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

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!

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

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?

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

Mendeleev’s Periodic Table As years went on, several elements were discovered Their properties were nearly identical to those that Mendeleev predicted Eka-aluminium (Ea) (Mendeleev’s Prediction) Gallium (Ga) (Discovered Element) Atomic weight About 68 69.72 Density of solid 6.0 g/cm3 5.9 g/cm3 Melting point low 29.78oC Valency 3

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

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

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

Periods Rows on the periodic table are called periods

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 1st orbital, the element is in the 1st period If an elements outermost electrons are in the 4th orbital, the element is in the 4th period

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?

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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…