Download Electron Configuration, Noble Gas Configuration

NEED MORE EMPHASIS ON ISOTOPES
C4.10c Calculate the average atomic mass of an element given the percent abundance and mass of
the individual isotopes.
C4.10d Predict which isotope will have the greatest abundance given the possible isotopes for an
element and the average atomic mass in the periodic table
C4.10 e Write the symbol for an isotope in nuclear notation
C4.8h
Describe the shape and
orientation of s and p
orbitals.
___ Orbital (S, P, D, F) ___ Noble Gas Configuration
___ WS – Electron and Noble Gas Configurations
___ Activity – Electron Configuration Battleship.
___ Quiz – Electron Configurations
Student Expectations – Changing the Electrons and Neutrons within Atoms
Big Idea / Question(s):
1. What types of changes can occur to atoms without altering the atom’s elemental identity?
2. How do the changes that occur to atoms effect the properties of those atoms?
Overview: In this short unit we will see how the periodic table can be used to deepen our understanding
of atom models. We will see that even atoms of the same element can be different. Isotopes are atoms
of the same element with different masses. Isotopes are created when atoms of the same element do
not have the same number of neutrons. Atoms of the same element may also have different numbers of
electrons. If an atom changes its number of electrons and the atom has an unequal number of protons
and electrons then the atom will be charged. Charged atoms are called Ions. Even though atoms of the
same element may have different numbers of neutrons or electrons we need to remember that they are
still the same element. Only changing protons (or atomic number) changes the element. The concepts
and terms learned in this unit will be important to us throughout the rest of chemistry. Perhaps the
most important of these concepts are valence electrons, ions and isotopes.
Vocabulary Terms:
___ Ion
___ Electron Configuration
___ Average Atomic Mass
___ Charge
___ Isotope
___ Element Symbol
___ Atomic Number
___ Mass Number
___ Metallic Character
___ State of Matter
___ Valence Electrons
___ Hyphen Notation
___ Nuclear Notation
Resources:
 Section 3.3 (pages 77 through 82) – Subatomic Particles, Atomic Mass, Mass Number and Atomic
Number
Assignments:
___ Outline (pages 77 through 82) and Section Review 3.3 # 1 a-d, h, 2, 3 (Subatomic Particles, Atomic
Mass, Mass Number and Atomic Number)
___ WS – SubAtomic Particles and Periodic Table Basics
___ Quiz - SubAtomic Particles, Electron Configurations and Periodic Table Basics
CONCEPTS TO KNOW (BOLDED ARE MORE IMPORTANT)
Introduced: _______ Basic: _________ Mastered: _________
the differences between charged and neutral atoms.
I can identify and describe
What is the difference between a neutral fluorine atom and a fluoride atom which is an atom of fluorine
with a 1_ charge?
Introduced: _______ Basic: _________ Mastered: _________
of each subatomic particle in any given atom.
I can find out the number
Introduced: _______ Basic: _________ Mastered: _________
element in question from the number of subatomic particles.
I can determine the
If an element has 25 protons what is the element?
If an element has a 2+ charge and 10 electrons what is the element?
What subatomic particle cannot be use to identify an element?
Introduced: _______ Basic: _________ Mastered: _________
I can describe how an atom
becomes charged and how to determine the exact numerical charge of the ion. I can describe ions as
either anions (negative atoms) or cations (positive atoms).
Describe how sodium (Na) becomes a 1+ ion? Is Na1+ a cation or anion? Why would Na become a positive
ion and fluorine (F) would be a 1-?
Introduced: _______ Basic: _________ Mastered: _________
I can define an isotope.
Compare and contrast isotopes of Uranium – 234, Uranium – 235 & Uranium – 238?
C4.10c Introduced: _______ Basic: _________ Mastered: _________
I can calculate the
average atomic mass of an element given the percent abundance and mass of the individual isotopes.
Calculate the atomic mass of rubidium. The two isotopes of rubidium have atomic masses and relative
abundancies of 84.91 amu (72.16%) and 86.91 amu (27.84%).
C4.10d Introduced: _______ Basic: _________ Mastered: _________
I can predict which
isotope will have the greatest abundance given the possible isotopes for an element and the average
atomic mass in the periodic table
Which isotope of lithium is more abundant Lithium – 6 or Lithium – 7? Explain
C4.10 e Introduced: _______ Basic: _________ Mastered: _________
for an isotope in nuclear notation
I can write the symbol
Write the nuclear notation for isotopes of uranium 235 and 238.
Introduced: _______ Basic: _________ Mastered: _________
among isotopes of the same element.
I can describe the differences
Introduced: _______ Basic: _________ Mastered: _________
get metallic character and state of matter.
I can read the periodic table to
Describe the basic trend for metallic character within the periodic table. Give examples that support
your trend.
Describe the basic trend for state of matter within the periodic table. Give examples
that support your trend.
C4.8x Introduced: _______ Basic: _________ Mastered: _________
energy levels and orbital blocks within the periodic table.
I can identify the
What block and energy level do the following elements belong: K, V, C, U?
C4.8e Introduced: _______ Basic: _________ Mastered: _________
I can construct the
electron configuration and the noble gas configuration for S and P block elements.
Write the electron configuration and noble gas configuration for I.
C4.8x Electron Configuration - Electrons are arranged in main energy levels with sublevels that
specify particular shapes and geometry. Orbitals represent a region of space in which an
electron may be found with a high level of probability. Each defined orbital can hold two
electrons, each with a specific spin orientation. The specific assignment of an electron to an
orbital is determined by a set of 4 quantum numbers. Each element and, therefore, each
position in the periodic table is defined by a unique set of quantum numbers.;
C4.8e Write the complete electron configuration of elements in the first four rows of the
periodic table.
C4.8f Write kernel structures for main group elements.
C4.8h Describe the shape and orientation of s and p orbitals.
Include!
Demo - Mind Reading Game;
Lecture on the Reading Periodic Table, WS - Periodic Table Basics
Quiz - Periodic Table Basics
Plan - SubAtomic Particles, Electron Configurations and Periodic Table Basics
Day 1 and 2 – Assign Out (pages 77 through 82) and SR 3.3 # 1 a-d, h, 2, 3 – Subatomic
Particles, Atomic Mass, Mass Number and Atomic Number. This assignment will be due Day
4. Use the C4.10 A – D. WS – SubAtomic Particles and Periodic Table Basics as the means
of learning how to determine the number of each subatomic particle in the atom, whether the
atom is charged, difference between isotopes, and how to read the periodic table to get
metallic character and state of matter.
Day 2 and 3 – Students will learn how to construct an electron and noble gas configuration
using WS – Electron and Noble Gas Configurations and Activity – Electron Configuration
Battleship.
Day 4 – Check-In and Review Out and SR 3. 3 (pages 77 through 82).
Quiz - SubAtomic Particles, Electron Configurations and Periodic Table Basics
Teach students how to write the electron configurations for main group elements, Finish with
Electron Configuration Battleship; WS - Electron Configurations (or do H thru K, Ga, Br, Te, Cs,
Pb, Rn); Quiz – Electron Configurations