Quarter 2 Final Exam Study Guide Flashcards
Facts about Oxygen
- Nonmetal
- Most abundant element on Earth
- 21% of the volume of atmospheric air
- 89% of the mass of water
- Formula: O2 Symbol: O
Oxygen on the Periodic Table
- VIA Element
- 6 valence electrons
- Oxygen means “acid former”
- When combined with some inorganic elements, acids form
Oxygen’s Physical Properties
- Colorless, odorless. & tasteless
- Heavier than air
- Slightly soluble in water
- Can be liquified & solidified by extreme pressure & low temperature
Oxygen’s Chemical Properties
- Reacts with many substances slowly at ordinary temperatures but rapidly at high temperatures
- Reacts with many metallic & nonmetallic elements to form oxides
- Supports combustion/helps things burn
Ways to define Oxidation
- the addition of oxygen to a substance
- the removal of hydrogen from a substance
- the removal of electrons from a substance
- the increase in oxidation number of a substance
Allotropic
When an element exists in two or more different forms, each with its own physical & chemical properties
O,O2,O3
Hard Water
Water that contains minerals in solution that destroy the cleansing action of soap
Calcium, magnesium, and sometimes iron
True Solutions
- Homogeneous mix of two or more substances
- elements or compounds
- gases, liquids or solids
- boils in higher temps; freezes at lower temps
Solid Solutions
- Alloys
- Solids are dispersed throughout each other
- Brass, bronze, stainless steel, sterling silver etc
Solute vs Solvant
Solute: The substance being dissolved
Solvant: The substance that does the dissolving
Solubility
Measure of solute dissolved in a solvent
The measure of how much of a solute can be dissolved in a solvent
Saturated vs Unsaturated
Super Saturated: Too much solute than solvent can hold
Saturated: more solute than solvent can hold
Unsaturated: less solute than solvent can hold
What factors influence Solubility?
Temperature: Solubility of gases in liquids is decreased as temps rise
Pressure: Solubility of gas rises as pressure rises
Dilute Solution vs Concentrated
Dilute: Contains a relatively small amount of solute
Concentrated: contains large amount of solute
Percent by Mass
Mass of solute/total weight of solution X 100
Percent by Volume
Volume of solute/total volume of solution X 100
Index
Concentration of formaldehyde in embalming fluid
Index=HCHO g/100 ml of solution
Osmotic Principles to Embalming
Hypotonic: use on Normal/Dehydrated cases
Hypertonic: use on Edema cases
Isotonic: leaves bodies unembalmed
Properties of Acids
- Acids in solution taste sour
- Sting the skin
- Neutralization Reaction: React with bases to form water & salt
Salts
- Composed of ions of metallic elements or the positive ammonium ion in combination with one or more ions of a nonmetallic element
- Are Ionic substances (have a charge)
Electrolytes
- Salts that dissolve in water and dissociate into positive and negative ions
- The presence of ions in a solutions enables it to conduct electricity
Electrolysis
The passage of an electric current through a solution
can be acids, bases, or salts
- Solutions that allow electrolysis are electrolytes
pH Hydrogen Ion Concentration
- Measure of Hydrogen Ion Concentration
- A neutral solution would have the same concentration of hydrogen ion and hydroxide ion concentration
- pH 7 is neutral
- Less than 7 is acidic
- More than 7 is basic/alkaline
Weak electrolytes
weak conductors of electricity
Strong electrolytes
good conductors of electricity
pH of blood
7.3-7.5
pH of Human Gastric Juice
1.0-3.0
pH of Pure Water
7.0
pH of Embalming Fluid
6.5-9.0
Buffers
Protective mechanism in the blood that protect against changes in pH
Number of Ionizable Hydrogens
- Monoprotic Acids
- Polyprotic Acids: Diprotic & Tripotic
- how many hydrogens will it give up?
- they donate x amount of protons or hydrogen atoms per molecule to an aqueous solution
Number of Elements
- Binary Acids: hydrogen & 1 other element
- Ternary Acids: Oxygen, hydrogen & a nonmetallic element
Arrhenius Theory on Acids
Acids are substances that dissociate(break apart) in an aqueous solution to yield hydrogen ions
Arrhenius Theory on Bases
Bases disassociate to create hydroxide ions
Bases are substances that dissociate in an aqueous solution to yield hydroxide ions
Hydrochloric Acid
HCl
Binary
Strong Acid
Monoprotic
Nitric Acid
HNO3
Ternary
Strong Acid
Monoprotic
Sulfuric Acid
H2SO4
Ternary
Strong Acid
Diprotic
Phosphoric Acid
H3PO4
Ternary
Moderate Acid
Triprotic
Carbonic Acid
H2CO3
Ternary
Weak Acid
Diprotic
Acetic Acid
HC2H3O2
Ternary
Weak Acid
Monoprotic
Strong Acid
Molecules that completely dissociate into their ions when it’s in water
Weak Acid
Molecules that partially dissociate into their ions when it’s in water
Sodium Hydroxide
NaOH
Lye
Potassium Hydroxide
KOH
Calcium Hydroxide
Ca(OH)2
Magnesium Hydroxide
Mg(OH)2
Bases
Taste Bitter
Feel Slippery
Bases react with acids to form salts and water (neutralization reaction)
Usually have a hydroxide group - OH
Ammonia
NH3
Weak Base
Polar Molecule
Polar molecules are those that possess regions of positive and negative charge
Nonpolar Molecule
Bonding electrons shared equally between two atoms
Concentration
The amount of a particular solute in a given volume of solution
Vehicle
A carrier or inert medium used as a solvent (or diluent)
Ratio
the relationship in quantity, amount, or size between two or more things : proportion
Molarity
the amount of a substance in a certain volume of solution.
Molarity is defined as the moles of a solute per liters of a solution
Parts Per Million
ppm
A weight to weight ratio used to describe concentrations.
Parts per million (ppm) is the number of units of mass of a contaminant per million units of total mass.
Parts Per Billion
ppb
Tincture
a medicine made by dissolving a drug in alcohol.
Aqueous Solution
water that contains one or more dissolved substance
Hydrolysis
the destruction/reaction of an organic chemical with water to form two or more new substances
Ionization
the process when ions are formed by gain or loss of an electron from an atom or molecule
Nonelectrolytes
A compound that does not conduct an electric current in either aqueous solution or in the molten state.
Facts about Hydrogen
- Most abundant element in the universe
- found in both organic and inorganic compounds
- Tissue gas is largely free hydrogen
- Atmospheric Hydrogen: H2 (diatomic molecule)
- Atomic Number 1
- 1 Valence Electron
Physical Properties of Hydrogen
Colorless, odorless, tasteless gas
Lighter than air
Slightly soluble in water
Chemical Properties of Hydrogen
- Burns with hot, blue flame forming water
- Doesn’t support combustion
- means “water producer”
Ways to Define Reduction
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
Facts about water
- most abundant compound on earth
- Covering about 75% of the earths surface
- Present in air as water vapor
- Found in all plant and animal tissue
- Human body consist of about 50 to 60% water
- bacterial cells contain about 85% water
Water on the periodic table (facts about water)
- H2O
- Bent molecule; 105°
- atomic mass of 18
Physical properties of water
- Colorless odorless tasteless liquid
- Freezes at 0°C
- boils at 100°C
- Very good solvent for many substances
- heat of a vaporization: 450 cal per gram
Hydrogen bonding
Attractive force that exists among molecules
Water molecules are polar, which means there is a positive and negative pole
The positive side is attracted to the negative end of another pole
Properties of electronegativity apply
Surface tension
A force that causes the surface of a liquid to contract
Caused by hydrogen bonding
Water has high surface tension
Why is surface tension important to embalmers?
Surface tension is important because it occurs between arterial solutions and cell membranes
- Interferes with the diffusion of embalming chemicals from the capillaries into the tissues
- To overcome this problem, use surface tension reducing agents in embalming fluids
Chemical properties of water
- Very stable substance
- Thermally stable
Chemically reacts with active metals to liberate hydrogen - Reacts with metallic oxides to form bases
- Reacts with non-metallic oxide to form acids
- Forms hydrates
- Enters into hydrolysis reactions
- Key factor in decomposition
