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Advanced Anatomy & Physiology > Chapter 2: Chemistry Comes Alive > Flashcards

Chapter 2: Chemistry Comes Alive Flashcards

1
Q

Matter

A

Anything that occupies space and has mass

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2
Q

Energy

A

The capacity to do work, or to put matter in motion

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3
Q

Kinetic Energy

A

Energy in action

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4
Q

Potential Energy

A

Stored energy

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5
Q

What is the connection between matter and energy?

A

They are inseparable; Matter is substance and energy is the mover of the substance

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6
Q

Chemical Energy

A

The form stored in the bonds of chemical substances

1) Atoms rearrange
2) PE is released
3) KE

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7
Q

Describe Eating

A

1) Food E is captured temporarily in the bonds of a chemical called ATP
2) ATP bonds are broken, PE is released for cellular work

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8
Q

Electrical Energy

A

Results from the movement of charged particles

  • Electrical currents (ions move across cell membranes)
  • Nerve impulses
  • Pumping blood
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9
Q

Mechanical Energy

A

Energy directly moving matter

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10
Q

Radiant Energy/ Electromagnetic Radiation

A

Energy that travels in waves

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11
Q

Electromagnetic Spectrum

A

Waves that are varied in length

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12
Q

Energy Conversions

A
  • Energy can easily convert
  • Inefficient: Initial energy is always “lost” in the environment as heat (unusable energy)
  • All conversions give off heat: helps with homeostasis
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13
Q

Elements

A

Unique substances that cannot be broken down into simpler substances by ordinary chemical means

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14
Q

Atoms

A

Identical particles or building blocks of elements

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15
Q

Physical Properties

A

Those we can detect with our senses or measure

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16
Q

Chemical Properties

A

Pertain to the way atoms interact with other atoms

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17
Q

Nucleus

A

(1) Control center of a cell; contains genetic material; (2) center of an atom; contains protons and neutrons

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18
Q

Protons

A

Positive electrical charge

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19
Q

Neutron

A

Neutral, so nucleus is positive overall

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20
Q

What are the connections between protons, neutrons and the nucleus

A

1) Protons and neutrons are heavy subatomic particles of the nucleus
2) Nucleus is dense= 99.99% mass of the atom

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21
Q

Electrons

A

Negative charge equal in strength to the positive charge of the proton

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22
Q

What are all atoms charged?

A

Neutral; the # of protons in an atom is balanced by its # of electrons

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23
Q

Planetary Model

A

A simplified model of atomic structure

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24
Q

Orbital

A

Regions around the nucleus in which a given electron or electron pair is likely to be found most of the time

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25
Q

Orbital Model

A

More useful for predicting the chemical behavior of atoms

- predicts probable regions of greatest electron density by denser shading (electron cloud)

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26
Q

Atomic number

A

Equal to the # of protons (electrons)

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27
Q

Mass number

A

The sum of the masses of its protons and neutrons

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28
Q

Isotopes

A

2 or more structural variations of elements that have the same # of protons and electrons but a different # of neutrons

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29
Q

Atomic Weights

A

An average of the relative weights of all the isotopes of an element
- Atomic # = Mass # of most abundant isotope

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30
Q

Radioactivity

A

The process of atomic decaying spontaneously into more stable forms because of unstable heavier isotopes

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31
Q

Radioisotopes

A

Isotopes that exhibit radioactivity

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32
Q

Quarks

A

Smaller particles of the nucleus that associate one way to form protons and another neutrons
- holds nuclear particles together and is weaker in heavier isotopes

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33
Q

Molecule

A

A combination of 2 or more atoms of the same element held together by chemical bonds

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34
Q

Compound

A

2 or more different kinds of atoms bind, they form molecules of a compound

  • Chemically Pure
  • Identical Molecules
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35
Q

Mixtures

A

Substances composed of 2 or more components physically intermixed

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36
Q

What are the 3 basic types of mixtures?

A

1) Solutions
2) Colloids
3) Suspension

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37
Q

Solutions

A

Homogeneous mixtures of components that may be gases, liquids or solids

  • Particles are very tiny
  • Do not settle
  • Scatter light
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38
Q

Solvent

A

The substance in the greatest amount (or dissolving medium)

- Usually liquid

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39
Q

Solute

A

Substances present in smaller amounts (dissolved in the solvent)

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40
Q

True Solutions

A

Contains gases, liquids or solids dissolved in water

  • Usually transparent
  • Ex: Saline Solution, Mix: Glucose/ Water, and Mineral Water
  • Solutes are minute
  • Do not settle out/ scatter light
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41
Q

How do you describe True Solutions?

A

By their concentration

  • College/ Hospital: percent (parts per 100 parts) of the solute in the total solution (water is the assumed solvent)
  • Blood Concentration: Milligrams per deciliter
  • Molarity
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42
Q

Molarity

A

Moles per liter, M

- Complicated but useful

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43
Q

Mole

A

Equal to any element or compounds atomic weight or molecular weight

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44
Q

Molecular weight

A

Sum of atomic weights

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45
Q

Avogadro’s Number

A

6.02 X 10(23)

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46
Q

Colloids/ Emulsions

A

Heterogeneous mixtures

  • Translucent/ Milky
  • Large particles
  • Scatter light
  • Do not settle
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47
Q

Sol-gel Transformation

A

To change reversibly from a fluid (sol) state to a more solid (gel) state
- Ex: Jell-O
• Underlie important cell activities

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48
Q

Suspensions

A

Heterogeneous mixtures

  • Very large particles
  • Often visible solutes that settle out
  • Ex: Blood
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49
Q

What are the differences between mixtures and compounds?

A

1) No chemical bonding in mixtures (only physically intermixed)
2) Mixtures can be separated by physical means
Compounds—> Chemical means
3) Mixtures: Homogeneous/ Heterogeneous
Compounds: Homogeneous

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50
Q

Chemical Bonds

A

An energy relationship between the electrons of the reacting atoms

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51
Q

Electron Shells

A

The regions of space of an atom around the nucleus where electrons are forming an electron cloud

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52
Q

Valence Shell

A

An atoms outermost energy level containing the electrons that are chemically reactive

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53
Q

What are the 3 major types of chemical bonds?

A

1) Ionic
2) Covalent
3) Hydrogen

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54
Q

Ions

A

Charged particles that form when the balance of + and - are lost

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55
Q

Ionic Bond

A

A Chemical bond between atoms formed by the transfer of one or more electrons from one atom to another

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56
Q

Electron Acceptor

A

The atom that gains one or more electrons

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57
Q

Anion

A

The negative net charge in an electron acceptor

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58
Q

Electron Donor

A

The atom that loses its electrons

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59
Q

Cation

A

A positive net charge in an electron donor

60
Q

Describe an Ionic Bond

A

Both anions and cations are formed whenever electron transfer between atoms occur. Opposite charges attract so these ions tend to stay close together= Ionic bond

61
Q

Crystals

A

Large arrays of cations and anions held together by ionic bonds

62
Q

Covalent Bond

A

Electrons sharing produces molecules in which the shared electrons occupy a single orbital common in both atoms

63
Q

What are the 2 types of molecules in covalent bonds?

A

1) Polar

2) Non Polar

64
Q

Non Polar molecule

A

Equal sharing of electrons

- Don’t have separate + and - poles of charge

65
Q

Polar molecule

A

Unequal sharing of electrons

66
Q

Electronegativity

A

Electron hungry and attract electrons very strongly

67
Q

Electropositive

A

Atoms with only 1 or 2 valence electron shells

  • Potassium
  • Sodium
68
Q

What is another name for a polar molecule?

A

Dipole

69
Q

Hydrogen Bonds

A

When a hydrogen atom, already covalently linked to one electronegative atom, is attracted by another electronegative atom, so that a “bridge” forms between them

70
Q

Chemical Reaction

A

Occurs whenever chemical bonds are formed, rearranged or broken

71
Q

Subscript

A

Indicates that atoms are joined by chemical bonds

72
Q

Prefix

A

Denotes the # of unjointed atoms or molecules

73
Q

Reactants

A

The # and kinds of the interacting substances

74
Q

Products

A

The chemical composition of the result of the reaction

75
Q

Relative Proportions

A

Balanced equations indicated the relative proportion of each reactant and product

76
Q

Molecular Formula

A

Representation of a product in a molecule

77
Q

Synthesis/ Combination Reaction

A

Involves bond formation

A + B—-> AB

78
Q

Anabolic(sm)

A

Energy requiring building phase of metabolism in which simpler substances are combined to form more complex substances

79
Q

Name an example of synthesis reaction

A

Amino acids are joined together to form a protein molecule

- smaller particles of bonded together to form larger, more complex molecules

80
Q

Decomposition Reaction

A

Occurs when a molecule is broken down into smaller molecules
AB—-> A + B
- Reverse Synthesis

81
Q

Catabolic(sm)

A

Process in which living cells breakdown substances into simpler substances

82
Q

Exchange/ Displacement Reaction

A

Involve both synthesis and decomposition bonds of both made and broken. An exchange reaction occurs when ATP reacts with glucose and transfers it end phosphate group to glucose forming glucose phosphate at the same time, the ATP becomes ADP this important it reaction occurs whenever glucose into the body cells and is effectively traps the glucose fuel molecule inside the cell

83
Q

Oxidation-Reduction/ Redox Reaction

A

Decomposition reactions in that they are the basis of all the actions in which food fuels all broken down for energy (ATP). Electrons are exchanged between the reactants. The reactant losing that electrons is the electron donor and is said to be oxidized. The reactant taking up the transferred electrons is the electron acceptor and it said to be reduced

84
Q

Exergonic Reactions

A

Reactions that release energy. These reactions yield products with less energy than the initial reactants along with energy that can be harvested for other uses with few exceptions catabolic and oxidative reactions on exergonic

85
Q

Endergonic

A

The products of energy absorbing. Contain more tensional energy in the chemical bonds than did the reactants
- Ex: Anabolic Reactions

86
Q

What is the reversibility represented in a chemical reaction?

A

Double arrows

  • when arrows differ in length the longer arrow indicates the major direction in which the reaction proceeds
  • when the arrows are of equal length, the molecule of the product forms one molecule, breaks down releasing the reactants A & B. This chemical reaction is in a state of chemical equilibrium
87
Q

What happens when the chemical equilibrium is reached?

A

There is no for the net change in the amounts of reactants and products unless more of either are added to the mix

88
Q

What factors influence the rate of chemical reactions?

A

1) Temperature
2) Concentration
3) Particle Size
4) Catalyst

89
Q

Temperature

A

Increasing the temperature of a substance increases the kinetic energy of its particles and the force of their collisions

90
Q

Concentration

A

Occurs when the reacting particles are present in high numbers because the chance of successful collisions is greater. As the concentration of the reactants declines, the reaction slows. Chemical equilibrium eventually occurs.

91
Q

Particle Size

A

Smaller particles move faster than larger ones and tend to collide more frequently and more forcefully

92
Q

Catalysts

A

Substances that increase the weight of chemical reactions without themselves becoming chemically changed or part of the product

93
Q

What are biological catalysts called?

A

Enzymes

94
Q

Biochemistry

A

The study of the chemical composition and reactions of living matter

95
Q

What 2 Major categories do the chemicals in the body fall into?

A

1) Organic

2) Inorganic

96
Q

Organic Compounds

A
  • Contains carbon
  • Covalently bonded
  • Many are large
97
Q

Inorganic Compounds

A

All other chemicals in the body (not carbon)

- Ex: Water, Salts, many acids and bases

98
Q

What are the 5 properties of water?

A

1) High Heat Capacity
2) High Heat of Vaporization
3) Polar Solvent
4) Reactivity
5) Cushioning

99
Q

High Heat Capacity

A

Absorbs and releases large amounts of heat before changing appreciably in temperature itself.
Prevents sudden changes in temperature caused by external factors or by internal conditions that release heat rapidly
- External: Sun, Wind Exposure
- Internal: Vigorous muscle activity
Redistributes heat among body tissues ensuring temperature homeostasis

100
Q

High Heat of Vaporization

A

When water evaporates it requires large amounts of heat being absorbed to break the hydrogen bonds that hold water molecules together
- Ex: Perperation

101
Q

Polar Solvent

A

Because water molecules are polar they orient themselves with their slightly negative and toward the positive ends of the solutes and vice versa first attracting the solute molecules and then surrounding them. This polarity of water explains why ionic compounds and other small reactive molecules dissociate in water there ions separating from each other and becoming evenly scattered in the water forming to solutions

102
Q

What are the water molecule layers called?

A

Hydration layers

103
Q

Hydration Layers

A

Forms layers around large charged particles, such as proteins shielding them from the effects of other charged substances in the vicinity and preventing them from settling out of solution

104
Q

What are protein-water mixtures called?

A

Biological Colloids

- Ex: Blood plasma, cerebrospinal fluid

105
Q

Reactivity

A

Water is an important reactant in many chemical reactions

106
Q

Cushioning

A

By forming a resilient cushion around certain body organs, water helps protect them from physical trauma

107
Q

Salt

A

An ionic compound containing cations other than H+ and anions other than the hydroxyl ion (OH-)

108
Q

What happens when salts dissolve into water?

A

They dissociate into their component ions

- Ex: Sodium Sulfate, Na2SO4—-> 2 Na+ ions and 1 SO4 2- ion

109
Q

Electrolyte

A

Substances that conduct an electrical current in solution

110
Q

Polyatomic ions

A

Groups of atoms that bear and overall charge (Ex: Sulfate)

111
Q

What are the most commonly found salts in the body?

A
  • NaCl
  • CaCO3 (calcium carbonate)
  • KCl (Potassium Chloride)
112
Q

Acids

A

A substance that releases hydrogen ions in detectable amounts

  • Proton Donor
  • Sour taste
  • can react with (dissolve) many metals
  • Ex: Acetic Acid (HC2H3O2/ HAc), carbonic acid (H2CO3)
  • The hydrogen is always first in an acidic molecule!!!!!
113
Q

Proton Donor

A

When a hydrogen ion is just a hydrogen nucleus

114
Q

What determines the acidity of a solution?

A

The concentration of protons

115
Q

Bases

A
  • Bitter taste
  • Feel slippery
  • Proton acceptors
  • Inorganic bases: Hydroxides
116
Q

Proton Acceptors

A

Take up hydrogen ions (H+) in detectable amounts

117
Q

Hydroxyl ions

A

Ions liberated when a hydroxide is dissolved in water

118
Q

Bicarbonate ion (HCO3-)

A

An important base in the body, particularly abundant in blood

119
Q

Ammonia

A

A common waste product of protein breakdown in the body (also base)
It has 1 pair of unshared electrons that strongly attracts protons
By accepting a proton, ammonia becomes an ammonium ion
NH3 + H+ —–> NH4+

120
Q

pH units

A

The concentration units used to measure the relative concentration of hydrogen ions in various body fluids

121
Q

Who created the pH scale?

A

Danish biochemist and beer brewer Sören Sörensen in 1909

122
Q

Neutralization Reaction

A

When acids and bases on mixed, because the joining of H+ and OH- form water neutralizes the solution

123
Q

Buffers

A

The chemical systems of homeostasis that regulates acid-base balance

124
Q

Hydroxyl

A

-OH

125
Q

Carbonyl

A

=aldehydes; ketones

126
Q

Carboxyl

A

-COOH

carboxylic acids

127
Q

Amino

A

-NH2

amines

128
Q

Sulfhydryl

A

-SH

thiols

129
Q

Phosphate

A

-PO4

organic carbohydrates

130
Q

Dehydration Reaction

A

Process by which a large molecule is synthesized by removing water and covalently bonding smaller molecules together; water splitting 2 molecules

131
Q

Hydrolysis

A

Process in which water is used to split a substance into smaller particles; water leaves causing a junction

132
Q

Monomer

A

1 subunit

133
Q

Polymers

A

Many subunits

134
Q

What is the major function of Carbohydrates?

A

Immediate energy source; some structural support

135
Q

What are the major functions of a Protein?

A

1) Structure
2) Signaling (hormones)
3) Enzymes/ Catalysts
4) Transport

136
Q

Enzymes

A
  • Substrate specific

- Denatured by heat, pH extremes, chemicals, electricity, radiation

137
Q

What do Proteins contain?

A
  • An amino and carboxyl group

* Peptide Bonds

138
Q

What are the Macromolecules of Carbohydrates?

A
  • Disaccharides (sucrose)

- Polysaccharides (starch, glycogen)

139
Q

What are the major functions of Lipids?

A

1) Cell membrane
2) Insulation
3) Nerve transmission
4) Energy Reserve

140
Q

Saturated Fats

A
  • All single bonds

* Animal products

141
Q

Unsaturated Fats

A
  • Double or triple bond

* Plant products

142
Q

What is the major function of Nucleic Acids?

A

Determines the synthesis of proteins; control the cell (information)

143
Q

DNA

A 
Deoxyribonucleic acid
• Double strand
• Sugar: Dioxyribose
• Bases: Adenine, Thymine, Guanine, Cytosins
• Carries instructions to make proteins 
• Permanent
144
Q

RNA

A 
Ribonucleic acid
• Single strand
• Sugar: ribose
• Bases: Adenine, Uracil, Cytosine, Guanine 
• Works to make the proteins
• Temporary
145
Q

What are the building blocks of Organic Phosphates?

A

Adenine and Phosphate

146
Q

What is the major function of Organic Phosphates?

A

Cell’s energy molecule

147
Q

When are Organic Phosphates made?

A

Cellular Respiration

Advanced Anatomy & Physiology (11 decks)

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