06+Periodic+Table

=Objectives= __Chapter IV: Section I:__ __Chapter IV: Section II:__ __Chapter IV: Section III:__
 * How did chemists begin to organize the known elements?
 * How did Mendeleev organize his periodic table?
 * How is the modern periodic table organized?
 * What are three broad classes of elements?
 * What type of information can be displayed in a periodic table?
 * How can elements be classified based on their electron configurations?
 * What are the trends among the elements for atomic size?
 * How do ions form?
 * What are the trends among the elements for first ionization energy, ionic size, and electronegativity?
 * What is the underlying cause of periodic trends?

=Outlined Notes= A. Searching for an Organizing Principle__** 1.***Chemists used the properties of elements to sort them into groups.** 2. J.W Dobereiner published a classfication system a. //tetrad//- set of 3 elements with similar properties 1.***Menedeleev aranged the elements in his perodic table in order of increasing atomic mass. __C. The Perodic Table__** 1. Menedeleev put some elements out of order because they did not go well with the family of elements. He believed that it was incorrect to put them in the other order. 2. Henry Moseley determined on atomic number for each element 3. ***In the modern perodic table, elements are arranged in order of increasing atomic number.** 4. //Periodic Law//- When elements are arranged in order of increasing atomic number, there is a periodic repeition of their physical and chemical properties. a.***Three classes of elements are metals,nonmetals, and metalloids.** 1.**__Metals__** a. //Metals-// are good conductors of heat and electric current. b. all solids exept mercury. 2.**__Nonmetals__** a. //Nonmetals-// poor conductors of heat and eletric current. Carbon is an exeption to this rule. 3. **__Metalloids__** a. //Metalloids-// hsa properties that are similar of those of metals and nonmetals.
 * __Chapter 6- Section 1-Organizing the Elements
 * __B. Mendeleev's Perodic Table__**
 * __D. Metals,Nonmetals, and Metalloids__**


 * [[image:http://www.schenectady.k12.ny.us/users/title3/Future%20Grant%20Projects/Projects/periodictable/Regions.jpg width="542" height="315"]]

II. Classifying the Elements** //**A.**// Squares in the Periodic Table 1. The periodic table displays the symbols and names of the elements, along with information about the structure of their atoms. 2. The background colors in the squares are used to distinguish groups of elements. a. Two shades of gold are used for the metals inGroups 1A and 2A. b. The Group 1A elements are called alkali metals, and the Group 2A elements are called alkaline earth metals. 3. Some groups of nonmetals have special names. a. The nonmetals in Group 7A are called halogens. 1.Elements can be sorted into noble gases, representative elements, transition metals, or inner transition metals, based in their electron configurations. a. The noble gases are the elements in Group 8A of the periodic table. b. Elements in Groups 1A through 7A are often refered to as representative gases. This is because they display a wide range of physical and chemical properties. c. The transition metals are the Group B elements that are usually displayed in the main body of the periodic table. i. In the atoms of transition metals, the highest occupied //s// sublevel and a nearby //d// sublevel contain electrons. ii. these elements are characterized by the presence of electrons in the //d// orbital. d. The inner transition metals appear below the main body of the periodic table. i. In atoms of an inner transition metal, the highest occupied //s// sublevel and nearby //f// sublevel generally contain electrons. ii. The inner transition metals are characterized by f orbitals that contain electrons. 2. If you consider both the electron configurations and the positions of the elemetnt s in the periodic table, another pattern emerges. a.The periodic table is divided into sections, or blocks, that correspond ti the highest occupied sublevels. 1. The atomic radius is one half the distance between the nuclei of two atoms of the same element when the atoms are joined. 2. In general, atomic size increases from top to bottom within a group and decreases from left to right across a period 3. Grop Trends in Atomic Size a. as the atomic number increases within a group, the charge on the nucleus increases and the number of occupied energy levels increase. b. atomic size increases 4. Periodic Trends in Atomic Size a. In general, atomic size decreases across a period (left to right) b. atomic size decreases 1. an __ion__ is an atom or group of atoms that has a positive or negative charge. 2. Positive and negative ions form when electrons are transferred between atoms a. an ion with a net positive charge is called a __cation__ b. an ion with a net negative charge is called a __anion__ 1. the energy required to remove an electron from anatom is called __ionization energy__ a. measured in gaseous state 2. first ionization energy tends to decrease from top to bottom within a group and increase from left to right across a period a. can help predict which ion elements will form 3. Group Trends in Ionization Energy a. in general, first ionization energy decreases from top to bottomwithin a group. b. As the size of the atom increases, nuclear charge has a smaller effect on the electrons in the highest occupied energy level. i. less energy is required to remove an electron from this energy level and the first ionization energy is lower. 4. Periodic Trends in Ionization Energy a. In general, the first ionization energy of representative elements tend to increase fromleft to right across the period. i. This trend can be explained by the nuclear charge, which increases, and the shielding effect, which remains constant. 1. in reactions between metals and nonmetals, metal atoms tend to lose electrons and nonmetal atoms tend to gain electrons a. cations are always smaller than the atoms from which they form b. anions are always larger than the atoms from which they form c. size generally decreases from top to bottom in groups d. size generally decreases from left to right in periods //**E.**// Trends in Electronegativity 1) __electronegativity__ is the ability of an atom of an element to attract electrons when the atom is in a compound a) Linus Pauling was first to define 2) In general electronegativity values decrease from top to bottom within a group. For representative elements, the values tend to increase from left to right across a period. 1) the trends that exist among these properties can be explained by variations in atomic structure. 2) Increases in shielding have a significant effect.
 * //B.//** Electron Configurations in Groups
 * III. Periodic Trends**
 * //A.//** Trends in Atomic Size
 * //B.//** Ions
 * //C.//** Trends in Ionization Energy
 * //D.//** Trends in Ionic Size
 * //F.//** Summary of Trends

=Reference Pages=




 * **Group 1A** || * Known as Alkali Metals
 * Very reactive
 * Never found free in nature
 * React readily with water ||
 * **Group 2A** || * Known as Alkaline earth elements
 * All are metals
 * Occur only in compounds
 * React with oxygen in the general formula EO (where O is oxygen and E is Group 2A element) ||
 * **Group 3A** || * Metalloids
 * Includes Aluminum (the most abundant metal in the earth)
 * Forms oxygen compounds with a X2O3 formula ||
 * **Group 4A** || * Includes metals and nonmetals
 * Go from nonmetals at the top of the column to metals at the bottom
 * All oxygen form compounds with a XO2 formula ||
 * **Group 5A** || * All elements form an oxygen or sulfur compound with E2O3 or E2S3 formulas ||
 * **Group 6A** || * Includes oxygen, one of the most abundant elements.
 * Generally, oxygen compound formulas within this group are EO2 and EO3 ||
 * **Group 7A** || * Elements combine violently with alkali metals to form salts
 * Called halogens, which mean "salt forming"
 * Are all highly reactive ||
 * **Group 8A** || * Least reactive group
 * All elements are gases
 * Not very abundant on earth
 * Given the name noble gas because they are not very reactive ||

of Electrons ||
 * ~ Subshell ||~ Number of Orbitals ||~ Maximum Number
 * s || 1 || 2 ||
 * p || 3 || 6 ||
 * d || 5 || 10 ||
 * f || 7 || 14 ||

Practice Problems [] **Periodic Jeopardy**

=Assignments=

=Labs=
 * [] Periodic Table Labs**

=Sample Test= Practice Test [] [] [] [] [] []

= = =Links [] Element crossword puzzle[] Element Flash Cards [] Element word scramble [] Element matching game []= ===http://chemistry.about.com/od/k12gradelessons/a/periodictable.htm [|://www.cs.ubc.ca/cgi-bin/nph-pertab/tab/periodic-table http://chemistry.about.com/od/elements/a/memorizeelement.htm http://chemistry.about.com/library/blperiodictablekids.htm]=== =**Extra Tables**= 
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