Power Notes Measurements and Dealing with Data 2
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This document provides an overview of key concepts for measurements and data analysis in chemistry: 1) It defines the International System of Units (SI units) that are used as standard units of measurement in chemistry, including units for length, mass, volume, temperature, amount of substance, and time. 2) It explains the importance of clearly labeling all measurements with their corresponding units and discusses sources of uncertainty in measurements. 3) It introduces tools for collecting data in chemistry experiments and defines common variables like independent and dependent variables that are used to analyze relationships in data. Graphs and mathematical models are presented as ways to interpret data.
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Power Notes Measurements and Dealing with Data
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2) It discusses the importance of labeling measurements with units and outlines sources of uncertainty in measurements.
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Power Notes Measurements and Dealing with Data
1. This document outlines an assignment log and notes for a chemistry class, including assignments, units of measurement, and key concepts around collecting and analyzing scientific data.
2. It discusses the International System of Units (SI units) that are used in chemistry and defines common units of measurement for properties like length, mass, volume, temperature, and time.
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The document outlines the materials and assignments for a chemistry class, including colored pencils, stapled notes on measurements and dealing with data, and a stapled assignment on tools of the trade that is due. It also provides information on units of measurement in the International System of Measurements, tools used to measure various quantities, and variables in data analysis. Students are asked to complete notes on measurements and dealing with data for homework.
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This document provides instructions and assignments for a chemistry class. It includes a checklist of assignments with due dates, instructions for an in-class quick write assessment, notes on extra credit opportunities, corrections to a crossword puzzle, and directions for completing power notes on measurements and dealing with data. Students are asked to have materials ready, log into an online system, and work on completing their power notes during class. Homework includes finishing any past due assignments and completing the power notes by the following Tuesday.
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This document provides instructions for a chemistry class assignment. Students are asked to bring specific supplies including a pencil, colored pencils, and stapled assignments. They must update their assignment log online and submit a stapled assignment. The document then reviews power notes on measurements and dealing with data that students must complete for homework. It instructs students to log into the classroom website to view the slideshow and take notes by paraphrasing, abbreviating, and highlighting the material, which is due the next day. Students are also told their seats will be changed for the next class.
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Power Notes Measurements and Dealing with Data
1) The document provides an overview of measurements and units used in chemistry, including the metric system prefixes and units for length, mass, volume, temperature, amount of substance, and time.
2) It discusses the importance of labeling measurements with units and outlines sources of uncertainty in measurements.
3) The final sections cover tools for collecting data, analyzing data through graphs and mathematical models, and identifying direct and indirect relationships between variables in an experiment.
Power Notes Measurements and Dealing with Data
1. This document outlines an assignment log and notes for a chemistry class, including assignments, units of measurement, and key concepts around collecting and analyzing scientific data.
2. It discusses the International System of Units (SI units) that are used in chemistry and defines common units of measurement for properties like length, mass, volume, temperature, and time.
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This document provides instructions and information for a chemistry class. Students are asked to bring specific materials to class including pencil/pen, colored pencils/markers, and completed power note papers. An assignment log is included listing upcoming assignments and due dates. The class will then focus on completing a set of power notes on measurements and dealing with data. These notes cover topics like units, the international system of units, prefixes, zero kelvin, accuracy vs precision, variables in experiments, and analyzing data through graphs. Students are instructed to paraphrase, abbreviate and highlight the notes. Homework includes completing any past due assignments and the power notes.
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This document provides instructions for a chemistry class assignment. Students are asked to bring specific supplies including a pencil, colored pencils, and stapled assignments. They must update their assignment log online and submit a stapled assignment. The document then reviews power notes on measurements and dealing with data that students must complete for homework. It instructs students to log into the classroom website to view the slideshow and take notes by paraphrasing, abbreviating, and highlighting the material, which is due the next day. Students are also told their seats will be changed for the next class.
Power Notes Measurements and Dealing with Data
This document provides instructions and assignments for students in a chemistry class. It includes:
1. A list of materials needed for class today, including notes on measurements and dealing with data.
2. Instructions to log into an online system to access and complete the power notes on measurements and dealing with data.
3. An assignment log tracking assignments that have been given and are due, along with points possible and earned.
4. The power notes on measurements and dealing with data, which include topics like units, the international system of units, prefixes, absolute zero, Celsius, accuracy vs precision, tools used to measure, variables in experiments, graphs, and patterns between variables.
Errors and uncertainities net
- Random uncertainties arise from imprecision in measurements and can cause readings to be above or below the true value. They can be reduced by more precise instruments or repeating measurements.
- Systematic uncertainties result in all readings being consistently too high or too low. They may be due to instrumentation errors or experimental technique and can sometimes be addressed through calibration.
- Uncertainty is incorporated into measurements as a range rather than a single value, and it is important to propagate uncertainties through calculations.
Measurement
Measurement involves assigning a number to an object's characteristic that can be compared to other objects. There are two main systems of measurement: the English system used in the U.S. which uses feet, pounds, and seconds, and the metric system used internationally which is based on units like meters, grams, and liters. Converting between units requires understanding the relationships between prefixes and moving decimals accordingly.
Uncertainties rules 1
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Scientific notation and SI units are used in measurement to help scientists communicate measurements clearly across countries. The basic SI units include meters, kilograms, seconds, amperes, moles, candelas, and kelvins. Derived units are calculated from the basic units, such as newtons from kilograms and meters/seconds. SI prefixes modify the scale of units, from centi to giga. The precision of calculations is limited by the measurement with the fewest significant figures. Temperature in kelvins is calculated by adding 273 to degrees Celsius.
Mass and volume
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- Volume measurement using graduated cylinders and the displacement method
- Mass measurement using a triple beam balance in grams
- Temperature measurement using a thermometer in Celsius, Fahrenheit, or Kelvin
It also discusses metric unit conversions using the "King Henry" method where the number of metric "hops" determines where to place the decimal, and the factor label method using unit cancellation.
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Power Notes Measurements and Dealing with Data
This document provides instructions and assignments for students in a chemistry class. It includes:
1. A list of materials needed for class today, including notes on measurements and dealing with data.
2. Instructions to log into an online system to access and complete the power notes on measurements and dealing with data.
3. An assignment log tracking assignments that have been given and are due, along with points possible and earned.
4. The power notes on measurements and dealing with data, which include topics like units, the international system of units, prefixes, absolute zero, Celsius, accuracy vs precision, tools used to measure, variables in experiments, graphs, and patterns between variables.
Errors and uncertainities net
- Random uncertainties arise from imprecision in measurements and can cause readings to be above or below the true value. They can be reduced by more precise instruments or repeating measurements.
- Systematic uncertainties result in all readings being consistently too high or too low. They may be due to instrumentation errors or experimental technique and can sometimes be addressed through calibration.
- Uncertainty is incorporated into measurements as a range rather than a single value, and it is important to propagate uncertainties through calculations.
Measurement
Measurement involves assigning a number to an object's characteristic that can be compared to other objects. There are two main systems of measurement: the English system used in the U.S. which uses feet, pounds, and seconds, and the metric system used internationally which is based on units like meters, grams, and liters. Converting between units requires understanding the relationships between prefixes and moving decimals accordingly.
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This document discusses how to write uncertainties with measured data. It explains that uncertainties are written with the symbol "±" and provides examples. It outlines the two types of uncertainties - absolute and fractional. Absolute uncertainties are simply added when adding or subtracting quantities, while fractional uncertainties are added when multiplying or dividing quantities. Fractional uncertainties are calculated by dividing the absolute uncertainty by the measured value.
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The test will cover material from Chapter 10, including multiple choice, fill-in-the-blank, short answer, and calculation questions. Students should bring a calculator and be prepared to convert between temperature scales, use the heat equation q=mCpΔT, and calculate enthalpy changes from chemical reactions. Key terms, formulas, and a periodic table will be provided.
Measuring temperature
The document discusses different temperature scales and how thermometers work. It explains that the Fahrenheit scale was invented first and sets water's freezing point at 32 degrees and boiling point at 212 degrees. Later, Celsius was invented and set water's freezing point at 0 degrees and boiling point at 100 degrees. Thermometers work by measuring how the volume of a liquid changes with temperature in a bulb and narrow tube.
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Scientific notation and SI units are used in measurement to help scientists communicate measurements clearly across countries. The basic SI units include meters, kilograms, seconds, amperes, moles, candelas, and kelvins. Derived units are calculated from the basic units, such as newtons from kilograms and meters/seconds. SI prefixes modify the scale of units, from centi to giga. The precision of calculations is limited by the measurement with the fewest significant figures. Temperature in kelvins is calculated by adding 273 to degrees Celsius.
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Mass can be calculated using a balance scale by weighing an object against another item, or with an electric scale by measuring weight and recording results. Volume is the amount of matter an object can contain and can be calculated by using a graduated cylinder to measure displacement of water, or by measuring the length, width, and height of a rectangular prism.
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Mass measures the amount of matter in an object, while capacity measures how much a container can hold. The metric units for mass are grams and kilograms, with benchmarks being a paper clip for 1 gram and textbook for 1 kilogram. The metric units for capacity are milliliters and liters, with benchmarks being an eye dropper for 1 milliliter and large water bottle for 1 liter. Examples are provided to demonstrate using the appropriate metric units to measure common objects.
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The document provides notes on various lab measurement techniques including:
- Volume measurement using graduated cylinders and the displacement method
- Mass measurement using a triple beam balance in grams
- Temperature measurement using a thermometer in Celsius, Fahrenheit, or Kelvin
It also discusses metric unit conversions using the "King Henry" method where the number of metric "hops" determines where to place the decimal, and the factor label method using unit cancellation.
Metric System
The metric system is the standard system of measurement used by scientists. It uses units like meters, liters, and grams to measure length, volume, mass, weight, density, and temperature. Conversion between units uses dimensional analysis and conversion factors that equal 1. Common metric units include meters for length, liters and milliliters for volume, grams and kilograms for mass, Newtons for weight, and Celsius degrees for temperature.
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This document provides instructions and background information for conducting several science experiments. It discusses the key components of experiments including variables (factors that can be changed), manipulated variables (what is changed by the experimenter), responding variables (what is observed and measured), and control variables (factors kept the same). It then provides details on setting up and conducting experiments to test how different types of batteries affect flashlight brightness, what type of coffee cup keeps coffee warmest, and how light level, light color, and carbon dioxide affect the rate of photosynthesis in elodea plants. Students are instructed to make hypotheses, collect data, and analyze results.
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This document discusses standards of measurement and the metric system. It introduces the International System of Units (SI) and common SI prefixes used to denote multiplying factors of 10 when converting between units. Examples of converting between Kelvin, Celsius, meters, centimeters, and other units are provided. Guidance is given for reading measurement units and converting between larger and smaller units by moving the decimal point.
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The document discusses different types of weather and temperature scales. It describes common weather conditions like sunny, windy, rainy. It then explains the three main temperature scales - Celsius, Fahrenheit and Kelvin - including who invented them and how they work. Formulas are provided for converting between the different scales. Finally, there is a brief overview of different world climates.
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Power Notes Measurements and Dealing with Data 2
- 2. Assignment Log #1 Check Off Date Given Date Due Name of Assignment Possible Pts. Earned Pts. 1/24 1/30 Orientation Guide 35 1/23 2/1 E-Mail Me 40 1/30 1/31 Cornell Notes 70 1/31 2/1 (end of the period) Tools of the Trade 125 2/1 2/3 Power Notes – Measurement & Dealing w/Data 75
- 4. Notes In order to communicate effectively scientists around the world need to speak the same math language. The acceptable measurement system in chemistry is the International System of Measurements . This system is known as SI , short for the French term “ S ystem I nternational d’unites”. This system is the metric system and works in multiples of 10. Prefixes added to the base unit (gram, meter or liter) change the size of the base measurement. Zero Kelvin is called “absolute zero”. This is the temperature at which particles would actually stop moving. A type of matter known as Bose Einstein Condensates or BECs, have been cooled to this state.
- 5. Notes Celsius is the metric temperature unit we will be using in chemistry. To convert Celsius to Kelvin you just ADD 273 to whatever Celsius temperature you measure. Quantitative Science is concerned with measurements which analyze quantities of matter. There is no such thing as a “perfect” measurement as there is always some uncertainty in measurement . Limitations always exist due to the tools or the carelessness of the people making the measurement. Interactive Reader – Pg. 24 – Accuracy vs. Precision Estimation Digit – In this class we will be rounding to the nearest 100 th (2 places to the right of the decimal)
- 6. Collection of Data Tool Used to Measure Unit Label Graduated Cylinder (most accurate) Volume L Beaker Volume L Flask Volume L Meter Stick Volume cm3 Meter Stick Distance m Triple Beam Balance Mass g Electronic Scale Mass g Stop Watch Time s Thermometer Temperature C or K
- 7. Notes Analysis of Data Mathematical models: use equations and data to explain or predict things. Graphs: interpret what the data means; makes the relationship of numbers easier to see Variable = in science, something that may be changed or changed during an experiment Independent variable = the thing in an experiment that is changed by the scientist. (Time, Amount of Water, Type of Popcorn) Dependent variable = the thing in an experiment that changes because of what the scientist changed . (Distance, Growth of a plant, Number of Popped Cornels )
- 8. Notes Y Axis Dependent Variable X Axis Independent Variable
- 9. Notes Y Axis Dependent Variable X Axis Independent Variable A Direct Relationship between variables indicates that both the variables are either increasing or decreasing in the same direction . e.g. If the X variable is getting bigger so is the Y variable.
- 10. Notes Y Axis Dependent Variable X Axis Independent Variable An Indirect Relationship (inverse) between variables indicates that one variable is changing in the opposite direction than the other . e.g. If the X variable is getting bigger the Y variable is getting smaller…volume vs. pressure
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