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GEN CHM > Vocab & Trends > Flashcards

Vocab & Trends Flashcards

1
Q

What is the difference between Paramagnetic and Diamagnetic?

A

Paramagnetic: unpaired e-

Diamagnetic: paired e-

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2
Q

What are the 5 elements that are exceptions to the electron configuration rule?

eg. [Ar] 4s1, 3d5

A

Cr Cu
Mo Ag
Au

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3
Q

What are symbols and names of the 4 quantum numbers?

A

Name what?

n—>”principal #” —> Shell
l —>”azimuthal #” —-> Subshell
ml–>”magnetic #”—-> Specific orbital
ms–>”spin

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4
Q

What is the difference between alpha-decay,

beta-decay (-). beta-decay (+), and electron capture?

A

alpha-decay: reduces mass # (large nuclei–> Z>83)

beta-decay (-): n—>p [N/Z is high]

beta-decay (+): p—>n [N/Z is low]

electron capture: p—>n [N/Z is low]

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5
Q

What is the formula for Nuclear Binding Energy?

A

E = mc^2

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6
Q

What element has the highest nuclear binding energy?

A

Fe (iron-56)

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7
Q

What are the trends of the periodic table?

A

l. electronegativity and 1st ionization energy follow same
trend (top right) group 3 and 6 are exceptions

ll. e- affinity (——>)

lll. atomic radius follow opposite trend of electronegativity
(bottom left)

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8
Q

What is another way of asking “which is the most polar”?

A

Which has the biggest difference in electronegativity

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9
Q

What are the 3 types of bonding and define the characteristics that describe?

A
  1. Covalent (non-metal + non-metal)
    • molecular or network solids
    • low m.p. and b.p.
  2. Ionic (metal + non-metal)
    • crystals
    • high m.p. and b.p.
    • brittle
  3. Metallic (metal + metal)
    • high m.p. and b.p.
    • conducts electricity, malleable, ductile, shiny
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10
Q

What is the molecular geometry of 3 electron domains and 0 non-bonding electrons?

A

trigonal planar

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11
Q

What is the molecular geometry of 3 electron domains and 1 non-bonding electrons?

A

bent

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12
Q

What is the molecular geometry of 4 electron domains and 0 non-bonding electrons?

A

tetrahedral

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13
Q

What is the molecular geometry of 4 electron domains and 1 non-bonding electrons?

A

trigonal pyramidal

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14
Q

What is the molecular geometry of 4 electron domains and 2 non-bonding electrons?

A

bent

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15
Q

What is the molecular geometry of 5 electron domains and 0 non-bonding electrons?

A

trigonal bipyramidal

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16
Q

What is the molecular geometry of 5 electron domains and 1 non-bonding electrons?

A

see-saw

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17
Q

What is the molecular geometry of 5 electron domains and 2 non-bonding electrons?

A

T-shaped

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18
Q

What is the molecular geometry of 5 electron domains and 3 non-bonding electrons?

A

linear

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19
Q

What is the molecular geometry of 6 electron domains and 0 non-bonding electrons?

A

octahedral

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20
Q

What is the molecular geometry of 6 electron domains and 1 non-bonding electrons?

A

square pyramidal

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21
Q

What is the molecular geometry of 6 electron domains and 2 non-bonding electrons?

A

square planar

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22
Q

What are the 3 Intermolecular forces?

A

H-bonding (H-FON)

Dipole-dipole

London dispersion (Van der Waals)

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23
Q

The phase change from solid—>liquid is known as ________ and is ____exothermic / endothermic____.

A

Fusion “melting”

Endothermic (H>0), (S>0)

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24
Q

The phase change from liquid—>gas is known as ________ and is ____exothermic / endothermic____.

A

Vaporization “boiling”

Endothermic (H>0), (S>0)

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25
Q

The phase change from solid—>gas is known as ________ and is ____exothermic / endothermic____.

A

Sublimation (eg. dry ice)

Endothermic (H>0), (S>0)

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26
Q

The phase change from liquid—>solid is known as ________ and is ____exothermic / endothermic____.

A

Crystallization “freezing”

Exothermic (H<0) (S<0)

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27
Q

The phase change from gas—>liquid is known as ________ and is ____exothermic / endothermic____.

A

Condensation

Exothermic (H<0) (S<0)

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28
Q

The phase change from gas—>solid is known as ________ and is ____exothermic / endothermic____.

A

Deposition “deposit that in your brain”

Exothermic (H<0) (S<0)

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29
Q

What formula would you use on a Calorimetry calculation?

A

q = mc*(delta T)

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30
Q

What is the definition of tripple pt. on a phase diagram?

A

All there phases (solid, liquid, gas) are occurring simultaneously

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31
Q

What are the 2 Ideal Gas Assumptions?

A
  1. Gas molecules themselves have no volume (only true @ low temp and large volume)
  2. No intermolecular attractions between molecules (only true @ high temps)
    (All collisions are elastic)
    [kinetic energy is proportional to temp]
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32
Q

What is the formula for the Ideal Gas Law?

A

PV = nRT

P --> Pressure (atm) [1atm = 760 torr = 760mmHg]
V --> Volume (Liters) [1 cm^3 = 1mL]
n --> moles
R --> 0.08206
T --> Temperature (Kelvin)
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33
Q

What is the temperature and pressure @ STP?

A

0 degrees Celcius or 273K

1 atm

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34
Q

How many liters is 1 mole of gas @ STP?

A

22.4L

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35
Q

What does Boyle’s Law state?

A

Pressure is inversely proportional to Volume

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36
Q

What does Charle’s Law state?

A

Temperature and Volume are directly proportional

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37
Q

What does Avogadro’s Law state?

A

moles and volume are directly proportional

38
Q

What is the formula for the Combined Gas Law?

A

(P1)(V1) / (n1)(T1) = (P2)(V2) / (n2)(T2)

hint: when DAT asks this question they may not tell you how many moles—-> assume 1 mole

39
Q

What is the formula for Dalton’s Law of Partial Pressure?

A

P(total) = P1 + P2 + P3….

eg. What % of the total pressure is N2?

given:
- P(total) = 50atm
- 10 mol N2
- 6 mol O2
- 4 mol CO2

10mol N2/ 20 mol = .5 = 50%

50% of 50atm = 25atm N2

40
Q

What is the formula for Graham’s Law of Effusion?

A

r1/r2 = (M2/M1)^1/2

41
Q

What is the formula for Molarity?

A

Molarity = mol(solute) / L(solution)

42
Q

What is the formula for molality?

A

molality = mol(solute) / kg(solvent)

43
Q

What do the 2 main solubility rules state?

A
  1. ALL Group 1 metal, NH4, NO3, ClO4, C2H3O2 salts are soluble
  2. Most Ag, Pb, Hg salts are soluble
44
Q

What are the 3 Phase Solubility in Liquids Rules?

when are solids and gases more soluble

A
  1. Solids are more soluble @ high temps
  2. Gases are less soluble @ high temps
  3. Gases are more soluble @ high pressures
45
Q

What is the formula for Osmotic Pressure?

A

“pie” = iMRT

46
Q

What is the formula for Freezing Pt. Depression?

A

delta T(f) = -iK(f)m

47
Q

What is the formula for Boiling Pt. Depression?

A

delta T(f) = iK(f)m

48
Q

What is the rate determining step also known as?

A

“slow step”

49
Q

How does a catalyst speed up rxns?

A

catalyst lower the activation energy by providing an alternate mechanism (pathway) for the rxn to occur

50
Q

Which direction will the equilibrium favor if K>1?

A

products

51
Q

Which direction will the equilibrium favor if K<1?

A

reactants

52
Q

Which direction will the equilibrium favor K=1?

A

@ equilibrium

53
Q

Which direction will the equilibrium favor K>Q?

A

products

54
Q

Which direction will the equilibrium favor K

A

reactants

55
Q

Which direction will the equilibrium favor K=Q?

A

@ equilibrium

56
Q

What is the definition of Equilibrium?

A

forward rate = reverse rate

57
Q

What temperature are solids more soluble?

A

Higher temps

58
Q

Are gases more or less soluble at higher temperatures?

A

Less soluble

59
Q

Are gases more or less soluble at higher pressures?

A

More soluble

60
Q

Bonsted-Lowry defines acids and bases as__________.

A

proton donors and acceptors

61
Q

Lewis defines acids and bases as___________.

A

e- donors and acceptors

62
Q

What are the 7 strong acids?

A
  1. HI
  2. HBr
  3. HCl
  4. HClO3
  5. HClO4
  6. H2SO4
  7. HNO3
63
Q

What is the binary acid trend state?

A

Down and to the right

opposite of basic trends

64
Q

What is the Oxoacid trend state?

A

More oxygens = more acidic

eg. HClO3>HClO2

More electronegative heteroatom = more acidic

eg. HClO3>HBrO3

65
Q

What is the formula for calculating pH given [H+]?

A

pH= -log[H+]

66
Q

What is the formula for calculating [H+] given pH?

A

[H+] = 10^-pH

67
Q

What is the formula for calculating pOH when given the pH?

A

14 = pH + pOH

pOH = 14 - pH

68
Q

What is the formula for weak acid dissociation in water?

eg. The Ka of acetic acid is approximately 2 x 10–5. What is the pH of a 0.5 M solution of acetic acid?

A

[H+] = sqr root [(Ka) (HA)]

eg. after using the equation above, convert [H+] —> pH

69
Q

What is the trend for determining negligible cations and anions in the hydrolysis of salts?

A

Negligible cations= groups 1 & 2 on periodic table
(strong bases)

Negligible anions= Cl-, Br-, I-, NO3-, ClO3-, ClO4-
(strong acids)
exception: HSO4-

70
Q

What is the definition of a buffer?

A

Resists change in pH

71
Q

What are the 4 ways of making a buffer?

A
  1. strong acid + strong base [1:1]
  2. strong acid + weak base [1:2]
  3. strong base + weak acid [1:2]
  4. weak acid + conj base [1:1]
72
Q

What are the 3 Laws of Thermodynamics?

A
  1. Conservation of energy (some released as heat)
    “energy can’t be created of destroyed”
  2. For a spontaneous process, the entropy of the universe increases
  3. A perfect crystal at 0K has zero entropy
73
Q

When G<0 the rxn is said to be __________.

A

spontaneous

74
Q

When G>0 the rxn is said to be __________.

A

Nonspontaneous

75
Q

When G=0 the rxn is said to be___________.

A

@ equilibrium

76
Q

When H is negative and S is positive the rxn is ___spontaneous/nonspontaneous_____.

A

Spontaneous @ all temps

77
Q

When H is positive and S is negative the rxn is ___spontaneous/nonspontaneous_____.

A

Nonspontaneous @ all temps

78
Q

When H is negative and S is negative the rxn is ___spontaneous/nonspontaneous_____.

A

spontaneous @ low temps

79
Q

When H is positive and S is positive the rxn is ___spontaneous/nonspontaneous_____.

A

spontaneous @ high temps

80
Q

Oxidation is the _________ of e- and reduction is the _________ of e-.

A

oxidation = loss of e-

reduction = gain of e-

81
Q

The oxidizing agent is the species being _________ and the reducing agent is the species being _________.

A

oxidizing agent = species being reduced

reducing agent = species being oxidized

* Elements or compounds are oxidized/reduced whereas only COMPOUNDS act as reducing/oxidizing agents*

82
Q

The anode is the site of _____oxidation/reduction______,

whereas the cathode is the site of ____oxidation/reduction____,

A

anode = oxidation

cathode = reduction

83
Q

What happens to boiling pt and melting pt of a substance if you decrease pressure?

A

B.P = Decreases

M.P = Increases

84
Q

Which of the following 0.25M solutions would exhibit the lowest electrical conductivity?

A. HCl 
B. K2SO4
C. NaCl
D. HF
E. Ba(NO3)2
A

D. HF (Weak acids are week electrolytes?

85
Q

What is the equation for rate of disappearance?

A

rate = - (delta-Concentration) / (delta-time)

rate = (C2 - C1) / (T2 - T1)

86
Q

What is true of reaction intermediates?

A

They never appear in rate equations

87
Q

The more ___positive/negative___ a reduction potential the ___stronger/weaker___ the reducing agent.

A

Negative; Stronger

The reduction potential is a measure of the tendency for a reduction to occur. The greater the tendency for reduction, the less likely the oxidation is. The strongest reducing agent is the one with the highest tendency for oxidation, i.e. with the lowest (more negative) reduction potential. Thus, of the given metals, Zn is the strongest reducing agent.

88
Q

Distinguish between the following:

Alpha emission: 
Positron emission:
Beta emission:
Gamma emission:
Electron capture:
A

Alpha emission: an alpha particle (identical to an He nucleus) with 2 neutrons and 2 protons is ejected from the nucleus. Because the alpha particle contains 2 protons, alpha particles have a +2 charge.

Positron emission: a proton converts into a neutron and emits a positron (a positively charged electron). Because a proton is converting into a neutron, the atomic mass stays the same but the atomic number decreases by 1.

Beta emission: a neutron converts into a proton and emits an electron. Atomic number increases (1 more proton) but atomic mass stays the same.

Neutron swap is not a type of nuclear decay (made up term).

Gamma emission: a nucleus in an excited state releases a photon. This does not change atomic mass or atomic number, but takes the nucleus from a high energy state to a low energy state.

Electron capture: an inner shell electron is drawn into the nucleus and combines with a proton, forming a neutron. The mass number stays the same whereas the atomic number decreases by 1 (like positron emission).

89
Q

What type of nuclear reaction is involved when C-11 decays to B-11?

A

Positron emission

one less proton

90
Q

What is the difference between precision and accuracy?

A

Precision- how close your values in lab are

Accuracy- how close your value is to the actual value

91
Q

Which separation technique is based on differences in the particle size of the substances being separated?

A

Vacuum filtration

Fractional distillation is a method to separate the components of a solution. The solution is gradually heated up, and the substance with the lower boiling point will boil first and exit the solution as a gas. The gas can then be cooled, condensed, and collected.

GEN CHM (3 decks)

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