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Nursing 104 > Lecture 3: Chemistry 1A > Flashcards

Lecture 3: Chemistry 1A Flashcards

1
Q

What is Chemistry?

A

Something we can’t directly SEE.

Involves very complex SYSTEMS.

We TRY to understand systems using MODELS.

Study how systems CHANGE.

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2
Q

Something

A

We can’t directly see

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3
Q

Involves

A

Very complex systems

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4
Q

We

A

try understand systems using models

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5
Q

Study

A

how systems change

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6
Q

Chemical Composition of the Human Body

A

Oxygen (O): 65.0%
Carbon (C): 18.0%
Hydrogen (H): 10.0%
Nitrogen (N): 3.0%
Calcium (Ca): 1.4%
Phosphorus (P): 1.0%
Magnesium (Mg): 0.50%
Potassium (K): 0.34%
Sulphur (S): 0.26%
Sodium (Na): 0.14%
Chlorine (Cl): 0.14%
Iron (Fe): 0.004%
Zinc (Zn): 0.003%

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7
Q

Matter

A

Anything with mass that occupies space

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8
Q

What are the three states of matter

A

Solid, Liquid, Gas

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9
Q

Solid

A

Rigid/compact
Fixed shape
Fixed volume

eg; Ice cube, bone, diamond

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10
Q

Liquid

A

Free flowing
Takes shape of container
Defined volume

eg; Water, blood, gasoline

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11
Q

Gas

A

No fixed shape
No fixed volume
Takes shape and volume of container
Lots of energy!

eg; Air, Oxygen, helium

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12
Q

Physical Change

A

involves states of matter and energy.

No new substance is created, but the matter takes a different form.
Reversible Physical Change:

Original form can be restored.
Examples: Dissolving salt in water, melting ice.
Irreversible Physical Change:

Original form cannot be restored.
Examples: Cutting hair, pulverizing tablets.

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13
Q

involves

A

states of matter and energy.

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14
Q

No

A

new substance is created during a physical change, although the matter take a different form

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15
Q

In a reversible

A

physical change, the original form of the matter can be restored eg dissolving salt in water, melting ice

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16
Q

In an irreversible

A

physical change, the original form cannot be restored eg cutting hair, pulverising tablets

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17
Q

Physical Change (II)

A

A reversible process usually onset by a change in environment (temperature)

No rearrangements of atoms, ie no change incomposition just a change in neighbouring interactions

can be measured or observed

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18
Q

A reversible

A

A reversible process usually onset by a change in environment (temperature)

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19
Q

No rearrangments

A

No rearrangements of atoms, ie no change incomposition just a change in neighbouring interactions

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20
Q

can

A

can be measured or observed

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21
Q

Physical Changes (III)

A

Cellular Respiration

Carbon dioxide is a waste product.

Converted to bicarbonate ion (HCO₃⁻) in the blood.

In the lungs, it is converted back and released as CO₂.

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22
Q

Cellular

A

Cellular Respiration

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23
Q

Carbon dioxide

A

Carbon dioxide is a waste product.

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24
Q

Converted

A

Converted to bicarbonate ion (HCO₃⁻) in the blood.

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25
In the lungs
In the lungs, it is converted back and released as CO₂.
26
Chemical properties
irreversible change, rearrangement of atoms, new chemical properties, formation of at least one new substance.
27
Examples of Chemical Changes (II)
In Life: Lighting a match Cooking an egg Bread becoming toast Milk going sour Nails rusting Burning wood In the Body: Digestion: Converting food ingeted into usable parts by the body eg. protein, fat and carbohydrates into amino acids, glucose. frutose, fatty acids
28
Elements
The simplest substances - cannot be broken down using chemical reactions (cf fission/fusion) Thirteen major ones in the human body In chemistry elements are arranged in the peroidic table arranged in order of atomic number - elements with similar atomic structure (and hence similar chemical properties) appear in vertical columns
29
The simplest substances
The simplest substances - cannot be broken down using chemical reactions (cf fission/fusion)
30
Thirteen
Thirteen major ones in the human body
31
In chemistry
In chemistry elements are arranged in the peroidic table
32
Arranged
arranged in order of atomic number - elements with similar atomic structure (and hence similar chemical properties) appear in vertical columns
33
Atoms
The basic unit of matter 'The smallest particle of a chemical element that can exist'
34
Structure of an atom
Made up of 3 subatomic particles: Protons – Located in the nucleus (center). Neutrons – Also in the nucleus. Electrons – Move around the nucleus in a small cloud.
35
Chemistry mass range
-30 ~ +8 log kgs
36
Proton
Charge: 1+ Mass: 1 Symbol: P+
37
Neutron
Charge:0 Mass: 1 Symbol: n
38
Electron
Charge: -1 Mass: 1/1840 Symbol: e-
39
Basic Atomic model (the rutherford-bohr model)
6 protons 6 electrons 6 neutrons
40
Name and valence electrons
Each shell or orbit has a name starting with 'K' on the inner shell The shells are labelled from the nucleus outward K shell - 2 e- L shell - 8 e- M shell - 18 e- N shell - 32 e- each shell contains a specific number of electrons
41
Valence electron numbers
Valency = Number of electrons an atom can gain, lose, or share. Last digit of the group number = Number of valence electrons. Elements in the same group have the same number of outer orbit electrons.
42
Atomic mass (Mass Number, M)
Approximetely equivalent to the number of protons and neutrons in the atom
43
Isotopes
Equal numbers of protons but different numbers of neutrons in their nuclei
44
Medical uses of radioactive isotopes
Carbon 13 - MRI Iodine-131 for the evaluation of hyperthyroidism
45
Periodic table
An element - has atoms of only one kind * Has the same number of protons * the same atomic number * chemically the simplest substances * cannot be broken down using chemical reactions
46
Has
Has the same number of protons
47
The same
* the same atomic number
48
Chemically
chemically the simplest substances
49
Cannot
* cannot be broken down using chemical reactions
50
Symbols
abbreviations for chemical elements names First letter of name, capitalised. Can have two letters. First letter capital, second lowercase
51
Element
52
Periodic table
53
Molecule
when two or more atoms join together.
54
Compound
A molecule with at least 2 different atoms that are chemically bonded
55
Sucrose is a common table sugar (I)
= disaccharide =composed of the two monosaccharides - gluose and fructose
56
Sucrose is a common table sugar (II)
Molecular formular = C12H22O11 (numbers down) Melting point = 186C soluble in water
57
Glucose (I)
Molecular formula C6H12O6 preferred energy source for the body
58
Glucose (II)
Most carbohydrates you eat are converted into gluose Used for energy or to be stored in muscle cells or the liver as glycogen for later use
59
Gluten (I)
important in baking (provides structure to bread) formed from two other proteins
60
Gluten (II)

Nursing 104 (9 decks)

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