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BIOS1167 > Online Module: Introductions to the foundation of biomedical science > Flashcards

Online Module: Introductions to the foundation of biomedical science Flashcards

1
Q

How many of the 118 elements on the periodic table make up our bodies?

A

Only 20 of the 118 elements including, H, C, O, N, Na, Mg, Si, P, S, Cl, K, Ca, V, Cr, Mn, Fe, Co, Cu, Zn, As, Se, Mo and I

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2
Q

What is an atom ?

A

An atom is the smallest unit of matter that makes up an element and which takes place in a chemical reaction.

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3
Q

What percentage of water is found in our bodies?

A

60-75%

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4
Q

What is an element?

A

Elements are pure substances (which means they can only be made up of the one type of atom) and are responsible for bodily functions . They cannot be simplified and there are 118 elements.

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5
Q

What elements are found in proteins

A

Carbon, hydrogen, oxygen and nitrogen

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6
Q

What elements are found in fats and carbohydrates?

A

Carbon, hydrogen and oxygen

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7
Q

What elements are found in bone?

A

Calcium and phosphorus

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8
Q

What percentage does C, H, O and N make in the body

A

95%

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9
Q

What is a molecule?

A

Simplest unit of a pure substance retaining characteristics of the substance. When atoms of identical elements come together to form bonds H2, O2, etc

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10
Q

Compound

A

When atoms of different elements combine to form molecules they are referred to as compounds.

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11
Q

What is an atom made of?

A
  • Positively charged proton
  • Negatively charged Electron
  • Neutrally charged neutron
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12
Q

Why don’t electrons, orbiting the nucleus spiral away?

A

Due to the electrostatic attraction between the positively charged nucleus and the negative electrons

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13
Q

What is the mass of a proton

A

1 atomic mass unit

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14
Q

What is a mass of a neutron

A

1 atomic mass unit

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15
Q

What is a mass of an electron?

A

relatively 0

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16
Q

What does the atomic number of an element indicate

A

The number of protons in the atom, and therefore, the number of electrons

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17
Q

What does the atomic mass (molecular mass) indicate

A

The proton + neutron (in amu)

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18
Q

Do all atoms of the same element have the same mass?

A

No, even though they are the same element, isotopes of an element do exist which causes the atom to vary in mass. These isotopes of the elements must all share the same number of protons but their neutrons may vary.

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19
Q

What is an isotope

A

An isotope is an atom of an element with different mass. They share the same number of protons but they differ in the number of neutrons causing them to have different mass

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20
Q

What is relative atomic mass

A

The mass of an element when taking into account
- the number of different isotopes
- the weight of the isotopes
- how abundant they are in nature
It is the average mass of the naturally occurring atoms of an element in atomic mass units

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21
Q

What are principal energy levels

A

These are the levels in which the electrons orbit around the nucleus. Each level can hole a maximum amount of electrons before a new level is introduced. As we go down the periodic table, atoms of that particular element would require an additional level.

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22
Q

What component of the atom is most involved in bonding and chemical reactions

A

The valence electrons. The noble gas (group 8) element have full outer valence orbitals and therefore do not participate in chemical reactions as easily

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23
Q

Octet Rule

A

States that atoms require 8 electrons in the outer orbital in order to be stable. They do this by gaining, losing or sharing electrons

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24
Q

What is an ion

A

An atom is a neutrally charged particle as the number of protons are equal to the number of electrons. However, when these atoms lose or gain electrons, they become charged and are called ions

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25
Q

WHat is a cation

A

An atom which as lost an electron making it partially positively charged. usually happens to metals

26
Q

What is an anode

A

An atom which has gained an electron making it negatively charged. Usually occurs with non-metals

27
Q

Polyatomic ions

A

Group of atoms which are bound together chemically and carry an overall charge due to the excess or deficiency of electrons. They behave as one particle in a solution - that is when they dissociate they remain intact

28
Q

Hydroxide

A

OH-

29
Q

Phosphate

A

PO4^3-

30
Q

Ammonium

A

NH4+

31
Q

carbonate

A

CO3^2-

32
Q

Bicarbonate

A

HCO3-

33
Q

Nitrate

A

NO3-

34
Q

Sulphate

A

SO4^2-

35
Q

What is an ionic bond

A

The bond made between metals and non metals. It is formed when electrons are removed one atom and given to another, causing them to become oppositely charged. The electrostatic attraction between the positive and negative charge is what bonds the two together (overall charge is neutral) They are strong bonds that are non - directional meaning they form experience electrostatic attraction in all directions making a lattice crystal structure. \

36
Q

What happens when ionic compounds are placed in solutions

A

They are dissociated completely into individual ions, resulting in a charged solution. They are referred to as electrolytes

37
Q

What are covalent bonds

A

They occur when the electrons are shared between the two atoms either equally (producing a non - polar covalent bond) or non-equally (producing a polar covalent bond). These bonds usually form between metals and are not easily broken. They are uncharged and therefore, when they dissociate in a solution they do not cause a current in the solution

38
Q

What is electronegativity

A

The measure of an atoms ability to attract electrons to itself in a covalent bond

39
Q

WHat is polarity

A

Charge separation

40
Q

What is a hydrogen bond

A

It is the inter molecular bond formed between molecules. They are weaker than ionic and covalent bonds

41
Q

What is an acid

A

A proton donator - releases a proton when dissolved in water

42
Q

Properties of acid

A

Turn litmus paper red and is sour

43
Q

What is a base

A

A proton acceptor

44
Q

Properties of a base

A

Turns litmus paper blue and has a slippery soapy feel

45
Q

Strong acids

A

Dissociate almost completely, releasing a high concentration of hydrogen in the solution Eg. HCl

46
Q

Weak acids

A

Slightly dissociated, releasing a small concentration of protons in the solution Eg. Acetic acid CH3COOH and lactic acid

47
Q

What is a pH scale

A

The negative log of hydrogen ion concentration

pH = -log(H+)

48
Q

What is the pH of blood

A

7.4

49
Q

What is classified as pH <7

A

Acids

50
Q

What is classified as pH >7

A

Basic (alkali)

51
Q

pH of gastric fluid

A

1.6

52
Q

pH of urine

A

6.0

53
Q

pH of bile

A

8.0

54
Q

What is a Buffer

A

A solution that resists changes in pH that would otherwise result with the addition of an acid, base or water (dilution)

55
Q

What are Biological buffer of blood

A

Blood must remain at 7.4 and can only steer away from that by +/-0.1. The buffers for blood include H2CO3-/HCO3- , amino acids and proteins

56
Q

What are the biological buffers for body fluids

A

Lungs and kidneys

57
Q

What is a solution

A

When a solid or gas (solute) dissolves in a solvent

58
Q

What are the four characteristics of solutions

A
  1. they are homogeneous mixtures
  2. cannot be separated by standing or filtration
  3. Almost always transparent
  4. Composed of small molecules/ions
59
Q

What is a concentration

A

Amount of solute dissolved in a given quantity of solvent

60
Q

What is Solubility

A

maximum amount of the solid that will dissolve in a given amount of liquid at a given temp

61
Q

What is molarity

A

number of moles of solute dissolved in 1 litre of solution

BIOS1167 (4 decks)

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