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Anatomy 1 > Chapter 2, Chemical basis for life > Flashcards

Chapter 2, Chemical basis for life Flashcards

1
Q

3 subatomic particles

A

protons, neutrons, electrons

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2
Q

Adhesion in water molecules

A

The attraction between water molecules

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3
Q

Describe Carbohydrates

A

Consist of Carbon, hydrogen, oxygen in a 1:2:1 ratio.. Small in size, electrically neutral, shares electrons with other atoms (enables formation of long hydrocarbon chains or rings). Functional groups can attach to carbon rings or chains. Types- monosaccharide, disaccharide and polysaccharide
Not as important - Essential component in organic molecules.

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4
Q

Carbohydrates are used for?

A

Used for energy, storage of energy and cellular structures.

Cells use them for energy as well as structure materials

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5
Q

chemical bonding

A

The force by which atoms are bound in a molecule. The types of chemical bonding are covalent, ionic and hydrogen bonds

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6
Q

chemical symbol

A

Represents an element. For example H stands for Hydrogen

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7
Q

cholesterol

A

Found in every cell of our body. A steroid alcohol that is found in many fat based tissues throughout the body. Cholesterol can by synthesized in the body or obtained through diet.

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8
Q

Cohesion of water molecules results in

A

Results in high surface tension

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9
Q

Colloid

A

Heterogeneous containing larger sized solutes
Solutes do not precipitate out, but often reflect light
Colloids have the ability to transform from fluid to solid and back again. This is called sol-gel transformation.

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10
Q

compounds

A

A substance made up of two or more elements (think of a compound word)

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11
Q

Covalent Bonding

A

Macromolecules/Life molecules. Usually organic, sharing one or more pairs of atoms. Covalent bonds make organic molecules hold together. Often carbon molecules

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12
Q

Define chemical reaction

A

forming or breaking bonds. Requires input or release of energy. 3 types - synthesis, decomposition and exchange.

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13
Q

Define functional group

A

the reactive part of a molecule that determines the molecule’s chemical activity.

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14
Q

Describe Amino Acids

A

The amino acid contains a central carbon atom attached to a hydrogen atom (C-H), an amino group (H2N), a carboxyl group O=C-OH and a unique side chain R.

20 Different AA found in the body. They are the basic building blocks of peptides and proteins.

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15
Q

Describe ATP (formula)

A

Glucose (C6H12O6) burned in 02 gives us CO2 + H20 + 36 - 38 ATP. Occurs in the mitochondria

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16
Q

Describe lipids

A

Fatty and other oily substances. Made of carbon, oxygen and hydrogen. They are all insoluble
Cells use them for energy storage, structural support, and signaling molecules
There are 4 types-
Neutral fats, Phospholipids, Steroids, Eicosanoids- mode up of 20 fatty acids in a ring structure

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17
Q

Describe proteins

A

Organic molecules composed of amino acids joined by peptide bonds. Contain Carbon, hydrogen, oxygen and nitrogen. They are the most abundant molecule in the human body.

Form enzymes and hormones and control all metabolic and biochemical reactions and processes in cells (cell structure, regulating growth, transporting molecules, defending the body against invaders),

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18
Q

Describe the polar water molecule

A

In a water molecule, the oxygen atom and hydrogen atoms share electrons in covalent bonds, but the sharing is not equal. In the covalent bond between oxygen and hydrogen, the oxygen atom attracts electrons a bit more strongly than the hydrogen atoms. Water molecules attract one another based on the attraction between the positive end of one water molecule and the negative end of another.

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19
Q

Describe the structure of DNA

A

DNA molecules consist of two parallel strands of the nucleotides A, G, C, and T. The strands are connected by hydrogen bonds between the nitrogenous bases. Each nitrogenous base can hydrogen bond with only one other specific nitrogenous base. Adenine can bond only with thymine, and guanine can bond only with cytosine. The two strands of bonded nucleic acid twist around each other in a spiral called a double helix. The order of the nucleotides is unique to each individual and is carried in every cell of the individual.

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20
Q

Difference between organic and inorganic bonds

A

Organic compounds are molecules that contain hydrocarbon chains and groups (hydrogen and carbon) and usually are covalently bonded. They are large and complex and are essential components of all living things. Examples: proteins, carbs, triglycerides and nucleic acids

Inorganic molecules, on the other hand, rarely contain carbon and do not contain hydrogen-carbon. This micromolecules are often ionically bonded. Examples are water, salts, acids and bases

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21
Q

differences between mixtures and compounds

A

Compounds are homogenous, chemically bounded and separation is difficult.

Mixtures can be homogenous or heterogenous and components can be easily separated (filtration, evaporation centrifugation or straining)

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22
Q

Electrons

A

negatively charged particles, they are wavicles in constant motion around the nucleus

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23
Q

Elements that make up the body

A

In the body 96% is Nitrogen, hydrogen, oxygen, carbon. Minor elements are Na, Mg, K, Ca, P, S, Cl92 Naturally occurring elements in nature.

Less important- In the body 96% is Nitrogen, hydrogen, oxygen, carbon. Minor elements are Na, Mg, K, Ca, P, S, Cl

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24
Q

How does a nucleotide differ from an amino acid

A

Nucleotides are the building blocks of nucleic acids such as DNA, but amino acids are the building blocks of proteins.

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25
Q

How does a weak acid act as a buffer

A

It helps the cell maintain a neutral pH by not allowing excessive hydrogen or hydroxyl ions to accumulate. In water, a weak acid will initially ionize into: (1) free hydrogen (H+) ions, (2) a weak base product, and (3) remaining intact weak acid molecules. The pH of the solution is not changed much because some of the chemical remains in acid form and some remains in the form of a weak base.

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26
Q

How does an ATP molecule supply a cell with energy

A

As a nutrient (for example, glucose) is catabolized, the energy created is stored in ATP molecules.

ATP stores this energy in the bonds between its phosphate groups. When these bonds are broken (catabolized/hydrolyzed), that energy is released from the ATP molecule. To use the energy stored in ATP, enzymes must move the terminal phosphate group to another molecule. The receiving molecule is then temporarily has energy to do some work.

During this process the ATP molecule loses a phosphate group and becomes ADP. Another phosphate group can also be used, resulting in the creation of a molecule of AMP. As more glucose and other nutrients are metabolized, phosphate groups are joined to AMP, creating a renewed source of ATP.

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27
Q

How does an enzyme work

A

Enzymes speed up or catalyze chemical reactions without being destroyed or altered. Enzymes are specific to the reaction they catalyze and the substrates they use

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28
Q

How does ATP differ from a nucleotide

A

ATP is an RNA nucleotide containing the nitrogen base adenine with three aditional phosphate groups attached.

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29
Q

How is an ion different from an atom

A

Atoms are neutral. They contain the same number of protons as electrons.

An ion is an electrically charged particle produced by either removing electrons from a neutral atom to yield a positive ion or adding electrons to a neutral atom to yield a negative ion.

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30
Q

How many nitrogenous bases are there. Discuss

A

There are five different nitrogenous bases: adenine (A), cytosine (C), guanine (G), uracil (U), and thymine (T). Adenine, cytosine, guanine, and thymine are found in DNA. Adenine, cytosine, guanine, and uracil are found in RNA.

Much less important -These five nitrogenous bases are further divided into two groups based on their molecular structure: purines and pyrimidines. Purines include adenine and guanine and have two rings in their molecular structure. Pyrimidines, which include thymine, cytosine, and uracil, are single-ringed molecules.

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31
Q

hydrophyllic

A

Chemicals/molecules that mix well or disolve in water

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32
Q

Ion

A

An electrically charged atom or molecule. It has gained or lost an electron Cations are positive (more protons than electrons) and Anions are negative (more electrons than protons).

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33
Q

Isotope

A

One or more atoms with a different number of neutrons than protons. Atomic number # protons) is different than their mass.

If it has eight neutrons they become radioactive isotope (Carbon 14)

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34
Q

Keytones

A

Produced by lipid metabolism. Too many can make you sick.

Not as important- Usually produced by AcetylCoA from fatty aids in the liver.

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35
Q

List the inorganic molecules important for life

A

Water, salts, and acids and bases

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36
Q

List the organic molecules important for life

A

Carbohydrates, lipids, proteins, and nucleic acids

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37
Q

Matter

A

Anything that occupies space and has mass, can often be identified with out senses, is not the same as weight, composed of one or more elements

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38
Q

molecules

A

A group of atoms (or sometimes a single atom) bonded together, the smallest unit of a compound that retains the chemical properties of that compound

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39
Q

Monosaccharides

A

Simple sugars composed of only one monomer. They are so small they need no digestion before being absorbed.

less important- A type of carbohydrate. Examples - glucose, fructose and ribose.

40
Q

Neutrons

A

neutrally charged particle, located in the nucleus

41
Q

Nucleotides

A

A nucleotide is the building block of nucleic acids (DNA and RNA) and AA. They are small organic compounds that contain one or more phosphate groups and a five carbon sugar attached to a nitrogenous b
ase. Has C, H, O, N, P.

42
Q

Oligosaccharides

A

a carbohydrate whose molecules are composed of a relatively small number of monosaccharide units. The short chains of sugar monomers covalent bonded together. If it’s only two it’s a dissacharide. Examples- lactose, sucrose.

43
Q

Polar Molecule

A

Electrons spend more time on one atom than another, creating oppositely charged ends. A good example is the water molecule

44
Q

Polysaccharides

A

complex carbohydrates with many sugar monomers that form chains or branches (glycogen, starch and cellulose)

45
Q

Protons

A

positive charged particles, located in the nucleus

46
Q

Salts

A

Mineral compounds that have ionic bonds. The principle form of minerals that enter and are stored in the body. When salts are added to water they immediately ionize. In the ionized form they are known as electrolytes (ions) and can transmit an electric charge

47
Q

Solution

A

Homogeneous - can be gas, liquid,sold
Solutes are tiny
Solutes evenly distributed, do not settle or reflect light
Solutions are usually clear

48
Q

Structures of proteins

A

1st - amino acids
2nd- hydrogen bonds along length of AA, causing bending
3rd - bonding of AA, causing further looping
4th - Hydrogen bonds or bonds between R groups join two or more polypeptide chains.

Primary structure is the sequence of AA linked together to form peptide chains. Secondary structure is the natural bends of the peptide chains. The tertiary structure is the overall shape of a protein molecule. The quaternary structure is when to or more protein chains join to form a complex macromolecule

49
Q

Suspension

A

Heterogeneous mixtures that contain large solutes that readily separate from the solution when there’s no movement of suspension

50
Q

The rate of a chemical reaction is influenced by:

A

concentration of reactants- more reactants means they are more likely to come in contact with each other and react
Temperature of environment - Warmer molecules move faster and the more likely they are to come into contact with each other
Activation energy- Some reactions have a higher activation energy and require an input of more energy for the reaction to occur. These reactions will occur at a slower pace.
Presence of catalyst (enzyme)

51
Q

Three types of chemical reaction. Describe each

A

Synthesis, decomposition, exchange

synthesis- A new, more complex chemical is made from multiple simpler chemicals. X+Y= XY. Anabolic

Decomposition - A complex substance breaks down into its simpler parts. XY ->X + Y
. Catabolic

Certain atoms are exchanged between molecules. It is a combination of a synthesis and a decomposition reaction. WX+YZ-> WY+XZ

52
Q

Water’s unique qualities (4)

A

Water is the universal solvent
Water is an ideal transport medium
Water has high heat capacity and high heat of vaporization
Water is used for lubrication

53
Q

Water/Solid make up of body

A

The body is 60% water. This is made up of ECF (Extracellular Fluid that surrounds cells) which is approximately 20% of body weight - 15% interstitial (between the cells) and 5% plasma(in blood).
40% of the body is solids; ICF (intracellular fluid) makes up 40% of that.

54
Q

Ways to break a mixture into component parts-

A

filtration, straining, evaporation and centrifugation

55
Q

What feature does carbon possess that makes it particularly well suited for creating the chemistry of living creatures

A

Carbon is electrically neutral and can form four covalent bonds with other atoms, including other carbon atoms. It can take on a linear structure or a ring structure from which functional groups extend.

56
Q

What important functions do hydrogen bonds preform in organic and inorganic chemicals

A

Hydrogen bonds can form between molecules. Hydrogen bonding is the key to water’s unique properties as a universal medium.

Hydrogen bonds can also form between parts of the same molecule, giving it increased stability. DNA is a double helix because hydrogen bonds hold together base pairs. The complex folding in protein molecules is because of hydrogen bonds

57
Q

What is a compound

A

A compound includes two or more elements that are chemically bonded to one another via covalent or ionic bonds. The elements are present in a specific ratio, which is consistent for a particular compound.

58
Q

What is a mixture

A

A mixture is a combination of two or more ingredients that are chemically unchanged when combined with one another. Mixtures can be homogeneous and heterogeneous. Three types- solution, colloid, suspension

59
Q

What is a peptide bond

A

A peptide is a molecule consisting of two or more amino acids in which the carboxyl group of one acid is linked to the amino group of the other.

60
Q

What is an element

A

An element is matter that cannot be divided by ordinary chemical processes into another substance.

61
Q

What process joins simple sugars, explain

A

Dehydration synthesis, which is a synthesis reaction joining two monosaccharides and forming a disaccharide. Water is formed during the reaction and extracted from the saccharides

62
Q

What three elements are found in all carbohydrates

A

Carbon, hydrogen, and oxygen

63
Q

What three elements are found in all lipids

A

Carbon, hydrogen, and oxygen

64
Q

When do hydrogen bonds occur

A

Occur when there is a weak attraction between a slightly negative atom in a polar covalent bond and slightly positive hydrogen atom involved in a second polar covalent bond.

Hydrogen bonds are formed mostly between molecules (for example, between water molecules) and act to stabilize the solution. Hydrogen bonding is the key to water’s unique properties as a universal solvent and a medium for the life processes. Hydrogen bonds can also form between parts of the same molecule. This works to stabilize and hold the shape of large, complex molecules such as proteins and DNA.

65
Q

Which is a proton donor - Acid or Base. Why

A

Acid.
Acids are substances that can donate H+ ions to bases. Since a hydrogen atom is a proton and one electron, technically an H+ ion is just a proton. So an acid is a “proton donor”, and a base is a “proton acceptor”. The reaction between an acid and base is essentially a proton transfer.

66
Q

Elements

A

Any of 116 known substances that cannot be separated into smaller substances. The smallest unit of an element is an atom

67
Q

Hydrogen bonds

A

Occur when there is a weak attraction between a slightly negative atom in a polar covalent bond and slightly positive hydrogen atom involved in a second polar covalent bond. It is more of an electrostatic attraction than a true bond.

68
Q

List the characteristics of each subatomic particle

A

Protons are positive and found in the nucleus, neutron are neutral found in the nucleus electrons-arenegative circling the outside of the atom. A neutral atom has the same number of protons and electrons.

69
Q

List the major elements

A

Carbon, hydrogen, nitrogen and oxygen. Shown in orange on the periodic table.

70
Q

Differentiate the difference between a molecule and a compound

A

A compound is a type of molecule in which the atoms forming it are different from each other. A molecule is the union of two more atoms of the same (or different) elements and is the smallest unit of a compound.

71
Q

List the types of chemical bonds that may form between elements

A

Covalent, ionic and the hydrogen bond

72
Q

Triglycerides

A

Neutral Fats. One glycerol unit and 3 fatty acid chains. Double bonds are unsaturated (oils) and single chains are saturated (fats)

73
Q

Hydrolysis

A

Water is utilized when a disaccharide is decomposed into monosaccharides

74
Q

Sugars form?

A

Building block for carbs and nucleic acids

75
Q

Steroids

A

lipids that take the form of 4 interlocking hydrocarbon rings. An important one is cholesterol.

76
Q

Disaccharides

A

Two sugar units. Lactose is an example.

77
Q

Peptide

A

Two or more amino acids linked together

77
Q

Peptide

A

Two or more amino acids linked together

78
Q

Types of proteins

A

structural proteins (most) - used for adding strength to tissues or cells. fibrous protein. Examples- collagen, fibrin, keratin. Globular proteins are specialized structural proteins. Globular- Examples hormones, antibodies hormone based enzymes and steroids
Functional protein -highly chemical active molecule. (Enzymes are an example)

79
Q

Buffers

A

Weak acids or bases. They do not completely ionize in water. They stabilize the solution. Most common buffer system in medicine - Bicarbonate. (body PH is 7.4)

80
Q

Bases

A

Alkaline compound, freely releases OH ions into the water, electrolyte. Example sodium hydroxide

81
Q

Nucleic Acid

A

Largest molecule in the body. Composed of C, H, O, N, P. Found in DNA, RNA, ATP. Formed through long chains of nucleotides

82
Q

Synthesis reaction

A

New and more complex chemicle is made by combining smaller molecules . X + Y -> XY. An example a protein molecue. Formed through amino acids. This is an anabolic process. Seen with growth and repair of tissues

83
Q

Decomposition reaction

A

A single chemical is broken into multiple chemical units. XY -> X+Y. An example is glycogen is broken down to release glucose molecules. (Glycogen is found in the liver and muscles). Seen in digeston

84
Q

What is a Gene make up

A

Sequence of nucleotides that carries information to make one peptide chain

85
Q

Acids

A

H+ donor. Freely releases H into water, electrolyte. Example NaCl

86
Q

Factors influencing chemical reactions

A

concentration of chemicals, temperature of environment, activation energy, presence of a catalyst.

87
Q

Exchange Reaction

A

Certain atoms are exchanged between molecules. ATP is an example. The terminal phosphate is moved

88
Q

ATP Chemistry

A

ATP is the energy currency of cells, ATP is an RNA nucleotide. Adenine with two phosphate groups attached. Energy is stored in the phosphate bonds

89
Q

Metabolism

A

The complex , interrelated chemical processes that make life possible. Two components - anabolism and catabolism

90
Q

Neutral fats

A

They are a lipid made of three fatty acids and a glycerol molecule. They are triglycerides (3 fatty acids).

91
Q

Phospholipids

A

Lipids made up of two fatty acids, glycerol and a phosphate group. Lipid Bilayer- surrounded by water

92
Q

Eicosanoids-

A

Made up of 20 fatty acids in a ring structure

93
Q

Fatty Acid

A

A lipid with a chain of carbon atoms with one or two hydrogen atoms.
most abundant in the body, provide more than twice the energy of carbs
**Saturated fatty acids- found in butter and lard
**Unsaturated fatty acids- derived from plants (corn oil, olive oil)

94
Q

Monosaccharide formula

A

Chemical formula is C6H12O6

Anatomy 1 (11 decks)

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