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G12 Q3 > GC2 > Flashcards

GC2 Flashcards

1
Q
  • provides an overview of the microscopic properties of molecules or atoms and their interactions.
  • It describes the microscopic properties of matter and how they translate to the state and other properties of matter.
A

kinetic molecular theory of matter

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2
Q

Kinetic Molecular Theory of Matter 4 statements:

A
  1. Matter is composed of small particles.
  2. The molecules interact with one another through attractive forces. The strength of these forces is related to the distance between the particles.
  3. These molecules are always in constant random motion.
  4. The temperature of a substance is a measure of the average kinetic energy of the molecules.
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3
Q

The attractive forces between molecules are known as the

A

intermolecular forces or IMFA

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4
Q

The stronger the interaction between two molecules, the ____ their distance will be.

A

smaller

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5
Q

Higher temperature means (faster/slower) motion?

A

faster

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6
Q

Stronger IMFAs means means
(faster/slower) motion

A

slower

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7
Q

Solids have …. motion.

A

restricted

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8
Q

TRUE or FALSE: Liquid particles are able to move past each other

A

TRUE

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9
Q

TRUE or FALSE: Gas particles are able to move in relatively small distances.

A

FALSE; long distances

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10
Q

are therefore consequences of the capabilities of their molecules to move about.

A

States

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11
Q

TRUE or FALSE: Temperature plays a role in determining the
state of matter.

A

TRUE

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12
Q
  • refers to the uneven distribution of charge over the whole molecule or large portion of it.
A

Molecular polarity

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13
Q

The distribution of charges in molecules is determined by the electrons. Where electrons reside more often, that region becomes more (positive/negative).

A

negative

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14
Q

Molecular polarity is determined by

A
  • The polarity of the individual bonds that make up the molecules
  • The molecular geometry of the molecule.
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15
Q

The polarity of the bonds in a molecule is determined by … of the atoms in the bond.

A

electronegativity

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16
Q

is the ability of an atom to pull towards itself the shared electrons in a bond.

A

Electronegativity

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17
Q

Less than 0.4

A

nonpolar

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18
Q

0.4–1.8

A

polar

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19
Q

More than 1.8

A

ionic

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20
Q

TRUE or FALSE: The polarity of bonds in a molecule alone do not determine whether the entire molecule itself will be polar or nonpolar.

A

TRUE

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21
Q

TRUE or FALSE: If the atoms bonded to a central atom are the same and they make polar bonds, the geometry ultimately don’t determines the polarity of the molecule.

A

FALSE; it does determine the polarity of the molecule

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22
Q

attractive forces present in between molecules.

A

Intermolecular forces

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23
Q

is the interaction between oppositely charged particles.

A

Ion-ion interaction

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24
Q

TRUE or FALSE: Atoms with higher electronegativity will attract electrons towards itself more than those with lower electronegativity.

A

TRUE

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25
If a molecule is polar, then it is considered to be a ..., one wherein one side is partially positive, and one side wherein it is partially negative.
dipole
26
happen when an ion attracts a dipole so that the opposite charges attract each other.
Ion-dipole interactions
27
Attraction can also happen between two dipoles.
dipole-dipole interactions
28
A special interaction similar to a dipole-dipole interaction is present when a hydrogen atom is attached to highly electronegative element (F, O, N). This is called the
hydrogen bond
29
These molecules also rely on the presence of dipoles. However, these dipoles are only temporary. These interactions are called
London dispersion forces
30
Because of the temporary dipoles, London dispersion forces are the (strongest, weakest)
weakest
31
TRUE or FALSE: The properties of liquids can be attributed to the intermolecular forces of attraction that hold the molecules together in order to occupy a volume of a certain space of a container.
TRUE
32
Liquid properties that can be attributed to the IMFAs are
surface tension, viscosity, and vapor pressure.
33
- is the tendency of a fluid to acquire the least possible surface area. - It is caused by the different attractive forces felt by molecules within the interior of the liquid and those found near the surface.
surface tension
34
Which molecule seem to experience a greater net force of attraction: the molecule inside or the molecule near the surface?
near the surface
35
TRUE or FALSE: to increase attractions and become more stable, a surface molecule tends to move towards the exterior.
FALSE; interior
36
is the attraction between unlike molecules
Adhesion
37
is the attraction between like molecules
Cohesion
38
TRUE or FALSE: The relative magnitudes of adhesion and cohesion in a liquid affects how they interact with other materials.
TRUE
39
is the curved upper surface of a liquid in a tube
meniscus
40
TRUE or FALSE: The shape of the meniscus is dependent on adhesive and cohesive forces.
TRUE
41
In a liquid having a concave meniscus, which is stronger, adhesion or cohesion?
adhesion
42
is the measure of a fluid’s resistance to flow
Viscosity
43
Molecules with (weaker/stronger) intermolecular forces have greater viscosity
stronger
44
When the temperature is high, the molecules have (less/more) energy and it becomes (easier/harder) to overcome the IMFA. This leads to (lower/higher) viscosity.
more, easier, lower
45
is the process where a fraction of the kinetic energy of a liquid escapes from the surface to enter the vapor phase.
Vaporization
46
is the heat required to induce this phase change.
enthalpy of vaporization (∆Hvap), also called the heat of vaporization
47
Vaporization occurs more readily with (Higher/Lower) temperature
higher
48
Vaporization occurs more readily with - (Larger/Smaller) surface area of the liquid - (Stronger/Weaker) IMFAs
larger, weaker
49
is the pressure exerted by a vapor in equilibrium with its liquid phase in a closed system
Vapor pressure
50
TRUE or FALSE: Molecules with stronger intermolecular forces have less tendency to escape into gas, and thus, have lower vapor pressure compared to those with weaker IMFA
TRUE
51
is the temperature at which a substance changes from liquid to gas. Specifically, it is the temperature at which the vapor pressure of a liquid becomes equal to the atmospheric pressure.
Boiling point
52
specific heat capacity (liquid water)
4.18 J/g · ºC
53
specific heat capacity (water vapor)
2.11 J/g · ºC
54
specific heat capacity (ice)
2.00 J/g · ºC
55
This formation that results from an ion being surrounded by several water molecules is called a
hydration shell or hydration sphere
56
TRUE or FALSE: Like dissolves like
CHREW
57
Both has hydrophilic and hydrophobic parts
Amphiphatic
58
is the amount of heat required to raise the temperature of a substance by 1 ºC
Heat capacity
59
refers to the amount of heat required to raise the temperature of one gram of a substance by 1 ºC.
Specific heat capacity
60
TRUE or FALSE: The hydrogen bonds are able to absorb the energy in the form of heat. That’s why water does not increase its temperature as easily as the others.
TRUE
61
ice is (less/more) dense than water
less
62
substances less dense than water tend to…
float
63
- They are solids in which the atoms, ions, or molecules are arranged in a regular repeating pattern. - Held together by strong and uniform IMFAs. - Results in solids having regular shapes.
Crystalline Solids
64
- The smallest repeating pattern in crystalline solids - Made of a unique arrangement of atoms - Represent the structure of the solid - The entire crystal structure can be built by piling the unit over and over
Unit Cell
65
- Lacks the order found in crystalline solids - Structures at the atomic level are similar to liquids. - Does not have the well-defined shape of a crystal
Amorphous Solids
66
TRUE or FALSE: Crystalline solids have a precise melting point, while amorphous solids melt over a wide temperature range.
TRUE
67
is the quantity of heat necessary to melt a solid.
heat of fusion
68
Solids with stronger IMFAs have (lower/higher) heats of fusion
HIGHER
69
TRUE or FALSE: For crystalline solids, the heat of fusion is fixed and definite. Amorphous solids have no precise values.
CHREW
70
is the property of substances where the physical and mechanical properties vary with different orientation and molecular axes. Exhibited by crystalline solids.
Anisotropy
71
is the property of substances where the physical and mechanical properties are equal in all directions. Exhibited by amorphous solids.
Isotropy
72
is the ability of a solid to be formed into a variety of shapes by hammering it or rolling it into thin sheets.
Malleability
73
is ability of a material to have its shape changed (usually by pulling) without losing strength or breaking.
Ductility
74
TRUE or FALSE: Most of the time, malleability and ductility don't coexist.
FALSE; it does coexist most of the time

G12 Q3 (11 decks)

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