1. Topic 4 – Classifying Elements

2. Elements All elements were named as they were discovered.
The person who discovered the elements got to choose how it was named.
Just think… Watsonium – has a nice ring to it 
The chemist Marie Curie discovered the element polonium and named it after the country of her birth, Poland.
Uranium was named after the planet Uranus.
Einsteinium was named after the physicist Albert Einstein.

3. Naming Elements Most people named their discovered elements after:
Latin/Greek based on their properties
Themselves
Place of discovery, country or planets
From the mineral in which it was found
Named to honor a place or person
Since it would be very difficult and time consuming to write names like these over and over again, a system of element symbols was developed. The system provided symbols for all the known elements.

4. Early Chemists used symbols to name their elements.
These are some of the more common element symbols
CONFUSING!!

5. Dalton created a “better” system… but there were too many to remember… 

6. Early Chemists
Although every language has its own way of saying and spelling the names of the elements, the symbols that are used to represent the elements are the same throughout the world.

7. Now, we’ve got it!
We now use element symbols to identify the elements.
But this periodic table is out of date! Look at the incomplete bottom row!

8. New Elements! Elements 113, 115, 117 and 118
The new elements are all synthetic, and were arrived at by smashing very light nuclei into each other and tracking the elements that potentially appear in the decay tails. The issue with elements at the end of the periodic table stems from their faint stability.
The international union of applied chemistry has initiated the process of formalizing names and symbols for these elements temporarily named as ununtrium (Uut or element 113), ununpentium (Uup, element 115), ununseptium (Uus, element 117) and ununoctium (Uuo, element 118).
How to create an element:

9. Nihonium - symbol Nh, for the element 113,
Moscovium - symbol Mc, for the element 115,
Tennessine - symbol Ts, for the element 117, and.
Oganesson - symbol Og, for the element 118.

10. The current names came from….
The FIRST initial of the common name
H for Hydrogen
O for Oxygen
C for Carbon
The FIRST TWO letters (or 1st and 3rd) of the common name
Mg for Magnesium
Al for Aluminum
Initials of the Latin name
Cu for Copper (Cuprum)
Au for Gold (Aurum)

11. Elements 104 to 109
were created by laboratories in the USA, Germany and Russia over the last two decades (all discovered )
Only a few atoms of these elements ever existed and none survived after its creation for more than a few seconds before decaying radioactively into atomic debris.
To clarify – in ordinary physical or chemical processes atoms are conserved. Dalton was correct – they cannot be created or destroyed. In the physical process of evaporation or melting the only thing that changes is the separation between atoms. Water and ice are both still H20. If the atoms were to become linked in other ways then you have a chemical change (like burning, rusting or digestion) these processes create new materials (not new atoms) by recombining or disassociating the same old atoms.
As a result when we die, most of our atoms will be recycled in a sense and they will be part of future humans, plans, animals, or just flow in rivers!
Most – because radioactive atoms are not conserved. Some atoms have unstable nuclei and these can break down into smaller elements.
Potassium – 40 and Carbon – 14 are two examples, they break down into calcium and nitrogen which are each totally different atoms.
Another kind of nuclear reaction occurs in stars where smaller hydrogen atoms fuse to produce larger helium atoms. And in larger exploding stars many of the bigger atoms essential for life such as carbon and iron are formed by processes in which atoms are NOT conserved.

12. Recognize any of these? 104-Rutherfordium (Rd) 105-Dubnium (Db)
106-Seaborgium (Sg)
107-Bohroum (Bh)
108-Hassium (Hs)

13. HUGE MESS
Because so many people made these elements there were HUGE arguments about who would name them.
IUPAC (International Union of Pure and Applied Chemistry) eventually came up with the names in 1997.
There is as of this week debate over what to name elements the 4 newest elements.

14. Synthentic Elements
A synthetic element is an element that does not occur in nature.
are produced by converting a lighter element into a heavier one

15. Here’s How 1. Increase the number of protons
2. Get a nuclear reactor and a beta particle
3. Create nuclear explosions that produce a vast number of neutrons
4. Successive electron emissions produces a new element
all synthetic elements have a half-life in seconds
(Lawrencium-13.0 seconds)
Beta particles are high-energy, high-speed electrons emitted by certain types of radioactive nuclei such as potassium.

16. Different types of tables
Mendeleev was the first person to build the periodic table.
He was a card player and wrote all the properties of the elements on cards and organized them for years…
He left empty spaces where he predicted elements would fit once they were discovered

18. Triangular Table by Emil Zmaczynski

19. Spiral Table by Thoedor Benfey

20. Periodic Table By Discovery

21. Periodic Table Visually

22. Atomic Number
The Atomic number indicates the number of protons in the nucleus of an atom.
The biggest, and most obvious number on the table (and they go in order, 1, 2, 3, 4, …)

23. Periodic Table Facts:
As you go across the horizontal rows or PERIODS the atomic number increases by one
The vertical columns are called groups and are also known as FAMILIES
(each family has the same number of electrons in their outer shell)

24. Periodic Table Facts:
Groups or families

25. Metals Metals conduct electricity and heat.
They can be hammered into sheets or spread into wires
Physical Properties: Malleability, ductility
Shiny appearance
All are solids at room temperature except Mercury

26. Non-Metals
At room temperature, some are gases, some are solids and only one is a liquid.
Solid and Brittle
Do not conduct electricity, cannot be formed into wires

27. Metalloids
These are elements that lie in between the properties of metals and non-metals
Depending on what you are exposing the metalloids to, they will have properties of metals and non-metals at different times.

28. Where do you find them?

29. Where do you find them?

30. Families of the Periodic Table
You will be able to locate major families of the periodic table.

31. Alkali Metals Family Found in Group/Family 1
Li, Na, K, Rb, Cs, Fr
Soft, silvery, white metals
Very malleable
Good conductors of heat
REACT HIGHLY WITH WATER

32. Alkali Metals Family CANNOT BE FOUND IN NATURE IN A PURE STATE
Alkali Metals Video
Have one electron in their outer shell (group 1 = 1 electron)

33. Alkaline Earth Metals Family

34. Alkaline Earth Metals Family
Found in group 2
Silvery, white metals
Soft but not as soft as the Alkali metals
Not as reactive as Alkali Metals so can be found in nature in a pure state.
Has 2 electrons in the outer shell (group 2 = 2 electrons)

35. Alkaline Earth Metals Family
Alkali and Alkaline Earth metals burn very bright colors.
Potassium (K)
Barium (Ba)
Sodium (Na)
Calcium (Ca)
Magnesium (Mg)

36. The Noble Gases

37. The Noble Gases INCLUDE: He, Ne, Ar, Kr, Xe, Rn Un-reactive
All are Gases
Odorless, tasteless and colorless
Outer Shell is full of electrons
Noble Gases and Balloons

38. Halogens

39. Halogens INCLUDE: F, Cl, Br, I, At Gas, Liquids and Solids
Extremely corrosive and harmful
Poisonous
Naturally found in the form of compounds because they react with almost every other element
Compounds formed are useful (salt, toothpaste)
Have 7 unpaired electrons in the outer shell
physical properties of Halogens

40. Transition Metals
There are 38 elements in groups 3-12 called the Transition Metals
3 elements that are important in this group are nickel, cobalt and iron
These are the ONLY elements known to produce a magnetic field