Question: the octet rule states that in chemical compounds atoms tend to have the electron configuration of a
[{'answer': 'noble gas', 'provenance': [{'wikipedia_id': '266466', 'title': 'Octet rule', 'start_paragraph_id': 1, 'start_character': 216, 'end_paragraph_id': 1, 'end_character': 225, 'bleu_score': 1.0, 'section': 'Section::::Abstract.'}]}, {'provenance': [{'wikipedia_id': '266466', 'title': 'Octet rule', 'start_paragraph_id': 1, 'start_character': 0, 'end_paragraph_id': 1, 'end_character': 354, 'bleu_score': 0.8093487731004061, 'meta': {'yes_no_answer': 'NONE', 'annotation_id': 11211858005968091771}, 'section': 'Section::::Abstract.'}]}, {'provenance': [{'wikipedia_id': '41529166', 'title': 'Noble gas configuration', 'section': 'Section::::Abstract.', 'start_paragraph_id': 1, 'end_paragraph_id': 1, 'meta': {'evidence_span': ['Noble gas configuration is the tendency for chemical elements to gain or lose electrons to reach the electronic configuration of a noble gas. This may refer to:', 'Noble gas configuration is the tendency for chemical elements to gain or lose electrons to reach the electronic configuration of a noble gas. This may refer to:']}}]}, {'provenance': [{'wikipedia_id': '3797882', 'title': 'Tetrahedral molecular geometry', 'section': 'Section::::Examples.:Water structure.\n', 'start_paragraph_id': 10, 'end_paragraph_id': 10, 'meta': {'evidence_span': ['. Many complexes with incompletely filled d-shells are often tetrahedral, e.g. the tetrahalides of iron(II), cobalt(II), and nickel(II). In the gas phase, a single water molecule has an oxygen atom surrounded by two hydrogens and two lone pairs, and the HO geometry is simply described as bent without considering the nonbonded lone pairs. However in liquid water or in ice, the lone pairs form hydrogen bonds with neighboring water molecules. The most common arrangement of hydrogen atoms around an oxygen is tetrahedral with two hydrogen atoms covalently bonded to oxygen and two attached by hydrogen bonds. Since the hydrogen bonds vary in length many of these water molecules are not symmetrical and form transient irregular tetrahedra between their four associated hydrogen atoms.', '. Many complexes with incompletely filled d-shells are often tetrahedral, e.g. the tetrahalides of iron(II), cobalt(II), and nickel(II). In the gas phase, a single water molecule has an oxygen atom surrounded by two hydrogens and two lone pairs, and the HO geometry is simply described as bent without considering the nonbonded lone pairs. However in liquid water or in ice, the lone pairs form hydrogen bonds with neighboring water molecules. The most common arrangement of hydrogen atoms around an oxygen is tetrahedral with two hydrogen atoms covalently bonded to oxygen and two attached by hydrogen bonds. Since the hydrogen bonds vary in length many of these water molecules are not symmetrical and form transient irregular tetrahedra between their four associated hydrogen atoms.']}}]}, {'provenance': [{'wikipedia_id': '266466', 'title': 'Octet rule', 'section': 'Section::::Abstract.', 'start_paragraph_id': 1, 'end_paragraph_id': 1, 'meta': {'evidence_span': ['The octet rule is a chemical rule of thumb that reflects observation that elements tend to bond in such a way that each atom has eight electrons in its valence shell, giving it the same electronic configuration as a noble gas. The rule is especially applicable to carbon, nitrogen, oxygen, and the halogens, but also to metals such as sodium or magnesium.', 'observation that elements tend to bond in such a way that each atom has eight electrons in its valence shell, giving it the same electronic configuration as a noble gas', 'The octet rule is a chemical rule of thumb that reflects observation that elements tend to bond in such a way that each atom has eight electrons in its valence shell, giving it the same electronic configuration as a noble gas. The rule is especially applicable to carbon, nitrogen, oxygen, and the halogens, but also to metals such as sodium or magnesium.']}}]}]