Download Chem.-Chapter-6-notes

Chapter 6 Notes
Key Concepts:
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How did chemists begin to order the elements?
Chemists used the properties of elements to sort them into groups.
How did Mendeleev organize his periodic table?
Mendeleev arranged the elements in his periodic table in order of increasing atomic mass.
How is the modern periodic table organized?
In the modern periodic table, elements are arranged in order of increasing atomic number.
What are the three broad classes of elements?
Three classes of elements are metals, nonmetals, and metalloids.
Vocabulary
1. Periodic Law- when the elements are arranged in order of increasing atomic number, there is a
periodic repetition of their physical and chemical properties
2. Metals- one of a class of elements that are good conductors of heat and electric current; metals
tend to be ductile, malleable, and shiny
3. Nonmetals- an element that tends to be a poor conductor of heat and electric current;
nonmetals generally have properties opposite to those of metals
4. Metalloids- an element that tends to have properties that are similar to those of metals
and nonmetals
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Organizing the Elements
Searching for an Organizing Principle
o Summary
Mendeleev’s Periodic Table
o Summary
The Periodic Law
o Summary
Metals, Nonmetals & Metalloids
o Summary
1. Metals
 Summary
2. Nonmetals
 Summary
3. Metalloids
 Summary
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Key Concepts:
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What type of information can be displayed in the periodic table?
The periodic table displays the symbols and names of the elements, along with information
about the structure of their atoms.
How can elements be classified based on their electron configurations?
Elements can be sorted into noble gases, representative elements, transition metals, or inner
transition metals based on their electron configurations.
Vocabulary
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Alkali Metals- any metal in Group 1A of the periodic table
Alkaline Earth Metals- any metal in Group 2A of the periodic table
Halogens- a nonmetal in Group 7A of the periodic table
Noble gases- an element in Group 8A of the periodic table; thes and p sublevels of the highest
occupied energy level are filled
Representative Metals- an element in an “A” group in the periodic table; as a group these
elements display a wide range of physical and chemical properties. In their atoms,
the s and psublevels in the highest occupied energy level are partially filled
Transition Metals- one of the Group B elements in which the highest occupied s sublevel and a
nearby dsublevel generally contain electrons
Inner Transition Metals- an element in the lanthanide or actinide series; the highest
occupied s sublevel and nearby f sublevel of its atoms generally contain electrons; also called
inner transition element
Classifying the Elements
A. Squares in the Periodic table
o Summary
B. Electron Configurations in Groups
1. The Noble Gases
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Summary
The Representative Elements
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Summary
C. Transition Elements
o Summary
1. Blocks of Elements
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Summary
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Key Concepts:
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What are the trends among the elements for atomic size?
In general, atomic size increases from top to bottom within a group and decreases from left to
right across a period.
How do ions form?
Positive and negative ions form when electrons are transferred between atoms.
What are the trends among the elements for first ionization energy, ionic size, and
electronegativity?
First ionization energy tends to decrease from top to bottom within a group and increase from
left to right across a period. Cations are always smaller than the atoms from which they form.
Anions are always larger than the atoms from which they form. In general, electronegativity
values decrease from top to bottom within a group. For representative elements, the values
tend to increase from left to right across a period.
What is the underlying cause of periodic trends?
The trends that exist among these properties can be explained by variations in atomic structure.
Vocabulary:
1. Atomic radius- the wave’s height from zero to the crest
2. Ion - represented by λ (the Greek letter lambda), is the distance between the crests.
3. Cation- represented by ν (the Greek letter nu), is the number of wave cycles to pass a given
point per unit of time
4. Anion- the unit of frequency, equal to one cycle per second
5. Ionization energy- waves that travel in a vacuum at a speed of 2.998 X 108m/s; includes radio
waves, microwaves, infrared waves, visible light, ultraviolet waves, X-rays, and gamma rays
6. Electronegativity- wavelengths of visible light that are separated when a beam of light passes
through a prism; range of wavelengths of electromagnetic radiation
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Periodic Trends
A. Trends in Atomic Size
o Summary
1. Group Trends in Atomic Size
 Summary
2. Periodic Trends in Atomic Size
 Summary
B. Ions
o Summary
C. Trends in Ionization Energy
o Summary
1. Group trends in Ionization Energy
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Summary
2. Periodic Trends in Ionization Energy
 Summary
D. Trends in Ionic Size
o Summary
E. Trends in Electronegativity
o Summary
F. Summary of Trends
o Summary
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