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| The optimum distance between nuclei where the net attractive forces are maximized. |
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| A formula for a molecule that shows specific bonds between atoms. |
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| Molecular formula. Gives the number and type of each element in the molecule. |
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| The amount of energy that must be supplied when a bond breaks or the amount of energy released when a bond is formed. |
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| The ability of an atom to attract shared electrons in a covalent bond. Increases from left to right along a period of the periodic table. Increases from bottom to top of a group on the periodic table. |
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| Lewis Structure. A structure that represents an atom's valence electrons by dots and indicates by the placement of dots how the valence electrons are distributed in a molecule. |
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| Nonbonding pair; A pair of valence electrons assigned to an atom in a Lewis structure that are not involved in bonding. |
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| Shared valence electrons in a dot structure that make up bonds between atoms |
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| The number of valence electrons for a free atom minus the number of valence electrons assigned to a bonded atom. |
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| A covalent bond in which the bonding electrons are shared unequally. |
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| A covalent bond in which the bonding electrons are shared equally. |
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| Valence-Shell Electron-Repulsion (VSEPR) Model |
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| A model for predicting the approximate shape of a molecule. |
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| A cloud of electrons assigned to an atom in a molecule and used to determine the approximate shape of the molecule. A single charge cloud could be one lone pair, one single bond, one double bond, or one triple bond. |
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| The angle at which two adjacent bonds intersect. |
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| A theory that visualizes the orbital picture of how electron pairs are shared in a covalent bond. |
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| A bond that forms from the head-on overlap of atomic orbitals. Always the first bond to form between two atoms in a molecule. |
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| A bond that forms from the parallel overlap of two p orbitals. Only present in double (1 pi) or triple bonds (2 pi). |
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| An atomic orbital formed by the hybridization of an s orbital with two p orbitals. |
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| An atomic orbital formed by the hybridization of an s orbital with one p orbitals. |
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| An atomic orbital formed by the hybridization of an s orbital with three p orbitals. |
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| A wave function whose square gives the probability of finding an electron within a given region of space in a molecule. |
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| A wave function whose square gives the probability of finding an electron within a given region of space in an atom. |
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| Molecular Orbital (MO) Theory |
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| A quantum mechanical description of bonding in which electrons occupy molecular orbitals that below to the entire molecule rather than to an individual atom. |
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| Bonding Molecular Orbital |
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| A molecular orbital that is lower in energy than the atomic orbitals from which it is derived. |
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| Anti-Bonding Molecular Orbital |
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| A molecular orbital that is higher in energy than the atomic orbitals from which it is derived. |
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| The number of electron pairs between atoms. (# of bonding electrons - # of antibonding electrons) divided by two. |
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| Group 1A elements. Rapidly react with water to form alkaline products. Soft, silvery metals. Never found in a pure state in nature. |
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| Group 2A elements. Lustrous, silvery metals. Less reactive than the Group 1A elements. Never found in a pure state in nature. |
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| Group 7A elements. Found in nature only in combination with other elements, such as salts. |
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| Group 8A elements. Colorless gases with very low or no chemical reactivity. |
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| 1000 calories or 1 kilocalorie or 4.184 kJ |
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| a unit of energy measured as the amount of energy required to increase the temperature of 1 g of water by 1 degree Celcius |
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| If the first digit you remove is a 5 and there are nonzero digits following, round up. |
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| If the first digit you remove is a 5 with nothing or a 0 following, round down. |
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