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Chapter 10
Periodic Trends
Density
Atomic and Ionic Radii
Density
Density
• Iridium (Z = 77) has the highest density.
• Why not Meitnerium (Z = 109?)
• We can predict that an element is more
dense if it is closer to Iridium.
Density
Effective Nuclear Charge (Zeff)
• The effective nuclear charge (Zeff) of an
atom is basically how well it is able to hold
on to its most loosely held electron.
Atomic radius (radii)
• The atomic radius is essentially the size
of an atom.
• The largest atom is Francium (Z = 87).
Atomic Radius
Xylophone monkey
Rank the atoms from smallest to largest
Na, K, O, N
O < N < Na < K
Atomic Radius and Effective
Nuclear Charge
• The atomic radius decreases as effective
nuclear charge increases.
Effective Nuclear Charge (Zeff)
•
The effective nuclear charge of an atom
is primarily determined by:
1. The nuclear charge
2. The shielding effect
The Nuclear Charge (Z)
• Example: Carbon vs. Nitrogen
• Which atom would you predict to be
smaller?
The Nuclear Charge (Z)
Carbon
Nitrogen
Both atoms are in the 2nd row (period) of
the periodic table. What does this tell us?
Conclusion: Nitrogen has a greater effective nuclear charge than
carbon because nitrogen has 7 protons to pull in its two energy
levels of whereas carbon only has 6 protons holding it’s two energy
levels. Therefore nitrogen atoms are smaller than carbon atoms.
Nitrogen
Carbon
The Nuclear Charge (Z)
• The size of atoms in the same period
(row) is determined by the nuclear
charge (number of protons in the
nucleus).
Nuclear charge explains why atoms get smaller across a period
Atomic Radius
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Shielding Effect.
• The shielding effect is when electrons
between the nucleus and the outermost
electrons in an atom shield or lessen the
hold of the nucleus on the outermost
electrons.
Shielding Effect.
Why is He smaller than Ne?
He
Ne
Conclusion: Helium has a greater effective nuclear charge
than neon because helium has a lower shielding effect from
having only one energy level whereas helium two.
He
Ne
Shielding Effect explains why atoms get larger down a group
Atomic Radius
Xylophone monkey
Chemical Reactivity
Chemical Reactivity
Chemical Reactivity
• Metals tend to lose electrons when reacting.
– Large metal atoms are more reactive.
• Nonmetals tend to gain electrons when
reacting.
– Small nonmetal atoms are more reactive.
Chemical Reactivity
• Metals
increase in
reactivity left
and down.
• Nonmetals
become more
reactive up
and to the
right.
• Most reactive
metal is? Fr
• Most reactive
nonmetal is?F
Francium
• Francium is the least stable
naturally occurring element with a
half-life of only 22 minutes.
• It has been calculated that there
is at most 30 g of francium in the
Earth's crust at any time.
Ionic Radius
• Ionic Radius is the size of an ion.
Size Change in Ion Formation
Rules for Ionic Radius
• Anions (negative ions) are “always” larger
than cations (positive ions).
• Ionic Radius goes by the same rules as
atomic radius (ions get larger as we move
down and to the left).
• However it is necessary to treat anions
and cations separately. (Anions are
bigger).
Rank the ions from smallest to largest
K+, N3-, Na+, O2-
+
Na
+
<K <
2O
<
3N
Homework
• Worksheet: Density, Atomic and Ionic Radii
(due tomorrow).
• Lab Summary: Reactivity and the Periodic
Table (due Monday).
• Study Guide Chapter 10 (due Tuesday).