SUMMARY OF PERIODIC TRENDS IN PROPERTIES Summarizing Periodic

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SUMMARY OF PERIODIC TRENDS IN PROPERTIES Summarizing Periodic Table Organization • The periodic table

SUMMARY OF PERIODIC TRENDS IN PROPERTIES Summarizing Periodic Table Organization • The periodic table is divisible into four blocks corresponding to the filling of the four quantum sublevels (s, p, d, and f ). • The group number of a main-group element is equal to the number of valence electrons for that element. • The row number of a main-group element is equal to the highest principal quantum number of that element. © 2015 Pearson Education, Ltd.

Metallic Behavior and Electron Configuration © 2015 Pearson Education, Ltd.

Metallic Behavior and Electron Configuration © 2015 Pearson Education, Ltd.

Electron Configuration and Ion Formation • Ion formation can be predicted by an element’s

Electron Configuration and Ion Formation • Ion formation can be predicted by an element’s location in the periodic table. • These atoms form ions that will result in an electron configuration that is the same as that of the nearest noble gas. • Metals form cations (positively charged atoms). – Alkali metals (group 1 A) form only +1 cations. – Alkaline earth metals (group 2 A) form only +2 cations. – Transition, inner transition, and p-block metals form a variety of charged cations. • Nonmetals form anions (negatively charged atoms). – Halogens (group 7 A) usually gain one electron to form – 1 anions. – Other nonmetals can form a variety of charged anions. © 2015 Pearson Education, Ltd.

Electron Configuration and Ion Formation: Elements that Form Ions with Predicable Charges © 2015

Electron Configuration and Ion Formation: Elements that Form Ions with Predicable Charges © 2015 Pearson Education, Ltd.

Problem Solving: Predicting Ionic Charge © 2015 Pearson Education, Ltd.

Problem Solving: Predicting Ionic Charge © 2015 Pearson Education, Ltd.

Problem Solving: Predicting Atomic Radii © 2015 Pearson Education, Ltd.

Problem Solving: Predicting Atomic Radii © 2015 Pearson Education, Ltd.

Summary on First Ionization Energy for Quantum-Mechanical Explanation for the Main-Group Elements Trends in

Summary on First Ionization Energy for Quantum-Mechanical Explanation for the Main-Group Elements Trends in First Ionization Energy First ionization energy generally • decreases as we move down a column (or family) in the periodic table because electrons in the outermost principal level are increasingly farther away from the positively charged nucleus and are therefore held less tightly; • increases as we move across (left to right) a row (or period) in the periodic table because electrons in the outermost principal energy level experience a greater attraction to the nucleus. © 2015 Pearson Education, Ltd.

Characteristics of Metals versus Nonmetals • Metals – Malleable and ductile – Shiny, lustrous,

Characteristics of Metals versus Nonmetals • Metals – Malleable and ductile – Shiny, lustrous, reflect light – Conduct heat and electricity – Most oxides basic and ionic – Form cations in solution – Lose electrons in reactions—oxidized © 2015 Pearson Education, Ltd. • Nonmetals – Brittle in solid state – Dull, nonreflective, solid surface – Electrical and thermal insulators – Most oxides acidic and molecular – Form anions and polyatomic anions – Gain electrons in reactions—reduced

Periodic Trend: Metallic Character © 2015 Pearson Education, Ltd.

Periodic Trend: Metallic Character © 2015 Pearson Education, Ltd.

Ionization Energy Problem © 2015 Pearson Education, Ltd.

Ionization Energy Problem © 2015 Pearson Education, Ltd.

Problem Solving: Ionization Energy © 2015 Pearson Education, Ltd.

Problem Solving: Ionization Energy © 2015 Pearson Education, Ltd.

Electron Problem Configuration Solving: Core and the Valence Periodic Electrons. Table © 2015 Pearson

Electron Problem Configuration Solving: Core and the Valence Periodic Electrons. Table © 2015 Pearson Education, Ltd.