S and P-Block Elements DEMO

Explanation A

Explanation C
As we go down group electropositive character increases because I.E. decreases.

Explanation A
Be belongs to second group. All other elements belong to first group, which are more reactive as compared to elements of second group members

Explanation C
The charge density of alkaline earth metals decreases down the group. Therefore the attraction of ions and water is decreased i.e. heat of hydration decreases.

Explanation C
Potassium is more electropositive than Na, so it displace Na from compounds

Explanation: C
reducing power of IIA group elements increase down the group because down the group number of inner shell increase, atomic radii increase and shielding effect increases. As a result ionization energy decreases and metallic character increases and thus reducing power of IIA group elements increases

Explanation C
BeO is acidic as well as basic

Explanation C
Top to bottom → increase while
Left to right → decrease

Explanation B
They are lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr).

Explanation A
Be is only alkaline earth metal which does not react with water even at red hot temperature because Be has least metallic character (tendency to loose electron) due to high charge density.

Explanation B
Ionization energy value decreases down the group due to increase in size.

Explanation B
Group 2A (or IIA) of the periodic table are the alkaline earth metals: beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra).
(i). They give alkalis in water.
(ii). Exist abundantly on earth crust in form of carbonates and silicates

Explanation C
The f-block elements are the lanthanides and actinides and are called the inner transition elements because of their placement in the periodic table due to their electron configurations.
In these elements, three outermost shells are not completely filled. The last electron in them enters in the (n-2) subshells.

Explanation: B
Atomic number 29 has the electric configuration –[Ar]4s¹3d¹⁰. Since the last electrons enter the d orbital, it is a d-block elements.

Explanation C
Alkali metals have only electron in outermost orbitals, so they show only one oxidation state of +1. Second ionization energy of alkali metals is very high which rules out multiple oxidation states for them.

Explanation D
Radium is an alkaline earth metal. Others belong to group I-A

Explanation: A
Potassium superoxide reacts with water as follows
2KO₂ + 2H₂O ⟶ 2KOH + H₂O₂ + O₂

Explanation: D
A = 2, 8 = 10: It is the electronic configuration of neon.

B = 2, 8, and 7 = 17: It is the configuration of the halogen family of chlorine atom which is non-metal

C = 2, 8, and 2 = 12: It is the configuration of alkaline earth metals of magnesium atom which is metal.

Therefore, A is a noble gas, B is a non-metal, and C is a metal.

Explanation D
The oxides and hydroxides of II-A are alkaline in nature and they are present in the earth’s crust.

Explanation C
Amongst the given elements, sodium is not abundantly present in earth’s crust.
Oxygen, silicon and aluminum are top three elements

Explanation A
Cs is at the bottom of I-A and has most loosely held electrons and thus very reactive substance among the alkali metals.

Explanation A
K is the most electropositive element from the given ones

Explanation A
The values of ionization energy decrease down the group. So the highest ionization energy is shown by nitrogen which is the first member of the series.

Explanation C
Li does not form superoxide while other alkali metals do form superoxide

Explanation B
Elements in the I-A and II-A subgroups are also called s block elements because their valence electrons are available in the s orbital

Explanation C
Boron (B) has five electrons and five protons

Explanation D
The ionization energy or ionization potential is the energy necessary to remove an electron from the neutral atom. It is a minimum for the alkali metals which have a single electron outside a closed shell. It generally increases across a row on the periodic maximum for the noble gases or inert gases which have closed shells.

Explanation D
They are called Alkali metals because of their property to form strong alkalies with water.

Explanation A
Energy is generally released when the first electron is absorbed by an element. This energy is called electron affinity. For the absorption of the second electron energy is generally absorbed.

Explanation D
Except number of shells all mentioned above vary along a period.

Explanation B
Fluorine is the third smallest element. Refer to the table below to observe the trends.

Explanation D
Ionization energy increases from left to right in a period. This is because moving from left to right, outer shell remains same but greater nuclear charge causes the electrons to bound more strongly to the nucleus. In the given list Oxygen is furthest right in the period two, hence, has the highest ionization energy in the given list. 

Explanation A
Atomic radius increase from top to down within a same group and decrease from left to right in a period. So the graph is for atomic radius. 

Explanation D
Electron affinity depends on all of the following factors
(i) Size of the atom
(ii) Nuclear charge
(iii) Vacancies in the outermost shell

Explanation B
Hydration energy is highly dependent on the charge to size ratio and increases with an increase in the charge to size ratio of ions.

Explanation D
More ionization results in tightly held electron difficult to remove. Therefore it results in less metallic character.

Explanation D       
Ionization energy is affected by all these factors

Explanation D
Oxides of relatively less electropositive elements such as Be, Al, Bi and Zn are amphoteric in nature.

Explanation A
Screening effect decreases proceeding from s-orbital to f-orbital

Explanation A
Melting point decreases with the strength of metallic bonding decreases with increasing size of atom.

Explanation: A

Explanation D
Small size, low electro positivity and high charge density of cation

Explanation C
I.E ∝ (1/size) ∝ atomic number (atomic number of IIA is greater than IA while atomic size of IA is greater than IIA)

Explanation D
Ne is a noble gas and does not allow burning.

Explanation B
Due to very high 2^nd I.E Na will not lose 2^nd electron in any reaction hence +2 O.S is ruled out.

Explanation: B

Explanation C
Melting and boiling point increase upto IV-A group due to increase the number of binding electrons in the outermost shell.

Explanation A
Both ionization energy and electron affinity increase from left to right so ionization energy and electron affinity of group IA has minimum value.

Explanation C
Ionization energy ∝ nuclear charge ∝ nuclear pull on electrons.
Ionization energy ∝ (1/ Atomic size)
Order of ionization energy: s > p > d > f

Explanation D
Noble means least interacting species.

Explanation: D

Explanation: D
Na metal is very reactive so it is stored in non-polar solvent like hexane, benzene and kerosene. Ethanol is a polar solvent.

Explanation: B
IIA group hydroxides are generally hygroscopic but caustic soda (NaOH) is highly deliquescent

Explanation: B
₁₁Na = 1s²2s²2p⁶3s¹
₁₀Ne =1s²2s²2p⁶

Explanation: A
Spodumene is LiAl(SiO₃)₂(Lithium aluminium silicate)

Explanation: D
Cs has lowest ionization energy value due to its large size

Explanation: A
Milk of magnesia is basic in nature which neutralizes acidity.

Explanation: D
Cation always smaller than neutral atom and anion is always larger than neutral atom.

Explanation: B
Hydration energy α charge / size.

Explanation: B
Electrical conductance increases from IA to IIIA.

Explanation: A
Solubility of G-IA increases down the group due to decrease in lattice energy.

Explanation: A
Alkali metals are the most reactive metals in periodic table

Explanation: A
BeO is amphoteric oxide and shows basic as well as acidic properties.

Explanation: C
In the second period, the 2s sublevel, with two electrons, and the 2p sublevel with six electrons, are being filled. Consequently, the second period contains eight elements.

Explanation: C
Li combines with nitrogen and carbon to form Lithium nitride (Li₃N) and lithium carbide (Li₄C). 

Explanation: B
Cs is the most electropositive element in the periodic table. It belongs to the first group and sixth period in the periodic table. It can easily donate its one valence electron to attain noble gas configuration.

Explanation: D

Explanation: A

Explanation: A

Explanation: D
Alkali metals are good reducing agents as they have low value of ionization energy that decrease as we move down the group. Alkali metals are good reducing agents as they readily lose their electrons due to low ionization enthalpy.

Explanation: D
Reduction power is when a substance can easily donate electron, for halogens
Oxidizing power : F₂ > Cl₂ > Br₂ > I₂
Reducing power : I^– > Br^– > Cl^– > F^–

Explanation: A
Penetration effect of s orbital is greatest so electron is nearest to nucleus. Order is s > p > d > f

Explanation: D
f – orbital is least penetrating so its screening is least.

Explanation: B
Both nuclear charge and effective charge increase along the period but decrease in size is due to effective nuclear charge, screening remains constant along the period.
Z_off = z – screening

Explanation: B
Dobereiner → Law of triads
Newland → Law of octaves
Moseley → Arranged in ↑ order of atomic numbers
Mendeleev → groups and periods, arranged according to ↑ atomic number

Explanation: C
I.E:- ↑ along period, ↓ down the group
Trend along period: GI < GII > GIII < GIV < GV > GVI < GVII < GVIII

Explanation: C
Second E.A is usually endothermic, for O^– + e^– → O^2–.
E.A = +780 kJ/mol

Explanation: D
As anions are always larger in size than their parent atom and cations are always smaller in size than their parent atom.

Explanation: B
As down the group ionization energy decreases.

Explanation: B
Reference Text book.
Yes, sometimes Examiners copy/paste information directly from book

Explanation: A
Reactivity increases down the group.

Explanation: D

Explanation: C
The  second electron affinity of oxygen is 780kJ/mol.
The second electron affinity of oxygen is particularly high because the electron is being forced into a small, very electron-dense space

Explanation: A
In excess alkane, monosubstituted product is favored.
In limited alkane, tetrasubstituted product is favored.

Explanation: C
In IIA group, ionization energy decreases down the group due to
(i) Increase in atomic size
(ii) Decrease in effective nuclear charge

Explanation: D
In heterocyclic compounds, the heteroatom might be O, N or S.

Explanation: B
E.N increases along the period and maximum for ns² np⁵ while minimum for ns² np².

Explanation: C
Iodine can form upto 7 bonds due to hyper valance as in IF₇.

Explanation: D
Iodine has smallest is orbital in all due to greatest nuclear charge on it. So its contribution in screening is maximum.

Explanation: B
Metals for down the group have ↓ polarizing power and non-metals above in the group have ↓ polarizability. Such elements are most favourable for the formation of ionic bond.

Explanation: C
Removal of electron from Li is difficult as compared to Na & K but due to its higher hydration energy & resulting stability, it less above both in electrochemical series.

Explanation: C
Mg has 2e^– in its valance shell, removal of 3^rd e^– is very difficult so it is observed in +2 oxidation state only.

Explanation:   B
As down the group ionization energy decreases.

Explanation: D
As anions are always larger in size than their parent atom and cations are always smaller in size than their parent atom.

Explanation B
Reference Text book
Page#36

Explanation C
Reference Text Book
page#7

Explanation:   A
Both have zero electron affinity

Explanation:   A
CaO-basic, CO₂ and SiO₂-acidic, SnO₂-amphoteric, as it reacts both with acids and bases.
SnO₂+4HClèSnCl₄+2H₂O
SnO₂+2NaOHèNa₂SnO₃+H₂O

Explanation:   D

Explanation B
Reference Text book
page# 8

Explanation C
Reference Text Book
page# 9

Explanation D
Hydrogen is a unique element in the periodic table and resembles the properties of group IA, IVA or VIIA.

Explanation B
O and S belong to the same group

Explanation B
B is not true. Negative ions are larger in size as compared to the parent atom because repulsion between the electrons cause expansion of the shell.
All other statements are correct.

Explanation B
Reference Text book.
Yes, sometimes Examiners copy/paste information directly from book

Explanation:  A
F and O belong to 2^nd period whereas Cl and Br belong to 3^rd and 4^th periods respectively. Hence the sequence of the E.N is F> O> CI> Br

Explanation:  A
First period has H and He only out of which He is inert, hence, H behaves as a highly electropositive as well as electronegative.

Explanation:  D
Melting point of alkali metals decreases with increases in size.

Explanation C
Hint: The lower elements of group III-A, IV-A and V-A form amphoteric oxides

Explanation C
Hint: Elements with more than one electron in the outer shell have more than one value of ionization energy.

Explanation: C
The electronic configuration [Xe] 6S¹ is the configuration of Cs which is highly electropositive element of alkali metal family. It has lowest I.P. in its family.

Explanation B 
All the species given in the question are isoelectronic. The size of such species is inversely related to atomic number. Hence, the decreasing order of size is: –
₁₆S^2- > ₁₇Cl^– > ₁₉K⁺ > ₂₀Ca²⁺

Explanation D
Iodine has the lowest value of ionization potential. Due to this it has some tendency to lose electron. Hence, it is most basic in nature.

Explanation:  A
Generally the halides of lower oxidation state are ionic and those of higher oxidation state tend to be covalent *PbCl₂ is ionic * PbCl₄ is covalent

Explanation C
Every eighth element is in the same group. So 7th and (7+8 =15) 15th element would be in the same group and have similar properties.

Explanation D
Because of large size, electron is more loosely bonded.
Hence it is most reactive in alkali metals

Explanation A.
HClO < HCl  < HCl  <HCl  
As the oxidation number of Cl (or halogen) increases, acidity increases 

Explanation D
Hint: Ionization energy increases from left to right in a period. This is because moving from left to right, outer shell remains same but greater nuclear charge causes the electrons to bound more strongly to the nucleus. In the given list Oxygen is furthest right in the period two, hence, has the highest ionization energy in the given list. 

Explanation D
Important Hit, favorite question of ETEA:
Oxides of relatively less electropositive elements such as Be, Al, Bi and Zn are amphoteric in nature.

Explanation D
Basic character of oxides decrease within a period from left to right. All the given elements are in the period 2 and Na is the left most element of period 2.

Explanation D
Electron affinity decrease from lighter to heavier elements within a group. So Iodine has smallest electron affinity.

Explanation D
Acidity increases with increasing oxidation state. As Mn₂O₇ has the highest oxidation state, it is most acidic in nature.

Explanation B
In periodic table on going across a period, the metallic character decreases with increase in atomic number because size of atom decreases and attraction for e is greater on right side of periodic table, while in group down the metallic character increases

Exaptation D
P has five valence electrons.Three are shared with three Cl atoms and so total electrons in the valence shell of P in PCl₃ are 8.

Explanation A
Hint: Cation is smaller in size than parent neutral atom

Explanation B
Li(z=3) is the lightest metal in the periodic table, while hydrogen(z=1) and He(z=2) are gases.

Explanation: A
Ionization energy decreases down the group from N to Bi as
N>P>As>Sb>Bi

Explanation: C
1^st ionization energy of
            Li = 5.4 eV
Electron affinity of
          Cl = 3.61 eV
Hence, ΔH = I.E – E.A.
                    = 5.4 – 3.61
                    ≈ 1.8 eV
As we know that
             1 eV =  1.6 x 10^-19 J
or 1.6 x 10^-22 kJ
1.8 x 1.6 x 10^-22 = 2.86 x 10^-22 kJ
(Hint you can asume 1.6 as 1.5 to speed up the calculation time)