View the Model 3 video to help you with this part.
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1
1
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4
View the Model 4 video to help you with this part.
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Question 17
17.
List at least 2 patterns that you notice from the data table and Periodic Table showing the atomic radius of elements.
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1
1
1
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Question 22
22.
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.
Question 1
1.
Carefully read and annotate the passage using CHAT in the folders.
Question 2
2.
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
Question 3
3.
What is 1 question or idea from the passage you need clarified to understand Model 1 better?
Question 4
4.
Question 5
5.
Question 6
6.
View the Model 2 Video to help you with this section.
Question 7
7.
Draw a Bohr Diagram of Be
Remember:
Atomic Number = protons
Protons= electrons
Atomic Mass - Atomic Number= neutrons
Question 8
8.
Question 9
9.
Draw a Bohr Diagram of B.
Remember:
Atomic Number = protons
Protons= electrons
Atomic Mass - Atomic Number= neutrons
Question 10
10.
Question 11
11.
What is the relationship between the number of valence electrons and the core charge of a neutral atom?
Question 12
12.
Question 13
13.
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.
Question 14
14.
Question 15
15.
Question 16
16.
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.
Question 18
18.
Question 19
19.
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.
Question 20
20.
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.
Question 21
21.
Based on Model 1: Which of the following are true? Select all that apply
Valence electrons are in the outermost shell
Valence electrons are in the inner shells
Core electrons are in the outermost shell
Core electrons are in the inner shells
The strength of the electrostatic force of attraction within atoms is between the positively charged ______________ and negatively charged __________________.
nucleus, core electrons
nucleus, valence electrons
core electrons, nucleus
valence electrons, nucleus
If an element has a greater core charge it will have a ____________ electrostatic attraction holding the protons and electrons together within the atom.
stronger
weaker
Drag the correct number under each category for the valence electrons and core charge for Be.
0
1
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3
4
# of valence electrons
Core Charge
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
Drag the correct number of valence electrons and core charge for each element.
3
4
5
6
7
8
C
N
O
F
Ne
Drag the numbers to each term below to determine the # of energy levels/shells, valence electrons and core charge for Ne
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8
# of energy levels/shells
# of valence electrons
Core Charge
Drag the numbers to each term below to determine the # of energy levels/shells, valence electrons and core charge for Na
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2
3
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5
6
7
8
# of energy levels/shells
# of valence electrons
Core Charge
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.
Na has more electrons than Argon.
Na has only 1 valence electron while Ar has 8.
Na is a metal and Ar is a nonmetal
Na has 1 more shell with electrons than Ar does
The nucleus of Na has a much weaker attraction to its valence electrons than Ar does
The nucleus of Na has a much stronger attraction to its valence electrons than Ar does
Compare the sizes of positive cations to the sizes of negative anions.
Cations are always larger than anions for the same element
Cations are always smaller than anions for the same element
