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A&P 1 > Chapter 2 Chemical Level of Organization > Flashcards

Chapter 2 Chemical Level of Organization Flashcards

1
Q

Smallest stable units of matter made up of “subatomic particles”

A

Atoms

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2
Q

What are the 3 subatomic particles.

A
  • Protons
  • Neutrons
  • Electrons
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3
Q

Which subatomic particles are the same size and mass?

A

-neutrons and protons

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4
Q

Smaller subatomic particle.

A

-electron

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5
Q

Atoms contain a equal number of what subatomic particles.

A

-Protons and electrons

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6
Q

A equal number of protons and electron give the atom a what charge?

A

Neutral

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7
Q

Which subatomic particles are located in the nucleus

A

Protons & Neutrons

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8
Q

The pathway that an electron follows around the nucleus.

A

Orbits

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9
Q

The electron orbit and proton-neutron nucleus make up what?

A

Electron cloud

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10
Q

The number of protons is known as the ______.

A

Atomic number

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11
Q

The total number of protons and neutrons is known as the ______.

A

Atomic mass

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12
Q

The layering of electrons around the nucleus.

A

Shell

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13
Q

Atoms are classified by the number of protons into groups called ______.

A

Elements

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14
Q

Two or more elements are combined to form _____ _____.

A

Chemical compounds

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15
Q

How many elements are in the human body?

A

26
13 in large quantities
13 in small quantities

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16
Q

Created in nature by adding additional neutrons to nucleus of element.

A

Isotopes

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17
Q

Isotopes that emit subatomic paticles or radiation from its nucleus.

A

Radioisotopes

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18
Q

This is the time it takes for the radioisotope to breakdown or degrade by half of its original strength.

A

Half life

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19
Q

Quantity of an element that is equal to the elements atomic weight.

A

Mole

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20
Q

Elements that do not react with other atoms are said to be _____. Outer shell is complete.

A

Inert/Stable

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21
Q

Elements that interact with other elements are called _____.

A

Reactive

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22
Q

What are the types of chemical bonds?

A
  • Ionic bonds
  • Covalent bonds
  • Hydrogen bonds
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23
Q

Strong bond when compounds are in solid form but weak when in liquid form.

A

Ionic bond

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24
Q

Two types of ions?

A
  • Anion

- Cation

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25
Q

Negatively charged atom.

A

Anion

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26
Q

Positively charged atom.

A

Cation

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27
Q

One atom will lose an electron (electron donor)

A

Cation (+)

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28
Q

One atom will gain an electron (electron acceptor)

A

Anion (-)

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29
Q

Strong bond in which two atoms can complete their outer shell by sharing electrons. Strong bond. Can be single, double, or triple.

A

Covalent bonds

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30
Q

What are the 2 types of covalent bonds?

A

Non-polar

Polar

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31
Q

Type of covalent bond that has equal sharing of electrons.

A

Non-polar covalent bonds

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32
Q

Type of covalent bond that has unequal sharing of electrons, which creates a slightly negative charge and a slight positive charge.

A

Polar covalent bonds

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33
Q

Weak bond in which the attraction between positive delta of hydrogren of one molecule to negative delta of oxygen of another molecule.

A

Hydrogen bond

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34
Q

What are the 3 states of matter?

A
  • Solids
  • Liquids
  • Gases
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35
Q

All of the atomic weights of all elements in a molecular or chemical compound.

A

Molecular Weight

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36
Q

New chemical bonds form between two or more atoms to make a new molecule or compound.

A

Chemical Reactions

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37
Q

Molecules that begin the reaction.

A

Reactants

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38
Q

New molecule that is formed.

A

Products

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39
Q

All chemical reactions in an organism.

A

Metabolism

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40
Q

How do cells maintain homeostasis?

A

By use of chemical reactions

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41
Q

Movement or change in the physical structure of matter.

A

Work

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42
Q

The capacity or ability to perform the work.

A

Energy

Work requires energy to be performed

43
Q

What are the 2 types of energy?

A

Kinetic energy

Potential energy

44
Q

Energy that is doing work or being used.

A

Kinetic energy

45
Q

Stored energy (In battery.) ATP and ADP are examples.

A

Potential energy

46
Q

What is ATP?

A

Energy stored in the human body

47
Q

What is ADP?

A

Potential energy

48
Q

Three types of chemical reactions?

A
  • Decomposition
  • Synthesis
  • Exchange
49
Q

Chemical reaction when a larger molecule is broken into smaller molecules.

A

Decomposition

50
Q

In decomposition which is larger, reactants or the products?

A

Reactants

51
Q

Decomposition involving water.

A

Hydrolysis

52
Q

Decomposition of molecules within cells.

A

Catabolism

53
Q

Chemical reaction that is the opposite of decomposition. A larger molecule is formed from two smaller molecules or atoms.

A

Synthesis.

54
Q

In a synthesis reaction which is smaller reactants or the product?

A

Reactants.

55
Q

What are the 2 types of synthesis?

A
  • Dehydration synthesis

- Anabolism

56
Q

Type of synthesis in which there is formation of a larger molecule by the removal of H2O.

A

Dehydration synthesis

57
Q

Type of synthesis. The synthesis of new compounds within the body.

A

Anabolism

58
Q

Chemical reaction that parts of reacting molecules are shifted around.

A

Exchange

59
Q

What happens when a reaction reaches equilibrium?

A

There are equal numbers of decomposition reactions taken place as there are synthesis reactions.

60
Q

Amount of energy required to start a reaction.

A

Activation energy

61
Q

Chemicals the body uses to lower the activation energy to the reaction can occur with less energy.

A

Enzymes

62
Q

Another name for enzymes

A

Catalysts

63
Q

Compounds that can speed up reactions with out themselves being destroyed.

A

Catalysts

64
Q

Compounds that can reduce the amount of heat by reducing the activation energy.

A

Catalysts

65
Q

Compounds of the human body that do not have carbon and hydrogen as the primary structure.

A

Inorganic compounds

66
Q

Main inorganic compounds of the human body? (4)

A
  • Carbon Dioxide
  • Oxygen
  • Acids, Bases, Salts
  • Water
67
Q

Any solute that dissociates in solution and releases a hydrogen ion thus reducing the pH.

A

Acids

68
Q

Any solute that dissociates in solution and releases a hydroxide ion thus increases the pH.

A

Bases

69
Q

An ionic compound consisting of any cation (except a hydrogen ion) or anion (except a hydroxide ion)

A

Salts

70
Q

Water is the universal solvent so many compounds are dissolved in water.

A

Solubility

71
Q

Uniform mixture of two or more substances.

A

Solution

72
Q

The medium the substances are dissolved in

A

Solven

73
Q

Chemical reactions in our bodies occur in water.

A

Reactivity

74
Q

Ability to absorb and retain heat due to hydrogen boding.

A

High heat capasity.

Water’s high head capacity allows blood plasma to recirculate heat as it circulates through the body

75
Q

Separates two layers and keeps them slippery, reducing friction.

A

Lubrication

76
Q

Water molecule is a polar covalent molecule, also called a dipole.

A

Polarity

77
Q

What happens when salts are dissociated in water?

A

Electrical current can pass from one ion to the next ion.

78
Q

Any soluble inorganic molecules whos ions will carry a charge.

A

Electrolytes

79
Q

What is a neutral pH?

A

7

80
Q

What is the homeostatic pH range of blood/tissue fluids.

A

7.35-7.45

81
Q

What is it called when pH below 7 in the body causes coma.

A

Acidosis

82
Q

What is it called when pH above 7.8 in the body causes uncontrollable muscle contractions.

A

Alkalosis

83
Q

Organic molecule that contains carbon, hydrogen, and oxygen. Includes sugars and starches.

A

Carbohydrates

84
Q

Monomer for Carbohydrates. Source of energy used immediately. Called a simple sugar

A

Monosaccharides

85
Q

Complex sugar stored for future use.

A

Disaccharides/polysaccharaides

86
Q

what is the 1:2:1 ratio for carbohydrates.

A

1 carbon : 2 hydrogen : 1 oxygen

87
Q

Kinds of monosaccharides

A
  • 3-Triose
  • 4-Tetrose
  • 5-Pentose
  • 6-Hexose
  • 7-Heptose
88
Q

Most important fuel that the body uses

A

Glucose

89
Q

What kind of monosaccharide is glucose?

A

Hexose

90
Q

Glucose and fructose are types of what?

A

Monosaccharides

91
Q

Made up of 2 or more monosaccharides

A

Disaccharides and polysaccharides

92
Q

Have a 1:2 ratio of carbon to hydrogen but contains fewer oxygen molecules than carbohydrates.

A

Lipids

93
Q

Make up fats oils and waxes.

A

Lipids

94
Q

Used as energy storage. Cell membrane components and chemical messengers.

A

Lipids

95
Q

Has a long chain of several carbons bound with hydrogens with carboxylic acid tail.

A

Fatty Acids

96
Q

Type of fatty acid that all carbons are single bonds

A

Saturated

97
Q

Type of fatty acid that carbons have a double bond.

A

Unsaturated

98
Q

Type of fatty acid that carbons only have 1 double bond.

A

Monounsaturated

99
Q

Type of fatty acid that carbons have more than 1 double bond.

A

Polyunsaturated

100
Q

Made from arachadonic acid

A

Eicosanoids

101
Q

Must come from food, body can not make it.

A

Arachadonic acid

102
Q

Short chain fatty acid, with 5 carbons in a ring. Released by damaged tissue to produce pain. Helps trigger labor contractions.

A

Prostaglandins

103
Q

Produced in response to injury/disease by WBC’s.

A

Leukotrienes

A&P 1 (6 decks)

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