Exam Flash Cards

Question 1

From a Thermochemical standpoint, the formation of a chemical bond is:

Answer 1

Exothermic

Question 2

The lattice energy of an ionic compound can be calculated using the:

Answer 2

Born-Haber Cycle

Question 3

Atoms of different electronegativity form [ ] [ ] bonds

Answer 3

Polar Covalent

Question 4

Defined as “the ability to attract electrons to itself in a chemical bond”

Answer 4

Electronegativity

Question 5

Different, but formally correct Lewis structures of a molecule are called:

Answer 5

Resonance Structures

Question 6

The acronym for the method of predicting molecular structure based on their Lewis structures is:

Answer 6

VSEPR

Question 7

A central atom surrounded by 5 electron pairs always puts a lone pair in what position?

Answer 7

Equatorial

Question 8

The mixing of orbitals in the Valence Bond Theory is called:

Answer 8

Hybridization

Question 9

The full name of the SI unit for pressure, which is equal to 1 N/m², is:

Answer 9

Pascal

Question 10

22.4 L of a gas at standard temperature (273.15K) and pressure (atm) is called the:

Answer 10

Molar Volume

Question 11

The pressure of a gas coexisting in equilibrium with a liquid is its:

Answer 11

Vapor Pressure

Question 12

U_rms is a measure of the [ ] [ ] of the particles of gas.

Answer 12

average velocity

Question 13

The weakest of the intermolecular forces are:

Answer 13

Dispersion Forces

Question 14

The type of intermolecular force giving water its unusually high boiling point is:

Answer 14

Hydrogen Bonding

Question 15

The phase change directly from a solid to a gas is called:

Answer 15

Sublimation

Question 16

Solid, liquid, and gas coexist in equilibrium at the:

Answer 16

Triple Point

Question 17

The body centered cubic unit cell contains how many atoms?

Answer 17

two

Question 18

Which forces are recognized as intermolecular forces?

Answer 18

1. Dispersion Forces
2. Dipole-dipole Forces
3. Ion-dipole Forces
4. Hydrogen Bonding

Question 19

What is the coordination number of any atom in a body-centered cubic lattice?

Answer 19

8

Question 20

LCAO is the acronym for a technique used in:

Answer 20

Valence Bond Theory

Question 21

What is the formula of Ozone?

Answer 21

O₃

Question 22

The thermodynamic quantity that drives mixing of gases and solutions is the:

Answer 22

Entropy

Question 23

A measure of solution concentration defined as n_solute/(n_solute + n_solvent) is called the:

Answer 23

Mole Fraction

Question 24

Vapor pressure lowering and boiling point elevation are examples of:

Answer 24

Colligative Properties

Question 25

The equation P_soln = X_solvent • P^o_solvent is known as:

Answer 25

Raoult's Law

Question 26

The rate law d[A] / dt = k[A]² belongs to a reaction [ ] [ ] in [A].

Answer 26

Second Order

Question 27

The time required for a reactant to decrease to half of its original concentration is called a:

Answer 27

Half Life

Question 28

The temperature dependence of reaction rates is governed by what equation?

Answer 28

Arrhenius Equation

Question 29

A substance that facilitates a chemical reaction without being used up in the process is called a:

Answer 29

Catalyst

Question 30

The notion that at equilibrium the rate of the forward reaction equals that of the reverse reaction is called:

Answer 30

Dynamic Equilibrium

Question 31

The equation giving the concentrations of an equilibrium is the:

Answer 31

The Law of Mass Action

Question 32

The tendency of equilibria to counteract imposed changes is:

Answer 32

Le Chatelier's Principle

Question 33

In the context of the Bronsted-Lowry definition, a base is a:

Answer 33

Proton Acceptor

Question 34

The reaction 2H₂O ⇔ H₃O⁺ + OH^- is called the [ ] of water.

Answer 34

Autoionization

Question 35

The negative decadic logarithm of the hydroxide concentration is the:

Answer 35

pOH

Question 36

The defining criterion of a 'strong acid' is that it is:

Answer 36

Completely Dissociated

Question 37

Determining the concentration of a base with the aid of a buret is a lab technique called:

Answer 37

Titration

Question 38

The numerical value of the ion product of water is:

Answer 38

1.0 x 10^-14

Question 39

A Lewis base is defined as an:

Answer 39

Electron Pair Donor

Question 40

As T increases, the solubility of gases in liquids:

Answer 40

Goes through a minimum at T_crit

Question 41

Molality is a measure of concentration (of x) defined as:

Answer 41

n_x / m_solvent

Question 42

The osmotic pressure π is given by:

Answer 42

π = MRT

Question 43

A change in [ ] changes the rate constant of a reaction.

Answer 43

Temperature

Question 44

What plot for a first-order reaction (A→B) gives a straight line?

Answer 44

ln[A] vs. t

Question 45

The correct form of the Arrhenius equation is:

Answer 45

k = A*e*^{(-E_a / kT)}

Question 46

A rule of thumb that close to room temperature an increase in T by 10^oC:

Answer 46

Increases rate by a factor of 2-3

Question 47

The half-life of a first-order reaction is:

Answer 47

t_1/2 = 0.693 / k

Question 48

The relationship between K_c and K_p is:

Answer 48

K_p = K_c(RT)^Δn

Question 49

An equimolar mixture of a weak base and its conjugate acid is a:

Answer 49

Buffer

Question 50

The pH of a buffer is given by what equation?

Answer 50

Henderson-Hsselbalch

Question 51

During the titration of a base of unknown concentration, an equal amounts of acid has been added at the:

Answer 51

Equivalence Point

Question 52

The equilibrium constant governing solubility of salts is the:

Answer 52

Solubility Product

Question 53

A process involving the 'gain of electrons' is a:

Answer 53

Reduction

Question 54

A voltaic Cell consists of two [ ] [ ] connected by a wire and a salt bridge.

Answer 54

Half Cells

Question 55

The electrode where the oxidation occurs is called the:

Answer 55

Anode

Question 56

All standard reduction potentials are quoted in Volt versus the potential of the:

Answer 56

Standard Hydrogen Electrode

Question 57

What constant gives the charge of a mole of electrons?

Answer 57

Faraday Constant

Question 58

Cell potentials in non-standard state concentrations and pressures can be calculated with the:

Answer 58

Nernst Equation

Question 59

The splitting of water by an electrical current is called the [ ] of water.

Answer 59

Electrolysis

Question 60

The electrochemical oxidation of water to O₂ encounters a significant:

Answer 60

Overvoltage

Question 61

Most elements are composed of several:

Answer 61

Isotopes

Question 62

The inherent instability of heavy nuclei is the cause of:

Answer 62

Radioactivity

Question 63

α-decay

Answer 63

Decay of a nuclide accompanied by ejection of a ⁴₂He particle.

Question 64

The kinetics of radioactive decay are:

Answer 64

First Order

Question 65

Nuclear Power Plants harvest the energy of nuclear [ ].

Answer 65

Fission

Question 66

According to Einstein, the energy released in nuclear reactions is associated with a:

Answer 66

Mass Defect

Question 67

At the equivalence point of a titration of a weak base with a strong acid, the solution is:

Answer 67

Mildly Acidic

Question 68

The pH of a buffer made with equal amounts (# moles) of acetic acid and acetate is:

Answer 68

4.74

Question 69

At a pH below 7.00, the indicator phenolphthalein is:

Answer 69

Colorless

Question 70

The correct relationship between ΔG^o and E^o is:

Answer 70

ΔG^o = -nFE^o

Question 71

A common fuel cell extracts energy from what reaction:

Answer 71

2H₂ + O₂ → 2H₂O

Question 72

What is the heat of fission of 1 mole of ²³⁵U?

Answer 72

1.66 x 10¹⁰ kJ/mol

Question 73

A process involving the 'loss of electrons' is an:

Answer 73

Oxidation

Question 74

β-Decay

Answer 74

Decay of a nuclide accompanied by ejection of a ⁰_-1*e* particle.

Question 75

The MO Theory predicts that O2 has 2 unpaired electrons and thus is:

Answer 75

Paramagnetic

Question 76

What is true for conjugate acid/base pairs?

Answer 76

pK_a + pK_b = 14

Question 77

What is the halflife of ²²⁰Rn?

Answer 77

55.6 sec

Question 78

What is the halflife of ²³⁵U?

Answer 78

703 million years