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4.2 Periodic Table Properties: Core Charge and Atomic Radius

Last updated over 3 years ago
18 questions
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1

Which of the following are true? Select all that apply

1

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

1

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

View the Model 2 Video to help you with this section.
1

Draw a Bohr Diagram of Be

1

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

  • 0
  • 1
  • 2
  • 3
  • 4
  • # of valence electrons
  • Core Charge
1

Draw a Bohr Diagram of B.

1

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

  • 0
  • 1
  • 2
  • 3
  • 4
  • # of valence electrons
  • Core Charge
1
View the Model 3 video to help you with this part.
1

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

  • 3
  • 4
  • 5
  • 6
  • 7
  • 8
  • C
  • N
  • O
  • F
  • Ne
1

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.

1

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

  • 1
  • 2
  • 3
  • 4
  • 5
  • 6
  • 7
  • 8
  • # of energy levels/shells
  • # of valence electrons
  • Core Charge
1

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

  • 1
  • 2
  • 3
  • 4
  • 5
  • 6
  • 7
  • 8
  • # of energy levels/shells
  • # of valence electrons
  • Core Charge
1

Click on Edit Background to answer question 13.

View the Model 4 video to help you with this part.
1

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

1

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.

1

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

1

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

1

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.