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AP Chem > Chapter 8 & 9 > Flashcards

Chapter 8 & 9 Flashcards

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1
Q

Electrons are transferred; electronegativity differences are generally greater than 1.7; formation is always exothermic

A

ionic bonding

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2
Q

Electronegativity difference is not the final determination of __ __; compounds are ionic if they conduct electricity in their __ state

A

ionic charactermolten

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3
Q

__ are larger than __ because of higher effective nuclear charge

A

anions, cations

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4
Q

Ionic compounds form solid crystals at __ temperatures; ionic compounds organize in a characteristic __ __ of alternating positive and negative ions; all __ are ionic compounds and form crystals

A

ordinarycrystal latticesalts

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5
Q

Properties of Ionic compounds:Structure:Melting point:Boiling point:Electrical conductivity:Solubility in H2O:

A

Structure: crystalline solidsMelting point: generally highBoiling point: generally highElectrical conductivity: excellent conductors in molten and aqueous statesSolubility in H2O: generally soluble

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6
Q

Ionic size from largest to smallest with charges:3+, 2+, +, -, 2-

A

2- > - > + > 2+ > 3+

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7
Q

Greater the effective nuclear charge, __ the ionic size

A

smaller

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8
Q

nonmetal atoms come together to form bonds to become more stable by sharing electrons to achieve a noble gas electron configuration; type of bond that holds atoms together in a molecule

A

covalent bonding

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9
Q

atoms form covalent bonds in such a way that all atoms get 8 electrons in its highest occupied energy level, except hydrogen which only needs 2 electrons

A

octet rule

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10
Q

ability of an atom in a bond to attract shared electrons to itself; __ across a period and up a group

A

electronegativityincreases

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11
Q

electrons are equally shared; electronegativity difference of 0 - .4

A

Non polar-covalent bonds

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12
Q

electrons are unequally shared; electronegativity difference of .5 - 1.7; has two poles- a positive and negative end

A

polar covalent bond

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13
Q

Polar bonds:electrons concentrate around the more __ atom in a molecule; atom gains a partial __ charge; since electrons spend __ time around the other atom, other atom gains a partial __ charge

A

electronegativenegativelesspositive

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14
Q

Covalent bonding forces:Electron - electron __ forcesProton - proton __ forcesElectron - proton __ forces

A

repulsiverepulsiveattractive

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15
Q

1) Longest and weakest bonds2) shortest and stronger than single bonds3) shortest and strongest type of covalent bond

A

1) single bonds2) double bonds3) triple bonds

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16
Q

distance between the nuclei of two covalently bonded atoms; optimum distance __ attraction, __ repulsions

A

bond lengthmaximizingminimizing

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17
Q

Shorter bond length = __ bond energy = __ bondBonds b/w elements become __ and __ as multiplicity increases

A

higherstrongershorterstronger

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18
Q

polarity depends on __ __ and __ around central atom

A

individual bondsgeometry

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19
Q

representative elements generally form __ to achieve a noble gas configuration

A

ions

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20
Q

ions from representative metals are usually __ with one of the noble gases (have the same electron configuration)

A

isoelectronic

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21
Q

Transition metals lose __ electrons before the __ electrons when forming cations

A

sd

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22
Q

distance from the nucleus to the outermost electrons in an ion

A

ionic radii

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23
Q

An atom loses electrons to form a __; it has a __ radius than its corresponding atom

A

cationsmaller

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24
Q

An atom gains electrons to form an __; it has a __ radius than its corresponding atom

A

anionlarger

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25
Q

innermost electrons belonging to filled electron shells

A

core electrons

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26
Q

electrons in the outermost shell; they combine with other atoms with unfilled shells to become stable; lead to chemical bonds and reactions b/w atoms

A

valence electrons

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27
Q

Many bonds forming, a lot of __ is released; __ released more than makes up for the __ __ required

A

energyenergyionization energy

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28
Q

energy required to convert and ionic compound into gaseous ions; quantitative measure of the strength of the ionic bonds in the compound

A

lattice energy

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29
Q

Relative strength of an ionic bonds is determined by the following:1) Charges of ions: __ the charge, the stronger the bond2) Distance b/w two ions: __ distance, stronger the bond

A

highershorter

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30
Q

The strength of the ionic bond is generally determined foremost by the __, and only if the __ are similar does one compare the distance b/w nuclei to determine the strength of the bond and the resulting lattice energy

A

chargescharges

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31
Q

Estimate heat of formation for NaCl:Na(s) + 1/2 Cl2(g) -> NaCl(s)Lattice energy = -786 kJ/molIonization energy for Na = 495 kJ/molElectron affinity for Cl = - 349 kJ/molBond energy of Cl2 = 239 kJ/molEnthalpy of sublimation for Na = 109 kJ/mol

A

Na(s) -> Na(g) = 109 kJ/molNa(g) -> Na+(g) + e- = 495 kJ/mol1/2Cl2(g) -> Cl(g) = 1/2(239 kJ/mol)Cl(g) + e- -> Cl-(g) = - 349 kJ/molNa+(g) + Cl-(g) -> NaCl(s) = -786 kJ/molTOTAL:Na(s) + 1/2Cl2(g) -> NaCl(s) = -412 kJ/mol

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32
Q

ions form in a __ state

A

gaseous

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33
Q

energy required to break a particular bond in the gas phase; always positive since it takes energy to break a bond; quantitative measure of a bond’s strength (__)

A

bond energystability

34
Q

Enthalpy of formation = sum of bonds broken (energy __) - sum of bonds formed (energy __)

A

requiredreleased

35
Q

__ bonds always requires energy (endothermic, +)__ bonds always releases energy (exothermic, -)

A

breakingforming

36
Q

covalent compounds involve atoms of __ only

A

nonmetals

37
Q

the term __ is used exclusively for covalent bonding

A

molecule

38
Q

When drawing lewis structure, put least __ atom as central atom and surround with other atoms

A

electronegative

39
Q

ternary oxyacids contain __, __, and one other element

A

oxygenhydrogen

40
Q

In ternary oxyacids, the central atom is the __ element which is surrounded by __ and the __ atoms are bonded directly to the __ atoms

A

otheroxygenhydrogenoxygen

41
Q

what atoms are satisfied with less than an octet?

A

Be, and B

42
Q

Atoms is and beyond the __ period can have more than 8 electrons when in a compound

A

third

43
Q

hypothetical charge an atom would have if bonding electrons are shared equally and lone pairs belong solely to a single atom

A

formal charge

44
Q

formal charge = total # of __ electrons - total # of __ electrons - total # of __

A

valencenonbondingbonds

45
Q

For neutral molecules, sum of formal charges must equal _. For ions, the sum of formal charges must equal __

A

0charge

46
Q

Lewis formulas with no formal charges is __ to one with formal charges; Lewis formula with large formal charges is __ plausible than one with lower formal charges; most plausible formula has negative formal charge on __ electronegative atom

A

preferablelessmore

47
Q

electrons spread between more than two atoms

A

delocalized electrons

48
Q

one of two or more lewis structures representing a single molecule that cannot be described fully with only one lewis structure

A

resonance structure

49
Q

the 3-D arrangement of atoms in molecules; responsible for many physical and chemical properties of molecules

A

molecular geometry (shape)

50
Q

a molecule’s shape results from the electrons on its central atom orienting themselves to be as far away from each other as possible

A

VSEPR model

51
Q

If there are only two atoms, the molecule must be __

A

linear

52
Q

If there are more than two atoms in the molecule, the shape depends on the number of __ around the central atom

A

electrons

53
Q

Hydrogen forms __ covalent bond

A

one

54
Q

Oxygen and Sulfur form __ covalent bonds (__ double or __ single bonds)

A

212

55
Q

Nitrogen and Phosphorus form __ covalent bonds(__ triple bond, __ single bonds, or __ double & __ single bond)

A

3, 1, 3, 1, 1

56
Q

Carbon and Silicon form __ covalent bonds (__ double bonds, __ single bonds, __ triple & __ single, or __ double & __ single bonds)

A

4, 2, 4, 1, 1, 1, 2

57
Q

Resonance bonds are __ and __ than single bonds. They are also __ and __ than double bonds

A

shorterstrongerlongerweaker

58
Q

electron pairs can be thought of as belonging to pairs of atoms when bonding

A

LEM model

59
Q

Shape: Shared electrons (bonds): 2Lone pairs of electrons: 0Hybridization:Bond angle(s):

A

Shape: linearShared electrons (bonds): 2Lone pairs of electrons: 0Hybridization: spBond angle(s): 180

60
Q

Shape:Shared electrons (bonds): 3Lone pairs of electrons: 0Hybridization:Bond angle(s):

A

Shape: trigonal planarShared electrons (bonds): 3Lone pairs of electrons: 0Hybridization: sp2Bond angle(s): 120

61
Q

Shape:Shared electrons (bonds): 2Lone pairs of electrons: 1Hybridization:Bond angle(s):

A

Shape: bentShared electrons (bonds): 2Lone pairs of electrons: 1Hybridization: sp2Bond angle(s): 120>

62
Q

Shape:Shared electrons (bonds): 4Lone pairs of electrons: 0Hybridization:Bond angle(s):

A

Shape: tetrahedralShared electrons (bonds): 4Lone pairs of electrons: 0Hybridization: sp3Bond angle(s): 109.5

63
Q

Shape:Shared electrons (bonds): 3Lone pairs of electrons: 1Hybridization:Bond angle(s):

A

Shape: trigonal pyramidalShared electrons (bonds): 3Lone pairs of electrons: 1Hybridization: sp3Bond angle(s): 109.5>

64
Q

Shape:Shared electrons (bonds): 2Lone pairs of electrons: 2Hybridization:Bond angle(s):

A

Shape: bentShared electrons (bonds): 2Lone pairs of electrons: 2Hybridization: sp3Bond angle(s): 109.5>

65
Q

Shape:Shared electrons (bonds): 5Lone pairs of electrons: 0Hybridization:Bond angle(s):

A

Shape: trigonal bipyramidalShared electrons (bonds): 5Lone pairs of electrons: 0Hybridization: sp3dBond angle(s): 90 and 120

66
Q

Shape:Shared electrons (bonds): 4Lone pairs of electrons: 1Hybridization:Bond angle(s):

A

Shape: see-sawShared electrons (bonds): 4Lone pairs of electrons: 1Hybridization: sp3dBond angle(s): 90> & 120>

67
Q

Shape:Shared electrons (bonds): 3Lone pairs of electrons: 2Hybridization:Bond angle(s):

A

Shape: T-shapedShared electrons (bonds): 4Lone pairs of electrons: 1Hybridization: sp3dBond angle(s): 90> & 120>

68
Q

Shape:Shared electrons (bonds): 2Lone pairs of electrons: 3Hybridization:Bond angle(s):

A

Shape: linearShared electrons (bonds): 4 Lone pairs of electrons: 1Hybridization: sp3dBond angle(s): 180

69
Q

Shape:Shared electrons (bonds): 6Lone pairs of electrons: 0Hybridization:Bond angle(s):

A

Shape: octahedralShared electrons (bonds): 6Lone pairs of electrons: 0Hybridization: sp3d2Bond angle(s): 90

70
Q

Shape:Shared electrons (bonds): 5Lone pairs of electrons: 1Hybridization:Bond angle(s):

A

Shape: square pyramidShared electrons (bonds): 5Lone pairs of electrons: 1Hybridization: sp3d2Bond angle(s): 90>

71
Q

Shape:Shared electrons (bonds): 4Lone pairs of electrons: 2Hybridization:Bond angle(s):

A

Shape: square planarShared electrons (bonds): 4Lone pairs of electrons: 2Hybridization: sp3d2Bond angle(s): 90

72
Q

__ is the combining of two or more orbitals of nearly equal energy within the same atom into orbitals of equal energy

A

Hybridization

73
Q

In the case of methane, they call the hybridization sp3, meaning that an __ orbital is combined with three __orbitals to create __ equal hybrid orbitals. These new orbitals have slightly __ energy than the 2s orbital and slightly energy than the 2p orbitals.

A

spfourmoreless

74
Q

sp hybridization, in which one _ orbital combines with a single _ orbital. This produces _ hybrid orbitals, while leaving _ normal p orbitals

A

sp2two

75
Q

Another hybrid is the sp2, which combines two orbitals from a _ sublevel with one orbital from an _ sublevel. _ p orbital remains unchanged.

A

psOne

76
Q

attractions between moleculesoccur within a molecule and include covalent bonds b/w atoms

A

intermolecular forcesintramolecular forces

77
Q

Intermolecular attractions:1) attractions b/w opposite charges, strongest kind2) attraction b/w 2 polar molecules that increases with higher polarity3) special type of dipole-dipole b/w H, F, O or N4) occur in all substances, very weak

A

1) ion-ion2) dipole-dipole3) hydrogen bonding4) london dispersion forces

78
Q

Put the four types of intermolecular attractions in order from strongest to weakest

A

ion-ion, hydrogen bonding, dipole-dipole, dispersion

79
Q

Flame Tests: Red/orange: __, orange: __, orange/yellow: __, magenta: __, yellow/green: __, green/blue: __, violet: __, white: ___

A

Red/orange: strontium, orange: calcium, orange/yellow: sodium, magenta: lithium, yellow/green: barium, green/blue: copper, violet: potassium, white: magenesium

80
Q

Single bond: _ sigma bond(s), _ pi bond(s)Double bond: _ sigma bond(s), _ pi bond(s)Triple bond: _ sigma bond(s), _ pi bond(s)

A

Single bond: 1 sigma bond(s), 0 pi bond(s)Double bond: 1 sigma bond(s), 1 pi bond(s)Triple bond: 1 sigma bond(s), 2 pi bond(s)

81
Q

Bond order:0: __ 1: __2: __3: __

A

0: doesn’t exist1: single bond2: double bond3: triple bond

AP Chem (11 decks)

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