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Part 3 Flashcards

1
Q

this is the ability of atoms to attract electrons in a bond

A

Electronegativity

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2
Q

difference in electronegativity for nonpolar covalent bond

A

<0.4

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3
Q

difference in electronegativity for polar covalent bond

A

0.4< ^EN < 1.7

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4
Q

difference in electronegativity for ionic bond

A

^EN >~ 1.7

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5
Q

is the force that holds two atoms together

A

Chemical Bond

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6
Q

is formed by the attraction of the positive nucleus of one atom and the negative electrons of another atom

A

Bond

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7
Q

these are the different types of chemical bonds

A

Metallic, Covalent, Ionic

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8
Q

this is the attraction between the electropositive atoms and the delocalized electrons within the metal lattice

A

Metallic Bond

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9
Q

this is the attraction resulting from the sharing of electrons of atoms

A

Covalent Bond

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10
Q

this results in the overlap of orbitals of the atoms

A

Covalent Bond

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11
Q

this basically means “same valency”

A

Covalent

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12
Q

this is the resulting bond when two nonmetals combine

A

Covalent Bond

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13
Q

this results from the attraction of the nucleus and the electron of two or more atoms

A

Covalent Bond

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14
Q

this is the attraction resulting from the transfer of electrons between atoms (MRII)

A

Ionic Bond

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15
Q

results when atoms of a metal (low electronegativity) and a nonmetal (high electronegativity) combine

A

Ionic Bond

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16
Q

results from the attraction of two opposite charged particles (MRII)

A

Ionic Bond

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17
Q

this type of bond involves a metal and a nonmetal

A

Ionic Bond

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18
Q

polarity of bonding is dictated by

A

electronegativity

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19
Q

this shows the direction of flow in a covalent bond; the direction of arrows

A

dipole moment

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20
Q

bonding interactions are characterized by

A

bond energy, bond length, bond order

21
Q

what are the Properties of a Chemical Bond

A
  1. Bond Energy; 2. Bond Length; 3. Bond Order
22
Q

this is the amount of energy involved when a bond is broken, which is of the same magnitude for the energy released when a bond is formed

A

Bond Energy

23
Q

is the distance between the nuclei of the atoms forming the bond

A

Bond Length

24
Q

is the number of bonds between two atoms in a covalent bond

A

Bond Order

25
Q

pertains to single bond, double bond, triple bond, and those intermediate between single and double bonds

A

Bond Order

26
Q

give the trend of the properties of bonds

A

^^ Bond Order, ^^Bond Energy , lower Bond Length

therefore, ^^ Bond Strength

27
Q

what are the octet/duet rule’s strict followers

A

H, O, N, F

28
Q

this is the apparent charge of an atom in a molecule

A

Formal Charge

29
Q

the observed tendency of each atom of the main group elements to lose, gain, or share electrons in order to acquire 8 electrons in its valence shell resulting in the same electron configuration as a noble gas

A

Octet Rule

30
Q

this rules is especially applicable to carbon, nitrogen, oxygen, and the halogens, but also to metals such sodium and magnesium

A

Octet Rule

31
Q

this represents the arrangement of valence electrons among the atoms in a molecule.

A

Lewis Structure

32
Q

these are cases wherein there is more than one Lewis Structure to represent a molecule or polyatomic ion

A

Resonance Structure

33
Q

this vary in their contribution to the true structure of the molecule or ion. Some of “this” are equivalent and contribute equally to the true strunture

A

Resonance Structure

34
Q

the model used for the approximation of molecular geometry is

A

VSEPR or valence shell electron pair

35
Q

this states that the structure around an atom is determined principally by minimizing electron pair repulsions

A

VSEPR or valence shell electron pair

36
Q

this type of geometry only considers the arrangement of the bonds, ignoring the lone pairs

A

Molecular geometry

37
Q

this type of geometry considers the arrangement of all electron pairs

A

Electron pair geometry

38
Q

what is the meaning of IMFA

A

Intermolecular Forces of Attraction

39
Q

collective term for all the interactions of all the molecules

A

Van der Waals Forces

40
Q

what are the three types of IMFA

A
  1. London Dispersion Force (LDF)
  2. Dipole-Dipole Interaction (DDI)
  3. Hydrogen Bonding (HB)
41
Q

this IMFA has a temporary or instantaneous dipole; this also exists in all molecules and atoms

A

London Dispersion Force (LDF)

42
Q

what are the two factors that affect LDF and how do they affect it?

A
  1. Molar mass - direct proportional; higher mass molar mass means higher dipole
  2. Arrangement - the more linear, the stronger LDF
43
Q

this IMFA is exhibited by polar molecules; has a permanent dipole; and is generally stronger than LDF

A

Dipole-Dipole Interaction (DDI)

44
Q

this IMFA is a special type of DDI which is the strongest among the three

A

Hydrogen Bonding

45
Q

this type of IMFA is present is the number is bonded to a highly electronegative atom (F,O,N)

A

Hydrogen Bonding

46
Q

this type of interaction is technically not an intermolecular force (not IMFA) but is an interaction

A

Ion-Dipole Interaction

47
Q

what are some of the properties that are affected by IMFA

A
  1. Directly Proportional:
    - Boiling/Melting Point
    - Heat of Vaporization/Fusion
    - Viscosity
    - Surface Tension
  2. Inversely Proportional:
    - Vapor Pressure
48
Q

what are the general guidelines for assessment for the IMFA

A
  1. difference in molar mass, significantly large, LDF will dominate
  2. difference in molar mass, NOT significantly large, DDI will dominate
  3. Hydrogen Bonding will generally dominate

GIC (2 decks)

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