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SEM 1 > Gen Chem/PIC > Flashcards

Gen Chem/PIC Flashcards

1
Q

It is study of matter and the changes it undergoes.

A

Chemistry

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2
Q

Matter that can be physically separated

A

Mixture

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3
Q

Matter that cannot be physically separated

A

Pure Substance

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4
Q

Uniform mixture

A

Homogenous

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5
Q

Pure substance that can be chemically decomposed

A

Compound

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6
Q

Pure substance that cannot be chemically decomposed

A

Element

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7
Q

Solid to Gas

A

Sublimation

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8
Q

Gas to Solid

A

Deposition

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9
Q

It is a form of matter that has a definite composition and distinct properties

A

Substance

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10
Q

It is a combination of two or more substances in which the substances retain their distinct identities.

A

Mixture

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11
Q

It does not have a constant composition

A

Mixture

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12
Q

It does not depend on how much matter is being considered.

Ex: density, freezing point, boiling point, conductivity, pressure, odor, color

A

Intrinsic/Intensive

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13
Q

It depends on how much matter is being considered.

Ex: mass, length, volume

A

Extrinsic/Extensive

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14
Q

It is observed or measured without changing the identity of matter

Ex. MP, BP, Solubility, Ƿ, malleability, ductility

A

Physical Property

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15
Q

It describe the change or the reaction a substance undergoes

Ex. Flammability, reactivity, inertness

A

Chemical Property

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16
Q

 It cannot be separated into simpler substances by chemical means
 Most are naturally occurring
 Symbols are used to represent

A

Element

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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

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18
Q

What are the metalloids in the periodic table

A

Silicon
Germanium
Polonium
Sb - Antimony
Arsenic
Telurium
Boron

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19
Q

aka Coarse Mixture; finely divided solid material distributed in a liquid where solid is insoluble

A

Suspension

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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.

A

Colloid

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21
Q

uniform mixture

A

Solution

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22
Q

Less than 1

A

Very Soluble

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23
Q

From 1 to 10

A

Freely Soluble

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24
Q

From 10 to 30

A

Solublr

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25
Q

From 30 to 100

A

Sparingly Soluble

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26
Q

From 100 to 1000

A

Slightly Soluble

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27
Q

From 1000 to 10,000

A

Very Slightly Soluble

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28
Q

10,000 and over

A

Practically Insoluble

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29
Q

Simplest method of separation

A

Decantation

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30
Q

Fe + S → FeS

A

Direct Union/Combination

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31
Q

H2O → H2 + O2

A

Decomposition/Analysis

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32
Q

Zn + CuSO4 → ZnSO4 + Cu

A

Single Displacement

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33
Q

NaCl + AgNO3 → NaNO3 + AgCl

A

Double Displacement/Metathesis

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34
Q

SA + SB

A

Neutral Salt

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35
Q

SA + WB

A

Acidic Salt

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36
Q

WA + SB

A

Basic Salt

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37
Q

Strong Acids

A

HCl
Hbr
HNO3
HI
HClO4
H2SO4

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38
Q

Coined the term “Atomos”

A

Democritus

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39
Q

“Billiard Ball Model”

A

John Dalton

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40
Q

“Raisin Bread Model” / electron

A

JJ Thomson

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41
Q

“Gold Foil Expt” / proton in the nucleus

A

Ernest Rutherford

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42
Q

Neutron

A

James Chadwick

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43
Q

“Planetary Model”

A

Niels Bohr

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44
Q

“Quantum Mechanic Model” / 3D model

A

Erwin Schrodinger

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45
Q

Basic unit of Matter

A

Atom

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46
Q

Greek word for atom; indivisible/uncuttable

A

Atomos

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47
Q

Found in the NUCLEUS…. collectively called NUCLEONS

A

Protons
Neutrons

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48
Q

Electron is 1,836 times lighter than a proton; thus, the weight is negligible.

A
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49
Q

It is the total number of neutrons and protons present in the nucleus of an atom

A

Mass Number

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50
Q

It is the number of protons in the nucleus of each atom

A

Atomic Number

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51
Q

It describes the MAIN ELECTRON SHELL and the SIZE of the e- cloud

A

Principal Quantum Number

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52
Q

It describes the SUBSHELL and the SHAPE of the e- cloud

A

Azimuthal/Angular Quantum Number

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53
Q

It describes the ORBITAL or ORIENTATION in space

A

Magnetic Quantum Number

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54
Q

No 2 e- can have the same set of quantum numbers

A

Pauli’s Exclusion Principle

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55
Q
  • “Building up” Principle
  • Electrons are placed first on the subshell with lowest energy level
A

Aufbau Principle

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56
Q

Electrons are spread singly before pairing up

A

Hund’s Rule

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57
Q

o groups of three similar elements
o forerunner of the idea of Groups

A

Johanne Dobereiner’s Triads (1829)

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58
Q

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

A

John Newlands Law of Octaves (1865)

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59
Q

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

A

Dmitri Mendeleev’s Table (1869)

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60
Q

3RD MOST ABUNDANT ELEMENT ON EARTH CRUST

A

Aluminum

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61
Q

2ND MOST ABUNDANT ELEMENT ON EARTH CRUST

A

Silicon

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62
Q

MOST ABUNDANT METAL

A

Aluminum

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63
Q

MOST ABUNDANT ELEMENT & ESSENTIAL OF ALL ON EARTH CRUST

A

Oxygen

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64
Q

MOST ABUNDANT ELEMENT IN THE UNIVERSE

A

Hydrogen

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65
Q

1ST ELEMENT PRODUCED ARTIFICIALLY

A

Technetium

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66
Q

ELEMENT COMMON TO ALL ACIDS

A

Hydrogen

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67
Q

ELEMENT PRESENT IN INSULIN

A

Zinc

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68
Q

DISCOVERED OXYGEN AND CALLED IT EMPYREAL AIR

A

Carl Wilhelm Scheele

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69
Q

DENSIEST ELEMENT IN THE PERIODIC TABLE

A

Osmium

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70
Q

ARTIFICIAL AIR

A

20% Oxygen
80 % Helium

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71
Q

HEAVY WATER

A

D2O deuterium

72
Q

SALT FORMING GROUP OF ELEMENTS

A

Halogens

73
Q

A MEASURE OF THE ACIDITY OF THE SOLUTION

A

pH

74
Q

ACID FOUND IN THE STOMACH

A

HCI

75
Q

COMPONENT OF HARD WATER

A

Magnesium
Calcium

76
Q

MOST ACTIVE OF METALLIC ELEMENTS

A

Group IA - Alkali Metals

77
Q

SOFTEST MINERAL KNOWN

A

Talc

78
Q

ABUNDANT ELEMENT THAT IS CHEMICALLY ACTIVE IN RESEARCH INVOLVING PHOTOSYNTHESIS

A

Magnesium

79
Q

LAUGHING GAS

A

N2O - Nitrous Oxide

80
Q

ELEMENT THAT APPEARS WIDELY DISTRIBUTED IN NATURE

A

Oxygen

81
Q

MOST METALLIC OF THE HALOGENS

A

Iodine

82
Q

MOST REACTIVE OF THE ELECTRONEGATIVE ELEMENT

A

Fluorine

83
Q

ELEMENT THAT OCCURS FREE IN THE ATMOSPHERE

A

78% Nitrogen

84
Q

IMPT. ELEMENT IN THE TRANSPORTATION OF OXYGEN BY HEMOGLOBIN.

A

Iron

85
Q

1⁄2 the distance between 2 nuclei
Right to left increases
Top to bottom increases

A

Atomic Radius

86
Q

Ability to attract electrons
Left to right increases
Going up increases

A

Electronegativity

87
Q

Ability to remove an electron from a
positively charged atom

Left to right increases
Going up increases

A

Ionization Energy or Potential

88
Q

Property to accept an electron
Right to left increases
Top to bottom increases

A

Electron Affinity

89
Q

• 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

A

Fluid Maintenance

90
Q

It is needed when there is a heavy loss of water and electrolve

A

Electrolyte Replacement

91
Q

Composition of Ringer’s Injection

A

8.6g NaCI
0.3g KCl
0.33g Ca Chloride per liter

92
Q

Composition of Lactated Ringer’s Injection

A

600 mg NaCI
30 mg KCI
20 mg Ca
310 mg Na lactate per 10 ml

93
Q
  • to supply water and electrolyte ni amount needed for maintenance
  • given to replace mild tomoderate fluid loss
A

Oral Electrolyte Solution

94
Q

It is not synthesized by the body and must be included in the diet

A

Essential Ions

95
Q

It is required for normal functioning but does not need to be included in the diet

A

Trace Ions

96
Q

Constituent of hemoglobin

A

Iron (Fe2+ or Fe3+)

97
Q

Clinical Manifestation of Iron Deficiency

A

Anemia

98
Q

Constituent of thyroxin and triiodothyronine

A

Iodine (I-)

99
Q

Clinical Manifestation of Iodine Deficiency

A

Endemic (simple) goiter
Cretinism

100
Q

Constituent of Vit. B12 (cyanocobalamin)

A

Cobalt (Co2+)

101
Q

Clinical Manifestation of Cobalt Deficiency

A

Deficiency of Vit. B12
Pernicious anemia
Polycythemia

102
Q

Constituent of insulin and carbonic anhydrase

A

Zinc (Zn2+)

103
Q

Clinical Manifestation of Zinc Deficiency

A

Anemia
Stunted growth
Hypogonadism

104
Q

Formation of hemoglobin (increases iron utilization)

Constituent of oxidase enzymes

A

Copper (Cu2+)

105
Q

Clinical Manifestations of Copper Deficiency

A

Hypochromic anemia
Wilson’s disease

106
Q

Constituent of proteins mucopolsaccharides, heparin, biotin, detoxication

A

Sulfur (S2-)

107
Q

Clinical Manifestations of Sulfur Deficiency

A

Cystinuria
Cystine renal calculi

108
Q

Compounds that involve a metal binding with either a non-metal or a semi-metal

A

Ionic Bonding

109
Q

Compounds that are composed of only non-metals or semi-metals with non-metals

A

Covalent Bonding; Molecular Compound

110
Q

 composed of positive and negative ions.
 usually formed from a metal and non- metal.
 these elements are not attached to one another.

A

Ionic Compounds

111
Q

tightly bound groups of atoms that
behave as a unit and carry a charge.

A

Polyatomic Ions

112
Q

for cations having more than one charge, the charge must be given in the name (in Roman numerals)

A

Stock System

113
Q

• composed of molecules in
which elements share electrons.
• usually composed of 2 nonmetals.
• these elements are attached

A

Molecular Compounds

114
Q

It shows the numbers and kinds of atoms present in a molecule of a compound.

A

Molecular Compound

115
Q

Positive Electrode

A

Anode

116
Q

Negative Electrode

A

Cathode

117
Q

Color of Sodium in Non Luminous Flame

A

Persistent Golden Yellow

118
Q

Color of Potassium in Non Luminous Flame

A

Violet

119
Q

Color of Lithium in Non Luminous Flame

A

Carmine Red

120
Q

Color of Calcium in Non Luminous Flame

A

Brick Red

121
Q

Color of Strontium in Non Luminous Flame

A

Crimson

122
Q

Color of Barium in Non Luminous Flame

A

Yellowish Green

123
Q

Color of Borate, Cu, Tl, P in Non Luminous Flame

A

Green

124
Q

Color of Pb, As, Sb, Bi, Cu in Non Luminous Flame

A

Blue

125
Q

Color of Ammonium in Non Luminous Flame

A

Colorless

126
Q

Color of Sodium Under cobalt glass

A

Nil

127
Q

Color of Potassium Under cobalt glass

A

Crimson

128
Q

Color of Lithium Under cobalt glass

A

Purple

129
Q

Color of Calcium Under cobalt glass

A

Light Green

130
Q

Color of Strontium Under cobalt glass

A

Purple

131
Q

Color of Barium Under cobalt glass

A

Bluish Green

132
Q

Color of Pb, As, Sb, Bi, Cu Under cobalt glass

A

Yellow

133
Q

gradual mixing of molecules of one gas with the molecules of another gas by virtue of their kinetic properties

A

Diffusion

134
Q

passage of a gas under pressure through a small opening

A

Effusion

135
Q

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.

A

Graham’s Law

136
Q

Volume is inversely proportional to pressure

A

Boyle’s Law

137
Q

Volume is directly proportional to temperature (Kelvin)

A

Charles’ Law

138
Q

Volume is directly proportional to moles

A

Avogadro’s Law

139
Q

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

A

Dalton’s Law of Partial Pressure

140
Q

composed of a weak acid & its salt

A

Conjugate Base

141
Q

weak base & its salt

A

Conjugate Acid

142
Q

pair or related chemical compounds capable of resisting large change in the pH of a solution

A

Buffers

143
Q

Acids in methyl orange

A

Pink/Red

144
Q

Bases in methyl orange

A

Yellow

145
Q

Based in Phenolphthalein

A

Pink to Violet

146
Q

Acids in Phenolphthalein

A

Colorless

147
Q

Vibration molecular motion

A

Solid

148
Q

Gliding molecular motion

A

Liquid

149
Q

Strongest IFA strength

A

Solid

150
Q

Characteristics of Metals

A
  • Good conductor of heat and electricity
  • Form Basic Oxides
  • Lustrous, Ductile, Malleable
  • High Density
  • High Melting Point
  • Tends to lose e-
151
Q

Characteristics of Non Metals

A
  • Poor conductors
  • Form Acidic Oxides
  • Dull and Brittle if solid
  • Low Density
  • Low Melting Point
  • Tends to accept e-
152
Q

It is an element which has properties in between those of metals and nonmetals

A

Metalloids

153
Q

Classification of Mixture according to nature of particles

A

Homogenous
Heterogenous

154
Q

Classification of mixture according to size of particles

A

Solution
Suspension
Colloid

155
Q

The solubility decreases with increase in temp (Mg citrate)

A

Exothermic

156
Q

The solubility increases with increases in temp

A

Endothermic

157
Q

Porous material is used to separate

A

Filtration

158
Q

The simplest process of separating mixture

A

Decantation

159
Q

Separating different liquids

A

Distillation

160
Q

Ex. Separating water and salt

A

Evaporation

161
Q

Ex. Separation of Salt and Iron

A

Magnetic Separation

162
Q

Process used to obtain a precipitate

A

Centrifugation

163
Q

Separation used between substances with different freezing points

A

Fractional Crystallization

164
Q

Change where no energy is produced

A

Physical change

165
Q

Change where energy is produced (generation of heat)

A

Chemical Change

166
Q

Oxidation Reduction

A

Lose Electrons - Oxidation
Gain Electrons - Reduction

167
Q

Reaction between acid and base will yield salt and water

A

Neutralization

168
Q

The loss of water

A

Hydrolysis

169
Q

Oil and base (NaOH) is used to form soap

A

Saponification

170
Q

Absorbs moisture, dissolves and liquefies

A

Deliquescent (NaOH)

171
Q

Absorbs moisture, expands in size and does not liquefy

A

Hygroscopic (CH3COOH)

172
Q

WA + WB

A

No reaction

173
Q

If the ratio of the elements are the same, you will get the same compound

A

Law of Definite Proportions

174
Q

If the ratio between elements is different, you will get a different compound

A

Law of Multiple Proportions

175
Q

It is the total number of neutrons and protons present in the nucleus of an atom

A

Mass Number

176
Q

It is the number of protons in the nucleus of each atom

A

Atomic Number

SEM 1 (8 decks)

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