Question 1
Question
Lewis structures show [blank_start]bonds[blank_end], but Lewis structures can't [blank_start]predict[blank_end] so they came up with two new models: the [blank_start]valence[blank_end] bond theory and the [blank_start]molecular[blank_end] orbital theory.
Answer
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bonds
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predict
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valence
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molecular
Question 2
Question
Valence bond theory: a model of chemical bonding that states that atoms fill their valence shells by filling vacancies in particular [blank_start]orbitals[blank_end]. Partially filled orbitals of two atoms [blank_start]overlap[blank_end], and a [blank_start]covalent[blank_end] bond is formed. This theory is also called the [blank_start]localized[blank_end] electron theory.
Answer
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orbitals
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overlap
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covalent
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localized
Question 3
Question
Sigma bonds: The orbitals overlap [blank_start]end[blank_end] to end. The orbital overlap is located [blank_start]between[blank_end] the nuclei. They can form from various orbital combinations: two s orbitals, two p orbitals, or an s and a p orbital. Sigma bonds always form [blank_start]first[blank_end].
Question 4
Question
Pi bonds: The orbitals overlap [blank_start]side[blank_end] to side. The orbital overlap is located above and [blank_start]below[blank_end] the nuclei. Pi bonds can combine with [blank_start]sigma[blank_end] bonds and other pi bonds to form [blank_start]double[blank_end] and triple bonds. One sigma and one pi= (double bond.) One sigma and two pi= ([blank_start]triple[blank_end] bond.) Pi bonds always form [blank_start]after[blank_end] sigma bonds.
Answer
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side
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below
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sigma
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double
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triple
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after
Question 5
Question
Sigma bonds are the [blank_start]strongest[blank_end]. Pi bonds are [blank_start]weaker[blank_end] than sigma bonds because the electrons are spread out over a greater volume of space around the bond axis. The combination of a sigma and a pi bond is [blank_start]stronger[blank_end] than either bond by itself.
Answer
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strongest
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weaker
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stronger
Question 6
Question
Resonance: the state of molecules that can have [blank_start]two[blank_end] or more possible Lewis structures. No [blank_start]single[blank_end] Lewis structure can completely describe electron distribution in resonance molecules. There are NO single or double bonds in these molecules- the bonds are experimentally identical. A resonance molecule is depicted with a [blank_start]hybrid[blank_end] Lewis structure.
Question 7
Question
Some molecules form without an octet for each bonded atom: this happens when there is an [blank_start]odd[blank_end] number of valence electrons, electron [blank_start]deficiency[blank_end], and hypervalent molecules.
Question 8
Question
Some molecules have an odd number of valence electrons to share. Substances with these unpaired electrons are called [blank_start]free[blank_end] [blank_start]radicals[blank_end] and tend to be fairly [blank_start]reactive[blank_end].
Question 9
Question
Electron Deficiency: elements with [blank_start]less[blank_end] than 8 valence electrons.
Question 10
Question
Hypervalent Molecules: The central atom has [blank_start]more[blank_end] than 8 valence electrons. This occurs only in Period [blank_start]3[blank_end] and higher. These molecules are described as having [blank_start]expanded[blank_end] octets.
Question 11
Question
The Molecular Orbital Theory: the orbitals of an atom are replaced by [blank_start]new[blank_end] orbitals when a molecule forms. Each molecule has a [blank_start]unique[blank_end] set of molecular orbitals equal to the [blank_start]sum[blank_end] of the atomic orbitals of the original atoms. Molecular orbitals are much [blank_start]larger[blank_end] than atomic orbitals, up to the size of the entire molecule. Orbitals are ranked in order of [blank_start]increasing[blank_end] energy.
Answer
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new
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unique
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larger
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sum
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increasing
Question 12
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[blank_start]Paramagnetism[blank_end]: the attraction of a molecule to a magnetic field
Question 13
Question
Factors affected by the arrangement of a molecule's electrons:
- bond [blank_start]formation[blank_end] (bonding and antibonding)
- bond [blank_start]type[blank_end] (single, double, triple bonds)
- molecular properties (like paramagnetism)
Question 14
Question
Bonding orbitals:
- [blank_start]constructive[blank_end] interference
- [blank_start]between[blank_end] nuclei
- [blank_start]lower[blank_end] in energy than the atomic orbitals from which they form
- stable molecules
Answer
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constructive
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between
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lower
Question 15
Question
Antibonding orbitals:
- [blank_start]destructive[blank_end] interference
- [blank_start]outside[blank_end] of the molecule, far away from the nuclei
- [blank_start]higher[blank_end] in energy than the atomic orbitals
- unstable
Answer
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destructive
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outside
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higher