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BIOC 3021 EXAM 1 REVIEW SHEETS Questions with 100% Correct Answers
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BIOC 3021 EXAM 1 REVIEW SHEETS Questions with 100% Correct Answers What are the six most common elements present as covalent components of bioorganic compounds? - H, O, N, C, S, P, Cl What are covalent bonds, and how strong and permanent are they relative to other bonds in living organisms? - ...

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  • December 7, 2024
  • 43
  • 2024/2025
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BIOC 3021 EXAM 1 REVIEW SHEETS

Questions with 100% Correct Answers


What are the six most common elements present as covalent components

of bioorganic compounds? - ✔✔H, O, N, C, S, P, Cl

What are covalent bonds, and how strong and permanent are they relative

to other bonds in living organisms? - ✔✔Covalent bonds are the sharing of

electrons between two species. Non polar covalent bonds are the strongest

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

combinations of atoms are involved in these two kinds of covalent bonds? -

✔✔Polar covalent bonds: The EN differs (C-O bonds)

Non-polar covalent bonds: En is identical or is very similar (H-H bonds)

What are common ionic elements in biological systems? What happens to

ionic substances in the aqueous environment of living organisms? What

are the properties of the ionic bonds that occur between inorganic ions or

between organic ions? - ✔✔Common ionic elements: Na and Cl

In aqueous environments ionic substances dissociate



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,Inorganic compounds form ionic bonds that have high melting points that

are made up of a single element or compound that does not include carbon

or hydrogen.

What are hydrogen bonds? What organic structures are involved in

hydrogen bonding? What is the importance of hydrogen bonding in living

organisms? - ✔✔Hydrogen bonds are polar bonds that have a partially

positive H interacting with a partially negative element (like O or N).

Important because they are essential for protein structure, binding of

enzymes to substrate and they hold the DNA helixx together.

What are two types of nonpolar bonds? Why do nonpolar molecules

aggregate together in water? - ✔✔Van der waals forces and hydrophobic

interactions

Van der Waals forcesCaused by induced electrical interactions between

closely approaching atoms

E clouds fluctuate together to "fit together"

Strength depends on size of atoms and the distance

Bigger e- clouds from stronger interactions

Strength is inversely proportional to the 6th power of distance

Atoms need to be 2nm apart

Hydrophobic Interactions

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©JOSHCLAY 2024/2025. YEAR PUBLISHED 2024.

,These bonds form due to exclusion of water from groups of non polar

molecules

Water molecules prefer each other (strongest interactions)

Forces nonpolar molecules together

Hydrophobic molecules are not really attracted to each other, they just

herded together by water so that the maximum number of water-water

interactions can form

Water molecules push hydrophobic molecules together so that fewer water

molecules need to be near hydrophobic molecules, water water H bonding

can be maximized

What is pH and how does it relate to the molarity of hydrogen ions in

solution? - ✔✔pH is the numerical value of -log[H+]. It describes the

solutions acidity It is inversely related to the hydrogen ion concentration. So

if pH decreases then H ion increases tenfold.

What is a strong acid? What is the percent dissociation of a strong acid in

water? When a strong acid is present in water, why are the molarity of the

strong acid and the molarity of the hydrogen ion the same? - ✔✔A strong

Acid completely dissociates in water. The concentrations of Hydrogen ion

and acid are equal since it dissociates completely in an aqueous

environment.

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©JOSHCLAY 2024/2025. YEAR PUBLISHED 2024.

, What is a weak acid, and why are weak acids not completely dissociated?

Why are the molarity of the weak acid and the molarity of the hydrogen ion

not the same? If a 0.1 M solution of a weak acid is 10% dissociated, what is

the molarity of hydrogen ions? - ✔✔Weak Acid does not dissociate

completely in water. Molarities are not the same due to the lack of complete

dissociation.

0.1M x (10/100)= 0.01 M

What is a buffer solution? Why is a mixture of a weak acid and its

conjugate base needed to give good buffering? Why doesn't a solution

containing just a weak acid serve as a buffer? Why don't strong acids serve

as buffers? - ✔✔A buffer solution consists of a weak acid and its conjugate

base equilibrium in an aqueous solvent. It can resist changes in pH when a

strong acid or strong base is added. Can't have just one because then the

equation would only go one way. A strong acid can't be a buffer because it

ionizes completely.

Write the Henderson-Hasselbach equation. What are the definitions of pH,

pKa and log A-/HA? Why do all weak acids give the same shaped titration

curve? At what pH does a weak acid and conjugate base combination give

the best buffering? If a weak acid has a pKa of 5 what is the pHwhen the

weak acid is 10%, 50% and 90% titrated with NaOH? - ✔✔pH=pKA+log[A-
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