Periodic Trends Activity 3

Objectives Today I will be able to:

Explain why I got multiple choice questions wrong on the electrons exam

Analyze how the trends of atomic radius, ionization energy and electronegativity change across a period and down a family

Compare the atomic radius, ionization energy and electronegativity of 2 or more elements

Informal assessment: monitoring student questions and interactions as we complete the practice and exam corrections

Formal assessment: analyzing the students interpretations of the trends, practice and exit ticket

Common Core Connection Model with mathematics Look for and express regularity in repeated reasoning

Lesson Sequence

Evaluate: Warm – Up Explain: Electrons Exam Corrections Elaborate: Periodicity Practice

Worksheet Elaborate: Applying the trends

worksheet Evaluate: Exit Ticket

Warm - Up

How does the atomic radius change across a period and down a family?

How does electronegativity/ionization energy change across a period and down a family?

Objective

Today I will be able to: Explain why I got multiple choice questions

wrong on the electrons exam Analyze how the trends of atomic radius,

ionization energy and electronegativity change across a period and down a family

Compare the atomic radius, ionization energy and electronegativity of 2 or more elements

Homework

Finish Analyzing the Trends Worksheet

Study for the Multiple Choice Re-quiz at the beginning of next class

Agenda

Warm-Up Electrons Exam Corrections Periodicity Practice Analyzing the trends Worksheet Exit Ticket

Complete the corrections at your desk. Ms. Ose will explain the requirements for the re-quiz next class

Atomic Radius…

Decreases across a period Why?

More protons in the nucleus, pulling the electron cloud closer to the nucleus

Increases down a family Why?

More energy levels for the electrons to fill

Atomic Radius

Ionization Energy

Increases across a period Why?

A greater number of valence electrons makes it more difficult to remove an electron

Decreases down a family Why?

The electrons are farther away from the nucleus. They are less attracted to the atom making them easier to remove

Electronegativity

Increases across a period Why?

Atoms are closer to reaching stability so they want to attract electrons

Decreases down a family Why?

The electrons are farther away from the nucleus in higher energy levels. They are not attracted to the nucleus as easily

Electronegativity

Complete the worksheet using your notes. Ask Ms. Ose for help if you have questions we will review selected problems.

Complete the analyzing the trends worksheet. If you do not finish in class, it will become homework. Be sure to respond to all parts of the question

Exit Ticket

For the following set of elements: Ba Mg O

Circle the element that has the smallest atomic radius

Underline the element with the smallest ionization energy

Box the element with the greatest electronegativity value