1. ** MAJOR PART FOR CH. 5 Chapter menu Resources
B.8.C.1 Determine ion formation tendencies for groups on the Periodic Table:
􀁸 main group elements
􀁸 transition elements
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2. Chapter menu Resources
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3. might use the m.socrative.com later
Pick up computer & go to m.socrative.com in firefox and work on opener question.
Use the following hypothetical outermost (valence) energy level electron configurations:
A: 3s1 B: 3s2 C: 3s23p3 D: 3s23p5 E: 2s22p5
1. Identify each element above using periodic table.
2. Which element would you predict to have the least electronegativity value? the greatest?
3. Which element would have the greatest first ionization energy most likely?
4. Which element would have the greatest atomic radii?
5. Which element(s) would most likely perform a cation?
Turn in Ch. 4 Review pg #1-41 ex2,12
HW: Study Guide questions - TURN IN TOMORROW.
TEST ch.4-5 is TOMORROW!
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4. Opener #3 - WED. , Nov. 20, 2013 (B Day). Thursday - Nov
Opener #3 - WED., Nov. 20, 2013 (B Day) Thursday - Nov. 21, 2013 (A Day)
Use the following hypothetical outermost (valence) energy level electron configurations:
A: 3s1 B: 3s2 C: 3s23p3 D: 3s23p5 E: 2s22p5
1. Identify each element above using periodic table.
2. Which element would you predict to have the least electronegativity value? the greatest?
3. Which element would have the greatest first ionization energy most likely?
4. Which element would have the greatest atomic radii?
5. Which element(s) would most likely perform a cation?
HW: Study Guide questions & answers provided
TEST ch. 5 Monday (A Day) - Friday (B Day)
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5. OPENER #2 - MON - B DAY - NOV. 18, 2013 & TUE - A DAY - NOV. 19, 2013
1. How did Mendeleev’s periodic table differ from today’s?
2. What is the periodic law?
3. How do noble gases differ from other elements?
4. Write the noble gas notation for Phosphorus.
CW: Quiz
CW: Notes 5.3 using computers
CW: Finish and turn in periodic table questions & coloring activity
CW: Be sure you turned in the periodic table activity with clues
CW: New lab questions with 3-D trends models started along with periodic table puzzle if time allows
Check Grades online when finished with 5.3 notes.
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6. 5.3
Periodic Trends
Sodium chloride (table salt) produced the geometric pattern in the photograph. Such a pattern can be used to calculate the position of nuclei in a solid. You will learn how properties such as atomic size are related to the location of elements in the periodic table.
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7. 5.3
Periodic Trends
>
Trends in Atomic Size
Trends in Atomic Size
What are the trends among the elements for atomic size?
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8. Section 3 Electron Configuration and Periodic Properties
Chapter 5
Atomic Radii
The boundaries of an atom are fuzzy, and an atom’s radius can vary under different conditions.
To compare different atomic radii, they must be measured under specified conditions.
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9. 5.3
Periodic Trends
>
Trends in Atomic Size
Atomic radius may be defined as one- half the distance between the nuclei of identical atoms that are bonded together.
This diagram lists the atomic radii of seven nonmetals. An atomic radius is half the distance between the nuclei of two atoms of the same element when the atoms are joined.
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10. Chapter 5 Atomic Radius skip for whole class demo.
Visual Concepts
Chapter 5
skip for whole class demo.
except Van der Waals
Atomic Radius
Click below to watch the Visual Concept.
Visual Concept
van der Waals says not bonded together. ?
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11. Atomic Radii, continued
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Atomic Radii, continued
Atoms tend to be smaller the farther to the right they are found across a period.
The trend for Atomic radii decreases across a period is caused by the increasing positive charge of the nucleus, which attracts electrons toward the nucleus.
Atoms tend to be larger the farther down in a group they are found.
The trend for atomic radii increases down a Group is caused by the increasing size of the electron cloud around an atom as the number electron sublevels increases.
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12. 5.3 > Periodic Trends Trends in Atomic Size 12 End Show
This graph plots atomic radius versus atomic number for 55 elements. INTERPRETING GRAPHS a. Analyzing Data Which alkali metal has an atomic radius of 238 pm? b. Drawing Conclusions Based on the data for alkali metals and noble gases, how does atomic size change within a group? c. Predicting Is an atom of barium, atomic number 56, smaller or larger than an atom of cesium (Cs)?
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13. Periodic Trends of Radii
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Periodic Trends of Radii
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14. TRENDS IN ATOMIC RADII 5.3 > Atomic radii increases Periodic Trends
Trends in Atomic Size
TRENDS IN ATOMIC RADII
Atomic radii increases
The size of atoms tends to decrease from left to right across a period and increase from top to bottom within a group. Predicting If a halogen and an alkali metal are in the same period, which one will have the larger radius?
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15. Atomic Radii, continued
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Atomic Radii, continued
Sample Problem E
Of the elements magnesium, Mg, chlorine, Cl, sodium, Na, and phosphorus, P, which has the largest atomic radius? Explain your answer in terms of trends of the periodic table.
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16. Atomic Radii, continued
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Atomic Radii, continued
Sample Problem E Solution
Sodium has the largest atomic radius
All of the elements are in the third period. Of the four, sodium has the lowest atomic number and is the first element in the period. Atomic radii decrease across a period.
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17. Now practice pg. 152 #1-3 TEXTBOOK PRACTICE PROBLEMS
If you need more room, you may attach notebook paper.
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18. Now practice pg. 152 #1-3 TEXTBOOK PRACTICE PROBLEMS ANSWERS
If you need more room, you may attach notebook paper.
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19. Some compounds are composed of particles called ions.
5.3
Periodic Trends
>
Ions
Some compounds are composed of particles called ions.
An ion is an atom or group of atoms that has a positive or negative charge.
A cation is an ion with a positive charge.
An anion is an ion with a negative charge.
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20. Chapter 5 Ionization Energy
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Ionization Energy
An ion is an atom or group of bonded atoms that has a positive or negative charge.
Sodium (Na), for example, easily loses an electron to form Na+.
Any process that results in the formation of an ion is referred to as ionization.
The energy required to remove one electron from a neutral atom of an element is the ionization energy, IE (or first ionization energy, IE1).
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21. Ions How do ions form? 5.3 > Periodic Trends Ions 21 End Show Slide
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22. Visual Concepts
Chapter 5
Ion
Click below to watch the Visual Concept.
Visual Concept
Skip if doing as class whole
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23. 5.3
Periodic Trends
>
Ions
Positive and negative ions form when electrons are transferred between atoms.
When a sodium atom loses an electron, it becomes a positively charged ion. When a chlorine atom gains an electron, it becomes a negatively charged ion. Interpreting Diagrams What happens to the protons and neutrons during these changes?
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24. 5.3
Periodic Trends
>
Ions
Positive and negative ions form when electrons are transferred between atoms.
When a sodium atom loses an electron, it becomes a positively charged ion. When a chlorine atom gains an electron, it becomes a negatively charged ion. Interpreting Diagrams What happens to the protons and neutrons during these changes?
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25. Trends in Ionization Energy
5.3
Periodic Trends
>
Trends in Ionization Energy
The energy required to remove an electron from an ion with a 1+ charge is called the second ionization energy.
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26. Trends in Ionization Energy
5.3
Periodic Trends
>
Trends in Ionization Energy
Group and Periodic Trends in Ionization Energy
First ionization energy tends to increase from left to right across a period and decrease from top to bottom within a group.
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27. Trends in Ionization Energy
5.3
Periodic Trends
>
Trends in Ionization Energy
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28. Trends in Ionization Energy
5.3
Periodic Trends
>
Trends in Ionization Energy
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29. Trends in Ionization Energy
5.3
Periodic Trends
>
Trends in Ionization Energy
First ionization energy tends to increase from left to right across a period and decrease from top to bottom within a group. Predicting Which element would have the larger first ionization energy—an alkali metal in period 2 or an alkali metal in period 4?
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30. Ionization Energy, continued
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Ionization Energy, continued
In general, ionization energies of the main-group elements increase across each period.
This increase is caused by increasing nuclear charge.
A higher charge more strongly attracts electrons in the same energy level.
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31. In general, nonmetals have higher ionization energy than metals.
What group has the highest ionization energy? Noble Gases
What group has the lowest ionization energy? Alkali Metals.
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32. Ionization Energy, continued
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Ionization Energy, continued
Among the main-group elements, ionization energies generally decrease down the groups.
Electrons removed from atoms of each succeeding element in a group are in higher energy levels, farther from the nucleus.
The electrons are removed more easily.
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33. Ionization Energy, continued
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Ionization Energy, continued
Periodic trends in ionization energy are shown in the graph below.
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34. Chapter menu Resources
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35. Ionization Energy, continued
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Ionization Energy, continued
Sample Problem F
Consider two main-group elements, A and B. Element A has a first ionization energy of 419 kJ/mol. Element B has a first ionization energy of 1000 kJ/mol. Decide if each element is more likely to be in the s block or p block. Which element is more likely to form a positive ion?
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36. Ionization Energy, continued
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Ionization Energy, continued
Sample Problem F Solution
Element A has a very low ionization energy, which means that atoms of A lose electrons easily.
Element A is most likely to be an s-block metal because ionization energies increase across the periods.
Element B has a very high ionization energy which means that atoms of B have difficulty losing electrons.
Element B would most likely lie at the end of a period in the p block.
Element A is more likely to form a positive ion because it has a much lower ionization energy than element B does.
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37. Now practice pg. 156 #1a-e TEXTBOOK PRACTICE PROBLEMS
If you need more room, you may attach notebook paper.
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38. Now practice pg. 156 #1a-e TEXTBOOK PRACTICE PROBLEMS
If you need more room, you may attach notebook paper.
ANSWERS
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39. Ionization Summary videoclip - show this
Visual Concepts
Chapter 5
Ionization Summary videoclip - show this
Click below to watch the Visual Concept.
Visual Concept
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40. Chapter 5 Electron Affinity
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Electron Affinity
The energy change that occurs when an electron is acquired by a neutral atom is called the atom’s electron affinity.
Electron affinity generally increases across periods and as electrons add to the same p sublevel of atoms with increasing nuclear charge, electron affinities become more negative. The halogen group gains electrons easier than other groups and has a large negative value of electron affinities. The more negative the value, the easier it is to attract another electron.
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41. Chapter 5 Electron Affinity
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Electron Affinity
Increasing nuclear charge along the same sublevel attracts electrons more strongly
Electron affinity generally decreases down groups.
The larger an atom’s electron cloud is, the farther away its outer electrons are from its nucleus.
Second electron affinities are always positive because it is always harder to add a second electron to an already negatively charged ion.
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42. Chapter 5 Electron Affinity
Visual Concepts
Chapter 5
Electron Affinity
Click below to watch the Visual Concept.
Visual Concept
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43. General trend for Electron Affinity
NEED TO ADD WITH NOTES
General trend for Electron Affinity
Notice opposite trend of ionization energy
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44. 5.3
Periodic Trends
>
Trends in Ionic Size
Trends in Ionic Size
During reactions between metals and nonmetals, metal atoms tend to lose electrons, and nonmetal atoms tend to gain electrons. The transfer has a predictable effect on the size of the ions that form.
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45. Comparing Cations and Anions
Visual Concepts
Chapter 5
Comparing Cations and Anions
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46. Chapter 5 Ionic Radii A positive ion is known as a cation.
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Ionic Radii
A positive ion is known as a cation.
The formation of a cation by the loss of one or more electrons always leads to a decrease in atomic radius.
The electron cloud becomes smaller.
The remaining electrons are drawn closer to the nucleus by its unbalanced positive charge.
A negative ion is known as an anion.
The formation of an anion by the addition of one or more electrons always leads to an increase in atomic radius.
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47. 5.3
Periodic Trends
>
Trends in Ionic Size
Cations are always smaller than the atoms from which they form. Anions are always larger than the atoms from which they form.
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48. Chapter 5 Ionic Radii, continued
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Ionic Radii, continued
Cationic and anionic radii decrease across a period.
The electron cloud shrinks due to the increasing nuclear charge acting on the electrons in the same main energy level.
The outer electrons in both cations and anions are in higher energy levels as one reads down a group.
There is a gradual increase of ionic radii down a group.
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49. Relative Sizes of Some Atoms and Ions
5.3
Periodic Trends
>
Trends in Ionic Size
Relative Sizes of Some Atoms and Ions
This diagram compares the relative sizes of atoms and ions for selected alkali metals and halogens. The data are given in picometers. Comparing and Contrasting What happens to the radius when an atom forms a cation? When an atom forms an anion?
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50. Chapter 5 Ionic Radius Visual Concepts Chapter menu Resources
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51. Trends in Ionic Size 5.3 > Size of cation increases
Periodic Trends
>
Trends in Ionic Size
Trends in Ionic Size
Size of cation increases
Size of anion increases
Size generally increases
The ionic radii for cations and anions decrease from left to right across periods and increase from top to bottom within groups.
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52. Chapter 5 Valence Electrons
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Valence Electrons
Chemical compounds form because electrons are lost, gained, or shared between atoms.
The electrons that interact in this manner are those in the highest energy levels.
The electrons available to be lost, gained, or shared in the formation of chemical compounds are referred to as valence electrons.
Valence electrons are often located in incompletely filled main-energy levels.
example: the electron lost from the 3s sublevel of Na to form Na+ is a valence electron.
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53. Valence Electrons - SHOW THIS
Visual Concepts
Chapter 5
Valence Electrons - SHOW THIS
Click below to watch the Visual Concept.
Visual Concept
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54. Electronegativity: the ability of an atom in a bond to pull on the electron. (Linus Pauling)

55. Chapter 5 Electronegativity
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Electronegativity
Valence electrons hold atoms together in chemical compounds.
In many compounds, the negative charge of the valence electrons is concentrated closer to one atom than to another.
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56. Chapter 5 Electronegativity
Visual Concepts
Chapter 5
Electronegativity
Click below to watch the Visual Concept.
Visual Concept
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57. Trends in Electronegativity
5.3
Trends in Electronegativity
Electronegativity is a measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound.
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.
Periodic Trends
>
Trends in Electronegativity
Electronegativities tend to increase across periods, and decrease or remain about the same down a group.
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58. Trends in Electronegativity
5.3
Periodic Trends
>
Trends in Electronegativity
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59. Trends in Electronegativity
5.3
Periodic Trends
>
Trends in Electronegativity
Only the Representative Elements in Groups 1A through 7A
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0.7 also 59
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60. GENERAL TREND FOR ELECTRONEGATIVITY ADD TO NOTES
Periodic Trends
>
GENERAL TREND FOR ELECTRONEGATIVITY ADD TO NOTES
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61. Electronegativity, continued
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Electronegativity, continued
Sample Problem G
Of the elements gallium, Ga, bromine, Br, and calcium, Ca, which has the highest electronegativity? Explain your answer in terms of periodic trends.
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62. Electronegativity, continued
Section 3 Electron Configuration and Periodic Properties
Chapter 5
Electronegativity, continued
Sample Problem G Solution
All of these elements are in the fourth period.
Bromine has the highest atomic number and is farthest to the right in the period.
Bromine should have the highest electronegativity because electronegativity increases across the periods.
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63. Practice Problems pg. 162-163 Chapter menu Resources
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64. Practice Problems pg. 162-163 ANSWERS Chapter menu Resources
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65. Periodic Properties of the d- and f-Block Elements
*The atomic radii of the d-block elements generally decrease across the periods.
*Ionization energies of the d-block and f-block elements generally increase across the periods. The first ionization energies of the d-block generally decrease down each group because the electrons available for ionization in the outer s sublevels are less shielded from the increasing nuclear charge by electrons in the d sublevels.
*The d-block elements also follow the general trend for electronegativity values to increase as radii decrease.
The f-block elements all have similar electronegativities.
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66. Summary of Trends What is the underlying cause of periodic trends? 5.3
>
Summary of Trends
Summary of Trends
What is the underlying cause of periodic trends?
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67. 5.3
Periodic Trends
>
Summary of Trends
The trends that exist among these properties can be explained by variations in atomic structure.
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68. BASIC SUMMARY OF TRENDS ARROWS SHOW IN DIRECTION OF INCREASE
Periodic Trends
>
BASIC SUMMARY OF TRENDS ARROWS SHOW IN DIRECTION OF INCREASE
Electronegativity increases &
& Ionic Radii increase right to left
(or decrease across periods (left to right))
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69. Assess students’ understanding of the concepts in Section 5.3
Section Assessment
Assess students’ understanding of the concepts in Section
5.3
Continue to: Launch:
-or-
Section Quiz
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70. 1. Which of the following sequences is correct for atomic size?
5.3 Section Quiz
1. Which of the following sequences is correct for atomic size?
Mg > Al > S
Li > Na > K
F > N > B
F > Cl > Br
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71. gain electrons to form cations. gain electrons to form anions.
5.3 Section Quiz
2. Metals tend to
gain electrons to form cations.
gain electrons to form anions.
lose electrons to form anions.
lose electrons to form cations.
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72. 3. Which of the following is the most electronegative? Cl Se Na I
5.3 Section Quiz
3. Which of the following is the most electronegative? Cl Se Na I
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73. Online Self-Check Quiz
Complete the online Quiz and record answers. Ask if you have any questions about your answers.
click here for online Quiz 5.3
(10 questions)
You must be in the “Play mode” for the slideshow for hyperlink to work.
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74. SCI LINKS FOR CHAPTER Additional Student SCI LINKS for CHAPTER 5
The NSTA-sponsored SciLinks Web site contains links to accurate and up-to-date science
information on the Internet. Just click on the button below to go to the SciLinks site at
and log in. Then, type in the SciLinks code for the topic you want to
research. The following is a list of the SciLinks codes for this chapter.
Chapter 5: The Periodic Law
Topic: Periodic Table
SciLinks code: HC61125
Topic: Noble Gases
SciLinks code: HC61038
Topic: Alkali Metals
SciLinks code: HC60043
Topic: Alkaline-Earth Metals
SciLinks code: HC60044
Topic: Halogens
SciLinks code: HC60710
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75. VIDEOS FOR ADDITIONAL INSTRUCTION
Additional Videos for
Section 5.3: Electron Configuration and Periodic Properties
Atomic Radii - Ionic Radii (3:38)
Ionization Energy - Periodic Trends (2:37)
Valence Electrons (2:19)
Electronegativity (4:26)
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