Download Periodic trends - poynette.k12.wi.us

Name: ___________________________
Periodic Trends
Define the following:
Nuclear charge –
Outermost orbital –
Shielding effect Atomic Radius
Prepare a graph of atomic radius (R) vs. atomic number using the data below.
1. What is a picometer (pm)?
2. Define atomic radius.
3. What general trend occurs in atomic radii as you move across a period? Down a
group?
4. Give an explanation for these trends.
5. What group of elements seems to defy this trend?
6. What is the range in atomic radii (smallest to largest)?
Ionization Energy
Prepare a graph of first, second, and third ionization energy vs. atomic number.
1. What is a kJ/mol?
2. Define ionization energy.
3. Why are second and third ionization energies higher than first ionization
energies?
Name: ___________________________
Periodic Trends
4. Why doesn’t helium have a third ionization energy?
5.
What general trend occurs in ionization energies as you move across a period?
Down a group?
6. Give and explanation for these trends.
7. Why are the ionization energies for the alkaline earth metals relatively high?
Electronegativity
Prepare a graph of electronegativity vs. atomic number
1. Define electronegativity.
2. What is the range in electronegativity (smallest to largest)? Which element has
the highest ionization energy?
3.
What general trend occurs in electronegativity as you move across a period?
Down a group?
4. Elements in which part of the periodic table tend to have the highest
electronegativities? The lowest?
Ionic Radii
Prepare a bar graph of atomic radii compared to ionic radii.
1. Metals __________________ electrons, nonmetals ____________________
electrons.
2. Positive ions are called ___________________, negative ions are called
_________________.
3. How do the size of positive ions compare to the neutral atom? How do the size of
negative ions compare to the neutral atom?
4. Why are the noble gases not included?