New Area of Focus: Periodic Table of the Elements. New Area of Focus: Periodic Table of the Elements. Copyright © 2010 Ryan P. Murphy

New Area of Focus: Periodic Table of the Elements. New Area of Focus: Periodic Table of the Elements. Copyright © 2010 Ryan P. Murphy

The Periodic Table of the Elements is a… The Periodic Table of the Elements is a… Copyright © 2010 Ryan P. Murphy

A chart of all the known elements. A chart of all the known elements. Copyright © 2010 Ryan P. Murphy

Is in order of increasing atomic number and mass. Is in order of increasing atomic number and mass. Copyright © 2010 Ryan P. Murphy

HHe LiBeBCNOFNe NaMgAlSiPSClAr KCaScTiGaGeAsSeBrKr Atomic Mass and Atomic Number increases as you move across and down. Copyright © 2010 Ryan P. Murphy

The table puts elements into groups with similar characteristics. The table puts elements into groups with similar characteristics. Copyright © 2010 Ryan P. Murphy

Allows us to recognize trends over the whole array of elements. Allows us to recognize trends over the whole array of elements. Copyright © 2010 Ryan P. Murphy

All of the elements in a period have the same number of atomic orbitals. Copyright © 2010 Ryan P. Murphy

Horizontal row is called a Period. Horizontal row is called a Period. (Same # of electron orbitals) (Same # of electron orbitals) Vertical column is called a group/family. Vertical column is called a group/family. (Same # of valence electrons) (Same # of valence electrons) Copyright © 2010 Ryan P. Murphy

AMU increases from left to right and top to bottom. AMU increases from left to right and top to bottom. Copyright © 2010 Ryan P. Murphy

Density of elements increase down a group

HHe LiBeBCNOFNe NaMgAlSiPSClAr KCaScTiGaGeAsSeBrKr AMU increases as you go from left to right, and from top to bottom Copyright © 2010 Ryan P. Murphy

Electronegativity increases from lower left to upper right. Electronegativity increases from lower left to upper right. Copyright © 2010 Ryan P. Murphy Moving top to bottom down the periodic table, electronegativity decreases.

HHe LiBeBCNOFNe NaMgAlSiPSClAr KCaScTiGaGeAsSeBrKr Electron negativity Copyright © 2010 Ryan P. Murphy

The most strongly electronegative element, Fluorine (F). The least electronegative element is Francium (Fr). Copyright © 2010 Ryan P. Murphy “I want to give away one electron.” “I want to gain one electron” “I want to gain one electron” “You guys should get together.”

Electronegativity - chemical property that describes the tendency of an atom to attract electrons towards itself. Electronegativity - chemical property that describes the tendency of an atom to attract electrons towards itself. affected by both its atomic number and the distance at which its valence electrons reside from the charged nucleus. affected by both its atomic number and the distance at which its valence electrons reside from the charged nucleus. Copyright © 2010 Ryan P. Murphy

–Electrons with low ionization energies have a low electronegativity because their nuclei do not exert a strong attractive force on electrons. –Elements with high ionization energies have a high electronegativity due to the strong pull exerted on electrons by the nucleus. Copyright © 2010 Ryan P. Murphy and Ions) Ionization energy is the energy required to remove an electron. (Gases and Ions)

The ionization energy (IE) is defined as the amount of energy required to remove electron from the outer shell electron -increase as one moves from left to right within a given row (period) due to more electrons being added -decrease as one moves down a column (group) because the outer electron shell is getting further away from the nucleus

As atoms get smaller, the valence electrons are closer to the nucleus so the attractive force holding the electrons is stronger and makes it harder to remove

New Area of Focus: Electron Orbitals New Area of Focus: Electron Orbitals Copyright © 2010 Ryan P. Murphy

Valence electrons: Electrons in the outer most shell. Valence electrons: Electrons in the outer most shell. Copyright © 2010 Ryan P. Murphy Total Electrons

Lewis Dot Structure- atom model that represents the valence electrons only. - the valence electrons of atoms are the electrons that interact during the formation of compounds

Drawing the Lewis Dot Structure for the first three rows. Drawing the Lewis Dot Structure for the first three rows. Copyright © 2010 Ryan P. Murphy

Ion- an atom that has lost or gained electrons - if losing electrons, the ion becomes more positive; ex. If it loses 2 electrons, it will have a +2 charge - if gaining electrons, then the ion becomes more negative; ex. If it gains 2 electrons, it will have a -2 charge

Transition Metals are found in the middle. Transition Metals are found in the middle. Copyright © 2010 Ryan P. Murphy

Transition Metals are… Transition Metals are… Copyright © 2010 Ryan P. Murphy

Malleable: To be shaped / made into sheets. Malleable: To be shaped / made into sheets. Copyright © 2010 Ryan P. Murphy

Ductile: Made into wire. Ductile: Made into wire.

Good conductors of electricity. Good conductors of electricity. Copyright © 2010 Ryan P. Murphy

Copper (Cu) is a good conductor of electricity. –It is malleable and ductile. Copyright © 2010 Ryan P. Murphy

Have a high luster (shine). Have a high luster (shine). Copyright © 2010 Ryan P. Murphy

Conducts heat well. Conducts heat well. Copyright © 2010 Ryan P. Murphy

Most have a high density. Most have a high density. Copyright © 2010 Ryan P. Murphy

Most are solid. Most are solid. Hg (mercury is a liquid metal) Hg (mercury is a liquid metal) Copyright © 2010 Ryan P. Murphy

Metallically bonded. Metallically bonded. Copyright © 2010 Ryan P. Murphy

Many metals are reactive to chemicals. Many metals are reactive to chemicals. Copyright © 2010 Ryan P. Murphy

Many metals are reactive to chemicals. Many metals are reactive to chemicals. Copyright © 2010 Ryan P. Murphy

Many metals are reactive to chemicals. Many metals are reactive to chemicals. Copyright © 2010 Ryan P. Murphy

Almost 75% of all elements are classified as metals. Almost 75% of all elements are classified as metals. Copyright © 2010 Ryan P. Murphy

Alloys: Metals are easily combined Alloys: Metals are easily combined Copyright © 2010 Ryan P. Murphy

Bronze age: Copper and tin Copyright © 2010 Ryan P. Murphy

Continued Metals… Copyright © 2010 Ryan P. Murphy

Some of the metals. Use your table…. –Actinide Metals, Lanthanide Metals, Alkali Metals, Alkaline-Earth Metals, Noble Metals, Rare Metals, Rare-Earth Metals, and Transition Metals Copyright © 2010 Ryan P. Murphy

Flame test –Can be used to visually determine the identity of an unknown metal or metalloid ion based on the characteristic color when burned. –The heat of the flame converts the metal ions into atoms which become excited and emit visible light. –The characteristic emission spectra can be used to differentiate between some elements. Learn more at… _demonstration.pdfhttp:// _demonstration.pdf

Metalloids / Semi metals: Properties of metals and non-metals Metalloids / Semi metals: Properties of metals and non-metals Copyright © 2010 Ryan P. Murphy

Semi-conductors Semi-conductors Copyright © 2010 Ryan P. Murphy

Brittle Brittle Copyright © 2010 Ryan P. Murphy

Can have luster. Can have luster. Copyright © 2010 Ryan P. Murphy

HHe LiBeBCNOFNe NaMgAlSiPSClAr KCaScTiGaGeAsSeBrKr Key: Metalloids / Semimetals Copyright © 2010 Ryan P. Murphy

Non-Metals Non-Metals Not metals Not metals Copyright © 2010 Ryan P. Murphy

HHe LiBeBCNOFNe NaMgAlSiPSClAr KCaScTiGaGeAsSeBrKr Key: Non-metals Copyright © 2010 Ryan P. Murphy H

Non-metals… Non-metals… Copyright © 2010 Ryan P. Murphy

H and He are non-metals. H and He are non-metals. Copyright © 2010 Ryan P. Murphy

They are poor conductors. They are poor conductors. Copyright © 2010 Ryan P. Murphy

They are brittle (break when hit). They are brittle (break when hit). Copyright © 2010 Ryan P. Murphy

Dull in color. (No Luster) Dull in color. (No Luster) Copyright © 2010 Ryan P. Murphy

Poor conductors of heat. Poor conductors of heat. Copyright © 2010 Ryan P. Murphy

They may be transparent or translucent. They may be transparent or translucent. Copyright © 2010 Ryan P. Murphy

They exist as a… (s), (l), (g). They exist as a… (s), (l), (g). Copyright © 2010 Ryan P. Murphy Solid Liquid Gas S Sulfur Br Bromine Cl Chlorine

Covalently bonded. Covalently bonded. Copyright © 2010 Ryan P. Murphy CH 4 Methane Electron Negativity Diff. Hydrogen = 2.20 Carbon = – 2.20 =.35 Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar.

They have a low density. They have a low density. Copyright © 2010 Ryan P. Murphy