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1
CLIFFS NOTES
CHEMISTRY
Chapter 2: The Cliff Notes to
Chemistry
• What is Chemistry?
• Atoms
• Subatomic Particles
• Chemical Bonds
• H2O
Chapter 2: The Cliff Notes to
ChemistryCLIFFS NOTES
CHEMISTRY
•Every object around you is made up of mass.
•Mass is made up of matter.
•Matter is made up of little particles called atoms.
• Chemistry is the science that deals with matter
• Matter is anything that takes up space and has
mass
– Living or non-living
• Smallest stable units of mass are atomsCLIFFS NOTES
CHEMISTRY
Why is Chemistry Important to
Biology?
CARBON ATOM
All living things are made of atoms
CARBON ATOM
Another Example
DNA
A Cell
Cells
Nucleus within cell
Kidney Tissue
An organ: Frog Kidney
An organism: A frog
All living things are made of
atoms
DNA
A Cell
DNA is a large molecule, comprised of atoms!!
nucleus
CARBON
ATOM
Zoom in
on DNA
2
• Atoms are composed of subatomic particles
The Structure of Atoms
– A proton is positively charged
– A neutron is electrically neutral
– An electron is negatively charged ]
Packed
In the atomic
nucleus
Orbits the
nucleus
How many protons, neutrons and electrons does a carbon atom have?
CARBON ATOM
The Structure of Atoms
How many protons, neutrons and
electrons does a helium atom have?
HELIUM ATOM
http://www.purchon.com/chemistry/helium.htm
The Structure of Atoms
• OK, atoms are obviously very, very, small and theyprobably don’t ‘weigh’ very much, or have much mass
• But, believe it or not, atoms do have mass
• Atomic mass is determined by the # of protons andneutrons.
• What is the atomic mass of a carbon atom? A heliumatom?
• Electrons do not contribute (much) to the mass (weight)of an atom.
Atoms
• Atomic mass (# of protons plus the # of
neutrons)
• Atomic number (# of protons)
• What about the electrons?++
++
What do you think makes a carbon
atom a carbon atom, and not a helium
atom?
HELIUM ATOM CARBON ATOM
Who am I?
What makes me
me?
What is the
meaning of life?
I think,
therefore I
am…a
carbon atom
Elements– Atoms are classified into groups called
elements
– Elements are substances that cannot be
broken down into other substances
– There are 92 naturally occurring elements on
Earth
– You can find all of them on the periodic table
HeliumLead
3
groups
periods
Periodic Table
(of course you do not have to memorize this!)
(C) Carbongroups
periods
Periodic Table
(of course you do not have to memorize this!)
Just focus
on these
four
elements
Why these four elements?
– 25 elements are
essential for life
– Four of these
make up about
96% of the
weight of the
human body
– Trace elements
occur in smaller
amounts
1.
2.3.
4.
The Periodic Table contains lots of
useful information
What does this tell us?
What does this tell us?
Why do we care?
• In an atom of carbon, if the atomic numberis 6, how many protons are there?
• How many electrons are there??
• It’s the electrons that we really care about!
+++
+
Electrons Orbit the Atomic Nucleus
• If protons were the size of a
tennis ball, electrons would
be orbiting the nucleus at a
distance of 6 miles away!!
• Outer most electrons (or
the lack-thereof) determine
how one atom interacts with
another atom
•Atoms may interact and form bonds, generating
larger, more complex molecules (like DNA)
4
DNA is a molecule
Molecules are made of atomsElectron Arrangement
• Electrons (e-) are arranged around the
atomic nucleus in electron shells (orbitals).
• Electron shells closest to the nucleus have
the lowest energy, while electrons farther
from the nucleus have greater energy.
• The first electron shell holds only 2 electrons
• The next electron shell holds up to 8 electrons
• The four elements most abundant in living things
only have these two shells (phew!)
Electron Shells
In case you forgot those four elements,
they are:
HYDROGEN (only has the first shell)
CARBON
NITROGEN
OXYGEN
Electron Arrangement in a Carbon Atom
Firstelectron shell(can hold2 electrons)
Outermostelectron shell(can hold8 electrons)
Carbon (C)Atomic number = 6
Electron Arrangement in a Carbon Atom
Firstelectron shell(can hold2 electrons)
Outermostelectron shell(can hold8 electrons)
Carbon (C)Atomic number = 6
Rules to figuring out electron
arrangement:
1. What is the atomic number?
2. The number of total electrons is
the SAME as the atomic number.
- For carbon, it is 6
3. Place two electrons in the ‘first’
inner shell
4. Place remaining electrons in the
outer shell.
***To understand how an atom will
interact with other atoms, look at
how many ‘open atom spots’
there are left in the outer shell!
What is the arrangement of outer
shell electrons in an oxygen atom?8
O16
5
Atoms of the four elements most
abundant in life
Electron
Firstelectron shell(can hold2 electrons)
Outermostelectron shell(can hold8 electrons)
Carbon (C)Atomic number = 6
Nitrogen (N)Atomic number = 7
Oxygen (O)Atomic number = 8
Hydrogen (H)Atomic number = 1
Outer shell
electrons?
Outer shell
electrons?Outer shell
electrons?
Outer shell
electrons?
Atoms ‘prefer’ to have their outer
shell FILLED with electrons!
Oxygen (O)Atomic number = 8
Hydrogen (H)Atomic number = 1
I, HYDROGEN,
would strongly
prefer to have 2
electrons in my
outer shell, and
not just 1!
I, OXYGEN,
would strongly
prefer to have 8
electrons in my
outer shell, and
not just 6!
• The first electron shell holds only 2 electrons
• The next electron shell holds up to 8 electrons
• Atoms (with the exception of Hydrogen and
Helium) prefer to have 8 electrons in the outer
electron shell
• The octet rule.
Atoms can ‘fill’ their outer electron shells
by forming chemical bonds with other
atoms
• Atoms can steal electrons from other
atoms; atoms can lose electrons to other
atoms
– Ionic bonds
• Atoms can share electrons with another
atom or atoms
– Covalent bonds
Next up….Chemical Bonds
Oxygen (O)Atomic number = 8Hydrogen (H)
Atomic number = 1
…..OR, what
will happen
when an atom
of OXYGEN
‘sees’ an atom
of
‘HYDROGEN’?
..Two atoms of
HYDROGEN??
Elements with unfilled electron
shells are reactive
• Chemical bonds are formed
• Three types of chemical bonds
1. Ionic bonds
2. Covalent bonds
3. Hydrogen bonds
Oxygen (O)Atomic number = 8
Hydrogen (H)Atomic number = 1
Hey there
hydrogen,
you wanna
bond??
6
Ionic bonds are formed between
ions
• Remember that the atoms we have
discussed so far are electrically neutral
• Because the number of protons (+) was
equal to the number of electrons (e-)
• An ion is a charged species
– Anions
– Cations
Anions and Cations
• If an atoms gains an electron (e-), what happens
to its electrical charge?
• If an atom loses an electron (e-) what happens
to its electrical charge?
Formation of a sodium ion, Na+
Ionic bonds are formed between
ions
Sodium metal Chlorine GasTable salt (NaCl)
+
Ionic Bonding
Reactant(s) Product(s)
In a CHEMICAL REACTION there are reactants and
products. Note that during chemical reactions no atoms
are gained or lost, they are just rearranged!
Na Cl
http://jchemed.chem.wisc.edu/JCESoft/CCA/CCA0/Movies/NACL1.html
Covalent bonds occur when
atoms share electrons
or H-H or H2H H
e- e-
http://www.visionlearning.com
Covalent Bonds
• Example from www.visionlearning.com
• For every pair of electrons shared
between two atoms, a single covalent
bond is formed.
– In H2 there is ONE covalent bond
• Some atoms can share multiple pairs of
electrons, forming multiple covalent bonds.
7
Methane is a simple compound, consisting of one
atom of carbon and 4 atoms of hydrogen
In methane, Carbon has four covalent bonds to 4
different hydrogen atoms
Covalent Bonds
C
H
H
H
H
Covalent Bonds
• Are strong because the shared electrons
hold the atoms together
• Typically, the atoms involved in covalent
bonds remain electrically neutral
• Found in most of the carbon-containing
structural components of living things
H H
e- e-
Scary Figure Polar Covalent Bonds
• Polar covalent bonds are a type of
covalent bond
• Characterized by an unequal sharing of
electrons
e- Unfair!
Polar Covalent Bonds
• Polar covalent bonds form because
some atoms have a stronger affinity
for electrons than do other atoms
• Electronegativity
e-
Strongly
electronegative
Polar covalent bonds can result
in polar molecules
• In a polar covalent bond, one atom ‘pulls’ onelectrons more tightly than the other atom.
• The more electronegative atom ‘hogs’ electrons
• Thus, electrons will spend more time (onaverage) around the electronegative atom
• A slight or partial negative charge results
• The ‘electronegative’ end of the molecule has aparital negative charge
8
Polar covalent bonds can result
in polar molecules
• Oxygen is an electron (e-) hog
– oxygen is a very electronegative atom
– Oxygen has a strong desire for electrons,and once it has them, it ‘pulls’ on them verytightly
• Oxygen forms polar covalent bonds withhydrogen atoms
• Water (H2O) is one oxygen bound to twohydrogens
• H2O is a polar molecule
Polar Covalent Bonds: H2O
Oxygen (O)Atomic number = 8Hydrogen (H)
Atomic number = 1
What will happen when an atom of OXYGEN
‘sees’ an atom of ‘HYDROGEN’?
..Two atoms of HYDROGEN??
Oxygen (O)Atomic number = 8Hydrogen (H)
Atomic number = 1
What will happen when an atom of OXYGEN
‘sees’ an atom of ‘HYDROGEN’?
..Two atoms of HYDROGEN??
Hydrogen (H)Atomic number = 1
Polar Covalent Bonds: H2O
e- e-
Polar Covalent Bonds: H2O
•www.visionlearning.com
Polar covalent bonds can result
in polar molecules
2!-
!+
!+
Polar covalent bonds can result
in polar molecules
2!-
!+
!+
Partial negative
charge
Partial
positive
charge
9
What happens when one water
molecule ‘sees’ another water
molecule?
H
O
H
H
O
H
Hydrogen bonding occurs
between water molecules
Which of the following orientations of two
H2O molecules is most likely to occur?
POP QUIZ
Which of these do you think is
correct?
2!-
A. B. C.
Opposites will attract!
2!-
A. B. C.
Opposite charges will
attract one anotherLike charges would repel one another
Hydrogen bonding occurs
between water molecules
2!-
A. B. C.
Hydrogen
Bonds!
Like charges would repel one another
Hydrogen bonding
• Weak but important forces
• Can exist between adjacent molecules
• Occur when (partial negative ) !- is attracted to
(partial positive ) !+ of a Hydrogen atom
10
Hydrogen bonds are weak (but
biologically important) bonds
•Hydrogen bonding
between water molecules
is transient (fleeting)
•Hydrogen bonding
keeps water molecules
very tightly associated
with one another
Hydrogen bonding gives H2O many
unique properties
• Water as a good solvent
• Water molecules stick
together
– Cohesion and surface tension
• Water can resist
temperature change better
than other liquids
Water as a Solvent
Ion in solution
Salt crystal
• What happens, at the molecular level,
when water is mixed with an ionic
compound, like table salt (NaCl)?
Ion in solution
Salt crystal
• What happens, at the molecular level,
when water is mixed with an ionic
compound, like table salt (NaCl)?
Na+
Cl- Water molecules surround the
charged species, interact closely with
them, and disrupt the salt crystal.
Water as a Solvent
http://programs.northlandcollege.edu/biology/Biology1111/animations/dissolve.html
• Water moleculesstick together asa result ofhydrogenbonding
The Cohesion of Water
– This is called
cohesion
– Cohesion is vital
for water
transport in plants
Microscopic tubes
evaporation
H2O
The Cohesion of Water
11
• Surface tension is the measure of howdifficult it is to stretch or break the surface ofa liquid
– Hydrogen
bonds give
water an
unusually high
surface tension
Figure 2.13
What is heat?
Molecules are always moving
around randomly, they ‘jiggle’.
Heat is just a measure of ALL
of these molecular movements,
in a body of matter.
TEMPERATURE: the
average SPEED of this
movement….”JUST HOW
FAST IS THIS MATTER
MOVING?”
What happens when a
solution of methane is
heated?
What happens when water
is heated??What happens FIRST???
What happens NEXT??
Water accounts for 2/3rds of
total body weight• Water can dissolve many molecules
making a solution
• Water is needed for some chemical
reactions
• Water can absorb and retain heat
How might water interact with
uncharged, non-polar molecules?
• Olive oil, a lipid
• A generalized triglyceride structure….
Gly
cero
l
Long, non-polar (not charged) chains of
carbons and hydrogens
Do water and oil ‘mix’?
Water molecules tend to be attracted
more to each other than to a non-
polar region of a molecule.
This results in the
non-polar
molecules being
‘excluded’ by
water.
non-polar region
12
Hydrophilic and Hydrophobic
Compounds• Hydrophilic compounds react readily with
water molecules
• Hydrophobic molecules do not readily
react with water
Na+
Cl
-
Hydrophilic Hydrophobic
Ionic and covalent bonds form…
• Molecules: a chemical structure containing
two or more atoms that are held together by
covalent bonds
• Compounds: a chemical substance made of
atoms of 2 or more elements