Term
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Definition
| noble gases (consist of single atoms) |
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Term
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Definition
| a bond formed by the sharing of electrons between atoms |
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Term
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Definition
| a neutral group of atoms joined together by covalent bonds |
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Term
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Definition
| a molecule consisting of two atoms |
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Term
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Definition
| a compound that is composed of molecules Ex) H2O |
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Term
| what are all molecules of a molecular compound |
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Definition
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Term
| what are molecular compound melting and boiling points like |
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Definition
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Term
| what are molecular compounds at room temperature |
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Definition
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Term
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Definition
| a chemical formula of a molecular compound that shows the kinds and numbers of atoms present in a molecule of a compound |
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Term
| why do covalent bonds occur |
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Definition
| so that atoms can attain the octet rule and noble gas VE structure |
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Term
| what groups tend to form covalent bonds? |
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Definition
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Term
| what noble gas VE structure does hydrogen gain thourhg covalent bonding |
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Definition
| The VE structure of Helium (2 VEs) |
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Term
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Definition
| a bond formed when two atoms share a pair of electrons |
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Term
| what represents a single covalent bond in a structural formula? |
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Definition
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Term
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Definition
| a chemical formula that shows the arrangement of atoms in a molecule or a polyatomic ion: each dash between a pair of atoms indicates a pair of shared electrons |
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Term
| double covalent bond in a structural formula |
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Definition
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Term
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Definition
| a pair of valence electrons that is not shared between atoms |
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Term
| why can't oxygen form a diatomic molecule? |
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Definition
| experimental evidence says that oxygen has to have unattached electrons because it is magnetic |
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Term
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Definition
| a covalent bond in which two pairs of electrons are shared by two atoms |
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Term
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Definition
| a covalent bond in which three pairs of electrons are shared by two atoms Ex N2 |
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Term
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Definition
| a covalent bond in which one atom contributes both bonding electrons |
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Term
| what represents a coordinate covalent bond in a structural formula? |
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Definition
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Term
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Definition
| a tightly bound group of atoms that behaves as a unit and has a positive or negative charge |
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Term
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Definition
| the energy required to break the bond between two covalently bonded atoms; this value is usually expressed in kJ per mol of substance |
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Term
| what has a higher bond dissociation energy? a double covalent bond or a triple covalent bond? |
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Definition
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Term
| oxygen atoms in the ozone are |
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Definition
| a mixture of extremes represented by resonance forms |
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Term
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Definition
| one of the two or more equally valid electron dot structures of a molecule or polyatomic ion |
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Term
| when are their exceptions to the octet rule? |
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Definition
| odd number of ve/ less then 8 ve/ more than 8 ve |
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Term
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Definition
| an orbital that applies to the entire molecule |
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Term
| each molecular orbital is full if it contains... |
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Definition
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Term
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Definition
| a molecular orbital that can be occupied by two electrons of a covalent bonds |
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Term
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Definition
| a bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei |
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Term
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Definition
| oval with two nuclei (two circles, s oribitals, combined) |
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Term
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Definition
| a covalent bond in which the bonding electrons are most likely to be found in sausage-shaped regions above and below the bond axis of the bonded atoms |
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Term
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Definition
| two ovals with the two nuclei in between ,two p orbitals (barbells)combined |
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Term
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Definition
| a bond angle of 109.5 degrees that results when a central atom forms four bonds directed toward the center of a regular tetrahedron (tripod) |
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Term
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Definition
| valence –shell electron-pair repulsion theory; because electron pairs repel, molecules adjust their shapes so that valence electron pairs are as far apart as possible |
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Term
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Definition
| the mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals |
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Term
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Definition
| a covalent bond in which the electrons are shared equally by the two atoms |
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Term
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Definition
| a covalent bond between atoms in which electrons are shared unequally |
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Term
| electronegative atoms in covalent bonds |
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Definition
| attract electrons and gain a slightly negative charge (polar covalent bond) |
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Term
| less electronegative atoms in covalent bonds |
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Definition
| have a slighlty positive charge |
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Term
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Definition
| a molecule in which one side of the molecule is slightly negative and the opposite side is slightly positive |
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Term
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Definition
| a molecule that has two poles, or regions, with opposite charges |
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Term
| intermolecular attractions are what compared to ionic and covalent bonds? |
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Definition
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Term
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Definition
| the two weakest intermolecular attractions-dispersion forces and dipole interactions |
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Term
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Definition
| intermolecular forces resulting from the attraction of oppositely charged regions of polar molecules |
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Term
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Definition
| attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules |
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Term
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Definition
| attractive forces in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom |
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Term
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Definition
| a solid in which all of the atoms are covalently bonded to each other |
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Term
| the requirements for melting a network solid |
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Definition
| breaking covalent bonds throughout the solid |
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