Coloring the Periodic Table - Families

Bellringer 9/27Write the Bohr model for CalciumPeriodic Table Trends

Periodic TablePeriodic Table arrangement of elements in order of increasing atomic number with elements having similar properties in vertical columnsGroups vertical columnsPeriods horizontal rowsALKALI METALSGroup 1Hydrogen is not a member, it is a non-metal1 electron in the outer shellSoft and silvery metalsVery reactive, esp. with waterConduct electricity

Image: http://www.learner.org/interactives/periodic/groups2.html ALKALINE EARTH METALSGroup 22 electrons in the outer shellWhite and malleableReactive, but less than Alkali metalsConduct electricity

TRANSITION METALSGroups 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.

BORON FAMILY Group 33 electrons in the outer shellMost are metalsBoron is a metalloid

CARBON FAMILY Group 44 electrons in the outer shellContains metals, metalloids, and a non-metal Carbon (C)

NITROGEN FAMILY Group 55 electrons in the outer shellCan share electrons to form compoundsContains metals, metalloids, and non-metals

OXYGEN FAMILY Group 66 electrons in the outer shellContains metals, metalloids, and non-metalsReactive

HalogensGroup 77 electrons in the outer shellAll are non-metalsVery reactive are often bonded with elements from Group 1

Noble GasesGroup 8Exist as gasesNon-metals8 electrons in the outer shell = FullHelium (He) has only 2 electrons in the outer shell = FullNot reactive with other elements

Rare Earth MetalsSome are RadioactiveThe rare earths are silver, silvery-white, or gray metals. Conduct electricity

GroupsRepresentative elements group A elements

Transition elements group B elements

Lanthanide and actinide series = inner transition metalsGroups (reminder)The group = number of valence electrons that the element hasValence electrons are electrons in the outermost shell of the atomAll group 1A elements have 1 valence electron. Likewise, all group 8A elements have 8 valence electrons.ChargesEvery element wants 8 valence electrons to become stable. They will gain or lose valence electrons to form an octetFor exampleGroup 1A elements have 1 valence electron. They can either gain 7 electrons to have an octet or lose 1.What is easier?Lose 1If an element loses 1 electron (1 negative charge) what charge will the resulting ion have?+1

Oxidation numbers

The charge an element would have if it released or obtained electrons to look like a noble gas.

Metals release electronsNonmetals obtain electronsCharacteristicsElements in the same group exhibit similar chemical characteristics due to the fact that they all have the same number of valence electrons.

The most stable number of valence electrons is 8

called an octetPredict the oxidation numbers for the followingA. AlB. MgC. ND. NaE. ClPhysical States and Classes of the ElementsMajority of the elements are metals. They occupy the entire left side and center of the periodic table.Nonmetals occupy the upper-right-hand corner.Metalloids are located along the boundary between metals and nonmetalsMetalsMetals elements that have luster, conduct heat and electricity, and usually bend without breaking.Transition MetalsThe elements in Groups 3 through 12 of the periodic table are called the transition elements.All transition elements are metals.Many transition metals can have more than one chargeInner Transition MetalsIn the periodic table, two series of elements, atomic numbers 58-71 and 90-103, are placed below the main body of the table.These elements are separated from the main table because putting them in their proper position would make the table very wide.The elements in these two series are known as the inner transition elements.Inner Transition MetalsLanthanidesFirst series of inner transition element follow element number 57, lanthanum.actinides, 2nd series of inner transition elementshave atomic numbers ranging from 90 (thorium, Th) to 103 (lawrencium, Lr).

Non MetalsAlthough the majority of the elements in the periodic table are metals, many nonmetals are abundant in natureMost nonmetals dont conduct electricity, are much poorer conductors of heat than metals, brittle when solid.Many are gases at room temperature; those that are solids lack the luster of metals.Properties of Metals and Nonmetals

MetalloidsMetalloids have some chemical and physical properties of metals and other properties of nonmetals.In the periodic table, the metalloids lie along the border between metals and nonmetals.Bellringer 9/28Given: iodine, helium, sulfur, or hydrogen, which is a halogen?Periodic TrendsPeriodic Trends are trends that occur across the periodic table and down the periodic tableThey include: atomic radius, Ionization energy, electro negativity, metallic characterionic radiusAtomic RadiusAtomic Radius size of the atom

IncreasesDecreasesAtomic radiusThe distance from the outer edge of the electron cloud to the nucleus.The radius increases as the principle quantum number increases. So elements increase going from top to bottom.The period they are in increased, radius increases.As you move from left to right across the period things change.The # of protons in the nucleus increases. This causes the electrons to be attracted to the nucleus more and the size of the elements decrease.As you move from left to right radius decreases.Which element in the pair is larger?A. Sn, SrB. Cl, IC. S,PD. Ac, UE. Na, RbF. B, Al

Determining the Atomic Radius of a Nonmetal (Chlorine)Click in this box to enter notes.

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Determining the Atomic Radius of a Metal (Molybdenum)Click in this box to enter notes.

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Ionization energyThe energy required to remove the most loosely held electron from an element.Large radii elements lose electrons easilySmall radii elements require energy to remove electrons.

Metals- dont like electrons lose them easilyNonmetals like electrons, want to keep them, require energy to remove them.

Electro negativityElectro negativity the ability of an atom to attract another atom

DecreasesIncreasesMetallic CharacterMetallic character how much like a metal the element is

IncreasesDecreasesElectron affinityThe ability of an atom to attract electrons to itself.

Metal = low affinityNonmetals = high affinity

Large radius = low affinitySmall radius high affinityMetals and nonmetalsMetals tend to lose electrons.Nonmetals tend to gain electrons.The goal is to get enough electrons in the outer energy level to look like a noble gas.

Every electron lost leaves behind a net + charge.Energy electron gained causes a net charge.

These charges effect the radius of the elements.

Elements with charges are called ionsIonic radiusThe more + charge an ion has the greater the ability to attract electrons to itself and is therefore smaller.The more charge an ion has the more electrons it has pulling away from the nucleus and therefore they are larger.

Ionic RadiusWhen you talk about ionic radius, you are comparing an atom and its ionWhen an atom has a negative charge, you have added electronsWhich makes it biggerFor example, which will be larger:Cl or Cl-1Ionic RadiusWhen an atom has a positive charge, you have taken away electronsWhich makes it smallerFor example, which will be larger:Na or Na+1Which is larger?A. Ca, Ca+2B. Cl, Cl-C. Br-, F-D. Pb, Pb+4

Periodic Table TrendsClick in this box to enter notes.

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Ionic RadiiCopyright Houghton Mifflin Company. All rights reserved.Click in this box to enter notes.

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