Mcat General Chemistry

Front 1

1L= ? cm^3

Back 1

1000cm^3

Front 2

? dm^3=1000cm^3

Back 2

1dm^3

Front 3

1000L= ? m^3

Back 3

1m^3

Front 4

6.02x10^3amu= ?g

Back 4

1g

Front 5

? amu= 1/12 C

Back 5

1amu

Front 6

What is the Oxidation Number of the H in CH4?

Back 6

0

Front 7

What is the Oxidation Number of the H in CaH2?

Back 7

-1

Front 8

What is the Oxidation Number of the O in H2O2?

Back 8

-1

Front 9

What is the Oxidation Number of the H in H2SO4

Back 9

1

Front 10

What is the Oxidation Number of the O in CO2

Back 10

-2

Front 11

Which energy level will electrons fill first: 2d, 4s, or 4f?

Back 11

2d

Front 12

What does Diamagnetic mean?

Back 12

That no electrons are unpaired

Front 13

Which will be attracted by a magnetic field: a Diamagnetic atom or a Paramagnetic atom?

Back 13

Paramagnetic

Front 14

What does Paramagnetic mean?

Back 14

That there are unpaired electrons

Front 15

How many electrons are in the 3rd energy level?

Back 15

18

Front 16

How many electrons are in the 7th energy level?

Back 16

98

Front 17

How many electrons are in the 3s subshell?

Back 17

2

Front 18

How many electrons are in the 5d subshell?

Back 18

10

Front 19

How many orbitals are in the 2nd energy level

Back 19

4

Front 20

How many orbitals are in the 4th energy level?

Back 20

16

Front 21

What is the equation for Energy when given Mass?

Back 21

E=mc^2

Front 22

What is the equation for Energy when given Wavelength?

Back 22

E=hc/λ

Front 23

What is the equation for Energy when given frequency?

Back 23

E=hf

Front 24

Which has the longer wavelength, a photon with E=15 or E=22?

Back 24

E=15

Front 25

What is the equation for Angular Momentum given Mass, Velocity, and Radius?

Back 25

mvr

Front 26

What is the equation for Angular Momentum given Moment of Inertia and Angular Velocity?

Back 26

Iw

Front 27

What is the equation for the Angular Velocity of an electron given the Quantum Number?

Back 27

nh/2π

Front 28

What is the equation for the Energy of an electron given the Quantum Number?

Back 28

E=-R/n^2

Front 29

What is the equation for the Energy Change given the initial and final Quantum Numbers?

Back 29

E=-R(1/n^2 - 1/n^2)

Front 30

How many wavelengths are in the Balmer Series?

Back 30

4: 400-650nm

Front 31

What is the equation for Wavelength given Velocity and Mass?

Back 31

λ=h/mv

Front 32

Increasing the KE of an electron will increase the Frequency, Wavelength, or Energy?

Back 32

The frequency and energy increase while the wavelength decreases

Front 33

Which form of decay decreases the atomic number by 1?

Back 33

Electron capture

Front 34

Which form of decay changes a neutron into a proton and releases an electron?

Back 34

B- decay

Front 35

Which form of decay releases a positron and decreases the atomic number?

Back 35

B+ decay

Front 36

Nuclear Binding Energy

Back 36

Energy required to break the nucleons apart

Front 37

Mass Defect

Back 37

Mass of nucleons - mass of nucleus

Front 38

What is the equation for Nuclear Binding Energy?

Back 38

E=(ΔM)c^2 (if kg)

E=(ΔM)931.5 MeV

Front 39

Which has the more negative Electron Affinity: Mg, Ca, or Sr?

Back 39

Mg

Front 40

Which has the more negative Electron Affinity: Al, Si, or P?

Back 40

P

Front 41

Sort these acids in increasing order: H3PO4, HCl, H2SO4.

Back 41

H3PO4<H2SO4<HCl

Front 42

Sort these acids in decreasing order: HBr, HF, HCl.

Back 42

HBr>HCl>HF

Front 43

Which has the higher melting point: Li or Be?

Back 43

Be

Front 44

Which has the higher density: K or Ca?

Back 44

Ca

Front 45

What are the characteristics of the Alkali Metals?

Back 45

Low density, low melting point, react exothermically with water to form metal hydroxides and hydrogen gas, form peroxides with O2.

Front 46

What are the characteristics of the alkaline earth metals?

Back 46

More dense and higher m.p. than alkali metals, heavier, more reactive.

Front 47

Which elements can form two extra bonds with a lewis base?

Back 47

Si, Ge, Sn, Pb, N, P, As, Sb, Bi

Front 48

What is the equation for Formal Charge?

Back 48

Valence-1/2Bonded-Unbonded

Front 49

How many electron groups and lone pairs does an Octahedral configuration have?

Back 49

6 electron groups and 0 lone pairs

Front 50

Which Geometric Structure has 4 electron groups and 0 lone pairs?

Back 50

Tetrahedral

Front 51

Which Geometric Structure has 3 electron groups and 0 lone pairs?

Back 51

trigonal planar

Front 52

How many electron groups and lone pairs does a bent geometric structure have?

Back 52

4 electron groups and 2 lone pairs

Front 53

Which geometric structure has 4 electron groups and 1 lone pair?

Back 53

trigonal pyramidal

Front 54

Which geometric structure has 2 electron groups and and 0 lone pairs?

Back 54

Linear

Front 55

How many electron groups and lone pairs does a trigonal bipyramidal geometric configuration have?

Back 55

5 electron groups and 0 lone pairs

Front 56

How many electron groups and lone pairs does a octahedral geometric configuration have?

Back 56

6 electron groups and 0 lone pairs

Front 57

Which geometric configuration has 5 electron groups and 1 lone pair?

Back 57

See Saw

Front 58

How many electron groups and lone pairs does a square pyramid geometric structure have?

Back 58

6 electron groups and 1 lone pair

Front 59

Which geometric structure has 4 electron groups and 2 lone pairs?

Back 59

bent

Front 60

How many electron groups and lone pairs does a T-shaped geometric structure have?

Back 60

5 electron groups and 2 lone pairs

Front 61

How many electron groups and lone pairs does a square planar configuration have?

Back 61

6 electron groups and 2 lone pairs

Front 62

What is the equation for Dipole Moment?

Back 62

μ=qr

Front 63

What is a physical change?

Back 63

No intramolecular bonds are broken, only intermolecular bonds

Front 64

Fusion

Back 64

Solid to liquid

Front 65

Sublimation

Back 65

Solid to gas

Front 66

Deposition

Back 66

Gas to solid

Front 67

Heat of fusion

Back 67

Amount of heat required to melt

Front 68

Heat of Transition

Back 68

q=nΔH

Front 69

1 Calorie

Back 69

4.2 Joules

Front 70

What is the equation for the amount of energy released or absorbed between phases?

Back 70

q=mcΔT

Front 71

What does 1/c represent?

Back 71

The slope of a phase diagram

Front 72

Which has a higher melting point: CH3COCH2CH2CH3 or CH3CH2COCH2CH3 and why?

Back 72

CH3CH2COCH2CH3, because melting point increases with symmetry

Front 73

Triple Point

Back 73

The Temperature and pressure in which all three phases exist in equilibrium.

Front 74

Critical point

Back 74

The end of the liquid gas boundary consisting of the supercritical fluid

Front 75

supercritical fluid

Back 75

liquid that will not condense no matter how high the pressure

Front 76

Kinetic Molecular Theory

Back 76

Molecules take up no volume, Avg KE is proportional to temperature, Collisions are elastic, molecules feel no intermolecular forces

Front 77

What are the main characteristics of an Ideal Gas?

Back 77

1.) Lower molecular weight
2.) Higher pressure, lower temp
3.) Smaller molecular size
4.) Monatomic gases are favored
5.) Weak intermolecular forces

Front 78

What is the kinetic energy of a gas equal to?

Back 78

3/2RT

Front 79

What is the equation for Graham's Law of Effusion?

Back 79

vrmsA = (sqrt)molar mass of B
vrms B (sqrt)molar mass of A

Front 80

If I add .5L of 2M of NaCl to 2L of .5M of CaBr2 what is the concentration of the final solution?

Back 80

M1V1+M2V2=M'V'=.8

Front 81

Is molality dependent on or independent from temperature and pressure?

Back 81

Independent

Front 82

What are the solubility rules?

Back 82

1.) All silver, lead, and mercury salts are insoluble.
2.) Silver, lead, and mercury nitrates, perchlorates, and acetates are soluble
3.) all nitrate, perchlorate, and acetate salts are soluble
4.) All group 1 and NH4+ salts are soluble

Front 83

Which has the higher vapor pressure: a solution with a BP of 50 or a solution with a BP of 35?

Back 83

The solution with a BP of 35

Front 84

What is the equation for the resulting vapor pressure of combined solutions with volatile solutes?

Back 84

P=X1P1+X2P2

Front 85

What happens to the freezing point of a solution when solute is continually added to it?

Back 85

It will initially decrease and then will increase

Front 86

What is the equation for Osmotic Pressure?

Back 86

MiRT

Front 87

What is a reaction rate dependent on?

Back 87

1.) Frequency of collision
2.) energy of collisions
3.) orientation of collisions

Front 88

Write the rate law of the following reaction if an acid is the catalyst: 2A + B --> A2B

Back 88

rate=k[A]^2[B]+k(H+)[H+][A][B]

Front 89

What is the rate constant dependent on?

Back 89

Pressure, temperature, and catalysts

Front 90

Which is more important in determining the rate law: the mechanism or experimental data?

Back 90

The mechanism

Front 91

In the following unimolecular reaction, how does A decrease: A--> products?

Back 91

Exponentially with a constant half life

Front 92

In the following bimolecular reaction, how does A decrease: 2A--> products?

Back 92

Each subsequent half life is twice as long as the previous one

Front 93

Consider the following mechanism:
A + B --> C + D (step 1)
C + D--> CD (step 2)
If step 2 is the rate determining step, what can you conclude about step 1?

Back 93

That it is at equilibrium

Front 94

Why will an evaporating glass of water never reach equilibrium?

Back 94

Because it is not a closed system

Front 95

Write the equilibrium constant expression for the following reaction:
A(g)+2B(aq)+C2(s)-->AC2 (l)+ B2(g)

Back 95

keq=[B]/[A][B]^2

Front 96

If a noble gas is added to the reaction: A(g)+2B(g)-->AB2(g) which way will the equilibrium shift?

Back 96

It will not shift since noble gases are considered nonreactive gases

Front 97

Where does the point of maximum entropy occur in a reaction: when Q>Keq, when Q=Keq, or when Q<Keq?

Back 97

when Q=Keq at equilibrium

Front 98

Which sulfates are insoluble?

Back 98

Ca, Sr, Ba, and PbSO4

Front 99

Which oxides are soluble?

Back 99

Ca, Sr, and BaO

Front 100

Which hydroxides are soluble?

Back 100

Ca, Sr, and BaOH2

Front 101

Name all of the carbonates, phosphates, sulfides, and Sulfur trioxides that are soluble?

Back 101

Na, Li, K, Rb, Cs, Fr, and NH4+

Front 102

The conjugate base of a ? has no basic properties.

Back 102

Strong acid

Front 103

The conjugate acid of a strong base has no ? properties.

Back 103

Acidic

Front 104

The conjugate base of a weak acid is a ? base.

Back 104

Weak

Front 105

The pH of a softdrink is 4. What is the [OH-]?

Back 105

1x10^-10

Front 106

Which of the following [H+] solutions has acidic properties: 10^-7, 10^-3, 10^-10?

Back 106

10^-3

Front 107

What is the pH of a solution with a [H+] of 10^-3 and what equation would you use?

Back 107

3; [H+]=10^-pH

Front 108

What is the pH of a solution with a [H+] of 5.6x10^-4: 2.4, 5.7, 10.2, or 3.3?

Back 108

3.3 because n-1 to n should be the pH

Front 109

what does (ka)(kb) equal?

Back 109

1x10^-14

Front 110

What are the two henderson hasselbalch equations?

Back 110

pH=pKa+log[A-]/[HA]

pOH=pKb+log[HA]/[A-]

Front 111

Equivalence point

Back 111

point where all acid or base has been neutralized

Front 112

Half equivalence point

Back 112

[HA]=[A-]

Front 113

What is the pH of a solution with a pKa of 2.17 at the half equivalence point?

Back 113

2.17

Front 114

What do each of the symbols in the equation: ΔU=Q+PV stand for?

Back 114

U is the internal energy
Q is the heat transferred
+PV is the work done on the system

Front 115

What is the change in entropy if the amount of heat lost at 250K is 50J?

Back 115

.2 (ΔS=Q/T)

Front 116

what is the ΔS of the universe always equal to?

Back 116

> or equal to 1

Front 117

isobaric

Back 117

constant pressure and the work done equals the area under a graph.

Front 118

isochoric

Back 118

constant volume

Front 119

Adiabatic

Back 119

all energy transferred is work

Front 120

What is different about calculating the heat of formation and the bond dissociation enthalpies?

Back 120

ΔHproducts-ΔHreactants

E broken bonds-E formed bonds

Reactants and products are reversed

Front 121

When ΔH is negative and ΔS is negative, at what temperature will a reaction be spontaneous?

Back 121

At a low temperature

Front 122

When ΔH is positive and ΔS is positive, at what temperature will the reaction be spontaneous?

Back 122

High temperature

Front 123

What is the equation for Gibbs free energy?

Back 123

ΔG=ΔG*+RT LnQ

Front 124

Are products or reactants favored when ΔG*<0 and Keq>1?

Back 124

The products are favored

When ΔG*>1 and Keq<1 the reactants are favored

Front 125

What is the proper way to write a Galvanic Cell notation?

Back 125

Anode|Anodic solution||Cathodic solution|Cathode

Front 126

If the Standard Reduction Potential is -2.0 and the number of moles is 10^-2, what is the ΔG*?

Back 126

1.93x10^3

Front 127

What is the relationship between reduction potentials and reduction strength?

Back 127

The more negative the potential, the better the product is at reducing

Front 128

What is the relationship between reduction potential and oxidation strength?

Back 128

The more positive the reduction potential, the better the reactant is at oxidizing

Front 129

List the following elements in order of best to worst reducer: Mg, Zn, Au, Pd, Ag, Cu, H2, Li, Al, Fe, Pb, and Pt.

Back 129

Li>Mg>Al>Zn>Fe>Pb>H2>Cu>Ag>Pd>Pt>Au

Front 130

Do electrolytic cells drive spontaneous or nonspontaneous reactions?

Back 130

Nonspontaneous

Front 131

In electrolytic cells what is the charge on the anode and cathode respectively?

Back 131

+ and -

Front 132

What would increase the chemical process in a cell?

Back 132

Increasing the current

Front 133

which color radiates and absorbs light better: Navy or yellow?

Back 133

Navy

Front 134

Which color reflects light better: White or brown?

Back 134

White

Front 135

What does ppm stand for?

Back 135

mass of solute(10^6)/mass of solution