Biochemistry Flashcards

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1
Q

Chemical Fundamentals

A

Living things are composed of matter

Definition: Matter is anything that has mass and occupies space

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2
Q

Atom

A

Smallest unit of matter composed of:

  • protons
  • neutrons
  • electrons
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3
Q

Isotopes

A

elements of an atom with the same number of protons but different number of neutrons
ex. carbon, a major constituent of living organisms has 3 isotopes ie. C12, C13, C14
C12=most abundant
C14=least abundant

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4
Q

Radioisotopes

A

isotope that decays or decomposes into smaller atoms, subatomic particles of energy.
ex. C14 is radioactive breaks down to N14
Definition: Half-life is the time it takes for one half of the nuclei in a radioactive sample to decay

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5
Q

Uses of Radioisotopes

A

Radiometric dating

nuclear medicine for diagnosis and treatment

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6
Q

Two main types of chemical bonding

A

Intra-molecular forces (forces WITHIN the molecules)

Inter-molecular forces (forces BETWEEN molecules)

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7
Q

Intra-molecular forces

A

Two types:

Ionic bonds, and covalent bonds

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8
Q

Ionic bond

A

bond between atoms that have lost or gained electrons and have become charged

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9
Q

Ions

A

Charged atoms

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10
Q

Cation

A

Ion that is negatively charge

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11
Q

Anion

A

ion that is negatively charged

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12
Q

Covalent bond

A

bonds formed when atoms share one or more pairs of valance electrons
They can be either polar or non-polar

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13
Q

Electronegatively

A

measure of an atom’s ability to attract a shared electron pair when it is participating in a covalent bond
ex. En for noble gases is 0

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14
Q

Symmetrical molecules

A

Bonds are all polar are nonpolar

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15
Q

Asymmetrical molecule

A

are non polar if all the bonds are non polar, and they are polar if at least one bond is polar

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16
Q

Inter-molecular bonds

A
chemical bonds between molecules
weaker then intramolecular bonds
THREE TYPES:
London dispersion forces
Dipole-dipole forces
Hydrogen bonds
17
Q

London dispersion forces

A

weakest bond, they exist between all molecules. Only forces between noble gases and non polar molecules

18
Q

Dipole-dipole forces

A

hold polar molecules together

19
Q

Hydrogen bonds

A

forms between a partial positive charged H atom with a partially negative charged O,N and F atom in another molecule
This bond is the strongest and most biologically significant, and responsible for many unique properties of water

20
Q

Water

A

Very important to life. Without we wouldn’t exist
All organisms have water
Ex. control body temp, keep eyeballs moist, lubricate joints

21
Q

Water properties

A
  • colourless, odourless, and tasteless
  • can exist as a solid, liquid, and gas in temp range found on earth
  • chemical composition H2O
  • It’s polar due to - polar bond & asymmetrical shape
22
Q

Water the versatile solvent

A
  • more substances dissolve in it
  • Most chemicals of biological interest dissolve in water
    ex. NaCl dissolve in water
    NaCl is an ionic compound, it dissociates in water i.e breaking of the ionic bond
    Polar molecules = dissolve in water
23
Q

Hydrophobic molecules

A

non-polar molecules that are not strongly attached to water

24
Q

Hydrophilic molecules

A

polar or charged molecules that are strongly attracted to water

25
Q

Miscible

A

describes liquids that dissolve into one another

ex, ethanol (alcohol in beverages) and ethylene glycol (alcohol in antifreeze) = miscible in water

26
Q

Immiscible

A

describes liquids that form separate layers instead of dissolving into one another
ex. oil and gas = immiscible with water