Download Name Date Class Chapter 6 – The Periodic Table Guided Reading

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Chapter 6 – The Periodic Table
Guided Reading
Section 1 - Organizing the Elements - This section describes the development of the periodic table and explains the
periodic law. It also describes the classification of elements into metals, nonmetals, and metalloids.
As you read Chapter 6 Section 1 define the following words:
Periodic law –
Metals –
Nonmetals –
Metalloid –
As you read Chapter 6 Section 1 complete the following questions:
By the year 1700 how many elements were known? By 1775?
How did J.W. Dobereiner organize the elements? In what year?
Who was Dmitri Mendeleev and how did he organize the elements?
What brave/crazy thing did Mendeleev do when he published his periodic table?
In Figure 6.3 a fourth element is grouped with chlorine (Cl), bromine (Br), and iodine (I). What is this element's symbol?
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In Figure 6.4 how many elements are there in the second period?
How did Henry Moseley improve on Mendeleev’s periodic table?
Periodic comes from the Greek roots peri meaning "around" and hodos, meaning "path." In a periodic table, properties
repeat from left to right across each period. the Greek word metron means "measure." What does perimeter mean?
How many periods are there in a periodic table?
What does IUPAC stand for and what do they do?
In Figure 6.5 what is the purpose for the black stair step line?
Describe the metals and state some of their properties, including where they are located in the periodic table.
Describe the nonmetals and state some of their properties, including where they are located in the periodic table.
Describe the metalloids and state some of their properties, including where they are located in the periodic table.
Which type of elements tend to be good conductors or heat and electrical current?
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Section 2 - Classifying the Elements - This section explains why you can infer the properties of an element based on
the properties of other elements in the periodic table. It also describes the use of electron configurations to classify
elements.
As you read Chapter 6 Section 2 define the following words:
Alkali metals –
Alkaline earth metals –
Halogens –
Noble gases –
Representative elements –
Transition metal –
Inner transition metal –
As you read Chapter 6 Section 2 complete the following questions:
Label the sample square from the periodic table below. Use the labels element name, element symbol, atomic number,
and average atomic mass.
In Figure 6.8 what does the data in the square tell you about the structure of sodium atoms?
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The origin of the names alkali and alkaline earth metals is Arabic. What is that word and what does it mean?
The origin of the name halogen is both Greek and Latin. What are these words and what does each mean?
In which group are the alkali metals located? The alkaline earth metals? The halogens? The noble gases?
Look at Figure 6.9 on pages 162 and 163. Make four observations about the information on these two pages.
In Figure 6.10 what does the ability of a helium-filled blimp to rise in the air tell you about the density of helium?
How is the electron configuration related to the group an element is located in?
Describe what the representative elements are and where they are located.
Why are noble gases sometimes referred to as inert gases?
Compare and contrast the transition and inner transition metals.
Describe how the periodic table is broken up into blocks that relate to the electron configuration.
In Figure 6.12 in the highest occupied energy level of a halogen atom, how many electrons are in the p sublevel?
Look at the Technology & Society after Section 2. What is something that you found interesting?
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Section 3 - Periodic Trends - This section explains how to interpret group trends and periodic trends in atomic size,
ionization energy, ionic size, and electronegativity.
As you read Chapter 6 Section 3 define the following words:
Atomic radius –
Ion –
Cation –
Anion –
Ionization energy –
Electronegativity –
As you read Chapter 6 Section 3 complete the following questions:
Draw a picture of how atomic radius of an atom figured?
What are groups on the periodic table? Rows?
In Figure 6.14 answer the Interpreting Graphs questions here:
a. Which alkali metal has an atomic radius of 238pm?
b. Based on the data for alkali metals and noble gases, how does atomic size change within a group?
c. Is an atom of barium, atomic number 56, smaller or larger than an atom of cesium (Cs)?
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In Figure 6.15 if a halogen and an alkali metal are in the same period, which one will have the larger radius?
With your best guess explain what the nuclear charge of atoms is.
What are ions and how do they form?
What is the difference between a cation and an anion?
How is ionization energy determined?
In Figure 6.17 answer the Interpreting Graphs questions here:
a. Which element in period 2 has the lowest first ionization energy? in Period 3?
b. What is the group trend for first ionization energy for noble gases and alkali metals?
c. If you drew a graph for second ionization energy, which element would you have to omit? Explain.
In Figure 6.14 which element would have the larger first ionization energy - an alkali metal in period 2 or an alkali metal
in period 4?
In Figure 6.20 what happens to the radius when an atom forms a cation? When an atom forms an anion?
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What are the period and group trends for ion size?
In your own words describe what electronegativity is.
What are the period and group trends for electronegativity?
Why are values for noble gases omitted from Table 6.2?
In Figure 6.20 which properties tend to decrease across a period?
Use Figure 6.20 to help you fill in this picture with the summary of periodic trends.
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