Chemistry vocabulary

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  1. 3. An atom that has lost one or more electrons. A positively charged ion.
  2. 5. principle: The aufbau principle states that in the ground state (Links to an external site.) of an atom or ion, electrons (Links to an external site.) fill atomic orbitals (Links to an external site.) of the lowest available energy levels (Links to an external site.) before occupying higher levels.
  3. 8. affinity: The change in energy (in kJ/mole) of a neutral atom (in the gaseous phase) when an electron is added to the atom to form a negative ion. In other words, the neutral atom's likelihood of gaining an electron.
  4. 9. gases: Any of the gaseous elements helium, neon, argon, krypton, xenon, and radon, occupying Group 0 (18) of the periodic table. They were long believed to be totally unreactive but compounds of xenon, krypton, and radon are now known. All noble gases have full valance orbitals.
  5. 13. elements: All elements in the s and p blocks of the periodic table. The most abundant elements in the periodic table.
  6. 14. configuration: A simplified version of electron configuration.
  7. 16. radius: The measure of the size of the atom. The larger the atomic radius the larger the size of the atom.
  8. 19. energy: The amount of energy required to remove an electron from a gaseous atom or ion.
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  1. 1. The measure of how hard an atom hold onto its electrons.
  2. 2. configuration: The distribution of the electrons of an atom in the atom's orbitals.
  3. 4. exclusion principle: The quantum mechanical principle which states that two or more identical electrons cannot occupy the same quantum state within a quantum system simultaneously.
  4. 6. The measure of the ease with which an electricity can pas through a material.
  5. 7. Metal families: Alkali metals, Alkali earth metals, Inner transition metal (actinides and lanthanides), transition metals, post- transition metals, metalloids: Follow link.
  6. 10. rule: Every suborbital of a orbital is singly occupied with one electron before any one suborbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.
  7. 11. law: the physical and chemical properties of the elements recur in a systematic and predictable way when the elements (Links to an external site.)are arranged in order of increasingatomic number (Links to an external site.).
  8. 12. Any chemical element that is an effective conductor of electricity and heat can be defined as a metal. A metal is also good at forming bonds and cations with non-metals. Atoms inside of a metal quickly lose electrons in order to make positive ions or cations. The ions in turn are surrounded by the electrons that are delocalized, which give the metal its electric conductivity.
  9. 15. Nonmetal, substance that does not exhibit such characteristic properties ofmetals as hardness, mechanical adaptability, or the ability to conduct electricity.
  10. 17. notation: Orbital notation is a way of writing an electron configuration to provide more specific information about the electrons in an atom of an element. Orbital notation can be used to determine the quantum numbers of an electron.
  11. 18. An atom that has gained one or more electrons. A negatively charged ion.