1. The document discusses the basic chemistry concepts of matter, elements, atoms, and the structure of atoms. It explains that all matter is made of elements, which are made of only one type of atom consisting of protons, neutrons, and electrons. 2. Key concepts like the periodic table, atomic structure, isotopes, chemical bonds, and chemical formulas are defined. Ionic and covalent bonding are explained as the two main types of chemical bonds that form compounds. 3. Water is discussed as an essential compound for living things due to its unique polar molecular structure and ability to form hydrogen bonds, giving it cohesive and adhesive properties important for biological functions. Solutions and suspensions are also defined.

1. The Chemistry of LifeThe Chemistry of Life
Presented By:
Mrs. Nelson

2. ““Matter and Elements”Matter and Elements”
 Everything on earth is made of matter
 Matter - has mass and takes up space
(volume).
 Matter is made up of atoms.
 Atom - smallest unit of matter.
 Element – made of only one type of atom.

3. Periodic TablePeriodic Table
Element Symbols to LearnElement Symbols to Learn
 Hydrogen
 Carbon
 Nitrogen
 Oxygen
 Sodium
 Magnesium
 Silicon
 Phosphorus
 Uranium
 Sulfur
 Chlorine
 Potassium
 Calcium
 Iron
 Zinc
 Iodine
 Mercury
 Lead

4. ““Structure of the Atom”Structure of the Atom”
 Nucleus: core
contains protons
and neutrons
 Protons (+)
 Neutrons (0)
 Electrons (-) orbit
the nucleus
 Atoms are
electrically neutral.

5. ““Element Key”Element Key”
Atomic #
Symbol
Atomic Mass

6. Mass of an AtomMass of an Atom
 The mass of an atom is due to the mass of protons,
neutrons, electrons.
 Protons and neutrons are HUGE vs. electrons.
 Protons and neutrons have essentially the same mass
(1 amu).
 The more protons and neutrons, the heavier the
atom.
 Electrons have essentially no mass (0.00001 amu).
 Most of the mass of atom located in nucleus.

7. Atomic Mass vs. Mass Number
Atomic mass- average mass of all the
isotopes of an element (listed on the
periodic table)
Mass Number- the amount of all the
particles with “significant” mass in an atom
(technically not given on the periodic table)
-protons + neutrons

8. ““Element Key”Element Key”
Atomic #
Symbol
Atomic Mass
(determines mass number)

9. IsotopesIsotopes
All atoms of same element have same # of
protons and electrons.
Ex.) Carbon has 6 protons and 6 electrons.
Not all atoms have same # of neutrons.
Carbon has 3 isotopes: Carbon-12, Carbon-
13, Carbon-14

10. Isotopes (cont.)Isotopes (cont.)
Carbon has an atomic number of 6.
This tells us?
Carbon atoms all have 6 protons.
Carbon has 3 isotopes: C-12, C-13, C-14.

11. IsotopesIsotopes
How many neutrons does each have?
To determine the number of neutrons –
must subtract number protons from mass
number
Carbon-12 (6 p, 6 n, 6 e)
Carbon-13 (6p, 7 n, 6 e)
Carbon-14 (6p, 8n, 6 e)
* The atomic mass of an atom is calculated by
averaging the masses of all the isotopes of
an element.

12. “Happy vs. Sad Atoms”
 Atoms want to
have full outer
level of electrons.
 2,8,8
 Valence
electrons

13. “Atomic Bonding”
In order for atoms to be “happy,”
they must gain, lose, or share
electrons.
Results in “bonding.”
When atoms bond, they form
compounds.

14. “Chemical Formula”

15. Chemical FormulasChemical Formulas
Shows …
1. The types of atoms in the compound.
2. The number of atoms in the molecule.
3. The total number of molecules.
CO2
Subscript
2
Coefficient

16. Chemical BondsChemical Bonds
The atoms in a compound are held together
by chemical bonds.
There are two general types of chemical
bonds.
1. Ionic bonds
2. Covalent bonds

17. ““Ionic Bonding”Ionic Bonding”
Ex.) Sodium Chloride
Results in atoms losing or
gaining electrons.
“Ions” are formed.
“Ions” atoms with charges.
Charge results from an unequal
number of protons and electrons.

18. Ionic BondingIonic Bonding

19. ““Covalent Bonding”Covalent Bonding”
Sometimes atoms don’t like to give
or take electrons.
Atoms may “share” electrons.

20. “Polarity”
 Sometimes sharing is
“unequal.”
 In water, the oxygen
atom “pulls” harder
on electrons.
 Gives oxygen a
negative charge and
hydrogen positive
charge.

21. The Chemistry of WaterThe Chemistry of Water
Water is the single most
abundant compound found in
living things.
Water is an essential component
to your cells.
The inside of every body cell
consists of over 90% water.

22. The Water MoleculeThe Water Molecule
Water molecules contain
“covalent” bonds.
The water molecule is
“polar.”
Negative pole is near the
oxygen end.
Positive pole is near the
hydrogen end.

23. Hydrogen BondsHydrogen Bonds
Because of their partial
+ and – charges, water
molecules attract each
other.
Remember… Opposites
attract!!!

24. CohesionCohesion
The hydrogen bonds that
form between water
molecules are what allows
spiders to walk on water.
Water is cohesive.
Cohesion is the attraction
between molecules of THE
SAME substance.
Water sticks to itself.

25. AdhesionAdhesion
Adhesion is the attraction between molecules
of DIFFERENT substances.
Water sticks to other stuff!

26. SolutionsSolutions
Water is not always pure.
It is often found mixed with other substances.
Solutions occur when a substance is dissolved in
water. The substance is evenly distributed
throughout the water.
In every solution, there is a solute and solvent.
The solvent does the dissolving
The solute gets dissolved.
Ex.) saltwater

27. SuspensionsSuspensions
A suspension occurs when materials don’t
dissolve in a substance.
Ex.) Italian salad dressing.
Ex.) Blood – actually is a solution and a
suspension.