Transcript Jeopardy Unit 5 Periodicity

Buckyballs
et al
Molecular
Shapes
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VESPR
Model
Pi and
Sigma
Periodic
Table
Potpourri
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The Atom
Bonding
Reactions
Matter
Math of
Chemistry
Solubility
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Final Jeopardy
Final Jeopardy
Semester 1
Knowledge
Final Jeopardy
Ionic
Polar Covalent
Pure Covalent
X > 1.7
1.7  X  .5
X < .5
Write down the 3 divisions
and numbers that you must
use after you subtract the
Electronegativity numbers
between 2 atoms in a
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Properties of the elements that repeat
consistently across the periods, determined
by electron configuration
What is the definition of
Periodic Properties?
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Amount of pull the valence electrons feel
from protons in the nucleus
What is the effective Nuclear
Charge (Z)?
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Stays the same
The effective nuclear charge
trend for going down a
family…
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Goes up, because protons increase while
shielding electrons stays the same
Going across a period, the
effective nuclear charge...
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Atomic size
What is the size of an atom
called?
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Effective nuclear charge and energy levels
What are factors which affect
the size of an atom and how
they affect it ?
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Increases due to the adding of more energy
levels
Trend of atomic size going
down a family…
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Trend of atomic size going across a period
What Decreases due to energy level
staying the same, while effective
nuclear charge increases (more pull
on valence electrons)?
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Ionization Energy
What is the energy needed
to move an electron?
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The effective nuclear charge and atom size
What are factors which
affect ionization energy
and how they affect it ?
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Trend of ionization energy going down a
family
What decreases (easier to
remove) because size is
bigger, so valence electrons
are further away ?
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Trend of ionization energy going across a
period
What increases (harder to remove)
due to effective nuclear charge
increasing (more pull - more likely
to attract electrons) ?
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Electronegativity
What energy is needed to add
an electron (likeliness to
gain)?
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effective nuclear charge and atom size
What factors which affect
electronegativity and how
they affect it ?
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Decreases.. if size is bigger, less pull from
nucleus
•What is the trend of
electronegativity going down
a family
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Increases due to effective nuclear charge
being greater
Trend of electronegativity
going across a period
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Ionic Size
Size of an ion
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to organize elements in meaningful way
Why was periodic table
developed?
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Mendeleev - increasing molar mass, while
today’s is increasing atomic number
How was Medeleevs scheme
for listing elements different
from that used in the modern
periodic table?
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elements in same group have same number
of valence electrons
What relationship can be seen
between an elements
placement within a group and
its electron configuration?
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Noble gases had not been discovered yet
due to their inactivity
Why did Group 8 not appear
on the Mendeleev periodic
table?
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increasing tendency to form neg ions
therefore use less energy (minus -:
Exothermic
Trend of electron affinity
across left to right
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farther from nucleus therefore uses less
energy to add an electron also shielding can
add electrons
Trend of electron affinity
down top to bottom
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X + e− → X−
Equation electron affinity
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M(g) + hn ® M+ + e-.
Equation for ionization
energy
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both negative ions (right side) give off
energy to gain an electron + ions use energy
Electron affinity energy can
be what: + or -?
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1) shielding 2) Effective (Strong) nuclear
charge 3) add another orbit of electrons
increases distance from nucleus
Name 3 concepts that can
affect periodicity
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Protons and neutrons in element 114
What exactly do these two
pictures represent and where
are the from?
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The equal the levels from the nucleus out.
How do the periods on the
periodic table relate to the
electron orbitals and the
nucleus.
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1s2 2s2 2p6 3s2 3p2 and [Ne] 3s2 3p2
Long and short electron
configuration for silicon.
Daily
Double
Dalton, Thompson, Rutherford and
Bohr…Schrödinger, and Heisenberg
st
1
Name the five scientists in
“The Atom Song
The Jeopardy champion!