General Chemistry 1 - Vocabulary Flashcards

Vocabulary flashcards covering key terms and concepts from the lecture notes on General Chemistry 1.

Chemistry

The study of matter — its properties, composition, structure, changes it undergoes, energy involved, and the laws and principles that govern such changes.

Central science

Chemistry is the central science that connects physics, biology, geology, and other disciplines.

Servant science

Chemistry is described as a servant science, providing tools and concepts to other fields.

Environmental Science

A field including Ecology, Pollution Studies, and Greenhouse Effect; applies chemistry to environmental problems.

Ecology

The study of interactions between organisms and their environment.

Greenhouse Effect

The process by which greenhouse gases trap heat in Earth’s atmosphere.

Biology

The science dealing with living organisms, including cell biology, genetics, and more.

Biochemistry

Chemistry of living things; the chemistry underlying biological processes.

Geology

The science dealing with Earth’s physical structure, materials, and history.

Medicine and other allied health sciences

Fields such as pharmacology, nutrition, and radiology that apply chemistry to health.

Astronomy

The study of celestial objects and phenomena; includes Solar, Galactic, Astrophysics, and Astrometry.

Physics

Science dealing with matter, energy, and their interactions (e.g., atomic/nuclear physics, quantum mechanics, biomechanics, spectroscopy).

Nuclear Chemistry

Chemistry of radioactive and nuclear processes; study of the nucleus and radiochemistry.

Organic chemistry

Branch of chemistry dealing with carbon-containing compounds.

Inorganic chemistry

Branch of chemistry dealing with all substances except carbon-containing compounds.

Physical chemistry

Branch focusing on measuring physical properties and the physical basis of chemical phenomena.

Analytical chemistry

Branch dealing with qualitative and quantitative analysis of substances.

Branches of chemistry

Major subdivisions: Inorganic, Organic, Biochemistry, Physical, Analytical.

Solid

Phase with definite shape and fixed volume.

Liquid

Phase with indefinite shape but fixed volume.

Gas

Phase with indefinite shape and indefinite volume; highly compressible.

Plasma

Fourth phase of matter consisting of ionized gas.

Bose-Einstein Condensate

State of matter at near-absolute zero where particles share the same quantum state.

Pure substance

Matter with uniform composition that cannot be separated into simpler substances by physical means.

Mixture

Matter containing two or more substances that can be separated by physical means.

Homogeneous

Mixture with uniform composition throughout (also called a solution).

Heterogeneous

Mixture with non-uniform composition.

Solution

A homogeneous mixture composed of a solute dissolved in a solvent.

Compound

Substance made of two or more elements chemically combined in fixed proportions.

Suspension

Mixture in which particles are dispersed and may settle out over time.

Physical change

Change that alters form or appearance but not chemical composition.

Chemical change

Change that alters the chemical composition of a substance.

Nuclear change

Change involving the nucleus, such as radioactive decay.

Endothermic

A process that absorbs heat.

Exothermic

A process that releases heat.

Radiant energy

Electromagnetic energy carried by radiation (light, waves, etc.).

Heat energy

Thermal energy; energy associated with temperature.

Chemical energy

Energy stored in chemical bonds that can be released or absorbed during reactions.

Significant figures

Digits known with certainty plus the first digit that is uncertain.

Addition/subtraction significant figures rule

Results should not have more decimal places than the least precise measurement.

Multiplication/division significant figures rule

Results should not have more significant figures than the measurement with the fewest significant figures.

Scientific notation

A way to express very large or small numbers as a × 10^n to maintain precision.

SI prefixes

Prefixes indicating powers of ten, e.g., kilo (k)=10^3, milli (m)=10^-3, mega (M)=10^6, etc.

Accuracy

How closely a measurement agrees with the true value.

Precision

How close repeated measurements are to each other (the average value).

Intrinsic properties

Properties inherent to the substance and independent of amount or sample.

Extrinsic properties

Properties that vary between samples of the same material (mass, volume, shape, size).

Extensive properties

Properties that depend on the amount of material (mass, volume, weight).

Intensive properties

Properties that do not depend on the amount of material (odor, taste, hardness, color).

Physical properties

Characteristics related to a substance’s physical appearance or transformations without changing its composition.

Chemical properties

Characteristics related to a substance’s tendency to undergo chemical change.

Alchemy

Ancient practice aimed at turning base metals into gold; sought the Philosopher’s Stone.

Transmutation

Supposed conversion of one element into another; a concept from alchemy.

Scientific Method

Seven steps: Problem, Research, Hypothesis, Experiment, Observations, Conclusions, Communicate.

Problem

The question you want to answer in a study.

Hypothesis

An educated guess or prediction about the outcome.

Experiment

Tests the hypothesis.

Observation

Data collected during the experiment.

Conclusion

Determines if the hypothesis was supported by the results.

Communicate

Present findings in a talk or written report.