Here below some basic MCQ’s about “Periodic Table” with answer which explained in details. Lets check one by one which is given below.
- The element with the highest ionization energy in the periodic table is:
A) Helium
B) Fluorine
C) Neon
D) Oxygen
Answer: A) Helium
Explanation: Ionization energy is the energy required to remove an electron from an atom. Helium has the highest ionization energy because it has a small atomic size and its electrons are very tightly bound to the nucleus, making it difficult to remove an electron.
- Which of the following elements has the largest atomic radius?
A) Sodium
B) Magnesium
C) Potassium
D) Calcium
Answer: C) Potassium
Explanation: Atomic radius increases down a group due to the addition of new electron shells. Among the given options, Potassium (K) is located further down in Group 1, hence it has a larger atomic radius compared to the others.
- Which of the following elements has the most metallic character?
A) Fluorine
B) Oxygen
C) Sodium
D) Cesium
Answer: D) Cesium
Explanation: Metallic character increases as you move down a group and decreases across a period from left to right. Cesium (Cs), being in Group 1 and farthest down, has the most metallic character.
- Which of the following is the correct order of electron affinity?
A) F > Cl > Br > I
B) Cl > F > Br > I
C) I > Br > Cl > F
D) Br > Cl > I > F
Answer: B) Cl > F > Br > I
Explanation: Although fluorine is more electronegative, chlorine has a slightly higher electron affinity than fluorine due to less electron-electron repulsion in its relatively larger size. Hence, the correct order is Cl > F > Br > I.
- Which of the following oxides is amphoteric?
A) Na₂O
B) Al₂O₃
C) SO₂
D) CaO
Answer: B) Al₂O₃
Explanation: Amphoteric oxides can act as both acids and bases. Aluminum oxide (Al₂O₃) is an amphoteric oxide, meaning it can react with both acids and bases to form salts and water.
- The first ionization energy generally:
A) Increases across a period
B) Decreases across a period
C) Decreases down a group
D) A and C
Answer: D) A and C
Explanation: Ionization energy increases across a period due to increasing nuclear charge, which pulls electrons closer, making them harder to remove. It decreases down a group because the outer electrons are further from the nucleus and are more easily removed.
- Which of the following is the most electronegative element?
A) Oxygen
B) Fluorine
C) Nitrogen
D) Chlorine
Answer: B) Fluorine
Explanation: Fluorine is the most electronegative element in the periodic table, as it has the greatest tendency to attract electrons towards itself when forming a bond.
- Which group in the periodic table contains elements that are all nonmetals?
A) Group 2
B) Group 14
C) Group 18
D) Group 15
Answer: C) Group 18
Explanation: Group 18 consists of the noble gases (e.g., helium, neon, argon), which are all nonmetals. These elements are characterized by their lack of reactivity due to having a complete valence shell.
- The d-block elements are also known as:
A) Alkali metals
B) Transition elements
C) Noble gases
D) Metalloids
Answer: B) Transition elements
Explanation: The d-block elements, located in groups 3–12 of the periodic table, are also referred to as transition elements. These elements typically form colored compounds and exhibit variable oxidation states.
- Which of the following statements is true about the modern periodic table?
A) Elements are arranged in order of decreasing atomic masses
B) Elements are arranged in order of increasing atomic numbers
C) All elements in the same group have the same number of neutrons
D) Elements are arranged in alphabetical order
Answer: B) Elements are arranged in order of increasing atomic numbers
Explanation: In the modern periodic table, elements are arranged in order of increasing atomic numbers, which reflect the number of protons in the nucleus of each element. This arrangement accounts for the periodic recurrence of chemical properties.
- The element with the lowest electronegativity is:
A) Helium
B) Francium
C) Lithium
D) Fluorine
Answer: B) Francium
Explanation: Electronegativity decreases down a group. Francium, being in the bottom left corner of the periodic table, has the lowest electronegativity.
- Which of the following elements has the highest electron affinity?
A) Fluorine
B) Chlorine
C) Bromine
D) Iodine
Answer: B) Chlorine
Explanation: While fluorine is more electronegative, chlorine has the highest electron affinity due to its larger atomic size, allowing it to accommodate the extra electron more easily than fluorine.
- Which of the following trends occurs as you move across a period from left to right?
A) Atomic radius decreases
B) Ionization energy decreases
C) Metallic character increases
D) Electronegativity decreases
Answer: A) Atomic radius decreases
Explanation: As you move across a period from left to right, the atomic radius decreases due to increased nuclear charge pulling the electrons closer to the nucleus.
- The elements of which group in the periodic table are known as the alkali metals?
A) Group 1
B) Group 2
C) Group 13
D) Group 17
Answer: A) Group 1
Explanation: Group 1 elements are known as alkali metals. They are characterized by having one electron in their outermost shell, making them highly reactive.
- Which element belongs to the same group as carbon?
A) Nitrogen
B) Silicon
C) Oxygen
D) Phosphorus
Answer: B) Silicon
Explanation: Silicon (Si) is in the same group as carbon (Group 14), meaning they both have four electrons in their outermost shell and share similar chemical properties.
- Which of the following elements is a metalloid?
A) Sulfur
B) Sodium
C) Boron
D) Chlorine
Answer: C) Boron
Explanation: Metalloids have properties of both metals and nonmetals. Boron (B) is a metalloid and lies along the diagonal dividing line between metals and nonmetals in the periodic table.
- Which of the following blocks in the periodic table contains the lanthanides?
A) s-block
B) p-block
C) d-block
D) f-block
Answer: D) f-block
Explanation: The lanthanides, along with the actinides, are found in the f-block of the periodic table. These are the elements in the two rows separated from the main body of the periodic table.
- Which of the following elements has a diagonal relationship with lithium?
A) Sodium
B) Magnesium
C) Beryllium
D) Potassium
Answer: C) Beryllium
Explanation: Lithium and beryllium show a diagonal relationship in the periodic table, meaning they exhibit similarities in properties despite being in different groups. This is due to their comparable charge densities.
- Which of the following elements is a halogen?
A) Argon
B) Neon
C) Bromine
D) Krypton
Answer: C) Bromine
Explanation: Halogens are found in Group 17 of the periodic table, and bromine (Br) is one of them. These elements are known for their high reactivity, especially with alkali metals.
- Which of the following pairs of elements belong to the same period?
A) Li and Be
B) Na and K
C) Mg and Ca
D) F and Cl
Answer: A) Li and Be
Explanation: Li (Lithium) and Be (Beryllium) belong to Period 2 of the periodic table. Elements in the same period have the same number of electron shells.
- Which of the following elements has the highest atomic number?
A) Oxygen
B) Fluorine
C) Nitrogen
D) Neon
Answer: D) Neon
Explanation: Among these elements, neon (Ne) has the highest atomic number, 10. Atomic numbers increase as you move from left to right across a period.
- Which of the following is the correct order of atomic radius?
A) Na > K > Rb > Cs
B) Cs > Rb > K > Na
C) Na < K < Rb < Cs D) Cs < Rb < K < Na Answer: B) Cs > Rb > K > Na
Explanation: Atomic radius increases down a group because additional electron shells are added, which increases the distance between the nucleus and the outermost electrons.
- The first element of each period in the periodic table has:
A) One electron in its valence shell
B) A complete octet in its valence shell
C) Two electrons in its valence shell
D) A valency of zero
Answer: A) One electron in its valence shell
Explanation: The first element of each period is an alkali metal (Group 1), which has one electron in its outermost shell, making it highly reactive.
- The electron configuration of an element is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s². What is the element?
A) Calcium
B) Magnesium
C) Potassium
D) Zinc
Answer: A) Calcium
Explanation: The given configuration represents calcium (Ca), which has 20 electrons (atomic number 20). The configuration ends in 4s², indicating that calcium is in Group 2.
- Which of the following groups contains only transition elements?
A) Group 2
B) Group 3-12
C) Group 15
D) Group 18
Answer: B) Group 3-12
Explanation: Transition elements are located in Groups 3-12 of the periodic table. They are characterized by their ability to form colored compounds and variable oxidation states.
- Which element is known as a noble gas?
A) Hydrogen
B) Oxygen
C) Argon
D) Nitrogen
Answer: C) Argon
Explanation: Noble gases are elements in Group 18 of the periodic table. Argon (Ar) is one of the noble gases, known for its lack of reactivity due to its full valence shell.
- Which of the following statements is true about alkali metals?
A) They form acidic oxides
B) They have low reactivity
C) They form basic oxides
D) They have high melting points
Answer: C) They form basic oxides
Explanation: Alkali metals (Group 1) form basic oxides when they react with oxygen. For example, sodium forms sodium oxide (Na₂O), which is basic in nature.
- Which of the following is an s-block element?
A) Iron
B) Potassium
C) Chlorine
D) Zinc
Answer: B) Potassium
Explanation: Potassium (K) belongs to Group 1, which is part of the s-block. Elements in this block have their valence electrons in s-orbitals.
- Which of the following elements has a half-filled p-subshell in its ground state?
A) Nitrogen
B) Oxygen
C) Neon
D) Sulfur
Answer: A) Nitrogen
Explanation: Nitrogen has an electron configuration of 1s² 2s² 2p³. A p-subshell can hold up to six electrons, and with three electrons in its p-orbital, nitrogen has a half-filled p-subshell.
- What is the period number of an element with the electron configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁵?
A) Period 3
B) Period 4
C) Period 5
D) Period 6
Answer: B) Period 4
Explanation: The element has electrons filling up to the 4th shell, so it belongs to Period 4. The configuration matches that of bromine (Br), which is in Period 4.
- Which of the following elements shows maximum number of oxidation states?
A) Scandium
B) Titanium
C) Vanadium
D) Chromium
Answer: D) Chromium
Explanation: Chromium (Cr) can exhibit a variety of oxidation states, the most common being +2, +3, and +6. The availability of multiple oxidation states is due to the presence of both s and d electrons.
- Which of the following groups contains only nonmetals?
A) Group 1
B) Group 14
C) Group 16
D) Group 2
Answer: C) Group 16
Explanation: Group 16 elements (oxygen, sulfur, selenium) are nonmetals. These elements, also known as the chalcogens, have six electrons in their outermost shell and are chemically reactive.
- The most electronegative element in Group 17 is:
A) Chlorine
B) Bromine
C) Fluorine
D) Iodine
Answer: C) Fluorine
Explanation: Fluorine is the most electronegative element in the periodic table, with an electronegativity value of 3.98 on the Pauling scale. Its small atomic radius and high nuclear charge make it highly effective at attracting electrons.
- Which element has the electron configuration [Ne] 3s² 3p¹?
A) Magnesium
B) Aluminum
C) Silicon
D) Phosphorus
Answer: B) Aluminum
Explanation: The electron configuration [Ne] 3s² 3p¹ corresponds to aluminum (Al). It has 13 electrons, with the outermost three electrons located in the 3s and 3p orbitals.
- Which of the following elements has the lowest first ionization energy?
A) Oxygen
B) Nitrogen
C) Fluorine
D) Carbon
Answer: D) Carbon
Explanation: Among the given options, carbon (C) has the lowest ionization energy. As you move across a period, ionization energy increases due to the stronger attraction between the nucleus and electrons. Fluorine has the highest, and carbon the lowest, ionization energy in this group.
- Which of the following elements is a post-transition metal?
A) Iron
B) Copper
C) Tin
D) Titanium
Answer: C) Tin
Explanation: Post-transition metals are located to the right of the transition metals in the periodic table. Tin (Sn) is a post-transition metal, exhibiting metallic properties but being softer and having lower melting points compared to transition metals.
- Which of the following elements has the highest atomic mass?
A) Nitrogen
B) Phosphorus
C) Arsenic
D) Antimony
Answer: D) Antimony
Explanation: Among the given options, Antimony (Sb) has the highest atomic mass. Atomic mass increases as you move down a group and across a period from left to right.
- Which element is a liquid at room temperature?
A) Bromine
B) Chlorine
C) Iodine
D) Fluorine
Answer: A) Bromine
Explanation: Bromine (Br) is one of the two elements that are liquid at room temperature, the other being mercury. It is a halogen with distinct reddish-brown color in its liquid form.
- Which of the following elements has sp³ hybridization in its ground state?
A) Beryllium
B) Boron
C) Carbon
D) Nitrogen
Answer: C) Carbon
Explanation: Carbon in its ground state has sp³ hybridization, forming four equivalent sp³ hybrid orbitals that participate in forming four sigma bonds, as seen in methane (CH₄).
- Which element has the electron configuration [Kr] 4d¹⁰ 5s² 5p⁴?
A) Tin (Sn)
B) Antimony (Sb)
C) Tellurium (Te)
D) Iodine (I)
Answer: C) Tellurium
Explanation: The electron configuration [Kr] 4d¹⁰ 5s² 5p⁴ corresponds to Tellurium (Te), which is in Group 16 of the periodic table.
- Which of the following elements is most likely to form a +3 oxidation state?
A) Oxygen
B) Nitrogen
C) Aluminum
D) Sodium
Answer: C) Aluminum
Explanation: Aluminum (Al) commonly exhibits a +3 oxidation state by losing three electrons, forming Al³⁺ ions.
- Which of the following statements is true about the lanthanides?
A) They are all transition metals.
B) They are f-block elements.
C) They are found in Group 18.
D) They have completely filled d-orbitals.
Answer: B) They are f-block elements.
Explanation: Lanthanides are a series of 15 f-block elements from Lanthanum (La) to Lutetium (Lu), known for their similar chemical properties and are located in the f-block of the periodic table.
- Which of the following elements has the greatest tendency to form cations?
A) Nitrogen
B) Phosphorus
C) Sodium
D) Chlorine
Answer: C) Sodium
Explanation: Sodium (Na) readily loses one electron to form Na⁺ cations, demonstrating a strong tendency to form positive ions.
- Which of the following elements is least likely to form a covalent bond?
A) Carbon
B) Hydrogen
C) Oxygen
D) Sodium
Answer: D) Sodium
Explanation: Sodium (Na) typically forms ionic bonds by losing an electron rather than sharing electrons to form covalent bonds.
- Which of the following elements has the highest metallic character?
A) Lithium
B) Beryllium
C) Boron
D) Carbon
Answer: A) Lithium
Explanation: Metallic character decreases across a period from left to right. Lithium (Li) is the most metallic among the given elements.
- Which of the following elements has a filled d-subshell in its ground state?
A) Scandium
B) Titanium
C) Zinc
D) Chromium
Answer: C) Zinc
Explanation: Zinc (Zn) has the electron configuration [Ar] 3d¹⁰ 4s², indicating a filled d-subshell.
- Which of the following elements is a gas at standard temperature and pressure (STP)?
A) Nitrogen
B) Sulfur
C) Bromine
D) Aluminum
Answer: A) Nitrogen
Explanation: Nitrogen (N₂) is a diatomic gas at STP, whereas sulfur and bromine are solids and liquids, respectively, and aluminum is a solid metal.
- Which of the following is a characteristic of nonmetals?
A) High electrical conductivity
B) Malleability
C) Brittleness
D) Lustrous appearance
Answer: C) Brittleness
Explanation: Nonmetals are generally brittle in solid form, lack metallic luster, and have poor electrical conductivity.
- Which of the following elements is an alkaline earth metal?
A) Lithium
B) Potassium
C) Calcium
D) Fluorine
Answer: C) Calcium
Explanation: Calcium (Ca) belongs to Group 2, which consists of the alkaline earth metals known for their two valence electrons.
- Which element is placed in Period 3 and Group 17 of the periodic table?
A) Chlorine
B) Bromine
C) Iodine
D) Fluorine
Answer: A) Chlorine
Explanation: Chlorine (Cl) is located in Period 3 and Group 17, which is the halogen group.
- Which of the following elements has the highest electron density?
A) Lithium
B) Beryllium
C) Boron
D) Carbon
Answer: D) Carbon
Explanation: Electron density generally increases across a period. Carbon (C) has a higher electron density compared to lithium, beryllium, and boron.
- Which of the following elements has the largest atomic size?
A) Nitrogen
B) Oxygen
C) Fluorine
D) Neon
Answer: A) Nitrogen
Explanation: Atomic size decreases across a period from left to right. Nitrogen (N) has the largest atomic radius among the given elements.
- Which of the following elements does not belong to the carbon group (Group 14)?
A) Carbon
B) Silicon
C) Germanium
D) Nitrogen
Answer: D) Nitrogen
Explanation: Nitrogen (N) is in Group 15, not Group 14, which includes Carbon (C), Silicon (Si), Germanium (Ge), Tin (Sn), and Lead (Pb).
- Which of the following elements is a noble gas?
A) Nitrogen
B) Argon
C) Chlorine
D) Bromine
Answer: B) Argon
Explanation: Argon (Ar) is a noble gas located in Group 18, known for its inertness and full valence electron shell.
- Which of the following elements has the smallest atomic radius?
A) Lithium
B) Beryllium
C) Boron
D) Carbon
Answer: D) Carbon
Explanation: Atomic radius decreases across a period from left to right. Carbon (C) has the smallest atomic radius among the listed elements.
- Which of the following elements is an example of a metalloid?
A) Sulfur
B) Phosphorus
C) Boron
D) Sodium
Answer: C) Boron
Explanation: Boron (B) is a metalloid, exhibiting properties intermediate between metals and nonmetals.
- Which of the following elements has the electron configuration [Xe] 4f¹⁴ 5d¹⁰ 6s² 6p³?
A) Bismuth
B) Thallium
C) Polonium
D) Antimony
Answer: D) Antimony
Explanation: The given electron configuration corresponds to Antimony (Sb), which is in Group 15 and Period 6.
- Which of the following elements is a poor reducing agent?
A) Lithium
B) Sodium
C) Potassium
D) Fluorine
Answer: D) Fluorine
Explanation: Fluorine (F) is a strong oxidizing agent, not a reducing agent. The other elements listed are good reducing agents due to their tendency to lose electrons.
- Which of the following elements has a filled p-subshell in its ground state?
A) Nitrogen
B) Oxygen
C) Neon
D) Fluorine
Answer: C) Neon
Explanation: Neon (Ne) has a filled p-subshell with the electron configuration 1s² 2s² 2p⁶.
- Which element has the highest electronegativity in the third period?
A) Sodium
B) Magnesium
C) Aluminum
D) Chlorine
Answer: D) Chlorine
Explanation: Among the third-period elements, Chlorine (Cl) has the highest electronegativity.
- Which of the following elements has the highest first ionization energy?
A) Sodium
B) Magnesium
C) Aluminum
D) Silicon
Answer: D) Silicon
Explanation: Ionization energy generally increases across a period. Silicon (Si) has a higher first ionization energy compared to Sodium, Magnesium, and Aluminum.
- Which of the following elements is a p-block element?
A) Iron
B) Calcium
C) Carbon
D) Titanium
Answer: C) Carbon
Explanation: Carbon (C) is a p-block element, located in Group 14. The other elements listed belong to the d-block or s-block.
- Which element has the highest melting point?
A) Carbon
B) Silicon
C) Germanium
D) Boron
Answer: A) Carbon
Explanation: Carbon, especially in its diamond form, has the highest melting point among the listed elements due to its strong covalent bonding.
- Which of the following elements is most likely to form covalent bonds?
A) Sodium
B) Magnesium
C) Chlorine
D) Calcium
Answer: C) Chlorine
Explanation: Chlorine (Cl) tends to gain electrons and form covalent bonds by sharing electrons with other nonmetals.
- Which of the following elements is a d-block element?
A) Scandium
B) Boron
C) Sulfur
D) Potassium
Answer: A) Scandium
Explanation: Scandium (Sc) is a d-block element, located in Group 3 and known as a transition metal.
- Which of the following elements is an example of a Group 17 element?
A) Oxygen
B) Nitrogen
C) Bromine
D) Helium
Answer: C) Bromine
Explanation: Bromine (Br) is a halogen, belonging to Group 17 of the periodic table.
- Which of the following elements has the electron configuration [Ar] 3d¹⁰ 4s² 4p¹?
A) Gallium
B) Germanium
C) Arsenic
D) Selenium
Answer: A) Gallium
Explanation: The electron configuration [Ar] 3d¹⁰ 4s² 4p¹ corresponds to Gallium (Ga), which is in Group 13.
- Which of the following elements is a member of the actinide series?
A) Uranium
B) Lead
C) Bismuth
D) Thallium
Answer: A) Uranium
Explanation: Uranium (U) is part of the actinide series, which consists of 15 elements from Actinium to Lawrencium.
- Which element is a strong oxidizing agent?
A) Lithium
B) Sodium
C) Chlorine
D) Magnesium
Answer: C) Chlorine
Explanation: Chlorine (Cl₂) is a strong oxidizing agent as it readily accepts electrons during chemical reactions.
- Which of the following elements is the most electropositive?
A) Francium
B) Cesium
C) Potassium
D) Sodium
Answer: A) Francium
Explanation: Francium (Fr) is the most electropositive element, meaning it has the highest tendency to lose electrons and form cations.
- Which of the following elements has the highest atomic number?
A) Krypton
B) Rubidium
C) Strontium
D) Bromine
Answer: A) Krypton
Explanation: Krypton (Kr) has a higher atomic number (36) compared to Rubidium (Rb, 37), Strontium (Sr, 38), and Bromine (Br, 35).
Correction:
Answer: C) Strontium
Explanation: Strontium (Sr) has an atomic number of 38, which is higher than Krypton (Kr, 36), Rubidium (Rb, 37), and Bromine (Br, 35).
- Which of the following elements is a liquid at room temperature?
A) Mercury
B) Gallium
C) Cesium
D) All of the above
Answer: D) All of the above
Explanation: Mercury (Hg) is liquid at room temperature. Gallium (Ga) melts just above room temperature, and Cesium (Cs) has a low melting point making it liquid near room temperature under certain conditions.
- Which of the following elements has the highest electron gain enthalpy?
A) Oxygen
B) Sulfur
C) Chlorine
D) Fluorine
Answer: C) Chlorine
Explanation: Chlorine (Cl) has the highest electron gain enthalpy, meaning it releases the most energy when gaining an electron, despite fluorine being more electronegative.
- Which of the following elements is a solid at room temperature and has metallic properties?
A) Bromine
B) Iodine
C) Mercury
D) Sodium
Answer: D) Sodium
Explanation: Sodium (Na) is a solid metal at room temperature, exhibiting typical metallic properties like conductivity and malleability. Mercury is a liquid, bromine is a liquid, and iodine is a solid nonmetal with different properties.
- Which element has the ground-state electron configuration of [Xe] 4f¹⁴ 5d¹⁰ 6s² 6p³?
A) Bismuth
B) Polonium
C) Antimony
D) Tellurium
Answer: C) Antimony
Explanation: The electron configuration [Xe] 4f¹⁴ 5d¹⁰ 6s² 6p³ corresponds to Antimony (Sb), which is in Group 15.
- Which of the following elements has the highest metallic character?
A) Aluminum
B) Gallium
C) Indium
D) Thallium
Answer: D) Thallium
Explanation: Metallic character increases down a group. Thallium (Tl) is below Aluminum, Gallium, and Indium, making it the most metallic among them.
- Which of the following elements is a chalcogen?
A) Nitrogen
B) Oxygen
C) Carbon
D) Boron
Answer: B) Oxygen
Explanation: Chalcogens are elements in Group 16, which include Oxygen (O), Sulfur (S), Selenium (Se), etc.
- Which of the following elements has the largest metallic radius?
A) Magnesium
B) Calcium
C) Strontium
D) Barium
Answer: D) Barium
Explanation: Metallic radius increases down a group. Barium (Ba) has the largest metallic radius among the listed elements.
- Which of the following elements has the highest number of valence electrons?
A) Boron
B) Carbon
C) Nitrogen
D) Oxygen
Answer: D) Oxygen
Explanation: Oxygen has six valence electrons, which is the highest among the listed elements (Boron – 3, Carbon – 4, Nitrogen – 5).
- Which of the following elements is most likely to form a -2 oxidation state?
A) Sulfur
B) Phosphorus
C) Nitrogen
D) Carbon
Answer: A) Sulfur
Explanation: Sulfur (S) commonly forms a -2 oxidation state by gaining two electrons, especially in compounds like H₂S and SO₃²⁻.
- Which element has the highest melting point?
A) Tungsten
B) Iron
C) Carbon
D) Titanium
Answer: C) Carbon
Explanation: Carbon, in its diamond form, has the highest melting point due to its strong covalent bonding network.
- Which of the following elements is a nonmetal?
A) Nickel
B) Selenium
C) Zinc
D) Gallium
Answer: B) Selenium
Explanation: Selenium (Se) is a nonmetal, whereas Nickel, Zinc, and Gallium are metals.
- Which of the following elements is an example of a p-block metal?
A) Iron
B) Zinc
C) Aluminum
D) Calcium
Answer: C) Aluminum
Explanation: Aluminum (Al) is a p-block metal, located in Group 13. Iron and Zinc are d-block, and Calcium is an s-block metal.
- Which of the following elements has the greatest tendency to form anions?
A) Lithium
B) Fluorine
C) Sodium
D) Magnesium
Answer: B) Fluorine
Explanation: Fluorine (F) has the highest tendency to gain electrons and form F⁻ anions due to its high electronegativity.
- Which of the following elements has the electron configuration [Ne] 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s²?
A) Strontium
B) Zirconium
C) Yttrium
D) Rubidium
Answer: A) Strontium
Explanation: The electron configuration corresponds to Strontium (Sr), which is in Group 2 and Period 5.
- Which of the following elements is a p-block element?
A) Sodium
B) Magnesium
C) Aluminum
D) Potassium
Answer: C) Aluminum
Explanation: Aluminum (Al) is a p-block element located in Group 13. Elements in the p-block have their valence electrons in p-orbitals.
- Which of the following statements is correct regarding the d-block elements?
A) They are also known as alkali metals.
B) They show variable oxidation states.
C) They are nonmetals.
D) They are noble gases.
Answer: B) They show variable oxidation states.
Explanation: d-block elements are transition metals, and they are known for showing variable oxidation states due to the availability of d-electrons for bonding.
- Which of the following is a property of noble gases?
A) High reactivity
B) Low ionization energy
C) High melting points
D) Complete outer electron shells
Answer: D) Complete outer electron shells
Explanation: Noble gases have complete outer electron shells, making them chemically inert and stable, with very low reactivity.
- Which of the following elements is a member of the halogen family?
A) Neon
B) Argon
C) Fluorine
D) Helium
Answer: C) Fluorine
Explanation: Fluorine (F) belongs to Group 17, known as the halogen family. These elements are highly reactive and form salts with metals.
- Which element in Group 1 has the lowest ionization energy?
A) Lithium
B) Sodium
C) Potassium
D) Cesium
Answer: D) Cesium
Explanation: Cesium (Cs) has the lowest ionization energy in Group 1 because it is located furthest down the group, where the outer electron is farthest from the nucleus, making it easier to remove.
- Which of the following statements is true about metalloids?
A) They are excellent conductors of electricity.
B) They are malleable like metals.
C) They have properties of both metals and nonmetals.
D) They are highly reactive with water.
Answer: C) They have properties of both metals and nonmetals.
Explanation: Metalloids have characteristics that are intermediate between metals and nonmetals. They can exhibit both metallic and non-metallic behaviors.
- Which of the following elements is likely to form an ionic compound with chlorine?
A) Sulfur
B) Phosphorus
C) Magnesium
D) Argon
Answer: C) Magnesium
Explanation: Magnesium (Mg) is a metal and tends to lose two electrons to form Mg²⁺ ions, which can combine with Cl⁻ ions to form the ionic compound MgCl₂.
- Which of the following elements is found in the d-block of the periodic table?
A) Oxygen
B) Copper
C) Neon
D) Calcium
Answer: B) Copper
Explanation: Copper (Cu) is a transition metal found in the d-block of the periodic table. It has variable oxidation states and is known for its good electrical conductivity.
- Which of the following elements is a noble gas?
A) Hydrogen
B) Helium
C) Nitrogen
D) Oxygen
Answer: B) Helium
Explanation: Helium (He) is a noble gas with a complete outer electron shell. It is inert and does not easily form compounds.
- Which element has the highest first ionization energy in Group 15?
A) Nitrogen
B) Phosphorus
C) Arsenic
D) Antimony
Answer: A) Nitrogen
Explanation: Nitrogen (N) has the highest first ionization energy among Group 15 elements due to its small atomic size and strong nuclear attraction for its valence electrons.
- Which of the following elements is a member of the actinide series?
A) Lanthanum
B) Uranium
C) Hafnium
D) Yttrium
Answer: B) Uranium
Explanation: Uranium (U) belongs to the actinide series, which includes elements with atomic numbers 89 to 103. These elements are located in the f-block of the periodic table and are radioactive.
- Which of the following elements is most likely to form covalent bonds?
A) Sodium
B) Magnesium
C) Carbon
D) Potassium
Answer: C) Carbon
Explanation: Carbon (C) commonly forms covalent bonds by sharing electrons with other atoms. It has four valence electrons and can form multiple covalent bonds.
- Which element is located in Group 14 and Period 3?
A) Silicon
B) Carbon
C) Germanium
D) Tin
Answer: A) Silicon - Which element in the periodic table has the highest electronegativity?
A) Fluorine
B) Oxygen
C) Chlorine
D) Nitrogen
Answer: A) Fluorine - Which of the following elements has the smallest atomic radius?
A) Potassium
B) Sodium
C) Chlorine
D) Bromine
Answer: C) Chlorine - Which element is a member of the alkali metals?
A) Calcium
B) Sodium
C) Magnesium
D) Aluminum
Answer: B) Sodium - Which element has the electronic configuration [Ne] 3s² 3p¹?
A) Magnesium
B) Aluminum
C) Silicon
D) Phosphorus
Answer: B) Aluminum
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