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Objective Questions

Latest Punjab Lecturer Chemistry Exam Question (Objective Questions), MCQ in English

Subjects : Chemistry

Question Bank Punjab Lecturer Chemistry Exam - English
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Chemistry

Question 1Single Answer
The modern periodic law is based primarily on?
  1. Amass number
  2. Bneutron number
  3. Catomic mass
  4. Datomic number
Question 2Single Answer
Across a period, the effective nuclear charge generally?
  1. Aincreases
  2. Bbecomes zero
  3. Cdecreases
  4. Dremains exactly constant
Question 3Single Answer
Across a period, atomic radius generally?
  1. Aremains constant
  2. Bincreases
  3. Cdecreases
  4. Dfirst becomes infinite
Question 4Single Answer
Down a group, atomic radius generally?
  1. Aremains constant
  2. Bincreases
  3. Cdecreases
  4. Dbecomes zero
Question 5Single Answer
The first ionization enthalpy generally increases across a period because of?
  1. Aincreasing effective nuclear charge
  2. Bincreasing shielding by a new shell
  3. Ccomplete absence of electron-electron repulsion
  4. Ddecreasing nuclear charge
Question 6Single Answer
The first ionization enthalpy generally decreases down a group mainly because of?
  1. Aincreased size and shielding
  2. Bdecreased number of shells
  3. Cincreased effective attraction without shielding
  4. Dloss of all core electrons
Question 7Single Answer
Among alkali metals, the lowest first ionization enthalpy is expected toward the?
  1. Atop of the group
  2. Bbottom of the group
  3. Cmiddle only
  4. Dnoble-gas end of the same period
Question 8Single Answer
A cation is usually smaller than its parent atom because?
  1. Aelectron gain increases shielding
  2. Bneutrons expand the electron cloud
  3. Cthe nucleus loses protons
  4. Delectron loss reduces repulsion and may remove the outer shell
Question 9Single Answer
An anion is usually larger than its parent atom because?
  1. Athe principal quantum number always decreases
  2. Ba proton is removed
  3. Cthe nuclear charge increases
  4. Dadded electron-electron repulsion expands the electron cloud
Question 10Single Answer
In an isoelectronic series, ionic radius decreases as?
  1. Anuclear charge increases
  2. Bnumber of electrons increases
  3. Cprincipal shell number increases
  4. Dnuclear charge decreases
Question 11Single Answer
The most electronegative element on the Pauling scale is?
  1. Anitrogen
  2. Bchlorine
  3. Cfluorine
  4. Doxygen
Question 12Single Answer
Electronegativity generally decreases down a group because?
  1. Aeffective nuclear charge becomes infinite
  2. Bnuclear charge decreases to zero
  3. Cvalence shells disappear
  4. Datomic size and shielding increase
Question 13Single Answer
Electron affinity is most directly associated with?
  1. Aaddition of an electron to a gaseous atom
  2. Baddition of a neutron
  3. Cremoval of an electron from a solid
  4. Dremoval of a proton
Question 14Single Answer
The relatively low electron affinity of fluorine compared with chlorine is largely due to?
  1. Agreater electron-electron repulsion in the compact 2p shell
  2. Bfilled d orbitals in fluorine
  3. Cabsence of nuclear charge in fluorine
  4. Dlarger size of fluorine
Question 15Single Answer
The exceptionally high ionization enthalpy of noble gases is related to?
  1. Aabsence of protons
  2. Bsingle valence electrons
  3. Cstable closed-shell configurations
  4. Dvery large atomic radii
Question 16Single Answer
The first ionization enthalpy of Be is higher than that of B mainly because Be has?
  1. Aa filled 2p subshell
  2. Ba filled 2s subshell
  3. Cone fewer proton
  4. Da larger atomic radius
Question 17Single Answer
The first ionization enthalpy of N is higher than that of O mainly because N has?
  1. Aa half-filled 2p subshell
  2. Ba filled 2p subshell
  3. Ca larger principal shell
  4. Dno p electrons
Question 18Single Answer
Lanthanide contraction arises mainly from?
  1. Aloss of all 5d electrons
  2. Bpoor shielding by 4f electrons
  3. Cdecreasing nuclear charge
  4. Dexcellent shielding by 4f electrons
Question 19Single Answer
Diagonal relationship is especially prominent between?
  1. AF and Cl
  2. BBe and Mg
  3. CLi and Mg
  4. DLi and Na
Question 20Single Answer
The inert-pair effect becomes more important down the p-block because?
  1. Athe ns2 pair becomes less available for bonding
  2. Bp orbitals vanish
  3. Celectronegativity always increases
  4. Dall valence electrons become unpaired
Question 21Single Answer
The metallic character generally increases?
  1. Adown a group
  2. Bwith increasing ionization enthalpy
  3. Ctoward fluorine
  4. Dacross a period from left to right
Question 22Single Answer
The nonmetallic character generally increases?
  1. Aacross a period from left to right
  2. Bwith decreasing electronegativity
  3. Cdown alkali-metal group
  4. Dwith increasing atomic radius
Question 23Single Answer
A large jump between successive ionization enthalpies usually indicates?
  1. Aelectron affinity has become positive
  2. Bthe atom has become neutral again
  3. Cnuclear charge has decreased
  4. Dremoval has begun from an inner closed shell
Question 24Single Answer
Slater's rules are used to estimate?
  1. Amolecular symmetry only
  2. Bnuclear spin
  3. Cbond order directly
  4. Dshielding and effective nuclear charge
Question 25Single Answer
The shielding ability of subshells of the same principal shell generally follows?
  1. Ad > s > p > f
  2. Bp > s > f > d
  3. Cs > p > d > f
  4. Df > d > p > s
Question 26Single Answer
The radius commonly assigned to nonbonded atoms in neighboring molecules is the?
  1. Avan der Waals radius
  2. Bcovalent radius
  3. CBohr magneton
  4. Dmetallic radius
Question 27Single Answer
Covalent radius is commonly defined from?
  1. Aelectron affinity
  2. Bhalf the distance between ions in any crystal
  3. Chalf the internuclear distance between identical covalently bonded atoms
  4. Dthe nuclear diameter
Question 28Single Answer
The smallest species among O2-, F-, Na+, and Mg2+ is?
  1. ANa+
  2. BF-
  3. CMg2+
  4. DO2-
Question 29Single Answer
The largest species among N3-, O2-, F-, and Na+ is?
  1. AO2-
  2. BNa+
  3. CF-
  4. DN3-
Question 30Single Answer
The anomalous behavior of second-period elements is strongly related to?
  1. Aabsence of p orbitals
  2. Bvery large size and filled d shells
  3. Csmall size and absence of low-lying d orbitals
  4. Dzero electronegativity
Question 31Single Answer
The maximum covalency shown by second-period elements is limited mainly by?
  1. Alack of accessible d orbitals in the valence shell
  2. Black of s orbitals
  3. Ccomplete shielding
  4. Dabsence of nuclear charge
Question 32Single Answer
The tendency to form multiple pĪ€-pĪ€ bonds is strongest for?
  1. Asecond-period elements
  2. Blanthanides only
  3. Calkali metals only
  4. Dheaviest p-block elements
Question 33Single Answer
The electropositive character is greatest toward the?
  1. Alower-left region of the periodic table
  2. Btop of halogen group
  3. Ccenter of noble-gas group
  4. Dupper-right region
Question 34Single Answer
The electron-gain tendency is generally strongest toward the?
  1. Aupper-right region excluding noble gases
  2. Bmiddle of alkali group
  3. Clanthanide series only
  4. Dlower-left region
Question 35Single Answer
A species with a higher effective nuclear charge on the same shell generally has?
  1. Azero ionization energy
  2. Ba smaller radius
  3. Cthe same radius necessarily
  4. Da larger radius
Question 36Single Answer
The second ionization enthalpy of an alkali metal is very high because it removes an electron from?
  1. Aa noble-gas core
  2. Ba newly added anion orbital
  3. Ca diffuse d orbital
  4. Da singly occupied valence s orbital
Question 37Single Answer
Which option correctly completes the statement: The modern periodic law is based primarily on?
  1. Aneutron number
  2. Batomic mass
  3. Catomic number
  4. Dmass number
Question 38Single Answer
Which option correctly completes the statement: Across a period, the effective nuclear charge generally?
  1. Aremains exactly constant
  2. Bincreases
  3. Cbecomes zero
  4. Ddecreases
Question 39Single Answer
Which option correctly completes the statement: Across a period, atomic radius generally?
  1. Aremains constant
  2. Bdecreases
  3. Cfirst becomes infinite
  4. Dincreases
Question 40Single Answer
Which option correctly completes the statement: Down a group, atomic radius generally?
  1. Adecreases
  2. Bremains constant
  3. Cbecomes zero
  4. Dincreases
Question 41Single Answer
Which option correctly completes the statement: The first ionization enthalpy generally increases across a period because of?
  1. Aincreasing shielding by a new shell
  2. Bcomplete absence of electron-electron repulsion
  3. Cdecreasing nuclear charge
  4. Dincreasing effective nuclear charge
Question 42Single Answer
Which option correctly completes the statement: The first ionization enthalpy generally decreases down a group mainly because of?
  1. Aincreased effective attraction without shielding
  2. Bloss of all core electrons
  3. Cdecreased number of shells
  4. Dincreased size and shielding
Question 43Single Answer
Which option correctly completes the statement: Among alkali metals, the lowest first ionization enthalpy is expected toward the?
  1. Anoble-gas end of the same period
  2. Bbottom of the group
  3. Ctop of the group
  4. Dmiddle only
Question 44Single Answer
Which option correctly completes the statement: A cation is usually smaller than its parent atom because?
  1. Aneutrons expand the electron cloud
  2. Bthe nucleus loses protons
  3. Celectron loss reduces repulsion and may remove the outer shell
  4. Delectron gain increases shielding
Question 45Single Answer
Which option correctly completes the statement: An anion is usually larger than its parent atom because?
  1. Athe principal quantum number always decreases
  2. Badded electron-electron repulsion expands the electron cloud
  3. Ca proton is removed
  4. Dthe nuclear charge increases
Question 46Single Answer
Which option correctly completes the statement: In an isoelectronic series, ionic radius decreases as?
  1. Anuclear charge decreases
  2. Bprincipal shell number increases
  3. Cnuclear charge increases
  4. Dnumber of electrons increases
Question 47Single Answer
Which option correctly completes the statement: The most electronegative element on the Pauling scale is?
  1. Achlorine
  2. Bnitrogen
  3. Coxygen
  4. Dfluorine
Question 48Single Answer
Which option correctly completes the statement: Electronegativity generally decreases down a group because?
  1. Aatomic size and shielding increase
  2. Bnuclear charge decreases to zero
  3. Cvalence shells disappear
  4. Deffective nuclear charge becomes infinite
Question 49Single Answer
Which option correctly completes the statement: Electron affinity is most directly associated with?
  1. Aremoval of an electron from a solid
  2. Bremoval of a proton
  3. Caddition of an electron to a gaseous atom
  4. Daddition of a neutron
Question 50Single Answer
Which option correctly completes the statement: The relatively low electron affinity of fluorine compared with chlorine is largely due to?
  1. Aabsence of nuclear charge in fluorine
  2. Blarger size of fluorine
  3. Cfilled d orbitals in fluorine
  4. Dgreater electron-electron repulsion in the compact 2p shell
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