SAT Chemistry Test Strategy: How to Use the Periodic Table

Instructions:

Choose an answer and hit 'next'. You will receive your score and answers at the end.

question 1 of 3

Considering the trend for ionization energy on the periodic table, which of the following elements has the highest ionization energy?

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1. Why does cesium (Cs) have a larger atomic radius than lithium (Li)?

2. Which of the following families are an exception to the periodic trend rule?

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About This Quiz & Worksheet

The periodic table is more than just a list of known elements. In fact, there is a lot you can learn about an element based solely on where it lies on the periodic table. Complete this assessment to test your understanding of a few of the many uses of the periodic table.

Quiz & Worksheet Goals

With this brief assessment, you will test your understanding of:

  • Trends for ionization energy on the periodic table
  • The reason that cesium has a larger atomic radius than lithium
  • Exceptions to the periodic trend rule
  • Determining the electronegativity of atoms
  • Periodic classifications

Skills Practiced

A few of the basic skills you will use to complete this assessment include:

  • Interpreting information - verify that you can read information regarding uses of the periodic table and interpret it correctly
  • Information recall - access the knowledge you've gained regarding information you can learn about an element that has the highest ionization energy
  • Knowledge application - use your knowledge to answer questions about various elements

Additional Learning

To learn more about the periodic table, complete the lesson, SAT Chemistry Test Strategy: How to Use the Periodic Table. Through this lesson, you will study:

  • Uses of periods and groups on the periodic table
  • The three basic classifications of elements
  • Where you can find the atomic number, atomic symbol an atomic mass of an element
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