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37 Cards in this Set
- Front
- Back
Matter
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Anything that takes up space and has mass
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Element
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Substance that cannot be broken down to other substances by chemical reactions
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Compound
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Substance consisting of two or more elements combined in a fixed ratio
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Trace Elements
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Those required by an organism in only minute quantities
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Atom
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smallest unit of matter that still retains the properties ot an element
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John Dalton
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British scientist who helped develop atomis theory around 1800. The atomic theory measures the mass of atoms and subatomic particles
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Atomic Number
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Number of protons found in the nuclei of an element
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Mass Number
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The sum of protons plus netrons in the nucleus of an atom
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Atomic Weight
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The approximation of the total mass of an atom
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Isotopes
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One of several atomic forms of an element each containing a diffrent number of neutrons and thus giving a diffrent atomic mass
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Radioactive Isotope
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An isotope that is unstable, the nucleus decays spontaniously, giving of detectable particles and energy
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Energy
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The capacity to do work
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Potencial Energy
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The energy stored by matter as a result of its location or spatial arrangement
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Energy Levels
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The diffrent states of potential energy for electrons in an atom
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Electron Shells
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An evergy level representing the distance of an electron from the nucleus of an atom
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Valence Electron
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Electrons in the outer most electron shell
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Valence Shell
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The outermost energy of an atom containing the valence electrons involved in the chemical reactions of that atom
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Chemical Bonds
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An attraction between two atoms resulting from a sharing of outer-shell electrons or the presence of opposite chrges on the atoms the bonded atoms gain complete outer electron shells
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Covalent Bonds
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A type of strong chemical bond in which two atoms share one pair of valence electrons
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Molecule
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Two or more atoms held together by covalent bonds
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Structural Formula
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A type of molecularnotation in which the constituent atoms are joined by lines representing covalent bonds
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Molecular Formula
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A type of molecular notation indicating only the quantity of the contituent atons
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Double Covalent Bond
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A type of covalent bond in which two atoms share two pairs of electrons smbolized by a pair of lines between the bonded atoms
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Valence
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The bonding capacity of an atom generally equal to the number of unpaired electrons in the atom's outermost shell
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Electronegativity
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The attraction of an atom for the electrons of a covalent bond
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Nonpolar covalent bonds
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A type of covalent bond in which electrons are shared equally between two atsoms of similar electronegativity
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Polar covalent bonds
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A type of covalent bond between atoms that differ in electronegativity The shared electrons are pulles closer to the more electronegative atom making it slightly negative and the other atom slightly positive
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Ion
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An atom that has gained or lost electrons thus acquiring a charge
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Cation
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An ion with a positive charge produced by the loss of one or more electrons
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Anion
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A negitively charged ion
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Ionic Bonds
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A chemical bond resulting from the attraction between oppositly charged ions
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Ionic compounds
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Compounds resulting from the formation of ionic bonds,also known as salt
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Hydrogen Bonds
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A type of weak chemical bond formed when the slightly positive hydrogen atom of a polar covalent bond in one molecule is attracted to the slightly negative atom of a polar covalent bond in another molecule
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Chemical reactions
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A process leading to chemical changes in matter, involves the makind and/or breaking of chemical bonds
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reactants
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The starting material in a chemical reactions
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Products
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An ending material in a chemical reation
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Chemical equalibrium
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In a reversible chemical reaction the point at whthe rate of the forward reaction equals the rate of the reverse reaction
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