Chapter 9 Flashcards

1
Q

What are bond angles?

A

angles made by the lines joining the nuclei of atoms

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2
Q

What 2 things determine the size and shape of the molecule?

A

bond angles and bond lengths

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3
Q

What is a tetrahedral?

A

4 corners, 4 faces, each an equilateral triangle

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4
Q

What is a bent shape?

A

if atom A lies above 2 atom Bs

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5
Q

What is a trigonal planar?

A

if atom A is on the same plane as atom Bs

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6
Q

What is a trigonal pyrimidal?

A

if atom A lies above the plane of 3 atom Bs

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7
Q

What are the 5 basic molecular arrangement shapes?

A

linear AB2 | trigonal pyramidal AB3 | tetrahedral AB4 | trigonal bipyramidal AB5 | octahedral AB6

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8
Q

What does VESPR stand for?

A

valence shell electron pair

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9
Q

What is the VESPR model?

A

based on the idea that electron domains are negatively charged and repel one another

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10
Q

What is an electron domain?

A

a region in which the bonding-pair electrons are found

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11
Q

What is the best arrangement of a given number of electron domains?

A

one that minimizes the repulsions among them

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12
Q

What is electron domain geometry?

A

arrangement of electron domains about the central atom of an ABn molecule/ion (includes lone pairs)

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13
Q

What is molecular geometry?

A

an arrangement of the atoms

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14
Q

How can we determine the molecular geometry?

A

based on how many electron domains there are due to bonds

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15
Q

What is the effect of non-bonding electrons on bond angles?

A

exert a greater repulsive force on neighboring electron domains = compress (decrease) bond angles

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16
Q

What is the effect of multiple bonds on bond angles?

A

multiple bonds = larger electron domains = exert greater repulsive force on neighboring electron domains

17
Q

What is the most stable 5 electron domain shape and why?

A

trigonal bipyramidal due to less repulsion

18
Q

What is the most stable 6 electron domain shape and why?

A

octahedron, all angles are 90

19
Q

How are the shapes of larger molecules determined?

A

determine VESPR shape of each central atom

20
Q

What does the dipole moment depend on for molecules with 2< atoms?

A

both the polarities of the individual bonds and the geometry of the molecule

21
Q

What indicates if a molecule with 2< atoms is nonpolar?

A

dipole vectors point at OPPOSITE directions

22
Q

What indicates if a molecule with 2< atoms is polar?

A

dipole vectors point at the SAME direction

23
Q

What is the valence bind theory?

A

bonding electron pairs are concentrated in the regions between atoms | nonbonding e- pairs lie in regions in space

24
Q

What is Lewis’s theory?

A

covalent bonding happens due to the concentration of electron density between 2 nuclei from the atoms sharing electrons

25
Q

What is the optimum distance between 2 nuclei in a covalent bond?

A

when the attractive forces between opposite charges are balanced by the repulsive forces between like charges