Unit 4B For each unit you are to complete Vocabulary Cards for the 10 required vocabulary words. Reading guides are found online at http://titanchem.wikispaces.com/Notes+and+Documents as are extra notes and power point presentations. For extra problems CYNTK Practice will be found in the CYNTK book at http://titanchem.wikispaces.com/KH+Chemistry+Textbook. Each chapter is a separate document in pdf format. The practice for each section is found at the end of the section.

Unit / KH CYNTK Section / Glencoe Pages / North Carolina Essential Standard / Student Objectives / Unit Vocabulary
Glowing Things Unit 4b / 4.4 / 151-157, 159-161 / 1.3.1• / o  Identify groups as vertical columns on the periodic table.
o  Know that main group elements in the same group have similar properties, the same number of valence electrons, and the same oxidation number.
o  Identify periods as horizontal rows on the periodic table.
o  Identify regions of the periodic table where metals, nonmetals, and metalloids are located.
o  Classify elements as metals/nonmetals/metalloids based on location.
o  Identify representative (main group) elements as A groups or as groups 1, 2, 13-18.
o  Identify alkali metals, alkaline earth metals, halogens, and noble gases based on location on periodic table.
o  Identify transition elements as B groups or as groups 3-12. / Required Vocabulary
1.  Ionization energy
2.  Electronegativity
3.  Atomic radius
4.  Ionic radius
5.  Group/Family
6.  Period
7.  Octet rule
8.  Periodic Law
9.  Transition element
10.  Representative element
Other Vocabulary
11.  Metal
12.  Nonmetal
13.  Metalloid
14.  Alkali metals
15.  Alkaline earth metals
16.  Inner transition metals
17.  Halogens
18.  Noble gases
19.  Electromagnetic spectrum
20.  Electromagnetic radiation
21.  Electromagnetic wave
22.  Frequency
23.  Emission spectrum
24.  Absorption spectrum
25.  Ground state
26.  Excited state
4.5 / 163-169 / 1.3.1•
1.3.2. / o  Summarize that reactivity increases as you go down within a group for metals and decreases for nonmetals.
o  Define atomic radius and ionic radius
o  Know group and period general trends for atomic radius
o  Apply trends to arrange elements in order of increasing or decreasing atomic radius. Explain the reasoning behind the trends.
o  Compare cation and anion radius to neutral atom.
o  Compare the metallic character of elements.
o  Use electron configuration and behavior to justify metallic character. (Metals tend to lose electrons in order to achieve the stability of a filled octet.)
o  Relate metallic character to ionization energy, electron affinity, and electronegativity.
o  Write electron configurations, including noble gas abbreviations (no exceptions to the general rules). Included here are extended arrangements showing electrons in orbitals.
o  Define ionization energy and know group and period general trends for ionization energy. Explain the reasoning behind the trend.
o  Apply trends to arrange elements in order of increasing or decreasing ionization energy.
o  Define electronegativity and know group and period general trends for electronegativity. Explain the reasoning behind the trend.
o  Apply trends to arrange elements in order of increasing or decreasing electronegativity.
4.6/4.7 / 117-120 / 1.1.3•. / o  Understand that energy exists in discrete units called quanta
o  Describe the concepts of excited and ground state of electrons in the atom: 1. When an electron gains an amount of energy equivalent to the energy difference, it moves from its ground state to a higher energy level. 2. When the electron moves to a lower energy level, it releases an amount of energy equal to the energy difference in these levels as electromagnetic radiation (emissions spectrum).
o  Articulate that this electromagnetic radiation is given off as photons.
o  Understand the inverse relationship between wavelength and frequency, and the direct relationship between energy and frequency.
o  Use the “Bohr Model for Hydrogen Atom” and “Electromagnetic Spectrum” diagrams from the Reference Tables to relate color, frequency, and wavelength of the light emitted to the energy of the photon.
o  Describe the wave/particle duality of electrons.