Chemistry 11
Paul Lee, Sally Kim
Block : D
ANALYSIS QUESTIONS
Based on your graphs, what is the trend in atomic radius across aperiod? Down a family?
Atomic radius decreases across a period and decreases down a family
Based on your graphs, what is the trend in ionization energy across a period? Down a family?
Ionization energy increases across a period and decreases down a family
Based on your graphs, what is the trend in electronegativity across a period? Down a family?
Electronegativity increases across a period and decreases down a family
*Atomic radius decreases, Ionization energy and electronegativity increases
# valence e: 1 2 2 for all transition metals 3 4 5 6 7 8
Ion charge: +1 +2 +2 for most of the transition metals +3 +4 -3 -2 -1 0*
4. a) What is happening to the number of protonsand the number of energy levels as you move across the periodic table from left to right? How and why does this affect atomic radius.
As you move across the periodic table, the number of the protons stays the same and the number of the electron increases. This affects the atomic radius because if the number of energy level changes, the the atom will become bigger or smaller, which will directly affect the atomic radius
b) What happens to the number of energy levels as you move down a column on the periodic table. How and why does this effect ionization energy?
As you move down a column of the periodic table, the number of energy levels increases as the number of electrons increase. This effects ionization energy becuase as the number of energy level changes the energy that is required to gain or lose an electron changes to become an ion.
c) What happens to the effective nuclear charge as you move across a period on the periodic table? How does this effect ionization energy and electronegativity
Effective nuclear charge increases as you move across a period. Since the energy that holds the valence electrons increases, the ionisation energy and electronegativity will increase because it becomes more hard to gain an electron.
5. a) Which group contains elements which are easiest to ionize? Explain why this is the case.
Alkali metal. It is located on the left side. There is more space between the electron and the nucleus since the atomic radius is the larger than any other groups, so you need less ionization energy, so it is easiest to ionize.
b) Explain why the third ionization energy of Calcium would be much higher than the 1st and 2nd ionization energy.
The third ionization energy of Calciumwould be much higher than the 
6. Which element would have the highest electronegativity in each set below? Explain why this is.
a)Ca, Be or Mg b) B, Li, or F
a) Be. Beryllium would have the highest electronegativity because electronegativity decreases as it goes down the group.
b) F. Flourine would have the highest electronegativity because electromegativity increases across the period.
7. Compare the graphs for ionic and atomic radii. In general, what happens to metals when they form an ion? What happens to nonmetals when they form an ion?
When metals form an ion, atoms of metal loses electron(s), in their highest energy level and become positively charged ions. Non-metal atoms gain electron(s), from another atom to become negatively charged ions.
8. Write the electron configuration each atom (high-light the valence electrons) and it’s corresponding ion below each sketch (atomic radii are given in angstroms (1 x 10-10 M as opposed to picometers used in yourgraph data: 1 x 10-12 M)
9. In the blank periodic table provides write the number of valence electrons and the expected charge of the ions for the transition metal block and for the families to the left and right of the transitions metals (the alkali metals have been done as an example).
Note: Carbon and boron do not normally form ions and are thus blanked-out