10/20 Opener Determine the electron configuration of the following elements: Cl K Al

Organizing the Elements Labeling the Periodic Table Properties of M, NM, & Metalloids

I. Labeling the Periodic Table The columns are called groups or families Groups are numbered 1-8 1 8 2 3 4 5 6 7 The rows are called periods Skip these All Elements greater than uranium did not exist on Earth until people produced them in nuclear reactors

I. Labeling the Periodic Table Boron Family Carbon Family Nitrogen Family Oxygen Family Nobel Gases Alkaline Earth Metals Halogens Alkali Metals Transition Metals Rare Earth Elements

I. Labeling the Periodic Table Finally, color the non-metals. Next, let’s identify all the elements that are normally gases by coloring the upper right hand corner with different color. First, let’s identify all the elements that are normally liquids by coloring the upper right hand corner with one of your five colors. Now, let’s identify all the elements that are metals. Remember that metals are found to the left of the stair step line. Color the metals one of your colors. Now, let’s identify all the elements that are diatomic by coloring the lower left hand corner with different color.

Properties of Metals (Put this in your notebook!) Conduct heat and electricity well Called “conductors” Malleable – can be hammered into this sheets Ductile – can be pulled into long thin wires Metals have a metallic luster – they shine when polished

Properties of Non-Metals (Put this in your notebook!) Poor conductors of heat and electricity Called “insulators” Tend to be much more brittle than metal When you hit a non-metal with a hammer it tends to shatter and not flatten out Not ductile or malleable

Metalloids (Put this in your notebook!) Elements that border the stair step line that separates metals from non-metals are known as metalloids Their properties are a mixture of metallic and non-metallic

Periodic Trends Atomic Radius Electronegativity Ionization Energy

Periodic Trends: Atomic Radius Atomic Radius is ½ the distance between nuclei of two atoms of the same element joined

Going Down a Group In general atomic size increases from top to bottom With each new energy level added the atom gets bigger. 1 2 3 Etc. …

Going Across a Period No new energy levels added, but more more p+ added to nucleus

Ions An atom or group of atoms that has a positive or negative charge These form when electrons are transferred from atom to atom A cation is positive (+) (think cats have paws-pawsitive) A anion is negative (-) (think onions anions yuck-negative)

Trends in Ionization Ionization energy is the energy required to remove an electron from an atom Ionization energy tends to decrease from top to bottom and increase from left to right across a period

Group and Period Trends As the size of an atom increases within a group, it gets easier to pull off an electron As you move across a period, shielding remains constant while nuclear charge/pull increases. It gets more difficult to remove an electron.

Trends in Ionic Size Cations are always smaller than the atoms from which they form Anions are always larger than the atoms from which they form K+ K Cl Cl-

Trends in Electronegativity Electronegativity is the ability of an atom to attract electrons when the atom is in a compound Electronegativity decreases from top to bottom in a group Electronegativity tends to increase from left to right across the table

Periodic Trends (Put this in your notebook!) Atomic Radius Atomic Radius is ½ the distance between nuclei of two atoms of the same element joined In general atomic size increases from top to bottom & decreases from left to right across a period Electronegativity the ability of an atom to attract electrons when the atom is in a compound Tends to decreases from top to bottom in a group & increase from left to right across the table Ionization Energy Ionization energy is the energy required to remove an electron from an atom Ionization energy tends to decrease from top to bottom and increase from left to right across a period