Coloring the Periodic Table Families Mendeleevs Periodic Table

Coloring the Periodic Table Families

Mendeleev's Periodic Table Original Russian Version Mendeleev is credited with creating the first real periodic table of the elements, where trends (periodicity) could be seen when the elements were ordered according to atomic weight. See the ? and blank spaces? Those are where elements were predicted.

Periodic Table • The periodic table organizes the elements in a particular way. A great deal of information about an element can be gathered from its position in the period table. • For example, you can predict with reasonably good accuracy the physical and chemical properties of the element. You can also predict what other elements a particular element will react with chemically. • Understanding the organization and plan of the periodic table will help you obtain basic information about each of the 118 known elements.

Properties of Metals • Metals are good conductors of heat and electricity. • Metals are shiny. • Metals are ductile (can be stretched into thin wires). • Metals are malleable (can be pounded into thin sheets). • A chemical property of metal is its reaction with water which results in corrosion.

Properties of Non-Metals • Non-metals are poor conductors of heat and electricity. • Non-metals are not ductile or malleable. • Solid non-metals are brittle and break easily. • They are dull. • Many non-metals are gases. Sulfur

Properties of Metalloids • Metalloids (metal-like) have properties of both metals and non-metals. • They are solids that can be shiny or dull. • They conduct heat and electricity better than nonmetals but not as well as metals. • They are ductile and malleable. Silicon

Families on the Periodic Table • Elements on the periodic table can be grouped into families bases on their chemical properties. • Each family has a specific name to differentiate it from the other families in the periodic table. • Elements in each family react differently with other elements.

ALKALI METALS Group 1 • Hydrogen is not a member, it is a non-metal • 1 electron in the outer shell • Soft and silvery metals • Very reactive, esp. with water • Conduct electricity • Alkali metals are never found as free elements in nature. They are always bonded with another element. Image: http: //www. learner. org/interactives/periodic/groups 2. html

ALKALINE EARTH METALS Group 2 • 2 electrons in the outer shell • White and malleable • Reactive, but less than Alkali metals • Conduct electricity • They are never found uncombined in nature

TRANSITION METALS Groups in the middle Good conductors of heat and electricity. Some are used for jewelry. The transition metals are able to put up to 32 electrons in their second to last shell. Can bond with many elements in a variety of shapes.

Transition Metals • 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-tooutermost level.

Transition Elements • Transition elements have properties similar to one another and to other metals, but their properties do not fit in with those of any other family. • Many transition metals combine chemically with oxygen to form compounds called oxides.

BORON FAMILY Group 3 • 3 electrons in the outer shell • Most are metals • Boron is a metalloid

CARBON FAMILY Group 4 • 4 electrons in the outer shell • Contains metals, metalloids, and a non-metal Carbon (C) • The element carbon is called the “basis of life. ” There is an entire branch of chemistry devoted to carbon compounds called organic chemistry.

NITROGEN FAMILY Group 5 • 5 electrons in the outer shell • Can share electrons to form compounds • Contains metals, metalloids, and non-metals

OXYGEN FAMILY Group 6 • 6 electrons in the outer shell • Contains metals, metalloids, and non -metals • Reactive • Oxygen is the most abundant element in the earth’s crust. It is extremely active and combines with almost all elements.

Halogens Group 7 • 7 electrons in the outer shell • All are non-metals • Very reactive are often bonded with elements from Grp 1 • Halogen atoms only need to gain 1 electron to fill their outermost energy level. • They react with alkali metals to form salts.

Noble Gases Group 8 Exist as gases Non-metals 8 electrons in the outer shell = Full Helium (He) has only 2 electrons in the outer shell = Full Not reactive with other elements The family includes helium, neon, argon, krypton, xenon, and radon. All the noble gases are found in small amounts in the earth's atmosphere.

Rare Earth Metals • Some are Radioactive • The rare earths are silver, silverywhite, or gray metals. • The thirty rare earth elements are composed of the lanthanide and actinide series.

Trend in Atomic Radius • The size of atomic species as determined by the boundaries of the valence e-. Largest atomic species are those found in the SW corner

Trend in Atomic Radius • The atomic radius refers to the distance between an atom's nucleus and its valence electrons. Remember, the closer an electron is to the nucleus, the lower its energy and the more tightly it is held. • As atomic number increases, the charge on the nucleus increases and the number of occupied energy levels increases. • Electrons are drawn closer to the nucleus and there is an increase in positive charge

Trend in Ionization Potential The energy required to remove the valence electron from an atomic species. Largest toward NE corner of PT since these atoms hold on to their valence e- the tightest.

Trend in Ionization Potential • The ionization energy is the energy it takes to fully remove an electron from the atom. • Electrons are more stable when they have a full valence shell; they are also relatively more stable when they at least have a full subshell.