Chapter 3 Flashcards

1
Q

A sigma bond is formed by the overlap of atomic orbitals.

A

True

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2
Q

Bonds can be sigma or pi; no antibonding in Valence Bond Theory.

A

True

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3
Q

In transition metals, which are considered valence electrons?

A

Electrons in the ns and (n-1)d orbitals.

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4
Q

Ionic Bonds

A

Metal + Nonmetal (Normally)

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5
Q

Covalent Bond

A

Nonmetal atoms (Normally)

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6
Q

Formal Charge equation

A

FC=X-(Z/2)-Y where X are the electrons in the free atom, Z are the shared electrons, and Y are nonbonding electrons

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7
Q

The octect rule only applies for the second row of the periodic table.

A

True

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8
Q

What are some exceptions to the octect rule?

A
  1. When the number of total electrons is an odd number, no full octects are possible
  2. NO, BF3 are electron deficient
  3. PCl5 has an expanded octect (possible for 3rd row and below)
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9
Q

Molecular Geometries name molecules looking ONLY at bonds.

A

True

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10
Q

Order of polarity of Hydrogen halides in gas form

A

HF>HCl>HBr>HI

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11
Q

Order of polarity of Hydrogen halides in water

A

HF

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12
Q

The bonds in a molecule can be polar but the overall molecule can be nonpolar.

A

True; because of the overall dipole moment

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13
Q

Bond Order equation

A

Bond Order=(Total # of electron pairs used for a type of bond)/(Total # of bonds of that type)

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14
Q

Bond length depends on size of bonded atoms

A

True; bigger atoms show longer bonds

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