1. Reactivity: Atomic size Return Test Agenda:
Homework:
Agenda:
Objective: To understand the physical and chemical properties of atoms based on their position on the Periodic Table
Warm-up: Properties of Groups
Trends in properties
How do we use the Periodic Table to predict properties of elements?
Reactivity:
Atomic size
Ionization Energy
Electronegativity
Return Test
Next Unit is forming bonds and compounds based on reactivity

2. Warm-up: Properties of Groups
Alkali Metals, Halogens, Noble Gases
Which group is the least reactive?
In Group 1, which elements are most reactive? Why?
In Group 17, which elements are most reactive? Why?
Which Group contains all gases?
Which group always forms ionic compounds?
What other properties change in a Group when going down the PT?

3. Predicting how easily an element reacts
What characteristics of an element impact how easily it reacts with other elements to form a chemical compound?
The electron arrangement of each atom determines its chemical behavior (how it reacts and bonds).
Forming ions based on number of valence electrons
Atomic size
Ionization energy
Electronegativity

4. Atoms lose, gain or share valence electrons
in order to be stable like the Noble Gases.
Metals will: Non-metals will:

5. Forming Compounds
Ions come together to form a ______________ ______________ .
Many formula units are held together to make an _______ compound.

6. Focus on Reactivity Atomic size Ionization Energy Electronegativity
Periodic Trends Using the Periodic Table to predict Properties of Elements and Groups
Focus on Reactivity
Atomic size
Ionization Energy
Electronegativity

7. Atomic Radii
Atomic Radius – measurement of the size (volume) of the atom
Defined by the edge of its orbital but since the edges are fuzzy, difficult to determine
Atomic Radii – half the distance between the nuclei of identical atoms that are bonded together

8. Ionization Energy
Ionization energy – the energy required to remove one electron
X + energy  X+ + e-
An electron can be removed from an atom if enough energy is absorbed (+) by the atom
Note: measurements of this are made on individual atoms in gas phase to avoid interactions with nearby atoms
Adding energy = Endothermic

9. How do metal atoms lose electrons? Ionization energy
Ground State, Excited State, Ionization energy
Lithium 9

10. Electronegativty
Electonegativity: An atoms’ ability to attract electrons from another atom
Electron Affinity: The energy released when an electron is added to an atom
X + e-  X- + energy
Releasing energy =
Exothermic

11. How do non-metal atoms gain electrons? Electronegativity
Large non-metal Small non-metal atom atom 11

12. Examining properties & trends
Use Interactive Periodic Table –
Click on Properties
Work in pairs
Each person completes the table
When completed, investigate the properties of the transition metals
Homework: Summary on a separate paper
Define the property
Summarize its trends: across periods and down groups
Summarize the characteristics of the property in each of the 3 groups studies

13. Linking Electron Arrangement to the PT
Use Interactive Periodic Table –
Click on Orbitals
S P D F blocks
Which are being filled?

14. Noble Gas Notation – using the PT

15. Periods ?
Rules for Group 1 & Group 2

16. Periods?
Rules for Groups

17. Rules for Transition Metals
Period ?

18. 7. Reactivity
Group 18 (called the _______________) are ____________ (also called ________ or _____________), because:
Group 1 (called ____________) are the most reactive metals because:
Group 17 (called ___________) are the
most reactive nonmetals because: 18

19. Trends for Ionization Energy & Electronegativity Arrows to show trends for metals & non-metals
Reactivity: trends for metals and non-metals

20. Ca vs. Br C vs. Sn F vs. I Si vs. Cl Na vs. P Li vs. K
Predicting Properties of Elements
- based on the position on the Periodic Table : Size; IE; EN
Property: which element has the largest value?
Ca vs. Br C vs. Sn F vs. I Si vs. Cl
Na vs. P Li vs. K
Be vs. O S vs. Ar
Al vs. S Ne vs. Kr
B vs. Al B vs. Ne

21. Periodic Trend Animation
Atomic size
Ionic size Interactive animations
Ionization
Electronegativity
For later used: bond formation

22. Periodic Table
Objective: To understand the physical and chemical properties of atoms based on their position on the Periodic Table
NC Essential Standards 1.3
Physical properties:
Chemical properties:

23. Periodic Tables Groups
Interactive Periodic Table – useful for trends of properties

24. Periodic Trends Using the Periodic Table to predict Properties of Elements and Groups
Focus on Reactivity
Atomic size
Ionization Energy
Electronegativity
Electron Affinity

25. Atomic Radii
Atomic Radius – measurement of the size (volume) of the atom
Defined by the edge of its orbital but since the edges are fuzzy, difficult to determine
Atomic Radii – half the distance between the nuclei of identical atoms that are bonded together

26. Atomic Radii atoms get smaller
Across Period:
atoms get smaller
because of the increased number of protons attracting the electrons
the electrons added in the same energy level do not shield electrons from nuclear charge
Down Group:
atoms get larger
increases
because the energy levels being added to the atom

29. Atomic/Ionic Radii

30. Ionization Energy
Ionization energy – the energy required to remove one electron
X + energy  X+ + e-
An electron can be removed from an atom if enough energy is absorbed (+) by the atom
Note: measurements of this are made on individual atoms in gas phase to avoid interactions with nearby atoms

31. Ionization Energy

32. Ionization Energy
Across Period:
requires more energy to remove an electron so increases
because electrons added in the same energy level do not shield electrons from nuclear charge
Down Group:
requires less energy to remove electron so decreases
because the valence electrons are farther away from protons attracting them

33. Ionization Energy

34. Ionization Energy

35. Electronegativty Ability to attract electrons
Non-metals (excluding Noble Gases)
High electronegativity

36. Electronegativity Increases Non-metals attract electrons Smaller atoms
Across Period:
Increases
Non-metals attract electrons
Smaller atoms
Down Group:
Decreases
Protons in the nucleus are shielded by inner energy levels
Harder to attract electrons

37. Electronegativity

38. Periodic Trend Animation
Atomic size
Ionic size Interactive animations
Ionization
Electronegativity
For later used: bond formation

39. Trends for Ionization Energy & Electronegativity Arrows to show trends for metals & non-metals
Reactivity: trends for metals and non-metals

40. 6. Octet Rule Atoms tend to ______, ______, or _______
electrons in order to have _____ valence electrons.
_______ valence electrons gives stability.
Exception:
Duet rule: Hydrogen 40

41. 7. Reactivity
Group 18 (called the _______________) are ____________ (also called ________ or _____________), because:
Group 1 (called ____________) are the most reactive metals because:
Group 17 (called ___________) are the
most reactive nonmetals because: 41

42. Trends for Ionization Energy & Electronegativity Arrows to show trends for metals & non-metals
Reactivity: trends for metals and non-metals

43. Ca vs. Br C vs. Sn F vs. I Si vs. Cl Na vs. P Li vs. K
Predicting Properties of Elements
- based on the position on the Periodic Table : Size; IE; EN
Property: which element has the largest value?
Ca vs. Br C vs. Sn F vs. I Si vs. Cl
Na vs. P Li vs. K
Be vs. O S vs. Ar
Al vs. S Ne vs. Kr
B vs. Al B vs. Ne

44. Periodic Table videos New Periodic Table Song
Prism website