review of atomic structure from physical...
TRANSCRIPT
![Page 1: Review of Atomic Structure from Physical Sciencemacsciencecafe.weebly.com/.../9/8/0/39808139/atomic... · Sub-Atomic Particles ... particle with a negative charge that is found in](https://reader033.vdocuments.net/reader033/viewer/2022050406/5f83ef300f23be62525bf8af/html5/thumbnails/1.jpg)
Review of
Atomic Structure
from Physical
Science
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Two major parts of an atom
Nucleus
(not to scale)
Electron
Cloud
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Three Major
Sub-Atomic Particles
• Protons
• Neutrons
• Electrons
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a single, relatively large
particle with a
positive charge that is
found in the nucleus
PROTON (p+)
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THE PROTON
p+
• Fat
(heavy)
• Positive
(charge)
• Doesn’t move
(lazy)
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a single, relatively large
particle with a
neutral charge that is
found in the nucleus
NEUTRON (N°)
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THE NEUTRON
N°
• Fat
(heavy)
• Neutral
(charge)
• Doesn’t move
(lazy)
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a single, very small
particle with a
negative charge that is
found in a “cloud”
around the nucleus
ELECTRON (e-)
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THE ELECTRON
• Skinny
(very light)
• Negative
(charge)
• Moves a lot
(runs around)
e-
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Review: Subatomic Particles
e-
N°
p+
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ELEMENTS a type of matter that
can not be broken
down by ordinary
chemical means
(everything on the PT)
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Elements are the
simplest form of
matter. They can’t
be broken down
anymore. They are
the building blocks
of all matter!
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If its on the PT, its an Element!
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Atoms of the same
element that differ in
charge.
(They have the same # of
p+, but different # of e-)
ION
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If an atom GAINS
electrons, its overall charge
becomes more negative.
If it LOSES electrons, its
charge becomes more
positive
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Positive Ions (cations)
Negative Ions (anions)
• Na+ (lost 1 e-)
• Ca2+ (lost 2 e-)
• Al3+ (lost 3 e-)
• Pb4+ (lost 4 e-)
• H+ (lost 1 e-)
• Cl- (gain 1 e-)
• O2- (gain 2 e-)
• P3- (gain 3 e-)
• S2- (gain 2 e-)
• OH- (gain 1 e-)
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An ion comprised of
a single atom
(Na+, O2-)
Monatomic Ion
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An ion made up of
two or more atoms
(i.e. O22- or SO4
2-)
Polyatomic Ion
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The charge on a
monatomic ion
( O2- )
OXIDATION #
Oxidation #
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The charge on a
polyatomic ion
( SO42- )
CHARGE
Charge
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Writing and
Naming Ionic
Compounds
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How to Write
Ionic Formulas
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LiBr Al2O3
BaS
Na2O
CaBr2 K2Se
AlF3
MgCl2
B2S3 MgTe NaF
NaAt CaI2
KCl BI3
•Group the above compounds by similarities.
Make as many groups as you want. Put your
results on a piece of paper.
• Based on your patterns, write rules
concerning the ratio of elements in a
compound.
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PRISMS pg.
142???
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When writing
ionic formulas the
sum of the charges
must equal zero
GOAL
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Remember the
goal is to get the
overall charge to
equal 0.
Al3+ with O2-
Al2O3
Al = + + +
O = - - Al O
1 +++ = 3 - - = 2
2 +++
+++ = 6
- - - - = 4
3 +++++
++++ = 9
- - -
- - - = 6
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Parentheses must
be used when
adding subscripts
to polyatomic ions
HINT
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Remember the
goal is to get the
overall charge to
equal 0.
Al3+ with SO4
2-
Al2(SO4)3
Al = + + +
SO42- = - -
Al SO42-
1 +++ = 3 - - = 2
2 +++
+++ = 6
- - - - = 4
3 +++++
++++ = 9
- - -
- - - = 6
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Kris Kross Method!
Ca3As2
Ca2+As3-
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Just kris kross the
positive and the
negative charges
Na1+Cl1- NaCl
Li1+O2- Li2O
Pb4+NO31- Pb(NO3)4
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HINTS • If the charge is “1”, you don’t
need to kriss kross it down
• If the charges are the same, you
don’t need to kriss kross them
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How to Name
Ionic Formulas
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Compound made up
of only two types of
elements
(NaCl; Fe2O3)
Binary Compound
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An ion with a
POSITIVE
charge
CATION
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An ion with a
NEGATIVE
charge
ANION
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1) Write the name of the
cation
Naming Binary
Formulas
2) Write the name of the
anion, drop the
ending, and add -ide
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Don’t forget to include the
Roman Numeral when you
are naming atoms with
multiple oxidation states
CAUTION
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Name: Fe2O3
Naming Roman
Numerals
Iron (III) Oxide
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Old way of Naming
Roman Numerals
Fe2+ = Ferrous
Fe3+ = Ferric
Use endings –ous (smaller) or –ic
(bigger) on the root of the Latin
name to represent charges
Cu1+ = Cuprous
Cu2+ = Cupric
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1) Write the name of the
cation
Naming Other Ionic
Compounds
2) Write the name of the
anion (if it’s a polyatomic)
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HINTS ON NAMING
-ites are oxyanions with
less oxygen than -ates
Sulfate = SO42- Sulfite = SO3
2-
Nitrate = NO31- Nitrite = NO2
1-
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HINTS ON NAMING Hypo- (less O) and Per- (more O) are
used to indicate relative Oxygen
Hypochlorite = ClO1-
Chlorite = ClO21-
Chlorate = ClO31-
Perchlorate = ClO41-
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Compound made up
of more than two
elements NaClO3; (Hg2)3 (PO4)2
Ternary Compound
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Oxidation #s of
Ternary Compounds *** Must get all the charges to equal 0 ***
In Na2SO4 what is the oxidation number on S?
Na = (1+) * (2) = 2+ O = (2-) * (4) = 8-
Without Sulfur, the charge is 6-.
Thus, to get to an overall charge of
0, Sulfur must be a 6+!
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Oxidation #s of
Polyatomic Ions *** Must get all the charges to equal
charge on polyatomic ion ***
In NO31- what is the oxidation number on N?
O = (2-) * (3) = 6-
Without Nitrogen, the charge is 6-. Thus,
to get to an overall charge of 1-, Nitrogen
must be a 5+!
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Atom that always
occurs naturally in
pairs
Diatomic Atom
I2, H2, N2, O2, F2, Cl2, Br2
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Working with
Hydrocarbons
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1) Count the # of C and
pick the correct stem.
Naming
Hydrocarbons
2) Add the suffix –ane
3) If ring, add prefix–cyclo
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1) Linear =
(2 x (# of C)) + 2
Finding the Formula
for Hydrocarbons
2) Ring =
2 x (# of C)
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The formula for a
substance as it exists
in its molecular state
MOLECULAR
FORMULA
Benzene: C6H6
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The simplest formula
for a substance
EMPIRICAL
FORMULA
Benzene: C6H6 CH
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Molecular Formula
C6H12O6
Molecular/Ionic Formula
vs. Empirical Formula
Empirical Formula
CH2O
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The coefficient before a
compound that
represents the amount of
substance present
FORMULA UNIT
7 C6H6