1. 1 Periodic Trend of Ionic Charges 18
2 13 14 15 16 17
3 4 5 6 7 8 9 10 11 12
+1
+/- 4
tend to have
+2
-2
+3
-1
-3
more than one option
+3
+ 3 or + 4
2. Trends when atoms form Ions
Empirical Observation
“when forming ions, elements tend to lose or gain
electrons to be more like the nearest noble gas”
3. Trends when atoms form Ions
Empirical Observation
“when forming ions, elements tend to lose or gain
electrons to be more like the nearest noble gas”
Metals tend to lose e-’s
4. Trends when atoms form Ions
Empirical Observation
“when forming ions, elements tend to lose or gain
electrons to be more like the nearest noble gas”
Metals tend to lose e-’s
Nonmetals tend to gain e-’s
6. Atomic Radius
Definition: Half the distance
across a neutral atom
Radius decreases across a period
7. Atomic Radius
Definition: Half the distance
across a neutral atom
Radius decreases across a period
The electrons are pulled in tighter as the # of
protons increases
8. Atomic Radius
Definition: Half the distance
across a neutral atom
Radius decreases across a period
The electrons are pulled in tighter as the # of
protons increases
Radius increases down a group
9. Atomic Radius
Definition: Half the distance
across a neutral atom
Radius decreases across a period
The electrons are pulled in tighter as the # of
protons increases
Radius increases down a group
Each row on the periodic table adds a “shell” or
energy level to the atom. This makes atoms larger
with each added shell, just like an onion
12. Ionic Radius Definition: Half the distance across an Ion
Cations
Anions
13. Ionic Radius Definition: Half the distance across an Ion
Positively charged ions formed when
Cations an atom of a metal loses one or
more electrons
Anions
14. Ionic Radius Definition: Half the distance across an Ion
Positively charged ions formed when
Cations an atom of a metal loses one or
more electrons
Smaller than the neutral atom
Anions
15. Ionic Radius Definition: Half the distance across an Ion
Positively charged ions formed when
Cations an atom of a metal loses one or
more electrons
Smaller than the neutral atom
Negatively charged ions formed
when nonmetal atoms gain one
Anions
or more electrons
16. Ionic Radius Definition: Half the distance across an Ion
Positively charged ions formed when
Cations an atom of a metal loses one or
more electrons
Smaller than the neutral atom
Negatively charged ions formed
when nonmetal atoms gain one
Anions
or more electrons
Larger than the neutral atom
21. Trends in Atomic and Ionic Size
Metals
Group 1
Li
152
Na
186
K
227
22. Trends in Atomic and Ionic Size
Metals
Group 1
e
Li
152
Na
186
K
227
23. Trends in Atomic and Ionic Size
Metals
Group 1
e
Li Li+
152 60
Na
186
K
227
24. Trends in Atomic and Ionic Size
Metals
Group 1
e
Li Li+
152 60
e
Na
186
K
227
25. Trends in Atomic and Ionic Size
Metals
Group 1
e
Li Li+
152 60
e
Na+
Na
95
186
K
227
26. Trends in Atomic and Ionic Size
Metals
Group 1
e
Li Li+
152 60
e
Na+
Na
95
186
e
K
227
27. Trends in Atomic and Ionic Size
Metals
Group 1
e
Li Li+
152 60
e
Na+
Na
95
186
e
K+
K
133
227
28. Trends in Atomic and Ionic Size
Metals
Group 1 Group 13
e
Li Li+
152 60
e
e e
e
Na+ Al3+
Na Al
95 143 50
186
e
K+
K
133
227
29. Trends in Atomic and Ionic Size
Metals
Group 1 Group 13
e
Li Li+
152 60
e
e e
e
Na+ Al3+
Na Al
95 143 50
186
e
K+
K
133
227
Cations are smaller than parent atoms
30. Trends in Atomic and Ionic Size
Metals Nonmetals
Group 1 Group 13
e
Li Li+
152 60
e
e e
e
Na+ Al3+
Na Al
95 143 50
186
e
K+
K
133
227
Cations are smaller than parent atoms
31. Trends in Atomic and Ionic Size
Metals Nonmetals
Group 1 Group 13 Group 17
e
Li Li+
152 60
e
e e
e
Na+ Al3+
Na Al
95 143 50
186
e
K+
K
133
227
Cations are smaller than parent atoms
32. Trends in Atomic and Ionic Size
Metals Nonmetals
Group 1 Group 13 Group 17
e
Li Li+
F
152 60 64
e
e e
e
Na+ Al3+
Na Al Cl
95 143 50 99
186
e
K+
K Br
114
133
227
Cations are smaller than parent atoms
33. Trends in Atomic and Ionic Size
Metals Nonmetals
Group 1 Group 13 Group 17
e
e
Li Li+
F F-
152 60 64
e 136
e e
e
Na+ Al3+
Na Al Cl
95 143 50 99
186
e
K+
K Br
114
133
227
Cations are smaller than parent atoms
34. Trends in Atomic and Ionic Size
Metals Nonmetals
Group 1 Group 13 Group 17
e
e
Li Li+
F F-
152 60 64
e 136
e e e
e
Na+ Al3+
Na Al Cl Cl-
95 143 50 99
186 181
e
K+
K Br
114
133
227
Cations are smaller than parent atoms
35. Trends in Atomic and Ionic Size
Metals Nonmetals
Group 1 Group 13 Group 17
e
e
Li Li+
F F-
152 60 64
e 136
e e e
e
Na+ Al3+
Na Al Cl Cl-
95 143 50 99
186 181
e e
K+
K Br Br-
114
133 195
227
Cations are smaller than parent atoms
36. Trends in Atomic and Ionic Size
Metals Nonmetals
Group 1 Group 13 Group 17
e
e
Li Li+
F F-
152 60 64
e 136
e e e
e
Na+ Al3+
Na Al Cl Cl-
95 143 50 99
186 181
e e
K+
K Br Br-
114
133 195
227
Cations are smaller than parent atoms Anions are larger than parent atoms
39. Periodic Properties
• How does the size of an atom change
when electrons are added or
removed?
As an Atom loses
1 or more electrons
(becomes positive),
it loses an orbit or
energy level and
therefore, its radius
decreases.
41. Periodic Properties
• How does the size of an atom change
when electrons are added or
removed?
As an Atom gains
1 or more electrons
(negative), it fills its
outermost energy
level, therefore, its
radius increases.
42.
43. Electron Shielding
CORE electrons are
closer to the nucleus
and therefore have a
stronger attraction to
the positive nucleus.
This “shields”
valence electrons
from feeling as
strong of a pull from
the positive nucleus.
45. Effective Nuclear Charge
• In atoms with many
electrons, electrons are
both attracted to the
nucleus and repelled by
other electrons.
46. Effective Nuclear Charge
• In atoms with many
electrons, electrons are
both attracted to the
nucleus and repelled by
other electrons.
• Opposite charges attract.
Like charges repel.
47. Effective Nuclear Charge
• In atoms with many
electrons, electrons are
both attracted to the
nucleus and repelled by
other electrons.
• Opposite charges attract.
Like charges repel.
• The nuclear charge that
an electron experiences
depends on how close it
is to the nucleus and how
many other electrons are
around it.
53. Electronegativity
Definition: The ability of an atom to attract or hold
onto electrons
o Electronegativity INCREASES across a
period
o WHY? As the atomic radius decreases,
electrons get closer to the atom’s nucleus
54. Electronegativity
Definition: The ability of an atom to attract or hold
onto electrons
o Electronegativity INCREASES across a
period
o WHY? As the atomic radius decreases,
electrons get closer to the atom’s nucleus
o Electronegativity tends to DECREASE
down a group
55. Electronegativity
Definition: The ability of an atom to attract or hold
onto electrons
o Electronegativity INCREASES across a
period
o WHY? As the atomic radius decreases,
electrons get closer to the atom’s nucleus
o Electronegativity tends to DECREASE
down a group
o WHY? As the atomic radius increases,
electrons are farther from the atom’s
nucleus
59. Ionization Energy
• Amount of energy required to
remove an electron from an atom.
First ionization energy is that
energy required to remove first
electron.
60. Ionization Energy
• Amount of energy required to
remove an electron from an atom.
First ionization energy is that
energy required to remove first
electron.
Second ionization energy is that
energy required to remove second
electron, etc.
62. Trends in First Ionization Energies
• Down a GROUP,
ionization energy
decreases
• For atoms in the same
group, Zeff is essentially
the same, but the valence
electrons are farther from
the nucleus.
• Across a PERIOD,
ionization energy
increases
