• Shuffle
    Toggle On
    Toggle Off
  • Alphabetize
    Toggle On
    Toggle Off
  • Front First
    Toggle On
    Toggle Off
  • Both Sides
    Toggle On
    Toggle Off
  • Read
    Toggle On
    Toggle Off

Card Range To Study



Play button


Play button




Click to flip

Use LEFT and RIGHT arrow keys to navigate between flashcards;

Use UP and DOWN arrow keys to flip the card;

H to show hint;

A reads text to speech;

24 Cards in this Set

  • Front
  • Back
Dmitri Mendeleev
the creator of the first version of the periodic table of elements. Using the table, he predicted the properties of elements yet to be discovered
Periods on the Periodic Table
Groups on the Periodic Table
Noble Gas
the elements in the farthest right column of the periodic table; have a full octet which makes them very stable and un-reactive
Emission Spectra
the spectrum of frequencies of electromagnetic radiation emitted by the element's atoms or the compound's molecules when they are returned to a lower energy state
Neils Bohr
1) electrons travel in discrete orbits around the atom's nucleus
2) chemical properties of an element are determined by the electrons in the outermost orbit
Energy Level
the various places of different amounts of energy that can host electrons
Heisenberg Uncertainty Principle
the velocity and position of an electron cannot be known at the same time
the "spherical" shapes hold the electrons surrounding the nucleus
Electron Configuration
the arrangement of electrons of an atom, a molecule, or other physical structure. It concerns the way electrons can be distributed in the orbitals of the given system
Ionization Energy Increases
Moving Left --> Right
Atomic Radius Decreases
Moving Left --> Right
Electronegativity Increases
Moving Left --> Right
Electronegativity Decreases
Moving Top --> Bottom
Ionization Energy Decreases
Moving Top --> Bottom
Atomic Radius Increases
Moving Top --> Bottom
Valence Electrons
the electrons occupying the orbital of the highest energy level for each orbital type
Octet Rule
states that atoms tend to combine in such a way that they each have eight electrons in their valence shells, giving them the same electronic configuration as a noble gas
Ionic Bonds
type of chemical bond formed through electrostatic attraction between two oppositely charged ions
Properties of Ionic Compounds
High Boiling and Melting points
Properties of Molecular (Covalent) Compounds
- Low Melting and Boiling Points
- liquids and gases at room temp.
VSEPR Theory
because of the similar charges of electron orbitals, they repel each other and form 3D configurations
Ionization Energy
the energy needed to remove electrons from an atom
describes the tendency of an atom or a functional group to attract electrons (or electron density) towards itself and thus the tendency to form negative ions