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CHEM 111 > Exam 3 > Flashcards

Exam 3 Flashcards

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1
Q

Chemical Bond

A

The forces that hold the atoms together in substances

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2
Q

Lewis electron-dot symbol

A

The symbol of the element with one dot to represent each valence electron

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3
Q

Ionic Bonding

A

The bonding that results from the electrostatic attraction between positively charged cations and negatively charged anions

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4
Q

Lattice Energy

A

The energy required to separate one mole of an ionic solid into isolated gaseous ions

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5
Q

Antibonding Molecular Orbital

A

an orbital that reduces the electron density in the region between the atoms in the molecule

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6
Q

Bonding Pairs

A

pairs of electrons shared between two atoms

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7
Q

Central Atom

A

an atom bonded to two or more other atoms

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8
Q

Covalent Bond

A

the bond that arises from atoms sharing electron pairs

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9
Q

Double Bond

A

The bond formed by sharing two pairs of electrons between two atoms

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10
Q

Lewis Structure

A

a representation of covalent bonding, using Lewis symbols, that shows shared electrons as dots or lines between atoms and unshared electrons as dots

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11
Q

Lone Pairs

A

Pairs of electrons that are not shared

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12
Q

Octet Rule

A

Each atom in a molecule shares electrons until it is surrounded by eight valence electrons. The octet rule is most important for elements in the second period

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13
Q

Dipole Moment

A

The magnitudes of separated charges times the distance between the charges

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14
Q

Single Bond

A

the bond formed by sharing one pair of electrons between two atoms

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15
Q

Skeleton Structure

A

the drawing that shows which atoms are bonded to each other in a molecule

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16
Q

Triple Bond

A

the bond formed by sharing three pairs of electrons between two atoms

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17
Q

Expanded Valence Shell Molecule

A

A molecule with more than eight electrons about an atom in a Lewis structure

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18
Q

Hybrid Orbitals

A

Orbitals obtained by mixing two or more atomic orbitals on the same atom

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19
Q

Isomers

A

Different compounds with the same molecular formula but with different structural formulas

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20
Q

Resonance Structures

A

structures that differ only in the distribution of the valence electrons; the skeleton structure does not change, only the placement of the electrons

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21
Q

Bonding Molecular Orbital

A

an orbital that concentrates the electron density between the atoms in the molecule

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22
Q

Homonuclear Diatomic Molecule

A

a molecule formed by two atoms of the same element

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23
Q

Odd Electron Molecule

A

any molecule that has an odd number of valence electrons must violate the octet rule

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24
Q

Oxyacid

A

a molecule of the general formula (OH)mXOn that has at least one hydrogen atom attached to an oxygen atom

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25
Q

Delocalized Molecular Orbital

A

A molecular orbital that involves atomic orbitals on more than two atoms

26
Q

Heteronuclear Diatomic Molecule

A

a molecule formed by one atom of each of two different elements

27
Q

Molecular Shape

A

a description of the positions of the atoms, not the lone pairs

28
Q

Valence-Shell Electron-Pair Repulsion (VSEPR)

A

a model that predicts the shapes of molecules that is based on the premise that electron pairs on a central atom repel each other so they are as far apart as possible

29
Q

Polar Molecule

A

a molecule that contains an unequal distribution of charge and thus has a dipole moment

30
Q

Valence Bond Theory

A

a theory that describes bonds as being formed by atoms sharing valence electrons in overlapping valence orbitals

31
Q

Sigma Bond

A

a bond in which the shared pair of electrons is concentrated along the line joining the nuclei of the bonded atoms

32
Q

Heteronuclear Diatomic Molecule

A

a molecule formed by one atom of each of two different elements

33
Q

Polar Bond

A

a covalent bond in which the bonding electrons are not equally shared by the two atoms

34
Q

Molecular Orbital Theory

A

a model that treats bonding as delocalized over the entire molecule

35
Q

Intermolecular Forces

A

the attractive forces that exist between molecules

36
Q

Boiling Point

A

the temperature at which the vapor pressure of a liquid is equal to the applied pressure

37
Q

Condensation

A

the conversion of a gas to a liquid

38
Q

Critical Pressure

A

the minimum pressure needed to cause the liquid state to exist up to the critical temperature

39
Q

Critical Temperature

A

the maximum temperature at which a substance can exist in the liquid phase

40
Q

Deposition

A

the direct conversion of a gas to a solid. Deposition is the reverse of sublimation

41
Q

Dynamic Equilibrium

A

a situation in which two opposing changes occur at equal rates, so no net change is apparent

42
Q

Enthalpy of Fusion

A

the enthalpy change that accompanies the conversion of one mole of a solid to the liquid phase

43
Q

Enthalpy of Sublimation

A

the enthalpy change for the conversion of one mole of a solid to the gaseous state

44
Q

Enthalpy of Vaporization

A

the enthalpy change that accompanies the conversion of one mole of a liquid to the gas phase

45
Q

Evaporation

A

the escape of molecules from the liquid phase into the gas phase

46
Q

Melting Point

A

the temperature at which a solid substance changes to the liquid phase

47
Q

Normal Boiling Point

A

the boiling point at a pressure of 1 atm

48
Q

Sublimation

A

the direct conversion of a solid to a gas without first changing to a liquid

49
Q

Supercooling

A

reducing the temperature of a liquid below its freezing point without forming a solid. This is an unstable condition

50
Q

Supercritical Fluid

A

the single fluid phase that exists above the critical temperature and pressure

51
Q

Vapor Pressure

A

the partial pressure of a substance that is in equilibrium with one of the condensed phases of that substance

52
Q

Phase Diagram

A

a graph of pressure versus temperature that shows the regions of stability for each phase (solid, liquid, and gas). The lines between the phases represent conditions of temperature and pressure at which two or more phases are in equilibrium

53
Q

Triple Point

A

the unique combination of pressure and temperature at which all three phases (solid, liquid, and gas) exist in equilibrium

54
Q

Dipole-Dipole Attraction

A

the intramolecular forces that arise from electrostatic attractions between molecular dipoles

55
Q

Dipole-Induced Dipole Attraction

A

the intramolecular force that arises between a polar molecule and an induced dipole moment in a nonpolar molecule

56
Q

Hydrogen Bonding

A

a particularly strong intermolecular attraction between a hydrogen atom that is bonded to a highly electronegative atom and a lone pair of electrons on N, O, or F .

57
Q

Induced Dipole

A

a dipole caused by the presence of an electrical charge close to an otherwise nonpolar molecule

58
Q

Instantaneous Dipole

A

a dipole moment that results from unequal charge distribution within a molecule caused by the motion of the electrons

59
Q

London Dispersion Forces

A

the instantaneous dipole-induced dipole attractions that explain the attractions between nonpolar molecules, but contribute to the attractions between all molecules

60
Q

Polarizability

A

the ease with which the electron cloud of a molecule can be distorted

61
Q

van der Waals Forces

A

the weak intermolecular forces between small molecules. The term includes both dipole-dipole attractions and London dispersion forces

CHEM 111 (4 decks)

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