S and P Test 1

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MCQs 1:

Which property of Group IIA elements diminishes as you proceed down the group?





Topic: Trends in Group IIA Elements

Correct Answer: C) Ionization energy

Detailed Hint:
  • The properties of elements in group IIA exhibit certain patterns or trends as we move down the group.
  • One of these trends is the reduction of ionization energy. Ionization energy refers to the amount of energy required to remove an electron from an atom or ion.
  • As we proceed down Group IIA, the ionization energy decreases. This is attributed to an increase in atomic size and a decrease in effective nuclear charge, which makes it easier to remove an electron.
  • Therefore, the correct answer is C, "Ionization energy," which decreases down the group.

MCQs 2:

What is the nature of beryllium oxides?





Topic: Nature of Beryllium Oxides

Correct Answer: C) Amphoteric

Detailed Hint:
  • Beryllium forms oxides that have both acidic and basic properties.
  • This dual behavior of being able to react as both an acid and a base is known as amphotericity.
  • Hence, BeO is neither purely acidic nor purely basic, but amphoteric in nature.
  • Therefore, the correct answer is C, "Amphoteric."

MCQs 3:

What would be the second electron affinity of oxygen if its first electron affinity is -141 kJ/mol?





Topic: Electron Affinity of Oxygen

Correct Answer: C) +780 kJ/mol

Detailed Hint:
  • Electron affinity is the energy change when an electron is added to a neutral atom to form a negative ion.
  • For most elements, the second electron affinity is endothermic, meaning energy is absorbed.
  • For oxygen, adding an electron to an already negatively charged O- ion to form O2- requires 780 kJ/mol of energy.
  • Hence, the correct answer is C, "+780 kJ/mol."

MCQs 4:

Which among the following doesn’t react with water even at high temperatures?





Topic: Reactivity with Water

Correct Answer: A) Be

Detailed Hint:
  • Not all elements react with water. The reactivity can be influenced by factors such as temperature and the element's inherent properties.
  • Beryllium (Be) is unique among alkaline earth metals because it does not react with water, even at red hot temperatures.
  • This is due to Be’s high charge density and low tendency to lose electrons, thereby demonstrating the least metallic character among the options.
  • Hence, the correct answer is A, "Be."

MCQs 5:

What is the correct trend of reduction power amongst halogens?





Topic: Reduction Power in Halogens

Correct Answer: D) F– < Cl– < Br– < I–

Detailed Hint:
  • Reduction power refers to a substance's ability to donate electrons.
  • For halogens, the trend in reduction power is inverse to that of oxidizing power.
  • The greater the size of the halogen ion, the higher its reduction power. Thus, the reduction power increases from fluorine to iodine.
  • So, the correct trend in reduction power amongst halogens is I– > Br– > Cl– > F–, represented by option D.

MCQs 6:

What method did Newland employ to classify elements in the periodic table?





Topic: Newland's Law of Octaves

Correct Answer: B) Law of octaves

Detailed Hint:
  • John Newlands, an English chemist, proposed his Law of Octaves for the classification of elements.
  • He organized elements into groups of eight, where the properties of the first and eighth elements were similar, much like the octaves in music.
  • Therefore, Newland used the Law of Octaves for element classification, represented by option B.

MCQs 7:

What is the correct order of ionic radii for iodine?





Topic: Ionic Radii of Iodine

Correct Answer: D) I– > I > I+

Detailed Hint:
  • The size of ions differs from their parent atom due to the addition or removal of electrons.
  • Anions, which are negatively charged ions, are larger in size than their parent atom as the added electron increases electron-electron repulsion.
  • Cations, which are positively charged ions, are smaller than their parent atom due to the removal of an electron which decreases electron-electron repulsion.
  • Hence, the correct order for iodine's ionic radii is I– (anion) > I (parent atom) > I+ (cation), as in option D.

Question 8:

Why isn't MgCl3 commonly observed?





Topic: Magnesium Ionization Energy

Correct Answer: C) The third ionization energy of Mg is very high

Detailed Hint:
  • The ionization energy of an element refers to the amount of energy required to remove an electron from an atom.
  • Magnesium has two electrons in its valence shell, and removing a third electron is significantly more difficult, meaning the third ionization energy is noticeably high.
  • This high ionization energy hinders the formation of MgCl3, as the Mg can't easily reach a +3 oxidation state.
  • Therefore, the correct answer is C, "The third ionization energy of Mg is very high."

Question 9:

What is the correct order of alkali metals?





Topic: Alkali Metals Order

Correct Answer: B) Li, Na, K, Rb, Cs, Fr

Detailed Hint:
  • The alkali metals are a group of chemical elements from the s-block of the periodic table with very similar properties.
  • They are arranged in the periodic table in order of increasing atomic number, which corresponds to the order in option B: lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr).
  • Therefore, option B represents the correct order of alkali metals.

Question 10:

Why is sodium more reactive with water than lithium?





Topic: Reactivity of Alkali Metals

Correct Answer: C) Sodium is more electropositive

Detailed Hint:
  • The reactivity of alkali metals with water is based on their electropositive character, which increases as we move down the group in the periodic table.
  • This increase in electropositive character is due to decreasing ionization energy.
  • As sodium is below lithium in the periodic table, it has a higher electropositive character and lower ionization energy, which makes it more reactive with water.
  • Hence, the correct answer is C, "Sodium is more electropositive."

Question 11:

Which ion holds the highest polarizing power?





Topic: Polarizing Power

Correct Answer: D) Al3+

Detailed Hint:
  • Polarizing power refers to the ability of a positive ion to distort the electron cloud of a negative ion.
  • It is directly proportional to charge and inversely proportional to size.
  • Among the given options, Al3+ has the highest charge and smaller size, making its polarizing power the highest.
  • Therefore, option D, "Al3+," is the correct answer.

Question 12:

Which elements are most likely to form an ionic bond?





Topic: Ionic Bond Formation

Correct Answer: B) Elements with low polarizing power and low polarizability

Detailed Hint:
  • Ionic bonds are typically formed between metals and non-metals.
  • Metals lower down the group possess low polarizing power and non-metals higher in the group exhibit low polarizability.
  • Such elements are most favorable for the formation of ionic bonds.
  • Thus, option B, "Elements with low polarizing power and low polarizability," is the correct answer.

Question 13:

Which of the following elements can commonly form more than five bonds?





Topic: Element Bonding Capacity

Correct Answer: C) Iodine

Detailed Hint:
  • Some elements can form more than a typical number of bonds because of their ability to utilize d-orbitals in bonding – a phenomenon known as hypervalence.
  • Among the options, iodine can form up to seven bonds, as demonstrated in the compound IF7.
  • Therefore, option C, "Iodine," is the correct answer.

Question 14:

How does the heat of hydration of alkaline earth metals change as we move down the group?





Topic: Heat of Hydration of Alkaline Earth Metals

Correct Answer: C) It decreases

Detailed Hint:
  • The heat of hydration refers to the energy released when water molecules surround and interact with ions.
  • Alkaline earth metals' charge density decreases down the group, reducing the ions' attraction to water molecules.
  • Consequently, the heat of hydration decreases as we move down the group of alkaline earth metals.
  • Thus, option C, "It decreases," is the correct answer.

Question 15:

Which of the following outermost electronic configurations matches the least electronegative element in a given period?





Topic: Electronegativity and Electron Configuration

Correct Answer: B) ns2 np2

Detailed Hints:
  • Electronegativity refers to an atom's ability to attract shared electrons in a bond and increases along a period.
  • The electronic configuration with ns2 np5 corresponds to the most electronegative element within a period, whereas ns2 np2 indicates the least electronegative element.
  • Therefore, option B, "ns2 np2," is the correct answer.

Question 16:

Which of the following orbitals contributes the least to electron shielding?






Topic: Electron Shielding

Correct Answer: D) f – orbital

Detailed Hints:
  • Electron shielding, or screening, refers to the ability of inner shell electrons to reduce the effective nuclear charge experienced by outer shell electrons.
  • Different orbitals vary in their ability to screen electrons, with the f-orbital being the least effective due to its lower penetration.
  • Therefore, option D, "f – orbital," is the correct answer.

Question 17:

Which property of Group IIA elements exhibits an increasing trend down the group?





Topic: Group IIA Elements' Properties

Correct Answer: C) Reductive capacity

Detailed Hints:
  • With increasing atomic number in Group IIA, the number of inner shells increases, atomic radius enlarges, and the shielding effect intensifies.
  • These changes progressively lower ionization energy, enhancing metallic character and consequently increasing the reductive capacity of the elements in the group.
  • This brings us to option C, "Reductive capacity," which is the correct answer.

Question 18:

Which sequence represents the correct order of first ionization potential?





Topic: First Ionization Potential

Correct Answer: B) Be > Mg > Ca

Detailed Hints:
  • Ionization energy refers to the energy required to remove an electron from its atomic shell.
  • This energy tends to decrease down a group as atomic radii increase and the outermost electrons become easier to detach.
  • The sequence "Be > Mg > Ca" correctly reflects this trend, making option B the correct answer.

Question 19:

In which type of orbital is the electron closest to the nucleus?





Topic: Electron Orbital Penetration

Correct Answer: A) s – orbital

Detailed Hint:
  • Different types of orbitals allow electrons different levels of proximity to the atomic nucleus, a concept known as penetration.
  • The order of penetration is s > p > d > f, meaning the s-orbital enables the closest approach to the nucleus.
  • Thus, the correct answer is option A, "s – orbital."

Question 20:

Among the following metals, which one exhibits the lowest reactivity?





Topic: Reactivity of Metals

Correct Answer: A) Be

Detailed Hint:
  • The reactivity of a metal is determined by its ability to lose electrons and form positive ions.
  • Alkali metals, such as sodium (Na), potassium (K), and lithium (Li), are known to be highly reactive due to their outermost electronic configuration.
  • Beryllium (Be), however, is an alkaline earth metal and is less reactive compared to alkali metals.
  • Consequently, the correct answer is option A, "Be."

Question 21:

In which of the following elements does the 1s orbital contribute most significantly to electron screening?





Topic: Electron Screening in Orbitals

Correct Answer: D) I

Detailed Hint:
  • Electron screening refers to the repulsion effect experienced by outer shell electrons due to the presence of inner shell electrons.
  • The 1s orbital, being closest to the nucleus, is highly effective at screening.
  • Of the options, iodine (I) has the highest atomic number and hence the greatest nuclear charge, which increases the effectiveness of its 1s orbital in electron screening.
  • Therefore, the correct answer is option D, "I."

Question 22:

Which of the following is less likely to be found as a heteroatom in general heterocyclic compounds?





Topic: Heteroatoms in Heterocyclic Compounds

Correct Answer: D) Bromine

Detailed Hints:
  • Heterocyclic compounds are those that contain at least one heteroatom — an atom other than carbon — in their cyclic structure.
  • Typically, the heteroatoms in such compounds are elements like oxygen (O), nitrogen (N), and sulphur (S).
  • Bromine (Br) is less commonly found as a heteroatom in heterocyclic compounds.
  • Thus, the correct answer is option D, "Bromine."

Question 23:

What makes Lithium occupy a superior position in the electrochemical series?





Topic: Positioning in the Electrochemical Series

Correct Answer: C) Its high hydration energy

Detailed Hints:
  • The position of an element on the electrochemical series is influenced by various factors, including ionization energy, electron affinity, hydration energy, and polarizability.
  • Though Lithium (Li) has a higher ionization energy compared to Sodium (Na) and Potassium (K), making electron removal difficult, it places higher in the electrochemical series.
  • This is due to its high hydration energy, which results in greater stability.
  • Therefore, the correct answer is option C, "Its high hydration energy."

Question 24:

Why can Potassium dislodge Sodium from Sodium Chloride?





Topic: Displacement Reactions

Correct Answer: C) Because Potassium is more electropositive

Detailed Hints:
  • Displacement reactions, in which one element displaces another from a compound, are governed by the principle of electropositivity.
  • In this case, Potassium (K) can displace Sodium (Na) from Sodium Chloride (NaCl).
  • This is because Potassium is more electropositive than Sodium, giving it a higher tendency to lose electrons and form positive ions.
  • Hence, the correct answer is option C, "Because Potassium is more electropositive."

Question 25:

Why does the atomic radius decrease along a period?





Topic: Atomic Radius in the Periodic Table

Correct Answer: B) Because of increasing effective nuclear charge

Detailed Hints:
  • The atomic radius usually decreases across a period on the periodic table due to various factors.
  • While both the nuclear charge and the effective nuclear charge increase along a period, the decrease in atomic size is primarily due to the increase in effective nuclear charge.
  • Screenings effects remain relatively constant across the period.
  • Consequently, the correct answer is option B, "Because of increasing effective nuclear charge."

Question 26:

What color of flame is produced when Sodium burns in Chlorine?





Topic: Sodium's Reaction with Chlorine

Correct Answer: B) Orange

Detailed Hints:
  • The reactions of metals with halogens can often be visually observed due to the distinctive colors of the flames produced.
  • Sodium (Na), when it burns in chlorine (Cl), produces a specific flame color.
  • Reference materials, such as textbooks, indicate that the flame produced in this reaction is orange.
  • Hence, the correct answer is option B, "Orange."

Question 27:

Which alkali metal reacts least vigorously with water to produce hydroxides and dihydrogen?





Topic: Reactive Nature of Alkali Metals

Correct Answer: A) Lithium (Li)

Detailed Hints:
  • Alkali metals are known to react vigorously with water, forming hydroxides and dihydrogen.
  • However, not all alkali metals react with the same intensity; the reactivity increases down the group.
  • Thus, Lithium (Li), being at the top of the alkali metals group, reacts least vigorously.
  • Therefore, the correct answer is option A, "Lithium (Li)."

Question 28:

Which statement is correct about ionization energy?






Topic: Ionization Energy Trends

Correct Answer: C) Beryllium has higher ionization energy than Boron

Detailed Hints:
  • Ionization energy refers to the energy required to remove an electron from an atom or molecule.
  • Its trend on the periodic table is specific: it generally increases along a period (from left to right) and decreases going down a group.
  • In Group II (Beryllium) and Group III (Boron), Beryllium has a higher ionization energy.
  • Consequently, the correct answer is option C, "Beryllium has higher ionization energy than Boron."

Question 29:

What is the second electron affinity value of Oxygen?





Topic: Electron Affinity of Oxygen

Correct Answer: C) +780 KJ/mol

Detailed Hint:
  • Electron affinity is a measure of the energy change when an electron is added to a neutral atom to form a negative ion.
  • The second electron affinity involves the addition of a second electron.
  • For Oxygen, this process requires forcing the electron into a small, very electron-dense space, resulting in a high second electron affinity value.
  • Therefore, the correct answer is option C, "+780 KJ/mol."

Question 30:

What is the major product when excess Methane reacts with Chlorine?






Topic: Methane and Chlorine Reaction

Correct Answer: A) Chloromethane

Detailed Hint:
  • The reaction between Methane and Chlorine can yield several products, depending on the conditions.
  • In an excess of Methane, a monosubstituted product, Chloromethane, is favored.
  • Tetrasubstituted products are favored in limited Methane conditions, but this is not the case here.
  • Hence, the correct answer is option A, "Chloromethane."

Question 31:

In which group of elements does the atomic radius decrease with increasing atomic number?





Topic: Atomic Radii Trends in the Periodic Table

Correct Answer: C) Elements from Lithium to Neon

Detailed Hint:
  • Atomic radius, the size of an atom, exhibits specific trends on the periodic table.
  • Generally, atomic radius increases from top to bottom and decreases from left to right.
  • Therefore, in the group of elements from Lithium to Neon, the atomic radii decreases as the atomic number increases.
  • Consequently, the correct answer is option C, "Elements from Lithium to Neon."

Question 32:

How does ionization energy change in a group and period?





Topic: Trends of Ionization Energy

Correct Answer: A) It diminishes from top to bottom in a group

Detailed Hint:
  • The ionization energy is the energy required to strip an electron from an atom or molecule.
  • This energy changes in a predictable manner across the periodic table, often referred to as trends.
  • Within a group (vertical column), the ionization energy tends to decrease from top to bottom. This is due to the increasing size of atoms and the greater number of electron shells.
  • However, along a period (horizontal row), the ionization energy generally increases, as electrons are added to the same shell while protons are added to the nucleus, increasing the nuclear charge.
  • Therefore, the correct answer is option A, "It diminishes from top to bottom in a group."
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