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Abeka Chemistry: Precision and Design Test 5
Terms in this set (52)
Says physical and chemical properties are periodic functions of their atomic number.
Says when a p, d, or f subshell is being filled, one electron will occupy each orbital before pairing.
Pauli Exclusion Principle
Says no two electrons have the same quantum number.
Says electrons occupy the lowest orbital possible.
Says it is impossible to determine the momentum and position of an electron simultaneously
When an element is vaporized, light forms in a what?
Says light consists of tiny bundles or packets of energy
High point of a wave
Arrangement of all forms of electromagnetic radiation in order of frequency and wavelength
Speed of light in a vacuum
Lowest point in a series of waves
Number of waves that pass a point in a given time
Periodic table columns
Periodic table rows
Distance between two corresponding points on a wave
Lowest energy state
The principle quantum number describes the what?
The magnetic quantum number describes the what?
Unit measuring wave frequency
Maximum number of valence electrons
Electromagnetic Waves, Photons
What light consists of
Amplitude is the measure of a waves what?
Individual packets of light energy
Not an Alkali metal
Most important property of chlorine
Group of elements referred to as "salt formers"
Alkaline Earth Metals
Metals existing as 2+ ions
Photons emitted as electrons drop from higher to lower energy levels
What lines in the hydrogen spectrum represent
Developed the periodic table
As wavelength decreases, frequency must what?
Group 1 elements
Alkaline Earth Metals
Group 2 elements
Group 17 elements
Group 18 elements
Main - Group (Representative)
Groups 1-2, 13-18 elements
Element that rarely undergoes chemical reactions
Formula for bromide of beryllium
Element category including nitrogen, oxygen, and chlorine
Type of halogen
Ion requiring the least energy to form
Know Lewis symbol for phosphorus
Amount of valence electrons in boron
Amount of valence electrons in tin
Determines atoms chemical behavior
Importance for knowing electron configuration
Element category including vandium and platinum
Element with greatest electronegativity
[Ne] 3s^2 2p^2
Electron configuration for Silicon
Product of the reaction between lithium and water
Formula for the Fluoride of Nitrogen
Electron repulsion causes energy overlap between electron shells
Why the 4s orbital fills before the 3d orbital
Smallest atom from the group of atoms
Rutherford: electrons pictured as orbiting nucleus like planets orbiting the Sun replaced because it required electrons to continually radiate energy and spiral inward until they collide with nucleus.
Bohr: electron pictured as orbiting nucleus in circular orbits with energy quantized so that only specific orbits are possible. Model replaced because it could only describe the hydrogen Spectrum. It cannot be used for atoms with more than one electron.
Born: electrons are pictured as moving unpredictably in orbital's, three dimensional regions of varying shape. The energy of electrons is quantized to values corresponding with the orbitals present in the atom.
Compare Rutherford's, Bhors, and Born's model of the atom; include a brief description of the problems that led to the replacement of Rutherford's and Bohr's models.
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