Download Thursday, October 31, 2013 D-day

Thursday, October 31, 2013
D-day
As you enter, take out your 5.1 & 5.3
reading guides and prepare for a quiz.
Review of special groups
Important info (hint, hint)
• Alkali metals
– Group ??
– 1 valence electron
– VERY reactive to water and oxygen.
• Alkaline Earth metals
– Group ??
– Too reactive to occur naturally in nature as pure
elements.
– NOT as reactive as alkali metals.
• Halogens
– Only group which has all three states of matter at
STP. (what is STP?)
– Most reactive nonmetals.
– These elements are all brightly colored.
• Noble Gases
– Have their valence shell filled.
– VERY unreactive (inert).
• Radioactive Elements- no naturally occurring
stable isotope (what is an isotope?).
– These elements loose neutrons and protons and
emit them as particles.
– All manmade elements are radioactive.
• Transuranium elements- element with an
atomic number above 92 (uranium).
• Diatomic elements- two atoms of the same
element bonded together.
– “BrINClHOF”
– Place a dot on your periodic table to indicate
these elements are diatomic.
Periodic Trends
• Jigsaw activity
– At the end we will regroup and review the
material.
Block 3 Groups
Group 1
Group 2
Group 3
Alexis
Michael R.
Allison
SkyLynn
Bianca
Andrea
Kayla
Tyler
Jacob
Skylar
Amanda
Cassie
Kollin
Group 4
Group 5
Group 6
Adam
Laura
Christen
Nephy
Carly
Beth
Gabbi
Shelby
Michael H.
Ross
Aimee
Julie
Jigsaw groups
Group 1
Group 2
Group 3
Alexis
Shelby
Amanda
Michael R.
Gabbi
Cassie
Allison
Beth
Skylar
Group 4
Group 5
Group 6
SkyLynn
Carly
Kollin
Adam
Jacob
Michael H.
Laura
Tyler
Ross
Group 7
Group 8
Christen
Kayla
Aimee
Nephy
Andrea
Julie
Bianca
Block 4 Groups
Group 1
Group 2
Group 3
Alex
Cal
Bri
YingYing
Hope
Avery
Simran
Josh
Trevor
Brooke
Addison
Kim
Stephen
Jigsaw Groups
Group 1
Group 2
Alex
Avery
Kim
Trevor
Cal
Hope
Brooke
Group 3
Group 4
Bri
Josh
Addison
Ying Ying
Simran
Stephen
Atomic Radius
• Half the distance
between the nuclei of
two atoms of the same
element when the
elements are joined.
• Trend- Size increases
from top to bottom
within a group and
decreases from left to
right in a period.
• Why?
Ionization energy
• Amount of energy needed to strip an electron
from the valence shell of an atom.
• Trend- Ionization energy decreases from top
to bottom in a group and increases from left
to right in a period.
• Why?
– Electron Shielding
Ionic Radii
• As atoms gain and lose electrons, their radius
changes accordingly.
• Cations- always smaller than the atoms from
which they form.
– Why?
• Anions- always larger than the atoms from
which they form?
– Why?
Electronegativity
• Ability of an atom to gain electrons when in a
compound.
– Based on ionization energy and other factors.
• Trend- Decreases from top to bottom of a
group and increase from left to right.
– Where in the reference tables can you find
electronegativity?
• Why do we see this trend?