Atomic structure, isotopes, compounds, formulae and equations Flashcards
Atomic number
The number of protons in the nucleus of an atom.
Bohr Model
Describes an atom as a small dense nucleus with electrons orbiting around the nucleus. This model explains different periodic properties of atoms.
Electron
Negatively charged sub atomic particle.
Relative mass- 1/1836.
Isotopes
Atoms of the same element with the same number of protons and electrons but different numbers of neutrons. Isotopes of an element have different masses.
Mass number
The total number of protons and neutrons in the nucleus of an atom.
Mass spectrometry
An instrument which gives accurate information about relative isotopic mass and the relative abundance of isotopes.
Neutron
Neutral subatomic particle.
Relative mass- 1.
Proton
Positively charged subatomic particle.
Relative mass-1.
Relative abundance
The amount of one substance compared with another.
Relative atomic mass
The weighted mean mass of an atom compared with 1/12th mass of an atom of carbon 12.
Relative isotopic mass
The mass of an atom of an isotope compared with 1/12th of an atom of carbon-12.
Relative formula mass
The mass of the formula unit of a compound with a giant structure. For example NaCl has a relative formula mass of 58.44z
Relative molecular mass (Mr)
The mass of a simple molecule.