an inner orbital electron combines with a proton to form a neutron.
  • The atomic number decreases by one and the mass number stays the same.



Types of Radioactive Decay, continued

Gamma Emission

Gamma rays () are high-energy electromagnetic waves emitted from a nucleus as it changes from an excited state to a ground energy state.



What type of particle is emitted?

Identify the product that balances the following nuclear reaction.

nuclear reactions continued
Nuclear Reactions, continued

This is an alpha emission type of reaction

mass number: 212 − 4 = 208 atomic number: 84 − 2 = 82

2. The nuclide has a mass number of 208 and an

atomic number of 82,

3. The balanced nuclear equation is



  • Half-life, t1/2, is the time required for half the atoms of a radioactive nuclide to decay.
  • Each radioactive nuclide has its own half-life.
  • More-stable nuclides decay slowly and have longer half-lives.

Half-Life, continued

Sample Problem B

Phosphorus-32 has a half-life of 14.3 days. How many

milligrams of phosphorus-32 remain after 57.2 days if

you start with 4.0 mg of the isotope?

Sample Problem B Solution

Given:original mass of phosphorus-32 = 4.0 mg

half-life of phosphorus-32 = 14.3 days

time elapsed = 57.2 days

Unknown:mass of phosphorus-32 remaining after 57.2 days


Half-Life, continued


Step 1: find number of half lives

Step 2:find amount of phosphorus remaining after time has lapsed

Step 1: 57.2 days = 4 half lives

14.3 days

Step 2: 4 mg x ½ x ½ x ½ x ½ = .25 mg

OR 4 mg (1/2) 4 = .25 mg

FORMULA: (original amount of substance) x (1/2 life) (number of ½ lifes)



Fission isa reaction when the nucleus of an atom, having captured a neutron, splits into two or more nuclei, and in so doing, releases a significant amount of energy as well as more neutrons. These neutrons then go on to split more nuclei and a chain reaction takes place.



Fusion is a process where nuclei collide and join together to form a heavier atom, usually deuterium and tritium. When this happens a considerable amount of energy gets released at extremely high temperatures: nearly 150 million degrees Celsius. At extreme temperatures, electrons are separated from nuclei and a gas becomes a plasma—a hot, electrically charged gas.




mass stability
Mass Stability

The difference between the mass of an atom and the sum of the masses of its protons, neutrons, and electrons is called the mass defect.

Nuclear Binding Energy

  • According to Albert Einstein’s equation E = mc2, mass can be converted to energy, and energy to mass.
  • This is the nuclear binding energy, the energy released when a nucleus is formed from nucleons.
  • The nuclear binding energy is a measure of the stability of a nucleus.

The binding energy per nucleon is the binding energy of the nucleus divided by the number of nucleons it contains

Elements with intermediate atomic masses have the greatest binding energies per nucleon and are therefore the most stable. The elements with an atomic number of 82 or less have stable isotopes


band of stability
Band of Stability

Alpha particle

The graph has a plot of stable elements, this part is called band of stability. At the higher end of the band of stability lies alpha decay, below is positron emission or electron capture, above is beta emissions and elements beyond the atomic mass of 83 are unstable radioactive elements.



Alpha particle

Alpha decay is located at the top of the plotted line, because the alpha decay decreases the mass number of the element in order to keep the isotope stable. This is done by using the element helium (He). An unstable isotope's protons are decreased by 2 and its neutrons are decreased by 4, and because the isotope was originally unstable before it went through alpha decay, the elements are still considered unstable.



Beta decay accepts protons so it changes the amount of protons and neutrons. the number of protons increase while neutrons decrease. To make things easier to understand think of the ratio of the isotope: there are too many neutrons compared to the number of protons therefore it is above the band of stability.



Positron emission and electron capture is when the isotope gains more neutrons. Positron emission and electron capture are below the band of stability because the ratio of the isotope has more protons than neutrons, think of it as there are too few protons for the amount of neutrons and that is why it is below the band of stability.



The band of stability can be explained by the relationship between the nuclear force and the electrostatic forces between protons.

Stable nuclei tend to have even numbers of nucleons.

This is referred to as the even-odd rule

According to the nuclear shell model, nucleons exist in different energy levels, or shells, in the nucleus.

The numbers of nucleons that represent completed nuclear energy levels—2, 8, 20, 28, 50, 82, and 126—are calledmagic numbers.




  • Nuclides containing odd numbers of both protons and neutrons are the least stable
  • means more radioactive.
  • Nuclides containing even numbers of both protons and neutrons are most stable
  • means less radioactive.
  • Nuclides contain odd numbers of protons and even numbers of neutrons are less stable than nuclides containing even numbers of protons and odd numbers of neutrons.
  • In general, nuclear stability is greater for nuclides containing even numbers of protons and neutrons or both




Magic numbers are natural occurrences in isotopes and are stable. Below is a list of numbers of protons and neutrons; isotopes that have these numbers occurring in either the proton or neutron are stable. In some cases there the isotopes can consist of magic numbers for both protons and neutrons; these would be called double magic numbers. But the double numbers only occur for isotopes that are heavier, because the repulsion of the forces between the protons.  

The magic numbers:

proton: 2, 8, 20, 28, 50, 82, 114

neutron: 2, 8, 20, 28, 50, 82, 126, 184

Also, there is the concept that isotopes consisting a combination of even-even, even-odd, odd-even, and odd-odd are all stable. There are more nuclides that have a combination of even-even than odd-odd. (See chart.)



Decay Series

  • A decay series is a series of radioactive nuclides produced by successive radioactive decay until a stable nuclide is reached.
  • The heaviest nuclide of each decay series is called the parent nuclide.
  • The nuclides produced by the decay of the parent nuclides are calleddaughter nuclides.


uranium 238 decay
Uranium-238 Decay



Artificial Transmutations

  • Artificial radioactive nuclides are radioactive nuclides not found naturally on Earth.
  • They are made by artificial transmutations, bombardment of nuclei with charged and uncharged particles.
  • Transuranium elements are elements with more than 92 protons in their nuclei.
    • Artificial transmutations are used to produce the transuranium elements.



Radiation Exposure

Nuclear radiation can transfer the energy from nuclear decay to the electrons of atoms or molecules and cause ionization.

The roentgen (R) is a unit used to measure nuclear radiation exposure; it is equal to the amount of gamma and X ray radiation that produces 2  109 ion pairs when it passes through 1 cm3 of dry air.

Aremis a unit used to measure the dose of any type of ionizing radiation that factors in the effect that the radiation has on human tissue.