Chemistry Basics Quiz
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Questions and Answers

What is a defining characteristic of gases?

  • They are compressible.
  • They maintain a fixed volume.
  • They have a defined shape.
  • They expand to fill their container. (correct)

Which of the following correctly describes chemical elements?

  • They cannot be broken down by ordinary means. (correct)
  • They are compounds of other chemical substances.
  • They can be decomposed into simpler substances.
  • They are mixtures of several substances.

Who is the scientist known for creating an early version of the periodic table?

  • Dmitri Mendeleev (correct)
  • Albert Einstein
  • John Dalton
  • Glenn Seaborg

How many elements are currently recognized in the periodic table?

<p>116 (D)</p> Signup and view all the answers

Which of the following statements about atoms is correct?

<p>Atoms are the smallest particles of an element with its chemical properties. (A)</p> Signup and view all the answers

What did Glenn Seaborg contribute to chemistry?

<p>He discovered 8 new elements. (A)</p> Signup and view all the answers

Which of the following substances is a mixture?

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

Which of these is an example of a pure substance?

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

What describes the particulate view of matter?

<p>Matter is made up of atoms and molecules in motion. (A)</p> Signup and view all the answers

Which statement is true regarding the states of matter?

<p>Solids and liquids can both be understood reasonably well. (C)</p> Signup and view all the answers

How are chemical reactions symbolically represented?

<p>Using chemical symbols and formulas. (B)</p> Signup and view all the answers

What characterizes solids compared to liquids?

<p>Solids cannot be compressed. (C)</p> Signup and view all the answers

Which of the following best explains the kinetic nature of matter?

<p>All forms of matter consist of particles in motion. (C)</p> Signup and view all the answers

What is the main difference between the macroscopic and particulate views of matter?

<p>The macroscopic view focuses on what can be seen. (C)</p> Signup and view all the answers

In which state of matter do the particles have a fixed shape?

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

Why do chemists use symbols to describe matter?

<p>To communicate universally across languages. (A)</p> Signup and view all the answers

What does density represent in physical properties?

<p>Mass per unit volume (A)</p> Signup and view all the answers

Which of the following is an example of a physical change?

<p>Boiling of water (C)</p> Signup and view all the answers

What is the density of a substance with a mass of 57.54 g and a volume of 6.4 cm³?

<p>9.0 g/cm³ (D)</p> Signup and view all the answers

What is true about density as a property of matter?

<p>Density is an intensive property (D)</p> Signup and view all the answers

How is volume calculated for objects with rectangular dimensions?

<p>Length × Height × Width (A)</p> Signup and view all the answers

Which of the following statements accurately describes melting?

<p>It is the transition of a solid to a liquid (D)</p> Signup and view all the answers

What is the formula for calculating percent error?

<p>% error = (Your value – Accepted value) x 100 / Accepted value (B)</p> Signup and view all the answers

What does a homogeneous mixture refer to?

<p>A mixture with uniform composition throughout (B)</p> Signup and view all the answers

Which of the following is an example of experimental error?

<p>Incorrect measurement from a faulty instrument (B)</p> Signup and view all the answers

What is indicated by the odor of a substance?

<p>Its chemical composition (A)</p> Signup and view all the answers

In terms of significant figures, how many are present in the number 0.0012300?

<p>5 (D)</p> Signup and view all the answers

Which statement about trailing zeros in significant figures is correct?

<p>Trailing zeros in a number with a decimal are considered significant. (D)</p> Signup and view all the answers

Which of the following statements about leading zeros is true?

<p>Leading zeros do not count as significant figures. (A)</p> Signup and view all the answers

What defines an extensive property?

<p>Depends on quantity of matter (C)</p> Signup and view all the answers

What is the mass of 95 mL of mercury, given its density of 13.6 g/cm³?

<p>1.3 x 10³ g (D)</p> Signup and view all the answers

How is a chemical change defined?

<p>Transformation of one substance into another (C)</p> Signup and view all the answers

Which measurement unit is NOT part of the SI units system?

<p>Feet for length (C)</p> Signup and view all the answers

What is the volume of mercury (in cm³) calculated from 95 mL?

<p>95 cm³ (A)</p> Signup and view all the answers

Which is NOT a characteristic of qualitative observations?

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

Which of the following temperature units is part of the SI system?

<p>Both B and C (A)</p> Signup and view all the answers

What conversion would you use to find the mass in pounds from grams when converting 1.3 x 10³ g?

<p>Divide by 454 (A)</p> Signup and view all the answers

What is the equivalent of 100˚C in Kelvin?

<p>373 K (D)</p> Signup and view all the answers

What is the boiling point of water in Fahrenheit?

<p>212 ˚F (A)</p> Signup and view all the answers

Which temperature scale has the same increment as degree Celsius?

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

If the body temperature of 37˚C is converted to Kelvin, what is the result?

<p>310 K (A)</p> Signup and view all the answers

What is the distance of the O—H bond in nanometers (nm)?

<p>0.0958 nm (D)</p> Signup and view all the answers

What is the freezing point of water in Celsius?

<p>0 ˚C (B)</p> Signup and view all the answers

What does precision in measurements refer to?

<p>The range of measurements (B)</p> Signup and view all the answers

Which of the following temperatures is equivalent to liquid nitrogen at -196˚C in Kelvin?

<p>77 K (D)</p> Signup and view all the answers

Flashcards

States of Matter

Matter exists in three states: solid, liquid, and gas. Solids have a fixed shape and volume, liquids have a fixed volume but take the shape of their container, and gases have no fixed shape or volume.

Chemistry's Approach

Chemistry explores the macroscopic world (what we can see) to understand the particulate worlds we can't see.

Kinetic Nature of Matter

Matter is made up of constantly moving atoms and molecules.

Symbolic Representation in Chemistry

Chemists use symbols to represent and describe the world of atoms and molecules, both visually and mathematically.

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Solids and Atomic Arrangement

Solids have a regular, repeating arrangement of atoms or molecules. This arrangement defines their shape and volume.

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Liquids and Atomic Arrangement

Liquids have a less defined structure than solids. Atoms or molecules move around, and can be described as a fluid arrangement.

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Gases and Atomic Arrangement

Gases have no defined shape or volume. Atoms or molecules are widely spaced and move freely. Their behavior can be more difficult to predict due to their high energy.

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What is a key characteristic of gases?

Gases expand to fill their container. This means they take the shape and volume of their container.

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What is a chemical element?

A pure substance that cannot be broken down into simpler substances by ordinary chemical means.

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What is the periodic table?

Elements are arranged in a table based on their properties and atomic number.

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What information does the periodic table provide?

The periodic table contains a comprehensive list of elements with their unique chemical properties.

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Who is credited with organizing the first periodic table?

Dmitri Mendeleev organized the first periodic table, laying the foundation for understanding the relationships between elements.

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Who is Glenn Seaborg and what is he known for?

Glenn Seaborg discovered eight new elements and was the only living person to have an element named after him.

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What is an atom?

The smallest particle of an element that retains the chemical properties of that element.

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How many elements are on the periodic table?

The periodic table contains over 100 elements, each with its unique properties.

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Intensive Property

A property that does not depend on the amount of matter present. Examples include temperature, density, and boiling point.

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Extensive Property

A property that depends on the amount of matter present. Examples include mass, volume, and length.

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Density

The ratio of mass to volume. It tells us how much mass is packed into a given space.

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Chemical Change

A change that alters the chemical composition of a substance. Typically, this is irreversible.

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Qualitative Observation

Observations that describe the characteristics of a substance, but do not involve numerical measurements. Examples include color, shape, and odor.

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Quantitative Measurement

Observations that involve numerical measurements. Examples include mass, volume, and temperature.

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SI Units

A system of units commonly used in science, based on the metric system.

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Millimeter (mm)

A unit of measurement equal to one-thousandth of a meter (1 mm = 0.001 m).

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Nanometer (nm)

One billionth of a meter (1 nm = 1.0 x 10^-9 m).

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Celsius Scale

A scale used to measure temperature, where water freezes at 0 degrees Celsius and boils at 100 degrees Celsius.

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Fahrenheit Scale

A scale used to measure temperature, where water freezes at 32 degrees Fahrenheit and boils at 212 degrees Fahrenheit.

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Kelvin Scale

A scale used to measure temperature where absolute zero is 0 Kelvin. Kelvin units are the same size as Celsius units.

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Precision

A measure of the agreement between repeated measurements.

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Accuracy

A measure of how close a measurement is to the true or accepted value.

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Error

The difference between a measured value and the accepted value.

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Melting and Boiling Point

A physical property that describes a substance's ability to change from a solid to a liquid (melting) or from a liquid to a gas (boiling). It depends on the temperature at which these changes occur.

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Atomic Structure

The arrangement of atoms or molecules in a substance, particularly in a solid. This arrangement affects the substance's physical properties.

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Physical Property

A physical property of matter that can be observed or measured without changing the substance's chemical composition.

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Solution

A homogeneous mixture where one substance (solute) is dissolved evenly into another (solvent).

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Percent Error

A measure of how close an experimental value is to the accepted value, expressed as a percentage.

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Experimental Error

Error that results from mistakes made during an experiment, such as misreading measurements or incorrect calculations.

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Laboratory Error

Error that is inherent in the method or equipment used in an experiment, such as limitations in the precision of measuring instruments.

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Significant Figures

Digits in a measurement that reflect the certainty of the measurement and contribute to its accuracy.

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Leading Zeros

Zeroes to the left of the first non-zero digit in a number are not significant because they simply indicate the location of the decimal point.

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Study Notes

Chemistry and Chemical Reactivity 6th Edition, Chapter 1: Matter and Measurement

  • The book is titled Chemistry and Chemical Reactivity, 6th edition, written by John C. Kotz, Paul M. Treichel, and Gabriela C. Weaver.
  • The chapter is titled Matter and Measurement.
  • The lectures were written by John Kotz.
  •  Matter is anything that occupies space and has mass.
  • Chemistry explores the macroscopic world—what we see—to understand the particulate worlds we cannot see.
  • Symbols are used to describe these worlds.
  •  A chemist's view of matter involves macroscopic, particulate, and symbolic representations.
  • Matter exists in three states: solid, liquid, and gas.
  • Solids have a rigid shape and fixed volume.
  • Liquids have no fixed shape but fill a container completely.
  • Gases expand to fill their container.
  •  Solids are reasonably well understood, liquids are not well understood, and gases have a good theoretical understanding.
  • Matter is classified into heterogeneous and homogeneous matter.
  • Heterogeneous matter has a nonuniform composition, while homogeneous matter has a uniform composition throughout.
  • Pure substances have a fixed composition and cannot be further purified.
  • Compounds are elements united in fixed ratios.
  • Solutions are homogeneous mixtures with uniform compositions that can vary widely.
  •  Chemical elements are pure substances that cannot be broken down into other substances by ordinary means.
  •  Elements are found on the periodic table.
  • There are 116 elements.
  • Glenn Seaborg discovered 8 new elements.
  • An atom is the smallest particle of an element with the chemical properties of that element.
  • Atoms consist of a nucleus (of protons and neutrons) and electrons in space surrounding the nucleus.
  • Chemical compounds are composed of atoms and can be decomposed into those atoms.
  •  A molecule is the smallest unit of a compound that retains the chemical characteristics of the compound.
  •  Molecular formulas are used to describe the composition of molecules.
  • Elements form compounds by combining.
  •  Chemists study the nature of matter and how it relates to its atoms and molecules.
  • Physical properties include color, melting and boiling point, and odor.
  •  Density is a physical property equal to mass divided by volume.
  • Density is an intensive property and does not depend on the quantity of matter.
  • Intensive properties are contrasted with extensive properties which depend on the quantity of matter present, like mass and volume.
  • Calculations involving temperature often require using kelvins.
  • The formula for converting Celsius to Kelvin is T (K) = t (°C) + 273.15.
  • Precision refers to the agreement of multiple measurements.
  • Accuracy measures how close a measurement is to the accepted value.
  • Error includes experimental error and laboratory error.
  • Significant figures reflect measurement accuracy. Rules for determining significant figures are provided.

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Description

Test your knowledge on the fundamental concepts of chemistry, including the states of matter, atomic structure, and the periodic table. This quiz will challenge your understanding of both macroscopic and particulate views of matter, as well as chemical elements and reactions.

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