Chapter 2.1 : Introduction to Chemistry & Inorganic Chemistry Flashcards
(85 cards)
1
Q
Atoms make
A
Molecules
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
3
Q
Who developed the modern atomic theory in 1803?
A
John Dalton
4
Q
Who created the Periodic Table?
A
Dmitri Mendeleev
5
Q
Who invented chemistry?
A
Bohr
He invented the electron orbital model
6
Q
What is chemistry?
A
the study of matter
7
Q
What is the atomic mass of a proton?
A
1 amu (atomic mass unit) or Dalton
8
Q
What is the atomic mass of a neutron?
A
1 amu (atomic mass unit) or Dalton
9
Q
What is the atomic mass of a electron?
A
.0005 Dalton
Travel around electron
10
Q
Atom’s charge is neutral when
A
The amount of electrons and protons is the same.
11
Q
Valence electrons
A
Electrons on the outermost shell of the atom
12
Q
What determines the chemical properties of an atom?
A
The number of protons
Ex. Carbon = 6 protons
Gold = 79 protons
13
Q
What is the strongest bond?
A
Nonpolar covalent bond
14
Q
Covalent bond
A
Atoms SHARE electrons
15
Q
Compound
A
substance that contains atoms of two ro more
different elements
16
Q
Cation
A
Positive charged atom
17
Q
Anion
A
Negative charged atom
18
Q
Ionic Bonds
A
Electrons are DONATED
this is is weak attraction
19
Q
Ions
A
charged particles with unequal number of protons and electrons
20
Q
Ionization
A
Transfer of electrons from one to another
21
Q
The first orbit, electron shell, of an atom has a maximum of how many electrons?
A
2
22
Q
The second and third orbits of an atom can have a maximum of how many electrons?
A
8
23
Q
What’s the charge of an atom if it gains electrons?
A
negative
24
Q
What’s the charge of an atom if it losses electrons (Therefore having more protons than it does electrons)?
A
positive
25
Hydrophilic
Water loving
My understanding of it: Things with unequal/oppositive charges attract to water because it gives water something to interact with.
26
Hydrophobic
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.
27
Hydrogen bond
a weak attraction between a slightly positive hydrogen atom in one molecule and a slightly negative oxygen or nitrogen atom in another molecule.
28
Hydrogen bonds do not hold atoms together so they don't form
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)
29
Why does water expand when it freezes?
Hydrogen bonds get pushed farther apart as water freezes
30
Isomers
molecules with identical molecular formulae but different
arrangement of their atoms
31
Isomers
molecules with identical molecular formulae but different
arrangement of their atoms
32
Free Radicals
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!
33
What neutralizes free radicals?
Antioxidants
34
Isotopes
same element that differ from one another only in the number of neutrons
35
Isotopes of Hydrogen
Hydrogen = no neutron
Deuterium = 1 neutron
Tritium = 2 neutron
36
Radioisotopes
- unstable isotopes that give off radiation // beta particle
- every element has at least one radioisotope
37
Radioactivity
– radioisotopes decay to stable isotopes by releasing radiation
– we are all mildly radioactive
– Below is beta decay
38
Electrolytes
Salts that ionize in water and form solutions
capable of conducting an electric current.
39
What is the importance of electrolytes?
– chemical reactivity
– osmotic effects (influence water movement)
– electrical effects on nerve and muscle tissue
40
Electrolyte balance is one of the most
important considerations in
patient care
* Imbalances have ranging effects from muscle
cramps, brittle bones, to coma, cardiac arrest, and
death.
41
Minerals
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
Electrolytes required for nerve and muscle function
mineral salts
43
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?
– solvency
– cohesion
– adhesion
– chemical reactivity
– thermal stability
44
Solvency
ability to dissolve other chemicals
Water is called the Universal Solvent
* All biologic chemical reactions depend on the
solvency of water
45
Chemical Reactivity of Water
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
Thermal Stability of Water
Water helps stabilize the internal temperature of the body
47
Water has a high heat capacity
the amount of heat required to raise the
temperature of 1 g of a substance by 1 degree C.
48
calorie (cal)
the amount of heat that raises the temperature of
1 g of water 1 degree C
49
Mixtures
consists of substances physically blended, but
not chemically combined
50
Solution
consists of particles
of matter called the solute mixed
with a more abundant substance
(usually water) called the
solvent
51
Solute
can be gas, solid or liquid
52
Solutions are defined by the
following properties:
– solute particles under 1nm
– solute particles do not scatter
light
– will pass through most
membranes
– will not separate on standing
53
Solution appearance
Particles extremely small and not visible; do not settle out; one component dissolves in the other component.
54
Colloids
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
Colloids appearance
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
Suspension appearance
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
Emulsion
suspension of one liquid in another // e.g. fat in milk
58
pH
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
acid
a proton donor (releases H+
ions in water)
60
base
a proton acceptor (accepts H+
ions) // (or releases OH- ions in water)
61
A change of one number on the pH scale represents
a 10 fold change in H+ concentration
62
Our body uses _____ to resist changes in pH
buffers
– slight pH disturbances can disrupt physiological
functions and alter drug actions
– deviations from this range cause tremors, paralysis
or even death
63
pH of blood ranges from
7.35 to 7.45
64
chemical reaction
a process in which a
covalent or ionic bond is formed or broken
65
chemical equation
symbolizes the course of
a chemical reaction
reactants (on left) -> products (on right)
66
Classes of chemical reactions
– decomposition reactions
– synthesis reactions
– exchange reactions
67
____ atoms forms the “backbone” for the macromolecules of life
Carbon
Carbon's four valence electrons allow carbon to make macromolecules that form linear chains, branching chains, and ring structures.
68
Decomposition Reactions
Large molecule breaks
down into two or more
smaller ones
* AB > A + B
69
Decomposition Reactions
Large molecule breaks
down into two or more
smaller ones
* AB > A + B
70
Synthesis Reactions
Two or more small
molecules combine to
form a larger one
* A + B > AB
71
Two molecules exchange atoms or group of atoms
AB+CD > ABCD > AC + BD
72
Reversible Reactions
Can go in either direction under different circumstances
73
The most important equations in human
physiology
CO2 + H2O <> H2CO3 <> HCO3- + H
carbon dioxide plus water forms
carbonic acid which dissociates into bicarbonate and a proton
74
What determines the direction of reversible reactions?
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
Equilibrium exists in reversible reactions when
the ratio of products to reactants is stable
76
Basis for chemical reactions is
molecular motion and collisions
– reactions occur when molecules collide with enough force and the correct orientation
77
Reaction Rates affected by:
– 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
What is an enzyme? What is a substrate?
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
Metabolism
All the chemical reactions that occur within a cell
80
Catabolic
energy releasing (exergonic) decomposition
reactions
* breaks covalent bonds
* produces smaller molecules
* releases useful energy
81
Anabolic
energy storing (endergonic) synthesis reactions
* requires energy input
* E.g. production of protein or fat
* driven by energy that catabolism releases
82
Oxidation
– 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
Reduction
– 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
Oxidation-reduction (redox) reactions
– 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
Biochemistry
the study of the arrange of
different elements molecules that compose
living organisms
– Carbohydrates
– Fats
– Proteins
– Nucleic acids
