Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

CHEM 111 > Exam 2 > Flashcards

Exam 2 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

Thermochemistry

A

the study of the relationship between heat and chemical reactions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Kinetic Energy

A

energy possessed by matter because it is in motion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Thermal Energy

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What happens to thermal energy as temperature increases?

A

As temperature rises, thermal energy increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Heat

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What happens when you add heat to a sample?

A

adding heat to a sample increases its temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Potential Energy

A

the energy derived from the position or condition of matter

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Chemical Energy

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

System

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Surroundings

A

all other matter in the universe

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Law of Conservation of Energy

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What makes a reaction exothermic?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What makes a reaction endothermic?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What kind of thermochemical reaction is a combustion reaction?

A

combustion reactions are exothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Enthalpy

A

a measure of the energy of the system

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Change in Enthalpy, ΔH

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What kind of reaction has a negative ΔH?

A

exothermic reactions have a negative ΔH, the system loses energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What kind of reaction has a positive ΔH?

A

endothermic reactions have a positive ΔH, the system gains energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Thermochemical Equation

A

an equation for which ΔH is given

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Calorimetry

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Specific Heat

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

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

A

q = m C ΔT

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Path Function

A

a property that depends on how the particular change took place

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What type of function is enthalpy?

A

Enthalpy is a state function

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Hess’s Law

A

when two or more thermochemical equations are added, the enthalpy change of the resulting equation is the sum of those for the added equations

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Standard State

A

the standard state of a substance at a specified temperature is the pure form at 1 atm pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Standard Enthalpy of Formation

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

Solid (volume & shape)

A

a solid has fixed volume and shape

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Liquid (volume & shape)

A

a liquid has fixed volume but no definite shape

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

Gas (volume & shape)

A

a gas has no fixed volume or definite shape

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

Pressure

A

the force per unit area exerted on a surface

34
Q

Ideal Gas Law

A

PV=nRT

35
Q

Partial Pressure

A

The pressure exerted by each has in a mixture

36
Q

Mole Fraction (X, chi)

A

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
Q

Effusion

A

The passage of a gas through a small hole into an evacuated space

38
Q

What kind of gases effuse more rapidly?

A

Gases with low molar masses

39
Q

Diffusion

A

The mixing of particles due to motion

40
Q

Graham’s Law of Effusion

A

Relative rates of effusion can be used to determine molar mass (M)

41
Q

Waves

A

Periodic disturbances; the repeat at regular intervals of time and distance

42
Q

Wavelength (lambda)

A

Is the distance between one peak and the next

43
Q

Frequency (v)

A

The number of eaves that pass a fixed point each second

44
Q

What does electromagnetic radiation consist of?

A

Light or electromagnetic radiation consists of oscillating electric and magnetic fields

45
Q

How much visible light is one the electromagnetic spectrum?

A

Visible light is only a very small portion of the electromagnetic spectrum

46
Q

What is the smallest unit of energy?

A

A quantum

47
Q

What is the equation for the energy of a quantum?

A

E=hv

h is Planck’s constant

48
Q

Spectrum

A

A graph of light intensity as a function of wavelength or frequency

49
Q

Continuum or Continuous Spectrum

A

The light emitted by heated objects (light of all wavelengths is present)

50
Q

What kind of spectrum do gaseous atoms produce?

A

Gaseous atoms produce a line spectrum (one that contains light only at specific wavelengths and not at others)

51
Q

Wave Functions (Ψ)

A

Gives the amplitude of the electron wave at any point in space

52
Q

What does Ψ^2 give?

A

The probability of finding the electron at any point in space

53
Q

What does the solution of the wave equation produce?

A

The solution of the wave equation produces quantum numbers that describe the characteristics of the electron wave

54
Q

Atomic Orbital

A

A wave function of the electron for specific values of n, l, & m(l)

55
Q

What is the principle quantum number?

A

n

56
Q

What does the principle quantum number provide?

A

The principle quantum number, n, provides information about the energy and the distance of the electron from the nucleus

57
Q

What does a larger value of n mean?

A

The larger the value of n, the greater the average distance of the electron from the nucleus

58
Q

Principal Shell (or just Shell)

A

All atomic orbitals that have the same value of n

59
Q

What is the Angular Momentum Quantum Number?

A

l

60
Q

What is the angular momentum quantum number, l, for?

A

The angular momentum quantum number, l, is associated with the shape of the orbital

61
Q

What are the allowed values of l, the angular momentum quantum number?

A

0 and positive integers up to n-1

The l quantum number can never equal or exceed the value of n

62
Q

Subshell

A

All possible orbitals that have the same values of both n and l

63
Q

What is the Magnetic Quantum Number?

A

m(l)

64
Q

What does the magnetic quantum number, m(l), indicate?

A

The magnetic quantum number, m(l), indicates the orientation of the atomic orbital in space

65
Q

What are the allowed values of the magnetic quantum number?

A

-l to l, including 0

66
Q

Orbital

A

A wave function described by all three quantum numbers (n, l, m(l))

67
Q

What is the Electron Spin Quantum number?

A

m(s)

68
Q

What does the electron spin quantum number, m(s), represent?

A

The electron spin quantum number, m(s), represents one of the two allowed spin values, +1/2 and -1/2

69
Q

What is the shape of p orbitals?

A

p orbitals (l=1) have two lobes of electron density on opposite sides of the nucleus

70
Q

Electron shielding (screening)

A

The result of the influence of electrons on the effective nuclear charge

71
Q

Effective Nuclear Charge (Z(eff))

A

A weighted average of the nuclear charge that affects an electron in the atom

72
Q

Pauli Exclusion Principle

A

No two electrons in the same atom can have the same set of four quantum numbers

73
Q

Aufbau Principle

A

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
Q

Ground State

A

The resulting atom in its lowest energy state

75
Q

Orbital Diagram

A

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
Q

Hund’s Rule

A

One electron occupies each degenerate orbital with the same spin before a second electron is placed in an orbital

77
Q

Valence Electrons

A

Electrons with the highest principal quantum number and any electrons in an infilled subshell from a lower shell

78
Q

Valence Orbitals

A

Orbitals of those subshells that hold the valence electrons

79
Q

Isoelectronic Series

A

A group of atoms and ions with the same number of electrons

80
Q

Atomic Radius

A

One half the distance between adjacent atoms of the same element in a molecule

81
Q

Ionization Energy

A

The energy required to remove an electron from a gaseous atom or ion in its electronic ground state

82
Q

Electron Affinity

A

The energy change that accompanies the addition of an electron to a gaseous atom to form an anion

CHEM 111 (4 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions