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71 Cards in this Set
- Front
- Back
Ionic bonding uses what types of elements?
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Metal to nonmetal
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Covalent bonding uses what type of elements?
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nonmetal to nonmetal
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Metallic bonding uses what type of elements?
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metal to metal
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Metals __ valence e- making them a ___
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lose.
cation. |
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nonmetals___ valence e- making them an ___
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gain.
anion. |
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Electronnegativity is
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the abiltiy of an element to attract e- to itself within a covalent bond
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Pure covalent bonds (nonpolar bonds) have no ____ moment.
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dipole
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Mass % =
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Mass Solute
______________ x 100 Mass Solution |
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Mole fraction =
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Mole solute/ mole soulte + mole slovent
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Molality =
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Moles of solute/ kg of slovent
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Molarity =
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Moles of soute/ L of solution
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Mass solution =
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mass solute + mass solvent
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Molarity containing density =
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mass solution= d solution x v solution
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metals lose ______ e- and become ______.
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valence, cations
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nonmetals gain ______ e- and become _______.
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valence, anions
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Ionic bonding
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metal to nonmetal
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covalent bonding
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metal to metal
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Nonpolar covalent bonds
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Bonds between two nonmetal atoms with equal EN.
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The _______ the EN, the closer bonding e- pair to itself
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greater
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polar molecules dissolve ________ molecules.
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polar
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nonpolar molecules dissolve __________ molecules.
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nonpolar
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intramolecular forces
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forces between atoms/ ions (within molecules)
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ion-dipole forces
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forces between ions and charge centers from polar molecules.
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dipole-dipole forces
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attraction of opposite charge poles of two molecules
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The more _____ the molecule the more attraction between molecules, the _____ the forces.
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Polar, stronger
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The more electrons, the more ________.
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polarizability
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The greater the ______ the more polarizability.
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size
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Down a group, polarizability
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increases
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Cross a period (L to R)
polarizability |
decreases
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less polarizable
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cations
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more polarizable
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anion
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The greater ________, the more space and easier for charge to
build up, the greater ________ _______ moment |
polarizability, instaneous, dipole
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The more ________ in a
molecule, the ______ size of a molecule, the _______ polarizability, the greater _________ |
electrons, bigger, greater, induced dipole
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London forces (Dispersion forces)
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Instantaneous dipole – induced dipole forces
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Exist in ALL covalent molecules
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London forces (Dispersion forces)
Instantaneous dipole – induced dipole forces |
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The more electrons within a molecule, the stronger _______.
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london forces
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The larger the molecule, the stronger ________
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london (dispersion) forces
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Occur in all polar molecules
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dipole-dipole forces
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The more polarity, the stronger the
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dipole forces
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London < dipole if molecules are less
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polarizable
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London > dipole if molecules are more
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polarizable
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The greater the intermolecular forces, the higher
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boiling point
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The greater intermolecular forces, the
more ________ molecules to move around |
difficult
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The higher the IM forces, the _______ ΔHvap, the _____ Pvap
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higher, lower
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The _______ the T, the ______ Pvap
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higher, higher
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A liquid “boils” when its vapor pressure is _______ to an
externally applied pressure |
equal
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Line where liquid and solid
phases exist in equilibrium |
fusion curve
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Line where liquid and gas
phases exist in equilibrium |
Vaporization curve
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Line where solid and gas
phases exist in equilibrium |
sublimation curve
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________ occurs when
substance has a triple point higher than 1 atm |
Sublimation
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A combination of lowest T, P
where liquid and gas phases are no longer distinct |
critical point
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The temperature on the
vaporization curve where Pressure is 1 atm |
normal boiling point
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The temperature on the fusion curve where Pressure is 1 atm
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normal melting point
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the slope of a positive fusion curve m.p. increases as P _______, solid occupies _______ space and has a ______ density.
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increases, less, greater
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P increases⇒ V ________, when the slope of fusion curve is positive.
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decreases
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m.p. ______ as P increase when the slope of the fusion curve is negative
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decreases
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When the slope of the fusion curve is negative, solid occupies _____ space and has _____ density.
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more, less
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different molecular forms of the same element
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allotropes
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2 C.C
0 lone pairs |
Linear
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3 C.C
0 lone pairs |
Trigonal planar
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3 C.C
1 lone pair |
Bent shape
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4 C.C
0 lone pairs |
Tetrahedral
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4 C.C.
1 lone pair |
Trigonal pyramidal
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4 C.C.
2 lone pairs |
Bent
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5 C.C.
0 lone pairs |
trigonal bipyramidal
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5 C.C.
1 lone pair |
seesaw
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5 C.C
2 lone pairs |
T-shape
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5 C.C
3 lone pairs |
linear
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6 C.C
0 lone pairs |
octahedral
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6 C.C
1 lone pair |
Square pyramidal
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6 C.C
2 lone pairs |
Square planar
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