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
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
3
Q
This is a single oxygen atom, and is rare. This is when oxygen is not combined with something else.
A
Nascent oxygen
4
Q
Three oxygen atoms joined by electrification of air (lightning).
A
Ozone (O3)
5
Q
- Gas at room temperature
- Denser than air
- Colorless
- Odorless
- Slightly soluble in liquids.
A
Physical properties of oxygen
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
7
Q
Oxidation at a slow pace, usually at a low temperature.
- i.e.- rusting
A
Slow oxidation
8
Q
Oxidation at a rapid pace, usually at a high temperature.
i.e.- burning wood
A
Rapid oxidation
9
Q
The temperature at which a substance will burst into flames.
A
Kindling point
10
Q
Slow oxidation of organic matter caused by aerobic bacteria.
A
Decay
11
Q
Slow oxidation of organic matter caused by anaerobic bacteria.
A
Putrefaction
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
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
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
15
Q
A single hydrogen atom not combined with someone else. This is rare.
A
Nascent hydrogen
16
Q
- Gas at RT
- Colorless
- Odorless
- Tasteless
- Lighter than O2
- Highly diffusible
A
Physical properties of hydrogen
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
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
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)
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
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
22
Q
- Universal solvent
- Cohesion and adhesion
- Resistant to temperature changes
- Resistant to state changes
- Density
A
Characteristics of water
23
Q
Dissolves the solute.
A
Solvent
24
Q
Substance being dissolved into a solvent.
A
Solute
25
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.
Universal solvent
26
Water loving. Will dissolve in water.
Hydrophilic
27
Will not dissolve in water.
- Oils
- Fats
- Gasoline
Hydrophobic
28
Water is attracted to itself.
| - Allows water to pull together and form droplets or form an interface between it and other surfaces. (surface tension)
Cohesion
29
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).
Adhesion
30
The amount of heat that must be absorbed or lost for 1g of that substance to change its temperature by 1 degree C.
Specific heat capacity
31
- 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.
Water resists changes in temperature
32
- 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).
Water resists changes in state.
33
The quantity of heat a liquid must absorb for 1g of it to be converted from the liquid to the gaseous state.
Heat of vaporization
34
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.
Density - property of water
35
- Element
- Compound
- Mixture
This is a homogenous mixture of two or more substances (solutes) in a dissolving medium (solvent or vehicle).
Solution
36
Substance being dissolved (usually less of this than the solvent).
Solute
37
The substance being dissolved into (usually more of this than the solute).
Solvent/vehicle
38
A solution where alcohol is the solvent.
Tincture
39
A solution where water is the solvent.
Aqueous solution
40
Solid solution made of two or more metallic elements.
Alloy
41
The property that allows a solute to dissolve into the solvent.
- depends on temperature and pressure.
Solubility
42
When the solvent can no longer dissolve anymore solute and contains all the solute it can hold.
Saturation
43
Polar molecules will form solutions with:
Other polar molecules
44
Non-polar molecules will form solutions with:
Other non-polar molecules
45
Subjective description of the amount of solute a solvent can contain.
Qualitative
46
Precise, and measured way of describing the amount of solute that a solvent can contain.
Quantitative
47
- Dilute
- Concentrated
- Saturated
- Supersaturated
- Unsaturated
Qualitative solution terms
48
Contains "little" amounts of solute.
Dilute
49
Contains "large" amounts of solute.
Concentrated
50
Contains all of the solute a solvent is able to hold at a certain pressure and temperature.
Saturated
51
Contains more solute than the solvent can normally hold- this is very difficult to achieve.
Supersaturated
52
Any solution that has not reached saturation point.
Unsaturated
53
- Percentage
- Ratio
- Index
- Molarity
Quantitative solution terms.
54
Mass of volume.
Percentage
55
Weight of solute to weight of solution.
| - can be any measurement as long as it's the same for both the solvent and solute.
Ratio
56
Concentration of formaldehyde in embalming fluid. (grams of formaldehyde/100ml).
Index
57
The formula weight (in grams) dissolved in 1 liter of solute.
Molarity
58
- True solutions may have properties that are different from those of individual solutes and solvents that make them up.
- True solutions undergo diffusion.
Chemical properties of solutions
59
A difference in concentration of a substance.
Concentration gradient
60
The net movement of particles from a region of higher to lower concentration down a concentration gradient.
- all compounds undergo this.
Diffusion
61
Particles are uniformly distributed.
| - Diffusion ends here.
Equilibrium
62
The diffusion of water across a membrane.
| - important to cells since all cells have membranes.
Osmosis
63
More concentrated with solute.
| - the cell shrinks
Hypertonic
64
Less concentrated with solute.
| - the cell expands and can lyse (burst)
Hypotonic
65
Equally concentrated.
| - cells will not change shape.
Isotonic
66
Embalming fluid must be this kind of osmotic pressure to flow out of the circulatory system into the tissue.
Hypotonic
67
If embalming fluid is this, fluid in the tissue will move into the circulatory system.
Hypertonic
68
If embalming fluid is this, there will be very little movement of the fluid into the tissues.
Isotonic
69
Particles are extremely tiny and can not be separated out by physical means.
True solution
70
Contains particles that can pass through filters, but not through membranes.
- Exhibit brownian movement
- Milk, blood plasma
Collodial solution
71
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).
Suspension
