Periodic Table and Periodic Properties Competitive Exams
100 questions · General Science
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Question 1 of 100
Group 11 of the periodic table includes which of the following 'coinage metals'?
ExplanationGroup 11 contains copper, silver, and gold, historically called 'coinage metals' due to their use in coins and jewelry.
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Question 2 of 100
According to Fajans' rules, covalent character in an ionic bond increases with:
ExplanationFajans' rules state that greater covalent character arises from smaller, highly charged cations and larger, more polarizable anions.
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Question 3 of 100
As you move across a period from left to right, ionization energy generally:
ExplanationIonization energy increases across a period due to increasing nuclear charge, making electron removal more difficult.
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Question 4 of 100
Which of the following elements is a representative (main group) element?
ExplanationSodium (group 1, s-block) is a representative element; iron, copper, and zinc belong to the d-block (transition metals or related).
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Question 5 of 100
Within the same period, which type of element generally shows the highest ionization energy?
ExplanationNoble gases, at the far right of a period, have the highest ionization energies due to their stable, complete valence shells and high effective nuclear charge.
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Question 6 of 100
How many periods are there in the modern periodic table?
ExplanationThe modern periodic table has 7 horizontal periods.
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Question 7 of 100
Who is known as the father of the modern periodic table?
ExplanationDmitri Mendeleev arranged elements by increasing atomic mass and recognized periodic recurrence of properties, creating the first widely accepted periodic table in 1869.
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Question 8 of 100
Mendeleev left gaps in his periodic table to:
ExplanationMendeleev left gaps for undiscovered elements, successfully predicting properties of elements like gallium and germanium before their discovery.
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Question 9 of 100
The periodic table's 'lanthanide contraction' refers to the:
ExplanationLanthanide contraction is the unusually large decrease in atomic and ionic radii across the lanthanide series due to poor shielding by 4f electrons.
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Question 10 of 100
Which of these elements is a nonmetal?
ExplanationOxygen is a nonmetal; iron, copper, and sodium are metals.
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Question 11 of 100
As you move down a group, ionization energy generally:
ExplanationIonization energy decreases down a group since valence electrons are farther from the nucleus and more shielded, making them easier to remove.
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Question 12 of 100
Which periodic property determines how 'willing' an atom is to form a negative ion?
ExplanationHigh (more negative) electron affinity indicates an atom readily gains electrons to form negative ions (anions).
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Question 13 of 100
The element with atomic number 11 is:
ExplanationSodium has atomic number 11, a reactive alkali metal.
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Question 14 of 100
Non-metallic character generally __________ across a period (left to right).
ExplanationNon-metallic character increases across a period as elements gain more valence electrons and higher electronegativity.
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Question 15 of 100
Group 16 elements of the periodic table are often called:
ExplanationGroup 16 elements (O, S, Se, Te) are called chalcogens, meaning 'ore-forming' elements.
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Question 16 of 100
Acidic oxides are typically formed by:
ExplanationNonmetal oxides are generally acidic, reacting with bases to form salts and water.
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Question 17 of 100
Most elements in the periodic table are classified as:
ExplanationThe majority of elements in the periodic table (over 80%) are metals, located on the left and center of the table.
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Question 18 of 100
The element with atomic number 1 is:
ExplanationHydrogen has atomic number 1, the simplest and lightest element.
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Question 19 of 100
Why are noble gases generally unreactive?
ExplanationNoble gases have fully filled valence shells, making them energetically stable and resistant to forming bonds.
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Question 20 of 100
The element with atomic number 8 is:
ExplanationOxygen has atomic number 8, essential for respiration and combustion.
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Question 21 of 100
Which of the following best explains why electronegativity increases across a period despite electron shielding being roughly constant?
ExplanationAcross a period, nuclear charge increases while shielding from inner electrons stays roughly constant, so the increased effective nuclear charge attracts bonding electrons more strongly, raising electronegativity.
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Question 22 of 100
Döbereiner's Law of Triads grouped elements in sets of:
ExplanationDöbereiner observed that in certain triads of elements, the atomic mass of the middle element was approximately the average of the other two.
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Question 23 of 100
Covalent radius is best described as:
ExplanationCovalent radius is defined as half the internuclear distance between two identical atoms joined by a single covalent bond.
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Question 24 of 100
The s-block of the periodic table consists of groups:
ExplanationThe s-block comprises Group 1 (alkali metals) and Group 2 (alkaline earth metals), where the last electron enters an s orbital.
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Question 25 of 100
The modern periodic table arranges elements in order of increasing:
ExplanationHenry Moseley's work established that atomic number, not atomic mass, is the basis of periodicity in the modern periodic table.
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Question 26 of 100
As you move across a period from left to right, electronegativity generally:
ExplanationElectronegativity increases across a period due to increasing nuclear charge and decreasing atomic radius.
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Question 27 of 100
Successive ionization energies of an atom (1st, 2nd, 3rd, etc.) generally:
ExplanationEach successive ionization requires removing an electron from an increasingly positive ion with reduced electron shielding, so successive ionization energies increase.
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Question 28 of 100
The anomaly where Group 15 elements have higher ionization energy than adjacent Group 16 elements is due to:
ExplanationGroup 15 elements have a half-filled np³ configuration, which is more stable (due to exchange energy) and harder to ionize than Group 16's np⁴ configuration.
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Question 29 of 100
Period 6 of the periodic table contains how many elements (including lanthanides)?
ExplanationPeriod 6 contains 32 elements, including the lanthanide series, as it incorporates s, p, d, and f subshells.
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Question 30 of 100
Elements in groups 3 to 12 of the periodic table are called:
ExplanationGroups 3-12 are collectively called transition metals (or transition elements), known for variable oxidation states and colored compounds.
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Question 31 of 100
The term 'amphoteric oxide' refers to an oxide that can react with:
ExplanationAmphoteric oxides (like aluminum oxide) can react with both acids and bases, showing dual acidic and basic character, typical of elements near the metal-nonmetal boundary.
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Question 32 of 100
The f-block elements of the periodic table are positioned:
ExplanationTo keep the table compact, the f-block elements (lanthanides and actinides) are placed separately below the main table.
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Question 33 of 100
Elements with low ionization energy and low electronegativity are generally classified as:
ExplanationMetals typically have low ionization energy (easily lose electrons) and low electronegativity (weak pull on shared electrons).
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Question 34 of 100
Which of the following statements about Group 12 elements (Zn, Cd, Hg) is correct?
ExplanationZinc, cadmium, and mercury have completely filled d¹⁰ configurations in their common oxidation states, so some chemists exclude them from the strict definition of transition metals.
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Question 35 of 100
As you move down a group, electronegativity generally:
ExplanationElectronegativity decreases down a group as atomic radius increases and the nucleus's pull on shared electrons weakens.
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Question 36 of 100
Within the same period, which type of element generally shows the lowest ionization energy?
ExplanationAlkali metals, at the far left of a period, have the lowest ionization energies since they readily lose their single valence electron.
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Question 37 of 100
Lanthanides and actinides are collectively known as:
ExplanationLanthanides and actinides, found below the main table, are called inner transition elements or f-block elements, as they fill f subshells.
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Question 38 of 100
Elements with high ionization energy and high electronegativity are generally classified as:
ExplanationNonmetals typically have high ionization energy (hold onto electrons tightly) and high electronegativity (strongly attract shared electrons).
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Question 39 of 100
The periodic trend where oxide character changes from basic to acidic across a period reflects a change in:
ExplanationAs metallic character decreases across a period, oxides change from basic (metal oxides) to amphoteric to acidic (nonmetal oxides).
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Question 40 of 100
Which periodic property determines how 'willing' an atom is to form a positive ion?
ExplanationLow ionization energy indicates an atom readily loses electrons to form positive ions (cations).
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Question 41 of 100
Metallic character generally __________ across a period (left to right) and __________ down a group.
ExplanationMetallic character decreases across a period (elements become more nonmetallic) and increases down a group (elements become more metallic).
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Question 42 of 100
Elements in the same group of the periodic table have the same number of:
ExplanationElements within the same group share the same number of valence electrons, giving them similar chemical properties.
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Question 43 of 100
Which of the following elements is the most reactive metal (among common alkali metals)?
ExplanationReactivity of alkali metals increases down the group; Francium (and Cesium among commonly studied) is the most reactive due to its very low ionization energy.
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Question 44 of 100
Group 1 elements of the periodic table are called:
ExplanationGroup 1 elements (Li, Na, K, etc.) are known as alkali metals, highly reactive with a single valence electron.
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Question 45 of 100
Electron affinity is defined as the energy change when a gaseous atom:
ExplanationElectron affinity is the energy released (or sometimes absorbed) when a neutral gaseous atom gains an electron to form an anion.
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Question 46 of 100
Which of the following best describes the trend in reactivity of halogens down the group?
ExplanationReactivity of halogens decreases down the group as atomic size increases and electron affinity becomes less negative, making electron gain less favorable.
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Question 47 of 100
A large jump between successive ionization energies indicates:
ExplanationA large jump in ionization energy signals that the next electron being removed comes from a lower, more stable, completely filled shell, requiring much more energy.
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Question 48 of 100
Cationic radius compared to its parent atom's radius is always:
ExplanationCations are smaller than their parent atoms because losing electrons reduces electron-electron repulsion and often removes an entire shell.
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Question 49 of 100
The element with the highest number of naturally occurring elements belongs to which block?
ExplanationThe d-block, containing the transition metals, has the largest number of naturally occurring elements among the blocks.
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Question 50 of 100
Elements in the same period of the periodic table have the same number of:
ExplanationElements across a period have the same number of electron shells, though valence electrons increase left to right.
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Question 51 of 100
Which of the following correctly ranks ionization energies in increasing order (smallest to largest)?
ExplanationIonization energy increases across period 3, so the order from smallest to largest among these is Na < Mg < Cl.
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Question 52 of 100
How many groups are there in the modern periodic table?
ExplanationThe modern periodic table has 18 vertical groups (columns).
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Question 53 of 100
Which of the following is a diagonal relationship in the periodic table?
ExplanationDiagonal relationships occur between elements of period 2 and period 3 diagonally adjacent, e.g., Li (group 1) resembles Mg (group 2) due to similar charge density.
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Question 54 of 100
Which group of the periodic table contains elements that are generally liquid, solid, and gas at room temperature (halogens)?
ExplanationGroup 17 (halogens) shows varied physical states at room temperature: fluorine and chlorine are gases, bromine is liquid, and iodine is solid.
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Question 55 of 100
Which scientist's work on X-ray spectra led to the correction of Mendeleev's table based on atomic number?
ExplanationHenry Moseley's X-ray spectroscopy studies established atomic number as the true basis for periodicity, correcting inconsistencies in Mendeleev's mass-based table.
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Question 56 of 100
Which periodic property is primarily responsible for the exceptional stability of noble gas electron configurations?
ExplanationA completely filled valence shell (octet rule, or duet for helium) provides exceptional electronic stability, explaining noble gases' inertness.
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Question 57 of 100
Group 17 elements of the periodic table are called:
ExplanationGroup 17 elements (F, Cl, Br, I) are called halogens, meaning 'salt-formers', as they react with metals to form salts.
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Question 58 of 100
A major limitation of Mendeleev's periodic table was that it was based on:
ExplanationMendeleev's table used atomic mass, causing some elements to be misplaced since atomic number (unknown at the time) is the true basis of periodicity.
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Question 59 of 100
Which period of the periodic table contains only 2 elements?
ExplanationPeriod 1 contains only Hydrogen and Helium, as the first shell (n=1) can hold a maximum of 2 electrons.
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Question 60 of 100
Hydrogen is often placed uniquely in the periodic table because it:
ExplanationHydrogen has one valence electron (like alkali metals) but can also gain one electron to complete its shell (like halogens), giving it a unique dual position.
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Question 61 of 100
As you move down a group, atomic radius generally:
ExplanationAtomic radius increases down a group as additional electron shells are added, increasing the distance from nucleus to outer electrons.
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Question 62 of 100
Another classic example of a diagonal relationship is between:
ExplanationBeryllium (group 2) shows a diagonal relationship with Aluminum (group 13), sharing similar amphoteric properties.
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Question 63 of 100
Newlands' Law of Octaves stated that every eighth element had properties similar to the:
ExplanationNewlands observed that when elements were arranged by increasing atomic mass, every eighth element showed properties similar to the first, akin to musical octaves.
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Question 64 of 100
Basic oxides are typically formed by:
ExplanationMetal oxides are generally basic, reacting with acids to form salts and water.
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Question 65 of 100
The d-block of the periodic table consists of groups:
ExplanationThe d-block, containing transition metals, spans groups 3 to 12, where the last electron enters a d orbital.
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Question 66 of 100
The anomaly where Group 2 elements have higher ionization energy than adjacent Group 13 elements is due to:
ExplanationGroup 2 elements have a fully filled ns² subshell, which is more stable and harder to ionize than Group 13's ns²np¹ configuration, despite Group 13 having one more proton.
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Question 67 of 100
The p-block of the periodic table consists of groups:
ExplanationThe p-block comprises groups 13 to 18, where the last electron enters a p orbital.
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Question 68 of 100
Which of the following elements is the most reactive nonmetal?
ExplanationFluorine is the most reactive nonmetal due to its small size and very high electronegativity, readily gaining electrons.
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Question 69 of 100
The periodic property 'polarizing power' of a cation increases with:
ExplanationAccording to Fajans' rules, a cation's polarizing power (ability to distort an anion's electron cloud) increases with smaller ionic size and higher charge density.
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Question 70 of 100
Noble gases are generally characterized by:
ExplanationNoble gases have complete outer electron shells, making them largely chemically inert.
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Question 71 of 100
Which of the following elements would likely form an amphoteric oxide, based on its position near the metal-nonmetal boundary?
ExplanationAluminum, located near the metalloid staircase, forms the amphoteric oxide Al₂O₃, reacting with both acids and bases.
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Question 72 of 100
Which of the following best explains why transition metal compounds are often colored?
ExplanationPartially filled d orbitals allow electron transitions that absorb specific wavelengths of visible light, producing colored compounds.
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Question 73 of 100
As you move across a period from left to right, atomic radius generally:
ExplanationAtomic radius decreases across a period due to increasing nuclear charge pulling electrons closer, with electrons added to the same shell.
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Question 74 of 100
Group 15 elements of the periodic table are often called:
ExplanationGroup 15 elements (N, P, As, etc.) are called pnictogens.
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Question 75 of 100
Which element generally has the largest atomic radius?
ExplanationFrancium (and Cesium) have among the largest atomic radii, being located in the bottom-left of the periodic table where atoms are large and loosely held.
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Question 76 of 100
The term 'periodic property' refers to a property that:
ExplanationPeriodic properties (like atomic radius, ionization energy) exhibit regular, repeating trends across periods and down groups, underlying the structure of the periodic table.
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Question 77 of 100
Which trend correctly describes the general change in melting point across period 3 (Na to Ar)?
ExplanationMelting points rise toward silicon (strong covalent network) then drop sharply for molecular/monatomic nonmetals (P, S, Cl, Ar) with weaker intermolecular forces.
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Question 78 of 100
Which periods of the periodic table contain 18 elements each?
ExplanationPeriods 4 and 5 contain 18 elements each, as they include the d-block (transition metals) in addition to s and p blocks.
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Question 79 of 100
As you move across a period from left to right, electron affinity generally becomes:
ExplanationElectron affinity generally becomes more negative across a period as atoms more readily attract additional electrons due to increasing nuclear charge.
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Question 80 of 100
Which of the following correctly ranks atomic radii in increasing order (smallest to largest)?
ExplanationAtomic radius decreases across period 2 from left to right, so Nitrogen > Oxygen > Fluorine, meaning increasing order is F < O < N.
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Question 81 of 100
Elements are broadly classified into metals, nonmetals, and:
ExplanationMetalloids (like silicon, boron) have properties intermediate between metals and nonmetals.
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Question 82 of 100
Anionic radius compared to its parent atom's radius is always:
ExplanationAnions are larger than their parent atoms because gaining electrons increases electron-electron repulsion, causing the electron cloud to expand.
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Question 83 of 100
Transition metals are known for exhibiting multiple:
ExplanationTransition metals commonly exhibit variable oxidation states due to the involvement of both s and d electrons in bonding.
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Question 84 of 100
Which group generally has the most negative (highest magnitude) electron affinities?
ExplanationHalogens have a strong tendency to gain one electron to achieve a stable noble gas configuration, giving them highly negative electron affinities.
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Question 85 of 100
The term 'periodicity' in chemistry refers to the:
ExplanationPeriodicity describes how certain physical and chemical properties recur periodically as atomic number increases, forming the basis of the periodic table's structure.
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Question 86 of 100
Which periods of the periodic table contain 8 elements each?
ExplanationPeriods 2 and 3 each contain 8 elements, filling s and p subshells without d orbitals being involved yet.
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Question 87 of 100
The element with atomic number 6 is:
ExplanationCarbon has atomic number 6, forming the basis of organic chemistry.
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Question 88 of 100
The 'effective nuclear charge' experienced by an electron is the net positive charge felt after accounting for:
ExplanationEffective nuclear charge is the actual positive charge experienced by an electron, reduced from the full nuclear charge due to shielding by inner electrons.
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Question 89 of 100
Which element has the smallest atomic radius in the periodic table?
ExplanationHelium has the smallest atomic radius, as its two electrons are held very tightly by its small, highly charged nucleus relative to its size.
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Question 90 of 100
Actinides are generally characterized by being:
ExplanationAll actinide elements are radioactive, with many being synthetic and having very short half-lives.
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Question 91 of 100
Which periodic property is generally used to explain why metals conduct electricity well?
ExplanationMetals have low ionization energies, meaning their valence electrons are loosely held and free to move, enabling electrical conductivity.
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Question 92 of 100
The element with atomic number 17 is:
ExplanationChlorine has atomic number 17, a reactive halogen.
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Question 93 of 100
Which element is considered the most electronegative on the Pauling scale?
ExplanationFluorine has the highest electronegativity (about 4.0 on the Pauling scale) of all elements.
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Question 94 of 100
Group 2 elements of the periodic table are called:
ExplanationGroup 2 elements (Be, Mg, Ca, etc.) are known as alkaline earth metals, having two valence electrons.
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Question 95 of 100
Group 18 elements of the periodic table are called:
ExplanationGroup 18 elements (He, Ne, Ar, etc.) are called noble gases, characterized by their general chemical inertness due to complete valence shells.
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Question 96 of 100
Isoelectronic species (same number of electrons) with higher nuclear charge (more protons) have:
ExplanationAmong isoelectronic species, higher nuclear charge pulls the same number of electrons closer, resulting in a smaller radius.
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Question 97 of 100
Which of the following best describes the trend in reactivity of alkali metals down the group?
ExplanationReactivity of alkali metals increases down the group as ionization energy decreases, making it easier to lose the valence electron.
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Question 98 of 100
Ionization energy is defined as the energy required to:
ExplanationIonization energy is the minimum energy needed to remove the most loosely bound electron from an isolated gaseous atom.
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Question 99 of 100
Which of these elements is a metalloid?
ExplanationSilicon is a metalloid, exhibiting properties intermediate between metals and nonmetals, widely used in semiconductors.
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Question 100 of 100
Electronegativity is defined as the tendency of an atom to:
ExplanationElectronegativity measures an atom's ability to attract the shared pair of electrons in a covalent bond towards itself.
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