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Unit 1: Foundations of Chemistry

Unit 1: Foundations of Chemistry. Chapters 1, 2, & 3 Chemistry 1L Cypress Creek High School. Table of Contents. Chapter 1: Introduction to Chemistry 1.2: Chemistry & Matter 1.3: Scientific Method Chapter 2: Data Analysis 2.1: Units of Measurement

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Unit 1: Foundations of Chemistry

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  1. Unit 1: Foundations of Chemistry Chapters 1, 2, & 3 Chemistry 1L Cypress Creek High School

  2. Table of Contents • Chapter 1: Introduction to Chemistry • 1.2: Chemistry & Matter • 1.3: Scientific Method • Chapter 2: Data Analysis • 2.1: Units of Measurement • 2.2: Scientific Notation & Dimensional Analysis • 2.3: How Reliable are Measurements? • 2.4: Representing Data • Chapter 3: Matter – Properties & Changes • 3.1: Properties of Matter • 3.2: Changes in Matter

  3. 1.2 Chemistry & Matter Composition, Structure, and Behavior • Chemistry is the science that investigates and explains the structure and properties of matter. • Matter is anything that takes up space and has mass. • Mass is the measure of the amount of matter that an object contains. • The structure of matter refers to its composition—what matter is made of—as well as how matter is organized. • The properties of matter describe the characteristics and behavior of matter, including the changes that matter undergoes.

  4. 1.3 Scientific Method Scientific Methods • A scientific method is a systematic approach to answer a question or study a situation. • It is both an organized way for scientists to do research and a way for scientists to verify the work of other scientists. • A typical scientific method includes: • making observations, • forming a hypothesis, • performing an experiment, • and arriving at a conclusion.

  5. 1.3 Scientific Method Scientific Methods • Often, a scientist will begin with qualitative data—information that describes some physical characteristic that relates to the five senses. • Chemists also use numerical quantitative data. • A hypothesis is a possible explanation for what has been observed. • An experiment is a set of controlled observations that test a hypothesis. • The variable that is changed in an experiment is called the independent variable. • The variable that you watch to see how it changes as a result of your changes to the independent variable is called the dependent variable.

  6. 1.3 Scientific Method Scientific Methods • Many experiments also include a control, which is a standard for comparison. • A conclusion is a judgment based on the data obtained in the experiment. • If data support a hypothesis, the hypothesis is tentatively affirmed. Hypotheses are never proven; they are always subject to additional research.

  7. 2.1 Units of Measurement SI Units • Scientists need to report data that can be reproduced by other scientists. • In 1795, French scientists adopted a system of standard units called the metric system. • In 1960, an international committee of scientists met to update the metric system. • The revised system is called the Système Internationale d’Unités, which is abbreviated SI. • There are seven base units in SI. • A base unit is a defined unit in a system of measurement that is based on an object or event in the physical world. • A base unit is independent of other units.

  8. 2.1 Units of Measurement Base Units

  9. 2.1 Units of Measurement Time

  10. 2.1 Units of Measurement Length & Mass • The SI base unit for length is the meter (m). • A meter is the distance that light travels through a vacuum in 1/299 792 458 of a second. • A vacuum is a space containing no matter. • A meter, which is close in length to a yard, is useful for measuring the length and width of a room. • Recall that mass is a measure of the amount of matter. • The SI base unit for mass is the kilogram (kg). • A kilogram is about 2.2 pounds. The kilogram is defined by a platinum-iridium metal cylinder.

  11. 2.1 Units of Measurement Measuring Matter • The mole, commonly abbreviated mol, is the SI base unit used to measure the amount of a substance. • It is the number of representative particles, carbon atoms, in exactly 12 g of pure carbon-12. • Through years of experimentation, it has been established that a mole of anything contains 6.022 136 7 x 1023 representative particles. • A representative particle is any kind of particle such as atoms, molecules, formula units, electrons, or ions. Click box to view movie clip.

  12. 2.1 Units of Measurement Measuring Matter • The number 6.022 136 7 x 1023 is called Avogadro’s number in honor of the Italian physicist and lawyer Amedeo Avogadro who, in 1811, determined the volume of one mole of a gas. • If you write out Avogadro’s number, it looks like this. • 602 000 000 000 000 000 000 000

  13. 2.1 Units of Measurement Measuring Matter • One-mole quantities of three substances are shown, each with a different representative particle. • The representative particle in a mole of water is the water molecule. • The representative particle in a mole of copper is the copper atom.

  14. 2.1 Units of Measurement Derived Units • Not all quantities can be measured with base units. • A unit that is defined by a combination of base units is called a derived unit. • Two quantities that are measured in derived units are volume and density.

  15. 2.1 Units of Measurement Volume  • Volume is the space occupied by an object. • The derived unit for volume is the cubic meter, which is represented by a cube whose sides are all one meter in length, the more useful unit for volume is the cubic centimeter (cm3). • The metric unit for volume equal to one cubic decimeter is a liter (L). • Liters are used to measure the amount of liquid in a container of bottled water or a carbonated beverage. • One liter has about the same volume as one quart.

  16. 2.1 Units of Measurement Density • Density is a ratio that compares the mass of an object to its volume. • The units for density are often grams per cubic centimeter (g/cm3). • Density is a property that can be used to identify an unknown sample of matter. Every sample of pure aluminum has the same density.

  17. 2.1 Units of Measurement Temperature Scales • Scientists use two temperature scales. • The Celsius scale uses the temperatures at which water freezes and boils to establish the scale because these temperatures are easy to reproduce. • The freezing point is 0 and the boiling point is 100. • The distance between these points are divided into 100 equal units, or degrees Celsius.

  18. 2.1 Units of Measurement Temperature Scales • A kelvin (K) is the SI base unit of temperature. • On the Kelvin scale, water freezes at about 273 K and boils at about 373 K. • It is easy to convert from the Celsius scale to the Kelvin scale. • To convert temperatures reported in degrees Celsius into kelvins, you just add 273.

  19. 2.3 How Reliable are Measurements? Accuracy and Precision • When scientists make measurements, they evaluate both the accuracy and the precision of the measurements. • Accuracy refers to how close a measured value is to an accepted value. • Precision refers to how close a series of measurements are to one another.

  20. 2.3 How Reliable are Measurements? Significant Figures  • Scientists indicate the precision of measurements by the number of digits they report. • A value of 3.52 g is more precise than a value of 3.5 g. • The digits that are reported are called significant figures. • Significant figures include all known digits plus one estimated digit.

  21. 2.3 How Reliable are Measurements? Rules for Significant Figures • Non-zero numbers are always significant. • Zeros between non-zero numbers are always significant. • All final zeros to the right of the decimal place are significant. • Zeros that act as placeholders are not significant. Convert quantities to scientific notation to remove the placeholder zeros. • Counting numbers and defined constants have an infinite number of significant figures.

  22. 2.3 How Reliable are Measurements? Applying Significant Figure Rules • Determine the number of significant figures in the following masses. • Count all non-zero numbers (rule 1), zeros between non-zero numbers (rule 2), and final zeros to the right of the decimal place (rule 3). Ignore zeros that act as placeholders (rule 4).

  23. 2.3 How Reliable are Measurements? Rules for Rounding Numbers • If the digit to the immediate right of the last significant figure is less than five, do not change the last significant figure. • If the digit to the immediate right of the last significant figure is greater than five, round up the last significant figure. • If the digit to the immediate right of the last significant figure is equal to five and is followed by a nonzero digit, round up the last significant figure. • If the digit to the immediate right of the last significant figure is equal to five and is not followed by a nonzero digit, look at the last significant figure. If it is an odd digit, round it up. If it is an even digit, do not round up.

  24. 2.3 How Reliable are Measurements? Addition and Subtraction • When you add or subtract measurements, your answer must have the same number of digits to the right of the decimal point as the value with the fewest digits to the right of the decimal point. • The easiest way to solve addition and subtraction problems is to arrange the values so that the decimal points line up. • Then do the sum or subtraction. Identify the value with the fewest places after the decimal point. • Round the answer to the same number of places.

  25. 2.3 How Reliable are Measurements? Multiplication and Division • When you multiply or divide numbers, your answer must have the same number of significant figures as the measurement with the fewest significant figures.

  26. 2.2 Scientific Notation & Dimensional Analysis Scientific Notation • Scientific notation expresses numbers as a multiple of two factors: a number between 1 and10; and ten raised to a power, or exponent. • The exponent tells you how many times the first factor must be multiplied by ten. • When numbers larger than 1 are expressed in scientific notation, the power of ten is positive. • When numbers smaller than 1 are expressed in scientific notation, the power of ten is negative.

  27. 2.2 Scientific Notation & Dimensional Analysis Using Multiple Conversion Factors • It is common in scientific problems to use dimensional analysis to convert more than one unit at a time. • For example, what is a speed of 550 meters per second in kilometers per minute? • First convert meters to kilometers. Set up the conversion factor so that the meter units will cancel out. • Next convert seconds to minutes. Set up the conversion factor so that the seconds cancel out.

  28. 2.2 Scientific Notation & Dimensional Analysis Convert Data into Scientific Notation • Change the following data into scientific notation. • The diameter of the Sun is 1 392 000 km. • The density of Sun’s atmosphere is 0.000 000 028 g/cm3. • Move the decimal point to produce a factor between 1 and 10. Count the number of places the decimal point moved and the direction. • Remove the extra zeros at the end or beginning of the factor. • Multiply the result by 10n where n equals the number of places moved. • Remember to add units to the answers.

  29. 2.2 Scientific Notation & Dimensional Analysis Adding and Subtracting Using Scientific Notation  • When adding or subtracting numbers written in scientific notation, you must be sure that the exponents are the same before doing the arithmetic. • Suppose you need to add 7.35 x 102 m + 2.43 x 102 m. • You note that the quantities are expressed to the same power of ten. You can add 7.35 and 2.43 to get 9.78 x 102 m. • If the quantities are not expressed to the same power of ten, change one of the numbers to match the power of ten of the other number.

  30. 2.2 Scientific Notation & Dimensional Analysis Multiplying and Dividing Using Scientific Notation  • Multiplying and dividing also involve two steps, but in these cases the quantities being multiplied or divided do not have to have the same exponent. • For multiplication, you multiply the first factors. Then, you add the exponents. • For division, you divide the first factors. Then, you subtract the exponent of the divisor from the exponent of the dividend.

  31. 2.2 Scientific Notation & Dimensional Analysis A Problem Solving Strategy • When you analyze a problem, you first separate what is known from what is unknown. • Then you decide on a strategy that uses the known data to solve for the unknown. • After you solve a problem, you need to evaluate your answer to decide if it makes sense.

  32. 2.2 Scientific Notation & Dimensional Analysis A Problem Solving Strategy

  33. 2.2 Scientific Notation & Dimensional Analysis A Problem Solving Strategy

  34. 2.2 Scientific Notation & Dimensional Analysis A Problem Solving Strategy

  35. 2.2 Scientific Notation & Dimensional Analysis Dimensional Analysis • Dimensional analysis is a method of problem-solving that focuses on the units used to describe matter. • For example, if you want to convert a temperature in degrees Celsius to a temperature in kelvins, you focus on the relationship between the units in the two temperature scales. • A conversion factor is a ratio of equivalent values used to express the same quantity in different units.

  36. 2.2 Scientific Notation & Dimensional Analysis Dimensional Analysis • A conversion factor is always equal to 1. • Because a quantity does not change when it is multiplied or divided by 1, conversion factors change the units of a quantity without changing its value. • Dimensional analysis often uses conversion factors. • Suppose you want to know how many meters are in 48 km. • You need a conversion factor that relates kilometers to meters. • You know that 1 km is equal to 1000 m. • Because you are going to multiply 48 km by the conversion factor, you want to set up the conversion factor so the kilometer units will cancel out.

  37. 2.4 Representing Data Graphing • Using data to create a graph can help to reveal a pattern if one exists. • A graph is a visual display of data.

  38. 2.4 Representing Data Circle Graphs • A circle graph is sometimes called a pie chart because it is divided into wedges like a pie or pizza. • A circle graph is useful for showing parts of a fixed whole. • The parts are usually labeled as percents with the circle as a whole representing 100%.

  39. 2.4 Representing Data Bar Graph • A bar graph often is used to show how a quantity varies with factors such as time, location, or temperature. • In those cases, the quantity being measured appears on the vertical axis (y-axis). • The independent variable appears on the horizontal axis (x-axis). • The relative heights of the bars show how the quantity varies.

  40. 2.4 Representing Data Line Graphs • In chemistry, most graphs that you create and interpret will be line graphs. • The points on a line graph represent the intersection of data for two variables. • The dependent variable is plotted on the y-axis. • Remember that the independent variable is the variable that a scientist deliberately changes during an experiment.

  41. 2.4 Representing Data Line Graphs • Sometimes points are scattered, the line cannot pass through all the data points. • The line must be drawn so that about as many points fall above the line as fall below it. • This line is called a best fit line.

  42. 2.4 Representing Data Interpreting Graphs • An organized approach can help you understand the information on a graph. • First, identify the independent and dependent variables. • Decide if the relationship between the variables is linear or nonlinear. • If the relationship is linear, is the slope positive or negative? • If a graph has multiple lines or regions, study one area at a time. • You can extend the line beyond the plotted points and estimate values for the variables. • This process is called extrapolation.

  43. 3.1 Properties of Matter Physical Properties • Physical properties are characteristics that a sample of matter exhibits without any change in its identity. • Density, taste, color, hardness, odor, melting point, and boiling point are common physical properties that scientists record as identifying characteristics of a substance.

  44. 3.1 Properties of Matter Extensive and Intensive Properties  • Physical properties can be further described as being one of two types. • Extensive properties are dependent upon the amount of substance present. • Length and volume are also extensive properties. • Intensive properties are independent of the amount of substance present. • For example, density of a substance is the same no matter how much substance is present.

  45. 3.1 Properties of Matter Chemical Properties of Matter • The ability of a substance to combine with or change into one or more other substances is called a chemical property. • Every substance has its own unique set of physical and chemical properties. • Observations of properties may vary depending on the conditions of the immediate environment. • It is important to state the specific conditions in which observations are made because both chemical and physical properties depend on temperature and pressure.

  46. 3.2 Changes of Matter Physical Changes • A physical change is a change in matter that does not involve a change in the chemical identity of individual substances. • Examples include: boiling, freezing, melting, dissolving, evaporating, and crystallizing. • When you encounter terms such as boil, freeze, condense, vaporize, or melt in your study of chemistry, the meaning generally refers to a phase change in matter.

  47. 3.2 Changes of Matter Chemical Properties • Chemical properties are those that can be observed only when there is a change in the composition of the substance. • A chemical property always relates to a chemical change, the change of one or more substances into other substances. • Another term for chemical change is chemical reaction.

  48. 3.2 Changes of Matter Chemical Changes Click box to view movie clip.

  49. 3.2 Changes of Matter Chemical Changes • The new substances formed in the reaction have different compositions and different properties from the substances present before the reaction occurred. • When a freshly exposed iron surface is left in contact with air, it slowly changes into a new substance, namely, the rust. • In chemical reactions, the starting substances are called reactants and the new substances that are formed are called products.

  50. 3.2 Changes of Matter Chemical Reactions andEnergy • All chemical changes also involve some sort of energy change. • Energy is either taken in or given off as the chemical change takes place. • Chemical reactions that give off heat energy are called exothermic reactions. • Chemical reactions that absorb heat energy are called endothermic reactions. • Photosynthesis is probably the most important endothermic process on Earth.

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