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Anatomy and Physiology 1 > Chapter 2.1 > Flashcards

Chapter 2.1 Flashcards

1
Q

Element

A

The simplest form of matter to have unique chemical properties.

(An atom is the smallest amount of an element)

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2
Q

Atom

A

The smallest amount of an element; Can’t be further divided

Made of protons, neutrons, and electrons

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3
Q

Molecule

A

Two or more atoms that are chemically joined together

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4
Q

Compound

A

A substance that contains more than one element

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5
Q

Covalent bond

A

Atoms bonded by sharing electrons

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6
Q

Ionic bond

A

Electrons completely transferring from one atom to another

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7
Q

Six most abundant elements in the human body

A
  1. O - Oxygen 65%
  2. C - carbon 18%
    3. H - Hydrogen 10%
  3. N - Nitrogen 3%
  4. Ca - Calcium 1.5%
  5. P - Phosphorus one percent
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8
Q

Six lesser elements of the human body

A
  1. S - Sulphur
  2. K - potassium
  3. Na - Sodium
  4. Cl - Chlorine
  5. Mg - Magnesium
  6. Fe - Iron
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9
Q

Structure of an atom

A

 nucleus at the center made of protons (p+) And neutrons (n0), Surrounded by one or more clouds of electrons on electron shells

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10
Q

Atomic mass

A

Atomic mass = Proton+neutron

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11
Q

Proton

A

A single positive charge that weighs approximately one atomic mass unit

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12
Q

Neutron

A

Has no charge, weighs approximately one atomic mass unit

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13
Q

Electrons

A

Tiny particles with a single negative charge and very low mass. They determine the chemical properties of an atom.

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14
Q

Electron shells (energy levels)

A

Where are electrons swarm about the nucleus in concentric regions.

In atoms dealing with human physiology there are not more than four

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15
Q

Valence electrons

A

Electrons of the outer most shell.

Determine the chemical bonding properties of an atom

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16
Q

Isotopes

A

Variety of the same element that differ from one another only in number of neutrons – so also atomic mass. Behave the same chemically

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17
Q

Deuterium

A

Isotope of hydrogen atom with one proton one neutron (2H)

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18
Q

Tritium

A

Isotope of Hydrogen atom with one proton and two neutrons (3H)

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19
Q

Atomic weight

A

Relative atomic mass: accounts for the fact that an element is a mixture of isotopes, so slightly different than atomic mass

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20
Q

Radioisotopes

A

Unstable isotopes that decay two more stable isotopes by giving off radiation

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21
Q

Radioactivity

A

The process of decay of unstable isotopes

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22
Q

Ionizing radiation

A

High energy radiation eject electrons and energy from atoms, converting atoms to ions

Ions Destroy molecules and produces dangerous free radicals and ions in human tissues

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23
Q

A High dose of ionizing radiation is

A

Fatal

24
Q

In lower doses of ionizing radiation, it can be what?

A

Mutagenic – causing mutations in DNA

Carcinogenic Dash triggering cancer as a result of mutation

25
Q

Examples of ionizing radiation

A

Ultraviolet raise, x-rays, and alpha beta and gamma particles produced by nuclear decay

26
Q

Alpha particle

A

Two protons, two neutrons, too large to penetrate skin, but dangerous when emitted by radioisotopes that have gotten into the body

27
Q

Beta particle

A

A free electron. 

28
Q

How do isotopes of the same element differ from each other?

A

They have a different number of neutrons so a different atomic mass

29
Q

How do radioisotopes differ from other isotopes?

A

They are unstable isotopes and decay to more stable isotopes by giving off radiation

30
Q

Clinical relevance of ionizing radiation

A

It destroys molecules and produces dangerous free radicals and ions in human tissues. can be fatal in high doses. In low-doses it can be Mutagenic in carcinogenic

Ex:Strontium 90 released by nuclear accidents settles onto pastures and contaminates cows milk. In the body behaves complete like calcium, becoming incorporated into the bones, where it emits beta particles for years.

31
Q

Three forms of ionizing radiation

A

Ultraviolet rays, x-rays, and radiation produced by nuclear decay: alpha particles beta particles and gamma rays

32
Q

Difference between the physical and biological half-life of a radio isotope

A

Physical half-life: time required for 50% of Adams to decay two more stable isotope

Biological half-life: time required for half of it to disappeared from the body by radioactive decay and excretion

33
Q

Clinical relevance of difference between physical and biological half life

A

Physical half-lives can be really really long. Biological half life’s can be much shorter because they exit the body

34
Q

The difference between an ion and an atom is:

A

Atoms are neutral particle; ions are positively or negatively charged particle

35
Q

How ions form

A

Elements with 1-3valence electrons give them up, and those with 4-7 electrons gain more. If an atom of the first kind is exposed to an atom of the second, electrons may transfer from one to the other and turn them both into ions (ionization)

36
Q

Two types of ions are:

A

Anion: the particle that GAINS electrons=negative charge

Cation: The particle that LOSES electrons= positive charge

37
Q

Example of anion

A

Sodium (Na) and chlorine (Cl) meet. One electron transfers from Na to Cl, producing a chloride ion with a unit negative charge (Cl-)

38
Q

Example of cation

A

Sodium (Na) and chlorine (Cl) meet. One electron transfers from Na to Cl, producing a sodium ion with a unit positive charge (Na+)

39
Q

How electrolytes differ from atoms and ions

A

Electrolytes are the chemical compounds from which ions are made

(Chemical compound that produces ions when it is dissolved in water)

40
Q

Most common electrolytes

A 
Sodium (Na)
Potassium (K)
Chloride (Cl)
Bicarbonate (HCO3)
Calcium (Ca)
Phosphorus (P)
41
Q

Functions and medical relevance of electrolytes

A
  • Can detect electrical activity of muscles, heart, brain because electrolytes conduct electrical currents from organs to skin surface
  • Imbalance Can cause cramps, brittle bones, coma, cardiac arrest.
  • Electrolytes Important for:
    1. Chemical reactivity
    2. Osmosis effects
    3. Electrical effects
42
Q

Free radical

A

Unstable, highly reactive chemical particles with an odd number of electrons.
Produced by: Some normal metabolic reactions, radiation, chemical such as nitrates.
Ex: superoxide anion O2-• —>dot symbolizes odd electron

43
Q

Medical relevance of free radicals

A

They quickly combine with molecules such as fats proteins and DNA, converting them into free radicals and triggering chain reactions to destroy more molecules. Ex: Free radicals can cause some forms of cancer and myocardial infarction (death of heart tissue)

44
Q

Molecule versus compound

A

Molecules: chemical particles composed of two or more atoms united by a chemical bond, either same or different.

Compound: molecules composed of two or more Different elements

45
Q

Isomers

A

Molecules with identical molecular formulae but different arrangements of their atoms.
Ex: ethanol and ethyl ether
Ethanol: MF: C2H6O, SF: CH3CH2OH
Ethyl Ether: MF: C2H6O SF: CH3OCH3

46
Q

How to determine a molecules molecular weight

A

Sum of the atomic weights of its atoms. Needed to compute measures of concentration

47
Q

What is the nature and distinguishing characteristics of ionic bonds

A

Relatively weak attraction between an anion and a cation. Easily disrupted in water as when salt dissolves

48
Q

Covalent bond and types

A

Sharing of one or more pairs of electrons between nuclei

  1. Single covalent
  2. Double covalent
  3. Triple covalent
    And
    -Nonpolar covalent
    -Polar covalent
49
Q

 Single covalent bond

A

Sharing of one electron pair

50
Q

Double covalent bond

A

Sharing of two electron pairs.

Ex: carbon atoms
carbon and oxygen atoms
carbon and nitrogen atoms

51
Q

Nonpolar covalent

A

Covalent bond in which electrons are equally attracted to both nuclei.

52
Q

Polar covalent bond

A

Electrons are more attracted to one nucleus than the other, resulting in slightly positive and negative regions in one molecule. Maybe single or double

53
Q

Hydrogen bond

A

Weak attraction between polarized molecules or between polarized regions of the same molecule. important in a three-dimensional folding and coiling of large molecules. Easily disrupted by temperature and pH changes

54
Q

Van der waals force

A

Week, brief attraction due to random disturbances in the electron clouds of adjacent Adams. We just of all bonds individually, but can have strong effects collectively

55
Q

Polar covalent bonds give rise to hydrogen bonds how?

A

When hydrogen bonds with oxygen the electrons are more attracted to the oxygen nucleus in orbit more than they do the hydrogen. This makes the oxygen region of the molecule slightly negative in the hydrogen region slightly positive

Anatomy and Physiology 1 (45 decks)

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