Copy of John, The Project Electron Configuration 2 PDF

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This is a project over electron configuration. For Chemistry one....

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Course: Chemistry Unit: Discovery of Atoms Assignment Electron Configurations : Lab Report Expectations and Instructions: Lab report grades make up 40% of each unit grade. Completing and doing well on projects is very important for your unit and overall grade. For this project, you will be using Gizmos simulations through www.explorelearning.com. Please login to your Gizmos account (Gizmos Login) and open the “Electron Configurations” simulation.

This document will walk you through how to use the Gizmos simulation. Please answer all questions in the Answer boxes in complete sentences. Leave the rest of the document intact. Your teacher will include notes in the document and add points in the “Points Earned” column. ** Please read over the teacher comments after the report is submitted and graded. **

Electron Configurations Student Name: Date: Name of Grader:

Quaid Mull 9/20/21

Goals: ● Explain the relationship between the atomic number and the number of protons & electrons in a neutral atom. ● Understand what is meant by shell, subshell, and orbital. ● Determine the electron configuration of various elements

Hypothesis: ● A prediction of what you think the results of the project will be before you complete the project. ● Create an if, then statement for each part of the lab that is related to the goal(s) of the experiment. (Example: Goal: To determine what improves student grades. Hypothesis: If students get adequate rest, then grades will improve).

Hypotheses

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If the atomic number increases, then the number of electrons will increase in a neutral atom.

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If the electron configuration changes, then the element changes also.

Vocab: Atomic Number, Aufbau Principle, Diagonal Rule, Electron Configuration, Hund’s Rule, Orbital, Pauli Exclusion Principle, Period, Shell, Spin, Subshell

Prior Knowledge Questions (Do these BEFORE using the Gizmo.) Question Answer Points Possibl e 1. Elvis Perkins, a rather The back seat on the left. 1 shy fellow, is getting on the bus shown at the right. Which seat do you think he will probably sit in? 2. Marta Warren gets on Front right with the other 1 the bus after Elvis. She person. is tired after a long day at work. Where do you think she will sit? 3. In your experience, do No strangers do not like to sit 1 strangers getting on a together. bus like to sit with other people if there is an empty seat available?

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Gizmo Warm-up Just like passengers getting on a bus, electrons orbit the nuclei of atoms in particular patterns. You will discover these patterns (and how electrons sometimes act like passengers boarding a bus) with the Electron Configuration Gizmo. To begin, check that Lithium is selected on the PERIODIC TABLE tab

1.

Question Answer The atomic number is There are 3 protons. equal to the number of protons in an atom. How many protons are in a lithium atom?

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2.

A neutral atom has the same number of electrons and protons. How many electrons are in a neutral atom of lithium?

There are 3 electrons.

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3. Select the ELECTRON CONFIGURATION tab, and check that Energy is selected. Click twice in the 1s box at lower left and once in the 2s box. Observe the atom model at right. Question

Answer

A.

What do you see?

B.

Click Check. Is this electron configuration correct?

I see three dots/balls orbiting the nucleus. Yes.

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Get the Gizmo ready: Activity A: Small atoms

● On the PERIODIC TABLE tab, select H (hydrogen). ● Select the ELECTRON CONFIGURATION tab. ● Click Reset.

Introduction: Electrons are arranged in orbitals, subshells, and shells. These levels of organization are shown by the boxes of the Gizmo. Each box represents an orbital. The subshells are labeled with letters (s, p, d, and f) and the shells are labeled with numbers. Question: How are electrons arranged in elements with atomic numbers 1 through 10 1. Arrange: The Aufbau principle states that electrons occupy the lowest-energy orbital. When Energy is selected, the orbitals are arranged from lowest-energy at the bottom to highest-energy at the top. Click once in the 1s box to add an electron to the only orbital in the s subshell of the first shell.

Click ‘Configuration in order of subshell filling’ under the box where you see the e- configuration written out.

2.

Question

Answer

Click Check. What is the electron configuration of hydrogen?

1s 1

Question

Answer

Arrange: Click Next element to select helium. Add another electron to the 1s orbital. The arrows represent the

On faces up and one faces down.

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spin of the electron. What do you notice about the arrows? The Pauli exclusion principle states that electrons sharing an orbital have opposite spins.

3.

Question

Answer

Check your work: Click Check. What is the electron configuration of helium?

1s

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4. Arrange: Click Next element and create electron configurations for lithium, beryllium, and boron. Click Check to check your work, and then list each configuration below: **If you are not using superscripts in your configurations, please make sure to put a space between each term.** Question Answer Possibl Earne e d A. Lithium 1s 2, 2s 1 1 B. Beryllium 1s 2, 2s 2 1 C. Boron 1s 2, 2s 2, 2p 1 1 5. Arrange: Click Next element to select carbon. Add a second electron to the first 2p orbital. Question

Answer

Click Check. What feedback is given?

That it is the incorrect number of electrons.

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6. Rearrange: Hund’s rule states that electrons will occupy an empty orbital when it is available in that subshell. Rearrange the electrons within the 2p subshell and click Check.

7.

Question

Answer

Is the configuration correct now?

Yes.

Write the configuration.

1s 2, 2s 2, 2p 2.

Question

Answer

Compare: How are the electrons in the 2p subshell similar to passengers getting on a bus?

The people on the bus will choose an empty seat until there are no empty ones left just like an electron will do with an orbital.

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8. Practice: In the spaces below, write and illustrate electron configurations for the next four elements: nitrogen, oxygen, fluorine, and neon. When you are finished, use the Gizmo to check your work. Correct any improper configurations.

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A. B. C. D.

Question

Answer

Nitrogen Oxygen Fluorine Neon

1s 2, 2s 2, 2p 3 1s 2, 2s 2, 2p 4 1s 2, 2s 2, 2p 5 1s 2, 2s 2, 2p 6

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9. Apply: Atoms are most stable when their outermost shell is full. If their outermost shell is not full, atoms tend to gain, lose, or share electrons until the shell fills up. While doing this, atoms react and form chemical bonds with other atoms.

10 .

Question

Answer

Based on this, what can you infer about the reactivity of helium and neon? Explain Think and discuss: Select the PERIODIC TABLE tab, and look at the second row, or period, of the table. How does this row reflect the subshells of the second shell?

Helium loses electrons very quickly so therefore Neon is much stronger than Helium. The second row reflects the subshells because if you look at how many electrons are in the element you can tell that the rows change when the subshells change as well.

Activity B: Atomic Radii

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Get the Gizmo ready: ● On the PERIODIC TABLE tab, select Na (sodium). ● Select the ELECTRON CONFIGURATION tab.

Investigate: How do the radii of atoms change across a period of the periodic table?

1.

2.

3.

Question

Answer

Predict: Positively charged protons in the nucleus of an atom are attracted to negatively charged electrons.

It will decrease as electrons are added to the shell.

How do you think the atomic radii will change as electrons are added to a shell? Arrange: Create a proper electron configuration for sodium. After clicking Check, note the Electron configuration and the Atomic radius now listed at right. Compare: Click Next element, and then add an electron to the

Sodium electron configuration:

1s 2, 2s 2, 2p 6, 3s 1

Atomic radius:

190

Magnesium electron

1s 2, 2s 2, 2p 6, 3s 2

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magnesium atom. Click check, and record the electron configuration and atomic radius below.

configuration: Atomic radius:

145

4 . Gather data: Create electron configurations for the next six elements. Record the electron configuration and atomic radius of each. (Note: The symbol for picometer is pm.)

5.

6 7.

8.

9.

Element

Number of electrons

Electron configuration

Atomic radius (pm)

Aluminum

13

1s 2, 2s 2, 2p 6, 3s 2, 3p 1

118

Silicon

14

1s 2, 2s 2, 2p 6, 3s 2, 3p 2

111

Phosphorus

15

1s 2, 2s 2, 2p 6, 3s 2, 3p 3

98

Sulfur

16

1s 2, 2s 2, 2p 6, 3a 2, 3p 4

88

Chlorine

17

1s 2, 2s 2, 2p 6, 3a 2, 3p 5

79

Argon

18

1s s, 2s 2, 2p 6, 3a 2, 3p 6

71

Question

Answer

Analyze: How does the atomic radius change across a period of the periodic table? Interpret: Select the ATOMIC RADIUS tab. What do you notice? Predict: On the ATOMIC RADIUS tab click Clear. Select the PERIODIC TABLE tab. Elements in the same column of the periodic table are called chemical families, or groups.

The more electrons and the bigger the atom the more the atomic radius decreases. That all the elements are moving down the bigger they get. They will get bigger because on the periodic table they are going from top to bottom.

How do you think the size of atoms will change from top to bottom within a chemical family? Test: Hydrogen, lithium, and sodium are all in the same chemical family. Use the Gizmo to find the atomic radius of each, and list them below.

Hydrogen radius

53

Lithium radius

167

Sodium radius

190

Analyze: How does the atomic radius

As you go from top to bottom the

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change as you go from the top to the bottom of a chemical family?

radius gets bigger.

10. Challenge: Think about the factors that control atomic radius and the patterns you’ve seen. Question

Answer

A.

Why does the atomic radius decrease as electrons are added to a shell?

B.

Why does the atomic radius increase as you go from the top to the bottom of a chemical family?

The atomic radius decreases because they attract each other therefore everything shrinks and the atomic radius decreases. The atomic radius increases when it goes from the top to the bottom because it's adding energy therefore it can hold more electrons and be bigger.

11 .

Question

Answer

Think and discuss: Compare the electron configurations of hydrogen, lithium, and sodium. Why do you think these elements are grouped in the same family?

They are in the same family because they all have the same amount of electrons.

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Get the Gizmo ready: Activity C: The diagonal rule

● On the PERIODIC TABLE tab, select Ar (argon). ● Select the ELECTRON CONFIGURATION tab. ● Turn on Show number of electrons.

Question: How are the electron configurations of elements beyond argon determined?

1.

2.

Question

Answer

Arrange: Create the correct electron configuration for argon. Then, click Next element to get to potassium (K). Click once in the first 3d orbital, and then click Check.

The feedback given is that the electrons are not placed in the correct energy level.

What feedback is given? Rearrange: The 4s subshell is a lowerenergy subshell than 3d, so it is filled first. Remove the electron from the 3d orbital and place it in the 4s orbital. Click Check. (Note: For simplicity, all

Yes, the electron configuration is correct. The configuration is 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 1.

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but the outer shell electrons will disappear on the Bohr Model.)

3.

4.

5.

Is this configuration correct? What is the configuration? Arrange: Click Next element and add an electron for calcium. Click Check. What is the electron configuration for calcium? Arrange: Click Next element and add an electron for scandium. Try different orbitals until you find the right one. What is the configuration for scandium? Observe: Scandium is the first element to contain electrons in the d subshell. How many orbitals does the d subshell have, and how many electrons can fit in the d subshell?

The electron configuration is 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 2.

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The correct electron configuration is 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 3d 1, 4s 2.

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Subshell d has 5 orbitals and it can fit 10 electrons.

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6.

Infer: Select the PERIODIC TABLE tab. The middle section of the table contains ten groups that make up the transition metals. Why do you think this section is ten columns wide?

It is ten columns wide because it holds no more than ten electrons.

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7.

Observe: Select the ELECTRON CONFIGURATION tab. Make sure the subshells are ordered by Energy, which will arrange them from lowest to highest energy, bottom to top.

The subshells closest to the nucleus with the lowest energy will be filled first.

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Based on what you see, in what order do you think subshells will be filled? 8. Make a rule: Next to Subshells ordered by, select Number. The diagonal rule at right shows which subshell will be filled next. To follow the rule, move down along an arrow until you reach the end of the arrow. Then move to the start of the next arrow to the right.

A . B. C.

Question Which subshell is filled after 4p? Which subshell is filled after 6s? Which subshell is filled

Answer 5s.

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4f.

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6p.

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after 5d? 9. Practice: Determine the electron configurations of the following elements. Use the Gizmo to check your work. (Note: In some cases, the diagonal rule doesn’t work perfectly. If you submit a theoretically correct configuration, the Gizmo will give you the actual configuration.)

A. B. C.

D.

Question

Answer

Cobalt (Co) Atomic Number: 27 Germanium (Ge) Atomic Number: 32 Neodymium (Nd) Atomic Number: 60

1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 3d 7, 4s 2. 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 2, 3d 10, 4p 2. 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 2, 3d 10, 4p 6, 5s 2, 4d 10, 5p 6, 6s 2, 4f 4.

Gold (Au) Atomic Number 79

1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 2, 3d 10, 4p 6, 5s 2, 4d 10, 5p 6, 6s 1, 4f 14, 5d 10.

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10. Infer: Select the PERIODIC TABLE tab. Earlier you saw that the transition metals represent the filling of the d subshells. Now locate the purple lanthanides and actinides on the bottom rows of the periodic table. Question

Answer

A.

How many elements are in the lanthanides series?

B.

Which subshell specifically is represented by the lanthanides series? Which subshell specifically is represented by the actinides series? In general, how does the shape of the periodic table relate to the electron configuration?

There are 14 elements in the lanthanides series of the periodic table. The f subshell is specifically represented by the lanthanides.

C. D.

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Subshell d.

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The periodic table's shape is based on what elements have the same electrons in the outer shell and if they do they are grouped together on the table.

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Conclusion: Question

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God says that humans are “fearfully and wonderfully made”. As you see the components and internal order of atoms, do you think this applies to the rest of nature as well? Why? Please explain.

This project has shown me that God has a specific way for everything he does. Everything has to be in a perfect order, if there is one wrong thing in something then something could dramatically change. For example if one electron is misplaced in an electron configuration then the entire periodic table could get thrown off.

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Look back at hypotheses you wrote on page 1. What was your hypothesis and was it correct? (2-3 sentences)

My first hypothesis is, If the atomic number increases, then the number of electrons will increase in a neutral atom. This hypothesis is correct. My second hypothesis is, If the electron configuration changes, then the element changes also. This hypothesis is also correct.

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How do you know your hypothesis was correct or incorrect? Use relevant data/observations to support your answer. (3-5 sentences)

My first hypothesis is correct because I used the Bohr Model to experiment with the electron configuration/electrons to find what configuration matches what element/atomic number. In doing that, I came to the observation that when you change the amount of electrons, it will also change the atomic number. My second hypothesis is also correct. By experimenting with the Bohr Model I was able to conclude that when the electron configuration changes so is the element of the periodic table.

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Go back and read the goals for this lesson on page 1. Form a summary statement for each goal, showing you understand and have met the goals of this lab. Be sure to explain all major concepts and relationships presented

Using the Bohr Model I learned that the atomic number and the number of protons and electrons sho...