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CHEM 111 > Exam 2 > Flashcards

Exam 2 Flashcards

1
Q

Thermochemistry

A

the study of the relationship between heat and chemical reactions

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2
Q

Kinetic Energy

A

energy possessed by matter because it is in motion

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3
Q

Thermal Energy

A

energy in the form of random motion of particles in any sample of matter

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4
Q

What happens to thermal energy as temperature increases?

A

As temperature rises, thermal energy increases

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5
Q

Heat

A

energy that causes a change in the thermal energy of a sample

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6
Q

What happens when you add heat to a sample?

A

adding heat to a sample increases its temperature

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7
Q

Potential Energy

A

the energy derived from the position or condition of matter

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8
Q

Chemical Energy

A

a form of potential energy derived from the forces that hold the atoms together in compounds

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9
Q

System

A

a sample of matter on which we focus our attention, generally the atoms involved on a chemical reaction

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10
Q

Surroundings

A

all other matter in the universe

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11
Q

Law of Conservation of Energy

A

the energy of the universe is constant during a chemical or physical change

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12
Q

What makes a reaction exothermic?

A

a reaction is exothermic when the system transfers heat to the surroundings
GET HEAT

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13
Q

What makes a reaction endothermic?

A

a reaction that absorbs heat from the surroundings is called endothermic NEED HEAT

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14
Q

What kind of thermochemical reaction is a combustion reaction?

A

combustion reactions are exothermic

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15
Q

Enthalpy

A

a measure of the energy of the system

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16
Q

Change in Enthalpy, ΔH

A

equal to the heat absorbed or given off by the system at constant pressure

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17
Q

What kind of reaction has a negative ΔH?

A

exothermic reactions have a negative ΔH, the system loses energy

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18
Q

What kind of reaction has a positive ΔH?

A

endothermic reactions have a positive ΔH, the system gains energy

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19
Q

Thermochemical Equation

A

an equation for which ΔH is given

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20
Q

Calorimetry

A

the experimental measurement of heat released or absorbed by a chemical reaction

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21
Q

Specific Heat

A

the heat needed to increase the temperature of 1 gram of matter by 1 K

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22
Q

What is the relation between heat (q), mass (m), and change in temperature (ΔT)?

A

q = m C ΔT

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23
Q

How do you calculate q(surrounding)?

A

measuring the temperature change of the calorimeter, along with the mass and heat capacity, allows us to calculate q(surrounding)

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24
Q

State Function

A

a property of the system that is fixed by the present conditions and is independent of the system’s history

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25
Path Function
a property that depends on how the particular change took place
26
What type of function is enthalpy?
Enthalpy is a state function
27
Hess's Law
when two or more thermochemical equations are added, the enthalpy change of the resulting equation is the sum of those for the added equations
28
Standard State
the standard state of a substance at a specified temperature is the pure form at 1 atm pressure
29
Standard Enthalpy of Formation
the enthalpy change when one mole of a substance in its standard state is formed from the most stable form of its constituent elements in their standard state
30
Solid (volume & shape)
a solid has fixed volume and shape
31
Liquid (volume & shape)
a liquid has fixed volume but no definite shape
32
Gas (volume & shape)
a gas has no fixed volume or definite shape
33
Pressure
the force per unit area exerted on a surface
34
Ideal Gas Law
PV=nRT
35
Partial Pressure
The pressure exerted by each has in a mixture
36
Mole Fraction (X, chi)
The number of moles of one component of a mixture divided by the total number of moles of all substances present in the mixture
37
Effusion
The passage of a gas through a small hole into an evacuated space
38
What kind of gases effuse more rapidly?
Gases with low molar masses
39
Diffusion
The mixing of particles due to motion
40
Graham’s Law of Effusion
Relative rates of effusion can be used to determine molar mass (M)
41
Waves
Periodic disturbances; the repeat at regular intervals of time and distance
42
Wavelength (lambda)
Is the distance between one peak and the next
43
Frequency (v)
The number of eaves that pass a fixed point each second
44
What does electromagnetic radiation consist of?
Light or electromagnetic radiation consists of oscillating electric and magnetic fields
45
How much visible light is one the electromagnetic spectrum?
Visible light is only a very small portion of the electromagnetic spectrum
46
What is the smallest unit of energy?
A quantum
47
What is the equation for the energy of a quantum?
E=hv | h is Planck’s constant
48
Spectrum
A graph of light intensity as a function of wavelength or frequency
49
Continuum or Continuous Spectrum
The light emitted by heated objects (light of all wavelengths is present)
50
What kind of spectrum do gaseous atoms produce?
Gaseous atoms produce a line spectrum (one that contains light only at specific wavelengths and not at others)
51
Wave Functions (Ψ)
Gives the amplitude of the electron wave at any point in space
52
What does Ψ^2 give?
The probability of finding the electron at any point in space
53
What does the solution of the wave equation produce?
The solution of the wave equation produces quantum numbers that describe the characteristics of the electron wave
54
Atomic Orbital
A wave function of the electron for specific values of n, l, & m(l)
55
What is the principle quantum number?
n
56
What does the principle quantum number provide?
The principle quantum number, n, provides information about the energy and the distance of the electron from the nucleus
57
What does a larger value of n mean?
The larger the value of n, the greater the average distance of the electron from the nucleus
58
Principal Shell (or just Shell)
All atomic orbitals that have the same value of n
59
What is the Angular Momentum Quantum Number?
l
60
What is the angular momentum quantum number, l, for?
The angular momentum quantum number, l, is associated with the shape of the orbital
61
What are the allowed values of l, the angular momentum quantum number?
0 and positive integers up to n-1 | The l quantum number can never equal or exceed the value of n
62
Subshell
All possible orbitals that have the same values of both n and l
63
What is the Magnetic Quantum Number?
m(l)
64
What does the magnetic quantum number, m(l), indicate?
The magnetic quantum number, m(l), indicates the orientation of the atomic orbital in space
65
What are the allowed values of the magnetic quantum number?
-l to l, including 0
66
Orbital
A wave function described by all three quantum numbers (n, l, m(l))
67
What is the Electron Spin Quantum number?
m(s)
68
What does the electron spin quantum number, m(s), represent?
The electron spin quantum number, m(s), represents one of the two allowed spin values, +1/2 and -1/2
69
What is the shape of p orbitals?
p orbitals (l=1) have two lobes of electron density on opposite sides of the nucleus
70
Electron shielding (screening)
The result of the influence of electrons on the effective nuclear charge
71
Effective Nuclear Charge (Z(eff))
A weighted average of the nuclear charge that affects an electron in the atom
72
Pauli Exclusion Principle
No two electrons in the same atom can have the same set of four quantum numbers
73
Aufbau Principle
As electrons are added to an atom one at a time, they are assigned the quantum numbers of the lowest energy orbital that is available
74
Ground State
The resulting atom in its lowest energy state
75
Orbital Diagram
Represents each orbital with a box, with orbitals in the same subshell in connected boxes; electrons are shown as arrows in the boxes, pointing up or down to indicate their spins
76
Hund’s Rule
One electron occupies each degenerate orbital with the same spin before a second electron is placed in an orbital
77
Valence Electrons
Electrons with the highest principal quantum number and any electrons in an infilled subshell from a lower shell
78
Valence Orbitals
Orbitals of those subshells that hold the valence electrons
79
Isoelectronic Series
A group of atoms and ions with the same number of electrons
80
Atomic Radius
One half the distance between adjacent atoms of the same element in a molecule
81
Ionization Energy
The energy required to remove an electron from a gaseous atom or ion in its electronic ground state
82
Electron Affinity
The energy change that accompanies the addition of an electron to a gaseous atom to form an anion

CHEM 111 (4 decks)

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