4.2 Periodic Table Properties: Core Charge and Atomic Radius

Last updated over 3 years ago

18 questions

This is also posted on ActivelyLearn.com if you would like to take notes on the reading, use audio or receive translations for this.

View the Model 3 video to help you with this part. 

View the Model 4 video to help you with this part. 

List at least 2 patterns that you notice from the data table and Periodic Table showing the atomic radius of elements.

Use what you know about atomic structure, core charge and atomic radius patterns to explain a possible reason for why the sizes of cations are different than the sizes of anions.

4.2 Periodic Table Properties: Core Charge and Atomic Radius

4.2 Periodic Table Properties: Core Charge and Atomic Radius

List at least 2 patterns that you notice from the data table and Periodic Table showing the atomic radius of elements.

Use what you know about atomic structure, core charge and atomic radius patterns to explain a possible reason for why the sizes of cations are different than the sizes of anions.

Draw a Bohr Diagram of Be

Draw a Bohr Diagram of B.

Describe any patterns or trends you notice about the number of valence electrons and core charge as you go acrossa period on the periodic table.

Click on Edit Background to answer question 13.

List at least 2 patterns that you notice from the data table and Periodic Table showing the atomic radius of elements.

Go Back to question 13 and add at least 1 additional Reason to explain why the claim you chose is true.

Use what you know about atomic structure, core charge and atomic radius patterns to explain a possible reason for why the sizes of cations are different than the sizes of anions.

Which of the following are true? Select all that apply

The strength of the electrostatic force of attraction within atoms is between the positively charged and negatively charged ____.

If an element has a greater core charge it will have a ____________ electrostatic attraction holding the protons and electrons together within the atom.

Draw a Bohr Diagram of Be

Drag the correct number under each category for the valence electrons and core charge for Be.

Draw a Bohr Diagram of B.

Drag the correct number under each category for the valence electrons and core charge for B.

Drag the correct number of valence electrons and core charge for each element.

Describe any patterns or trends you notice about the number of valence electrons and core charge as you go acrossa period on the periodic table.

Drag the numbers to each term below to determine the # of energy levels/shells, valence electrons and core charge for Ne

Drag the numbers to each term below to determine the # of energy levels/shells, valence electrons and core charge for Na

Click on Edit Background to answer question 13.

Why does sodium (Na) have a much larger atomic radius than argon (Ar) even though they are in the same period? CHOOSE THE BEST OPTON.

Go Back to question 13 and add at least 1 additional Reason to explain why the claim you chose is true.

Compare the sizes of positive cations to the sizes of negative anions.

4.2 Periodic Table Properties: Core Charge and Atomic Radius

4.2 Periodic Table Properties: Core Charge and Atomic Radius

List at least 2 patterns that you notice from the data table and Periodic Table showing the atomic radius of elements.

Use what you know about atomic structure, core charge and atomic radius patterns to explain a possible reason for why the sizes of cations are different than the sizes of anions.

Draw a Bohr Diagram of Be

Draw a Bohr Diagram of B.

Describe any patterns or trends you notice about the number of valence electrons and core charge as you go acrossa period on the periodic table.

Click on Edit Background to answer question 13.

List at least 2 patterns that you notice from the data table and Periodic Table showing the atomic radius of elements.

Go Back to question 13 and add at least 1 additional Reason to explain why the claim you chose is true.

Use what you know about atomic structure, core charge and atomic radius patterns to explain a possible reason for why the sizes of cations are different than the sizes of anions.

Which of the following are true? Select all that apply

The strength of the electrostatic force of attraction within atoms is between the positively charged ______________ and negatively charged __________________.

If an element has a greater core charge it will have a ____________ electrostatic attraction holding the protons and electrons together within the atom.

Draw a Bohr Diagram of Be

Drag the correct number under each category for the valence electrons and core charge for Be.

Draw a Bohr Diagram of B.

Drag the correct number under each category for the valence electrons and core charge for B.

Drag the correct number of valence electrons and core charge for each element.

Describe any patterns or trends you notice about the number of valence electrons and core charge as you go acrossa period on the periodic table.

Drag the numbers to each term below to determine the # of energy levels/shells, valence electrons and core charge for Ne

Drag the numbers to each term below to determine the # of energy levels/shells, valence electrons and core charge for Na

Click on Edit Background to answer question 13.

Why does sodium (Na) have a much larger atomic radius than argon (Ar) even though they are in the same period? CHOOSE THE BEST OPTON.

Go Back to question 13 and add at least 1 additional Reason to explain why the claim you chose is true.

Compare the sizes of positive cations to the sizes of negative anions.

The strength of the electrostatic force of attraction within atoms is between the positively charged and negatively charged ____.