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BME 533 > Chemistry: Energy > Flashcards

Chemistry: Energy Flashcards

1
Q

Matter

A

Anything that has mass and occupies space
- weight-pull of gravity in mass
- States of Matter: Solid,Liquid, Gas

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2
Q

Energy

A
  • Capacity to for work or put matter into motion
  • Types: Kinetic, Potential
    -Energy can be transferred
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3
Q

Chemical Energy

A

Stored in bonds of chemical substances

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4
Q

Electrical Energy

A

Results from movement of charged particles

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5
Q

Mechanical Energy

A

Directly involved in moving matter

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6
Q

Radiant or electromagnetic energy

A

Travels in waves

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7
Q

Atomic structure

A
  • Protons, Neutrons, Electrons
  • P & N found in nucleus
  • E orbit the nucleus in a cloud
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8
Q

Atoms

A
  • atomic # = # of protons
  • Molecular weight = Protons+ Neutrons
  • # of electrons = # of protons
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9
Q

Isotopes

A
  • Structural variation of atoms
  • Differ in the number of neurons they contain
  • Atomic numbers same; mass numbers different
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10
Q

Atomic Weight

A

Average of mass numbers of all isotopes if an atom

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11
Q

Election configurations

A
  • the extent to which another atom interacts with others is deterred by the electron configuration
  • Filled shell = inert
  • Unfilled shell p unstable reactive
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12
Q

What types of elects are found in living organisms?

A

Unstable, reactive elements

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13
Q

Chemical bonds

A
  • Energy relationships between electrons of reacting atoms
  • electrons can occupy up to seven electron shells around the nucleus
  • electrons in valance shells
    • have the most potential energy
    • are chemically reactive
  • octet rule
    • except for the first shell atoms interact to have eight electrons in their valance shell
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14
Q

Major elements of the human body

A
  • Carbon, Hydrogen, Oxygen, Nitrogen
  • makeup 96.1% of body mass
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15
Q

Lesser elements of the human body

A
  • 9 elements make up 3.9% of body mass
  • Ca, P, K, S, Na, Cl, Mg, I, Fe
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16
Q

Trace elements in the body

A
  • 11 elements make up <0.01% of body mass
  • Cr, Cu, F, Mn, Si, Zn
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17
Q

Chemical composition of cells

A

Cells are primarily composed of macromolecules, which define the physics and chemistry of the cell

18
Q

Chemical bonds of cellular molecules

A

Water is an important chemical component of cell bonds
- polar
-water molecules form hydrogen bonds with each other
-solvent for most cellular molecules
-Reaction or product in biochemical reactions

19
Q

Mixtures

A

most matter exists as mixtures
-three types: Solution, Colloids, Suspensions

20
Q

Solutions

A

-Homogeneous mixtures
-most are true solutions in the body
- gases, liquid, solid
- Solvent: substance present in great amount
- Solute: Present in smaller amount

21
Q

Concentration of true solution

A
  • % of solute in total solution
    • parts solute per 100 parts solvent
  • milligrams per deciliter
  • molarity or moles per liter (M)
    • 1 mole of any substance contain 6.02x10^23 molecules
    • 1 mole of any element = atomic #
22
Q

Colloids

A
  • heterogeneous mixtures
  • large solute particles do not settle out
  • some undergo sol-gel transfer
23
Q

Suspension

A
  • heterogeneous mixtures
  • large, visible solutes settlers out
24
Q

Mixtures

A

-no chemical bonding between compounds
- can be separated by physical means, such as straining
- Heterogenous or homogeneous

25
Q

compounds

A
  • chemical bonding between compounds
  • can be separated only by breaking bonds
26
Q

intramolecular interaction

A
  • covalent bonds
    -noncovalent bonds
  • electrostatic attraction
  • hydrogen bonds
  • van der Waals attraction
27
Q

Intermolecular interactions

A
  • electrostatic interactions
  • Hydrogen bonds
    -van der Waals attraction
  • Hydrophobic forces
28
Q

Covalent bonds

A
  • abundant in cellular molecules
  • electrons shared
  • short length and strongest
  • single bonds (2E)
    -double bonds(4E)
  • nonpolar: equally shared electrons
  • polar: two different elements, unequal sharing
29
Q

Noncovalent bonds

A
  • ionic bonds
    -hydrogen bonding
    -van der Waals attraction
30
Q

Hydrophobic forces

A
  • molecules can be hydrophobic or hydrophilic
    hydrophilic: polar or charged that dissolve in water
    hydrophobic: nonpolar, insoluble in water
  • nonpolar surfaces tend to be pushed out of the water molecules’ network
  • hydrophobic effects stabilize biological structures
31
Q

Chemical reactions

A
  • Synthesis
  • Decomposition
  • Exchange
32
Q

Synthesis(condensation)

A

A+B -> AB
Anabolic: construct molecules from smaller units

33
Q

Decomposition(Hydrolysis)

A

AB -> A+B
Catabolic: molecules broken down into smaller units that are wither oxidized to realise energy, or used in another anabolic reaction

34
Q

Exchange(displacement)

A

AB+C -> AC+B
bonds are both broken and made

35
Q

Redox reaction

A
  • decomposition reaction
  • exchange reaction because electrons are exchanged between reactions
36
Q

Energy Flow

A

Exergonic: net release of energy
- products have less energy than reactants
- catabolic and oxidative reactions
Endergonic: net absorption of reaction
- products have more energy potential than reactants
- anabolic reactions

37
Q

Rate of reaction

A

Affected by:
- increase temperature, increase in reaction rate
- increased concentration of reactants, increase in reaction rate
- decrease particle size, increase in reaction rate
- Catalyst: increases reaction rate

38
Q

First law

A
  • there are many forms of energy: mechanical, electrical, chemical
  • in chemical reaction, energy is transformed from one to another: ∆U = q-w
  • q<0 = exothermic
  • q>0 = endothermic
39
Q

Free Energy

A

∆H = ∆G +T∆S
∆H: overall change in boding energy
∆G: Change in free energy
∆S: change in bond energy
- when ∆G <0 :exergonic, forward reaction is spontaneous
- when ∆G >0 :endergonic, reverse reaction tens to occur
- when ∆G =0 : forward or reverse reaction equally probable, living things are not in equilibrium

For A+B –> C+D
∆G = ∆Gº +RT ln{([C][D])/([A][B])}

39
Q

Second law

A

∆S1 + ∆S2 = ∆Su >0
S= entropy
S1 = entropy of the system
S2 = Entropy of surrounding
Su = entropy of universe
- if + then there’s in increase in disorder
- all spontaneous change occurs with an increase of entropy of the universe
- the sum of all entropy change for the system and the surrounding must be positive for a spontaneous process

40
Q

Enzymes

A
  • most chemical reactions require an energy input to start
    • activation energy
    • needed to overcome repulsive bonds between electrons of two molecules, break existing bonds
  • in living cells, enzymes lower the activation energy
    • hold substrates in a way that reduces activation energy

BME 533 (4 decks)

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