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) 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 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 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

Periodic Table Transition Metals {big flap- grps 3-12} Heaviest metals Belong to the d-orbital (5 orbitals; 10 e- across) 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} Carbon Family {grp 14} 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} Halogens {grp 17} 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