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Introduction to physiology > Chemistry > Flashcards

Chemistry Flashcards

1
Q

______-is a pure substance that is distinguished from all other matter by the fact that
it cannot be created or broken down by ordinary chemical means

A

Elements

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2
Q

_______-the smallest quantity of matter that still retains the properties of an element

A

Atom

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3
Q

______-composed of subatomic particles

A

Structure of atoms

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4
Q

_____-positively charged particles found in the nucleus (center) of an atom

A

Protons

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5
Q

_____-neutral or have no charge; are also found in the nucleus

A

Neutrons

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6
Q

_____-negatively charged and exist in the orbits/shells around the nucleus.

A

Electrons

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7
Q

______-two or more atoms held together by a chemical bond.

A

Molecules

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8
Q

What type of chemical bonds is this?
_____-formed between oppositely charged ions
• When an atom loses or gains electrons, it becomes electrically charged
• Ions are charged atoms or molecules
o Examples: Sodium (Na+), Chloride (Cl-), Potassium (K+), calcium (Ca2+),
hydrogen (H+), ferrous iron (Fe2+), and ferric iron (Fe3+) are examples of
important ionic atoms in the body. Phosphate (PO43-), monohydrogen phosphate
(HPO42-), dihydrogen phosphate (H2PO4-), carbonate (CO32-), bicarbonate
(HCO3-), amino acids, and nucleotides are examples of important ionic
molecules

A

Ionic Bonds

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9
Q

What type of chemical bonds is this?

_____-form when electrons are shared between atoms

A

Covelent Bonds

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10
Q

What type of chemical bonds is this?
Covalent bonds
_____-electrons shared equally
o Example: Molecular oxygen (O2), Carbon dioxide (CO2), and triglycerides are
examples of important non-polar molecules.

A

Non polar bonds

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11
Q 
What type of chemical bonds is this?
Covalent bonds
\_\_\_\_\_\_-electrons are NOT shared equally
o Examples: Water (H2O), glucose (C6H12O6), and Urea (CO(NH2)2) are examples
of important polar molecules
A

Polar bonds

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12
Q

______-interaction between partial charges of polar molecules. In water
there is partial positive charge of hydrogens atoms and a partial negative charge on the oxygen
because oxygen strongly attracts electrons. Molecules that contain hydrogen bound to nitrogen or
sulfur can also form this type of bond with other polar molecules.

A

Hydrogen bonds

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13
Q

______-of water results in hydrogen bonds between neighboring water molecules
giving water some unique vital properties

A

Polarity

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14
Q

Vital properties:
_____-water molecules are attracted to each other and this property causes
them to exclude nonpolar molecules that cannot form hydrogen bonds with water.

A

Cohesive

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15
Q

Vital properties:
_____-the dissolving agent in a solution. Water dissolves polar chemicals,
making it a good medium for transporting biological molecules.

A

Solvent

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16
Q

Solvent:

_____-is a liquid consisting of two or more substances evenly mixed

A

Solution

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17
Q

Solvent:

_____-is the substance being dissolved

A

Solute

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18
Q

Solvent:
______-ions and polar molecules are water
soluble.

A

Hydrophilic (water loving)

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19
Q

Solvent:
_____-Non-polar molecules do not dissolve in
water.

A

Hydrophobic (water fearing)

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20
Q

Solvent:
_____-molecules that have polar and non-polar regions are
both hydrophilic and hydrophobic.
o Example: Phospholipids

A

Amphiphilic

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21
Q

Solvent:
____-quantity of solute dissolved in a volume of solution.
Ø pH: measurement of the concentration of hydrogen ions (H+) in a
solution (acidity).

A

Concentration

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22
Q

pH=

A

-log [H]

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23
Q

High acidity corresponds to a 13)____ pH

and a 14)______ concentration of H+

A

13) low

14) high

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24
Q

High 15)______________ - water requires a lot of energy to increase in temperature, and
releases a lot of energy when it cools.
o Water in blood transports heat through the body helping to stabilize body
temperature

A

15) High specific heat

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25
Q

High 16)______________ – it takes a large amount of heat to evaporate water.
o Example of sweat as a mechanism of evaporative cooling: heat is removed from
the body to provide energy for the evaporation of water from sweat.

A

16) Heat evaporation

26
Q

Chemical reaction:
______-a catabolic reaction in which a water molecule is
consumed to breaks a covalent bond in another molecule apart
§ Example: Hydrolysis of a polymer (such as the polysaccharide amylose a
common form of starch) to release a monomer (amylose is a long chain of
glucose monomers).

A

Hydrolysis

27
Q

Chemical reaction;
_____-anabolic reaction mechanism removes water to form bonds
§ Example: Opposite of above dehydration synthesis forms polymers (such
as amylose) from monomers (such as glucose).

A

Dehydration synthesis

28
Q

_____-chemicals do not contain carbon.
• Examples: Water (H2O), Sodium (Na+), Chloride (Cl-), Potassium (K+), calcium (Ca2+),
hydrogen (H+), ferrous iron (Fe2+), ferric iron (Fe3+), Phosphate (PO43-),
Monohydrogen phosphate (HPO42-), Dihydrogen phosphate (H2PO4-), Carbonate (CO32-
), and Bicarbonate (HCO3-)

A

Inorganic chemicals

29
Q

______-molecules containing carbon and hydrogen. Biological
macromolecules are important large organic molecules that contain carbon bound to hydrogen
and oxygen. Some also contain nitrogen, sulfur, phosphorus, or selenium.

• Specific macromolecules have unique three-dimensional structures that define their
functions in an organism. The macromolecules of your body recognize one another based
on their shapes.
• Most macromolecules are polymers. Polymers are made by stringing together many
smaller molecules called monomers (subunits).
o Examples: Polysaccharides are polymers of monosaccharides. Nucleic acids are
polymers of nucleotides. Peptides are polymers of amino acids.

A

Organic chemicals

30
Q

_____-includes sugars and starches

Contain carbon, hydrogen, and oxygen (1:2:1 ratio)
• Monomer = monosaccharide
• Classified according to size

A

Carbohydrates

31
Q

Classification of carbohydrates according to size:
____-one sugar, referred to as simple sugars
§ Examples: Glucose, fructose, and galactose.

A

Monosaccharides

32
Q

Classification of carbohydrates according to size:
_____-a double sugar
§ Examples: Maltose (produced from amylose), lactose (found in milk), and
sucrose (table sugar).

A

Disaccharide

33
Q

Classification of carbohydrates according to size:
____-complex carbohydrates formed by long chains of
monosaccharides
§ Examples: Glycogen (animal), amylose (starch common in plants),
cellulose (cell walls of plants).

A

Polysaccharides

34
Q

____-hydrophobic chemicals.

• Composed of mostly carbon and hydrogen with a small amount of oxygen

A

Lipids

35
Q 
Types of lipids:
\_\_\_\_\_\_-triglycerides
o A combination of glycerol and three fatty acids
o Found in fat deposits (adipose tissue)
o Source of stored energy and insulation
o Cushions organs
*Unsaturated fatty acids
*Saturated fatty acids -
A

Fat or neutral fat

36
Q

Types of Fat or neutral fat:
_____-have less than the maximum number of
hydrogen bonded to the carbons and are usually liquid at room
temperature.
Ø Examples: Most plant oils; vegetable or corn oil

A

Unsaturated fatty acids

37
Q

Types of Fat or neutral fat:
_____-have the maximum number of hydrogen bonded
to the carbons
Ø Example: Most animal fats

A

Saturated fatty acids

38
Q

Types of Fat or neutral fat:
____-composed of phosphate head (hydrophilic) and two lipid tails
(hydrophobic)
o Forms cell membranes and the myelin sheaths of neurons

A

Phospholipids

39
Q

Types of Fat or neutral fat:
_____-a 20 carbon fatty acid with a 5 or 6 carbon ring
o Examples: prostaglandins, leukotrienes, thromboxanes

A

Eicosanoids

40
Q

Types of Fat or neutral fat:
____-the carbon skeleton is bent to form four fused rings
o Cholesterol is the “base steroid” from which your body produces other steroids
o Example: testosterone, estrogen, cortisol, bile salts, vitamin D.

A

Steriods

41
Q

______- a macromolecule consisting of one or more polymers called polypeptides
constructed from monomers called Amino Acids

A

Proteins

42
Q

Proteins-a macromolecule consisting of one or more polymers called 28______
constructed from monomers called 29__________.

A

28) Polypeptides

29) Amino acids

43
Q

______-Contain C, H, O, N, and sometimes S
• There are 20 different amino acids commonly found peptides
• The arrangement and combination of amino acids makes each protein different
• Amino acids are held together by peptide bonds

A

Protein

44
Q

_____-protein’s shape is sensitive to the surrounding environment

A

Protein Shape

45
Q

What protein shape is this?

_____-order of amino acids

A

Primary structure

1*

46
Q

What protein shape is this?

____–polypeptide folded into a helix or a sheet

A

Secondary Structure

2*

47
Q

What protein shape is this?

_____-sheets and helices folded into a 3-D globule

A

Tertiary Structure

3*

48
Q

What protein shape is this?
_____-several tertiary units put together
*A slight change in the primary structure of a protein affects its ability to function
§ Example: sickle cell anemia
Denaturation-high temperature and extreme pH can cause a protein to unravel
and lose its shape

A

Quaternary structure

4*

49
Q

Types of proteins:
_____-Provides for construction materials for body tissues
o Important role in structure
o Examples: collagen, elastic fibers, keratin, actin, and myosin.

A

Fibrous Proteins

50
Q

Types of proteins:
_____-Relies on complex folded structure to function
o Plays a vital role in cell function
o Act as enzymes, hormones, transport proteins or antibodies
o Examples: enzymes (renin, amylase, carbonic anhydrase), transport proteins
(hemoglobin, albumin, transferrin), hormones (insulin, growth hormone, leptin),
transmembrane proteins (receptors, channels and transporter proteins), defense
proteins (perforin, complement proteins, and antibodies).

A

Globular proteins

51
Q

_____-polymers that function as genetic information storage molecules.

A

Nucleic Acids

52
Q

Nuclei Acids :
Consist of monomers called 36)____________ that are linked by bonds
(phosphodiester bonds) between the phosphate groups forming a sugar-phosphate
backbone

A

Nucleotides

53
Q

Nucleic Acids:

Monomers consist of______

A

5 carbons sugars
phosphate group
Nucleic base

54
Q

What are the two Types of Nucleic Acids:

A

Deoxyribonucleic Acid (DNA)

Ribonucleic acid (RNA

55
Q

what type of nucleic acids is this?
Composed of 4 types of nucleotides
§ Purines – Adenine (A) and Guanine (G)
§ Pyrimidines – Thymine (T) and Cytosine (C)
o Organized by complimentary base pairing to form a double stranded helix
§ Guanine (G) forms hydrogen bonds with 37)___cytosine __
§ Adenine (A) forms hydrogen bonds with 38)_thymine____
§ The nucleotides of the two stands are joined by hydrogen bonds

A

Deoxyribonucleic Acid (DNA)

56
Q 
Deoxyribonucleic Acid (DNA)
Composed of 4 types of nucleotides;
Purines:\_\_\_\_\_\_\_
A

Adenine (A) and Guanine (G)

57
Q 
Deoxyribonucleic Acid (DNA)
Composed of 4 types of nucleotides;
Pyrimidines:\_\_\_\_\_\_\_
A

Thymine (T) and Cytosine (C)

58
Q

Deoxyribonucleic Acid (DNA)

Organized by complimentary base pairing to form a double stranded helix:
Guanine (G) forms hydrogen bonds with 37)________

A

Cytosine

59
Q

Deoxyribonucleic Acid (DNA)

Organized by complimentary base pairing to form a double stranded helix:

Adenine (A) forms hydrogen bonds with 38)________

The nucleotides of the two stands are joined by hydrogen bonds

A

Thymine

60
Q

Ribonucleic acid (RNA)

RNA is different from DNA in that:
§ Its sugar is 39)_________ instead of deoxyribose
§ It has the base 40)_________ instead of thymine (T)
§ The most common forms such as messenger RNA (mRNA) are single
stranded polymers in contrast to the double stranded structure of DNA.

A

39) Ribose

40) Uracil

Introduction to physiology (9 decks)

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