Chapter 2 Section 6: Investigate

Open Ended

Niels Bohr was able to explain the spectrum of light emitted by hydrogen using a model that assigned the electron to specific energy levels. Hydrogen is a simple atom that contains only one electron. The atoms of other elements contain more than one electron. 

• How do you think an increase in the number of electrons would impact the spectrum of an atom?

Match

Match the following

• the amount of energy needed to totally remove an electron from an atom.

• atoms that have lost or gained electrons.

• the arrangement of the electrons of an atom in its different energy sublevel(s).

• an electron of an atom that has absorbed enough energy to be raised to a higher energy sublevel.

ionization energy:

ions:

electron configuration:

excited state:

• ionization energy:

• ions:

• electron configuration:

• excited state:

Match

Match the following

• the lowest energy level that an electron of an atom can occupy.

• a family of elements in the periodic table that have similar electron configurations and properties.

• a horizontal row of elements in the periodic table.

• states that it is impossible to precisely determine the exact position and momentum of an electron at the same time.

ground state:

chemical group:

period:

Heisenberg uncertainty principle:

• ground state:

• chemical group:

• period:

• Heisenberg uncertainty principle:

Word Cloud

What is the name of the element spectra you just observed?

Word Cloud

Name 2 colors you saw.

Draw

Make a diagram of the spectrum 

(pattern of colors) you see inside the diffraction grating.

Open Ended

How this spectrum is similar to and different from the hydrogen spectrum?

Word Cloud

What is the name of the element spectra you just observed?

Word Cloud

Name 2 colors you saw.

Draw

Make a diagram of the spectrum 

(pattern of colors) you see inside the diffraction grating.

Open Ended

How this spectrum is similar to and different from the hydrogen spectrum?

Word Cloud

What is the name of the element spectra you just observed?

Word Cloud

Name 2 colors you saw.

Open Ended

How this spectrum is similar to and different from the hydrogen spectrum?

Draw

Make a diagram of the spectrum 

(pattern of colors) you see inside the diffraction grating.

Multiple Choice

What is the primary challenge that arises in atoms with multiple electrons, according to the provided information?

• Difficulty in visualizing electron transitions

• Increased complexity in labeling electron energy levels

• Lack of distinct patterns in energy level arrangements

• Inability to emit light during electron transitions

Multiple Choice

What does the investigation mentioned in the passage aim to explore?

• Patterns of electron energy levels in atoms with more than one electron

• The efficiency of ionization energies in removing electrons

• The simplicity of Bohr's theory in multiple-electron atoms

• The visual appeal of helium and neon spectra

Multiple Choice

What information does the chart of ionization energies provide?

• Energy required to remove the first and second outermost electrons

• Visualization of electron transitions

• Complexity in labeling electron energy levels

• The simplicity of Bohr's theory for hydrogen's single electron

Open Ended

What kinds of patterns do you see?

Open Ended

How could you quickly relate the shape of the graph to someone who had not seen it?

Draw

If you were given a piece of blank paper and only five seconds, how would you sketch the pattern of ionization energies?

Multiple Choice

Where are the ionization energies the largest?

• Transition metals
• Alkali metals
• Halogens
• Noble gases

Multiple Choice

Where are the ionization energies the smallest?

• Transition metals
• Alkali metals
• Halogens
• Noble gases

Multiple Choice

What happens to the ionization energies as the atomic number increases?

• the ionization energy fluctuates

• the ionization energy stays the same

• the ionization energy increases

• the ionization energy decreases

Draw

Group the elements by their ionization energies into four consecutive horizontal rows called periods. List the range of atomic numbers in each group.

Open Ended

Is there any interruption in the general trend of ionization energies as the atomic number increases for a period? If so, describe it.

Open Ended

 Look at the second colored graph line you drew. 

Describe how the two graphs are alike and/or different. 

Do you see similarities between the two graphs?

Multiple Choice

Which element in the first period (atomic numbers 1 and 2) has the most stable configuration of electrons in its atoms?

• Oxygen has the highest ionization energy.

• Helium has the highest ionization energy.

• Hydrogen has the highest ionization energy.

• Lithium has the highest ionization energy.

Multiple Choice

Which elements in the second period (atomic numbers 3 through 10) of the periodic table have the most stable arrangements of electrons in their atoms? 

• Neon has the most stable arrangement. Secondary stabilities could be assumed at beryllium and nitrogen.

• Fluorine has the most stable arrangement. Secondary stabilities could be assumed at oxygen and carbon.

• Lithium has the most stable arrangement. Secondary stabilities could be assumed at Boron and Carbon

• Oxygen has the most stable arrangement. Secondary stabilities could be assumed at Hydrogen and Lithium

Multiple Choice

Which elements in the third period (atomic numbers 11 through 18) of the periodic table have the most stable arrangements of electrons in their atoms?

• Argon has the most stable arrangement. Secondary stabilities could be assumed at magnesium and phosphorus.

• Carbon has the most stable arrangement. Secondary stabilities could be assumed at boron and fluorine.

• Lithium has the most stable arrangement. Secondary stabilities could be assumed at radium and tin.

• Silicon has the most stable arrangement. Secondary stabilities could be assumed at aluminum and chlorine

Multiple Choice

Which elements in the fourth period (atomic numbers 19 through 36) of the periodic table have the most stable arrangements of electrons in their atoms?

• Krypton has the most stable arrangement. Secondary stabilities are at calcium and arsenic. Zinc is quite stable as well.

• Carbon has the most stable arrangement. Secondary stabilities could be assumed at boron and fluorine.

• Fluorine has the most stable arrangement. Secondary stabilities could be assumed at oxygen and carbon.

• Silicon has the most stable arrangement. Secondary stabilities could be assumed at aluminum and chlorine

Multiple Choice

In which sublevel is the one electron in hydrogen and the two electrons in helium?

• 4d
• 2p
• 3s
• 1s

Multiple Choice

In which region of the periodic table are electrons added in an s sublevel?

• Transition Metals.

  d-block

• Inner Transition Metals.

  f-block

• 
  Nonmetals, Metalloids.

  p-block

• Alkali metals and alkaline earth metals (groups IA and IIA)

  s-block

Multiple Select

In which region of the periodic table are electrons added in a p sublevel?

• Boron through neon

• Aluminum through argon

• Potassium through zinc

• Lithium through francium

Multiple Select

In which region of the periodic table are electrons added in a d sublevel?

• Scandium through zinc

• Aluminum through argon

• Potassium through zinc

• Lithium through francium

Open Ended

How does the number and location of the electrons in the outermost sublevel relate to chemical properties?

Open Ended

At the beginning of this investigation, you constructed a graph of the ionization energy versus the atomic number. If you take this graph and rotate it 90°, you will find that the graph reminds you of the periodic table, constructed by Mendeleev because of similar chemical and physical properties of elements. 

What is the relationship between ionization energies and the rows of the periodic table?

The Periodic Table

-Divided into different sections

-Helps to identify the energy levels of the elements

How to Write an Electron Configuration:

1. Start with the shell/period number

2. Followed by the type of orbital

3. Finally the superscript indicates the number of electrons in the orbital

Example: B = 1s² 2s² 2p¹

Expanded Periodic Table

How the f block fits into the periodic table with the other energy levels

Read the energy levels from left to right, top to bottom

Hydrogen (1s¹)

-The first element on the periodic table

-The element that starts the electron configuration levels

-1 electron on the inner most shell

Helium (1s²)

-The second element in period 1

-2 electrons on the inner most shell

-Start at H and move across the period to count the valence electrons

Open Ended

Look at the cartoon at the beginning of this section. 

Now that you have completed this section, what additional features do you see that demonstrate you have a better understanding of ionization energy?

Open Ended

At the beginning of the section, you were asked the following: 

• How do you think an increase in the number of electrons would impact the spectrum of an atom? 

Your response might have been along the lines of “it will become more complicated, more complex.” Now that you have additional information about line spectra, describe what you would see and why you would see it when you have more than one electron in an atom.