Periodic Table Families and Properties

Periodic Table Families and Properties

Metals, Non-Metals, and Metalloids

• Metals – Shiny, lustrous, ductile and malleable, and very good conductors of heat and electricity.  Usually solid.

• Metalloids – Shiny, brittle and a fair conductor of heat and electricity.

• Nonmetals – Dull, brittle, poor conductors of heat and electricity.  Usually liquid and gas.

Hydrogen

• Represented by the symbol H and the electron configuration 1s1.

• A colorless, odorless, tasteless gas.

• Hydrogen forms more compounds than any other element. Most abundant element in the universe.

• Very little free H in the earth’s atmosphere. It is a diatomic gas; H₂

• Has the lowest density of ALL gases at room temperature and pressure.

• It is flammable.

Group 1: Alkali Metals

• Li, Na, K, Rb, Cs, and Fr (Notice H is NOT a Alkali metal)

• Do NOT occur in nature as elements.

• Usually a white salt compound

• Are very reactive metals (Very reactive with H₂O)

• 1 valence e-

• Forms 1+ ions

Group 1: Alkali Metals

• Are good conductors of heat and electricity.

• Are ductile, malleable and are soft enough to be cut with a knife.

• Have a silvery luster

• Low density

• Low melting/boiling point

Group 2: Alkaline Earth Metals

• Be, Mg, Ca, Sr, Ba, and Ra

• Do NOT occur naturally in their elemental state. - Usually a salt

• Are less reactive than alkali metals.

• Are good conductors of heat and electricity, ductile are malleable and have silvery luster

• 2 valence e-

• Forms 2+ ions

Groups 3-12: Transition Metals

• Consist of metals

• Valence e- not predictable so no predictable charges for ions.

• Usually harder and more brittle than metals in groups 1 & 2

• Have higher m.p. and b.p. than metals in groups 1 & 2

• Are malleable and ductile

• Have silvery luster, except copper & gold

The Lanthanides & Actinides

• Lanthanides: Shiny, silvery metals similar in reactivity to group 2.

• Actinides: All radioactive, Three were found on earth, the rest were man-made.

Group 13: Boron Family

• B, Al, Ga, In, and Tl

• Do NOT occur in element form.(except Al)

• Are scarce in nature (except Al, which is the most abundant metallic element).

• Are metallic solids (except B, which is a solid metalloid).

• Are soft and have low m.p. (except B, which is hard and has a high m.p.).

• Are chmclly rxtive @ moderate temperatures (except B).

• 3 valence e- : Forms 3+ ions

Group 14: Carbon Family

• C, Si, Ge, Sn and Pb

• Includes a nonmetal (C), two metalloids (Si & Ge), and two metals (Sn & Pb).

• Vary greatly in both physical & chemical properties

• Occur in nature in both combined and elemental forms.

• 4 valence e- : Forms 4+/4- ions

• Are relatively unreactive

Group 15: Nitrogen Family

• N, P, As, Sb, and Bi

• Consist of two nonmetals (N & P), two metalloids (As & Sb) and one metal (Bi)

• Range from very abundant elements

  (N & P) to relatively rare elements

  (As, Sb & Bi).

• Contain 5 valence e-

• Forms 3- ions

Group 16: Oxygen Family

• O, S, Se, Te and Po.

• Occur naturally as elements & in combined states.

• Consist of 3 nonmetals (O, S & Se), 1 metalloid (Te) and 1 metal (Po).

• Tend to exist as polyatomic molecules, such as O₂, O₃, S₆, S₈ and Se₈.

• 6 valence e-

• Forms 2- ions

Group 17: Halogen Family

• F, Cl, Br, I and At

• Are all nonmetals

• Are found in the rocks of Earth’s crust and dissolved in sea water.

• Exist at room temp as a gas (F₂ & Cl₂), a liquid (Br₂) and a solid (I₂ & At). - Most are diatomic

• Are highly reactive

• Have 7 valence e-

• Forms 1- ions

Group 18: The Noble Gases

• All elements in the group are gases: He, Ne, Ar, Kr, Xe, Rn.

• Found in minute quantities in the atmosphere. 

• Helium can be obtained from natural gas wells where it has accumulated as a result of radioactive decay.

• 8 valence electrons

• Do not form ions

Group 18: The Noble Gases

• All gases & are monatomic.

• Originally named the “inert gases”, b/c it was thought they formed no compounds.

• Generally considered to be unreactive, b/c they have “closed-shell” configurations.

• Krypton reacts with Fluorine to form KrF₂

• Xenon forms a wide range of compounds w/ O₂ and F.

Multiple Choice

Which color on the image of the periodic table corresponds with the metalloids.

• bright yellow

• gold

• teal

• light blue

Multiple Choice

Has 8 valence electrons and a stable electron configuration

• Alkali metals

• Alkaline Earth metals

• Halogens

• Noble gases

• Oxygen group

Multiple Choice

Has a +2 charge

• Alkali metals

• Alkaline Earth metals

• Halogens

• Noble gases

• Oxygen group

Multiple Choice

Has 6 valence electrons

• Alkali metals

• Alkaline Earth metals

• Halogens

• Noble gases

• Oxygen group

Multiple Choice

This type of element is dull, brittle solids and gases, insulators, poor conductors of heat and electricity, as well as having low melting points.

• metals

• metalloids

• nonmetals

Multiple Choice

The is family has properties of both metals and nonmetals.

• Alkali

• Halogens

• Nonmetals

• Metalloids

Multiple Choice

Which of the following is the most reactive group of non-metals? 

• Alkali
• Alkali Earth
• Halogen
• Noble Gas

Multiple Choice

The elements in this family are soft, silvery, and very reactive with water.

• Alkaline Earth Metals

• Alkali Metals

• Transition Metals

• Lanthanides

Multiple Choice

What group on the Periodic Table contains the elements of the alkaline earth family?

• 1
• 2
• 17
• 18

Multiple Choice

Which properties are characteristic of the Group 1 metals?

• high reactivity and the formation of unstable compounds
• low reactivity and the formation of unstable compounds
• high reactivity and the formation of stable compounds
• low reactivity and the formation of stable compounds