1. Unit 2: Atomic Structure and the Periodic Table
Periodic Table Trends

2. The Periodic Table
group: columns
period:
rows

3. Metals and Nonmetals
Metals
Nonmetals

4. Groups of the Periodic Table
Alkali metals
Noble gases
Alkaline earth metals
(Group 2 Metals)
Halogens
Transition Metals

5. Atomic Radius
Atomic radius:
the size of an atom

6. DECREASES due to fewer electron energy levels
Atomic Radius
DECREASES due to more protons (increased effective nuclear charge)
DECREASES due to fewer electron energy levels

7. Ionization Energy Ionization energy:
The energy required to remove the outermost (highest energy) electron from a neutral atom in its ground state.

8. Ionization Energy
INCREASES – smaller atom means electrons are closer to the nucleus, thus harder to remove
INCREASES – electrons are closer to the nucleus and there is less shielding

9. Electronegativity Electronegativity:
ability of an atom in a molecule (covalent bond) to attract electrons

10. INCREASES – due to more protons (increased effective nuclear charge)
Electronegativity
INCREASES – due to more protons (increased effective nuclear charge)
INCREASES – due to fewer electron energy levels (increased effective nuclear charge)

11. Periodic Table Trends Assignment
ATOMIC RADIUS
read p
do p. 288: 7.4, 7.23
IONIZATION ENERGY
read p
do p. 290: 7.41 (skip a), 7.43, 7.45
ELECTRONEGATIVITY
read p. 308
do p. 334: 8.36, 8.37