Chemistry XI Unit 4 Questions: 72 Time Limit: 72 minutes Passing Score: 60% Start Quiz Chemistry XI Unit 4 Question 1 of 72 Chemical bond is formed due to: attraction between nuclei repulsion between electrons lowering of overall system energy random electron movement Ionic bond forms between: two nonmetals metal and nonmetal two metals noble gases Covalent bond is formed by: transfer of electrons sharing of electrons attraction between nuclei repulsion between electrons In ionic compound NaCl: Na⁺ and Cl⁻ ions Na and Cl atoms Na⁻ and Cl⁺ ions neutral atoms Covalent compounds generally have: high melting points low melting points high ionic character poor electrical conductivity In a covalent bond between two identical atoms: electrons are equally shared electrons drift toward more electronegative atom one atom loses electrons electrons are not shared Polar covalent bonds occur between atoms with: same electronegativity different electronegativity no electronegativity zero charge difference The bond dissociation energy is: energy required to form bond energy required to break bond heat released in reaction energy of free atoms Lewis structure represents: three-dimensional structure valence electrons as dots/dashes all electrons in atom nuclear charge Octet rule states: atoms have 8 electrons total atoms tend to have 8 valence electrons all atoms follow octet rule atoms repel each other Electronegativity difference between bonded atoms determines: bond strength only bond polarity atomic size atomic number A triple bond consists of: 3 single bonds 1 σ and 2 π bonds 3 σ bonds 3 π bonds Sigma (σ) bond is formed by: head-on overlap side-by-side overlap bent overlap no overlap Pi (π) bond is formed by: head-on overlap side-by-side overlap end-to-end overlap no overlap Ionic compounds conduct electricity: in solid state in molten state always never Coordinate covalent bond (dative bond) involves: sharing of electrons from both atoms equally donation of electron pair from one atom to another complete transfer of electrons no electron involvement Metallic bonding involves: fixed electron positions sea of delocalized electrons ionic attractions no electron movement Hybridization occurs to: explain bonding and molecular geometry increase atomic size decrease electronegativity create new orbitals from nothing sp hybridization involves mixing of: s and one p orbital s and two p orbitals s, p, and d orbitals only p orbitals sp² hybridization results in: linear geometry trigonal planar geometry tetrahedral geometry octahedral geometry sp³ hybridization results in: linear geometry trigonal planar geometry tetrahedral geometry octahedral geometry The shape of CH₄ is: linear trigonal planar tetrahedral square planar In CO₂, the carbon is: sp hybridized sp² hybridized sp³ hybridized not hybridized Resonance structures are: different spatial arrangements different electronic arrangements showing distributed electrons incorrect structures multiple stable compounds Formal charge is calculated to: find ionic charge determine electron distribution find oxidation state calculate molecular mass The bond angle in NH₃ is approximately: 90° 109.5° 107° 120° The bond angle in H₂O is approximately: 90° 104.5° 109.5° 120° VSEPR theory predicts: electronic structure molecular geometry from electron pairs bond order energy of bonds In benzene (C₆H₆): all C-C bonds identical length alternating single-double bonds all bonds partial double no electrons delocalized Hydrogen bonding occurs between: H and any atom H bonded to F, O, or N with lone pairs on other molecule all H atoms H and C only FILLBLANK:Bond _____ is energy required to break a chemical bond. dissociation energy formation energy activation energy potential energy FILLBLANK:Mixing of orbitals to form new ones is called _____ hybridization resonance ionization oxidation FILLBLANK:A _____ bond has electrons equally shared between atoms. nonpolar covalent polar covalent ionic coordinate FILLBLANK:A _____ bond has electrons unequally shared. polar covalent nonpolar covalent metallic coordinate FILLBLANK:sp² hybridization gives _____ geometry. trigonal planar linear tetrahedral square planar FILLBLANK:The _____ describes molecular shape based on electron pair arrangement. VSEPR theory Bohr model Lewis theory Valence bond theory FILLBLANK:A _____ bond forms when H bonded to F, O, N attracts lone pair. hydrogen bond ionic bond covalent bond metallic bond FILLBLANK:The _____ is measure of electron density in bonding region. bond order bond strength bond length ionization energy FILLBLANK:_____ is the force holding atoms together in molecules. Chemical bonding Gravity Friction Cohesion FILLBLANK:The shape of CH₄ is _____ tetrahedral linear trigonal planar square planar FILLBLANK:The shape of NH₃ is _____ trigonal pyramidal tetrahedral trigonal planar octahedral FILLBLANK:The shape of BeF₂ is _____ linear trigonal planar tetrahedral bent FILLBLANK:The shape of BCl₃ is _____ trigonal planar tetrahedral linear pyramidal FILLBLANK:The shape of PCl₅ is _____ trigonal bipyramidal octahedral tetrahedral square planar FILLBLANK:The shape of SF₆ is _____ octahedral trigonal bipyramidal square planar tetrahedral FILLBLANK:Lone pairs _____ bond angle compared to bonded pairs. decrease increase keep same vary FILLBLANK:_____ involves transfer of electrons from metal to nonmetal. Ionic bonding Covalent bonding Metallic bonding Hydrogen bonding TRUE/FALSE: Covalent bonds are stronger than ionic bonds. TRUE FALSE TRUE/FALSE: Noble gases form chemical bonds easily. TRUE FALSE TRUE/FALSE: Electronegativity increases across a period. TRUE FALSE TRUE/FALSE: Single bond has higher bond energy than double bond. TRUE FALSE TRUE/FALSE: Hydrogen bonding is covalent bond. TRUE FALSE TRUE/FALSE: Metallic bonding has delocalized electrons. TRUE FALSE TRUE/FALSE: Formal charge equals oxidation state. TRUE FALSE TRUE/FALSE: Polar covalent bonds occur between identical atoms. TRUE FALSE TRUE/FALSE: Coordinate covalent bonds are weaker than regular covalent. TRUE FALSE TRUE/FALSE: VSEPR theory predicts molecular structure. TRUE FALSE TRUE/FALSE: sp hybridization forms tetrahedral geometry. TRUE FALSE TRUE/FALSE: Double bond consists of two sigma bonds. TRUE FALSE TRUE/FALSE: Resonance is different arrangement in space. TRUE FALSE TRUE/FALSE: CH₄ has tetrahedral geometry. TRUE FALSE TRUE/FALSE: NH₃ has trigonal planar geometry. TRUE FALSE TRUE/FALSE: H₂O has bond angle of 109.5°. TRUE FALSE TRUE/FALSE: Pi bond can form without sigma bond. TRUE FALSE TRUE/FALSE: Hydrogen bond is strongest intermolecular force. TRUE FALSE TRUE/FALSE: Octet rule applies to all atoms. TRUE FALSE TRUE/FALSE: Electronegativity increases down a group. TRUE FALSE TRUE/FALSE: NaCl is covalent compound. TRUE FALSE TRUE/FALSE: Molecular orbital theory explains bonding better than VB theory. TRUE FALSE TRUE/FALSE: Carbon always forms four bonds. TRUE FALSE TRUE/FALSE: Lone pair occupies more space than bonded pair. TRUE FALSE TRUE/FALSE: Electronegativity is measured in joules. TRUE FALSE Previous Next Submit Quiz Want to save your progress? Create an account or log in to track your quiz scores! Register/Login