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Chemistry Lab 1430 > Final Exam Terms > Flashcards

Final Exam Terms Flashcards

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1
Q

Uncertainty

A

used in a measurement to tell how well something is known…degree of potential error

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2
Q

Scientific Uncertainty

A

A range of possible values in which the actual value lies

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3
Q

What is the detection limit?

A

How to determine the uncertainty on different instruments

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4
Q

Examples of detection limits

A

graduation lines, table provided, last decimal place

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5
Q

Implicitly Reporting Uncertainty

A

Showing all values in the decimal place where the uncertainty lies

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6
Q

Explicitly Reporting Uncertainty

A

Showing all values in he decimal place where the uncertainty lies and stating the uncertainty

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7
Q

what is the max weight for a weighing vial?

A

120g

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8
Q

what does uncertainty indicate?

A

reliability of the device

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9
Q

Personal / Human Error

A

you made a mistake in the lab.

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10
Q

Random Error

A

caused by an unknown and unpredictable changes in a measuring instrument or in the environment

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11
Q

Percision

A

measure of the reproducibility of an experiment and quantifies random error

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12
Q

how to determine percision?

A

1/2 range, and STDEV

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13
Q

Systematic Error

A

occurs when there are flaws in the measuring device itself

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14
Q

What causes systematic error?

A

incorrect calibration, design flaw, incorrect method for problem

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15
Q

Accuracy

A

how close you come to the actual aimed for value

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16
Q

how to determine accuracy?

A

% Error

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17
Q

Mixture

A

when two or more substances that do not react chemically are united

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18
Q

how to separate a mixture?

A

physical means

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19
Q

Homogenous Mixture

A

also called solutions, appear uniform throughout

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20
Q

Heterogenous Mixture

A

ar enot uniform throughout

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21
Q

Physical Separation

A

using differences in physical properties of the compound of a mixture, such as solubility, boiling point, to separate.

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22
Q

Examples of Physical Separation?

A

Extraction, Evaporation, Sublimation, Decantation, Filtration.

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23
Q

Extraction

A

separation of a substance from a mixture by preferentially dissolving that substance in suitable solvent. By doing this, a soluble compound is usually separated from the insoluble compound.

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24
Q

Evaporation

A

involves heating a solution to remove the solvent.

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25
Q

What is left over in an evaporation?

A

residue. is the substance originally dissolved in the solvent

26
Q

Sublimation

A

process in which a solid passes directly to the gaseous state without going through the liquid state.

27
Q

Decantation

A

Separating a liquid from a solid “sediment” by gently pouring the liquid from the solid so as not to disturb the solid

28
Q

What is the liquid called in decantation?

A

Supernatant Liquid

29
Q

Filtration

A

separating solid from liquid by porous substance

30
Q

what is the liquid called in filtration?

A

filtrate

31
Q

Two types of filtration?

A

Gravity & Vacuum

32
Q

Chemical Separation

A

involves the selective reaction of one of the components of a mixture to form a new substance

33
Q

Chromatography

A

Process that permits the separation of a mixture into its components as a result of differences in rates in which the component travels through the column

34
Q

Mobile Phase

A

Gas, liquid

35
Q

Stationary Phase

A

film absorbed, paper, granular or porous solid

36
Q

Migration

A

based upon the repeated transfer of solute molecules back and forth between the two phases as solute is being swept down the column

37
Q

What technique did we use for gas chromatography?

A

Flame Ionization Detector (FID)

38
Q

Peak Area

A

directly proportionate to concentration

38
Q

Retention Time

A

time started to time it comes off. This is a characteristic of the specific component.

39
Q

Emperical Formula

A

shows the smallest whole number ratio in which the atoms combine to form a compound

40
Q

Molecular Formula

A

Gives the actual number of atoms in a molecule

41
Q

Law of Definite Proportions

A

The combining ratio of elements in a particular compound is constant regardless of the method of preparation

42
Q

Law of Multiple Proportions

A

When the same elements combine to form two different compounds, the two compounds will have different mass ratios.

43
Q

What is a dessicator?

A

a sealed container that keeps moisture out to protect and dry samples, chemicals, and other sensitive items:

44
Q

When to substances combine to form a compound

A

combination reactions

45
Q

When the compound breaks apart to form two or more products

A

decomposition

46
Q

when one element displace another element from a compound

A

single displacement

47
Q

Redox Reactions

A

when the oxidation states of one or more substances changes. Transfer of valence electrons.

48
Q

When do ion combination reactions form?

A

precipitate formation, gas formation, form a weak acid or non electrolyte

49
Q

Limiting Reagent

A

reagent that is used up first in a reaction

50
Q

Titration

A

a technique of accurately measuring the volume of a solution required to react with another reagent

51
Q

What does it mean for something to be standardized?

A

It went through the process of determining the exact concentration

52
Q

Auto-Catalytic Reaction

A

it produces its own catalyst

53
Q

what does a pale pink color mean in titration

A

reaction is complete.

54
Q

Enthalpy Change

A

the energy change of a reaction that occurs at standard conditions

55
Q

what values are enthalpy change for exothermic reactions?

A

less than zero

56
Q

what values are enthalpy change for endothermic reactions?

A

greater than zero

57
Q

calorimetery

A

the heat liberated during a reaction that causes a temperature change

58
Q

what is the calorimeter constant?

A

the heat absorbed from its surrondings, making it “imperfect”

59
Q
A

Chemistry Lab 1430 (2 decks)

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