Transcript Middle East Jeopardy

Periodic Jeopardy
Group
Properties
Electron
Configurations
Atomic Radii
Ionization
Energy
Electronegativit
y
100
100
100
100
100
200
200
200
200
200
300
300
300
300
300
400
400
400
400
400
500
500
500
500
500
FINAL
Group Properties 100
What group of elements forms no
charges, or bonds due to stable s2p6
octets of valence electrons?
Noble Gases
Group Properties 200
What group of elements can be cut
with a knife, may react explosively
in water, & form +1 ions due to their
s1 valence electrons?
Alkali Metals
Group Properties 300
What group of elements tend include
very reactive gases, a liquid & a
solid that tend to form -1 ions or a
single bond due to their s2p5
valence electrons?
Halogens
Group Properties 400
What group of elements behave as
reactive metals and tend to form +2 ions
due to their s2 valence electrons?
Alkaline Earth Metals
Group Properties 500
What group of elements behave as metals
with loose ‘s’ electrons. However, they
may form multiple ions of different
charges due to their incomplete ‘d’
sublevel.
Transition Metals
Electron Configurations 100
What are the common valence electrons
of elements in the Oxygen group?
2
4
sp
Electron Configurations 200
What is the kernel of the electron
configuration for zinc?
[Ar]
Electron Configuations 300
What element has the following
abbreviated electron configuration?
[Kr]5s24d105p5
Iodine
Electron Configurations 400
What sublevel can contain up to 6 total
electrons, has dumb-bell shaped orbitals,
and is located on the 3rd primary energy
level?
3p
Electron Configurations 500
Which sublevel is the first to have a lower
than expected energy due to it’s simplicity
and lack of electron traffic such that it is
filled before another sublevel with a lower
primary energy level?
4s
Atomic Radii 100
Which direction do atomic radii
increase in the periodic table?
Downward
Atomic Radii 200
The “Size Surprise” is that atomic radii
decrease as you move _____ in the periodic
table.
Right
Atomic Radii 300
Atomic radii increase down the
periodic table due to additional
_____ _____.
Energy Levels
Atomic Radii 400
Atomic radii decrease across each period
of the periodic table due to increased
positive _____ _____ with the outermost
“valence” electrons.
Nuclear Attractions
Atomic Radii 500
Increased atomic radii down a group is
reinforced by interference of inner shell
electrons with attraction of the positive
nucleus for outer shell electrons. This is
called the _____ effect
Shielding
Ionization Energy 100
Ionization energy refers to the energy
required to _____ an electron from an atom.
remove
Ionization Energy 200
Ionization energy _____ as you move
right across the periodic table
increases
DAILY DOUBLE – Ionization
Energy
Rank the following 3 elements in order
from lowest to highest ionization
energy:
O, Ba, Si
Ba, Si, O
Ionization Energy 400
As you move right across the periodic table,
the ionization energy gets higher because the
_____ _____ get stronger.
Nuclear attractions
Ionization Energy 500
Name one technological application that
depends on overcoming the ionization
energy.
Geiger counters, smoke detectors,
cathode ray tubes and/or solar cells.
Electronegativity 100
Electronegativity refers to how tight an
atom holds _____ electrons in a covalent
bond.
shared
Electronegativity 200
The element which shows the greatest
electronegativity in the periodic table is
_____.
fluorine
Electronegativity 300
In which direction does electronegativity
decrease?
down
Electronegativity 400
As you move down the periodic table the
ionization energy gets weaker because
there is more interior shielding and the
_____ to the nucleus is greater.
distance
Electronegativity 500
In a molecule of water, H2O, which atom
would hold the electrons more tightly due to
higher electronegativity?
oxygen
FINAL JEOPARDY!
Who organized the then known elements in
horizontal patterns of atomic mass versus
vertical patterns of similar properties and
thereby accurately predicted the existence
and properties of yet undiscovered elements?
Dmitri Mendeleev