A) It calculates the formal charge of every atom. B) It eliminates the need for electron counting. C) It uses quantum mechanics to determine orbital shape. D) It provides the exact bond length of the molecule.
A) By sharing lone pairs between oxygen atoms. B) By subtracting electrons from the central atom. C) By pairing up valence electrons of the atoms involved. D) By calculating the difference between protons and neutrons.
A) By forming a double bond with a noble gas. B) By removing protons from the nucleus. C) By dividing the total valence electrons by two. D) By adding electrons to the appropriate atoms.
A) By multiplying the valence electrons by four. B) By ignoring the valence shell of the central atom. C) By removing electrons from the appropriate atoms. D) By adding neutrons to the central atom.
A) Determine the electronegativity of each atom. B) Draw the resonance structures. C) Calculate the formal charge of the molecule. D) Count up the valence electrons.
A) The mass number of each constituent atom. B) The number of electrons needed to complete the octet rule. C) The total number of protons in the molecule. D) The number of inner-shell electrons.
A) 2 electrons. B) 4 electrons. C) 6 electrons. D) 8 electrons.
A) The total number of neutrons. B) The number of electrons that make up the bonds. C) The total number of lone pairs. D) The formal charge of the molecule.
A) Form metallic bonds. B) Become part of the nucleus. C) Are discarded from the calculation. D) Fill all the other atoms' octets.
A) It needs 8 electrons. B) It does not have valence electrons. C) It needs 2 electrons. D) It always forms triple bonds.
A) Octet diagrams B) Valence shell graphs C) Lewis dot formulas D) Atomic orbital maps
A) John Dalton B) Gilbert N. Lewis C) Dmitri Mendeleev D) Linus Pauling
A) Two B) Four C) Six D) Eight
A) As a subscript inside brackets B) As a superscript outside brackets C) Next to the central atom only D) By adding more dots
A) The central atom B) Those with lower electronegativity C) Those with higher electronegativity D) The smallest atoms
A) The structure becomes unstable B) The atom loses two electrons C) The total valence count decreases D) An additional line is drawn
A) Covalently bonded molecules and coordination compounds B) Metallic bonds only C) Noble gases only D) Ionic lattices only
A) Zero B) One C) The number of atoms D) Negative one
A) The charge on the ion B) The number of protons C) Zero D) The number of electrons
A) Four B) One C) Three D) Two
A) On the hydrogen atoms B) On the more electronegative elements C) On the least electronegative elements D) On the central atom
A) Water B) Nitrate ion C) Carbon dioxide D) Sulfur hexafluoride
A) NO2 B) N2O C) NO2- D) NO3-
A) Both are central B) Oxygen C) Neither D) Nitrogen
A) 8 B) 7 C) 6 D) 5
A) 17 B) 16 C) 18 D) 19
A) 4 B) 2 C) 6 D) 8
A) 10 B) 16 C) 12 D) 14
A) Remove a single bond B) Form a double bond C) Add more lone pairs D) Add an electron
A) Isomerization B) Polarization C) Hybridization D) Resonance
A) Double-sided equilibrium arrow B) Single-headed arrow C) Dashed arrow D) Double-headed arrow
A) Space-filling diagram B) Condensed formula C) Resonance structure D) Bond-line formula
A) They are not shown B) With the symbol H C) With dashed lines D) With dots
A) Subscripts B) Superscripts C) Coefficients D) Parentheses only
A) Twenty-first century B) Mid twentieth century C) Late nineteenth century D) Early twentieth century
A) Inorganic chemistry B) Quantum chemistry C) Nuclear chemistry D) Organic chemistry
A) Ionic bonding B) Electronegativity C) Aromaticity D) Covalent bonding
A) VSEPR theory B) Lewis structure theory C) Valence-bond theory D) Molecular orbital theory
A) Destabilization B) Special stabilization beyond normal delocalization C) Complete loss of bonding D) No deviation from normal behavior
A) Valence-shell energy plots B) Lewis-dot electron maps C) Molecular orbital diagrams D) Curve-arrow notation |