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Unit 2 Atomic Structure Study Guide
Know and Define the following rules and principles:
1.
2.
3.
4.
5.
The Law of Definite Proportions
Hund’s Rule
The Aufbau Principle
The Pauli Exclusion Principle
The Law of Conservation of Energy
Know the following Scientist and there theories:


1.
2.
3.
4.
5.
What did they use in their experiment
What did they discover? (ie protons, neutrons, electrons, etc)
Dalton
Rutherford
Bohr
Chadwick
Thompson
Atoms, Ions, Isotopes
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
Define Ions
Define Isotopes
Protons
Electrons
Neutrons
Nucleus
Which two particles have the same mass?
What particles make up the nucleus?
What particles are NOT in the nucleus?
What particles make up the atomic mass?
What particles have insignificant mass, but take up most of the space of an atom?
Atoms of the same element but have a different mass are _______________ ?
Atoms of the same element but have a charge are ___________________ ?
Example Problems
a. An isotope written 178O has how many….
Protons:
Electrons:
Neutrons:
b. An ion written O2- has how many…
Protons:
Electrons:
15. The two ways of writing an isotope. Know what each number/symbol represents
a. Ex Carbon-14
Unit 2 Atomic Structure Study Guide
b. 146𝐶
16. What is an anion? Which particles does it have more of: electrons or protons?
17. What is a cation? Which particles does it have more of: electrons or protons?
Average Atomic Mass
1. How do you calculate the average atomic mass of an element?
2. Example: The Carbon atom has three isotopes: Carbon-12 at 98.2%, Carbon-13 at 1.2%, and
Carbon-14 at 0.6%. What is the average atomic mass of Carbon?
Valence Electrons
1.
2.
3.
4.
5.
What are they?
What two orbitals make up the valence electrons
What group do all atoms want to be?
Using number 3, how many valence electrons do all atoms want to have?
What do atoms form to have this number of valence electrons/
Electrons Configuration
1. What are the 4 main orbitals types that exist and how many types (shapes) does each have?
a.
b.
c.
2. How many electrons can each type (shape) have?
3. So after answering #2, what is the maximum number of electrons that can each of the main
orbitals have?
a.
b.
c.
d.
4. What is the “complete” electron configuration of Oxygen?
5. What is the “complete” orbital notation of Oxygen?
6. What is the “complete” electron configuration of Oxygen ion (Oxide)?
7. What is the noble gas (shorthand) configuration of Oxygen?
8. What is the noble gas (shorthand) orbital notation of Oxygen?
9. What is the excited state?
10. What do atoms “give off” when they are in an excited state?
11. What is the ground state?
Past Topics to be covered on this test:
1. SigFigs
2. Temperature Conversion from Celsius to Kelvin
Unit 2 Atomic Structure Study Guide
3. Dimensional Analysis
4. Linear Equations
Example Problems:
Unit 2 Atomic Structure Study Guide
Unit 2 Atomic Structure Study Guide