Week 3 - CHEMISTRY · 64, 68, 71, 72 STP all 6 28, 30, 32, 35, 36 - 46, 48 - 59 . 61 - 63 STP all Suggested problems from the textbook "Chemistry" (Prentice Hall). These are only

Week 3Quarter 2

Using Matter: How to make homogeneous mixtures/solutions

Agenda

• Mid Semester Evaluation (ALEKS)

• www. ALEKS.com

• Student Evaluations

• https://forms.gle/DasdpE2Maus3M8Wj6

• Unit 2 Introduction

• Resources:

• Textbook chapters 4 – 6

• Inspire Chemistry Unit 1: Modules 3 – 5

ALEKS

www.aleks.com

Sign in using your new codes.

Learning Goals

• HS-PS1-1. Use the periodic table as a model to predict the relative properties of elements based on the patterns of electrons in the outermost energy level of atoms.

• HS-PS1-3. Plan and conduct an investigation to gather evidence to compare the structure of substances at the bulk scale to infer the strength of electrical forces between particles.

• HS-PS1-8. Develop models to illustrate the changes in the composition of the nucleus of the atom and the energy released during the processes of fission, fusion, and radioactive decay.

• HS-PS2-6. Communicate scientific and technical information about why the molecular-level structure is important in the functioning of designed materials.*

Problem Pools

Chapter Questions Standardized Test Prep

4 34, 38, 39, 44, (46), 48, 50, 65, 69, 72,74 STP all

5 26, 29, 30,33, 36, 37, 38, 39, 40, 44, 47, 49, 50, 52, 55, 56, 63,

64, 68, 71, 72

STP all

6 28, 30, 32, 35, 36 - 46, 48 - 59 . 61 - 63 STP all

Suggested problems from the textbook "Chemistry" (Prentice Hall). These are only from the

Assessment and Standardized Test Prep found at the end of the chapters. There are also

questions available at the end of each section for more practice.

Main Concepts

• Elements in the Periodic Table (chemical symbol, chemical name, atomic number and average atomic mass)

• Atomic Structure (who did what? Big ideas)

• Subatomic Particles

• Subatomic Particles Masses in grams and a.m.u

• Valence Electrons

• Atoms vs. Ions vs. Isotopes

• Atoms:

o Bohr Model vs. Lewis Structure

o Electronic Configuration (Energy levels, sublevels, and orbitals)

• Ions:

o Electronic Confiuration

• Isotopes:

o Average Atomic Mass

o Nuclear Decay (Chemical reactions vs. Nuclear reactions)

• Electromagnetic Spectrum

• Trends in the Periodic Table

• Initial Concepts of Bonding

Resources

• Textbook Chapters 4 – 6

• Inspire Chemistry Unit 1:

Modules 3 – 5

Inspire Chemistry

Unit 1: Modules 3 – 5

Let's delve further on what IC has to offer. Each Unit has Modules and each Module has Lessons. Click on Module 3.

• Unit

• Module

o Lesson

The main parts we use in the Module are the

• Science Notebook

• Supplemental Problems

• Module Test

• Study Guide

• Other Labs and ActivitiesTextbook Notes Guide

Inspire Chemistry

Unit 1: Modules 3 – 5

Click on Lesson 1 in Module 3:

• Learnsmart

• Science notebook

• Explore and Explain

• Challenge Problems

• Lesson Checks

• PhET Simulations

• Other labs and activities

Lesson Checks

Each Unit has Modules and each

module has Lessons.

Unit

• Module

o Lesson

Lesson checks are found in the

evaluate section.

Atomic Structure

What do

you

think?

Illustration on the blank side of the card:

1. What does an atom look like? Label all parts.

Answer on the lined side of the card:

1. How is the periodic table organized? Use terminology. Labeled illustrations are acceptable.

2. Why do atoms want to bond with other atoms?

3. How do they bond? Write/illustrate parts of the atom involved in bonding.

4. What is the overlying theme in chemistry (all sciences)? Use only 1 word.

Periodic Table

How is it organized?

And what does it mean?

How is the organization of the periodic

table related to the structure of the

atom?

Demo: Alkali Metals

1. Which group on the periodic

table?

2. Physical and Chemical

Properties

3. Reacts with Water

- Chemical reaction of metal with

water

https://www.youtube.com

/watch?v=uixxJtJPVXk

Periodic Table

Take out the big periodic table and note that you will start using it as a reference to specific details about

atoms and how they bond with each other.

1) Color in the groups of the periodic table.

2) Use the internet and textbook to learn some basic properties that

belong to each GROUP. Take notes in your One Note.

Elements

Groups vs. Periods

Atomic Structure

Coulombic Attraction

Strong Nuclear Force

Atomic Number

Atomic Mass

Ions

Isotopes

Elements

Groups vs. Periods

Atomic Structure

Coulombic Attraction

Strong Nuclear Force

Atomic Number

Atomic Mass

Ions

Isotopes

Elements

Groups vs. Periods

Atomic Structure

Coulombic Attraction

Strong Nuclear Force

Atomic Number

Atomic Mass

Ions

Isotopes

Atoms vs. Ions

Elements

Groups vs. Periods

Atomic Structure

Coulombic Attraction

Strong Nuclear Force

Atomic Number

Atomic Mass

Ions

Isotopes

Elements

Groups vs. Periods

Atomic Structure

Coulombic Attraction

Strong Nuclear Force

Atomic Number

Atomic Mass

Ions

Isotopes

Activity:Build an Atom PhET

One Note: Content Library: Unit 2:

Topic 2

Complete the accompanying

worksheet for practice.

https://phet.colorado.edu/en/simula

tion/build-an-atom

Band of Stability

A plot of the number of neutrons

versus the number of protons

for stable nuclei reveals that

the stable isotopes fall into a

narrow band. This region is known

as the band of stability (aka. Zone

of stability)

Expressing the

Elements

• When referring to a single type

of nucleus, we often use the

term nuclide and identify it by

the notation , where X is the

symbol for the element, A is the

mass number, and Z is the

atomic number (for example, ).

Often a nuclide is referenced by

the name of the element

followed by a hyphen and the

mass number. For example, is

called “carbon-14.”