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ANATOMY & PHYSIOLOGY II > APII: Basic Chemistry > Flashcards

APII: Basic Chemistry Flashcards

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1
Q

What is the fundamental unit of matter?

A

Atom

An atom consists of protons, neutrons, and electrons.

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2
Q

What are the three parts of an atom?

A
  • Protons
  • Neutrons
  • Electrons
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3
Q

What is the charge and weight of protons?

A

Positively charged (+), weight is defined as 1 atomic mass unit (amu)

Protons determine the element’s identity.

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4
Q

What is the charge and weight of neutrons?

A

No charge / neutral, weight is 1 amu

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5
Q

What is the charge and weight of electrons?

A

Negatively charged (-), weight is negligible

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6
Q

Where are protons and neutrons located in an atom?

A

In the nucleus

Electrons orbit around the nucleus.

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7
Q

What determines the element of an atom?

A

The number of protons

This is also referred to as the atomic number.

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8
Q

What is the atomic number?

A

The number of protons in an atom

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9
Q

What is the mass number?

A

The total number of protons and neutrons

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10
Q

What are isotopes?

A

Atoms of a given element that have a different number of neutrons

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11
Q

What are the electron energy levels also known as?

A

Shells

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12
Q

How many electrons can the first shell hold?

A

2 electrons

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13
Q

How many electrons can the second shell hold?

A

8 electrons

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14
Q

What is the most stable electron configuration for an atom?

A

8 electrons in the outermost shell

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15
Q

What are valence electrons?

A

Electrons in the outermost shell that determine an atom’s chemical reactivity

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16
Q

What happens when atoms transfer or share electrons?

A

Molecular bonds are formed

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17
Q

What is a molecule?

A

2 or more atoms chemically bonded together

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18
Q

What defines an element?

A

Contains all atoms of the same kind (same number of protons)

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19
Q

What is a compound?

A

2 or more different atoms chemically bonded in a fixed ratio

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20
Q

What are intramolecular bonds?

A

Bonds within the molecule that hold it together

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21
Q

What are the two types of intramolecular bonds?

A
  • Ionic
  • Covalent
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22
Q

What is the difference between intramolecular and intermolecular bonds?

A

Intramolecular bonds are within the molecule, while intermolecular bonds are between molecules.

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23
Q
A
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24
Q

What are ionic bonds?

A

Ionic bonds occur when 1 or more electrons are transferred from one atom to another, changing the overall charge of the individual atoms and holding them together by magnetic force (positive attracts negative).

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25
What is an ion?
An ion is a charged particle.
26
What is a cation?
A cation is a positively charged particle.
27
What is an anion?
An anion is a negatively charged particle.
28
What role do ions play in the body?
Ions are involved in virtually every physiological process in the body.
29
What are covalent bonds?
Covalent bonds occur when atoms share pairs of electrons, making them stronger than ionic bonds.
30
What is a single covalent bond?
A single covalent bond is formed by 1 pair of shared electrons.
31
What is a double covalent bond?
A double covalent bond is formed by 2 pairs of shared electrons.
32
What is a triple covalent bond?
A triple covalent bond is formed by 3 pairs of shared electrons.
33
What are polar covalent bonds?
Polar covalent bonds occur when the pair of electrons is more attracted to the larger nucleus of one atom than to the smaller nucleus of the other atom.
34
What is a hydrogen bond?
A hydrogen bond is a type of intermolecular bond between two molecules, where the positive hydrogen end of a polar molecule has a weak attraction to the negative ends of other polar molecules or negative ions.
35
Why is water essential for life on Earth?
Water is a polar molecule that forms hydrogen bonds with itself, which is essential for life on Earth.
36
Why does water form a bead on a freshly waxed car?
Water forms a bead on a freshly waxed car because nonpolar liquids flatten out.
37
Why does ice float?
Ice floats because, due to polar attractions between water molecules, they spread out and arrange themselves in a crystal lattice structure, becoming less dense as a solid.
38
Why do slide covers stick to slides?
Slide covers stick to slides due to hydrogen bonding between water molecules.
39
Why do premature babies need surfactant?
Premature babies do not produce enough surfactant, which is why they need to be put on a ventilator.
40
Why does water dissolve salts well?
Water dissolves salts well due to its polar nature.
41
42
What are mixtures?
Combinations of 2 or more substances that can be separated by ordinary physical means.
43
What is a solution?
A mixture in which the component particles remain evenly distributed.
44
What is a solute?
The substance present in smaller amount that is being dissolved.
45
What is a solvent?
The substance present in larger amount that does the dissolving.
46
What are suspensions?
Mixtures involving a liquid that settle if not shaken. ## Footnote Example: blood.
47
What are colloidal suspensions?
Particles in liquid that do not dissolve but are so small they do not settle.
48
What is the absorbability of metallic minerals?
Metallic minerals are 3-5% absorbable across intestinal membrane.
49
What is the absorbability of colloidal minerals?
Colloidal minerals are 98% absorbable.
50
Where are we meant to get our minerals from?
We are meant to get our minerals from plants and not dirt and rocks.
51
What are electrolytes?
Substances that break apart or dissociate in solution to form ions.
52
What types of substances are electrolytes?
Acids, bases, and salts are types of electrolytes.
53
Why are they called electrolytes?
Because the ions (charged particles) help conduct an electric current.
54
What is an acid?
Any substance that releases hydrogen ions in solution. ## Footnote Acids are called proton donors.
55
What are hydrogen ions?
Very reactive ions that are a single proton that has lost its electron.
56
What is a base?
Any substance that removes hydrogen ions from solution. ## Footnote Bases are called proton acceptors.
57
How is the strength of acids and bases determined?
By the percentage of molecules that dissociate or break apart in solution.
58
What is hydrochloric acid (HCl)?
Considered a strong acid because most of the molecules in solution break apart into hydrogen ions (H+) and chlorine ions (Cl-).
59
What is carbonic acid (H2CO3)?
Considered a weak acid because most of the molecules in solution remain intact and only a few dissociate into hydrogen ions (H+) and bicarbonate ions (HCO3-).
60
61
What does the pH scale measure?
The strength of acids and bases.
62
What is the range of the pH scale?
The scale goes from 0 to 14, with 7 being neutral.
63
What does a pH less than 7 indicate?
It indicates an acid, with lower numbers representing stronger acids.
64
What does a pH greater than 7 indicate?
It indicates a base/alkaline solution, with higher numbers representing stronger bases.
65
What does a decrease of 1 on the pH scale mean?
It means there are 10 times more hydrogen ions in solution.
66
What is a neutralization reaction?
It is when an acid and base react to produce water and a salt. ## Footnote Example: HCl + NaOH > H2O + NaCl
67
What are buffers?
Solutions that resist changes in pH when a strong acid or base is added.
68
What is a matching route in buffers?
It is made up of a weak acid and a salt from that same acid, which acts like a weak base.
69
Why are buffers important?
They are crucial in maintaining blood pH.
70
What is the normal range for blood pH?
Blood pH must be maintained within very narrow limits of 7.35 to 7.45.
71
What happens if blood pH falls below 7.3?
You get sick, a condition known as acidosis.
72
What happens if blood pH falls below 7?
You die because nerves cannot fire, leading to coma and death.
73
What happens if blood pH rises above 7.5?
You get sick, a condition known as alkalosis.
74
What happens if blood pH rises above 7?
You die because nerves can't stop firing, leading to convulsions and rigor.
75
What are the components of one of the most important buffers in the body?
Carbonic acid (H2CO3) and its salt sodium bicarbonate (NaHCO3).
76
What is the formula for carbonic acid?
H2CO3 = (H+)(HCO3-)
77
What is the formula for sodium bicarbonate?
NaHCO3 = (Na+)(HCO3-)
78
How do buffers react with strong acids and bases?
They react with either a strong acid or a strong base, resisting drastic changes in pH.
79
What is an example of a strong acid?
HCl = (H+)(Cl-) which most break up and reacts with salt. ## Footnote Example: (H+)(Cl-) + (Na+)(HCO3-) › (Na+)(Cl-) + (H+)(HCO3-)
80
What is an example of a strong base?
NaOH = (Na+)(OH-) which most break up and reacts with acid. ## Footnote Example: (Na+)(OH-) + (H+)(HCO3-) › (Na+)(HCO3-) + H2O

ANATOMY & PHYSIOLOGY II (11 decks)

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