Chemistry DMA
Write out the abbreviated electron configuration
for the following elements:
Li [He]2s1
Na
K
Rb
Cs [Xe]6s1
O
S [Ne]3s23p4
Se
Te
Po
Ne
Ar
Kr [Ar]4s23d104p6
Xe
Rn
Ions
Identity and Change Unit
Soluble/Insoluble
A soluble substance can be dissolved.
If something will not dissolve, it is
insoluble. If two or more chemicals are
mixed in a solution and a solid appears,
the solid is insoluble. In this case, the
solid is called a precipitate.
Solution
Solutions are mixtures of solvents and
solutes.
Solvents are substances that dissolve –
they cause another substance to disperse,
disintegrate, break apart.
Solutes are substances that dissolve in
solvents. Solutes break apart in solvents.
Diagram the demo set-up
Light bulb
Beaker
Magnetic stir plate
Ion
A charged particle
(either a single atom or a molecule)
Cation
A positively charged particle
Na+ H+ Ca2+ Cu2+ NH4+
Anion
A negatively charged particle
Cl- O2- OH- NO3- SO42-
Valence Electron
An electron in the outermost energy level
for an atom.
The electrons that interact when atoms
form bonds.
H
Li
Na
C
N
F
Valence electrons
The s and p electrons in the outermost
primary energy level.
There are 2 valence electrons for the 1st
primary energy level. (Period 1)
There are 8 valence electrons in every
other primary energy level. (Periods 2-7)
Bohr Models of Atoms and Ions
Sodium atom
Sodium ion
11 protons
Na
11 protons
Na
11 electrons
Chlorine atom
10 electrons
Chlorine ion
17 protons
Cl
17 protons
Cl
17 electrons
18 electrons
Ionic bond
A bond formed by the attraction between a
cation and an anion. Ionic bonds create an
ionic compound. Although the cations and
anions they are made from have positive and
negative charges, ionic compounds have a
balance of positive and negative charges, and
hence, no net charge.
Na
Na
Cl
Cl
Valence Electrons Practice
Identify the number of valence electrons in each
of the following elements:
Be
B
N
F
Mg
Al
P
Cl
Ca
As
Br
Sr
I
Dot diagram
A graphic representation of the number
and placement of valence electrons for an
atom or ion.
VSEPR theory
Valence
Shell
Electron
Pair
Repulsion
A theory based on experimental observations
that suggests valence electrons occur in pairs
that separate as far as possible three
dimensionally from other pairs in the same
valence shell.
Dot diagram practice
Draw dot diagrams for the following elements:
Li
B
N
F
Ne
Na
Si
S
Ar
Ca Ga Ge
As
Br
Rb
Sn
Te
Xe
Ba Tl
Bi Po At
Dot diagram practice
Draw dot diagrams for the following anions:
HN3O2FP3S2Cl Se2Br I-
Ionic compounds:
Chemical combinations of two or more
different elements in a fixed ratio.
Contain ions which are attracted to each
other due to opposite electrical charges.
Have no net charge due to balancing of
the charges on the cation (+) and anion (-).
Ionic compounds are generally formed
between a metallic cation and an anion.
Ionic bond:
A chemical bond resulting from the
transfer of electrons from one bonding
atom to another.
A bond involving ions.
Na
Cl
Na+ Cl-
Nomenclature: Names to Formulas
sodium chloride
sodium bromide
potassium iodide
rubidium bromide
calcium sulfide
strontium oxide
sodium sulfide
sodium nitride
calcium chloride
barium iodide
aluminum chloride
aluminum oxide
Nomenclature: Names to Formulas
NaCl
NaBr
KI
RbBr
CaS
SrO
Na2S
Na3N
CaCl2
BaI2
AlCl3
Al2O3
Nomenclature: Names to Formulas
copper (I) chloride
copper (I) bromide
iron (II) sulfide
lead (II) oxide
calcium carbonate
strontium sulfate
copper (I) sulfide
mercury (I) chloride
calcium nitrate
barium hydroxide
aluminum phosphate
nickel (II) phosphate
Nomenclature: Names to Formulas
CuCl
CuBr
FeS
PbO
CaCO3
SrSO4
Cu2S
Hg2Cl2
Ca(NO3)2
Ba(OH)2
AlPO4
Ni3(PO4)2
Molecular Weight
Sum of the atomic masses of all atoms
represented in a chemical formula,
represented either in atomic mass units
(amu) or g
Nomenclature: Formulas to Names
KI
MgS
NaOH
KNO3
CaSO4
NaClO4
NaHCO3
Zn(NO3)2
SrCl2
Ba3(PO4)2
(NH4)2Cr2O7
H2O2
Nomenclature: Formulas to Names
potassium iodide
165.998
magnesium sulfide
56.370
sodium hydroxide
39.997
potassium nitrate
94.102
calcium sulfate
136.139
sodium perchlorate
78.442
sodium hydrogen carbonate
161.998
zinc nitrate
127.394
strontium chloride
158.526
barium phosphate
601.930
ammonium dichromate
252.062
hydrogen peroxide
33.996
Nomenclature: Formulas to Names
CuO
Cu(OH)2
NiCO3
Al(NO3)3
NiCl2
AgC2H3O2
FeSO4
Fe2(SO4)3
Pb(NO3)2
Hg2Cl2
HgCl2
Cu2O
Nomenclature: Formulas to Names
copper (II) oxide
copper (II) hydroxide
nickel (II) carbonate
aluminum nitrate
nickel (II) chloride
silver acetate
iron (II) sulfate
iron (III) sulfate
lead (II) nitrate
mercury (I) chloride
mercury (II) chloride
copper (I) oxide
Distilled Water
Water + glucose
Water + starch
Water + sodium chloride
Water + sodium hydroxide
Water + copper (II) nitrate
Water + copper (II) nitrate + sodium hydroxide
Lewis structures
A system designed by
American chemist
Gilbert Lewis
to demonstrate the
interactions of
valence electrons in
the formation of
compounds.
F
Cl
C
F
Cl
Ionic Compounds: Lewis Structures
Draw Lewis Structures for the following ionic compounds:
NaCl
KF
RbBr
CsI
MgO
CaS
Na2O
K2S
AlP
Mg3N2
Na3N
KH