Unit Two: Structure and Properties Flashcards
Emission Spectrum
A characteristic spectrum of distinct, coloured lines that result when excited atoms emit light: can be observed through a spectroscope or a diffraction grating when a high voltage is passed through a gas in a gas tube.
Absorption Spectrum
The spectrum that is produced when electrons of atoms absorb photons of certain wavelengths, causing the electrons to be excited from lower energy levels to higher energy levels.
Orbitals
Solved wave functions that describe a region of probable location of electrons.
Quantum Mechanical Model of the Atom
A model that describes atoms as having certain allowed quantities of energy because of the wave-like properties of their electrons.
Ground State
The most stable energy state.
Principal Quantum Number (n)
A positive whole number (integer) that indicates the energy level and relative size of an atomic orbital.
Magnetic Quantum Number (m1)
An integer that indicates the orientation of an orbital in the space around the nucleus; values range from -1 to +1, including 0.
Pauli Exclusion Principle
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Spin Quantum Number (ms)
The quantum number that specifies the direction in which the electron is spinning with values of +1/2 and -1/3.
Electron Configuration
A shorthand notation that shows the number and arrangement of electrons in an atom’s orbitals.
Aufbau Principle
The principle behind an imaginary process of building up the electron structure of the atoms, in order of atomic number.
Orbital Diagram
A diagram that uses a box for each orbital in any given principal energy level.
Hund’s Rule
The rule stating that the lowest energy state for an atom has the maximum number of unpaired electrons allowed by the Pauli exclusion principle in a given energy sublevel.
Atomic Radius
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Ionization Energy
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Electron Affinity
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Chemical Bonds
The force that holds atoms together in the form of an ionic compound or molecule.
Lattice Energy
The energy that is given off as an ionic crystal forms from the gaseous ions of its elements.
Polar Covalent Bond
A bond in which electrons are unequally shared between two atoms.
Metallic Bond
The force of attraction between positively charged metal atoms, and the pool of valence electrons that moves among them.
Co-ordinate Covalent Bond
A covalent bond in which one atom contributes both electrons to the shared electron pair bond.
Resonance Structures
Two or more Lewis Structures that show the same relative position of atoms but different positions of electron pairs.
Expanded Valence Energy Level
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Valence-Shell Electron-Pair Repulsion Theory
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Dipole
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Intramolecular Forces
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Intermolecular Forces
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Dipole-Dipole Forces
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Ion-Dipole Force
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Ion-Induced Dipole Force
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Dipole-Induced Dipole Force
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Hydrogen Bonding
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Crystalline Solids
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Amorphous Solids
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Atomic Solids
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Network Solids
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Allotropes
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Ionic Crystal
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Dalton’s Model
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Photons
A quantum of electromagnetic energy that has particle-like properties.
