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40 Cards in this Set
- Front
- Back
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molecules
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atoms of elements combine to form these
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chemical bonds
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attractive forces between atoms aka the valence electrons
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octet rule exceptions
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H, He, B, Li, Be, period 3 and below can have more than 8e-
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octet rule followers
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C, N, F, Na, Mg, O
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ionic bond
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halogen and an alkali metal
no sharing of electrons |
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covalent bonding
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shared electrons
3 types of bonding with this |
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ionic bonds properties
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cation and anion formed
greater than 1.7 difference EN high mp/bp dissolve in polar/h2o solvents good conductors in solvent form crystalline lattice |
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covalent bonds properties
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weaker intermolecular attractions
low mp, low bp do not break into constituent ions when in solvent poor conductors |
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bond order ____ with the increase in the number of bonds
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increases; hence 1<2<3
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covalent bond described by 3 factors
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bond length, bond energy and polarity
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bond length trend
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decreases with increasing bond number
hence 1>2>3 |
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bond energy trend
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increases with bond number
hence 1<2<3 |
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polarity
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dependent upon EN difference
polar bond = dipole + = less EN - = more EN |
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non polar covalent bond
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between like elements
no dipole N2, O2, F2, Cl2, Br2, I2 |
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polar covalent bond
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unequal sharing of e-
0.4-1.7 EN difference ex) HCl has a dipole moment points from (+) to (-) |
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coordinate covalent bond
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bond where 1 element provides all the electrons and the other provides nothing
ex) BCl3 and (CH3)3N |
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formal charge
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periodic table reference - (number of unpaired electrons) - number of bonds
ex) CH3-OH oxygen = 6 - (4unpaired) - (2bonds) = 0 etc |
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resonance
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measures stability
more resonance = more stability the one with (-) on more EN atom is more stable the one that has the lowest overall charge is also the most stable |
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lewis structure
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1. small/no formal charge
2. less separation of charges 3. (-) charges on EN atoms preferred arrangement |
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VSPER theory
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know
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electronic geometry
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describes the spatial arrangement of all pairs of electrons around the central atom; bonding and lone pairs included
ex) CH4, NH3, H2O have the same electronic geometry of sp3 = 4 pairs of electrons total linear, trigonal planar, tetrahedral, trigonal pyrimidal, octahedral |
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molecular geometry
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spatial arrangement of only the bonding pairs of electrons
ex) CH4 = tetrahedral NH3 = trigonal pyrimidal H2O = bent linear, trigonal planar, tetrahedral/bent/trigonal pyramidal, trigonal bipyramidal, octahedral |
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a compound with nonpolar bonds is ____ nonpolar
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always
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a compound with polar bonds is _____ polar
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sometimes;
polar vectors are capable of cancelling |
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polar bonds are capable of forming both ____ and _____ compounds
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polar; nonpolar
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a polar molecule must have _____ bonds
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polar
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subshells (refresh Q)
l = 0 --> l = 1 --> l = 2 --> l = 3 --> |
subshells
s p d f |
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bonding orbital forms when the signs of two atomic orbitals are ______
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the same
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antibonding orbitals form when the signs of two atomic orbitals are _____
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different
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a single bond creates a ____ bond
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sigma
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a double bond creates a ____ bond and a ____ bond
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sigma; pi
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a triple bond creates a ____ bond and 2 ____ bonds
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sigma; pi
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pi bonds do not allow for ______ unlike sigma bonds
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rotation about axis
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name the intermolecular forces
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london
dipole hydrogen |
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london forces
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weakest
found in everything short-lived dipole moments type of vander waals force force directly related to size |
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dipole forces
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polar molecules
more permanent dipole present in solid/liquid phases negligible in gase phases due to spacing between molecules -higher mp/bp due to dipoles polar > non polar with this also |
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hydrogen bonds
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hydrogens interact with F, O, N
dipole-interaction -strongest of the 3 -no sharing/transfer of electrons occurs in carboxylic acids, amines, alcohols, water high boiling points ex) NH3 > NH2R > NHR2 > NR3 due to hydrogen bond capabilities |
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Cr structure off table
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[Ar]4s1, 3d5
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1
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1
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1
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1
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