1. The Periodic Table & Quantum Theory
Unit 2
The Periodic Table & Quantum Theory

2. Mendeleev’s Periodic Table
6.1
Mendeleev’s Periodic Table
Mendeleev’s Periodic Table – THE FIRST
Arranged the elements in his periodic table in order of increasing atomic mass
Also arranged using properties of the elements
The periodic table can be used to predict the properties of undiscovered elements.
1869

3. Mendeleev’s Periodic Table
6.1
Mendeleev’s Periodic Table
An Early Version of Mendeleev’s Periodic Table
A Song
Another Song
In this early version of Mendeleev’s periodic table, the rows contain elements with similar properties. Observing A fourth element is grouped with chlorine (Cl), bromine (Br), and (I) iodine. What is this element’s symbol?

4. The MODERN Periodic Table
6.1
The Periodic Law
The MODERN Periodic Table
Elements are arranged in order of increasing atomic number.
Another Song
In the modern periodic table, the elements are arranged in order of increasing atomic number. Interpreting Diagrams How many elements are there in the second period?

5. 6.1
Periodic Law
When elements are arranged in order of increasing atomic number, a repeating pattern of properties can be seen.

6. Searching For an Organizing Principle
6.1
Searching For an Organizing Principle
Elements with similar properties are grouped in a columns (up and down)
Called groups or FAMILIES

7. Squares in the Periodic Table
6.2
Squares in the Periodic Table
The Group 1A elements are called alkali metals.
The Group 2A elements are called alkaline earth metals.
Alkali Metal Reactions
Alkaline Earth Metal Reactions

8. The nonmetals of Group 7A are called halogens.
Halogen Video
Group 8A – noble gases
Noble Gases

9. Metals, Nonmetals, and Metalloids
6.1
Metals, Nonmetals, and Metalloids
Three Kinds of Elements
One way to classify elements in the periodic table is as metals, nonmetals, and metalloids. Inferring What is the purpose for the black stair-step line?

10. Metals, Nonmetals, and Metalloids
6.1
Metals, Nonmetals, and Metalloids
Metals
Most elements are metals
High luster (shiny)
Ductile (able to be pulled into a wire)
Malleable (able to be bent)
Good conductors of heat and electricity

11. Metals, Nonmetals, and Metalloids
6.1
Metals, Nonmetals, and Metalloids
Metalloids
A metalloid generally behaves kind of like a metal and kind of like a nonmetal.
Information about Metalloids

12. Metals, Nonmetals, and Metalloids
6.1
Metals, Nonmetals, and Metalloids
Nonmetals
Most are gases at room temperature.
Some are solids(sulfur and phosphorus & iodine)
One nonmetal, bromine, is a dark-red liquid
Poor conductors of heat and electricity

13. Periodic Trend - Atomic Radius
Distance from the nucleus to the edge of the electron cloud.

16. Periodic Trend - Electronegativity
Electronegativity is the power of an atom to attract an electron
Higher the number them more an atom wants an electron
Highest number is flourine

18. The Development of Atomic Models
5.1
The Development of Atomic Models
A NEW Question
Rutherford’s atomic model could not explain why objects change color when heated.
Rutherford’s model fails to explain why objects change color when heated. As the temperature of this horseshoe is increased, it first appears black, then red, then yellow, and then white. The observed behavior could be explained only if the atoms in the iron gave off light in specific amounts of energy. A better atomic model was needed to explain this observation.

19. The Development of Atomic Models
5.1
The Development of Atomic Models
The timeline shows the development of atomic models from 1803 to 1911.
These illustrations show how the atomic model has changed as scientists learned more about the atom’s structure.

20. The Development of Atomic Models
5.1
The Development of Atomic Models
The timeline shows the development of atomic models from 1913 to 1932.
These illustrations show how the atomic model has changed as scientists learned more about the atom’s structure.

21. 5.1
The Bohr Model
The Bohr Model
Bohr proposed that an electron is found only in specific circular paths, or orbits, around the nucleus.

22. Electrons have fixed energy Fixed energies are called energy levels
5.1
The Bohr Model
BOHR Findings
Electrons have fixed energy
Fixed energies are called energy levels
Quantum is the amount of energy required to move an electron from one energy level to another energy level.

23. Energy Levels are Kind Of Like a Ladder Because…
5.1
The Bohr Model
Energy Levels are Kind Of Like a Ladder Because…
Energy levels are spaced out (not all equally)
Ground State – close to the nucleus (low energy)
Excited states – move away from lowest energy level – move up the ladder – higher energy
These ladder steps are somewhat like energy levels. In an ordinary ladder, the rungs are equally spaced. The energy levels in atoms are unequally spaced, like the rungs in this ladder. The higher energy levels are closer together.

24. The Quantum Mechanical Model
5.1
The Quantum Mechanical Model
Erwin Schrödinger (1887–1961)
Quantum mechanical model
Mathematical proof
Creates a “fuzzy” cloud of where electrons are likely to be found
Give an address to location using quantum numbers.

25. The Electromagnetic Spectrum
5.3
Light
The Electromagnetic Spectrum

26. Electromagnetic Radiation
5.3
Light
Electromagnetic Radiation
Travels at  108 m/s.
Only small potion is visible
Non visible
Radio waves
Microwaves
Infrared waves
UV (ultra violet)
X-rays
Gamma Rays

27. Important Words When Talking About Radiation
5.3
Light
Important Words When Talking About Radiation
Wavelength - is the distance between the crests.
Frequency - is the number of wave cycles to pass a given point per unit of time (measured in Hertz or Hz)

28. 5.3
Light
The wavelength and frequency of light are inversely proportional to each other.
The frequency and wavelength of light waves are inversely related. As the wavelength increases, the frequency decreases.

29. Slinky Demonstrations
What is the relationship between energy and wavelength and frequency?

30. Where is the HIGH ENERGY Radiation?
5.3
Light
Where is the HIGH ENERGY Radiation?
Describe the frequency and the wavelength of the high energy radiation.

31. Atomic Spectra & How is it Created?
5.3
Atomic Spectra
Atomic Spectra & How is it Created?
Atoms absorb energy
Electrons move into higher energy levels.
Electrons then lose energy by emitting light
Return to lower energy levels.

32. Each line in spectrum represents energy levels!
5.3
Atomic Spectra
Each line in spectrum represents energy levels!
Mercury
No two elements have the same emission spectrum. a) Mercury vapor lamps produce a blue glow. b) Nitrogen gas gives off a yellowish-orange light.

33. Flame Test Lab – Looking at Atomic Spectra

34. Electron Configurations
5.2
Electron Configurations
Give an address using quantum numbers describing where an electron lives

35. The s orbitals are spherical, and p orbitals are dumbbell-shaped.
5.1
Atomic Orbitals
Different atomic orbitals are denoted by different letters and numbers.
The s orbitals are spherical, and p orbitals are dumbbell-shaped.
The electron clouds for the s orbital and the p orbitals are shown here.

36. d orbitals f orbitals 5.1 Atomic Orbitals
The d orbitals are illustrated here. Four of the five d orbitals have the same shape but different orientations in space. Interpreting Diagrams How are the orientations of the dxy and dx2 – y2 orbitals similar? How are they different?

37. Electron Configurations
5.2
Electron Configurations
Learning How to Write Electron Configurations – Long Form

40. Electron Configurations
5.2
Electron Configurations
Method #2 = Writing a Noble Gas Configuration (the short cut way)