New User Special Price Expires in

Let's log you in.

Sign in with Facebook


Don't have a StudySoup account? Create one here!


Create a StudySoup account

Be part of our community, it's free to join!

Sign up with Facebook


Create your account
By creating an account you agree to StudySoup's terms and conditions and privacy policy

Already have a StudySoup account? Login here

CHEM 1030, Week 1/2 Notes

by: Alyssa Anderson

CHEM 1030, Week 1/2 Notes CHEM 1030

Marketplace > Chemistry > CHEM 1030 > CHEM 1030 Week 1 2 Notes
Alyssa Anderson

Preview These Notes for FREE

Get a free preview of these Notes, just enter your email below.

Unlock Preview
Unlock Preview

Preview these materials now for free

Why put in your email? Get access to more of this material and other relevant free materials for your school

View Preview

About this Document

These notes cover what we discussed in class 1/14/16, 1/19/16, and 1/21/16.
Fundamentals Chemistry I
Dr. Streit
Class Notes
25 ?




Popular in Fundamentals Chemistry I

Popular in Chemistry

This 5 page Class Notes was uploaded by Alyssa Anderson on Tuesday January 19, 2016. The Class Notes belongs to CHEM 1030 at a university taught by Dr. Streit in Spring 2016. Since its upload, it has received 44 views.


Reviews for CHEM 1030, Week 1/2 Notes


Report this Material


What is Karma?


Karma is the currency of StudySoup.

You can buy or earn more Karma at anytime and redeem it for class notes, study guides, flashcards, and more!

Date Created: 01/19/16
Alyssa Anderson Chemistry Notes Weeks 1 and 2 1/13/16-1/22/16 Chemistry- the study of matter and changes that matter undergoes Matter- anything that has mass and occupies space Scientific Method- a procedure/set of guidelines to organize and publish efficiently 1. Gather data through observations and experiments 2. Identify patterns and trends in collected data and note any initial thoughts 3. Summarize findings with a law- a concise statement that makes a relation between phenomena 4. Formulate a hypothesis by observing the cause and effect relationship 5. With time, the hypothesis may evolve into a theory which can predict future occurrences Chemists classify matter as either a substance or a mixture of substances 1. Substance- a form of matter that has a definite composition and distinct properties - example: salt (NaCl), iron, water (H20), mercury, carbon dioxide (CO2) - substances differ from each other in composition and may be identified by appearance, taste, smell, etc. 2. Mixture- physical combination of 2 or more substances a. homogenous- uniform throughout solution - example: seawater, apple juice, cake b. heterogenous- not uniform throughout solution - example: trail mix, chicken noodle soup, shells in sand Classification of Matter 1. Solid- particles are held close together in an ordered position and DO NOT conform to the container it is placed in 2. Liquid- particles are held relatively close together but do not have an organized pattern and DO conform to the the container it is placed in 3. Gas- particles are far apart and have no set pattern but DO conform to the container it is placed in 4. In principle, all substances can exist in the solid, liquid, or gaseous stage 5. We can convert a substance by changing its identity 6. Mixtures can be separated by physical means into its component without changing the identities of the components - example: magnet to separate sand and iron (iron is magnetic) - example: boil water to separate salt and water (water has a much lower boiling point) - example: boil water to separate water and alcohol (different boiling points) Properties of Matter 1. Quantitative- properties measured/expressed with a number/unit (QUANTITY) 2. Qualitative- properties measured without measurements but rather are based on observations using the senses (taste, color, smell, etc.) (QUALITY) 3. Physical Property- one that can be observed or measured without changing the identity of the substance - example: color, melting point, boiling point 4. Chemical Property- one that a substance exhibits as it interact with another substance - example: flammability, corrosiveness, rust 5. Physical Change- change where the state of matter changes but the identity of the matter does not change - example: changes of state (melting, boiling, freezing, condensing) 6. Chemical Change- change in the composition so that the original composition no longer exists - example: digestion, combustion, oxidation 7. Extensive Property- depends on the amount of matter present - example: mass, volume, aka additive properties 8. Intensive Property- does NOT depend on the amount present - example: temperature, density 9. Physical Process- mixtures are separated but the identities do not change 10. Chemical Process- a process of changing mixtures/chemicals Scientific Measurement 1. Properties that can be measured are called quantitative 2. A measured quantity must always include a unit 3. Systems A. English- foot, gallon, pound, Fahrenheit B. Metric- meter, liter, kilogram C. International System of Units (SI units)- universally used by scientists 1. Meter 2. Kilogram 3. Kelvin 4. Second 5. Ampere 6. Mole 7. Candela 4. Mass (g or kg or amu) A. a CONSTANT measure of amount of matter in an object/sample B. Gravity varies from location to location constant so weight = mass x gravity C. the mass of an atom is 1 amu= 1.6605378 x 10^-24 g 5. Temperature (Celsius or Kelvin or Fahrenheit) A. Celcius- for water, freezing point is O*C, boiling point 100*C B. Kelvin (*SI UNIT*)- “absolute” scale because 0 K is the absolute lowest C. K = *C + 273.15 OR C* = K - 273.15 D. Fahrenheit- for water, freezing point is 32*F and boiling point is 212*F E. *F = (9/5)(*C) + 32*F OR *C = (5/9)(*F - 32) 6. Volume (meter^3 or Liter) A. V = (length)^3 B. 1 dm^3 = 1 L C. 1 cm^3 = 1 mL 7. Density (kg/m^3) A. d = mass/volume so d = mass/length^3 B. solid = g/cm^3 C. liquid = g/mL D. gas = g/L E. example: if d1>d2 then m1<m2 OR v1>v2 Uncertainty in Measurements 1. Exact Numbers- defined values or counted numbers - example: 1 kg = 1000 g - example: 1 dozen = 12 items - example: 28 students in a class 2. Inexact Numbers- measured by anything but counting such as length, volume, mass A. It must be reported to indicate uncertainty by using significant digits B. The last digit reported is called the uncertain digit C. example: if we have an item against a ruler and we think it’s about 2.5 inches long, we know it’s for sure 2 inches but not sure about the .5, so we put 2.5 +/- 0.1 inch, and with a more accurate ruler we could put 2.45 inches +/- 0.01 inch D. Guidelines of Significant Figures 1. Any nonzero numbers ARE significant 2. Zeros between nonzero numbers ARE significant 3. Zeros to the LEFT of the first nonzero digit are NOT significant 4. Zeros to the RIGHT of the nonzero digits in decimals ARE significant 5. Zeros to the RIGHT of the last nonzero digit in a number without a decimal MAY OR MAY NOT be significant - example: 100 could have 1 2 or 3 significant figures Calculations with Measured Numbers 1. Addition/Subtraction- line up the decimals and take the answer with the smaller amount of digits (rounding may be necessary) 2. Multiplication/Division- preform the action then take the fewer amount of digits from the original numbers given (rounding may be necessary) 3. NOTE: Be sure not to include exact numbers, such as the counted number - example: when finding the mass of each of 2 pennies, knowing together they equal 15 grams, 2 is not included in the measurement of significant figures. Therefor, since together they had 15 grams and that is 2 significant figures, your answer will have 2 significant figures 4. Rounding A. Leave rounding for the LAST step. DO NOT ROUND AFTER EACH STEP B. If the last digit is greater than 5, round UP (ex: 318.175 = 318.18) C. If the last digit is less than 5, round DOWN (ex: 318.174 = 318.17) 5. NOTE: Be aware of powers of 10. Make sure that you are calculating variables with the same power, then proceed 6. NOTE: Significant figures matter even when scientific notation changes 7. NOTE: Be sure to calculate the right mass or volume before proceeding to find density or weight 8. Accuracy- how close the measurement is to the TRUE value 9. Precision- how close a series of measurements are to one another Using Units and Solving Problems 1. Conversion Factor- fraction in which same quantity is expressed one way in the numerator and another in the denominator - example: 1 inch = 2.54 cm aka 1 in/2.54 cm OR 2.54 cm/1 inch 2. Dimensional Analysis- use of conversion factors in problem solving A. Also known as the factor-label method B. example: convert 12 inches to meters (NOTE: only use significant figures of the thing you are converting (so 2 s.f. because 12 inches has 2 s.f.); 12 inches x 2.54 cm/1 inch x 1m/100 cm = 0.3048 m = 0.30 m


Buy Material

Are you sure you want to buy this material for

25 Karma

Buy Material

BOOM! Enjoy Your Free Notes!

We've added these Notes to your profile, click here to view them now.


You're already Subscribed!

Looks like you've already subscribed to StudySoup, you won't need to purchase another subscription to get this material. To access this material simply click 'View Full Document'

Why people love StudySoup

Jim McGreen Ohio University

"Knowing I can count on the Elite Notetaker in my class allows me to focus on what the professor is saying instead of just scribbling notes the whole time and falling behind."

Janice Dongeun University of Washington

"I used the money I made selling my notes & study guides to pay for spring break in Olympia, Washington...which was Sweet!"

Steve Martinelli UC Los Angeles

"There's no way I would have passed my Organic Chemistry class this semester without the notes and study guides I got from StudySoup."

Parker Thompson 500 Startups

"It's a great way for students to improve their educational experience and it seemed like a product that everybody wants, so all the people participating are winning."

Become an Elite Notetaker and start selling your notes online!

Refund Policy


All subscriptions to StudySoup are paid in full at the time of subscribing. To change your credit card information or to cancel your subscription, go to "Edit Settings". All credit card information will be available there. If you should decide to cancel your subscription, it will continue to be valid until the next payment period, as all payments for the current period were made in advance. For special circumstances, please email


StudySoup has more than 1 million course-specific study resources to help students study smarter. If you’re having trouble finding what you’re looking for, our customer support team can help you find what you need! Feel free to contact them here:

Recurring Subscriptions: If you have canceled your recurring subscription on the day of renewal and have not downloaded any documents, you may request a refund by submitting an email to

Satisfaction Guarantee: If you’re not satisfied with your subscription, you can contact us for further help. Contact must be made within 3 business days of your subscription purchase and your refund request will be subject for review.

Please Note: Refunds can never be provided more than 30 days after the initial purchase date regardless of your activity on the site.