Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

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Presentation transcript:

Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen 2.To learn about valence electrons and core electrons 3.To learn about the electron configurations of atoms with Z < 18 4.To understand the general trends in properties in the periodic table Objectives

Section 11.4 Electron Configurations and Atomic Properties A. Electron Arrangements in the First 18 Atoms on the Periodic Table H atom –Electron configuration – electron arrangement – 1s 1 –Orbital diagram – orbital is a box grouped by sublevel containing arrow(s) to represent electrons

Section 11.4 Electron Configurations and Atomic Properties A. Electron Arrangements in the First 18 Atoms on the Periodic Table He atom –Electron configuration– 1s 2 –Orbital diagram

Section 11.4 Electron Configurations and Atomic Properties A. Electron Arrangements in the First 18 Atoms on the Periodic Table

Section 11.4 Electron Configurations and Atomic Properties Look at electron configurations for K through Kr B. Electron Configurations and the Periodic Table

Section 11.4 Electron Configurations and Atomic Properties Orbital filling and the periodic table B. Electron Configurations and the Periodic Table

Section 11.4 Electron Configurations and Atomic Properties B. Electron Configurations and the Periodic Table

Section 11.4 Electron Configurations and Atomic Properties C. Atomic Properties and the Periodic Table Metals and Nonmetals Metals tend to lose electrons to form positive ions. Nonmetals tend to gain electrons to form negative ions.

Section 11.4 Electron Configurations and Atomic Properties C. Atomic Properties and the Periodic Table Atomic Size Size tends to increase down a column. Size tends to decrease across a row.

Section 11.4 Electron Configurations and Atomic Properties C. Atomic Properties and the Periodic Table Ionization Energies Ionization Energy – energy required to remove an electron from an individual atom (gas) –Tends to decrease down a column –Tends to increase across a row