Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

GEAS > CHEMISTRY > Flashcards

CHEMISTRY Flashcards

1
Q

Hot ionized gas

A

PLASMA

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

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

A

EXTENSIVE PROPERTY

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Is one with two or more distinct phases

A

HETEROGENEOUS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

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

A

PURE SUBSTANCE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Mixtures that settle at the bottom upon standing

A

SUSPENSION

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Mixtures which particles do not settle at the bottom upon standing

A

COLLOIDS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

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

A

INTENSIVE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

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

A

ELEMENT

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

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

A

BOSE EINSTEIN CONDENSATES

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Type of mixture that is uniform all through out

A

HOMOGENEOUS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

CLASSIFICATIONS OF MATTER

A

MATTER

PURE SUBSTANCE MIXTURES

ELEMENT HOMOGENEOUS
COMPOUND HETEROGENOUS

                                         SUSPENSION,                 COLLIODS COURSE MIXTURES
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

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

A

FILTRATION

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

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

A

DISTILLATION

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

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

A

FRACTIONAL DISTILLATION

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

the process of separating volatile oils from plants

A

STEAM DISTILLATION

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

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

A

MECHANICAL SEPARATION

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

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

A

CENTRIFUGATION

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Process of extracting gold from its ore

A

AMALGATION

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

The process of extracting gold from its ore by using cyanide

A

CYANIDATION

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Difference between the accepted value and the measured value
ERROR
26
Liquid to gas
EVAPORATION
27
Solid to gas
SUBLIMATION
28
Gas to solid. Water vapor changes directly into ice during winter
DESPOSITION
29
A mixture which one substance of microscopically dispersed insoluble particle is suspended throughout another substance
COLLIODS
30
Solid dispersed in gas (SMOKE OR EXHAUST)
SOLID AEROSOL
31
Liquid dispersed in gas (FOG)
LIQUID AEROSOL
32
Gas dispersed in solid (MARSHMALLOW)
SOLID FOAM
33
Gas dispersed in liquid (SHAVING CREAM)
LIQUID FOAM
34
Liquid dispersed in liquid (MILK)
LIQUID EMULSION
35
Liquid dispersed in solid (PEANUT BUTTER)
Solid Emmulsion
36
Solid dispersed in liquid
LIQUID SOL
37
Solid dispersed in solid
SOLID SOL
38
Solid expanding through out liquid
GEL
39
Ability of colloidal substance to scatter light
TYNDALL EFFECT
40
Random motion due to bombardment of atoms
BROWNIAN MOVEMENT
41
Motion dispersed particles under influence of electric field
ELECTROPHORESIS
42
Cannot pass through semi - permeable membrane
OSMOTIC PRESSURE
43
Separating mixtures by densities of liquid
EXTRACTIONS
44
Separating mixtures by differences in solubility at temperatures
CRYSTALLIZATION
45
Separating mixtures in differences in appearance and size
MECHANICAL SEPARATION
46
"Mass is neither created nor destroyed"
LAW OF CONSERVATION OF MASS
47
A given compound always contains exactly the same proportion of elements by mass
LAW DEFINITE PROPORTION
48
When two elements form a series of compounds, the ratios of the masses of the second element ..... SMALL WHOLE NUMBERS
LAW OF MULTIPLE PROPORTIONS
49
Smallest particle of an element and contains all the characteristics of an element
ATOMS
50
Discovered electrons
Joseph John Thomson
51
Discovered neutron
James Chadwick
52
Discovered proton
ERNEST RUTHERFORD
53
The number of protons contained in the nucleus of each of its atom
ATOMIC NUMBER
54
Sum of protons and neutrons in the nucleus of the atom
MASS NUMBER OR ATOMIC WEIGHT
55
Outermost she'll
VALENCE SHELL
56
Electrons residing in the outermost she'll
VALENCE ELECTRONS
57
Determines the energy state of an electron. It can have integer values of 1,2,3 up to 7
PRINCIPAL (n)
58
Angular or subshell number defines the orbital shape. It's values are s = 0 , p = 1 , d= 2 and f = 3
AZIMUTHAL (l)
59
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
MAGNETIC (m)
60
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.
SPIN (s)
61
No two electrons can have identical quantum numbers
PAULI'S EXCLUSION PRINCIPLE
62
German word meaning "building up" Atoms fill the lowest available energy levels before filling higher levels.
AFBAU PRINCIPLE
63
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
HUND'S RULE
64
Equal number of protons
ISOTOPES
65
Equal number of neutrons
ISOTONES
66
Equal mass number
ISOBARS
67
Same molecular formulas but differ in structures and properties
ISOMERS
68
Same number of electrons
ISOELECTRONIC SPECIES
69
PERIODIC TABLE TRENDS
Electron negativity, electron affinity and ionization energy (TOP TO BOTTOM DECREASING, LEFT TO RIGHT INCREASING) VICE VERSA OF Atomic Number and Metallic characteristics
70
Amount of energy required to remove a valence electron
IONIZATION ENERGY
71
Measure of the tendency to ATTRACT a bonding pair of electrons
ELECTRONEGATIVITY
72
Measure of energy change when an electron is ADDED to a neutral atom to form a negative ion
ELECTRON AFFINITY
73
Tendency to lose electrons and form cation
METALLIC CHARACTERISTIC
74
Tendency to gain electron and form anion
NON METALLIC CHARACTERISTIC
75
Metals are solids at room temperature with the exception of mercury which is liquid at room temperature
STATE
76
Metals have the quality of reflecting light from its surface and can be polished
LUSTER
77
Metals have the ability to withstand hammering and can be made into thin sheets known as foils
MALLEABILITY
78
Metals can be drawn into wires
DUCTILITY
79
All metals are hard except sodium and potassium
HARDNESS
80
Good conductors
METALS
81
Two best conductors
SILVER AND COPPER
82
Poorest conductor of heat
LEAD
83
Has the highest melting and boiling point
TUNGSTEN
84
Derived from experiment, simplest whole number ratio
EMPIRICAL FORMULA
85
Exact number of atoms
MOLECULAR FORMULA
86
Electrons unequally shares by atoms
POLAR COVALENT / UNSYMMETRICAL
87
Electron pairs are equally shared by atoms
NON POLAR COVALENT BOND / SYMMETRICAL
88
Transfer of electrons from metallic to non metallic to form ions
IONIC BOND
89
Force of attraction between valence electrons and metal ions
METALLIC BOND
90
Involves the combination of two or more reactants to form one product.
DIRECT COMBINATION OR SYNTHESIS
91
Involves breakdown of a single reactant into two or more products and ENDOTHERMIC by nature
ANALYSIS OR DECOMPOSITION
92
Absorbs heat
ENDOTHERMIC
93
Releases heat
EXOTHERMIC
94
Uncombined element replaces another element that is part of a compound
SINGLE REPLACEMENT OR SUBSTITUTION
95
Two elements in different compounds replace each other
DOUBLE REPLACEMENT / METHATHESIS
96
Reaction that gives off heat energy with oxygen as one of reactants often EXOTHERMIC by nature
COMBUSTION
97
Single bond between carbon atoms
ALKANES
98
Contain double bonds between carbon atoms
ALKENES
99
Contain triple bonds between carbon atoms
ALKYNES
100
Dissolving element
SOLVENT
101
Being dissolved
SOLUTE
102
Solution with less solute concentration
HYPOTONIC
103
Solution with greater solute concentration
HYPERTONIC
104
Same concentration of SOLUTE
ISOMIC
105
Number of miles solute divided by the number of moles of solvent and all solute a
MOLE FRACTION
106
Defined as the number of moles of solute dissolved in 1 kg of solvent
MOLALITY
107
Less solute dissolved by solvent
UNSATURATED
108
More solute that the maximum can be dissolved
SUPER SATURATED
109
Max amount of solute dissolved
SATURATED
110
Defined as the number of moles of solute dissolved in 1 liter of solution
MOLARITY
111
The process of adding solvent (usually water) to a concentrated solution to achieve a solution of the desired concentration
DILUTION
112
"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"
RAOULT'S LAW
113
the boiling point of a pure solvent is increased by the addition of a non volatile solute
EBULLIOSCOPY (Boiling Point Elevation)
114
The freezing point of a pure solvent is lowered by the addition of a h is insoluble in the solvent
CRYOSCOPY
115
Compounds that dissociates in water into H+ ions
ACID
116
Compound that dissociates with OH- ions
BASE
117
Father of Plogiston
George Stahl
118
The rate at which gas passes through a small hole into a vacuum
EFFUSION
119
The spread of one substance through another
DIFFUSION
120
Radio activity was discovered by
HENRY BECQUEREL
121
These are elements from Group 1A to Group 7A and are found in the leftmost and rightmost part of the table.
REPRESENTATIVE ELEMENTS
122
Avogadro's number was named after
LORENZO AMADEO AVOGADRO
123
Relationship between the amount of reactants that must be used and the mount of product desired in every chemical reaction
STOICHIOMETRY
124
Atmospheric pressure first noticed by
EVANGELISTA TORECELLI
125
Constant temperature
BOYLE'S LAW
126
Constant pressure
CHARLE'S LAW (Jacques Alexandre CHARLE'S)

GEAS (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions