Free Periodic Properties and Trends MCQs with Answers
606 Periodic Properties and Trends MCQs from Chemistry, each with the correct answer and a written explanation of why it is correct. Free and unlimited, with no account needed.
Periodic properties arise from electron configuration and effective nuclear charge, producing trends in atomic and ionic radius, ionization energy, electron affinity, electronegativity, metallic character and reactivity. Comparisons run across periods and down groups, with attention to common exceptions. The topic also relates these trends to the behavior of s-block and p-block elements.
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606 questions · page 16 of 31
- A. Decrease in atomic radius from 'Si' to 'P'
- B. Change in bonding and structure of two elements
- C. Different universities of two elements
- D. Increase in electron density from 'Si' to 'P'
Explanation: From Si onwards, the bonding and structure of the element change from covalent to weak van der Waal forces that cause the decrease in…
Correct answer: Change in bonding and structure of two elements- A. Melting and boiling points first decrease then increase
- B. Melting and boiling points increase gradually
- C. Melting and boiling points first increase then decrease
- D. Melting and boiling points decrease gradually
Explanation: In general, the melting point increases across a period up to group 14 and then decreases from group 14 to group 18.From sodium to…
Correct answer: Melting and boiling points first increase then decrease- A. Increase in number of electrons in valence shells
- B. Increase in number of protons in the nucleus
- C. Decrease in number of shells
- D. Increase in number of shells
Explanation: Along a period, the number of shells increases (electrons are added to the same principal energy level), and the atomic number increases.
Correct answer: Increase in number of protons in the nucleus- A. The s-block elements
- B. The p-block elements
- C. The d and f block elements
- D. None of the blocks
Explanation: In the case of d-block elements due to the presence of electrons at d orbitals, is closer to the outermost shell of the metal.
Correct answer: The d and f block elements- A. 18
- B. 8
- C. 32
- D. 10
Explanation: Second and third period are called short periods and contain eight elements.The third period contains eight elements: sodium, magnesium…
Correct answer: 8- A. Shielding effect
- B. Transition effect
- C. Intervening effect
- D. Electronic effect
Explanation: The screening effect is also known as the "shielding effect" If the electron shells are wider in space, the interaction between the…
Correct answer: Shielding effect- A. Electronegativity
- B. Electropositivity
- C. Ionisation energy
- D. electron affinity
Explanation: Ionization energy, also called ionization potential, is the amount of energy required to remove one mol of electron from an isolated atom…
Correct answer: Ionisation energy- A. 18 elements each
- B. 32 elements each
- C. 8 elements each
- D. 14 elements each
Explanation: Fact.The 2nd-period elements: lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine, and neon.
Correct answer: 8 elements each- A. s
- B. d
- C. p
- D. f
Explanation: S orbital has only 1 orbital and is defined by letter S.
Correct answer: s- A. V is more reactive than Y
- B. W has more metallic character than Y
- C. Y has a lower melting point than V
- D. Option a and c both are correct
Explanation: the melting points of Group I elements (alkali metals) decrease as you move down the group.
Correct answer: Y has a lower melting point than V- A. V is more reactive than Y
- B. W has more metallic character than V
- C. Y has a lower melting point than V
- D. Z is more reactive than X
Explanation: A. Reactivity for metals increases down the group so V is less reactive than Y which is below V.B.
Correct answer: Y has a lower melting point than V- A. The number of electrons used in bonding
- B. The number of electron shells
- C. The atomic number
- D. The atomic mass
Explanation: The correct answer is Option A: 'The number of electrons used in bonding'.
Correct answer: The number of electrons used in bonding- A. Potassium and Calcium
- B. Sodium and Magnesium
- C. Cesium and Barium
- D. Lithium and Beryllium
Explanation: Because of small size and high charge density, the first member of every group differs from the rest of members of same group.
Correct answer: Lithium and Beryllium- A. Sulphur has strong vander waal forces
- B. Sulphur has weak vander waal forces
- C. Phosphorous has strong vander waals forces
- D. None of these.
Explanation: Sulfur molecules have a larger number of electrons compared to phosphorus, leading to stronger van der Waals forces, which result in a…
Correct answer: Sulphur has strong vander waal forces- A. Li
- B. Na
- C. K
- D. Rb
Explanation: When Lithium is heated in air it only forms Li2O which is a normal oxide as it contains an O2- ion.
Correct answer: Li- A. Be
- B. Cs
- C. Ca
- D. K
Explanation: Option A is correct as Beryllium is one of the 2 alkaline earth metals that does not impart colour to flame test.
Correct answer: Be- A. CaO
- B. BaO2
- C. Na2O2
- D. RbO2
Explanation: Option D is correct. In superoxides oxygen has a charge of -1/2 which is the case in option D.
Correct answer: RbO2- A. Na
- B. Mg
- C. Cs
- D. K
Explanation: The metallic character of elements increases down a group (column) in the periodic table.
Correct answer: Cs- A. Solid state
- B. Liquid state
- C. Crystalline form
- D. Condensed form
Explanation: At room temperature and atmospheric pressure, chlorine (Cl2) is a yellow-green gas, while bromine (Br2) is a reddish-brown liquid.
Correct answer: Liquid state- A. Metal of II-A group
- B. Metalloid of V-A group
- C. Non-metal of VII-A group
- D. Non-metal of V-A group
Explanation: The electronic configuration [Ne] 5s2 5p5 indicates that the unknown element has:- A noble gas core (Ne)- 2 electrons in the 5s orbital- 5…
Correct answer: Non-metal of VII-A group