10/31 Happy Halloween OPENER: Identify the element based on it’s electron configuration. Turn in your Periodic Trends POGIL if you didn’t yesterday!

Periodic Trends Identify trend patterns within the periodic table and predict element traits based on their position.

Properties of Metals 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 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 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

PLICKER TIME An elemental sample shattered when hammered, what type of element is it? A. Metal B. Non Metal C. Metalloid

PLICKER TIME An elemental sample was drawn into wire and conducts electricity, what type of element is it? A. Metal B. Non Metal C. Metalloid

PLICKER TIME An elemental sample conducts electricity but is not malleable, what type of element is it? A. Metal B. Non Metal C. Metalloid

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 Ionic Size Cations are always smaller than the atoms from which they form Anions are always larger than the atoms from which they form Talk with your neighbor-WHY? K K+ Cl Cl-

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. Why is this true? As you move across a period, nuclear shielding remains constant while nuclear charge/pull increases. It gets more difficult to remove an electron. What does this mean?

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 How can we explain this in terms of coulombic attraction?

Columbic Attraction The Coulomb force between two or more charged bodies is the force between them due to Coulomb's law. If the particles are both positively or negatively charged, the force is repulsive; if they are of opposite charge, it is attractive. Like charges repel, opposites attract.

PLICKER TIME Based on its position on the periodic table, predict which element has the highest electronegativity. A. Barium (Ba) B. Lead (Pb) C. Carbon (C) D. Tungsten (W)

PLICKER TIME Based on its position on the periodic table, predict which element has the highest atomic radius. A. Barium (Ba) B. Lead (Pb) C. Carbon (C) D. Tungsten (W)

PLICKER TIME Based on its position on the periodic table, predict which element has the lowest ionization energy. A. Barium (Ba) B. Lead (Pb) C. Carbon (C) D. Tungsten (W)

PLICKER TIME What combination of subatomic particles would attract each other? A. Two Electrons B. An electron & neutron C. An electron & proton D. A proton & neutron

Periodic Trends 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