Unit Plan 6:
Arrangement of Electrons in Atoms
Chemistry Level
2/Mrs. Wissler
Learning
Objectives: The student will be able to
- Explain
the mathematical relationship among the speed, wavelength, and frequency
of electromagnetic radiation.
- Discuss
the dual wave-particle nature of light.
- Describe
the Bohr model of the hydrogen atom.
- Compare
and contrast the Bohr model and the quantum model of the atom.
- Explain
how the Heisenberg uncertainty principle and the Schrodinger wave equation
led to the idea of atomic orbitals.
- List
the four quantum numbers and describe their significance.
- Relate
the number of sublevels corresponding to each of an atom’s main energy
levels, the number of orbitals per sublevel, and the number of orbitals
per main energy level.
- List
the total number of electrons needed to fully occupy each main energy
level.
- State
and apply Aufbau principle, the Pauli Exclusion Principle, and Hund’s
rule.
- Describe
the electron configurations for the atoms of any element using orbital
notation and electron-configuration notation.
Essential
Questions: How can atomic
models be used to explain atoms and help us understand the interaction of
elements and compounds?
Central Concepts:
Atomic models are used to explain atoms and help us understand the interaction
of elements and compounds observed on a macroscopic scale. The periodic table displays the repeating
patterns, which are related to the atoms’ outermost electrons.
Text: Ch. 4 - all section objectives and
bolded vocabulary
Activities/Lab/Assessments:
Day 1 A,B
– 12/21 D-12/22
Notes: Wave and Particle Properties of Light,
Electromagnetic Spectrum
Flame
Test Set Up and Lighting Practice
HW: Guided Reading Sec 4.1 The Development
of a New Atomic Model #1-13
Day 2 A,B – 12/23 D-1/4
Lab: Flame Test
HW: Guided Reading questions #14-22 (D
block)
Day 3 A,B – 1/5 D- 1/6
Demonstration: Spectroscopes Natural and Artificial Light
Notes: Line-Emission Spectra and the Bohr Model
Lab: Complete Unknowns for Flame Test
HW:
Flame Test Lab Report
Day 4 A,B
– 1/7 D-1/8
Warm
Up: Bohr Model Quiz Review
Group
Study Questions
Powerpoint: Wave and Particle Properties of Electrons,
Heisenberg and Schrodinger
HW: Study for Bohr Model Quiz
Day 5
A,B – 1/11 D-1/12
Bohr
Model Quiz
Finish
Wave and Particle Properties of Electrons
Graphic
Organizer/Models: Quantum Model of the
Atom and Orbital Shapes
Midterm
Review Materials
HW: Sec 4.2 Guided Reading, Review for Midterm
Day 6 A,B
– 1/13 D-1/14
Graphic
Organizer: spdf block Periodic Table
Notes: electron configuration and atomic
sublevels/energy graph
Practice: Electron Configuration Notation and Orbital
Notation
Notes: Aufbau Principle, Pauli Exclusion Principle
and Hund’s Rule
HW: Electron
Configuration Practice, Review for Midterm
Day 7 A,B – 1/15 D-1/19
Unit
1-5 Review
Practice
Midterm
HW:
study for Midterm, prepare notecard
MIDTERM
MCAS
Chemistry Frameworks:
ü MCAS
2.3 Recognize discoveries from Dalton (atomic theory), Thomson (the electron),
Rutherford (the nucleus), and Bohr (planetary model of atom), and understand
how each discovery leads to modern theory.
ü MCAS 2.4 Write the electron configurations for the first twenty
elements of the periodic table.
ü MCAS 3.3 Relate the position of an element on the periodic table
to its electron configuration and compare its reactivity to the reactivity of
other elements in the table.
ü MCAS 3.4 Identify
trends on the periodic table (ionization energy, electronegativity, and
relative sizes of ions).
ü