1. The Periodic Law Chapter 5 Pages 132 - 164

2. History of the Periodic Table Who is the father of the periodic table? Dmitri Mendeleev ~1869 He initially arranged ~60 elements in order of increasing atomic mass. What two questions remained? 1. Why could most of the elements be arranged in the order of increasing atomic mass but a few could not? 2. What was the reason for chemical periodicity? Give an example of something that is periodic. Henry Mosely, who worked with Ernest Rutherford discovered by viewing spectral data, that the table fit into patterns better when arranged by increasing nuclear charge – or increasing _________ __________.

3. History of the Periodic Table Periodicity or the periodic law states that the physical and chemical properties of the elements are functions of their atomic numbers – when elements are arranged in order of increasing atomic number, elements with similar properties appear at regular intervals.

4. Electron Configuration and the Periodic Table Based on electronic configurations of the elements, the periodic table can be divided into four blocks  s, p, d, and f.

5. Electron Configuration and the Periodic Table Alkali metals are group 1 on periodic table. silvery soft enough to be cut with a knife very reactive cannot be found in nature as free elements react strongly with water Alkaline earth metals are group 2 on the periodic table. harder, denser and stronger than group 1 higher melting points than group 1 less reactive than group 1 Groups 1 & 2 are also known as the s-block elements.

6. Electron Configuration and the Periodic Table d-block elements are called transition metals. good conductors high luster typically less reactive than groups 1 & 2 exist in nature as free elements What are three very unreactive elements listed by your text? palladium, Pd platinum, Pt gold, Au

7. Electron Configuration and the Periodic Table p-block elements are called the main-group elements all metalloids all nonmetals (except hydrogen and helium) the halogens (group 17) the halogens are the most reactive nonmetals why? because they have 7 valence electrons f-block elements are the lanthanides and actinides lanthanides are shiny and similar in reactivity to group 2 actinides are mostly laboratory-made elements

8. Electron Configuration and Periodic Properties _________ ___________ may be defined as one-half the distance between the nuclei of identical atoms that are bonded together. From left to right (across a period), atomic radii trend smaller. Why? As atomic numbers get bigger (one per element), this means that each subsequent element has one more ___________. Because of this increasing nuclear charge (or positive charge), the electrons orbiting the nucleus are pulled in closer and closer. From top to bottom (down a group), atomic radii trend larger. Why? As elements trend down a group, more s-sublevels are added and so the 1s is small, but each s sublevel is a bit larger than the previous.

9. Electron Configuration and Periodic Properties https://youtu.be/VopLrkfXfGw

10. Electron Configuration and Periodic Properties __________ __________ are available to be lost, gained, or shared in the formation of chemical compounds. They are often located in incompletely filled outer orbitals. They are the electrons that participate in chemical bonding. Often, the charge of valence electrons is concentrated closer to one atom than to another. This uneven concentration of charge has significant effects on the chemical properties of a compound. ______________ is a measure of the ability of an atom in a compound to attract electrons from another atom in a compound. The most electronegative element is fluorine. Electronegativity generally increases left to right (across a period) and decreases top to bottom (down a group). Why?

11. Electron Configuration and Periodic Properties https://youtu.be/nqaclvioesw

12. Electron Configuration and Periodic Properties

13. An ______ is an atom or group of bonded atoms that has a positive or negative charge. Any process that results in the formation of an ion is referred to as _____________. Ionization energy (IE) is the energy required to remove an electron from a neutral atom of an element. IE increases left to right (across a period) and decrease top to bottom (down a group). Why? As elements become more and more like the noble gases, more and more energy is required to remove an electron and create an ion. https://youtu.be/ksZoOde-7zY

15. The Periodic Law Slide Quiz In the modern periodic table, elements are arranged according to what? Group 17 (halogens) are the most reactive of the nonmetals because? What does the periodic law state? Across period 3 (left to right), the energy needed to remove an electron from an atom (increases/decreases)? Which element has the highest electronegativity? How does ionization trend? How does atomic radius trend? How does electronegativity trend?

16. Funny Chemistry