1. Atomic Structure and the Periodic Table
Students can describe the parts of an atom
Students can read the element information on the periodic table
Students can describe the reactivity of alkali metals
Students can describe how various types of bonding in different categories of materials effects their behavior

2. Atoms
smallest particle of an element that has the properties of the element
made of 3 basic subatomic particles
there are now many more subatomic particles – theoretical physics

3. nucleus small, dense center of atom
contains almost all the mass of the atom
contains protons and neutrons

4. Atomic Mass Unit (amu)
metric unit to measure the mass of VERY small objects (particles)
a unit to measure the mass of atoms
Just like we have light years for measuring very large distances

5. in shells around nucleus
Subatomic Particles
Name
Protons (p or +)
Neutrons (n)
Electrons (e-)
Charge +1
No charge -1
Location
in nucleus
in shells around nucleus
Mass
≈ 1 amu
≈ 2000 x smaller
“Job”
Determines
identity of
element
Supplies proper
mass to hold
nucleus together
bonding/
how it reacts
Number

6. Subatomic Particles Number Atomic # Atomic mass – atomic # =
Name
Protons (p or +)
Neutrons (n)
Electrons (e-)
Charge +1
No charge -1
Location
in nucleus
in shells around nucleus
Mass
≈ 1 amu
≈ 2000 x smaller
“Job”
Determines identity of element
Supplies proper mass to hold nucleus together
Determines bonding/ how it reacts
Number
Atomic #
Atomic mass – atomic # =
# of neutrons
Same as # of protons

7. # of protons atomic number whole number on periodic table
number of protons in an atom of an element
does NOT vary in an element – the same in all atoms of an element
Use the flexcam and a copy of the periodic tables they have in their notebooks to show them the location of the atomic number and atomic mass.
Try several examples.

8. # of electrons atoms are neutral (+) = (-)
# of protons = # of electrons
p = e-
Do several examples.

9. atomic mass (weight)
decimal number on the periodic table – it is for all the atoms of the element
number of protons plus the number of neutrons – it’s an average on the table
weighted average of all the isotopes of that element
the mass of one atom is a whole number
use the average weight of students analogy (all girls = 100 lbs, all boys = 200 lbs. – same # of girls and boys – more girls than boys)

10. Isotopes
iso = same
atoms of the same element with different numbers of neutrons
have different atomic masses but the same atomic number
some are stable, some are radioactive (carbon-12 and carbon-14)

12. # of neutrons atomic mass n + p - atomic # - p # of neutrons n
Work some sample problems on how to determine the # of protons, electrons, and neutrons in an atom of an element. Let the students choose the elements.

13. Free Write
What do you know about:
atoms
the periodic table

14. Introduction to the Periodic Table
Atomic Number ● Symbol ● Atomic Weight
Element ● Compound ● Mixture

15. I made the PERIODIC TABLE !
I am Dmitri Mendeleev!
I made the PERIODIC TABLE !

16. What is the PERIODIC TABLE?
Shows all known elements in the universe.
Organizes the elements by chemical properties.

17. Periodic Table rows How is the periodic table arranged?
arranged by increasing atomic number
rows
called periods
tells number of electron shells
number them down the left side of the periodic table – 1 through 7
discuss the history of the periodic table briefly.
Use the overhead to show them how to mark/label the rows.

18. Periodic Table columns called families or groups
elements in same column have similar chemical properties
same number of valence electrons

19.
Periodic table lesson plans

20. How do you read the PERIODIC TABLE?

21. What is the ATOMIC NUMBER?
The number of protons found in the nucleus of an atom Or
The number of electrons surrounding the nucleus of an atom.

22. What is the SYMBOL?
An abbreviation of the element name.

23. What is the ATOMIC WEIGHT?
The number of protons and neutrons in the nucleus of an atom.

24. How do I find the number of protons, electrons, and neutrons in an element using the periodic table?
# of PROTONS = ATOMIC NUMBER
# of ELECTRONS = ATOMIC NUMBER
# of NEUTRONS = ATOMIC _ ATOMIC
WEIGHT NUMBER

25. Now you are almost as smart as I am!
But not as handsome!
Man, I look GOOD!

26. Elements, Compounds, and Mixtures

27. What is an ELEMENT? A substance composed of a single kind of atom.
Cannot be broken down into another substance by chemical or physical means.

28. What is a COMPOUND?
A substance in which two or more different elements are CHEMICALLY bonded together.

29. What is a MIXTURE?
Two or more substances that are mixed together but are NOT chemically bonded.

30. Element, Compound or Mixture?

31. Element, Compound or Mixture?

32. Element, Compound or Mixture?

33. Element, Compound or Mixture?

34. Element, Compound or Mixture?

35. Element, Compound or Mixture?

36. You are still not as handsome as the great Mendeleev!
I am working this beard!
Man, I look GOOD!

37. Periodic Table valence electrons electrons in outermost shell
involved in bonding
number the columns on your periodic table with the correct number of valence electrons
Use the overhead to show them how to mark/label the columns.

39. Stability stable number of electrons = 8 in the outermost shell
8 valence e-
octet rule
exception – 1st shell is stable with 2 e-

40. Metals 1 to 3 valence electrons givers of electrons lose electrons
make (+) ions
left side of periodic table

41. Nonmetals 5 to 8 valence electrons takers of electrons gain electrons
make (-) ions
right side of periodic table

42. Ion atom with a charge atom has gained or lost electrons
gained e- = (-) charge
lost e- = (+) charge
(+) ion = cation
(-) ion = anion

43. Column 1 alkali metals want to give away one electron
most reactive metals

44. Column 7 halogens want one more electron most reactive nonmetals
can take an electron from almost anyone

45. Column 8
Noble gases
very stable
don’t want to form compounds or bonds

47. Bonding
atoms achieve a stable number of electrons (ionic and covalent)
involves valence (outer) electrons
make compounds and/or solids
fill out types of bonding chart using overhead
show overhead of metallic bonding
draw examples of ionic bonding – use skeletal models - MgO, NaCl, CaCl2, K2S
draw examples of covalent bonding – use skeletal models – CO2, H2O, O2

49. Metallic Bonding
All pure metals have metallic bonding and therefore exist as metallic structures.  Metallic bonding consists of a regular arrangement of positive ion cores of the metals surrounded by a mobile delocalized sea of electrons.

51. Metallic Bonding Each atom donates its valence electrons to the whole
Atom therefore becomes a cation (here called an ion core)
Donated electrons form an electron cloud surrounding all the ion cores
Electron cloud binds all the ion cores together by coulombic forces

52. Metallic Bonding Valence electrons are delocalized:
Shared by all atoms in the material
Electrons are free to drift throughout the material
Provides unique properties only found in metals
shiny metallic luster
good electrical and thermal conductivity
many others ...

53. Metallic Bonds: Mellow dogs with plenty of bones to go around
These bonds are best imagined as a room full of puppies who have plenty of bones to go around and are not possessive of any one particular bone.  This allows the electrons to move through the substance with little restriction.  The model is often described as the "kernels of atoms in a sea of electrons."

54. Ionic Bonding (ceramics and polymers)

55. Ionic Bonds: One big greedy thief dog!
Ionic bonding can be best imagined as one big greedy
dog stealing the other dog's bone.  If the bone
represents the electron that is up for grabs, then when
the big dog gains an electron he becomes negatively
charged and the little dog who lost the electron
becomes positively charged.  The two ions (that's where
the name ionic comes from) are attracted very strongly
to each other as a result of the opposite charges.

57. Sodium lets Chlorine use its valance electron

58. Covalent Bonding (Ceramics)

59. Covalent Bonds: Dogs of equal strength.
Covalent bonds can be thought of as two or more dogs
with equal attraction to the bones.  Since the dogs
(atoms) are identical, then the dogs share the pairs of
available bones evenly.  Since one dog does not have
more of the bone than the other dog, the charge is
evenly distributed among both dogs.  The molecule is not
"polar" meaning one side does not have more charge than
the other.

60. Polar Covalent Bonds: Unevenly matched but willing to share.
These bonds can be thought of as two or more dogs that
have different desire for bones.  The bigger dog has
more strength to possess a larger portion of the
bones.  Sharing still takes place but is an uneven
sharing.  In the case of the atoms, the electrons spend
more time on the end of the molecule near the atom
with the greater electronegativity (desire for the
electron) making it seem more negative and the other
end of the molecule seem more positive.

63. http://www. matsceng. ohio-state

65. Covalent Network Solid
only covalent bonds
extremely large molecules or networks
usually have at least one element from carbon family
very strong and hard
very high melt T°
some glass and ceramics, diamond
polymers are usually not because they make linear chains instead of networks

66. intermolecular forces high melt temps, nonconductors as solids,
Type of bonding
metallic
ionic
covalent
intermolecular forces
Type of elements used
Between metals
Metals and nonmetals
Between nonmetals
Between molecules
Givers &/or takers of electrons
Between givers
Between givers and takers
Between takers
Description
Valence e- roam freely between many atoms (delocalized). Sea of e- surrounding (+) kernels.
Transfer e-
Makes (+) and
(-) ions that are attracted to each other.
Share e-
Forms discrete molecules.
Hold covalently bonded molecules together as a solid.
Type of material formed
Solid metallic elements and alloys
Ceramics and glass
Polymers and some ceramics/glasses
Helps form solid polymers
Strength of bond
Relatively strong
Very strong
Weak
Properties
Produced
Good conductors, workable, corrode easily, generally high melt temps but variable
Brittle,
high melt temps, nonconductors as solids,
don’t corrode
Insulators,
Help determine a lot of properties of covalent compounds (polymers). Soft and plastic

67.
Read the 4 slides and take the quiz at the end
Patterns in the periodic table
Ionic bonding Electron numbers ions and aions
Covalent bonding
Structure of the atom