Chemistry Chapter 1: Chemical Foundations
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Questions and Answers

What is the correct conversion formula from Celsius to Fahrenheit?

  • $F = 1.8C + 32$ (correct)
  • $F = 1.8C - 32$
  • $F = C + 32$
  • $F = C imes 32$

    • What is the boiling point of liquid nitrogen in Kelvin?

  • 100 K
  • 77 K (correct)
  • 150 K
  • 273 K

    • Which temperature represents the same value on both the Celsius and Fahrenheit scales?

  • 0°C
  • -40°C (correct)
  • 100°C
  • -100°C

    • What is the symbol for temperature in Kelvin?

    <p>K (D)</p> Signup and view all the answers

    In terms of zero points, how do the Kelvin and Celsius scales differ?

    <p>Kelvin is 273 units higher than Celsius at zero. (B)</p> Signup and view all the answers

    Which of the following is correct about the Celsius and Kelvin scales?

    <p>Their size of temperature units is the same. (C)</p> Signup and view all the answers

    What is the formula to convert from Kelvin to Celsius?

    <p>$C = K - 273$ (C)</p> Signup and view all the answers

    In the Fahrenheit scale, what would be a full conversion of a temperature of -40°F to Celsius?

    <p>-40°C (A)</p> Signup and view all the answers

    What is the metric unit equivalent to one pound?

    <p>0.4536 grams (C)</p> Signup and view all the answers

    Which of these prefixes denotes a factor of one billion?

    <p>Giga (C)</p> Signup and view all the answers

    If an object has a mass of 5.67 grams, how many significant figures does this measurement have?

    <p>4 (A)</p> Signup and view all the answers

    What is the correct scientific notation for the number 0.00045?

    <p>4.5 x 10^-4 (C)</p> Signup and view all the answers

    Which temperature degree scale is based on the absolute zero concept?

    <p>Kelvin (B)</p> Signup and view all the answers

    In the SI system, which unit is used to measure the amount of substance?

    <p>mole (D)</p> Signup and view all the answers

    How would you express 1500 in scientific notation?

    <p>1.5 x 10^3 (D)</p> Signup and view all the answers

    Which of the following is not a base unit in the Metric SI system?

    <p>Liter (B)</p> Signup and view all the answers

    What is the primary advantage of using exponential notation?

    <p>It simplifies the representation of very large or small numbers. (B)</p> Signup and view all the answers

    When multiplying two measurements, how is the number of significant figures in the result determined?

    <p>By using the measurement with the least number of significant figures. (C)</p> Signup and view all the answers

    How many significant figures are in the number 0.000060?

    <p>2 (B)</p> Signup and view all the answers

    In the result of the calculation 25 × 5 = 125, how many significant figures should the final answer have?

    <p>2 (D)</p> Signup and view all the answers

    Which of the following numbers accurately represented in scientific notation has one significant figure?

    <p>6 × 10⁻³ (B)</p> Signup and view all the answers

    If a calculation yields a result of 754, with significant figures taken from inputs of 25 and 50, how should the result be expressed?

    <p>750 (A)</p> Signup and view all the answers

    Which of these measurements would have four significant figures?

    <p>50.00 (C)</p> Signup and view all the answers

    Identify the correct representation of a number with three significant figures in scientific notation.

    <p>8.00 × 10⁻³ (D)</p> Signup and view all the answers

    Flashcards

    Significant Figures

    Digits in a number that contribute to its precision.

    Exponential Notation

    A way to express numbers using powers of ten.

    Advantages of Exponential Notation

    Simplifies the representation of significant figures.

    Multiplication Rule for Significant Figures

    Result has the same significant figures as the least precise measurement.

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    Division Rule for Significant Figures

    Similar to multiplication, the result follows the least precision.

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    Zeroes in Significant Figures

    Leading zeros do not count, but trailing zeros do in decimal numbers.

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    Limiting Term

    The measurement in a calculation that has the least significant figures.

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    Adding Significant Figures

    The result should be reported to the least number of decimal places.

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    SI Unit

    The International System of Units used for measurements.

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    Gram

    A basic unit of mass in the metric system equivalent to a pound in the imperial system.

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    Meter

    The fundamental unit of length in the metric system.

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    Kinetic Energy

    The energy an object possesses due to its motion.

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    Prefixes in SI System

    Symbols attached to units to indicate scale, such as kilo-, milli-, etc.

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    Micro

    A metric prefix indicating one-millionth (10^-6).

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    Mole (mol)

    A unit in chemistry that measures quantity of substance.

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    Candela (cd)

    The SI unit of luminous intensity, measuring the brightness of light.

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    Celsius scale

    A temperature scale where water freezes at 0°C and boils at 100°C.

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    Kelvin scale

    An absolute temperature scale starting at absolute zero, where 0 K is equivalent to -273.15°C.

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    Fahrenheit scale

    A temperature scale commonly used in engineering, where water freezes at 32°F and boils at 212°F.

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    Temperature conversion

    The process of converting temperature from one scale to another.

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    -40°C and -40°F

    These two temperatures are equivalent on their respective scales.

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    Conversion formulas

    Equations used to convert between Celsius, Kelvin, and Fahrenheit.

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    Normal body temperature

    Typically around 37°C, 98.6°F, or 310 K.

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    Liquid nitrogen boiling point

    The boiling point of liquid nitrogen is 77 K or -196°C.

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    Study Notes

    Chemistry - Chapter 1: Chemical Foundations

    • Chemistry is the study of matter and its changes.
    • Matter is composed of atoms.
    • Atoms are the smallest particle that retains the properties of an element.
    • Individual atoms are observable via scanning tunneling microscopes (STMs).
    • Elements combine to form new substances.
    • Water is composed of two hydrogen atoms and one oxygen atom.
    • Chemical elements can exist as diatomic molecules (two-atom molecules).
    • The decomposition of water can be represented as 2H₂O → 2H₂ + O₂

    The Scientific Method

    • Science uses a framework for organizing and gaining knowledge.
    • Procedure for processing and understanding information.
    • The scientific method lies at the center of scientific inquiry and varies based on the problem and investigator.
    • Steps in the scientific method:
      • Make observations (qualitative and quantitative).
      • Formulate a hypothesis (possible explanation).
      • Perform experiments to test the hypothesis.
      • Gather new information to assess validity.
      • Experiments often lead to new observations, requiring further inquiry within the process.
    • Scientific models (or theories) are sets of tested hypotheses that explain natural phenomena.
    • Models explain why nature behaves in a specific way.
    • Models are constantly refined or replaced as more information becomes available, and they explain natural phenomenon using human experiences.
    • Natural law summarizes observed measurable behavior.
    • Example: The law of conservation of mass. The total mass of materials is unchanged during a chemical change.
    • Laws versus theories: A law states what consistently happens; a theory explains why it happens.

    Units of Measurement

    • Measurement consists of a number and a unit of scale.
    • Standard systems of units include English and metric systems.
    • The SI system (International System) is based on the metric system and internationally used in scientific work.
    • Fundamental SI units include kilogram (mass), meter (length), second (time), kelvin (temperature), ampere (electric current), mole (amount of substance), and candela (luminous intensity).
    • Prefixes are used to denote multiples or submultiples of SI units.
    • Common units for length, mass, and volume are included in examples.

    Uncertainty in Measurement

    • Measurements possess inherent uncertainty.
    • Certain digits are numbers with no uncertainty.
    • Uncertain digits, which must be estimated, vary.
    • Reporting measurements: Record all certain digits plus the first uncertain digit.
    • The measurement result depends on the precision of the device used..
    • Uncertainty in last digits is +/- 1, unless otherwise specified.
    • Accuracy reflects agreement with the true value; precision reflects reproducibility.
    • Random errors have equal probability of being high or low; are associated with the measurement device; often involve estimating the last digit.
    • Systematic errors consistently occur in the same direction, showing bias.

    Significant Figures

    • Significant figures (sig figs) indicate precision in a measurement.
    • Rules for counting significant figures
      • Nonzero integers are always significant figures.
      • Zeros between nonzero digits (captive zeros) are significant.
      • Trailing zeros in a number containing a decimal point are significant.
      • Leading zeros are not significant.
    • Exact numbers have infinite sig figs (determined by counting).
    • Operations for Calculations: Multiply/Divide - Lowest sig figs in calculation used gives the answer with appropriate precision. Add/Subtract- lowest decimal place is the correct number of decimal place to express the answer.

    Dimensional Analysis

    • Used to convert between units of measurement.
    • Equivalence statements relate different units.
    • Unit factors are derived with the direction of change to cancel unwanted units.
    • Multiply the value to be converted by the unit factor to find the value in the desired units.
    • Use provided equivalence statements to complete conversions.

    Temperature

    • Celsius and Kelvin scales are commonly used in physics.
    • Fahrenheit is frequently used in engineering.
    • Temperature conversions are provided to convert between scales (e.g. given Degrees Celsius, and convert to degrees Fahrenheit).

    Density

    • Density is the mass per unit volume, providing an identification tag for substances.
    • It represents the quantity of matter in a specific volume.
    • Density of liquids can be determined by weighing a known volume.
    • Example of calculating density given mass and volume.

    Classification of Matter

    • Matter occupies space and possesses mass.
    • Matter exists in three states (solid, liquid, and gas).
    • Solids are rigid with fixed volume and shape; slightly compressible.
    • Liquids have definite volume but conform to container shape, with slight compressibility.
    • Gases take on both the shape and volume of the container; most highly compressible.
    • Mixtures can be homogeneous or heterogeneous, have variable composition, and can be separated into pure components.
    • Pure substances, either elements or compounds, have fixed compositions.
    • Elements cannot be decomposed chemically, while compounds can be broken down into elements.
    • Methods for separating mixture components include filtration, distillation, and chromatography.

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    Description

    Explore the fundamental principles of chemistry in this quiz covering the basics of chemical foundations. Understand the nature of matter, the composition of atoms, and the scientific method used in scientific inquiry. Prepare to dive into essential concepts such as atoms, elements, and water decomposition.

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