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2ND SEM HAEYAJI > CHEM2 > Flashcards

CHEM2 Flashcards

1
Q

determines the chemical properties of liquids and solids

A

Covalent Bond

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2
Q

highly ordered packing arrangement of crystalline structure

A

Crystal Lattice

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3
Q

allowing molecules to freely move; capacity to flow

A

Liquids

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4
Q

more dense and less compressible than gases

A

Liquids

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5
Q

definite volume; independent size and shape

A

Liquids

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6
Q

not very compressible due to lack of space

A

Solids

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7
Q

strong enough to keep locked in position

A

Solids

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8
Q

movement of molecules and move around

A

Kinetic Energy

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9
Q

force that keeps particles attached together

A

Intermolecular Forces

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10
Q

As the pressure increases, the IMF

A

Increases

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11
Q

Pressure and temperature have ___ proportional relationship

A

Indirectly

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12
Q

property of crystalline solids where different direction has different reaction

A

Anisotropy

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13
Q

property are equal regardless of the direction which force is applied

A

Isotropic

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14
Q

type of solid that has no orderly internal structure

A

Amorphous solids

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15
Q

highly electronegative atoms attaches with hydrogen atom such as F, O, N

A

Hydrogen Bonds

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16
Q

between oppositely charged poles of polar molecules

A

Dipole-dipole forces

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17
Q

ion and polar molecule

A

Ion-dipole forces

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18
Q

weak IMF arise from interactive forces between induced dipoles

A

Dispersion/ London-dispersion forces

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19
Q

Proposed London-dispersion forces

A

Fritz London

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20
Q

molecules attract each other at a moderate range

A

Van der Waals Force

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21
Q

proponent of van der waals force

A

Johaness Diderik Van Der Waals

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22
Q

Polar covalent forces has ___ IMF

A

strong

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23
Q

cohesive forces between liquid molecules

A

Surface Tension

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24
Q

fluid’s resistance to flow

A

Viscosity

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25
rise/depression of a liquid in a small passage such as tube
Capillarity
26
lesser cohesion than adhesion
Capillarity Rise
27
more cohesion than adhesion
Capillarity Fall
28
same molecules attracted to each other
Cohesion
29
one substance is attracted to another substance
Adhesion
30
tendency of particles to escape from liquid
Vapor Pressure
31
substance that has high vapor pressure at normal temperature
Volatile
32
atmospheric pressure boiling point of liquid
Normal Boiling Point
33
bubble expands fast
Bumping
34
energy required transform a given quantity of a substance from liquids to gas
Heat of Vaporization
35
molecular geometry of water molecule
Tetrahedral geometry
36
Water molecules are bonded with ionic or covalent bond
covalent bond
37
flow of electrons from one place to another
Electricity
38
materials do not conduct electricity
Electrical insulators
39
transfer of energy between adjacent molecules
Conduction
40
movement of hot liquid
Convection
41
emission of electromagnetic rays
Radiation
42
solid that have low heat conductivity
Heat Insulator
43
ability to hammer a solid into sheet w/ breaking
Malleability
44
stretch solid to form a wire
Ductility
45
universal solvent/solution
Water
46
amount of mass per unit volume
Density
47
solid depends on the strength of IMF
Melting Point
48
smallest repeating structure of solid
Unit cell
49
14 types of lattice; named after Auguste Bravais
Bravais Lattice
50
solids without form/pseudo solids (not true)
Amorphous solids
51
solid to liquid
Melting
52
liquid to solid
Freezing
53
Liquid to gas
Evaporation
54
Gas to liquid
Condensation
55
Solid to gas
Sublimation
56
gas to solid
Deposition
57
A dynamic equilibrium is disturbed by changing conditions, the position of equilibrium shifts to counteract the change to reestablish an equilibrium
Le Chatelier's Principle
58
Art of changing inexpensive metals into expensive ones
Khemia
59
behavior of matter
Kinetic Molecular Theory
60
orderly repeating arrangement of particles
crystal lattice
61
originated from Greek word khemeia
Alchemy
62
chemistry came from Egyptian
Keme
63
Keme means
Earth
64
concerned composition, structure, properties of matter and changes during chemical reactions
Keme
65
homogeneous of two substances uniformly distributed
Solution
66
dissolved substance
Solute
67
dissolved medium
Solvent
68
low concentration in amount of solvent
Dilute solution
69
maximum amount in given amount of solvent
Saturated solution
70
more than maximum amount of solute in given amount of solvent
Supersaturated solution
71
higher concentration of solution inside the cell
Hypotonic Solution
72
causes cell to burst
Hypotonic solution
73
equal concentration outside and inside cell
Isotonic solution
74
higher concentration on the outside of the cell
Hypertonic solution
75
causes cell to shrink
Hypertonic solution
76
concentration of cell must be at equilibrium to ensure normal functioning
Tonicity
77
moves particles faster causing dissolution faster
Stirring
78
greater collision of solvent to solute particles increases the rate of dissolution
Heating
79
smaller size of solute particles, greater surface area contact with solvent
Powdering
80
To maintain the pressure exerted by CO2 on the surface of the liquid. The solubility of CO2 decreases as the pressure is released
Henry's Law
81
proponent of Henry's Law
William Henry
82
high atmospheric pressure treatment
Hyperbaric
83
amount of substance divided by total volume of mixture
Concentration

2ND SEM HAEYAJI (4 decks)

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