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Bio 12 > Quiz 1 - Biochem > Flashcards

Quiz 1 - Biochem Flashcards

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1
Q

What is Biochemistry?

A

A field that bridges bio and chem, studying the chemistry of the molecules that make life possible

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2
Q

What are the chemical foundations of life?

A

Carbon, Hydrogen, Nitrogen, Oxygen, Phosphorus, Sulfur

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3
Q

What do the six important elements provide?

A

Provides the underlying structure of the biological molecules (carbohy, proteins, lipids, nucleic acids)

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4
Q

Explain the classifications for InTRAmolecular bonds

A

-Covalent Bonds (sharing); polar (unequal), non-polar (equal)
-Ionic Bonds (transfer)

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4
Q

What are organic molecules?

A

Organic molecules are CARBON BASED, (involve carbon atoms bonded to each other and to Hydrogen (also maybe N,O,P,S)

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5
Q

What are chemical bonds?

A

The attraction between atoms

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6
Q

What are the types of chemical bonds

A

-InTRAmolecular bonds (within mol)
-InTERmolecular bonds (between mol)

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7
Q

What is the difference between Covalent and Ionic Bonds?

A

Covalent bonds involves the sharing of electrons to achieve stable valence shells, and this is between non-metals. Whereas Ionic bonds involves the transfer of electrons between atoms to achieve stable valence shells. metal-nonmetal.

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8
Q

Define Electronegativity

A

A measure of how strongly an atom attracts electrons.

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9
Q

What are the electronegativity rules?

A

If the electronegativity difference is:
0 - 0.5 = non-polar cov
0.5 - 1.7 = poalr cov
> 1.7 = ionic

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10
Q

What factors determine polarity?

A
  • Geometry; sym vs asym
  • Bond Polarity (elecneg diff)
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10
Q

Explain a water molecule in terms of polarity

A

in a water molecule, the oxygen atom is much more electronegative than the hydrogen atom, thus the electron pair is pulled more towards oxygen, making the O partially negative, leaving the H partially positive.

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11
Q

Why is Polarity important in bio?

A

-It affects physical properties of a substance - eg. solubility “LIKE DISSOLVES LIKE”
- Determines strength and type of intermolecular attraction between molecules

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12
Q

How do you determine polarity?

A

It depends on bond polarity and molecular shape
-Sym arrangement of polar bonds will result in a nonpolar mol (dipoles will cancel)
-asym arrangement of polar bonds will result in polar mol

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13
Q

explain the number of bonds an atom forms

A
  • Relates to the number of electrons needed to fill the valence shell
    Single = 1 shared pair of val elec
    Double = 2 shared
    Triple = 3 shared
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14
Q

Do ionic bonds have structural diagrams? Why or why not?

A

Ionic compounds do not share electrons, there is no covalent bonds- so NO structural diagrams

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14
Q

How is Lewis-d-d diff from bohr?

A

It only shows the valence electrons

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15
Q

What are the type of INTERmolecular bonds?

A

-London Forces (van der)
-Dipole-dipole
-Hydrogen Bonds

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16
Q

Give 4 points to explain INTERmolecular bonds

A

-Bonds BETWEEN molecules
-Responsible for many biological properties
-Weaker than intramolecular bonds within molecules
-Sometimes referred to as “van-der-waals interactions” (distance-dependent

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17
Q

Explain London forces

A
  • Weakest intermolecular force
    -Due to temporary equal distribution of electrons as they randomly move about nuclei forming temporary dipoles
    -only forces that hold non-polar molecules together
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17
Q

Explain Dipole-dipole interactions

A

-Stronger than London Forces (weaker than ionic of covalent bonds)
-partial positive of one molecule attracts partial negative of adjacent molecule
-only has a significant effect if molecules are close together

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18
Q

Explain hydrogen bonds

A

-Strongest force
-due to dipole-dipole forces that form between partially positive hydrogen of one polar molecule and the partially negative atom (usually N, O or F) of an adjacent polar molecule

19
Q

What is the chemistry of water?

A

-Colourless, odourless, tasteless
-Exists as a solid, liquid, and gas at normal temperatures
-Highly polar

20
Q

What is the difference between hydrophilic and hydrophobic

A

Hydrophilic means water LOVING, whereas hydrophobic is the opposite (non polar mol)

20
Q

What are some bio significances of water

A

-Help control body temp
-Keeps eyeballs moist
-Lubricates joints
-required for photosynthesis

20
Q

What are the unique properties of water?

A

-Water is a versatile solvent
-Water clings
-Water absorbs heat
-Ice floats

21
Q

Explain how water is a versatile solvent

A

-More substances dissolve in water than in any other liquid
-“Like dissolves like”
-Water can dissolve ionic compounds; hydration shells

22
Q

Explain how water clings

A

theres 2 types
COHESION - water mol cling to other water mol; result in surface tension

ADHESION: Water mols h-bond with other polar mols; result ; capillary action.
Overall; water clings through h-bonding

23
Q

Explain how water absorbs heat

A

Water can absorb a lot of heat without a significant temperature increase because the heat first goes into breaking hydrogen bonds. Only after these bonds are disrupted can the kinetic energy of the water molecules increase, leading to a rise in temperature.

24
Q

What is a specific heat capacity?

A

Amount of heat required to raise or lower the water temperature by 1 degree. Water has a HIGH SHC

25
Q

What is the bio sig of water having a high heat capacity?

A

-water temp is very stable even when air temp is not

-since organisms are made of mostly water, then they too resist temp change because of its high specific heat capacity

26
Q

SHC results in evaporative cooling; what is this?

A

-as liquid evaporates, surface that remains behind cools down

bio sig:
global climate is moderated
keeps leaves cool as water evaporates from leaves
cools organisms that pant
cools organisms that sweat

27
Q

Explain the differences in water and methane

A

Water is polar, methane is non-polar. This means water absorbs more heat before changing state (h-bonds)
Water has a higher heat of vaporization (energy absorbed as it changes from a liquid to vapour)

28
Q

Explain how ice floats

A

solid water is less dense than liquid water (one of few substances that are less dense as a solid than a liquid) so ice floats.

29
Q

How does water become ice; explain density.

A

at 0 degrees, kinetic energy decreases and molecules become locked in a “crystalline lattice structure” with each water molecule bonding to 4 partners. This bonding structure keeps the molecules at “arm’s length” - far enough apart to make ice ~10% less dense than liquid water

29
Q

What would happen if ice was more dense than water?

A

ice would freeze at the bottom of oceans, making ecosystems die.

30
Q

What so special about carbon?

A

-Great ability to form complex mol (proteins, DNA, carbohy)
-Carbon has 4 valence electrons, maiing it vv compatible

31
Q

what are the major atomic components of organic mols

A

Carbon, Hydrogen, Nitrogen, Oxygen

32
Q

What is the history of organic chem?

A

Prevailing early belief; VITALISM - a “life-force” outside the realm of physics or chemistry was responsible for the processes of life; believed that only living organisms could produce organic compounds because chemists could not artificially synthesize organic compounds

33
Q

what is Urea

A

a nitrogen-containing compound found in urine
-produced when there is an excess of amino acids in body, synthesized in liver->kidney

34
Q

Who was the german chemist?

A

Wohler. he “accidentally” made urea (an organic compund) from inorganic salts

35
Q

Who was stanley miller?

A

a man who perfromed a classic experiment in which he found that organic molecules could arise spontaneously under conditions thought to have existed on early Earth.

36
Q

what were the scientists’ results?

A

Organic molecules can be made from abiotic (non-living, inorganic) sources

37
Q

What is mechanism?

A

the view that physical and chemical laws govern all natural phenomena

38
Q

What are the four types of carbon skeletons?

A
  1. Length
  2. Branching
  3. Double bond position
  4. Presence of rings
39
Q

What are hydrocarbons?

A

-Combos of C & H
-Non polar (not soluble in h2o; hydrophobic)
-Stable
-Very little attraction between molecules
Ex: Methane

40
Q

Explain hydroxyl

A
  • OH
    -organic comp w/ OH = alcohols
    -Polar due to elecneg O
    -names typically end in -ol
41
Q

What are the six functional groups?

A

-Hydroxyl
-Carbonyl
-Carboxyl
-Amino
-Sulfhydryl
-Phosphate

42
Q

Explain Carbonyl

A

C=O
- If C=O at end mol = aldehyde
- If middle = ketone

43
Q

Explain Sulfhydryl

A
  • SH
    -THIOLS
    -stabilize the structure of proteins
43
Q

Explain Carboxyl

A
  • COOH
  • C=O & single bond to OH
    -Polar
    -ACIDS
43
Q

Explain Amino

A
  • NH2
    -Nitrogen w/ 2 H
    -AMINES; polar
44
Q

Explain phosphate

A

-PO4
-highly polar
-ATP
-ORGANIC PHOSPHATES

Bio 12 (2 decks)

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