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GEAS > CHEMISTRY > Flashcards

CHEMISTRY Flashcards

1
Q

Hot ionized gas

A

PLASMA

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2
Q

Combination of two or more elements chemically combined in fixed proportions. It can be separated by chemical means into its respective components

A

COMPOUND

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3
Q

Depends on the amount or on the substance or matter being studied

A

EXTENSIVE PROPERTY

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4
Q

Is one with two or more distinct phases

A

HETEROGENEOUS

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5
Q

Matter that has definite composition and properties. It cannot be separated into two or more substances by physical means

A

PURE SUBSTANCE

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6
Q

Mixtures that settle at the bottom upon standing

A

SUSPENSION

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7
Q

Mixtures which particles do not settle at the bottom upon standing

A

COLLOIDS

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8
Q

Properties that are independent on the amount of substance or matter being studied

A

INTENSIVE

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9
Q

Pure substance that cannot be broken down into simpler substance by chemical means

A

ELEMENT

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10
Q

State of matter of a dilute gas college to temperature very close to absolute 0 Kelvin

A

BOSE EINSTEIN CONDENSATES

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11
Q

Type of mixture that is uniform all through out

A

HOMOGENEOUS

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12
Q

CLASSIFICATIONS OF MATTER

A

MATTER

PURE SUBSTANCE MIXTURES

ELEMENT HOMOGENEOUS
COMPOUND HETEROGENOUS

                                         SUSPENSION,                 COLLIODS COURSE MIXTURES
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13
Q
  • The process of separating large solid particles from liquids by allowing the liquid to flow while the large solid particles to settle.
  • separating mixtures by differences of density
A

DECANTATION / FLOATATION

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14
Q

Process of separating small solid particles from liquid by passing the mixture through a porous medium

A

FILTRATION

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15
Q

Process of separating the liquid by BOILING the mixture to vaporize the liquid then cooling the vapor to condense it.

A

DISTILLATION

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16
Q

Process of separating liquid mixtures whose component substances have narrow differences in boiling point.

A

FRACTIONAL DISTILLATION

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17
Q

the process of separating volatile oils from plants

A

STEAM DISTILLATION

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18
Q

Process involving the use of tools such as forceps, sieves etc

A

MECHANICAL SEPARATION

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19
Q

Process that speeds up the settling of the precipitates using a centrifuge which is a motor driven apparatus

A

CENTRIFUGATION

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20
Q
  • The process of using difference in degree to which the substances are absorbed on the surface of an inert substance
  • separation by inner molecular attractions
A

CHROMATOGRAPHY

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21
Q

Process of separating the mixtures to its component substances by making use of the difference in solubility of the substances

A

SOLVENT EXTRACTION

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22
Q

Process of extracting gold from its ore

A

AMALGATION

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23
Q

The process of extracting gold from its ore by using cyanide

A

CYANIDATION

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24
Q

Revised metric system of units proposed by the General Conference of Weights and Measures in 1960

A

SI ( SYSTEM INTERNATIONALE d’ UNITES or INTERNATIONAL SYSTEM OF UNITS)

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25
Q

Difference between the accepted value and the measured value

A

ERROR

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26
Q

Liquid to gas

A

EVAPORATION

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27
Q

Solid to gas

A

SUBLIMATION

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28
Q

Gas to solid. Water vapor changes directly into ice during winter

A

DESPOSITION

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29
Q

A mixture which one substance of microscopically dispersed insoluble particle is suspended throughout another substance

A

COLLIODS

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30
Q

Solid dispersed in gas (SMOKE OR EXHAUST)

A

SOLID AEROSOL

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31
Q

Liquid dispersed in gas (FOG)

A

LIQUID AEROSOL

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32
Q

Gas dispersed in solid (MARSHMALLOW)

A

SOLID FOAM

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33
Q

Gas dispersed in liquid (SHAVING CREAM)

A

LIQUID FOAM

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34
Q

Liquid dispersed in liquid (MILK)

A

LIQUID EMULSION

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35
Q

Liquid dispersed in solid (PEANUT BUTTER)

A

Solid Emmulsion

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36
Q

Solid dispersed in liquid

A

LIQUID SOL

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37
Q

Solid dispersed in solid

A

SOLID SOL

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38
Q

Solid expanding through out liquid

A

GEL

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39
Q

Ability of colloidal substance to scatter light

A

TYNDALL EFFECT

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40
Q

Random motion due to bombardment of atoms

A

BROWNIAN MOVEMENT

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41
Q

Motion dispersed particles under influence of electric field

A

ELECTROPHORESIS

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42
Q

Cannot pass through semi - permeable membrane

A

OSMOTIC PRESSURE

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43
Q

Separating mixtures by densities of liquid

A

EXTRACTIONS

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44
Q

Separating mixtures by differences in solubility at temperatures

A

CRYSTALLIZATION

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45
Q

Separating mixtures in differences in appearance and size

A

MECHANICAL SEPARATION

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46
Q

“Mass is neither created nor destroyed”

A

LAW OF CONSERVATION OF MASS

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47
Q

A given compound always contains exactly the same proportion of elements by mass

A

LAW DEFINITE PROPORTION

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48
Q

When two elements form a series of compounds, the ratios of the masses of the second element ….. SMALL WHOLE NUMBERS

A

LAW OF MULTIPLE PROPORTIONS

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49
Q

Smallest particle of an element and contains all the characteristics of an element

A

ATOMS

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50
Q

Discovered electrons

A

Joseph John Thomson

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51
Q

Discovered neutron

A

James Chadwick

52
Q

Discovered proton

A

ERNEST RUTHERFORD

53
Q

The number of protons contained in the nucleus of each of its atom

A

ATOMIC NUMBER

54
Q

Sum of protons and neutrons in the nucleus of the atom

A

MASS NUMBER OR ATOMIC WEIGHT

55
Q

Outermost she’ll

A

VALENCE SHELL

56
Q

Electrons residing in the outermost she’ll

A

VALENCE ELECTRONS

57
Q

Determines the energy state of an electron. It can have integer values of 1,2,3 up to 7

A

PRINCIPAL (n)

58
Q

Angular or subshell number defines the orbital shape. It’s values are s = 0 , p = 1 , d= 2 and f = 3

A

AZIMUTHAL (l)

59
Q

Orbital number which specifies the spatial orientation of an orbital. It has an integer values of 0 for s, -1 to +1 for p, -2 to +2 for d and -3 to +3 for f

A

MAGNETIC (m)

60
Q

Can have values of +1/2 for unpaired or -1/2 for paired orbital and does not depend upon values of n, l, or m.

A

SPIN (s)

61
Q

No two electrons can have identical quantum numbers

A

PAULI’S EXCLUSION PRINCIPLE

62
Q

German word meaning “building up”

Atoms fill the lowest available energy levels before filling higher levels.

A

AFBAU PRINCIPLE

63
Q

Every orbital in a subshell is singly occupied with one electron before any orbital doubly occupied and all electrons in singly occupied orbitals have the same spin

A

HUND’S RULE

64
Q

Equal number of protons

A

ISOTOPES

65
Q

Equal number of neutrons

A

ISOTONES

66
Q

Equal mass number

A

ISOBARS

67
Q

Same molecular formulas but differ in structures and properties

A

ISOMERS

68
Q

Same number of electrons

A

ISOELECTRONIC SPECIES

69
Q

PERIODIC TABLE TRENDS

A

Electron negativity, electron affinity and ionization energy (TOP TO BOTTOM DECREASING, LEFT TO RIGHT INCREASING)

VICE VERSA OF Atomic Number and Metallic characteristics

70
Q

Amount of energy required to remove a valence electron

A

IONIZATION ENERGY

71
Q

Measure of the tendency to ATTRACT a bonding pair of electrons

A

ELECTRONEGATIVITY

72
Q

Measure of energy change when an electron is ADDED to a neutral atom to form a negative ion

A

ELECTRON AFFINITY

73
Q

Tendency to lose electrons and form cation

A

METALLIC CHARACTERISTIC

74
Q

Tendency to gain electron and form anion

A

NON METALLIC CHARACTERISTIC

75
Q

Metals are solids at room temperature with the exception of mercury which is liquid at room temperature

A

STATE

76
Q

Metals have the quality of reflecting light from its surface and can be polished

A

LUSTER

77
Q

Metals have the ability to withstand hammering and can be made into thin sheets known as foils

A

MALLEABILITY

78
Q

Metals can be drawn into wires

A

DUCTILITY

79
Q

All metals are hard except sodium and potassium

A

HARDNESS

80
Q

Good conductors

A

METALS

81
Q

Two best conductors

A

SILVER AND COPPER

82
Q

Poorest conductor of heat

A

LEAD

83
Q

Has the highest melting and boiling point

A

TUNGSTEN

84
Q

Derived from experiment, simplest whole number ratio

A

EMPIRICAL FORMULA

85
Q

Exact number of atoms

A

MOLECULAR FORMULA

86
Q

Electrons unequally shares by atoms

A

POLAR COVALENT / UNSYMMETRICAL

87
Q

Electron pairs are equally shared by atoms

A

NON POLAR COVALENT BOND / SYMMETRICAL

88
Q

Transfer of electrons from metallic to non metallic to form ions

A

IONIC BOND

89
Q

Force of attraction between valence electrons and metal ions

A

METALLIC BOND

90
Q

Involves the combination of two or more reactants to form one product.

A

DIRECT COMBINATION OR SYNTHESIS

91
Q

Involves breakdown of a single reactant into two or more products and ENDOTHERMIC by nature

A

ANALYSIS OR DECOMPOSITION

92
Q

Absorbs heat

A

ENDOTHERMIC

93
Q

Releases heat

A

EXOTHERMIC

94
Q

Uncombined element replaces another element that is part of a compound

A

SINGLE REPLACEMENT OR SUBSTITUTION

95
Q

Two elements in different compounds replace each other

A

DOUBLE REPLACEMENT / METHATHESIS

96
Q

Reaction that gives off heat energy with oxygen as one of reactants often EXOTHERMIC by nature

A

COMBUSTION

97
Q

Single bond between carbon atoms

A

ALKANES

98
Q

Contain double bonds between carbon atoms

A

ALKENES

99
Q

Contain triple bonds between carbon atoms

A

ALKYNES

100
Q

Dissolving element

A

SOLVENT

101
Q

Being dissolved

A

SOLUTE

102
Q

Solution with less solute concentration

A

HYPOTONIC

103
Q

Solution with greater solute concentration

A

HYPERTONIC

104
Q

Same concentration of SOLUTE

A

ISOMIC

105
Q

Number of miles solute divided by the number of moles of solvent and all solute a

A

MOLE FRACTION

106
Q

Defined as the number of moles of solute dissolved in 1 kg of solvent

A

MOLALITY

107
Q

Less solute dissolved by solvent

A

UNSATURATED

108
Q

More solute that the maximum can be dissolved

A

SUPER SATURATED

109
Q

Max amount of solute dissolved

A

SATURATED

110
Q

Defined as the number of moles of solute dissolved in 1 liter of solution

A

MOLARITY

111
Q

The process of adding solvent (usually water) to a concentrated solution to achieve a solution of the desired concentration

A

DILUTION

112
Q

“The partial pressure of a solvent over a solution is given by the vapor pressure of the pure solvent times the mole fraction of the solvent in the solution”

A

RAOULT’S LAW

113
Q

the boiling point of a pure solvent is increased by the addition of a non volatile solute

A

EBULLIOSCOPY (Boiling Point Elevation)

114
Q

The freezing point of a pure solvent is lowered by the addition of a h is insoluble in the solvent

A

CRYOSCOPY

115
Q

Compounds that dissociates in water into H+ ions

A

ACID

116
Q

Compound that dissociates with OH- ions

A

BASE

117
Q

Father of Plogiston

A

George Stahl

118
Q

The rate at which gas passes through a small hole into a vacuum

A

EFFUSION

119
Q

The spread of one substance through another

A

DIFFUSION

120
Q

Radio activity was discovered by

A

HENRY BECQUEREL

121
Q

These are elements from Group 1A to Group 7A and are found in the leftmost and rightmost part of the table.

A

REPRESENTATIVE ELEMENTS

122
Q

Avogadro’s number was named after

A

LORENZO AMADEO AVOGADRO

123
Q

Relationship between the amount of reactants that must be used and the mount of product desired in every chemical reaction

A

STOICHIOMETRY

124
Q

Atmospheric pressure first noticed by

A

EVANGELISTA TORECELLI

125
Q

Constant temperature

A

BOYLE’S LAW

126
Q

Constant pressure

A

CHARLE’S LAW (Jacques Alexandre CHARLE’S)

GEAS (5 decks)

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