{"id":14760,"date":"2024-03-28T11:46:25","date_gmt":"2024-03-28T06:16:25","guid":{"rendered":"https:\/\/tsboardsolutions.in\/?p=14760"},"modified":"2024-04-01T17:41:41","modified_gmt":"2024-04-01T12:11:41","slug":"ts-10th-class-physical-science-bits-chapter-8","status":"publish","type":"post","link":"https:\/\/tsboardsolutions.in\/ts-10th-class-physical-science-bits-chapter-8\/","title":{"rendered":"TS 10th Class Physical Science Bits Chapter 8 Chemical Bonding"},"content":{"rendered":"

These\u00a0TS 10th Class Physical Science Bits with Answers<\/a> Chapter 8 Chemical Bonding will help students to enhance their time management skills.<\/p>\n

TS 10th Class Physical Science Bits Chapter 8 Chemical Bonding<\/h2>\n

Question 1.
\nAn ionic bond is also called : ( )
\n(A) metallic bond
\n(B) electrovalent bond
\n(C) coordinate covalent bond
\n(D) none of these
\nAnswer:
\n(B) electrovalent bond<\/p>\n

Question 2.
\nAn example of an ionic compound : ( )
\n(A) MgCl2<\/sub>
\n(B) NH3<\/sub>
\n(C) H2<\/sub>O
\n(D) all of these
\nAnswer:
\n(D) all of these<\/p>\n

Question 3.
\nThe negative ion formed from chlorine atom is called : ( )
\n(A) cation
\n(B) anion
\n(C) neutral ion
\n(D) all of these
\nAnswer:
\n(B) anion<\/p>\n

Question 4.
\nThe scientist who proposed the ionic bond is : ( )
\n(A) Lewis
\n(B) Rutherford
\n(C) Lavoiser
\n(D) Kossel
\nAnswer:
\n(D) Kossel<\/p>\n

Question 5.
\nThe bond formed when two atoms share their valency electrons between them is ………………… . ( )
\n(A) Ionic
\n(B) Covalent
\n(C) Electrovalent
\n(D) Metallic
\nAnswer:
\n(B) Covalent<\/p>\n

\"TS<\/p>\n

Question 6.
\nThe ion whose configuration is 1s2<\/sup>2s2<\/sup>2p6<\/sup> is : ( )
\n(A) calcium ion
\n(B) potassium ion
\n(C) fluoride ion
\n(D) sodium ion
\nAnswer:
\n(D) sodium ion<\/p>\n

Question 7.
\nThe factor that does not change when an atom is changed into ion: ( )
\n(A) charge
\n(B) atomic number
\n(C) no of electrons
\n(D) chemical property
\nAnswer:
\n(D) chemical property<\/p>\n

Question 8.
\nThe number of electron pairs in the bond formation of oxygen molecule ( )
\n(A) 1
\n(B) 4
\n(C) 6
\n(D) 2
\nAnswer:
\n(C) 6<\/p>\n

Question 9.
\nAn example of a covalent molecule: ( )
\n(A) Mgo
\n(B) Na2<\/sub>S
\n(C) NaCl
\n(D) HCl
\nAnswer:
\n(D) HCl<\/p>\n

Question 10.
\nThe electron present in outermost energy level of an atom is called ( )
\n(A) far most electron
\n(B) bond electron
\n(C) valence electron
\n(D) unpaired electron
\nAnswer:
\n(A) far most electron<\/p>\n

Question 11.
\nThe bond present in oxygen molecules ( )
\n(A) ionic
\n(B) coordinate covalent
\n(C) sigma
\n(D) double
\nAnswer:
\n(B) coordinate covalent<\/p>\n

Question 12.
\nThe reaction in which atoms combine to form a molecule is ( )
\n(A) exothermic
\n(B) endothermic
\n(C) reduction
\n(D) pyro-chemical total
\nAnswer:
\n(B) endothermic<\/p>\n

\"TS<\/p>\n

Question 13.
\nThe total number of electrons In the bond formation of Nitrogen molecule :
\n(A) 4
\n(B) 6
\n(C) 8
\n(D) 2
\nAnswer:
\n(D) 2<\/p>\n

Question 14.
\nAn example of a linear molecule: ( )
\n(A) SO3<\/sub>
\n(B) CO2<\/sub>
\n(C) H2<\/sub>S
\n(D) H2<\/sub>O
\nAnswer:
\n(C) H2<\/sub>S<\/p>\n

Question 15.
\nThe equilibrium distance between the nuclei of two atoms which form a covalent bond is called : ( )
\n(A) bond strength
\n(B) bond angle
\n(C) bond space
\n(D) bond length
\nAnswer:
\n(D) bond length<\/p>\n

Question 16.
\nIn sodium chloride crystal the coordination number of Na is ( )
\n(A) 2
\n(B) 4
\n(C) 6
\n(D) 8
\nAnswer:
\n(D) 8<\/p>\n

Question 17.
\nThe atoms possessing the following properties form cations ( )
\n(A) low ionization energy
\n(B) low electron affinity & low electro negativity
\n(C) high atomic size
\n(D) all the above
\nAnswer:
\n(A) low ionization energy<\/p>\n

Question 18.
\nThe atoms of elements with: ( )
\n(A) high I.P & high electron affinity
\n(B) small atomic size
\n(C) high electronegativity
\n(D) all the above
\nAnswer:
\n(C) high electronegativity<\/p>\n

Question 19.
\nThe number of electrons that a neutral sodium atom should lose in order to form a cation : ( )
\n(A) 1
\n(B) 2
\n(C) 6
\n(D) 3
\nAnswer:
\n(B) 2<\/p>\n

Question 20.
\nGroup VII A elements are called: ( )
\n(A) noble elements
\n(B) alkali metals
\n(C) halogens
\n(D) alkaline earth metals
\nAnswer:
\n(C) halogens<\/p>\n

Question 21.
\nWhich of these elements belongs to Group VI A In periodic table? ( )
\n(A) N
\n(B) O
\n(C) P
\n(D) F
\nAnswer:
\n(D) F<\/p>\n

Question 22.
\nThe number of C-H covalent bonds present in Methane molecule. ( )
\n(A) 2
\n(B) 3
\n(C) 4
\n(D) 6
\nAnswer:
\n(B) 3<\/p>\n

\"TS<\/p>\n

Question 24.
\nThe bond length In atoms between H-H molecules in (in A\u00b0) ( )
\n(A) 0.96
\n(B) 1.95
\n(C) 1.42
\n(D) 0.74
\nAnswer:
\n(A) 0.96<\/p>\n

Question 25.
\nThe bond dissociation energy between H-O in H20 molecule (in KJ\/mol)( )
\n(A) 298
\n(B) 460
\n(C) 390
\n(D) 151
\nAnswer:
\n(B) 460<\/p>\n

Question 26.
\nThe bond dissociation energy between Cl-Cl in Cl2 molecule is (In KJ mol-1<\/sup>) ( )
\n(A) 243
\n(B) 159
\n(C) 436
\n(D) 390
\nAnswer:
\n(D) 390<\/p>\n

Question 27.
\nThe shape of NH3<\/sub> molecule is ( )
\n(A) tetra hedral
\n(B) trigonal pyramidal
\n(C) hexagonal
\n(D)\u2019V-shaped
\nAnswer:
\n(C) hexagonal<\/p>\n

Question 28.
\nThe bond angle in img of water molecule is ( )
\n(A) 109\u00b028′
\n(B) 120\u00b0
\n(C) 107\u00b048′
\n(D) 104\u00b031\u2019
\nAnswer:
\n(B) 120\u00b0<\/p>\n

Question 29.
\nIn HCl molecule ‘1s’ orbital of H atom overlaps the following bond of chlorine atom: ( )
\n(A) 1p
\n(B) 2p
\n(C) 3p
\n(D) 3d
\nAnswer:
\n(A) 1p<\/p>\n

Question 30.
\nThe phenomenon of intermixing of atomic orbitals of equal energy which are present in outer shells of atoms is called : ( )
\n(A) chronic
\n(B) hybridization
\n(C) grafting
\n(D) intermixing
\nAnswer:
\n(B) hybridisation<\/p>\n

Question 31.
\nThe number of B-F bonds in BF3<\/sub> is ( )
\n(A) 3
\n(B) 2
\n(C) 1
\n(D) many
\nAnswer:
\n(B) 2<\/p>\n

Question 32.
\nThe compound which has polar covalent bond is ( )
\n(A) NaCl
\n(B) HCl
\n(C) O2<\/sub>
\n(D) N2<\/sub>
\nAnswer:
\n(A) NaCl<\/p>\n

Question 33.
\nSince the forces of attractions among covalent molecules are ………………… most of the covalent compounds are gases or liquids at room temperature. ( )
\n(A) weak
\n(B) strong
\n(C) balanced
\n(D) none of these
\nAnswer:
\n(B) strong<\/p>\n

Question 34.
\nThe type of bond that forms between two atoms depends is ……………… . ( )
\n(A) number of protons
\n(B) number of neutrons
\n(C) number of valence electrons
\n(D) number of paired electrons
\nAnswer:
\n(C) number of valence electrons<\/p>\n

\"TS<\/p>\n

Question 35.
\nThe noble gas that has no octet configuration is ………………… . ( )
\n(A) Ar
\n(B) Rn
\n(C) Xe
\n(D) He
\nAnswer:
\n(C) Xe<\/p>\n

Question 36.
\nThe type of overlap that takes place in NH3<\/sub> molecule is ( )
\n(A) s-s
\n(B) s-p
\n(C) p-p
\n(D) lateral
\nAnswer:
\n(D) lateral<\/p>\n

Question 37.
\nThe bond formed due to overlap of orbitals is known as: ( )
\n(A) Ionic bond
\n(B) hydrogen bond
\n(C) covalent bond
\n(D) metallic bond
\nAnswer:
\n(B) hydrogen bond<\/p>\n

Question 38.
\nThe number of s bonds in nitrogen molecule is ( )
\n(A) 0
\n(B) 1
\n(C) 2
\n(D) 3
\nAnswer:
\n(C) 2<\/p>\n

Question 39.
\nThe bond formed between two atoms having the same electro-negative value ( )
\n(A) ionic bond
\n(B) hydrogen bond
\n(C) metallic bond
\n(D) Covalent bond,
\nAnswer:
\n(B) hydrogen bond<\/p>\n

Question 40.
\nThe substance which has the highest melting point among the following: ( )
\n(A) NH3<\/sub>
\n(B) CsF
\n(C) H2<\/sub>O
\n(D) CHCl3<\/sub>
\nAnswer:
\n(A) NH3<\/sub><\/p>\n

\"TS<\/p>\n

Question 41.
\nStrongest among the following bonds. ( )
\n(A) single bond
\n(B) double bond
\n(C) triple bond
\n(D) hydrogen bond
\nAnswer:
\n(D) hydrogen bond<\/p>\n

Question 42.
\nThe bond formed when the orbitals undergo \u2018end on end\u2019 overlap is ( )
\n(A) N2<\/sub>
\n(B) O2<\/sub>
\n(C) H2<\/sub>O
\n(D) H3<\/sub>
\nAnswer:
\n(A) N2<\/sub><\/p>\n

Question 43.
\nA triple bond is present in the following molecule: ( )
\n(A) N2<\/sub>
\n(B) O2<\/sub>
\n(C) H2<\/sub>O
\n(D) H2<\/sub>
\nAnswer:
\n(C) H2<\/sub>O<\/p>\n

Question 44.
\nThe shape of water molecule is ………………………….. . ( )
\n(A) pyramidal
\n(B) tetra hedral
\n(C) trigonal bi pyramidal
\n(D) ‘v-shaped
\nAnswer:
\n(C) trigonal bi pyramidal<\/p>\n

Question 45.
\nComplete transfer of electrons from one atom to another lead to the formation of ( )
\n(A) Ionic bond
\n(B) Covalent bond
\n(C) Metallic bond
\n(D) none
\nAnswer:
\n(A) Ionic bond<\/p>\n

Question 46.
\ns – s overlap is found In ( )
\n(A) Cl2<\/sub>
\n(B) F2<\/sub>
\n(C) H2<\/sub>
\n(D) N2<\/sub>
\nAnswer:
\n(B) F2<\/sub><\/p>\n

Question 47.
\nThe number of valency electrons in carbon atom (Z=6) is ( )
\n(A) 1
\n(B) 2
\n(C) 4
\n(D) 6
\nAnswer:
\n(A) 1<\/p>\n

Question 48.
\np-p overlap is found In: ( )
\n(A) Br2<\/sub>
\n(B) H2<\/sub>
\n(C) HCl
\n(D) HBr
\nAnswer:
\n(B) H2<\/sub><\/p>\n

Question 49.
\nA molecule which has double bond : ( )
\n(A) Cl2<\/sub>
\n(B) C2<\/sub>H4<\/sub>
\n(C) C2<\/sub>H2<\/sub>
\n(D) N2<\/sub>
\nAnswer:
\n(C) C2<\/sub>H2<\/sub><\/p>\n

Question 50.
\nAn ionic compound among the following is ………………………. . ( )
\n(A) CaH2<\/sub>
\n(B) HCl
\n(C) H2<\/sub>O
\n(D) H2<\/sub>S
\nAnswer:
\n(D) H2<\/sub>S<\/p>\n

Question 51.
\nNumber of electrons present In the penultimate shell of magnesium atom. ( )
\n(A) 2
\n(B) 8
\n(C) 18
\n(D) 32
\nAnswer:
\n(B) 8<\/p>\n

Question 52.
\nIf the atomic number is 12, what kind of bond does it form with the other kind of atoms ? ( )
\n(A) covalent bond
\n(B) coordinate bond
\n(C) doesn\u2019t form bond at all
\n(D) ionic bond
\nAnswer:
\n(B) coordinate bond<\/p>\n

Question 53.
\nWhich of the following molecules show lone pair of electrons? ( )
\n(A) BeCl2<\/sub>
\n(B) HCl
\n(C) NH3<\/sub>
\n(D) PCl
\nAnswer:
\n(C) NH3<\/sub><\/p>\n

Question 54.
\nWhich of the following pairs of molecules show triple bond? ( )
\n(A) C2<\/sub>H2<\/sub> ; Cl2<\/sub>
\n(B) C2<\/sub>H2<\/sub>; N2<\/sub>
\n(C) NH3<\/sub>; C2<\/sub>H4<\/sub>
\n(D) F2<\/sub>, O2<\/sub>
\nAnswer:
\n(B) C2<\/sub>H2<\/sub>; N2<\/sub><\/p>\n

Question 55.
\nA bond formed between a metal and non metal is …………………….. . ( )
\n(A) metallic bond
\n(B) ionic bond
\n(C) covalent bond
\n(D) hydrogen bond
\nAnswer:
\n(D) hydrogen bond<\/p>\n

\"TS<\/p>\n

Question 56.
\nIn sodium chloride crystal each of Na+<\/sup> ion is surrounded by ……………….. Cl ions. ( )
\n(A) 4
\n(B) 5
\n(C) 6
\n(D) 7
\nAnswer:
\n(B) 5<\/p>\n

Question 57.
\nbond is present between the two oxygen atoms in oxygen molecule. ( )
\n(A) single
\n(B) double
\n(C) triple
\n(D) hydrogen
\nAnswer:
\n(D) hydrogen<\/p>\n

Question 58.
\nWhich one is the inert gas of the following
\n(A) Sodium
\n(B) Potassium
\n(C) Oxygen
\n(D) Neon
\nAnswer:
\n(D) Neon<\/p>\n

Question 59.
\nIn the formation of MgCl2<\/sub> number of electrons transferred from Mg to Cl is
\n(A)1
\n(B) 2
\n(C) 3
\n(D) 4
\nAnswer:
\n(B) 2<\/p>\n

Question 60.
\nFactors affecting the formation of the ionic bond ( )
\n(A) atomic size
\n(B) ionization energy
\n(C) electron affinity
\n(D) all the above
\nAnswer:
\n(A) atomic size<\/p>\n

Question 61.
\nThe bond angle In water molecules is ………………………… . ( )
\n(A) 180\u00b0
\n(B) 120\u00b0
\n(C) 109\u00b028′
\n(D) 104\u00b028′
\nAnswer:
\n(C) 109\u00b028′<\/p>\n

Question 62.
\nCovalent compounds are generally soluble in ………………………… . ( )
\n(A) polar solvents
\n(B) non-polar solvents
\n(C) concentrated acids
\n(D) all solvents
\nAnswer:
\n(A) polar solvents<\/p>\n

Question 63.
\nWhich of the following molecules contains a triple bond? ( )
\n(A) N2<\/sub>
\n(B) C2<\/sub>H4<\/sub>
\n(C) PH3<\/sub>
\n(D) CCl4<\/sub>
\nAnswer:
\n(B) C2<\/sub>H4<\/sub><\/p>\n

\"TS<\/p>\n

Question 64.
\nWhich of the following can lose two electrons to attain the configuration of argon? ( )
\n(A) Mg
\n(B) Br
\n(C) Ca
\n(D) S
\nAnswer:
\n(D) S<\/p>\n

Question 65.
\nThe formation of a chemical bond is accompanied by ( )
\n(A) decrease in energy
\n(B) increase in energy
\n(C) Neither decrease nor increase in energy
\n(D) The repulsion forces overcoming the attraction forces
\nAnswer:
\n(B) increase in energy<\/p>\n

Question 66.
\nWhich one amongest the following is the weakest? ( )
\n(A) H-bond
\n(B) Vander Waals forces
\n(C) Three electrons bond
\n(D) Ion-dipole interaction
\nAnswer:
\n(C) Three electrons bond<\/p>\n

Question 67.
\nWhich of the following is an ionic compound? ( )
\n(A) CO2<\/sub>
\n(B) HCl
\n(C) H2<\/sub>O
\n(D) CaO
\nAnswer:
\n(C) H2<\/sub>O<\/p>\n

Question 68.
\nCovalent bond is formed by ( )
\n(A) electron transfer
\n(B) electron sharing
\n(C) electron donation
\n(D) electron acceptance
\nAnswer:
\n(B) electron sharing<\/p>\n

Question 69.
\nThe number of valency electrons in carbon atom (z = 6) is ………………….. . ( )
\n(A) 0
\n(B) 2
\n(C) 4
\n(D) 6
\nAnswer:
\n(A) 0<\/p>\n

Question 70.
\nThe total number of electrons that take part in forming the bonds in N2<\/sub> is ………………… .
\n(A)2
\n(B) 4
\n(C) 6
\n(D) 10
\nAnswer:
\n(C) 6<\/p>\n

Question 71.
\nElectrons in ………………………. shell are called valence electrons. ( )
\n(A) innermost
\n(B) outermost
\n(C) present in nucleus
\n(D) free
\nAnswer:
\n(A) innermost<\/p>\n

Question 72.
\nExcept ………………………………. gas all other noble gases have octet In their valence shell.
\n(A) He
\n(B) Ne
\n(C) Ar
\n(D) Kr
\nAnswer:
\n(B) Ne<\/p>\n

\"TS<\/p>\n

Question 73.
\nValence bond theory was proposed by …………………………… . ( )
\n(A) Lewls
\n(B) Milliken
\n(C) Sidgwick and Powell
\n(D) Bohr
\nAnswer:
\n(B) Milliken<\/p>\n

Question 74.
\nIn ………………………. bonding the valence electrons are shared among all the atoms of the metallic elements. ( )
\n(A) covalent
\n(B) Ionic
\n(C) hybrid
\n(D) triple
\nAnswer:
\n(C) hybrid<\/p>\n

Question 75.
\nThe chloride ion has a …………………. charge. ( )
\n(A) positive
\n(B) negative
\n(C) no charge
\n(D) depends upon reaction
\nAnswer:
\n(B) negative<\/p>\n

Question 76.
\nNa+<\/sup> and Cl–<\/sup> ions combine together to form an ………….. solid. ( )
\n(A) covalent
\n(B) ionic
\n(C) metallic
\n(D) non-metallic
\nAnswer:
\n(C) metallic<\/p>\n

Question 77.
\nNoble gases exist as individual …………………….. . ( )
\n(A) solids
\n(B) molecules
\n(C) atoms
\n(D) gases
\nAnswer:
\n(C) atoms<\/p>\n

Question 78.
\nThe chlorine atom can ……………………… one electron to become a chloride ion. ( )
\n(A) lose
\n(B) gain
\n(C) retain
\n(D) donate
\nAnswer:
\n(C) retain<\/p>\n

Question 79.
\nTwo atoms of nitrogen form a nitrogen molecule by sharing pairs of electrons. ( )
\n(A) one
\n(B) two
\n(C) three
\n(D) four
\nAnswer:
\n(A) one<\/p>\n

Question 80.
\nThe chemical formula of ferric carbonate is …………………… . ( )
\n(A) Fe2<\/sub>(CO3<\/sub>)2<\/sub>
\n(B) Fe(CO3<\/sub>)3<\/sub>
\n(C) Fe2<\/sub>(CO3<\/sub>)3<\/sub>
\n(D) Fe2<\/sub>CO3<\/sub>
\nAnswer:
\n(B) Fe(CO3<\/sub>)3<\/sub><\/p>\n

\"TS<\/p>\n

Question 81.
\nThe chemical formula of zinc phosphate is ……………………….. . ( )
\n(A) Zn3<\/sub>(PO4<\/sub>)3<\/sub>
\n(B) Zn3<\/sub>PO4<\/sub>
\n(C) Zn(PO4<\/sub>)3<\/sub>
\n(D) Zn(PO4<\/sub>)3<\/sub>
\nAnswer:
\n(A) Zn3<\/sub>(PO4<\/sub>)3<\/sub><\/p>\n

Question 82.
\nMolecular formula of methane is ………………………. . ( )
\n(A) CH3<\/sub>
\n(B) CH4<\/sub>
\n(C) C2<\/sub>H4<\/sub>
\n(D) C2<\/sub>H6<\/sub>
\nAnswer:
\n(B) CH4<\/sub><\/p>\n

Question 83.
\nH2<\/sub> molecule has the configuration of the inert gas …………………. . ( )
\n(A) He
\n(B) H3<\/sub>O+<\/sup>
\n(C) H+<\/sup>
\n(D) OH–<\/sup>
\nAnswer:
\n(C) H+<\/sup><\/p>\n

Question 84.
\nA sigma bond is formed by ……………………….. overlap of orbitals. ( )
\n(A) axial
\n(B) co-axial
\n(C) side-way
\n(D) without overlapping
\nAnswer:
\n(C) side-way<\/p>\n

Question 85.
\nA pi bond is formed by …………………… overlap of orbitals. ( )
\n(A) axial
\n(B) lateral
\n(C) without overlapping
\n(D) can’t form
\nAnswer:
\n(D) can’t form<\/p>\n

Question 86.
\n………………………. overlap is present in F2<\/sub> molecule. ( )
\n(A) s-s
\n(B) s-p
\n(C) p-p
\n(D) none
\nAnswer:
\n(D) none<\/p>\n

Question 87.
\nThe number of valence shell &ectrons that a group LA element loses to get octet configuration : ( )
\n(A) 7
\n(B) 2
\n(C) 1
\n(D) 2
\nAnswer:
\n(C) 1<\/p>\n

Question 88.
\nNoble gases belong to the following group : ( )
\n(A) Group VII A
\n(B) Group V A
\n(C) Group III A
\n(D) Group VIII A
\nAnswer:
\n(D) Group VIII A<\/p>\n

Question 86.
\nAny species attains stability when It has …………………….. number of electrons in its valence shell ( )
\n(A) 1
\n(B) 2
\n(C) 3
\n(D) 8
\nAnswer:
\n(D) 8<\/p>\n

Question 87.
\nThe force of attraction between any two atoms or a group of atoms that results in a stable entity is known as : ( )
\n(A) chemical bond
\n(B) crystalline bond
\n(C) crystal lattice
\n(D) none of these
\nAnswer:
\n(A) chemical bond<\/p>\n

\"TS<\/p>\n

Question 88.
\nAH2<\/sub> is formed when element A\u2019 reacts with hydrogen. Then the number of electrons in valence shell of \u2018A\u2019 are generally ………………………. . ( )
\n(A) 2
\n(B) 3
\n(C) 5
\n(D) 8
\nAnswer:
\n(A) 2<\/p>\n

Question 89.
\nIonic compound in the following is ……………………. . ( )
\n(A) C2<\/sub>H6<\/sub>
\n(B) HCl
\n(C) NaCl
\n(D) H2<\/sub>
\nAnswer:
\n(C) NaCl<\/p>\n

Question 90.
\nNumber of moles of Oxygen need to produce 4 moles of water on reacting with 4 moles of Hydrogen gas is ……………………….. . ( )
\n(A) 1 mole
\n(B) 2 moles
\n(C) 3 moles
\n(D) 4 moles
\nAnswer:
\n(B) 2 moles<\/p>\n","protected":false},"excerpt":{"rendered":"

These\u00a0TS 10th Class Physical Science Bits with Answers Chapter 8 Chemical Bonding will help students to enhance their time management skills. TS 10th Class Physical Science Bits Chapter 8 Chemical Bonding Question 1. An ionic bond is also called : ( ) (A) metallic bond (B) electrovalent bond (C) coordinate covalent bond (D) none of … Read more<\/a><\/p>\n","protected":false},"author":2,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[16],"tags":[],"jetpack_featured_media_url":"","_links":{"self":[{"href":"https:\/\/tsboardsolutions.in\/wp-json\/wp\/v2\/posts\/14760"}],"collection":[{"href":"https:\/\/tsboardsolutions.in\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/tsboardsolutions.in\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/tsboardsolutions.in\/wp-json\/wp\/v2\/users\/2"}],"replies":[{"embeddable":true,"href":"https:\/\/tsboardsolutions.in\/wp-json\/wp\/v2\/comments?post=14760"}],"version-history":[{"count":2,"href":"https:\/\/tsboardsolutions.in\/wp-json\/wp\/v2\/posts\/14760\/revisions"}],"predecessor-version":[{"id":14764,"href":"https:\/\/tsboardsolutions.in\/wp-json\/wp\/v2\/posts\/14760\/revisions\/14764"}],"wp:attachment":[{"href":"https:\/\/tsboardsolutions.in\/wp-json\/wp\/v2\/media?parent=14760"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/tsboardsolutions.in\/wp-json\/wp\/v2\/categories?post=14760"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/tsboardsolutions.in\/wp-json\/wp\/v2\/tags?post=14760"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}