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20 Cards in this Set
- Front
- Back
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Isotope
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Same number of protons, differing in number of electrons
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Orbital
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Region where electron would most likely be found
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Ground-State electron Configuration
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Lowest-energy arrangement of electrons
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Valence Shell
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The outermost shell in an atom
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Ionic Bond
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A bond between two atoms where one atom donates an electron and the other accepts, based on the electronegativity of the atoms. This bond is stronger than the other type of bond.
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Covalent Bond
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When two atoms share electrons to achieve a stable outer shell.
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Molecule
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Neutral collection of atoms held together by atomic bonds
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Lewis Structures
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Electron -dot structure. Representation of molecules with the use of dots to represent bonds.
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Kekule Structures
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Line-bond structure. Representation of molecules with use of lines to represent bonds
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Nonbonding electrons (lone-pair electrons)
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Valence electrons not used for bonding
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Bond Strength
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the amount of energy needed to break a bond in kJ/mol
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Bond length
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The distance between two bonded atoms
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sp^3 hybrid orbitals
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a hybridized orbital with one 's' shell and three 'p' shells.
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bond angle
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angle formed between bonds. Common angle by H-C-H is 109.5
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Sigma Bond
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Bond where overlap of orbitals lies on the bond axis.
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Pi bond
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Bond where overlap of orbitals occurs above and below an atom's bond axis. common for double bonds.
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polar covalent bonds
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A bond between two atoms with differing electronegativity in which the electrons in the bond are more attracted to one of the more electronegative atoms .
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electronegativity
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the ability of an atom to attract electrons in a covalent bonds.
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functional group
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group of atoms with a larger molecule with a characteristic chemical behavior
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saturated hydrocarbons
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1) contains only carbon and hydrogen atoms and have only C-C and C-H
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