Module 2: Foundations Of Chemsitry And Biology Flashcards

1
Q

Homeostasis Overview

A
  • A relatively stable state of equilibrium
    -Self-regulating process by which biological systems tend to maintain stability. Necessary for maintaining life, function, repair and HEALTH.

Go to page 7 of Notably to look at drawings

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2
Q

Negative Feedback Loop

A

NFL
Stimulus —> Sensor —> Control —> Effector
Body Temp. exceeds 37 degrees C —> Nerve cells in skin and brain —> Temp. Regulatory center in brain —> sweat glands throughout the body

Look at page 9 on notably

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3
Q

Positive Feedback Loop

A

PFL
- When the body amplifies a change in a variable is will increase or decrease to further the normal dynamic or homeostatic range
Example: Blood clotting and child birth

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4
Q

List the Levels of Organization

A

Atoms - Molecules/compounds - Organelles - Cells - Tissues - Organs - Organ systems - Organism

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5
Q

What are Atoms?

What are molecules?

A
  • Smallest fundamental form of matter (hydrogen, oxygen, carbon, calcium, and phosphorus)
  • When two or more atoms of the same type are chemically bonded together (O2) COMPOUNDS = two or more atoms of different types are chemically bonded (H2O)
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6
Q

What are Organelles?

What is Cellular?

A
  • Sub-cellular structures that preform specific functions in the cell. (Nucleus, mitochondria, endoplasmic ret., ribosome, cell membrane)
  • Most basic level of organization in the body, basic structural levels of living matter, capable of reproducing itself (Neurons, myocytes, epithelial cells)
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7
Q

Define tissue and the four main types of tissue.

A
  • Group of cells organized together that perform a similar function.

Four types:
Neuronal tissue,
Muscular tissue,
Connective,
Epithelial

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8
Q

Define Organs, and Organ system.

A
  • When two or more tissues work together to perform a specific function. Most organs contain all four tissues (heart, lung, small intestine)

-When two or more organs work together to preform a specific function (Respiratory, Urinary etc.)

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9
Q

Define Organism within the levels of organization.

A

Preforming all physiological functions

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10
Q

Differentiate Individual, population, and community.

A

Individual is the basic unit of ecological study, a population is a group of individuals of the same species living in a specific area, and a community comprises all the different populations that live together in a defined area.

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11
Q

Differentiate Ecology, Ecosystem, Biome, and Biosphere.

A

Ecology- Scientific discipline within biology that studies the relationships between living organisms and their interactions with their nature

Ecosystem- Community comprised of biological, physical, and chemical components, considered as a unit.

Biome - An area classified according to the species that live in that location

Biosphere - The region of earth that encompasses all living organisms: plants, animals and bacteria.

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12
Q

*Fluid compartment
Extracellular Fluid (ECF)

A

Fluid outside of the cell, fluid within the BV

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13
Q

*Fluid compartment
Intercellular fluid (ICF)

A

Fluid in the cell (surrounding cells)

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14
Q

If any body fluid such as Na+/K+/Cl- increases or decreases in the blood plasma it will then… What?

A

Increase or decrease within the interstitial fluid to match the blood plasma

EXAMPLE: Decrease in blood plasma will decrease interstitial fluid and effect the function (and fluid volume) of a cell (intracellular fluid)

Decrease in Ca2+ in blood plasma, decrease interstitial fluid = muscle spasms in skeletal muscle

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15
Q

ISF Composition (Plasma)

A

Na+ (sodium) *
Cl- (chloride) *. Increase Na+, Cl-, Ca2+
Ca+2 (calcium) *. Decrease K+, P
HCO3- (bicarbonate)

OUTSIDE OF BANANA

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16
Q

ICF Composition

A

K+ (composition) * Increase K+, P
Phosphate (-) * Decrease Na+, Cl-, Ca2+
Proteins (-)

INSIDE OF BANANA

17
Q

Of cations and anions which are positive and negative?

A

Cations are +
EX: Na+

Anions are -
EX: Cl-

18
Q

Differentiate Osmolarity and Osmolality.

A

Osmolarity - measurement of the total number of solutes in a liquid solution expressed in osmoles (Osm) of solute particles per litre of solvent (solution)
*Per liter measured (mOsm/L)

Osmolality - Measurement of the total number or solutes in a liquid solution expressed in osmoles (Osm) of solute particles per kilogram of solvent (solution)
*per kilogram (mOsm/kg)

*we want mOsm/L of plasma = mOsm/L of ISF = mOsm/L of ICF

*all come out equal (300 mOsm/L)

19
Q

Define Tonicity

A

Concentration of solute ion as compared to another solution
Ability of a solution surrounding a cell to cause that cell to gain or lose water
Movement of one solution to another solution

20
Q

Overview of osmotic pressure gradient

A

When two solutions with different osmolarities are separated by a membrane that causes water to move from across the membrane from one solution to the other
- Water moves from the solution with a LOW concentration of solutes to the solution with the HIGH concentration os solutes

21
Q

Different Tonicities
Isotonic
Hypertonic
Hypotonic

A

Isotonic -solutions have equal osmoti pressure
Hypertonic- A solution that has a higher solute concentration (higher osmolarity)
Hypotonic - A solution that has a lower solvate concentration (lower osmolarity)

*Pictures on Module 2, Pages 17-18

22
Q

Define Essential Elements

A

Required by an organism for healthy growth.

Less than 30 of the naturally occurring elements are essential to life

23
Q

What elements are most abundant?

A

CHNOPS

24
Q

What elements make up biological matter?

A

CHNO

Make up >99% of the mass of cells
- Lightest elements capable of forming one, two, three, or four bonds.

25
Q

What are bulk body elements? What are Trace elements?

A

Bulk body elements are most found in the body.

Trace elements are ones only needed in small amounts

26
Q

Describe Non reversible reactions vs Reversible reactions.

A

Non reversible reactions proceed in one direction until reactants are used. Showed with a unidirectional arrow

2H+O ——> H2O
Reactant. Product.

Reversible reactions have an equilibrium state
Shown with two parallel arrows pointing in opposite directions or a double-headed arrow.

HCO3- + H+ —-> H2CO3
<—

For more, look at example on module 2: page 22

27
Q

Describe and explain the two types of covalent bonds.

A

Polar covalent bonds have electrons unequally shared between two atoms. Bonds between atoms of elements with different electro negativity (a measure of how much the nucleus is attracted to e-)
*—>Elements with weak electronegativity: C, H
*—> Elements with strong electro negativity: N, O, P, S

*Polar bonds make molecules water soluble: Hydrophilic

Non-polar covalent bonds are equally shared between two atoms. EXAMPLE: Bonds between atoms of the same element C-C, O2
Bonds between atoms of similar electronegativity C-H
Bonds in symmetrical molecules CO2

*Non-polar bonds make molecules less-water-soluble: Hydrophobic

28
Q

Define organic molecules and biomolecules.

A

Organic molecules contain at least one C and H

Biomolecules are natural organic molecules

29
Q

Look over pages 28-30 on module 2. Have an understanding of pH/buffers/acids and bases.

A
30
Q

Look at pages 32- 37 of chemical bonding/models, configuration, conformation, and oxygen containing groups

A