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_____ Flashcards

1
Q

This is the smallest energy that can be emitted (or absorbed) in the form of electromagnetic waves

A

QUANTUM

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2
Q

A phenomena where electrons from the surface of certain metals exposed to light of at least a certain minimum frequency

A

PHOTOELECTRIC EFFECT.

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3
Q

An electron bound to the nucleus behaves like a

A

STANDING WAVE.

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4
Q

First known laser

A

RUBY LASER

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5
Q

It states that it is impossible to form an image of an object that is smaller than half the wavelength of the light used for observation

A

LAW OF OPTICS

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6
Q

A quantum number that relates the average distance of the electrons from the nucleus in a particular orbital.The larger this, the greater the average distance of an electron in the orbital from the nucleus and therefore the larger the orbital.

A

(PRINCIPAL QUANTUM NUMBER (N))

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7
Q

Group of elements which have incompletely filled d subshells

A

TRANSITION METALS

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8
Q

Series of elements that are not usually found in nature but is always synthesized

A

Actinide series

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9
Q

Group of elements that have incompletely filled 4f subshells

A

LANTHANIDES OR RARE EARTH

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10
Q

This is defined as a reduction in the effectivenuclear chargeon theelectroncloud, due to a difference in the attraction forces of theelectronson the nucleus.

A

SHIELDING EFFECT

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11
Q

Atoms of elements with low ionization energies tend to form

A

CATIONS

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12
Q

Atoms with high electron affinities tend to form

A

ANIONS

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13
Q

The elements that are most likely to form cations in ionic compounds are

A

ALKALI METALS AND ALKALI EARTH METALS

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14
Q

These are elements that are likely to form anions

A

HALOGENS AND OXYGEN

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15
Q

A poisonous white powder used in lowering the melting point of solders in manufacturing ceramics.

A

LITHIUM FLUORIDE

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16
Q

This is the energy required to completely separate one mole of a solid ionic compound into gaseous ions-

A

LATTICE ENERGY

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17
Q

This cycle relates lattice energies of ionic compounds to ionization energies, electron affinities, and other atomic and molecular properties

A

BORN HABER CYCLE

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18
Q

To form an ionic bond the electronegativity difference between two bonding atoms should be-

A

2.0 or more.

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19
Q

Violators of Octet Rule:

A

• Atoms of the second period elements cannot have more than eight valence electrons around the central atom.

-• Atoms of elements in and beyond the third period of the periodic table form some compound in which more than eight electrons surround the central atom.

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20
Q

Mathematicalequationthat describes the changes over time of a physical system in which quantum effects, such as wave–particle duality, are significant.

A

Schrodinger Equation

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21
Q

Which rule is followed by Hydrogen

a. duet rule b. octet rule c. triad rule

A

a. duet rule

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22
Q

Who proposed the hexagonal structure of benzene?

A

August Kekule

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23
Q

Resonance structures with formal charges greater than____ are usually considered highly implausible and can be discarded.

A

+2 or -2

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24
Q

Which period of elements in the table cannot have an expanded octet?

A

Second-period

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25
Q

The most reactive metals are in ____ and the most reactive nonmentals in ___.

A

Group 1A, Group 7A

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26
Q

What element melts in a person’s body?

A

Gallium

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27
Q

Mendeleev proposed the existence of an unknown element he called ____ which has properties close to Gallium.

A

eka-aluminum

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28
Q

His work on periodic classification of elements is regarded by many as the most significant achievement I chemistry in nineteenth century.

A

Dmitri Mendeleev

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29
Q

He discovered the chemical affinity of hemoglobin for oxygen.

A

Julius Lothar Meyer

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30
Q

The non-valence electrons are called

A

core electrons

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31
Q

The representative elements are the elements in _____, all of which have incompletely filled s or p subshells of the highest principal quantum number.

A

Groups 1A through 7A

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32
Q

The transition metals are the elements in ____, which have incompletely filled d subshells.

A

Group 1B, 3B through 8B

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33
Q

The ____ is the nuclear charge felt by an electron when both the actual nuclear charge and the repulsive effects of other electrons are taken into account.

A

effective nuclear charge

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34
Q

The increase in effective nuclear charge from_____ a period and from ____ in a group for representative elements.

A

left to right across a period and from top to bottom

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35
Q

It is one half the distance between the two nuclei in two adjacent metal atoms or in a diatomic molecule.

A

Atomic radius

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36
Q

The radius of a cation or an anion.

A

Ionic radius

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37
Q

TRUE OR FALSE. The radii of tripositive ions are smaller than those of dipositive ions.

A

. TRUE

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38
Q

How many Elements are gases under atmospheric conditions?

A

11 Elements .

They are the Group 8A elements and the other five are H2, N2, O2, F2, and Cl2.

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39
Q

How many Elements are liquid under atmospheric conditions?

A

There are only two liquid elements at 25C. These are mercury and bromine. Francium melts at 23C.

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40
Q

It is the minimum energy required to remove an electron from a gaseous atom in its ground state.

A

Ionization energy

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41
Q

Electron affinity is positive if the reaction is_____.

Negative if the reaction is ____.

A

EXOTHERMIC; ENDOTHERMIC

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42
Q

Similarities between pairs of elements in different groups and periods of periodic table.

A

Diagonal Relationship

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43
Q

The charge ion divided by its volume.

A

Charge density

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44
Q

Peroxides (contains O22- ion). ______ (contains O2- ion).

A

Superoxides

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45
Q

This oxide display both the acidic and basic properties.

A

Amphoteric

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46
Q

This should not be stored in Pyrex Glass.

A

NaOH

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47
Q

Ramsay and Lord Rayleigh discovered _____ which means “the lazy one”. Also in 1898 Ramsay isolated helium from uranium ores.

A

Argon

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48
Q

Ramsay and his student, Morris Travers set out to find the unknown gases. They used a ____ to first produce liquid air. Applying a technique called ______, they then allowed the liquid air to warm up gradually and collected components that boiled off at different temperatures. In this manner, they analyzed and identified three new elements—neon, krypton, and xenon—in only three months. Three new elements in three months is a record that may never be broken!

A

refrigeration machine; fractional distillation

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49
Q

Chemists define_____ as directed energy change resulting from a process.

A

work

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50
Q

is the energy associated with the random motion of atoms and molecules. The more vigorous the motion of the atoms and molecules in a sample of matter, the hotter the sample is and the greater its thermal energy.

A

Thermal energy

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51
Q

is stored within the structural units of chemical substances; its quantity is determined by the type and arrangement of constituent atoms.

A

Chemical energy

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52
Q

study of heat change in chemical reactions.

A

Thermochemistry

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53
Q

In thermodynamics, we study changes in the _____ which is defined by the values of all relevant macroscopic properties, for example, composition, energy, temperature, pressure, and volume.

A

state of a system

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54
Q

Melting 1 mole of ice at 0°C

A

endothermic process

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55
Q

Burning 1 mole of methane in oxygen gas

A

exothermic process

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56
Q

Sodium reacting with water to can also form

A

hydrogen gas

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57
Q

Carbon monoxide burns in air to form

A

carbon dioxide

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58
Q

is the measurement of heat changes

A

Calorimetry

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59
Q

The “sea level” reference point for all enthalpy expressions is called

A

standard of enthalpy of formation

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60
Q

By convention, the standard enthalpy of formation of any element in its most stable form is

A

zero

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61
Q

White phosphorus burns in air to form

A

P4O10.

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62
Q

can be stated as follows: When reactants are converted to products, the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps.

A

Hess’s law

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63
Q

is called the father of thermochemistry.

A

Germain Henri Hess

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64
Q

An ______ has a high flame temperature (3000°C) and is used to weld metals.

A

oxyacetylene torch

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65
Q

The energy required to completely separate one mole of a solid ionic compound into
gaseous ions is called

A

lattice energy (U).

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66
Q

Which of the following is a ketose?

a. fructose b. glucose c. sucrose d. lactose

A

a. fructose

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67
Q

Which of the following amino acid is polar?

a. glutamine b. arginine c. proline d. alanine

A

a. glutamine

68
Q
  1. Plastic used for synthetic leather?

a. PVC b. PE c. PS d. PTFE

A

a. PVC

69
Q
  1. The least number of atoms in alkynes

a. 4 b. 6 c. 5 d. 7

A

a. 4

70
Q

Deuterium is an isotope of

a. hydrogen b. oxygen c. aldehydes d. esters

A

a. hydrogen

71
Q

Ethylene glycol is a

a. triol b. ester c. diol d. phenol

A

c. diol

72
Q

A nuclei of tritium atom would contain ____neutrons.

a. 1 b.2 c. 3 d. 4

A

b.2

73
Q

Transition elements are found in the

a. d and f energy level b. s energy level c. d energy level d. p energy level

A

a. d and f energy level

74
Q
  1. The noble gases are

a. diaotomic b. monoatomic c. triatomic d. monoclinic

A

b. monoatomic

75
Q
  1. The oxidation state of Cr in K2CrO4

a. +6 b. -6 c. -2 d.+7

A

a. +6

76
Q

NO2 is a molecule with a bent structure, the number of lone pair/s in its central atom is
a. one b. two c. three d. four

A

a. one

77
Q

The structure of water can be described as

a. polar and tetrahedral
b. polar linear
c. polar and bent
d. nonpolar and bent

A

c. polar and bent

78
Q

The phenomenon in which a steel needle can, with proper care, be made to float on the surface of some water illustrates a property of liquid known as:
a. compressibility b. polarizability c. surface tension d. triple point

A

c. surface tension

79
Q

From what mineral is radium obtained?

a. limestone b. rutile c. pitch blend d. hematite

A

c. pitch blend

80
Q

Protium atom contains no

a. electron
b. protom
c. neutron
d. positron

A

c. neutron

81
Q

Which of the following is the lightest?

a. alpha particle b. beta particle c. proton d. Hydrogen

A

b. beta particle

82
Q

The shape of “s” orbital is

a. pyramidal
b. tetrahedral
c. spherical
d. dumb-bell shaped

A

c. spherical

83
Q

Isotopes have different

a. period number b. group number c. number of nucleons d. atomic number

A

c. number of nucleons

84
Q

Hydrogen sulfide is removed from water by contacting the solution with warm air. The operation is
a. distillation b. leaching c. absorption d. stripping

A

d. stripping

85
Q
  1. Sulfur is undesirable in petroleum because
    a. it causes engine knocking
    b. it poisons the catalyst in knocking process
    c. it increases the boiling point of fuel
    d. all of the above.
A

a. it causes engine knocking

86
Q

What medicine is also known as acetylsalicylic acid

a. vitamin d b. aspirin c. paracetamol

A

b. aspirin

87
Q

% composition of N2 in air

a. 78.98 b. 78.56 c. 78.03

A

c. 78.03

88
Q

How many litres of blood are there in average adult?

a. 10 L b. 5 L c. 8 L

A

b. 5 L

89
Q

Another important source of oxygen aside from photosynthesis is
a. photodecomposition b.photolysis c.phototrophic

A

a. photodecomposition

90
Q

The violent eruption on the surface of the sun is called

a. solar flare b. solar degeneration c. aurora

A

a. solar flare

91
Q

Lighthing enables production of

a. nitric oxide b. carbon dioxide c. ozones

A

a. nitric oxide

92
Q

The term used by some environmental chemists to describe the corrosion of stone because of acid rain
a. stone degradation b. stone rusting c. stone leprosy

A

c. stone leprosy

93
Q

Photodissociation is the breaking of chemical bonds by

a. radiant energy b. light energy c. sun energy

A

a. radiant energy

94
Q

Stalactites and stalagmites are commonly found in caves. These are made up of
a. sodium sulfate b. magnesia c. calcium carbonate

A

c. calcium carbonate

95
Q

The difference in global temperature between today and the last ice age is only

a. 1-5 deg C
b. 5-8 deg C.
c. 4-5 deg C
d. 6-7 deg C

A

c. 4-5 deg C

96
Q

A dramatic illustration of the greenhouse effect is found on

a. Mars b. Jupiter c. Venus d. Saturn

A

c. Venus

97
Q

Milk of magnesia is commonly used to

a. treat hay fever b. treat acid indigestion c. treat loss of bowel movement

A

b. treat acid indigestion

98
Q

The egg white is also called as

a. melanine b. albumen c. wolk

A

b. albumen

99
Q

Which of the following does not exist in gaseous state?
a. H2 b. O2 c. S2 d. F2

A

c. S2

100
Q

Which of the following is a heavy water?

a. hydrogen dioxide b. tritium oxide c. deuterium oxide d. dihydrogen oxide

A

c. deuterium oxide

101
Q

It commonly known as yellowish gas.

a. Cl2 b. N2 c. CO2 d. H2

A

a. Cl2

102
Q

Which of the following elements and compounds is unstable in its pure form?

a. sodium b. helium c.carbon dioxide d. neon

A


a. sodium

103
Q

The critical point for a mixture occurs for which of the following gases?

a. the vapor and liquid have a single form
b. the vapor phase is stable
c. the liquid has no absorbed gas
d. the liquid is completely vaporized.

A

a. the vapor and liquid have a single form

104
Q

A substance is oxidized when which of the following occurs?

a. it turns red
b. it loses electron
c. it becomes more negative
d. it gives off heat

A

b. it loses electron

105
Q

Because water molecules are associated through hydrogen bonding, water has a high
a. temperature b. density c. boiling point d. solubility

A

c. boiling point

106
Q

It is a generic term for atomic emission involving various noble gases, mercury and phosphor.
a. luminescence b. neon lights c.phospholight

A

b. neon lights

107
Q

The study of ability to follow chemical reaction at molecular level is
a. nanotechnology b.reaction kinetics c. femtochemistry

A

c. femtochemistry

108
Q

Manufacturing of nitric acid follows

a. Ostwald Process b. Holloway process b. Bosch Process

A

a. Ostwald Process

109
Q

. In reality, no acids are known to ionize in water.

a. true b. false c. not at all times

A

a. true

110
Q

The higher the oxidation number of metal, the more ionic the compound.
a. true b. false c. not at all times

A

b. false

111
Q

The total number of electron at 4th energy level.

a. 2 b.10 c. 18 d. 32

A

32

112
Q
  1. Who discovered positron?

a. Anderson b. Pauli c. Heisenberg d. Bohr

A

a. Anderson

113
Q

Magnesium is obtained from

a. sea shells b. sea water c. bentonite d. corals

A

b. sea water

114
Q

Which of the following test will distinguish 1-propanol from 2-propanol?
a. Fehling’s test b. Tollen’s tests c. Benedict tests d. Lucas test

A

d. Lucas test

115
Q

A carboxylic acid which contributes to the strong odor of rancid butter and other fats.
a. caproic acid b. acetic acid c. lactic acid d. butyric acid

A

d. butyric acid

116
Q

The more positive the Emf is, the greater the tendency for the substance to be _____.

A

reduced

117
Q

This principle states that under standard state conditions, any species on the left of a given half cell reaction will react spontaneously with a species that appears on the right side of any half cell reaction

A

DIAGONAL RULE

118
Q

Changing the stoichiometric coefficient of a half cell reaction does not affect the value of emf because electrode potentials are

A

intensive properties.

119
Q

It represents the maximum amount of useful work that can be obtained from a reaction:
a. Internal Energy b. Activation energy c. Free Energy d. Kinetic energy

A

c. Free Energy

120
Q

A series of galvanic cell that can be used as a source of direct electric current at a constant voltage

A

. BATTERY

121
Q

A galvanic cell that requires a continuous supply of reactants to keep functioning

A

FUEL CELL

122
Q

. Process in which electrical energy is used to cause a non-spontaneous chemical reaction to occur

A

ELECTROLYSIS

123
Q

Stereomers that cannot be interconverted without breaking a chemical bond

A

Geometric Isomers

124
Q

These are superimposable mirror images

A

Optical Isomers

125
Q

A gaseous mixture ofpositive ions and electrons is called

A

Plasma

126
Q

For a process at equilibrium, the total entropy is equal to

A

zero

127
Q

It states that we can use a thermodynamically favorable reaction to drive an unfavorable one-

A

Coupling Theory.

128
Q

All elements having an atomic number greater than ____ are radioactive.

A

83

129
Q

A phenomena that results from the bombardment of nuclei by neutrons, protons or other nuclei.

A

Nuclear Transmutation

130
Q

The stability of any nucleus is determined by the difference between

A

Coulombic repulsion and short-range attraction

131
Q

What happens to the nucleus if repulsion outweighs attraction?

A

The nucleus disintegrates, emitting particles and/or radiation.

132
Q

What happens to the nucleus when attractive forces prevail rather than repulsion?

A

It becomes stable

133
Q

Nuclei that contains ____number of protons and neutrons are generally more stable than those with ___ numbers of this particle.

A

EVEN, ODD

134
Q

Which is not a magic number?

A. 2 B. 126 C. 96 D. 50 E. 82 F. 20 G. 8

A

C. 96

135
Q

This is the energy required to break up a nucleus into its component protons and neutrons.

A

Nuclear Binding Energy

136
Q

The difference between the mass of an atom and the sum of the masses of its protons, neutrons and electrons is called-

A

Mass defect

137
Q

A sequence of nuclear reactions that ultimately result in the formation of stable isotope –

A

Radioactive Series decay

138
Q

. Elements with atomic number greater than 92 is called

A

Transuranium Elements.

139
Q

This is the minimum mass of fissionable material required to generate a self-sustaining nuclear chain reactions-

A

Critical Mass

140
Q

First application of Nuclear Fission

A

manufacture of Nuclear Bomb

141
Q

These are substances that can reduce the kinetic energy of neutrons

A

Moderators.

142
Q

What is the difference between an atomic bomb and a nuclear reactor?

A

This is that the chain reaction that takes place in a nuclear reactor is kept under control at all times.

143
Q

This type of reactor produces more fissionable materials than it uses

A

Breeder Reactor

144
Q

The natural abundance of U-235

A
  • 0.7202 %
145
Q

Nuclear Fusion reactions are also called

A

Thermonuclear reactions.

146
Q

Isotopes that are used to trace the path of the atoms of an element in a chemical or biological process are called-

A

TRACERS

147
Q

This is an isotope that is injected into the bloodstream as a salt solution that can monitor the traceof the flow of blood.

A

Sodium- 24

148
Q

An isotope that is used to test the activity of the thyroid gland

A
  • Iodine 131
149
Q

An isotope used to image the brain

A

Iodine 123

150
Q

The first artificially prepared element

A

Technetium

151
Q

These are molecular fragments having one or more unpaired electrons

A

Radicals

152
Q

Isotopes that are used as radiation sources for most food preservations are

A

Cobalt 60 and Cesium-137

153
Q

A type of radiation damage that affects the organism during its own lifetime-

A

Somatic

154
Q

This is the type of ice that burns

A

Methane Hydrate

155
Q

Violent eruptions on the surface of the sun

A

SOLAR FLARES

156
Q

The layer of the atmosphere that contains about 80% of the total mass of air and practically all of the atmosphere’s water vapor.

A

Troposphere

157
Q

The ozonolysis of Alkene produces

A

Aldehyde and Ketone

158
Q

It states that the halogen attaches to the carbon that is more alkyl substituted thus producing a higher alkyl halide.

A

Markovnikoff’s Rule

159
Q

The Dehydration of an Aklyl halide in the presence of a base catalyst produces

A

Alkene

160
Q

Region of space about the nucleus in which there is a high probability of finding an electron

A

Atomic Orbital

161
Q

Head to head overlap

A

Sigma Bond

162
Q

Side by side overlap

A

Pi Bond

163
Q

States that alkyl formed is the one that is more alkyl substituted

A

Saitsev Rule

164
Q

Hydration of Alkene produces

A

Alcohol

165
Q

The odor of rotting fish is caused by

A

Methylamine

166
Q

Major constituent of photochemical smog

A

ozone

167
Q

Species that contain a negatively charges, trivalent carbon

A

Carbanion

Algebra (2 decks)

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