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Integrated Sciences Chemistry > Integrated Sciences Test 1 > Flashcards

Integrated Sciences Test 1 Flashcards

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1
Q

What are the four basic forms of matter

A

Gases, Liquids, Solids, Plasma

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2
Q

Def of Gases

A

Possess neither volume nor shape, they expand indefinitely Ex: Steam

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3
Q

Def of Liquids

A

Possess Volume and assume the shape of the container Ex; Water

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4
Q

Def of Solids

A

Possess volume and shape, they can not be compressed Ex: Ice cube

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5
Q

Def of Plasma

A

A mixture of ionized gas and free floating electrons. Some believe that more than 99% of the universe’s matter is plasma

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6
Q

What affects the behavior of matter?

A

Temperature and pressure

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7
Q

What substance is most abundant in the body?

A

Water

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8
Q

What is a compound?

A

A pure substance made up of two or more elements in a fixed proportion by weigh
EX: H20 or NaCl

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9
Q

What is a molecule?

A

A tightly bound group of atoms that act as a unit (Connected by chemical bonds)

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10
Q

What is the difference between Ionic bonds and covalent bonds?

A

Ionic bonds give up electrons and covalent bonds share electrons

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11
Q

Chemical bonds are…

A

Powerful attractions that hold atoms together

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12
Q

Atoms are found in the…

A

Periodic table

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13
Q

How is the atomic number established?

A

By the number of protons

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14
Q

What is an element

A

A pure substance that cannot be broken down into simpler substances by chemical reactions.

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15
Q

There are currently how many elements?

A

118

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16
Q

How many elements will health care providers going to encounter in their practice?

A

Typically about 30-40

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17
Q

Daltons atomic theory states that..

A

All matter is made up of tiny particles called atoms, all atoms of the same element are identical to each other, atoms of any one element are different from those of any other element, and atoms combine to for molecules.

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18
Q

An electrons charge is..

A

Negative

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19
Q

A protons charge is…

A

Positive

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20
Q

A neutrons charge is…

A

Neutral

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21
Q

The number of protons in a atom is its…

A

Atomic number

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22
Q

In the periodic table rows are called…

A

Periods and increase with atomic weight

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23
Q

In the periodic table columns are called…

A

Families- elements within family have similar Chemical and Physical properties

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24
Q

Column VIIA in the periodic table is the…

A

Halogen Group

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25
Q

Column O in the periodic table is the…

A

Noble Gases

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26
Q

What is an isotope?

A

Where 2 or more elements have the same atomic number (same number of protons) but different number of neutrons…So it will have a different atomic mass, but same chemical properties

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27
Q

What is an Ion?

A

Atoms that have gained or loss electrons from their natural composition

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28
Q

What is an Anion?

A

An atom that has gained an electron (Has a negative charge)

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29
Q

What is a Cation?

A

An atom that has lost an electron (Has a positive charge)

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30
Q

What are atoms electrical charge?

A

Neutral… bc they have protons that are balanced by the electron.

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31
Q

The atomic mass is the sum of the

A

Number of protons and neutrons

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32
Q

Protons are larger than…

A

Electrons

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33
Q

Electrons are smaller than…

A

Protons and neutrons and orbit around the nucleus…There actual size is 1/1800th that of the nucleus

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34
Q

Electrons circle the nucleus in various…

A

Orbits (also called energy levels)

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35
Q

The first three orbits allow how many electrons on each row?

A

2-8-8

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36
Q

What is the theory of Octet?

A

Electrons are more stable if they have an outer electron ring that is made up of exactly 8 electrons

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37
Q

What are the noble gases?

A

Helium, Neon, Argon, Krypton, Xenon, & Radon

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38
Q

What are the big four? (Necessary for human life)

A

Carbon, Hydrogen, Oxygen, and nitrogen…these 4 make up the basis of organic chemistry

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39
Q

Calcium in the body…

A

Strengthens bones and teeth, aids in blood clotting, has role in muscle contraction and heartbeat control. About 90% of calcium in the body is present in bones as calcium phosphate and carbonates.

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40
Q

Phosphorus in the body..

A

Present in phosphates, which regulate neutrality of body fluids and is involved in energy transfer

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41
Q

Potassium in the body…

A

Helps regulate electrical balance of body fluids.

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42
Q

Sulfur in the body…

A

An essential component of proteins, important in protein structure.

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43
Q

Chloride in the body…

A

Helps regulate electrical balance of body fluids

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44
Q

Sodium in the body…

A

Helps regulate electrical balance of body fluids

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45
Q

Magnesium in the body…

A

Helps nerve and muscle action; necessary for action of certain enzymes, and present in bones and teeth.

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46
Q

Function of the Trace element, Chromium…

A

Increases effectiveness of insulin

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47
Q

Function of the trace element Cobalt…

A

A part of Vitamin B12

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48
Q

Function of the trace element Copper…

A

Strengthens Bones; assists enzyme action, traces of copper aid in the formation of hemoglobin

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49
Q

Function of the trace element Fluorine…

A

Reduces dental cavities

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50
Q

Function of the trace element Iodine

A

Necessary for thyroid function

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51
Q

Function of the trace element Iron…

A

Each hemoglobin molecule contains 4 Ferrous (Fe) ions, each of which serve as a point of attachment for an oxygen molecule.

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52
Q

Function of the the trace element Manganese

A

Present in bone forming enzymes; aids fat and carbohydrate metabolism

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53
Q

Function of the trace element Molybdenum

A

Necessary for action of certain enzymes

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54
Q

Function of trace element Zinc…

A

Necessary for normal growth.

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55
Q

What are chemical bonds…

A

Powerful attractions that hold atoms together

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56
Q

An ion is a particle with…

A

An unequal number of protons and electrons (bc it gave one up or it took one->all trying to get to 8 on its orbit)

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57
Q

Bonding occurs from…

A

Direct sharing of an electron or by thermodynamic interaction

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58
Q

Atoms can be bonded to atoms of the same element…give an example.

A

Oxygen…is O2

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59
Q

Which bond is stronger…a covalent bond or an electrostatic bond?

A

Covalent bond

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60
Q

Electrostatic bonds are when…

A

Negative attracts positive…“opposites attract”

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61
Q

There are 4 types of electrostatic bonding…what are they?

A

Ionic bond (Ion to Ion), Dipole-Dipole bond, Ion dipole bonding, Hydrogen Bonding, and London forces.

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62
Q

Metals react well with?

A

Nonmetals

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63
Q

Looking at the periodic table…how would magnesium and oxygen for an ionic bond?

A

Magnesium has 12 electrons…oxygen has 8 electrons…magnesium is going to give 2 electrons to oxygen to make both of them have 8 on their outer shells

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64
Q

Calcium chloride…the formula is CaCl2….So in this case how do you get them to bond?

A

Calcium has 20 electrons…So it needs to get rid of 2 electrons to get 8 on that outer shell..Chloride has 17 electrons…it needs 1 more to become stable…so the calcium gives up an atom to both sets of chloride

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65
Q

What is dipole-dipole attraction?

A

It is the attraction between the opposite (partial) charges of polar molecules..Example is hydrogen chloride bonding to another pair of hydrogen chloride (look in powerpoint)

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66
Q

Bond strength of covalent bond

A

400

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67
Q

Bond strength of hydrogen

A

12-16

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68
Q

Bond strength of Dipole-Dipole

A

1-2

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69
Q

Bond strength of London Dispersion Forces

A

<1

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70
Q

Bond strength in order…

A

Covalent 400, Hydrogen 12-16, Dipole-Dipole 1-2, and London Forces <1

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71
Q

Organic chem is the study of…

A

Carbon-Containing molecules

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72
Q

Saturated hydrocarbons are…

A

Single-bonded carbon chains with all available carbons attached to hydrogen

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73
Q

Unsaturated hydrocarbons..

A

Have one or more double or triple bonds between carbon molecules.

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74
Q

Alkane

A

Hydrocarbons containing a single-bonded carbon atom

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75
Q

Alkene

A

A hydrocarbon where two carbon atoms are joined together by a double bond

76
Q

Alkynes

A

Hydrocarbons containing triple bonded carbons

77
Q

Hydrocarbons are…

A

Molecules composed of carbon atoms with hydrogen atoms attached

78
Q

Compounds made up mainly of one or more carbon atoms with their respective hydrogen attachments are called…

A

Hydrocarbons

79
Q

The _____ bond provides the foundation of organic chemistry…

A

Covalent

80
Q

Why does Carbon go so well with hydrogen?

A

Because Carbon has 6 electrons total…4 on its outer ring…Hydrogen is 1 electron…so it can hook on 4 times (Shares electrons)!!!! Which will bring the Hydrogen to having 2 electrons (which is their goal) and the carbon to having 8 electrons on its outer shell (goal :))

81
Q

Hydrocarbons are often found in what format?

A

In straight chains with or without branches

82
Q

The simplest form of an organic hydrocarbon is the gas known as what?

A

Methane

83
Q

Methane, which is the simplest form of an organic hydrocarbon is made up of what….

A

A single carbon and 4 hydrogen atoms

84
Q

The strongest of the electrostatic bonds are what?

A

Ion to Ion bonding

85
Q

Molecules with ionic bonds have what?

A

high melting and boiling points

86
Q

What is an example of an Ion-ion bond?

A

NaCl….So the sodium gives up an electron to the Chloride and they attract…basically ion to ion is giving another element an electron. Because the sodium gave the chloride an electron it is positive, because the chloride accepted it, it is negative. Negative and positive attract in ion to ion bonding.

87
Q

What are valence electrons?

A

electrons in the outer shell

88
Q

Two oxygen molecules binding together is an example of what type of bond?

A

Covalent bond

89
Q

Ionic bonds are when what two things on the periodic table come together?

A

Nonmetal and metal

90
Q

Covalent bonds are always…

A

2 nonmetals.

91
Q

Water is what type of bond?

A

Covalent bond…because the oxygen has 6 electrons and the oxygen shares both electrons from hydrogen…so oxygen now has 8 and hydrogen has 2

92
Q

Dipole to Dipole bonding is bringing what together?

A

MOLECULES

93
Q

Dipole means what?

A

The molecule has a positive side and a negative side

94
Q

So what is dipole-dipole bonding

A

When you are bringing together two molecules…the positive end of one polar molecule is bonded to the negative end of another polar molecule Ex: HCl binding to HCl…chloride end is partially negative and hydrogen is partially positive

95
Q

Water to water bonding is an example of what type of bond?

A

Hydrogen bonding…The hydrogen are partially positive and the oxygen is partially negative…so these molecules attract one another…this is the strongest of the dipole-dipole bonding.

96
Q

Hydrogen bonding is only possible when hydrogen is bonded to what other atoms?

A

F, O, or N….all considered electronegative atoms

97
Q

Hydrogen bonding holds the water molecules in the…

A

liquid state and prevents the water in our bodies from exploding away into the gas state.

98
Q

Boiling point for water is…

A

100 degree Celsius

99
Q

What is the weakest intermolecular forces?

A

London Forces

100
Q

Methane is a gas at….

A

Room temperature

101
Q

London forces are are created when electrons in a molecule are…

A

unevenly distributed…

102
Q

What is ion-dipole bonding?

A

Occurs between an ion and a polar molecule. Allows ionic solids to dissolve in water. Ex: bonding of sodium and chloride to a water molecule.

103
Q

CH3 is referred to as a…

A

methyl group- a common chemical group found in many organic substances including pharmacologic drugs.

104
Q

The methyl group acts as a….

A

RADICAL

105
Q

What is a radical?

A

Any group of atoms that have bonded together to act like an individual atom in chemical reactions… Example: Phosphate (PO4)3- Carbonate (CO3) 2-

106
Q

What are the halogens…

A

Cl (chlorine), F (Fluorine), Br (Bromine), I (Iodine), and At ( ) all of the halogen groups only have one covalent bond bc they all need one hydrogen to become “stable”

107
Q

The second most common hydrocarbon is what?

A

ETHANE—> two chain hydrocarbon

108
Q

Ethane contains what?

A

2 carbons that share an electron while the remaining electrons are paired with hydrogen electrons.

109
Q

Hydrocarbon with 3 carbon atoms…

A

Propane

110
Q

Hydrocarbon with 4 carbon atoms…

A

Butane

111
Q

Hydrocarbon with 5 carbon atoms…

A

Pentane

112
Q

Hydrocarbon with 6 carbon atoms…

A

Hexane

113
Q

Hydrocarbon with 8 carbon atoms…

A

Octane

114
Q

Hydrocarbon with 9 carbon atoms…

A

Nonane

115
Q

Hydrocarbon with 10 carbon atoms…

A

Decane

116
Q

Halothane is made up of what?

A

2 carbons, 1 hydrogen, 1 bromine, and 3 Florine and 1 chlorine.

117
Q

What is an isomer?

A

A compound with identical molecular formula (ex: C4H10), but several alternate structures (may look totally different drawn out)

118
Q

A type of isomer where written out it has an exact molecular formula but differ in chemical and physical properties…

A

Structural Isomer

119
Q

What is the definition of stereoisomers…

A

They have identical formulas but differ in their spatial arrangement (look similar drawn out but may have one tiny change in arrangement)

120
Q

What are the two types of stereoisomers:

A

Optical isomers and Geometric isomers

121
Q

Optical isomers are…

A

“Mirror images”

122
Q

This type of isomer occurs when groups attach to the carbon atom differ from one another in such a way as to polarize (bend) light…

A

Optical isomer—> Those that bend light to the right are called dextroisomers. Those that bend light to the left are called levoisomers

123
Q

When there is a mixture of both dextro and levoisomers, such that no bending of light occurs, the mixture is called…

A

Racemic….Ex: Racemic epinephrine (this is still a form of optical isomers)

124
Q

Geometric isomers are what?

A

Geometric isomers occur when compounds contain two carbon atoms with a double bond; the double bond prevents axial rotation.

125
Q

Two geometric isomers can occur what are they?

A

Cis isomer: where the groups are on the same side of the double bond (Cis isomer)
Trans isomer: When the groups are on the opposite side of the double bonds. (You have a picture in your phone)

126
Q

Molecules that share the same chemical formula but have their atoms connected differently, or arranged differently in space, are known as…

A

ISOMERS

127
Q

In Functional Groups…what does the R mean?

A

R stands for a carbon based group…so a carbon with a bunch of hydrogens.

128
Q

In Functional Groups…What does the X mean?

A

It is any Halogen atom (F, Cl, BR, I)
Generic Halogen formula= R-X where Ra means carbon chain and X means halogen atom…Most of the inhalation anesthetic agents fall into this class.

129
Q

The science that deals with structure and composition of matter is…

A

Chemistry

130
Q

What are a combination of elements and compounds

A

Mixtures Ex: Blood and air

131
Q

Molecular formula:

A

Gives a number of each type of atom in a molecule…Ex H20…the formula says 2 hydrogen and 1 oxygen

132
Q

Ion to Dipole bonding:

A

Occurs between an Ion and a polar molecule. Allows ionic solids to dissolve in water

133
Q

Hydrogen bonding is generally stronger than what other type of bond?

A

Dipole-Dipole

134
Q

This type of bond is arguable the most important of the intermolecular forces?

A

Hydrogen bonding

135
Q

The weakest of the intermolecular forces is what?

A

London forces

136
Q

What is london forces?

A

An instantaneous dipole that is created whenever electrons in a molecule are unevenly distributed

137
Q

Organic molecules have two parts: What are they?

A

Carbon backbone and one or more functional groups

138
Q

What is the generic halogen formula?

A

R-X, where X is any halogen

139
Q

Sevo, Iso, Enflurane, Des, and Halothane are all what?

A

Ethers

140
Q

_____ compounds are made by interacting an alcohol with an acid

A

Esters

141
Q

Ester formula

A

R-COO-R

142
Q

Ether Formula

A

R-O-R

143
Q

What is the study of the behavior of atoms and molecules that make up elements of matter?

A

Physics

144
Q

Heat

A

Is a form of energy

145
Q

Centigrade freezing point is ____ and boiling point is _____

A

0 and 100

146
Q

Fahrenheit freezing point is ____ and boiling point is ____?

A

32 and 212

147
Q

Kelvin begins at absolute zero and goes up

A

-273.16 C

148
Q

Conversion of Fahrenheit to centigrade:

A

C= (F - 32)/1.8

149
Q

Heat is transferred from areas of high temperature to areas of ________

A

low temperature

150
Q

Cold operating room are conductive for what?

A

Development of hypothermia

151
Q

Patient populations at increased risk for heat loss are who?

A

Children- increased body surface area and no body fat

Elderly- unable to increase BMR for heat production

152
Q

Transfer of heat from one molecule to another is an example of what?

A

Conduction: cold room temperature and cold surgical table

153
Q

What is the transfer of heat in electromagnetic waves?

A

Radiation: exposed patients (give warm blankets and use bear hugger)

154
Q

What is the transfer of heat by air currents?

A

Convection: Ex: Operating room air turnover = 15/hr, cold IV fluids

155
Q

What is the transfer of heat through humidity?

A

Evaporation: administering cold dry gases…can fix this with humidifiers on anesthesia circuits

156
Q

What is pressure?

A

The forces exerted by a collection of atoms or molecules

157
Q

Pressure is generated by what to sources?

A

Gravitational influences on the atom or molecule

The energy sources operating within the atom or molecule

158
Q

What is the kinetic theory of matter?

A

Movement of atoms/molecules is constant; the speed (velocity), direction (vectors), and movement (energy) can vary

159
Q

When molecules of gas collide, ______ is exerted

A

pressure

160
Q

What is the atmospheric pressures of gas at sea level?

A

760 torr

161
Q

A full E cylinder of oxygen measures ____ PSIG?

A

2200

162
Q

A full E cylinder of nitrous oxide measures ____ PSIG?

A

745

163
Q

What is the space occupied by a collection of atoms/molecules?

A

Volume

164
Q

Volume measurements?

A

Solids: cm^3, cc, m^3

Liquids and gases: mL or L

165
Q

The empirical gas laws demonstrate the interrelationships between..

A

Temperature, pressure, and volume

166
Q

Gases can be easily?

A

Compressed

167
Q

What do gases do?

A

Expand easily, are readily compressed, possess high velocities, and have weak intermolecular forces –> high degree of random motion

168
Q

Solutions help chemical reactions proceed more….

A

Quickly

169
Q

What is a solvent?

A

The substance into which the solute is placed

170
Q

What is a solute

A

The dissolved substance

171
Q

Solutions are not always liquid, they can be a…

A

Gas

172
Q

What is a homogeneous mixture that consists of one or mole solutions uniformly dispersed at the molecular or ionic level throughout a medium known as a solvent.

A

Solution

173
Q

The amount of solute that is dissolvable in a given amount of solvent depends on the what?

A

Temperature

174
Q

What are the two solution states?

A

Unsaturated: solutions permit the addition of more solute
Saturated: Solutions do not allow the addition of more solute without some of the solute precipitating out. However, heating the solvent allows for addition of more solute, producing a supersaturated solution

175
Q

What is the universal solvent?

A

Water

176
Q

Density is typically 1gm/ml unless altered by…

A

Temperature or pressure

177
Q

One of the most valuable functions of water is its ability to ______ many different substances.

A

Dissolve

178
Q

In a water molecule: The oxygen (atomic number 8) binds easily with 2 hydrogen because they share electrons (covalent bond) Is the hydrogen positive or negative?

A

The hydrogens are the positives and the oxygens are negative

179
Q

Because of the polar-ness of water the ionic substance such as NaCl break up into individual cations (Na+) and anions (Cl-) and…

A

dissolve into the solution

180
Q

What is the movement of water across a semi-permeable membrane to equilibrate a concentration gradient?

A

Osmosis

181
Q

The relative concentration of solutes in osmotic systems is called….

A

Tonicity

182
Q

If two fluids exert the same osmotic pressure then they are…

A

Isotonic: Ex: the solutions exert equal pressures but in opposite directions. Ex: 0.9% NS and PRBCS

183
Q

What is a solution that exerts higher osmotic pressure?

A

Hypertonic

Ex: 3% NaCL

184
Q

What do hypertonic solutions do?

A

They draw water from the surrounding RBC’s causing them to shrink

185
Q

What is a solution that has less of an osmotic pressure than that of blood?

A

Hypotonic solution

186
Q

What do hypotonic solutions do?

A

They cause surrounding RBC’s to take in more water, enlarging the cell.
Ex: water

Integrated Sciences Chemistry (1 decks)

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