CHM101_OBJ_Questions.txt

[MAX]110[/MAX]

[QUESTIONS]

<1>In the periodic table,period 6 contains ------ elements

<2>Which of these is not an isotope of hydrogen?

<3>__________ forms an oxide also known as heavy water.

<4>Which of the isotopes of hydrogen is radioactive?

<5>All these can be used as raw materials for the production of oxygen except

<6>Hydrogen can be obtained economically as a bi-product in the electrolysis of -----

<7>Which if these is not a property of hydrogen?

<8>Hydrogen may be used for all but one of the following.

<9>Hydrogen may not be advantagous as a fuel because-------

<10>Hydrogen may be used for all but one of the following

<11>______types of hydride compounds can be formed depending on the electronegativity of the elements

<12>When alkali metals are heated with hydrogen they form--------hydrides

<13>Silt is an example of ------ hydride

<14>Which of these statements is not true of metallic hydrides?

<15>Sodium Hydride is an example of ------- hydride

<16>All these are types of metal lattices except-------

<17>Which of these statements is not true of metallic elements?

<18>All these are consequences of the sole valence electron in alkali metals except ------

<19>Which of these statements is not true?

<20>In the group of the alkali metals the degree of hydration-------- down the group.

<21>When a metal is sourrounded by solvent molecules not water, the phenomenon is called--------

<22>Which of these element does not belong to the alkali metals

<23>Decrease in hydration energy makes a compound ------

<24>Which of these increases solubility of compounds

<25>The charge on cations------ down a group

<26>Hydrides of alkali metals react with water to librate------

<27>Alkali metals react with sulphur to form ---- types of sulphides

<28>Ionization energy------ down the group within the alkali metals

<29>Within the alkali metals atomic size -------

<30>Potassium compounds can be used for all but one of the following

<31>Alkali metals can be used for all but one of the following

<32>A consequence of ------- is the formation of a chelate ring

<33>Which of these hydrides has the high boiling point?

<34>Which of these metals is radioactive?

<35>The most abundant metal in sea water is -------

<36>Which of these bonds has the weakest bond energy?

<37>The attractive force which binds a hydrogen atom of one molecule with an electronegative atom of another molecule of the same compound is called---------

<38>Increase in principal quantum number(n) means-----of the atomic radii

<39>Except for rubidium and caesium,

<40>_____is defined as one-half of the distance between the nuclei of two adjacent metal atoms in the close packed crystal lattice

<41>_____states that as far as possible in a given atom in the ground state, electrons in the same sub shell will occupy different orbitals and will have parallel spins.

<42>The alkali metals belong to the ------ elements

<43>Which is of these peroids of the peroidic table has only eight elements?

<44>Increase in principal quantum number(n) means-----of the atomic radii

<45>In the equation for ionization,effective nuclear charge is represented as------

<46>The ability of an element to participate in a chemical reaction is measured in form of its ---------

<47>____is the energy released or absorbed when an electron is added to the gaseous atom in its ground state

<48>Electron affinity can be affected by all but one of the following

<49>Halogens have ------ electron affinity

<50>An orbital can have at the most two electrons of opposite spin can be called the -------

<51>In the mordern form of Mendeleev peroidic table, elements are arranged in --------horizontal rows.

<52>The positions of K and Ar,Co and Ni do not remain anomalous any longer since --------- is used in arranging the elements.

<53>The properties of elements are periodic functions of their atomic numbers is the-----------

<54>What property was used by Mendeleev to classify the elements?

<55>_________ used the Law of the Octave to arrange atoms

<56>__________ arranged elements in order of increasing atomic weight on a line which spiraled around a cylinder from bottom to top

<57>________and____________ tried to classify elements into periods

<58>_________is the tendency of an atom to attract towards itself the shared electron pair of a bond in which it is involved

<59>The second ionization energy of alkaline earth metals is less than that of corresponding alkali metals because--------

<60>____________is the enthalpy change when one mole of crystal lattice is formed from the isolated gaseous ions

<61>A hybrid orbitals that has greater s-character is more likely to possess --------

<62>Which of these is an sp-hybridized compound?

<63>The presence of hydrogen bond in most molecules is responsible for the following except;

<64>Which of these is not a covalent hydride?

<65>When alkali metals are heated with hydrogen they form--------hydrides

<66>Hydrogen can be obtained economically as a bi-product in the electrolysis of ------

<67>One of these elements behave partly as the alkaline metals as well as a halogen element;

<68>The tendency of an atom to attract shared electron pair of bond towards itself is known as

<69>Which of the following is not true as we move down a group of s and p-block elements in the periodic table

<70>The energy required to remove two valency electrons of a metallic atom is called;

<71>Which of these elements has the electonic configuration of 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10}4s^{1}

<72>All common cations are smaller than all common anions except one of these;

<73>One half of the distance between the nuclei of two atoms bonded together by a single bond is known as

<74> one of the following is not a d-block element?

<75>Which of these is not an s-block element

<76>The energy absorbed or released when an electron is added to a gaseous atom is known as

<77> One half of the distance between the nuclei of two adjacent metal atoms in a close crystal lattice is called

<78>One of the following scientists never made any contribution to the development of periodic table?

<79>Which of these is not a property of metallic element?

<80>Newlands law of octaves was rejected mainly because of;

<81>What is the oxidation state of H2?

<82>What is the oxidation state of gold in Au(CN)4-?

<83>What is the oxidation state of Xe in XeOF4?

<84>In which of the following compounds does O have an oxidation state not equal to -2?

<85>Which of the following reactions is NOT a redox reaction?

<86>Give the line notation for a cell that reduces CuSO4 to Cu and oxidizes Zn to Zn2+.

<87>In the following galvanic cell, identify the direction of electron flow: Pt (s) | MnO4- (aq), Mn2+ (aq), H+ (aq) || Fe2+ (aq), Fe3+ (aq) | Pt (s)

<88>What is the direction of ion flow through a porous disk in a galvanic cell?

<89>What is the sign of E for a galvanic cell?

<90>Which half-reaction takes place at the anode?

<91>What is the free energy of formation for water, given its Eo for decomposition into hydrogen and oxygen is -1.23 V?

<92>Using your chemical intuition, which of the following species is the strongest oxidizing agent?

<93>What is a faraday?

<94>What happens to the cell potential of a non-standard state reaction when the temperature increases?

<95>Which of the following statements about concentration cells are true?

<96>What is the direction of ion flow through the porous disk in a concentration cell?

<97>Which of the following redox reactions is primarily responsible for producing most of what you eat?

<98>At which electrode is H2 in the electrolysis of water?

<99>Which of the following is NOT produced during the electrolysis of water?

<100>Using your chemical intuition, what combination of elements would make a very powerful battery?

<101>What is meant by the total rate of a reaction?

<102>Which of the following rate laws could describe a third order reaction?

<103>What are the units for k in a zeroth order reaction?

<104>If a reaction requires two moles of a single reagent to produce one mole of product, what is the ratio of the rate of product formation to the rate of reactant consumption?

<105>Under what circumstances should you not use the method of initial rates to determine the rate law for a reaction?

<106>Which of the following is a technique used to stop a reaction for analysis?

<107>What is a half-life?

<108>A mechanism...

<109>Which of the following is not true about the action of a catalyst?

<110>What is rate?

[/QUESTIONS]

[OPTIONS]

<1>32
16
24
8

<2>Protrium
Deutrium
Tritium
Neutrium

<3>Protrium
Deutrium
Tritium
Neutrium

<4>Tritium
Protium
Deutrium
Neutrium

<5>steam
coke
carbon(II)oxide
nitrogen

<6>brine
sodium hydroxide
water
platinium

<7>it is colourless
it has a pungent smell
it can be oxidized to water
It reduces sulphur to hydogen sulphide

<8>synthesis of zinc
hydrogenation of oil
manufacture of methanol
Synthesis of ammomia

<9>It has unlimited quantities in the sea
It is pollution free
It can be stored and used when needed
it is a secondary source of energy

<10>Synthesis of ammomia
hydrogenation of oil
manufacture of methanol
synthesis of zinc

<11>1
2
3
4

<12>covalent
ionic
mettalic
non-stoichiometric

<13>superior
covalent
mettalic
ionic

<14>they are volatile
they are deficient in hydrogen
most have metallic appearance
They are all conductors of heat

<15>covalent
ionic
mettalic
non-stoichiometric

<16>body-centred cubic
bexagonal
hexagonal
cubic close packed

<17>they are ductile
they have lustre
They form acidic oxides
they are malleable

<18>the metals are soft
good conduction of electricity
good conduction of heat
the silvery luster

<19>liquid ammonia is is used to form carbides
All metals react with carbon to form carbides
lithium reacts with carbon to form ionic carbides
Acetylene is neccesary for the formation of some carbide

<20>decreases
increases
is constant
has no fixed pattern

<21>instability
hydration
complexation
solvation

<22>caesuim
rubidium
lithium
Radium

<23>electropositive
electronegative
insoluble
soluble

<24>two cations
a small cation and a large anion
a large cation and anion
a small cation and anion

<25>remains constant
does not have a fixed pattern
increases
decreases

<26>light
oxygen
hydrogen
ammonia

<27>2
3
4
5

<28>increases
has no fixed pattern
decreases
remains constant

<29>has no pattern
remains the same
increases down the group
decreases down the group

<30>manufacture of glass
liquid detergent
plant fertilizer
gun powder

<31>street lights
rocket fuel
as a coolant
undergroud high voltage transmission

<32>intramolecular covalent bonding
intermolecular covalent bonding
intramolecular hydrogen bonding
intermolecular hydrogen bonding

<33>boron hydride
stannane
water
methane

<34>rubbium
francium
pottasium
littium

<35>zinc
sodium
lithium
rubidium

<36>hydrogen bond
electrovalent bond
covalent bond
mettalic bond

<37>nuclear bond
electromagnetic force
hydrogen bond
covalent bond

<38>shrinking
no change
increase
decrease

<39>all common cations are smaller than all common anions
all common cations are larger than all common anions
all common cations are of the same size with all common anions
the cations are not avaliable

<40>ionic radius
metallic radius
covalent radius
atomic radius

<41>Paul Exclusion principles
Hund's rule
Guy's law
Aufbau's principle

<42> d-block
f-block
p-block
s-block

<43>1
3
5
7

<44>shrinking
no change
increase
decrease

<45>I
Z*
e
v

<46>electron density
electron cloud
ionization energy
nuclear charge

<47>electron charge
electronegativity
ionization energy
electron affinity

<48>effective nuclear charge
atomic radius
mass number
electronic configuration

<49>exothermic
endothermic
positive
zero

<50>aufbau principle
Hendry's law
Hund's rule
Exclusion principle

<51>6
7
8
9

<52>mass number
atomic weight
atomic number
moecular mass

<53>Lecoq de Biosbaudran' law
Mordern periodic law
Newlands'law
Mendeleev law

<54>atomic number
atomic weight
mass number
chemical properties

<55>John Newlands
Meyer
De Chancourtois
Dobereiner

<56>John Newlands
Meyer
De Chanourtios
Mendeleev

<57>De Chancourtois and Dobereiner
Gibbs and Dobereiner
De Chancourtois and Le Chatiler
Graham and Dalton

<58>electron affinity
electronegativity
atomic attraction
bonding

<59>the alkaline earth metals have higher nuclear charge and are smaller in size
the alkali metals have no nuclear charge
of stability of a closed shell configuration
the alkali metals have higher nuclear charge and are smaller in size

<60> hydration energy
lattice energy
ionisation energy
gaseous energy

<61>Higher ionization energy
Greater electronegativity
Lower electronegativity
All of the above

<62>CH_{4}
C_{2}H_{4}
C_{2}H_{2}
C_{2}H-{6}

<63>High melting point
Low boiling point
High solubility in water
Very high boiling point

<64>Ammonia
Ethyne
Hydrochloric acid gas
NaH

<65>covalent
Ionic
metallic
non-stoichiometric

<66>brine
water
Sodium hydroxide
Calcium chloride

<67>Helium
Fluorine
Hydrogen
Silicon

<68>Electronegativity
Electron affinity
Ionization energy
Hydrogen bonding

<69>Effective nuclear charge is relatively constant
Atomic radius increase steadly
The value of principal quantum number increases
Electronegativity also increases

<70>Ionization energy
Electron affinity
Activation energy
Second ionization energy

<71>Cu
Zn
Ca
Kr

<72>Rubidium
Calcium
Sodium
Magnesium

<73>Covalent radius
Ionic radius
Van der waals radius
ionic radius

<74>Vanadium
Zinc
Titanium
Aluminium

<75>K
Ca
Zn
Mg

<76>Electronegativity
Ionization energy
Electron affinity
corrosion

<77>Ionic radius
Covalent radius
Metallic radius
Van der waal's radius

<78> J.J Thompson
John Newlands
Luther Meyer
Mendeleev

<79>Form basic oxide
Conduct heat and electricity
They are malleable and lustrous
They form acidic oxide

<80>Elements were arranged in increasing order of atomic mass
The cycle of repetition shown by elements is similar to octave in music
It could not hold good for elements heaver than calcium
Many radioactive elements have not been discovered then

<81>1
0
-1
1/2

<82>3
-1
0
4

<83>2
-2
6
-6

<84>H2O
HOF
ClO4-
H2SO4

<85>Na + Cl ---> NaCl
H2O2 ---> HO2- + H+
Ni2+ + Fe ---> Fe2+ + Ni
NaOH + HCl ---> NaCl + H2O

<86>Cu (s) | Cu2+ (aq) || Zn2+ (aq) | Zn (s)
Zn (s) | Zn2+ (aq) || Cu2+ (aq) | Cu (s)
Zn (s) | Zn2+ (aq), SO42- (aq) || Cu2+ (aq), SO42- (aq) | Cu (s)
Cu (s) | Cu2+ (aq), SO42- (aq) || Zn2+ (aq), SO42- (aq) | Zn (s)

<87>From anode to cathode: right half-cell to left half-cell
From cathode to anode: right half-cell to left half-cell
From cathode to anode: left half-cell to right half-cell
From anode to cathode: left half-cell to right half-cell

<88>There is no ion flow through the disk whose purpose is to separate the two half-cells
Negative ions flow from the oxidation half-cell to the reduction half-cell
Positive ions flow from the anode half-cell to the cathode half-cell
Negative ions flow from the oxidation half-cell to the reduction half-cell

<89>Positive
Negative
Either positive or negative
Zero

<90>The one with the greater reduction potential
The one that transfers the most number of electrons
The reduction
The oxidation

<91>-475 kJ / mol
-237 kJ / mol
237 kJ / mol
475 kJ / mol

<92>F2
H2
Br2
Ca

<93>A unit of current
A unit of energy
A unit of charge
A mole of electrons

<94>Decreases
Increases
Stays the same
Not enough information to solve the problem

<95>The electrons flow from the cathode to the anode
Their potentials are constant in time
Useful voltages cannot be harnessed from such cells
Reduced material can plate at the cathode

<96>Negative ions flow from the anode compartment to the cathode compartment
Positive ions flow from the oxidation half-cell to the reduction half-cell
There is no ion flow in a concentration cell because it is not a real reaction
Positive ions flow from the reduction half-cell to the oxidation half-cell

<97>CH4 + O2 ---> CH3OH
C2H6 + O2 ---> C2H5OH
CO2 + H2O ---> C6H12O6
CO2 + CH4 ---> C2H4O2

<98>The anode
The electrode connected to the negative side of the battery
The cathode
Cannot be determined with the given information

<99>Electricity
Acid
Hydrogen
Oxygen

<100>F and Cl
F and Li
I and Fe
Cd and Fe

<101>The forward rate of the reaction
The reverse rate of the reaction
The sum of the forward and reverse rates of the reaction
None of the above

<102>rate = 3
rate = k [A]
rate = k [A]2
rate = k [A] [B] [C]

<103>M / s
None
s-1
M

<104>2 : 1
1 : 2
1 : 1
Cannot be determined

<105>Very fast reactions
Colored reactions
Clear, colorless reactions
Very slow reactions

<106>Quenching
Photoelectron spectroscopy
NMR
Method of initial rates

<107>The time it takes for one-half of the products to be produced
The time it takes for one-half of the limiting reagent to be consumed
Half of the time the reaction takes to go to completion
40 years old

<108>is experimentally determined.
is a series of reactions.
is not valid because it cannot be proven.
can never be proven.

<109>It speeds up a reaction
It is present in the balanced equation for the reaction it catalyzes
It lowers the activation energy of the reaction
It is involved in the mechanism of the reaction

<110>The time rate of change in the concentrations of reactants
The time rate of change in the concentration of products
rate = [A] [B]
None of the above

[/OPTIONS]

[ANSWERS]

<1>32

<2>Neutrium

<3>Deutrium

<4>Tritium

<5>nitrogen

<6>brine

<7>it has a pungent smell

<8>synthesis of zinc

<9> it is a secondary source of energy

<10>synthesis of zinc

<11>3

<12>ionic

<13>covalent

<14>they are volatile

<15>ionic

<16>hexagonal

<17>They form acidic oxides

<18>the metals are soft

<19>All metals react with carbon to form carbides

<20>decreases

<21>solvation

<22>Radium

<23>insoluble

<24>a small cation and a large anion

<25>remains constant

<26>hydrogen

<27>2

<28>decreases

<29>increases down the group

<30>manufacture of glass

<31>rocket fuel

<32>intramolecular hydrogen bonding

<33>water

<34>francium

<35>sodium

<36>hydrogen bond

<37>hydrogen bond

<38>increase

<39>all common cations are smaller than all common anions

<40>metallic radius

<41>Hund's rule

<42> s-block

<43>3

<44>increase

<45>Z*

<46>ionization energy

<47>electron affinity

<48>mass number

<49>exothermic

<50>Exclusion principle

<51>7

<52>atomic number

<53>Mordern periodic law

<54>chemical properties

<55>John Newlands

<56>De Chanourtios

<57>De Chancourtois and Dobereiner

<58>electronegativity

<59>of stability of a closed shell configuration

<60>lattice energy

<61>Greater electronegativity

<62>C_{2}H_{2}

<63>Low boiling point

<64>NaH

<65>Ionic

<66>brine

<67>Hydrogen

<68>Electronegativity

<69>Electronegativity also increases

<70>Second ionization energy

<71>Cu

<72>Rubidium

<73>Covalent radius

<74>Aluminium

<75>Zn

<76>Ionization energy

<77>Metallic radius

<78> J.J Thompson

<79>They form acidic oxide

<80>It could not hold good for elements heaver than calcium

<81>0

<82>3

<83>6

<84>HOF

<85>H2O2 ---> HO2- + H+

<86>Zn (s) | Zn2+ (aq) || Cu2+ (aq) | Cu (s)

<87>From anode to cathode: left half-cell to right half-cell

<88>Positive ions flow from the anode half-cell to the cathode half-cell

<89>Positive

<90>The oxidation

<91>-237 kJ / mol

<92>F2

<93>A unit of charge

<94>Decreases

<95>Reduced material can plate at the cathode

<96>Positive ions flow from the oxidation half-cell to the reduction half-cell

<97>CO2 + H2O ---> C6H12O6

<98>The cathode

<99>Electricity

<100>F and Li

<101>The sum of the forward and reverse rates of the reaction

<102>rate = k [A] [B] [C]

<103>M / s

<104>1 : 2

<105>Very fast reactions

<106>Quenching

<107>The time it takes for one-half of the limiting reagent to be consumed

<108>can never be proven.

<109>It is present in the balanced equation for the reaction it catalyzes

<110>The time rate of change in the concentration of products

[/ANSWERS]