Atomic Theory and Particle Theory Lecture

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A set of vocabulary flashcards covering fundamental ideas from the lecture: particle theory, phases of matter, subatomic particles, key historical atomic models, and related atomic properties.

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18 Terms

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Particle Theory of Matter

States that: (1) all matter is composed of tiny particles; (2) particles of the same substance are identical regardless of state; (3) particles attract each other; (4) spaces between particles are large compared with particle size; (5) particles are in constant motion.

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Matter

Anything that occupies space and has mass; composed of atoms and molecules and exists in solid, liquid, and gas phases.

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Atom

The smallest unit of an element that retains the element’s properties; originally thought to be indivisible and solid in Dalton’s model.

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Subatomic Particle

Particles that make up the atom—protons, neutrons, and electrons.

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Proton

Positively charged (+) subatomic particle located in the nucleus; contributes to atomic mass.

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Neutron

Neutral subatomic particle found in the nucleus; adds mass but carries no charge.

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Electron

Negatively charged (–) subatomic particle that occupies specific energy levels (orbits) around the nucleus.

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Nucleus

Tiny, dense, positively charged core of an atom containing protons and neutrons; most of the atom’s mass resides here.

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Energy Level (Orbit)

Fixed region around the nucleus where an electron is likely to be found; each has a specific size and energy.

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Electron Transition

Movement of an electron between energy levels: it moves outward when it gains energy and inward when it loses energy.

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Solid Sphere Model (Dalton, 1803)

Early atomic model describing the atom as an indivisible, solid sphere with unique properties for each element.

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Plum Pudding Model (J. J. Thomson, 1904)

Model portraying the atom as an electrically neutral sphere of positive charge with embedded negative electrons.

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Nuclear Model (Ernest Rutherford, 1911)

Model that introduced a central nucleus: atoms are mostly empty space with electrons outside the dense, positive nucleus.

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Planetary/Bohr Model (Niels Bohr, 1913)

Model in which electrons travel in fixed circular orbits around the nucleus, each orbit having quantized energy.

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Intermolecular (Particle) Attraction

Force that causes particles to attract one another; strength affects a substance’s state and physical behavior.

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Compound Formation

Process in which atoms of different elements chemically combine, forming substances with new properties.

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Atomic Neutrality

Condition in which an atom’s total positive charge equals its total negative charge, resulting in no overall charge.

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Indivisibility Postulate

Dalton’s assertion that atoms cannot be subdivided, created, or destroyed in chemical reactions.