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Abeka Chemistry: Precision and Design Test 5

Terms in this set (52)

Periodic Law
Says physical and chemical properties are periodic functions of their atomic number.
Hund's Rule
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.
Aufbau Principle
Says electrons occupy the lowest orbital possible.
Uncertainty Principle
Says it is impossible to determine the momentum and position of an electron simultaneously
Line Spectrum
When an element is vaporized, light forms in a what?
Quantum Theory
Says light consists of tiny bundles or packets of energy
Crest
High point of a wave
Electromagnetic Spectrum
Arrangement of all forms of electromagnetic radiation in order of frequency and wavelength
3.00×10^8 m/s
Speed of light in a vacuum
Trough
Lowest point in a series of waves
Frequency
Number of waves that pass a point in a given time
Groups
Periodic table columns
Periods
Periodic table rows
Wavelength
Distance between two corresponding points on a wave
Ground State
Lowest energy state
Electron Shell
The principle quantum number describes the what?
Orbital Orientation
The magnetic quantum number describes the what?
Hertz
Unit measuring wave frequency
Eight
Maximum number of valence electrons
Electromagnetic Waves, Photons
What light consists of
Strength
Amplitude is the measure of a waves what?
Photons
Individual packets of light energy
Calcium
Not an Alkali metal
Electron Affinity
Most important property of chlorine
Halogens
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
Dmitri Mendeleev
Developed the periodic table
Increase
As wavelength decreases, frequency must what?
Alkali Metals
Group 1 elements
Alkaline Earth Metals
Group 2 elements
Halogens
Group 17 elements
Noble Gasses
Group 18 elements
Main - Group (Representative)
Groups 1-2, 13-18 elements
Argon
Element that rarely undergoes chemical reactions
BeBr^2
Formula for bromide of beryllium
Non-metals
Element category including nitrogen, oxygen, and chlorine
Iodine
Type of halogen
Na+
Ion requiring the least energy to form
...
Know Lewis symbol for phosphorus
Three
Amount of valence electrons in boron
Four
Amount of valence electrons in tin
Determines atoms chemical behavior
Importance for knowing electron configuration
Transition Metals
Element category including vandium and platinum
Fluorine (F)
Element with greatest electronegativity
[Ne] 3s^2 2p^2
Electron configuration for Silicon
LiOH
Product of the reaction between lithium and water
NF^3
Formula for the Fluoride of Nitrogen
Electron repulsion causes energy overlap between electron shells
Why the 4s orbital fills before the 3d orbital
Sulfur (S)
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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