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Chemistry 111 > Chapter 1 > Flashcards

Chapter 1 Flashcards

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1
Q

What is chemistry?

A

Chemistry is the study of matter and the changes it undergoes.

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2
Q

What is matter?

A

Anything that has a mass and occupies space.

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3
Q

Define macroscopic. Give an example.

A

Anything large enough to be seen with the naked eye.

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4
Q

Define submicroscopic. Give an example.

A

Anything too small to be seen even with a microscope.

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5
Q

Define scientific method.

A

Scientific method is a set of guidelines that scientists must follow when doing experiments.

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6
Q

What is a law?

A

A law is a concise verbal or mathematical statement of a reliable relationship of phenomena.

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7
Q

Define a hypothesis.

A

A hypothesis is a tentative explanation of scientists observations.

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8
Q

What is a theory?

A

A theory is a unifying principle that explains a body of experimental observations and the laws that are based on them.

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9
Q

What are the steps in the scientific method?

A

Observations. Hypothesis. Experiment. Theory. Conclusion or further experiment. CEPHO.

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10
Q

What are the essential elements of the scientific method?

A

Essential elements of the scientific method are astute observations, inductive reasoning, and careful experimentation.

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11
Q

Define quantitative properties

A

Quantitative properties are measured and expressed using numbers.

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12
Q

What are the Base SI Units, their base quantity, name of unit, and symbol?

A
  1. Length (meter, m)
  2. Mass (Kilogram, kg)
  3. Time (Second, s)
  4. Electric current (ampere, A)
  5. Temperature (Kelvin, K)
  6. Amount of substance (mole, mol)
  7. Luminous intensity (candela, cd)
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13
Q

What are the prefixes used with SI Units?

A 
Tera - T - 1 x 10^12
Giga - G - 1 x 10^9
Mega - M - 1 x 10^6
Kilo - K - 1 x 10^3
Deci - d - 1 x 10^-1
Centi - c - 1 x 10^-2
Mili - m - 1 x 10^-3
Micro - u - 1 x 10^-6
Nano - n - 1 x 10^-9
Pico - p - 1 x 10^-12
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14
Q

What is mass?

A

Mass is the measure of the amount of matter in an object.

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15
Q

Define weight.

A

Weight is the force exerted by an object or sample due to gravity.

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16
Q

What is AMU?

A

AMU is Atomic Mass Unit, used to express the masses of atoms - and other objects of similar size.

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17
Q

What is angstrom?

A

Angstrom is a measure of length that is equal to 1 x 10^10m.

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18
Q

What is a burette?

A

A burette is used to measure the volume of a liquid that has been added to a container.

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19
Q

What is a volumetric pipette used for?

A

A volumetric pipette is used to deliver a precise amount of liquid. 5 ml for example.

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20
Q

What is a graduated cylinder?

A

A graduated cylinder is used to measure a volume of a liquid.

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21
Q

What is a volumetric flask?

A

A volumetric flask is used to prepare a precise volume of a solution for the use in a laboratory.

22
Q

What is the freezing point and boiling point of water on the Celsius scale?

A

Freezing: 0
Boiling: 100

23
Q

What is absolute zero?

A

Absolute zero is a theoretical temperature where the kinetic energy of particles is 0. In other words, particles in a substance do not move.

24
Q

What is absolute zero on the Kelvin scale?

A

0 K

25
Q

What is the equation used to convert Kelvin to Celsius?

A

K = C° + 273.15

26
Q

What is the freezing point of water on the farenheit scale?

A

Freezes: 32°F
Boils: 212°F

27
Q

What equation is used to convert °F to °C?

A

(9/5) x (temperature in C°) + 32°F

28
Q

What is density?

A

Density is the ratio of mass to volume.

29
Q

What are exact numbers?

A

Exact numbers include numbers with defined values such as 2.54 in the definition 1 inch (in) = 2.54 cm. Exact numbers also include those that are obtained by counting.

30
Q

What are inexact numbers?

A

Numbers measured by any method other than counting are inexact. Measured numbers are inexact because of the measuring devices that are used,
the individuals who use them, or both. For example, a ruler that is poorly calibrated
will result in measurements that are in error—no matter how carefully it is used.

31
Q

What are significant figures?

A

Significant figures are the meaningful digits in a reported number.

32
Q

What are the significant figures guidlines?

How many sig figs are in

  1. 0.00005
  2. 10
  3. 10.0
  4. 5.0023
  5. -102
  6. 35,529.98
A
  1. Any digit that is not a zero is significant (112.1 has 4 sig figs)
  2. Zeros located between nonzero digits are significant (305 has 3 significant figures, and 50.08 has 4 significant figures.)
  3. Zeros to the left of the first nonzero digit are not significant. (0.0023 has two
    significant figures, and 0.000001 has one significant figure).
  4. Zero s to the right of the last nonzero digit are significant if the number contains
    a decimal point (1.200 has four significant figures).
  5. Zeros to the right of the the last nonzero number that does not contain a decimal point are significant.
  6. 1
  7. 1
  8. 3
  9. 5
  10. 3
  11. 7
33
Q

Define precision.

A

Precision tells us how close a series of replicate measurements are to one another.

34
Q

What is accuracy?

A

Accuracy tells us how close a measurement is to the true value.

35
Q

What is conversion factor.

A

Conversion factor is a fraction in which the same quantity is expressed one way in the numerator and another way in the denominator. By definition, for example, 1 in = 2.54 cm.

36
Q

What is dimensional analysis or - the factor label method?

A

The use of conversion factors in problem solving is called dimensional analysis or the factor-label method.

37
Q

What is a substance?

A

A substance is a form of matter that has a specific chemical composition and distinct, observable properties such as color, state of matter (solid, liquid, or gas) and solubility (does it dissolve in water or not?). Chemists classify all matter either as pure substance or as a mixture of substances.

salt (sodium chloride): white, crystalline solid; dissolves in water

∙ iron: greyish metal; rusts when left exposed to air and water; does not dissolve in water

∙ mercury: silvery liquid; does not dissolve in water

∙ carbon dioxide: colorless gas; does not support combustion (can be used to extinguish flames)

∙ oxygen: colorless gas; supports combustion (will accelerate a fire)

38
Q

What is a mixture? Give examples.

A

A mixture is a combination of two or more substances in which each substance retains its distinct identity.

Like pure substances, mixtures can be solids, liquids, or gases. Some familiar examples are trail mix, sterling silver, apple juice, seawater, and air.

39
Q

What is a homogeneous mixture?

A

A homogeneous mixture consists of parts that are the same; uniform in structure or composition. The mixture we get when we dissolve sodium chloride in water is a homogeneous mixture because the composition of the mixture is uniform throughout.

40
Q

What is a heterogeneous mixture?

A

A heterogeneous mixture is when the composition is not uniform.

41
Q

What is condensing?

A

Condensing is water that evaporates.

42
Q

What is a physical process?

A

A physical process is one that does not change the identity of any substance. For example, melting ice causes a change in the physical state of water (solid to liquid), but it does not change the identity of the substance (water).

43
Q

What is qualitative property?

A

A qualitative property is a substance that does not require explicit measurements and is described without the use of numbers. Ex: color.

44
Q

What is a physical property? Give examples.

A

A physical property is one that can be observed and measured without changing the identity of a substance.

Examples of physical properties: color, melting / boiling point, phase of the substance.

45
Q

What is a physical change?

A

A physical change is one in which the state of matter changes, but the identity of the matter does not change.

46
Q

Define chemical property.

A

a property used to characterize materials in reactions that change their identity.

47
Q

Define chemical process.

A

A chemical process is when a chemical property of a substance must change in order for us to observe that property.The statement “iron rusts when it is exposed to water and air” describes a chemical property of iron, because for us to observe this property, a chemical change or chemical process must occur. In this case, the chemical change is corrosion or oxidation of iron. After a chemical change, the original substance (iron metal, in this case) no longer exists. What remains is a different substance (rust, in this case). There is no physical process by which we can recover the iron from the rust.

48
Q

What is an extensive property?

A

An extensive property is dependent on the amount of matter.Values of the same extensive property can be added together. For example, two copper coins will have a combined mass that is the sum of the individual masses of each coin, and the volume occupied by two copper coins is the sum of their individual volumes. Both mass and volume are extensive properties.

49
Q

What is an intensive property?

A

An intensive property is independent of the amount of matter.Consider again the example of copper coins. The density of copper is the same regardless of how much copper we have; and the same is true regarding the melting point of copper. Density and melting point are intensive properties. Unlike mass and volume,
which are additive, density, melting point, and other intensive properties are not additive.

50
Q

What are the values with prefixes of SI units?

A 
Tera - T - 1 x 10^12
Giga - G - 1 x 10^9
Mega - M - 1 x 10^6
Kilo - K - 1 x 10^3
Deci - d - 1 x 10^-1
Centi - c - 1 x 10^-2
Mili - m - 1 x 10^-3
Micro - u - 1 x 10^-6
Nano - n - 1 x 10^-9
Pico - p - 1 x 10^-12

Chemistry 111 (2 decks)

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