Periodic Table
Foldable
Dilley HS
Chemistry
Shutter fold piece
• Should have 4 sections labeled on
the outside: Electronegativity,
Atomic Radius, Ionization
Energy, and Cations vs
Anions
• The following slides include exactly
what to write under each flap.
Electronegativity
• Electronegativity is an elements attraction
for electrons…higher #=higher
electronegativity
• EN increases up and to the right across
the periodic table.
• FLUORINE is the MOST EN element
• Noble gases have no EN value.
Atomic Radius
• Atomic radius is generally how large a
neutral atom is.
• AR increases down and to the left across
the PT.
• FRANCIUM has the largest atomic radius
of any neutral element.
Ionization Energy (IE)
• IE is the energy required to remove an
electron from an atom.
• IE increases as you move up and right
across the periodic table.
• Noble gases have the highest IE because
they do not like to lose ANY electrons.
Cations vs. Anions
• CATIONS—positive
ions that result from a
LOSS of electrons.
• CATIONS are smaller
than their neutral
atoms.
• EX: Ca+2 the +2
shows that Ca has
LOST two electrons.
• ANIONS—negative
ions that result from a
GAIN of electrons.
• ANIONS are larger
than their neutral
atoms.
• EX: N-3 the -3 shows
that N has GAINED
three electrons
Tri - fold piece
(Pink)
• Should have 3 sections labeled on
the outside: Metals, Metalloids,
and Nonmetals
• The following slides include exactly
what to write under each flap.
Metals, Metalloids, & Non-Metals
(pink tri-fold)
• Metals
– Most of the periodic table is made up of
metals (entire LEFT of stair step line)
– Good conductors of heat & electricity
– Malleable & ductile
– Form alloys when mixed together (metallic
bonding)
– All form POSITIVE ions due to a loss of
electrons.
Metals, Metalloids, & Non-Metals
• Metalloids
– Can have characteristics of both metals and
non-metals
– Includes B, Si, Ge, As, Sb, and Te
– Includes part of groups 13-16
– Appear on the stair step line on the PT
Metals, Metalloids, & Non-Metals
• Non-Metals
– Solids are brittle
– Non-metals include elements in all three states of
matter—solid, liquid, gas
– Includes elements from part of groups 14-16 and all
of 17 & 18
– Properties of each group become more metallic as
you move down the group in groups 14-17
– Groups 15-17 form NEGATIVE ions because they
gain electrons.
Periodic table Overlay
• On the outside of the flaps, you will be
labeling the groups
• Under the flaps, you will be writing down
the info about the group (if needed you
may extend into the unfolded area of your
overlay)
• The following slides have the info for you
to write (don’t write what’s in {} b/c that’s
just to help you label them  )
Periodic Table
• Alkali Metals {group 1, lst flap on the left}
– Most reactive group of metals
– Form +1 ions because of S1 valence
– Belong to the s-block
• Alkaline Earth Metals {group 2-2nd flap}
– Reactive group of metals
– Form a +2 ion because of s2 valence
– Belong to the s-block
Periodic Table
• Transition Metals {big flap- grps 3-12}
– Heaviest metals
– Belong to the d-orbital (5 orbitals; 10 eacross)
– Most can have multiple charges (all +)
– Tend to be lustrous (shiny), good conductors
of heat & electricity, malleable, & ductile
– All metals LOSE e- to form cations—(+)
ions—to become stable.
Periodic Table
• Boron Family {grp 13}
– Form a +3 ion
– Have s2p1 for 3 valence electrons
• Carbon Family {grp 14}
– Can form a +4 or -4 ion
– Have s2p2 for 4 valence electrons
• Nitrogen Family {grp15}
– Tend to form a -3 ion
– Have s2p3 for 5 valence electrons
Periodic Table
• Oxygen Family {grp16}
– Tend to form -2 ions
– Have a s2p4 for 6 valence electrons
• Halogens {grp 17}
– Always form -1 ions
– Have a s2p5 for 7 valence electrons
• Noble Gases {grp 18}
– Do not form ions…charge is 0
– Have a s2p6 for 8 valence electrons (except
He which just has a s2 configuration)
Periodic Table
• Inner Transition Metals
– Highly reactive metals
– Many are radioactive
– Belong to the f-block (7 orbitals; 14 e- across)
– {Ms. Clark forgot to have you make this
strip…sorry. You may create a flap that
covers the Actinide and Lanthanide series.
You’ll have to glue it directly onto your
Periodic table Then label the outside inner
transition metals and write info underneath. I’ll
leave my example for you}
On your white Periodic Table
• s, p, d, f
– Color the blocks accordingly using color
pencils…use notes pg after “5” to help you
label (don’t forget to make a key)
• On the BACK of the PT
– Mendeleev first ordered the periodic table
according to increasing atomic mass
– Moseley then ordered the modern PT
according to increasing atomic NUMBER
– The PT is mostly metals (all to the left of the
stair step line)
On the Yellow Sheet
• Label the parts of the element symbol
• Complete the electron configuration for Si
using your books.
• Draw in the bohr model for Si (remember
1st orbital has 2 electrons, 2nd orbital has 8
electrons, and 3rd will have the remaining)
• Fill in the info below the model