Brainscape's Knowledge GenomeTM

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


See full index

MCAT-GENERAL CHEMISTRY > Bonding and Intermolecular Forces > Flashcards

Bonding and Intermolecular Forces Flashcards

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

single bond

A

a bond formed from two electrons

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

how many electrons are involved in a double bond?

A

4

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

how many electrons are involved in a triple bond?

A

6

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

resonance hybrid

A

the “average” of possible resonance structures

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

bond dissociation energy (BDE)

A

the energy required to break a bond homolytically

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

homolytic bond cleavage

A

one electron of the bond being broken goes to each fragment of the molecule

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

heterolytic bond cleavage (dissociation)

A

both electrons of the electron pair that make up the bond end up the same atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

what does homolytic bond cleavage form?

A

radicals (has BDE)

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

what does heterolytic bond cleavage form?

A

ions

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

are the energies of heterolytic and homolytic bond breaking similar?

A

no, completely different energies

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

for similar bonds, the higher the bond order…

A

the shorter and stronger the bond

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

bond order

A

the number of bonds between adjacent atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

comparisons of bond length and BDE should only be made for:

A

similar bonds

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

the greater the s-character in the hybrid orbitals:

A

the shorter the bond (s-orbitals are closer to the nucleus)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

when comparing the same types of bonds, the longer the bond….

A

the weaker it is, the shorter the bond, the stronger it is

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

covalent bond

A

formed between atoms when each contributes one or more of its unpaired valence electrons so that the electrons are shared by both atoms to help complete both octets

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

polarity

A

when a molecule is partially negative on one end and partially positive on the other end

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

dipole moment

A

the polarity present in a polar molecule

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

what constitutes a polar bond?

A

if the electron density between the two nuclei is uneven

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

the greater the difference in electronegativity of the bonding atoms…

A

the more uneven the electron density and the greater the dipole moment

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

what constitutes a nonpolar bond?

A

the electron density between the two nuclei is even

22
Q

coordinate covalent bond

A

when one atom donates both of the shared electrons in a bond

23
Q

what are two other synonyms for Lewis base?

A

ligand or nucleophile

24
Q

what’s another word for Lewis acid?

A

electrophile

25
Q

what happens to the electrons in the breaking of a coordinate covalent bond?

A

the electrons that come from the ligand will leave with that ligand

26
Q

ionic bond

A

cation and anions held together by electrostatic attraction

27
Q

in ionic bonds, what is the strength of the bond proportional to?

A

the charges on the ions

28
Q

in ionic bonds, what is the strength of the bond inversely proportional to?

A

the distance between ions, or the ionic radii

29
Q

valence shell electron-pair repulsion theory (VSEPR)

A

since electrons repel one another, electron pairs, whether bonding or nonbonding, attempt to move as far apart as possible

30
Q

molecular geometry

A

the shape of a molecule

31
Q

how are sigma bonds formed?

A

formed by the end-to-end overlap of one hybridized orbital (or an s orbital in the case of hydrogen) from each of the two atoms participating in the bond

32
Q

sigma bond

A

consists of two electrons that are localized between two nuclei

33
Q

how are pi bonds formed?

A

formed by the proper, parallel, side-to-side alignment of two unhybridized p orbitals on adjacent atoms

34
Q

pi bond

A

composed of two electrons that are localized to the region that lies on opposite sides of the plane formed by the two bonded nuclei and immediately adjacent atoms, not directly between the two nuclei

35
Q

intermolecular forces

A

the relatively weak interactions that take place between neutral molecules

36
Q

ion-dipole forces

A

polar molecules are attracted to ions

37
Q

dipole-dipole forces

A

attraction between the positive end of one polar molecule and the negative end of another polar molecule

38
Q

what is the strongest dipole-dipole force?

A

hydrogen-bonding

39
Q

dipole-induced dipole force

A

a permanent dipole in one molecule induces a momentary dipole in a neighbouring nonpolar molecule

40
Q

London dispersion forces

A

an instantaneous dipole in a nonpolar molecule may induce a dipole in a neighbouring nonpolar molecule: weak and transient interaction

41
Q

how could LDF forces increase?

A

if size of molecule and its number of electrons increases-this increases partial charge of induced dipole

42
Q

van der Waals forces

A

collectively refers to dipole forces, hydrogen bonding, and London forces

43
Q

what is required for hydrogen bonding to occur?

A

1) a molecule must have a covalent bond between H and either N, O, or F
2) a molecule must have a lone pair of electrons on an N, O, or F atom

44
Q

vapour pressure

A

the pressure exerted by the gaseous phase of a liquid that evaporated from the exposed surface of the liquid

45
Q

what is the relationship between a substance’s intermolecular forces and vapour pressure?

A

weaker intermolecular forces=higher vapour pressure, more easily evaporated

46
Q

volatile

A

easily vaporized liquids

47
Q

aside from intermolecular forces, what influences vapour pressure?

A

temperature: increased temperature of substance=increased vapour pressure

48
Q

ionic solid

A

held together by the electrostatic attraction between cations and anions in a lattice structure; the bonds that hold all the ions together in the crystal lattice are the same as the bonds that hold each pair of ions together

49
Q

network solid

A

atoms are connected in a lattice of covalent bonds (all interactions between atoms are covalent bonds); the intermolecular forces are identical to the intramolecular forces

50
Q

metallic solids

A

a covalently bound lattice of nuclei and their inner shell electrons surrounded by a “sea” of electrons

51
Q

conduction electrons

A

freely roaming valence electrons in metallic solids that are not bound to any particular atom and is free to move throughout the lattice, allows for excellent conduction of electricity and heat

52
Q

molecular solids

A

the particles at the lattice points of a crystal of a molecular solid are molecules held together by one of the three types of intermolecular interactions (H bond, dipole, LDF)

MCAT-GENERAL CHEMISTRY (6 decks)

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