Unit 3: Periodic Table Notes Packet - Gardencity.k12.ny.us

Unit 3: Periodic Table Notes Packet You will be expected to always have your notebook for diagrams and note taking that is supplementary to the note sheets.

Name: Date: Introduction to the Periodic Table, Metals, Nonmetals and Metalloids Aim: How is the Periodic Table arranged and what patterns emerge among the elements? Do Now: Please examine how the periodic table is arranged and with the person next to you, find as many patterns as you can. Periodic Law: Organization of the Table Groups 1-18: Periods 1-7: Groups Elements in the same group have the: Periods Elements in the same period have the 1

Name: Date: Introduction to the Periodic Table, Metals, Nonmetals and Metalloids Dmitri Mendeleev: Father of the Periodic Table Mendeleev organized the periodic table by listing elements in rows by increasing atomic mass. He also put them in groups by reactivity. Mendeleev’s table was close to the table we use today. Mendeleev’s Table Modern Table Arranged elements by mass Ordered elements in groups by reactivity The boron staircase is the dividing line for metals and nonmetals. Metals, Nonmetals and Metalloids Metals . IT IS ONLY IN GROUP 1 BECAUSE IT HAS 1 VALENCE ELECTRON. Nonmetals Metalloids Metalloid elements: 2

Name: Date: Introduction to the Periodic Table, Metals, Nonmetals and Metalloids Properties of Metals, Nonmetals and Metalloids Aim: How do the properties of metals and nonmetals differ? Metal Properties All metals are solids except for mercury which is a liquid. 1. 2. 3. 4. 5. Nonmetal Properties The nonmetals exist as mostly gases, some solids and 1 liquid (Bromine) 1. 2. 3. 4. 5. Metalloid Properties Metalloids can behave as a metal or a nonmetal, depending upon what type of element they are reacting with. 1. 2. 3. 4. 5. 3

Name: Date: Introduction to the Periodic Table, Metals, Nonmetals and Metalloids Metallic and Nonmetallic Character 4

Aim: What are the properties of the representative element groups in the periodic table? Do Now: 1. Write the electron configuration for ATOM of the element below. 2. Write the electron configuration for its ION form. 3. Identify the noble gas electron configuration it matches when forming its’ ion. Atom Ion symbol symbol w/ charge Atom’s e- configuration from periodic table Ion’s e- configuration after Noble gas match e- were lost/gained Mg Mg2 Sr Sr2 Why do elements in the same group have similar physical and chemical properties? Groups of the Periodic Table The representative elements are found in groups 1,2 and 13-18. The transition metals are a shorter block of columns. These elements stand out from the other groups because they do not follow the same patterns and trends with their valence electrons and reactivities. Properties of Transition Metals Groups 3-12 Electrons: Ions: Reactivity: 5

Properties of the Representative Element Groups of the Periodic Table Group 1: Properties: Electrons and Ions: Ionization energy and Electronegativity: Reactivity: General Reactivity of Metals Group 2: Properties: Electrons and Ions: Ionization energy and Electronegativity: Reactivity: 6

Group 17: Properties: Electrons and Ions: Ionization energy and Electronegativity: Reactivity: Phases: General Reactivity of Nonmetals Group 18: Properties: Electrons and Ions: Ionization energy and Electronegativity: Reactivity: 7

Aim: To explain the trends in atomic radius, electronegativity and ionization energy in terms of nuclear charge and nuclear shielding. Definitions: 1. Electronegativity: 2. Ionization energy: 3. Atomic radius: 4. Nuclear charge: 5. Nuclear shielding: 8

Answer the following questions using your reference tables and knowledge of chemistry. A. Trends across a period: Complete the missing information for the elements below: Lithium Fluorine Ionization Energy Electronegativity Atomic Radius Electron Configuration # of Occupied PEL’s Nuclear Charge 1. In general, state what happens to each of the following properties as you move across period 2 (indicate if it increases or decreases) a. Ionization energy: b. Electronegativity: c. Atomic Radius: 2. Why is the nuclear charge of Fluorine greater than the nuclear charge of Lithium? 3. Explain, in terms of nuclear charge, why Fluorine has a greater electronegativity AND ionization energy than Lithium? 4. Explain, in terms of nuclear charge, why Fluorine pulls it’s 2 principle energy levels in closer and has a SMALLER atomic radius than lithium? 9

B. Trends down a Group: Complete the missing information for the elements to the left: 5. In general, state what happens to each of the following properties as you move down Group 1 (indicate if it increases or decreases) a. Ionization energy: b. Electronegativity: c. Atomic Radius: 6. Explain, in terms of atomic structure, why Francium has a larger atomic radius than Lithium? 7. What happens to the amount of nuclear shielding (electrons blocking the nucleus) for an element when you move down a group? Explain in terms of number of electrons and principle energy levels. 8. Why is it easier to remove a valence electron from Francium than from Lithium? Explain your answer in terms of nuclear shielding and electron shells. 9. Why does Francium have a lower electronegativity than Lithium? Explain your answer in terms of nuclear shielding and electron shells. 10

Electronegativity, ionization energy and atomic radius down a Group Atomic radius The electronegativity and ionization energy Electronegativity, ionization energy and atomic radius across a Period The electronegativity and ionization energy Atomic radius 11

Introduction to the Periodic Table, Metals, Nonmetals and Metalloids 2 Dmitri Mendeleev: Father of the Periodic Table Mendeleev organized the periodic table by listing elements in rows by increasing atomic mass. He also put them in groups by reactivity. Mendeleev's table was close to the table we use today.