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. Subatomic Particles Name Protons (p or +) Neutrons (n) Electrons (e-)
Charge
Location
Mass
“Job”
Number

4. Subatomic Particles Charge +1 No charge -1 Protons (p or +)
Name
Protons (p or +)
Neutrons (n)
Electrons (e-)
Charge +1
No charge -1
Location
Mass
“Job”
Number

5. Subatomic Particles Location in nucleus in shells around nucleus
Name
Protons (p or +)
Neutrons (n)
Electrons (e-)
Charge +1
No charge -1
Location
in nucleus
in shells
around nucleus
Mass
“Job”
Number

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

7. 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
≈ 2000x smaller
“Job”
Number

8. 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

9. 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

10. 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

11. # 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.

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

13. 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)

14. 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)

16. # 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.

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

18. 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.

19.
Periodic table lesson plans

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

21. 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.

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

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

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

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

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

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

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

30. Alkali metals on the show brainiac

32. 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

34. intermolecular forces
Type of bonding
metallic
ionic
covalent
intermolecular forces
Type of elements used
Givers &/or takers of electrons
Description
Type of material formed
Strength of bond
Properties
Produced

35. intermolecular forces
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
Description
Type of material formed
Strength of bond
Properties
Produced

36. intermolecular forces Between givers and takers
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
Type of material formed
Strength of bond
Properties
Produced

37. (-) ions that are attracted to each other. Share e-
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
Strength of bond
Properties
Produced

38. Type of material formed Solid metallic elements and alloys
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
Properties
Produced

39. intermolecular forces
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

40. 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

41. 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.

43. 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

44. 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 ...

45. 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."

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

47. low to moderate; ductile, malleable soft and plastic
Ionic
Covalent
Metallic
Intermolecular
Bond strength
strong
very strong
moderate and variable
weak
Hardness
moderate to high
very hard, brittle
low to moderate; ductile, malleable
soft and plastic
Electrical conductivity
conducts by ion transport only when dissociated
insulator in solid and liquid
good conductors; by electron transport
insulators in solid and liquid states
Melting point
low
generally high
Solubility
soluble in polar solvents
very low solubilities
insoluble
soluble in organic solvents
Examples
most minerals
diamond, oxygen, organic molecules
Cu, Ag, Au, other metals
ice, organic solids (crystals)

48. Ionic Bonding (ceramics and polymers)

49. 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.

51. Sodium lets Chlorine use its valance electron

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

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

54. Covalent Bonding (Ceramics)

55. 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.

56. 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.

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

62. 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

63.
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