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General Chemistry > Lesson 1 - MATTER > Flashcards

Lesson 1 - MATTER Flashcards

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1
Q

HE STUDY THAT DEALS WITH THE STRUCTURE

COMPOSITIONS, REACTION OF MATTER AND THE CHANGES THAT IT UNDERGOES

A

CHEMISTRY

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2
Q

ANYTHING THAT OCCUPIES SPACE AND HAS MASS

A

MATTER

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3
Q

Differentiate Mass from Weight

A

Mass - amount of matter in an object

Weight - a measure of how the force of gravity acts upon that mass

rationale:

your body’s mass is a set value for both, but your weight is different on the Moon compared with on Earth

If you change your location with respect to gravity, mass will remain unchanged, but weight will not.

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4
Q

objective

A

Mass

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5
Q

subjective

A

Weight

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6
Q

3 KINETIC THEORY OF MATTER

A

ALL MATTER IS COMPOSED OF SMALL PARTICLES (ATOM)

THESE PARTICLES ARE IN CONSTANT MOTION

THESE PARTICLES ARE COLLIDING WITH EACH OTHER AND THE WALLS OF THEIR CONTAINE

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7
Q

CLASSIFICATION OF MATTER (BASED ON

PHYSICAL STATE): VOLUME

A

SOLID - DEFINITE (because they are solids?)

LIQUID - DEFINITE
(liquids follow the shape of their container)
ex. 2ml of liquid is still 2ml in a different container

GAS - INDEFINITE (cannot be measured in ml)

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8
Q

CLASSIFICATION OF MATTER (BASED ON

PHYSICAL STATE): SHAPE

A

SOLID - DEFINITE

LIQUID - INDEFINITE (their shapes are dynamic, they follow the shape of their container)

GAS - INDEFINITE

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9
Q

CLASSIFICATION OF MATTER (BASED ON

PHYSICAL STATE): MOLECULAR MOTION

A

SOLID - VIBRATION (compact molecules vibrate)

LIQUID - GLIDING (ex. waves)

GAS - WEAKEST

keyword: molecular motion; collisions of molecules
rationale: The intermolecular space between gaseous molecules is very large, thus, making their molecular motion the weakest

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10
Q

CLASSIFICATION OF MATTER (BASED ON

PHYSICAL STATE): TEMPERATURE

A

SOLID - LOWEST TEMPERATURE; molecules are together

LIQUID - LOWER TEMPERATURE; gas condenses

GAS - HIGH TEMPERATURE;
rationale: molecules are moving around faster and have less chance of sticking together
LOW PRESSURE; molecules are far apart from each other and won’t interact as much

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11
Q

GAS

A

HIGH KINETIC ENERGY (the are large spaces between molecules, thus, higher energy)

WEAK ATTRACTIVE FORCES

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12
Q

SUPER HEATED MATTER. ELECTRONS ARE RIPPED AWAY FROM THE ATOMS FORMING IONIZED GAS

A

PLASMA

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13
Q

ionized gas between cation and anion in a superheated condition

A

PLASMA

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14
Q

group of atoms cooled to within a hair of absolute zero.

A

Bose-Einstein condensate

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15
Q

Similarities of both

A

Collision of cations and anions

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16
Q

KINETIC MOLECULAR THEORY OF GASES

A

TOTAL VOLUME OF GAS IS NEGLIGIBLE COMPARED TO THE VOLUME OF SPACE

GAS PARTICLES DO NOT ATTRACT ONE ANOTHER BUT RATHER MOVE INDEPENDENTLY FROM EACH OTHER

PARTICLES EXHIBIT CONTINUOUS RANDOM MOVEMENT DUE TO THEIR KINETIC ENERGY.

GAS MOLECULES EXHIBIT PERFECT ELASTICITY

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17
Q

KEY OBSERVATIONS IN GASES

A

NTERMOLECULAR FORCES OF ATTRACTION IN GASES ARE VIRTUALLY NON EXISTENT AT
ROOM TEMPERATURE

MOLECULES IN THE GASEOUS STATE MOVE IN ALL DIRECTIONS, AT HIGH VELOCITIES UNTIL
COLLISIONS OCCUR

THEY EXERT PRESSURE AT FORCE PER UNIT AREA EXPRESSED IN ATMOSPHERE OR IN MMHG

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18
Q

WHEN A GAS IS COOLED, IT LOSES SOME OF ITS KINETIC ENERGY IN THE FORM OF HEAT, AND THE VELOCITY OF THE MOLECULES DECREASES

A

LIQUEFACTION OF GASES

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19
Q

VAN DER WAALS

INTERACTION FORCES

A

BECAUSE OF THESE, LIQUIDS ARE CONSIDERABLY DENSER THAN GASES AND OCCUPY A DEFINITE VOLUME.

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20
Q

SOLID STATES: 3 TYPES

A

CRYSTALLINE
AMORPHOUS
POLYMERIC

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21
Q

CRYSTALLINE (diamonds, sugar, table salt)

A

atoms vibrate in a fixed pattern

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22
Q

AMORPHOUS (powder like structure)

A

vibrate in random arrangements

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23
Q

TRUCTURAL UNITS OF CRYSTALLINE SOLIDS (ice, sodium chloride, etc)

A

ARRANGED IN FIXED GEOMETRIC PATTERN

-HAVE DEFINITE SHAPES AND AN
ORDERLY ARRANGED UNITS

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24
Q 
CUBIC
TETRAGONAL
HEXAGONAL
RHOMBIC
MONOCLINIC
TRIGONAL
A 
SODIUM CHLORIDE
UREA
IODOFORM
IODINE
SUCROSE
BORIC ACID
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25
Q

THE HARDNESS AND STRENGTH OF METALS DEPEND ON…

A

LATTICE DEFECTS (IMPERFECTIONS) IN THEIR CRYSTAL

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26
Q

can be seen under microscope

A

Atomic crystals and organic structures

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27
Q

Crystal System

A

Visible because of indicators

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28
Q

AMORPHOUS

A

depends of the level of extraction; glasses; no definite color

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29
Q

SOLIDS THAT HAVE MORE THAN CRYSTALLINE FORMS

A

POLYMORPHS

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30
Q

Plasma to gas

A

deionization

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31
Q

gas to plasma

A

ionization

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32
Q

gas to solid

A

deposition

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33
Q

solid to gas

A

sublimation

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34
Q

gas to liquid

A

condensation

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35
Q

liquid to gas

A

vaporization

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36
Q

solid to liquid

A

melting

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37
Q

liquid to solid

A

freezing

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38
Q

FACTORS AFFECTING PHASE TRANSITIONS

A

NTENSITY OF INTERMOLECULAR FORCES

TEMPERATURE.

ENTHALPY - each transition/transformation

ENTROPY ( MOLECULAR RANDOMNESS) - from start to finish; complete cycle

LATENT HEAT - CHANGE OF STATE TAKES PLACE WITHOUT A TEMPERATURE CHANGE.

HEAT OF VAPORIZATION

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39
Q

AMOUNT OF ENERGY REQUIRED FOR A SUBSTANCE TO GO FROM SOLID TO LIQUID

A

HEAT OF FUSION

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40
Q

(SOLID-LIQUID-GAS)

ENERGY REQUIRING

A

ENDOTHERMIC CHANGE

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41
Q

(GAS- LIQUID-SOLID)

REMOVAL OF ENERGY

A

EXOTHERMIC CHANGE

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42
Q

AMOUNT OF ENERGY REQUIRED TO CHANGE A LIQUID TO GAS

A

HEAT OF EVAPORATION

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43
Q

ANY PROPERTY OF A SOLUTION THAT
DEPENDS ON THE NUMBER OF SOLUTE
PARTICLES; NOT IN ITS NATURE

A

COLLIGATIVE PROPERTY

44
Q

“plain water easily boils than water with ingredients added” - aka ung sa sinigang

A

BOILING POINT ELEVATION

-BOILING POINT - VAPOUR PRESSURE EQUALS THE
ATMOSPHERIC PRESSURE

45
Q

boiling point of water

A

100°C (212°F)

46
Q 
a drop in the temperature at which a 
substance freezes (plain water cools faster)
A

FREEZING POINT DEPRESSION

47
Q

AMOUNT OF EXTERNAL PRESSURE THAT MUST BE

APPLIED TO MORE CONCENTRATED SOLUTION

A

OSMOTIC PRESSURE

48
Q

Why is there a need for osmosis?

-from lower to higher concentration

A

for chemical equilibrium and homeostasis

rationale: when a persons perspires, ions will be released, thus making the low concentrated part of the blood vessels need more nutrients. Storage of ions will then provide ions to the low concentration which came from drinks, vitamins a person intakes.

49
Q

PROPERTIES THAT CAN BE MEASURED AND
OBSERVED WITHOUT CHANGING THE
MATERIAL’S COMPOSITION

A

PHYSICAL PROPERTIES

COLOR
DENSITY
VOLUME
MASS
BOILING POINT
50
Q

MATERIAL’S POSSIBILITY TO UNDERGO
CHEMICAL CHANGE IN ITS CHEMICAL
COMPOSITION

A

CHEMICAL PROPERTIES

CHEMICAL REACTIVITY
TOXICITY
FLAMMABILITY
OXIDATION STATE
CHEMICAL STABILITY
51
Q

PROPERTIES THAT DO NOT DEPEND ON THE

AMOUNT OF THE SUBSTANCE.

A

INTRINSIC PROPERTIES

BOILING POINT
DENSITY
STATE OF MATTER
COLOR
MELTING POINT
ODOR
TEMPERATURE
52
Q

DEPENDS ON THE AMOUNT OF SUBSTANCE

A

EXTRINSIC PROPERTIES

MASS
VOLUME
LENGTH
DIMENSION

53
Q

changes where chemical reaction changes the product

A

Chemical Changes

combustion
rusting
digestion
rotting

54
Q

matter changes but the chemical composition does not

A

Physical Changes

melting
shredding
boiling
chopping

55
Q

CANNOT BE SEPARATED INTO SIMPLER COMPOUNDS BY CHEMICAL MEANS

A

ELEMENT

56
Q

COMPOSED OF 2 OR MORE ELEMENTS

A

COMPOUND

57
Q

BASIC UNIT OF ELEMENT OR MATTER

A

ATOM

58
Q

ATLEAST TWO ATOMS

A

MOLECULES

59
Q

ATOM OR GROUP OF ATOMS WITH (+) OR (-) CHARGES.

A

ION

60
Q

COMPONENTS CAN BE SEPARATED BY PHYSICAL MEANS

A

MIXTURE

heterogeneous - not uniform
homogeneous - uniform

61
Q

CANNOT BE BROKEN DOWN THROUGH PHYSICAL

MEANS

A

PURE SUBSTANCE

62
Q

uniform throughout at the molecular level; equally distributed, most stable

A

SOLUTIONS

solute - dissolved
solvent - dissolves

63
Q 
ATLEAST TWO PHASES WITH ONE OR 
MORE DISPERSED (INTERNAL) PHASES CONTAINED IN A 
SINGLE CONTINUOUS (EXTERNAL) PHASE
A

DISPERSION

64
Q

DESCRIPTIVE TERMS OF SOLUBILITY

A 
VERY SOLUBLE = 1
FREELY SOLUBLE 1-10
SOLUBLE 10-30
SPARINGLY SOLUBLE 30-100
SLIGHTLY SOLUBLE 100-1000
VERY SLIGHTLY SOLUBLE 1000-10,000
PRACTICALLY INSOLUBLE >/= 10,000
65
Q

MAXIMUM AMOUNT OF SOLUTE THAT CAN BE DISSOLVED IN A

GIVEN AMOUNT OF SOLVENT

A

SOLUBILITY

66
Q

CLASSIFICATION OF SOLUTION

A.) BASED ON ELEMENTAL COMPOSITION

A

ORGANIC- COMPOUNDS CONTAINING CARBON
(EXCEPT CO2, CARBONATES AND CYANIDES)

INORGANIC- COMPOUNDS OF OTHER ELEMENTS
INCLUDING ACIS, BASES, SALTS

67
Q

CLASSIFICATION OF SOLUTION

B.) BASED ON IONIZATION/ ELECTROLYTIC PROPERTY OF SOLUTE

A

1.) ELECTROLYTES

STRONG ELECTROLYTES

WEAK ELECTROLYTES

2.) NON-ELECTROLYTES

68
Q

CONTAIN IONS; CONDUCT ELECTRICITY

EX: SALTS/SODIUM CHLORIDE

A

STRONG ELECTROLYTES

69
Q

PRODUCES SMALL AMOUNTS OF IONS; PARTIALLY DISSOCIATED INTO IONS.
EX: acetic acid “suka”CH3 COOH

A

WEAK ELECTROLYTES

70
Q

DOES NOT DISSOCIATE INTO IONS; FORM CONDUCTING SOLUTIONS.

EXAMPLE: UREA, SUGAR, GLYCERIN, NAPHTHALENE

A

NON-ELECTROLYTES

71
Q

TYPES OF SOLUTION

A

DILUTE

CONCENTRATED

72
Q

SOLUTION WITH LOW SOLUTE

CONCENTRATION

A

DILUTE

73
Q

ONE WITH HIGH SOLUTE

CONCENTRATION

A

CONCENTRATED

74
Q

TYPES OF SOLUTION BASED ON DEGREE OF SATURATION

A

UNSATURATED
SATURATED
SUPERSATURATED

75
Q

LOW SOLUTE; more solute dissolved

A

UNSATURATED

76
Q

NORMAL SOLUTE; no more solute dissolves

A

SATURATED

77
Q

HIGH SOLUTE; crystals may grow

A

SUPERSATURATED

78
Q

FACTORS
AFFECTING
SOLUBILITY

A

TEMPERATURE - higher temp, higher solubility

NATURE OF SOLUTE AND SOLVENT

POLARITY

PRESSURE (FOR GASES)

EFFECT OF DISSOLVED SUBSTANCES ON

SOLUBILITY

PARTICLE SIZE/ SURFACE AREA

MOLECULAR SIZE

BOILING POINT

INFLUENCE OF SUBSTITUENT

CRYSTAL PROPERTIES

PH LEVEL

79
Q

releases energy in the form of heat

A

exothermic reactions

80
Q

absorbs energy in the form of heat

A

endothermic reactions

81
Q

hydrophilic - hydrophobic

A

water loving - water hating

82
Q

NATURE OF SOLUTE AND SOLVENT

A

MISCIBLE LIQUIDS - LIQUID TO LIQUID
EX. ETHANOL AND WATER

IMMISCIBLE LIQUIDS- LIQUIDS THAT DO NOT MIX.
EX. OIL AND WATER

MISCIBILITY- SOLUBILITY BETWEEN GASES OR LIQUIDS

83
Q

LIQUID-LIQUID SYSTEM MAY BE DIVIDED INTO 2 CATEGORIES

A

COMPLETE MISCIBILITY - ALCOHOL AND WATER

PARTIAL MISCIBILITY - PHENOL AND WATER

84
Q

lipophilic

A

oil loving

85
Q

lipophobic

A

oil hating

86
Q

CORRELATION OF 4 PHOBICS AND PHILICS

A

most solvents are hydrophilic and lipophilic

all lipophilic are hydrophilic, all hydrophilic are lipophobic

87
Q

both oil and water

A

amphoteric

-because of emulsifiers

88
Q

makes chemical reactions to the amphoteric

A

emulsifiers

89
Q

makes the surface area to a certain size to be fairly dissolved

A

emulsion

-finds the common denominator using the surface area

90
Q

SUBSTANCES WITH SIMILAR
INTERMOLECULAR ATTRACTIVE
FORCES TEND TO BE SOLUBLE IN ONE
ANOTHER

A

LIKE DISSOLVES LIKE

91
Q

POLAR- POLAR

SALTS, SUGAR DISSOLVES IN WATER

A

has hydrogen atoms which is easier to attract into substances that are more stable

92
Q

NON POLAR - NON POLAR
(NAPHTHALENE DISSOLVES IN
BENZENE)

A

oily, made from a lot of hydrogen

93
Q

blackening of oil; chemical reaction

A

hydrogenation

94
Q

PRESSURE (FOR GASES)

A

PRESSURE ABOVE THE SOLUTION IS RELEASED, THE
SOLUBILITY OF THE GAS DECREASES

TEMPERATURE INCREASES THE SOLUBILITY OF GASES DECREASES

95
Q

EFFECT OF DISSOLVED SUBSTANCE ON SOLUBILITY

A

ELECTROLYTES LOWERS SOLUBILITY OF GASES

HIGH DISSOLVED SUBSTANCE = LOW SOLUBILITY

96
Q

PARTICLE SIZE (SURFACE AREA)

A

LOW PARTCLE SIZE, HIGH SURFACE AREA AND SOLUBILITY

97
Q

MOLECULE SIZE

A

LARGER MOLECULES ARE MORE
DIFFICULT TO SURROUND WITH
SOLVENT MOLECULES IN ORDER TO
SOLVATE THE SUBSTANCE

98
Q

THE INFLUENCE OF SUBSTITUENTS

A

HYDROPHOBIC OR HYDROPHILIC, DEPENDING ON THEIR POLARITY

non polar - lipophilic; hydrophobic
polar - hydrophilic; lipophobic

99
Q

SUBSTITUENTS POSITIONS

A

SUBSTITUENT
META, 4oclock
ORTHO, 2oclock
PARA, 6oclock

100
Q

ONE OF THE PRIMARILY INFLUENCES
ON THE SOLUBILITY OF MOST DRUGS
THAT CONTAIN IONIZABLE GROUPS.

A

PH

101
Q

colloid properties:

A

TYNDALL EFFECT- ABILITY TO SCATTER LIGHT

BROWNIAN MOVEMENTZIGZAG MOVEMENT OF
COLLOIDAL PARTICLES

ELECTRICALLY CHARGEDELECTROPHORESIS

ADSORPTION- ABILITY TO ADHERE TO SURFACES

102
Q

ZEROTH

LAW OF THERMODYNAMICS

A

HEAT AND ITS RELATION TO ENERGY AND WORK

103
Q

FIRST LAW

A

ENERGY CAN BE TRANSFORMED

104
Q

SECOND LAW

A

HEAT CANNOT SPONTANEOUSLY FLOW FROM A COLDER LOCATION TO A

HOTTER LOCATION

105
Q

THIRD LAW

A

AS THE TEMPERATURE APPROACHES ABSOLUTE ZERO, THE ENTROPY OF

THE SYSTEM APPROACHES ITS MINIMUM

106
Q

EXPRESSIONS OF CONCENTRATIONS

A

MOLARITY = GRAMS OF SOLUTE/LITERS OF SOLUTION

MOLALITY = GRAMS OF SOLUTE/KG OF SOLVENT

MASS PERCENT = MASS OF SOLUTE/MASS OF SOLUTION X 100%

General Chemistry (3 decks)

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