Atomic theory and periodic trends Flashcards
Father of the modern atomic theory.
John Dalton
Building blocks of matter
Atoms
Who discovered electrons?
Joseph John Thomson
Who discovered protons?
Ernest Rutherford
Who discovered Neutrons?
James Chadwick
Electrons are discovered through observation of the ______________.
cathode ray tube
Protons are discovered through ________________.
gold foil experiment
Weight of the nucleus
atomic mass
Atoms of the same element with different number of neutrons
Isotopes
Unstable isotopes that tend to decay often by emitting certain type of radiation.
Radioactive isotopes
A Danish physicist that said electrons are not stationary and created the planetary model.
Neils Bohr
State where an atom has the lowest energy arrangement of electrons
Ground state
Atom that absorbs energy through heat and electricity.
Excited state
An Austrian physicist that said the behavior of electrons within an atom can be explained by treating it as matter waves.
Erwin Schrodinger
Region surrounding the nucleus where electrons are found.
Orbital
A wave function for an electron in an atom
atomic orbital
specifies the energy of an electron and the size of the orbital
Principal quantum number
specifies the shape of an orbital within a particular principal quantum number
Angular momentum quantum number
Orientation in space
Magnetic quantum number
Describes the spin of an electron
Spin quantum number
The order in which electrons are placed into the orbitals is based on the order of their energy.
Aufbau principle
Distance between the nucleus and the outermost electron.
Atomic radius
Energy required to remove an electron from its valence shell.
Ionization energy
ability to attract electrons
electronegativity
Ability to accept electrons
electron affinity
ability to lose electrons
metallic character
electrically charged atoms
ions
who created the nuclear model?
Ernest Rutherford
Who created the plum pudding model?
Joseph John Thomson
Symbol for atomic number
Z
Symbol for atomic mass
M
The formula used to determine the number of electrons in an energy orbital.
2n^2
