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A&P : Unit 1 > Chapter 2.1 : Introduction to Chemistry & Inorganic Chemistry > Flashcards

Chapter 2.1 : Introduction to Chemistry & Inorganic Chemistry Flashcards

1
Q

Atoms make

A

Molecules

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2
Q

In the late 1700’s, scientists started to study air. They
discovered air was made up of different types of air. What did they call these gasses?

A

Special airs

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3
Q

Who developed the modern atomic theory in 1803?

A

John Dalton

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4
Q

Who created the Periodic Table?

A

Dmitri Mendeleev

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5
Q

Who invented chemistry?

A

Bohr

He invented the electron orbital model

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6
Q

What is chemistry?

A

the study of matter

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7
Q

What is the atomic mass of a proton?

A

1 amu (atomic mass unit) or Dalton

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8
Q

What is the atomic mass of a neutron?

A

1 amu (atomic mass unit) or Dalton

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9
Q

What is the atomic mass of a electron?

A

.0005 Dalton

Travel around electron

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10
Q

Atom’s charge is neutral when

A

The amount of electrons and protons is the same.

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11
Q

Valence electrons

A

Electrons on the outermost shell of the atom

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12
Q

What determines the chemical properties of an atom?

A

The number of protons

Ex. Carbon = 6 protons
Gold = 79 protons

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13
Q

What is the strongest bond?

A

Nonpolar covalent bond

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14
Q

Covalent bond

A

Atoms SHARE electrons

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15
Q

Compound

A

substance that contains atoms of two ro more
different elements

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16
Q

Cation

A

Positive charged atom

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17
Q

Anion

A

Negative charged atom

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18
Q

Ionic Bonds

A

Electrons are DONATED

this is is weak attraction

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19
Q

Ions

A

charged particles with unequal number of protons and electrons

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20
Q

Ionization

A

Transfer of electrons from one to another

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21
Q

The first orbit, electron shell, of an atom has a maximum of how many electrons?

A

2

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22
Q

The second and third orbits of an atom can have a maximum of how many electrons?

A

8

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23
Q

What’s the charge of an atom if it gains electrons?

A

negative

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24
Q

What’s the charge of an atom if it losses electrons (Therefore having more protons than it does electrons)?

A

positive

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25
Q

Hydrophilic

A

Water loving

My understanding of it: Things with unequal/oppositive charges attract to water because it gives water something to interact with.

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26
Q

Hydrophobic

A

Water hating

My understanding of it: Does not interact with water because it has an equal/stable charge and has nothing for the negative and positive ends of the water molecule to interact with.

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27
Q

Hydrogen bond

A

a weak attraction between a slightly positive hydrogen atom in one molecule and a slightly negative oxygen or nitrogen atom in another molecule.

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28
Q

Hydrogen bonds do not hold atoms together so they don’t form

A

compounds, however.

Hydrogen bonds are opposite charge between two molecules or across from opposite charges in the same molecule. Therefore, hydrogen bonds….

– 1) Hold 3D shape of same molecule together (e.g. protein)
– 2) Hold different molecules together (e.g. water molecules)

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29
Q

Why does water expand when it freezes?

A

Hydrogen bonds get pushed farther apart as water freezes

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30
Q

Isomers

A

molecules with identical molecular formulae but different
arrangement of their atoms

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31
Q

Isomers

A

molecules with identical molecular formulae but different
arrangement of their atoms

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32
Q

Free Radicals

A

chemical particles with an odd number of electrons // FR
need another electron to make themselves stable

Produced by /// normal metabolic reactions, radiation, or toxic chemicals

FR damage tissue / may cause cell death!

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33
Q

What neutralizes free radicals?

A

Antioxidants

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34
Q

Isotopes

A

same element that differ from one another only in the number of neutrons

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35
Q

Isotopes of Hydrogen

A

Hydrogen = no neutron
Deuterium = 1 neutron
Tritium = 2 neutron

36
Q

Radioisotopes

A
  • unstable isotopes that give off radiation // beta particle
  • every element has at least one radioisotope
37
Q

Radioactivity

A

– radioisotopes decay to stable isotopes by releasing radiation
– we are all mildly radioactive
– Below is beta decay

38
Q

Electrolytes

A

Salts that ionize in water and form solutions
capable of conducting an electric current.

39
Q

What is the importance of electrolytes?

A

– chemical reactivity
– osmotic effects (influence water movement)
– electrical effects on nerve and muscle tissue

40
Q

Electrolyte balance is one of the most
important considerations in

A

patient care

  • Imbalances have ranging effects from muscle
    cramps, brittle bones, to coma, cardiac arrest, and
    death.
41
Q

Minerals

A

Inorganic elements extracted from soil
by plants and passed up the food
chain to humans

– Ca, P, Cl, Mg, K, Na, I, Fe, Zn, Cu, and S
constitute about 4% of body weight

– structure (teeth, bones, etc)
– enzymes

42
Q

Electrolytes required for nerve and muscle function

A

mineral salts

43
Q

Polar covalent bonds and its V-shaped
molecule gives water a set of properties
that account for its ability to support life. What are these abilities?

A

– solvency
– cohesion
– adhesion
– chemical reactivity
– thermal stability

44
Q

Solvency

A

ability to dissolve other chemicals

Water is called the Universal Solvent

  • All biologic chemical reactions depend on the
    solvency of water
45
Q

Chemical Reactivity of Water

A

It is the ability of water to participate in
chemical reactions

– water ionizes into H+
and OH-
– water ionizes other chemicals (acids and
salts)
– water involved in hydrolysis and dehydration
synthesis reactions

46
Q

Thermal Stability of Water

A

Water helps stabilize the internal temperature of the body

47
Q

Water has a high heat capacity

A

the amount of heat required to raise the
temperature of 1 g of a substance by 1 degree C.

48
Q

calorie (cal)

A

the amount of heat that raises the temperature of
1 g of water 1 degree C

49
Q

Mixtures

A

consists of substances physically blended, but
not chemically combined

50
Q

Solution

A

consists of particles
of matter called the solute mixed
with a more abundant substance
(usually water) called the
solvent

51
Q

Solute

A

can be gas, solid or liquid

52
Q

Solutions are defined by the
following properties:

A

– solute particles under 1nm
– solute particles do not scatter
light
– will pass through most
membranes
– will not separate on standing

53
Q

Solution appearance

A

Particles extremely small and not visible; do not settle out; one component dissolves in the other component.

54
Q

Colloids

A

Most common colloids in the body
are mixtures of protein and water
* Many can change from liquid to gel
state within and between cells

55
Q

Colloids appearance

A

Two distinct components;
particles small and not visible; but do not settle out; hydrated.

– particles range from 1 – 100 nm in
size
– scatter light and are usually cloudy
– particles too large to pass through
semipermeable membrane
– particles remain permanently
mixed with the solvent when
mixture stands

56
Q

Suspension appearance

A

Particles large and
usually visible; settle out.

  • particles exceed 100nm
  • too large to penetrate
    selectively permeable
    membranes
  • cloudy or opaque in
    appearance
  • separates on standing
57
Q

Emulsion

A

suspension of one liquid in another // e.g. fat in milk

58
Q

pH

A

a scale that measures the number of “free” hydrogen
protons (H+) in the water

  • Strong acid = pH 0 // Strong base = pH 14 // water’s pH is 7
59
Q

acid

A

a proton donor (releases H+
ions in water)

60
Q

base

A

a proton acceptor (accepts H+
ions) // (or releases OH- ions in water)

61
Q

A change of one number on the pH scale represents

A

a 10 fold change in H+ concentration

62
Q

Our body uses _____ to resist changes in pH

A

buffers

– slight pH disturbances can disrupt physiological
functions and alter drug actions
– deviations from this range cause tremors, paralysis
or even death

63
Q

pH of blood ranges from

A

7.35 to 7.45

64
Q

chemical reaction

A

a process in which a
covalent or ionic bond is formed or broken

65
Q

chemical equation

A

symbolizes the course of
a chemical reaction

reactants (on left) -> products (on right)

66
Q

Classes of chemical reactions

A

– decomposition reactions
– synthesis reactions
– exchange reactions

67
Q

____ atoms forms the “backbone” for the macromolecules of life

A

Carbon

Carbon’s four valence electrons allow carbon to make macromolecules that form linear chains, branching chains, and ring structures.

68
Q

Decomposition Reactions

A

Large molecule breaks
down into two or more
smaller ones
* AB > A + B

69
Q

Decomposition Reactions

A

Large molecule breaks
down into two or more
smaller ones
* AB > A + B

70
Q

Synthesis Reactions

A

Two or more small
molecules combine to
form a larger one
* A + B > AB

71
Q

Two molecules exchange atoms or group of atoms

A

AB+CD > ABCD > AC + BD

72
Q

Reversible Reactions

A

Can go in either direction under different circumstances

73
Q

The most important equations in human
physiology

A

CO2 + H2O <> H2CO3 <> HCO3- + H

carbon dioxide plus water forms
carbonic acid which dissociates into bicarbonate and a proton

74
Q

What determines the direction of reversible reactions?

A

Law of mass action determines direction

– proceeds from the side of equation with greater quantity of reactants to the side with the lesser quantity
– Required enzyme (biocatalyst) carbonic anhydrase

75
Q

Equilibrium exists in reversible reactions when

A

the ratio of products to reactants is stable

76
Q

Basis for chemical reactions is

A

molecular motion and collisions

– reactions occur when molecules collide with enough force and the correct orientation

77
Q

Reaction Rates affected by:

A

– Concentration // reaction rates increase when the reactants are more concentrated

– Temperature // reaction rates increase when the temperature rises

– Catalysts –substances that temporarily bond to reactants, hold them in favorable position to react with each other, and may change the shapes of reactants in ways that make them more likely to react.

  • speed up reactions without permanent change to itself
  • holds reactant molecules in correct orientation
  • catalyst not permanently consumed or changed by the reaction
  • Enzymes are important biological catalysts
78
Q

What is an enzyme? What is a substrate?

A
  1. The substrates
    approach
    the enzyme.
  2. When the substrates bind
    the enzyme, both the
    substrates and the enzyme
    change shape.
  3. The substrates enter
    the transition state
    and are converted
    into products.
  4. The product and enzyme
    dissociate, and the enzyme
    returns to its original shape.
79
Q

Metabolism

A

All the chemical reactions that occur within a cell

80
Q

Catabolic

A

energy releasing (exergonic) decomposition
reactions

  • breaks covalent bonds
  • produces smaller molecules
  • releases useful energy
81
Q

Anabolic

A

energy storing (endergonic) synthesis reactions
* requires energy input
* E.g. production of protein or fat
* driven by energy that catabolism releases

82
Q

Oxidation

A

– any chemical reaction in which a molecule gives up electrons and releases energy
– molecule is said to be oxidized in this process
– electron acceptor molecule is the oxidizing agent // oxygen is often involved as the
electron acceptor

83
Q

Reduction

A

– any chemical reaction in which a molecule gains electrons and also gains energy
– molecule is said to be reduced when it accepts electrons
– molecule that donates electrons is the reducing agent

84
Q

Oxidation-reduction (redox) reactions

A

– oxidation of one molecule is always accompanied by the reduction of another
– electrons are often transferred as hydrogen atoms
– molecules like NAD and FAD (i.e. co-enzymes) are used to transfer H+ and electron

85
Q

Biochemistry

A

the study of the arrange of
different elements molecules that compose
living organisms

– Carbohydrates
– Fats
– Proteins
– Nucleic acids

A&P : Unit 1 (11 decks)

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