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Section 7.1 Present-Day Atomic Theory
Section 7.2 The Periodic Table and Atomic Structure
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4. Present-Day Atomic Theory
Relate emission spectra to the electron configurations of atoms.
Relate energy sublevels and orbitals within the atom.
Section 7.1

5. Present-Day Atomic Theory
electromagnetic spectrum: the entire range of electromagnetic radiation
Section 7.1

6. Present-Day Atomic Theory
sublevel
aufbau principle
Heisenberg uncertainty principle
orbital
electron configuration
Electrons are organized in energy levels and sublevels.
Section 7.1

7. Expanding the Model of the Atom
Danish physicist Niels Bohr suggested that electrons revolve around the nucleus like planets revolve around the Sun.
Section 7.1

8. Expanding the Model of the Atom (cont.)
Bohr’s model explained hydrogen’s emission spectrum, but failed to explain any other element’s emission spectrum.
The current atomic model explains electron behavior by interpreting the emission spectra of all the elements.
Section 7.1

9. Expanding the Model of the Atom (cont.)
The periodic table reflects each element’s electron arrangement.
Section 7.1

10. Expanding the Model of the Atom (cont.)
To calculate the exact amount of energy released by the electrons in atoms:
the higher the frequency of a wave and the shorter wavelength, the greater the energy of the radiation
the lower the frequency and the longer the wavelength, the lower the energy released
Section 7.1

11. Expanding the Model of the Atom (cont.)
Section 7.1

12. Expanding the Model of the Atom (cont.)
By absorbing a specific amount of energy, an electron can jump to a higher energy level.
When the electron falls back to the lower energy level, it releases the same amount of energy in the form of radiation with a definite frequency.
Section 7.1

13. Expanding the Model of the Atom (cont.)
Section 7.1

14. Expanding the Model of the Atom (cont.)
Energy levels within an atom are characteristic of each element.
Section 7.1

15. Expanding the Model of the Atom (cont.)
Closely spaced lines in a spectrum suggest that sublevels—divisions within a level—exist within an energy level.
The energy sublevels are indicated as s, p, d, or f.
Section 7.1

16. Expanding the Model of the Atom (cont.)
The aufbau principle states that each electron occupies the lowest energy sublevel available.
Section 7.1

17. Electrons Distribution in Energy Levels
Each energy level has a specific number of sublevels, which is the same number of the energy level.
Section 7.1

18. Electrons Distribution in Energy Levels (cont.)
Section 7.1

19. Electrons Distribution in Energy Levels (cont.)
The Heisenburg uncertainty principle states that it is fundamentally impossible to know precisely both the velocity and position of a particle at the same time.
Section 7.1

20. Electrons Distribution in Energy Levels (cont.)
The only quantity that can be known is the probability for an electron to occupy a certain region around the nucleus.
Section 7.1

21. Electrons Distribution in Energy Levels (cont.)
The space in which there is a high probability of finding an electron is called an orbital.
Each energy level relates to orbitals of different sizes and shapes.
Section 7.1

22. Electrons Distribution in Energy Levels (cont.)
Section 7.1

23. Electrons Distribution in Energy Levels (cont.)
The most stable arrangement of electrons in sublevels and orbitals is called an electron configuration.
Because orbitals are mostly empty space, this space can be used by another pair of electrons and the orbitals can overlap.
Section 7.1

24. Section Assessment
Atoms move in circular orbits in which atomic model?
A. quantum mechanical model
B. Rutherford’s model
C. Bohr’s model
D. de Broglie’s model
Section 7.1

25. Section Assessment Electron behavior is explained by interpreting ___.
A. emission spectra
B. the number of energy levels
C. how quickly the electrons revolve around the nucleus
D. the number of covalent bonds
Section 7.1

26. End of Section 7.1

27. The Periodic Table and Atomic Structure
Distinguish the s, p, d, and f blocks on the periodic table and relate them to an element’s electron configuration.
Predict the electron configurations of elements using the periodic table.
Section 7.2

28. The Periodic Table and Atomic Structure
orbital: space in which there is a high probability of finding an electron
Section 7.2

29. The Periodic Table and Atomic Structure
inner transition element
A predictable pattern can be used to determine electron arrangement in an atom.
Section 7.2

30. Patterns of Atomic Structure
The shape of the modern periodic table is a direct result of the order in which electrons fill energy sublevels and their orbitals.
Section 7.2

31. Building Electron Configurations
Chemical properties repeat when elements are arranged by atomic number because electron configurations repeat in a certain pattern.
Section 7.2

32. Building Electron Configurations (cont.)
Section 7.2

33. Building Electron Configurations (cont.)
Noble gas notation uses symbols in brackets to shorten inner electron configurations of other elements.
The stable electron configurations explain the lack of reactivity of the noble gases.
Section 7.2

34. Building Electron Configurations (cont.)
Section 7.2

35. Building Electron Configurations (cont.)
Experimental evidence indicates that the 4s and 3d sublevels are close in energy, with the 4s sublevel having a slightly lower energy.
Section 7.2

36. Building Electron Configurations (cont.)
The transition elements are any of the elements in group 3 through 12 of the periodic table, all of which are metals.
They lose electrons to attain a more stable configuration.
Most have multiple oxidation numbers because their s and d orbitals are so close in energy that electrons can be lost from both orbitals.
Section 7.2

37. Building Electron Configurations (cont.)
The lanthanides and actinides are called the inner transition elements because their last electron occupies a 5f orbital in the seventh period.
Section 7.2

38. The Size of the Orbitals
The higher the energy, the farther the outermost electrons are from the nucleus.
As the valence electron gets farther from the nucleus, the s orbital it occupies gets larger and larger.
Section 7.2

39. Section Assessment
As the valence electron gets farther from the nucleus, its s orbital becomes:
A. positively charged
B. negatively charged
C. larger
D. smaller
Section 7.2

40. Section Assessment
The most common oxidation number for the inner transition elements is:
A. 1+
B. 2+
C. 3+
D. 4+
Section 7.2