Organic Chemistry Laboratory Flashcards
1
Q
What is the function of a beaker?
A
Contains and heats liquids but not for precise measurements.
2
Q
Which apparatus measures liquid volumes accurately?
A
Graduated Cylinder
3
Q
What is the most accurate volume measurement tool?
A
Volumetric Pipette
4
Q
What is the purpose of an analytical balance?
A
Used for precise mass measurements.
5
Q
What is a volumetric flask used for?
A
To contain a specified volume of reagents, solvents, or other liquids.
6
Q
What does a filter funnel do?
A
Helps separate solids from liquids during filtration.
7
Q
What is the function of a separatory funnel?
A
Used for liquid-liquid extractions.
8
Q
What happens if you fail to tare a balance?
A
Results in higher measured weight.
9
Q
What is large pore filter paper used for?
A
Allows solid particles to pass through.
10
Q
What are standard solutions?
A
Require careful weighing and taring.
11
Q
What is the process of filtration?
A
Separates solids from liquids.
12
Q
What does distillation separate?
A
Separates liquids based on boiling points.
13
Q
What is sublimation?
A
Solid to gas transition (e.g., iodine crystals).
14
Q
What is crystallization?
A
Slow cooling forms larger, purer crystals.
15
Q
What is fractional distillation ineffective for?
A
Ineffective if boiling points are too similar.
16
Q
What effect does excess solvent have in crystallization?
A
Reduces yield.
17
Q
What indicator is used for strong base titrations?
A
Phenolphthalein
18
Q
Which indicator is suitable for weak acid titrations?
A
Methyl Red
19
Q
What can overshooting in titration alter?
A
Alters molarity calculations.
20
Q
Why is rinsing a buret important?
A
Prevents dilution errors.
21
Q
What is formed during the combustion of magnesium?
A
Magnesium oxide.
22
Q
What occurs in decomposition reactions?
A
Single reactant breaks into multiple products.
23
Q
What does the reaction of zinc with HCl produce?
A
Hydrogen gas.
24
Q
What happens when ferrous sulfate is heated?
A
Turns brown due to oxidation.
25
What color flame does copper produce in a flame test?
Green.
26
What color flame does potassium produce?
Purple.
27
What color flame does sodium produce?
Yellow.
28
What occurs when electrons move to lower energy levels?
Light is emitted.
29
What is the relationship between wavelength and energy?
Shorter wavelengths have higher energy.
30
How should NaOH be handled?
Add slowly to prevent exothermic splashes.
31
What is a hazard of HCl?
Corrosive to the respiratory system.
32
How should chemical waste be disposed of?
In designated containers.
33
Why is wearing goggles important in the lab?
Protects against NaOH and acid splashes.
34
What is the purpose of cleaning copper wire?
Removes oxidation for clear reactions.
35
What mistake can occur with buret rinsing?
Rinsing with water dilutes the titrant, causing errors.
36
What must be done with spills in the lab?
Must be cleaned to prevent contamination and accidents.
37
What safety measure should be taken during flame tests?
Avoid using plastic spatulas.
38
How should nichrome wire be cleaned?
With HCl and flame heating.
39
What is the proper titration technique?
Slow swirling ensures endpoint accuracy.
40
What does hot filtration prevent?
Prevents premature crystallization.
41
What effect do impurities have on boiling points?
Raises boiling point, making separation harder.
42
What do color changes in reactions help identify?
Help identify compounds.
43
What is a key lab practice for safety?
Maintain a clean workspace to avoid hazards.
44
What should you review for your exam?
Lab apparatus functions and uses.
45
What should you understand regarding separation techniques?
Their applications.
46
What is a tip for exam preparation?
Read questions carefully and review experiment procedures.
47
What are atoms?
Building blocks of matter. Smallest particles of an element that still have the element’s properties.
48
What are the three types of sub-atomic particles?
* Protons - positive electric charge
* Electrons - negative electric charge
* Neutrons - neutral in electric charge
49
Define matter.
Substance made up of various types of particles that occupies physical space and has inertia.
50
What is an element?
Composed of only one type of atom. Cannot convert to simpler matter by physical or chemical methods.
51
What is a molecule?
A group of two or more atoms held together by forces called chemical bonds.
52
What is a compound?
A pure substance that consists of atoms of two or more elements always chemically combined in the same proportion.
53
What distinguishes a mixture?
Two or more pure substances mixed such that the ratio of the constituents is variable.
54
What are the two types of mixtures?
* Homogeneous – components are evenly distributed
* Heterogeneous – components are not thoroughly mixed
55
What are the characteristics of solids?
* Has a definite shape
* Has a definite volume
* Fixed, very close arrangement of particles
* Very strong interaction between particles
* Particles vibrate in fixed positions
56
What are the characteristics of liquids?
* Takes the shape of the container
* Has a definite volume
* Random, close arrangement of particles
* Strong interaction between particles
* Particles move slowly around each other
57
What are the characteristics of gases?
* Takes the shape of the container
* Fills the volume of the container
* Random, far apart arrangement of particles
* Essentially no interaction between particles
* Particles move rapidly and spread out
58
Define physical properties.
Characteristics that can be observed or measured without affecting the identity of a substance.
59
What is a physical change?
When matter undergoes a change in state, size, or appearance, but its composition does not change.
60
Define chemical properties.
Describe the ability of a substance to change into a new substance.
61
What is a chemical change?
A change in which the original substance is converted to one or more new substances.
62
What is energy?
Ability to do work.
63
What is kinetic energy?
Energy of motion given by the equation KE = ½ mv².
64
What is potential energy?
Stored energy, typically given by the equation PE = mgh.
65
What is the Law of Conservation of Energy?
Energy cannot be created or destroyed, only transformed.
66
What is an exothermic reaction?
Chemical reactions that release energy.
67
What is an endothermic reaction?
Chemical reactions that absorb energy.
68
Who arranged the periodic table in 1869?
Dmitri Mendeleev.
69
What is a group in the periodic table?
A vertical column of elements with similar properties.
70
What is a period in the periodic table?
A row of chemical elements where all elements have the same number of electron shells.
71
What are alkali metals?
Soft, shiny metals that are good conductors of heat and electricity with low melting points.
72
What are alkaline earth metals?
Shiny metals that are good conductors of electricity but not as reactive as alkali metals.
73
Define halogens.
Highly reactive non-metals that form compounds with most elements.
74
What are noble gases?
Unreactive gases that are seldom found in combination with other elements.
75
What are metalloids?
Elements that exhibit properties of both metals and nonmetals and are considered semiconductors.
76
Define wavelength.
Distance from a crest or trough in the wave to the next crest or trough.
77
What is frequency?
Number of waves that pass a fixed place in a given amount of time.
78
What is the wave equation?
c = λν where c is the speed of light.
79
How is energy related to wavelength?
Energy is inversely related to wavelength.
80
What is an atomic spectrum?
The unique lines of different colors produced when light emitted from heated elements is passed through a prism.
81
What are electron energy levels?
Specific energy values assigned to electrons in an atom, denoted by the principal quantum number (n).
82
What happens when an atom absorbs energy?
An electron moves to a higher energy level called an excited state.
83
What is the Pauli exclusion principle?
States that each orbital can hold a maximum of two electrons with opposite spins.
84
What are intramolecular forces?
Forces that keep the atoms or ions together in a compound.
85
What are intermolecular forces?
* Dipole-dipole attractions
* Hydrogen bonds
* Dispersion forces
86
Fill in the blank: The maximum number of electrons allowed in energy level 2 is _______.
8
87
Fill in the blank: Alkali metals are found in group _______.
1A
88
What forms compounds?
Compounds form when electrons are transferred or shared between atoms to give stable electron configurations to the atoms.
89
What is the octet rule?
Atoms lose, gain, or share valence electrons to acquire an octet of eight valence electrons.
90
What occurs during ionic bonds?
Ionic bonds occur when the valence electrons of atoms of a metal are transferred to atoms of nonmetals.
91
Give an example of an ionic compound.
NaCl, formed when sodium atoms lose electrons and chlorine atoms gain electrons.
92
What are covalent bonds?
Covalent bonds form when atoms of nonmetals share valence electrons.
93
What happens to metal atoms in Groups 1A, 2A, and 3A?
Metal atoms readily lose their valence electrons, making them positively charged ions.
94
What characterizes nonmetal atoms in Groups 5A, 6A, or 7A?
Nonmetal atoms do not easily lose their valence electrons and can gain one or more, making them negatively charged ions.
95
What is electronegativity?
Electronegativity is the ability of an atom to attract the shared electrons in a chemical bond.
96
Which type of atoms have higher electronegativities?
Nonmetals have higher electronegativities than metals.
97
Do noble gases have electronegativity values?
No, noble gases do not typically form bonds, so they have no electronegativity values.
98
What is a dipole?
A dipole is a polar covalent bond that has a separation of charges, with a positive end (δ+) and a negative end (δ-).
99
What does the difference in electronegativity values indicate?
The difference in electronegativity values can be used to predict whether a bond is ionic or covalent.
100
What is the formula for an ionic compound?
Represents the symbols and subscripts in the lowest whole-number ratio of the atoms or ions.
101
What is the naming convention for ionic compounds?
The name of the metal ion is the same as its element name; the nonmetal ion uses the first syllable followed by -ide.
102
How are metals with variable charges named?
A Roman numeral indicating the ionic charge is placed in parentheses after the name of the metal.
103
What is a polyatomic ion?
A group of covalently bonded atoms that has an overall ionic charge.
104
What is the charge of most polyatomic ions?
Almost all polyatomic ions are anions with charges of 1-, 2-, or 3-.
105
What is a chemical change?
A chemical change occurs when a substance is converted into one or more new substances.
106
What is a chemical equation?
A representation of a chemical reaction, showing reactants on the left and products on the right.
107
What denotes the physical state of a substance in a chemical equation?
Abbreviations such as (s), (l), (g), or (aq) denote solid, liquid, gas, or aqueous solution respectively.
108
What is the first step in balancing chemical equations?
Identify the number of atoms of each element on both sides of the equation.
109
What is a combination reaction?
A reaction where two or more elements or compounds bond to form one product.
110
What is a decomposition reaction?
A reaction where a reactant splits into two or more simpler products.
111
What does a single replacement reaction involve?
A reacting element switches place with an element in another reacting compound.
112
What characterizes a double replacement reaction?
Positive ions in the reacting compounds switch places.
113
What is combustion?
A reaction where a carbon-containing compound burns in oxygen to produce carbon dioxide, water, and energy.
114
What is oxidation-reduction (redox)?
A reaction where electrons are transferred from one substance to another.
115
What does OIL and RIG stand for?
OIL: Oxidation Is Loss of electrons; RIG: Reduction Is Gain of electrons.
