Matter And Measurement 1 Matter and Measurement

Matter And Measurement 2 Length The measure of how much space an object occupies; The basic unit of length, or linear measure is the meters (m).

Matter And Measurement 3 Mass The basic unit of mass, or the amount of matter, is the kilograms (kg).

Matter And Measurement 4 Volume The most commonly used metric units for volume are the liter (L) and the milliliter (mL). □A liter is a cube 1 dm long on each side. □A milliliter is a cube 1 cm long on each side.

Matter And Measurement 5 Temperature: A measure of the average kinetic energy of the particles in a sample.

Matter And Measurement 6 Temperature In scientific measurements, the Celsius and Kelvin scales are most often used. The Celsius scale is based on the properties of water. □0  C is the freezing point of water. □100  C is the boiling point of water.

Matter And Measurement 7 Temperature The Kelvin is the SI unit of temperature. At 0 K,  C (absolute zero) all molecule motion theoretically stops. There are no negative Kelvin temperatures. K =  C

Matter And Measurement 8 Temperature The Fahrenheit scale is not used in scientific measurements.  F = 9/5(  C) + 32  C = 5/9(  F − 32)

Matter And Measurement 9 SI Units Système International d’Unités Uses different units and abbreviations for each quantity

Matter And Measurement 10 Metric System Prefixes help convert the base units into units that are appropriate for the item being measured.

Matter And Measurement 11 Metric System Conversions Factors King Henry Died ByBy drinking chocolate milk

Matter And Measurement 12 Dimensional Analysis Equality: An expression that says “this” equals “that” 1 hour 60 minutes Conversion factor : A ratio of the equivalent values in the equality 1 hour 60 minutes 60 minutes 1 hour = or

Matter And Measurement Dimensional Analysis Dimensional analysis : A method of problem-solving that helps convert between the units used to describe matter This “t-chart” format is the same as: # given units # find units ratio of equality/ conversion factor # given units # find units # given units x problem

Matter And Measurement Dimensional Analysis Example 1: Oak Ridge students attend school from 7:16 am until 2:35 pm. This is 7.32 hours a day. How many minutes is this? Given: 7.32 hours Equality: 1hour = 60 minutes Find: # minutes Ratios: 1 hour 60 minutes 60 minutes 1 hour 7.32 hours or 1 hour 60 minutes = 7.32 x 60 minutes 1 = minutes

Matter And Measurement 15 Dimensional Analysis/ Metric Conversions 1) A 5k (km) run is 3.1 miles. How many meters is this? 2) A 10k (km) run is 6.2miles. How many centimeters is this? = =

Matter And Measurement 16 More Conversion Problems 3) At 20 weeks a zygote is about 17cm. How many millimeters is this? 4) When eyes are dilated for an eye exam they expand 5 mm. How many cm is this? = =

Matter And Measurement 17 SCIENTIFIC NOTATION Because sometimes numbers are just too big or small to work with M. x 10 n base number exponent

Matter And Measurement 18 Scientific Notation x 10 3 Consists of a number with only ONE DIGIT to the LEFT of the decimal times some power of 10. base number exponent

Matter And Measurement 19 Standard Numeral to Scientific Notation: 1. Whole numbers will have: Positive power of 10, move decimal to left Examples: 8,500 = = 8.5 x 10 3

Matter And Measurement 20 Standard Numeral to Scientific Notation: 2. Decimal Numbers will have: negative power of 10; move decimal to right Examples: = = 7.89 x 10 -1

Matter And Measurement 21 Changing from Scientific Notation to Standard Numeral 1. If the exponent is (+): Move the decimal to the right! Examples: 1.5 x 10 3 = = 1500

Matter And Measurement If the exponent is (-): Move the decimal to the left. Examples: 2.63 x = = Changing from Scientific Notation to Standard Numeral

Matter And Measurement 23 MATHEMATICAL CALCULATIONS USING SCIENTIFIC NOTATION

Matter And Measurement 24 MULTIPLICATION A. Multiply base numbers B. Add powers of 10 Example: (1.5 x 10 3 ) ( 2.0 X 10 5 ) = 3.0 x 10 8

Matter And Measurement 25 DIVISION A. Divide base numbers B. Subtract powers of 10 (numerator - denominator) 4.0 x x 10 4 numerator denominator = 2.0 x 10 -2

Matter And Measurement 26 ADDITION AND SUBTRACTION *Exponents must be the SAME! (6.5 x 10 2 ) + (2.0 x 10 3 ) + (30.0 x 10 3 ) (0.65 x 10 3 ) + (2.0 x 10 3 ) + (30.0 x 10 3 ) x 10 3 = x 10 4

Matter And Measurement 27 Every answer should be written in correct scientific notation!! 632 x 10 2 = 6.32 x x 10 3 = 7.54 x 10 1 *Move decimal RIGHT = MORE NEGATIVE *Move decimal LEFT = MORE POSITIVE *ALL NUMBERS IN THE BASE NUMBER ARE SIGNIFICANT

Matter And Measurement 28 Uncertainty in Measurements Different measuring devices have different uses and different degrees of precision. The more subdivisions an instrument has, the more precise that instrument is.

Matter And Measurement 29 Which of the following is more precise? The one with more marks between the same numbers. A B

Matter And Measurement 30 Reading Instruments Step 1 - Read the measurement to the smallest subdivision of your instrument (Subdivision = the distance between two of the smallest lines) Step 2 - Estimate one more digit Example: What is the reading of the measurement below? _____ estimated digit

Matter And Measurement 31 Accuracy vs. Precision How close measurement comes to the true value of that measurement. How often you get the same measurement; reproducibility; consistent data. How close measurements are to each other

Matter And Measurement 32 Accuracy & Precision Examples Neither accurate nor precise Precise but not accurate Precise AND accurate

Matter And Measurement 33 Accuracy and Precision cont… Example: Three different groups of students (A, B, and C) measured the mass of the same piece of iron that has a known mass of 5.5 grams. Which set is both precise and accurate? _______ C

Matter And Measurement 34 Significant Figures The term significant figures refers to digits that were measured. When rounding calculated numbers, we pay attention to significant figures so we do not overstate the accuracy of our answers.

Matter And Measurement 35 Significant Figures 1.All non-zero digits are significant. 2.Zeroes in between two significant figures are themselves significant. 3.Zeroes at the beginning of a number are never significant. 4.Zeroes at the end of a number are significant if a decimal point is written in the number.

Matter And Measurement 36 Counting Significant Digits m m m x 10 3 m m 43,010 m All of these measurements contain 4 significant digits.

Matter And Measurement 37 Calculating Using Sig Figs 1.Multiplying & Dividing 1) Multiply or divide to get an answer 2) Round your answer to the LEAST number of SIGNIFICANT DIGITS Example: 8.02 x 0.43 = = _______ 3.4

Matter And Measurement 38 Calculation practice 18.4cm 2 / 2.30cm= 29.5 m x 3.1 m= x.00003=

Matter And Measurement 39 Calculating Using Sig Figs 2. Adding & Subtracting 1) Add or subtract to get an answer 2) Round your answer to the LEAST number of DECIMAL PLACES Example: = ________

Matter And Measurement 40 Calculation practice

Matter And Measurement 41 Which weighs more a ton of feathers or a ton of lead??? Density

Matter And Measurement 42 The ratio that compares the mass of an object to its volume It is an intensive physical property; Units: g/mL or g/cm 3 Density Density = Mass 0 Volume

Matter And Measurement 43 If substances do not mix, the less dense substance will float. Density 1) What is the density of substance A? _______ 2) What is the density of substance D? _______ 3) If an object with a density of 0.95 g/mL is dropped into the column where would it settle? __________________ Given the densities of the four liquids: 0.69 g/mL 1.26 g/mL

Matter And Measurement 44 A block of wood measures 3.2 cm by 4.5 cm by 6.1cm. When placed on the scale it weighs 29 g. What is the density? Density Example 1

Matter And Measurement 45 A marble weighs 15grams. When placed in a graduated cylinder that had a volume of 29 mL of water in it, the water level raised to 34 mL. What is the density of the marble? Density Example 2 Final Initial

Matter And Measurement 46 Pure Gold has a density of g/cm3. If you have a chunk of gold that weighs 52 grams, what is the volume? Density Example 3