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chemistry > Quarter 2 Final Exam Study Guide > Flashcards

Quarter 2 Final Exam Study Guide Flashcards

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1
Q

Facts about Oxygen

A
  • Nonmetal
  • Most abundant element on Earth
  • 21% of the volume of atmospheric air
  • 89% of the mass of water
  • Formula: O2 Symbol: O
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2
Q

Oxygen on the Periodic Table

A
  • VIA Element
  • 6 valence electrons
  • Oxygen means “acid former”
  • When combined with some inorganic elements, acids form
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3
Q

Oxygen’s Physical Properties

A
  • Colorless, odorless. & tasteless
  • Heavier than air
  • Slightly soluble in water
  • Can be liquified & solidified by extreme pressure & low temperature
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4
Q

Oxygen’s Chemical Properties

A
  • 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
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5
Q

Ways to define Oxidation

A
  • 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
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6
Q

Allotropic

A

When an element exists in two or more different forms, each with its own physical & chemical properties
O,O2,O3

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7
Q

Hard Water

A

Water that contains minerals in solution that destroy the cleansing action of soap
Calcium, magnesium, and sometimes iron

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8
Q

True Solutions

A
  • Homogeneous mix of two or more substances
  • elements or compounds
  • gases, liquids or solids
  • boils in higher temps; freezes at lower temps
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9
Q

Solid Solutions

A
  • Alloys
  • Solids are dispersed throughout each other
  • Brass, bronze, stainless steel, sterling silver etc
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10
Q

Solute vs Solvant

A

Solute: The substance being dissolved
Solvant: The substance that does the dissolving

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11
Q

Solubility

A

Measure of solute dissolved in a solvent

The measure of how much of a solute can be dissolved in a solvent

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12
Q

Saturated vs Unsaturated

A

Super Saturated: Too much solute than solvent can hold
Saturated: more solute than solvent can hold
Unsaturated: less solute than solvent can hold

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13
Q

What factors influence Solubility?

A

Temperature: Solubility of gases in liquids is decreased as temps rise
Pressure: Solubility of gas rises as pressure rises

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14
Q

Dilute Solution vs Concentrated

A

Dilute: Contains a relatively small amount of solute
Concentrated: contains large amount of solute

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15
Q

Percent by Mass

A

Mass of solute/total weight of solution X 100

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16
Q

Percent by Volume

A

Volume of solute/total volume of solution X 100

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17
Q

Index

A

Concentration of formaldehyde in embalming fluid
Index=HCHO g/100 ml of solution

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18
Q

Osmotic Principles to Embalming

A

Hypotonic: use on Normal/Dehydrated cases
Hypertonic: use on Edema cases
Isotonic: leaves bodies unembalmed

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19
Q

Properties of Acids

A
  • Acids in solution taste sour
  • Sting the skin
  • Neutralization Reaction: React with bases to form water & salt
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20
Q

Salts

A
  • 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)
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21
Q

Electrolytes

A
  • Salts that dissolve in water and dissociate into positive and negative ions
  • The presence of ions in a solutions enables it to conduct electricity
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22
Q

Electrolysis

A

The passage of an electric current through a solution
can be acids, bases, or salts
- Solutions that allow electrolysis are electrolytes

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23
Q

pH Hydrogen Ion Concentration

A
  • 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
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24
Q

Weak electrolytes

A

weak conductors of electricity

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25
Q

Strong electrolytes

A

good conductors of electricity

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26
Q

pH of blood

A

7.3-7.5

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27
Q

pH of Human Gastric Juice

A

1.0-3.0

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28
Q

pH of Pure Water

A

7.0

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29
Q

pH of Embalming Fluid

A

6.5-9.0

30
Q

Buffers

A

Protective mechanism in the blood that protect against changes in pH

31
Q

Number of Ionizable Hydrogens

A
  • 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
32
Q

Number of Elements

A
  • Binary Acids: hydrogen & 1 other element
  • Ternary Acids: Oxygen, hydrogen & a nonmetallic element
33
Q

Arrhenius Theory on Acids

A

Acids are substances that dissociate(break apart) in an aqueous solution to yield hydrogen ions

34
Q

Arrhenius Theory on Bases

A

Bases disassociate to create hydroxide ions

Bases are substances that dissociate in an aqueous solution to yield hydroxide ions

35
Q

Hydrochloric Acid

A

HCl
Binary
Strong Acid
Monoprotic

36
Q

Nitric Acid

A

HNO3
Ternary
Strong Acid
Monoprotic

37
Q

Sulfuric Acid

A

H2SO4
Ternary
Strong Acid
Diprotic

38
Q

Phosphoric Acid

A

H3PO4
Ternary
Moderate Acid
Triprotic

39
Q

Carbonic Acid

A

H2CO3
Ternary
Weak Acid
Diprotic

40
Q

Acetic Acid

A

HC2H3O2
Ternary
Weak Acid
Monoprotic

41
Q

Strong Acid

A

Molecules that completely dissociate into their ions when it’s in water

42
Q

Weak Acid

A

Molecules that partially dissociate into their ions when it’s in water

43
Q

Sodium Hydroxide

A

NaOH
Lye

44
Q

Potassium Hydroxide

A

KOH

45
Q

Calcium Hydroxide

A

Ca(OH)2

46
Q

Magnesium Hydroxide

A

Mg(OH)2

47
Q

Bases

A

Taste Bitter
Feel Slippery
Bases react with acids to form salts and water (neutralization reaction)
Usually have a hydroxide group - OH

48
Q

Ammonia

A

NH3
Weak Base

49
Q

Polar Molecule

A

Polar molecules are those that possess regions of positive and negative charge

50
Q

Nonpolar Molecule

A

Bonding electrons shared equally between two atoms

51
Q

Concentration

A

The amount of a particular solute in a given volume of solution

52
Q

Vehicle

A

A carrier or inert medium used as a solvent (or diluent)

53
Q

Ratio

A

the relationship in quantity, amount, or size between two or more things : proportion

54
Q

Molarity

A

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

55
Q

Parts Per Million

A

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.

56
Q

Parts Per Billion

A

ppb

57
Q

Tincture

A

a medicine made by dissolving a drug in alcohol.

58
Q

Aqueous Solution

A

water that contains one or more dissolved substance

59
Q

Hydrolysis

A

the destruction/reaction of an organic chemical with water to form two or more new substances

60
Q

Ionization

A

the process when ions are formed by gain or loss of an electron from an atom or molecule

61
Q

Nonelectrolytes

A

A compound that does not conduct an electric current in either aqueous solution or in the molten state.

62
Q

Facts about Hydrogen

A
  • 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
63
Q

Physical Properties of Hydrogen

A

Colorless, odorless, tasteless gas
Lighter than air
Slightly soluble in water

64
Q

Chemical Properties of Hydrogen

A
  • Burns with hot, blue flame forming water
  • Doesn’t support combustion
  • means “water producer”
65
Q

Ways to Define Reduction

A

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

66
Q

Facts about water

A
  • 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
67
Q

Water on the periodic table (facts about water)

A
  • H2O
  • Bent molecule; 105°
  • atomic mass of 18
68
Q

Physical properties of water

A
  • 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
69
Q

Hydrogen bonding

A

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

70
Q

Surface tension

A

A force that causes the surface of a liquid to contract
Caused by hydrogen bonding
Water has high surface tension

71
Q

Why is surface tension important to embalmers?

A

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

72
Q

Chemical properties of water

A
  • 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

chemistry (22 decks)

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