Chemistry: Chapter 1 - Matter, Measurement, and Problem Solving

Vocabulary flashcards covering key definitions, scientific methods, units of measurement, properties, and classifications of matter from Chapter 1.

Chemistry

The science that seeks to understand the behavior of matter by studying the behavior of atoms and molecules.

Atoms

Submicroscopic particles that constitute the fundamental building blocks of ordinary matter.

Molecules

Particles formed when two or more atoms bind together in specific geometrical arrangements.

Empirical Approach

An approach to scientific knowledge that is based on observation and experiment.

Observations

Descriptions about the characteristics or behavior of nature, also known as data.

Hypothesis

A tentative interpretation or explanation of observations that is falsifiable through experiment.

Scientific Law

A brief statement that summarizes past observations and predicts future ones.

Law of Conservation of Mass

A scientific law stating that in a chemical reaction, matter is neither created nor destroyed.

Scientific Theory

A well-established model for the way nature is that tries to explain not merely what nature does, but why.

Matter

Anything that occupies space and has mass.

Solid Matter

A state of matter in which atoms or molecules pack close to each other in fixed locations, resulting in a fixed volume and rigid shape.

Crystalline Solid

Solid matter whose atoms or molecules are arranged in patterns with long-range, repeating order.

Amorphous Solid

Solid matter whose atoms or molecules do not have any long-range order.

Liquid Matter

A state of matter in which atoms or molecules pack closely but are free to move relative to each other, giving it a fixed volume but no fixed shape.

Gaseous Matter

A state of matter in which atoms or molecules have a lot of space between them and are free to move relative to one another, making it compressible.

Pure Substance

A substance made up of only one component whose composition is invariant.

Mixture

A substance composed of two or more components in proportions that can vary from one sample to another.

Element

A pure substance that cannot be chemically broken down into simpler substances.

Compound

A pure substance composed of two or more elements in fixed definite proportions.

Heterogeneous Mixture

A mixture in which the composition varies from one region of the mixture to another.

Homogeneous Mixture

A mixture composed of multiple substances that mix uniformly so that all portions have the same composition and properties.

Decanting

A method of separating a mixture by carefully pouring off a liquid into another container.

Distillation

A separation technique for homogeneous liquid mixtures where heating boils off the most volatile component, which is then recondensed and collected.

Volatile

Describing a substance that is easily vaporizable.

Filtration

A process in which a mixture of an insoluble solid and a liquid is poured through filter paper in a funnel to trap the solid.

Physical Change

A change that alters only the state or appearance of a substance without altering its chemical composition.

Chemical Change

A change that alters the composition of matter by rearranging atoms to form different substances.

Physical Property

A property that a substance displays without changing its composition, such as odor, color, melting point, or density.

Chemical Property

A property that a substance displays only by changing its composition via a chemical reaction, such as flammability, acidity, or toxicity.

Energy

The capacity to do work.

Work

The action of a force through a distance.

Kinetic Energy

The energy associated with the motion of an object.

Potential Energy

The energy associated with the position or composition of an object.

Thermal Energy

The type of kinetic energy associated with the temperature of an object, arising from the motion of its constituent atoms or molecules.

Law of Conservation of Energy

A fundamental law stating that energy is always conserved in physical or chemical changes and is neither created nor destroyed.

Meter ($\text{m}$)

The SI base unit of length, defined as the distance light travels through a vacuum in $1/299,792,458\,\text{s}$.

Kilogram ($\text{kg}$)

The SI base unit of mass.

Mass

A measure of the quantity of matter within an object.

Weight

A measure of the gravitational pull on the matter of an object.

Second ($\text{s}$)

The SI base unit of time, defined as the duration of $9,192,631,770$ periods of radiation emitted from a specific transition in a cesium-133 atom.

Kelvin ($\text{K}$)

The SI base unit of temperature, which measures the average kinetic energy of atoms or molecules in matter.

Absolute Zero

The zero point on the Kelvin scale ($0\,\text{K}$ or $-273.15^\circ\text{C}$), representing the coldest possible temperature where molecular motion virtually stops.

Derived Unit

A unit formed from a combination of other SI base units, such as volume ($\text{cm}^3$) or density ($\text{g/cm}^3$).

Density

The ratio of a substance's mass to its volume, calculated as $\text{Density} = \frac{\text{Mass}}{\text{Volume}}$.

Intensive Property

A characteristic of matter that is independent of the amount of substance present, such as density.

Extensive Property

A characteristic of matter that depends on the amount of substance present, such as mass.

Significant Figures

Digits in a measured quantity that reflect its precision, where every digit is certain except the last, which is estimated.

Exact Numbers

Numbers that have an unlimited number of significant figures, originating from accurate counting of discrete objects, defined quantities, or integral numbers in equations.

Accuracy

Refers to how close a measured value is to the actual or true value.

Precision

Refers to how close a series of measurements are to one another or how reproducible they are.

Random Error

An error in measurement that has an equal probability of being too high or too low.

Systematic Error

An error in measurement that tends toward being consistently either too high or too low.

Dimensional Analysis

A problem-solving method that uses units as a guide to setting up and solving calculations.

Conversion Factor

A fractional quantity created from a unit equation with the unit being converted from on the bottom and the desired unit on the top.

The Scientific Approach Diagram

A flowchart depicting how observations lead to hypotheses or laws, which are continuously tested by experiments to confirm or revise hypotheses, laws, and theories.

Classification of Matter Scheme

A diagram classifying matter based on variable composition into pure substances (elements/compounds) and mixtures (heterogeneous/homogeneous).

Distillation Setup Diagram

An illustration of distillation showing a heated liquid mixture, boiling of the volatile component, cooling via a water condenser, and collection of pure liquid.

Filtration Setup Diagram

An illustration of filtration showing a solid-liquid mixture poured through a funnel with filter paper, trapping the solid while collecting the liquid below.

Temperature Scales Diagram

A comparison diagram displaying Fahrenheit, Celsius, and Kelvin scales with benchmark points for water boiling, water freezing, and absolute zero.

Precision and Accuracy Comparison Diagram

Bar charts illustrating measurement results for Student A (inaccurate, imprecise), Student B (inaccurate, precise), and Student C (accurate, precise) measuring a $10.00\,\text{g}$ mass.