PERIODIC TABLE OF ELEMENTS

You need:• Colored pencils

– Brown, blue, red, green, purple, pink, yellow, tan, orange

• Mechanical pencil• Eraser• Ruler

(Front; Top-Center) Title: • Periodic Table of Elements

• “Frame” hydrogen• (Maybe done on your table.) Use a ruler to add

squares for elements # 110 – 118• Add brackets & lines connecting

Ba to La; Ra to Ac

H

Add brackets & lines connecting Ba to La; Ra to Ac - Do not add color.

Front (Periods)• Number rows 1 through 7• Title “PERIODS” – on the left side

Front (Groups/Families)Number columns 1 through 18

– Left to right H to He

Label Roman numerals 1 – IA 7 – VIIB 15 – VA2 – IIA 8,9,10 – VIIIB 16 VIA3 – IIIB 11 – IB 17 VIIA4 - IVB 12 – IIB 18 - VIIIA5 – VB 13 – IIIA6 – VIB 14 – IVA

Back – divide page; draw lines in with a ruler.

Back – Notes - Upper left cornerDo not write in large letters or you won’t have enough space.

• Columns –

–Elements have similar but not identical properties.• Elements in a family have the same number of

valence e-

# 1 – 18 (Groups or Families)

Back – Notes - Upper left corner

• Rows – –Elements in a period are not alike in

properties.– The period reflects how many energy

levels are present for that row of elements. (Period 1 = 1 energy level)

–Pattern – (left to right)• 1st column (left) very reactive elements• Last column (right) always an unreactive

gas• Going left to right – elements become less

metallic.

# 1 – 7 (Periods)

Back – Notes - Upper left corner

• Valence pattern – 1, 2, 3, 4, 3, 2, 1, 0

–Valence number – the number of electrons available for bonding in the valence level.

Back – Notes - Upper left corner

• Family 1 has 1 valence electron (s) 2 – 12 1 – 2 valence e- s 13 3 14 4 15 5 16 6 17 7 18 8

Front - Metals/Nonmetals• Box in the Nonmetals• Use a ruler to draw a line to

delineate the metals. If the line is present, write in the title – Metals.

• Title both the Metals & Nonmetals

• Title the RARE EARTH ELEMENTS at the bottom of the table.

Back – (lower left box for notes)

• Metals – (95 of the 118 elements) left side of the table

– Properties: luster, ductility, malleability, good conductors of heat & electricity; corrode – react chemically• Valence of 1, 2, 3, 4 e- – tend to lose

electrons

(Notes – under “Metals”)• Nonmetals – (right side of the table)

–Properties: no luster – dull, do not conduct heat or electricity, brittle – break easily, not ductile or malleable.• Valence # of 5, 6, 7, or 8 - will

gain 3, 2, or 1 e-

Front - • Filling in the atomic squares:• The following slide shows where you

will be placing the information contained in the squares.

• We will be adding one component of the table at a time. Ex. All the atomic #’s.

• Please note the precautions before beginning.

Precautions: Consider everything that will be put into the square. Don’t write too large.

Element Name

Element Symbol

At. #

Atomic Mass

Remember:You will be putting color on the edge of the squares too. The star will only be put into squares when the element is radioactive.

Front - #104 - 118• Add names of elements 104 – 118 to

the squares. (On the next slide.)

• Write neatly & small.

• Do not cross out the name that is there (Messy!) – just write the new name under the old name.

Front - #104 – 118 Do not write in the symbols (green) yet. The symbols are included here as a reference. They will be added later.

• Unnilquadium = Rutherfordium Rf• Unnilpentium = Dubnium Db• Unnilhexium = Seaborgium Sg• Unnilseptium = Bohrium Bh• Unniloctium = Hassium Hs• Unnilennium = Meitnerium Mt

Front - Atomic Sq’s # 110 - 116

• Carefully add the names (shown on the next slide) to the empty squares.

Front - #104 - 118

• Darmstadtium Ds (Unuunilium) • Under – Platinum

• Roentgenium Rg (Unununium) • (Under – Gold)

• Copernicium Cn (Ununbium)• (Under – Mercury)

Front - #104 – 118 (Continued)

• Ununtrium Uut (Under – Thallium)

• Ununquadium Uuq (Under – Lead)

• Ununpentium Uup (Under – Bismuth)

• Ununhexium Uuh (Under – Polonium)

• Ununseptium Uus Uus (Under – Astatine)

• Ununoctium Uuo (Under – Radon)

Front – Atomic Numbers• In the upper right hand corner of

each atomic square, write in the ATOMIC NUMBER of each element.

• H – 1• He – 2 …• Make sure you have considered the

Rare Earth elements.

This is where to place your At. #’s.Remember to save space for coloring the edges of the square.

Element Name

Element Symbol

At. #

Atomic Mass

Atomic #’s• Period 1 – At. # 1 & 2• Period 2 – At. #’s 3 – 10• Period 3 – At. # ’s 11 – 18• Period 4 – At. # ’s 19 – 36• Period 5 – At. # ’s 37 – 54• Period 6 – At. # ’s 55 – 86• Period 7 – At. # ’s 87 - 118

Front – Chemical Symbol Key• In the lower left hand corner make a

key for the chemical symbols.

•CHEMICAL SYMBOLSRED = Gases

BLUE = LiquidsBLACK = Solids

GREEN = Manmade (Synthetic)

Front• As the teacher says the element, then its

symbol, write in the symbols for each element into its appropriate square. Use the appropriate color for the state of the element at “normal” earth temperatures.

– Don’t make your symbols too big.

–Remember: First letter is always a capital. Other letters – lower case.

This is where to place your Atomic Symbols.

Element Name

Element Symbol

At. #

Atomic Mass

Examples:

CuUuoNHg

Back - Notes• On the lower left hand side – write in

the notes for Metalloids & Rare Earth Elements.

Metalloids: (both sides of the zigzag line on the table)

• Properties: metalloids have the prop’s of both metals & nonmetals.– Solids can be dull or shiny (luster).– Will conduct heat or electricity but not as

well as metals.

Transition Metals & Rare Earth Elements:

• Families 3 – 12– Form alloys easily

• Lanthanide Series – (Period 6)– Soft, high luster & conductivity– Used in industry for high quality glass

& alloys

(Rare Earth Elements: Transition Metals)

• Actinide Series – (Period 7)– All are radioactive– All (except for the 1st four) are man

made in laboratories.– The best known is Uranium – used for

fuel in nuclear reactors.

Front – Atomic Masses• Write in the atomic masses of each

element – in the center bottom of the square, under the chemical symbol.)– Be careful- some of the numbers are

long. They need to fit into to the squares.

– Remember to write above the lines. You will need to add color to the squares.

Element Name

Element Symbol

At. #

Atomic Mass

Some masses are 8 digits long. (F)Listen carefully & record the data as the masses are read to you.

Front - Radioactivity• Add a symbol/key for radioactivity at the

bottom of the table. (Under # 114) - Radioactive

• An orange star or dot is good. • Place a star in each element’s square that

is radioactive. (Upper left hand corner of the square.)

• There are 36 elements that are radioactive (117 & 118 probably will be).

Element Name

Element Symbol

At. #

Atomic Mass

Put a star into the following squares. These elements are radioactive.

• #’s 43, 61, • 84 to 118

• (All of Period 7)

Color coding the Families of the Periodic Table

• We will make a key for the color coding of the table.

• Color each family on the front.– Color the inside edges of each box the

appropriate color.– Be careful NOT to color over any of the data

for the square.• Take notes about the family on the back

right side.• We will do one family at a time.

Front – Add the Families Key under the title – P. T. of E’s; center-left, above the metals line.

Families:

Alkali Metals Metalloids Alkaline Earth Metals Nonmetals Transition Metals Halogens Other Metals Noble Gases

Notes (back, right side.)

Title: FAMILIES/GROUPS• Precautions:

– You will need to be careful not to write too large. You will be using most of this space.

– Write the names of the families in regular pencil. Underline in the family’s color to code.

– Use your ruler to add the color to the inside edges of the atomic squares – neater & faster.

Front - Add brown to the inside edges of the Alkali Metal family

• Alkali Metals

–Family # 1 – all except Hydrogen• 6 squares – Lithium down to

Francium

Notes (back, right side.) Write the names of the families in regular pencil. Underline in the family’s color to code.

Title: FAMILIES/GROUPS

• Alkali Metals – (family # 1)– Valence # of 1; very reactive especially

with water; never found uncombined in nature.

– Soft, silver white; good conductors, lose electrons

Front - Add orange to the inside edges of the Alkaline Earth Metal family

Alkaline Earth Metals – all of family # 2- Beryllium down to Radium

- 6 squares

Notes (back, right side – under Alkali Metals)

• Alkaline Earth Metals – (family # 2)– Valence # of 2; very reactive but not as

reactive as family 1. (Lose electrons)– never found uncombined in nature - exist

in bonded compounds.

Front - Add pink to the inside edges of the Transition Metals family

Transition Metals– all of families # 3 - 12- All of the Rare Earth elements

- 68 squares

Notes - (back, right side – under Alkaline Earth Metals)

• Transition Metals – (families # 3 - 12)– Valence # of 1 or 2; valence electrons can be

lost or shared.– Properties similar to metals yet different;

“unpredictable”, good conductors.

Front - Add purple to the inside edges of the Other Metals family

• Other Metals – • 12 Elements (EVERY THING but Ge

and Sb)• Al, Ga, In, Tl, Pb, Bi, Po, Sn, Uut,

Uuq, Uup, Uuh

Notes - (back, right side – under Alkaline Earth Metals)

• Other Metals – (See notes to the left - Metals)

Front - Add blue to the inside edges of the Metalloids family• Metalloids - found on both sided of the

zigzag line.

• # 5 Boron - B• # 14 Silicon - Si• # 32 Germanium – Ge• # 33 Arsenic – As• # 51 Antimony – Sb• # 52 Tellurium – Te

Notes

• Boron – (Family 13) valence of 3 e- (Boron is a metalloid but the other elements in this family are “other” metals.

– Aluminum – most abundant metal; 3rd most abundant element in Earth’s crust

Front - Add green to the inside edges of the Nonmetals family• 6 elements

• # 6 Carbon• # 7 Nitrogen• # 8 Oxygen• # 15 Phosphorus• # 16 Sulfur• # 34 Selenium

Notes (back) – Carbon is a nonmetal but the other elements in this family are metalloids or other metals.• Carbon – (Family 14) 4 valence e-

– Carbon is the basis for life; makes carbon compounds like sugars & starches.

– Silicon – (a metalloid) second most abundant element in Earth’s crust.• Used for glass, cement, electronics

Notes (back) – Another family with a mixture of types.

• Nitrogen – (Family 15) 5 valence e- – tend to share e-– N = 78% of the Earth’s atmosphere– Used for fertilizers, explosives, medicines,

dyes

(Notes - back) • Oxygen – (Family 16) 6 valence e-

– Most e- are shared– Most abundant element in Earth’s crust– 2nd most abundant element in the

atmosphere– Combines with almost every other element.– O3 = ozone; Earth’s protective layer of the

atmosphere

• Front - Add gold or dark yellow to the inside edges of the Halogen family.

• 6 elements (Family # 17)• Fluorine down to Iodine

– # 9 Fluorine– # 17 Chlorine– # 35 Bromine– # 53 Iodine– # 85 Astatine - At– # 117 Ununseptium

Notes – (Back)• Halogens (Family 17) 7 valence e-

– Most reactive nonmetals (need only to gain 1 e-)

– Never found “free” – unbonded in nature– React with Family 1 readily. (React with metals

of family 1 to form salts. Ex. NaCl – sodium chloride or NaF – sodium fluoride)

Front - Add yellow to the inside edges of the Noble Gas family.

• 6 elements – Family 18– Helium down to Radon– # 2– # 10– # 18– # 36– # 54– # 86– #118

Notes – (Back)• Noble Gases – (Family 18) 8 valence e-

– Unreactive; do not readily form compounds because their valence levels are full.

– All found in small amounts in Earth’s atmosphere.

Finishing the Periodic Table• Make sure all of the information in

the squares is accurate & legible.• You will be graded on neatness

(legibility) & completeness on both sides.