Biochemistry

Question 1

Chemical Energy

Answer 1

• main type of energy

Stored in bonds of chemical substances.

Question 2

Radioisotopes

Answer 2

Are isotopes that decompose to more stable forms.

Question 3

Radioisotopes

-Atom loses various subatomic particles

Answer 3

Sometimes loss results in an isotope becoming a different element.

Question 4

Radioisotopes

-As isotopes decay, subatomic particles that are being given off release some energy…

Answer 4

This is called radioactivity

• can be detected and measured with a scanner.

Question 5

Three basic types of mixtures…

Answer 5

Solution

Colloid

Suspension

Question 6

Solutions

Answer 6

Solute partials are very tiny, do not settle out or scatter light

Example: mineral water, sugar water

This a homogeneous mixture

*compounds don’t separate (layers) over time when left standing

Question 7

Colloid (mixture)

Answer 7

Solute partials are larger than in a solution and scatter light; do not settle out.

Example: jell-o, whole milk and shampoo

Considered heterogenous mixture

*compounds don’t separate (layers) over time

Question 8

Suspension (mixture)

Answer 8

Solute particles are very large, settle out, and may scatter light.

Examples: oil shaken in water, muddy water, and blood

Considered a heterogeneous mixture

*compounds separate (layers) when left standing over time.

Question 9

What kind of bonds form between water molecules?

Answer 9

Hydrogen bonds

**But each molecule itself has a covalent bond

Question 10

Oxygen and Argon are both gasses. Oxygen combines readily with other elements, but Argon does not. Why?

Answer 10

Argon’s valence shell is full. So non-reactive

Question 11

Assume imaginary compound XY has a polar covalent bond. How does it’s charge distribution differ from that of XX molecules?

Answer 11

Electrons would spend more time in the vicinity of the more electronegative atom in XY , whereas electrons in XX would orbit both X atoms to an equal extent.

Question 12

Covalent bond

Answer 12

Electron sharing that produces a molecule in which shares electrons occupy a single orbital common to both atoms.

Question 13

Chemical bonds

Answer 13

Energy relationships between electrons of exacting atoms.

* not actual physical structures

Question 14

Octet Rule

Answer 14

Atoms want 8 electrons in their valence shell.
(Exception of small atoms like H and He they only want 2)

Wanting 8 electrons is the driving force of chemical reactions
(Noble gases have full octets and are less reactive)

Question 15

Ionic Bonds

Answer 15

Involve transfer of valence shell electrons from one atom to another, resulting in ions

Question 16

Anion

Answer 16

Negative charged

• ion that’s gains one or more electrons.

Question 17

Cation

Answer 17

Positive charge

*ion that lost one or more electrons.

Question 18

Polar Covalent Bonds

Answer 18

Unequal sharing of electrons between 2 atoms, results in electrically polar molecules.

*Atoms have different electron- attracting abilities.

Question 19

Synthesis reaction

Answer 19

Building

Small particles (monomers) are bonded to form a larger, more complex molecules (polymers).

Example: amino acids join together to form a protein molecule

Question 20

Decomposition Reactions

Answer 20

Breaking Down

Bonds are broken in larger molecules, resulting in smaller, less complex molecules.

Example: glycogen is broken down to release glucose molecules.

Question 21

Salts are electrolytes. What does that mean?

Answer 21

Electrolytes are substances that will conduct an electrical current in aqueous solution.

Question 22

Which ion is responsible for increasing acidity?

Answer 22

H+

Question 23

Which ion is responsible for increasing basicity?

Answer 23

OH-

Question 24

To minimize the sharp pH shift that occurs when a strong acid is added to a solution, is it better to add a weak base or a strong base, why?

Answer 24

A weak base to act as a buffer to the strong acid.

Question 25

How does the structure of a water molecule make it and excellent solvent ?

Answer 25

Because the polarity. As a dipole it can orient itself to the end of the other molecule, causing them to dissociate or go into solution.

Question 26

Inorganic compounds

Answer 26

Water, salt, acids and bases

*do not contain carbon

Question 27

Organic Compunds

Answer 27

Carbohydrates, Fats,lipids, proteins and nucleic acids

• contain carbon (usually larger and covalently bonded)

Question 28

Which are more essential for life inorganic or organic compounds?

Answer 28

Both are equally essential

Question 29

pH scale is neutral at 7 (10^-7 H+ and OH-) what is important in to note?

Answer 29

As H+ ions decrease acidity increase (10-0 is most acidic)

And as OH- ions decrease basicity increase (10-1 is most basic)

Question 30

Dehydration Synthesis

Answer 30

Monomers are joined by removal of OH from one monomer and removal of H from the other at the site of bond formation.

• water is removed to from new bond
• covalently links monomers

Question 31

Hydrolysis

Answer 31

Monomers are released by the addition of a water molecule, adding OH to one monomer and H to the other.

*water is added to brake a polymer

Question 32

What occurs when fats are digested in your small intestine?

Answer 32

Decomposition reaction

Question 33

What specific name is given to decomposition reactions in which food fuels are broken down for energy?

Answer 33

Oxidation- reduction (redox) reactions.

Question 34

Phospholipid

Answer 34

Important in cell membrane structure “membranes” “soap bubbles”

*heads are hydrophilic and tails are hydrophobic

Question 35

Denaturation

Answer 35

Globular proteins unfold and what is their function

Example: cooking an egg dramatically changes its consistency

Question 36

Nucleic acids

Answer 36

Are the largest molecule in the body they are polymers made up of monomers called nucleotides

Two classes:
Deoxyribonucleic acid and ribonucleic acid

Question 37

ATP

Answer 37

Chemical energy released when glucose is broken down and captured

ATP directly powers chemical reactions in cells and it is the bodies energy currency

Question 38

Property of matter includes

Answer 38

Matter can exist in solid, liquid, or gaseous state.

Question 39

Something with a pH of 6 would have fewer or more H+ ions

Answer 39

Have more H+ ions than OH- ions

Question 40

T or F, isotopes have the same number of protons but differ in the number of neutrons they contain.

Answer 40

True

Question 41

T or F; atoms of any given element will differ from those of all other elements and provide its unique physical and chemical properties.

Answer 41

True

Question 42

Best way to define physiology

Answer 42

The study of how the body parts work and carry out their life-sustaining activities.