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3.6 Core Charge and Atomic Radius Trends

Last updated over 3 years ago
22 questions
1

Carefully read and annotate the passage using CHAT in the folders.

1

Respond to 1 question below about the passage you read in question 1.

1. What is the main idea of this passage?

2. What do you think the model is showing?

3. Choose 1-2 direct quotes that are most important to understand the model

1

What is 1 question or idea from the passage you need clarified to understand Model 1 better?

1

Based on Model 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

Remember:
Atomic Number = protons
Protons= electrons
Atomic Mass - Atomic Number= neutrons

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.

Remember:
Atomic Number = protons
Protons= electrons
Atomic Mass - Atomic Number= neutrons

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

What is the relationship between the number of valence electrons and the core charge of a neutral atom?

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
4

Click on Show your Work to answer question 16.

NOTE: You fill in the reasoning for the CLAIM that you think is correct. Leave the other side blank.

See the link that says rubric under the question # to help with response.

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 16 and add an additional piece of evidence based on the atomic radius trend you notice for elements as you go across a period.

1

What is 1 Got and 1 Need you have?

Got- Something you're taking away or understand from this formative

Need- A question you have or a topic you want to go over more.

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.