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CHEM 110 > CHEM 110 - FINAL > Flashcards

CHEM 110 - FINAL Flashcards

(66 cards)

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1
Q

Which kind of bond has the shortest bond length?

A

Triple Bond

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2
Q

Which bond has the longest bond length?

A

Single Bond

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3
Q

Which bond is the strongest and most difficult to break?

A

Triple bond

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4
Q

Electronegativity trend ____ across a period and ______ along the groups

A

increases (to the right), increases (up)

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5
Q

What electronegative values classify a covalent bond?

A

0

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6
Q

What electronegative values classify an ionic bond?

A

> or equal to 2

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7
Q

What electronegative values classify a polar covalent bond?

A

Values between 0 and 2

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8
Q

Increasing bond polarity is present when _____.

A

there is a dipole moment or when there are large differences in electronegativity (ie. Lithium bonding with Cl and they are far away from each other on the periodic table)

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9
Q

Formal charge formula?

A

(total # of valence electrons) - (total # of nonbonding electrons) - 1/2 (total # of bonding electrons)

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10
Q

Why is BF3 an exception to the octet rule?

A

B does not complete the octet (only forms 3 bonds)

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11
Q

Why is SF6 an exception to the octet rule?

A

It has an expanded octet - sulfur has d-orbitals that allow the element to bond to more than 3 atoms

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12
Q

Why is NO an exception to the octet rule?

A

Results in odd electron molecules (where N has 3 lone electrons)

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13
Q

How do you calculate bond enthalpy in a reaction?

A

Subtract products of bond enthalpies (would have to be given specific values) from the reactants

(Also multiply by the bond enthalpies coefficients in the reaction as well!)

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14
Q

Bond angle of tetrahedral geometry?

A

109.5 degrees

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15
Q

VSEPR model vs. molecular geometry?

A

VSEPR model: expresses how electron groups are arranged - named based on electrons repelling each other
Molecular geometry: 3D arrangement of atoms in a molecule - named based on the atom arrangement

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16
Q

When do VSEPR and molecular geometry names line up?

A

Generally when there are no lone pairs (ie. CH4 will have an electron geometry AND molecular geometry of tetrahedral)

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17
Q

Bond angle for linear compounds?

A

180 degrees

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18
Q

What is the greatest repulsive interaction within a compound?

A

lone-pair repulsion vs. lone pair repulsion

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19
Q

A lone pair will _____ the bond angle between bonding pairs (increase/decrease)

A

decrease

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20
Q

Lone pairs prefer to occupy ____ positions because they are weaker than ____ positiions

A

equatorial; axial

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21
Q

A species will be nonpolar overall if _____

A

1) individual bond dipoles cancel
OR
2) has identical bonds and a symmetrical geometry

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22
Q

A species will be polar overall if ___

A

1) individual bond dipoles do not cancel
OR
2) has an unsymmetrical geometry

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23
Q

Is CCl4 polar or nonpolar?

A

Nonpolar; it has C-Cl dipoles but they cancel out

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24
Q

AB2 - Molecular Geometry & VSEPR?

A

Linear

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25
AB3 - Molecular Geometry & VSEPR?
Trigonal Planar
26
AB4 MG & VSEPR?
Tetrahedral
27
AB5 MG & VSEPR?
Trigonal bipyramidal
28
AB6 MG & VSEPR?
Octahedral
29
AB2E VSEPR?
Trigonal planar
30
AB2E MG?
Bent
31
AB3E VSEPR?
Tetrahedral
32
AB3E MG?
Trigonal pyramidal
33
AB2E2 MG?
Bent
34
AB2E2 VSEPR?
Tetrahedral
35
AB4E VSEPR?
Trigonal bipyramidal
36
AB4E MG?
Distorted tetrahedral
37
AB3E2 VSEPR?
Trigonal bipyramidal
38
AB3E2 MG?
T-shaped
39
AB2E3 VSEPR?
Trigonal bipyramidal
40
AB2E3 MG?
Linear
41
AB5E VSEPR?
Octahedral
42
AB5E MG?
Square pyramidal
43
AB4E2 VSEPR?
Octahedral
44
AB4E2 MG?
Square planar
45
Does BrCl have a dipole moment?
Yes; polar (Cl is more electronegative)
46
Does BF3 have a dipole moment?
No dipole moment; has polar interactions but they cancel out
47
Does CH2Cl2 have a dipole moment?
Yes!
48
The closer electrons are too each other the ____ the potential energy would be?
Lower (but then it spikes up after)
49
Why do we use hybridization to describe compounds?
To describe an overlap of hybrid orbitals and consider bond types in an atom (which VSEPR and molecular geometry do not consider)
50
What type of hybridization is associated with 2 (# lone pairs + # of bonded atoms)?
sp hybridization
51
What type of hybridization is associated with 3 (# lone pairs + # of bonded atoms)?
sp2 hybridization
52
What type of hybridization is associated with 4 (# lone pairs + # of bonded atoms)?
sp3 hybridization
53
What type of hybridization is associated with 5 (# lone pairs + # of bonded atoms)?
sp3d hybridization
54
What type of hybridization is associated with 6 (# lone pairs + # of bonded atoms)?
sp3d2
55
CH4 has which hybridization type?
sp3
56
BeH2 has which hybridization type?
sp hybridization
57
PF3 hybridization?
sp3 hybridization
58
A single bond consists of ____ bond.
1 sigma bond
59
A double bond consists of ____ bonds.
1 sigma bond and 1 pi bond
60
A triple bond consists of ___ bonds.
1 sigma and 2 pi bonds
61
Molecular Orbital Configuration?
Draw from bottom up following orbital rules
62
How to calculate bond order of MO Configurations?
1/2 (# of electrons in bonding MOs - # of electrons in anti-bonding MOs)
63
Bond Enthalpy
Manipulate the 3 enthalpies, make your final lewis structure to see how many bonds need to be broken, and divide the enthalpy total by number of bonds broken
64
What kind of atoms in a lewis structure will form delocalized molecular orbitals?
Atoms that are prone to resonance structures (ie. between two oxygen bonds)
65
What is the difference between bonding and antibonding molecular orbitals?
Bonding - lower energy, more stable Antibonding - higher energy, less stable
66
When creating molecular orbitals, you always want to fill the ____ energy orbitals first.
Lower

CHEM 110 (4 decks)

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