Unit 1 Summative Assessment

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Across
  1. 6. Sublevels can be broken down into regions called orbital. An orbital is defined as the most probable location for finding an electron. Each orbital holds 2 electrons.
  2. 7. # of Neutrons = Atomic Mass Number - Atomic Number
  3. 8. Atoms of the same element which have a different Mass Number due to a differing number of neutrons. The symbol for an Isotope is the element symbol followed by the Mass Number, for example: Na-23 and Na-24
  4. 9. Vertical Column on the periodic table. Elements in the same family have similar properties.
  5. 13. A shorthand method of writing the location of electrons by sublevels.
  6. 15. Absorbed when an electron moves from its ground state to its excited state.
  7. 18. Negatively charged subatomic particles. Electrons can be found in the space around the nucleus. This area is often called the electron cloud. Electrons have NO mass.
  8. 21. Positively charged subatomic particle. Contained inside the nucleus. Neutrons and Protons weigh roughly the same (1 atomic mass unit).
  9. 22. Positively Charged Ions. In general, cations are metals.
  10. 24. The center of an atom. Contains the protons and neutrons. Since neutrons have no charge and protons are positively charged, the nucleus has an overall positive charge.
Down
  1. 1. Tendency of an atom to attract electrons to itself when it combines with another element. Electronegativity increases from left to right across a period on the periodic table. Electronegativiy decreases as you go down a group on the periodic table.
  2. 2. Mass Number Also known as the Mass Number or Atomic Mass.
  3. 3. Above groups/families Roman Numerals represent the number of valence electrons. When writing the name of an ionic compound which includes a transition metal a Roman Numeral is used to denote the quantity of positive charge associated with that transition metal.
  4. 4. Size Size of an atom. Depends on the number of energy levels and the overall charge of the nucleus (the nucleus's charge depends on the number of protons). As you go down a group you are adding energy levels (rings around the nucleus) so the atomic size increases. As you go across a period the atomic size decreases because the energy levels (which contain negative electrons) are increasingly attracted to the positive protons in the nucleus of the atom.
  5. 5. Horizontal row on the periodic table.
  6. 10. The possible locations around an atom where electrons having specific energy values (quantum number) may be found. Divided into sublevels s, p, d, and f.
  7. 11. When filling sublevels other than s, electrons are placed in individual orbitals before they are paired up. Electrons fill like people do on a bus. You would never sit right next to someone you do not know if there are free seats available, unless of course all the seats are taken then you must pair up. So, when working with the p sublevel, electrons fill like this...up, up, up....down, down, down...
  8. 12. If there are two electrons in an orbital, they must have opposite (paired) spins.
  9. 14. Shorthand method of writing the location of electrons by orbital.
  10. 16. Neutrally charged subatomic particle. (No charge) Contained inside the nucleus. Neutrons and Protons weigh roughly the same (1 atomic mass unit)
  11. 17. Energy given off in the form of light by an excited electron. Otherwise known as a nquanta of light n.
  12. 19. Principal energy levels are broken down into sublevels designated s, p, d, or f upon which electrons travel.
  13. 20. Atoms or groups of atoms with a charge. To have a charge an atom must have gained or lost electrons. If an atom gains electrons it becomes negatively charged. If an atom loses electrons it will become positively charged.
  14. 23. Negatively charged Ions. Anions are negatively charged because they have gained an electron(s) (electrons are negative). In general, anions are nonmetals.