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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
Q

rise/depression of a liquid in a small passage such as tube

A

Capillarity

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26
Q

lesser cohesion than adhesion

A

Capillarity Rise

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27
Q

more cohesion than adhesion

A

Capillarity Fall

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28
Q

same molecules attracted to each other

A

Cohesion

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29
Q

one substance is attracted to another substance

A

Adhesion

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30
Q

tendency of particles to escape from liquid

A

Vapor Pressure

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31
Q

substance that has high vapor pressure at normal temperature

A

Volatile

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32
Q

atmospheric pressure boiling point of liquid

A

Normal Boiling Point

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33
Q

bubble expands fast

A

Bumping

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34
Q

energy required transform a given quantity of a substance from liquids to gas

A

Heat of Vaporization

35
Q

molecular geometry of water molecule

A

Tetrahedral geometry

36
Q

Water molecules are bonded with ionic or covalent bond

A

covalent bond

37
Q

flow of electrons from one place to another

A

Electricity

38
Q

materials do not conduct electricity

A

Electrical insulators

39
Q

transfer of energy between adjacent molecules

A

Conduction

40
Q

movement of hot liquid

A

Convection

41
Q

emission of electromagnetic rays

A

Radiation

42
Q

solid that have low heat conductivity

A

Heat Insulator

43
Q

ability to hammer a solid into sheet w/ breaking

A

Malleability

44
Q

stretch solid to form a wire

A

Ductility

45
Q

universal solvent/solution

A

Water

46
Q

amount of mass per unit volume

A

Density

47
Q

solid depends on the strength of IMF

A

Melting Point

48
Q

smallest repeating structure of solid

A

Unit cell

49
Q

14 types of lattice; named after Auguste Bravais

A

Bravais Lattice

50
Q

solids without form/pseudo solids (not true)

A

Amorphous solids

51
Q

solid to liquid

A

Melting

52
Q

liquid to solid

A

Freezing

53
Q

Liquid to gas

A

Evaporation

54
Q

Gas to liquid

A

Condensation

55
Q

Solid to gas

A

Sublimation

56
Q

gas to solid

A

Deposition

57
Q

A dynamic equilibrium is disturbed by changing conditions, the position of equilibrium shifts to counteract the change to reestablish an equilibrium

A

Le Chatelier’s Principle

58
Q

Art of changing inexpensive metals into expensive ones

A

Khemia

59
Q

behavior of matter

A

Kinetic Molecular Theory

60
Q

orderly repeating arrangement of particles

A

crystal lattice

61
Q

originated from Greek word khemeia

A

Alchemy

62
Q

chemistry came from Egyptian

A

Keme

63
Q

Keme means

A

Earth

64
Q

concerned composition, structure, properties of matter and changes during chemical reactions

A

Keme

65
Q

homogeneous of two substances uniformly distributed

A

Solution

66
Q

dissolved substance

A

Solute

67
Q

dissolved medium

A

Solvent

68
Q

low concentration in amount of solvent

A

Dilute solution

69
Q

maximum amount in given amount of solvent

A

Saturated solution

70
Q

more than maximum amount of solute in given amount of solvent

A

Supersaturated solution

71
Q

higher concentration of solution inside the cell

A

Hypotonic Solution

72
Q

causes cell to burst

A

Hypotonic solution

73
Q

equal concentration outside and inside cell

A

Isotonic solution

74
Q

higher concentration on the outside of the cell

A

Hypertonic solution

75
Q

causes cell to shrink

A

Hypertonic solution

76
Q

concentration of cell must be at equilibrium to ensure normal functioning

A

Tonicity

77
Q

moves particles faster causing dissolution faster

A

Stirring

78
Q

greater collision of solvent to solute particles increases the rate of dissolution

A

Heating

79
Q

smaller size of solute particles, greater surface area contact with solvent

A

Powdering

80
Q

To maintain the pressure exerted by CO2 on
the surface of the liquid. The solubility of CO2 decreases as the pressure is released

A

Henry’s Law

81
Q

proponent of Henry’s Law

A

William Henry

82
Q

high atmospheric pressure treatment

A

Hyperbaric

83
Q

amount of substance divided by total volume of mixture

A

Concentration

2ND SEM HAEYAJI (4 decks)

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