Post on 16-Jan-2016
transcript
Periodic Jeopardy
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Group Properties
Electron Configurati
ons
Atomic Radii
Ionization Energy
Electronegativity
FINAL
Group Properties 100Group Properties 100
What group of elements forms no charges, or bonds due to stable s2p6
octets of valence electrons?
Noble Gases
Group Properties 200Group 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 300Group 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 400Group 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 500Group 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 100Electron Configurations 100
s2p4
What are the common valence electrons of elements in the Oxygen group?
Electron Configurations 200Electron Configurations 200
What is the kernel of the electron configuration for zinc?
[Ar]
Electron Configuations 300Electron Configuations 300
What element has the following abbreviated electron configuration?
[Kr]5s24d105p5
Iodine
Electron Configurations 400Electron 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 500Electron 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 100Atomic Radii 100
Which direction do atomic radii increase in the periodic table?
Downward
Atomic Radii 200Atomic Radii 200
The “Size Surprise” is that atomic radii decrease as you move _____ in the periodic
table.
Right
Atomic radii increase down the periodic table due to additional
_____ _____.
Atomic Radii 300Atomic Radii 300
Energy Levels
Atomic Radii 400Atomic 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 500Atomic 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 100Ionization Energy 100
Ionization energy refers to the energy required to _____ an electron from an atom.
remove
Ionization Energy 200Ionization Energy 200
Ionization energy _____ as you move right across the periodic table
increases
DAILY DOUBLE – Ionization Energy
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 400Ionization Energy 400
As you move right across the periodic table, the ionization energy gets higher because the
_____ _____ get stronger.
Nuclear attractions
Ionization Energy 500Ionization 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 100Electronegativity 100
Electronegativity refers to how tight an atom holds _____ electrons in a covalent
bond.
shared
Electronegativity 200Electronegativity 200
The element which shows the greatest electronegativity in the periodic table is
_____.
fluorine
Electronegativity 300Electronegativity 300
In which direction does electronegativity decrease?
down
Electronegativity 400Electronegativity 400
distance
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.
Electronegativity 500Electronegativity 500
In a molecule of water, H2O, which atom would hold the electrons more tightly due to
higher electronegativity?
oxygen
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
FINAL JEOPARDY!FINAL JEOPARDY!