1. Periodic Table
Trends

2. Mendeleev Period Group Family Alkali metals Earth metals
OUTCOME QUESTION(S):
S1-2-06
How is the Periodic Table organized for the elements and what trends exist?
Vocabulary & Concepts 
Mendeleev Period Group
Family Alkali metals Earth metals
Transition Metals Chalcogens Halogens
Noble gases

3. Elemental symbols originated from a Greek or Latin root word
Modern Symbols
Alchemist Symbols
Dalton Symbols
Antimony Sb
Arsenic As
Bismuth Bi
Carbon C
Copper Cu
Gold Au
Iron Fe
Lead Pb
Mercury Hg
Silver Ag
Sulpher S
Tin Sn
Zinc Zn

4. Russian scientist and professor
Mendeleev (1870)
Russian scientist and professor
Arranged the 63 elements by atomic mass
Noticed a repetition of properties (periodicity)
Called the pattern of properties “Periodic Law”
Mendeleev (correctly) predicted the mass of elements yet to be discovered and left spaces open for them

5. Repetition of properties (periodicity) became more clear
Moseley (1913)
Experiments showed proton number was a better method to organize the elements.
Repetition of properties (periodicity) became more clear
Modern Periodic Law:
“The properties of elements are a periodic function of increasing atomic number”
We know now that most element properties are due to the number of valence electrons

6. Non-metals
M e t a l s
An updated Periodic Table containing ALL 118 elements – separated into metal and non-metal atoms make up EVERYTHING in the Universe.

7. Element with properties opposite to those of metals (brittle, dull…)
Rows of the periodic table are called periods.
Elements in periods do not have similar properties
Left to right
Elements change from metals to non-metals
Non-metal
Element with properties opposite to those of metals (brittle, dull…)
periods

8. Family names and locations need to be memorized
Columns of the periodic table are called groups.
Elements in groups have similar properties
A family is a group with a specific name:
Family names and locations need to be memorized
GROUP
Alkali metals
Alkaline Earth metals
Chalogens
Halogens
Inert (noble) gases

11. (make coloured compounds, speed up chemical reactions…)
Transition Metals: groups 3 – 12
unique properties different from group 1 and 2 metals
(make coloured compounds, speed up chemical reactions…)

14. Can you connect these two ideas together to explain reactivity?

15. Simplest atomic structure - only 1 e- and 1 p+
Hydrogen*
Group 1
Non-metal gas
1 valence electron
Simplest atomic structure - only 1 e- and 1 p+
Highly chemically reactive
The placement of hydrogen is only because of its structure - 1 proton… Sometimes a table will have it raised above the Alkali Metals to avoid confusion

16. The Octet Rule of Chemical Reactions
Atoms with a FULL outer orbit are very stable
Chemical reactions happen when atoms work together to try to get a full valence orbit
Atoms will acquire a full outer shell in 3 ways:
Give away extra electron(s) to another atom
Take extra electron(s) from another atom
Share an e- with another atom
We’ll skip this one until next year

17. Increasing Reactivity
The LESS electrons needed, the GREATER the chemical reactivity of the element
Increasing Reactivity
A Chemical Reaction
Movement of electrons between combining atoms that results in the formation of a NEW substance.

18. How many valence electrons does the element have?
Does it make sense to lose or gain electrons in a reaction?
What trends (“periodicity”) have you found?

19. CAN YOU ANSWER THESE QUESTIONS? S1-2-06
How is the Periodic Table organized for the elements and what trends exist?
Vocabulary & Concepts 
Mendeleev Period Group
Family Alkali metals Earth metals
Transition Metals Chalcogens Halogens
Noble gases