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Chemistry chapter 10-13 > Chem final > Flashcards

Chem final Flashcards

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1
Q

1-2 letter abbreviations for elements

A

Most are straightforward (O = oxygen, Si = Silicon, etc)

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2
Q

Elements based on Latin or Greek names

A

-Pb = Lead
-Hg = Mercury
-Cu = Copper
-Fe = Iron
=K = Potassium
-Sb = Antimony
-Ag = Silver
Au = Gold

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3
Q

All matter: Mixtures

A
  • If the matter can be separated by a physical process then it is a mixture.
  • If the matter can not be separated by a physical process it is not a mixture
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4
Q

All matter: Compounds or elemnets

A
  • If the matter is not separated by a physical process it turns into a pure substance.
  • If the substance can be broken down into simpler ones by chemical means, then it is a compound.
  • If it can not be broken down into simpler ones by chemical means then it is an element
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5
Q

Classification of matter

A
  • The four components of matter are solids, liquids, gases, and plasmas
  • Matter can be divided into pure substances and mixtures.
  • Pure substances may be elements (containing atoms of the same type–for instance, silicon (Si) or compounds (containing 2 or more different types of atoms–for example, silicon dioxide (SiO2)
  • Mixtures may be heterogeneous (with a composition that caries throughout, such as gravel) or homogeneous (with a unifrm composition throughout, such as solutions of sugar dissolved in water)
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6
Q

Molecule

A
  • A space-filling model for a water molecule is H2). There’s two hydrogen atoms, and one oxygen atom.
  • A molecule is a fixed number of atoms held together by chemical bonds in certain spatial arrangement .
  • The chemical formula symbolically represents the type and number of each element present
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7
Q

Classifying matter: Compounds

A
  • Carbon dioxide
  • Cocaine.
  • Water
  • Table salt
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8
Q

Classifying matter: Element

A
  • Nickel.

- Fluorine

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9
Q

Classifying matter: Mixture

A
  • Soap.

- Sea water

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10
Q

Atoms: Compounds

A
  • Ionic compounds are composed of oppositely charged ions. Electrons are either added or subtracted from atoms to form ions.
  • Molecular compounds are composed of molecules, which ate made up of atoms.
  • The four states of matter, elements, compounds, and mixtures are on the macroscopic scale (can view with the naked eye), individual molecules, ions, and atoms are on the sub-microscopic or nanoscale (one-billionth of a meter)
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11
Q

Example: Different compounds containing the same element will have different physical and chemical properties

A
  • Fe: Magnetic

- Fe2O3: Non magnetic

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12
Q

Properties of subatomic particles: Prton

A
  • Relative charge: +1
  • Relative mass: 1
  • Actual mas, kg: 1.67 x 10^-27
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13
Q

Properties of subatomic particles: Neutron

A

-Relative charge: 0
-Relative mass: 1
Actual mass, kg: 1.67 x 10^-27

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14
Q

Properties of subatomic particles: Electron

A
  • Relative charge: -1
  • Relative mass: 0**
  • Actual mass, kg: 9.11 x 10^-31
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15
Q

**0

A

This value is zero when rounded to the nearest whole number. it does have a mass, though it’ve very small

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16
Q

Properties of subatomic particle

A
  • Most of the mass in an atom is found in the nucleus.
  • Protons and neutrons are found in the nucleus.
  • Electrons are located outside the nucleus
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17
Q

Atomic number (Z)

A

the number of protons (nuclear charge)

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18
Q

Mass number (A)

A

The sum of the protons and neutrons

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19
Q

Electrical conductivity

A
  • Metals are electrically and thermally conductive.

- Electrical conductivity involves the movment of electrons through the 3-D structure of a conductor

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20
Q

Cu

A
  • Atomic number = 29
  • Therefore ti contains 29 protons (29+ charge).
  • To balance the charge, it contains 29 lectrons (29 - charge).
  • Mass number = number of protons + number of neutrons (0 charge)
  • Number of neutrons = 63 -29 = 34
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21
Q

Allotrope

A

Is two or more forms of the same element that differ in their chemical structure and therefore their properties

22
Q

Atomic composition of the earth’s crust

A
  • Al: 8%
  • Si: 28%
  • O: 47%
  • Fe: 5%
  • Group 1-2: 11%
  • Other: 1%
23
Q

Non-zero digits are significant

A

For instance, 1.55 g = 3 significant figures

24
Q

All zeroes embedded between non-zero digits are significant

A

For instance, 1.003 mL = 4 significant figures

25
Q

Trailing zeroes are significant

A

For instance, 1.000 g = 4 significant figures

26
Q

Leading zeroes are not significant

A

For instance, 0.00305 mL = 3 significant figures

27
Q

Addition/subtraction

A
  • Answer is based on the smallest decimal places.

- For instance, 1.003 + 0.2 + 0.001 g = 1.2 g

28
Q

Multiplication/division

A
  • Answer based on the smallest number of significant figures.
  • For instance, 1.002 cm times 0.005 cm = 0.05 cm = 0.005 cm^2
29
Q

Scientific notation

A 
11000 = 1.1 x 10^4
0.00021 = 2.1 x 10^-4
0.001021 = 1.021 x 10^-3
1730 = 1.73 x 10^3
**The same number of significant figures on both sides of each example
30
Q

Scientific notation: Moving decimals

A

Very small numbers move the decimal to the right, large numbers move the decimal to the left

31
Q

Moving decimals

A 
0.00000012 = 1.2 x 10^-7
2300000000 = 2.3 x 10^9
32
Q

12N silicon (Si)

A
  • 99.9999999999
  • An analogy for the 12N purity of silicon: Stack 170 yellow tennis balls from Earth to the moon, replace 1 yellow tennis ball with a red one, this reflects how few impurities are present in this ultra-high purity silicon
33
Q

From silicon to computer chip

A
  • Ultra-high purity silicon (5N, 7N, or 12N purity)
  • At high temperatures, silicon is fabricated into cylinders (ingots) and sliced into wafers
  • Hundreds of processing steps are used to fabricate a computer chip on the surface of silicon wafers
  • Chips are removed from the wafer and tested
  • The chips that are tested satisfactorily are sealed and packaged
34
Q

Chip testing

A

Technicians work inside “clean rooms” and wear “bunny suits’ to prevent contamination by dust particles

35
Q

Size comparison

A
  • To relate how small the components of chips are, the scale bars in the bottom electron microscope images are comparable to:
    a. Diameter of a coud water droplet
    b. Diameter of mold spores
    c. Diameter of a human hair fiber
    d. Diameter of beach sand
    e. Thickness of a human cornea
    f. Diameter of a pinhead
    g. Diameter of a pupil
36
Q

Transistors

A

Computer chips contain billions of tiny components of these and are sued to perform the calculations needed by our coputers and portable electronic devices

37
Q

Prince Rupert of the Rhine, Duke of Cumberland, KG, PC, FRS (17 December 1619- 29 November 1682)

A

German army officer, admiral, scientist and colonial governor.
-He firs came to promience as a Cavalier cavalry commander during the English Civil War

38
Q

Sustainability: Three pillars

A
  • Environmental: Pollution prevention, natural resource use
  • Social: Better quality of life for all members of society
  • Economic: Fair distribution and efficient allocation of resources
39
Q

The composition of air

A

It’s a mixture: A physical combination of two or more substances present in variable amounts

40
Q

What’s in a breath

A

In addition to nitrogen, oxygen, and other colorless gases, there are harmful nitrogen oxides and particulate matter that contribute to air pollution

41
Q

Air inversions

A
  • Cooler air can be trapped beneath warmer air due to weather conditions
  • Pollutants often accumulate in the cooler air of an inversion layer.
  • This situation is worsened when air flow is limited, such as in cities surrounded by mountains
42
Q

Visualizing the molecules in air

A
  • A molecule is a fixed number of atoms held together by chemical bonds in a certain spatial arrangement.
  • The chemical formula symbolically represents the type and number of each element present.
  • Chemists use three viewpoints to study and understand matter, macroscopic, symbolic, and particulate
43
Q

Molecular structures

A

The particulate view of matter shows the 3-D molecular structure, with atoms color-coded

44
Q

Naming binary compounds of nonmetals

A
  • Prefixes are used to designate the number of each type of element:
  • N2O = dinitrogen monoxide (also known as nitrous oxide, or laughing gas)
  • P2O5 = diphosphrous pentoxide
45
Q

Risk assessment

A

Evaluating scientific data and making predictions in an organized manner about the probabilitie of an occurrence

  • Toxicity: Intrinsic health hazard of a substance
  • Exposure: The amount of the substance encountered
46
Q

Parts per hundred (percent)

A

Atmosphere is 21% oxygen = 21 oxygen molecules per 100 molecules and atoms in air

47
Q

Parts per million (ppm)

A

0.4 ozone molecules/1 x 10^6 molecules and atoms in air

48
Q

Parts per billion (ppb)

A

30 sulfur dioxide molecules/ 1 x 10^9 molecules and atoms in air

49
Q

21 % means 21 parts per hundred…

A
  • Means 210 parts per thousand.
  • Means 2,100 parts per ten thousand.
  • Means 21,000 parts per hundred thousand.
  • Means 210,000 parts per million
50
Q

These gases represent the most harmful for our health and the health of our planet

A
  • Carbon monoxide.
  • Ozone.
  • Sulfure dioxide (SO2) and nitrogen dioxide (NO2)
  • Particlate matter (PM)
51
Q

Air quality monitoring and reproting

A

The average concentration of air pollutants in the Unoted States have decreased dramatically since 2000

52
Q

The number of unhealthy days per year

A

Although air quality has improved in recent years, on average, people in some metropolitan areas breathe air containing unhealthy levels of pollutants

Chemistry chapter 10-13 (2 decks)

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