Download Unit 2 Atomic Structure Study Guide

Unit 2 Atomic Structure Study Guide
Know and Define the following rules and principles:
1. The Law of Definite Proportions
2. Hund’s Rule
3. The Aufbau Principle
4. The Pauli Exclusion Principle
5. The Law of Conservation of Energy
Know the following Scientist and there theories:
• What did they use in their experiment
• What did they discover? (ie protons, neutrons, electrons,
etc)
1. Dalton
2. Rutherford
3. Bohr
4. Chadwick
5. Thompson
Atoms, Ions, Isotopes
1. Define Ions
2. Define Isotopes
3. Protons
4. Electrons
5. Neutrons
6. Nucleus
7. Which two particles have the same mass?
8. What particles make up the nucleus?
9. What particles are NOT in the nucleus?
10.What particles make up the atomic mass?
11.What particles have insignificant mass, but take up most of
the space of an atom?
12.Atoms of the same element but have a different mass are
_______________ ?
13.Atoms of the same element but have a charge are
___________________ ?
14.Example Problems
a. An isotope written O has how many….
Protons:
Electrons:
Neutrons:
b. An ion written O has how many…
Protons:
Electrons:
15.The two ways of writing an isotope. Know what each
number/symbol represents
a. Ex Carbon-14
16.b.
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: Carbon12 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. What are they?
2. What two orbitals make up the valence electrons
3. What group do all atoms want to be?
4. Using number 3, how many valence electrons do all atoms
want to have?
5. 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
17
8
2-
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
3. Dimensional Analysis
4. Linear Equations
Example Problems: