NEET Chemistry Study Of Representative Elements Revision Notes

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Revision Notes for Full Course Study of Representative Elements Study Of Representative Elements

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Study Of Representative Elements Notes Full Course Study of Representative Elements

 

Study of Representative
Elements (spdf blocks)
 
Revision Notes on s-Block Elements:
 
Alkali Metals (Group I elements of modern periodic table):
 
NEET Chemistry Study of Representative Elements Revision Notes
 
*ppm (parts per million)
** percentage by weight
 
Physical Properties of Alkali Metals:
 
• These are soft in nature and can be cut with the help of knife except the lithium.
• The atoms of alkali metals have the largest size in their respective periods.
•  The first ionization energy of the alkali metals are the lowest as compared to the elements in the other group.
•  The alkali metals show +1 oxidation state.
•  The alkali metals have low values of reduction potential (as shown in table-I) and therefore have a strong tendency to lose electrons and act as good reducing agents.
•  The melting and boiling points of alkali metals are very low because the intermetallic bonds in them are quite weak.
•  ll the alkali metals form ionic (electrovalent) compounds.
•  The alkali metals are good conductors of heat and electricity.
•  Alkali metals (except Li) exhibit photoelectric effect
•  The alkali metals and their salts impart a characteristic colour to flame
 
NEET Chemistry Study of Representative Elements Revision Notes-1
 
Hydroxides of Alkali Metals:
 
a) All the alkali metals, their oxides, peroxides and superoxides readily dissolve in water to produce corresponding hydroxides which are strong alkalies.
 
 2Na + 2H2O → 2NaOH + H2
 Na2O + 2H2O 2NaOH
 Na2O2 + 2H2O → 2NaOH + H2O2
 2KO2 + 2H2O → 2KOH + H2O2 + O2
 
b) The basic strength of these hydroxides increases as we move down the group Li to Cs.
c) All these hydroxides are highly soluble in water and thermally stable except lithium hydroxide.
d) Alkali metals hydroxides being strongly basic react with all acids forming salts.
 
 NaOH + HCI → NacI + H2O
 2NaOH + H2 SO4 → Na2SO4 + 2H2O
 
Halides of Alkali metals:
M2O + 2HX → 2MX + H2O
MOH + HX → MX + H2O
M2CO3 + 2HX → 2MX + CO2 + H2O (M = Li, Na, K, Rb or Cs)
(X = F, Cl, Br or I)
 
a) Standard enthalpies of formation in (kJ/mol-1)
 
NEET-Chemistry-Study-of-Representative-Elements-Revision-Notes 1
 
b) Covalent Character:
 Small cation and large anion favors covalency.
 Order: LiCl > NaCl > KCl > RbCl > CsCl & . LiI > LiBr > LiCl > LiF
 Greater the charge on the cation greater is its polarizing power and hence larger is the covalent character: Na+CI- < Mg+2CI2 < AI+3 CI3
 Greater the charge on the anion, more easily it gets polarized thereby imparting more covalent character to the compound formed eg covalent character increase in the order.
NaCI < Na2SO4 < Na3PO4
 
c) Lattice Energies: Amount of energy required to separate one mole of solid ionic compound into its gaseous ions.Greater the lattice energy, higher is the melting point of the alkali metals halide and lower is its solubility in water
 
d) Hydration Energy: Amount of energy released when one mole of gaseous ions combine with water to form hydrated ions.
 M+ (g) + aq → M+ (aq) + hydration energy
 X- (g) + aq → X- (aq) + hydration energy
Higher the hydration energy of the ions greater is the solubility of the compound in water.
 
The solubility of the most of alkali metal halides except those of fluorides decreases on descending the group since the decrease in hydration energy is more than the corresponding decrease in the lattice energy.
 
Due to high hydration energy of Li+ ion, Lithium halides are soluble in water except LiF which is sparingly soluble due to its high lattice energy.
 
For the same alkali metal the melting point decreases in the order
fluoride > chloride > bromide > iodide
For the same halide ion, the melting point of lithium halides are lower than those of the corresponding sodium halides and thereafter they decrease as we move down the group from Na to Cs.
The low melting point of LiCl (887 K) as compared to NaCl is probably because LiCl is covalent in nature and NaCl is ionic.
 
Anomalous Behavior of Lithium and diagonal relationship with Magnesium:
Li has anomalous properties due to
 
• Very small size
 High polarizing Power
 
Lithium show diagonal relationship with magnesium because both elements have almost same polarizing power.
 The melting point and boiling point of lithium are comparatively high.
 
 Lithium is much harder than the other alkali metals. Magnesium is also hard metal.
 
 Lithium reacts with oxygen least readily to form normal oxide whereas other alkali metals form peroxides and superoxides.
 
 LiOH like Mg (OH)2 is weak base. Hydroxides of other alkali metals are strong bases.
 
 Due to their appreciable covalent nature, the halides and alkyls of lithum and magnesium are soluble in organic solvents.
 
 Unlike elements of group 1 but like magnesium. Lithium forms nitride with nitrogen.6Li + N2 → 2Li3N
 
 LiCl is deliquescent and crystallizes as a hydrate, LiCI2H2O. Other alkali metals do not form hydrates. also forms hydrate, MgCI2.8H2O .
 
 Unlike other alkali metals lithium reacts directly with carbon to form an ionic carbide.Magnesium also forms a similar carbide.
 

Question. Which of the following properties of red P and white P are related to their structure?
a. Large difference in m.p.
b. Difference in hardness
c. Ignition behavior
d. None of these
Answer : A, B, C

Question. Electrolysis of KH produces H2 :
a. at the cathode
b. at the anode
c. either at the cathode or at the anode
d. Cannot be predicted
Answer : A, B

Question. In which of the following cases, does N2 evolve as agaseous product?
a. KNO3 reacts with K on heating
b. Na2O2 reacts with NH3
c. NH3 reacts with bleaching powder
d. None of these
Answer : A, B, C

Question. Which of the following form dimeric halides
a. Al
b. Mg
c. In
d. Ga
Answer : A, C, D

Question. Which of the following processes cannot give Cl2 gas as aproduct?
a. Electrolysis of aq. NaCl
b. Oxidation of conc. HCl by K2CrO4
c. Electrolysis of very dilute aq. NaCl
d. Oxidation of conc. HCl by MnO2
Answer : A, B, C

Question. The temporary hardness of water is caused by which of the following compound(s):
a. CaCl2
b. Mg(HCO3)2
c. Ca(HCO3)2
d. MgSO4
Answer : B, C

Question. Which of the following statements are correct regardingthe diagonal relationship between Al and Be?
a. BeO and Al2O3 are amphoteric in nature
b. Carbides of both produce the same gas on hydrolysis
c. Both can form complexes.
d. Hydrides of both the elements are covalent in nature
Answer : A, B, C

Question. Which of the following statements are correct?
a. NO is a diamagnetic liquid
b. B2 and C2 are diamagnetic
c. N2O4 is diamagnetic
d. BH3 loses its planarity on dimerization
Answer : A, C

Question. Phosphine is obtained from the following ore
a. Calcium superphosphite
b. Calcium phosphide
c. Potassium phosphide
d. Calcium hypophosphide
Answer : B, C

Question. Which statement is false
a. Electronegativity of fluorine is maximum
b. Electron affinity of fluorine is maximum
c. Melting point of fluorine is minimum
d. Boiling point of fluorine is maximum
Answer : B, D

Question. White phosphorus (P4) has
a. Six P - P single bonds
b. Four P - P single bonds
c. Four lone pairs of electrons
d. PPP angle of 60°
Answer : A, D

Question. Among the members of V A group (N, P, As, Sb and Bi), which of the following properties shows an increase as we go down from nitrogen to bismuth:
a. Stability of +3 oxidation state
b. Reducing character of hydrides
c. Electronegativity
d. Acidic nature of the pentoxide
Answer : A, B

Question. SO2 is obtained when
a. Oxygen reacts with dilute sulphuric acid
b. Hydrolysis of dilute H2SO4
c. Concentrated H2SO4 reacts with Na2SO3
d. All of these
Answer : B, C

Question. When NaOHis prepared, the gas released is:
a. Cl2
b. H2
c. O2
d. H2O
Answer : A, B

Question. Ammonia on reaction with hypochlorite anion, can form:
a. NO
b. NH4Cl
c. N2H4
d. HNO2
Answer : B,C

Assertion and Reason

Note: Read the Assertion (A) and Reason (R) carefully to mark the correct option out of the options given below:
a. If both assertion and reason are true and the reason is the correct explanation of the assertion.
b. If both assertion and reason are true but reason is not the correct explanation of the assertion.
c. If assertion is true but reason is false.
d. If the assertion and reason both are false.
e. If assertion is false but reason is true.

Question. Assertion: HF, NH3 and H2O form intermolecular hydrogen bonding.
Reason: HF, NH3 and H2O molecules are bonded in same manner.

Answer : C

Question. Assertion: SeCl4, does not have a tetrahedral structure.
Reason: Se in SeCl4 has two lone pairs.

Answer : C

Question. Assertion: H2O2 is stored in wax-lined glass.
Reason: Presence of metal surfaces, traces of alkali (present in glass) etc. increases its decomposition.

Answer : A

Question. Assertion: Reaction of SO2 and H2S in the presence of Fe2O3 catalyst gives elemental sulphur.
Reason: SO2 is a reducing agent.

Answer : B

Question. Assertion: Calgon is used for removing Ca2+ and Mg2+ ions from hard water.
Reason: Calgon forms precipitate with Ca2+ and Mg2+ ions.

Answer : D

Question. Assertion: A nearly tetrahedral arrangement of the orbitals about the oxygen atom allows each water molecule to form hydrogen bonds with as many as four neighbouring water molecules.
Reason: In ice each water molecule form four hydrogen bond as each molecule is fixed in the space.

Answer : A

Question. Assertion: Hard water does not lather with soap.
Reason: In hard water, the sodium stearate of soap changes to the corresponding calcium magnesium salt which precipitates out.

Answer : A

Question. Assertion: Borax bead test is not suitable for Al(III).
Reason: Al2O3 is insoluble in water.

Answer : B

Question. Assertion: Ozone is a powerful oxidizing agent in comparison to O2.
Reason: Ozone is diamagnetic but O2 is paramagnetic.

Answer : B

Question. Assertion: Halogens do not occur in free-state.
Reason: Halogens are highly reactive.

Answer : A

Question. Assertion: The fluorine has lower reactivity.
Reason: F – F bond has low bond dissociation energy.

Answer : C

Question. Assertion: SiF62− is known but SiCl62− is not.
Reason: Size of fluorine is small and its lone pair of electrons interacts with d-orbitals of Si strongly.

Answer : A

Question. Assertion: Potassium and caesium are used in photoelectric cells.
Reason: Potassium and caesium emit electrons on exposure to light.

Answer : A

Question. Assertion: Lithium forms Lithium oxide (LIO2).
Reason: N2 molecule have unpaired electrons.

Answer : A

Question. Assertion: Liquid NH3 is used for refrigeration.
Reason: Liquid NH3 quickly vaporises.

Answer : A

Comprehension Based

Paragraph –I

s-block elements having ns–1 (alkali metals) or ns2 (alkaline earth metals) include Li, Na, K, Rb, Cs, Fr and Be, Mg, Ca, Sr, Ba, Ra respectively. These metals are soluble in NHand their ammonia solution is strongly conducting, paramagnetic as well as show colour. All of these are reactive metals due to low values of ionization energy. The physical properties of alkali metals almost describe a regular trend form Li to Cs whereas no such trend is noticed in alkaline earth metals. Also the properties such as density m.pt, b.pt for alkaline earth metals are more than alkali metals. Li in alkali metals and Be in alkaline earth metals differ markedly in many of their properties with their respective group elements.

Question. The conductivity of alkali metals in liq. NH3 at –33ºC:
a. Increases with increase in temperature
b. Decrease with increase in temperature
c. Remains same with increase or decrease in temperature
d. Due to ions furnished by metals
Answer : B

Question. Which set of statements are correct?
(I) ΔHhyd for Sr2+ > ΔHhyd for Ag+
(II) Ca(OH2)is less soluble in water than Ba(OH2)
(III) Ba2+ is more powerful reducing agent than Ca2+ in acidic solution
(IV) Ca2+ is more powerful reducing agent in alkaline medium
a. I, II, III, IV
b. I, II
c. I, III, IV
d. II, IV
Answer : C

Question. Select the wrong statement:
a. Hydration energy: Mg2+ Mg Na+
b. λ released during flame colour: Li > Na > K > Rb > Cs
c. Conducting power in solution: Cs+ > Rb> K+ Na+ Li+
d. Density: Be > Mg > Ca > Sr > Ba > Ra
Answer : D

Paragraph –II

Group 14 of periodic table includes C, Si, Se Te and Po. Carbon forms two oxides CO (neutral) and CO(acidic) whereas other members of group 14 forms amphoteric oxides. Both CO and CO2 are covalent compounds. Si does not form monoxide.

Question. CO although neutral acts as acid as well as π-electron acceptor in the reactions respectively:

""NEET-Chemistry-Study-Of-Representative-Elements-Revision-Notes
a. I, II
b. II, III
c. III, II
c. I, IV
Answer : A 

Question. Which statement is not correct?
a. The CO2 molecule possesses sp-hybridization and also shows resonating structure
b. The structure of CO is [:C =C:]
c. Ammoniacal CuCl absorbs CO forms adduct product
d. Asphyxia is law level poisoning produced in a atmosphere of CO2
Answer : D

Question. Which statement is not correct?
a. CO is isoelectronic with N2 but less reactive than N2
b. CO is isoelectronic with N2 and possesses more bond energy
c. CO is isoelectronic with N2 and more reactive than N2
d. CO is isoelectronic with N2 and required for respiration
Answer : A

Paragraph –III

Group 15 includes pnicogens i.e., N, P, As, Sb and Bi elements with ns2np3 configuration. Nis gas. All these elements except Bi show allotropy. Phosphorus exists in three allotropic forms, white phosphorus, red phosphorus and black phosphorus. The later being most stable (thermodynamically) form of P. Each member of this forms hydrides of the molecular formula MH3 .Nitrogen however forms three hydrides NH3, N3H and N2H4. The thermal stability, basic nature and solubility in water of hydrides (MH3) however decreases form N to Bi.

Question. The correct order for acidic nature is:
a. NH+4 < PH+4 < AsH +4
b. NH+4 > PH+4 > AsH+4
c. AsH+4 > NH+4 > PH+4
d. AsH+4 < NH+4 < PH+4
Answer : A

Question. Which hydride of group 15 is most powerful reducing agent?
a. NH3
b. PH3
c. AsH3
d. SbH3
Answer : D

Question. The correct order of bond angles is:
a. NH3 > PN3 > AsH3 >SbH3
b. SbH3 > AsH3 >PN3 > NH3
c. SbH3 > PN3 > AsH3 >NH3
d. PN3 > NH3 > SbH3 > BiH3
Answer : A

Paragraph –IV

There are some deposits of nitrates and phosphates in earth’s crust. Nitrates are more soluble in water. Nitrates are difficult to reduce under the laboratory conditions but microbes do it easily. Ammonia forms larger number of complexes with transition metal ions. Hybridization easily explains the ease of sigma donation capability of NH3 and PH3. Phosphine is a flammable gas and is prepared form white phosphorus.

Question. Among the following, the correct statement is:
a. Phosphates have no biological significance in humans
b. between nitrates and phosphates, phosphates are less abundant in earth’s crust
c. Between nitrates and phosphates, nitrates are less abundant in earth’s crust
d. Oxidation of nitrates is possible in soil
Answer : C

Question. Among the following, the correct statement is:
a. Between NH3 and PH3,NH3 is a better electron donor because the lone pair of electrons occupies spherical ‘s’ orbital and is less directional
b. Between NH3 and PH3,NH3 is a better electron donor because the lone pair of electrons occupies sp3- orbital and is more directional
c. Between NH3 and PH3,NH3 is a better electron donor because the lone pair of electrons occupies sp3- orbital and is more directional
d. Between NH3 and PH3,NH3 is a better electron donor because the lone pair of electrons occupies spherical ‘s’ orbital and is less directional
Answer : C

Question. White phosphorus on reaction with NaOH gives PH3 as one of the products. This is a:
a. dimerization reaction
b. disproportionation reaction
c. condensation reaction
d. precipitation reaction
Answer : B

Match the Column

Question. Match the chemical properties with the compounds:

Column IColumn II
(A) Ca1. Produces Hon reaction with H2O.
(B) CaH22. Produce Ca(OH)2 on reaction with H2O
(C) CaO3. The compound is ionic.
(D) CaC24. Can absorb N2 under hot conditions

a. A→1,4; B→1,2,3; C→2,3; D→2,3,
b. A→1,3,4; B→1,2,4; C→2,3; D→2,3,4
c. A→1,2,4; B→1,3; C→2,3; D→2,3,4
d. A→1,2,4; B→1,2,3; C→2,3; D→2,3,4
Answer : D

Question. Match the compounds with their uses / properties:

Column IColumn II
(A) NaCO3 ⋅10H2O1. Desiccating agent
(B) CaCl2(anhydride)2. Used for preparing freezing mixture
(C) CaSO4(anhydride)3. Washing soda
(D) NaCl4. Dead burnt.
 5. Soluble in water.

a. A→1,5; B→1,4; C→4; D→2,5
b. A→3,5; B→1,5; C→4; D→2,3
c. A→3,5; B→1,5; C→4; D→2,5
d. A→3,5; B→3,5; C→4; D→1,5
Answer : C

Question. Match the xenon compounds with their properties.

Column IColumn II
(A) XeO64-1. Central atom in sp3dhybridized
(B) XeF42. On treatment with conc. H2SO4 produces XeO4.
(C) XeO33. Only one lone pair is present on the central atom
(D) XeO2F44. Central atom of the molecule has four surrounding atoms

a. A→1,3; B→1,2; C→3; D→3,4
b. A→1,3; B→2,4; C→3; D→3,4
c. A→1,2; B→1,4; C→3; D→3,4
d. A→1,2; B→1,4; C→1; D→1,4
Answer : C

Integer

Question. Among the following elements, the number of elements that release H2 on reaction with NaOH is …………… Be, Al, B, Mg, Ca, Zn, Sn
Answer : 5

Question. The Among the following compounds, the number of compounds which do not produce acidic or basic solutions which do not produce acidic or basic solutions when dissolved in water is ……………? NaCl2, BeCl2 , Li2 O,MgO,CaH2, CaSO4
Answer : 3

Question. The number of bicarbonates that do not exist in solid form among the following is ……………
LiHCO3, NaHCO3, Ca(HCO3)2 ,KHCO3, NH4HCO3, Ba(HCO3)2, Mg(HCO3)2

Answer : 4

Question. The ratio of the number of water of crystallization in gypsum and that in plaster of Paris is ……………
Answer : 4

Question. The number of planes of symmetry in [BeH4]2– is ……………
Answer : 6

 
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