_____ Flashcards
1
Q
This is the smallest energy that can be emitted (or absorbed) in the form of electromagnetic waves
A
QUANTUM
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.
3
Q
An electron bound to the nucleus behaves like a
A
STANDING WAVE.
4
Q
First known laser
A
RUBY LASER
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
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))
7
Q
Group of elements which have incompletely filled d subshells
A
TRANSITION METALS
8
Q
Series of elements that are not usually found in nature but is always synthesized
A
Actinide series
9
Q
Group of elements that have incompletely filled 4f subshells
A
LANTHANIDES OR RARE EARTH
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
11
Q
Atoms of elements with low ionization energies tend to form
A
CATIONS
12
Q
Atoms with high electron affinities tend to form
A
ANIONS
13
Q
The elements that are most likely to form cations in ionic compounds are
A
ALKALI METALS AND ALKALI EARTH METALS
14
Q
These are elements that are likely to form anions
A
HALOGENS AND OXYGEN
15
Q
A poisonous white powder used in lowering the melting point of solders in manufacturing ceramics.
A
LITHIUM FLUORIDE
16
Q
This is the energy required to completely separate one mole of a solid ionic compound into gaseous ions-
A
LATTICE ENERGY
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
18
Q
To form an ionic bond the electronegativity difference between two bonding atoms should be-
A
2.0 or more.
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.
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
21
Q
Which rule is followed by Hydrogen
a. duet rule b. octet rule c. triad rule
A
a. duet rule
22
Q
Who proposed the hexagonal structure of benzene?
A
August Kekule
23
Q
Resonance structures with formal charges greater than____ are usually considered highly implausible and can be discarded.
A
+2 or -2
24
Q
Which period of elements in the table cannot have an expanded octet?
A
Second-period
25
The most reactive metals are in ____ and the most reactive nonmentals in ___.
Group 1A, Group 7A
26
What element melts in a person’s body?
Gallium
27
Mendeleev proposed the existence of an unknown element he called ____ which has properties close to Gallium.
eka-aluminum
28
His work on periodic classification of elements is regarded by many as the most significant achievement I chemistry in nineteenth century.
Dmitri Mendeleev
29
He discovered the chemical affinity of hemoglobin for oxygen.
Julius Lothar Meyer
30
The non-valence electrons are called
core electrons
31
The representative elements are the elements in _____, all of which have incompletely filled s or p subshells of the highest principal quantum number.
Groups 1A through 7A
32
The transition metals are the elements in ____, which have incompletely filled d subshells.
Group 1B, 3B through 8B
33
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.
effective nuclear charge
34
The increase in effective nuclear charge from_____ a period and from ____ in a group for representative elements.
left to right across a period and from top to bottom
35
It is one half the distance between the two nuclei in two adjacent metal atoms or in a diatomic molecule.
Atomic radius
36
The radius of a cation or an anion.
Ionic radius
37
TRUE OR FALSE. The radii of tripositive ions are smaller than those of dipositive ions.
. TRUE
38
How many Elements are gases under atmospheric conditions?
11 Elements .
| They are the Group 8A elements and the other five are H2, N2, O2, F2, and Cl2.
39
How many Elements are liquid under atmospheric conditions?
There are only two liquid elements at 25C. These are mercury and bromine. Francium melts at 23C.
40
It is the minimum energy required to remove an electron from a gaseous atom in its ground state.
Ionization energy
41
Electron affinity is positive if the reaction is_____.
| Negative if the reaction is ____.
EXOTHERMIC; ENDOTHERMIC
42
Similarities between pairs of elements in different groups and periods of periodic table.
Diagonal Relationship
43
The charge ion divided by its volume.
Charge density
44
Peroxides (contains O22- ion). ______ (contains O2- ion).
Superoxides
45
This oxide display both the acidic and basic properties.
Amphoteric
46
This should not be stored in Pyrex Glass.
NaOH
47
Ramsay and Lord Rayleigh discovered _____ which means “the lazy one”. Also in 1898 Ramsay isolated helium from uranium ores.
Argon
48
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!
refrigeration machine; fractional distillation
49
Chemists define_____ as directed energy change resulting from a process.
work
50
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.
Thermal energy
51
is stored within the structural units of chemical substances; its quantity is determined by the type and arrangement of constituent atoms.
Chemical energy
52
study of heat change in chemical reactions.
Thermochemistry
53
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.
state of a system
54
Melting 1 mole of ice at 0°C
endothermic process
55
Burning 1 mole of methane in oxygen gas
exothermic process
56
Sodium reacting with water to can also form
hydrogen gas
57
Carbon monoxide burns in air to form
carbon dioxide
58
is the measurement of heat changes
Calorimetry
59
The “sea level” reference point for all enthalpy expressions is called
standard of enthalpy of formation
60
By convention, the standard enthalpy of formation of any element in its most stable form is
zero
61
White phosphorus burns in air to form
P4O10.
62
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.
Hess’s law
63
is called the father of thermochemistry.
Germain Henri Hess
64
An ______ has a high flame temperature (3000°C) and is used to weld metals.
oxyacetylene torch
65
The energy required to completely separate one mole of a solid ionic compound into
gaseous ions is called
lattice energy (U).
66
Which of the following is a ketose?
| a. fructose b. glucose c. sucrose d. lactose
a. fructose
67
Which of the following amino acid is polar?
| a. glutamine b. arginine c. proline d. alanine
a. glutamine
68
3. Plastic used for synthetic leather?
| a. PVC b. PE c. PS d. PTFE
a. PVC
69
4. The least number of atoms in alkynes
| a. 4 b. 6 c. 5 d. 7
a. 4
70
Deuterium is an isotope of
| a. hydrogen b. oxygen c. aldehydes d. esters
a. hydrogen
71
Ethylene glycol is a
| a. triol b. ester c. diol d. phenol
c. diol
72
A nuclei of tritium atom would contain ____neutrons.
| a. 1 b.2 c. 3 d. 4
b.2
73
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. d and f energy level
74
9. The noble gases are
| a. diaotomic b. monoatomic c. triatomic d. monoclinic
b. monoatomic
75
10. The oxidation state of Cr in K2CrO4
| a. +6 b. -6 c. -2 d.+7
a. +6
76
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. one
77
The structure of water can be described as
a. polar and tetrahedral
b. polar linear
c. polar and bent
d. nonpolar and bent
c. polar and bent
78
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
c. surface tension
79
From what mineral is radium obtained?
| a. limestone b. rutile c. pitch blend d. hematite
c. pitch blend
80
Protium atom contains no
a. electron
b. protom
c. neutron
d. positron
c. neutron
81
Which of the following is the lightest?
| a. alpha particle b. beta particle c. proton d. Hydrogen
b. beta particle
82
The shape of “s” orbital is
a. pyramidal
b. tetrahedral
c. spherical
d. dumb-bell shaped
c. spherical
83
Isotopes have different
| a. period number b. group number c. number of nucleons d. atomic number
c. number of nucleons
84
Hydrogen sulfide is removed from water by contacting the solution with warm air. The operation is
a. distillation b. leaching c. absorption d. stripping
d. stripping
85
10. 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. it causes engine knocking
86
What medicine is also known as acetylsalicylic acid
| a. vitamin d b. aspirin c. paracetamol
b. aspirin
87
% composition of N2 in air
| a. 78.98 b. 78.56 c. 78.03
c. 78.03
88
How many litres of blood are there in average adult?
| a. 10 L b. 5 L c. 8 L
b. 5 L
89
Another important source of oxygen aside from photosynthesis is
a. photodecomposition b.photolysis c.phototrophic
a. photodecomposition
90
The violent eruption on the surface of the sun is called
| a. solar flare b. solar degeneration c. aurora
a. solar flare
91
Lighthing enables production of
| a. nitric oxide b. carbon dioxide c. ozones
a. nitric oxide
92
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
c. stone leprosy
93
Photodissociation is the breaking of chemical bonds by
| a. radiant energy b. light energy c. sun energy
a. radiant energy
94
Stalactites and stalagmites are commonly found in caves. These are made up of
a. sodium sulfate b. magnesia c. calcium carbonate
c. calcium carbonate
95
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
c. 4-5 deg C
96
A dramatic illustration of the greenhouse effect is found on
| a. Mars b. Jupiter c. Venus d. Saturn
c. Venus
97
Milk of magnesia is commonly used to
| a. treat hay fever b. treat acid indigestion c. treat loss of bowel movement
b. treat acid indigestion
98
The egg white is also called as
| a. melanine b. albumen c. wolk
b. albumen
99
Which of the following does not exist in gaseous state?
a. H2 b. O2 c. S2 d. F2
c. S2
100
Which of the following is a heavy water?
| a. hydrogen dioxide b. tritium oxide c. deuterium oxide d. dihydrogen oxide
c. deuterium oxide
101
It commonly known as yellowish gas.
| a. Cl2 b. N2 c. CO2 d. H2
a. Cl2
102
Which of the following elements and compounds is unstable in its pure form?
a. sodium b. helium c.carbon dioxide d. neon
a. sodium
103
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. the vapor and liquid have a single form
104
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
b. it loses electron
105
Because water molecules are associated through hydrogen bonding, water has a high
a. temperature b. density c. boiling point d. solubility
c. boiling point
106
It is a generic term for atomic emission involving various noble gases, mercury and phosphor.
a. luminescence b. neon lights c.phospholight
b. neon lights
107
The study of ability to follow chemical reaction at molecular level is
a. nanotechnology b.reaction kinetics c. femtochemistry
c. femtochemistry
108
Manufacturing of nitric acid follows
| a. Ostwald Process b. Holloway process b. Bosch Process
a. Ostwald Process
109
. In reality, no acids are known to ionize in water.
| a. true b. false c. not at all times
a. true
110
The higher the oxidation number of metal, the more ionic the compound.
a. true b. false c. not at all times
b. false
111
The total number of electron at 4th energy level.
| a. 2 b.10 c. 18 d. 32
32
112
7. Who discovered positron?
| a. Anderson b. Pauli c. Heisenberg d. Bohr
a. Anderson
113
Magnesium is obtained from
| a. sea shells b. sea water c. bentonite d. corals
b. sea water
114
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
d. Lucas test
115
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
d. butyric acid
116
The more positive the Emf is, the greater the tendency for the substance to be _____.
reduced
117
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
DIAGONAL RULE
118
Changing the stoichiometric coefficient of a half cell reaction does not affect the value of emf because electrode potentials are
intensive properties.
119
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
c. Free Energy
120
A series of galvanic cell that can be used as a source of direct electric current at a constant voltage
. BATTERY
121
A galvanic cell that requires a continuous supply of reactants to keep functioning
FUEL CELL
122
. Process in which electrical energy is used to cause a non-spontaneous chemical reaction to occur
ELECTROLYSIS
123
Stereomers that cannot be interconverted without breaking a chemical bond
Geometric Isomers
124
These are superimposable mirror images
Optical Isomers
125
A gaseous mixture ofpositive ions and electrons is called
Plasma
126
For a process at equilibrium, the total entropy is equal to
zero
127
It states that we can use a thermodynamically favorable reaction to drive an unfavorable one-
Coupling Theory.
128
All elements having an atomic number greater than ____ are radioactive.
83
129
A phenomena that results from the bombardment of nuclei by neutrons, protons or other nuclei.
Nuclear Transmutation
130
The stability of any nucleus is determined by the difference between
Coulombic repulsion and short-range attraction
131
What happens to the nucleus if repulsion outweighs attraction?
The nucleus disintegrates, emitting particles and/or radiation.
132
What happens to the nucleus when attractive forces prevail rather than repulsion?
It becomes stable
133
Nuclei that contains ____number of protons and neutrons are generally more stable than those with ___ numbers of this particle.
EVEN, ODD
134
Which is not a magic number?
| A. 2 B. 126 C. 96 D. 50 E. 82 F. 20 G. 8
C. 96
135
This is the energy required to break up a nucleus into its component protons and neutrons.
Nuclear Binding Energy
136
The difference between the mass of an atom and the sum of the masses of its protons, neutrons and electrons is called-
Mass defect
137
A sequence of nuclear reactions that ultimately result in the formation of stable isotope –
Radioactive Series decay
138
. Elements with atomic number greater than 92 is called
Transuranium Elements.
139
This is the minimum mass of fissionable material required to generate a self-sustaining nuclear chain reactions-
Critical Mass
140
First application of Nuclear Fission
manufacture of Nuclear Bomb
141
These are substances that can reduce the kinetic energy of neutrons
Moderators.
142
What is the difference between an atomic bomb and a nuclear reactor?
This is that the chain reaction that takes place in a nuclear reactor is kept under control at all times.
143
This type of reactor produces more fissionable materials than it uses
Breeder Reactor
144
The natural abundance of U-235
- 0.7202 %
145
Nuclear Fusion reactions are also called
Thermonuclear reactions.
146
Isotopes that are used to trace the path of the atoms of an element in a chemical or biological process are called-
TRACERS
147
This is an isotope that is injected into the bloodstream as a salt solution that can monitor the traceof the flow of blood.
Sodium- 24
148
An isotope that is used to test the activity of the thyroid gland
- Iodine 131
149
An isotope used to image the brain
Iodine 123
150
The first artificially prepared element
Technetium
151
These are molecular fragments having one or more unpaired electrons
Radicals
152
Isotopes that are used as radiation sources for most food preservations are
Cobalt 60 and Cesium-137
153
A type of radiation damage that affects the organism during its own lifetime-
Somatic
154
This is the type of ice that burns
Methane Hydrate
155
Violent eruptions on the surface of the sun
SOLAR FLARES
156
The layer of the atmosphere that contains about 80% of the total mass of air and practically all of the atmosphere’s water vapor.
Troposphere
157
The ozonolysis of Alkene produces
Aldehyde and Ketone
158
It states that the halogen attaches to the carbon that is more alkyl substituted thus producing a higher alkyl halide.
Markovnikoff’s Rule
159
The Dehydration of an Aklyl halide in the presence of a base catalyst produces
Alkene
160
Region of space about the nucleus in which there is a high probability of finding an electron
Atomic Orbital
161
Head to head overlap
Sigma Bond
162
Side by side overlap
Pi Bond
163
States that alkyl formed is the one that is more alkyl substituted
Saitsev Rule
164
Hydration of Alkene produces
Alcohol
165
The odor of rotting fish is caused by
Methylamine
166
Major constituent of photochemical smog
ozone
167
Species that contain a negatively charges, trivalent carbon
Carbanion
