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CHE 202 > chapter 11 > Flashcards

chapter 11 Flashcards

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1
Q

what is an intermolecular force?

A

attractive force that hold particles together in the condensed phases

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2
Q

what is a dipole-dipole interaction?

A

attractive force that acts between polar molecules

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3
Q

what is hydrogen bonding?

A

occurs in molecules that contain H bonded to a small, highly electronegative atoms, such as N, O, or F

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4
Q

what are dispersion forces?

A

forces that occur as a result of nonuniform distribution of electron density and create a fleeting, temporary dipole called an instantaneous dipole

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5
Q

what does a larger dipole moment mean?

A

stronger intermolecular force, which means a higher boiling point

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6
Q

what are London dispersion forces?

A

forces that arise out of dipoles that are induced by neighbouring molecules

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7
Q

what are ion-dipole interactions?

A

coulombic attractions between ions (+ or -) and polar molecules

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8
Q

the magnitude of ion-dipole interactions depend on the ________ and the _______ of the ion

A

charge; size

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9
Q

the magnitude of ion-dipole interactions depend on the _________ and _______ of the polar molecule

A

dipole moment; size

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10
Q

what is surface tension?

A

the amount of energy required to stretch or increase the surface of a liquid by a unit area

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11
Q

a liquid with strong intermolecular forces has a ______ surface tension

A

high

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12
Q

what is viscosity?

A

measure of a liquid’s resistance to flow

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13
Q

what does a higher viscosity mean?

A

stronger intermolecular forces

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14
Q

vapour pressure increases with ___________

A

temperature

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15
Q

the ____________ of intermolecular forces is what determines whether the particles that make up a substance are a gas, liquid, solid

A

magnitude

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16
Q

what is a van der Waals force?

A

attractive forces between atoms or molecules in a pure substance and they include dipole-dipole interactions, including hydrogen bonding and dispersion forces

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17
Q

what is interesting about hydrogen bonding?

A

molecules capable of hydrogen bonding have a higher boiling point than expected based on molecular size trends

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18
Q

what does the magnitude of disperson forces depend on?

A

it depends on how easily the molecule’s electrons can be polarized and the polarizability of a molecule increases with increasing number of electrons

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19
Q

what is vapor pressure?

A

pressure of gas above liquid

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20
Q

what is special about substanes with high vapor pressures at room temperature?

A

they are said to be volatile (able to shift from the liquid to gas phase quickly)

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21
Q

higher vapor pressure indicates _________ intermolecular forces

A

weak

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22
Q

what is a crystalline solid?

A

it possesses rigid and long-range order; it’s atoms, molecules, or ions occupy specific positions

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23
Q

what is the arrangement of the particles in a crystalline solid and what does it depend on?

A

it is called the lattice structure and it depend on the nature and size of the particles involved

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24
Q

what is a unit cell?

A

a unit cell is the basic repeating structural unit of a crystalline solid

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25
what does each sphere in a unit cell represent?
it represents an atom, ion, or molecule and is called a lattice point
26
what is a coordination number and what does it indicate?
it is the number of atoms surrounding an atom in a crystal lattice and it indicates how tightly the atoms are packed together - the larger the coordination number, the closer the atoms are to one another
27
what is a simple cubic cell (scc) and what are the other types of cubic cells?
* it is the basic repeating unit in the array of atoms and is also called the primitive cubic cell * the other types of cubic cells are the body-centered cubic cell (bcc) and the face-centered cubic cell (fcc)
28
how many particles are in each unit cells?
* scc: 1 particle per cell * bcc: 2 particles per cell * fcc: 4 particles per cell
29
what are the coordination numbers of all the cubic cells?
* scc: 6 * bcc: 8 * fcc: 12
30
how many unit cells share the corner atom?
8 unit cells
31
how many unit cells share an edge atom?
4 unit cells
32
how many unit cells share a face-centered atom
2 unit cells
33
what is the hexagonal close-packed structure
34
what is the cubic-close packed structure?
35
how many spheres per unit cell does a CCP arrangement have?
A CCP arrangement has a total of 4 spheres per unit cell
36
how many spheres per unit cell does a HCP arrangement have?
an HCP arrangement has 8 spheres per unit cell.
37
what is the coordination number of the CCP and HCP structure?
both configurations have a coordination number of 12
38
what are ionic crystals?
they are composed of anions/cations held together by Coulombic forces
39
what determines the crystal structure?
Size and relative number of each ion determines the crystal structure.
40
what are the characterisitics of an ionic crystal?
* High melting point. * High lattice energy. * Does not conduct electricity.
41
what are covalent crystals?
the atoms are held together in an extensive, three-dimensional network entirely by covalent bonds
42
what are molecular crystals?
the lattice points are occupied by molecules, so the attractive forces between them are van der Waals forces and/or hydrogen bonding
43
what are metallic crystals?
every lattice point in a metallic crystal is occupied by an atom of the same metal. metallic crystals are usually BCC, FCC, or HCP
44
what are the cohesive forces in ionic crystals?
coulombic attraction and dispersion forces
45
what are the cohesive forces in covalent crystals?
covalent bonds
46
what are the cohesive forces in molecular crystals?
dispersion and dipole-dipole forces, and hydrogen bonds
47
what are the cohesive forces in metallic crystals?
metallic bonds
48
what are the general properties of ionic crystals?
they are hard, brittle, have a high melting point, and are poor conductors of heat and electricity. ie: NaCl, LiF, MgO, and CaCO3
49
what are the general properties of covalent crystals ?
they are hard, brittle, have high melting points, and are poor conductors of heat and electricity. ie: C (diamond)\* and SiO2 (quartz)
50
what are the general properties of molecular crystals?
they are soft, have low melting points, and are poor conductors of heat and electricity ie: Ar, CO2, I2, H2O, C12H22O11
51
what are the general properties of metallic crystals?
they have variable hardness and melting points, and they are good conductors of heat and electricity. ie: all metallic elements, such as Na, Mg, Fe, and Cu
52
what are amorphous solids?
they lack a regula three-dimensional arrangement of atoms. ie: glass
53
what is a phase?
homogeneous part of a system that is separated from the rest of the system by a well- defined boundary.
54
what is a phase change?
When a substance goes from one phase to another phase
55
describe phase changes as they undergo changes in temperature
56
what is a boiling point?
the temperature at which its vapor pressure equals the external, atmospheric pressure
57
what is a normal boiling point?
The temperature at which the vapor pressure of a liquid is equal to 1 atm
58
how do particles interact with intermolecular forces? (the chart)
59
what is the molar heat of vaporization (ΔHvap)?
it is the amount of heat required to vaporize a mole of substance at its boiling point
60
what is a critical temperature (Tc)?
the temperature above which its gas phase cannot be liquified, no matter how great the applied pressure
61
what is the critical pressure (Pc)?
it is the minimum pressure that must be applied to liquify a substance at its critical temperature
62
what is a supercritical fluid?
a fluid at a temperature and pressure that exceed Tc and Pc
63
what is the molar heat of fusion ( ΔHfus)?
energy required to melt 1 mole of a solid
64
what is supercooling?
a phenomenon in which a liquid can be temporarily cooled to below its freezing point
65
how does solid-liquid phase transition work?
66
what is the molar enthalpy of sublimation ( ΔHsub)?
the eneergy required to sublime 1 mole of a solid
67
what is a phase diagram?
summarizes the conditions (temperature and pressure) at which a substance exists as a solid, liquid, or gas.

CHE 202 (5 decks)

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