CHEM 111: Measurement, Dimensional Analysis, and Properties of Matter

Vocabulary flashcards defining fundamental chemical concepts, measurement metrics, unit conversions, and classification of matter from Chapters 1.2 through 1.7.

Quantitative

Relating to, measuring, or measured by the quantity of something.

Metric System

A system of units used for scientific measurements.

SI Units

The preferred metric units for scientific use, consisting of seven base units from which all other units are derived.

Watt (W)

The SI unit of power, representing the rate at which energy is generated or consumed, defined as $1\,\text{W} = 1\,\text{J/s}$.

Joule (J)

The SI unit of energy, defined as $1\,\text{J} = 1\,\text{kg}\cdot\text{m}^2/\text{s}^2$.

Kilogram (kg)

The SI base unit of mass, equal to $2.20\,\text{lb}$.

Meter (m)

The SI base unit of length, equal to $1.09\,\text{yd}$.

Temperature

A physical property that determines the direction of heat flow, measuring the hotness or coldness of an object.

Celsius Scale

A temperature scale based on the properties of water, where $0\,^\circ\text{C}$ is the freezing point and $100\,^\circ\text{C}$ is the boiling point.

Kelvin (K)

The SI unit of temperature based on gas properties, where absolute zero is $0\,\text{K}$, calculated as $\text{K} = ^\circ\text{C} + 273.15$.

Absolute Zero

The lowest possible temperature, defined as $0\,\text{K}$.

Volume

A derived SI unit from length ($\text{m}^3$), most commonly measured in liters ($\text{L}$) or milliliters ($\text{mL}$).

Liter (L)

A metric unit of volume equal to a cube that is $1\,\text{decimeter (dm)}$ long on each side.

Milliliter (mL)

A metric unit of volume equal to a cube that is $1\,\text{centimeter (cm)}$ long on each side, equivalent to $1\,\text{cm}^3$.

Density

A physical property representing the mass per unit volume of a substance, defined as $\text{Density} = \frac{\text{Mass}}{\text{Volume}}$.

Calorie (cal)

A unit of energy equal to $4.184\,\text{Joules}$.

Nutritional Calorie (Cal)

An energy unit equivalent to $1\,\text{kilocalorie (kcal)}$ or $1000\,\text{calories (cal)}$.

Exact Numbers

Values that are known precisely, such as counted quantities or defined conversion values.

Inexact Numbers

Values obtained by measurement that contain inherent uncertainty due to equipment or human error.

Precision

The closeness of agreement among several measurements of the same quantity.

Accuracy

A measure of how closely individual measurements agree with the correct or true value.

Significant Figures

All digits of a measured quantity, including the last estimated digit, which is uncertain.

Dimensional Analysis

A method of problem solving where units are multiplied or divided to ensure calculations yield desired units.

Conversion Factor

A fraction whose numerator and denominator represent the same quantity expressed in different units.

Matter

The physical material of the universe, defined as anything that has mass and occupies space.

Solid

A state of matter that has both a definite shape and a definite volume and is not easily compressed.

Liquid

A state of matter that has a distinct volume independent of its container, assumes the shape of the portion of the container it occupies, and is not easily compressed.

Gas (Vapor)

A state of matter that has no fixed volume or shape, uniformly fills its container, and can expand or compress.

Pure Substance

Matter with fixed composition and distinct properties, categorized as either an element or a compound.

Element

A substance that cannot be decomposed into simpler substances, composed of only one kind of atom.

Compound

A substance composed of two or more elements chemically combined in definite proportions.

Mixture

A combination of two or more substances in which each substance retains its chemical identity.

Law of Constant Composition

A principle stating that compounds have a definite composition, meaning the relative number of atoms of each element is the same in any sample.

Heterogeneous Mixture

A mixture that varies in composition throughout a sample.

Homogeneous Mixture (Solution)

A mixture that has the same uniform composition throughout a sample.

Physical Properties

Properties that can be observed or measured without changing the chemical composition of a substance.

Chemical Properties

Properties that describe the way a substance may change or react to form other substances.

Intensive Properties

Properties that do not depend on the amount of sample being examined and can be used to identify substances.

Extensive Properties

Properties that depend on the amount of sample examined, such as mass and volume.

Physical Changes

Changes in physical appearance that occur with no change in chemical composition.

Chemical Changes

Transformations in which a substance is converted into a chemically different substance.

Filtration

A separation method used to separate solid substances from liquids and solutions.

Distillation

A separation method that uses differences in boiling points to separate components of a liquid homogeneous mixture.

Chromatography

A separation method that separates substances based on differences in their ability to adhere to a solid surface.

Energy

The capacity to do work or transfer heat.

Work

The energy transferred when a force exerted on an object causes displacement of that object, expressed as $w = F \times d$.

Heat

The energy transferred to cause the temperature of an object to increase.

Force

Any push or pull exerted on an object.

Potential Energy

Stored energy that depends on the relative position of an object compared to other objects.

Kinetic Energy

The energy of motion, calculated using mass and velocity as $E_k = \frac{1}{2}mv^2$.

Electrostatic Potential Energy

The stored energy of charged particles based on their positions relative to each other.