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Thanatochemistry > Oxygen, Hydrogen and Water > Flashcards

Oxygen, Hydrogen and Water Flashcards

1
Q

Means acid former and is the most abundant element on earth.

- combined with certain inorganic elements, acid is formed.

A

Oxygen

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2
Q

Exists as a diatomic molecule O2.

- it has 6 valance electrons and needs 2 to complete the octet rule so it creates a double covalent bond to be stable.

A

Elemental oxygen

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3
Q

This is a single oxygen atom, and is rare. This is when oxygen is not combined with something else.

A

Nascent oxygen

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4
Q

Three oxygen atoms joined by electrification of air (lightning).

A

Ozone (O3)

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5
Q
  • Gas at room temperature
  • Denser than air
  • Colorless
  • Odorless
  • Slightly soluble in liquids.
A

Physical properties of oxygen

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6
Q
  • Reacts slowly at RT
  • Supports combustion
  • Forms oxides (any compound that contains oxygen)
  • Acts as an oxidizing agent
  • Oxides complete a chemical reaction known as oxidation.
A

Chemical properties of oxygen

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7
Q

Oxidation at a slow pace, usually at a low temperature.

- i.e.- rusting

A

Slow oxidation

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8
Q

Oxidation at a rapid pace, usually at a high temperature.

i.e.- burning wood

A

Rapid oxidation

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9
Q

The temperature at which a substance will burst into flames.

A

Kindling point

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10
Q

Slow oxidation of organic matter caused by aerobic bacteria.

A

Decay

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11
Q

Slow oxidation of organic matter caused by anaerobic bacteria.

A

Putrefaction

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12
Q
  • Add oxygen to a substance (most common form)
  • Remove hydrogen from a substance.
  • Remove electrons from a substance
  • Increase the oxidation number of a substance.
A

Oxidation reaction

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13
Q

Means “water former” and is the smallest and lightest element on earth.

  • the most abundant element in the universe.
  • Does not contain a neutron in its nucleus.
A

Hydrogen

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14
Q

Exist as a diatomic molecule H2.

- It has 1 valance electron and needs 1 to complete the first shell (K) so it creates a covalent bond to be stable.

A

Elemental hydrogen

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15
Q

A single hydrogen atom not combined with someone else. This is rare.

A

Nascent hydrogen

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16
Q
  • Gas at RT
  • Colorless
  • Odorless
  • Tasteless
  • Lighter than O2
  • Highly diffusible
A

Physical properties of hydrogen

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17
Q
  • Burns with a hot blue flame (flammable)
  • Does not support combustion (not combustible)
  • Acts as a reducing agent.
A

Chemical properties of Hydrogen

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18
Q
  • The removal of oxygen from a substance
  • The addition of hydrogen to a substance
  • The addition of electrons to a substance
  • The decrease in oxidation number of a substance.
A

Reduction

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19
Q

Has a positive end and a negative end.

  • Each hydrogen atom has a partial positive charge.
  • Oxygen has a partial negative charge.
A

Polar molecule (water)

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20
Q

Molecules with partial charges are attracted to other molecules with partial charges.

  • Can form between any polar molecules
  • An individual of this bond is weaker than both covalent and ionic bonds. Multiple of this bond are very strong.
  • Responsible for many of water’s unique properties.
A

Hydrogen bonds

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21
Q
  • Ionic compounds dissociate into ions in water because they attract water molecules.
  • A solution with ions in it is capable of conducting electricity.
    • deionized water cannot
A

Ionic molecules in water

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22
Q
  • Universal solvent
  • Cohesion and adhesion
  • Resistant to temperature changes
  • Resistant to state changes
  • Density
A

Characteristics of water

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23
Q

Dissolves the solute.

A

Solvent

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24
Q

Substance being dissolved into a solvent.

A

Solute

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25
Q

The polar nature of water makes it this.

  • ionic compounds and polar molecules dissolve
  • Many kinds of polar molecules are dissolved into water to create biological fluids such as blood, sap and cytoplasm.
A

Universal solvent

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26
Q

Water loving. Will dissolve in water.

A

Hydrophilic

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27
Q

Will not dissolve in water.

  • Oils
  • Fats
  • Gasoline
A

Hydrophobic

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28
Q

Water is attracted to itself.

- Allows water to pull together and form droplets or form an interface between it and other surfaces. (surface tension)

A

Cohesion

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29
Q

Due to their polar nature, water molecules are attracted and will attach to other surfaces.
- This property of water helps move fluids through vessels in plants and animals (capillary action).

A

Adhesion

30
Q

The amount of heat that must be absorbed or lost for 1g of that substance to change its temperature by 1 degree C.

A

Specific heat capacity

31
Q
  • Water has a high specific heat capacity
  • Water will retain its temperature after absorbing large amounts of heat, and retain its temperature after losing equally large amounts of heat.
  • This property of water protects organisms in water from rapid temperature changes. It also helps organisms maintain their body temperature.
A

Water resists changes in temperature

32
Q
  • Even though hydrogen bonds are fairly weak it takes a lot of energy to break all of those bonds and evaporate water.
  • Contributes to evaporative cooling. Stabilizes the temperatures on the earth, in lakes and ponds, and the internal temperature of terrestrial organisms (sweating).
A

Water resists changes in state.

33
Q

The quantity of heat a liquid must absorb for 1g of it to be converted from the liquid to the gaseous state.

A

Heat of vaporization

34
Q

Water is unique because it is less dense as a solid than it is as a liquid.

  • as water cools hydrogen bonds tend to break less often.
  • As hydrogen bonds become more permanent the water molecules form a lattice.
  • Ice protects organisms below the surface.
  • Ice floats so bodies of water freeze from the top down.
  • When ice melts the colder water sinks, creating circulation of nutrients and organic material.
A

Density - property of water

35
Q
  • Element
  • Compound
  • Mixture
    This is a homogenous mixture of two or more substances (solutes) in a dissolving medium (solvent or vehicle).
A

Solution

36
Q

Substance being dissolved (usually less of this than the solvent).

A

Solute

37
Q

The substance being dissolved into (usually more of this than the solute).

A

Solvent/vehicle

38
Q

A solution where alcohol is the solvent.

A

Tincture

39
Q

A solution where water is the solvent.

A

Aqueous solution

40
Q

Solid solution made of two or more metallic elements.

A

Alloy

41
Q

The property that allows a solute to dissolve into the solvent.
- depends on temperature and pressure.

A

Solubility

42
Q

When the solvent can no longer dissolve anymore solute and contains all the solute it can hold.

A

Saturation

43
Q

Polar molecules will form solutions with:

A

Other polar molecules

44
Q

Non-polar molecules will form solutions with:

A

Other non-polar molecules

45
Q

Subjective description of the amount of solute a solvent can contain.

A

Qualitative

46
Q

Precise, and measured way of describing the amount of solute that a solvent can contain.

A

Quantitative

47
Q
  • Dilute
  • Concentrated
  • Saturated
  • Supersaturated
  • Unsaturated
A

Qualitative solution terms

48
Q

Contains “little” amounts of solute.

A

Dilute

49
Q

Contains “large” amounts of solute.

A

Concentrated

50
Q

Contains all of the solute a solvent is able to hold at a certain pressure and temperature.

A

Saturated

51
Q

Contains more solute than the solvent can normally hold- this is very difficult to achieve.

A

Supersaturated

52
Q

Any solution that has not reached saturation point.

A

Unsaturated

53
Q
  • Percentage
  • Ratio
  • Index
  • Molarity
A

Quantitative solution terms.

54
Q

Mass of volume.

A

Percentage

55
Q

Weight of solute to weight of solution.

- can be any measurement as long as it’s the same for both the solvent and solute.

A

Ratio

56
Q

Concentration of formaldehyde in embalming fluid. (grams of formaldehyde/100ml).

A

Index

57
Q

The formula weight (in grams) dissolved in 1 liter of solute.

A

Molarity

58
Q
  • True solutions may have properties that are different from those of individual solutes and solvents that make them up.
  • True solutions undergo diffusion.
A

Chemical properties of solutions

59
Q

A difference in concentration of a substance.

A

Concentration gradient

60
Q

The net movement of particles from a region of higher to lower concentration down a concentration gradient.
- all compounds undergo this.

A

Diffusion

61
Q

Particles are uniformly distributed.

- Diffusion ends here.

A

Equilibrium

62
Q

The diffusion of water across a membrane.

- important to cells since all cells have membranes.

A

Osmosis

63
Q

More concentrated with solute.

- the cell shrinks

A

Hypertonic

64
Q

Less concentrated with solute.

- the cell expands and can lyse (burst)

A

Hypotonic

65
Q

Equally concentrated.

- cells will not change shape.

A

Isotonic

66
Q

Embalming fluid must be this kind of osmotic pressure to flow out of the circulatory system into the tissue.

A

Hypotonic

67
Q

If embalming fluid is this, fluid in the tissue will move into the circulatory system.

A

Hypertonic

68
Q

If embalming fluid is this, there will be very little movement of the fluid into the tissues.

A

Isotonic

69
Q

Particles are extremely tiny and can not be separated out by physical means.

A

True solution

70
Q

Contains particles that can pass through filters, but not through membranes.

  • Exhibit brownian movement
  • Milk, blood plasma
A

Collodial solution

71
Q

The particle size is larger and the particles can not pass through membranes or filters.
- They will settle out if left long enough (river water).

A

Suspension

Thanatochemistry (12 decks)

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