P-block and periodic properties

The elements in which last electron enters into _________ are known as p-block elements.

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