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Periodic TrendsLearning Target:• I can use the Periodic Table to identify and explain periodic trends,
including atomic and ionic radii, electronegativity, and ionization energy.
Criteria For Success:• I can explain effective nuclear charge and electron shielding.• I can explain how increasing effective nuclear charge across a period
influences the atomic radius, electronegativity and ionization energy.• I can explain how increased electron shielding down a group
influences atomic radius, electronegativity and ionization energy.• I can explain the trend of ionic radius and how the magnitude and
the sign of the ionic charge influences ionic radius
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Periodic TrendsA. Attraction between the nucleus and electrons• 1. Coulomb’s law- the force of
attraction between two oppositely charged particles is directly proportional to the magnitude of the charges and inversely proportional to the distance between those charges.
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Periodic TrendsCoulomb’s Law
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Periodic Trends2. Effective nuclear charge (Zeff)- the net nuclear pull experienced by the valence electrons in an atom.
a. Zeff = # protons - # core (non-valence) electrons
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Periodic Trends
http://inntrending.com/effective-nuclear-charge-trends/
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Periodic Trends
http://inntrending.com/effective-nuclear-charge-trends/
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Periodic Trends3. Electron shielding- the inner electrons shield the outer electrons from some of the nucleus’ attractive force.• a. Going down a group adds another
principle energy level adds more shielding.
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Periodic Trends
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Periodic Trendsb. Adding another energy level also increases the distance between the outer electrons and the nucleus which decreases the force- Coulomb’s Law!
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Periodic Trends
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Periodic Trends• B. Periodic trends are patterns
in the periodic table relating to the size and other properties of elements.
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Periodic Trends1.ATOMIC RADIUS is the
distance between the nucleus and the outer edge of the electron cloud.
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Periodic Trends
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Periodic Trends
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Periodic Trends
2.IONIZATION ENERGY is the energy required to remove an electron from the atom.
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Periodic Trendsa) Each additional electron requires
MORE energy to remove than the previous one, so the second ionization energy will be greater than the first ionization energy, and so on.
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Periodic Trends
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Periodic Trends
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Periodic Trendsb. EXCEPTIONS!!!
O vs. N- It’s easier to remove an electron from O because of the repulsion of the paired electrons.
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Periodic Trendsb. EXCEPTIONS!!!
Be vs. B- It’s easier to remove an electron from B because it’s a p electron vs. an s electron and electrons in p orbitals are held less tightly.
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Periodic Trends3. ELECTRONEGATIVITY is the ability of
an atom in a molecule [meaning it’s participating in a bond] to attract shared electrons to itself.a. Think of the atoms as playing “tug
of war” with their outer shell electrons.
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Periodic Trends
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Periodic Trends
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Periodic Trends4.IONIC RADIUS is the distance
from the nucleus to the outer edge of the electron cloud in a charged ion.
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Periodic Trendsa. Cation- the atom LOST electron(s),
has a positive chargeb. Anion- the atom GAINED
electron(s), has a negative chargec. All atoms want a full valence shell,
and will gain/lose electrons to get there.
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Periodic TrendsCharges of Ions
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Periodic Trends
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Periodic TrendsC. Periodic trends can be justified by using one of the following generalizations:
1. Use Z eff to explain trends across a period.2. Use electron shielding (increased energy
levels, increased distance) to explain trends down a group.