Gen Chem/PIC Flashcards
(176 cards)
1
Q
It is study of matter and the changes it undergoes.
A
Chemistry
2
Q
Matter that can be physically separated
A
Mixture
3
Q
Matter that cannot be physically separated
A
Pure Substance
4
Q
Uniform mixture
A
Homogenous
5
Q
Pure substance that can be chemically decomposed
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Compound
6
Q
Pure substance that cannot be chemically decomposed
A
Element
7
Q
Solid to Gas
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Sublimation
8
Q
Gas to Solid
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Deposition
9
Q
It is a form of matter that has a definite composition and distinct properties
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Substance
10
Q
It is a combination of two or more substances in which the substances retain their distinct identities.
A
Mixture
11
Q
It does not have a constant composition
A
Mixture
12
Q
It does not depend on how much matter is being considered.
Ex: density, freezing point, boiling point, conductivity, pressure, odor, color
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Intrinsic/Intensive
13
Q
It depends on how much matter is being considered.
Ex: mass, length, volume
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Extrinsic/Extensive
14
Q
It is observed or measured without changing the identity of matter
Ex. MP, BP, Solubility, Ƿ, malleability, ductility
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Physical Property
15
Q
It describe the change or the reaction a substance undergoes
Ex. Flammability, reactivity, inertness
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Chemical Property
16
Q
It cannot be separated into simpler substances by chemical means
Most are naturally occurring
Symbols are used to represent
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Element
17
Q
Substance composed of atoms of two or more elements chemically united in fixed proportions.
Can be separated only by chemical means
A
Compound
18
Q
What are the metalloids in the periodic table
A
Silicon
Germanium
Polonium
Sb - Antimony
Arsenic
Telurium
Boron
19
Q
aka Coarse Mixture; finely divided solid material distributed in a liquid where solid is insoluble
A
Suspension
20
Q
particles of solute not broken down to the size of the molecules but are small enough to remain suspended and evenly dispersed throughout the medium.
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Colloid
21
Q
uniform mixture
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Solution
22
Q
Less than 1
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Very Soluble
23
Q
From 1 to 10
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Freely Soluble
24
Q
From 10 to 30
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Solublr
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From 30 to 100
Sparingly Soluble
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From 100 to 1000
Slightly Soluble
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From 1000 to 10,000
Very Slightly Soluble
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10,000 and over
Practically Insoluble
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Simplest method of separation
Decantation
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Fe + S → FeS
Direct Union/Combination
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H2O → H2 + O2
Decomposition/Analysis
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Zn + CuSO4 → ZnSO4 + Cu
Single Displacement
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NaCl + AgNO3 → NaNO3 + AgCl
Double Displacement/Metathesis
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SA + SB
Neutral Salt
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SA + WB
Acidic Salt
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WA + SB
Basic Salt
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Strong Acids
HCl
Hbr
HNO3
HI
HClO4
H2SO4
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Coined the term “Atomos”
Democritus
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“Billiard Ball Model”
John Dalton
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“Raisin Bread Model” / electron
JJ Thomson
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“Gold Foil Expt” / proton in the nucleus
Ernest Rutherford
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Neutron
James Chadwick
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“Planetary Model”
Niels Bohr
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“Quantum Mechanic Model” / 3D model
Erwin Schrodinger
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Basic unit of Matter
Atom
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Greek word for atom; indivisible/uncuttable
Atomos
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Found in the NUCLEUS.... collectively called NUCLEONS
Protons
Neutrons
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Electron is 1,836 times lighter than a proton; thus, the weight is negligible.
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It is the total number of neutrons and protons present in the nucleus of an atom
Mass Number
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It is the number of protons in the nucleus of each atom
Atomic Number
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It describes the MAIN ELECTRON SHELL and the SIZE of the e- cloud
Principal Quantum Number
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It describes the SUBSHELL and the SHAPE of the e- cloud
Azimuthal/Angular Quantum Number
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It describes the ORBITAL or ORIENTATION in space
Magnetic Quantum Number
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No 2 e- can have the same set of quantum numbers
Pauli’s Exclusion Principle
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- “Building up” Principle
- Electrons are placed first on the subshell with lowest energy level
Aufbau Principle
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Electrons are spread singly before pairing up
Hund’s Rule
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o groups of three similar elements
o forerunner of the idea of Groups
Johanne Dobereiner’s Triads (1829)
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o where around 60 known elements have been arranged in increasing RAM.
o Elements had similar properties to those 8 places before them and 8 places after them
o Forerunner of the idea of Periods and led to the name Periodic Table
John Newlands Law of Octaves (1865)
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o Arranged elements in order of increasing RAM
o Placed elements with similar properties underneath each other
o He left gaps where elements still to be discovered and predicted their properties
Dmitri Mendeleev’s Table (1869)
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3RD MOST ABUNDANT ELEMENT ON EARTH CRUST
Aluminum
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2ND MOST ABUNDANT ELEMENT ON EARTH CRUST
Silicon
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MOST ABUNDANT METAL
Aluminum
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MOST ABUNDANT ELEMENT & ESSENTIAL OF ALL ON EARTH CRUST
Oxygen
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MOST ABUNDANT ELEMENT IN THE UNIVERSE
Hydrogen
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1ST ELEMENT PRODUCED ARTIFICIALLY
Technetium
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ELEMENT COMMON TO ALL ACIDS
Hydrogen
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ELEMENT PRESENT IN INSULIN
Zinc
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DISCOVERED OXYGEN AND CALLED IT EMPYREAL AIR
Carl Wilhelm Scheele
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DENSIEST ELEMENT IN THE PERIODIC TABLE
Osmium
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ARTIFICIAL AIR
20% Oxygen
80 % Helium
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HEAVY WATER
D2O deuterium
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SALT FORMING GROUP OF ELEMENTS
Halogens
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A MEASURE OF THE ACIDITY OF THE SOLUTION
pH
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ACID FOUND IN THE STOMACH
HCI
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COMPONENT OF HARD WATER
Magnesium
Calcium
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MOST ACTIVE OF METALLIC ELEMENTS
Group IA - Alkali Metals
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SOFTEST MINERAL KNOWN
Talc
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ABUNDANT ELEMENT THAT IS CHEMICALLY ACTIVE IN RESEARCH INVOLVING PHOTOSYNTHESIS
Magnesium
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LAUGHING GAS
N2O - Nitrous Oxide
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ELEMENT THAT APPEARS WIDELY DISTRIBUTED IN NATURE
Oxygen
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MOST METALLIC OF THE HALOGENS
Iodine
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MOST REACTIVE OF THE ELECTRONEGATIVE ELEMENT
Fluorine
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ELEMENT THAT OCCURS FREE IN THE ATMOSPHERE
78% Nitrogen
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IMPT. ELEMENT IN THE TRANSPORTATION OF OXYGEN BY HEMOGLOBIN.
Iron
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1⁄2 the distance between 2 nuclei
Right to left increases
Top to bottom increases
Atomic Radius
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Ability to attract electrons
Left to right increases
Going up increases
Electronegativity
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Ability to remove an electron from a
positively charged atom
Left to right increases
Going up increases
Ionization Energy or Potential
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Property to accept an electron
Right to left increases
Top to bottom increases
Electron Affinity
89
• to supply normal regrement for water and electrolytes to those who cannot take them orally
• should contain at least 5% dextrose to minimize the build-up of metabolites associated with starvation
(urea, phosphate and ketone bodies)
• general electrolyte composition: Na, C,I HCO3, Mg &Pions
Fluid Maintenance
90
It is needed when there is a heavy loss of water and electrolve
Electrolyte Replacement
91
Composition of Ringer’s Injection
8.6g NaCI
0.3g KCl
0.33g Ca Chloride per liter
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Composition of Lactated Ringer’s Injection
600 mg NaCI
30 mg KCI
20 mg Ca
310 mg Na lactate per 10 ml
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- to supply water and electrolyte ni amount needed for maintenance
- given to replace mild tomoderate fluid loss
Oral Electrolyte Solution
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It is not synthesized by the body and must be included in the diet
Essential Ions
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It is required for normal functioning but does not need to be included in the diet
Trace Ions
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Constituent of hemoglobin
Iron (Fe2+ or Fe3+)
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Clinical Manifestation of Iron Deficiency
Anemia
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Constituent of thyroxin and triiodothyronine
Iodine (I-)
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Clinical Manifestation of Iodine Deficiency
Endemic (simple) goiter
Cretinism
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Constituent of Vit. B12 (cyanocobalamin)
Cobalt (Co2+)
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Clinical Manifestation of Cobalt Deficiency
Deficiency of Vit. B12
Pernicious anemia
Polycythemia
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Constituent of insulin and carbonic anhydrase
Zinc (Zn2+)
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Clinical Manifestation of Zinc Deficiency
Anemia
Stunted growth
Hypogonadism
104
Formation of hemoglobin (increases iron utilization)
Constituent of oxidase enzymes
Copper (Cu2+)
105
Clinical Manifestations of Copper Deficiency
Hypochromic anemia
Wilson's disease
106
Constituent of proteins mucopolsaccharides, heparin, biotin, detoxication
Sulfur (S2-)
107
Clinical Manifestations of Sulfur Deficiency
Cystinuria
Cystine renal calculi
108
Compounds that involve a metal binding with either a non-metal or a semi-metal
Ionic Bonding
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Compounds that are composed of only non-metals or semi-metals with non-metals
Covalent Bonding; Molecular Compound
110
composed of positive and negative ions.
usually formed from a metal and non- metal.
these elements are not attached to one another.
Ionic Compounds
111
tightly bound groups of atoms that
behave as a unit and carry a charge.
Polyatomic Ions
112
for cations having more than one charge, the charge must be given in the name (in Roman numerals)
Stock System
113
• composed of molecules in
which elements share electrons.
• usually composed of 2 nonmetals.
• these elements are attached
Molecular Compounds
114
It shows the numbers and kinds of atoms present in a molecule of a compound.
Molecular Compound
115
Positive Electrode
Anode
116
Negative Electrode
Cathode
117
Color of Sodium in Non Luminous Flame
Persistent Golden Yellow
118
Color of Potassium in Non Luminous Flame
Violet
119
Color of Lithium in Non Luminous Flame
Carmine Red
120
Color of Calcium in Non Luminous Flame
Brick Red
121
Color of Strontium in Non Luminous Flame
Crimson
122
Color of Barium in Non Luminous Flame
Yellowish Green
123
Color of Borate, Cu, Tl, P in Non Luminous Flame
Green
124
Color of Pb, As, Sb, Bi, Cu in Non Luminous Flame
Blue
125
Color of Ammonium in Non Luminous Flame
Colorless
126
Color of Sodium Under cobalt glass
Nil
127
Color of Potassium Under cobalt glass
Crimson
128
Color of Lithium Under cobalt glass
Purple
129
Color of Calcium Under cobalt glass
Light Green
130
Color of Strontium Under cobalt glass
Purple
131
Color of Barium Under cobalt glass
Bluish Green
132
Color of Pb, As, Sb, Bi, Cu Under cobalt glass
Yellow
133
gradual mixing of molecules of one gas with the molecules of another gas by virtue of their kinetic properties
Diffusion
134
passage of a gas under pressure through a small opening
Effusion
135
The rate of the effusion of two gases (and diffusion) are inversely proportional to the square roots of their densities providing the temperature and pressure are the same for the two gases.
Graham’s Law
136
Volume is inversely proportional to pressure
Boyle’s Law
137
Volume is directly proportional to temperature (Kelvin)
Charles’ Law
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Volume is directly proportional to moles
Avogadro’s Law
139
States that the pressure exerted by a mixture of gases is the sum of the partial pressures that each gas in the mixture exert individually
Dalton’s Law of Partial Pressure
140
composed of a weak acid & its salt
Conjugate Base
141
weak base & its salt
Conjugate Acid
142
pair or related chemical compounds capable of resisting large change in the pH of a solution
Buffers
143
Acids in methyl orange
Pink/Red
144
Bases in methyl orange
Yellow
145
Based in Phenolphthalein
Pink to Violet
146
Acids in Phenolphthalein
Colorless
147
Vibration molecular motion
Solid
148
Gliding molecular motion
Liquid
149
Strongest IFA strength
Solid
150
Characteristics of Metals
- Good conductor of heat and electricity
- Form Basic Oxides
- Lustrous, Ductile, Malleable
- High Density
- High Melting Point
- Tends to lose e-
151
Characteristics of Non Metals
- Poor conductors
- Form Acidic Oxides
- Dull and Brittle if solid
- Low Density
- Low Melting Point
- Tends to accept e-
152
It is an element which has properties in between those of metals and nonmetals
Metalloids
153
Classification of Mixture according to nature of particles
Homogenous
Heterogenous
154
Classification of mixture according to size of particles
Solution
Suspension
Colloid
155
The solubility decreases with increase in temp (Mg citrate)
Exothermic
156
The solubility increases with increases in temp
Endothermic
157
Porous material is used to separate
Filtration
158
The simplest process of separating mixture
Decantation
159
Separating different liquids
Distillation
160
Ex. Separating water and salt
Evaporation
161
Ex. Separation of Salt and Iron
Magnetic Separation
162
Process used to obtain a precipitate
Centrifugation
163
Separation used between substances with different freezing points
Fractional Crystallization
164
Change where no energy is produced
Physical change
165
Change where energy is produced (generation of heat)
Chemical Change
166
Oxidation Reduction
Lose Electrons - Oxidation
Gain Electrons - Reduction
167
Reaction between acid and base will yield salt and water
Neutralization
168
The loss of water
Hydrolysis
169
Oil and base (NaOH) is used to form soap
Saponification
170
Absorbs moisture, dissolves and liquefies
Deliquescent (NaOH)
171
Absorbs moisture, expands in size and does not liquefy
Hygroscopic (CH3COOH)
172
WA + WB
No reaction
173
If the ratio of the elements are the same, you will get the same compound
Law of Definite Proportions
174
If the ratio between elements is different, you will get a different compound
Law of Multiple Proportions
175
It is the total number of neutrons and protons present in the nucleus of an atom
Mass Number
176
It is the number of protons in the nucleus of each atom
Atomic Number
