02.01 Atomic Theory

Page 1: Introduction
Reflect on how scientists have theorized about atoms.

Page 2: What are the postulates of Dalton's atomic theory?
Describe the five main ideas in Dalton's hypothesis. Feel free to draw in order to illustrate your written answer:

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Page 3: How did various scientists add to our knowledge of atomic theory?
Write key contributions and changes to the model of the atom:

•	J.J. Thompson

•	Ernest Rutherford

•	Niels Bohr

•	James Chadwick 

Complete the sentences: In science, the benefit of disagreement is

Page 4: How did experimental evidence support the development of atomic theory?
Write key points related to the experiments of:

•	Sir William Crookes
•	Sir J.J. Thomson
•	Rutherford
•	Niels Bohr 

Page 5: What are the features of modern atomic theory?
Label the parts of the atom:

Explain when atoms have the following charge:
•	Positive charge:
•	Negative charge:
•	Neutral:
Complete the sentence: The nucleus of an atom is positively charged because 

Draw the image of a hydrogen atom.	Draw the image of a helium atom.	

		

02.02 Periodic Table
Page 1: Introduction
Reflect on how the elements are organized.

Page 2: What is the early history of the periodic table?
Complete the sentence: The simplest way to organize things is

Video:
Complete the sentences:
•	The periodic table was first described by _______________, who theorized that substances were made of invisible unbreakable particles called ____________________.
•	The four fundamental elements are ___________, __________, __________, and _________. 
•	___________ theorized that the four elements could be mixed to create new materials, which created interest in ______________.
•	French chemist Antoine Laurent de Lavoisier described "element" as ____________.
•	John Dalton was able to ___________________________________________. 
•	Scientists kept observing patterns in the list of elements, and eventually in the mid to late 1800s, ______________ discovered the periodic table.

Complete the sentence: Interpretation is a strength of science because 

Page 3: What categories of elements exist based on similar properties?
List physical properties of metals.	List physical properties of nonmetals.	

	

	

Video: Complete the sentences referring to the periodic table:

The letter H symbolizes the ___________________.

The top arrow is pointing to the ________________.

The bottom arrow is pointing to the ______________.
			
The horizontal row is called a ___________________.

All the elements of a period have _________________. 
		
The columns are called _________________________.

In most groups, the elements have _______________________. 	
Elements can be divided into three groups: _____________, ____________ and ____________.
Most elements in the table are _________________________.
Transition metals can be found in ______________________.
Transition metals include groups _______________________.
Group 1 elements are called ______________. Group 2 elements are called ______________.
Elements in groups 1 and 2 are very ___________. Some names are ____________________.
Elements in groups 13 through 16 are a ________________ called __________ by some researchers.
Page 4: What is the atomic mass of an element?
Complete the sentence: The mass number of the most common isotope of an element can be determined by

Explain how average atomic mass is calculated.

Illustrate how isotopes are represented.

Provide two examples of how isotopes are used in real life:
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•	
Page 5: What does the periodic table tell us about an element?

Video
Explain how you find the number of neutrons in an element. Feel free to draw in your explanation.

Complete the sentences:
•	Alkali metals are extremely 
•	Alkaline earth metals can be used in
•	Halogens are used in
•	Noble gases are used in
02.03 Atomic Models
Page 1: Scientific models
Reflect on models and their observations.

Page 2: How do scientists use models to show the motion and location of an electron?
Complete the sentence: The quantum model is

Video. Complete the sentences:
•	Niels Bohr proposed that __________________________and decided that ______________.
•	The lowest energy shell is called __________________.
•	Very stable noble gases do not ____________________.
•	Every atom can be described by ___________________.
•	______ is the principal quantum number and goes up to 7.
•	The closest shell to the atom nucleus has n= _____.
•	The angular momentum quantum number is abbreviated with the symbol ________________.

•	True or false:
_____ As an atom gets bigger, its electrons contain more energy.
_____ According to the Uncertainty Principle, you know both the position and the velocity or momentum of a particle at the same time.

Page 3: How is the electron cloud divided into multiple energy levels?
Where are electrons located?

Complete the chart:
Subshells	Number of Orbitals	Shape of Orbital	Number of Electrons	

				

Page 4: How do electron configurations show electron arrangements within an atom?
Describe the parts of an electron configuration.

Video. Electron configuration for titanium
Write the electron configuration for titanium. Take notes of how it is determined.

Page 5: How do orbital notation diagrams model electron arrangement?
Describe what orbital notation is.

Summarize Hund's first and second rules.

Video: Draw the orbital notation for titanium. Take notes of how it is determined.

02.04 Electromagnetic Radiation

Page 1: Introduction 
Reflect on the phenomena presented.

Page 2: In what ways do electrons act as particles and waves?
Complete the sentences: 

Albert Einstein and Max Planck agreed that 

Quanta is defined as

Feynman's double split experiment demonstrated that

Explain Feynman's double split experiment.

Page 3: What are the characteristics of waves?
Draw and label the parts of a wave:

Define:
•	Wavelength
•	Frequency

Describe the relationship between wavelength and frequency.

Compare wavelength and frequency on a wave.

Page 4: What are the different forms of electromagnetic radiation?
Complete the sentences: 
Electromagnetic radiation is ______________________.
Visible light is _________________________________.
Invisible types of EMR are ________________________.
All forms of AMR travel at _______________. Other types of EMR move through ______________.

Page 6: What is the relationship between speed, wavelength, and frequency of wave?
Write the formula of the speed of light using these symbols: λ, c, f:

Example: What is the wavelength of microwaves that have a frequency of 1.00 × 1010 Hz?

02.05 Atomic Energy Journal (Notes)
Note: This is NOT the lab assignment. This is for your notes, not to be submitted.
Page 1: Introduction
Reflect on the phenomenon introduced.

Page 2: Why do transitioning electrons release or absorb energy?
Complete the sentences:
Transitioning electrons release or absorb energy because
An emission spectrum is created when
Electrons jump to other orbits around the nucleus and fall again due to

Describe:
Excited electrons
Ground electrons

Explain how "laser cooling" is helpful

Complete the sentences:
The closer the orbit is to the central nucleus, the
The farther the orbit is to the nucleus, the 
As an electron falls, energy equal to the difference between the two orbits is emitted in the form of 

Page 3: How do scientists determine the energy of photons?
Define photon:

In the formula E = hƒ, explain: 
E
h
ƒ

Complete the blank boxes with two expressions in each box:

02.06 Honors Periodic Trends

Page 1: Introduction
Reflect about Demetri Mendeleev’s and Henry Mosley’s contribution to the periodic table.

Page 2: What are nuclear charges and their trends?
Complete the sentences:
Negatively charged electrons _______ one another.
Protons (+) and electrons (–) ___________ each other.
The overall nuclear charge increases by ______ with each additional proton.
Each atom also has an additional electron in its ______ energy level.
The number of inner core electrons in the lower energy levels remains __________________.

Describe the following:
•	Electrostatic forces
•	Effective nuclear forces (zeff)

Complete the statement: The competing components that affect the effective nuclear charge are

1.	
2.	

Complete the sentence: The nuclear charge of outer shell electrons stays _________________ for each element down a group because ___________________________________________.

Page 3: What determines the strength of forces between charged particles?
Describe what causes trends in the periodic table.

This formula  is called 
Label each part of the formula.
F is
k is
q1 is
q2 is 
d2 is 

As the magnitude of either charge increases, the electrostatic force of attraction or repulsion _________________.
As the distance between charges increase, the electrostatic force _______________.
As the distance increases towards infinity, the force decreases to ___________.

Example: Let's look at an example of how to find the electrostatic force between an electron and a proton separated by 10−12 m. The charge e = 1.6 × 10−19 coulomb.

Page 4: What can we learn about radius, ionization, and electronegativity from periodic trends?
Complete the sentences:

Atomic radius _____________ moving down the column.
Atomic radius _____________ moving across the row from left to right.

Ionization energy is the energy required to remove one __________ from an atom, resulting in a __________ ion.
Elements with a lower effective nuclear charge require ________ energy to give up electrons, so their ionization energy is _______, due to _________ attraction between the outer shell electrons and the positively charged nucleus.
Ionization energy _________ from left to right and moving up a group on the periodic table. It generally __________ down a group as the size of atoms increases because it requires _________________ to remove an electron when it is in an outer shell much farther from the positively charged nucleus.

__________ are positively charged and result from a loss of electrons.
__________ are negatively charged and result from a gain of electrons.
Metals naturally form ______________that are smaller than neutral atoms by losing one or more ________________. When metals lose all the __________ from their outermost energy shell, the remaining ___________ cloud is ____________.
Nonmetals naturally form _________________ that are larger than neutral atoms by gaining one or more _________________. When nonmetals gain enough _________________ to fill their outermost energy shell, the _____________ experience additional repulsive forces between them, and the __________________ cloud spreads out and gets ____________.

In the periodic table, the ionic radii of cations _____________ from left to right within metals, the ionic radii of anions _______________ from left to right within the nonmetals, and the ionic radii _________________ down a group for metals and nonmetals.

Electronegativity is _____________________________________.
The higher an element's electronegativity, the _________________ its attraction for electrons in a chemical bond.
Elements with a _________________________ exert a strong attractive force on their outer shell electrons.
Fluorine has the _____________________electronegativity value, and all other elements were given values by comparing their electronegativity to that of fluorine. Both cesium (Cs) and francium (Fr) have the ____________________electronegativity values.
Page 5: How can scientists predict the reactivity of elements from periodic trends?
Complete the sentences:
The chemical reactivity of metals going down a column _________.
The chemical reactivity of nonmetals going right a row _________.
Define electron affinity.

Complete the sentences:
When energy is released, the electron affinity value is represented as a ________ value. When energy is absorbed, electron affinity is represented with a __________ value. An atom that requires energy to force it to accept an electron will not be stable and will __________ that electron spontaneously.

Explain electron affinity across a period from group 1 to 17.

Explain electron affinity going down a group.

Explain why alkaline earth metals in group 2 and nonmetals in group 15 have electron affinity close to 0.

Explain why the noble gases in group 18 all have positive electron affinity values.