Across
- 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.
- 5. The highly reactive nonmetals in Group 17 that have seven valence electrons and readily gain one electron to form −1 ions.
- 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.
- 10. A horizontal row of the periodic table; elements in the same period have the same number of occupied electron energy levels.
- 13. The overall volume or diameter of an atom, determined largely by the distance of its outermost electrons from the nucleus.
- 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.
- 16. A positively charged ion formed when an atom loses one or more electrons.
- 18. A negatively charged ion formed when an atom gains one or more electrons.
- 19. An element that is typically dull, brittle, and a poor conductor of heat and electricity; nonmetals tend to gain or share electrons.
- 21. An element with properties intermediate between metals and nonmetals, located along the staircase line on the periodic table; often semiconductors.
- 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.
- 23. The energy change that occurs when an atom gains an electron; a measure of how strongly an atom attracts an added electron.
- 24. The distance from the center of an atom's nucleus to the outer edge of its electron cloud; one measure of atomic size.
- 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. The physical law stating that the electrostatic force between two charged particles is dependent on the charge and distance between them.
- 2. The reactive metals in Group 2 that have two valence electrons and readily lose them to form +2 ions.
- 4. The very unreactive gases in Group 18 that have full valence shells, making them stable and chemically inert under normal conditions.
- 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.
- 8. The electrons in an atom that occupy inner energy levels and are not involved in chemical bonding.
- 9. The degree to which an element displays the properties of a metal, such as conductivity, luster, and the tendency to lose electrons.
- 11. The number of protons in the nucleus of an atom, which uniquely identifies the element and determines its position on the periodic table.
- 12. The electrons in the outermost energy level of an atom, which determine its chemical properties and bonding behavior.
- 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).
- 17. The amount of energy required to remove an electron from a gaseous atom or ion.
- 20. The highly reactive metals in Group 1 (excluding hydrogen) that have one valence electron and readily lose it to form +1 ions.