Chapter Two Vocab Crossword

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Across
  1. 3. The elements in groups 1, 2, and 13–18 (the s-block and p-block), whose valence electrons occupy the outermost s and p orbitals.
  2. 5. The highly reactive nonmetals in Group 17 that have seven valence electrons and readily gain one electron to form −1 ions.
  3. 6. An organizational chart of all known elements, arranged in order of increasing atomic number, with elements placed in columns (groups) and rows (periods) based on similar chemical properties.
  4. 10. A horizontal row of the periodic table; elements in the same period have the same number of occupied electron energy levels.
  5. 13. The overall volume or diameter of an atom, determined largely by the distance of its outermost electrons from the nucleus.
  6. 15. An element that is typically shiny, malleable, ductile, and a good conductor of heat and electricity; metals tend to lose electrons and form positive ions.
  7. 16. A positively charged ion formed when an atom loses one or more electrons.
  8. 18. A negatively charged ion formed when an atom gains one or more electrons.
  9. 19. An element that is typically dull, brittle, and a poor conductor of heat and electricity; nonmetals tend to gain or share electrons.
  10. 21. An element with properties intermediate between metals and nonmetals, located along the staircase line on the periodic table; often semiconductors.
  11. 22. The reduction in the attractive force between the nucleus and outer (valence) electrons caused by inner (core) electrons blocking some of the nuclear charge.
  12. 23. The energy change that occurs when an atom gains an electron; a measure of how strongly an atom attracts an added electron.
  13. 24. The distance from the center of an atom's nucleus to the outer edge of its electron cloud; one measure of atomic size.
  14. 25. A predictable pattern in a periodic property (such as atomic radius or ionization energy) that changes gradually across a period or down a group due to atomic structure
Down
  1. 1. The physical law stating that the electrostatic force between two charged particles is dependent on the charge and distance between them.
  2. 2. The reactive metals in Group 2 that have two valence electrons and readily lose them to form +2 ions.
  3. 4. The very unreactive gases in Group 18 that have full valence shells, making them stable and chemically inert under normal conditions.
  4. 7. A vertical column of the periodic table; elements in the same group have the same number of valence electrons and share similar chemical properties.
  5. 8. The electrons in an atom that occupy inner energy levels and are not involved in chemical bonding.
  6. 9. The degree to which an element displays the properties of a metal, such as conductivity, luster, and the tendency to lose electrons.
  7. 11. The number of protons in the nucleus of an atom, which uniquely identifies the element and determines its position on the periodic table.
  8. 12. The electrons in the outermost energy level of an atom, which determine its chemical properties and bonding behavior.
  9. 14. The net positive charge experienced by a valence electron, equal to the actual nuclear charge minus the shielding effect of core electrons (Zeff ≈ Z − S).
  10. 17. The amount of energy required to remove an electron from a gaseous atom or ion.
  11. 20. The highly reactive metals in Group 1 (excluding hydrogen) that have one valence electron and readily lose it to form +1 ions.