1. Chemistry 1 Chapter 6 Notes
The Periodic Table & Periodic Law
Chemistry 1 Chapter 6 Notes
Last Updated January 13, 2019

2. Priority Standards

3. Big Idea
The periodic table organizes all known elements and provides useful information for making predictions in chemistry.
Core Concepts
In the periodic table, elements are arranged in order of increasing number of protons.
Vertical groups in the periodic table have similar physical and chemical properties due to the same outer electron configurations (valence electrons).
By understanding valence electrons, the periodic table can be used to predict chemical bonding.

4. Michigan HSCE Priority Standards
C4.9A Identify elements with similar chemical and physical properties using the periodic table.
C4.9b Identify metals, non-metals, and metalloids using the periodic table.
C4.9c Predict general trends in atomic radius, first ionization energy, and electronegativity of the elements using the Periodic table.
C4.10c Calculate the average atomic mass of an element given the percent abundance and mass of the individual isotopes.
C4.10d Predict which isotope will have the greatest abundance given the possible isotopes for an element and the average atomic mass in the periodic table.
C5.5A Predict if the bonding between two atoms of different elements will be primarily ionic or covalent.
C5.5B Predict the formula for binary compounds of main group elements.
C5.5c Draw Lewis structures for simple compounds.

5. Antoine Lavoisier Late 1790s French Scientists
Compiled a list of elements
Only 23 elements known at the time

6. John Newlands 1864 English Chemist
Proposed an organization scheme for the elements based on increasing atomic mass noting that properties repeated every eighth element.
Idea did not work for all elements

7. Meyer and Mendeleev Meyer-German Chemist Mendeleev-Russian Chemist
Mendeleev published his organization scheme first and is therefore given more credit.

8. Mendeleev Continued
Mendeleev arranged elements according to increasing atomic masses but into columns with similar properties
Was able to predict the properties of yet undiscovered elements

9. Not entirely accurate as new elements were discovered and atomic masses of known elements were more accurately determined.

10. Henry Mosley 1913 English Chemist
Arranged elements according to increasing atomic number
Resulted in clear Periodic Patterns

11. Periodic Law
The periodic repetition of chemical and physical properties of the elements when they are arranged by increasing atomic number

12. Review/Discuss Groups – Columns Periods – Rows Main Block Elements
1-18 Current Numbering system for groups
Number has changed over time and will be discussed
Periods – Rows
Main Block Elements
(Groups 1A-8A or 1-2,13-18)
Transition Elements
(Groups 1B-8B or 3-12)

13. Know the location Metals Non-metals Metalloids Transition
Inner Transition
Alkali-metals
Alkaline Earth Metals
Halogens
Noble Gases

15. Classification of the elements
Valence e- and the Periodic Table
See Figure 6-9 page 160

16. Blocks s p d f
Know the location of each block

17. Periodic Trends Atomic Radius  in picometers (1 x 10-12 meters)
Generally Decreases from left to right and increases as you move down the periodic table

19. Ion Charged Particle due to loss gain or sharing of electrons
Loss of electrons = smaller radius
Gain of electrons = larger radius
Compare Trends from Fig 6-11 pg 163 to Fig 6-14 pg. 166
Lost e- are generally valence e-

20. Ions Continued Across Periods moving left to right
+ ions decrease in size
Ions decrease in size
Down Groups Both + and – ions increase radii

21. Ionization Energy- Energy required to remove an e- from a gaseous atom
First ionization energy = 1 e- to remove
Ionization Energy can be thought of as how strongly an atom’s nucleus holds on to its valence e-

22. Atoms with large ionization energy are less likely to form + ions
Low ionization energy indicates an atom loses e- easily likely to form + ions

24. Octet Rule- atoms tend to lose, gain or share e- in order to acquire a full set of eight valence e-
Electronegativity- ability of an atom to attract e- to itself in a chemical bond
Units are arbitrary and are called Paulings, for Linus Pauling

25. Electronegativity decrease as you move down a group and increases as you move left to right
Lowest electronegative = lower left
Highest electronegative = upper right