The Greatest Table on Earth!!!

1. The Periodic Table of Elements The Greatest Table on Earth!!!

2. Periodic Table • Ever wondered: • Why the Periodic Table is shaped the way it is? • Why is it called the Periodic Table? • Why are there 2 disconnected rows? • What information does it have? • Well today is your lucky day, because we are about to find out!

3. Periodic Table • The Periodic Table of the Elements shows every known type of atom. • It contains a large amount of information • Much of the information we can get just from the organization and shape of the periodic table

4. The Beginning • The Periodic Table was first made in 1869 by a Russian named Dmitri Mendeleev • His table looked something like this: What do you notice about his periodic table?

5. Mendeleev’s Periodic Table • Mendeleev ordered the elements by their atomic mass (he didn’t know protons existed yet) • He grouped those similar elements into columns • He started a new column every time the physical or chemical properties changed • Mendeleev left spaces for new, undiscovered elements and tried to predict their properties

6. Mendeleev’s Periodic Table • As years went on, several elements were discovered • Their properties were nearly identical to those that Mendeleev predicted

7. What Mendeleev’s Predictions Tell Us? • Mendeleev showed us there are patterns and trends to the elements • These patterns show us we can organize the elements by their properties

8. Atomic Number • The most obvious way that the periodic table is organized by increasing atomic number • However, this doesn’t explain why the elements are grouped the way they are

9. Atomic Mass • The atomic mass also increases (generally) as the atomic number increases • This, also, does not explain the element groupings

10. Periods • Rows on the periodic table are called periods

11. Periods • Elements are organized into periods based on where their electrons are • The outermost orbital filled by electrons determines what period an element is in • If an elements outermost electrons are in the 1storbital, the element is in the 1st period • If an elements outermost electrons are in the 4th orbital, the element is in the 4th period

12. Groups • The vertical columns of the periodic table are organized by common physical and chemical properties • Why do you think these groups have similar properties?

13. Groups • Draw an atom of hydrogen, lithium, and sodium. • What do you notice about each of these atoms?

14. Groups • Each atom has 1 electron in it’s outside orbital • Remember that electrons determine an atoms behaviour • Since each atom has the same number of electrons in its outside orbital, they all behave the same Na H Li

15. Groups • This outside orbital is the same for every atom in a group • This means that atoms in a group behave pretty much the same • Now let’s take a look at some notable groups

16. Group 1 • Group 1 are called alkali metals • They include the entire first column (excluding hydrogen) • They all: • Are soft, shiny, grey metals • Are extremely reactive • Have low densities, low hardness, and low boiling points • All burn with red, pink, or yellow colours

17. Group 2 • Group 2 are called Alkali Earth Metals • Includes Beryllium, Magnesium, Calcium, Strontium, Barium, and Radium • All are somewhat shiny, silvery-white, and are much harder than group 1 • All make strong bases when mixed with water • Are about twice as dense as group 1

18. Group 17 • Group 17 are called halogens • Contains Fluorine, Chlorine, Bromine, Iodine, and Astatine • All are extremely reactive • All are extremely dangerous to living things (except iodine) • All make acids with hydrogen • All are vividly coloured

19. Group 18 • Group 18 are called the Noble Gases • They include helium, neon, krypton, argon, xenon, and radon • Are all gases • All do not react at all • All glow with bright colours when electricity is passed through them

20. Metals to Non-metals • The periodic table also organizes metals all the way to what are called non-metals • Metals are materials that: • Have a shiny lustre • Conduct electricity • Conduct heat • Are malleable

21. Transition Metals • The transition metals go from group 3 (scandium group) to group 12 (zinc group) • They are all conductors of electricity and heat • They all have a shiny lustre

22. Transition Metals • They are all malleable • They are all silver except for gold and copper • The only 3 magnetic elements are in the transition metals • Iron • Cobalt • Nickel

23. Poor Metals • Poor metals are in group 13, 14, 15, and 16 • Below the ‘staircase’ • Are very malleable • Very soft • Poor electrical conductors • Low boiling points

24. Non-metals • Non-metals do not conduct electricity or heat • Have a dull lustre (mostly) • Are brittle • Not malleable • Exist as solids, liquids, and gasses • Most are brightly coloured

25. The ‘Staircase’ • Between the poor metals and the non-metals is a staircase • This line shows a separation between elements that act like metals and elements that don’t

26. Metalloids • Elements along the staircase are called metalloids • They act like metals and non-metals • Includes boron, silicon, germanium, arsenic, antimony, tellurium, and polonium

27. Metalloids • Metalloids conduct some electricity • The hotter they are, the more conductive they are • Somewhat brittle • Shiny lustre • Make computers possible

28. Lanthanides & Actinides • The ‘disconnected’ rows of the periodic table are called the lanthanides and actinides • They are all radioactive • All are very reactive Lanthanides Actinides

29. Blocks • New information about how electrons work has taught us about things called shells • The periodic table is also organized by which electron shell is furthest to the outside of an atom • There are 4 shells • S – shaped like spheres • P – shaped like dumbbells • D – many shapes • F – many shapes

30. Groups • All atoms in the ‘s’ block have their outer most electrons in the ‘s-shell’ • All elements in the ‘d’ block have their outer most electrons in the ‘d-shell’ • And so on…