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chem 110 > CHEM 110 - FINAL > Flashcards

CHEM 110 - FINAL Flashcards

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AP® Chemistry flashcards Periodic Table flashcards
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
Q

AB3 - Molecular Geometry & VSEPR?

A

Trigonal Planar

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26
Q

AB4 MG & VSEPR?

A

Tetrahedral

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27
Q

AB5 MG & VSEPR?

A

Trigonal bipyramidal

28
Q

AB6 MG & VSEPR?

A

Octahedral

29
Q

AB2E VSEPR?

A

Trigonal planar

30
Q

AB2E MG?

A

Bent

31
Q

AB3E VSEPR?

A

Tetrahedral

32
Q

AB3E MG?

A

Trigonal pyramidal

33
Q

AB2E2 MG?

A

Bent

34
Q

AB2E2 VSEPR?

A

Tetrahedral

35
Q

AB4E VSEPR?

A

Trigonal bipyramidal

36
Q

AB4E MG?

A

Distorted tetrahedral

37
Q

AB3E2 VSEPR?

A

Trigonal bipyramidal

38
Q

AB3E2 MG?

A

T-shaped

39
Q

AB2E3 VSEPR?

A

Trigonal bipyramidal

40
Q

AB2E3 MG?

A

Linear

41
Q

AB5E VSEPR?

A

Octahedral

42
Q

AB5E MG?

A

Square pyramidal

43
Q

AB4E2 VSEPR?

A

Octahedral

44
Q

AB4E2 MG?

A

Square planar

45
Q

Does BrCl have a dipole moment?

A

Yes; polar (Cl is more electronegative)

46
Q

Does BF3 have a dipole moment?

A

No dipole moment; has polar interactions but they cancel out

47
Q

Does CH2Cl2 have a dipole moment?

A

Yes!

48
Q

The closer electrons are too each other the ____ the potential energy would be?

A

Lower (but then it spikes up after)

49
Q

Why do we use hybridization to describe compounds?

A

To describe an overlap of hybrid orbitals and consider bond types in an atom (which VSEPR and molecular geometry do not consider)

50
Q

What type of hybridization is associated with 2 (# lone pairs + # of bonded atoms)?

A

sp hybridization

51
Q

What type of hybridization is associated with 3 (# lone pairs + # of bonded atoms)?

A

sp2 hybridization

52
Q

What type of hybridization is associated with 4 (# lone pairs + # of bonded atoms)?

A

sp3 hybridization

53
Q

What type of hybridization is associated with 5 (# lone pairs + # of bonded atoms)?

A

sp3d hybridization

54
Q

What type of hybridization is associated with 6 (# lone pairs + # of bonded atoms)?

A

sp3d2

55
Q

CH4 has which hybridization type?

A

sp3

56
Q

BeH2 has which hybridization type?

A

sp hybridization

57
Q

PF3 hybridization?

A

sp3 hybridization

58
Q

A single bond consists of ____ bond.

A

1 sigma bond

59
Q

A double bond consists of ____ bonds.

A

1 sigma bond and 1 pi bond

60
Q

A triple bond consists of ___ bonds.

A

1 sigma and 2 pi bonds

61
Q

Molecular Orbital Configuration?

A

Draw from bottom up following orbital rules

62
Q

How to calculate bond order of MO Configurations?

A

1/2 (# of electrons in bonding MOs - # of electrons in anti-bonding MOs)

63
Q

Bond Enthalpy

A

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
Q

What kind of atoms in a lewis structure will form delocalized molecular orbitals?

A

Atoms that are prone to resonance structures (ie. between two oxygen bonds)

65
Q

What is the difference between bonding and antibonding molecular orbitals?

A

Bonding - lower energy, more stable
Antibonding - higher energy, less stable

66
Q

When creating molecular orbitals, you always want to fill the ____ energy orbitals first.

A

Lower

chem 110 (4 decks)

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