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2
Atoms: The Constituents of Matter
• All matter is composed of atoms.
• Each atom consists of at least one proton and
one electron.
• Atoms have mass. The mass comes mostly from
the proton and a neutrally charged body called a
neutron.
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Atoms: The Constituents of Matter
• Each element contains only one type of atom.
• Information on elements is arranged in logical
order in a table called the periodic table.
• The periodic table arranges elements left to right
based on their atomic number, and in columns
based on similarities in their properties.
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Atoms: The Constituents of Matter
• Each element has a unique atomic number
which is the number of protons found in an atom
of the element.
• The mass number is the number of protons plus
the number of neutrons.
• The mass number is used as the weight of the
atom, in units called daltons.
• Each element has a unique symbol: H is
hydrogen, C is carbon, Na is sodium, and Fe is
iron.
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Atoms: The Constituents of Matter
• All atoms of an element have the same number of
protons, but not necessarily the same number of
neutrons.
• Atoms of the same element that have different
atomic weights are called isotopes.
2
Chemical Bonds: Linking Atoms Together
• Covalent bonds are very strong.
• Each covalent bond has a predictable length, angle,
and direction, which makes it possible to predict the
three-dimensional structures of molecules.
• A double covalent bond occurs when atoms share
two pairs of electrons; in triple covalent bonds
atoms share three electron pairs.
Figure 2.10 Covalent Bonding With Carbon
Properties of Molecules
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Chemical Bonds: Linking Atoms Together
• Electrons are not always shared equally between
covalently bonded atoms.
• The attractive force that an atom exerts on
electrons is called electronegativity.
• When a molecule has nuclei with different
electronegativities, an electron spends most of its
time around the nucleus with the greater
electronegativity.
2
Chemical Bonds: Linking Atoms Together
• Unequal sharing of electrons causes a partial
negative charge around the more electronegative
atom, and a partial positive charge around the
less electronegative atom, resulting in a polar
covalent bond.
• Molecules that have polar covalent bonds are
called polar molecules.
Figure 2.11 The Polar Covalent Bond in the Water Molecule
Properties of Molecules
2
Chemical Bonds: Linking Atoms Together
• Hydrogen bonds may form within or between
atoms with polar covalent bonds.
• The – portion of one molecule has a weak
attraction to the + portion of another molecule.
Each of these attractions is called a hydrogen bond.
• Hydrogen bonds do not share electrons.
• Although hydrogen bonds are weak, they tend to be
additive, and they are of profound biological
importance.
Figure 2.12 Hydrogen Bonds Can Form between or within Molecules
Properties of Molecules
2
Chemical Bonds: Linking Atoms Together
• Ionic bonds involve a complete transfer of one or
more electrons.
• Ions are formed when an atom loses or gains
electrons.
• Positively charged ions are called cations.
• Negatively charged ions are called anions.
Figure 2.13 Formation of Sodium and Chloride Ions
Properties of Molecules
2
Chemical Bonds: Linking Atoms Together
• Ionic bonds are formed by the electrical
attraction between ions with opposite charges.
• Table salt has chloride and sodium ions, held
together by ionic bonds.
• When salt is introduced into water, the partial
charges of the water molecules can easily
interfere with the ionic bonds.
Figure 2.14 Water Molecules Surround Ions
Properties of Molecules
2
Chemical Bonds: Linking Atoms Together
• Polar molecules tend to be hydrophilic.
Substances that are ionic or polar often dissolve
in water due to hydrogen bonds.
• Nonpolar molecules are called hydrophobic
because they tend to aggregate with other
nonpolar molecules.
• Nonpolar molecules are also attracted to each
other via relatively weak attractions called van
der Waals forces.
2
Chemical Reactions: Atoms Change Partners
• Chemical reactions occur when atoms combine or
change partners.
• In a chemical reaction, reactants are converted to
products.
• A chemical reaction can be written as an
equation. The equation must balance because
matter is neither created nor destroyed.
2
Chemical Reactions: Atoms Change Partners
• Changes in energy usually accompany chemical
reactions.
• Stored energy, such as that in chemical bonds, is
called potential energy and is available for future
use.
2
Water: Structure and Properties
• Due to its shape, polarity, and ability to form
hydrogen bonds, water has some unusual
properties.
2
Water: Structure and Properties
• Ice is held in a crystalline structure by the
orientation of water molecules’ hydrogen bonds.
• Each molecule forms hydrogen bonds with four
other molecules.
• These four hydrogen bonds increase the space
the water molecules take up, so water expands as
it freezes, and ice is less dense than liquid water.
• For these reasons, ice floats in liquid water.
2
Water: Structure and Properties
• A great deal of heat energy is required to change
the temperature of liquid water because the
hydrogen bonds must be broken.
• Specific heat is the number of calories needed to
raise one gram of a substance 1oC. The specific
heat of liquid water is 1.
• Liquid water has a higher specific heat than most
other small molecules in liquid form.
2
Water: Structure and Properties
• The heat of vaporization is the amount of heat
needed to change a substance from its liquid
state to its gaseous state.
• A lot of heat is required to change water to a
gaseous state because the hydrogen bonds of the
liquid water must be broken.
• Evaporation has a cooling effect by absorbing
calories.
• Condensing has the opposite effect, releasing
heat.
2
Water: Structure and Properties
• Water has a cohesive strength because of
hydrogen bonds.
• The cohesive strength of water molecules allows
the transport of water from the roots to the tops of
trees.
• Water has high surface tension, which means that
the surface of liquid water is relatively difficult to
puncture.
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Water: Structure and Properties
• Water is the solvent of life.
• Living organisms are over 70 percent water by
weight and many reactions take place in this
watery environment.
2
Water: Structure and Properties
• The mole concept is fundamental to quantitative
analysis. A mole is the amount of a substance in
grams whose weight is equal to its molecular
weight.
• One mole of any given compound contains
approximately 6.03 x 1023 molecules of that
compound (Avogadro’s number).
2
Acids, Bases, and the pH Scale
• Some substances dissolve in water and release
hydrogen ions (H+); these are called acids. Their
release is called ionization.
• Other substances dissolve in water and release
hydroxide ions (OH–); these are called bases.
• Acids donate H+; bases accept H+.
2
Acids, Bases, and the pH Scale
• Acids release H+ ions in solution.
• If the reaction is complete, it is a strong acid, such
as HCl.
• The carboxyl group (—COOH) is common in
biological compounds. It functions as an acid
because
 —COOH  —COO– + H+
2
Acids, Bases, and the pH Scale
• Bases accept H+ in solution.
• NaOH ionizes completely to Na+ and OH–. The
OH– absorbs H+ to form water. It is a strong
base.
• The amino group (—NH2) is an important part of
many biological compounds; it functions as a
weak base by accepting H+:
 —NH2 + H+  —(NH3)+
2
Acids, Bases, and the pH Scale
• Ionization of strong acids is virtually irreversible.
• Ionization of weak acids and bases is somewhat
reversible.
• Many large molecules in biological systems
contain weak acid or base groups.
2
Acids, Bases, and the pH Scale
• Water is really a weak acid and has a slight
tendency to ionize into H+ and OH–.
• This ionization is very important for living
creatures and the chemical reactions they must
perform because the H+ ion is so reactive.
2
Acids, Bases, and the pH Scale
• pH is the measure of hydrogen ion concentration.
• It is defined as the negative logarithm of the
hydrogen ion concentration in moles per liter.
• The pH scale indicates the strength of a solution
of an acid or base. The scale values range from 1
through 14.
• A pH 7 means the concentration of hydrogen ions
is 1 x 10–7 moles per liter of water.
2
Acids, Bases, and the pH Scale
• A buffer is a mixture of a weak acid and its
corresponding base.
• Because buffers can react with both added bases
and acids, they make the overall solution resistant
to pH change.
2
Properties of Molecules
• Functional groups give specific properties to
molecules.
• Functional groups are covalently bonded to
organic molecules.
• Amino acids are biological molecules that contain
both a carboxyl group and an amino group.
Figure 2.20 Some Functional Groups Important to Living Systems (Part 1)
Properties of Molecules
Figure 2.20 Some Functional Groups Important to Living Systems (Part 2)
Properties of Molecules
Figure 2.20 Some Functional Groups Important to Living Systems (Part 3)
Properties of Molecules
2
Properties of Molecules
• Isomers are molecules that have the same
chemical formula but different arrangements of
the atoms.
• Structural isomers differ in terms of how atoms
are joined together.
• Optical isomers are mirror images of each other.
• Optical isomers can occur whenever a carbon has
four different atoms or groups attached to it.
Figure 2.21 Optical Isomers
Properties of Molecules