Unit 3 STUDY GUIDE
(section 3.3 and chapter 4 in textbook)
Vocab
Ch.3:
orbital,
electromagnetic spectrum,
ROYGBIV,
line-emission spectrum,
visible light,
excited state,
ground state,
energy level,
sublevel,
orbital,
electron spin,
Pauli exclusion principle,
electron configuration,
aufbau principle,
Hund’s rule
Ch.4:
John Newland,
law of octaves,
Dmitri Mendeleev,
periodic law,
valance electrons,
group/ family,
period/ series,
metal,
nonmetal,
metalloid/semimetal/semiconductor,
alkali metal,
alkaline earth metal,
transition element,
rare earth element,
lanthanide,
actinide,
s-block,
p-block,
d-block,
f-block,
halogens,
noble gases,
chalcogen,
pnicogen,
ionization energy,
atomic (bond) radius,
ionic radius,
electronegativity
Radiant Energy
The electromagnetic spectrum
What is on it? What does the order represent? What is the order?
What are the different types we talked about?
What makes each type unique?
What happens to the electrons in the atoms to explain what we see?
Describe the relationship of frequency, wavelength and energy
Quantum Theory
Light & matter act as both particles and waves
What is a quantum? A photon?
How does a continuous spectrum compare to a line spectrum? How is each
produced?
How does Bohr’s model of the atom compare to today’s model?
What predictions were made using the Bohr model?
What was wrong with Bohr’s model?
The Quantum Mechanical Model
What are orbitals?
What are the different types of orbitals we discussed?
What are the shapes of various orbitals?
How many electrons can each orbital hold? Each energy level?
What do we know about electron spin and magnetism?
What’s an energy level, sublevel and orbital? How are they related/different?
Electron Configurations
Can you write electron configurations using only the periodic table?
What are the three rules that govern how electrons fill the orbitals?
What do Aufbau or orbital diagrams look like?
How can you predict magnetism from electron configurations?
What are the exceptions?
Concepts
Know who the key people (Newlands, Mendeleev, Meyer, Mosley) were who
contributed to the development of the periodic table and what they did. And
whether or not their ideas are still used today
Know the three different group naming systems
Know how to identify an element in a particular period and group
Know the trends for atoms and ions in groups and periods. Be able to compare
elements within a group or period. Describe what causes the trend based on the 3
factors we discussed in class (energy levels, nuclear charge, & shielding effect.)
Know how to write an electron configuration using only the periodic table, also be
able to write the abbreviated version.
Know how to use the periodic table to determine the number of valence electrons
in an element and write a Lewis dot diagram
Know the four different trends ( atomic radius, ionic radius, ionization energy, &
electronegativity) and be able to compare them across and down the periodic table
as well as interpret and extrapolate data from a graph. Be able to explain why
each trend is the way that it is.
Format ( at least 60 points)
~20 multiple choice
~ 10 multi-part short answer
Lab practical question
(Study your notes, homework and lab activities.)
STUDY TIP #1:
Try to make-up questions that combine several different concepts and then answer them.
STUDY TIP #2:
Try to think of the hardest questions, the teacher might ask you. Figure out the answers.
The better you get at this the easier and easier tests become. Your ability to do this will
improve over time if you continue to try to do it.