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