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Nutrition 1 (Semester I) > 3a. Chemistry - Elements, Atoms > Flashcards

3a. Chemistry - Elements, Atoms Flashcards

1
Q

What is an atom?

A

Small particles that make up matter

like Lego bricks

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2
Q

What makes up an atom?

A

Protons
Neutrons
Electrons

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3
Q

What is an element?

A

A substance made up of just one type of atom

It can’t be split up into simpler substances

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4
Q

What is a molecule?

A

Two or more atoms bonded together

Not visible to humans

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5
Q

Examples of molecules

A

Oxygen (O2)
Carbon dioxide (CO2)
Nitrogen (N2)

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6
Q

What is a compound?

A

Two or more different elements bonded together

Visible to humans

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7
Q

Examples of compounds

A

Table salt (NaCl)
Vinegar (C2H4O2)
Methane (CH4)

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8
Q

How many different elements are normally present in the human body?

A

26

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9
Q

What are the 4 major elements found in the human body?

A

Carbon
Hydrogen
Oxygen
Nitrogen

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10
Q

What percentage of the human body is made up of the 4 major elements?

A

96%

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11
Q

Chemical symbol: Hydrogen

A

H

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12
Q

Chemical symbol: Sodium

A

Na

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13
Q

Chemical symbol: Magnesium

A

Mg

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14
Q

Chemical symbol: Calcium

A

Ca

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15
Q

Chemical symbol: Vanadium

A

V

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16
Q

Chemical symbol: Chronium

A

Cr

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17
Q

Chemical symbol: Manganese

A

Mn

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18
Q

Chemical symbol: Iron

A

Fe

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19
Q

Chemical symbol: Cobalt

A

Co

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20
Q

Chemical symbol: Nickel

A

Ni

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21
Q

Chemical symbol: Copper

A

Cu

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22
Q

Chemical symbol: Zinc

A

Zn

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23
Q

Chemical symbol: Molybdenum

A

Mo

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24
Q

Chemical symbol: Mercury

A

Hg

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25
Q

Chemical symbol: Boron

A

B

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26
Q

Chemical symbol: Carbon

A

C

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27
Q

Chemical symbol: Nitrogen

A

N

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28
Q

Chemical symbol: Oxygen

A

O

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29
Q

Chemical symbol: Fluorine

A

F

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30
Q

Chemical symbol: Aluminium

A

Al

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31
Q

Chemical symbol: Silicon

A

Si

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32
Q

Chemical symbol: Phosphorus

A

P

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33
Q

Chemical symbol: Sulfur

A

S

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34
Q

Chemical symbol: Chlorine

A

Cl

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35
Q

Chemical symbol: Selenium

A

Se

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36
Q

Chemical symbol: Iodine

A

I

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37
Q

Proton: charge and weight

A

Positive

1 atomic unit

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38
Q

Neutron: charge and weight

A

No charge

1 atomic unit

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39
Q

Electron: charge and weight

A

Negative

No weight

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40
Q

Structure of an atom

A 
Nucleus - made up of equal protons and neutrons
Electron shell(s) - made up of electrons
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41
Q

How do electrons arrange themselves in the electron shell?

A

Pairs

2-8-8

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42
Q

What makes an atom reactive?

A

If the outer electron shell isn’t full or if it loses an electron

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43
Q

Atom analogy

A

Each proton is an adult with one child (electron)
Each neutron is an adult with no children
The adults hang out together in the nucleus and make up the mass of the family
The children whizz around the adults not weighing anything
Each proton has a positive charge
Each electron has a negative charge
These opposites attract each other and keep the family together

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44
Q

Periodic table example

A

19 (atomic number)
K (element symbol)
Potassium (element name)
39.0983 (atomic mass)

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45
Q

What is the atomic number of an element?

A

The number of protons

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46
Q

What is the mass number of an element?

A

Number of protons + number of neutrons

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47
Q

How can you calculate the number of neutrons in an element?

A

Atomic mass - atomic number

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48
Q

What element is required for thyroid health?

A

Iodine

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49
Q

Why are fluoride and chlorine relevant in thyroid health?

A

They share similar chemical and physical properties to iodine (same column on periodic table)
If they are present in the body, they can prevent the formation of T3 and T4

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50
Q

Where can we find fluoride?

A

Tap water
Toothpaste
Mouthwashes

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51
Q

Where can we find chlorine?

A

Swimming pools

Chlorinated washed vegetables

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52
Q

What is an isotope?

A

Atoms of the same element which have different numbers of neutrons in the nucleus

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53
Q

What affect does an isotope have on an element?

A

Changes the mass

Doesn’t affect the chemical activity though

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54
Q

What does a massive imbalance of protons and neutrons create?

A

Makes the atom very unstable

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55
Q

What does an imbalanced isotope cause?

A

Radioactivity

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56
Q

Examples of isotopes in medicine

A

Radiotherapy

Breath test for H. pylori

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57
Q

How does the breath test for H. pylori work?

A

Breath test 1
Take urea - labelled as radioactive carbon-14 or non-radioactive carbon-13
Wait 10-30 mins
Breath test 2
If urease is present (enzyme that H. pylori uses to metabolise urea), there will be a higher amount of CO2 in 2nd breath test

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58
Q

What does H+ mean?

A

It’s a hydrogen ion

It’s a proton as the electron has become separated from the outer shell

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59
Q

Why does hydrogen easily react with other atoms?

A

Because H has only one electron in its outer shell, it will often go looking for another atom that needs one electron to fill its shell

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60
Q

What are inert elements?

A

Elements that don’t easily react as they have their outer shell filled with the perfect number
They rarely get involved in chemical reactions

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61
Q

Why do atoms try to bond?

A

To get the right number of electrons in their outer shell so they can become more stable

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62
Q

What are the two types of bonding?

A

Ionic bonding

Covalent bonding

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63
Q

What is ionic bonding?

A

When one atom donates some of its electrons to another

64
Q

When does ionic bonding usually occur?

A

When there are 1, 2 or occasionally 3 electrons to donate

65
Q

What is ionisation?

A

The process of giving or gaining electrons

66
Q

What is an ion?

A

An atom that has given up or received electrons to fill its outer shell

67
Q

How is an ion written?

A

With their corresponding - or + charge

68
Q

How do you write a sodium ion if it has given an electron away?

69
Q

What is a covalent bond?

A

When two elements share electrons so that they can both have the magic number of electrons they are looking for

70
Q

When does covalent bonding tend to occur?

A

When the two atoms are similar

When there are a lot of spaces to be filled to reach a full outer shell

71
Q

Between what type of atoms does ionic bonding occur?

A

Atoms that have different electronegativity

Ions that are oppositely charged

72
Q

What is a polar covalent bond?

A

When atoms with different electronegativities share electrons in a covalent bond but one of the elements has more electronegativity which pulls the shared electrons towards themselves

73
Q

What makes an element more electronegative?

A

Having lots of protons

a strong positively charged centre

74
Q

What does a polar covalent bond lead to?

A

An uneven distribution of charge

75
Q

Which elements are the most electronegative?

A

Chlorine
Fluoride
Oxygen
Nitrogen

76
Q

What is one of the most important examples of a polar bond?

A

The bonds between O2 and H in water

77
Q

What happens during a O2 and H polar bond?

A

The O2 pulls the electrons towards itself resulting in a negative charge over the oxygen and a positively charged area over each hydrogen
The positive hydrogens on one water molecule are attracted to the negatively charged oxygens on the next molecule

78
Q

What are the interactions between the O2 and H molecules called?

A

Hydrogen bonds

79
Q

What qualities do the hydrogen bonds give to water?

A

Surface tension

Ability to dissolve many substances

80
Q

Why is water considered to be the universal solvent?

A

The polar bonds are ideal for dissolving chemicals into their separate ions

The different electrical charges allow water molecules to become attracted to other molecules (hence why water dissolves salt/sugar)

81
Q

What are hydrophilic molecules?

A

Polar bonds
Dissolve easily in water
(e.g. alcohol)

82
Q

What are hydrophobic molecules?

A

Non-polar covalent bonds
Don’t dissolve easily in water
(e.g. fats)

83
Q

What is an electrolyte?

A

An ionic compound that dissolves in water

e.g. salt

84
Q

What do electrolytes do?

A

Conduct electricity

85
Q

What are the key electrolytes in the body?

A 
Sodium
Potassium
Magnesium
Bicarbonate
Chloride
Calcium
Phosphate
86
Q

Why are electrolytes important?

A

Conduct electricity for nerve/muscle function
Exert osmotic pressure for water/BP balance
Acid-base balance

87
Q

What is an acid?

A

A substance that releases a high amount of H+ ions when dissolved in water

88
Q

What is a base?

A

A substance which binds to H+ in a solution

Creates lots of OH- (hydroxide)

89
Q

Why is water a neutral solution?

A

For every H+ released, a OH- is also created

90
Q

What is the pH of water?

91
Q

What is the optimal pH of blood?

92
Q

What is the optimal pH of the stomach?

93
Q

Why are fruit and veg acidic before consumption but alkaline after?

A

Their organic acids are metabolised by the body and intestinal bacteria to become alkaline
They are also high in alkaline minerals e.g. K, Mg, Ca

94
Q

Why is meat and dairy more alkaline before consumption but acidic after?

A

High protein/sulphur amino acid content

The sulphur amino acids increase sulphuric acid formation

95
Q

What happens when sulphuric acid is increased in the body?

A

Disrupts blood pH
Calcium is drawn from the bones
Increased calcium is then lost in urine

96
Q

What other foods are acidic apart from dairy and meat?

A

Refined sugars

Processed foods

97
Q

What can also contribute to an acidic environment?

A

Stress

Sedentary lifestyle

98
Q

Which pathology thrives in an acidic environment?

99
Q

What level of pH or above could start to kill cancer cells?

100
Q

How can body acidity be measured?

A

pH test of urine or saliva

101
Q

How do you do a urine pH test?

A

Urinate onto strip of pH paper
2nd urine output of the day
Measure pH midstream

102
Q

How do you do a saliva pH test?

A

Wash mouth with plain water upon waking
Wait 10 mins
Spit onto pH paper

103
Q

What pH do many cancer patients have?

104
Q

What should your pH be ideally?

A

Neutral (7) or slightly alkaline

105
Q

What creates a chemical reaction?

A

When different molecules form new bonds or break existing ones

106
Q

What does every chemical reaction involve?

A

Transfer of energy to stored energy
Kinetic energy
Heat

107
Q

What are the starting materials of a chemical reaction called?

108
Q

What are the end products of a chemical reaction called?

109
Q

How are chemical reactions written in formula?

110
Q

What does endothermic mean?

A

Takes in heat

111
Q

What does exothermic mean?

A

Gives off heat

112
Q

How do chemical reactions occur?

A

Two molecules need to collide (collision theory)

113
Q

What can speed up the chance of a chemical reaction?

A

Number of molecules
The energy of the molecules (faster)
Temperature
Pressure changes

114
Q

What is the energy of activation?

A

The minimum energy that is required for a reaction to take place

115
Q

What does a catalyst do?

A

Speeds up reactions by lowering the energy of activation

116
Q

How can catalysts benefit reactions?

A

Means the reactions are faster

Can also happen at lower temperatures

117
Q

What are catalysts in the body called?

118
Q

What are inhibitors?

A

They stop catalysts from being so effective

Make the activation energy higher so slows down the reaction time

119
Q

Example of an inhibitor drug

A

Statins

HMG-CoA reductase inhibitors

120
Q

What are anabolic reactions?

A

Building
Making new substances
Building new bonds

A+B = AB

121
Q

What does an anabolic reaction require?

122
Q

What are catabolic reactions?

A 
Breaking down
(e.g. breaking down food and releasing energy for storage)

AB = A+B

123
Q

What is hydrolysis?

A

A catabolic reaction where water breaks down molecules into smaller pieces

124
Q

What is a dehydration synthesis?

A

When water becomes a waste production of a reaction

e.g. when glucose bonds come together to form a carbohydrate

125
Q

What are reversible reactions?

A

Reactions where the products of the reaction can react together to produce the original reactants
Helps maintain homeostasis

126
Q

What is a buffer?

A

Substances that maintain the H+ concentration in the body within the normal limits

127
Q

What does the bicarbonate buffer system do?

A

Mops up excess acidity

128
Q

What happens during the bicarbonate buffer system?

A

CO2 from respiration reacts with H2O in blood and creates carbonic acid (H2CO3)
This quickly dissociates to form bicarbonate and hydrogen ions (HCO3- and H+)

129
Q

How are excess H+ mopped up?

A

Increased breathing rate to exhale CO2 through lungs

Kidneys produce HCO3- buffer to excrete excess H+

130
Q

Why do kidneys struggle with high acidity?

A

Kidney buffering system is fairly slow and puts strain on the organs

131
Q

What is oxidation?

A

The removal of electrons from an atom or molecule

132
Q

How does oxidation effect the potential energy in a compound?

A

It reduces it

133
Q

What element usually helps with oxidation?

134
Q

What is a dehydration reaction?

A

When hydrogen electrons are lost during oxidation

135
Q

What happens during a reduction reaction?

A

Electrons are gained

136
Q

What does gaining an electron do to the potential energy of a molecule?

A

Increases it

137
Q

What does OIL RIG stand for?

A

Oxidation Is Losing

Reduction Is Gaining

138
Q

What are free radicals?

A

Molecules or compounds that have an unpaired electron in their outer shell

139
Q

How do free radicals try to stabilise their outer shell?

A

By stealing electrons from other stable molecules

140
Q

Why are free radicals destructive?

A

By losing an electron, this causes oxidation
The attacked molecule then becomes unstable and so on
Leads to a chain reaction of oxidative damage

141
Q

Why is taking electrons from DNA destructive?

A

Damages genes

Can result in cancerous changes

142
Q

Which conditions can oxidative damage lead to?

A

Cancer
Atherosclerosis
Fibromyalgia
Neurodegenerative diseases

143
Q

How can free radicals develop?

A 
Aerobic respiration
Inflammation
Metabolism
Pollution
Sunlight
Strenuous exercise
X-rays
Smoking
Alcohol
144
Q

How can free radicals be mopped up?

A

Reduce exposure to the production sources of free radicals

Optimise antioxidant status

145
Q

What are antioxidants?

A

Groups of vitamins, phytochemicals and enzymes that donate an electron to the free radicals
This converts them to harmless molecules without being damaged themselves

146
Q

Examples of antioxidants

A 
Beta-carotene
Vit C
Vit E
Quercetin
Glutathione
147
Q

Why do antioxidants work better together?

A

They recycle each other

148
Q

Why is it better to get antioxidants from food rather than a supplement?

A

Food substances contain a mix of AO

Supplements may lead you to take too much of one particular one

149
Q

What are functional groups?

A

Groups of atoms that are attached to a carbon skeleton

150
Q

What do functional groups do?

A

Contribute to the structure and function of a molecule

Determines how they behave

151
Q

What are the characteristics of the hydroxyl functional group?

A 
R-O-H
Alcohols
Polar
Hydrophilic
Dissolve easily in water
152
Q

What are the characteristics of the sulfhydryl functional group?

A

R-S-H
Found in protein chains (amino acid cysteine)
Polar
Hydrophilic

153
Q

What are the characteristics of the carboxyl functional group?

A

R-C-OH=O
Found in amino acids
Hydrophilic
Weak acid/negative particle

154
Q

What are the characteristics of the amine functional group?

A

R-N-H-H
Found in amino acids
The -NH2 group can act as a weak base (alkalising) if necessary mopping up H+

155
Q

What are the characteristics of the esters functional group?

A

R-C-OR’=O

Predominate bond in triglycerides

156
Q

What are the characteristics of the phosphates functional group?

A 
R-O-P-OH-OH=O
Found in ATP
Very hydrophilic
Dissolve easily in water
Forms a double negative charge

Nutrition 1 (Semester I) (15 decks)

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