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BIO 235 Athabasca > The Chemical Level Of Organization > Flashcards

The Chemical Level Of Organization Flashcards

1
Q

____________is the force of gravity acting on matter, that does not change.

A

Weight

Is the force of gravity acting on matter, that does not change

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2
Q

Name the four major elements in your body that compromise 96% of body mass.

A

carbon, hydrogen, oxygen, nitrogen

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3
Q

How many lesser elements are found in the body’s mass? 3.6%

A

8 lesser elements

Na
P
k
s
cl
mg
Fe

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4
Q

How many trace elements are found in the body? 0.4%

A

14 trace elements

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5
Q

Oxygen is about _____ % of total body mass.

A

65 % oxygen
-oxygen is a part of water and many organic (carbon containing) molecules
-used to generate ATP

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6
Q

What forms the backbone chains and rings of all organic molecules?

A

carbon

-forms backbone chains and rings of all organic molecules: carbohydrates, lipids, proteins, and nucleic acid (DNA and RNA)

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7
Q

Carbon is about _____% of total body mass.

A

18.5 % carbon

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8
Q

Hydrogen is about ____% of total body mass.

A

9.5 % hydrogen

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9
Q

Nitrogen is about _____% of total body mass.

A

3.2 % nitrogen

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10
Q

What chemical element in it’s ionized form (h+) makes body fluids more acidic?

A

Hydrogen

(9.5% in body mass)

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11
Q

What chemical element is part of water and most organic molecules?

A

Hydrogen

(9.5% in body mass)

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12
Q

__________ is a component of all proteins and nucleic acids.

A

Nitrogen

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13
Q

Calcium is about ____% of total body mass.

A

Calcium 1.5 % of body mass

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14
Q

What element in it’s iodized form is needed for blood clotting?

A

Ca2+
Calcium

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15
Q

______________is a component of nucleic acids and ATP; also it is required for normal bone and tooth structure.

A

phosphorus

(1.0% in body mass)

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16
Q

__________ is the most plentiful cation in intracellular fluid; is needed to generate action potentials.

A

ionized form of potassium

(k+)

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17
Q

What type of charge does a cation have?

A

positive

Cation is a positively charged particle

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18
Q

The number of proton’s in the nucleus is an atom’s __________ ____________.

A

Atomic number

Oxygen has 8 protons, so it’s atomic number is 8

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19
Q

The _________number of an atom is the sum of its protons and _____________.

proton + neutron = __________ _________.

A

The mass number of an atom is the sum of it’s protons and neutrons.

proton + neutron= mass number

Sodium has 11 protons and 12 neutrons. 11 + 12 = 23
Mass number is 23

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20
Q

________________ are atoms of the same element that have the same number of protons, but different number of neutrons.

A

Isotopes

So they also have same atomic number, same position on periodic table but a different number of neutrons, meaning that their mass number varies.

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21
Q

Explain the difference between stable and unstable isotopes.

A

Unstable -change over time, harmful or helpful
Stable-does not change over time

Most isotopes are STABLE, which means there nuclear structure does not change over time.

UNSTABLE isotope, called radioactive isotopes; their nuclei decay (spontaneously change) into a stable structure. They can be helpful or harmful

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22
Q

In what ways are radioactive isotopes helpful or harmful?

A

HELPFUL- when used as tracers in medical imaging, tests for diagnosis, and procedures

HARMFUL-radiation can break apart molecules causing tissue damage or cancer

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23
Q

___________ is the time required for half of the radioactive atom of isotope to decay into more stable time.

A

The half-life of an isotope is the time required for a half of the radioactive atoms in a sample of that isotope to decay into a more stable form.

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24
Q

What is the standard unit for measuring the mass of atoms and their sub atomic particles called?

A

dalton
atomic mass unit (amu)

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25
Q

A ________ has a mass of 1.008 daltons, and a________ has a mass of 1.007, and a _________ has a mass of 0.0005 dalton.

A

neutron 1.008 daltons
protron 1.007 daltons
electron 0.0005 dalton

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26
Q

The average mass of all naturally occurring isotopes in an element is called the _________ _______ or the ________ ________.

A

The atomic mass or the atomic weight.
‘

Usually the atomic mass of an element is close to the mass number of its most abundant isotope

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27
Q

What is a compound?

A

2 or more different atoms

A substance that contains atoms of two or more elements.

Most of the atoms of the body are joined into compounds- H20 and NaCl (table salt, sodium chloride)

**a molecule of oxygen (02) is NOT a compound it only has atoms of one element

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28
Q

What is a molecule?

A

2 more atoms - share electrons 02

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29
Q

What is a free radical?

A

atom (s) with unpaired electron in outermost shell (usually unstable and reactive)

Having an unpaired electron makes a free radial highly reactive, and destructive to nearby molecules.

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30
Q

How do free radicals become stable?

A

Either giving up their unpaired electron or stealing one from another molecule.

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31
Q

What are the atomic number, mass number and atomic mass of carbon? How are they related?

A

atomic number = # of protons

mass number = protons + neutrons in an atom

atomic mass= average mass of all stable atoms of a given element in daltons

Atomic # is 6
(6 protons)
Mass # is

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32
Q

List the 12 most abundant chemical elements in the human body.

A

oxygen (65.0)
carbon (18.5)
hydrogen (9.5)
nitrogen. (3.2)

calcium (1.5)
phosphorus (1.0)
potassium (0.35)
sulfur
sodium
cholride
magnesium
iron

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33
Q

The outermost cell of an atom is called it’s __________ ____________.

A

valence shell

*the likelihood of a chemical bond forming depends on the number of electrons in the valence shell.

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34
Q

How does the octet rule- help explain why atoms interact in a predictable way?

A

atom goal is stability- achieved when there is 8 valence electrons.

For chemical stability (valence 8) to happen the atom either:
- empties it’s partially filled valence shell
-fills it with donated electrons
-or shares electrons with other atoms

It is predictable because the way that valence electrons are distributed determines the kind chemical bond will results (ionic, covalent, hydrogen)

Octet rule- under the right conditions two or more atoms can interact in ways that produce a chemically stable arrangement of eight valence electrons for each atom.

atomic hookups– atoms want stability and an atom with a valence shell holding 8 electrons is chemically stable.

On atom is more likely to interact with another atom if doing so will leave both atoms with 8 valence electrons.

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35
Q

Ionic bond

sodium : 1 valence electron
chlorine: 7 valence electrons

A

The force of attraction that holds together ions with opposite charges together.

Example: NaCl
a) if sodium loses one electron it can have complete octet in outermost shell
b) chlorine atom needs one electron for an octet in valence shell
c) ionic bond may form between oppositely charged ions

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36
Q

cation

A

positively charged ion formed when an atom LOSES one ore more valence electrons

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37
Q

When an ionic compound breaks apart into positive and negative ions in a solution, what is this called?

A

an electrolyte

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38
Q

anion

A

negatively charged ion

formed when an atom GAINS one ore more valence electrons

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39
Q

How do atoms form a covalently bonded molecule?

A

By sharing one, two or three pairs of valence electrons.

Sharing is covalently caring.

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40
Q

What are the most common chemical bonds in the body?

A

covalent bonds

***most of the body’s structures are formed from covalently compounded chemical bonds.

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41
Q

What is the main difference between an ionic bond and a covalent bond?

A

Ionic bond either gains or gives up a valence electron.

A covalent bond shares valence electrons.

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42
Q

What type of bonds share electrons equally?

A

non polar covalent bonds, two atoms share the electrons equally—-two identical atoms are always non-polar covalent bonds.

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43
Q

When the sharing of electrons between two atoms is not equal, what is this called?

A

polar covalent bonds

ie. water molecule

When the sharing of electrons between two atoms is unequal—the nucleus of one atom attracts the shared electrons more than the other atom.

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44
Q

The power of an atom to attract electrons to itself is called _________________.

A

electronegativity

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45
Q

What does it mean when something is polar?

A

It means it can attract or repel. (positive or negative)

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46
Q

A hydrogen bond is special in that it has a special type of dipole-dipole attraction. What does this mean?

A

dipole-dipole forces are the attractive forces of the positive end of one polar molecule to the negative end of another polar molecule.

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47
Q

How strong are hydrogen bonds compared to ionic and covalent bonds?

A

WEAKER than ionic and covalent.
* they can’t bind atoms to into molecules

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48
Q

Hydrogen bonds do establish important links between molecules or between different parts of a large molecule such as a protein or nucleic acid.

A

Yes they do

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49
Q

A spider walks on water or a leaf floats on water. Examples of the tendency of like particles to stay together, this is called _________ ___________.

A

Surface tension

cohesion in hydrogen bonds that link water molecules together

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50
Q

__________ ____________ occur when new bonds form or old bonds break between atoms.

A

Chemical reactions occur when new bonds form or old bonds break between atoms.

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51
Q

The basis for all chemical reactions happens in the ____________ shell.

A

Valence shell, the interaction between valance electrons

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52
Q

The starting substances two H2 and one O2 are known as ___________.

The ending substances–two molecules of H20 are the _____________.

A

reactants
products

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53
Q

What is the term used to describe all chemical reactions occurring in the body?

A

metabolism

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54
Q

What type of energy is stored in the bonds of compounds and molecules?

A

Chemical Energy

It’s a form of potential energy which is energy stored by matter due to its position.

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55
Q

The total amount of energy present at the beginning and end of a chemical reaction is the same. It can neither be created or destroyed. What is this principle known as?

A

The law of conservation of energy.

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56
Q

Some of the chemical energy in the food we eat is eventually converted into various forms of kinetic energy, such as mechanical energy used to walk and talk. What is this principle called?

A

The law of conservation of energy.

Conversion of energy from one form to another releases heat, which is used to maintain normal body temperature.

57
Q

What type of reaction releases more energy than it absorbs?

A

EXIT:
exergonic reactions

EX= OUT

58
Q

What type of reaction absorbs more energy than it releases?

A

Endergonic reactions (end= within)

59
Q

What is kinetic energy?

A

energy associated with matter in motion
the water that is released from the dam

60
Q

What is potential energy?

A

the energy is stored due to its position

the water that is held back by the dam

61
Q

What is activation energy?

A

Its the energy needed to break down chemical bonds in the reactant molecules so a reaction can start.

62
Q

Both the _____________ of particles and the ______________ influence the chance that a collision will occur and cause a chemical reaction.

A

concentration of particles
*closer together more chance to collide

temperature rises, the particles move more rapidly

63
Q

Substances called catalysts are chemical compounds that play a very important role in chemical reactions in the human body. Explain this important role.

A

Catalysts, speed up chemical reactions by lowering the activation energy needed for a reaction to occur.

NOTE: a catalyst does not alter the difference in potential energy between reactants and products.
It LOWERS the energy needed. Such as directing a particle of matter to hit another at a precise spot.

64
Q

What are the most important catalysts in the body?

A

enzymes
-proteins that are biological catalysts that speed up biochemical reactions
-molecules upon which enzymes act are called substrates

65
Q

True or False

After a chemical reaction takes place, the atoms of the reactants are rearranged to yield products with new chemical properties.

A

TRUE

66
Q

When two or more atoms, ions or molecules combine to form new and larger molecules, the processes are called ________________ reactions.

A

Synthesis reactions

67
Q

All of the synthesis reactions that occur in the body are referred to as ____________.

A

anabolism
synthesis reactions
endergonic

**most anabolism reactions are usually endergonic because they absorb more energy than they release.

68
Q

Combining simple molecules like amino acids to form large molecules such as proteins is an example of ___________.

A

anabolism

**most anabolism reactions are usually endergonic
(absorb more energy then release).

69
Q

Collectively known as catabolism, these types of reactions spilt up large molecules into smaller atoms, ions or molecules.

A

decomposition reactions
catabolism
break down
exergonic

70
Q

What type of reactions are these?

The series of reactions that break down glucose to pyruvic acid, with the net production of two molecules of ATP.

A

Catabolic reactions

they break down
they release energy
exergonic
decomposition reactions

71
Q

An exchange reaction consists of both__________ and __________ reactions.

A

exchange reactions

Synthesis-anabolism, endogenic
Decomposition- catabolism, exergonic

72
Q

In a ___________ ____________ the products can revert to the original reactants.

A

In a reversible reaction, the products can revert to the original reactants.

A reversible reaction is indicated by two half-arrows pointing in opposite directions.

73
Q

___________ refers to the loss of electrons; in the process the ___________ substance releases energy.

A

oxidation- loss of electrons

oxidized substance releases energy

Oxidation-reduction reactions are essential to life

*these reactions break down food molecules that produce energy

74
Q

_________ refers to the gain of electron; in the process the ___________ substance gains energy.

A

reduction- gain of electrons

reduced substance gains energy

75
Q

What reactions are essential to human life, are concerned with the transfer of electrons between atoms and molecules and are always parallel?

A

oxidation-reduction reactions

when on substance is oxidized (loses electron) another is reduced (gains an electron) at the same time.

76
Q

What is the relationship between reactants and products in a chemical reaction?

A

reactants (starting substance)
products (ending substances)

total mass of reactants=total mass of products
*the chemical reaction rearranges the atoms and results in different chemical properties

77
Q

Compare potential energy and kinetic energy.

A

potential energy (stored energy based on position)
-has capacity to produce energy
-chemical bonds

kinetic energy
(energy in motion)
-particles
-waves of sun rays

78
Q

How are anabolism and catabolism related to synthesis and decompositions reactions, respectively?

A

synthesis- anabolism
add 2 or more molecules together to make a larger molecule
small to large

decomposition-catabolism
break down- (releases more energy than absorbs)
large to small

79
Q

Why are oxidation-reduction reactions so important?

A

-they are essential to life
-principal source of energy
-oxidation of molecules by removal of hydrogen liberates large amounts of energy
(respiration, digestion)

80
Q

Most of the chemicals in our bodies exist in the form of compounds. Biologists and chemists divide these into what two principal classes?

A

Organic compounds
38-43% of body
-carbon containing + covalent bonds always and forever

Inorganic compounds
55-66% of body water
1-2% all other inorganic compounds
-usually lack carbon + simple
-molecules with only a few atoms so limited in functions
-covalent or ionic
-H20, salts, acids, bases

inorganic compounds that do contain carbon are (C02, HC03-, H2CO3)
carbon dioxide, bicarbonate ion and carbonic acid

81
Q

This type of compound usually lacks carbons, structurally simple and CANNOT be used by cells to perform complicated biological functions.

A

inorganic compounds
-water, salts, acids bases
-covalent or ionic

82
Q

This type of compound ALWAYS contains carbon, usually contains hydrogen and is always covalent.

A

organic compounds

large molecules, long carbon chains

83
Q

Inorganic compounds that CONTAIN carbon include :
1.
2.
3.

A

C02
Carbon dioxide

HC03
Bicarbonate ion

H2C03
Carbonic acid

84
Q

What is the most abundant and important inorganic compound in all living systems? What is it’s most important property?

A

water
polarity

  • uneven sharing of valence electrons confers a partial negative charge near the one oxygen atom and two positive charges near the two hydrogen atoms in a water molecule
85
Q

What makes water an excellent solvent for other ionic or polar substances?

A

polarity

  • it gives water molecules cohesion
    -allows water to resist temperature changes
86
Q

In a _____________, a substance called a _________ dissolves another substance called the _________.

A

In a solution a substance called a solvent dissolves another substance called the solute.

87
Q

Usually there is more solvent than solute in a solution.

TRUE or FALSE

A

TRUE

Your sweat is a dilute solution of water (the solvent) plus small amount of salts (the solutes).

88
Q

Solutes that are charged or contain polar covalent bonds are ____________.

A

hydrophilic- water loving

Sugar and salt are solutes that dissolve easily in water and are examples of water loving hydrophilic compounds.

89
Q

Molecules that contain mainly non-polar covalent bonds are water fearing, not very water-soluble are known as _____________ compounds.

A

hydrophobic- water fearing

ie. animal fats and vegetable oils

90
Q

Explain how polar water molecules dissolve salts and polar substances.

A
91
Q

Table sugar (sucrose) easily dissolves in water but is NOT an electrolyte. Is it likely that all the covalent bonds between atoms in table sugar are non polar bonds? Why or why not?

A

NOT likely non polar covalent bonds between atoms in table sugar because—

table sugar easily dissolves in water—-which means—-that if it is not charged it must contain polar covalent bonds.

water loving solutes either are 1. charged or 2. contain polar covalent bonds—which makes them dissolve easily in water.

92
Q

During digestion, decomposition reactions, break down (catabolize) large nutrient molecules into smaller molecules by the addition of water molecules. What is this type of reaction called?

A

hydrolysis reaction

hydrolysis reactions enable dietary nutrients to be absorbed into the body.

93
Q

When two smaller molecules join to form a larger molecule in a __________ ____________ reaction, a water molecule is one of the products formed.

A

dehydration synthesis reaction

94
Q

What is the product of a dehydration synthesis?

A

water molecule

95
Q

What is the reason that water is said to have a high heat capacity?

Why can water absorb or release large amounts of heat without any significant effects to it’s own temperature? Most other substances can not.

A

high heat capacity due to the large number of HYDROGEN BONDS

As water absorbs heat, some energy is used to break hydrogen bonds.

Which means less energy is left over/available to increase the motion of the water molecules which would have increased the waters temperature.

96
Q

Heat of Vaporization
insert question

A
97
Q

Water is a major component of mucus and other lubricating fluids in the body. Provide some examples throughout the body.

A

Lubrication:
-chest (pleural and pericardial cavity)
-abdomen (peritoneal cavity)
-where internal organs tough or slide over each other
-at joints, bones, ligaments and tendons that rub against each other
-inside the GI tract, mucus moist food, aids through smooth passage through GI tract

98
Q

A combination of elements or compounds that are physically blended together but not bound by chemical bonds?

A

Mixture
Example:
The air we breathe is a mixture of gases that include nitrogen, oxygen, argon, and carbon dioxide.

99
Q

What is a mixture?

Name three common liquid mixtures.

A

Mixture is a combination of elements or compounds that physically blended (not chemically bound)

solutions
colloids
suspensions

100
Q

How is a colloid different than a solution?

How are they similar?

A

DIFFERENT
colloid mixture
-solute particles large enough to scatter light
-color translucent or opaque
Ex-fog scatter car head beam light

SIMILAR
-solutes do not settle out and accumulate on the bottom of container

101
Q

What type of of a mixture is milk?

A

both solution and colloid

-solution: calcium salts, milk sugar (lactose), ions, and other small particles

-colloid: large milk protein

102
Q

When freshly drawn from the body, blood has an even, reddish color. After blood sets for a while in a test tube, red blood cells settle out the suspension and drift to the bottom of the tube. The upper layer, the liquid portion of blood, appears pale yellow and is called blood plasma.

What is this an example of?

A

Suspension

The suspended material eventually settles out.

103
Q

characteristics of a solution

A

solute particles very small

looks transparent
(due to solute particles very small)

once mixed together solutions in a solution remain evenly dispersed among the solvent molecules

like colloids particles do not settle

104
Q

characteristics of a colloid

A

size of particles are larger than in a suspension

size of particles large enough to scatter light

usually appears translucent or opaque

like solutions particles do not settle

105
Q

characteristics of a a suspension

A

particles will eventually settle

106
Q

To make a 10% NaCl solution, take 10g of NaCl and add enough water to make a total of 100 ml of solution.

What is this an example of?

A

percentage (mass per volume)
# of grams of a substance per 100 ml of solution

mass/volume = mass of solute/volume of solution (in ml) x 100%

Concentration of a solution:
mass per volume- percentage

mass– amount of atoms, molecules, compounds etc (matter)

107
Q

To make a 1 molar (1 M) solution of NaCl, dissolve 1 mole of NaCl (58.44g) in enough water to make a total of 1 litre of solution .

What is this an example of?

A

Molarity- moles (mol) per liter

A 1 molar (1m) solution = 1 mole of a solute in 1 litre of a solution

concentration of a solution
molarity

108
Q

The amount of any substance that has a mass in grams equal to the sum of the atomic masses of all its atoms.

What is this??

A

Mole

1 mole of the element chlorine (atomic mass= 35.45) is 35.45 grams

1 mole of the salt sodium chloride (NaCl) is 58.44 grams ( 22.99 for Na + 35.45 for Cl)

109
Q

Just as a dozen always means 12 of something, a __________ of anything always has the same number of particles: 6.023 x 10(23).

This huge number is called __________’s number.

A

mole

avogadros number

110
Q

Measurements that are stated in moles tell us about the number of _________, ________ or ___________ present. Why is this important?

A

atoms, ions, molecules

Important when chemical reactions are occurring because each reaction requires a set number of atoms of specific elements.

111
Q

What does it mean to be an acid?

What is another term that an acid is referred to as?

A

proton donor

Dissociates into:
H+ hydrogen ion(s)
one ore more anions

acid is inorganic

PROTON DONOR because:
H+ is a single proton with one positive charge

112
Q

What is a base and what else is it referred to as?

I love me some H+

A

proton aceptor

Dissociates into:
OH- hydroxide ion(s)
one or more cations

Removes H+ from a solutions

113
Q

When dissolved in water a ________ dissociates into cations and anions, neither of which is H+ or OH-.

A

Salt

114
Q

When dissolved in water a _________ dissociates into H+ and anions.

A

acid
proton donor

115
Q

When dissolved in water a _________ dissociates into OH- and cations.

A

base
proton acceptor

116
Q
A

acids and bases react with each other to form salts

117
Q
A

Calcium carbonate dissociates into both H+ and OH- making it a salt

Sulfuric acid dissociates into two H+ ions and an anion making it an acid.

118
Q

To maintain homeostasis, ICF and EFC must contain balanced quantities of ___________ and _____________.

A

acids (more H+) acidic

bases (more OH-) basic
alkaline

119
Q

What scale is based on the concentration of H+ in moles per litre?

A

pH scale

0-14

neutral midpoint 7
(equal H+ and OH-) water

120
Q

A pH of 6 means that there are ______ times more ______ than a pH of 7.

A

pH of 6 means there are 10 times more H+ than a pH of 7.

121
Q

Make card about pH scale

A
122
Q

A solution that has more H+ than OH- is a(n) ___________.

A solution that has more OH- than H+ is a(n) _____________.

A

acid solution (below 7)

basic solution (above 7)

123
Q
A

closer to 7 = closer to neutral

124
Q

Blood must be between ____ and _____ ph.

A

7.35 - 7.45
-just slightly more basic than pure water

125
Q

How do bicarbonate ions prevent buildup of excess H+?

A

By functioning as a weak base and removing the excess H+.

126
Q

The molecular formulas for the sugars glucose and fructose are both C6H1206.
The same formulas but structured differently, what is this called?

A

isomer- same same but different

same molecular formula-

atoms are positioned differently along the carbon skeleton- giving the sugars different chemical properties

127
Q

Macromolecules are usually ____________. A _________ is a large molecule formed by the _________ bonding of many identical or similar building block molecules called ___________.

A

polymers (many parts)

Polymer

covalent bonding

monomers (one part)

128
Q

What are the three major groups of carbonhydrates?

A

(simple sugars)
monosaccharides
disaccharides

(complex sugars)
polysaccharides

Based on their size

129
Q

What type of reaction is usually responsible for joining monomers?

A

dehydration synthesis

hydrogen atom removed
hydroxyl group removed
= H20

130
Q

Which functional group helps stabilize the shape of proteins?

A

sulfhydryl group

131
Q

What is the main function of carbohydrates?

A

source of chemical energy for generating ATP needing to drive metabolic reactions

**only a few carbohydrates are for building structural units (deoxyribose for DNA)

132
Q

What are the elements found in carbohydrates?

A

carbon, oxygen and hydrogen

ratio of hydrogen to oxygen is usually 2:1 (same as water)

133
Q

How many carbon atoms do monosaccharides have?
What are they called?

A

3 to 7 ‘ose’
3 carbon- trioses
4 tetroses
5 pentoses
6 hexoses
7 heptoses

134
Q

A ____________ is a molecule formed from the combination of two monosaccharides by _____________ _____________.

A

disaccharide

dehydration synthesis

**disaccharides can also be spilt into smaller simpler molecules by hydrolysis.

135
Q

A molecule of sucrose may be hydrolyzed into its components, glucose and fructose by the addition of _________.

A

water

136
Q

Each polysaccharide molecule contains tens or hundreds of ______ joined through ____________ ___________.

A

tens or hundreds of monosaccharides joined by dehydration synthesis reactions.

137
Q

Unlike simple sugars, polysaccharides usually are insoluble in water and do not taste sweet.

TRUE or FALSE

A

true

138
Q

What is the main polysaccharide in the human body?

  • a limited amount of this is stored in the liver and skeletal muscles
A

glycogen
-glucose monomers linked to one another in branching chains.

139
Q
A

BIO 235 Athabasca (3 decks)

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