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2. Composition of Matter
• Matter is anything that occupies
space and has mass.
• Mass is the quantity of matter an
object has.
• Mass and weight are different.
• Weight depends on the amount of
gravity.
• You would weigh less on the moon
than on earth but have the same
mass.
• http://www.exploratorium.edu/ronh/weight
4. Element
• An element is a pure substance that
cannot be broken down into simpler kinds
of matter.
• Each element has a different chemical
symbol.
• More than 100 elements have been
identified.
• More than 90% of the mass of living
things is composed of oxygen, carbon,
hydrogen and nitrogen
5.
6. Atom
• An atom is the simplest part of an element that
retains the properties of that element.
• The properties of atoms determine how the
element will behave in nature.
• An atoms consists of three parts.
• The nucleus contains protons and neutrons.
• Electrons float around the outside of the
nucleus.
• The number of protons is called the atomic
number.
• Protons are charges positively, electrons are
negative and neutrons are neutral or zero
charge.
7.
8. Atomic Particles
Name of Location Charge Related
Particle Info
Proton Nucleus + Measured
by atomic
number
Neutron Nucleus 0 Measured
by atomic
mass
Electron Outside - Helps
the with
nucleus bonding
9. Electrons
• Electrons are responsible for making
chemicals.
• Electrons are set in different layers
called energy levels.
• Each level can hold up to 8
electrons except the innermost level
which can only hold 2.
10.
11. Compounds
• A compound is a pure substance made up of
two or more elements.
• A chemical formula shows what elements and
how many are in a compound.
• An atom is chemically stable when its outer shell
has 8 electrons with the exception of helium and
hydrogen.
• That is why elements bond together.
• When elements bond together they create a
chemical reaction which makes the atoms happy
and stable.
12. Covalent bonds
• Covalent bonds form when atoms
share one or more pairs of
electrons.
• This usually happens between
nonmetals.
• A molecule is formed when a
covalent bond is used.
• Examples are: water, carbon dioxide
and oxygen gas
13.
14.
15. Ionic Bonds
• Ionic bonds form when one atom
transfers electrons from itself to
another atom.
• When this occurs, an ion is formed.
• Ionic bonds usually happen between
a metal and a nonmetal.
16.
17. Energy and Matter
• Energy is the ability to do work or
cause change
• Free energy is the energy in a
system available for work.
• There are three main states of
matter.
• Solid, liquid and gas.
18. Energy and Chemical
Reactions
• Living things undergo thousands of
chemical reactions as part of their
life processes.
• The reactants are shown on the left
side of the equation.
• The products are shown on the right
side.
• Reactants are converted to
products.
• Energy is required for the chemical
reaction to occur.
19. A chemical reaction must make
something totally different that has
different properties from when it
started.
You start with the reactants And you end with the products
21. When you make a
sandwich, what do
you do?
Products
Reactants
22. How can you recognize a chemical
reaction?
Breaking glass
Ice pack Rusting car
Frying an egg
Burning a match
Boiling water
Shaking pop
Hand warmers
Chopping
Freezing veggies
water Cooking
Baking a cake
macaroni
23.
24. Energy Transfer
• Chemical reactions that release energy
are called exergonic reactions.
• Chemical reactions that absorb energy
are called endergonic reactions.
• Both exergonic and endergonic reactions
require energy to start the process.
• This is called activation energy.
• Certain chemicals called catalysts, reduce
the amount of activation energy required.
• The reaction happens easier.
• One catalyst in the body is called an
enzyme.
25.
26. Redox reactions
• Many chemicals reactions that help
transfer energy in living things involve the
transfer of electrons.
• These are called reduction-oxidation
reactions or redox reactions.
• In oxidation, a reactant loses one or more
electrons, making it a positive ion.
• In reduction, a reactant gains one or more
electrons making it more negative.
• There is always an atom that is oxidized
and an atom that is reduced.
27. Solutions
• A solution is a mixture in which one or more
substances is uniformly distributed in another
substance.
• A solution has two parts.
• The solute is the substance dissolved in the
solution.
• The solvent is the substance in which the solute
in dissolved.
• The concentration is the measurement of the
amount of solute dissolved in the solvent.
• A saturated solution is one in which no more
solute can dissolve.
• An aqueous solution are solutions in which water
is the solvent. These are very common.
28. Acids and Bases
• Dissociation is the breaking apart of
water.
• When water breaks, two things are made.
• The hydroxide ion is OH-
• The hydrodium ion is H3O+
• If the number of hydrodium ions is greater
than the number of hydroxide ions, the
solution is an acid.
• Sometimes hydrodium is just written H+
• If the number of hydroxide ions is greater
than the hydrodium ions, then the solution
is a base.
29.
30. pH and Buffers
• pH is the scale for comparing the relative
concentrations of hydronium in a solution.
• The scale ranges from 0 to 14.
• The smaller the number, the more acidic a
solution is. The higher the number, the more
basic it is.
• For example, stomach acid has a pH of about 2.
Ammonia has a pH of about 12.
• Buffers are chemicals that neutralize acids and
bases in the body.
• Buffers help maintain good pH levels in the
body.
31.
32. Which
Exchange or
have an
give/take
Atoms electrons electric
Charge
Which makes
Ionic bonds
and Ions
34. Essential Questions
• How are particles arranged in an atom?
• How does an ionic bond differ from a covalent
bond?
• Why doesn’t Neon combine with elements very
often?
• What are the 3 state of matter?
• Explain how a catalyst affects a reaction.
• Why does a reduction always happen with an
oxidation?
• Describe the dissociation of water.
• What is neutral pH?
• What is a buffer? Why is it important to the
body?