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Slide 1 of 31 Periodic Trends 6.3 Section Periodic Trends II
Slide 2 of 31 © Copyright Pearson Prentice Hall 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
© Copyright Pearson Prentice Hall Slide 3 of 31 Periodic Trends > Trends in Ionization Energy What are the trends among the elements for first ionization energy, ionic size, and electronegativity? 6.3-2
© Copyright Pearson Prentice Hall Slide 4 of 31 Periodic Trends > Trends in Ionization Energy ionization energy The energy required to remove an electron from an atom is called ionization energy. The energy required to remove the first electron from an atom is called the first ionization energy. The energy required to remove an electron from an ion with a 1+ charge is called the second ionization energy
© Copyright Pearson Prentice Hall Slide 5 of 31 Periodic Trends > Trends in Ionization Energy Group and Periodic Trends in Ionization Energy First ionization energy tends to decrease from top to bottom within a group and increase from left to right across a period
© Copyright Pearson Prentice Hall Slide 6 of 31 Periodic Trends > Trends in Ionization Energy 6.3-2
© Copyright Pearson Prentice Hall Slide 7 of 31 Periodic Trends > Trends in Ionization Energy Largest Smallest
© Copyright Pearson Prentice Hall Slide 8 of 31 Periodic Trends > Trends in Ionization Energy smallest largest
Slide 9 of 31 © Copyright Pearson Prentice Hall Periodic Trends > Trends in Electronegativity Electronegativity is the ability of an atom of an element to attract electrons when the atom is in a 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
Slide 10 of 31 © Copyright Pearson Prentice Hall Periodic Trends > Trends in Electronegativity Representative Elements in Groups 1A through 7A Largest Smallest
© Copyright Pearson Prentice Hall Periodic Trends > Slide 11 of 31 Summary of Trends What is the underlying cause of periodic trends? 6.3-2
Slide 12 of 31 © Copyright Pearson Prentice Hall Periodic Trends > Summary of Trends The trends that exist among these properties can be explained by variations in atomic structure
© Copyright Pearson Prentice Hall Slide 13 of 31 Periodic Trends > Summary of Trends Atomic Size Increases Decreases Size of cationsShieldingNuclear ChargeElectronegativityIonization energySize of anionsIonic size Constant 6.3-2
© Copyright Pearson Prentice Hall Slide 14 of Which of the following sequences is correct for atomic size? a.Mg > Al > S b.Li > Na > K c.F > N > B d.F > Cl > Br 6.3 Section Quiz
© Copyright Pearson Prentice Hall Slide 15 of Section Quiz 2. Metals tend to a.gain electrons to form cations. b.gain electrons to form anions. c.lose electrons to form anions. d.lose electrons to form cations.
© Copyright Pearson Prentice Hall Slide 16 of Section Quiz 3. Which of the following is the most electronegative? a.Cl b.Se c.Na d.I
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Slide 1 of 31 Periodic Trends 6.3. © Copyright Pearson Prentice Hall Slide 2 of 31 Periodic Trends Sodium chloride (table salt) produced the geometric.
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Periodic Trends. Definition: Half of the distance between nuclei in covalently bonded diatomic molecule Radius decreases across a period Increased.
Trends in the periodic table: Ionization Energy Atomic Radius Electron Affinity Electronegativity.
Periodic Table and Periodic Trends Notes. Mendeleevs Periodic Table By the mid-1800s, about 70 elements were known to exist By the mid-1800s, about 70.
Periodic Properties of the Elements Early versions of the Periodic table were constructed by Mendeleev and Meyer. We now know that the periodic properties.
Atomic size a) Ne or Ar b) B or C c) P or Ge Patterns in Atomic Size Electron configuration for Br: [Ar]4s 2 3d 10 4p 5, valence electron configuration.
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The properties of Periodic table of elements.. Under normal conditions each atom is electrically neutral, since the number of electrons is equal to that.
Periodic Trends u OBJECTIVES: Interpret group trends in atomic radii, ionic radii, ionization energies, m.p., b.p., electronegativity and chemical properties.
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Periodic Trends (SL) u OBJECTIVES: Interpret group and period trends in atomic radii, ionic radii, ionization energies and electronegativity (m.p., b.p.,
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