November 07, 2014 Periodic Trends Remember from the "Periodic Table" Notes... • The periodic table is a tabular display of the chemical elements, organized by their atomic number, electron configuration, and recurring properties. • Periodic law: There is a periodic repetition of chemical and physical properties of the elements when they are arranged by increasing atomic number
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November 07, 2014
Periodic TrendsRemember from the "Periodic Table" Notes...• The periodic table is a tabular display of the chemical
elements, organized by their atomic number, electron configuration, and recurring properties.
• Periodic law: There is a periodic repetition of chemical and physical properties of the elements when they are arranged by increasing atomic number
November 07, 2014
Atomic Radius Graph
• What are some initial observations about the atomic radius data/graph?
• What is atomic radius?
November 07, 2014
Go finish the rest of the worksheet with your group! You have 20 minutes.
November 07, 2014
Atomic Radius Trend Discussion
• What happens to atomic radius as you go across the period? Why?
• What happens to atomic radius as you go down the group? Why?
November 07, 2014
Periodic Trends Notes
Get your handout out!
November 07, 2014
Why is it called a periodic table?
• The properties of the elements in the table repeat in a "periodic" way (specific pattern).
• Periodic law: There is a periodic repetition of chemical and physical properties of the elements when they are arranged by increasing atomic number
• The modern periodic table is arranged by > atomic number = # of protons> properties> electron configuration
November 07, 2014
Alkali Metals Halogens
Periodic Law
• Now lets look at some properties of elements> We looked at some of these in "Meet My Family"!
November 07, 2014
Periodic Trends
• Chemical properties of elements are determined by their electron configuration.
• Properties are periodic because the number of valence electrons is periodic.
November 07, 2014
Electron Configuration and the Periodic Table
• Remember electrons are found in atomic orbitals> Principle energy level (n, shells) tells us the
relative size and energy of atomic orbitals.> Each shell can hold a certain number of electrons.> # of e- = # of p+ for a neutral atom> Valence electrons = electrons in outermost shell
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November 07, 2014
Electron Configuration and the Periodic Table
• If we draw these orbital diagrams for H, He, Li, Be Na, Mg,
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November 07, 2014
Electron Configuration and the Periodic Table
• Periods: Period equals the highest principle energy level of electrons (shell of the valence electrons)
• Groups: Elements in the same group have the same number of valence electrons
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Now lets look at two trends
1. Atomic radius
2. Ionization energy
November 07, 2014
1. Atomic RadiusThe electron cloud surrounding a nucleus is based on probability and does not have a clearly defined edge.• Atomic radius: half the distance between nuclei of
adjacent identical atoms> Adjacent nuclei in a crystal> Nuclei of two atoms bonded together
• Atomic radius is determined by the strength of attraction between the valence electrons and the nucleus> # of protons in nucleus> # of shielding electrons that "block" protons from
valence electrons
November 07, 2014
Atomic Radius Trend
• What happens to atomic radius as you go across the period?
• What happens to atomic radius as you go down the group?
Example 1: Order the following atoms from smallest to biggest atomic radius:
Ga, Se, K
I, F, Cl
November 07, 2014
2. Ionization Energy
• Ionization energy = energy required to remove an electron from a gaseous atom. (kJ/mol)
When you remove an electron from an atom, what do you get?
November 07, 2014
Na Na+ + e- H=495.8 kJ/mol
Mg Mg+ + e- H=737.7 kJ/mol
Mg+ Mg2+ + e- H=1450.6 kJ/mol
Ionization energy
• Ionization energy is an indication of how strongly an atom's nucleus holds onto its valence electrons> Greater IE = harder to ionize
• Ionization energy is always a positive value• You can take off more than one electron!
> IE1 (1st ionization energy) = energy required to remove 1st valence e-
> IE2 (2nd ionization energy) = energy required to remove a 2nd e-
November 07, 2014
Ionization Energy
• Is an atom with a high ionization energy more likely or less likely to form a positive ion?
• What about one with low ionization energy?
What is the periodic trend for ionization energy?
What factors affect ionization energy?
November 07, 2014
Ionization Energy
What pattern do you see?
November 07, 2014
Ionization Energy
• Moving down a group: IE decreases > There are more electrons in between the nucleus
and the valence electrons (shielding effect)> Electrons are not as tightly bound to nucleus.> Electrons are further away, attraction decreases.
• Moving across a period: IE increases > Increased nuclear charge (more p+, greater
attractive force)
November 07, 2014
Ionization Energy
• What about successive IE (removing more than one e-)?> Successive IE increases
• There is a big "jump" in some IE required. Why?> W/in a sublevel: small increases> Between sublevels: greater increase> Between energy levels: greatest increase