Modern Periodic Table MCQ Quiz - Objective Question with Answer for Modern Periodic Table - Download Free PDF

The correct answer is Xenon.

Key Points

• Xenon is a noble gas, which is typically found as a monoatomic gas in nature.
• Xenon is chemically inert and does not readily form compounds with other elements.
• It is one of the rare gases found in the Earth's atmosphere, with a concentration of about 0.0000087% by volume.
• Being monoatomic means that Xenon exists as single atoms rather than molecules.

Additional Information

• Noble Gases
  • Noble gases include Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), and Radon (Rn).
  • These gases are characterized by their lack of chemical reactivity due to having complete valence electron shells.
• Monoatomic Gases
  • Monoatomic gases consist of single atoms not bonded to each other.
  • Examples include noble gases like Helium, Neon, and Argon, in addition to Xenon.
• Uses of Xenon
  • Xenon is used in flash lamps, arc lamps, and as a general anesthetic.
  • It is also utilized in ion propulsion systems for spacecraft.
• Chemical Inertness
  • The inertness of noble gases makes them ideal for use in conditions where reactions are undesirable.
  • This property is due to their filled outer electron shells, which make them stable and unreactive.

The correct answer is Metalloids.

Key Points

• Metalloids are elements that exhibit properties of both metals and non-metals.
• Boron (B), Silicon (Si), and Germanium (Ge) are commonly classified as metalloids due to their intermediate characteristics.
• Metalloids are typically found along the "stair-step" line of the periodic table that separates metals and non-metals.
• They are semiconductors, which means they conduct electricity under certain conditions, making them valuable in electronics.
• Metalloids often form covalent bonds and have variable oxidation states, contributing to their unique chemical behavior.

Additional Information

• Periodic Table Classification:
  • The periodic table is divided into metals, non-metals, and metalloids based on their physical and chemical properties.
  • Metalloids lie on the dividing line (zigzag pattern) between metals and non-metals, including elements such as Boron, Silicon, Germanium, Arsenic, Antimony, and Tellurium.
• Semiconductors:
  • Metalloids like Silicon and Germanium are widely used as semiconductors in electronic devices such as transistors and integrated circuits.
  • Semiconductors have a conductivity that is between that of conductors (metals) and insulators (non-metals).
• Applications:
  • Boron is used in the production of borosilicate glass and as a doping agent in semiconductors.
  • Silicon is a key material in the electronics industry and is used in solar panels and computer chips.
  • Germanium is used in infrared optics, fiber-optic systems, and as a semiconductor material.
• Characteristics of Metalloids:
  • They often have a metallic appearance but are brittle like non-metals.
  • Metalloids can react differently depending on the substances they interact with, showing metallic or non-metallic chemical behavior.

CONCEPT:

Valency of Anions

• Valency refers to the combining capacity of an element or ion. It is determined by the number of electrons an atom can lose, gain, or share to achieve a full outer shell.
• Anions are negatively charged ions formed when atoms gain electrons. The valency of an anion is equal to the number of electrons gained by the atom.

EXPLANATION:

• To determine which anion has a valency of -3, we need to look at the common anions and their charges:
  • Nitride (N^3-): Nitrogen gains 3 electrons to achieve a full outer shell, resulting in a valency of -3.
  • Nitrate (NO₃^-): The nitrate ion has a valency of -1.
  • Sulphide (S^2-): Sulfur gains 2 electrons to form the sulphide ion, giving it a valency of -2.
  • Sulphate (SO₄^2-): The sulphate ion has a valency of -2.

Therefore, the anion with a valency of -3 is Nitride (N^3-).

CONCEPT:

Chemical vs Physical Properties

• Chemical properties are characteristics of a substance that become evident during a chemical reaction; they include reactivity, combustibility, and acidity.
• Physical properties can be observed or measured without changing the composition of matter; they include melting point, boiling point, and density.

EXPLANATION:

• Among the given options:
  • Melting point, boiling point, and density are physical properties because they can be observed without altering the chemical structure of the substance.
  • Combustibility is a chemical property because it describes how a substance reacts with oxygen to produce heat and light during combustion.
• Therefore, the correct answer is:
  • Option 1, 2, and 3 are physical properties.
  • Option 4 (Combustibility) is a chemical property.

Therefore, the option that is a chemical property is Combustibility.

The correct option is 13-17.

Key Points

•  In the new periodic table, the elements from groups 13 to 17 are called intermediate elements.
• The intermediate elements are called metalloids.
• Metalloids are semi-metals, which means they can show the properties of both metals and non-metals.

Additional InformationGroup 1,2

• Group 1st elements are called alkali metals. There are 6 alkali metals. 
• Group 2nd elements are called alkaline earth metals. There are 6 alkaline earth metals.

Group 3-12

• Groups 3 to 12 are called transition metals.
• There are d-block elements present in the 3 to 12th group of the periodic table.

Group17

• Group 17 elements are called halogen elements.
• They are much reactive in nature.
• There are 6 halogen elements in the periodic table.

The correct answer is 17th.

• The Halogens are the elements belonging to Group 17 in the periodic table.

• A periodic table is an arrangement of elements based on their atomic numbers and chemical properties.
• It is divided into 18 groups and 7 periods running vertically and horizontally respectively.
• The periodic table accommodates a discrete combination of metal, non-metals, and metalloids.
• The elements in the periodic table are arranged horizontally in ascending order of their atomic numbers known as periods.
• Vertically the elements having identical chemical properties are clubbed together known as groups.
• The 18 groups are also known as columns and the 7 periods are also known as the rows.

Explanation:

Periods:

• Elements are arranged in increasing the atomic number of elements in a period.
• One extra electron gets added to the outermost shell as we move along the periods from left to right.
• The electron gets added to the same shell or orbit and thus the electrons present for bonding increase by one unit.
• Thus, the shell number remains the same but the number of electrons present for bonding increases along a period.

Groups:

• Elements having the same number of outer electrons are put in the same group of the periodic table.
• When we move down a group, new shells get added.
• The outermost shell has electrons present for bonding.
• Though the number of shells increases as we go down in a group, the number of electrons in the outermost shell remains the same.
• For example, the Halogens F, Cl, Br, I, At all belong to group 17 and have 7 electrons in the outermost shell.
• Similarly, Group 16 elements have 6 electrons in the outermost shell, group 15 has 5 electrons in the outermost shell, and so on.

Hence, group 17 is called halogens.

The correct answer is 118.

Key Points

• Modern Periodic Table has 18 Groups and 7 Periods.
• It has 118 Elements.
• The periodic table generally displays only the symbol of the element and not its entire name.
• Each of the tables has a vertical row is called groups.
• Elements in groups have similar chemical and physical properties because they have the same number of outer electrons.
• Each of the tables has horizontal rows is called periods. During a period, a gradual change in chemical properties occurs from one element to another.
• It was given by Dmitri Mendeleev.
• The Modern Periodic table is used to organize all the known elements.

The correct answer is Helium.

Key Points

• The noble gas family has zero valencies.
• The valency of an element is related to how many electrons are in the outer shell.
• The electronic configuration of Helium (He) is 2, 0.
  • Hence, the Valency of the element Helium is 0.
• Neon, Radon, and Argon have zero valencies because they have their outer shell completely filled and are chemically inert gas.

Additional Information

• The combining capacity of an atom is known as its valency.
  • The number of bonds that an atom can form as part of a compound is expressed by the valency of the element.
  • Valence electrons are those electrons that are present in the outermost orbit of the atom.
  • These electrons have a weak attraction towards the atomic nucleus; thus, atoms can easily remove or share these electrons with other atoms.
  • By sharing, gain or donating electrons, chemical bonds are formed between the atoms.
• Lithium has one valency.
• Beryllium has two valencies.
• Fluorine has one valency.

​

The modern periodic table has 18 columns.

Hence the Statement, Modern periodic table has 15 columns is not Correct.

Key Points

The First Periodic Table:

• In the 1860s, a scientist named Dmitri Mendeleev also saw the need to organize the elements.
• He created a table in which he arranged all of the elements by increasing atomic mass from left to right across each row.
• When he placed eight elements in each row and then started again in the next row, each column of the table contained elements with similar properties. He called the columns of elements groups.
• Mendeleev’s table is called a periodic table and the rows are called periods. That’s because the table keeps repeating from row to row, and periodic means “repeating.”

The Modern Periodic Table:

• The modern periodic table is used to organize all the known elements. Elements are arranged in the table by increasing atomic number.
• In the modern periodic table, each element is represented by its chemical symbol. The number above each symbol is its atomic number. Atomic numbers increase from left to right and from top to bottom in the table.
• Rows of the periodic table are called periods. From left to right across a period, each element has one more proton than the element before it.
• Columns of the periodic table are called groups. Elements in the same group have similar properties.
• All elements can be classified into one of three classes: metals, metalloids, or nonmetals. Elements in each class share certain basic properties. From left to right across each period of the periodic table, elements change from metals to metalloids to nonmetals.

The correct answer is Bridge Element.

Explanation:

• Mosley gave the modern Long form of Periodic table where the base of classification was the atomic number.
• According to Mosley's periodic law, the physical and chemical properties of elements are periodic functions of their Atomic number.

• In the long-form periodic table, horizontal rows are called Periods and vertical rows are called groups.
• A diagonal relationship is said to exist between certain pairs of diagonally adjacent elements in the second and third periods (first 20 elements) of the periodic table. 
• These pairs are (lithium (Li) and magnesium (Mg), beryllium (Be), and aluminum (Al), boron (B), and silicon (Si).

• For example, Lithium and magnesium are showing similar properties, so second-period elements are known as Bridge elements.
• Bridge elements are the gap between the alkali and alkali earth metals (groups 1 & 2) on one side and the metalloids/nonmetals (groups 13 - 18) on the other side.
• The third period elements( Na, Mg, Al,Si,P,S,Cl) are called the TYPICAL elements.They are called so because they represent properties of their own group.
• Transition elements refer to elements of d -block in the periodic table because their valencies show transitions.
• Elements belonging to the s- and p-blocks in the periodic table are called the normal elements or main group elements.

 So, Elements of the II^nd period are known as Bridge elements.

The correct answer is H, Li, Na, K.
Key Points 

• Elements like H, Li, Na, and K are related to the alkali metal group. 
• The alkali metals consist of the chemical elements lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs), and francium (Fr).
• Together with hydrogen, they constitute group 1, which lies in the s-block of the periodic table.
• The Group 1 elements are called alkali metals.
•  All the Group 1 elements are very reactive.
• They must be stored under oil to keep air and water away from them.
• Group 1 elements form alkaline solutions when they react with water, which is why they are called alkali metals.

Additional Information

• Modern Periodic table showing Groups and Periods:

The correct answer is I. 

Concept:

Electronegativity- 

• The tendency of an atom or element to attract a shared pair of electrons towards it.
• Is generally measured by the Pauling scale denoted by χr, on a relative scale running from 0.8 to 3. 98.
• Electronegativity is affected by the atomic number as well as the distance of electrons from the nucleus.
• Electronegativity is not the property of an atom alone but the property of an atom in a molecule.

• Electronegativity increases across a period because the number of charges on the nucleus increases. That attracts the bonding pair of electrons more strongly. As electronegativity increases, electropositivity decreases.
• Electronegativity decreases across moving down in a group, due to an increase in the distance between the nucleus and the valence electron shell. As electronegativity decreases, electropositivity increases.

​

Explanation:

• F, Cl, Br, I all are present in the same group of halogens.
• F is at the top and I is at the bottom of the group.
• As we go down a group, the electropositivity increases, and hence Iodine (I) becomes the most electropositive element. As it is the least electronegative, it is the most electropositive.
• Iodine is the least reactive of the halogens as well as the most electropositive halogen.
• Iodine has a tendency to lose electrons and form positive ions during chemical reactions.
• It is also the heaviest and the least abundant of stable halogens.
• The value of electronegativity of Iodine is 2.5.

Order of electropositivity:

I > Br > Cl > F

So, Iodine is the most electropositive element among halogens.

Mistake Points

• Fluorine (F) is the most electronegative element in the periodic table, so it is the least electropositive element.

Concept:

• Metalloids are elements that have properties similar to both metals and non-metals. In some of their properties, they show similarity with metals and in others with non-metals.
• They are hence placed in between metals and non-metals. 
• Metalloids can also be called semimetals.
• They are found in groups 13, 14, 15, 16 and 17 of the p-block.

Explanation:

• Metalloids include Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium and Polonium.
• Total elements are 118 out of which 91 are metals, 7 are metalloids, and 20 are non-metals.

In the modern periodic table, metalloids are in Right of the periodic table

Explanation:

• Mosley gave the modern Long form of Periodic table where the base of classification was the atomic number.
• According to Mosley's modern periodic law, the physical and chemical properties of elements are periodic functions of their Atomic number.

• In the long-form periodic table, horizontal rows are called Periods and vertical rows are called groups.
• In the long-form periodic table, Period 1 has two elements Hydrogen (H) and Helium (He).
• There are seven periods in the periodic table and period 1 has two elements, 2nd and 3rd have 8 elements, 4th and 5th have 18 elements and  6th and 7th have 32 elements.
• The lanthanides and actinides group in 6th and 7th periods respectively are placed separately.

So, Modern periodic law was given by Mosley.

• According to Mendeleev's periodic law, the physical and chemical properties of elements are periodic functions of their Atomic mass.

The correct answer is Chlorine.

• The most commonly used bleaching agent for disinfecting the drinking water supply is Chlorine.
• The compound of chlorine is used disinfecting drinking water - Bleaching powder (CaOCl2)

Key Points

Chlorine

• Atomic number - 17
• Mass number - 35.45
• Chlorine is the second lightest element in the Halogens family.
• Chlorine belongs to P-block elements.
• Chlorine is yellow-green colour gas at room temperature.
• Chlorine is an oxidizing agent.
• Deacon's process - Production of Chlorine
• Chlorine is extracted from seawater.
• Chlorine is discovered by Carl Wilhelm Scheele 
• Chlorine is used to purify water.
• Chlorine is used to kill germs in swimming pools.
• Chlorine is commonly used as an antiseptic.
• The solvent used as an anaesthetic - Chloroform (CHCl₃)
• The compound of chlorine is used in the plastics - PVC (Poly Vinyl Chloride)