Honors Chemistry Notes

Day 1

Welcome and Introduction

  • Initial Tasks:
    • Obtain a copy of the Minilab and Syllabus from the front counter.
    • Leave your phone on the stand behind the desk in the numbered slot assigned to your name.
    • Use the poker chip to find your seat by matching the element.

Agenda

  • Topics Covered:
    • Policies
    • Introductions
    • Quick Safety Briefing
    • Labette - Chemistry In A Bag
    • Quiz, Quiz, Trade
    • Syllabus
    • Honors Chemistry Website

Policies & Guiding Principles

  • Guiding Principles/Rules & Expectations:
    • Be Responsible
    • Be Ready To Learn
    • Be Respectful

Phone Policy

  • Phone Usage:
    • Place phones in the phone stand upon entering the classroom.
    • Phones are allowed for authorized purposes only, with teacher discussion.
    • Phones are not allowed in the restroom.
  • Attendance:
    • Attendance will be taken using the phone stand. A missing phone indicates absence.
    • Reminder to put the phone in the stand results in a tardy mark.
    • A one-week grace period is given to adjust to this policy.

Restroom Policy

  • Restroom Use:
    • Only one student is allowed to use the restroom at a time.
    • Electronic sign-out is managed by the teacher. Students are cleared to go upon approval, and must check back in upon return.
    • If the name is already on the out section of the board, the student must put their name on the waiting list.
    • No permission is needed; however, students should be respectful and go during transition times if possible.

Introductions

  • Sharing personal stories by Mrs. Bude, Mrs. Morgan and Dr. Parker relating to their education or personal background.
  • Students are prompted to introduce themselves to their tablemates using suggested prompts:
    • Share something fun you did over the summer.
    • What are you currently binge-watching?
    • Do you have any pets?
    • If you were a potato, what kind of potato would you be?

Safety

  • Lab Safety Guidelines:
    • Hair should be pushed back.
    • Protective gloves should be worn.
    • Closed-toe shoes are required.
    • Proper clothing is necessary.
  • Goggles:
    • Goggles must be worn at all times during the lab and must remain on (and over the eyes.)
    • Failure to follow safety procedures will have serious consequences.

Chemistry In A Bag Lab

  • Instructions:

    • Work in assigned lab groups to complete the activity, following the instructions carefully to achieve expected results.
    • Record procedures and observations in the T-chart on the worksheet.

  • Cleanup:

    • Empty bag contents into the waste container.
    • Dispose of the empty bag in the large gray trash can.
    • Return all unused materials to the designated white bin and return the bin to the side counter where it was obtained.
    • Clean the lab table with a Clorox wipe and return used materials to their proper location.

Quiz, Quiz, Trade Activity

  • Instructions:
    • Each person takes a colored slip of paper from the center of their table.
    • Find someone unfamiliar and ask them the question on your paper. After answering each other’s questions, trade papers and find someone new.

Syllabus

  • Syllabus Review:
    • Students and their parent/guardian should read the entire syllabus and complete the online acknowledgment form.
    • Lack of reading the syllabus or forgetting class policies does not excuse consequences.

Honors Chemistry Website

  • The Honors Chemistry Website's address is bit.ly/HC24-25

Student Survey

  • A survey is available for students to complete as homework by Tuesday.

Name Pronunciation

  • Students are requested to provide the correct pronunciation of their names via a Padlet assignment linked on the Chemistry Website.
    • How to correctly pronounce your name
    • Preference between waffles and pancakes

Homework

  • Assignments:
    • Complete Chemistry In A Bag if not finished in class, to be brought to class on Monday, August 19.
    • Syllabus Acknowledgement Form to be completed by both student and parent/guardian, due on Monday, August 19.
    • Complete the Welcome To Honors Chemistry Survey and Say My Name Padlet assignment, both due on Tuesday, August 20.

Day 2

Warm-Up

  • Tasks:
    • Place cell phones in the stand.
    • Obtain a copy of the worksheets from the front counter.
    • Discuss "What is the difference between a scientific theory and a scientific law?" with your table.

Padlet Reminder

  • Complete the "Say My Name, Say My Name" Padlet assignment by Tuesday, ensuring a video submission is included.

Agenda

  • Topics:
    • Practice vs. Homework & Portfolio
    • Elemental "You"
    • Theory vs. Law
    • Safety Video & Contract
    • Measurement & Significant Figures

Homework

  • Assignments that will be collected and graded
    • Completing assignments started in class
    • Pre-/Post-lab write ups
    • Advance reading
  • NOT optional

Practice

  • This work is NOT required and is NOT graded, but HIGHLY RECOMMENDED. Answers are posted for you to assess your understanding.
  • Practice will help you with understanding the concepts we discuss in class (both old and new).
  • This work, completed or not, should go in your Portfolio.

Portfolio

  • A compilation of all of the work that you did for a unit.
  • Use as a study guide for the unit exam.
  • Turn it in for credit on the day of the unit exam.

Formative Assessment

  • Online, assessment style questions you do on your own
  • Use it to assess how ready you are for the exam - you can take it multiple times
  • HIGHLY RECOMMENDED but not for a grade

Elemental "You"

  • Create a personalized version of a Periodic Table "box" reflecting who you are.
  • Follow the same basic format as the example on the worksheet.
  • Due Tuesday 8/20 or Wednesday 8/21

Theory vs. Law

  • Discuss individually statements that apply to scientific theories
  • Discuss your answers as a group. Note any questions or differing opinions

The Scientific Method

  • A systematic approach to studying nature involving observations, hypotheses, and experiments.

    • Make Observations
    • Ask Questions
    • Collect Data
    • Formulate Hypotheses
    • Perform Experiments

  • Scientific theories can change as new information is gathered.

  • Scientific Method Process

    • Ask a question
    • Research your topic
    • Make a hypothesis
    • Test hypothesis with an experiment
    • Analyze the data and draw conclusions
    • Communicate results

  • If the experiment is not working, try to fix the experiment/procedure!

  • From the Scientific Method to Scientific Law

    • Observations / Experimental Data
    • Hypothesis
    • Scientific Theory
    • Scientific Law ModificationRevision

Scientific Law vs. Scientific Theory

  • Describes WHAT happens vs Explains WHY or HOW it happens
  • Examples:
    • Special Relativity
    • Universal Gravitation
  • Scientific Law: description of observed phenomena (patterns), tells us what happens, sometimes expressed as a mathematical formula
  • Scientific Theory: well-supported explanation of observations, repeatedly tested and confirmed, attempts to explain why it happens
  • A law is an observation of WHAT happens. A theory attempts to explain WHY something happens.

Types of Observations

  • Qualitative: non-numerical, asks “what?”. Example: larger orange
  • Quantitative: numerical, asks “how much?”. Example: 52 liters, 3×1083 \times 10^8 m/s
  • Quantitative observations are also called measurements

Safety

  • Watch the Safety Video posted on the course website
  • Complete the Video Notes including the classroom diagram
  • Take and grade the Safety Quiz (it will go in your portfolio). The key is posted on the website.
  • Read and sign the Safety Contract. Make sure your parent/guardian signs it too

Measuring & Significant Figures

  • When making a measurement, always estimate one digit beyond the scale reported on the instrument.
  • For Example: 4.78 cm
  • We can never report data to a higher degree of precision than is appropriate.
  • The significant figures in a measurement include all the digits that can be known unmistakably plus a last digit that must be estimated.
  • For Example: 4.78 cm has 3 significant figures
  • When you use the measurements in your calculations, your answer cannot be MORE precise than the least precise measurement.
  • The purpose of significant figures is to communicate the accuracy of a measurement as well as the measuring capacity of the instrument used.
  • Significant digits are digits believed to be correct by the person making and recording a measurement.

Measured Numbers

  • Involve estimation
  • Have a defined number of significant figures

Significant Figures - The Rules

  • Rule 1: All non-zero numbers in a recorded measurement are significant.
    • 3. 57 mL has three significant digits
    • 28 kg has two significant digits
  • Rule 2: Leading zeros are never significant.
    • 0. 1 mm has only one significant digit
    • 0. 01 cm3^3 has only one significant digit
    • Leading zeros precede all of the nonzero digits. They are placeholder numbers.
  • Rule 3: Captive Zeros are always significant figures.
      1. 8 mL has three significant digits
      1. 08 cm has four significant digits. Captive zeros fall between non-zero digits. They are also called sandwich zeros.
  • Rule 4: Trailing zeros are significant if they terminate a number containing a decimal place.
    • 0. 010 mg has two significant digits
    • 3.20×1043.20 \times 10^4 kg has three significant digits
    • 30 m has one significant digit
      1. m has two significant digits

Exact Numbers

  • Exact numbers are known to be absolutely correct
  • Obtained by counting or by definition.
    • 10 experiments, 3 apples
    • 1 km = __ m
    • 1 century = ___ years
    • 1 dozen = _ eggs
  • Infinite Number of Significant Digits

Let’s Practice

  • Indicate how many significant figures the number has. Also indicate which rule you used to determine the sig figs (it could be more than one).
    1. 10 grams
  • 30080 moles
  • 00420 molecules
  • 100 g/mL
  • 1 g/mL

HOMEWORK

  • Due Monday, August 19:

    • Chemistry In A Bag
    • Syllabus Acknowledgement Form (Google Form)

  • Due Tuesday/Wednesday August 20/21:

    • Elemental You
    • Welcome To Honors Chemistry Survey & Say My Name Flipgrid

  • Due Thursday/Friday August 22/23:

    • Safety Video & Quiz
    • Safety Contract

  • Practice

  • Scientific Method Handout & Worksheet

  • Significant Figures Worksheets A & B

Day 3

Warm Up

  • Write the statement and classify it as a law, a theory, an experiment, a hypothesis, a qualitative observation, or a quantitative observation.

    • Measured amounts of acid were added to a Rolaids tablet to see whether it really “consumes excess stomach acid.”
    • Heat always flows from hot objects to cooler ones and can be measured.
    • The universe was formed by a massive explosion that propelled matter allowing atoms to form and then molecules.
    • Roses watered with Vitamin B will grow faster than roses watered with Vitamin E.
    • Limestone dissolves in dilute acid.
    • The current passing through the device was 4.5 amperes.

  • Have Your Chemistry in a Bag Assignment Out For A Stamp!

Answers

  • Experiment
  • Law
  • Theory
  • Hypothesis
  • Qualitative observation
  • Quantitative observation

Syllabus & Course Information

  • Measuring Activity - practice with Significant Figures. Record the measurement of each of the items on your table to the correct number of significant figures.
  • Clean Up - Return all materials to the container on your table. Return any borrowed materials to their original location.
  • Absent students use these images to practice reading measurements:

Accuracy and Precision

  • Accuracy refers to how well your measurement agrees with a known quantity.

  • Precision is how well your measurements agree with each other.

  • Accuracy

    • How close a result is to the “true” value
    • Is a measure of rightness

  • Precision

    • How close measurements are to each other
    • Reflects reproducibility of results
    • Is a measure of exactness

  • Examples

  • Practice!

    • You measure a string three times and get 7.5cm, 7.4cm and 7.5 cm. The string is known to be 9cm. Accuracy? Precision? - Not Accurate Precise
    • True value of the mass of a piece of iron is 66g. The student’s measures of the mass of the iron are 60g, 55g, and 4g Accuracy? Precision? - Not Precise Not Accurate
    • The true value of the density of a piece of copper is 15 g/cm3. A student’s measurements of the density are 15 g/cm3, 14.9 g/cm3 and 15.1 g/cm3. Accuracy? Precision? - Accurate Precise

Homework

  • Due Tuesday/Wednesday August 20/21:
    • Elemental You
    • Welcome To Honors Chemistry Survey & Say My Name Flipgrid
  • Due Thursday/Friday August 22/23:
    • Safety Video & Quiz
    • Safety Contract

Day 4

Warm-Up

  • How many significant figures are in each of the following? Explain which “zero” rule(s) you used.

    • 709

    • 00709

    • 007090

    • 1040

    • 1040.

    • 34500.05060

    • Now write each number in correct scientific notation?

Scientific Notation

  • Chemists use very large and small numbers.

  • For example:

    • The mass of a hydrogen atom is 0.00000000000000000000000167 grams
    • Hydrogen molecules: 602000000000000000000000

  • It is Helpful to write these numbers in scientific notation

  • The mass of a hydrogen atom is 0.00000000000000000000000167 grams. This can be written in scientific notation as: 1.67×10−241.67 \times 10^{-24} grams

  • Hydrogen molecules: 602000000000000000000000. This can be written in scientific notation as: 6.02×10236.02 \times 10^{23} molecules

  • Numbers written in scientific notation have three parts:

    • coefficient
    • base
    • exponent

  • COEFFICIENT: The coefficient must be greater than or equal to 1 and less than 10. The coefficient must contain all of the significant figures in a number.

  • BASE: For scientific notation, we typically use base 10. You may have seen other bases in your math classes.

  • EXPONENT: The exponent tells you how many times to multiply the coefficient times 10.

    • 6.02×10×10×10×10×10×10×10×10×10×10×10×10×10×10×10×10×10×10×10×10×10×10×106.02 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10 \times 10

  • IMPORTANT!! When writing numbers in scientific notation in Science, we use an “x” , not a dot. If you write your number with a dot, it will be counted wrong!

  • NUMBERS GREATER THAN 10

    • Numbers greater than 10 have a positive exponent.

    • The exponent is equal to the number of places that the decimal point has been moved to the left.

    • 10=1×10110 = 1 \times 10^1

    • 12,000,000=1.2×10712,000,000 = 1.2 \times 10^7

    • 85,130=8.513×10485,130 = 8.513 \times 10^4

    • 85,130.=8.5130×10485,130. = 8.5130 \times 10^4 This decimal makes the zero significant

  • An Example:

    • 23000 is 2.3×1042.3 \times 10^4

  • NUMBERS LESS THAN 1

    • Numbers less than 1 have a negative exponent.

    • The exponent is equal to the number of places that the decimal point has been moved to the right.

    • 0.00005=5×10−50.00005 = 5 \times 10^{-5}

    • 0.0342=3.42×10−20.0342 = 3.42 \times 10^{-2}

    • 0.00200=2.00×10−30.00200 = 2.00 \times 10^{-3}

    • 0.002=2×10−30.002 = 2 \times 10^{-3}

  • An Example:

    • 00023 is 2.3×10−42.3 \times 10^{-4}

  • NUMBERS BETWEEN 10 AND 1

    • You really don’t need scientific notation
    • You would be making the number more complicated.
    • 9=9×1009 = 9 \times 10^0
    • 1.2=1.2×1001.2 = 1.2 \times 10^0
    • 7.562580=7.562580×1007.562580 = 7.562580 \times 10^0 **Don’t write numbers 1 < x < 10 using 100 in this class! Just writing the regular number counts as “scientific notation.