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Composition of Matter
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Atom= building block of an element
Smallest part of matter
Protons= + charge
Neutrons= 0 charge
Electrons= -1 charge
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Protons & neutrons= IN NUCLEUS
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Electrons= Orbit OUTSIDE nucleus
Subatomic Particles
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Proton: positive charge, +1 mass, in
nucleus
Neutron: no charge, +1 mass, in
nucleus
Electron: negative charge, 0 mass,
outside nucleus
***# of protons ALWAYS = # Electrons
Identifying Elements:
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Atomic Number:
number of protons
in an element
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Zr=40 protons…and
_______electrons
Mass Number:
Protons + neutrons
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H= 1 mass #
He=4 mass #
Sodium
Mass Number = 23
Atomic number = 11
+
11p
12n
2-8-1
23 protons &
neutrons
- 11 protons
__________________
12 neutrons
In a neutral sodium atom
the number of protons
(11) = the number of
electrons (11)
Beryllium
Mass Number = 9
Atomic number = 4
+
4p
5n
2-2
9 protons &
neutrons
- 4 protons
__________________
5 neutrons
In a neutral beryllium
atom the number of
protons (4) =
the number of electrons
(4)
Nitrogen
Mass Number = 14
Atomic number = 7
+
7p
7n
2-5
14 protons &
neutrons
- 7 protons
__________________
7 neutrons
In a neutral nitrogen
atom
the number of protons
(7) = the number of
electrons (7)
Sulfur
Mass Number = 32
Atomic number = 16
+
16p
16n
2-8-6
32 protons &
neutrons
- 16 protons
__________________
16 neutrons
In a neutral sulfur atom
the number of protons
(16) = the number of
electrons (16)
Silicon
Mass Number = 28
Atomic number = 14
+
14p
14n
2-8-4
28 protons &
neutrons
- 14 protons
__________________
14 neutrons
In a neutral silicon atom
the number of protons
(14)= the number of
electrons (14)
Potassium
Mass Number = 39
Atomic number = 19
+
19p
20n
2 - 8 - 8- 1
39 protons &
neutrons
- 19 protons
__________________
20 neutrons
In a neutral potassium
atom the number of
protons (19) = the
number of electrons
(19)
Periodic Table
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Columns on the table are called Groups
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Group # is # of valence electrons
Rows are called Periods
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Period # tells how many shells you have
Atomic Weight & Isotopes
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Isotopes= same # of protons &
electrons, but DIFFER in neutrons
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Ex) Hydrogen, H2, H3
They still have same chemical properties
Radioisotopes= heavier isotopes that
are unstable and decay
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Can be harmful to cells
Can be used to tag biological molecules
Chemical Compounds
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Chemical combination of 2 or more
elements
Water = H2O
A compound can behave differently
than the elements that make it up
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Ex) Water. Hydrogen is gas, Oxygen is gas.
Together they form a liquid.
Types of Chemical Bonds:
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Ionic Bond: when
electrons are
transferred from one
element to another
When an atom gains
electrons, it becomes
negatively charged and
is called Anion.
Cation = positive
charge, when element
gave up electron
Covalent Bonds:
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When atoms share
electrons
The valence shell is
satisfied by both
molecules
Van der Waals Forces
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When atoms share electrons, sharing is
not always equal.
+ and – charges attract to each other
Water Polarity
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Because of unequal distribution of
electrons, water is polar.
Negative pole of oxygen is attracted to
the positive pole of hydrogen
Solutions & Suspensions
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Solutions=all components in a mixture
are equally distributed
Suspensions= mixture of water and
undissolved solutes
Solute=substance dissolved
Solvent=dissolves solute
Acids and Bases
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Acids=produces H ions
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Value below 7
Bases=produce OH ions
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Value above 7
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Look on pg. 43
pH Scale
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Created to indicate the concentration of
H ions.
Low # = acid
High #= base
Carbon Compounds
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Organic Chemistry is the study of all
compounds containing carbon
Carbon can form millions of different
bonds
4 types of compounds:
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Carbs
Lipids
Nucleic acids
Proteins
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Carbs= main source of energy
Proteins= form bones, muscles, made
of amino acids
Nucleic Acids= store/transmit genetic
information
Lipids= store energy, make up
membranes