Periodic Trends Density Atomic and Ionic Radii
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Transcript of Periodic Trends Density Atomic and Ionic Radii
Chapter 10Periodic Trends
DensityAtomic 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?
The Nuclear Charge (Z)Carbon Nitrogen
The greater the number of protons in the nucleus the greater the effective nuclear charge.
Conclusion: Nitrogen is a smaller atom than carbon because nitrogen has 7 protons to pull in its two levels of electrons whereas
carbon only has 6 protons holding it’s two levels of electrons.
Carbon Nitrogen
For atoms with the same number of energy levels the greater the number of protons in the nucleus the greater the effective nuclear charge.
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).
Atomic Radius
Xylophone monkey
Nuclear charge explains why atoms get smaller across a period
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?
HeNe
Conclusion: Neon is larger than helium because it has an increased shielding effect from having two energy levels whereas helium only has one energy level.
HeNe
Atomic Radius
Xylophone monkey
Shielding Effect explains why atoms get larger down a group
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?
• Most reactive nonmetal is?
Fr
F
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 + < O2- < N3-
Homework
• Worksheet: Density, Atomic and Ionic Radii