General Chemistry 1 Midterm Review Flashcards

Vocabulary practice flashcards covering General Chemistry 1 midterm concepts, including matter classification, lab apparatus, techniques, safety, atomic theory, and atomic structure.

Chemistry

Deals with the study of matter, its composition, structure, properties, the changes it undergoes, and how substances interact.

Matter

Anything that takes up space and can be weighed.

Pure Substance

A form of matter that has a definite composition and distinct properties.

Element

The simplest form of matter that can no longer be broken down into simpler substances.

Compound

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

Mixture

Combinations of two or more substances in which each substance retains its distinct identity.

Homogeneous Mixture

A mixture with a uniform composition where individual components are difficult to distinguish.

Heterogeneous Mixture

A mixture with a non-uniform composition containing identifiable components.

Intensive Properties

Properties of matter that are not dependent on the size or mass of a sample, such as boiling point, color, temperature, luster, and hardness.

Extensive Properties

Properties of matter that are dependent on the size or amount of matter, such as volume, mass, size, weight, and length.

Physical Changes

Changes that do not lead to the formation of new substances and involve only a change in physical properties.

Chemical Changes

Changes where a substance reacts and produces one or more new substances.

Beaker

A cylindrical laboratory container used for holding, mixing, and heating substances.

Erlenmeyer Flask

A conical-shaped laboratory vessel used for mixing, heating, storing, and swirling liquids to prevent splashes.

Volumetric Flask

Precision glassware/flask used for accurately preparing and measuring a specific volume of liquid.

Florence Flask

A round-bottom flask with a long neck designed for uniform heating and distillation processes.

Watch Glass

A round and shallow piece of glass used to cover beakers or evaporate small amounts of liquid.

Spatula

A flat and scoop laboratory tool used for transferring solid chemicals and scraping substances.

Funnel

A cone-shaped apparatus used to channel liquids or fine-grained substances into narrow containers.

Stirring Rod

A slender glass rod used for mixing substances and aiding in the transfer of liquids.

Graduated Cylinder

A tall, narrow tube used to measure and dispense specific volumes of liquids.

Graduated Pipette

Calibrated glass equipment with markings used to transfer precise volumes of liquids.

Volumetric Pipette

A precision glass tool designed to deliver a single accurate volume when preparing standard solutions.

Aspirator

A rubber bulb or suction device used for drawing air or liquids into pipettes.

Pasteur Pipette

A small pipette with a bulb at one end used to transfer and dispense small amounts of liquid.

Test Tube and Rack

Glass tubes and a supporting stand used for holding and mixing small quantities of liquid chemicals.

Cork

A cylindrical stopper used to seal laboratory containers.

Spot Plate

Porcelain equipment containing small depressions used to perform and study micro-scale chemical reactions.

Thermometer

An instrument used for measuring temperature in laboratory experiments.

Acid-Base Burette

Graduated glass tube with a stopcock used for the precise delivery of an acid or base during titration.

Separatory Funnel

A conical-shaped glass apparatus equipped with a stopcock used for separating immiscible liquids.

Reagent Bottles

Glass containers used for storing, protecting, and preserving chemical reagents.

Vials

Small glass or plastic bottles used for storing and transporting small amounts of liquid or solid samples.

Wash Bottle

A squeeze bottle used to dispense a controlled stream of water, rinse laboratory equipment, add reagents, or dilute solutions.

Triple Beam Balance

A mechanical balance used to measure mass using sliding weights corresponding to graduated beams.

Analytical Balance

A high-precision balance enclosed in glass to prevent dust and air currents from interfering when measuring small masses in the sub-milligram range.

pH Pen

A digital device used to measure the acidity or basicity of a solution.

Centrifuge

A laboratory machine that rotates samples rapidly to separate particles suspended in a liquid.

Fume Hood

A ventilated enclosure used to limit exposure to hazardous or toxic chemical fumes.

Decantation

A technique used to separate a liquid from a solid sediment by carefully pouring off the liquid with the help of a glass rod.

Random Error

An experimental error that occurs without a consistent pattern.

Systematic Error

An experimental error that occurs consistently in the same direction across repeated measurements.

Theoretical Yield

The maximum calculated amount of product that can be obtained from a reaction.

Actual Yield

The amount of product that is experimentally obtained from a reaction.

Percent Yield

A quantitative measurement of reaction efficiency calculated as \text{Percent Yield} = \n\n\frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100\%.

Democritus

A 5th-century philosopher who taught atomism, stating that all material things are made up of indivisible particles called atoms.

Solid Sphere Model

Atomic model proposed by John Dalton in 1803 describing the atom as an indestructible solid sphere similar to a billiard ball.

Plum Pudding Model

Atomic model proposed by Joseph John Thomson in 1897 depicting negatively charged electrons scattered throughout a positively charged sphere.

Alpha-Scattering Experiment

Experiment conducted by Ernest Rutherford in 1911 bombarding thin gold foil with alpha particles, leading to the discovery of the dense central nucleus and protons.

Planetary Model

Atomic model proposed by Niels Bohr in 1913 describing electrons moving in concentric circular orbits or specific energy levels around the nucleus.

Quantum Mechanical Model

Atomic model proposed by Erwin Schrodinger in 1926 where electrons occupy orbitals representing regions of high probability around the nucleus.

James Chadwick

Scientist who discovered the neutron in 1932 using a Beryllium foil experiment.

Atomic Mass ($A$)

The total mass of an atom's nucleus measured in atomic mass units, calculated as the sum of protons and neutrons ($A = Z + N$).

Atomic Number ($Z$)

The position of an element in the periodic table, which equals the number of protons in the nucleus of an atom.

Ions

Electrically charged particles formed when atoms gain or lose electrons, carrying positive (cations) or negative (anions) charges.

Isotopes

Atoms of the same element that have the same number of protons but different numbers of neutrons, resulting in different atomic masses.

Average Atomic Mass

The weighted average mass of naturally occurring isotopes of an element, calculated using $A_{\text{ave}} = \frac{m_1(\%_1) + m_2(\%_2) + m_3(\%_3)\dots}{100}$.