1. Atoms and the Periodic Table of Elements
February 2016

2. Atoms Nucleus Center of the Atom Protons and Neutrons Found Here
Contains Almost ALL of the Atom’s Mass
Electron Cloud
Area Around the Nucleus where the Electrons are Found

3. Blurry Area Containing
Atoms…Continued
Electron Cloud
Blurry Area Containing
Electrons
Nucleus
Protons + Neutrons

4. Atoms…Relative Size One dust particle has millions of atoms
100 million million billion hydrogen atoms are in a regular size balloon
Twenty thousand billion billion atoms are in a nickel
Imagine 1 grain of rice is one electron. 2,000 grains of rice represent a proton.
Imagine that an electron is as big as a grain of sand. Then the nucleus of an atom would be as big as a marble. The electron cloud would have a radius of 25 meters!
If we could magnify the simplest hydrogen atom to the size of the earth, then the nucleus (a proton) would only be about the size of a basketball. It would be at the very center of the earth and that lonely electron would be found somewhere out in earth's atmosphere. All of the space in between the electron and the basketball-size nucleus is empty!

5. Atoms…Relative Size…Continued

6. Subatomic Particles Proton Positive “1” Charge Mass of “1”
Found in Nucleus
Determines the ELEMENT (3P = Li; 30P = Zn)
Neutron
Neutral or Zero Charge
Electron
Negative “1” Charge
Very Little “0” Mass
Found in Electron Cloud Surrounding Nucleus

7. Subatomic Particles…Continued

8. Atom Variations BrainPOP - IONS Isotopes
Atoms of the SAME ELEMENT with a Different (+ or -) number of NEUTRONS
ONLY the Atomic Mass changes
Read and Written as “Carbon-14” or “Uranium-236”
Ions
An Atom or Molecule that has a Different Number of Electrons than Protons
Adding Electrons Creates a NEGATIVE ion
Subtracting Electrons Creates a POSITIVE ion
BrainPOP - IONS

10. The Periodic Table INB page 126 - 127
Method of organization
Dmitri Mendeleev
1869
Predicted the properties of elements and predicted the discovery of other elements based on the trends in the table.
Based on atomic mass.
Moseley discovered that a more appropriate basis was atomic number.
Periodic Law—When elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic pattern.

11. The Periodic Table Periodic
Occurring or Recurring at Regular Intervals
Columns are called “Groups”
Rows are called “Periods”
Elements are Arranged in Many Ways on the Periodic Table
Similar Properties
Reactivity
Atomic Size
Density
Etc…

12. Trends
Size of Atoms
Decreases from LEFT to RIGHT and Increases from TOP to BOTTOM
Largest: Cesium
Smallest: Helium

13. Trends…continued Density Increases from TOP to BOTTOM
Increases from the OUTSIDE INWARD
Hydrogen: g/cm3
Osmium: g/cm3
Melting and Boiling Points decrease as you move down a group and increase as you move left to right across a period.

14. On Your Periodic Table, Add:
Alkali
Metals
Noble
Gases
Oxygen
Group
Carbon
Group
Alkaline
Earth
Metals
Halogens
Boron
Group
Nitrogen
Group 1 18 1 2
Transition
Metals 13 14 15 16 17 2 3 4 5 6 7 8 9 3 10 11 12 4 5 6 7

15. Metals & Nonmetals Nonmetals (right of zig-zag line) No luster
Metals (left of zig-zag line)
Luster/shine
Good conductors of heat and electricity.
Malleable (hammered or rolled into sheets)
Ductile (stretched or drawn into wires)
All are solids except for Mercury
Nonmetals (right of zig-zag line)
No luster
Poor conductors
Not malleable or ductile
Many are gases; Bromine is a liquid; some are solids

16. Metalloids Metalloids ( 7 Eelements ALONG zig-zag line)
Called semi-metals
Have properties of BOTH metals and nonmetals
Example – Silicon
Shiny
Brittle
Poor electrical conductor
Example – Boron
Acts as a metal when reacting with Fluorine
Acts as a nonmetal when reacting with Sodium

17. Element “Boxes” Atomic Number Determines Element = Protons = Electrons
Atomic Symbol
1 or 2 Letters
1st is Capitalized
2nd is NOT
Atomic or Element
Name
Atomic Mass
= Protons + Neutrons

18. Atomic Math! 99 # Protons = _____ (Same as Atomic Number)
# Electrons = _____ (Same as Atomic Number)
# Neutrons = _____ (Rounded Atomic Mass MINUS Atomic Number) 99
153 41
# Protons = ____
# Electrons = _____
# Neutrons = _____ 41 52

19. Group 1: Alkali Metals K 1 Valence Electron
Never found in elemental form in nature
Very Reactive
Stored under oil
Silver in Color
Soft
Form “Salts” with Halogens K

20. Group 2: Alkaline Earth Metals
2 Valence Electrons
Moderately Reactive
Silver in Color
Soft Mg

21. Groups 3-12: Transition Metals
All “useful” metals
Random properties and electron configurations

22. Group 13: Boron Group
3 Valence Electrons Ga

23. Group 14: Carbon Group
4 Valence Electrons C

24. Group 15: Nitrogen Group 5 Valence Electrons Moderately Reactive
Some VERY TOXIC (P, As, Sb) P

25. Group 16: Oxygen Group
6 Valence Electrons
Moderately Reactive Te

26. Group 17: Halogens 7 Valence Electrons Very Reactive
All form Acids with Hydrogen
Forms “salts” with Alkali Metals At

27. Group 18: Noble Gases 8 Valence Electrons (*2 for Helium)
Full Valence Shells
Non Reactive (Inert) Kr

28. Periodic Table “QUIZ” Foldable
Group / Family Name
# Valence Electrons (except groups 3-12)
Lewis Dot Structure – (Choose an Element in Each Group – Do NOT Do a Lewis Dot Diagram for Groups !)
Facts
Group 1: 3 Facts
Group 2: 2 Facts
Groups 3-12: 1 Fact
Group 15: 1 Fact
Group 16: 1 Fact
Group 17: 2 Facts
Group 18: 2 Facts