Why do you think there are question marks here? Image taken from: Mendeleev’s Published Periodic Table of Elements

Date Predicted 1871Date Discovered 1886 Atomic Mass72Atomic Mass72.6 Density5.5 g/cm 3 Density5.47 g/cm 3 Bonding Power4 4 ColorDark GrayColorGrayish White “Ekasilicon”Germanium Notice how Mendeleev’s predictions (orange column) were very accurate when compared to Germanium’s actual characteristics (green column)

Image taken from:

Activity! Your table group is going to get a group of cards. Each table one at a time will lay down the cards in a logical order. Think Dimitri Mendeleev and organizing according to valence and atomic mass. Copyright © 2010 Ryan P. Murphy

Answer! Copyright © 2010 Ryan P. Murphy

Sulfur

Silicon

antimony (Sb) H Li Na K Rb Cs Fr Be ScTi Mg VCrMnFeCoNiCuZnGaGeSeBrCaKr YZrNbMoTcRuPdAgCdInSnSbSrTeRh BaHfTaWReOsIrAuHgTlPbBiPoLaAtPt RaRfDbSgBhHsMt??Ac? AlP NO SCl FNe Ar Rn I Si Xe He BC As Fe MgSP S P Cu IISb iodine (I) iron (Fe) copper (Cu) phosphorus (P) sulfur (S) magnesium (Mg)

Metals and non-metals in the periodic table The periodic table is a list of all the known elements which are arranged according to the similarities in their properties. Non-metals are mostly on the right. Metals are on the left and in the centre. What type of elements are between metals and non-metals? Xe

Types of elements in the periodic table

Metal, non-metal or metalloid? H Li Na K Rb Cs Fr Be ScTi Mg VCrMnFeCoNiCuZnGaGeSeBrCaKr YZrNbMoTcRuPdAgCdInSnSbSrTeRh BaHfTaWReOsIrAuHgTlPbBiPoLaAtPt RaRfDbSgBhHsMt??Ac? AlP NO SCl FNe Ar Rn I Si Xe He BC As silicon (Si) metalloid francium (Fr) metal scandium (Sc) metal krypton (Kr) non-metal cobalt (Co) metal What are metalloids? Which side are the non- metals on? Which side are the metals on? Along the stair-step line. Metalloids sometimes behave like metals and sometimes like non-metals. Metals are on the left and in the center. Non-metals are mostly on the right.

Copyright © 2010 Ryan P. Murphy

Periods go at the end of sentences and sentences go across.

All of the elements in a period have the same number of atomic shells or energy levels. Copyright © 2010 Ryan P. Murphy

One shell

Copyright © 2010 Ryan P. Murphy One shell Valence Electrons

Copyright © 2010 Ryan P. Murphy

Two shells

Copyright © 2010 Ryan P. Murphy

Periods = Rows In the periodic table, elements have something in common if they are in the same row. All of the elements in a period have the same number of atomic shells or energy levels.atomic Every element in the top row (the first period) has one shell for its electrons. All of the elements in the second row (the second period) have two shells for their electrons. It goes down the periodic table like that. electrons

Vertical column is called a group/family. Copyright © 2010 Ryan P. Murphy Families should stand tall together Elements in the same family have similar properties, much like you have similar “properties” to members of your family. Elements in a family have the same number of valence electrons.

The hydrogen square sits atop Family AI, but it is not a member of that family. Hydrogen is in a class of its own. It’s a gas at room temperature. It has one proton and one electron and only one energy level. Hydrogen only needs 2 electrons to fill up its valence shell.

The alkali family is found in the first column of the periodic table. Atoms of the alkali metals have a single electron in their outermost level, in other words, 1 valence electron. They are shiny, have the consistency of clay, and are easily cut with a knife.

They are the most reactive metals. They react violently with water. Alkali metals are never found as free elements in nature. They are always bonded with another element.

They are never found uncombined in nature. They have two valence electrons. Alkaline earth metals include magnesium and calcium, among others.

These are the metals you are probably most familiar: copper, tin, zinc, iron, nickel, gold, and silver. They are good conductors of heat and electricity.

The compounds of transition metals are usually brightly colored and are often used to color paints. Transition elements have 1 or 2 valence electrons, which they lose when they form bonds with other atoms. Some transition elements can lose electrons in their next-to- outermost level.

The Boron Family is named after the first element in the family. Atoms in this family have 3 valence electrons. This family includes a metalloid (boron), and the rest are metals. This family includes the most abundant metal in the earth’s crust (aluminum).

Atoms of this family have 4 valence electrons. This family includes a non-metal (carbon), metalloids, and metals. The element carbon is called the “basis of life.” There is an entire branch of chemistry devoted to carbon compounds called organic chemistry.

The nitrogen family is named after the element that makes up 78% of our atmosphere. This family includes non-metals, metalloids, and metals. Atoms in the nitrogen family have 5 valence electrons. They tend to share electrons when they bond. Other elements in this family are phosphorus, arsenic, antimony, and bismuth.

Atoms of this family have 6 valence electrons. Most elements in this family share electrons when forming compounds. Oxygen is the most abundant element in the earth’s crust. It is extremely active and combines with almost all elements.

The elements in this family are fluorine, chlorine, bromine, iodine, and astatine. Halogens have 7 valence electrons, which explains why they are the most active non- metals. They are never found free in nature. Halogen atoms only need to gain 1 electron to fill their outermost energy level. They react with alkali metals to form salts.

Noble Gases are colorless gases that are extremely un-reactive. One important property of the noble gases is their inactivity. They are inactive because their outermost energy level is full. Because they do not readily combine with other elements to form compounds, the noble gases are called inert. The family of noble gases includes helium, neon, argon, krypton, xenon, and radon. All the noble gases are found in small amounts in the earth's atmosphere.