Brainscape's Knowledge GenomeTM

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


See full index

Gen Chem > Vocab > Flashcards

Vocab Flashcards

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

The point above which a gas cannot be converted into a liquid is known as what

A

Critical point

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

Point in titration curve where the pKa or pKb can be determined

A

Infection point

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

Point during titration when the moles of titrant are equal to the moles of titrate (acid = base)

A

Equivalence point

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

Point during titration when an indicator shows a color change and has reached the equivalence point

A

End point

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

Temperature and pressure at which all three phases exist together

A

Triple point

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

What best describes the energy conversion process of a battery operating in a remote controller?

A

Chemical to electrical

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

Energy associated with objects in motion

A

Kinetic energy

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

Energy associated with an object’s relative position to the ground

A

Potential energy

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

Energy associated with an object’s potential to do work

A

Mechanical energy

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

Energy associated with dissipated heat from a chemical reaction

A

Thermal energy

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

Energy associated with making or breaking chemical bonds

A

Chemical energy

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

Energy associated with the ability to supply current and voltage

A

Electrical energy

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

Positive terminal in an electrochemical cell of a battery

A

Cathode

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

Negative terminal in an electrochemical cell of a battery

A

Anode

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

Samples analyzed from a variety of sources possess the same ratio of elements within each sample

A

Compound

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

A type of mixture in which an immiscible element type is suspended evenly and uniformly in a dispersing medium

A

Colloid

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

Solid to liquid

A

Fusion

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

Liquid to gas

A

Vaporization

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

Solid to gas

A

Sublimation

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

What kind of reactions are fusion, vaporization, and sublimation?

A

Endothermic

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

Gas to liquid

A

Condensation

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

What kind of reactions are freezing, condensation, and deposition?

A

Exothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Gas to solid

A

Deposition

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What best describes signs of heat and internal energy if no work is done in a reaction but heat is lost?

A

q < 0, ΔE < 0

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

What condition will always create a spontaneous process?

A

ΔH°= -‘ve, ΔS°= +’ve

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

Unit that depends only on the change between initial and final states of a system

A

State function

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

Unit that depends only on the process by which the change occurs

A

Path function

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

Why does a proton and neutron weigh more separately than when they are bound together?

A

Mass is converted into nuclear binding energy

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

Method of separation used to separate solids from liquids

A

Filtration

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

Separate liquids of different polarities. Different liquids move at different rates through a solid phase based on how much they are attracted to it

A

Chromatography

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

Separates different liquids based on their boiling points

A

Distillation

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

Separatory funnel shaken and allows for immiscible liquids (polar and nonpolar) to be separated into distinct layers

A

Extraction

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

Spins fast to allow dense elements in a mixture to move to the bottom of a vessel.

A

Centrifugation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

Diatomic atoms mneomic

A

Have No Fear Of Ice Cold Beer

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

What diatomic element is liquid at room temperature?

A

Br2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

What diatomic element is solid at room temperature?

A

I2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

All of the diatomic molecules except I2 and Br2 are what at room temperature?

A

Gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

Compared to benzene, when naphthalene is placed under UV light using a prism block, the resulting mixture appears more opaque. What physical property has changed to account for the difference in opacity between benzene and napthalene?

A

Molar absorptivity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

Consider a solution that consists of a weak acid [HA] and its conjugate base [A-]. If a small amount of a strong base is added to the buffer, how will the pH change and why?

A

The pH will increase because the ratio of [A-]/[HA] is increased

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

What is the maximum number of electrons that can be held in the 4p subshell?

A

3x2 = 6

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

What must be true for a chemical reaction that has the same activation energy for the forward and reverse directions?

A

ΔG° = 0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

Why is adding water to concentrated acid unsafe?

A

An extremely exothermic reaction occurs and acid may start boiling. Acid should be added to water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

Rhyme for adding acid to watter

A

Do what you oughta, add acid to water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

What physical property is described when the vapor pressure of a liquid equals the atmospheric pressure?

A

Boiling point

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
45
Q

Pressure exerted by the vapor in equilibrium with its condensed phases in a closed system, at a given temperature

A

Vapor pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
46
Q

Pressure exerted by the weight of air in the atmosphere

A

Atmospheric pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
47
Q

What is true with regards to signs of thermodynamic parameters if a pure substance in the solid phase sublimes spontaneously?

A

ΔH° = + | ΔS° = +| ΔG° = -

48
Q

What happens if the temperature is lowered for a liquid in a sealed container?

A

There are less gas molecules

49
Q

What would be a good equipment to measure mL of a liquid?

A

Burette

50
Q

The definition of molality is best defined as

A

Moles of solute / kg of solvent

51
Q

The definition of molarity is best defined as

A

Moles of solute / liters of solution

52
Q

A solution that cannot dissolve any more solute at room temperature is

A

Saturated

53
Q

Contains less than the maximum amount of solute that can be dissolved at that temperature

A

Unsaturated

54
Q

Contains more than the maximum amount of solute that can be dissolved at that temperature. It is unstable and the solute will usually begin to crystallize, especially if disturbed

A

Supersaturated

55
Q

One that cannot exchange matter or energy with its surroundings

A

Isolated system

56
Q

Can exchange energy with its surrounding but not matter

A

Closed system

57
Q

Can exchange both energy and matter with its surroundings

A

Open system

58
Q

Energy cannot be created nor destroyed

A

First law of thermodynamics

59
Q

For a spontaneous process, the entropy of the universe increases

A

Second law of thermodynamics

60
Q

If the temperature of an ideal gas is quadrupled under isovolumetric conditions, what will occur to the pressure?

A

4x the original pressure

61
Q

Weaker intermolecular forces result in a higher

A

Vapor pressure

62
Q

What are the seven strong acids?

A

HI, HBr, HCl, HClO4, HClO3, H2SO4, and HNO3

63
Q

Why is sodium more reactive than magnesium?

A

Sodium has a lowest electronegativity

64
Q

Covalent bonds made by the end-to-end overlap of atomic orbitals

A

Sigma bonds

65
Q

Covalent bonds made by the side-to-side (lateral) overlap of p-orbitals

A

Pi bonds

66
Q

Energy required to break a bond

A

Bond energy

67
Q

Energy required for a reaction to proceed

A

Activation energy

68
Q

Electrochemical cells which release electrical energy from spontaneous oxidation-reduction reactions. Purpose is to produce electrical energy

A

Galvanic cells

69
Q

If a reaction has a negative ΔH value the reaction will be

A

Exothermic (energy released)

70
Q

An incorrectly calibrated pipet is used during an experiment. What will this cause?

A

Systematic error

71
Q

Error that is not determined by chance, but it is introduced by an inaccuracy inherent in the system, leading to consistent inaccuracies in data collection.

A

Systematic error (not tarring balancing correctly)

72
Q

Errors caused by experimenter carelessness or equipment failure

A

Gross error

73
Q

Errors caused by uncontrollable fluctuations in variables that affect experimental

A

Random error

74
Q

Errors due to faulty procedure adopted by the person making measurements

A

Personal error

75
Q

Shape of the orbital

A

Azimuthal quantum number

76
Q

Orbital size and energy level

A

Principal quantum number

77
Q

Electron spin direction

A

Spin quantum number

78
Q

Orbital orientation

A

Magnetic quantum number

79
Q

Electron acceptor

A

Lewis acid

80
Q

Electron donor

A

Lewis base

81
Q

Proton donor

A

Bronsted-Lowry acid

82
Q

Proton acceptor

A

Bronsted-Lowry base

83
Q

Dissociate to form hydroxide (OH) ions

A

Arrhenius bases

84
Q

Dissociate in water forming proton ions

A

Arrhenius acids

85
Q

The atomic theory states that matter is composed of

A

Atoms

86
Q

What gas law states that two gases of equal volumes will also have equal number of molecules at the same temperature and pressure

A

Avogadro’s Law

87
Q

Volume of a gas is directly proportional to the temperature when the pressure is held constant

A

Charles Law

88
Q

Pressure of a gas is directly proportional to the temperature when volume is held constant

A

Gay-Lussac’s Law

89
Q

Total pressure exerted by a mixture of gases is equal to the sum of the individuals gases partial pressures

A

Dalton’s Law

90
Q

Volume of a gas is inversely proportional to the pressure when temperature is held constant

A

Boyle’s Law

91
Q

If you halve the temperature of a gas at constant pressure, what happens to the volume?

A

Volume will be halved

92
Q

What process occurs when the vapor pressure of a liquid equals the atmospheric pressure?

A

Boiling

93
Q

Example of a random error

A

Reading the meniscus at a different angle each time

94
Q

Elements that have 7 electrons in their outer shells and commonly form salts during chemical reactions are known as?

A

Halogens

95
Q

What’s the molecular geometry for PCl5?

A

Trigonal bypyramidal

96
Q

What conditions do gases NOT behave ideally?

A

High pressure

97
Q

When all replicates are close to the expected value

A

Accuracy

98
Q

When all replicates have similar values in magnitude

A

Precision

99
Q

What types of glassware sits below the burette in an acid-base titration?

A

Erlenmeyer flask

100
Q

Two different compounds of identical weight and initial temperature absorb the same amount of energy and undergo temperature changes. Which compound has the higher temperature?

A

The compound with the lower specific heat

101
Q

The high boiling point of water can be best attributed to

A

Extensive hydrogen bonds

102
Q

What is the number of parts per million of NaCl in a 0.50% saline solution?

A

10000x0.50 = 5000

103
Q

The energy required to disassemble the nucleus of an atom into its components

A

Nuclear binding energy

104
Q

If you halve the pressure of a gas at a constant temperature, what happens to volume?

A

Volume will double

105
Q

What conditions must there be for a supercritical fluid to be changed back to liquid gas?

A

Decrease temperature

106
Q

Forces between two neighboring molecules

A

Intermolecular forces

107
Q

Forces that hold a molecule together

A

Intramolecular forces

108
Q

Examples of intramolecular forces

A

Covalent, metallic, and ionic bonds

109
Q

Examples of intermolecular forces

A

Van der waals, dipole-induced, dipole-dipole, hydrogen bonds, ion-dipole

110
Q

Transition metals have partially filled

A

d-subshells

111
Q

What property determines the strength of an acid?

A

Stability of a conjugate base

112
Q

Works for compounds that have boiling points that are <25 degrees celcius apart

A

Fractional distillation

113
Q

Works for compounds that have boiling points 150> degrees celcius apart

A

Vacuum distillation

114
Q

What are the type of simple distillation?

A

Fractional and vacuum

115
Q

Which diatomic atom forms double bonds?

A

Oxygen

116
Q

Which diatomic atom forms triple bonds?

A

Nitrogen

117
Q

What is typically found in alkaline buffer?

A

Weak base and its conjugate acid

Gen Chem (1 decks)

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