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