Chemistry 9 Chapter 3 MCQs Tests by admin | Class 9 MCQs Tests | 0 comments In this post, we have prepared 4 MCQs tests of Federal Board Chemistry 9 Chapter 3 MCQs Tests. For more Class 9 Chemistry MCQs Tests visit this page. Chemistry 9 Chapter 3 MCQs Tests Practice MCQs Test No 1 8 Class 9 Chemistry Chapter 3 Practice MCQs Test No 1 1 / 20 The elements of Group VIIA are called: Alkaline earth metals Alkali metals Noble gases Halogens 2 / 20 First _____ periods are called short periods. 3 4 2 5 3 / 20 Atomic number was discovered by: Mendeleev John Newland Moseley Neil Bohr 4 / 20 The Group VIIIA elements are called: Halogens Noble gases Alkaline earth metals Alkali metals 5 / 20 The horizontal rows of the periodic table are called: Groups Lenthanides Periods Actinides 6 / 20 Group A elements are called: All of these Main group elements Normal elements Representative elements 7 / 20 Metallic elements in Group 1A are called: Noble gases Alkali metals Halogens Alkaline earth metals 8 / 20 The atomic number was discovered in: 1906 1913 1900 1918 9 / 20 Elements are arranged in the order of increasing: Atomic mass Neutron number Nucleon number Atomic number 10 / 20 By 1925, ____ elements were known. 109 23 65 88 11 / 20 Last _____ periods are long periods. 4 5 2 3 12 / 20 Group B elements are called: Transition elements Representative elements Normal elements Main Group elements 13 / 20 Number of periods in the Periodic table are: 6 7 9 8 14 / 20 A table showing systematic arrangement of elements is called: Periods Groups Elements table Periodic table 15 / 20 Elements with similar valance shell electronic configuration are placed in the same: Block Period Group List 16 / 20 By the end of 18th century, _______ elements were known. 23 65 109 88 17 / 20 Elements of Group IA and Group IIA contain their valence electrons in: s sub-shell p sub-shell f sub-shell d sub-shell 18 / 20 Group IIA elements are called: Alkali metals Noble gases Alkaline earth metals Halogens 19 / 20 Each vertical column of elements in the periodic table is called a: group or family family group period 20 / 20 On the basis of outermost valence sub-shell, elements in the periodic table can also be classified into: 8 groups 4 blocks 7 blocks 6 blocks Your score is The average score is 52% LinkedIn Facebook Twitter VKontakte 0% Restart quiz Practice MCQs Test No 2 6 Class 9 Chemistry Chapter 3 Practice MCQs Test 2 1 / 20 The elements of Group IIIA to VIIIA (except He) are known as: p – block elements s – block elements d – block elements f – block elements 2 / 20 The horizontal rows in a periodic table are known as _____. Groups Rows Columns Periods 3 / 20 Element having configuration 1s2 belongs to group: 8A 2A 1A 6A 4 / 20 The elements of B-group are called _____. Halogens Alkaline Earth metals Alkali metals and alkaline earth metals Transition elements 5 / 20 The number of electrons in the valence shell of halogens are _____. 2 7 4 5 6 / 20 ____________ of element indicates n value of the valence shell. Group number Block number Period number Atomic number 7 / 20 Elements in the same vertical group of the periodic table have same _____. Number of valence electrons Atomic Mass (A) Atomic Number (Z) Avogadro's number 8 / 20 Valence shell configuration of Na is: 1s2 , 2s2, 2p6, 3s1 2p6 , 3s1 3s1 2s2 , 2p6 9 / 20 Across a period (left to right), shielding effect _____. remains constant becomes zero increases decreases 10 / 20 What is the period number of Nitrogen -7 ? 4 3 2 1 11 / 20 Which of the elements are not p-block representative elements? Halogens Alkali metals Group V-A Noble gases 12 / 20 The number of elements in the first period is _____. 18 2 8 32 13 / 20 Physical properties depend on the: Sizes of atoms Valence shell electronic configuration Electronic configuration Number of neutrons 14 / 20 John Newland found the similarity in properties of every ________ element. 4 6 8 10 15 / 20 The number of electrons in the valence shell of alkali metals is _____ 4 2 5 1 16 / 20 Chemical properties depend on the: first shell electronic configuration Number of neutrons Atomic mass valence shell electronic configuration 17 / 20 Which of the following has the lowest shielding effect? Be Ca Rb Mg 18 / 20 Which of the following has the highest shielding effect? Br F I Cl 19 / 20 Because all the elements of a particular group have similar valence shell electronic configuration, they possess similar: Chemical properties Number of shells Number of neutrons Physical properties 20 / 20 __________ of element indicates the number of electrons in the valence shell. Block number Group number Period number Atomic mass Your score is The average score is 53% LinkedIn Facebook Twitter VKontakte 0% Restart quiz Practice MCQs Test No 3 /15 5 Class 9 Chemistry Chapter 3 Practice MCQs Test No 3 1 / 15 The number of elements in the first period is _____. 2 32 18 8 2 / 15 Element having configuration 1s2 belongs to group 6A 8A 2A 1A 3 / 15 Which of the following has the lowest shielding effect? Rb Mg Be Ca 4 / 15 What is the period number of Nitrogen -7 ? 3 4 1 2 5 / 15 Atomic number is discovered by Dalton Moseley Bohr Rutherford 6 / 15 Which of the following has the highest shielding effect? Br I Cl F 7 / 15 John Newland found the similarity in properties of every ------ element. 10 6 8 4 8 / 15 The elements of B-group are called _____. Alkalineearthmetals Transitionelements Alkalimetalsandalkalineearthmetals Halogens 9 / 15 Across a period (left to right), shielding effect _____. Remainsconstant Decreases Increases Becomeszero 10 / 15 Which of the elements are not p-block representative elements? Halogens Alkalimetals Noblegases GroupV-A 11 / 15 The number of electrons in the valence shell of alkali metals is _____. 2 1 4 5 12 / 15 The horizontal rows in a periodic table are known as _____. Rows Groups Periods Columns 13 / 15 Elements in the same vertical group of the periodic table have same _____. AtomicNumber(Z) Numberofvalenceelectrons AtomicMass(A) Avogadro'snumber 14 / 15 The number of electrons in the valence shell of halogens are _____. 2 5 4 7 15 / 15 Valence shell configuration of Na is 3s1 1s2,2s2,2p6,3s1 2s2,2p6 2p6,3s1 Your score is LinkedIn Facebook Twitter VKontakte 0% Restart quiz Send feedback Practice MCQs Test No 4 /15 5 Class 9 Chemistry Chapter 3 Practice MCQs Test No 4 1 / 15 Which element has the highest electronegativity? F Cl I Br 2 / 15 The state required for Chlorine to release energy and form a uninegative ion is _____. Liquid atoms Solid molecules Gaseous atoms Gaseous molecules 3 / 15 Electron affinity involves _____. Addition of an electron to the nucleus of an atom Addition of a proton to the nucleus Removal of an electron from the outermost shell an atom Addition of an electron to the outermost shell of an atom 4 / 15 Ionization energy is a/an _____. Cation formation Bond breaking process Bond making process Anion formation 5 / 15 Which of the following has the highest electron affinity? C O N B 6 / 15 When atomic radius increases, electron affinity _____. Becomes zero Decreases Increases Remains constant 7 / 15 Which of these represents an element with a large electron affinity? Ability to gain an electron easily to form a positive ion Ability to lose an electron easily to form a positive ion Ability to gain an electron easily to form a negative ion Ability to lose an electron easily to form a negative ion 8 / 15 Arrange the elements in decreasing ionization energy. Li,Na,K Li>Na>K K>Na>Li Li<Na<K 9 / 15 Ionization energy is measured in _____. J/sec kJ/mol kW/mol kJ/h 10 / 15 Element in group II A with smallest atomic radius is _____. Ca Sr Mg Be 11 / 15 Negative sign is given to electron affinity because energy is _____. Released No effect Remain same Gained 12 / 15 Ionization results in the ejection of _____. Electrons Protons Nucleus Neutrons 13 / 15 Electronegativity refers to _____. the ability of an atom to attract the electrons toward nucleus tendency of an atom to attract a shared electron pair towards itself the energy required to remove an electron from a gaseous atom in the ground state. the ability of an atom to attract the electrons in a chemical bond toward itself 14 / 15 Atomic radii decreases because of Increase in attractive forces of the nucleus and valence electrons Increase in number of protons Increas in number of valence electrons All of these 15 / 15 In general, ionization energy _____ going bottom to top within a group in the periodic table. Becomes zero Decreases Remains unchanged Increases Your score is LinkedIn Facebook Twitter VKontakte 0% Restart quiz Send feedback Submit a Comment Cancel replyYou must be logged in to post a comment.