Anatomy Lecture Chapter 2

Front 1

Matter (define)

Back 1

Has mass and occupies space

Front 2

3 states of matter

Back 2

Solid, liquid, and gas

Front 3

Nucleus (Atomic structure)

Back 3

-protons (p+), positively charged

-neutrons (n0), neutral no charge

Front 4

Identify the main chemical elements of the body & know their symbols.

Back 4

Oxygen- O

Carbon- C

Hydrogen- H

Nitrogen- N

Front 5

Describe trace elements

Back 5

Vital for maintaining health. Insufficient intake can cause nutritional deficiency.

Ex) iron, iodine, fluoride

Front 6

Describe the charge, mass and relative locations of protons, neutrons, and electrons

Back 6

D

Front 7

Interpret diagrams of atoms depicting electron shells.

Back 7

D

Front 8

Explain how isotopes of an element are formed.

Back 8

F

Front 9

Describe how a radioactive isotope is different from a nonradioactive isotope.

Back 9

Radioactive- unstable and emit radiation at a constant rate. (Half live and lose energy overtime.)

Nonradioactive- stable and by there own incapable of emitting energy.

Front 10

Distinguish among the terms: atomic number, mass number, and atomic weight.

Back 10

Atomic number- number if protons in the nucleus of an atom.

Mass number- number of protons and number of neutrons

Atomic weight- average weight of an atom of an element

Front 11

Use the periodic table to determine an elements atomic number and atomic weight.

Back 11

D

Front 12

Compare and contrast the terms: molecule and compound, and provide examples.

Back 12

Molecule- when 2 or more atoms share electrons.

Compound- contains atoms of 2 or Moore different elements.

Front 13

Relate the number of electrons in the valence shell to an atom's chemical stability and its ability to form chemical bonds(ionic and covalent)

Back 13

D

Front 14

Describe the formation of cations and anions.

Back 14

Cations- positively charged ions

Anion- negatively charged ions

Front 15

Describe the formation of an ionic bond

Back 15

R

Front 16

Provide the locations of most ionic bonds in the body

Back 16

D

Front 17

Describe electrolytes and provide common examples in body fluids

Back 17

Ions dissolved in the body's fluids.

Sodium ion- Na+

Hydrogen ion- H+

Hydroxide ion- OH-

Cloride ions- Cl-

Front 18

State the distribution of covalent bonds in the body compared to ionic bonds

Back 18

K

Front 19

Describe the formation of single covalent, double covalent , and triple covalent bond

Back 19

Single covalent= 1 pair

Double covalent= 2 pairs

Triple covalent= 3 pairs

Front 20

Interpret structural formulas and molecular formulas of molecules

Back 20

J

Front 21

Compare and contrast nonpolar covalent and polar covalent bonds

Back 21

-polar (water, sugar, etc) unequal sharing-- Hydrophilic

-non polar (oil,fats) equal sharing--- hydrophobic

Ions are attracted to polar but not nonpolar compounds

Front 22

Describe the formation of hydrogen bond

Back 22

Forms when a hydrogen atom with a partial positive charge attracts the partial negative charge of electronegative atoms.

Front 23

Compare the strength of hydrogen bonds to covalent bonds

Back 23

M

Front 24

Specifically describe hydrogen bonding between water molecules

Back 24

Hydrogen bonds occur because hydrogen atoms in one water molecule are attracted to the partial negative charge of the oxygen atom in another water molecule.

Front 25

Define metabolism

Back 25

K

Front 26

Define chemical reaction

Back 26

K

Front 27

Define reactants

Back 27

K

Front 28

Define products

Back 28

J

Front 29

Define work and energy and relate these terms to cell metabolism

Back 29

K

Front 30

Describe the various forms of energy and state the law of conservation of energy

Back 30

K

Front 31

Compare and contrast endergonic and exergonic reaction

Back 31

I

Front 32

Explain the role of activation energy and catalyst (enzymes) in chemical reaction

Back 32

S

Front 33

Define synthesis

Back 33

K

Front 34

Define decomposition

Back 34

K

Front 35

Define exchange

Back 35

J

Front 36

Define reversible

Back 36

M

Front 37

Define oxidation- reduction (redox)

Back 37

D

Front 38

Distinguish between the terms solution, solvent, and solute

Back 38

X

Front 39

Discuss the physiologically important properties of water

Back 39

J

Front 40

Define the term pH

Back 40

Measures amount of H+ in solution

Front 41

Define the term acid base

Back 41

K

Front 42

Define the term salt

Back 42

M

Front 43

Compare and acidic solution to an alkaline solution

Back 43

K

Front 44

Define the term buffer and describe the importance of buffers in body fluids.

Back 44

Resist drastic changes in pH of a solution.

Weak acids / weak bases do not fully ionized so they can react to changing conditions

Front 45

Define the term organic compound

Back 45

M

Front 46

Compare and contrast dehydration synthesis reactions and hydrolysis reaction

Back 46

M

Front 47

Identify the monomers and polymers of (carbohydrates, proteins, lipids, and nucleic acids)

Back 47

K

Front 48

Describe general molecule structure of (carbohydrates, proteins, lipids, and nucleic acid)

Back 48

D

Front 49

Provide specific examples of (carbohydrates ,proteins, lipids, and nucleic acids)

Back 49

S

Front 50

Discuss physiologicalogical and structural roles in the human body of (carbohydrates, proteins, lipids, and nucleic acids

Back 50

C

Front 51

Describe the four levels of protein structure and discuss the importance of protein shape for protein function

Back 51

D

Front 52

Discuss the structure and function of enzymes in catalyzing biological reactions

Back 52

X

Front 53

Describe the structure of ATP

Back 53

J

Front 54

Explain the role of ATP hydrolysis and releasing energy for the cell.

Back 54

D