Advanced Chemistry

Name: ____________________

Period: _____ Date: _______ Chapter 6: Periodic Table California Standards: Atomic and Molecular Structure 1. The periodic table displays the elements in increasing atomic number and shows how periodicity of the physical and chemical properties of the elements relates to atomic structure. As a basis for understanding this concept: a. Students know how to relate the position of an element in the periodic table to its atomic number and atomic mass. b. Students know how to use the periodic table to identify metals, semimetals, nonmetals, and halogens. c. Students know how to use the periodic table to identify alkali metals, alkaline earth metals and transition metals, trends in ionization energy, electronegativity, and the relative sizes of ions and atoms. d. Students know how to use the periodic table to determine the number of electrons available for bonding.

6.1 Organizing the elements I. Searching for an Organizing Principle A. How did chemists begin to organize the known elements? 1. Chemists used the _________________ of elements to sort them into groups. e.g: Chlorine, bromine, and iodine have very similar chemical properties. B. How is the modern periodic table organized? 1. In the modern periodic table, elements are arranged in order of ________________ __________________________________. 2. The Periodic Law -

3. The properties of the elements within a period ______________ as you move across a period from left to right. 4. The pattern of properties within a period ________________ as you move from one period to the next. II. Metals, Nonmetals and Metalloids A. The periodic table is organized into 3 broad classes of elements. These are 1. ___________________ 2.____________________3.__________________ Across a period, the properties of elements become _______________________ _____________________________________.

1

B. Properties of metals a. b. c. Examples of metals are: C. Properties of nonnmetals a. b. c. d. One nonmetal, bromine, is a dark-red ______________ D. Properties of metalloids a. A metalloid generally has properties that are _____________ those of metals and nonmetals. b. The behavior of a metalloid can be controlled by changing conditions. III. What type of information can be displayed in a periodic table? A. Squares in the Periodic Table 1. Each square in the periodic table displays the symbols and names of the elements, along with information about the structure of their atoms.

2

B. The horizontal rows of the periodic table are called __________________ C. The vertical columns are called ______________________ D. Some element groups have special names. 1. The Group 1A elements are called ______________________ 2. The Group 2A elements are called ______________________ 3. The nonmetals of Group 7A are called ___________________ 4. The elements in group 8A are called ____________________ 5. Representative elements are in groups __________________ 6. Transition elements are in groups ______________________

6.2 Relating Electron Configurations to Groups I. Electron Configurations in Groups A. Elements can be sorted into noble gases, representative elements, transition metals, or inner transition metals based on their electron configurations. 1. He – Ne – Ar – Kr – 2. The Representative Elements Elements in __________________________ are often referred to as representative elements because they display a wide range of physical and chemical properties. 3. For these elements, the ______and _______sublevels of the highest occupied energy level are not completely filled. 4. The group number is equal to the ____________________________ ___________________________________.

3

Electron Configurations Group IA elements: Li – Na – KIn atoms of the Group 1A elements, there is only ______ electron in the highest occupied energy level. Group IV A elements: C– Si – Ge – Sn In atoms of the Group 4A elements, there are ______ electrons in the highest occupied energy level. 5. Transition Elements: There are two types of transition elements— a. b. They are classified based on their electron configurations. 6.3 Trends in Atomic Size A. Atomic Radius B. In general, atomic size 1. __________________________from top to bottom within a group 2. __________________________ from left to right across a period.

4

C. Ion 1. Cation 2. Anion D. During reactions between metals and nonmetals, 1. Metal atoms tend to ____________ electrons to form cations 2. Nonmetal atoms tend to ____________ electrons to form anions. 3. The transfer has a predictable effect on the size of the ions that form. E. Trends in Ionic Size 1. Cations are always ________________than the atoms from which they form. 2. Anions are always _________________ than the atoms from which they form. Examples: Relative Sizes of Some Atoms and Ions

5

F. Trends in Ionic Size

G. Trends in Ionization Energy 1. Ionization energy – 2. Group and Periodic Trends in Ionization Energy a) Ionization energy ________________ from top to bottom within a group b) It ____________________________ from left to right across a period.

H. Trends in Electronegativity 1. Electronegativity 2. Electronegativity values a) ___________________from top to bottom within a group. b)

from left to right across a period.

6

Check Your Understanding. 1. The modern periodic table has elements arranged in order of a) colors. b) melting and boiling points. c) increasing atomic mass. d) increasing atomic number. 2. Which one of the following is NOT a general property of metals? a) ductility b) malleability c) having a high luster d) poor conductor of heat and electricity 3. Which of the following information about elements is usually NOT included in a periodic table? a) color b) symbol c) atomic number d) atomic mass 4. Which one of the following is incorrectly labeled? a) Ne, noble gas b) Cu, transition metal c) Ga, transition metal d) Cl, halogen 5. Transition metals are characterized as being different than representative elements because they have electrons in which suborbitals? a) p b) d c) s d) f 6. Which of the following sequences is correct for atomic size? Mg > Al > S Li > Na > K F>N>B F > Cl > Br 7. Metals tend to a) gain electrons to form cations. b) gain electrons to form anions. c) lose electrons to form anions. d) lose electrons to form cations. 8. Which of the following is the most electronegative? a) Cl b) Se c) Na

d) I

7