Nomenclature of Elements MCQ Quiz - Objective Question with Answer for Nomenclature of Elements - Download Free PDF

The correct answer is As. 

Key Points

• The chemical formula of arsenic is As.
• Arsenic:
  • Atomic number: 33
  • Atomic mass: 74.93 u
• Arsenic is an element that causes arsenicosis.
• It is found in water that has flowed through arsenic-rich rocks.
• Arsenic and fluoride have been recognized by the World Health Organization (WHO) as the most serious inorganic contaminants in drinking water on a worldwide basis.

Additional Information

• There are 7  metalloids in the modern periodic table.
• The seven commonly recognized metalloids are:-
• Boron (B), Silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), tellurium (Te), and Polonium.
• Metalloids Silicon and Germanium are widely used in the semiconductor industry.

The correct answer is option 1 i.e P

Key Points

• Atomic radii- The distance from the centre of the nucleus to the outermost shell containing electrons called the atomic radius.
• While moving left to right across a period in the periodic table, the atomic number increases.
• Due to this the effective nuclear charge also increases.
• This is because the nucleus pull is high for the electrons, 
• From right to left in the periodic table the atomic radius increase.
• As Ar is the 18 group element, Cl is the 17 group element, S is the 16 group element, and P is the 15 group element so P has the largest- size ions among these elements.

The correct answer is bleaching powder.

Key Points

• Bleaching powder:
• The chlorine produced on passing electricity through brine solution undergoes a reaction with dry slaked lime [Ca (OH)2] to produce Bleaching powder.
• The reaction is as follows: Ca(OH)2 + Cl2 → CaOCl2 + H2Owhere,
  • Ca(OH)2 is calcium hydroxide or dry-slaked lime.
  • Cl2 is chlorine gas
  • CaOCl2 is a bleaching powder or calcioxychlorate.​

Additional Information

• Bleaching powder is used for several purposes:
  • As a bleaching agent for bleaching cotton and linen in the textile industry,
  • To bleach wood pulp in the paper manufacturing industry.
  • To bleach washed clothes in the laundry.
  • As an oxidizing agent in many chemical industries.
  • To disinfect drinking water and make it germ-free.

Important Points

The correct answer is Potassium and gold.

Key Points

• Potassium is the most reactive metal in the reactivity series. It reacts explosively with water and even moisture in the air.
• Gold is one of the least reactive metals and does not tarnish or corrode easily, maintaining its luster over time.
• The reactivity series is a list of metals arranged in order of decreasing reactivity to help predict their behavior in reactions.
• Potassium's high reactivity is due to its single electron in the outermost shell, which it loses easily to form positive ions.
• Gold's low reactivity is due to its full d-subshell and high ionization energy, making it less likely to participate in chemical reactions.

Additional Information

• Reactivity Series
  • The reactivity series, also known as the activity series, is a ranking of metals based on their reactivity from highest to lowest.
  • It helps predict how metals will react with acids, water, and other compounds.
  • Metals high in the series, like potassium, sodium, and calcium, react more vigorously than those lower down, like gold, platinum, and silver.
• Reactivity of Alkali Metals
  • Alkali metals, such as potassium and sodium, are highly reactive due to their single valence electron.
  • They tend to lose this electron easily, forming positive ions and engaging in reactions with water, oxygen, and halogens.
• Gold's Chemical Properties
  • Gold is known for its resistance to corrosion and tarnish, making it highly valuable in jewelry and electronics.
  • It is a noble metal, meaning it is resistant to reacting with most chemicals.
• Applications of Reactivity Series
  • The reactivity series is used in metallurgy to extract metals from their ores.
  • It is also used in predicting the outcomes of displacement reactions in chemistry.

CONCEPT:

Transition Metal Chemistry and Stability of Oxidation States

• Fluorine is highly electronegative and small in size, which allows it to stabilize higher oxidation states in transition metals. However, the primary factor is not lattice enthalpy but the strong ionic bonds formed due to fluorine's electron-withdrawing ability.
• The second and third ionization enthalpies of certain transition metal ions can be lower than expected due to the stability of half-filled or fully-filled d-subshells that occur after ionization.
• Transition metals tend to form alloys easily because their atomic radii are similar, typically within about 15%, which allows for easy substitution in the lattice structure.
• The reducing and oxidizing abilities of transition metal ions, even when having the same electron configuration (like d4), depend on their overall stability and redox potentials.

EXPLANATION:

• Option 1: "Ability of Fluorine to stabilise higher oxidation states in transition metals is due to the low lattice enthalpy of the fluorides."
  • This statement is incorrect. Fluorine stabilizes higher oxidation states of transition metals due to its high electronegativity and small ionic size, which lead to strong ionic bonds and a high electron-withdrawing capacity. Lattice enthalpy is not the primary factor. In fact, fluorides typically have high lattice enthalpies due to these strong ionic interactions.
• Option 2: "The second and third Ionisation enthalpies of Mn2+ and Fe3+ respectively have lower values than expected."
  • This statement is correct. The lower-than-expected ionization enthalpies of Mn2+ and Fe3+ can be attributed to the stability provided by their half-filled (Mn2+ with d5 configuration) and filled (Fe3+ with d5 configuration) subshells, which make further ionization less energetically costly.
• Option 3: "Transition metals readily form alloys because their metallic radii are within about 15% of each other."
  • This statement is correct. The similar atomic radii of transition metals (within 15%) allow them to easily substitute for one another in the crystal lattice, which is why they form alloys so readily.
• Option 4: "Cr2+ acts as reducing agent while Mn3+ acts as an oxidising agent though both the ions have d4 configuration."
  • This statement is correct. Although both Cr2+ and Mn3+ have d4 configurations, Cr2+ is a reducing agent because it prefers to be oxidized to Cr3+, which is more stable. Mn3+, on the other hand, prefers to be reduced to Mn2+, making it an oxidizing agent.

Therefore, the incorrect statement is Option 1.

The correct answer is Tin.

Important Points

• Silicon, Germanium, Arsenic are metalloids.
• Tin is a metal.

Key Points

The basic difference between Metals, Non-metals, and Metalloids.

The correct answer is Sulphuric acid.

• Sulfuric acid is the chemical name of ‘oil of vitriol’.

Key Points 

• Sulfuric acid is a dense, colourless, oily, corrosive liquid.
• It is one of the most commercially important of all chemicals. 
• It is prepared industrially by the reaction of water with sulfur trioxide.
• Vitriol is any of certain hydrated sulfates or sulfuric acid.
• Uses of Sulphuric acid (H2SO4):
  • In lead storage battery.
  • In the manufacturing of HCl.
  • In the manufacturing of Alum.
  • In the manufacturing of fertilisers,
    drugs, detergents and explosives.

The correct answer is As. 

Key Points

• The chemical formula of arsenic is As.
• Arsenic:
  • Atomic number: 33
  • Atomic mass: 74.93 u
• Arsenic is an element that causes arsenicosis.
• It is found in water that has flowed through arsenic-rich rocks.
• Arsenic and fluoride have been recognized by the World Health Organization (WHO) as the most serious inorganic contaminants in drinking water on a worldwide basis.

Additional Information

• There are 7  metalloids in the modern periodic table.
• The seven commonly recognized metalloids are:-
• Boron (B), Silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), tellurium (Te), and Polonium.
• Metalloids Silicon and Germanium are widely used in the semiconductor industry.

The correct answer is Potassium.

Key Points

• The Reactivity series of metals refers to the arrangement of metals in the descending order of their reactivities.
• ​Features of Reactivity series:
  • The metals at the top of the reactivity series are powerful reducing agents since they are easily oxidized and get corroded very easily.
  • The reducing ability of the metals grows weaker while traversing down the series.
  • The electro positivity of the elements also reduces while moving down the reactivity series of metals.
  • All metals that are found above hydrogen in the activity series liberate H2 gas upon reacting with dilute HCl or dilute H₂SO₄.
  • Metals that are placed higher on the reactivity series have the ability to displace metals that are placed lower from their salt solutions.

Additional Information

• Cesium is the most reactive metal in the periodic table.
  • It is a rare metal than other alkali metals.
  • It is silvery gold, soft, and ductile. 

Important Points

• Cesium, Gallium, and Mercury are the only three metals that are liquid at or around room temperature.

The correct answer is option 1 i.e P

Key Points

• Atomic radii- The distance from the centre of the nucleus to the outermost shell containing electrons called the atomic radius.
• While moving left to right across a period in the periodic table, the atomic number increases.
• Due to this the effective nuclear charge also increases.
• This is because the nucleus pull is high for the electrons, 
• From right to left in the periodic table the atomic radius increase.
• As Ar is the 18 group element, Cl is the 17 group element, S is the 16 group element, and P is the 15 group element so P has the largest- size ions among these elements.

The correct answer is Magnesium.

• Magnesium is known as alkaline earth metal.

Key Points

• The alkaline earth metals are named after the alkaline earth whose old-fashioned names were beryllia, magnesia, lime, strontia, and baryta, after their oxides. When mixed with water, these oxides are simple (alkaline).
• The elements of Group 2 of the periodic table are alkaline earth metals.
• Beryllium, magnesium, calcium, strontium, barium, and radium are the elements in Group 2.
  • For two reasons, these elements are referred to as Alkaline Earth metals. Their oxides remain in the crust of the earth and are very heat-stable.
• In group 1 of the periodic table, alkali metals are the elements.
  • The key distinction between alkaline and alkali is that there is one valence electron in alkali metals, while two valence electrons are in alkaline earth metals.

Additional Information 

The correct answer is Halogens.

Key Points

• The Halogens are a group of six elements of Group 17 in the periodic table.
  • Fluorine (F)
  • Chlorine (Cl)
  • Bromine (Br)
  • Iodine (I)
  • Astatine (At)
  • Tennessine (Ts)
• Halogens are nonmetals.
• Halogens are very reactive, the reactivity decreases from Fluorine to Astatine.
• Physical Properties of Halogens:
  • They have a strong and often nasty smell.
  • They are extremely toxic.
  • They are poor conductors of heat and electricity.
  • They have low melting and boiling points.
• Chemical Properties of Halogens:
  • Their Molecules are diatomic.
  • They have seven valence electrons as their one electron missing, they form negative ions and are highly reactive.
  • They can gain an electron by reacting with atoms of other elements.

Additional Information

• Group 15 of the periodic table is known as Pnictogens (Nitrogen group). The elements are as follows:
  • Nitrogen (N)
  • Phosphorous (P)
  • Arsenic (As)
  • Antimony (Sb)
  • Bismuth (Bi)
• Group 16 of the periodic table is known as Chalcogens (Oxygen group). The elements are as follows:
  • Oxygen (O)
  • Sulphur (S)
  • Selenium (Se)
  • Tellurium (Te)
  • Polonium (Po)
• Group 18 of the periodic table is known as Noble gases. The elements are as follows:
  • Helium (He)
  • Neon (Ne)
  • Argon (Ar)
  • Krypton (Kr)
  • Xenon (Xe)
  • Radon (Rn)

The correct answer is Chlorine.

Key Points

• The element having electronic configuration 2,8,7 is Chlorine. 
• It is the member of group 17. It is a p - block element which means the valence shell containing the valence shell electrons in the p subshell.
• The systematic way of writing the configuration is 1s2, 2s2 2p6, 3s2 3p5. so the last 5 electrons are filled in p subshell.
• Chlorine is a chemical element with the symbol Cl and atomic number 17.
• The second-lightest of the halogens, it appears between fluorine and bromine in the periodic table and its properties are mostly intermediate between them.
• Chlorine is a yellow-green gas at room temperature.

Additional Information 

• Chlorine has a variety of uses:
  • It is used to disinfect water and is part of the sanitation process for sewage and industrial waste.
  • During the production of paper and cloth, chlorine is used as a bleaching agent.
  • It is also used in cleaning products, including household bleach which is chlorine dissolved in water.

The correct answer is Cm.

• Cm is the chemical symbol of Curium.
• Curium is a transuranic, radioactive chemical element with the symbol Cm and atomic number 96.
• This element of the actinide series was named after eminent scientists Marie and Pierre Curie.

 Additional Information

• Modern Periodic Table:

The correct answer is 3, 5.

Key Points

• The atomic number of phosphorus is 15.
• The number of electronic configuration are 2,8,5.
• When the atom gains 3 electrons the orbit is filled. or otherwise the atoms should lose 5 electrons. the valency is the combining capacity of the atom. therefore the valency of phosphorus is 3 and 5. Hence option 4 is correct.

Additional Information

• We know that the atomic number of phosphorus is 15 and its electronic configuration in the ground state is [Ne] 3s²3p³. 
• We know that phosphorus also has a vacant 3d-orbital. In an excited state, electrons are excited from a lower energy level to a higher energy level. Here in phosphorus in an excited state, an electron is excited from 3s to 3d orbit. Now, the electronic configuration of phosphorus in the excited state is 
  [Ne]3s13p33d1. 
• In the electronic configuration of the excited state of phosphorus, we can see that there are five unpaired electrons in it.
• The valency of an atom is its tendency to make bonds with other atoms.
• Here, the exciting state phosphorus has five unpaired electrons means it can form five bonds with some other atoms.
• Then the valency of phosphorus in the excited state is 5.