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37 Cards in this Set
- Front
- Back
Element
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A fundamental form of matter that has mass, takes up space, and cannot be broken down into something else on Earth.
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Atoms
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particles that retain the properties of an element.
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Protons
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Positive charge, one in every atom.
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Neutrons
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No charge, one in every atom.
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Nucleus
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Core of atoms; protons and neutrons
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Electrons
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Negative charge, normally equal amounts of electrons and protons.
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Atomic number
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Number of protons in each atom.
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Mass number
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Combined number of neutrons and protons.
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Isotopes
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Atoms that vary in neutron number.
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Radioisotope
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Isotope with unstable nucleus, stabilizes by emitting energy and particles.
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Radioactive decay
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Transforms a radioisotope into a new element.
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Tracers
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Substances with an isotope attached to them (often radioisotopes).
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Radiation therapy
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Radioisotopes stop activity of abnormal body cells.
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Orbital
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Space around nucleus in which electrons are likely to be found.
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Shell model
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A “shell” encloses all orbitals available to electrons at the same energy level.
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Inert atoms
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Atoms with no vacancies.
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Chemical bond
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Union between electron structures of atoms.
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Molecule
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Two or more bonded atoms.
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Diatomic molecules
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Molecules with two of the same element.
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Compounds
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Molecules with elements in proportions that never vary.
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Mixture
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Two or more elements or compounds intermingled in proportions that usually vary.
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Ionic bond
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Association of two ions with opposing charges.
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Ion
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Atom that has either lost or received an electron (charged).
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Covalent bond
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sharing of a pair of electrons between two atoms.
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Non-polar covalent bond
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No difference in change between ends of bond, atoms share electrons equally.
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Polar covalent bond
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More attractive (electronegative atom) exerts stronger pull on electrons --> slightly negative (No molecular net charge).
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Hydrogen bond
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Weak attraction between an electronegative atom and a hydrogen atom taking part in a second polar covalent bond.
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Hydrophilic substances
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Polar substances, attracted to water.
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Hydrophobic substances
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Non-polar molecules, repel hydrophilic substances and water.
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Temperature
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Measure of molecular motion.
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Cohesion
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Capacity to resist rupturing when placed under tension.
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“Spheres of Hydration”
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Formed when water molecules cluster around oppositely charged solute (dissolved substances) ions or molecules
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pH scale
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Determines H+ concentration in liquids.
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Neutrality
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pH = 7, pure water, [H=] = [OH-]
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Acids
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pH = 0-7, proton donators (lemon juice, coffee)
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Bases
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pH = 7-14, proton acceptors (seawater, baking soda, “alkaline” fluids).
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Salts
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Compounds that release ions other than H= and OH- in solutions.
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