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HB 1 > Introduction > Flashcards

Introduction Flashcards

1
Q

What is biochemistry? What fields of chemistry does it incorporate? What is it the basis of

A

The chemistry of living organisms (molecular level)
Organic (carbon), Inorganic (metal ions), Physical, Analytical
Basis for cellular biology and biology/medicine

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2
Q

What 4 elements are considered for the biochemistry of the eye?

A

Genetics
Nutrition
Environment
Lifestyle

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3
Q

What is the extracellular matrix? What does it aid in facilitating for the cell?

A

Large network of proteins and other molecules that surround, support, and give structure to cells (in a tissue)

Cell attachment/movement
Cell communication

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4
Q

What are two cell properties that can determine cell shape? (ex: RPE)

A

Molecular makeup and cytoskeleton

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5
Q

What are the monomers of protein, carbohydrate, lipid, and Nucleic acid?

A

Amino acid
Monosaccharide
Glycerol (fatty acid)
Nucleotide

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6
Q

Is water a polar or nonpolar molecule?

A

Polar

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7
Q

Does water act as a solute or solvent?

A

Solvent

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8
Q

How does water accelerate biochemical reactions?

A

Provides ions
Act as transport medium

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9
Q

What is the opposite of dehydration?

A

Edema (fluid retention in tissues)

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10
Q

Describe the structure of water. What bonds hold it together?

A

2 hydrogen atoms and 1 oxygen atom
Bound by covalent bonds

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11
Q

Describe the structure of an atom.

A

Nucleus- positively charged, contains protons and neutrons
Surrounded by electron shell
Overall is neutral

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12
Q

Describe the distribution of charge in water.

A

Hydrogen has 1 proton and 1 electron
Oxygen has 8 protons and 8 neutrons and 8 electrons (2 in the inner shell, 6 in the outer)

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13
Q

Describe the orientation of the water molecule. (Bonds, sharing of electrons). What is the bond angle?

A

Each hydrogen atom shares an electron pair with oxygen
Polar covalent bond
Bond angle is 104.5

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14
Q

What dictates the shapes of the water molecule? What property does the bend provide water with?

A

The shapes of the outer electron orbitals of the O-atom
Polar/ dipole

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15
Q

Does the water molecules have equal sharing of electrons? If not, which atom is stronger? What is formed as a result of this sharing?

A

Unequal sharing
The oxygen atoms attracts electrons more strongly than hydrogen
Electric dipoles are formed (two positive H, one negative O)

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16
Q

What kind of bonds are between water molecules? What causes these bonds? Are these bonds strong or weak?

A

Hydrogen bond (electrostatic attraction between oxygen of one water and hydrogen of another)
The dipole character of water causes this
Weak bonds

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17
Q

Can polar and non polar mix? Can polar molecules combine and why? Can nonpolar molecules combine and why?

A

Only polar/polar and nonpolar/nonpolar mix
Polar molecules mix because they are hydrophilic (salt, ions)
Nonpolar molecules will not mix because they are hydrophobic (fat, oil)

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18
Q

Does hydrogen attract positive or negative ions? What does oxygen attract?

A

Positive H attracts negative ions
Negative O attracts positive ions

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19
Q

What are amphipathic (amphiphilic) compounds? What are some examples?

A

Contain regions that are polar (hydrophilic) and regions that are nonpolar (hydrophobic)
Ex: proteins, pigments, phospholipids of membranes

20
Q

Describe micelle formation.

A

The smallest hydrophobic area that form when the non-polar regions cluster together

21
Q

What is an example of water as a solvent and transport medium in the eyes?

A

Tears prevent dryness, protect from irritants and also transport oxygen and nutrients
Different tears have different compositions

22
Q

Where is the water content in the eye from highest to lowest?

A

Vitreous
Cornea
Sclera

23
Q

According to the Bronsted-Lowry theory are which of acids and bases are donors/ acceptors?

A

Acids are proton (H+) donors (givers)
Bases are proton acceptors (takers)

24
Q

What affects do acids have on H+ concentration and pH? Which are more biologically important: weak or strong acids?

A

Acids increase H+ concentration and lower the pH
Weak

25
Q

What affects do bases have on H+ concentration and pH? Which are more biologically important: weak or strong bases?

A

Basis decrease H+ concentration and increase the pH
Weak

26
Q

At what temperature is water equilibrium reached?

A

25 Celsius (room temp)
H2O(l) ⇄ H+(aq) + OH− (aq)

27
Q

What is the pH scale? What does it measure? What is the classification of hydrogen and hydroxide ions?

A

Expresses the acidity or alkalinity of a solution on a logarithmic scale
Hydrogen concentration
Hydrogen is acidic
Hydroxide (OH-) id basic

28
Q

How is pH calculated?

A

pH Calculation: pH = -log10 [H+ concentration]

29
Q

What are amphoteric substances? Examples?

A

Can act as acids or bases
Amino Acids- basic amine group, acidic carboxyl group

30
Q

What are the two types of buffers? What are their functions?

A

A mixture of weak acids and their salts of strong bases (or) A mixture of weak bases and their salts of strong acids.
Maintain normal pH of biological systems
Neutralize small quantities of acid or bases

31
Q

What is buffer capacity?

A

The amount of cid or base that can be added to a buffer before changing its pH

32
Q

How does blood function as a buffer? What kind of buffer system? What does it eliminate? Describe the reaction that occurs.

A

Bicarbonate buffer system (carbonate weak acid and bicarbonate conjugate base)
Eliminate CO2 and protons from plasma
H+ added to blood (ex: from lactic acid) bind to bicarbonate ion, increases carbonic acid, increases CO2 in blood plasma and lungs

33
Q

What is normal blood pH? What condition occurs when it get too low or too high?

A

7.35 to 7.45
0.2 pH units lower than normal: acidosis
Increase of pH of 0.2 and more: alkalosis

34
Q

What is the Henderson-Hasselbalch equation used to calculate? What does the value K represent?

A

PH of a buffered solution
K=equilibrium constant

35
Q

What is respiratory acidosis?

A

Increase of carbonic acid concentration as a result of asthma or pneumonia

36
Q

What are used to adjust buffers? What are two examples?

A

Acids and bases
NAOH and HCl

37
Q

Describe carbon. Atomic number? Metallic or nonmetallic? How many electrons are available to form covalent bonds? What is this called?

A

6
Nonmetallic
Tetravalent- 4 electrons available, one carbon atom can form a total of 4 covalent bonds

38
Q

Describe the orientation of the carbon atom. How many p, n , and e? What kind of attachment can they form? What is it called when carbon bonds to itself? What elements does carbon bind to?

A

6 electrons in the shell
6 protons and 6 neutrons in nucleus
Cantenation (bonds to itself)
Can form chains, branched chains, and rings
Binds to H, N, O, S

39
Q

What is the basis of all biomolecules?

A

Carbon

40
Q

What happens when carbon is combined with O and H? N and S? Phosphorus?

A

Sugars and fats form
Amino acids and proteins form
DNA and RNA (Nucleic acids), ATP, and chemical code carriers of life form

41
Q

What are the 3 main types of strong chemical bonds?

A

covalent bond (electron share, single, double, triple)
ionic bond (electrostatic attraction between two oppositely charged ions, electron transfer)
metallic bond

42
Q

What is the difference between polar covalent and nonpolar covalent bonds?

A

Nonpolar is between atoms that are the same
Polar is between atoms that are different

43
Q

What are the 4 types of non covalent (weak) interactions among biomolecules in aqueous solvents?

A

Hydrogen bonds
Ionic interactions (attraction and repulsion)
Hydrophobic interactions
Van der Waals interaction (close proximity)

44
Q

What are intermolecular forces? What are they defined by? Give and example.

A

Interaction between molecules (nonbonding)
Functional groups define the type and strength of interactions
Ex: Hydrogen bonds are interactions between an electronegative atom (O or N) and a hydrogen atom (H)

45
Q

What is the difference between intramolecular and intermolecular forces? Which are weak, which are strong? Give 3 examples of each.

A

Intramolecular is within a molecule, strong, ex: covalent, ionic, metallic
Intermolecular is between 2 molecules, weak, ex: hydrogen, dipole-dipole, London dispersion

46
Q

What are functional groups? What do they participate in? What atoms do they include?

A

Groups of atoms that contribute to the chemical characteristics of a molecule and their chemical reactions.
Participate in predictable reaction
Can contain O, N, S, and P

HB 1 (6 decks)

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