Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

CHEM 110 > CHEM 110 - FINAL > Flashcards

CHEM 110 - FINAL Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

Which kind of bond has the shortest bond length?

A

Triple Bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Which bond has the longest bond length?

A

Single Bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Which bond is the strongest and most difficult to break?

A

Triple bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Electronegativity trend ____ across a period and ______ along the groups

A

increases (to the right), increases (up)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What electronegative values classify a covalent bond?

A

0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What electronegative values classify an ionic bond?

A

> or equal to 2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What electronegative values classify a polar covalent bond?

A

Values between 0 and 2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Formal charge formula?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Why is BF3 an exception to the octet rule?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Why is NO an exception to the octet rule?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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!)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Bond angle of tetrahedral geometry?

A

109.5 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Bond angle for linear compounds?

A

180 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What is the greatest repulsive interaction within a compound?

A

lone-pair repulsion vs. lone pair repulsion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

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

A

decrease

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

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

A

equatorial; axial

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

A species will be nonpolar overall if _____

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

A species will be polar overall if ___

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Is CCl4 polar or nonpolar?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

AB2 - Molecular Geometry & VSEPR?

A

Linear

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

AB3 - Molecular Geometry & VSEPR?

A

Trigonal Planar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

AB4 MG & VSEPR?

A

Tetrahedral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions