Ch. 2 The Nature Of Molecules And The Properties Of Water Flashcards

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1
Q

_______ have a nucleus made of _______ and ______ which is surrounded by orbiting ______. The numbers of these particles determine the character of an element.

A

Atoms; protons; neutrons; electrons

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2
Q

What’s the charge of each sub-atomic particle? Protons? Neutrons? Electrons?

A

Positive, neutral (no charge), negative

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3
Q

Any substance in the universe that has mass and occupies space is defined as ______

A

Matter

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4
Q

All matter is composed of extremely small particles called ________

A

Atoms

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5
Q

Different atoms are defined by the # of protons, a quantity called the ________ ________

A

Atomic number

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6
Q

An _______ is any substance that cannot be broken down to any other other substance by ordinary chemical means

A

Element

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7
Q

The ________ of an atom is equal to the sum of the masses of its protons and neutrons.

A

Atomic mass

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8
Q

The mass of atoms and subatomic particles is measured in units called _________

A

Daltons

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9
Q

Electrons are located in regions called _________ along atom _________

A

Orbitals; shells

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10
Q

An atom with an unequal amount of protons and electrons is known as a(n) _______

A

Ion

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11
Q

Atoms with more protons than electrons, being positively charged are called ________

A

Cations

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12
Q

Atoms with more electrons than protons, being negatively charged are called ______

A

Anions

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13
Q

Atoms of a single element with different numbers of neutrons are called _______

A

Isotopes

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14
Q

Decay time is expressed as ________

A

Half-life

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15
Q

No orbital can contain more than _______ electrons

A

Two

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16
Q

The loss of an electron is called ______, the gain of an electron is called _______

A

Oxidation; reduction

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17
Q

When oxidation + reduction occur at the same time

A

Redox reactions

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18
Q

Electrons on outermost energy level/shell

A

Valence electrons

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19
Q

Electrons possessing all eight electrons in their outer most energy level are _______, these elements are known as ________

A

Nonreactive; noble gasses

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20
Q

A group of atoms held together by energy is called a ______

A

Molecule

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21
Q

Molecules contains atoms of more than one element are called _______

A

Compounds

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22
Q

Atoms within molecules are joined by _______

A

Chemical bonds

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23
Q

_______ bonds occur when opposite charges attract each other (Na- Cl+)

A

Ionic

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24
Q

________ bonds occur when atoms share one or more pair of valence electrons (sharing) H2O

A

Covalent

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25
Q

Atoms differ in their affinity for electrons, a property called ________

A

Electronegativity

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26
Q

The strength of covalent bonds is dependent on the number of shared _______

A

Electrons

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27
Q

Bonds between identical atoms, with the affinity for electrons being the same are termed ________

A

Non polar

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28
Q

Atoms that differ greatly in electronegativity, where electrons can not be shared as easily/equally are termed _______

A

Polar

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29
Q

When drawing polar molecules, partial charges are symbolized by the lowercase Greek letter _________

A

Delta (S)

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30
Q

The formation and breaking of chemical bonds is termed a _______

A

Chemical reaction

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31
Q

Original molecules________, result from reaction _________

A

Reactants; products

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32
Q

What 3 factors increase the rate of a reaction?

A

Heat/Temperature; concentration of reactants/products (more reactants available=more frequent collisions); catalysts i.e. enzymes

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33
Q

Many reactions in nature are _______, meaning _________ may also be __________

A

Reversible; products; reactants

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34
Q

How is a covalent bond different from an ionic bond?

A

An ionic bond results when there is a complete ‘ ‘ transfer of electrons between atoms, resulting in positive and negative ions that are attracted to each other. Covalent bonds are the result of two atoms sharing electrons. Polar covalent bonds involve unequal sharing of electrons, producing regions of partial charge. (Draw examples)

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35
Q

_________ bonds form between the partially negative O atoms and the partially positive H atoms of two water molecules

A

Hydrogen Bonds

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36
Q

Water likes substances with which it can form hydrogen bonds. _______ is responsible for ___________. (The polarity of water causes it to be attracted to other polar molecules as well)

A

Adhesion; Capillary action

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37
Q

The polarity of WATER allows WATER molecules to be attracted to one another, this property is known as _________. _______ is responsible for __________.

A

Cohesion; surface tension

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38
Q

Hydrogen bonds absorb heat when they break and release heat when they form, minimizing temp changes.

A

High specific heat

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39
Q

Water stabilizes the temp of organisms and the environment

A

High specific heat

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40
Q

Many hydrogen bonds must be broken for water to evaporate

A

High heat of vaporization

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41
Q

Evaporation of water cools body surfaces

A

High heat of vaporization

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42
Q

Water molecules in an ice crystal are spaced relatively far apart because of hydrogen bonding

A

Lower density of ice

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43
Q

Due to the ___________, lakes do not freeze solid, allows fish & other life in lakes to survive the winter

A

Lower density of ice

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44
Q

Polar water molecules are attracted to ions and polar compounds, makings these compounds _________

A

Soluble; solubility

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45
Q

Many kinds of molecules may move freely in cells, permitting a diverse array of chemical reactions

A

Solubility

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46
Q

________ molecules shrink from contact with water. Water molecules act to exclude them.

A

Hydrophobic; water-hating

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47
Q

Polar molecules, which readily form hydrogen bonds with water are considered ________

A

Hydrophilic; water-loving

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48
Q

A _______ is defined as the weight of a substance in grams that corresponds to the atomic masses of all the atoms in a molecule of that substance

A

Mole

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49
Q

The concentration of hydrogen + hydroxide ions in a solution is described using _______

A

Acidity & basicity

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50
Q

The pH scale is________, a difference of 1 on the scale represents a 10-fold change in ___.

A

Logarithmic; H+

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51
Q

Any substance that dissociates in water to increase the ____ & ______ the pH is called an _______

A

H+; lower; acid

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52
Q

Any substance that combines with ____ when dissolved in water, lowering the ____ is called a ______

A

H+; H+; base

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53
Q

The _______ an ______ is, the more _______ ions it produces and the ________ its pH

A

Stronger; acid; hydrogen; lower

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54
Q

A ______ is a substance that resists change in pH.

A

Buffer

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55
Q

_______ act by _________ hydrogen ions when a base is added and __________ hydrogen ions when acid is added, with the overall effect of keeping _______ relatively constant.

A

Buffers; releasing; absorbing; H+

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56
Q

__________ bonds involve unequal sharing of electrons, producing regions of partial charge.

A

Polar covalent

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57
Q

Any substance that has mass + occupies space

A

Matter

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58
Q

All matter is composed of small particles called ______

A

Atoms

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59
Q

At the center ______, made up of _______ + _______

A

Nucleus;protons;neutrons

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60
Q

of protons, otherwise known as ________;

A

Atomic Number

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61
Q

Substance that cannot be broken down to other substance by normal means

A

Element

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62
Q

Proton (); Electron (); Electrically neutral if ______

A

Positive;Negative;Equal

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63
Q

Amount of a substance

A

Mass

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64
Q

Force gravity exerts on a substance

A

Weight

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65
Q

Sum of proton + neutron masses

A

Atomic Mass

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66
Q

Mass of atoms & subatomic particles expressed in ______

A

Daltons

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67
Q

Electrons are maintained in their _______ by their attraction to ______ charged nucleus

A

Orbitals;positively

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68
Q

Electrons not equally protons results in formation of

A

Ions

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69
Q

Protons>electrons

A

Cations (NA+)

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70
Q

Protons

A

Anions(Cl-)

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71
Q

Single element with dif # of neutrons results in

A

Isotopes

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72
Q

Unstable, ________ decay -> radioactive ________; decay expressed as ______

A

Radioactive;isotopes;half-life

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73
Q

No orbital can contain more than ______ electrons

A

Two

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74
Q

Atoms contain ________ _______ levels

A

Discrete;energy

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75
Q

Loss of electron = _______

A

Oxidation

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76
Q

Gain of electron =

A

Reduction

77
Q

Loss & gain of electron =

A

Redox reaction

78
Q

________ determine the chemical behavior of atoms

A

Electrons

79
Q

____ of electrons increases as distance from nucleus ________

A

PE; increases

80
Q

Periodic table based on interactions of _________ in the ________ energy level

A

Electrons;outermost/valence

81
Q

Chemical behavior reflects how many of the _______ positions are filled

A

Eight

82
Q

Majority of molecules that make up the body

A

Organic compounds

83
Q

Elements with filled outermost energy levels are __________

A

Nonreactive

84
Q

Group of atoms held together by energy

A

Molecules

85
Q

Molecules with atoms of more than 1 element

A

Compound

86
Q

Atoms in molecule are joined together by __________

A

Chemical bonds

87
Q

__________ charges attract eachother = __________

A

Opposite;ionic bonds

88
Q

Sharing of 1 or more pairs of electrons = ________

A

Covalent bonds

89
Q

Strength of covalent bond depends on the _________ of shared _________

A

Number;electrons

90
Q

Atoms differ in their affinity for electron =

A

Electronegativity

91
Q

Electrons equally shared, similar electronegativity =

A

Nonpolar

92
Q

Atoms unequally shared, differ greatly in electronegativity

A

Polar

93
Q

Unequal distribution results in partial _________ charge near the ______ electronegative atom & regions of partial _______ charge near the less electronegative atoms = _______

A

Negative;more;positive;polar covalent bond

94
Q

Greek letter to represent partial charge

A

Delta (S)

95
Q

Formation + breaking of chemical bonds =

A

Chemical reaction

96
Q

Original molecules in reaction =

A

Reactants

97
Q

Results in chemical reaction =

A

Products

98
Q

Factors influencing rate of reaction include ______,_______, and ________

A

Temp/heat;concentration of reactants;catalysts

99
Q

Reactants & products can be ________

A

Reversible

100
Q

Ionic bonds form _______

A

Crystals

101
Q

Water facilitates __________ bonding

A

Hydrogen

102
Q

Waters most important chemical property

A

Hydrogen Bonding

103
Q

Weak chemical associations between water molecules

A

Hydrogen bonds

104
Q

H bonds form between partially ________ O atoms and partially _________ H atoms of two water molecules

A

Negative;positive

105
Q

The _________ of water allows water molecules to be attracted to one another = _________

A

Polarity;cohesion

106
Q

Oxygen end(); Hydrogen end()

A

-;+

107
Q

Cohesion is responsible for ___________

A

Surface tension

108
Q

Surface water molecules hydro bonded to molecules below them

A

Surface tension

109
Q

Polarity allows water to be attracted to other polar molecules

A

Adhesion

110
Q

Adhesion is responsible for __________

A

Capillary action

111
Q

NaCl ________ with water due to water ability to form ________ bond with _________ molecules

A

Dissolves;hydrogen;polar

112
Q

Water is the _______; sugar/table salt is the _______

A

Solvent;solute

113
Q

Water molecules surround NaCl ions; prevents it from association with other sucrose materials

A

hydration shell

114
Q

Water moderates _______ through 2 properties, ________ & _________

A

Temperature;high specific heat; heat of vaporization

115
Q

1g of substance must absorb or lose to change its temp by 1C

A

High specific heat

116
Q

Property that allows organisms to maintain a relatively constant internal temp

A

High specific heat

117
Q

Amount of energy required to change 1g of a substance from a liquid to a gas

A

Heat of vaporization

118
Q

Property responsible for sweating/evaporative cooling

A

Heat of vaporization

119
Q

________ water is less dense than ______ water

A

Solid;liquid

120
Q

Property responsible for ice floating, fish + animals from freezing

A

Ice less dense than liquid water

121
Q

Water molecules gather ________ around any substance that bears an _________ charge

A

Closely;electrical

122
Q

________ molecules ie. _____, are unable to form hydrobonds when placed in water

A

Non polar;oils

123
Q

Water molecules act to exclude, non polar molecules aggregate/clump together

A

Hydrophobic

124
Q

Polar molecules readily form _______ bonds = ________

A

Hydrogen;Hydrophilic

125
Q

Concentration of hydrogen ions + hydroxide ions =

A

Acidity & basicity

126
Q

Ph scale is _______, dif of 1 on scale is ________fold

A

Logarithmic;10fold

127
Q

Any substance that dissociates in water to ___________ the H+ and _______ the pH is a(n)

A

Increase;lower;acid

128
Q

Stronger the acid, ______ H+ is produces and _______ its pH

A

more;lower

129
Q

A substance that ________ with H+ in water to _________ its own H+ is a _________

A

Combines;lower;base

130
Q

Substance that resists pH change

A

Buffer

131
Q

Release H+ for _____

A

Bases

132
Q

Absorb H+ for ______

A

Acids

133
Q

Tendency of non polar molecules to aggregate is known as _________

A

Hydrophobic exclusion

134
Q

Spontaneous ion formation of water

A

Ionization

135
Q

Weight of a substance in g; cooresponds to atomic mass of all atoms in a substance

A

Moles

136
Q

When 2 atoms with different electronegative potentials engage in a covalent bond, it will result in a ________ charge

A

Partial

137
Q

>>=

A

O;N;C;H

138
Q

Why do water molecules stick to eachother

A

Water molecules are polar so the partially negative Oxygens are attracted to the partially positive Hydrogens

139
Q

Weak association found with hydrogen in polar covalent bonds

A

Hydrogen bonds

140
Q

In water, partially ________ Hydrogen is associated with partially _______ Oxygen; little _______

A

Positive;negative;magnets

141
Q

Hydrogen bonds are _________ ________ bonds

A

Weak transient

142
Q

Why is water a good solvent?

A

It’s ability to form hydrogen bonds with other molecules, ability to make weak associates, associate with other molecules

143
Q

If something is soluble in water….

A

It can form a hydrogen bond

144
Q

Why can’t oil dissolve in water?

A

Oil is hydrophobic, inability to form hydrogen bonds

145
Q

Molecules that have charges that can form hydrogen bonds

A

Hydrophilic, water loving

146
Q

Molecules that lack charges and cannot form hydrogen bonds

A

Hydrophobic

147
Q

Electronegativity differs -> ______ charges -> ability to ______ ______ bonds

A

Partial;form;hydrogen

148
Q

Bonding between unlike molecules, ex. _______

A

Adhesion;capillary action

149
Q

Bonding between like molecules, ex. ________

A

Cohesion;surface tension

150
Q

Density - ______>______>______

A

Water;ice;water vapor

151
Q

Why is ice less dense?

A

Water molecules with ice crystalline matrix are further in distance from one another than in liquid water

152
Q

What is an ionic bond?

A

Two atoms held together through opposite charges gained via the movement/transfer of an electron from one atom to another

153
Q

What is a molecule?

A

Group of atoms bonded together, most fundamental unit of a chemical compound

154
Q

What are the relative electronegativities of the four most abundant atoms found in living things?

A
155
Q

What partial charge would be created by the exposed protons from the hydrogens?

A

Partial Positive

156
Q

What partial charge would be created by the exposed electron pairs from the oxygen

A

Partial negative

157
Q

What Greek letter is used to denote partial charges created by electronegativity?

A

Delta (S)

158
Q

Why does table salt readily dissolve in water?

A

The negative Cl- is attracted to the positively charged Hydrogen atom of a water molecule, with the Na+ being attracted to the negatively charged Oxygen atom of the molecule

159
Q

What property of water molecules makes it a solvent

A

Waters partial positive and negative charges determine its polarity, and its polarity along with its ability to form hydrogen bonds and break substances down makes it a good solvent

160
Q

What is molecular cohesion and how does it relate to water?

A

Molecular cohesion is the attraction between the same kinds of molecules, water is strongly cohesive due to its ability to hydrogen bond.

161
Q

What is molecular adhesion and how does it related to water?

A

Molecular adhesion is the attraction to different kinds of molecules, and water possesses this property due to its polarity

162
Q

Why is oil insoluble in water?

A

Oils and fats are non polar so they are unable to break the hydrogen bonds of water. This causes the oil to stay separate and exclude itself from the water.

163
Q

H+Cl- is the formula for hydrochloric acid. Why would this molecule make an acidic solution?

A

Hydrochloric acid is held together by ionic bonds and when placed into water, breaks away to form hydrogen ions, resulting in an acidic liquid. HCl has a very low pH, thus is very acidic.

164
Q

H2O + H+Cl- -> _____ + _____

A

H3O+;Cl-

165
Q

Na+OH- is the formula for sodium hydroxide, a strong base. What makes this molecule basic?

A

Sodium hydroxide is a strong base because it dissociates entirely in water to form sodium cations an hydroxide anions. The hydroxide anions make this solution a strong base.

166
Q

If you add lemon to your tea how is the pH affected?

A

Lemon juice is acidic, so in adding lemon to your tea would lower its pH.

167
Q

How does adding lemon to tea affect the proton/hydronic content of the tea?

A

Lemon juice is highly acidic thus having a very high amount of hydrogen ions. Adding lemon to your tea would not only lower its pH, but increase its H+ ions and concentration as well.

168
Q

If you add milk to coffee, how is the pH of the coffee affected?

A

The pH of coffee is raised due to milks higher pH, making it slightly less acidic and more basic

169
Q

How does adding milk to coffee affect the proton/hydronic content of the coffee?

A

Adding milk to coffee lowers the concentration of H+ ions in the coffee ….

170
Q

If a proton attaches to water it forms a ________

A

Molecule

171
Q

A molecule defined as a base removes _______ from a solution

A

Hydrogen ions

172
Q

A molecule defined as an acid adds excess ______ to a solution

A

Hydrogen ions

173
Q

PH is determined by the concentration of _______ in a solution

A

Hydrogen ions

174
Q

What is a covalent bond?

A

Two atoms held together because they share a pair of electrons

175
Q

What is a molecule?

A

Two or more atoms held together by a covalent bond

176
Q

What is a hydrogen bond?

A

The electrostatic interaction between the partial positive charge of an exposed proton (hydrogen) in one molecule and the partial negative charge of outer shell electrons in the other

177
Q

What is an ionic bond?

A

A transfer of electrons between oppositely charged attracted atoms

178
Q

Why does table salt readily dissolve in water?

A

The full charges of the Na+ and Cl- attract the partial charges found on the water molecule

179
Q

What property of water molecules makes it a solvent?

A

It’s ability to form hydrogen bonds with charged or partially charged atoms

180
Q

What is a hydrophilic molecule?

A

A molecule with a partial or full charge that is attracted to water

181
Q

What is a hydrophobic molecule?

A

A neutral molecule that is not attracted to water

182
Q

What is molecular cohesion and how does it relate to water?

A

The attraction of like molecules to one another & water molecules are attracted to one another by way of partial charges

183
Q

What is molecular adhesion and how does it relate to water?

A

The attraction of unlike molecules to one another, water molecules are attracted to any molecules with a full or partial charge, other polar molecules

184
Q

Which is more dense and why, water vapor, water, or ice?

A

Liquid water is more dense than solid ice or water vapor because the molecules of liquid water are closer than those of ice or vapor

185
Q

Why is oil insoluble in water?

A

Oil is a neutral molecule so there are no charges for water to attach

186
Q

Why did we start a biology class by reviewing basic chemistry?

A

Living things themselves are made up of chemical composition. Our survival is dependent on the chemical reactions taking place inside our bodies.

187
Q

Explain one way a covalent bond differs from a hydrogen bond

A

Covalent bonds differ in that they are sharing chemical bonds that are found due to the sharing of electrons between atoms, whereas hydrogen bonds are weak bonds formed by the partial attractions between H & O atoms of water molecules.

188
Q

Explain why water has partial charges even though the molecule has a net equal number of electrons and protons, i.e. the overall charge of the molecule is neutral.

A

While water does have an equal number of electrons and protons, due to a difference in electronegativity, the electrons are unequally shared which results in these partial positive and partial negative charges seen with H and O.

189
Q

Explain the role of hydrogen bonding in creating the properties of liquid water

A

Hydrogen bonds cause water to be strongly attracted to other water molecules, which gives way for its cohesive property and water being the ultimate solvent, being able to form hydrogen bonds with like molecules.