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Inorganic and Organic Chemistry (Lab) > Laboratory > Flashcards

Laboratory Flashcards

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1
Q

Explain the Law of Multiple Proportions

A

In a compound, the mass of element B combined with the fixed mass of element A has a ratio of small whole numbers.

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2
Q

Used to weigh solids that will be transferred to another vessel

A

Weighing boat

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3
Q

1 ounce is equal to how many grams

A

28.350 grams

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4
Q

Formula for converting F to C

A

F = 5/9 (C -32)

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5
Q

Used to heat solids, particularly metals at a very high temperature

A

Crucible

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6
Q

What is an exothermic reaction?

A

When the bonding releases more energy to produce a substance than when breaking down the reactants.

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7
Q

What is an endothermic reaction?

A

Chemical reactions that absorb heat energy from the surroundings to form products.

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8
Q

When is the beaker used?

A

Used in holding solids and liquids that do not release gas and are unlikely to splatter

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9
Q

It has a narrow neck to prevent splash exposure

A

Florence flask

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10
Q

Erlenmeyer flask

A

Used for holding solids and liquids that release gases and are most likely to splatter

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11
Q

Used to measure small volumes of liquids

A

Graduated cylinder

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12
Q

Gas collecting bottle

A

hold large volume of gases extracted through displacement of water

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13
Q

Test tube

A

hold chemicals at smaller amount

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14
Q

Used to close containers and to prevent contamination within the substance

A

Rubber stoppers

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15
Q

Used to perform multiple small reactions at the same time

A

Spot Plates

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16
Q

Watch glass

A

To hold small amount of solids, usually a product

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17
Q

Glass stir rod

A

To manually stir and transfer a drop

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18
Q

Medicine dropper

A

To transfer small amount of liquids

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19
Q

To pick up small pieces

A

Forceps

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20
Q

Funnel

A

To transfer a substance to another vessel

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21
Q

Measure exact volumes of liquids

A

Mohr pipet

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22
Q

Used to put distilled water in a specific area

A

Wash bottle

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23
Q

Spatulas

A

Used to dispense small solid particles

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24
Q

Used to hold heated beakers

A

Beaker thong

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25
Q

Bunsen Burners

A

used to heat nonvolatile solids and liquids

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26
Q

Evaporating dish

A

to heat stable compounds and elements

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27
Q

holds crucible when heating through a bunsen burner

A

Clay triangle

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28
Q

Triangular files

A

Used to cut stir rod

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29
Q

a convenient way of heating using bunsen burners

A

Ring stand

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30
Q

Iron rings

A

provide stable and elevated platform when heating through a bunsen burner

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31
Q

Utility clamps

A

Used to hold test tubes

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32
Q

Double buret clamps

A

Used to hold burets when heating

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33
Q

What is a buret?

A

Mostly used in titration

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34
Q

Wire Gauze

A

a place to stand a beaker

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35
Q

Pressed fiber pad

A

a platform to avoid contact between a cold counter top and a heated beaker

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36
Q

Strikers

A

Used to ignite bunsen burners

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37
Q

True or False. Use water displacement in measuring the volume of things that has no definite shape.

A

True

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38
Q

Define measurement.

A

Process of comparing quantity to a standard quantity and identifying if it exceeds or is less than the standard.

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39
Q

The method used in measuring

A

Type

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40
Q

An actual numerical value

A

Magnitude

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41
Q

Unit

A

standard quantity

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42
Q

Random errors in a measurement

A

Uncertainty

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43
Q

Where did the SI Units originate?

A

France

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44
Q

SI Units stands for?

A

International System of Units

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45
Q

Enumerate the big 7 and its corresponding units.

A 
Length - meter
Mass - kilograms
Time - second
Temperature - kelvin
Amount of substance - mole
Luminous intensity - candela
Electric current - Ampere
46
Q

Also known as the general system

A

Metric system

47
Q

What system uses measurements that have no definite ratio and proportion?

A

The British / Imperial System

48
Q

How many ounces in a pound?

A

16 oz

49
Q

1 lb = ? grams

A

453.592 grams

50
Q

What is the process of filtration?

A

Solids are separated from liquids through a filter medium that only permits liquids to pass.

51
Q

Distillation

A

Used to separate substances with different boiling temperatures.

52
Q

True or False. In distillation, a substance that has a very low boiling temperature is the last to pass in the process.

A

False.

53
Q

Explain the process of distillation.

A

The mixture is heated until it reaches its boiling temperature, the substance is transferred to a condenser and it will be the one separated. The other is left behind in the distillate.

54
Q

Used to separate a soluble solid into a liquid.

A

Evaporation

55
Q

A process involving impure solids dissolved in a heated solvent and cooled down at room temperature until crystals formed

A

Crystallization

56
Q

The device used in centrifugation

A

Centrifuge

57
Q

What happens when a mixture is placed on the centrifuge?

A

The denser component of a mixture will sink at the bottom due to the centripetal force they experienced during the process.

58
Q

What is the difference between sedimentation and decantation?

A

Sedimentation is where solid particles settle out of a liquid duet to force of gravity. Decantation is similar but with insoluble liquids and is a slow and tedious process.

59
Q

A separation that uses magnets to attract magnetic materials in a composition

A

Magnetic separation

60
Q

A separation where the other component goes from solid to vapor without passing through a liquid state.

A

Sublimation

61
Q

A law that states that mass can neither be created nor destroyed and must remain constant over time.

A

Law of Conservation of Mass

62
Q

True or False. Total mass of reactants = total mass of the products

A

True

63
Q

Law of Definite Proportions

A

A chemical compound has a fixed and constant proportion by its corresponding elements.

64
Q

The formula in calculating the percentage mass.

A

% = (mass of element in one mole/ mass of compound in one mole ) * 100

65
Q

A good conductor of heat and electricity

A

Metals

66
Q

Also known as insulators

A

Nonmetals

67
Q

True or False. Nonmetals have large atomic radii, high ionization, and large negative electron affinities.

(If false, correct the statement)

A

False. Nonmetals have small atomic radii, high ionization, and large negative electron affinities.

68
Q

Also known as elements in “stairsteps”

A

Metalloids

69
Q

True or False. A metalloid is metal-like with nonmetal properties.

A

True

70
Q

What elements are halogens?

A

F, Br, Cl, I, As

71
Q

Which halogen is the most reactive and why?

A

Fluorine due to its high electronegativity

72
Q

Define electronegativity.

A

The measure of tendency of an atom to attract bonding electrons.

73
Q

True or False. The more reactive element displaces the less reactive in a compound

A

True

74
Q

Organic Chemistry

A

The study of compounds of carbons and its derivatives.

75
Q

A small atom that forms a single, double, and triple bond

A

Carbon

76
Q

True or False. Organic compounds are all compounds of carbon except oxides of carbon, carbonates, bicarbonates and carbides of metals

A

True

77
Q

True or False. Organic compounds are ionic in nature.

If false, correct the statement

A

False. They are covalent and nonpolar in nature.

78
Q

True or False. Organic compounds burn exothermically

If false, correct the statement

A

True

79
Q

Compounds that have the same molecular formula but different structural formula

A

Isomerism

80
Q

Used in finding out if a substance is present in a sample

A

Qualitative analysis

81
Q

What is quantitative analysis?

A

Used to find out how much substance in a sample.

82
Q

A group of atoms found within molecules that are involved in the characteristics of the chemical reaction of those molecules

A

Functional Groups

83
Q

Hydrocarbons can be classified as either?

A

Aromatic or aliphatic compounds

84
Q

Differentiate saturated and unsaturated compounds.

A

Saturated are those having a single bond with a hydrogen atom. Unsaturated consist of a double or triple bond

85
Q

What does EAS stand for?

A

Electrophilic Aromatic Substitution

86
Q

Gives the actual number of atoms present in a compound

A

Molecular formula

87
Q

Smallest whole number ratio

A

Empirical formula

88
Q

Enumerate and explain the two classifications of matter.

A

Pure substance are those that cannot be broken down into simplest form and has a constant properties. Mixture is when two or more substances are physically combined.

89
Q

What are the two types of a mixture?

A

Homogeneous and heterogeneous mixture.

90
Q

Malleability

A

The capability of being shaped or extended

91
Q

Used to measure a substance’s ability to conduct heat

A

Thermal conductivity

92
Q

Zn, Fe, Ni, Mg are examples of?

A

Metals

93
Q

True or False. Silicon and Carbon are nonmetals

If false, correct the statement.

A

False. Si and C are metalloids.

94
Q

Reactivity of displacement of Cl

A

Reacts with Br & I

95
Q

What are Fl and Cl’s physical states?

A

Gas

96
Q

True or False. I and As are Solid at room temperature.

A

True

97
Q

Define thermal decomposition

A

Breaking down of a composition through heating

98
Q

Which color of flame is rare?

A

Blue

99
Q

Determine the color of the element in the flame test.

Potassium

A

Lilac

100
Q

Determine the color of the element in the flame test.

Barium

A

Pale Green

101
Q

Determine the color of the element in the flame test.

Calcium

A

Orange

102
Q

Determine the color of the element in the flame test.

Lithium

A

Red

103
Q

Determine the color of the element in the flame test.

Copper

A

Blue Green

104
Q

Determine the color of the element in the flame test.

Strontium

A

Pink

105
Q

Determine the color of the element in the flame test.

Sodium

A

Yellow Orange

106
Q

What is the relationship between electronegativity and reactivity?

A

Elements with higher electronegativity tend to be more reactive

107
Q

What is the product in an experiment for the thermal stability of carbonates?

A

Metal oxide and carbon dioxide

108
Q

Who was the proponent of Law of Definite Proportions and when was it proposed?

A

Joseph Louis Proust of France in 1794

109
Q

Who was the proponent of Law of Multiple Proportions and when was it proposed?

A

John Dalton in 1804

110
Q

Define accuracy.

A

How close is the measured value to the true value

111
Q

Define precision.

A

How close the measured values are to each other.

112
Q

Enumerate elements in halogen group and its corresponding color

A 
Fluorine - pale green
Chlorine - greenish-yellow
Bromine - reddish brown
Iodine - Purple
Astatine - black

Inorganic and Organic Chemistry (Lab) (2 decks)

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