Module 1.1: Intro to Life Science for Midwifery

Question 1

What does chemistry examine?

Answer 1

• the properties, composition, and structure of elements and compounds
• how these change
• the energy released or absorbed when they change

Question 2

What is a compound?

Answer 2

Substances formed by two or more
elements

Question 3

What is an element?

Answer 3

A substance that cannot be separated into
simpler substances by chemical means

Question 4

What does an element consist of?

Answer 4

An element consists of an atom with a unique combination of protons, neutrons, and electrons

Question 5

What are the three classifications of elements?

Answer 5

major, minor, trace

Question 6

what percentage do major elements make up?

Answer 6

96%

Question 7

what are some examples of major elements?

Answer 7

Oxygen, Carbon, Hydrogen, Nitrogen

Question 8

what percentage do minor elements make up?

Answer 8

3.6%

Question 9

what are some examples of minor elements?

Answer 9

Calcium, Phosphorous, Potassium,
Sulfur, Sodium, Chlorine,
Magnesium, Iron

Question 10

what percentage do trace elements make up?

Answer 10

0.4%

Question 11

what are some examples of trace elements?

Answer 11

Aluminium, Cobalt, Copper, Fluorine,
Iodine, Manganese, Molybdenum,
Selenium, Silicon, Tin, and Zinc

Question 12

what is an atom?

Answer 12

• Basic building block of chemistry
• Smallest unit of an element

Question 13

what does an atom consist of?

Answer 13

protons, neutrons, and electrons

Question 14

what is located within the nucleus?

Answer 14

protons and neutrons

Question 15

what surrounds the nucleus?

Answer 15

electrons

Question 16

how do electrons act?

Answer 16

surround the nucleus, not static but rather always in motion

Question 17

what is the bohr atom model?

Answer 17

Visualizes electron
shells as concentric circles
surrounding the nucleus

Question 18

when is an atom considered neutral? (Generally)

Answer 18

of electrons = # of protons = ‘0’
charge

Question 19

when are atoms not neutral?

Answer 19

Filling the shells with electrons push
atoms to have charges and react with
one another

Question 20

how many electrons can the first shell hold? the second shell?

Answer 20

first shell: 2 electrons
second shell: 8 electrons

Question 21

when is an atom stable and unlikely to form a bond with another atom?

Answer 21

when its outer electron shell is full

Question 22

what is the octet rule?

Answer 22

• Atoms will tend to form bonds to achieve a full outer shell of 8 electrons
• To do this, they can lose, gain or share electrons
  between atoms

Question 23

what is the atomic number? where is it found?

Answer 23

the number of protons in the
nucleus. top left corner

Question 24

what is the mass number?

Answer 24

the sum of its protons and
neutrons

Question 25

what is an isotope?

Answer 25

Variation of an element that has the same number of protons BUT different number of neutrons in its nucleus

Question 26

how do the atomic number and mass number differ in isotopes?

Answer 26

Same atomic number but mass number differs because of varying number of neutrons

Question 27

why do all isotopes have the same chemical properties?

Answer 27

Have the same number of electrons (which determines its chemical properties)

Question 28

what types of isotopes are radioactive?

Answer 28

unstable isotopes

Question 29

what are the two kinds of isotopes?

Answer 29

stable and unstable

Question 30

explain how radioactive isotopes are created

Answer 30

* Nuclei spontaneously change (decay) over time to a more stable configuration * As they decay, they emit radiation and particles

Question 31

what is atomic mass

Answer 31

average mass of all isotopes of an element

Question 32

what is atomic mass measured in?

Answer 32

Measured in daltons (atomic mass units)

Question 33

what is an ion?

Answer 33

A particle with either a * Negative (-) Charge or * Positive (+) Charge

Question 34

what makes an ion?

Answer 34

an unequal number of electrons compared to protons

Question 35

Cl- = chlorine ion = -1 charge did this gain or lose an electron?

Answer 35

gain

Question 36

Ca2+ = calcium ion = +2 charge did this gain or lose electrons?

Answer 36

lose

Question 37

what is a free radical?

Answer 37

An atom with an unpaired electron in its outermost shell

Question 38

how do free radicals behave?

Answer 38

the atom is unstable, highly reaction and destructive to other tissues

Question 39

what is an example of a free radical?

Answer 39

Oxygen can form free radicals in the body, which can damage cells

Question 40

what is the effect of a free radical?

Answer 40

Cause damage to cell membranes, DNA, can alter biochemical compounds

Question 41

how can free radicals become stable?

Answer 41

* By giving up an electron or “stealing” an electron from another molecule, breaking apart important body molecules * When they steal an electron, they may create a new free radical

Question 42

what produce free radicals?

Answer 42

* Ultraviolet light in sunlight * X-rays * Normal metabolic reactions * Air pollution * Cigarette smoke * Alcohol * Drugs

Question 43

what diseases are linked to free radicals?

Answer 43

* Premature aging * Pre-eclampsia * Fetal alcohol syndrome

Question 44

how can damage of free radicals be slowed?

Answer 44

Damage may be slowed with antioxidants such as vitamins C and E and selenium

Question 45

what is a cofactor?

Answer 45

a compound that helps enzymes function (mainly trace elements)

Question 46

how are cofactors obtained?

Answer 46

normally through diet so theres minimal concern about deficiency

Question 47

what are some examples of cofactors?

Answer 47

cobalt, copper, iodine, manganese, molybdenum, zine, selenium

Question 48

what is florine used for?

Answer 48

seen as fluoride and used to prevent tooth decay and make enamel stronger

Question 49

how many elements are there and how many of them are found on nature?

Answer 49

118 98

Question 50

what is hydrogen important for?

Answer 50

organic molecule

Question 51

what are sodium and potassium important for?

Answer 51

electrolytes

Question 52

what are magnesium and calcium important for?

Answer 52

teeth and bones + electrolytes

Question 53

what is calcium important for?

Answer 53

smooth muscles contraction potentials + electrolytes

Question 54

what is iron important for?

Answer 54

anemia/blood related disorders

Question 55

what is carbon important for?

Answer 55

backbone of organic molecules

Question 56

what is nitrogen important for?

Answer 56

carbon compounds like amino acids

Question 57

what is phosphorous important for?

Answer 57

phosphate + magnesium = bone

Question 58

what is oxygen important for?

Answer 58

oxidative metabolism

Question 59

what is sulfur important for?

Answer 59

Protein structure (disulfide bonds + cross bridging)

Question 60

what is chorine important for?

Answer 60

electrolytes

Question 61

What is iodine important for?

Answer 61

formation of thyroid hormone

Question 62

what is an example of a radio isotope?

Answer 62

iodine-123 emits gamma radiation used for imaging

Question 63

what are some harmful effects of radio isotopes?

Answer 63

cause cancer or disease (ex. radon 222 is associated w lung cancer in non-smokers)

Question 64

What are some beneficial effects of radio isotopes?

Answer 64

medical imaging for diagnosis or treatment (ex. imagine thyroid (I-123) treatments for hyperthyroidism (I-131) cancer