Honors: Unit 2 : Periodic Table and Trends Study Guide

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1 Name: Date: Period: Honors: Unit 2 : Periodic Table and Trends Study Guide Objectives to Study: Any objectives from previous assessments can possibly be on the test :-) Names of groups and their properties on the Periodic Table - Chart with Colored PT on Back Predicted Charges and number of valence electrons for those groups - Chart with Colored PT on Back Properties/Characteristics/Location of the Periodic Table for Metals, Nonmetals, and Metalloids Definitions and Trends of Nuclear Charge, Shielding, Atomic Radius, Ionization Energy, and Electronegativity (2.2 Notes) Know how to read graphs for ionization energy, electronegativity, atomic radius, and phase changes Be able to explain electronegativity, ionization energy, and atomic radius using electron shielding and nuclear charge*** Identify characteristics of solids, liquids and gases (States of Matter Review) Name/Identify each phase change and state of matter (States of Matter Review) Know the difference between physical and chemical properties and changes (Foldable) Relate particle motion to temperature, energy, and state of matter (States of Matter Review) Understanding the Periodic Trends: Name Definition Trend Down Groups Trend Across Periods Effective Nuclear Charge Shielding Atomic Radius Ionic Radius Reactivity 1st Ionization Energy Electronegativity As you move DOWN the periodic table, Shielding because you have more which reduces the attraction of the to the electrons. What is the trend for electronegativity as you move across the periodic table from left to right? EXPLAIN why!

2 Metals, Nonmetals, and Metalloids: Know where they are found on the periodic table Type of Atom Characteristics Metal Nonmetal Metalloid Fill out the table below using a drawing and words to explain the difference between atoms and their ions in terms of size. Atoms vs. Anions Atoms vs. Cations Complete the following table by calculating Z eff Show your work within the table a. Write the formula. Argon Rubidium Work for calculating Z eff Answer - Z eff How many valence electrons do the following elements have? a. Oxygen (O) c. Sodium (Na) b. Carbon (C) d. Bromine (Br)

3 In the table below, compare Lithium and Potassium. Circle the correct term to explain which element is higher or lower for that particular trend. Lithium Potassium Reactivity HIGHER or LOWER HIGHER or LOWER Ionization energy HIGHER or LOWER HIGHER or LOWER Atomic Radius HIGHER or LOWER HIGHER or LOWER Electronegativity HIGHER or LOWER HIGHER or LOWER Shielding HIGHER or LOWER HIGHER or LOWER Nuclear Charge HIGHER or LOWER HIGHER or LOWER States of Matter Characteristics Particle Diagram (What it looks like) Motion (Relative Speed) Shape and Volume Density (High, Medium, Low) Solid Liquid Gas Draw a visual diagram to show all of the ways that a substance can pass from solid to liquid to gas. Explain how shielding affects reactivity for metals and for nonmetals. Write the equation for 1st ionization energy below:

In the Atomic Radius graph below, highlight period 2, period 3, and period 4 each in different colors. a. Describe the atomic radius trend for each period by relating it to how shielding and nuclear charge effect the size of an atom.

occurred) Using the table to the right, answer the questions below: Which group has a predicted charge of 0? An element from which group gains 1 electron when it forms its common ion?

4 In the Atomic Radius graph below, highlight period 2, period 3, and period 4 each in different colors. a. Describe the atomic radius trend for each period by relating it to how shielding and nuclear charge effect the size of an atom. Complete the chart by writing what each means as well as providing a few examples: Physical Properties Chemical Properties Physical Changes Chemical Changes (include ways to tell if a reaction has occurred) Using the table to the right, answer the questions below: Which group has a predicted charge of 0? An element from which group gains 1 electron when it forms its common ion? Which group possesses the most reactive metals? Which group(s) has/have metals that can form multiple charges? Between the Alkali Metals and Halogens, which would have the smaller atomic radius?

5 Use the graph above to answer parts A through E. a. In the graph above, draw a circle around Fluorine and a circle around Chlorine. b. Which element has the higher ionization energy between them? c. Explain why that element has a higher ionization energy by explaining the difference between the shielding for Fluorine and Chlorine. d. In the graph above, draw a square around Rubidium and a square around Iodine. e. Between Rubidium and Iodine, which has a higher nuclear charge? Given the two elements Na and S which element has greater Ionization Energy? EXPLAIN why! Label the states of matter and phase changes in the graph on the right. a. What processes are occurring at #2 and at #4? b. How is the energy of the material changing over time? c. What is the relationship between temperature and energy of the particles in a substance?

6 Match the group of elements with the correct description of its properties : 1. Alkali Metals 3. Alkaline Earth Metals 2. Noble Gases 4. Halogens Colorless gases; completely unreactive; 8 valence electrons Harder than Group 1 elements; very reactive; 2 valence electrons HIGHLY reactive; soft metals; 1 valence electron HIGHLY reactive; three gases, a liquid, and a solid; 7 valence electrons Using the answer choices in the question above (1-4), label the groups of the periodic table below. Then, label the sublevel blocks (s,p,d, and f):

Name Date Class ORGANIZING THE ELEMENTS

Name Date Class ORGANIZING THE ELEMENTS 6.1 ORGANIZING THE ELEMENTS Section Review Objectives Explain how elements are organized in a periodic table Compare early and modern periodic tables Identify three broad classes of elements Vocabulary