Studied by 41 people
The elements in which last electron enters into _________ are known as p-block elements.
p-subshell
The general electronic configuration of p-block elements is __________. There are six groups in p-block.
ns²np^1-6
Atomic radii order for group 13 is_____________ (ascending order)
B<Ga<Al< In = Tl
Atomic radius of Ga is less than that of Al because of ___________ of 3d subshell in Ga.
Poor shielding of electron
Ionization energy order for group 13 is ________________ (descending)
B>Tl>Ga>Al>In
Electronegativity order for group 13 is _____________
Al < Ga < In < T l< B
Down the group E.N first decreases from B to Al and then increases marginally because of the differences in _________ of the elements.
Atomic Size
____________ is the element of group 13 which is not a metal.
Boron
The relative stability of +1 oxidation state progressively increases for heavier elements in group 13. The order is (ascending) _______________
Al < Ga < In< Tl
In thallium _______ Oxidation state is predominant whereas the +3 oxidation state is highly oxidizing in character.
+1
The compounds in +1 oxidation state, are more ionic than those in ____________ oxidation state.
+3
Density of the elements ___________ down the group from boron to thallium.
Increases
Melting point ___________ up to Ga and then _________ up to Tl.
Decreases, Increases
Thallium show different oxidation states, The reason is ____________
Inert pair effect
Elements of Group 13 react with halogens to form tri-halides except______________
Thallium
Boron chloride, unlike other chlorides of the group do not dimerize and due to ____________ nature, can form adduct with ammonia.
Lewis Acid
Boron trioxide is acidic and reacts with basic(metallic) oxides forming _____________
Metal Borates
Aluminum and gallium oxides are _____________ and those of indium and thallium are basic in their properties
amphoteric
__________ is second most abundant element in the earth’s crust.
Silicon
General electronic configuration for group 14 elements are ___________.
ns²np²
Atomic radii order for group 14 is _______________(ascending)
C < Si < Ge < Sn < Pb
Ionization energy order (descending) for group 14 is ______________
C > Si > Ge > Pb > Sn
The first ionization enthalpy of group 14 members is _______________ than the corresponding members of group 13.
higher
Electronegativity order for group 14 is _______________(descending)
C > Pb > Si = Ge = Sn
The electronegativity values for elements from Si to Pb are ________.
Almost the same
Compounds in +4 oxidation state are generally ________ in nature.
Covalent
In heavier members the tendency to show +2 oxidation state increases in the sequence: Ge < Sn < Pb, due to ______________
Inert pair effect
Lead compounds in +2 state are _____ and in +4 state are strong _______ agents.
stable, oxidizing
Germanium forms stable compounds in ________ state and only few compounds in +2 state.
+4
Carbon cannot exceed its covalence more than ___________
Four
Metallic character _______ down the group and non-metallic character ___________ down the group.
Increases, Decreases
Tin and Lead are ___________ metals with _________ melting points.
soft, low
Melting point ________ up to Sn and then slightly __________
Decreases, Increases
Oxides in higher oxidation states of elements are generally more ______________ than those in lower oxidation states.
Acidic
SnO2 and PbO2 are ______________ in nature.
amphoteric
Tin react with stream to form dioxide and __________ gas.
hydrogen
Lead is unaffected by water, probably because of a ___________ formation.
protective oxide film
Most of the MX4 are ________________ in nature except SnF4 and PbF4.
covalent
Carbon differs from rest of the members of its group due to its _______________ , higher electronegativity, higher ionization enthalpy and unavailability of _____________ orbitals
Atomic size, d
In group 14, Down the group the size increases and electronegativity decreases, and , thereby, tendency to show catenation __________.
Decreases
The order of catenation in group 14 is ____________.
C > > Si > Ge = Sn
___________ allotrope of carbon has layered structure.
Graphite
Carbon Monoxide is ____________ and odorless gas.
Neutral
In graphite and diamond, the percentage of p-characters of the hybrid orbitals in hybridization are ______ and ______.
67% and 75%
___________ is a greenhouse gas is present in very high quantities.
CO2
Electronic configuration of group 15 is __________. Extra stable electronic configuration due to ___________.
ns²np³, half- filled p-orbital
Arsenic, Antimony, and ____________ are found mainly as sulphides.
Bismuth
In group 15, ionization enthalpy __________ due to gradual increase in ____________.
Decreases, atomic size
The IE of the group 15 is _________ than group 14 due to extra stable _____________.
more, half-filled p orbitals
In group 15, all the elements have allotropes except _____________.
Nitrogen
The boiling points __________ from top to bottom.
increases
Metallic character _________ down the group.
Increases
All group 15 elements form hydrides of formula MH3 which is _______________ in shape.
Trigonal Pyramidal
In group 15, thermal stability __________ down the group because of _____________ in size of the element which results in weaker bonds.
Decreases, Increase
In group 15, Reducing property _________ down the group because the bond strength __________ as the bond lengths ____________ down the group.
Increases, Decrease, Increase
In group 15 the boiling point order is __________________ (ascending order).
PH3 < AsH3 < NH3 < SbH3 < BiH3
In group 15 the melting point order is _________________ (Descending order)
NH3 > SbH3 > AsH3 > PH3
In group 15 the Basic character order is _____________ (Descending order).
NH3 > PH3 > AsH3 > SbH3 >= BiH3
Bismuth does not form ____________ due to ____________ rest all M2O5 are ___________ in nature.
Bi2O5, Inert pair effect, acidic
The oxide in the higher Oxidation state of the element is more ___________ than that of lower O.S.
Acidic
Nitrogen does not form ____________ due to non-availability of the d-orbitals in valence shell.
pentahalide
In group 15, the increasing order of enthalpy of vaporization is ______________.
PH3 > AsH3 > NH3
Sb4O6 oxides is ___________ in nature.
Amphoteric
Nitrogen has the unique ability to form __________ multiple bonds with itself and with other elements having _____ size and _____________ electronegativity.
pπ-pπ, small, high
P, As, and Sb form ______ bond while bismuth forms metallic bonds in elemental state.
single
The single N-N bond is _______ than the single P-P bond because of ___________ inter-electronic repulsion of the non-bonding electrons.
weaker, high
Phosphorous and arsenic act as _______ and can also form bonds with transition metals in their compounds like P(C2H5)3 and As(C6H5)3.
Ligand, dπ-dπ
Phosphorus has large diffused atomic orbitals thus they cannot have effective ___________ overlapping.
pπ-pπ
In group 16, electron gain enthalpy order is ____________ .
S > Se > Te > Po > O
____________ has the second largest electronegativity value amongst the elements.
Oxygen
Oxygen exists as a ________ molecule whereas sulphur exists as ______________ molecule.
Diatomic, polyatomic
Catenation property is maximum in group - 16 for __________ .
Sulphur
O shows ________ oxidation state in the case of OF2.
+2
H2O has ________ bonding whereas H2S does not.
Hydrogen
In group 16, the oxides melting and boiling point order is __________ (Descending order).
H2O > H2Te > H2Se > H2S
_____________ is the correct reducing nature order(Ascending) for EO2 (E = S, Se, Te).
TeO2 < SeO2 < SO2
The order(descending) of stability of halides of sulphur with different halogens is _____________.
F- > Cl - > Br- > I -
The halogens are highly reactive ___________ elements.
Non - metallic
Chile Salt petre contains up to 0.2% of _____________ .
Sodium iodate
The atomic radius of F is extremely __________ .
small
___________ is the most electronegative element in the periodic table.
Fluorine
Electron gain enthalpy with negative sign of F is less than that of Cl due to _____________ .
Small size of F atom
All halogens are ________ due to the absorption of light on promoting an electron from the ground state to a higher state.
Colored
The bond energy in the X2 molecules is ____________ .
Cl2 > Br2 > F2 > I2
F can show _________ state only because it does not have valence d-electrons.
-1
In group 17, the boiling point and density order is ___________ .
F2 < Cl2 < Br2 < I2
The non -metal that does not exhibit positive oxidation state is _______.
F
All the halogens are highly ___________ , reactivity ____________ down the group.
reactive, decreases
In group 17, thermal stability of hydride order is _____________ (descending).
HF > HCL > HBr > HI
In group 17, acidic strength of hydride order is ___________ (ascending) .
HF < HCl < Hbr < HI
In group 17, melting point of hydride order(Descending) is _______________ .
HI > HF > HBr > HCl
In group 17, Boiling point of hydride order is ____________ .
HF > HI > HBr > HCl
_____________ displaces Br2 from an aqueous solution containing bromide ions.
Chlorine
In
HF has highest boiling point among hydrogen halides because it has ____________ .
H bond
In group 18, Ionization energy ________ down the group with ___________ in atomic size.
decreases, increases
In group 18, Density, melting point and boiling points ___________ down the group.
Increases
All noble gases have general electronic configuration _______________ except helium which has 1s².
ns²np^6
____________________ intermolecular force is most responsible in allowing Xe gas to liquefy.
Instantaneous dipole- induced dipole
_____________ noble gas is not found in atmosphere.
Rn and Og
