Atomic Structure
Mindmap for F321 1.1.1 Atomic Structure. Outlines the subatomic particles, isotopes and nuclides.
- Created by: TayaMairead
- Created on: 23-10-13 21:27
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- F321 1.1.1 Atomic Structure
- The Sub-Atomic Particles
- An atom must have the same number of electrons as protons. This makes all atoms neutral
- Nuclides
- The term used to describe any atom of which the atomic number and the mass number are specified
- Written as-
- Mass Number
- (nucleon number)
- The number of protons and neutrons present in the nucleus of the atom
- (nucleon number)
- X
- Atomic Number
- (proton number)
- the number of protons present in the nucleus of the atom
- in atoms the proton number is always equal to the number of electrons
- the number of protons present in the nucleus of the atom
- (proton number)
- Mass Number
- Calculations
- Number of Electrons
- Positive ion (cation)
- Subtract charge from atomic number
- Negative ion (anion)
- Add charge to atomic number
- Positive ion (cation)
- Number of Neutrons
- Subtract atomic number from mass number
- Number of Electrons
- Isotopes
- Definitions
- Isotope
- Relative atomic mass (Ar)
- Average mass of the naturally occurring isotopes of the element relative to the mass of an atom of Carbon-12 which has a mass of 12
- Relative isotopic mass
- Average mass of a naturally occurring isotope of the element relative to the mass of an atom of Carbon-12 which has a mass of 12
- Calculating relative atomic mass from isotopic abundance
- Multiply abundance (%) by isotopic masses
- Definitions
- The Sub-Atomic Particles
- Found in NUCLEUS
- Neutrons
- 0 Charge (neutral)
- Relative Mass= 1
- The Sub-Atomic Particles
- An atom must have the same number of electrons as protons. This makes all atoms neutral
- Protons
- +1 Charge
- Relative mass= 1
- Every atom of the same element has the same proton number
- Nucleus is tiny and extremely dense compared to the volume of an atom
- Neutrons
- Occupy a space somewhere OUTSIDE Nucleus
- Electrons
- -1 Charge
- Relative Mass= 1/2000
- Held in place my an electrostatic force from the nucleus
- Electrons
- Add them together
- Multiply abundance (%) by isotopic masses
- Divide by 100
- Add them together
- Add them together
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