Vocab Flashcards
(117 cards)
1
Q
The point above which a gas cannot be converted into a liquid is known as what
A
Critical point
2
Q
Point in titration curve where the pKa or pKb can be determined
A
Infection point
3
Q
Point during titration when the moles of titrant are equal to the moles of titrate (acid = base)
A
Equivalence point
4
Q
Point during titration when an indicator shows a color change and has reached the equivalence point
A
End point
5
Q
Temperature and pressure at which all three phases exist together
A
Triple point
6
Q
What best describes the energy conversion process of a battery operating in a remote controller?
A
Chemical to electrical
7
Q
Energy associated with objects in motion
A
Kinetic energy
8
Q
Energy associated with an object’s relative position to the ground
A
Potential energy
9
Q
Energy associated with an object’s potential to do work
A
Mechanical energy
10
Q
Energy associated with dissipated heat from a chemical reaction
A
Thermal energy
11
Q
Energy associated with making or breaking chemical bonds
A
Chemical energy
12
Q
Energy associated with the ability to supply current and voltage
A
Electrical energy
13
Q
Positive terminal in an electrochemical cell of a battery
A
Cathode
14
Q
Negative terminal in an electrochemical cell of a battery
A
Anode
15
Q
Samples analyzed from a variety of sources possess the same ratio of elements within each sample
A
Compound
16
Q
A type of mixture in which an immiscible element type is suspended evenly and uniformly in a dispersing medium
A
Colloid
17
Q
Solid to liquid
A
Fusion
18
Q
Liquid to gas
A
Vaporization
19
Q
Solid to gas
A
Sublimation
20
Q
What kind of reactions are fusion, vaporization, and sublimation?
A
Endothermic
21
Q
Gas to liquid
A
Condensation
22
Q
What kind of reactions are freezing, condensation, and deposition?
A
Exothermic
23
Q
Gas to solid
A
Deposition
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
25
What condition will always create a spontaneous process?
ΔH°= -'ve, ΔS°= +'ve
26
Unit that depends only on the change between initial and final states of a system
State function
27
Unit that depends only on the process by which the change occurs
Path function
28
Why does a proton and neutron weigh more separately than when they are bound together?
Mass is converted into nuclear binding energy
29
Method of separation used to separate solids from liquids
Filtration
30
Separate liquids of different polarities. Different liquids move at different rates through a solid phase based on how much they are attracted to it
Chromatography
31
Separates different liquids based on their boiling points
Distillation
32
Separatory funnel shaken and allows for immiscible liquids (polar and nonpolar) to be separated into distinct layers
Extraction
33
Spins fast to allow dense elements in a mixture to move to the bottom of a vessel.
Centrifugation
34
Diatomic atoms mneomic
Have No Fear Of Ice Cold Beer
35
What diatomic element is liquid at room temperature?
Br2
36
What diatomic element is solid at room temperature?
I2
37
All of the diatomic molecules except I2 and Br2 are what at room temperature?
Gas
38
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?
Molar absorptivity
39
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?
The pH will increase because the ratio of [A-]/[HA] is increased
40
What is the maximum number of electrons that can be held in the 4p subshell?
3x2 = 6
41
What must be true for a chemical reaction that has the same activation energy for the forward and reverse directions?
ΔG° = 0
42
Why is adding water to concentrated acid unsafe?
An extremely exothermic reaction occurs and acid may start boiling. Acid should be added to water
43
Rhyme for adding acid to watter
Do what you oughta, add acid to water
44
What physical property is described when the vapor pressure of a liquid equals the atmospheric pressure?
Boiling point
45
Pressure exerted by the vapor in equilibrium with its condensed phases in a closed system, at a given temperature
Vapor pressure
46
Pressure exerted by the weight of air in the atmosphere
Atmospheric pressure
47
What is true with regards to signs of thermodynamic parameters if a pure substance in the solid phase sublimes spontaneously?
ΔH° = + | ΔS° = +| ΔG° = -
48
What happens if the temperature is lowered for a liquid in a sealed container?
There are less gas molecules
49
What would be a good equipment to measure mL of a liquid?
Burette
50
The definition of molality is best defined as
Moles of solute / kg of solvent
51
The definition of molarity is best defined as
Moles of solute / liters of solution
52
A solution that cannot dissolve any more solute at room temperature is
Saturated
53
Contains less than the maximum amount of solute that can be dissolved at that temperature
Unsaturated
54
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
Supersaturated
55
One that cannot exchange matter or energy with its surroundings
Isolated system
56
Can exchange energy with its surrounding but not matter
Closed system
57
Can exchange both energy and matter with its surroundings
Open system
58
Energy cannot be created nor destroyed
First law of thermodynamics
59
For a spontaneous process, the entropy of the universe increases
Second law of thermodynamics
60
If the temperature of an ideal gas is quadrupled under isovolumetric conditions, what will occur to the pressure?
4x the original pressure
61
Weaker intermolecular forces result in a higher
Vapor pressure
62
What are the seven strong acids?
HI, HBr, HCl, HClO4, HClO3, H2SO4, and HNO3
63
Why is sodium more reactive than magnesium?
Sodium has a lowest electronegativity
64
Covalent bonds made by the end-to-end overlap of atomic orbitals
Sigma bonds
65
Covalent bonds made by the side-to-side (lateral) overlap of p-orbitals
Pi bonds
66
Energy required to break a bond
Bond energy
67
Energy required for a reaction to proceed
Activation energy
68
Electrochemical cells which release electrical energy from spontaneous oxidation-reduction reactions. Purpose is to produce electrical energy
Galvanic cells
69
If a reaction has a negative ΔH value the reaction will be
Exothermic (energy released)
70
An incorrectly calibrated pipet is used during an experiment. What will this cause?
Systematic error
71
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.
Systematic error (not tarring balancing correctly)
72
Errors caused by experimenter carelessness or equipment failure
Gross error
73
Errors caused by uncontrollable fluctuations in variables that affect experimental
Random error
74
Errors due to faulty procedure adopted by the person making measurements
Personal error
75
Shape of the orbital
Azimuthal quantum number
76
Orbital size and energy level
Principal quantum number
77
Electron spin direction
Spin quantum number
78
Orbital orientation
Magnetic quantum number
79
Electron acceptor
Lewis acid
80
Electron donor
Lewis base
81
Proton donor
Bronsted-Lowry acid
82
Proton acceptor
Bronsted-Lowry base
83
Dissociate to form hydroxide (OH) ions
Arrhenius bases
84
Dissociate in water forming proton ions
Arrhenius acids
85
The atomic theory states that matter is composed of
Atoms
86
What gas law states that two gases of equal volumes will also have equal number of molecules at the same temperature and pressure
Avogadro's Law
87
Volume of a gas is directly proportional to the temperature when the pressure is held constant
Charles Law
88
Pressure of a gas is directly proportional to the temperature when volume is held constant
Gay-Lussac's Law
89
Total pressure exerted by a mixture of gases is equal to the sum of the individuals gases partial pressures
Dalton's Law
90
Volume of a gas is inversely proportional to the pressure when temperature is held constant
Boyle's Law
91
If you halve the temperature of a gas at constant pressure, what happens to the volume?
Volume will be halved
92
What process occurs when the vapor pressure of a liquid equals the atmospheric pressure?
Boiling
93
Example of a random error
Reading the meniscus at a different angle each time
94
Elements that have 7 electrons in their outer shells and commonly form salts during chemical reactions are known as?
Halogens
95
What's the molecular geometry for PCl5?
Trigonal bypyramidal
96
What conditions do gases NOT behave ideally?
High pressure
97
When all replicates are close to the expected value
Accuracy
98
When all replicates have similar values in magnitude
Precision
99
What types of glassware sits below the burette in an acid-base titration?
Erlenmeyer flask
100
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?
The compound with the lower specific heat
101
The high boiling point of water can be best attributed to
Extensive hydrogen bonds
102
What is the number of parts per million of NaCl in a 0.50% saline solution?
10000x0.50 = 5000
103
The energy required to disassemble the nucleus of an atom into its components
Nuclear binding energy
104
If you halve the pressure of a gas at a constant temperature, what happens to volume?
Volume will double
105
What conditions must there be for a supercritical fluid to be changed back to liquid gas?
Decrease temperature
106
Forces between two neighboring molecules
Intermolecular forces
107
Forces that hold a molecule together
Intramolecular forces
108
Examples of intramolecular forces
Covalent, metallic, and ionic bonds
109
Examples of intermolecular forces
Van der waals, dipole-induced, dipole-dipole, hydrogen bonds, ion-dipole
110
Transition metals have partially filled
d-subshells
111
What property determines the strength of an acid?
Stability of a conjugate base
112
Works for compounds that have boiling points that are <25 degrees celcius apart
Fractional distillation
113
Works for compounds that have boiling points 150> degrees celcius apart
Vacuum distillation
114
What are the type of simple distillation?
Fractional and vacuum
115
Which diatomic atom forms double bonds?
Oxygen
116
Which diatomic atom forms triple bonds?
Nitrogen
117
What is typically found in alkaline buffer?
Weak base and its conjugate acid
