Honors Chemistry – Atomic Structure / Periodic Table Test
Practice Problems -- Answers
1. 1s22s22p63s2 (longhand), [Ne] 3s2 (core notation), for box/arrow notation be sure you have 12 arrows, all boxes should have pairs
2. P=55, N=78, e=55
3. P=55, N=82
4. conductor=any metal, semiconductor=any metalloid, and insulator=any non-metal solid
of definite composition:
compounds will always contain the same elements
in the same proportions
Law of conservation of mass: mass cannot be created or destroyed in a closed system
6. Bohr stated that electrons reside in definite energy levels, like rungs on a ladder
10. Noble gases are extremely unreactive because their valence electron levels (s & p) are filled
12. ionization energy:
the energy required to remove an electron. Increases
toward right and top.
Higher at top because they are closer and less
shielding. Higher to the right because of greater pull from the nucleus.
electronegativity: -- tendency to attract electrons during bonding. Follows same trend as electron affinity. Generally are more negative from left to right because of nuclear charge, atomic radius, and shielding effect. Generally decreases from top to bottom because of nuclear charge, atomic radius, and shielding effect.
13. Each element has a different electron configuration and gives off different wavelengths of light when their electrons are excited and then drop to lower energy levels.