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Inorganic Chemistry > Measurements > Flashcards

Measurements Flashcards

Week 2

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1
Q

tool of science

A

Math

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2
Q

We measure mass quantity of
matter

A

Measurement

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3
Q

invariable and independent

A

Mass (kg,g)

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4
Q
  • Varies relation to distance
  • Depend on the gravitational force
  • The lower the gravitational force, the lower the weight and vice versa
A

Weight

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5
Q
  • Space occupied by substance or object
  • Bigger space = bigger volume
A

Volume (liter, mL)

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6
Q
  • Distance covered of the certain object
  • How long or short the object is
A

Length

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7
Q

Volume, mass degrees Fahrenheit, Celsius (American system), or kelvin (absolute temperature). Amount of kinetic energy present in a substance.

A

Temperature

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8
Q

High Temp (hot)

A

Large K.E

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9
Q

Low Temp (cold)

A

Low K.E

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10
Q

Water Boils at

A

100 degrees celsius, 112 degrees Fahrenheit, 373 Kelvin

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11
Q
  • Derived dimension and derived units.
  • lightness /heaviness of a substance
  • Dense or not dense
  • Depends on mass per given volume
A

Density (g/mL)

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12
Q

The ratio of density of the substance being referred to and density of water.

A

Specific Gravity

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13
Q
  • Close to each other
  • e.g. 76,77,76
A

Precise

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14
Q

Close agreement in true value

A

Accurate

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15
Q

(Internet, books)

A

True values

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16
Q

Measurement can be

A

Metric System (Philippines)

17
Q

Metric System

A

Kilogram (mass)

18
Q
  • Rounded off
  • Reliability in terms of large numbers
  • More accurate = more significant
A

Significant Figures

19
Q
  • useful for very large and very small numbers, especially in non-SI units.
  • Diamond is a pure carbon
    Arrangement of carbon
A

Scientific Notation

20
Q

empirical science

A

Chemistry

21
Q

Chemistry is studied by

A
  • Measuring physical properties and observing chemical reactions. (Boiling point, formation of bubbles? change in color so there is a reaction)
  • Supported by facts and evidences
22
Q

are created to explain observations and organize collected data.

A

Models

23
Q

recorded via measurements. (Recorded the
temperature)

A

Observation in Science

24
Q

included in observation

A

UNIT OF MEASUREMENTS

25
Q
  • how close the observed value is to the “true” value.
A

Accuracy

26
Q
  • the spread in values obtained from measurements; the reproducibility of values.
  • Trial 4 close to the trial 1,2,,3
  • As long as magkalapit ‘yong values REGARDLESS if tama
  • how close a set of measurements
    are to each other
A

Precision

27
Q
  • may make a measurement randomly too high or too low. (e.g., variation associated with equipment limitations)
  • There can be random errors like there is a problem in equipment.
  • Maling calibration = maling results
A

Random Error

28
Q
  • may make a measurement consistently too high or too low. (e.g., the presence of an impurity)
  • More on the procedures
  • Contamination = impurity
A

Systematic Error

29
Q

fps system (foot – pound – second)

A

English System or British System

30
Q

cgs system (centimeter-gram – second) mks system (meter – kilogram – second) - SI (Systeme Internationale)

A

Metric System

31
Q

Chemists quantify data

A

expressing collected data with units and significant figures.

32
Q
  • designate the type of quantity measured.
  • Units of mass are pound, grams, kilogram
  • Lengths are meters, millimeters
A

Units

33
Q
  • provide scale to a base unit.
  • Centi - 100
  • Milli - 1000
A

Prefixes

34
Q
  • The base unit designates the type of quantity being measured.
  • meter
A

Base Units

35
Q

cm, dm

A

smallest Scale

36
Q

km

A

Bigger Scale

37
Q

indicate the amount of information that is reliable when discussing a measurement.

A

Significant Figure

38
Q

are the base units of science.

A

SI units (from French Système International)

39
Q

Some units comprise combinations of these base units

A

derived units

Inorganic Chemistry (7 decks)

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