Honors Chemistry
On test day please bring:
Chapter Seven:
Test Date: . pencil
eraser
scientific calculator 
Development of the Periodic Table o Dimitri Mendeleev – how did he organized the elements? o Henry Moseley – how did he organize the elements?
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Effective Nuclear Charge o Definition & trend across a period o What does the effective nuclear charge depend upon?
 Hint: 2 factors that affect attraction between nucleus and electrons in an atom o Z eff is responsible for all the trends as you move across a period (left to right)
 For example… the reason why atomic radius decreases across a period is because the effective nuclear charge of the atom increases resulting in a greater attraction between the nucleus & the electrons. This pulls the electrons in closer to the nucleus resulting in a smaller atomic radius (This same logic can be manipulated for ALL of the periodic trends)
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What is responsible for trends as you move down a column?
o Trends down a column are primarily based upon the fact that down a column Z eff does not change much but a whole additional energy level (and many inner core electrons) has been added to the atom
 For example: Ionization energy decreases down a column because with the addition of another energy level and many more inner core electrons the atoms is much bigger.
This means the valence electrons are further away from the nucleus and they are less attracted to the nucleus due to all the inner core electrons. This makes the removal of an electron much easier resulting in a lower ionization energy as you move down a column. (This same logic can be manipulated for ALL of the periodic trends)
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Atomic Radii o Definition o Trends (across a period & down a column) o Ranking elements in order of increasing or decreasing atomic radii size o Hint elements: Francium (largest) and Fluorine (smallest)
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Ionic Radii o Definition o Trends – if comparing all anions or all cations the trend follows that of atomic radius o Comparing cations to their parents and anions to their parents o Ranking elements in order of increasing or decreasing ionic radii size
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Ionization Energy o Definition o Trends(across a period & down a column)

o Hint Families – Noble Gases (highest) and Alkali Metals (lowest) o Know about successive ionization energies (1 st , 2 nd , 3 rd , 4 th , etc.)
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Isoelectronic o Know what this means and be able to write and/or recognize isoelectronic series
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Electron Configurations of Ions o Be able to write electron configurations for ions such as Ca 2+ of N 3etc…
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Electron Affinity and Electronegativity o Definitions – know both terms and the difference between the two o How does electron affinity relate to ionization energy?
o Trends (across a period & down a column) o Why are negative energy values for electron affinity favorable and positive EA values are unfavorable?
o What family has the lowest electron affinity? Why?
o Which family has the highest electron affinity? Why?
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Metals, Nonmetals, Metalloids o Properties of each – lustrous, conductive, malleable, brittle, melting points (high or low), etc… o Which are most likely to form cations? Anions?
o Within the alkali and alkali earth families, what is the trend of reactivity?
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Ions o How is an ion different from an atom?
o What is a cation? Anion?
o How is a cation formed? How is an anion formed?
o Know the number of valence electrons in an elements (1-8 valence electrons possible) o Know the charge that an ion will have (what ion would Na become? P? Al?, etc) o Be able to determine the number of electron in an ion vs. and atom of the same element
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Key Terms: o Cation, anion, valence e , inner core e , e shielding, malleable, ductile, conductor