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| 15184090971 | covalent bonds | sharing electrons | 0 | |
| 15184094555 | group number | number of valence electrons | 1 | |
| 15184102899 | hydrogen | only needs 2 electrons; only bond once | 2 | |
| 15184107839 | boron | only need 3 bonds | 3 | |
| 15184107840 | halogens | only bond once | 4 | |
| 15184113679 | nitrogen | one lone pair | 5 | |
| 15184113680 | oxygen | two bonds, two lone pairs | 6 | |
| 15184117071 | carbon | central atom with octet | 7 | |
| 15184123517 | electrons | arrange themselves to be as far apart as possible | 8 | |
| 15184126717 | single bond | longest and weakest bond | 9 | |
| 15184130706 | triple bond | shortest and strongest bond | 10 | |
| 15184134817 | bond polarity | electrons in covalent bond are not always shared equally | 11 | |
| 15184146171 | bonds | most average length | 12 | |
| 15184148828 | lowest formal charge | most stable structure | 13 | |
| 15184154289 | resonance structure | one of the two or more equally valid electron dot structures of a molecule or polyatomic ion; bond length identical in resonance structures; se equivalent structures are known as resonance structures and involve the shifting of electrons and not of actual atoms. Depending on the compound, the shifting of electrons may cause a change in formal charges. Most often, Lewis structures are drawn so that the the formal charge of each atom is minimized. | 14 | |
| 15184178733 | alloy | mixture of metals; stronger | 15 | |
| 15184185465 | average bond enthalpies | energy required to break a bond; positive (bond breaking in endothermic); averages over many compound; electronegativity influences bond enthalpies | 16 | |
| 15184193966 | Electronegativity | A measure of the ability of an atom in a chemical compound to attract electrons | 17 | |
| 15184196750 | multiple bonds | are stronger than a single bond; bond enthalpy greater for | 18 | |
| 15184205944 | decreases | as the number of bonds between atoms increases, the bond length decreases | 19 | |
| 15184215465 | molecular orbital theory | s and p orbitals blend together | 20 | |
| 15184223930 | 2sp | 1s1p | 21 | |
| 15184228771 | 3sp^2 | 1s2p | 22 | |
| 15184232469 | 4sp^3 | 1s3p | 23 | |
| 15184237126 | molecular shape | depends on molecular properties | 24 | |
| 15184244059 | AB2 linear | 180 |  | 25 |
| 15184246879 | AB2 bent |  | 26 | |
| 15184250356 | AB2 Trigonal planar |  | 27 | |
| 15184258062 | AB3 trigonal pyramidal |  | 28 | |
| 15184270591 | shape | determined by bond angles, electro pair repulsion, and electron pairs being far apart as possible | 29 | |
| 15184275451 | electron domains | regions about a central atom in which electrons are likely to be found; double bonds=1 domain; domain IS AREA OF ELECTRON DENSITY | 30 | |
| 15184281562 | VSEPR | best arrangement of given number of electron domains is one that minimizes the repulsions among them | 31 | |
| 15184292393 | molecular geometrics | 1. Draw the best lewis structure 2. Determine the electron domain geometry 3. Use arrangement of bonded atoms to determine the molecular geometry -straight line-in plane -shaded wedge-coming out -dashed wedge- going away from you | 32 | |
| 15184309186 | nonbonding domains | electron pairs associated with single atom; change angle lone pair occupies more space than bond because a bond is confined; thus these are physically larger and repulsions greater; more nonbonding domains results in smaller bond angles | 33 | |
| 15185131213 | valence electrons | electrons involved in chemical bonding; those in the outermost occupied shells | 34 | |
| 15185139588 | octet tule | atoms gain lose or share electrons to=number of electrons in noble gas; thus they gain, lose, or share electrons until they are surrounded by eight valence electrons; full s and p subshells | 35 | |
| 15185166770 | ionic substances | metals and nonmetals; reaction often exothermic; electron transfer from metal to nonmetal | 36 | |
| 15185175567 | ionization energy | how easily an electron can be removed from an atom |  | 37 |
| 15185189674 | electron affinity | how much an atom wants to gain an electron |  | 38 |
| 15185200962 | ionic properties | brittle, high melting points, crystalline, cleaved | 39 | |
| 15185211001 | enthalpy of formation | the enthalpy change that accompanies the formation of a substance from the most stable forms of its component elements | 40 | |
| 15185214816 | exothermic | when nonmetal gains an electron; release of energy | 41 | |
| 15185220491 | endothermic | removing an electron; requires energy | 42 | |
| 15185228254 | lattice energy | energy required to completely separate one mole of a solid ionic compound into its gaseous ions; large positive values indicate that the ions are strongly attracted to one another in ionic solids; energy released by attraction of ions with opposite charge makes the formation of ionic compounds exothermic; magnitude depends on charges of ions, sized and arrangement | 43 | |
| 15185259763 | increases | lattice energy... as the charges on the ion increase and their radii decrease | 44 | |
| 15185265524 | atomic radii |  | 45 | |
| 15185283389 | covalent substances | low melting points; low points of vaporization | 46 | |
| 15185288972 | covalent bond | positively charged nuclei repel each other; and the negatively charged electrons repel each other; nuclei and electrons attract each other; attractive forces>repulsive force as stable |  | 47 |
| 15185313277 | bond polairty | how equally or unequally electrons in a covalent bond are shared; from difference in ability to attract electrons | 48 | |
| 15185320231 | electronegativity | the ability of an atom in a molecule to attract itself |  | 49 |
| 15185348832 | more polar bond | greater difference in electronegativity | 50 | |
| 15185351620 | electronegativity difference | The difference in electronegativity between two elements in a bond. |  | 51 |
| 15185376950 | formal charge | the charge an atom in a molecule would have if each bonding electron pair in a molecule were shared equally between atoms |  | 52 |
| 15185398751 | dominant lewis structure | one in which atoms bear formal charges closest to zero; negative charges in more dominant are on more electronegative atoms | 53 | |
| 15185409000 | oxidation number | charge on an atom if bonds were completely ionic | 54 | |
| 15185427324 | resonance structures | Individual Lewis structures in cases where two or more Lewis structures are equally good descriptions of a single molecule. The resonance structures in such an instance are "averaged" to give a more accurate description of the real molecule; arrangement of electrons differ | 55 | |
| 15185469803 | average bond length | represents the average length of a bond between two particular atoms in a large number of compounds | 56 | |
| 15185469804 | shorter and stronger | as the number of bonds between two atoms increase, the bond grows shorter and stronger | 57 | |
| 15185522757 | bond angles | determines shape of a molecule; angles made by lines joining the nuclei of the atoms in the molecule | 58 | |
| 15185533953 | linear | 180 | 59 | |
| 15185533954 | bent | does not equal 180 | 60 | |
| 15185545197 | shapes of AB2 and AB3 molecules |  | 61 | |
| 15185552633 | VSEPR | A model that accounts for the geometric arrangements of shared and unshared electron pairs around a central atom in terms of the repulsions between electron pairs. | 62 | |
| 15185594178 | electron domain | region in which electrons are most likely found | 63 | |
| 15185603124 | bonding pair | pair of electrons shared by two atoms |  | 64 |
| 15185609100 | nonbonding pairs | electron domain that is located principally on one atom |  | 65 |
| 15185628532 | best arrangement | ... of a given number of electron domains is one that minimizes the repulsions among them | 66 | |
| 15185637811 | electron-domain geometries | The three-dimensional arrangement of the electron domains around an atom according to the VSEPR model. | 67 | |
| 15185649551 | molecular geometry | The arrangement in space of the atoms of a molecule; involves only electron domains due to bonds | 68 | |
| 15185713821 | Using VSEPR model | 1. Draw lewis structure of a molecule or ion and count the number of electron domains around central atom 2. determine electron domain geometry by arranging central atoms to reduce repulsions 3. USe to determine molecular geometry | 69 | |
| 15185740884 | effect of nonbonding electrons on bond angles | no lone pairs on tetrahedral e.d geometry- 109.5 one lone pair- 107 2 lone pairs- 104.5 | 70 | |
| 15185754914 | decrease | bond angles... as the number of nonbonding electron pairs increases | 71 | |
| 15185776975 | dipole moment | depends on polarity of individual bonds and the geometry of the molecule; | 72 | |
| 15185781481 | bond dipole | The dipole moment that is due only to unequal electron sharing between two atoms in a covalent bond | 73 | |
| 15185790660 | valence bond theory | bonding electron pairs are concentrated in regions between atoms and nonbonding electron pairs lie in directed region of space; buildup of delectron density between two nuclei occurs when a valence atomic orbital overlaps with valence atomic orbital of another atom | 74 | |
| 15185817487 | hybrid orbitals | An orbital that results from the mixing of different kinds of atomic orbitals on the same atom. For example, an sp3 hybrid results from the mixing, or hybridizing, of one s orbital and three p orbitals.; shape of hybrid orbital is different than originial | 75 | |
| 15185822533 | sp hybrid orbitals | linear; mix 2s with one 2p to generate two new orbitals |  | 76 |
| 15185835777 | sp2 and sp3 hybrid orbitals |  | 77 | |
| 15265525317 | molecular polairty | polar bonds (significant difference in electronegativity) and not symmetrical (C-H nonpolar; diatomic nonpolar) | 78 | |
| 15265535222 | hybridization | atomic orbitals do not work to explain molecular geometry; atomic orbitals change make molecule optimize electron locations | 79 | |
| 15265543776 | sp hybridizations | 2 electron pairs around the central atom; blend one s and on p orbital of the valence electrons to end up with linear geometry; end up with two lone pairs 180 degrees apart | 80 | |
| 15265562853 | sp2 hybridization | 3 electrons around the central atom; blend s and two p orbitals to end up with trigonal planar geometry; | 81 | |
| 15265570496 | sp3 hybridization | four electron pairs; blend s-and 3 p-orbitals of valence electron and end up with tetrahedral geometry | 82 | |
| 15265579665 | sigma bond | single bond; formed by overlap of orbitals in the plane; between two atoms; forms first because lowest energy | 83 | |
| 15265587279 | pi bonds | formed by the overlap of p orbitals; sideways | 84 | |
| 15265590550 | double bond | electrons exist between atoms and above and below pi bond; one sigma and one pi bond; 2 electrons total above and below sigma bond | 85 | |
| 15265607840 | triple bond | either side of bond; one sigma two pi | 86 | |
| 15265610997 | localized electron model summary | draw lewis structures to arrange electron pairs; electron pairs shared by two atoms. electro pairs located between two, electron pairs around centralized atom to minimize repelling; molecular hybridized orbitals form to account for different geometries; resonance indicaet pair of electrons shared; | 87 |
